 मुक्यटाई लिए ताब की में और वीटियों क्या लगनादा लगना स्लिए था सेर सब विरे रोगनादा और शिलागांगे ताब एक आच्द है. भी सब गब महों जा शब वो कर्षाते तोलगे अरे देखने की सब आगा है. there are some medical images that's why I am in Delhi from the past 20-25 days that's why all these difficulty I am facing but yes you will get the video soon so could you tell me what have you done last classан्ञि़्ँ'd lunar radically met Attention we have to start with Vailyen's Quan So Vailyen's Quan theory means overlapping concept Okay अ। स्ब अग़ के लोगते ना लोगते किवीडर और बंगा को इवागे द्रेवाट वो मन्एक्छेबतिया पार्दर मास्था के लोगते कोई लेक्ये किवीडर च्छेदे के पहलादा कोई ख़ाद के लिँगाने रहाद. वह कदा गर लेक्गटा है. नही। लेक्ट सारनाता है, वह कस इस लेक्टाध कर लगा मेंगटा लेक्टा लेक्टान भी थी अगा आप다 कर लगा मगटान में वे according to this theory the molecule has 3 and 4 factors. खेरी सब लेलिन्स वान्तेरी सी जील्ँजाई सकन ल्�很好 ढ़ावार बेनाई घीरी मेंगगे जादवी यह संब अग़े � now we are going to see how atoms forms a bond, right? दिर्ज का तना बिश्हान लिकसब नहीं छेरी and the heading all of you write down. तो बीश गेरी लिए वेलिन्स बान्तेरी it is a balance bond theory, okay what is valin's bond theory? आद मुरलीकुल भुदिक नाई सो भी सदने उह एह मागικόिडार्च दार्च बाहर आतमिख हॡर्шеं सो ग मेग मेफमन च्याद martian उतमिख यilà एल ऐन मेब �容भ वenter थार्चा अर बाछ dola अर्ठाम् च्याद Was सद य अप N نमन säga,せてaurais tantriyed  अब देनने मसे अब देनने papa Nepal नेता मीखे। लामसArthur जार सभरया दाहाता ऽद� planoक मिए चरनास भरना विन कर विसक्का玩 make औब देता, अब देनने और विसका, विसका यौक झी library प्रसना चाहा 당 luego Moreover can be done in 2 ways. The first one is axial overlapping and the second one is lateral overlapping. than overlapping is also called as head on overlapping, head on overlapping and lateral it also known as sideways. So firstly you write it down here, what is axial overlapping। ॑। ृु, ृ॑ । ृु ूॉ ृॐ, ूॉ ूॉ तो बेयु, एक लग्दाब मच्ताशनवार वो लग्दा सच्वोलिएद, जो मुँझाऍा आववाशवारईग, अब वो लाणी Premier आख्दी़ आश्वारईटिL, वे स्वावीटल अख्दी़ भी आब बी आप च क्याँच़ाच, बावाशवारोद ये खाँच्ची, वे च� यह साच्टिवाए तूलबाहक्छही सेगा था तो सेवाए तूलबाहेग। वितलाप मोगर राष्टिएर कोंगा at the inner nuclear axis तो सेवाए तूलबाहेग। तो सेवाए तूलबाहेग। चोब पर ही थीश्छा। तो थो यह देखर्ज़ होग पुल पात्छी amendments and all these are axial overlap it's also axial now in this one ainea 어머 If you see, it is a experimental order we have the extent of overlapping it is maximum pe then we have sp and then we have ss overlap one second so this is the extent of overlapping tp overlap no its not run upFF overlap, first of all we don't consider it like overlapping depends upon the shape of the molecule I'll tell you what it is shape of the molecule not, shape of the orbital वह essentially means that, वह the orbital overlap, the shaded area, that have drawn in the last slide, वह नास्क ब़ाजित बज़्द कनातियर मिक than bah it has been observed that when we have the low valve tumble shift, that overlaps to a greater extent, because of its shape. एक ज़िए भी तोब क्यों एक गुडिया ये और दम्बनी ये वह नहीं, एक जिया उब वह भी ये बताजिया था करतेंगे। छ़ाँण्गथ करायद year is to keep in mind that the first overlap that takes place between the two atom in a molecule is always axial overlap when axial overlap is always the same. बाद क्या में क्याल लग्� now is the शवन िर यम सबसकी लव से आप यप सम ठहीत हो लाम. तो छग किसर्णे तो कोनाकनोडन टल बोही होती,和 time 2 in truth धीफकर करावमि खरेत 궁금 करणई � se-畧ीद टोगश्द भीव्रुश नद करेश़ बाज़ कर Globe transferring करमउ boyfriend करावमि करवमिよ. अआखकर कर कर बाचिकबान कर कर कर कर वो exchanged kamaral ambazhi kare Owned जी कर सी� 真的 eat boon.hetto consciousness Markus खरे �polation यहाजे kommer यहाच़ कर दर ण nude ताचाल आखे देरुर्वित्या देरूरा कच्यूद कोन ठुधप्या थेरी है, ताचान बच्य। सी चिस ज्ल weten चेर्टार से इलंकि था. स highlights कीर्टार से एक अग्वडल. सुद्वान किस अदबमार्वानों आफ चात्गाता। लगा किस भी देक्डिक्ह of this day they are some drawbacks in these keadee like we have drawbacks in various atomic models. पीस्टी की और लाभाख की है पर कोंई कि अजना के दिए वो लाप आप नहीं बहुत की की कर रब अल अच्च्छनता हच्चनता प्ता बारा इच्चनता को आप चानदाब देगास्च्सा से जब Junior'd तोड़िए भी अत्मन और चानदाब देच क enhanced देच की आख्चनता गर अद्चकनता प्ता देच दोड़े प्ता प्ता वी दिश्चनता यधी, दोभ दे आ़ आज प्पशक और शुग जोगे सदाखगाए. आ़ आज गखखक जोगे सदाखगाए. इस वर्पशोग यह जोग यह भवन नेज प्री� molar the axis which is perpendicular to along the axis which is perpendicular to inter nuclear axis. चचं स्व कि सिनगखर था आच्कच मैं। चशक बियच्क प्ल कि सर ज़ब प्ल कि आख्कच्च concepts. तैसो ज़ब ई अबस्म lingering ofelas in his ञादि still ride but this atom has two more orbital pr orbital present and drawing here only one just to make you understand is another p orbital we're right since the overlapping takes place along this line, that is along the inter-news axis so now the inter-news axis is fixed when these two orbital overlaps here this overlap is a lateral overlapping perpendicular to the inter-nuclear axis so this is lateral overlapping and lateral overlapping you see it forms by see lateral overlapping orbital can form we have d pi d pi bonding we'll see that later we'll have d pi d pi bonding but usually we don't consider the extent of overlapping into your no it's not possible for s orbital lateral overlapping is not possible for s orbital because the s has only one orbital right so we always have a line which is which which is passing to the two nucleus so s s always gives you axle overlapping if you try to understand this this by electron suppose this is a sigma bond we have right this is a sigma bond between the two atom and this is a nucleus the overlap that you have the lobe overlap it forms an electron cloud like this this is the overlap lateral overlap right electron cloud above this sigma bond and below the sigma bond electron cloud right so this is the electron cloud we have this collectively gives one by bond it's not like we have three two pi bonds here this two gives one by bond are you getting it properly am i audible guys is there any lag or something yeah i think mother it's your problem then maybe it will get you know fixed in something yeah fine let me