cambridge international examinations cambridge ... · a calcium nitrate from calcium carbonate and...

The syllabus is approved for use in England, Wales and Northern Ireland as a Cambridge International Level1/Level 2 Certificate.

This document consists of 14 printed pages and 2 blank pages.

IB17 06_0620_11/FP © UCLES 2017 [Turn over

*2950887077*

Cambridge International Examinations Cambridge International General Certificate of Secondary Education

CHEMISTRY 0620/11

Paper 1 Multiple Choice (Core) May/June 2017

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

READ THESE INSTRUCTIONS FIRST Write in soft pencil. Do not use staples, paper clips, glue or correction fluid. Write your name, Centre number and candidate number on the Answer Sheet in the spaces provided unless this has been done for you. DO NOT WRITE IN ANY BARCODES. There are forty questions on this paper. Answer all questions. For each question there are four possible answers A, B, C and D. Choose the one you consider correct and record your choice in soft pencil on the separate Answer Sheet. Read the instructions on the Answer Sheet very carefully. Each correct answer will score one mark. A mark will not be deducted for a wrong answer. Any rough working should be done in this booklet. A copy of the Periodic Table is printed on page 16. Electronic calculators may be used.

2

© UCLES 2017 0620/11/M/J/17

1 The diagram shows some changes of state.

solid liquid gas

P Q

R S

Which words describe the changes of state, P, Q, R and S?

P Q R S

A freezing boiling melting evaporation

B melting evaporation freezing condensation

C melting sublimation freezing evaporation

D sublimation evaporation melting condensation 2 The diagram shows part of a thermometer.

31

30

What is the reading on the thermometer?

A 30.2 B 30.3 C 31.7 D 31.8 3 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

3

© UCLES 2017 0620/11/M/J/17 [Turn over

4 Pure copper(II) sulfate crystals can be made by adding copper(II) oxide to hot dilute sulfuric acid.

The copper(II) oxide is added until it ......1...... .

The solution is ......2...... and then ......3...... to obtain the pure crystals.

Which words complete gaps 1, 2 and 3?

1 2 3

A is in excess cooled filtered

B is in excess filtered cooled

C changes colour cooled filtered

D changes colour filtered cooled 5 Which part of an atom has a relative mass of 1 and a relative charge of 0?

A electron

B neutron

C nucleus

D proton 6 Which molecule contains exactly two single covalent bonds?

A Cl 2 B CH4 C H2O D HCl 7 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

4

© UCLES 2017 0620/11/M/J/17

8 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. 9 What is the relative formula mass of ammonium nitrate, NH4NO3?

A 80 B 108 C 122 D 150 10 Concentrated aqueous sodium chloride is electrolysed.

What is the main product formed at the positive electrode (anode)?

A chlorine

B hydrogen

C oxygen

D sodium 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?

fuel formula melting point / °C

boiling point / °C

A hydrogen H2 –259 –253

B methane CH4 –182 –164

C octane C8H18 –57 126

D wax C31H64 60 400

5


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 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 14 Which row correctly matches the experiment and observations to the identity of the underlined

substance?

experiment and observations identity of the underlined substance

A

Blue crystals are heated. The crystals turn white and steam is given off.

hydrated cobalt(II) chloride

B

Pink crystals are heated. The crystals turn blue and steam is given off.

anhydrous cobalt(II) chloride

C

Water is added to a blue solid. The blue solid turns pink.

hydrated copper(II) sulfate

D

Water is added to a white solid. The white solid turns blue.

anhydrous copper(II) sulfate

6

© UCLES 2017 0620/11/M/J/17

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

bung

marblechips 25 cm3 of dilute

hydrochloric acid

gas syringe

Which changes slow down the rate of reaction?

temperature of acid

concentration of acid

surface area of marble chips

A decrease decrease decrease

B decrease decrease increase

C increase decrease decrease

D increase increase increase 16 The reactions shown may occur in the air during a thunder-storm.

N2 + O2 2NO

2NO + O2 2NO2

NO + O3 NO2 + O2

Which row shows what happens to the reactant molecules in each of these reactions?

N2 NO O3

A oxidised oxidised oxidised

B oxidised oxidised reduced

C reduced reduced oxidised

D reduced reduced reduced

7


17 Hydrochloric acid is added to magnesium metal and to sodium carbonate in separate tests.

Which row shows the observations?

magnesium metal sodium carbonate

A effervescence effervescence

B effervescence no reaction

C no reaction effervescence

D no reaction no reaction 18 Which oxide dissolves in water to form a basic solution?

A carbon dioxide

B nitrogen dioxide

C sodium oxide

D sulfur dioxide 19 Which salt preparation uses a burette and a pipette?

A calcium nitrate from calcium carbonate and nitric acid

B copper(II) sulfate from copper(II) hydroxide and sulfuric acid

C potassium chloride from potassium hydroxide and hydrochloric acid

D zinc chloride from zinc and hydrochloric acid 20 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

8

© UCLES 2017 0620/11/M/J/17

21 Part of the Periodic Table is shown.

Which element is a soft solid that reacts violently with cold water?

DC

AB

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 An element has the following properties.

It forms coloured compounds.

It acts as a catalyst.

It melts at 1539 °C.

In which part of the Periodic Table is the element found?

A Group I

B Group VII

C Group VIII

D transition elements 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.

9


25 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 26 Some reactions of three metals and their oxides are shown.

metal metal reacts with dilute hydrochloric acid

metal oxide reacts with carbon

S no yes

T yes no

U yes yes

What is the order of reactivity of the metals?

least reactive most

reactive

A S T U

B S U T

C T S U

D U T S 27 Which statement about the extraction of iron in a blast furnace is not correct?

A Calcium oxide reacts with acidic impurities.

B Iron(III) oxide is reduced to iron by carbon dioxide.

C Molten iron is formed at the base of the blast furnace.

D The raw materials are hematite, limestone and coke.

10

© UCLES 2017 0620/11/M/J/17

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 Which gas is colourless and poisonous?

A carbon monoxide

B chlorine

C hydrogen

D nitrogen

11


31 Two experiments involving water are described.

1 Water turns purple when potassium manganate(VII) is added to it.

2 Adding water to sodium causes the temperature to increase.

Which row describes the role of water in 1 and 2?

1 2

A as a chemical reagent as a chemical reagent

B as a chemical reagent as a solvent

C as a solvent as a chemical reagent

D as a solvent as a solvent 32 In which process is carbon dioxide not formed?

A burning of natural gas

B fermentation

C heating lime

D respiration 33 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. 34 The structures of three substances are shown.

H C

H

H

O H H C

H

H

C

H

H

O H H C

H

H

C

H

H

C

H

H

O H

Why do these substances all belong to the same homologous series?

A They are all compounds.

B They are all saturated.

C They all contain oxygen.

D They all contain the same functional group.

12

© UCLES 2017 0620/11/M/J/17

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 Cracking is an important process in the petroleum industry.

The products of cracking include ......1...... and an ......2...... of ......3...... relative molecular mass than the ......4...... that was cracked.

Which words complete gaps 1, 2, 3 and 4?

1 2 3 4

A hydrogen alkane greater alkene

B hydrogen alkene smaller alkane

C steam alkane greater alkene

D steam alkene smaller alkane 37 Which compound rapidly decolourises aqueous bromine?

A ethane

B ethanoic acid

C ethanol

D ethene 38 There are two methods for producing ethanol.

method 1 catalytic addition of steam to ethene

method 2 fermentation

Which statement is not correct?

A Method 1 produces carbon dioxide.

B Method 1 requires high temperature and pressure.

C Method 2 produces carbon dioxide.

D Method 2 requires a source of sugar.

13

© UCLES 2017 0620/11/M/J/17

39 Which statement about aqueous ethanoic acid is not correct?

A It produces carbon dioxide when it reacts with magnesium carbonate.

B It produces hydrogen when it reacts with magnesium.

C It neutralises magnesium oxide.

D It turns red litmus paper blue. 40 The diagram shows part of the molecule of a polymer.

H

H

C

H

H

C

H

H

C

H

H

C

H

H

C

H

H

C

H

H

C

H

H

C

H

H

C

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

A B C D

H H

H

H

C H C

H

H

C H

H

H

H C

H

H

C O

H

H

HC C

H

H

H

H

14

© UCLES 2017 0620/11/M/J/17

BLANK PAGE

15

Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the publisher will be pleased to make amends at the earliest possible opportunity. To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge International Examinations Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at www.cie.org.uk after the live examination series. Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge. © UCLES 2017 0620/11/M/J/17

