In `SOCl_(2)`, the Cl-S-Cl and Cl-S-O bond angles are

Options

A. `130^(@) and 115^(@)`
B. `106^(@) and 96^(@)`
C. `107^(@) and 108^(@)`
D. `96^(@) and 106^(@)`

Explanation

To determine the Cl-S-Cl and Cl-S-O bond angles in SOCl₂ (thionyl chloride), we can follow these steps:

### Step 1: Determine the Hybridization of SOCl₂
- SOCl₂ has a sulfur atom (S) bonded to one oxygen atom (O) and two chlorine atoms (Cl).
- The central atom, sulfur, has 4 regions of electron density: 2 single bonds with Cl and 1 double bond with O, plus 1 lone pair.
- The hybridization of sulfur in SOCl₂ is sp³.

**Hint:** Remember that hybridization is determined by the number of bonding pairs and lone pairs around the central atom.

### Step 2: Identify the Molecular Geometry
- With sp³ hybridization and 4 regions of electron density, the ideal geometry is tetrahedral.
- However, the presence of a lone pair will distort the geometry, leading to a trigonal pyramidal shape.

**Hint:** Consider how lone pairs affect the bond angles by repelling bonding pairs more strongly.

### Step 3: Analyze the Bond Angles
- In a perfect tetrahedral geometry, the bond angles would be 109.5°.
- However, due to the lone pair on sulfur, the bond angles will be slightly less than 109.5° for the Cl-S-Cl angle.
- The Cl-S-Cl bond angle is approximately 96°.
- The Cl-S-O bond angle is affected by the presence of the double bond with oxygen, which pulls the bonding pairs closer together, leading to a bond angle of approximately 106°.

**Hint:** Use the concept of lone pair repulsion to understand how bond angles are modified from ideal values.

### Step 4: Conclusion
- The Cl-S-Cl bond angle is approximately 96°.
- The Cl-S-O bond angle is approximately 106°.

### Final Answer:
- Cl-S-Cl bond angle: 96°
- Cl-S-O bond angle: 106°