Cambridge A Level Chemistry 9701 — 2023 May/June Paper 1 · Variant 2

7KLVGRFXPHQWKDVSDJHV$Q\EODQNSDJHVDUHLQGLFDWHG ,%B B753 ‹8&/(6 >7XUQRYHU *9804289175* &DPEULGJH,QWHUQDWLRQDO$6 $/HYHO &+(0,675<  3DSHU0XOWLSOH&KRLFH 0D\-XQH KRXUPLQXWHV <RXPXVWDQVZHURQWKHPXOWLSOHFKRLFHDQVZHUVKHHW <RXZLOOQHHG  0XOWLSOHFKRLFHDQVZHUVKHHW 6RIWFOHDQHUDVHU 6RIWSHQFLO W\SH%RU+%LVUHFRPPHQGHG  ,16758&7,216 x 7KHUHDUHIRUW\TXHVWLRQVRQWKLVSDSHU$QVZHUDOOTXHVWLRQV x )RUHDFKTXHVWLRQWKHUHDUHIRXUSRVVLEOHDQVZHUV$%&DQG'&KRRVHWKHRQH\RXFRQVLGHUFRUUHFW DQGUHFRUG\RXUFKRLFHLQVRIWSHQFLORQWKHPXOWLSOHFKRLFHDQVZHUVKHHW x )ROORZWKHLQVWUXFWLRQVRQWKHPXOWLSOHFKRLFHDQVZHUVKHHW x :ULWHLQVRIWSHQFLO x :ULWH\RXUQDPHFHQWUHQXPEHUDQGFDQGLGDWHQXPEHURQWKHPXOWLSOHFKRLFHDQVZHUVKHHWLQWKH VSDFHVSURYLGHGXQOHVVWKLVKDVEHHQGRQHIRU\RX x 'RQRWXVHFRUUHFWLRQIOXLG x 'RQRWZULWHRQDQ\EDUFRGHV x <RXPD\XVHDFDOFXODWRU ,1)250$7,21 x 7KHWRWDOPDUNIRUWKLVSDSHULV x (DFKFRUUHFWDQVZHUZLOOVFRUHRQHPDUN x $Q\URXJKZRUNLQJVKRXOGEHGRQHRQWKLVTXHVWLRQSDSHU x 7KH3HULRGLF7DEOHLVSULQWHGLQWKHTXHVWLRQSDSHU x ,PSRUWDQWYDOXHVFRQVWDQWVDQGVWDQGDUGVDUHSULQWHGLQWKHTXHVWLRQSDSHU

When chlorine gas is analysed in a mass spectrometer 35Cl + ions are detected. Which row is correct? 1 electronic configuration of 35Cl + number of neutrons in 35Cl + 1s22s22p63s23p4 17 A 1s22s22p63s23p6 17 B 1s22s22p63s23p4 18 C 1s22s22p63s23p6 18 D Which species is a free radical? 2 Zn D O2– C Be– B He A Which statement is correct? 3 The first ionisation energy of chlorine is more than the first ionisation energy of argon. A The second ionisation energy of calcium is more than the second ionisation energy of magnesium. B The second ionisation energy of sulfur is equal to the first ionisation energy of phosphorus. C The eighth ionisation energy of chlorine is more than the first ionisation energy of neon. D If 1 mole of hexane combusts in an excess of oxygen, how many moles of products are formed? 4 14 D 13 C 12 B 11 A Separate samples, each of mass 1.0g, of the compounds listed are treated with an excess of dilute acid. Which compound releases the largest amount of CO2? 5 1.0g Na2CO3 D 1.0g MgCO3 C 1.0g Li2CO3 B 1.0g CaCO3 A Which statement about the Cl–N=O molecule is correct? 6 A It is a non-polar molecule. B It is a linear molecule. C The nitrogen atom is sp2 hybridised . D 2 ‹8&/(6 0- EachmoleculecontainsoneS
andtwoP
bonds.

