The correct statement regarding `SO_(2)` molecule is :

Options

A. two `p pi -d pi `bonds
B. molecule has 2 lone pair, `2sigma` bonds and `2pi` bonds
C. two `p pi-p pi` bonds
D. one `p pi - p pi` and one `p pi - dpi` bond

Answer

To determine the correct statement regarding the SO₂ molecule, we can follow these steps:

### Step 1: Identify the Valence Electrons
Sulfur (S) is in group 16 of the periodic table and has 6 valence electrons. Each oxygen (O) atom also has 6 valence electrons. Therefore, the total number of valence electrons in SO₂ is:
\[ 6 \text{ (from S)} + 2 \times 6 \text{ (from 2 O)} = 18 \text{ valence electrons} \]

### Step 2: Determine the Hybridization of Sulfur
To find the hybridization of the central atom (sulfur), we use the formula:
\[ \text{Hybridization number} = \frac{1}{2} \left( \text{Number of valence electrons} + \text{Number of bonded atoms} \right) \]
In SO₂, sulfur is double bonded to two oxygen atoms, so the number of bonded atoms is 2. Therefore:
\[ \text{Hybridization number} = \frac{1}{2} (6 + 2) = \frac{8}{2} = 4 \]
This indicates that sulfur is \( sp^2 \) hybridized.

### Step 3: Determine the Number of Lone Pairs and Bond Pairs
From the hybridization, we know sulfur has 3 hybrid orbitals (since it is \( sp^2 \)). The number of bond pairs is 2 (due to the two double bonds with oxygen). Thus, the number of lone pairs can be calculated as:
\[ \text{Lone pairs} = \text{Hybrid orbitals} - \text{Bond pairs} = 3 - 2 = 1 \]

### Step 4: Analyze the Bonding in SO₂
In SO₂, sulfur forms two double bonds with oxygen. Each double bond consists of one sigma bond and one pi bond. The pi bonds in SO₂ are formed as follows:
- The \( sp^2 \) hybrid orbitals of sulfur overlap with the \( p \) orbitals of oxygen to form sigma bonds.
- The remaining \( p \) orbitals of sulfur and oxygen overlap to form pi bonds.

### Step 5: Identify the Types of Bonds
- The two pi bonds formed in SO₂ consist of:
- One \( p \pi - p \pi \) bond (from the \( p \) orbital of sulfur and the \( p \) orbital of one oxygen).
- One \( p \pi - d \pi \) bond (from the \( p \) orbital of sulfur and the \( d \) orbital of the other oxygen).

### Conclusion
Based on the analysis, the correct statement regarding the SO₂ molecule is:
**Option D: One \( p \pi - p \pi \) bond and one \( p \pi - d \pi \) bond.**