Illustrated are four ions — A, B, X, and Y— showing their relative ionic radii. The ions shown in red carry positive charges: a 2+ charge for A and a 1+ charge for B. Ions shown in blue carry negative charges: a 1- charge for X and a 2- charge for Y. (b) Among the combinations in part (a), which leads to the ionic compound having the largest lattice energy?

Key Concepts

Ionic Radius

Ionic radius refers to the size of an ion in a crystal lattice. Cations (positively charged ions) are generally smaller than their parent atoms due to the loss of electrons, which reduces electron-electron repulsion. Conversely, anions (negatively charged ions) are larger because they gain electrons, increasing repulsion among them. Understanding ionic radii is crucial for predicting the stability and properties of ionic compounds.

Lattice Energy

Lattice energy is the energy released when gaseous ions combine to form an ionic solid. It is a measure of the strength of the forces between the ions in an ionic compound. Larger charges and smaller ionic radii typically result in higher lattice energy, as the electrostatic attraction between oppositely charged ions increases. This concept is essential for determining the stability and solubility of ionic compounds.

Charge Density

Charge density is defined as the charge of an ion divided by its volume, which is influenced by its ionic radius. Higher charge density indicates a stronger electrostatic attraction between ions, leading to greater lattice energy. In the context of ionic compounds, ions with higher charges and smaller radii will have higher charge densities, significantly affecting the overall stability and properties of the resulting compound.