What happens to the lattice enthalpy when a solid forms ions?

Lattice enthalpy is a measure of the strength of the forces between the ions in an ionic solid. When a solid ionic compound forms from its constituent ions, the lattice enthalpy reflects the energy released when the gaseous ions come together to form the solid structure.

The value of the lattice enthalpy is typically expressed as a positive quantity when considering the energy required to break the ionic solid apart into its gaseous ions. Conversely, it can be considered negative when we look at the formation of the solid from ions because energy is released when the solid forms.

Understanding that lattice enthalpy is indicative of the strength of attraction between the ions allows one to assess the stability of the ionic solid. Stronger attractions result in higher lattice enthalpy values, suggesting a more stable solid. This is integral in predicting behaviors such as solubility and melting points of ionic compounds.

Thus, saying that lattice enthalpy measures the strength of the solid encapsulates its role in understanding the stability and interactions within ionic compounds.