In which of the following is the O-O bond dis | vedclass

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(D) To determine the $O-O$ bond distance,we look at the bond order of the species:$1$. $O_2$: Bond order = $2.0$ (Electronic configuration: $\sigma 1s

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Dioxygen $(O_2)$

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(D) To determine the $O-O$ bond distance,we look at the bond order of the species:$1$. $O_2$: Bond order = $2.0$ (Electronic configuration: $\sigma 1s^2, \sigma^* 1s^2, \sigma 2s^2, \sigma^* 2s^2, \sigma 2p_z^2, \pi 2p_x^2 = \pi 2p_y^2, \pi^* 2p_x^1 = \pi^* 2p_y^1$).$2$. $O_2^-$ (Superoxide): Bond order = $1.5$.$3$. $O_2^{2-}$ (Peroxide): Bond order = $1.0$.Since bond distance is inversely proportional to bond order,the species with the highest bond order will have the minimum bond distance.$O_2$ has the highest bond order $(2.0)$,therefore it has the shortest $O-O$ bond distance.

In which of the following is the $O-O$ bond distance minimum?

Similar Questions

From elementary molecular orbital theory,the electronic configuration of the singly positive nitrogen molecular ion $N_2^+$ is:

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According to molecular orbital theory,the species among the following that does not exist is

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