HClO3 Lewis structure

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HClO₃ (chloric acid) has one hydrogen atom, one chlorine atom, and three oxygen atoms.

In the HClO₃ Lewis structure, there are two double bonds and one single bond around the chlorine atom, with three oxygen atoms attached to it. The oxygen atom with double bonds has two lone pairs, the right oxygen atom (with which the hydrogen atom is attached) also has two lone pairs, and on the chlorine atom, there is one lone pair.

Steps

Use these steps to correctly draw the HClO₃ Lewis structure:

#1 First draw a rough sketch
#2 Mark lone pairs on the atoms
#3 Calculate and mark formal charges on the atoms, if required
#4 Convert lone pairs of the atoms, and minimize formal charges
#5 Repeat step 4 if needed, until all charges are minimized, to get a stable Lewis structure

Let’s discuss each step in more detail.

#1 First draw a rough sketch

• First, determine the total number of valence electrons

In the periodic table, hydrogen lies in group 1, chlorine lies in group 17, and oxygen lies in group 16.

Hence, hydrogen has one valence electron, chlorine has seven valence electrons, and oxygen has six valence electrons.

Since HClO₃ has one hydrogen atom, one chlorine atom, and three oxygen atoms, so…

Valence electrons of one hydrogen atom = 1 × 1 = 1
Valence electrons of one chlorine atom = 7 × 1 = 7
Valence electrons of three oxygen atoms = 6 × 3 = 18

And the total valence electrons = 1 + 7 + 18 = 26

Learn how to find: Hydrogen valence electrons, Chlorine valence electrons, and Oxygen valence electrons

• Second, find the total electron pairs

We have a total of 26 valence electrons. And when we divide this value by two, we get the value of total electron pairs.

Total electron pairs = total valence electrons ÷ 2

So the total electron pairs = 26 ÷ 2 = 13

• Third, determine the central atom

Here hydrogen can not be the central atom. Because the central atom is bonded with at least two other atoms, and hydrogen has only one electron in its last shell, so it can not make more than one bond.

Now we have to choose the central atom from chlorine and oxygen. Place the least electronegative atom at the center.

Since chlorine is less electronegative than oxygen, assume that the central atom is chlorine.

Therefore, place chlorine in the center and hydrogen and oxygen on either side.

• And finally, draw the rough sketch

#2 Mark lone pairs on the atoms

Here, we have a total of 13 electron pairs. And four bonds are already marked. So we have to only mark the remaining nine electron pairs as lone pairs on the sketch.

Also remember that hydrogen is a period 1 element, so it can not keep more than 2 electrons in its last shell. Chlorine is a period 3 element, so it can keep more than 8 electrons in its last shell. And oxygen is a period 2 element, so it can not keep more than 8 electrons in its last shell.

Always start to mark the lone pairs from outside atoms. Here, the outside atoms are oxygens and hydrogen. But no need to mark on hydrogen, because hydrogen already has two electrons.

So for top oxygen and left oxygen, there are three lone pairs, for right oxygen, there are two lone pairs, and for chlorine, there is one lone pair.

Mark the lone pairs on the sketch as follows:

#3 Calculate and mark formal charges on the atoms, if required

Use the following formula to calculate the formal charges on atoms:

Formal charge = valence electrons – nonbonding electrons – ½ bonding electrons

For hydrogen atom, formal charge = 1 – 0 – ½ (2) = 0

For chlorine atom, formal charge = 7 – 2 – ½ (6) = +2

For top oxygen and left oxygen atom, formal charge = 6 – 6 – ½ (2) = -1

For right oxygen atom, formal charge = 6 – 4 – ½ (4) = 0

Here, both chlorine and oxygen atoms have charges, so mark them on the sketch as follows:

The above structure is not a stable Lewis structure because both chlorine and oxygen atoms have charges. Therefore, reduce the charges (as below) by converting lone pairs to bonds.

#4 Convert lone pairs of the atoms, and minimize formal charges

Convert a lone pair of the left oxygen atom to make a new Cl — O bond with the chlorine atom as follows:

#5 Repeating step 4 to get a stable Lewis structure

Since there are charges on chlorine and oxygen atoms, again convert a lone pair of the top oxygen atom to make a new Cl — O bond with the chlorine atom as follows:

In the above structure, you can see that the central atom (chlorine) forms an octet. The outside atoms (oxygens) also form an octet, and hydrogen forms a duet. Hence, the octet rule and duet rule are satisfied.

Also, the above structure is more stable than the previous structures. Therefore, this structure is the stable Lewis structure of HClO₃.

Next: MnO₄^– Lewis structure

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External links

• https://topblogtenz.com/hclo3-lewis-structure-molecular-geometry-acid-or-base/
• https://lambdageeks.com/hclo3-lewis-structure/
• https://www.thegeoexchange.org/chemistry/bonding/Lewis-Structures/HClO3-lewis-structure.html