A Level Chemistry 9701 Paper 41, Oct/Nov 2025

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9701/41 · Oct/Nov 2025

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a(i)

Solutions of Group 2 hydrogencarbonates, ${M(HCO}_{3})_{2}$ , decompose on heating to give the corresponding metal carbonate, carbon dioxide and water. Write an equation for the decomposition of strontium hydrogencarbonate, ${Sr(HCO}_{3})_{2}$ .

[1]

a(ii)

The thermal stability of Group 2 carbonates increases down the group. Explain this trend.

[2]

The hydroxides and fluorides of Group 2 elements show similar trends in solubility. Describe the trend in the solubility of the fluorides of calcium, strontium and barium. Explain your answer. .................................... .................................... .................................... least soluble most soluble explanation ............................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... .............................................................................................................................................

[4]

c(i)

Define enthalpy change of hydration, $Δ H_{hyd}$ .

[1]

c(ii)

State the main factors that affect the magnitude of enthalpy change of hydration. Explain your answer.

[2]

Table 1.1 shows various energy changes. Table 1.1

energy change	value / $kJ {mol}^{- 1}$
lattice energy of ${MgF}_{2}$	$- 2957$
enthalpy change of hydration, $Δ H_{hyd}$ , of ${Mg}^{2 +}$	$- 1926$
enthalpy change of hydration, $Δ H_{hyd}$ , of $F^{-}$	$- 505$

Use data from Table 1.1 to calculate the enthalpy change of solution, $Δ H_{sol}$ , for ${MgF}_{2} (s)$ . It may be helpful to draw a labelled energy cycle. Show your working. $Δ H_{sol} of {MgF}_{2} (s) = .............................. kJ {mol}^{- 1}$

[2]

e(i)

Mercury(I) fluoride, ${Hg}_{2} F_{2}$ , is sparingly soluble in water. The cation in ${Hg}_{2} F_{2}$ exists as the diatomic ion ${Hg}_{2}^{2 +}$ with a covalent $Hg - Hg$ bond. Write the expression for the solubility product, $K_{sp}$ , of ${Hg}_{2} F_{2}$ . Include the units. $K_{sp} =$ units ..............................

[2]

e(ii)

The solubility of ${Hg}_{2} F_{2}$ is $9.20 \times 10^{- 3} mol {dm}^{- 3}$ at $298 K$ . Calculate the value of $K_{sp}$ of ${Hg}_{2} F_{2}$ at $298 K$ . $K_{sp} = ..............................$

[1]

Iron can form stable ions in the +2 and +3 oxidation states. Explain why transition elements have variable oxidation states.

[1]

Aqueous solutions of iron(II) salts contain the complex ion $[Fe (H_{2} O)_{6}]^{2 +}$ . Define complex ion.

[1]

c(i)

$[Fe (H_{2} O)_{6}]^{2 +}$ can be converted into $[Fe (H_{2} O)_{4} (OH)_{2}]$ . Suggest a suitable reagent for this conversion. State the type of reaction. reagent .............................................................................................................................. type of reaction ..................................................................................................................

[1]

c(ii)

$[Fe (H_{2} O)_{4} (OH)_{2}]$ is a green precipitate that turns brown on standing in air. Table 2.1 shows electrode potentials for some electrode reactions. Table 2.1

electrode reaction	$E^{⊖} / V$
$Fe (H_{2} O)_{3} (OH)_{3} + H_{2} O + e^{-} ⇌ Fe (H_{2} O)_{4} (OH)_{2} + {OH}^{-}$	$- 0.56$
$O_{2} + 2 H_{2} O + 4 e^{-} ⇌ 4 {OH}^{-}$	$+ 0.40$

Use the information in Table 2.1 to explain why $[Fe (H_{2} O)_{4} (OH)_{2}]$ turns brown on standing in air. Include an equation for this reaction.

