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

C O < C O_{3}^{2 -} = C O_{2}

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C O < C O_{3}^{-} < C O_{2}

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C O < C O_{2} < C O_{3}^{2 -}

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C O_{2} < C O_{3}^{2 -} < C O

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Solution

The correct option is C $C O < C O_{2} < C O_{3}^{2 -}$
The order is $C O < C O_{2} < C O_{3}^{2 -}$

CO: When drawing the lewis structure here, we end up with a triple bond between the carbon and the oxygen.

$C O_{2}$ : This lewis structure gives one double bond between each oxygen and the carbon.

$C O_{3}^{2 -}$ : When we draw the lewis structure for this ion, we get a double bond between one oxygen and the carbon, with single bonds between the other two oxygen atoms and the carbon. Because each of the oxygens wants a double bond to the carbon, they have resonating structures, meaning that in the end, we get a bond something between a double and a single bond for each Carbon-Oxygen bond. Therefore, this bond will be longer than a single bond, but shorter than a double bond.

And we know the order of bond length: $T r i p l e b o n d < d o u b l e b o n d < s i n g l e b o n d$

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Similar questions

The correct order of C - O bond length among $C O, C O_{3}^{2 -}, C O_{2}$ is:

The correct order of increasing C-O bond length of $C O, C O_{3}^{2 -}, C O_{2}$ is

C - O

C O

C O_{2}

C O_{3}^{2 -}

C - O

C O, C O_{3}^{2 -} and C O_{2}

C O, C O_{3}^{2 -}

C O_{2}

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