Question

Oxygen molecule is paramagnetic in nature. What is the paramagnetic content in terms of the magnetic moment in $O_2^{-}$?

• A. 1.732
• B. 3
• C. 1.5
• D. 2.5

Answer 1

Answer: (A)

1.732

$\left(\sigma 1s^2\right)(\sigma \ast 1s^2)\left(\sigma 2s^2\right)(\sigma \ast 2s^2)\left(\sigma 2p_z^2\right)(\pi 2p_x^2=\pi 2p_y^2)(\pi \ast 2p_x^2=\pi \ast 2p_y^1)$

Total number of unpaired electrons in $O_2^{-}$ is one

So to calculate magnetic moment,forumla is here:-

$M.M.=\sqrt{n(n+2)}$

$n=numberofunpairedelectrons$

$M.M.=\sqrt{1(1+2)}=\sqrt{3}=1.732$

So the correct option is [A].