BLANK PAGE

16

© UCLES 2017 0620/11/M/J/17

Gro

up

The

Perio

dic

Tabl

e of

Ele

men

ts

1 Hhy

drog

en1

2 He

heliu

m4

III

IIIIV

VV

IV

IIV

III

3 Lilit

hium 7

4 Be

bery

llium

9

atom

ic n

umbe

r

atom

ic s

ymbo

l

Key

nam

ere

lativ

e at

omic

mas

s

11 Na

sodi

um23

12 Mg

mag

nesi

um24

19 Kpo

tass

ium

39

20 Ca

calc

ium

40

37 Rb

rubi

dium

85

38 Sr

stro

ntiu

m88

55 Cs

caes

ium

133

56 Ba

bariu

m13

7

87 Frfra

nciu

m–

88 Ra

radi

um –

5 B boro

n11 13 Al

alum

iniu

m27 31 Ga

galli

um70 49 In indi

um11

5

81 Tlth

alliu

m20

4

6 Cca

rbon

12 14 Si

silic

on28 32 Ge

germ

aniu

m73 50 Sn tin 119

82 Pb

lead

207

22 Titit

aniu

m48 40 Zr

zirc

oniu

m91 72 Hf

hafn

ium

178

104

Rf

ruth

erfo

rdiu

m–

23 Vva

nadi

um51 41 Nb

niob

ium

93 73 Tata

ntal

um18

1

105

Db

dubn

ium

–

24 Cr

chro

miu

m52 42 Mo

mol

ybde

num

96 74 Wtu

ngst

en18

4

106

Sg

seab

orgi

um–

25 Mn

man

gane

se55 43 Tc

tech

netiu

m– 75 Re

rhen

ium

186

107

Bh

bohr

ium

–

26 Fe iron

56 44 Ru

ruth

eniu

m10

1

76 Os

osm

ium

190

108

Hs

hass

ium

–

27 Co

coba

lt59 45 Rh

rhod

ium

103

77 Iriri

dium

192

109

Mt

mei

tner

ium

–

28 Ni

nick

el59 46 Pd

palla

dium

106

78 Pt

plat

inum

195

110

Ds

darm

stad

tium

–

29 Cu

copp

er64 47 Ag

silv

er10

8

79 Au

gold

197

111

Rg

roen

tgen

ium

–

30 Zn zinc 65 48 Cd

cadm

ium

112

80 Hg

mer

cury

201

112

Cn

cope

rnic

ium

–

114 Fl

flero

vium

–

116

Lvliv

erm

oriu

m–

7 Nni

troge

n14 15 P

phos

phor

us31 33 As

arse

nic

75 51 Sb

antim

ony

122

83 Bi

bism

uth

209

8 Oox

ygen

16 16 S sulfu

r32 34 Se

sele

nium

79 52 Tete

lluriu

m12

8

84 Po

polo

nium

–

9 Fflu

orin

e19 17 Cl

chlo

rine

35.5

35 Br

brom

ine

80 53 Iio

dine

127

85 At

asta

tine

–

10 Ne

neon 20 18 Ar

argo

n40 36 Kr

kryp

ton

84 54 Xe

xeno

n13

1

86 Rn

rado

n–

21 Sc

scan

dium

45 39 Yyt

trium 89

57–7

1la

ntha

noid

s

89–1

03ac

tinoi

ds

57 Lala

ntha

num

139

89 Ac

lant

hano

ids

actin

oids

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3 a

t roo

m te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.).

actin

ium

–

58 Ce

ceriu

m14

0

90 Th thor

ium

232

59 Pr

pras

eody

miu

m14

1

91 Pa

prot

actin

ium

231

60 Nd

neod

ymiu

m14

4

92 Uur

aniu

m23

8

61 Pm

prom

ethi

um– 93 Np

nept

uniu

m–

62 Sm

sam

ariu

m15

0

94 Pu

plut

oniu

m–

63 Eu

euro

pium

152

95 Am

amer

iciu

m–

64 Gd

gado

liniu

m15

7

96 Cm

curiu

m–

65 Tb terb

ium

159

97 Bk

berk

eliu

m–

66 Dy

dysp

rosi

um16

3

98 Cf

calif

orni

um–

67 Ho

holm

ium

165

99 Es

eins

tein

ium

–

68 Er

erbi

um16

7

100

Fm ferm

ium

–

69 Tm thul

ium

169

101

Md

men

dele

vium

–

70 Yb

ytte

rbiu

m17

3

102

No

nobe

lium

–

71 Lu lute

tium

175

103 Lr

law

renc

ium

–

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

This document consists of 16 printed pages.

IB17 O6_0620_21_VI_LIL/FP © UCLES 2017 [Turn over

*8889844006*


CHEMISTRY 0620/21

Paper 2 Multiple Choice (Extended) May/June 2017

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

READ THESE INSTRUCTIONS FIRST Write in soft pencil. Do not use staples, paper clips, glue or correction fluid. Write your name, Centre number and candidate number on the Answer Sheet in the spaces provided unless this has been done for you. DO NOT WRITE IN ANY BARCODES. There are forty questions on this paper. Answer all questions. For each question there are four possible answers A, B, C and D. Choose the one you consider correct and record your choice in soft pencil on the separate Answer Sheet. Read the instructions on the Answer Sheet very carefully. Each correct answer will score one mark. A mark will not be deducted for a wrong answer. Any rough working should be done in this booklet. A copy of the Periodic Table is printed on page 16. Electronic calculators may be used.

2

© UCLES 2017 0620/21/M/J/17

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

KMnO4

dish 2

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

3


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

Which substance has an Rf value of 0.6?

solvent front

baseline

A B C D

5.5 cm 5.2 cm 5.8 cm 6.3 cm

10.5 cm

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.

4

© UCLES 2017 0620/21/M/J/17

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.

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.

V

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?

fuel formula melting point / °C

boiling point / °C

A hydrogen H2 –259 –253

B methane CH4 –182 –164

C octane C8H18 –57 126

D wax C31H64 60 400

6

© UCLES 2017 0620/21/M/J/17

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.

C

H

H

H

H

C H Cl Cl Cl Cl+ +H C

H

H

H

H

CH H

The reaction is exothermic.

The bond energies are shown in the table.

bond bond energy 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

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.

bung

marble

chips 25 cm3 of dilute

hydrochloric acid

gas syringe

Which changes slow down the rate of reaction?

temperature of acid

concentration of acid

surface area of marble chips

A decrease decrease decrease

B decrease decrease increase

C increase decrease decrease

D increase increase increase

8

© UCLES 2017 0620/21/M/J/17

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 hydrochloric acid

reaction with aqueous

sodium hydroxide

A key

B = reaction occurs

C = reaction does not occur

D

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 concentration pH

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

10

© UCLES 2017 0620/21/M/J/17

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.

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.

12

© UCLES 2017 0620/21/M/J/17

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.

13


31 Photosynthesis and respiration are important natural processes.


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?

temperature / °C pressure / atm catalyst

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.

14

© UCLES 2017 0620/21/M/J/17

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 C

H

H

C

H

H

O H H C

H

H

C

H

H

C

O

H

H

C

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

C

H

H

C

H

H

C

H

H

C

H

H

C

H

H

C

H

H

C

H

H

C

H

H

C

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

A B C D

H H

H

H

C H C

H

H

C H

H

H

H C

H

H

C O

H

H

HC C

H

H

H

H

15

Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the publisher will be pleased to make amends at the earliest possible opportunity. To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge International Examinations Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at www.cie.org.uk after the live examination series. Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge. © UCLES 2017 0620/21/M/J/17

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


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

CH

H

H

C H

C

H

HH

C

O

O

Which row is correct?

name of ester names of the carboxylic acid and 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

16

© UCLES 2017 0620/21/M/J/17

Gro

up

The

Perio

dic

Tabl

e of

Ele

men

ts

1 Hh

yd

rog

en

1

2

He

he

lium

4

III

III

IVV

VI

VII

VIII

3 Li

lith

ium

7

4 Be

be

rylli

um

9

ato

mic

nu

mb

er

ato

mic

sym

bo

l

Key

na

me

rela

tive

ato

mic

ma

ss

11

Na

so

diu

m

23

12

Mg

ma

gn

esiu

m

24

19 K

po

tassiu

m

39

20

Ca

ca

lciu

m

40

37

Rb

rub

idiu

m

85

38

Sr

str

on

tiu

m

88

55

Cs

ca

esiu

m

13

3

56

Ba

ba

riu

m

13

7

87

Fr

fra

nciu

m

–

88

Ra

rad

ium

–

5 Bb

oro

n

11

13

Al

alu

min

ium

27

31

Ga

ga

lliu

m

70

49 In

ind

ium

11

5

81 Tl

tha

lliu

m

20

4

6 Cca

rbo

n

12

14 Si

sili

co

n

28

32

Ge

ge

rma

niu

m

73

50

Sn

tin

11

9

82

Pb

lea

d

20

7

22 Ti

tita

niu

m

48

40

Zr

zirco

niu

m

91

72

Hf

ha

fniu

m

17

8

10

4

Rf

ruth

erf

ord

ium

–

23 V

va

na

diu

m

51

41

Nb

nio

biu

m

93

73

Ta

tan

talu

m

18

1

10

5

Db

du

bn

ium

–

24

Cr

ch

rom

ium

52

42

Mo

mo

lyb

de

nu

m

96

74

Wtu

ng

ste

n

18

4

10

6

Sg

se

ab

org

ium

–

25

Mn

ma

ng

an

ese

55

43

Tc

tech

ne

tiu

m

– 75

Re

rhe

niu

m

18

6

10

7

Bh

bo

hriu

m

–

26

Fe

iro

n

56

44

Ru

ruth

en

ium

10

1

76

Os

osm

ium

19

0

10

8

Hs

ha

ssiu

m

–

27

Co

co

ba

lt

59

45

Rh

rho

diu

m

10

3

77 Ir

irid

ium

19

2

10

9

Mt

me

itn

eriu

m

–

28

Ni

nic

ke

l

59

46

Pd

pa

llad

ium

10

6

78

Pt

pla

tin

um

19

5

11

0

Ds

da

rmsta

dtiu

m

–

29

Cu

co

pp

er

64

47

Ag

silv

er

10

8

79

Au

go

ld

19

7

111

Rg

roe

ntg

en

ium

–

30

Zn

zin

c

65

48

Cd

ca

dm

ium

11

2

80

Hg

me

rcu

ry

20

1

11

2

Cn

co

pe

rnic

ium

–

11

4

Fl

fle

roviu

m

–

11

6

Lv

live

rmo

riu

m

–

7 Nn

itro

ge

n

14

15 P

ph

osp

ho

rus

31

33

As

ars

en

ic

75

51

Sb

an

tim

on

y

12

2

83 Bi

bis

mu

th

20

9

8 Oo

xyg

en

16

16 S

su

lfu

r

32

34

Se

se

len

ium

79

52

Te

tellu

riu

m

12

8

84

Po

po

lon

ium

–

9 Fflu

orin

e

19

17

Cl

ch

lorin

e

35.5

35

Br

bro

min

e

80

53 I

iod

ine

12

7

85

At

asta

tin

e

–

10

Ne

ne

on

20

18

Ar

arg

on

40

36

Kr

kry

pto

n

84

54

Xe

xe

no

n

13

1

86

Rn

rad

on

–

21

Sc

sca

nd

ium

45

39 Y

ytt

riu

m

89

57

–7

1

lan

tha

no

ids

89

–1

03

actin

oid

s

57

La

lan

tha

nu

m

13

9

89

Ac

lan

tha

no

ids

actin

oid

s

Th

e v

olu

me

of

on

e m

ole

of

an

y g

as is 2

4 d

m3 a

t ro

om

te

mp

era

ture

an

d p

ressu

re (

r.t.

p.)

