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- 1 -
Sixth Form Entrance 2017
CHEMISTRY
1 hour
Name (Capital Letters): ......................................................................
Present School: ……………………………………………………….
Answer ALL the questions
TOTAL MARK = 60
Answers to Section A should be answered on the question paper.
Answers to Section B should be written on the blank pages at the end of the question paper.
A copy of the Periodic Table is included with the question paper (back page).
If you know the name of the examination board and the title of the chemistry course you are
currently studying e.g. AQA Chemistry, Edexcel, OCR Gateway or 21st Century Science,
IGCSE write it below. Indicate if you are doing Triple Science (i.e. you will get separate
grades in Biology, Chemistry and Physics) or Double Science.
Board_________________ Course________________________ Triple/Double __________
- 2 -
SECTION A
Q1 Use the Periodic Table to help you with this question.
Complete the table below by putting in the missing symbols or numbers.
Symbol Number of
protons
Number of
neutrons
Mass
number
Electron
arrangement
P 15 16
11 23 2.8.1
Ca2+ 20
[TOTAL = 7]
Q2 (a) You are given the formulae of the following ions. Write the chemical formula of
the following substances. The first one is shown as an example.
Ion Formula Ion Formula
Ammonium NH4+ Iodide I−
Magnesium Mg2+ Nitride N3−
Lithium Li+ Hydroxide OH−
Potassium K+ Hydrogencarbonate HCO3−
Lead(II) Pb2+ Carbonate CO32−
Iron(III) Fe3+ Sulfate SO42−
Barium Ba2+ Nitrate NO3−
Example: barium hydroxide Ba(OH)2
(i) Ammonium iodide..........................................................................
(ii) Magnesium hydroxide....................................................................
(iii) Iron (III) nitrate.............................................................................
(iv) Lithium sulfate..............................................................................
(v) Barium nitride................................................................................
[5]
- 3 -
(b) Put numbers in front of the formulae as necessary to balance the equations
below:
(i) ........K + .........H2O .........KOH + .........H2
(ii) ........Fe2O3 + ........CO ........Fe + ..........CO2
(iii) ........C10H22 + ........O2 ........CO2 + ........H2O
[3]
[TOTAL = 8]
Q3 The following table gives some information about several substances.
Substance Melting
point /
°C
Boiling
point /
°C
Electrical
conductivity
when solid
Electrical
conductivity
when molten
Solubility in
water
A 1410 2355 poor poor insoluble
B -25 144 poor poor insoluble
C 712 1418 poor good soluble
D -101 -35 poor poor soluble
E 1660 3287 good good insoluble
For each of the substances, A to E, decided the type of bonding and structure present. Circle
the correct answers below.
(a) A: Bonding – Covalent / Ionic / Metallic
Structure – Giant / Simple Molecular
(b) B: Bonding – Covalent / Ionic / Metallic
Structure – Giant / Simple Molecular
(c) C: Bonding – Covalent / Ionic / Metallic
Structure – Giant / Simple Molecular
(d) D: Bonding – Covalent / Ionic / Metallic
Structure – Giant / Simple Molecular
(e) E: Bonding – Covalent / Ionic / Metallic
Structure – Giant / Simple Molecular
[TOTAL = 5]
- 4 -
Q4 The table shows the names of some common pieces of laboratory apparatus used to
make measurements.
(a) Complete the table to show the name of the quantity that can be measured by each piece
of apparatus, and a common unit used for that quantity. One example of each has been done
for you.
[6]
(b) Which piece of apparatus is needed to make measurements in a paper chromatography
experiment?
[1]
A balance
B gas syringe
C ruler
D stop clock
[TOTAL = 7]
- 5 -
Q5 The table shows the displayed formulae of six organic compounds, P, Q, R, S, T and U.
(a) (i) What is the molecular formula of compound S?
[1]
......................................................................................................................................................
(ii) What is the empirical formula of compound T?
[1]
......................................................................................................................................................
(b) (i) Give the letters of two compounds that belong to the homologous series of alkenes.
[1]
....................................................................... and .......................................................................
(ii) The general formula of this homologous series is
[1]
A CnH2n–2
B CnH2n+2
C Cn + H2n
D CnH2n
- 6 -
(c) Which of these conversions is an example of an addition reaction?
[1]
A compound P → compound Q
B compound Q → compound T
C compound R → compound Q
D compound R → compound U
(d)
Complete the table to show the displayed formula and name of the isomer of compound T.
[2]
(e) The equation represents a reaction between compound P and bromine.
(i) Complete the equation to show the displayed formula of the organic product.
[1]
(ii) State the name of this organic product.
[1]
......................................................................................................................................................
(iii) State the condition used in this reaction.
