Lattice energy is the energy required to separate 1 mol of an ionic solid into gaseous ions. Lattice enthalpy and lattice energy are commonly used as if they mean exactly the same thing, although there is a difference between them which relates to the conditions under which they are calculated.

Lattice enthalpy (H) values are usually represented in kilojoules (KJ). Lattice enthalpy is usually applicable to ionic compounds, which are compounds formed by metals and non-metals. For example, if we say 'sodium chloride crystal lattice', we mean a regular geometrical pattern of sodium and chloride ions. The 3-dimensional arrangement of atoms or ions in a organised crystallin pattern within is referred as crystal lattice. In chemistry, when the term lattice is used, we usually refer to a crystal lattice which is a highly transparent substance with a regular geometric shape.

The Born-Haber cycle represents a series of steps leading to the formation of an ionic compound from its constituent gaseous ions.

Lattice enthalpy increases with the charges and decreases with the size of the ions.

Lattice energy is the energy required to separate 1 mol of an ionic solid into gaseous ions.

Lattice enthalpy is a measure of the strength of the forces between the ions in an ionic solid.

Born haber cycle problems pdf