If the magnetic moment of a dioxygen species | vedclass

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(A) The magnetic moment $(\mu)$ is given by the formula $\mu = \sqrt{n(n+2)} \; B.M$,where $n$ is the number of unpaired electrons. For $\mu = 1.73 \;

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

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(A) The magnetic moment $(\mu)$ is given by the formula $\mu = \sqrt{n(n+2)} \; B.M$,where $n$ is the number of unpaired electrons. For $\mu = 1.73 \; B.M$,we have $n = 1$.SpeciesUnpaired electrons $(n)$$O_{2}^{+}$$1$$O_{2}^{-}$$1$$O_{2}$$2$Since both $O_{2}^{+}$ and $O_{2}^{-}$ have $1$ unpaired electron,they both exhibit a magnetic moment of $1.73 \; B.M$.

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

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