Question

Explain why nitride of lithium $(L{i_3}N)$ is more stable than nitride of potassium $({K_3}N)$ ?

Answer 1

Alkali metals have just a solitary electron in the peripheral orbital, so can achieve just a positive charge of +1. So as to shape a cation of most extreme charge thickness, you require an exceptionally little particle to begin with. Lithium is the littlest particle among antacid metals. In this manner $L{i^ + }$ will have the most noteworthy +ve charge thickness.

Complete step by step answer:
Lithium is the main gathering 1 component that can frame a steady salt metal nitride (at standard conditions), the other gathering 1 components will respond (at various response conditions) to shape their individual nitrides (on account of rubidium, $R{b_3}N$ (rubidium nitride), however the compound will be temperamental and break down rapidly. The responses of the soluble base metals (other than lithium) with nitrogen would not deliver enough cross section energy and would along these lines be endothermic, so they don't frame nitrides at standard conditions.

Additional information
Lithium responds with nitrogen gas at room temperature $({N_2})$ and it structures Lithium Nitride $(L{i_3}N)$ which is steady, on the grounds that the grid energy delivered from the development of $(L{i_3}N)$ is sufficiently high to make the general response exothermic.

Note:
Lithium, the lightest of the soluble base metals, is the main salt metal which responds with nitrogen at standard conditions, and its nitride is the main stable antacid metal nitride. Acid neutralizers are medicine that kill stomach corrosive to eliminate indigestion.