Why is bond order of graphite more than that of diamond??
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But Diamond has more bond power than Graphite
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In diamond each carbon is joined to other four carbon tetrahedrally and carbon-carbon bond length is 1.54A° and bond angle is 109°28' having sp3 hybridisation on each carbon. All four eletrons in carbon are involved in bonding hence, it is bad conductor of heat and electricity.
Each carbon is sp3 hybridrised. It has layered structure. These layers are attracted by Van dar Walls force. Each carbon has one free electron in p-orbital, so it is a good conductor of electricity. All eleteons get delocalized in one layer and form π-bond. Elctron jumps from one orbital to another hence it is a good conductor of heat and electricity. In graphite carbon-carbon bond length is 141.5 pm and distance between adjacent graphite layer is 340 pm.
Hope it will help you .
Each carbon is sp3 hybridrised. It has layered structure. These layers are attracted by Van dar Walls force. Each carbon has one free electron in p-orbital, so it is a good conductor of electricity. All eleteons get delocalized in one layer and form π-bond. Elctron jumps from one orbital to another hence it is a good conductor of heat and electricity. In graphite carbon-carbon bond length is 141.5 pm and distance between adjacent graphite layer is 340 pm.
Hope it will help you .
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