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

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

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?

Similar Questions

What are the similarities and differences in the Lewis structures of $H_2SO_4$ and $SO_4^{2-}$?

Identify the type of bonding in $CCl_4$ and $CaH_2$.

Identify the correct statements from the following.
$(I)$ $SnCl_2$ is ionic,but $SnCl_4$ is covalent in nature.
$(II)$ All linear diatomic molecules have zero dipole moment.
$(III)$ Both $NO$ and $O_2$ are paramagnetic.

Which of the following pairs of molecules have almost identical bond dissociation energy?

Observe the following structure. The formal charges on the atoms $1, 2, 3$ respectively are:

Vedclass Test Series

Exam Paper Generator

Online Exam Module