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

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Element X has six more protons than element Y. Which statement must be correct? 1 Atoms of element Y are smaller than atoms of element X. A Element X has a full shell of electrons. B Element X and element Y are in the same group. C Element X and element Y are in the same period. D Which statement explains why calcium has a higher melting point than barium? 2 Calcium cations are smaller than barium cations and have a stronger attraction to the delocalisedelectrons. A The structure of calcium is partly giant molecular. B C Therearemoredelocalisedelectronsincalciumthaninbariumasithasalowerionisation energy. There is greater repulsion between barium atoms as they have more complete electron shellsthancalciumatoms. D Three statements about potassium and chlorine and their ions are listed. 3 The atomic radius of a potassium atom is greater than the atomic radius of a chlorine atom. 1 The first ionisation energy of potassium is greater than the first ionisation energy of chlorine. 2 The ionic radius of a potassium ion is greater than the ionic radius of a chloride ion. 3 Which statements are correct? 2 and 3 D 1 and 3 C 2 only B 1 only A For which equilibrium do both of the equilibrium constants Kc and Kp have no units? 4 H2(g) + I2(g) ⇋2HI(g) A N2(g) + 3H2(g) ⇋2NH3(g) B N2O4(g) ⇋2NO2(g) C SO2(g) + O2(g) ⇋SO3(g) D 2 ‹8&/(6 0-

Calciumcarbide,CaC2,reactswithwater,asshown.Thedatabelowtheequationshow,inkJmol–1, thestandardenthalpiesofformationofthecompoundsinvolved. 5 C2H2(g) + CaO(s) → H2O(l) + CaC2(s) +228 –635 –286 –60 What is the standard enthalpy change of the reaction shown? –753kJmol–1 A –61kJmol–1 B +61kJmol–1 C +753kJmol–1 D Inthesodiumchloridelatticethenumberofchlorideionsthatsurroundeachsodiumioniscalled thecoordinationnumberofthesodiumions. Whatarethecoordinationnumbersofthesodiumionsandthechlorideionsinthesodiumchloride lattice? 6 coordination number of chloride ions coordination number of sodium ions 6 4 A 4 6 B 6 6 C 6 8 D 3 ‹8&/(6 0- [Turn over

Histidine is an amino acid. 7 histidine C C C H H N C C H O O N H N H H H C H H 1 2 3 What are the approximate bond angles 1, 2, and 3? 3 2 1 90° 107° 109.5° A 109.5° 107° 120° B 90° 120° 120° C 109.5° 120° 120° D The Contact process takes place at a pressure between 100000Pa and 200000Pa. A catalyst is used. Which statement is correct? 8 A V2O5 catalyst is added to increase the equilibrium yield of the reaction. A Changes in pressure have no effect on the position of equilibrium. B The equilibrium yield of the reaction is very high under the conditions used. C An iron catalyst is added to increase the rate of reaction. D 4 0- ‹8&/(6

Bromine reacts with aqueous sodium hydroxide at 25 °C. reaction 1 Br2(aq) + 2NaOH(aq) →NaBr(aq) + NaOBr(aq) + H2O(l) The NaOBr formed is unstable at 25 °C and reacts further. reaction 2 3NaOBr(aq) →2NaBr(aq) + NaBrO3(aq) Which reactions are disproportionations? 9 both reaction 1 and reaction 2 A neither reaction 1 nor reaction 2 B reaction 1 only C reaction 2 only D Which statement is correct? 10 The relative atomic mass of a 35Cl atom is 35.5. A The relative formula mass of CaCO3 is 100.1. B The relative isotopic mass of a 24Mg atom is 24.3. C The relative molecular mass of O2 is 16.0. D Iodine and propanone react according to the following equation. I2(aq) + CH3COCH3(aq) →CH3COCH2I(aq) + HI(aq) If the concentration of propanone is increased, keeping the total reaction volume constant, the initial rate of the reaction also increases. What could be the reason for this? 11 A greater proportion of collisions are successful at the higher concentration. A The particles are further apart at the higher concentration. B The particles have more energy at the higher concentration. C There are more collisions per second between particles at the higher concentration. D 5 0- ‹8&/(6 [Turn over