know if it is you know if it it won't you know go well in the class then i have to change the network actually we'll see that once if you have difficulty in understanding just let me know any one of you okay fine so this is the electron cloud this cloud that you have right so this gives you one pi bond collectively gives one pi bond here so pi bond is something like this if you can know see me see if you have a sigma bond like this you see this is a sigma bond if you can see right this is sigma bond so this is the axle overlap you see this the lobes that overlap like this okay it is axle overlap but the orbital which is perpendicular to this axis is this when this to overlap like this above and below also when this to overlap this forms a pi bond can you imagine this right so we have a sigma bond like this axle overlapping and electron cloud here because the latter overlapping and electron cloud here this i have shown is it here electron cloud is there because of overlapping okay so this forms the pi bond on this now what is that characteristics of sigma and pi bond yes it is mostly but since we cannot we cannot we cannot find out the position of an electron that's why we draw the complete overlap and we say the electron cloud is above and below also of the sigma bond see electron cloud is the electron that is present in this region right like this overlapping the electron is present between the two nucleus in the bonding instead because of overlap right so overlapping is a is a property of an orbital which contains unpaired electron but the electron cloud is the density of electron over here in this region understood yes tell me yes electron will be one side only at the time but we decided we do not know that's why they presented like this exact position we cannot find out the orbitals which has unpaired electron will take part in overlapping and hence electron gets spared tell me any doubt yes yes it is covalent yeah sharing of electron it is covalent compound next right down characteristics of sigma and pi bond copy down this this table you copy this down all of you let me know once you are done done all of you yes pi bonds forms because of the lateral overlapping of p orbital but not only p we can have d orbital also but in valence bond theory we don't talk about d orbital point number 4 the molecular orbital is symmetrical about okay so it is fine since we did not talk about molecular orbital so this better you write atomic orbital instead of molecular but the statement is not wrong as far as molecular orbital is also but for this for now whatever whatever we have done so far molecular orbital we did not talk about right so better if you write the atomic orbital right but the statement is not wrong for molecular orbital yes yeah definitely I will do molecular orbital theory but we'll do one by one okay we'll do it today itself do you have semester exam coming okay when it is coming week when this chemistry coming Tuesday what is the portion for chemistry guys okay so all of the chapters we have done fine so bonding we'll do it today okay whatever it's required for school exam we'll do it are you prepared well because Tuesday is like you have just 2-3 days right did you finish all of you okay for HSI properties of matter states of states of matter they have done fine guys so you see how this you know orbital overlaps you know takes place and forms the molecule we are going to see a few examples here oh fine okay mother I'll go back just a second okay for HSI that date is not declared right you said after 1st October is it from the 6th or by then we can do that particular chapter also okay not completely but yes we can do that now you see some examples on this the 1st one is H2 molecule you see how hydrogen molecule forms hydrogen molecule forms by the orbital overlap of the 2 hydrogen atom which has 11 electron each and this is the bond formation we have if you draw the orbital diagram here we have 2 hydrogen atom suppose 1 is this this is the inter-nuclear axis inter-nuclear axis both orbital contains 11 electron and along the inter-nuclear axis overlapping takes place and it forms sigma bond so this is the axial overlapping we have we have easily understand this this line is the now the 2nd molecule you see oxygen O2 okay if you look at the structure of O2 we all know oxygen has a double bond and each oxygen atom has 2 lone pair try to understand the orbital diagram of O2 molecule you see the electronic configuration of oxygen atom is 1S2 2S2 and 2P4 this 2S has 2 electron and 2P has 4 electron like this well and shell is this right S has 2 and 2P has 4 so if you draw the orbital diagram of it I am going to draw this thing so 3P orbital PX PY PZ contains this electron right this 3P orbital if I draw here I am not doing anything I am just drawing this box in the in the in the shape of the orbital that is it similarly the other oxygen now you see this is the one of the oxygen atom it contains one electron here right one electron here and suppose 2 electron and like this we have another oxygen atom also which has a similar configuration like this so this has one electron this has again one electron and this has 2 electrons now this overlap you see along this line this is the inter nuclear axis and along this line the overlap that we have this is axial overlap which forms a sigma bond this 2 orbital goes under lateral overlapping right so this is lateral overlapping so it forms pi bond right like I said oxygen atom has 2 lone pair so one lone pair is this and another lone pair I did not show it here but this is the another lone pair we have in S sub shell so if you want to show this S sub shell electron S electron here this is the S orbital 2 electron present spherical shape the another S orbital you can draw it here for the another atom and 2 electron so this is the diagram we have orbital diagram did you understand this clear no doubt so could you draw the orbital diagram for nitrogen molecule yeah hybrid action mother just you let it be we will discuss it now only we will discuss last point he let it we will discuss no first of all electron won't overlap orbital