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

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

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

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

Lewis structure of SHF contains a single bond between the Hydrogen (H) & Sulfur (S) atom as well as between the Sulfur (S) and Fluorine (F) atom. The Sulfur atom (S) is at the center and it is surrounded by Hydrogen and Fluorine atom. The Sulfur has 2 lone pairs and the Fluorine has 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 SHF).

6 Steps to Draw the Lewis Structure of SHF

Step #1: Calculate the total number of valence electrons

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

• 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 Hydrogen: 

Hydrogen is a group 1 element on the periodic table.

Hence, the valence electron present in hydrogen is 1 (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 SHF molecule, 

Valence electrons given by Sulfur (S) atom = 6
Valence electron given by Hydrogen (H) atom = 1
Valence electrons given by Fluorine (F) atom = 7
So, total number of Valence electrons in SHF molecule = 6 + 1 + 7 = 14

Step #2: Make the rough sketch

From the chemical formula itself, you can get the idea that a sulfur atom will be at the center and it is surrounded by Hydrogen (H) and Fluorine (F) on the outer sides.

So let’s draw a rough sketch for the SHF molecule.

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

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

These pairs of electrons present between the Hydrogen (H), Sulfur (S) and Fluorine (F) atoms form a chemical bond, which bonds these atoms with each other in a SHF 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 SHF, the outer atoms are hydrogen atom and fluorine atom.

Hydrogen already has a duplet (see below image).

So now, you have to complete the octet on fluorine atom (because fluorine requires 8 electrons to have a complete outer shell).

Now, you can see in the above image that the fluorine atom forms an octet.

Also, only 10 valence electrons of SHF molecule are used in the above structure.

But there are total 14 valence electrons in SHF molecule (as calculated in step #1).

So the number of electrons left to be kept on the central atom = 14 – 10 = 4.

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

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 is having 8 electrons or not.

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 hydrogen atom (H), sulfur atom (S) as well as fluorine atom (F).

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

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

• For Hydrogen:
  Valence electrons = 1 (as it is in group 1)
  Nonbonding electrons = 0
  Bonding electrons = 2
• 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 electrons	–	Nonbonding electrons	–	(Bonding electrons)/2
H	=	1	–	0	–	2/2	=	0
S	=	6	–	4	–	4/2	=	0
F	=	7	–	6	–	2/2	=	0

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

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

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

Related lewis structures for your practice:
Lewis Structure of SeS3
Lewis Structure of IBr5
Lewis Structure of AsI3
Lewis Structure of SbF6-
Lewis Structure of SbCl3 

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