Metals:
* Free Electrons: Metals have a "sea" of delocalized electrons that are not tightly bound to any particular atom. These electrons are free to move throughout the material, allowing for easy transport of electrical charge.
* Metallic Bonding: The atoms in metals are held together by a "sea" of delocalized electrons, which contribute to their high conductivity.
* High Electron Mobility: The free electrons in metals can move quickly and easily in response to an electric field, making them excellent conductors of electricity and heat.
Ceramics:
* Covalent Bonding: Ceramics are typically held together by strong covalent bonds, where electrons are shared between atoms. These bonds are localized, meaning the electrons are not free to move easily.
* Ionic Bonding: Some ceramics also have ionic bonds, where electrons are transferred between atoms, creating charged ions. This can further limit electron mobility.
* Limited Electron Mobility: The strong and localized bonding in ceramics restricts the movement of electrons, leading to poor conductivity.
In summary:
Metals have free-moving electrons due to their bonding structure, making them excellent conductors. Ceramics, with their strong and localized bonding, have limited electron mobility, resulting in poor conductivity.
