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IB16 06_0620_11/4RP © UCLES 2016 [Turn over

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Cambridge International Examinations Cambridge International General Certificate of Secondary Education

CHEMISTRY 0620/11

Paper 1 Multiple Choice (Core) May/June 2016

45 Minutes Additional Materials: Multiple Choice Answer Sheet Soft clean eraser Soft pencil (type B or HB is recommended)

READ THESE INSTRUCTIONS FIRST

Write in soft pencil.

Do not use staples, paper clips, glue or correction fluid.

Write your name, Centre number and candidate number on the Answer Sheet in the spaces provided unless this has been done for you.

DO NOT WRITE IN ANY BARCODES.

There are forty questions on this paper. Answer all questions. For each question there are four possible answers A, B, C and D.

Choose the one you consider correct and record your choice in soft pencil on the separate Answer Sheet.

Read the instructions on the Answer Sheet very carefully.

Each correct answer will score one mark. A mark will not be deducted for a wrong answer.

Any rough working should be done in this booklet.

A copy of the Periodic Table is printed on page 16.

Electronic calculators may be used.

2

© UCLES 2016 0620/11/M/J/16

1 In which changes do the particles move further apart? W X

gas liquid solid Y Z

A W and X B W and Z C X and Y D Y and Z 2 A sample of a dye is investigated by chromatography.

A line is drawn across a piece of chromatography paper and a spot of the dye is placed on it.

The paper is placed in water.

water

chromatographypaper

linespot of dye

Which row is correct?

what is used to draw the line

position of spot

A ink above the level of the water

B ink below the level of the water

C pencil above the level of the water

D pencil below the level of the water

3 One of the instructions for an experiment reads as follows.

Quickly add 50 cm3 of acid.

What is the best piece of apparatus to use?

A a burette

B a conical flask

C a measuring cylinder

D a pipette

3

© UCLES 2016 0620/11/M/J/16 [Turn over

4 Diamond and graphite are macromolecules.

Which statement about diamond and graphite is not correct?

A They are giant structures with high melting points.

B They are non-conductors of electricity.

C They contain only atoms of a non-metal.

D They have covalent bonds between the atoms. 5 The table shows the electronic structure of four atoms.

atom electronic structure

W 2,8,1

X 2,8,4

Y 2,8,7

Z 2,8,8

Which two atoms combine to form a covalent compound?

A W and X B W and Y C X and Y D X and Z 6 An aluminium atom has a nucleon number of 27 and a proton number of 13.

How many neutrons does this aluminium atom contain?

A 13 B 14 C 27 D 40 7 What happens when a bond is formed between a green gaseous element and a soft metallic

element?

A The gas atoms gain an electron.

B The gas atoms lose an electron.

C The metal atoms gain an electron.

D The two elements share a pair of electrons. 8 The equation shows the reaction between magnesium and sulfuric acid.

[Ar: H, 1; O, 16; Mg, 24; S, 32]

Mg + H2SO4 → MgSO4 + H2

In this reaction, which mass of magnesium sulfate is formed when 6 g of magnesium react with excess sulfuric acid?

A 8 B 24 C 30 D 60

4

© UCLES 2016 0620/11/M/J/16

9 The diagram shows an electrical cable.

metal core

plastic coating

Which statement about the substances used is correct?

A The coating is plastic because it conducts electricity well.

B The core is copper because it conducts electricity well.

C The core is copper because it is cheap and strong.

D The core is iron because it is cheap and strong. 10 When substance X is electrolysed, the amount of gases P and Q formed is shown.

P Q

+–

substance X

What is substance X?

A concentrated aqueous sodium chloride

B concentrated hydrochloric acid

C dilute sulfuric acid

D molten lead(II) bromide

5


11 The energy level diagram for the reaction between sodium hydrogen carbonate and dilute hydrochloric acid is shown.

sodium chloride + water +carbon dioxide

sodium hydrogen carbonate +dilute hydrochloric acid

energy

Which row correctly describes the type of reaction and the energy of the reactants and products?

type of reaction energy of the reactants

and products

A

endothermic

the products have more energy than the reactants

B

endothermic

the reactants have more energy than the products

C

exothermic

the products have more energy than the reactants

D

exothermic

the reactants have more energy than the products

12 The diagram shows some properties that substances may have.

To which labelled part of the diagram does 235U belong?

compoundused as

an energy source

radioactive

A

B D C

6

© UCLES 2016 0620/11/M/J/16

13 A liquid X reacts with solid Y to form a gas.

Which two diagrams show suitable methods for investigating the rate (speed) of the reaction?

XY

X

cotton wool cotton wool1 2

3 4

Y

XY

XY

stopper

balance

balance

stopper

A 1 and 3 B 1 and 4 C 2 and 3 D 2 and 4

7


14 An experiment, S, is carried out to measure the volume of hydrogen produced when excess dilute sulfuric acid is added to zinc.

A second experiment, T, is carried out using the same mass of zinc but under different conditions.

The results of the two experiments are shown.

00

time

total volumeof hydrogen

S

T

Which changes in the conditions between experiments S and T give curve T?

addition of a catalyst

the zinc is in large pieces not powdered

A � �

B � �

C � �

D � �

15 Aluminium reacts with iron(III) oxide as shown.

iron(III) oxide + aluminium → iron + aluminium oxide

Which statement about this reaction is correct?

A Aluminium is oxidised.

B Aluminium oxide is reduced.

C Iron(III) oxide is oxidised.

D Iron is oxidised. 16 Which reaction is reversible?

A Cu + ZnSO4 → CuSO4 + Zn

B CuO + H2SO4 → CuSO4 + H2O

C CuO + H2 → Cu + H2O

D CuSO4.5H2O → CuSO4 + 5H2O

8

© UCLES 2016 0620/11/M/J/16

17 Which statements are properties of an acid?

1 reacts with ammonium sulfate to form ammonia

2 turns red litmus blue

1 2

A � �

B � �

C � �

D � �

18 Part of the Periodic Table is shown.

Which element forms an acidic oxide?

A B CD

19 A method used to make copper(II) sulfate crystals is shown.

1 Place dilute sulfuric acid in a beaker.

2 Warm the acid.

3 Add copper(II) oxide until it is in excess.

4 Filter the mixture.

5 Evaporate the filtrate until crystals start to form.

6 Leave the filtrate to cool.

What are the purposes of step 3 and step 4?

step 3 step 4

A to ensure all of the acid has reacted to obtain solid copper(II) sulfate

B to ensure all of the acid has reacted to remove excess copper(II) oxide

C to speed up the reaction to obtain solid copper(II) sulfate

D to speed up the reaction to remove excess copper(II) oxide

9


20 The results of two tests on solid X are shown.

test observation

aqueous sodium hydroxide added green precipitate formed

acidified silver nitrate added yellow precipitate formed

What is X?

A copper(II) chloride

B copper(II) iodide

C iron(II) chloride

D iron(II) iodide

21 Where in the Periodic Table is the metallic character of the elements greatest?

left or right

side of a period at the top or bottom

of a group

A left bottom

B left top

C right bottom

D right top

22 Some properties of four elements, P, Q, R and S, are shown in the table.

Two of these elements are in Group I of the Periodic Table and two are in Group VII.

element reaction with water physical state at

room temperature

P reacts vigorously solid

Q does not react with water solid

R reacts explosively solid

S dissolves giving a coloured solution liquid

Which statement is correct?

A P is below R in Group I.

B Q is above R in Group I.

C Q is below S in Group VII.

D R is below S in Group VII.

10

© UCLES 2016 0620/11/M/J/16

23 Which of the following could be a transition element?

melting point

in °C

density in g / cm3 colour

electrical conductor

A 114 4.9 purple no

B 659 2.7 grey yes

C 1677 4.5 grey yes

D 3727 2.3 black yes

24 Two statements about argon are given.

1 Argon has a full outer shell of electrons.

2 Argon is very reactive and is used in lamps.

Which is correct?

A Both statements are correct and statement 2 explains statement 1.

B Both statements are correct but statement 2 does not explain statement 1.

C Statement 1 is correct but statement 2 is incorrect.

D Statement 2 is correct but statement 1 is incorrect. 25 Three students, X, Y and Z, were told that solid P reacts with dilute acids and also conducts

electricity.

The table shows the students’ suggestions about the identity of P.

X Y Z

copper iron graphite

Which of the students are correct?

A X, Y and Z B X only C Y only D Z only

11


26 W, X and Y are metals, one of which is copper and one of which is iron.

• W has a coloured oxide which can be reduced by carbon.

• X has a black oxide and is also found in nature as a pure metal.

• Y has an oxide which cannot be reduced by carbon.

Which metal is the most reactive and what is the possible identity of W?

most reactive

metal possible identity

of W

A X Cu

B X Fe

C Y Cu

D Y Fe

27 Tin is a metal that is less reactive than iron and is extracted from its ore cassiterite, SnO2.

Which statements about tin are correct?

1 Tin can be extracted from cassiterite using carbon.

2 Tin does not conduct electricity.

3 Tin is hard and shiny.

A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only 28 Which statement about the uses of metals is correct?

A Aluminium is used in the manufacture of aircraft because of its strength and high density.

B Copper is used in electrical wiring because of its strength and high density.

C Mild steel is used in the manufacture of car bodies because of its strength and resistance to corrosion.

D Stainless steel is used in the construction of chemical plant because of its strength and resistance to corrosion.

12

© UCLES 2016 0620/11/M/J/16

29 The diagram shows an experiment to investigate how paint affects the rusting of iron.

air

P Q

water

iron painted iron

What happens to the water level in tubes P and Q?

tube P tube Q

A falls rises

B no change rises

C rises falls

D rises no change

30 A new planet has been discovered and its atmosphere has been analysed.

atmosphere

planet

The table shows the composition of its atmosphere.

gas percentage by volume

carbon dioxide 4

nitrogen 72

oxygen 24

Which gases are present in the atmosphere of the planet in a higher percentage than they are in the Earth’s atmosphere?

A carbon dioxide and oxygen

B carbon dioxide only

C nitrogen and oxygen

D nitrogen only

13


31 Water was added to separate samples of anhydrous cobalt(II) chloride and anhydrous

copper(II) sulfate.

Which row describes the colour changes that take place in these reactions?

cobalt(II) chloride copper(II) sulfate

A blue to pink blue to white

B blue to pink white to blue

C pink to blue blue to white

D pink to blue white to blue

32 Which pollutant found in air does not have an effect on respiration?

A carbon monoxide

B lead compounds

C oxides of nitrogen

D sulfur dioxide 33 A farmer’s soil is very low in both nitrogen (N) and phosphorus (P).

Which fertiliser would improve the quality of this soil most effectively?

percentage

nitrogen (N) phosphorus (P) potassium (K)

A 11 11 27

B 12 37 10

C 28 10 10

D 31 29 9

34 When limestone is heated it forms lime (calcium oxide) and carbon dioxide.

CaCO3(s) → CaO(s) + CO2(g)

Which statement is not correct?

A Carbon dioxide is a greenhouse gas which may contribute to climate change.

B Slaked lime is used to neutralise industrial waste.

C The lime can be used to treat alkaline soil.

D This reaction is an example of thermal decomposition.

14

© UCLES 2016 0620/11/M/J/16

35 The diagram shows the separation of petroleum into fractions.

gasoline

X

Y

Z

bitumen

petroleum

What could X, Y and Z represent?

X Y Z

A diesel oil lubricating fraction paraffin

B lubricating fraction diesel oil paraffin

C paraffin lubricating fraction diesel oil

D paraffin diesel oil lubricating fraction

36 Which of the compounds shown are in the same homologous series?

1 CH3OH

2 CH3CH2OH

3 CH3COOH

4 CH3CH2CH2OH

A 1, 2 and 3 B 1, 2 and 4 C 1, 3 and 4 D 2, 3 and 4 37 Compound Q decolourises bromine water.

Compound Q has two carbon atoms in each molecule.

Which statement about compound Q is correct?

A It contains carbon-hydrogen double bonds.

B It has six hydrogen atoms per molecule.

C It has two carbon-carbon double bonds.

D It is produced by cracking alkanes.

15

Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the publisher will be pleased to make amends at the earliest possible opportunity. To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge International Examinations Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at www.cie.org.uk after the live examination series.

Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.

© UCLES 2016 0620/11/M/J/16

38 What is used in the production of ethanol from ethene?

A hydrogen and oxygen

B oxygen only

C steam

D yeast 39 Ethene forms an addition polymer as shown.

H

C...... +

H

H

C +

H

H

C

H

H

C + ...... ...... ......

H

H

C

H

H

C

H

H

C

H

H

C

H

Which terms describe this polymer?

A a saturated compound called poly(ethane)

B a saturated compound called poly(ethene)

C an unsaturated compound called poly(ethane)

D an unsaturated compound called poly(ethene) 40 The diagram shows a molecule of an organic compound W.

H C

H

H

C

OH

O


A A solution of W in water has a pH greater than pH 7.

B A solution of W in water reacts with sodium hydroxide solution.

C When copper(II) carbonate is added to a solution of W in water, a gas is produced.

D When magnesium is added to a solution of W in water, a gas is produced.

16

© UCLES 2016 0620/11/M/J/16

Gro

up

The

Perio

dic

Tabl

e of

Ele

men

ts

1 Hhy

drog

en1

2 He

heliu

m4

III

IIIIV

VV

IV

IIV

III

3 Lilit

hium 7

4 Be

bery

llium

9

atom

ic n

umbe

r

atom

ic s

ymbo

l

Key

nam

ere

lativ

e at

omic

mas

s

11 Na

sodi

um23

12 Mg

mag

nesi

um24

19 Kpo

tass

ium

39

20 Ca

calc

ium

40

37 Rb

rubi

dium

85

38 Sr

stro

ntiu

m88

55 Cs

caes

ium

133

56 Ba

bariu

m13

7

87 Frfra

nciu

m–

88 Ra

radi

um –

5 B boro

n11 13 Al

alum

iniu

m27 31 Ga

galli

um70 49 In indi

um11

5

81 Tlth

alliu

m20

4

6 Cca

rbon

12 14 Si

silic

on28 32 Ge

germ

aniu

m73 50 Sn tin 119

82 Pb

lead

207

22 Titit

aniu

m48 40 Zr

zirc

oniu

m91 72 Hf

hafn

ium

178

104

Rf

ruth

erfo

rdiu

m–

23 Vva

nadi

um51 41 Nb

niob

ium

93 73 Tata

ntal

um18

1

105

Db

dubn

ium

–

24 Cr

chro

miu

m52 42 Mo

mol

ybde

num

96 74 Wtu

ngst

en18

4

106

Sg

seab

orgi

um–

25 Mn

man

gane

se55 43 Tc

tech

netiu

m– 75 Re

rhen

ium

186

107

Bh

bohr

ium

–

26 Fe iron

56 44 Ru

ruth

eniu

m10

1

76 Os

osm

ium

190

108

Hs

hass

ium

–

27 Co

coba

lt59 45 Rh

rhod

ium

103

77 Iriri

dium

192

109

Mt

mei

tner

ium

–

28 Ni

nick

el59 46 Pd

palla

dium

106

78 Pt

plat

inum

195

110

Ds

darm

stad

tium

–

29 Cu

copp

er64 47 Ag

silv

er10

8

79 Au

gold

197

111

Rg

roen

tgen

ium

–

30 Zn zinc 65 48 Cd

cadm

ium

112

80 Hg

mer

cury

201

112

Cn

cope

rnic

ium

–

114 Fl

flero

vium

–

116

Lvliv

erm

oriu

m–

7 Nni

troge

n14 15 P

phos

phor

us31 33 As

arse

nic

75 51 Sb

antim

ony

122

83 Bi

bism

uth

209

8 Oox

ygen

16 16 S sulfu

r32 34 Se

sele

nium

79 52 Tete

lluriu

m12

8

84 Po

polo

nium

–

9 Fflu

orin

e19 17 Cl

chlo

rine

35.5

35 Br

brom

ine

80 53 Iio

dine

127

85 At

asta

tine

–

10 Ne

neon 20 18 Ar

argo

n40 36 Kr

kryp

ton

84 54 Xe

xeno

n13

1

86 Rn

rado

n–

21 Sc

scan

dium

45 39 Yyt

trium 89

57–7

1la

ntha

noid

s

89–1

03ac

tinoi

ds

57 Lala

ntha

num

139

89 Ac

lant

hano

ids

actin

oids

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3 a

t roo

m te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.)

actin

ium

–

58 Ce

ceriu

m14

0

90 Th thor

ium

232

59 Pr

pras

eody

miu

m14

1

91 Pa

prot

actin

ium

231

60 Nd

neod

ymiu

m14

4

92 Uur

aniu

m23

8

61 Pm

prom

ethi

um– 93 Np

nept

uniu

m–

62 Sm

sam

ariu

m15

0

94 Pu

plut

oniu

m–

63 Eu

euro

pium

152

95 Am

amer

iciu

m–

64 Gd

gado

liniu

m15

7

96 Cm

curiu

m–

65 Tb terb

ium

159

97 Bk

berk

eliu

m–

66 Dy

dysp

rosi

um16

3

98 Cf

calif

orni

um–

67 Ho

holm

ium

165

99 Es

eins

tein

ium

–

68 Er

erbi

um16

7

100

Fm ferm

ium

–

69 Tm thul

ium

169

101

Md

men

dele

vium

–

70 Yb

ytte

rbiu

m17

3

102

No

nobe

lium

–

71 Lu lute

tium

175

103 Lr

law

renc

ium

–


This document consists of 17 printed pages and 3 blank pages.


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CHEMISTRY 0620/12















2

© UCLES 2016 0620/12/M/J/16



A W and X B W and Z C X and Y D Y and Z 2 In the chromatography experiment shown, which label represents the solvent front?

C

D

B

A

3 One of the instructions for an experiment reads as follows.



A a burette

B a conical flask


D a pipette 4 Two statements about diamond are given.

1 Diamond has a giant three-dimensional covalent structure of carbon atoms.

2 Diamond is one of the hardest substances known.

Which is correct?




D Statement 2 is correct but statement 1 is incorrect.

3


5 The table shows the electronic structure of four atoms.


W 2,8,1

X 2,8,4

Y 2,8,7

Z 2,8,8


A W and X B W and Y C X and Y D X and Z 6 An atom of element Q contains 19 electrons, 19 protons and 20 neutrons.

What is Q?

A calcium

B potassium

C strontium

D yttrium 7 Lithium is in Group I of the Periodic Table. Nitrogen is in Group V of the Periodic Table.

Lithium reacts with nitrogen to form the ionic compound lithium nitride.

What happens to the electrons when lithium atoms and nitrogen atoms form ions?

lithium atoms nitrogen atoms

A

each lithium atom loses one electron to form a Li+ ion

each nitrogen atom gains three electrons to form an N3– ion

B

each lithium atom loses one electron to form a Li+ ion

each nitrogen atom gains five electrons to form an N5– ion

C

each lithium atom gains one electron to form a Li– ion

each nitrogen atom loses three electrons to form an N3+ ion

D

each lithium atom gains one electron to form a Li– ion

each nitrogen atom loses five electrons to form an N5+ ion

4

© UCLES 2016 0620/12/M/J/16

8 The equation shows the reaction between magnesium and sulfuric acid. [Ar: H, 1; O, 16; Mg, 24; S, 32]



A 8 B 24 C 30 D 60 9 The diagram shows an electrical cable.

metal core

plastic coating





D The core is iron because it is cheap and strong. 10 What are the products at the electrodes when dilute sulfuric acid is electrolysed using inert

electrodes?

anode cathode

A hydrogen oxygen

B oxygen hydrogen

C sulfur oxygen

D sulfur dioxide hydrogen

5


11 The energy level diagram for the reaction between magnesium and hydrochloric acid is shown.

Mg + 2HCl

MgCl 2 + H2

energy

Which statement about the reaction is not correct?

A Energy is given out during the reaction.

B The products are at a lower energy level than the reactants.

C The reaction is endothermic.

D The temperature increases during the reaction. 12 The diagram shows some properties that substances may have.


compoundused as

an energy source

radioactive

A

B D C

6

© UCLES 2016 0620/12/M/J/16



XY

X


3 4

Y

XY

XY

stopper

balance

balance

stopper


7


14 The results of two separate reactions between excess calcium carbonate and hydrochloric acid are shown.

volume ofgas collected

time

first reaction

second reaction

00

Which statement explains the differences between the reactions?

A More calcium carbonate was used in the second reaction.

B The same volume of more concentrated acid was used in the second reaction.

C The second reaction was allowed to react for longer.

D The temperature was higher in the second reaction. 15 The equations below all show redox reactions.

Fe2O3 + 3CO → 2Fe + 3CO2

2ZnO + C → 2Zn + CO2

Fe2O3 + 2Al → Al 2O3 + 2Fe

2CO + 2NO → 2CO2 + N2

Which oxide is oxidised in these reactions?

A Fe2O3 B CO C ZnO D NO 16 In which reaction is the colour change from blue to white?

A heating hydrated cobalt(II) chloride

B heating hydrated copper(II) sulfate

C adding water to anhydrous cobalt(II) chloride

D adding water to anhydrous copper(II) sulfate

8

© UCLES 2016 0620/12/M/J/16




1 2

A � �

B � �

C � �

D � �



A

B C D

19 What is the correct sequence of steps for the preparation of a pure sample of copper(II) sulfate

crystals from copper(II) oxide and sulfuric acid?

A dissolving → crystallisation → evaporation → filtration

B dissolving → evaporation → filtration → crystallisation

C dissolving → filtration → crystallisation → evaporation

D dissolving → filtration → evaporation → crystallisation

9


20 The following tests are carried out on an aqueous solution of salt X.

test observation

sodium hydroxide solution is added

a green precipitate is formed which dissolves in excess

a small piece of aluminium foil is then added to the mixture and the mixture is heated

a gas is given off which turns damp, red litmus paper blue

What is X?

A aluminium nitrate

B ammonium sulfate

C chromium(III) nitrate

D iron(II) nitrate


left or right


of a group

A left bottom

B left top

C right bottom

D right top

22 Rubidium is a Group I metal.

Which statement about rubidium is not correct?

A It has a higher melting point than lithium.

B It has one electron in its outer shell.

C It reacts vigorously with water.

D It reacts with chlorine to form rubidium chloride, RbCl .

10

© UCLES 2016 0620/12/M/J/16

23 The table gives information about four elements, P, Q, R and S.

melting point

in °C

electrical conductivity of element when solid

density in g / cm3 colour of iodide

of element

P 98 good 0.97 white

Q –39 good 13.53 red

R 1410 poor 2.33 colourless

S 1535 good 7.87 green

Which elements could be transition elements?

A P, Q and S B Q and S only C R and S only D S only 24 Part of the Periodic Table is shown.

Which element is a gas that does not form a compound with potassium?

A BC D

25 Which property is not considered a typical metallic property?

A good conductor of heat

B low melting point

C malleable (can be hammered into shape)

D strong

11


26 Some chemical properties of three metals W, X and Y and their oxides are shown.

metal reaction with steam reaction with dilute hydrochloric acid

reaction of metal oxide with carbon

W reacts reacts reacts

X no reaction no reaction reacts

Y reacts reacts no reaction

What is the order of reactivity of these metals, most reactive first?

A W → Y → X

B X → Y → W

C Y → W → X

D Y → X → W 27 Iron from a blast furnace is treated with oxygen and with calcium oxide to make steel.

Which substances in the iron are removed?

oxygen removes calcium oxide

removes

A carbon acidic oxides

B carbon basic oxides

C iron acidic oxides

D iron basic oxides

28 Copper is sometimes used to make cooking utensils.

saucepan

gas ring

Three properties of copper are given.

1 corrosion resistant

2 good conductor of electricity

3 good conductor of heat

Which properties make copper a suitable metal for making cooking utensils?

A 1 and 3 B 1 only C 2 and 3 D 2 only

12

© UCLES 2016 0620/12/M/J/16


air

P Q

water

iron painted iron


tube P tube Q

A falls rises

B no change rises

C rises falls

D rises no change


atmosphere

planet



carbon dioxide 4

nitrogen 72

oxygen 24





D nitrogen only

13


31 Which of the following are tests for water?

1 It turns anhydrous copper(II) sulfate blue.

2 It boils at 100 °C.

3 It turns anhydrous cobalt(II) chloride paper blue.

A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only

32 Sulfur dioxide, carbon monoxide and oxides of nitrogen are common gaseous pollutants found in

the air.

Which pollutants contribute to acid rain?

A carbon monoxide and sulfur dioxide

B oxides of nitrogen and sulfur dioxide

C oxides of nitrogen only

D sulfur dioxide only 33 Which compound is not used as a fertiliser?

A ammonium phosphate

B ammonium sulfate

C calcium carbonate

D potassium nitrate 34 Lime (calcium oxide) is used to treat waste water from a factory.

Which substance is removed by the lime?

A ammonia

B sodium chloride

C sodium hydroxide

D sulfuric acid

14

© UCLES 2016 0620/12/M/J/16


gasoline

X

Y

Z

bitumen

petroleum


X Y Z





36 Which compound is not an alkane, CnH2n+2?

A CH3CH2CH2CH3

B (CH3)2CHCH3

C CH3CHCHCH3

D (CH3)3CH

15


37 A hydrocarbon W burns to form carbon dioxide and water.

W decolourises bromine water.

What is the name of W and what is its structure?

name of W structure of W

A ethane C

H

H H

H

C

HH

B ethane C C

H

H

H

H

C ethene C

H

H H

H

C

HH

D ethene C C

H

H

H

H

38 Which term describes the formation of ethanol from glucose?

A cracking

B distillation

C fermentation

D polymerisation

16

© UCLES 2016 0620/12/M/J/16

39 Ethene forms an addition polymer as shown.

H

C...... +

H

H

C +

H

H

C

H

H

C + ...... ...... ......

H

H

C

H

H

C

H

H

C

H

H

C

H





D an unsaturated compound called poly(ethene) 40 Which statement about carboxylic acids is not correct?

A Aqueous ethanoic acid has a pH below pH 7.

B They contain the functional group –COOH.

