2

1 The first ionisation energy of potassium, K, is 418 kJ mol–1. The first ionisation energy of
strontium, Sr, is 548 kJ mol–1.

Which statement helps to explain why Sr has a greater first ionisation energy than K?
Cambridge International AS & A Level
A The charge on a Sr nucleus is greater than the charge on a K nucleus.
CHEMISTRY 9701/12 B The outer electron in a Sr atom experiences greater shielding than the outer electron in a K
atom.
Paper 1 Multiple Choice February/March 2022
1 hour 15 minutes C The outer electron in a Sr atom experiences spin-pair repulsion.
D The outer electron in a Sr atom is further from the nucleus than the outer electron in a K
You must answer on the multiple choice answer sheet.
atom.
*6097847289*

You will need: Multiple choice answer sheet

Soft clean eraser
2 What is the electronic configuration of Mg 2+?
Soft pencil (type B or HB is recommended)
A 1s2 2s2 2p6
INSTRUCTIONS
 There are forty questions on this paper. Answer all questions. B 1s2 2s2 2p6 3s2
 For each question there are four possible answers A, B, C and D. Choose the one you consider correct
and record your choice in soft pencil on the multiple choice answer sheet. C 1s2 2s2 2p6 3s2 3p2
 Follow the instructions on the multiple choice answer sheet. D 1s2 2s2 2p6 3s2 3p6 3d2 4s2
 Write in soft pencil.
 Write your name, centre number and candidate number on the multiple choice answer sheet in the
spaces provided unless this has been done for you.
3 Compound X contains the elements C, H and O only.
 Do not use correction fluid.
 Do not write on any bar codes. 2.00 g of X produces 4.00 g of carbon dioxide and 1.63 g of water when completely combusted.
 You may use a calculator.
What is the empirical formula of X?
INFORMATION A CHO2 B C2H2O C C2H4O D CH2O2
 The total mark for this paper is 40.
 Each correct answer will score one mark.
 Any rough working should be done on this question paper. 4 For which molecule is the dipole moment zero?
 The Periodic Table is printed in the question paper.
 Important values, constants and standards are printed in the question paper. A CH3Cl B CH2Cl 2 C CHCl 3 D CCl 4

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

IB22 03_9701_12/3RP
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5 Which dot-and-cross diagram is correct for Al 2Cl 6? 7 Elements X, Y and Z are all in the first two periods of the Periodic Table.

A B Their Pauling electronegativity values, EN, are shown.

3+ –
Cl key element EN
2 Al 6 Cl = e!ectrons from Al X 1.0
= e!ectrons from Cl
Cl Al Cl Y 2.1
Z 4.0
Cl Al Cl
Substances exist with formulae XZ, YZ and Z2.

Which row puts these substances in order of increasing melting point?

Cl
lowest highest
melting point melting point

C D A XZ YZ Z2
B XZ Z2 YZ
Cl Cl Cl C Z2 YZ XZ
D Z2 XZ YZ
Cl Al Cl Cl Al Al Cl

8 The equation for reaction 1 is shown.

Cl Al Cl Cl Cl
reaction 1 C6H12O6  2CO2 + 2C2H5OH

Cl
C6H12O6 a
C2H5OH b
6 The boiling points of some hydrogen halides are shown.
What is the correct expression for the enthalpy change of reaction 1?
hydrogen halide boiling point / K
A a+b B a–b C a + 2b D a – 2b
H–Cl 188
H–Br 206
H–I 238

What is the explanation for the trend in boiling point for the hydrogen halides from HCl to HI?

A The bond energies of the hydrogen halides increase from HCl to HI.

B There is an increase in the strength of the intermolecular forces of attraction from HCl to HI.

C The intermolecular hydrogen bonds become stronger from HCl to HI.

D There is an increase in the bond polarity from HCl to HI.

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9 Nitrogen monoxide is an atmospheric pollutant that is formed inside car engines by an 11 Hydrogen peroxide, H2O2, decomposes to form water and oxygen.
endothermic reaction between nitrogen and oxygen.
The reaction is catalysed by bromide ions.
N2(g) + O2(g)  2NO(g)
step 1 2Br –(aq) + H2O2(aq) + 2H+(aq)  2H2O(l) + Br2(aq)
Which diagram correctly represents the energy profile for this reaction?
step 2 H2O2(aq) + Br2(aq)  2Br –(aq) + 2H+(aq) + O2(g)
A B
Which row is correct?

type of catalyst in step 1

products products
energy Ea energy Ea
reactants !H reactants !H A heterogeneous bromide ions are oxidised
B heterogeneous bromide ions are reduced

0 0 C homogeneous bromide ions are oxidised

0 progress of 0 progress of
D homogeneous bromide ions are reduced
reaction reaction

12 Hydrogen and iodine react to form hydrogen iodide in an exothermic reaction. The equation is
C D shown.

H2(g) + I2(g) 2HI(g)

reactants Ea reactants Ea 3
A 1 m reaction vessel contains H2, I2 and HI gases at equilibrium. The temperature is changed
energy energy such that the total pressure in the 1 m3 vessel doubles.
!H products !H products

What is the effect on the value of Kp and on the position of equilibrium?

