Ionic bonding occurs between metal and non-metal atoms. In this type of bonding, electrons are transferred from the metal atom to the non-metal atom. This transfer creates positive and negative ions, which are held together by the electrostatic force of attraction.

For example, let's consider the compound sodium chloride (NaCl). Sodium (Na) has one valence electron, while chlorine (Cl) requires one more electron to complete its outer shell. Sodium easily donates its valence electron to chlorine, forming a positively charged sodium ion (Na+) and a negatively charged chloride ion (Cl-). The opposite charges of these ions attract each other, resulting in the formation of the ionic bond in sodium chloride.

Ionic compounds typically have high melting and boiling points due to the strong electrostatic forces between the ions. They also tend to be soluble in water and conduct electricity when dissolved or melted.