Lewis Structure of SOF2 (With 6 Simple Steps to Draw!)

Lewis Structure of SOF2

I’m super excited to teach you the lewis structure of SOF2 in just 6 simple steps.

Infact, I’ve also given the step-by-step images for drawing the lewis dot structure of SOF2 molecule.

So, if you are ready to go with these 6 simple steps, then let’s dive right into it!

Lewis structure of SOF2 contains a double bond between the Sulfur (S) & Oxygen (O) atom and two single bonds between Sulfur (S) & Fluorine (F) atoms. The Sulfur atom (S) is at the center and it is surrounded by two Fluorine (F) and one Oxygen atom (O).

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 SOF2).

6 Steps to Draw the Lewis Structure of SOF2

Step #1: Calculate the total number of valence electrons

Here, the given molecule is SOF2. In order to draw the lewis structure of SOF2, first of all you have to find the total number of valence electrons present in the SOF2 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 SOF2

  • 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 Oxygen:

Oxygen is a group 16 element on the periodic table.

Hence, the valence electron present in oxygen is 6 (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).

Hence in a SOF2 molecule, 

Valence electrons given by Sulfur (S) atom = 6
Valence electrons given by Oxygen (O) atom = 6
Valence electrons given by each Fluorine (F) atom = 7
So, total number of Valence electrons in SOF2 molecule = 6 + 6 + 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 SOF2 molecule, if we compare the sulfur atom (S), oxygen atom (O) and fluorine atom (F), then the sulfur is less electronegative.

So, sulfur should be placed in the center and the oxygen 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 SOF2 molecule, put the two electrons (i.e electron pair) between the sulfur-oxygen atoms and sulfur-fluorine atoms to represent a chemical bond between them.

step 2

These pairs of electrons present between the Sulfur & Oxygen atoms as well as between the Sulfur & Fluorine atoms form a chemical bond, which bonds these atoms with each other in a SOF2 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 SOF2, the outer atoms are fluorine atoms and oxygen atom.

You also have to see whether the oxygen atom as well as fluorine atoms are forming an octet or not! (because oxygen 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 oxygen atom forms an octet.

Also, only 24 valence electrons of SOF2 molecule are used in the above structure.

But there are total 26 valence electrons in SOF2 molecule (as calculated in step #1).

So the number of electrons left to be kept on the central atom = 26 – 24 = 2.

So let’s keep these 2 electrons (i.e 1 electron pairs) on the central atom.

step 4

Now, 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 sulfur) has an octet or not. 

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

step 5

As you can see from the above image, the central atom (i.e sulfur), has 8 electrons. So it fulfills the octet rule and the sulfur atom is 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 atom (S), oxygen (O) 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 Sulfur:
    Valence electrons = 6 (as it is in group 16)
    Nonbonding electrons = 2
    Bonding electrons = 6
  • For Oxygen:
    Valence electron = 6 (as it is in group 16)
    Nonbonding electrons = 6
    Bonding electrons = 2
  • 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
S=626/2=+1
O=662/2=-1
F=762/2=0

So you can see above that the formal charges on sulfur is +1 and the formal charge on the oxygen atom is -1.

step 7

This indicates that the above lewis structure of SOF2 is not stable and so we have to minimize the charges to get a more stable lewis structure.

This can be done by shifting the lone pair from negatively charged oxygen atom to the positively charged sulfur atom to form a bond.

step 8

Now, in the above structure, you can see that the charges are minimized and the above lewis structure of SOF2 is the final stable structure.

Each electron pair (:) in the lewis dot structure of SOF2 represents the single bond ( | ). So the above lewis dot structure of SOF2 can also be represented as shown below.

sof2 lewis structure

Related lewis structures for your practice:
Lewis Structure of SeBr4
Lewis Structure of BrCl2-
Lewis Structure of CF2S
Lewis Structure of PI5
Lewis Structure of SO2F2 

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