Cambridge International AS & A Level
*0464412317*
CHEMISTRY9701/22
Paper 2 AS Level Structured Questions
February/March 2020
1 hour 15 minutes
You must answer on the question paper.
You will need:
Data booklet
INSTRUCTIONS
●● Answer all questions.
●● Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●● Write your name, centre number and candidate number in the boxes at the top of the page.
●● Write your answer to each question in the space provided.
●● Do not use an erasable pen or correction fluid.
●● Do not write on any bar codes.
●● You may use a calculator.
●● You should show all your working, use appropriate units and use an appropriate number of significant
figures.
INFORMATION
●● The total mark for this paper is 60.
●● The number of marks for each question or part question is shown in brackets [ ].
This document has 16 pages. Blank pages are indicated.
IB20 03_9701_22/4RP
© UCLES 2020
[Turn over
2
Answer all the questions in the spaces provided.
1Group 2 metals form alkaline solutions in water.
(a) (i)Write the equation for the reaction of calcium oxide with water.
........................................................................................................................................ [1]
(ii)Identify the ion that causes an aqueous solution to be alkaline.
........................................................................................................................................ [1]
(b)The table shows the melting points of some Group 2 metal oxides.
compound
melting point / °C
MgO
2825
CaO
2613
SrO
2531
BaO
1923
Explain the trend in the melting points of the oxides down Group 2.
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [2]
(c)Oxygen reacts readily with some metals, but each Group 2 metal requires strong heating to
start the reaction with oxygen.
Suggest why strong heating is required to start these reactions.
.....................................................................................................................................................
............................................................................................................................................... [1]
(d)Beryllium oxide reacts with hydrochloric acid to form molecules of BeCl 2.
Deduce the bond angle in BeCl 2.
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(e)Unlike the other oxides of Group 2 metals, beryllium oxide is amphoteric.
(i)Give the meaning of the term amphoteric.
..............................................................................................................................................
........................................................................................................................................ [1]
(ii)Beryllium oxide and aluminium oxide have similar chemical properties.
The Be(OH)42– anion is a product of the reaction between beryllium oxide and excess
concentrated OH–(aq).
Construct an equation for this reaction.
........................................................................................................................................ [1]
(f)Magnesium oxide reacts reversibly with chlorine according to the following equation.
2MgO(s) + 2Cl 2(g)
2MgCl 2(s) + O2(g)
Under certain conditions, a dynamic equilibrium is established.
(i)State two features of a reaction that is in dynamic equilibrium.
1 ...........................................................................................................................................
2 ...........................................................................................................................................
[2]
(ii)The equilibrium constant, Kp, is given by the following expression.
Kp =
pO
2
2
pCl
2
At 1.00 × 105 Pa and 500 K, 70% of the initial amount of Cl 2(g) has reacted.
Calculate Kp and state its units.
Kp = ..............................
units = ..............................
[3]
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(g)Magnesium peroxide, MgO2, is made in the following reaction.
MgO(s) + H2O2(l)
MgO2(s) + H2O(l)
compound
enthalpy change of
formation, ∆Hf / kJ mol–1
MgO(s)
–602
H2O2(l)
–188
H2O(l)
–286
∆H = –96 kJ mol–1
(i)The peroxide ion is O22–.
Deduce the average oxidation number of oxygen in the peroxide ion.
........................................................................................................................................ [1]
(ii)
Define the term enthalpy change of formation.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(iii)Use the data given to calculate the enthalpy change of formation of MgO2(s).
© UCLES 2020
∆Hf MgO2(s) = .............................. kJ mol–1 [2]
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(iv)Magnesium peroxide decomposes slowly to form magnesium oxide and oxygen.
MgO2(s)
1
MgO(s) + 2 O2(g)
Use your answer to (g)(iii) and the data in the table to calculate the enthalpy change of
this reaction.
If you were unable to obtain an answer to (g)(iii), use the value ∆Hf = –550 kJ mol–1. This
is not the correct answer.
enthalpy change of reaction = .............................. kJ mol–1 [1]
[Total: 19]
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2The Group 17 elements, chlorine, bromine and iodine, are non-metals that show trends in their
physical and chemical properties.
(a)Describe the trend in the colour of the Group 17 elements down the group.
.....................................................................................................................................................
............................................................................................................................................... [1]
(b)The Group 17 elements can oxidise many metals to form halides.
(i)Describe the relative reactivity of the elements in Group 17 as oxidising agents.
..............................................................................................................................................
........................................................................................................................................ [1]
(ii)Chlorine reacts with hot tin metal to form tin(IV) chloride, SnCl 4.
SnCl 4 is a colourless liquid at room temperature that reacts vigorously with water to form
an acidic solution.
Suggest the type of structure and bonding shown by SnCl 4. Explain your answer.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(c) The Group 17 elements form soluble halides with sodium.
(i)Describe what is seen when dilute AgNO3(aq) is added to NaBr(aq) followed by aqueous
ammonia.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
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(ii)NaCl reacts with concentrated H2SO4 to form HCl and NaHSO4.
Explain the difference between the reactions of concentrated H2SO4 with NaCl and with
NaI. Your answer should refer to the role of the sulfuric acid in each reaction.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [3]
(d)The hydrogen halides are useful reagents in organic and inorganic reactions.
(i)Describe and explain the trend in the boiling points of the hydrogen halides, HCl, HBr and
HI.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(ii)Describe and explain the trend in the thermal stabilities of the hydrogen halides, HCl, HBr
and HI.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
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(e)Lucas’s reagent is a mixture of HCl and ZnCl 2. Primary, secondary and tertiary alcohols can
be distinguished by their reaction with Lucas’s reagent.
Alcohols react with the HCl in Lucas’s reagent to form halogenoalkanes.
ZnCl 2 acts as a homogeneous catalyst for these reactions.
(i)Explain the meaning of the term homogeneous.
..............................................................................................................................................
........................................................................................................................................ [1]
(ii)Pentan-3-ol, C2H5CH(OH)C2H5, reacts slowly with HCl to form a secondary halogenoalkane.
Complete the equation for this reaction using structural formulae.
C2H5CH(OH)C2H5 + ���������������������������������������������������������������������������������������������������� [1]
(iii)The fastest reaction shown by Lucas’s reagent is with a tertiary alcohol.
Draw the structure of the tertiary alcohol that is an isomer of pentan-3-ol.
[1]
(iv)Tertiary alcohols tend to react with Lucas’s reagent using the same mechanism as in their
reaction with HCl.
Suggest the type of reaction shown by tertiary alcohols with Lucas’s reagent.
........................................................................................................................................ [1]
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3Glycerol, CH2(OH)CH(OH)CH2OH, is widely used in the food industry and in pharmaceuticals.
(a)A series of reactions starting from glycerol is shown.
P
CH2OH
H
C
OH
Q
COOH
HOOC
reaction 1
CH2OH
O
C
HOOC
NaCN and HCN
reaction 2
NC
C
OH
COOH
(i)Suggest the reagent(s) and conditions for reaction 1.
..............................................................................................................................................
........................................................................................................................................ [2]
(ii)Name the reaction mechanism for reaction 2.
........................................................................................................................................ [1]
(iii)Give the observation you would make when 2,4-dinitrophenylhydrazine is added to P.
........................................................................................................................................ [1]
(iv)
Q does not show optical isomerism.
Explain why.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [1]
(v)When Q is heated with excess aqueous ethanoic acid in the presence of a catalytic amount
of sulfuric acid, two reactions take place to form compound R.
R
COOH
HOOC
C
OCOCH3
COOH
Identify the two types of reaction that occur.
1 ...........................................................................................................................................
2 ...........................................................................................................................................
[2]
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(b)Glycerol can be used as a starting material in the manufacture of nitroglycerine, C3H5N3O9.
Nitroglycerine decomposes rapidly on heating to form a mixture of gases.
4C3H5N3O9(l)
12CO2(g) + 10H2O(g) + 6N2(g) + O2(g)
A sample of nitroglycerine decomposes, releasing 1.06 dm3 of O2(g) at 850 K and 1.00 × 105 Pa.
(i)Calculate the mass of nitroglycerine that decomposes.
mass of nitroglycerine = .............................. g [3]
(ii)Calculate the total volume of gas released by this decomposition at 850 K and 1.00 × 105 Pa.
© UCLES 2020
total volume of gas = .............................. dm3 [1]
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(c)Fats are compounds made from glycerol and unsaturated carboxylic acids.
4-pentenoic acid is an example of an unsaturated carboxylic acid.
4-pentenoic acid
(CH2)2COOH
H
H
H
(i)Give the molecular formula of 4-pentenoic acid.
........................................................................................................................................ [1]
(ii)Draw the repeat unit of the addition polymer that can be formed from 4-pentenoic acid.
[1]
(iii)Unsaturated acids are often brominated before being added to soft drinks.
Complete the mechanism for the addition of Br2 to 4-pentenoic acid.
●●
●●
Include the structures of the intermediate and the product of the reaction.
Include all charges, partial charges, lone pairs and curly arrows.
In the mechanism, R has been used to represent (CH2)2COOH.
R
H
H
H
Br
Br
[4]
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(d)A reaction of another unsaturated carboxylic acid, T, is shown.
T
U
C6H13
HOOC
C6H13
HOOC
Br
Br
(i)
T is one of a pair of geometrical (cis-trans) isomers.
Draw the other geometrical isomer of T and explain why the molecules exhibit this form of
isomerism.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
[3]
(ii)Identify the reagent used to convert T to U.
........................................................................................................................................ [1]
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(iii)The C–Br bond has an absorption between 500 cm–1 and 600 cm–1 in an infrared spectrum.
The infrared spectra for both T and U have absorptions between 2850 cm–1 and 2950 cm–1.
These correspond to C–H bonds.
Identify:
●● two other absorptions that would be seen in the infrared spectra of both T and U
●● one other absorption that would only be seen in the infrared spectrum of T.
For each absorption, give the range of the absorption and the bonds that correspond to
these absorptions.
absorption 1 present in both spectra ...................................................................................
..............................................................................................................................................
..............................................................................................................................................
absorption 2 present in both spectra ...................................................................................
..............................................................................................................................................
..............................................................................................................................................
absorption only present in spectrum of T ............................................................................
..............................................................................................................................................
..............................................................................................................................................
[3]
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BLANK PAGE
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BLANK PAGE
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2020
9701/22/F/M/20
Cambridge International AS & A Level
*2460000734*
CHEMISTRY9701/22
Paper 2 AS Level Structured Questions
May/June 2020
1 hour 15 minutes
You must answer on the question paper.
You will need:
Data booklet
INSTRUCTIONS
●● Answer all questions.
●● Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●● Write your name, centre number and candidate number in the boxes at the top of the page.
●● Write your answer to each question in the space provided.
●● Do not use an erasable pen or correction fluid.
●● Do not write on any bar codes.
●● You may use a calculator.
●● You should show all your working, use appropriate units and use an appropriate number of significant
figures.
INFORMATION
●● The total mark for this paper is 60.
●● The number of marks for each question or part question is shown in brackets [ ].
This document has 12 pages. Blank pages are indicated.
IB20 06_9701_22/3RP
© UCLES 2020
[Turn over
2
Answer all the questions in the spaces provided.
1Gallium is an element in Group 13.
A sample of gallium is analysed using a mass spectrometer. The mass spectrum produced is
shown.
60.11%
39.89%
% relative
abundance
mass
69 71
(a)Explain what is meant by the term relative atomic mass.
.....................................................................................................................................................
............................................................................................................................................... [2]
(b) Calculate the relative atomic mass of gallium in this sample. Give your answer to 4 significant
figures.
Show your working.
relative atomic mass = .............................. [2]
(c)Complete the table which describes a gaseous atom of gallium.
isotope
71
nucleon
number
total number
of electrons in
lowest energy level
type of orbital which
contains the electron in
the highest energy level
Ga
[3]
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(d)When gallium is heated in excess chlorine, gallium trichloride, GaCl 3, is made.
Draw the shape of the gallium trichloride molecule and suggest the Cl –Ga–Cl bond angle.
shape of molecule
bond angle .................................................................
[2]
(e)Gallium oxide, Ga2O3, and aluminium oxide react in the same way with HCl (aq) and with
NaOH(aq).
(i)Suggest the equation for the reaction between Ga2O3 and HCl (aq).
........................................................................................................................................ [1]
(ii)Suggest an equation for the reaction between gallium oxide and NaOH(aq).
........................................................................................................................................ [2]
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2Nitric acid can be made in a 3-stage process.
Stage 1Ammonia is oxidised by oxygen from the air, to form nitrogen monoxide and water. This
reaction is carried out at 10–13 atmospheres pressure and 900 °C in the presence of a
platinum catalyst.
Stage 2Nitrogen monoxide reacts with more oxygen to form nitrogen dioxide.
2NO + O2
2NO2
∆H = –114 kJ mol–1
Stage 3Nitrogen dioxide reacts with water to make nitric acid and nitrogen monoxide.
3NO2 + H2O → 2HNO3 + NO
(a)Write an equation to show the reaction occurring in stage 1.
............................................................................................................................................... [1]
(b)Draw a ‘dot-and-cross’ diagram to show the arrangement of outer electrons in a molecule of
ammonia.
[1]
(c) (i)In the boxes, give the oxidation numbers of nitrogen in the nitrogen-containing species for
the reaction in stage 3.
3NO2 + H2O → 2HNO3 + NO
[2]
(ii)Explain why the reaction in stage 3 is described as a disproportionation reaction.
Include reference to transfer of electrons in your answer.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
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(d)The release of nitrogen monoxide into the atmosphere causes atmospheric pollution.
State and explain the effect of nitrogen monoxide gas in contact with moist air.
.....................................................................................................................................................
............................................................................................................................................... [2]
(e)The nitric acid made in stage 3 can then be reacted with ammonia to form ammonium nitrate.
Stage 3
3NO2 + H2O → 2HNO3 + NO
NH3 + HNO3 → NH4NO3
Calculate the volume of nitrogen dioxide, measured at room temperature and pressure,
required to make 40 tonnes of ammonium nitrate.
[1 tonne = 1000 kg]
Show your working.
volume of nitrogen dioxide = .............................. [3]
(f)State one use of ammonium nitrate.
............................................................................................................................................... [1]
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3Sucrose, C12H22O11, reacts with water to form glucose and fructose in reaction A.
C12H22O11 + H2O
glucose
fructose
O
H
O
HO
C
H
H
C
OH
H
C
OH
C
H
C
OH
HO
C
H
H
C
OH
H
C
OH
+
C
CH2OH
CH2OH
CH2OH
reaction A
(a)Suggest a name for this type of reaction.
............................................................................................................................................... [1]
(b)Explain in detail, why glucose and fructose are a pair of structural isomers. Your answer should
refer specifically to these two molecules.
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [2]
(c)Reaction A occurs faster in the presence of an enzyme. This is reaction B.
(i)The activation energy for reaction B is +29 kJ mol–1.
Predict a value for the activation energy of reaction A.
........................................................................................................................................ [1]
(ii)The enthalpy change for reaction A is –14 kJ mol–1.
Predict a value for the enthalpy change for reaction B.
........................................................................................................................................ [1]
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(iii)Sketch a labelled energy level diagram for reaction B. Use relevant values from (c)(i) and
(c)(ii).
energy
/ kJ mol–1
progress of reaction
[2]
(d)1.00 g of sucrose, C12H22O11, is completely combusted. The heat energy produced is used to
increase the temperature of 250 g of water inside a calorimeter from 25.0 °C to 40.7 °C.
These data can be used to calculate the enthalpy change of combustion of sucrose.
(i)Explain what is meant by the term enthalpy change of combustion of sucrose.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(ii)Use the Data Booklet to calculate the enthalpy change, in kJ mol–1, for the combustion of
sucrose.
Assume that all of the heat energy produced is transferred to the water.
Show your working.
enthalpy change of combustion of sucrose = .............................. kJ mol–1
[3]
© UCLES 2020
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4
(a)An unlabelled bottle contains a straight-chain halogenoalkane, Q. The molecular formula of Q
is C5H11X, where X is a halogen; bromine, chlorine or iodine.
A test is carried out to identify the halogen present in Q.
A sample of Q is added to NaOH(aq) and warmed. Dilute nitric acid is then added followed by
a few drops of aqueous silver nitrate. A cream precipitate is observed.
(i)Suggest the identity of X.
........................................................................................................................................ [1]
(ii)Write an ionic equation to describe the formation of the cream precipitate. Include state
symbols.
........................................................................................................................................ [1]
(iii)
Describe a further test which would confirm the identity of X.
test .......................................................................................................................................
expected result ....................................................................................................................
[2]
(b)The reaction of Q with NaOH(aq) tends to proceed via an SN2 mechanism.
(i)
Suggest the structural formula of the straight-chain halogenoalkane Q.
[1]
(ii)
Explain why the reaction tends to proceed via an SN2 mechanism rather than an SN1
mechanism.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
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(c)Two different halogenoalkanes, P and R, both with the molecular formula C4H9Cl, are separately
dissolved in ethanol and heated under reflux with sodium hydroxide.
The major organic product of each of these reactions is methylpropene.
(i)
Name the type of reaction occurring.
........................................................................................................................................ [1]
(ii)
Write an equation, using molecular formulae, to represent the reaction occurring.
........................................................................................................................................ [1]
(iii)Draw the skeletal formula of methylpropene.
[1]
(iv)Give the names of P and R.
........................................................................................................................................ [2]
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5The reaction sequence shows how ethene, C2H4, can be converted into other organic molecules.
C 2H 4
reaction 1
OH
reaction 5
reaction 2
Cl
reaction 6
NH2
O
reaction 3
HO
N
reaction 4
heat with dilute acid
W
(a)Complete the table to give
●● the name of the reaction mechanisms of reactions 1 and 6
●● the reagents and conditions required for reactions 1, 2 and 6.
reaction
name of reagents
and conditions
name of
mechanism
1
2
6
[6]
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(b)In reaction 3 the organic molecule reacts with HCN and a KCN catalyst.
(i)Complete the diagram to show the mechanism of the reaction occurring.
Include all relevant dipoles, lone pairs and curly arrows in your answer.
H
H
C
H 3C
O
C–
H3C
C
CN
H
–
O
H
H 3C
C
OH
CN
C
N
C–
N
N
[3]
(ii)Name the functional groups present in the product of reaction 3.
........................................................................................................................................ [2]
(c)
Draw the structure of the organic molecule W formed in reaction 4.
[1]
© UCLES 2020
[Total: 12]
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BLANK PAGE
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2020
9701/22/M/J/20
Cambridge International AS & A Level
*1309098231*
CHEMISTRY9701/22
Paper 2 AS Level Structured Questions
October/November 2020
1 hour 15 minutes
You must answer on the question paper.
You will need:
Data booklet
INSTRUCTIONS
●
Answer all questions.
●
Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●
Write your name, centre number and candidate number in the boxes at the top of the page.
●
Write your answer to each question in the space provided.
●
Do not use an erasable pen or correction fluid.
●
Do not write on any bar codes.
●
You may use a calculator.
●
You should show all your working, use appropriate units and use an appropriate number of significant
figures.
INFORMATION
●
The total mark for this paper is 60.
●
The number of marks for each question or part question is shown in brackets [ ].
This document has 16 pages. Blank pages are indicated.
IB20 11_9701_22/3RP
© UCLES 2020
[Turn over
2
Answer all the questions in the spaces provided.
1Atoms contain the subatomic particles electrons, protons and neutrons. Protons and electrons
were discovered by observations of their behaviours in electric fields.
(a)The diagram shows the behaviour of separate beams of electrons and protons in an electric
field.
protons
charge on plate
electrons
charge on plate
.........................
.........................
source
(i)Complete the diagram with the relative charge of each of the electrically charged plates.
[1]
(ii)On the diagram, draw a line to show how a separate beam of neutrons from the same
source behaves in the same electric field.
[1]
(b)Electrons in atoms up to 36Kr are distributed in s, p and d orbitals.
(i)State the number of occupied orbitals in an isolated atom of 36Kr.
type of orbital
s
p
d
number of orbitals
[3]
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(ii)Complete the diagram to show the number and relative energies of the electrons in an
isolated atom of 14Si.
4s
3p
3s
2p
2s
1s
[2]
(iii)The diagram shows a type of orbital.
State the total number of electrons that exist in all orbitals of this type in an atom of 9F.
........................................................................................................................................ [1]
(iv)The first ionisation energies of elements in the first row of the d block (21Sc to 29Cu) are
very similar. For all these elements, it is a 4s electron that is lost during the first ionisation.
Suggest why the first ionisation energies of these elements are very similar.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [3]
(c)
Hydron is a general term used to represent the ions 11H+, 12H+ and 13H+.
State, in terms of subatomic particles in the nucleus, what is the same about each of these ions
and what is different.
same ...........................................................................................................................................
different .......................................................................................................................................
[1]
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2The Period 3 elements, Na to S, all react with oxygen to form oxides.
(a)State the trend in acid/base behaviour of the oxides of the Period 3 elements, from Na to S.
.....................................................................................................................................................
............................................................................................................................................... [1]
(b)State and explain the trend, from Na to S, in the maximum oxidation number of the Period 3
elements in their oxides.
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [2]
(c)Sodium oxide and phosphorus(V) oxide both react with water.
Name the product of each reaction.
reaction
product
sodium oxide with water
phosphorus(V) oxide with water
[2]
(d)Explain why phosphorus(V) oxide has a low melting point of approximately 300 °C but
magnesium oxide has a high melting point of approximately 2850 °C.
.....................................................................................................................................................
.....................................................................................................................................................
.....................................................................................................................................................
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [3]
© UCLES 2020
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5
(e)Aluminium oxide, Al 2O3, reacts separately with both acids and alkalis.
(i)Write an equation for the reaction of aluminium oxide with excess aqueous hydrochloric acid.
........................................................................................................................................ [1]
(ii)
Write an equation for the reaction of aluminium oxide with excess aqueous sodium hydroxide.
........................................................................................................................................ [1]
(f)Describe the lattice structure of silicon(IV) oxide.
Your answer should include reference to the arrangement of the silicon and oxygen atoms and
the bonds between them.
.....................................................................................................................................................
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [2]
(g)Sodium oxide and silicon(IV) oxide react to form sodium silicate(IV), Na2SiO3.
Sodium oxide is obtained from the thermal decomposition of sodium carbonate.
Write equations for the following reactions:
(i)sodium oxide with silicon(IV) oxide
........................................................................................................................................ [1]
(ii)the thermal decomposition of sodium carbonate, forming sodium oxide and carbon dioxide.
........................................................................................................................................ [1]
© UCLES 2020
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6
3PCl 5, PCl 3 and NCl 3 are halides of Group 15 elements.
(a)PCl 5 can be formed from the reaction of phosphorus with chlorine. PCl 5 has a melting point of
161 °C.
(i)Write an equation for the formation of PCl 5 from the reaction of phosphorus and chlorine.
........................................................................................................................................ [1]
(ii)State the type of structure and bonding shown by liquid PCl 5.
........................................................................................................................................ [1]
(b)A small amount of PCl 5 is added to excess water. The PCl 5 reacts vigorously to form a
colourless solution.
(i)Give one other observation you would make when PCl 5 reacts with excess water.
........................................................................................................................................ [1]
(ii)Write the equation for the reaction of PCl 5 with excess water.
........................................................................................................................................ [1]
(iii)Estimate the pH of the resulting solution.
........................................................................................................................................ [1]
(c)PCl 3 is used to convert alcohols to chloroalkanes, such as compound T.
T
Cl
Cl
A possible synthesis of T is shown.
