What is ionic bonding?

Ionic bonding is fundamentally characterized by the transfer of electrons between atoms. This process typically occurs between metals and nonmetals. In an ionic bond, the more electronegative nonmetal atom attracts one or more electrons from the metal atom, resulting in the formation of ions. The metal atom loses electrons and becomes a positively charged cation, while the nonmetal atom gains those electrons, transforming into a negatively charged anion.

The strong electrostatic forces between these oppositely charged ions create the ionic bond, leading to the formation of ionic compounds. This type of chemical bond is distinct from covalent bonding, where atoms share electrons, and from metallic bonding, where electrons are delocalized across a lattice of metal cations. Ionic bonds also differ from weak interactions, such as hydrogen bonds, which involve attractions between molecules rather than the formation of distinct ions. Thus, the transfer of electrons is the hallmark of ionic bonding, making it a fundamental concept in understanding the behavior of elements in the periodic table and the properties of various compounds.