Cambridge Assessment International Education

Cambridge International Advanced Subsidiary and Advanced Level

CHEMISTRY 9701/11
Paper 1 Multiple Choice May/June 2019
1 hour
Additional Materials: Multiple Choice Answer Sheet
Soft clean eraser
*1984267027*

Soft pencil (type B or HB is recommended)

Data Booklet

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.
Electronic calculators may be used.

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

IB19 06_9701_11/4RP
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Section A

For each question there are four possible answers, A, B, C and D. Choose the one you consider to
be correct.

Use of the Data Booklet may be appropriate for some questions.

1 The temperature of a sample of an inert gas is increased.

What effect does this have on the number of molecules with the most probable energy and on the
number of molecules with high energy?

number of molecules with number of molecules

the most probable energy with high energy

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

2 A sample of element X is analysed using mass spectrometry. The mass spectrum obtained is
shown.

56%

41%

% abundance

3%

112 113 114 115 116

m/e

What is the relative atomic mass of this sample of element X?

A 113.7 B 114.0 C 114.2 D 114.4

3 A washing powder contains sodium hydrogencarbonate, NaHCO3, as one of the ingredients.

In a titration, a solution containing 1.00 g of this washing powder requires 7.15 cm3 of
0.100 mol dm–3 sulfuric acid for complete reaction. The sodium hydrogencarbonate is the only
ingredient that reacts with the acid.

What is the percentage by mass of sodium hydrogencarbonate in the washing powder?

A 3.0% B 6.0% C 12.0% D 24.0%

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4 The outermost electron in an atom of neon occupies a particular orbital.

Which row shows the relative energy and shape of this orbital?

energy of orbital relative

shape of orbital
to other occupied orbitals

A higher or equal

B higher or equal

C lower or equal

D lower or equal

5 In which species is there a lone pair of electrons?

A CH3 B CH3+ C CH3– D CH4

6 When an evacuated tube of volume 400 cm3 is filled with gas at 300 K and 101 kPa, the mass of
the tube increases by 0.65 g.

Assume the gas behaves as an ideal gas.

What could be the identity of the gas?

A argon
B helium
C krypton
D neon

7 Under which conditions will nitrogen behave most like an ideal gas?

temperature pressure

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

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8 Two reactions and their enthalpy changes are shown.

2C(s) + 2H2(g) → C2H4(g) ∆H o = +52.2 kJ mol–1

C2H2(g) + H2(g) → C2H4(g) ∆H o = –175.8 kJ mol–1

These data can be used to calculate the enthalpy change for the reaction shown.

2C(s) + H2(g) → C2H2(g) ∆H o = X

What is the value of X?

A –228.0 kJ mol–1
B –123.6 kJ mol–1
C +123.6 kJ mol–1
D +228.0 kJ mol–1

9 Ethanedioic acid, HO2CCO2H, can be oxidised by KMnO4 in dilute sulfuric acid. The products of
this reaction are carbon dioxide, water, potassium sulfate and manganese(II) sulfate.

In this reaction each ethanedioic acid molecule loses two electrons as it is oxidised. A
half-equation for this process is shown.

HO2CCO2H → 2CO2 + 2H+ + 2e–

How many water molecules are produced when five ethanedioic acid molecules are oxidised by
KMnO4 in dilute sulfuric acid?

A 5 B 8 C 10 D 16

10 Hydrogen iodide gas decomposes reversibly producing iodine vapour and hydrogen.

2HI(g) I2(g) + H2(g) ∆H = +12 kJ mol–1

The position of the equilibrium for this reaction may be altered by changing the external
conditions.

Which row correctly describes the change in position of equilibrium?

effect of increasing effect of increasing

the pressure the temperature

A moves to the right moves to the right

B moves to the right moves to the left
C no change moves to the right
D no change moves to the left

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11 The reaction between sulfur dioxide and oxygen is reversible.

2SO2(g) + O2(g) 2SO3(g) Kc = 280 mol–1 dm3 at 1000 K

In an equilibrium mixture at 1000 K the sulfur trioxide concentration is 6.00 mol dm–3.

The sulfur dioxide concentration is twice the oxygen concentration.

