So you have seen the above image by now, right?
Let me explain the above image in short.
SCl2 lewis structure has a Sulfur atom (S) at the center which is surrounded by two Chlorine atoms (Cl). There are 2 single bonds between the Sulfur atom (S) and each Chlorine atom (Cl). There are 2 lone pairs on the Sulfur atom (S) and 3 lone pairs on both the Chlorine atoms (Cl).
If you haven’t understood anything from the above image of SCl2 (sulfur dichloride) lewis structure, then just stick with me and you will get the detailed step by step explanation on drawing a lewis structure of SCl2.
So let’s move to the steps of drawing the lewis structure of SCl2.
Steps of drawing SCl2 lewis structure
Step 1: Find the total valence electrons in SCl2 molecule
In order to find the total valence electrons in SCl2 (sulfur dichloride) 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 SCl2 molecule
→ Valence electrons given by sulfur atom:
You can see the 6 valence electrons present in the sulfur atom as shown in the above image.
→ Valence electrons given by chlorine atom:
You can see the 7 valence electrons present in the chlorine atom as shown in the above image.
Total valence electrons in SCl2 molecule = valence electrons given by 1 sulfur atom + valence electrons given by 2 chlorine atoms = 6 + 7(2) = 20.
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 SCl2 (sulfur dichloride) and it contains sulfur atom (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 atom (S) is 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 SCl2 molecule, you have to put the electron pairs between the sulfur atom (S) and chlorine atoms (Cl).
This indicates that the sulfur (S) and chlorine (Cl) are chemically bonded with each other in a SCl2 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 SCl2 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 SCl2 molecule.
The SCl2 molecule has a total 20 valence electrons and out of these, only 16 valence electrons are used in the above sketch.
So the number of electrons which are left = 20 – 16 = 4.
You have to put these 4 electrons on the central sulfur atom in the above sketch of SCl2 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 atom (S) is stable or not.
In order to check the stability of the central chlorine (Cl) atom, we have to check whether it is forming an octet or not.
You can see from the above picture that the sulfur atom is forming an octet. That means it has 8 electrons.
And hence the central sulfur atom is stable.
Now let’s proceed to the final step to check whether the lewis structure of SCl2 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 SCl2.
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) atom as well as chlorine (Cl) atoms present in the SCl2 molecule.
For calculating the formal charge, you have to use the following formula;
Formal charge = Valence electrons – (Bonding electrons)/2 – Nonbonding electrons
For Sulfur (S) atom:
Valence electrons = 6 (because sulfur is in group 16)
Bonding electrons = 4
Nonbonding electrons = 4
For Chlorine (Cl) atom:
Valence electron = 7 (because chlorine is in group 17)
Bonding electrons = 2
Nonbonding electrons = 6
From the above calculations of formal charge, you can see that the sulfur (S) atom as well as chlorine (Cl) atom has a “zero” formal charge.
This indicates that the above lewis structure of SCl2 is stable and there is no further change in the above structure of SCl2.
In the above lewis dot structure of SCl2, you can also represent each bonding electron pair (:) as a single bond (|). By doing so, you will get the following lewis structure of SCl2.
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:
|H2SO4 lewis structure
|Ethanol (C2H5OH) lewis structure
|BeF2 lewis structure
|OH- lewis structure
|N2H2 lewis structure
|CH3Cl lewis structure
Jay is an educator and has helped more than 100,000 students in their studies by providing simple and easy explanations on different science-related topics. He is a founder of Pediabay and is passionate about helping students through his easily digestible explanations.
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