A Level Chemistry 9701 Paper 42, Oct/Nov 2025

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9701/42 · Oct/Nov 2025

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Magnesium nitrate, $M g (N O_{3})_{2}$ , and strontium nitrate, $S r (N O_{3})_{2}$ , both decompose when heated to form the metal oxide and a mixture of gases.

Write an equation for the thermal decomposition of $M g (N O_{3})_{2}$ .

[1]

State which of $M g (N O_{3})_{2}$ or $S r (N O_{3})_{2}$ decomposes at a lower temperature. Explain your answer. compound that decomposes at a lower temperature ............................................................... explanation ...............................................................................................................................

[2]

c(i)

Magnesium oxide, $M g O$ , and strontium oxide, $S r O$ , both react with dilute sulfuric acid. $M g O$ forms a soluble salt, A. $S r O$ forms an insoluble salt, B. Identify the products formed when $M g O$ reacts with dilute sulfuric acid.

[1]

c(ii)

Explain why A is more soluble than B.

[3]

Ethanal, $C H_{3} C H O$ , reacts with nitrogen dioxide, $N O_{2}$ . The products of the first step of this reaction are a $C H_{3} \dot{C} = O$ radical and a molecule of nitrous acid, $H N O_{2}$ . $C H_{3} C H O + N O_{2} \to C H_{3} \dot{C} = O + H N O_{2}$

a(i)

Use two words to complete the sentence. This reaction involves ........................................ ........................................ of the single covalent bond between a hydrogen atom and a carbon atom in $C H_{3} C H O$ .

[1]

a(ii)

The hydrogen atom mentioned in (a)(i) forms a covalent bond with one of the oxygen atoms of an $N O_{2}$ molecule. An $N O_{2}$ molecule has a single, unpaired electron on the nitrogen atom. All electrons are paired in an $H N O_{2}$ molecule. Draw dot-and-cross diagrams of $N O_{2}$ and $H N O_{2}$ in the boxes. Show outer shell electrons only.

[1]

a(iii)

Use VSEPR theory to predict the bond angle at the nitrogen atom in an $H N O_{2}$ molecule. bond angle = ..............................

[1]

The rate equation for the reaction between $C H_{3} C H O$ and $N O_{2}$ is shown. $r a t e = k [C H_{3} C H O] [N O_{2}]$ Under certain conditions, when the concentrations of both $C H_{3} C H O$ and $N O_{2}$ are $0.200 m o l d m^{- 3}$ , the rate of the reaction is $1.53 \times 10^{- 4} m o l d m^{- 3} s^{- 1}$ . Calculate the value of the rate constant, $k$ , under these conditions. Give the units of $k$ . $k =$ .............................. units ..............................

[2]

The reaction mixture described in (b) is monitored over a period of time. Predict whether the graph of $[N O_{2}]$ against time shows a constant half-life. Explain your answer. prediction .................................................................................................................. explanation ...............................................................................................................

[1]

$N O_{2}$ also reacts with ozone, $O_{3}$ . The rate equation is shown. $r a t e = k_{1} [N O_{2}]$ Under certain conditions, the value of $k_{1}$ is $0.0848 s^{- 1}$ . The reaction has a constant half-life under these conditions. Calculate the half-life in seconds. half-life = .............................. s

[1]

$N O_{2}$ is present in the exhaust gases of cars. It can react with carbon monoxide, $C O$ , on the surface of a heterogeneous catalyst in the car’s catalytic converter. Describe the mode of action of this heterogeneous catalyst.

[2]

a(i)

Define conjugate acid–base pair.

[1]

a(ii)

Give the formulas of the conjugate acid and the conjugate base of the hydrogen phosphate ion, $H P O_{4}^{2 -}$ . conjugate acid of $H P O_{4}^{2 -}$ .............................. conjugate base of $H P O_{4}^{2 -}$ ..............................

