The paramagnetic molecule at ground state amo | vedclass

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Question

(B) According to Molecular Orbital Theory $(MOT)$,the electronic configuration of $O_2$ ($16$ electrons) is:$O_2: (\sigma 1s)^2 (\sigma^* 1s)^2 (\sigm

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$O_2$

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(B) According to Molecular Orbital Theory $(MOT)$,the electronic configuration of $O_2$ ($16$ electrons) is:$O_2: (\sigma 1s)^2 (\sigma^* 1s)^2 (\sigma 2s)^2 (\sigma^* 2s)^2 (\sigma 2p_z)^2 (\pi 2p_x)^2 (\pi 2p_y)^2 (\pi^* 2p_x)^1 (\pi^* 2p_y)^1$.Due to the presence of two unpaired electrons in the antibonding $\pi^*$ orbitals,$O_2$ is paramagnetic.$H_2$,$N_2$,and $CO$ have all paired electrons and are diamagnetic.

List-$I$ (Molecule / ion)	List-$II$ (Bond order)
$1$. $NO$	$i$. $1.5$
$2$. $CO$	$ii$. $2.0$
$3$. $O_2^{-}$	$iii$. $2.5$
$4$. $O_2$	$iv$. $3.0$

The paramagnetic molecule at ground state among the following is

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According to molecular orbital theory,which of the following statements about the magnetic character and bond order is correct regarding $O_2^+$?

Match List-$I$ with List-$II$ and select the correct option:
List-$I$ (Molecule / ion) List-$II$ (Bond order)
$1$. $NO$ $i$. $1.5$
$2$. $CO$ $ii$. $2.0$
$3$. $O_2^{-}$ $iii$. $2.5$
$4$. $O_2$ $iv$. $3.0$

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