.

actin

ium

–

58

Ce

ce

riu

m

14

0

90

Th

tho

riu

m

23

2

59

Pr

pra

se

od

ym

ium

14

1

91

Pa

pro

tactin

ium

23

1

60

Nd

ne

od

ym

ium

14

4

92 U

ura

niu

m

23

8

61

Pm

pro

me

thiu

m

– 93

Np

ne

ptu

niu

m

–

62

Sm

sa

ma

riu

m

15

0

94

Pu

plu

ton

ium

–

63

Eu

eu

rop

ium

15

2

95

Am

am

ericiu

m

–

64

Gd

ga

do

liniu

m

15

7

96

Cm

cu

riu

m

–

65

Tb

terb

ium

15

9

97

Bk

be

rke

lium

–

66

Dy

dysp

rosiu

m

16

3

98

Cf

ca

lifo

rniu

m

–

67

Ho

ho

lmiu

m

16

5

99

Es

ein

ste

iniu

m

–

68

Er

erb

ium

16

7

10

0

Fm

ferm

ium

–

69

Tm

thu

lium

16

9

10

1

Md

me

nd

ele

viu

m

–

70

Yb

ytt

erb

ium

17

3

10

2

No

no

be

lium

–

71

Lu

lute

tiu

m

17

5

10

3

Lr

law

ren

ciu

m

–

READ THESE INSTRUCTIONS FIRST

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

Answer all questions.Electronic calculators may be used.A copy of the Periodic Table is printed on page 16.You may lose marks if you do not show your working or if you do not use appropriate units.

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

CHEMISTRY 0620/31

Paper 3 Theory (Core) May/June 2017

1 hour 15 minutes

Candidates answer on the Question Paper.

No Additional Materials are required.

Cambridge International ExaminationsCambridge International General Certifi cate of Secondary Education


[Turn overIB17 06_0620_31/FP© UCLES 2017

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

2

0620/31/M/J/17© UCLES 2017

1 (a) The electronic structures of fi ve atoms, A, B, C, D and E, are shown.

A B C D E

Answer the following questions about these atoms. Each atom may be used once, more than once or not at all.

Which atom, A, B, C, D or E,

(i) has a complete outer shell of electrons, .............................. [1]

(ii) has a proton number of 15, .............................. [1]

(iii) has 4 shells containing electrons, .............................. [1]

(iv) is a fl uorine atom, .............................. [1]

(v) is an atom of a metallic element? .............................. [1]

(b) Complete the table to show the number of electrons, neutrons and protons in the chlorine atom and bromide ion shown.

number of electrons number of neutrons number of protons

35Cl17 17

79Br –35 44

[3]

[Total: 8]

3

0620/31/M/J/17© UCLES 2017 [Turn over

2 (a) The table shows the ions present in a 1000 cm3 sample of polluted river water.

ion present formula of ion mass presentin mg / 1000 cm3

calcium Ca2+ 2.0

chloride Cl – 1.3

hydrogencarbonate HCO3– 2.0

magnesium Mg2+ 1.0

potassium K+ 4.0

silicate SiO32– 12.0

sodium Na+ 11.0

SO32– 3.0

Answer these questions using the information from the table.

(i) Which positive ion is present in the highest concentration?

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

(ii) State the name of the ion SO32–.

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

(iii) Calculate the mass of silicate ions present in 250 cm3 of this sample.

mass of silicate ions = .............................. mg [1]

(iv) Calculate the mass of solid formed when all the water is evaporated from the 1000 cm3 sample.

mass of solid formed = .............................. mg [1]

(v) Name the compound containing Ca2+ ions and HCO3– ions.

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

4

0620/31/M/J/17© UCLES 2017

(b) Describe a test for sodium ions.

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

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

(c) The formulae of some chlorides are given.

aluminium chloride, Al Cl 3 calcium chloride, CaCl 2 sodium chloride, NaCl

Deduce the formula for magnesium chloride.

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

(d) Molten calcium chloride can be electrolysed using inert electrodes.

Predict the products of this electrolysis at

the negative electrode (cathode), ..............................................................................................

the positive electrode (anode). ..................................................................................................[2]

[Total: 10]

5


3 The diagram shows part of the structures of three substances, X, Y and Z, at room temperature and pressure.

O C O

O C O

OC

O

OC

O

OC

O

Na+ Cl – Na+ Cl –

Na+ Cl – Na+ Cl –

Cl – Na+ Cl – Na+

X Y Z

(a) Describe substances X, Y and Z in terms of

● their bonding, ● the arrangement of their particles, ● the motion of their particles.

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

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

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

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

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

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

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

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

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

6

0620/31/M/J/17© UCLES 2017

(b) A closed gas syringe contains substance X.

X

end blockedgas syringe

Describe what happens to the volume of substance X in the syringe when the pressure is increased. The temperature remains constant. Explain your answer in terms of particles.

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

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

(c) Substance Z is diamond. Diamond is used in jewellery.

Give one other use of diamond.

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

(d) Substance Y undergoes physical and chemical changes.

Which two of the following are physical changes? Explain your answer.

A Substance Y dissolves easily in water.

B An aqueous solution of substance Y gives a white precipitate with acidified aqueous silver nitrate.

C Substance Y melts at 801 C.

D Substance Y reacts with concentrated sulfuric acid.

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

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

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

[Total: 11]

7


4 Chlorine is an element in Group VII of the Periodic Table.

(a) Chlorine is a diatomic molecule.

Explain what is meant by the term diatomic.

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

(b) Aqueous chlorine reacts with aqueous potassium bromide.

Cl 2 + 2KBr Br2 + 2KCl

(i) How does this equation show that chlorine is more reactive than bromine?

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

(ii) Aqueous potassium bromide and aqueous potassium chloride are both colourless.

Predict the colour change when aqueous chlorine reacts with aqueous potassium bromide.

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

(iii) Complete the chemical equation for the reaction of aqueous bromine with aqueous potassium iodide.

Br2 + 2KI ............... + ...............[2]

(c) Describe a test for iodide ions.

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

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

8

0620/31/M/J/17© UCLES 2017

(d) Chlorine is used to make the polymer PVC.

(i) Give one other use of chlorine.

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

(ii) The monomer used to make PVC is made by the thermal decomposition of dichloroethane.

CH2Cl –CH2Cl CH2=CHCl + HCl

Explain what is meant by the term thermal decomposition.

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

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

(iii) PVC is a non-biodegradable plastic.

Describe two pollution problems caused by non-biodegradable plastics.

1 ..........................................................................................................................................

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

[Total: 12]

9


5 Citronellol is found in rose oil.

The structure of citronellol is shown.

CH2 CH2CH2 CH2

C

C

C

H

H

CH3 CH3

CH3

OH

(a) On the structure shown draw a circle around the alcohol functional group. [1]

(b) How many hydrogen atoms are there in one molecule of citronellol?

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

(c) What feature of the citronellol structure shows that it is unsaturated?

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

10

0620/31/M/J/17© UCLES 2017

(d) The table shows the properties of some alkanes.

alkane number of carbonatoms in one molecule

melting pointin C

boiling pointin C

density of liquidalkane in g / cm3

methane 1 –182 –162 0.466

ethane 2 –183 –88 0.572

propane 3 –188 0.585

butane 4 0 0.601

pentane 5 –130 36 0.626

(i) Describe how the density of the liquid alkanes varies with the number of carbon atoms in one molecule.

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

(ii) Predict the boiling point of propane.

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

(iii) Why would it be diffi cult to predict the melting point of butane from the information in the table?

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

(iv) What is the state of pentane at 30 C? Explain your answer.

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

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

(v) Alkanes are hydrocarbons.

What is the meaning of the term hydrocarbon?

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

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

(vi) Draw the structure of ethane. Show all of the atoms and all of the bonds.

[1]

(vii) Complete the chemical equation for the combustion of propane.

C3H8 + .......O2 .......CO2 + 4H2O[2]

[Total: 13]

11


6 (a) The table shows the properties of some metals.

metal densityin g / cm3

melting pointin C

relativestrength

relativeelectrical

conductivitycost

aluminium 2.7 660 7.0 4.0 expensive

iron 7.9 1535 21.0 1.1 cheap

lead 11.3 328 1.5 0.5 expensive

silver 10.5 962 2.0 6.7 very expensive

tungsten 19.4 3420 12.0 2.0 expensive

Use the information in the table to answer the questions.

(i) Which metal would be most useful for making overhead power cables? Give two reasons for your answer.

metal ................................

reason 1 ..............................................................................................................................

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

(ii) Why is iron and not tungsten used to reinforce concrete?

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

(iii) The front part of a space rocket is called a nose cone. The nose cone gets very hot as the space rocket moves through the air.

Which metal is best to make a space rocket nose cone? Explain your answer.

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

(b) Tungsten is a transition element.

