Some require such high temperatures that they decompose before they can reach a melting and/or boiling point. It is this that causes ionic solids to have such high melting and boiling points. A lot of energy is released as the oppositely charged ions interact. However, the crystalline structure allows each ion to interact with multiple oppositely charge ions, which causes a highly favorable change in the enthalpy of the system. Some might expect such an ordered structure to be less stable because the entropy of the system would be low. Lattice Energy is used to explain the stability of ionic solids. Its values are usually expressed with the units kJ/mol. As implied in the definition, this process will always be exothermic, and thus the value for lattice energy will be negative. The other definition says that lattice energy is the reverse process, meaning it is the energy released when gaseous ions bind to form an ionic solid. This definition causes the value for the lattice energy to always be positive, since this will always be an endothermic reaction. In one definition, the lattice energy is the energy required to break apart an ionic solid and convert its component atoms into gaseous ions. Lattice Energy is a type of potential energy that may be defined in two ways.

Born haber cycle of cacl2