Question

Using MOT, which of the following pairs denote paramagnetic species?

• A. \( \text{B}_2 \) and \( \text{C}_2 \)
• B. \( \text{B}_2 \) and \( \text{O}_2 \)
• C. \( \text{N}_2 \) and \( \text{C}_2 \)
• D. \( \text{O}_2 \) and \( \text{O}_2^2 \)

Hint:

Paramagnetic species have unpaired electrons in their molecular orbitals, which cause them to be attracted to a magnetic field.

Answer 1

The Correct Option is B

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: \[ \boxed{\text{B}_2 \text{ and } \text{O}_2} \]