* Delocalized electrons: In a metallic bond, the outermost electrons of the metal atoms are not held tightly to any one atom. Instead, they are free to move about the entire lattice of metal atoms. This sea of delocalized electrons is what gives metals their characteristic properties, such as high electrical and thermal conductivity.

* Positive metal ions: The metal atoms in a metallic bond lose their outermost electrons, leaving behind positively charged metal ions. These positive ions are held together by the electrostatic attraction of the negatively charged delocalized electrons.

* Close packing: The metal atoms in a metallic bond are packed very close together, so that their outermost electron orbitals overlap. This allows the electrons to move freely between the metal atoms, forming the metallic bond.

Some additional characteristics of metallic bonds include:

* High melting and boiling points: The strong metallic bond between metal atoms makes it difficult to separate them, which is why metals have high melting and boiling points.

* High electrical and thermal conductivity: The delocalized electrons in a metallic bond are very mobile, which allows them to carry electrical current and heat very effectively.

* Luster: The shiny appearance of metals is due to the reflection of light by the delocalized electrons.

* Malleability and ductility: The strong metallic bond between metal atoms makes metals malleable (able to be hammered into thin sheets) and ductile (able to be drawn into thin wires).

Metallic bonds are found in all metals, as well as in some alloys and intermetallic compounds.