C They produce carbon dioxide when reacted with a metal carbonate.

D Methyl orange turns yellow in aqueous ethanoic acid.

17

© UCLES 2016 0620/12/M/J/16

BLANK PAGE

18

© UCLES 2016 0620/12/M/J/16

BLANK PAGE

19



© UCLES 2016 0620/12/M/J/16

BLANK PAGE

20

© UCLES 2016 0620/12/M/J/16

Gro

up

The

Perio

dic

Tabl

e of

Ele

men

ts

1 Hhy

drog

en1

2 He

heliu

m4

III

IIIIV

VV

IV

IIV

III

3 Lilit

hium 7

4 Be

bery

llium

9

atom

ic n

umbe

r

atom

ic s

ymbo

l

Key

nam

ere

lativ

e at

omic

mas

s

11 Na

sodi

um23

12 Mg

mag

nesi

um24

19 Kpo

tass

ium

39

20 Ca

calc

ium

40

37 Rb

rubi

dium

85

38 Sr

stro

ntiu

m88

55 Cs

caes

ium

133

56 Ba

bariu

m13

7

87 Frfra

nciu

m–

88 Ra

radi

um –

5 B boro

n11 13 Al

alum

iniu

m27 31 Ga

galli

um70 49 In indi

um11

5

81 Tlth

alliu

m20

4

6 Cca

rbon

12 14 Si

silic

on28 32 Ge

germ

aniu

m73 50 Sn tin 119

82 Pb

lead

207

22 Titit

aniu

m48 40 Zr

zirc

oniu

m91 72 Hf

hafn

ium

178

104

Rf

ruth

erfo

rdiu

m–

23 Vva

nadi

um51 41 Nb

niob

ium

93 73 Tata

ntal

um18

1

105

Db

dubn

ium

–

24 Cr

chro

miu

m52 42 Mo

mol

ybde

num

96 74 Wtu

ngst

en18

4

106

Sg

seab

orgi

um–

25 Mn

man

gane

se55 43 Tc

tech

netiu

m– 75 Re

rhen

ium

186

107

Bh

bohr

ium

–

26 Fe iron

56 44 Ru

ruth

eniu

m10

1

76 Os

osm

ium

190

108

Hs

hass

ium

–

27 Co

coba

lt59 45 Rh

rhod

ium

103

77 Iriri

dium

192

109

Mt

mei

tner

ium

–

28 Ni

nick

el59 46 Pd

palla

dium

106

78 Pt

plat

inum

195

110

Ds

darm

stad

tium

–

29 Cu

copp

er64 47 Ag

silv

er10

8

79 Au

gold

197

111

Rg

roen

tgen

ium

–

30 Zn zinc 65 48 Cd

cadm

ium

112

80 Hg

mer

cury

201

112

Cn

cope

rnic

ium

–

114 Fl

flero

vium

–

116

Lvliv

erm

oriu

m–

7 Nni

troge

n14 15 P

phos

phor

us31 33 As

arse

nic

75 51 Sb

antim

ony

122

83 Bi

bism

uth

209

8 Oox

ygen

16 16 S sulfu

r32 34 Se

sele

nium

79 52 Tete

lluriu

m12

8

84 Po

polo

nium

–

9 Fflu

orin

e19 17 Cl

chlo

rine

35.5

35 Br

brom

ine

80 53 Iio

dine

127

85 At

asta

tine

–

10 Ne

neon 20 18 Ar

argo

n40 36 Kr

kryp

ton

84 54 Xe

xeno

n13

1

86 Rn

rado

n–

21 Sc

scan

dium

45 39 Yyt

trium 89

57–7

1la

ntha

noid

s

89–1

03ac

tinoi

ds

57 Lala

ntha

num

139

89 Ac

lant

hano

ids

actin

oids

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3 a

t roo

m te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.)

actin

ium

–

58 Ce

ceriu

m14

0

90 Th thor

ium

232

59 Pr

pras

eody

miu

m14

1

91 Pa

prot

actin

ium

231

60 Nd

neod

ymiu

m14

4

92 Uur

aniu

m23

8

61 Pm

prom

ethi

um– 93 Np

nept

uniu

m–

62 Sm

sam

ariu

m15

0

94 Pu

plut

oniu

m–

63 Eu

euro

pium

152

95 Am

amer

iciu

m–

64 Gd

gado

liniu

m15

7

96 Cm

curiu

m–

65 Tb terb

ium

159

97 Bk

berk

eliu

m–

66 Dy

dysp

rosi

um16

3

98 Cf

calif

orni

um–

67 Ho

holm

ium

165

99 Es

eins

tein

ium

–

68 Er

erbi

um16

7

100

Fm ferm

ium

–

69 Tm thul

ium

169

101

Md

men

dele

vium

–

70 Yb

ytte

rbiu

m17

3

102

No

nobe

lium

–

71 Lu lute

tium

175

103 Lr

law

renc

ium

–




*8830351027*


CHEMISTRY 0620/13















2

© UCLES 2016 0620/13/M/J/16



A W and X B W and Z C X and Y D Y and Z 2 Chromatography experiments are carried out on four substances, P, Q, R and S.

The same solvent is used in each experiment.

The resulting chromatograms are shown below.

P Q R S

baseline


A P and Q are pure substances.

B P and R are different substances.

C R and S are pure substances.

D S is a mixture of substances. 3 One of the instructions for an experiment reads as follows.



A a burette

B a conical flask


D a pipette

3


4 The structures of diamond and graphite are shown.

diamond graphite

Which statement about diamond and graphite is not correct?

A Diamond is used in cutting tools because the strong covalent bonds make it very hard.

B Graphite acts a lubricant because of the weak bonds between the layers.

C Graphite conducts electricity because the electrons between the layers are free to move.

D Graphite has a low melting point because of the weak bonds between the layers. 5 The table shows the electronic structure of four atoms.


W 2,8,1

X 2,8,4

Y 2,8,7

Z 2,8,8


A W and X B W and Y C X and Y D X and Z 6 The table shows the atomic structure of four atoms.

Which atom is not a metal?

electrons neutrons protons

A 18 22 18

B 19 20 19

C 19 21 19

D 20 20 20

4

© UCLES 2016 0620/13/M/J/16

7 Potassium, K, forms a compound with fluorine, F.

Which statements about this compound are correct?

1 The compound is ionic.

2 The formula of the compound is KF.

3 The compound is soluble in water.

A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only 8 The equation shows the reaction between magnesium and sulfuric acid.

[Ar: H, 1; O, 16; Mg, 24; S, 32]



A 8 B 24 C 30 D 60 9 The diagram shows an electrical cable.

metal core

plastic coating





D The core is iron because it is cheap and strong.

5


10 Electricity is passed separately through concentrated hydrochloric acid, concentrated aqueous sodium chloride and dilute sulfuric acid.

In which rows are the electrolysis products correctly named?

cathode product anode product

1

concentrated hydrochloric acid

hydrogen

chlorine

2

concentrated aqueous sodium chloride

sodium

chlorine

3 dilute sulfuric acid hydrogen oxygen

A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only

11 The energy level diagram shows the energy of the reactants and products in a chemical reaction.

reactants

products

energy

Which row correctly describes the energy change and the type of reaction shown?

energy change type of reaction

A energy is given out

to the surroundings

endothermic

B energy is given out

to the surroundings

exothermic

C energy is taken in from

the surroundings

endothermic

D energy is taken in from

the surroundings

exothermic

6

© UCLES 2016 0620/13/M/J/16



compoundused as

an energy source

radioactive

A

B D C



XY

X


3 4

Y

XY

XY

stopper

balance

balance

stopper


7


14 Magnesium is reacted with a dilute acid.

The hydrogen gas is collected and its volume measured.

The results are shown on the graph.

40

30

20

10

00 1 2 3 4

time / minutes

volume ofhydrogen / cm3

5 6 7 8

Between which times was the reaction fastest?

A 0 and 1 minute

B 1 and 2 minutes

C 2 and 3 minutes

D 7 and 8 minutes

15 A violent reaction occurs when a mixture of chromium(III) oxide and aluminium is ignited with a

magnesium fuse as shown.

crucible

magnesium fuse

mixture ofchromium(III) oxideand aluminium

sand

The equation for the reaction is shown.

Cr2O3 + 2Al → 2Cr + Al 2O3

Which substance is oxidised in the reaction?

A aluminium

B aluminium oxide

C chromium

D chromium(III) oxide

8

© UCLES 2016 0620/13/M/J/16

16 Equations for the effect of water on anhydrous cobalt(II) chloride and anhydrous

copper(II) sulfate are shown.

CoCl 2(s) + 6H2O(l) → CoCl 2.6H2O(s)

CuSO4(s) + 5H2O(l) → CuSO4.5H2O(s)


A Both reactions can be reversed by changing the conditions.

B Both reactions can be used as a test for water.

C The colour change observed when hydrated copper(II) sulfate is heated is from blue to white.

D The colour change observed when water is added to anhydrous cobalt(II) chloride is from pink to blue.




1 2

A � �

B � �

C � �

D � �



A

B CD

9


19 Salts can be made by adding different substances to dilute hydrochloric acid.

For which substance could any excess not be removed by filtration?

A copper(II) oxide

B magnesium

C sodium hydroxide

D zinc hydroxide 20 A solution containing substance X was tested. The table shows the results.

test result

flame test lilac colour

acidified silver nitrate solution added yellow precipitate

What is X?

A lithium bromide

B lithium iodide

C potassium bromide

D potassium iodide 21 Where in the Periodic Table is the metallic character of the elements greatest?

left or right


of a group

A left bottom

B left top

C right bottom

D right top

22 Which statement about the elements in Group I is correct?

A Hydrogen is evolved when they react with water.

B Ions of Group I elements have a –1 charge.

C Sodium is more reactive than potassium.

D Solid sodium is a poor electrical conductor.

10

© UCLES 2016 0620/13/M/J/16

23 Osmium is a transition element.

Which row gives the expected properties of osmium?

melting point density compounds

formed

A high high coloured

B high high white

C high low white

D low high coloured

24 Two statements about noble gases are given. 1 Noble gases are reactive, monatomic gases.

2 Noble gases all have full outer shells of electrons.

Which is correct?




D Statement 2 is correct but statement 1 is incorrect. 25 Some properties of substance X are listed.

● It conducts electricity when molten.

● It has a high melting point.

● It burns in oxygen and the product dissolves in water to give a solution with pH 11.

What is X?

A a covalent compound

B a macromolecule

C a metal

D an ionic compound

11


26 The list shows the order of reactivity of some elements.

K Na Ca Mg Zn Fe (H) Cu

Which statement about the reactivity of these metals is correct?

A Copper reacts with steam to form hydrogen gas.

B Magnesium is more reactive than calcium.

C Potassium reacts with water to form hydrogen gas.

D Sodium oxide is reduced by carbon to sodium. 27 Iron is obtained from its ore in a blast furnace and is used to make steel.

Iron obtained from the blast furnace is contaminated with ......1...... .

In order to remove this substance, ......2...... is passed through the molten iron.

......3...... is also added to remove oxides of phosphorus and silicon which are ......4...... .

Which words complete the sentences about the conversion of iron to steel?

1 2 3 4

A carbon nitrogen calcium carbonate acidic

B carbon oxygen calcium oxide acidic

C carbon oxygen calcium oxide basic

D sand oxygen calcium oxide basic

28 Copper is a transition element used to make saucepans.

Which property is not correct for copper?


B insoluble in water

C low melting point

D malleable (can be hammered into shape)

12

© UCLES 2016 0620/13/M/J/16


air

P Q

water

iron painted iron


tube P tube Q

A falls rises

B no change rises

C rises falls

D rises no change


atmosphere

planet



carbon dioxide 4

nitrogen 72

oxygen 24





D nitrogen only

13


31 The following substances can be formed when petrol is burnt in a car engine.

Which substance is the main cause of acid rain?

A carbon

B carbon monoxide

C nitrogen dioxide

D water 32 Which statement about methane is not correct?

A It is a greenhouse gas.

B It is an alkene.

C It is formed by decomposition of vegetation.

D It is used as a fuel. 33 The formulae of four compounds, W, X Y and Z, are given.

compound formula

W FeSO4

X (NH4)3PO4

Y KNO3

Z NaCl

Which mixture of compounds makes a complete fertiliser?

A W and X B W and Z C X and Y D Y and Z 34 Which process is used to make lime (calcium oxide) from limestone (calcium carbonate)?

A chromatography

B electrolysis

C fractional distillation

D thermal decomposition

14

© UCLES 2016 0620/13/M/J/16


gasoline

X

Y

Z

bitumen

petroleum


X Y Z





36 Which compound does not belong to the same homologous series as the other three

compounds?

A CH3OH B C2H5COOH C C2H5OH D C7H15OH 37 Which reaction is used as a test for alkenes?

A Alkenes burn in air to give carbon dioxide and water.

B Alkenes decolourise aqueous bromine.

C Alkenes form polymers when heated in the presence of a catalyst.

D Alkenes react with steam to form alcohols. 38 Which statement about ethanol is correct?

A It burns in air to form ethene and water.

B It is prepared from ethene by fermentation.

C It is prepared from glucose in an addition reaction.

D It is the only product when ethene reacts with steam.

15



© UCLES 2016 0620/13/M/J/16

39 Ethene forms an addition polymer as shown.

H

C...... +

H

H

C +

H

H

C

H

H

C + ...... ...... ......

H

H

C

H

H

C

H

H

C

H

H

C

H





D an unsaturated compound called poly(ethene) 40 Liquid W burns completely to give carbon dioxide and water.

Liquid W is a compound containing carbon, hydrogen and oxygen.

A solution of liquid W in water is pH 7.

What is liquid W?

A ethanoic acid

B ethanol

C gasoline

D methane

16

© UCLES 2016 0620/13/M/J/16

Gro

up

The

Perio

dic

Tabl

e of

Ele

men

ts

1 Hhy

drog

en1

2 He

heliu

m4

III

IIIIV

VV

IV

IIV

III

3 Lilit

hium 7

4 Be

bery

llium

9

atom

ic n

umbe

r

atom

ic s

ymbo

l

Key

nam

ere

lativ

e at

omic

mas

s

11 Na

sodi

um23

12 Mg

mag

nesi

um24

19 Kpo

tass

ium

39

20 Ca

calc

ium

40

37 Rb

rubi

dium

85

38 Sr

stro

ntiu

m88

55 Cs

caes

ium

133

56 Ba

bariu

m13

7

87 Frfra

nciu

m–

88 Ra

radi

um –

5 B boro

n11 13 Al

alum

iniu

m27 31 Ga

galli

um70 49 In indi

um11

5

81 Tlth

alliu

m20

4

6 Cca

rbon

12 14 Si

silic

on28 32 Ge

germ

aniu

m73 50 Sn tin 119

82 Pb

lead

207

22 Titit

aniu

m48 40 Zr

zirc

oniu

m91 72 Hf

hafn

ium

178

104

Rf

ruth

erfo

rdiu

m–

23 Vva

nadi

um51 41 Nb

niob

ium

93 73 Tata

ntal

um18

1

105

Db

dubn

ium

–

24 Cr

chro

miu

m52 42 Mo

mol

ybde

num

96 74 Wtu

ngst

en18

4

106

Sg

seab

orgi

um–

25 Mn

man

gane

se55 43 Tc

tech

netiu

m– 75 Re

rhen

ium

186

107

Bh

bohr

ium

–

26 Fe iron

56 44 Ru

ruth

eniu

m10

1

76 Os

osm

ium

190

108

Hs

hass

ium

–

27 Co

coba

lt59 45 Rh

rhod

ium

103

77 Iriri

dium

192

109

Mt

mei

tner

ium

–

28 Ni

nick

el59 46 Pd

palla

dium

106

78 Pt

plat

inum

195

110

Ds

darm

stad

tium

–

29 Cu

copp

er64 47 Ag

silv

er10

8

79 Au

gold

197

111

Rg

roen

tgen

ium

–

30 Zn zinc 65 48 Cd

cadm

ium

112

80 Hg

mer

cury

201

112

Cn

cope

rnic

ium

–

114 Fl

flero

vium

–

116

Lvliv

erm

oriu

m–

7 Nni

troge

n14 15 P

phos

phor

us31 33 As

arse

nic

75 51 Sb

antim

ony

122

83 Bi

bism

uth

209

8 Oox

ygen

16 16 S sulfu

r32 34 Se

sele

nium

79 52 Tete

lluriu

m12

8

84 Po

polo

nium

–

9 Fflu

orin

e19 17 Cl

chlo

rine

35.5

35 Br

brom

ine

80 53 Iio

dine

127

85 At

asta

tine

–

10 Ne

neon 20 18 Ar

argo

n40 36 Kr

kryp

ton

84 54 Xe

xeno

n13

1

86 Rn

rado

n–

21 Sc

scan

dium

45 39 Yyt

trium 89

57–7

1la

ntha

noid

s

89–1

03ac

tinoi

ds

57 Lala

ntha

num

139

89 Ac

lant

hano

ids

actin

oids

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3 a

t roo

m te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.)

actin

ium

–

58 Ce

ceriu

m14

0

90 Th thor

ium

232

59 Pr

pras

eody

miu

m14

1

91 Pa

prot

actin

ium

231

60 Nd

neod

ymiu

m14

4

92 Uur

aniu

m23

8

61 Pm

prom

ethi

um– 93 Np

nept

uniu

m–

62 Sm

sam

ariu

m15

0

94 Pu

plut

oniu

m–

63 Eu

euro

pium

152

95 Am

amer

iciu

m–

64 Gd

gado

liniu

m15

7

96 Cm

curiu

m–

65 Tb terb

ium

159

97 Bk

berk

eliu

m–

66 Dy

dysp

rosi

um16

3

98 Cf

calif

orni

um–

67 Ho

holm

ium

165

99 Es

eins

tein

ium

–

68 Er

erbi

um16

7

100

Fm ferm

ium

–

69 Tm thul

ium

169

101

Md

men

dele

vium

–

70 Yb

ytte

rbiu

m17

3

102

No

nobe

lium

–

71 Lu lute

tium

175

103 Lr

law

renc

ium

–

The syllabus is approved for use in England, Wales and Northern Ireland as a Cambridge International Level 1/Level 2 Certificate.



*6622954837*


CHEMISTRY 0620/21

Paper 2 Multiple Choice (Extended) May/June 2016














2

© UCLES 2016 0620/21/M/J/16

1 The rate of diffusion of two gases, methane, CH4, and ethene, C2H4, is measured using the apparatus shown.

constantpressureapplied

gas syringe gasmetal foil – gasescapes throughsmall hole in the foil

Which gas diffuses faster and why?

gas that

diffuses faster reason

A

ethene

Ethene molecules are heavier and so move faster.

B

ethene

Ethene molecules have a double bond which makes them more reactive.

C methane Methane molecules are lighter and so move faster.

D

methane

Methane molecules are smaller so they can get out of the small hole more easily.

2 A sample of a dye is investigated by chromatography.

A line is drawn across a piece of chromatography paper and a spot of the dye is placed on it.

The paper is placed in water.

water

chromatographypaper

linespot of dye

Which row is correct?

what is used to draw the line

position of spot

A ink above the level of the water

B ink below the level of the water

C pencil above the level of the water

D pencil below the level of the water

3


3 The paper chromatogram below was obtained from four different dyes.

Which dye has an Rf value of 0.7?

A B C D

solvent front

baseline

4 Which statements about isotopes of the same element are correct?

1 They are atoms which have the same chemical properties because they have the same number of electrons in their outer shell.

2 They are atoms which have the same number of electrons and neutrons but different numbers of protons.

3 They are atoms which have the same number of electrons and protons but different numbers of neutrons.

A 1 and 2 B 1 and 3 C 2 only D 3 only



W 2,8,1

X 2,8,4

Y 2,8,7

Z 2,8,8


A W and X B W and Y C X and Y D X and Z

4

© UCLES 2016 0620/21/M/J/16

6 Which statement describes the attractive forces between molecules (intermolecular forces)?

A They are strong covalent bonds which hold molecules together.

B They are strong ionic bonds which hold molecules together.

C They are weak forces formed between covalently-bonded molecules.

D They are weak forces which hold ions together in a lattice. 7 The diagram represents the general structure of a solid Z.

+ + +

+ + +

+ + +–

––

– –

––––

What is Z?

A aluminium

B iodine

C silicon dioxide

D sulfur 8 A compound, X, contains 40.0% carbon, 6.7% hydrogen and 53.3% oxygen by mass.

The relative molecular mass, Mr, of X is 60.

What is the molecular formula of X?

A CH2O B CH4O C C2H4O D C2H4O2 9 25 cm3 of 0.1 mol / dm3 hydrochloric acid exactly neutralise 20 cm3 of aqueous sodium hydroxide.

The equation for this reaction is:

NaOH + HCl → NaCl + H2O

What is the concentration of the sodium hydroxide solution?

A 0.080 mol / dm3

B 0.800 mol / dm3

C 0.125 mol / dm3

D 1.25 mol / dm3

5


10 Which reactions could take place at the anode during electrolysis?

1 4OH–(aq) → 2H2O(I) + O2(g) + 4e–

2 2Cl –(aq) → Cl 2(g) + 2e–

3 Cu2+(aq) + 2e– → Cu(s)

4 2H+(aq) + 2e– → H2(g)

A 1 and 2 B 1 and 4 C 2 and 4 D 3 and 4 11 The diagram shows some properties that substances may have.


compoundused as

an energy source

radioactive

A

B D C

12 The diagram shows a simple cell.

voltmeter

copper electrodezinc electrode

electrolyte

V

Which statement about the process occurring when the cell is in operation is correct?

A Cu2+ ions are formed in solution.

B Electrons travel through the solution.

C The reaction Zn → Zn2+ + 2e– occurs.

D The zinc electrode increases in mass.

6

© UCLES 2016 0620/21/M/J/16

13 Hydrogen burns exothermically in oxygen.

The equation for the reaction is:

2H2 + O2 → 2H2O

The table shows the bond energies involved.

bond bond energy in kJ / mol

H–H 436

O=O 498

O–H 464

What is the energy given out during the reaction?

A –3226 kJ / mol

B –884 kJ / mol

C –486 kJ / mol

D –442 kJ / mol

7




XY

X


3 4

Y

XY

XY

stopper

balance

balance

stopper

A 1 and 3 B 1 and 4 C 2 and 3 D 2 and 4 15 Which statements explain why increasing temperature increases the rate of a chemical reaction?

1 Heat makes the molecules move faster and collide more often.

2 Heat makes the molecules collide with more energy so they are more likely to react.

3 Increasing temperature lowers the activation energy for the reaction.


8

© UCLES 2016 0620/21/M/J/16

16 Steam reacts with carbon in an endothermic reaction.

C(s) + H2O(g) CO(g) + H2(g)

Which conditions of temperature and pressure would give the largest yield of hydrogen?

temperature pressure

A high high

B high low

C low high

D low low

17 Which equation represents a reduction reaction?

A Fe2+ + e– → Fe3+

B Fe2+ → Fe3+ + e–

C Fe3+ + e– → Fe2+

D Fe3+ → Fe2+ + e– 18 Which statements are properties of an acid?



1 2

A � �

B � �

C � �

D � �

19 Which row describes whether an amphoteric oxide reacts with acids and bases?

reacts with acids reacts with bases

A no no

B no yes

C yes no

D yes yes

9


20 Which substance reacts with dilute sulfuric acid to form a salt that can be removed from the resulting mixture by filtration?

A aqueous barium chloride

B aqueous sodium hydroxide

C copper

D copper(II) carbonate


left or right


of a group

A left bottom

B left top

C right bottom

D right top

22 Some properties of four elements, P, Q, R and S, are shown in the table.

Two of these elements are in Group I of the Periodic Table and two are in Group VII.

element reaction with water physical state at

room temperature

P reacts vigorously solid

Q does not react with water solid

R reacts explosively solid

S dissolves giving a coloured solution liquid


A P is below R in Group I.

B Q is above R in Group I.

C Q is below S in Group VII.

D R is below S in Group VII.

10

© UCLES 2016 0620/21/M/J/16

23 Which of the following could be a transition element?

melting point

in °C

density in g / cm3 colour

electrical conductor

A 114 4.9 purple no

B 659 2.7 grey yes

C 1677 4.5 grey yes

D 3727 2.3 black yes

24 Two statements about argon are given.

1 Argon has a full outer shell of electrons.

2 Argon is very reactive and is used in lamps.

Which is correct?




D Statement 2 is correct but statement 1 is incorrect. 25 A student investigated the reactions of four metals, R, S, T and U, with solutions of their salts.

The results are given in the table.

metal metal salt result

R

R

S

S nitrate

T nitrate

U nitrate

reacts

reacts

no reaction

T U nitrate reacts

U R nitrate no reaction

What is the order of reactivity of the metals, most reactive first?

A R → S → U → T

B R → T → U → S

C S → U → T→ R

D U → R → T → S

11


26 Three students, X, Y and Z, were told that solid P reacts with dilute acids and also conducts electricity.

The table shows the students’ suggestions about the identity of P.

X Y Z

copper iron graphite

Which of the students are correct?

A X, Y and Z B X only C Y only D Z only 27 Which statement about the uses of metals is correct?

A Aluminium is used in the manufacture of aircraft because of its strength and high density.

B Copper is used in electrical wiring because of its strength and high density.

C Mild steel is used in the manufacture of car bodies because of its strength and resistance to corrosion.

D Stainless steel is used in the construction of chemical plant because of its strength and resistance to corrosion.

28 Aluminium is manufactured by electrolysis of aluminium oxide.

The diagram shows the electrolysis cell.

molten aluminium

aluminium oxidein molten cryolite

cathode

anode

+ +

Which statement about the process is not correct?

A Aluminium ions gain electrons during the electrolysis and are reduced.

B Cryolite is added to reduce the melting point of the aluminium oxide.

C The anode and cathode are made of graphite.

D The cathode has to be replaced regularly because it is burnt away.

