Chemistry 9701/11 October/November 2025: question paper and mark scheme

Question

What is the electronic configuration for the particle 27 + 13 Al ? A 1s22s22p63s13p1 B 1s22s22p63s2 C 1s22s22p63s23p2 D 1s22s22p63s23p63d74s1

Question

The data in the table gives the 5th to the 10th ionisation energies of three elements from Period 3 of the Periodic Table. ionisation energy / kJ mol–1 element 5th 6th 7th 8th 9th 10th X 6274 21 269 25 398 29 855 35 868 40 960 Y 7012 8 496 27 107 31 671 36 579 43 140 Z 6542 9 362 11 018 33 606 38 601 43 963 What are the correct identities of these three elements? element X element Y element Z A Na Mg Al B Mg Al Si C P S Cl D S Cl Ar

Question

What contains 9.03 × 1023 oxygen atoms? A 0.25 mol aluminium oxide B 0.75 mol sulfur dioxide C 1.5 mol sulfur trioxide D 3.0 mol water

Question

Methane and steam react to produce hydrogen. CH4(g) + 2H2O(g) → CO2(g) + 4H2(g) 0.80 g of methane and 1.35 g of steam react. One of the reactants is used up. Which volume of hydrogen, measured at room conditions, will be produced? A 1.80 dm3 B 3.60 dm3 C 4.80 dm3 D 7.20 dm3

Question

Which statement explains why sodium and potassium have different melting points? A The attraction between cations and delocalised electrons is stronger in sodium. B The attraction between cations and anions is stronger in sodium. C The attraction between atoms is stronger in sodium. D The attraction between nuclei and shared electron pairs is stronger in sodium.

Question

NH3 and HCN react together to form NH4CN, an ionic compound. Which row states the number of coordinate bonds and the number of π bonds in one formula unit of NH4CN? number of number of coordinate bonds π bonds A 0 2 B 1 2 C 0 3 D 1 3

Question

When 1.0 mol of ethanoic acid, CH3COOH, in aqueous solution is neutralised by an excess of aqueous sodium hydroxide, 55 kJ mol–1 of energy is released. Which statement about this reaction is correct? A The reaction is exothermic because only bond breaking takes place. B The reaction is exothermic because only bond forming takes place. C The reaction is exothermic because more energy is given out in breaking bonds than is taken in to form bonds. D The reaction is exothermic because more energy is given out in forming bonds than is taken in to break bonds.

Question

In an experiment, 1.60 g of a fuel is burnt. 45.0% of the energy released is absorbed by 200 g of water. The temperature of the water rises from 18.0 °C to 66.0 °C. What is the total energy released per gram of fuel burnt? A 25 100 J B 55 700 J C 89 200 J D 143 000 J

Question

Sulfite ions, SO32–, react separately with zinc and with manganese dioxide. a, b, c, d, w, x, y and z are all whole numbers. aSO32–(aq) + b H2O(l) + Zn(s) → Zn2+(aq) + c OH–(aq) + d S2O42–(aq) MnO2(s) + w SO32–(aq) + x H+(aq) → Mn2+(aq) + y S2O62–(aq) + z H2O(l) Which numbers are correct for a, b, w and x? a b w x A 1 2 2 4 B 2 2 2 4 C 1 2 4 2 D 2 2 4 2

Question

Which equation shows hydrogen acting as an oxidising agent? A H2 + 2K → 2K+H– B H2 + I2 → 2HI C H2 + Cu2S + ZnO → 2Cu + ZnS + H2O D 3H2 + N2 → 2NH3 11 1.00 g of nitrogen gas is stored in a 2.00 dm3 vessel at 40.0 °C. What is the pressure in the vessel? A 5940 Pa B 11 900 Pa C 46 400 Pa D 92 900 Pa

Question

In the question paper above.

Question

One molecule of haemoglobin, Hb, can bind with four molecules of oxygen according to the equation shown. Hb(aq) + 4O2(aq) Hb(O2)4(aq) When the equilibrium concentration of O2 is 7.6 × 10–6 mol dm–3, the equilibrium concentrations of Hb and Hb(O2)4 are equal. What is the numerical value of Kc for this equilibrium? A 3.0 × 1020 B 1.3 × 105 C 7.6 × 10–6 D 3.3 × 10–21

Question

Aqueous acid P and aqueous alkali Q have the same concentration. 20 cm3 of P is added to a conical flask. Q is slowly added to the flask and the volume of Q and the pH are recorded. The pH titration curve is shown. 14 12 10 8 pH 6 4 2 0 0 2 4 6 8 10 12 14 16 18 20 22 24 26 28 30 volume of Q added / cm3 Which row gives the identity of P and Q? P Q A HCl NaOH B H2SO4 NH3 C HCl Ba(OH)2 D CH3COOH Sr(OH)2

