explain anomalous behaviour of Nitrogen
Dear Student,
Nitrogen is found differ in many properties from the rest of the members of group 15.
This is because of the following :
(i) Its smallest size
(ii) Its high electronegativity
(iii) Its high ionisation enthalpy
(iv) Absence of d-orbitals in it.
Some of the properties in which it differs from other members are
I)Nitrogen has unique ability to form
Nitrogen is found differ in many properties from the rest of the members of group 15.
This is because of the following :
(i) Its smallest size
(ii) Its high electronegativity
(iii) Its high ionisation enthalpy
(iv) Absence of d-orbitals in it.
Some of the properties in which it differs from other members are
I)Nitrogen has unique ability to form
pπ -pπ multiple bonds with itself and with other elements having small size and high electronegativity (e.g., C, O).
II)Heavier elements of this group do not form pπ -pπ bonds as their atomic orbitals are so large and diffuse that they cannot have effective overlapping.
III) nitrogen exists as a diatomic molecule with a triple bond (one s and two p) between the two atoms. Consequently, its bond enthalpy
(941.4 kJ mol–1) is very high. On the contrary, phosphorus, arsenic and antimony form single bonds as P–P, As–As and Sb–Sb while
bismuth forms metallic bonds in elemental state.
IV)Single N–N bond is weaker than the single P–P bond because of high interelectronic repulsion of the non-bonding electrons, owing to the small bond length. As a result the catenation tendency is weaker in nitrogen.
Regards.
IV)Single N–N bond is weaker than the single P–P bond because of high interelectronic repulsion of the non-bonding electrons, owing to the small bond length. As a result the catenation tendency is weaker in nitrogen.
Regards.