12

© UCLES 2016 0620/21/M/J/16


air

P Q

water

iron painted iron


tube P tube Q

A falls rises

B no change rises

C rises falls

D rises no change


atmosphere

planet



carbon dioxide 4

nitrogen 72

oxygen 24





D nitrogen only

13


31 Many car exhaust systems contain a catalytic converter.

Which change does not occur in a catalytic converter?

A carbon dioxide → carbon

B carbon monoxide → carbon dioxide

C nitrogen oxides → nitrogen

D unburnt hydrocarbons → carbon dioxide and water 32 Ammonia is formed by a reversible reaction.

N2(g) + 3H2(g) 2NH3(g)

The forward reaction is exothermic. Which changes in conditions would increase the yield of ammonia?

increase in pressure

increase in temperature

A � �

B � �

C � �

D � �

33 The equation for an exothermic reaction in the Contact process is shown.

2SO2(g) + O2(g) → 2SO3(g)

Which effects do increasing the temperature and using a catalyst have on the rate of formation of sulfur trioxide, SO3?

increasing the temperature

using a catalyst

A rate decreases rate decreases

B rate decreases rate increases

C rate increases rate decreases

D rate increases rate increases

14

© UCLES 2016 0620/21/M/J/16

34 A farmer’s soil is very low in both nitrogen (N) and phosphorus (P).

Which fertiliser would improve the quality of this soil most effectively?

percentage

nitrogen (N) phosphorus (P) potassium (K)

A 11 11 27

B 12 37 10

C 28 10 10

D 31 29 9


gasoline

X

Y

Z

bitumen

petroleum


X Y Z





15


36 Which of the compounds shown are in the same homologous series?

1 CH3OH

2 CH3CH2OH

3 CH3COOH

4 CH3CH2CH2OH

A 1, 2 and 3 B 1, 2 and 4 C 1, 3 and 4 D 2, 3 and 4 37 Which compounds contain the same number of carbon, hydrogen and oxygen atoms?

W X Y Z

ethyl methanoate methyl ethanoate methyl methanoate ethyl ethanoate

A W and X B W and Y C X and Z D Y and Z

38 What is an advantage of producing ethanol by fermentation of sugar compared to the catalytic

addition of steam to ethene?

A The alcohol produced is purer.

B The process is faster.

C The process uses high temperature.

D The process uses renewable raw materials.

16

© UCLES 2016 0620/21/M/J/16

39 The structure of a monomer is shown.

C

Cl

H C H

F

Which polymer can be made from this monomer?

Cl

Cl

Cl

Cl

C C

Cl

Cl

C

Cl

Cl

C

A

H

Cl

H

F

C C

H

Cl

C

H

F

C

B

Cl

Cl

F

F

C C

Cl

Cl

C

F

F

C

C

Cl

F

Cl

F

C C

Cl

F

C

Cl

F

C

D

40 Which formula represents a polyester?

CD

O

C

O

C C

OO

N

H

N

H

N

H

N

H

C

O

NB

H

N

H

C

O

C

O

O

N

H

C

CC

O

C

O

C C

OO

O O O O

A O O O O

17

© UCLES 2016 0620/21/M/J/16

BLANK PAGE

18

© UCLES 2016 0620/21/M/J/16

BLANK PAGE

19



© UCLES 2016 0620/21/M/J/16

BLANK PAGE

20

© UCLES 2016 0620/21/M/J/16

Gro

up

The

Perio

dic

Tabl

e of

Ele

men

ts

1 Hhy

drog

en1

2 He

heliu

m4

III

IIIIV

VV

IV

IIV

III

3 Lilit

hium 7

4 Be

bery

llium

9

atom

ic n

umbe

r

atom

ic s

ymbo

l

Key

nam

ere

lativ

e at

omic

mas

s

11 Na

sodi

um23

12 Mg

mag

nesi

um24

19 Kpo

tass

ium

39

20 Ca

calc

ium

40

37 Rb

rubi

dium

85

38 Sr

stro

ntiu

m88

55 Cs

caes

ium

133

56 Ba

bariu

m13

7

87 Frfra

nciu

m–

88 Ra

radi

um –

5 B boro

n11 13 Al

alum

iniu

m27 31 Ga

galli

um70 49 In indi

um11

5

81 Tlth

alliu

m20

4

6 Cca

rbon

12 14 Si

silic

on28 32 Ge

germ

aniu

m73 50 Sn tin 119

82 Pb

lead

207

22 Titit

aniu

m48 40 Zr

zirc

oniu

m91 72 Hf

hafn

ium

178

104

Rf

ruth

erfo

rdiu

m–

23 Vva

nadi

um51 41 Nb

niob

ium

93 73 Tata

ntal

um18

1

105

Db

dubn

ium

–

24 Cr

chro

miu

m52 42 Mo

mol

ybde

num

96 74 Wtu

ngst

en18

4

106

Sg

seab

orgi

um–

25 Mn

man

gane

se55 43 Tc

tech

netiu

m– 75 Re

rhen

ium

186

107

Bh

bohr

ium

–

26 Fe iron

56 44 Ru

ruth

eniu

m10

1

76 Os

osm

ium

190

108

Hs

hass

ium

–

27 Co

coba

lt59 45 Rh

rhod

ium

103

77 Iriri

dium

192

109

Mt

mei

tner

ium

–

28 Ni

nick

el59 46 Pd

palla

dium

106

78 Pt

plat

inum

195

110

Ds

darm

stad

tium

–

29 Cu

copp

er64 47 Ag

silv

er10

8

79 Au

gold

197

111

Rg

roen

tgen

ium

–

30 Zn zinc 65 48 Cd

cadm

ium

112

80 Hg

mer

cury

201

112

Cn

cope

rnic

ium

–

114 Fl

flero

vium

–

116

Lvliv

erm

oriu

m–

7 Nni

troge

n14 15 P

phos

phor

us31 33 As

arse

nic

75 51 Sb

antim

ony

122

83 Bi

bism

uth

209

8 Oox

ygen

16 16 S sulfu

r32 34 Se

sele

nium

79 52 Tete

lluriu

m12

8

84 Po

polo

nium

–

9 Fflu

orin

e19 17 Cl

chlo

rine

35.5

35 Br

brom

ine

80 53 Iio

dine

127

85 At

asta

tine

–

10 Ne

neon 20 18 Ar

argo

n40 36 Kr

kryp

ton

84 54 Xe

xeno

n13

1

86 Rn

rado

n–

21 Sc

scan

dium

45 39 Yyt

trium 89

57–7

1la

ntha

noid

s

89–1

03ac

tinoi

ds

57 Lala

ntha

num

139

89 Ac

lant

hano

ids

actin

oids

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3 a

t roo

m te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.)

actin

ium

–

58 Ce

ceriu

m14

0

90 Th thor

ium

232

59 Pr

pras

eody

miu

m14

1

91 Pa

prot

actin

ium

231

60 Nd

neod

ymiu

m14

4

92 Uur

aniu

m23

8

61 Pm

prom

ethi

um– 93 Np

nept

uniu

m–

62 Sm

sam

ariu

m15

0

94 Pu

plut

oniu

m–

63 Eu

euro

pium

152

95 Am

amer

iciu

m–

64 Gd

gado

liniu

m15

7

96 Cm

curiu

m–

65 Tb terb

ium

159

97 Bk

berk

eliu

m–

66 Dy

dysp

rosi

um16

3

98 Cf

calif

orni

um–

67 Ho

holm

ium

165

99 Es

eins

tein

ium

–

68 Er

erbi

um16

7

100

Fm ferm

ium

–

69 Tm thul

ium

169

101

Md

men

dele

vium

–

70 Yb

ytte

rbiu

m17

3

102

No

nobe

lium

–

71 Lu lute

tium

175

103 Lr

law

renc

ium

–




*1301766353*


CHEMISTRY 0620/22















2

© UCLES 2016 0620/22/M/J/16

1 The particles of a substance gain energy and change from a regular ordered structure to a disordered structure with large distances between the particles.

Which change of state is described?

A boiling

B evaporation

C melting

D sublimation 2 In the chromatography experiment shown, which label represents the solvent front?

C

D

B

A

3 X is a mixture of colourless compounds. The diagram shows a chromatogram of X and of three

pure compounds, P, Q and R.

X P Q R


A A locating agent was used to develop the chromatogram of X.

B P and R could be present in X.

C P and R have different solubilities in the solvent.

D Q has a greater Rf value than R.

3









W 2,8,1

X 2,8,4

Y 2,8,7

Z 2,8,8


A W and X B W and Y C X and Y D X and Z 6 Which statement describes the attractive forces between molecules (intermolecular forces)?




D They are weak forces which hold ions together in a lattice. 7 Metals consist of a lattice of positive ions in a ‘sea of electrons’.

Why is aluminium malleable?

A Its ions are attracted to the ‘sea of electrons’.

B Its ions are tightly packed together.

C Its ions repel each other.

D Its layers of ions can slide over each other.

4

© UCLES 2016 0620/22/M/J/16

8 A sample of 16.0 g of a metal oxide, MO, is reduced to 12.8 g of the metal, M.

What is the relative atomic mass, Ar, of M?

A 32 B 64 C 80 D 128 9 The equation for the reaction between calcium carbonate and hydrochloric acid is shown.

CaCO3(s) + 2HCl (aq) → CaCl 2(aq) + H2O(l) + CO2(g)

How many moles of calcium carbonate will give 24 cm3 of carbon dioxide when reacted with an excess of the acid?

A 1 mol B 0.1 mol C 0.01 mol D 0.001 mol

10 The diagram shows the electrolysis of molten zinc chloride, ZnCl 2.

electrode Yelectrode X

molten zincchloride

+ –


A Oxidation occurs at electrode X and the equation is: 2Cl – → Cl 2 + 2e–.

B Oxidation occurs at electrode Y and the equation is: Zn2+ + 2e– → Zn.

C Reduction occurs at electrode X and the equation is: Zn2+ + 2e– → Zn.

D Reduction occurs at electrode Y and the equation is: 2Cl – → Cl 2 + 2e–.

5




compoundused as

an energy source

radioactive

A

B D C


dilutesulfuric acid

metal Ymetal X

flow of electrons

wire

For which pair of metals would electrons flow from metal X to metal Y?

X Y

A copper iron

B copper zinc

C iron zinc

D zinc iron

6

© UCLES 2016 0620/22/M/J/16

13 The energy level diagram for the combustion of methane is shown.

CH4(g) + 2O2(g)

CO2(g) + 2H2O(g)

energy energy change

Which row gives the equation and energy change for this reaction?

equation energy change in kJ / mol

A CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) +891

B CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) –891

C CH4(g) + 2O2(g) → CO2(g) + 2H2O(I) +891

D CH4(g) + 2O2(g) → CO2(g) + 2H2O(I) –891

7




XY

X


3 4

Y

XY

XY

stopper

balance

balance

stopper

A 1 and 3 B 1 and 4 C 2 and 3 D 2 and 4 15 Which row describes how the energy of collision between particles changes when concentration

and temperature are increased?

concentration temperature

A increases increases

B increases no change

C no change increases

D no change no change

8

© UCLES 2016 0620/22/M/J/16

16 Methanol is made by reacting carbon monoxide with hydrogen.

The reaction is exothermic and is a chemical equilibrium.


CO(g) + 2H2(g) CH3OH(g)

Which changes in temperature and pressure increase the yield of methanol?

temperature pressure

A decrease decrease

B decrease increase

C increase decrease

D increase increase

17 Which equation represents a reduction reaction?

A Fe2+ + e– → Fe3+

B Fe2+ → Fe3+ + e–

C Fe3+ + e– → Fe2+




1 2

A � �

B � �

C � �

D � �

9




A no no

B no yes

C yes no

D yes yes

20 Silver chloride is insoluble in water and is prepared by precipitation.

Which two substances can be used to make silver chloride?

A barium chloride and silver nitrate

B hydrochloric acid and silver

C hydrochloric acid and silver bromide

D sodium chloride and silver iodide 21 Where in the Periodic Table is the metallic character of the elements greatest?

left or right


of a group

A left bottom

B left top

C right bottom

D right top

22 Rubidium is a Group I metal.

Which statement about rubidium is not correct?

A It has a higher melting point than lithium.

B It has one electron in its outer shell.

C It reacts vigorously with water.

D It reacts with chlorine to form rubidium chloride, RbCl .

10

© UCLES 2016 0620/22/M/J/16

23 The table gives information about four elements, P, Q, R and S.

melting point

in °C

electrical conductivity of element when solid

density in g / cm3 colour of iodide

of element

P 98 good 0.97 white

Q –39 good 13.53 red

R 1410 poor 2.33 colourless

S 1535 good 7.87 green

Which elements could be transition elements?

A P, Q and S B Q and S only C R and S only D S only 24 Part of the Periodic Table is shown.

Which element is a gas that does not form a compound with potassium?

A BC D

25 Some magnesium compounds undergo thermal decomposition.

What are the products of thermal decomposition of magnesium nitrate, Mg(NO3)2, and magnesium hydroxide, Mg(OH)2?

Mg(NO3)2 Mg(OH)2

A MgO, NO2 and O2 MgO and H2O

B MgO, NO2 and O2 MgO and H2

C Mg(NO2)2 and O2 MgO and H2O

D Mg(NO2)2 and O2 MgO and H2

26 Which property is not considered a typical metallic property?


B low melting point

C malleable (can be hammered into shape)

D strong

11


27 Iron from a blast furnace is treated with oxygen and with calcium oxide to make steel.

Which substances in the iron are removed?

oxygen removes calcium oxide

removes

A carbon acidic oxides

B carbon basic oxides

C iron acidic oxides

D iron basic oxides

28 Why is cryolite used during the extraction of aluminium by electrolysis?

A It is a catalyst for the reaction.

B It lowers the melting point of the electrolyte.

C It protects the anodes.

D It separates the aluminium from the electrolyte. 29 The diagram shows an experiment to investigate how paint affects the rusting of iron.

air

P Q

water

iron painted iron


tube P tube Q

A falls rises

B no change rises

C rises falls

D rises no change

12

© UCLES 2016 0620/22/M/J/16


atmosphere

planet



carbon dioxide 4

nitrogen 72

oxygen 24





D nitrogen only 31 The gases coming from a car’s engine contain oxides of nitrogen.

How are these oxides formed?

A Nitrogen reacts with carbon dioxide.

B Nitrogen reacts with carbon monoxide.

C Nitrogen reacts with oxygen.

D Nitrogen reacts with petrol.

13


32 Ammonia is manufactured by a reversible reaction.

N2(g) + 3H2(g) 2NH3(g)

The forward reaction is exothermic.

What is the effect of increasing the pressure on the percentage yield and rate of formation of ammonia?

percentage yield rate of

formation

A decreases decreases

B decreases increases

C increases decreases

D increases increases

33 The Contact process is used for the manufacture of sulfuric acid.

Which statement about this process is not correct?

A A catalyst of iron is used.

B Oxygen from the air is used to react with sulfur dioxide.

C Sulfur trioxide dissolves in sulfuric acid to form oleum.

D The temperature used is around 450 °C. 34 Lime (calcium oxide) is used to treat waste water from a factory.

Which substance is removed by the lime?

A ammonia

B sodium chloride

C sodium hydroxide

D sulfuric acid

14

© UCLES 2016 0620/22/M/J/16


gasoline

X

Y

Z

bitumen

petroleum


X Y Z





36 Which compound is not an alkane, CnH2n+2?

A CH3CH2CH2CH3

B (CH3)2CHCH3

C CH3CHCHCH3

D (CH3)3CH 37 An ester is formed when a carboxylic acid reacts with an alcohol.

Which ester is formed when propanoic acid and ethanol react?

A CH3CO2CH2CH3

B CH3CO2CH2CH2CH3

C CH3CH2CO2CH3

D CH3CH2CO2CH2CH3

15



© UCLES 2016 0620/22/M/J/16

38 What is an advantage of producing ethanol by fermentation of sugar compared to the catalytic addition of steam to ethene?




D The process uses renewable raw materials. 39 In which row are the monomer and polymer chain correctly matched?

monomer part of the polymer chain

A CH3CH=CHCH3 –CH(CH3)–CH(CH3)–CH(CH3)–CH(CH3)–

B CH2=CHCl –CHCl –CHCl –CHCl –CHCl –

C CH3CH=CH2 –CH3–CH–CH2–CH3–CH–CH2–

D CH2=CHCH2CH3 –CH2–CH2–CH2–CH(CH2CH3)–

40 Which two polymers have the same linkages bonding the monomers together?

A nylon and complex carbohydrate

B nylon and protein

C Terylene and complex carbohydrate

D Terylene and protein

16

© UCLES 2016 0620/22/M/J/16

Gro

up

The

Perio

dic

Tabl

e of

Ele

men

ts

1 Hhy

drog

en1

2 He

heliu

m4

III

IIIIV

VV

IV

IIV

III

3 Lilit

hium 7

4 Be

bery

llium

9

atom

ic n

umbe

r

atom

ic s

ymbo

l

Key

nam

ere

lativ

e at

omic

mas

s

11 Na

sodi

um23

12 Mg

mag

nesi

um24

19 Kpo

tass

ium

39

20 Ca

calc

ium

40

37 Rb

rubi

dium

85

38 Sr

stro

ntiu

m88

55 Cs

caes

ium

133

56 Ba

bariu

m13

7

87 Frfra

nciu

m–

88 Ra

radi

um –

5 B boro

n11 13 Al

alum

iniu

m27 31 Ga

galli

um70 49 In indi

um11

5

81 Tlth

alliu

m20

4

6 Cca

rbon

12 14 Si

silic

on28 32 Ge

germ

aniu

m73 50 Sn tin 119

82 Pb

lead

207

22 Titit

aniu

m48 40 Zr

zirc

oniu

m91 72 Hf

hafn

ium

178

104

Rf

ruth

erfo

rdiu

m–

23 Vva

nadi

um51 41 Nb

niob

ium

93 73 Tata

ntal

um18

1

105

Db

dubn

ium

–

24 Cr

chro

miu

m52 42 Mo

mol

ybde

num

96 74 Wtu

ngst

en18

4

106

Sg

seab

orgi

um–

25 Mn

man

gane

se55 43 Tc

tech

netiu

m– 75 Re

rhen

ium

186

107

Bh

bohr

ium

–

26 Fe iron

56 44 Ru

ruth

eniu

m10

1

76 Os

osm

ium

190

108

Hs

hass

ium

–

27 Co

coba

lt59 45 Rh

rhod

ium

103

77 Iriri

dium

192

109

Mt

mei

tner

ium

–

28 Ni

nick

el59 46 Pd

palla

dium

106

78 Pt

plat

inum

195

110

Ds

darm

stad

tium

–

29 Cu

copp

er64 47 Ag

silv

er10

8

79 Au

gold

197

111

Rg

roen

tgen

ium

–

30 Zn zinc 65 48 Cd

cadm

ium

112

80 Hg

mer

cury

201

112

Cn

cope

rnic

ium

–

114 Fl

flero

vium

–

116

Lvliv

erm

oriu

m–

7 Nni

troge

n14 15 P

phos

phor

us31 33 As

arse

nic

75 51 Sb

antim

ony

122

83 Bi

bism

uth

209

8 Oox

ygen

16 16 S sulfu

r32 34 Se

sele

nium

79 52 Tete

lluriu

m12

8

84 Po

polo

nium

–

9 Fflu

orin

e19 17 Cl

chlo

rine

35.5

35 Br

brom

ine

80 53 Iio

dine

127

85 At

asta

tine

–

10 Ne

neon 20 18 Ar

argo

n40 36 Kr

kryp

ton

84 54 Xe

xeno

n13

1

86 Rn

rado

n–

21 Sc

scan

dium

45 39 Yyt

trium 89

57–7

1la

ntha

noid

s

89–1

03ac

tinoi

ds

57 Lala

ntha

num

139

89 Ac

lant

hano

ids

actin

oids

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3 a

t roo

m te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.)

actin

ium

–

58 Ce

ceriu

m14

0

90 Th thor

ium

232

59 Pr

pras

eody

miu

m14

1

91 Pa

prot

actin

ium

231

60 Nd

neod

ymiu

m14

4

92 Uur

aniu

m23

8

61 Pm

prom

ethi

um– 93 Np

nept

uniu

m–

62 Sm

sam

ariu

m15

0

94 Pu

plut

oniu

m–

63 Eu

euro

pium

152

95 Am

amer

iciu

m–

64 Gd

gado

liniu

m15

7

96 Cm

curiu

m–

65 Tb terb

ium

159

97 Bk

berk

eliu

m–

66 Dy

dysp

rosi

um16

3

98 Cf

calif

orni

um–

67 Ho

holm

ium

165

99 Es

eins

tein

ium

–

68 Er

erbi

um16

7

100

Fm ferm

ium

–

69 Tm thul

ium

169

101

Md

men

dele

vium

–

70 Yb

ytte

rbiu

m17

3

102

No

nobe

lium

–

71 Lu lute

tium

175

103 Lr

law

renc

ium

–




*0872645576*


CHEMISTRY 0620/23















2

© UCLES 2016 0620/23/M/J/16

1 The diagram shows an experiment to demonstrate diffusion.

cotton wool soaked inhydrochloric acid

cotton wool soaked inammonia solution

ammoniumchloride

Which statement explains why the ring of ammonium chloride appears as shown?

A Ammonia solution only produces a gas which moves until it meets the hydrochloric acid.

B Both solutions produce a gas, but ammonia moves quicker than hydrogen chloride because it is lighter.

C Hydrochloric acid produces hydrogen chloride which stays at one end of the tube until the ammonia reaches it.

D The two solutions run along the tube until they meet.

2 Chromatography experiments are carried out on four substances, P, Q, R and S.

The same solvent is used in each experiment.

The resulting chromatograms are shown below.

P Q R S

baseline


A P and Q are pure substances.

B P and R are different substances.

C R and S are pure substances.

D S is a mixture of substances.

3


3 The diagram shows the apparatus used to separate the different components of a mixture by chromatography.

baseline

solvent

spot

solvent front

chromatography paper

Which statement about this experiment is correct?

A A locating agent is used to find the position of the solvent front.

B The components to be separated must be soluble in the solvent.

C The baseline on which the spot of the mixture is placed is drawn in ink.

D The Rf value is calculated by component theby travelled distance the

front solvent theby travelled distance the






4

© UCLES 2016 0620/23/M/J/16



W 2,8,1

X 2,8,4

Y 2,8,7

Z 2,8,8


A W and X B W and Y C X and Y D X and Z 6 Which statement describes the attractive forces between molecules (intermolecular forces)?




D They are weak forces which hold ions together in a lattice. 7 Which substance exists as a lattice of positive ions in a ‘sea of electrons’?

A liquid potassium chloride

B solid graphite

C solid magnesium

D solid silicon(IV) oxide

8 Analysis of a compound formed between magnesium and nitrogen showed it contained 14.4 g of

magnesium and 5.6 g of nitrogen.

What is the empirical formula of the compound?

A Mg2N3 B Mg3N2 C Mg4N6 D Mg6N4 9 An excess of zinc is added to 100 cm3 of 1.0 mol / dm3 hydrochloric acid. The equation for the reaction is:

Zn + 2HCl → ZnCl 2 + H2

What is the maximum volume of hydrogen evolved at room temperature and pressure?

A 1.2 dm3 B 2.0 dm3 C 2.4 dm3 D 24 dm3

5


10 The diagram shows a method used to copper-plate a pan

pan

copper(II) sulfatesolution

copper

+ –

Which equation represents the reaction at the cathode?

A Cu2+ + 2e– → Cu

B 2H+ + 2e– → H2

C 4OH– → O2 + 2H2O + 4e–

D 2O2– → O2 + 4e– 11 The diagram shows some properties that substances may have.


compoundused as

an energy source

radioactive

A

B D C

6

© UCLES 2016 0620/23/M/J/16


dilutesulfuric acid

metal Qmetal P

wire

V

Which pair of metals produces the largest voltage?

metal P metal Q

A iron copper

B magnesium copper

C magnesium zinc

D zinc copper

13 Hydrazine, N2H4, decomposes as shown.

N

H

H

N N N H2+ H

H

H

The energy change for this reaction is –95 kJ / mol.

The table shows some bond energies involved.

bond bond energy in kJ / mol

N N 945

N–H 391

H–H 436

What is the bond energy of the N–N bond?

A 158 kJ / mol B 315 kJ / mol C 348 kJ / mol D 895 kJ / mol

7




XY

X


3 4

Y

XY

XY

stopper

balance

balance

stopper

A 1 and 3 B 1 and 4 C 2 and 3 D 2 and 4 15 Which row explains why increasing temperature increases the rate of reaction?

particles collide

more often particles collide

with more energy

A � �

B � �

C � �

D � �

8

© UCLES 2016 0620/23/M/J/16

16 Methanol is manufactured by reacting carbon monoxide and hydrogen together in the presence of an aluminium oxide catalyst.


CO(g) + 2H2(g) CH3OH(g)

The reaction is a reversible reaction.

The forward reaction is exothermic.

Which change in conditions increases the yield of methanol?

A decreasing the concentration of the carbon monoxide

B increasing the pressure

C increasing the rate of the reaction

D increasing the temperature 17 Which equation represents a reduction reaction?

A Fe2+ + e– → Fe3+

B Fe2+ → Fe3+ + e–

C Fe3+ + e– → Fe2+




1 2

A � �

B � �

C � �

D � �

9




A no no

B no yes

C yes no

D yes yes

20 Barium sulfate is an insoluble salt.

It can be made by reacting copper(II) sulfate solution with barium nitrate solution.

CuSO4(aq) + Ba(NO3)2(aq) → Cu(NO3)2(aq) + BaSO4(s)

What is the correct order of steps to obtain a pure, dry sample of barium sulfate from the reaction mixture?

step 1 step 2 step 3

A

filter

evaporate the filtrate to dryness

leave the solid formed to cool

B

filter

evaporate the filtrate to the point of crystallisation

leave the filtrate to cool

C

filter

leave the residue in a warm place to dry

wash the residue with water

D

filter

wash the residue with water

leave the residue in a warm place to dry


left or right


of a group

A left bottom

B left top

C right bottom

D right top

10

© UCLES 2016 0620/23/M/J/16

22 Which statement about the elements in Group I is correct?

A Hydrogen is evolved when they react with water.

