Sulphur is `sp^2` hybridised in

Options

A. `SO_3`
B. `SO_2`
C. `CO_2`
D. `CO`

Answer

To determine the hybridization of sulfur in various compounds, we can follow these steps:

### Step 1: Identify the Compound
We need to analyze the compounds where sulfur is present. The compounds mentioned in the video transcript are sulfur trioxide (SO₃) and sulfur dioxide (SO₂).

### Step 2: Determine the Valence Electrons
Sulfur (S) has 6 valence electrons (group 16 of the periodic table).

### Step 3: Draw the Lewis Structure
- For **SO₃**:
- Sulfur forms three double bonds with three oxygen atoms.
- The Lewis structure shows sulfur at the center with three double bonds to oxygen atoms.

- For **SO₂**:
- Sulfur forms two double bonds with two oxygen atoms and has one lone pair of electrons.
- The Lewis structure shows sulfur at the center with two double bonds to oxygen atoms and one lone pair.

### Step 4: Count Sigma Bonds and Lone Pairs
- In **SO₃**:
- There are 3 sigma bonds (one for each S=O bond) and 0 lone pairs.
- Total = 3 sigma bonds + 0 lone pairs = 3 regions of electron density.

- In **SO₂**:
- There are 2 sigma bonds (one for each S=O bond) and 1 lone pair.
- Total = 2 sigma bonds + 1 lone pair = 3 regions of electron density.

### Step 5: Determine Hybridization
Using the formula for hybridization:
- Hybridization = Number of sigma bonds + Number of lone pairs
- For **SO₃**: Hybridization = 3 + 0 = 3 → sp² hybridized.
- For **SO₂**: Hybridization = 2 + 1 = 3 → sp² hybridized.

### Conclusion
Sulfur is sp² hybridized in both SO₃ and SO₂.

### Final Answer
Sulfur is sp² hybridized in SO₃ and SO₂.

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