Question

Explain how nitrogen exhibits anomalous behavior amongst group 15 elements.

Answer 1

Hint: Remember the physical properties of all elements in group 15 for example nitrogen shows a large variety of oxidation.

Complete answer:
Nitrogen activity in group 15 components is anomalous. Nitrogen is the first of the 15 elements in a group that has,
- Total atomic scale.
- Overall electronegativity.
- The maximum potential for ionization, and
- Loss of D-orbitals.

In nature the difference between nitrogen and other 15 group elements is:
- Nitrogen is a gas while all other components are solid.
- Nitrogen occurs as a diatomic molecule, (${N_2}$) although there are other elements as tetratomic molecules (${P_4},A{s_4},S{r_4},etc$.)
- Nitrogen, possessing the highest electronegativity, forms hydrogen bonding while others do not.
- Nitrogen forms $p\pi - p\pi$ multiple bonds, while the other elements in the group form $p\pi - p\pi$ multiple bonds, respectively.
- Nitrogen shows a wide variety of −3 to +5 oxidation states while other elements show small oxidation states.
- $N{H_3}$ Is important while other hydrides are less common.
- Nitrogen trihalides (except $N{F_3}$) are unstable while the other trihalides are fairly stable.
- All other elements, except nitrogen, have vacant d-orbitals and, because of this nitrogen, do not undergo coordination compound formation.

Note: Group 15, also known as the family of nitrogen contains compounds such as nitrogen (N), phosphorus (P), arsenic (As), antimony (Sb), and bismuth (Bi). All Group 15 elements have in their outer shell the electron configuration $n{s^2}n{p^3}$, where n is equal to the primary quantum number.