State two physical properties of transition elements which are not shown by Group I elements.

1 .................................................................................................................................................

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

12

0620/31/M/J/17© UCLES 2017

(c) When extremely hot tungsten reacts with oxygen, tungsten(VI) oxide is formed.

Balance the chemical equation for this reaction.

......W + ......O2 2WO3[2]

(d) Some information about the reaction of four metals with oxygen is given.

cobalt: reacts slowly at high temperatures

iron: thin wire burns when heated strongly

magnesium: burns when heated

tungsten: reacts very slowly at extremely high temperatures

List these metals in order of their reactivity. Put the least reactive metal fi rst.

least reactive most reactive

[2]

(e) The table compares the time taken for reaction of an alloy with ethanoic acid, nitric acid and phosphoric acid, each at three different concentrations. The time taken for the alloy to decrease in mass by 1.0 g was measured. All other conditions were kept the same.

acidtime taken for reaction / hours

concentration of acid0.04 mol / dm3



ethanoic acid 92 190 410

nitric acid 2 6 18

phosphoric acid 19 39 80

(i) How does the concentration of acid affect the rate of reaction?

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

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

(ii) Which acid reacts most rapidly with the alloy?

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

13


(iii) Predict how long it would take for the alloy to decrease in mass by 1.0 g using phosphoric acid of concentration 0.03 mol / dm3.

time taken = .............................. hours [1]

(iv) Suggest which one of these pH values is the pH of concentrated aqueous ethanoic acid. Draw a circle around the correct answer.

pH 4 pH 7 pH 10 pH 13[1]

[Total: 14]

14

0620/31/M/J/17© UCLES 2017

7 Carbon is an element in Group IV of the Periodic Table. It reacts with oxygen to form carbon dioxide.

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

energy

C + O2

CO2

Explain how this diagram shows that the reaction is exothermic.

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

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

(b) Carbon monoxide, carbon dioxide and methane are all atmospheric pollutants.

● Give the sources of these gases. ● Describe the effects that both carbon dioxide and methane have on the environment. ● State an adverse effect of carbon monoxide on health.

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

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

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

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

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

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

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

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

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

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

15

0620/31/M/J/17© UCLES 2017

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.

(c) Calcium carbonate decomposes to form calcium oxide (lime) and carbon dioxide.

(i) State one use of calcium oxide.

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

(ii) Calculate the relative formula mass of calcium carbonate, CaCO3. Show all your working. Use your Periodic Table to help you.

relative formula mass = .............................. [2]

(d) Carbon and magnesium are both insoluble in water. Carbon does not react with hydrochloric acid but magnesium reacts to form a soluble salt and

a gas which escapes into the air.

Suggest how you could prepare a pure dry sample of carbon from a mixture of carbon powder and magnesium powder.

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

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

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

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

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

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

[Total: 12]

16

0620/31/M/J/17© UCLES 2017

Gro

up

The

Perio

dic

Tabl

e of

Ele

men

ts

1 Hhy

drog

en1

2 He

heliu

m4

III

IIIIV

VV

IV

IIV

III

3 Lilit

hium 7

4 Be

bery

llium

9

atom

ic n

umbe

r

atom

ic s

ymbo

l

Key

nam

ere

lativ

e at

omic

mas

s

11 Na

sodi

um23

12 Mg

mag

nesi

um24

19 Kpo

tass

ium

39

20 Ca

calc

ium

40

37 Rb

rubi

dium

85

38 Sr

stro

ntiu

m88

55 Cs

caes

ium

133

56 Ba

bariu

m13

7

87 Frfra

nciu

m–

88 Ra

radi

um –

5 B boro

n11 13 Al

alum

iniu

m27 31 Ga

galli

um70 49 In indi

um11

5

81 Tlth

alliu

m20

4

6 Cca

rbon

12 14 Si

silic

on28 32 Ge

germ

aniu

m73 50 Sn tin 119

82 Pb

lead

207

22 Titit

aniu

m48 40 Zr

zirc

oniu

m91 72 Hf

hafn

ium

178

104

Rf

ruth

erfo

rdiu

m–

23 Vva

nadi

um51 41 Nb

niob

ium

93 73 Tata

ntal

um18

1

105

Db

dubn

ium

–

24 Cr

chro

miu

m52 42 Mo

mol

ybde

num

96 74 Wtu

ngst

en18

4

106

Sg

seab

orgi

um–

25 Mn

man

gane

se55 43 Tc

tech

netiu

m– 75 Re

rhen

ium

186

107

Bh

bohr

ium

–

26 Fe iron

56 44 Ru

ruth

eniu

m10

1

76 Os

osm

ium

190

108

Hs

hass

ium

–

27 Co

coba

lt59 45 Rh

rhod

ium

103

77 Iriri

dium

192

109

Mt

mei

tner

ium

–

28 Ni

nick

el59 46 Pd

palla

dium

106

78 Pt

plat

inum

195

110

Ds

darm

stad

tium

–

29 Cu

copp

er64 47 Ag

silv

er10

8

79 Au

gold

197

111

Rg

roen

tgen

ium

–

30 Zn zinc 65 48 Cd

cadm

ium

112

80 Hg

mer

cury

201

112

Cn

cope

rnic

ium

–

114 Fl

flero

vium

–

116

Lvliv

erm

oriu

m–

7 Nni

troge

n14 15 P

phos

phor

us31 33 As

arse

nic

75 51 Sb

antim

ony

122

83 Bi

bism

uth

209

8 Oox

ygen

16 16 S sulfu

r32 34 Se

sele

nium

79 52 Tete

lluriu

m12

8

84 Po

polo

nium

–

9 Fflu

orin

e19 17 Cl

chlo

rine

35.5

35 Br

brom

ine

80 53 Iio

dine

127

85 At

asta

tine

–

10 Ne

neon 20 18 Ar

argo

n40 36 Kr

kryp

ton

84 54 Xe

xeno

n13

1

86 Rn

rado

n–

21 Sc

scan

dium

45 39 Yyt

trium 89

57–7

1la

ntha

noid

s

89–1

03ac

tinoi

ds

57 Lala

ntha

num

139

89 Ac

lant

hano

ids

actin

oids

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3 a

t roo

m te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.).

actin

ium

–

58 Ce

ceriu

m14

0

90 Th thor

ium

232

59 Pr

pras

eody

miu

m14

1

91 Pa

prot

actin

ium

231

60 Nd

neod

ymiu

m14

4

92 Uur

aniu

m23

8

61 Pm

prom

ethi

um– 93 Np

nept

uniu

m–

62 Sm

sam

ariu

m15

0

94 Pu

plut

oniu

m–

63 Eu

euro

pium

152

95 Am

amer

iciu

m–

64 Gd

gado

liniu

m15

7

96 Cm

curiu

m–

65 Tb terb

ium

159

97 Bk

berk

eliu

m–

66 Dy

dysp

rosi

um16

3

98 Cf

calif

orni

um–

67 Ho

holm

ium

165

99 Es

eins

tein

ium

–

68 Er

erbi

um16

7

100

Fm ferm

ium

–

69 Tm thul

ium

169

101

Md

men

dele

vium

–

70 Yb

ytte

rbiu

m17

3

102

No

nobe

lium

–

71 Lu lute

tium

175

103 Lr

law

renc

ium

–


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

Answer all questions.Electronic calculators may be used.A copy of the Periodic Table is printed on page 16.You may lose marks if you do not show your working or if you do not use appropriate units.


CHEMISTRY 0620/41

Paper 4 Theory (Extended) May/June 2017

1 hour 15 minutes



Cambridge International ExaminationsCambridge International General Certificate of Secondary Education

This document consists of 14 printed pages and 2 blank pages.

[Turn overIB17 06_0620_41/4RP© UCLES 2017

*3843148954*


2

0620/41/M/J/17© UCLES 2017

1 This question is about subatomic particles.

(a) Definetheterms

proton number, ..........................................................................................................................

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

nucleon number. ........................................................................................................................

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

(b) Why is the 1H1 hydrogen atom the only atom to have an identical proton number and nucleon number?

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

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

(c) Complete the table to show the number of protons, neutrons and electrons in the atoms and ions given.

number ofprotons

number ofneutrons

number ofelectrons

19F 9

26Mg 12

31P3–

87Sr2+

[6]

(d) (i) Writetheformulaofthecompoundformedfromfluorineandmagnesium.

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

(ii) Write the formula of the compound formed from Sr2+ and P3–.

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

[Total: 12]

3


2 Some oxides of some elements are listed.

CO CO2 Na2O MgO Al 2O3

SiO2 P4O10 SO2 Cl 2O7 Cr2O3

(a) Answer the following questions using only oxides from the list. Each oxide may be used once, more than once or not at all.

Give the formula of an oxide

(i) which is the main cause of acid rain, ..................................................................................

(ii) which would give a solution of pH 14 when added to water, ...............................................

(iii) which is coloured, ...............................................................................................................

(iv) which is the major impurity in iron ore, ................................................................................

(v) which is amphoteric, ............................................................................................................

(vi) which is neutral. ..................................................................................................................[6]

(b) Amphoteric oxides and neutral oxides are different from each other.

(i) What is meant by the term amphoteric oxide?

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

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

(ii) What is meant by the term neutral oxide?

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

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

[Total: 8]

4

0620/41/M/J/17© UCLES 2017

3 Magnesium sulfate and lead(II) sulfate are examples of salts.

(a) A student prepared magnesium sulfate crystals starting from magnesium carbonate. The student carried out the experiment in four steps.

step 1 The student added excess magnesium carbonate to a small volume of dilute sulfuric acid until no more magnesium carbonate would react.

step 2 Thestudentfilteredthemixture.

step 3 Thestudentheatedthefiltrateobtainedfromstep 2 until it was saturated.

step 4 Thestudentallowedthehotfiltratetocooltoroomtemperatureandthenremovedthe crystals which formed.

