Which of the following compound is paramagnetic?

Options

A. `N_(2)O_(4)`
B. `ClO_(2)`
C. `Cl_(2)O_(7)`
D. `N_(2)O`

Answer

To determine which of the given compounds is paramagnetic, we need to identify the presence of unpaired electrons in each compound. A compound is considered paramagnetic if it has one or more unpaired electrons, while it is diamagnetic if all electrons are paired.

Let's analyze each compound step by step:

### Step 1: Analyze N2O4
1. **Count the valence electrons:**
- Nitrogen (N) has 5 valence electrons, and there are 2 nitrogen atoms: \(2 \times 5 = 10\).
- Oxygen (O) has 6 valence electrons, and there are 4 oxygen atoms: \(4 \times 6 = 24\).
- Total valence electrons in N2O4: \(10 + 24 = 34\).

2. **Determine electron pairing:**
- 34 electrons will form 17 pairs.
- Since all electrons are paired, N2O4 is **diamagnetic**.

### Step 2: Analyze ClO2
1. **Count the valence electrons:**
- Chlorine (Cl) has 7 valence electrons, and there is 1 chlorine atom: \(1 \times 7 = 7\).
- Oxygen (O) has 6 valence electrons, and there are 2 oxygen atoms: \(2 \times 6 = 12\).
- Total valence electrons in ClO2: \(7 + 12 = 19\).

2. **Determine electron pairing:**
- 19 electrons will form 9 pairs and 1 unpaired electron.
- Since there is 1 unpaired electron, ClO2 is **paramagnetic**.

### Step 3: Analyze Cl2O7
1. **Count the valence electrons:**
- Chlorine (Cl) has 7 valence electrons, and there are 2 chlorine atoms: \(2 \times 7 = 14\).
- Oxygen (O) has 6 valence electrons, and there are 7 oxygen atoms: \(7 \times 6 = 42\).
- Total valence electrons in Cl2O7: \(14 + 42 = 56\).

2. **Determine electron pairing:**
- 56 electrons will form 28 pairs.
- Since all electrons are paired, Cl2O7 is **diamagnetic**.

### Step 4: Analyze N2O
1. **Count the valence electrons:**
- Nitrogen (N) has 5 valence electrons, and there are 2 nitrogen atoms: \(2 \times 5 = 10\).
- Oxygen (O) has 6 valence electrons, and there is 1 oxygen atom: \(1 \times 6 = 6\).
- Total valence electrons in N2O: \(10 + 6 = 16\).

2. **Determine electron pairing:**
- 16 electrons will form 8 pairs.
- Since all electrons are paired, N2O is **diamagnetic**.

### Conclusion
After analyzing all the compounds:
- **N2O4**: Diamagnetic (no unpaired electrons)
- **ClO2**: Paramagnetic (1 unpaired electron)
- **Cl2O7**: Diamagnetic (no unpaired electrons)
- **N2O**: Diamagnetic (no unpaired electrons)

Thus, the compound that is paramagnetic is **ClO2**.

### Final Answer
The correct answer is **ClO2**.

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