What is the molecular structure of the stable form of \({\rm{FN}}{{\rm{O}}_{\rm{2}}}\) ? (\({\rm{N}}\)is the central atom.)

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.

The compound\({\rm{FN}}{{\rm{O}}_{\rm{2}}}\)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\({\rm{1\;}}{{\rm{s}}^{\rm{2}}}{\rm{2\;}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{3}}}\), 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\({\rm{A}}{{\rm{X}}_{\rm{3}}}\)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: