Nitrogen forms the largest number of oxides as it is capable of forming stable multiple bonds with oxygen. They range from `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 important regarding the study of oxides of nitrogen
(a) All oxides of nitrogen except `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 breakble to give oxygen and hence oxides of nitrogen are said to be better oxidising agents.
(c) Except `N_(2)O_(5)`, all are gases at ordinary temperature `N_(2)O_(3)` is stable only at lower temperature (253 K).
(d) Except `N_(2)O` and NO which are neutral oxides, all are acidic oxides which dissolve in water forming corresponding oxy acids.
(e) They are also good example for illustrating the concept of resonance
Which of the following statements is correct for the oxides of nitrogen ?
A. Dinitrogen trioxide dissolves in potassium hydroxide forming potassium nitrate
B. Aqueous solution of nitrogen dioxide behaves both as a reducing agent and as an oxidising agent
C. Nitrous oxide is fairly soluble in cold water and turns blue litmus red
D. Nitrogen dioxide is not acidic oxide