[1]

b(i)

The $K_{a}$ of propanoic acid, $C H_{3} C H_{2} C O O H$ , is $1.35 \times 10^{- 5} m o l d m^{- 3}$ at $298 K$ . Solution C is a solution of $C H_{3} C H_{2} C O O H$ with a pH of $3.60$ at $298 K$ . Calculate the concentration of $C H_{3} C H_{2} C O O H$ in solution C. $[C H_{3} C H_{2} C O O H] =$ .............................. $m o l d m^{- 3}$

[2]

b(ii)

Calculate the concentration of hydroxide ions in solution C. $[O H^{-}] =$ .............................. $m o l d m^{- 3}$

[1]

b(iii)

Calculate the concentration of a solution of hydrochloric acid with the same pH as solution C. concentration = .............................. $m o l d m^{- 3}$

[1]

b(iv)

Table 3.1 shows three possible values of the $K_{a}$ of dimethylpropanoic acid, $(C H_{3})_{3} C C O O H$ . Place a tick in Table 3.1 to show the correct value. Explain your answer. Table 3.1 value of $K_{a} / m o l d m^{- 3}$ | place one tick (✓) in this column 9.33 $\times 10^{- 6}$ 1.35 $\times 10^{- 5}$ 3.35 $\times 10^{- 5}$ explanation .......................................................................................................................

[3]

c(i)

Solution D is made by mixing $100 c m^{3}$ of $0.100 m o l d m^{- 3}$ $C H_{3} C H_{2} C O O H$ and $100 c m^{3}$ of $0.100 m o l d m^{- 3}$ $N a C l$ . The pH of solution D is measured as small amounts of $H_{2} S O_{4} (a q)$ are added to it, and when small amounts of $N a O H (a q)$ are added to it. Solution D only acts as a buffer solution when one of these solutions is added to it. Complete the sentence and write an equation for the reaction that occurs. Solution D acts as a buffer when ................................................................ is added to it. equation ............................................................................................................................

[1]

c(ii)

Complete the sentence and explain why solution D does not act as a buffer when the other solution is added. Solution D does not act as a buffer when .................................................. is added to it. explanation .......................................................................................................................

[1]

d(i)

Manganese(II) hydroxide, $M n (O H)_{2}$ , is only slightly soluble in water. The solubility of $M n (O H)_{2}$ in water is $3.28 \times 10^{- 3} g d m^{- 3}$ at $298 K$ . Calculate the concentration of a saturated solution of $M n (O H)_{2}$ at $298 K$ . $[M n (O H)_{2}] =$ .............................. $m o l d m^{- 3}$

[1]

d(ii)

Write an expression for the $K_{s p}$ of $M n (O H)_{2}$ . Give the units of $K_{s p}$ . $K_{s p} =$ units = ..............................

[2]

d(iii)

Use your answers to (d)(i) and (d)(ii) to calculate the value of $K_{s p}$ of $M n (O H)_{2}$ at $298 K$ . $K_{s p} =$ ..............................

[1]

Define enthalpy change of atomisation, $Δ H_{a t}$ .

[1]

Define first electron affinity, EA.

[1]

Explain why the first electron affinity of chlorine is more exothermic than the first electron affinity of iodine.

[2]

The enthalpy change for the reaction $C l_{2} (g) + 2 e^{-} \to 2 C l^{-} (g)$ is $- 486 k J m o l^{- 1}$ . The first electron affinity of chlorine is $- 364 k J m o l^{- 1}$ . Calculate the enthalpy change of atomisation of chlorine. $Δ H_{a t}$ of chlorine = .............................. $k J m o l^{- 1}$

[2]

Cobalt is a transition element which forms compounds containing $C o^{2 +}$ and $C o^{3 +}$ ions. Cobalt(II) sulfate dissolves in water to form a solution containing the $[C o (H_{2} O)_{6}]^{2 +}$ complex ion.

a(i)

Complete the electronic configurations of a $C o^{2 +}$ ion and a $C o^{3 +}$ ion. $C o^{2 +} = [A r]$ .............................. $C o^{3 +} = [A r]$ ..............................

[1]

a(ii)

Explain why transition elements can form complex ions.