[1]
......................................................................................................................................................
- 7 -
(iv) What term is used for this type of reaction?
[1]
A addition
B hydration
C neutralisation
D substitution
[TOTAL = 11]
Q7. Some students investigated the rate of reaction between sodium thiosulfate solution
and hydrochloric acid. The equation for the reaction is
Na2S2O3(aq) + 2HCl(aq) → 2NaCl(aq) + H2O(l) + S(s) + SO2(g)
The precipitate of sulfur makes the reaction mixture go cloudy.
The students used this method.
Place a mixture of sodium thiosulfate solution and water in a conical flask
Add some dilute hydrochloric acid, swirl the mixture and start a timer
Place the flask over a black cross marked on a piece of paper
Record the time taken for the cross to disappear when viewed from above. The
students used 10 cm3 of dilute hydrochloric acid in each experiment.
They carried out all the experiments at the same temperature.
They used different volumes of sodium thiosulfate solution and water in each experiment.
They were told to keep the total volume of sodium thiosulfate solution and water constant.
The table shows their results.
- 8 -
(a) Explain why the results of student 7 should not be used.
[1]
..............................................................................................................................................
(b) Plot the results of the six other students on the grid below. Draw a curve of best fit
through the points.
[4]
- 9 -
(c) The students used this equation to calculate the rate of each reaction in their investigation.
Calculate the rate of reaction for student 1's experiment.
Give your answer to one decimal place.
[2]
Rate = ...............................................
(d) Another group of students used the same method but with different solutions of sodium
thiosulfate and hydrochloric acid. They calculated the rate of reaction for each experiment
they did. Their results are shown on the following graph.
- 10 -
(i) Describe the relationship between rate and concentration as shown by the graph.
[2]
......................................................................................................................................................
......................................................................................................................................................
......................................................................................................................................................
......................................................................................................................................................
(ii) Explain why increasing the concentration has this effect on the rate.
[3]
......................................................................................................................................................
......................................................................................................................................................
......................................................................................................................................................
......................................................................................................................................................
......................................................................................................................................................
......................................................................................................................................................
......................................................................................................................................................
[TOTAL = 12]
- 11 -
SECTION B
Write your answers to this section on the blank pages which follow.
Write notes on TWO of the following [5 marks each]. Use diagrams and chemical equations
where relevant.
(a) Cracking
(b) The structures, properties and uses of TWO polymers
(c) Catalysts
(d) The bonding and structure of graphite and diamond
(e) The manufacture of aluminium from its ore
