Multiple Choice25]_multiple_choice.pdfMultiple Choice 14 Barcode Typesetter code Section B Answer all questions in this section. Only one answer per question is allowed. For each answer

Multiple Choice

14

Barcode Typesetter code

Section B

Answer all questions in this section.

Only one answer per question is allowed.

For each answer completely fill in the circle alongside the appropriate answer.

If you want to change your answer you must cross out your original answer as shown. If you wish to return to an answer previously crossed out, ring the answer you now wish to select as shown.

Which change requires the largest amount of energy?

[1 mark] A He+(g) He2+(g) + e– B Li(g) Li+(g) + e– C Mg+(g) Mg2+(g) + e– D N(g) N+(g) + e–

A sample of 2.18 g of oxygen gas has a volume of 1870 cm3 at a pressure of 101 kPa.

What is the temperature of the gas? The gas constant is R = 8.31 J K–1 mol–1.

[1 mark] A 167 K B 334 K C 668 K D 334 000 K

0 6

CORRECT METHOD WRONG METHODS

0 7

15

Barcode Typesetter code Turn over

An ester is hydrolysed as shown by the following equation.

RCOOR/ + H2O RCOOH + R/OH What is the percentage yield of RCOOH when 0.50 g of RCOOH (Mr = 100) is obtained from 1.0 g of RCOOR/ (Mr = 150)?

[1 mark]

A 33%

B 50%

C 67%

D 75%

A saturated aqueous solution of magnesium hydroxide contains 1.17 × 10–3 g of Mg(OH)2 in 100 cm3 of solution. In this solution, the magnesium hydroxide is fully dissociated into ions. What is the concentration of Mg2+(aq) ions in this solution?

[1 mark]

A 2.82 × 10–2 mol dm–3

B 2.01 × 10–3 mol dm–3

C 2.82 × 10–3 mol dm–3

D 2.01 × 10–4 mol dm–3

Turn over for the next question

0 8

0 9

16


The rate equation for the hydrogenation of ethene

C2H4(g) + H2(g) C2H6(g) is Rate = k[C2H4][H2] At a fixed temperature, the reaction mixture is compressed to triple the original pressure. What is the factor by which the rate of reaction changes?

[1 mark] A 6 B 9 C 12 D 27

When one mole of ammonia is heated to a given temperature, 50% of the compound dissociates and the following equilibrium is established.

NH3(g) 12N2(g) + 3

2H2(g)

What is the total number of moles of gas present in this equilibrium mixture?

[1 mark] A 1.5 B 2.0 C 2.5 D 3.0

Which change would alter the value of the equilibrium constant (Kp) for this reaction?

2SO2(g) + O2(g) 2SO3(g)

[1 mark]

A Increasing the total pressure of the system. B Increasing the concentration of sulfur trioxide. C Increasing the concentration of sulfur dioxide. D Increasing the temperature.

1 0

1 1

1 2

17


What is the pH of a 0.020 mol dm–3 solution of a diprotic acid which is completely dissociated?

[1 mark]

A 1.00 B 1.40 C 1.70 D 4.00

The acid dissociation constant, Ka, of a weak acid HA has the value 2.56 × 10–4 mol dm–3 What is the pH of a 4.25 × 10–3 mol dm-3 solution of HA?

[1 mark]

A 5.96 B 3.59 C 2.98 D 2.37

Magnesium reacts with hydrochloric acid according to the following equation.

Mg + 2HCl MgCl2 + H2 A student calculated the minimum volume of 2.56 mol dm–3 hydrochloric acid required to react with an excess of magnesium to form 5.46 g of magnesium chloride (Mr = 95.3). Which of the following uses the correct standard form and the appropriate number of significant figures to give the correct result of the calculation?

[1 mark]

A 4.476 × 10–2 dm3 B 4.48 × 10–2 dm3 C 4.50 × 10–2 dm3 D 44.8 × 10–3 dm3

1 3

1 4

1 5

18


In which reaction is hydrogen acting as an oxidising agent?

[1 mark]

A Cl2 + H2 2HCl B (CH3)2CO + H2 (CH3)2CHOH C N2 + 3H2 2NH3 D 2Na + H2 2NaH

In which reaction is the metal oxidised? [1 mark]

A 2Cu2+ + 4I– 2CuI + I2 B [Fe(H2O)6]

3+ + Cl– [Fe(H2O)5(Cl)]2+ + H2O C [CoCl4]

2– + 6H2O [Co(H2O)6]2+ + 4Cl–

D Mg + S MgS

The following cell has an EMF of +0.46 V.

Cu Cu2+ Ag+ Ag

Which statement is correct about the operation of the cell? [1 mark]

A Metallic copper is oxidised by Ag+ ions. B The silver electrode has a negative polarity. C The silver electrode gradually dissolves to form Ag+ ions. D Electrons flow from the silver electrode to the copper electrode via an external circuit.

1 8

1 6

1 7

19


In an experiment to identify a Group 2 metal (X), 0.102 g of X reacts with an excess of aqueous hydrochloric acid according to the following equation.

X + 2HCl XCl2 + H2

The volume of hydrogen gas given off is 65 cm3 at 99 kPa pressure and 303 K. The gas constant is R = 8.31 J K–1 mol–1.

Which is X?

[1 mark]

A Barium B Calcium C Magnesium D Strontium

What forms when a solution of sodium carbonate is added to a solution of gallium(III) nitrate?

[1 mark]

A A white precipitate of gallium(III) carbonate. B A white precipitate of gallium(III) hydroxide. C A white precipitate of gallium(III) carbonate and

bubbles of carbon dioxide. D A white precipitate of gallium(III) hydroxide and bubbles of carbon dioxide.

Which compound gives a colourless solution when an excess of dilute aqueous ammonia is added?

[1 mark]

A MgCl2 B AgCl C CuCl2 D AlCl3

1 9

2 0

2 1

20


What is the final species produced when an excess of aqueous ammonia is added to aqueous aluminium chloride?

[1 mark]

A [Al(NH3)6]3+

B [Al(OH)3(H2O)3] C [Al(OH)4(H2O)2]

– D [Al(OH)(H2O)5]

2+

The following equation represents the oxidation of vanadium(IV) ions by manganate(VII) ions in acid solution.

5V4+ + MnO4

– + 8H+ 5V5+ + Mn2+ + 4H2O

What volume of 0.020 mol dm–3 KMnO4 solution is required to oxidise completely a solution containing 0.010 mol of vanadium(IV) ions?

[1 mark]

A 10 cm3 B 25 cm3 C 50 cm3 D 100 cm3

How many isomers have the molecular formula C5H12? [1 mark]

A 2 B 3 C 4 D 5

2 2

2 3

2 4

21


Which molecule is not produced when ethane reacts with bromine in the presence of ultraviolet light?

[1 mark]

A C2H4Br2 B HBr C H2 D C4H10

How many structural isomers have the molecular formula C4H9Br? [1 mark]

A 2 B 3 C 4 D 5

What is the major product of the reaction between but-1-ene and DBr? (D is deuterium and represents 2H)

[1 mark]

A CH2DCH2CH2CH2Br B CH2DCH2CHBrCH3 C CH3CH2CHBrCH2D D CH3CH2CHDCH2Br

Why are fluoroalkanes unreactive? [1 mark]

A Fluorine is highly electronegative. B The F– ion is very stable. C They are polar molecules. D The C–F bond is very strong.

2 5

2 6

2 7

2 8

22


Which alcohol could not be produced by the reduction of an aldehyde or a ketone?

[1 mark]

A 2-methylbutan-1-ol B 2-methylbutan-2-ol C 3-methylbutan-1-ol D 3-methylbutan-2-ol

Which compound forms optically active compounds on reduction? [1 mark]

A CH3CH2C(CH3)=CHCH3 B CH3CH2C(CH3)=CH2 C CH3COCH3 D CH3CH2COCH3

How many secondary amines have the molecular formula C4H11N? [1 mark]

A 2 B 3 C 4 D 5

Which compound has the highest boiling point? [1 mark]

A C2H4 B C2H6 C CH3NH2 D CH3F

2 9

3 0

3 1

3 2

23


Which compound can polymerise by reaction with itself?

[1 mark]

A NH2CH2CH2NH2 B CH3CH2CONH2 C HOOCCH2COOH D NH2CH2COCl

A drug is designed to simulate one of the following molecules that adsorbs onto the active site of an enzyme.

Which molecule requires the design of an optically active drug?

[1 mark]

A

H CH

OH

COOH

B

CH3 C

O

COOH

C

CH3 CH

OH

COOH

D CH2 CH2 COOH

OH

Turn over for the next question

3 3

3 4

24


Which amine has only three peaks in its proton NMR spectrum?

[1 mark]

A Methylamine B Trimethylamine

C Diethylamine

D Propylamine

END OF QUESTIONS

Copyright © 2014 AQA and its licensors. All rights reserved.

3 5

2

*N35131A0224*

SECTION A

Answer ALL the questions in this section. You should aim to spend no more than 20 minutes on this section. For each question, select one answer from A to D and put a cross in the box .

If you change your mind, put a line through the box and then mark your new answer with a cross .

1 The isotopes of magnesium, 2412Mg and 25

12Mg, both form ions with charge 2+. Which of the following statements about these ions is true?

A Both ions have electronic configuration 1s2 2s2 2p6 3s2.

B 2512Mg2+ has more protons than 24

12Mg2+.

C The ions have the same number of electrons but different numbers of neutrons.

D The ions have the same number of neutrons but different numbers of protons.

(Total for Question 1 = 1 mark)

2 Chlorine has two isotopes with relative isotopic mass 35 and 37. Four m/z values are given below. Which will occur in a mass spectrum of chlorine gas, Cl2, from an ion with a single positive charge?

A 35.5

B 36

C 71

D 72


Use this space for any rough working. Anything you write in this space will gain no credit.

3

*N35131A0324* Turn over

3 The human body contains around 0.025 g of iodine molecules, I2. Which of the following shows the number of iodine atoms in 0.025 g of I2?

The Avogadro constant is 6.02 × 1023 mol–1.

A 0 025126 9

6 02 1023..

.× ×

B 0 025253 8

6 02 1023..

.× ×

C 253 80 025

6 02 1023..

.× ×

D 126 90 025

6 02 1023..

.× ×


4 Which equation represents the reaction for which the enthalpy change is the standard enthalpy change of formation, ∆Hf

○ , of sodium nitrate, NaNO3?

A 2Na(s) + N2(g) + 3O2(g) → 2NaNO3(s)

B Na(s) + ½N2(g) + 1½O2(g) → NaNO3(s)

C Na(s) + N(g) + 3O(g) → NaNO3(s)

D Na(g) + ½N2(g) + 1½O2(g) → NaNO3(g)


5 Which equation represents the reaction for which the enthalpy change, ∆H, is the mean bond enthalpy of the C–H bond?

A ¼CH4(g) → ¼C(g) + H(g)

B CH4(g) → C(s) + 2H2(g)

C CH4(g) → C(g) + 4H(g)

D CH4(g) → C(g) + 2H2(g)


4

*N35131A0424*

6 The first ionization energies, in kJ mol–1, of four elements with consecutive atomic numbers are shown below.

A 1680

B 2080

C 496

D 738

(a) Which element could be an inert gas?(1)

A

B

C

D

(b) Which element could be X in a covalent compound with formula HX?(1)

A

B

C

D

(c) Which element could be Y in an ionic compound with formula YH2?(1)

A

B

C

D

(Total for Question 6 = 3 marks)

5


7 The graph below shows the second ionization energy of a series of elements with consecutive atomic numbers.

Which element could be lithium?

A

B

C

D


8 The first five ionization energies, in kJ mol–1, of aluminium are

578 1817 2745 11 578 14 831

The orbitals from which the first five electrons are removed during ionization, starting with the first electron, are

A 1s 2s 2p 3s 3p

B 1s 1s 2s 2s 2p

C 3p 3s 2p 2s 1s

D 3p 3s 3s 2p 2p


Atomic number increasing in steps of 1

Second ionization energy / kJ mol–1

A

D

C

B

6

*N35131A0624*

9 Going across the Periodic Table from sodium to aluminium,

A the melting temperature increases.

B the radius of the atom increases.

C the radius of the metal ion increases.

D the bonding in the element changes from metallic to covalent.


10 Going down Group 1 from lithium to rubidium

A the radius of the atom decreases.

B the radius of the ion decreases.

C the first ionization energy decreases.

D the polarizing power of the ion increases.


11 A drop of concentrated nickel(II) sulfate solution, which is green, is placed on moist filter paper on a microscope slide and the ends of the slide are connected to a 24 V DC power supply. After ten minutes,

A a blue colour has moved towards the negative terminal and a yellow colour towards the positive terminal.

B a blue colour has moved towards the positive terminal and a yellow colour towards the negative terminal.

C a green colour has moved towards the negative terminal but there is no other visible change.

D a green colour has moved towards the positive terminal but there is no other visible change.



7


12 The bonding in magnesium oxide, MgO, is

A ionic.

B metallic and ionic.

C ionic and covalent.

D metallic and covalent.


13 Which of the following mixtures could not form when octane, C8H18, is cracked?

A propane + pentene

B butane + butene

C pentane + propene

D heptane + ethene



8

*N35131A0824*

14 This question is about the organic compounds with skeletal formulae as shown:

A

B

C

D

(a) Which compound is 2-methylpropane?(1)

A

B

C

D

(b) Which compound has the molecular formula C5H12?(1)

A

B

C

D

(c) Which compounds are isomers?(1)

A compound A and compound C

B compound B and compound C

C compound B and compound D

D compound C and compound D

9


(d) Which compound reacts with acidified potassium manganate(VII) to form a diol?(1)

A

B

C

D


15 The structural formula of 5-chloro-2,2-dimethylhexane is

A CH3 C CH2 C H

H

Cl

CH3

CH3

B H C CH2 CH2 CH2 C CH3

Cl

CH3

CH3

Cl

C CH3 C CH2 CH2 C CH3

H

CH3

CH3

Cl

D CH3 C CH2 CH2 C CH3

CH3

Cl

CH3

Cl


TOTAL FOR SECTION A = 20 MARKS

2

*N35692A0224*

SECTION A

Answer ALL the questions in this section. You should aim to spend no more than 20 minutes on this section. For each question, select one answer from A to D and put a cross in the box ( ).

If you change your mind, put a line through the box ( ) and then mark your new answer with a cross ( ).

1 Which of the following bond angles occur in a molecule of ethanol, C2H5OH?

A 90° and 180°

B 104.5° and 180°

C 104.5° and 109.5°

D 109.5° and 120°


2 Which of the following molecules is linear?

A Carbon dioxide, CO2

B Sulfur dioxide, SO2

C Water, H2O

D Methanal, HCHO


3 Which of the following molecules contains polar bonds but is not a polar molecule?

A Chlorine, Cl2

B Hydrogen chloride, HCl

C Trichloromethane, CHCl3

D Tetrachloromethane, CCl4


4 Which of the following has dipole-dipole interactions between its molecules, but no hydrogen bonding?

A Methane, CH4

B Methanol, CH3OH

C Ammonia, NH3

D Hydrogen iodide, HI


3


5 Which list below shows the compounds in order of increasing boiling temperature?

A CH4, HCl, HF

B HF, CH4, HCl

C HCl, HF, CH4

D HF, HCl, CH4


6 Which of the following has the highest boiling temperature?

A Pentane, CH3CH2CH2CH2CH3

B Hexane, CH3CH2CH2CH2CH2CH3

C 2-methylbutane, CH3CH(CH3)CH2CH3

D 2-methylpentane, CH3CH(CH3)CH2CH2CH3


7 Which of the following could not be an element in Group 2?

A An element with an oxide which forms a solution of pH 10.

B An element with an insoluble sulfate.

C An element with a chloride which is liquid at room temperature.

D An element with a carbonate which decomposes on heating.


8 Chlorides of Group 1 elements produce coloured flames when

A electrons become excited to a higher energy level.

B excited electrons move from a higher to a lower energy level.

C an outer electron leaves the atom.

D electrons move between the negative and positive ions.


4

*N35692A0424*

9 This question is about the following compounds.

A Barium carbonate

B Lithium nitrate

C Potassium bromide

D Potassium nitrate

(a) Which compound gives a green colour in a flame test?(1)

A

B

C

D

(b) Which compound gives a lilac colour in a flame test and does not decompose on heating?

(1)

A

B

C

D



5


10 20 cm3 of sulfuric acid, concentration 0.25 mol dm–3, was neutralized in a titration with barium hydroxide, concentration 0.50 mol dm–3. The equation for the reaction is

Ba(OH)2(aq) + H2SO4(aq) → BaSO4(s) + 2H2O(l)

(a) The volume of barium hydroxide required was(1)

A 10 cm3

B 20 cm3

C 25 cm3

D 40 cm3

(b) During the titration, the barium hydroxide was added until it was present in excess. The electrical conductivity of the titration mixture

(1)

A increased steadily.

B decreased steadily.

C increased and then decreased.

D decreased and then increased.


11 Which of the following trends occurs going down the elements in Group 2?

A The solubility of the hydroxides increases.

B The first ionization energy increases.

C The solubility of the sulfates increases.

D The stability of the carbonates to heat decreases.


12 Which of the following is not a true statement about hydrogen iodide?

A It forms steamy fumes in moist air.

B It dissolves in water to form an acidic solution.

C It forms a cream precipitate with silver nitrate solution.

D It forms dense white smoke with ammonia.


6

*N35692A0624*

13 Chemical reactions may involve

A oxidation

B reduction

C no change in oxidation number

D disproportionation

Which of the terms above best describes what happens to the chlorine in the following reactions?

(a) Cl2(g) + H2O(l) → HCl(aq) + HOCl(aq)(1)

A

B

C

D

(b) Cl2(g) + 2Na(s) → 2NaCl(s)(1)

A

B

C

D

(c) NaCl(s) + H2SO4(l) → HCl(g) + NaHSO4(s)(1)

A

B

C

D


7


14 When chloroethane is heated with a concentrated solution of potassium hydroxide in ethanol, the reaction which occurs is

A substitution.

B elimination.

C hydrolysis.

D redox.



8

*N35692A0824*

15 Chloroethane reacts with aqueous potassium hydroxide solution, producing ethanol as the organic product.

(a) The hydroxide ion is acting as(1)

A an electrophile.

B a nucleophile.

C an oxidizing agent.

D a reducing agent.

(b) Which of the following shows the correct electron-pair movements in this reaction?(1)

A

B

C

D



H

ClCCH

H

HH

:OH–

H

ClCCH

H

HH

:OH–

H

ClCCH

H

HH

:OH–

H

ClCCH

H

HH

:OH–

2

*N36289A0228*

SECTION A

Answer ALL the questions in this section. You should aim to spend no more than 20 minutes on this section. For each question select one answer from A to D and put a cross in the box .

If you change your mind, put a line through the box and then mark your new answer witha cross .

1 Consider the equilibrium

Cl2(g) + PCl3(g) PCl5(g)

Which of the following is true when the total pressure of the system is increased at constant temperature?

Value of Kp Mole fraction of PCl5(g)

A decreases decreases

B unaltered increases

C decreases increases

D unaltered unaltered


2 In which of the following reactions is nitric acid acting as a base?

A HNO3 + NaOH → NaNO3 + H2O

B HNO3 + H2O → H3O+ + NO3–

C HNO3 + H2SO4 → H2NO3+ + HSO4

–

D HNO3 + NaHCO3 → NaNO3 + H2O + CO2


3 Why does phenolphthalein, which is colourless in acidic solutions, turn pink in alkaline solutions?

A It is oxidized to a pink compound by hydroxide ions.

B It forms a pink anion by loss of H+ ions.

C It forms a pink anion by gain of H+ ions.

D It forms a pink cation by gain of H+ ions.


3


4 The dissociation of ethanoic acid in aqueous solution is represented by

CH3COOH(aq) + H2O(l) H3O+(aq) + CH3COO–(aq)

Which of the following statements is true for this equilibrium?

A CH3COOH is an acid and its conjugate base is CH3COO–.

B H2O is an acid and its conjugate base is OH–.

C At equilibrium, the concentrations of each substance are the same.

D At equilibrium, the reaction from left to right and the reaction from right to left have stopped.


5 Why are aqueous solutions of sodium ethanoate slightly alkaline?

A The sodium ions react with water to give an alkali.

B The ethanoate ions react with water to give hydroxide ions.

C All sodium salts give alkaline solutions.

D The sodium ethanoate is fully ionized in solution.


6 When ammonium nitrate crystals dissolve in water, the entropy of the system

A remains the same.

B falls, because the hydrated ions are more ordered than the solid.

C rises, because the ions in the crystal become hydrated in the solution.

D rises, because the ions are arranged more randomly in the solution than in the crystal.



4

*N36289A0428*

7 Which of the following molecules is a methyl ester?

A CH3COOCH2CH3

B HCOOCH3

C CH3COCH2CH3

D CH3COCl(Total for Question 7 = 1 mark)

8 During the preparation of a liquid compound, samples were taken of the product at various stages in the purification procedure. Which of the following techniques would be most suitable for showing the change in composition of these samples during the purification procedure?

A Gas-liquid chromatography

B Fractional distillation

C Filtration

D Distillation


9 Which of the following compounds would react with lithium tetrahydridoaluminate (lithium aluminium hydride) and also with phosphorus(V) chloride (phosphorus pentachloride)?

A CH3CH2CH2COOH

B CH3CH2COCH3

C CH3CH=CHCH3

D CH2=CHCH2CH2OH



5


10 In the synthesis of an ester, the use of an acyl chloride and an alcohol gives a better yield than the use of a carboxylic acid and an alcohol.

This is because the reaction between

A an acyl chloride and an alcohol is an equilibrium.

B an acid and an alcohol goes to completion.

C an acid and an alcohol requires a catalyst.

D an acyl chloride and an alcohol goes to completion.


11 Not all molecules will absorb infrared radiation. Those that do

A change their dipole moment when their bonds stretch or bend.

B undergo homolytic fission.

C must be polar.

D are always organic substances.


12 Which of the following methods may be used in a single step to make carboxylic acids?

A Hydrolysis of an ester with an alkali.

B Reaction of acidified potassium manganate(VII) with an alkene.

C Hydrolysis of a nitrile with hydrochloric acid.

D Reaction of an acyl chloride with ammonia.



6

*N36289A0628*

13 A solution of a weak acid cannot be titrated with a weak base using an indicator to find the end-point because

A the pH change is too gradual close to the equivalence point.

B there are too few H+ ions to affect the indicator.

C there are too few OH– ions to affect the indicator.

D the pH change occurs outside the range of any indicator.


14 Which of the following reagents could be used to produce propanamide, CH3CH2CONH2?

A Ammonia and 1-chloropropane

B Ammonia and propanoyl chloride

C Methylamine and 1-chloropropane

D Methylamine and propanoyl chloride


15 The radio waves used in proton nmr

A must not be absorbed by the sample.

B cause electron transitions in the hydrogen atom.

C can only be used with organic substances.

D cause the hydrogen nucleus to change its spin state.



7


16 Which of the following graphs shows that a reaction is first order with respect to reactant X?

A

B

C

D


[X]

time

[X]

rate

time

[X]

[X]

rate

8

*N36289A0828*

17 Which of the following changes will lead to the greatest increase in the rate of the following endothermic reaction?

N2(g) + O2(g) → 2NO(g) ∆H +ve

Temperature Initial concentration of N2 and O2

A decrease by 15% decrease by 15%

B increase by 15% stay the same

C decrease by 15% increase by 15%

D increase by 15% increase by 15%


18 The repeat unit of the polyester formed from ethane-1,2-diol, HOCH2CH2OH, and

benzene-1,4-dicarboxylic acid, HOOC— —COOH, is

A —O—CH2CH2—O—C— —C—O—CH2CH2—O—

O O

B —O—CH2CH2—C—O— —O—C—CH2CH2—O—

O O

C —O—CH2CH2—O—C— —C—

O

O

D —O—CH2CH2—O—C— —C—O—

O O


9


19 Iron and steam at high temperature react in a closed vessel to give an equilibrium mixture

3Fe(s) + 4H2O(g) Fe3O4(s) + 4H2(g)

Which of the following is the correct expression for Kp?

A Kp = PP

H

H O

2

2

B Kp = P PP P

Fe O H

Fe H O

3 4 2

2

4

3 4

C Kp = PP

H

H O

2

2

4

4

D Kp = PH2

4


20 At 100 °C, pure water has a pH of 6, whereas at 25 °C it has a pH of 7. This is because

A the dissociation of water is endothermic, so the concentration of hydrogen ions is lower at 100 °C than it is at 25 °C.

B the dissociation of water is exothermic, so the concentration of hydrogen ions is lower at 100 °C than it is at 25 °C.

C the dissociation of water is endothermic, so the concentration of hydrogen ions is higher at 100 °C than it is at 25 °C.

D at 100 °C, water has a higher concentration of hydrogen ions than of hydroxide ions.



2

*N37962A0224*

SECTION A

Answer ALL the questions in this section. You should aim to spend no more than 20 minutes on

this section. For each question, select one answer from A to D and put a cross in the box .

If you change your mind, put a line through the box and then mark your new answer with

a cross .

1 The compound butane has

A the empirical formula C4H10 and the molecular formula C2H5.

B the empirical formula C2H5 and the molecular formula C4H10.

C the empirical formula C2H5 and the molecular formula CnH2n+2.

D the empirical formula CnH2n+2 and the molecular formula C4H10.


2 For the oxidation of ammonia

a NH3 + b O2 c NO + d H2O

the values of the coefficients in the balanced equation are

A a = 2, b = 3, c = 2 and d = 3

B a = 4, b = 7, c = 4 and d = 4

C a = 4, b = 5, c = 4 and d = 6

D a = 6, b = 7, c = 6 and d = 9


3 The Avogadro constant is 6.0 × 1023 mol–1. Therefore the number of atoms in 1 mol of

carbon dioxide is

A 2.0 × 1023

B 6.0 × 1023

C 1.2 × 1024

D 1.8 × 1024


3


4 The equation for the complete combustion of octane is

2C8H18 + 25O2 16CO2 18H2O

(a) The mass of 10 mol of octane is

(1)

A 0.66 kg

B 1.14 kg

C 2.10 kg

D 2.28 kg

(b) The volume of 1 mol of any gas (measured at room temperature and pressure)

is 24 dm3. Hence the volume of oxygen (measured at room temperature and

pressure) required for the complete combustion of 10 mol of octane is

(1)

A 240 dm3

B 300 dm3

C 3000 dm3

D 6000 dm3


5 The enthalpy change for the reaction

CH4(g) C(g) + 4H(g)

is +1648 kJ mol–1. Hence the mean bond enthalpy for the C–H bond is

A +329.6 kJ mol–1

B +412.0 kJ mol–1

C +1648 kJ mol–1

D +6592 kJ mol–1


4

*N37962A0424*

6 The graph below represents the successive ionization energies of an element X plotted

against the number of the electron removed. X is not the symbol for the element.

(a) From this graph it is possible to deduce the group in the Periodic Table to which X

belongs. X is in

(1)

A Group 1

B Group 3

C Group 5

D Group 7

(b) From the graph it is possible to deduce that the most stable ion of X will be

(1)

A X3+

B X+

C X–

D X3–



5

4.5

4

3.5

3

2.5

20

Electron removed

2 4 6 8 10 12

Logarithm

ionization

energy

5


7 Element R is in Group 1 of the Periodic Table and element T is in Group 6. R and T

are not the symbols for the elements.

(a) The compound of R and T will have the formula

(1)

A RT

B RT6

C RT2

D R2T

(b) The compound of R and T will have bonding which is predominantly

(1)

A ionic.

B covalent.

C dative covalent.

D metallic.

(c) In terms of its electrical conductivity, the compound of R and T will

(1)

A conduct when solid and liquid.

B conduct when solid but not when liquid.

C conduct when liquid but not when solid.

D not conduct when solid or liquid.



6

*N37962A0624*

8 Ethane reacts with chlorine when the substances are exposed to UV radiation.

(a) The equation for this reaction is

(1)

A C2H6 + Cl2 C2H5Cl + HCl

B C2H6 + Cl2 C2H4Cl2 + H2

C C2H6 + Cl2 2CH3Cl

D C2H4 + Cl2 C2H4Cl2

(b) The role of the UV radiation in the reaction is to

(1)

A break the Cl Cl bond forming Cl• free radicals.

B break the Cl Cl bond forming Cl+ and Cl– ions.

C break the C C bond in ethane forming CH3• free radicals.

D break a C H bond in ethane forming C2H5• free radicals.

(c) The overall reaction between ethane and chlorine is best described as

(1)

A addition.

B homolytic fission.

C heterolytic fission.

D substitution.



7


9 This question concerns the following compounds

A B C D

Which of these compounds will show geometric (E–Z or cis/trans) isomerism?

A

B

C

D


10 The correct name for the compound shown below is

A 2-methylbut-3-ene

B 3-methylbut-2-ene

C 3-methylbut-3-ene

D 2-methylbut-2-ene


11 Most compounds of lead are insoluble, an exception being lead(II) nitrate. Therefore a

good method of preparing lead(II) sulfate is

A adding dilute sulfuric acid to lead metal.

B adding concentrated sulfuric acid to lead metal.

C adding dilute sulfuric acid to lead(II) nitrate solution.

D adding dilute sulfuric acid to solid lead(II) oxide.


8

*N37962A0824*

12 Metals usually have high melting temperatures and boiling temperatures because there

are

A strong attractions between the ions.

B strong attractions between the delocalised electrons.

C strong attractions between the ions and the delocalised electrons.

D strong intermolecular forces.


13 In 2006, the concentration of carbon dioxide in the atmosphere was 382 ppm. This is

equivalent to

A 0.00382%

B 0.0382%

C 0.382%

D 3.82%


14 A hazard that is particularly associated with alkanes is that they are

A corrosive.

B flammable.

C toxic by inhalation.

D toxic by skin absorption.



2

*N37963A0224*

SECTION A




a cross .

1 The equation for the reaction between limewater and hydrochloric acid, including state

symbols, is

A CaOH(s) + HCl(aq) CaCl(aq) + H2O(l)

B Ca(OH)2(s) + 2HCl(aq) CaCl2(aq) + 2H2O(aq)

C CaOH(aq) + HCl(aq) CaCl(aq) + H2O(aq)

D Ca(OH)2(aq) + 2HCl(aq) CaCl2(aq) + 2H2O(l)


2 As you go down Group 2 of the Periodic Table, which of the following decreases?

A The reactivity of the elements.

B The solubility of the hydroxides of the elements.

C The solubility of the sulfates of the elements.

D The thermal stability of the carbonates of the elements.


3 Which concentrated acid would be best for mixing with a salt to carry out a flame test?

A Hydrochloric acid

B Nitric acid

C Phosphoric(V) acid

D Sulfuric acid


4 The flame produced by a compound containing barium in a flame test is

A colourless.

B green.

C red.

D yellow.


3


5 Which of the following is a greenhouse gas?

A Argon

B Nitrogen

C Oxygen

D Water vapour


6 For parts (a) and (b), use your knowledge of intermolecular forces to predict the

compound with the highest boiling temperature.

(a) A HF

B H2O

C NH3

D CH4

(1)

(b) A 1-iodobutane

B 1-chlorobutane

C 2-methyl-2-iodopropane

D 2-methyl-2-chloropropane

(1)



4

*N37963A0424*

7 Consider the following organic liquids:

A ethanal

B ethanol

C tetrachloromethane

D trichloromethane

(a) Each liquid is run from a burette. Which liquid would not be deflected significantly

by a charged rod?

(1)

A

B

C

D

(b) Which liquid would react with phosphorus(V) chloride to give a gas which fumes in

moist air?

(1)

A

B

C

D

(c) Which liquid would you expect to have the peak at the greatest mass/charge ratio in

its mass spectrum?

(1)

A

B

C

D

(d) Which liquid has an infrared spectrum with a broad absorption due to hydrogen

bonding?

(1)

A

B

C

D


5


8 Which of the following best defines the meaning of the term anthropogenic change?

It is a change caused by

A nature.

B plants.

C animals.

D humans.


9 Which of the following equations represents the change when concentrated sulfuric acid

is added to solid potassium chloride at room temperature?

A 8KCl + 5H2SO4 4K2SO4 + H2S + 4Cl2 + 4H2O

B 2KCl + 3H2SO4 2KHSO4 + SO2 + Cl2 + 2H2O

C 6KCl + 4H2SO4 3K2SO4 + S + 3Cl2 + 4H2O

D KCl + H2SO4 KHSO4 + HCl


10 The Maxwell-Boltzmann distribution of molecular energies is useful for explaining why

increasing temperature affects the rate of a chemical reaction.

(a) Which of the following statements describes how the shape of the Maxwell-

Boltzmann distribution curve changes as temperature increases?

(1)

A The peak decreases in height and moves to the left.

B The peak increases in height and moves to the left.

C The peak decreases in height and moves to the right.

D The peak increases in height and moves to the right.

(b) The main reason that reaction rates increase with temperature is that

(1)

A all the molecules move faster.

B all the molecules collide more frequently.

C more molecules collide with the correct orientation.

D a larger proportion of molecules have high energies.


6

*N37963A0624*

11 Four organic reactions are given below:

A CH3CH3 CH2 CH2 + H2

B nCH2 CH2 ( CH2 CH2 ) n

C CH2 CH2 + HBr CH3CH2Br

D CH3CH2Br + H2O CH3CH2OH + HBr

(a) Which reaction is a substitution reaction?

(1)

A

B

C

D

(b) Which reaction is an electrophilic addition reaction?

(1)A

B

C

D

(c) Which reaction involves initial attack by a nucleophile?

(1)A

B

C

D

(d) Which reaction requires an initiator?

(1)

A

B

C

D


7


12 Which of the following statements is true?

A CFCs and nitrogen monoxide, NO, are involved in the depletion of the ozone

layer.

B CFCs act as catalysts for the depletion of the ozone layer, while nitrogen

monoxide, NO, does not.

C CFCs and ozone are free radicals.

D CFCs and nitrogen monoxide, NO, are decomposed by UV radiation.



2

*N37949A0224*

SECTION A




a cross .

1 Methods for investigating reaction rates include

A colorimetry.

B measurement of change in volume.

C measurement of change of mass.

D quenching followed by titrating with acid.

Which method would be most suitable to investigate the rate of the following reactions?

(a) HCOOCH3(aq) + NaOH(aq) HCOONa(aq) + CH3OH(aq)

(1)

A

B

C

D

(b) (CH3)2C=CH2(g) + HI(g) (CH3)3CI(g)

(1)

A

B

C

D

(c) BrO3–(aq) + 5Br–(aq) + 6H+(aq) 3Br2(aq) + 3H2O(l)

(1)

A

B

C

D


3


2 2H2(g) + 2NO(g) 2H2O(g) + N2(g)

This reaction is first order with respect to hydrogen and second order with respect to

nitrogen(II) oxide.

By what factor will the initial rate increase if the concentration of hydrogen and

nitrogen(II) oxide are both tripled?

