10 free AS Level Chemistry Inorganic Chemistry questions written in the style of Cambridge Chemistry papers: 3 multiple-choice and 7 structured, each with its answer and mark scheme. 4 of them are A* challenge questions, built to catch the mistakes strong students still make.
This topic covers Periodicity, Group 2, Group 17, Nitrogen & sulfur. Work through the questions below, then generate a full Inorganic Chemistry paper with a fresh set every time.
Generate a full Inorganic Chemistry paper →Nitrogen and its compounds are important in the atmosphere.
1 Nitrogen oxides are removed from car exhausts by reaction with oxygen in catalytic converters.
2 NO2 acts as a catalyst in the oxidation of SO2 in the atmosphere.
3 Nitrogen is unreactive because of the strong N≡N triple bond.
Which statements are correct?
Answer: B
The hydrogen halides HCl, HBr and HI are compared.
1 Boiling point decreases from HCl to HI.
2 HI is the strongest reducing agent of the three.
3 The H–X bond energy decreases from HCl to HI.
Which statements are correct?
Answer: B
Which Group 2 hydroxide is least soluble in water?
Answer: C
The Group 2 elements and their compounds show trends.
Describe and explain the trend in reactivity of the Group 2 metals with water.
Write an equation for the thermal decomposition of calcium carbonate.
Explain why the thermal stability of Group 2 carbonates increases down the group.
| Part | Answer and marking points | Marks |
|---|---|---|
| (a) | increases down; IE decreases reactivity increases down the group B1 ionisation energies decrease B1 outer electrons further from nucleus/more shielded B1 | 3 |
| (b) | CaCO₃ → CaO + CO₂ CaCO₃ → CaO + CO₂ B1 | 1 |
| (c) | larger cation, less polarising cation radius increases so charge density decreases B1 less polarisation of the carbonate ion B1 | 2 |
A 3.00 g sample of magnesium carbonate is heated strongly until there is no further change in mass.
Write an equation for the reaction and calculate the expected loss in mass.
Explain the trend in thermal stability of the Group 2 carbonates down the group.
The solid product is added to water and the mixture tested with universal indicator. Write the equation and state the approximate pH.
State and explain the trend in the solubility of Group 2 sulfates, and a use of barium sulfate.
| Part | Answer and marking points | Marks |
|---|---|---|
| (a) | MgCO3 → MgO + CO2; 1.57 g balanced equation B1 moles = 3 ÷ 84.3 C1 1.57 A1 | 3 |
| (b) | stability increases; cation radius increases, charge density decreases; less polarisation/distortion of carbonate ion increases down the group B1 larger cation, lower charge density B1 carbonate anion polarised less B1 | 3 |
| (c) | MgO + H2O → Mg(OH)2; pH 9–10 equation B1 pH alkaline value consistent with solubility B1 | 2 |
| (d) | decreases down the group; barium meal for X-rays (insoluble, so not toxic) solubility decreases B1 barium meal / insoluble so safe B1 | 2 |
This question is about nitrogen and sulfur.
Explain why nitrogen gas is very unreactive.
Explain why ammonia acts as a Brønsted–Lowry base, and draw a dot-and-cross diagram of the ammonium ion.
Describe how oxides of nitrogen are formed in a car engine and removed by a catalytic converter. Include equations.
Explain the role of NO₂ as a catalyst in the oxidation of atmospheric SO₂. Include equations.
State one environmental consequence of nitrate fertiliser run-off.
| Part | Answer and marking points | Marks |
|---|---|---|
| (a) | N≡N triple bond, very high bond energy; non-polar the N≡N triple bond has a very high bond energy B1 and the molecule is non-polar B1 | 2 |
| (b) | lone pair accepts H⁺; NH₄⁺ with dative bond lone pair on N accepts a proton B1 NH₄⁺ diagram with four shared pairs B1 one dative bond shown / overall + charge B1 | 3 |
| (c) | N₂ + O₂ → 2NO at high T; 2NO + 2CO → N₂ + 2CO₂ high temperature in the engine allows N₂ and O₂ to react B1 N₂ + O₂ → 2NO B1 in the catalytic converter 2CO + 2NO → 2CO₂ + N₂ B1 on a platinum / rhodium surface B1 | 4 |
| (d) | NO₂ + SO₂ → NO + SO₃; NO + ½O₂ → NO₂; regenerated SO₂ + NO₂ → SO₃ + NO B1 NO + ½O₂ → NO₂ B1 NO₂ is regenerated so acts as a catalyst B1 | 3 |
| (e) | eutrophication eutrophication / algal bloom leading to deoxygenation of water B1 | 1 |
This question is about the Group 2 elements and their compounds.
Describe and explain the trend in first ionisation energy down Group 2.
Write the equation for the thermal decomposition of calcium nitrate.
Calculate the mass of calcium oxide formed when 3.70 g of anhydrous calcium nitrate is heated to constant mass. [Mᵣ: Ca(NO₃)₂, 164.1; CaO, 56.1]
Explain why the thermal stability of Group 2 nitrates increases down the group.
