Transcript for:
Hybridization in Chemistry

hi friends are you finding the topic of hybridization complicated in chemistry don't worry you are not alone every fun finds hybridization scary but in this video I'm going to make hybridization super easy for you I'm going to explain the concepts in a very simple way and we are going to do lots of examples and we're going to visualize hybridization together so guys make sure you watch the video till the end and I promise you you will find Hy ization easy after this video before we begin I just want to remind you that do check out the full courses on our website and Android app there you're going to get live classes quizzes mock tests revision notes so guys do check it out links are given below all right now let's dive into the world of hybridization as you know there are many theories in chemistry for Co valent bonding so in the previous videos we have looked at the Lewis Theory and the Lewis Dot Structure then we have also looked at the valance Bond Theory and this video we are going to focus on the next Theory which is about hybridization so the focus in today's video is going to be on hybridization following which there will also be a valence shell electron pair repulsion Theory we'll have a video on that and then the molecular orbital Theory so as scientists discovered you know different things where the theory was not able to explain it they came up with a new Theory so that is how science or chemistry evolves as as we've discussed in earlier videos electrons in the atom live inside orbitals what are these orbitals these are the places in the atom where the probability of finding the electron is maximum as you know there are different kinds of orbitals in an atom for example you have the S orbital which is spherical in shape s for sphere you can remember the p orbital is having this kind of a dumbbell shape the D orbital has a double dumbbell shape then you have the F or oral which is having a more complicated shape so keep these orbitals in mind because in hybridization we're going to talk a lot about these orbitals the valance Bond theory is for calent bonding which explains bonding as the overlapping of these Atomic orbitals if you want to know all the details about Valance Bond Theory do check out my video on that here I'm just going to summarize the main points of valence Bond Theory so what did it say that calent bonds so note we are talking about calent bonds only not ionic bonds they are formed by the overlapping overlapping of the atomic orbitals when the atoms obviously they come close to each other okay now what are the conditions for overlapping so orbitals overlap only when the orbitals are half fit because remember an orbital can have maximum two electrons so this Theory valence Bond Theory says that the orbital should be half filled not completely filled right having one electron so it will overlap with another orbital which is also having one electron in it but then the valence Bond Theory says that no hold on both the electrons cannot have the same spin for the orbitals to overlap they should have opposite spin so if one electron spin is clockwise the other one will have to be anticlockwise and then these two orbitals will overlap now how many kinds of overlap we can have the balance Bond Theory says there are two types of overlaps okay which is called the sigma Bond and Pi Bond so let's look at what is the difference between Sigma and Pi bond in the sigma Bond you have a headon or an axial overlap okay so where the atomic orbitals they overlap along the axis along the same axis and we call this a like a like we say head-on collision this is like a headon overlap so this is forms the sigma Bond so remember Sigma Bond means a headon overlap and example here is so the S orbital it always forms Sigma Bond so you can have this kind of ss overlap or you can have a uh overlap between the S orbital and the p orbital which has a direction right like let's say this is along the Zed axis if I take it along the Zed axis s orbital doesn't have any orientation so an SP overlap is also a headon overlap and forms the sigma bond this is all the valence Bond Theory right which we have studied in the earlier video and then you also have the the lateral overlapping right which is a parallel kind of overlap like this and this forms the pi Bond so in pi Bond you have the parallel overlap or you can say a side by side overlap right side by side overlapping is happening and this can happen between the let's say two P orbitals so this PP orbitals both are let's say along the y axis so we can say this is a py py overlap and this forms your Pi Bond so this was all the valance Bond Theory now we're going to look at the valence Bond theory for the methane molecule and let's try and understand what why hybridization Theory had to come in so first let's see what did the valance Bond theory for methane predict methane you know has the formula CH4 it is the simplest hydrocarbon one carbon four hydrogens now according to valence Bond Theory there is overlapping of the atomic orbitals so let's see what uh orbitals these atoms have so electronic configuration of carbon which is having six electrons will be 1 S2 2 S2 2 P2 right six electrons in it and hydrogen atom you guys know it is having just one electron so very simple configuration 1 S1 so now if we depict this electronic configuration of carbon we can see it will have two electrons in the 2s shell right and then in 2p there is one one electron okay and hydrogen there are four right so there are four hydrogen like this all having one electron in the 1 s orbitals now how will these overlap because there have four hydrogen atoms that want to overlap AP but only two orbitals are half filled the fully filled orbital cannot overlap according to valence Bond Theory so an interesting thing happens is that this electrons get shifted to the 2p orbital and we call this the excited state or the first excited state of carbon so we can say carbon under goes an excitation which I'm going to represent a c star and this electron I'm going to shift over here so I'm going to shift this electron over here now you can see that four orbitals are available for overlapping with these four orbitals and again according to valence Bond Theory they should not have the same spin so I should have really drawn them with the opposite Arrow so it's better to draw these like this that is the correct representation so these will have the opposite spin so now it's all good right these four orbitals 1 2s and 3 2p orbitals can overlap with the four 1s orbitals of hydrogen do you guys agree okay so it's going to look something like this where where you have all these four hydrogen atoms so basically what are we having this guy overlaps with this guy this guy overlaps with this this guy overlaps with this this guy overlaps with this so what kind of bonds do we have here so here you can see that we have a SS overlap this is a SS Bond here we have a 2p and 1s overlap I'm going to say SP Bond right now this this is one is let's say PX py p z right so we can say PX is overlapping with this S1 here again a py with an S so SP and here again a pz with an S so again an SP overlap clear now tell me guys so basically in the methane molecule we can say that the four bonds formed the four bonds formed are of this type SS sp sp and SP right so can you tell me are these four bonds identical are they going to be identical according to Valance Bond the right not according to our prediction according to Valance Bond Theory the answer is going to be no why because three bonds are of the same type they are of an SP overlap this kind of overlap right SP overlap and yes this will form a sigma Bond SS overlap is also a sigma Bond but the shape is definitely going to be different do you guys agree because this is an SS overlap two s orbitals overlapping here an S and P is overlapping so certainly these bonds should be different like this guy has to be different from these guys so three Bond same and one Bond different this is what Valance Bond theory predicts so we all agree that we are expecting different bonds here but but but experimental evidence showed that all the four bonds all the four bonds of methane guys are identical in all respects whether we talk about the bond length the bond energy everything they are all identical so this is where valence Bond Theory fails this is exactly where Valance Bond Theory fails because all these four bonds between the carbon and hydrogen atoms are all identical same so I can represent it like this or we can look at it like this overlapping structure where this red guy is the carbon right and these are the four hydrogens and you can see that the hydrogen are sort of overlapping with the carbons and experiment showed that all the bonds are identical so this is where valence Bond Theory failed and this is where hybridization comes in so this is exactly where hybridization tries to explain the deficiency of the valance Bond Theory and that's what we are going to discuss in this video so let's go on to hybridization the problem that hybridization was trying to solve is that carbon had 1 s and 3 p orbitals so it had these different orbitals and that is why it was predicting different types of bonds so let's try to understand hybridization in a very simple and exciting way and keep in mind that we have this kind of different orbital so we have to solve that problem so we are going to use a simple ice cream example to understand hybridization imagine you have four scoops of i ice cream like this right you have three vanilla Scoops and one chocolate scoop and let's say we have four children who want to eat the ice cream okay they want one scoop scoop each obviously there's going to be a fight some child is going to say or