(i) Howdidthestudentknowwhenthereactionhadfinishedinstep 1?

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

(ii) Name the residue in step 2.

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

(iii) A saturated solution forms in step 3.

What is a saturated solution?

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

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

(iv) Explain why magnesium sulfate crystals form during step 4.

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

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

5


(b) Magnesium sulfate crystals are hydrated. Another student heated some hydrated magnesium sulfate crystals in a crucible and obtained the following results.

mass of hydrated magnesium sulfate crystals = 4.92 g

mass of water removed = 2.52 g

(i) Calculate the number of moles of water removed.

moles of water = ............................. mol [1]

(ii) Calculate the number of moles of anhydrous magnesium sulfate remaining in the crucible. The Mr of anhydrous magnesium sulfate is 120.

moles of anhydrous magnesium sulfate = ............................. mol [1]

(iii) Calculate the ratio of moles of anhydrous magnesium sulfate : moles of water. Give your answer as whole numbers.

ratio = ................ : ................ [1]

(iv) Suggest the formula of hydrated magnesium sulfate crystals.

formula of hydrated magnesium sulfate crystals = ............................................ [2]

6

0620/41/M/J/17© UCLES 2017

(c) Lead(II) sulfate, PbSO4, is insoluble.

Describe how you would prepare a pure dry sample of lead(II) sulfate crystals starting from solutions of lead(II) nitrate and sodium sulfate.

Include a series of key steps in your answer.

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

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

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

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

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

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

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

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

(d) Write the ionic equation for the reaction which takes place between solutions of lead(II) nitrate and sodium sulfate.

Include state symbols.

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

[Total: 16]

7


4 Zinc is a very important metal.

(a) Zincisextractedfromitsore,zincblende.Zincblendecontainszincsulfide,ZnS.

Zincsulfideisconvertedtozincoxideinanindustrialprocess.

(i) Describehowzincsulfideisconvertedtozincoxideinthisindustrialprocess.

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

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

(ii) Write the chemical equation for this reaction.

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

(b) Zinc oxide is then reduced in a furnace.

(i) Name the substance added to the furnace to reduce the zinc oxide.

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

(ii) Describe how the pure zinc is removed from the furnace and collected.

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

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

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

8

0620/41/M/J/17© UCLES 2017

(c) When rods of zinc and copper are placed into dilute sulfuric acid as shown, electricity is generated.

copper rod

dilute sulfuric acid

zinc rod

bulb

(i) Write the ionic half-equation for the reaction occurring at the zinc rod.

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

(ii) Write the ionic half-equation for the reaction occurring at the copper rod.

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

(iii) The copper rod was replaced by an iron rod.

Suggest the change, if any, in the intensity of the light emitted from the bulb and give a reason for your answer.

change ................................................................................................................................

reason .................................................................................................................................

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

[Total: 12]

9


5 When barium carbonate is added to dilute hydrochloric acid, carbon dioxide gas is formed.

A student carried out an experiment to measure the volume of gas formed as a reaction proceeds. The student added a small mass of powdered barium carbonate to an excess of 0.1 mol / dm3 hydrochloric acid. A graph of the results was drawn.

The graph is shown.

400

300

200

100

0

volumeof gas/ cm3

0 30 60 90 120

time / s

150 180 210 240

(a) Name the two pieces of apparatus needed to take the measurements shown on the graph.

1 .................................................................................................................................................

2 .................................................................................................................................................[1]

(b) On the axes below, sketch a graph to show how the rate of reaction changes as the reaction proceeds.

Assume the initial rate of reaction is represented by the point at X.

00

120906030time / s

rate ofreaction

X

[2]

10

0620/41/M/J/17© UCLES 2017

(c) The total volume of gas collected was 180 cm3 at room temperature and pressure.

Calculate the mass, in grams, of barium carbonate used.

BaCO3 + 2HCl BaCl 2 + H2O + CO2

mass of barium carbonate = ............................. g [3]

(d) The original graph has been drawn again.

On the grid, draw the graph expected if the same mass of barium carbonate is added as large lumps instead of as a powder. All other conditions are the same as in the original experiment.

Explain why your graph is different from the original graph.

400

300

200

100

0

volumeof gas/ cm3

0 30 60 90 120

time / s

150 180 210 240

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

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

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

11


(e) The original graph has been drawn again.

On the grid, draw the graph expected if the concentration of dilute hydrochloric acid is changed from 0.1 mol / dm3 to 0.2 mol / dm3. All other conditions are the same as in the original experiment.

Explain, in terms of particles, why your graph is different from the original graph.

400

300

200

100

0

volumeof gas/ cm3

0 30 60 90 120

time / s

150 180 210 240

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

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

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

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

(f) The experiment is changed and the mass of powdered barium carbonate is doubled. All other conditions are the same as in the original experiment. The acid is still in excess.

Deduce the volume of gas formed at room temperature and pressure, in cm3, in this experiment.

volume of gas = .............................. cm3 [1]

[Total: 13]

12

0620/41/M/J/17© UCLES 2017

6 The alkenes and alkanes are both examples of homologous series which are hydrocarbons.

(a) What is meant by the term hydrocarbon?

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

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

(b) Give three characteristics of an homologous series.

1 .................................................................................................................................................

2 .................................................................................................................................................

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

(c) Name and draw the structure of the second member of the alkene homologous series. Show all of the atoms and all of the bonds.

name ..........................................................................................................................................

structure

[2]

(d) Alcohols can be made from alkenes.

Name the reagent and conditions needed to convert an alkene into an alcohol.

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

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

13


(e) The alcohol butanol, CH3CH2CH2CH2OH, can be converted into a carboxylic acid with four carbon atoms.

(i) Name the carboxylic acid formed from butanol and draw its structure. Show all of the atoms and all of the bonds.

name ...................................................................................................................................

structure

[2]

(ii) Ethanoic acid can be formed from ethanol by fermentation. It can also be formed by the addition of a suitable chemical reagent.

Name the reagent needed to convert ethanol into ethanoic acid.

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

(iii) State the type of chemical change which occurs when ethanol is converted into ethanoic acid.

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

(f) Describe how a student could prepare the ester methyl ethanoate in a school laboratory. In your description give

● thenamesofthetwo starting organic chemicals, ● theessentialreactionconditionsneeded, ● achemicalequationforthereaction.

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

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

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

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

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

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

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

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

[Total: 19]

14

0620/41/M/J/17© UCLES 2017

BLANK PAGE

15

0620/41/M/J/17© UCLES 2017




BLANK PAGE

16

0620/41/M/J/17© UCLES 2017

Gro

up

The

Perio

dic

Tabl

e of

Ele

men

ts

1 Hhy

drog

en1

2 He

heliu

m4

III

IIIIV

VV

IV

IIV

III

3 Lilit

hium 7

4 Be

bery

llium

9

atom

ic n

umbe

r

atom

ic s

ymbo

l

Key

nam

ere

lativ

e at

omic

mas

s

11 Na

sodi

um23

12 Mg

mag

nesi

um24

19 Kpo

tass

ium

39

20 Ca

calc

ium

40

37 Rb

rubi

dium

85

38 Sr

stro

ntiu

m88

55 Cs

caes

ium

133

56 Ba

bariu

m13

7

87 Frfra

nciu

m–

88 Ra

radi

um –

5 B boro

n11 13 Al

alum

iniu

m27 31 Ga

gallium70 49 In indium

115

81 Tlthallium

204

6 Ccarbon

12 14 Si

silicon

28 32 Ge

germanium

73 50 Sn tin 119

82 Pb

lead207

22 Tititanium

48 40 Zrzirconium

91 72 Hf

hafnium

178

104

Rf

rutherfordium

–

23 Vvanadium

51 41 Nb

niobium

93 73 Tatantalum

181

105

Db

dubnium

–

24 Cr

chromium

52 42 Mo

molybdenum

96 74 Wtungsten

184

106

Sg

seaborgium

–

25 Mn

manganese

55 43 Tctechnetium

– 75 Re

rhenium

186

107

Bh

bohrium

–

26 Fe iron

56 44 Ru

ruthenium

101

76 Os

osmium

190

108

Hs

hassium

–

27 Co

cobalt

59 45 Rh

rhodium

103

77 Iriridium

192

109

Mt

meitnerium

–

28 Ni

nickel

59 46 Pd

palladium

106

78 Pt

platinum

195

110

Ds

darmstadtium

–

29 Cu

copper

64 47 Ag

silver

108

79 Au

gold

197

111

Rg

roentgenium

–

30 Zn zinc 65 48 Cd

cadmium

112

80 Hg

mercury

201

112

Cn

copernicium

–

114 Fl

flerovium

–

116

Lvlivermorium

–

7 Nnitrogen

14 15 Pphosphorus

31 33 As

arsenic

75 51 Sb

antimony

122

83 Bi

bismuth

209

8 Ooxygen

16 16 S sulfur

32 34 Se

selenium

79 52 Tetellurium

128

84 Po

polo

nium

–

9 Fflu

orin

e19 17 Cl

chlo

rine

35.5

35 Br

brom

ine

80 53 Iio

dine

127

85 At

asta

tine

–

10 Ne

neon 20 18 Ar

argo

n40 36 Kr

kryp

ton

84 54 Xe

xeno

n13

1

86 Rn

rado

n–

21 Sc

scan

dium

45 39 Yyt

trium 89

57–7

1la

ntha

noid

s

89–1

03ac

tinoi

ds

57 Lala

ntha

num

139

89 Ac

lant

hano

ids

actin

oids

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3 a

t roo

m te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.).

actin

ium

–

58 Ce

ceriu

m140

90 Th thorium

232

59 Pr

praseodymium

141

91 Pa

protactinium

231

60 Nd

neodymium

144

92 Uuranium

238

61 Pm

promethium

– 93 Np

neptunium

–

62 Sm

samarium

150

94 Pu

plutonium

–

63 Eu

europium

152

95 Am

americium

–

64 Gd

gadolinium

157

96 Cm

curium

–

65 Tb terbium

159

97 Bk

berkelium

–

66 Dy

dysprosium

163

98 Cf

californium

–

67 Ho

holmium

165

99 Es

einsteinium

–

68 Er

erbium

167

100

Fm fermium

–

69 Tm thulium

169

101

Md

mendelevium

–

70 Yb

ytterbium

173

102

No

nobelium

–

71 Lu lutetium

175

103 Lr

lawrencium

–



Answer all questions.Electronic calculators may be used.You may lose marks if you do not show your working or if you do not use appropriate units.Notes for use in qualitative analysis are provided on pages 7 and 8.


