Discuss the general characteristics of Group - 15 elements with reference to their electronic configuration, oxidation state, atomic size, ionization enthalpy and electronegativity.

Explanation

1) Electronic Configuration : All these elements of this group have `s^(2)p^(3)` configuration in their respective outmost orbits.
Nitrogen (N) : [He] `2s^(2)2p^(3)`, phosphorus (P) : [Ne] `3s^(2)3p^(3)`, Arsenic (As) : [Ar] `3d^(10)4s^(2)4p^(3)`
Atimony (Sb) : [Kr] `4d^(10)5s^(2)5p^(3)` and Bismuth (Bi) = [Xe] `4f^(14)5d^(10)6s^(2)6p^(3)`
2) Oxidation States : As per their configurations, these elements may utilize either the three electrons in the p-orbitals or the five electrons present in both s -and p -orbitals in the exhibition of oxidation states. Consequently, they exhibit common oxidation states +III and +V.
3) Atomic size : In Group-15 elements atomic size increase down the group. A considerable increase in covalent radius observed from N to P and from As to Bi only a small increase in atomic size observed.
4) Ionisation enthalpy : In group - 15 elements ionisation enthalpy decreases down the group due to gradual increase in atomic size.
5) Electronegativity : In group-15 elements electronegativity values decrease down the group with increase in atomic size.