What characterizes ionic bonds?

Ionic bonds are characterized by the attraction between oppositely charged ions. This occurs when one atom donates an electron to another, resulting in the formation of cations (positively charged ions) and anions (negatively charged ions). The electrostatic force of attraction between these oppositely charged ions creates a strong bond, which is a defining feature of ionic compounds.

In ionic bonding, the transfer of electrons leads to the formation of stable electron configurations for both atoms involved, typically resembling the electron configurations of noble gases. This process differs fundamentally from covalent bonding, where atoms share electron pairs. The nature of ionic bonds also influences properties such as high melting and boiling points, as well as the ability of ionic compounds to conduct electricity when dissolved in water or molten. These characteristics distinguish ionic bonds clearly from other bonding types.