the elements of the periodic table that have the last electron reaches their There is not just one such d orbital but several The elements are in the periodic table and such all elements taken together are called d block elements hello everyone i hope that you are all good and today I brought hmm class 12th chemistry d block One short video of the elements is always will eliminate the entire d block elements in just this one video and D&F This is our first look at block elements After watching the whole video, As always your concepts will be Crystal clear so I am the light from Lan Hup the free learning platform where You can study Physics, Chemistry, Maths, Biology etc. You can read something absolutely for free at learn.com I am sure everyone will be ready people let's get Group numbers of the started periodic table Locate from group number three to group number 12 We call the elements that contain d Block Elements are called Transition Metals It is also called because of their position If you look carefully at the periodic table So s block elements and p block are located between the elements Transition metals as we all know that wherever there are A block elements On the other hand we mostly find metals if Let us go to the opposite side where P block is located There are elements where we find most nonmetals right in the middle these metals which are in the middle, these There are elements which show transition We have a journey from A to P block and that is why they are called the transition metals d block elements Why do we call them that because these the last electron of the elements The electron is the outer most d goes into orbital okay let's take an example yes let's talk about nickel so nickel's if We look at the outer electronic configuration focus then it sage 3d 884 s2 ok What will you feel when you take a look at this Ma'am the last electron is 4s I am going d I am not going But actually this is not happening which is happening with the outer screen. the most electron is the last electron he's going in 3d not 4s like this why is it so because electronic When we write configuration then who we write based on the principle of of bo principle absolutely correct what we Let's decide which orbital will be filled first which fill will come after that which fill will come after that Phil will be how we find it out in order of their increasing I learned about energizers last minute, like 1s 2s 2p 3s 3p so in this order off bo According to the principle we are Electron okay let's keep putting it in so this off bow As per the order of the principal, when we The ones that add electrons are 4s and In 3D, whose number comes first? Why does the number come 4s because 4s for n + l remember the n + l rule of n + l When will the electrons in the one which has lower value be I will go first, I will go later, we'll see let's talk about the 4s in the case of the 4s in the case What is the value of l 0 The value of n is 4 So 4 + 0 is 4. Okay, now let's talk about 3D. In this case the value of n is three and that of l is what is the value of d orbital AD value of d there is two so that means here 3 + 2 that is 5 So where is the value of n + l greater than 3d there is more in it, that means the electrons are later will it go in 3d first which will it go in 4s It will go okay, I understood this a little I got I'm pretty sure I recapped it You all were with me in 11th class chemistry Have you read all these things or not? If it is there then go quickly and read it. So for now it is enough to know that As per the principle of Bhaiya of Bow Our electronic confine writes and According to that confine we see that Our 4s is filled first, then 3d I feel that what I mean to say is that if we If we talk about nickel, then its last one Which orbital are the electrons going into is going into 3d d orbital So it is a d block element talk about it Outer electronics of iron key look at the confine th 3 d6 4s 2 so which one is the most The last electron went into which 3d went inside so it is d block element So overall my story is something like this All the D block elements for kids their last electron is always goes into a d orbital now here this A doubt at the beginning of the whole story I make it clear many times that we It is said that only D block elements We can also talk about transition elements or transitions. Metals say right then many people The question that comes to mind is whether All of these are d block elements Are they transition metals or transition metals? The elements are well here you have to tell one thing Need to know about transition metals or Then how do we define the transition element we say that it is like this There are elements that are incompletely filled d orbital is listen very carefully d The orbital is incompletely filled if this is the case regardless of its ground state but in any other oxidation state what we need is its d orbital should be fed incompletely if this happens then we call it a transition element okay now this means that joe d Most of the elements are d block Elements that are there transition elements but there are some exceptions which are d There are block elements but those transitions does not contain elements such as zinc like cadmium like mercury why their Look at the electronic confine of zinc If we look at confine, then 3d 10 4s 2 d The last electron has gone into the orbital but D orbital is a complete feed, so That is, it is a d block element but this is not a transition element talk about it 4d 105s 2 of cadmium same story here that brother d orbital is complete feed i.e. This is also not a transition element, talk about it Mercury's 5d 10 6s 2 or same here Exactly same to same story friend that D What is a block, it is a complete field, so Zinc Cadmium Mercury which is this transition There are no elements, the same question as always that maam why to study d block elements Hey friend, there are so many precious metals Be it gold or silver be platinum, under whose influence do all these fall all of them fall under d block The elements are not only as many as Industrially useful metals are: Iron, copper, titanium - all of these also fall are under d block elements so brother where But there are so many important elements I follow it, you can leave it without reading it can't leave it at all That's the time we go to D Block Would have given the elements a little bit of high halo Let us introduce these elements There are a lot of elements along with it But we can see them inside D block. How will we understand these if they are arranged in a row? Each and every row has been liked by us A series is called as First Series second series third series fourth series ok we also notice that a series The elements that bring it into the body are: There are a lot of similarities between them infact We will shortly review their properties. We will also read about the trends for now It is not necessary that all of you remember the series because that is Not really required at your level but If you remember our first series If you keep it then you will benefit because Going forward, when we look at the trends in properties If we understand then everywhere we will do the first series You will understand only by taking an example, if you If you remember that series by heart then you will be trending it will be very easy to understand so Let's have a special meeting first Scandium Titanic Nadium from the series Chromium Manganese Iron Cobalt Nickel Copper Zinc so this is our first series and it You have to remember, how will you remember the memory Of course I give you some tips here A memory tip to science teacher Vani Kaur Ask for Cobalt Nickel Copper Zinc again Once again Vani Kaur will be the science