Chapter 6, Problem 46QRT

Two Lewis structures can be written for nitrosyl fluoride, which contains one nitrogen, one oxygen, and one fluorine atom per molecule. Write the two Lewis structures land assign a formal charge to each atom.

Interpretation Introduction

Interpretation:

The Lewis structure of Nitrosyl Fluoride and a formal charge of each atom have to be written.

Concept Introduction:

Lewis structure otherwise known as Lewis dot diagrams or electron dot structures.  The bond between atoms and lone pairs of electrons that is present in the molecule.  Lewis structure represents each atom and their position in structure using the chemical symbol.  Excess electrons forms the lone pair are given by pair of dots, and are located next to the atom.

The formula for the formal charge can be written as

  $\text{Formal}\text{charge=}\text{Valence}\text{electrons-lone}\text{pair}\text{electrons}\text{-}\frac{\text{Bonding}\text{electrons}}{\text{2}}$

Explanation of Solution

The correct Lewis structure of the Nitrosyl Fluoride can be drawn as,

Draw a chart:

  $\overline{\begin{array}{l}\text{O}\text{N}\text{F}\\ \text{I}\text{II}\text{I}\text{II}\text{I}\text{II}\\ \overline{\underset{\_}{\begin{array}{l}\text{Valence}\text{electrons}\text{6}\text{6}\text{5}\text{5}\text{7}\text{7}\\ \text{Lone}\text{pair}\text{electrons}\text{6}\text{4}\text{2}\text{2}\text{4}\text{6}\\ \text{Bonding}\text{electrons}\text{2}\text{4}\text{6}\text{6}\text{4}\text{2}\\ \text{Formal}\text{charge}\text{-1}\text{0}\text{0}\text{0}\text{+1}\text{0}\end{array}}}\end{array}}$

The total number of valence electron is $18.$  the central Nitrogen atom wants to one multiple bond.

Nitrosyl Fluoride has two resonance structures, the best Lewis structure (II) because the lowest number formal charge structure.