Correct Answer is : O2+,O2{O}₂^{+} , {O}₂O2+,O2 - Both paramagnetic

{O}₂,{O}₂²-} - Both diamagnetic

{O}^{+} , {O}₂²-} - Both paramagnetic

{O}₂^{+} , {O}₂ - Both paramagnetic

{O},{O}₂²-} - Both paramagnetic

Correct Answer is : O2+,O2{O}₂^{+} , {O}₂O2+,O2 - Both paramagnetic

Test Index

VITEEE 2012 Paper

Section: Chemistry

Question : 43 of 120

Marks: +1, -0

Solution:

The molecular orbital configurations of

\mathrm{O}_2^{+}

\mathrm{O}_2^{-}

\mathrm{O}_2^{2-}

and

\mathrm{O}_2

are

\mathrm{O}_2^{+}

\sigma 1s^{2}

, σ*

1s^{2} , \sigma 2s^{2}

, σ*

2s^{2} , \sigma 2p_{z}^{2} , \pi 2p_{x}^{2}

\pi 2p_{y}^{2} , \pi^{*} 2p_{x}^{1}

\pi^{*} 2p_{y}^{0}

\mathrm{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}^{2}

\pi^{*} 2p_{y}^{1}

\mathrm{O}_2^{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}^{2}

\pi^{*} 2p_{y}^{2}

\mathrm{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}

and the electronic configuration of O and

\mathrm{O}^{+}

are

O =

1s^{2} , 2s^{2} , 2p_{x}^{2} , 2p_{y}^{1} , 2p_{z}^{1}

\mathrm{O}^{+}

1s^{2} , 2s^{2} , 2p_{x}^{1} , 2p_{y}^{1} , 2p_{z}^{1}

\mathrm{O}_2^{+} , \mathrm{O}_2 , \mathrm{O}_2^{-} , \mathrm{O}

and

\mathrm{O}^{+}

have unpaired electrons, hence are paramagnetic.

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