O
HO
reaction 1
OH
HO
using PCl 3
Cl
Cl
OH
(i)Identify a reagent that could be used in reaction 1.
........................................................................................................................................ [1]
© UCLES 2020
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7
(ii)
T exhibits optical isomerism.
Explain what is meant by the term optical isomer and circle any atom(s) in T that give rise
to optical isomerism.
T
Cl
Cl
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
[2]
(iii)
T is a minor product in the reaction of compound S with excess HCl.
S
Draw the structure of the major product of the reaction of S with excess HCl.
[1]
© UCLES 2020
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8
(d)NCl 3 is a yellow liquid that can be used to bleach flour.
(i)Predict the shape of the NCl 3 molecule and the Cl –N–Cl bond angle.
shape ...................................................................................................................................
bond angle ...........................................................................................................................
[2]
(ii)NCl 3 reacts with water to form HOCl, a weak Brønsted-Lowry acid.
Explain fully what is meant by the term weak Brønsted-Lowry acid.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(iii)NCl 3(l) decomposes according to the equation shown.
2NCl 3(l) → N2(g) + 3Cl 2(g)
A sealed container of volume 250 cm3 contains an unreactive gas at a pressure of
1.00 × 105 Pa.
0.241 g of NCl 3(l) was injected into the sealed container.
The sealed container was heated to make the NCl 3(l) decompose fully and then cooled to
20 °C.
Calculate the final total pressure inside the sealed container at 20 °C after the NCl 3(l) has
fully decomposed.
final total pressure = .............................. Pa
[4]
© UCLES 2020
[Total: 17]
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9
4
Some reactions of compound G are shown.
G
O
OH
H
reaction 1
HOOC(CH2)2COOH
reaction 2
O
reaction 3
Tollens’ reagent
OH
HO
H2SO4, heat
under reflux
reaction 4
Na
H
O
O
(a) (i)State the type of reaction that occurs in reaction 1.
........................................................................................................................................ [1]
(ii)Suggest the reagent(s) and conditions required for reaction 1.
..............................................................................................................................................
........................................................................................................................................ [2]
(iii)Draw the structure of the organic product, H, from reaction 2.
[1]
(iv)State what you would observe in reaction 3.
........................................................................................................................................ [1]
(v)Give the type of reaction shown by reaction 4.
........................................................................................................................................ [1]
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(b)
G and J are structural isomers of each other.
G
J
O
O
OH
H
OH
H
(i)Name the type of structural isomerism shown by G and J.
........................................................................................................................................ [1]
(ii)Suggest one chemical test that can distinguish G from J. Give the result of the test with
each compound.
test .......................................................................................................................................
result with G .........................................................................................................................
result with J .........................................................................................................................
[2]
In the reaction schemes below, G and J are converted into organic compound K.
J
G
NaBH4
NaBH4
HO(CH2)3CH2OH
Al 2O3
heat
K
Al 2O3
heat
HO(CH2)2CH(OH)CH3
(iii)State the role of NaBH4 in the reactions with G and J.
........................................................................................................................................ [1]
(iv)Identify the organic product K.
........................................................................................................................................ [1]
© UCLES 2020
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(c)
P and Q have the same molecular formula as G.
P
Q
O
O
HO
OH
Complete the table with the expected observations for the reactions of P and Q with the named
reagents.
reagent
result with P
result with Q
Br2(aq)
2,4-dinitrophenylhydrazine
aqueous sodium carbonate
[3]
© UCLES 2020
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12
(d)The structure of compound L is shown. R represents a hydrocarbon chain.
L
O
R
O
A student was asked to deduce the full structure of L.
The student analysed L using infrared spectroscopy. The following spectrum was obtained.
100
transmittance
%
50
X
0
4000
3000
2000
Y
Z
1500
1000
500
wavenumber / cm
–1
(i)Identify the bonds responsible for the absorptions marked X and Z.
X ..........................................................................................................................................
Z ..........................................................................................................................................
[1]
© UCLES 2020
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Absorption Y shows that L has a C=C bond present in the R group.
The student decided to treat L with hot concentrated acidified potassium manganate(VII). The
products of the reaction are shown.
O
L
O
O
hot concentrated
acidified KMnO4
R
O
OH
O
+
M
CH3(CH2)4COOH
(ii)Name M.
........................................................................................................................................ [1]
(iii)Use the information in (d) to deduce the molecular formula of L.
molecular formula of L = .............................. [1]
[Total: 17]
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BLANK PAGE
© UCLES 2020
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BLANK PAGE
© UCLES 2020
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BLANK PAGE
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2020
9701/22/O/N/20
Cambridge International AS & A Level
*9722650000*
CHEMISTRY9701/22
Paper 2 AS Level Structured Questions
February/March 2021
1 hour 15 minutes
You must answer on the question paper.
You will need:
Data booklet
INSTRUCTIONS
●
Answer all questions.
●
Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●
Write your name, centre number and candidate number in the boxes at the top of the page.
●
Write your answer to each question in the space provided.
●
Do not use an erasable pen or correction fluid.
●
Do not write on any bar codes.
●
You may use a calculator.
●
You should show all your working, use appropriate units and use an appropriate number of significant
figures.
INFORMATION
●
The total mark for this paper is 60.
●
The number of marks for each question or part question is shown in brackets [ ].
This document has 12 pages.
IB21 03_9701_22/2RP
© UCLES 2021
[Turn over
2
Answer all the questions in the spaces provided.
1
The rate of chemical reactions is affected by changes in temperature and pressure.
(a) (i)
raw a curve on the axes to show the Boltzmann distribution of energy of particles in a
D
sample of gaseous krypton atoms at a given temperature.
Label the curve T1 and label the axes.
[2]
(ii)
On the diagram in (a)(i), draw a second curve to show the distribution of energies of the
krypton atoms at a higher temperature.
Label the second curve T2.[1]
(b) The Boltzmann distribution assumes that the particles behave as an ideal gas.
(i)State two assumptions of the kinetic theory as applied to an ideal gas.
1 ...........................................................................................................................................
..............................................................................................................................................
2 ...........................................................................................................................................
..............................................................................................................................................
[2]
(ii)
2.00 g of krypton gas, Kr(g), is placed in a sealed 5.00 dm3 container at 120 °C.
alculate the pressure, in Pa, of Kr(g) in the container.
C
Assume Kr(g) behaves as an ideal gas.
Show your working.
© UCLES 2021
pressure = ........................................ Pa [3]
9701/22/F/M/21
3
(iii)
State and explain the conditions at which krypton behaves most like an ideal gas.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(c) K
rypton reacts with fluorine in the presence of ultraviolet light to make krypton difluoride,
KrF2(g).
Kr(g) + F2(g) → KrF2(g)
activation energy for the reaction, Ea = +385 kJ mol–1
enthalpy change of formation of KrF2, ∆Hf = +60.2 kJ mol–1
(i)
Use this information to complete the reaction profile diagram for the formation of KrF2.
Label Ea and ∆Hf on the diagram.
Assume the reaction proceeds in one step.
energy
/ kJ mol–1
reactants
progress of reaction
[2]
(ii)
xplain, in terms of activation energy, Ea, and the collision of particles, how an increase in
E
temperature affects the rate of a chemical reaction.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
© UCLES 2021
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2Chlorine, Cl 2, is a reactive yellow-green gas. It is a strong oxidising agent.
(a)State how Cl 2 is used in water purification.
.....................................................................................................................................................
............................................................................................................................................... [1]
(b) Chlorine has the highest first ionisation energy of the Period 3 elements Na to Cl.
(i)
Construct an equation for the first ionisation energy of chlorine.
Include state symbols.
........................................................................................................................................ [1]
(ii)
Explain the general increase in the first ionisation energies of the Period 3 elements.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
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5
(c)The halide ions, X– (where X = Cl, Br, I), show clear trends in their physical and chemical
properties.
(i)
State and explain the relative thermal stabilities of the hydrogen halides, HX.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
The halide ions react easily with concentrated H2SO4.
The main sulfur-containing product of each reaction is shown in the table.
halide ion
Cl –
Br –
I–
main sulfur-containing product of
reaction with concentrated H2SO4
HSO4–
SO2
H 2S
oxidation number of sulfur
(ii)
omplete the table to show the oxidation number of sulfur in each of the sulfur-containing
C
products.[1]
(iii)
Explain why different sulfur-containing products are produced when each of these halide
ions reacts with concentrated H2SO4.
..............................................................................................................................................
........................................................................................................................................ [1]
(d)Cl 2 reacts with aqueous sodium hydroxide in a disproportionation reaction.
(i)
State what is meant by disproportionation.
..............................................................................................................................................
........................................................................................................................................ [1]
(ii)Write an equation for the reaction of Cl 2 with cold aqueous sodium hydroxide.
........................................................................................................................................ [1]
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6
(e)Aluminium reacts with chlorine to form aluminium chloride.
luminium chloride can exist as the gaseous molecule Al 2Cl 6(g). This molecule contains
A
coordinate bonds.
(i)
Draw a diagram that clearly shows all the types of bond present in Al 2Cl 6(g).
[2]
(ii)
Describe what you would see when solid aluminium chloride reacts with water.
Name the type of reaction that occurs.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(f)0.020 mol of element Z reacts with excess Cl 2 to form 0.020 mol of a liquid chloride.
The liquid chloride has formula ZCl n, where n is an integer.
ZCl n reacts vigorously with water at room temperature to give an acidic solution and a white
solid.
When excess AgNO3(aq) is added to the solution, 11.54 g of AgCl (s) forms.
(i)
Suggest the type of bonding and structure shown by ZCl n.
........................................................................................................................................ [1]
(ii)Calculate the value of n in ZCl n.
© UCLES 2021
n = .............................. [2]
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7
(g) Dichloromethane, CH2Cl 2, is widely used as an organic solvent.
CH2Cl 2 can be prepared by reacting CH3Cl and Cl 2 at room temperature.
The reaction proceeds via several steps, as shown.
Cl 2
Cl • + CH3Cl
Cl 2 + •CH2Cl
Cl • + •CH2Cl
initiation
propagation 1
propagation 2
final step
2Cl •
HCl + •CH2Cl
products
CH2Cl 2
(i)Give the name of the mechanism of this reaction.
........................................................................................................................................ [1]
(ii)
State the essential condition required for the initiation step to take place.
........................................................................................................................................ [1]
(iii)
Give the electronic configuration of Cl •.
1s2 .................................................................................................................................. [1]
(iv)
Identify the products of the step labelled propagation 2.
........................................................................................................................................ [1]
(v)
Name the type of reaction shown in the final step.
........................................................................................................................................ [1]
(vi)
uggest the identity of another organic molecule that is a product of the reaction of CH3Cl
S
and Cl 2 under the same conditions.
........................................................................................................................................ [1]
© UCLES 2021
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8
3Compounds P, Q and R have all been found in the atmosphere of one of Saturn’s moons.
P
Q
R
H
N
C
C
C
C
N
H
C
C
C
H
C
N
C
H
C
N
(a) The equation for the complete combustion of P, C4N2(l), is shown.
C4N2(l) + 4O2(g) → 4CO2(g) + N2(g)
(i)
∆H = –2036 kJ mol–1
The enthalpy change of formation, ∆Hf, of CO2(g) is –384 kJ mol–1.
Calculate the enthalpy change of formation, ∆Hf, of P, in kJ mol–1.
∆Hf of P = ............................. kJ mol–1 [2]
(ii)
One of the products of the complete combustion of P is nitrogen gas, N2(g).
Explain the lack of reactivity of nitrogen.
........................................................................................................................................ [1]
© UCLES 2021
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9
(b)
Q forms when HCN reacts with ethyne, H
(i)
C
C
H.
Ethyne, HCN and Q are all weak Brønsted–Lowry acids.
Explain what is meant by the term weak Brønsted–Lowry acid.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(ii)
Ethyne, HCN and Q all contain triple bonds between two atoms.
A triple bond consists of one sigma (σ) and two pi (π) bonds.
Draw a labelled diagram to show the formation of one pi (π) bond.
[2]
(c)
P and Q can be detected in the atmosphere by infrared spectroscopy.
Identify two absorptions, and the bonds that correspond to these absorptions, that will appear
in the infrared spectra of both P and Q.
1 ..................................................................................................................................................
.....................................................................................................................................................
2 ..................................................................................................................................................
.....................................................................................................................................................
[2]
© UCLES 2021
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10
(d) The flow chart shows some reactions of R.
R
H
H
C
C
reaction 1
C
H
H
H
C
C
H
C
N
reaction 3
dilute H2SO4(aq)
heat under reflux
reaction 2
S
N
H2(g)
T
CH3CH2CH2NH2
(i)
Name the type of reaction shown in reaction 1.
........................................................................................................................................ [1]
(ii)Draw the structure of S, the organic product of reaction 2.
[1]
(iii)
Name T.
........................................................................................................................................ [1]
(iv)
T can also be formed by the reaction of CH3CH2CH2Br with ammonia.
State the necessary conditions of this reaction.
........................................................................................................................................ [1]
© UCLES 2021
[Total: 13]
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11
4
Hydroxyethanal, HOCH2CHO, has been observed in dust clouds near the centre of our galaxy.
hydroxyethanal
H
HO
C
O
C
H
H
(a) Predict the bond angles labelled x and y in the diagram of hydroxyethanal.
HO
x
H
O
C
C y
H
H
x = ..............................°
y = ..............................°
[2]
(b) Hydroxyethanal reacts separately with 2,4-dinitrophenylhydrazine (2,4-DNPH) and with Tollens’
reagent.
State what you would observe in each reaction.
reaction with 2,4-DNPH ..............................................................................................................
reaction with Tollens’ reagent .....................................................................................................
[2]
(c) H
ydroxyethanal is converted to ethanedioic acid, (CO2H)2, when it reacts with excess acidified
dichromate(VI) ions, Cr2O72–.
(i)
State the role of acidified Cr2O72– in this reaction.
........................................................................................................................................ [1]
(ii)
State and explain any other necessary conditions for this reaction to be successful.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
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(d) Hydroxyethanal can be reduced to ethane-1,2-diol, (CH2OH)2, as shown.
hydroxyethanal
H
HO
C
H
(i)
O
C
ethane-1,2-diol
[H]
HO
H
H
H
C
C
H
H
OH
Write an equation for the reduction of hydroxyethanal to (CH2OH)2.
Use [H] to represent an atom of hydrogen from the reducing agent.
........................................................................................................................................ [1]
(ii)
Identify a reagent for this reduction reaction.
........................................................................................................................................ [1]
(iii)
(CH2OH)2 also forms when an alkene A reacts with cold, dilute, acidified manganate(VII)
ions.
Name A.
........................................................................................................................................ [1]
[Total: 10]
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
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2021
9701/22/F/M/21
Cambridge International AS & A Level
*6703041968*
CHEMISTRY9701/22
Paper 2 AS Level Structured Questions
May/June 2021
1 hour 15 minutes
You must answer on the question paper.
You will need:
Data booklet
INSTRUCTIONS
●
Answer all questions.
●
Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●
Write your name, centre number and candidate number in the boxes at the top of the page.
●
Write your answer to each question in the space provided.
●
Do not use an erasable pen or correction fluid.
●
Do not write on any bar codes.
●
You may use a calculator.
●
You should show all your working, use appropriate units and use an appropriate number of significant
figures.
INFORMATION
●
The total mark for this paper is 60.
●
The number of marks for each question or part question is shown in brackets [ ].
This document has 12 pages. Any blank pages are indicated.
IB21 06_9701_22/4RP
© UCLES 2021
[Turn over
2
Answer all the questions in the spaces provided.
1A Group 2 metal combines with bromine to form a crystalline solid, MBr2.
Excess aqueous AgNO3 is added to a solution of MBr2 and a precipitate forms. The mixture is
filtered. The precipitate is dried and the mass of the precipitate is recorded.
(a)State the formula and colour of the precipitate.
............................................................................................................................................... [2]
(b)Complete the equation to represent the reaction between MBr2 and AgNO3.
......MBr2 + ......AgNO3 → ...................................................................
[1]
(c)A 0.250 g sample of pure MBr2 contains 8.415 × 10–4 mol MBr2.
Calculate the relative formula mass, Mr, of MBr2. Use this to identify M.
Show your working.
Mr = ..............................
M = ..............................
[3]
(d)A sample of MBr2 is dissolved in water. Chlorine gas is then bubbled into the solution.
(i)Describe the observations for this reaction.
..............................................................................................................................................
........................................................................................................................................ [1]
(ii)Name the type of reaction that occurs when MBr2 reacts with chlorine gas.
........................................................................................................................................ [1]
© UCLES 2021
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3
(e)Compound Y is a pure insoluble solid which contains halide ions.
A single reagent is added directly to compound Y to determine the halide ion present.
Identify the reagent added. State the observation which would confirm that Y contains bromide
ions.
reagent .......................................................................................................................................
observation .................................................................................................................................
[2]
(f)Separate 1.0 g samples of three different magnesium salts are tested in order to identify the
anion present in each sample.
(i)Explain how the action of heat is used to identify which sample is:
●
●
●
MgCO3
Mg(NO3)2
MgO.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [3]
(ii)Complete the electron configuration of the magnesium cation present in these salts.
1s2 .................................................................................................................................. [1]
(g)A sample of MgCO3(s) is distinguished from a sample of Mg(OH)2(s) by adding a small amount
of each solid to HCl (aq).
State one similarity and one difference in these two reactions.
similarity ......................................................................................................................................
.....................................................................................................................................................
difference ....................................................................................................................................
.....................................................................................................................................................
[2]
© UCLES 2021
[Total: 16]
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4
2The strength of interaction between particles determines whether the substance is a solid, liquid or
gas at room temperature.
(a)Lithium sulfide, Li2S, is a crystalline solid with a melting point of 938 °C. It conducts electricity
when it is molten.
(i)Give the formulae of the particles present in solid lithium sulfide.
........................................................................................................................................ [1]
(ii)Explain, in terms of the structure of the crystalline solid, why lithium sulfide has a high
melting point.
..............................................................................................................................................
........................................................................................................................................ [2]
(b)Carbon monoxide, CO, is a gas at room temperature and pressure. It contains a coordinate
bond.
(i)Explain what is meant by coordinate bond.
..............................................................................................................................................
........................................................................................................................................ [1]
(ii)Draw a ‘dot-and-cross’ diagram to show the arrangement of outer electrons in CO.
Show the electrons belonging to the C atom as ×.
Show the electrons belonging to the O atom as ●.
[2]
© UCLES 2021
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5
(c)Nitrogen, N2, is also a gas at room temperature and pressure. Neither CO nor N2 is an ideal
gas.
(i)State two assumptions that are made about the behaviour of particles in an ideal gas.
1 ...........................................................................................................................................
..............................................................................................................................................
2 ...........................................................................................................................................
..............................................................................................................................................
[2]
(ii)Explain why N2 does not behave as an ideal gas at very high pressures.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(iii)Complete the table by naming all the types of intermolecular forces (van der Waals’) in
separate samples of N2(g) and CO(g).
N2(g)
CO(g)
number of electrons per molecule
14
14
presence of a dipole moment


–195.8
–191.5
boiling point / °C
intermolecular forces (van der Waals’)
[2]
(iv)Suggest why the bond in a molecule of CO contains a dipole moment.
........................................................................................................................................ [1]
© UCLES 2021
[Total: 13]
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6
3A large excess of 2-bromo-2-methylpropane is added to 0.0010 mol of NaOH(aq), which contains
a few drops of phenolphthalein indicator. A stopwatch is started as soon as the substances are
mixed. The time taken for the pink colour to disappear is recorded.
The experiment is repeated at different temperatures, keeping all concentrations and volumes of
reagents constant.
temperature
/ °C
time taken for
pink colour to disappear / s
20
300
25
65
35
20
(a)Explain what is meant by the term rate of reaction.
.....................................................................................................................................................
............................................................................................................................................... [1]
(b)The graph shows the energy distribution of molecules in a sample of 2‑bromo‑2‑methylpropane
at 25 °C.
Ea represents the activation energy for the reaction.
proportion
of molecules
with a given
energy
0
0
Ea
molecular energy
(i)Label the graph to show the proportion of 2‑bromo‑2‑methylpropane molecules which
have sufficient energy to react.
[1]
(ii)Use the same axes to sketch the distribution of energies of molecules in a sample of
2‑bromo‑2‑methylpropane at 50 °C.[2]
(iii)State the effect of an increase in temperature on Ea for this reaction.
........................................................................................................................................ [1]
© UCLES 2021
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7
(c) (i)Draw the mechanism to show the reaction of 2‑bromo‑2‑methylpropane with OH–(aq).
Show the intermediate formed in this reaction.
Include all charges, partial charges, lone pairs and curly arrows as appropriate.
CH3
Br
C
H 3C
CH3
[3]
(ii)Name the mechanism for this reaction.
........................................................................................................................................ [1]
(d)
The original experiment is repeated at 25 °C with 2‑chloro‑2‑methylpropane instead of
2‑bromo‑2‑methylpropane. All other variables remain constant.
Predict the effect of using 2‑chloro‑2‑methylpropane compared to 2‑bromo‑2‑methylpropane
on the time taken for the pink colour to disappear. Explain your answer.
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [2]
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8
4
(a)
The table shows the structural formulae of four compounds, A, B, C and D, with molecular
formula C4H8.
(i)Complete the table by giving the systematic name of A, B, C and D.
structural formula
A
name
CH3CH2CH=CH2
H
H
C
B
C
H3C
CH3
H3C
H
C
C
H
C
CH3
D
CH2=C(CH3)2
[4]
(ii)Explain what is meant by stereoisomerism.
..............................................................................................................................................
........................................................................................................................................ [1]
(b)
W is an alkene with formula C4H8. It reacts with HBr to form two possible carbocations,
CH3C+(H)(CH2CH3) and H2C+CH2CH2CH3.
(i)Identify W as compound A, B, C or D.
........................................................................................................................................ [1]
© UCLES 2021
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9
(ii)Draw the skeletal formula of the major organic product formed when HBr reacts with W.
Explain why this is the major organic product.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
[3]
(c)A sample of propan‑1‑ol reacts with concentrated sulfuric acid to form propene.
Identify the role of concentrated sulfuric acid in this reaction.
............................................................................................................................................... [1]
(d)Alcohol Y reacts completely when warmed with acidified Cr2O72– to form Z.
Z is distilled from the reaction mixture as soon as it is made.
Tollens’ reagent is added to a sample of Z and warmed. A silver mirror forms.
(i)Name the type of reaction that occurs when Y reacts to form Z.
........................................................................................................................................ [1]
(ii)Identify with a tick () the functional group(s) present in Z.
functional group
present in Z
aldehyde
ketone
carboxylic acid
[1]
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10
5
S is a secondary alcohol with molecular formula C4H10O.
(a)Draw the displayed formula of S.
[1]
(b)
S is converted to V in a three‑step reaction sequence.
S
step 1
T
C4H10O
PBr3
C4H9Br
U
step 3
C4H9CN
dilute
acid
step 2
V
In step 1, the secondary alcohol S reacts with PBr3 to produce T, which has molecular formula
C4H9Br.
(i)Give the systematic name of T.
........................................................................................................................................ [1]
(ii)Name the type of reaction that occurs in step 1.
........................................................................................................................................ [1]
(iii)State the reagent(s) and conditions for step 2.
..............................................................................................................................................
........................................................................................................................................ [2]
(iv)Step 3 involves heating C4H9CN with dilute acid to form V.
Complete the equation for this reaction.
.....C4H9CN + .....H+ + .....H2O → ........................................
© UCLES 2021
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[2]
11
(v)An unlabelled sample contains either S, T or U.