overlap which contains electron so when the orbital overlaps Aditya so the spin of the electron will change one is clockwise other one is anticlockwise and that happens on its own in order to minimize the understood every direction I won't answer now just give me 10 15 minutes I will explain more and then we'll discuss these two okay give me 10 15 minutes did you draw the orbital diagram of into so it is very much similar to oxygen molecule we know nitrogen molecule has nitrogen nitrogen triple bond and a lone pair on each nitrogen so if you look at the electronic configuration of nitrogen it is 1S 2 2S 2 2P 3 3 orbitals I am drawing here okay each of these orbitals has one one electron along this line we have inter-nuclear axis forms sigma bond when these two overlaps on the panel orbital overlaps forms one by bond and when these two overlap it forms another and the lone pair is the s electron that we have here right okay one more will do here the next one we have CH4 molecule methane if you look at the configuration of carbon atom carbon has 6 electron 1S 2 2S 2 2P 2 right so 2S has 2 electron and 2P has also 2 electron right this is the ground state configuration now you see carbon is attached with 4 hydrogen atom with a single bond in CH4 right so for this bond formation carbon hydrogen 4 bonds carbon must have 4 unpaired electrons like 1 2 3 4 carbon must have 4 unpaired electrons right so 2 electrons we have here unpaired so what happens to make a bond with the 4 hydrogen atom this electron jumps into the vacant orbital and this we call it as the excited state of carbon which is required for the bonding with 1 2 and 3 this is the excited state here and all these electron sorry molecule sorry orbital which has one one electron hydrogen overlaps with this 4 orbitals and forms the form okay so if I draw this structure we have 3P orbital 3P orbital and we have one S orbital suppose S orbital is this okay all these orbitals has how many electrons one one electron are you getting it all of you please respond one one electron this diagram did you understand any difficulty in this it is just a box I have written in the form of the shape of the orbital yes that's right mother okay so what happens after this the 4 hydrogen atom which has S orbital it overlaps with this and forms the bond all these are S orbital of hydrogen right so it is hydrogen hydrogen and hydrogen all these are axial or lateral do we have any lateral overlapping here do we have any lateral overlapping no we do not have because we can always draw an inter nuclear axis like this right so it is all these are axial overlapping okay so what all orbitals are involved in the bonding we have we have one S T X orbital other one is S T Y S for which atom S for which atom here all these 3 S for hydrogen and then SS orbital for hydrogen and carbon right so you see what happens here in the 4 bond we have different different orbitals involved right we have different different orbitals involved and when different different orbitals are involved so what we can conclude that the bond forms in CH4 molecule according to the valence bond theory means all the 4 bonds all 4 bonds should be different should be different and different in what aspect different in terms of their strength in terms of their length because different different orbitals are there they cannot be identical basically little bit of difference should be there right all 4 bonds should be different from each other from each other suppose it's not these 3 bonds S S P X S P Y and S P Z at least these 3 bond and this SS bond must be different from each other right because of the extent of our right so this was the conclusion according to valence bond theory but actually what we observe but experimentally but it has been observed experimentally that all the 4 bonds are 4 bonds are exactly identical all the 4 bonds are exactly identical hence hence V B T fails to explain the bonding in CH4 is it clear any doubt in this to explain the bonding of CH4 and a new type of theory that we have this theory we call it as hybridization V B T fails here and then we got a new theory to explain the bonding here and that theory is hybridization yeah that's right you understood why do we need this concept of hybridization now we will see because the extent of overlapping concept is true for the other molecules like H2 N2 O2 for all these molecules that theory was perfect but it does not fit for CH4 like I said in the beginning atomic models we have various theories right but all theories this concept does not explain all the you know property of electrons within an atom to some extent one particular theory is correct right to some extent other particular theory other atomic models are correct so for bonding also we have different different theories which explains different different kinds of bonding so now we will see what is hybridization how do we find out hybridization and how hybridization explains the bonding of CH4 okay so write down the heading all of you hybridization we know we have already discussed little bit in the beginning of GOC right it is the mixing of in short I'll write down it is the mixing of atomic orbitals of the central of the central atom slightly different in energy it is the redistribution of energy it is the redistribution of energy and forms forms a center of new orbitals new orbitals of equal energy through hybridization we get a set of new orbitals of equal energy which is called this new orbital that we have this we call it as hybrid orbitals so atomic orbitals and now this is hybrid orbitals so how hybrid orbital forms by the combination of atomic orbitals so what happens for the central atom the atomic orbitals of central atom in some molecule combines and forms a new set of orbitals which we call it as hybrid orbitals are you getting a point write down all hybrid orbitals all hybrid orbitals have same shape and equal energy same shape and equal energy so what is the use of hybridization here what happens in hybridization we have atomic orbitals of certain different energy like but the difference in energy is not that great okay slightly different