Cambridge International Examinations

Cambridge International General Certificate of Secondary Education

CHEMISTRY 0620/22
Paper 2 Multiple Choice (Extended) May/June 2017

45 minutes
Additional Materials: Multiple Choice Answer Sheet
Soft clean eraser
*6632393932*

Soft pencil (type B or HB is recommended)

READ THESE INSTRUCTIONS FIRST

Write in soft pencil.

Do not use staples, paper clips, glue or correction fluid.
Write your name, Centre number and candidate number on the Answer Sheet in the spaces provided unless
this has been done for you.
DO NOT WRITE IN ANY BARCODES.

There are forty questions on this paper. Answer all questions. For each question there are four possible
answers A, B, C and D.
Choose the one you consider correct and record your choice in soft pencil on the separate Answer Sheet.

Read the instructions on the Answer Sheet very carefully.

Each correct answer will score one mark. A mark will not be deducted for a wrong answer.
Any rough working should be done in this booklet.
A copy of the Periodic Table is printed on page 16.
Electronic calculators may be used.

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

This document consists of 15 printed pages and 1 blank page.

IB17 06_0620_22/2RP
© UCLES 2017 [Turn over
 2

1 Small crystals of purple KMnO4 (Mr = 158) and orange K2Cr2O7 (Mr = 294) were placed at the
centres of separate petri dishes filled with agar jelly. They were left to stand under the same
physical conditions.

After some time, the colour of each substance had spread out as shown.

dish 1 dish 2

KMnO4 K2Cr2O7

The lengths of the arrows indicate the relative distances travelled by particles of each substance.

Which statement is correct?

A Diffusion is faster in dish 1 because the mass of the particles is greater.

B Diffusion is faster in dish 2 because the mass of the particles is greater.
C Diffusion is slower in dish 1 because the mass of the particles is smaller.
D Diffusion is slower in dish 2 because the mass of the particles is greater.

2 Impurities change the melting and boiling points of substances.

Sodium chloride is added to a sample of pure water.

How does the addition of sodium chloride affect the melting point and boiling point of the water?

melting point boiling point

A increases increases
B increases decreases
C decreases increases
D decreases decreases

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3 The diagram shows a chromatogram of four substances.

Which substance has an Rf value of approximately 0.32?

solvent front
19 cm

14 cm
12 cm

6 cm

4 cm

baseline
0 cm
A B C D

4 Which element does not form a stable ion with the same electronic structure as argon?

A aluminium
B chlorine
C phosphorus
D potassium

5 Graphite and diamond are both forms of the element carbon.

Which row shows the number of other carbon atoms that each carbon atom is covalently bonded
to in graphite and diamond?

graphite diamond

A 3 3
B 3 4
C 4 3
D 4 4

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6 Which statement describes metallic bonding?

A The attraction between a lattice of negative ions and delocalised protons.

B The attraction between a lattice of positive ions and delocalised electrons.
C The attraction between delocalised protons and electrons.
D The attraction between oppositely charged ions.

7 Which equations are balanced?

1 Fe2O3 + 3CO → 2Fe + 3CO2

2 ZnCO3 + 2HCl → ZnCl 2 + CO2 + 2H2O

3 Mg(NO3)2 + NaOH → Mg(OH)2 + 2NaNO3

4 CaCO3 + H2SO4 → CaSO4 + H2O + CO2

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

8 Calcium carbide, CaC2, reacts with water to form ethyne, C2H2, and calcium hydroxide.

The equation for the reaction is shown.

CaC2(s) + 2H2O(l) → C2H2(g) + Ca(OH)2(s)

Which volume of ethyne is produced when 6 g of water react completely with calcium carbide?

A 4 dm3 B 8 dm3 C 36 dm3 D 72 dm3

9 Which statement about electrolysis is correct?

A Electrons move through the electrolyte from the cathode to the anode.
B Electrons move towards the cathode in the external circuit.
C Negative ions move towards the anode in the external circuit.
D Positive ions move through the electrolyte towards the anode during electrolysis.

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10 The reactivity series for a number of different metals is shown.

most reactive least reactive

magnesium zinc iron copper silver platinum

The diagram shows different metal strips dipped into an electrolyte.

metal strip metal strip

electrolyte

Which pair of metals produces the highest voltage?

A copper and magnesium

B magnesium and platinum
C magnesium and zinc
D silver and platinum

11 Which statement about fuels is correct?

A Heat energy can only be produced by burning fuels.

B Hydrogen is used as a fuel although it is difficult to store.
C Methane is a good fuel because it produces only water when burned.
D Uranium is burned in air to produce energy.

12 Which statements about exothermic and endothermic reactions are correct?

1 During an exothermic reaction, heat is given out.

2 The temperature of an endothermic reaction goes up because heat is taken in.
3 Burning methane in the air is an exothermic reaction.

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

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13 The equation for the reaction between hydrogen and chlorine is shown.

H2(g) + Cl 2(g) → 2HCl (g)

The reaction is exothermic.

The bond energies are shown in the table.

bond energy
bond
in kJ / mol

Cl –Cl +240
H–Cl +430
H–H +436

What is the energy change for the reaction?

A –1536 kJ / mol
B –184 kJ / mol
C +184 kJ / mol
D +246 kJ / mol

14 A gas is produced when calcium carbonate is heated.

Which type of change is this?

A chemical
B exothermic
C physical
D separation

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15 A student was investigating the reaction between marble chips and dilute hydrochloric acid.

gas syringe

bung

marble
chips 25 cm3 of dilute
hydrochloric acid

Which changes slow down the rate of reaction?

temperature concentration surface area

of acid of acid of marble chips

A decrease decrease decrease

B decrease decrease increase
C increase decrease decrease
D increase increase increase

16 The reaction used to manufacture ammonia from nitrogen and hydrogen is reversible.

An equilibrium can be established between ammonia, nitrogen and hydrogen.

Which statement describes the equilibrium?