Question

Photochromic glass, used for sunglasses, darkens when exposed to bright light and becomes more transparent again when the light is less bright. The darkness of the glass is due to the presence of silver atoms. The following reactions are involved. reaction 1 Ag+ + Cl – Ag + Cl reaction 2 Cu+ + Cl → Cu2+ + Cl – reaction 3 Cu2+ + Ag → Cu+ + Ag+ Which statement about these reactions is correct? A Cu+ and Cu2+ ions act as catalysts. B Cu+ ions act as an oxidising agent in reaction 2. C Reaction 3 increases the darkness of the glass. D Silver atoms are reduced in reaction 3.

Question

The reversible reaction between methanol and ethanoic acid liquids is catalysed by adding a small volume of concentrated sulfuric acid. Two statements about this reaction are listed. 1 The sulfuric acid is a homogeneous catalyst. 2 The sulfuric acid lowers the activation energy of the reverse reaction. Which statements are correct? A both 1 and 2 B 1 only C 2 only D neither 1 nor 2

Question

The atomic radii and ionic radii for three elements in Period 3 are shown. atomic radius / nm ionic radius / nm element X 0.118 0.053 element Y 0.099 0.180 element Z 0.160 0.072 Using this data, which statement is correct? A Element X has lower electrical conductivity than element Y. B Element Y has a higher melting point than element X. C Element Y and element Z react to form an ionic compound. D Element Z forms ionic compounds by gaining electrons.

Question

Three equations are listed. x, y and z are all whole numbers. 1 x Al + y O2 → zAl 2O3 2 x Mg + y O2 → z MgO 3 x Na + y O2 → z Na2O Which equations can be balanced if x = 4 and z = 2? A 1 and 3 B 1 only C 2 only D 3 only

Question

Which oxide has a simple structure rather than a giant structure? A MgO B Al 2O3 C SiO2 D P4O10

Question

The trends seen in Group 2 can be used to predict the properties of radium and its compounds. Which statement is correct? A Radium has the highest second ionisation energy of the elements in Group 2. B Radium hydroxide is the least soluble of the hydroxides of the elements in Group 2. C Radium carbonate has the lowest thermal stability of the carbonates of the elements in Group 2. D Radium reacts faster with water than the other elements in Group 2.

Question

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

Question

Equation 1 and equation 2 show two different reactions of halide ion Q– with concentrated sulfuric acid. equation 1 H2SO4 + Q– → HSO4– + HQ equation 2 H2SO4 + 2Q– + 2H+ → SO2 + Q2 + 2H2O What is Q? A Cl – or Br – B Br – or I – C Cl – only D I – only

Question

What happens when iodine solution is added to a solution of sodium bromide? A A reaction occurs without changes in oxidation state. B Bromide ions are oxidised; iodine atoms are reduced. C Bromide ions are reduced; iodine atoms are oxidised. D No reaction occurs.

Question

Which statement is correct? A Nitrogen is unreactive due to the absence of lone pairs in the molecule. B Aqueous ammonia contains both NH3(aq) and NH4+(aq). The NH4+(aq) ion is a Brønsted–Lowry acid. C High temperatures are needed to supply the energy to break the strong double bonds in nitrogen molecules when they react. D Atmospheric SO2 reacts with unburnt hydrocarbons to form a component of photochemical smog.

Question

When dry ammonia and hydrogen chloride gases are mixed, a solid white ionic compound is formed. Two statements are listed. 1 The formation of the ionic compound is a redox reaction. 2 During the formation of the ionic compound, the H–N–H bond angle increases. Which statements are correct? A both 1 and 2 B 1 only C 2 only D neither 1 nor 2

Question

The diagrams show skeletal formulas of some isomers of C6H12O. O O 1 2 O O 3 4 Which statement is correct? A 1 and 3 are chain isomers of each other and positional isomers of each other. B 2 and 3 are functional group isomers of each other and both have a chiral centre. C 1 and 4 are functional group isomers of each other and both have a chiral centre. D 2 and 4 are positional isomers of each other and functional group isomers of each other.

Question

The skeletal formulas of two compounds are shown. progesterone testosterone O OH O O Which statements about progesterone and testosterone are correct? A They both contain a ketone group, and they both have geometrical isomers due to the C=C bond. B They have the same molecular formula, and they both have geometrical isomers. C They have the same number of chiral carbons, and they have the same molecular formula. D They have the same number of chiral carbons, and they both contain a ketone group.

