Which of the following is the correct statement for hybridization of C-atom and number of and II bonds in the Carbonyl group?

The correct option is:
$\begin{array}{c}s{p}^2,3\sigma ,1\pi \end{array}$

Step-by-Step Explanation:

1. Structure of the Carbonyl Group:
A carbonyl group consists of a carbon atom double-bonded to an oxygen atom:
C=O
The carbon atom in the carbonyl group is also bonded to two other atoms or groups (such as hydrogen or alkyl groups, represented by R), forming a planar arrangement:
R₂C=O

2. Determining the Hybridization of the Carbon Atom:
To determine the hybridization of the carbonyl carbon, we calculate its steric number (number of sigma (σ) bonds + number of lone pairs on the carbon atom):
• Number of single/sigma (σ) bonds formed by carbon = 3 (one σ-bond with oxygen, and two σ-bonds with the other two groups/atoms).
• Number of lone pairs on carbon = 0.
Steric Number = 3 + 0 = 3.
A steric number of 3 corresponds to sp² hybridization, resulting in a trigonal planar geometry around the carbon atom with bond angles of approximately 120°.

3. Counting the Number of Sigma (σ) and Pi (π) Bonds:
Let's analyze the bonding of the carbon atom in the carbonyl group:
• There are two single bonds connecting carbon to the other two substituent groups (R). Each single bond is a sigma (σ) bond (2 σ-bonds).
• There is a double bond connecting carbon to the oxygen atom (C=O). A double bond always consists of exactly one sigma (σ) bond and one pi (π) bond.
• Adding these up:
Total σ-bonds = 2 (with substituents) + 1 (with oxygen) = 3 σ-bonds.
Total π-bonds = 1 (with oxygen) = 1 π-bond.

Therefore, the carbon atom in a carbonyl group is sp² hybridized and contains 3 σ-bonds and 1 π-bond.