Here's why:

* Metallic Bonding: In metallic bonding, the valence electrons of the metal atoms are delocalized, meaning they are not bound to any specific atom but rather form a "sea" of electrons that move freely throughout the entire metal structure. This creates a strong electrostatic attraction between the positively charged metal ions and the negatively charged electron cloud, holding the metal together.

* Copper's Properties: Copper's excellent electrical conductivity and malleability (the ability to be hammered into different shapes) are direct results of its metallic bonding. The free-flowing electrons allow for easy electrical current transmission, while the delocalized nature of the electrons allows the metal atoms to slide past each other without breaking the bond.

Let me know if you have any other questions!