What is ionic bonding?

Ionic bonding is characterized by one atom transferring one or more electrons to another atom, resulting in the formation of charged ions. When an atom loses an electron, it becomes a positively charged ion (cation), and when another atom gains that electron, it becomes a negatively charged ion (anion). The electrostatic attraction between these oppositely charged ions creates a strong bond known as an ionic bond.

This process typically occurs between a metal and a non-metal, where the metal tends to lose electrons while the non-metal tends to gain them, facilitating the formation of stable ionic compounds. The solid lattice structure formed by these ions in ionic compounds also contributes to their high melting and boiling points.

In contrast, a bond formed between two metals would generally be metallic bonding, which involves the sharing of a "sea of electrons" rather than the transfer of charge. Bonds characterized by the sharing of electrons are described as covalent bonds, wherein two non-metals share electron pairs. Also, bonding does not have to occur exclusively in liquid states; ionic bonds typically form in solid states at room temperature and can also exist in molten or aqueous states.