What is metallic bonding?

Metallic bonding is characterized by the electrostatic attraction between positively charged metal ions and a 'sea' of delocalized electrons. In metallic structures, metal atoms release some of their electrons, which move freely throughout the structure, creating a network of positive ions surrounded by this cloud of delocalized electrons. This arrangement is what gives metals their unique properties, such as electrical conductivity, malleability, and ductility.

The presence of these delocalized electrons allows metals to conduct electricity well, as the electrons are free to move in response to an electric field. Additionally, the strong attraction between the positive ions and the free electrons holds the metal structure together, which contributes to its strength and ability to deform without breaking.

The other options do not accurately describe metallic bonding. For instance, the attraction between ions and nonmetals refers to ionic bonding, while the sharing of electrons pertains to covalent bonding. Likewise, the formation of ionic bonds involves the transfer of electrons from metals to nonmetals, which distinctly differs from the behavior of electrons in metallic bonding.