What type of bond involves the sharing of electron pairs between atoms?

A covalent bond involves the sharing of electron pairs between atoms. This type of bond occurs when two nonmetal atoms come together, and instead of completely transferring electrons as seen in ionic bonds, they share one or more pairs of electrons. This sharing allows each atom to attain a full outer electron shell, achieving greater stability.

In a covalent bond, the strength of the bond is determined by the amount of shared electron pairs; for example, a single bond involves one pair of shared electrons, while double and triple bonds involve two and three pairs, respectively. This sharing of electrons creates a strong bond between the atoms, characteristic of many molecules such as water (H₂O) and carbon dioxide (CO₂).

The other types of bonds, while important in their own contexts, do not involve the sharing of electron pairs in the same manner. Ionic bonds involve the transfer of electrons from one atom to another, forming charged ions. Hydrogen bonds are a form of weak attraction that occurs between a hydrogen atom bonded to a highly electronegative atom and another electronegative atom. Metallic bonds involve a 'sea of electrons' that are shared among a lattice of metal atoms rather than being shared in specific pairs between two atoms.