The sample produces the infrared spectrum shown.
100
transmittance
/%
50
0
4000
3000
2000
1500
1000
500
wavenumber / cm
–1
Explain how this spectrum confirms that the unknown sample contains U.
In your answer identify one relevant absorption in the infrared spectrum and the bond that
corresponds to this absorption in the region above 1500 cm–1.
..............................................................................................................................................
........................................................................................................................................ [1]
© UCLES 2021
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BLANK PAGE
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2021
9701/22/M/J/21
Cambridge International AS & A Level
*2578092005*
CHEMISTRY9701/22
Paper 2 AS Level Structured Questions
October/November 2021
1 hour 15 minutes
You must answer on the question paper.
You will need:
Data booklet
INSTRUCTIONS
●
Answer all questions.
●
Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●
Write your name, centre number and candidate number in the boxes at the top of the page.
●
Write your answer to each question in the space provided.
●
Do not use an erasable pen or correction fluid.
●
Do not write on any bar codes.
●
You may use a calculator.
●
You should show all your working, use appropriate units and use an appropriate number of significant
figures.
INFORMATION
●
The total mark for this paper is 60.
●
The number of marks for each question or part question is shown in brackets [ ].
This document has 12 pages.
IB21 11_9701_22/4RP
© UCLES 2021
[Turn over
2
Answer all the questions in the spaces provided.
1Hydrogen iodide, HI, is a colourless gas at room temperature.
(a) (i)Explain why HI has a higher boiling point than HCl and HBr.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(ii)The bar chart shows the boiling points of HCl, HBr and HI. The boiling point of HF is not
shown.
300
280
260
boiling 240
point / K 220
200
180
160
HF
HCl
HBr
HI
Hydrogen bonds form between HF molecules.
Draw a bar on the bar chart to predict the boiling point of HF.
Explain your answer.
..............................................................................................................................................
........................................................................................................................................ [2]
(b)The standard enthalpy change of formation,
, of HI(g) is +26.5 kJ mol–1.
Define the term standard enthalpy change of formation.
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [2]
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(c)HI(g) can be formed by reacting H2(g) with I2(g). The reaction is reversible, and an equilibrium
forms quickly at high temperatures.
H2(g) + I2(g)
2HI(g)
(i)Construct an expression for the equilibrium constant, Kp, for the reaction of H2(g) and I2(g)
to form HI(g).
Kp =
[1]
(ii)The equilibrium partial pressures of the gases at 200 °C are as follows.
pH2(g) = 895 Pa
pI2(g) = 895 Pa
pHI(g) = 4800 Pa
Calculate Kp for this reaction.
Kp = .............................. [1]
(iii)State how the value of Kp would change, if at all, if the reaction were carried out at 100 °C
rather than 200 °C.
Explain your answer.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
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(d)HI reacts with oxygen to form iodine and water.
(i)Construct an equation for the reaction of HI with oxygen.
........................................................................................................................................ [1]
(ii)Explain, with reference to oxidation numbers, why this reaction is a redox reaction.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(e)HI(g) can also be formed by the reaction of I2(g) with hydrazine, N2H4(g).
2I2(g) + N2H4(g) → 4HI(g) + N2(g)
State the change in pressure that would occur when 2 mol I2(g) fully reacts with 1 mol N2H4(g)
in a sealed container at constant temperature. Explain your answer.
.....................................................................................................................................................
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [2]
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(f)In the laboratory, HI(aq) can be formed in a two-step process.
step 1
3I2(s) + 2P(s) → 2PI3(s)
step 2
PI3(s) + 3H2O(l) → H3PO3(aq) + 3HI(aq)
(i)Draw a ‘dot-and-cross’ diagram of a PI3 molecule.
[2]
(ii)Name the type of reaction in step 2.
........................................................................................................................................ [1]
(iii)H3PO3(aq) and HI(aq) are both strong Brønsted–Lowry acids.
Give the meaning of the term strong Brønsted–Lowry acid.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(iv)Give the formula of the conjugate base of H3PO3.
........................................................................................................................................ [1]
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6
(g)HI(g) reacts with propene, CH3CH=CH2(g) to form a mixture of 1-iodopropane and
2-iodopropane.
(i)Identify which of 1-iodopropane and 2-iodopropane is the major product of this reaction.
Explain your answer.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(ii)Complete the diagram to show the mechanism of the reaction between HI and CH3CH=CH2
that forms the major product identified in (g)(i).
Include curly arrows, lone pairs of electrons and charges as necessary.
H 3C
H
C
C
H
H
H
+
I
–
[3]
© UCLES 2021
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7
2
(a)Table 1 gives physical data for some of the Period 3 elements.
Table 1
atomic number, Z
11
bonding present in element
M
first ionisation energy / kJ mol–1
494
12
13
14
15
16
C
736
577
786
1060
1000
maximum oxidation number
anionic radius / nm
17
1260
+7
–
–
–
0.271
0.212
0.184
0.181
(i)Complete the row in the table labelled ‘bonding present in element’.
Use C = covalent, I = ionic, M = metallic, as appropriate.
(ii)
[1]
xplain the difference between the first ionisation energies of the elements with atomic
E
numbers 11 and 17.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(iii)
xplain the difference between the first ionisation energies of the elements with atomic
E
numbers 15 and 16.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(iv)Complete the row in the table labelled ‘maximum oxidation number’.
[1]
(v)Explain the variation in anionic radius for the elements with atomic numbers 14 to 17.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
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(b)Use the axes to sketch a graph that shows the trend in melting points of the elements with
atomic numbers 11 to 17.
melting point
of element
11
12
13
14
15
16
17
atomic number, Z
[2]
(c) Dmitri Mendeleev published the first Periodic Table in 1869.
Mendeleev used his knowledge of chemical periodicity to propose the properties of gallium,
31Ga, a Group 13 element.
Table 2 gives some chemical and physical data of elements in Group 13.
Table 2
element
density
/ g cm–3
boiling point
/K
cationic radius
/ nm
B
2.34
3930
0.020
2470
0.050
5
13
31
Al
Ga
5.91
In
7.30
Tl
11.8
49
81
2400
0.081
1460
Complete the table by predicting values for the missing data.
© UCLES 2021
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0.095
[3]
9
(d)Indium and aluminium are elements in Group 13 of the Periodic Table.
Indium has very similar chemical properties to aluminium.
●
●
●
Indium reacts vigorously with hydrochloric acid to form a colourless gas and a salt in
solution.
Indium oxide, In2O3, is amphoteric.
Gaseous indium bromide has the formula In2Br6. This molecule contains coordinate bonds.
(i)Identify the formula of the salt formed when indium reacts with hydrochloric acid.
........................................................................................................................................ [1]
(ii)Construct an equation for the reaction of In2O3 with excess aqueous NaOH.
........................................................................................................................................ [1]
(iii)Draw a diagram that clearly shows the types of bond present in In2Br6(g).
[2]
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10
3Compound T is an isomer of C6H12.
T
(a)Name T.
............................................................................................................................................... [1]
(b)
Draw the skeletal formula of a structural isomer of T that shows cis-trans (geometrical)
isomerism.
[1]
(c)Each carbon atom in T forms a sigma (σ) bond to at least one other carbon atom, as shown.
H 3C
C
H3C
C
CH3
CH3
(i)On the diagram, draw the orbitals that represent the pi (π) bond that is also present in T.
[1]
(ii)State the hybridisation of the two carbon atoms between which the pi (π) bond forms.
........................................................................................................................................ [1]
(d)A reaction scheme starting with T is shown. Reaction 2 occurs in the presence of a catalyst;
knowledge of the mechanism for this reaction is not required.
T
U
reaction 1
HO
V
OH
reaction 2
catalyst
O
(i)Give the reagent(s) and conditions for reaction 1.
........................................................................................................................................ [1]
© UCLES 2021
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11
(ii)State and explain how 2,4-dinitrophenylhydrazine (2,4-DNPH) can be used to detect the
presence of V as a product of reaction 2.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(iii)The progress of reaction 2 can be monitored by infrared spectroscopy.
The absorption caused by O–H bonds is always present because water is used as a
solvent.
Identify two absorptions, and the bonds responsible for these absorptions, whose
appearance will change significantly during the reaction.
1 ...........................................................................................................................................
..............................................................................................................................................
2 ...........................................................................................................................................
..............................................................................................................................................
[2]
(e)
V is used in a wide range of organic reactions.
Some reactions of V are shown.
W
V
O
reaction 3
O
alkaline
aqueous I2
O–
reaction 4 NaBH4
X
Y
OH
reaction 5
reaction 6
dehydration
addition
polymerisation
Z
(i)
V and W are colourless and soluble in water.
State what you would observe in reaction 3.
........................................................................................................................................ [1]
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12
(ii)Reaction 3 is a redox reaction.
Identify which of the reactants is reduced in this reaction.
........................................................................................................................................ [1]
(iii)Construct an equation for reaction 4.
Use [H] in the equation to represent an atom of hydrogen from NaBH4.
C6H12O + ��������������������������������������������������������������������������������������������������������������������� [1]
(iv)
X is a mixture of two optical isomers.
Draw the two optical isomers in the boxes provided.
[2]
(v)Both optical isomers of X can be dehydrated to form a single product, Y.
Give the reagent(s) and conditions required for reaction 5.
........................................................................................................................................ [1]
(vi)
Y can form an addition polymer Z.
Draw one repeat unit of Z.
[1]
(vii)Reaction 6 does not proceed quickly at room temperature.
Suggest why this is the case.
..............................................................................................................................................
........................................................................................................................................ [1]
[Total: 17]
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
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2021
9701/22/O/N/21
Cambridge International AS & A Level
*8748629381*
CHEMISTRY9701/22
Paper 2 AS Level Structured Questions
February/March 2022
1 hour 15 minutes
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●
Answer all questions.
●
Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●
Write your name, centre number and candidate number in the boxes at the top of the page.
●
Write your answer to each question in the space provided.
●
Do not use an erasable pen or correction fluid.
●
Do not write on any bar codes.
●
You may use a calculator.
●
You should show all your working and use appropriate units.
INFORMATION
●
The total mark for this paper is 60.
●
The number of marks for each question or part question is shown in brackets [ ].
●
The Periodic Table is printed in the question paper.
●
Important values, constants and standards are printed in the question paper.
This document has 16 pages.
IB22 03_9701_22/4RP
© UCLES 2022
[Turn over
2
Answer all the questions in the spaces provided.
1Fig. 1.1 shows how first ionisation energies vary across Period 2.
A
ionisation
energy
Li
Be
B
C
N
element
O
F
Ne
Fig. 1.1
(a)Construct an equation to represent the first ionisation energy of oxygen.
Include state symbols.
............................................................................................................................................... [1]
(b) (i)
State and explain the general trend in first ionisation energies across Period 2.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [3]
(ii)Explain why ionisation energy A in Fig. 1.1 does not follow the general trend in first
ionisation energies across Period 2.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
© UCLES 2022
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3
(c)Element E is in Period 3 of the Periodic Table.
The first eight ionisation energy values of E are shown in Table 1.1.
Table 1.1
ionisation
1st
2nd
3rd
4th
5th
6th
7th
8th
ionisation energy / kJ mol–1
577
1820
2740
11 600
14 800
18 400
23 400
27 500
Deduce the full electronic configuration of E.
Explain your answer.
full electronic configuration of E = ..............................................................................................
explanation .................................................................................................................................
.....................................................................................................................................................
.....................................................................................................................................................
[3]
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2Some oxides of elements in Period 3 are shown.
Na2O
Al 2O3
P4O6
P4O10
SO2
SO3
(a)Na reacts with O2 to form Na2O. Na is the reducing agent in this reaction.
(i)
Define reducing agent.
..............................................................................................................................................
........................................................................................................................................ [1]
(ii)Write an equation for the reaction of Na2O with water.
........................................................................................................................................ [1]
(b)Al 2O3 is an amphoteric oxide found in bauxite.
(i)State what is meant by amphoteric.
..............................................................................................................................................
........................................................................................................................................ [1]
(ii)Al 2O3 is purified from bauxite in several steps. The first step involves heating Al 2O3 with
an excess of NaOH(aq). A colourless solution forms.
Write an equation for this reaction.
........................................................................................................................................ [1]
© UCLES 2022
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5
(iii)Al 2O3 is used as a catalyst in the dehydration of alcohols.
tate the effect of using Al 2O3 as a catalyst in the dehydration of alcohols. Use the
S
Boltzmann distribution in Fig. 2.1 to help explain your answer.
number of
molecules
energy
Fig. 2.1
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [3]
(c)P4O6 is a white solid that has a melting point of 24 °C. Solid P4O6 reacts with water to form
H3PO3.
(i)Deduce the type of structure and bonding shown by P4O6. Explain your answer.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(ii)Determine the oxidation number of P in H3PO3.
........................................................................................................................................ [1]
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6
(iii)When P4O6(s) is heated with oxygen it forms P4O10(s).
P4O6(s) + 2O2(g) → P4O10(s)
∆Hr = –1372 kJ mol–1
The enthalpy change of formation, ∆Hf, of P4O10(s) is –3012 kJ mol–1.
Calculate the enthalpy change of formation, ∆Hf, of P4O6(s).
∆Hf of P4O6(s) = .............................. kJ mol–1 [1]
(iv)Write an equation for the reaction of P4O10 with water.
........................................................................................................................................ [1]
(d)SO2 and SO3 are found in the atmosphere.
The oxidation of SO2 to SO3 in the atmosphere is catalysed by NO2.
The first step of the catalytic oxidation is shown in equation 1.
equation 1
SO2(g) + NO2(g)
SO3(g) + NO(g)
(i)Construct an equation to show how NO2 is regenerated in the catalytic oxidation of SO2.
........................................................................................................................................ [1]
(ii)NO2 can also react with unburned hydrocarbons to form photochemical smog.
State the product of this reaction that contributes to photochemical smog.
........................................................................................................................................ [1]
© UCLES 2022
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7
(iii)
Fig. 2.2 shows how the temperature of the atmosphere varies with height from the ground.
110
100
90
80
70
height / km
60
50
40
30
20
10
0
–120 –100 –80 –60 –40 –20
0
20
temperature / C
Fig. 2.2
The equilibrium reaction in equation 1 has ∆Hr = –168 kJ mol–1.
Suggest how the position of this equilibrium differs at a height of 20 km compared with a
height of 50 km from the ground.
Explain your answer.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
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8
3The hydrogen halides HCl, HBr and HI are all colourless gases at room temperature.
(a)The hydrogen halides can be formed by reacting the halogens with hydrogen.
Describe and explain the relative reactivity of the halogens down the group when they react
with hydrogen to form HCl, HBr and HI.
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [2]
(b)HCl is a product of several different reactions. Some of these are shown in Fig. 3.1.
SiCl 4
NaCl
reaction 1
H2O
reaction 2
concentrated H2SO4
HCl
Fig. 3.1
(i)Write an equation for reaction 1.
........................................................................................................................................ [1]
© UCLES 2022
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9
(ii)In reaction 2, NaCl reacts with concentrated H2SO4 to form HCl and NaHSO4.
When NaBr reacts with concentrated H2SO4, the products include Br2 and SO2.
Identify the type(s) of reaction that occur in each case by completing Table 3.1.
Explain the difference in these reactions.
Table 3.1
reactants
type(s) of reaction
NaCl and concentrated H2SO4
NaBr and concentrated H2SO4
explanation ..........................................................................................................................
..............................................................................................................................................
[3]
(c)When heated with a Bunsen burner, HCl does not decompose, whereas HI forms H2 and I2.
Explain the difference in the effect of heating on HCl and HI.
.....................................................................................................................................................
............................................................................................................................................... [1]
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(d)The hydrogen halides dissolve in water to form strong Brønsted–Lowry acids.
The concentration of a strong acid can be determined by titration.
(i)State what is meant by strong Brønsted–Lowry acid.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(ii)On Fig. 3.2, sketch the pH titration curves produced when:
● 0.1 mol dm–3 NaOH(aq) is added to 25 cm3 of 0.1 mol dm–3 HBr(aq), to excess
● 0.1 mol dm–3 NH3(aq) is added to 25 cm3 of 0.1 mol dm–3 HBr(aq), to excess.
reaction of NaOH(aq) and HBr(aq)
pH
reaction of NH3(aq) and HBr(aq)
14
14
12
12
10
10
8
pH
6
8
6
4
4
2
2
0
0
5
10 15 20 25 30 35 40 45
volume of NaOH / cm3
0
0
5
10 15 20 25 30 35 40 45
volume of NH3 / cm3
Fig. 3.2
[3]
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(e)HBr reacts with propene to form two bromoalkanes, CH3CH2CH2Br and (CH3)2CHBr.
(i)Complete the diagram to show the mechanism of the reaction of HBr and propene to form
the major organic product.
Include charges, dipoles, lone pairs of electrons and curly arrows, as appropriate.
Draw the structures of the intermediate and the major organic product.
H
H
H
C
H
C
C
H
H
H
Br
[4]
(ii)Explain why the two bromoalkanes are not produced in equal amounts by this reaction.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(iii)The reaction of CH3CH2CH2Br and NaOH is different depending on whether water or
ethanol is used as a solvent.
Complete Table 3.2 to identify the organic and inorganic products of the reaction of
CH3CH2CH2Br and NaOH in each solvent.
Table 3.2
solvent
organic product(s)
inorganic product(s)
water
ethanol
[2]
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12
4Compounds J and K are found in plant oils.
J
K
OH
O
C
H 3C
C
COOH
H
CHO
C
H
CH3
C
CH3
Fig. 4.1
(a) (i)Complete Table 4.1 to state what you would observe when J reacts with the reagents
listed.
Table 4.1
reagent
observation with J
2,4-dinitrophenylhydrazine
(2,4-DNPH)
Tollens’ reagent
sodium metal
[3]
(ii)
J has two optical isomers.
Draw the three-dimensional structures of the two optical isomers of J.
[2]
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13
(b)
K is used to make the addition polymer Perspex®. A synthesis of Perspex® is shown in Fig. 4.2.
M
K
COOH
H
C
H
C
CH3
reactant L
reaction 1
COOCH3
H
C
C
H
CH3
reaction 2
Perspex®
Fig. 4.2
(i)Identify L. State the conditions required for reaction 1.
L = .......................................................................................................................................
conditions = .........................................................................................................................
[2]
(ii)Draw one repeat unit of the addition polymer Perspex®.
[2]
(iii)Use information from Table 4.2 to suggest how the infrared spectra of M and Perspex®
would differ. Explain your answer.
..............................................................................................................................................
........................................................................................................................................ [1]
Table 4.2
bond
functional group containing the bond
C–O
hydroxy, ester
1040–1300
C=C
aromatic compound, alkene
1500–1680
C=O
amide
carbonyl, carboxyl
ester
1640–1690
1670–1740
1710–1750
C≡N
nitrile
2200–2250
C–H
alkane
2850–3100
N–H
amine, amide
3300–3500
O–H
carboxyl
hydroxy
2500–3000
3200–3650
© UCLES 2022
characteristic infrared absorption range
(in wavenumbers) / cm–1
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14
(iv)
K can be made from propanone in the three-step synthesis shown in Fig. 4.3.
K
propanone
O
H 3C
C
step 1
CH3
OH
H3C
C
C
N
step 2
OH
H3C
CH3
C
COOH
step 3
CH3
H
COOH
C
H
C
CH3
Fig. 4.3
Complete Table 4.3 to identify the reagent(s) used and the type of reaction in each step.
Table 4.3
step
reagent(s)
type of reaction
1
2
3
Al 2O3
[5]
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15
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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21
20
19
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57–71
56
104
88
actinoids
lanthanoids
–
–
Ra
radium
Fr
francium
90
89
232.0
thorium
actinium
–
Th
Ac
140.1
cerium
138.9
lanthanum
59
231.0
protactinium
Pa
91
140.9
praseodymium
Pr
–
58
Ce
–
Db
dubnium
Rf
105
180.9
tantalum
73
Ta
92.9
niobium
Nb
41
50.9
vanadium
V
23
5
rutherfordium
La
57
actinoids
89–103
178.5
87
137.3
hafnium
132.9
barium
72
Hf
caesium
lanthanoids
Ba
55
91.2
zirconium
Zr
40
47.9
titanium
Ti
22
4
name
238.0
uranium
U
92
144.4
neodymium
60
Nd
–
Sg
seaborgium
106
183.8
tungsten
74
W
95.9
molybdenum
Mo
42
52.0
Cr
24
6
chromium
relative atomic mass
atomic number
Key
atomic symbol
Cs
88.9
yttrium
87.6
strontium
rubidium
85.5
Sr
Rb
Y
39
38
45.0
37
40.1
scandium
39.1
calcium
Ca
potassium
K
Sc
3
24.3
magnesium
23.0
sodium
12
Mg
Na
11
9.0
beryllium
lithium
6.9
Be
4
3
Li
2
1
–
neptunium
Np
93
–
promethium
61
Pm
–
Bh
bohrium
107
186.2
rhenium
75
Re
–
technetium
Tc
43
54.9
manganese
Mn
25
7
9
10
11
12
B
C
N
O
8
16
F
9
17
2
18
–
plutonium
Pu
94
150.4
samarium
62
Sm
–
Hs
hassium
108
190.2
osmium
76
Os
101.1
ruthenium
Ru
44
iron
55.8
Fe
26
8
1.0
–
americium
Am
95
152.0
europium
63
Eu
–
Mt
meitnerium
109
iridium
192.2
77
Ir
102.9
rhodium
Rh
45
58.9
cobalt
Co
27
–
curium
Cm
96
157.3
gadolinium
64
Gd
–
Ds
darmstadtium
110
195.1
platinum
78
Pt
106.4
palladium
Pd
46
58.7
nickel
Ni
28
–
berkelium
Bk
97
158.9
terbium
65
Tb
–
Rg
roentgenium
111
gold
197.0
79
Au
silver
107.9
Ag
47
63.5
copper
Cu
29
–
californium
Cf
98
162.5
dysprosium
66
Dy
–
Cn
copernicium
112
200.6
mercury
80
Hg
112.4
cadmium
Cd
48
zinc
65.4
Zn
30
–
einsteinium
Es
99
164.9
holmium
67
Ho
–
Nh
nihonium
113
204.4
thallium
81
Tl
114.8
indium
In
49
69.7
gallium
Ga
31
27.0
aluminium
13
Al
10.8
boron
–
fermium
Fm
100
167.3
erbium
68
Er
–
Fl
flerovium
114
lead
207.2
82
Pb
tin
118.7
Sn
50
72.6
germanium
Ge
32
28.1
silicon
14
Si
12.0
carbon
–
mendelevium
Md
101
168.9
thulium
69
Tm
–
Mc
moscovium
115
209.0
bismuth
83
Bi
121.8
antimony
Sb
51
74.9
arsenic
As
33
31.0
phosphorus
P
15
14.0
nitrogen
–
nobelium
No
102
173.1
ytterbium
70
Yb
–
Lv
livermorium
116
–
polonium
84
Po
127.6
tellurium
Te
52
79.0
selenium
Se
34
32.1
sulfur
S
16
16.0
oxygen
–
Lr
lawrencium
103
175.0
lutetium
71
Lu
–
Ts
tennessine
117
–
astatine
85
At
iodine
126.9
I
53
79.9
bromine
Br
35
35.5
chlorine
17
Cl
19.0
fluorine
–
oganesson
Og
–
118
radon
86
Rn
xenon
131.3
54
Xe
83.8
krypton
36
Kr
39.9
argon
18
Ar
neon
20.2
10
Ne
4.0
helium
7
15
hydrogen
6
14
He
5
13
H
1
Group
The Periodic Table of Elements
16
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge International AS & A Level
*5046493367*
CHEMISTRY9701/22
Paper 2 AS Level Structured Questions
May/June 2022
1 hour 15 minutes
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●
Answer all questions.