A 3

B 9

C 12

D 27


3 Which reaction has the most positive entropy change for the system, Ssystem?

A NaOH(aq) + HCl(aq) NaCl(aq) + H2O(l)

B AgNO3(aq) + NaCl(aq) AgCl(s) + NaNO3(aq)

C C2H4(g) + HCl(g) C2H5Cl(l)

D C4H10(g) C2H4(g) + C2H6(g)


4 Barium carbonate decomposes in an endothermic reaction when heated to 1500 K.

BaCO3(s) BaO(s) + CO2(g)

What are the signs of the entropy changes at 1500 K?

Ssystem Ssurroundings

A + +

B + –

C – +

D – –



4

*N37949A0424*

5 What are the units of Kc for the following equilibrium?

2SO2(g) + O2(g) 2SO3(g)

A atm

B atm–1

C dm3 mol–1

D mol dm–3


6 The graph below shows the yield of product in a gaseous equilibrium at different

temperatures and pressures.

The forward reaction in the equilibrium is

A exothermic, and the number of moles of gas is increasing.

B endothermic, and the number of moles of gas is increasing.

C exothermic, and the number of moles of gas is decreasing.

D endothermic, and the number of moles of gas is decreasing.



% product at

equilibrium 300 atm

200 atm

Temperature/ C

5


7 Hydrogen cyanide, HCN, reacts with propanal, CH3CH2CHO, in the presence of

potassium cyanide, KCN.

(a) The mechanism for this reaction is

(1)

A nucleophilic addition.

B nucleophilic substitution.

C electrophilic addition.

D electrophilic substitution.

(b) The first stage of the mechanism of this reaction is

(1)

A the lone pair of electrons on carbon in CN– attacking C + of propanal.

B the lone pair of electrons on nitrogen in CN– attacking C + of propanal.

C the lone pair of electrons on oxygen in propanal attacking C + of HCN.

D the lone pair of electrons on oxygen in propanal attacking H + in HCN.

(c) The product of the reaction is

(1)

A 1-hydroxypropanenitrile.

B 2-hydroxypropanenitrile.

C 1-hydroxybutanenitrile.

D 2-hydroxybutanenitrile.


8 Which of the following does not have hydrogen bonding in a pure sample, but forms

hydrogen bonds with water when it dissolves?

A Propane

B Propanal

C Propanol

D Propanoic acid


6

*N37949A0624*

9 Which of the following has both optical and E-Z isomers?

A ClCH2CHClCH=CH2

B CH2=CClCH2CH2Cl

C ClCH2CH=CHCH2Cl

D CHCl=CHCHClCH3


10 One optically active isomer of 2-chlorobutane reacts with hydroxide ions to form

butan-2-ol.

C2H5CHClCH3 + OH– C2H5CH(OH)CH3 + Cl–

The organic product is a mixture of enantiomers because

A butan-2-ol contains a chiral carbon atom.

B the reaction is a nucleophilic substitution.

C 2-chlorobutane forms a carbocation intermediate.

D 2-chlorobutane forms a five-bonded transition state.


11 The organic product of the reaction between ethanoyl chloride and methylamine has the formula

A CH3NHCH2C

O

Cl

B CH3CH(NH2)C

O

Cl

C CH3C

O

NH2

D CH3C

O

NHCH3


7


12 A section of a polymer is shown below. Which of the following monomers would form

this polymer?

OCH2CH2COCH2CH2C

O O

A HOCH2CH2OH and ClCOCH2CH2COCl

B HOCH2CH2OH and HOOCCH2CH2COOH

C ClCH2CH2COCl alone

D HOCH2CH2COOH alone


13 Which of the following is not a reaction of a BrØnsted-Lowry acid and base?

A CH3Cl + OH– CH3OH + Cl–

B NH3 + HCl NH4+ + Cl–

C H2O + HSO4– H2SO4 + OH–

D HCO3– + H2O CO3

2– + H3O+


14 A buffer solution is made from ammonia and ammonium chloride. When a small

amount of acid is added to this buffer

A hydrogen ions in the acid combine with chloride ions to make HCl.

B hydrogen ions in the acid combine with NH3 to make NH4+.

C NH4+ ions dissociate to make more NH3.

D the hydrogen ions in the acid prevent dissociation of the NH4Cl.



8

*N37949A0824*

15 Information about four samples of acid is shown below.

Sample 1: 1.0 mol dm–3 HCl

Sample 2: 1.0 mol dm–3 H2SO4

Sample 3: 0.1 mol dm–3 HCl

Sample 4: 0.1 mol dm–3 CH3COOH

Which of the following lists shows the samples in order of increasing pH?

A 1, 2, 3, 4

B 4, 3, 2, 1

C 2, 1, 3, 4

D 4, 3, 1, 2


16 Which reaction has an enthalpy change equal to the enthalpy of hydration of the sodium

ion?

A Na+(g) + excess H2O(l) Na+(aq)

B Na+(g) + 1 mol of H2O(l) Na+(aq)

C Na+(s) + excess H2O(l) Na+(aq)

D Na+(s) + 1 mol of H2O(l) Na+(aq)



2

*N37954A0224*

SECTION A




a cross .

1 What type of bonding occurs between the metal ion and ligand in the complex ion

[Cu(H2O)6]2+?

A Metallic

B Ionic

C Hydrogen

D Dative covalent


2 Which of these four amino acids could not rotate the plane of plane-polarised light?

A H2NCH(CH3)COOH

B H2NCH(CH2COOH)COOH

C H2NCH2COOH

D H2NCH(CH2SH)COOH


3 In the solid state, the amino acid serine exists in the form

A H3N+CH(CH2OH)COOH

B H3N+CH(CH2OH)CO2

C H2NCH(CH2OH)COOH

D H2NCH(CH2OH)CO2


4 The best method for separating a mixture of amino acids in solution is

A distillation.

B solvent extraction.

C chromatography.

D recrystallization.


3


5 How many different peaks due to hydrogen atoms would you expect to see in a low

resolution proton nmr spectrum of propanoic acid, CH3CH2COOH?

A Two

B Three

C Five

D Six


6 In a high resolution proton nmr spectrum of ethanoic acid, CH3COOH, the peak due to

the hydrogen atoms in the methyl group would be a

A singlet.

B doublet.

C triplet.

D quartet.


7 Which of these compounds will not form an amide in a reaction with ethanoyl chloride?

A NH3

B CH3CH2NH2

C CH3CH2NH(CH3)

D CH3CH2N(CH3)2



4

*N37954A0424*

8 This question concerns the following organic compounds.

A CH3COCl

B CH3COOH

C CH3COOCH2CH3

D C6H5OH

Which compound is most likely to

(a) form the solution with the lowest pH when mixed with water?

(1)

A

B

C

D

(b) burn with a smoky flame?

(1)

A

B

C

D

(c) have a fruity smell?

(1)

A

B

C

D

(d) have an absorption in its IR spectrum at about 1795 cm 1?

(1)

A

B

C

D


5


9 This question is about the reaction scheme below.

Which step is most likely to need

(a) tin and concentrated hydrochloric acid?

(1)

A Step 1

B Step 2

C Step 3

D Step 4

(b) a catalyst of iron(III) chloride?

(1)

A Step 1

B Step 2

C Step 3

D Step 4

(c) a nickel catalyst?

(1)

A Step 1

B Step 2

C Step 3

D Step 4


Cl

NO2

Cl

NH2

step 1 step 2 step 3

Cl

NH2

step 4

Cl

6

*N37954A0624*

10 The apparatus below can be used to measure the value of Ecell for the reaction

2Fe3+(aq) + Zn(s) 2Fe2+(aq) + Zn2+(aq)

The electrodes are:

electrode 1 electrode 2

A zinc iron

B iron zinc

C zinc platinum

D platinum platinum


11 Copper reacts with silver ions according to the reaction below.

Cu(s) + 2Ag+(aq) Cu2+(aq) + 2Ag(s)

E cell for this reaction is

A +0.46 V

B +1.14 V

C +1.26 V

D +1.94 V


electrode 1

ZnSO4(aq)

electrode 2

FeSO4(aq) / Fe2(SO4)3(aq)

V

7


12 E cell for four reactions are shown in the table below.

E cell / V

Reaction 1 +1.10

Reaction 2 +0.65

Reaction 3 +0.10

Reaction 4 –1.30

Which reaction

(a) is thermodynamically not feasible?

(1)

A Reaction 1

B Reaction 2

C Reaction 3

D Reaction 4

(b) has the largest value for ln K?

(1)

A Reaction 1

B Reaction 2

C Reaction 3

D Reaction 4


8

*N37954A0824*

13 Consider the reaction scheme below and calculate the mass of aspirin you would expect

to form if you started with 47 g of phenol.

A 31.96 g

B 61.20 g

C 74.25 g

D 90.00 g


14 Which of the monomers A to D would form the polymer below?

A

Cl

B

Cl

C

Cl

D

Cl



step 1

yield 85%

step 2

yield 80%

OH OH OCOCH3

CO2HCO2H

phenol, Mr = 94 aspirin, Mr = 180

C C

CH3 C2H5

HCl

⎡

⎣

⎢⎢⎢⎢ ⎡

⎣

⎢⎢⎢⎢

n

2

*P39295A0224*

SECTION A



1 A molecule is

A a group of atoms bonded by ionic bonds.

B a group of atoms bonded by covalent bonds.

C a group of ions bonded by covalent bonds.

D a group of atoms bonded by metallic bonds.


2 The relative atomic mass is defined as

A the mass of an atom of an element relative to 1/12 the mass of a carbon-12 atom.

B the mass of an atom of an element relative to the mass of a hydrogen atom.

C the average mass of an element relative to 1/12 the mass of a carbon atom.

D the average mass of an atom of an element relative to 1/12 the mass of a carbon-12 atom.



3

*P39295A0324* Turn over

3 The definition of the mole is

A the amount of any substance which occupies a volume of 24 dm3 at room temperature and pressure.

B the amount of any substance containing the same number of identical entities as there are in exactly 12 g of the carbon-12 isotope.

C the number of atoms in exactly 12 g of the carbon-12 isotope.

D the number of molecules in exactly 2 g of hydrogen at room temperature and pressure.


4 The concentration of blood glucose is usually given in millimoles per dm3 or mmol dm–3. A reading of 5.0 mmol dm–3 is within the normal range. Glucose has a molar mass of 180 g mol–1. What mass of glucose dissolved in 1 dm3 of blood would give this normal reading?

A 0.090 g

B 0.18 g

C 0.90 g

D 9.0 g


5 In an experiment performed to measure the enthalpy change for the reaction

Cu2+ 2+(aq)

3.0 g of zinc powder (an excess) was added to 30.0 cm3 of copper(II) sulfate solution of concentration 1.00 mol dm–3. The temperature rise of the mixture was 47.6 K. Assuming that the heat capacity of the solution is 4.2 J K–1 g–1, the enthalpy change for the reaction is given by

A H

B H

C H

D H


4

*P39295A0424*

6 H for the process

A I2(s) I2(g)

B I2(s) 2I(g)

C I2(g) 2I(g)

D ½I2(s) I(g)


7 The enthalpy change for the reaction

C(s, graphite) + ½O2(g) CO(g)

cannot be measured directly since some carbon dioxide is always formed in the reaction. It can be calculated using Hess’s Law and the enthalpy changes of combustion of graphite and of carbon monoxide.

C(s, graphite) + O2(g) CO2 H –1

CO(g) + ½O2(g) CO2 H –1

The enthalpy change for the reaction of graphite with oxygen to give carbon monoxide is

A –1

B –1

C –1

D –1



5


8 –1.

C3H8 C4H10C5H12C6H14

–1.

A C7H16

B C8H18

C C9H20

D C10H22


9 If the mean C H bond enthalpy is +x, which of the following represents a process with an enthalpy change of +4x?

A C(g) + 4H(g) CH4(g)

B CH4(g) C(g) + 4H(g)

C CH4(g) C(s, graphite) + 2H2(g)

D C(s, graphite) + 2H2(g) CH4(g)


10 –1):

789, 1577, 3232, 4356, 16091, 19785, 23787, 29253.

The element is in

A Group 1

B Group 2

C Group 3

D Group 4


6

*P39295A0624*

11 Which of the graphs shows (from left to right) the trend in the ionic radius of the isoelectronic ions N3–, O2–, F–, Na+, Mg2+, Al3+?

A B

C D



N3– Mg2+O2– F– (Ne) Na+ Al3+ N3– Mg2+O2– F– (Ne) Na+ Al3+

N3– Mg2+O2– F– (Ne) Na+ Al3+

Ionic radius

N3– Mg2+O2– F– (Ne) Na+ Al3+

Ionic radius

Ionic radius

Ionic radius

7


12 Oxygen can be prepared using several different reactions. Which of those given below has the highest atom economy by mass?

A NaNO3 NaNO2 + ½O2

B H2O2 H2O + ½O2

C Cl2 + H2O 2HCl + ½O2

D PbO2 PbO + ½O2


13 The ionic radii in nm of some ions are given below.

Li+ 0.074 F– 0.133Ca2+ 0.100 Cl– 0.180

O2– 0.140S2– 0.185

(a) Which of the following compounds has the most exothermic lattice energy? They all have the same crystal structure.

(1)

A LiF

B LiCl

C CaO

D CaS

(b) Which of the following compounds will show the greatest difference between the experimental (Born-Haber) lattice energy and that calculated from a purely ionic model?

(1)

A LiF

B Li2O

C CaO

D CaS


8

*P39295A0824*

14 Which of the following is the correct order for the processes used to obtain petrol from petroleum (crude oil)?

A Petroleum fractional distillation reforming petrol.

B Petroleum reforming fractional distillation petrol.

C Petroleum reforming fractional distillation petrol.

D Petroleum fractional distillation reforming petrol.


15 In the reaction between ethene and bromine, the bromine molecule acts as an electrophile.

CH2 CH2 + Br2 BrCH2CH2Br

Which of the following statements is true?

A Ethene acts as a nucleophile because it is polar.

B Ethene acts as a nucleophile because it can donate a pair of electrons to bromine.

C Ethene is not a nucleophile in this reaction.

D Ethene acts as a nucleophile because it donates a single electron to bromine.


16

A Z-4-ethylhex-4-ene

B E-3-ethylhex-2-ene

C Z-3-ethylhex-2-ene

D E-3-propylpent-2-ene


C C

H3C

H

CH2CH2CH3

CH2CH3

9


17 If propene, CH3CH CH2, is reacted with aqueous acidified potassium manganate(VII) the organic product is

A CH3CH(OH)CH2OH

B CH3CH(OH)CH3

C HOCH2CH2CH2OH

D CH3CH2CH2OH


18 How many compounds have the formula C5H12?

A 1

B 2

C 3

D 4


19 An organic compound reacts with chlorine in the presence of ultraviolet light. The relative molecular mass of the product has increased by 34.5 compared with the original compound. What is the reaction mechanism?

A Free radical substitution

B Electrophilic substitution

C Nucleophilic substitution

D Free radical addition



2

*P39303A0224*

SECTION A



1 This question concerns the shapes of molecules and ions:

A linear

B trigonal planar

C pyramidal

D tetrahedral

Select from A to D the shape of

(a) boron trichloride, BCl3(1)

A

B

C

D

(b) the ammonium ion, NH4+

(1) A

B

C

D

(c) carbon dioxide, CO2(1)

A

B

C

D


3


2 Tetrachloromethane, CCl4, is a

A polar molecule with polar bonds.

B polar molecule with non-polar bonds.

C non-polar molecule with polar bonds.

D non-polar molecule with non-polar bonds.


3 The difference in boiling temperature between methane (Tb = 109 K) and ethane (Tb = 185 K) is best explained by the different numbers of

A protons.

B electrons.

C covalent bonds.

D hydrogen bonds.


4 What is the oxidation number of oxygen in OF2?

A

B

C +1

D +2


5 In which of the following reactions is sulfuric(IV) acid, H2SO3, acting as an oxidizing agent?

A 2NaOH + H2SO3 Na2SO3 + 2H2O

B 2FeCl3 + H2SO3 + H2O 2FeCl2 + H2SO4 + 2HCl

C 2H2S + H2SO3 3H2O + 3S

D H2SO3 H2O + SO2


4

*P39303A0424*

6 Ethanol is soluble in water. The best explanation for this is

A ethanol molecules form hydrogen bonds with water molecules.

B ethanol molecules form London (dispersion) forces with water molecules.

C ethanol molecules form permanent dipole interactions with water molecules.

D ethanol and water are miscible liquids.


7 During a titration, when the solution in a pipette is transferred to a conical flask, a small amount of liquid remains in the tip of the pipette. This situation should be dealt with by

A leaving the liquid in the pipette which is calibrated to allow for it.

B slightly over-filling the pipette to compensate for the additional volume.

C carefully blowing the liquid out of the pipette to ensure that it is empty.

D repeating the titration.


8 The tolerance of a 25 cm3 pipette is ±0.06 cm3. The percentage error in the measurement of 25 cm3 using this pipette is

A ±0.06%

B ±0.12%

C ±0.24%

D ±0.48%


9 A series of titrations is carried out using the same conical flask. Before carrying out each titration, the conical flask must be

A rinsed with ethanol.

B rinsed with distilled or deionised water.

C rinsed with the solution that it will contain.

D dried to remove all traces of liquid.


5


10 When excess calcium is added to water, effervescence occurs and

A a clear colourless solution is formed.

B a cloudy suspension is formed.

C an orange-red flame is seen.

D a yellow flame is seen.


11 When samples of magnesium nitrate, Mg(NO3)2, and calcium nitrate, Ca(NO3)2, are heated

A both compounds decompose to form the corresponding nitrite and oxygen.

B both compounds decompose to form the corresponding oxide, nitrogen dioxide and oxygen.

C magnesium nitrate decomposes to form magnesium nitrite and oxygen whereas calcium nitrate decomposes to form calcium oxide, nitrogen dioxide and oxygen.

D magnesium nitrate decomposes to form magnesium oxide, nitrogen dioxide and oxygen whereas calcium nitrate decomposes to form calcium nitrite and oxygen.


12 Which of the following properties of the elements chlorine, bromine and iodine increases with increasing atomic number?

A Boiling temperature

B Bond enthalpy

C Electronegativity

D First ionization energy



6

*P39303A0624*

13 Which of the following is a secondary alcohol?

A butan-1-ol

B butan-2-ol

C 2-methylpropan-1-ol

D 2-methylpropan-2-ol


14 The compound

has the systematic name

A 2-chlorobutane

B 3-chlorobutane

C 1-chloro-1-methylpropane

D 1-chloro-2-methylbutane


15 When a chloroalkane is heated with aqueous sodium hydroxide

A no reaction occurs with primary, secondary or tertiary chloroalkanes.

B a reaction occurs with primary and secondary chloroalkanes but not with tertiary chloroalkanes.

C a reaction occurs with tertiary chloroalkanes but not with primary and secondary chloroalkanes.

D a reaction occurs with primary, secondary and tertiary chloroalkanes.



Cl

7


16 Brown nitrogen dioxide, NO2, exists in equilibrium with colourless dinitrogen tetroxide, N2O4.

2NO2(g) N2O4 H brown colourless

(a) The pressure is increased. When equilibrium is restored, the appearance of the mixture of gases will be

(1)

A colourless.

B unchanged.

C paler brown.

D darker brown.

(b) The temperature is increased. When equilibrium is restored, the appearance of the mixture of gases will be

(1) A colourless.

B unchanged.

C paler brown.

D darker brown.


17 When propanal, CH3CH2CHO, and propanone, CH3COCH3, are compared using physical methods of analysis, which of the following is not correct?

A The carbonyl groups absorb at very similar frequencies of the IR spectrum.

B The compounds will have different patterns in the fingerprint region of the IR spectrum.

C The compounds will form different fragmentation patterns in a mass spectrum.

D The compounds will have molecular ion peaks at different mass to charge ratios in a mass spectrum.



2

*P39304A0224*

SECTION A



1 The reaction between carbon monoxide and hydrogen reaches a dynamic equilibrium.

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

(a) Which of these statements about a dynamic equilibrium is not true?(1)

A The forward rate of reaction is equal to the backward rate of reaction.

B The concentrations of the products and reactants do not change.

C The concentrations of the products and reactants are equal.

D The equilibrium can be approached from either direction.

(b) The Kc expression for the above reaction is(1)

A Kc3

22

[CH OH][CO] × [H ]

=

B Kc2

3

[CO] × 2[H ][CH OH]

=

C Kc2

2

3

[CO] × [H ][CH OH]

=

D Kc3

2

[CH OH][CO] × 2[H ]

=



3


2 Hydrogen and iodine, both with an initial concentration of 0.010 mol dm , were allowed to react. At equilibrium, the concentration of hydrogen iodide was 0.0030 mol dm .

H2(g) + I2(g) 2HI(g)

Kc is calculated using the values

H2(g) / mol dm I2(g) / mol dm HI(g) / mol dm

A 0.0070 0.0070 0.0030

B 0.0040 0.0040 0.0030

C 0.0040 0.0040 0.0060

D 0.0085 0.0085 0.0030


3 The reaction below reached a dynamic equilibrium from an initial mixture of all four substances P, Q, R and S in aqueous solution.

P + Q R + S

The following data were obtained.

Substance Concentration at equilibrium / mol dm–3

P 0.050

Q 0.040

R 0.020

S 0.010

Kc for the equilibrium is

A 0.10

B 0.33

C 3.00

D 10.0


4

*P39304A0424*

4 The Haber process is used to make ammonia from nitrogen and hydrogen at 450 C.

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

(a) If the partial pressures of these gases were measured in atm, the units of the equilibrium constant Kp will be

(1)

A atm

B atm2

C atm

D atm

(b) When the temperature of the system is increased(1)

A Kp decreases.

B Kp increases.

C Kp stays the same.

D Kp first decreases and then increases.


5 In high performance liquid chromatography, HPLC, which of these factors does not affect the time taken for a component to pass through the column?

A Type of detector

B Material of stationary phase

C Particle size of stationary phase

D Temperature of column


6 When equimolar amounts of the solutions below are mixed, which forms a buffer solution with a pH less than 7?

A Hydrochloric acid and sodium chloride

B Ethanoic acid and sodium ethanoate

C Sodium hydroxide and sodium chloride

D Ammonia and ammonium chloride


5


7 The pH of a 1.5 mol dm–3 solution of hydrochloric acid, HCl(aq), is

A

B

C 0.18

D 1.50


8 Which of these solid substances is likely to have the greatest standard entropy? Use of the data booklet is not required.

A SnO

B SnO2

C SnBr2

D SnBr4


9 What is the correct name for the molecule shown below?

A Z-2-bromobut-2-ene

B E-2-bromobut-2-ene

C E-3-bromobut-2-ene

D Z-3-bromobut-2-ene



C C

H CH3

BrH3C

6

*P39304A0624*

10 Ketones react with hydrogen cyanide, HCN, in the presence of cyanide ions, CN .

(a) Which of these ketones does not form a racemic mixture in this reaction?(1)

A CH3CH2CH2COCH3

B CH3CH2COCH2CH3

C CH3CH2CH2CH2COCH3

D CH3CH2CH2COCH2CH3

(b) This type of reaction is classified as (1)

A nucleophilic substitution.

B nucleophilic addition.




11 Which of these is not observed when ethanoyl chloride reacts with water?

A Misty fumes given off.

B The gas given off turns damp blue litmus paper red.

C The mixture gets hot.

D A white precipitate forms.


12 UV light is useful in initiating some reactions because it

A lowers the activation energy of the reaction.

B causes bonds in molecules to stretch and bend.

C causes molecules to form ions.

D causes molecules to form free radicals.


7


13 Butane-1,4-diol, HO(CH2)4OH, and benzene-1,4-dicarboxylic acid,

HOOC COOH, react to form a polyester.

(a) The repeat unit of the polyester is(1)

A O (CH2)4 O C C O (CH2)4 O⎡

⎣⎢

⎤

⎦⎥

O

O

B O (CH2)4 C C (CH2)4 O⎡

⎣⎢

⎤

⎦⎥

O

O

C O (CH2)4 O C C⎡

⎣⎢

⎤

⎦⎥

O

O

D O (CH2)4 O C C O⎡

⎣⎢

⎤

⎦⎥

O

O

(b) The type of reaction is(1)

A hydrolysis.

B addition.

C substitution.

D condensation.


8

*P39304A0824*

14 The equation for the enthalpy of hydration for a magnesium ion is

A Mg2+(s) + aq Mg2+(aq)

B Mg2+(g) + aq Mg2+(aq)

C Mg2+(aq) Mg2+(g) + aq

D Mg2+(aq) Mg2+(s) + aq


15 The IR spectrum of a substance is shown below.

Which of the following substances has this spectrum?

You may use the information on page 6 of the data booklet.

A Propan-1-ol

B Propanal

C Propanone

D Propanoic acid


100

4000

50

03000 2000 1500 1000 500

Wavenumber / cm–1

Transmittance / %

9


16 Two ketones, CH3COCH2CH2CH3 and CH3CH2COCH2CH3, both have Mr = 86. Which peak due to fragmentation into singly charged ions would you expect to be present in the mass spectrum of one but not the other?

A 71

B 57

C 43

D



2

*P35302A0228*

SECTION A



1 An electrochemical cell consists of a standard hydrogen electrode and a Cu2+(aq)|Cu(s) electrode which uses copper(II) sulfate solution. Which one of the following does not affect the e.m.f. of the cell?

A The volume of the copper(II) sulfate solution.

B The temperature.

C The pressure of the hydrogen.

D The concentration of the copper(II) sulfate solution.


2 Which answer corresponds to the correct value of Ecell for the oxidation of hydrogen peroxide by manganate(VII) ions? The half-reactions are

2H+ + O2 + 2e– H2O2 E = + 0.68 V

MnO4– + 8H+ + 5e– Mn2+ + 4H2O E = + 1.51 V

The overall equation is

2MnO4– + 6H+ + 5H2O2 2Mn2+ + 8H2O + 5O2

A Ecell = + 2.19 V

B Ecell = – 0.83 V

C Ecell = – 0.38 V

D Ecell = + 0.83 V



3


3 The transition metal complex Pt(NH3)2Cl2 exists as two geometric isomers. This is because the complex

A is square-planar.

B is tetrahedral.

C contains a double bond.

D is octahedral.


4 Hydrogen peroxide, H2O2, can be analysed by titration. The hydrogen peroxide solution is treated with acidified potassium iodide solution, and the liberated iodine is titrated with a standard solution of sodium thiosulfate, Na2S2O3. The products are iodide ions and tetrathionate ions, S4O6

2 .

Which of the following applies to this reaction?

Action of H2O2 Action of S2O3

A oxidizing agent oxidizing agent

B oxidizing agent reducing agent

C reducing agent oxidizing agent

D reducing agent reducing agent


5 A hydrated transition metal ion is colourless. Which of the following could be the electronic configuration of this ion?

A [Ar] 3d54s2

B [Ar] 3d8

C [Ar] 3d104s2

D [Ar] 3d10



4

*P35302A0428*

6 Which of the following reagents would enable you to separate iron(III) hydroxide from a mixture of iron(III) hydroxide and copper(II) hydroxide?

A Dilute hydrochloric acid

B Aqueous ammonia

C Dilute nitric acid

D Sodium hydroxide solution


7 When a solution containing 0.10 mol of chromium(III) chloride, CrCl3.6H2O, is treated with excess silver nitrate solution, 0.20 mol of silver chloride, AgCl, is immediately precipitated. The formula of the complex ion in the solution is

A [Cr(OH)6]3–

B [Cr(H2O)6]3+

C [CrCl(H2O)5]2+

D [CrCl2(H2O)4]+


8 Which of the following species is not able to act as a ligand in the formation of transition metal complexes?

A C6H5NH2

B NH3

C NH2CH2CH2CH2NH2

D NH4+


9 The element zinc, with electronic configuration 1s22s22p63s23p63d104s2, is not regarded as a transition element because

A the oxide of zinc is amphoteric.

B none of its ions has an unpaired electron in the d-subshell.

C it does not readily form complex ions.

D it has a boiling temperature low enough for it to be easily distilled.


5


10 The compounds below were heated with aqueous sodium hydroxide solution. Which one of them did not give sodium ethanoate, CH3COONa, as one of the products?

A CH3COOCH3

B CH3COCH3

C CH3COOH

D CH3COCl


11 Which of the following products is formed when phenylamine (aniline) is reacted with dilute sulfuric acid?

A

NO2

B

SO3H

C

+ –NH3HSO4

D

NH2

SO3H



6

*P35302A0628*

12 For the nitration of phenol, which is the most suitable set of conditions and the reason for its use?

ConditionsReactivity of phenol to electrophiles compared

with benzene

A dilute nitric acid at room temperature more reactive

B concentrated nitric and sulfuric acid at room temperature more reactive

C concentrated nitric and sulfuric acid at 55 °C the same

D dilute nitric acid and dilute sulfuric acid at room temperature less reactive


13 Phenol reacts with excess bromine water to give as the organic product(s)

A

BrOH

and

OH

Br

B

Br

C

BrOH

Br

Br

D


7


14 An organic compound, X, shows the following properties:

Oxidation of compound X produces a substance that reacts with 2,4-dinitrophenylhydrazine to give a yellow precipitate but does not react with Fehling’s or Benedict’s solution.

Compound X reacts with ice-cold nitrous acid to form a compound that gives a yellow precipitate with an alkaline solution of phenol.

What is the formula of compound X?

A

CHO

NH2

B

CH(OH)CH3

NH2

C

CHO

CH3

D

CHOHCH3

CH3


8

*P35302A0828*

15 Which sequence shows the bases in order of decreasing strength?

A C6H5NH2 > CH3NH2 > NH3

B NH3 > CH3NH2 > C6H5NH2

C CH3NH2 > NH3 > C6H5NH2

D NH3 > C6H5NH2 > CH3NH2


16 Bromoethane can be made by heating ethanol under reflux with 50% sulfuric acid and sodium bromide. When the mixture is distilled, the products include sulfur dioxide, bromine, hydrogen bromide and water as well as bromoethane.

The product mixture is shaken with sodium carbonate solution and later with anhydrous sodium sulfate before being re-distilled. Which of the following shows the correct list of impurities removed at each step?

Aqueous sodium carbonate wash

Addition of sodium sulfate

A HBr SO2, Br2, water

B SO2, Br2 HBr, water

C SO2, HBr Br2, water

D SO2, Br2, HBr water


17 A compound is known to have either the structure H2NCH2CH2NH2 or H2NCH2COOH. Which of the following tests would best distinguish between the two compounds?

A Reaction with concentrated aqueous sodium hydroxide.

B Reaction with nitrous acid.

C Reaction with aqueous sodium hydrogencarbonate.

D Reaction with ethanoyl chloride.


9


18 Poly(ethenol) is a water-soluble polymer. A section of the chain has the structure shown below.

The polymer is used for making hospital laundry bags so that laundry can be loaded directly into washing machines without it having to be handled.

Poly(ethenol) is water soluble because the polymer

A is broken down by the water into monomers.

B is broken down by the washing detergent.

C breaks into monomers at the temperature of the wash.

D forms many strong hydrogen bonds with the water.


19 Which of the following substances is capable of damaging the ozone layer?

A NaCl

B CO2

C C2HF5

D C2F3Cl3


20 Analysis suggests that a particular organic synthesis produces a medicine that contains trace impurities that may be hazardous. What is the best way for this discovery to be reported and evaluated?

A In a scientific journal which subjects its articles to peer review.

B On the Internet in an article on a website.

C In a newspaper article in several broadsheet newspapers.

D In a widely circulated magazine.



C C C C

H H H H

H OH H OH

2

*P41212A0224*

SECTION A

Answer ALL the questions in this section. You should aim to spend no more than 20 minutes

on this section. For each question, select one answer from A to D and put a cross in the box .


a cross .

1 When aqueous solutions of barium chloride and potassium sulfate are mixed, a white precipitate forms. The ionic equation for the reaction is

A K+(aq) + Cl− (aq) � KCl(s)

B K2+(aq) + 2Cl− (aq) � KCl2(s)

C Ba+(aq) + SO4− (aq) � BaSO4(s)

D Ba2+(aq) + SO42− (aq) � BaSO4(s)


2 Which of the following processes has the highest atom economy?

A Making poly(ethene) from ethene.

B Making ethene from eicosane, C20H42.

C Making chloromethane from methane.

D Making magnesium chloride from magnesium and hydrochloric acid.


3 How many molecules are present in 16 g of oxygen gas, O2(g)?

[Avogadro constant = 6 × 1023 mol−1]

A 96 × 1023

B 12 × 1023

C 6 × 1023

D 3 × 1023


3


4 Nickel(II) sulfate is prepared by adding an excess of nickel(II) carbonate to 0.010 mol of dilute sulfuric acid.

NiCO3(s) + H2SO4(aq) � NiSO4(aq) + H2O(l) + CO2(g)

Solid nickel(II) sulfate crystals are produced with a 20% yield. How many moles of nickel(II) sulfate crystals are obtained?

A 0.001

B 0.002

C 0.010

D 0.050


5 When 0.635 g of copper (relative atomic mass, RAM = 63.5) is added to an excess of silver nitrate solution, 2.158 g of silver (RAM = 107.9) form. The ionic equation for the reaction is

A Cu(s) + Ag2+(aq) � Cu2+(aq) + Ag(s)

B Cu(s) + Ag+(aq) � Cu+(aq) + Ag(s)

C 2Cu(s) + Ag2+(aq) � 2Cu+(aq) + Ag(s)

D Cu(s) + 2Ag+(aq) � Cu2+(aq) + 2Ag(s)


6 In an experiment to measure the enthalpy change of a reaction involving gases, which of the following conditions must always be kept constant?

A Pressure

B Temperature

C Volume

D Temperature and pressure


4

*P41212A0424*

7 In an endothermic reaction in aqueous solution, which of the following is correct?

Temperature Sign of enthalpy change

A Increases Positive

B Increases Negative

C Decreases Positive

D Decreases Negative


8 The enthalpy change for the reaction to form hydrated sodium thiosulfate crystals cannot be measured directly.

The following Hess cycle can be used.

Na2S2O3(s) + 5H2O(l) � Na2S2O3.5H2O(s)

Na2S2O3 (aq)

The enthalpy change for the reaction, �Hr , is equal to

A �H1 + �H2

B �H1 − �H2

C −�H1 − �H2

D −�H1 + �H2



�Hr

+aq �H1 +aq�H2

5


9 When 10 cm3 of 2 mol dm–3 hydrochloric acid is reacted with 10 cm3 of 2 mol dm–3 sodium hydroxide solution, the temperature change is �T.

HCl(aq) + NaOH(aq) � NaCl(aq) + H2O(l)

When the reaction is repeated with 50 cm3 of each solution, the temperature change is

A �T

B 5 × �T

C 15

× �T

D 10 × 2 × �T


10 An isotope of an element, atomic number z, has mass number 2z + 4. How many neutrons are in the nucleus of the element?

A z + 4

B z + 2

C z

D 4


11 When an Al4+ ion is formed from an Al atom, the fourth electron is lost from the

A 1s sub-shell.

B 2s sub-shell.

C 2p sub-shell.

