What type of bond is formed by the sharing of electron pairs between two atoms?

A covalent bond is formed when two atoms share electron pairs. This sharing allows each atom to attain a more stable electron configuration, similar to that of noble gases. The shared electrons help to hold the atoms together, resulting in the formation of a molecule. Covalent bonds can vary in strength and may involve single, double, or triple bonds, depending on the number of shared electron pairs.

In a covalent bond, the electronegativity of the atoms involved plays a crucial role in determining how equally the electrons are shared, leading to polar or nonpolar covalent bonds. This property is essential for understanding molecular structure and reactivity in chemistry.

The other types of bonds listed do not involve the sharing of electron pairs. Ionic bonds involve the transfer of electrons from one atom to another, resulting in charged ions that attract each other. Hydrogen bonds are relatively weak interactions that occur when a hydrogen atom covalently bonded to an electronegative atom is attracted to another electronegative atom. Metallic bonds involve the pooling of free electrons among a lattice of metal atoms, which allows for conductivity and malleability characteristic of metals.