B Ions of Group I elements have a –1 charge.

C Sodium is more reactive than potassium.

D Solid sodium is a poor electrical conductor. 23 Osmium is a transition element.

Which row gives the expected properties of osmium?

melting point density compounds

formed

A high high coloured

B high high white

C high low white

D low high coloured

24 Two statements about noble gases are given. 1 Noble gases are reactive, monatomic gases.

2 Noble gases all have full outer shells of electrons.

Which is correct?




D Statement 2 is correct but statement 1 is incorrect.

11


25 Some properties of substance X are listed.

● It conducts electricity when molten.

● It has a high melting point.

● It burns in oxygen and the product dissolves in water to give a solution with pH 11.

What is X?

A a covalent compound

B a macromolecule

C a metal

D an ionic compound 26 Four metals P, Q, R and S are added to separate aqueous solutions of their ions.

The results are shown.

metal P2+ Q2+ R2+ S2+

P � � � � key

Q � � � � �= reaction occurs

R � � � � �= reaction does not occur

S � � � �

What is the order of reactivity of the metals, most reactive first?

A Q → P → S → R

B Q → S → P → R

C R → P → S → Q

D R → S → P → Q 27 Copper is a transition element used to make saucepans.

Which property is not correct for copper?


B insoluble in water

C low melting point

D malleable (can be hammered into shape)

12

© UCLES 2016 0620/23/M/J/16

28 Aluminium is extracted by electrolysis of a mixture of aluminium oxide and cryolite.


A The electrodes are made from graphite.

B The formula for aluminium oxide is Al 2O3.

C The purpose of the cryolite is to lower the melting point of the mixture.

D The reaction taking place at the anode is Al 3+ + 3e– → Al . 29 The diagram shows an experiment to investigate how paint affects the rusting of iron.

air

P Q

water

iron painted iron


tube P tube Q

A falls rises

B no change rises

C rises falls

D rises no change

13



atmosphere

planet



carbon dioxide 4

nitrogen 72

oxygen 24





D nitrogen only 31 Catalytic converters are used to remove some gaseous pollutants from car exhaust fumes.

Which gas is removed from the fumes by oxidation?

A carbon dioxide

B carbon monoxide

C nitrogen

D nitrogen oxide 32 Ammonia is produced by the Haber process.

N2(g) + 3H2(g) → 2NH3(g).

Which statement about the Haber process is not correct?

A An iron catalyst is used to increase the rate of reaction.

B The reaction is carried out at high temperature to increase the rate of reaction.

C The reaction is carried out at low pressure to increase the yield of ammonia.

D The reaction is reversible.

14

© UCLES 2016 0620/23/M/J/16

33 One step in the manufacture of sulfuric acid is the oxidation of sulfur dioxide to sulfur trioxide.

Which conditions are used for this step?

temperature

/ °C

pressure / atmospheres

catalyst

A 450 1.5 iron

B 450 1.5 vanadium(V) oxide

C 450 200 iron

D 450 200 vanadium(V) oxide

34 Which process is used to make lime (calcium oxide) from limestone (calcium carbonate)?

A chromatography

B electrolysis

C fractional distillation

D thermal decomposition 35 The diagram shows the separation of petroleum into fractions.

gasoline

X

Y

Z

bitumen

petroleum


X Y Z





15


36 Which compound does not belong to the same homologous series as the other three compounds?

A CH3OH B C2H5COOH C C2H5OH D C7H15OH 37 The structure of an alkene and the structure of an ester are shown.

C

H

H

C

H

H

H

C

H

H

C

H

H

HCC

H

C

H

H

H

CC

H

C

H

H

H

O

O

P Q

What are the names of P and Q?

P Q

A but-1-ene ethyl propanoate

B but-1-ene propyl ethanoate

C but-2-ene ethyl propanoate

D but-2-ene propyl ethanoate

38 What is an advantage of producing ethanol by fermentation of sugar compared to the catalytic

addition of steam to ethene?




D The process uses renewable raw materials.

16

© UCLES 2016 0620/23/M/J/16

39 A polymer has the formula shown.

n

C

CH3

COOH

C

H

H

From which monomers can it be formed?

C

H

H

C

COOH

CH3

R

C

H

H

C

COOH

CH3

S

C

H

H

C

COOH

CH3

T

C

H

H

C

COOH

CH3

U

A R and S B R and T C S and U D T and U 40 Which row shows a natural polymer with the same linkages as a synthetic polymer?

natural polymer synthetic polymer

A complex carbohydrate nylon

B complex carbohydrate Terylene

C protein nylon

D protein Terylene

17

© UCLES 2016 0620/23/M/J/16

BLANK PAGE

18

© UCLES 2016 0620/23/M/J/16

BLANK PAGE

19



© UCLES 2016 0620/23/M/J/16

BLANK PAGE

20

© UCLES 2016 0620/23/M/J/16

Gro

up

The

Perio

dic

Tabl

e of

Ele

men

ts

1 Hhy

drog

en1

2 He

heliu

m4

III

IIIIV

VV

IV

IIV

III

3 Lilit

hium 7

4 Be

bery

llium

9

atom

ic n

umbe

r

atom

ic s

ymbo

l

Key

nam

ere

lativ

e at

omic

mas

s

11 Na

sodi

um23

12 Mg

mag

nesi

um24

19 Kpo

tass

ium

39

20 Ca

calc

ium

40

37 Rb

rubi

dium

85

38 Sr

stro

ntiu

m88

55 Cs

caes

ium

133

56 Ba

bariu

m13

7

87 Frfra

nciu

m–

88 Ra

radi

um –

5 B boro

n11 13 Al

alum

iniu

m27 31 Ga

galli

um70 49 In indi

um11

5

81 Tlth

alliu

m20

4

6 Cca

rbon

12 14 Si

silic

on28 32 Ge

germ

aniu

m73 50 Sn tin 119

82 Pb

lead

207

22 Titit

aniu

m48 40 Zr

zirc

oniu

m91 72 Hf

hafn

ium

178

104

Rf

ruth

erfo

rdiu

m–

23 Vva

nadi

um51 41 Nb

niob

ium

93 73 Tata

ntal

um18

1

105

Db

dubn

ium

–

24 Cr

chro

miu

m52 42 Mo

mol

ybde

num

96 74 Wtu

ngst

en18

4

106

Sg

seab

orgi

um–

25 Mn

man

gane

se55 43 Tc

tech

netiu

m– 75 Re

rhen

ium

186

107

Bh

bohr

ium

–

26 Fe iron

56 44 Ru

ruth

eniu

m10

1

76 Os

osm

ium

190

108

Hs

hass

ium

–

27 Co

coba

lt59 45 Rh

rhod

ium

103

77 Iriri

dium

192

109

Mt

mei

tner

ium

–

28 Ni

nick

el59 46 Pd

palla

dium

106

78 Pt

plat

inum

195

110

Ds

darm

stad

tium

–

29 Cu

copp

er64 47 Ag

silv

er10

8

79 Au

gold

197

111

Rg

roen

tgen

ium

–

30 Zn zinc 65 48 Cd

cadm

ium

112

80 Hg

mer

cury

201

112

Cn

cope

rnic

ium

–

114 Fl

flero

vium

–

116

Lvliv

erm

oriu

m–

7 Nni

troge

n14 15 P

phos

phor

us31 33 As

arse

nic

75 51 Sb

antim

ony

122

83 Bi

bism

uth

209

8 Oox

ygen

16 16 S sulfu

r32 34 Se

sele

nium

79 52 Tete

lluriu

m12

8

84 Po

polo

nium

–

9 Fflu

orin

e19 17 Cl

chlo

rine

35.5

35 Br

brom

ine

80 53 Iio

dine

127

85 At

asta

tine

–

10 Ne

neon 20 18 Ar

argo

n40 36 Kr

kryp

ton

84 54 Xe

xeno

n13

1

86 Rn

rado

n–

21 Sc

scan

dium

45 39 Yyt

trium 89

57–7

1la

ntha

noid

s

89–1

03ac

tinoi

ds

57 Lala

ntha

num

139

89 Ac

lant

hano

ids

actin

oids

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3 a

t roo

m te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.)

actin

ium

–

58 Ce

ceriu

m14

0

90 Th thor

ium

232

59 Pr

pras

eody

miu

m14

1

91 Pa

prot

actin

ium

231

60 Nd

neod

ymiu

m14

4

92 Uur

aniu

m23

8

61 Pm

prom

ethi

um– 93 Np

nept

uniu

m–

62 Sm

sam

ariu

m15

0

94 Pu

plut

oniu

m–

63 Eu

euro

pium

152

95 Am

amer

iciu

m–

64 Gd

gado

liniu

m15

7

96 Cm

curiu

m–

65 Tb terb

ium

159

97 Bk

berk

eliu

m–

66 Dy

dysp

rosi

um16

3

98 Cf

calif

orni

um–

67 Ho

holm

ium

165

99 Es

eins

tein

ium

–

68 Er

erbi

um16

7

100

Fm ferm

ium

–

69 Tm thul

ium

169

101

Md

men

dele

vium

–

70 Yb

ytte

rbiu

m17

3

102

No

nobe

lium

–

71 Lu lute

tium

175

103 Lr

law

renc

ium

–

Cambridge International ExaminationsCambridge International General Certificate of Secondary Education

0620/31May/June 2016

1 hour 15 minutes

CHEMISTRYPaper 3 Theory (Core)

Candidates answer on the Question Paper.

Additional Materials: No Additional Materials are required.


Write your Centre number, candidate number and name on all the work you hand in.Write in dark blue or black pen.You may use an HB pencil for any diagrams or graphs.Do not use staples, paper clips, glue or correction fluid.DO NOTWRITE IN ANY BARCODES.

Answer all questions.Electronic calculators may be used.A copy of the Periodic Table is printed on page 20.You may lose marks if you do not show your working or if you do not use appropriate units.

At the end of the examination, fasten all your work securely together.The number of marks is given in brackets [ ] at the end of each question or part question.



[Turn over06_0620_31_2016_1.11© UCLES 2016

*3293960889*

The structures of some substances containing chlorine are shown.1

Cl − K+ Cl − K+

K+ Cl − K+ Cl −

Cl − K+ Cl − K+Cl

Cl

C

A B

D E

C

Cl Cl

Cl Cl

Cl

Cl

ClCl

Cl

Al

Cl

Cl

Al

ClC

H H F

H F

C C F

Answer the following questions about these substances.(a)

Which substance is a diatomic molecule?(i)

................................................................................................................................ [1]

Which substance represents part of an ionic structure?(ii)

................................................................................................................................ [1]

Which substance is an element?

Explain your answer.

(iii)

................................................................................................................................

................................................................................................................................ [2]

Determine the simplest formula for substance D.(iv)

................................................................................................................................ [1]

06_0620_31_2016_1.11© UCLES 2016

2

The symbols for two isotopes of chlorine are shown.(b)

Cl Cl

How do these two isotopes differ in their atomic structure?(i)

................................................................................................................................ [1]

Determine the number of neutrons present in one atom of the isotope Cl .(ii)

................................................................................................................................ [1]

Draw the electronic structure of a chlorine atom. Show all shells and all electrons.(iii)

[2]

[Total: 9]

[Turn over06_0620_31_2016_1.11© UCLES 2016

3

A bicycle maker wants to choose a suitable material to make bicycle frames.The table shows the properties of some materials that could be used.

2

cost per tonnein $ / tonne

resistance tocorrosion

densityin g / cm3

relativestrength

material

1500very good2.78aluminium

450poor7.921iron

600very good7.924stainlesssteel

15000very good4.527titanium

1300good7.114zinc

Which material is the most suitable for making the bicycle frame?

Explain your answer using information from the table.

(a)

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

........................................................................................................................................... [3]

Aluminium is extracted from aluminium oxide by electrolysis.(b)

State the name of the main ore of aluminium.(i)

................................................................................................................................ [1]

Suggest why aluminium is extracted by electrolysis and not by reduction with carbon.(ii)

................................................................................................................................ [1]

Molten aluminium oxide is electrolysed using graphite electrodes.

Predict the products of this electrolysis at

(iii)

the positive electrode (anode), ..............................................................................

the negative electrode (cathode). ........................................................................ [2]

06_0620_31_2016_1.11© UCLES 2016

4

The diagram shows the changes of state when zinc vapour is cooled slowly to room temperature.(c)

zincvapour

moltenzinc

solidzinc

condensation freezing(solidification)

Explain what happens during these changes in terms of

• the distance between the particles,

• the type of motion shown by the particles.

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

........................................................................................................................................... [4]

[Total: 11]

[Turn over06_0620_31_2016_1.11© UCLES 2016

5

The table shows some properties of the Group I metals.3

boiling point/ ºC

melting point/ ºC

densityin g / cm3

metal

13421810.53lithium

88398sodium

760630.86potassium

686391.53rubidium

66929caesium

Describe the trend in boiling points of the Group I metals.(i)(a)

................................................................................................................................ [1]

Predict the density of caesium.(ii)

................................................................................................................................ [1]

Deduce the state of caesium at 20 ºC.


(iii)

................................................................................................................................

................................................................................................................................ [2]

Complete the word equation for the reaction of rubidium with water.(b)

[2]rubidium + water → ............................................. + .............................................

06_0620_31_2016_1.11© UCLES 2016

6

The dye, indigotin, is formed when compound F is exposed to air.The structure of compound F is shown below.

(c)

C N

CC C C

C C CH

O– Na+

H

H

H

H H

Complete the table and calculate the relative molecular mass of compound F.

atomic massnumber of atomstype of atom

8 12 96128carbon

hydrogen

1 14 14141nitrogen

1 16 16161oxygen

sodium

relative molecular mass = .............................................. [2]

[Turn over06_0620_31_2016_1.11© UCLES 2016

7

Three dye mixtures, J, K and L, were spotted onto a piece of chromatography paper. Threepure dyes, X, Y and Z, were also spotted onto the same piece of paper.

(d)

The diagram shows the results of this chromatography.

J K L X Y Z

Suggest why the base line was drawn in pencil and not in ink.(i)

................................................................................................................................ [1]

Which dye mixture, J, K or L, contains a dye which did not move during thischromatography?

(ii)

................................................................................................................................ [1]

Which dye mixture, J, K or L, contains both dye X and dye Y?(iii)

................................................................................................................................ [1]

Which dye mixture, J, K or L, does not contain dye Z?(iv)

................................................................................................................................ [1]

[Total: 12]

06_0620_31_2016_1.11© UCLES 2016

8

The structures of some organic compounds are shown.4

C

C

P

H H

H HH

H

HH

H

HC C

C C

CH

H

H

C

Q

H

H

H

C

H

CH

H

H

C

R

H H

H

C

H

S

CH

H

H

C

T

H

H

H

CH

H

H

C

H

H

H

C

H

O

H

CH

H

H

C

H

H

H

C

H

O

H

C

H

H

U

Which two of these compounds are alcohols?


(i)(a)

................................................................................................................................

................................................................................................................................ [2]

Which two of these compounds are saturated hydrocarbons?(ii)

................................................................................................................................ [1]

Methanol and ethanol are alcohols in the same homologous series.

Complete the following sentence about a homologous series using words from the list.

(b)

elementscompoundschemicalalcohols

physicalmixturesfunctional

[3]

A homologous series is a family of similar .......................................... with similar

.......................................... properties due to the same .......................................... group.

[Turn over06_0620_31_2016_1.11© UCLES 2016

9

Ethene is an alkene.(c)

Draw the structure of ethene showing all atoms and all bonds.(i)

[1]

Describe how aqueous bromine is used to show that ethene is an unsaturatedcompound.

(ii)

................................................................................................................................

................................................................................................................................ [2]

Ethene is manufactured by cracking.

State the conditions needed for cracking.

(iii)

................................................................................................................................ [1]

Complete the chemical equation for the cracking of hexadecane, C16H34 , to form propeneand one other hydrocarbon.

(iv)

[1]C16H34 → C3H6 + .........................

[Total: 11]

06_0620_31_2016_1.11© UCLES 2016

10

The Group VII elements are called the halogens.5

Describe the trends in

• the physical properties of the halogens,

• the reactivity of halogens with other halide ions.

Include a relevant word equation in your answer.

(a)

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

........................................................................................................................................... [5]

Iodine reacts with hot concentrated nitric acid.(b)

I2 10HNO3 2HIO3 4H2O 10NO2

Explain why this reaction could have an adverse effect on health if not carried out in afume cupboard.

(i)

................................................................................................................................

................................................................................................................................ [2]

Nitric acid is strongly acidic.

Which one of the following pH values represents a strongly acidic solution?

Put a ring around the correct answer.

(ii)

pH 13DpH 9CpH 7BpH 1A

[1]

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11

Nitric acid reacts with zinc oxide.

State the names of the products of this reaction.

(iii)

[2]............................................ and ............................................

[Total: 10]

Ammonia is manufactured by the reaction of nitrogen with hydrogen in the presence of a catalyst.6

What is the purpose of a catalyst?(a)

........................................................................................................................................... [1]

The reaction is reversible.

Complete the equation below by adding the sign for a reversible reaction.

(b)

2NH3N2 + 3H2

[1]

The energy level diagram for this reaction is shown.

Is this reaction exothermic or endothermic?

Give a reason for your answer.

(c)

energy

N2 + 3H2

2NH3

...........................................................................................................................................

........................................................................................................................................... [1]

06_0620_31_2016_1.11© UCLES 2016

12

The graph shows how the percentage yield of ammonia changes with temperature when thepressure is kept constant.

(d)

100

80

60

40

20

00 100 200 300 400

temperature / °C

500 600 700

% yieldof ammonia

Describe how the percentage yield of ammonia changes with temperature.(i)

................................................................................................................................ [1]

Determine the percentage yield of ammonia at 350 ºC.(ii)

................................................................................................................................ [1]

Describe a test for ammonia.(e)

test.....................................................................................................................................

result.................................................................................................................................. [2]

[Turn over06_0620_31_2016_1.11© UCLES 2016

13

Ammonia is a weak base.

Describe how you would measure the pH of an aqueous solution of a weak base using UniversalIndicator.

(f)

...........................................................................................................................................

........................................................................................................................................... [2]

Complete the chemical equation for the reaction of ammonia with chlorine.(g)

[2]........NH3 + 3Cl2 → N2 + ......HCl

[Total: 11]

Calcium carbonate reacts with dilute hydrochloric acid.7

CaCO3(s) + 2HCl(aq) → CaCl2(aq) + CO2(g) + H2O(I)

A student investigated this reaction by measuring the volume of carbon dioxide released everyminute at constant temperature.

Draw a diagram of the apparatus that the student could use to investigate this reaction.(a)

[2]

06_0620_31_2016_1.11© UCLES 2016

14

The graph shows the results of this reaction using three samples of calcium carbonate of thesame mass: large pieces, medium-sized pieces and small pieces.

(b)

50

40

30

20

10

00 50 100 150 200

time / s

250 300 350

volume ofcarbon dioxide/ cm3

small

medium

large

Which sample, large, medium or small pieces, gave the fastest initial rate of reaction?

Use the graph to explain your answer.

(i)

................................................................................................................................

................................................................................................................................ [2]

The experiment was repeated using powdered calcium carbonate of the same mass.Draw a line on the grid above to show how the volume of carbon dioxide changes withtime for this experiment. [2]

(ii)

At what time was the reaction just complete when small pieces of calcium carbonatewere used?

(iii)

................................................................................................................................ [1]

[Turn over06_0620_31_2016_1.11© UCLES 2016

15

When calcium carbonate is heated strongly, calcium oxide is formed.(c)

Give one use of calcium oxide.(i)

................................................................................................................................ [1]

What type of oxide is calcium oxide?


(ii)

................................................................................................................................

................................................................................................................................ [2]

[Total: 10]

A teacher passed hydrogen gas over hot copper(II) oxide.8

CuO(s) + H2(g) → Cu(s) + H2O(g)

Which substance is reduced in this reaction?


(a)

...........................................................................................................................................

........................................................................................................................................... [2]

06_0620_31_2016_1.11© UCLES 2016

16

The diagram shows the apparatus used.(b)

dryhydrogen gas

copper(II) oxide

waterice bath

The hydrogen was passed over the hot copper(II) oxide until the reaction was complete.

As the experiment proceeds, suggest what happens to the mass of copper(II) oxide.(i)

................................................................................................................................ [1]

Suggest why electrical heating is used in this experiment and not a Bunsen burner.(ii)

................................................................................................................................ [1]

Describe the chemical test for the presence of water.(iii)

test..........................................................................................................................

result....................................................................................................................... [2]

[Total: 6]

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17

BLANK PAGE

06_0620_31_2016_1.11© UCLES 2016

18

BLANK PAGE

06_0620_31_2016_1.11© UCLES 2016

19

Gro

up

The

Perio

dic

Tabl

e of

Ele

men

ts

1 Hhy

drog

en1

2 He

heliu

m4

III

IIIIV

VV

IV

IIV

III

3 Lilit

hium 7

4 Be

bery

llium

9

atom

ic n

umbe

r

atom

ic s

ymbo

l

Key

nam

ere

lativ

e at

omic

mas

s

11 Na

sodi

um23

12 Mg

mag

nesi

um24

19 Kpo

tass

ium

39

20 Ca

calc

ium

40

37 Rb

rubi

dium

85

38 Sr

stro

ntiu

m88

55 Cs

caes

ium

133

56 Ba

bariu

m13

7

87 Frfra

nciu

m–

88 Ra

radi

um –

5 B boro

n11 13 Al

alum

iniu

m27 31 Ga

galli

um70 49 In indi

um11

5

81 Tlth

alliu

m20

4

6 Cca

rbon

12 14 Si

silic

on28 32 Ge

germ

aniu

m73 50 Sn tin 119

82 Pb

lead

207

22 Titit

aniu

m48 40 Zr

zirc

oniu

m91 72 Hf

hafn

ium

178

104

Rf

ruth

erfo

rdiu

m–

23 Vva

nadi

um51 41 Nb

niob

ium

93 73 Tata

ntal

um18

1

105

Db

dubn

ium

–

24 Cr

chro

miu

m52 42 Mo

mol

ybde

num

96 74 Wtu

ngst

en18

4

106

Sg

seab

orgi

um–

25 Mn

man

gane

se55 43 Tc

tech

netiu

m– 75 Re

rhen

ium

186

107

Bh

bohr

ium

–

26 Fe iron

56 44 Ru

ruth

eniu

m10

1

76 Os

osm

ium

190

108

Hs

hass

ium

–

27 Co

coba

lt59 45 Rh

rhod

ium

103

77 Iriri

dium

192

109

Mt

mei

tner

ium

–

28 Ni

nick

el59 46 Pd

palla

dium

106

78 Pt

plat

inum

195

110

Ds

darm

stad

tium

–

29 Cu

copp

er64 47 Ag

silv

er10

8

79 Au

gold

197

111

Rg

roen

tgen

ium

–

30 Zn zinc 65 48 Cd

cadm

ium

112

80 Hg

mer

cury

201

112

Cn

cope

rnic

ium

–

114 Fl

flero

vium

–

116

Lvliv

erm

oriu

m–

7 Nni

troge

n14 15 P

phos

phor

us31 33 As

arse

nic

75 51 Sb

antim

ony

122

83 Bi

bism

uth

209

8 Oox

ygen

16 16 S sulfu

r32 34 Se

sele

nium

79 52 Tete

lluriu

m12

8

84 Po

polo

nium

–

9 Fflu

orin

e19 17 Cl

chlo

rine

35.5

35 Br

brom

ine

80 53 Iio

dine

127

85 At

asta

tine

–

10 Ne

neon 20 18 Ar

argo

n40 36 Kr

kryp

ton

84 54 Xe

xeno

n13

1

86 Rn

rado

n–

21 Sc

scan

dium

45 39 Yyt

trium 89

57–7

1la

ntha

noid

s

89–1

03ac

tinoi

ds

57 Lala

ntha

num

139

89 Ac

lant

hano

ids

actin

oids

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3 a

t roo

m te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.)

actin

ium

–

58 Ce

ceriu

m14

0

90 Th thor

ium

232

59 Pr

pras

eody

miu

m14

1

91 Pa

prot

actin

ium

231

60 Nd

neod

ymiu

m14

4

92 Uur

aniu

m23

8

61 Pm

prom

ethi

um– 93 Np

nept

uniu

m–

62 Sm

sam

ariu

m15

0

94 Pu

plut

oniu

m–

63 Eu

euro

pium

152

95 Am

amer

iciu

m–

64 Gd

gado

liniu

m15

7

96 Cm

curiu

m–

65 Tb terb

ium

159

97 Bk

berk

eliu

m–

66 Dy

dysp

rosi

um16

3

98 Cf

calif

orni

um–

67 Ho

holm

ium

165

99 Es

eins

tein

ium

–

68 Er

erbi

um16

7

100

Fm ferm

ium

–

69 Tm thul

ium

169

101

Md

men

dele

vium

–

70 Yb

ytte

rbiu

m17

3

102

No

nobe

lium

–

71 Lu lute

tium

175

103 Lr

law

renc

ium

–

To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge InternationalExaminations Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at www.cie.org.uk afterthe live examination series.

06_0620_31_2016_1.11© UCLES 2016

20


0620/32May/June 2016

1 hour 15 minutes









This document consists of 19 printed pages and 1 blank page.

[Turn over06_0620_32_2016_1.12© UCLES 2016

*0963380272*

The structures of some substances containing phosphorus are shown.1

P

HH H

A CB

D E

PH4+ I– PH4

+ I–

PH4+ I–

Na+ Na+

Na+

P3–

Na+ Na+

Na+

P3–

Na+ Na+

Na+

P3–

PH4+ I–

I– PH4+ I– PH4

+

P

PP

P

OO

O

O

O O

P

P

P

P

Answer the following questions about these substances.(a)

Which two of these substances are ionic?(i)

[1]....................................................... and .......................................................

Which one of these substances is an element?


(ii)

................................................................................................................................

