Lewis Structure of CF2S (With 6 Simple Steps to Draw!)

Lewis Structure of CF2S

Ready to learn how to draw the lewis structure of CF2S?

Awesome!

Here, I have explained 6 simple steps to draw the lewis dot structure of CF2S (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 CF2S contains a double bond between the Carbon (C) & Sulfur (S) atom and two single bonds between Carbon (C) & Fluorine (F) atoms. The Carbon atom (C) is at the center and it is surrounded by two Fluorine (F) and one Sulfur atom (S).

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 CF2S).

6 Steps to Draw the Lewis Structure of CF2S

Step #1: Calculate the total number of valence electrons

Here, the given molecule is CF2S. In order to draw the lewis structure of CF2S, first of all you have to find the total number of valence electrons present in the CF2S 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 CF2S

  • For Carbon:

Carbon is a group 14 element on the periodic table.

Hence, the valence electrons present in carbon is 4 (see below image).

  • For Fluorine: 

Fluorine is a group 17 element on the periodic table.

Hence, the valence electrons present in fluorine is 7 (see below image).

  • For Sulfur:

Sulfur is a group 16 element on the periodic table.

Hence, the valence electrons present in sulfur is 6 (see below image).

Hence in a CF2S molecule, 

Valence electrons given by Carbon (C) atom = 4
Valence electrons given by each Fluorine (F) atom = 7
Valence electrons given by Sulfur (S) atom = 6
So, total number of Valence electrons in CF2S molecule = 4 + 7(2) + 6 = 24

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 CF2S molecule, if we compare the carbon atom (C), sulfur atom (S) and fluorine atom (F), then the carbon is less electronegative.

So, carbon should be placed in the center and the sulfur atom as well as fluorine atom will surround it.

step 1

Step #3: Put two electrons between the atoms to represent a chemical bond

Now in the above sketch of CF2S molecule, put the two electrons (i.e electron pair) between the carbon-sulfur  atoms and carbon-fluorine atoms to represent a chemical bond between them.

step 2

These pairs of electrons present between the Carbon & Sulfur atoms as well as between the Carbon & Fluorine atoms form a chemical bond, which bonds these atoms with each other in a CF2S 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 CF2S, the outer atoms are fluorine atoms and sulfur atom.

You also have to see whether the sulfur atom as well as fluorine atoms are forming an octet or not! (because sulfur and fluorine both require 8 electrons to have a complete outer shell).

step 3

You can see in the above image that both the fluorine atoms as well as one sulfur atom forms an octet.

Also, all the 24 valence electrons of CF2S molecule (as calculated in step #1) are used in the above structure. So there are no remaining electron pairs.

Hence there is no change in the above sketch of CF2S.

Let’s move to the next step.

Step #5: Check whether the central atom has octet or not. If it does not have an octet, then move the electron pair from the outer atom to form a double bond or triple bond

In this step, we have to check whether the central atom (i.e carbon) has an octet or not. 

In simple words, we have to check whether the central Carbon (C) atom has 8 electrons or not.

step 4

As you can see from the above image, the central atom (i.e carbon) has only 6 electrons. So it does not fulfill the octet rule.

Now, in order to fulfill the octet of a carbon atom, we have to move the electron pair from the outer atom (i.e sulfur atom) to form a double bond.

step 5

Now you can see from the above image that the central atom (i.e carbon), is having 8 electrons. So it fulfills the octet rule.

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 carbon atom (C), sulfur (S) atom as well as fluorine atoms (F).

For that, you need to remember the formula of formal charge;

Formal charge = Valence electrons – Nonbonding electrons – (Bonding electrons)/2

step 6
  • For Carbon:
    Valence electrons = 4 (as it is in group 14)
    Nonbonding electrons = 0
    Bonding electrons = 8
  • For Sulfur:
    Valence electron = 6 (as it is in group 16)
    Nonbonding electrons = 4
    Bonding electrons = 4
  • For Fluorine:
    Valence electron = 7 (as it is in group 17)
    Nonbonding electrons = 6
    Bonding electrons = 2
Formal charge=Valence electronsNonbonding electrons(Bonding electrons)/2
C=408/2=0
S=644/2=0
F=762/2=0

So you can see above that the formal charges on carbon, sulfur as well as fluorine are “zero”.

Hence, there will not be any change in the above structure and the above lewis structure of CF2S is the final stable structure only.

Each electron pair (:) in the lewis dot structure of CF2S represents the single bond ( | ). So the above lewis dot structure of CF2S can also be represented as shown below.

cf2s lewis structure

(Note: In step 5, if we had moved the electron pair from the fluorine atom, then there will be +1 and -1 charges on fluorine and sulfur respectively. But here we move the electron pair from the sulfur atom, which gives the more stable structure (having “zero” charges on all the atoms.))

Related lewis structures for your practice:
Lewis Structure of PI5
Lewis Structure of SO2F2
Lewis Structure of OPBr3
Lewis Structure of PH2-
Lewis Structure of NS2 

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