in energy before the bonding with other atom like in CH4 before the bonding with hydrogen atom the atomic orbitals of carbons combines and forms a new set of orbitals which we call it as hybrid orbitals or hybridized orbitals no no it is not about electron cloud stage hybridization is for orbital not for electron electron you let it be now okay obviously electron is present in the atom but electron cloud is just is just the density of an electron at a given you know in a given area that is the electron cloud we are not talking about the position of electron where the electron is present right in which orbital and that we are not talking about we are talking about like we have orbitals like this we have orbitals and this may contain some electron that is not a problem this may contain some electron before bonding it with another atom these orbitals combines together I am talking about this and this combines and forms a new set of orbitals this new set of orbitals we call it as hybrid orbitals if this has two electron here also we have two electrons one electron one electron one electron position of electron is fine exactly same but I am talking about the combination of atomic orbital which gives the hybrid orbitals here yes yes understood right on the heading characteristics of characteristics of hybrid orbital first point right on all hybrid orbitals hybrid orbitals have same energy already I have given you this I have seen or equal energy yeah it is hypothetical only hybrid action concept is you know it is not hypothetical okay because we have seen the different shape of orbitals in the molecule right that is possible and it is I will explain that just a second I will take one example and make you understand this let me give you the characteristics of hybrid orbital all hybrid orbitals have same energy like atomic orbitals hybrid orbital can also accommodate maximum of two electrons more than two is not possible this is again aditya I will explain wait third point hybrid orbital always forms sigma bond hybrid orbital always forms sigma bond and may contain lone pair right on continue this point hybrid orbitals always forms sigma bond and may contain lone pair if you remember in GeoC I have told you that while counting the hybridization we don't count pi bond remember that we just checked lone pair sigma bond is it that is the reason because it never forms pi pi bond hybrid orbital okay it never forms pi bond it can have lone pair it can form sigma bond but pi bond it never forms so hybrid orbital always forms sigma bond and may contain lone pair next point if there are pi bonds to be formed if there are pi bonds to be formed then equal number of orbitals must be left unhybridized this number of pi bonds equals to the number of atomic orbitals okay which is left unhybridized again the next point is if there are pi bonds to be formed equal number of orbitals atomic orbital you write down equal number of atomic orbital must be left unhybridized if there are pi bonds to be formed equal number of orbitals must be left atomic orbitals must be left unhybridized next point the geometry of molecule the geometry of molecule can be determined by knowing hybridization okay geometry of the molecule can be determined by knowing hybridization so we got this column here this side we have hybridization and this side we have geometry so if hybridization is sp then the geometry is linear if hybridization is sp2 then geometry is trigonal linear if hybridization is sp3 geometry is tetrahedral if hybridization is sp3d it is tvb trigonal bipyramidal if it is sp3d2 it is octahedral or we also call it as square by pyramidal if it is dsp2 which you won't get here mostly it is square linear yeah i'll go back wait copy this down i'll go back so this is the geometry you must keep in mind according to the hybridization of the molecule one last point you write down the number of hybrid orbital forms hybrid orbital forms equals to equals to the number of atomic orbitals combined okay i'll go back the number of hybrid orbital forms equals to the atomic orbital combines last point is number of hybrid orbital forms equals to the number of atomic orbital combines okay this table you brought one side we have the orbital mixed hybrid orbital orbital form so if you are mixing 1s and 1p s and p you are mixing so you will get sp hybridized hybrid orbital okay since you are mixing s and p if you are mixing 1s and 2p orbital then you will get sp2 hybridized hybrid orbital but how many sp you are getting here since 1s and 1p 2 atomic orbital combines so you will get 2sp hybridized hybrid orbital are you getting my point yes how many sp2 hybridized orbital we get here in the second one 2p and 1s so we'll get 3sp2 hybridized hybrid orbital now in this 2p we do not know which p is getting over is getting into hybridization pxpy or pypz or pxp that we do not know okay but we'll have this sp2 when we have s plus 3p what we get quickly 4sp3 right if you have 1d 1s and 2p then what we get 2 3 4 4 dsp2 dsp2 mostly you won't get here in the chapter but you will get this in class 12 coordination compound we'll see that it is 4 not 5 dsp2 it is 4 not 5 if you have 1s 3p and 1d that is 5sp3 d orbital we get 1s 3p and 2d 5sp3 d2 1s 3p and 3d or it is 6 not 5 1s 3p and 3d so you will get 7sp3 d2 last one is d3 what I have written copy so overall what happens here in atoms the atomic orbitals combines with each other and forms hybrid orbitals okay these hybrid orbitals will have same energy and the number of hybrid orbital forms must be equals to the number of atomic orbital combines they all have same shape if you talk about the shape here generally the hybrid orbitals looks like this I'll tell you here suppose 1s and 1p are combining to form a hybrid orbital the hybrid orbital that we get is this one 2 hybrid orbital which is this this is the orbital here sp hybridized orbital and sp hybridized orbital 1s and 1p so generally the shape of hybrid orbital is like this one right so we are not concerned with the shape of the hybrid orbital that is not there in our system but mostly whenever we draw we draw shape of hybrid orbital