Question

The hybridization present in $C{H}_4,C_2{H}_6,and{C}_2{H}_4$ are respectively:

• A. sp³, sp², sp²
• B. sp², sp², sp²
• C. sp³, sp³, sp²
• D. sp³, sp², sp

Answer 1

The correct option is C sp³, sp³, sp²

Let's take a look at the electronic configuration of carbon:

Now, in case of $C{H}_4$


Four $s{p}^3$ hybrid orbitals are formed,

Which will combine with four hydrogen atoms Hybridization $⟹$ $s{p}^3$ [One s-orbital Three p-orbitals]

Now, in case of $C_2{H}_6$ $⟹$
It is two $C{H}_3$ bonded together.
What is the bond between two carbon atoms?
Let’s take a look.


Four $s{p}^3$ hybrid orbitals are formed.

One $s{p}^3$ hybrid orbital will combine with $s{p}^3$ hybrid orbital of other carbon. (σ bond)
Three $s{p}^3$ hybrid orbitals will combine with three hydrogen for each carbon Hybridization $⟹$ $s{p}^3$ [ one s-orbital, three p-orbitals]

Now, in case of $C_2{H}_4$

Three $s{p}^2$ hybrid orbitals are formed.
In this case, what is the bond between two carbon atoms??
Let's take a look:

Three $s{p}^2$ hybrid orbitals are formed.

One orbital containing one electron will form $\pi$ bond with the other carbon atom.
Three $s{p}^2$ orbitals will form $\sigma$ bonds with hydrogen and $\sigma$ bond with the other carbon.
$⟹$ Therefore, there will be two bonds between two carbons (one $\sigma$ and one $\pi$)
Hybridization $⟹$ $s{p}^2$ [one s-orbital, two p-orbitals]

$C{H}_4$ $⟹$



$C_2{H}_6$ $⟹$


$C_2{H}_2$ $⟹$