Graphite is a much better conductor of heat and electricity than diamond. This is due to the fact that each carbon atom in graphite:
undergoes sp² hybridization and forms three sigma bonds with three neighbouring carbon atoms
undergoes sp³ hybridization
is tetrahedrally bonded
is free from van der Waals force
Answer is Right!
Answer is Wrong!
This question was previously asked in
UPSC NDA-2 – 2015
Graphite’s structure consists of layers of carbon atoms arranged in hexagonal lattices. Each carbon atom in graphite is sp² hybridized and forms three strong sigma bonds with three adjacent carbon atoms within the same layer. The remaining unhybridized p-orbital on each carbon atom overlaps sideways with p-orbitals of neighbouring atoms, forming a delocalized pi electron system across the layer. These delocalized electrons are free to move within the layers, making graphite a good conductor of heat and electricity.