Covalent compounds are poor conductors of electricity because they do not contain free-moving charged particles, such as ions or delocalized electrons, which are necessary for electrical conduction. In covalent compounds, electrons are shared between atoms rather than being free to move throughout the material. Therefore, covalent compounds do not conduct electricity well.
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Covalent compounds are generally poor conductors of electricity because they lack free-moving charged particles. In covalent compounds, electrons are shared between atoms to form molecules, and the electrons are localized within the bonds. Unlike ionic or metallic compounds where charged particles (ions or delocalized electrons) can move freely, covalent compounds do not have mobile charges. As a result, they do not conduct electricity well in either solid or liquid states. Exceptions include certain covalent compounds that ionize or dissociate in solution, forming ions that can conduct electricity, but this behavior is less common compared to ionic or metallic substances.