Question

Out of ${\mathrm{NO}}^{+}$, ${\mathrm{NO}}_2^{-}$, and ${\mathrm{NO}}_3^{-}$ which has the longest $\mathrm{NO}$ bond and which has the shortest $\mathrm{NO}$ bond?

Answer 1

Bond length:

• The measure of the distance between the nuclei of two chemically bonded atoms in a molecule is called bond length.

Bond order of NO compounds:

• The Bond Order can be given by drawing the lewis structure and then applying the following formula: $Bondorder=\frac{Totalnumberofbonds}{No.ofbondgroups}$
• Bond groups are the number of atoms/molecules attached to the central atom.
• The bond order for ${\mathrm{NO}}^{+}$ is $\frac{3}{1}=3$ as it has 3 bonds and 1 bond group.
• The bond order for ${\mathrm{NO}}_2^{-}$is $\frac{3}{2}=1.5$ as it has 3 bonds and 2 bond groups.
• The bond order for ${\mathrm{NO}}_3^{-}$ is $\frac{4}{3}=1.33$ as it has 4 bonds and 3 bond groups.
• Bond length is inversely proportional to bond order. Higher the bond order shorter the bond length.

${\mathrm{NO}}^{+}$has the highest bond order and ${\mathrm{NO}}_3^{-}$ has the least bond order. Therefore, ${\mathrm{NO}}^{+}$ has the least bond length and ${\mathrm{NO}}_3^{-}$ has the longest bond length.