Question:

Hybridised states of carbon in Graphite and Diamond are respectively

Updated On: Apr 2, 2024
  • $sp^3,sp^3$
  • $sp^3,sp^2$
  • $sp^2,sp^2$
  • $sp^2,sp^3$
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The Correct Option is D

Solution and Explanation

In graphite, carbon is $s p^{2}$ hybridised. Each carbon is thus linked to three other carbon atoms forming hexagonal rings. On the other hand, in diamond carbon is $sp ^{3}$ hybridised. Each carbon is tetrahedrally linked to four strong $C - C$, $s p^{3}-s p^{3} \sigma$ -bonds.
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Concepts Used:

P-Block Elements

  • P block elements are those in which the last electron enters any of the three p-orbitals of their respective shells. Since a p-subshell has three degenerate p-orbitals each of which can accommodate two electrons, therefore in all there are six groups of p-block elements.
  • P block elements are shiny and usually a good conductor of electricity and heat as they have a tendency to lose an electron. You will find some amazing properties of elements in a P-block element like gallium. It’s a metal that can melt in the palm of your hand. Silicon is also one of the most important metalloids of the p-block group as it is an important component of glass.

P block elements consist of: