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The hybridisation states of carbon in diamond and graphite are, respectively:

1. sp³ and sp³
2. sp² and sp²
3. sp² and sp³
4. sp³ and sp²

Correct answer: sp³ and sp²

Solution

Diamond: Each carbon atom is bonded to 4 other carbon atoms in a tetrahedral arrangement with no pi bonds. This corresponds to sp³ hybridisation (like methane). Graphite: Each carbon atom is bonded to 3 neighbouring carbons in a planar hexagonal network. Three sp² orbitals form sigma bonds; the remaining unhybridised p orbital participates in delocalised pi bonding across the layer. This is sp² hybridisation.

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