To determine which statement is correct regarding the paramagnetic or diamagnetic nature of the given molecules, we will analyze each option based on the presence of unpaired electrons in their molecular orbital configurations.
### Step-by-Step Solution:
1. **Understanding Paramagnetism and Diamagnetism**:
- **Paramagnetic** substances have unpaired electrons and are attracted to magnetic fields.
- **Diamagnetic** substances have all electrons paired and are slightly repelled by magnetic fields.
2. **Analyzing Hydrogen (H₂)**:
- Hydrogen has 1 electron each, so in H₂, there are 2 electrons.
- The molecular orbital configuration is:
- σ(1s)² (bonding orbital)
- σ*(1s)² (antibonding orbital)
- Both electrons are in the bonding orbital, thus they are paired.
- **Conclusion**: H₂ is **diamagnetic**.
3. **Analyzing Nitrogen (N₂)**:
- Nitrogen has 7 electrons, so in N₂, there are 14 electrons.
- The molecular orbital configuration is:
- σ(1s)², σ*(1s)², σ(2s)², σ*(2s)², and then filling the 2p orbitals:
- σ(2p)², π(2p)², π(2p)² (total of 14 electrons).
- All electrons are paired in the molecular orbitals.
- **Conclusion**: N₂ is **diamagnetic**.
4. **Analyzing Oxygen (O₂)**:
- Oxygen has 8 electrons, so in O₂, there are 16 electrons.
- The molecular orbital configuration is:
- σ(1s)², σ*(1s)², σ(2s)², σ*(2s)², σ(2p)², π(2p)², and then filling the remaining:
- π(2p)¹, π(2p)¹ (total of 16 electrons).
- There are 2 unpaired electrons in the π(2p) orbitals.
- **Conclusion**: O₂ is **paramagnetic**.
5. **Final Evaluation of Statements**:
- **Statement A**: Hydrogen is Paramagnetic - **Incorrect** (H₂ is diamagnetic).
- **Statement B**: Nitrogen is Paramagnetic - **Incorrect** (N₂ is diamagnetic).
- **Statement C**: Oxygen is Paramagnetic - **Correct** (O₂ has unpaired electrons).
- **Statement D**: Oxygen is Diamagnetic - **Incorrect** (O₂ is paramagnetic).
### Correct Answer:
The correct statement is **C: Oxygen is Paramagnetic**.
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