rather maybe all the children are going to say we all want chocolate or there's going to be you know a fight that we want the same ice cream so what will you do what will your solution be you'll say simple I'm going to take all these ice cream Scoops and let's mix them let's blend them together and form four new ice cream Scoops right which will have a flavor of vanilla and chocolate so then all the kids are equal right they're happy now the kids will not fight because he can't say oh you got the better flavor you got the best one right so what will you do you will mix all of these right you'll put it in the blender and you will produce Four Scoops of vanilla chocolate and you'll tell the kids hey this one is more tasty than these individual ones okay so with this fun example you can remember hybridization how what is the analogy here so think it this way let's say these are your P orbitals carbon had three p orbitals and it had one s orbital so let's say your chocolate is the S orbital so if you mix these if you mix these orbitals right what are you doing you are producing four so see number doesn't change we started with Four Scoops we are having four uh Scoops here so you are producing four new identic iCal orbitals and each one having the flavor of vanilla and chocolate so this whole intermixing this whole intermixing of the orbitals to produce right so understand intermixing of different orbitals to produce identical orbitals equal in number this is the concept of hybridization right so now when the sharing happens with the four hydrogen atoms or with the four children you can thing they are all getting a they're sharing with the identical orbitals here and that is why experiment showed that these bonds are identical in all respects so if you keep this idea in mind hybridization is going to be very easy for you so remember this simple ice cream example and this is how you should view hybridization now I'm sure you're thinking that you've shown us the mixing of ice creams how does the mixing of orbitals look like right so let's go back to the shape of the orbital so we were talking about mixing of carbon had 1 s right and 3 p orbitals remember so this could be like a a px or whichever nomenclature you want to use if you want to call this a py a px a pz doesn't matter right you can use whatever naming uh whatever convention you want so we are mixing these four orbitals right so these three are having the same shape and this is an S orbital so when we intermix them we will produce four identical orbitals like this these are the four identical orbitals you can see one 2 3 4 okay and they will have the same shape right same energy same length everything is same about them and these are called as since they were formed by mixing I'm just going to write p over here right so 1 s and 3 PS we say that these orbitals are called sp3 orbitals so we have four such sp3 orbitals clear and they have the identical shape so you will see in the books the hybrid orbitals they are represented with this kind of a lop L shape right and they will have the identical shape and sometimes you'll see also you know it is a full L here Big L followed by a small lobe on the other side so if you take this orbital right so basic idea is that this is the entire orbital it's represented like this with a small lobe on the other side so this represents a hybrid orbital sometimes that small lobe is also neglected so we are representing it like this so there are four such sp3 hybrid orbitals these are hybridization has occurred so we call this the four hybrid orbitals have been formed which are identical so hybridization you can understand is now explaining why the bonds are identical and the other important thing hybridization is explaining the geometry of the compound because it is explaining how these orbitals are aligned how are they arranged because they contain electrons so they will want to repel right each other they want to space out in the maximum way and they will give this kind of a tetrahedral shape so they will be giving this kind of a tetrahedral geometry so keep that in mind we are going to be talking about geometry not shape so that is where you can see the scientists also checked that the methane molecule is having this kind of tetrahedral geometry containing identical bonds and this is beautifully explained by hybridization remember the inter mixing of orbitals to form this tetrahedral geometry which orbitals as we discussed 1s and 3p mix so these all these guys mix together they go into the blender and out like magic comes four sp3 orbitals we call them the sp3 orbitals or the these are your hybrid orbitals and they're Nam like this why because they're formed from 1 s and 3p orbitals so is this crystal clear now that you've understood the basic concept of hybridization and why we need hybridization let's discuss the important points for hybridization so as we have talked about in hybridization the atomic orbitals they combine right or they mix to form a new set of equivalent equivalent means equal orbitals and we call these the the new orbitals as the hybrid orbitals so if you take an example as we have discussed if you have 1 s and let's say three p orbitals and all these guys mix together so all these four orbitals you can see they're mixing together to form these new hybrid orbitals so four hybrid orbitals have been formed here these are your hybrid orbitals and we call them the sp3 orbitals so each one is called the sp3 and these are all equal like we discussed clear the second important point is unlike the pure orbitals the hybrid orbitals are responsible in bond formation what are pure orbitals pure orbitals means before hybridization right so please understand that in hybridization uh first the hybridization happens then the bond formation with the other atoms right so here basically these are your pure orbitals they are not involved in bond formation right otherwise that was valence Bond theory was saying but hybridization says no hold on first Bond formation will not happen overlapping will not happen first hybridization will occur so that you get these equal orbitals and then the bond formation will happen right so hybrid orbitals are forming the bonds so let's say this forms the bond with one hydrogen atom so they're overlapping here this one with the hydrogen again the 1 s right of the hydrogen this with another hydrogen atom and this with another one and these are all the 1s so clear it is the hybrid orbitals that are involved in bond formation not the original orbitals or what you call as the pure orbitals now let's discuss the next point which is very important it says that can any orbitals intermix to form hybrid orbitals so can hybridization happen for any random orbitals the answer is no hybridization happens only only for or this intermixing of orbitals happens only for orbitals having equal or similar SL very slightly different energies if the orbitals have very different energy it cannot happen Okay so these slightly different orbitals only they can intermix and redistribute the energy forming these new orbitals having exactly equal energy and shape so let's understand this with an example so when we were talking about the hybridization of the orbitals in carbon atom right in the formation of methane who were the guys involved remember the configuration of carbon was this right 1 S2 2 S2 2 P2 when it got excited in the first excited state it is 2 s is having one and all the P orbitals have one each right so what are The intermixing Happening Here between the 2s and these three 2p orbitals now since they are in the same shell the 2s and 2p are in the same shell so they are having similar energy so if you look closely here see these three orbitals are identical energy these are all 2p so these are all 2p orbitals they are all equal energy they're different from 2s but since they are in the same shell 2s and 2p in the same shell so we can say they have similar energy right not very very different okay and that is why hybridization can occur because if you can't do hybridization with a 1s and these 2ps right because that will be very different or 1s and some 3p orbital too much difference so here 2s 2p it was absolutely fine right so that is the important thing here which we are trying to stress is that this was a 2s orbital and these guys were the 2p orbitals okay just to tell you which shell they have come from they are of similar energy so naturally I'll just remove the to notation in case it'll be confusing for you so basically reminding you that these are the similar energy and that is why they can intermix and form new orbitals having exactly the same energy these hybrid orbitals this is a very very important point so you cannot have hybridization of random orbitals they should be having similar energy let's discuss some more important points regarding hybridization so as we talked about the number of hybrid orbitals the number of hybrid orbitals it is always equal to the number of atomic orbitals that is before hybridization or we can call them the pure orbitals so as we have discussed if you have four orbitals here 1 s and 3p orbitals so these are your pure orbitals before hybridization when they intermix when they get hybridized how many orbitals are going to be formed that's right it will be the same number right so four combined here to form four hybrid orbitals so note that the number remains same so this is a very simple point it's clear okay the next Point says which we have already discussed that the hybridized orbitals that is the hybrid orbitals formed they are equivalent in energy and shape so all these four orbitals hybrid orbitals formed here they have exactly the same energy same length and same shape okay so they are equivalent the next point is very important because