Question

The compound $N{F}_3$ is quite stable, but ${\text{NCl}}_3$ is very unstable ${\text{NCl}}_3$ was first synthesized in 1811 by P. L. Dulong, who lost three fingers and an eye studying its properties). The compounds ${\text{NBr}}_3$ and ${\text{NI}}_3$ are unknown, although the explosive ${\text{NI}}_3$. $N{H}_3$is known. How do you account for the instability of these halides of nitrogen?

Short answer

The instability of these halides of nitrogen is due to the large difference in size of the atoms involved.

Step-by-step solution

Define Nitrogen trihalides

The compounds having the general formula $\mathit{N}{\mathit{X}}_{\mathbf{3}}$ are known as nitrogen trihalides

Describe the comparison and stability of nitrogen trihalides

Nitrogen trihalides have limited stability except for ${\text{NF}}_3$. On the other hand nitrogen triiodide (${\text{NI}}_3$)is dangerously explosive.

Nitrogen trichloride (${\text{NCl}}_3$) is a yellow oil that is very endergonic and explosive. It was originally used as anoxidizingbleach for flour and is now made commercially by electrolysis of an aqueous solution of ammonium chloride.

The electronegativities of nitrogen and chlorine atoms are the same and thus the_{$\text{N}-\text{Cl}$} bond is almost nonpolar.

Nitrogen tribromide (${\text{NBr}}_3$) is an explosive, deep red oil.

Nitrogen has a very small size as compared to halogens, which have much larger sizes. Due to this, they can not remain bonded to the nitrogen atom and hence are highly unstable.

Thus, the instability of these compounds is due to the large difference in size.