Nitrogen forms the largest number of oxides as it is capable of forming stable multiple bonds with oxygen. They range of `N_(2)O` (O.S of nitrogen +1) through `NO, N_(2)O_(3),NO_(2),N_(2)O_(4)` "to" `N_(2)O_(5)` (O.S of nitrogen +5). Following points are improtant regarding the study of oxides of nitrogen.
(a) All oxides of nitrogen expect `N_(2)O_(5)` are endothermic as a large amount of energy is required to dissociate the stable molecule of oxygen and nitrogen.
(b) The small electronegativity difference between oxygen and nitrogen make N-O bond easily breakle to give oxygen and hence oxides of nitrogen are said to be better oxidising agents.
(c) Expect `N_(2)O_(5)`, all are gases at ordinary temperature. `N_(2)O_(3)` is stable only at lower temperature (253K).
(d) Expect `N_(2)O` and NO which are neutal oxides, all are acidic oxides which dissolve in water forming coresponding oxy acids.
(e) They are also good example for illustrating the concept of resonance.
The gas which is acidic in nature is :
A. In `N_(2)O_(4)` the `N-N` bond length is longer than the usual `N-N` is single bond distance
B. `NO_(2)` molecule is angular with `N-O` distance equal to intermediate distance between a single and a double bond.
C. `N_(2)O` is a linear molecule and has a small dipole moment
D. The bond angle of `NO_(2)` is less than `120^(@)`