it explains us why hybridization happens because these hybrid orbitals they are more effective in forming stable bonds than the pure atomic orbital so this point is answering why hybridization because you know nature will favor stability if the hybrid orbitals are giving bonds of lower energy right the system is more stable definitely it will prefer that so this is why hybridization or happens right why hybrid orbitals get formed the next point is very very important that the hybrid orbitals they are directed in space in such a way in such a preferred Direction to minimize the repulsion so let's understand this point so once again going to our methane example now these orbitals they're looking like balloons here but basically they contain electrons electrons are spinning inside them like this so now the question is how do they arrange themselves to have minimal repulsion because electrons are negatively charged particles negative negative like charges they repel each other so they want minimum repulsion maximum stability here so how will they arrange themselves they will arrange themselves in this kind of t tedral shape what is tetrahedral shape it is basically you can imagine it is like this where you have this hybrid orbital on top and let's say these three below in fact it's exactly like the tripod that I'm looking at right so my camera is set here on a tripod in a tripod you know there are three legs of the tripod and then the head of uh the the stick holding the camera so this is basically you can imagine the three legs of the tripod and this this is the uh the top holding of the camera this is how these four hybrid orbitals are arranged this is the geometry hybridization is explaining you the geometry and they are spreading themselves in the maximum possible way uh as far away from each other so that the repulsion is minimum clear so this was the goal of hybridization to explain the geometry because it's forming a stable configuration so hybridization is is indicating you very important point the geometry of your molecules not the shape shape we'll talk about later because that depends on the atoms involved right and the bonds formed here we are talking about the shape clear and that is why hybridization is successfully able to explain the tetrahedral shape of uh the tetrahedral again sorry I'm saying shape remember it's geometry it is able to explain the tetrahedral geometry of methane clear that it is formed like this kind of this is the tripod you can see the three here and one over there this is exactly what the uh methane molecules forms and just uh and again the whole goal is you want minimum repulsion maximum stability just like I hope my tripod is more stable so that the camera doesn't fall off right uh otherwise I lose a lot of money so the same thing over here right they want maximum stability so they spread themselves in such a way so that you get uh minimum repulsion maximum stability and it hybridization is explaining you that why the methane molecule is tetrahedral in shape in keep saying shape no no it is explaining you tetrahedral in geometry geometry geometry so please remember that okay because there's a difference between geometry and shape which we'll talk about now let's talk about what is the conditions needed for hybridization to happen okay okay so the first condition is that the orbital should be present in the valent shell of the atom okay so only the valance uh orbitals are hybridized Valance shell you know it means basically the outermost shell the last shell so only they will undergo hybridization the next point is that which we've already discussed orbitals undergoing hybridization they should have almost equal energy okay so you cannot have hybridization if the energy difference is a lot we've already talked about this the third point is that promotion of the electron promotion means remember that excited state so promotion of electrons is not needed so right this is not essential for hybridization so in our carbon example we had talked about that for carbon to undergo bonding one electron gets promoted from the s to the the 2s to the 2p orbital but that is not necessary okay so take a note of that you do not need to have this excited state the fourth Point says that it is not necessary for only half filled orbitals to participate in hybridization so please understand that hybridization can happen in half filled orbitals it could even happen for fully filled orbitals like the lone pairs right or it could also happen for empty orbitals like in the coordinate Bond so please note it could be either half filled it could be completely fill fil fully filled right or it could be empty also these all can form hybrid orbitals very very important point and the last point is very important which says hybridization is only for Sigma bonds and lone pairs remember in Valance Bond Theory what are the two types of bonds so remember in bance bond Theory we talked about the sigma bond which is the headon overlap and the pi bond which is the parallel the side side by side overlap so Pi bond is not involved in hybridization it is only for Sigma bonds or for lone pairs so this is a very important point for you to keep in mind that it is not for pi bonds so these are all the important conditions of hybridization so for hybridization to happen sometimes they can give you a question they can give these conditions will hybridization happen so based on these conditions you can easily answer a yes or no so please note them down till now we have seen one example of hybridization which is in the methane molecule and we saw that was sp3 hybridization but there can be different types of hybridization depending on the number of atomic orbitals that get that are getting hybridized and also the name is given according to that so let's take a look at the different examples so first I'm going to start with the bottom of the slide here we look at the simple hybridization of One S orbital mixing with one p orbital so when these two mix right the inter mixing happens how many hybrid orbitals will be formed there are two pure orbitals so naturally it will form two hybrid orbitals as you can see represented here and this is each hybrid orbital will be called the SP hybrid orbital right so there are two of them and this is known as SP hybridization clear again remember this kind of lobe is representing each lobe is representing one hybrid orbital now what is the geometry here what geometry will you tell here as you can see these two hybrid orbitals will lie flat like this as far away from each other so that again the inter electronic repulsion is minimum and since they're in a straight line This is called the linear shape so as you can see the geometry here is linear this is linear geometry linear because it is lying in a line clear next if you have one One S orbital mixing with two P orbitals so let's say an atom has 2 p orbitals and when these intermix how many orbitals will be formed that's right three because we have three pure orbitals involved in hybridization so on mixing they're going to form three hybrid orbitals and these are labeled as SP2 so each one you can say is SP2 hybrid orbital or we can say this is of the type SP2 hybridization clear and what is the geometry here so when you have three hybrid orbitals they will try to lie as far away from each other in this kind of a triangular shape and you can this imagine this is a plane plane is a flat surface so one hybrid orbital is here one is here one is here and they are lying as far away right uh in this triangular pattern here so that is why this is called triangular planer geometry so let's write that down guys the geometry is triangular planer as you can see it is forming a triangle clear and let me write the linear word here close to SP so note the naming that we are giving it here it was called SP hybridization because only one s and one p was involved here you have 1 s and 2p involved so we write SP2 right two is written like a power so SP2 hybridization is the type and and it gives you a geometry of triangular planum and sp3 hybridization we've already seen in methane in all our slides so you had 1 s and 3 p orbitals of the carbon atom and they were forming this kind of a sp3 hybridization and as we discussed the shape is tetrahedral because they lie in this kind of a tetrahedron pattern again you have to think in 3D here and the example I gave you was of a tripod right so this is how the SP 3 hybridization looks like now can you have more the answer is yes so after sp3 you can have a sp3 d hybridization where there is 1 s 3p and 1 D orbital involved so you can have this one also s sp3 dehybridization right and total how many orbitals hybrid orbitals 1 s 3p and 1 D so see you'll have five hybrid orbitals like this now the question is what is the geometry here again I want you guys to think in 3D so here what is happening is you can see that these three orbitals so look here these three orbitals are forming this kind of a triangular planer structure here so if you imagine this as the plane one is lying like this one like this one like this right so they are forming this triangular planer and the other two orbitals are like this so one up here and one down here clear so this is forming a triangular planer one orbital up like this one down like this so what will the name you uh give to this shape what name are you going to give to this shape so look at this carefully and I want you to think in 3D can you see that this is forming a triangle over here in this plane okay and if you start joining these what kind of shape are you going to form at the top and at the bottom here so again I know this is not a perfect diagram but you need to think in 3D over here so what kind of shape will you form on top so imagine you're joining