[1]

a(iii)

An excess of concentrated $H C l$ is added to a solution containing $[C o (H_{2} O)_{6}]^{2 +}$ . Describe the colour change observed and the state of the cobalt-containing product. The colour changes from .............................. to .............................. . The state of the cobalt-containing product is .............................. .

[2]

a(iv)

Write an equation for the reaction occurring in (a)(iii).

[1]

a(v)

Name the type of reaction occurring in (a)(iii).

[1]

a(vi)

Write an equation for the reaction that occurs when an excess of $N a O H (a q)$ is added to a solution containing $[C o (H_{2} O)_{6}]^{2 +}$ .

[1]

b(i)

Cobalt metal can be oxidised by acidified $K_{2} C r_{2} O_{7}$ . The relevant half-equations, and their $E^{⊖}$ values, are shown. $C o^{2 +} + 2 e^{-} ⇌ C o E^{⊖} = - 0.28 V$ $C r_{2} O_{7}^{2 -} + 14 H^{+} + 6 e^{-} ⇌ 2 C r^{3 +} + 7 H_{2} O E^{⊖} = + 1.33 V$ A $C o^{2 +} / C o$ electrode is constructed in which $[C o^{2 +}]$ is $0.020 m o l d m^{- 3}$ at $298 K$ . Use the Nernst equation to show that the $E$ value for this $C o^{2 +} / C o$ electrode is $- 0.33 V$ .

[2]

b(ii)

An electrochemical cell is constructed using the $C o^{2 +} / C o$ electrode described in (b)(i) and a $C r_{2} O_{7}^{2 -} / C r^{3 +}$ electrode in which all conditions are standard. Calculate the value of $E_{c e l l}$ . $E_{c e l l} =$ ..............................

[1]

b(iii)

A current is drawn from the electrochemical cell described in (b)(ii). Write an equation for the reaction taking place in the cell.

[1]

b(iv)

Complete the sentences to identify the negative electrode and the direction of electron flow when a current is drawn from the cell described in (b)(ii). The .............................. electrode is the negative electrode. Electrons flow from the .............................. electrode to the .............................. electrode.

[1]

A molten $C o^{2 +}$ salt is electrolysed using a current of $0.500 A$ . $0.547 g$ of cobalt metal forms at the cathode. Under the conditions used no other reduction reaction occurs at the cathode. Calculate the time in minutes for which the current flows to produce this mass of cobalt. Give your answer to three significant figures. time = .............................. min

[3]

a(i)

Nickel forms complexes. Give the formula and charge of the tetrahedral complex formed by $N i$ atoms with carbon monoxide molecules. Carbon monoxide is a monodentate ligand. This is complex E. E = ...............................................................................................................................

[1]

a(ii)

Give the formula and charge of the octahedral complex formed by $N i^{2 +}$ ions with ethanedioate ions. This is complex F. F = ...............................................................................................................................

[2]

a(iii)

Identify which complex, E or F, exists as a mixture of two stereoisomers and the type of stereoisomerism involved. The complex which exists as a mixture of two stereoisomers is .............................. . The type of stereoisomerism involved is .............................. .

[1]

b(i)

Cadmium forms complexes with methylamine, $C H_{3} N H_{2}$ , and 1,2-diaminoethane, en. The values of the stability constants, $K_{s t a b}$ , of these complex ions are given in Table 6.1. Table 6.1 complex | $K_{s t a b}$ $[C d (C H_{3} N H_{2})_{4}]^{2 +}$ | $3.5 \times 10^{6}$ $[C d (e n)_{2}]^{2 +}$ | $4.0 \times 10^{10}$ Explain, by reference to its structure, why $C H_{3} N H_{2}$ acts as a monodentate ligand.

[1]

b(ii)

Some $C d^{2 +} (a q)$ is added to a solution containing equal concentrations of $C H_{3} N H_{2}$ and en. Predict which of the two complexes in Table 6.1 forms at the higher concentration. Explain your answer. complex that forms at the higher concentration ................................................................ explanation .......................................................................................................................