[3]

The complex $[Co ({NH}_{3})_{6}]^{2 +}$ reacts with hydrogen peroxide as shown. reaction 1 $2 [Co ({NH}_{3})_{6}]^{2 +} + H_{2} O_{2} \to 2 [Co ({NH}_{3})_{6}]^{3 +} + 2 {OH}^{-} E_{cell}^{⊖} = + 1.67 V$ Calculate $Δ G^{⊖}$ , in $kJ {mol}^{- 1}$ , for reaction 1. $Δ G^{⊖} = .............................. kJ {mol}^{- 1}$

[2]

Solid manganese(IV) oxide, ${MnO}_{2}$ , catalyses the decomposition of hydrogen peroxide. $2 H_{2} O_{2} (aq) \to 2 H_{2} O (l) + O_{2} (g)$ State the type of catalysis for this reaction. Explain your answer.

[1]

b(i)

Hydrogen peroxide reacts with iodide ions in acidic conditions as shown. $H_{2} O_{2} + 2 I^{-} + 2 H^{+} \to 2 H_{2} O + I_{2}$ The initial rate of this reaction is investigated with different concentrations of $H_{2} O_{2}$ , $I^{-}$ and $H^{+}$ . The results obtained are shown in Table 3.1. Table 3.1

experiment	$[H_{2} O_{2}] / mol {dm}^{- 3}$	$[I^{-}] / mol {dm}^{- 3}$	$[H^{+}] / mol {dm}^{- 3}$	initial rate / $mol {dm}^{- 3} s^{- 1}$
1	0.0450	0.0300	0.0125	$2.42 \times 10^{- 3}$
2	0.0225	0.0600	0.0125	$2.42 \times 10^{- 3}$
3	0.0225	0.120	0.0125	$4.84 \times 10^{- 3}$
4	0.0450	0.120	0.0500	$9.68 \times 10^{- 3}$

Use the information in Table 3.1 to deduce the rate equation for this reaction. Explain your reasoning.

[4]

b(ii)

Use your rate equation from (b)(i) and the data from Experiment 1 to calculate the rate constant, $k$ , for this reaction. Include the units of $k$ . $k = .............................. units ..............................$

[2]

c(i)

The rate of the thermal decomposition of azomethane, ${CH}_{3} N = {NCH}_{3}$ , is investigated. ${CH}_{3} N = {NCH}_{3} \to N_{2} + C_{2} H_{6}$ Fig. 3.1 shows the results obtained. The reaction is first order with respect to ${CH}_{3} N = {NCH}_{3}$ . Use Fig. 3.1 to calculate two half-lives, $t_{\frac{1}{2}}$ , to show that the reaction is first order.

[2]

c(ii)

Use your answer to (c)(i) to calculate the rate constant, $k$ , for the decomposition of azomethane. $k = .............................. s^{- 1}$

[1]

Describe the effect of increasing temperature on the rate constant and on the rate of a reaction.

[1]

Define standard cell potential, $E_{cell}^{⊖}$ . Include a description of standard conditions.

[2]

b(i)

The Daniell cell is an electrochemical cell consisting of a ${Cu}^{2 +} (aq) / Cu (s)$ electrode and a ${Zn}^{2 +} (aq) / Zn (s)$ electrode. Draw a labelled diagram of this electrochemical cell. Include all necessary substances and relevant pieces of apparatus needed to measure the $E_{cell}^{⊖}$ . It is not necessary to state the conditions used.

[3]

b(ii)

State the charge carriers that transfer current through the solutions and through the wire. the solutions .............................. the wire ..............................

