In graphite, each carbon atom is bonded to three other carbon atoms

[amp_mcq option1=”forming a three-dimensional structure” option2=”in the same plane giving a hexagonal array” option3=”in the same plane giving a square array” option4=”in the same plane giving a pentagonal array” correct=”option2″]

This question was previously asked in

UPSC CDS-2 – 2019

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Graphite has a layered structure. Within each layer, carbon atoms are arranged in a hexagonal lattice, where each carbon atom is covalently bonded to three other carbon atoms in the same plane. These layers are stacked on top of each other and held together by weak van der Waals forces.

Graphite has a layered structure with carbon atoms bonded hexagonally in flat planes.

This layered structure with weak interlayer forces explains graphite’s properties, such as its softness and lubricating ability, which contrast sharply with the hardness of diamond, where carbon atoms form a three-dimensional tetrahedral network.

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