Lattice energy

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Lattice energy deals primarily with metals. The lattice energy, or lattice enthalpy, of an ionic solid is a measure of the strength of bonds in that ionic compound. It is given the symbol U and is equivalent to the amount of energy required to separate a solid ionic compound into gaseous ions.Lattice energy can also be considered as the energy given off when gaseous ions form an ionic solid. It is dependent on ionic charge and the ionic radius: as the charge of the ions increases the lattice energy increases (becomes more negative), and as the radius decreases (the ions in the ionic solid are closer together) the lattice energy increases.

It cannot be determined directly but can be by using experimental data in the Born Haber cycle and from theoretical calculations.

Lattice energy is the energy change when an ionic compound is separated into its gaseous ions. It is given in units of kilojoules per mole. For example, when solid sodium chloride is separated into gaseous sodium and chlorine ions ( $\text{NaCl (s)} \to \text{Na}^+ \text{(g)} + \text{Cl}^- \text{(g)}$ ), the lattice energy is -786 kJ/mol.

Born-Mayer and Kapustinskii equations can also be used.

Lattice energy is usually calculated by using the Born-Haber cycle.

Lattice energy, the potential energy of two interacting ions (taken as two point charges), can also be calculated by using a modified version of Coulomb's law: $E = k\cdot \frac{q_1q_2}{d}$ , where $k=8.99 \cdot 10^9 \text{J-m}/\text{C}^2$ , $d$ is the distance between the centers of the ions, and $q 1, q 2$ are the charges on the ions.^[1]