The **Lewis structure of S _{2}Cl_{2}** 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.

## Steps

By using the following steps, you can easily draw the Lewis structure of S_{2}Cl_{2}.

#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 S_{2}Cl_{2} 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 S_{2}Cl_{2} something like this:

**Also read:** How to draw Lewis structure of XeF_{6} (4 steps)

### #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:

**Also read:** How to draw Cl^{–} Lewis structure (3 steps)

### #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 S_{2}Cl_{2} looks something like this:

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.

**Also read:** How to draw Lewis structure of IBr (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 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 S_{2}Cl_{2} looks something like this:

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 S _{2}Cl_{2}**.

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

## Related

- Lewis structure of XeF
_{6} - Cl
^{–}Lewis structure - Lewis structure of IBr
- Lewis structure of SbF
_{5} - Lewis structure of C
_{5}H_{12}

## External links

- Chemical Bonding: S2Cl2 Lewis Structure – The Geoexchange
- S2Cl2 Lewis Structure in 6 Steps (With Images) – Pediabay
- What is the molecular geometry of S (sulfur) in S2CL2? – Quora
- For s2cl2 draw an appropriate lewis structure (clsscl) – Brainly
- Draw and explain the Lewis structure for S2Cl2 – Homework.Study.com
- For S2Cl2 draw an appropriate Lewis structure (ClSSCl) – Chegg
- How do you determine the bond angle of S2Cl2? – Socratic
- Sulfur monochloride | S2Cl2 | CID 24807 – National Institutes of Health (.gov)
- Determine the geometry of S2Cl2 using VSEPR theory – Studocu
- Are S2Cl2 and SCl the same thing? – Physics Forums
- What is structure of sulfur monochloride S2Cl2? – Answers
- Draw the electron dot structures for S2Cl2 (ClSSCl) then determine the molecular geometry (use either S) – Numerade
- S2Cl2 (Disulfur Dichloride) Oxidation Number – ChemicalAid
- Determine if disulfur dichloride, S2Cl2, is polar or nonpolar – Pearson

Deep

Rootmemory.com was founded by Deep Rana, who is a mechanical engineer by profession and a blogger by passion. He has a good conceptual knowledge on different educational topics and he provides the same on this website. He loves to learn something new everyday and believes that the best utilization of free time is developing a new skill.