S2Cl2 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.

S2Cl2 lewis structure has a single bond between the two Sulfur atoms (S) and as well as between the Sulfur atom (S) and Chlorine atoms (Cl). There are 2 lone pairs on the Sulfur atoms (O) and 3 lone pairs on the Chlorine atoms (Cl).

If you haven’t understood anything from the above image of S2Cl2 lewis structure, then just stick with me and you will get the detailed step by step explanation on drawing a lewis structure of S2Cl2.

So let’s move to the steps of drawing the lewis structure of S2Cl2.

Steps of drawing S2Cl2 lewis structure

Step 1: Find the total valence electrons in S2Cl2 molecule

In order to find the total valence electrons in a S2Cl2 molecule, first of all you should know the valence electrons present in sulfur atom as well as chlorine 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 sulfur as well as chlorine using a periodic table.

Total valence electrons in S2Cl2 molecule

→ Valence electrons given by sulfur atom:

Sulfur is a group 16 element on the periodic table. ^[1] Hence the valence electrons present in sulfur is 6.

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

→ Valence electrons given by chlorine atom:

Chlorine is group 17 element on the periodic table. ^[2] Hence the valence electrons present in chlorine is 7.

You can see the 7 valence electrons present in the chlorine atom as shown in the above image.

Hence, 

Total valence electrons in S2Cl2 molecule = valence electrons given by 2 sulfur atom + valence electrons given by 2 chlorine atoms = 6(2) + 7(2) = 26.

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.

Now here the given molecule is S2Cl2 and it contains sulfur atoms (S) and chlorine atoms (Cl).

You can see the electronegativity values of sulfur atom (S) and chlorine atom (Cl) in the above periodic table.

If we compare the electronegativity values of sulfur (S) and chlorine (Cl) then the sulfur atom is less electronegative.

So here, the sulfur atoms (S) are the center atom and the chlorine atoms (Cl) are the outside atoms.

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

Now in the S2Cl2 molecule, you have to put the electron pairs between the sulfur-sulfur atoms and between the sulfur-chlorine atoms.

This indicates that these atoms are chemically bonded with each other in a S2Cl2 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 S2Cl2 molecule, you can see that the outer atoms are chlorine atoms.

These outer chlorine atoms are forming an octet and hence they are stable. 

Also, in step 1 we have calculated the total number of valence electrons present in the S2Cl2 molecule.

The S2Cl2 molecule has a total 26 valence electrons and out of these, only 18 valence electrons are used in the above sketch.

So the number of electrons which are left = 26 – 18 = 8.

You have to put these 8 electrons on both the central sulfur atoms in the above sketch of S2Cl2 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 sulfur atoms (S) are stable or not.

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

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

And hence the central sulfur atoms are stable.

Now let’s proceed to the final step to check whether the lewis structure of S2Cl2 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 S2Cl2.

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 sulfur (S) atoms as well as chlorine (Cl) atoms present in the S2Cl2 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 S2Cl2 molecule in the image given below.

For Sulfur (S) atom:
Valence electrons = 6 (because sulfur is in group 16)
Bonding electrons = 4
Nonbonding electrons = 4

For Chlorine (Cl) atom:
Valence electrons = 7 (because chlorine is in group 17)
Bonding electrons = 2
Nonbonding electrons = 6

Formal charge	=	Valence electrons	–	(Bonding electrons)/2	–	Nonbonding electrons
S	=	6	–	4/2	–	4	=	0
Cl	=	7	–	2/2	–	6	=	0

From the above calculations of formal charge, you can see that the sulfur (S) atoms as well as chlorine (Cl) atoms have a “zero” formal charge.

This indicates that the above lewis structure of S2Cl2 is stable and there is no further change in the above structure of S2Cl2.

In the above lewis dot structure of S2Cl2, you can also represent each bonding electron pair (:) as a single bond (|). By doing so, you will get the following lewis structure of S2Cl2.

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:

BeBr2 Lewis Structure	CSe2 Lewis Structure
BrCl Lewis Structure	AsCl3 Lewis Structure
C2H2Br2 Lewis Structure	SbCl5 Lewis Structure