Which type of bond is characterized by the transfer of electrons from one atom to another?

The ionic bond is characterized by the transfer of electrons from one atom to another. In an ionic bond, one atom, typically a metal, donates one or more of its electrons to another atom, usually a nonmetal. This process creates positively charged ions (cations) and negatively charged ions (anions). The electrostatic attraction between these oppositely charged ions forms a strong bond that holds the compounds together.

This transfer of electrons leads to the formation of stable electron configurations for both the donating and receiving atoms, often resulting in the formation of compounds with distinct properties, such as high melting and boiling points, and the ability to conduct electricity when dissolved in water or melted.

Understanding that other types of bonds do not involve this transfer of electrons is important as it clarifies why they do not fit this description. For example, covalent bonds involve the sharing of electrons between atoms rather than their transfer, while metallic bonds involve a "sea of electrons" shared collectively among metal atoms. Hydrogen bonds, on the other hand, are weak attractions between polarized molecules or within different parts of a single molecule and do not involve any transfer of electrons.