the top point point to these three points it's going to form a pyramid right like we talk about Pyramids of Giza so what type of pyramid you have over here this pyramid is going to have three faces not four faces 1 2 3 and same one at the bottom because it's joining the triangle so this shape is called triagonal B pyramidal there are two triangular pyramids placed like this clear so this shape will be called Tri trional bipyramidal please check if my spellings are correct so triagonal bipyramidal is uh the geometry again maybe I said shape so again my mistake I keep saying the word shape again shape we're going to talk about later the geometry geometry here is uh sp3d for geometry will be triagonal bamal geometry means how these uh hybrid orbitals are oriented in space it's giving you an idea of how they are arranged in space and then you can have also sp3 and 2 D orbitals involved so sp3d2 hybridization over here right we write it like this so 1 s 3p and 2D that will give us total six hybrid orbitals 1 + 3 + 2 clear and what kind of shape will they take up so if you look over here these four hybrid orbitals like lie over here so we can say that they are forming a sort of a square over here right they are belonging to this square and if you join these the the four orbitals will lie along the sort of the diagonals of the square you can say are you guys getting the idea here one this way one this way one this way one this way so they are forming the diagonals of a square and then the remaining two orbitals one on top one below like this so one on top one below and the four are forming the diagonals of the square so finally what shape are you getting over here you can see that this is the shape of a so if you join these points so how many sides do you get on top you can see one side here two side three side four side because it is a square so if I start joining from this vertex I start drawing these triangles we can see there'll be four sides on top and similarly four sides below again guys remember you have to think this is all in 3D I've drawn it on the board like this it's on a flat surface here but you have to think in 3D so basically one side here one here one here and one here four on top and four below so if you have 4 + 4 eight sides this is called an octahedron so we say the geometry here is octahedral so see the naming of hybridization is very easy right like for example if there's 1 s and 2p it will be called SP2 hybridization the geometry is what you need to remember because every time in the exam you're not going to sit and visualize this so you can remember this way that SP hybridization will give you linear geometry SP2 hybridization Tri triagonal planer right triangular planer geometry sp3 hybridization will give you a tetrahedral geometry sp3d hybridization will give you triagonal bipyramidal right the Triangular pyramids on top and below and this will give you this octahedral because you have a a kind of a square pyramid on top and a square pyramid below so if you count four plus four sides it is eight sides so sp3d2 hybridization gives you octahedral so remember these geometries very very important and the naming of the hybridization is pretty easy clear as we have discussed in hybridization it is basically the intermixing of the atomic orbitals right like we know the S orbital is sperical in shape p orbital has this kind of dumbbells uh dumbbell shape over here and the D orbital has the double dumbbell and F orbital is more complicated we'll not look at that right so these have these orbitals the pure Atomic orbitals have this kind of shape now when they intermix what will be the shape how do we represent the hybrid orbital so here one thing is simple you do not have to learn different shapes like this the hybrid orbitals they are always represented like with a large L and then you'll see a sort of a tiny L sometimes is shown so this is the proper way to represent a hybrid orbital okay one large l and a tiny L but sometimes you know the books neglect the tiny L they only show one single l so if you look at something like that immediately you will know that these are Hy ibrid orbitals and you can see the shape differs from these guys right like this is spherical this is a dumbbell so that is not the same like a don't say that this is a p orbital because p orbital has the big lobe on both sides this has a big lobe and then a small lobe similarly so if you have this kind of uh three Atomic orbitals you'll arrange them like this see okay you'll draw them like this one large L and one small L again one large one small one large one small so this is your SP2 hybridization and as I said many times we neglect the small lob so we sometimes the books just draw it like this so then immediately know yeah this is hybridization because it doesn't look like any of these orbitals it is not the pure Atomic orbitals these are the hybrid orbitals clear now let's look at the examples of hybridization with some real molecules so we are going to start off with SP hybridization and the example we're going to take is berum chloride so let's understand why berum chloride is sp hybridization and what will be its geometry so here the atoms involved are berum and chlorine berium you know has four electrons so its electronic configuration is 1 S2 2 S2 okay chlorine atom has 17 electrons so its configuration is 1 S2 2 S2 2 P6 so that's 10 electrons are done 3 S2 3 p 5 17 electrons clear so let's represent the orbitals here so berum the 2s orbital is going to have two electrons in it right we are again representing only the valent shell same way here the valent shell is shell number three so that is having uh 3s2 so two electrons here in the S orbital and P will have five electrons so one 2 3 4 and I'm purposely going to draw this down for sharing right the with the opposite spin so now how will berum berium chloride form because this is completely filled right so it will not want to overlap with this uh half field orbital for Valance Bond Theory or for overlapping you need the half field so what do we do here so again berum goes into excited state because remember the 2p orbital is empty so this is your 2s and 2p is empty so it will go into excited state the first excited state where the electron will jump from 2s to a 2p or bital so we can draw it like this so one electron goes over here and now berium is ready for forming bonds with chlorine so now you guys can guess that one chlorine atom will form bond with this guy and a second chlorine atom will form a bond with this guy right so this will be the other chlorine will form a bond here so you can see that this will be the overlapping right so one uh 2s orbital will want to overlap here and this thing but hybridization tells us no this is not going to happen because when you have these two different orbitals of similar energy right because you have an A 2s here and a 2p here right or we can say a s orbital here and a p orbital they basically want to mix right because the uh structure formed the molecule form will be more stable lower in energy so there is going to be hybridization over here so since there is one s involved and 1 P what will be the type of hybridization very good it's going to be SP hybridization clear so how will berum look like so basically berium is going to form this two hybrid orbitals right each one is of the type SP hybridized so basically what's happening over here these two orbitals are intermixing to give you two new orbitals and each one is basically like you can think as an SP orbital clear we are calling it SP so now these can overlap with the two chlorines right so the overlapping will happen and chlorine is a orbital of the type p p means what is the shape remember so see p is dumbbell shaped and hybrid orbitals I'm showing with the large lobe and the small lobe again you can ignore the small lobe if you want or if they allow you in school that you don't have to represent small lobe you don't show that so this one is the hybrid orbital and the chlorine atoms p orbital let's draw it here maybe I should have drawn this in green color we were showing all the hybrid orbitals in green green color so let me draw that for you here so this was berium 2 hybrid orbitals okay the sp hybridized sp hybridized and then you will have the two chlorine orbitals which is the p orbital they are having this kind of a dumbbell shape so this is berium and this is the chlorine so simple is this clear to you right because we had two pure orbitals it Formed two hybrid orbitals to give you the SP type hybridization and what do we see here we can see that the structure uh the geometry is going to be linear over here because remember in Sp hybridization what had we discussed automatically if you see SP hybridization you know it will be the type the geometry is going to be linear over here clear and experimentally they have seen so like magic I'll show you so there you can see I had hidden it from you that berium chloride structure looks exactly like this and hybridization explains that this because hybridization is basically explaining us that why doesn't berum choride why doesn't it look something like this you know why not like this or some other weird shape why not something like you know this so the gometry is going to be linear because of this whole hybridization the two orbitals formed are equivalent equal and so they will overlap they will uh be on either side and overlap with the P orbitals of chlorine and this is how you get your SP hybridization is it clear because remember the hybrid orbitals formed here are two SP orbitals and these guys are overlapping with the the two chlorine so there's another of chlorine I'm not drawing it again so that's how the overlapping happens clear so this is how the geometry looks like and that's why when we show berium chloride we draw the molecule like this and this is beautifully explained with our hybridization concept clear now let's look at SP2 hybridization the example of SP2 hybridization we're going to look at is boron chloride again these are examples right so let's see why it is SP2 hybridization and what is its geometry Boron you know has atomic number of five so it's configuration is going to be 1 S2 2 S2 2 P1 right and chlorine as we have discussed it has uh I'm just going to write the three uh third shell so 3 S2 3 P5 that it's electronic configuration now if you draw the atomic orbitals how does it look like so we'll draw for the valance shell uh 2 s over here and 1 p orbital has one electron in it so that's how it looks like this is boron but again you can see the problem because you want three chlorine over there and what is the electronic configuration of chlorine so chlorine I'm drawing the 3p orbital and as we discussed it has one half filed orbital two are completely filled right this is the 3p orbital now you can see there are three chlorine here so three of these guys will want to overlap right with Boron but the problem is there is only one half field orbital so once again we Boron goes into its first excited state where one of the electron jumps so one electron from 2s jumps over here and now you get three half-field orbitals so now it is clear why the uh sharing is going to happen the overlapping is going to happen uh but again before overlapping hybridization Theory says that these you have a 2s and two 2p orbitals are going to combine together to form three hybrid orbitals is it clear so these guys will combine to form you can think this way three hybrid orbitals and these are SP2 1 s and 2p that is why the name is given SP2 and these guys will now be able to overlap with the p orbital of chlorine right because you can imagine there are three of these right clear so what will the geometry look like what will the geometry look like we said that when you have when you have SP2 hybridization it will look like this triangle so triagonal planer right we call this triagonal planer because triangle lying on a plane so let's represent Boron Tri chloride it's going to look like this so with boron in the center here having one oops two see geometry is important I need to draw them in a triangle like this and three so these are boron's uh three hybrid orbitals of boron and they are overlapping with the chlorines so I'm just drawing it roughly here but you guys are getting the picture it is overlapping with the the p orbital the dumbbell shaped orbital of chlorine these are the three chlorine atoms so see hybridization beautifully explains us why Boron chlorides structure should look something like this right triagonal planer this triangular shaped in a plane this is how Boron chloride structure looks like and this is an example of SP2 hybridization and so they're like magic let me show you the molecule here this is your Boron Tri chloride so this is boron in the center and the three chlorine atoms around it and you can see it is matching our expectation this is what we wanted so Boron Tri chloride is a great example of SP2 hybridization giving you a triagonal planer geometry you can have other example also like you can have Boron Tri floride BF3 that will also have the same thing again remember the three SP2 hybrid orbitals are overlapping so one one overlapping with each of the chlorines clear the next example we've already looked at which is SP P3 hybridization and the example we have seen is methane because remember the carbon excited atom so I'll directly write the excited atom it it looks like this where you have four electrons one in the 2s and three in the 2p so these four pure Atomic orbitals are involved in hybridization and as a result it gives you the four sp3 orbitals okay so you can see we are getting four sp3 uh orbitals and these are your hybrid orbitals they are having the equal shape equal energy and they are going to be combining with the hydrogen's uh orbital overlapping with them because hydrogen has only one orbital which is the 1s so each of these guys will combine with the four of hydrogen right because hydrogen has four of them right so don't consider this thing so so the actual overlapping is like this and then this will overlap with another one and so on right so as a result what will we get we will be getting sp3 hybridization and we discussed that is tetrahedral in shape and the scientists have analyzed that yes the methane molecule looks exactly like this it is tetrahedral in shape uh you can see that the uh carbon atom is here in the center you have three hydrogens like this forming this kind of tripod and one hydrogen on top over here so you have to imagine this in 3D this is no longer in a plane so you can imagine the carbon atom here in the center so the three hydrogens are going down like this right and one hydrogen on top over here so this is forming this kind of a tetrahedral geometry because this shape in mathematics is known as a regular tetrahedron clear so sp3 hybridization giving you a tetrahedral geometry next let's look at the example of sp3d hybridization so here you have 1 s 3p and 1 D or ital involved and the example we're going to look at is phosphorus pentac chloride pcl5 so what is the electronic configuration of phosphorus let's start with that phosphorus again I'm going to just show the the valence shell right so it has uh two electrons in the 3s orbital so it is 3s2 three electrons in the 3p orbital and then the D orbital is entirely vacant okay so 3D is entirely vacant now as you can see phosphorus wants to combine with five chlorine so obviously it has to get into an excited state one electron should go from here to here so we are directly going to show the excited state of phosphorus here where there's just one electron here and the that electrons jumps into the 3D orbital again you can see all these orbitals are of similar energy right they are in the third shell so they will undergo hybridization before they overlap with the chlorine atom and chlorine we know it has that one half fill orbital in the 3p shell correct so these guys are going to undergo hybridization and it will Form 1 2 3 4 and five orbitals so we can say these are the sp3 D orbitals of phosphorus this is after hybridization clear and now chlorine atom we know chlorine atom has uh 3 S2 and 3p so this is your 3s and 3p5 so it has five electrons here in the 3p orbital and this one see I'm drawing it with the opposite spin so this is going to be shared right so we can uh understand that the overlapping will happen between the chlorine atoms over here and this orbital right so this uh 3p orbital is going to overlap with the hybrid orbitals of phosphorus and this is how the structure is going to be formed is it clear so if you have to draw the geometry of this how is it going to look like okay so you can see that there are five bonds so if I put phosphorus in the center okay I can put the three chlorines on a triangular plane like this and what about the other two chlorines so now you have to think in 3D so these are the three chlorines one chlorine is coming out like this and one going behind it right so I'm just going to draw it over here so as if one chlorine is coming out like this and one is going behind over there are you guys able to visualize this so basically it's again in 3D you have the three chlorine over here and one going uh behind one coming out and This shape was called triagonal bipyramidal because you have two uh these triangular pyramids one in front and one at the back let's see how it looks like in 3D so your 3D structure is going to look something like this there you go can you see you have these three chlorine atoms forming this triangular plane and one chlorine coming out one going at the back see again the geometry is perfect where you have minimum repulsion maximum you know maximum far apart these orbital the uh overlapping orbitals are and this shape is known as trional not all this down please check my spellings also B pyramidal okay why because you can from this chlorine atom you can form a pyramid like this see and from the chlorine atom at the back you can form another pyramid like this so one pyramid in front one at the back that's why triagonal by two Pyramids by pyramidal clear so this is how the hybridization for pcl5 Works sp3 D hybridization so naming is very easy based on the orbitals involved the next hybridization example we are going to look at is sp3d2 hybridization and the example here is sulfur hexafluoride you can see sulfur with six Florine atoms attached to it so sulfur's configuration we know is it is of the form 3s2 3p4 so if you guys draw out the Atomic orbitals it's going to look like this so 3s orbital completely filled p orbital one is completely filled two orbitals are half filled and then I will also draw the vacant orbital because we know here D orbital is also involved so we going to draw 3s this is your 3p and 3D so sulfur in its excited state do you guys you can guess what's going to happen since you need six bonds to be formed so you can imagine that one electron is going to go from here to here so see one electron gets excited and goes here and so there's a you know two electrons are getting excited and another one goes from the 3s shell so finally you have five half-filled orbitals like this so let's show them here 1 3s three uh so one uh s orbital 3 p orbitals and 2 D orbitals and then again before the bonding they will undergo hybridization giving rise to how many 1 2 3 4 5 6 see number of hybrid orbitals will be same so you will be getting six hybrid orbitals now oh my God 1 2 3 4 1 2 3 4 5 6 and this is of the type sp3d2 hybridization and you can see they are having one electron