CHEMISTRY 0620/51

Paper 5 Practical Test May/June 2017

1 hour 15 minutes


Additional Materials: As listed in the Confidential Instructions



[Turn overIB17 06_0620_51/3RP© UCLES 2017

*2045765175*


For Examiner’s Use

Total

2

0620/51/M/J/17© UCLES 2017

1 You are going to investigate the reaction between aqueous sodium thiosulfate and two different aqueous solutions of potassium iodate labelled solution C and solution D.

Read all the instructions carefully before starting the experiments.

Instructions You are going to carry out two experiments.

(a) Experiment 1

● Filltheburetteprovideduptothe0.0cm3 mark with the aqueous sodium thiosulfate. ● Useameasuringcylindertopour20cm3 of solution C into a conical flask. ● Add10cm3ofdilutesulfuricacidintotheflaskand1gofpotassiumiodide.Swirltheflask

to mix the contents. ● Addtheaqueoussodiumthiosulfateslowlyfromtheburettetotheflask,andswirltomix

thoroughly. ● Whenthecontentsoftheflaskarepaleyellow,add1cm3 of starch solution to the flask. ● Continuetoaddaqueoussodiumthiosulfateslowlytotheflaskuntilthesolutionjustturns

colourless. ● Recordtheburettereadingsinthetable.

(b) Experiment 2

● Emptytheconicalflaskandrinseitwithdistilledwater. ● RepeatExperiment1,usingsolutionD instead of solution C. ● Recordtheburettereadingsinthetableandcompletethetable.

Experiment1 Experiment2

finalburettereading/cm3

initialburettereading/cm3

difference/cm3

[4]

(c) Describe the appearance of the solution in the conical flask before adding the aqueous sodium thiosulfate.

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

(d) Beforetheadditionofthestarchsolution,describethechangestothecolourofthesolutionintheconicalflaskastheaqueoussodiumthiosulfateisadded.

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

(e) Whatcolourchangeisobservedintheconicalflaskwhenthestarchsolutionisadded?

from .......................................................... to ......................................................................[1]

3


(f) (i) Whichsolutionofpotassiumiodate,solutionC or solution D,isthemoreconcentrated?Explainyouranswer.

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

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

(ii) Howmanytimesmoreconcentratedisthissolutionofpotassiumiodate?

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

(g) Predict the volume of aqueous sodium thiosulfate which would be needed to react completely with30cm3 of solution D.

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

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

(h) (i) Statetwo sources of error in the experiments.

1 ..........................................................................................................................................

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

(ii) Suggesttwo improvements to reduce the sources of error in (h)(i).

1 ..........................................................................................................................................

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

[Total:16]

4

0620/51/M/J/17© UCLES 2017

2 You are provided with two solids E and F. Carryoutthefollowingtestsoneachsolid,recordingallofyourobservationsateachstage.

tests on solid E

(a) Describe the appearance of solid E.

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

(b) Place a small amount of solid E in a hard glass test-tube. Heat the solid gently then strongly. Recordyourobservations.

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

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

(c) (i) Place a small amount of solid Einatest-tubeandaddabout2cm3 of dilute sulfuric acid. Test the gas given off.

Recordyourobservations.

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

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

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

(ii) Now gradually add an excess of aqueous ammonia to the mixture in the test-tube. Recordyourobservations.

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

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

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

(d) CarryoutaflametestonsolidE. Recordyourobservations.

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

(e) Identify solid E.

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

5


tests on solid F

(f) Describe the appearance of solid F.

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

Addabout4cm3 of distilled water to about half of solid F in a test-tube and shake the test-tube to dissolve solid F.

Divide the solution into two equal portions in two test-tubes and carry out the following tests.

(g) (i) Tothefirstportionofthesolution,addanexcessofaqueoussodiumhydroxide. Recordyourobservations.

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

(ii) Tothesecondportionofthesolution,addabout1cm3 of dilute nitric acid and aqueous silver nitrate.

Recordyourobservations.

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

(h) CarryoutaflametestonsolidF. Recordyourobservations.

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

(i) Identify solid F.

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

[Total:18]

6

0620/51/M/J/17© UCLES 2017

3 Asampleoffurniturecleanercontainsaqueoussodiumchloride,aqueousammoniaandsand.

(a) Give a test to show the presence of ammonia in the mixture.

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

(b) Plan experiments to obtain a sample of

(i) purewaterfromthemixture, ...............................................................................................

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

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

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

(ii) pure sand from the mixture. ................................................................................................

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

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

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

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

[Total:6]

7

0620/51/M/J/17© UCLES 2017

Notes for use in qualitative analysisTests for anions

anion test test result

carbonate (CO32–) add dilute acid effervescence, carbon dioxide

produced

chloride (Cl –)

[in solution]acidify with dilute nitric acid, then add aqueous silver nitrate

white ppt.

bromide (Br –)[in solution]

acidify with dilute nitric acid, then add aqueous silver nitrate

cream ppt.

iodide (I–)[in solution]

acidify with dilute nitric acid, then add aqueous silver nitrate

yellow ppt.

nitrate (NO3–)

[in solution]add aqueous sodium hydroxide, then aluminium foil; warm carefully

ammonia produced

sulfate (SO42–)

[in solution]acidify, then add aqueous barium nitrate

white ppt.

sulfite (SO32–) add dilute hydrochloric acid, warm

gently and test for the presence ofsulfur dioxide

sulfur dioxide produced will turn acidified aqueous potassium manganate(VII) from purple to colourless

Tests for aqueous cations

cation effect of aqueous sodium hydroxide effect of aqueous ammonia

aluminium (Al 3+) white ppt., soluble in excess giving a

colourless solutionwhite ppt., insoluble in excess

ammonium (NH4+) ammonia produced on warming –

calcium (Ca2+) white ppt., insoluble in excess no ppt., or very slight white ppt.

chromium(III) (Cr3+) green ppt., soluble in excess grey-green ppt., insoluble in excess

copper(II) (Cu2+) light blue ppt., insoluble in excess light blue ppt., soluble in excess, giving a dark blue solution

iron(II) (Fe2+) green ppt., insoluble in excess green ppt., insoluble in excess

iron(III) (Fe3+) red-brown ppt., insoluble in excess red-brown ppt., insoluble in excess

zinc (Zn2+) white ppt., soluble in excess, giving a colourless solution

white ppt., soluble in excess, giving a colourless solution

8

0620/51/M/J/17© UCLES 2017




Tests for gases Flame tests for metal ions

gas test and test results metal ion flame colour

ammonia (NH3) turns damp, red litmus paper blue lithium (Li+) red

carbon dioxide (CO2) turns limewater milky sodium (Na+) yellow

chlorine (Cl 2) bleaches damp litmus paper potassium (K+) lilac

hydrogen (H2) ‘pops’ with a lighted splint copper(II) (Cu2+) blue-green

oxygen (O2) relights a glowing splint

sulfur dioxide (SO2) turns acidified aqueous potassium manganate(VII) from purple to colourless


[Turn overIB17 06_0620_61/FP© UCLES 2017

*3090986058*



Answer all questions.Electronic calculators may be used.You may lose marks if you do not show your working or if you do not use appropriate units.


CHEMISTRY 0620/61

Paper 6 Alternative to Practical May/June 2017

1 hour





2

0620/61/M/J/17© UCLES 2017

1 A student prepared strontium nitrate crystals.

The diagram shows some of the stages in this preparation.

strontiumcarbonate

added

stage 1 stage 2 stage 3

dilute acidunreactedsolid

strontium nitratesolution

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

(a) (i) Complete the box to identify the apparatus. [1]

(ii) What is used to add the strontium carbonate to the acid in stage 1?

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

(iii) Name the dilute acid used.

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

(iv) Give one expected observation in stage 2.

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

(b) Why is heat not necessary in stage 2?

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

(c) Which of the reactants is in excess? Explain your answer.

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

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

(d) Describe how crystals of strontium nitrate could be obtained from the mixture in stage 3.

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

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

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

[Total: 10]

3


2 A student investigated the reaction between aqueous sodium thiosulfate and two different aqueous solutions of potassium iodate labelled solution C and solution D.

Two experiments were carried out.

Experiment 1

● Aburettewasfilledwithaqueoussodiumthiosulfate.Theinitialburettereadingwasrecorded. ● Usingameasuringcylinder,20cm3 of solution Cwerepouredintoaconicalflask.10cm3 of

dilutesulfuricacidand1gofpotassiumiodidewereaddedtotheflasktoformasolutionofiodine.Theflaskwasswirledtomixthecontents.

● Aqueoussodiumthiosulfatewasslowlyaddedfromtheburettetotheflaskandswirledtomixthoroughly.

