The hybridisation of sulphur in sulphur dioxide is

Options

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

Explanation

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

### Step 1: Determine the Valence Electrons
First, we need to calculate the total number of valence electrons in the SO₂ molecule.

- Sulfur (S) has 6 valence electrons.
- Each oxygen (O) atom has 6 valence electrons, and there are 2 oxygen atoms.

So, the total number of valence electrons (V) can be calculated as follows:
\[ V = \text{Valence electrons of S} + 2 \times \text{Valence electrons of O} \]
\[ V = 6 + 2 \times 6 = 6 + 12 = 18 \]

### Step 2: Calculate Bond Pairs and Lone Pairs
Next, we divide the total number of valence electrons by 8 to determine the number of bond pairs and lone pairs.

\[ \text{Bond pairs} = \frac{V}{8} = \frac{18}{8} = 2 \text{ (whole number part)} \]
The whole number part (2) indicates the number of bond pairs.

Now, we find the remainder:
\[ \text{Remainder} = V - (8 \times \text{Bond pairs}) = 18 - (8 \times 2) = 18 - 16 = 2 \]
Since the remainder is 2, this indicates that there are 2 lone electrons, which means there is 1 lone pair (since each lone pair consists of 2 electrons).

### Step 3: Determine Hybridization
Now, we can determine the hybridization based on the number of bond pairs and lone pairs.

- Number of bond pairs = 2
- Number of lone pairs = 1

The hybridization can be determined using the formula:
\[ \text{Hybridization} = \text{Number of bond pairs} + \text{Number of lone pairs} \]
\[ \text{Hybridization} = 2 + 1 = 3 \]

The hybridization corresponding to 3 regions of electron density (2 bond pairs and 1 lone pair) is **sp²**.

### Step 4: Determine the Molecular Shape
With the hybridization being sp² and having one lone pair, the molecular geometry will be bent or V-shaped due to the repulsion between the lone pair and the bond pairs.

### Final Answer
The hybridization of sulfur in sulfur dioxide (SO₂) is **sp²**.

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