What characterizes metallic bonding?

Metallic bonding is characterized by the delocalization of electrons across a lattice structure formed by metal atoms. In metallic bonds, the outermost electrons of the metal atoms are not bound to any particular atom but instead are free to move throughout the entire metallic structure. This sea of delocalized electrons contributes to many of the distinctive properties of metals, such as electrical conductivity and malleability.

The presence of these delocalized electrons allows for the metallic lattice to maintain its integrity while enabling the atoms to slide over one another, which is what makes metals ductile and flexible. Therefore, the essence of metallic bonding lies in this sharing of electrons across the entire lattice rather than their localization or tight binding.