Statement -1 : `NO_(2)` and `CIO_(2)` both being odd electron molecules dimerise.
Statement -2 : On dimerisation, `NO_(2)` is coverted to stable `N_(2)O_(4)` molecule with even number of electrons.

Options

A. Statement -1 and Statement- 2 both are False.
B. Statement -1 is true, Statement- 2 is false.
C. Statement -1 is true , Statement-2 is true, Statement-2 is a correct explantion for Statement -1.
D. Statement -1 is False, Statement- 2 is True.

Explanation

To solve the question, we need to analyze both statements regarding the molecules NO₂ and ClO₂.

### Step 1: Analyze Statement 1
**Statement 1**: "NO₂ and ClO₂ both being odd electron molecules dimerize."

- **NO₂** (Nitrogen dioxide) has an odd number of electrons (11 electrons total). It is known to dimerize to form N₂O₄ (Dinitrogen tetroxide), which has an even number of electrons (24 electrons total).

- **ClO₂** (Chlorine dioxide) also has an odd number of electrons (19 electrons total). However, ClO₂ does not dimerize due to the presence of d orbitals in chlorine, which allows for electron delocalization and stabilization of the molecule in its monomeric form.

**Conclusion for Statement 1**: This statement is false because while NO₂ dimerizes, ClO₂ does not.

### Step 2: Analyze Statement 2
**Statement 2**: "On dimerization, NO₂ is converted to stable N₂O₄ molecule with even number of electrons."

- As established, when two NO₂ molecules combine, they form N₂O₄. This process results in a molecule that has an even number of electrons (24 electrons total). The dimerization of NO₂ is indeed a well-known reaction.

**Conclusion for Statement 2**: This statement is true.

### Final Conclusion
- **Statement 1** is false.
- **Statement 2** is true.

### Answer
The correct option is **Option 4**: Statement 1 is false, Statement 2 is true.

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