Lewis Structure| Dot Structure of NO2

A simple procedure for writing Dot Electron Structures was given in a previous article entitled “Lewis Structures and the Octet Rule”. 

Several worked examples relevant to this procedure were given in previous posts please see the Sitemap - Table of Contents (Lewis Electron Dot Structures).

Let us consider the case of  NO₂. How can I draw the Lewis structure?

Step 1: Connect the atoms with single bonds

Fig. 1 : Connect the NO₂ atoms with single bonds.

 Step 2:  Calculate the # of electrons in π bonds (multiple bonds) using  formula (1): 

Where n in this case is 3. Where V = (6 + 5 + 6)  = 17 , V is the number of valence electrons of the molecule.

Therefore, P = 6n + 2 – V = 6 * 3 + 2 – 17  = 3   Therefore, there is 1 double bond and an unpaired electron.

Step 3 & 4: The   dot resonance structures of  NO₂  are as follows:

Fig. 2 : Plausible Lewis Resonance Dot Structures of NO₂

The lone electron is placed on the N atom which is more electropositive than O and can accommodate better a positive charge