A Both the forward reaction and the backward reaction have the same rate.
B The rate of the backward reaction is greater than the rate of the forward reaction.
C The rate of the forward reaction is greater than the rate of the backward reaction.
D The forward and backward reactions have both stopped.

17 An example of a redox reaction is shown.

Zn + Cu2+ → Zn2+ + Cu

Which statement about the reaction is correct?

A Zn is the oxidising agent and it oxidises Cu2+.

B Zn is the oxidising agent and it reduces Cu2+.
C Zn is the reducing agent and it oxidises Cu2+.
D Zn is the reducing agent and it reduces Cu2+.

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18 Which type of oxide is aluminium oxide?

A acidic
B amphoteric
C basic
D neutral

19 Which statements about a weak acid, such as ethanoic acid, are correct?

1 It reacts with a carbonate.

2 It does not neutralise aqueous sodium hydroxide solution.
3 It turns red litmus blue.
4 It is only partially ionised in aqueous solution.

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

20 Silver chloride is a white solid which is insoluble in water.

Which statement describes how a sample of pure silver chloride can be made?

A Add aqueous silver nitrate to aqueous sodium chloride and then filter.
B Add aqueous silver nitrate to dilute hydrochloric acid, evaporate and then crystallise.
C Add silver carbonate to dilute hydrochloric acid, evaporate and then crystallise.
D Add silver to dilute hydrochloric acid, filter and then wash the residue.

21 Dilute sulfuric acid is added to two separate aqueous solutions, X and Y. The observations are
shown.

solution X white precipitate

solution Y bubbles of a colourless gas

Which row shows the ions present in the solutions?

solution X solution Y

A Ba2+ CO32–
B Ca2+ Cl –
C Cu2+ CO32–
D Fe2+ NO3–

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22 Which element is less reactive than the other members of its group in the Periodic Table?

A astatine
B caesium
C fluorine
D rubidium

23 The elements oxygen and sulfur are in the same group of the Periodic Table.

Which statement about oxygen and sulfur is not correct?

A They are non-metals.

B They have giant covalent structures.
C They have six electrons in their outer shells.
D They react together to form an acidic oxide.

24 Why are weather balloons sometimes filled with helium rather than hydrogen?

A Helium is found in air.

B Helium is less dense than hydrogen.
C Helium is more dense than hydrogen.
D Helium is unreactive.

25 Which process is involved in the extraction of zinc from zinc blende?

A Cryolite is added to lower the melting point of zinc blende.

B Molten zinc blende is electrolysed.
C Zinc blende is heated with carbon.
D Zinc blende is roasted in air.

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26 Element E:

• forms an alloy

• has a basic oxide

• is below hydrogen in the reactivity series.

What is E?

A carbon
B copper
C sulfur
D zinc

27 A list of metals is shown.

aluminium
copper
iron
magnesium
silver
zinc

Which metal will displace all of the other metals from aqueous solutions of their salts?

A aluminium
B iron
C magnesium
D zinc

28 Stainless steel is an alloy of iron and other metals. It is strong and does not rust but it costs much
more than normal steel.

What is not made from stainless steel?

A cutlery
B pipes in a chemical factory
C railway lines
D saucepans

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29 The diagram shows some uses of water in the home.

1 2 3

For which uses is it important for the water to have been treated?

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

30 The carbon cycle includes the processes combustion, photosynthesis and respiration.

Which row shows how each process changes the amount of carbon dioxide in the atmosphere?

combustion photosynthesis respiration

A decreases decreases increases

B decreases increases decreases
C increases decreases increases
D increases increases decreases

31 Which statement about the conditions used in the Haber process is not correct?

A A high temperature is used because the forward reaction is exothermic.

B A high pressure is used because there are fewer moles of gas in the products than in the
reactants.
C An iron catalyst is used to increase the rate of the forward reaction.
D The unreacted hydrogen and nitrogen are recycled to increase the amount of ammonia
produced.

32 Which chemical reaction decreases pollution in the air?

A S + O2 → SO2

B N2 + O2 → 2NO

C 2CH4 + 3O2 → 2CO + 4H2O

D 2NO + 2CO → 2CO2 + N2

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33 Which statement about sulfuric acid is correct?

A It is made by the Haber process.

B It is made in the atmosphere by the action of lightning.
C It reacts with ammonia to produce a fertiliser.
D It reacts with copper metal to produce hydrogen gas.

34 Statements about methods of manufacture and uses of calcium oxide are shown.

1 It is manufactured by reacting acids with calcium carbonate.

2 It is manufactured by heating calcium carbonate.
3 It is used to desulfurise flue gases.
4 It is used to treat alkaline soil.

Which statements are correct?

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

35 The industrial fractional distillation of petroleum is shown.

refinery gas

gasoline fraction

naphtha fraction

kerosene fraction

diesel oil

fuel oil fraction

petroleum Y

lubricating fraction
and bitumen

Which process happens at Y?

A burning
B condensation
C cracking
D evaporation

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36 Which statement about homologous series is not correct?

A Alkenes have the same general formula, CnH2n+2.

B Each member of the homologous series of alkanes differs from the next by CH2.
C The members of a homologous series all have similar chemical properties.
D The members of a homologous series all have the same functional group.

37 The diagram shows part of the molecule of a polymer.

H H H H H H H H H

C C C C C C C C C

H H H H H H H H H

Which diagram shows the monomer from which this polymer could be manufactured?

A B C D
H H H H H H H

H C H H C C H C C H C C O H

H H H H H H H

38 Ethanol is manufactured by fermentation or by the catalytic addition of steam to ethene.

What is an advantage of ethanol manufacture by fermentation instead of by the catalytic addition

of steam to ethene?

A Ethanol manufactured by fermentation is purified by distillation.

B Ethanol manufacture by fermentation produces purer ethanol.
C Ethanol manufacture by fermentation uses large areas of land.
D Ethanol manufacture by fermentation uses renewable resources.

