Which of the following is/are V-shaped molecule (s)

Options

A. `SnCl_(2)`
B. `SnCl_(4)`
C. `COS `
D. `PbCl_(2)`

Explanation

To determine which of the given molecules are V-shaped, we need to analyze the molecular geometry of each option based on their hybridization and the presence of lone pairs. Let's go through the options step by step.

### Step 1: Analyze SNCl2
1. **Valence Electrons**:
- Sulfur (S) has 6 valence electrons.
- Each Chlorine (Cl) has 7 valence electrons, and there are 2 Cl atoms.
- Total valence electrons = 6 + (2 × 7) = 20 electrons.

2. **Lewis Structure**:
- S is the central atom with 2 Cl atoms bonded to it.
- There will be 1 lone pair on the sulfur atom.

3. **Hybridization**:
- The hybridization can be determined by the formula:
\[ \text{Hybridization} = \text{Number of bond pairs} + \text{Number of lone pairs} \]
- Here, there are 2 bond pairs (from 2 Cl) and 1 lone pair.
- Hybridization = 2 + 1 = 3 → sp².

4. **Molecular Shape**:
- With 1 lone pair and 2 bond pairs, the shape is V-shaped (or angular).

### Step 2: Analyze SNCl4
1. **Valence Electrons**:
- Sulfur has 6 valence electrons.
- Each Chlorine has 7 valence electrons, and there are 4 Cl atoms.
- Total valence electrons = 6 + (4 × 7) = 34 electrons.

2. **Lewis Structure**:
- S is the central atom with 4 Cl atoms bonded to it.
- There are no lone pairs on the sulfur atom.

3. **Hybridization**:
- Hybridization = 4 bond pairs + 0 lone pairs = 4 → sp³.

4. **Molecular Shape**:
- With 4 bond pairs and no lone pairs, the shape is tetrahedral, not V-shaped.

### Step 3: Analyze COS
1. **Valence Electrons**:
- Carbon has 4 valence electrons.
- Oxygen has 6 valence electrons.
- Sulfur has 6 valence electrons.
- Total valence electrons = 4 + 6 + 6 = 16 electrons.

2. **Lewis Structure**:
- The molecule is linear with double bonds between C=O and C=S.

3. **Hybridization**:
- There are no lone pairs and 2 double bonds.
- Hybridization = 0 lone pairs + 2 bond pairs = 2 → sp.

4. **Molecular Shape**:
- The shape is linear, not V-shaped.

### Step 4: Analyze PbCl2
1. **Valence Electrons**:
- Lead (Pb) has 4 valence electrons.
- Each Chlorine has 7 valence electrons, and there are 2 Cl atoms.
- Total valence electrons = 4 + (2 × 7) = 18 electrons.

2. **Lewis Structure**:
- Pb is the central atom with 2 Cl atoms bonded to it.
- There will be 1 lone pair on the lead atom.

3. **Hybridization**:
- Hybridization = 2 bond pairs + 1 lone pair = 3 → sp².

4. **Molecular Shape**:
- With 1 lone pair and 2 bond pairs, the shape is V-shaped (or angular).

### Conclusion
The V-shaped molecules from the options provided are:
- **SNCl2**
- **PbCl2**