Cambridge A Level Chemistry 9701 — 2022 Feb/March Paper 1 · Variant 2

This document has 20 pages. Any blank pages are indicated. IB22 03_9701_12/3RP © UCLES 2022 [Turn over *6097847289* Cambridge International AS & A Level CHEMISTRY 9701/12 Paper 1 Multiple Choice February/March 2022 1 hour 15 minutes You must answer on the multiple choice answer sheet. You will need: Multiple choice answer sheet Soft clean eraser Soft pencil (type B or HB is recommended) INSTRUCTIONS  There are forty questions on this paper. Answer all questions.  For each question there are four possible answers A, B, C and D. Choose the one you consider correct and record your choice in soft pencil on the multiple choice answer sheet.  Follow the instructions on the multiple choice answer sheet.  Write in soft pencil.  Write your name, centre number and candidate number on the multiple choice answer sheet in the spaces provided unless this has been done for you.  Do not use correction fluid.  Do not write on any bar codes.  You may use a calculator. INFORMATION  The total mark for this paper is 40.  Each correct answer will score one mark.  Any rough working should be done on this question paper.  The Periodic Table is printed in the question paper.  Important values, constants and standards are printed in the question paper.

2 © UCLES 2022 9701/12/F/M/22 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? A The charge on a Sr nucleus is greater than the charge on a K nucleus. B The outer electron in a Sr atom experiences greater shielding than the outer electron in a K atom. 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 atom. 2 What is the electronic configuration of Mg2+? A 1s2 2s2 2p6 B 1s2 2s2 2p6 3s2 C 1s2 2s2 2p6 3s2 3p2 D 1s2 2s2 2p6 3s2 3p6 3d2 4s2 3 Compound X contains the elements C, H and O only. 2.00 g of X produces 4.00 g of carbon dioxide and 1.63 g of water when completely combusted. What is the empirical formula of X? A CHO2 B C2H2O C C2H4O D CH2O2 4 For which molecule is the dipole moment zero? A CH3Cl B CH2Cl 2 C CHCl 3 D CCl 4

3 © UCLES 2022 9701/12/F/M/22 [Turn over 5 Which dot-and-cross diagram is correct for Al 2Cl 6? Al A B Cl Al Al Al Al Cl Cl Cl 3+ – 6 2 Cl Cl C D key = e
ectrons from Al = e
ectrons from Cl Cl Cl Cl Cl Cl Cl Cl Al Al Cl Cl Cl Cl Cl Cl 6 The boiling points of some hydrogen halides are shown. hydrogen halide boiling point / K 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.

4 © UCLES 2022 9701/12/F/M/22 7 Elements X, Y and Z are all in the first two periods of the Periodic Table. Their Pauling electronegativity values, EN, are shown. element EN X 1.0 Y 2.1 Z 4.0 Substances exist with formulae XZ, YZ and Z2. Which row puts these substances in order of increasing melting point? lowest melting point highest melting point A XZ YZ Z2 B XZ Z2 YZ C Z2 YZ XZ D Z2 XZ YZ 8 The equation for reaction 1 is shown. reaction 1 C6H12O6  2CO2 + 2C2H5OH C6H12O6 a C2H5OH b What is the correct expression for the enthalpy change of reaction 1? A a + b B a – b C a + 2b D a – 2b

5 © UCLES 2022 9701/12/F/M/22 [Turn over 9 Nitrogen monoxide is an atmospheric pollutant that is formed inside car engines by an endothermic reaction between nitrogen and oxygen. N2(g) + O2(g)  2NO(g) Which diagram correctly represents the energy profile for this reaction? energy progress of reaction reactants reactants reactants reactants products products products products 0 0 A Ea
H Ea
H energy progress of reaction B energy progress of reaction C Ea
H Ea
H energy progress of reaction D 0 0 0 0 0 0 10 Two half-equations are shown. MnO4 – + 2H2O + 3e–  MnO2 + 4OH– 2OH– + SO3 2–  SO4 2– + H2O + 2e– The equation for the reaction between manganate(VII) ions and sulfite ions is shown. uMnO4 – + vH2O + wSO3 2–  xMnO2 + ySO4 2– + 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

