What characterizes an ionic bond?

An ionic bond is characterized by the attraction between charged ions, which typically occurs when one atom donates an electron to another, resulting in the formation of oppositely charged ions. This transfer of electrons leads to one atom becoming positively charged (cation) and the other negatively charged (anion). The electrostatic force of attraction between these charges holds the ions together.

This definition aligns with many common examples of ionic bonds, such as that found in sodium chloride (table salt), where sodium donates an electron to chlorine, creating Na⁺ and Cl⁻ ions that are attracted to each other. The key aspect of ionic bonds is this transfer and resultant attraction of charged ions, distinguishing it from other types of bonds such as covalent bonds, where electrons are shared rather than transferred.

The other options do not accurately define an ionic bond. Sharing electrons defines covalent bonds, specifying particular elements or compounds does not encompass the broad nature of ionic bonding, and the mention of organic compounds does not pertain to the fundamental characteristics of ionic bonds.