each and this is going to combine with the Florine Florine we know is 1 S2 2 S2 2p5 so florine's uh final orbital is going to look like this your 2s and 2p so this guy is going to combine with the sulfur orbital right so you can imagine this p orbital is going to or Florine is going to combine with the sulfur overlap over there and this is how you will have your sf6 being formed is this clear now what will be the geometry of sf6 so one way to think of this is that that if you draw your sulfur here in the middle right we can draw four Florine as part of diagonals of this Square here and then one Florine on top and one below so again you have to think this in 3D right so this is the entire structure in 3D and this geometry is known as very good you got it right octahedral because you can see it is going to form a eight sided shape right so if I start joining these points and I'll be forming a square pyramid on top square below it's octahedral and the molecule is going to look something like this there you go that's the molecule so you can see sulfur right in the middle the king is over here and the one Florine on top one below and one and four Florine atoms are lying on this Square plane here right so can you guys see the geometry again you have to think this is in 3D right so this is how it looks like and this kind of geometry is called octahedra the spellings are really complicated right so octahedral geometry for sp3d2 hybridization and let's look at our last example of hybridization which is sp 3d3 hybridization so this example is seen in if7 right iodine and Florine so iodine you can say HEPA fluoride here if7 is your molecule okay and it is showing SP 3d3 hybridization which means how many pure Atomic orbitals were involved very good 1 s 3p and 3D so that means total seven orbitals are involved that means how many hybrid orbitals will be formed that's right seven hybrid orbitals are going to be formed right so you can uh imagine that iodine is going to have seven hybrid orbitals so this time I'm not showing the electronic configuration I'm directly showing you the hybrid orbitals this is the sp3 D3 hybridization containing 1 2 3 4 5 6 7 I hope I got it right so it will be having seven boxes like this seven uh hybrid orbitals and that's going to share with Florine which has uh I'll just show it's 2p or bital 2p looks something like this right so you can imagine the sharing is going to be done like this one Florine atom is going to overlap with each of these because you have seven Florine atoms here so one each overlapping with the seven sp3 D3 orbitals so what will the geometry of the if7 molecule look like here we have seven bonds so how are you going to draw this so remember last time when we had five bonds like pcl5 the shape was trigonal P bipyramidal we had these three chlorine atoms over here like this this was also a chlorine and then two chlorines one on top and one below when we had six bonds then it was four forming a square like this one on top one below so now can you guess when you have seven what will the geometry look like so this time let's draw iodine in the center iodine is the king here and then you have 1 2 3 4 5 flines so what shape will these five flines which are all in the same plane same flat surface they are going to form a pentagon that's right so let's join this as you can see these guys will show form a pentagon shape in one plane and then you will have a Florine on top here and a Florine atom below here so what will be the geometry that's right it's going to be pentagonal by pyramidal right you have two pyramids and pentagonal shaped pyramids because when you start joining these so I'm just roughly showing it to you here when you start joining all of this it's going to form a pyramid on top and then one below so finally the molecule is going to look something like this in 3D so iodine right in the center over here five Florine atoms as you can see forming a pentagon shape in this plane right these are all lying in the flat surface one Florine on top one Florine down as far away from each other right uh to minimize the repulsion and this geometry is known as pentagonal bipyramidal for all these seven bonds clear so please learn these names and of course please check their spellings also these geometry names are important and it is an example of sp3 D3 hybridization where you have seven hybrid orbitals like this now that you're clear about the concept of hybridization and how to work out the hybridization using the electronic configuration and looking at the orbitals of the atoms so you guys are clear about how to work out the hybridization right but now let me teach you a nice trick where we do not have to go down to the electronic configuration or look at all the orbitals we can directly find the type of hybridization like for example is it SP SP2 sp3 you can know the type and based on the type you can easily predict the geometry so what what is this trick this trick is based on the number of Sigma bonds and the lone pairs of the central atom so what you guys need to calculate is the number of Sigma bonds and the number of Lone pairs of the central atom and this is denoted by Zed and guys you remember what are Sigma bonds Sigma bonds are the bonds formed by the headon right headon overlap and these are the first bonds formed between atoms because remember the first bond is a sigma Bond and there is only one Sigma bond between the atoms the remaining bonds are Pi bonds so you guys should find the number of Sigma bonds and add to that the number of Lone pairs on the central atom you'll get this number which we denote by zed zed is not atomic number here right it is basically this number for hybridization and based on Zed we can predict the hybridization let's understand with a simple example let's take the example of the water molecule so water you know H2O How does the structure look like so to get this hybridization trick you need to know the structure because you need to understand who's the central atom how many Sigma Bonds are there how many lone pairs are there right so for that we need to know the structure either we'll be given the structure or you have to work it out so in water we know in the water molecule oxygen is the central atom and it is bonded to two other hydrogen atoms with the sigma bonds and oxygen you know has six valence electrons so there will be two lone pairs over here because one one electron is being used over here and remaining four electrons are forming the are in the lone pair so we have two lone pairs right total six valence electrons of oxygen so now if you look at this water molecule what does our Zed work out to be Zed is the number of Sigma bonds which is two plus the number of Lone pairs how many lone pairs here 1 and two two so 2 + 2 my Zed works out to be four here now what does this tell us what will be the hybridization so here you need to remember this simple table which is very easy that if the Zed turns out to be two then the hybridization type will be SP hybridization because you can remember as if like there are two hybrid orbitals so naturally SP right if it is three there are three hybrid orbitals obviously it will be SP2 hybridization if there are four hybrid hybrid orbitals then sp3 hybridization if there are five hybrid orbitals then sp3 dehybridization if there are six hybrid orbitals then sp3 D2 hybridization clear so now based on this number Zed can you tell me what is the hybridization of water the water molecule that's right because you can see Z has turned out to be four over here Zed is four so therefore it has to be sp3 hybridization because see Zed is four okay so directly we do not have to go back into those orbital levels and draw out the electrons and all of that we directly say Z is equal to 4 so water is sp3 hybridization and this directly gives us the correct geometry of the water molecule because sp3 hybridization means it will be having a tetra geometry like that tripod remember so it will be having a tetrahedral geometry so if we draw it out how is the water molecule going to look like it's not going to look look like this right so that is the advantage of hybridization it gives us the geometry of the molecule the geometry is going to be something like this where you have the oxygen atom okay here and there's going to be one lone pair over here another lone pair here and then then you have your two hydrogens so you guys are realizing again I've shown it in 3D right so this is your tetrahedral those are your legs of the tripod and this uh the top part over here so 1 2 3 4 it's forming a tetrahedron sp3 hybridization tetrahedron so isn't this hybridization trick easy so we do not you do not have to go down to that orbital level you can easily work out Z number of Sigma bonds not Pi bonds not the double or triple bonds only the single Bond right or I should only the single Bond the first Bond right so basically the number of Sigma bonds plus the number of Lone pairs you work out Zed and immediately you know the type of hybridization and also the geometry so geometries you have to learn based on the type clear let's understand the trick with another example we are going to take ammonia molecule this time ammonia you know is NH3 so again hydrogen can't be the central atom so nitrogen is the Central atom over here clearly right and what does its structure look like so we know that you have nitrogen hydrogen forms these Sigma bonds the which is a shared pair of electrons with nitrogen and nitrogen you know it has five valence electrons so one see 1 2 3 are already used up so there will be a lone pair here correct three already used up so a lone pair so now based on this you can see that we have three sigma bonds and one lone pair right it is not counted as two one lone pair so what will be the