A Level Chemistry 9701 Paper 42, May/June 2026

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9701/42 · May/June 2026

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a(i)

Transition elements have variable oxidation states and form complex ions. State two other typical chemical properties of a transition element. 1 ........................................................................................................................................ 2 ........................................................................................................................................

[1]

a(ii)

Explain why transition elements have variable oxidation states.

[1]

b(i)

An aqueous solution of chromium(III) ions, ${Cr}^{3 +}$ , contains the $[Cr (H_{2} O)_{6}]^{3 +}$ complex ion. Complete Figure 1.1 to show the electronic configuration for ${Cr}^{3 +}$ .

[1]

b(ii)

State the type of bonding that exists between $H_{2} O$ and ${Cr}^{3 +}$ in $[Cr (H_{2} O)_{6}]^{3 +}$ .

[1]

Explain why transition elements form complex ions.

[1]

d(i)

$[Cr (H_{2} O)_{6}]^{3 +}$ can be converted into the $[Cr (H_{2} O)_{3} (OH)_{3}]$ complex. Suggest a suitable reagent for this conversion. State the type of reaction. reagent .............................................................................................................................. type of reaction ..................................................................................................................

[1]

d(ii)

$[Cr (H_{2} O)_{3} (OH)_{3}]$ reacts with an excess of ${NH}_{3} (aq)$ to form $[Cr ({NH}_{3})_{6}]^{3 +}$ . Complete the equation for this reaction. State the type of reaction. $[Cr (H_{2} O)_{3} (OH)_{3}] +$ ........................................................................................................... type of reaction ..................................................................................................................

[2]

$[Cr (H_{2} O)_{3} (OH)_{3}]$ shows stereoisomerism. Draw three-dimensional diagrams in Figure 1.2 to suggest the two stereoisomers of $[Cr (H_{2} O)_{3} (OH)_{3}]$ .

[2]

f(i)

An aqueous solution of iron(III) ions, ${Fe}^{3 +}$ , contains the $[Fe (H_{2} O)_{6}]^{3 +}$ complex ion. This solution is acidic in a similar way to an aqueous solution of ${Al}^{3 +}$ . Suggest why a solution of ${Fe}^{3 +}$ is acidic. Include an equation in your answer.

[2]

f(ii)

An aqueous solution of iron(II) ions, ${Fe}^{2 +}$ , contains the $[Fe (H_{2} O)_{6}]^{2 +}$ complex ion. This solution is also acidic. Predict how the pH of $1.00 mol {dm}^{- 3} {Fe}^{2 +} (aq)$ differs from the pH of $1.00 mol {dm}^{- 3} {Fe}^{3 +} (aq)$ . Explain your answer.

[1]

Suggest why solutions of silver(I) salts are colourless.

[2]

A mixture contains sodium ethanedioate, ${Na}_{2} C_{2} O_{4}$ , ethanedioic acid dihydrate, $H_{2} C_{2} O_{4} \cdot 2 H_{2} O$ , and an unreactive solid. $5.00 g$ of this mixture is dissolved in distilled water and made up to $500 {cm}^{3}$ in a volumetric flask to form solution A. Two different titration experiments are carried out using A. In the first experiment, $25.0 {cm}^{3}$ of A requires $21.80 {cm}^{3}$ of acidified $0.0250 mol {dm}^{- 3} {MnO}_{4}^{-} (aq)$ to reach the end-point. $2 {MnO}_{4}^{-} + 5 C_{2} O_{4}^{2 -} + 16 H^{+} \to 2 {Mn}^{2 +} + 10 {CO}_{2} + 8 H_{2} O$ In the second experiment, $25.0 {cm}^{3}$ of A requires $13.60 {cm}^{3}$ of $0.150 mol {dm}^{- 3} {OH}^{-} (aq)$ to reach the end-point. $H_{2} C_{2} O_{4} + 2 {OH}^{-} \to C_{2} O_{4}^{2 -} + 2 H_{2} O$ Calculate the percentage by mass of ${Na}_{2} C_{2} O_{4}$ in the mixture. [ $M_{r}$ : ${Na}_{2} C_{2} O_{4}$ , 134.0] percentage by mass of ${Na}_{2} C_{2} O_{4} =$ ......................................................%

[5]

Group 2 carbonates decompose on heating to form the corresponding metal oxide and carbon dioxide.