●
Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●
Write your name, centre number and candidate number in the boxes at the top of the page.
●
Write your answer to each question in the space provided.
●
Do not use an erasable pen or correction fluid.
●
Do not write on any bar codes.
●
You may use a calculator.
●
You should show all your working and use appropriate units.
INFORMATION
●
The total mark for this paper is 60.
●
The number of marks for each question or part question is shown in brackets [ ].
●
The Periodic Table is printed in the question paper.
●
Important values, constants and standards are printed in the question paper.
This document has 16 pages. Any blank pages are indicated.
IB22 06_9701_22/5RP
© UCLES 2022
[Turn over
2
1
(a)Magnesium has a melting point of 650 °C and high electrical conductivity.
Explain these properties of magnesium by referring to its structure and bonding.
.....................................................................................................................................................
............................................................................................................................................... [2]
(b)When magnesium is heated in air, magnesium oxide, MgO, is the major product. Smaller
amounts of magnesium nitride, Mg3N2, are also made.
(i)Calculate the oxidation number for magnesium and for the nitrogen species in Mg3N2 to
complete Table 1.1.
Table 1.1
species
magnesium in Mg3N2
nitrogen in Mg3N2
oxidation number
[1]
(ii)Identify the type of reaction which takes place between magnesium and nitrogen.
Explain your answer.
..............................................................................................................................................
........................................................................................................................................ [1]
(iii)
Define enthalpy change of formation.
..............................................................................................................................................
........................................................................................................................................ [2]
(iv)When 3.645 g of Mg(s) burns in excess N2(g) to form Mg3N2(s), 23.05 kJ of energy is
released.
Calculate the enthalpy change of formation, ∆Hf, of Mg3N2. Show your working.
∆Hf (Mg3N2) = .............................................. [3]
[Total: 9]
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3
Question 2 starts on the next page.
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2Radium, Ra, is an element found in Group 2 of the Periodic Table. It is a crystalline solid at room
temperature and conducts electricity.
Radium chloride, RaCl 2, has a melting point of 900 °C and is soluble in water.
(a)Predict the lattice structure of RaCl 2(s) based on the properties described.
............................................................................................................................................... [1]
(b)Draw a dot-and-cross diagram to show the arrangement of outer electrons in RaCl 2.
[1]
(c)Solid Ra and Ca show similar reactions with H2O, but the reactions occur at different rates.
Separate samples, each containing a single piece of solid Ra or Ca, are added to equal
volumes of cold water.
Each sample contains equal numbers of moles of solid and the H2O is in excess.
(i)Construct an equation for the reaction of Ra with H2O.
........................................................................................................................................ [1]
(ii)Identify which element, Ra or Ca, reacts with H2O at a faster rate. Suggest how the
observations of each reaction would differ.
..............................................................................................................................................
........................................................................................................................................ [1]
(iii)
Suggest why these reactions occur at different rates.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
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5
(iv)
One of the solutions is cloudy when the reaction has finished.
At the end of each reaction, universal indicator is added to each reaction mixture.
Suggest pH values of the solutions made in both reactions. Explain your answer.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(d)A sample of aqueous calcium halide, CaX2(aq), contains either chloride, bromide or iodide
ions.
Complete Table 2.1 to describe a two-step process that could be used to identify the halide ion
present.
Table 2.1
step
method
observation
with CaCl 2
observation
with CaBr2
observation
with CaI2
step 1
step 2
[3]
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3
(a)0.025 mol of HI(g) is added to a closed vessel and left to reach dynamic equilibrium. The total
pressure of the vessel is 100 kPa.
equation 1
2HI(g)
H2(g) + I2(g)
(i)Explain what is meant by dynamic equilibrium.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(ii)Describe one difference in the initial appearance of the reaction mixture compared to the
mixture at equilibrium.
........................................................................................................................................ [1]
(iii)Write an expression for Kp for the reaction described in equation 1.
Kp =
[1]
(iv)At equilibrium the partial pressure of HI(g) is 86.4 kPa.
Calculate the amount of HI(g) present in the mixture at equilibrium. Show your working.
© UCLES 2022
amount of HI(g) = .............................. mol [2]
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7
(b)Use equation 1 and the bond energy values in Table 3.1 to calculate the change in enthalpy,
∆H, for the thermal decomposition of 1 mole of HI(g). Show your working.
Table 3.1
bond
bond energy / kJ mol–1
H–H
436
I–I
151
H–I
299
∆H = .............................. kJ mol–1 [2]
(c) Describe the effect of increasing pressure on the value of Kp for the decomposition of HI(g).
............................................................................................................................................... [1]
(d)HCl (g) is prepared by adding NaCl (s) to concentrated H2SO4.
HI(g) is not prepared by adding NaI(s) to concentrated H2SO4 because the HI(g) produced
also reacts with concentrated H2SO4.
(i)Identify the type of reaction that occurs when NaI(s) reacts with concentrated H2SO4 to
form HI(g).
........................................................................................................................................ [1]
(ii)
Write an equation for the reaction of HI(g) and concentrated H2SO4.
........................................................................................................................................ [1]
(iii)Explain why HI(g) reacts with concentrated H2SO4 whereas HCl does not.
........................................................................................................................................ [1]
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4
(a)Bromine reacts with butane in the presence of ultraviolet light to form bromobutane.
Two structural isomers with the molecular formula C4H9Br are produced during this reaction.
(i)Draw the two structural isomers and state the systematic name of each isomer.
structural isomer 1
structural isomer 2
name ..............................................
name ..............................................
[2]
(ii)Identify the type of structural isomerism shown in (a)(i).
........................................................................................................................................ [1]
(b)Halothane is an anaesthetic.
halothane
F
F
Cl
C
C
F
Br
H
Fig. 4.1
(i)Identify the chiral centre in halothane and mark it with an asterisk (*).
[1]
When halothane reacts in ultraviolet light, homolytic fission occurs and the C–Br bond is
broken.
(ii)
Construct an equation to show the homolytic fission of halothane, CF3CHBrCl.
........................................................................................................................................ [1]
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9
(iii)
omplete Fig. 4.2 to show the arrangement of electrons in a bromine atom using the
C
electrons in boxes notation.
[Ar]
3d
4s
4p
Fig. 4.2
[1]
(c)
X is an addition polymer.
X
Cl
n
Fig. 4.3
(i)Draw the monomer of X.
[1]
(ii)Suggest one reason why the disposal of items made from X is difficult.
........................................................................................................................................ [1]
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5
Fig. 5.1 shows three reactions of 2-bromopropane, CH3CH(Br)CH3.
CH3CH(Br)CH3
reaction 1
CH3CH(OH)CH3
reaction 2
CH3CH(NH2)CH3
reaction 3
H2C=CHCH3
Fig. 5.1
(a)Complete Table 5.1 for each reaction, by:
●
●
s tating the reagent and conditions used
identifying the type of reaction that occurs.
Table 5.1
reaction
reagent and conditions
type of reaction
1
2
3
[6]
(b)A sample of 2-iodopropane, CH3CH(I)CH3, reacts under the same conditions as reaction 1 to
produce CH3CH(OH)CH3.
Explain why 2-iodopropane reacts at a faster rate than 2-bromopropane.
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [2]
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(c) Fig. 5.2 shows how butan-1-ol can be made from 1-bromopropane in three steps.
HO
N
Br
step 1
step 2
HO
step 3
O
Fig. 5.2
(i)In step 1, 1-bromopropane reacts with CN– to form butanenitrile.
omplete Fig. 5.3 to show the mechanism for step 1. Include charges, dipoles, lone pairs
C
of electrons and curly arrows as appropriate.
H
H
H
H
C
C
C
H
H
H
Br
H
C
H
H
H
C
C
C
H
H
H
C
N
Br –
–
N
Fig. 5.3
[2]
(ii)In step 2, butanenitrile is heated with HCl (aq). A hydrolysis reaction occurs.
Construct an equation for the reaction in step 2.
........................................................................................................................................ [1]
(iii)Step 3 is a reduction reaction.
Construct an equation for the reduction reaction in step 3. Use [H] to represent one atom
of hydrogen from the reducing agent.
........................................................................................................................................ [1]
(iv)State the identity of a suitable reducing agent in step 3.
........................................................................................................................................ [1]
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6
Z is a molecule which contains the elements carbon, hydrogen and oxygen only.
Z contains only alkene and carboxyl functional groups.
(a) C
omplete Table 6.1 by describing the observations that occur when two different reagents are
added to separate samples of Z(aq).
Table 6.1
reagent added
to Z(aq)
observation
Br2(aq)
Na2CO3(s)
[2]
(b)Table 6.2 shows the percentage by mass of each element present in Z.
Table 6.2
element
percentage by mass / %
carbon
41.38
hydrogen
3.45
oxygen
55.17
Using the data in Table 6.2, demonstrate that the empirical formula of Z is CHO.
Show your working.
[1]
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13
(c) Fig. 6.1 shows the mass spectrum of Z.
45
100
80
60
relative
abundance
40
71
20
0
116
117
10
20
30
40
50
60
70
80
90
100
110
120
m/e
Fig. 6.1
(i)Deduce the molecular formula of Z. Explain your answer by referring to the molecular ion
peak in Fig. 6.1 and the empirical formula of Z.
[1]
(ii)
Use Fig. 6.1 to suggest the formulae of the fragments with m / e peaks at 45 and at 71.
m / e 45 .................................................................................................................................
m / e 71 .................................................................................................................................
[2]
(iii)Suggest the structure of Z using relevant information from Table 6.1, (b) and (c).
[1]
© UCLES 2022
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[Turn over
14
BLANK PAGE
© UCLES 2022
9701/22/M/J/22
15
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)
© UCLES 2022
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© UCLES 2022
21
20
19
9701/22/M/J/22
57–71
56
104
88
actinoids
lanthanoids
–
–
Ra
radium
Fr
francium
90
89
232.0
thorium
actinium
–
Th
Ac
140.1
cerium
138.9
lanthanum
59
231.0
protactinium
Pa
91
140.9
praseodymium
Pr
–
58
Ce
–
Db
dubnium
Rf
105
180.9
tantalum
73
Ta
92.9
niobium
Nb
41
50.9
vanadium
V
23
5
rutherfordium
La
57
actinoids
89–103
178.5
87
137.3
hafnium
132.9
barium
72
Hf
caesium
lanthanoids
Ba
55
91.2
zirconium
Zr
40
47.9
titanium
Ti
22
4
name
238.0
uranium
U
92
144.4
neodymium
60
Nd
–
Sg
seaborgium
106
183.8
tungsten
74
W
95.9
molybdenum
Mo
42
52.0
Cr
24
6
chromium
relative atomic mass
atomic number
Key
atomic symbol
Cs
88.9
yttrium
87.6
strontium
rubidium
85.5
Sr
Rb
Y
39
38
45.0
37
40.1
scandium
39.1
calcium
Ca
potassium
K
Sc
3
24.3
magnesium
23.0
sodium
12
Mg
Na
11
9.0
beryllium
lithium
6.9
Be
4
3
Li
2
1
–
neptunium
Np
93
–
promethium
61
Pm
–
Bh
bohrium
107
186.2
rhenium
75
Re
–
technetium
Tc
43
54.9
manganese
Mn
25
7
9
10
11
12
B
C
N
O
8
16
F
9
17
2
18
–
plutonium
Pu
94
150.4
samarium
62
Sm
–
Hs
hassium
108
190.2
osmium
76
Os
101.1
ruthenium
Ru
44
iron
55.8
Fe
26
8
1.0
–
americium
Am
95
152.0
europium
63
Eu
–
Mt
meitnerium
109
iridium
192.2
77
Ir
102.9
rhodium
Rh
45
58.9
cobalt
Co
27
–
curium
Cm
96
157.3
gadolinium
64
Gd
–
Ds
darmstadtium
110
195.1
platinum
78
Pt
106.4
palladium
Pd
46
58.7
nickel
Ni
28
–
berkelium
Bk
97
158.9
terbium
65
Tb
–
Rg
roentgenium
111
gold
197.0
79
Au
silver
107.9
Ag
47
63.5
copper
Cu
29
–
californium
Cf
98
162.5
dysprosium
66
Dy
–
Cn
copernicium
112
200.6
mercury
80
Hg
112.4
cadmium
Cd
48
zinc
65.4
Zn
30
–
einsteinium
Es
99
164.9
holmium
67
Ho
–
Nh
nihonium
113
204.4
thallium
81
Tl
114.8
indium
In
49
69.7
gallium
Ga
31
27.0
aluminium
13
Al
10.8
boron
–
fermium
Fm
100
167.3
erbium
68
Er
–
Fl
flerovium
114
lead
207.2
82
Pb
tin
118.7
Sn
50
72.6
germanium
Ge
32
28.1
silicon
14
Si
12.0
carbon
–
mendelevium
Md
101
168.9
thulium
69
Tm
–
Mc
moscovium
115
209.0
bismuth
83
Bi
121.8
antimony
Sb
51
74.9
arsenic
As
33
31.0
phosphorus
P
15
14.0
nitrogen
–
nobelium
No
102
173.1
ytterbium
70
Yb
–
Lv
livermorium
116
–
polonium
84
Po
127.6
tellurium
Te
52
79.0
selenium
Se
34
32.1
sulfur
S
16
16.0
oxygen
–
Lr
lawrencium
103
175.0
lutetium
71
Lu
–
Ts
tennessine
117
–
astatine
85
At
iodine
126.9
I
53
79.9
bromine
Br
35
35.5
chlorine
17
Cl
19.0
fluorine
–
oganesson
Og
–
118
radon
86
Rn
xenon
131.3
54
Xe
83.8
krypton
36
Kr
39.9
argon
18
Ar
neon
20.2
10
Ne
4.0
helium
7
15
hydrogen
6
14
He
5
13
H
1
Group
The Periodic Table of Elements
16
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge International AS & A Level
*1663220061*
CHEMISTRY9701/22
Paper 2 AS Level Structured Questions
October/November 2022
1 hour 15 minutes
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●
Answer all questions.
●
Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●
Write your name, centre number and candidate number in the boxes at the top of the page.
●
Write your answer to each question in the space provided.
●
Do not use an erasable pen or correction fluid.
●
Do not write on any bar codes.
●
You may use a calculator.
●
You should show all your working and use appropriate units.
INFORMATION
●
The total mark for this paper is 60.
●
The number of marks for each question or part question is shown in brackets [ ].
●
The Periodic Table is printed in the question paper.
●
Important values, constants and standards are printed in the question paper.
This document has 16 pages. Any blank pages are indicated.
IB22 11_9701_22/3RP
© UCLES 2022
[Turn over
2
1Species such as NH4+, CO32– and PO43– are examples of molecular ions.
(a) Ionic and covalent bonds both involve an electrostatic attraction between different species.
Identify the species that are electrostatically attracted to one another in:
●
an ionic bond
.....................................................................................................................................................
●
a covalent bond.
.....................................................................................................................................................
[2]
(b)Complete Table 1.1 to show the total numbers of protons and electrons in the molecular ions
NH4+, CO32– and PO43–.
Table 1.1
molecular
ion
total number
of protons
total number
of electrons
NH4+
CO32–
PO43–
[3]
(c)NH4+ is a Brønsted–Lowry acid.
(i)
Define Brønsted–Lowry acid.
..............................................................................................................................................
........................................................................................................................................ [1]
(ii)When NH4+(aq) is heated with NaOH(aq), a pungent gas is produced.
Write an ionic equation for this reaction.
........................................................................................................................................ [1]
© UCLES 2022
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3
(iii)The nitrogen atom in NH4+ is sp3 hybridised. sp3 orbitals form from the mixing of one 2s and
three 2p orbitals.
Sketch the shapes of a 2s and a 2px orbital on the axes in Fig. 1.1.
z
z
y
y
x
x
2s
2px
Fig. 1.1
[2]
(d)There are many naturally occurring hydrated compounds that contain the anion PO43–.
(i)Name the anion PO43–.
........................................................................................................................................ [1]
(ii)Struvite is a soft hydrated mineral with Mr = 245.3. The anhydrous form of the mineral has
the formula NH4MgPO4.
Calculate the number of molecules of water of crystallisation in struvite.
Give your answer to the nearest integer. Show your working.
© UCLES 2022
number of molecules of water of crystallisation = .............................. [2]
9701/22/O/N/22
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4
(e)OH–(aq) reacts with 2-bromo-2-methylpropane in an SN1 reaction.
The molecular ion (CH3)3C+ forms as the intermediate in this reaction.
(i)Draw the mechanism for the SN1 reaction of OH– with 2-bromo-2-methylpropane.
Include charges, dipoles, lone pairs of electrons and curly arrows as appropriate.
Draw the structures of the organic reactant and organic product.
H 3C
+
C
CH3
CH3
[3]
(ii)2-bromo-2-methylpropane is a tertiary bromoalkane.
Define tertiary bromoalkane.
..............................................................................................................................................
........................................................................................................................................ [1]
(iii)Organic compound M forms when 2‑bromo‑2‑methylpropane is heated with ethanolic
OH–.
Draw the structure of M.
[1]
© UCLES 2022
[Total: 17]
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5
2The chlorides of some of the Period 3 elements are shown in Table 2.1.
Table 2.1
Period 3 chloride
NaCl
Al Cl 3
SiCl 4
PCl 5
PCl 3
SCl 2
bonding
C
C
structure
S
S
oxidation state of Period 3 element
(a)Complete Table 2.1.
● Identify the bonding shown by each chloride under standard conditions.
Use C = covalent, I = ionic, M = metallic.
● Identify the structure shown by each chloride under standard conditions.
Use G = giant, S = simple.
● Deduce the oxidation state of the Period 3 element in each chloride.
[4]
(b)Write equations for the reactions of NaCl and PCl 5 with water.
Include state symbols in both equations.
NaCl ...........................................................................................................................................
PCl 5 ............................................................................................................................................
[3]
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6
(c)In the gas phase, Al Cl 3(g) exists at equilibrium with Al 2Cl 6(g) as shown.
equation 1
2Al Cl 3(g)
Al 2Cl 6(g)
∆Hr = –63 kJ mol–1
(i)Complete the dot-and-cross diagram to show the bonding in Al 2Cl 6.
Cl
Al
Cl
[2]
(ii)
tate the effect of an increase in temperature on the equilibrium mixture in equation 1.
S
Explain your answer.
..............................................................................................................................................
........................................................................................................................................ [1]
(d) A 3.30 g sample of a Period 3 chloride is heated to 500 K in a sealed flask.
At this temperature, the chloride is a gas of volume 250 cm3 and the pressure in the flask is
323 kPa.
Use the ideal gas equation pV = nRT to calculate the Mr of the Period 3 chloride.
Deduce its formula.
Mr = ..............................
formula of Period 3 chloride = ..............................
[3]
© UCLES 2022
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7
(e) (i)An excess of Cl –(aq) is added to 1 cm3 of Br2(aq).
Describe what is observed. Explain your answer.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(ii)SCl 2 has Mr = 103.1 and is a liquid at room temperature. SBr2 has Mr = 191.9 and is a gas
at room temperature.
xplain the difference in the physical state of SCl 2 and SBr2. Give your answer in terms of
E
intermolecular forces.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
(f)Bismuth is a dense metal in the same group as phosphorus.
(i)Draw a labelled diagram to show the bonding in bismuth metal.
[2]
(ii)Bismuth reacts with chlorine to form BiCl 3.
BiCl 3 is a solid at room temperature. It melts when heated gently.
BiCl 3 reacts vigorously with water at room temperature to form an acidic solution.
Suggest the type of bonding and structure shown by BiCl 3. Explain your answer.
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [2]
© UCLES 2022
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8
3Organic compounds can be distinguished using chemical tests and analytical techniques.
(a)Table 3.1 shows four pairs of organic compounds.
Table 3.1
organic compounds
reagent
A1
A2
O
O
positive result of
chemical test on
identified compound
H
B1
B2
O
O
C1
O
C2
O
O
D1
D2
CH3
OH
OH
(i)Complete Table 3.1 to:
● identify a reagent which can distinguish between the compounds in each pair
● give the positive result of the chemical test and identify which compound shows this
result.
Use a different reagent for each test.
[8]
(ii)
A1 and A2 are structural isomers.
Define structural isomers.
..............................................................................................................................................
........................................................................................................................................ [1]
© UCLES 2022
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9
(iii)Give the systematic name of B2.
........................................................................................................................................ [1]
(iv)Deduce the molecular formula of D1.
........................................................................................................................................ [1]
(b)
D2 forms polymer Z when heated gently.
(i)Identify the type of polymer that forms from D2.
........................................................................................................................................ [1]
(ii)Draw one repeat unit of polymer Z.
[2]
© UCLES 2022
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10
(c)Organic compound E contains three carbon atoms.
E reacts with cold dilute acidified KMnO4(aq) to form a single compound F with Mr = 154.9.
Fig. 3.1 shows the infrared spectrum of E.
Fig. 3.2 shows the infrared spectrum of F.
E
100
transmittance
/%
50
0
4000
3000
2000
1500
1000
500
1000
500
wavenumber / cm–1
Fig. 3.1
F
100
transmittance
/%
50
0
4000
3000
2000
1500
wavenumber / cm–1
Fig. 3.2
© UCLES 2022
9701/22/O/N/22
11
Table 3.2
bond
functional group containing the bond
characteristic infrared absorption range
(in wavenumbers) / cm–1
C–O
hydroxy, ester
1040–1300
C=C
aromatic compound, alkene
1500–1680
C=O
amide
carbonyl, carboxyl
ester
1640–1690
1670–1740
1710–1750
C≡N
nitrile
2200–2250
C–H
alkane
2850–3100
N–H
amine, amide
3300–3500
O–H
carboxyl
hydroxy
2500–3000
3200–3650
oth spectra show absorptions between 2850 and 2950 cm–1 owing to C–H bonds in each
B
molecule.
(i)Use the two infrared spectra and Table 3.2 to identify the functional group present only
in E.
Explain your answer, referring only to absorptions at frequencies greater than 1500 cm–1.
functional group ...................................................................................................................
explanation ..........................................................................................................................
..............................................................................................................................................
[1]
(ii)Use the infrared spectrum of F to identify the functional group formed when E reacts with
cold dilute acidified KMnO4(aq).
Explain your answer, referring only to absorptions at frequencies greater than 1500 cm–1.
functional group ...................................................................................................................
explanation ..........................................................................................................................
..............................................................................................................................................
[1]
(iii)The mass spectrum of E shows a molecular ion peak and an M+2 peak of approximately
equal abundance at m/e = 120 and 122.
Deduce the relative molecular mass, Mr, of E.
Mr = .............................. [1]
© UCLES 2022
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12
(iv)Use the information in 3(c) to suggest a structure for E.
[1]
(v)Complete the equation for the reaction of E with cold dilute acidified KMnO4(aq) to form F.
In the equation, [O] represents cold dilute acidified KMnO4(aq).
H2O + [O] + ........................................... → ....................................................................
[1]
(d)
C2 can be synthesised using A1 as a single organic reactant.
C2
A1
O
O
O
H
Devise a multi-step synthetic route to form C2 from A1.
Identify relevant reagents and conditions, and state the organic products of each step.
.....................................................................................................................................................
.....................................................................................................................................................
.....................................................................................................................................................
.....................................................................................................................................................
.....................................................................................................................................................