[1]

b(iii)

Complete the expression for the $K_{s t a b}$ of $[C d (C H_{3} N H_{2})_{4}]^{2 +}$ . $K_{s t a b} =$

[1]

P, Q, R, S, T, U, and V are the seven structural isomers with molecular formula $C_{5} H_{10} O$ that have a carbonyl group. P $C H_{3} (C H_{2})_{3} C H O$ Q $C H_{3} C H_{2} C H (C H_{3}) C H O$ R $(C H_{3})_{2} C H C H_{2} C H O$ S $(C H_{3})_{3} C C H O$ T $C H_{3} C H_{2} C H_{2} C O C H_{3}$ U $C H_{3} C H_{2} C O C H_{2} C H_{3}$ V $(C H_{3})_{2} C H C O C H_{3}$

Only one of these seven compounds has stereoisomers. Draw three-dimensional diagrams of the two stereoisomers of this compound.

[2]

b(i)

P, Q, R, S, T, U, and V are treated separately with alkaline $I_{2} (a q)$ and the product mixture is acidified. Identify the two compounds that give a positive result with alkaline $I_{2} (a q)$ . ............................................................... and ...............................................................

[1]

b(ii)

Describe the observations when one of the compounds you have identified in (b)(i) is treated with alkaline $I_{2} (a q)$ and give the structural formulae of the two carbon-containing products of this reaction. observations ...................................................................................................................... two carbon-containing products ........................................................................................ and ........................................................................................

[2]

c(i)

The proton ( $^{1} H$ ) NMR spectra of P, Q, R, S, T, U, and V are compared. Identify the only compound that gives a spectrum with two singlets and no other peaks.

[1]

c(ii)

Fig. 7.1 shows the spectrum obtained from one of the compounds. Identify the compound that gives this spectrum.

[1]

c(iii)

Name the splitting pattern of the peak at $δ = 1.1$ in Fig. 7.1. Give the reason for this splitting. name .............................. reason ...............................................................................................................................

[1]

c(iv)

Identify the substance that gives the small peak at $δ = 0$ in Fig. 7.1.

[1]

The carbon-13 NMR spectra of R, S, T and U are compared. Complete Table 7.1 to state the number of peaks in the spectrum of each compound. Table 7.1 compound | number of peaks R $(C H_{3})_{2} C H C H_{2} C H O$ S $(C H_{3})_{3} C C H O$ T $C H_{3} C H_{2} C H_{2} C O C H_{3}$ U $C H_{3} C H_{2} C O C H_{2} C H_{3}$

[2]

Asparagine and aspartic acid are two naturally occurring amino acids. Their structures and isoelectric points are shown in Table 8.1. Table 8.1 amino acid | structure | isoelectric point asparagine | $H O O C C H (N H_{2}) C H_{2} C O N H_{2}$ | 5.41 aspartic acid | $H O O C C H (N H_{2}) C H_{2} C O O H$ | 2.77

Define isoelectric point.

[1]

Draw the structures of asparagine and aspartic acid at pH 2.

[2]

Asparagine and aspartic acid are treated separately with an excess of $L i A l H_{4}$ . Draw the structures of the organic products of these reactions.

[2]

d(i)

Propanedioic acid, $H O O C C H_{2} C O O H$ , is treated with an excess of thionyl chloride, $S O C l_{2}$ . Propanedioyl chloride, $C l O C C H_{2} C O C l$ , is formed. Write an equation for this reaction.

[1]

d(ii)

Propanedioyl chloride reacts with an excess of asparagine to form compound G with molecular formula $C_{11} H_{16} N_{4} O_{8}$ . Each molecule of compound G has four amide groups. Draw the structure of compound G.

[2]

Asparagine is hydrolysed with an excess of hot $N a O H (a q)$ . Draw the structure of the organic product of this reaction.

[2]

A polymer can form from asparagine, $H O O C C H (N H_{2}) C H_{2} C O N H_{2}$ , as the only monomer. Draw a length of the polymer chain containing three monomer residues. Clearly label the repeat unit of the polymer on your diagram.

