`NO_(2)` and `N_(2)O_(4)` are two forms of nitrogen dioxide. One exists in gaseous state while other in liquid state. The nature of `NO_(2)` and `N_(2)O_(4)` forms are

Options

A. Both are diamagnetic
B. Both are paramagnetic
C. `NO_(2)` is dimagnetic while `N_(2)O_(4)` is paramagnetic
D. `NO_(2)` is paramagnetic while `N_(2)O_(4)` is diamagnetic

Explanation

To determine the nature of the compounds NO₂ (nitrogen dioxide) and N₂O₄ (dinitrogen tetroxide), we need to analyze their electronic configurations and magnetic properties.

### Step-by-Step Solution:

1. **Identify the Compounds**:
- NO₂ is nitrogen dioxide, which is a brown gas.
- N₂O₄ is dinitrogen tetroxide, which is a colorless liquid.

2. **Determine the Structure of NO₂**:
- The molecular structure of NO₂ consists of one nitrogen atom bonded to two oxygen atoms.
- The nitrogen atom has one unpaired electron, which can be visualized using Lewis structures.

3. **Check for Unpaired Electrons in NO₂**:
- In the Lewis structure of NO₂, nitrogen has five valence electrons. It forms two bonds with oxygen and has one unpaired electron.
- Since there is at least one unpaired electron, NO₂ is classified as **paramagnetic**.

4. **Determine the Structure of N₂O₄**:
- N₂O₄ is formed by the dimerization of two NO₂ molecules.
- In N₂O₄, the nitrogen atoms share their unpaired electrons, resulting in a stable structure where all electrons are paired.

5. **Check for Unpaired Electrons in N₂O₄**:
- In the Lewis structure of N₂O₄, both nitrogen atoms achieve a complete octet, and there are no unpaired electrons.
- Therefore, N₂O₄ is classified as **diamagnetic**.

6. **Conclusion**:
- NO₂ is paramagnetic due to the presence of an unpaired electron.
- N₂O₄ is diamagnetic because it has no unpaired electrons.

### Final Answer:
The correct statement regarding the nature of NO₂ and N₂O₄ is: **NO₂ is paramagnetic while N₂O₄ is diamagnetic**.