Cambridge International AS & A Level

CHEMISTRY 9701/11
Paper 1 Multiple Choice May/June 2024
1 hour 15 minutes

You must answer on the multiple choice answer

*5097018829*

sheet. You will need: Multiple choice answer sheet

Soft clean eraser
Soft pencil (type B or HB is recommended)

INSTRUCTIONS
 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 multiple choice answer sheet.
 Follow the instructions on the multiple choice answer sheet.
 Write in soft pencil.
 Write your name, centre number and candidate number on the multiple choice
answer sheet in the spaces provided unless this has been done for you.
 Do not use correction fluid.
 Do not write on any bar codes.
 You may use a calculator.

INFORMATION
 The total mark for this paper is 40.
 Each correct answer will score one mark.
 Any rough working should be done on this question paper.
 The Periodic Table is printed in the question paper.
 Important values, constants and standards are printed in the question paper.

This document has 20 pages. Any blank pages are indicated.

IB24 06_9701_11/2RP
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1 Sample X is added to water and made up to a total volume of 200 cm3. This gives a
solution of
0.100 mol dm–3 HCl.

What is X?

A 10 cm3 of 1.00 mol dm–3 HCl

B 30 cm3 of 0.90 mol dm–3 HCl

C 50 cm3 of 0.40 mol dm–3 HCl

D 100 cm3 of 0.30 mol dm–3 HCl

2 A mixture of 10 cm3 of methane and 10 cm3 of ethane was sparked with an

excess of oxygen. After cooling, the residual gas was passed through aqueous
potassium hydroxide.

All gas volumes were measured at the same temperature and

pressure. Which volume of gas was absorbed by the alkali?

A 15 cm3 B 20 cm3 C 30 cm3 D 40 cm3

3 Z is a compound of two elements, X and Y.

Element X shows a very large increase between its 5th and 6th ionisation energies.
It has the second largest 1st ionisation energy in its group.

Element Y shows a very large increase between its 6th and 7th ionisation energies.
It has the largest 1st ionisation energy in its group.

What is compound Z?

A NO2 B PCl 5 C P4O10 D SF6

131
4 Which statement about
5 I is correct?
3
131
A A negative ion of5 I contains 53 neutrons and 52 electrons.
3
131
B A negative ion of5 I contains 53 neutrons and 54 electrons.
3
131
C A negative ion of5 I contains 78 neutrons and 52 electrons.
3
131
D A negative ion of5 I contains 78 neutrons and 54 electrons.
3

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5 When solid aluminium chloride is heated, Al 2Cl 6 is formed.

Which bonding is present in Al 2Cl 6?

A covalent and coordinate (dative covalent)

B covalent only
C ionic and coordinate (dative covalent)
D ionic only

6 The structure of the sulfur dioxide molecule is shown.

O S O
What is the shape of the sulfur dioxide molecule?

A linear
B non-linear
C pyramidal
D tetrahedral

7 What is the density of a sample of fluorine gas at 32 C and 100 000 Pa? Assume
fluorine behaves as an ideal gas under these conditions.

A 1.4 g dm–3 B 1.5 g dm–3 C 1.6 g dm–3 D 1.7 g dm–3

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8 The graph shows the boiling points of the hydrogen compounds of Group 16 elements.

100 H2O

boiling point
C
/ 0
H2T
H2Se e
H2S
–100

Which statement correctly explains why water does not fit the trend of the other
compounds?

A There are fewer electrons in the oxygen atoms so there is less shielding of
the nuclear charge.
B There are strong hydrogen bonds in water but not in the other compounds.
C The covalent bonds in water are much stronger than in the other compounds.
D The water molecules are smaller and so have stronger van der Waals’ forces.

9 An energy cycle is shown.

CH4 + 2O2

X Y

C + 2H2 + CO2 + 2H2O

2O2 Z

The energy changes involved are X, Y and Z.

The numerical value of energy change Y is either –890

or +890. The numerical value of energy change Z is

either –964 or +964. Which of the three values are

negative?

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

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10 For a certain endothermic reaction, the activation energy is numerically equal to

twice the enthalpy change of reaction.

Which reaction pathway diagram is correct for this reaction?

A B

energy energy

progress of reaction progress of reaction

C D

energy energy

progress of reaction progress of reaction

11 Sodium chromate(VI), Na2CrO4, is manufactured by heating chromite, FeCr2O4,

with sodium carbonate in an oxidising atmosphere. Chromite contains
4 Cr 2O 2– ions.

2FeCr2O4 + 4Na2CO3 + 3 21 O2  4Na2CrO4 + Fe2O3 + 4CO2

What happens in this reaction?

A Chromium and iron are the only elements oxidised.

B Chromium, iron and carbon are oxidised.
C Only chromium is oxidised.
D Only iron is oxidised.

