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Write a note on nature of bonding of gro...

Write a note on nature of bonding of group-15 elements.

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Nitrogen is restricted to a maximum covalency of 4 since only four (one 5 and three p) orbitals are available for bonding. The heavier elements have vacant d- orbitals in the outermost shell which can be used for bonding (covalency) and hence can expand their covalence.
Ex. : `PCl_(5), [PCl_(6)]^(-), [PF_(6)]^(-)` - etc. Nitrogen forms pn-pn bonds due to its small size while other elements donot form pn-pn bonds. Hence in their elemental state Phosphorus, Arsenic and antimony exists as `P_(4), As_(4)` and `Sb_4` respectively as tetrahedral molecules.
Due to non-availability of rf-orbitals in nitrogen it cannot form `dpi-d pi` bonds which are possible with other elements.
Ex: `R_(3)P=O` or `R_(3)P = CH_(2)` (R = alkyl group)
Phosphorus and arsenic forms `dpi`- bonds with transition metals when their compounds act as ligand. For example : `P(C_(2)H_(5))_(3)`
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