Lewis structure of H2O2

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The Lewis structure of H₂O₂ contains three single bonds, with two oxygens in the center, and each oxygen is attached with one hydrogen. There are two lone pairs on each oxygen atom, and the hydrogen atom does not have any lone pair.

Steps

By using the following steps, you can easily draw the Lewis structure of H₂O₂:

#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)

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 and oxygen is a group 16 element. Hence, hydrogen has one valence electron and oxygen has six valence electrons.

Now H₂O₂ has two hydrogen atoms and two oxygen atoms.

So the total number of valence electrons = (valence electrons of hydrogen atom × 2) + (valence electrons of oxygen atom × 2)

Therefore, the total number of valence electrons = 2 + 12 = 14

• 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 oxygen as the central atom.

But there are two oxygen atoms in H₂O₂. Hence, we can assume any one as the central atom. Let’s assume that right oxygen is the central atom.

So now, put two oxygens in the center and two hydrogens on either side. And draw the rough skeleton structure for the Lewis structure of H₂O₂ something like this:

Also read: How to draw Lewis structure of ClO₃^– (5 steps)

#2 Show chemical bond

Place two electrons between the atoms to show a chemical bond. Since two oxygens are surrounded by two hydrogens, use six electrons to show three chemical bonds as follows:

Also read: How to draw Lewis structure of CH₂Cl₂ (4 steps)

#3 Mark lone pairs

As calculated earlier, we have a total of 14 valence electrons. And in the above structure, we have already used six valence electrons. Hence, eight valence electrons are remaining.

Two valence electrons represent one lone pair. So eight valence electrons = four lone pairs.

Note that hydrogen is a period 1 element, so it can not keep more than 2 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 hydrogens and left oxygen. 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 will get two lone pairs. And the central atom (right oxygen) will also get two lone pairs.

Now draw the Lewis structure of H₂O₂ something like this:

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

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

Also read: How to draw Lewis structure of PCl₅ (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 each hydrogen atom

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

Formal charge = 1 – 0 – ½ (2) = 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 H₂O₂ looks something like this:

In the above structure, you can see that the formal charges of both (hydrogen and oxygen) are zero. Therefore, this is the stable Lewis structure of H₂O₂.

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

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Related

• Lewis structure of ClO₃^–
• Lewis structure of CH₂Cl₂
• Lewis structure of PCl₅
• Lewis structure of C₂H₆
• Lewis structure of CHCl₃

External video

• H2O2 Lewis Structure – How to Draw the Dot Structure for H2O2 – Wayne Breslyn

External links

• How to Draw the Dot Structure for H2O2 – Pinterest
• H2O2 Lewis Structure, Hybridization, Molecular Geometry and Bond Angle – Geometry of Molecules
• H2O2 molecular geometry, lewis structure, bond angle, hybridization – Topblogtenz
• H2O2 Lewis Structure in 6 Steps (With Images) – Pediabay
• What is the Lewis structure for H2O2? – Homework.Study.com
• H2O2 Lewis Structure, Molecular Geometry, Hybridization, and Polarity – Techiescientist
• Hydrogen Peroxide (H2O2) Lewis Structure – Chemistry School
• H2O2 Lewis Structure – Kemicalinfo
• Chemical Bonding: H2O2 Lewis Structure – The Geoexchange
• Drawing the Lewis Structure for H2O2 – The University of Maryland
• Construct a lewis structure for hydrogen peroxide, h2o2, in which each atom achieves an octet of electrons – Brainly
• Construct a Lewis structure for hydrogen peroxide – Chegg
• How can you determine the Lewis dot structure of H2O2? – Quora
• Draw a Lewis dot electron dot structure for a molecule of hydrogen peroxide, H2O2 – Quizlet
• Draw a Lewis dot electron dot structure for a molecule of hydrogen peroxide, H2O2 – Bartleby