H2S MOLECULAR GEOMETRY HOW TO

The left-hand side will contain the atomic orbitals of sulfur i.e 3s2 3px2 3py1 3pz1.Īnd on the right-hand side, there will be atomic orbitals of hydrogen.Ĩ valence electrons are filled in the MO orbitals. The molecular orbital diagram of H2S can be explained in the following way. The repulsion changes the bond pairs from a straight to bent shape.Īll these explain the molecular geometry of H2S. The later one considers the lone pair as well, which causes the major difference in the shape.Īnother point to keep in mind is that the repulsion between the 2 lone pairs in H2S also plays a major role in making its bent molecular geometry. Whereas electron geometry considers all the electrons present. Moving to the difference between electron geometry and molecular geometry.īasically, molecular geometry only takes into account the atoms of the molecules while determining the shape. Thus, we can say that the molecular geometry of H2S is bent. The chart is attached below!įrom this chart, we can see that H2S is an AX2E2 type molecule, where X represents the surrounding atoms and E represents the lone pairs of the central atom. So, both the geometries can be found from the VSEPR chart.

H2S MOLECULAR GEOMETRY HOW TO

Now before jumping into the difference between these two, let us see how to find them. Thus, this is another explanation saying, H2S has no hybridization.Īnother important point is the electron geometry of H2S, which is tetrahedral. Moreover, adding to this rule, another factor is that the vacant orbital of Sulfur and 1s orbital of Hydrogen has a very large energy difference.

Thus this explains that H2S has no hybridization. Also, the electronegativity of hydrogen is 2.1. The central atom i.e sulfur is in the 3rd period, it has 2 lone pairs and no positive charge. Well surely, H2S does pass all the conditions. This rule is valid for 6 molecules ie PH3, AsH3, SbH3, H2S, H2Se, H2Te There should not be any positive charge present in the central atom. The surrounding atoms should have electronegativity below or equal to 2.5.ģ. The central atom must be present in the 3rd period or below the 3rd period, with at least one lone pair.Ģ. There are certain conditions for this rule to come into action, they are-ġ. So there will be no hybridization of the central atom. Moving on to the next topic, let’s put some light on the hybridization of H2S!Īccording to Drago’s rule, H2S has no hybridization.ĭrago’s Rule – This rule states that no mixing of orbitals or we can say no hybridization takes place if the energy difference between the atomic orbitals of the atoms is too high. You can calculate the same with the formula given below Step 6: At last make sure all the atoms are having their lowest possible formal charge. Step 5: Give multiple bonds if required for fulfilling the octet of the atoms. Keep in mind to start with the electronegative atoms and proceed to the electropositive one. Step 4: Fill up the octet of the atoms with the remaining electrons. Step 3: Draw a skeletal structure with single bonds only. Step 2: Choose a central atom generally the atom with the highest bonding sites. Do take care of +, – signs while calculating. Step 1: Find out the total number of valence electrons in the molecule. Lastly, we need to check that all atoms are having their lowest possible formal charge to complete the lewis structure of H2S.įor making this whole learning about drawing a Lewis structure, a bit more simple, I have jotted down the steps below. Now the next task for drawing the lewis structure of H2S will be filling up the remaining electrons (after the formation of single bonds in the sketch) around the sulfur atom. Thus hydrogen needs only 1 more electron to gain stability. Similarly, hydrogen has only 1s shell and its octet can be filled with 2 electrons only. In this compound, sulfur has 6 electrons, so to attain octet i.e 8 electrons, it needs 2 more electrons. Every atom tries to fulfill its octet to attain stability. It’s good to know that lewis structure is all about electrons and atoms fulfilling their octet. Here, the central atom will be the sulfur atom.Īfter finding the central atom we need to sketch a skeletal structure of H2S with single bonds only. The central atom is basically the atom with the highest number of bonding sites. Now the next work will be, finding out the central atom. In this compound valence electron will be as following: Now to understand this we need to know the steps to draw a lewis structure at first.įirst and foremost it is important to determine how many valence electrons are present in the compound.

H2s molecular geometry