Ready to learn how to draw the lewis structure of S2Cl2?
Here, I have explained 6 simple steps to draw the lewis dot structure of S2Cl2 (along with images).
So, if you are ready to go with these 6 simple steps, then let’s dive right into it!
Lewis structure of S2Cl2 contains a single bond between the two Sulfur (S) atoms as well as between Sulfur (S) & Chlorine (Cl) atoms. The two Sulfur atoms (S) are at the center and they are surrounded by 2 Chlorine atoms (Cl). The Sulfur atoms have 2 lone pairs, while the Chlorine atoms have 3 lone pairs.
Let’s draw and understand this lewis dot structure step by step.
(Note: Take a pen and paper with you and try to draw this lewis structure along with me. I am sure you will definitely learn how to draw lewis structure of S2Cl2).
6 Steps to Draw the Lewis Structure of S2Cl2
Step #1: Calculate the total number of valence electrons
Here, the given molecule is S2Cl2. In order to draw the lewis structure of S2Cl2, first of all you have to find the total number of valence electrons present in the S2Cl2 molecule.
(Valence electrons are the number of electrons present in the outermost shell of an atom).
So, let’s calculate this first.
Calculation of valence electrons in S2Cl2
- For Sulfur:
Sulfur is a group 16 element on the periodic table.
Hence, the valence electrons present in sulfur is 6 (see below image).
- For Chlorine:
Chlorine is a group 17 element on the periodic table.
Hence, the valence electron present in chlorine is 7 (see below image).
Hence in a S2Cl2 molecule,
Valence electrons given by each Sulfur (S) atom = 6
Valence electron given by each Chlorine (Cl) atom = 7
So, total number of Valence electrons in S2Cl2 molecule = 6(2) + 7(2) = 26
Step #2: Select the center atom
While selecting the center atom, always put the least electronegative atom at the center.
(Remember: Fluorine is the most electronegative element on the periodic table and the electronegativity decreases as we move right to left in the periodic table as well as top to bottom in the periodic table).
Here in the S2Cl2 molecule, if we compare the sulfur atom (S) and chlorine atom (Cl), then sulfur is less electronegative than chlorine.
So, both the sulfur atoms should be placed in the center and the remaining 2 chlorine atoms will surround it.
Step #3: Put two electrons between the atoms to represent a chemical bond
Now in the above sketch of S2Cl2 molecule, put the two electrons (i.e electron pair) between the sulfur-sulfur atoms and sulfur-chlorine atoms to represent a chemical bond between them.
These pairs of electrons present between the Sulfur atoms as well as between the Sulfur and Chlorine atoms form a chemical bond, which bonds these atoms with each other in a S2Cl2 molecule.
Step #4: Complete the octet (or duplet) on outside atoms. If the valence electrons are left, then put the valence electrons pair on the central atom
Don’t worry, I’ll explain!
In the Lewis structure of S2Cl2, the outer atoms are chlorine atoms.
So now, you have to complete the octet on these chlorine atoms (because chlorine requires 8 electrons to have a complete outer shell).
Now, you can see in the above image that all the chlorine atoms form an octet.
Also, only 18 valence electrons of S2Cl2 molecule are used in the above structure.
But there are total 26 valence electrons in S2Cl2 molecule (as calculated in step #1).
So the number of electrons left to be kept on the central atom = 26 – 18 = 8.
So let’s keep these eight electrons (i.e 4 electron pairs) on the central atoms.
Now, let’s move to the next step.
Step #5: Check whether the central atom has octet or not
In this step, we have to check whether the central atoms (i.e two sulfur atoms) have an octet or not.
In simple words, we have to check whether the central Sulfur (S) atoms has 8 electrons or not.
As you can see from the above image, the central atoms (i.e sulfur), has 8 electrons. So they fulfill the octet rule and both the sulfur atoms are stable.
Step #6: Final step – Check the stability of lewis structure by calculating the formal charge on each atom
Now, you have come to the final step and here you have to check the formal charge on sulfur atoms (S) as well as chlorine atoms (Cl).
For that, you need to remember the formula of formal charge;
Formal charge = Valence electrons – Nonbonding electrons – (Bonding electrons)/2
- For Sulfur:
Valence electrons = 6 (as it is in group 16)
Nonbonding electrons = 0
Bonding electrons = 8
- For Chlorine:
Valence electrons = 7 (as it is in group 17)
Nonbonding electrons = 6
Bonding electrons = 2
|Formal charge||=||Valence electrons||–||Nonbonding electrons||–||(Bonding electrons)/2|
So you can see above that the formal charges on sulfur as well as chlorine are “zero”.
Hence, there will not be any change in the above structure and the above lewis structure of S2Cl2 is the final stable structure only.
Each electron pair (:) in the lewis dot structure of S2Cl2 represents the single bond ( | ). So the above lewis dot structure of S2Cl2 can also be represented as shown below.