0 0
0 progress of 0 progress of effect on the effect on the
reaction reaction value of Kp position of equilibrium

A decreases moves left

10 Two half-equations are shown.
B increases moves right
MnO4– + 2H2O + 3e–  MnO2 + 4OH– C no change moves left
2OH– + SO32–  SO42– + H2O + 2e– D no change no change

The equation for the reaction between manganate(VII) ions and sulfite ions is shown.

uMnO4– + vH2O + wSO32–  xMnO2 + ySO42– + zOH–

Which statements are correct?

1 u=x=z
2 Manganese is reduced to oxidation state +4.
3 Sulfur is oxidised from oxidation state +4 to +6.

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

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13 Diethylzinc, (C2H5)2Zn, is added to NaOH(aq). Two reactions occur. 15 The Boltzmann distribution for one mole of a gas at temperature T is shown.

reaction 1 (C2H5)2Zn + H2O  ZnO + 2C2H6

reaction 2 H2O + ZnO + 2OH–  Zn(OH)42–

number of
In these reactions, which compounds act as Brønsted–Lowry acids? particles with
energy, E
reaction 1 reaction 2
0
A (C2H5)2Zn H2O 0 energy, E

B H2O H2O One mole of the same gas is added, and the gas remains at temperature T.
C H2O ZnO
Which dotted curve shows the distribution with the added gas?
D the reaction is not acid / base ZnO
A B

14 Which statement about atoms and molecules is correct?

number of number of
A The molecular formula of a compound is the simplest whole number ratio of atoms of each
particles with particles with
element in the compound.
energy, E energy, E
B One mole of any substance contains 6  1023 atoms.
C The relative atomic mass of an element is the ratio of the average mass of one atom of the 0 0
0 energy, E 0 energy, E
element to the mass of an atom of carbon-12.
D The relative formula mass of a compound is the sum of the individual atomic masses of all
the atoms in the formula.
C D

number of number of
particles with particles with
energy, E energy, E

0 0
0 energy, E 0 energy, E

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16 In the reaction shown, the concentrations of both X and Y are reduced to half of their original 19 The table shows the melting points of SiO2 and P4O6.
values whilst keeping the total volume of the solution constant.
oxide SiO2 P4O6
X(aq) + Y(aq)  XY(aq)
melting point / K 1883 297
Simultaneously the temperature is increased from 298 K to 348 K.
Which statement explains the difference between the melting points of SiO2 and P4O6?
Which prediction is definitely true?
A The bonding of the oxides changes from ionic to covalent.
A A smaller proportion of collisions between particles of X and particles of Y will be successful.
B The metallic character of the elements decreases across Period 3.
B The average kinetic energy of particles of X and particles of Y will increase.
C The oxidation number of the element increases from Si to P.
C The rate of the reaction will be unaffected.
D The structure changes from giant molecular to simple molecular.
D The frequency of collisions between particles of X and particles of Y will halve.

20 Equal masses of CaCO3, Ca(NO3)2, BaCO3 and Ba(NO3)2 are thermally decomposed. The
17 A student investigated the chloride of a Period 3 element. This is what the student wrote down as volume of gas produced in each experiment is measured under the same conditions.
a record.
Which compound will produce the greatest volume of gas?

The compound was a white crystalline solid. It dissolved easily in water to A CaCO3 B Ca(NO3)2 C BaCO3 D Ba(NO3)2
give a solution of pH 12. When placed in a test-tube and heated in a
roaring Bunsen flame, the compound melted after several minutes heating.
21 Which row gives correct comparisons between the solubilities of calcium hydroxide and
barium hydroxide and the thermal stabilities of calcium carbonate and barium carbonate?
What can be deduced from this record?

A At least one of the recorded observations is incorrect. solubility thermal stability

calcium hydroxide barium hydroxide calcium carbonate barium carbonate
B The compound was magnesium chloride, MgCl 2.
A higher lower higher lower
C The compound was phosphorus pentachloride, PCl 5.
B higher lower lower higher
D The compound was sodium chloride, NaCl.
C lower higher higher lower

18 The elements in Period 3 and their compounds show trends across the period from sodium to D lower higher lower higher
chlorine.

Which row is correct? 22 Which statement relating to the elements in Group 17 and their compounds is correct?