............................................................................................................................................... [3]
© UCLES 2022
[Total: 22]
9701/22/O/N/22
13
BLANK PAGE
© UCLES 2022
9701/22/O/N/22
14
BLANK PAGE
© UCLES 2022
9701/22/O/N/22
15
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)
© UCLES 2022
9701/22/O/N/22
© UCLES 2022
21
20
19
9701/22/O/N/22
57–71
56
104
88
actinoids
lanthanoids
–
–
Ra
radium
Fr
francium
90
89
232.0
thorium
actinium
–
Th
Ac
140.1
cerium
138.9
lanthanum
59
231.0
protactinium
Pa
91
140.9
praseodymium
Pr
–
58
Ce
–
Db
dubnium
Rf
105
180.9
tantalum
73
Ta
92.9
niobium
Nb
41
50.9
vanadium
V
23
5
rutherfordium
La
57
actinoids
89–103
178.5
87
137.3
hafnium
132.9
barium
72
Hf
caesium
lanthanoids
Ba
55
91.2
zirconium
Zr
40
47.9
titanium
Ti
22
4
name
238.0
uranium
U
92
144.4
neodymium
60
Nd
–
Sg
seaborgium
106
183.8
tungsten
74
W
95.9
molybdenum
Mo
42
52.0
Cr
24
6
chromium
relative atomic mass
atomic number
Key
atomic symbol
Cs
88.9
yttrium
87.6
strontium
rubidium
85.5
Sr
Rb
Y
39
38
45.0
37
40.1
scandium
39.1
calcium
Ca
potassium
K
Sc
3
24.3
magnesium
23.0
sodium
12
Mg
Na
11
9.0
beryllium
lithium
6.9
Be
4
3
Li
2
1
–
neptunium
Np
93
–
promethium
61
Pm
–
Bh
bohrium
107
186.2
rhenium
75
Re
–
technetium
Tc
43
54.9
manganese
Mn
25
7
9
10
11
12
B
C
N
O
8
16
F
9
17
2
18
–
plutonium
Pu
94
150.4
samarium
62
Sm
–
Hs
hassium
108
190.2
osmium
76
Os
101.1
ruthenium
Ru
44
iron
55.8
Fe
26
8
1.0
–
americium
Am
95
152.0
europium
63
Eu
–
Mt
meitnerium
109
iridium
192.2
77
Ir
102.9
rhodium
Rh
45
58.9
cobalt
Co
27
–
curium
Cm
96
157.3
gadolinium
64
Gd
–
Ds
darmstadtium
110
195.1
platinum
78
Pt
106.4
palladium
Pd
46
58.7
nickel
Ni
28
–
berkelium
Bk
97
158.9
terbium
65
Tb
–
Rg
roentgenium
111
gold
197.0
79
Au
silver
107.9
Ag
47
63.5
copper
Cu
29
–
californium
Cf
98
162.5
dysprosium
66
Dy
–
Cn
copernicium
112
200.6
mercury
80
Hg
112.4
cadmium
Cd
48
zinc
65.4
Zn
30
–
einsteinium
Es
99
164.9
holmium
67
Ho
–
Nh
nihonium
113
204.4
thallium
81
Tl
114.8
indium
In
49
69.7
gallium
Ga
31
27.0
aluminium
13
Al
10.8
boron
–
fermium
Fm
100
167.3
erbium
68
Er
–
Fl
flerovium
114
lead
207.2
82
Pb
tin
118.7
Sn
50
72.6
germanium
Ge
32
28.1
silicon
14
Si
12.0
carbon
–
mendelevium
Md
101
168.9
thulium
69
Tm
–
Mc
moscovium
115
209.0
bismuth
83
Bi
121.8
antimony
Sb
51
74.9
arsenic
As
33
31.0
phosphorus
P
15
14.0
nitrogen
–
nobelium
No
102
173.1
ytterbium
70
Yb
–
Lv
livermorium
116
–
polonium
84
Po
127.6
tellurium
Te
52
79.0
selenium
Se
34
32.1
sulfur
S
16
16.0
oxygen
–
Lr
lawrencium
103
175.0
lutetium
71
Lu
–
Ts
tennessine
117
–
astatine
85
At
iodine
126.9
I
53
79.9
bromine
Br
35
35.5
chlorine
17
Cl
19.0
fluorine
–
oganesson
Og
–
118
radon
86
Rn
xenon
131.3
54
Xe
83.8
krypton
36
Kr
39.9
argon
18
Ar
neon
20.2
10
Ne
4.0
helium
7
15
hydrogen
6
14
He
5
13
H
1
Group
The Periodic Table of Elements
16
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge International AS & A Level
* 6 1 7 1 3 8 5 9 1 3 *
CHEMISTRY
9701/22
Paper 2 AS Level Structured Questions
February/March 2023
1 hour 15 minutes
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●
Answer all questions.
●
Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●
Write your name, centre number and candidate number in the boxes at the top of the page.
●
Write your answer to each question in the space provided.
●
Do not use an erasable pen or correction fluid.
●
Do not write on any bar codes.
●
You may use a calculator.
●
You should show all your working and use appropriate units.
INFORMATION
●
The total mark for this paper is 60.
●
The number of marks for each question or part question is shown in brackets [ ].
●
The Periodic Table is printed in the question paper.
●
Important values, constants and standards are printed in the question paper.
This document has 16 pages. Any blank pages are indicated.
DC (RW/CB) 309508/3
© UCLES 2023
[Turn over
2
1
The Pauling electronegativity values of elements can be used to predict the chemical properties of
compounds.
Use the information in Table 1.1 to answer the following questions.
Table 1.1
element
H
Li
C
O
S
Pauling electronegativity value
2.1
1.0
2.5
3.5
2.6
first ionisation energy / kJ mol–1
1310
519
1090
1310
1000
second ionisation energy / kJ mol–1
—
7300
2350
3390
2260
(a) (i)
Define electronegativity.
...........................................................................................................................................
..................................................................................................................................... [1]
(ii)
O and S are in Group 16.
Explain the difference in the Pauling electronegativity values of O and S.
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [2]
(b) (i)
LiH is an ionic compound.
Draw a dot‑and‑cross diagram of LiH.
Include all electrons.
[2]
(ii)
Suggest the shape of a molecule of H2S.
..................................................................................................................................... [1]
© UCLES 2023
9701/22/F/M/23
3
(c) (i)
Write an equation that represents the first ionisation energy of H.
..................................................................................................................................... [1]
(ii)
Explain why there is no information given in Table 1.1 for the second ionisation energy
of H.
..................................................................................................................................... [1]
(iii)
Give the full electronic configuration of S2+(g).
..................................................................................................................................... [1]
(d) CO2 and SO2 are acidic gases.
(i)
Write an equation for the reaction of SO2 with H2O.
..................................................................................................................................... [1]
(ii)
Write an equation for the reaction of SO2 with NaOH.
..................................................................................................................................... [1]
(iii)
Construct an equation for the reaction of CO2 with Mg(OH)2.
..................................................................................................................................... [1]
© UCLES 2023
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(e) (i)
Complete Table 1.2 by placing a tick (✓) to show which of the compounds have molecules
with an overall dipole moment.
Table 1.2
compound
O=C=O
O=S=O
S=C=S
S=C=O
overall dipole
moment
[2]
(ii)
At 150 °C and 103 kPa, all of the compounds listed in Table 1.2 are gases.
Under these conditions, 0.284 g of one of the compounds occupies a volume of 127 cm3.
Use this information to calculate the Mr of the compound. Hence, identify the compound
from those given in Table 1.2.
Show your working.
Mr = .............................................. identity of compound = ..............................................
[3]
[Total: 17]
© UCLES 2023
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© UCLES 2023
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2
The Group 2 elements Mg to Ba are all silvery‑white reactive metals.
(a) (i)
Draw a labelled diagram to show the bonding and structure of the Group 2 metals at
room temperature.
[2]
(ii)
Explain why Mg has a higher electrical conductivity than Na.
...........................................................................................................................................
..................................................................................................................................... [1]
(b) Write an equation for the reaction of magnesium with cold water.
............................................................................................................................................. [1]
(c) Identify a single reagent that can be used to distinguish separate samples of dilute
Mg(NO3)2(aq) and dilute Ba(NO3)2(aq).
Explain your answer.
reagent .....................................................................................................................................
explanation ...............................................................................................................................
...................................................................................................................................................
[2]
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(d) (i)
Describe what is observed when SrI2(aq) reacts with concentrated sulfuric acid.
...........................................................................................................................................
..................................................................................................................................... [2]
(ii)
Compound X, an anhydrous Group 2 bromide, is dissolved in water and titrated against
aqueous silver nitrate.
A solution containing 0.250 g of X requires 33.65 cm3 of 0.0500 mol dm–3 AgNO3(aq) for
complete reaction.
Identify X.
Show your working.
X = ......................................................... [3]
[Total: 11]
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3
Alkenes undergo an addition reaction with a 1:1 mixture of CO and H2 to form aldehydes.
Fig. 3.1 shows the reaction of propene with a 1:1 mixture of CO and H2.
CO
propene
H2
CHO
and
A
CHO
B
Fig. 3.1
(a) (i)
Define addition reaction.
...........................................................................................................................................
..................................................................................................................................... [1]
(ii)
Aldehydes A and B are structural isomers.
State the type of structural isomerism shown by A and B.
..................................................................................................................................... [1]
(iii)
Name A.
..................................................................................................................................... [1]
(iv)
The complete reaction of propene with a 1:1 mixture of CO and H2 produces A and B
only. The product mixture contains 96% A and 4% B.
Calculate the mass of A produced in this reaction when 5.00 × 103 kg of propene is used.
mass of A = ..................................................... kg [1]
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9
(b) A and B show reactions typical of aliphatic aldehydes.
(i)
A undergoes a nucleophilic addition reaction with a mixture of HCN and KCN, forming
compound C.
Complete the diagram to show the mechanism for this reaction.
Include charges, dipoles, lone pairs of electrons and curly arrows, as appropriate.
Draw the structure of the organic intermediate.
A
C
O
H
C
OH
H
C3H7
C3H7
C
CN
[4]
(ii)
Table 3.1 shows information about three experiments involving B.
Complete Table 3.1.
Table 3.1
experiment
observation with B
reagents
1
solution turns from orange to green
2
a silver mirror forms on the sides of
the reaction vessel
3
Br2(aq)
[3]
(iii)
B, C4H8O, is oxidised by acidified potassium manganate(VII).
Complete the equation for this reaction. Use [O] to represent one atom of oxygen from
the oxidising agent.
C4H8O + ...................................................................................................................... [1]
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(iv)
C is a chiral molecule.
Circle any chiral centres in the structure of C shown in Fig. 3.2.
C
H
OH H
H
H
C
C
C
C
C
III
N
H
H
H
H
Fig. 3.2
[1]
(c) When propene reacts with CO and an excess of H2, an alkane and a mixture of alcohols are
formed instead. The alcohols are isomers of each other.
Suggest the molecular formulae of the alkane and the alcohols that are formed under these
conditions.
molecular formula of alkane .....................................................................................................
molecular formula of alcohols ...................................................................................................
[2]
(d) The reaction of ethene, C2H4, with a 1:1 mixture of CO and H2 is shown in equation 1.
equation 1
C2H4(g) + CO(g) + H2(g)
CH3CH2CHO(g)
At atmospheric pressure a cobalt‑based catalyst is used in this reaction.
(i)
State and explain the effect of using a catalyst on this reaction.
...........................................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [2]
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(ii)
Explain why the yield of CH3CH2CHO(g) increases when the overall pressure of the
reaction mixture is increased.
...........................................................................................................................................
..................................................................................................................................... [1]
(iii)
Use the information in Table 3.2 to calculate the enthalpy change, ΔHr, of the reaction in
equation 1.
equation 1
C2H4(g) + CO(g) + H2(g)
CH3CH2CHO(g)
Table 3.2
compound
enthalpy change of
formation, ΔHf / kJ mol–1
C2H4(g)
+52
CO(g)
–111
CH3CH2CHO(g)
–187
ΔHr = ............................................ kJ mol–1 [2]
(iv)
The reaction mixture is cooled to collect CH3CH2CHO as a liquid.
Identify all types of van der Waals’ forces that are present between molecules of
CH3CH2CHO.
...........................................................................................................................................
..................................................................................................................................... [1]
[Total: 21]
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4
Fig. 4.1 shows some reactions of compound D, 2‑bromobutane.
D
E
reaction 1
Br
addition
polymer
reaction 4
KCN dissolved
in ethanol
reaction 2
AgNO3(aq) in
ethanol
F
G
OH
CN
reaction 5
LiAl H4
H
CH2NH2
reaction 3
alkaline I2(aq)
yellow
precipitate
+
an organic ion
Fig. 4.1
(a) (i)
State the reagent and conditions used to form E in reaction 1.
..................................................................................................................................... [1]
(ii)
Draw the structure of one repeat unit of the addition polymer that forms from E.
[1]
(iii)
E also forms when F is heated strongly in the presence of an Al 2O3 catalyst.
Write an equation for this reaction.
..................................................................................................................................... [1]
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(b) (i)
Predict what is observed in reaction 2.
..................................................................................................................................... [1]
(ii)
Identify the yellow precipitate and the organic ion formed in reaction 3.
yellow precipitate ...............................................................................................................
organic ion .........................................................................................................................
[2]
(c) (i)
State the type of reaction that occurs in reaction 4.
..................................................................................................................................... [1]
(ii)
Reaction 5 is similar to the reaction of LiAl H4 with carboxylic acids to form alcohols.
Suggest the role of LiAl H4 in reaction 5.
..................................................................................................................................... [1]
(d) (i)
Fig. 4.2 shows the infrared spectrum of one of the compounds D, E, F, G or H.
100
transmittance
50
/%
0
4000
3000
2000
1500
wavenumber / cm–1
1000
500
Fig. 4.2
Use information from Table 4.1 (on page 14) to identify which of the compounds D, E, F,
G or H produces the infrared spectrum in Fig. 4.2.
Explain your answer.
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [2]
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Table 4.1
bond
functional groups containing the bond
C–O
hydroxy, ester
1040–1300
C=C
aromatic compound, alkene
1500–1680
C=O
amide
carbonyl, carboxyl
ester
1640–1690
1670–1740
1710–1750
C≡N
nitrile
2200–2250
C–H
alkane
2850–2950
N–H
amine, amide
3300–3500
O–H
carboxyl
hydroxy
2500–3000
3200–3600
(ii)
characteristic infrared absorption range
(in wavenumbers) / cm–1
In the mass spectrum of D, the relative abundance of the molecular ion peak is 3.4.
Predict the relative abundance of the M+2 peak for D.
Explain your answer.
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [1]
[Total: 11]
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15
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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20
19
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57–71
56
104
88
actinoids
lanthanoids
–
–
Ra
radium
Fr
francium
90
89
232.0
thorium
actinium
–
Th
Ac
140.1
cerium
138.9
lanthanum
59
231.0
protactinium
Pa
91
140.9
praseodymium
Pr
–
58
Ce
–
Db
dubnium
Rf
105
180.9
tantalum
73
Ta
92.9
niobium
Nb
41
50.9
vanadium
V
23
5
rutherfordium
La
57
actinoids
89–103
178.5
87
137.3
hafnium
132.9
barium
72
Hf
caesium
lanthanoids
Ba
55
91.2
zirconium
Zr
40
47.9
titanium
Ti
22
4
name
238.0
uranium
U
92
144.4
neodymium
60
Nd
–
Sg
seaborgium
106
183.8
tungsten
74
W
95.9
molybdenum
Mo
42
52.0
Cr
24
6
chromium
relative atomic mass
atomic number
Key
atomic symbol
Cs
88.9
yttrium
87.6
strontium
rubidium
85.5
Sr
Rb
Y
39
38
45.0
37
40.1
scandium
39.1
calcium
Ca
potassium
K
Sc
3
24.3
magnesium
23.0
sodium
12
Mg
Na
11
9.0
beryllium
lithium
6.9
Be
4
3
Li
2
1
–
neptunium
Np
93
–
promethium
61
Pm
–
Bh
bohrium
107
186.2
rhenium
75
Re
–
technetium
Tc
43
54.9
manganese
Mn
25
7
9
10
11
12
B
C
N
O
8
16
F
9
17
2
18
–
plutonium
Pu
94
150.4
samarium
62
Sm
–
Hs
hassium
108
190.2
osmium
76
Os
101.1
ruthenium
Ru
44
iron
55.8
Fe
26
8
1.0
–
americium
Am
95
152.0
europium
63
Eu
–
Mt
meitnerium
109
iridium
192.2
77
Ir
102.9
rhodium
Rh
45
58.9
cobalt
Co
27
–
curium
Cm
96
157.3
gadolinium
64
Gd
–
Ds
darmstadtium
110
195.1
platinum
78
Pt
106.4
palladium
Pd
46
58.7
nickel
Ni
28
–
berkelium
Bk
97
158.9
terbium
65
Tb
–
Rg
roentgenium
111
gold
197.0
79
Au
silver
107.9
Ag
47
63.5
copper
Cu
29
–
californium
Cf
98
162.5
dysprosium
66
Dy
–
Cn
copernicium
112
200.6
mercury
80
Hg
112.4
cadmium
Cd
48
zinc
65.4
Zn
30
–
einsteinium
Es
99
164.9
holmium
67
Ho
–
Nh
nihonium
113
204.4
thallium
81
Tl
114.8
indium
In
49
69.7
gallium
Ga
31
27.0
aluminium
13
Al
10.8
boron
–
fermium
Fm
100
167.3
erbium
68
Er
–
Fl
flerovium
114
lead
207.2
82
Pb
tin
118.7
Sn
50
72.6
germanium
Ge
32
28.1
silicon
14
Si
12.0
carbon
–
mendelevium
Md
101
168.9
thulium
69
Tm
–
Mc
moscovium
115
209.0
bismuth
83
Bi
121.8
antimony
Sb
51
74.9
arsenic
As
33
31.0
phosphorus
P
15
14.0
nitrogen
–
nobelium
No
102
173.1
ytterbium
70
Yb
–
Lv
livermorium
116
–
polonium
84
Po
127.6
tellurium
Te
52
79.0
selenium
Se
34
32.1
sulfur
S
16
16.0
oxygen
–
Lr
lawrencium
103
175.0
lutetium
71
Lu
–
Ts
tennessine
117
–
astatine
85
At
iodine
126.9
I
53
79.9
bromine
Br
35
35.5
chlorine
17
Cl
19.0
fluorine
–
oganesson
Og
–
118
radon
86
Rn
xenon
131.3
54
Xe
83.8
krypton
36
Kr
39.9
argon
18
Ar
neon
20.2
10
Ne
4.0
helium
7
15
hydrogen
6
14
He
5
13
H
1
Group
The Periodic Table of Elements
16
To avoid the issue of disclosure of answer‑related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge International AS & A Level
* 9 1 0 1 9 6 5 1 5 9 *
CHEMISTRY
9701/22
Paper 2 AS Level Structured Questions
May/June 2023
1 hour 15 minutes
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●
Answer all questions.
●
Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●
Write your name, centre number and candidate number in the boxes at the top of the page.
●
Write your answer to each question in the space provided.
●
Do not use an erasable pen or correction fluid.
●
Do not write on any bar codes.
●
You may use a calculator.
●
You should show all your working and use appropriate units.
INFORMATION
●
The total mark for this paper is 60.
●
The number of marks for each question or part question is shown in brackets [ ].
●
The Periodic Table is printed in the question paper.
●
Important values, constants and standards are printed in the question paper.
This document has 16 pages. Any blank pages are indicated.
DC (LK/SG) 308406/5
© UCLES 2023
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1
The melting points of some solids are shown in Table 1.1.
Table 1.1
solid
(a) (i)
melting point / K
magnesium
923
phosphorus
317
sodium chloride
1074
sulfur
392
State the type of bonding present in magnesium and in sodium chloride.
bonding in magnesium ......................................................................................................
bonding in sodium chloride ...............................................................................................
[1]
(ii)
Explain the difference in the melting points of magnesium and sodium chloride.
...........................................................................................................................................
..................................................................................................................................... [1]
(iii)
Explain the difference in the melting points of phosphorus and sulfur in terms of structure
and bonding.
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [2]
(b) (i)
Define electronegativity.
...........................................................................................................................................
..................................................................................................................................... [1]
(ii)
Explain why electronegativity increases across a period.
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [2]
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(iii)
Name the strongest intermolecular force that exists between NH3(l) molecules.
..................................................................................................................................... [1]
(iv)
Draw a diagram to show the formation of the strongest intermolecular force between
two molecules of NH3(l).
Include any relevant lone pairs of electrons and dipoles.
[2]
(v)
The melting points of ice and ammonia are shown in Table 1.2.
Table 1.2
solid
melting point / K
ice
273
ammonia
195
Suggest two reasons for the difference in the melting points of ice and ammonia.
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [2]
[Total: 12]
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2
Chlorine is a reactive element. It forms many compounds.
(a) (i)
Complete Table 2.1 to show the maximum oxidation number of the elements Na to P in
their chlorides.
Table 2.1
element
Na
Mg
Al
Si
P
maximum oxidation number
[1]
(ii)
State what determines the maximum oxidation number of elements in Period 3.
...........................................................................................................................................
..................................................................................................................................... [1]
(b) An excess of cold water is added to the chloride of silicon.
(i)
Write an equation for the reaction between an excess of cold water and the chloride of
silicon.
..................................................................................................................................... [1]
(ii)
Suggest the pH of the solution produced in (b)(i).
..................................................................................................................................... [1]
(c) An excess of cold water is added to the chloride of phosphorus.
(i)
Write an equation for the reaction between an excess of cold water and the chloride of
phosphorus.
..................................................................................................................................... [1]
(ii)
Suggest the pH of the solution produced in (c)(i).
..................................................................................................................................... [1]
(d) (i)
Write an equation for the reaction of chlorine with water.
..................................................................................................................................... [1]
(ii)
Write an equation for the reaction of chlorine with hot NaOH(aq).
..................................................................................................................................... [1]
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(e) Bleach is used as a cleaning product to kill bacteria. It is made by adding compounds like
sodium chlorate(I), NaCl O, to water.
(i)
Identify the formula of the ion present in bleach that kills bacteria.
..................................................................................................................................... [1]
(ii)
Sodium chlorate(I), NaCl O, reacts with hydrogen peroxide to produce sodium chloride,
water and oxygen gas.
Construct an equation for this reaction.
..................................................................................................................................... [1]
(iii)
A sample of bleach W contains an unknown concentration of sodium chlorate(I).
10.0 cm3 of W is diluted with distilled water to make a total volume of 100 cm3 of
bleach solution. 25.0 cm3 of this diluted bleach solution is added to an excess of
hydrogen peroxide and the volume of gas produced measured under room conditions.
The experiment is repeated and on average 25.0 cm3 of diluted bleach solution produces
42.0 cm3 of gas.
Calculate the concentration, in g dm–3, of sodium chlorate(I) in W.
concentration of NaCl O in W = .............................. g dm–3 [3]
[Total: 13]
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3
Fig. 3.1 describes a sequence of reactions that can be used to produce a food additive,
compound Y, from CH3CH2Cl .
CH3CH2Cl
step 1
X
CH3CH2CN
step 2
dilute acid
CH3CH2COOH
step 3
Y
Ca(s)
Fig. 3.1
(a) (i)
State the reagent and conditions for step 1 in Fig. 3.1.
..................................................................................................................................... [1]
(ii)
Give the systematic name of X.
..................................................................................................................................... [1]
(iii)
Identify the type of reaction that occurs when dilute acid is added to X in step 2.