Which row is correct? 7 total number of pairs of electrons in the valence shell of the central atom shape molecule two linear CO2 A three trigonal planar BF3 B four regular tetrahedral NH3 C six octahedral PF5 D Thevolumeofavesselis1.20s
10–3m3.Itcontainspureargonatapressureof1.00s
105Pa, andatatemperatureof25.0°C.Undertheseconditionsitcanbeassumedthatargonbehavesas anidealgas. Which mass of argon does it contain? 8 23.0g D 10.4g C 1.93g B 0.0485g A A student mixed 25.0cm3 of 4.00moldm–3 hydrochloric acid with an equal volume of 4.00moldm–3 sodium hydroxide. The initial temperature of both solutions was 15.0°C. The maximum temperature recorded was 30.0°C. The heat capacity of the final solution can be assumed to be 4.18JK–1g–1 and the density of this solution can be assumed to be 1.00gcm–3. Using these results, what is the enthalpy change of neutralisation of hydrochloric acid? 9 –62.7kJmol–1 A –31.4kJmol–1 B –15.7kJmol–1 C –3.14kJmol–1 D 3 >7XUQRYHU 0- ‹8&/(6

Nitrogen monoxide is rapidly oxidised to nitrogen dioxide. 2NO(g) + O2(g) →2NO2(g) Nitrogen dioxide can then dimerise to form dinitrogen tetroxide. 10 2NO2(g) N2O4(g) ΔH o = –58 kJ mol–1 ΔH oNO = +91 kJ mol–1 and ΔH oNO2 = +34 kJ mol–1 f f What is the value of the standard enthalpy change for the reaction shown? 2NO(g) + O2(g) →N2O4(g) –172kJmol–1 D –115kJmol–1 C –1kJmol–1 B +56kJmol–1 A LiAlH4 contains AlH4 – ions in which aluminium has an oxidation state of +3. LiAlH4 reacts with water, as shown. LiAlH4 + 4H2O →4H2 + LiOH + Al(OH)3 In this reaction, each of the four water molecules produces one hydroxide ion. It does this by losing one H+ ion, which reacts with the LiAlH4. Which changes in oxidation number occur in this reaction? 11 Al increases by 1 and H decreases by 1. A H decreases by 2 and also increases by 1. B H increases by 1 and also decreases by 1. C O decreases by 1 and H increases by 1. D Thevanadiumsalt,VOSO4,issolubleinwaterandreactsreadilywithpowderedmanganesein dilutesulfuricacid. Theequationforthereactionisshown. Mn(s) + 2VOSO4(aq) + 2H2SO4(aq) →
V2(SO4)3(aq) + MnSO4(aq) + 2H2O(l) Whichstatementaboutthisreactioniscorrect? 12 Hydrogen is oxidised in the reaction. A Manganese is the reducing agent in this reaction. B Sulfuric acid is the oxidising agent in this reaction. C The oxidation state of the vanadium changes from +5 to +3. D 4 ‹8&/(6 0-

Inwhichequilibriumwillanincreaseinpressureatconstanttemperatureincreasetheyieldofthe productsontheright-handsideoftheequation? 13 CaCO3(s) ⇋CaO(s) + CO2(g) A 4HCl(g) + O2(g) ⇋2H2O(g) + 2Cl 2(g) B 2HI(g) ⇋H2(g) + I2(g) C 3Fe(s) + 4H2O(g) ⇋Fe3O4(s) + 4H2(g) D Hydrogeniodideisaddedtoanevacuatedreactionvessel.Thevesselissealedandwarmed.A decompositionreactionoccurs.Hydrogenandiodineareformed.Somehydrogeniodideremains. Whenequilibriumisestablished,thetotalpressureis1.20s
105Pa.Thepartialpressureofhydrogen is4.00s
103Pa. Hydrogeniodide,hydrogenandiodineareallgaseousundertheconditionsused. WhatisthevalueofKpfortheequilibriumatthistemperature,assumingthedecompositionisthe forwardreaction? 14 1.43s
10–3 D 1.38s
10–3 C 1.28s
10–3 B 1.19s
10–3 A The equations for two reactions are shown. reaction X 2NOBr →2NO + Br2 reaction Y 2NOCl →2NO + Cl 2 The two reactions have similar reaction mechanisms. The initial rate of reaction X is greater than that of reaction Y when measured under identical conditions of temperature, pressure and reactant concentration. Which statements explain this difference? 15 3 only D 1 only C 2 and 3 B 1 and 2 A 5 >7XUQRYHU 0- ‹8&/(6 1 2 TheactivationenergyforreactionXislessthanthatofreactionY. TheBr−BrbondisweakerthantheCl−Clbond. AhigherfrequencyofcollisionsbetweenmoleculesofNOBroccurthanbetween moleculesofNOCl. 3

