* Atomic Structure: Metals have a unique structure where their outer electrons are loosely bound and can easily move freely throughout the material. These "free electrons" are responsible for conducting heat and electricity. Nonmetals, on the other hand, have tightly bound electrons that are localized to individual atoms.
* Bonding: Metals typically form metallic bonds, where electrons are shared in a sea of delocalized electrons. This allows for easy electron movement. Nonmetals form covalent bonds, where electrons are shared between specific atoms, hindering free electron movement.
Exceptions:
While most nonmetals are poor conductors, there are some exceptions:
* Graphite: A form of carbon, has a layered structure with free electrons within each layer, making it a good conductor of electricity.
* Silicon and Germanium: These metalloids are semiconductors, meaning they conduct electricity better than nonmetals but not as well as metals. Their conductivity can be manipulated by adding impurities, making them vital in electronics.
In Summary:
Nonmetals are generally poor conductors compared to metals due to their different atomic structure and bonding. While some nonmetals show exceptional conductivity, they are still far less conductive than metals overall.