value of Zed over here so for ammonia Zed is going to be equal to the number of Sigma bonds 3 + one lone pair so Zed is four once again four like the water molecule immediately you can say since Zed is equal to 4 it is sp3 hybridization and it will have a tetrahedral geometry immediately we know the answer so here the best part is we can directly say so this is sp3 hybridization and it is going to have a tetrahedral geometry so if you have to draw the geometry of ammonia molecule what will it look like not like this right you are going to draw it like this nitrogen the lone pair here okay and then you will have the three hydrogens forming the legs of the tripod over here see tetrahedral geometry that is the whole advantage of hybridization because uh the the Louis Dot Structure was not able to give us the geometry of the molecule right here we are getting that through hybridization clear another important point to remember about the geometry of hybridization is it is the geometry of the orbitals right it is not the geometry of the atoms right because lone pair is also involved here so it is the geometry of this orbital this orbital this orbital and this orbital right because you're having these sp3 orbitals right nitrogen has this hybridization of sp3 type there are four sp3 orbitals over here so sp3 here involved sp3 involved here from nitrogen side again we are talking only of the central atom so you're getting the geometry of the orbitals take a note of that let's look at another example let's say I tell you sulfur trioxide right what will be the hybridization involved in sulfur trioxide so sulfur trioxide gas is S3 again we need to know know it structure right so who's the central atom it's sulfur right the atom which is least in number so we are taking sulfur over here and the three oxygen atoms okay and here there will be double bonds so this is how it's going to look like right so you'll be having double bonds and sulfur has six valence electrons so all have been used up in uh bonding right in forming these bonds so there is definitely no lone pair left for sulfur okay so what are the types of bonds since we have double bonds there is one Sigma one PI right this is a sigma bond this is a pi bond this is a sigma bond this is a pi bond this is a sigma bond this is a pi Bond right remember the second Bond third bond is always Pi first one is Sigma so what is the value of Zed here guys so for sulfur because see we have to do on the central atom which is sulfur here so for sulfur we don't look at oxygen Zed is going to be equal to the number of Sigma bonds 1 2 3 plus lone pairs is z so Z is equal to 3 so what will be the hybridization over here that's right for Z equal 3 it will be S2 hybridization hybridization type will be SP2 so sulfur therefore shows SP2 hybridization and the geometry geometry is going to be trional planer that means should I draw it like this the answer is no hybridization tells us this hybridization Theory tells us it's SP2 hybridization the geometry of this molecule is going to look like triagonal planner so the orbitals are going to be arranged like this which means sulfur is right here in the middle and oxygen atoms are forming this kind of Tri triangular shape so this is the geometry of sulfur trioxide molecule again remember hybridization is the geometry of the orbitals not the atoms because they could be lone pairs right so here there are no lone pairs so also the atoms are arranged in this way we'll talk about shape and stuff right but this is the geometry of the orbitals the nice thing about this hybridization trick is that we do not have to go down to the orbital level but we need to know the structure right we need to know the number of Sigma bonds the number of Lone pairs to predict the hybridization now the question is is there a shorter trick where we can work out the hybridization without the structure and the answer is yes so let me share the hybridization shortcut with you so in this hybridization shortcut you can directly work out Zed without the structure how do you do that what is the magic formula it is equal to half so remember this entire formula is multiplied by half so half times the number of valence electrons on the central atom so you have to identify who's the central atom se's number of valence electrons plus any negative charge in case there's an ion right or subtract out any positive charge plus the number of monovalent atoms bonded to the central atom okay so let's take a look and see how this magic formula works and how we can do without the structure so we'll start with the same example of water which we had done with the structure now we'll try to do without it so if you look at the water molecule clearly oxygen is the central atom Okay so let's work out Zed come on let's work it out together based on this formula so what will Zed work out to be for oxygen oxygen is our Central atom here how many valence electrons does oxygen have you know oxygen has total eight electrons 2 comma 6 so the valence shell has six electrons so I'm going to write the formula Z will be equal to half * 6 the number of valence electrons in oxygen plus the negative charge on it and minus the positive charge on it but water doesn't have any uh charge right it's a neutral molecule so we can ignore that plus the number of monovalent atoms that are bonded to this right so you can see there are two monovalent atoms hydrogen so I'm going to say 6 + 2 over here hydrogen is monovalent correct so what will it work out to be Zed you can see will work out to be half * 8 and that is equal to 4 and this is exactly the same Zed we got based on the structure we'll take a look and so if Zed is 4 four it has to be sp3 hybridization with a tetrahedral geometry immediately you can see that okay so based on this magic formula let's take a look did we get the same answer see based on the structure the number of uh Sigma bonds and lone pairs we had worked it out we had got Z equal to 4 and obviously it'll be sp3 hybridization so you can directly get Zed using this shortcut so you don't have to work out the structure just use this shortcut and see you will get the same answer here let's try another example let's try ammonia so ammonia is NH3 now what will be Zed over here once again you have to identify the central atom that is the first thing Central atom is nitrogen so what will be the value of zed zed is going to be half times the number of valence electrons on nitrogen nitrogen has five valence electrons right 2 comma five so five over there there's no positive or negative charge and how many monov valent atoms are here you can see hydrogen is monovalent three monovalent atoms so half * 8 and the answer is once again going to be equal to 4 and four means it is again going to be sp3 hybridization and the geometry is going to be Tetra hydral and remember we got the same answer for ammonia you can see zal 4 sp3 hybridization and we are getting the same answer with the shortcut trate that's the beauty let's take a look at sulfur trioxide so s SO3 s SO3 again what will be the value of Zed guys First Look What is the central atom the guy who's in the minimum number sulfur sulfur is the central atom how many valence electrons sulfur has sulfur has six valence electrons plus the number of negative charge minus the positive charge there's no charge so we will ignore these two terms and plus the number of monovalent atoms should I write three here no no no oxygen is not monovalent oxygen has valency of two monovalent means valency of 1 so obviously we will not add oxygen here so it will be half * 6 which is equal to 3 so Z is equal three that means it is SP2 hybridization and immediately you can write and the geometry is going to be triagonal planer and let's check it here so see for sulfur trioxide also we got exactly the same answer Zed was equal to three so you guys like the shortcut trick make sure you guys use it and you can directly find the type of hybridization quick and based on that you can predict the geometry let's look at some more examples this time we going to look at some ions so let's say if I give you you need to find the type of hybridization in nitrate ion or let's say sulfate ion how will you work it out using this shortcut trick so once again remember identify the central atom and use this formula so let's try it out so in nitrate who's the central atom nitrogen the guy who's least in number and what will be the value of Zed over here Zed is going to be equal equ Al to so half times we need to look at the number of valence electrons on the central atom nitrogen has how many valence electrons five balence electrons let's put that in plus the negative charge so negative charge is added you can see there is one minus so I need to add + one over here there is no positive charge so minus 0 plus the number of monovalent atoms that are bonded to nitrogen are there any monovalent atoms the answer is no it is just uh o o over there so this will be zero and based on this the answer is going to turn out to be half + half * 6 which means Z is equal to 3 so what is the type of hybridization this is going to be SP2 hybridization and based on this we can guess the geometry will be triagonal planer so can you see how this shortcut trick works where you do not even need to know the structure now one important thing here is here I give you nitrate but let's say I had given you nitric acid hno3 so see once again the central atom is nitrogen so when you apply this formula what will you do half * 5 right plus this time the charge is going to be zero right so Z will equal to half * 5 plus the charge here is going to be zero plus the number of monovalent atoms so you can see that there is one monovalent atom here hydrogen so we are going to put that one so see again it is turning