* Electron Sharing: In covalent bonds, electrons are shared between atoms, forming a strong bond. These electrons are localized between the atoms, not free to move throughout the material.

* No Free Electrons: Unlike metallic bonds where electrons are delocalized and can move freely, covalent bonds lack free electrons to carry electrical current.

Exceptions:

While most covalent compounds are poor conductors, there are a few exceptions:

* Graphite: Graphite is a good conductor due to its unique structure. While the carbon atoms within each layer are held together by strong covalent bonds, the layers are held together by weak van der Waals forces. This allows electrons to move freely between the layers, making graphite a good conductor of electricity.

* Conductive Polymers: Some polymers with conjugated systems (alternating single and double bonds) can exhibit conductivity due to the delocalization of electrons along the chain.

In summary: Covalent bonds typically form materials that are poor conductors of electricity. However, specific structures, such as graphite and some conductive polymers, can exhibit conductivity.