Question

Why is the N-N bonds length in N2 shorter than the N-N bond legth in N20 even when both have a triple bond?

Answer 1

Answer:

Based on the N−O bond distances of 116.9 and 144.2 pm on HNO2 , I would expect the bond length to be between 116.9 and 144.2 pm (perhaps since there is a 0 formal charge on nitrogen, then the oxygens each share a The higher the bond order, the stronger the bond and thus the shorter the bond.

Explanation:

Answer 2

N−Nσ bond is weaker than P−Pσ bond due to the small bond length between the nitrogen atoms.

2. The non-bonding electrons(lone pair of electrons) of both the atoms repel each other making it weaker than P−Pσ bond. This is why the catenation tendency is not present in Nitrogen.

3. But nitrogen also has a tendency to form strong pπ−pπ bonds with itself which is not present in other Group 15 elements as the overlapping between the large atoms is diffuse.

4. So the N−Nπ− bond is stronger than P−Pπ−bond.