..................................................................................................................................... [1]
(iv)
In step 3, Y and a gas are produced.
Construct an equation for step 3.
..................................................................................................................................... [2]
(b) CH3CH2COOH can also be formed from propan-1-ol and potassium dichromate(VI).
State the conditions required.
............................................................................................................................................. [1]
(c) Complete Table 3.1 to show the number of sigma bonds (σ ) and pi bonds (π) present in a
molecule of X.
Table 3.1
type of bond
number of bonds in X
sigma (σ )
pi (π)
[2]
[Total: 8]
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4
In industry, ethanol is made by reacting ethene with steam in the presence of H3PO4.
reaction 1
C2H4(g) + H2O(g)
C2H5OH(g)
(a) Use the bond energy values in Table 4.1 to calculate the enthalpy change, ΔHr , for reaction 1.
Table 4.1
bond
bond energy / kJ mol–1
C–C
350
C=C
610
C≡C
840
C–H
410
C–O
360
C=O
740
O–H
460
ΔHr = .............................. kJ mol–1 [2]
(b) Reaction 1 reaches equilibrium at constant temperature and pressure.
Deduce what effect increasing the pressure will have on the amount of ethanol in the new
equilibrium mixture. Use Le Chatelier’s principle to explain your answer.
effect of increasing pressure .....................................................................................................
explanation ...............................................................................................................................
...................................................................................................................................................
[2]
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(c) The mechanism for reaction 1 can be described in three steps. Steps 1 and 2 for reaction 1
are shown in Fig. 4.1.
step 1
CH2
H 2C
H
H
H
H 2C
C+
O
HO
P
O–
OH
HO
O
step 2
H
H 2C
H
P
OH
O
H
H
C+
H
H3C
O
H
CH2
O+
H
H
Fig. 4.1
(i)
Describe the behaviour of H3PO4 in step 1 in Fig. 4.1. Explain your answer.
...........................................................................................................................................
..................................................................................................................................... [1]
(ii)
Identify the species that behaves as an electrophile in step 2 in Fig. 4.1. Explain your
answer.
...........................................................................................................................................
..................................................................................................................................... [1]
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(iii)
Complete Fig. 4.2 to show the mechanism for step 3 of reaction 1. Include charges,
dipoles, lone pairs of electrons and curly arrows, as appropriate.
H 3C
CH2
O+
H 3C
H
CH2
O
H
H
H
O–
HO
P
O
OH
HO
O
P
OH
O
Fig. 4.2
(iv)
[2]
Describe how a catalyst affects a reaction. Explain your answer.
...........................................................................................................................................
..................................................................................................................................... [2]
(v)
Use Fig. 4.1 and Fig. 4.2 to justify why H3PO4 is described as a catalyst in reaction 1.
...........................................................................................................................................
..................................................................................................................................... [1]
(vi)
Propene also reacts with steam. A mixture of organic products is produced.
Explain why propan-2-ol is produced in the higher yield.
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [2]
(d) Describe the covalent bonds present between the carbon atoms in an ethene molecule by
completing Table 4.2.
Table 4.2
sigma (σ )
pi (π)
type of orbitals involved in bond
how the orbitals overlap
[2]
[Total: 15]
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5
(a) Describe structural isomerism.
...................................................................................................................................................
............................................................................................................................................. [1]
(b) A and B are structural isomers with molecular formula C5H10O.
They are both straight-chained molecules with only one functional group.
Table 5.1 describes observations when separate samples of A and B are added to different
reagents.
Table 5.1
reagent
2,4-dinitrophenylhydrazine
(2,4-DNPH reagent)
(i)
A
B
orange precipitate appears orange precipitate appears
Tollens’ reagent
silver mirror appears
no reaction
alkaline I2(aq)
no reaction
no reaction
Name the functional group present in both A and B.
..................................................................................................................................... [1]
(ii)
Draw the structures of A and B in the boxes.
B
A
[2]
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(c) C is a structural isomer of A and B.
C is straight chained and has two functional groups.
C shows only one type of stereoisomerism.
Table 5.2 describes observations when separate samples of C are added to different
reagents.
Table 5.2
(i)
reagent
C
2,4-dinitrophenylhydrazine
(2,4-DNPH reagent)
no reaction
Br2(aq)
orange to colourless
alkaline I2(aq)
yellow precipitate appears
Draw the structure of C in the box.
C
[2]
(ii)
Name the type of stereoisomerism shown by molecules of C.
..................................................................................................................................... [1]
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(d) D reacts in the presence of a sulfuric acid catalyst to form E and water.
The structure of E is shown in Fig. 5.1.
E
O
O
Fig. 5.1
(i)
Name the functional group present in E.
..................................................................................................................................... [1]
(ii)
Identify the type of reaction that occurs when D reacts to form E.
..................................................................................................................................... [1]
(iii)
Draw the structure of D in the box.
D
[1]
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(iv)
The infrared spectrum of E is shown in Fig. 5.2.
100
transmittance / % 50
0
4000
3000
2000
1500
wavenumber / cm–1
1000
500
Fig. 5.2
Table 5.3
bond
functional groups containing the bond
characteristic infrared absorption range
(in wavenumbers) / cm–1
C–O
hydroxy, ester
1040–1300
C=C
aromatic compound, alkene
1500–1680
C=O
amide
carbonyl, carboxyl
ester
1640–1690
1670–1740
1710–1750
C≡N
nitrile
2200–2250
C–H
alkane
2850–2950
N–H
amine, amide
3300–3500
O–H
carboxyl
hydroxy
2500–3000
3200–3600
Use Fig. 5.2 and Table 5.3 to predict two differences in the absorptions above 1500 cm–1
of the infrared spectrum of D compared to E. Explain your answer.
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [2]
[Total: 12]
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15
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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21
20
19
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57–71
56
104
88
actinoids
lanthanoids
–
–
Ra
radium
Fr
francium
90
89
232.0
thorium
actinium
–
Th
Ac
140.1
cerium
138.9
lanthanum
59
231.0
protactinium
Pa
91
140.9
praseodymium
Pr
–
58
Ce
–
Db
dubnium
Rf
105
180.9
tantalum
73
Ta
92.9
niobium
Nb
41
50.9
vanadium
V
23
5
rutherfordium
La
57
actinoids
89–103
178.5
87
137.3
hafnium
132.9
barium
72
Hf
caesium
lanthanoids
Ba
55
91.2
zirconium
Zr
40
47.9
titanium
Ti
22
4
name
238.0
uranium
U
92
144.4
neodymium
60
Nd
–
Sg
seaborgium
106
183.8
tungsten
74
W
95.9
molybdenum
Mo
42
52.0
Cr
24
6
chromium
relative atomic mass
atomic number
Key
atomic symbol
Cs
88.9
yttrium
87.6
strontium
rubidium
85.5
Sr
Rb
Y
39
38
45.0
37
40.1
scandium
39.1
calcium
Ca
potassium
K
Sc
3
24.3
magnesium
23.0
sodium
12
Mg
Na
11
9.0
beryllium
lithium
6.9
Be
4
3
Li
2
1
–
neptunium
Np
93
–
promethium
61
Pm
–
Bh
bohrium
107
186.2
rhenium
75
Re
–
technetium
Tc
43
54.9
manganese
Mn
25
7
9
10
11
12
B
C
N
O
8
16
F
9
17
2
18
–
plutonium
Pu
94
150.4
samarium
62
Sm
–
Hs
hassium
108
190.2
osmium
76
Os
101.1
ruthenium
Ru
44
iron
55.8
Fe
26
8
1.0
–
americium
Am
95
152.0
europium
63
Eu
–
Mt
meitnerium
109
iridium
192.2
77
Ir
102.9
rhodium
Rh
45
58.9
cobalt
Co
27
–
curium
Cm
96
157.3
gadolinium
64
Gd
–
Ds
darmstadtium
110
195.1
platinum
78
Pt
106.4
palladium
Pd
46
58.7
nickel
Ni
28
–
berkelium
Bk
97
158.9
terbium
65
Tb
–
Rg
roentgenium
111
gold
197.0
79
Au
silver
107.9
Ag
47
63.5
copper
Cu
29
–
californium
Cf
98
162.5
dysprosium
66
Dy
–
Cn
copernicium
112
200.6
mercury
80
Hg
112.4
cadmium
Cd
48
zinc
65.4
Zn
30
–
einsteinium
Es
99
164.9
holmium
67
Ho
–
Nh
nihonium
113
204.4
thallium
81
Tl
114.8
indium
In
49
69.7
gallium
Ga
31
27.0
aluminium
13
Al
10.8
boron
–
fermium
Fm
100
167.3
erbium
68
Er
–
Fl
flerovium
114
lead
207.2
82
Pb
tin
118.7
Sn
50
72.6
germanium
Ge
32
28.1
silicon
14
Si
12.0
carbon
–
mendelevium
Md
101
168.9
thulium
69
Tm
–
Mc
moscovium
115
209.0
bismuth
83
Bi
121.8
antimony
Sb
51
74.9
arsenic
As
33
31.0
phosphorus
P
15
14.0
nitrogen
–
nobelium
No
102
173.1
ytterbium
70
Yb
–
Lv
livermorium
116
–
polonium
84
Po
127.6
tellurium
Te
52
79.0
selenium
Se
34
32.1
sulfur
S
16
16.0
oxygen
–
Lr
lawrencium
103
175.0
lutetium
71
Lu
–
Ts
tennessine
117
–
astatine
85
At
iodine
126.9
I
53
79.9
bromine
Br
35
35.5
chlorine
17
Cl
19.0
fluorine
–
oganesson
Og
–
118
radon
86
Rn
xenon
131.3
54
Xe
83.8
krypton
36
Kr
39.9
argon
18
Ar
neon
20.2
10
Ne
4.0
helium
7
15
hydrogen
6
14
He
5
13
H
1
Group
The Periodic Table of Elements
16
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge International AS & A Level
* 5 1 5 4 5 0 8 9 5 9 *
CHEMISTRY
9701/22
Paper 2 AS Level Structured Questions
October/November 2023
1 hour 15 minutes
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●
Answer all questions.
●
Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●
Write your name, centre number and candidate number in the boxes at the top of the page.
●
Write your answer to each question in the space provided.
●
Do not use an erasable pen or correction fluid.
●
Do not write on any bar codes.
●
You may use a calculator.
●
You should show all your working and use appropriate units.
INFORMATION
●
The total mark for this paper is 60.
●
The number of marks for each question or part question is shown in brackets [ ].
●
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.
DC (LK/SG) 308426/4
© UCLES 2023
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1
The elements silicon, phosphorus and sulfur are in Period 3 of the Periodic Table.
(a) (i)
Describe the variation in atomic radius from silicon to sulfur.
..................................................................................................................................... [1]
(ii)
The melting point of silicon is 1410 °C. The melting point of sulfur is 113 °C.
Explain this difference.
...........................................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [3]
(b) Table 1.1 shows some properties of the elements Si to S.
The first ionisation energy of P is not shown.
Table 1.1
property
Si
P
S
total number of electrons in s subshells
total number of electrons in p subshells
(i)
first ionisation energy / kJ mol–1
786
formula of most common chloride
SiCl 4
1000
PCl 5
SCl 2
Complete Table 1.1 to show the total number of s and p electrons in an atom of Si, P
and S.
[2]
(ii)
Construct an equation to represent the first ionisation energy of Si.
..................................................................................................................................... [1]
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(iii)
Three possible values for the first ionisation energy of P are given.
619 kJ mol–1
893 kJ mol–1
1060 kJ mol–1
Circle the correct value.
Explain your choice, including a comparison of your chosen value to those of Si and S.
...........................................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [4]
(iv)
SiCl 4 and PCl 5 each react with water, forming misty fumes.
Identify the chemical responsible for the misty fumes.
..................................................................................................................................... [1]
(v)
Predict the shape of the SCl 2 molecule.
..................................................................................................................................... [1]
[Total: 13]
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2
NO and NO2 react at 25 °C to give N2O3 as shown in the equation.
NO(g) + NO2(g)
N2O3(g)
ΔH = –7.2 kJ mol–1
The reaction is reversible and reaches equilibrium in a closed system.
(a) Fig. 2.1 shows how the rate of the forward reaction changes with time.
Initially, the rate of the reverse reaction is zero.
Complete Fig. 2.1 to sketch how the rate of the reverse reaction changes with time.
rate of
reaction
time
Fig. 2.1
[1]
(b) State how the position of equilibrium changes, if at all, when the reaction takes place at
100 °C.
Explain your answer.
Assume the pressure remains constant.
...................................................................................................................................................
...................................................................................................................................................
...................................................................................................................................................
............................................................................................................................................. [2]
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(c) Table 2.1 shows the composition of an equilibrium mixture of NO(g), NO2(g) and N2O3(g) at
101 kPa.
Table 2.1
gas
number of moles at
equilibrium / mol
NO
0.605
NO2
0.605
N2O3
0.390
Calculate Kp , the equilibrium constant with respect to partial pressures.
Deduce the units of Kp.
Kp = ..................................... units .......................................
[3]
(d) Identify one natural process and one man-made process that cause the formation of
atmospheric NO and NO2.
natural process .........................................................................................................................
man-made process ....................................................................................................................
[2]
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(e) NO2 is a brown gas that can be used to form nitric acid.
(i)
NO2 is a free radical.
Define free radical.
..................................................................................................................................... [1]
(ii)
NO2 has a catalytic role in the oxidation of atmospheric sulfur dioxide.
Write equations to show the catalytic role of NO2 in this oxidation.
...........................................................................................................................................
..................................................................................................................................... [2]
(iii)
State one environmental consequence of the oxidation of atmospheric sulfur dioxide.
..................................................................................................................................... [1]
(f)
A student titrates nitric acid with a base to form a solution containing aqueous magnesium
nitrate.
(i)
Identify a base that the student could use.
..................................................................................................................................... [1]
(ii)
The student evaporates the water to obtain magnesium nitrate solid. When this solid is
heated it decomposes.
Write an equation for the decomposition of magnesium nitrate.
..................................................................................................................................... [1]
(iii)
State how the thermal stability of Group 2 nitrates changes down the group.
..................................................................................................................................... [1]
[Total: 15]
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3
Phosphoric(V) acid, H3PO4, is used in both inorganic and organic reactions.
(a) H3PO4 is made in a two-step process from phosphorus.
(i)
step 1
Phosphorus reacts with an excess of oxygen to form a white solid.
step 2
The white solid then reacts with water to form H3PO4.
Write an equation for each step.
step 1 ................................................................................................................................
step 2 ................................................................................................................................
[2]
(ii)
H3PO4 is a weak Brønsted–Lowry acid.
Define weak Brønsted–Lowry acid.
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [2]
(b) H3PO4 is also formed in the process shown in reaction 1.
4H3PO3
reaction 1
3H3PO4 + PH3
Table 3.1 shows some relevant thermodynamic data.
Table 3.1
(i)
compound
enthalpy change of formation,
ΔHf / kJ mol–1
H3PO3
–972
H3PO4
–1281
PH3
+9
Define enthalpy change of formation.
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [2]
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(ii)
Use the data in Table 3.1 to calculate the enthalpy change, ΔH r , of reaction 1.
ΔH r = ................................................. kJ mol–1
[2]
(iii)
Explain why reaction 1 is a disproportionation reaction.
Explain your reasoning with reference to relevant oxidation numbers.
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [2]
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(c) Fig. 3.1 shows a reaction scheme that involves H3PO4 in several reactions.
OH
reaction 2
oxidation
O
A and H3PO4
KBr and H3PO4
B
reaction 3
CH3COOH
and H3PO4
O
O
Fig. 3.1
(i)
Identify A, which reacts with propene in the presence of H3PO4 in reaction 2.
..................................................................................................................................... [1]
(ii)
Draw the structure of B.
[1]
(iii)
Name the type of reaction that occurs in reaction 3.
..................................................................................................................................... [1]
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(iv)
Reaction 3 is monitored using infrared spectroscopy. It is not possible to use the O—H
absorption frequency to monitor the reaction.
Use Table 3.2 to identify a suitable bond whose absorption frequency can be used to
monitor the progress of reaction 3.
State the change you would see in the infrared spectrum during reaction 3.
bond ..................................................................................................................................
change in infrared spectrum ..............................................................................................
...........................................................................................................................................
[2]
Table 3.2
characteristic infrared absorption range
(in wavenumbers) / cm–1
bond
functional groups containing the bond
C–O
hydroxy, ester
1040–1300
C=C
aromatic compound, alkene
1500–1680
C=O
amide
carbonyl, carboxyl
ester
1640–1690
1670–1740
1710–1750
C–H
alkane
2850–2950
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(d) H3PO4 also reacts with alcohols to form organophosphates.
Organophosphates are compounds similar to esters. They have the general structure shown
in Fig. 3.2.
O
R
P
O
O
R
O
R
R = alkyl group
Fig. 3.2
(i)
Complete the equation to suggest the products of the reaction of H3PO4 with methanol,
CH3OH.
H3PO4 + 3CH3OH
(ii)
.................................................................................................. [1]
Compound T is a simple organophosphate.
The mass spectrum of T shows a molecular ion peak at m / e = 182. This peak has a
relative intensity of 12.7.
The relative intensity of the M +1 peak is 0.84.
Deduce the number of carbon atoms in T.
Hence suggest the molecular formula of T.
Assume that phosphorus and oxygen exist as single isotopes.
Show your working.
number of carbon atoms in T = .............................................
molecular formula of T = .......................................................
[3]
[Total: 19]
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4
Lactic acid, CH3CH(OH)COOH, and pyruvic acid, CH3COCOOH, both contain two functional
groups.
lactic acid
H
H 3C
C
O
pyruvic acid
O
H 3C
O
C
C
H
O
O
C
O
H
H
Fig. 4.1
(a) (i)
Explain why lactic acid exists as optical isomers.
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [1]
(ii)
Give the systematic name of lactic acid.
..................................................................................................................................... [1]
(iii)
Lactic acid forms hydrogen bonds with water.
Complete Fig. 4.2 to show the formation of a hydrogen bond between one molecule of
lactic acid and one molecule of water.
Label the hydrogen bond. Show any relevant dipoles and lone pairs of electrons.
H
H 3C
C
O
C
O
O
H
H
Fig. 4.2
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(b) Two possible syntheses of pyruvic acid are shown in Fig. 4.3 and Fig. 4.4.
Each synthesis has a total of three steps.
propene
Br2
first step
[O]
pyruvic acid
third step
CH3COCOOH
lactic acid
[O]
pyruvic acid
CH3CH(OH)COOH
third step
CH3COCOOH
Br
Br
second step
Fig. 4.3
ethanal
O
first step
second step
Fig. 4.4
(i)
Complete the diagram in Fig. 4.5 to show the mechanism for the reaction of propene
with Br2.
Include charges, dipoles, lone pairs of electrons and curly arrows, as appropriate.
Br
Br
Br
Br
Fig. 4.5
(ii)
[3]
Write an equation for the oxidation of lactic acid to pyruvic acid, the third step of Fig. 4.4.
Use [O] to represent one atom of oxygen from an oxidising agent.
CH3CH(OH)COOH + ................................................................................................... [1]
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(iii)
Complete Table 4.1 to give details of the reagents and conditions used in each of the two
syntheses shown in Fig. 4.3 and Fig. 4.4.
Table 4.1
synthesis from propene
(shown in Fig. 4.3)
first step
reagents and
conditions used
synthesis from ethanal
(shown in Fig. 4.4)
Br2
second step
third step
[4]
[Total: 13]
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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 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)
© UCLES 2023
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20
19
9701/22/O/N/23
57–71
56
104
88
actinoids
lanthanoids
–
–
Ra
radium
Fr
francium
90
89
232.0
thorium
actinium
–
Th
Ac
140.1
cerium
138.9
lanthanum
59
231.0
protactinium
Pa
91
140.9
praseodymium
Pr
–
58
Ce
–
Db
dubnium
Rf
105
180.9
tantalum
73
Ta
92.9
niobium
Nb
41
50.9
vanadium
V
23
5
rutherfordium
La
57
actinoids
89–103
178.5
87
137.3
hafnium
132.9
barium
72
Hf
caesium
lanthanoids
Ba
55
91.2
zirconium
Zr
40
47.9
titanium
Ti
22
4
name
238.0
uranium
U
92
144.4
neodymium
60
Nd
–
Sg
seaborgium
106
183.8
tungsten
74
W
95.9
molybdenum
Mo
42
52.0
Cr
24
6
chromium
relative atomic mass
atomic number
Key
atomic symbol
Cs
88.9
yttrium
87.6
strontium
rubidium
85.5
Sr
Rb
Y
39
38
45.0
37
40.1
scandium
39.1
calcium
Ca
potassium
K
Sc
3
24.3
magnesium
23.0
sodium
12
Mg
Na
11
9.0
beryllium
lithium
6.9
Be
4
3
Li
2
1
–
neptunium
Np
93
–
promethium
61
Pm
–
Bh
bohrium
107
186.2
rhenium
75
Re
–
technetium
Tc
43
54.9
manganese
Mn
25
7
9
10
11
12
B
C
N
O
8
16
F
9
17
2
18
–
plutonium
Pu
94
150.4
samarium
62
Sm
–
Hs
hassium
108
190.2
osmium
76
Os
101.1
ruthenium
Ru
44
iron
55.8
Fe
26
8
1.0
–
americium
Am
95
152.0
europium
63
Eu
–
Mt
meitnerium
109
iridium
192.2
77
Ir
102.9
rhodium
Rh
45
58.9
cobalt
Co
27
–
curium
Cm
96
157.3
gadolinium
64
Gd
–
Ds
darmstadtium
110
195.1
platinum
78
Pt
106.4
palladium
Pd
46
58.7
nickel
Ni
28
–
berkelium
Bk
97
158.9
terbium
65
Tb
–
Rg
roentgenium
111
gold
197.0
79
Au
silver
107.9
Ag
47
63.5
copper
Cu
29
–
californium
Cf
98
162.5
dysprosium
66
Dy
–
Cn
copernicium
112
200.6
mercury
80
Hg
112.4
cadmium
Cd
48
zinc
65.4
Zn
30
–
einsteinium
Es
99
164.9
holmium
67
Ho
–
Nh
nihonium
113
204.4
thallium
81
Tl
114.8
indium
In
49
69.7
gallium
Ga
31
27.0
aluminium
13
Al
10.8
boron
–
fermium
Fm
100
167.3
erbium
68
Er
–
Fl
flerovium
114
lead
207.2
82
Pb
tin
118.7
Sn
50
72.6
germanium
Ge
32
28.1
silicon
14
Si
12.0
carbon
–
mendelevium
Md
101
168.9
thulium
69
Tm
–
Mc
moscovium
115
209.0
bismuth
83
Bi
121.8
antimony
Sb
51
74.9
arsenic
As
33
31.0
phosphorus
P
15
14.0
nitrogen
–
nobelium
No
102
173.1
ytterbium
70
Yb
–
Lv
livermorium
116
–
polonium
84
Po
127.6
tellurium
Te
52
79.0
selenium
Se
34
32.1
sulfur
S
16
16.0
oxygen
–
Lr
lawrencium
103
175.0
lutetium
71
Lu
–
Ts
tennessine
117
–
astatine
85
At
iodine
126.9
I
53
79.9
bromine
Br
35
35.5
chlorine
17
Cl
19.0
fluorine
–
oganesson
Og
–
118
radon
86
Rn
xenon
131.3
54
Xe
83.8
krypton
36
Kr
39.9
argon
18
Ar
neon
20.2
10
Ne
4.0
helium
7
15
hydrogen
6
14
He
5
13
H
1
Group
The Periodic Table of Elements
20
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
Cambridge International AS & A Level
* 6 8 4 0 7 5 2 3 0 5 *
CHEMISTRY
9701/22
Paper 2 AS Level Structured Questions
February/March 2024
1 hour 15 minutes
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●
Answer all questions.
●
Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●
Write your name, centre number and candidate number in the boxes at the top of the page.
●
Write your answer to each question in the space provided.
●
Do not use an erasable pen or correction fluid.
●
Do not write on any bar codes.
●
You may use a calculator.
●
You should show all your working and use appropriate units.
INFORMATION
●
The total mark for this paper is 60.
●
The number of marks for each question or part question is shown in brackets [ ].
●
The Periodic Table is printed in the question paper.
●
Important values, constants and standards are printed in the question paper.
This document has 16 pages. Any blank pages are indicated.
DC (LK/SG) 347696/6
© UCLES 2024
[Turn over
2
1
Bismuth is an element in Group 15 of the Periodic Table.
(a) Bismuth has metallic bonding.
Draw a labelled diagram to show the metallic bonding in bismuth.
[1]
(b) Bismuth reduces water to form bismuth oxide, Bi2O3. A colourless gas that ignites with a
squeaky pop also forms.
(i)
Construct an equation for the reduction of water by bismuth.
..................................................................................................................................... [1]
(ii)
Bi2O3 is a yellow insoluble solid that melts at 1090 K. The molten compound conducts
electricity.
Deduce the structure and bonding of Bi2O3. Explain your answer.
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [2]
(c) Bi2O3 can be used to form NaBiO3, as shown in equation 1.
equation 1
(i)
Na2O + Bi2O3 + O2
2NaBiO3
Deduce the oxidation number of Bi in Bi2O3 and in NaBiO3.
oxidation number of Bi:
in Bi2O3 ................................................. in NaBiO3 ...........................................................
[1]
(ii)
Identify the reducing agent in equation 1.
..................................................................................................................................... [1]
© UCLES 2024
9701/22/F/M/24
3
(d) NaBiO3 is an oxidising agent with similar properties to KMnO4.
Fig. 1.1 shows an example of the use of NaBiO3 as an oxidising agent.
X
Y
Z
OH
O
NaBiO3
+
O
OH
H
Fig. 1.1
(i)
Explain the term oxidising agent.
...........................................................................................................................................
..................................................................................................................................... [1]
(ii)
Compound X forms when methylbut-2-ene reacts with KMnO4.
State the essential conditions for this reaction.
..................................................................................................................................... [1]
(iii)
Complete Table 1.1 to show what is observed when compounds Y and Z react separately
with the named reagents.
Table 1.1
reagent
observation with Y
Na2CO3(aq)
no reaction
observation with Z
alkaline I2(aq)
2,4-dinitrophenylhydrazine
(2,4-DNPH)
Tollens’ reagent
[4]
(iv)
Construct an equation for the reaction of Z with NaBH4.
Use [H] to represent an atom of hydrogen from the reducing agent.
..................................................................................................................................... [1]
© UCLES 2024
9701/22/F/M/24
[Turn over
4
(e) NaBiO3 can be used to determine the concentration of Mn2+(aq). The ionic equation for the
reaction is shown in equation 2.
equation 2
2Mn2+ + 5BiO3– + 14H+
2MnO4– + 5Bi3+ + 7H2O
A student uses the following procedure in an experiment.
•
•
•
Add 100.0 cm3 of a saturated solution of Mn2+(aq) to a volumetric flask.
Add distilled water to the flask to make a 1.00 dm3 diluted solution.
Titrate a 25.00 cm3 sample of the diluted solution with 0.100 mol dm–3 NaBiO3(aq).
The 25.00 cm3 sample of the diluted solution of Mn2+(aq) reacts completely with exactly
21.50 cm3 of 0.100 mol dm–3 NaBiO3(aq).
Calculate the concentration, in mol dm–3, of Mn2+(aq) in the saturated solution.
Show your working.
concentration of Mn2+(aq) in the saturated solution = ......................................... mol dm–3 [3]
[Total: 16]
© UCLES 2024
9701/22/F/M/24
5
2
Chlorine, Cl 2, reacts with many elements and compounds to form chlorides.
Table 2.1 shows information about some chlorides of Period 3 elements.
Table 2.1
Na
Mg
Si
formula of chloride
structure of chloride
giant
bonding of chloride
covalent
pH of solution formed
on addition of
chloride to water
6.2
(a) Complete Table 2.1.
[3]
(b) When Cl 2 reacts with cold NaOH(aq), Cl 2 is both oxidised and reduced. The products are
NaCl, water and G.
(i)
State the type of redox reaction in which the same species is both oxidised and reduced.
..................................................................................................................................... [1]
(ii)
Identify G.
..................................................................................................................................... [1]
(iii)
Write an equation for the reaction between Cl2 and hot NaOH(aq).
..................................................................................................................................... [1]
(iv)
Describe fully what is observed when AgNO3(aq) is added to the aqueous solution of the
chloride of sodium, followed by dilute NH3(aq).
...........................................................................................................................................
..................................................................................................................................... [2]
© UCLES 2024
9701/22/F/M/24
[Turn over
6
(c) An excess of Cl 2 reacts with phosphorus to form PCl 5.
(i)
PCl 5 is a simple molecule in the gas phase.
It also exists in a solid form as two ions, PCl4+ and PCl 6–.
Complete Table 2.2 to identify the shapes of each of these species.
Table 2.2
species
PCl4+
PCl5
shape
PCl6–
tetrahedral
[2]
(ii)
PCl5 reacts with J to form H3PO4.
Identify J and state the type of reaction.
J ................................. type of reaction .............................................................................
[2]
© UCLES 2024
9701/22/F/M/24
7
(d) Cl 2 reacts readily with propene to form K, 1,2-dichloropropane.
K can be used to form L.
propene
Cl2
K
L
Cl
Cl
reaction 2
reaction 1
Cl
Fig. 2.1
(i)
Complete Fig. 2.2 to show the mechanism for the reaction of Cl 2 with propene in
reaction 1.
Include charges, dipoles, lone pairs of electrons and curly arrows, as appropriate.
H
H
C
C
H
H
CH3
H
H
C
C
CH3
Cl Cl
Cl
Cl
Fig. 2.2
(ii)
[4]
Identify the reagent and conditions for reaction 2.
..................................................................................................................................... [1]
(iii)
Draw one repeat unit of the addition polymer that forms from L.
[1]
[Total: 18]
© UCLES 2024
9701/22/F/M/24
[Turn over
8
3
Nitrogen, N2, is generally an unreactive molecule but it does react under certain conditions.
(a) Give two reasons to explain the lack of reactivity of nitrogen.
1 ................................................................................................................................................
2 ................................................................................................................................................
[2]
(b) N2 can react with oxygen in an internal combustion engine to form a mixture of NO and NO2.
Fig. 3.1 shows a reaction scheme involving N2.
reaction 1
N2
reaction 2
NO2
reaction 3
NO2
O2
H 2O
unburned hydrocarbons
NO and NO2
products
peroxyacetyl nitrate (PAN)
Fig. 3.1
(i)
Write an equation to show the formation of a mixture of NO and NO2 in reaction 1.
..................................................................................................................................... [1]
(ii)
Give the formulae of the products of reaction 2.
..................................................................................................................................... [1]
(iii)
State one environmental consequence of reaction 3.
..................................................................................................................................... [1]
© UCLES 2024
9701/22/F/M/24
9
(c) The Haber process involves the reaction of N2 and H2 to form ammonia, NH3.
A catalyst is used, which allows the process to be carried out at a lower temperature and
pressure.
N2(g) + 3H2(g)
(i)
2NH3(g)
ΔH = –92 kJ mol–1
Use the information in (c) to complete Table 3.1.
Table 3.1
compound
enthalpy change of
formation, ΔHf / kJ mol–1
N2
H2
NH3
(ii)
[2]
Explain how the presence of a catalyst affects the reaction.
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [1]
(iii)
State and explain the effect, if any, on the rate of the Haber process as the pressure is
lowered.
...........................................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [2]
© UCLES 2024
9701/22/F/M/24
[Turn over
10
(d) The N2F2 molecule has a double covalent bond between its nitrogen atoms. This consists of
a σ and a π bond.
(i)
Complete Fig. 3.2 to show the dot-and-cross diagram for N2F2.
Show outer electrons only.
F
N
N
Fig. 3.2
(ii)
F
[2]
Deduce the hybridisation of the N atoms in N2F2.
..................................................................................................................................... [1]
(iii)
Draw a diagram of the π bond between the N atoms in N2F2 and describe how it
forms.
...........................................................................................................................................
...........................................................................................................................................
[2]
[Total: 15]
© UCLES 2024
9701/22/F/M/24
11
4
Compound S is used in food flavourings. A possible synthesis of S is shown in Fig. 4.1.
P
S
R
HBr
reaction 1
Q
H+(aq)
KCN in ethanol
reaction 2
reaction 3
CN
COOH
Fig. 4.1
(a) P, Q, R and S show stereoisomerism.
Complete Table 4.1 by identifying with a tick (3) the type of stereoisomerism that each
molecule shows.
The type of stereoisomerism shown by Q is given.
Table 4.1
P
Q
R
S
geometrical
isomerism
optical
isomerism
3
[2]
(b) (i)
Give the structural formula of Q.
..................................................................................................................................... [1]
(ii)
Name the mechanism in reaction 2.
..................................................................................................................................... [1]
(iii)
Complete the equation for reaction 3. R is represented as C4H9CN.
C4H9CN + .................................................................................................................... [1]
© UCLES 2024
9701/22/F/M/24
[Turn over
12
(c) Compounds S and T react to form organic compound U, which has a single functional group.
S
+
T
U
+
H2 O
COOH
Table 4.2 shows some data from the mass spectrum of U.
Table 4.2
(i)
peak
relative abundance
M+
7.2
[M+1]+
0.55
Use the data from Table 4.2 to show that U contains 7 carbon atoms.
Show your working.
[2]
(ii)
Fig. 4.2 shows the infrared spectrum of U.
100
80
60
transmittance / %
40
20
0
4000
3000
2000
1500
wavenumber / cm–1
Fig. 4.2
© UCLES 2024
9701/22/F/M/24
1000
500
13
Table 4.3
bond
functional groups containing the bond
characteristic infrared absorption
range (in wavenumbers) / cm–1
C–O
hydroxy, ester
1040–1300
C=C
aromatic compound, alkene
1500–1680
C=O
amide
carbonyl, carboxyl
ester
1640–1690
1670–1740
1710–1750
C≡N
nitrile
2200–2250
C–H
alkane
2850–2950
N–H
amine, amide
3300–3500
O–H
carboxyl
hydroxy
2500–3000
3200–3650
Use Fig. 4.2 and Table 4.3 to identify the functional group present in U.
Explain your answer fully.
functional group .................................................................................................................
explanation ........................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
[2]
(iii)
T also has a single functional group.
Use the information in (c)(i) and your answer to (c)(ii) to identify T and U.
Draw the structures of T and U in the boxes.
T
U
[2]
[Total: 11]
© UCLES 2024
9701/22/F/M/24
14
BLANK PAGE
© UCLES 2024
9701/22/F/M/24
15
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)
© UCLES 2024
9701/22/F/M/24
© UCLES 2024
39
38
9701/22/F/M/24
57–71
Fr
Ra
actinoids
–
radium
lanthanoids
–
francium
90
89
–
actinium
Ac
232.0
thorium
Th
140.1
cerium
138.9
231.0
protactinium
Pa
91
140.9
praseodymium
Pr
–
59
Ce
–
58
Db
dubnium
Rf
105
180.9
tantalum
73
Ta
92.9
niobium
Nb
41
50.9
vanadium
V
23
5
rutherfordium
lanthanum
57
La
actinoids
104
89–103
178.5
88
137.3
87
132.9
hafnium
72
Hf
91.2
zirconium
Zr
barium
lanthanoids
88.9
56
Ba
87.6
yttrium
Y
strontium
Sr
40
47.9
titanium
Ti
22
4
Cr
24
6
Sg
238.0
uranium
U
92
144.2
neodymium
60
Nd
–
seaborgium
106
183.8
tungsten
74
W
95.9
molybdenum
Mo
42
52.0
chromium
relative atomic mass
name
atomic number
Key
atomic symbol
caesium
Cs
55
85.5
rubidium
Rb
45.0
37
40.1
scandium
39.1
calcium
Ca
potassium
K
Sc
21
20
19
24.3
3
23.0
magnesium
Mg
12
9.0
beryllium
sodium
Na
11
6.9
lithium
Be
4
3
Li
2
1
Bh
–
neptunium
Np
93
–
promethium
61
Pm
–
bohrium
107
186.2
rhenium
75
Re
–
technetium
Tc
43
54.9
manganese
Mn
25
7
Hs
–
plutonium
Pu
94
150.4
samarium
62
Sm
–
hassium
108
190.2
osmium
76
Os
101.1
ruthenium
Ru
44
55.8
iron
Fe
26
8
1.0
hydrogen
H
1
Mt
–
americium
Am
95
152.0
europium
63
Eu
–
meitnerium
109
iridium
192.2
77
Ir
102.9
rhodium
Rh
45
58.9
cobalt
Co
27
9
Ni
28
10
Ds
–
curium
Cm
96
157.3
gadolinium
64
Gd
–
darmstadtium
110
195.1
platinum
78
Pt
106.4
palladium
Pd
46
58.7
nickel
Group
Rg
–
berkelium
Bk
97
158.9
terbium
65
Tb
–
roentgenium
111
197.0
gold
79
Au
107.9
silver
Ag
47
63.5
copper
Cu
29
11
The Periodic Table of Elements
Cn
–
californium
Cf
98
162.5
dysprosium
66
Dy
–
copernicium
112
200.6
mercury
80
Hg
112.4
cadmium
Cd
48
65.4
zinc
Zn
30
12
Nh
–
einsteinium
Es
99
164.9
holmium
67
Ho
–
nihonium
113
204.4
thallium
81
Tl
114.8
indium
In
49
69.7
gallium
Ga
31
27.0
aluminium
13
Al
10.8
boron
B
5
13
Fl
–
fermium
Fm
100
167.3
erbium
68
Er
–
flerovium
114
207.2
lead
82
Pb
118.7
tin
Sn
50
72.6
germanium
Ge
32
28.1
silicon
14
Si
12.0
carbon
C
6
14
Mc
–
mendelevium
Md
101
168.9
thulium
69
Tm
–
moscovium
115
209.0
bismuth
83
Bi
121.8
antimony
Sb
51
74.9
arsenic
As
33
31.0
phosphorus
P
15
14.0
nitrogen
N
7
15
Lv
–
nobelium
No
102
173.1
ytterbium
70
Yb
–
livermorium
116
–
polonium
84
Po
127.6
tellurium
Te
52
79.0
selenium
Se
34
32.1
sulfur
S
16
16.0
oxygen
O
8
16
Ts
Lr
–
lawrencium
103
175.0
lutetium
71
Lu
–
tennessine
117
–
astatine
85
At
iodine
126.9
I
53
79.9
bromine
Br
35
35.5
chlorine
17
Cl
19.0
fluorine
F
9
17
Og
–
oganesson
118
–
radon
86
Rn
131.3
xenon
54
Xe
83.8
krypton
36
Kr
39.9
argon
18
Ar
20.2
neon
10
Ne
4.0
helium
He
2
18
16
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
* 0019655306501 *
,
,
Cambridge International AS & A Level
¬OŠ. 3mG{YMª6zU W
¬œx`@¤;xhxI˜Pt‰4‚
¥•E•5•¥u¥5 • E¥e5U
* 9 2 1 8 2 8 8 7 5 9 *
CHEMISTRY
9701/22
Paper 2 AS Level Structured Questions
May/June 2024
1 hour 15 minutes
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●
Answer all questions.
●
Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●
Write your name, centre number and candidate number in the boxes at the top of the page.
●
Write your answer to each question in the space provided.
●
Do not use an erasable pen or correction fluid.
●
Do not write on any bar codes.
●
You may use a calculator.
●
You should show all your working and use appropriate units.
INFORMATION
●
The total mark for this paper is 60.
●
The number of marks for each question or part question is shown in brackets [ ].
●
The Periodic Table is printed in the question paper.
●
Important values, constants and standards are printed in the question paper.
This document has 16 pages. Any blank pages are indicated.
DC (PQ/SW) 324893/3
© UCLES 2024
[Turn over
2
,
1
,
(a) Complete Table 1.1 using relevant information from the Periodic Table.
Table 1.1
nucleon number
Mg2+
24
Al 3+
27
proton number
number of electrons
[2]
(b) State and explain the difference in the ionic radius of Al 3+ compared to Mg2+.
...................................................................................................................................................
...................................................................................................................................................
...................................................................................................................................................
............................................................................................................................................. [3]
DO NOT WRITE IN THIS MARGIN
DO NOT WRITE IN THIS MARGIN
* 0019655306502 *
DO NOT WRITE IN THIS MARGIN
(c) Draw a labelled diagram to show the structure and bonding in sodium.
2500
melting
point / K
2000
1500
1000
500
0
Na Mg
Al
Si
element
Fig. 1.1
© UCLES 2024
ĬÍĊ®Ġ³íÇûÙāÍĪ·ü×Ğ×
ĬĜöß½Ĩ¯ĒÏòĂæàæı¼Ă
ĥÅÕĕõõåĕÕõÕÕąąąĥĕÕ
9701/22/M/J/24
P
S
Cl
DO NOT WRITE IN THIS MARGIN
(d) Fig. 1.1 shows the variation in melting point of some Period 3 elements in their standard
states at room temperature and pressure.
DO NOT WRITE IN THIS MARGIN
[1]
DO NOT WRITE IN THIS MARGIN
* 0019655306503 *
3
,
,
(i)
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [1]
(ii)
Complete Fig. 1.1 to show the variation in the melting points of the elements P, S and Cl.
[2]
(e) Two Period 3 elements react with an excess of oxygen at room pressure.
(i)
Complete Table 1.2.
Table 1.2
1
2
3
Period 3 element
state of oxide at
room temperature and
pressure
approximate pH of
solution made when
oxide is added to water
Na
DO NOT WRITE IN THIS MARGIN
DO NOT WRITE IN THIS MARGIN
Explain why Si has a high melting point.
S
[2]
(ii)
The solutions made in column 3 of Table 1.2 are mixed together.
Name the type of reaction that occurs.
..................................................................................................................................... [1]
(iii)
Write an equation to describe the reaction between P4O10 and an excess of water.
DO NOT WRITE IN THIS MARGIN
DO NOT WRITE IN THIS MARGIN
..................................................................................................................................... [1]
(f)
Aluminium hydroxide is amphoteric.
(i)
Explain what is meant by amphoteric.
...........................................................................................................................................
..................................................................................................................................... [1]
(ii)
Write an equation to describe the reaction that occurs when aluminium hydroxide,
Al (OH)3, reacts with NaOH(aq).
..................................................................................................................................... [1]
[Total: 15]
© UCLES 2024
ĬÏĊ®Ġ³íÇûÙāÍĪ·ú×Ğ×
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9701/22/M/J/24
[Turn over
4
Separate samples of Na2CO3 and NaHCO3 react with HCl (aq) to produce the same products, as
shown in Table 2.1.
Table 2.1
∆H / kJ mol–1
1
Na2CO3 + 2HCl
2NaCl + H2O + CO2
∆H1
2
NaHCO3 + HCl
NaCl + H2O + CO2
∆H2 = +27.2
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equation
(a) Complete the reaction pathway diagram in Fig. 2.1 for reaction 2.
Label the diagram to show the enthalpy change, ∆H2, and the activation energy, EA.
energy
/ kJ mol–1
NaHCO3 + HCl
progress of reaction
Fig. 2.1
[2]
(b) The value for ∆H1 is determined by experiment using the following method.
•
•
•
•
50.0 cm3 of 2.00 mol dm–3 HCl (aq) is added to a polystyrene cup.
The initial temperature of the acid is recorded as 19.6 °C.
0.0400 mol of Na2CO3 is added and the mixture is stirred.
All the solid Na2CO3 disappears and a colourless solution is produced.
The maximum temperature recorded during the reaction is 26.2 °C.
(i)
Describe one other observation that shows the reaction is complete.
..................................................................................................................................... [1]
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reaction
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2
,
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* 0019655306504 *
5
,
,
(ii)
Calculate the value of ∆H1 in kJ mol–1.
Assume the specific heat capacity of the reaction mixture is the same as for water and
no heat is lost to the surroundings.
Show your working.
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* 0019655306505 *
∆H1 = .............................. kJ mol–1 [3]
(iii)
reaction 3
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Thermal decomposition occurs when NaHCO3 is heated.
2NaHCO3
Na2CO3 + H2O + CO2
Calculate the enthalpy change for reaction 3, ∆Hr , using the data in Table 2.1 and the
value of ∆H1 calculated in (b)(ii).
(If you were unable to calculate a value for ∆H1 in (b)(ii), assume the enthalpy change is
–38.4 kJ mol–1. This is not the correct value.)
∆Hr = .............................. kJ mol–1 [2]
(c) Z is a salt that contains a Period 4 element from Group 2. When Z is heated brown gas forms.
Identify the formula of Z and use it to write an equation for the reaction.
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............................................................................................................................................. [2]
[Total: 10]
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9701/22/M/J/24
[Turn over
6
,
3
,
(a) Describe what is meant by dynamic equilibrium.
...................................................................................................................................................
...................................................................................................................................................
............................................................................................................................................. [2]
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* 0019655306506 *
Fe3+(aq) + SCN–(aq)
reaction 4
yellow
FeSCN2+(aq)
colourless
red
An equilibrium mixture contains Fe3+(aq), SCN–(aq) and FeSCN2+(aq). A few colourless
crystals of soluble KSCN(s) are added. The mixture is then left until it reaches equilibrium
again. The temperature of both equilibrium mixtures is the same.
Deduce the changes that occur, if any, in the equilibrium mixture after KSCN(s) is added
compared to the original equilibrium mixture.
•
change in appearance
....................................................................................................................................
•
change in relative concentration of Fe3+(aq)
....................................................................................................................................
•
change in value of the equilibrium constant, Kc
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[3]
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(i)
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(b) Reaction 4 describes the reversible reaction between yellow Fe3+(aq) and colourless
SCN–(aq) to produce red FeSCN2+(aq).
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* 0019655306507 *
7
,
(ii)
,
The expression for the equilibrium constant, Kc, for reaction 4 is shown.
Kc =
[FeSCN2+(aq)]
[Fe3+(aq)] × [SCN–(aq)]
5.00 × 10–5 mol of Fe3+(aq) and 5.00 × 10–5 mol of SCN–(aq) are added together and
allowed to reach equilibrium. The total volume of the mixture is 25.0 cm3.
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At equilibrium the concentration of FeSCN2+(aq) is 4.23 × 10–4 mol dm–3.
Calculate the equilibrium constant, Kc, for reaction 4.
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Include the units in your answer.
Kc = ..............................
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units ..............................
[4]
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8
,
(c) Determine the full electronic configuration of Fe3+.
............................................................................................................................................. [1]
(d) SCN–(aq) is colourless.
Complete the dot-and-cross diagram in Fig. 3.1 to show the arrangement of outer electrons in
an SCN– ion.
S
C
Fig. 3.1
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–
N
[2]
© UCLES 2024
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[Total: 12]
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,
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9
BLANK PAGE
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[2]
(b) A sample of CH3(CH2)5CHBrCH3 reacts with NaOH to make CH3(CH2)5CH(OH)CH3 in an
SN1 mechanism.
