Lewis structure of S2Cl2

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Lewis structure of S2Cl2
Lewis structure of S2Cl2

The Lewis structure of S2Cl2 contains three single bonds, with two sulfurs in the center, and each sulfur is attached with one chlorine. There are three lone pairs on each chlorine atom, and two lone pairs on each sulfur atom.


By using the following steps, you can easily draw the Lewis structure of S2Cl2.

#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… sulfur is a group 16 element and chlorine is a group 17 element. Hence, sulfur has six valence electrons and chlorine has seven valence electrons.

Now S2Cl2 has two sulfur atoms and two chlorine atoms.

So the total number of valence electrons = (valence electrons of sulfur atom × 2) + (valence electrons of chlorine atom × 2)

Therefore, the total number of valence electrons = 12 + 14 = 26

  • Now decide the central atom

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

Electronegativity value of sulfur = 2.58
Electronegativity value of chlorine = 3.16

Obviously, sulfur is less electronegative than chlorine. Hence, assume that right sulfur is the central atom (as there are two sulfurs).

So now, put two sulfurs in the center and two chlorines on either side. And draw the rough skeleton structure for the Lewis structure of S2Cl2 something like this:

Skeleton structure for Lewis structure of S2Cl2

#2 Show chemical bond

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

Three chemical bonds shown between atoms

#3 Mark lone pairs

As calculated earlier, we have a total of 26 valence electrons. And in the above structure, we have already used six valence electrons. Hence, twenty valence electrons are remaining.

Two valence electrons represent one lone pair. So twenty valence electrons = ten lone pairs.

Note that both (sulfur and chlorine) are the period 3 elements, so they can keep more than 8 electrons in their 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 chlorines and left sulfur, so each chlorine will get three lone pairs. And left sulfur and the central atom (right sulfur) will get two lone pairs.

So the Lewis structure of S2Cl2 looks something like this:

Lone pairs marked on Lewis structure of S2Cl2

In the above structure, you can see that the octet is completed on the central atom (right sulfur), 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.

#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 sulfur atom

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

Formal charge = 6 – 4 – ½ (4) = 0

  • For each chlorine atom

Valence electrons = 7
Nonbonding electrons = 6
Bonding electrons = 2

Formal charge = 7 – 6 – ½ (2) = 0

Mention the formal charges of atoms on the structure. So the Lewis structure of S2Cl2 looks something like this:

Formal charges are calculated, and got the stable Lewis structure of S2Cl2

In the above structure, you can see that the formal charges of both (sulfur and chlorine) are zero. Therefore, this is the stable Lewis structure of S2Cl2.

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


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