Question:
Using MOT, which of the following pairs denote paramagnetic species?
Using MOT, which of the following pairs denote paramagnetic species?
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Paramagnetic species have unpaired electrons in their molecular orbitals, which cause them to be attracted to a magnetic field.
Updated On: Mar 24, 2026
- \( \text{B}_2 \) and \( \text{C}_2 \)
- \( \text{B}_2 \) and \( \text{O}_2 \)
- \( \text{N}_2 \) and \( \text{C}_2 \)
- \( \text{O}_2 \) and \( \text{O}_2^2 \)
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The Correct Option is B
Solution and Explanation
Step 1: Apply Molecular Orbital Theory (MOT).
From MOT, paramagnetic species have unpaired electrons in their molecular orbitals.
Step 2: Conclusion.
Both \( \text{B}_2 \) and \( \text{O}_2 \) have unpaired electrons, making them paramagnetic. Final Answer: \[ \boxed{\text{B}_2 \text{ and } \text{O}_2} \]
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