teacher Ask for Cobalt Nickel Copper Zinc Clear So if you remember this statement, you will This sequence will also be remembered very easily Now just like this if you want you can do a second Memory Tip for Series Third Series Itself You can make it and if you have such a memory tap If you make it then definitely write it in the comments tell me then we will talk first So in general the electronic configuration of which are d block elements The electronic configuration is something like this It is of the format n - 1d 1 to 10 n s 1 two 2 means it means that the brother who is a orbital s orbital will be n a orbital now that could be 3s 4s 5s 6x isn't it one of ns2 can have two electrons because There are maximum two cells in any s orbital and the n - 1d right In orbital it can now be n - 1d 3d It could be 4d, it could be 5d, how many are there in it Electrons will be 1 to 10, maximum 10 only There can be d orbital from one to Anything between 10 and 16 electrons You can have outer electronics in it configuration which is any d block the element will be something like this okay like this I've already explained why configuration happens Told that according to the principle of how do we fill the electrons in the order of Increasing Energy of the Orbital How do we find out the increasing energy n By + l rule the value of n + l which is greater he has more energy okay so that We fill the electrons in sequence are in different orbital okay so off bow The sequence which follows according to the principle it goes something like this 1s 2s 2p 3s 3p 4s 3d and so on which is the outer most shell we call it valence shell like Assume that the general configuration has a S A which is that denotes that this s is that is the valence shell right after that n -1 Which is the shell that is that's what we call the Pen Ultimate Shell and that It also has an inner shell which we call it It is called Anti Pain Ultimate Shell Terminology you should know Although you will see that when we discuss No, we mostly tell you DS just like this which orbital are we talking about but these are some of the terminology that you You should know the outermost shell valence the shell inside him the penalty mate inside him wala anti penalty mate so kids now we We are going to discuss D block elements about trends that mean different things How is the trend of properties in a particular The thing we notice here is that D Horizontal in case of block elements There are more similarities when compared to Do you understand group similarities group which there are vertical columns ok but here But we notice that the horizontal row has elements that bring in values such as The elements that are in the low series one are: there are many similarities in the same way There are two series in which there is a lot of difference between them there are similarities and so on okay so Here we will discuss all the properties We will discuss everywhere based on A series or brother what is in this series Are there similarities or are there exceptions and I mean let me tell you up front that bro d When we look at trends in block elements If you read it, you will get exceptions everywhere. The exception which is part of D block If the elements are ok then which properties We will discuss physical properties We will then discuss atomic size then the ionization enthalpy Oxidation States Standard Electrode Potential Magnetic Properties Catalytic Properties Formation of Coloured Ice complexation interstitial compounds so brother The list is long yes so let's go through these one by one Discuss all the properties in detail We will understand the trends conceptually First of all, we are going to talk about physical properties okay so as the name work exactly as i said d We call block elements transitions Why metals? Because when we are physical If you look at the properties, inside them Lots of metallics, like metals Properties we get to see here such as tensile strength ductility In other words, it's like we pull the metals Can be made in the form of thin wires right we call it ductile or ductility so the property of ductility we It is also seen in these elements If you say dirty, we will beat them thin. can be made in the form of sheets e.g. Aluminium sheet is a sheet of gold If it happens right then this is also one of their specialties It is metallic and has a shine like metal There is high thermal conductivity on their surface In other words, it allows the heat to pass through itself. These provide high electrical conductivity electricity to be conducted through its Let them have one more typical metallic structures at room temperature though There are some exceptions, such as zinc. Cadmium Mercury They are very hard and very What is low voltage volatile which is big Easily goes into its vapor state But he is not one of those who go away easily They are right but there are exceptions to these too Which zinc, cadmium and mercury metals are Similarly, their melting point and boiling point are also different. It is quite high, why does this happen, the question is It must be coming to your mind, let's understand ok now see what the melting point is we can melt anything like Suppose let's take the example of ice. it is in solid, if you melt the solid What will happen if it goes into liquid then it will become solid to be transferred to liquid form from Basically what are the particles happening inside should increase the distance between is right because the particles in the solid We make very close pacts with solids If you want to carry it in liquid then the bonding that occurs between the particles By breaking it between us, we keep them a little distance away then it goes into liquid state I mean you are understanding the peacock and lace thing Great now see what will happen here we Talking about the elements of D block We are talking about the elements, one special among them The thing is that those who have valence shell electrons i.e. the AA ones which electrons and the pen is the ultimate shell electrons, that is, n - The electrons that are in 1d are both Only electrons participate in these inter atomic metallic bonding which bonding It makes those who participate in it There are many electrons in the valence shell There are also Pen Ultimate Shells Both of them participate together, right? Now everybody knows that brother which electrons in bonding etc the outer electrons evolve the outer electrons now these ones here If the number of electrons is so large then what will happen the more you have The unpaired electron will remain in the outer shell How strong will the bonding be now? The stronger the bonding, the more it will melt It is so difficult to get it done or to boil it it will be absolutely correct because By breaking that bonding you We have to send them far away to understand the right story I understood the logic, great means this Overall the bottom line of the story is this that the greater the number of unpaired the higher the electron is, the higher the bolic or The melting point will be right meaning greater the number of unpaired electrons higher is the Understanding melting point and boiling point I have seen superb now see the trend here If we try to understand the trend So do I have to look for it Electronic Confine OK Series One Pay We will focus on what is our series one Scandium Titanic M Tenniel is not from us The science teacher will say okay from the memory tip Vani asks for more Cobalt Iron Copper Nickel Okay so now if we look here So first of all what is scandium scandium what is the outer confine of 3d 1 4s 2 her after titanic let's go 3d 2 4s 2 then 3d 3 fors2 3d 4s right what's happening what's happening As we move left in the first series going to the