Question

The above bond between carbon atom $(1)$ and carbon atom $(2)$ in compound $HN = C - CH - C{H_2}$ involves the hybrid as:
(A) sp² and sp²
(B) sp³ and sp
(C) sp and sp²
(D) sp and sp

Answer 1

Hint: Here in this question, we have to find the hybridization of the first and second carbon of the given equation above. As we all know that by calculating the sigma and pi bond of the carbons we can easily find the hybridization of the above carbon atoms.

Complete step by step solution:
As we mentioned above, how we have to find the hybridization of the above carbon atoms,
The equation by which we have to find the hybridization of the carbon atom is,
$HN = C - CH - C{H_2}$
As we get detail from the above equation, we get the detail of the hybridization as,
First carbon’s Hybridization is $s{p^2}$ , as per the calculations of sigma and pi bonds.
Second carbon’s Hybridization is $s{p^2}$.
As in the above hybridization calculation we get both carbon’s hybridization as $s{p^2}$ . As from which we can easily justify the answer from the above options.
Therefore, the correct answer for the hybridization of the carbon atoms is sp² and sp²

Hence, the correct option is (A)

Note: In order to create a degraded new form of orbitals with the same energy levels, two atomic orbitals are mixed in a process known as hybridization. The foundation for this mixing is quantum mechanics. Linear, trigonal planar, tetrahedral, trigonal bipyramidal, and octahedral are the five fundamental hybridization shapes.