What defines a covalent bond?

A covalent bond is defined by the sharing of a pair of electrons between two atoms. This type of bond occurs when two nonmetals come together, allowing each atom to attain a more stable electron configuration. By sharing electrons, each atom can effectively increase the number of electrons in their outer shell, which often leads to fulfillment of the octet rule for stability.

In contrast, the transfer of electrons from one atom to another is characteristic of ionic bonding, where one atom donates electrons and another accepts them, resulting in the formation of charged ions. The formation of charged ions involves electron transfer and does not accurately describe the nature of a covalent bond. Additionally, electrostatic attraction without electron sharing refers to ionic interactions, again differing from the essence of covalent bonding.

Understanding that covalent bonds are about the mutual sharing of electrons helps to distinguish them from other types of chemical bonds and emphasizes the nature of molecular formation in covalent compounds.