[1]

b(iii)

The standard electrode potential, $E^{⊖}$ , for the ${Zn}^{2 +} (aq) / Zn (s)$ electrode is $- 0.76 V$ . Water is added to a standard ${Zn}^{2 +} (aq) / Zn (s)$ electrode. The new concentration of ${Zn}^{2 +} (aq)$ is $0.25 mol {dm}^{- 3}$ . Use the Nernst equation to calculate the electrode potential, $E$ , for this new ${Zn}^{2 +} (aq) / Zn (s)$ electrode. $E ({Zn}^{2 +} (aq) / Zn (s)) = .............................. V$

[2]

c(i)

An electrochemical cell consists of a $ZnO / Zn$ electrode and a ${MnO}_{2} / {Mn}_{2} O_{3}$ electrode in an alkaline electrolyte. The standard cell potential, $E_{cell}^{⊖}$ , for this cell is $+ 1.47 V$ . The half-equation at each electrode when this cell is discharging is shown. $Zn + 2 {OH}^{-} \to ZnO + H_{2} O + 2 e^{-}$ $2 {MnO}_{2} + H_{2} O + 2 e^{-} \to {Mn}_{2} O_{3} + 2 {OH}^{-}$ Use this information to determine the change in oxidation state of manganese when this cell is discharging. from .............................. to ..............................

[1]

c(ii)

Write the equation for the overall reaction that occurs when this cell is discharging.

[1]

c(iii)

The $E^{⊖}$ for the $ZnO / Zn$ electrode is $- 1.28 V$ . Calculate the standard electrode potential, $E^{⊖}$ , for the ${MnO}_{2} / {Mn}_{2} O_{3}$ electrode. $E^{⊖} ({MnO}_{2} / {Mn}_{2} O_{3}) = .............................. V$

[1]

Copper shows typical properties of transition elements, including its behaviour as a catalyst. Complete Table 5.1 to show the total number of unpaired electrons in the 3d and 4s orbitals of an isolated gaseous Cu atom and a ${Cu}^{2 +}$ ion. Table 5.1

species	number of unpaired electrons
species	3d	4s
$Cu$
${Cu}^{2 +}$

[1]

The 3d orbitals in an isolated ${Cu}^{2 +}$ ion are degenerate. Complete the diagram to show the relative energies of the 3d orbitals in an isolated ${Cu}^{2 +}$ ion and in ${Cu}^{2 +}$ in a tetrahedral complex.

[2]

Explain why transition elements behave as catalysts.

[2]

${CN}^{-}$ is a monodentate ligand. Table 5.2 shows information about two complex ions that contain only ${CN}^{-}$ ions as ligands. Complete Table 5.2. Table 5.2

metal ion	coordination number	formula of complex ion	charge of complex ion
${Ag}^{+}$	2
${Fe}^{2 +}$			4-

[2]

The complex ion $[Au (CN)_{2} {Br}_{2}]^{-}$ displays geometrical (cis/trans) isomerism. Draw the structure of trans- $[Au (CN)_{2} {Br}_{2}]^{-}$ . State its shape and the Br-Au-Br bond angle. shape .............................. Br-Au-Br bond angle = ..............................

[2]

f(i)

An impure sample of a vanadium(V) compound of mass $0.250 g$ is dissolved in aqueous acid. This solution contains ${VO}_{3}^{-}$ ions. An excess of zinc is added to this solution. All the ${VO}_{3}^{-}$ ions are reduced to $V^{2 +}$ ions and Zn atoms are oxidised to ${Zn}^{2 +}$ ions. The unreacted zinc is removed and the resulting solution is titrated with acidified ${MnO}_{4}^{-}$ . The end-point is reached when $22.5 {cm}^{3}$ of $0.0750 mol {dm}^{- 3} {MnO}_{4}^{-}$ is added. A redox reaction takes place and all the $V^{2 +}$ reacts forming ${VO}_{3}^{-}$ . $3 {MnO}_{4}^{-} + 5 V^{2 +} + 3 H_{2} O \to 3 {Mn}^{2 +} + 5 {VO}_{3}^{-} + 6 H^{+}$ Calculate the percentage by mass of vanadium in the $0.250 g$ of impure sample. Assume the impurities do not contain any vanadium ions. Show your working. percentage of vanadium = ..............................