D 3s sub-shell.



6

*P41212A0624*

12 Metals are good conductors of electricity because

A metal atoms are arranged in a regular lattice.

B metal ions are very close to each other.

C metal ions are free to move through the lattice.

D electrons are free to move through the lattice.


13 Which of the following statements is evidence for the existence of ions in ionic compounds?

A Ionic compounds, in the solid state, conduct electricity.

B When any ionic compound in solution is electrolysed, the migration of ions can be seen.

C In electron density maps for ionic compounds, there is no single line representing electron density that surrounds both cations and anions.

D In electron density maps for ionic compounds, there are some single lines representing electron density that surround both cations and anions.


14 White phosphorus consists of

A a giant structure of atoms.

B a giant structure of ions.

C small molecules.

D single atoms.


15 Isomers have different

A empirical formulae.

B molecular formulae.

C skeletal formulae.

D molar masses.


7


BLANK PAGE

8

*P41212A0824*

16 Four of the reactions of propene are shown on the diagram below.

(a) Nickel is often used as the catalyst for Reaction 1. Use your Periodic Table to select which of the following metals can be used instead of nickel to catalyse Reaction 1.

(1)

A Potassium

B Calcium

C Gallium

D Palladium

(b) The name of the reagent and the product for Reaction 2 are(1)

Reagent Product

A bromine water dibromopropane

B bromine dibromopropane

C bromine water 1,2-dibromopropane

D bromine 1,2-dibromopropane

CH3CH2CH3

CH3CH(OH)CH2OH

Reaction 1 Hydrogen / catalyst

CH3CH CH2

Reaction 4CH3CHBrCH2Br

Reaction 2

Reaction 3 HBr

Compound A

9


(c) What is formed in Reaction 3?(1)

A Only 1-bromopropane

B Only 2-bromopropane

C A mixture of bromopropanes containing mainly 2-bromopropane

D A mixture of bromopropanes containing mainly 1-bromopropane

(d) A mixture of dilute sulfuric acid and which of the following reagents is needed for Reaction 4?

(1)

A KOH

B KMnO4

C H2O2

D O2

(e) The reaction of propene in Reaction 4 can be classified both as (1)

A addition and reduction.

B addition and oxidation.

C free radical substitution and reduction.

D free radical substitution and oxidation.



2

*P41213A0224*

SECTION A




a cross .

1 Which of these bond angles is the largest?

A Cl–B–Cl in BCl3

B H–N–H in NH3

C Cl–Be–Cl in BeCl2

D H–O–H in H2O


2 In propene, CH2=CH–CH3,

A the C=C double bond is longer and stronger than the C–C single bond.

B the C=C double bond is shorter and stronger than the C–C single bond.

C the C=C double bond is shorter and weaker than the C–C single bond.

D the C=C double bond is longer and weaker than the C–C single bond.


3 Which of the following molecules is not polar?

A HCl

B CH3Cl

C CHCl3

D CCl4


4 The O–H bond in water is polar because, compared with the hydrogen atom, the oxygen atom has

A more electrons.

B more neutrons.

C greater electronegativity.

D a larger atomic radius.


3


5 Which of the following compounds has the highest boiling temperature?

A CH4

B CH3Cl

C HCHO

D CH3OH


6 The oxidation number of sulfur in thiosulfate ions, S2O32–, is

A +2

B +3

C +4

D +6


7 Which of the following is a redox reaction?

A Ca + 2H2O � Ca(OH)2 + H2

B MgO + H2O � Mg(OH)2

C NaCl + AgNO3 � AgCl + NaNO3

D Na2CO3 + 2HCl � 2NaCl + CO2 + H2O


8 A solid gives a red colour in a flame test and reacts with concentrated sulfuric acid to produce steamy fumes, but no other gases. The solid could be

A lithium bromide.

B strontium chloride.

C calcium bromide.

D sodium chloride.


4

*P41213A0424*

9 Which of the following statements is correct?

A Barium sulfate is less soluble in water than calcium sulfate.

B Barium hydroxide is less soluble in water than calcium hydroxide.

C Barium nitrate undergoes thermal decomposition more readily than calcium nitrate.

D Barium shows more than one oxidation state in its compounds.


10 Going down Group 7 from chlorine to iodine

A the boiling temperature of the hydrogen halide decreases.

B the polarity of the hydrogen halide bond increases.

C the reducing power of the halide ion increases.

D the oxidizing power of the halogen element increases.


11 What colour is the vapour which forms when concentrated sulfuric acid is added to solid potassium iodide?

A Green

B Orange

C Brown

D Purple


12 Calculate the volume of dilute hydrochloric acid, concentration 0.200 mol dm–3, needed to neutralize 20 cm3 of aqueous calcium hydroxide, concentration 0.100 mol dm–3.

2HCl(aq) + Ca(OH)2(aq) � CaCl2(aq) + 2H2O(l)

A 10 cm3

B 20 cm3

C 40 cm3

D 80 cm3


5


13 The reaction of heated magnesium with steam is faster than the reaction of magnesium with cold water. This is mainly because

A in cold water, the water molecules do not collide as frequently with magnesium.

B the coating of oxide on magnesium decomposes when it is heated.

C the fraction of particles with energy greater than the activation energy is higher in the reaction with steam.

D the reaction with steam goes by an alternative route with lower activation energy.


14 Which of these compounds would not react when heated with a mixture of potassium dichromate(VI) and sulfuric acid?

A CH3OH

B CH3(CH2)2OH

C (CH3)2CHOH

D (CH3)3COH



6

*P41213A0624*

15 Under certain conditions, butan-1-ol can be oxidized to the compound with infrared spectrum shown below.

O–H stretching vibrations alcohols 3750 – 3200 cm–1

O–H stretching vibrations carboxylic acids 3300 – 2500 cm–1

C=O stretching vibrations aldehydes and ketones 1740 – 1680 cm–1

C=O stretching vibrations carboxylic acids 1725 – 1700 cm–1

The compound is most likely to be

A butan-2-ol.

B butanal.

C butanone.

D butanoic acid.


16 Which of the following is a secondary alcohol?

A 2-methylpentan-3-ol

B 2-methylpropan-2-ol

C 2,2-dimethylpropan-1-ol

D ethane-1,2-diol


Wavenumber / cm–1

Transmittance / %

3000 2000 1000

80

60

40

20

0

7


17 Propanal, CH3CH2CHO, and propanone, CH3COCH3, are isomers, but only propanal has a significant peak in its mass spectrum at mass/charge ratio

A 15

B 29

C 43

D 58


18 The reaction of the halogenoalkane, C2H5Cl, with alcoholic ammonia is


B electrophilic substitution.

C reduction.

D elimination.


19 The formation of a carbocation from a halogenoalkane is an example of

A homolytic fission.

B heterolytic fission.

C an initiation reaction.

D a propagation reaction.


20 The equations below show some reactions which occur in the upper atmosphere.

O3 � O + O2 NO + O3 � NO2 + O2 NO2 + O � NO + O2

Which of the following statements is not correct?

A Oxygen free radicals are formed by the action of ultraviolet light.

B NO acts as a catalyst.

C NO acts as an oxidizing agent.

D NO is released by aircraft engines.



2

*P41214A0228*

SECTION A




a cross .

1 Methods for investigating reaction rates include

A colorimetry

B collecting and measuring the volume of a gas

C quenching, followed by titration with acid

D quenching, followed by titration with iodine solution.

Which method would be most suitable to investigate the rate of the following reactions?

(a) H2O2(aq) + 2I�(aq) + 2H+(aq) � 2H2O(l) + I2(aq)(1)

� �A

� �B

� �C

� �D

(b) C4H9Br(l) + OH−(aq) � C4H9OH(l) + Br−(aq)(1)

� �A

� �B

� �C

� �D



3


2 For a given initial reactant pressure, the half-life for a first order gaseous reaction was found to be 30 minutes.

If the experiment were repeated at half the initial reactant pressure, the half-life would be

� A 15 minutes.

� B 30 minutes.

� C 45 minutes.

� D 60 minutes.


3 To determine the activation energy (Ea) for a reaction, the variation of reaction rate with temperature is investigated.

The rate constant, k, for the reaction is related to the absolute temperature, T, by the expression

In T

constantakER

= − × ⎛⎝⎜

⎞⎠⎟

+1

where R is the gas constant.

The activation energy for the reaction could be obtained by plotting a graph of

vertical axis horizontal axis

� A k T

� B k 1T

� C ln k T

� D ln k 1T



4

*P41214A0428*

4 Energy is evolved when one mole of gaseous calcium ions is hydrated.

Ca2+(g) + aq � Ca2+(aq)

This reaction is more exothermic than the corresponding value for barium ions, Ba2+, because the

� A ionization energy of calcium is greater than that of barium.

� B lattice energy of calcium oxide is more exothermic than that of barium oxide.

� C solubility of calcium hydroxide in water is less than that of barium hydroxide.

� D ionic radius of Ca2+ is less than that of Ba2+.


5 The following cycle represents the enthalpy changes w, x, y and z, occurring when an ionic solute, AX2(s), dissolves in water.

Which of the changes is the lattice energy of AX2(s)?

� �A ½ w

� �B − w

� �C z

� �D z − x − y


A2+(g) + 2X–(g)

A2+(aq) + 2X–(aq)

AX2(s)

w

z

x + y

5


6 The equation for the synthesis of methanol is

CO(g) + 2H2(g) � CH3OH(g)

At equilibrium, when the temperature is 340 K, the total pressure is 20 atm. The moles of each component present at equilibrium are shown in the table below.

Formula Equilibrium moles / mol Mole fraction

CO 0.15 0.23

H2 0.32

CH3OH 0.18 0.28

(a) The mole fraction of hydrogen in the equilibrium mixture is(1)

� A 0.23

� B 0.46

� C 0.49

� D 0.92

(b) The numerical value for the equilibrium partial pressure of the carbon monoxide, in atmospheres, is

(1)

� A 3.0

� B 4.6

� C 5.0

� D 9.2

(c) Units for the equilibrium constant, Kp, for this reaction are(1)

� A no units

� B atm

� C atm−1

� D atm−2


6

*P41214A0628*

7 An aqueous solution of ammonium chloride, NH4Cl, has a pH of less than 7 because

� A the ammonium ions donate protons to water molecules giving rise to oxonium ions, H3O+(aq).

� B the chloride ions combine with hydrogen ions from water to form hydrochloric acid, HCl(aq).

� C an aqueous solution of ammonium chloride is unstable and evolves ammonia gas, NH3(g), leaving dilute hydrochloric acid.

� D the ammonium chloride reacts with carbon dioxide from the atmosphere giving ammonium carbonate, (NH4)2CO3(aq), and hydrochloric acid, HCl(aq).


8 Which one of the following indicators is most suitable for titrating ethanoic acid with 0.1 mol dm�3 sodium hydroxide?

(Refer to page 19 of your data booklet.)

� A Thymol blue (acid)

� B Bromothymol blue

� C Thymol blue (base)

� D Alizarin yellow R


9 What is the conjugate base of the acid, HCO3−?

� A H2CO3

� B CO32−

� C OH−

� D CO2



7


10 What is the approximate pH of a buffer solution containing 0.20 mol of a weak acid, HA, (pKa = 4.8) and 0.20 mol of the sodium salt of the acid, NaA, in a total volume of 1 dm3 of solution?

� A 7.0

� B 5.8

� C 4.8

� D 3.8


11 Ethanal, CH3CHO, can be converted by a two-step synthesis into 2-hydroxypropanoic acid.

C C

H

OOH

O H

H3C

2-hydroxypropanoic acid

The reagents and conditions are

1st step 2nd step

� A Na2Cr2O7 and dilute H2SO4, NaOH(aq), heat under reflux heat under reflux

� B Cl2, UV light NaOH(aq), heat under reflux

� C LiAlH4 in dry ether CO2, room temperature

� D HCN, in presence of KCN(aq) dilute HCl(aq), heat under reflux



8

*P41214A0828*

12 Questions (a) to (d) concern the following organic compounds.

Compound A H3C C C OH

CH3

CH3

H

CH2CH3

Compound B H3C C C O

CH3H

H

Compound C H3C C C O

CH3 H

H

Compound D H3C C C O CH3

CH3 O

H

9


Select from A to D the compound that

(a) forms iodoform with iodine in the presence of alkali.(1)

� A

� B

� C

� D

(b) is chiral.(1)

� A

� B

� C

� D

(c) reacts with Tollens’ reagent.(1)

� A

� B

� C

� D

(d) can be oxidized to form a ketone.(1)

� A

� B

� C

� D


10

*P41214A01028*

13 Ethanoic acid, CH3COOH, can be converted into ethanoyl chloride, CH3COCl, by the action of

� A phosphorus(V) chloride.

� B chlorine.

� C dilute hydrochloric acid.

� D concentrated hydrochloric acid.


14 A compound, Q, gives an orange precipitate with 2,4-dinitrophenylhydrazine. Compound Q is resistant to oxidation.

On reduction, Q gives a product made up of a pair of optical isomers.

Which of the following compounds could be compound Q?

� A CH3CH2CH2COCH3

� B CH3CH CHCH(OH)CH3

� C CH3CH2CH2CH2CHO

� D CH3CH2COCH2CH3



2

*P41215A0224*

SECTION A



If you change your mind, put a line through the box and then mark your new answer with a

cross .

1 The reaction between iron and nickel(II) sulfate may be represented by the ionic equation

Ni2+(aq) + Fe(s) � Ni(s) + Fe2+(aq)

(a) This reaction is classified as a redox reaction because(1)

A the nickel(II) ions are oxidized and iron acts as an oxidizing agent.

B the nickel(II) ions are oxidized and iron acts as a reducing agent.

C the nickel(II) ions are reduced and iron acts as a reducing agent.

D the nickel(II) ions are reduced and iron acts as an oxidizing agent.

(b) This reaction proceeds spontaneously, therefore (1)

A Ecell and �Stotal for this reaction must both be positive.

B Ecell and �Stotal for this reaction must both be negative.

C Ecell for this reaction must be positive and �Stotal negative.

D Ecell for this reaction must be negative and �Stotal positive.



3


2 The diagram below shows an electrochemical cell.

(a) The salt bridge in this cell is best prepared by soaking filter paper in a(1)

A 1 mol dm−3 solution of potassium bromide.

B 1 mol dm−3 solution of potassium chloride.

C saturated solution of potassium nitrate.

D saturated solution of potassium iodide.

(b) The relevant standard electrode potentials for this cell are shown below.

Cr3+(aq) + 3e− � Cr(s) E � = −0.74 V

Ag+(aq) + e− � Ag(s) E � = +0.80 V

The emf of the cell shown in the diagram is(1)

A +1.54 V

B −1.54 V

C +0.06 V

D −0.06 V

(c) The mass of 1 mol of chromium(III) sulfate (Cr2(SO4)3) is 392 g. Hence, for the cell in the diagram to measure the standard electrode potential, 1 dm3 of the chromium(III) sulfate solution used must contain

(1)

A 104 g of chromium(III) sulfate.

B 196 g of chromium(III) sulfate.

C 392 g of chromium(III) sulfate.

D 784 g of chromium(III) sulfate.


chromium strip

silver nitrate solution

silver strip

V salt bridge

chromium(III) sulfate solution

4

*P41215A0424*

3 Vanadium is classified as a transition metal. This is because vanadium

A is a d-block element.

B has incompletely filled d orbitals.

C forms stable ions with incompletely filled d orbitals.

D forms stable ions in which it has different oxidation states.


4 Copper(II) sulfate solution is blue. This is because

A excited electrons emit light in the blue region of the spectrum as they drop back to the ground state.

B excited electrons emit light in the red region of the spectrum as they drop back to the ground state.

C electrons absorb light in the red region of the spectrum and the residual frequencies are observed.

D electrons absorb light in the blue region of the spectrum and the residual frequencies are observed.


5 One method of manufacturing hydrazine (N2H4) involves the action of sodium chlorate(I) on excess ammonia at 443 K and 50 atm. The yield is normally around 80% but, if just 1 part per million of copper(II) ions is present, the yield drops to 30%.

The most likely explanation for this is the ability of copper(II) ions to

A form complex ions with ammonia.

B catalyse reactions producing other nitrogen compounds.

C reduce the hydrazine as it is formed.

D reduce the sodium chlorate(I).



5


6 Platinum forms a complex with the formula Pt(NH3)2Cl2 and chromium forms a complex ion with the formula CrCl4

−.

(a) Considering the shapes of these complexes,(1)

A both complexes are square planar.

B both complexes are tetrahedral.

C Pt(NH3)2Cl2 is tetrahedral and CrCl4− is square planar.

D Pt(NH3)2Cl2 is square planar and CrCl4− is tetrahedral.

(b) Considering the structures of these complexes,(1)

A both complexes form stereoisomers.

B neither complex forms a stereoisomer.

C Pt(NH3)2Cl2 forms a stereoisomer but CrCl4− does not.

D CrCl4− forms a stereoisomer but Pt(NH3)2Cl2 does not.

(c) Considering the bonding between the central atom and the ligands in these complexes,

(1)

A the bonding in both complexes is dative covalent.

B the bonding in both complexes is ionic.

C the bonding in Pt(NH3)2Cl2 is dative covalent and in CrCl4− is ionic.

D the bonding in Pt(NH3)2Cl2 is ionic and in CrCl4− is dative covalent.



6

*P41215A0624*

7 When concentrated ammonia solution is added to a green solution of chromium(III) sulfate, a green precipitate is formed which slowly dissolves in excess of the concentrated ammonia solution.

The chromium-containing species formed in these reactions are

Green precipitate Resulting solution

A Cr(OH)3 [Cr(OH)6]3−

B Cr(OH)3 [Cr(NH3)6]3+

C (NH4)2CrO4 [Cr(OH)6]3−

D (NH4)2CrO4 [Cr(NH3)6]3+


8 Bromine reacts much faster with phenylamine than with benzene. This is because

A N H bonds are weaker than C H bonds.

B nitrogen is very electronegative.

C the benzene ring has greater electron density in phenylamine than in benzene.

D phenylamine reacts by addition whereas benzene reacts by substitution.


9 X-ray diffraction provides evidence that benzene molecules have

A delocalized � electrons.

B carbon−carbon bonds that are all the same length.

C lower thermodynamic stability than molecules of 1,3,5-cyclohexatriene.

D greater thermodynamic stability than molecules of 1,3,5-cyclohexatriene.


7


10 Benzene is nitrated using a mixture of concentrated nitric and sulfuric acids. The sulfuric acid

A acts as a solvent for the benzene and the nitric acid.

B protonates the benzene to speed up the reaction.

C protonates the nitric acid which acts as a base.

D reacts with the benzene to form a benzenesulfonic acid intermediate.


11 The compound shown below is found in cocoa beans and in chocolate. Which of the groups listed is not present in its structure?

A Alkyl

B Amide

C Amine

D Ketone


12 The distinguishing characteristic of combinatorial chemistry is that it involves the

A simultaneous synthesis of many products.

B interaction of starting materials to form a unique product.

C use of catalysts.

D use of polymer supports.



C

O

N

H

C

ON

CH3

N

N

CH3

8

*P41215A0824*

13 Phenylamine (aniline), C6H5NH2, may be prepared from nitrobenzene, C6H5NO2.

(a) The reagent normally used for this reaction is(1)

A lithium tetrahydridoaluminate(III) (lithium aluminium hydride) in ether.

B concentrated ammonia in ethanol.

C potassium dichromate(VI) in sulfuric acid.

D tin in concentrated hydrochloric acid.

(b) The phenylamine is separated from the reaction mixture by(1)

A paper chromatography.

B steam distillation.

C filtration.

D recrystallization.

(c) One test for phenylamine is to convert it into a diazonium ion which is then reacted with phenol to form an azo dye. The structure of this dye is

(1)

A N N OH

B N N NH2

C N OH

H

D N

H

NH2



2

*H34471A0228*

SECTION A



1 The nucleus of a 2311

Na atom contains

A 11 protons and 12 neutrons.

B 11 protons and 12 electrons.

C 23 protons and 11 neutrons.

D 23 protons and 11 electrons.


2 The mass spectrum for a sample of a metal is shown below.

The relative atomic mass of the metal is

A 63.2

B 63.4

C 63.6

D 64.0


relative abundance

70

30

6563

mass/charge ratio

3

*H34471A0328* Turn over

3 Some mean bond enthalpy values are given in the table below.

Bond Mean bond enthalpy / kJ mol–1

H H +436

I I +151

H I +299

What is the enthalpy change for the reaction shown below in kJ mol–1?

H2(g) + I2(g) → 2HI(g)

A +436 + 151 – 299 = +288

B –436 – 151 + 299 = –288

C +436 +151 – (2 × 299) = –11

D –436 – 151 + (2 × 299) = +11


4 A compound was analysed and found to contain

1.45 g carbon 0.482 g hydrogen 1.69 g nitrogen

[Relative atomic masses: C = 12; H = 1; N = 14]

The empirical formula of the compound is

A CH3N

B CH4N

C CH5N

D C2H4N


4

*H34471A0428*

5 17.1 g of aluminium sulfate, Al2(SO4)3, was dissolved in water.

Calculate the number of sulfate ions, SO42–, present in the solution formed.

[Assume the molar mass of Al2(SO4)3 is 342 g mol–1 and the Avogadro Constant is 6 × 1023 mol–1.]

A 3 × 1021

B 1 × 1022

C 3 × 1022

D 9 × 1022


6 Calculate the mass of calcium hydroxide, Ca(OH)2, present in 100 cm3 of a 0.100 mol dm–3 solution.

[Assume the molar mass of Ca(OH)2 is 74.0 g mol–1.]

A 0.570 g

B 0.740 g

C 1.85 g

D 3.70 g



5


7 The first five successive ionization energies of an element, X, are shown in the table below.

Ionization energy first second third fourth fifth

Value/ kJ mol–1 590 1100 4900 6500 8100

Which ion is X most likely to form when it reacts with chlorine?

A X+

B X2+

C X3+

D X4+


8 Which of the following alkenes exhibits E-Z isomerism?

A H3CCH=C(CH3)2

B (CH3)2C=CH2

C H2C=CHCH2CH3

D H3CCH=CHCH3


9 Which of the following covalent bonds is the shortest?

A H F

B H Cl

C H Br

D H I


6

*H34471A0628*

10 Which of the following substances, obtained from the fractional distillation of crude oil, has the lowest boiling temperature?

A refinery gas

B kerosene

C diesel oil

D lubricating oil


11 Sodium hydrogensulfate, NaHSO4, reacts with sodium hydroxide, NaOH, as shown below.

NaHSO4(aq) + NaOH(aq) → Na2SO4(aq) + H2O(l)

0.0100 mol of sodium hydrogensulfate is neutralized with dilute sodium hydroxide, concentration 0.200 mol dm–3.

Calculate the volume of sodium hydroxide required.

A 20.0 cm3

B 50.0 cm3

C 100 cm3

D 500 cm3


12 Which of the following ions would undergo the greatest deflection in amass spectrometer?

A 35Cl2+

B 35Cl+

C 37Cl+

D 35Cl37Cl+


7


13 Which pair of atomic numbers represents elements which are both in the p-block of the Periodic Table?

A 4, 8

B 6, 12

C 8, 16

D 10, 20


14 The electronic structure of an atom of an element in Group 6 of the Periodic Table could be

A 1s2 2s2 2p2

B 1s2 2s2 2p4

C 1s2 2s2 2p6 3s2 3p6 3d6 4s2

D 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6


15 Which of the following formulae for compounds of germanium, Ge, is unlikely to be correct, given the position of germanium in the Periodic Table?

A GeF3

B GeS2

C GeO2

D GeH4



8

*H34471A0828*

16 The electronic configurations of the atoms of four different elements are given below. For which element would you expect the value of the first ionization energy to be the largest?

A 1s1

B 1s2

C 1s2 2s1

D 1s2 2s2


17 Which of the following gas samples occupies the greatest volume at the same temperature and pressure?

[Relative atomic masses: H = 1; C = 12; O = 16; F = 19; Ne = 20]

A 1 gram of ethane

B 1 gram of oxygen

C 1 gram of fluorine

D 1 gram of neon


18 Which of the following has the smallest ionic radius?

A F–

B Na+

C Mg2+

D O2–



9


19 Which of the following does not have exactly 10 electrons?

A An ion of fluorine, F–

B A molecule of methane, CH4

C A molecule of nitrogen, N2

D An ion of sodium, Na+


20 Which of the following statements correctly describes an environmental problem caused by the burning of hydrocarbon fuels?

A The carbon dioxide is toxic and kills plants.

B The smoke produced reflects sunlight and leads to global warming.

C The water produced results in a damaging increase in rainfall.

D The carbon dioxide produced absorbs heat radiated from the Earth and leads to global warming.




2

*h34472A0224*

SECTION A



1 What is the oxidation number of chlorine in the ClO3– ion?

A –1

B +4

C +5

D +6


2 Which of these reactions is not a redox reaction?

A Mg(NO3)2(s) → MgO(s) + 2NO2(g) + ½O2(g)

B HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)

C Fe(s) + CuSO4(aq) → FeSO4(aq) + Cu(s)

D Cl2(aq) + 2Br–(aq) → 2Cl–(aq) + Br2(aq)



3

*h34472A0324* Turn over

3 Which of these carbon structures is represented by the diagram below?

A Graphite

B Diamond

C A fullerene

D A carbon nanotube


4 What colour precipitate would you expect to see if 1-bromopropane was heated with a solution of silver nitrate?

A Orange

B White

C Yellow

D Cream


5 Which of these bond angles is the smallest?

A HNH in NH3

B HCH in CH4

C HOH in H2O

D OCO in CO2


4

*h34472A0424*

6 Which statement best describes the shape and bond angles in the molecule SF6?

A Octahedral, 90° and 180°

B Trigonal bipyramidal, 90° and 180°

C Octahedral, 90° and 120°

D Trigonal bipyramidal, 90° and 120°


7 Which of the following values for the mass/charge ratio for singly charged ions would be present in the mass spectrum of propanal, CH3CH2CHO, but not of propanone, CH3COCH3?

A 15

B 29

C 43

D 58



5


8 The infrared spectrum below is most likely to be that of a member of which homologous series?

C Cl stretching vibrations 600 – 800 cm–1

O H stretching vibrations 2500 – 3300 cm–1

C O stretching vibrations 1680 – 1740 cm–1

A Alcohol

B Chloroalkane

C Aldehyde

D Carboxylic acid



Transmittance / %

4000 3000 2000 1500 1000 500

100

50

0

Wavenumber / cm–1

6

*h34472A0624*

9 In the reaction profile below, which energy change would alter if a catalyst was added to the reaction?

A

B

C

D



B

Reaction co-ordinate

D

CA

Products

Reactants

Energy

7


10 In the equilibrium below, what effect would the changes described have on the system?

2H2S(g) + SO2(g) 3S(s) + 2H2O(g) ∆H is negative

(a) Increase in temperature(1)

A increase rate, decrease yield

B increase rate, increase yield

C decrease rate, decrease yield

D decrease rate, increase yield

(b) Decrease in pressure(1)

A increase rate, decrease yield

B increase rate, increase yield

C decrease rate, decrease yield

D decrease rate, increase yield



8

*h34472A0824*

11 What is the correct systematic name for the alcohol shown below?

A hexan-4-ol

B hexan-2-ol

C pentan-4-ol

D pentan-2-ol


12 Which of these compounds is a secondary halogenoalkane?

A CH3CH(OH)CH3

B CH3CCl(CH3)CH3

C CH3CHClCH3

D CH3CH2CH2Cl


13 The bonding in gaseous hydrogen halides is best described as

A mainly covalent with an increasing tendency towards ionic as you go down the group.

B mainly covalent with an increasing tendency towards ionic as you go up the group.

C mainly ionic with an increasing tendency towards covalent as you go down the group.

D mainly ionic with an increasing tendency towards covalent as you go up the group.


OH

9


14 What would be the colour of the solution when iodine is dissolved in a hydrocarbon solvent?

A Grey

B Brown

C Yellow

D Purple


15 Starch is often used as an indicator in titrations between sodium thiosulfate and iodine solutions. What colour change would you see at the end-point as sodium thiosulfate is added to iodine solution in the presence of starch?

A Yellow to colourless

B Colourless to yellow

C Blue-black to colourless

D Colourless to blue-black


16 An electric field can affect the direction of a stream of some liquids. Which of these liquids would be affected by an electric field?

A 1-chloropropane

B Pentane

C Tetrachloromethane

D Cyclopentane



10

*h34472A01024*

17 Which of these isomers has the highest boiling temperature?

A

B

C

D


18 Which of the following statements is true?

A Calcium hydroxide is more soluble in water than magnesium hydroxide.

B Chlorine is more electronegative than fluorine.

C Iodine is a stronger oxidizing agent than bromine.

D The first ionization energy of barium is greater than that of strontium.


19 Iodine can react with sodium hydroxide solution to form NaIO3(aq), according to the equation below.

3I2(aq) + 6NaOH(aq) → 5NaI(aq) + NaIO3(aq) + 3H2O(l)

Which of the statements about the reaction is false?

A The oxidation number of some iodine atoms goes up.

B At high temperatures NaIO(aq) also forms.

C Sodium ions are spectator ions.

D The oxidation number of some iodine atoms goes down.



2

*N35691A0228*

BLANK PAGE

3


SECTION A



1 The equations below show some reactions of magnesium and its compounds.

A 2Mg(s) + O2(g) → 2MgO(s)

B Mg(NO3)2(s) → MgO(s) + 2NO2(g) + O2(g)

C MgO(s) + 2HCl(aq) → MgCl2(aq) + H2O(1)

D Mg(s) + CuSO4(aq) → MgSO4(aq) + Cu(s)

(a) Which equation is not balanced?(1)

A

B

C

D

(b) Which equation can be classified as a displacement reaction?(1)

A

B

C

D


2 Which of these equations represents the electron affinity of chlorine?

A Cl2(g) + 2e− → 2Cl−(g)

B Cl2(g) − 2e− → 2Cl−(g)

C ½Cl2(g) + e− → Cl−(g)

D Cl(g) + e− → Cl−(g)


4

*N35691A0428*

3 Which of these equations represents the second ionization of magnesium?

A Mg+(g) → Mg2+(g) + e−

B Mg(g) → Mg2+(g) + 2e−

C Mg+(g) + e− → Mg2+(g)

D Mg(g) + 2e− → Mg2+(g)


4 The sketch graph below shows the trend in first ionization energies for some elements in Periods two and three.

Select, from the elements A to D, the one that

(a) has atoms with five p electrons.(1)

A

B

C

D

Ionization energy / kJ mol–1

2500

2000

1500

1000

500

0

Atomic number

A

C

D

B

5


(b) is a member of Group 3.(1)

A

B

C

D

(c) is likely to be very unreactive.(1)

A

B

C

D

(d) normally forms four covalent bonds per atom.(1)

A

B

C

D


5 Which of these ions has the greatest ability to polarize an anion?

A Ba2+

B Ca2+

C Cs+

D K+


6

*N35691A0628*

6 Which of these electron density maps best represents the bonding in the compound lithium iodide, LiI?

A

–+

B

–+

C

–

+

D

δ–

δ+


7 Which of these statements is incorrect?

A The atomic radius of metals increases down a Group.

B The trend in the melting temperature of successive elements across Period 2 is similar to that in Period 3.

C A metallic structure is held together by attractions between metal atoms and delocalized electrons.

D Na+ and O2− ions are isoelectronic.


8 A sample of gas was prepared for use in helium-neon lasers. It contained 4 g of helium and 4 g of neon. What is the ratio of helium atoms to neon atoms in the sample?

A 1 : 1

B 2.5 : 1

C 1 : 5

D 5 : 1


7


9 The overall equation for the reaction between sulfur and oxygen to form sulfur trioxide is shown below.

2S(s) + 3O2(g) → 2SO3(g)

0.9 mol of O2(g) reacted completely with excess sulfur. What volume, in dm3, ofsulfur trioxide would form?

[Assume the molar gas volume = 24 dm3 mol−1]

A (0.9 × 3/2) × 24

B (0.9 × 3/2) ÷ 24

C (0.9 × 2/3) × 24

D (0.9 × 2/3) ÷ 24


10 Which of these solutions does not contain the same total number of ions as the others?

A 10.00 cm3 of 0.100 mol dm−3 NaCl(aq)

B 20.00 cm3 of 0.050 mol dm−3 NaCl(aq)

C 20.00 cm3 of 0.050 mol dm−3 MgCl2(aq)

D 13.33 cm3 of 0.050 mol dm−3 MgCl2(aq)



8

*N35691A0828*

11 Which of these diagrams correctly represents an endothermic reaction?


12 Which of these statements about carbon-carbon double bonds is false?

A The two ends of a molecule cannot rotate relative to each other, about the axis of the double bond.

B They are twice as strong as a carbon-carbon single bond.

C They have a higher electron density than a single bond.

D They consist of a sigma bond and a pi bond.



Reactants

Products

Enthalpy

ΔH –ve

Reactants

Products

Enthalpy

ΔH +ve

Reactants

ProductsEnthalpy

ΔH –ve

Reactants

ProductsEnthalpy

ΔH +ve

A

D

B

C

9


13 What is the correct name for the compound below?

A E-2,3-dibromopent-2-ene

B E-2,3-dibromopent-3-ene

C Z-2,3-dibromopent-3-ene

D Z-2,3-dibromopent-2-ene



Br Br

10

*N35691A01028*

14 The equations below show some of the processes that occur when methane and chlorine react.

A Cl2(g) → 2Cl•(g)

B Cl•(g) + CH4(g) → CH3•(g) + HCl(g)

C CH3•(g) + CH3•(g) → C2H6(g)

D Cl2(g) + CH4(g) → CH3Cl(g) + HCl(g)

(a) Which equation shows a propagation step?(1)

A

B

C

D

(b) Which equation shows an initiation step?(1)

A

B

C

D

(c) Which equation shows a termination step?(1)

A

B

C

D



2

*N36390A0224*

SECTION A



1 This question is about bond angles.

A 90°

B 104°

C 107°

D 109.5°

Select, from A to D above, the most likely value for the bond angle of

(a) HCH in methane, CH4.(1)

A

B

C

D

(b) FSF in sulfur hexafluoride, SF6.(1)

A

B

C

D

(c) FOF in oxygen difluoride, OF2.(1)

A

B

C

D


3


2 Consider the following compounds, P, Q, R and S.

CH3CH2CH2CH3

Compound P Compound Q

CH3CH2CH2CH2Br

Compound R Compound S

The boiling temperatures of compounds P, Q, R and S increase in the order

A P Q R S

B R S P Q

C Q S P R

D Q P S R



CH3

H3C C CH3

H

CH3

H3C C Br

CH3

4

*N36390A0424*

3 Buckminsterfullerene has the formula C60. Its structure is shown below.

The bonding in buckminsterfullerene is similar to the bonding in graphite.

Which of the following is true?

A All the bond angles in buckminsterfullerene are 120°.

B The melting temperature of buckminsterfullerene is higher than that of graphite.

C There are delocalized electrons in buckminsterfullerene.

