Why are the valance electrons of metallic bonds different from other bonds?

Answer 1

• In a metal the valence electrons delocalize into the conduction band, becoming an "electron gas" that fills the metal's bulk volume.
• In covalent bonds the valence electrons are shared between local pairs of atoms.
• In ionic bonds the valence electrons leave the "metal" and move to the "nonmetal" creating a pair of separate oppositely charged ions.
• In resonance bonds the valence electrons oscillate between being shared between two nearby local pairs of atoms.
• etc.

To summarize in metals the valence electrons become delocalized, in other bonds the valence electrons stay local.

Answer 2

Valence electrons in metallic bonds are not localized between specific atoms but are free to move throughout the metal lattice, leading to properties such as high electrical conductivity and malleability. In contrast, valence electrons in other bonds are typically shared between specific atoms, leading to the formation of distinct molecules or structures.