................................................................................................................................ [2]

Determine the simplest formula for substance D.(iii)

................................................................................................................................ [1]

06_0620_32_2016_1.12© UCLES 2016

2

Phosphorus has one naturally occurring isotope.(b)

Determine the number of neutrons present in one atom of the isotope P.(i)

................................................................................................................................ [1]

How many electrons are there in the outer shell of one phosphorus atom?(ii)

................................................................................................................................ [1]

Determine the total number of electrons present in a phosphorus molecule, P4.(iii)

................................................................................................................................ [1]

What type of oxide is phosphorus(V) oxide?


(c)

...........................................................................................................................................

........................................................................................................................................... [2]

[Total: 9]

[Turn over06_0620_32_2016_1.12© UCLES 2016

3

The table describes the ease of reduction of some metal oxides with carbon.(a)2

ease of reduction on heatingmetal oxide

moderate heating at 200 °C neededlead oxide

high temperature at 750 °C needednickel oxide

very high temperatures above 1700 °C neededtitanium oxide

very high temperature at 900 °C neededzinc oxide

Put the metals in order of their reactivity. Put the least reactive metal first.

least reactive most reactive

[2]

Aluminium is extracted by the electrolysis of molten aluminium oxide.

Predict the products of this electrolysis at the

(b)

positive electrode (anode),................................................................................................

negative electrode (cathode)............................................................................................. [2]

When iron reacts with dilute hydrochloric acid, an aqueous solution containing iron(II) ions isformed.

Describe a test for iron(II) ions.

(c)

test.....................................................................................................................................

result.................................................................................................................................. [2]

Iron rusts very easily.(d)

Complete the following sentence.(i)

Iron rusts in the presence of ..................................... and ..................................... . [2]

06_0620_32_2016_1.12© UCLES 2016

4

Describe one method of rust prevention and explain how it works.(ii)

................................................................................................................................

................................................................................................................................

................................................................................................................................ [2]

[Total: 10]

[Turn over06_0620_32_2016_1.12© UCLES 2016

5

Sulfur dioxide reacts with excess oxygen to form sulfur trioxide.3

2SO3(g)⇌O2(g)+2SO2(g)

What is the meaning of the symbol ⇌ ?(a)

........................................................................................................................................... [1]

The energy level diagram for the reaction is shown.(b)

energy

2SO2(g) + O2(g)

2SO3(g)



...........................................................................................................................................

........................................................................................................................................... [1]

06_0620_32_2016_1.12© UCLES 2016

6

The graph shows how the percentage yield of sulfur trioxide changes with temperature whenthe pressure is kept constant.

(c)

100

95

90

85

80

75100 200 300 400

temperature / °C

% yield ofsulfur trioxide

500 600

Describe how the percentage yield of sulfur trioxide changes with temperature.(i)

................................................................................................................................ [1]

Determine the percentage yield of sulfur trioxide when the temperature is 500 ºC.(ii)

................................................................................................................................ [1]

Describe a test for sulfur dioxide.(d)

test ....................................................................................................................................

result ................................................................................................................................. [2]

Give one use of sulfur dioxide.(e)

........................................................................................................................................... [1]

[Turn over06_0620_32_2016_1.12© UCLES 2016

7

Sulfur dioxide reacts with magnesium.

2Mg + SO2 → 2MgO + S

Which substance is reduced in this reaction?


(f)

...........................................................................................................................................

........................................................................................................................................... [2]

Sulfur dioxide reacts with water to form sulfurous acid, H2SO3. Sulfurous acid reacts withhydrogen sulfide to form water and sulfur.

Complete the chemical equation for this reaction.

(g)

H2SO3 + 2H2S → .....H2O + 3S

[1]

[Total: 10]

06_0620_32_2016_1.12© UCLES 2016

8

Alkanes, alkenes and alcohols are three different homologous series of organic compounds.4

What is meant by the term homologous series?(a)

...........................................................................................................................................

........................................................................................................................................... [2]

The structures of some alkanes, alkenes and alcohols are shown below.(b)

C

H

F

HH

H

C

H

OH H

H

C

H

G

HH

H

C

H

H

C

H

OH H

H

C

H

H

C

H

H

C

HH

H

HC C

H

H

H

I J K

C

C

H

C C

H

H

H HH

H

H

Which two of these compounds, F, G, H, I, J and K, are saturated hydrocarbons?


(i)

................................................................................................................................

................................................................................................................................ [3]

Which one of these compounds is the main constituent of natural gas?(ii)

................................................................................................................................ [1]

Which two of these compounds are alkenes?(iii)

[2].................................................................and .......................................................

Why are two compounds, I and K, not hydrocarbons?(iv)

................................................................................................................................ [1]

[Turn over06_0620_32_2016_1.12© UCLES 2016

9

The table gives some information about four alcohols.(c)

boiling point/ ºC

densityin g / cm3

molecularformula

alcohol

0.793CH4Omethanol

790.789C2H6O

980.804C3H8Opropanol

1170.810C4H10Obutanol

Give the name of the alcohol with the formula C2H6O.(i)

................................................................................................................................ [1]

A student predicts that the density of the alcohols increases as the number of carbonatoms increases.Does the data in the table support this prediction?


(ii)

................................................................................................................................

................................................................................................................................

................................................................................................................................ [1]

Suggest a value for the boiling point of methanol.(iii)

................................................................................................................................ [1]

06_0620_32_2016_1.12© UCLES 2016

10

The alcohol with the formula C2H6O burns in a limited supply of air to form carbon monoxideand water.

(d)

Complete the chemical equation for this reaction.(i)

C2H6O + 2O2 → .....CO + .....H2O

[2]

State an adverse effect of carbon monoxide on health.(ii)

................................................................................................................................ [1]

[Total: 15]

[Turn over06_0620_32_2016_1.12© UCLES 2016

11

Chlorine, bromine and iodine are halogens.5

The melting point of bromine is –7 ºC. The boiling point of bromine is +59 ºC.

Deduce the state of bromine at +6 ºC. Explain your answer.

(a)

...........................................................................................................................................

........................................................................................................................................... [2]

Complete the word equation for the reaction of chlorine with potassium iodide.

chlorine + potassium iodide → ................................... + .................................. [2]

(i)(b)

Suggest why iodine does not react with aqueous potassium bromide.(ii)

................................................................................................................................

................................................................................................................................ [1]

The structure of the dye Lithol fast yellow is shown.(c)

C

CC C

O O

C CCl Cl

H HN

HH H

C

H

H

N

H

N

H

O ON

C

CC C

C C

H

Complete the table and calculate the relative molecular mass of Lithol fast yellow.


13 × 12 = 1561213carbon

10 × 1 = 10110hydrogen

4 × 14 = 56144nitrogen

oxygen

chlorine

relative molecular mass = ........................... [2]

06_0620_32_2016_1.12© UCLES 2016

12

Chromatography is used to separate a mixture of dyes.(d)

Draw a cross on the diagram to show where the mixture of dyes is placed at the startof the chromatography.

(i)

solvent

[1]

Suggest a suitable solvent that could be used.(ii)

................................................................................................................................ [1]

Describe what you would observe as the experiment proceeds.(iii)

................................................................................................................................

................................................................................................................................ [1]

[Total: 10]

[Turn over06_0620_32_2016_1.12© UCLES 2016

13

Sodium is a metal in Group I of the Periodic Table.6

Describe some physical and chemical properties of sodium. In your answer include(a)

• any observations about the reactions of sodium,

• at least one word equation.

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

........................................................................................................................................... [5]

The presence of sodium in compounds can be confirmed using a flame test.

Describe how a flame test is carried out and give the result of the test for sodium.

(b)

test ....................................................................................................................................

...........................................................................................................................................

result ................................................................................................................................. [2]

Aqueous sodium hydroxide is strongly alkaline.(c)

Which one of the following values is the pH of a strongly alkaline solution?

Put a ring around the correct answer.

(i)

pH 13DpH 7CpH 2BpH 1A

[1]

Describe how you could use litmus to show that aqueous sodium hydroxide is alkaline.(ii)

................................................................................................................................

................................................................................................................................ [2]

06_0620_32_2016_1.12© UCLES 2016

14

Sodium sulfite, Na2SO3, reacts with hydrochloric acid.

Na2SO3(s) + 2HCl(aq) → 2NaCl(aq) + SO2(g) + H2O(l)

Explain why this reaction could have an adverse effect on health if not carried out in a fumecupboard.

(d)

...........................................................................................................................................

........................................................................................................................................... [2]

[Total: 12]

[Turn over06_0620_32_2016_1.12© UCLES 2016

15

When magnesium reacts with hydrochloric acid, the products are aqueous magnesium chlorideand hydrogen.

7

Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)

A student used the apparatus shown to follow the progress of this reaction.

dilutehydrochloric acid

magnesium

Complete the diagram by putting the correct labels in the boxes.[2]

(a)

The student conducted two experiments using the samemass of magnesium in each experimentand two different concentrations of hydrochloric acid. The hydrochloric acid was in excess. Allother conditions were kept constant.The student measured the volume of hydrogen produced over a period of time. The graphshows the results.

(b)

504540353025201510

50

0 60 120 180 240time / s

300 360 420 480

volume ofhydrogen/ cm3

0.5 mol / dm3 HCl

1.0 mol / dm3 HCl

06_0620_32_2016_1.12© UCLES 2016

16

Which concentration of hydrochloric acid gave the faster initial rate of reaction?

Use the graph to explain your answer.

(i)

................................................................................................................................

................................................................................................................................ [1]

Draw a curve on the graph on page 16 to show how the volume of hydrogen wouldchange if a third experiment was carried out using 1.5mol / dm3 hydrochloric acid andthe same mass of magnesium.

[2]

(ii)

Give one use of hydrogen.(c)

........................................................................................................................................... [1]

Explosions have occasionally been reported where tiny particles of metal dust escape into theair.

Explain why metal dust can form an explosive mixture with air.

(d)

...........................................................................................................................................

........................................................................................................................................... [1]

[Total: 7]

[Turn over06_0620_32_2016_1.12© UCLES 2016

17

Solder is an alloy of lead and tin.8

What is the meaning of the term alloy?(a)

........................................................................................................................................... [1]

State the name of another alloy.(b)

........................................................................................................................................... [1]

A student heated a piece of solder carefully.The diagram shows what happens to the solder.

(c)

at the start after 2 minutes

solder solder

iron plate

Use the kinetic particle theory to describe and explain what happens to the solder as it changesstate.

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

........................................................................................................................................... [4]

When heated above 1744 °C, lead forms a vapour.

Describe a general property of a vapour (gas) which is not shown by a solid.

(d)

........................................................................................................................................... [1]

[Total: 7]

06_0620_32_2016_1.12© UCLES 2016

18

BLANK PAGE

[Turn over06_0620_32_2016_1.12© UCLES 2016

19

Gro

up

The

Perio

dic

Tabl

e of

Ele

men

ts

1 Hhy

drog

en1

2 He

heliu

m4

III

IIIIV

VV

IV

IIV

III

3 Lilit

hium 7

4 Be

bery

llium

9

atom

ic n

umbe

r

atom

ic s

ymbo

l

Key

nam

ere

lativ

e at

omic

mas

s

11 Na

sodi

um23

12 Mg

mag

nesi

um24

19 Kpo

tass

ium

39

20 Ca

calc

ium

40

37 Rb

rubi

dium

85

38 Sr

stro

ntiu

m88

55 Cs

caes

ium

133

56 Ba

bariu

m13

7

87 Frfra

nciu

m–

88 Ra

radi

um –

5 B boro

n11 13 Al

alum

iniu

m27 31 Ga

galli

um70 49 In indi

um11

5

81 Tlth

alliu

m20

4

6 Cca

rbon

12 14 Si

silic

on28 32 Ge

germ

aniu

m73 50 Sn tin 119

82 Pb

lead

207

22 Titit

aniu

m48 40 Zr

zirc

oniu

m91 72 Hf

hafn

ium

178

104

Rf

ruth

erfo

rdiu

m–

23 Vva

nadi

um51 41 Nb

niob

ium

93 73 Tata

ntal

um18

1

105

Db

dubn

ium

–

24 Cr

chro

miu

m52 42 Mo

mol

ybde

num

96 74 Wtu

ngst

en18

4

106

Sg

seab

orgi

um–

25 Mn

man

gane

se55 43 Tc

tech

netiu

m– 75 Re

rhen

ium

186

107

Bh

bohr

ium

–

26 Fe iron

56 44 Ru

ruth

eniu

m10

1

76 Os

osm

ium

190

108

Hs

hass

ium

–

27 Co

coba

lt59 45 Rh

rhod

ium

103

77 Iriri

dium

192

109

Mt

mei

tner

ium

–

28 Ni

nick

el59 46 Pd

palla

dium

106

78 Pt

plat

inum

195

110

Ds

darm

stad

tium

–

29 Cu

copp

er64 47 Ag

silv

er10

8

79 Au

gold

197

111

Rg

roen

tgen

ium

–

30 Zn zinc 65 48 Cd

cadm

ium

112

80 Hg

mer

cury

201

112

Cn

cope

rnic

ium

–

114 Fl

flero

vium

–

116

Lvliv

erm

oriu

m–

7 Nni

troge

n14 15 P

phos

phor

us31 33 As

arse

nic

75 51 Sb

antim

ony

122

83 Bi

bism

uth

209

8 Oox

ygen

16 16 S sulfu

r32 34 Se

sele

nium

79 52 Tete

lluriu

m12

8

84 Po

polo

nium

–

9 Fflu

orin

e19 17 Cl

chlo

rine

35.5

35 Br

brom

ine

80 53 Iio

dine

127

85 At

asta

tine

–

10 Ne

neon 20 18 Ar

argo

n40 36 Kr

kryp

ton

84 54 Xe

xeno

n13

1

86 Rn

rado

n–

21 Sc

scan

dium

45 39 Yyt

trium 89

57–7

1la

ntha

noid

s

89–1

03ac

tinoi

ds

57 Lala

ntha

num

139

89 Ac

lant

hano

ids

actin

oids

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3 a

t roo

m te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.)

actin

ium

–

58 Ce

ceriu

m14

0

90 Th thor

ium

232

59 Pr

pras

eody

miu

m14

1

91 Pa

prot

actin

ium

231

60 Nd

neod

ymiu

m14

4

92 Uur

aniu

m23

8

61 Pm

prom

ethi

um– 93 Np

nept

uniu

m–

62 Sm

sam

ariu

m15

0

94 Pu

plut

oniu

m–

63 Eu

euro

pium

152

95 Am

amer

iciu

m–

64 Gd

gado

liniu

m15

7

96 Cm

curiu

m–

65 Tb terb

ium

159

97 Bk

berk

eliu

m–

66 Dy

dysp

rosi

um16

3

98 Cf

calif

orni

um–

67 Ho

holm

ium

165

99 Es

eins

tein

ium

–

68 Er

erbi

um16

7

100

Fm ferm

ium

–

69 Tm thul

ium

169

101

Md

men

dele

vium

–

70 Yb

ytte

rbiu

m17

3

102

No

nobe

lium

–

71 Lu lute

tium

175

103 Lr

law

renc

ium

–


06_0620_32_2016_1.12© UCLES 2016

20


0620/33May/June 2016

1 hour 15 minutes









This document consists of 19 printed pages and 1 blank page.

[Turn over06_0620_33_2016_1.10© UCLES 2016

*6622432628*

The structures of some substances containing carbon are shown.1

C C

H

H

H

H

Ca2+C22–

C22–

C22–

C22–

C22– C2

2–

Ca2+ Ca2+

Ca2+

Ca2+ Ca2+

CC C

CC

CC C

CCC C

C CC

C

C CCC

CC

CC C

CC

CC C

CCC C

C CC

C

C CCC

CC

CC CC

CC C

CCC C

CC

CCC

C

CC

C C

CCC

CC

CC

C C CC C

C

CC

CC

C

CC

C

C

CC

C

A B

D E

C

C

C CC

H

H

HH

H

Cl

Cl

Cl

ClCl

C

Answer the following questions about these substances.

Which two substances have giant covalent structures?(i)(a)

[1]....................................................... and .................................................................

Which substance decolourises aqueous bromine?(ii)

................................................................................................................................ [1]

Which substance is most likely to be a gas at room temperature and pressure?(iii)

................................................................................................................................ [1]

Which substance is a hydrocarbon?(iv)

................................................................................................................................ [1]

Determine the simplest formula for substance D.(v)

................................................................................................................................ [1]

06_0620_33_2016_1.10© UCLES 2016

2

Two isotopes of carbon are C and C.(b)

How do these two isotopes differ in their atomic structure?(i)

................................................................................................................................ [1]

Determine the number of neutrons present in one atom of the isotope C.(ii)

................................................................................................................................ [1]

[Total: 7]

[Turn over06_0620_33_2016_1.10© UCLES 2016

3

This question is about metals.2

The table shows some properties of the metals, R, S, T and U.(a)

melting point/ °C

density ing / cm3

relative heatconductivity

relative electricalconductivity

metal

6602.711.84.3R

15357.94.21.2S

10838.922.36.2T

4207.112.44.1U

Which metal would be best to make the base of a pan for cooking food?

Use the information in the table to explain your answer.

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

........................................................................................................................................... [3]

Zinc chloride can be made by reacting excess zinc with hydrochloric acid.

Suggest how the excess zinc can be removed from the reaction mixture.

(b)

........................................................................................................................................... [1]

Zinc can be obtained from molten zinc chloride by electrolysis.(c)

What is meant by the term electrolysis?(i)

................................................................................................................................

................................................................................................................................ [2]

06_0620_33_2016_1.10© UCLES 2016

4

Draw a labelled diagram of the apparatus that could be used to electrolyse moltenzinc chloride.

(ii)

[3]

Give one advantage of recycling metals.(d)

........................................................................................................................................... [1]

[Total: 10]

[Turn over06_0620_33_2016_1.10© UCLES 2016

5

The table gives some information about the halogens.3

boiling point / °Cmelting point / °Ccolourelement

–35–101light greenchlorine

+59–7red-brownbromine

+184+114grey-blackiodine

+337+302astatine

Predict the colour of astatine.(i)(a)

................................................................................................................................ [1]

Describe the trend in the boiling points of the halogens.(ii)

................................................................................................................................ [1]

Deduce the state of chlorine at –50 °C.


(iii)

................................................................................................................................

................................................................................................................................ [2]

Complete the word equation for the reaction of bromine with aqueous potassium astatide.(i)(b)

bromine + potassium astatide → ...................................... + .....................................

[2]

Suggest why bromine does not react with aqueous potassium chloride.(ii)

................................................................................................................................

................................................................................................................................ [1]

06_0620_33_2016_1.10© UCLES 2016

6

Compound X is used to prepare the dye methyl orange.

The structure of compound X is shown.

(c)

C C

C C

C N+ NCl –CS

O

O

H

H

H

H

OH

Complete the table and calculate the relative molecular mass of compound X.


6 × 12 = 72126carbon

5 × 1 = 515hydrogen

2 × 14 = 28142nitrogen

1 × 32 = 32321sulfur

oxygen

chlorine

relative molecular mass = ........................... [2]

Describe how you could usemethyl orange to distinguish between solutions of hydrochloric acidand sodium hydroxide.

(d)

...........................................................................................................................................

........................................................................................................................................... [2]

[Turn over06_0620_33_2016_1.10© UCLES 2016

7

Methyl orange and Congo red are dyes. A mixture of methyl orange and Congo red can beseparated by chromatography.

Draw a labelled diagram to show how the apparatus is arranged to carry out chromatography.

(e)

[3]

[Total: 14]

06_0620_33_2016_1.10© UCLES 2016

8

BLANK PAGE

TURN OVER TO CONTINUE

[Turn over06_0620_33_2016_1.10© UCLES 2016

9

Petroleum is a mixture of hydrocarbons.4

What is the meaning of the term hydrocarbon?(a)

........................................................................................................................................... [1]

Petroleum can be separated into different fractions by fractional distillation.

The diagram shows a fractionating column. The fractions are shown by letters.

(b)

petroleum

A

B

C

D

E

Ffurnace

Describe how fractional distillation is used to separate the petroleum into fractions.

In your answer refer to

• changes of state,

• differences in boiling points.

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

........................................................................................................................................... [5]

06_0620_33_2016_1.10© UCLES 2016

10

The properties of the fractions are shown in the table.(c)

boiling range

/ °C

percentage by mass of thefraction

number ofcarbon atoms

fraction

less than 4031 – 4A

40 – 160144 – 10B

160 – 2501310 – 16C

250 – 300916 – 20D

300 – 350920 – 25E

more than 350more than 25F

total = 100

Describe how the number of carbon atoms affects the boiling range.(i)

................................................................................................................................

................................................................................................................................ [1]

Determine the percentage by mass of fraction F in this sample of petroleum.(ii)

................................................................................................................................ [1]

Which one of the fractions is mainly gaseous at 25 °C?(iii)

................................................................................................................................ [1]

Fraction F is the residue. It contains bitumen.

Give one use of bitumen.

(iv)

................................................................................................................................ [1]

Fraction C can be cracked to form alkenes.(d)

Describe one condition required for cracking.(i)

................................................................................................................................ [1]

[Turn over06_0620_33_2016_1.10© UCLES 2016

11

Complete the chemical equation for the cracking of dodecane, C12H26 , to form heptane,C7H16, and one other hydrocarbon.

C12H26 → C7H16 + .............

[1]

(ii)

[Total: 12]

Iron is a transition element.5

Describe the physical and chemical properties of iron.(a)

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

...........................................................................................................................................

........................................................................................................................................... [5]

Iron carbonyl, Fe(CO)5, is a covalent liquid.(b)

Suggest two physical properties of iron carbonyl.(i)

................................................................................................................................

................................................................................................................................ [2]

When heated above 200 °C, iron carbonyl undergoes thermal decomposition.

Fe(CO)5(I) → Fe(s) + 5CO(g)

Explain why this reaction could have an adverse effect on health if not carried out in afume cupboard.

(ii)

................................................................................................................................

................................................................................................................................ [2]

[Total: 9]

06_0620_33_2016_1.10© UCLES 2016

12

Ethanol can be manufactured by reacting ethene with steam.6

C2H4(g) + H2O(g) ⇌ C2H5OH(g)

What is the meaning of the symbol ⇌ ?(a)

........................................................................................................................................... [1]

State two conditions needed for this reaction.(b)

...........................................................................................................................................

........................................................................................................................................... [2]

The energy level diagram for this reaction is shown.(c)

energy

C2H4(g) + H2O(g)

C2H5OH(g)



...........................................................................................................................................

........................................................................................................................................... [2]

[Turn over06_0620_33_2016_1.10© UCLES 2016

13

The graph below shows how the percentage yield of ethanol changes with temperature whenthe pressure is kept constant.

(d)

50

40

30

20

10100 200 300

temperature / °C

% yieldof ethanol

400

Describe how the percentage yield changes with temperature.(i)

................................................................................................................................

................................................................................................................................ [1]

Determine the percentage yield when the temperature is 350 °C.(ii)

................................................................................................................................ [1]

Complete the structure of ethanol, C2H5OH, to show all atoms and all bonds.(i)(e)

H

H C

H

[1]

Give one use of ethanol.(ii)

................................................................................................................................ [1]

06_0620_33_2016_1.10© UCLES 2016

14

Complete the chemical equation for the complete combustion of ethanol.

C2H5OH + 3O2 → ....CO2 + ....H2O

[2]

(iii)

[Total: 11]

[Turn over06_0620_33_2016_1.10© UCLES 2016

15

A student investigated the reaction between zinc and sulfuric acid at 20 °C using the apparatusshown. The zinc was in excess.

7

zinc gas syringe

sulfuric acid

What should the student do to start the reaction?(a)

........................................................................................................................................... [1]

The graph shows the volume of hydrogen released as the reaction proceeds.(b)

50

40

30

20

10

00 2 4 6

time / minutes8 10 12 14

volume ofhydrogen/ cm3

06_0620_33_2016_1.10© UCLES 2016

16

Explain why the volume of gas stays the same after 10 minutes.(i)

................................................................................................................................ [1]

How long did it take for the first 20cm3 of gas to be collected?(ii)

................................................................................................................................ [1]

The student repeated the experiment at 30 °C. All other conditions remained the same.

Draw the shape of the line on the grid on page 16 when the reaction was carried outat 30 °C.

[2]

(iii)

The student repeated the experiment using zinc powder instead of small pieces of zinc.

Describe and explain how the rate of reaction differs when zinc powder is used.

(c)

...........................................................................................................................................

........................................................................................................................................... [2]

Sulfuric acid is a compound.(d)

What is the meaning of the term compound?(i)

................................................................................................................................

................................................................................................................................ [1]

Sulfur is used to make sulfuric acid.

Give one source of sulfur.

(ii)

................................................................................................................................ [1]

Sulfur is oxidised by air to form sulfur dioxide.

Give one use of sulfur dioxide.

(iii)

................................................................................................................................ [1]

[Total: 10]

[Turn over06_0620_33_2016_1.10© UCLES 2016

17

The graph shows how increasing the pressure at constant temperature changes the volume of afixed mass of carbon dioxide gas.

8

volume

pressure

Describe how the volume of gas changes with pressure.(a)

...........................................................................................................................................

...........................................................................................................................................

........................................................................................................................................... [2]

What happens to the average distance of the molecules from each other when the pressureis decreased?

(b)

........................................................................................................................................... [1]

Carbon dioxide can be reduced by magnesium.(c)

2Mg(s) + CO2(g) → 2MgO(s) + C(s)

Use the information in the equation to show that carbon dioxide gets reduced.(i)

................................................................................................................................ [1]

Which one of these processes does not produce carbon dioxide?

Tick one box.

(ii)

respiration

reaction of an acid with a metal oxide

reaction of an acid with a carbonate

thermal decomposition of limestone

[1]

06_0620_33_2016_1.10© UCLES 2016

18

Give two problems caused by increasing the amount of carbon dioxide in theatmosphere.

(iii)

................................................................................................................................

................................................................................................................................

