Name the oxide of chlorine which has odd number of electrons and paramagnetic in nature.

Answer

To solve the question regarding the oxide of chlorine that has an odd number of electrons and is paramagnetic in nature, we can follow these steps:

### Step 1: Identify the Oxides of Chlorine
Chlorine forms several oxides, including:
- Chlorine monoxide (ClO)
- Chlorine dioxide (ClO2)
- Chlorine trioxide (ClO3)
- Chlorine pentoxide (ClO5)

### Step 2: Determine the Electron Count for Each Oxide
Next, we need to calculate the total number of electrons in each oxide:
- **ClO**: Chlorine (17 electrons) + Oxygen (8 electrons) = 25 electrons (odd)
- **ClO2**: Chlorine (17 electrons) + 2 × Oxygen (2 × 8 electrons) = 33 electrons (odd)
- **ClO3**: Chlorine (17 electrons) + 3 × Oxygen (3 × 8 electrons) = 41 electrons (odd)
- **ClO5**: Chlorine (17 electrons) + 5 × Oxygen (5 × 8 electrons) = 57 electrons (odd)

### Step 3: Identify the Paramagnetic Nature
A molecule is paramagnetic if it has unpaired electrons. We need to check the electron configuration of ClO2:
- In ClO2, the total number of electrons is 33.
- When we distribute these electrons, we find that there is one unpaired electron.

### Step 4: Conclusion
Since ClO2 has an odd number of electrons (33) and contains unpaired electrons, it is paramagnetic in nature. Therefore, the oxide of chlorine that meets the criteria of having an odd number of electrons and being paramagnetic is **chlorine dioxide (ClO2)**.

### Final Answer
The oxide of chlorine which has an odd number of electrons and is paramagnetic in nature is **chlorine dioxide (ClO2)**.

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