Lesson 5.2.1

5.2.1 Lattice enthalpy Quiz: OCR Chemistry, Unit 4

20 questions

Written by Revision Ninja · Last reviewed 11 October 2026

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Lesson 5.2.1, Lattice enthalpy: 20 multiple choice questions for the OCR Chemistry (H432), Unit 4: Physical chemistry and transition elements, written with Revision Ninja.

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The 20 questions

  1. What product is formed in the definition of lattice enthalpy of formation?

    • Gaseous atoms
    • Solid ionic compound
    • Liquid compound
    • Aqueous ions

  2. What is the sign of lattice enthalpy for lattice formation from gaseous ions?

    • Zero
    • Negative
    • Variable
    • Positive

  3. How does increasing ionic charge affect the lattice enthalpy of an ionic compound?

    • Unchanged
    • Endothermic
    • More exothermic
    • Less exothermic

  4. How does decreasing ionic radius affect the lattice enthalpy of formation?

    • Less exothermic
    • Endothermic
    • Unchanged
    • More exothermic

  5. What is formed when gaseous ions dissolve in water during hydration?

    • Solid lattice
    • Liquid water
    • Aqueous ions
    • Gaseous molecules

  6. Which enthalpy change occurs when one mole of gaseous atoms gains electrons?

    • Hydration enthalpy
    • Electron affinity
    • Atomisation enthalpy
    • Ionisation energy

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

    • Enthalpy of atomisation
    • First ionisation energy
    • Lattice enthalpy
    • Electron affinity

  8. A Born-Haber cycle for NaCl uses these values in kJ mol^-1: enthalpy change of formation -411, atomisation of Na +107, first ionisation energy of Na +496, atomisation of 1/2 Cl2 +122, electron affinity of Cl -349. What is the lattice enthalpy?

    • -35 kJ mol^-1
    • -787 kJ mol^-1
    • +787 kJ mol^-1
    • -376 kJ mol^-1

  9. Using the Born-Haber route for MgCl2 with these values in kJ mol^-1: enthalpy change of formation -641, atomisation of Mg +147, first and second ionisation energies of Mg +738 and +1451, atomisation of 2 Cl +244, and 2 x electron affinity of Cl -698. What is the lattice enthalpy?

    • +2523 kJ mol^-1
    • -2523 kJ mol^-1
    • -1882 kJ mol^-1
    • -641 kJ mol^-1

  10. For NaCl, the enthalpy change of solution is +4 kJ mol^-1 and the lattice enthalpy is -787 kJ mol^-1. What is the total enthalpy change of hydration of the gaseous ions?

    • +791 kJ mol^-1
    • -4 kJ mol^-1
    • -783 kJ mol^-1
    • -791 kJ mol^-1

  11. Which compound has the more exothermic lattice enthalpy, MgO or NaF?

    • MgS
    • NaF
    • NaCl
    • MgO

  12. Which ion has a more exothermic enthalpy change of hydration, Mg2+ or Ca2+?

    • Ba2+
    • Mg2+
    • Ca2+
    • Sr2+

  13. What does a more exothermic lattice enthalpy indicate about ionic bonding strength?

    • Weaker ionic bonding
    • Stronger ionic bonding
    • Lower ionic charge
    • Greater solubility

  14. What is the total enthalpy change when completing a full Born-Haber cycle?

    • Variable
    • Zero
    • Negative
    • Positive

  15. Which electron affinity step in a Born-Haber cycle is always endothermic?

    • Zero electron affinity
    • Second electron affinity
    • Third electron affinity
    • First electron affinity

  16. Why does an experimental lattice enthalpy differ from a purely ionic theoretical model?

    • Isotope presence
    • Partial covalent character
    • Nuclear shielding
    • Pure ionic bonding

  17. Which ion property leads to a more exothermic lattice enthalpy for ions of equal charge?

    • Greater atomic mass
    • Lower charge density
    • Smaller ionic radius
    • Larger ionic radius

  18. Which force primarily determines the magnitude of a lattice enthalpy?

    • London dispersion forces
    • Dipole-dipole attraction
    • Electrostatic attraction
    • Covalent bonding

  19. Which enthalpy change converts gaseous ions directly into a solid ionic lattice?

    • Hydration enthalpy
    • Enthalpy of formation
    • Lattice enthalpy
    • Enthalpy of atomisation

  20. Which two enthalpy changes are summed to calculate the enthalpy of solution?

    • Combustion and neutralisation
    • Ionisation and affinity
    • Formation and atomisation
    • Lattice and hydration

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