What is the sulfur dioxide concentration?

A 0.175 mol dm–3

B 0.254 mol dm–3
C 0.318 mol dm–3
D 0.636 mol dm–3

12 1.15 g of a metallic element needs 300 cm3 of oxygen for complete reaction, under room
conditions, to form an oxide which contains O2– ions.

What could be the identity of this metallic element?

A calcium
B magnesium
C potassium
D sodium

13 The relative melting points of four consecutive elements in the Periodic Table are shown in the
graph.

The elements all have proton numbers less than 20.

Which element is in Group 16?

melting
point / K

B C
273
D
proton number

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14 Substance X reacts with water. A gas is given off and the pH of the solution increases. The
solution is then reacted with sulfuric acid and a white precipitate forms.

What could be substance X?

A barium
B barium oxide
C magnesium
D magnesium oxide

15 Solutions of 0.1 mol dm–3 Mg(NO3)2 and 0.1 mol dm–3 Ba(NO3)2 separately undergo a series of
reactions using pure reagents.

sodium
carbonate excess HCl (aq) excess
solution then boil NaOH(aq)
Mg(NO3)2(aq) M N P
sodium
carbonate excess HCl (aq) excess
solution then boil NaOH(aq)
Ba(NO3)2(aq) Q R S

M, N and P are magnesium compounds.

Q, R and S are barium compounds.

How many of M, N, P, Q, R and S are white precipitates?

A 2 B 3 C 4 D 5

16 Concentrated sulfuric acid is added to separate solid samples of sodium chloride, sodium
bromide and sodium iodide.

With which samples does sulfuric acid act as an oxidising agent?

A sodium chloride only

B sodium chloride and sodium bromide
C sodium bromide and sodium iodide
D sodium iodide only

17 The reaction of bromine with warm NaOH(aq) produces products with the same oxidation
numbers, in the same ratios, as the reaction of chlorine with hot NaOH(aq).

In one reaction between bromine and warm NaOH(aq), 30.2 g of a product containing sodium,
bromine and oxygen is produced.

Which mass of NaOH has reacted?

A 8.00 g B 10.2 g C 20.3 g D 48.0 g

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18 At 550 °C nitrogen dioxide reacts with unburnt hydrocarbon fragments such as CH3 in the
catalytic converter of a motor vehicle.

4CH3 + 7NO2 → 3 21 N2 + 4CO2 + 6H2O

Which row gives the energy change for this reaction and a possible reason for it?

energy change reason why the reaction is endothermic

of reaction or exothermic

A endothermic chemical energy is converted to heat energy

B endothermic the N≡N bond energy is very high
C exothermic CO2 and H2O have negative values
D exothermic double bonds are broken in NO2

19 Which statement is correct?

A Ammonia reacts with alkalis to form the ammonium ion.

B Ammonium chloride contains ionic, covalent and co-ordinate bonds.
C The ammonium ion reacts with acids to produce ammonia.

D The bond angle in the ammonium ion is approximately 107°.

20 The diagrams show two different compounds.

O O

1 2

What is

● the total number of structural isomers, including compound 2, that could be formed
by adding a second methyl group to the ring of compound 1,

● the number of π electrons in each compound?

number of number of
isomers π electrons

A 3 2
B 3 4
C 5 2
D 5 4

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21 Which compound has the molecular formula C6H10O?

A B C D
O
O
O
OH

22 What is the structural formula of the major product when hydrogen bromide reacts with
2-methylbut-2-ene?

A CH2BrCH(CH3)CH2CH3
B (CH3)2CBrCH2CH3
C (CH3)2CHCHBrCH3
D (CH3)2CHCH2CH2Br

23 Which reaction is most likely to involve the formation of a positively charged intermediate?

A 1-bromopentane and warm dilute NaOH(aq)

B 1-bromo-2,2-dimethylpropane and warm dilute NaOH(aq)
C 1-bromo-3-methylbutane and warm dilute NaOH(aq)
D 2-bromo-2-methylbutane and warm dilute NaOH(aq)

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24 The infra-red spectrum of a substance with empirical formula C2H4O is shown.

