When ions form through the transfer of electrons, what type of bond is created?

When ions form through the transfer of electrons, an ionic bond is created. In this process, one atom donates electrons and becomes a positively charged ion (cation), while another atom accepts those electrons and becomes a negatively charged ion (anion). The electrostatic attraction between these oppositely charged ions leads to the formation of an ionic bond.

This type of bonding typically occurs between metals and non-metals, where the metal loses electrons easily and the non-metal gains them, resulting in a stable electron configuration for both ions. Ionic bonds are characterized by their strength and high melting and boiling points, which are indicative of the strong forces holding the ionic compounds together in a crystal lattice structure.

In contrast, covalent bonds involve the sharing of electrons between atoms, resulting in a different kind of molecular stability. Hydrogen bonds are weaker interactions that depend on partial charges and are important in biological systems, while metallic bonds involve the sharing of free electrons among a lattice of metal cations, giving rise to properties such as conductivity and malleability.