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.
Identify the incorrect statement.

Options

A. In `N_2O_4` the N-N bond length is longer than the usual N-N 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_2O` is a linear molecule and has a small dipole moment
D. None of these

Answer

D

Explanation

(A)N-N bond length (1.75 Å) is longer than usual N-N single bond length which is believed to be due to `delta^-` charge and lone pair of electrons on N atoms which causes repulsion.

(C )`:N-=underset(sp)N:tounderset(ddot)overset(ddot)O:` and the structure suggests that it will have some dipole moment.