# Lewis Electron Dot Structures of Hydrogen Cyanide (HCN) and Nitronium Ion (NO_{2}^{+})

A simple procedure for drawing **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 index page **Lewis Structures & the Octet Rule - Theory & Examples** . Let us examine the case of nitronium ion NO_{2}^{+}and hydrogen cyanide HCN.

Let us consider the case of NO_{2}^{+}. The **Lewis dot structures of NO _{2}^{+} with formal charges** are as follows:

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

Step 2: Calculate the # of electrons in p bonds (pi bonds, multiple bonds) using
formula (**1)** in the article entitled **
Lewis Structures and the Octet Rule.**

Where n in this case is 3 since NO_{2}^{+} consists of three atoms.
Where V = (6 + 5 + 6) - 1 = 16
Therefore, P = 6n + 2 - V = 6 * 3 + 2 - 16 =
4

Therefore,there
are 4
electrons (pi electrons) in NO_{2}^{+} ^{ } and 2 double bonds must be added to the structure of Step 1 or 1 triple bond.

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