The mechanism for this decomposition involves the carbonate ion breaking down to form carbon dioxide and oxide ions. Add two curly arrows to the carbonate ion in Figure 2.1 to suggest a mechanism for this decomposition.

[1]

The radii of some cations are shown in Table 2.1. Table 2.1

cation	${Ca}^{2 +}$	${Cu}^{2 +}$	${Pb}^{2 +}$
radius/nm	0.099	0.073	0.120

Use the data in Table 2.1 to predict the trend in thermal stability of the metal carbonates containing these cations. Explain your answer. .............................. > .............................. > .............................. most stable least stable explanation ............................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ...................................................................................................................................................

[2]

Suggest why the solubility of the Group 2 sulfates decreases down the group.

[3]

d(i)

Magnesium hydroxide, $Mg (OH)_{2}$ , is sparingly soluble in water at $298 K$ . Write the expression for the solubility product, $K_{sp}$ , of $Mg (OH)_{2}$ . State the units for $K_{sp}$ . $K_{sp} =$ units ...............................................................

[2]

d(ii)

A saturated solution of $Mg (OH)_{2}$ has a pH of 10.35 at $298 K$ . Calculate the concentration of hydroxide ions, ${OH}^{-}$ , in $mol {dm}^{- 3}$ , in this solution. concentration of ${OH}^{-} =$ .......................................... $mol {dm}^{- 3}$

[1]

d(iii)

Use your answers to 2(d)(i) and 2(d)(ii) to calculate the value of $K_{sp}$ for $Mg (OH)_{2}$ . $K_{sp}$ for $Mg (OH)_{2} =$ .........................................................

[1]

a(i)

Ethanal, ${CH}_{3} CHO$ , reacts with methanol, ${CH}_{3} OH$ , under acidic conditions to form compound B, as shown in reaction 1. reaction 1 ${CH}_{3} CHO + 2 {CH}_{3} OH \overset{H^{+}}{\to} {CH}_{3} CH ({OCH}_{3})_{2} + H_{2} O$ The initial rate of reaction is investigated using different starting concentrations of ${CH}_{3} CHO$ , ${CH}_{3} OH$ and $H^{+}$ . The results obtained are shown in Table 3.1. Table 3.1

experiment	$[{CH}_{3} CHO] / mol {dm}^{- 3}$	$[{CH}_{3} OH] / mol {dm}^{- 3}$	$[H^{+}] / mol {dm}^{- 3}$	initial rate $/ mol {dm}^{- 3} s^{- 1}$
1	0.500	0.040	0.100	$2.500 \times 10^{- 3}$
2	0.500	0.060	0.100	$3.750 \times 10^{- 3}$
3	0.250	0.120	0.300	$1.125 \times 10^{- 2}$
4	0.250	0.120	0.400	$1.500 \times 10^{- 2}$

Use the information in Table 3.1 to deduce the rate equation for this reaction. Explain your reasoning. State clearly which experiments you use in your explanation. rate =

[4]

a(ii)

State the units of the rate constant, $k$ , for this reaction.

[1]

a(iii)

Another experiment to investigate reaction 1 is carried out as shown in Table 3.2. Table 3.2

experiment	$[{CH}_{3} CHO] / mol {dm}^{- 3}$	$[{CH}_{3} OH] / mol {dm}^{- 3}$	$[H^{+}] / mol {dm}^{- 3}$
5	0.250	0.250	0.250

Calculate the initial rate of experiment 5. initial rate = ..................................... $mol {dm}^{- 3} s^{- 1}$

[1]

The reaction of propanone, ${CH}_{3} {COCH}_{3}$ , with bromine, ${Br}_{2}$ , in the presence of an acid catalyst is shown in reaction 2. reaction 2 ${CH}_{3} {COCH}_{3} + {Br}_{2} \overset{H^{+}}{\to} {CH}_{3} {COCH}_{2} Br + HBr$ The rate of reaction is first order with respect to $[{CH}_{3} {COCH}_{3}]$ and first order with respect to $[H^{+}]$ under certain conditions. A three-step mechanism for reaction 2 is suggested. Complete Table 3.3 to suggest steps 1 and 3 of the mechanism.

[2]

Catalysts can be described as homogeneous or heterogeneous. Describe the mode of action of a heterogeneous catalyst.

[2]

State what is meant by partition coefficient, $K_{pc}$ .

[1]

Ethanedioic acid, $H_{2} C_{2} O_{4}$ , is more soluble in water than in the organic solvent ethoxyethane. $2.70 g$ of ethanedioic acid is shaken with a mixture of $50 {cm}^{3}$ of ethoxyethane and $50 {cm}^{3}$ of water at $298 K$ and left until there is no further change in concentrations. The ethoxyethane layer requires $16.5 {cm}^{3}$ of $0.200 mol {dm}^{- 3} NaOH (aq)$ for complete neutralisation. $H_{2} C_{2} O_{4} + 2 NaOH \to {Na}_{2} C_{2} O_{4} + 2 H_{2} O$ Calculate the partition coefficient, $K_{pc}$ , for ethanedioic acid between ethoxyethane and water. $K_{pc} =$ .........................................................

[3]

The formula of ethanedioic acid is $HOOCCOOH$ . The formula of butanedioic acid is ${HOOCCH}_{2} {CH}_{2} COOH$ . Both acids are soluble in ethoxyethane and in water. Suggest how the value of $K_{pc}$ of butanedioic acid between ethoxyethane and water compares to the value of $K_{pc}$ for ethanedioic acid between ethoxyethane and water. Explain your answer.

[2]

Define standard electrode potential, $E^{⊖}$ , including a description of standard conditions.

[2]

b(i)

Table 5.1 shows the standard electrode potentials for three redox systems. Table 5.1

redox system	electrode reaction	$E^{⊖} / V$
1	${Fe}^{3 +} + e^{-} ⇌ {Fe}^{2 +}$	+0.77
2	${NO}_{3}^{-} + 10 H^{+} + 8 e^{-} ⇌ {NH}_{4}^{+} + 3 H_{2} O$	+0.87
3	${Zn}^{2 +} + 2 e^{-} ⇌ Zn$	-0.76

Use the information in Table 5.1 to write equations for two reactions that are feasible. Explain why these reactions are feasible. equation 1 ......................................................................................................................... equation 2 ......................................................................................................................... explanation ........................................................................................................................ ........................................................................................................................................... ...........................................................................................................................................

[3]

b(ii)

Suggest why the feasible reactions in 5(b)(i) may not take place under standard conditions.

[1]

b(iii)

An electrochemical cell is set up to measure $E^{⊖}$ for redox system 2 in Table 5.1. Complete Figure 5.1 to show a labelled diagram of this electrochemical cell. Include all necessary substances and relevant pieces of apparatus needed to measure $E^{⊖}$ . It is not necessary to state the conditions used.

[3]

A different electrochemical cell is set up. The cell reaction for this electrochemical cell is shown. $Cr + 3 {Mn}^{3 +} \to 3 {Mn}^{2 +} + {Cr}^{3 +} Δ G^{⊖} = - 645.6 kJ {mol}^{- 1}$ Calculate the standard cell potential, $E_{cell}^{⊖}$ , for this cell reaction. $E_{cell}^{⊖} =$ ...................................................... V

[2]

a(i)

Phenol reacts with ${Br}_{2} (aq)$ . State all the expected observations when ${Br}_{2} (aq)$ is added dropwise to a solution of phenol.

[1]

a(ii)

Draw the structure of the organic product formed when phenol reacts with an excess of ${Br}_{2} (aq)$ .

[1]

Explain the relative acidities of phenol and water.

[2]

c(i)

Compound C can undergo both addition and condensation polymerisation. Draw one repeat unit of the addition polymer formed from C.

[1]

c(ii)

Draw two repeat units of the condensation polymer formed from C. The new functional group formed should be displayed.

[2]

C can react with ${LiAlH}_{4}$ . C can also react with an excess of $H_{2} (g)$ with a nickel catalyst. Draw the structure of the organic product formed in each reaction in Figure 6.2.

[2]

e(i)

Compound F can be synthesised from phenol in three steps, as shown in Figure 6.3. Draw the structures of compounds D and E in the boxes in Figure 6.3.

[2]

e(ii)

Suggest reagents and conditions for steps 1 to 3 in Figure 6.3. step 1 ................................................................................................................................ step 2 ................................................................................................................................ step 3 ................................................................................................................................

[3]

a(i)

Alanine, ${CH}_{3} CH ({NH}_{2}) COOH$ , is an amino acid that contains a chiral centre. Different synthetic routes to produce alanine can lead to the formation of an optically active sample or a racemic mixture. Describe what is meant by optically active.

[1]

a(ii)

Describe what is meant by racemic mixture.

[1]

b(i)

Alanine has an isoelectric point of 6.11. Explain what is meant by isoelectric point.

[1]

b(ii)

Draw the structure of alanine at pH 10.

[1]

Alanine molecules can react together to form the tripeptide Ala–Ala–Ala. Draw the structure for this tripeptide. The functional groups formed should be displayed.

[2]

d(i)

Compound J can be synthesised from alanine in three steps, as shown in Figure 7.1. Draw the structures of compounds G and H in the boxes in Figure 7.1.

[2]

d(ii)

Suggest reagents and conditions for steps 1 to 3 in Figure 7.1. step 1 ................................................................................................................................ step 2 ................................................................................................................................ step 3 ................................................................................................................................

[3]

Give the full name of the substance used in NMR spectroscopy as the standard for chemical shift measurements.

[1]

b(i)

Compound K is analysed by carbon-13 NMR and proton ( $^{1} H$ ) NMR spectroscopy in $D_{2} O$ . Predict the number of peaks in the carbon-13 NMR spectrum of K.

[1]

b(ii)

The proton ( $^{1} H$ ) NMR spectrum of K in $D_{2} O$ shows four peaks, for the proton environments labelled w, x, y and z on the structure of K in Figure 8.2. Complete Table 8.1 to identify the splitting patterns for proton environments w, x, y and z.

[2]

b(iii)

A separate sample of K is dissolved in ${CDCl}_{3}$ and analysed using proton ( $^{1} H$ ) NMR spectroscopy. The proton ( $^{1} H$ ) NMR spectrum of K dissolved in ${CDCl}_{3}$ contains one more peak than the spectrum of K dissolved in $D_{2} O$ . Explain why there is one more peak, and suggest the chemical shift range in which it occurs. chemical shift range $δ =$ ........................................................ ppm

[2]

Compound K reacts with an excess of hot $NaOH (aq)$ . The products are isolated from the reaction mixture at pH 10. Draw the structures of the two organic products of the complete alkaline hydrolysis of K.

[2]

Compound P and compound Q are isomers. State the relative basicities of P, Q and ammonia. Explain your answer. .............................. > .............................. > .............................. most basic least basic explanation ............................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ...................................................................................................................................................

[4]

b(i)

P can be prepared from methylbenzene in two steps, as shown in Figure 9.2. Suggest reagents and conditions for steps 1 and 2 in Figure 9.2. step 1 ................................................................................................................................ step 2 ................................................................................................................................

[2]

b(ii)

Complete the equation in Figure 9.3 for step 2. Use [H] to represent an atom of hydrogen from the reducing agent.

[1]

c(i)

Figure 9.4 shows a two-step synthesis of azo dye N. Draw the structure of compound M in the box in Figure 9.4.

[1]

c(ii)

Give the reagents and conditions for steps 1 and 2 in Figure 9.4. step 1 ................................................................................................................................ step 2 ................................................................................................................................

[2]

Mark scheme

9701/42 · May/June 2026

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1a(i) · 1 mark

1 mark
they behave as catalysts AND (they form) coloured compounds / complexes / ions BOTH

1a(ii) · 1 mark

1 mark
the d and s sub-shells / orbitals are close / similar in energy / electrons in d and s sub-shells / orbitals available for bonding

1b(i) · 1 mark

1 mark
3d: [↑][↑][↑][ ][ ] 4s: [ ]

1b(ii) · 1 mark

1 mark
dative (covalent) / coordinate

1c · 1 mark

1 mark
vacant (d) orbital(s) are energetically accessible or vacant (d) orbital(s) can form dative bonds with ligands or vacant (d) orbital(s) can accept a (lone) pair of electrons to form a dative bond

1d(i) · 1 mark

1 mark
NaOH / OH– and precipitation / ligand exchange / neutralisation / deprotonation / acid-base BOTH

1d(ii) · 2 marks

M1
[Cr(H2O)3(OH)3] + 6NH3 → [Cr(NH3)6]3+ + 3H2O + 3OH–
M2
ligand exchange / replacement / substitution / displacement

1e · 2 marks

M1
one correct 3D structure of [Cr(H2O)3(OH)3]
M2
correct 3D structure of the other isomer

1f(i) · 2 marks

M1
[Fe(H2O)6]3+ / Fe3+ weakens O–H bonds / polarises O–H bonds
M2
[Fe(H2O)6]3+ → [Fe(H2O)5OH]2+ + H+

1f(ii) · 1 mark

1 mark
Fe3+ has lower pH / Fe2+ has a higher pH and Fe3+ has a higher charge / smaller radii / higher charge density (so easier to hydrolyse) BOTH ora

1g · 2 marks

M1
(Ag+) d-subshell is full / complete or d10 or d-orbitals are full
M2
no d-d(*) transition or no d electrons promoted / excited or cannot absorb light in the visible spectrum

1h · 5 marks

M1
any two of: • moles MnO4– = 0.025 × 0.02180 = 5.45 × 10–4 • moles C2O42– = 2.5 × 5.45 × 10–4 = 1.3625 × 10–3 ecf (moles MnO4– × 2.5) • moles OH– = 0.150 × 0.0136 = 2.04 × 10–3 • moles H2C2O4 = ½ × 2.04 × 10–3 = 1.02 × 10–3 ecf (moles OH– x ½)
M2
all four of the above mole calculations correct
M3
moles Na2C2O4 = 1.3625 × 10–3 – 1.02 × 10–3 = 3.425 × 10–4 ecf (in 25 cm3 A)
M4
moles Na2C2O4 = 3.425 × 10–4 × 20 = 6.85 × 10–3 ecf (in 500 cm3 A) AND mass Na2C2O4 = 6.85 × 10–3 × 134 = 0.9179 g
M5
% = 0.9179 / 5.00 × 100 = 18.4 / 18.358 min 2sf ecf

2a · 1 mark

1 mark
BOTH arrows (ARROW 1 from O– to C–O bond; ARROW 2 from C–O bond to the other O–)

2b · 2 marks

1 mark
PbCO3(most) CaCO3 CuCO3 (least)
1 mark
(stability increases) as (ionic) radii increases / size of M2+ increases / or Pb2+ largest radii ora AND less polarisation / distortion of carbonate ion / anion / CO3(2)– or less weakening of CO bond / C-O / C=O

2c · 3 marks

M1
ΔHlatt and ΔHhyd (both) become less exothermic / less negative
M2
ΔHhyd changes more / changes faster / dominant factor / becomes less exothermic by a larger extent ora
M3
ΔHsol becomes less exothermic / less negative or ΔHsol becomes more endothermic / more positive

2d(i) · 2 marks

M1
(Ksp for Mg(OH)2) = [Mg2+][OH–]2
M2
units mol3 dm–9 ecf from M1

2d(ii) · 1 mark

1 mark
[H+] = 10–10.35 = 4.47 × 10–11 AND [OH–] = 1 × 10–14 ÷ 4.47 × 10–11 = 2.24 × 10–4 min 2sf

2d(iii) · 1 mark

1 mark
Ksp = (0.5 × 2.24 × 10–4) × (2.24 × 10–4)2 = 5.61(2) / 5.62 × 10–12 u / c min 2sf ecf for 2(d)(i) and 2(d)(ii)

3a(i) · 4 marks

M1
Exp 1 & 2 [CH3OH] × 1.5 rate × 1.5 or [CH3OH] × 2 / 3 rate × 2 / 3 and so first order to [CH3OH] u / c
M2
Exp 3 & 4 [H+] × 1.33 rate × 1.33 or [H+] × 3 / 4 rate × 3 / 4 and so first order to [H+] u / c
M3
Exp 2 & 3 [CH3CHO] × 0.5, [CH3OH] × 2 and [H+] × 3 rate × 3 and so first order to [CH3CHO] ecf
M4
Rate = k[CH3OH][H+][CH3CHO] u / c ecf or rate = 1.25 [CH3OH][H+][CH3CHO]

3a(ii) · 1 mark

1 mark
mol–2dm6s–1 u / c ecf from 3(a)(i)

3a(iii) · 1 mark

1 mark
initial rate = 0.0195 u / c ecf from 3(a)(i) min 2sf

3b · 2 marks

1 mark
step 1: protonated propanone H3C—C(=+OH)—CH3
1 mark
step 3: bromo-propanone H3C—C(=O)—CH2Br + HBr

3c · 2 marks

1 mark
(reactants) adsorb (to surface of catalyst)
1 mark
bonds (in reactant) weaken AND (reaction occurs and the) product(s) are desorbed / reaction occurs and substances are desorbed

4a · 1 mark

1 mark
(the) ratio of the concentrations of a solute / substance / compound between two (immiscible) solvents / two liquids (at) equilibrium

4b · 3 marks

M1
Solution 1: moles of (COOH)2 in ether = 0.00165 (subsumes moles of NaOH = 0.0033) OR Solution 2: mass of (COOH)2 in ether = 0.1485 g
M2
Solution 1: moles of (COOH)2 in water = 0.0300 – 0.00165 = 0.02835 ecf OR Solution 2: mass of (COOH)2 in water = 2.70 – 0.1485 = 2.5515 g ecf
M3
Kpc = 0.00165 / 0.02835 = 0.058(2) min 2sf ecf from bullets 3 & 4 only

4c · 2 marks

1 mark
Kpc would be higher / larger (if Kpc < 1 in 4(b)) (for butanedioic acid) (ecf from 4(b)) ora
1 mark
butanedioic acid is less polar / more non-polar ora AND so less soluble in water / more soluble in ethoxyethane ora (or dissolves less in water / dissolves more in ethoxyethane)

5a · 2 marks

M1
emf / potential difference / voltage and between / compared to and a standard hydrogen electrode and another electrode
M2
under standard conditions of 1 atm / 101 kPa / 100 kPa, 298 K / 25 °C, (all solutions being) 1M / 1 mol dm–3 u / c

5b(i) · 3 marks

M1
any one or two of the three equations correct
M2
all three equations correct: • Zn + 2Fe3+ → Zn2+ + 2Fe2+ • NO3– + 10H+ + 8Fe2+ → NH4+ + 3H2O + 8Fe3+ • NO3– + 10H+ + 4Zn → NH4+ + 3H2O + 4Zn2+
M3
Ecell is positive (to be feasible) or Eo of Fe3+ / Fe2+ and NO3– / NH4+ is more positive or Eo of redox system 1 and 2 are more positive ora u / c

5b(ii) · 1 mark

1 mark
high Ea for the reaction OWTTE

5b(iii) · 3 marks

1 mark
any 3 of the 9 marking features correct
1 mark
any 6 of the 9 marking features correct
1 mark
all 9 marking features correct

5c · 2 marks

M1
ΔGo = -nEcellF AND –645.6 × 1000 = –3 × E × 96 500
M2
Ecell = (+)2.23 (V) min 2sf

6a(i) · 1 mark

1 mark
white ppt. and (solution) decolourises / turns colourless / orange colour disappears

6a(ii) · 1 mark

1 mark
structure of 2,4,6-tribromophenol

6b · 2 marks

M1
lone pair on oxygen / O delocalised / overlaps and into the ring / π system / delocalised system or p-orbital on oxygen / O delocalised / overlaps and with ring / π system / delocalised system
M2
weakens O—H and phenol is more acidic or (phenol forms) anion / conjugate base / phenoxide ion is more stable and phenol is more acidic

6c(i) · 1 mark

1 mark
repeat unit with 1,2-substituted phenol and —COOH group

6c(ii) · 2 marks

M1
ester linkage shown between phenol & COOH
M2
rest of the structure correct

6d · 2 marks

M1
structure of 2-(3-hydroxyprop-1-en-1-yl)phenol
M2
structure of 2-(3-hydroxypropyl)phenol / 3-(2-hydroxyphenyl)propanoic acid

6e(i) · 2 marks

M1
correct structure of D
M2
correct structure of E

6e(ii) · 3 marks

1 mark
step 1: CH3Cl (and AlCl3) CON (aq), CON other reagents
1 mark
step 2: hot / reflux / heat / boil / T ⩾ 60 °C and (alkaline / acidified / neutral) MnO4– / KMnO4
1 mark
step 3: CH3COCl CON (aq) CON any other reagent e.g. cH2SO4

7a(i) · 1 mark

1 mark
(a substance able to) rotate plane polarised light

7a(ii) · 1 mark

1 mark
(a mixture containing) equal amounts / proportions / concentrations and of optical isomers / enantiomers / stereoisomers

7b(i) · 1 mark

1 mark
pH at (which a molecule / amino acid) has no overall charge / is neutral / is a zwitterion