right what's happening The electrons in d keep increasing okay first there was an electron now Look how many boxes are there inside d there are five boxes what is the right box We are basically inside the d orbital You can add a total of 10 electrons, right? These are the basic things that we have studied before how are all the 10 electrons added first One electron is put into the box at a time After that one by one more pair up happens Isn't it so, in the same pattern as the electrons? Let's put it in, right? So now see what happens will happen from scandium as we go So what happens on the right side is first 3d 1 That is, there is one unpaired electron in d Then 3d 2 i.e. two unpaired electrons Then 3d 3 means three unpaired electrons then 3d unpaired electron then 3d 5 five As soon as the unpaired electron but 3d s So how many unpaired electrons are back? So there are four unpaired electrons right? So what I mean to say is that the number of unpaired electron is moving first going to the middle and getting maximum after that Again the number of unpaired electorate decreases If so, then according to this logic, your How is the trend of melting point or bolic? it will also be like this right that first he will increase will increase will increase maximum in the middle After that its trend will decrease Why would it feel like that because we just learned that The greater the number of unpaired electrons the higher the melting point or The boiling point will be infact if melting If you look at the graph of the point, then look at the graph as well how does it look like in the middle some how sa maximum is coming right like this The graph is there but exceptions are everywhere As I said earlier, right Look in the middle, there is manganese where there is a rotting substance There is a dip, look in the middle there is a TC Technician there is a sudden dip there as well these are exceptions but in general if you If you look at the pattern of the graph, what is the pattern like? the melting point is increasing, increasing, increasing It is increasing at maximum in the center then it starts decreasing right and now this Everyone should understand why the trend is like this. The next physical property we will discuss is do that is enthalpy of atomization okay First of all, we will understand what happens Understand that these are the d block elements don't they have high enthalpy of atomization That's alright ma'am but what is this enthalpy of atomization so look at enthalpy We call the enthalpy change of atomization are which companies separation of all the atoms in a given substance okay if we take a If we talk about transition metal then it is Transition metals form lattices How will the lattice be formed between the atoms A Fix From Bonding to a Perfect Lattice The structure will be built, right, but I am saying it Enthalpy of atomization means that all these atoms are there right, all these atoms Separating the atoms, that is atomization When we want to separate these atoms then What will have to be done to the bonds between them all those bonds have to be broken and As we know, any bond We have to provide energy to break it energy will have to be provided, right and this energy We will have to pay for this energy accounts The Enthalpy of Atomization Explained super now this means when I did this He said that these are d block elements They have high enthalpy of atomization that is, if I have to see their atoms If we want to separate out then I am not able to do that. You have to give all your energy ok this is clear now let's understand How will the trend of this trend be? It's the same story from back then, see how many more valence electrons will be valence what do electrons participate in The more valences in bonding The more electrons there are, the deeper the bond will be the stronger the bond will be and the more Energy has to be expended to break that bond right for so what would be that much Enthalpy of atomization will be okay okay so If I were to look at a trend, the trend I have to focus to see what Pay Electronic Configuration Pay What does the electronic configuration say Brother, talk about the first series, okay? Science teacher Veena Kaur asks for cobalt again nickel copper zinc is ok so if first When we talk about the series, what do we Let's look at the electronic configuration focus on outer configuration 3d 1 then 3d 2 then 3d 3 then 3d 3d 5 right what is it is the number of unpaired electrons d The more we are growing in orbital Unpaired electrons are as deep as bonding The stronger the bonding, the more Energy has to be given to atomize them in order to separate their atoms That is, the enthalpy of atomization is also As you go from left to right It will increase, it will increase, it will reach its peak in the middle And after that the right will start decreasing again And that is what exactly the graph is If we also look at the Tales as graph The graph looks almost like this but as I told you earlier that half of If an exception is made then this was the story the first series of a series now when we Looking at the values of enthalpy of atomization are you from second series or third series then we What do you notice? Focus on the graph. It is clearly seen from the graph that The enthalpy of atomisation of the second series it is more of third than first series The enthalpy of atomization of the series is If it is more than the second series then kids now The next trend we are going to discuss is that is atomic size atomic size Explains two con concepts first is the effective nuclear charge which we call It is said that Z is effective and the other one is Screening effect: First of all, we will Let us first understand these two concepts Also discussed are mostly class 11th But there is no one to discuss again in chemistry we will do it okay now look at any atom What is the arrangement of electrons inside There is a nucleus in the middle, which is positively charged, and then This is how electrons are arranged in shells okay now the one who is on the outside the electron which is the outer most electron What is the charge of the nucleus? The experience will depend on that between this electron and this nucleus How many more electrons are there in the correct thing I am understanding that it is like let us suppose that you're sitting in a classroom right now The teacher is writing something, something, something on the board If you are teaching by writing then there is a lot of Everything is written down, okay, now you can lie down No matter where you are sitting, sit on the last bench ho butt board and anything in between you What will happen to you if you don't have it at all The board will be clearly visible but let us Suppose I put curtains in between I have put up a thin curtain and now you It won't be visible that clearly now that I have looked at the middle If I put two or three curtains then what will happen to you What was the clarity that the board provided for you? it will keep decreasing right so that means these are the screens, these ones in the middle electrons what do they produce Is it a screening effect or a shield? Effect okay now that you are sitting you can effectively As much of the board as you can see We say that speaking effectively means The outer most electron is How many positives are there in the effective nucleus? We are experiencing the charge It is said that the root is effective or effective Nuclear charge understood this story ok so in this story whose There is evolution in the story that brother the outermost electron and in the middle of the nucleus did someone else Have you put up a lot of curtains? Electrons have evolved on these things It depends on how effective