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  • If the magnetic moment of a dioxygen species is 1.73 B.M, it may be:  Option: 1 <img alt="O_{2}, O_{2}^{-}or O_{2}^{+}" src="https://l

If the magnetic moment of a dioxygen species is 1.73 B.M, it may be:

 

Option: 1

O_{2}, O_{2}^{-}or O_{2}^{+}


Option: 2

O_{2}^{-} or O_{2}^{+}


Option: 3

O_{2}or O_{2}^{-}


Option: 4

O_{2}or O_{2}^{+}


Answers (1)

best_answer

The electronic configuration of O2 molecule is given below:

Thus, the electronic configuration of O2 molecule can be written as:

σ1s2 σ*1s2 σ2s2 σ*2s2 σ2pz2 π2px2 π2py2 π*2px1 π*2py1

 

\mathrm{O}_{2}=\sigma 1 \mathrm{s}^{2} \sigma^{\star} 1 \mathrm{s}^{2} \sigma 2 \mathrm{s}^{2} \sigma^{\star} 2 \mathrm{s}^{2} \sigma 2 \mathrm{p} z^{2} \pi 2 \mathrm{p} x^{2}=\pi 2 \mathrm{py}^{2} \pi^{\star} 2 \mathrm{px}^{1}=\pi^{\star} 2 \mathrm{py}^{1}

The magnetic moment of dioxygen species = 1.73 B.M means it has one unpaired electron. One unpaired electron is present in \mathrm{O}_2^+, \mathrm{O}_2^{-}.

Hence, option number (2) is correct.

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chirag

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