[3]

f(ii)

Complete the equation for the reaction between acidified ${VO}_{3}^{-}$ ions and Zn metal. ...... ${VO}_{3}^{-}$ + ...... Zn + ............ $\to$ ...... $V^{2 +}$ + ...... ${Zn}^{2 +}$ + ..............

[2]

a(i)

Thin-layer and gas/liquid chromatography can be used to separate mixtures into their individual components. Define the following terms used in chromatography. $R_{f}$ value ............................................................................................................................. ........................................................................................................................................... retention time .................................................................................................................... ...........................................................................................................................................

[2]

a(ii)

Each type of chromatography makes use of a stationary phase and a mobile phase. Complete Table 6.1 with a description of each of these. Table 6.1

	stationary phase	mobile phase
thin-layer chromatography
gas/liquid chromatography

[1]

A mixture of two substances A and B is analysed by thin-layer chromatography. The $R_{f}$ value of substance A is larger than that of substance B. Suggest why substance A has a larger $R_{f}$ value.

[1]

c(i)

The two isomeric compounds Y and Z are analysed by proton ( $^{1} H$ ) NMR spectroscopy. Complete Table 6.2 to predict the number of peaks observed in the proton ( $^{1} H$ ) NMR spectra for Y and Z. Table 6.2

compound	number of peaks observed
Y
Z

[1]

c(ii)

Name all the different splitting patterns observed in the proton ( $^{1} H$ ) NMR spectra for Y and Z. Y ........................................................................................................................................ Z ........................................................................................................................................

[2]

State the relative acidities of bromoethanoic acid, ${BrCH}_{2} COOH$ , chloroethanoic acid, ${ClCH}_{2} COOH$ , ethanoic acid, ${CH}_{3} COOH$ and ethanol, ${CH}_{3} {CH}_{2} OH$ . Explain your answer. .................................. .................................. .................................. .................................. most acidic least acidic ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ...................................................................................................................................................

[4]

Fig. 7.1 shows the reaction of methylbenzene and ethanedioic acid with ${KMnO}_{4}$ . Predict the major carbon-containing product for each of these reactions.

[2]

c(i)

Polyamide X can be synthesised from ethanedioic acid and benzene-1,4-diamine. Draw the repeat unit of polyamide X in the box. The new functional group formed should be shown displayed. polyamide X

[2]

c(ii)

Benzene-1,4-diamine can be formed by reduction of 1,4-dinitrobenzene. Complete the equation for this reduction. [H] represents one atom of hydrogen from a reducing agent. + .......... [H] $\to H_{2} N - C_{6} H_{4} - {NH}_{2}$ + .......................................................... .....................

[1]

d(i)

Fig. 7.2 shows the two-step synthesis of the azo compound W. Suggest structures for compounds V and W and draw them in the boxes in Fig. 7.2.

[2]

d(ii)

Give the reagents and conditions for step 1.

[1]

a(i)

In the electrophilic substitution of arenes, different substituents can direct to different ring positions. Describe the directing effect of the $- {NO}_{2}$ group. Explain your answer.

[1]

a(ii)

The nitration of arenes uses a mixture of concentrated ${HNO}_{3}$ and concentrated $H_{2} {SO}_{4}$ to generate the ${NO}_{2}^{+}$ electrophile. Write an equation for the formation of the ${NO}_{2}^{+}$ electrophile.

[1]

b(i)

Carbon-carbon bond formation is an important reaction in organic synthesis. Fig. 8.1 shows the synthesis of compound Q from benzene in two reaction steps. Draw the structure of compound P in the box in Fig. 8.1.

[1]

b(ii)

Suggest reagents and conditions for reactions 1 and 2 in Fig. 8.1. reaction 1 .......................................................................................................................... reaction 2 ..........................................................................................................................

