Which bond is shorter: C=O or N=O? Why? | vedclass

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Question

(A) . The bond length depends on the atomic radii and bond order.
In $C=O$ (as in carbon monoxide,$CO$),the bond length is approximately $1.128 \ \ma

Vedclass · Accepted Answer

$C=O$ is shorter due to higher bond order.

Vedclass · Answer

(A) . The bond length depends on the atomic radii and bond order.
In $C=O$ (as in carbon monoxide,$CO$),the bond length is approximately $1.128 \ \mathring{A}$.
In $N=O$ (as in nitric oxide,$NO$),the bond length is approximately $1.150 \ \mathring{A}$.
Therefore,$C=O$ is shorter than $N=O$. This is primarily due to the higher bond order and the specific electronic environment in $CO$ compared to the $NO$ radical.

Which bond is shorter: $C=O$ or $N=O$? Why?

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