brother is or what will be the screening effect Children, now understand this logic very carefully As the z effective increases the z effective will increase, meaning that the outer electron Experience an effective positive charge The right of the nucleus is like that What will happen to this outsider as it grows? in the electron and in the nucleus Attraction will increase when there is attraction in them If the size increases then it will be smaller right This is exactly what should happen and this is exactly what happens Ok, now let's see the logic behind the trend Did you understand it? Now you will see the trend. when we look at the trend we first The series goes from left to right okay as we move from left to right if we go then what is happening to me The atomic number increases by one it's happening okay the atomic number is increasing So what is happening as the true number of layers So the edges are not really increasing in between the curtains It is not true that only electrons are coming The outer shell is growing one by one in okay so that means screening which it is not happening so much but the Judd is effective right means with each Electron added which net root we experience what you are doing is just as right in a They we can say that as we move left Screening moves to the right from The effect is not happening because of which If layers are not increasing then size increases there is no question of it happening okay so size rather what is happening size rather less Why is this happening because the root effect is increasing is the effective nuclear charge which is If it is growing then that means in the middle If attraction is happening then the size is getting smaller ok so my story was going well Scandium Titanic Chromium Manganese Iron The story was going well till here what was happening, the size was decreasing why was it declining because the z It is effective, what was happening, it was growing It was ok but what happens after that The size of iron, cobalt and nickel it becomes equal why does this happen This happens because if you What if you focus on electronic conferencing? is happening by the time we get to the iron Till then the number of electrons in 3d is There is also a considerable increase in scandium Let's start with 3d 1 then 3d 1 3d 2 3d 3 3d 3d 5 3d s right so when the d orbital the number of electrons becomes much higher in so what starts to happen is that these electrons are those in the d orbital electrons are those in the 4s orbital These are electrons, these electrons are also among themselves Now the correct electrons start to repel There are so many brothers that these people are fighting with each other I am repelling these people myself The screens are becoming Screening effect is coming in the picture So what is happening now from iron to cobalt and We expected more from cobalt that brother the reason for the effective increase Their size should be smaller than but Due to the repulsion of electrons, their The size is a little bigger and one side is smaller Should have been a little bigger on one side So overall their size becomes equal okay after that when we get to the first copper and When we go to Zinc, what do we find there? Let's see brother atomic size decreases Atomic size increase is far from happening Why did this start happening because copper zinc As we go up to the number of electrons and If it increases too much then there is a screening effect Now it has become stronger so here The effect of the screening effect is that The root became more than effective whose because of what started happening here the size which it has started increasing okay so it's complete The concept of atomic size is known to everyone If you understand then look at the atomic size Two things to understand the whole concept It must be absolutely crystal clear first z effect second screening effect then Whenever we see this trend, what's happening to the iron at the beginning is z effective more pre dominant because of which atomic size decreases what happens after that is iron cobalt Nickel is as much root as is in this section The more effective the effect the heavier it is The screening effect outweighs Because of this their sizes are equal Then when we moved towards copper and zinc when we go there then there is a screening effect The side which is on the shoulder becomes heavier because of which If atomic size starts increasing then Brother this was the story from left to right down What is the story of The Group? Now look at what we have Read the trend in your periodic table According to that we were from top to bottom what happens whenever you go The number of shells increases so the atomic The size increases in this pattern when we If you observe here then brother series one And this pattern is seen in series two. is the atomic size of series one Correspondingly to Series Two What do we notice when we look at the ments? Let's use elements from Series Three The atomic size is that of series two is equal to the atomic size of the elements Ideally, they should have increased because down the group atomic size increases but why did it not increase here and The answer is lanthanide contraction so kids what is lanthanide contraction Contraction means something being contracted Smallness means Lanthanide contraction There is regular decrease in atomic size Due to the filling of 4f orbital before 5d orbital is ok evolution of 4f orbital As soon as it becomes electronic right there in the configuration we have to see Why do we get ethaneide contraction? because the f orbital electrons This is a very poor shield effect What they mean is that they are very good Does not work like screens Understand it like this that the curtain is not that curtain If the curtain is transparent If it happens then the shield effect will not be good right so it means when the shield effect is good if it is not there then what will happen which is the outer most electrons and the nucleus The curtain in the middle is not very effective which means that outside Electrons are more effective Nuclear charge experience will do right So what will happen if z effective is more Its size will be small, you understand that Why does this happen? Picture of 4f orbital Why does contraction occur as soon as I come in Because 4f electrons are not only 4f but any other electron f orbital electrons which are very Poor shield effect is shown due to which z effective is greater than z effective If it is too much then the size is small So now let's go back to our trend What did we see on the trend, down the group we I expect that brother size will increase It should happen if we go from series one to series two Size increased exactly from series two When I went to series three, the size remained the same why did it remain because from series two to series three As soon as we went to three, we expected did that the size would increase but lanthanide The size got reduced a bit due to the contraction Edge result became equal between series 2 and series 3 Size of three is clear now another exception look here is not exactly the exception which The first group is Scandium Vitum Lantham this is my first group here We see as we go down size increases Doesn't it mean that vitum is also larger than scandium? Lantham's size is also increasing due to white is increasing then you must be thinking that Why are the sizes not equal here? It did not happen because Lanham is that is not a block element of lantham If we look at the electronic configuration So it's 5d 1 6s 2 here on the f orbital. evolution has not occurred because a If the evolution of the orbital has not occurred then There has been no construction, that is why here There are no exceptions