Final answer:
Metallic bonding in metals allows for conductivity, malleability, and ductility due to the free-flowing electrons that prevent atoms from coming in contact.
Step-by-step explanation:
Metallic bonding is the electrostatic attraction between the positively charged atomic nuclei of metal atoms and the delocalised electrons in the metal. This bonding model explains the physical properties of metals.
Metals conduct electricity and heat very well because of their free-flowing electrons. When a force is applied to a metal, the free-flowing electrons can slip in between the stationary cations and prevent them from coming in contact, making metals malleable and ductile.