Chemistry 9701/12 October/November 2023: question paper and mark scheme

Question

Which particle contains 8 protons, 9 neutrons and 10 electrons? A B C D

Question

The second ionisation energy of oxygen is greater than the second ionisation energy of fluorine. Which factor explains this difference? A The atomic radius of an oxygen atom is smaller than that of fluorine. B The covalent bond in a fluorine molecule is weaker than the bond in an oxygen molecule. C A spin-paired electron is removed from fluorine but not from oxygen. D Fluorine has more electrons in total than oxygen. This causes a greater shielding of the nuclear attraction in fluorine.

Question

Zinc reacts with concentrated nitric acid giving three products only: zinc nitrate, an oxide of nitrogen and water. 2+ 3.0 moles of zinc react with 8.0 moles of nitric acid. Zinc nitrate contains Zn ions. What could be the formula of the oxide of nitrogen? A N2O B NO C N2O3 D NO2 3 –3

Question

A 3.7 g sample of copper(II) carbonate is added to 25 cm of 2.0 mol dm hydrochloric acid. Which volume of gas is produced at room conditions? 3 3 3 3 A 0.60 dm B 0.72 dm C 1.20 dm D 2.40 dm +

Question

Ammonium ions, NH4 , are formed when ammonia gas reacts with hydrogen chloride gas. Which statement about the changes that occur in this reaction is correct? A The dipole moment of an ammonium ion is greater than the dipole moment of an ammonia molecule. B The H−N−H bond angle decreases when an ammonium ion is formed. C The hybridisation of nitrogen does not change. D There is electron transfer from nitrogen to chlorine.

Question

Which feature is present in both ethene and poly(ethene)? A bond angles of 109.5° B covalent bonds C covalent bonds D 3 sp orbitals

Question

Two compounds of boron are sodium borohydride, NaBH4, and boron trifluoride, BF3. What are the shapes of the borohydride ion and the boron trifluoride molecule? borohydride ion boron trifluoride A square planar pyramidal B square planar trigonal planar C tetrahedral pyramidal D tetrahedral trigonal planar 3

Question

In an experiment, 0.100 mol of propan-1-ol is burnt completely in 12.0 dm of oxygen, measured at room conditions. What is the final volume of gas, measured at room conditions? 3 3 3 3 A 7.20 dm B 8.40 dm C 16.80 dm D 18.00 dm –4

Question

At a temperature of 2500 K and a pressure of 1.00 × 10 Pa, a sample of 0.321 g of sulfur vapour 6 3 has a volume of 2.08 × 10 m . What is the molecular formula of sulfur under these conditions? A S B S2 C S4 D S8

Question

In the structure of solid SiO2 each silicon atom is bonded to x oxygen atoms each oxygen atom is bonded to y silicon atoms each bond is a z type bond. What is the correct combination of x, y and z in these statements? x y z A 2 1 covalent B 2 1 ionic C 4 2 covalent D 4 2 ionic

Question

Nitric acid is made industrially by the oxidation of ammonia. The overall equation for the process is shown. equation 1 NH3 + 2O2 → HNO3 + H2O The process happens in three stages. The equations and enthalpy changes for these stages are given. 4NH3 + 5O2 → 4NO + 6H2O −1 stage 1 H = −904 kJ mol 2NO + O2 → 2NO2 −1 stage 2 H = −114 kJ mol 4NO2 + O2 + 2H2O → 4HNO3 −1 stage 3 H = −348 kJ mol What is the enthalpy change of the process shown in equation 1? −1 A −1480 kJ mol −1 B −370 kJ mol −1 C −341.5 kJ mol −1 D +82 kJ mol

Question

Chlorine reacts with sodium bromide. Cl 2 + NaBr → NaCl + Br2 Which words correctly describe this reaction? 1 redox 2 displacement 3 disproportionation A 1, 2 and 3 B 1 and 2 only C 1 only D 2 only

Question

The equation for the reaction between aqueous copper ions and aqueous iodide ions is as follows. 2+ – 2Cu (aq) + 4I (aq) → 2CuI(s) + I2(aq) What is the change in oxidation state of copper? A +2 to –1 B +2 to 0 C +2 to +1 D +4 to +2

Question

A mixture of the three gases, oxygen, nitrogen and argon, is at a total pressure of 500 kPa. There is a total of 1.2 moles of gas in the mixture. If the oxygen gas alone occupied the entire volume of the mixture, it would exert a pressure of 150 kPa. 3 At room conditions the amount of nitrogen gas in the mixture would occupy a volume of 5.76 dm . What is the partial pressure of the argon gas in the mixture? A 150 kPa B 200 kPa C 250 kPa D 300 kPa 3 15 0.200 mol of sulfur dioxide and 0.200 mol of oxygen are placed in a 1.00 dm sealed container. The gases are allowed to react until equilibrium is reached. 2SO2 + O2 2SO3 At equilibrium there is 0.100 mol of SO3 in the container. What is the value of Kc? –3 A 0.150 mol dm –3 B 0.800 mol dm –1 3 C 1.25 mol dm –1 3 D 6.67 mol dm

Question

In the question paper above.

