H2O2 Lewis Structure in 6 Steps (With Images)

So you have seen the above image by now, right?

Let me explain the above image in short.

H2O2 (hydrogen peroxide) lewis structure has a single bond between the two Oxygen atoms (O) as well as between the Oxygen atom (O) and Hydrogen atom (H). There are 2 lone pairs on both the Oxygen atoms (O).

If you haven’t understood anything from the above image of H2O2 (hydrogen peroxide) lewis structure, then just stick with me and you will get the detailed step by step explanation on drawing a lewis structure of H2O2.

So let’s move to the steps of drawing the lewis structure of H2O2.

Steps of drawing H2O2 lewis structure

Step 1: Find the total valence electrons in H2O2 molecule

In order to find the total valence electrons in H2O2 molecule, first of all you should know the valence electrons present in hydrogen atom as well as oxygen atom.
(Valence electrons are the electrons that are present in the outermost orbit of any atom.)

Here, I’ll tell you how you can easily find the valence electrons of hydrogen as well as oxygen using a periodic table.

Total valence electrons in H2O2 molecule

→ Valence electrons given by hydrogen atom:

Hydrogen is group 1 element on the periodic table. ^[1] Hence the valence electron present in hydrogen is 1.

You can see that only 1 valence electron is present in the hydrogen atom as shown in the above image.

→ Valence electrons given by oxygen atom:

Oxygen is group 16 element on the periodic table. ^[2] Hence the valence electrons present in oxygen is 6.

You can see the 6 valence electrons present in the oxygen atom as shown in the above image.

Hence, 

Total valence electrons in H2O2 molecule = valence electrons given by 2 hydrogen atoms + valence electrons given by 2 oxygen atoms = 1(2) + 6(2) = 14.

Step 2: Select the central atom

For selecting the center atom, you have to remember that the atom which is less electronegative remains at the center.

(Remember: If hydrogen is present in the given molecule, then always put hydrogen outside.)

Now here the given molecule is H2O2 (or hydrogen peroxide) and it contains hydrogen atoms (H) and oxygen atoms (O).

You can see the electronegativity values of hydrogen atom (H) and oxygen atom (O) in the above periodic table.

If we compare the electronegativity values of hydrogen (H) and oxygen (O) then the hydrogen atom is less electronegative. But as per the rule we have to keep hydrogen outside.

So here both the oxygen atoms (O) are the center atom and the hydrogen atoms (H) are the outside atoms.

Step 3: Connect each atoms by putting an electron pair between them

Now in the H2O2 molecule, you have to put the electron pairs between the oxygen-oxygen atoms and between the oxygen-hydrogen atoms.

This indicates that these atoms are chemically bonded with each other in a H2O2 molecule.

Step 4: Make the outer atoms stable. Place the remaining valence electrons pair on the central atom.

Now in this step, you have to check the stability of the outer atoms.

Here in the sketch of H2O2 molecule, you can see that the outer atoms are hydrogen atoms.

These outer hydrogen atoms are forming a duplet and hence they are stable. 

Also, in step 1 we have calculated the total number of valence electrons present in the H2O2 molecule.

The H2O2 molecule has a total 14 valence electrons and out of these, only 8 valence electrons are used in the above sketch.

So the number of electrons which are left = 14 – 8 = 6.

You have to put these 6 electrons on both the central oxygen atoms in the above sketch of H2O2 molecule.

Now let’s proceed to the next step.

Step 5: Check the octet on the central atom

In this step, you have to check whether the central oxygen atoms (O) are stable or not.

In order to check the stability of the central oxygen (O) atoms, we have to check whether they are forming an octet or not.

You can see from the above picture that the oxygen atoms are forming an octet. That means they have 8 electrons.

And hence the central oxygen atoms are stable.

Now let’s proceed to the final step to check whether the lewis structure of H2O2 is stable or not.

Step 6: Check the stability of lewis structure

Now you have come to the final step in which you have to check the stability of lewis structure of H2O2.

The stability of lewis structure can be checked by using a concept of formal charge.

In short, now you have to find the formal charge on hydrogen (H) atoms as well as oxygen (O) atoms present in the H2O2 molecule.

For calculating the formal charge, you have to use the following formula;

Formal charge = Valence electrons – (Bonding electrons)/2 – Nonbonding electrons

You can see the number of bonding electrons and nonbonding electrons for each atom of H2O2 molecule in the image given below.

For Hydrogen (H) atom:
Valence electron = 1 (because hydrogen is in group 1)
Bonding electrons = 2
Nonbonding electrons = 0

For Oxygen (O) atom:
Valence electrons = 6 (because oxygen is in group 16)
Bonding electrons = 4
Nonbonding electrons = 4

Formal charge	=	Valence electrons	–	(Bonding electrons)/2	–	Nonbonding electrons
H	=	1	–	2/2	–	0	=	0
O	=	6	–	4/2	–	4	=	0

From the above calculations of formal charge, you can see that the hydrogen (H) atoms as well as oxygen (O) atoms have a “zero” formal charge.

This indicates that the above lewis structure of H2O2 is stable and there is no further change in the above structure of H2O2.

In the above lewis dot structure of H2O2, you can also represent each bonding electron pair (:) as a single bond (|). By doing so, you will get the following lewis structure of H2O2.

I hope you have completely understood all the above steps.

For more practice and better understanding, you can try other lewis structures listed below.

Try (or at least See) these lewis structures for better understanding:

CH2Cl2 lewis structure	ClO2- lewis structure
ClO3- lewis structure	HCl lewis structure
H2 lewis structure	N3- lewis structure