Final answer:
Metals are good conductors of heat and electricity due to their unique bonding called metallic bonding. In metallic bonding, the atoms in the metal lattice form a sea of delocalized electrons, which allows for the efficient transfer of heat and electricity.
Step-by-step explanation:
Metals are good conductors of heat and electricity due to their unique bonding called metallic bonding. In metallic bonding, the atoms in the metal lattice form a sea of delocalized electrons. These free electrons are not bound to any specific atom and can easily move throughout the structure. This free movement of electrons allows metals to conduct both heat and electricity effectively.
For example, when heat is applied to one end of a metal, the free electrons transfer their kinetic energy rapidly by colliding with neighboring electrons and atoms, thus spreading the heat throughout the material. Similarly, when an electric potential difference is applied across a metal, the free electrons move in response, carrying the electric charge and allowing electricity to flow.