SCl2 Lewis structure

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SCl₂ (sulfur dichloride) has one sulfur atom and two chlorine atoms.

In the SCl₂ Lewis structure, there are two single bonds around the sulfur atom, with two chlorine atoms attached to it. Each chlorine atom has three lone pairs, and the sulfur atom has two lone pairs.

Steps

To properly draw the SCl₂ Lewis structure, follow these steps:

#1 Draw a rough sketch of the structure
#2 Next, indicate lone pairs on the atoms
#3 Indicate formal charges on the atoms, if necessary

Let’s break down each step in more detail.

#1 Draw a rough sketch of the structure

• 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 SCl₂ has one sulfur atom and two chlorine atoms, so…

Valence electrons of one sulfur atom = 6 × 1 = 6
Valence electrons of two chlorine atoms = 7 × 2 = 14

And the total valence electrons = 6 + 14 = 20

Learn how to find: Sulfur valence electrons and Chlorine valence electrons

• Second, find the total electron pairs

We have a total of 20 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 = 20 ÷ 2 = 10

• 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 sulfur.

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

• And finally, draw the rough sketch

#2 Next, indicate lone pairs on the atoms

Here, we have a total of 10 electron pairs. And two S — Cl bonds are already marked. So we have to only mark the remaining eight 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.

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

Mark the lone pairs on the sketch as follows:

#3 Indicate formal charges on the atoms, if necessary

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

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

For 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.

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

Therefore, this structure is the stable Lewis structure of SCl₂.

Next: PF₅ Lewis structure

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External links

• https://geometryofmolecules.com/scl2-lewis-structure-molecular-geometry-hybridization-bond-angle-and-shape/
• https://topblogtenz.com/scl2-lewis-structure-molecular-geometry-polarity/
• https://techiescientist.com/scl2-lewis-structure/
• https://www.chemistryscl.com/general/SCl2-lewis-structure/
• https://www.thegeoexchange.org/chemistry/bonding/Lewis-Structures/SCl2-lewis-structure.html
• https://lambdageeks.com/scl2-lewis-structure/
• https://sciedutut.com/scl2-lewis-structure/