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Which of the following orders regarding the bond length is correct?

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a

O_{2}^{-} > O_{2} > O_{2}^{+}

b

O_{2}^{-} > O_{2} < O_{2}^{+}

c

O_{2}^{-} < O_{2} > O_{2}^{+}

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detailed solution

Correct option is A

As bond order increases bond length decreases the bond order of species are:

$\frac{Number of bonding electron - Number of a . b . electron}{2} for O_{2} = \frac{10 - 6}{2} = 2 O_{2}^{+} = \frac{10 - 5}{2} = 2.5 O_{2}^{-} = \frac{10 - 7}{2} = 1.5 so bond order O_{2}^{+} > O_{2} > O_{2}^{-} and bond length are O_{2}^{-} > O_{2} > O_{2}^{+}$

Hence , the correct option (A). ${O_{2}}^{-}, O_{2}, {O_{2}}^{+}$

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