Lewis dot structures - Electron dot structure of CO -#43

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 carbon monoxide CO. Carbon monoxide is an odorless, colorless, non-irritant gas. It is the most common cause of fatal poisoning in Britain today. It causes the accidental deaths of up to 50 persons each year in the U.K. alone and a much larger number of non-fatal poisonings.

 

Step 1: Connect the atoms with single bonds. 

Fig. 1: Connect the atoms of  CO with single bonds.

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

Where n in this case is 2. Where V = (4 + 6)  = 10 , V is the number of valence electrons of the carbon monoxide molecule.

Therefore, P = 6n + 2 – V = 6 * 2 + 2 – 10  = 4   \  So, there are either 2 double bonds or a triple bond.

Since the molecule has only two atoms there is no possibility for 2 double bonds.

Step 3 & 4: The   dot resonance structures of  CO  areas follows:

Fig. 2 : Plausible Lewis Resonance Dot Structures of CO

 Lewis dot structure #2 is more stable since there is no charge separation and the octet rule is obeyed.