● Whenthecontentsoftheflaskturnedpaleyellow,starchsolutionwasaddedandthesolutionturnedblue-black.

● Moreaqueoussodium thiosulfatewas thenaddedslowly to theflaskuntil thesolution justturnedcolourless.Thefinalburettereadingwasrecorded.

(a) Usetheburettediagramstorecordthereadingsinthetableandcompletethetable.

4

5

6

initial reading

37

38

39

final reading



difference/cm3

[2]

4

0620/61/M/J/17© UCLES 2017

Experiment 2

● Theconicalflaskwasemptiedandrinsedwithdistilledwater. ● Experiment1wasrepeatedusingsolutionD instead of solution C.

(b) Usetheburettediagramstorecordthereadingsinthetableandcompletethetable.

20

21

22

initial reading

3

4

5

final reading



difference/cm3

[2]

(c) (i) Whichsolutionofpotassiumiodate,solutionC or solution D,isthemoreconcentrated?Explain your answer.

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

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

(ii) How many times more concentrated is this solution of potassium iodate?

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

(d) Predict the volume of aqueous sodium thiosulfate which would be needed to react completely with 30 cm3 of solution D.

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

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

5


(e) (i) State two sources of error in the experiments.

1. .........................................................................................................................................

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

(ii) Suggest two improvements to reduce the sources of error in (e)(i).

1. .........................................................................................................................................

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

[Total: 13]

6

0620/61/M/J/17© UCLES 2017

3 Twosolids,E and F,wereanalysed.SolidF was potassium iodide. Tests were carried out on each solid. Some of the observations on solid E are shown.

tests on solid E observations

Appearance of solid E. green solid

test 1

Solid E was heated gently then strongly. thesolidturnedblack

test 2

Dilute sulfuric acid was added to solid E.

The gas given off was tested.

Excess aqueous ammonia was then added to the mixture in the test-tube.

rapid effervescence

limewaterturnedmilky

apaleblueprecipitateformed,whichthendissolvedtoformadarkbluesolution

test 3

AflametestwascarriedoutonsolidE. blue-green colour

(a) Test 1 states that the solid should be heated gently then strongly.

Intermsofsafety,explainwhyitisnecessarytoheatgentlyatfirst.

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

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

(b) Identify the gas given off in test 2.

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

(c) Identify solid E.

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

7


tests on solid F

Complete the expected observations.

(d) Describe the appearance of solid F.

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

Distilled water was added to solid Finatest-tubeandshakentodissolvesolidF.

(e) (i) Tothefirstportionofthesolution,anexcessofaqueoussodiumhydroxidewasadded.

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

(ii) To thesecondportionof thesolution,dilutenitricacidandaqueoussilvernitratewereadded.

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

(f) AflametestwascarriedoutonsolidF.

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

(g) Describehowyouwouldcarryoutaflametest.

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

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

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

[Total: 11]

8

0620/61/M/J/17© UCLES 2017




4 Asampleoffurniturecleanercontainsaqueoussodiumchloride,aqueousammoniaandsand.

(a) Give a test to show the presence of ammonia in the mixture.

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

(b) Plan an investigation to obtain a sample of

(i) purewaterfromthemixture, ...............................................................................................

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

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

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

(ii) pure sand from the mixture. ................................................................................................

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

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

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

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

[Total: 6]

® IGCSE is a registered trademark.

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


© UCLES 2017 [Turn over


CHEMISTRY 0620/11 Paper 1 Multiple Choice (Core) May/June 2017

MARK SCHEME

Maximum Mark: 40

Published

This mark scheme is published as an aid to teachers and candidates, to indicate the requirements of the examination. Mark schemes should be read in conjunction with the question paper and the Principal Examiner Report for Teachers. Cambridge will not enter into discussions about these mark schemes. Cambridge is publishing the mark schemes for the May/June 2017 series for most Cambridge IGCSE®, Cambridge International A and AS Level and Cambridge Pre-U components, and some Cambridge O Level components.

0620/11 Cambridge IGCSE – Mark Scheme PUBLISHED

May/June 2017

© UCLES 2017 Page 2 of 3

Question Answer Marks

1 B 1

2 B 1

3 C 1

4 B 1

5 B 1

6 C 1

7 B 1

8 C 1

9 A 1

10 A 1

11 B 1

12 C 1

13 C 1

14 D 1

15 A 1

16 B 1

17 A 1

18 C 1

19 C 1

20 D 1

21 D 1

22 A 1

23 D 1

24 D 1

25 B 1

26 B 1

27 B 1

28 C 1


May/June 2017



29 A 1

30 A 1

31 C 1

32 C 1

33 D 1

34 D 1

35 C 1

36 B 1

37 D 1

38 A 1

39 D 1

40 C 1






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

MARK SCHEME

Maximum Mark: 40

Published

This mark scheme is published as an aid to teachers and candidates, to indicate the requirements of the examination. Mark schemes should be read in conjunction with the question paper and the Principal Examiner Report for Teachers. Cambridge will not enter into discussions about these mark schemes. Cambridge is publishing the mark schemes for the May/June 2017 series for most Cambridge IGCSE®, Cambridge International A and AS Level and Cambridge Pre-U components, and some Cambridge O Level components.


May/June 2017



1 D 1

2 C 1

3 D 1

4 B 1

5 C 1

6 D 1

7 B 1

8 A 1

9 B 1

10 B 1

11 B 1

12 C 1

13 B 1

14 C 1

15 A 1

16 C 1

17 D 1

18 A 1

19 C 1

20 D 1

21 D 1

22 A 1

23 C 1

24 D 1

25 A 1

26 B 1

27 C 1

28 C 1


May/June 2017



29 A 1

30 D 1

31 D 1

32 C 1

33 C 1

34 D 1

35 C 1

36 C 1

37 C 1

38 C 1

39 B 1

40 C 1






CHEMISTRY 0620/31 Paper 3 Theory (Core) May/June 2017

MARK SCHEME

Maximum Mark: 80

Published

This mark scheme is published as an aid to teachers and candidates, to indicate the requirements of the examination. It shows the basis on which Examiners were instructed to award marks. It does not indicate the details of the discussions that took place at an Examiners’ meeting before marking began, which would have considered the acceptability of alternative answers. Mark schemes should be read in conjunction with the question paper and the Principal Examiner Report for Teachers. Cambridge will not enter into discussions about these mark schemes. Cambridge is publishing the mark schemes for the May/June 2017 series for most Cambridge IGCSE®, Cambridge International A and AS Level and Cambridge Pre-U components, and some Cambridge O Level components.


May/June 2017



1(a)(i) A 1

1(a)(ii) E 1

1(a)(iii) C 1

1(a)(iv) B 1

1(a)(v) C 1

1(b) number of electrons in Br – = 36 1

number of neutrons in Cl = 18 1

number of protons in Cl = 17 AND number of protons in Br – = 35 1


2(a)(i) Na+ / sodium 1

2(a)(ii) sulfite / sulfate(IV) 1

2(a)(iii) 3 (mg) 1

2(a)(iv) 36.3 (mg) 1

2(a)(v) calcium hydrogencarbonate 1

2(b) flame test 1

yellow 1

2(c) MgCl2 1


May/June 2017



2(d) negative electrode: calcium / Ca 1

positive electrode: chlorine / Cl2 1


3(a) any 5 of: X has covalent bonding X particles are randomly arranged / irregularly arranged X particles are moving rapidly / freely / randomly / irregularly Y has ionic bonding / ionic Y particles are regularly arranged / lattice / in rows / uniformly arranged Y particles (only) vibrate / do not move from place to place Z has covalent bonding Z particles are regularly arranged / lattice / in a tetrahedral shape Z particles (only) vibrate / do not move from place to place

5

3(b) volume gets smaller 1

particles get closer together 1

3(c) drill tips / drills / cutting (tools) 1

3(d) A / substance Y dissolves easily in water 1

C / substance Y melts (at 8015 °C) 1

the change can be reversed by altering the conditions 1


May/June 2017



4(a) has two atoms in a molecule / two atoms combined 1

4(b)(i) the chlorine has displaced / replaced the bromine (in KBr) 1

4(b)(ii) (from green / colourless) to orange 1

4(b)(iii) I2 1

KBr 1

4(c) add (nitric acid then aqueous) silver nitrate 1

yellow precipitate 1

4(d)(i) water purification / water treatment / killing bacteria / in (swimming) pools / disinfectant 1

4(d)(ii) breaking down of a compound / breaking down of a substance 1

(using) heat 1

4(d)(iii) any 2 distinct pollution problems: • litter OR eyesore • sticks in gullets OR throats of birds / animals • blocking of drains OR watercourses • animals gets trapped OR tangled (in plastic) • poisonous vapours when burned • fills landfill sites

2


May/June 2017



5(a) circle drawn around the OH group 1

5(b) 20 1

5(c) C=C double bond 1

5(d)(i) increases with an increasing number of carbon atoms ORA 1

5(d)(ii) any value between –88 and 0 (°C) (exclusive of these values) 1

5(d)(iii) there is no (clear) trend / the numbers go down and up 1

5(d)(iv) liquid 1

30 °C is between melting and boiling point / 30 °C is above the melting point and below the boiling point 1

5(d)(v) substance containing carbon and hydrogen 1

only / and no other element 1

5(d)(vi)

1

5(d)(vii) 3 (CO2) 1

5 (O2) 1

C C

H H

H H

H H


May/June 2017



6(a)(i) aluminium

low density 1

good electrical conductivity 1

6(a)(ii) iron is cheap(er) / tungsten is (too) expensive OR iron is strong(er) / tungsten is weaker

1

6(a)(iii) tungsten because it has a (very) high melting point 1

6(b) any 2 properties: • high melting point / high boiling point • high density • hard / strong • sonorous / rings (when hit) • ions are coloured / compounds are coloured

