Hybridization of Sulphur in `SO_(2)` is :

Options

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

Explanation

To determine the hybridization of sulfur in \( SO_2 \), we can follow these steps:

### Step 1: Determine the number of valence electrons for sulfur
Sulfur (S) is in group 16 of the periodic table, which means it has 6 valence electrons.

### Step 2: Identify the number of monovalent groups attached to the central atom
In \( SO_2 \), sulfur is the central atom, and it is bonded to two oxygen atoms. Each oxygen is considered a monovalent group. Therefore, the number of monovalent groups is 2.

### Step 3: Calculate the steric number
The steric number can be calculated using the formula:
\[ \text{Steric Number} = \text{Number of valence electrons on central atom} + \text{Number of monovalent groups} + \text{Charge} \]
In this case:
- Number of valence electrons on sulfur = 6
- Number of monovalent groups = 2 (from the two oxygen atoms)
- Charge = 0 (since \( SO_2 \) is neutral)

Plugging in the values:
\[ \text{Steric Number} = 6 + 2 + 0 = 8 \]

### Step 4: Determine the hybridization based on the steric number
The hybridization can be determined from the steric number:
- A steric number of 2 corresponds to \( sp \) hybridization.
- A steric number of 3 corresponds to \( sp^2 \) hybridization.
- A steric number of 4 corresponds to \( sp^3 \) hybridization.
- A steric number of 5 corresponds to \( sp^3d \) hybridization.
- A steric number of 6 corresponds to \( sp^3d^2 \) hybridization.

In our case, the steric number is 3, which corresponds to \( sp^2 \) hybridization.

### Conclusion
The hybridization of sulfur in \( SO_2 \) is \( sp^2 \).

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