Paramagnetic oxide is

Options

A. `N_(2)O`
B. `N_(2)O_(3)`
C. `NO`
D. `N_(2)O_(4)`

Answer

To determine which of the given oxides is paramagnetic, we need to analyze the number of electrons in each compound and check for the presence of unpaired electrons. A species is considered paramagnetic if it has one or more unpaired electrons.

### Step-by-Step Solution:

1. **Identify the Compounds**: The options provided are:
- A) N2O
- B) N2O3
- C) NO
- D) N2O4

2. **Calculate the Total Number of Electrons for Each Compound**:
- **For N2O**:
- Nitrogen (N) has 7 electrons, and there are 2 nitrogen atoms: 2 × 7 = 14 electrons.
- Oxygen (O) has 8 electrons: 1 × 8 = 8 electrons.
- Total = 14 + 8 = 22 electrons (even).

- **For N2O3**:
- Nitrogen (N): 2 × 7 = 14 electrons.
- Oxygen (O): 3 × 8 = 24 electrons.
- Total = 14 + 24 = 38 electrons (even).

- **For NO**:
- Nitrogen (N): 7 electrons.
- Oxygen (O): 8 electrons.
- Total = 7 + 8 = 15 electrons (odd).

- **For N2O4**:
- N2O4 is a dimer of NO2.
- Each NO2 has: N (7) + O (16) = 23 electrons.
- Since N2O4 consists of two NO2 units, total = 2 × 23 = 46 electrons (even).

3. **Determine Paramagnetism**:
- A species is paramagnetic if it has an odd number of electrons, which indicates the presence of unpaired electrons.
- From the calculations:
- N2O: 22 electrons (not paramagnetic)
- N2O3: 38 electrons (not paramagnetic)
- NO: 15 electrons (paramagnetic)
- N2O4: 46 electrons (not paramagnetic)

4. **Conclusion**: The only compound that is paramagnetic among the options is **C) NO**.

### Final Answer:
The paramagnetic oxide is **C) NO**.

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