How are ions formed during ionic bonding?

Ions are formed during ionic bonding primarily through the complete transfer of electrons from one atom to another. In ionic bonds, typically, one atom (often a metal) donates one or more electrons, resulting in a positively charged ion known as a cation. The other atom (often a nonmetal) receives those electrons and becomes a negatively charged ion known as an anion. This transfer creates an electrostatic attraction between the oppositely charged ions, resulting in the formation of an ionic compound.

The concept of transferring electrons is crucial in understanding how ionic bonds differ from covalent bonds, where electrons are shared between atoms. In the case of ionic bonding, the significant difference lies in this transfer mechanism, leading to the formation of distinct ions with opposite charges. This transfer and subsequent attraction are responsible for the properties associated with ionic compounds, such as high melting points and electrical conductivity when dissolved in water.