Lesson 3.1.3.7

3.1.3.7 Forces between molecules Quiz: AQA Chemistry, Unit 1

20 questions

Written by Revision Ninja · Last reviewed 11 October 2026

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Lesson 3.1.3.7, Forces between molecules: 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 three types of intermolecular force are named in the specification?

    • Permanent dipole-dipole, induced dipole-dipole and hydrogen bonding
    • Ionic, covalent and metallic
    • Dative, single and double
    • Van der Waals forces only

  2. Which intermolecular force is present between all molecules?

    • Permanent dipole-dipole
    • Hydrogen bonding
    • Induced dipole-dipole
    • Ionic bonding

  3. Hydrogen bonding occurs between which atoms?

    • Two metal atoms
    • A hydrogen bonded to N, O or F and a lone pair on another N, O or F
    • A hydrogen bonded to carbon and a lone pair on carbon
    • Any two polar molecules

  4. Which molecule shows hydrogen bonding?

    • CH3OCH3
    • CH3Cl
    • CH3CH3
    • CH3CH2OH

  5. Which is the strongest of the intermolecular forces listed?

    • Hydrogen bonding
    • Induced dipole-dipole
    • London forces
    • Permanent dipole-dipole

  6. What mainly determines the strength of induced dipole-dipole forces?

    • The presence of ionic bonds
    • The number of protons in the nucleus only
    • The melting point of the solid
    • The number of electrons and the surface area of the molecule

  7. Why does bromine, Br2, have a higher boiling point than chlorine, Cl2?

    • Br2 has stronger covalent bonds
    • Cl2 has more lone pairs
    • Br2 forms hydrogen bonds
    • Br2 has more electrons, so it has stronger induced dipole-dipole forces

  8. Why does H2O have a higher boiling point than H2S?

    • Water is an ionic compound
    • Water has stronger covalent bonds
    • Water forms hydrogen bonds, whereas H2S has only weaker dipole-dipole forces
    • H2S has more electrons

  9. Why does HF have a higher boiling point than HCl?

    • HF is an ionic compound
    • HF forms hydrogen bonds, which are stronger than the dipole-dipole forces in HCl
    • HF has a higher relative molecular mass than HCl
    • HF has no lone pairs

  10. Which substance has the highest boiling point: propane, butane or butan-1-ol?

    • Butane
    • All would be equal
    • Butan-1-ol
    • Propane

  11. Why does pentane have a higher boiling point than 2,2-dimethylpropane?

    • Branching increases the strength of intermolecular forces
    • Pentane's longer chain gives a larger surface area for London forces
    • 2,2-dimethylpropane has more hydrogen bonds
    • They are equal because they have the same number of carbon atoms

  12. Which molecule has permanent dipole-dipole forces but no hydrogen bonding?

    • H2O
    • NH3
    • CH3CH2OH
    • HCl

  13. Which is the strongest intermolecular force in ammonia, NH3?

    • Hydrogen bonding
    • Metallic bonding
    • Ionic bonding
    • Induced dipole-dipole only

  14. Why is the boiling point of methane, CH4, very low?

    • It has delocalised electrons
    • It has hydrogen bonds between molecules
    • Only weak induced dipole-dipole forces act between small non-polar molecules
    • It has ionic bonds between molecules

  15. Which statement correctly compares ethanal and propane, which both have Mr 44?

    • Propane has higher boiling point because it has no electrons
    • Ethanal has higher boiling point because it has permanent dipole-dipole forces as well as London forces
    • Propane has higher boiling point because it has more C-H bonds
    • They have equal boiling points because their Mr is the same

  16. Why does NH3 have an unusually high boiling point compared with PH3?

    • NH3 forms hydrogen bonds, whereas PH3 has only weaker dipole-dipole forces
    • PH3 has hydrogen bonding
    • NH3 is heavier than PH3
    • PH3 is an ionic compound

  17. Which statement about London forces is correct?

    • They only exist between polar molecules
    • They are covalent bonds between molecules
    • They are stronger than hydrogen bonds
    • They arise from temporary uneven electron distribution and exist between all molecules

  18. Which molecule has the highest boiling point: CH3F, CH3Cl, CH3Br or CH3I?

    • CH3I
    • CH3F
    • CH3Br
    • CH3Cl

  19. Why do alkanes have higher boiling points as chain length increases?

    • Longer chains have more hydrogen bonds
    • Longer chains have more electrons and larger surface area, so stronger London forces
    • Longer chains have fewer electrons
    • Longer chains have more ionic bonds

  20. A student claims that water's high boiling point is due to its O-H covalent bonds breaking on boiling. Is this correct?

    • No, water has no intermolecular forces
    • Yes, ionic bonds in water break on boiling
    • No, boiling overcomes the hydrogen bonds between molecules, not the O-H covalent bonds
    • Yes, the O-H covalent bonds break on boiling

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