# Lewis Dot Structures of N_{2}O_{2}

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 N _{2}O_{2}**. Dinitrogen dioxide is the brown film we see in the atmosphere all over highly polluted cities. The resonance structures for N

_{2}O

_{2}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 N_{2}O_{2} 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 N_{2}O_{2} 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 **N _{2}O_{2}** are as follows:

**Figure 1: Lewis structures for N**

_{2}O_{2}. 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.
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