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  • What is the number of unpaired electron(s) in the highest occupied molecular orbital of the following species : <img alt="\mathrm{N}_2 ; \mathrm{N}_2^{+} ; \mathrm{O}_2 ; \mathrm{O}_2^{+} \text {?

What is the number of unpaired electron(s) in the highest occupied molecular orbital of the following species : \mathrm{N}_2 ; \mathrm{N}_2^{+} ; \mathrm{O}_2 ; \mathrm{O}_2^{+} \text {? }

Option: 1

2,1,0,1


Option: 2

0, 1, 0, 1


Option: 3

0,1,0,1


Option: 4

2,1,2,1


Answers (1)

best_answer

\mathrm{N}_2=\sigma_{1 \mathrm{~s}^2}, \sigma_{1 \mathrm{~s}^2}^*, \sigma_{2 \mathrm{~s}^2}, \sigma_{2 \mathrm{~s}^2}^*, \pi_{2 \mathrm{Px}^2}=\pi_{2 \mathrm{Py}^2}, \sigma_{2 \mathrm{Pz}^2}

no. of \mathrm{e}^{-} present in Homo =0
$$ \mathrm{N}_2^{+}=\sigma_{1 \mathrm{~s}^2}, \sigma_{1 \mathrm{~s}^2}^*, \sigma_{2 \mathrm{~s}^2}, \sigma_{2 \mathrm{~s}^2}^*, \pi_{2 \mathrm{Px}^2}=\pi_{2 \mathrm{Py}^2}, \sigma_{2 \mathrm{Pz}^1}
no. of unpaired \mathrm{e}^{-}present in \mathrm{HOMO}=1
$$ \mathrm{O}_2=\sigma_{1 \mathrm{~s}^2}, \sigma_{1 \mathrm{~s}^2}^*, \sigma_{2 \mathrm{~s}^2}, \sigma_{2 \mathrm{~s}^2}^*, \sigma_{2 \mathrm{Pz}^2}, \pi_{2 \mathrm{Px}^2}=\pi_{2 \mathrm{Py}^2}, \pi_{2 \mathrm{Px}}^* 1=\pi_{2 \mathrm{Py}} 1
no. of unpaired \mathrm{e}^{-} present in \mathrm{HOMO}=2
$$ \mathrm{O}_2^{+}=\sigma_{1 \mathrm{~s}^2}, \sigma_{1 \mathrm{~s}^*}^*, \sigma_{2 \mathrm{~s}^2}, \sigma_{2 \mathrm{~s}^*}, \sigma_{2 \mathrm{Pz}^2}, \pi_{2 \mathrm{Px}^2}=\pi_{2 \mathrm{Py}}^2, \pi_{2 \mathrm{Px}^*}=\pi_{2 \mathrm{Py}}^* 0
no. of unpaired \mathrm{e}^{-} present in \mathrm{HOMO}=1

Posted by

Kuldeep Maurya

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