(f) The industrial manufacture of ammonia
SECTION B ANSWER
- 13 -
3 11
19
37
55
87
4 12
20
38
56
88
21
39
57
89
22
40
72
104
23
41
73
105
24
42
74
106
25
43
75
58
90
59
91
60
92
61
93
62
94
63
95
64
96
65
97
66
98
67
99
68
100
69
101
70
102
71
103
26
44
76
27
45
77
28
46
78
29
47
79
30
48
80
5 13
31
49
81
6 14
32
50
82
7 15
33
51
83
8 16
34
52
84
9 17
35
53
85
10
18
36
54
86
Li
Na K Rb
Cs
Fr7 23
39
85
133
(223
)
9 24
40
88
137
(226
)
45
89
139
(227
)
48
91
178
(261
)
51
93
18
1
(26
2)
52
96
184
(263
)
55
(99
)
18
6
140
232
141
(231)
14
4
23
8
(14
7)
(23
7)
15
0
(24
2)
15
2
(24
3)
15
7
(24
7)
159
(245
)
163
(251
)
165
(254
)
167
(253
)
169
(256
)
173
(254)
17
5
(25
7)
56
10
1
19
0
59
10
3
19
2
59
10
6
19
5
63
.5
10
8
19
7
65
.4
112
201
11
27
70
11
5
204
12
28
73
11
9
207
14
31
75
122
209
16
32
79
12
8
(21
0)
19
35.5
80
12
7
(21
0)
20
40
84
13
1
(22
2)
Lith
ium
So
diu
m
Po
tassiu
m
Ru
bid
ium
Ca
esiu
m
Fra
nciu
m
Bery
lium
Mag
ne
siu
m
Ca
lciu
m
Str
on
tium
Ba
riu
m
Ra
diu
m
Sca
ndiu
m
Ytt
riu
m
Lanth
an
um
Actiniu
m
Titaniu
m
Zircon
ium
Hafn
ium
Un
nilq
ua
diu
m
Va
na
diu
m
Nio
biu
m
Tan
talu
m
Un
nilp
entium
Ch
rom
ium
Mo
lybd
en
um
Tun
gste
n
Un
nilh
exiu
m
Mang
an
ese
Te
chn
etiu
m
Rh
en
ium
Ceriu
m
Tho
riu
m
Pra
seo
dym
ium
Pro
tactiniu
m
Neo
dim
ium
Ura
niu
m
Pro
me
thiu
m
Ne
ptu
niu
m
Sa
mari
um
Plu
toniu
m
Euro
piu
m
Am
eri
ciu
m
Gad
olin
ium
Curi
um
Terb
ium
Be
rke
lium
Dyspro
siu
m
Ca
lifo
rniu
m
Ho
lmiu
m
Ein
ste
iniu
m
Erb
ium
Fe
rmiu
m
Thu
lium
Men
dele
viu
m
Ytte
rbiu
m
Nob
eliu
m
Lute
tiu
m
Law
renciu
m
Iron
Ru
the
niu
m
Osm
ium
Co
ba
lt
Rho
diu
m
Irid
ium
Nic
kel
Pa
llad
ium
Pla
tin
um
Co
pp
er
Silv
er
Go
ld
Zin
c
Cad
miu
m
Me
rcury
Boro
n
Alu
min
ium
Ga
llium
Indiu
m
Tha
lliu
m
Carb
on
Sili
con
Germ
aniu
m
Tin
Lea
d
Nitro
gen
Ph
osp
ho
rus
Ars
en
ic
An
tim
on
y
Bis
mu
th
Oxyg
en
Su
lph
ur
Sele
niu
m
Tellu
riu
m
Polo
niu
m
Flu
ori
ne
Chlo
rin
e
Bro
min
e
Iodin
e
Asta
tine
Ne
on
Arg
on
Kry
pto
n
Xen
on
Rad
on
Heliu
mH
ydro
gen
12
14
H
Be
Mg
Ca
Sr
Ba
Ra
Sc Y La
Ac
Ti
Zr
Hf
Un
q
V Nb
Ta
Un
p
Cr
Mo
W
Un
h
Mn
Tc
Re
Ce
Th
Pr
Pa
Nd U
Pm
Np
Sm
Pu
Eu
Am
Gd
Cm
Tb
Bk
Dy
Cf
Ho
Es
Er
Fm
Tm
Md
Yb
No
Lu
Lr
Fe
Ru
Os
Co
Rh Ir
Ni
Pd
Pt
Cu
Ag
Au
Zn
Cd
Hg
B Al
Ga
In Ti
C Si
Ge
Sn
Pb
N P As
Sb
Bi
O S Se
Te
Po
F Cl
Br I At
Ne
Ar
Kr
Xe
Rn
He
Ato
mic
Num
ber
Sym
bo
l
Nam
e
Mola
r m
ass in
g m
ol–
1
Peri
od
Ke
y
Gro
up
TH
E P
ER
IOD
IC T
AB
LE
12
34
56
70
1 2 3 4 5 6 7
La
nth
an
ide
ele
me
nts
Ac
tin
ide
ele
me
nts
- 1 -
Sixth Form Entrance 2015
CHEMISTRY
1 hour
Name (Capital Letters): ......................................................................
Present School: ……………………………………………………….
Answer ALL the questions
TOTAL MARK = 70
Answers to Section A should be answered on the question paper.
Answers to Section B should be written on the blank pages at the end of the question paper.
A copy of the Periodic Table is included with the question paper (back page).
If you know the name of the examination board and the title of the chemistry course you are
currently studying e.g. AQA Chemistry, Edexcel, OCR Gateway or 21st Century Science,
IGCSE write it below. Indicate if you are doing Triple Science (i.e. you will get separate
grades in Biology, Chemistry and Physics) or Double Science.
Board_________________ Course________________________ Triple/Double __________
- 2 -
SECTION A
Q1 Use the Periodic Table to help you with this question.
Complete the table below by putting in the missing symbols or numbers.
Symbol Number of
protons
Number of
neutrons
Mass
number
Electron
arrangement
O 8 8
17 37 2.8.7
S2- 32
[TOTAL = 7]
Q2 (a) You are given the formulae of the following ions. Write the chemical formula of
the following substances. The first one is shown as an example.
Ion Formula Ion Formula
Ammonium NH4+ Iodide I−
Magnesium Mg2+ Nitride N3−
Lithium Li+ Hydroxide OH−
Potassium K+ Hydrogencarbonate HCO3−
Lead(II) Pb2+ Carbonate CO32−
Iron(III) Fe3+ Sulfate SO42−
Barium Ba2+ Nitrate NO3−
Example: barium hydroxide Ba(OH)2
(i) ammonium nitrate............................................................................
(ii) Magnesium nitride..........................................................................
(iii) Barium hydrogencarbonate............................................................
