What is an ionic bond?

An ionic bond is characterized by the transfer of electrons from one atom to another, resulting in the formation of ions. In this process, one atom donates electrons, becoming a positively charged cation, while the other atom accepts those electrons, becoming a negatively charged anion. The electrostatic attraction between these oppositely charged ions creates a strong ionic bond.

This type of bond typically occurs between elements with significantly different electronegativities, such as metals and nonmetals. For instance, sodium (a metal) can transfer one electron to chlorine (a nonmetal), leading to the formation of sodium ions (Na⁺) and chloride ions (Cl⁻), which bond together as sodium chloride (table salt).

The other answer choices suggest different types of bonding: sharing electrons describes covalent bonds, molecular interactions refer to weak attractions like van der Waals forces, and minute interactions between atoms could point towards intermolecular forces, which differ fundamentally from the strong ionic bonds formed through electron transfer. Therefore, recognizing that ionic bonds specifically arise from electron transfer clarifies why this choice is correct.