100

transmittance
50

Y
0
4000 3000 2000 1500 1000 500
–1
wavenumber / cm

Which bonds are responsible for peak X and peak Y?

peak X peak Y

A C–H C=C
B C–H C=O
C O–H C=C
D O–H C=O

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25 The structure of coniine is shown.

coniine

N CH2CH2CH3
H

Coniine can be synthesised by reacting ammonia with a dibromo compound, X.

NH3 + C8H16Br2 → coniine + 2HBr

X

What is the name of compound X?

A 1,1-dibromo-2-propylcyclopentane
B 1,2-dibromo-2-propylcyclopentane
C 1,4-dibromooctane
D 1,5-dibromooctane

26 Structural isomerism and stereoisomerism should be considered when answering this question.

3-methylhexan-3-ol reacts with hot, concentrated sulfuric acid to form several isomeric
compounds with the molecular formula C7H14.

3-methylhexan-3-ol

HO

How many isomeric compounds could be formed in this reaction?

A 3 B 4 C 5 D 6

27 An organic compound T undergoes the following reactions.

● T is oxidised by hot, acidified potassium manganate(VII).

● T reacts with sodium to give hydrogen.

What could be compound T?

A CH3CH2CH(OH)CH3
B CH3CH2CH2CHO
C (CH3)3COH
D CH3CH2COCH3

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28 Compound X is treated with two reagents successively, forming compound Z.

CHO a mild
oxidising
agent NaBH4
Y Z

COCH3

What could be Z?

A B C D

CO2H CH2OH CH2OH CO2H

CH(OH)CH3 CH(OH)CH3 CH(OH)CH3 CH(OH)CH3

29 Which reagent may be used to distinguish between propanone and ethanol?

A 2,4-dinitrophenylhydrazine
B bromine water
C Fehling’s reagent
D Tollens’ reagent

30 Which compound is chiral?

A 1-chloro-3-methylbutane
B 2-chloro-2-methylbutane
C 2-chloro-3-methylbutane
D 3-chloropentane

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Section B

For each of the questions in this section, one or more of the three numbered statements 1 to 3 may
be correct.

Decide whether each of the statements is or is not correct (you may find it helpful to put a tick against
the statements that you consider to be correct).

The responses A to D should be selected on the basis of

A B C D

1, 2 and 3 1 and 2 2 and 3 1 only

are only are only are is
correct correct correct correct

No other combination of statements is used as a correct response.

Use of the Data Booklet may be appropriate for some questions.

31 An atom of calcium-48 can form a 2+ ion.

Which statements about this ion are correct?

1 It has 20 protons.
2 It has 28 neutrons.
3 It has 22 electrons.

32 Four elements, W, X, Y and Z, have electronic configurations as shown.

W X Y Z

2,4 2,6 2,8,2 2,8,8,1

Which formulae represent compounds that have boiling points below room temperature?

1 WX2
2 YX
3 Z2X

33 Which statements about enthalpy changes are correct?

1 The enthalpy change of atomisation is always positive.

2 The enthalpy change when a C–C bond is broken is positive.
3 The enthalpy change of neutralisation of a weak acid is always negative.

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34 Vanadium and pepsin can both act as catalysts. Vanadium is a metal. Pepsin is an enzyme.

Which statements are correct for both vanadium and pepsin?

1 They will speed up any chemical reaction.

2 They can lower the activation energy for a reaction.
3 They are not used up when they act as catalysts.

35 Which oxides, when placed in cold water for one day, will react with the water?

1 MgO
2 Al 2O3
3 SiO2

36 A mixture of magnesium carbonate and magnesium nitrate is heated strongly in a hard-glass

test-tube.

Which gases are formed?

1 carbon dioxide
2 nitrogen dioxide
3 oxygen

37 Which statements about poly(alkene)s are correct?

1 Poly(alkene)s do not react with Br2(aq) in the dark.

2 Disposal of poly(alkene)s by combustion can produce harmful products.

3 Poly(alkene)s do not readily biodegrade.

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The responses A to D should be selected on the basis of

A B C D

1, 2 and 3 1 and 2 2 and 3 1 only

are only are only are is
correct correct correct correct

No other combination of statements is used as a correct response.