12 Oxygen can be prepared by the reaction of potassium manganate(VII),

KMnO4, hydrogen peroxide, H2O2, and sulfuric acid, H2SO4. Each H2O2 molecule loses
two electrons in this reaction. The other products of the reaction are potassium
sulfate, manganese(II) sulfate and water.

How many moles of oxygen gas are produced when 1.0 mol of KMnO4 reacts with an
excess of H2O2 in acidic conditions?

A 2.0 mol B 2.5 mol C 4.5 mol D 5.0 mol

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13 An alcohol, ROH, reacts reversibly with ethanoic acid to produce an ester.

ROH(l) + CH3COOH(l) CH3COOR(l) + H2O(l)

3.0 mol of ROH, 2.0 mol of ethanoic acid and 1.0 mol of water are mixed together. At
equilibrium,
1.5 mol of CH3COOR is present.

What is the value of the equilibrium constant, Kc, for this reaction?

A 0.20 B 0.25 C 2.00 D 5.00

14 Graphs can be drawn to show the percentage of ammonia at equilibrium when

nitrogen and hydrogen are mixed at different temperatures and pressures.

Which diagram correctly represents these two graphs?

A B
40 40
400 500
% NH3 at C C
% NH3 at
equilibrium 2
equilibrium 2
0 500 0 400
0 C C
0
0
10 0 10 20

20
pressure / 103 kPa pressure / 103 kPa

C D
40 500 C 40 400 C

% NH3 at 400 C % NH3 at 500 C

20 20
equilibriu equilibriu
m m
0 0
0 10 0 10 20

20
pressure / 103 kPa pressure / 103 kPa

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15 The Boltzmann distribution for the hydrogenation of an alkene at a particular

temperature in the absence of a catalyst is shown.

proportion
of
molecules Ea
with energy E

0
0 molecular energy E

Which row correctly describes the effects of adding a nickel catalyst to the reaction
vessel?

the shape of the

activation energy, Ea
Boltzmann
distribution
A changes decreases
B changes increases
C does not change decreases
D does not change increases

16 Elements Y and Z are both in Period 3 of the Periodic Table.

When the chloride of element Y is added to water, it reacts and a solution of pH 2 is

produced. When the chloride of element Z is added to water, it dissolves and a

solution of pH 7 is produced. Which statement explains these observations?

A Both chlorides hydrolyse in water.

B Element Y is magnesium and element Z is sodium.
C Element Y is phosphorus and element Z is aluminium.
D Element Y is silicon and element Z is sodium.

17 Aluminium, silicon and phosphorus are elements in Period 3 of the Periodic Table.
Each element forms an oxide.

Which row is correct?

Al 2O3 SiO2 P4O10

A basic amphoteric acidic

B giant ionic giant ionic simple molecular
C high melting point high melting point low melting point
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D vigorous reaction with slight reaction with vigorous reaction with
water water water

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18 Which statement is correct?

A The atomic radius of silicon is larger than that of aluminium.

B The boiling point of chlorine is higher than that of silicon.
C The first ionisation energy of sulfur is greater than that of phosphorus.
D The electrical conductivity of magnesium is greater than that of sodium.

19 All solubility data in this question is given at the same temperature.

The table gives some data for compounds of calcium and for compounds of X, an
unidentified element in Group 2.

decompositi
solubility of sulfate solubility of
element on
/ mol per 100 g of hydroxide
temperature
water / mol per 100 g of
of carbonate
water
/ C
Ca 840 4.66  10–3 1.53  10–3
X 1150

What is the missing data for element X?

solubility of sulfate solubility of

/ mol per 100 g of hydroxide
water / mol per 100 g of
water
A 7.11  10–5 2.00  10–5
B 7.11  10–5 3.37  10–3
C 1.83  10–1 2.00  10–5
D 1.83  10–1 3.37  10–3

20 What is the total volume of gas produced, measured at room conditions, when
0.010 mol of anhydrous magnesium nitrate is completely decomposed by heating?

A 240 cm3 B 480 cm3 C 600 cm3 D 720 cm3

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21 A solid sodium halide, NaX, is reacted with concentrated sulfuric acid. The lowest
oxidation state of sulfur in the products is +4.

Halogen Y2 is less volatile than halogen X2.

What are the identities of sodium halide NaX and halogen Y2?

sodium halide NaX halogen Y2

A sodium bromide chlorine

B sodium bromide iodine
C sodium iodide bromine
D sodium iodide astatine

22 Compound Q dissolves in water. Q(aq) does not react with dilute sulfuric acid.

Q(aq) forms a precipitate when aqueous silver nitrate is added. This precipitate is
partially soluble in aqueous ammonia.

What could be compound Q?

A barium bromide
B barium iodide
C magnesium bromide
D magnesium iodide

23 Nitrogen dioxide is a gas that contributes to air pollution. It is produced in internal

combustion engines.