................................................................................................................................ [2]

[Total: 7]

[Turn over06_0620_33_2016_1.10© UCLES 2016

19

Gro

up

The

Perio

dic

Tabl

e of

Ele

men

ts

1 Hhy

drog

en1

2 He

heliu

m4

III

IIIIV

VV

IV

IIV

III

3 Lilit

hium 7

4 Be

bery

llium

9

atom

ic n

umbe

r

atom

ic s

ymbo

l

Key

nam

ere

lativ

e at

omic

mas

s

11 Na

sodi

um23

12 Mg

mag

nesi

um24

19 Kpo

tass

ium

39

20 Ca

calc

ium

40

37 Rb

rubi

dium

85

38 Sr

stro

ntiu

m88

55 Cs

caes

ium

133

56 Ba

bariu

m13

7

87 Frfra

nciu

m–

88 Ra

radi

um –

5 B boro

n11 13 Al

alum

iniu

m27 31 Ga

galli

um70 49 In indi

um11

5

81 Tlth

alliu

m20

4

6 Cca

rbon

12 14 Si

silic

on28 32 Ge

germ

aniu

m73 50 Sn tin 119

82 Pb

lead

207

22 Titit

aniu

m48 40 Zr

zirc

oniu

m91 72 Hf

hafn

ium

178

104

Rf

ruth

erfo

rdiu

m–

23 Vva

nadi

um51 41 Nb

niob

ium

93 73 Tata

ntal

um18

1

105

Db

dubn

ium

–

24 Cr

chro

miu

m52 42 Mo

mol

ybde

num

96 74 Wtu

ngst

en18

4

106

Sg

seab

orgi

um–

25 Mn

man

gane

se55 43 Tc

tech

netiu

m– 75 Re

rhen

ium

186

107

Bh

bohr

ium

–

26 Fe iron

56 44 Ru

ruth

eniu

m10

1

76 Os

osm

ium

190

108

Hs

hass

ium

–

27 Co

coba

lt59 45 Rh

rhod

ium

103

77 Iriri

dium

192

109

Mt

mei

tner

ium

–

28 Ni

nick

el59 46 Pd

palla

dium

106

78 Pt

plat

inum

195

110

Ds

darm

stad

tium

–

29 Cu

copp

er64 47 Ag

silv

er10

8

79 Au

gold

197

111

Rg

roen

tgen

ium

–

30 Zn zinc 65 48 Cd

cadm

ium

112

80 Hg

mer

cury

201

112

Cn

cope

rnic

ium

–

114 Fl

flero

vium

–

116

Lvliv

erm

oriu

m–

7 Nni

troge

n14 15 P

phos

phor

us31 33 As

arse

nic

75 51 Sb

antim

ony

122

83 Bi

bism

uth

209

8 Oox

ygen

16 16 S sulfu

r32 34 Se

sele

nium

79 52 Tete

lluriu

m12

8

84 Po

polo

nium

–

9 Fflu

orin

e19 17 Cl

chlo

rine

35.5

35 Br

brom

ine

80 53 Iio

dine

127

85 At

asta

tine

–

10 Ne

neon 20 18 Ar

argo

n40 36 Kr

kryp

ton

84 54 Xe

xeno

n13

1

86 Rn

rado

n–

21 Sc

scan

dium

45 39 Yyt

trium 89

57–7

1la

ntha

noid

s

89–1

03ac

tinoi

ds

57 Lala

ntha

num

139

89 Ac

lant

hano

ids

actin

oids

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3 a

t roo

m te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.)

actin

ium

–

58 Ce

ceriu

m14

0

90 Th thor

ium

232

59 Pr

pras

eody

miu

m14

1

91 Pa

prot

actin

ium

231

60 Nd

neod

ymiu

m14

4

92 Uur

aniu

m23

8

61 Pm

prom

ethi

um– 93 Np

nept

uniu

m–

62 Sm

sam

ariu

m15

0

94 Pu

plut

oniu

m–

63 Eu

euro

pium

152

95 Am

amer

iciu

m–

64 Gd

gado

liniu

m15

7

96 Cm

curiu

m–

65 Tb terb

ium

159

97 Bk

berk

eliu

m–

66 Dy

dysp

rosi

um16

3

98 Cf

calif

orni

um–

67 Ho

holm

ium

165

99 Es

eins

tein

ium

–

68 Er

erbi

um16

7

100

Fm ferm

ium

–

69 Tm thul

ium

169

101

Md

men

dele

vium

–

70 Yb

ytte

rbiu

m17

3

102

No

nobe

lium

–

71 Lu lute

tium

175

103 Lr

law

renc

ium

–


06_0620_33_2016_1.10© UCLES 2016

20


Write your Centre number, candidate number and name on all the work you hand in.Write in dark blue or black pen.You may use an HB pencil for any diagrams or graphs.Do not use staples, paper clips, glue or correction fluid.DO NOT WRITE IN ANY BARCODES.



CHEMISTRY 0620/41

Paper 4 Theory (Extended) May/June 2016

1 hour 15 minutes


No Additional Materials are required.



[Turn overIB16 06_0620_41/4RP© UCLES 2016

*4054381962*


2

0620/41/M/J/16© UCLES 2016

1 Protons, neutrons and electrons are subatomic particles.

(a) Complete the table to show the relative mass and relative charge of a proton, a neutron and an electron.

particle relative mass relative charge

proton

neutron

electron 18401

[3]

(b) Bromine has two isotopes.

(i) Define the term isotope.

.............................................................................................................................................

....................................................................................................................................... [2]

(ii) Explain why the two isotopes of bromine have the same chemical properties.

.............................................................................................................................................

....................................................................................................................................... [2]

(c) The table shows the number of protons, neutrons and electrons in some atoms and ions.

Complete the table.

particle number ofprotons

number ofneutrons

number ofelectrons

7Li3

-34 2S16

19 22 18

[5]

[Total: 12]

3

0620/41/M/J/16© UCLES 2016 [Turn over

2 Period 3 contains the elements sodium to argon. This question asks about the chemistry of each of the Period 3 elements or their compounds.

(a) Sodium nitrate is a white crystalline solid. When heated it melts and the following reaction occurs.

2NaNO3(l) → 2NaNO2(l) + O2(g)

A 3.40 g sample of sodium nitrate is heated.

Calculate the

• number of moles of NaNO3 used,

.................................. mol

• number of moles of O2 formed,

.................................. mol

• volume of O2 formed, in dm3 (measured at r.t.p.).

.................................. dm3

[3]

(b) Magnesium reacts slowly with warm water to form a base, magnesium hydroxide.

(i) Explain what is meant by the term base.

....................................................................................................................................... [1]

(ii) Write a chemical equation for the reaction between magnesium and warm water.

....................................................................................................................................... [2]

4

0620/41/M/J/16© UCLES 2016

(c) Aluminium oxide is amphoteric. It is insoluble in water.

Describe experiments to show that aluminium oxide is amphoteric.

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [3]

(d) Silicon(IV) oxide has a giant structure.

(i) Name the type of bonding in silicon(IV) oxide.

....................................................................................................................................... [1]

(ii) Give two physical properties of silicon(IV) oxide.

.............................................................................................................................................

....................................................................................................................................... [2]

(e) Calcium phosphate is used in fertilisers. The bonding in calcium phosphate is ionic. Calcium phosphate contains the phosphate ion, PO4

3–.

(i) What is ionic bonding?

.............................................................................................................................................

....................................................................................................................................... [2]

(ii) Deduce the formula of calcium phosphate.

....................................................................................................................................... [1]

5


(f) Sulfur tetrafluoride, SF4, can be made by combining gaseous sulfur with fluorine.

S(g) + 2F2(g) → SF4(g)

The reaction is exothermic.

(i) Complete the energy level diagram for this reaction. Include an arrow which clearly shows the energy change during the reaction.

energy

S(g) + 2F2(g)

[3]

(ii) During the reaction the amount of energy given out is 780 kJ / mol.

The F–F bond energy is 160 kJ / mol.

Use this information to determine the bond energy, in kJ / mol, of one S–F bond in SF4.

S + F→F FF F

S

F

F

F

.................................. kJ / mol [3]

6

0620/41/M/J/16© UCLES 2016

(g) Chlorine and compounds of chlorine are important in water treatment and in laboratory testing for water.

(i) Chlorine is added to water to make the water safe to drink.

Explain why adding chlorine makes water safe to drink.

....................................................................................................................................... [1]

(ii) A compound of chlorine is used in the laboratory to test for the presence of water.

Name the compound of chlorine used in this test and describe the colour change seen in a positive result of this test.

name of compound .............................................................................................................

colour change from ................................................... to ...................................................[3]

(h) Argon is an unreactive noble gas.

(i) Explain why argon is unreactive.

....................................................................................................................................... [1]

(ii) Give one use of argon.

....................................................................................................................................... [1]

[Total: 27]

7


Question 3 starts on the next page.

8

0620/41/M/J/16© UCLES 2016

3 When aqueous sodium thiosulfate and dilute hydrochloric acid are mixed, a precipitate of insoluble sulfur is produced. This makes the mixture difficult to see through.

Na2S2O3(aq) + 2HCl (aq) → S(s) + 2NaCl (aq) + H2O(l) + SO2(g)

The time taken for the cross to disappear from view is measured.

A student adds the following volumes of aqueous sodium thiosulfate, dilute hydrochloric acid and distilled water to the conical flask.

The time taken for the formation of the precipitate of sulfur to make the cross disappear from view is recorded.

experimentnumber

volume ofsodium thiosulfate

/ cm3

volume of hydrochloric acid

/ cm3

volume ofdistilled water

/ cm3

time taken for cross to disappear

from view / s

1 10 10 40 56

2 20 10 30 28

3

(a) State the order in which the aqueous sodium thiosulfate, hydrochloric acid and distilled water should be added to the flask.

....................................................................................................................................................

.............................................................................................................................................. [1]

9


(b) In experiment 3 the student wanted the sodium thiosulfate to be double the concentration used in experiment 2.

(i) Complete the table to show the volumes which should be used and the expected time taken for the cross to disappear from view in experiment 3. [2]

(ii) Use collision theory to explain why increasing the concentration of sodium thiosulfate would change the rate of reaction.

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [2]

(c) The student repeated experiment 1 at a higher temperature.

Use collision theory to explain why the rate of reaction would increase.

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [3]

[Total: 8]

10

0620/41/M/J/16© UCLES 2016

4 Electroplating steel objects with silver involves a three-step process.

step 1 A coating of copper is applied to the object.

step 2 A coating of nickel is applied to the object.

step 3 The coating of silver is applied to the object.

(a) A diagram of the apparatus used for step 1 is shown.

+ –

copper (anode)

steel object (cathode)

aqueous copper(II) sulfateelectrolyte

(i) The chemical process taking place on the surface of the object is

Cu2+(aq) + 2e– → Cu(s)

Explain whether this process is oxidation or reduction.

.............................................................................................................................................

....................................................................................................................................... [1]

(ii) Explain why the concentration of copper ions in the electrolyte remains constant throughout step 1.

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [2]

11


(b) Give two changes which would be needed in order to coat nickel onto the object in step 2.

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [2]

(c) Copper, nickel and silver are transition elements. Typical physical properties of transition elements are a high density and a high melting point.

Give three different properties of transition metals which are not typical of other metals.

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [3]

[Total: 8]

12

0620/41/M/J/16© UCLES 2016

5 Sulfuric acid is produced by the Contact process. The steps of the Contact process are shown.

startingmaterial

step 1 sulfurdioxide

sulfurtrioxide

sulfuricacid

oleumstep 2 step 3 step 4

(a) Sulfur is a common starting material for the Contact process.

Name a source of sulfur.

.............................................................................................................................................. [1]

(b) Describe step 2, giving reaction conditions and a chemical equation. Reference to reaction rate and yield is not required.

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [5]

(c) Step 3 involves adding sulfur trioxide to concentrated sulfuric acid to form oleum.

Complete the chemical equation for this reaction.

H2SO4 + SO3 → ................................[1]

13


(d) Dilute sulfuric acid is a typical acid.

A student adds excess dilute sulfuric acid to a sample of solid copper(II) carbonate in a test-tube.

(i) Give three observations the student would make.

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [2]

(ii) Give the names of all products formed.

.............................................................................................................................................

....................................................................................................................................... [1]

(e) Concentrated sulfuric acid has different properties to dilute sulfuric acid.

When concentrated sulfuric acid is added to glucose, C6H12O6, steam is given off and a black solid is formed.

(i) Name the black solid.

....................................................................................................................................... [1]

(ii) What type of reaction has occurred?

....................................................................................................................................... [1]

[Total: 12]

14

0620/41/M/J/16© UCLES 2016

6 Petroleum is a source of many important chemicals.

(a) Name two industrial processes which must take place to produce alkenes from petroleum.

....................................................................................................................................................

.............................................................................................................................................. [2]

(b) Ethene, CH2=CH2, and propene, CH2=CHCH3, can both be converted into polymers.

(i) What type of polymerisation takes place when ethene forms a polymer?

....................................................................................................................................... [1]

(ii) What is the empirical formula of the polymer formed from ethene?

....................................................................................................................................... [1]

(iii) Propene has the structural formula CH2=CHCH3.

Draw two repeat units of the polymer made from propene.

[2]

(c) Ethene will react with steam to form ethanol.

Propene will react with steam to form two isomers, both of which are alcohols.

Suggest the structures of these alcohols.

[2]

15

0620/41/M/J/16© UCLES 2016

Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the publisher will be pleased to make amends at the earliest possible opportunity.

To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge International Examinations Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at www.cie.org.uk after the live examination series.


(d) Esters are organic chemicals noted for their characteristic smells. Ethanoic acid and methanol will react to form an ester.

(i) Name the catalyst needed to form an ester from ethanoic acid and methanol.

....................................................................................................................................... [1]

(ii) Name the ester formed when ethanoic acid reacts with methanol.

....................................................................................................................................... [1]

(iii) Draw the structure of the ester formed when ethanoic acid reacts with methanol. Show all bonds.

[2]

(iv) Give the name of a polyester.

....................................................................................................................................... [1]

[Total: 13]

16

0620/41/M/J/16© UCLES 2016

Gro

up

The

Perio

dic

Tabl

e of

Ele

men

ts

1 Hhy

drog

en1

2 He

heliu

m4

III

IIIIV

VV

IV

IIV

III

3 Lilit

hium 7

4 Be

bery

llium

9

atom

ic n

umbe

r

atom

ic s

ymbo

l

Key

nam

ere

lativ

e at

omic

mas

s

11 Na

sodi

um23

12 Mg

mag

nesi

um24

19 Kpo

tass

ium

39

20 Ca

calc

ium

40

37 Rb

rubi

dium

85

38 Sr

stro

ntiu

m88

55 Cs

caes

ium

133

56 Ba

bariu

m13

7

87 Frfra

nciu

m–

88 Ra

radi

um –

5 B boro

n11 13 Al

alum

iniu

m27 31 Ga

galli

um70 49 In indi

um11

5

81 Tlth

alliu

m20

4

6 Cca

rbon

12 14 Si

silic

on28 32 Ge

germ

aniu

m73 50 Sn tin 119

82 Pb

lead

207

22 Titit

aniu

m48 40 Zr

zirc

oniu

m91 72 Hf

hafn

ium

178

104

Rf

ruth

erfo

rdiu

m–

23 Vva

nadi

um51 41 Nb

niob

ium

93 73 Tata

ntal

um18

1

105

Db

dubn

ium

–

24 Cr

chro

miu

m52 42 Mo

mol

ybde

num

96 74 Wtu

ngst

en18

4

106

Sg

seab

orgi

um–

25 Mn

man

gane

se55 43 Tc

tech

netiu

m– 75 Re

rhen

ium

186

107

Bh

bohr

ium

–

26 Fe iron

56 44 Ru

ruth

eniu

m10

1

76 Os

osm

ium

190

108

Hs

hass

ium

–

27 Co

coba

lt59 45 Rh

rhod

ium

103

77 Iriri

dium

192

109

Mt

mei

tner

ium

–

28 Ni

nick

el59 46 Pd

palla

dium

106

78 Pt

plat

inum

195

110

Ds

darm

stad

tium

–

29 Cu

copp

er64 47 Ag

silv

er10

8

79 Au

gold

197

111

Rg

roen

tgen

ium

–

30 Zn zinc 65 48 Cd

cadm

ium

112

80 Hg

mer

cury

201

112

Cn

cope

rnic

ium

–

114 Fl

flero

vium

–

116

Lvliv

erm

oriu

m–

7 Nni

troge

n14 15 P

phos

phor

us31 33 As

arse

nic

75 51 Sb

antim

ony

122

83 Bi

bism

uth

209

8 Oox

ygen

16 16 S sulfu

r32 34 Se

sele

nium

79 52 Tete

lluriu

m12

8

84 Po

polo

nium

–

9 Fflu

orin

e19 17 Cl

chlo

rine

35.5

35 Br

brom

ine

80 53 Iio

dine

127

85 At

asta

tine

–

10 Ne

neon 20 18 Ar

argo

n40 36 Kr

kryp

ton

84 54 Xe

xeno

n13

1

86 Rn

rado

n–

21 Sc

scan

dium

45 39 Yyt

trium 89

57–7

1la

ntha

noid

s

89–1

03ac

tinoi

ds

57 Lala

ntha

num

139

89 Ac

lant

hano

ids

actin

oids

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3 a

t roo

m te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.)

actin

ium

–

58 Ce

ceriu

m14

0

90 Th thor

ium

232

59 Pr

pras

eody

miu

m14

1

91 Pa

prot

actin

ium

231

60 Nd

neod

ymiu

m14

4

92 Uur

aniu

m23

8

61 Pm

prom

ethi

um– 93 Np

nept

uniu

m–

62 Sm

sam

ariu

m15

0

94 Pu

plut

oniu

m–

63 Eu

euro

pium

152

95 Am

amer

iciu

m–

64 Gd

gado

liniu

m15

7

96 Cm

curiu

m–

65 Tb terb

ium

159

97 Bk

berk

eliu

m–

66 Dy

dysp

rosi

um16

3

98 Cf

calif

orni

um–

67 Ho

holm

ium

165

99 Es

eins

tein

ium

–

68 Er

erbi

um16

7

100

Fm ferm

ium

–

69 Tm thul

ium

169

101

Md

men

dele

vium

–

70 Yb

ytte

rbiu

m17

3

102

No

nobe

lium

–

71 Lu lute

tium

175

103 Lr

law

renc

ium

–





CHEMISTRY 0620/42


1 hour 15 minutes






*3291778503*


2

0620/42/M/J/16© UCLES 2016

1 (a) For each of the following, give the name of an element from Period 2 (lithium to neon), which matches the description.

Elements may be used once, more than once or not at all.

(i) an element which is gaseous at room temperature and pressure

....................................................................................................................................... [1]

(ii) an element which forms an oxide that is a reactant in photosynthesis

....................................................................................................................................... [1]

(iii) an element that is a product of photosynthesis

....................................................................................................................................... [1]

(iv) an element that makes up approximately 78% by volume of the air

....................................................................................................................................... [1]

(v) an element which has atoms with a full outer shell of electrons

....................................................................................................................................... [1]

(vi) an element which exists as both diamond and graphite

....................................................................................................................................... [1]

(vii) an element that reacts vigorously with cold water

....................................................................................................................................... [1]

(viii) a soft metallic element which is stored in oil

....................................................................................................................................... [1]

(b) Give the formula of a compound that contains

(i) only boron and oxygen, ................................................................................................ [1]

(ii) only lithium and nitrogen. .............................................................................................. [1]

[Total: 10]

3


2 (a) (i) Define the term atomic number.

....................................................................................................................................... [1]

(ii) Define the term nucleon number.

.............................................................................................................................................

....................................................................................................................................... [2]

(b) The table shows the number of protons, neutrons and electrons in some atoms or ions.

Complete the table. The first line is given as an example.

particle number ofprotons

number ofelectrons

number ofneutrons

symbol orformula

A 6 6 6 C126

B 12 12 12

C 8 -2O168

D 11 10 13

[6]

[Total: 9]

4

0620/42/M/J/16© UCLES 2016

3 Gallium is a metallic element in Group III. It has similar properties to aluminium.

(a) (i) Describe the structure and bonding in a metallic element. You should include a labelled diagram in your answer.

.............................................................................................................................................

....................................................................................................................................... [3]

(ii) Explain why metallic elements such as gallium are good conductors of electricity.

....................................................................................................................................... [1]

(b) Give the formula of

gallium(III) chloride, ..................................................................................................................

gallium(III) sulfate. ....................................................................................................................[2]

(c) Gallium(III) oxide, Ga2O3, is amphoteric.

(i) Write the chemical equation for the reaction between gallium(III) oxide and dilute nitric acid to form a salt and water only.

....................................................................................................................................... [2]

(ii) The reaction between gallium(III) oxide and sodium hydroxide solution forms only water and a salt containing the negative ion Ga2O4

2–.

Write the chemical equation for this reaction.

....................................................................................................................................... [2]

(d) Alloys of gallium and other elements are often more useful than the metallic element itself.

Suggest two reasons why alloys of gallium are more useful than the metallic element.

....................................................................................................................................................

.............................................................................................................................................. [2]

[Total: 12]

5


4 Hydrogen can be manufactured from methane by steam reforming.

CH4(g) + H2O(g) CO(g) + 3H2(g)

The reaction is carried out using a nickel catalyst at temperatures between 700 °C and 1100 °C and using a pressure of one atmosphere.

The forward reaction is endothermic.

(a) What is meant by the term catalyst?

....................................................................................................................................................

.............................................................................................................................................. [2]

(b) Suggest two reasons why a temperature lower than 700 °C is not used.

....................................................................................................................................................

.............................................................................................................................................. [2]

(c) Suggest one advantage of using a pressure greater than one atmosphere.

.............................................................................................................................................. [1]

(d) Suggest one disadvantage of using a pressure greater than one atmosphere.

.............................................................................................................................................. [1]

(e) Hydrogen can also be manufactured by electrolysis. The electrolyte is concentrated aqueous sodium chloride. The electrodes are inert.

The products of electrolysis are hydrogen, chlorine and sodium hydroxide.

(i) Define the term electrolysis.

.............................................................................................................................................

....................................................................................................................................... [2]

(ii) Name a substance that can be used as the inert electrodes.

....................................................................................................................................... [1]

(iii) Write an ionic half-equation for the reaction in which hydrogen is produced.

....................................................................................................................................... [1]

(iv) Where is hydrogen produced in the electrolytic cell?

....................................................................................................................................... [1]

6

0620/42/M/J/16© UCLES 2016

(v) Describe a test for chlorine.

test ......................................................................................................................................

result ...................................................................................................................................[2]

(f) The electrolysis of concentrated aqueous sodium chloride can be represented by the following word equation.

sodium chloride + water → sodium hydroxide + hydrogen + chlorine

Construct a chemical equation to represent this reaction. Do not include state symbols.

.............................................................................................................................................. [2]

(g) State one use of

chlorine, .....................................................................................................................................

sodium hydroxide, .....................................................................................................................

hydrogen. ...................................................................................................................................[3]

[Total: 18]

7


5 (a) Hydrocarbons are compounds which contain hydrogen and carbon only.

• 10 cm3 of a gaseous hydrocarbon, CxHy, are burned in 100 cm3 of oxygen, which is an excess of oxygen.

• After cooling to room temperature and pressure, there is 25 cm3 of unreacted oxygen, 50 cm3 of carbon dioxide and some liquid water.

All volumes are measured under the same conditions of temperature and pressure.

(i) What is meant by an excess of oxygen?

....................................................................................................................................... [1]

(ii) What was the volume of oxygen that reacted with the hydrocarbon?

....................................................................................................................................... [1]

(iii) Complete the table below to express the smallest whole number ratio of

volume ofhydrocarbon reacted : volume of

oxygen reacted :volume of

carbon dioxideproduced

volume ofhydrocarbon reacted

volume ofoxygen reacted

volume ofcarbon dioxide

produced

smallest wholenumber ratio ofvolumes

[1]

(iv) Use your answer to (a)(iii) to find the mole ratio in the equation below. Complete the equation and deduce the formula of the hydrocarbon.

.........CxHy(g) + .........O2(g) → .........CO2(g) + .........H2O(l)

formula of hydrocarbon = ...........................................[2]

8

0620/42/M/J/16© UCLES 2016

(b) Cracking is used to convert long chain alkanes into shorter chain alkanes and alkenes. Alkenes are unsaturated compounds.

Decane, C10H22, can be cracked to give propene and one other product.

(i) Complete the chemical equation.

C10H22 → C3H6 + ...............[1]

(ii) What is meant by the term unsaturated?

....................................................................................................................................... [1]

(iii) Describe a test to show that propene is an unsaturated compound.

test ......................................................................................................................................

result ...................................................................................................................................[2]

(c) Propene can be polymerised. The only product is polypropene. The equation for the polymerisation is:

n

C

H

CH3

C

H

H

nC3H6

(i) Name the type of polymerisation that occurs.

....................................................................................................................................... [1]

(ii) Deduce the maximum mass of polypropene that could be produced from 1 kg of propene.

............... kg [1]

(iii) Give the empirical formula of

propene, .............................................................................................................................

polypropene. .......................................................................................................................[2]

[Total: 13]

9


6 Zinc is extracted from an ore called zinc blende, which consists mainly of zinc sulfide, ZnS.

(a) (i) The zinc sulfide in the ore is first converted into zinc oxide.

Describe how zinc oxide is made from zinc sulfide.

.............................................................................................................................................

....................................................................................................................................... [1]

(ii) Write a chemical equation for the reaction in (a)(i).

....................................................................................................................................... [2]

(b) Zinc oxide is converted into zinc. Zinc oxide and coke are fed into a furnace. Hot air is blown into the bottom of the furnace.

Zinc has a melting point of 420 °C and a boiling point of 907 °C. The temperature inside the furnace is over 1000 °C.

(i) Explain how zinc oxide is converted into zinc. Your answer should include details of how the heat is produced and equations for all the reactions you describe.

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [3]

(ii) Explain why the zinc produced inside the furnace is a gas.

....................................................................................................................................... [1]

(iii) State the name of the physical change for conversion of gaseous zinc into molten zinc.

