Simple Procedure for writing Lewis Structures for Diazomethane CH2N2 -#11

A simple procedure for writing Lewis structures is given in a previous article entitled “Lewis Structures and the Octet Rule”. Relevant worked examples were given in the following articles: Examples #1, #2, #3 , #4, #5, #6,  #7,  #8, #9 and #10. 

Another example  for writing Lewis structures following the above procedure is given bellow:

Let us consider the case of diazomethane (CH₂N₂) . Diazomethane is a yellow, poisonous, potentially explosive compound, which is a gas at room temperature. It is used in the organic chemistry laboratory for the conversion of carboxylic acids to methyl esters and for the conversion of alkenes to cyclopropane.

The resonance structures for CH₂N₂  are as follows:

Step 1: Connect the atoms with single bonds

Fig 1: Connecting the diazomethane atoms CH2N2 with single bonds (step 1 of the method)

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 CH₂N₂  consists of five atoms but two of them are hydrogen.

Where V = (4 + 2 * 1 + 5 + 5 ) = 16   

Therefore, P = 6n + 2 – V = 6 * 3 + 2 – 16 = 4    There are 4 π electrons in CH₂N_2.

Therefore, 2 double bonds or 1 triple bond must be added to the structure of Step 1.

Step 3 & 4: The Lewis structures for CH₂N₂ are as follows:

Figure 2: Lewis structures for CH₂N_2.  Delocalization of the carbon electron pair in structure 2 gives structure 3 which is more plausible since the positive charge is on the carbon atom which is more electropositive than N.

                                                                                   Figure 3: Diazomethane ESP structure

Lewis Dot Structures - Simple Procedure for writing Lewis Structures of Nitrous Oxide (N2O)

Lewis Electron Dot Structure of N₂O

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 nitrous oxide N₂O. Nitrous oxide is a colorless and odorless gas that is used as an anesthetic and analgesic in surgery and dentistry. It is also known as “laughing gas” due to the euphoric effects of inhaling it. It is used as an oxidizer in rocketry and in motor racing to increase the power output of engines. Nitrous oxide accounts for about 5% of the greenhouse  effect. Although its atmospheric concentration is only 320 ppb, it has 300 times greater ability to absorb infrared radiation than CO₂ does. The resonance structures for N₂O are as follows:

How can we construct the N₂O Lewis structure?

 

Step 1: The central atom will be the N atom since it is the less electronegative. Connect the atoms with single bonds:

 

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 N₂O consists of three atoms.

Where V = (5 + 5 + 6 ) = 16  

Therefore, P = 6n + 2 – V = 6 * 3 + 2 – 16 = 4  

There are 4 π electrons in N₂O.

Therefore, 2 double bonds or 1 triple bond must be added to the structure of Step 1.

Step 3 & 4: The Lewis structures for N₂O are as follows:

 

Please watch also the following video regarding the Lewis structures of Nitrous oxide:

Simple Procedure for writing Lewis Structures – Lewis Structures for Nitrogen Oxychloride NOCl

Lewis Structures for Nitrogen Oxychloride NOCl

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 Lewis electron dot structure of Nitrogen Oxychloride NOCl.

Nitrogen Oxychloride is a yellow gas. It is used in synthesis of pharmaceutical products (chlorinated agent).

 

Step 1:  The central atom will be the N atom since it is the less electronegative. Connect the atoms with single bonds:

 

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  NOCl consists of three atoms.

Where V = (5 + 6 +7 ) = 18  

Therefore, P = 6n + 2 – V = 6 * 3 + 2 – 18 = 2     So,   there are 2π electrons in NOCl _.

 

Step 3 & 4: Therefore, the Lewis electron dot structure of NOCl are as follows:

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Relevant Posts - Relevant Videos

Lewis Structures|Octet Rule: A Simple Method to write Lewis Structures

Simple Procedure for writing Lewis Structures – Lewis Structures for nitric acid (HNO3)

Lewis Electron - Dot Structure of NO3-

 

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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

resonance structures of nitric acid HNO3, Lewis electron structures of nitric acid, chemical formula of HNO3, simple procedure for drawing Lewis structures of nitric acid,

 

Simple Procedure for writing Lewis Structures – Lewis Structures for iodate ion IO3-

A simple procedure for writing Lewis structures is given in a previous article entitled “Lewis Structures and the Octet Rule”. Relevant worked examples were given in the following articles: Examples #1, #2, #3 and #4, #5, #6 and #7.

Another example  for writing Lewis structures following the above procedure is given bellow:

Let us consider the case of  IO₃^- :

Step 1: The central atom will be the I atom since it is the less electronegative. Connect the atoms with single bonds:

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 IO₃^- consists of four atoms.

Where V = (7 + 6 + 6 + 6 ) – (-1) = 26  

Therefore, P = 6n + 2 – V = 6 * 4 + 2 – 26 = 0     So,there are no π electrons in IO₃^-  

Step 3 & 4: Therefore, the Lewis structures for IO₃^-  are as follows:

Figure 1: Lewis structures for IO₃^-. The iodine atom is not restricted to an octet. Double bonds may be generated from the oxygen lone pairs so that to minimize charge separation.