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Explai how does nitrogen exhibit anomalous behaviour amongst group 15 elements. |
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Answer» Solution :Anomalous behaviour of nitrogen among group 15 elements. Nitrogen is the first amongst group 15 elements, which has, (a) The smallest atomic size. (b) Highest electronegativity. (c ) The highest ionisation ENERGY. (d) Absence of d-orbitals. The difference in the nature between nitrogen and other elements of 15 group are : (i) Nitrogen is a GAS while all the other elements are solid. (ii) Nitrogen exists as diatomic molecule, `(N_(2))` while other elements exist as tetra - atomic molecules `(P_(4),As_(4),Sr_(4)," etc. ")` (iii) Being the highest electronegative element in group 15 nitrogen forms HYDROGEN bonding while other does not. (iv) Nitrogen forms `ppi-dpi` multiple bonds while other elements in the group from `ppi-dpi` multiple bonds. (v) Nitrogen shows wide range of oxidation states from -3 to +5 while other elements show limited oxidation states . (VI) `NH_(3)` is basic while other HYDRIDES are very less basic. (vii) The trihalides of nitrogen (except `NF_(3)` ) are unstable while the trihalildes of the other elements are comparatively stable. (viii) Except nitrogen, all other elements have vacant d- orbitals, and due to this nitrogen does n't undergo formation of coordination compound. |
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