What is a metallic bond?

A metallic bond is characterized by the attraction between positively charged metal ions and the electrons that are delocalized around them. In metallic bonding, metal atoms release some of their electrons, which are not bound to any particular atom and can move freely throughout the metal structure. This creates a 'sea of electrons' that allows the metal to conduct electricity and heat efficiently. The electrostatic attraction between the positively charged metal ions and this sea of electrons is what holds the metal together, giving metals their unique properties such as malleability, ductility, and conductivity.

The other options do not accurately define metallic bonding. The sharing of electrons pertains to covalent bonding, while the attraction between charged particles relates more closely to ionic bonding. Options suggesting ionic interactions are also focused on different mechanisms of bonding that do not apply to metallic bonds, which distinctly rely on the movement of delocalized electrons surrounding cations.