Question

Consider following statement:
(I) In diamond, each carbon atom is linked tetrahedrally to four other carbon atoms by $s{p}^3$ bonds.
(II) Graphite has planar hexagonal layers of carbon atoms held together by weak vander walls forces.
(III) Silicon exists only in diamond structure due to its tendency to form $p\pi -p\pi$ bonds to itself.

Choose the correct option.

• A. Only I and II are correct
• B. Only I is correct
• C. Only II and III are correct
• D. All are correct statement

Answer 1

The correct option is D All are correct statement

Diamond: Carbon is $s{p}^3$ hybridised. Carbon is tetrahedrally linked to 4 neighbouring carbon atoms through 4 strong bonds between them as $s{p}^3$ bonds.

Graphite: Carbon is $s{p}^2$ hybridised. Each carbon is linked to 3 other creations forming hexagonal rings. So, It has 2-D 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 diamond cubic structure and form $p\pi -p\pi$ bonds with itself in $s{p}^3$ hybridization.