here as we go down the group size increases but after that from the rest of the groups that are there The elements which are at number three, that is, those which The elements of the third series are which are of Lanthanide Right Third Series What are these elements? These are the f block there is an evolution of the due to which we Let's see there whether Lanthanide So kids, next we will discuss construction ionization enthalpy ionization what is enthalpy in simple words what does it mean to organize Look at that electronic confine The outermost electron is how much energy do you need to give to extract it she is studying so that basically tells you the Ionization enthalpy means the process of ionizing it How much energy do you have to give for this? is it's ionization enthalpy okay perfect so How should one trend in general In the periodic table, if we look from left to right ionization enthalpy increases as There will be an increase, okay brother, we are studying are the d block elements where the exception is If there is only one exception then there is something here There will definitely be an exception here too notice as we move from the left move to the right if we talk about Series one i.e. scandium titanic Nadium Chromium Manganese Iron Cobalt nickel copper zinc here also when we left If we move to the right from the ionization Enthalpy increases except at Few places such as titanium to nadium till an exception is seen like that iron cobalt nickel here we have Exceptions are seen in these two What do we need to see in these two positions? we get that the ionization enthalpy Instead of increasing it would have been decreasing Now I already told you brother that D If you read block elements then you will get an exception Meaning it is in every vein of D block then you You will get a lot of exceptions, okay let's go And let's see what interesting things happen When we look at the trend of ionization enthalpy, we notice that zinc The ionization enthalpy of cadmium and mercury hota hai that is very very high they have the Why does this have the highest ionization enthalpy? why does their electronics answer this confine if their electronic confine So look at what it looks like that their d orbital Their s orbital is fully fielded It is feed, it is fully feed, it means completely He is stable, he has no disturbance I don't want it but you are saying no I want to ionize an electron Now I want to take it out brother, such is your demand that you make a stable person unstable If you want then why won't that person agree Right will accept it because he will not agree You have to give it a lot of energy to ionize and that is why zinc Ionization enthalpy of cadmium mercury Now the ionization enthalpy is highest while we're still talking we're talking are the first ionization enthalpy i.e. that if we were to remove the first one electron so that is the first ionization of any Enthalpy Now suppose an electron has I have taken it out, now I feel like choosing another one Brother, should I take out the electrons too? There is no end, I took out one, take out the other if so, the energy that would have to be expended at that time is ionization enthalpy to second order which we call the ionization energy So when we calculate the second ionization enthalpy So what do we notice here? Let's see keep looking at the values keep watching the trend of values okay you you will notice when we specially second If we are talking about ionization enthalpy then Here, chromium and copper are two such elements whose value is equal to Their value is more than what was required, right? who listen to me carefully seconds When talking about ionization enthalpy So the value of chromium and copper should be Their value is more than it should have been Why also answers this why The electronic configuration of chromium Look at the outer electronic confine it says 3d 5 4s is 1 right so when we have the first If we removed the electron then what did we remove? I took out 4S One so what's left now? what is 3d 5 3d 5 half feed d orbital half what is feed confin is it stable Now from this half field confine you're the second If you are trying to remove an electron, he will accept it he will not agree, he will not agree that is why his Its value is second ionization enthalpy There is a lot of talk about copper Look at the outer configuration of copper 3d 10 4s 1 okay so when the first electron you which one did you take out 4s 1 Now when you want to take out another one you Where are you trying to get it from 3D 10 is a joke Is there a 3d 10 fully fed edge table or not he will let me take it out but he doesn't let me take it out that's why Its second ionization enthalpy is that is very high than it should have been why is it so much because brother its Confine is fully stable it is stable I do not want to be unstable, this is exactly what In this way, if we focus on third ionization Don't worry about enthalpy, it means remove two electrons even the mind of the third electron is not satisfied now also have to take it out okay so when the third If you focus on ionization enthalpy What will you notice here? Manganese Notice the value, the value of manganese is quite It is more than it should have been It is much more than why it is more than Think you will answer it yourself right electronic configuration of manganese look 3d 5 4s 2 first electron removed 4s the second electron was removed from the Taken out in the forest again, now what is left in 3D 5 Half Field Stable is not to be given to him electron but you have to take it now if If you want to take it, you will have to give a lot of energy that is, the third ionization enthalpy that is very very high infact if we in If we focus on values, we see Nickel, Copper, Zinc for these three elements which is the value of third ionization enthalpy that is like very high and such a high value This thought of ours or this question also answers why these elements In we have more than two oxidation states It is not available whether it is copper or zinc Even if there is nickel in it we have more than two Oxidation state is not found because because after removing two electrons Much of this is more difficult Because their third ionization enthalpy is very very high now we will discuss We look at oxidation states that all the d block elements which are desho variable oxidation states However, there is an exception to this, and The exception is scandium and zinc right then Meaning if we focus on the series first Scandium is on the extreme left Zinc is on the extreme right There are two exceptions on the right side: Multiple or variable oxidation states Apart from this, I do not do any show for everyone else Shows all variable oxidation states why do they show variable oxidation Think a little about D Block Elements If we look at the electronic confines of Their valent shell is n A and pen ultimate shell means n-1d now in the energy between the two energy levels There is a gap that is very less right because of which What happens when you jump from one to another? It is a little simpler to do because you jump It is simple to cut, that is why we Variable oxidation state is observed okay let's give examples one by one First of all, we will talk about exceptions that's ok scand sm if we confine if you look at it its outer confine says 3d 1 4s 2 okay now scandium thinks that Brother, everybody thinks that we should be stable Being stable is everyone's concern is the same for scandium so scandium thinks two of the 4s do one thing electron 3d one electron these three give away the electron if So what will happen if you confine the noble gas will go i.e. stability right then Scandium says brother take these three If I gave away the electron, then its what is the oxidation state + 3 so Scandium only + 3 oxidation on the other hand if Talking about zinc, the configuration of zinc look 3d 10 4s 2 okay so zinc thinks that if I could somehow get both of the 4s What happens if I throw out the electron? I will come to +2 oxidation state but At the same time, my 3d orbital is He is fully fed, which means he is stable right so zinc thinks okay then my For this, +2 oxidation state is good. So this is the story of scandium and Zinc means the two sides Extreme Ends Are Their Story Done where we have variable oxidation state I don't get to see it, let's talk now titanium from leaches of other elements If we talk about titanium then the outer If we focus on the confine then its confine is 3d 2 4s 2 okay now look there are many there are possibilities there is a possibility that brother Titanium donates only two electrons of its 4s then its oxidation state will be + 2 If it loses two electrons of 4s and one electron of 3d then its The oxidation state will become + 3 if it has spent 4s also donated two electrons of 3d and two of 3e If it donates electrons then its oxidation state will become + 4 right so that means here But it has multiple possibilities The oxidation state can be +2, +3 or +4 it is possible then kids when it is possible for all of you If you look at the oxidation state, you will see a what kind of pattern will you see The elements that bring you in the middle Their variable oxidation states are many there are 4 five 6 seven so many numbers off are the oxidation states and as we If both go to extreme ends then Variable oxidation states are reduced look right you saw scandium yourself of is the same of zinc is the same but If we move a little further from scandium towards the center Titanium has three in the case of nadium There are four + 2 + 3 + 4 + 5 doing this If we talk about manganese, then from + 2 to If the oxidation states are up to +7 then these are why do we see such a pattern This is why the pattern looks like this Because to bring it to extreme ends the elements that are either have so few electrons that they So many variable oxidation states attended cannot do this as can scandium in case or they have so many electrons are those electrons You don't want to share it unnecessarily as in the case of zinc it's okay Now let's look at another example: manganese If the outer electronic composition of manganese is Talking about confine it is 3d 5 4s 2 So now look at how much manganese you have There are possibilities There is a possibility that the 4s if both the electrons of the The oxidation state will be + 2 second There is a possibility that both the 4s will come out and If only one of the 3d states is found then the oxidation state the third possibility is that of 4s If both come out and two come out of 3d then The oxidation state will be + 4 by doing this One last possibility would be that 4s will also Both should come out and all five of the 3d should also come out If so, in that case the oxidation state would be will go + 7 so in total we are looking at How many oxy states are possible here of manganese + 2 + 3 + 4 + 5 + 6 + 7 so All oxidation states are possible Although, out of all these oxidation states, Which of the two oxidation states is more stable + 2 end + 7 why because look when + 2 The oxidation state is occurring at that time how is the configuration 3d 5 right because 4s 2 so we figured out 3d 5 which that half the field is stable in the same way When we talk about oxidation state of + There are two 4s also going out and 3d phoens are also coming out so be careful what is the noble gas configuration that is stable in itself so that is why + 2 and + 7 these two oxidation states which are if there are more stable oxidation states then Kids now we are going to talk about standard Regarding electrode potential, here But which electrode potential do we use? If we talk about m2 + m then it means that The easier it will become standard, the more easily it will be compared to m2. The value of electrode potential is It will be more negative, okay what is this m means any element let us say that in these We denote any one element of this by m. what should he do to get to m2 two electrons would have to be loosed only then That will become m2 p, so m will be equal to m2 p. Electrode potential will be easily created The more negative the value the better So now let's see that these standards What is the trend of electrode potential? It happens, it's okay, we'll see the trend From left to right we go into the series before Let's we see that as we move from left to right Standard electrodes go to The value of potential is less negative it goes away meaning the value is negative but The value is becoming less negative Although it is a D block element, so brother If there has to be an exception then it is an exception Here too there are many places to see exceptions As in the case of copper we get Let's see that the value is not negative rather positive, in addition manganese We see nickel zinc in all these cases that the value is more than it should have been is more, that is, the more negative it is They are more negative than they should have been Values: Now this question will come to mind brother what is the reason for these exceptions No and who will tell the reason for these exceptions electronic confine means that the question There are many sessions for every question, every problem where is the solution hidden in the electronic configuration it is okay Let's look at the electronic configuration. If we talk about zinc, manganese and nickel If we talk about manganese then its outer the configuration is that is 3d 5 4s 2 okay That means if we look at manganese from mnnit.ac.in Because the d orbital is half field, means more stable right more stable Who is talking about this greater stability? high negative value of electrode The value of potential electrode potential If it is high then it has negative high value What means it goes into m2+ state? It is getting extra stable after Right now let's talk about zinc. focus on outer configuration 3d 10 4s 2 Same story here too if zinc goes to zn20 That means two electrons of 4s are lost How will its state be stable state yaar fully feed d orbital to stable State again that is why its value is here also What is a negative high negative value Isn't it the turn of electrode potential now What happens in a nickel case 3d 8 4s 2 okay now you will say maam here so it's not that kind of story, suppose nickel if goes from nickel to 2 ps state then 4s two electrons of will go but 3d A then It is neither fully fed nor partially fed So then well here its high negative is the value of its electrode potential The reason is something else and you know what that reason is This is because of high hydration enthalpy Due to the high value of hydration enthalpy Its standard is in the case of nickel The electrode potential is a high negative Value Now let's talk about the case of copper Why is its value positive again in Ask Copper from its Electronic Confine If we look at the electronic confine of So it is 3d 10 4s 1 right now I have to calculate copper I want to take cu2 to p state first the electron passed through 4s and then the second Where will the electron have to come out from 3d brother from 10 3d 10 is already stable I want to destabilize the state Will copper agree easily? No, absolutely not If he will accept it with great difficulty, that means in a copper case It is not easy to reach cu2 but it is very difficult that is why its The value of the electrode potential is What is the positive value in other cases what was it what did I say m to m2 m + 2 The easier it is to go with the electrodes The more