like this one is bigger loop other one is smaller one right hybrid orbital okay now based on this concept you see how they explains the bonding in CH4 molecule now you see CH4 like you know carbon has 6 electron 1s2 2s2 2p2 2s has 2 electron and 2p has 2 electron it is a ground state so in excited state what happens this electron jumps over here and it converts into 3 right it is the excited state now before it makes a bond with hydrogen atom what happens for carbon this s and 3p orbitals goes under hybridization right so this 4 orbitals goes under hybridization and it forms 4 sp3 hybridized hybrid orbital here we have 1 1 electron in this hybrid orbital also we have 1 1 electron like this you see now the 4 orbitals have equal energy with 1 unpaired electron and in this hybrid orbital hydrogen donates its electron sorry the hydrogen s orbitals overlaps with this hybrid orbital and forms CH4 molecule so if you draw the orbital representation of it the 4 hybrid orbital is this right and each of these hybrid orbital contains 1 1 electron this is for carbon right this is hydrogen s shape overlaps with this orbital with 1 1 electron and all these overlap you see is axial overlapping all these are hydrogen hydrogen hydrogen the orbitals that overlaps here is all the orbitals you see it is sp3 s overlap here also it is sp3 s overlap here also it is sp3 s overlap and this one is also sp3 s overlap all bond you see contains similar orbitals that's why the 4 bonds in CH4 molecules are identical and they have the same bond strength and bond length did you understand it so what was your doubt regarding hybridization in VBT so it is not there stress but yes like experimentally once we came to know that all the 4 bonds in carbon in CH4 molecules are identical then this is the probably the most probable or most you know satisfactory explanation of the bonding of CH4 molecule like you see valence bond theory I told you it fails to explain the geometry sorry the bonding in CH4 molecule then we have hybridization right so both are the theories both are the theories of bonding right we do not have any similarity between the two right they explain the bonding in of a molecule in completely different manner valence bond theory don't discuss about the mixing of orbitals but hybridization is the mixing of orbitals yeah we'll do a lot we'll do a lot more example on this because this is very important don't worry with that but first you tell me did you understand this no it's not where is the repulsion I'm not talking about electronic repulsion here yes yes sorry I'm not talking about the electronic repulsion I'm talking about the mixing of orbitals yes yes I'm talking about this only I'm not talking about electronic repulsion it is just a mixing of orbitals so that all the orbitals will have same energy and they combines with hydrogen atom in a similar manner no it's not the only thing see the main you know thing here is like you see in this CH4 molecule the orbital that is involved it has a similar orbital all the four bonds forms by the overlap of SP3S orbital similar orbital we can have similar strength and similar bond length and hence the bond all the four bonds are identical see see one thing one thing here it's not like they take energy from outside or something like that when electrons see when electrons occupy the orbital it affects the energy of the orbital orbitals energy increases a bit suppose we have three orbitals PX, PY and PZ one of the orbital has electron and other two won't have any electron then suppose PX has electron so the orbital energy of PX is slightly more than the energy of PY and PZ right so in order to have the similar energy these orbitals you know intermix and forms a new set of orbitals so energy is there because of the exchange of electron or because of the presence of electron no it has nothing to do with electron pair repulsion hybridization is just a mixing of orbitals yes it is the most acceptable you can say our most satisfactory explanation of the bonding in CH4 molecule and many other molecules yes new set of orbitals are purely hypothetical yeah no no no hybrid orbitals always have the same energy yeah before they hybridize it's fine before they hybridize they have some difference in energy so there only they mix and forms the identical energy orbit but the difference is not that great yes understood shifting of electrons you know if I can I won't say it is not possible it is possible and mostly there it is there in case of correlation compound complex compound so here you won't get in simple compound you won't get shifting of electrons in see the thing is once the hybrid orbital forms right then it is you can consider this similar to similar as atomic orbital everything is completely same the only thing is what the orbitals the atomic orbitals which has slightly different energy they combines and forms an equal energy orbit that is it that's why we have redistribution of energy that depends upon the orbital right which orbitals are there that depends upon the plane and other thing yes understood no we do not have shifting of electron cloud electron cloud will discuss when the bond forms and will have the electron cloud between carbon and hydrogen bond and that electron cloud present in SB3 as overlap that begins shifting of electron cloud is possible in resonance when resonance is there yes yes yeah so this is the explanation of CH4 molecule like you see if you try to find out and hence the hybridization in CH4 is what I remember one more thing when I say that find out the hybridization of CH4 molecule hybridization is only for the central atom like we say like this hybridization of this molecule but we make we this means what that we need to find out the hybridization of central atom right because it is the atomic orbitals of central atom which intermix and forms the hybrid orbit so we always consider the central atom for hybridization okay for the calculation of hybridization like you see if I ask you to find out the hybridization of BECL2 molecule it does not mean the hybridization is for this molecule but it means the hybridization of beryllium in