Which one of the following statements is not correct?

Which one of the following statements is not correct?

All carbons in diamond are linked by carbon-carbon single bond.

Graphite is layered structure in which layers are held together by weak van der Waals forces.

Graphite layers are formed by hexagonal rings of carbon atoms.

Graphite layers are held together by carbon-carbon single bond.

Answer is Right!

Answer is Wrong!

This question was previously asked in

UPSC NDA-2 – 2018

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The statement that graphite layers are held together by carbon-carbon single bonds is incorrect. Graphite layers (graphene sheets) are themselves held together by covalent bonds within the plane, but the forces *between* these layers are weak van der Waals forces.

– Diamond has a 3D tetrahedral structure where each carbon atom is covalently bonded to four other carbon atoms by single bonds (sp³ hybridization).
– Graphite has a layered structure. Each layer consists of carbon atoms arranged in hexagonal rings, with strong covalent bonds (sp² hybridization) within the layer.
– The layers in graphite are held together by relatively weak van der Waals forces. This allows the layers to slide easily over each other, giving graphite its properties as a lubricant and its softness.

The delocalized electrons within the layers of graphite allow it to conduct electricity, unlike diamond, which is an electrical insulator. The carbon-carbon bond length within a graphite layer is about 0.142 nm, while the distance between layers is about 0.335 nm.

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