negative the value of potential, the It would be a far cry from going here easily here it is enough to go from copper to cu2 2 plus it is difficult, so difficult that there To go, you'll probably need something from your pocket you will have to spend money it is like that Right, so that's why in the case of copper we see there is one exception where its standard If the electrode potential is positive then Children, we will still continue the story But now the standard electrode potential We will talk about m3 / m2, that is, any from m2 + state to m3 + state as easily its electrode potential will go up by that much It will be negative, okay, so here also we We are talking about electrode potential But which states are you talking about? PS to 3 P state ki ok hai examples Let us take many first examples Scandium is fine if scandium is dissolved in 2 If you want to take it from P to 3Ps state What will be the situation in electronic confine It is good to pay attention to Scandium 2 PS That means I have two electrons out of this If it is removed then its outer configuration now what will happen to scandium 2 p ka 3 d1 ok Now take me to the scandium 3 ps state I have to go to 3 ps which means total three from scandium if the electrons have been removed then it means that If we remove that one too, which was 3d 1 Which state will scandium go to? will move to the noble gas configuration which is highly stable right scandium I would definitely want to go to it Neither, that is, in the case of scandium Scandium Will Be Super Excited to Go from 2+ to 3+ state right so that's why we Notice that in the case of scandium the value of the electrode potential hey that is low and this low value what does it show Shows extra stability or the noble gas configuration of Scandium Okay, now let's take another example. If we talk about Zinc's Zinc 2P What is the outer configuration of zinc 2P? will be 3d 10 right because two of s We've already removed the electrons. Right because right now we are talking about zn20 okay now we will talk about its three plus state let's talk about an electron and do you want to remove one more electron It will not be easy at all because this is already stable state was in 3d 10 d orbital was fully filled and stable now You're saying that you're removing an electron. If it is then it will not be happy at all since Wright would not be happy then this one To remove an electron you need to You will have to spend your money right that is In this case, the electrode potential What will be the value, it will be positive The value will be Let's take the third example The state of manganese is mn2 When it happens then what will be its outer confine will be 3d 5 right because there is a mn2 i means So two of them have already left, okay? ok now i am going to take it to mn3 p I wish it would be easy, it won't be because Again the same story my friend D orbital half field it is stable, don't give it electrons it is easy but still you want to take it yes right then what will happen in such a case The value of electrode potential is positive hoga once again let's talk fourth For example, if we take the iron of iron If you look at the electronic configuration then it is 3d 6 4s 2 then when iron is in 2p state So what will happen is 3d 6, it will be exactly like this now If it is not extra stable then now iron if you want to take it to 3 p state This means one electron out of 3d 6 and you want to remove right one electron and remove If you give it, which state will it go to 3d 5 That means if we remove that one electron If we give it then iron is in stable state If it goes away then it means iron is for this change you will be interested for this you will be interested for this He will be absolutely energized with Iron 2 P 3+ to go i.e. in iron case which will be the value of electrode potential That will be low, right, so the low value of iron What does that tell about the electrode potential? he is telling that the fe3 p is its Telling the story of Extra Stability So kids now we are going to talk about the next has stability of higher oxidation States what did we see this is the D block These are variable oxidation states, right? We have seen that they do state show Right now, we'll first talk about okay about halides their Here is how halides are formed Interestingly, we notice that the All of them have higher oxidation states, right? Who cannot stabilize halides? It only contains fluoride so now you can think about it You must be wondering what is so special about fluorine, brother? There are two special things about it, one is its higher lattice energy and secondly its higher Bond energy if we talk about nadium of the halides we notice unless we go to higher oxidation state At higher oxidation state of nadium then There we get to see vf6 But no other halide is seen such as iodide or bromide or We don't get to see chloride right so here also what are we seeing that higher Who stabilizes the oxidation state? Fluoride is doing this for the rest of the halides what happens in general to the rest of the halides they are Oxo is made by hydraulics If we talk about copper halides Regarding halides, we see that copper In halides c2 where x is a halogen is Nonce c2 is found but an exception is thrown i2 i.e. iodide form of S which is It cannot be found, now you ask why This is because cu2 is the i- in i2 oxido if you look at this reaction carefully There is no chance of finding cui2 here no what are we getting here cu2 i2 infact if we look at the If we talk about it, we see that manganese is So it exists even in +7 oxidation state it does but we I don't get to see mn6 but what It is visible that m o 3f means oxo If fluoride is seen then this is something There were unique things when it comes to hell The rest you can see in this chart The way oxidation states are very important Similarly, there was variety of halides as well There is a lot of variety, just that which is higher oxidation states there we have Fluoride is found in large amounts Kids, now we are going to talk about Magnetic Properties Magnetic If we talk about properties then here We will talk about three classifications: param Magnetic diamagnetic and ferromagnetic These words are not new to you I am Pretty sure because we know about them We talk about this in physics too In other lessons of chemistry also we We have talked about it but right now what is our focus our focus is d block elements ok then params What are magnetic things that attract By the magnetic fields are right, which Magnetic field attracts dia Magnetic Repelled by Magnetic Field Ferromagnetic Very Strong Attracted Bi magnetic field means ferro magnetism which you could say is An extreme end of para magnetism what does it mean in param magnetism is attracted by the magnetic field There is a strong attract here meaning That's why I said extreme of Why are Paramguru Params magnetic? Why is it moving towards the magnetic field? are attracted because of the presence off unpaired electron if any You can peek and peep into the electronic confine let's see that there are unpaired electrons inside it then from that unpaired electron How will a magnetic moment be associated We extract the magnetic moment Magnetic moment is given by √ o n * n + 2 where n is the number of unpaired electrons this means as the number of The number of unpaired electrons will increase The magnetic moment will also increase right and depends on this magnetic moment what does the parameter of that material magnetic nature so that's why now if we Talk about trend Magnetic Property Talking about the trend of , what do we notice as you do electronically If you focus on confine you will know what is the number of unpaired electrons is growing