The correct order of C-O bond length is: | vedclass

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(D) We know that bond length $\propto \frac{1}{	ext{bond order}}$.Thus,a higher bond order corresponds to a shorter bond length.The bond order can be

Vedclass · Accepted Answer

$CO < CO_2 < CO_3^{2-}$

Vedclass · Answer

(D) We know that bond length $\propto \frac{1}{ ext{bond order}}$.Thus,a higher bond order corresponds to a shorter bond length.The bond order can be calculated as the average number of bonds per resonance structure.For $CO$ (carbon monoxide),the bond order is $3$.For $CO_2$ (carbon dioxide),the bond order is $2$.For $CO_3^{2-}$ (carbonate ion),the bond order is $\frac{4}{3} \approx 1.33$.Since the bond order follows the order $CO > CO_2 > CO_3^{2-}$,the bond length follows the inverse order:$CO < CO_2 < CO_3^{2-}$.

The correct order of $C-O$ bond length is:

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