# Method for Lewis dot structures: The nitrate ion NO_{3}^{-}

A **simple procedure for writing Lewis Dot 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 the **nitrate ion** **NO _{3}^{-}**. What are the

**Lewis structures of**?

**NO**_{3}^{-}__Step 1__: Connect the atoms with single bonds.

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

Where n in this case is 4. Where V = (5 +6*3) – (-1) = 24 , V is the number of valence electrons of the ion.
Therefore, P = 6n + 2 – V = 6 * 4 + 2 – 24 = 2 ** So, there is 1 double bond.**

__Step 3 & 4__: The * Lewis dot resonance structures* of the

**nitrate ion NO**are as follows:

_{3}^{-}

Therefore, there are 3 possible **Lewis resonance structures for NO _{3}^{-}.**

The above **simple four-step method for drawing Lewis structures** is presented in the following video:

__RELEVANT POSTS__

__REFERENCES__

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

__KEY TERMS__

**Lewis dot structures| NO3- ion | nitrate ion | method to draw dot structure| on line textbook, Lewis structure of no3- with formal charges, lewis structure of no3- molecule, resonance structures of no3-, resonance structures of no3-1, resonance lewis structure of no3-, lewis dot structures of no3-**

what is the Lewis structure of NO?

ReplyDeletePlease see the following post:

Deletehttp://chem-net.blogspot.com/2013/09/lewis-dot-structure-nitrogen-monoxide.html

Which of the above structures contributes more to the resonance?

ReplyDeleteThe above resonance structures are all equivalent because of the same charge separation and bond order. They are all contribute equally to the resonance.

DeleteWhy does the Nitrogen not have 2 double bonds and one single bond with the 3 oxygens? Doesn't that make the formal charges closer to 0 for all the elements?

ReplyDelete