Four successive ionisation energies (IE) of element E are shown. Element E is in Period 3 of the Periodic Table. 12 eighth IE /kJmol–1 seventh IE /kJmol–1 sixth IE /kJmol–1 fifth IE /kJmol–1 29000 24000 20000 16000 In which group of the Periodic Table is E? 17 D 16 C 15 B 14 A In this question you should assume that the gas formed behaves as an ideal gas. A 1.7g sample of Mg reacts with 50.0cm3 of 2.2moldm–3 HCl at 303K and 110400Pa. Which volume of gas is produced, measured under these conditions? 13 5.0dm3 D 2.5dm3 C 1.6dm3 B 1.3dm3 A Chlorine dioxide, ClO2, reacts with aqueous sodium hydroxide to produce water and a mixture of two sodium salts, NaClO2 and NaClO3. What is the mole ratio of NaClO2 to NaClO3 in the product mixture? 14 5:3 D 1:1 C 3:5 B 1:2 A The temperature of a sample of an inert gas is increased. What effect does this have on the number of molecules with the most probable energy and on the number of molecules with higher energy? 15 number of molecules with higher energy number of molecules with the most probable energy decreases decreases A increases decreases B decreases increases C increases increases D 6 0- ‹8&/(6

For which compound is there the greatest percentage loss of mass on strong heating? 16 anhydrous calcium carbonate A anhydrous calcium nitrate B anhydrous magnesium carbonate C anhydrous magnesium nitrate D The solids sodium chloride and sodium iodide both react with concentrated sulfuric acid at room temperature. With NaCl, the products are NaHSO4 and HCl. With NaI, the products are NaHSO4, HI, I2, SO2, H2O, S and H2S. What is the explanation for this difference in products? 17 Chloride ions will displace iodine from the solution. A Hydrogen chloride is more volatile than hydrogen iodide. B Iodide ions are better reducing agents than chloride ions. C Sulfuric acid is able to act as a dehydrating agent with NaI. D SiO2 has a melting point of 1713 °C. It reacts with hot NaOH(aq) to form sodium silicate, Na2SiO3, and water. No reaction occurs when SiO2 is added to hot H2SO4(aq). What can be deduced from this information? 18 structure of SiO2 chemical behaviour of SiO2 giant amphoteric A simple amphoteric B giant acidic C simple acidic D 7 0- ‹8&/(6 [Turn over

Element X has the second largest atomic radius in its period. An atom of X has three occupied electron shells only. The oxide of X is shaken with water. What could be the pH of the resulting solution? 19 14 D 9 C 7 B 5 A Which emission from an internal combustion engine contributes to the erosion of marble statues? 20 carbon monoxide A nitrogen B nitrogen dioxide C unburnt hydrocarbons D The diagram shows the melting points of eight elements with consecutive atomic numbers. Which element could be sodium? 21 melting point / K atomic number A B C D 8 0- ‹8&/(6

The boiling points of Br2, ICl and IBr are given in the table. 22 IBr ICl Br2 116 97 59 boiling point/°C Which row explains: boiling point of IBr is greater than ICl boiling point of ICl is greater than Br2 IBr has stronger instantaneous dipole-induced dipoles ICl has stronger instantaneous dipole-induced dipoles A IBr has stronger instantaneous dipole-induced dipoles ICl has permanent dipoles B IBr has stronger permanent dipoles ICl has stronger instantaneous dipole-induced dipoles C IBr has stronger permanent dipoles ICl has permanent dipoles D A solution contains both Mg2+(aq) and Sr2+(aq) at the same concentration. The solution is divided into two equal portions. Aqueous sodium hydroxide is added dropwise to one portion. Dilute sulfuric acid is added dropwise to the other portion. Which row is correct? 23 precipitate seen first when H2SO4(aq) is added precipitate seen first when NaOH(aq) is added magnesium sulfate magnesium hydroxide A strontium sulfate magnesium hydroxide B magnesium sulfate strontium hydroxide C strontium sulfate strontium hydroxide D 9 • whytheboilingpointofIClisgreaterthanBr2 • whytheboilingpointofIBrisgreaterthanICl? 0- ‹8&/(6 [Turn over

Structural isomerism and stereoisomerism should be considered when answering this question. If a molecule contains two non-identical chiral carbon atoms, four optical isomers exist. How many isomers are there with: 24 • molecular formula C7H14O and • a five-membered ring and • a tertiary alcohol group? 13 D 9 C 5 B 4 A Which reagent will react with pentan-3-ol to give a mixture of stereoisomers? 25 acidified potassium dichromate A concentrated sulfuric acid B ethanoic acid in the presence of a little concentrated H2SO4 C hydrogen chloride D An organic molecule W contains 3 carbon atoms. It requires 4.5 molecules of oxygen for complete combustion. What could W be? 26 propane A propanoic acid B propanone C propan-1-ol D Which equation represents a reaction that proceeds through initiation, propagation and termination steps? 27 C4H10 + Cl 2 →C4H9Cl + HCl A C5H11Br + NaOH →C5H11OH + NaBr B C6H12 + H2O →C6H13OH C C6H13CHO + HCN →C6H13CH(OH)CN D 10 0- ‹8&/(6

Structural
isomerism
and
stereoisomerism
should
be
considered
when
answering
this
question.
A
set
of
isomeric
hydrocarbons 28 • allcontain14.3%bymassofhydrogen • allreactwithbrominebyaddition,0.280gofeachhydrocarbonreactingwith0.799gof
bromine. What is the maximum number of isomeric compounds in the set? 5 D 4 C 3 B 1 A Which row describes the solvent used and type of reaction occurring when bromoethane reacts with NaOH to form ethene? 29 type of reaction solvent elimination ethanol A substitution ethanol B elimination water C substitution water D Whichrowdescribesthetypeofreactionthatoccurswhenpropan-1-olreactstoformthenamed carbon-containingproduct? 30 type of reaction carbon-containing product addition to propan-1-ol 1-chloropropane A complete combustion of propan-1-ol carbon monoxide B dehydration of propan-1-ol propene C reduction of propan-1-ol propanal D Which statement describes what happens when 2-chloro-2-methylpropane is warmed with NaOH(aq)? 31 This secondary halogenoalkane reacts by a mixture of an SN1 and an SN2 mechanism. A This secondary halogenoalkane reacts only by an SN2 mechanism. B This tertiary halogenoalkane reacts mostly by an SN1 mechanism. C This tertiary halogenoalkane does not react with hydroxide ions under these conditions. D 11 0- ‹8&/(6 [Turn over

How many structurally isomeric secondary alcohols are there with the molecular formula C5H12O? 32 4 D 3 C 2 B 1 A Which reagent: 33 • canconfirmthepresenceofacarbonylgroupinanorganiccompound • doesnotdistinguishbetweenaldehydesandketones? acidified K2Cr2O7 A 2,4-DNPH reagent B Fehling’s reagent C LiAlH4 D Whichcompoundgivesapositivetestwithalkalineaqueousiodineanddoesnotshowoptical isomerism? 34 CH3COCH2CH2OH A CH3CH2CH(OH)CHO B CH3COCH(OH)CH3 C (CH3)2C(OH)CHO D 12 0- ‹8&/(6

TwosamplesofcompoundXweretreatedseparatelywithdifferentreagentswhichwereaddedin excess. Theproductsofthesetworeactionsareshown. 35 O O OH O O OH OH compound X OH OH OH reaction 1 reaction 2 Which reagents could be used for reaction 1 and reaction 2? reaction 2 reaction 1 Na A NaBH4 B Na C NaBH4 hot acidifiedsodiumdichromate VI  hot acidifiedsodiumdichromate VI  Tollens’reagentfollowedbyHCl(aq) Tollens’reagentfollowedbyHCl(aq) D Which method could produce butanoic acid? 36 an acid–base reaction involving CH3CH2CH2CO2Na A the hydrolysis of CH3CH2CH2CH2CN B the acidic hydrolysis of CH3CH2COOCH2CH2CH3 C the oxidation of CH3CH2CH2OH D 13 0- ‹8&/(6 [Turn over

Which
ester
may
be
hydrolysed
to
produce
two
products,
one
of
which
may
be
reduced
to
the
other? 37 CH3CH2CO2CH3 A CH3CH(CH3)CO2CH2CH(CH3)2 B CH3CH2CO2CH(CH3)2 C (CH3)2CHCO2CH(CH3)2 D Two compounds, X and Y, are mixed and a little concentrated H2SO4 is added. Ester Z is found in the resulting mixture of products. 38 ester Z O O O O O O Which two compounds could be X and Y? Y X CH(CO2H)3 CH3CH2OH A CH3CO2CH2CH(OH)CH2OCOCH2CH3 CH3CH2OH B CH3CH2CO2CH2CH(OH)CH2OH CH3CO2H C CH2(OH)CH(OH)CH2(OH) CH3CO2H D The diagram shows a section of a polymer molecule. –CH2–CH=CH–CH2–CH2–CH=CH–CH2– Which monomer will produce this polymer? 39 CH2=CH2 A CH3CH=CH2 B CH3CH=CHCH3 C CH2=CH–CH=CH2 D 14 0- ‹8&/(6

40 There
are
two
naturally
occuring
isotopes
of
bromine.
One
isotope
has
44
neutrons.
The
other
isotope
has
46
neutrons. Ignoring
fragments,
how
many
peaks
are
there
in
the
mass
spectrum
of
tribromomethane,
12C1HBr3? A 2
B 3
C 4
D 6 15 0- ‹8&/(6

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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 –  0- ‹8&/(6

This document consists of 3 printed pages. © UCLES 2023 [Turn over Cambridge International AS & A Level CHEMISTRY 9701/11 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.

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

9701/11 Cambridge International AS & A Level – Mark Scheme PUBLISHED May/June 2023 © UCLES 2023 Page 3 of 3 Question Answer Marks 29 A 1 30 C 1 31 C 1 32 C 1 33 B 1 34 A 1 35 D 1 36 A 1 37 B 1 38 C 1 39 D 1 40 C 1