ThediagramshowstheBoltzmanndistributionofenergiesinagas.Thegascantakepartina reactionwithanactivationenergy,Ea.Thegasismaintainedataconstanttemperature. 16 proportion of molecules with a given energy molecular energy Ea P 0 0 Which statement is correct? If a catalyst is added, peak P will be lower and Ea will move to the left. A If a catalyst is added, peak P will be lower and Ea will move to the right. B If a catalyst is added, peak P will be the same and Ea will move to the left. C If a catalyst is added, peak P will be the same and Ea will move to the right. D L, M and N are three different elements from Period 3 of the Periodic Table. L is the element whose atoms have three unpaired electrons in its 3p sub-shell. M is the element with the highest electrical conductivity in the period. N is the element with the highest melting point in the period. Which statement about element L is correct? 17 L has a higher atomic number than M and a lower atomic number than N. A L has a lower atomic number than M and a higher atomic number than N. B L has a lower atomic number than both M and N. C L has a higher atomic number than both M and N. D 6 ‹8&/(6 0-

In reactions 1 and 2, X represents an element in Period 3. In each reaction, X is forming a product where X is in its highest oxidation state. reaction 1 chlorine + element X →XyCl z reaction 2 oxygen + element X →XpOq Which ratios show a steady increase from sodium to phosphorus? 18 neither z:y nor q:p A z:y only B q:p only C both z:y and q:p D Sodium, magnesium, aluminium, silicon and phosphorus are all elements in Period 3 of the Periodic Table. Three statements about the oxides and chlorides of these elements are given. 19 The ionically bonded oxides all react with dilute hydrochloric acid. 1 All metal chlorides produce neutral solutions when added to water. 2 The two most electronegative elements both form covalently bonded chlorides. 3 Which statements are correct? 2 and 3 only D 1 and 3 only C 1 and 2 only B 1, 2 and 3 A The table compares calcium with barium and calcium carbonate with barium carbonate. Which row is correct? 20 thermal stability of the metal carbonate reactivity of the element with water barium carbonate is more stable barium is more reactive A calcium carbonate is more stable barium is more reactive B barium carbonate is more stable calcium is more reactive C calcium carbonate is more stable calcium is more reactive D 7 >7XUQRYHU 0- ‹8&/(6

SolutionsPandQeachcontainadifferentGroup2ionatthesameconcentration.Onecontains Mg2+andtheothercontainsBa2+.Testsarecarriedoutonseparate5cm3samplesofPandQ. test1:add1cm3of0.1moldm–3Na2SO4(aq) test2:add1cm3of0.1moldm–3NaOH(aq) Whataretheresultsofthesetests? 21 results in test 2 results in test 1 more precipitate with Ba2+ more precipitate with Ba2+ A more precipitate with Mg2+ more precipitate with Ba2+ B more precipitate with Ba2+ more precipitate with Mg2+ C more precipitate with Mg2+ more precipitate with Mg2+ D 22 ammonium chloride A ammonium sulfate B sodium chloride C sodium hydroxide D 23 effect on pH of soil higher percentage of nitrogen by mass decrease ammonium nitrate A increase ammonium nitrate B decrease ammonium sulfate C increase ammonium sulfate D 8 ‹8&/(6 0- J dissolves in water to give an aqueous solution K. K gives a dense white precipitate when aqueous silver nitrate is added. When heated with aqueous potassium hydroxide, K gives off a gas that turns moist universal indicator paper blue. What is J? Ammonium sulfate, (NH4)2SO4, and ammonium nitrate, NH4NO3, are used as fertilisers. These salts have different percentages by mass of nitrogen. They have the same effect as each other on the pH of wet neutral soil. Which row is correct?

