# Lewis Electron Dot Structure of Chloric Acid HClO_{3}

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** electron dot structures of chloric acid HClO _{3}**. Chloric acid is a colorless liquid. It will accelerate the burning of combustible materials and can ignite most on contact. It is a strong oxidizing agent. It is used as a reagent in chemical analysis and to make other chemicals.

How can we construct the **Lewis structure of HClO _{3 }**?

__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 4 since HClO_{3} consists of 5 atoms but one of them is a hydrogen atom (remember n is the number of atoms in a molecule minus the hydrogen atoms).

Where V = (1 + 7 + 3 * 6 ) = 26

Therefore, P = 6n + 2 – V = 6 * 4 + 2 – 26 = 0 and therefore there are no π electrons in HClO_{3}.

** So the structure of Step 1 is the Lewis structure. **

Electrons are placed around each atom so that the octet rule is obeyed. **Formal charges** are assigned and equalized using ** resonance**.

__Step 3
& 4__: The **Lewis structure for HClO _{3} ** is as follows:

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