(iv) Iron(III) hydroxide.........................................................................
(v) Lead nitride.....................................................................................
[5]
- 3 -
(b) Put numbers in front of the formulae as necessary to balance the equations
below:
(i) ........Cs + .........H2O .........CsOH + .........H2
(ii) ........Fe2O3 + ........C ........Fe + ..........CO
(iii) ........C9H20 + ........O2 ........CO2 + ........H2O
(iv) ........ Al2(SO4)3 + ........Mg(OH)2 ........Al(OH)3 + .........MgSO4
[4]
[TOTAL = 9]
Q3 Atoms are made of electrons, neutrons and protons.
(a) Complete the table to show the relative mass and charge of an electron,
neutron and proton.
particle relative mass relative charge
electron -1
neutron 1
proton
[4]
(b) The diagram shows the electronic structure of an atom of an element.
(i) Name the element of which this is an atom.
Explain your answer.
..........................................................................................................................
..........................................................................................................................
[2]
×
×
××
× ×
×
×
×
×
×
××
×
×
×
×
- 4 -
(ii) What is the atomic number of this element?
..........................................................................................................................
[1]
(c) The table below shows some information about the isotopes of neon.
Isotope Mass
Number
Abundance
Lead - 207 207 90.1%
Lead - 208 208 3.4%
Lead - 210 210 6.5%
(i) What is the definition of an isotope?
…………………………………………………………………………..........
…………………………………………………………………………..........
…………………………………………………………………………..........
…………………………………………………………………………..........
[2]
(ii) Calculate the relative atomic mass of lead.
…………………………………………………………………………..........
…………………………………………………………………………..........
……………...…………………………………………………………...........
…………………………………………………………………………..........
[2]
[TOTAL = 11]
- 5 -
Q4 The following table gives some information about several substances.
Substance Melting
point /
°C
Boiling
point /
°C
Electrical
conductivity
when solid
Electrical
conductivity
when molten
Solubility in
water
A 705 1445 poor good soluble
B 1635 3350 good good insoluble
C -111 -45 poor poor soluble
D -25 154 poor poor insoluble
E 1435 2295 poor poor insoluble
For each of the substances, A to E, decided the type of bonding and structure present. Circle
the correct answers below.
(a) A: Bonding – Covalent / Ionic / Metallic
Structure – Giant / Simple Molecular
(b) B: Bonding – Covalent / Ionic / Metallic
Structure – Giant / Simple Molecular
(c) C: Bonding – Covalent / Ionic / Metallic
Structure – Giant / Simple Molecular
(d) D: Bonding – Covalent / Ionic / Metallic
Structure – Giant / Simple Molecular
(e) E: Bonding – Covalent / Ionic / Metallic
Structure – Giant / Simple Molecular
[TOTAL = 5]
Q5 (a) Draw a dot-cross diagram to show the bonding in an methane molecule. Show the
outer shell electrons only. Name the type of bonding.
[3]
- 6 -
(b) Draw one molecule of butane and one molecule of butene, showing all the
bonds.
butane butene
[4]
(c) Define the term isomerism
………………………………………………………………………………
………………………………………………………………………………
[2]
[TOTAL = 9]
Q6 Sodium nitrate decomposes on strong heating as shown:
2KNO3(s) 2KNO2(s) + O2(g)
If 51.0 g of potassium nitrate was completely decomposed by heating, what mass
of solid would remain? Show full working including relevant equations used with
appropriate units for each calculation.
[TOTAL = 6]
- 7 -
Q8 Hydrogen peroxide (H2O2) decomposes slowly at room temperature to form oxygen
and water.
(a) Write a balanced equation for this reaction including the relevant state
symbols.
..........................................................................................................................
[3]
(b) Iron (III) oxide acts as a catalyst for this reaction.
Andy added 1.0 g of Iron (III) oxide to 35 cm3 of hydrogen peroxide
solution at room temperature.
He measured the total volume of oxygen given off at one minute intervals.
His results are shown in the table.
Time (minutes) 0 1 2 3 4 5
Total volume of oxygen
(cm3)
0 62 80 94 96 96
Draw a graph of total volume of oxygen produced against time.
3
Totalvolumeof oxygenin cm
Time in minutes
- 8 -
[3]
(c) At the end of the experiment Andy filtered off the oxide.
What mass of oxide would you expect to be left?
..........................................................................................................................
[1]
(d) Define catalyst
..........................................................................................................................
..........................................................................................................................
[1]
(e) Andy then added 1.0 g of a different oxide to a fresh 20 cm3 sample of
hydrogen peroxide solution at the same temperature.
Again he measured the volume of oxygen produced at one minute intervals.
