Lewis structure of HClO4

The information on this page is ✔ fact-checked.

The Lewis structure of HClO₄ contains three double bonds and two single bonds, with chlorine in the center, and hydrogen and four oxygens on either side. There are two lone pairs on each oxygen atom, and chlorine atom and hydrogen atom do not have any lone pair.

Steps

By using the following steps, you can easily draw the Lewis structure of HClO₄.

#1 Draw skeleton
#2 Show chemical bond
#3 Mark lone pairs
#4 Calculate formal charge and check stability (if octet is already completed on central atom)
#5 Convert lone pair and calculate formal charge again (if formal charges are not closer to zero)

Let’s one by one discuss each step in detail.

#1 Draw skeleton

In this step, first calculate the total number of valence electrons. And then, decide the central atom.

• Let’s calculate the total number of valence electrons

We know that… hydrogen is a group 1 element, chlorine is a group 17 element, and oxygen is a group 16 element. Hence, hydrogen has one valence electron, chlorine has seven valence electrons, and oxygen has six valence electrons.

Now HClO₄ has one hydrogen atom, one chlorine atom, and four oxygen atoms.

So the total number of valence electrons = valence electrons of hydrogen atom + valence electrons of chlorine atom + (valence electrons of oxygen atom × 4)

Therefore, the total number of valence electrons = 1 + 7 + 24 = 32

• Now decide the central atom

We can not assume hydrogen as 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.

Therefore, choose the central atom from chlorine and oxygen.

The atom with the least electronegative value is placed at the center. By looking at the periodic table, we get the electronegativity values for chlorine and oxygen as follows:

Electronegativity value of chlorine = 3.16
Electronegativity value of oxygen = 3.44

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

So now, put chlorine in the center and hydrogen and oxygens on either side. And draw the rough skeleton structure for the Lewis structure of HClO₄ something like this:

Also read: How to draw Lewis structure of MnO₄^– (5 steps)

#2 Show chemical bond

Place two electrons between the atoms to show a chemical bond. Since chlorine is surrounded by hydrogen and four oxygens, use ten electrons to show five chemical bonds as follows:

#3 Mark lone pairs

As calculated earlier, we have a total of 32 valence electrons. And in the above structure, we have already used ten valence electrons. Hence, twenty-two valence electrons are remaining.

Two valence electrons represent one lone pair. So twenty-two valence electrons = eleven lone pairs.

Note 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.

Also, make sure that you start marking these lone pairs on outside atoms first. And then, on the central atom.

The outside atoms are hydrogen and oxygens. But hydrogen can not keep more than 2 electrons in its last shell. Hence, don’t mark the lone pairs on hydrogen.

So left oxygen, top oxygen, and bottom oxygen will get three lone pairs. The right oxygen will get two lone pairs, and the central atom (chlorine) will not get any lone pair, because all eleven lone pairs are used.

Now draw the Lewis structure of HClO₄ something like this:

In the above structure, you can see that the octet is completed on the central atom (chlorine), and also on the outside atoms. Therefore, the octet rule is satisfied.

Now calculate the formal charge and check the stability of the above structure.

Also read: How to draw Lewis structure of XeCl₂ (4 steps)

#4 Calculate formal charge and check stability

The following formula is used to calculate the formal charges on atoms:

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

Collect the data from the above structure and then, write it down below as follows:

• For hydrogen atom

Valence electrons = 1
Nonbonding electrons = 0
Bonding electrons = 2

Formal charge = 1 – 0 – ½ (2) = 0

• For chlorine atom

Valence electrons = 7
Nonbonding electrons = 0
Bonding electrons = 8

Formal charge = 7 – 0 – ½ (8) = -1

• For left oxygen, top oxygen, and bottom oxygen atom

Valence electrons = 6
Nonbonding electrons = 6
Bonding electrons = 2

Formal charge = 6 – 6 – ½ (2) = -1

• For right oxygen atom

Valence electrons = 6
Nonbonding electrons = 4
Bonding electrons = 4

Formal charge = 6 – 4 – ½ (4) = 0

Mention the formal charges of atoms on the structure. So the Lewis structure of HClO₄ looks something like this:

In the above structure, you can see that the formal charges of atoms are not closer to zero. Therefore, convert lone pair and calculate formal charge again.

Also read: How to draw Lewis structure of SeCl₄ (4 steps)

#5 Convert lone pair and calculate formal charge again

As mentioned earlier, chlorine is a period 3 element, so it can keep more than 8 electrons in its last shell.

So convert one lone pair from the left oxygen atom, top oxygen atom, and bottom oxygen atom to make a new bond with the chlorine atom. And then, the Lewis structure of HClO₄ looks something like this:

Now one last thing we need to do is, calculate the formal charge again and check the stability of the above structure.

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

Collect the data from the above structure and then, write it down below as follows:

• For hydrogen atom

Valence electrons = 1
Nonbonding electrons = 0
Bonding electrons = 2

Formal charge = 1 – 0 – ½ (2) = 0

• For chlorine atom

Valence electrons = 7
Nonbonding electrons = 0
Bonding electrons = 14

Formal charge = 7 – 0 – ½ (14) = 0

• For each oxygen atom

Valence electrons = 6
Nonbonding electrons = 4
Bonding electrons = 4

Formal charge = 6 – 4 – ½ (4) = 0

Mention the formal charges of atoms on the structure. So the Lewis structure of HClO₄ looks something like this:

In the above structure, you can see that the formal charges of all atoms are zero. Therefore, this is the stable Lewis structure of HClO₄.

And each horizontal line drawn in the above structure represents a pair of bonding valence electrons.

📝 Your feedback matters. Visit our contact page.

Related

• Lewis structure of MnO₄^–
• Lewis structure of XeCl₂
• Lewis structure of SeCl₄
• Lewis structure of SeS₂
• Lewis structure of TeCl₄

External links

• HClO4 Lewis Structure in 6 Steps (With Images) – Pediabay
• How is the Lewis structure of HClO4 determined? – Quora
• Lewis structure for HClO4 – Reddit
• Draw the Lewis structure of HClO4 – Chegg
• Lewis structure for HClO4 – ECHEMI
• Perchloric Acid | HClO4 | CID 24247 – National Institutes of Health (.gov)
• Draw the Lewis structure of HClO4 where the structure obeys octet rule – Numerade
• HClO4 (Perchloric Acid) Oxidation Number – ChemicalAid
• HClO4 Best Resonance Structure – Chemical Forums
• Perchloric acid | HClO4 – ChemSpider