S2Cl2 Lewis Structure

S2Cl2 Lewis Structure

S2Cl2 (disulfur dichloride) has two sulfur atoms and two chlorine atoms. In the lewis structure of S2Cl2, there is a single bond between the two sulfur atoms, and each sulfur is attached with one chlorine atom. Each chlorine atom has three lone pairs, and each sulfur atom has two lone pairs.

Steps

Here’s how you can draw the S2Cl2 lewis structure step by step.

Step #1: draw sketch
Step #2: mark lone pairs
Step #3: mark charges (if there are)

Let’s break down each step in detail.

#1 Draw Sketch

  • First, determine the total number of valence electrons

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

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

Since S2Cl2 has two sulfur atoms and two chlorine atoms, so…

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

And the total valence electrons = 12 + 14 = 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 sulfur is less electronegative than chlorine, assume that the central atom is right sulfur (as there are two sulfur atoms present here).

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

  • And finally, draw the rough sketch
S2Cl2 Lewis Structure (Step 1)

#2 Mark Lone Pairs

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 both (sulfur and chlorine) are the period 3 elements, so they can keep more than 8 electrons in their last shell.

Always start to mark the lone pairs from outside atoms. Here, the outside atoms are chlorines and left sulfur.

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

Mark the lone pairs on the sketch as follows:

S2Cl2 Lewis Structure (Step 2)

#3 Mark Charges

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

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

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

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

Here, both sulfur and chlorine atoms do not have charges, so no need to mark the charges.

And in the above structure, you can see that the central atom (right sulfur) forms an octet. Hence, the octet rule is satisfied.

Therefore, this structure is the stable lewis structure of S2Cl2.

Next: IBr Lewis Structure

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