6 © UCLES 2022 9701/12/F/M/22 11 Hydrogen peroxide, H2O2, decomposes to form water and oxygen. The reaction is catalysed by bromide ions. step 1 2Br –(aq) + H2O2(aq) + 2H+(aq)  2H2O(l) + Br2(aq) step 2 H2O2(aq) + Br2(aq)  2Br –(aq) + 2H+(aq) + O2(g) Which row is correct? type of catalyst in step 1 A heterogeneous bromide ions are oxidised B heterogeneous bromide ions are reduced C homogeneous bromide ions are oxidised D homogeneous bromide ions are reduced 12 Hydrogen and iodine react to form hydrogen iodide in an exothermic reaction. The equation is shown. H2(g) + I2(g) 2HI(g) A 1 m3 reaction vessel contains H2, I2 and HI gases at equilibrium. The temperature is changed such that the total pressure in the 1 m3 vessel doubles. What is the effect on the value of Kp and on the position of equilibrium? effect on the value of Kp effect on the position of equilibrium A decreases moves left B increases moves right C no change moves left D no change no change

7 © UCLES 2022 9701/12/F/M/22 [Turn over 13 Diethylzinc, (C2H5)2Zn, is added to NaOH(aq). Two reactions occur. reaction 1 (C2H5)2Zn + H2O  ZnO + 2C2H6 reaction 2 H2O + ZnO + 2OH–  Zn(OH)4 2– In these reactions, which compounds act as Brønsted–Lowry acids? reaction 1 reaction 2 A (C2H5)2Zn H2O B H2O H2O C H2O ZnO D the reaction is not acid / base ZnO 14 Which statement about atoms and molecules is correct? A The molecular formula of a compound is the simplest whole number ratio of atoms of each element in the compound. 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 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.

8 © UCLES 2022 9701/12/F/M/22 15 The Boltzmann distribution for one mole of a gas at temperature T is shown. number of particles with energy, E energy, E 0 0 One mole of the same gas is added, and the gas remains at temperature T. Which dotted curve shows the distribution with the added gas? number of particles with energy, E energy, E A 0 0 number of particles with energy, E energy, E B 0 0 number of particles with energy, E energy, E C 0 0 number of particles with energy, E energy, E D 0 0

9 © UCLES 2022 9701/12/F/M/22 [Turn over 16 In the reaction shown, the concentrations of both X and Y are reduced to half of their original values whilst keeping the total volume of the solution constant. X(aq) + Y(aq)  XY(aq) Simultaneously the temperature is increased from 298 K to 348 K. Which prediction is definitely true? A A smaller proportion of collisions between particles of X and particles of Y will be successful. B The average kinetic energy of particles of X and particles of Y will increase. C The rate of the reaction will be unaffected. D The frequency of collisions between particles of X and particles of Y will halve. 17 A student investigated the chloride of a Period 3 element. This is what the student wrote down as a record. The compound was a white crystalline solid. It dissolved easily in water to 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. What can be deduced from this record? A At least one of the recorded observations is incorrect. B The compound was magnesium chloride, MgCl 2. C The compound was phosphorus pentachloride, PCl 5. D The compound was sodium chloride, NaCl. 18 The elements in Period 3 and their compounds show trends across the period from sodium to chlorine. Which row is correct? electronegativity of the elements acid / base behaviour of the oxides of the elements A decreases basic  amphoteric  acidic B decreases acidic  amphoteric  basic C increases basic  amphoteric  acidic D increases acidic  amphoteric  basic

10 © UCLES 2022 9701/12/F/M/22 19 The table shows the melting points of SiO2 and P4O6. oxide SiO2 P4O6 melting point / K 1883 297 Which statement explains the difference between the melting points of SiO2 and P4O6? A The bonding of the oxides changes from ionic to covalent. B The metallic character of the elements decreases across Period 3. C The oxidation number of the element increases from Si to P. D The structure changes from giant molecular to simple molecular. 20 Equal masses of CaCO3, Ca(NO3)2, BaCO3 and Ba(NO3)2 are thermally decomposed. The volume of gas produced in each experiment is measured under the same conditions. Which compound will produce the greatest volume of gas? A CaCO3 B Ca(NO3)2 C BaCO3 D Ba(NO3)2 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? solubility thermal stability calcium hydroxide barium hydroxide calcium carbonate barium carbonate A higher lower higher lower B higher lower lower higher C lower higher higher lower D lower higher lower higher 22 Which statement relating to the elements in Group 17 and their compounds is correct? A Bromine will reduce KI to form iodine. B Iodide ions react to form a white precipitate when added to silver nitrate solution. C Bromide ions react to form a white precipitate when added to silver nitrate solution. D Chlorine reacts with hydrogen to form a colourless gas. 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

11 © UCLES 2022 9701/12/F/M/22 [Turn over 24 The product of the Contact process is Z. Which reaction or process leads to the formation of a gas that can neutralise an aqueous solution of Z? A atmospheric lightning B combustion of fuel in an internal combustion engine C the Haber process D thermal decomposition of Group 2 nitrates 25 When ammonia, NH3, is dissolved in water, a small concentration of ammonium ions, NH4 +, is formed. Which row is correct? number of electrons in one ammonium ion change of the H–N–H angle from ammonia to the ammonium ion A 8 decreases B 8 increases C 10 decreases D 10 increases 26 In this question, alkenes and cyclic alkanes should be considered. How many structural isomers of C4H8 are there? A 3 B 4 C 5 D 6 27 Which compound will decolourise Br2(aq)? A CH3CH2CH2CH2CH2CO2H B CH3CH2CH2CH2CH2CHO C CH3CHCHCH2CH2CH2OH D CH3CH2CH2CO2CH2CH3

12 © UCLES 2022 9701/12/F/M/22 28 Alkenes react with aqueous hydrogen bromide. The reaction proceeds via an intermediate carbocation. The more stable the intermediate, the faster the reaction. Which sequence correctly shows an increase in the speed of reaction of the alkenes with hydrogen bromide? A ethene, propene, 2-methylpropene B 2-methylpropene, ethene, propene C propene, ethene, 2-methylpropene D propene, 2-methylpropene, ethene 29 A reaction occurs when a sample of 1-chloropropane is heated under reflux with sodium hydroxide dissolved in ethanol. Which row is correct? type of reaction name of product A elimination propan-1-ol B elimination propene C substitution propan-1-ol D substitution propene 30 The diagram shows the structures of three halogenoalkanes. CH3 CH3 CH3 C P Br H H H C R Cl H H H C Q Br P, Q and R can all be hydrolysed. Which row is correct? relative speed of hydrolysis mechanism 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

13 © UCLES 2022 9701/12/F/M/22 [Turn over 31 A sample of 2.30 g of ethanol is mixed with an excess of aqueous acidified potassium 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%. Which mass of product is collected? A 1.32 g B 1.38 g C 1.80 g D 3.00 g 32 The structure of tartaric acid is shown. HO OH OH OH O O tartaric acid Four moles of substance X react with one mole of tartaric acid. What could be substance X? A sodium B sodium carbonate C sodium hydrogencarbonate D sodium hydroxide 33 Which compound gives both: ● an orange precipitate with 2,4-DNPH reagent ● and a yellow precipitate with alkaline I2(aq)? A ethanol B methanal C propanal D propanone

14 © UCLES 2022 9701/12/F/M/22 34 A student suggests two uses of LiAl H4. CH3 CH CH2 CH3CO2H CH3CH2OH CH3 CH2 CH3 reaction 1 LiAl H4 reaction 2 LiAl H4 Which reactions would give the product shown? A both reactions B reaction 1 only C reaction 2 only D neither reaction 35 Compound X contains a single ester group. X contains 27.6% by mass of oxygen. Which pair of products could be produced by the hydrolysis of X? A butan-1-ol and ethanoic acid B ethanol and propanoic acid C methanol and methanoic acid D propan-2-ol and butanoic acid 36 What is the least number of carbon atoms in a non-cyclic alkane molecule that has a chiral centre? A 7 B 8 C 9 D 10 37 A molecule of a polymer contains the sequence shown. C H H C Cl Cl Cl Cl Cl Cl H C H C H H C H H C H C H C H H C H H C H C H H C H Which monomer could produce this polymer by addition polymerisation? A CHCl =CHCl B CH2=CHCl C CH3CCl =CHCl D CH3CCl =CH2

15 © UCLES 2022 9701/12/F/M/22 [Turn over 38 Compound Y is heated with a mild oxidising agent. One of the products of the reaction reacts with hydrogen cyanide forming 2-hydroxybutanenitrile. What is compound Y? A butan-1-ol B butan-2-ol C propan-1-ol D propan-2-ol 39 The diagrams show the structures of lycopene and -carotene. CH3 CH3 CH3 CH3 CH3 CH3 CH3 CH3 CH3 CH3 lycopene CH3 CH3 CH3 CH3 CH3 CH3 CH3 CH3 CH3 CH3 β-carotene When lycopene is converted into -carotene, what is the gain or loss of hydrogen atoms per molecule? A 4 gained B 2 gained C no change D 2 lost

16 © UCLES 2022 9701/12/F/M/22 40 Which diagram shows the infrared spectrum of a compound that contains both a C=O and an O–H group? transmittance / % 3000 2000 wavenumber / cm–1 A 1000 3000 2000 1000 100 50 0 100 50 0 100 50 0 100 50 0 transmittance / % 3000 2000 wavenumber / cm–1 B 1000 transmittance / % wavenumber / cm–1 C transmittance / % wavenumber / cm–1 D 3000 2000 1000 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

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19 © UCLES 2022 9701/12/F/M/22 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)