39 The formula of an ester is CH3CH2CH2COOCH2CH2CH3.

Which acid and alcohol react together to make the ester?

acid alcohol

A butanoic acid butanol

B butanoic acid propanol
C propanoic acid butanol
D propanoic acid propanol

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40 Polyesters and polyamides are types of synthetic polymer.

Which statements are correct?

1 They are made by addition polymerisation.

2 They are made by condensation polymerisation.
3 The monomers from which they are made are unsaturated hydrocarbons.
4 The monomers from which they are made contain reactive functional groups at their
ends.

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

© UCLES 2017 0620/22/M/J/17

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publisher will be pleased to make amends at the earliest possible opportunity.

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

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

© UCLES 2017 0620/22/M/J/17

 The Periodic Table of Elements
Group
I II III IV V VI VII VIII

© UCLES 2017
1 2
H He
hydrogen helium
Key 1 4
3 4 atomic number 5 6 7 8 9 10
Li Be atomic symbol B C N O F Ne
lithium beryllium name boron carbon nitrogen oxygen fluorine neon
7 9 relative atomic mass 11 12 14 16 19 20
11 12 13 14 15 16 17 18

Na Mg Al Si P S Cl Ar
sodium magnesium aluminium silicon phosphorus sulfur chlorine argon
23 24 27 28 31 32 35.5 40
19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36
K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
potassium calcium scandium titanium vanadium chromium manganese iron cobalt nickel copper zinc gallium germanium arsenic selenium bromine krypton
39 40 45 48 51 52 55 56 59 59 64 65 70 73 75 79 80 84
37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54
Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe
rubidium strontium yttrium zirconium niobium molybdenum technetium ruthenium rhodium palladium silver cadmium indium tin antimony tellurium iodine xenon
85 88 89 91 93 96 – 101 103 106 108 112 115 119 122 128 127 131
16

55 56 57–71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86
lanthanoids
Cs Ba Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn

0620/22/M/J/17
caesium barium hafnium tantalum tungsten rhenium osmium iridium platinum gold mercury thallium lead bismuth polonium astatine radon
133 137 178 181 184 186 190 192 195 197 201 204 207 209 – – –
87 88 89–103 104 105 106 107 108 109 110 111 112 114 116
actinoids
Fr Ra Rf Db Sg Bh Hs Mt Ds Rg Cn Fl Lv
francium radium rutherfordium dubnium seaborgium bohrium hassium meitnerium darmstadtium roentgenium copernicium flerovium livermorium
– – – – – – – – – – – – –

57 58 59 60 61 62 63 64 65 66 67 68 69 70 71
lanthanoids La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
lanthanum cerium praseodymium neodymium promethium samarium europium gadolinium terbium dysprosium holmium erbium thulium ytterbium lutetium
139 140 141 144 – 150 152 157 159 163 165 167 169 173 175
89 90 91 92 93 94 95 96 97 98 99 100 101 102 103
actinoids Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
actinium thorium protactinium uranium neptunium plutonium americium curium berkelium californium einsteinium fermium mendelevium nobelium lawrencium
– 232 231 238 – – – – – – – – – – –

The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
 Cambridge International Examinations
Cambridge International General Certificate of Secondary Education

CHEMISTRY 0620/23
Paper 2 Multiple Choice (Extended) May/June 2017

45 minutes
Additional Materials: Multiple Choice Answer Sheet
Soft clean eraser
*0971587250*

Soft pencil (type B or HB is recommended)

READ THESE INSTRUCTIONS FIRST

Write in soft pencil.

Do not use staples, paper clips, glue or correction fluid.
Write your name, Centre number and candidate number on the Answer Sheet in the spaces provided unless
this has been done for you.
DO NOT WRITE IN ANY BARCODES.

There are forty questions on this paper. Answer all questions. For each question there are four possible
answers A, B, C and D.
Choose the one you consider correct and record your choice in soft pencil on the separate Answer Sheet.

Read the instructions on the Answer Sheet very carefully.

Each correct answer will score one mark. A mark will not be deducted for a wrong answer.
Any rough working should be done in this booklet.
A copy of the Periodic Table is printed on page 16.
Electronic calculators may be used.

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

This document consists of 15 printed pages and 1 blank page.

IB17 06_0620_23/3RP
© UCLES 2017 [Turn over
 2

1 Small crystals of purple KMnO4 (Mr = 158) and orange K2Cr2O7 (Mr = 294) were placed at the
centres of separate petri dishes filled with agar jelly. They were left to stand under the same
physical conditions.

After some time, the colour of each substance had spread out as shown.

dish 1 dish 2

KMnO4 K2Cr2O7

The lengths of the arrows indicate the relative distances travelled by particles of each substance.

Which statement is correct?

A Diffusion is faster in dish 1 because the mass of the particles is greater.

B Diffusion is faster in dish 2 because the mass of the particles is greater.
C Diffusion is slower in dish 1 because the mass of the particles is smaller.
D Diffusion is slower in dish 2 because the mass of the particles is greater.

2 A compound, X, has a melting point of 71 °C and a boiling point of 375 °C.

Which statement about X is correct?

A It is a liquid at 52 °C and a gas at 175 °C.

B It is a liquid at 69 °C and a gas at 380 °C.

C It is a liquid at 75 °C and a gas at 350 °C.

D It is a liquid at 80 °C and a gas at 400 °C.

© UCLES 2017 0620/23/M/J/17

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3 A student used chromatography to analyse a green food colouring.

The chromatogram obtained is shown.

solvent front
blue spot

yellow spot

baseline

The table lists some yellow food dyes and their Rf values.

Which yellow food dye does the green food colouring contain?

yellow food dye Rf value

A Quinolene Yellow 0.48

B Sunset Yellow 0.32
C tartrazine 0.69
D Yellow 2G 0.82

4 The electronic structures of atoms Q and R are shown.

Q R

Q and R form an ionic compound.

What is the formula of the compound?

A QR7 B Q2R4 C QR D Q7R

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5 Which substance is a macromolecule?

A ammonia
B carbon dioxide
C diamond
D water

6 The diagram shows metallic bonding.

Which labels are correct?

X Y

A atomic nucleus outer electron

B metal atom mobile electron
C metal ion mobile electron
D positive ion negative ion

7 Aqueous iron(III) sulfate and aqueous sodium hydroxide react to give a precipitate of
iron(III) hydroxide and a solution of sodium sulfate.

What is the balanced equation for this reaction?

A Fe2(SO4)3(aq) + 2NaOH(aq) → Fe(OH)3(s) + Na2SO4(aq)

B Fe2(SO4)3(aq) + 3NaOH(aq) → Fe(OH)3(s) + 3Na2SO4(aq)

C Fe2(SO4)3(aq) + 6NaOH(aq) → 2Fe(OH)3(s) + 3Na2SO4(aq)

D 2Fe2(SO4)3(aq) + 6NaOH(aq) → 4Fe(OH)3(s) + 6Na2SO4(aq)

8 The equation for the reaction between sodium carbonate and dilute hydrochloric acid is shown.

Na2CO3 + 2HCl → 2NaCl + H2O + CO2

What is the maximum volume of carbon dioxide produced when 26.5 g of sodium carbonate react
with dilute hydrochloric acid?

A 6 dm3 B 12 dm3 C 18 dm3 D 24 dm3

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9 Which statement about electrolysis is correct?

A Electrons move through the electrolyte from the cathode to the anode.
B Electrons move towards the cathode in the external circuit.
C Negative ions move towards the anode in the external circuit.
D Positive ions move through the electrolyte towards the anode during electrolysis.

10 The reactivity series for a number of different metals is shown.

most reactive least reactive

magnesium zinc iron copper silver platinum

The diagram shows different metal strips dipped into an electrolyte.

metal strip metal strip

electrolyte

Which pair of metals produces the highest voltage?

A copper and magnesium

B magnesium and platinum
C magnesium and zinc
D silver and platinum

11 Heat energy is produced when hydrocarbons burn in air.

Which equations represent this statement?

1 C2H5OH + 3O2 → 2CO2 + 3H2O

2 C2H4 + 3O2 → 2CO2 + 2H2O

3 CH4 + 2O2 → CO2 + 2H2O

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

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12 Which statements about exothermic and endothermic reactions are correct?

1 During an exothermic reaction, heat is given out.

2 The temperature of an endothermic reaction goes up because heat is taken in.
3 Burning methane in the air is an exothermic reaction.

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

13 Hydrogen and chlorine react to form hydrogen chloride.

The reaction is exothermic.

H2(g) + Cl 2(g) → 2HCl (g)

The overall energy change for this reaction is –184 kJ / mol.

The table gives some of the bond energies involved.

bond energy in
bond
kJ / mol

H–Cl +430
H–H +436

What is the energy of the Cl–Cl bond?

A –240 kJ / mol
B –190 kJ / mol
C +190 kJ / mol
D +240 kJ / mol

14 Which changes are physical changes?

1 melting ice to form water

2 burning hydrogen to form water
3 adding sodium to water
4 boiling water to form steam

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

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 7

15 A student was investigating the reaction between marble chips and dilute hydrochloric acid.

gas syringe

bung

marble
chips 25 cm3 of dilute
hydrochloric acid

Which changes slow down the rate of reaction?

temperature concentration surface area

of acid of acid of marble chips

A decrease decrease decrease

B decrease decrease increase
C increase decrease decrease
D increase increase increase

16 Hydrogen is produced when methane reacts with steam.

The equation for the reaction is shown.

CH4(g) + H2O(g) CO(g) + 3H2(g)

The forward reaction is endothermic.

Which conditions produce the highest yield of hydrogen?

pressure temperature

A high high
B high low
C low high
D low low

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17 An example of a redox reaction is shown.

Zn + Cu2+ → Zn2+ + Cu

Which statement about the reaction is correct?

A Zn is the oxidising agent and it oxidises Cu2+.

B Zn is the oxidising agent and it reduces Cu2+.
C Zn is the reducing agent and it oxidises Cu2+.
D Zn is the reducing agent and it reduces Cu2+.

18 Which oxide is amphoteric?

A Al 2O3 B CaO C Na2O D SO2

19 Chloric(I) acid, HCl O, is formed when chlorine dissolves in water. It is a weak acid.

What is meant by the term weak acid ?

A It contains fewer hydrogen atoms than a strong acid.

B It is easily neutralised by a strong alkali.
C It is less concentrated than a strong acid.
D It is only partially ionised in solution.

20 Silver nitrate reacts with sodium chloride to produce silver chloride and sodium nitrate. The
equation for the reaction is shown.

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

How is silver chloride separated from the reaction mixture?

A crystallisation
B distillation
C evaporation
D filtration

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21 Aqueous sodium hydroxide reacts with an aqueous solution of compound Y to give a green
precipitate.

Aqueous ammonia also reacts with an aqueous solution of compound Y to give a green
precipitate.

In each case the precipitate is insoluble when an excess of reagent is added.

Which ion is present in Y?

A chromium(III)

B copper(II)

C iron(II)

D iron(III)

22 Which element is less reactive than the other members of its group in the Periodic Table?

A astatine
B caesium
C fluorine
D rubidium

23 Ununseptium (atomic number 117) is a man-made element that is below astatine in Group VII of
the Periodic Table.

What is the expected state of ununseptium at room temperature?

A a diatomic gas
B a liquid
C a monatomic gas
D a solid

24 Why are weather balloons sometimes filled with helium rather than hydrogen?

A Helium is found in air.

B Helium is less dense than hydrogen.
C Helium is more dense than hydrogen.
D Helium is unreactive.

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25 Which equation from the zinc extraction process shows the metal being produced by reduction?

A ZnO + C → Zn + CO

B 2ZnS + 3O2 → 2ZnO + 2SO2

C Zn(g) → Zn(l)

D Zn(l) → Zn(s)

26 Element E:

• forms an alloy

• has a basic oxide

• is below hydrogen in the reactivity series.

