Question

The formula of hydride of nitrogen that is acidic in nature is:
A) $N{H_3}$
B) ${N_3}H$
C) ${N_2}{H_4}$
D) $N{H_2}OH$

Answer 1

Hint: The Lewis acid is a species that accepts the lone pair of electrons and the Lewis base is the species that has lone pair or can donate the lone pair of electrons. One can analyze the given options molecules and their structures and decide which can be acidic in nature.

Complete step by step answer:
1) First of all we will analyze all the given options one by one and decide which shows acidic or basic character. The first option molecule is $N{H_3}$ which is ammonia. The structure of ammonia is the pyramidal structure which has one lone pair at the axial position. As this structure contains one lone pair of electrons, this structure is basic in nature. Hence, this option is incorrect.
2) The second option molecule is ${N_3}H$ which is also called hydrazoic acid. The structure name contains the name acid itself and it can donate the proton easily. Hence, ${N_3}H$ is acidic in nature and this option is the correct choice.
3) The third option molecule ${N_2}{H_4}$ is called diazene diamine. The structure can be written as \[H - N = N - H\] and has a lone pair of electrons on both nitrogen atoms each. As this structure has a lone pair of electrons it shows basic nature. Hence, this option is an incorrect choice.
4) The fourth structure $N{H_2}OH$ is also called hydroxylamine. The structure contains a lone pair of electrons on the nitrogen atom hence, it shows basic nature and this option is incorrect.
Therefore, the formula of hydride of nitrogen that is acidic in nature is ${N_3}H$ which shows option B as the correct choice.

Note:
One can calculate the charge present on the nitrogen in each molecule by the formula of oxidation state. The less charge nitrogen possesses in the structure the more acidic will be the hydride of the nitrogen. The charge in the molecule $N{H_3}$, ${N_3}H$, ${N_2}{H_4}$, $N{H_2}OH$ is ${\text{ - 3, - }}\frac{1}{3},{\text{ - 2, - 1}}$ respectively.