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. © UCLES 2022 9701/12/F/M/22 Group The Periodic Table of Elements 1 H hydrogen 1.0 2 He helium 4.0 1 2 13 14 15 16 17 18 3 4 5 6 7 8 9 10 11 12 3 Li lithium 6.9 4 Be beryllium 9.0 atomic number atomic symbol Key name relative atomic mass 11 Na sodium 23.0 12 Mg magnesium 24.3 19 K potassium 39.1 20 Ca calcium 40.1 37 Rb rubidium 85.5 38 Sr strontium 87.6 55 Cs caesium 132.9 56 Ba barium 137.3 87 Fr francium – 88 Ra radium – 5 B boron 10.8 13 Al aluminium 27.0 31 Ga gallium 69.7 49 In indium 114.8 81 Tl thallium 204.4 6 C carbon 12.0 14 Si silicon 28.1 32 Ge germanium 72.6 50 Sn tin 118.7 82 Pb lead 207.2 22 Ti titanium 47.9 40 Zr zirconium 91.2 72 Hf hafnium 178.5 104 Rf rutherfordium – 23 V vanadium 50.9 41 Nb niobium 92.9 73 Ta tantalum 180.9 105 Db dubnium – 24 Cr chromium 52.0 42 Mo molybdenum 95.9 74 W tungsten 183.8 106 Sg seaborgium – 25 Mn manganese 54.9 43 Tc technetium – 75 Re rhenium 186.2 107 Bh bohrium – 26 Fe iron 55.8 44 Ru ruthenium 101.1 76 Os osmium 190.2 108 Hs hassium – 27 Co cobalt 58.9 45 Rh rhodium 102.9 77 Ir iridium 192.2 109 Mt meitnerium – 28 Ni nickel 58.7 46 Pd palladium 106.4 78 Pt platinum 195.1 110 Ds darmstadtium – 29 Cu copper 63.5 47 Ag silver 107.9 79 Au gold 197.0 111 Rg roentgenium – 30 Zn zinc 65.4 48 Cd cadmium 112.4 80 Hg mercury 200.6 112 Cn copernicium – 114 Fl flerovium – 116 Lv livermorium – 7 N nitrogen 14.0 15 P phosphorus 31.0 33 As arsenic 74.9 51 Sb antimony 121.8 83 Bi bismuth 209.0 8 O oxygen 16.0 16 S sulfur 32.1 34 Se selenium 79.0 52 Te tellurium 127.6 84 Po polonium – 9 F fluorine 19.0 17 Cl chlorine 35.5 35 Br bromine 79.9 53 I iodine 126.9 85 At astatine – 10 Ne neon 20.2 18 Ar argon 39.9 36 Kr krypton 83.8 54 Xe xenon 131.3 86 Rn radon – 113 Nh nihonium – 115 Mc moscovium – 117 Ts tennessine – 118 Og oganesson – 21 Sc scandium 45.0 39 Y yttrium 88.9 57–71 lanthanoids 89–103 actinoids 57 La lanthanum 138.9 89 Ac lanthanoids actinoids actinium – 58 Ce cerium 140.1 90 Th thorium 232.0 59 Pr praseodymium 140.9 91 Pa protactinium 231.0 60 Nd neodymium 144.4 92 U uranium 238.0 61 Pm promethium – 93 Np neptunium – 62 Sm samarium 150.4 94 Pu plutonium – 63 Eu europium 152.0 95 Am americium – 64 Gd gadolinium 157.3 96 Cm curium – 65 Tb terbium 158.9 97 Bk berkelium – 66 Dy dysprosium 162.5 98 Cf californium – 67 Ho holmium 164.9 99 Es einsteinium – 68 Er erbium 167.3 100 Fm fermium – 69 Tm thulium 168.9 101 Md mendelevium – 70 Yb ytterbium 173.1 102 No nobelium – 71 Lu lutetium 175.0 103 Lr lawrencium –

This document consists of 3 printed pages. © UCLES 2022 [Turn over Cambridge International AS & A Level CHEMISTRY 9701/12 Paper 1 Multiple Choice February/March 2022 MARK SCHEME Maximum Mark: 40 Published This mark scheme is published as an aid to teachers and candidates, to indicate the requirements of the examination. Mark schemes should be read in conjunction with the question paper and the Principal Examiner Report for Teachers. Cambridge International will not enter into discussions about these mark schemes. Cambridge International is publishing the mark schemes for the February/March 2022 series for most Cambridge IGCSE™, Cambridge International A and AS Level components and some Cambridge O Level components.

9701/12 Cambridge International AS & A Level – Mark Scheme PUBLISHED February/March 2022 © UCLES 2022 Page 2 of 3 Question Answer Marks 1 A 1 2 A 1 3 C 1 4 D 1 5 B 1 6 B 1 7 C 1 8 D 1 9 A 1 10 A 1 11 C 1 12 A 1 13 B 1 14 D 1 15 A 1 16 B 1 17 A 1 18 C 1 19 D 1 20 B 1 21 D 1 22 D 1 23 B 1 24 C 1 25 D 1 26 C 1 27 C 1 28 A 1

9701/12 Cambridge International AS & A Level – Mark Scheme PUBLISHED February/March 2022 © UCLES 2022 Page 3 of 3 Question Answer Marks 29 B 1 30 A 1 31 C 1 32 A 1 33 D 1 34 C 1 35 A 1 36 A 1 37 B 1 38 C 1 39 C 1 40 B 1