Which statement is correct?

A Nitrogen dioxide acts as a catalyst in the atmospheric oxidation of sulfur

dioxide to sulfur trioxide.
B Nitrogen dioxide reacts to form nitrogen monoxide in the catalytic converter of a
car exhaust system.
C PAN forms when nitrogen dioxide reacts with the gases formed by complete
combustion of the fuel.
D Under high pressure in an internal combustion engine, nitrogen dioxide forms
from impurities in the fuel.

24 What is the bond angle in the ammonium ion?

A 90 B 107 C 109.5 D 120

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25 Structural isomerism and stereoisomerism should be taken into account when

answering this question.

The structure of 3-methylcyclobutene is shown.

3-methylcyclobutene

A mixture containing all stereoisomers of 3-methylcyclobutene is treated with HBr.

This produces a mixture of isomeric bromomethylcyclobutanes.

How many stereoisomers does 3-methylcyclobutene have, and how

many isomeric bromomethylcyclobutanes are present in the product mixture?

3-methylcyclobutene bromomethylcyclobutanes

A 2 4
B 2 6
C 4 4
D 4 8

26 The diagram shows the structure of X.

X
NC H

H H

Which row is correct?

number of type of hybridisation

 bonds in X of the carbon atoms
in X
A 4 sp and sp2
B 4 sp2 and sp3
C 6 sp and sp2
D 6 sp2 and sp3

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27 The diagram shows the skeletal formula of citric acid.

citric acid
O
O OH

O
HO OH
OH

What is the molecular formula of citric acid?

A C6H8O7 B C6H4O7 C C8H8O7 D C10H8O7

28 Which reaction occurs when ethane and chlorine are mixed in diffused sunlight?

A a free-radical substitution with hydrogen given off

B a free-radical substitution with hydrogen chloride given off
C a free-radical substitution with no gas given off
D a nucleophilic substitution with hydrogen chloride given off

29 A molecule of geraniol is shown.

geraniol

OH

What is formed when geraniol is reacted with an excess of cold dilute acidified
4 MnO –?

A B
O

OH
HO HO OH
OH OH HO HO
O O

C
D
O
+ O + O
O
O OH OH
OH OH

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30 Q is either a primary or a tertiary halogenoalkane. Q undergoes hydrolysis

with aqueous sodium hydroxide.

The first step in the mechanism of this reaction involves two species reacting

together. Which row is correct?

Q behaviour of hydroxide ion

A primary halogenoalkane electrophile

B primary halogenoalkane nucleophile
C tertiary halogenoalkane electrophile
D tertiary halogenoalkane nucleophile

31 2-bromopropane is converted to 1,2-dibromopropane in a pathway involving two

reactions.

reaction reaction
2- compound 1,2-dibromopropane
1 2
bromopropane X

What are the reagents and conditions for the two reactions?

reaction 1 reaction 2

A heat under reflux with aqueous HBr(g) at room temperature

NaOH
B heat under reflux with aqueous Br2(l) at room temperature
NaOH
C heat under reflux with ethanolic HBr(g) at room temperature
NaOH
D heat under reflux with ethanolic Br2(l) at room temperature
NaOH

32 Compound X is a single, pure, optical isomer. Compound X is heated with an

excess of concentrated H2SO4. Only one organic product is formed.

What is compound X?

A B C D
OH
OH CH2OH
HO

33 Which reagents could be used to form 2-bromobutane from butan-1-ol?

A bromine and ultraviolet light

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B concentrated sulfuric acid with potassium bromide, under reflux
C concentrated sulfuric acid followed by bromine
D concentrated sulfuric acid followed by hydrogen bromide

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34 X is a non-cyclic ketone with a single carbonyl group and no other functional

groups. Ketone X has the following properties.

● When ketone X is treated with NaBH4, the organic product has a Mr

2.3256% greater than the Mr of ketone X.
● Ketone X gives a yellow precipitate with alkaline I2(aq).

How many isomeric ketones could be ketone X?

A 1 B 2 C 3 D 4

35 Compound Y:

● changes the colour of acidified K2Cr2O7 from orange to green

● has no effect on Fehling’s reagent

● produces an orange precipitate with 2,4-dinitrophenylhydrazine reagent.

What is compound Y?

A B C D

CH3CCH2C
CH3CCH2CCH3 CH3CCH2CH2OH HOCH2CH2CH2CH2OH
H

O O O O O

36 The product of the reaction between propanone and hydrogen cyanide is hydrolysed
under acidic conditions.

What is the formula of the final product?

A CH3CH(OH)COOH
B CH3CH2CH2COOH
C (CH3)2CHCONH2
D (CH3)2C(OH)COOH

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37 P is a carboxylic acid with molecular formula C5H10O2.