A Bromine will reduce KI to form iodine.

electronegativity acid / base behaviour of
of the elements the oxides of the elements B Iodide ions react to form a white precipitate when added to silver nitrate solution.
A decreases basic  amphoteric  acidic C Bromide ions react to form a white precipitate when added to silver nitrate solution.
B decreases acidic  amphoteric  basic D Chlorine reacts with hydrogen to form a colourless gas.
C increases basic  amphoteric  acidic
D increases acidic  amphoteric  basic 23 An excess of chlorine was bubbled into 100 cm3 of hot 6.0 mol dm–3 sodium hydroxide.

How many moles of sodium chloride would be produced in the reaction?

A 0.30 B 0.50 C 0.60 D 0.72

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24 The product of the Contact process is Z. 28 Alkenes react with aqueous hydrogen bromide. The reaction proceeds via an intermediate
carbocation. The more stable the intermediate, the faster the reaction.
Which reaction or process leads to the formation of a gas that can neutralise an aqueous solution
of Z? Which sequence correctly shows an increase in the speed of reaction of the alkenes with
hydrogen bromide?
A atmospheric lightning
A ethene, propene, 2-methylpropene
B combustion of fuel in an internal combustion engine
B 2-methylpropene, ethene, propene
C the Haber process
C propene, ethene, 2-methylpropene
D thermal decomposition of Group 2 nitrates
D propene, 2-methylpropene, ethene

25 When ammonia, NH3, is dissolved in water, a small concentration of ammonium ions, NH4+, is
formed. 29 A reaction occurs when a sample of 1-chloropropane is heated under reflux with
sodium hydroxide dissolved in ethanol.
Which row is correct?
Which row is correct?
number of change of the H–N–H
electrons in one angle from ammonia type of reaction name of product
ammonium ion to the ammonium ion
A elimination propan-1-ol
A 8 decreases B elimination propene
B 8 increases C substitution propan-1-ol
C 10 decreases D substitution propene
D 10 increases

30 The diagram shows the structures of three halogenoalkanes.

26 In this question, alkenes and cyclic alkanes should be considered.
P Q R
How many structural isomers of C4H8 are there?
CH3 H H
A 3 B 4 C 5 D 6
CH3 C Br H C Br H C Cl

27 Which compound will decolourise Br2(aq)? CH3 H H

A CH3CH2CH2CH2CH2CO2H P, Q and R can all be hydrolysed.

B CH3CH2CH2CH2CH2CHO
Which row is correct?
C CH3CHCHCH2CH2CH2OH
relative speed mechanism
D CH3CH2CH2CO2CH2CH3
of hydrolysis of hydrolysis
Q R P Q

A fast slow SN1 SN2

B fast slow SN2 SN1
C slow fast SN1 SN2
D slow fast SN2 SN1

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31 A sample of 2.30 g of ethanol is mixed with an excess of aqueous acidified potassium 34 A student suggests two uses of LiAl H4.
dichromate(VI). The reaction mixture is boiled under reflux for one hour. The required organic
product is then collected by distillation. The yield of product is 60.0%. LiAl H4
reaction 1 CH3 CH CH2 CH3 CH2 CH3
Which mass of product is collected?
LiAl H4
A 1.32 g B 1.38 g C 1.80 g D 3.00 g reaction 2 CH3CO2H CH3CH2OH

Which reactions would give the product shown?

32 The structure of tartaric acid is shown.
A both reactions
tartaric acid
B reaction 1 only
OH O
C reaction 2 only
HO
OH D neither reaction
O OH
35 Compound X contains a single ester group.
Four moles of substance X react with one mole of tartaric acid.
X contains 27.6% by mass of oxygen.
What could be substance X?
Which pair of products could be produced by the hydrolysis of X?
A sodium
B sodium carbonate A butan-1-ol and ethanoic acid

C sodium hydrogencarbonate B ethanol and propanoic acid

D sodium hydroxide C methanol and methanoic acid

D propan-2-ol and butanoic acid
33 Which compound gives both:
36 What is the least number of carbon atoms in a non-cyclic alkane molecule that has a chiral
● an orange precipitate with 2,4-DNPH reagent centre?
● and a yellow precipitate with alkaline I2(aq)?
A 7 B 8 C 9 D 10
A ethanol
B methanal 37 A molecule of a polymer contains the sequence shown.

C propanal H H H H H Cl H H H Cl H H
D propanone C C C C C C C C C C C C

H Cl Cl H H H Cl H H H H Cl

Which monomer could produce this polymer by addition polymerisation?

A CHCl =CHCl
B CH2=CHCl
C CH3CCl =CHCl

D CH3CCl =CH2

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38 Compound Y is heated with a mild oxidising agent. One of the products of the reaction reacts with 40 Which diagram shows the infrared spectrum of a compound that contains both a C=O and an
hydrogen cyanide forming 2-hydroxybutanenitrile. O–H group?

