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. What is the definition of lattice enthalpy, in the sense of lattice formation?

    • The energy change when one mole of gaseous atoms is formed from a solid element
    • The energy change when one mole of a solid ionic compound is dissolved in water
    • The energy change when one mole of gaseous ions is hydrated by water molecules
    • The energy change when one mole of a solid ionic compound is formed from its gaseous ions

  2. What is the enthalpy of atomisation of an element?

    • The energy change when one mole of the element is dissolved in water
    • The energy change when one mole of gaseous atoms gains one electron each
    • The energy change when one mole of the element is formed from its gaseous ions
    • The energy change when one mole of gaseous atoms is formed from the element in its standard state

  3. What is the first ionisation energy of an element?

    • The energy needed to form one mole of gaseous ions from the solid element
    • The energy released when one mole of gaseous atoms gains one electron
    • The energy needed to remove one electron from each atom in one mole of gaseous atoms
    • The energy needed to break one mole of bonds in a diatomic molecule

  4. What is the first electron affinity of an element?

    • The energy change when one mole of solid element is converted to gaseous atoms
    • The energy change when one mole of gaseous 1- ions loses one electron each
    • The energy change when one mole of gaseous ions is surrounded by water molecules
    • The energy change when one mole of gaseous atoms gains one electron each to form 1- ions

  5. What is the enthalpy of hydration of an ion?

    • The energy change when one mole of solid compound dissolves in water to make a saturated solution
    • The energy change when one mole of water is formed from hydrogen and oxygen
    • The energy change when one mole of gaseous ions is surrounded by water molecules
    • The energy change when one mole of gaseous atoms gains one electron each

  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. A Born-Haber calculation for an ionic compound gives a lattice enthalpy less exothermic than the value from a perfect ionic model. What does this suggest?

    • The bonding has some covalent character, so the perfect ionic model overestimates the lattice enthalpy
    • The ions are more strongly hydrated than the perfect model predicts, so less energy is released
    • The compound is metallic, because metals have lower lattice enthalpies than ionic solids
    • The bonding is purely ionic, and the perfect ionic model underestimates the lattice enthalpy

  12. Which property of ions gives the most exothermic lattice enthalpy of formation?

    • Small ionic radius and low charge, which give low charge density
    • Large ionic radius and high charge, which give high charge density
    • Large ionic radius and low charge, which give low charge density
    • Small ionic radius and high charge, which give high charge density

  13. Which compound has the more exothermic lattice enthalpy of formation, and why?

    • NaCl, because Mg2+ has a lower charge than Na+, so its ions are less strongly held together than sodium ions are
    • NaCl, because Na+ and Cl- are smaller than Mg2+ and O2-, so their ions are packed more tightly in the lattice
    • NaCl, because Na+ has a higher charge than Mg2+, so its ions attract each other more strongly in the lattice
    • MgO, because Mg2+ and O2- are more highly charged and smaller than Na+ and Cl-

  14. Why is the second electron affinity of oxygen endothermic?

    • The second electron removes a proton from the oxide ion, which requires energy
    • The second electron is added to a neutral atom, which releases energy only if it is filled
    • The second electron is added to a negative ion, so it must overcome electrostatic repulsion
    • The second electron is shared by two oxygen atoms, which requires energy to break a bond

  15. Which pair of values shows that LiF has a more exothermic lattice enthalpy than NaF?

    • Li+ and Na+ have the same radius, so the lattice enthalpies are equal in size
    • Li+ is more highly charged than Na+, which reduces the lattice enthalpy
    • Li+ is larger than Na+, so its charge density is lower and the lattice is more strongly held
    • Li+ is smaller than Na+, so its charge density is higher and the lattice is more strongly held

  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 Born-Haber step is an enthalpy of formation for the element and not a lattice term?

    • The formation of the element in its standard state from the element, as in delta Hf
    • The conversion of gaseous ions into a solid lattice, which releases the energy that the cycle is designed to measure
    • The addition of one electron to each gaseous atom to form an anion, which always absorbs energy in every cycle
    • The removal of one electron from each gaseous atom to form a cation, which always absorbs energy in every cycle

  18. Which statement about the first electron affinity of chlorine, -349 kJ/mol, is correct?

    • Energy is absorbed when one mole of gaseous chlorine atoms gains one electron each
    • Energy is absorbed when one mole of solid chlorine is converted to gaseous atoms
    • Energy is released when one mole of chloride ions loses one electron each
    • Energy is released when one mole of gaseous chlorine atoms gains one electron each

  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 the second ionisation energy of an element always larger than its first ionisation energy?

    • The second electron is removed from a neutral atom, which has more protons than the first
    • The second electron is removed from an atom that has gained a proton from the solvent
    • The second electron is removed from a positive ion, so it is held more strongly than the first
    • The second electron is in a higher energy shell, which is always more easily removed

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