Chapter 4, Problem 4.72SP

Interpretation Introduction

Interpretation:

Electron-dot resonance structure for trichloronitromethane $\left({\text{CCl}}_{\text{3}}{\text{NO}}_{\text{2}}\right)$ which obeys the octet rule has to be drawn and the formal charges on Nitrogen and Oxygen in both structures has to be shown.

Concept introduction:

Resonance hybrid:

Sum of valid electron dot structure of a molecule is called resonance hybrid.  It shows overall delocalization of electrons within the molecule.

Octet rule:

Octet rule states that atoms of main group elements have a tendency to react so that achieve a noble gas configuration in s and p subshell (eight electrons).

Electron-dot structure:

This is only way to show the sharing of electrons between atom in polar covalent bonds or covalent bond.  This is often called Lewis structure.  This structure denotes valence electrons of an atom by dots and also it shows the way of valence electron distributed within a molecule.

Formal charge:

The formula used to find the formal charge is,

$\text{Formal charge = }\left(\begin{array}{l}\text{Number of valence}\\ \text{ electron in free atom}\end{array}\right)\text{ - }\frac{1}{2}\left(\begin{array}{l}\text{Number of }\\ \text{bonding }\\ \text{electrons}\end{array}\right)-\left(\begin{array}{l}\text{Number of }\\ \text{non-bonding electrons}\end{array}\right)$