D On complete combustion, buckminsterfullerene forms carbon dioxide and water.


4 When concentrated sulfuric acid is added to solid sodium bromide, bromine is produced.

When concentrated sulfuric acid is added to solid sodium chloride, no chlorine is produced.

The reason for this difference is

A sulfuric acid is a strong acid.

B hydrogen chloride is a weak acid.

C the chloride ion is a weaker reducing agent than the bromide ion.

D bromine is less volatile than chlorine.



5


5 Compound X is a white solid. On heating this compound, a colourless, acidic gas is the only gaseous product. A flame test is carried out on the solid residue and a reddish flame is observed.

Compound X is

A calcium nitrate.

B calcium carbonate.

C magnesium carbonate.

D strontium nitrate.


6 Which of the following does not apply to the elements Mg, Ca, Sr and Ba in Group 2 of the Periodic Table?

A Their oxides, MO, are all basic.

B Their metal hydroxides, M(OH)2, become more soluble down the group.

C Their oxides, MO, react with water to form the metal hydroxide, M(OH)2.

D Their carbonates, MCO3, all decompose on gentle heating.


7 Which of the following compounds shows hydrogen bonding in the liquid state?

A Hydrogen bromide, HBr

B Hydrogen sulfide, H2S

C Silane, SiH4

D Ammonia, NH3



6

*N36390A0624*

8 For the reversible reaction

X Y

which of the following could represent the change in the concentrations of X and Y with time, starting with a mixture of both X and Y? Equilibrium is reached at time teqm.


9 Which of the following molecules is polar?


B Beryllium chloride, BeCl2

C Ammonia, NH3

D Boron trifluoride, BF3



Concentration

X

Y

teqm

Time

Concentration

X

Y

teqm

Time

Concentration

X

Y

teqm

Time

A

C

B

Concentration

X

Y

teqm

Time

D

7


10 The electronegativities of four pairs of elements are given below. Which pair would form the compound with the greatest ionic character?

A 0.7 and 4.0

B 0.7 and 3.5

C 1.0 and 4.0

D 0.8 and 2.8


11 Which of the following statements about the elements in Group 7 is incorrect?

A They all show variable oxidation states in their compounds.

B They all form acidic hydrides.

C Electronegativity decreases as the group is descended.

D They all exist as diatomic molecules.


12 What are the products, other than water, when chlorine is passed through cold, dilute aqueous sodium hydroxide solution?

A NaCl and NaClO

B NaClO and NaClO3

C NaCl and NaClO3

D NaClO and NaClO4



8

*N36390A0824*

13 When solutions of iodine are titrated with aqueous sodium thiosulfate solution, Na2S2O3(aq), the thiosulfate ions are oxidized to

A S2O42–

B S2O62–

C S2O82–

D S4O62–


14 The best method of converting ethanol, C2H5OH, into iodoethane, C2H5I, is to

A heat iodine and ethanol under reflux.

B react ethanol and potassium iodide in the presence of dilute acid.

C heat potassium iodide and ethanol with concentrated sulfuric acid.

D heat red phosphorus, ethanol and iodine under reflux.


15 The use of poly(ethene) packaging has been criticised mainly because

A the complete combustion of poly(ethene) produces dangerous fumes.

B large amounts of oil are consumed in producing the monomer, ethene.

C poly(ethene) degrades to form toxic products.

D the catalyst used in the polymerization of ethene is expensive.


16 Which of the following is essential if a species is to act as a nucleophile?

A A lone pair of electrons.

B A negative charge.

C An unpaired electron.

D A strongly polar bond.


9


17 Calculate the volume of dilute sulfuric acid, concentration 0.500 mol dm–3, required to neutralize 20.0 cm3 aqueous sodium hydroxide, concentration 0.100 mol dm–3.

H2SO4 + 2NaOH → Na2SO4 + 2H2O

A 2.0 cm3

B 4.0 cm3

C 8.0 cm3

D 20.0 cm3


18 Which of the following features is shown by the mass spectra of propanone and propanal?

propanone propanal

m/e of the molecular ion Fragmentation pattern

A same same

B same different

C different same

D different different



O

CH3CCH3

OCH3CH2C

H

2

*N36506A0224*

SECTION A



1 Propanone reacts with iodine in acidic solution as shown in the equation below.

CH3COCH3(aq) + I2(aq) → CH3COCH2I(aq) + H+(aq) + I–(aq)

The rate equation for the reaction is

Rate = k[CH3COCH3(aq)][H+(aq)]

(a) The most appropriate technique to investigate the rate of this reaction is(1)

A titrating samples of reaction mixture with acid.

B measurement of optical activity.

C measurement of the volume of gas given off.

D colorimetry.

(b) Which statement about the reaction is not correct?(1)

A The overall order of reaction is second order.

B The units of the rate constant are dm3 mol–1 s–1.

C The rate constant increases with temperature.

D The rate increases four times when the concentration of propanone and iodine are both doubled.

3


(c) The reaction is carried out using a large excess of both propanone and acid. Which of the graphs below shows the change of iodine concentration with time?

(1)


2 Which of the following is true for the exothermic reaction shown below?

Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)

A ∆H positive

B ∆Ssurroundings positive

C ∆Ssystem negative

D ∆Stotal negative



[I2]

time

[I2]

time

[I2]

time

[I2]

time

A

C

B

D

4

*N36506A0424*

3 In which reaction is water acting as a Brønsted-Lowry acid?

A H2O + HCl → H3O+ + Cl–

B H2O + SO3 → H2SO4

C H2O + NH3 → NH4+ + OH–

D H2O + CO2 → H2CO3


4 Which of the following compounds has both optical and E-Z isomers?

A CH3CH=CHCH2CH3

B CH3CHClCH=C(CH3)2

C CH3CCl=CClCH3

D CH3CHBrCH=CHCl


5 Which of the following reacts with hydrogen cyanide, HCN, to make a racemic mixture?

A Methanal, HCHO

B Ethanal, CH3CHO

C Propanone, CH3COCH3

D Pentan-3-one, C2H5COC2H5



A Ethanal reacting with Tollens’ reagent.

B Ethanoyl chloride reacting with ammonia.

C Ethanoic acid reacting with ethanol.

D Ethanoic acid reacting with sodium hydroxide.



5


7 The following methods can be used to distinguish between pairs of organic compounds without further tests.

A Warm each compound with Fehling’s or Benedict’s solution.

B Add solid sodium carbonate to each compound.

C Add 2,4-dinitrophenylhydrazine (Brady’s reagent) to each compound.

D Add water, drop by drop, to each compound.

(a) Which test would distinguish propanone from propan-1-ol?(1)

A

B

C

D

(b) Which test would distinguish between aqueous solutions of ethanoic acid and ethanol?(1)

A

B

C

D

(c) Which test would distinguish ethanoyl chloride from ethanol?(1)

A

B

C

D



6

*N36506A0624*

8 When propanone reacts with iodine in the presence of sodium hydroxide, the crystalline solid product has the formula

A CH3I

B CHI3

C CH3COCH2I

D CH3COCI3


9 When the following reaction mixtures are warmed, which will contain ethanoic acid as one of the products?

A Ethyl methanoate and sodium hydroxide solution.

B Ethyl methanoate and dilute sulfuric acid.

C Methyl ethanoate and sodium hydroxide solution.

D Methyl ethanoate and dilute sulfuric acid.(Total for Question 9 = 1 mark)

10 The spectra of the compounds with the formulae CH3CH(OH)CH3 and CH3CH2CH2OH can be distinguished by

A the value of m/e of the molecular ion in the mass spectrum.

B the presence of a fragment with m/e =15 in the mass spectrum.

C the presence of an absorption peak due to O–H in the infrared spectrum.

D the number of peaks in the nmr spectrum.


11 Which of the following has two singlet peaks in its nmr spectrum?

A Methanal, HCHO

B Methanol, CH3OH

C Chloromethane, CH3Cl

D Dichloromethane, CH2Cl2


7


12 The nmr spectrum of 2,2-dimethylpropane, H3C—C—CH3, contains

A one singlet peak.

B four singlet peaks.

C one quartet peak.

D four quartet peaks.


13 Which of the following solutions has the lowest pH?

A 0.010 mol dm–3 hydrochloric acid.

B 0.100 mol dm–3 hydrochloric acid.

C 0.010 mol dm–3 ethanoic acid.

D 0.100 mol dm–3 ethanoic acid.(Total for Question 13 = 1 mark)

14 Which of the following solutions, when mixed, would make a buffer with pHmore than 7?

A Methanoic acid and sodium methanoate.

B Sodium hydroxide and sodium chloride.

C Ammonia and ammonium chloride.

D Ammonium chloride and ammonium ethanoate.



CH3

CH3

8

*N36506A0824*

15 This question is about the equilibrium reaction

N2(g) + 3H2(g) 2NH3(g) ∆H = –92 kJ mol–1

Which statement is not correct?

A The units of Kp are atm–2.

B Kp increases as temperature is decreased.

C Kp increases when the pressure increases.

D Kp increases when the total entropy change, ∆Stotal, increases.


16 1,2-dichloroethane decomposes in the presence of a catalyst.

CH2ClCH2Cl(g) CH2=CHCl(g) + HCl(g) ∆H = +51 kJ mol–1

Which of the following would result in an increase in the equilibrium yield of chloroethene?

A Increasing the temperature.

B Increasing the pressure.

C Increasing the surface area of the catalyst.

D Changing the catalyst to a more efficient one.



2

*N36507A0228*

SECTION A



1 In the reaction of manganate(VII) ions with reducing agents in strongly acidic solution, the half-reaction for the reduction is

A MnO4– + 4H+ + 3e– → MnO2 + 2H2O

B MnO4– + 4H+ + 5e– → Mn2+ + 2H2O

C MnO4– + 8H+ + 3e– → Mn2+ + 4H2O

D MnO4– + 8H+ + 5e– → Mn2+ + 4H2O


2 In the titration of iodine with standard sodium thiosulfate solution, starch is often used as an indicator. The starch should not be added until nearly all the iodine has reacted because

A it is decomposed by high concentrations of iodine.

B the blue complex formed is bleached by high concentrations of iodine.

C the blue complex formed with high concentrations of iodine is insoluble and does not re-dissolve as more thiosulfate is added.

D the starch reacts with the thiosulfate ions being added.


3 The conditions needed for the E ○ value of the standard hydrogen electrode to be exactly 0 V are

A 1 mol dm–3 solution of hydrogen ions, 1 atm pressure of hydrogen, 25°C.

B 1 mol dm–3 solution of hydrogen ions, 1 atm pressure of hydrogen, room temperature.

C 1 mol dm–3 solution of hydrogen ions, laboratory pressure of hydrogen, 25°C.

D 0.1 mol dm–3 solution of hydrogen ions, 1 atm pressure of hydrogen, 25°C.


3


4 The electrode potential for a cell can be used to calculate the equilibrium constant for the cell reaction. This is because

A E ○cell is proportional to lnK.

B E ○cell is proportional to K.

C lnE ○cell is proportional to lnK.

D lnE ○cell is proportional to K.


5 Which of the following successive ionization energies (values in kJ mol–1) could have come from a transition element?

A 496 4563 6913 9544 13352 16611 20115 25941

B 590 1145 4912 6474 8144 10496 12320 14207

C 717 1509 3249 4940 6985 9200 11508 18956

D 2081 3952 6122 9370 12177 15239 19999 23069


6 Although platinum is very unreactive, it is used as a catalyst in catalytic converters in motor cars. Which of the following is true?

A It converts nitrogen oxides and carbon monoxide to nitrogen and carbon dioxide by adsorbing the reactants on its surface so weakening their bonds.

B It converts nitrogen oxides and carbon monoxide to nitrogen and carbon dioxide by being able to change its oxidation state.

C It oxidizes unburnt fuel to carbon monoxide.

D It oxidizes unburnt fuel to carbon dioxide.


7 Which of the following gives the electronic configuration for chromium and for the Cr3+ ion?

Cr Cr3+

A [Ar]3d44s2 [Ar]3d34s0

B [Ar]3d54s1 [Ar]3d24s1

C [Ar]3d54s1 [Ar]3d34s0

D [Ar]3d44s2 [Ar]3d14s2


4

*N36507A0428*

8 Which of the following gives the colours of solutions containing Cr2O72–, CrO4

2–, hydrated Cr3+ and hydrated Cr2+, in this order?

A Yellow, orange, green, blue

B Orange, yellow, green, blue

C Orange, yellow, blue, green

D Orange, green, yellow, blue


9 When dichromate(VI) ions, Cr2O72–, react with iron(II) ions in acidic solution, the

products are chromium(III) ions and iron(III) ions. In what ratio do the dichromate(VI) ions and the iron(II) ions react?

A 1:6

B 1:5

C 2:5

D 1:3


10 The compound [Pt(NH3)2Cl2] is

A tetrahedral with no isomers.

B square planar with no isomers.

C tetrahedral with two isomers.

D square planar with two isomers.


11 The hexaaquacopper(II) ion, [Cu(H2O)6]2+, is blue because the water ligands

A split the p-orbital energies and p-p electron transitions emit blue light.

B split the d-orbital energies and d-d electron transitions absorb all but blue light.

C split the p-orbital energies and p-p electron transitions absorb all but blue light.

D split the d-orbital energies and d-d electron transitions emit blue light.


5


12 If phenol and benzene are tested separately with bromine water, you would expect to see that

A benzene and phenol would both decolorize bromine water.

B benzene would decolorize bromine water, but phenol would not do so.

C neither benzene nor phenol would decolorize bromine water.

D benzene would not decolorize bromine water, but phenol would do so.


13 An organic compound X is much more soluble in dilute hydrochloric acid than in water. Compound X forms a coloured complex with aqueous copper(II) ions.

Compound X could be

A C6H5COOH

B C6H5NO2

C C6H5NH2

D C6H5OH


14 Which of the following shows the generation of the electrophile in the reaction of benzene with ethanoyl chloride in the presence of anhydrous aluminium chloride?

A CH3COCl + AlCl3 → [CH3CO]+ + AlCl4–

B CH3COCl + AlCl3 → [CH3CO]– + AlCl4+

C CH3CH2Cl + AlCl3 → [CH3CH2]+ + AlCl4–

D CH3COOCl + AlCl3 → [CH3COO]– + AlCl4+



6

*N36507A0628*

15 Which of the following reagents and conditions would enable phenylamine to be converted to the yellow dye 4-hydroxyazobenzene in a good yield?

A Sodium nitrite, NaNO2, in concentrated HCl, between 0°C and 10°C; followed by an alkaline solution of phenol.

B Sodium nitrite, NaNO2, in concentrated HCl, between 0°C and 10°C; followed by an acidic solution of phenol.

C Sodium nitrate, NaNO3, in concentrated HCl, between 0°C and 10°C; followed by an alkaline solution of phenol.

D Sodium nitrite, NaNO2, in concentrated HCl, room temperature; followed by an alkaline solution of phenol.


16 1-butylamine, CH3CH2CH2CH2NH2, reacts with ethanoyl chloride to form

A CH3CH2CH2CH2NH3+Cl–

B CH3CH2CH2CH2NHCOCH3

C CH3CH2CH2CH2NHCH2CH3

D CH3CH2CH2CH(COCH3)NH2



N N

OH

7


17 The addition polymer poly(ethenol) is water-soluble. The repeating unit of poly(ethenol) is

A

B

C

D



C C

OH H

H OH( (

C C

H H

H OH( (

C C

H OH

H OH( (

C C

OH

OH( (

OH

OH

8

*N36507A0828*

18 A white organic compound, X, is optically active and reacts with ninhydrin to give a coloured product. The structural formula of X could be

A

B

C

D



C

HOOCH

CH3

CH3

C

HOOCNH2

CH3

CH3

C

HOOCNH2

H

CH3

C

HOOCNH2

H

H

9


19 Glycine, H2NCH2COOH, is a solid that has a melting temperature of about 250°C, and it is very soluble in water. This is because of the

A formation of intermolecular hydrogen bonds in the solid and hydrogen bonds with water.

B formation of H3N+CH2COO– ions which interact strongly with each other in the solid and with water.

C dissociation of the molecule to form H2NCH2COO– and H+ ions in the solid and the solution.

D protonation of the molecule to form H3N+CH2COOH ions in both the solid and the solution.


20 Organic solids are often purified by recrystallization. This technique works on the basis that

A the impurities must be insoluble in the solvent used.

B the impurities must react with the solvent used.

C the impurities crystallize first when the hot solution is cooled.

D the cooled solution is saturated with the desired material but not with the impurities.



2

*P38433A0224*

SECTION A



1 In the following outline of the Periodic Table, the letters A to D are not the symbols of the elements.

D

A C

B

Select from A to D the element which

(a) is a non-metal with a high melting temperature and boiling temperature.(1)

A

B

C

D

(b) is in the d block of the Periodic Table.(1)

A

B

C

D

(c) has a very stable electronic structure.(1)

A

B

C

D

3


(d) is a metal with a high melting temperature and boiling temperature.(1)

A

B

C

D


2 The elements in Group 1 of the Periodic Table have very similar chemical properties. This is because

A they have the same number of outer electrons.

B they have the same number of filled shells of electrons.

C their outer electrons are in the s sub-shell.

D their outer electrons have very similar shielding.


3 The European Union has set a limit (with effect from January 2010) of 3.13 ppm for the proportion of the toxic gas carbon monoxide in the air that we breathe. This is equivalent to

A 3.13%

B 0.0313%

C 0.000313%

D 0.00000313%


4 For drivers in the UK, the legal limit of the concentration of ethanol (molar mass 46 g mol–1) in the blood is 80 mg per 100 cm3. This is equivalent to a concentration of

A 17.4 mol dm–3

B 1.74 mol dm–3

C 0.0174 mol dm–3

D 0.00174 mol dm–3


4

*P38433A0424*

5 An important reaction which occurs in the catalytic converter of a car is

2CO(g) + 2NO(g) 2CO2(g) + N2(g)

In this reaction, when 500 cm3 of CO reacts with 500 cm3 of NO at 650 °C (the operating temperature of the catalyst) and at 1 atm, the total volume of gases produced at the same temperature and pressure is

A 500 cm3

B 750 cm3

C 1000 cm3

D impossible to calculate without knowing the molar volume of gases under these conditions.


6 When a solution of barium chloride is added to sulfuric acid, a white precipitate is formed. The ionic equation (including state symbols) for this reaction is

A H+(aq) + Cl–(aq) HCl(s)

B Ba+(aq) + SO4–(aq) BaSO4(s)

C Ba2+(aq) + 2SO4–(aq) Ba(SO4)2(s)

D Ba2+(aq) + SO42–(aq) BaSO4(s)


7 The enthalpy change for the reaction between hydrochloric acid and sodium hydroxide is –56 kJ mol–1. Therefore

A the reaction is exothermic and the temperature rises.

B the reaction is exothermic and the temperature falls.

C the reaction is endothermic and the temperature rises.

D the reaction is endothermic and the temperature falls.


5


8 The standard enthalpy changes of formation of some sulfur species are:

Species Hf / kJ mol–1

S8(s) 0

S8(g) +103

S(g) +279

The enthalpy of atomization of sulfur is (in kJ mol–1)

A 103 ÷ 8

B 279 ÷ 8

C 279

D (103 ÷ 8) + 279


9 For which of the following reactions is the enthalpy change equal to the bond enthalpy of H–I?

A HI(g) ½H2(g) + ½I2(s)

B HI(g) ½H2(g) + ½I2(g)

C HI(g) H(g) + I(g)

D HI(g) H+(g) + I–(g)



6

*P38433A0624*

10 The equation for the complete combustion of pentane is

C5H12(g) + 8O2(g) 5CO2(g) + 6H2O(l) Hc = –3509 kJ mol–1

The standard enthalpy change of formation of CO2(g) is –394 kJ mol–1 and that of H2O(l) is –286 kJ mol–1.

The standard enthalpy change of formation of pentane (in kJ mol–1) is

A 5(–394) + 6(–286) + (–3509)

B 5(–394) + 6(–286) – (–3509)

C –5(–394) – 6(–286) + (–3509)

D –5(–394) – 6(–286) – (–3509)


11 All alkenes have

A the same empirical formula and the same general formula.

B the same molecular formula and the same general formula.

C the same molecular formula and the same empirical formula.

D the same empirical formula and the same structural formula.


12 Covalent bonding results from the strong electrostatic attractions between

A instantaneous dipoles.

B electron clouds.

C electrons in the bonding pair.

D bonding pairs of electrons and nuclei.



7


13 This question concerns the reaction of hydrogen bromide with propene.

(a) This reaction requires(1)

A normal laboratory conditions.

B the presence of UV light.

C the presence of a suitable catalyst.

D heating under reflux.

(b) The reaction is best described as(1)



C nucleophilic addition.

D electrophilic addition.

(c) The major product of the reaction will be(1)

A 1-bromopropane

B 2-bromopropane

C 1,2-dibromopropane

D 2-bromopropene


14 Many organic compounds have toxic vapours. For this reason

A a naked flame should never be used when carrying out experiments with organic compounds.

B gloves should usually be worn when carrying out experiments with organic compounds.

C a fume cupboard should be used wherever possible when carrying out experiments with organic compounds.

D most experiments with organic compounds are banned in schools and colleges.


8

*P38433A0824*

15 Ethanol (molar mass 46 g mol–1) is manufactured by the hydration of ethene (molar mass 28 g mol–1):

C2H4 + H2O C2H5OH

In a typical process 28 tonnes of ethene produces 43.7 tonnes of ethanol. The percentage yield of ethanol in this process is

A 64%

B 95%

C 100%

D 156%



2

*P38479A0220*

SECTION A



1 The correct balanced equation for the reaction between heated magnesium and steam, including state symbols, is

A Mg(s) + H2O(l) MgO(s) + H2(g)

B Mg(s) + 2H2O(g) Mg(OH)2(aq) + H2(g)

C Mg(s) + H2O(g) MgO(s) + H2(g)

D Mg(s) + 2H2O(l) Mg(OH)2(aq) + H2(g)


2 This question concerns the trends in properties on descending Group 2 of the Periodic Table.

(a) What are the trends in solubility of sulfates and hydroxides down Group 2?(1)

A Sulfates increase, hydroxides decrease.

B Sulfates decrease, hydroxides increase.

C Sulfates increase, hydroxides increase.

D Sulfates decrease, hydroxides decrease.

(b) What are the trends in thermal stability of carbonates and nitrates down Group 2?(1)

A Carbonates increase, nitrates decrease.

B Carbonates decrease, nitrates increase.

C Carbonates increase, nitrates increase.

D Carbonates decrease, nitrates decrease.

(c) What are the trends in first ionization energy and electronegativity of the elements down Group 2?

(1) A Ionization energy increases, electronegativity decreases.

B Ionization energy decreases, electronegativity increases.

C Ionization energy increases, electronegativity increases.

D Ionization energy decreases, electronegativity decreases.


3


3 Which silver halide is a cream coloured solid which darkens in sunlight and dissolves in concentrated ammonia solution?

A AgF

B AgCl

C AgBr

D AgI


4 What is the FBF bond angle in boron trifluoride, BF3?

A 180°

B 120°

C 109.5°

D 90°


5 What is the total number of electrons in the covalent bonds in a beryllium chloride molecule, BeCl2?

A 2

B 4

C 6

D 8


6 Which of the following molecules is linear?

A CO2

B C2H4

C H2O

D NH3


4

*P38479A0420*

7 Which of the following molecules is non-polar?

A CH3Cl

B CH2Cl2

C CHCl3

D CCl4


8 Methanol dissolves in water mainly due to the formation of new

A hydrogen bonds.

B dipole-dipole forces.

C London forces.

D covalent bonds.


9 Which of the following molecules does not absorb infrared radiation?

A N2

B NO2

C CO

D CO2


10 There would be a major peak in the mass spectrum for butan-1-ol, CH3CH2CH2CH2OH,but not for butan-2-ol, CH3CH2CH(OH)CH3, at m/e value

A 15

B 17

C 29

D 43



5


11 How many molecular ion peaks (parent ion peaks) occur in the mass spectrum of 1,2-dibromoethane, CH2BrCH2Br?

Assume the only isotopes present are 1H, 12C, 79Br and 81Br.

A 1

B 2

C 3

D 4


12 The following reactions have been used in the chemical industry to make liquid and solid products, allowing any gaseous products to escape into the atmosphere:

A CH3OH(g) + CO(g) CH3COOH(l)

B CaCO3(s) CaO(s) + CO2(g)

C CH4(g) + 3Cl2(g) CHCl3(l) + 3HCl(g)

D CH2CH2(g) + Cl2(g) CH2ClCH2Cl(l)

(a) Which reaction has an atom economy by mass of 56%?(1)

A

B

C

D

(b) Which reaction causes the most immediate damage to the environment?(1)

A

B

C

D

(c) Which reaction is an electrophilic addition?(1)

A

B

C

D


6

*P38479A0620*

13 Propan-1-ol and propan-2-ol are separately oxidized under mild conditions by acidified sodium dichromate(VI) and the product immediately distilled off. What is the oxidation product in each case?

Propan-1-ol Propan-2-ol

A propanal propanone

B propanoic acid propanone

C propanal propanoic acid

D propanone propanal


14 Unsaturated vegetable oils are hardened to make margarine by reaction with hydrogen and a nickel catalyst. Which terms could both be used to describe this type of reaction?

A Substitution and oxidation

B Substitution and reduction

C Addition and oxidation

D Addition and reduction


15 When iodomethane, CH3I, is heated in a sealed tube with an excess of alcoholic ammonia, which of the following cannot be formed?

A Methylamine, CH3NH2

B Ethylamine, CH3CH2NH2

C Dimethylamine, (CH3)2NH

D Ammonium iodide, NH4I



7


16 The enthalpy change of neutralization of an acid by an alkali is measured by adding 10.0 cm3 of hydrochloric acid to 10.0 cm3 of sodium hydroxide. 10.0 cm3 pipettes with an accuracy of ±0.04 cm3 are used to measure out both solutions.

The overall percentage error in measuring the total volume of the reaction mixture is

A ±0.04%

B ±0.08%

C ±0.4%

D ±4.0%



2

*P38482A0224*

SECTION A



1 Which of the following methods would not be suitable for measuring the rate of the reaction between methanoic acid and bromine?

HCOOH(aq) + Br2(aq) 2H+(aq) + 2Br (aq) + CO2(g)

A Colorimetry

B Measuring change in electrical conductivity

C Quenching samples and titrating with acid

D Measuring change in pressure


2 The equation below shows the hydrolysis of a bromoalkane.

RBr + OH ROH + Br

For a particular bromoalkane, the rate equation is

rate = k[RBr]

The bromoalkane, RBr, is most likely to be

A CH3Br

B CH3CH2Br

C (CH3)3CCH2Br

D (CH3)3CBr


3 A decrease in the entropy of the system, Ssystem, occurs when

A water freezes.

B water boils.

C water reacts with sodium.

D water reacts with ethanoyl chloride.


3


4 Methanol is produced in the equilibrium reaction

2H2(g) + CO(g) CH3OH(g) H = 18.3 kJ mol 1

Addition of more hydrogen to the equilibrium mixture at constant temperature

A increases the equilibrium yield of methanol.

B decreases the equilibrium yield of methanol.

C increases the value of Kp.

D decreases the value of Kp.


5 The equation for the equilibrium between NO2(g) and N2O4(g) can be written in two ways.

2NO2(g) N2O4(g) Equilibrium constant = Kc

or

NO2(g) ½N2O4(g) Equilibrium constant = K'c

Which expression is correct?

A Kc = K'c

B Kc = (K'c)2

C Kc = 2(K'c)

D Kc = ½K'c


6 4.0 mol of methanoic acid are reacted with 6.0 mol of ethanol.

HCOOH(l) + C2H5OH(l) HCOOC2H5(l) + H2O(l)

The equilibrium mixture contains 3.0 mol of HCOOC2H5.

The equilibrium constant, Kc, for the reaction is

A 0.33

B 1.0

C 3.0

D 4.0


4

*P38482A0424*

7 A solution of hydrochloric acid has pH 3.0. When it is made 10 times more dilute, the pH is

A 0.3

B 2.0

C 4.0

D 13.0


8 The titration curves below were obtained using different acids and bases, each with concentration 0.1 mol dm–3.

D

14 –12 –10 –8 –6 –4 –2 –0 ––

0

pH

–

10

–

20

–

30

–

40

C

14 –12 –10 –8 –6 –4 –2 –0 ––

0

pH

–

10

–

20

–

30

–

40

B

14 –12 –10 –8 –6 –4 –2 –0 ––

0

pH

–

10

–

20

–

30

–

40

A

14 –12 –10 –8 –6 –4 –2 –0 ––

0

pH

Volume 0.1 mol dm–3 solution added / cm3–

10–

20

–

30

–

40

Volume 0.1 mol dm–3 solution added / cm3



5


(a) Which curve is produced by adding ammonia to 25 cm3 of hydrochloric acid?(1)

A

B

C

D

(b) Which curve is produced by adding ethanoic acid to 25 cm3 of sodium hydroxide?(1)

A

B

C

D

(c) An indicator with pKIn 8.5 is suitable for the following titrations.(1)

A Titrations A and B only.

B Titrations A, B and D only.

C Titration C only.

D Titrations A, B, C and D.


9 Ethanoic acid is not a product in the reaction of

A ethanal with lithium tetrahydridoaluminate.

B ethanoyl chloride with water.

C ethyl ethanoate with dilute sulfuric acid.

D ethanol refluxed with potassium dichromate(VI) and sulfuric acid.



6

*P38482A0624*

10 This question is about four compounds with molecular formula C4H8O.

A CH3COCH2CH3

B CH3CH2CH2CHO

C CH3CH CHCH2OH

D CH2 CHOH CH2 CH2

(a) The compounds which react when heated with a mixture of potassium dichromate(VI) and sulfuric acid are

(1) A compounds A, B and C.

B compounds A, B and D.

C compounds A, C and D.

D compounds B, C and D.

(b) The compound which produces a yellow precipitate when heated with a mixture of iodine and sodium hydroxide is

(1) A compound A.

B compound B.

C compound C.

D compound D.

(c) There would not be a significant peak at mass/charge ratio of 15 in the mass spectrum of

(1) A compound A.

B compound B.

C compound C.

D compound D.


7


11 The following tests can be carried out on organic compounds.

A Warm with 2,4-dinitrophenylhydrazine.

B Warm with Fehling’s or Benedict’s solution.

C Add solid sodium carbonate.

D Add phosphorus(V) chloride, PCl5.

(a) Which test would give a positive result with propanoic acid but not with propan-1-ol?

(1) A

B

C

D

(b) Which test would give a positive result with propanoic acid and with propan-1-ol?(1)

A

B

C

D

(c) Which test would give a positive result with propanal but not with propanone?(1)

A

B

C

D



8

*P38482A0824*

12 Which of the following compounds is a Z isomer and contains a chiral carbon atom?

A

Cl

B

Cl

C

Cl

D

Cl


13 Which of the following statements about ethanoyl chloride is not correct?

A It reacts with ammonia to make an amine.

B It reacts with an amine to make an amide.

C It reacts with an alcohol to make an ester.

D It reacts with water to make an organic acid.


14 In gas chromatography, mixtures are passed through a long tube containing a liquid as the stationary phase. The mixtures are separated into their components because the components differ in

A relative molecular mass.

B melting temperature.

C volatility.

D force of attraction to the liquid.



2

*P38480A0224*

SECTION A



1 Four complex ions have the following formulae:

A Cu(edta)2

B Zn(H2O)62+

C Ni(NH3)62+

D CrCl42

(a) Which complex ion is most likely to be tetrahedral in shape?(1)

A

B

C

D

(b) Which complex ion is most likely not to be coloured?(1)

A

B

C

D

(c) Each of these complex ions may be formed by ligand exchange from an aqua complex. For which complex ion is the entropy change of this reaction most positive?

(1) A

B

C

D


3


2 When a few drops of aqueous ammonia are added to a solution containing [Cr(H2O)6]3+

ions the product formed will be

A [Cr(NH3)6]3+

B Cr(H2O)3(OH)3

C [Cr(NH3)4]3+

D [Cr(H2O)2(OH)4]


3 Which of these statements about a standard hydrogen electrode, for which E = 0 V, is not correct?

A The hydrogen gas is at a pressure of 1 atm.

B A solution containing 1 mol dm 3 of H+(aq) ions is used.

C A platinum electrode is used.

D The temperature is kept at 20 °C.



4

*P38480A0424*

4 Four polymers labelled A to D have the following formulae:

A —–C—(CH2)4—C—N—(CH2)6—N—–

O

H

O H

n

B

n

—–C—–C–—C–—C—––

H

H OH H OH

H H H

C —–C—–C––––––—C–—C–––––––—

H

H OOCCH3 H

H H H

OOCCH3

n

D —–C—–C–—C–—C—––

H

H CH3 H CH3

H H H n

(a) Which polymer is most soluble in hot water?(1)

A

B

C

D

5


(b) Which polymer is formed from the monomer shown below?(1)

A

B

C

D

(c) Which polymer is a condensation polymer?(1)

A

B

C

D



O

O

6

*P38480A0624*

5 The formulae of some organic compounds labelled A to D are shown below.

(a) Which compound reacts with sodium to form hydrogen?(1)

A

B

C

D

(b) Which compound forms a green complex ion with CuSO4(aq)?(1)

A

B

C

D

(c) Which compound forms an orange precipitate with 2,4-dinitrophenylhydrazine?(1)

A

B

C

D


CH3

OC

CH3

OHCH(CH3)2

NH2

A

C

B

D

7


6 How many peaks would you expect to see in a low resolution proton nmr spectrum of the ester HCOOCH2CH2CH3?

A 8

B 7

C 4

D 3


7 In a high resolution proton nmr spectrum of ethyl ethanoate, CH3COOCH2CH3, the peak due to the hydrogen atoms shown in bold would be a

A singlet.

B doublet.

C triplet.

D quartet.


8 Which of these compounds, whose formulae are shown below, cannot exist as a racemic mixture?

A CH2ClCHClCOOH

B HOOCCHClCOOH

C CH3CHClCOOH

D CH3CH(OH)COOH


8

*P38480A0824*

9 Phenol reacts with bromine water whereas benzene reacts with bromine in the presence of iron.

(a) The mechanism for both these reactions is(1)

A electrophilic substitution.

B electrophilic addition.

C nucleophilic substitution.

D nucleophilic addition.

(b) In the reaction of benzene with bromine, iron(1)

A acts as a heterogeneous catalyst.

B acts as a homogeneous catalyst.

C reacts with the bromine to make iron(III) bromide, FeBr3.

D allows bromine to attack the hydrogen atoms on benzene more readily.

(c) Bromine reacts more readily with phenol than with benzene because the OH group on phenol

(1) A is a good leaving group.

B attracts the bromine particles more readily.

C is a good nucleophile.

D increases the electron density of the ring.