Question

The decomposition of hydrogen peroxide in the presence of MnO2 produces water and oxygen gas. 2H2O2(aq) → 2H2O(l) + O2(g) The volume of gas collected when 0.2 g of MnO2 is added to two different hydrogen peroxide solutions at 20 °C is shown on the graph as curves X and Y. X Y volume of gas 0 0 time Which row shows the conditions that will result in curves X and Y? curve X curve Y concentration concentration volume of form of volume of form of 3 ofH2O2 3 ofH2O2 H2O2 / cm –3 MnO2 H2O2 / cm –3 MnO2 /moldm /moldm A 50 0.1 lumps 50 0.2 powder B 25 0.2 powder 25 0.1 lumps C 50 0.1 lumps 20 0.2 powder D 20 0.2 powder 40 0.1 lumps

Question

The diagram shows a gas syringe with a free-moving piston. The syringe contains gaseous hydrogen, gaseous iodine and gaseous hydrogen iodide at equilibrium. gaseous hydrogen, gaseous iodine and gaseous hydrogen iodide sealed end piston H2(g) + I2(g) 2HI(g) Three changes are listed. 1 increasing the total pressure by adding an inert gas and keeping the volume constant 2 increasing the pressure by adding more gaseous hydrogen iodide and keeping the volume constant 3 decreasing the volume by pushing the piston to the left Which changes will result in an equilibrium position at which the rate of the forward reaction has increased? A 2 only B 1 and 2 C 1 and 3 D 2 and 3

Question

Which row gives the best description of the variations in the melting points and the first ionisation energies of the elements in Period 3 from sodium to argon? melting points first ionisation energies A increase up to a peak at aluminium then decrease generally decrease B increase up to a peak at aluminium then decrease generally increase C increase up to a peak at silicon then decrease generally decrease D increase up to a peak at silicon then decrease generally increase

Question

X and Y are atoms of different elements in Period 3 of the Periodic Table. Neither X nor Y is argon. X is a non-metal. X has a greater atomic radius than Y. Which statement is correct? A X has more occupied electron shells than Y. B X has more protons in each atom than Y. C X has the same number of outer electrons in each atom as Y. D Y is a non-metal. 3

Question

Four mixtures are added to four separate 50 cm samples of water and stirred. Which mixture results in a solution with the highest pH? A 1.0 g of aluminium oxide and 1.0 g of aluminium chloride B 1.0 g of magnesium oxide and 1.0 g of magnesium chloride C 1.0 g of phosphorus oxide and 1.0 g of phosphorus chloride D 1.0 g of silicon dioxide and 1.0 g of silicon chloride

Question

What happens when a piece of magnesium ribbon is placed in cold water? A A vigorous effervescence occurs. B Bubbles of gas form slowly on the magnesium. C The magnesium floats on the surface of the water and reacts quickly. D The magnesium glows and a white solid is produced.

Question

The table gives some data for compounds of two elements from Group 2 of the Periodic Table. decomposition solubility of sulfate solubility of hydroxide element temperature of in mol / 100 g in mol / 100 g carbonate / °C of water of water –3 –3 calcium 840 4.66 × 10 1.53 × 10 –5 Z ? ? 2.00 × 10 What is the missing data for element Z? decomposition solubility of sulfate temperature of in mol / 100 g carbonate / °C of water –1 A 350 1.83 × 10 –5 B 350 7.11 × 10 –1 C 1100 1.83 × 10 –5 D 1100 7.11 × 10

Question

Q is a mixture of two compounds of Group 2 elements. Q undergoes thermal decomposition to produce a white solid and only two gaseous products. One of the gaseous products relights a glowing splint. What could be the components of mixture Q? A MgCl 2 and CaCO3 B MgCO3 and Ca(NO3)2 C Mg(NO3)2 and Ca(NO3)2 D MgO and CaO

Question

Iodine has a higher melting point than chlorine. What is the reason for this? A Iodine has stronger covalent bonds than chlorine. B Iodine molecules have stronger permanent dipoles than chlorine molecules. C Iodine is more volatile than chlorine. D Iodine has stronger instantaneous dipole–induced dipole forces than chlorine.

Question

When concentrated sulfuric acid is added to solid sodium chloride, HCl is formed but not Cl 2. When concentrated sulfuric acid is added to solid sodium iodide, I2 is formed. Which statement explains these observations? A Sulfuric acid is an oxidising agent and chloride ions are more easily oxidised than iodide ions. B Sulfuric acid is an oxidising agent and iodide ions are more easily oxidised than chloride ions. C Sulfuric acid is a reducing agent and chloride ions are more easily reduced than iodide ions. D Sulfuric acid is a reducing agent and iodide ions are more easily reduced than chloride ions.

