Born-Haber cycles and lattice enthalpy Quiz
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5 questions, one answer each
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1. Which equation represents the enthalpy of lattice dissociation of NaCl?
- A. Na⁺(g) + Cl⁻(g) → NaCl(s)
- B. Na(s) + ½Cl₂(g) → NaCl(s)
- C. NaCl(s) → Na⁺(g) + Cl⁻(g)
- D. NaCl(s) → Na(s) + ½Cl₂(g)
2. Sodium bromide has ΔHf = −361, ΔHat(Na) = +107, IE1(Na) = +496, ΔHat(Br) = +112 and EA(Br) = −325, all in kJ mol⁻¹. What is the enthalpy of lattice formation of NaBr?
- A. −751 kJ mol⁻¹
- B. −361 kJ mol⁻¹
- C. +751 kJ mol⁻¹
- D. −1141 kJ mol⁻¹
3. The Born–Haber lattice enthalpy of a compound is considerably more exothermic than the value from the perfect ionic model. What does this suggest?
- A. The bonding is purely ionic
- B. The ions are perfect spheres
- C. The compound has no lattice
- D. The bonding has some covalent character
4. Which compound is predicted to have the most exothermic enthalpy of lattice formation?
- A. NaCl
- B. MgO
- C. KCl
- D. CaCl₂
5. In the Born–Haber cycle for calcium chloride, CaCl₂, which terms are doubled compared with the cycle for CaCl?
- A. The first ionisation energy of calcium
- B. The atomisation of calcium
- C. The atomisation and the electron affinity of chlorine
- D. The enthalpy of formation