What is E?

A carbon
B copper
C sulfur
D zinc

27 The section of the reactivity series shown includes a newly discovered element, symbol X.

The only oxide of X has the formula XO.

Ca
Mg
Fe
X
H
Cu

Which equation shows a reaction which occurs?

A Cu(s) + X2+(aq) → Cu2+(aq) + X(s)

B 2X(s) + Cu2+(aq) → 2X+(aq) + Cu(s)

C X(s) + Fe2O3(s) → 2Fe(s) + 3XO(s)

D X(s) + 2HCl (aq) → XCl 2(aq) + H2(g)

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 11

28 Stainless steel is an alloy of iron and other metals. It is strong and does not rust but it costs much
more than normal steel.

What is not made from stainless steel?

A cutlery
B pipes in a chemical factory
C railway lines
D saucepans

29 The diagram shows some uses of water in the home.

1 2 3

For which uses is it important for the water to have been treated?

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

30 The carbon cycle describes how carbon dioxide gas is added to or removed from the
atmosphere.

Which row describes the movement of carbon dioxide during each process?

photosynthesis combustion respiration

A added to the added to the removed from
atmosphere atmosphere the atmosphere
B added to the removed from added to the
atmosphere the atmosphere atmosphere
C removed from added to the added to the
the atmosphere atmosphere atmosphere
D removed from added to the removed from
the atmosphere atmosphere the atmosphere

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 12

31 Which row gives the catalyst for the Haber process and the sources of the raw materials?

source of source of
catalyst
hydrogen nitrogen

A iron electrolysis fertiliser

B iron methane air
C vanadium pentoxide methane air
D vanadium pentoxide methane fertiliser

32 Petrol burns in a car engine to produce waste gases which leave through the car exhaust.

One of these waste gases is an oxide of nitrogen.

Which statement describes how this oxide of nitrogen is formed?

A Carbon dioxide reacts with nitrogen in the catalytic converter.

B Nitrogen reacts with oxygen in the car engine.
C Nitrogen reacts with oxygen in the catalytic converter.
D Petrol combines with nitrogen in the car engine.

33 Which statement about sulfuric acid is correct?

A It is made by the Haber process.

B It is made in the atmosphere by the action of lightning.
C It reacts with ammonia to produce a fertiliser.
D It reacts with copper metal to produce hydrogen gas.

34 Two equations are shown.

reaction 1 CaCO3 → CaO + CO2

reaction 2 CaO + H2O → Ca(OH)2

Which terms describe reactions 1 and 2?

reaction 1 reaction 2

A reduction hydration
B reduction hydrolysis
C thermal decomposition hydration
D thermal decomposition hydrolysis

© UCLES 2017 0620/23/M/J/17

 13

35 Fuel oil, gasoline, kerosene and naphtha are four fractions obtained from the fractional distillation
of petroleum.

What is the order of the boiling points of these fractions?

highest boiling point → lowest boiling point

A fuel oil → kerosene → gasoline → naphtha

B fuel oil → kerosene → naphtha → gasoline
C gasoline → naphtha → kerosene → fuel oil
D naphtha → gasoline → kerosene → fuel oil

36 Butane and methylpropane are isomers with molecular formula C4H10.

Which statements are correct?

1 They have similar chemical properties.

2 They have the same general formula.
3 They have the same structural formula.

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

37 The diagram shows part of the molecule of a polymer.

H H H H H H H H H

C C C C C C C C C

H H H H H H H H H

Which diagram shows the monomer from which this polymer could be manufactured?

A B C D
H H H H H H H

H C H H C C H C C H C C O H

H H H H H H H

© UCLES 2017 0620/23/M/J/17 [Turn over

 14

38 Ethanol can be produced by fermentation or by the catalytic addition of steam to ethene.

Which row shows an advantage and a disadvantage for each process?

catalytic addition
fermentation
of steam to ethene
advantage disadvantage advantage disadvantage
A batch slow continuous fast
process reaction process reaction
B fast continuous pure ethanol renewable
reaction process formed raw material
C renewable batch pure ethanol slow
raw material process formed reaction
D renewable impure ethanol fast finite raw
raw material formed reaction material

39 The structure of an ester is shown.

H H O
H C C C H H

H H O C C H

H H

Which alcohol and carboxylic acid produce this ester?

alcohol carboxylic acid

A ethanol ethanoic acid

B ethanol propanoic acid
C propanol ethanoic acid
D propanol propanoic acid

40 How can the amino acids in a protein be separated and identified?

A Add a locating agent to the protein.

B Hydrolyse the protein and then use chromatography.
C Polymerise the protein and then add a locating agent.
D Use chromatography on a solution of the protein.

© UCLES 2017 0620/23/M/J/17

 15

BLANK PAGE

Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.

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

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

© UCLES 2017 0620/23/M/J/17

 The Periodic Table of Elements
Group
I II III IV V VI VII VIII

© UCLES 2017
1 2
H He
hydrogen helium
Key 1 4
3 4 atomic number 5 6 7 8 9 10
Li Be atomic symbol B C N O F Ne
lithium beryllium name boron carbon nitrogen oxygen fluorine neon
7 9 relative atomic mass 11 12 14 16 19 20
11 12 13 14 15 16 17 18

Na Mg Al Si P S Cl Ar
sodium magnesium aluminium silicon phosphorus sulfur chlorine argon
23 24 27 28 31 32 35.5 40
19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36
K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
potassium calcium scandium titanium vanadium chromium manganese iron cobalt nickel copper zinc gallium germanium arsenic selenium bromine krypton
39 40 45 48 51 52 55 56 59 59 64 65 70 73 75 79 80 84
37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54
Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe
rubidium strontium yttrium zirconium niobium molybdenum technetium ruthenium rhodium palladium silver cadmium indium tin antimony tellurium iodine xenon
85 88 89 91 93 96 – 101 103 106 108 112 115 119 122 128 127 131
16

