Nitrogen forms the largest number of oxides as it is capable of forming stable multiple bonds with oxygen.They range from `N_2O`(O.S of nitrogen+1) through `NO, N_2O_3,NO_2,N_2O_4` to `N_2O_5`(O.S of nitrogen +5).
Following points are important regarding the study of oxides of nitrogen.
(a)All oxides of nitrogen except `N_2O_6` and 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 breakable to give oxygen and hence oxides of nitrogen are said to be better oxidising agents.
(c )Except `N_2O_5`, all are gases at ordinary temperature. `N_2O_3` is stable only at lower temperature (253 K).
(d) Except `N_2O` 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 the resonance.
Which of the following statement is correct for the oxides of nitrogen ?

Options

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 an odd electron molecule and in the liquid phase, exists in equilibrium with the dimer `N_2O_4`

Answer

B

Explanation

(A)`N_2O_3 + 2KOH to 2KNO_2 + H_2O`
(B)`H_2O + 2NO_2 to HNO_2` (reducing agent ) +`HNO_3` (oxidising agent)
(C )Neutral to litmus as neutral oxide
(D)In the liquid state, `N_2O_4` tends to ionise
`2NO_2 hArr N_2O_4 hArr NO^(+) + NO_3^-`