Lesson 4.2.2.3

4.2.2.3 Properties of ionic compounds Quiz: AQA Chemistry, Unit 2

20 questions

Written by Revision Ninja · Last reviewed 11 October 2026

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Lesson 4.2.2.3, Properties of ionic compounds: 20 multiple choice questions for the AQA GCSE Chemistry (8462), Unit 2: Bonding, structure, and the properties of matter, written with Revision Ninja.

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The 20 questions

  1. What structural arrangement is found in ionic compounds?

    • Metallic matrix
    • Simple molecular
    • Giant covalent
    • Giant ionic lattice

  2. Ionic compounds have which melting point?

    • High
    • Zero
    • Equal to ice
    • Very low

  3. Why do ionic compounds have exceptionally high melting points?

    • Strong electrostatic bonds
    • Weak intermolecular forces
    • Free electrons
    • Small molecular size

  4. When do ionic compounds conduct electricity?

    • When frozen cold
    • Only when solid
    • As pure gases
    • Melted or dissolved

  5. Why do molten ionic compounds conduct electricity?

    • Covalent bonds snap
    • Electrons are delocalised
    • Molecules break apart
    • Ions can move

  6. Why do solid ionic compounds fail to conduct electricity?

    • Ions are fixed
    • Bonds are weak
    • No atoms present
    • They lack charge

  7. What forces hold ions together in a giant ionic lattice?

    • Shared electrons
    • Electrostatic forces
    • Metallic bonding
    • Weak intermolecular

  8. Why do ionic compounds have high melting points?

    • Strong ionic bonds
    • Weak intermolecular forces
    • Low atomic mass
    • Free moving electrons

  9. What happens when an ionic compound dissolves in water?

    • Covalent bonds break
    • Ions separate
    • Molecules evaporate
    • Atoms become neutral

  10. What happens when an ionic compound is melted or dissolved in water?

    • Forms covalent bonds
    • Conducts electricity
    • Breaks into atoms
    • Does not melt

  11. What type of forces exist between oppositely charged ions in a lattice?

    • Electrostatic forces
    • Covalent bonds
    • Intermolecular forces
    • Metallic bonds

  12. Which compound is the specified example of an ionic structure?

    • Diamond
    • Sodium chloride
    • Iron
    • Methane

  13. What is required regarding specific structures of ionic compounds other than sodium chloride?

    • Memorise all lattices
    • Calculate mass ratios
    • Draw exact angles
    • Not required

  14. Why do aqueous ionic solutions conduct electricity?

    • Covalent bonds break
    • Water provides electrons
    • Ions move freely
    • Molecules carry charge

  15. Which compound would be expected to conduct when dissolved?

    • Potassium bromide
    • Methane
    • Water
    • Carbon dioxide

  16. What state are ionic compounds usually in at room temperature?

    • Plasma
    • Gas
    • Solid
    • Liquid

  17. Why must an ionic compound be melted or dissolved to conduct?

    • Ions must move
    • Atoms must shrink
    • Electrons must bond
    • Molecules must form

  18. What does electrical conduction in a liquid ionic compound prove?

    • Ions are mobile
    • Atoms have neutralised
    • Molecules are present
    • Covalent bonds exist

  19. Which property is caused by strong bonds throughout an ionic lattice?

    • Low density
    • Low melting point
    • High boiling point
    • Solubility in oil

  20. Why do ionic solids need more energy to melt than molecular gases?

    • More valence electrons
    • Strong ionic bonds
    • Weak intermolecular forces
    • Larger atomic radius

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