10 Ammonia (NH3), butylamine (CH3CH2CH2CH2NH2) and phenylamine (C6H5NH2) all form alkaline solutions in water. The order of increasing pH of equimolar solutions is

A C6H5NH2 < CH3CH2CH2CH2NH2 < NH3

B NH3 < CH3CH2CH2CH2NH2 < C6H5NH2

C C6H5NH2 < NH3 < CH3CH2CH2CH2NH2

D CH3CH2CH2CH2NH2 < NH3 < C6H5NH2


9


11 The distance on a chromatogram moved by an individual amino acid, in a mixture of different amino acids, mainly depends on

A the molar mass of the amino acid.

B the molar mass of the solvent used.

C the intermolecular forces between the solvent and the stationary phase.

D the intermolecular forces between the amino acid and both the solvent and the stationary phase.


12 Amino acids are crystalline solids with a high melting temperature because

A each molecule has a large number of electrons.

B each molecule forms hydrogen bonds at both ends.

C a proton is transferred from one end of the molecule to the other.

D their shape allows the molecules to pack close together.



2

*P39306A0224*

SECTION A



1 A solution contains 66 ppm of a solute. The mass of the solute dissolved in 1 kg of this solution is

A 66 g

B 0.66 g

C 0.066 g

D 0.000066 g


2 Complete combustion of 50 cm3 of a hydrocarbon vapour gave 350 cm3 of carbon dioxide, both gas volumes being measured at the same temperature and pressure. The formula of the hydrocarbon could be

A C8H18

B C7H16

C C6H14

D C5H12


3 Which of the following statements is true? The Avogadro constant is the number of

A grams of any element which contains 6.02 × 1023 atoms of that element.

B atoms contained in one mole of any element.

C atoms contained in one mole of any monatomic element.

D particles (atoms, molecules or ions) required to make one gram of a substance.


3


4 In an experiment to determine the enthalpy change of combustion of an alcohol, a spirit burner containing the alcohol was weighed, lit and placed under a copper can containing a known volume of water. The temperature rise of the water was measured and the burner re-weighed. The enthalpy change calculated from the results was much less exothermic than the value reported in the literature.

Which of the following factors is most likely to be the cause of this error?

A Heat loss around the side of the copper can.

B The use of a thermometer with a range of 0 – 110 °C rather than 0 – 50 °C.

C The use of a measuring cylinder for measuring the water rather than a pipette.

D Evaporation of the alcohol during the weighing.


5 The standard enthalpy changes of formation of carbon dioxide and of methanoic acid are ��–1�� –1 respectively. Calculate the enthalpy change for the reaction

H2(g) + CO2(g)��HCOOH(l)

A ��–1

B ��–1

C ��–1

D ��–1


6� For which of the following changes is the value of �H negative?

A K(g)��K+(g) + e–

B K+Cl–(s)��K+(g) + Cl–(g)

C Cl(g) + e–��Cl–(g)

D Cl2(g)��2Cl(g)


4

*P39306A0424*

7 In which of the following cases would a cation be most polarizing?

Radius Charge

A small small

B small large

C large small

D large large


8 Magnesium chloride, MgCl2, has two lattice energy values quoted in the data booklet. �� !�"�� #� $%�"��&'&��!��*�*/��–1; ��& ��&��!��*�*/��–1. Why are the two values different?

A The cation polarizes the anion leading to some covalent bonding.

B The anion polarizes the cation leading to some covalent bonding.

C Magnesium chloride is a covalent substance.

D The results from the Born-Haber cycle are too inaccurate to be reliable.


9 Which of the following represents the process occurring when the enthalpy change of atomization of bromine is measured?

A ½Br2(l)��Br(g)

B ½Br2(g)��Br(g)

C Br2(l)��Br+(g) + Br–(g)

D Br2(g)��Br+(g) + Br–(g)



5


10 An organic compound is represented by the skeletal formula shown below.

The compound is

A CH3CH2CH2CH(OH)CH2CH3

B (CH3)2CHC(OH)(CH3)2

C (CH3)2CHCH2CH(OH)CH3

D (CH3)2CHCH(OH)CH2CH3


11 How many structural isomers does the alkane C5H12 have?

A 4

B 3

C 2

D 1


12 When methane reacts with chlorine, a mixture of products forms. Which product provides the strongest evidence for a free radical mechanism?

A C2H6

B CH3Cl

C HCl

D CHCl3


OH

6

*P39306A0624*

13 What is the IUPAC name of the compound shown below?

A 2-ethyl-2-propylpentane

B 3-methyl-3-propylhexane

C 4-methyl-4-propylhexane

D 4-ethyl-4-methylheptane


14 The reaction of bromine with propene is an example of

A electrophilic substitution.

B free radical substitution.


D free radical addition.


15 A compound Z contains, by mass, 26.7% carbon, 2.2% hydrogen, and 71.1% oxygen. The empirical formula of Z is

A CHO2

B C2H2O4

C CHO

D C2H2O2


H3C C CH2CH2CH3

CH2CH3

CH2CH2CH3

7


7


16 In which of the following series does the melting temperature of the element increase from left to right?

A Li, Na, K

B Al, Si, P

C Si, P, S

D Na, Mg, Al


17 If X�� &� �"�� Y the element of atomic number 20, the compound formed between these two elements is

A covalent, YX2.

B ionic, YX2.

C covalent, YX.

D ionic, YX.


18 The equation representing the reaction between copper(II) oxide and dilute sulfuric acid is

CuO(s) + H2SO4(aq)��CuSO4(aq) + H2O(l)

The ionic equation for the reaction is

A Cu2+(s) + SO42–(aq)��CuSO4(aq)

B O2–(s) + H2SO4(aq)��H2O(l) + SO42–(aq)

C CuO(s) + 2H+(aq)��Cu2+(aq) + H2O(l)

D CuO(s) + H2SO4(aq)��Cu2+SO42–(aq) + H2O(l)


8

*P39306A0824*

19 Which of the following represents the electronic structure of a nitrogen atom?

1s 2s 2p

A ��

B ��

C ��

D ��


20 The electronic structures of four elements are given below. Which of these elements has the highest first ionization energy?

1s 2s 2p

A ��

B ��

C ��

D ��



2

*P39307A0220*

SECTION A



1 The diagram below shows the Maxwell-Boltzmann distribution of molecular energies for a gaseous system at two temperatures.

(a) The energy plotted on the horizontal axis is mainly(1)

A activation.

B kinetic.

C rotation.

D vibration.

(b) The rate of a chemical reaction increases with temperature mainly because(1)

A the activation energy increases.

B the activation energy decreases.

C more collisions occur with energy greater than the activation energy.

D the molecules collide more frequently.

300 K

310 K

Number of molecules with energy E

Energy E

3


(c) The total area under each curve(1)

A decreases with increasing temperature.

B increases with increasing temperature.

C increases or decreases with increasing temperature, depending on the size of the molecules.

D does not change with temperature.


2 The diagram below shows a dot and cross diagram of nitric acid.

(a) Identify which of the labelled sets of electrons represents a dative covalent bond.(1)

A

B

C

D

(b) In terms of orbital overlap, the double bond is(1)

A��

B��

C ��

D � ��


A

C

B

D

O

N O H

O

4

*P39307A0420*

3 The colour observed in a flame test is due to

A electrons jumping to a higher energy level, absorbing energy.

B electrons jumping to a higher energy level, emitting energy.

C electrons dropping from a higher energy level, absorbing energy.

D electrons dropping from a higher energy level, emitting energy.


4 The best way to confirm the presence of iodine in an aqueous solution is

A adding hexane to form a purple layer.

B adding hexane to form an orange layer.

C adding acidified silver nitrate solution to form a yellow precipitate which is soluble in concentrated ammonia.

D adding acidified silver nitrate solution to form a yellow precipitate which is insoluble in concentrated ammonia.


5 The oxidation number of sulfur in sodium hydrogensulfide, NaHS, is

A –2

B –1

C +1

D +2


6 Which of the following is not a disproportionation reaction?

A Cl2 + 2OH– � Cl– + ClO– + H2O

B Cu2O + H2SO4 � CuSO4 + Cu + H2O

C 3IO– � 2I– + IO3–

D Cu + 4HNO3 � Cu(NO3)2 + 2H2O + 2NO2



5


7 Hydrogen iodide has a higher boiling temperature than hydrogen bromide. This is because

A the H–I bond is stronger than the H–Br bond.

B hydrogen iodide has stronger London forces than hydrogen bromide.

C hydrogen iodide has a larger permanent dipole than hydrogen bromide.

D hydrogen iodide forms hydrogen bonds but hydrogen bromide does not.


8 Butane has a higher boiling temperature than 2-methylpropane. This is because butane has

A stronger C–H bonds.

B more electrons.

C a larger surface area.

D hydrogen bonds.


9 The oxygen atom in a molecule of water has two bonding pairs and two lone pairs of electrons. Based on the electron-pair repulsion theory, the H–O–H bond angle is most likely to be

A 180°

B 109.5°

C 107°

D 104.5°


10 The shape of a molecule of boron trifluoride, BF3, is

A trigonal planar.

B pyramidal.

C tetrahedral.

D T-shaped.


6

*P39307A0620*

11 When solid samples of sodium carbonate and magnesium carbonate are strongly heated

A both compounds decompose.

B sodium carbonate decomposes but magnesium carbonate does not.

C magnesium carbonate decomposes but sodium carbonate does not.

D neither compound decomposes.


12 As Group 2 is descended

A the solubility of hydroxides and of sulfates increases.

B the solubility of hydroxides increases and of sulfates decreases.

C the solubility of hydroxides decreases and of sulfates increases.

D the solubility of hydroxides and of sulfates decreases.


13 These questions concern the use of infrared (IR) spectra to identify organic compounds. The IR absorption ranges associated with some organic functional groups are given below.

A O–H stretching in alcohols at 3750 – 3200 cm–1

B C�O stretching in aldehydes at 1740 – 1720 cm–1

C C�O stretching in ketones at 1700 – 1680 cm–1

D C�O stretching in carboxylic acids at 1725 – 1700 cm–1

(a) When propan-2-ol is refluxed with potassium dichromate(VI) and sulfuric acid, the product will show a peak due to

(1) A

B

C

D

(b) When propan-1-ol is heated with potassium dichromate(VI) and sulfuric acid, the product, that is distilled off as it is formed, will show a peak due to

(1) A

B

C

D


7


14 Which of the following formulae does not represent 2,2-dimethylpropan-1-ol?

A OH

B

H C C C H

H

H H

H

H C H

H C OH

H

H

C

OH

D (CH3)3CCH2OH


15 Nucleophiles are

A electron pair donors that attack regions of high electron density.

B electron pair donors that attack regions of low electron density.

C electron pair acceptors that attack regions of high electron density.

D electron pair acceptors that attack regions of low electron density.


16 Which of the following is not true? Chlorofluorocarbons, CFCs,

A are flammable.

B are greenhouse gases.

C damage the ozone layer.

D are excellent refrigerants.



2

*P39308A0224*

SECTION A



1 Which of the following interacts with the nuclei of hydrogen atoms in a nuclear magnetic resonance spectrometer?

A Gamma rays

B X-rays

C Microwaves

D Radio waves


2 HPLC stands for

A high pressure liquid column.

B high performance liquid chromatography.

C heterogeneous phase liquid chromatography.

D homogenous phase liquid column.



3


3 Consider the equilibrium below.

CO(g) + Cl2(g) � COCl2(g)

(a) An increase in pressure by a factor of 2 will(1)

A quadruple Kp.

B double Kp.

C have no effect on Kp.

D halve Kp.

(b) The units of Kp are(1)

A atm��

B atm��

C atm

D atm2


4 Which of these will not improve the overall yield of the Haber process?

N2(g) + 3H2(g) � 2NH3��H��

A Increasing the pressure.

B Liquefying then removing the ammonia from the reaction.

C Increasing the temperature.

D Recycling unreacted nitrogen and hydrogen.


5 The equation for the reaction between ethanoic acid and phosphorus(V) chloride is

A CH3COOH + PCl5��3COCl + POCl3 + HCl

B CH3COOH + PCl5��3COOCl + PCl3 + HCl

C CH3COOH + PCl5��3COCl + PCl3 + HOCl

D 2CH3COOH + PCl5��3CO)2O + PCl3 + H2O + Cl2


4

*P39308A0424*

6 An example of a polyester is

(a) The two monomers needed to form this polymer are (1)

Monomer One Monomer Two

A HOOC OH HO(CH2)2OH

B HOOC COOH HO(CH2)2OH

C HO OH HOOC(CH2)2COOH

D HOOC COOH HOOC(CH2)2COOH

(b) The type of reaction to form this polymer is(1)

A addition.

B substitution.

C condensation.

D hydrolysis.


OO

O

C

⎛

⎝

⎜⎜⎜⎜⎜

⎞

⎠

⎟⎟⎟⎟⎟

H H

C

H H

C

O

C

5


7 In which of these reactions is the hydrogensulfate ion, HSO4�, behaving as a Brønsted-

Lowry base?

A HSO4� + H3O+ ��2SO4 + H2O

B HSO4� + Ba2+ ��4 + H+

C HSO4� + H2O ��4

�� + H3O+

D HSO4� + CO3

�� SO4�� + HCO3

�


8 The reaction below is carried out at 25 °C. Use the equation and the data to answer the questions that follow.

SO2(g) + 2H2��2��H��

Substance Standard molar entropy, S �� K��

SO2(g) 248

H2S(g) ��!

H2O(g) �"�

S(s) 32

� ��#$%��&�'*�/*�%'&/�01�6$�'�%��7�&$%��1�&%�9�:'� �� K��, is(1)

A� ��"!

B� ��"!

C� ��

D +233

� �;��#$%��&�'*�/*�%'&/�01�6$�'�%��7�&$%��<//�<'*:'��9�:'� �� K��, is(1)

A� ��=

B� ��=

C� ��"

D� ��"


6

*P39308A0624*

9 >�$��%'��'%9�@D9�/%�6&��E:&$�$1*/�F:*%�:�'�9��, to form an alcohol.

RX + OH��@��D�

The rate equation for the reaction is rate = k[RX]. Which of these statements is incorrect?

A Rate � [RX].

B� @D�:��0/:��/1�$��%'��'%�

C The reaction mechanism is SN��

D A carbocation intermediate forms in the reaction.


10 The rate equation for the reaction between hydrogen gas and nitrogen monoxide gas is

rate = k[NO]2[H2]

If the concentration of both reactants is doubled, the rate will increase by a factor of

A 3

B 4

C� !

D 8



7


11 A reaction has the rate equation rate = k[X][Y]2[Z]. The concentrations of each reactant are shown in the table below.

Reactant Concentration / mol dm��

X ��

Y ��

Z ��

� ��\7�&$%�/�&%��7�/%�6&:�'�<'*%/�&$%�%�6�'*:&:�'��$��^��<%��7��*�� s��, then the numerical value of k is

(1)

A� ��"�

B� ��=��

C� ��"�=

D� ��=�

(b) The units for the rate constant, k, are(1)

A mol�� dm��s��

B mol3 dm� s��

C mol�� dm�� s��

D mol3 dm�� s��



8

*P39308A0824*

12 This question is about the four organic substances shown below.

A CH3CH2CH2CH2CHO

B CH3CH2CH2CH2COOH

C CH3COCH2CH2CH3

D CH3CH2CH2CH2COCl

Which substance will

(a) give a positive result with both Brady’s and Tollens’ reagents?(1)

A

B

C

D

(b) be formed by the oxidation of a secondary alcohol?(1)

A

B

C

D

� �6��7�/��&$%��&��6:*:6��<&:�'�E$%'�%_<��<'&��/%�%�6$��:F%*�E:&$��6�3 of water?

(1) A

B

C

D

(d) form steamy fumes in the reaction with PCl5?(1)

A

B

C

D


9


13� \'��/*%/�&��%��3CH2CONHCH3, you could use

A CH3CH2COOCH3 + NH3

B CH3CH2COCl + CH3NH2

C CH3CH2COO�Na+ + CH3NH2

D CH3CH2CONH2 + CH3NH2



2

*P39309A0220*

SECTION A



1 The acid used in a standard hydrogen electrode to provide a 1 mol dm–3 solution of hydrogen ions is

A ethanoic acid.

B phosphoric(V) acid.

C sulfuric acid.

D hydrochloric acid.


2 To measure the standard electrode potential for the Ag+(aq)|Ag(s) electrode, the most suitable chemical for the solution in a salt bridge to connect the two half cells is

A potassium chloride.

B potassium iodide.

C potassium nitrate.

D potassium sulfate.


3 For any reversible reaction, ln K is proportional to

A� ��Stotal and Ecell.

B� �Stotal but not Ecell.

C Ecell but not �Stotal.

D neither Ecell��Stotal.


3


4 This question is about a titration to determine the iron content of a tablet. The iron(II) ions in the tablet are oxidized to iron(III) ions by acidified manganate(VII) ions which are reduced to manganese(II) ions.

(a) The mole ratio of iron(II) to manganate(VII) ions in the reaction is(1)

Fe2+ MnO4–

A 1 5

B 2 5

C 5 2

D 5 1

(b) A 0.200 g tablet is dissolved to make exactly 100 cm3 of solution. 10 cm3 of this solution is found to contain 5.38 � 10–5 mol of iron(II) ions.

The percentage by mass of iron (Ar = 55.8) in the tablet is(1)

A 5 3 0 55 80 200

10010

1005. .

.%8 1× × × ×

−

B 5 38 1055 8 0 200

10010

1005.

. .%×

×× ×

−

C 5 38 10 55 80 200

10100

1005. .

.%× × × ×

−

D 5 38 10 0 20055 8

10100

1005. ..

%× × × ×−



4

*P39309A0420*

5 Some fuel cells are used to produce energy from the combination of hydrogen and oxygen. The half-equations for a hydrogen-oxygen fuel cell in alkaline solution are

2H2O(l) + 2e– � H2(g) + 2OH–(aq) E � = –0.83 V

½O2(g) + H2O(l) + 2e– � 2OH–(aq) E � = +0.40 V

(a) The equation for the cell reaction is(1)

A 3H2O(l) + ½O2�� 2(g) + 4OH–(aq)

B H2(g) + 4OH–�� 2O(l) + ½O2(g)

C H2(g) + ½O2�� 2O(l)

D H2�� 2(g) + ½O2(g)

(b) From the data above, Ecell for the reaction in the hydrogen-oxygen fuel cell is(1)

A –0.43 V

B +0.43 V

C –1.23 V

D +1.23 V

(c) An advantage of operating a hydrogen fuel cell over a conventional jet engine for powering an aeroplane is

(1) A it is 100% efficient.

B it does not produce greenhouse gas emissions.

C it does not produce emissions which damage the ozone layer.

D hydrogen is easier to transport.


5


6 Benzocaine is used as a local anaesthetic.

Separate samples of a solution of benzocaine are added to 2,4-dinitrophenylhydrazine, hot aqueous sodium hydroxide, and dilute hydrochloric acid.

Which chemicals react with benzocaine?

A All three

B Only sodium hydroxide and hydrochloric acid

C Only hydrochloric acid

D Only sodium hydroxide


7 In the first commonly used breathalyser, acidified potassium dichromate(VI) was used which was reduced to chromium(III) by alcohol.

The colour change seen when alcohol was present in a motorist’s breath is from

A orange to green.

B orange to yellow.

C yellow to green.

D yellow to orange.


8 For which of the following are both tests acceptable evidence for a driver to be successfully prosecuted for excess alcohol in the blood in many countries?

A A dichromate(VI) breath analyser and a blood test.

B A dichromate(VI) breath analyser and a fuel cell breath analyser.

C A dichromate(VI) breath analyser and an infrared breath analyser.

D An infrared breath analyser and a blood test.


NH2

O

C

OCH2CH3

6

*P39309A0620*

9 The structural formula of caffeine, C8H10O2N4, is shown below.

(a) How many main peaks would you expect in the proton nuclear magnetic resonance spectrum of caffeine?

(1)

A 1

B 2

C 3

D 4

(b) At which of the following wavenumbers is an absorption peak not present in the infrared spectrum of caffeine?

(1)

A 3600 cm–1

B 2925 cm–1

C 1690 cm–1

D 1660 cm–1

(c) The parent ion peak of caffeine in the mass spectrum of caffeine would be at m/e ratio

(1) A 101

B 102

C 193

D 194

CH3

N

N

NO

O

CH3

N

CH3

7


(d) Intermolecular forces between caffeine molecules would include(1)

A London forces only.

B London forces and hydrogen bonds.

C London forces and permanent dipole forces.

D London forces, permanent dipole forces, and hydrogen bonds.


10 (a) The principal advantage of combinatorial chemistry over traditional methods for developing pharmaceuticals is that

(1) A very small amounts of compounds are used.

B many more compounds can be made in a given time.

C compounds formed are more powerful drugs.

D compounds formed have fewer side effects.

(b) A refinement of combinatorial chemistry involves initially attaching compounds firmly to polymer beads. The type of attachment is most likely to be by

(1) A metallic bonds.

B covalent bonds.

C London forces.

D permanent dipole forces.


8

*P39309A0820*

11 Four reactions involving the transition elements copper and chromium are given below.

1 Cu2+(aq) + 2OH−�� 2(s)

2 [Cu(H2O)4(OH)2](s) + 4NH3�� 2O)2(NH3)4]2+(aq) + 2OH−(aq) + 2H2O(l)

3 [Cr(H2O)3(OH)3](s) + 3OH−�� 6]3−(aq) + 3H2O(l)

4 [Cr(H2O)3(OH)3](s) + 3H+�� 2O)6]3+(aq)

(a) Which reaction produces a dark blue solution?(1)

A 1

B 2

C 3

D 4

(b) Which two reactions show the amphoteric behaviour of a metal hydroxide?(1)

A 1 and 2

B 2 and 3

C 2 and 4

D 3 and 4

(c) Predict, without calculation, which reaction has the most negative value for ΔSsystem.(1)

A 1

B 2

C 3

D 4



2

*P41649A0224*

SECTION A




a cross .

1 Which of the following quantities, used in the calculation of the lattice energy of lithium oxide, Li2O, has a negative value?

A The enthalpy change of atomization of lithium.

B The first ionization energy of lithium.

C The first electron affinity of oxygen.

D The second electron affinity of oxygen.


2 Which of the diagrams below best represents the shapes of the electron contours in sodium fluoride?

A

–

+

B +

–

C +

–

D �+

�–


3


3 Which of the equations below represents the first electron affinity for oxygen?

A O2(g) + 2e– � 2O–(g)

B O2(g) – 2e– � 2O–(g)

C ½O2(g) + e– � O–(g)

D O(g) + e– � O–(g)


4 Which pair of ions is isoelectronic?

A Ca2+ and O2–

B Na+ and O2–

C Li+ and Cl–

D Mg2+ and Cl–


5 A drop of sodium manganate(VII) solution is placed at the centre of a piece of moist filter paper on a microscope slide. The ends of the paper are clipped to a 30 V DC power supply. After a few minutes,

A a purple colour has moved towards the positive terminal.

B a purple colour has moved towards the negative terminal.

C an orange colour has moved towards the positive terminal.

D an orange colour has moved towards the negative terminal.


6 How many moles of ions are present in 20 cm3 of 0.050 mol dm–3 calcium chloride solution, CaCl2(aq)?

A 0.0050

B 0.0030

C 0.0020

D 0.0010


4

*P41649A0424*

7 The Avogadro constant is 6.0 x 1023 mol–1. The number of atoms in 1 mol of dinitrogen tetroxide, N2O4, is

A 3.6 × 1024

B 1.8 × 1024

C 6.0 × 1023

D 1.0 × 1023


8 The equation for the complete combustion of ethane is

2C2H6(g) + 7O2(g) � 4CO2(g) + 6H2O(l)

What volume of oxygen, measured at room temperature and pressure, is needed to completely burn 0.1 mol of ethane?

[The volume of 1 mol of any gas measured at room temperature and pressure is 24 dm3]

A 2.4 dm3

B 4.8 dm3

C 8.4 dm3

D 16.8 dm3


9 A sample of swimming pool water contains 0.482 parts per million (ppm) of chlorine. This is equal to a percentage of

A 0.000482

B 0.0000482

C 0.00000482

D 0.000000482


5


10 Bromine has two isotopes with relative isotopic masses 79 and 81. Which of the following values for mass/charge ratio could correspond to a peak in the mass spectrum of bromine, Br2? You should assume the ions detected have a single positive charge.

A 79.9

B 80

C 159

D 160


11 The first five ionization energies of an element, X, are shown in the table.

Ionization energy 1st 2nd 3rd 4th 5th

Value / kJ mol–1 631 1235 2389 7089 8844

What is the mostly likely formula of the oxide that forms when X burns in oxygen?

A X2O

B XO

C X2O3

D XO2


12 Which of the following has the largest ionic radius?

A S2–

B Cl–

C K+

D Ca2+


6

*P41649A0624*

13 Which of the following is a major effect caused by increased carbon dioxide levels arising from the burning of fossil fuels?

A Melting of polar ice caps.

B Damage to the ozone layer.

C Increased acid rain.

D Increased skin cancer.


14 Which of the following compounds shows geometric (E-Z or cis-trans) isomerism?

A but-1-ene

B 2-methylbut-1-ene

C but-2-ene

D 2-methylbut-2-ene


15 What is the systematic name for the compound with the following formula?

CH3CH CHCH3

CH3 CH2CH3

A 2-methyl-3-ethylbutane

B 1,2,3-trimethylbutane

C 2,3-dimethylpropane

D 2,3-dimethylpentane



7


16 This question is about the reaction of methane with bromine in sunlight.(1)

CH4 + Br2 � CH3Br + HBr

(a) This reaction is best described as

A electrophilic addition.


C free radical addition.

D free radical substitution.

(b) One of the steps in the mechanism of this reaction is(1)

•CH3 + Br• � CH3Br

This step is

A initiation.

B propagation.

C termination.

D reduction.

(c) This reaction produces a mixture of products.

Which of the following is most likely to form, as well as bromomethane?(1)

A ethane

B propane

C butane

D pentane

(d) When human skin is overexposed to sunlight, it is likely to lead to skin cancer.

What is the radiation in sunlight that leads to skin cancer?(1)

A microwaves

B infrared

C visible light

D ultraviolet


8

*P41649A0824*

17 Which equation represents the reaction for which the enthalpy change, �H, is the mean bond energy of the C-F bond?

A CF4(g) � C(g) + 4F(g)

B ¼CF4(g) � ¼C(g) + F(g)

C C(g) + 4F(g) � CF4(g)

D ¼C(g) + F(g) � ¼CF4(g)



2

*P41650A0224*

SECTION A

Answer ALL the questions in this section. You should aim to spend no more than 20 minutes on this section. For each question, select one answer from A to D and put a cross in the box . If you change your mind, put a line through the box and then mark your new answer with

a cross .

1 Which of the following molecules has the smallest bond angle?

A H2O

B NH3

C CH4

D SF6


2 A charged rod is held beside a stream of liquid coming from a burette. Which of the following liquids would NOT be significantly deflected?

A H2O

B CCl4

C C2H5OH

D C2H5Br


3 Which of the following statements about electronegativity is true?

A Non-metals have lower electronegativity than metals.

B Electronegativity decreases across a period in the Periodic Table.

C Electronegativity decreases going down a group in the Periodic Table.

D The bonds between atoms with equal electronegativity are always weak.

(Total for Question 3 = 1 mark)exem

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exem

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DRAFT

DRAFT

3


4 In which series of compounds does the covalent character increase, going from left to right?

A NaCl, MgCl2, AlCl3, SiCl4

B SiO2, Al2O3, MgO, Na2O

C LiI, NaI, KI, RbI

D KI, KBr, KCl, KF


5 Going down Group 2 from calcium to barium

A the first ionization energy of the element increases.

B the strength of the metallic bonding increases.

C the polarizing power of the 2+ ion decreases.

D the stability of the nitrate to heat decreases.


6 Fullerenes, graphite and diamond are all forms of carbon. Fullerenes dissolve in petrol, but diamond and graphite do not. This is because

A the bonds between the carbon atoms in fullerenes are weaker than in diamond or graphite.

B diamond and graphite are giant structures but fullerenes are molecular.

C there are delocalized electrons in diamond and graphite but not in fullerenes.

D there are covalent bonds in diamond and graphite, but not in fullerenes.


7 Sodium chloride is more soluble in water than in hexane because

A the intermolecular forces between water molecules are stronger than those between hexane molecules.

B hexane molecules cannot fit between the ions in the sodium chloride lattice.

C energy is released when the ions in sodium chloride are hydrated.

D sodium ions and chloride ions form hydrogen bonds with water.


exem

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DRAFT

DRAFT

4

*P41650A0424*

8 Hydrochloric acid and sodium carbonate solution react as shown below.

2HCl(aq) + Na2CO3(aq) → 2NaCl(aq) + CO2(g) + H2O(l)

Which sample of sodium carbonate solution will be neutralized by 20 cm3 of 0.05 mol dm–3 hydrochloric acid?

Volume of sodium carbonate/

cm3

Concentration of sodium carbonate/mol dm–3

A 10 0.05

B 40 0.05

C 40 0.10

D 10 0.10


9 A white solid produces oxygen when it is heated, but no other gases. The solid could be

A lithium nitrate.

B potassium nitrate.

C strontium nitrate.

D calcium oxide.


10 A solid is soluble in water and produces steamy acidic fumes with concentrated sulfuric acid. The solid could be

A potassium carbonate.

B magnesium sulfate.

C silver chloride.

D sodium chloride.

(Total for Question 10 = 1 mark)exem

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DRAFT

DRAFT

5


11

The systematic name of the compound with skeletal formula shown above is

A 1,1-dimethylethanol.

B 2,2-dimethylethanol.

C 2-methylpropan-1-ol.

D 2-methylpropan-2-ol.


12 Samples of 1-chloropropane and 1-bromopropane are warmed with water containing dissolved silver nitrate in the presence of ethanol. The 1-chloropropane reacts more slowly because

A the C—Cl bond is more polar than the C—Br bond.

B the C—Cl bond is stronger than the C—Br bond.

C 1-chloropropane is less soluble than 1-bromopropane.

D 1-chloropropane is a weaker oxidizing agent than 1-bromopropane.


13 The reaction of 1-chloropropane with water containing dissolved silver nitrate in the presence of ethanol is

A a redox reaction.

B a nucleophilic substitution.

C an electrophilic substitution.

D a free radical substitution.


OH

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DRAFT

DRAFT

6

*P41650A0624*

14 The compound with formula CH3CH(NH2)CH3 can be made by reacting alcoholic ammonia with

A propane.

B propene.

C 2-chloropropane.

D propan-2-ol.


15

The energy marked X in the Maxwell-Boltzmann distribution shows

A the most common energy of the molecules.

B the activation energy of the reaction.

C the activation energy of a catalysed reaction.

D the number of molecules with energy greater than the activation energy.



Fraction of molecules with energy, E

Energy, EX

exem

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DRAFT

DRAFT

7


16 In the industrial process involving gas phase reactions to produce ammonia, many collisions between molecules are unsuccessful because

A gas phase reactions are reversible.

B the collisions are not energetic enough to break the bonds in the molecules.

C gas phase reactions can only occur when a catalyst is present.

D gas phase reactions can only occur when UV light is present.


17 The molecular (parent) ion in the mass spectrum of a hydrocarbon containing 12C and 1H only

A is the peak with highest relative abundance.

B is the peak with highest charge.

C is the peak produced by the most stable fragment.

D is the peak with highest mass to charge ratio.


18 A compound which has major peaks with mass / charge ratio at 29, 57 and 58 in the mass spectrum could be

A propanal, CH3CH2CHO.

B propanone, CH3COCH3.

C propan-1-ol, CH3CH2CH2OH.

D propan-2-ol, CH3CH(OH)CH3.


19 Which of the following would not be used to assess whether the use of a biofuel produced from a crop of sugar cane is carbon neutral?

The amount of

A fuel used to operate farm machinery.

B pesticides and fertilisers used.

C energy released per tonne of biofuel.

D fuel used to process the crop.


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DRAFT

8

*P41650A0824*

20 The principal reason why scientists have recommended that chlorofluorocarbons (CFCs) are not used in aerosols is that they cause

A global warming.

B acid rain.

C ozone depletion.

D water pollution.



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2

*P42984A0224*

SECTION A



If you change your mind, put a line through the box and then mark your new answer

with a cross .

1 An important step in the production of sulfuric acid is the oxidation of sulfur dioxide.

2SO2(g) + O2(g) � 2SO3(g) �H = –196 kJ mol–1

Which of the conditions below is best suited to produce a high yield of sulfur trioxide, SO3?

A 1 atm pressure and 800 °C.

B 2 atm pressure and 800 °C.

C 1 atm pressure and 400 °C.

D 2 atm pressure and 400 °C.


2 Which of the following statements is true about all substances that form acidic solutions in water?

A They are corrosive.

B They are liquids.

C They contain hydrogen atoms.

D They form H+ (aq) ions.



3


3 Select the correct pH for each of the following solutions.

(a) Nitric acid, HNO3, of concentration 2 mol dm–3, assuming it is fully dissociated.(1)

A –0.3

B 0.0

C 0.3

D 2.0

(b) Sodium hydroxide, NaO H, of concentration 2 mol dm–3, using Kw = 1.0 × 10–14 mol2 dm–6

(1)

A –13.7

B 13.7

C 14.0

D 14.3

(c) Ethanoic acid, CH3COOH, of concentration 2 mol dm–3, making the usual assumptions.

Ka = [ ][ ]

[H CH COO

CH COOH]

+ −3

3 = 1.7 × 10–5 mol dm–3

(1)

A 2.2

B 2.4

C 4.5

D 4.8

(d) The mixture formed when 25 cm3 of 2 mol dm–3 sodium hydroxide solution is added to 50 cm3 of 2 mol dm–3 ethanoic acid, for which Ka = 1.7 × 10–5 mol dm–3.

(1)

A 2.2

B 2.5

C 4.5

D 4.8


4

*P42984A0424*

4 A solution of 2,4-dinitrophenylhydrazine (Brady’s reagent) is used as a test for organic functional groups.

(a) The positive result of the test is the formation of(1)

A a yellow solution.

B an orange precipitate.

C a red solution.

D a green precipitate.

(b) Which of the following gives a positive result with a solution of 2,4-dinitrophenylhydrazine?

(1)

A Only aldehydes

B Only ketones

C Only aldehydes and ketones

D Any compound containing the C O group

(c) The initial attack by 2,4-dinitrophenylhydrazine, when it reacts, is by(1)

A a free radical.

B an electrophile.

C a nucleophile.

D a negative ion.

(d) The product of a positive test, a 2,4-dinitrophenylhydrazone, contains which of the following bonds?

(1)

A N N

B C N

C C C

D C O


5


BLANK PAGE

Turn over for Question 5

6

*P42984A0624*

5 This question is about the following isomeric compounds with the molecular formula C4H8O and molar mass 72 g mol–1.

A CH3CH2CH2CHO

B (CH3)2CHCHO

C CH3CH2COCH3

D CH3CH CHCH2OH

(a) Which compound would you expect to give a peak at m/e = 41 in its mass spectrum?

(1)

A

B

C

D

(b) Which compound would NOT react with an acidified solution of potassium dichromate(VI)?