....................................................................................................................................... [1]

10

0620/42/M/J/16© UCLES 2016

(c) Rusting of steel can be prevented by coating the steel with a layer of zinc.

Explain, in terms of electron transfer, why steel does not rust even if the layer of zinc is scratched so that the steel is exposed to air and water.

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [4]

(d) When a sample of steel is added to dilute hydrochloric acid, an aqueous solution of iron(II) chloride, FeCl 2, is formed.

When a sample of rust is added to dilute hydrochloric acid, an aqueous solution of iron(III) chloride, FeCl 3, is formed.

(i) Aqueous sodium hydroxide is added to the solutions of iron(II) chloride and iron(III) chloride.

Complete the table below, showing the observations you would expect to make.

iron(II) chloride solution iron(III) chloride solution

aqueoussodium hydroxide

[2]

11

0620/42/M/J/16© UCLES 2016




Solutions of iron(II) chloride and iron(III) chloride were added to solutions of potassium iodide and acidified potassium manganate(VII). The results are shown in the table.

iron(II) chloride solution

iron(III) chloride solution

potassiumiodide solution no change

solution turnsfrom colourless

to brown

acidified potassiummanganate(VII)

solution

solution turnsfrom purple

to colourlessno change

(ii) What types of substance cause potassium iodide solution to turn from colourless to brown?

....................................................................................................................................... [1]

(iii) What types of substance cause acidified potassium manganate(VII) solution to turn from purple to colourless?

....................................................................................................................................... [1]

(iv) Which ion in iron(III) chloride solution causes potassium iodide solution to turn from colourless to brown?

....................................................................................................................................... [1]

(v) Which ion in iron(II) chloride solution causes acidified potassium manganate(VII) solution to turn from purple to colourless?

....................................................................................................................................... [1]

[Total: 18]

12

0620/42/M/J/16© UCLES 2016

Gro

up

The

Perio

dic

Tabl

e of

Ele

men

ts

1 Hhy

drog

en1

2 He

heliu

m4

III

IIIIV

VV

IV

IIV

III

3 Lilit

hium 7

4 Be

bery

llium

9

atom

ic n

umbe

r

atom

ic s

ymbo

l

Key

nam

ere

lativ

e at

omic

mas

s

11 Na

sodi

um23

12 Mg

mag

nesi

um24

19 Kpo

tass

ium

39

20 Ca

calc

ium

40

37 Rb

rubi

dium

85

38 Sr

stro

ntiu

m88

55 Cs

caes

ium

133

56 Ba

bariu

m13

7

87 Frfra

nciu

m–

88 Ra

radi

um –

5 B boro

n11 13 Al

alum

iniu

m27 31 Ga

galli

um70 49 In indi

um11

5

81 Tlth

alliu

m20

4

6 Cca

rbon

12 14 Si

silic

on28 32 Ge

germ

aniu

m73 50 Sn tin 119

82 Pb

lead

207

22 Titit

aniu

m48 40 Zr

zirc

oniu

m91 72 Hf

hafn

ium

178

104

Rf

ruth

erfo

rdiu

m–

23 Vva

nadi

um51 41 Nb

niob

ium

93 73 Tata

ntal

um18

1

105

Db

dubn

ium

–

24 Cr

chro

miu

m52 42 Mo

mol

ybde

num

96 74 Wtu

ngst

en18

4

106

Sg

seab

orgi

um–

25 Mn

man

gane

se55 43 Tc

tech

netiu

m– 75 Re

rhen

ium

186

107

Bh

bohr

ium

–

26 Fe iron

56 44 Ru

ruth

eniu

m10

1

76 Os

osm

ium

190

108

Hs

hass

ium

–

27 Co

coba

lt59 45 Rh

rhod

ium

103

77 Iriri

dium

192

109

Mt

mei

tner

ium

–

28 Ni

nick

el59 46 Pd

palla

dium

106

78 Pt

plat

inum

195

110

Ds

darm

stad

tium

–

29 Cu

copp

er64 47 Ag

silv

er10

8

79 Au

gold

197

111

Rg

roen

tgen

ium

–

30 Zn zinc 65 48 Cd

cadm

ium

112

80 Hg

mer

cury

201

112

Cn

cope

rnic

ium

–

114 Fl

flero

vium

–

116

Lvliv

erm

oriu

m–

7 Nni

troge

n14 15 P

phos

phor

us31 33 As

arse

nic

75 51 Sb

antim

ony

122

83 Bi

bism

uth

209

8 Oox

ygen

16 16 S sulfu

r32 34 Se

sele

nium

79 52 Tete

lluriu

m12

8

84 Po

polo

nium

–

9 Fflu

orin

e19 17 Cl

chlo

rine

35.5

35 Br

brom

ine

80 53 Iio

dine

127

85 At

asta

tine

–

10 Ne

neon 20 18 Ar

argo

n40 36 Kr

kryp

ton

84 54 Xe

xeno

n13

1

86 Rn

rado

n–

21 Sc

scan

dium

45 39 Yyt

trium 89

57–7

1la

ntha

noid

s

89–1

03ac

tinoi

ds

57 Lala

ntha

num

139

89 Ac

lant

hano

ids

actin

oids

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3 a

t roo

m te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.)

actin

ium

–

58 Ce

ceriu

m14

0

90 Th thor

ium

232

59 Pr

pras

eody

miu

m14

1

91 Pa

prot

actin

ium

231

60 Nd

neod

ymiu

m14

4

92 Uur

aniu

m23

8

61 Pm

prom

ethi

um– 93 Np

nept

uniu

m–

62 Sm

sam

ariu

m15

0

94 Pu

plut

oniu

m–

63 Eu

euro

pium

152

95 Am

amer

iciu

m–

64 Gd

gado

liniu

m15

7

96 Cm

curiu

m–

65 Tb terb

ium

159

97 Bk

berk

eliu

m–

66 Dy

dysp

rosi

um16

3

98 Cf

calif

orni

um–

67 Ho

holm

ium

165

99 Es

eins

tein

ium

–

68 Er

erbi

um16

7

100

Fm ferm

ium

–

69 Tm thul

ium

169

101

Md

men

dele

vium

–

70 Yb

ytte

rbiu

m17

3

102

No

nobe

lium

–

71 Lu lute

tium

175

103 Lr

law

renc

ium

–





CHEMISTRY 0620/43


1 hour 15 minutes






*2399434482*


2

0620/43/M/J/16© UCLES 2016

1 The diagram shows a blast furnace.

waste gases

raw materials:coke, Ciron ore, Fe2O3limestone, CaCO3

X

Y

(a) The following equations represent reactions which take place in the blast furnace.

A C + O2 → CO2

B CaCO3 → CaO + CO2

C CaO + SiO2 → CaSiO3

D CO2 + C → 2CO E Fe2O3 + 3CO → 2Fe + 3CO2

(i) Which reaction is used to increase the temperature inside the blast furnace? ........... [1]

(ii) Which reaction is an example of thermal decomposition? ........... [1]

(iii) In which reaction is carbon both oxidised and reduced? ........... [1]

(iv) Which equation shows the removal of an impurity from the iron? ........... [1]

(v) Which equation shows the reaction of an acidic substance with a basic substance?

........... [1]

(b) Use the diagram of the blast furnace to help you answer these questions.

(i) What enters the blast furnace at X?

....................................................................................................................................... [1]

(ii) What leaves the blast furnace at Y?

....................................................................................................................................... [1]

3


(iii) Name two waste gases that leave the blast furnace.

1. .........................................................................................................................................

2. .........................................................................................................................................[2]

(c) The graph shows how the malleability of iron changes as the percentage of carbon in the iron changes.

increasing percentageof carbon

malleability

high

low

(i) Describe how the malleability of iron changes as the percentage of carbon changes.

.............................................................................................................................................

....................................................................................................................................... [1]

(ii) Iron obtained from the blast furnace contains high levels of carbon.

Explain how the amount of carbon in the iron can be decreased.

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [2]

[Total: 12]

4

0620/43/M/J/16© UCLES 2016

2 The structures of six organic compounds are shown.

H C

H H

A

H H

C C

H H

B

C C

H

H H

H

C H

H C

HC

H

H H H

C

H

C

H H

H

H C

H

C

D E F

H O H

C

O

H C

H H

H OH

C H H HC

H H

H H

C C

H H

H H

C

(a) Give the name of F.

.............................................................................................................................................. [1]

(b) Identify two of the compounds that are members of the same homologous series. Give the general formula of this homologous series.

compounds ................................................................................................................................

general formula ..........................................................................................................................[2]

(c) Which two compounds are isomers of each other? Explain why they are isomers.

compounds ................................................................................................................................

explanation ................................................................................................................................

....................................................................................................................................................[3]

(d) Explain why B is an unsaturated hydrocarbon.

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [2]

5


(e) Describe how D is manufactured from B. Give a chemical equation for the reaction.

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [3]

(f) Compound A forms an addition polymer.

Draw two repeat units of the addition polymer formed from A.

[2]

[Total: 13]

6

0620/43/M/J/16© UCLES 2016

3 Clean dry air contains mainly nitrogen and oxygen.

(a) Name two other gases that are in clean dry air.

....................................................................................................................................................

.............................................................................................................................................. [2]

(b) Air often contains pollutants.

Identify three common gaseous pollutants in air and state how each of these pollutants are produced.

pollutant gas 1 ...........................................................................................................................

how it is produced ......................................................................................................................

....................................................................................................................................................

pollutant gas 2 ...........................................................................................................................


....................................................................................................................................................

pollutant gas 3 ...........................................................................................................................


....................................................................................................................................................[6]

[Total: 8]

7


4 (a) Potassium iodide is an ionic compound.

(i) Describe what happens, in terms of electron loss and gain, when a potassium atom reacts with an iodine atom.

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [2]

(ii) Describe the structure of solid potassium iodide. You may draw a diagram.

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [2]

(iii) Explain why potassium iodide has a high melting point.

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [2]

8

0620/43/M/J/16© UCLES 2016

(b) Potassium iodide and lead nitrate are both soluble. Lead iodide is insoluble.

(i) Describe how a pure dry sample of lead iodide could be made from solid potassium iodide and solid lead nitrate.

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [4]

(ii) Write an ionic equation for the formation of lead iodide, PbI2, when potassium iodide and lead nitrate react with each other.

State symbols are not required.

....................................................................................................................................... [2]

(c) When chlorine gas is bubbled through an aqueous solution of potassium iodide, a redox reaction takes place.

2I – + Cl 2 → I2 + 2Cl –

(i) State the colour change expected in this reaction.

start colour ..........................................................................................................................

end colour ...........................................................................................................................[2]

(ii) Identify the reducing agent in this reaction. Explain your answer.

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [2]

[Total: 16]

9


5 Dilute hydrochloric acid reacts with sodium carbonate solution.

2HCl (aq) + Na2CO3(aq) → 2NaCl (aq) + H2O(l) + CO2(g)

(a) Explain why effervescence is seen during the reaction.

....................................................................................................................................................

.............................................................................................................................................. [1]

(b) Dilute hydrochloric acid was titrated with sodium carbonate solution.

• 10.0 cm3 of 0.100 mol / dm3 hydrochloric acid were placed in a conical flask. • A few drops of methyl orange indicator were added to the dilute hydrochloric acid. • The mixture was titrated with sodium carbonate solution. • 16.2 cm3 of sodium carbonate solution were required to react completely with the acid.

(i) What colour would the methyl orange indicator be in the hydrochloric acid?

....................................................................................................................................... [1]

(ii) Calculate how many moles of hydrochloric acid were used.

............................ mol [1]

(iii) Use your answer to (b)(ii) and the equation for the reaction to calculate the number of moles of sodium carbonate that reacted.

............................ mol [1]

(iv) Use your answer to (b)(iii) to calculate the concentration of the sodium carbonate solution in mol / dm3.

............................ mol / dm3 [2]

(c) In another experiment, 0.020 mol of sodium carbonate were reacted with excess hydrochloric acid.

Calculate the maximum volume (at r.t.p.) of carbon dioxide gas that could be made in this reaction.

............................ dm3 [3]

[Total: 9]

10

0620/43/M/J/16© UCLES 2016

6 Concentrated ammonia solution gives off ammonia gas. Concentrated hydrochloric acid gives off hydrogen chloride gas. Ammonia, NH3, and hydrogen chloride, HCl, are both colourless gases.

Ammonia reacts with hydrogen chloride to make the white solid ammonium chloride.

Apparatus is set up as shown.

cotton woolsoaked in concentrated

hydrochloric acid

cotton woolsoaked in concentrated

ammonia solution

glass tube

A B C D

After ten minutes a white solid forms in the tube where the gases meet.

(a) (i) Write the chemical equation for the reaction of ammonia with hydrogen chloride.

....................................................................................................................................... [1]

(ii) Name the process by which the ammonia and hydrogen chloride gases move in the tube.

....................................................................................................................................... [1]

(iii) At which point, A, B, C or D, does the white solid form? Explain why the white solid forms at that point.

the solid forms at ..............

explanation .........................................................................................................................

.............................................................................................................................................[3]

(iv) The experiment was repeated at a higher temperature.

Predict how the results of the experiment would be different. Explain your answer.

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [3]

11


(b) Some of the white solid is removed from the tube and dissolved in water.

Describe how the white solid could be tested to show it contains,

(i) ammonium ions,

test ......................................................................................................................................

.............................................................................................................................................

result ...................................................................................................................................

.............................................................................................................................................[3]

(ii) chloride ions.

test ......................................................................................................................................

.............................................................................................................................................

result ...................................................................................................................................

.............................................................................................................................................[3]

(c) The diagram shows the electron arrangement in a molecule of ammonia, showing only outer shell electrons.

N H

H

H

(i) State the type of bonding in ammonia.

....................................................................................................................................... [1]

12

0620/43/M/J/16© UCLES 2016

(ii) Hydrazine, N2H4, is another compound of nitrogen and hydrogen.

Complete the diagram to show the electron arrangement in a molecule of hydrazine, showing only outer shell electrons.

NN

H

H

H

H

[3]

(d) Nylon and proteins are both polymers containing nitrogen.

(i) Name the linkages found in the polymers of nylon and protein.

....................................................................................................................................... [1]

(ii) Describe one difference in the structures of nylon and protein.

....................................................................................................................................... [1]

(iii) What is the general name given to the products of hydrolysis of proteins?

....................................................................................................................................... [1]

13


(e) Suggest the structure of the monomer used to make the polymer shown.

N

H

C

O

n

[1]

[Total: 22]

14

0620/43/M/J/16© UCLES 2016

BLANK PAGE

15

0620/43/M/J/16© UCLES 2016




BLANK PAGE

16

0620/43/M/J/16© UCLES 2016

Gro

up

The

Perio

dic

Tabl

e of

Ele

men

ts

1 Hhy

drog

en1

2 He

heliu

m4

III

IIIIV

VV

IV

IIV

III

3 Lilit

hium 7

4 Be

bery

llium

9

atom

ic n

umbe

r

atom

ic s

ymbo

l

Key

nam

ere

lativ

e at

omic

mas

s

11 Na

sodi

um23

12 Mg

mag

nesi

um24

19 Kpo

tass

ium

39

20 Ca

calc

ium

40

37 Rb

rubi

dium

85

38 Sr

stro

ntiu

m88

55 Cs

caes

ium

133

56 Ba

bariu

m13

7

87 Frfra

nciu

m–

88 Ra

radi

um –

5 B boro

n11 13 Al

alum

iniu

m27 31 Ga

galli

um70 49 In indi

um11

5

81 Tlth

alliu

m20

4

6 Cca

rbon

12 14 Si

silic

on28 32 Ge

germ

aniu

m73 50 Sn tin 119

82 Pb

lead

207

22 Titit

aniu

m48 40 Zr

zirc

oniu

m91 72 Hf

hafn

ium

178

104

Rf

ruth

erfo

rdiu

m–

23 Vva

nadi

um51 41 Nb

niob

ium

93 73 Tata

ntal

um18

1

105

Db

dubn

ium

–

24 Cr

chro

miu

m52 42 Mo

mol

ybde

num

96 74 Wtu

ngst

en18

4

106

Sg

seab

orgi

um–

25 Mn

man

gane

se55 43 Tc

tech

netiu

m– 75 Re

rhen

ium

186

107

Bh

bohr

ium

–

26 Fe iron

56 44 Ru

ruth

eniu

m10

1

76 Os

osm

ium

190

108

Hs

hass

ium

–

27 Co

coba

lt59 45 Rh

rhod

ium

103

77 Iriri

dium

192

109

Mt

mei

tner

ium

–

28 Ni

nick

el59 46 Pd

palla

dium

106

78 Pt

plat

inum

195

110

Ds

darm

stad

tium

–

29 Cu

copp

er64 47 Ag

silv

er10

8

79 Au

gold

197

111

Rg

roen

tgen

ium

–

30 Zn zinc 65 48 Cd

cadm

ium

112

80 Hg

mer

cury

201

112

Cn

cope

rnic

ium

–

114 Fl

flero

vium

–

116

Lvliv

erm

oriu

m–

7 Nni

troge

n14 15 P

phos

phor

us31 33 As

arse

nic

75 51 Sb

antim

ony

122

83 Bi

bism

uth

209

8 Oox

ygen

16 16 S sulfu

r32 34 Se

sele

nium

79 52 Tete

lluriu

m12

8

84 Po

polo

nium

–

9 Fflu

orin

e19 17 Cl

chlo

rine

35.5

35 Br

brom

ine

80 53 Iio

dine

127

85 At

asta

tine

–

10 Ne

neon 20 18 Ar

argo

n40 36 Kr

kryp

ton

84 54 Xe

xeno

n13

1

86 Rn

rado

n–

21 Sc

scan

dium

45 39 Yyt

trium 89

57–7

1la

ntha

noid

s

89–1

03ac

tinoi

ds

57 Lala

ntha

num

139

89 Ac

lant

hano

ids

actin

oids

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3 a

t roo

m te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.)

actin

ium

–

58 Ce

ceriu

m14

0

90 Th thor

ium

232

59 Pr

pras

eody

miu

m14

1

91 Pa

prot

actin

ium

231

60 Nd

neod

ymiu

m14

4

92 Uur

aniu

m23

8

61 Pm

prom

ethi

um– 93 Np

nept

uniu

m–

62 Sm

sam

ariu

m15

0

94 Pu

plut

oniu

m–

63 Eu

euro

pium

152

95 Am

amer

iciu

m–

64 Gd

gado

liniu

m15

7

96 Cm

curiu

m–

65 Tb terb

ium

159

97 Bk

berk

eliu

m–

66 Dy

dysp

rosi

um16

3

98 Cf

calif

orni

um–

67 Ho

holm

ium

165

99 Es

eins

tein

ium

–

68 Er

erbi

um16

7

100

Fm ferm

ium

–

69 Tm thul

ium

169

101

Md

men

dele

vium

–

70 Yb

ytte

rbiu

m17

3

102

No

nobe

lium

–

71 Lu lute

tium

175

103 Lr

law

renc

ium

–



Answer all questions.Electronic calculators may be used.You may lose marks if you do not show your working or if you do not use appropriate units.Practical notes are provided on pages 7 and 8.


CHEMISTRY 0620/51

Paper 5 Practical Test May/June 2016

1 hour 15 minutes


Additional Materials: As listed in the Confidential Instructions




*8113146472*


For Examiner’s Use

Total

2

0620/51/M/J/16© UCLES 2016

1 You are going to investigate the reaction between aqueous sodium carbonate and two different solutions of dilute hydrochloric acid labelled A and B.

Read all the instructions carefully before starting the experiments.

Instructions You are going to carry out three experiments.

(a) Experiment 1

Use a measuring cylinder to pour 25 cm3 of aqueous sodium carbonate into a conical flask. Add ten drops of thymolphthalein indicator to the conical flask. Fill the burette provided up to the 0.0 cm3 mark with solution A of dilute hydrochloric acid.

Add solution A from the burette while swirling the flask, until the solution just changes colour. Record the burette readings in the table below.

Experiment 2

Empty the conical flask and rinse it with distilled water. Repeat Experiment 1 using methyl orange indicator instead of thymolphthalein. Record the burette readings in the table below and complete the table.

Experiment 1 Experiment 2

final burette reading / cm3

initial burette reading / cm3

difference / cm3

[4]

(b) Experiment 3

Empty the conical flask and rinse it with distilled water. Pour away the contents of the burette and rinse the burette with solution B of dilute

hydrochloric acid. Repeat Experiment 1 using solution B instead of solution A. Record the burette readings in the table below and complete the table.

Experiment 3



difference / cm3

[2]

(c) What colour change was observed in the flask in Experiment 1?

from .............................................................. to .................................................................. [1]

3


(d) State one observation, other than colour change, when hydrochloric acid was added to sodium carbonate.

.............................................................................................................................................. [1]

(e) Complete the sentence below.

Experiment ........... needed the largest volume of hydrochloric acid to change the colour of the indicator. [1]

(f) What would be a more accurate method of measuring the volume of the aqueous sodium carbonate?

.............................................................................................................................................. [1]

(g) What would be the effect on the results, if any, if the solutions of sodium carbonate were warmed before adding the hydrochloric acid? Give a reason for your answer.

effect on results .........................................................................................................................

reason ........................................................................................................................................[2]

(h) (i) Determine the ratio of volumes of dilute hydrochloric acid used in Experiments 1 and 3.

....................................................................................................................................... [1]

(ii) Use your answer to (h)(i) to deduce how the concentration of solution A differs from that of solution B.

....................................................................................................................................... [1]

(i) Suggest a different method, using standard laboratory chemicals, to determine which of the solutions of dilute hydrochloric acid, A or B, is more concentrated.

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [3]

(j) Hydrochloric acid is hazardous.

Suggest one safety precaution to follow when using hydrochloric acid.

.............................................................................................................................................. [1]

[Total: 18]

4

0620/51/M/J/16© UCLES 2016

2 You are provided with two substances. Solid C is a salt and solution D is an aqueous solution of a different salt.

Carry out the following tests on each substance, recording all of your observations at each stage.

tests on solid C

Add about half of solid C to about 10 cm3 of distilled water in a test-tube and shake to dissolve.

Divide the solution into two equal portions in two test-tubes, and carry out the following tests.

(a) (i) Test the pH of the first portion of the solution.

pH ................................................................................................................................. [1]

(ii) To the second portion of the solution, add about 1 cm3 of dilute nitric acid followed by aqueous silver nitrate.

Record your observations.

....................................................................................................................................... [2]

(b) Carry out a flame test on the rest of solid C. Record your observations.

.............................................................................................................................................. [1]

(c) Identify solid C.

.............................................................................................................................................. [2]

tests on solution D

Divide the solution D into three equal portions in three test-tubes and carry out the following tests.

(d) (i) Describe the appearance of the solution.

....................................................................................................................................... [1]

(ii) To the first portion of the solution, add drops of aqueous sodium hydroxide until a change is seen.

Now add an excess of aqueous sodium hydroxide to the mixture. Record your observations.

.............................................................................................................................................

....................................................................................................................................... [3]

5


(iii) To the second portion of the solution, add drops of aqueous ammonia until a change is seen.

Now add an excess of aqueous ammonia to the mixture. Record your observations.

.............................................................................................................................................

....................................................................................................................................... [2]

(iv) To the third portion of the solution, add about 1 cm3 of dilute nitric acid followed by aqueous silver nitrate.


.............................................................................................................................................

....................................................................................................................................... [2]

(e) What conclusions can you draw about solution D?

....................................................................................................................................................

.............................................................................................................................................. [2]

[Total: 16]

6

0620/51/M/J/16© UCLES 2016

3 Calcium burns in air to form calcium oxide. The reaction is vigorous and some of the calcium oxide can be lost as smoke.

Plan an investigation to determine the maximum mass of oxygen that combines to form calcium oxide when 2 g of calcium granules are burnt in air.

You are provided with common laboratory apparatus and calcium granules.

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

..................................................................................................................................................... [6]

[Total: 6]

7

0620/51/M/J/16© UCLES 2016

NOTES FOR USE IN QUALITATIVE ANALYSISTest for anions

anion test test result

carbonate (CO32–) add dilute acid effervescence, carbon dioxide

produced

chloride (Cl –)

[in solution]acidify with dilute nitric acid, then add aqueous silver nitrate

white ppt.

bromide (Br –)[in solution]

acidify with dilute nitric acid, then add aqueous silver nitrate

cream ppt.

iodide (I–)[in solution]


yellow ppt.

nitrate (NO3–)

[in solution]add aqueous sodium hydroxide, then aluminium foil; warm carefully

ammonia produced

sulfate (SO42–)

[in solution]acidify, then add aqueous barium nitrate

white ppt.

sulfite (SO32–) add dilute hydrochloric acid, warm

gently and test for the presence ofsulfur dioxide

sulfur dioxide produced will turn acidified aqueous potassium manganate(VII) from purple to colourless

Test for aqueous cations

cation effect of aqueous sodium hydroxide effect of aqueous ammonia

aluminium (Al 3+) white ppt., soluble in excess giving a

colourless solutionwhite ppt., insoluble in excess

ammonium (NH4+) ammonia produced on warming –

calcium (Ca2+) white ppt., insoluble in excess no ppt. or very slight white ppt.

chromium(III) (Cr3+) green ppt., soluble in excess grey-green ppt., insoluble in excess

copper (Cu2+) light blue ppt., insoluble in excess light blue ppt., soluble in excess, giving a dark blue solution

iron(II) (Fe2+) green ppt., insoluble in excess green ppt., insoluble in excess

iron(III) (Fe3+) red-brown ppt., insoluble in excess red-brown ppt., insoluble in excess

zinc (Zn2+) white ppt., soluble in excess, giving a colourless solution

white ppt., soluble in excess, giving a colourless solution

8

0620/51/M/J/16© UCLES 2016




Test for gases Flame tests for metal ions

gas test and test results metal ion flame colour

ammonia (NH3) turns damp, red litmus paper blue lithium (Li+) red

carbon dioxide (CO2) turns limewater milky sodium (Na+) yellow

chlorine (Cl 2) bleaches damp litmus paper potassium (K+) lilac

hydrogen (H2) ‘pops’ with a lighted splint copper(II) (Cu2+) blue-green

oxygen (O2) relights a glowing splint

sulfur dioxide (SO2) turns acidifed aqueous potassium manganate(VII) from purple to colourless





CHEMISTRY 0620/52


1 hour 15 minutes






*3068860685*



Total

2

0620/52/M/J/16© UCLES 2016

1 You are going to investigate the rate of reaction between hydrogen peroxide and aqueous potassium iodide. When these chemicals react they form iodine. Sodium thiosulfate solution reacts with iodine and can be used to show how fast the reaction proceeds.