Theequationshowsareactionthatoccursbetweencarbonmonoxideandnitrogenmonoxideina catalyticconverter. 2CO(g)+2NO(g)→

2CO2(g)+N2(g) Whichstatementiscorrect? 24 The catalyst used is finely divided iron. A The reaction prevents greenhouse gas emissions into the atmosphere. B The reaction reduces the possibility of the formation of photochemical smog. C The reaction results in increased ozone depletion. D Which compound has the molecular formula C6H10O? 25 O O A B C D O OH The general formula for a non-cyclic alcohol is CnH2n+1OH. How many different structural isomers are there for n = 3 and n = 4? 26 n = 4 n = 3 2 2 A 4 2 B 4 3 C 8 3 D CompoundX,C5H10O3,hasonechiralcarbonatompermolecule.CompoundXproducesbubbles withNabutnotwithNa2CO3. WhichformulacouldrepresentcompoundX? 27 (CH3)2C(OH)CO2CH3 A HOCH2CH(CH3)CO2CH3 B CH3CH2C(CH3)(OH)CO2H C CH3CH(OH)CH(CH3)CO2H D 9 >7XUQRYHU 0- ‹8&/(6

Ethane reacts with an excess of chlorine in the presence of ultraviolet light to form a mixture of products. How many of these products contain two carbon atoms and one or more chlorine atoms? 28 9 D 8 C 7 B 6 A When bromoethane reacts with hot ethanolic sodium hydroxide a colourless gas is formed. This gas decolourises aqueous bromine. What is the colourless gas? 29 1,2-dibromoethane A ethanol B ethene C hydrogen bromide D Alkynes are hydrocarbons that contain one triple C≡C bond. Like alkenes, alkynes take part in addition reactions. A saturated compound can be formed. For example, ethyne, H–C≡C–H, reacts with an excess of hydrogen to form ethane. Propyne, C3H4, undergoes an addition reaction with an excess of hydrogen bromide in two stages. Markovnikov’s rule applies to the addition of HBr at each stage. What is the main product obtained when propyne reacts with an excess of hydrogen bromide? 30 CH2BrCH2CH2Br A CH3CH2CHBr2 B CH3CHBrCH2Br C CH3CBr2CH3 D Bromine reacts with alkenes by an electrophilic addition mechanism in which a cation is formed as an intermediate. Which mixture will produce the most stable intermediate cation? 31 3,3-dimethylpent-1-ene + bromine A ethene + bromine B methylpropene + bromine C propene + bromine D 10 ‹8&/(6 0-

Halogenoalkanes react with hot ethanolic potassium cyanide. The reaction mechanism is either SN1 or SN2. Which statement is correct? 32 All secondary halogenoalkanes react by the SN2 mechanism only. A Both the halogenoalkane and the cyanide ion are involved in the initial step of the SN1 mechanism. B Chloroethane reacts with cyanide ions by the SN1 mechanism only. C The SN2 mechanism involves a short-lived negatively charged transition state. D X, Y and Z are three isomeric alcohols. X CH3CH2CH2CH2CH2OH Y CH3CH2CH(OH)CH2CH3 Z (CH3)2C(OH)CH2CH3 Separatesamplesofeachalcoholarewarmedwithamildoxidisingagentandtheresultsnoted. Oneofthesealcohols,whendehydrated,willgiveapairofcis-transisomerswithmolecularformula C5H10. Whichrowiscorrect? 33 gives cis/trans isomers reacts with mild oxidising reagents Y only X, Y and Z A Z only X, Y and Z B Y only X and Y only C Z only X and Y only D Compound G gives a pale yellow precipitate with alkaline I2(aq). What could be compound G? 34 pentan-1-ol A pentan-2-ol B pentan-3-ol C 2-methylpentan-2-ol D 11 >7XUQRYHU 0- ‹8&/(6