(1)

A

B

C

D

(c) Which compound would give a pale yellow precipitate when reacted with iodine in alkaline solution?

(1)

A

B

C

D

(d) Which compound can be reduced to give a chiral product?(1)

A

B

C

D

7


(e) Which compound would NOT react with hydrogen cyanide under suitable conditions to form a hydroxynitrile?

(1)

A

B

C

D


6 Transesterification involves the conversion of

A esters into different esters.

B esters into carboxylic acids.

C cis carbon-carbon double bonds to the trans arrangement.

D trans carbon-carbon double bonds to the cis arrangement.


7 Biodiesel is formed by transesterification. It is used as a fuel in preference to untreated vegetable oils because

A on combustion, biodiesel produces less carbon dioxide than vegetable oils.

B on combustion, biodiesel produces more energy than vegetable oils.

C biodiesel vaporises more easily than vegetable oils.

D biodiesel is less volatile than vegetable oils.


8 The main reason for hardening vegetable oils when producing low-fat spreads is to

A prevent oxidation.

B make the oil less viscous.

C increase the melting temperature.

D decrease the cholesterol content.


8

*P42984A0824*

9 Which atoms are not detected by X-rays but are detected by nuclear magnetic resonance imaging which also shows their environments?

A Carbon

B Hydrogen

C Nitrogen

D Oxygen


10 In one type of high-performance liquid chromatography (HPLC), the stationary phase is non-polar and a polar solvent is used as the eluent. Which of the following would travel through the chromatography column most quickly?

A Tetrachloromethane

B Chloromethane

C Iodomethane

D Hexane



2

*P42982A0224*

SECTION A




a cross .

1 The first five ionization energies of an element, X, are

578, 1817, 2745, 11578 and 14831 kJ mol–1, respectively.

In which group of the Periodic Table is X found?

A 1

B 2

C 3

D 4


2 Which of the following oxides would be expected to have the most exothermic lattice energy?

A Na2O

B MgO

C CaO

D K2O


3 In which of the following compounds is the anion most polarized?

A LiF

B LiI

C KF

D KI


3


4 In the Born-Haber cycle for potassium iodide, which of the following steps is exothermic?

A K(s) � K(g)

B K(g) � K+(g) + e–

C ½I2(s) � I(g)

D I(g) + e– � I–(g)


5 Which of the following represents a pair of isotopes?

A 146C and 14

7N

B 3216S and 32

16S2–

C O2 and O3

D 20682Pb and 208

82Pb


6 Which of the following equations represents the second ionization energy of chlorine?

A Cl+(g) � Cl2+(g) + e–

B Cl(g) � Cl2+(g) + 2e–

C Cl(g) � Cl2–(g) − 2e–

D Cl–(g) � Cl2–(g) − e–


7 For Period 3 of the Periodic Table, from sodium to argon, what is the trend in the melting temperatures of the elements?

A A steady decrease

B A steady increase

C A decrease to silicon then an increase

D An increase to silicon then a decrease


4

*P42982A0424*

8 Given the following information

CH4(g) � C(g) + 4H(g) �H = +Q kJ mol–1

the mean bond enthalpy for the C–H bond in methane is

A +Q

B +Q/4

C –Q

D –Q/4


9 Consider the following information:

Bond Bond enthalpy / kJ mol–1

H–H +436

I–I +151

H–I +299

For the reaction

H2(g) + I2(g) � 2HI(g)

the enthalpy change, in kJ mol–1, is

A +288

B +144

C –11

D –5.5


5


10 The equation for the complete combustion of butanone, C2H5COCH3, is

C2H5COCH3(l) + 5½O2(g) � 4CO2(g) + 4H2O(l) �H� = –2440 kJ mol–1

Substance �Hf� / kJ mol–1

CO2(g) –394

H2O(l) –286

From the above data, the standard enthalpy change of formation of butanone, in kJ mol–1, is

A –280

B +280

C –1760

D +1760


11 A compound was found to contain 2.8 g of nitrogen and 8.0 g of oxygen.

What is the empirical formula of the compound?

Use the Periodic Table as a source of data.

A NO

B NO2

C N2O3

D N2O5


12 What is the total number of atoms in 1.8 g of water, H2O?

DATA � The molar mass of H2O is 18 g mol–1

� The Avogadro Constant is 6.0 × 1023 mol–1

A 6.0 × 1022

B 6.0 × 1023

C 1.8 × 1023

D 1.8 × 1024


6

*P42982A0624*

13 Phosphorus(V) chloride, PCl5, reacts with water according to the equation

PCl5(s) + 4H2O(l) � H3PO4(aq) + 5HCl(aq)

If 1.04 g of phosphorus pentachloride (molar mass = 208 g mol–1) is reacted completely with water and the solution made up to 1 dm3, the concentration of the hydrochloric acid in mol dm–3 is

A 0.001

B 0.005

C 0.025

D 0.250


14 A sample of sodium chlorate(V), NaClO3, was heated and 120 cm3 of oxygen gas was collected.

2NaClO3(s) � 2NaCl(s) + 3O2(g)

Calculate the number of moles of sodium chlorate(V) that were decomposed in the above reaction.

[Molar volume of a gas under the conditions of the experiment = 24000 cm3 mol–1]

A 2.50 × 10–3

B 3.33 × 10–3

C 5.00 × 10–3

D 7.50 × 10–3


15 In the ethene molecule, the C=C double bond is made up of

A two sigma bonds.

B one pi bond.

C two pi bonds.

D one sigma bond and one pi bond.


7


16 3.0 dm3 of sulfur dioxide reacts with 1.5 dm3 of oxygen, under suitable conditions, according to the equation below.

2SO2(g) + O2(g) � 2SO3(g)

What is the maximum volume of sulfur trioxide that can be formed in the above reaction?

[The volumes of the gases are measured at the same temperature and pressure.]

A 6.0 dm3

B 4.5 dm3

C 3.0 dm3

D 1.5 dm3


17 Which of the following alkenes exhibits E / Z isomerism?

A But-1-ene

B But-2-ene

C 2-Methylpropene

D Propene


18 An electrophile is defined as a species that

A is an electron pair acceptor.

B is an electron pair donor.

C has a negative charge.

D has a positive charge.


8

*P42982A0824*

19 The repeat unit of a polymer is shown below.

C C

CH3

H

⎡

⎣⎢ ⎡

⎣⎢

CH3

CH2CH3

The systematic name of the alkene monomer that forms this polymer is

A 2-methyl-3-ethylpropene

B 2-methylpent-2-ene

C 2-methylpent-3-ene

D 4-methylpent-2-ene


20 Cracking crude oil

A separates the mixture into pure compounds.

B separates the mixture into a number of fractions.

C separates saturated compounds from unsaturated ones.

D decreases the average number of carbon atoms per molecule.



2

*P42983A0220*

SECTION A




a cross .

1 Which of the following could be used to oxidize ethanol to ethanoic acid?

A Concentrated H2SO4

B H+/Cr2O72–

C H+/Cr3+

D Concentrated NaOH solution


2 The term “reflux” is best described as

A continuous evaporation and condensation.

B heating to evaporation and separation.

C heating under reduced pressure and separation.

D constant boiling.


3 The alcohol shown below can be classified as

OH

OH

A just primary.

B primary and secondary.

C just secondary.

D secondary and tertiary.


3


4

C2H5Br + NaOH � C2H4 + NaBr + H2O

This reaction is an example of

A addition.

B elimination.

C hydrolysis.

D oxidation.


5 Which of the following is not a greenhouse gas?

A H2O

B NO

C CH4

D O2


6 Which type of radiation is absorbed by molecules and results in the greenhouse effect?

A Infrared

B Microwave

C Ultraviolet

D X-ray


7 It is important to lower the level of carbon dioxide in the atmosphere because of concerns over which environmental problem?

A Acid rain

B Global warming

C Non-biodegradability

D Ozone depletion


4

*P42983A0420*

8 The meaning of homolytic fission is

A bond-breaking to form two free radicals.

B bond-making to form two free radicals.

C bond-breaking to form a cation and an anion.

D bond-making to form a cation and an anion.


9 What are the strongest forces between molecules of hydrogen fluoride, HF?

A Dipole-dipole forces.

B Hydrogen bonds.

C Ionic interactions.

D London forces.


10 The diagram below is taken from a student’s examination paper. It shows the hydrogen bonding between two water molecules.

Identify the error in the diagram.

A The H–O–H bond angle within each water molecule should be 90�.

B There should only be one lone pair of electrons on each oxygen atom.

¨ C The O–H–O bond angle between the water molecules should be 180�.

D The hydrogen atoms should be �– and the oxygen atoms should be �+.


5


11 The boiling temperatures from methane to propane increase because

A the number of ions increases, so there are stronger electrostatic attractions.

B the covalent bonds are getting stronger, so require more energy to break.

C there are more covalent bonds, so more energy is needed to break them.

D the number of electrons increases, so there are stronger London forces.


12 In a chemical reaction, which of the following factors increases the proportion of particles that have sufficient energy to react?

A A decrease in concentration

B An increase in concentration

C A decrease in temperature

D An increase in temperature


13 A ‘greener’ chemical process will be one that

A uses energy less efficiently.

B forms a non-polluting waste product.

C produces significant amounts of waste.

D makes use of non-renewable resources.


14 Which of the following cannot alter the position of a chemical equilibrium?

A Increasing the amount of catalyst

B Increasing the reactant concentration

C Increasing the temperature

D Increasing the total pressure


6

*P42983A0620*

15 CO(g) + 2H2(g) ��CH3OH(g) �H = –91 kJ mol–1

The conditions which would produce the greatest yield of methanol are

A high pressure and high temperature.

B high pressure and low temperature.

C low pressure and low temperature.

D low pressure and high temperature.


16 What is the oxidation number of chlorine in Cl2O7?

A –1

B +1

C –7

D +7


17 The concentration of a solution of potassium iodate(V) can be determined by the liberation of iodine, followed by titration with sodium thiosulfate.

A suitable indicator is

A methyl orange.

B phenolphthalein.

C starch.

D universal indicator.


7


18 The thermite reaction, shown below, is a useful industrial process.

Fe2O3(s) + 2Al(s) � 2Fe(l) + Al2O3(s)

The iron in this reaction undergoes

A disproportionation.

B oxidation.

C redox.

D reduction.


19 Which of the following molecules has a linear shape and bond angles of 180�?

A CH4

B H2O

C CO2

D SF6


20 What would be the experimental observations if chlorine gas was bubbled through potassium iodide solution, followed by the addition of cyclohexane?

A The solution turns brown, then two layers are produced and the top layer is purple.

B A white precipitate is formed, which then dissolves to leave a colourless solution.

C Bubbles of gas are seen and then a brown precipitate is formed.

D The solution remains colourless, and then two layers are seen with the bottom layer being brown.



2

*P41572A0224*

SECTION A




a cross .

1 The overall equation for a reaction between two chemicals, M and N, is

M + 2N � P + Q

(a) This reaction occurs spontaneously at room temperature. Which of the following must be true?

(1)

A �H �reaction is positive.

B �H �reaction is negative.

C �S �total is positive.

D �S �total is negative.

(b) The reaction above occurs in two stages via an intermediate, T.

M + N � T slow

N + T � P + Q fast

From this it can be deduced that the rate equation for the reaction between M and N is

(1)

A rate = k[M][N]

B rate = k[M][N]2

C rate = k[M][T]

D rate = k[N][T]



3


2 Calcium carbonate decomposes at high temperature to form calcium oxide and carbon dioxide:

CaCO3(s) � CaO(s) + CO2(g)

Calcium carbonate is thermodynamically stable at room temperature because for this reaction

A the activation energy is high.

B the enthalpy change, �H, is positive.

C entropy change of the system (�Ssystem) is positive.

D entropy change of the system (�Ssystem) is negative.


3 2-methylpropane has a smaller standard molar entropy at 298 K than butane. The best explanation for this is that 2-methylpropane has

A a lower boiling temperature.

B a higher standard molar enthalpy change of formation.

C fewer ways of distributing energy quanta.

D more ways of distributing energy quanta.



4

*P41572A0424*

4 (a) For the equilibrium reaction between hydrogen and iodine

H2(g) + I2(g) � 2HI(g)

increasing the pressure of the system(1)

A has no effect on the rate or the position of equilibrium.

B increases the rate but does not affect the position of equilibrium.

C increases the rate and shifts the equilibrium to the right.

D increases the rate and shifts the equilibrium to the left.

(b) The equation for the equilibrium reaction between hydrogen and iodine may also be written as

½H2(g) + ½I2(g) � HI(g)

This change to the equation, compared to that in part (a),(1)

A has no effect on the value of the equilibrium constant.

B halves the value of the equilibrium constant.

C doubles the value of the equilibrium constant.

D square roots the value of the equilibrium constant.



5


5 The first stage in the manufacture of nitric acid is the oxidation of ammonia:

4NH3(g) + 5O2(g) � 4NO(g) + 6H2O(g) �H = –906 kJ mol–1

(a) In modern industrial plants this reaction is carried out at a pressure of around 3 atm. Which of the following statements is incorrect? The raised pressure

(1)

A helps push the reactants through the reactor.

B shifts the position of equilibrium to the right.

C increases the cost of the reactor.

D increases the energy cost of this part of the process.

(b) A platinum-rhodium alloy catalyst is used in this reaction. Which of the following statements is incorrect? The catalyst

(1)

A lowers the activation energy of the reaction.

B has no effect on the equilibrium constant for the reaction.

C alters the enthalpy change of the reaction.

D reduces the energy cost of this part of the process.

(c) The operating temperature of this reaction is about 900�C. The use of a high temperature

(1)

A increases the rate of the reaction and the equilibrium yield.

B increases the rate of the reaction and decreases the equilibrium yield.

C decreases the rate of the reaction and the equilibrium yield.

D decreases the rate of the reaction and increases the equilibrium yield.



6

*P41572A0624*

6 Ammonium chloride decomposes on heating:

NH4Cl(s) � NH3(g) + HCl(g)

The equilibrium constant, Kp, for this reaction equals

A P PNH HCl3×

B 1

3P PNH HCl×

C P P

PNH HCl

NH Cl

3

4

×

D P

P PNH Cl

NH HCl

4

3×


7 The dissociation constant of water, Kw, increases with increasing temperature. When the temperature increases, water

A remains neutral.

B dissociates less.

C becomes acidic.

D becomes alkaline.


8 The reaction between concentrated sulfuric acid and pure ethanoic acid is

CH3COOH + H2SO4 � CH3COOH2+ + HSO4¯

The Brønsted-Lowry acids in this equilibrium are

A CH3COOH and H2SO4

B CH3COOH2+ and HSO4

–

C H2SO4 and CH3COOH2+

D CH3COOH and HSO4–


7


9 An aqueous solution of ethanoic acid is gradually diluted. Which of the following statements is incorrect?

A The pH decreases.

B The value of Ka is unchanged.

C The concentration of ethanoic acid molecules decreases.

D The proportion of ethanoic acid molecules which dissociates increases.


10 Methyl orange and phenolphthalein are both acid-base indicators. In the titration of a strong acid against a weak alkali

A methyl orange is a suitable indicator but phenolphthalein is not.

B phenolphthalein is a suitable indicator but methyl orange is not.

C both phenolphthalein and methyl orange are suitable indicators.

D neither phenolphthalein nor methyl orange is a suitable indicator.


11 Select the word that best describes the effect of a chiral molecule on the plane of plane-polarized light. The plane of polarization of light is

A reflected.

B refracted.

C resolved.

D rotated.


12 An organic compound reacts with both acidified potassium dichromate(VI) and lithium tetrahydridoaluminate (lithium aluminium hydride). The organic compound could be

A a primary alcohol.

B an aldehyde.

C a ketone.

D a carboxylic acid.


8

*P41572A0824*

13 Ketones react with

A both 2,4-dinitrophenylhydrazine solution and Tollens’ reagent.

B 2,4-dinitrophenylhydrazine solution but not with Tollens’ reagent.

C Tollens’ reagent but not with 2,4-dinitrophenylhydrazine solution.

D neither Tollens’ reagent nor 2,4-dinitrophenylhydrazine solution.


14 Ethanoic acid, CH3COOH, may be prepared from ethanenitrile, CH3CN. This reaction is best described as

A reduction.

B oxidation.

C hydrolysis.

D condensation.


15 Propanoic acid reacts with methanol to form an ester. The structure of the ester is

A H O C C C C H

O H

H

H

H

H

H

B

C C C H

H H

HH O

O

H C H

H

C H C C O C C H

OH

H

H

H

H

H

D H C C C O C H

OH

H

H

H

H

H


9


16 The boiling temperature of ethanoic acid is very much higher than that of butane although these molecules have similar numbers of electrons. This is because ethanoic acid has

A stronger covalent bonds.

B stronger ionic bonds.

C greater London forces.

D hydrogen bonding.



10

*P41572A01024*

SECTION B

Answer ALL the questions. Write your answers in the spaces provided.

17 The equation for the combustion of hydrogen is

H2(g) + ½O2(g) � H2O(l)

(a) Use the standard molar entropies on page 2 and page 25 of the data booklet to calculate the standard entropy change of the system (�S�system) for this reaction.

Note that the standard molar entropies of the elements are given per atom so that the standard molar entropy of oxygen, S�[½O2(g)] = +102.5 J mol–1 K–1.

(3)

(b) The standard enthalpy change for the combustion of hydrogen is –285.8 kJ mol–1. Use this value to calculate the entropy change of the surroundings for the combustion of hydrogen at 298 K. Give your answer to 3 significant figures and include a sign and units.

(3)

11


(c) Use your answers to (a) and (b) to calculate the total entropy change (�S�total) for the combustion of 1 mol of hydrogen. Include a sign and units in your answer.

(2)

*(d) By considering both the thermodynamic stability and the kinetic inertness of a mixture of hydrogen and oxygen, explain why hydrogen does not react with oxygen unless ignited.

(2)

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2

*P42970A0224*

SECTION A




a cross .

1 The correct sequence for the processes that occur in a mass spectrometer is

A vaporization, ionization, acceleration, deflection and detection.

B vaporization, acceleration, ionization, deflection and detection.

C ionization, vaporization, acceleration, deflection and detection.

D ionization, vaporization, deflection, acceleration and detection.

(Total for Question = 1 mark)

2 Which of the following ions would be deflected most in a mass spectrometer?

A 35Cl+

B 37Cl+

C 37Cl2+

D (35Cl —37Cl)+


3 A particle with a single positive charge and with the electronic configuration 1s2 2s2 2p6 is

A a sodium ion.

B a fluoride ion.

C an oxide ion.

D a potassium ion.


3


4 In which of the following electronic configurations are only two of the electrons unpaired?

A 1s2 2s2

B 1s2 2s2 2p3

C 1s2 2s2 2p4

D 1s2 2s2 2p5


5 Which of the following contains a dative covalent bond?

A N2

B NH3

C NH2–

D NH4+


6 Which of the following ions has the largest ionic radius?

A F–

B Mg2+

C Na+

D O2–


7 Which of the following observations provides the best evidence for the presence of ionic bonding in an unknown substance?

The substance conducts electricity

A in the solid state.

B in the solid state and in aqueous solution.

C in the solid state and when molten.

D when molten but not in the solid state.


4

*P42970A0424*

8 Which of the following can be determined, for an unknown alkene, using only

percentage composition by mass data?

A Molecular formula

B Empirical (simplest) formula

C Both the molecular formula and the empirical (simplest) formula

D Structural formula


9 1.12 g of iron reacts with oxygen to form 1.60 g of an oxide of iron. Use relative atomic masses: Fe = 56, O = 16.

What is the formula of this oxide of iron?

A FeO5

B Fe2O10

C Fe3O2

D Fe2O3


10 In an experiment, 1.226 g of potassium chlorate(V), KClO3, was heated. A mass of 0.320 g of oxygen gas, O2, was collected.

2KClO3(s) 2KCl(s) + 3O2(g)

Use the molar mass of KClO3 = 122.6 g mol−1 and relative atomic mass O = 16.

The percentage yield of oxygen in this experiment is

A 17.4%

B 26.1%

C 66.7%

D 100%


5


11 Oxygen gas, O2, can be converted into ozone, O3, by passing it through an electric discharge.

3O2(g) 2O3(g)

In an experiment, a volume of 300 cm3 of oxygen was used but only 10% of the oxygen was converted into ozone. All volumes were measured at the same temperature and pressure.

The total volume of gas present at the end of the experiment, in cm3, was

A 200

B 210

C 290

D 300


12 1.40 g of an alkene gave 3.77 g of a dichloroalkane on reaction with chlorine.

What is the molecular formula of the alkene?

A C2H4

B C3H6

C C4H8

D C6H12


13 The standard enthalpy change for the combustion of graphite is –393.5 kJ mol−1 and that of diamond is –395.4 kJ mol–1.

What is the standard enthalpy change for the reaction below, in kJ mol−1?

C(s, graphite) C(s, diamond)

A –1.9

B +1.9

C –788.9

D +788.9


6

*P42970A0624*

14 The standard enthalpy change of neutralization when an acid reacts with an alkali is the number of kilojoules released by the

A formation of one mole of salt.

B formation of one mole of water.

C neutralization of one mole of acid.

D neutralization of one mole of alkali.


15 Consider the following bond enthalpy values.

Bond Bond enthalpy / kJ mol–1

O O +146

O H +463

O O +496

For the reaction

H O O H(g) H O H(g) + ½O O(g)

the enthalpy change, in kJ mol–1, is

A –102

B +102

C +350

D +394



7


16 Using the data in the table below, calculate the standard enthalpy change, in kJ mol–1, for the reaction between carbon disulfide, CS2, and oxygen shown in the following equation.

CS2(g) + 3O2(g) CO2(g) + 2SO2(g)

Substance Standard enthalpy change of formation, Hf / kJ mol–1

CS2(g) +110

CO2(g) –390

SO2(g) –290

A –570

B –790

C –860

D –1080


17 (a) Which of the following represents a step in the mechanism during the reaction between ethene and hydrogen bromide?

(1)

A C2H4 + Br+ C2H4Br+

B C2H4 + HBr C2H5+ + Br–

C C2H4 + HBr C2H5 + Br

D C2H4 + HBr C2H4Br– + H+

(b) The mechanism of the reaction between ethene and hydrogen bromide is(1)

A electrophilic addition.


C nucleophilic addition.

D nucleophilic substitution.


8

*P42970A0824*

18 Which of the following pairs are cis-trans isomers?

1 2 3 4

A 1 and 2

B 1 and 4

C 2 and 3

D 3 and 4


19 What is the systematic name for the hydrocarbon shown below?

A 1,4-dimethylbutane

B 2,3-dimethylbutane

C 2,3-dimethylhexane

D 1,1,2,2-tetramethylethane



H

ClHC C

Cl Cl

HHC C

Cl H

HClC C

Cl Cl

HClC C

H

CH3

CH3

CH3CHCHCH3

2

*P42990A0228*

SECTION A




a cross .

1 Which of the following diagrams represents the electrons in the ground state of a boron atom?

1s 2s 2px 2py 2pz

A

B

C

D


2 Which of the following species contains the same number of electrons as neutrons?

A 511B

B 1123Na+

C 1224Mg2+

D 919F–


3 The recommended limit for safe exposure to sulfur dioxide in the air is 0.000025 %. What is this concentration in parts per million, ppm?

A 25

B 0.25

C 0.025

D 0.0025


3


4 For which of the following pairs of elements does the second have a higher 1st ionization energy than the first?

First element Second element

A Mg Al

B N O

C Ne Na

D K Na


5 In which of the following series of elements is there an increase in the melting temperatures from left to right?

A Na Mg Al

B Li Na K

C B C N

D Si P S


6 What is the number of atoms in 2.8 g of ethene, C2H4?

DATA

The molar mass of C2H4 is 28 g mol–1

The Avogadro constant is 6.0 × 1023 mol–1

A 1.0 × 1022

B 6.0 × 1022

C 1.2 × 1023

D 3.6 × 1023


4

*P42990A0428*

7 A compound has the following percentage composition by mass.

C 61.0% H 15.3% N 23.7%

The empirical formula of the compound is

A CH3N

B C3H9N

C C6H9N2

D C8H2N3


8 Carbon monoxide and oxygen react together as follows.

2CO(g) + O2(g) 2CO2(g)

If all volumes of gas are measured at the same temperature and pressure, the volume of carbon dioxide produced after 50 cm3 of carbon monoxide react with 25 cm3 of oxygen is

A 100 cm3

B 75 cm3

C 50 cm3

D 25 cm3


9 Potassium chlorate(V), KClO3, decomposes on heating as follows.

2KClO3(s) 2KCl(s) + 3O2(g)

What is the maximum volume of oxygen, measured in dm3 at room temperature and pressure, which could be obtained by heating 0.50 mol potassium chlorate(V)?

[Molar volume of a gas = 24 dm3 mol–1 at room temperature and pressure.]

A 8

B 18

C 36

D 72


5


10 A spot of blue solution was placed in the centre of a piece of moist filter paper supported on a microscope slide and the following experiment was carried out.

After some time, a blue colour moved towards the negative terminal, but no change was visible in the region of the positive terminal. This is because

A the negative ions in the solution were colourless and the positive ions were blue.

B the positive ions in the solution were colourless and the negative ions were blue.

C the negative ions in the solution had not moved but the positive ions had moved.

D the positive ions in the solution had not moved but the negative ions had moved.


11 The reaction for which the enthalpy change is the standard enthalpy change of formation of water, Hf,298, is

A H2(g) + ½O2(g) H2O(l)

B H2(g) + ½O2(g) H2O(g)

C 2H2(g) + O2(g) 2H2O(l)

D 2H2(g) + O2(g) 2H2O(g)


DC supply

moist filter paper on

microscope slideposition of

blue solution at start

+ –

6

*P42990A0628*

12 Which of the following molecules does not contain a double bond?

A CO2

B C2Cl4

C C3F8

D C2H2Cl2


13 The bonding in lithium iodide has some covalent character because

A the lithium ion polarizes the iodide ion.

B the iodide ion polarizes the lithium ion.

C there is a very large difference in electronegativity between lithium and iodine.

D there is a very small difference in electronegativity between lithium and iodine.


14 Which of the following data is not needed to calculate the lattice energy of sodium chloride when using a Born-Haber cycle?

A Enthalpy change of formation of sodium chloride.

B Enthalpy change of atomization of sodium.

C First ionization energy of chlorine.

D Electron affinity of chlorine.


15 The lattice energy of magnesium oxide is more negative than the lattice energy of magnesium fluoride because

A oxide ions are larger than fluoride ions.

B oxide ions are larger than magnesium ions.

C oxide ions are more highly charged than fluoride ions.

D there is only one oxide ion but two fluoride ions per magnesium ion.


7


16 This question is about the organic compounds shown below.

(a) The compounds which are isomers are(1)

A W and X

B W and Y

C W and Z

D X and Z

(b) Which compound can react with chlorine to form C6H12Cl2 as the only product?(1)

A Compound W

B Compound X

C Compound Y

D Compound Z

(c) Which compound is reformed in the oil industry, producing one mole of a compound with formula C6H6 and four moles of hydrogen, H2, only?

(1)

A Compound W

B Compound X

C Compound Y

D Compound Z



W X Y Z

8

*P42990A0828*

17 Which of the following equations shows the first step in the mechanism for the reaction between hydrogen bromide and ethene?

A

B

C

D



C C

H

H

H

HH

Br

H C C H + Br–

H

H

H

+

C C

H

H

H

HBr

H

H C C H + H+

H

Br

H

–

C C

H

H

H

HH

Br

H C C H + Br–

H

H

H

+

C C

H

H

H

HBr

H

H C C H + H+

H

Br

H

–

9


18 Scientists are developing sources of energy as alternatives to fuels produced from crude oil. Which of the following reasons for doing this is incorrect?

A Crude oil is being used up faster than it is being formed.

B Burning hydrocarbons affects global carbon dioxide levels.

C Hydrocarbons from crude oil are a source of essential chemicals other than fuels.

D Carbon dioxide produced by burning hydrocarbons is toxic to plants.



2

*P42971A0224*

SECTION A




a cross .

1 When sodium is added to ethanol, which of the following observations would be made?

A Colour change of orange to green

B Effervescence

C Yellow flame

D No change


2 Which of the following substances does not have intermolecular hydrogen bonds?

A Ethanoic acid, CH3COOH

B Propanone, CH3COCH3

C Methanol, CH3OH

D Water, H2O


3 Which of the following molecules has the lowest boiling temperature?

Pentane C3H6

A B C D

A

B

C

D


3


4 Which of the following molecules has the highest melting temperature?

A B C D

A

B

C

D


5 Which of the following isomeric alcohols, with molecular formula C5H12O, can be oxidized to a carboxylic acid with five carbon atoms?

A

OH

B

OH

C

OH

D OH


4

*P42971A0424*

6 Consider the infrared spectrum shown below.

The IR absorption ranges associated with some organic functional groups are given below.

O–H stretching in alcohols (variable, broad) 3750 – 3200 cm–1

O–H stretching in carboxylic acids (weak) 3300 – 2500 cm–1

C=O stretching in aldehydes (strong) 1740 – 1720 cm–1

C=O stretching in ketones (strong) 1700 – 1680 cm–1

C=O stretching in carboxylic acids, alkyl (strong) 1725 – 1700 cm–1

C–H stretching in aldehydes (weak) 2900 – 2820 cm–1 and 2775 – 2700 cm–1

Which of the following could have produced the above spectrum?

A An aldehyde

B An alcohol

C A carboxylic acid

D A ketone


Wavenumber / cm–1

Transmittance / %

4000 3000 2000 1500 1000 500

100

50

0

5


7 In a mass spectrum of butane, C4H10, where would a peak be seen for the molecular ion if it had a charge of 2+?

A 29

B 56

C 58

D 60


8 When a flame test is carried out on calcium iodide, the colour of the flame is

A yellow-red.

B pale green.

C purple.

D crimson.


9 The indicator methyl orange is a weak acid and may be represented by the formula HA(aq). The equation for its dissociation is shown below.

HA(aq) A–(aq) + H+(aq)

Colour: Red Yellow

Under certain conditions, at equilibrium, a solution of HA has a yellow colour. On addition of a small volume of dilute sodium hydroxide, the colour of this solution would

A change from yellow to red.

B change from yellow to orange.

C change from yellow to orange and then to red.

D not change.


6

*P42971A0624*

10 Consider the following Group 2 compounds.

Group 2 hydroxides Group 2 sulfates

Mg(OH)2 MgSO4

Ca(OH)2 CaSO4

Sr(OH)2 SrSO4

The solubility

A increases down the group for both hydroxides and sulfates.

B increases down the group for hydroxides but increases up the group for sulfates.

C increases up the group for hydroxides but increases down the group for sulfates.

D increases up the group for both hydroxides and sulfates.


11 Which of the following is the correct equation for the decomposition of the corresponding nitrate?

A 4LiNO3 2Li2O + 4NO2 + O2

B 4NaNO3 2Na2O + 4NO2 + O2

C Mg(NO3)2 Mg(NO2)2 + O2

D Ba(NO3)2 Ba(NO2)2 + O2


12 What is the oxidation number of phosphorus in P4O6?

A +3

B +4

C +5

D +6


7


13 For barium, the third ionization energy is higher than the second ionization energy because

A there is an increase in the number of protons.

B there is an increase in the shielding.

C the ionic radius is greater.

D the electron being removed is closer to the nucleus.


14 The reaction profile for an endothermic reaction is shown below.

(a) Which arrow represents the activation energy for the forward reaction?(1)

A

B

C

D

(b) Which arrow represents the activation energy for the backward reaction?(1)

A

B

C

D


Energy

Products

Reactants

A

B

C

D

Progress of reaction

8

*P42971A0824*

15 Consider the Maxwell-Boltzmann distribution of energies for a gas shown below. Ea represents the activation energy.

The shaded area of the diagram indicates the total number of particles that

A do have enough energy to react.

B do not have enough energy to react.

C do have enough energy to react in the presence of a catalyst.

D do not have enough energy to react in the presence of a catalyst.


16 Which of the following is a pure form of carbon that has both hexagonal and pentagonal rings in its structure and can conduct electricity?

A Charcoal

B Buckminsterfullerene

C Diamond

D Graphite


17 Hydrogen, H2, is not a completely ‘carbon neutral’ fuel. Which of the following is an incorrect reason for this?

A Some CO2 is released in the transportation of H2 fuel.

B CO2 is made when the electricity is generated for the manufacture of H2.

C A small amount of CO2 is produced on the combustion of H2 fuel.

D CO2 is released during the construction of the H2 manufacturing plant.


Number of particles with energy, E

Energy, E

Ea

9


18 When steam is passed over heated magnesium, which of the following occurs?

A Mg + H2O MgO + H2

B Mg + H2O MgOH + ½H2

C Mg + 2H2O Mg(OH)2 + H2

D There is no reaction with the magnesium.


19 Which of the following will not affect the rate of the reaction below?

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

A Surface area

B Concentration

C Pressure

D Temperature



2

*P42991A0224*

SECTION A




a cross .

1 This question concerns the shapes of the hydrides of Group 5 elements.

(a) What is the approximate H N H bond angle in the ammonium ion, NH4+?

(1)

A 90°

B 104.5°

C 107°

D 109.5°

(b) Suggest the shape of the phosphine molecule, PH3.(1)

A Trigonal planar

B Trigonal pyramidal

C Trigonal bipyramidal

D Octahedral


2 Graphite has a structure containing layers of carbon atoms in hexagonal rings. Why is graphite a good conductor of electricity?

A It has delocalized ions which can move and carry charge.

B It has delocalized electrons which are mobile.

C There are only weak London forces between the layers.

D Each carbon atom in the layers has only three covalent bonds.


3


3 The following system was allowed to reach equilibrium at 300 °C.

2HI(g) H2(g) + I2(g) H = 53.0 kJ mol–1

Colourless Colourless Purple

(a) What would you see if the equilibrium mixture was cooled to 250 °C?(1)

A No visible change.

B The colour gets lighter.

C The mixture turns colourless.

D The mixture goes a darker purple.

(b) The equilibrium mixture at 300 °C was compressed in a gas syringe to occupy a smaller volume. What would be seen immediately?

(1)




D The mixture goes a darker purple.


4 A solution of iodine in aqueous potassium iodide is brown. The following equilibrium exists in this solution.

I2(aq) + H2O(l) IO (aq) + I (aq) + 2H+(aq)

Brown Colourless

What would be the effect, if any, on the colour of the solution if five drops of dilute sodium hydroxide solution were added to 5 cm3 of the iodine solution?




D The mixture goes a darker colour.


4

*P42991A0424*

5 The skeletal formulae of some 6-carbon bromoalkanes are shown below.

A B C D

(a) Which of the above bromoalkanes is not a structural isomer of the others?(1)

A

B

C

D

(b) Which of the above is not a secondary bromoalkane?(1)

A

B

C

D



BrBr

BrBr

5


6

The molecule shown above is 3-chloro-3-methylhexane. It reacts with hot, alcoholic potassium hydroxide to produce a number of different alkenes. This reaction can be classified as

A elimination.

B oxidation.

