Simple Method for writing Lewis Structures for N2O2

Lewis Dot Structures of N₂O₂

A simple procedure for writing Lewis structures is 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).

Another example  for writing Lewis structures following the above procedure is given below.

Let us consider the case of the dot structures of dinitrogen dioxide N₂O₂. Dinitrogen dioxide is the brown film we see in the atmosphere all over highly polluted cities. The resonance structures for N₂O₂ are as follows:

 

Step 1: Connect the atoms with single bonds. The central atoms are the nitrogen atoms.

 

Step 2: Calculate the # of electrons in π bonds (multiple bonds) using formula (1) in the article entitled “Lewis Structures and the Octet Rule” :

Where n in this case is 4 since N₂O₂ consists of four atoms. Where V = (5 + 5 + 6 + 6 ) = 22

Therefore, P = 6n + 2 – V = 6 * 4 + 2 – 22 = 4

So there are 4π electrons in N₂O₂ and that means 2 double bonds or a triple bond must be added to the structure in Step 1.

Step 3 & 4: The Lewis structures for N₂O₂ are as follows:

Figure 1: Lewis structures for N₂O₂. Structure #1 is the only experimentally observed structure. Structure #4 is the least plausible since O the most electronegative of the elements in the above structure has a + charge and N the least electronegative of the atoms present a – charge.

Simple Method for writing Lewis Structures for Carbon Disufide CS2

Simple Method for writing Lewis Structures for Carbon Disulfide CS₂

 

A simple procedure for writing Lewis Dot Structures was given in a previous post 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 the Lewis dot structures of carbon disulfide CS₂.

Step 1:  Connect the atoms with single bonds. Carbon is the central atom since it is less electronegative.

 

 

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

Where n in this case is 3 since CS₂ consists of three atoms.

Where V = (4 + 6 + 6 ) = 16  

Therefore, P = 6n + 2 – V = 6 * 3 + 2 – 16 = 4     So there are 4π electrons in CS₂  and that means 2 double bonds or a triple bond must be added to the structure in Step 1.

Step 3 & 4: The Lewis structure for CS₂  is as follows:

 

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Relevant Posts

Lewis dot structures of phosgene COCl₂

Rules for writing Lewis electron resonance structures - formamidine

 

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References

1. G.N. Lewis, J.A.C.S, 38, 762-785, (1916)
2.  E. C. McGoran, J. Chem. Educ., 68, 19-23 (1991)
3. A.B.P. Lever, J. Chem. Educ., 49, 819-821, (1972)

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Key Terms

simple method for drawing Lewis structures, Lewis structures of CS₂, Lewis electron dot structures of CS₂, dot structures of CS₂,

 

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Simple method for writing Lewis Structures: Chlorine Dioxide ClO₂

A simple procedure for writing Lewis electron dot structures is 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).

Another example  for writing Lewis structures following the above procedure is given below.

Let us consider the case of the Lewis dot structures of chlorine dioxide ClO₂. Chlorine dioxide is used mainly for bleaching of wood pulp, for bleaching of flour and for the disinfection of municipal drinking water

How can we draw the  Lewis structure of ClO₂?

 

Step 1: Connect the atoms with single bonds. Chlorine is the central atom.

 

Step 2: Calculate the # of electrons in π bonds (multiple bonds) using  formula (1) in the article entitled “Lewis Structures and the Octet Rule”. 

Where n in this case is 3 since ClO₂ consists of three atoms.

Where V = (6 + 6 + 7 ) = 19 

Therefore, P = 6n + 2 – V = 6 * 3 + 2 – 19 = 1   So there is only 1 π electron in ClO₂ 

So the structure of Step 1 is the Lewis structure.

Electrons are placed around each atom so that the octet rule is obeyed. Since the number of valence electrons is odd the octet rule will not be obeyed in all atoms. Formal charges are assigned and equalized using resonance.

Step 3 & 4: The Lewis structures of ClO₂ are derived below: