A metallic bond is a type of chemical bond that holds metal atoms together. In this bond, the atoms of a metal release some of their outer (valence) electrons, which do not remain attached to any single atom. Instead, these electrons move freely throughout the entire structure of the metal, forming what is called a “sea of delocalized electrons.”
The positive metal ions (cations) are arranged in a regular pattern, and the freely moving electrons act like a glue that holds the lattice together. This unique bonding explains many important properties of metals:
- Electrical conductivity: Since the electrons are free to move, metals conduct electricity easily.
- Thermal conductivity: The free electrons transfer heat energy efficiently.
- Malleability and ductility: The layers of metal ions can slide over one another without breaking the bond, making metals easy to shape or stretch.
- Luster (shininess): The free electrons reflect light, giving metals their characteristic shine.
- High melting and boiling points: The strong attraction between metal ions and delocalized electrons makes metallic bonds very strong.
In short, a metallic bond is the electrostatic attraction between positive metal ions and the sea of delocalized electrons surrounding them.