out to be Zed is equal to three over here here right half * 6 so one important thing that the this monovalent atom need not be bonded only to the central atom because in nitric acid the structure will be like this right so there's going to be oxygen here and the hydrogen is bonded to the one of the oxygen atoms right that's how it releases this H+ in nitric acid so you have to count the monovalent atoms in the molecule like this clear next let's look at the sulfate ion sulfate ion is S so4 2 minus so let's work out the value of Z over here this is going to be half times what is the number of valence electrons in Sulfur sulfur has six valence electrons plus the negative charge negative charge this time is two so plus two right there's no positive charge and there are no mon monovalent atoms present here so plus 0 or we can simply say half * 8 over here which is equal to 4 so guys what will be the type of hybridization in sulfate very good the answer is going to be sp3 hybridization because value is four so sp3 hybridization and the geometry of the orbitals is going to be Tetra okay so remember this and uh though earlier I had mentioned in the examples that uh when I saying monovalent atoms I saying bonded to hydrogen but like I bonded to the central atom but like I showed you the example over there the monovalent atoms you're counting in the molecule right not necessarily only bonded to the central atom clear let's look at some more examples because the more you practice the more confident you'll become so let's say if I ask you to find the hybridization in Silicon fluoride right so sif4 so again use this trick okay so here who's the central atom obviously it is silicon the atom which is least in number so this is our Central atom over here now let's work out the hybridization Zed will equal to half times the number of valence electrons on Silicon silicon you know has four valence electrons like carbon right so we are going to put four over here there's no positive or negative charge and how many mo monovalent atoms are there Florine is monovalent it has valency 1 so four monovalent atoms so this is going to be half * 8 which is Al to 4 so guys when Zed is equal to 4 what is the hybridization very good it is sp3 hybridization and it will have a tetrahedral structure see it becomes so simple so if you don't know the structure you can easily predict it using this magic formula so make sure you remember it let's try one more example so this time rather than giving you sif4 if I'll give you XC F4 now you might be thinking oh my God Zenon is a noble gas does it have compounds the answer is yes chemistry is full of exceptions Xenon can form compounds like this so this is Xenon fluoride XC F4 okay and now what will be the hybridization here so let's work it out guys half times who's the central atom obviously it is the the noble gas over here the noble man Zenon and uh the number of valence electrons of the any noble gas you know except helium is two so here it's going to be 8 plus no negative charge no positive charge how many monovalent atoms does it have Florine is monovalent so four of them 8 + 4 so we are getting half * 12 which is equal to 6 and remember that table if Zed is equal to 6 it is sp3d2 you have six hybrid orbitals right so this is going to be sp3d2 you can also do a check by you know adding the pars here this is s ^ 1 so 1 + 3 + 2 The Power should add up right uh to this number six so s P3 D2 hybridization and do you guys remember the shape so when you have six things right you have uh this four in one plane one on top one below so it is forming a shape having eight faces which means it is octahedral OCTA means eight it is octahedral in not shape again I should say geometry because we are talking about geometry of orbitals shape we are going to talk about when we do valence shell electron pair repulsion Theory okay so this is all the geometry of orbitals and as you can see this hybridization shortcut trick it's really good so make sure you learn this magic formula and easily You can predict the hybridization and also the geometry without knowing the structure now I'm sure the question is coming to your mind that why did we learn all about hybridization if there's such a nice shortcut but you know sometimes uh if the structure is given that method is faster right and we also need to know the concept right why is hybridization happening so we had to look at the orbital level right so if possible definitely try to use the shortcut uh with this magic formula or if the structure is known you can definitely look at the number of Sigma bonds plus the number of Lone pairs on the central atom you work out Z and you can immediately get the hybridization using this table that we have discussed all right so let's try one more question on this so here's a question for you find the hybridization of all carbon atoms in propine okay who propine propine is that hydrocarbon it is the alkine type having triple bond so let's uh since we have to look at all carbon atoms let's draw the structure of propine so propine has one triple bond over here carbon has valency four so one hydrogen here uh this one all the valencies satisfied and this carbon has three hydrogens so if I tell you to work out the hybridization on each of these carbon atoms so atom number one atom number two atom number three how will you guys do it what method will you use so obviously we do not want to go down to the orbital level right so will we use the magic formula or will you look at the sigma bonds and lone pairs so I think since we have drawn out the structure actually here Sigma Bond and lone pair might be faster right do you guys agree so let's do that so we are going to Mark out the sigma bonds over here this carbon has one Sigma Bond here one Sigma and remember these are Pi bonds the double and triple bond is pi the first bond is Sigma so there's another Sigma here another Sigma here another Sigma here another Sigma here what about the lone pairs so this carbon has all the four electrons are in the valence shell they are all used up in bonding so no lone pairs same for this carbon 1 2 3 four electrons used up same for this carbon four electrons will be used up right so none of these carbons are having lone pairs which makes lives pretty easy so if you work out the Zed the value of Zed for each of these carbon atoms so I'm to say Z1 for this first carbon atom it is having uh remember the formula the number of Sigma bonds plus the lone pairs okay so this guy has uh two Sigma bonds so Z1 will be equal to two if Z1 is two that means there is sp hybridization involved and with SP hybridization the geometry is linear right lying in a line so Z1 is done for us what about carbon uh atom number two Z2 Z2 is having how many again two Sigma bonds Pi Bond doesn't count no lone pairs so Z2 will also be equal to two that means once again there is a SP hybridization and so the geometry will once again be linear the last one Z3 zed3 again having so this time it has four Sigma bonds right one with this carbon and three with the hydrogen and no lone pairs right because Valance shell has four electrons they are all used up in bonding so Z3 is equal 4 which means this is sp3 hybridization and the geometry will be tetrahedral so guys here we use the formula Z equal to number of Sigma bonds plus the number of Lone pairs I'll be lazy and write LPS okay so see here we use this method so again it depends if the structure is given or you can quickly draw the structure this one works fast or you can use this hybridization shortcut that we discussed so in summary what have we learned today we have learned about hybridization for calent bonding because remember all these theories are for covalent bonding and the beauty of hybridization is it explained this whole intermixing of orbitals why the bonds are same like in the methane molecule and it gave us the geometry right so the key thing is it helped us determine the geometry right based on this whole hybrid orbitals hybridization concept which the louw theory and balance Bond Theory could not give us so that's the good news the bad news is that hybridization Theory also has drawbacks there are certain things that it cannot explain and which is where the valence shell electron pair repulsion Theory comes in so what it can't explain it can explain us the geometry of the molecule but it does not it cannot explain the shape of the molecule right why does a certain molecule have a Bend shape or a V shape or a pyramidal shape that it because it just gives us the geometry of the hybrid orbitals it is not looking at the bond pairs only or the atoms and that is where V PR or valence shell electron pair repulsion Theory very long name that's going to fix all this and that is where this Theory comes in which we are going to look at in the next video so stay tuned friends I have a homework question for you can you find the hybridization in Xenon dioxy difluoride that is xc2 F2 so go ahead and use the concepts we have learned and find out the hybridization here and do let me know your answers by putting it in the comments below I look forward to reading your answers and I promise to reply to them so try this homework question and let me know your answers by putting it in the comments below friends I hope the hybridization Concept in chemistry is crystal clear to you now and do check out the full courses on our website manocha academy.com and our Android app I'll put the links below because we have courses on physics chemistry biology maths coding and artificial intelligence in these courses you're going to get live classes concept videos quizzes questions mock test and revision notes so guys what are you waiting for these courses are perfect for your exam 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