From his results he concluded that this different oxide was a better catalyst
than manganese(IV) oxide.
Add a line to your graph to show results which would support this
conclusion. Label this new line “Oxide”.
[2]
(f) Draw a labelled diagram to illustrate the apparatus you would use to investigate
this reaction and collect and measure the volume of gas produced.
[3]
[TOTAL = 13]
- 9 -
SECTION B
Write your answers to this section on the blank pages which follow.
Write notes on TWO of the following [5 marks each]. Use diagrams and chemical equations
where relevant.
(a) Fractional distillation
(b) The industrial manufacture of sulphuric acid
(c) The mole concept
(d) The bonding and structure of sodium and water
(e) The formation of soluble salts
(f) The manufacture of iron from its ore (include all relevant equations)
(g) The structures, properties and uses of TWO polymers
SECTION B ANSWER
- 12 -
3 11
19
37
55
87
4 12
20
38
56
88
21
39
57
89
22
40
72
104
23
41
73
105
24
42
74
106
25
43
75
58
90
59
91
60
92
61
93
62
94
63
95
64
96
65
97
66
98
67
99
68
100
69
101
70
102
71
103
26
44
76
27
45
77
28
46
78
29
47
79
30
48
80
5 13
31
49
81
6 14
32
50
82
7 15
33
51
83
8 16
34
52
84
9 17
35
53
85
10
18
36
54
86
Li
Na K Rb
Cs
Fr7 23
39
85
133
(223
)
9 24
40
88
137
(226
)
45
89
139
(227
)
48
91
178
(261
)
51
93
18
1
(26
2)
52
96
184
(263
)
55
(99
)
18
6
140
232
141
(231)
14
4
23
8
(14
7)
(23
7)
15
0
(24
2)
15
2
(24
3)
15
7
(24
7)
159
(245
)
163
(251
)
165
(254
)
167
(253
)
169
(256
)
173
(254)
17
5
(25
7)
56
10
1
19
0
59
10
3
19
2
59
10
6
19
5
63
.5
10
8
19
7
65
.4
112
201
11
27
70
11
5
204
12
28
73
11
9
207
14
31
75
122
209
16
32
79
12
8
(21
0)
19
35.5
80
12
7
(21
0)
20
40
84
13
1
(22
2)
Lith
ium
So
diu
m
Po
tassiu
m
Ru
bid
ium
Ca
esiu
m
Fra
nciu
m
Bery
lium
Mag
ne
siu
m
Ca
lciu
m
Str
on
tium
Ba
riu
m
Ra
diu
m
Sca
ndiu
m
Ytt
riu
m
Lanth
an
um
Actiniu
m
Titaniu
m
Zircon
ium
Hafn
ium
Un
nilq
ua
diu
m
Va
na
diu
m
Nio
biu
m
Tan
talu
m
Un
nilp
entium
Ch
rom
ium
Mo
lybd
en
um
Tun
gste
n
Un
nilh
exiu
m
Mang
an
ese
Te
chn
etiu
m
Rh
en
ium
Ceriu
m
Tho
riu
m
Pra
seo
dym
ium
Pro
tactiniu
m
Neo
dim
ium
Ura
niu
m
Pro
me
thiu
m
Ne
ptu
niu
m
Sa
mari
um
Plu
toniu
m
Euro
piu
m
Am
eri
ciu
m
Gad
olin
ium
Curi
um
Terb
ium
Be
rke
lium
Dyspro
siu
m
Ca
lifo
rniu
m
Ho
lmiu
m
Ein
ste
iniu
m
Erb
ium
Fe
rmiu
m
Thu
lium
Men
dele
viu
m
Ytte
rbiu
m
Nob
eliu
m
Lute
tiu
m
Law
renciu
m
Iron
Ru
the
niu
m
Osm
ium
Co
ba
lt
Rho
diu
m
Irid
ium
Nic
kel
Pa
llad
ium
Pla
tin
um
Co
pp
er
Silv
er
Go
ld
Zin
c
Cad
miu
m
Me
rcury
Boro
n
Alu
min
ium
Ga
llium
Indiu
m
Tha
lliu
m
Carb
on
Sili
con
Germ
aniu
m
Tin
Lea
d
Nitro
gen
Ph
osp
ho
rus
Ars
en
ic
An
tim
on
y
Bis
mu
th
Oxyg
en
Su
lph
ur
Sele
niu
m
Tellu
riu
m
Polo
niu
m
Flu
ori
ne
Chlo
rin
e
Bro
min
e
Iodin
e
Asta
tine
Ne
on
Arg
on
Kry
pto
n
Xen
on
Rad
on
Heliu
mH
ydro
gen
12
14
H
Be
Mg
Ca
Sr
Ba
Ra
Sc Y La
Ac
Ti
Zr
Hf
Un
q
V Nb
Ta
Un
p
Cr
Mo
W
Un
h
Mn
Tc
Re
Ce
Th
Pr
Pa
Nd U
Pm
Np
Sm
Pu
Eu
Am
Gd
Cm
Tb
Bk
Dy
Cf
Ho
Es
Er
Fm
Tm
Md
Yb
No
Lu
Lr
Fe
Ru
Os
Co
Rh Ir
Ni
Pd
Pt
Cu
Ag
Au
Zn
Cd
Hg
B Al
Ga
In Ti
C Si
Ge
Sn
Pb
N P As
Sb
Bi
O S Se
Te
Po
F Cl
Br I At
Ne
Ar
Kr
Xe
Rn
He
Ato
mic
Num
ber
Sym
bo
l
Nam
e
Mola
r m
ass in
g m
ol–
1
Peri
od
Ke
y
Gro
up
TH
E P
ER
IOD
IC T
AB
LE
12
34
56
70
1 2 3 4 5 6 7
La
nth
an
ide
ele
me
nts
Ac
tin
ide
ele
me
nts
- 1 -
THE KING’S SCHOOL, CANTERBURY
SIXTH FORM ENTRANCE EXAMINATION
2014-2015
CHEMISTRY
1 Hour
Name (Capital Letters): ......................................................................