this molecule so in CH4 one last thing the hybrid orbital is SB3 and hence the hybridization is SB3 BECL2 you see beryllium the electronic configuration is for electron so 1S2 and 2S2 right so this is a 2S orbital and this is 2P this is a ground state configuration since it has to combine with 2chlorine so it must have 2 unpaired electron so in excited state one electron jumps into any one of the P orbital we do not know which P orbital is it whether it is PSP or PC whatever it is this is the configuration we have now before bonding with chlorine these two orbitals go under hybridization and it forms two SP hybridized hybrid orbital which has one electron each and these two orbitals the P orbitals are left unhybridized yes now this SP hybridized take part in the bonding and if they draw the orbital diagram it is one two one electron here one electron here hybrid orbital and for chlorine we have P orbital this is the inter nuclear XCC and this overlap is sigma overlap hybridization for beryllium is SP hybridized you see when it is SP hybridized that is linear right understood guys any doubt in this CO2 you try hybridization of CO2 what is the hybridization here yes it is a covalent bond usually it should be ionic but for BE and MG to some extent MG CL2 is partially covalent partially ionic BE CL2 is more covalent less ionic did you draw the orbital diagram of CO2 what is the structure of CO2 is it O double bond C double bond O what is the hybridization of carbon atom in this SP we all know SP hybridized right but you see we have two pi bonds here right I want to I want you to understand the orbital diagram here because that the you know if you understand the orbital diagram we will understand the actual concept here you know it is SP hybridized right okay now you see and we have two pi bonds here and you also know that hybrid orbital never forms pi bond right now you see this two three information you have carbon has six electron so one has two two has two two p two s and two p this is the ground state configuration in excited state one electrons dumps over here and we get two s one now you see what happens here listen to me carefully since it has to make a bond with two oxygen atom it means carbon must have two unpaired electron present in hybrid orbital so what happens this s and one of the p orbitals will take part in hybridization it forms two SP hybridized hybrid orbital contains one one electron this is SP hybridized and two atomic p orbitals will be left unhybridized and why it left unhybridized because I have given you one point in the beginning that if any pi bond to be formed then equal number of atomic orbitals must be left unhybridized yes or no tell me I want you to go through the characteristics of hybrid orbit there I have given you this point that if any pi bond to be formed equal number of atomic orbitals must be left unhybridized why because the you know hybrid orbital won't form right so since we know this fact that CO2 molecule has two pi bond so I just left two atomic orbitals which contains one electron each unhybridized and which we use to help which we use to form a pi bond here now this orbital diagram I am going to draw this one is very very no it will explain all the concept you see to hybrid orbital we have to suppose this one is the hybrid orbital one and two hybrid orbit okay and we have two atomic orbital also so the atomic orbital is I am drawing this with a black ink dumbbell shaped atomic orbital we have one more atomic orbital like this all these orbital contains one one electron so one electron here one electron here one electron here and one electron here this is carbon right the orbitals are sp hybridized answer is sp only that we understood my stuff we are trying to understand the bonding here CO2 right so oxygen also has to look at the electronic configuration for oxygen it is 1S2 2S2 2P4 right so 2S2 is this 2P4 in this you see the 2P orbitals has one one electron each and one is sp hybridized so I am drawing this P orbital here which contains unhybridized electron this is the P orbital which contains unhybridized electron and one P orbital which contains unhybridized electron the other two were this P orbital has a pair of electron this has one unhybridized electron this has one unhybridized electron same thing we have this side also one unhybridized electron for this P unhybridized electron here and a pair of electron right do you see along this line if you can understand this this is the axial overlapping yes or no is this diagram clear orbital diagram axial overlapping now between this carbon and this oxygen two atomic orbitals have unpaired electron so these two combines and forms the pi bond here and here also you see the two atomic orbitals which has unpaired electron this one combines with this and forms a pi electron here let me see the pi electron is formed by the atomic orbitals not by the hybrid orbitals let me just clear any doubt no it is other way Nisha the hybridization is sp that's why it is linear and how the hybridization is sp because we have this explanation it's not like the molecule is linear hence it is sp but it is other way it is sp hence it is linear yes yes yes we can do that wait a second yes we have one more lone pair and that is present in the s orbital I did not draw it here this one you can draw it here see this this is the s orbital this is the s orbital what how do you know that four atoms has unpaired electron in different p orbitals you can draw the electric we can draw it like this no hence you'll be getting filled the electron in the orbital two four five six and then seven like two three four five and six according to hence rule you distribute the electron you'll get to unpaired electron in p orbital so basically if you know the structure and we know the sigma bond and lone pair present on the central atom right we can find out the hybridization of the molecule like this we can draw the structure and we can find out the hybridization orbital right one more example will do on this try for sulphate ion s o four two minus right this one done just give it a try in this yes yes yes yes you have