Lesson 3.2.3.1

3.2.3.1 Trends in properties Quiz: AQA Chemistry, Unit 2

20 questions

Written by Revision Ninja · Last reviewed 11 October 2026

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Lesson 3.2.3.1, Trends in properties: 20 multiple choice questions for the AQA Chemistry (7405), Unit 2: Inorganic chemistry, written with Revision Ninja.

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The 20 questions

  1. How does the electronegativity of the halogens change down Group 7?

    • It decreases, because the atoms lose electrons more easily down the group
    • It stays the same, because all halogens have seven outer electrons
    • It decreases, because the bonding pair is further from the nucleus and shielding increases
    • It increases, because the atoms become larger and attract electrons more strongly

  2. Why does the boiling point of the halogens increase down Group 7?

    • The molecules have stronger covalent bonds between the atoms, which need more energy to break
    • The molecules have more electrons and larger London forces between them
    • The molecules become smaller, so they pack together more tightly
    • The molecules become more ionic, so stronger electrostatic forces hold them together

  3. What is the boiling point trend across the halogens F2, Cl2, Br2 and I2?

    • It is the same for all four halogens
    • It decreases from fluorine to iodine
    • It increases from fluorine to iodine
    • It increases then decreases from fluorine to iodine

  4. How does the oxidising ability of the halogens change down Group 7?

    • It stays the same, because all halogens are diatomic molecules
    • It increases, so iodine is a stronger oxidising agent than chlorine
    • It increases steadily, so astatine is the weakest oxidising agent
    • It decreases, so chlorine is a stronger oxidising agent than iodine

  5. In aqueous solution, which displacement reaction occurs?

    • Br2 + 2Cl^- -> 2Br^- + Cl2
    • I2 + 2Cl^- -> 2I^- + Cl2
    • Cl2 + 2I^- -> 2Cl^- + I2 is not possible in water
    • Cl2 + 2Br^- -> 2Cl^- + Br2

  6. Which reagent turns a mixture of chlorine and sodium bromide solution orange, showing that bromine has formed?

    • Water, which reacts with bromide ions to form orange bromine
    • Chlorine, which displaces bromide ions to form orange bromine
    • Sodium hydroxide, which oxidises bromide ions to bromine
    • Sodium chloride, which reacts with bromide to form orange bromine

  7. How does the reducing ability of the halide ions change down Group 7?

    • It stays the same, because all halide ions have a 1- charge
    • It decreases, so chloride is a stronger reducing agent than iodide
    • It increases, so chloride is a stronger reducing agent than iodide
    • It increases, so iodide is a stronger reducing agent than chloride

  8. What is observed when solid sodium iodide is heated with concentrated sulfuric acid?

    • The sulfuric acid is reduced to sulfur dioxide only, with no iodine formed, since iodide is not oxidised by it
    • Only hydrogen chloride gas is formed, with no colour change, because iodide is a weaker reducing agent than chloride
    • The iodide is oxidised, giving iodine and sometimes hydrogen sulfide, with a purple vapour seen
    • No reaction occurs, because iodide ions are not reactive with acid and cannot be oxidised by concentrated sulfuric acid

  9. Why does NaBr react with concentrated sulfuric acid to form bromine, while NaCl does not?

    • Bromide ions are stronger reducing agents than chloride ions, so they are oxidised by the sulfuric acid
    • Chloride ions are stronger reducing agents than bromide ions, so they are oxidised more easily
    • Bromine is more stable than chlorine, so it does not form in any reaction
    • Sodium chloride is a covalent compound, so it cannot react with sulfuric acid

  10. Which reagent is used to identify and distinguish the halide ions?

    • Acidified barium chloride solution
    • Litmus solution, which changes colour with each halide
    • Dilute sodium hydroxide solution alone
    • Acidified silver nitrate solution

  11. What precipitate colours are formed with acidified silver nitrate for chloride, bromide and iodide ions respectively?

    • Cream, yellow and white
    • White, cream and yellow
    • Black, white and red
    • Yellow, white and cream

  12. Why is the silver nitrate solution acidified in the halide test?

    • To make the silver ions more reactive, so the reaction takes place much faster and the precipitate forms at once
    • To react with the halide ions and make them insoluble in the mixture, so that they settle out as a solid
    • To dissolve the silver halide precipitates so that they can be identified more easily by the colour change
    • To remove carbonate ions, which would also form a precipitate with silver ions and confuse the result

  13. Why is ammonia solution added after silver nitrate in the halide test?

    • To distinguish silver halides by their different solubility in ammonia
    • To neutralise the acid, so that the solution becomes alkaline
    • To react with the silver ions and remove them from solution completely
    • To make the silver halide precipitate form more quickly

  14. Which silver halide dissolves in dilute aqueous ammonia?

    • None of them, because all silver halides are insoluble in ammonia
    • Silver chloride
    • Silver iodide
    • Silver bromide only in concentrated ammonia, which is the same as silver iodide

  15. What is the trend in solubility of the silver halides in ammonia down the group?

    • It increases, so AgI dissolves most readily in ammonia
    • It stays the same for all silver halides in ammonia
    • It decreases, so AgCl is insoluble while AgI dissolves most readily
    • It decreases, so AgI is insoluble in ammonia while AgCl dissolves most readily

  16. Why is fluorine not used in school laboratory studies of the halogens?

    • It does not react with any halide ion, so it is of no interest in experiments
    • It is a liquid at room temperature, so it cannot be measured by volume
    • It is a noble gas, so it cannot take part in any reaction
    • It is too dangerous and reactive to handle safely in a school laboratory

  17. Which sodium halide gives sulfur-containing products such as H2S and S when heated with concentrated sulfuric acid?

    • Sodium iodide, because iodide is a strong reducing agent
    • Sodium fluoride, because fluoride is a strong reducing agent
    • Sodium chloride, because chloride is a strong reducing agent
    • Sodium bromide only, because bromide is the only halide that reduces sulfuric acid

  18. Which halogen is the most electronegative?

    • Iodine
    • Fluorine
    • Bromine
    • Chlorine

  19. Which halogen is the strongest oxidising agent?

    • Bromine
    • Fluorine
    • Iodine
    • Chlorine

  20. Why is acidified silver nitrate chosen to identify halide ions rather than an alternative reagent?

    • Silver nitrate turns the solution red whenever a halide is present, so the colour change identifies the halide ion
    • Silver nitrate is the only reagent that dissolves all halide ions completely, so it is used in every halide test
    • The silver halides have distinct colours and different solubilities in ammonia, which allow the halides to be distinguished
    • Silver nitrate reacts with the halide ions to release a gas that can be smelt, so the halides are identified by smell

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