Anomalous Behavior of Nitrogen

Anomalous Behavior of Nitrogen:- Nitrogen, the first member of group 15, differs from others group members because of :-

i)             Small size of N atom.

ii)           High value of electronegativity of N atom and high ionization energy.

iii)          Absence of d-orbitals in the valency shell.

iv)          Tendency of form multipole bonds.

The properties in which nitrogen differs from other members of 15 groups are listed below.

i)             Nitrogen is gas while others members are solids.

ii)           Nitrogen molecule is diatomic while other elements from teratomic molecules such as p₄, As₄ and Sb₄.

iii)          The catenation property is more pronounced in nitrogen.

iv)          Nitrogen forms five oxides of monomeric nature. Others can form at the most three types of oxides, X₄O₆, X₄O₁₀ of dimeric nature. N₂O₄ exists in dimeric from and is diamagnetic.

v)           Hydride of nitrogen is stable while the hydrides of other elements are not stable and acts as reducing agent. Hydrogen bonding is present in ammonia but not present in other hydrides.

vi)          Expect NF3, the halides of nitrogen are unstable and explosive. The halides of other elements are stable. Unlike P, as and Sb, nitrogen does not form pentahalides.

vii)        Nitrogen can form trinegative ion N^3-. This tendency is less in P but absent in other elements.

Dear Student


Anomalous Behavior of Nitrogen is due to the following reasons
a) Small size of N atom.
b) High value of electronegativity of N atom and high ionization energy.
c) Absence of d-orbitals in the valency shell.
d) Tendency of form multipole bonds.

Anomalous Properties of Nitrogen

1. Nitrogen is gas while others members are solids.
2. Nitrogen molecule is diatomic while other elements from teratomic molecules such as P₄, As₄and Sb₄.
3. The catenation property is more pronounced in nitrogen.
4. Nitrogen forms five oxides of monomeric nature. Others can form at the most three types of oxides, X₄O₆, X₄O₁₀ of dimeric nature. N₂O₄ exists in dimeric from and is diamagnetic.
5. Hydride of nitrogen is stable while the hydrides of other elements are not stable and acts as reducing agent. Hydrogen bonding is present in ammonia but not present in other hydrides.
6. Expect NF₃, the halides of nitrogen are unstable and explosive. The halides of other elements are stable. Unlike P, as and Sb, nitrogen does not form pentahalides.
7. Nitrogen can form trinegative ion N^3-. This tendency is less in P but absent in other elements.

I hope this answer will help you.
Thanks & Regards
Yash Chourasiya