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 :

Options

A. Dinitrogen trioxide dissolve in potassium hydroxide forming potassium nitrate
B. Aqueous solution of nitrogen dioxide be haves both as a reducing agent and as an oxidising agent
C. Nitrous oxides fairly soluble in cold water and turns blue litmus red
D. Nitrogen dioxide in gaseous state is diamagnetic

Answer

B

Explanation

`NO,N_(2)O` - neutral oxides
`N_(2)O_(5)` - acidic oxide
`N_(2)O_(3) +KOH rarr KNO_(2)+H_(2)O`
`NO_(2)` (gas) - paramagnetic
`overset((+4))(NO_(2))` : acts both as a reducing agent and oxidising agent
Bond angle in `NO_(2)=132^(@)`