38 Compound Y

● reacts with alkaline aqueous iodine to form a yellow precipitate

● changes the colour of warm, acidified potassium dichromate(VI) solution.

What could be compound Y?

OH
1

O
2
H

3
O

39 Carboxylic acids can be made by several different reactions.

Which statements are correct?

1 The acid hydrolysis of CH3CH2CN will make ethanoic acid.

2 The oxidation of CH3CH2CH2CH2OH will make butanoic acid.
3 The oxidation of CH3CH2CHO will make propanoic acid.

40 Carboxylic acids react with alcohols to produce esters.

Carboxylic acid X forms one ester only with molecular formula C5H10O2.

What could X be?

1 ethanoic acid
2 propanoic acid
3 butanoic acid

© UCLES 2019 9701/11/M/J/19

 Cambridge Assessment International Education
Cambridge International Advanced Subsidiary and Advanced Level
*6036196388*

CHEMISTRY 9701/21
Paper 2 AS Level Structured Questions May/June 2019
 1 hour 15 minutes
Candidates answer on the Question Paper.
Additional Materials: Data Booklet

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 fluid.
DO NOT WRITE IN ANY BARCODES.

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.
A Data Booklet is provided.

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.

This document consists of 10 printed pages and 2 blank pages.

IB19 06_9701_21/3RP
© UCLES 2019 [Turn over
 2

Answer all the questions in the spaces provided.

1 (a) Group 2 elements share common chemical properties.

(i) Calcium reacts in cold water more quickly than magnesium because more energy is
required to remove the outer electrons in magnesium. This occurs even though calcium
atoms have a greater nuclear charge.

Explain why more energy is required to remove the outer electrons in magnesium than in
calcium.

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

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

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

(ii) 0.001 mol of strontium reacts with an excess of cold water. When the reaction is complete
a colourless solution is seen.

Construct the equation for the reaction of strontium with cold water. Include state symbols.

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

(iii) 0.005 mol of calcium and 0.005 mol of strontium are added separately to two beakers.
Each beaker contains 100 cm3 of cold water.
At the end of each reaction a white solid and a colourless solution are seen in both beakers.

Predict which element, calcium or strontium, produces the more alkaline solution. Explain
your answer.

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

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

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

(iv) Describe one observation when magnesium carbonate is added to excess dilute sulfuric
acid.

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

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

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(b) Element X is a metal. X reacts with oxygen to form a black solid oxide. The oxidation state of
X in this oxide is +2. The carbonate of X, XCO3, is a green solid. It decomposes on heating to
form the oxide and a colourless gas.

(i) From the information given, state two similarities and one difference that metal X and its
compounds have with Group 2 metals and their compounds.

similarity 1 ............................................................................................................................

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

similarity 2 ............................................................................................................................

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

difference 1 ..........................................................................................................................

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

(ii) Write the formula of the oxide of X.

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

(iii) Write an equation for the reaction of XCO3 when it is heated.

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

 [Total: 12]

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2 Magnesium silicide, Mg2Si, is a compound made by heating magnesium with sand.

(a) Draw a ‘dot-and-cross’ diagram to show the arrangement of outer electrons present in a formula
unit of Mg2Si. Assume magnesium silicide is an ionic compound.

[2]

(b) When solid Mg2Si is added to water, silane gas, SiH4, and a solution of magnesium hydroxide
are produced.

Construct the equation for this reaction. Include state symbols.

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

(c) Suggest, with reference to structure and bonding, why SiH4 is a gas at room temperature.

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

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

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

(d) The table shows the electronegativity values of carbon, hydrogen and silicon.

element carbon hydrogen silicon

electronegativity 2.5 2.1 1.8

(i) C–H and Si–H bonds have weak dipoles.

Use the electronegativity values in the table to show the polarity of the C–H and Si–H
bonds.

C––H Si––H
[2]

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(ii) Explain why methane, CH4, has no overall dipole moment.

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

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

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

(e) SiH4 reacts in air without heating but CH4 must be ignited before combustion occurs.

