Lewis Structure of H2S (With 6 Simple Steps to Draw!)

I’m super excited to teach you the lewis structure of H2S in just 6 simple steps.

Infact, I’ve also given the step-by-step images for drawing the lewis dot structure of H2S molecule.

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

Lewis structure of H2S contains single bonds between the Sulfur (S) atom and each Hydrogen (H) atom. The Sulfur atom (S) is at the center and it is surrounded by 2 Hydrogen atoms (H). The Sulfur atom have 2 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 H2S).

6 Steps to Draw the Lewis Structure of H2S

Step #1: Calculate the total number of valence electrons

Here, the given molecule is H2S (dihydrogen sulfide). In order to draw the lewis structure of H2S, first of all you have to find the total number of valence electrons present in the H2S 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 H2S

• For Hydrogen: 

Hydrogen is a group 1 element on the periodic table. ^[1]

Hence, the valence electron present in hydrogen is 1 (see below image).

• For Sulfur:

Sulfur is a group 16 element on the periodic table. ^[2]

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

Hence in a H2S molecule, 

Valence electron given by each Hydrogen (H) atom = 1
Valence electrons given by Sulfur (S) atom = 6
So, total number of Valence electrons in H2S molecule = 1(2) + 6 = 8

Step #2: Select the center atom (H is always outside)

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). ^[3]

Here in the H2S molecule, if we compare the hydrogen atom (H) and sulfur atom (S), then hydrogen is less electronegative than sulfur. But as per the rule, we have to keep hydrogen outside.

So, sulfur should be placed in the center and the remaining 2 hydrogen atoms will surround it.

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

Now in the above sketch of H2S molecule, put the two electrons (i.e electron pair) between the sulfur atom and each hydrogen atom to represent a chemical bond between them.

These pairs of electrons present between the Sulfur (S) and Hydrogen (H) atoms form a chemical bond, which bonds the sulfur and hydrogen atoms with each other in a H2S 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 H2S, the outer atoms are hydrogen atoms.

So now, you have to check whether these hydrogen atoms are forming a duplet or not! (because hydrogen requires only 2 electrons to have a complete outer shell).

You can see in the above image that all the hydrogen atoms form a duplet.

Also, only 4 valence electrons of H2S molecule are used in the above structure.

But there are total 8 valence electrons in H2S molecule (as calculated in step #1).

So the number of electrons left to be kept on the central atom = 8 – 4 = 4.

So let’s keep these 4 electrons (i.e 2 electron pairs) on the central atom (i.e sulfur 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 sulfur atom (S) as well as each hydrogen atom (H).

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

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

• For Hydrogen:
  Valence electron = 1 (as it is in group 1)
  Nonbonding electrons = 0
  Bonding electrons = 2
• For Sulfur:
  Valence electrons = 6 (as it is in group 16)
  Nonbonding electrons = 4
  Bonding electrons = 4

Formal charge	=	Valence electrons	–	Nonbonding electrons	–	(Bonding electrons)/2
H	=	1	–	0	–	2/2	=	0
S	=	6	–	4	–	4/2	=	0

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

Hence, there will not be any change in the above structure and the above lewis structure of H2S is the final stable structure only.

Each electron pair (:) in the lewis dot structure of H2S represents the single bond ( | ). So the above lewis dot structure of H2S can also be represented as shown below.

Related lewis structures for your practice:
Lewis structure of OF2
Lewis structure of NF3
Lewis structure of CCl4
Lewis structure of CS2
Lewis structure of SF6

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