Lesson 3.1.3.4

3.1.3.4 Bonding and physical properties Quiz: AQA Chemistry, Unit 1

20 questions

Written by Revision Ninja · Last reviewed 11 October 2026

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Lesson 3.1.3.4, Bonding and physical properties: 20 multiple choice questions for the AQA Chemistry (7405), Unit 1: Physical chemistry, written with Revision Ninja.

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The 20 questions

  1. Which of these is NOT one of the four types of crystal structure in the specification?

    • Metallic
    • Ionic
    • Molecular
    • Ceramic

  2. Which crystal structure does diamond have?

    • Macromolecular (giant covalent)
    • Ionic lattice of charged ions
    • Metallic lattice of positive ions
    • Molecular, held together by weak forces

  3. Which of these is an example of a molecular structure?

    • Iodine
    • Sodium chloride
    • Magnesium
    • Diamond

  4. Which solid has a giant covalent structure and conducts electricity?

    • Iodine
    • Ice
    • Graphite
    • Diamond

  5. Which crystal structure does sodium chloride have?

    • Macromolecular
    • Molecular
    • Metallic
    • Ionic

  6. Why does ice have a lower density than liquid water?

    • Hydrogen bonds hold the molecules further apart in an open hexagonal lattice
    • Ice contains dissolved gases that expand the solid when the water freezes into ice
    • Ice contains more protons than liquid water, which makes its molecules repel more strongly
    • Ice has covalent bonds that expand as the solid forms, pushing the molecules further apart

  7. Which substance has a high melting point and conducts electricity in the solid state?

    • Solid sodium chloride
    • Iodine
    • Magnesium
    • Diamond

  8. Why does diamond have a very high melting point?

    • Many strong covalent bonds must be broken throughout the giant lattice
    • Diamond has ionic bonds between carbon atoms that need little energy to break apart
    • Diamond has weak van der Waals forces between atoms that are easily broken on heating
    • Diamond contains delocalised electrons that repel each other strongly on heating the solid

  9. Why does graphite conduct electricity?

    • Each carbon has a delocalised electron that can move between the layers
    • Graphite's layers are held together by metallic bonds, which allow electrons to flow
    • Graphite contains free ions that move through the solid when a voltage is applied to it
    • Graphite has no bonds between atoms, so electrons can move freely through its structure

  10. Why does iodine have a low melting point even though its covalent bonds are strong?

    • Melting releases delocalised electrons from the iodine atoms, which then move freely through the solid
    • Melting converts iodine into an ionic lattice, which then holds the atoms together much more strongly than before
    • Melting only overcomes the weak intermolecular forces between molecules, not the covalent bonds within each I2 molecule
    • Melting breaks the covalent bonds, which are weak in iodine and easily broken by a small input of heat

  11. When iodine sublimes, which energy change is involved?

    • Energy is released as iodine turns to gas, which is why iodine feels cold when it sublimes
    • No energy is involved in sublimation, because the molecules simply drift apart in the gas
    • Energy must be supplied to overcome the intermolecular forces between iodine molecules
    • Covalent bonds within I2 molecules must be broken before the iodine can turn into a gas

  12. Which description best fits an ice crystal?

    • Metallic, with delocalised electrons
    • Macromolecular, with covalent bonds throughout
    • Ionic, with a lattice of H+ and O2- ions
    • Molecular, with hydrogen bonds between molecules

  13. Solid magnesium conducts electricity but solid sodium chloride does not. Why?

    • In magnesium, delocalised electrons are free to move, but in solid NaCl the ions are fixed in the lattice
    • Magnesium is a molecular substance, so its electrons are free to flow between neighbouring molecules
    • Magnesium contains covalent bonds that allow electrons to conduct through the solid metal sample
    • NaCl has delocalised electrons that cannot move because they are locked into fixed positions

  14. Why do molten ionic compounds conduct electricity?

    • Electrons are delocalised in the melt
    • The ions are free to move and carry charge
    • Molecules move freely to carry current
    • Protons are released when the compound melts

  15. Which substance has the highest melting point: NaCl at 801 C, iodine at 114 C or diamond above 3500 C?

    • All three have similar melting points because they all involve comparable bonding in solids
    • NaCl, because its small ions pack tightly, so the lattice needs a great deal of energy
    • Iodine, because its molecules are large and need a great deal of energy to be separated
    • Diamond, because breaking covalent bonds throughout the giant lattice needs the most energy

  16. Why is graphite soft even though its covalent bonds within the layers are strong?

    • Graphite has ionic bonds that are weak
    • Graphite contains delocalised electrons that dissolve
    • Graphite molecules are small, so they melt easily
    • Layers are held by weak forces, so they can slide over each other

  17. A solid is hard, has a very high melting point and does not conduct electricity as a solid or as a liquid. Which structure is most likely?

    • Metallic lattice of positive ions
    • Molecular, held together by weak forces
    • Ionic lattice of oppositely charged ions
    • Macromolecular (giant covalent)

  18. Which set of properties is expected of a simple molecular substance such as iodine?

    • Malleable with conduction when solid
    • Low melting point and no conduction of electricity as a solid
    • High melting point and conduction when dissolved in water
    • Very high melting point and conduction when solid

  19. Which statement correctly relates structure to electrical conductivity?

    • Conduction needs charged particles free to move, such as delocalised electrons or mobile ions
    • Macromolecular structures always conduct electricity, because their covalent bonds carry current through them
    • Ionic solids conduct when solid because the ions are free to move through the rigid lattice
    • Only molecular substances conduct electricity, because their molecules carry free electrons across

  20. Which of these is a giant metallic structure?

    • Iodine
    • Ice
    • Graphite
    • Magnesium

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