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Which one of the following molecules is expected to exhibit diamagnetic behaviour ? [JEE M 2013]
- a)C2
- b)N2
- c)O2
- d)S2
Correct answer is option 'A,B'. Can you explain this answer?
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Verified Answer
Which one of the following molecules is expected to exhibit diamagneti...
The molecular orbital structures of C2 and N2 are
both N2 and C2 have paired electrons in its molecular orbital hence are diamagnetic.
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Which one of the following molecules is expected to exhibit diamagneti...
Understanding Diamagnetic Behavior
Diamagnetic materials are characterized by having all their electrons paired, resulting in no net magnetic moment. This means they do not have unpaired electrons, which would otherwise make them paramagnetic.
Analysis of the Given Molecules
1. C2 (Dicarbon)
- Electron Configuration: The molecular orbital configuration for C2 is σ2s² σ*2s² σ2p².
- Unpaired Electrons: There are no unpaired electrons in C2.
- Conclusion: C2 is diamagnetic.
2. N2 (Dinitrogen)
- Electron Configuration: The molecular orbital configuration for N2 is σ2s² σ*2s² σ2p² π2p².
- Unpaired Electrons: There are no unpaired electrons in N2.
- Conclusion: N2 is also diamagnetic.
3. O2 (Dioxygen)
- Electron Configuration: The molecular orbital configuration for O2 is σ2s² σ*2s² σ2p² π2p².
- Unpaired Electrons: O2 has two unpaired electrons in the π2p orbitals.
- Conclusion: O2 is paramagnetic.
4. S2 (Disulfur)
- Electron Configuration: The molecular orbital configuration for S2 is σ2s² σ*2s² σ2p² π2p⁴.
- Unpaired Electrons: S2 has unpaired electrons.
- Conclusion: S2 is also paramagnetic.
Final Conclusion
Therefore, the molecules exhibiting diamagnetic behavior from the options provided are:
- C2
- N2
The correct answer is indeed A and B.
Diamagnetic materials are characterized by having all their electrons paired, resulting in no net magnetic moment. This means they do not have unpaired electrons, which would otherwise make them paramagnetic.
Analysis of the Given Molecules
1. C2 (Dicarbon)
- Electron Configuration: The molecular orbital configuration for C2 is σ2s² σ*2s² σ2p².
- Unpaired Electrons: There are no unpaired electrons in C2.
- Conclusion: C2 is diamagnetic.
2. N2 (Dinitrogen)
- Electron Configuration: The molecular orbital configuration for N2 is σ2s² σ*2s² σ2p² π2p².
- Unpaired Electrons: There are no unpaired electrons in N2.
- Conclusion: N2 is also diamagnetic.
3. O2 (Dioxygen)
- Electron Configuration: The molecular orbital configuration for O2 is σ2s² σ*2s² σ2p² π2p².
- Unpaired Electrons: O2 has two unpaired electrons in the π2p orbitals.
- Conclusion: O2 is paramagnetic.
4. S2 (Disulfur)
- Electron Configuration: The molecular orbital configuration for S2 is σ2s² σ*2s² σ2p² π2p⁴.
- Unpaired Electrons: S2 has unpaired electrons.
- Conclusion: S2 is also paramagnetic.
Final Conclusion
Therefore, the molecules exhibiting diamagnetic behavior from the options provided are:
- C2
- N2
The correct answer is indeed A and B.
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Which one of the following molecules is expected to exhibit diamagnetic behaviour ? [JEE M 2013]a)C2b)N2c)O2d)S2Correct answer is option 'A,B'. Can you explain this answer?
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