Final answer:
The value of lattice enthalpy is primarily dependent on the ionic charges and internuclear distance, with additional influences from crystal structure, covalent character, and electron-electron interactions.
The Born-Haber cycle aids in calculating lattice energy indirectly and helps in evaluating other chemical properties.
Step-by-step explanation:
The value of the lattice enthalpy largely depends on the electrostatic attractions between the ions in the crystal lattice, which in turn depend on both the magnitude of the charges on the ions and the internuclear distance between them. As the ionic charges increase, the lattice energy typically increases;
likewise, as the internuclear distance decreases, the lattice energy also increases. Additional factors influencing lattice enthalpy include the crystal structure of the compound, the covalent character, and electron-electron interactions within the ionic solid. The way in which the ions are arranged in the solid lattice and their valence electron configurations are also relevant to determining the value.
Lattice energies are critical in determining the stability of an ionic compound, affecting properties such as melting points and hardness. These energies can be deduced using the Born-Haber cycle, a process which takes into account various thermochemical data to calculate the lattice energy indirectly.
The Born-Haber cycle is useful not only for determining the lattice energy, but also for evaluating related chemical properties which are otherwise difficult to measure.