Use the Born–Haber cycle and data from Appendix IIB and Table 9.3 to calculate the lattice energy of CaO. (ΔH_sub for calcium is 178 kJ/mol; IE₁ and IE₂ for calcium are 590 kJ/mol and 1145 kJ/mol, respectively; EA₁ and EA₂ for O are -141 kJ/mol and 744 kJ/mol, respectively.)

The Born-Haber cycle is a thermodynamic cycle that relates the lattice energy of an ionic compound to other thermodynamic quantities. It involves a series of steps, including the sublimation of the metal, ionization energy, electron affinity, and the formation of the ionic solid from its gaseous ions. This cycle allows for the calculation of lattice energy by applying Hess's law, which states that the total enthalpy change is the sum of the changes in each step.

Lattice energy is the energy released when gaseous ions combine to form an ionic solid, or the energy required to separate one mole of an ionic solid into its gaseous ions. It is a measure of the strength of the forces between the ions in an ionic compound. Higher lattice energy indicates stronger ionic bonds, which typically results in higher melting points and greater stability of the compound.

Ionization energy is the energy required to remove an electron from an atom or ion in the gas phase, while electron affinity is the energy change that occurs when an electron is added to a neutral atom in the gas phase. These concepts are crucial in the Born-Haber cycle as they help quantify the energy changes associated with forming cations and anions, which are essential for calculating the overall lattice energy of ionic compounds like CaO.