What type of bonds are formed in metallic bonding?

In metallic bonding, the primary feature is the presence of a "sea of electrons," which allows for the formation of metallic bonds. In this type of bonding, metal atoms collectively share their delocalized electrons, creating a strong attraction between positively charged metal ions and this electron sea. This delocalization not only enhances conductivity but also contributes to the malleability and ductility found in metals.

Unlike ionic and covalent bonds, which involve the transfer or sharing of electrons between specific atoms, metallic bonds embody a communal sharing of electrons that enables a network of metal ions to move relative to one another without breaking the bond. This characteristic is essential for explaining many physical properties of metals, such as their ability to conduct electricity and heat, and their shiny luster.

Understanding metallic bonds also highlights the differences with other types of bonding, helping to clarify why options like ionic, covalent, and hydrogen bonds are not suitable in this context. Each of these other bond types involves more localized interactions between specific pairs of atoms rather than the collective lattice structure seen in metallic bonding.