What distinguishes an ionic bond from a covalent bond?

An ionic bond is characterized by the transfer of electrons from one atom to another, resulting in the formation of charged ions. This typically occurs between atoms with significantly different electronegativities, such as a metal and a non-metal. The metal atom loses one or more electrons, becoming a positively charged cation, while the non-metal atom gains these electrons, forming a negatively charged anion. This electrostatic attraction between the oppositely charged ions forms the ionic bond.

In contrast, a covalent bond is formed when two atoms share one or more pairs of electrons. This sharing allows each atom involved in the bond to attain a more stable electron configuration, achieving a full valence shell. Covalent bonding typically occurs between nonmetals with similar electronegativities, where neither atom completely transfers electrons but rather shares them to create a stable molecule.

Recognizing the distinct nature of electron transfer in ionic bonds versus electron sharing in covalent bonds is crucial in understanding the fundamental differences in chemical bonding and the resulting properties of ionic and covalent compounds.