What is compound Y? A B
100 100
A butan-1-ol

transmittance / %

transmittance / %
B butan-2-ol
C propan-1-ol
50 50
D propan-2-ol

39 The diagrams show the structures of lycopene and -carotene.

0 0
lycopene 3000 2000 1000 3000 2000 1000
CH3 wavenumber / cm–1 wavenumber / cm–1
CH3 CH3
CH3 CH3

C D
CH3 CH3 CH3 CH3
100 100
CH3

transmittance / %

transmittance / %
β-carotene 50 50
CH3
CH3 CH3
CH3 CH3

CH3 CH3 0 0
CH3 CH3 3000 2000 1000 3000 2000 1000
CH3
wavenumber / cm–1 wavenumber / cm–1

When lycopene is converted into -carotene, what is the gain or loss of hydrogen atoms per
molecule? bond functional group containing the bond characteristic infrared absorption range
(in wavenumbers) / cm–1
A 4 gained C–O hydroxy, ester 1040–1300
B 2 gained C=C aromatic compound, alkene 1500–1680
C no change C=O amide 1640–1690
D 2 lost carbonyl, carboxyl 1670–1740
ester 1710–1750
C≡N nitrile 2200–2250
C–H alkane 2850–3100
N–H amine, amide 3300–3500
O–H carboxyl 2500–3000
hydroxy 3200–3650

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electronic charge
Faraday constant
Avogadro constant
molar gas constant

molar volume of gas

ionic product of water

specific heat capacity of water
19

9701/12/F/M/22
e = –1.60  10–19 C
R = 8.31 J K–1 mol–1

L = 6.022  1023 mol–1

F = 9.65  104 C mol–1
Important values, constants and standards

c = 4.18 kJ kg–1 K–1 (4.18 J g–1 K–1)

Vm = 24.0 dm3 mol–1 at room conditions
Kw = 1.00  10–14 mol2 dm–6 (at 298 K (25 C))
Vm = 22.4 dm3 mol–1 at s.t.p. (101 kPa and 273 K)

© UCLES 2022
The Periodic Table of Elements
Group
1 2 13 14 15 16 17 18
1 2
H He
hydrogen helium
Key 1.0 4.0
3 4 atomic number 5 6 7 8 9 10
Li Be atomic symbol B C N O F Ne
lithium beryllium name boron carbon nitrogen oxygen fluorine neon
6.9 9.0 relative atomic mass 10.8 12.0 14.0 16.0 19.0 20.2
11 12 13 14 15 16 17 18
Na Mg Al Si P S Cl Ar
sodium magnesium aluminium silicon phosphorus sulfur chlorine argon
23.0 24.3 3 4 5 6 7 8 9 10 11 12 27.0 28.1 31.0 32.1 35.5 39.9
19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36
at www.cambridgeinternational.org after the live examination series.

K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
potassium calcium scandium titanium vanadium chromium manganese iron cobalt nickel copper zinc gallium germanium arsenic selenium bromine krypton
39.1 40.1 45.0 47.9 50.9 52.0 54.9 55.8 58.9 58.7 63.5 65.4 69.7 72.6 74.9 79.0 79.9 83.8
37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54
20

Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe
rubidium strontium yttrium zirconium niobium molybdenum technetium ruthenium rhodium palladium silver cadmium indium tin antimony tellurium iodine xenon
85.5 87.6 88.9 91.2 92.9 95.9 – 101.1 102.9 106.4 107.9 112.4 114.8 118.7 121.8 127.6 126.9 131.3
9701/12/F/M/22

55 56 57–71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86
lanthanoids
Cs Ba Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
caesium barium hafnium tantalum tungsten rhenium osmium iridium platinum gold mercury thallium lead bismuth polonium astatine radon
132.9 137.3 178.5 180.9 183.8 186.2 190.2 192.2 195.1 197.0 200.6 204.4 207.2 209.0 – – –
87 88 89–103 104 105 106 107 108 109 110 111 112 113 114 115 116 117 118
actinoids
Fr Ra Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
francium radium rutherfordium dubnium seaborgium bohrium hassium meitnerium darmstadtium roentgenium copernicium nihonium flerovium moscovium livermorium tennessine oganesson
– – – – – – – – – – – – – – – – –

57 58 59 60 61 62 63 64 65 66 67 68 69 70 71
lanthanoids La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
lanthanum cerium praseodymium neodymium promethium samarium europium gadolinium terbium dysprosium holmium erbium thulium ytterbium lutetium
138.9 140.1 140.9 144.4 – 150.4 152.0 157.3 158.9 162.5 164.9 167.3 168.9 173.1 175.0
89 90 91 92 93 94 95 96 97 98 99 100 101 102 103
actinoids Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
actinium thorium protactinium uranium neptunium plutonium americium curium berkelium californium einsteinium fermium mendelevium nobelium lawrencium
– 232.0 231.0 238.0 – – – – – – – – – – –
Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download
To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge