Question

Elemental nitrogen exists as ${\mathit{N}}_{\mathbf{2}}$, whereas in the gas phase the elements phosphorus, arsenic, and antimony consist of${\mathbf{P}}_{\mathbf{4}}$,$\mathit{A}{\mathit{s}}_{\mathbf{4}}$, and$\mathit{S}{\mathit{b}}_{\mathbf{4}}$molecules, respectively. Give a possible reason for this difference between${\mathit{N}}_{\mathbf{2}}$and the other Group$\mathbf{5}\mathit{A}$elements.

Short answer

The$\mathrm{\pi }$ bond on${\mathrm{N}}_2$ is responsible for the elemental nitrogen's existence as ${\mathrm{N}}_2$.

Step-by-step solution

Define π bond:

Pi bonds (bonds) are covalent chemical bonds in which two lobes of an orbital (on one atom) overlap laterally with two lobes of an orbital on another atom.

${\mathrm{N}}_2$is the atomic form of nitrogen. The elements phosphorus, arsenic, and antimony are made up of $p_4$, $A{s}_4$, and${\mathrm{Sb}}_4$ molecules in the gas phase.The explanation will be examined below for a probable reason for the discrepancy between${\mathrm{N}}_2$ and the other components in group $5A$.

The elements of 5A group and ability to bond nitrogen

The elements nitrogen, phosphorus, arsenic, antimony, and bismuth make up the $5A$group.

Only nitrogen, in comparison to elements in group$5A$ like phosphorus, arsenic, and antimony, has the ability and capability to make a strong$\pi$ bond because only nitrogen can form two electrons or more than one electron.

Formation of strong π bond

On the other hand, for phosphorus, arsenic, and antimony, they only prefer to share one electron , than forming more than one electrons, making them lose the ability of forming strong pi bonds.

Therefore, pi bond on${\mathrm{N}}_2$ is responsible for the elemental nitrogen's existence as ${\mathrm{N}}_2$.