[3]

g(i)

Aspartic acid exists in two optically active forms. Plane polarised light is passed through pure samples of these two optically active forms in solutions of the same concentration. Describe two similarities and one difference in their effect on the plane polarised light. similarities ......................................................................................................................... ........................................................................................................................................... difference ........................................................................................................................... ...........................................................................................................................

[2]

g(ii)

Give the term used to describe a mixture of equal amounts of the two optically active forms.

[1]

Compound X is made from benzene by the route shown in Fig. 9.1.

Describe the bonding in benzene, $C_{6} H_{6}$ . Your answer should include: • the hybridisation of the six carbon atoms • the types of bond between the carbon atoms • the orbitals that overlap to produce the bonds between the carbon atoms • the type of bond between the carbon atoms and the hydrogen atoms • the orbitals that overlap to produce the bonds between the carbon atoms and the hydrogen atoms.

[3]

Describe the reagents and conditions required for step 1 in Fig. 9.1.

[1]

In step 1 of Fig. 9.1 benzene reacts with $^{+} C H_{3}$ . Complete Fig. 9.2 to show the mechanism for this reaction, including: • the movement of electron pairs using curly arrows • the structure of the intermediate involved.

[3]

Describe the reagents and conditions required for step 2 of Fig. 9.1.

[2]

Identify the reagents required for step 3 of Fig. 9.1. Compound W is the product of this step.

[1]

Name compound W.

[1]

The reagents commonly used for step 4 will not reduce the $- C O O H$ group. Identify the reagents and conditions required for step 4 of Fig. 9.1.

[1]

Benzene can also be used as a starting material to make compound Y. Describe how the route described in Fig. 9.1 (repeated below) can be changed to give compound Y instead of compound X. Explain your answer.

[2]

Mark scheme

9701/42 · Oct/Nov 2025

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1a · 1 mark

1 mark
Mg(NO3)2 → MgO + 2NO2 + ½O2 OR 2Mg(NO3)2 → 2MgO + 4NO2 + O2

1b · 2 marks

M1
Mg(NO3)2 / magnesium nitrate AND magnesium ion / Mg2+ AND is smaller / has higher charge density
M2
nitrate ion / anion is more distorted / polarised

1c(i) · 1 mark

1 mark
magnesium sulfate and water / MgSO4 and H2O

1c(ii) · 3 marks

M1
magnesium sulfate / A has a more exothermic Hlatt and Hhyd
M2
difference in Hhyd is greater
M3
magnesium sulfate / A has a more exothermic Hsol

2a(i) · 1 mark

1 mark
homolytic fission

2a(ii) · 1 mark

1 mark
•O• :N: •O• H:O• :N: •O•

2a(iii) · 1 mark

1 mark
115–120°

2b · 2 marks

M1
3.825  10–3 / 0.003825 / 0.00383 / 0.0038 / 3.8  10–3
M2
units = mol–1 dm3 s–1

2c · 1 mark

1 mark
not constant half-life because overall second order

2d · 1 mark

1 mark
8.17 / 8.2

2e · 2 marks

1 mark
reactants are adsorbed onto the catalyst surface
1 mark
bonds within reactant molecules are weakened
0 marks
products are desorbed from catalyst surface

3a(i) · 1 mark

1 mark
two species that differ by one proton / H+

3a(ii) · 1 mark

1 mark
H2PO4– AND PO43–

3b(i) · 2 marks

M1
[H+] = 2.51  10–4
M2
[CH3CH2COOH] = 4.67  10–3

3b(ii) · 1 mark

1 mark
3.98  10–11

3b(iii) · 1 mark

1 mark
[HCl] = 2.51  10–4

3b(iv) · 3 marks

M1
top box ticked AND weaker acid
M2
alkyl group is electron donating
M3
O–H bond strengthened / anion is destabilised

3c(i) · 1 mark

1 mark
NaOH AND CH3CH2COOH + OH– → CH3CH2COO– + H2O

3c(ii) · 1 mark

1 mark
H2SO4 AND conjugate base of CH3CH2COOH is not present

3d(i) · 1 mark

1 mark
3.69  10–5

3d(ii) · 2 marks

M1
Ksp = [Mn2+][OH–]2
M2
units = mol3 dm–9

3d(iii) · 1 mark

1 mark
2.0  10–13

4a · 1 mark

1 mark
energy required when one mole of gaseous atoms is formed from the element

4b · 1 mark

1 mark
energy released when one mole of gaseous atoms gains one mole of electrons and becomes one mole of gaseous 1– ions

