`H_2 SO_3` and `H_2 SO_4` involve hybridisation of the type

Options

A. Both `sp^3`
B. Both `sp^3 d`
C. `sp^3, sp^3 d`
D. Both `dsp^2`

Answer

To determine the hybridization of sulfur in sulfurous acid (H₂SO₃) and sulfuric acid (H₂SO₄), we will follow these steps:

### Step 1: Analyze the structure of H₂SO₃ (Sulfurous Acid)
1. **Draw the Lewis structure**: H₂SO₃ has the following structure:
- Sulfur (S) is the central atom.
- It forms one double bond with an oxygen (O) atom and two single bonds with two hydroxyl (OH) groups.
- There is one lone pair of electrons on the sulfur atom.

2. **Count the sigma bonds and lone pairs**:
- Sigma bonds: 3 (one double bond counts as one sigma bond, and two single bonds with OH).
- Lone pairs: 1 (on sulfur).

3. **Calculate the hybridization index**:
- Hybridization index = Number of sigma bonds + Number of lone pairs = 3 (sigma bonds) + 1 (lone pair) = 4.

4. **Determine the hybridization**:
- A hybridization index of 4 corresponds to sp³ hybridization.

### Step 2: Analyze the structure of H₂SO₄ (Sulfuric Acid)
1. **Draw the Lewis structure**: H₂SO₄ has the following structure:
- Sulfur (S) is the central atom.
- It forms two double bonds with two oxygen atoms and two single bonds with two hydroxyl (OH) groups.

2. **Count the sigma bonds and lone pairs**:
- Sigma bonds: 4 (two double bonds count as two sigma bonds, and two single bonds with OH).
- Lone pairs: 0 (on sulfur).

3. **Calculate the hybridization index**:
- Hybridization index = Number of sigma bonds + Number of lone pairs = 4 (sigma bonds) + 0 (lone pairs) = 4.

4. **Determine the hybridization**:
- A hybridization index of 4 corresponds to sp³ hybridization.

### Conclusion
Both H₂SO₃ and H₂SO₄ involve sp³ hybridization.

### Final Answer
The correct option is: **Both sp³**.

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