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Question

Consider the following statements:
I: In diamond, each carbon atom is linked tetrahedrally to four other carbon atoms by sp3 bonds.
II: Graphite has planar hexagonal layers of carbon atoms held together by weak van der Waal's forces.
III: Silicon exists only in diamond structure due to its tendency to form pπpπ bonds to itself.


In this:

A
only I and II are correct.
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B
only I is correct
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C
only II and III are correct.
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D
all the above are correct statement
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Solution

The correct option is D only I and II are correct.
Diamond: C is sp3 hybridised. C is tetrahedrally linked to 4 neighbouring C atoms through 4 strong bonds between them as sp3 bonds. It extends in 3D and give rise to 3D structure. It is very rigid. It is used as gems in making abrasive. Since all the electrons firmly held so it do not conduct electricity as no 'free electron' is present.

Graphite: C is sp2 hybridised. Each C is linked to 3 other creations forming hexagonal rings. So, it has 2D sheet-like structure. The various sheets are held by Van der Waal's force of attraction. The layers can slip over the other.

Silicon: It exists in different kinds of structures based on its bonding atoms.

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