Question

What is the molecular structure of the stable form of $\mathrm{F}\mathrm{N}{\mathrm{O}}_2$ ? ($\mathrm{N}$is the central atom.)

Short answer

The molecular structure of $\mathrm{F}\mathrm{N}{\mathrm{O}}_2$molecule is trigonal planar as shown in the below resonating structures:

Step-by-step solution

Definition of Concept

There are two types of bonds in trigonal bipyramidal structures: axial bonds and equatorial bonds. In total, there are five bonds in the trigonal bipyramidal geometry.

Find the molecular structure of the stable form

The compound$\mathrm{F}\mathrm{N}{\mathrm{O}}_2$is made up of one N, two O, and one F atom. The central atom N’s atomic number is 7, and its electronic configuration is$1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^3$, with valence electrons equal to 5, indicating that it has five valence electrons. As a result, there are three bonded atoms, three electron density regions, and no lone pairs on the central N-atom, giving rise to the$\mathrm{A}{\mathrm{X}}_3$type molecule. Three bonded atoms are present on the central N-atom, resulting in a trigonal planar molecular structure around the central atom, making the molecule much more stable by keeping the electron pairs as far apart as possible. Because both O-atoms contribute equally, charge separation will occur on both the O-atoms and th N-atom.

Therefore, the required structure is: