Graphite is good conductor of electricity but diamond is non-conductor because

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graphite is composed of positively charged carbon ions

graphite has hexagonal layer structure with mobile π - electrons while diamond has continuous tetrahedral covalent structure with no free electrons

diamond is hard and graphite is soft

graphite and diamond have different atomic configuration

answer is D.

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Detailed Solution

→ In graphite each carbon atom undergoing sp² hydridisation and form hexagonal layer structure. The unhybridised P-electrons of adjacent carbon atom form mobile π-electron cloud and hence graphite acts as conductor
→ Where as in diamond the carbon undergoing sp³ hybridisation, and froms four bonds tetrahedrally with other 4-carbon atom. Hence here no unpaired electron in diamond to show conductivity

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