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The correct response highlights that an ionic bond is characterized by the complete transfer of electrons from one atom to another. In this type of bond, one atom, typically a metal, donates one or more of its electrons to another atom, which is usually a nonmetal. This transfer results in the formation of charged ions: the donating atom becomes a positively charged cation, while the receiving atom becomes a negatively charged anion. The electrostatic attraction between these oppositely charged ions forms the ionic bond.

This process is crucial for the stability of many compounds, particularly salts, such as sodium chloride (table salt), where sodium donates an electron to chlorine, leading to the formation of Na+ and Cl- ions.

In contrast, covalent bonds involve the sharing of electrons between atoms rather than complete transfer. Hydrogen bonds are weaker attractions between polar molecules, and metallic bonds involve a sea of electrons that are shared among a lattice of metal atoms, allowing for conductivity and malleability, rather than a transfer of electrons. Understanding these differences is fundamental for grasping the various types of chemical bonding and their implications in molecular structure and reactivity.