Present School: ……………………………………………………….
Answer ALL the questions
TOTAL MARK = 70
Answers to Section A should be answered on the question paper.
Answers to Section B should be written on the blank pages at the end of the question paper.
A copy of the Periodic Table is included with the question paper (back page).
If you know the name of the examination board and the title of the chemistry course you are
currently studying e.g. AQA Chemistry, Edexcel, OCR Gateway or 21st Century Science,
IGCSE write it below. Indicate if you are doing Triple Science (i.e. you will get separate
grades in Biology, Chemistry and Physics) or Double Science.
Board_________________ Course________________________ Triple/Double __________
- 2 -
SECTION A
Q1 Use the Periodic Table to help you with this question.
Complete the table below by putting in the missing symbols or numbers.
Symbol Number of
protons
Number of
neutrons
Mass
number
Electron
arrangement
Si 14 14
13 27 2.8.2
O2- 16
[TOTAL = 7]
Q2 (a) You are given the formulae of the following ions. Write the chemical formula of
the following substances. The first one is shown as an example.
Ion Formula Ion Formula
Ammonium NH4+ Iodide I−
Magnesium Mg2+ Nitride N3−
Lithium Li+ Hydroxide OH−
Potassium K+ Hydrogencarbonate HCO3−
Lead(II) Pb2+ Carbonate CO32−
Iron(III) Fe3+ Sulfate SO42−
Barium Ba2+ Nitrate NO3−
Example: barium hydroxide Ba(OH)2
(i) lead(II) carbonate....................................................................
(ii) Potassium nitride....................................................................
(iii) ammonium hydroxide............................................................
(iv) ammonium sulfate..................................................................
(v) iron(III) hydrogencarbonate....................................................
[5]
- 3 -
(b) Put numbers in front of the formulae as necessary to balance the equations
below:
(i) ........Na + .........H2O .........NaOH + .........H2
(ii) ........Fe2O3 + ........CO ........Fe + ..........CO2
(iii) ........C7H16 + ........O2 ........CO2 + ........H2O
(iv) ........ Al2(SO4)3 + ........NaOH ........Al(OH)3 + .........Na2SO4
[4]
[TOTAL = 9]
Q3 Atoms are made of electrons, neutrons and protons.
(a) Complete the table to show the relative mass and charge of an electron,
neutron and proton.
particle relative mass relative charge
electron 1/1840
neutron 0
proton
[4]
(b) The diagram shows the electronic structure of an atom of an element.
(i) Name the element of which this is an atom.
Explain your answer.
..........................................................................................................................
..........................................................................................................................
[2]
×
×
××
× ×
×
×
×
×
×
××
×
×
×
×
- 4 -
(ii) What is the atomic number of this element?
..........................................................................................................................
[1]
(c) The table below shows some information about the isotopes of neon.
Isotope Mass
Number
Abundance
arsenic-74 74 9%
arsenic-75 75 91%
(i) What is the definition of an isotope?
…………………………………………………………………………..........
…………………………………………………………………………..........
…………………………………………………………………………..........
…………………………………………………………………………..........
[2]
(ii) Calculate the relative atomic mass of arsenic.
…………………………………………………………………………..........
…………………………………………………………………………..........
……………...…………………………………………………………...........
…………………………………………………………………………..........