[2]

Separate samples of $C_{6} H_{5} Br$ and $C_{6} H_{5} {CH}_{2} Br$ are added to warm ${AgNO}_{3} (aq)$ . State the expected observations, if any. Explain your answer. $C_{6} H_{5} Br$ with ${AgNO}_{3} (aq)$ ................................................ $C_{6} H_{5} {CH}_{2} Br$ with ${AgNO}_{3} (aq)$ ................................................ explanation ............................................................................................................................... ................................................................................................................................................... ................................................................................................................................................... ...................................................................................................................................................

[3]

d(i)

Acyl bromides, RCOBr, react readily with $H_{2} O$ . The mechanism of this reaction is similar to that of the reaction of $H_{2} O$ with acyl chlorides, RCOCl. Name the mechanism of this reaction.

[1]

d(ii)

Complete the mechanism in Fig. 8.2 for the reaction of RCOBr with $H_{2} O$ . Include all relevant lone pairs of electrons, curly arrows, charges and dipoles. Draw the structure of the intermediate.

[4]

Explain why amides are much weaker bases than amines.

[2]

b(i)

Fig. 9.1 shows the preparation of 2-phenylethylamine, $C_{6} H_{5} {CH}_{2} {CH}_{2} {NH}_{2}$ , by three different routes. Suggest structures for compounds M and N and draw them in the boxes in Fig. 9.1.

[2]

b(ii)

Give the reagents and conditions for reaction 1.

[1]

Fig. 9.2 shows compound H which is a useful starting material in organic synthesis. H contains an alkene and an amine functional group. Name the other functional group and give the classification of the amine group in H. other functional group in H ................................................ classification of amine ................................................

[1]

d(i)

Ozonolysis involves the oxidative cleavage of a C=C bond in alkenes using ozone, $O_{3}$ , as shown in Fig. 9.3. Fig. 9.4 shows the first step in this reaction which involves the formation of an ozonide intermediate. On Fig. 9.4, draw three curly arrows to complete the mechanism of this step.

[2]

d(ii)

L is formed from alkene K, $C_{8} H_{14}$ , by a similar reaction to that shown in Fig. 9.3. Suggest the structure of K. K $C_{8} H_{14}$

[1]

Mark scheme

9701/41 · Oct/Nov 2025

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1a(i) · 1 mark

1 mark
Sr(HCO3)2 → SrCO3 + CO2 + H2O

1a(ii) · 2 marks

M1
radius of cation / M2+ increases OR charge density of cation / M2+ decreases
M2
less polarisation / less distortion of the anion / carbonate ion

1b · 4 marks

M1
least soluble CaF2 < SrF2 < BaF2 most soluble
M2
Hlatt and Hhyd both become less exothermic / less negative
M3
Hhyd changes less / becomes less exothermic by a smaller extent OR Hlatt changes more / becomes less exothermic by a larger extent
M4
Hsol becomes more exothermic / more negative

1c(i) · 1 mark

1 mark
enthalpy change when one mole of gaseous ions dissolve in water to form a solution

1c(ii) · 2 marks

M1
ionic radii AND ionic charge
M2
(ionic) radii increase / charge density decreases AND ∆Hhyd decreases/less exothermic AND less attraction between water molecules and (gaseous) ions OR as ionic charge increases / charge density increases AND ∆Hhyd increases/more exothermic AND more attraction between water molecules and (gaseous) ions

1d · 2 marks

M1
use of –2957 / –1926 / –505 AND 2  (–505)
M2
correct signs and evaluation ∆Hsol of MgF2(s) = –1926 + (2  –505) – (–2957) = (+)21 kJ mol–1

1e(i) · 2 marks

M1
Ksp = [Hg22+] [F–]2
M2
units = mol3 dm–9

1e(ii) · 1 mark

1 mark
Ksp = 22  (9.20  10–3)3 = 3.11  10–6 min 2sf

2a · 1 mark

1 mark
the (3)d and (4)s sub-shells / orbitals / electrons are close / similar in energy

2b · 1 mark

1 mark
species or ion formed by a central metal atom/ion AND surrounded by/bonded to (one or more) ligands

2c(i) · 1 mark

1 mark
NaOH / OH–(aq) AND precipitation / ligand exchange / deprotonation / acid–base

2c(ii) · 3 marks

M1
Fe(H2O)4(OH)2 is oxidised (from + 2 to + 3 on standing)
M2
Eo of Fe(H2O)3(OH)3 is more negative than Eo of O2 OR Eocell = 0.40 – (–0.56) = (+)0.96 V
M3
4Fe(H2O)4(OH)2 + O2 → 4Fe(H2O)3(OH)3 + 2H2O

2d · 2 marks

M1
∆Go = –nEocellF AND n = 2 OR –2  1.67  96 500
M2
∆Go = –322.3 kJ mol–1

3a · 1 mark

1 mark
heterogeneous AND MnO2 is in a different state / phase to the reactants / H2O2

3b(i) · 4 marks

M1
(expt 2 and 3) [I–]  2 initial rate  2 so 1st order wrt [I–]
M2
(expt 1 and 2) [I–]  2, [H2O2]  0.5 initial rate  1 so 1st order wrt [H2O2] OR (expt 1 and 4) [I–]  4 initial rate  4 AND [H+]  4 so zero order wrt [H+] OR (expt 1 and 3) [I–]  4, [H2O2]  0.5 initial rate  2 so 1st order wrt [H2O2]
M3
(expt 1 and 4) [I–] x 4 , [H+]  4 initial rate  4 so zero order wrt [H+] OR (expt 3 and 4) [H2O2]  2 initial rate  2AND [H+] x 4 so zero order wrt [H+] OR (expt 3 and 4) [H2O2]  2, [H+]  4 initial rate  2 so 1st order wrt [H2O2]
M4
rate = k [H2O2] [I–] OR rate = k [H2O2] [I–] [H+]0

3b(ii) · 2 marks

M1
k = 2.42  10–3 ÷ (0.045  0.030) = 1.79 min 2sf
M2
units = dm3 mol-1 s-1

3c(i) · 2 marks

M1
calculation of one t1/2 = 60 s ± 5 s
M2
two t1/2 calculated that are constant

3c(ii) · 1 mark

1 mark
k = In2 ÷ 60 = 0.0116 OR k = 0.693 ÷ 60 = 0.0116 min 2sf

3d · 1 mark

1 mark
increases k and increases the rate of reaction

4a · 2 marks

M1
potential difference / voltage / EMF AND between two half-cells / two electrodes (in a cell)
M2
(at concentration of) 1 mol dm–3 AND (pressure of) 1 atm / 101 kPa AND (temperature of) 298 K / 25 °C

4b(i) · 3 marks

M1
salt bridge labelled AND voltmeter / V AND wire to electrode and liquid level shown [complete circuit]
M2
Cu(s) AND Cu2+(aq)
M3
Zn(s) AND Zn2+(aq)

4b(ii) · 1 mark

1 mark
ions AND electrons

4b(iii) · 2 marks

M1
Nernst equation E = Eo + (0.059/z) log(Zn2+/Zn)
M2
E = –0.76 + (0.059 / 2) log(0.25) = –0.778 V OR E = –0.76 + (8.31  298) / (96 500  2) ln(0.25) = –0.778 V min 2sf

4c(i) · 1 mark

1 mark
(from) +4 (to) +3

4c(ii) · 1 mark

1 mark
Zn + 2MnO2 → ZnO + Mn2O3

4c(iii) · 1 mark

1 mark
Eo(MnO2 / Mn2O3) = 1.47 – 1.28 = (+)0.19 V

5a · 1 mark

1 mark
species Cu: 3d = 0, 4s = 1; Cu2+: 3d = 1, 4s = 0

5b · 2 marks

1 mark
five 3d orbitals (lines, boxes) in the isolated Cu2+ ion of the same energy
1 mark
splitting: three higher and two lower d orbitals
1 mark
energy of all five d orbitals in complex higher than all d orbitals in isolated ion

5c · 2 marks

M1
more than one (stable) oxidation state / exist in variable oxidation states
M2
vacant / empty (d) orbitals are energetically accessible OR vacant / empty (d) orbitals can form dative bonds with ligands

5d · 2 marks

1 mark
Ag+: coordination number = 2, formula = Ag(CN)2, charge = 1–
1 mark
Fe2+: coordination number = 6, formula = Fe(CN)6, charge = 4–

5e · 2 marks

M1
stereoisomers drawn for Au(CN)2Br2
M2
(shape) square planar AND (bond angle) 180o

5f(i) · 3 marks

M1
moles MnO4– = 0.075  0.0225 = 1.6875  10–3
M2
moles V2+ = 5 / 3  1.6875  10–3 = 2.8125  10–3
M3
mass V = 50.9  2.8125  10–3 = 0.143 g % of V = 0.143 / 0.250  100 = 57.3 min 2sf

5f(ii) · 2 marks

M1
2 : 3 ratio on both sides
M2
rest of the equation correct

6a(i) · 2 marks

M1
(Rf value) is distance moved by a component / spot / solute AND divided by distance moved by solvent OR (Rf value) is the ratio of distance moved by a component / spot / solute AND by distance moved by solvent
M2
(retention time) is (the time) between injection and detection (of a component)

6a(ii) · 1 mark

1 mark
thin-layer chromatography: polar solvent OR non-polar solvent OR named solvent gas-liquid chromatography: non-volatile liquid OR high boiling point liquid

6b · 1 mark

1 mark
A is more soluble in the mobile phase OR A has less adsorption to the stationary phase

6c(i) · 1 mark

1 mark
Y: 2, Z: 2

6c(ii) · 2 marks

M1
Y (two) singlet(s)
M2
Z triplet AND quartet

7a · 4 marks

M1
ClCH2COOH BrCH2COOH CH3COOH CH3CH2OH (most acidic to least acidic)
M2
electron withdrawing groups / electronegative groups / negative inductive effect AND weakens O–H bond / more stable anion OR electron donating groups / positive inductive effect AND strengthens O-H bond / less stable anion
M3
chlorine is more electron-withdrawing / electronegative than bromine (related to XCH2COOH)
M4
electron withdrawing of C=O / negative inductive effect of C=O (related to COOH) OR positive inductive effect / electron donating of alkyl / ethyl / R group (related to ROH)

7b · 2 marks

M1
benzoic acid structure / C6H5COOH
M2
CO2

7c(i) · 2 marks

M1
correct displayed amide bond with C=O, (C6H5)−N and (C–)C=O
M2
rest of the structure correct with continuation bonds

7c(ii) · 1 mark

1 mark
O2N-C6H4-NO2 + 12[H] → H2N-C6H4-NH2 + 4H2O

7d(i) · 2 marks

M1
Cl- +N#N-C6H4-N#N+ Cl-
M2
structure of bis-azo dye

7d(ii) · 1 mark

1 mark
HNO2 (and HCl) AND ⩽10 °C OR NaNO2 AND HCl AND ⩽10 °C

8a(i) · 1 mark

1 mark
NO2 group directs to 3 (and 5) / meta position AND due to being an electron-withdrawing / electronegative group

8a(ii) · 1 mark

1 mark
HNO3 + H2SO4 → NO2+ + HSO4– + H2O OR HNO3 + 2H2SO4 → NO2+ + 2HSO4– + H3O+

8b(i) · 1 mark

1 mark
acetophenone / C6H5COCH3 structure

8b(ii) · 2 marks

M1
(reaction 1) ethanoyl chloride / CH3COCl AND AlCl3
M2
(reaction 2) 2-bromopropane / (CH3)2CHBr AND FeBr3

