why is graphite good conductor of electricity but not diamond
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Graphite can conduct electricity because of the delocalised (free) electrons in its structure. These arise because each carbon atom is only bonded to 3 other carbon atoms. ... However, in diamond, all 4 outer electrons on each carbon atom are used in covalent bonding, so there are no delocalised electrons.
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In a graphite molecule, one valence electron of each carbon atom remains free , Therefore graphite gained a name of a good conductor of electricity. Whereas in diamond, they have no free mobile electron.
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