4c · 2 marks

M1
iodine atom has greater radius
M2
less attraction between nucleus and incoming electron in iodine

4d · 2 marks

M1
½ (–486 + (2  364) )
M2
+121

5a(i) · 1 mark

1 mark
Co2+ = [Ar] 3d7 AND Co3+ = [Ar] 3d6

5a(ii) · 1 mark

1 mark
has vacant d orbitals that are energetically accessible

5a(iii) · 2 marks

1 mark
pink
1 mark
blue
0 marks
aqueous

5a(iv) · 1 mark

1 mark
[Co(H2O)6]2+ + 4HCl → [CoCl4]2– + 6H2O + 4H+ OR [Co(H2O)6]2+ + 4Cl– → [CoCl4]2– + 6H2O

5a(v) · 1 mark

1 mark
ligand exchange

5a(vi) · 1 mark

1 mark
[Co(H2O)6]2+ + 2OH– → Co(OH)2(H2O)4 + 2H2O OR [Co(H2O)6]2+ + 2OH– → Co(OH)2 + 6H2O

5b(i) · 2 marks

M1
Nernst equation E = E° + (0.059 / z) × log([oxidised]/[reduced])
M2
E = –0.28 + (0.059 / 2) × log(0.02)

5b(ii) · 1 mark

1 mark
1.66 V

5b(iii) · 1 mark

1 mark
3Co + Cr2O72– + 14H+ → 3Co2+ + 2Cr3+ + 7H2O

5b(iv) · 1 mark

1 mark
Co2+ / Co, Co2+/ Co, Cr2O72– / Cr3+

5c · 3 marks

M1
moles of cobalt = 0.547 / 58.9 = 0.00929
M2
coulombs required = 0.00929  96500  2 = 1792
M3
time required = 1792 / 0.50 = 3584.8 s = 59.7 minutes 3sf

6a(i) · 1 mark

1 mark
Ni(CO)4

6a(ii) · 2 marks

1 mark
ethanedioate given as C2O4
1 mark
formula shows one Ni and three ligands
0 marks
charge = 4–

6a(iii) · 1 mark

1 mark
F AND optical

6b(i) · 1 mark

1 mark
N atom can donate one lone pair of electrons

6b(ii) · 1 mark

1 mark
[Cd(en)2]2+ AND has a larger Kstab / is more stable

6b(iii) · 1 mark

1 mark
[[Cd(CH3NH2)4]2+] / ([Cd2+][CH3NH2]4)

7a · 2 marks

M1
Q CH3CH2CH(CH3)CHO
M2
3D enantiomers of CH3CH2CH(CH3)CHO drawn correctly

7b(i) · 1 mark

1 mark
T CH3CH2CH2COCH3 AND V (CH3)2CHCOCH3

7b(ii) · 2 marks

1 mark
yellow solid
1 mark
CH3CH2CH2COOH OR (CH3)2CHCOOH
0 marks
CHI3

7c(i) · 1 mark

1 mark
S (CH3)3CCHO

7c(ii) · 1 mark

1 mark
U CH3CH2COCH2CH3

7c(iii) · 1 mark

1 mark
triplet AND two hydrogen atoms on neighbouring carbon atoms

7c(iv) · 1 mark

1 mark
TMS / tetramethylsilane / Si(CH3)4

7d · 2 marks

1 mark
4
1 mark
3
0 marks
5
0 marks
3

8a · 1 mark

1 mark
the pH at which an amino acid exists as a zwitterion

8b · 2 marks

M1
[HOOCCH(NH3)CH2CONH2]+
M2
[HOOCCH(NH3)CH2COOH]+

8c · 2 marks

M1
HOCH2CH(NH2)CH2CH2NH2
M2
HOCH2CH(NH2)CH2CH2OH

8d(i) · 1 mark

1 mark
HOOCCH2COOH + 2SOCl2 → ClOCCH2COCl + 2SO2 + 2HCl

8d(ii) · 2 marks

M1
three molecules joined, with four correct amide groups only
M2
whole structure correct as above, displayed formula accepted, skeletal formula as below accepted

