`SO_2` and `So_3` involve hybridisation of the type

Options

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

Answer

To determine the hybridization of sulfur dioxide (SO₂) and sulfur trioxide (SO₃), we can follow these steps:

### Step 1: Determine the Valence Electrons
- Sulfur (S) has 6 valence electrons.
- Oxygen (O) has 6 valence electrons.

### Step 2: Draw the Lewis Structure
- For SO₂:
- Sulfur forms a double bond with each oxygen atom.
- There is one lone pair of electrons on the sulfur atom.

The Lewis structure can be represented as:
```
O
||
O = S
|
(Lone Pair)
```

- For SO₃:
- Sulfur forms a double bond with each of the three oxygen atoms.
- There are no lone pairs on the sulfur atom.

The Lewis structure can be represented as:
```
O
||
O = S = O
```

### Step 3: Calculate the Hybridization Index
The hybridization index (H) can be calculated using the formula:
\[ H = \text{Number of sigma bonds} + \text{Number of lone pairs on the central atom} \]

- For SO₂:
- Number of sigma bonds = 2 (one from each double bond)
- Number of lone pairs on sulfur = 1
- Hybridization index = 2 + 1 = 3
- Therefore, the hybridization of SO₂ is **sp²**.

- For SO₃:
- Number of sigma bonds = 3 (one from each double bond)
- Number of lone pairs on sulfur = 0
- Hybridization index = 3 + 0 = 3
- Therefore, the hybridization of SO₃ is also **sp²**.

### Step 4: Conclusion
Both SO₂ and SO₃ have a hybridization of **sp²**.

### Final Answer
The hybridization of SO₂ and SO₃ is **sp²**.

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