Complete Fig. 4.1 to show the mechanism for the reaction of CH3(CH2)5CHBrCH3 and NaOH.
Include charges, dipoles, lone pairs of electrons and curly arrows, as appropriate.
H
CH3(CH2)5
C
H
CH3(CH2)5
Br
CH3
C
OH
CH3
Fig. 4.1
[3]
(c) Separate samples of CH3(CH2)5CHBrCH3, CH3(CH2)5CH(OH)CH3 and CH3(CH2)5CHCH2
are tested with different reagents.
Complete Table 4.1. If no reaction occurs, write × in the relevant box.
Table 4.1
reagent added
observation with
CH3(CH2)5CHBrCH3
observation with
CH3(CH2)5CH(OH)CH3
observation with
CH3(CH2)5CHCH2
Br2(l) in the dark
PCl 5(s)
AgNO3(aq)
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(a) Draw the three-dimensional structures of the two stereoisomers of CH3(CH2)5CHBrCH3.
R can be used to represent CH3(CH2)5.
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CH3(CH2)5CHBrCH3 exists as a pair of stereoisomers.
[3]
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4
,
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10
,
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* 0019655306611 *
11
,
,
(d) CH3(CH2)5CHBrCH3 is heated with D to produce three different molecules, E, F and G.
E
F
G
Fig. 4.2
(i)
Name the type of reaction.
..................................................................................................................................... [1]
(ii)
Identify D and the conditions used.
..................................................................................................................................... [1]
(e) (i)
Both σ and π bonds are present in a molecule of E as a result of different types of
hybridisation in the carbon atoms.
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Complete Table 4.2 to show the number of carbon atoms with each type of hybridisation
in a molecule of E.
Table 4.2
number of carbon atoms
sp hybridised
E
F
sp2 hybridised
sp3 hybridised
G
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[2]
(ii)
Describe the essential feature of an unbranched hydrocarbon that causes its molecules
to show stereoisomerism. Explain how this feature leads to stereoisomerism.
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [3]
[Total: 15]
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5
,
Compound W has molecular formula C4H10O. It contains only one functional group.
(a) Table 5.1 shows the two peaks with the greatest m / e values in the mass spectrum of W.
Table 5.1
(i)
m/e
relative abundance
74
50
75
x
Calculate the relative abundance, x, of the peak at m / e = 75 using the information from
Table 5.1.
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* 0019655306612 *
The mass spectrum of W also shows peaks at m / e = 29 and m / e = 59.
Suggest the molecular formulae of these fragments.
m / e = 29 ..............................
m / e = 59 ..............................
[2]
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(b) A sample of W, C4H10O, is heated under reflux with an excess of acidified K2Cr2O7 until there
is no further reaction. Only one organic product, X, is present in the mixture at the end of the
reaction.
Fig. 5.1 shows the infrared spectrum of W.
100
80
60
transmittance / %
40
20
A
0
4000
3500
3000
2500
2000
1500
wavenumber / cm–1
Fig. 5.1
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1000
500
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(ii)
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x = .............................. [1]
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* 0019655306613 *
13
,
,
Fig. 5.2 shows the infrared spectrum of X.
100
80
60
transmittance / %
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40
20
0
4000
3500
3000
2500
2000
1500
wavenumber / cm–1
1000
500
Fig. 5.2
Table 5.2
bond
functional groups containing the bond
C–O
hydroxy, ester
1040–1300
C=C
aromatic compound, alkene
1500–1680
C=O
amide
carbonyl, carboxyl
ester
1640–1690
1670–1740
1710–1750
C≡N
nitrile
2200–2250
C–H
alkane
2850–2950
N–H
amine, amide
3300–3500
O–H
carboxyl
hydroxy
2500–3000
3200–3650
(i)
characteristic infrared absorption range
(in wavenumbers) / cm–1
Absorption A is shown in Fig. 5.1.
Absorption B is shown in Fig. 5.2.
Complete Table 5.3 using the information given in Fig. 5.1, Fig. 5.2 and Table 5.2.
Table 5.3
absorption
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B
bond
functional group
containing the bond
A
B
[1]
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[Turn over
,
Use the information in (a) and (b)(i) to draw the structure of X in the box in Fig. 5.3.
X
+ acidified
K2Cr2O7
W
C4H10O
Fig. 5.3
[1]
(c) Y is a structural isomer of W.
Both W and Y produce colourless bubbles when sodium is added to them.
Y does not react when heated with acidified K2Cr2O7.
Y does not react when warmed with alkaline I2(aq).
Name the functional group present in Y.
..................................................................................................................................... [1]
(ii)
Complete the equation to describe the reaction of W or Y with sodium.
..........C4H10O + ..........Na
(iii)
........................................................................................ [1]
Draw the structure of Y.
[1]
[Total: 8]
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(i)
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(ii)
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14
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15
,
,
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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strontium
87.6
rubidium
85.5
name
9
10
11
12
actinoids
actinoids
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
–
nobelium
–
mendelevium
–
fermium
–
einsteinium
–
californium
–
berkelium
–
curium
–
americium
–
plutonium
–
neptunium
–
uranium
238.0
protactinium
231.0
thorium
232.0
actinium
–
–
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Lr
lawrencium
No
Md
Fm
Es
Cf
Bk
Cm
Am
Pu
Np
U
Pa
Th
Ac
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103
102
101
100
99
98
97
96
95
94
93
92
91
90
89
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175.0
173.1
168.9
167.3
164.9
162.5
158.9
157.3
152.0
150.4
–
144.2
140.9
138.9
Og
oganesson
16
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lutetium
ytterbium
thulium
erbium
holmium
dysprosium
terbium
gadolinium
europium
samarium
promethium
neodymium
praseodymium
cerium
140.1
lanthanum
71
Lu
70
Yb
69
Tm
68
Er
67
Ho
66
Dy
65
Tb
64
Gd
63
Eu
62
Sm
61
Pm
60
Nd
59
Pr
58
–
Ce
–
–
Ts
tennessine
57
Lv
livermorium
Mc
moscovium
La
–
–
–
–
–
–
–
–
–
–
–
–
–
lanthanoids
Fl
flerovium
Nh
nihonium
Cn
copernicium
Rg
roentgenium
Ds
darmstadtium
Mt
meitnerium
Hs
hassium
Bh
bohrium
Sg
seaborgium
Db
dubnium
Rf
rutherfordium
Ra
radium
Fr
francium
118
–
117
116
115
114
113
112
111
110
109
108
107
106
105
104
89–103
–
88
radon
astatine
–
lead
polonium
86
Rn
85
At
84
131.3
xenon
Xe
54
83.8
krypton
209.0
204.4
200.6
195.1
190.2
186.2
183.8
180.9
178.5
137.3
36
Kr
Po
126.9
iodine
I
53
79.9
bromine
Br
83
127.6
tellurium
Te
52
79.0
selenium
Se
35
Bi
121.8
antimony
Sb
51
74.9
arsenic
As
34
bismuth
thallium
mercury
gold
197.0
platinum
iridium
192.2
osmium
rhenium
tungsten
tantalum
hafnium
barium
Pb
82
118.7
tin
Sn
50
72.6
germanium
Ge
33
,
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9701/22/M/J/24
207.2
81
Tl
80
Hg
79
Au
78
Pt
77
Ir
76
114.8
indium
In
49
69.7
gallium
Ga
32
39.9
31
Os
112.4
cadmium
Cd
48
65.4
zinc
Zn
30
75
107.9
silver
Ag
47
63.5
copper
Cu
29
Re
106.4
palladium
Pd
46
58.7
nickel
Ni
28
35.5
32.1
31.0
28.1
27.0
74
102.9
rhodium
Rh
45
58.9
cobalt
Co
27
argon
chlorine
sulfur
phosphorus
silicon
aluminium
W
101.1
ruthenium
Ru
44
55.8
iron
Fe
26
8
73
–
technetium
Tc
43
54.9
manganese
Mn
25
7
S
P
Ta
95.9
molybdenum
Mo
42
52.0
chromium
Cr
24
6
18
Ar
17
Cl
16
15
14
Si
13
19.0
16.0
14.0
12.0
10.8
Al
neon
20.2
fluorine
oxygen
nitrogen
carbon
boron
72
92.9
niobium
Nb
41
50.9
vanadium
V
23
5
relative atomic mass
10
Ne
F
O
N
C
B
4.0
9
8
7
6
5
helium
18
1.0
17
hydrogen
16
2
15
He
14
H
13
1
Group
Hf
87
91.2
88.9
Sr
Rb
132.9
zirconium
yttrium
38
37
caesium
Zr
Y
40.1
39.1
57–71
40
39
calcium
potassium
lanthanoids
47.9
45.0
Ca
K
56
titanium
scandium
20
19
Ba
Ti
Sc
24.3
23.0
55
22
21
magnesium
sodium
Cs
4
3
12
9.0
6.9
Mg
beryllium
lithium
atomic number
Key
atomic symbol
11
Be
Li
Na
4
2
,
3
1
The Periodic Table of Elements
* 0019655306616 *
* 0000800000001 *
,
,
Cambridge International AS & A Level
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CHEMISTRY
9701/22
Paper 2 AS Level Structured Questions
October/November 2024
1 hour 15 minutes
You must answer on the question paper.
No additional materials are needed.
INSTRUCTIONS
●
Answer all questions.
●
Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
●
Write your name, centre number and candidate number in the boxes at the top of the page.
●
Write your answer to each question in the space provided.
●
Do not use an erasable pen or correction fluid.
●
Do not write on any bar codes.
●
You may use a calculator.
●
You should show all your working and use appropriate units.
INFORMATION
●
The total mark for this paper is 60.
●
The number of marks for each question or part question is shown in brackets [ ].
●
The Periodic Table is printed in the question paper.
●
Important values, constants and standards are printed in the question paper.
This document has 16 pages.
DC (DE/CB) 326364/3
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2
1
,
Vanadium, niobium and tantalum are metals in the same group of the Periodic Table.
(a) The shorthand electronic configuration of vanadium in the ground state is [Ar]3d34s2.
(i)
State what is meant by the term ground state.
..................................................................................................................................... [1]
(ii)
Show the electronic configuration of vanadium using electrons in boxes notation.
[Ar]
(iii)
[1]
Deduce the total number of electrons in the p sub-shells of a vanadium atom.
..................................................................................................................................... [1]
(b) Pelopium was the suggested name for a new element discovered in a mineral.
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,
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* 0000800000002 *
Pelopium was later found to be a mixture of niobium, Nb, and tantalum, Ta.
Table 1.1
isotope
relative isotopic
mass
93
41Nb
92.91
181
73Ta
180.95
number of
protons
number of
neutrons
[2]
(ii)
Define relative isotopic mass.
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [2]
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Complete Table 1.1.
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(i)
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Only one naturally occurring isotope exists for each of Nb and Ta.
3
,
(iii)
,
181
A sample of pelopium contains 90.9% by mass 93
41Nb and 9.1% by mass 73Ta.
Calculate the theoretical relative atomic mass of pelopium based on these data and
Table 1.1.
Give your answer to two decimal places.
Show your working.
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theoretical relative atomic mass of pelopium = ..............................
[2]
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[Total: 9]
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4
Oxygen is a Group 16 element.
(a) (i)
Write equations for the following reactions.
•
sodium and oxygen
...........................................................................................................................................
•
sulfur and oxygen
...........................................................................................................................................
[2]
(ii)
Draw a dot-and-cross diagram to show the species present in Al2O3.
Draw outer electrons only.
[1]
(iii)
The maximum oxidation state of the Period 3 elements in their oxides varies across the
period.
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2
,
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...........................................................................................................................................
...........................................................................................................................................
[2]
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State and explain the variation.
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5
,
(b) H2O reacts with both inorganic and organic compounds.
(i)
Complete Table 2.1 to give details of the reactions of some Period 3 oxides with H2O.
Table 2.1
Period 3 oxide
product of reaction
with H2O
pH of solution formed
Mg(OH)2
P4O10
[2]
(ii)
Write an equation for the reaction of CH3CN with H2O in acidic conditions.
CH3CN + ......H2O + ......H+ ...............................................................................................
[1]
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(iii)
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,
Draw the structures of the two alcohols formed in the reaction shown in equation 1.
equation 1
C3H6(g) + H2O(g)
H3PO4
C3H8O(g)
[2]
(iv)
Explain why alcohols are less acidic than water.
...........................................................................................................................................
...........................................................................................................................................
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..................................................................................................................................... [2]
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6
,
(c) Fig. 2.1 shows the boiling points of H2O and other Group 16 hydrides.
390
340
290
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boiling point
/K
240
190
140
H 2O
H 2S
H2Se
H2Te
Fig. 2.1
(i)
Explain the trend in the boiling points of the Group 16 hydrides H2S to H2Te.
...........................................................................................................................................
...........................................................................................................................................
...........................................................................................................................................
..................................................................................................................................... [2]
(ii)
Explain why the boiling point of H2O is much higher than that of H2S.
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,
..................................................................................................................................... [1]
[Total: 15]
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7
,
3
,
Nitrogen and phosphorus are elements in Group 15 of the Periodic Table.
(a) Nitrogen is found in inorganic compounds such as nitrogen oxides (NOx), nitrates and nitric
acid.
(i)
Identify one natural and one man-made occurrence of nitrogen oxides in the atmosphere.
natural ...............................................................................................................................
man-made .........................................................................................................................
[2]
(ii)
Write an equation to describe the role of NO2 in the direct formation of acid rain.
..................................................................................................................................... [1]
(iii)
Peroxyacetyl nitrate, PAN, is a component of photochemical smog.
Describe how PAN forms from NO2.
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...........................................................................................................................................
..................................................................................................................................... [1]
(iv)
Nitric acid reacts with basic oxides to form nitrates.
Write an equation for the reaction of nitric acid with calcium oxide.
..................................................................................................................................... [1]
(v)
Describe what is seen when solid calcium nitrate is heated strongly.
..................................................................................................................................... [1]
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(b) A common test for nitrates is the reaction with NaOH and Al. Equation 1 shows the reaction.
equation 1
(i)
3NH3 + 8[Al(OH)4]–
Deduce the oxidation state of nitrogen in NO3–.
..................................................................................................................................... [1]
(ii)
Identify the species that is oxidised in equation 1.
..................................................................................................................................... [1]
(iii)
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3NO3– + 8Al + 5OH– + 18H2O
NH3 is a basic gas.
Describe how NH3 is able to act as a base.
...........................................................................................................................................
..................................................................................................................................... [1]
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8
,
(iv)
,
Suggest the shape of the [Al(OH)4]– ion.
..................................................................................................................................... [1]
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(c) Fig. 3.1 shows a sketch of some of the ionisation energies of phosphorus, P.
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2nd
3rd
4th
5th
6th
7th
8th
9th
10th
ionisation
Fig. 3.1
(i)
Construct an equation to represent the third ionisation energy of P.
..................................................................................................................................... [1]
(ii)
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Complete the graph in Fig. 3.1 to show the third to sixth ionisation energies of P.
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[2]
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1st
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ionisation energy
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9
,
,
(d) Complete Table 3.1 to show the properties of nitrogen and phosphorus in their standard
states.
Table 3.1
state and appearance
of standard state
nitrogen
phosphorus
colourless gas
white solid
electrical conductivity
poor
type of bonding
type of structure
simple
[2]
(e) A form of solid nitrogen has a lattice structure similar to solid iodine.
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Identify the type of lattice structure of solid nitrogen.
............................................................................................................................................. [1]
(f)
At very high temperatures, phosphorus can form P2 molecules.
P2 contains a triple bond, P P.
(i)
Describe the formation of the P P bond in terms of orbital overlap.
...........................................................................................................................................
...........................................................................................................................................
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...........................................................................................................................................
..................................................................................................................................... [2]
(ii)
The bond energy of P P is 485 kJ mol–1. The bond energy of N N is 944 kJ mol–1.
Compare the reactivity of P2 and N2. Explain your answer.
...........................................................................................................................................
...........................................................................................................................................
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..................................................................................................................................... [1]
[Total: 19]
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10
Bromoalkanes are used widely in industry, although there is increasing concern about their
environmental impact.
Fig. 4.1 shows a reaction scheme involving 1,2-dibromoethane.
A
Br2
reaction 1
Br
Br
NaOH(aq)
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H2C=CH2
reaction 2
NaOH in
ethanol
reaction 3
B
Br
reaction 4
polymer C
an excess of
NaOH in ethanol
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name .....................................
reaction 5
HBr, H2O and D
Fig. 4.1
(a) Complete Fig. 4.2 to show the mechanism for the formation of 1,2-dibromoethane in
reaction 1.
Include charges, dipoles, lone pairs of electrons and curly arrows as appropriate.
H 2C =
CH2
Br
Br
Br
Br
Fig. 4.2
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[3]
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4
,
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11
,
,
(b) The enthalpy change of reaction 1, ΔHr = –90.0 kJ mol–1.
H2C=CH2
Br2
reaction 1
Br
Br
The enthalpy change of formation of ethene, ΔHf = +52.2 kJ mol–1.
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Calculate the enthalpy change of formation of 1,2-dibromoethane.
ΔHf of 1,2-dibromoethane = .............................. kJ mol–1 [1]
(c) (i)
Complete Fig. 4.1 to:
•
•
(ii)
draw the structure of compound A
name compound B.
[2]
Draw the structure of one repeat unit of polymer C in the box.
one repeat unit of polymer C
[1]
(iii)
In reaction 5, compound B reacts with an excess of NaOH dissolved in ethanol. The
products are HBr, H2O and an unsaturated hydrocarbon D.
Suggest the identity of D.
..................................................................................................................................... [1]
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12
,
(d) Compound E is the only isomer of 1,2-dibromoethane.
Alkaline hydrolysis of E gives compound F.
E
F
Br
O
Br
(i)
H
Identify the type of isomerism shown by E and 1,2-dibromoethane.
..................................................................................................................................... [1]
(ii)
Name the homologous series that F belongs to.
..................................................................................................................................... [1]
(iii)
Complete Table 4.1 to state what is observed when F reacts with the reagents listed.
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,
Table 4.1
2,4-dinitrophenylhydrazine
(2,4-DNPH reagent)
Tollens’ reagent
alkaline I2(aq)
[3]
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observation with F
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reagent
13
,
,
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Question 4 continues on page 14.
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14
,
,
(e) Compound F reacts with reagent G to form compound H.
F
O
G
H
H
The infrared spectrum of H is shown in Fig. 4.3.
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50
0
4000
3000
2000
1500
1000
wavenumber / cm–1
Fig. 4.3
500
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transmittance / %
100
functional groups containing the bond
C–O
hydroxy, ester
1040–1300
C=C
aromatic compound, alkene
1500–1680
C=O
amide
carbonyl, carboxyl
ester
1640–1690
1670–1740
1710–1750
C N
nitrile
2200–2250
C–H
alkane
2850–2950
N–H
amine, amide
3300–3500
O–H
carboxyl
hydroxy
2500–3000
3200–3600
© UCLES 2024
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characteristic infrared absorption range
(in wavenumbers) / cm–1
bond
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Table 4.2
15
,
,
H also shows a molecular ion peak at m/e = 60 in its mass spectrum.
(i)
Use the information in (e), Fig. 4.3 and Table 4.2 to deduce the structure of H. Explain
your answer fully.
H
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...........................................................................................................................................
[3]
(ii)
Suggest the role of reagent G.
...........................................................................................................................................
[1]
[Total: 17]
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 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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silver
112
actinoids
actinoids
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
at www.cambridgeinternational.org after the live examination series.
–
nobelium
–
mendelevium
–
fermium
–
einsteinium
–
californium
–
berkelium
–
curium
–
americium
–
plutonium
–
neptunium
–
uranium
238.0
protactinium
231.0
thorium
232.0
actinium
–
neon
–
oganesson
Og
118
–
radon
Rn
86
131.3
xenon
Xe
54
83.8
krypton
Kr
36
39.9
argon
Ar
18
20.2
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Lr
lawrencium
No
Md
Fm
Es
Cf
Bk
Cm
Am
Pu
Np
U
Pa
Th
Ac
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103
102
101
100
99
98
97
96
95
94
93
92
91
90
89
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175.0
173.1
168.9
167.3
164.9
162.5
158.9
157.3
152.0
150.4
–
144.2
140.9
138.9
10
Ne
16
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lutetium
ytterbium
thulium
erbium
holmium
dysprosium
terbium
gadolinium
europium
samarium
promethium
neodymium
praseodymium
cerium
140.1
lanthanum
71
Lu
70
Yb
69
Tm
68
Er
67
Ho
66
Dy
65
Tb
64
Gd
63
Eu
62
Sm
61
Pm
60
Nd
59
Pr
58
–
–
Ce
Ts
tennessine
Lv
57
–
moscovium
La
–
–
–
–
–
–
–
–
–
–
–
–
–
lanthanoids
Fl
flerovium
Nh
nihonium
Cn
copernicium
Rg
roentgenium
Ds
darmstadtium
Mt
meitnerium
Hs
hassium
Bh
bohrium
Sg
seaborgium
Db
dubnium
Rf
rutherfordium
Ra
radium
Fr
francium
117
–
astatine
At
85
126.9
iodine
I
53
79.9
bromine
Br
35
35.5
chlorine
Cl
17
19.0
fluorine
F
livermorium
116
115
114
113
Mc
–
lead
polonium
84
Po
83
127.6
tellurium
Te
52
79.0
selenium
Se
Bi
121.8
antimony
Sb
51
74.9
arsenic
As
209.0
204.4
200.6
195.1
190.2
186.2
183.8
180.9
178.5
32.1
31.0
bismuth
thallium
mercury
gold
197.0
platinum
iridium
192.2
osmium
rhenium
tungsten
tantalum
hafnium
Pb
82
118.7
tin
Sn
50
72.6
germanium
Ge
sulfur
phosphorus
34
S
33
16
P
16.0
14.0
15
oxygen
nitrogen
207.2
81
Tl
80
Hg
79
Au
78
Pt
77
Ir
76
Os
75
Re
74
W
73
Ta
72
114.8
indium
In
49
69.7
gallium
Ga
Hf
111
28.1
27.0
32
silicon
aluminium
31
14
Si
13
12.0
10.8
Al
carbon
boron
O
N
9
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lanthanoids
110
112.4
cadmium
109
107.9
108
106.4
palladium
Cd
107
102.9
rhodium
Ag
48
65.4
zinc
Zn
30
106
101.1
ruthenium
Pd
47
63.5
copper
Cu
29
105
–
technetium
Rh
46
58.7
nickel
Ni
28
104
95.9
molybdenum
Ru
45
58.9
cobalt
Co
27
89–103
92.9
niobium
Tc
44
55.8
iron
Fe
26
88
87.6
85.5
Mo
43
12
87
57–71
strontium
rubidium
Nb
42
54.9
manganese
11
137.3
91.2
88.9
Sr
Rb
41
52.0
chromium
10
barium
zirconium
yttrium
38
37
50.9
vanadium
Mn
9
132.9
Zr
Y
40.1
39.1
Cr
25
8
caesium
40
39
calcium
potassium
V
24
7
56
47.9
45.0
Ca
K
23
6
Ba
titanium
scandium
20
19
5
55
Ti
Sc
24.3
23.0
name
relative atomic mass
C
B
8
7
4.0
6
5
helium
18
1.0
17
hydrogen
16
2
15
He
14
H
13
1
Cs
22
21
magnesium
sodium
4
3
12
9.0
6.9
Mg
beryllium
lithium
atomic number
Key
atomic symbol
11
Be
Li
Na
4
2
,
3
1
Group
The Periodic Table of Elements
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