C reduction.

D substitution.


7 A reaction mechanism is shown below.

The hydroxide ion is acting as

A an electrophile.

B a catalyst.

C a free radical.

D a nucleophile.


8 Which of the following reagents gives a positive result with a tertiary alcohol?

A Acidified potassium dichromate(VI) solution

B Phosphorus(V) chloride

C Dilute sulfuric acid

D Bromine water


Cl

:OH–

:Br–H3C C + Br –

CH3

CH3

H3C C+

CH3

CH3

H3C C CH3 + :Br–

CH3

OH

6

*P42991A0624*

9 What effect does infrared radiation have on the covalent bonds in water molecules in the atmosphere?

A They are broken to form free radicals.

B They are broken into ions.

C The bonds vibrate more vigorously.

D There is no effect on the bonds.


10 Alkanes are now being used as aerosol propellants as an alternative to CFCs. Although they have no effect on the ozone layer, they have the disadvantage of

A having high reactivity.

B being hard to evaporate.

C being greenhouse gases.

D having an unpleasant smell.


11 One definition of the term ‘carbon footprint’ is

‘the amount of carbon dioxide produced when a fuel is burned.’

Fuel Energy density / MJ l–1 CO2 produced on combustion / g l–1

Paraffin 46 2580

Given the information above, what is the carbon footprint for paraffin in terms of grams of CO2 produced per MJ of energy?

A 46

B 56.09

C 2580

D 118 680


7


12 The diagram below shows the Maxwell-Boltzmann distribution of molecular energies for a catalysed reaction.

(a) If the temperature were lowered, what would be the effect on the shape of the curve?

(1)

A The peak would shift to the left and be higher.

B The peak would shift to the left and be lower.

C The peak would shift to the right and be higher.

D The peak would shift to the right and be lower.

(b) Which of the following would shift the activation energy line to the right?(1)

A An increase in reactant concentration.

B The removal of the product.

C The removal of the catalyst.

D The use of smaller particles with a larger surface area.



Number of molecules with energy, E

Ea

Energy, E

8

*P42991A0824*

13 Which of the arrows, A, B, C, D, indicates the activation energy for a catalysed reaction on the reaction profile shown?

A

B

C

D



A CO2

B SO2

C SO3

D O2



Energy Reactants

Products

A

B C

D

Progress of reaction

9


15 Although they have the same relative molecular mass, the boiling temperatures of hexane (69 °C) and 2,2-dimethylbutane (49 °C) are significantly different. The reason for this is that

A the intermolecular forces are stronger between hexane molecules because it has more electrons.

B there are significantly stronger permanent dipole forces between hexane molecules.

C the covalent bonds in hexane are stronger and so it requires more energy to break them.

D the molecular shape of hexane molecules allows them to form stronger London forces.


16 Which of the following reactions is the most likely to occur with chlorine in hot, concentrated sodium hydroxide solution?

A Cl2 + 2NaOH NaCl + NaClO + H2O

B 2Cl2 + 4NaOH 3NaCl + NaClO2 + 2H2O

C 3Cl2 + 6NaOH 5NaCl + NaClO3 + 3H2O

D 4Cl2 + 8NaOH 7NaCl + NaClO4 + 4H2O



2

*P42972A0224*

SECTION A




a cross .

1 This question is about four organic compounds, each containing two carbon atoms.

A CH3CH2OH

B

CH3CHO

C CH3COOH

D CH3COCl

(a) Which is oxidized by ammoniacal silver nitrate?(1)

A

B

C

D

(b) Which has the highest boiling temperature? (1)

A

B

C

D

(c) 0.01 mol of each compound is heated separately with excess acidified sodium dichromate(VI).

Which compound reduces the largest amount of sodium dichromate(VI)?(1)

A

B

C

D

3


(d) 0.01 mol of each compound is added separately to identical volumes of water. Which solution would have the lowest pH?

(1)

A

B

C

D



4

*P42972A0424*

2 Four sketch graphs are shown below.

(a) Which could be a graph of the concentration of a reactant, on the vertical axis, against time for a zero order reaction?

(1)

A

B

C

D

(b) Which could be a graph of rate of reaction, on the vertical axis, against the concentration of a reactant for a first order reaction?

(1)

A

B

C

D

A B

C D

5


(c) Which could be a graph of rate of reaction, on the vertical axis, against the square of the concentration of a reactant for a second order reaction?

(1)

A

B

C

D

(d) Which could be a graph of the concentration of a reactant, on the vertical axis, against time for a reaction which is catalysed by a product?

(1)

A

B

C

D


3 Which of the following mixtures would form the best buffer solution with pH 9 for use in a school laboratory?

A Ethanoic acid and sodium ethanoate

B Sodium chloride and sodium hydroxide

C Hydrocyanic acid and sodium cyanide

D Ammonium chloride and ammonia



6

*P42972A0624*

4 Select the correct pH for each of the following solutions.

(a) 2 mol dm−3 nitric acid.(1)

A −2

B −0.3

C +0.3

D +2

(b) 0.10 mol dm−3 barium hydroxide, Ba(OH)2. Kw = 1.0 10−14 mol2 dm−6.(1)

A 13.0

B 13.3

C 13.7

D 14.3

(c) A mixture of 20 cm3 of 1.0 mol dm−3 hydrochloric acid and 10 cm3 of 1.0 mol dm−3 sodium hydroxide.

(1)

A 0

B 0.30

C 0.48

D 7


5 Ammonia reacts with water in a reversible reaction. Which are the Brønsted-Lowry bases?

A H2O and OH–

B NH3 and OH–

C NH4+ and H2O

D NH4+ and NH3


7


6 The formula for oleic acid, which is present in fingerprints, is shown below.

C C

CH3(CH2)7

HH

(CH2)7COOH

(a) The systematic name for oleic acid is(1)

A E-octadec-9-enoic acid.

B Z-octadec-9-enoic acid.

C E-octadec-8-enoic acid.

D Z-octadec-8-enoic acid.

(b) Which intermolecular forces are present between oleic acid molecules?(1)

A Hydrogen bonds only.

B Hydrogen bonds and permanent dipole-dipole forces only.

C Hydrogen bonds, permanent dipole-dipole forces and London forces.

D Hydrogen bonds and London forces only.

(c) Which of the following species is most likely to cause a peak at m/e = 45 in the mass spectrum of oleic acid?

(1)

A CH2CH2OH

B CH2CH2OH+

C COOH

D COOH+

(d) What would you expect to see if oleic acid is tested separately with bromine water and with phosphorus(V) chloride, PCl5?

(1)

Bromine water Phosphorus(V) chloride, PCl5

A Decolorises Steamy fumes

B No colour change No visible change

C Decolorises No visible change

D No colour change Steamy fumes


8

*P42972A0824*

7 Methane hydrate is found on continental shelves deep in oceans. It forms methane in an endothermic equilibrium reaction, which may be represented as

CH4.6H2O(s) CH4(g) + 6H2O(l)

(a) Which of the following changes would increase the equilibrium yield of methane?

(1)

A Increasing the temperature and decreasing the pressure.

B Decreasing both the temperature and the pressure.

C Increasing both the temperature and the pressure.

D Decreasing the temperature and increasing the pressure.

(b) Which of the following would decrease the value of the equilibrium constant, Kp, for the above equilibrium?

(1)

A Decreasing the pressure

B Increasing the pressure

C Decreasing the temperature

D Increasing the temperature


8 When one optically active isomer of 3-chloro-3-methylhexane reacts with hydroxide ions to form 3-methylhexan-3-ol, a racemic mixture forms because

A 3-chloro-3-methylhexane forms a carbocation intermediate.

B the reaction is a nucleophilic substitution.

C 3-chloro-3-methylhexane forms a five-bonded transition state.

D 3-methylhexan-3-ol contains a chiral carbon.



2

*P42988A0224*

SECTION A



If you change your mind, put a line through the box and then mark your new answer

with a cross .

1 Four organic compounds are:

A CH3OH

B HCHO

C HCOOH

D HCOOCH3

(a) Which of these compounds has a fruity smell?(1)

A

B

C

D

(b) 0.01 mol of each compound is added separately to identical volumes of water. Which solution would have the lowest pH?

(1)

A

B

C

D

(c) 0.01 mol of each compound is heated separately with excess acidified sodium dichromate(VI) solution. Which compound reduces the largest amount of sodium dichromate(VI)?

(1)

A

B

C

D

3


(d) Which compound has the highest boiling temperature?(1)

A

B

C

D

(e) Which of these compounds can be oxidized by ammoniacal silver nitrate?(1)

A

B

C

D



4

*P42988A0424*

2 Four sketch graphs are shown below.

(a) Which could be a graph of rate of reaction, on the vertical axis, against the concentration of a reactant for a zero order reaction?

(1)

A

B

C

D

(b) Which could be a graph of rate of reaction, on the vertical axis, against the square of the concentration of a reactant for a second order reaction?

(1)

A

B

C

D

A B

C D

5


(c) Which could be a graph of the concentration of a reactant, on the vertical axis, against time for a first order reaction?

(1)

A

B

C

D

(d) Which could be a graph of ln(rate), on the vertical axis, against reciprocal of temperature, 1/T, for a reaction?

You may use the equation ln( )rateT

constanta= − × +ER

1

(1)

A

B

C

D


3 Which of the following mixtures would form the best buffer solution with pH 5 for use in a school laboratory?

A Ethanoic acid and sodium ethanoate

B Hydrochloric acid and sodium chloride

C Sodium hydroxide and sodium methanoate

D Ammonium chloride and ammonia



6

*P42988A0624*

4 Suggest the most likely pH for each of the following solutions.

(a) 5.0 mol dm–3 hydrochloric acid.(1)

A +5

B +0.7

C –0.7

D –5

(b) 0.20 mol dm–3 strontium hydroxide, Sr(OH)2

Kw = 1.0 10–14 mol2 dm–6

(1)

A 13.3

B 13.6

C 14.0

D 14.3

(c) A mixture of 20 cm3 of 1.0 mol dm–3 nitric acid and 10 cm3 of 1.0 mol dm–3 sodium hydroxide.

(1)

A 0

B 0.30

C 0.48

D 7


5 In liquid ammonia the following equilibrium is present.

NH2− + NH4

+ 2NH3

Identify the Brønsted-Lowry base(s).

A NH2− only

B NH4+ only

C NH2− and NH3

D NH4+ and NH3


7


6 The formula for oleyl alcohol, which is present in sperm whale oil and was used as a lubricant, is shown below.

CH3(CH2)7

H

C

(CH2)7CH2OH

H

C

(a) The systematic name for oleyl alcohol is(1)

A E-octadec-9-en-1-ol.

B Z-octadec-9-en-1-ol.

C E-octadec-8-en-1-ol.

D Z-octadec-8-en-1-ol.

(b) Which intermolecular forces are present between oleyl alcohol molecules?(1)

A London forces only

B Hydrogen bonds and London forces only

C Hydrogen bonds and permanent dipole–dipole forces only

D Hydrogen bonds, permanent dipole–dipole and London forces

(c) Which of the following is the most likely structure of the species to cause a peak at m/e 31 in the mass spectrum of oleyl alcohol?

(1)

A CH3O

B CH2OH

C CH3O+

D CH2OH+

(d) What would you expect to see if oleyl alcohol is tested separately with bromine water and heated with acidified sodium dichromate(VI) solution?

(1)

Bromine water Acidified sodium dichromate(VI) solution

A Decolorises Turns green

B No colour change No colour change

C Decolorises No colour change

D No colour change Turns green


8

*P42988A0824*

7 Methane hydrate is found on continental shelves deep in oceans. It forms methane in an endothermic equilibrium reaction, which may be represented as

CH4.6H2O(s) CH4(g) + 6H2O(l)

(a) Which of the following changes would decrease the equilibrium yield of methane?

(1)

A Decreasing the temperature and decreasing the pressure.

B Increasing the temperature and decreasing the pressure.

C Decreasing the temperature and increasing the pressure.

D Increasing the temperature and increasing the pressure.

(b) Which of the following would increase the value of the equilibrium constant, Kp, for the above equilibrium?

(1)

A Decreasing the pressure

B Increasing the pressure

C Decreasing the temperature

D Increasing the temperature



2

*P42973A0228*

SECTION A




cross .

1 In which of the following ions does the metal have an oxidation number of +3?

A MnO42–

B VO2+

C [Fe(CN)6]4–

D [CrCl2(H2O)4]+


2 Copper metal is oxidized to Cu2+ by nitrate(V) ions which are reduced to nitrogen monoxide, NO. By considering the changes to the oxidation numbers of copper and nitrogen, it can be deduced that in this reaction

A 2 mol of copper reacts with 3 mol of nitrate(V) ions.

B 2 mol of copper reacts with 5 mol of nitrate(V) ions.

C 3 mol of copper reacts with 2 mol of nitrate(V) ions.

D 5 mol of copper reacts with 2 mol of nitrate(V) ions.



3


3 The diagram below shows a cell set up between a copper metal / copper(II) ion electrode and a reference electrode, known as a calomel electrode.

Under standard conditions, the emf of this cell was −0.07 V. The standard electrode potential of the copper metal / copper(II) ion electrode is +0.34 V. Hence the standard electrode potential of the calomel electrode is

A −0.41 V

B −0.27 V

C +0.27 V

D +0.41 V


4 For the reaction

2NO2(g) N2O4(g)

at 450 K the total entropy change, Stotal, is negative. Hence the equilibrium constant, Kp, for this reaction at 450 K is

A zero.

B positive and greater than 1.

C positive and less than 1.

D negative.


copper metal

calomel electrodecopper(II) sulfate

solution

salt bridge

V

4

*P42973A0428*

5 The standard electrode potentials of two half reactions are shown below.

½Cl2 + e− Cl− E = +1.36 V

Co3+ + e− Co2+ E = +1.82 V

Which of the following processes is thermodynamically favourable? The reaction of

A Co2+ with Cl2 to form Cl−

B Co2+ with Cl− to form Cl2

C Co3+ with Cl2 to form Cl−

D Co3+ with Cl– to form Cl2


6 A solution of potassium manganate(VII) was used to determine the concentration of iron(II) ions in solution by titration in the presence of excess dilute sulfuric acid.

(a) With the potassium manganate(VII) in the burette, the end-point of the reaction is when the solution in the conical flask turns

(1)

A colourless.

B pink.

C green.

D orange.

(b) If insufficient acid is added, the titre value is(1)

A low and a brown precipitate forms.

B low and a green precipitate forms.

C high and a brown precipitate forms.

D high and a green precipitate forms.


7 What is the electronic configuration of the stable scandium ion?

A [Ar] 3d0 4s2

B [Ar] 3d1 4s1

C [Ar] 3d0 4s1

D [Ar] 3d0 4s0


5


8 The shapes of the complexes [CrCl4]– and [Pt(NH3)2Cl2] are

[CrCl4]− [Pt(NH3)2Cl2]

A square planar square planar

B tetrahedral tetrahedral

C square planar tetrahedral

D tetrahedral square planar


9 The compound 1,2-diaminoethane, H2NCH2CH2NH2, is a bidentate ligand; in formulae, it is usually abbreviated to ‘en’.

When 1,2-diaminoethane is added to [Co(NH3)6]2+ in aqueous solution, [Co(en)3]2+ is formed. What is the best explanation for this?

A There are much stronger bonds between the ligands and the cobalt(II) ion in [Co(en)3]2+ than in [Co(NH3)6]2+.

B When [Co(en)3]2+ is formed from [Co(NH3)6]2+ the reaction is exothermic.

C When [Co(en)3]2+ is formed from [Co(NH3)6]2+ the total entropy change is positive.

D When [Co(en)3]2+ is formed from [Co(NH3)6]2+ the reaction has a low activation energy.


10 When aqueous sodium hydroxide is added to an aqueous solution of a transition metal compound, a green precipitate is formed which dissolves in excess sodium hydroxide forming a green solution. The transition metal ion present in the original solution is

A Cr3+

B Fe3+

C Fe2+

D Ni2+


6

*P42973A0628*

11 Benzene reacts with a nitrating mixture of concentrated nitric and sulfuric acids. Which species is least likely to be present in the nitrating mixture?

A NO3−

B H3O+

C HSO4−

D NO2+


12 Benzene (Tb = 80.1 C) has a higher boiling temperature than ethanol (Tb = 78.5 C). This is because the

A benzene ring is stabilised.

B London forces between benzene molecules are stronger than the hydrogen bonds between ethanol molecules.

C hydrogen bonds between benzene molecules are stronger than the hydrogen bonds between ethanol molecules.

D C–H bonds in benzene are stronger than the C–H bonds in ethanol.


13 Separate 0.1 mol dm−3 aqueous solutions of ammonia, methylamine and phenylamine were prepared. Which of the following sequences shows the solutions in order of increasing pH?

A phenylamine, methylamine, ammonia

B phenylamine, ammonia, methylamine

C methylamine, ammonia, phenylamine

D methylamine, phenylamine, ammonia



7


14 The benzenediazonium ion, C6H5N2+, is an intermediate in the preparation of azo dyes.

(a) In the formation of an azo dye, the benzenediazonium ion is(1)

A an electrophile.

B a nucleophile.

C a carbocation.

D a substituent.

(b) The temperature of the aqueous reaction mixture must be kept below 10 C to prevent the benzenediazonium ion being converted into

(1)

A benzene.

B nitrobenzene.

C phenylamine.

D phenol.



8

*P42973A0828*

15 The monomer of the addition polymer poly(propenol) may be represented as CH3–CH=CHOH.

The repeat unit of the addition polymer is

A

OH⎡

⎣⎢ ⎡

⎣⎢

B

OH⎡

⎣⎢ ⎡

⎣⎢

C

OH⎡

⎣⎢ ⎡

⎣⎢

D

OH

⎡

⎣⎢ ⎡

⎣⎢


16 Chromatography may be used to separate mixtures of amino acids. This is best explained by the fact that different amino acids have different interactions with

A the mobile phase only.

B the stationary phase only.

C the mobile phase and the stationary phase.

D ninhydrin.


9


17 In an aqueous solution with a pH of 7, the amino acid alanine exists mainly as

A H2N CH

CH3

HO

C O

B H2N CH

CH3

–O

C O

C H3

+N CH

CH3

HO

C O

D H3

+N CH

CH3

–O

C O


18 When a solid is purified by recrystallization, the procedure involves the removal of impurities by filtration of the hot mixture followed by filtration of the cold mixture. Which impurities are removed by these two filtrations?

Hot filtration Cold filtration

A insoluble impurities insoluble impurities

B insoluble impurities soluble impurities

C soluble impurities insoluble impurities

D soluble impurities soluble impurities



2

*P42989rA0228*

SECTION A




cross .

1 In which of the following ions does the metal have an oxidation number of +2?

A MnO42–

B VO2+

C [Fe(CN)6]4–

D [CrCl2(H2O)4]+


2 Sulfur dioxide reacts with hydrogen sulfide to form water and sulfur. By considering the changes in the oxidation numbers of sulfur, it can be deduced that, in this reaction

A 1 mol of sulfur dioxide oxidizes 2 mol of hydrogen sulfide.

B 1 mol of sulfur dioxide reduces 2 mol of hydrogen sulfide.

C 2 mol of sulfur dioxide oxidizes 1 mol of hydrogen sulfide.

D 2 mol of sulfur dioxide reduces 1 mol of hydrogen sulfide.



3

*P42989rA0328* Turn over

3 The diagram below shows a cell set up between a standard copper metal / copper(II) ion electrode and a silver metal / silver(I) ion electrode in which the silver ion concentration is 0.1 mol dm–3.

At 298 K, the emf of this cell was +0.40 V. The electrode potential of the copper metal / copper(II) ion electrode is +0.34 V. What is the electrode potential of this silver metal / silver(I) ion electrode?

A –0.74 V

B –0.06 V

C +0.06 V

D +0.74 V


4 For the reaction

Zn(s) + Cu2+(aq) Cu(s) + Zn2+(aq)

E cell is positive. From this it can be deduced that, for this reaction,

A Stotal and ln K are positive.

B Stotal and ln K are negative.

C Stotal is positive and ln K is negative.

D Stotal is negative and ln K is positive.


copper metal

0.1 mol dm–3 silver nitrate solution

silver metalsalt bridge

1.0 mol dm–3 copper(II) sulfate solution

V

4

*P42989rA0428*

5 Sodium thiosulfate was used to determine the concentration of iodine by titration.

(a) The sodium thiosulfate solution was prepared by dissolving 4.5 g of sodium thiosulfate in water and making the solution up to 250 cm3 in a volumetric flask. The volumetric flask is accurate to ± 0.3 cm3 so, to match this accuracy, the mass of the sodium thiosulfate should be accurate to at least

(1)

A ± 0.5 g

B ± 0.05 g

C ± 0.005 g

D ± 0.0005 g

(b) With the sodium thiosulfate in the burette, what is the colour of the solution in the conical flask at the end-point of the reaction?

(1)

A Blue-black

B Colourless

C Red-brown

D Yellow


6 In a hydrogen-oxygen fuel cell, hydrogen is

A oxidized at the anode.

B oxidized at the cathode.

C reduced at the anode.

D reduced at the cathode.



5


7 The electronic configuration of iron is [Ar]3d64s2. What is the electronic configuration of the iron(II) ion, Fe2+?

3d 4s

A [Ar]

B [Ar]

C [Ar]

D [Ar]


8 Chromium has the electronic configuration [Ar]3d54s1. Which of the following compounds is unlikely to exist?

A K3CrO4

B CrO2Cl2

C KCrO2Cl

D KCrO4


9 The shapes of the complexes [CrCl4]– and [CuCl2]– are

[CrCl4]– [CuCl2]–

A tetrahedral linear

B square planar linear

C tetrahedral V-shaped

D square planar V-shaped


6

*P42989rA0628*

10 When EDTA is added to [Cu(NH3)4]2+ in aqueous solution, the copper(II)-EDTA complex, [Cu(EDTA)]2–, predominates in the resulting solution.

This is best explained by the fact that when [Cu(EDTA)]2– is formed from [Cu(NH3)4]2+

A there are much stronger bonds between the ligands and the copper(II) ion.

B the reaction has a low activation energy.

C the reaction is exothermic.

D the total number of particles on the right-hand side of the equation is greater than on the left.


11 The graph below shows the variation in the colour intensity of different solutions formed by mixing a 0.05 mol dm–3 solution of a metal ion X and a 0.05 mol dm–3 solution of a complexing agent Y, in the proportions shown on the graph.

The most likely formula of the complex formed is

A X2Y

B XY2

C XY3

D X3Y


Colour intensity

cm3 of Y

cm3 of X

0 1 2 3 4 5 6 7 8 9 10

10 9 8 7 6 5 4 3 2 1 0

7


12 When benzene reacts with fuming sulfuric acid, which species is most likely to be the electrophile?

A H3O+

B SO3

C HSO4–

D SO42–


13 Benzene reacts with propanoyl chloride in the presence of a suitable catalyst.

The skeletal formula of propanoyl chloride is

Cl

O

What is the organic product of this reaction?

A O

B O

CO

D

O


8

*P42989rA0828*

14 Excess dilute sulfuric acid is added to phenylamine. What is the product of the reaction?

AS

O

O

OH

BS

O

OHO

NH2

CS

OO–

ONH4+

D S

O–

O–

OO

NH3+

2

⎡

⎣

⎢⎢⎢⎢

⎡

⎣

⎢⎢⎢⎢


9


15 Butylamine (Tb = 77.8 C) has a higher boiling temperature than propylamine (Tb = 47.7 C). This is because the

A hydrogen bonds of butylamine are stronger than the hydrogen bonds of propylamine.

B London forces of butylamine are stronger than the hydrogen bonds of propylamine.

C London forces of butylamine are stronger than the London forces of propylamine.

D C–H bonds of butylamine are stronger than the C–H bonds of propylamine.


16 Ninhydrin is used in thin-layer chromatography to help with the identification of amino acids. This is because the ninhydrin

A reacts with amino acids to form a compound which has an intense colour.

B reacts with amino acids to form compounds each of which has a characteristic colour.

C increases the separation of the amino acids on the chromatogram.

D ensures that the mobile phase maintains a nearly constant pH for all the amino acids.



10

*P42989rA01028*

17 The monomer of the addition polymer poly(propenamide) is CH2=CHCONH2. The repeat unit of the polymer is

AC

O

CH2

C

H

N

⎡

⎣

⎢⎢⎢⎢

⎡

⎣

⎢⎢⎢⎢

B

O

CH2

H2C

H

N

⎡

⎣

⎢⎢⎢⎢

C

⎡

⎣

⎢⎢⎢⎢

C

O

H2C ⎡

⎣

⎢⎢⎢⎢

C

HC

NH2

⎡

⎣

⎢⎢⎢⎢

D

O

CH

CH

H

N

⎡

⎣

⎢⎢⎢⎢

C

⎡

⎣

⎢⎢⎢⎢


11


18 15 cm3 of a gaseous hydrocarbon requires 90 cm3 of oxygen for complete combustion, both volumes being measured at 15 C and 1 atm. The formula of the hydrocarbon is

A C4H6

B C4H8

C C4H10

D impossible to calculate without knowing the molar volume of gases under these conditions.


19 In an aqueous solution with a pH of 12, the amino acid alanine exists mainly as

A H2N CH

C O

HO

CH3

B H2N CH

C O

–O

CH3

C

H3 N CH

C O

HO

CH3

+

D

H3 N CH

C O

–O

CH3

+



2

*P44879A0224*

SECTION A




a cross .

1 Which molecule does not exhibit E / Z isomerism?

A

B

C

D


2 What is the systematic name for the compound with the following formula?

C2H5

CH3

H3C CH CH2 CH3CH

A 2-methyl-4-ethylpentane

B 2-ethyl-4-methylpentane

C 2,4-dimethylhexane

D 3,5-dimethylhexane


Br

HH3C

C C

CH3

Br

CH3H

C C

CH3

CH2Br

HHC C

H3C

Br

BrH3C

C C

CH3

3


3 Which of the following molecules is formed on adding bromine water to ethene?

A ethanol

B ethane-1,2-diol

C bromoethane

D 2-bromoethanol


4 A section of a polymer is shown below.

C

CH3

C

CH3

C

CH3

C

CH3

C2H5 C2H5 HH

What is the monomer for this polymer?

A C

CH3

C

CH3

C2H5

H H

H

B

CH3

C2H5

C C

CH3

C C

CH3

C2H5CH3

C

CH3

HC2H5

C C

CH3

D

CH3

CH3

C C

H

C2H5


4

*P44879A0424*

5 Which of the following equations has the correct state symbols for the reaction of dilute hydrochloric acid with magnesium oxide?

A MgO(s) + 2HCl(aq) → MgCl2(s) + H2O(l)

B MgO(s) + 2HCl(aq) → MgCl2(aq) + H2O(l)

C MgO(s) + 2HCl(l) → MgCl2(s) + H2O(l)

D MgO(s) + 2HCl(l) → MgCl2(aq) + H2O(l)


6 This question is about the reaction between sodium carbonate solution and dilute nitric acid.

Na2CO3(aq) + 2HNO3(aq) → 2NaNO3(aq) + CO2(g) + H2O(l)

(a) What is the ionic equation for this reaction?(1)

A Na2CO3(aq) + 2H+(aq) → 2Na+(aq) + CO2(g) + H2O(l)

B Na+(aq) + NO3−(aq) → NaNO3(aq)

C CO32_

(aq) + 2H+(aq) → CO2(g) + H2O(l)

D CO32_

(aq) + 2HNO3(aq) → 2NO3−(aq) + CO2(g) + H2O(l)

(b) What is the volume of carbon dioxide produced from the complete reaction of 0.10 mol of nitric acid at room temperature and pressure?

[1 mol of any gas occupies 24 dm3 at room temperature and pressure.](1)

A 1.2 dm3

B 1.8 dm3

C 2.4 dm3

D 3.6 dm3

(c) What volume of sodium carbonate solution of concentration 0.500 mol dm–3, would be needed to completely react with 25.0 cm3 of nitric acid of concentration 0.250 mol dm–3?

(1)

A 6.25 cm3

B 12.50 cm3

C 18.75 cm3

D 25.00 cm3


5


7 Lithium reacts with water to produce hydrogen.

Li(s) + H2O(l) → LiOH(aq) + ½H2(g)

(a) In an experiment, 0.069 g (0.01 mol) of lithium produced 90 cm3 of hydrogen at room temperature and pressure. What is the percentage yield of hydrogen?

[1 mol of any gas occupies 24 dm3 at room temperature and pressure.] (1)

A 45%

B 60%

C 75%

D 90%

(b) Which of the following is not a possible reason for the yield being less than 100%?

(1)

A Some oil remained on the surface of the lithium.

B Hydrogen gas is very soluble in water.

C A layer of oxide was present on the surface of the lithium.

D Some of the hydrogen gas escaped collection.


8 How many moles of atoms are present in 240 cm3 of carbon dioxide at room temperature and pressure?

[1 mol of any gas occupies 24 dm3 at room temperature and pressure.]

A 0.010

B 0.020

C 0.024

D 0.030


6

*P44879A0624*

9 What is the percentage by mass of nitrogen in ammonium nitrate, NH4NO3?

[Molar masses/g mol−1: N = 14.0; H = 1.0; O = 16.0]

A 14.0%

B 17.5%

C 28.0%

D 35.0%


10 The first five successive ionization energies for an element J, in kJ mol_1, are

1st 2nd 3rd 4th 5th

738 1450 7733 10543 13630

The formula of the compound of chlorine with element J is

A JCl

B JCl2

C JCl3

D J2Cl3


11 Which of the following is the correct order of increasing melting temperature of elements of Period 3?

A Na, Mg, Al, Si

B Na, Mg, Si, Al

C Si, Na, Mg, Al

D Si, Al, Mg, Na


7


12 Which one of the following elements undergoes the change in electronic configuration shown when it forms the stated ion?

Atom 1s22s22p63s23p3 Ion 1s22s22p63s23p6

A B to B3+

B Al to Al3+

C N to N3–

D P to P3–


13 Which of the following compounds has the most polarized anion?

A Na2O

B MgO

C K2O

D CaO


8

*P44879A0824*

14 The diagram shows a Born-Haber cycle for calcium chloride. It is not drawn to scale. All units are in kJ mol_1.

Ca2+(g) + 2Cl_(g)

P = −2258

Q = +1735 R = (−346 × 2) = −692

S = (+121 × 2) = +242

CaCl2(s)

Ca(g) 2Cl(g)

+178

+

+

Ca(s) Cl2(g)

(a) Which enthalpy change is correctly labelled on the diagram?(1)

A Enthalpy change for the formation of calcium chloride (P).

B First ionization energy of calcium (Q).

C Electron affinity of chlorine (R).

D Twice the enthalpy change of atomization of chlorine (S).

(b) What is the value of X, in kJ mol_1?(1)

A +795

B –795

C +3721

D –3721


X = ?

9


15 Calculate the enthalpy change, in kJ mol_1, for the reaction

H2(g) + ½O2(g) → H2O(g)

DATA:

Bond Bond enthalpy / kJ mol_1

H−H +436

O=O +498

H−O +464

A −243

B −6

C +6

D +221


16 The chemical properties of an element are determined by its

A electronic structure.

B number of neutrons.

C relative atomic mass.

D number of protons plus neutrons.



2

*P44881A0224*

SECTION A




a cross .

1 The bond angle in beryllium chloride, BeCl2, is most likely to be

A 90°

B 104.5°

C 120°

D 180°


2 Graphite and buckminsterfullerene are forms of carbon. Buckminsterfullerene dissolves in octane but graphite does not. This is because

A the bonds between carbon atoms in buckminsterfullerene are weaker than those in graphite.

B buckminsterfullerene is molecular whereas graphite is a giant structure.

C graphite has delocalised electrons but buckminsterfullerene does not.

D graphite has covalent bonds and London forces but buckminsterfullerene has just London forces.




B Silicon tetrachloride, SiCl4

C Ammonia, NH3

D Boron trifluoride, BF3


3


4 In which series of compounds does covalent character increase when going from left to right?

A KI, KBr, KCl

B NaI, KI, RbI

C NaCl, MgCl2, AlCl3

D SO2, P4O10, SiO2


5 Hydrogen bromide has a lower boiling temperature than hydrogen iodide. This is because

A hydrogen bromide has a smaller permanent dipole than hydrogen iodide.

B hydrogen bromide has weaker London forces than hydrogen iodide.

C hydrogen iodide forms hydrogen bonds but hydrogen bromide does not.

D the H I bond is stronger than the H Br bond.


4

*P44881A0424*

6 Consider the following compounds, E, F, G and H.

l CH2

CH2 CH2

CH3

G

Cl CH2

CH2 CH2

CH3

E

C

CH3

CH3

CH3l

H

C

CH3

CH3

CH3Cl

F

The boiling temperature of these compounds increases in the order

A H G F E

B G H E F

C E F G H

D F E H G


7 In which of the following reactions is sulfuric(IV) acid, H2SO3, acting as an oxidizing agent?

A H2SO3 + H2O H3O+ + HSO3–

B H2SO3 SO2 + H2O

C H2SO3 + 2FeCl3 + H2O 2FeCl2 + H2SO4 + 2HCl

D H2SO3 + 2H2S 3H2O + 3S


5


8 Which of the following properties decreases on descending Group 2 of the Periodic Table?

A Solubility of the sulfates.

B Solubility of the hydroxides.

C Reactivity of the elements.

D Ionic character of the oxides.


9 Compound X is an anhydrous, white solid which decomposes on heating to form a white solid residue, a colourless gas, and a colourless vapour which condenses to a colourless liquid.

Compound X is

A sodium carbonate.

B sodium hydrogencarbonate.

C sodium nitrate.

D sodium sulfate.


6

*P44881A0624*

10 These questions concern the Maxwell-Boltzmann energy distribution shown below.

Fraction of particles with a specific energy

Energy Ea

(a) What is the best way to describe the activation energy, Ea, of a reaction?(1)

A The average energy of the particles that react.

B The minimum energy required for a reaction to occur.

C The energy difference between the reactants and products.

D The energy produced by the particles that react.

(b) How does the curve above change when the temperature is increased?(1)

A The peak increases in height and moves to the left.

B The peak increases in height and moves to the right.

C The peak decreases in height and moves to the left.

D The peak decreases in height and moves to the right.

7


(c) What would be the effect on the diagram if the reactant concentrations were increased?

(1)

A There would be no change.

B The Ea line would move to the right.

C The Ea line would move to the left.

D The peak decreases in height and moves to the right.

(d) What would be the effect on the diagram if a catalyst was added? The activation energy would

(1)

A be unchanged and the peak would move to the right.

B move to the left and the peak would move to the right.

C move to the left and the peak would move to the left.

D move to the left and the peak would be unchanged.


11 Propanal, CH3CH2CHO, and propanone, CH3COCH3, are carbonyl compounds. When these compounds are compared using physical methods of analysis, which of the following statements is not correct?

A The compounds produce different patterns in the fingerprint region of the IR spectrum.

B The carbonyl groups absorb at frequencies in the same region of the IR spectrum.

