Which type of bond typically involves a complete transfer of electrons?

An ionic bond is characterized by the complete transfer of electrons from one atom to another. This typically occurs between metals and nonmetals, where the metal, having a low electronegativity, loses one or more electrons, becoming a positively charged cation. In contrast, the nonmetal, possessing a higher electronegativity, gains those electrons, forming a negatively charged anion.

The resulting electrostatic attraction between these oppositely charged ions constitutes the ionic bond. This bond is distinct from covalent bonds, where electrons are shared between atoms, and hydrogen bonds, which are weak interactions involving hydrogen atoms bonded to electronegative elements. Metallic bonds, on the other hand, are characterized by a 'sea of electrons' that are shared among many metal atoms, but do not involve a complete transfer of electrons as seen in ionic bonding.