# Cl2O2 Lewis structure

Cl2O2 (chlorine peroxide) has two chlorine atoms and two oxygen atoms.

In Cl2O2 Lewis structure, there is a single bond between the two oxygen atoms, and each oxygen is attached with one chlorine atom. Each chlorine atom has three lone pairs, and each oxygen atom has two lone pairs.

Contents

## Steps

Here’s how you can easily draw the Cl2O2 Lewis structure step by step:

#1 Draw a rough skeleton structure
#2 Mention lone pairs on the atoms
#3 If needed, mention formal charges on the atoms

Now, let’s take a closer look at each step mentioned above.

### #1 Draw a rough skeleton structure

• First, determine the total number of valence electrons

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

Hence, chlorine has seven valence electrons and oxygen has six valence electrons.

Since Cl2O2 has two chlorine atoms and two oxygen atoms, so…

Valence electrons of two chlorine atoms = 7 × 2 = 14
Valence electrons of two oxygen atoms = 6 × 2 = 12

And the total valence electrons = 14 + 12 = 26

• 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

We have to place the least electronegative atom at the center.

Since chlorine is less electronegative than oxygen, the central atom should be chlorine, right?

But if we place chlorine in the center and oxygen outside, and calculate the formal charge, then we do not get the formal charges on atoms closer to zero.

And the structure with the formal charges on atoms closer to zero is the best Lewis structure.

Hence, here we have to assume that the central atom is oxygen. But there are two oxygen atoms, so we can assume any one as the central atom.

Let’s assume that the central atom is left oxygen.

Therefore, place oxygens in the center and chlorines on either side.

• And finally, draw the rough sketch

### #2 Mention lone pairs on the atoms

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

Also remember that 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 chlorines and right oxygen.

So for each chlorine, there are three lone pairs, for each oxygen, there are two lone pairs.

Mark the lone pairs on the sketch as follows:

### #3 If needed, mention formal charges on the atoms

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

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

For each chlorine atom, formal charge = 7 – 6 – ½ (2) = 0

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

Here, the atoms do not have charges, so no need to mark the charges.

In the above structure, you can see that the central atom (left oxygen) forms an octet. And the outside atoms (right oxygen and chlorines) also form an octet. Hence, the octet rule is satisfied.

Therefore, this structure is the stable Lewis structure of Cl2O2.

Next: XeI2 Lewis structure