8c · 3 marks

M1
with C6H5Br no change / no precipitate AND with C6H5CH2Br cream precipitate
M2
in C6H5Br: lone pair / p-orbital on Br delocalised / overlaps with ring /  system
M3
C–Br bond stronger / has partially double bond character

8d(i) · 1 mark

1 mark
(nucleophilic) addition–elimination

8d(ii) · 4 marks

M1
any two of: lone pair on O; curly arrow from (lone pair) O (in H2O) to C (of C=O); correct dipole on C=O; curly arrow from the C=O bond to O atom
M2
all four of: lone pair on O; curly arrow from (lone pair) O (in H2O) to C (of C=O); correct dipole on C=O; curly arrow from the C=O bond to O atom
M3
correct intermediate
M4
curly arrow from (lone pair on) O(–) to C–O bond AND curly arrow from C–Br to Br

9a · 2 marks

M1
(basicity linked to) ability of lone pair / p-orbital to AND accept / coordinate with a proton / H+
M2
(lone pair of) electrons on N is delocalised into C=O group (and make amides neutral)

9b(i) · 2 marks

M1
structure M (C6H5CH2CH2CN)
M2
structure N (C6H5CH2CH2Br)

9b(ii) · 1 mark

1 mark
LiAlH4

9c · 1 mark

1 mark
ketone / carbonyl AND secondary / 2o

9d(i) · 2 marks

1 mark
curly arrow 1: from O lone pair to C atom (in C=C)
1 mark
curly arrow 2: from C=C bond to the right-hand O atom in O=O AND curly arrow 3: from O=O bond to O+

9d(ii) · 1 mark

1 mark
structure of 1-ethyl-2-methylcyclopentene

Questions

1
Question 115 marks
Mark scheme ›
2
Question 28 marks
Mark scheme ›
3
Question 311 marks
Mark scheme ›
4
Question 411 marks
Mark scheme ›
5
Question 514 marks
Mark scheme ›
6
Question 67 marks
Mark scheme ›
7
Question 712 marks
Mark scheme ›
8
Question 813 marks
Mark scheme ›
9
Question 99 marks
Mark scheme ›

A Level Chemistry 9701 Paper 41, Oct/Nov 2025

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Mark scheme

1a(i) · 1 mark

1a(ii) · 2 marks

1b · 4 marks

1c(i) · 1 mark

1c(ii) · 2 marks

1d · 2 marks

1e(i) · 2 marks

1e(ii) · 1 mark

2a · 1 mark

2b · 1 mark

2c(i) · 1 mark

2c(ii) · 3 marks

2d · 2 marks

3a · 1 mark

3b(i) · 4 marks

3b(ii) · 2 marks

3c(i) · 2 marks

3c(ii) · 1 mark

3d · 1 mark

4a · 2 marks

4b(i) · 3 marks

4b(ii) · 1 mark

4b(iii) · 2 marks

4c(i) · 1 mark

4c(ii) · 1 mark

4c(iii) · 1 mark

5a · 1 mark

5b · 2 marks

5c · 2 marks

5d · 2 marks

5e · 2 marks

5f(i) · 3 marks

5f(ii) · 2 marks

6a(i) · 2 marks

6a(ii) · 1 mark

6b · 1 mark

6c(i) · 1 mark

6c(ii) · 2 marks

7a · 4 marks

7b · 2 marks

7c(i) · 2 marks

7c(ii) · 1 mark

7d(i) · 2 marks

7d(ii) · 1 mark

8a(i) · 1 mark

8a(ii) · 1 mark

8b(i) · 1 mark

8b(ii) · 2 marks

8c · 3 marks

8d(i) · 1 mark

8d(ii) · 4 marks

9a · 2 marks

9b(i) · 2 marks

9b(ii) · 1 mark

9c · 1 mark

9d(i) · 2 marks

9d(ii) · 1 mark

Questions

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