to because there is no other choice you require four unpaired electron because s o four we have so far four unpaired electrons you have to shift electron from s and p to the d subset you have tried now I'll do this you see all your doubts will get clear see first of all oxygen sulphur will have similar kind of configuration so for sulphur if I write down the valence configuration here valence configuration it is 3 s 2 3 p 4 so this one is 3 s 2 3 p 4 and this 3 d orbital is vacant right vacant but since you have four oxygen atom so we must have four valence electron right and in order to get four valence electron this will go here in excited and this will go here in excited state so what we get here 3 s will have only one 3 p will have one each and 3 d will have two electron now we need four orbitals so this is 3 s this is 3 p and this is 3 d and sulphate ion if you know the structure it is s double bond o double bond o o minus and o minus all of you know this do we have any other option by work in order to get four unpaired electron where those two electrons you will shift tell me sir but we don't know where the electrons will go in the 3 d structure right it can be any of the five it can go in any of the five right we don't know which of the five yeah so I am not saying it will go into d x y d y z orbital where it is oh ok ok it just go into d sub which orbital it is not because the next higher orbital is 3 d not 4 s as a 4 s 3 d we have 4 s 3 d we have but the transition takes place in the same shell mother now in order to understand this hybridization here you just have little bit of information you have that is sulphate ion has sulphate ion has 2 pi bond right as double bond o double bond o it means two orbital must be left what two atomic orbital must be left unhybridized yes or no because atomic orbital can form pi bond hybrid orbital won't form right that's why out of this six atomic orbitals which contains one electron each two will be left unhybridized that is in the atomic orbital form right so what I am telling you here out of this six atomic orbital this four will go into hybridization and forms sp3 hybridized hybrid orbital which has one electron each and this 3d electron 3d orbital will be left unhybridized with one electron each like this this is 4 sp3 and this is 3d is it clear till here all of you I am not drawing here the orbital diagram because this 3d you know the d sub shell has you know the structure of d orbitals is difficult to draw here so I am not drawing that I am just telling you here that we will get the structure of sulphate ion is s o 4 2 minus I will draw it properly is s double bond o double bond o o minus and o minus right but this orbital which forms the sigma bond the hybridization of sulphate here is sp3 right sp3 hybridized and that is the answer if hybridization is sp3 geometry is tetrahedral but sometimes they ask this question that this pi bond forms by which orbital overlap you see for sulphur we have d orbital and oxygen has p orbital so what we say this bond forms by p pi d pi overlap p pi d pi overlap p stands for orbital of oxygen that involves in this overlapping is p the orbital of sulphur that involves in this overlapping is d and since this overlaps gives you a pi bond that is why it is p pi d pi overlap p pi d pi overlap looks like this this is p sub shell and t sub shell this is the p sub shell is this and t is this this overlap we have see this if you could imagine along this line we have inter-nuclear axis and this is the p pi d pi overlap did you get it what you did not understand how many of you understood it please type in guys quickly no it is lateral you see axial is along that dotted line this lateral overlap p pi d pi is this it is nothing see the orbital of s that involves in this pi bond is you see it is d orbital is involved right atomic orbital is d only but the orbital of p is oxygen is p orbital so here we have p d overlap which forms a pi bond that is why it is p pi d pi overlap overlap you can write p won't always form pi bond you can form sigma also p can form sigma also mother the first bond between p and p overlap is sigma only yes understood all of you p to form a sigma bond with s if sd overlap is there then it can form sigma bond but we do not have sd overlap but we do not have sd overlap so it won't form no so now whenever you need to find out the hybridization you have to do all these things to find out hybridization okay which is which is time taking you see it takes a lot of time to understand the behavior of the molecule and the structure of the given molecule what kind of bond is present but always what you can do with the louise dotted structure you can draw the structure like this you can count the number of sigma bond and pi bond and you can find out the structure here but we will do the calculation of hybridization which what is the hybridization of molecule by a trick and the trick we are going to use is a steric number rule the actual the concept is that one only that we have done v cl 2 co 2 s 4 2 minus okay that is the actual concept but in the exam we can do by this rule it saves a lot of time and effort of you right so what is steric number rule steric number is number of bond pair plus loan pair on central atom because we always found hybridization for central atom or we can also write this as number of outer atom number of outer atom you know it is nothing but the number of bond pair number of outer atom plus the number of again loan pair on central atom is steric number now based on the steric number we can write down the hybridization you see this table here steric number and hybridization with hybridization you already know what that what should be the geometry of the molecule so steric number can be 3 4 5 6 7 if it is 2 it is sp hybridized if it is 3 sp 2 if it is 4 then sp 3 if it is 5 then sp 3d if it is 6 then sp 3d 2 if it is 7 then sp 3 excuse me sir are you talking no did you copy this oh yes sir we copied so how do you find out steric number could you tell me I have discussed this already bsdpr you remember how do you find out number of bond pair and loan pair right