Question

why is graphite a good conductor of electricity but diamond is not good conductor of electricity

Answer 1

Diamond: each carbon atom has a covalent bond with four other carbon atoms in a tetrahedral arrangement to form a rigid structure. This is a stable arrangement where the outer electron layer of all atoms are filled with 8 electrons; so, there are no free electrons to move and create electric current. Thus diamond is an insulator/dielectric.

Graphite: covalent structure, with each carbon bonded to three other carbon atoms in a hexagonal arrangement. Three out of four valence electrons are used for covalent bonding with other carbon atoms. Remaining valence electron can easily (with low energy) be moved across the planes of carbon atoms, making it easy to pass an electric current. Thus, graphite is a good conductor.

Answer 2

Graphite is a good conductor of electricity as it has a free electron structure while the diamond does not have this and hence, it can not conduct electricity.

Explanation:

• Graphite can conduct electricity as the electron structure it carries allows one valence electron of every atom to remain free.
• While the diamond comprises a covalent bond and therefore, no electron is free to allow the electricity to conduct. Thus, it doesn't contain any delocalized electrons.
• Hence, Graphite can conduct electricity while diamond can not.

Learn more: good conductor

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