The mechanism for the reaction between ethanal and hydrogen cyanide starts with the step shown. 35 C H H O H C H CN– What is the correct structure of the intermediate ion formed, and what is the next step in this mechanism? C H H C A H H CN H C N +O C H H C B H H CN H C N – O C H H C C C H H C H H CN H C N – O D H H CN H C N +O Which compound reacts with 2,4-dinitrophenylhydrazine reagent but does not react with Tollens’ reagent? 36 CH3COCO2H A CH3CH(OH)CHO B CH3COCHO C CH3CH(OH)CH3 D Compound X has stereoisomers and forms a precipitate when warmed with Fehling’s reagent. What could be the structure of compound X? 37 O A O B O C O D 12 ‹8&/(6 0-

Which reaction will form propanoic acid? 38 acidic hydrolysis of propyl ethanoate A alkaline hydrolysis of ethyl propanoate B acidic hydrolysis of propanenitrile C acidic hydrolysis of ethanenitrile D Lactide is an intermediate in the manufacture of a synthetic fibre. 39 O O lactide O O Which compound, on heating with an acid catalyst, can produce lactide? hydroxyethanoic acid A 2-hydroxybutanoic acid B 2-hydroxypropanoic acid C 3-hydroxypropanoic acid D The diagram shows the relative abundance of different isotopes of lead in a sample of lead ore. The abundance of 208 is half that of 206. The abundances of 208 and 209 are equal. 40 100 75 50 25 0 % abundance 206 207 208 209 Ar What is the relative atomic mass of the lead in the sample? 207.67 D 207.50 C 207.25 B 207.00 A 13 0- ‹8&/(6

BLANK PAGE 14 ‹8&/(6 0-

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‹8&/(6 0- ,PSRUWDQWYDOXHVFRQVWDQWVDQGVWDQGDUGV  PRODUJDVFRQVWDQW R -.± PRO± )DUDGD\FRQVWDQW F  u &PRO± $YRJDGURFRQVWDQW L u PRO± HOHFWURQLFFKDUJH e ±u± & PRODUYROXPHRIJDV VP GP PRO±DWVWS N3DDQG.  VP GP PRO±DWURRPFRQGLWLRQV LRQLFSURGXFWRIZDWHU KZ u± PRO GP± DW . q&  VSHFLILFKHDWFDSDFLW\RIZDWHU c N-NJ± .± -J± .±  15

‹8&/(6 0- 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 – 16

This document consists of 3 printed pages. © UCLES 2023 [Turn over Cambridge International AS & A Level CHEMISTRY 9701/12 Paper 1 Multiple Choice May/June 2023 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 May/June 2023 series for most Cambridge IGCSE, Cambridge International A and AS Level and Cambridge Pre-U components, and some Cambridge O Level components.

9701/12 Cambridge International AS & A Level – Mark Scheme PUBLISHED May/June 2023 © UCLES 2023 Page 2 of 3 Question Answer Marks 1 C 1 2 B 1 3 D 1 4 C 1 5 B 1 6 D 1 7 B 1 8 B 1 9 B 1 10 D 1 11 C 1 12 B 1 13 B 1 14 B 1 15 C 1 16 C 1 17 D 1 18 D 1 19 C 1 20 A 1 21 B 1 22 A 1 23 A 1 24 C 1 25 A 1 26 B 1 27 B 1 28 D 1

9701/12 Cambridge International AS & A Level – Mark Scheme PUBLISHED May/June 2023 © UCLES 2023 Page 3 of 3 Question Answer Marks 29 C 1 30 D 1 31 C 1 32 D 1 33 C 1 34 B 1 35 D 1 36 A 1 37 D 1 38 C 1 39 C 1 40 B 1