The carbon atom of the carbonyl group is :

Options

A. `sp^(2)` hybridized
B. `sp^(3)` hybridized
C. `sp` hybridized
D. `dsp^(2)` hybridized

Explanation

To determine the hybridization of the carbon atom in the carbonyl group, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Carbonyl Group**:
The carbonyl group is characterized by a carbon atom double-bonded to an oxygen atom (C=O).

2. **Determine the Bonding**:
In the carbonyl group, the carbon atom is involved in a double bond with oxygen. This double bond consists of one sigma (σ) bond and one pi (π) bond.

3. **Hybridization Concept**:
To find the hybridization of the carbon atom, we need to consider the types of bonds formed:
- A single bond (σ) involves sp³ hybridization.
- A double bond (σ + π) involves sp² hybridization.
- A triple bond (σ + 2π) involves sp hybridization.

4. **Analyze the Carbon Atom**:
Since the carbon atom in the carbonyl group forms a double bond with oxygen, it will have sp² hybridization. This is because one of the orbitals is used to form the sigma bond with oxygen, and the remaining two orbitals are involved in forming sigma bonds with other atoms or groups.

5. **Geometric Structure**:
The geometry around the carbon atom in the carbonyl group is trigonal planar due to the sp² hybridization. This means that the bond angles around the carbon atom are approximately 120 degrees.

6. **Conclusion**:
Therefore, the carbon atom of the carbonyl group is sp² hybridized.

### Final Answer:
The carbon atom of the carbonyl group is **sp² hybridized**.

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