Describe the trend in solubility of the Group 2 hydroxides and sulfates, and give one use of each trend.
| Part | Answer and marking points | Marks |
|---|---|---|
| (a) | decreases; outer electron further from nucleus; more shielding outweighs increased nuclear charge decreases down the group B1 outer electrons are in shells further from the nucleus B1 increased shielding outweighs the increase in nuclear charge B1 | 3 |
| (b) | 2Ca(NO₃)₂ → 2CaO + 4NO₂ + O₂ correct products B1 balanced B1 | 2 |
| (c) | 1.26 g moles = 3.70/164.1 = 0.0225 M1 1.26 g A1 | 2 |
| (d) | cation larger, lower charge density; polarises nitrate anion less; less distortion of N–O bonds cation radius increases down the group B1 charge density decreases so the cation polarises / distorts the nitrate ion less B1 more heat is needed to break the N–O bonds B1 | 3 |
| (e) | hydroxides more soluble down; sulfates less soluble down; Mg(OH)₂ antacid / BaSO₄ in barium meals or test for sulfate hydroxides become more soluble down the group B1 sulfates become less soluble B1 use: e.g. Mg(OH)₂ as antacid / barium sulfate test or barium meal B1 | 3 |
The elements of Period 3 show trends in their properties.
Explain the trend in atomic radius across Period 3.
Describe the reactions of Na₂O and SO₂ with water, giving the approximate pH of each solution.
| Part | Answer and marking points | Marks |
|---|---|---|
| (a) | nuclear charge increases, same shielding nuclear charge increases B1 shielding is similar, so electrons are pulled closer B1 | 2 |
| (b) | NaOH pH 14; H₂SO₃ pH 2–3 Na₂O + H₂O → 2NaOH B1 pH 13–14 B1 SO₂ + H₂O → H₂SO₃ B1 pH 2–3 B1 | 4 |
Nitrogen and sulfur oxides are atmospheric pollutants.
Explain why nitrogen is unreactive.
Explain how oxides of nitrogen catalyse the oxidation of SO₂ in the atmosphere.
| Part | Answer and marking points | Marks |
|---|---|---|
| (a) | strong triple bond; non-polar strong N≡N triple bond (high bond energy) B1 non-polar molecule B1 | 2 |
| (b) | NO₂ oxidises SO₂, NO regenerated NO₂ + SO₂ → NO + SO₃ B1 NO + ½O₂ → NO₂ (catalyst regenerated) B1 | 2 |
This question is about the halogens and their compounds.
Explain the trend in volatility of the halogens down Group 17.
Concentrated sulfuric acid is added separately to solid sodium chloride and to solid sodium iodide. Describe the products in each case and explain the difference.
Chlorine reacts with cold dilute aqueous sodium hydroxide. Write the equation and state the oxidation numbers of chlorine in each product.
Name this type of reaction and explain your answer.
Describe how aqueous silver nitrate followed by aqueous ammonia distinguishes between chloride, bromide and iodide ions.
| Part | Answer and marking points | Marks |
|---|---|---|
| (a) | volatility decreases; more electrons, stronger instantaneous dipole–induced dipole forces volatility decreases down the group B1 larger molecules with more electrons have stronger instantaneous dipole–induced dipole (London) forces B1 | 2 |
| (b) | NaCl: HCl fumes only; NaI: HI, then SO₂, S, H₂S and purple I₂; I⁻ stronger reducing agent NaCl gives steamy fumes of HCl only B1 NaI gives HI and also SO₂ / S / H₂S with purple vapour / black solid iodine B1 iodide ions are stronger reducing agents than chloride ions B1 they reduce sulfuric acid (S from +6 to lower oxidation states) B1 | 4 |
| (c) | Cl₂ + 2NaOH → NaCl + NaClO + H₂O; −1 and +1 Cl₂ + 2NaOH → NaCl + NaClO + H₂O B1 NaCl: −1 B1 NaClO: +1 B1 | 3 |
| (d) | disproportionation; chlorine both oxidised and reduced disproportionation B1 the same element (chlorine) is simultaneously oxidised (0 to +1) and reduced (0 to −1) B1 | 2 |
| (e) | Cl⁻ white ppt dissolves in dilute NH₃; Br⁻ cream ppt dissolves in conc NH₃; I⁻ yellow ppt insoluble chloride: white precipitate, soluble in dilute ammonia B1 bromide: cream precipitate, soluble in concentrated ammonia B1 iodide: yellow precipitate, insoluble in concentrated ammonia B1 | 3 |
In the 9701 syllabus, Inorganic Chemistry covers Periodicity, Group 2, Group 17, Nitrogen & sulfur.
This page has 10 Inorganic Chemistry questions with answers. For more, the free generator on mentorriyaz.in builds a new Inorganic Chemistry paper with a full mark scheme each time you click.
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Meet Riyaz →Original Cambridge-style practice questions written for mentorriyaz.in. These are not Cambridge past paper questions, and this site is not affiliated with or endorsed by Cambridge University Press & Assessment. Updated 2026-11-04. Paper generator · mentorriyaz.in