Lesson 4.2.2.7

4.2.2.7 Properties of metals and alloys Quiz: AQA Chemistry, Unit 2

20 questions

Written by Revision Ninja · Last reviewed 11 October 2026

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Lesson 4.2.2.7, Properties of metals and alloys: 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 type of bonding holds the atoms together in a pure metal?

    • Hydrogen bonding
    • Covalent bonding
    • Ionic bonding
    • Metallic bonding

  2. Why do most metals have high melting and boiling points?

    • Mobile protons
    • Weak intermolecular forces
    • Simple molecular structure
    • Strong metallic bonds

  3. How are atoms arranged in pure metals to allow shaping?

    • Random networks
    • Fixed molecules
    • In layers
    • Rigid lattices

  4. Why are pure metals often mixed with other elements?

    • Too dense
    • Too soft
    • Too unreactive
    • Too brittle

  5. What is an alloy defined as?

    • A covalent compound
    • An ionic crystal
    • A metal mixture
    • A pure element

  6. Why are alloys harder than pure metals?

    • Layers slide easily
    • Layers distorted
    • Atoms become smaller
    • Bonds become weaker

  7. Which feature of pure metals allows them to be bent easily?

    • Sliding layers
    • Strong molecules
    • Rigid bonds
    • Fixed atoms

  8. What holds atoms together in a giant metallic structure?

    • Covalent bonds
    • Ionic bonds
    • Intermolecular forces
    • Metallic bonds

  9. Which change makes a pure metal harder?

    • Heating the metal
    • Stretching the lattice
    • Purifying the metal
    • Adding different atoms

  10. How are atoms structured in a pure metal?

    • Isolated pairs
    • Molecules
    • Layers
    • Random chains

  11. Which feature allows pure metals to be malleable?

    • Random atoms
    • Layers of atoms
    • Fixed molecules
    • Rigid network

  12. Why is bronze harder than pure copper?

    • Bonds are weaker
    • Layers slide freely
    • Molecules are smaller
    • Atoms distort layers

  13. Are metals usually giant structures or simple molecules?

    • Simple molecules
    • Giant covalent networks
    • Giant structures
    • Small ionic clusters

  14. What type of bonding explains a metal's high melting point?

    • Simple covalent
    • Hydrogen bonds
    • Metallic bonds
    • Weak electrostatic

  15. Why can a pure metal be shaped without breaking?

    • Layers slide
    • Ions repel
    • Bonds snap
    • Atoms melt

  16. Which subatomic particle is delocalized within a metallic lattice structure?

    • Nucleus
    • Electron
    • Neutron
    • Proton

  17. What best describes the structure of a pure metal?

    • Isolated molecules
    • Hexagonal rings
    • Layers of atoms
    • Random lattice

  18. Which two properties make metals useful for electrical wires?

    • Conductivity and malleability
    • Brittleness and density
    • Hardness and opacity
    • Insulation and strength

  19. What structural feature allows pure metals to be hammered into shape?

    • Fixed molecular chains
    • Strong ionic forces
    • Rigid covalent bonds
    • Layers of atoms

  20. Why are pure metals typically soft?

    • Weak covalent bonds
    • Layers slide easily
    • Ions are fixed
    • Molecules are small

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