55 56 57–71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86
lanthanoids
Cs Ba Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn

0620/23/M/J/17
caesium barium hafnium tantalum tungsten rhenium osmium iridium platinum gold mercury thallium lead bismuth polonium astatine radon
133 137 178 181 184 186 190 192 195 197 201 204 207 209 – – –
87 88 89–103 104 105 106 107 108 109 110 111 112 114 116
actinoids
Fr Ra Rf Db Sg Bh Hs Mt Ds Rg Cn Fl Lv
francium radium rutherfordium dubnium seaborgium bohrium hassium meitnerium darmstadtium roentgenium copernicium flerovium livermorium
– – – – – – – – – – – – –

57 58 59 60 61 62 63 64 65 66 67 68 69 70 71
lanthanoids La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
lanthanum cerium praseodymium neodymium promethium samarium europium gadolinium terbium dysprosium holmium erbium thulium ytterbium lutetium
139 140 141 144 – 150 152 157 159 163 165 167 169 173 175
89 90 91 92 93 94 95 96 97 98 99 100 101 102 103
actinoids Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
actinium thorium protactinium uranium neptunium plutonium americium curium berkelium californium einsteinium fermium mendelevium nobelium lawrencium
– 232 231 238 – – – – – – – – – – –

The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
 Cambridge International Examinations
Cambridge International General Certificate of Secondary Education

CHEMISTRY 0620/21
Paper 2 Multiple Choice (Extended) May/June 2017

45 minutes
Additional Materials: Multiple Choice Answer Sheet
Soft clean eraser
*8889844006*

Soft pencil (type B or HB is recommended)

READ THESE INSTRUCTIONS FIRST

Write in soft pencil.

Do not use staples, paper clips, glue or correction fluid.
Write your name, Centre number and candidate number on the Answer Sheet in the spaces provided unless
this has been done for you.
DO NOT WRITE IN ANY BARCODES.

There are forty questions on this paper. Answer all questions. For each question there are four possible
answers A, B, C and D.
Choose the one you consider correct and record your choice in soft pencil on the separate Answer Sheet.

Read the instructions on the Answer Sheet very carefully.

Each correct answer will score one mark. A mark will not be deducted for a wrong answer.
Any rough working should be done in this booklet.
A copy of the Periodic Table is printed on page 16.
Electronic calculators may be used.

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

This document consists of 16 printed pages.

IB17 O6_0620_21_VI_LIL/FP
© UCLES 2017 [Turn over
 2

1 Small crystals of purple KMnO4 (Mr = 158) and orange K2Cr2O7 (Mr = 294) were placed at the
centres of separate petri dishes filled with agar jelly. They were left to stand under the same
physical conditions.

After some time, the colour of each substance had spread out as shown.

dish 1 dish 2

KMnO4 K2Cr2O7

The lengths of the arrows indicate the relative distances travelled by particles of each substance.

Which statement is correct?

A Diffusion is faster in dish 1 because the mass of the particles is greater.

B Diffusion is faster in dish 2 because the mass of the particles is greater.
C Diffusion is slower in dish 1 because the mass of the particles is smaller.
D Diffusion is slower in dish 2 because the mass of the particles is greater.

2 Pure water has a boiling point of 100 °C and a freezing point of 0 °C.

What is the boiling point and freezing point of a sample of aqueous sodium chloride?

boiling point / °C freezing point / °C

A 98 –2
B 98 2
C 102 –2
D 102 2

© UCLES 2017 0620/21/M/J/17

 3

3 A chromatogram obtained from the chromatography of four substances is shown.

Which substance has an Rf value of 0.6?

solvent front

10.5 cm

5.8 cm 6.3 cm
5.5 cm 5.2 cm
baseline
A B C D

4 Sodium reacts with chlorine to form sodium chloride.

Which statements describe what happens to the sodium atoms in this reaction?

1 Sodium atoms form positive ions.

2 Sodium atoms form negative ions.
3 Sodium atoms gain electrons.
4 Sodium atoms lose electrons.

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

5 Diamond is extremely hard and does not conduct electricity.

Which statement explains these properties?

A It has a lattice of positive carbon ions in a ‘sea of electrons’.

B It has delocalised electrons and each carbon atom forms three covalent bonds with other
carbon atoms.
C It has no delocalised electrons and each carbon atom forms four covalent bonds with other
carbon atoms.
D It has strong ionic bonds between each carbon atom.

6 Which statement about metals is not correct?

A Metals are malleable because the metal ions can slide over one another.
B Metals conduct electricity because electrons can move through the lattice.
C Metals consist of a giant lattice of metal ions in a ‘sea of electrons’.
D Metals have high melting points because of the strong attraction between the metal ions.

© UCLES 2017 0620/21/M/J/17 [Turn over

 4

7 Aluminium reacts with fluorine.

xAl (s) + y F2(g) → zAl F3(s)

Which values of x, y and z balance the equation?

x y z

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

8 Carbon monoxide burns in oxygen to produce carbon dioxide.

2CO(g) + O2(g) → 2CO2(g)

Which mass of carbon dioxide is produced from 14 g of carbon monoxide?

A 22 g B 28 g C 44 g D 88 g

9 Which statement about electrolysis is correct?

A Electrons move through the electrolyte from the cathode to the anode.
B Electrons move towards the cathode in the external circuit.
C Negative ions move towards the anode in the external circuit.
D Positive ions move through the electrolyte towards the anode during electrolysis.

© UCLES 2017 0620/21/M/J/17

 5

10 The reactivity series for a number of different metals is shown.

most reactive least reactive

magnesium zinc iron copper silver platinum

The diagram shows different metal strips dipped into an electrolyte.

metal strip metal strip

electrolyte

Which pair of metals produces the highest voltage?

