Graphite is a good conductor of electricity. It is because of its

linear structure

tetrahedral structure

triangular planar structure

hexagonal multilayer structure

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This question was previously asked in

UPSC CISF-AC-EXE – 2018

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Graphite is a good conductor of electricity because of its structure. It consists of layers of carbon atoms arranged in a hexagonal lattice. Within each layer, carbon atoms are bonded covalently, with each carbon atom bonded to three others. This $sp^2$ hybridization leaves one unhybridized p-orbital per carbon atom, which overlaps with adjacent p-orbitals to form a delocalized pi electron system across the entire layer. These delocalized electrons are mobile and can carry electric charge, making the layers conductive. The overall structure is described as hexagonal multilayer, which creates the environment for these delocalized electrons.

The electrical conductivity of graphite is due to the presence of delocalized electrons in its layered hexagonal structure.

The layers in graphite are weakly bonded by Van der Waals forces, allowing them to slide easily, which is why graphite is soft and used as a lubricant. This contrasts with diamond, which has a rigid tetrahedral structure with all valence electrons localized in sigma bonds, making it an electrical insulator.

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