Read all the instructions carefully before starting the experiment.

Instructions

(a) Fill the burette up to the 40.0 cm3 mark with sodium thiosulfate solution. Use the large measuring cylinder to pour 100 cm3 of distilled water into the conical flask. Use the small measuring cylinder to add 6 cm3 of sulfuric acid, 1 cm3 of starch solution and

4 cm3 of aqueous potassium iodide to the flask. Add 1.0 cm3 of sodium thiosulfate solution from the burette to the mixture in the flask and swirl

to mix.

Several measurements will be taken during this experiment. Once the timer has been started leave it running until the experiment is complete.

Use the small measuring cylinder to start the reaction by adding 3 cm3 of hydrogen peroxide solution to the flask. Immediately start your timer and swirl the mixture.

Note the time taken for a blue colour to appear and record the time in the table.

Add a further 0.5 cm3 of sodium thiosulfate solution to the mixture in the conical flask and swirl until the blue colour disappears.

Note the time when the blue colour reappears and record the time in the table below.

Continue the experiment adding a further 0.5 cm3 of sodium thiosulfate solution at a time until a total of 4.0 cm3 of sodium thiosulfate solution has been added, noting the times for the blue colour to appear after each addition and recording the times in the table.

Complete the table.

total volume ofsodium thiosulfate solution

added / cm3

time at whichblue colour appears / s

1.0

1.5

4.0[4]

3


(b) Plot the results you have obtained on the grid and draw a best-fit straight-line graph.

0.0 0.5 1.0 1.5 2.0

volume of sodium thiosulfate solution / cm3

2.5 3.0 3.5 4.0 4.5

time/ s

[5]

(c) (i) From your graph deduce the time for the blue colour to appear if only 0.5 cm3 of sodium thiosulfate solution had been added to the mixture in the conical flask.

Show clearly on the grid how you worked out your answer.

....................................................................................................................................... [3]

(ii) Sketch on the grid the graph you would expect if the experiment was repeated at a higher temperature. [1]

4

0620/52/M/J/16© UCLES 2016

(d) Suggest the purpose of the starch solution.

.............................................................................................................................................. [1]

(e) (i) Suggest one advantage of using a pipette to measure the volume of the hydrogen peroxide.

....................................................................................................................................... [1]

(ii) Suggest and explain one disadvantage of using a pipette to measure the volume of the hydrogen peroxide.

.............................................................................................................................................

....................................................................................................................................... [2]

(f) Explain one disadvantage of using a beaker instead of a conical flask.

....................................................................................................................................................

.............................................................................................................................................. [1]

[Total: 18]

5


2 You are provided with two solids, E and F, which are both water soluble. Carry out the following tests on the solids, recording all of your observations at each stage.

tests on solid E

(a) Use a spatula to place half of solid E into a test-tube. Add about 10 cm3 of distilled water to the solid and shake the mixture to dissolve.

Divide the solution into three equal portions in three test-tubes and carry out the following tests.

(i) Add about 1 cm3 of aqueous sodium hydroxide to the first portion of the solution. Record your observations.

....................................................................................................................................... [1]

(ii) Add about 1 cm3 of aqueous barium nitrate to the second portion of the solution. Now add excess dilute nitric acid to the mixture. Record your observations.

.............................................................................................................................................

....................................................................................................................................... [2]

(iii) Pour the third portion of the solution into a boiling tube and add about 1 cm3 of dilute hydrochloric acid. Warm the mixture gently. Test the gas given off with a piece of filter paper soaked in aqueous potassium manganate(VII) solution.


.............................................................................................................................................

....................................................................................................................................... [2]

(b) Carry out a flame test on the rest of solid E. Record your observations.

.............................................................................................................................................. [1]

(c) What conclusions can you draw about solid E?

....................................................................................................................................................

.............................................................................................................................................. [2]

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tests on solid F

Use a spatula to divide solid F into two portions in two test-tubes.

(d) Describe the appearance of solid F.

.............................................................................................................................................. [1]

(e) (i) Heat the first portion of solid F, gently then strongly. Test the gas given off with damp red litmus paper. Record your observations.

.............................................................................................................................................

....................................................................................................................................... [3]

(ii) Let the solid residue cool down for a few minutes. To the residue add a few drops of copper(II) sulfate solution followed by a few drops of aqueous sodium hydroxide and shake the mixture.


....................................................................................................................................... [1]

(f) Tip the second portion of solid F into a boiling tube. Add about 3 cm3 of aqueous sodium hydroxide to the boiling tube and heat the mixture gently.

Test the gas given off. Record your observations.

....................................................................................................................................................

.............................................................................................................................................. [2]

(g) Identify one of the ions in solid F.

.............................................................................................................................................. [1]

[Total: 16]

7


3 Potassium sulfate is the salt made when sulfuric acid is neutralised by potassium hydroxide solution. The correct amount of potassium hydroxide solution must be added to neutralise all of the sulfuric

acid. Plan an experiment to obtain pure crystals of potassium sulfate from sulfuric acid and

potassium hydroxide solution. You are provided with common laboratory apparatus.

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

..................................................................................................................................................... [6]

[Total: 6]

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produced

chloride (Cl –)


white ppt.



cream ppt.



yellow ppt.

nitrate (NO3–)


ammonia produced

sulfate (SO42–)


white ppt.
















12

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CHEMISTRY 0620/53


1 hour 15 minutes






*9424482312*



Total

2

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1 You are going to investigate what happens when dilute hydrochloric acid and copper(II) sulfate solution react with different metals.

Read all the instructions carefully before starting the experiments.

Instructions You are going to carry out five experiments.

(a) Experiment 1

Use a measuring cylinder to pour 10 cm3 of dilute hydrochloric acid into a boiling tube. Put the boiling tube into a rack for support.

Measure the temperature of the hydrochloric acid and record it in the table below. Add 1 g of zinc to the boiling tube and stir the mixture with the thermometer. Measure and record the maximum temperature reached by the mixture. Pour the mixture away

and rinse the boiling tube.

Experiment 2

Repeat Experiment 1 using 1 g of iron instead of zinc. Record your results in the table.

Experiment 3

Repeat Experiment 1 using 1 g of magnesium instead of zinc. Record your results in the table. Complete the final column in the table.

experiment initial temperatureof acid / °C

maximum temperaturereached / °C

temperaturerise / °C

1

2

3[3]

(b) Experiment 4

Use a measuring cylinder to pour 10 cm3 of copper(II) sulfate solution into a boiling tube. Measure the temperature of the solution and record it in the table on page 3.

Add 1 g of magnesium to the boiling tube and stir the mixture with the thermometer. Test the gas given off with a splint and record your result in the space below. Measure the

maximum temperature reached by the mixture and record it in the table. Pour the mixture away and rinse the boiling tube.

test .............................................................................................................................................

result ..........................................................................................................................................[1]

3


(c) Experiment 5

Repeat Experiment 4 using 1 g of iron instead of magnesium. You do not need to test the gas. Record your observations in the space below and record your temperatures in the table.

Complete the final column in the table.

experiment initial temperature / °C maximumtemperature / °C


4

5

observation ................................................................................................................................[3]

(d) Draw a labelled bar chart for the results of Experiments 1, 2, 3, 4 and 5 on the grid.


[3]

4

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Use your results and observations for Experiments 1, 2 and 3 to answer the following questions.

(e) (i) Which experiment, 1, 2 or 3, produced the largest temperature rise?

....................................................................................................................................... [1]

(ii) Suggest why this experiment produced the largest temperature rise.

.............................................................................................................................................

....................................................................................................................................... [1]

(f) Name the gas given off in Experiment 4.

.............................................................................................................................................. [1]

(g) Suggest why potassium was not used as one of the metals in these experiments.

.............................................................................................................................................. [1]

(h) Give one advantage of using a measuring cylinder to add the hydrochloric acid to the boiling tube.

.............................................................................................................................................. [1]

(i) Suggest and explain one change to improve the accuracy of these experiments.

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [2]

[Total: 17]

5


2 You are provided with a mixture of two solids, G and H. Solid G is water soluble and solid H is insoluble in water. Carry out the following tests on the mixture, recording all of your observations at each stage.

Add about 15 cm3 of distilled water to the mixture in a boiling tube. Shake the boiling tube for one minute. Filter the contents of the tube, keeping the filtrate and the

residue. Divide the filtrate into four equal portions in four test-tubes and carry out the following tests.

tests on filtrate

(a) (i) Add several drops of aqueous sodium hydroxide to the first portion of the solution and shake the test-tube.

Now add excess aqueous sodium hydroxide to the test-tube. Record your observations.

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [3]

(ii) Using the second portion of the solution, repeat the test in (a)(i) using aqueous ammonia instead of aqueous sodium hydroxide.


.............................................................................................................................................

....................................................................................................................................... [2]

(iii) Add a few drops of dilute nitric acid to the third portion of the solution followed by about 1 cm3 of aqueous silver nitrate.


....................................................................................................................................... [1]

(iv) Pour the fourth portion of the solution into a boiling tube. Add about 1 cm3 of aqueous sodium hydroxide and a small piece of aluminium foil. Warm the mixture carefully and test the gas given off. Record your observations.

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [3]

(b) Identify solid G.

....................................................................................................................................................

.............................................................................................................................................. [2]

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tests on the residue

(c) Use a spatula to transfer some of the residue into a test-tube. To the residue, add about 2 cm3 of dilute hydrochloric acid. Test any gases given off. Record your observations.

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [3]

(d) Carry out a flame test on the residue. Record your observations.

.............................................................................................................................................. [1]

(e) Identify solid H.

....................................................................................................................................................

.............................................................................................................................................. [2]

[Total: 17]

7


3 Nickel sulfate-6-water, NiSO4.6H2O, is a blue crystalline salt. Plan an experiment to obtain a sample of pure water from this salt. Your answer should include

a diagram of the apparatus, any expected observations and a test to show the presence of pure water.

You are provided with common laboratory apparatus.

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

..................................................................................................................................................... [6]

[Total: 6]

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11

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produced

chloride (Cl –)


white ppt.



cream ppt.



yellow ppt.

nitrate (NO3–)


ammonia produced

sulfate (SO42–)


white ppt.
















12

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*3845366912*



Answer all questions.Electronic calculators may be used.You may lose marks if you do not show your working or if you do not use appropriate units.


CHEMISTRY 0620/61

Paper 6 Alternative to Practical May/June 2016

1 hour





2

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1 The diagram shows the apparatus used to separate a mixture of water, boiling point 100 °C, and ethanol, boiling point 78 °C.

heatheat

water andethanol mixture

condenser

(a) Complete the boxes to name the apparatus. [2]

(b) Label the arrows on the condenser. [1]

(c) Identify one mistake in the apparatus.

.............................................................................................................................................. [1]

(d) Which liquid would collect first? Explain your answer.

....................................................................................................................................................

.............................................................................................................................................. [2]

(e) Why would it be better to use an electrical heater instead of a Bunsen burner to heat the water and ethanol mixture?

.............................................................................................................................................. [1]

[Total: 7]

3


2 A student investigated the reaction between aqueous sodium carbonate and two different solutions of dilute hydrochloric acid, A and B.

The reaction is:

Na2CO3(aq) + 2HCl (aq) → 2NaCl (aq) + H2O(l) + CO2(g)

Three experiments were carried out.

(a) Experiment 1

Using a measuring cylinder, 25 cm3 of aqueous sodium carbonate were poured into a conical flask.

Thymolphthalein indicator was added to the conical flask. A burette was filled up to the 0.0 cm3 mark with solution A of dilute hydrochloric acid. A was

added to the flask, until the solution just changed colour. Use the burette diagram to record the reading in the table.

12

13

14

final reading

Experiment 2

Experiment 1 was repeated using methyl orange indicator instead of thymolphthalein. Methyl orange is red-orange in acidic solutions and yellow in alkaline solutions. Use the burette diagrams to record the readings in the table and complete the table.

38

39

40

final reading

12

13

14

initial reading

experiment 1 experiment 2



difference / cm3

[4]

4

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(b) What colour change was observed in the flask in experiment 2?

from ................................................................ to ................................................................ [1]

(c) Experiment 3

Experiment 1 was repeated using solution B of acid instead of solution A.

Use the burette diagrams to record the readings in the table and complete the table.

15

16

17

final reading

8

9

10

initial reading

experiment 3



difference / cm3

[2]

(d) Suggest one observation, other than colour change, that is made when hydrochloric acid is added to sodium carbonate.

.............................................................................................................................................. [1]

(e) Complete the sentence below.

Experiment .......... needed the largest volume of hydrochloric acid to change the colour of the indicator. [1]

(f) What would be a more accurate method of measuring the volume of the aqueous sodium carbonate?

.............................................................................................................................................. [1]

5


(g) What would be the effect on the results, if any, if the solutions of sodium carbonate were warmed before adding the hydrochloric acid? Give a reason for your answer.

effect on results .........................................................................................................................

reason ........................................................................................................................................[2]

(h) (i) Determine the ratio of volumes of dilute hydrochloric acid used in experiments 1 and 3.

....................................................................................................................................... [1]

(ii) Use your answer to (h)(i) to deduce how the concentration of solution A differs from that of solution B.

....................................................................................................................................... [1]

(i) Suggest a different method, using standard laboratory chemicals, to determine which of the solutions of dilute hydrochloric acid, A or B, is more concentrated.

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [3]

[Total: 17]

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3 Two substances, C and D, were analysed. Solid C was a salt and solution D was an aqueous solution of chromium(III) chloride.

The tests on solid C, and some of the observations, are in the following table.

tests observations

tests on solid C

Solid C was added to distilled water in a test-tube and shaken to dissolve.

The solution was divided into two portions in test-tubes, and the following tests carried out.

Appearance of the solution.

The pH of the first portion of the solution was tested.

colourless liquid

pH = 7

Dilute nitric acid was added to the second portion of the solution followed by aqueous silver nitrate.

cream precipitate

A flame test was carried out on solid C. yellow flame colour

(a) Identify solid C.

.............................................................................................................................................. [2]

(b) Describe the appearance of solution D.

.............................................................................................................................................. [1]

(c) Tests were carried out on solution D.

Complete the observations for tests 1, 2 and 3.

(i) test 1

Drops of aqueous sodium hydroxide were added to solution D.

Excess aqueous sodium hydroxide was then added to the mixture.

observations .......................................................................................................................

....................................................................................................................................... [3]

7


(ii) test 2

Excess aqueous ammonia was added to solution D.

observations ................................................................................................................. [2]

(iii) test 3

Dilute nitric acid was added to solution D followed by aqueous silver nitrate.

observations ................................................................................................................. [1]

(d) Chromium(III) can be converted to chromium(VI). Chromium(VI) is hazardous.

Suggest one safety precaution when using chromium(VI).

.............................................................................................................................................. [1]

[Total: 10]

8

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4 Calcium burns in air to form calcium oxide. The reaction is vigorous and some of the calcium oxide can be lost as smoke.

Plan an investigation to determine the maximum mass of oxygen that combines to form calcium oxide when 2 g of calcium granules are burnt in air.

You are provided with common laboratory apparatus and calcium granules.

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

..................................................................................................................................................... [6]

[Total: 6]



*2553361951*





CHEMISTRY 0620/62


1 hour





2

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1 The diagram shows the apparatus used to reduce copper(II) oxide with hydrogen.

hydrogen

copper(II) oxide excess hydrogenburning in air

ice

colourless liquid

(a) Complete the boxes to name the apparatus. [2]

(b) Use an arrow to indicate where heat is applied. [1]

(c) The colour of the copper(II) oxide changes from ............................. to ............................ . [2]

(d) Suggest a reason why the U-tube is surrounded by ice.

.............................................................................................................................................. [1]

(e) (i) Identify the colourless liquid formed.

....................................................................................................................................... [1]

(ii) Give a chemical test for this liquid.

test ......................................................................................................................................

result ...................................................................................................................................[2]

(iii) How could you show that this liquid is pure?

....................................................................................................................................... [1]

[Total: 10]

3


2 A student investigated the rate of reaction between hydrogen peroxide and aqueouspotassium iodide. When these chemicals react they form iodine. Sodium thiosulfate solution reacts with iodine and can be used to show how fast the reaction proceeds.

(a) A burette was filled up to the 0.0 cm3 mark with sodium thiosulfate solution. Using a large measuring cylinder, 100 cm3 of distilled water were poured into a conical flask. Using a small measuring cylinder, 6 cm3 of sulfuric acid, 1 cm3 of starch solution and 4 cm3 of

aqueous potassium iodide were added to the flask. 0.5 cm3 of sodium thiosulfate solution was added from the burette to the mixture in the flask

and swirled to mix. The reaction was then started by adding 3 cm3 of hydrogen peroxide solution to the mixture,

and the timer started. The time taken for a blue colour to appear was noted. A further 0.5 cm3 of sodium thiosulfate solution was added to the mixture in the conical flask,

swirled and the blue colour disappeared. The time when the blue colour reappeared was noted. The experiment continued by adding further 0.5 cm3 portions of sodium thiosulfate solution

until a total of 3.0 cm3 of sodium thiosulfate solution had been added, noting the times at which the blue colour reappeared.

Use the timer diagrams on page 4 to record the times in seconds in the table.

4

0620/62/M/J/16© UCLES 2016

0.5

total volume ofsodium thiosulfate

solution added / cm3

timerdiagram

time at whichblue colourappeared / s

1.0

1.5

2.0

2.5

3.0

seconds

minutes

0

0

10

30

151545 5

0

0

10

30

151545 5

0

0

10

30

151545 5

0

0

10

30

151545 5

0

0

10

30

151545 5

0

0

10

30

151545 5

[3]

5


(b) Plot the results you have obtained on the grid and draw a best-fit straight-line graph.

0.0 0.5 1.0 1.5 2.0

volume of sodium thiosulfate solution / cm3

2.5 3.0 3.5 4.0

time / s

[5]

(c) (i) From your graph deduce the time at which the blue colour would appear if a total of 4.0 cm3 of sodium thiosulfate solution were added to the mixture in the conical flask.

Show clearly on the grid how you worked out your answer.

....................................................................................................................................... [3]

(ii) Sketch on the grid the graph you would expect if the experiment was repeated at a higher temperature. [1]

6

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(d) Suggest the purpose of the starch solution.

.............................................................................................................................................. [1]

(e) (i) Suggest one advantage of using a pipette to measure the volume of the hydrogen peroxide.

....................................................................................................................................... [1]

(ii) Suggest and explain one disadvantage of using a pipette to measure the volume of the hydrogen peroxide.

.............................................................................................................................................

....................................................................................................................................... [2]

(f) Explain one disadvantage of using a beaker instead of a conical flask.

....................................................................................................................................................

.............................................................................................................................................. [1]

[Total: 17]

7


3 Two solids, E and F, were analysed. Solid E was sodium sulfite. Both solids were found to be water soluble.

The tests on the solids, and some of the observations, are shown below.

tests on solid E

(a) Describe the appearance of the solid.

.............................................................................................................................................. [1]

(b) Distilled water was added to solid E in a test-tube and shaken to dissolve.

The solution was divided into two portions in two test-tubes and the following tests carried out.

(i) Aqueous sodium hydroxide was added to the first portion of the solution.

observations ................................................................................................................. [1]

(ii) Dilute hydrochloric acid was added to the second portion of the solution. The mixture was warmed. The gas given off was tested with a piece of filter paper soaked in aqueous acidified potassium manganate(VII) solution.

observations .......................................................................................................................

....................................................................................................................................... [2]

(c) A flame test was carried out on solid E.

observations ........................................................................................................................ [1]

tests on solid F

tests observations

The solid was heated. The gas given off was tested with damp, red litmus paper.

pungent gas evolved

red litmus paper turned blue

Aqueous sodium hydroxide was added to solid F and the mixture heated. The gas given off was tested.

pungent gas evolved

Universal Indicator paper showed pH 10

(d) Identify the gas given off in the tests on solid F.

.............................................................................................................................................. [1]

(e) Identify one of the ions in solid F.

.............................................................................................................................................. [1]

[Total: 7]

8

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4 Potassium sulfate is the salt produced when sulfuric acid is neutralised by potassium hydroxide solution.

The correct amount of potassium hydroxide solution must be added to neutralise all of the sulfuric acid.

Plan an experiment to obtain pure crystals of potassium sulfate from sulfuric acid and potassium hydroxide solution.


...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

..................................................................................................................................................... [6]

[Total: 6]



*9448353441*





CHEMISTRY 0620/63


1 hour





2

0620/63/M/J/16© UCLES 2016

1 Air is a mixture of gases. The diagram shows the apparatus used to find the percentage of oxygen in air.

50 cm3 of air were passed backwards and forwards over excess heated copper until there was no further change. The apparatus was left to cool and the volume of gas remaining was 40 cm3.

20 40 60 80 10020406080100

copper

(a) Complete the box to name the apparatus. [1]

(b) Use an arrow to indicate where heat is applied. [1]

(c) The colour of the copper changed from ........................... to ........................... . [2]

(d) From the results, work out the percentage of oxygen in the air.

............................ % [2]

[Total: 6]

3


2 A student investigated what happens when dilute hydrochloric acid and copper(II) sulfate solution react with different metals.

Five experiments were carried out.

(a) Experiment 1

A measuring cylinder was used to pour 10 cm3 of dilute hydrochloric acid into a boiling tube. The temperature of the hydrochloric acid was measured. 1 g of zinc was added to the boiling tube and the mixture stirred with a thermometer. The maximum temperature reached by the mixture was measured.

Experiment 2

Experiment 1 was repeated using 1 g of iron instead of zinc.

Experiment 3

Experiment 1 was repeated using 1 g of magnesium instead of zinc.

Use the thermometer diagrams to record the results in the table. Complete the final column in the table.

experiment thermometerdiagram

initialtemperatureof acid / °C

thermometerdiagram

maximumtemperaturereached / °C


1

30

25

20

30

25

20

2

30

25

20

30

25

20

3

30

25

20

65

60

55

[3]

(b) The gas produced in experiment 3 was tested with a lighted splint and the result recorded below.

test ............................................................................ result ............................................................................

Name the gas given off in experiment 3.

.............................................................................................................................................. [1]

lighted splintpopped

4

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(c) Experiment 4

A measuring cylinder was used to pour 10 cm3 of copper(II) sulfate solution into a boiling tube. The temperature of the solution was measured.

1 g of magnesium was added to the boiling tube and the mixture stirred with a thermometer. The maximum temperature reached by the mixture was measured.

Experiment 5

Experiment 4 was repeated using 1 g of iron instead of magnesium. The observation was recorded below.

..............................................................................................................

Use the thermometer diagrams to record the results in the table. Complete the final column in the table.

experiment thermometerdiagram

initialtemperatureof acid / °C

thermometerdiagram

maximumtemperaturereached / °C


4

30

25

20

50

45

40

5

30

25

20

30

25

20

[2]

The solution turned colourless and a brown deposit formed.

5


(d) Draw a labelled bar chart for the results of experiments 1, 2, 3, 4 and 5 on the grid below.


[3]

(e) Use the results for experiments 1, 2 and 3 to answer the following questions.

(i) Which experiment, 1, 2 or 3, produced the largest temperature rise?

....................................................................................................................................... [1]

(ii) Suggest why this experiment produced the largest temperature rise.

.............................................................................................................................................

....................................................................................................................................... [1]

6

0620/63/M/J/16© UCLES 2016

(f) Explain the observations in experiment 5.

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [2]

(g) Suggest why potassium was not used as one of the metals in these experiments.

.............................................................................................................................................. [1]

(h) Give one advantage of using a measuring cylinder to add the hydrochloric acid to the boiling tube.

.............................................................................................................................................. [1]

(i) Suggest and explain one improvement to increase the accuracy of these experiments.

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [2]

[Total: 17]

7


3 A mixture of two solids, G and H, was analysed. Solid G was zinc nitrate, which is water soluble, and solid H is insoluble in water.

The tests on the mixture, and some of the observations, are shown.

Distilled water was added to the mixture in a boiling tube and shaken. The contents of the boiling tube were filtered keeping the filtrate and the residue.

tests on filtrate

(a) The filtrate was divided into four test-tubes and the following tests carried out.

(i) Drops of aqueous sodium hydroxide were added to the first portion of the solution. Excess aqueous sodium hydroxide was then added to the test-tube.

observations .......................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [3]

(ii) Using the second portion of the solution, the test in (a)(i) was repeated using aqueous ammonia instead of aqueous sodium hydroxide.

observations .......................................................................................................................

....................................................................................................................................... [2]

(iii) Dilute nitric acid was added to the third portion of the solution followed by aqueous silver nitrate.

observations ................................................................................................................. [1]

(iv) Aqueous sodium hydroxide and aluminium foil were added to the fourth portion of the solution.

The mixture was warmed and the gas given off was tested.

observations .......................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [3]

8

0620/63/M/J/16© UCLES 2016

tests on residue

Two tests are carried out and the following observations made.

tests observations

A spatula was used to transfer some of the residue into a test-tube.

Dilute hydrochloric acid was added to the residue. The gas given off was tested.

rapid effervescence,limewater turned milky

A flame test was carried out on the residue. red flame colour

(b) Identify solid H.

....................................................................................................................................................

.............................................................................................................................................. [2]

[Total: 11]

9


4 Nickel sulfate-6-water, NiSO4.6H2O, is a blue crystalline salt.

Plan an experiment to obtain a sample of pure water from this salt. Your answer should include a diagram of the apparatus, any expected observations and a test to show the presence of pure water.


...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

..................................................................................................................................................... [6]

[Total: 6]

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