How is ionic bonding characterized?

Ionic bonding is characterized by the transfer of electrons between atoms. In this type of bond, one atom (typically a metal) loses one or more electrons, becoming a positively charged ion (cation), while another atom (usually a nonmetal) gains those electrons, becoming a negatively charged ion (anion). This transfer results in an electrostatic attraction between the oppositely charged ions, leading to the formation of an ionic compound.

The process is fundamentally different from sharing electrons, which is characteristic of covalent bonding, where atoms bond by sharing pairs of electrons to achieve stability. Additionally, protons and neutrons do not play a role in ionic bonding as they are found in the nucleus of atoms and do not participate in the formation of bonds between atoms. Thus, focusing on the mechanism of electron transfer provides a clear understanding of how ionic bonds are formed and why this is the defining characteristic of ionic bonding.