Lesson 3.1.8.1

3.1.8.1 Born–Haber cycles Quiz: AQA Chemistry, Unit 1

20 questions

Written by Revision Ninja · Last reviewed 11 October 2026

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Lesson 3.1.8.1, Born–Haber cycles: 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 enthalpy change forms one mole of a solid ionic lattice from its gaseous ions?

    • Enthalpy of atomisation
    • Lattice dissociation enthalpy
    • Enthalpy of solution
    • Lattice formation enthalpy

  2. Which enthalpy change forms one mole of gaseous atoms from an element in its standard state?

    • Lattice dissociation enthalpy
    • First ionisation energy
    • Bond dissociation enthalpy
    • Enthalpy of atomisation

  3. Which enthalpy change removes one mole of electrons from one mole of gaseous atoms?

    • Enthalpy of atomisation
    • First electron affinity
    • First ionisation energy
    • Lattice formation enthalpy

  4. Which enthalpy change adds one mole of electrons to one mole of gaseous atoms?

    • Enthalpy of atomisation
    • First ionisation energy
    • Enthalpy of hydration
    • First electron affinity

  5. Which enthalpy change dissolves one mole of gaseous ions in water to form aqueous ions?

    • Enthalpy of solution
    • Lattice dissociation enthalpy
    • Enthalpy of hydration
    • Enthalpy of atomisation

  6. For NaCl, delta Hf = -411 kJ/mol, enthalpy of atomisation of Na = +107 kJ/mol, first ionisation energy of Na = +496 kJ/mol, enthalpy of atomisation of 1/2 Cl2 = +122 kJ/mol, and first electron affinity of Cl = -349 kJ/mol. What is the lattice enthalpy of formation of NaCl?

    • -787 kJ/mol
    • +787 kJ/mol
    • -411 kJ/mol
    • -376 kJ/mol

  7. Using the same NaCl data (atomisation of Na +107, ionisation energy +496, atomisation of 1/2 Cl2 +122, electron affinity -349 kJ/mol), what is the sum of these four enthalpy changes?

    • +411 kJ/mol
    • +787 kJ/mol
    • -376 kJ/mol
    • +376 kJ/mol

  8. A Born-Haber cycle for KCl uses delta Hf = -437, atomisation of K = +89, first ionisation energy of K = +419, atomisation of 1/2 Cl2 = +122 and electron affinity of Cl = -349, all in kJ/mol. What is the lattice formation enthalpy?

    • +718 kJ/mol
    • -718 kJ/mol
    • -437 kJ/mol
    • -281 kJ/mol

  9. The bond enthalpy of Cl2 is 242 kJ/mol. In a Born-Haber cycle, what is the enthalpy of atomisation of 1/2 Cl2?

    • 61 kJ/mol
    • 121 kJ/mol
    • 484 kJ/mol
    • 242 kJ/mol

  10. Using a Born-Haber cycle with delta Hf(CaF2) = -1219, atomisation of Ca = +178, IE1 = +590, IE2 = +1145, bond enthalpy of F2 = 158, electron affinity of F = -328 (per F atom), all in kJ/mol, what is the lattice formation enthalpy of CaF2?

    • -1415 kJ/mol
    • +2634 kJ/mol
    • -804 kJ/mol
    • -2634 kJ/mol

  11. What type of bonding character causes experimental lattice enthalpy to differ from theoretical ionic calculations?

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

  12. Which combination of ionic properties produces the most exothermic lattice enthalpy of formation?

    • Small, singly charged
    • Large, singly charged
    • Large, highly charged
    • Small, highly charged

  13. Which ionic compound has the most exothermic lattice enthalpy of formation?

    • Calcium oxide
    • Sodium chloride
    • Potassium chloride
    • Magnesium oxide

  14. What causes the second electron affinity of oxygen to be endothermic?

    • Electron shielding
    • Nuclear attraction
    • Electrostatic repulsion
    • Covalent bond formation

  15. Why is the lattice enthalpy of lithium fluoride more exothermic than sodium fluoride?

    • Higher lithium charge
    • Lower lithium charge
    • Larger lithium radius
    • Smaller lithium radius

  16. The standard enthalpy of solution of an ionic compound can be found from lattice enthalpy and hydration enthalpies. For NaCl with lattice dissociation enthalpy +787 kJ/mol and hydration enthalpies Na+ = -406 and Cl- = -364 kJ/mol, what is the enthalpy of solution?

    • -1153 kJ/mol
    • +1153 kJ/mol
    • +17 kJ/mol
    • -17 kJ/mol

  17. Which enthalpy change converts an element in its standard state into gaseous atoms?

    • Enthalpy of atomisation
    • Enthalpy of formation
    • Electron affinity
    • First ionisation energy

  18. What process corresponds to the first electron affinity of chlorine atoms?

    • Losing one electron
    • Atomising chlorine gas
    • Forming covalent bonds
    • Gaining one electron

  19. For NaCl, the lattice formation enthalpy is -787 kJ/mol. What is the lattice dissociation enthalpy of NaCl?

    • -787 kJ/mol
    • +411 kJ/mol
    • +787 kJ/mol
    • +376 kJ/mol

  20. Why is an element's second ionisation energy always greater than its first ionisation energy?

    • Lower electrostatic attraction
    • Decreased nuclear charge
    • Greater electrostatic attraction
    • Increased electron shielding

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