A) \[O_{2}^{+}>{{O}_{2}}>O_{2}^{-}\]
B) \[O_{2}^{+}>O_{2}^{-}>{{O}_{2}}\]
C) \[{{O}_{2}}>O_{2}^{+}>O_{2}^{-}\]
D) \[O_{2}^{-}>{{O}_{2}}>O_{2}^{+}\]
Correct Answer: A
Solution :
As bond order increase bond length decrease the bond order of species are \[=\frac{\text{number of bonding electron -Number of }a\text{.}b\text{. electron}}{2}\] 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 \[O_{2}^{+}>{{O}_{2}}>O_{2}^{-}\].
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