8e · 2 marks

M1
hydrolysis of amide to carboxylate ion
M2
hydrolysis of –COOH to carboxylate ion and rest of molecule / –OOCCH(NH2)CH2COO–

8f · 3 marks

1 mark
three monomer residues
1 mark
all linkages correct
1 mark
correct trailing bonds
0 marks
repeat unit marked contains correct atoms

8g(i) · 2 marks

1 mark
rotate the plane of the plane polarised light
1 mark
by the same angle
0 marks
in opposite directions

8g(ii) · 1 mark

1 mark
racemic mixture

9a · 3 marks

1 mark
all C atoms are sp2 hybridised
1 mark
bonds between C atoms are  and 
1 mark
C–C  bonds are formed by overlap of sp2 hybrid orbitals
0 marks
C–C  bonds are formed by overlap of p orbitals
0 marks
bonds between C and H atoms are 
0 marks
C–H bonds are formed by overlap of sp2 hybrid orbitals and s orbitals

9b · 1 mark

1 mark
CH3Cl and AlCl3

9c · 3 marks

M1
curly arrow from within hexagon towards +C
M2
intermediate, usual rules for horseshoe and + charge
M3
curly arrow from C–H bond into ring AND H+ product

9d · 2 marks

M1
HNO3 AND H2SO4
M2
concentrated AND 25 °C ⩽ T ⩽ 60 °C

9e · 1 mark

1 mark
alkaline KMnO4

9f · 1 mark

1 mark
4-nitrobenzoic acid

9g · 1 mark

1 mark
(hot) concentrated HCl and Sn

9h · 2 marks

M1
perform step 3 before step 2 OR perform step 2 before step 1
M2
COOH is 3-directing OR NO2 is 3-directing

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A Level Chemistry 9701 Paper 42, Oct/Nov 2025

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1c(ii) · 3 marks

2a(i) · 1 mark

2a(ii) · 1 mark

2a(iii) · 1 mark

2b · 2 marks

2c · 1 mark

2d · 1 mark

2e · 2 marks

3a(i) · 1 mark

3a(ii) · 1 mark

3b(i) · 2 marks

3b(ii) · 1 mark

3b(iii) · 1 mark

3b(iv) · 3 marks

3c(i) · 1 mark

3c(ii) · 1 mark

3d(i) · 1 mark

3d(ii) · 2 marks

3d(iii) · 1 mark

4a · 1 mark

4b · 1 mark

4c · 2 marks

4d · 2 marks

5a(i) · 1 mark

5a(ii) · 1 mark

5a(iii) · 2 marks

5a(iv) · 1 mark

5a(v) · 1 mark

5a(vi) · 1 mark

5b(i) · 2 marks

5b(ii) · 1 mark

5b(iii) · 1 mark

5b(iv) · 1 mark

5c · 3 marks

6a(i) · 1 mark

6a(ii) · 2 marks

6a(iii) · 1 mark

6b(i) · 1 mark

6b(ii) · 1 mark

6b(iii) · 1 mark

7a · 2 marks

7b(i) · 1 mark

7b(ii) · 2 marks

7c(i) · 1 mark

7c(ii) · 1 mark

7c(iii) · 1 mark

7c(iv) · 1 mark

7d · 2 marks

8a · 1 mark

8b · 2 marks

8c · 2 marks

8d(i) · 1 mark

8d(ii) · 2 marks

8e · 2 marks

8f · 3 marks

8g(i) · 2 marks

8g(ii) · 1 mark

9a · 3 marks

9b · 1 mark

9c · 3 marks

9d · 2 marks

9e · 1 mark

9f · 1 mark

9g · 1 mark

9h · 2 marks

Questions

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