The lowest O-O bond length in the following m | vedclass

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(B) To determine the $O-O$ bond length,we look at the bond order of the oxygen-oxygen bond in each molecule:$1$. In $O_2$,the bond order is $2.0$ (dou

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$O_2$

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(B) To determine the $O-O$ bond length,we look at the bond order of the oxygen-oxygen bond in each molecule:$1$. In $O_2$,the bond order is $2.0$ (double bond).$2$. In $O_3$ (ozone),the bond order is $1.5$ (resonance hybrid).$3$. In $H_2O_2$,the bond order is $1.0$ (single bond).$4$. In $O_2F_2$,the bond order is $1.0$,but due to the high electronegativity of fluorine,the $O-O$ bond is significantly weakened and elongated compared to $H_2O_2$.Comparing the bond orders,$O_2$ has the highest bond order $(2.0)$,which corresponds to the shortest bond length. Therefore,$O_2$ has the lowest $O-O$ bond length.

The lowest $O-O$ bond length in the following molecules is:

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