Metallic bonding is the bonding within metals. It involves the delocalized sharing of free electrons among a lattice of metal atoms. Thus, metallic bonds may be compared to molten salts.

Metal atoms typically contain a high number of electrons in their valence shell compared to their period or energy level. These become delocalized and form a Sea of Electrons surrounding a giant lattice of positive ions.

Metals seem to have higher boiling and melting points which might suggest stronger bonds between the atoms.

Metallic bonding is non-polar, in that there is no (for pure elemental metals) or very little (for alloys) electronegativity difference among the atoms participating in the bonding interaction, and the electrons involved in that interaction are delocalized across the crystalline structure of the metal.

The metallic bond accounts for many physical characteristics of metals, such as strength, malleability, ductility, conduction of heat and electricity, and lustre. See also chemical bond.

Metallic bonding is the electrostatic attraction between the metal atoms or ions and the delocalised electrons. This is why atoms or layers are allowed to slide past each other, resulting in the characteristic properties of malleability and ductility.

Metal atoms have at least one valence electron, they do not share these electrons with neighboring atoms, nor do they lose electrons to form ions. Instead the outer energy levels of the metal atoms overlap. They are like covalent bonds.

Kovová vazba | Metallische Bindung | Enlace metálico | Liaison métallique | Legame metallico | קשר מתכתי | 金属結合 | Metallbinding | Metallbinding | Wiązanie metaliczne | Kovová väzba | Metallisidos | พันธะโลหะ | Liên kết kim loại | 金属键