Metallic Bonding

Metallic bonding is the electrostatic attraction between positively charged metal ions and the delocalized electrons surrounding them, allowing metals to conduct electricity and heat.

Metals are typically malleable, ductile, good conductors of heat and electricity, and have a shiny appearance due to metallic bonding.

Delocalized electrons are free-moving electrons that contribute to the conductivity and malleability of metals, allowing them to deform without breaking.

Metallic bonding involves a sea of delocalized electrons, while ionic bonding involves the transfer of electrons between atoms, and covalent bonding involves the sharing of electrons.

The 'sea of electrons' model explains how metal atoms can lose their valence electrons, creating a pool of electrons that allows for conductivity and flexibility.

As temperature increases, metallic bonds can weaken, leading to increased malleability and ductility, but can also result in melting if the temperature is high enough.

Tungsten (W) is an example of a metal with strong metallic bonding, which contributes to its high melting point and strength.

The presence of delocalized electrons in metallic bonding allows metals to conduct electricity efficiently.

CuCl₂

Mn₂O₃