Each carbon atom in benzene is in the state of hybridization

Options

A. `sp^(3)`
B. `sp^(2)`
C. `sp`
D. `s^(3) p`

Explanation

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

### Step-by-Step Solution:

1. **Identify the Structure of Benzene**:
- Benzene has the molecular formula C₆H₆ and consists of six carbon atoms arranged in a hexagonal ring. Each carbon atom is bonded to one hydrogen atom.

2. **Count the Bonds Around Each Carbon Atom**:
- In benzene, each carbon atom forms three sigma (σ) bonds: two with adjacent carbon atoms and one with a hydrogen atom. Additionally, there is one pi (π) bond formed due to the delocalization of electrons across the ring.

3. **Determine the Hybridization**:
- The hybridization of an atom can be determined by the number of sigma bonds and lone pairs around it. Each carbon atom in benzene has:
- 3 sigma bonds (2 with neighboring carbon atoms and 1 with hydrogen).
- No lone pairs.
- The hybridization can be calculated using the formula:
- Hybridization = Number of sigma bonds + Number of lone pairs.
- For each carbon atom in benzene:
- Hybridization = 3 sigma bonds + 0 lone pairs = 3.

4. **Identify the Type of Hybridization**:
- A hybridization state of 3 corresponds to sp² hybridization. This means that one s orbital and two p orbitals mix to form three equivalent sp² hybrid orbitals.

5. **Conclusion**:
- Therefore, each carbon atom in benzene is sp² hybridized.

### Final Answer:
Each carbon atom in benzene is in the state of **sp² hybridization**.

---