H2S or hydrogen sulfide gas is colorless in nature. With many other miscellaneous pet names prefer sour gas, sewage system gas, etc this gas is poisonous and also corrosive together well.

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I am sure you room not expecting a great odor native this gas! fine yes, you are right, hydrogen sulfide gas smells favor rotten eggs!!

The molar fixed of H2S is 34.08 g/mol and also its thickness is 1.363 g dm-3. The melting allude and boiling point of H2S are -82℃ and -60℃ respectively.

H2S has actually a covalent bond because the sulfur atom completes its octet by share 2 electrons through 2 hydrogen atoms and thus forms a covalent bond.

I have likewise written specifically on it, check out the write-up on the covalent binding of H2S.

Let us inspect these fundamentals through the explanation that the lewis framework of H2S.

H2S Lewis Structure

The lewis framework of H2S is together below.


Now to understand this we need to understand the procedures to draw a lewis structure at first.

First and foremost the is essential to determine how plenty of valence electron are present in the compound.

In this link valence electron will be as following:

Hydrogen valence electron = 1

2* Hydrogen atom = 2

Sulfur’s valence electron = 6

Thus total valence electron = 2 + 6 = 8

Now the next work will be, finding out the main atom.

The main atom is basically the atom v the highest number of bonding sites. Here, the central atom will certainly be the sulfur atom.

After recognize the main atom we have to sketch a skeletal framework of H2S with single bonds only.

It’s good to know that lewis structure is all around electrons and also atoms fulfilling their octet. Every atom tries to accomplish its octet to obtain stability.

In this compound, sulfur has 6 electrons, therefore to obtain octet i.e 8 electrons, it requirements 2 an ext electrons. Similarly, hydrogen has actually only 1s shell and its octet can be filled through 2 electron only.

Thus hydrogen needs only 1 an ext electron to gain stability.

Now the following task for drawing the lewis framework of H2S will be filling up the staying electrons (after the formation of solitary bonds in the sketch) roughly the sulfur atom.

Lastly, we require to examine that every atoms are having their lowest possible formal fee to complete the lewis structure of H2S.

For make this totality learning around drawing a Lewis structure, a bit much more simple, I have actually jotted under the measures below.

Step 1: find out the total number of valence electrons in the molecule. Do take care of +, – indications while calculating.

Step 2: Choose a main atom; usually the atom v the highest bonding sites.

Step 3: attract a skeletal structure with single bonds only.

Step 4: Fill upthe octet of the atoms with the staying electrons. Keep in psychic to begin with the electronegative atoms and proceed come the electropositive one.

Step 5: Give multiple binding if compelled for fulfilling the octet that the atoms.

Step 6: At critical make sure all the atom are having actually their lowest possible formal charge. You deserve to calculate the very same with the formula provided below


Moving on come the following topic, let’s put some irradiate on the hybridization the H2S!

H2S Hybridization

According come Drago’s rule, H2S has actually no hybridization.

Drago’s dominion – This dominance states the no mixing of orbitals or we deserve to say no hybridization takes location if the energy difference in between the atom orbitals the the atom is also high.

So there will certainly be no hybridization that the main atom. Over there are details conditions because that this ascendancy to come right into action, castle are-

1. The main atom have to be present in the 3rd period or below the 3rd period, through at least one lone pair.

2. The neighboring atoms should have electronegativity below or equal to 2.5.

3. There need to not be any positive charge existing in the main atom.

This preeminence is valid for 6 molecules ie; PH3, AsH3, SbH3, H2S, H2Se, H2Te

Well surely, H2S does happen all the conditions.

The main atom i.e sulfur is in the 3rd period, it has 2 lone pairs and also no positive charge. Also, the electronegativity the hydrogen is 2.1.

Thus this defines that H2S has actually no hybridization.

Moreover, adding to this rule, another factor is the the vacant orbit of Sulfur and also 1s orbital of Hydrogen has actually a very huge energy difference.

So over there is no hybrid orbit formation. Thus, this is another explanation saying, H2S has no hybridization.

H2S Geometrical Structure

The molecular geometry that H2S is bent.


Another important allude is the electron geometry of H2S, i m sorry is tetrahedral. Now before jumping right into the difference in between these two, let us see just how to uncover them.

So, both the geometries deserve to be found from the VSEPR chart. The chart is enclosed below!


From this chart, we can see that H2S is one AX2E2 kind molecule, whereby X represents the bordering atoms and also E represents the lone pairs of the central atom.

Thus, we have the right to say that the molecule geometry the H2S is bent.

Moving to the difference in between electron geometry and also molecular geometry.

Basically, molecule geometry just takes into account the atom of the molecule while identify the shape. Whereas electron geometry considers all the electrons present.

The later on one considers the lone pair as well, which causes the major difference in the shape.

Another suggest to store in mind is the the repulsion in between the 2 lone pairs in H2S likewise plays a major role in making its bent molecule geometry.

The repulsion changes the bond bag from a directly to bend shape.

All these explain the molecule geometry that H2S.

H2S Molecular orbital (MO) Diagram

The molecular orbital diagram that H2S deserve to be described in the adhering to way.


This is the MO diagram of H2S. The left-hand side will contain the atom orbitals that sulfur i.e 3s2 3px2 3py1 3pz1.

And top top the right-hand side, there will be atomic orbitals of hydrogen.

8 valence electrons room filled in the MO orbitals. There room two non-bonding orbitals current as well. The anti-bonding orbitals space vacant and bonding orbitals are filled.

From a MO chart of H2S, we can gain to know around the shortcut order, link length, and also bond security of the compound together well.

Also, it must be kept in mind the the vacant orbitals the sulfur and 1s the hydrogen have actually a big energy difference. Yet the MO diagram can be formed after that as well!

let us additionally study the preparation techniques of H2S in the below subtopic.

Polarity of H2S

The molecule H2S is thought about to be a polar molecule as the molecule has actually a bending shape. The dipole across both H-S binding does no cancel the end each other and also has a network dipole moment.

For more detail, ns request girlfriend to additionally read once the write-up on the polarity the H2S.

H2S Preparation

Hydrogen sulfide deserve to be created in different ways, some of those are,

The most common way is the ready from tart gas (any gas having actually high H2S content).

Hydrogen sulfide can be acquired by treating hydrogen with molten elemental sulfur at ~450℃.

Lab ready – reacting ferrous sulfide and also a strong acid in Kipp generator.

FeS + 2HCl ——-> FeCl2 + H2S

Another qualitative analysis, where thioacetamide is used to develop H2S.

CH3C(S)NH2 + H2O ———> CH3C(O)NH2 + H2S

6 H2O + Al2S3 ——–> 3H2S +2 Al(OH)3 is an additional reaction for development of hydrogen sulfide.

Now, us all know H2S is provided in numerous reactions because that the formation of different compounds.

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For basic understanding of these reactions, we require to very first have an idea about the structure, bonding, and hybridization of hydrogen sulfide the are explained above!


This post revolves roughly the lewis structure, hybridization, bonding the H2S. These things are very essential come know around so that we have the right to learn equations entailing H2S smoothly.

I hope after analysis the short article you gained a little bit that knowledge about this compound. Though over there is a lot more to learn, it’s good to go step by step! ~ all, chemistry is a very large subject!

If friend have any questions regarding any subject in this article, feel totally free to asking me the end anytime!