Question

Which intermediate ion forms in the greatest amount during the addition of HBr to propene? A CH3CH+CH3 B CH3CH2CH2+ C CH3CH–CH2Br D CH3CHBrCH2–

Question

Two hydrocarbons, R–CH3 and R'–CH3, react separately with bromine in the presence of ultraviolet light. One of these hydrocarbons is unsaturated. In each case, free radical substitution reactions occur. R is CH3CHC(CH3). R' is CH3CH(CH3)CH2. Which row is correct? a propagation stage for a termination stage for the saturated hydrocarbon the unsaturated hydrocarbon A R–CH2• + Br• → R–CH2Br R'–CH2• + Br• → R'–CH2Br B R–CH2• + Br2 → R–CH2Br + Br• R'–CH2• + Br2 → R'–CH2Br + Br• C R'–CH3 + Br• → R'–CH2• + HBr 2R–CH2• → R–CH2CH2–R D 2R'–CH2• → R'–CH2CH2–R' R–CH3 + Br• → R–CH2• + HBr

Question

The fumes from the exhausts of petrol-burning cars contain the following pollutants. 1 unburnt hydrocarbons 2 nitrogen dioxide 3 carbon monoxide Which pollutants are removed by oxidation in a catalytic converter? A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only

Question

Compound X, C7H11ICl 2, is dissolved in ethanol and the solution mixed with warm aqueous silver nitrate. A precipitate is seen immediately. compound X CH2Cl Cl I What is the colour of this precipitate and what is the structural formula of the first organic product? colour of structural formula of the precipitate the first organic product CH2Cl HO A cream OH CH2OH HO B cream OH CH2OH HO C white I CH2Cl Cl D yellow OH 31 1,4-dibromobutane reacts with an excess of ethanolic sodium hydroxide until no further reaction takes place. What is the relative formula mass of the major organic product? A 54 B 56 C 74 D 90

Question

In the question paper above.

Question

A small section of a polymer produced from two monomers is shown. –CH2–C(CH3)2–CH(CH3)–CH2– What are the two monomers? A but-1-ene and propene B but-2-ene and propene C ethene and pent-2-ene D methylpropene and propene

Question

The balanced equation for the reaction of X with an excess of acidified K2Cr2O7 is shown. X + 3[O] → Y + H2O Compound Y is the only organic product of the reaction. Which compound is X? A B H H O H H OH O C C C H HO C C C H CH H H 2C H HO CH3 OH C D H H OH H H O HO C C C H O C C C H H OH H C O H

Question

Three mixtures are heated under reflux. Which mixtures will produce sodium propanoate as one product? 1 CH3CH2CHO + NaBH4(aq) 2 CH3CH2CH2OH + Na(s) 3 CH3CH2CN + NaOH(aq) A 1, 2 and 3 B 1 and 2 only C 2 and 3 only D 3 only

Question

Which compound is a product of the hydrolysis of CH3CO2CH2C2H5 using aqueous sodium hydroxide? A CH3CO2–Na+ B CH3CO2H C C2H5CH2O–Na+ D C2H5CH2CO2–Na+

Question

Compound Q reacts when heated with HCN in the presence of a catalyst to produce compound R. Molecules of compound R each contain four carbon atoms. What is compound Q? A B C D O H OH O Cl O

Question

The table shows the reagents and products of three reactions. reagents products 1 ethanoic acid + Na2CO3 CH3CO2Na + H2O + CO2 2 ethanoic acid + Mg (CH3CO2)2Mg + H2O 3 ethanoic acid + CH3OH CH3CO2CH3 + H2O Which rows are correct? A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only

Question

Seven aldehydes and ketones ● contain only one oxygen atom per molecule ● have four or fewer carbon atoms in their structures. Alkaline I2(aq) is added to each of these carbonyl compounds separately. How many of these carbonyl compounds produce a yellow precipitate with alkaline I2(aq)? A 1 B 2 C 3 D 4

Question

Some properties of compound X are listed. ● 1.0 mol X reacts with exactly 8.5 mol oxygen when completely combusted. ● X does not react when heated with acidified KMnO4. What are the possible identities of X? OH HO O OH 1 2 3 4 A 1 and 3 B 2 and 4 C 3 only D 4 only

Question

A sample of magnesium contains the isotopes 24Mg, 25Mg and 26Mg only. The percentage abundance of 25Mg and 26Mg is the same. The relative atomic mass of magnesium in the sample is 24.3. What is the percentage abundance of 24Mg? A 10% B 20% C 60% D 80% 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 = 6.02 × 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) 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 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 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 138.9 140.1 140.9 144.2 – 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 – – – – – – – – – – –