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Ionic bonding is characterized by the transfer of electrons from one atom to another, leading to the formation of ions. In this type of bond, an atom with a relatively low electronegativity, typically a metal, loses one or more electrons, becoming positively charged (a cation). Meanwhile, an atom with a higher electronegativity, usually a nonmetal, gains these electrons, resulting in a negatively charged ion (an anion). The resulting electrostatic attraction between the positively and negatively charged ions forms a strong ionic bond, which is a fundamental aspect of ionic compounds.

This process contrasts with other types of bonding. For example, the sharing of electrons between atoms defines covalent bonding, which is not applicable in ionic bonding. Ionic bonds typically form between atoms with significant differences in electronegativity rather than those with similar values. Additionally, the mention of aqueous solutions and covalent compounds pertains to different interactions than those involved in ionic bonding.