What are the factors affecting lattice energy in ionic compounds?

The factors affecting lattice energy in ionic compounds are the charge on the ions and the size of the ions.

Lattice energy is the energy required to break apart an ionic compound into its individual ions. It is a measure of the strength of the forces between the ions in an ionic compound. The greater the lattice energy, the stronger the forces between the ions and the more stable the compound.

The charge on the ions is one of the key factors affecting lattice energy. The greater the charge on the ions, the stronger the electrostatic forces between them, and hence the greater the lattice energy. For example, an ionic compound made up of ions with charges of +2 and -2 will have a greater lattice energy than a compound made up of ions with charges of +1 and -1. This is because the electrostatic forces between ions with charges of +2 and -2 are stronger than those between ions with charges of +1 and -1.

The size of the ions also affects the lattice energy. Smaller ions are able to get closer together than larger ions, resulting in stronger electrostatic forces and hence a greater lattice energy. For example, an ionic compound made up of small ions will have a greater lattice energy than a compound made up of larger ions. This is because the smaller ions can get closer together, resulting in stronger electrostatic forces.

In summary, the lattice energy of an ionic compound is affected by the charge on the ions and the size of the ions. The greater the charge and the smaller the ions, the greater the lattice energy. This is because these factors result in stronger electrostatic forces between the ions, making the compound more stable.