Answer
See explanation
Work Step by Step
1. NO (Nitric oxide):
The nitrogen-oxygen bond in nitric oxide (NO) is the shortest among the given species. This is because the bond is a triple bond, which is very strong and has a short bond length.
2. NO2 (Nitrogen dioxide):
In nitrogen dioxide (NO2), the nitrogen-oxygen bonds are slightly longer than the bond in nitric oxide (NO) due to the presence of a single bond and a partial double bond character.
3. N2O (Nitrous oxide):
Nitrous oxide (N2O) has a longer nitrogen-oxygen bond compared to NO and NO2. This is because the nitrogen-oxygen bond in N2O is a single bond.
4. H2NOH (Hydroxylamine):
In hydroxylamine (H2NOH), the nitrogen-oxygen bond is longer than in the previous species due to the presence of a single bond and the influence of the hydrogen atoms.
5. NO3 (Nitrate ion):
The nitrate ion (NO3-) has the longest nitrogen-oxygen bond among the given species. This is because the nitrogen-oxygen bonds in the nitrate ion are single bonds, and the formal negative charge on the oxygen atoms also contributes to the longer bond length.
To place the given species in order of the shortest to the longest nitrogen-oxygen bond, we need to consider the bond lengths and the formal charges on the nitrogen and oxygen atoms.
Shorter bonds correspond to higher bond order (more shared electrons). The correct order from the shortest to the longest nitrogen-oxygen bond is:
1. $NO^{+}$
2. $N_2O$
3. $NO_2^{-}$
4. $NO_3^{-}$
5. $H_2NOH$