Question

NaOH(aq) is added to NH4Cl (aq). The mixture is warmed. The gas that is produced turns damp red litmus paper blue. Which row is correct? behaviour of the ammonium behaviour of the water present ion in NH4Cl on the litmus paper A Brønsted–Lowry acid Brønsted–Lowry base B Brønsted–Lowry acid Brønsted–Lowry acid C Brønsted–Lowry base Brønsted–Lowry acid D Brønsted–Lowry base Brønsted–Lowry base

Question

Artemisinin is a powerful anti-malarial drug. artemisinin CH3 O O CH3 O O O CH3 How many chiral centres are there in each molecule of artemisinin? A 4 B 6 C 7 D 8

Question

Which row shows the correct name and classification of the halogenoalkane shown? CH3(CH2)2CBr(CH3)CH2CH3 classification of name halogenoalkane A 3-bromo-3-methylhexane secondary B 3-bromo-3-methylhexane tertiary C 3-bromo-4-methylhexane tertiary D 4-bromo-5-methylhexane secondary

Question

How many geometrical (cis/trans) isomers are there of hex-2,4-diene, CH3CH=CHCH=CHCH3? A none; hex-2,4-diene does not show geometric isomerism B 2 C 3 D 4

Question

The structure of compound X is shown. compound X One mole of compound X reacts completely with two moles of hydrogen bromide. What is the structure of the major product of this reaction? A B Br Br Br Br C D Br Br Br Br

Question

The formulae of three compounds are shown. C3H7CHO C2H5COCH3 CH2CHCH2CH2OH Only one of these compounds will decolourise bromine water. Only one of these compounds will produce a silver mirror with Tollens’ reagent. Which row shows the correct results? forms a silver mirror with decolourises bromine water Tollens’ reagent A C3H7CHO C2H5COCH3 B C2H5COCH3 C3H7CHO C CH2CHCH2CH2OH C2H5COCH3 D CH2CHCH2CH2OH C3H7CHO

Question

Which list contains a compound that is not made during the free radical substitution of methane with chlorine? A CH3Cl , CCl 4, C2H6 B Cl 2, CH2Cl 2, CCl 4 C CH3Cl , CH2Cl 2, CHCl 3 D CH3Cl , CHCl 3, C2H2Cl 2

Question

Propanoic acid can be used to make propene by a two-stage synthesis. Which row shows suitable reagents for this synthesis? reagent for first stage reagent for second stage A LiAl H4 conc. H2SO4 B LiAl H4 NaOH in ethanol C NaBH4 conc. H2SO4 D NaBH4 NaOH in ethanol

Question

Which alcohol reacts with alkaline I2(aq) to produce ethanoate ions? A ethanol B methylpropan-2-ol C propan-2-ol D butan-2-ol

Question

HeatingcompoundX,C7H14O2,underrefluxwithanexcessofacidifiedpotassiumdichromate(VI) producescompoundY. CompoundYproduceshydrogengaswithsodiummetalandformsorangecrystalswith2,4-DNPH reagent. Whatcould;be? A B C D CH2OH OH CH3 OH (CH3)2C(OH)CH2CH2CH2CHO CH3 CH2OH OH OH

Question

Which reaction takes place by a nucleophilic addition mechanism? A propene reacting with hydrogen bromide B 2-bromopropane reacting with sodium hydroxide in ethanol C propanone reacting with hydrogen cyanide D methane reacting with chlorine

Question

Three equations are shown. 1 CH3COOH + MgCO3 → CH3COOMg + CO2 + H2O 2 CH3CH2COOH + Na → CH3CH2COONa + H2 3 CH3CH2COOH + 2Ba(OH)2 → CH3CH2COOBa2 + 2H2O Which of the equations are correct? A 1, 2 and 3 B 1 and 2 only C 2 only D 3 only

Question

How many esters with the molecular formula C5H10O2 can be made by reacting a primary alcohol with a carboxylic acid? A 4 B 5 C 6 D 8

Question

The diagram shows an ester. It is heated under reflux with an excess of NaOH(aq). O O Which row shows the 2 products of the reaction? product 1 product 2 A O OH OH B O ONa OH C O OH ONa D O ONa ONa 16 17 18

Question

Oxygen has three stable isotopes, O, O and O. All three isotopes are present in a sample of oxygen gas, O2, which was analysed using a mass spectrometer. + How many peaks associated with the O2 ion would be expected? A 3 B 5 C 6 D 9 Important values, constants and standards –1 –1 molar gas constant R = 8.31 J K mol 4 –1 Faraday constant F = 9.65 × 10 C mol 23 –1 Avogadro constant L = 6.022 × 10 mol –19 electronic charge e = –1.60 × 10 C 3 –1 molar volume of gas Vm = 22.4 dm mol at s.t.p. (101 kPa and 273 K) 3 –1 Vm = 24.0 dm mol at room conditions –14 2 –6 ionic product of water Kw = 1.00 × 10 mol dm (at 298 K (25 °C)) specific heat capacity of –1 –1 –1 –1 c = 4.18 kJ kg K (4.18 J g K ) water 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 www.cambridgeinternational.org after the live examination series. 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 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 16 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 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 11_9701_12_2023_1.11R 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 – – – – – – – – – – – International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge Assessment