SiH4 + 2O2 SiO2 + 2H2O

CH4 + 2O2 CO2 + 2H2O

Suggest, with reference to bond energies from the Data Booklet, why SiH4 reacts in air without
heating but CH4 must be ignited.

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

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

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

(f) Silicon dioxide reacts with hot, concentrated sodium hydroxide.

(i) Identify the two products formed during this reaction.

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

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

(ii) Describe the behaviour of the silicon dioxide during this reaction.

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

 [Total: 15]

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3 (a) Construct an equation for the second ionisation energy of argon.

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

(b) The graph shows successive ionisation energies for the element argon.

Complete the graph with predictions for the eighth and ninth ionisation energies of argon.
Use a cross (×) for each data point. [2]

50 000

45 000

40 000

35 000

30 000
ionisation
energy 25 000
/ kJ mol–1
20 000

15 000

10 000

5000

0
1 2 3 4 5 6 7 8 9 10
number of electrons removed

(c) T
 he energy value required to remove the first electron from an atom of argon is circled on the
graph.

Sketch the shape of the orbital that contains this electron.

[1]

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(d) Chlorine exists as a diatomic gas, Cl 2(g). A sample of Cl 2(g) was made during a chemical
reaction. When measured at 404 kPa and 25 °C the sample occupied a volume of 20.0 cm3.

(i) Calculate the mass, in grams, of Cl 2(g) formed.

For this calculation, assume that chlorine behaves as an ideal gas under these conditions.

 mass of Cl 2(g) = .............................. g [3]

(ii) Calculate the number of chlorine atoms in this sample of Cl 2(g). You may find it helpful to
use your answer to (d)(i).

If you are unable to calculate an answer to (d)(i), use 0.36 g of Cl 2. This is not the correct
answer.

 number of chlorine atoms = .............................. [2]

(iii) Cl 2(g) does not behave as an ideal gas under these conditions.

Explain why Cl 2(g) behaves even less ideally at:

● very high pressures

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

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

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

● very low temperatures.

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

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

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

 [Total: 11]

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4 The structure of compound Y is shown.

Y
H H H
a b
Cl C C C

H H

(a) Give the systematic name for Y.

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

(b) Predict the values for the bond angles a and b shown in the diagram.

a ......................................

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

(c) When Y reacts with cold, dilute, acidified manganate(VII) ions, compound Z is produced.

Z
OH
Cl OH

(i) State the molecular formula of Z.

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

(ii) Name the type of reaction occurring when Y is converted into Z.

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

(iii) Alcohols can be classified as primary, secondary or tertiary.

Identify with a tick () the alcohol group(s) present in Z.

alcohol group
present in Z
primary
secondary
tertiary
[1]

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(d) Samples of organic compounds, A, B, C and D, are placed in unlabelled bottles.

A B C D
CH3CH2COCH3 CH3(CH2)2CHO CH3CH2OH CH3CO2H

(i) Identify all of the compound(s), A–D, that contain a carbonyl group.

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

(ii) 
A–D are reacted separately with the reagents given in the table.

Complete the table to:

● identify which of the compounds, A–D, reacts with the reagents
● give an appropriate observation when a reaction occurs.

reagent compounds identified observation when a reaction occurs

Tollens’ reagent

alkaline solution of iodine

sodium metal

[8]

 [Total: 15]

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5 Ethanal reacts with a mixture of HCN and NaCN to make 2-hydroxypropanenitrile, CH3CH(OH)CN.

The reaction mechanism is nucleophilic addition.

(a) Explain the meaning of the term nucleophile and identify the species which acts as the
nucleophile during this reaction.

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

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

species acting as nucleophile .....................................................................................................

[2]

(b) CH3CH(OH)CN exists as a pair of stereoisomers.

(i) Name the type of stereoisomerism shown by CH3CH(OH)CN.

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

(ii) Draw three-dimensional diagrams of this pair of stereoisomers.

Indicate with an asterisk (*) the chiral centre on one of the structures drawn.

[3]

(c) 
Give the structure of the organic product of the reaction of CH3CH(OH)CN with dilute
sulfuric acid.

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

 [Total: 7]

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