2

6(c) 2 (W) 1

3 (O2) 1

6(d) tungsten < cobalt < iron < magnesium IF full credit is not awarded, allow 1 mark for either a correct sequence apart from a consecutive pair reversed OR for the whole sequence reversed

2

6(e)(i) the more concentrated the acid, the greater the rate ORA 1

6(e)(ii) nitric (acid) 1

6(e)(iii) any value between 19 and 39 hours (exclusive of these values) 1

6(e)(iv) pH 4 1


May/June 2017



7(a) the energy of the reactants is greater than the energy of the products / the product has less energy than the reactants / the arrow is going down (from reactants to product)

1

7(b) any 2 sources: • carbon monoxide from incomplete combustion of fossil fuels / named fossil fuel / named carbon-containing fuel • carbon dioxide from combustion of fossil fuels / respiration • methane from animal flatulence / rice paddy fields / bacteria / decomposition of vegetation / decomposition of

animals any 3 effects:

• carbon dioxide: global warming / greenhouse effect / acidification of oceans • methane: global warming / greenhouse effect • carbon monoxide: poisonous / toxic

5

7(c)(i) making mortar / whitewash / neutralising (acidic) soils / neutralising acidic lakes / flue gas desulfurisation / steelmaking / glassmaking / making plaster

1

7(c)(ii) 100 IF full credit is not awarded, allow 1 mark for (Ca =) 40, (C =) 12 and (O =) 16

2

7(d) add hydrochloric acid to the mixture 1

filter off the carbon 1

wash carbon (with water or other solvent) AND dry in an oven / air dry / leave in air / leave to dry 1






CHEMISTRY 0620/41 Paper 4 Theory Extended May/June 2017

MARK SCHEME

Maximum Mark: 80

Published



May/June 2017



1(a) proton number: the number of protons 1

nucleon number: the total number of protons and neutrons 1

nucleon number: in the nucleus / nuclei (of an atom) 1

1(b) (hydrogen is the only atom to have) no neutrons 1

1(c)

number of protons

number ofneutrons

number ofelectrons

19F 9 10 9 26Mg 12 14 12 31P3– 15 16 18 87Sr2+ 38 49 36

fluorine protons AND neutrons correct 1

magnesium neutrons AND electrons correct 1

phosphorus protons AND neutrons correct 1

phosphorus electrons correct 1

strontium protons AND neutrons correct 1

strontium electrons correct 1

1(d)(i) MgF2 1

1(d)(ii) Sr3P2 1


May/June 2017



2(a)(i) SO2 1

2(a)(ii) Na2O 1

2(a)(iii) Cr2O3 1

2(a)(iv) SiO2 1

2(a)(v) Al2O3 / Cr2O3 1

2(a)(vi) CO 1

2(b)(i) an amphoteric oxide will react with acids AND with bases 1

2(b)(ii) a neutral oxide will not react with acids or with bases 1


3(a)(i) no (more) effervescence 1

3(a)(ii) magnesium carbonate 1

3(a)(iii) (a solution in which) no more solute will dissolve 1

at that temperature 1

3(a)(iv) the solubility deceases as the temperature decreases 1

3(b)(i) moles of water = 2.52 / 18 = 0.14 (mol) 1

3(b)(ii) moles of anhydrous magnesium sulfate = 0.02 (mol) 1

3(b)(iii) ratio = 0.02 / 0.02 : 0.14 / 0.02 = 1 : 7 1


May/June 2017



3(b)(iv) MgSO4.7H2O M1 MgSO4 M2 rest of the formula correct

2

3(c) mix and stir the two solutions 1

filter (to obtain residue) 1

wash (the residue) using water 1

dry the residue between filter papers / in a warm place 1

3(d) Pb2+(aq) + SO42–(aq) → PbSO4(s)

M1 correct species M2 correct state symbols

2


4(a)(i) roast in air 1

4(a)(ii) 2ZnS + 3O2 → 2ZnO + 2SO2 M1 correct species M2 correct balancing

2

4(b)(i) coke 1

4(b)(ii) zinc is vaporised / boiled 1

and is condensed 1


May/June 2017



4(c)(i) Zn → Zn2+ + 2e– M1 correct species M2 correct balancing

2

4(c)(ii) 2H+ + 2e– → H2 M1 correct species M2 correct balancing

2

4(c)(iii) change: (the intensity would) decrease 1

reason: the difference in reactivity between zinc and iron is less than the difference in reactivity between zinc and copper 1


5(a) (stop-) watch AND syringe 1

5(b) graph starts at X and is a curve with a decreasing gradient 1

graph hits zero rate at 114 ± 6 seconds 1

5(c) M1 moles of carbon dioxide = 180 / 24 000 = 0.0075 1

M2 molar mass of barium carbonate = 197 1

M3 mass of barium carbonate = M1 × M2 = 1.48 (g) 1

5(d) curve starts from (0,0) and has a lower gradient than the original curve 1

because lumps have a lower surface area 1


May/June 2017



5(e) curve starts from (0,0) and has a steeper gradient than the original curve 1

finishes at the same volume of gas 1

because there are more particles per unit volume / dm3 / cm3 1

because there are more collisions per second / unit time OR a greater collision rate 1

5(f) 360 (cm3) 1


6(a) (compound that) contains carbon and hydrogen 1

and no other elements / only 1

6(b) any 3 from: • same / similar chemical properties • (same) general formula • (consecutive members) differ by CH2 • same functional group • common (allow similar) methods of preparation • physical properties vary in predictable manner / show trends / gradually change / example of a physical property

variation

3

6(c) propene 1

structure correctly shown 1

6(d) steam 1

catalyst 1


May/June 2017



6(e)(i) butanoic acid 1

1

6(e)(ii) acidified 1

(potassium) manganate(VII) 1

6(e)(iii) oxidation 1

6(f) methanol 1

ethanoic acid 1

catalyst 1

heat 1

CH3COOH + CH3OH → CH3COOCH3 + H2O 1






CHEMISTRY 0620/51 Paper 5 Practical Test May/June 2017

MARK SCHEME

Maximum Mark: 40

Published



May/June 2017



1(b) initial and final readings completed correctly 1

differences completed correctly 1

all readings to 1 d.p. 1

results comparable to the Supervisor’s results 1

1(c) red / brown / amber / orange 1

1(d) (becomes) yellow / orange / paler 1

1(e) yellow to blue / black 1

1(f)(i) solution C is more concentrated 1

a greater volume of thiosulfate was needed 1

1(f)(ii) ratio of the candidate’s differences from the table in (b) 1

1(g) 1.5 × value from table in (b) for Experiment 2 1

unit: cm3 1

1(h)(i) 2 sources of error, e.g.: • using a measuring cylinder to measure solution C / solution D • only carrying out the experiments once • going past the end-point

2

1(h)(ii) 2 meaningful improvements related to (h)(i): • use a pipette / burette • repeat the experiment • improvement linked to going past the end-point

2


May/June 2017



2(a) green 1

2(b) any 2 from: • turns black • condensation / drops of liquid formed • moves / jumps around

2

2(c)(i) any 3 from: • blue (solution) • bubbles / fizz • limewater • milky

3

2(c)(ii) blue 1

precipitate 1

(with excess) deep / royal blue solution / clear / precipitate dissolves 1

2(d) blue-green 1


May/June 2017



2(e) copper / Cu2+ 1

carbonate / CO32– 1

2(f) white 1

2(g)(i) no reaction / no change 1

2(g)(ii) yellow precipitate 1

2(h) lilac 1

2(i) potassium / K+ 1

iodide / I– 1


3(a) (red) litmus turns blue 1

3(b)(i) heat / boil the mixture 1

condense the vapour 1

3(b)(ii) filter / decant 1

wash residue (with water) 1

dry 1






CHEMISTRY 0620/61 Paper 6 Alternative to Practical May/June 2017

MARK SCHEME

Maximum Mark: 40

Published



May/June 2017



1(a)(i) stirrer / glass rod 1

1(a)(ii) Spatula 1

1(a)(iii) nitric (acid) 1

1(a)(iv) bubbles / fizz / effervescence 1

1(b) the reaction is (fast) at room temperature 1

1(c) strontium carbonate 1

solid is left behind 1

1(d) filter 1

heat / evaporate 1

to crystallising point / glass rod test / until saturation point 1


2(a) initial and final readings completed correctly: 4.1, 38.3 1

difference completed correctly: 34.2 1

2(b) initial and final readings completed correctly: 3.7, 20.8 1

difference completed correctly: 17.1 1

2(c)(i) solution C is more concentrated 1

a greater volume of thiosulfate was needed 1

2(c)(ii) 2 × as concentrated 1


May/June 2017



2(d) 1.5 × value from table in (b) for Experiment 2 1

unit: cm3 1

2(e)(i) 2 sources of error, e.g.: • using a measuring cylinder to measure solution C / solution D • only carrying out the experiments once • going past the end-point

2

2(e)(ii) 2 meaningful improvements related to (e)(i): • use a pipette / burette • repeat the experiment • improvement linked to going past the end-point

2


3(a) solid spits out of the tube / the tube might crack 1

3(b) carbon dioxide 1

3(c) copper / Cu2+ 1

carbonate / CO32– 1

3(d) white 1

3(e)(i) no reaction / change 1

3(e)(ii) yellow 1

precipitate 1

3(f) lilac 1


May/June 2017



3(g) any 2 from: • blue / roaring / hot flame • use of a splint / wire to introduce the solid into the flame • use of (concentrated) hydrochloric acid

2


4(a) (red) litmus turns blue 1

4(b) heat / boil the mixture 1

condense the vapour 1

4(c) filter / decant 1

wash residue (with water) 1

dry 1

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