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(D) To determine the paramagnetic nature,we use Molecular Orbital Theory $(MOT)$ to find the number of unpaired electrons:$1. B_{2} (10 \ e^-): (\sigm

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$4$

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(D) To determine the paramagnetic nature,we use Molecular Orbital Theory $(MOT)$ to find the number of unpaired electrons:$1. B_{2} (10 \ e^-): (\sigma 1s)^2 (\sigma^* 1s)^2 (\sigma 2s)^2 (\sigma^* 2s)^2 (\pi 2p_x)^1 (\pi 2p_y)^1$ ($2$ unpaired electrons,paramagnetic)$2. Li_{2} (6 \ e^-): (\sigma 1s)^2 (\sigma^* 1s)^2 (\sigma 2s)^2$ ($0$ unpaired electrons,diamagnetic)$3. C_{2} (12 \ e^-): (\sigma 1s)^2 (\sigma^* 1s)^2 (\sigma 2s)^2 (\sigma^* 2s)^2 (\pi 2p_x)^2 (\pi 2p_y)^2$ ($0$ unpaired electrons,diamagnetic)$4. C_{2}^{-} (13 \ e^-): (\sigma 1s)^2 (\sigma^* 1s)^2 (\sigma 2s)^2 (\sigma^* 2s)^2 (\pi 2p_x)^2 (\pi 2p_y)^2 (\sigma 2p_z)^1$ ($1$ unpaired electron,paramagnetic)$5. O_{2}^{2-} (18 \ e^-): (\sigma 1s)^2 (\sigma^* 1s)^2 (\sigma 2s)^2 (\sigma^* 2s)^2 (\sigma 2p_z)^2 (\pi 2p_x)^2 (\pi 2p_y)^2 (\pi^* 2p_x)^2 (\pi^* 2p_y)^2$ ($0$ unpaired electrons,diamagnetic)$6. O_{2}^{+} (15 \ e^-): (\sigma 1s)^2 (\sigma^* 1s)^2 (\sigma 2s)^2 (\sigma^* 2s)^2 (\sigma 2p_z)^2 (\pi 2p_x)^2 (\pi 2p_y)^2 (\pi^* 2p_x)^1$ ($1$ unpaired electron,paramagnetic)$7. He_{2}^{+} (3 \ e^-): (\sigma 1s)^2 (\sigma^* 1s)^1$ ($1$ unpaired electron,paramagnetic)Thus,the paramagnetic species are $B_{2}, C_{2}^{-}, O_{2}^{+},$ and $He_{2}^{+}$. The total count is $4$.

The number of paramagnetic species among the following is $......$
$B_{2}, Li_{2}, C_{2}, C_{2}^{-}, O_{2}^{2-}, O_{2}^{+},$ and $He_{2}^{+}$

Similar Questions

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The number of paramagnetic species among the following is $......$$B_{2}, Li_{2}, C_{2}, C_{2}^{-}, O_{2}^{2-}, O_{2}^{+},$ and $He_{2}^{+}$