A copper and magnesium

B magnesium and platinum
C magnesium and zinc
D silver and platinum

11 Some properties of four fuels are shown in the table.

Which fuel is a gas at room temperature and makes two products when it burns in a plentiful
supply of air?

melting point boiling point

fuel formula
/ °C / °C

A hydrogen H2 –259 –253

B methane CH4 –182 –164
C octane C8H18 –57 126
D wax C31H64 60 400

© UCLES 2017 0620/21/M/J/17 [Turn over

 6

12 Which statements about exothermic and endothermic reactions are correct?

1 During an exothermic reaction, heat is given out.

2 The temperature of an endothermic reaction goes up because heat is taken in.
3 Burning methane in the air is an exothermic reaction.

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

13 Chlorine reacts with ethane to produce chloroethane and hydrogen chloride.

H H H H

H C C H + Cl Cl H C C Cl + H Cl

H H H H

The reaction is exothermic.

The bond energies are shown in the table.

bond energy
bond
in kJ / mol

C–Cl +340
C–C +350
C–H +410
Cl –Cl +240
H–Cl +430

What is the energy change for the reaction?

A –1420 kJ / mol
B –120 kJ / mol
C +120 kJ / mol
D +1420 kJ / mol

© UCLES 2017 0620/21/M/J/17

 7

14 When sulfur is heated it undergoes a ......1...... change as it melts.

Further heating causes the sulfur to undergo a ......2...... change and form sulfur dioxide.

Which words complete gaps 1 and 2?

1 2

A chemical chemical
B chemical physical
C physical chemical
D physical physical

15 A student was investigating the reaction between marble chips and dilute hydrochloric acid.

gas syringe

bung

marble
chips 25 cm3 of dilute
hydrochloric acid

Which changes slow down the rate of reaction?

temperature concentration surface area

of acid of acid of marble chips

A decrease decrease decrease

B decrease decrease increase
C increase decrease decrease
D increase increase increase

© UCLES 2017 0620/21/M/J/17 [Turn over

 8

16 Nitrogen, hydrogen and ammonia gases are placed inside a container. The container is then
sealed. After some time, an equilibrium forms.

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

Which statement describes the equilibrium in this container?

A The amount of ammonia remains constant from the moment the container is sealed.
B The amounts of ammonia, nitrogen and hydrogen in the container are always equal.
C The rate of formation of ammonia is equal to the rate of decomposition of ammonia.
D The rate of formation of ammonia is faster than the rate of decomposition of ammonia.

17 An example of a redox reaction is shown.

Zn + Cu2+ → Zn2+ + Cu

Which statement about the reaction is correct?

A Zn is the oxidising agent and it oxidises Cu2+.

B Zn is the oxidising agent and it reduces Cu2+.
C Zn is the reducing agent and it oxidises Cu2+.
D Zn is the reducing agent and it reduces Cu2+.

18 Zinc oxide is amphoteric.

Which row describes the reactions of zinc oxide?

reaction with
reaction with
aqueous
hydrochloric acid
sodium hydroxide

A   key
B   = reaction occurs
C   = reaction does not occur
D  

© UCLES 2017 0620/21/M/J/17

 9

19 Which row shows how the hydrogen ion concentration and pH of ethanoic acid compare to those
of hydrochloric acid of the same concentration?

ethanoic acid compared to

hydrochloric acid
hydrogen ion
pH
concentration

A higher higher
B higher lower
C lower higher
D lower lower

20 A pure sample of the insoluble salt barium carbonate can be made using the method given.

step 1 Dissolve barium chloride in water.

step 2 Separately dissolve sodium carbonate in water.
step 3 Mix the two solutions together.
step 4 Filter the mixture.
step 5
step 6 Dry the residue between two sheets of filter paper.

Which instruction is missing from step 5?

A Heat the residue to dryness.

B Heat the residue to the point of crystallisation.
C Place the filtrate in an evaporating basin.
D Wash the residue with water.

21 Substance X reacts with warm dilute hydrochloric acid to produce a gas which decolourises
acidified aqueous potassium manganate(VII).

Substance X gives a yellow flame in a flame test.

What is X?

A potassium chloride
B potassium sulfite
C sodium chloride
D sodium sulfite

© UCLES 2017 0620/21/M/J/17 [Turn over

 10

22 Which element is less reactive than the other members of its group in the Periodic Table?

A astatine
B caesium
C fluorine
D rubidium

23 The elements in Group IV of the Periodic Table are shown.

carbon
silicon
germanium
tin
lead
flerovium

What does not occur in Group IV as it is descended?

A The proton number of the elements increases.

B The elements become more metallic.
C The elements have more electrons in their outer shells.
D The elements have more electron shells.

24 Why are weather balloons sometimes filled with helium rather than hydrogen?

A Helium is found in air.

B Helium is less dense than hydrogen.
C Helium is more dense than hydrogen.
D Helium is unreactive.

© UCLES 2017 0620/21/M/J/17

 11

25 Metal X is added to a colourless aqueous solution of the sulfate of metal Y.

A coloured solution is formed and metal Y is deposited at the bottom of the beaker.

Which row describes elements X and Y and their relative reactivity?

type of element relative reactivity

A X is a transition element X is more reactive than Y

B X is a transition element Y is more reactive than X
C Y is a transition element X is more reactive than Y
D Y is a transition element Y is more reactive than X

26 Element E:

• forms an alloy

• has a basic oxide

• is below hydrogen in the reactivity series.

What is E?

A carbon
B copper
C sulfur
D zinc

27 Zinc metal is extracted from its ore zinc blende in a similar method to that used to extract iron
from hematite.

In which way is zinc extraction different from iron extraction?

A Carbon and carbon monoxide are the main reducing agents.

B Hot air at the base of the furnace reacts with coke to keep the furnace hot.
C The metal is removed as a vapour at the top of the furnace.
D The metal oxide is added into the top of the furnace.

© UCLES 2017 0620/21/M/J/17 [Turn over

 12

28 Stainless steel is an alloy of iron and other metals. It is strong and does not rust but it costs much
more than normal steel.

What is not made from stainless steel?