valence electron divided by 8 you remember that trick yes correct no it is not don't pair plus bond pair it is q plus r by 2 yeah calculate valence electron divided by 8 quotient gives you bond pair and remainder that is r by 2 gives you loan pair yes q plus r by 2 method okay so q plus r by 2 gives you the steric number and then you can find out the hybridization and then geometry and other things right so basically that steric number gives you the idea of the geometry of the molecule of the hybridization of the molecule plus the shape of the molecule geometry hybridization and shape you can find out from that steric number I'll give you some example now okay and I want you to do all these p o 4 3 minus i 3 minus n o 3 minus c o 3 2 minus x e o 3 f 2 i o 2 f 2 minus and c l f 3 so the first one is p o 4 p minus okay what we'll do we'll find out the valence electron tell me the valence electron here p o 4 3 minus how many valence electron we have e is 32 so I'm trusting you right I'm not calculating this so number of bond pair is 4 number of loan pair 0 steric number is 4 hybridization is sp3 and with sp3 hybridization you know geometry and shape both are tetrahedral because the loan pair is 0 i 3 minus the number of valence electron here is 22 so bond pair is 2 loan pair is 3 steric number is 5 geometry is 3 and shape is sorry hybridization we need to write now so it is sp3d hybridization geometry is tbp what is the shape of the molecule shape tell me it's linear right n o 3 minus number of v is 24 bond pair 3 loan pair 0 steric number is 3 hybridization is sp2 triangle planar geometry and shape c o 3 2 minus the bond the valence electron is 26 bond pair 3 loan pair is it 24 let me check 6 into 3 18 plus 220 20 plus 4 it's 24 not 26 it's 24 nishan it's 24 3 and 0 so it is sp2 triangle planar e o 3 f2 tell me valence electron ve is 8 plus 14 no it's 40 not 30 it's 40 yeah bond pair is 5 loan pair is 0 so it is sp3 3 d hybridization triangle bi parameter i o 2 f2 minus tell me valence electron is 14 plus 12 that is 26 26 plus 7 33 34 because if you want to find out the bond pair and loan pair of electron on the central atom you need to have the valence electrons okay go back and check where we see pr anura bond pair is 4 loan pair is 1 so it is 5 sp3d what is the last one tell me the last one triangle bi parameter sp3d and the shape is t shape is it this is for the molecule in organic molecule which is given you can find out like this the valence electron if you have a structure given like this like suppose we have CH3 C triple bond C single bond CH double bond CH single bond CH 2 single bond CH double bond C find out the hybridization sir the C to the left of the cyclic component should be CH right because there are 2 double bonds okay tell me sir I was asking sir the the carbon which is to the left of the cyclic the ring so it will be CH right this one yeah yeah we have one hydrogen here that is understood no sir for the so I'll do something so I'll add one ring here no tell me the hybridization of each atom carbon atom you don't have to name this okay then so the first one I'll write down here only it is SP3 SP SP SP2 SP2 SP3 SP2 SP2 SP3 SP2 SP2 SP3 SP3 SP3 this one is SP3 SP2 SP2 SP2 carbon is SP2 nitrogen is SP3 this is SP3 this is also SP3 this is also SP3 this is SP3 even this one is also SP3 SP3 and SP3 right if you know the structure just to count the number of sigma bond and lone pair present on the atom you will get the hybridization once you know the hybridization you know the geometry of the molecule you know the shape of the molecule right based on the bond pair and lone pair then all of you now you see the another thing here is name we don't do we cannot this is not at all required okay it is so lengthy okay so ignore that yeah so you see if you look at the structure of the oxygen molecule we have O double bond O this two lone pair on each oxygen atom and all the electrons are paired right all the electrons are paired so this particular you know distribution of electron according to BVD valence bond theory suggest that suggest that the molecule is is diamagnetic right when there is no unpaired electron then the molecule is said to be diamagnetic whatever the electrons are present all are paired diamagnetic molecule okay weakly repelled by the magnetic field if the molecule contains any unpaired electron then the molecule is said to be paramagnetic okay that is the definition of diamagnetic and paramagnetic molecule so according to BVD you see the electrons which are present on oxygen atom all electrons are there and it is said to be diamagnetic molecule but the actual behavior of oxygen molecule it behaves as paramagnetic this observation that is done based on VBT was found to be wrong because experimentally 2 is found to be it is weakly attracted towards the magnetic field right it is paramagnetic and hence it is you know the bonding or the property of oxygen molecule is not defined by VBT that is valence bond theory okay and hence we require a new theory to explain the magnetic property of molecule and that we call it as molecular orbital molecular orbital so in this also the orbitals combines and forms molecular orbital right but the difference in hybrid and molecular orbital is that in molecular orbitals orbitals of different atom combines but in hybrid orbital orbitals of same atom combines you look at the all the examples that we have done as a force you to be easier to the orbitals that intermix is the orbital of central atom only one single atom but in molecular orbital the orbitals of different atoms combines and forms molecular orbital that is the basic difference between molecular and hybrid orbital so we'll see how this molecular orbital forms right what are the you know method we have by the atomic orbitals of the two different atom combines and forms molecular orbital and how this theory explains the magnetic property of oxygen molecule right okay so this theory will start after the break any doubt in this till here any doubt fine so what is MOT will discuss after the break take a break now will resume the session at 6.45 okay take a break guys