Which of the following best describes a metallic bond?

A metallic bond is best described as the attraction between delocalized electrons and positive metal ions. In metallic bonding, metal atoms release some of their electrons, which become delocalized and can move freely throughout the metal structure. This creates a "sea of electrons" that are not attached to any specific atom, allowing for electrical conductivity and malleability, which are characteristic properties of metals.

The positive metal ions, which are formed when the atoms lose electrons, create a lattice structure that the delocalized electrons surround. This cohesive interaction between the mobile electrons and the fixed positive ions explains many of the physical properties of metals, such as strength and ductility. The presence of these delocalized electrons is crucial in understanding how metals exhibit their unique properties compared to other types of bonding, such as ionic or covalent bonds.