A cutlery
B pipes in a chemical factory
C railway lines
D saucepans

29 The diagram shows some uses of water in the home.

1 2 3

For which uses is it important for the water to have been treated?

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

30 Oxides of nitrogen are found in polluted air.

Which statement about oxides of nitrogen is correct?

A Oxides of nitrogen are formed by the reaction of nitrogen with oxygen during the fractional
distillation of liquid air.
B Oxides of nitrogen are formed in a car engine by the reaction of petrol with nitrogen from the
air.
C Oxides of nitrogen are removed from exhaust gases by reaction with carbon dioxide in a
catalytic converter.
D Oxides of nitrogen are removed from exhaust gases by reduction in a catalytic converter.

© UCLES 2017 0620/21/M/J/17

 13

31 Photosynthesis and respiration are important natural processes.

Which statement is correct?

A Carbon dioxide is formed by the reaction of glucose with water during photosynthesis.
B Carbon dioxide is removed from the air by respiration.
C Glucose reacts with water to form oxygen during respiration.
D Photosynthesis produces glucose and oxygen.

32 Which row gives the conditions for the Haber process?

pressure
temperature / °C catalyst
/ atm

A 200 2 V2O5
B 200 450 Fe
C 450 200 Fe
D 500 250 V2O5

33 Which statement about sulfuric acid is correct?

A It is made by the Haber process.

B It is made in the atmosphere by the action of lightning.
C It reacts with ammonia to produce a fertiliser.
D It reacts with copper metal to produce hydrogen gas.

34 Which statement is not correct?

A Converting limestone into lime is a thermal decomposition reaction.

B Flue gas desulfurisation is a neutralisation reaction.
C In the extraction of iron, calcium carbonate is converted into calcium oxide.
D Slaked lime is added to soil as a fertiliser.

© UCLES 2017 0620/21/M/J/17 [Turn over

 14

35 Which fraction of petroleum is not matched to its correct use?

fraction use

A bitumen making roads

B gasoline fuel for cars
C kerosene fuel for ships
D naphtha chemical industry

36 The diagram shows the structures of two organic molecules.

H H H H O H

H C C O H H C C C C H

H H H H H H

Which statement about these molecules is not correct?

A They are both alcohols.

B They both produce carbon dioxide and water when they burn in oxygen.
C They contain different functional groups.
D They have the same general formula.

37 The diagram shows part of the molecule of a polymer.

H H H H H H H H H

C C C C C C C C C

H H H H H H H H H

Which diagram shows the monomer from which this polymer could be manufactured?

A B C D
H H H H H H H

H C H H C C H C C H C C O H

H H H H H H H

© UCLES 2017 0620/21/M/J/17

 15

38 Ethanol is manufactured by fermentation or by the catalytic addition of steam to ethene.

Which statement is correct?

A Fermentation uses a higher temperature than the catalytic addition of steam to ethene.
B Fermentation uses a non-renewable resource.
C The catalytic addition of steam to ethene produces purer ethanol than fermentation.
D The catalytic addition of steam to ethene uses a biological catalyst.

39 The structure of an ester is shown.

H H O
H C C C H

H H O C H

Which row is correct?

names of the carboxylic acid and

name of ester
the alcohol used to form the ester

A methyl propanoate methanoic acid and propanol

B methyl propanoate methanol and propanoic acid
C propyl methanoate methanoic acid and propanol
D propyl methanoate methanol and propanoic acid

40 Keratin is a protein that is found in human hair.

Keratin is chemically broken down to produce amino acids.

What is the name of this chemical process?

A catalysis
B hydration
C hydrolysis
D polymerisation

Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.

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

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

© UCLES 2017 0620/21/M/J/17

 The Periodic Table of Elements
Group
I II III IV V VI VII VIII

© UCLES 2017
1 2
H He
hydrogen helium
Key 1 4
3 4 atomic number 5 6 7 8 9 10
Li Be atomic symbol B C N O F Ne
lithium beryllium name boron carbon nitrogen oxygen fluorine neon
7 9 relative atomic mass 11 12 14 16 19 20
11 12 13 14 15 16 17 18

Na Mg Al Si P S Cl Ar
sodium magnesium aluminium silicon phosphorus sulfur chlorine argon
23 24 27 28 31 32 35.5 40
19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36
K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
potassium calcium scandium titanium vanadium chromium manganese iron cobalt nickel copper zinc gallium germanium arsenic selenium bromine krypton
39 40 45 48 51 52 55 56 59 59 64 65 70 73 75 79 80 84
37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54
Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe
rubidium strontium yttrium zirconium niobium molybdenum technetium ruthenium rhodium palladium silver cadmium indium tin antimony tellurium iodine xenon
85 88 89 91 93 96 – 101 103 106 108 112 115 119 122 128 127 131
16

55 56 57–71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86
lanthanoids
Cs Ba Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn

0620/21/M/J/17
caesium barium hafnium tantalum tungsten rhenium osmium iridium platinum gold mercury thallium lead bismuth polonium astatine radon
133 137 178 181 184 186 190 192 195 197 201 204 207 209 – – –
87 88 89–103 104 105 106 107 108 109 110 111 112 114 116
actinoids
Fr Ra Rf Db Sg Bh Hs Mt Ds Rg Cn Fl Lv
francium radium rutherfordium dubnium seaborgium bohrium hassium meitnerium darmstadtium roentgenium copernicium flerovium livermorium
– – – – – – – – – – – – –

57 58 59 60 61 62 63 64 65 66 67 68 69 70 71
lanthanoids La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
lanthanum cerium praseodymium neodymium promethium samarium europium gadolinium terbium dysprosium holmium erbium thulium ytterbium lutetium
139 140 141 144 – 150 152 157 159 163 165 167 169 173 175
89 90 91 92 93 94 95 96 97 98 99 100 101 102 103
actinoids Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
actinium thorium protactinium uranium neptunium plutonium americium curium berkelium californium einsteinium fermium mendelevium nobelium lawrencium
– 232 231 238 – – – – – – – – – – –

The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).