Carboxylic acid P reacts with an excess of LiAl H4 to form compound Q.

Which pairs of molecules could be carboxylic acid P and compound

Q?

carboxylic acid P compound Q

1 CH3(CH2)3COOH CH3(CH2)3OH
2 CH3(CH2)3COOH CH3(CH2)3CHO
3 (CH3)3CCOOH (CH3)3CCH2OH

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

38 Compound X is treated with an excess of dilute aqueous potassium hydroxide.

X
O

What is the structure of the organic product?

A B
O
O
–
O OH HO OH

C
D
O
O
–
O
HO OH
OH

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39 A section showing two repeat units of an addition polymer is shown.

CH3 CH3 CH3 CH3

C C C C

Cl CH3 Cl CH3

What is the identity of the monomer that produced this polymer?

A 2-chloro-3-methylbutane
B 2-chloro-3-methylbut-2-ene
C 2-chloropent-2-ene
D 2,4-dichloro-3,3,4,5-tetramethylhexane

40 The relative atomic mass of antimony is 121.76.

Antimony has two isotopes. The mass numbers of the two isotopes differ by two.
The isotope with the lower mass number is the more abundant.

What is the percentage abundance of the isotope with the higher mass number?

A 12% B 38% C 62% D 88%

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Important values, constants and standards

molar gas constant R = 8.31 J K–1 mol–1

Faraday constant F = 9.65  104 C mol–1
Avogadro constant L = 6.022  1023 mol–1
electronic charge e = –1.60  10–19 C
molar volume of gas Vm = 22.4 dm3 mol–1 at s.t.p. (101 kPa and 273
K)
Vm = 24.0 dm3 mol–1 at room conditions
ionic product of water Kw = 1.00  10–14 mol2 dm–6 (at 298 K (25 C))
specific heat capacity of water c = 4.18 kJ kg–1 K–1 (4.18 J g–1 K–1)

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To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the
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is freely available to download at www.cambridgeinternational.org after the live examination series.

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

The Periodic Table of Elements

Group
1 2 13 14 15 16 17 18
1 2

H He
hydrogen helium
Key 1.0 4.0
3 4 atomic number 5 6 7 8 9 10

Li Be atomic symbol B C N O F Ne
lithium beryllium name boron carbon nitrogen oxygen fluorine neon
6.9 9.0 relative atomic mass 10.8 12.0 14.0 16.0 19.0 20.2
11 12 13 14 15 16 17 18

Na Mg Al Si P S Cl Ar
sodium magnesium aluminium silicon phosphorus sulfur chlorine argon
23.0 24.3 3 4 5 6 7 8 9 10 11 12 27.0 28.1 31.0 32.1 35.5 39.9
19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36

K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
24
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potassium calcium scandium titanium vanadium chromium manganese iron cobalt nickel copper zinc gallium germanium arsenic selenium bromine krypton
39.1 40.1 45.0 47.9 50.9 52.0 54.9 55.8 58.9 58.7 63.5 65.4 69.7 72.6 74.9 79.0 79.9 83.8
37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54

20
Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe
rubidium strontium yttrium zirconium niobium molybdenum technetium ruthenium rhodium palladium silver cadmium indium tin antimony tellurium iodine xenon
85.5 87.6 88.9 91.2 92.9 95.9 – 101.1 102.9 106.4 107.9 112.4 114.8 118.7 121.8 127.6 126.9 131.3
55 56 57–71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86

Cs Ba lanthanoids
Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
caesium barium hafnium tantalum tungsten rhenium osmium iridium platinum gold mercury thallium lead bismuth polonium astatine radon
132.9 137.3 178.5 180.9 183.8 186.2 190.2 192.2 195.1 197.0 200.6 204.4 207.2 209.0 – – –
87 88 89–103 104 105 106 107 108 109 110 111 112 113 114 115 116 117 118

Fr Ra actinoids
Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
francium radium rutherfordium dubnium seaborgium bohrium hassium meitnerium darmstadtium roentgenium copernicium nihonium flerovium moscovium livermorium tennessine oganesson
– – – – – – – – – – – – – – – – –

57 58 59 60 61 62 63 64 65 66 67 68 69 70 71

lanthanoids La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
lanthanum cerium praseodymium neodymium promethium samarium europium gadolinium terbium dysprosium holmium erbium thulium ytterbium lutetium
138.9 140.1 140.9 144.4 – 150.4 152.0 157.3 158.9 162.5 164.9 167.3 168.9 173.1 175.0
89 90 91 92 93 94 95 96 97 98 99 100 101 102 103

actinoids Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
actinium thorium protactinium uranium neptunium plutonium americium curium berkelium californium einsteinium fermium mendelevium nobelium lawrencium
– 232.0 231.0 238.0 – – – – – – – – – – –