Which set of oxide of nitrogen is paramagnetic in monomeric state?

Options

A. `NO , N_(2) O`
B. `NO_(2) , N_(2) O`
C. `NO , NO_(2)`
D. `N_(2) O , NO , NO_(2)`

Answer

To determine which set of oxides of nitrogen is paramagnetic in its monomeric state, we need to analyze the valence electrons of the given nitrogen oxides: N₂O, NO, and NO₂.

### Step-by-Step Solution:

1. **Understanding Paramagnetism**:
- A species is considered paramagnetic if it has unpaired electrons. This typically occurs when there is an odd number of total valence electrons.

2. **Calculating Valence Electrons**:
- The valence electron count for nitrogen (N) is 5 and for oxygen (O) is 6.
- Therefore, the total number of valence electrons in a molecule can be calculated based on its composition.

3. **Analyzing Each Oxide**:
- **For N₂O**:
- The total valence electrons = (5 * 2 for N) + (6 * 1 for O) = 10 + 6 = 16 (even).
- Since 16 is even, N₂O is not paramagnetic.

- **For NO**:
- The total valence electrons = (5 for N) + (6 for O) = 5 + 6 = 11 (odd).
- Since 11 is odd, NO is paramagnetic.

- **For NO₂**:
- The total valence electrons = (5 for N) + (6 * 2 for O) = 5 + 12 = 17 (odd).
- Since 17 is odd, NO₂ is also paramagnetic.

4. **Conclusion**:
- The oxides of nitrogen that are paramagnetic in their monomeric state are NO and NO₂.

### Final Answer:
The set of oxides of nitrogen that is paramagnetic in the monomeric state is **NO and NO₂**.