In the diamond modification of solid carbon each atom is covalently bonded to ex
ID: 1854673 • Letter: I
Question
In the diamond modification of solid carbon each atom is covalently bonded to exactly four nearest neighbors that are configured in a tetrahedral pattern around it. In the graphite modification of carbon the carbon atoms form planar sheets that are relatively widely separated from one another. Each carbon atom is bonded to three near neighbors in the plane, and has a weak interaction with atoms in adjacent planes. Diamond is an electrical insulator and is one of the hardest substances known. Interpret these properties in terms of its bonding.Explanation / Answer
As In case of diamond 3-D network of covalent bond is present due to tetrahedral structure of C atom due to SP3 hybridization of C atom as a result of which it is the hardest substance in the nature... While in Graphite C atom is present in SP2 hybridization and planner structure or thin like sheets are formed which can overlap each other by applying external force As these thin sheets are bounded by week wander wall force of attraction so Graphite is soft in nature...