[2]
[TOTAL = 11]
- 5 -
Q4 The following table gives some information about several substances.
Substance Melting
point /
°C
Boiling
point /
°C
Electrical
conductivity
when solid
Electrical
conductivity
when molten
Solubility in
water
A 1410 2355 poor poor insoluble
B -25 144 poor poor insoluble
C 712 1418 poor good soluble
D -101 -35 poor poor soluble
E 1660 3287 good good insoluble
For each of the substances, A to E, decided the type of bonding and structure present. Circle
the correct answers below.
(a) A: Bonding – Covalent / Ionic / Metallic
Structure – Giant / Simple Molecular
(b) B: Bonding – Covalent / Ionic / Metallic
Structure – Giant / Simple Molecular
(c) C: Bonding – Covalent / Ionic / Metallic
Structure – Giant / Simple Molecular
(d) D: Bonding – Covalent / Ionic / Metallic
Structure – Giant / Simple Molecular
(e) E: Bonding – Covalent / Ionic / Metallic
Structure – Giant / Simple Molecular
[TOTAL = 5]
Q5 (a) Draw a dot-cross diagram to show the bonding in an ammonia molecule. Show the
outer shell electrons only. Name the type of bonding.
[3]
- 6 -
(b) Draw one molecule of ethane and one molecule of ethene, showing all the
bonds.
ethane ethene
[4]
[TOTAL = 7]
Q6 Molten, impure iron is made from iron ore in the blast furnace.
(a) In the blast furnace, reducing agents change iron ore into iron.
Give the name of ONE substance which can act as a reducing agent in the
blast furnace.
………………………………………………………………………………
[1]
(b) The main impurity in iron ore is silicon dioxide (SiO2).
Describe how this is removed.
Give the name of the raw material which must be present to remove this
impurity and describe the reactions involved, naming the waste product
formed.
You should include equations for the chemical reactions taking place.
………………………………………………………………………………
………………………………………………………………………………
………………………………………………………………………………
………………………………………………………………………………
………………………………………………………………………………
………………………………………………………………………………
………………………………………………………………………………
………………………………………………………………………………
………………………………………………………………………………
[5] [TOTAL = 6]
- 7 -
Q7 Sodium nitrate decomposes on strong heating as shown:
2KNO3(s) 2KNO2(s) + O2(g)
If 51.0 g of potassium nitrate was completely decomposed by heating, what mass
of solid would remain? Show full working.
[TOTAL = 4]
Q8 Hydrogen peroxide (H2O2) decomposes slowly at room temperature to form oxygen
and water.
(a) Write a balanced equation for this reaction.
..........................................................................................................................
[2]
(b) Manganese(IV) oxide acts as a catalyst for this reaction.
Andy added 1.0 g of manganese(IV) oxide to 20 cm3 of hydrogen peroxide
solution at room temperature.
He measured the total volume of oxygen given off at one minute intervals.
His results are shown in the table.
Time (minutes) 0 1 2 3 4 5
Total volume of oxygen
(cm3)
0 31 41 46 48 48
Draw a graph of total volume of oxygen produced against time.
- 8 -
[3]
(c) At the end of the experiment Andy filtered off the oxide.
What mass of oxide would you expect to be left?
..........................................................................................................................
[1]
(d) Andy then added 1.0 g of a different oxide to a fresh 20 cm3 sample of
hydrogen peroxide solution at the same temperature.
Again he measured the volume of oxygen produced at one minute intervals.
From his results he concluded that this different oxide was a better catalyst
than manganese(IV) oxide.
Add a line to your graph to show results which would support this
conclusion. Label this new line “Oxide”.
[2]
(e) Draw a labelled diagram to illustrate the apparatus you would use to investigate
this reaction and collect and measure the volume of gas produced.
[3]
[TOTAL = 11]
3
Totalvolumeof oxygenin cm
Time in minutes
- 9 -
SECTION B
Write your answers to this section on the blank pages which follow.
Write notes on TWO of the following [5 marks each]. Use diagrams and chemical equations
where relevant.
