H2S or hydrogen sulfide gas is colorless in nature. With countless other miscellaneous pet names prefer sour gas, sewage system gas, and so on this gas is poisonous and also corrosive as well.

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

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

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

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

H2S Lewis Structure

The lewis framework of H2S is together below.


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

First and foremost that is crucial to identify how numerous valence electrons are existing 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 main atom.

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

After finding the central atom we need to sketch a skeletal structure of H2S with solitary bonds only.

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

In this compound, sulfur has actually 6 electrons, so to achieve octet i.e 8 electrons, it demands 2 an ext electrons. Similarly, hydrogen has only 1s shell and also its octet have the right to be filled through 2 electron only.

Thus hydrogen needs only 1 more electron to get stability.

Now the following task for drawing the lewis structure of H2S will certainly be filling up the staying electrons (after the development of solitary bonds in the sketch) around the sulfur atom.

Lastly, we need to check that every atoms are having their lowest feasible formal charge to complete the lewis framework of H2S.

For making this entirety learning about drawing a Lewis structure, a bit much more simple, I have actually jotted down the measures below, in bullets,

Find the end the total variety of valence electrons in the molecule. Carry out take treatment of +, – indicators while calculating.Choose a central atom; typically the atom v the greatest bonding sites.Draw a skeletal framework with single bonds only.Fillup the octet that the atoms with the staying electrons. Store in mind to start with the electronegative atoms and proceed come the electropositive one.Give multiple bonds if required for fulfilling the octet of the atoms.At last make sure all the atoms are having actually their lowest possible formal charge. You deserve to calculate the exact same with the formula given below


Moving on to the following topic, let’s put some light on the hybridization that H2S!

H2S Hybridization

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

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

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

1. The central atom need to be existing in the third period or below the third period, through at the very least one lone pair.

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

3. There have to not be any type of positive charge present in the main atom.

This rule is valid because that 6 molecule 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 optimistic charge. Also, the electronegativity the hydrogen is 2.1.

Thus this explains that H2S has actually no hybridization.

Moreover, including to this rule, an additional factor is the the vacant orbital of Sulfur and also 1s orbital of Hydrogen has actually a very large energy difference.

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

H2S Geometrical Structure

The molecule geometry of H2S is bent.


Another important allude is the electron geometry that H2S, which is tetrahedral. Now prior to jumping right into the difference in between these two, let us see exactly how to uncover them.

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


From this chart, we can see that H2S is one AX2E2 type molecule, wherein X represents the bordering atoms and E to represent the lone pairs of the central atom.

Thus, we can say the the molecule geometry that H2S is bent.

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

Basically, molecular geometry only 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 causes the significant difference in the shape.

Another allude to store in mind is that the repulsion between the 2 lone pairs in H2S likewise plays a significant role in do its bent molecular geometry.

The repulsion changes the bond bag from a straight to bent shape.

All these define the molecular geometry that H2S.

H2S Molecular orbit (MO) Diagram

The molecular orbital diagram the H2S have the right to be described in the following way.


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

And on 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 are vacant and bonding orbitals space filled.

From a MO diagram of H2S, us can gain to know about the bond order, link length, and also bond security of the compound as well.

Also, it need to be kept in mind that the vacant orbitals the sulfur and also 1s the hydrogen have a big energy difference. But the MO diagram deserve to be created after that as well!

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

Polarity of H2S

The molecule H2S is thought about to it is in a polar molecule as the molecule has a bent shape. The dipole across both H-S bonds carry out not cancel out each other and have a net dipole moment.

For an ext detail, i request girlfriend to also read when the short article on the polarity of H2S.

H2S Preparation

Hydrogen sulfide deserve to be created in various ways, several of those are,

The many common means is the preparation from cake gas (any gas having high H2S content).

Hydrogen sulfide have the right to be derived by treating hydrogen with molten element sulfur at ~450℃.

Lab ready – reaction ferrous sulfide and a solid acid in Kipp generator.

FeS + 2HCl ——-> FeCl2 + H2S

Another qualitative analysis, wherein thioacetamide is provided to develop 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, we all know H2S is used in numerous reactions because that the formation of various compounds.

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For an easy understanding of these reactions, we need to an initial have one idea about the structure, bonding, and hybridization the hydrogen sulfide the are described above!


This post revolves roughly the lewis structure, hybridization, bonding that H2S. These points are very essential to know about so the we can learn equations involving H2S smoothly.

I hope after reading the post you obtained a tiny bit of knowledge about this compound. Though over there is a lot much more to learn, it’s great to go action by step! ~ all, chemistry is a very substantial subject!

If you have any kind of questions about any topic in this article, feel totally free to ask me out anytime!