What type of bond is characterized by the sharing of electrons between nonmetals?

The correct answer is a covalent bond, which is defined by the sharing of electrons between two nonmetal atoms. In a covalent bond, each atom contributes one or more of its electrons to form a mutual bond that holds them together in a stable arrangement. This process allows both atoms to attain a full outer electron shell, which is typically associated with greater stability.

Covalent bonds are commonly found in molecules formed between nonmetals, such as hydrogen (H), oxygen (O), and carbon (C), which often share electrons to achieve the electronic configuration similar to that of noble gases. This sharing can involve single, double, or even triple bonds, depending on how many pairs of electrons the atoms share.

In contrast, ionic bonds involve the transfer of electrons from one atom to another, typically between metals and nonmetals, resulting in the formation of charged ions that attract one another. Metallic bonds are characterized by a "sea of electrons" that are delocalized over a lattice of metal cations, and hydrogen bonds are not typical bonds between atoms but rather weak attractions between a hydrogen atom bonded to an electronegative atom and another electronegative atom.