(a) Cracking
(b) The structures, properties and uses of TWO polymers
(c) The mole concept
(d) Catalysts
(e) The bonding and structure of graphite and diamond
(f) The formation of insoluble salts
(g) The manufacture of aluminium from its ore
(h) The industrial manufacture of ammonia
SECTION B ANSWER
- 11 -
3 11
19
37
55
87
4 12
20
38
56
88
21
39
57
89
22
40
72
104
23
41
73
105
24
42
74
106
25
43
75
58
90
59
91
60
92
61
93
62
94
63
95
64
96
65
97
66
98
67
99
68
100
69
101
70
102
71
103
26
44
76
27
45
77
28
46
78
29
47
79
30
48
80
5 13
31
49
81
6 14
32
50
82
7 15
33
51
83
8 16
34
52
84
9 17
35
53
85
10
18
36
54
86
Li
Na K Rb
Cs
Fr7 23
39
85
133
(223
)
9 24
40
88
137
(226
)
45
89
139
(227
)
48
91
178
(261
)
51
93
18
1
(26
2)
52
96
184
(263
)
55
(99
)
18
6
140
232
141
(231)
14
4
23
8
(14
7)
(23
7)
15
0
(24
2)
15
2
(24
3)
15
7
(24
7)
159
(245
)
163
(251
)
165
(254
)
167
(253
)
169
(256
)
173
(254)
17
5
(25
7)
56
10
1
19
0
59
10
3
19
2
59
10
6
19
5
63
.5
10
8
19
7
65
.4
112
201
11
27
70
11
5
204
12
28
73
11
9
207
14
31
75
122
209
16
32
79
12
8
(21
0)
19
35.5
80
12
7
(21
0)
20
40
84
13
1
(22
2)
Lith
ium
So
diu
m
Po
tassiu
m
Ru
bid
ium
Ca
esiu
m
Fra
nciu
m
Bery
lium
Mag
ne
siu
m
Ca
lciu
m
Str
on
tium
Ba
riu
m
Ra
diu
m
Sca
ndiu
m
Ytt
riu
m
Lanth
an
um
Actiniu
m
Titaniu
m
Zircon
ium
Hafn
ium
Un
nilq
ua
diu
m
Va
na
diu
m
Nio
biu
m
Tan
talu
m
Un
nilp
entium
Ch
rom
ium
Mo
lybd
en
um
Tun
gste
n
Un
nilh
exiu
m
Mang
an
ese
Te
chn
etiu
m
Rh
en
ium
Ceriu
m
Tho
riu
m
Pra
seo
dym
ium
Pro
tactiniu
m
Neo
dim
ium
Ura
niu
m
Pro
me
thiu
m
Ne
ptu
niu
m
Sa
mari
um
Plu
toniu
m
Euro
piu
m
Am
eri
ciu
m
Gad
olin
ium
Curi
um
Terb
ium
Be
rke
lium
Dyspro
siu
m
Ca
lifo
rniu
m
Ho
lmiu
m
Ein
ste
iniu
m
Erb
ium
Fe
rmiu
m
Thu
lium
Men
dele
viu
m
Ytte
rbiu
m
Nob
eliu
m
Lute
tiu
m
Law
renciu
m
Iron
Ru
the
niu
m
Osm
ium
Co
ba
lt
Rho
diu
m
Irid
ium
Nic
kel
Pa
llad
ium
Pla
tin
um
Co
pp
er
Silv
er
Go
ld
Zin
c
Cad
miu
m
Me
rcury
Boro
n
Alu
min
ium
Ga
llium
Indiu
m
Tha
lliu
m
Carb
on
Sili
con
Germ
aniu
m
Tin
Lea
d
Nitro
gen
Ph
osp
ho
rus
Ars
en
ic
An
tim
on
y
Bis
mu
th
Oxyg
en
Su
lph
ur
Sele
niu
m
Tellu
riu
m
Polo
niu
m
Flu
ori
ne
Chlo
rin
e
Bro
min
e
Iodin
e
Asta
tine
Ne
on
Arg
on
Kry
pto
n
Xen
on
Rad
on
Heliu
mH
ydro
gen
12
14
H
Be
Mg
Ca
Sr
Ba
Ra
Sc Y La
Ac
Ti
Zr
Hf
Un
q
V Nb
Ta
Un
p
Cr
Mo
W
Un
h
Mn
Tc
Re
Ce
Th
Pr
Pa
Nd U
Pm
Np
Sm
Pu
Eu
Am
Gd
Cm
Tb
Bk
Dy
Cf
Ho
Es
Er
Fm
Tm
Md
Yb
No
Lu
Lr
Fe
Ru
Os
Co
Rh Ir
Ni
Pd
Pt
Cu
Ag
Au
Zn
Cd
Hg
B Al
Ga
In Ti
C Si
Ge
Sn
Pb
N P As
Sb
Bi
O S Se
Te
Po
F Cl
Br I At
Ne
Ar
Kr
Xe
Rn
He
Ato
mic
Num
ber
Sym
bo
l
Nam
e
Mola
r m
ass in
g m
ol–
1
Peri
od
Ke
y
Gro
up
TH
E P
ER
IOD
IC T
AB
LE
12
34
56
70
1 2 3 4 5 6 7
La
nth
an
ide
ele
me
nts
Ac
tin
ide
ele
me
nts