Which of the following molecule has odd `e^(-)`

Options

A. `ClO_(2)`
B. `O Cl_(2)`
C. `SCl_(2)`
D. None of these

Answer

To determine which of the given molecules has an odd number of electrons, we will follow these steps:

### Step 1: Identify the molecules
The molecules we need to analyze are:
1. ClO2 (Chlorine dioxide)
2. OCl2 (Oxygen dichloride)
3. SCl2 (Sulfur dichloride)

### Step 2: Calculate the total number of valence electrons for each molecule

#### For ClO2:
- Chlorine (Cl) has 7 valence electrons.
- Each Oxygen (O) has 6 valence electrons, and there are 2 Oxygens.
- Total valence electrons = 7 (from Cl) + 2 × 6 (from O) = 7 + 12 = 19 electrons.

#### For OCl2:
- Oxygen (O) has 6 valence electrons.
- Each Chlorine (Cl) has 7 valence electrons, and there are 2 Chlorines.
- Total valence electrons = 6 (from O) + 2 × 7 (from Cl) = 6 + 14 = 20 electrons.

#### For SCl2:
- Sulfur (S) has 6 valence electrons.
- Each Chlorine (Cl) has 7 valence electrons, and there are 2 Chlorines.
- Total valence electrons = 6 (from S) + 2 × 7 (from Cl) = 6 + 14 = 20 electrons.

### Step 3: Determine the number of unpaired electrons for each molecule

#### For ClO2:
- The Lewis structure shows that ClO2 has one unpaired electron and one lone pair on the chlorine atom.
- Thus, ClO2 has an odd number of electrons (19).

#### For OCl2:
- The Lewis structure shows that OCl2 has no unpaired electrons; all electrons are paired.
- Thus, OCl2 has an even number of electrons (20).

#### For SCl2:
- The Lewis structure shows that SCl2 also has no unpaired electrons; all electrons are paired.
- Thus, SCl2 has an even number of electrons (20).

### Step 4: Conclusion
From the analysis above, the only molecule with an odd number of electrons is **ClO2**.

### Final Answer:
**ClO2 has an odd number of electrons.**

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