Which among the following is paramagnetic ?

Options

A. `Cl_(2)O`
B. `ClO_(2)`
C. `Cl_(2)O_(7)`
D. `Cl_(2)O_(6)`

Explanation

To determine which among the given compounds is paramagnetic, we need to analyze each compound for the presence of unpaired electrons. A species is paramagnetic if it has one or more unpaired electrons in its molecular or atomic orbitals.

### Step-by-Step Solution:

1. **Understanding Paramagnetism**:
- A substance is paramagnetic if it has unpaired electrons. This can be determined by examining the electron configuration of the species.

2. **Analyzing Cl2O**:
- The structure of Cl2O can be drawn, and upon examining the electron configuration, we find that all electrons are paired.
- **Conclusion**: Cl2O is diamagnetic.

3. **Analyzing ClO2**:
- For ClO2, we can draw its Lewis structure. Chlorine (Cl) forms one coordinate bond and one double bond with oxygen (O).
- Chlorine has 7 valence electrons, and in this configuration, there are 3 remaining electrons around chlorine, which results in unpaired electrons.
- **Conclusion**: ClO2 is paramagnetic.

4. **Analyzing Cl2O7**:
- The structure of Cl2O7 (dichlorine heptoxide) can be drawn, and upon examination, we find that all electrons are paired.
- **Conclusion**: Cl2O7 is diamagnetic.

5. **Analyzing Cl2O6**:
- In Cl2O6 (dichlorine hexoxide), Cl atoms are bonded to three O atoms each, and upon drawing the structure, we find that all electrons are paired.
- **Conclusion**: Cl2O6 is diamagnetic.

6. **Final Conclusion**:
- After analyzing all the compounds, the only species that is paramagnetic is **ClO2**.

### Summary:
The paramagnetic species among the options provided is **Option B: ClO2**.