Metallic bonds are the type of chemical bonds that hold metal atoms together. In this bonding model, metal atoms release some of their valence electrons, which become delocalized—meaning they are not bound to any specific atom. These free electrons form a “sea of electrons” that moves freely throughout the metal structure.
This shared pool of electrons creates a strong electrostatic attraction between the positively charged metal ions and the surrounding electrons, binding the atoms together in a lattice.
Metallic bonding gives metals their characteristic properties:
- High electrical and thermal conductivity (due to free-moving electrons)
- Malleability and ductility (layers of atoms can slide without breaking the bond)
- Luster or shine (electrons reflect light)
- High melting and boiling points
This unique bonding is what allows metals like copper, iron, and gold to be so useful in construction, electronics, and machinery.