Given below are two statements:Statement (I): | vedclass

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(C) Statement $I$: According to Molecular Orbital Theory $(MOT)$, the bond orders are: $O_2^+ (2.5)$, $O_2 (2.0)$, $O_2^- (1.5)$, and $O_2^{2-} (1.0)$

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Statement $I$ is true but Statement $II$ is false

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(C) Statement $I$: According to Molecular Orbital Theory $(MOT)$, the bond orders are: $O_2^+ (2.5)$, $O_2 (2.0)$, $O_2^- (1.5)$, and $O_2^{2-} (1.0)$.Since bond length is inversely proportional to bond order, the correct sequence of bond lengths is $O_2^+ Statement $II$: The number of unpaired electrons in these species are: $O_2$ $(2)$, $O_2^+$ $(1)$, $O_2^-$ $(1)$, and $O_2^{2-} (0)$.The correct sequence is $O_2 > O_2^+ = O_2^- > O_2^{2-}$.Therefore, the sequence given in Statement $II$ $(O_2 > O_2^+ > O_2^- > O_2^{2-})$ is incorrect because $O_2^+$ and $O_2^-$ have the same number of unpaired electrons. Thus, Statement $II$ is false.

Given below are two statements:
Statement $(I)$: The correct sequence of bond lengths in the following species is:
$O_2^+ < O_2 < O_2^- < O_2^{2-}$
Statement $(II)$: The correct sequence of number of unpaired electrons in the following species is:
$O_2 > O_2^+ > O_2^- > O_2^{2-}$

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Given below are two statements:Statement $(I)$: The correct sequence of bond lengths in the following species is:$O_2^+ < O_2 < O_2^- < O_2^{2-}$Statement $(II)$: The correct sequence of number of unpaired electrons in the following species is:$O_2 > O_2^+ > O_2^- > O_2^{2-}$