Question

Oxygen molecule is paramagnetic in nature. What is the paramagnetic content in terms of magnetic moment in $O^{-}_{2}$?

• A. $1.732$
• B. $3$
• C. $1.5$
• D. $2.5$

Answer 1

Answer: (A)

$1.732$

Answer 2

$O_{2}^{-} : \left(\sigma 1s^{2}\right)\left(\sigma^* 1s^{2}\right)\left(\sigma 2s^{2}\right)\left(\sigma^* 2s^{2}\right) \left(\sigma 2P_{z}^{2}\right)$ $\left(\pi 2p_{x}^{2} = \pi2p_{y}^{2}\right) \left(\pi^{ *} 2p_{x}^{2} = \pi^{ *} 2p_{y}^{1}\right)$ $O_{2}^{-}$ has $1$ unpaired electron. $\mu=\sqrt{n\left(n+2\right)}B.M.$ $= \sqrt{1\left(1+2\right)} = \sqrt{3}$ $= 1.732 B.M.$