In benzene, each carbon atom undergoes

Options

A. `sp` hybridisation
B. `sp^(2)` hybridisation
C. `sp^(3)` hybridisation
D. `sp^(2)` and `sp^(3)` hybridisation

Answer

To determine the hybridization of carbon atoms in benzene, we can follow these steps:

### Step 1: Understand the Structure of Benzene
Benzene (C6H6) is a cyclic compound consisting of six carbon atoms arranged in a ring, with alternating single and double bonds. Each carbon atom is bonded to one hydrogen atom.

### Step 2: Count the Sigma Bonds
Each carbon atom in benzene forms three sigma (σ) bonds:
1. One σ bond with another carbon atom.
2. One σ bond with another adjacent carbon atom.
3. One σ bond with a hydrogen atom.

### Step 3: Determine the Steric Number
The steric number (SN) can be calculated using the formula:
\[ \text{SN} = \text{Number of Sigma Bonds} + \text{Number of Lone Pairs} + \text{Charge} \]
In the case of benzene:
- Each carbon has 3 sigma bonds (as calculated in Step 2).
- There are no lone pairs on the carbon atoms.
- There is no charge on the carbon atoms.

Thus, the steric number for each carbon atom is:
\[ \text{SN} = 3 + 0 + 0 = 3 \]

### Step 4: Determine the Hybridization
Based on the steric number:
- If SN = 2, the hybridization is sp.
- If SN = 3, the hybridization is sp².
- If SN = 4, the hybridization is sp³.

Since the steric number for each carbon atom in benzene is 3, the hybridization of each carbon atom is sp².

### Step 5: Conclusion
All carbon atoms in benzene undergo sp² hybridization.

### Final Answer
Each carbon atom in benzene undergoes **sp² hybridization**.

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