C The compounds produce different fragmentation patterns in a mass spectrum.

D The compounds have molecular ion peaks at different mass to charge ratios in a mass spectrum.


8

*P44881A0824*

12 A sample of propanone, CH3COCH3, was heated under reflux with potassium dichromate(VI)acidified with sulfuric acid, and then the mixture was distilled. Apart from the peaks

due to the C C and C H bonds, what peak(s) would be present in the IR spectrum of the distillate?

A A peak due to the C O only.

B A peak due to the O H only.

C Peaks due to C O and O H.

D Peaks due to C O, C O and O H.


13 Which of the following describes the appearance of iodine under the stated conditions?

Solid Dissolved in aqueous potassium iodide

Dissolved in a liquid hydrocarbon

A purple brown purple

B brown blue-black yellow

C shiny grey brown purple

D shiny grey brown brown


14 Why do calculations of global warming exclude the effect of water vapour in the atmosphere?

A Water vapour is not a greenhouse gas.

B Water vapour is a much less potent greenhouse gas than carbon dioxide.

C The average concentration of water vapour in the atmosphere is fairly constant.

D The concentration of water vapour in the atmosphere is much lower than that of carbon dioxide.


9


15 A compound of nitrogen and hydrogen only is analyzed and found to contain 97.7% by mass of nitrogen. What is the empirical formula of the compound?

Molar masses /g mol–1: H = 1; N = 14

A NH3

B NH2

C N3H5

D N3H


16 Chlorofluorocarbons, CFCs, damage the ozone layer. The mechanism of the process involves

A homolytic fission.

B heterolytic fission.


D nucleophilic substitution.


17 Electrophiles are

A electron pair donors that are attracted to regions of high electron density.

B electron pair donors that are attracted to regions of low electron density.

C electron pair acceptors that are attracted to regions of high electron density.

D electron pair acceptors that are attracted to regions of low electron density.



2

*P42978A0228*

SECTION A




a cross .

1 Name the compound below.

C C

CH3

CH2CH3Cl

H

A E-2-chloropent-2-ene

B Z-2-chloropent-3-ene

C E-2-chloropent-3-ene

D Z-2-chloropent-2-ene



3


2 Which of the following compounds is not chiral?

A

O

B

C O

NH2

OH

HO

D

O OH

HO



4

*P42978A0428*

3 Calculate the pH of a solution of HCl, of concentration 0.25 mol dm–3.

A –0.60

B 0.25

C 0.60

D 1.39


4 Which gas is the least suitable as a carrier gas in Gas-Liquid Chromatography?

A Argon

B Carbon dioxide

C Oxygen

D Nitrogen


5 What are the units of the equilibrium constant (Kc) for the hypothetical reaction below?

2A(aq) + B(aq) 4C(aq) + D(aq)

A mol2 dm–9

B mol–2 dm9

C mol2 dm–6

D mol–2 dm6



5


6 This question is about the reversible reaction below.

2NO2(g) N2O4(g)

(a) A chemist investigating this reaction started with 10 moles of NO2 and allowed the system to reach equilibrium. If 3 moles of N2O4 are formed, the number of moles of NO2 at equilibrium is

(1)

A 8.5

B 7

C 6

D 4

(b) Under different conditions, 40% of the moles present at equilibrium is N2O4. If the total pressure of the system is 2.0 atm, the numerical value of the equilibrium constant, Kp is

(1)

A 0.56

B 0.67

C 1.5

D 1.8



6

*P42978A0628*

7 Carbon monoxide and chlorine react together and reach equilibrium:

CO(g) + Cl2(g) COCl2(g)

If the pressure of the system is then increased at constant temperature, which of the following statements is correct?

A The equilibrium moves to the left and Kp decreases.

B The equilibrium moves to the right and Kp increases.

C The equilibrium moves to the right, then back to the left and Kp remains the same.

D The equilibrium moves to the right and Kp remains the same.


8 The table shows some data about metal ions, non-metal ions and their compounds.

IonEnthalpy change

of hydration / kJ mol–1

Compound Lattice energy / kJ mol–1

Mg2+(g) –1921MgCl2(s) –2526

Cl–(g) –340

Cs+(g) –276CsF(s) –747

F–(g) –483

Use the data to calculate

(a) the standard enthalpy change, in kJ mol−1, for the following process.

Mg2+(g) + 2Cl−(g) Mg2+(aq) + 2Cl−(aq)(1)

A –1241

B –1581

C –2261

D –2601

7


(b) the standard enthalpy change of solution, in kJ mol−1, of caesium fluoride, CsF.(1)

A –12

B +12

C –1506

D +1506


9 Which of these solvents is most likely to be warmed by microwave radiation?

A Hexane

B Cyclohexane

C Cyclohexanol

D Cyclohexene



8

*P42978A0828*

10 Some chemical tests are described below.

A Warm with Fehling’s (or Benedict’s) solution

B Warm with acidified potassium dichromate(VI) solution

C Add sodium carbonate solution

D Add 2,4-dinitrophenylhydrazine solution

(a) Which test always gives a positive result with carbonyl compounds?(1)

A

B

C

D

(b) Which test would give a positive result with ethane-1,2-diol?(1)

A

B

C

D

(c) Which test would result in effervescence with ethanoic acid?(1)

A

B

C

D



9


11 Consider the four compounds shown below.

A CH3COOCH3

B CH3COOH

C CH3CONHCH2CH3

D CH3COCl

Which of these compounds

(a) will react most vigorously with water?(1)

A

B

C

D

(b) forms methanol when refluxed with aqueous sodium hydroxide?(1)

A

B

C

D

(c) has at least one triplet in its high resolution proton nmr spectrum?(1)

A

B

C

D



10

*P42978A01028*

12 The diagram below shows part of the mechanism for the nucleophilic addition of hydrogen cyanide to butanone.

C

H3C

O

C H2

CH3

CN–

Step 1Intermediate X

Organic Products

Step 2

(a) The formula of the intermediate X is(1)

A C + C

H2

H3C

OCN

CH3

B CC

H2

H3C

O–

CH3

CN

C CC

H2

H3C

O

CH3

CN

D CC

H2

H3C

OH+

CH3

CN–

11


(b) Consider the dissociation of the weak acid, HCN.

HCN(aq) H+(aq) + CN–(aq)

Which of the following reagents would shift the position of the equilibrium towards formation of the nucleophile, CN–?

(1)

A KOH

B KCN

C H2SO4

D CH3COOH

(c) Which statement about the mixture of organic products formed is not correct?(1)

A The mixture contains products with chiral molecules.

B The mixture rotates the plane of plane-polarized light.

C The mixture contains products with the nitrile functional group.

D The mixture contains products each of which has four carbon atoms in a straight chain.



2

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SECTION A




cross .


A Cr2O72– + 2OH– 2CrO4

2– + H2O

B [Cu(H2O)6]2+ + 4Cl– [CuCl4]2– + 6H2O

C 4OH– + 4MnO4– 4MnO4

2– + 2H2O + O2

D [Fe(H2O)6]3+ + 3OH– [Fe(H2O)3(OH)3] + 3H2O


2 The oxidation state of nickel is not +2 in

A [Ni(CO)4]

B [Ni(H2O)4(OH)2]

C [Ni(NH3)6]2+

D [Ni(CN)4]2–


3 Which of the statements about a standard hydrogen electrode, for which E = 0 V, is correct?

A A suitable solution for use in the electrode is hydrochloric acid with a concentration of 0.1 mol dm–3.

B The pressure of the hydrogen has no effect on the value of E .

C The metal used in the electrode is platinum.

D The temperature is 273 K.



3

*P45073RA0328* Turn over

4 The table below gives the standard electrode potentials of three half cells.

System E / V

H+(aq) + e— ½H2(g) 0.00

Ag+(aq) + e— Ag(s) +0.80

Ag2+(aq) + e— Ag+(aq) +1.98

From these data it may be deduced that, under standard conditions,

A Ag is a stronger reducing agent than H2.

B Ag2+ ions are stronger oxidizing agents than H+ ions.

C Ag+ ions will disproportionate.

D Ag+ ions will react with H+ ions.


5 The value of Ecell indicates whether the cell reaction is thermodynamically feasible. Which of the following is a correct statement about Ecell?

A Ecell is directly proportional to the equilibrium constant.

B Ecell is directly proportional to the entropy change of the system, Ssystem.

C Ecell is directly proportional to the total entropy change, Stotal.

D The value of In Ecell is directly proportional to the total entropy change, Stotal.


6 In a methanol fuel cell, the following half-reaction occurs

CH3OH(l) + H2O(l) 6H+(aq) + CO2(g) + 6e–

The half-reaction occurring in the other half of the fuel cell is

A H2(g) + O2(g) + 2e– 2OH–(aq)

B 2H+(aq) + ½O2(g) + 2e– H2O(l)

C 2OH–(aq) H2(g) + O2(g) + 2e–

D H2O(l) 2H+(aq) + ½O2(g) + 2e–


4

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7 Which of the following statements about fuel cells is not true?

A Reactants must constantly be fed into the cell when it is in use.

B Fuel cells are 100% efficient.

C Fuel cells convert chemical energy directly into electrical energy.

D Fuel cells produce electricity more efficiently than a diesel generator.


8 Copper(II) ions combine with three molecules of 1,2-diaminoethane, NH2CH2CH2NH2, to form a complex ion.

A bond angle, N — Cu — N, in this complex is

A 120°

B 109.5°

C 107°

D 90°


9 Which of the following does not have a central metal ion having six bonds and an oxidation state of +2?

A [Cu(C2O4)3]4–

B [Co(CN)5(H2O)]3–

C [Fe(CN)6]3–

D [Zn(OH)4(H2O)2]2–


10 The reaction

[Fe(H2O)6]2+ + H2O [Fe(H2O)5(OH)]+ + H3O+

is an example of

A oxidation.

B reduction.

C ligand exchange.

D acid-base behaviour.


5


11 Hydrated crystals of a compound have the formula CrCl3(H2O)6. A solution containing one mole of the compound reacts with two moles of silver nitrate to form two moles of silver chloride. The complex chromium ion in the compound is most likely to be

A [Cr(H2O)3Cl3] 3+

B [Cr(H2O)4Cl2] +

C [Cr(H2O)5Cl] 2+

D [Cr(H2O)6] 3+


12 A heterogeneous catalyst is often preferred to a homogenous catalyst for an industrial process because

A it is easily separated from the products.

B it has empty d-orbitals.

C it has more than one oxidation state.

D it cannot be poisoned.


13 In the reaction of benzene with chloromethane, aluminium chloride is added because it reacts with

A benzene to produce an electrophile.

B benzene to produce a nucleophile.

C chloromethane to produce a nucleophile.

D chloromethane to produce an electrophile.


14 The reaction below can be catalysed by either Fe2+ ions or Fe3+ ions.

S2O82–(aq) + 2I–(aq) 2SO4

2–(aq) + I2(aq)

This is because

A both reactants can react with Fe2+ ions.

B both reactants can react with Fe3+ ions.

C S2O82– ions can be oxidized by Fe3+ ions and I– ions can be reduced by Fe2+ ions.

D S2O82– ions can be reduced by Fe2+ ions and I– ions can be oxidized by Fe3+ ions.


6

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15 The enthalpy changes of the reactions below are similar. The equilibrium constants for the two reactions are K1 and K2 respectively.

Reaction 1 [Cu(H2O)6]2+(aq) + EDTA4–(aq) [Cu(EDTA)]2–(aq) + 6H2O(l)

Reaction 2 [Cu(H2O)6]2+(aq) + 4Cl–(aq) [CuCl4]2–(aq) + 6H2O(l)

The value of K1 is greater than K2 because

A Ssystem is much more positive in Reaction 1.

B Ssurroundings is much more positive in Reaction 1.

C the EDTA4– is more highly charged than Cl–.

D a lower concentration of EDTA4– is needed than Cl–.


16 Which of the following reacts with benzene under suitable conditions to form C6H5COC6H5?

A C6H5CHO

B C6H5COOH

C C6H5CH2OH

D C6H5COCl


17 Benzene is converted to benzenesulfonic acid, C6H5SO3H, by reaction with

A sulfuric(IV) acid, H2SO3.

B sulfuric(VI) acid, H2SO4.

C sulfur dioxide dissolved in sulfuric(IV) acid.

D sulfur trioxide dissolved in sulfuric(VI) acid.



7


18 Benzene reacts with chlorine to produce 1,2,3,4,5,6-hexachlorocyclohexane, C6H6Cl6, by

A free radical addition.

B free radical substitution.




19 The skeletal formula of an organic compound is shown below.

O

N

This compound is

A an amino acid.

B an amide.

C a primary amine.

D a secondary amine.


20

CH3 H ⎡

⎣

⎢⎢⎢⎢

C

⎡

⎣

⎢⎢⎢⎢

CH3 CH3

C

n

Which is the IUPAC name for the monomer which reacts to make the polymer shown above?

A 2-methylbut-1-ene

B 2-methylbut-2-ene

C 1,2-dimethylpropene

D 1,1,2-trimethylethene



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SECTION A




a cross .

1 The mass of magnesium ions in 1 kg of sea water is 1.3 g. The concentration in parts per million (ppm) is

A 1.3 × 106

B 1.3 × 103

C 1.3 × 10–3

D 1.3 × 10–6


2 Calculate the total number of ions in 7.41 g of calcium hydroxide, Ca(OH)2.

The molar mass of calcium hydroxide is 74.1 g mol–1.

The Avogadro constant is 6.0 × 1023 mol–1.

A 6.0 × 1022

B 1.2 × 1023

C 1.8 × 1023

D 3.0 × 1023


3 Which of the following has the highest melting temperature?

A Hg

B K

C C10H22

D SiO2


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4 Which of these has a dative covalent bond?

A NH3

B OH–

C H2O

D H3O+


5 What is the equation for the first electron affinity of sulfur?

A S(s) + e– S–(g)

B S(g) + e– S–(g)

C S(s) S+(g) + e–

D S(g) S+(g) + e–


6 100 cm3 of hydrogen is mixed with 25 cm3 of oxygen at a temperature of 150 C. The gases react as shown in the equation below.

2H2(g) + O2(g) 2H2O(g)

The total volume of gas present at the end of the reaction is

A 50 cm3

B 100 cm3

C 125 cm3

D 150 cm3


Use this space for rough working. Anything you write in this space will gain no credit.

4

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7 Sodium nitrate decomposes on heating.

2NaNO3(s) 2NaNO2(s) + O2(g)

What is the maximum volume of oxygen, measured in dm3 at room temperature and pressure, which could be obtained by heating 0.50 mol of sodium nitrate?

[Molar volume of a gas = 24 dm3 mol–1 at room temperature and pressure]

A 3

B 6

C 12

D 24


8 An excess of copper(II) oxide is mixed with 40.0 cm3 of 2.50 mol dm–3 hydrochloric acid.

CuO(s) + 2HCl(aq) CuCl2(aq) + H2O(l)

(a) If the mass of copper(II) chloride produced is 5.50 g, what is the percentage yield of copper(II) chloride?

[Molar mass of copper(II) chloride = 134.4 g mol–1](1)

A 81.8%

B 67.2%

C 40.9%

D 20.4%

(b) The ionic equation for the reaction is(1)

A Cu2+(s) + 2Cl–(aq) CuCl2(aq)

B CuO(s) + 2H+(aq) Cu2+(aq) + H2O(l)

C CuO(s) + 2H+(aq) + 2Cl–(aq) Cu2+(Cl–)2(aq) + H2O(l)

D CuO(s) + 2Cl–(aq) CuCl2(aq) + O2–(l)

5


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(c) Some facts about copper(II) chloride are given below.

Which of these gives the best evidence that the bonding in copper(II) chloride is ionic?

(1)

A It has a melting temperature of 620 C.

B It does not conduct electricity as a solid.

C It decomposes before it reaches its boiling temperature.

D In the electron density map, there are no contour lines around more than one nucleus.


9 The melting temperature of sodium is lower than the melting temperature of magnesium. The best explanation for this is

A sodium atoms are smaller than magnesium atoms.

B sodium ions have a larger charge density than magnesium ions.

C the repulsion between the ions in sodium is less than in magnesium.

D the number of delocalised electrons per atom is fewer in sodium than in magnesium.


10 A trend going down Group 1 is that the

A first ionization energy of the element decreases.

B lattice energy of the chloride becomes more negative.

C radius of the atom decreases.

D melting temperature of the element increases.


11 Which of the following ions has the biggest radius?

A S2–

B Cl–

C K+

D Ca2+


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12 When 0.1 mol of aqueous potassium hydroxide was added to 0.1 mol of nitric acid, 5200 J were transferred to the surroundings. What is the enthalpy change, in kJ mol–1, for this reaction?

KOH(aq) + HNO3(aq) KNO3(aq) + H2O(l)

A –52

B –26

C +26

D +52


13 A compound has the composition 62.1% C, 10.3% H and 27.6% O.

What is its empirical formula?

A CH2O

B C6H2O

C C6H3O

D C3H6O


14 What is the systematic name of the following?

A 3-methyl-2-propylpentane

B 3-methyl-4-propylpentane

C 3,4-dimethylheptane

D 4,5-dimethylheptane


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15 Which of the following shows geometric isomerism?

A prop-1-ene

B but-1-ene

C 1,1-dichloroethene

D 1,2-dichloroethene


16 This question is about the organic compounds with skeletal formulae as shown.

1

2

3

4

(a) Which compounds are isomers?(1)

A 1 and 2

B 1 and 3

C 1 and 4

D 2 and 3

(b) Which compound has the same molecular formula and empirical formula?(1)

A 1

B 2

C 3

D 4


8

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17 What is the formula of poly(but-1-ene)?

A C C C C

H

H

H

H n

⎡

⎣⎢ ⎡

⎣⎢H

H

H

H

B C C

H

H

H

CH2CH3 n

⎡

⎣⎢ ⎡

⎣⎢

C C C

H H

CH3 n

⎡

⎣⎢ ⎡

⎣⎢

CH3

D C C C

H

CH3 n

⎡

⎣⎢ ⎡

⎣⎢H

H

H

H



2

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SECTION A




a cross .

1 How many molecular ion peaks (parent ion peaks) are in the mass spectrum of 1,2-dibromoethane?

Assume the only isotopes present are 1H, 12C, 79Br and 81Br.

A 1

B 2

C 3

D 4


2 Four compounds that contribute to global warming are given below.

A Sulfur hexafluoride

B Dichlorodifluoromethane

C Methane

D Carbon dioxide

(a) Which of these molecules is polar?(1)

A

B

C

D


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(b) Which of these compounds is emitted in the largest quantity by anthropogenic activity?

(1)

A

B

C

D

(c) Which of these compounds depletes the ozone layer?(1)

A

B

C

D

(d) Which of these molecules has an octahedral structure?(1)

A

B

C

D


3 Which of the following is a tertiary alcohol?

A 3-methylbutan-2-ol

B 2-methylbutan-2-ol

C 2-methylbutan-1-ol

D 2,2-dimethylpropan-1-ol


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4 This question is about two isomeric alcohols and two isomeric carbonyl compounds.

Butan-1-ol, CH3CH2CH2CH2OH

Butan-2-ol, CH3CH2CH(OH)CH3

Butanal, CH3CH2CH2CHO

Butanone, CH3CH2COCH3

(a) Which of these compounds would not produce a colour change when heated with acidified sodium dichromate(VI) solution?

(1)

A Butan-1-ol

B Butan-2-ol

C Butanal

D Butanone

(b) Which compound could give a peak at m/e = 31 in its mass spectrum?(1)

A Butan-1-ol

B Butan-2-ol

C Butanal

D Butanone

(c) Which compound could not give a peak at m/e = 43 in its mass spectrum?(1)

A Butan-1-ol

B Butan-2-ol

C Butanal

D Butanone


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(d) The infrared spectrum of one of these compounds is given below.

Wavenumber / cm–1

Tran

smitt

ance

(%)

4000 3000 2000 1500 1000 500

100

50

0

Use the infrared absorptions, in wavenumbers, to identify the compound.

Bond Wavenumber range / cm–1

O–H (alcohol) 3750 – 3200

C–H (alkane) 2962 – 2853

C–H (aldehyde) 2900 – 2820 and 2775 – 2700

C=O (aldehyde or ketone) 1740 – 1680

The compound with this IR spectrum is(1)

A butan-1-ol.

B butan-2-ol.

C butanal.

D butanone.


6

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5 A Maxwell-Boltzmann curve shows the distribution of molecular energies in a reaction system. When the temperature in this system is increased, the peak is

A higher and further to the right.

B higher and further to the left.

C lower and further to the right.

D lower and further to the left.


6 This question is about the equilibrium reaction between hydrogen and carbon dioxide.

H2(g) + CO2(g) H2O(g) + CO(g) H = +40 kJ mol–1

What effect would the following changes have on the rate of reaction and the yield of carbon monoxide?

(a) Increase in temperature.(1)

Rate Yield of CO

A increase increase

B increase decrease

C increase no change

D no change decrease

(b) Increase in pressure.(1)

Rate Yield of CO

A increase increase

B increase decrease

C increase no change

D no change no change


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7 Which is the equation for the reaction when steam passes over strongly heated magnesium?

A Mg(s) + 2H2O(l) Mg(OH)2(aq) + H2(g)

B Mg(s) + 2H2O(g) Mg(OH)2(s) + H2(g)

C Mg(s) + H2O(l) MgO(s) + H2(g)

D Mg(s) + H2O(g) MgO(s) + H2(g)


8 What happens to the solubilities of the hydroxides and sulfates as Group 2 is descended?

Solubility of hydroxides Solubility of sulfates

A decreases decreases

B decreases increases

C increases decreases

D increases increases


9 Which one of the following substances forms when a few drops of concentrated sulfuric acid is added to sodium chloride?

A H2O

B Cl2

C NaHSO4

D SO2



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10 25.00 cm3 of 1.00 mol dm–3 sulfuric acid is fully neutralized by 50.00 cm3 of 1.00 mol dm–3 sodium hydroxide.

(a) What is the concentration of sodium sulfate solution produced by the reaction, in mol dm–3?

(1)

A 1.00

B 0.67

C 0.50

D 0.33

(b) The volumes are measured using burettes, with each burette reading having an uncertainty of ±0.05 cm3.

The percentage error in measuring the 25.00 cm3 of the acid is(1)

A ±0.05%

B ±0.10%

C ±0.20%

D ±0.40%


11 Pentan-1-ol is less soluble than ethanol in water. The best explanation for this is that

A pentan-1-ol molecules cannot form hydrogen bonds with water molecules, but ethanol molecules can.

B London forces are stronger between pentan-1-ol molecules than between ethanol molecules.

C carbon-carbon bonds are stronger in pentan-1-ol than in ethanol.

D permanent dipole forces are stronger in pentan-1-ol than in ethanol.



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12 Along the series of the Group 5 hydrides (NH3, PH3 and AsH3), the boiling temperatures

A decrease.

B decrease then increase.

C increase.

D increase then decrease.



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SECTION A




a cross .

1 Consider the reaction

CH3COOC2H5 + CH3OH CH3COOCH3 + C2H5OH

This is an example of

A acylation.

B hydrolysis.

C substitution.

D transesterification.


2 When a vegetable oil such as palm oil is hydrolysed, the alcohol produced is

A propan-1-ol

B propane-1,2-diol

C propane-1,3-diol

D propane-1,2,3-triol


3 Which of the following types of radiation can directly result in bond breaking?

A Infrared

B Microwave

C Radio wave

D Ultraviolet


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4 The first steps of two different reaction mechanisms are shown.

(a) What do both reaction mechanism steps have in common?(1)

A They involve addition.

B They involve substitution.

C As one bond is made, one bond is broken.

D The attack is on a planar group.

(b) Only one of the first steps above(1)

A leads to the formation of a racemic mixture.

B involves initial attack by a nucleophile.

C involves initial attack by an electrophile.

D leads to an elimination.



C

H

C

H

H

O

C

C

H

H

H

H H

NC–

+

First Reaction Mechanism

C

H

C

H

HBr

C

H

H HHO –

H

SecondReaction Mechanism

+

4

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5 The following molecules are structural isomers with molecular formula C5H10O.

(a) Which of the molecules would exhibit optical isomerism?(1)

A W

B X

C Y

D Z

(b) Which of the molecules would exhibit geometric isomerism?(1)

A W

B X

C Y

D Z

(c) Which of the molecules would produce iodoform when reacting with iodine in alkaline solution?

(1)

A W only

B W and X

C W and Y

D W and Z

C O

C

C

C

HH

H

HH

C

HH

H

H

H

C

OC

C

C

HH

H

HH

C

HH

H

HH C H

C

CH

HH

H

C

OH

H

H

H

CH

CH

CH

C

C

HH

H

OHH

C

HH

H

W X Y Z

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(d) Which of the molecules would be oxidized to a carboxylic acid using acidified sodium dichromate(VI)?

(1)

A X only

B Z only

C X and Y

D X, Y and Z

(e) Which of the molecules would form a crystalline product with 2,4-dinitrophenylhydrazine?

(1)

A W only

B W and X

C W, X and Z

D X only



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6 Chromatography is used to separate the components of a mixture and can be carried out in a range of different ways.

(a) A suitable example of a ‘carrier gas’ in gas chromatography is(1)

A chlorine.

B nitrogen.

C steam.

D not possible to state, as there should be a vacuum.

(b) Separation is achieved in gas chromatography due to the components in the mixture having different

(1)

A interactions with the stationary phase.

B interactions with the mobile phase.

C colours.

D solubility in the moving solvent.



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7 Polyesters are condensation polymers.

(a) PET, polyethylene terephthalate, can be produced from the condensation of ethane-1,2-diol and benzene-1,4-dicarboxylic acid.

Which of the following is the repeat unit of this polymer?(1)

A B

C D

(b) The repeat unit of the biodegradable polymer PHB, is shown below.

This is made from a single monomer which could be(1)

A 2-hydroxybutanoic acid.

B 3-hydroxybutanoic acid.

C 2-hydroxy-2-methylpropanoic acid.

D 3-hydroxy-3-methylpropanoic acid.


C

O

C

O

O CH2 CH2 O O C

O

O CH2 CH2 O

C

O

O O CH2 CH2 O O O C CH2 CH2 C

O O

O CH CH2 C

CH3 O

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8 The reaction of ammonia with propanoyl chloride, C2H5COCl, forms

A C2H5NH2

B C2H5CONH2

C C2H5CH(OH)NH2

D C2H5CONHC2H5


9 The dihydrogenphosphate-hydrogenphosphate ion system is an important buffer in the human body.

H2PO4− + H2O HPO4

2− + H3O+

(a) In this system, there are two acid-base conjugate pairs. These are(1)

acid with its conjugate base base with its conjugate acid

A H2PO4− / HPO4

2− H2O / H3O+

B H2O / H3O+ HPO42− / H2PO4

−

C H3O+ / H2O H2PO4− / HPO4

2−

D H2PO4− / HPO4

2− H3O+ / H2O

(b) A formula that can be used for the calculation of the pH of this buffer solution is

pH = pKa + logHPO

H PO

42

2 4

−

−

⎡⎣

⎤⎦

⎡⎣

⎤⎦

⎛

⎝⎜⎜

⎞

⎠⎟⎟

Calculate the pH of this buffer using

pKa = 7.20 [HPO42–] = 3.98 × 10–8 mol dm–3 [H2PO4

–] = 3.89 × 10–7 mol dm–3

(1)

A 6.19

B 6.21

C 7.20

D 8.19


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10 The Ostwald Process is a method for making nitric acid. The equation for the first stage of this process is

4NH3(g) + 5O2(g) 4NO(g) + 6H2O(g) H = –905 kJ mol−1

(a) The equilibrium yield of nitrogen monoxide, NO, is increased by (1)

A increasing both the pressure and the temperature.

B decreasing both the pressure and the temperature.

C decreasing the pressure and increasing the temperature.

D increasing the pressure and decreasing the temperature.

(b) For this stage of the process, the catalyst is an alloy of platinum and rhodium. A pressure of between 4 and 10 atm and a temperature of 1150 K are used. Unreacted reactants are recycled.

Which one of the following changes will affect the value of the equilibrium constant, Kp?

(1)

A Changing the composition of the platinum-rhodium catalyst.

B Increasing the pressure above 10 atm.

C Decreasing the temperature below 1150 K.

D Not recycling unreacted reactants.



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11 Iodine is soluble in both water and hexane. If iodine is added to a mixture of the two solvents, then the following equilibrium is set up.

I2(aq) I2(hexane)

The equilibrium constant, known as the partition coefficient, is 85.

The density of hexane is 0.66 g cm−3. The density of water is 1.00 g cm−3.

Which of the following diagrams is correct for this system at equilibrium?

A B

C D



Water with low iodine concentration

Water with high iodine concentration

Water with low iodine concentration

Water with high iodine concentration

Hexane with low iodine concentration

Hexane with high iodine concentration

Hexane with high iodine concentration

Hexane with low iodine concentration

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SECTION A




cross .

1 Which of the following gives the oxidation states of manganese in the ions shown?

MnO42− MnO3

–

A +7 +6

B +6 +5

C +7 +5

D +6 +6


2 Which of the following gives the electrodes and electrolyte that are used in an alkaline hydrogen fuel cell?

Electrodes Electrolyte

A graphite potassium hydroxide solution

B graphite water with a little salt

C platinum potassium hydroxide solution

D platinum water with a little salt


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3 Which of the following cannot be used to detect alcohol in a breathalyser test?

A Fractional distillation

B Fuel cell

C Infrared spectroscopy

D Reduction of dichromate(VI) ions


4 A titration using potassium manganate(VII) in dilute sulfuric acid can be used to determine the percentage of

A aspirin in aspirin tablets.

B chlorine in bleach.

C copper in an alloy.

D iron(II) sulfate in iron tablets.


5 Which of the following gives the electronic configurations for a chromium atom and a chromium(II) ion?

Cr Cr2+

A [Ar]3d44s2 [Ar]3d4

B [Ar]3d54s1 [Ar]3d4

C [Ar]3d44s2 [Ar]3d24s2

D [Ar]3d54s1 [Ar]3d34s1


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6 Aqueous sodium hydroxide and aqueous ammonia are added to separate solutions of the same metal ion. The observations are shown in the table below.

Reagent added A few drops Excess

NaOH(aq) green precipitate green precipitate remains

NH3(aq) green precipitate green precipitate dissolves to form a blue solution

The metal ion is

A Cr3+(aq).

B Fe2+(aq).

C Fe3+(aq).

D Ni2+(aq).


7 The reaction between cerium(IV) ions and thallium(I) ions is very slow.

2Ce4+(aq) + Tl+(aq) 2Ce3+(aq) + Tl3+(aq)

Which of these ions could catalyse this reaction?

A Al3+

B Fe3+

C Na+

D Zn2+


8 Which of these hydroxides is amphoteric?

A Cu(OH)2

B Mg(OH)2

C Ni(OH)2

D Zn(OH)2


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9 During a titration between acidified manganate(VII) ions and sulfate(IV) ions, the manganate(VII) ions are reduced to manganese(II) ions and the sulfate(IV) ions are oxidized to sulfate(VI) ions.

The mole ratio of manganate(VII) ions to sulfate(IV) ions in this reaction is

A 5:2

B 7:4

C 2:5

D 4:7


10 The total number of compounds with the structural formula C6H3CH3(NO2)2, which contain a benzene ring, is

A four.

B five.

C six.

D seven.



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11 This question is about the ester shown below.

CH3 CH O C CH2 CH3

OCH3

(a) The number of peaks seen in the low resolution proton nmr spectrum of this ester is

(1)

A two.

B three.

C four.

D five.

(b) The peak in the high resolution proton nmr spectrum corresponding to the proton in bold on the structure above will

(1)

A not be split.

B be split into three peaks.

C be split into four peaks.

D be split into seven peaks.



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12 Safranal is one of the substances that contributes to the aroma of saffron.

O

Separate samples of safranal were tested with bromine water, 2,4-dinitrophenylhydrazine and Fehling’s solution.

What are the final observations when safranal is tested with each of those reagents?

Bromine water 2,4-dinitrophenylhydrazine Fehling’s solution

A orange solution orange solution red precipitate

Bcolourless solution orange precipitate red precipitate

C orange solution orange solution blue solution

Dcolourless solution orange precipitate blue solution



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13 The structure of the organic product of the reaction between phenol and excess bromine water is

A

B

C

D



Br

OH

Br

OH

Br Br

OHBr Br

Br

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14 If it is assumed that the structure of benzene has three localised double bonds (structure X), the calculated standard enthalpy change of hydrogenation is −360 kJ mol–1.

structure X

The actual standard enthalpy change of hydrogenation of benzene is −208 kJ mol–1.

From these data, it can be deduced that the

A actual benzene structure is kinetically more stable than structure X as it requires a high activation energy to react.

B actual benzene structure is thermodynamically more stable than structure X as it has a lower enthalpy content.

C structure X is kinetically unstable as it undergoes addition reactions at room temperature.

D structure X is thermodynamically more stable than the actual benzene structure as the standard enthalpy change of hydrogenation is more exothermic.



+ 3H2

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15 The repeat unit for poly(propenamide) is

A

B

C

D



C C

H

H

NH2

C O

H ⎡

⎣

⎢⎢⎢⎢

⎡

⎣

⎢⎢⎢⎢

N C C C

H H

H

OH

H

⎡

⎣

⎢⎢⎢⎢

⎡

⎣

⎢⎢⎢⎢

N C C C

H H OH ⎡

⎣

⎢⎢⎢⎢

⎡

⎣

⎢⎢⎢⎢

C C

H

NH2

C O

⎡

⎣

⎢⎢⎢⎢

⎡

⎣

⎢⎢⎢⎢

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16 The structures of three amino acids are shown in the table.

Amino acid Structure

cysteine HSCH2CH(NH2)COOH

glycine H2NCH2COOH

threonine CH3CH(OH)CH(NH2)COOH

The tripeptide glycine-cysteine-threonine is

A H2NCH2CONHCH(CH(OH)CH3)CONHCH(CH2SH)COOH

B H2NCH2CONHCH(CH2SH)CONHCH(CH(OH)CH3)COOH

C H2NCH(CH(OH)CH3)CONHCH(CH3SH)CONHCH2COOH

D H2NCH(CH2SH)CONHCH2 CONHCH(CH(OH)CH3)COOH


17 The amino acid alanine, H2NCH(CH3)COOH, exists as a solid at room temperature.

The most important reason for this is that it

A exists as a zwitterion.

B forms hydrogen bonds.

C is amphoteric.

D has strong London forces.


18 Complete combustion of a hydrocarbon produced 0.66 g of carbon dioxide and 0.225 g of water.

Which of the following molecular formulae is consistent with these data?

A C3H6.

B C3H8.

C C6H6.

D C6H10.


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19 Phenol can be produced from benzene as shown in the reaction sequence below.

benzeneMr = 78

Step 1yield 80%

Step 2yield 90%

SO3H OH

phenolMr = 94

The mass of phenol, to 2 decimal places, produced from 3.90 g of benzene is

A 3.38 g.

B 3.76 g.

C 4.23 g.

D 4.70 g.



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