H2S or hydrogen sulfide gas is colorless in nature. With many other miscellaneous pet names like sour gas, drain gas, and so on this gas is poisonous and also corrosive together well.

You are watching: Hydrogen sulfide, h2s, has a shape similar to

I am certain you are not expecting a good odor from this gas! well yes, you are right, hydrogen sulfide gas smells like rotten eggs!!

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

H2S has a covalent bond because the sulfur atom completes the octet by sharing 2 electrons with 2 hydrogen atoms and thus creates a covalent bond.

Let us examine these fundamentals through the explanation of the lewis structure of H2S.

H2S Lewis Structure

The lewis framework of H2S is as below.


Now to understand this we need to recognize the steps to attract a lewis framework at first.

First and foremost that is essential to recognize how countless valence electrons are current in the compound.

In this link valence electron will certainly be together following:

Hydrogen valence electron = 12* Hydrogen atom = 2Sulfur’s valence electron = 6Thus total valence electron = 2 + 6 = 8

Now the next work will certainly be, finding the end the central atom.

The main atom is basically the atom through the highest variety of bonding sites. Here, the main atom will be the sulfur atom.

After finding the central atom we should sketch a skeletal structure of H2S with single bonds only.

It’s an excellent to know that lewis framework is all around electrons and also atoms fulfilling your octet. Every atom do the efforts to meet its octet to acquire stability.

In this compound, sulfur has 6 electrons, so to attain octet i.e 8 electrons, it requirements 2 more electrons. Similarly, hydrogen has only 1s shell and also its octet deserve to be filled with 2 electrons only.

Thus hydrogen demands only 1 more electron to get stability.

Now the next task for drawing the lewis structure of H2S will certainly be pour it until it is full up the continuing to be electrons (after the formation of solitary bonds in the sketch) approximately the sulfur atom.

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

For do this whole learning about drawing a Lewis structure, a bit an ext simple, I have jotted under the actions below, in bullets,

Find out the total number of valence electron in the molecule. Do take treatment of +, – indications while calculating.Choose a main atom; normally the atom v the greatest bonding sites.Draw a skeletal structure with solitary bonds only.Fillup the octet of the atoms through the continuing to be electrons. Save in mind to start with the electronegative atoms and also proceed to the electropositive one.Give multiple bonds if forced for fulfilling the octet of the atoms.At critical make sure all the atom are having their lowest feasible formal charge. You can calculate the exact same with the formula provided below


Moving on to the following topic, let’s placed some irradiate on the hybridization the H2S!

H2S Hybridization

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

Drago’s rule – This ascendancy states that no mix of orbitals or we deserve to say no hybridization takes ar if the power difference between the atom orbitals the the atoms is too high.

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

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

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

3. There need to not be any positive charge present in the central atom.

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

Well surely, H2S does pass all the conditions.

The central 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 describes that H2S has actually no hybridization.

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

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

H2S Geometrical Structure

The molecular geometry of H2S is bent.


Another important suggest is the electron geometry that H2S, which is tetrahedral. Now before jumping right into the difference in between these two, let us see how to find them.

So, both the geometries can be found from the VSEPR chart. The graph is fastened below!


From this chart, we have the right to see that H2S is an AX2E2 kind molecule, wherein X represents the neighboring atoms and E represents the lone pairs of the main atom.

Thus, we deserve to say the the molecule geometry of H2S is bent.

Moving come the difference between electron geometry and molecular geometry.

Basically, molecule geometry just takes into account the atom of the molecule while determining the shape. Conversely, electron geometry considers every the electron present.

The later on one considers the lone pair together well, which reasons the significant difference in the shape.

Another suggest to save in psychic is the the repulsion in between the 2 lone pairs in H2S also plays a major role in make its bent molecule geometry.

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

All these explain the molecular geometry of H2S.

H2S Molecular orbital (MO) Diagram

The molecular orbital diagram of H2S have the right 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 certainly be atom orbitals of hydrogen.

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

From a MO diagram of H2S, we can acquire to know about the shortcut order, bond length, and also bond security of the compound as well.

Also, it should be preserved in mind that the vacant orbitals the sulfur and also 1s the hydrogen have actually a large energy difference. Yet the MO diagram deserve to be formed after that as well!

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

Polarity the H2S

The molecule H2S is considered to it is in a polar molecule together the molecule has actually a bending shape. The dipole across both H-S bonds perform not cancel out each other and have a net dipole moment.

For an ext detail, ns request you to likewise read when the write-up on the polarity that H2S.

H2S Preparation

Hydrogen sulfide deserve to be developed in various ways, some of those are,

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

Hydrogen sulfide can be obtained by dealing with hydrogen v molten elemental sulfur at ~450℃.

Lab preparation – reaction ferrous sulfide and also a strong acid in Kipp generator.

FeS + 2HCl ——-> FeCl2 + H2S

Another qualitative analysis, whereby thioacetamide is offered to create H2S.

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

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

Now, us all recognize H2S is offered in plenty of reactions for the formation of various compounds.

See more: What Does Tk316 Mean On A Ring Mean? Tk316: What Is The Stamp On The Inside Of My Ring

For simple understanding of these reactions, we need to first have one idea around the structure, bonding, and hybridization that hydrogen sulfide the are described above!


This write-up revolves approximately the lewis structure, hybridization, bonding the H2S. These points are really essential to know around so the we have the right to learn equations entailing H2S smoothly.

I hope after analysis the post you obtained 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! after ~ all, chemistry is a very vast subject!

If girlfriend have any questions regarding any topic in this article, feel complimentary to ask me the end anytime!