Which of the following best defines an ionic bond?

An ionic bond is characterized by the attraction between positively charged ions (cations) and negatively charged ions (anions). This type of bond typically forms when an atom with low ionization energy, usually a metal, transfers its electrons to an atom with high electronegativity, generally a nonmetal. As a result, the metal atom becomes positively charged, and the nonmetal atom becomes negatively charged, leading to a strong electrostatic force of attraction between these oppositely charged ions. This interaction is what constitutes an ionic bond.

The other options do not adequately describe an ionic bond. For instance, weak attractions between polar molecules refer to dipole-dipole interactions or hydrogen bonds, neither of which involves the transfer of electrons or the formation of charged ions. The strong covalent interactions mentioned involve the sharing of electron pairs between nonmetals, which is fundamentally different from the electron transfer in ionic bonding. Finally, the sharing of electrons between atoms pertains to covalent bonds rather than ionic bonds, as these bonds do not result in the formation of charged particles.