Question:

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

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Updated On: Oct 10, 2024

(A) $C O_{3}^{2 -} < C O_{2} < C O$
(B) $C O_{2} < C O_{3}^{2 -} < C O$
(C) $C O < C O_{3}^{2 -} < C O_{2}$
(D) $C O < C O_{2} M < C O_{3}^{2 -}$

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The Correct Option is C

Approach Solution - 1

Explanation:
The order of

C - O

bond length in the given species can be determined by finding out the number of bonds between the constituent atoms.The structures of the given species are as follows:1.

C O : {}^{-}C \equiv O^{+}

There is a triple bond between

C

and

O

atoms.2.

C O_{2} : O \equiv C = O

There are two double bonds between

C

and

O

atoms.3.

C O_{3}^{2 -}

There is a single, as well as a double-bond, showed between

C

and

O

atoms.From the above structures, it is clear that bond order for the given compounds increases as:

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

We know that Bond Length ∝

\frac{1}{b o n d o r d e r}

Thus, the increasing order of

C - O

bond length is:

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

Hence, the correct option is (D).

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Approach Solution -2

Ans: The bond length of C-O in the following compounds are:

The bond length is shorter in CO₂ as compared to CO₃²⁻ . This is because the oxygen forms a double bond with a carbon atom and, double bond is shorter than the single bond. The bond order of carbon dioxide is 2.

CO₃²⁻ has a longer C-O bond that carbon dioxide. It forms a single bond with Oxygen. The bond order for CO₃²⁻ is 1.33.

CO forms a triple bond. The bond order of CO is 3.