7b(ii) · 1 mark

1 mark
CH3CH(NH2)COO–

7c · 2 marks

M1
two peptide linkage shown (C=O needs to be displayed but allow NH not displayed)
M2
rest of the structure correct DEP on M1 (except for specific ecfs in guidance)

7d(i) · 2 marks

M1
structure of G (CH3CONHCH(CH3)COOH)
M2
structure of H (CH3CONHCH(CH3)COCl)

7d(ii) · 3 marks

M1
step 1: CH3COCl CON (aq), CON additional reagent e.g. AlCl3, cH2SO4
M2
step 2: PCl3 + heat or SOCl2 or PCl5 CON (aq)
M3
step 3: C6H6 and AlCl3 CON (aq)

8a · 1 mark

1 mark
tetramethylsilane

8b(i) · 1 mark

1 mark
5 / five

8b(ii) · 2 marks

1 mark
any two of w = doublet, x = multiplet, y = triplet, z = triplet
1 mark
all four correct: w = doublet, x = multiplet, y = triplet, z = triplet

8b(iii) · 2 marks

M1
δ 5 –12
M2
(N-H peak appears and) no proton / hydrogen exchanges / replaces / substitutes with deuterium / D / D+ ora

8c · 2 marks

M1
structure of sodium 3-methyl-2-oxobutanoate / 3-methyl-2-oxobutanoate ion
M2
structure of 3-aminopropan-1-ol H2NCH2CH2CH2OH

9a · 4 marks

M1
order of basicity: Q > ammonia > P
M2
(basicity linked to) ability of lone pair / p-orbital to accept / donate to / coordinate with a proton / H+
M3
any one of: • lone pair / p-orbital from N (in P) and delocalised / overlaps with (π-)ring / benzene • electron donating / +I and R / alkyl / CH2 grp (in Q) • increases electron density on N or N is more electron rich or N LP is more available (in Q) ora
M4
all three explanation points correct

9b(i) · 2 marks

M1
step 1: HNO3 and H2SO4 and conc. / concentrated
M2
step 2: Sn and conc. HCl

9b(ii) · 1 mark

1 mark
6 [H] and 2 H2O

9c(i) · 1 mark

1 mark
structure of diazonium salt (4-methylbenzenediazonium ion)

9c(ii) · 2 marks

M1
step 1: NaNO2 with HCl or HNO2 and ⩽10 °C
M2
step 2: alkaline / NaOH and sodium 4-hydroxybenzenesulfonate / 4-hydroxybenzenesulfonic acid

Questions

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2
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3
Question 310 marks
Mark scheme ›
4
Question 46 marks
Mark scheme ›
5
Question 511 marks
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6
Question 614 marks
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7
Question 711 marks
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8
Question 88 marks
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9
Question 910 marks
Mark scheme ›

A Level Chemistry 9701 Paper 42, May/June 2026

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Question paper

Mark scheme

1a(i) · 1 mark

1a(ii) · 1 mark

1b(i) · 1 mark

1b(ii) · 1 mark

1c · 1 mark

1d(i) · 1 mark

1d(ii) · 2 marks

1e · 2 marks

1f(i) · 2 marks

1f(ii) · 1 mark

1g · 2 marks

1h · 5 marks

2a · 1 mark

2b · 2 marks

2c · 3 marks

2d(i) · 2 marks

2d(ii) · 1 mark

2d(iii) · 1 mark

3a(i) · 4 marks

3a(ii) · 1 mark

3a(iii) · 1 mark

3b · 2 marks

3c · 2 marks

4a · 1 mark

4b · 3 marks

4c · 2 marks

5a · 2 marks

5b(i) · 3 marks

5b(ii) · 1 mark

5b(iii) · 3 marks

5c · 2 marks

6a(i) · 1 mark

6a(ii) · 1 mark

6b · 2 marks

6c(i) · 1 mark

6c(ii) · 2 marks

6d · 2 marks

6e(i) · 2 marks

6e(ii) · 3 marks

7a(i) · 1 mark

7a(ii) · 1 mark

7b(i) · 1 mark

7b(ii) · 1 mark

7c · 2 marks

7d(i) · 2 marks

7d(ii) · 3 marks

8a · 1 mark

8b(i) · 1 mark

8b(ii) · 2 marks

8b(iii) · 2 marks

8c · 2 marks

9a · 4 marks

9b(i) · 2 marks

9b(ii) · 1 mark

9c(i) · 1 mark

9c(ii) · 2 marks

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