is growing is growing increasing up to a point and then decreasing it seems he is in a similar way to that The associated magnetic moment will also according to it will increase and then decrease then children This is another special thing about D block people. that they form coloured eyes coloured eyes Where did the color come from, look at the picture It is a general thing whenever we see colors are visible doesn't it mean that some such radiation during the happening of the thing which is being emitted falling in the visible range it's right we all have tro magnetic have read about the spectrum which Ultraviolet Light Infrared Race Inside There are many such radiations but we Which are the ones that are visible in the visible range? falls right into the range of visible light I fall okay now what's here This is happening to those in D block What is so special about these colored diys They make it well, the special thing about them is hidden in electronic confine If we look at their electronic confine If you look at them, their d orbitals are partially fed is ok and in This is because of the partially fed D orbital We make coloured ice, it happens like this The unpaired electron in the d orbital what are they they are unpaired That means they are well, they haven't been paired with someone because that well they get electrons from here and there, from somewhere If we get energy then what are they They get excited and become very happy They think, oh friend, I have got some money in my hand let's fly right so now this unpaired The electron is in an excited state We reach there with that energy After reaching an excited state, he Let's relive that excited state friend I am not that stable at all We are jumping a lot but we are absolutely stable if it is not there then what do you do then immediately returns back to the ground state when The energy with which they come back during that time we release the same energy that we used to go up So this energy which is released, it is emitted in the form of radiation and this the wavelength or frequency of the radiation It happens and falls in the visible range And that is why we see these colors And that's why we say that Joe D What are these block elements? Let's make this colored ice, now you can make it You will ask that maam tell me one thing that this D electrons in orbital jumped so much Why do you do this from one of your states? why do you jump to other states then This gives the answer to the d orbital energy splitting so these are the d orbitals splits into two energy levels Like I told you it's a little A while back I was telling you that the d orbital means five boxes, if we say five boxes then D A total of 10 electrons could fit into the orbital There are two electrons in each box on the right they pair up okay now this is actually When we look in terms of energy levels so out of these five, whichever three energies There are levels, right, at the same energy level live like dx1 dx1 z the other two that is dx2 - y s and d z s are slightly higher energy levels If you live there then it is basically D-byte. Two energy levels were formed inside these two There is a slight energy gap between the hey right so now you understand it is like oh the guy who was there jumped up, how did he do that there was something only then he was able to go up, something up If it doesn't happen, then where does it go? The story is that if he gets it from somewhere then his If money is coming in your hand then take that money The fur is going up because there is something up there what's up here which is the d orbital right It is getting split into two different energies This is because the electrons are present on the levels They are getting a chance to jump around and they are jumping around at the same time Radiation is emitted when it is excited You are coming from that state to the ground state The radiation that is being emitted is what we call the time Looking at as a color based on it Now let's talk about wavelength or frequency are you okay with these colored eyes trend Let's take some exams and see Suppose we are talking about Scandium 3 Plus ok scandium 3 plus electronic What will be the confinement of normal scandium what happens 3d 1 4s 2 now i am saying hum scandium 3ps means three electrons If you remove it then how will its configuration be? orbital will have zero electrons okay Brother, there is no electron in the d orbital So who will jump and leap when he jumps and leaps If it won't happen then what's the point of color right If you don't jump around then there is radiation it will not emit so that is why its color what will happen colorless let's talk Titanium 3+ is ok what about titanium outer configuration is 3d 2 4s 2 I said Titanium 3+ means out of these If you remove three then what is the outer configuration will become 3d 1 i.e. inside the d orbital has one unpaired electron, that is, it is a The unpaired electron jumped around can get excited when he goes up will return to the ground state it will emit energy so here we see what color do we get from it it is purple Let's make purple ice okay now exactly Which colour ion will be formed depends on what It will depend on the radiation that is emitted Are you remembering its frequency? we have the line spectrum of hydrogen I remember I had read lime in bracket Balmer P Funt, we had read all these things there what did we do, we used to calculate that brother what is their wavelength what is the wavelength We tell you which colour brother It will look right now let's do another one here Let's take an example from Let's Titanium 4 pas ok titanium 4 p if we take So what will be its outer configuration? is back from 3d 0 gets d in no If there is no electron then what does color mean If it will be a colorless right then now you will understand the logic These are the forms of colored ice By what logic are different colors made and Now it is most important for you to understand this These people from D block should Understand the reason why colored ice is made I have come, why do you make everybody because they have unpaired electrons in their d orbital and these d electrons in orbitals that are not As soon as they got energy they started jumping around and at the same time we get colored eyes See the specialty of our D Block people there is not one there are many which till now We have already come to know about this D block There are quite a few of them, aren't they? Complexion eyes are also called complex First of all what are ices How will you recognize complexion wherever you are? also you can see a metal ion okay so that Many non-periodicals are connected These are properties, we call them Let's take a look at the complexion example below: ptcl4 2e pt kya hai platinum which is A metal Who is associated with this metal is right of chloride then it becomes a Let's take the complexification f hole to the to the power of 3 Look at the minus, this is also an ion, overall in this There is a negative charge right at its center What is an Iron Which is a Metal Iron Ke is connected with cn-cs 4 - Or if we talk about hexa copper all this is about There are examples of complexion whose In the middle you get a metal ion which Some ana ais are connected i.e. Negatively charged ice or neutral molecule overall this ion is its have some characteristic properties Now the next question that comes to the mind is, There are so many transition metals Why does complexion make you special? It is among these D block people that there are so many of them If so, here are its three main reasons. First Comparatively smaller size of the metal eyes The size of metal ice is small due to which than it surrounds itself with others Binders take up second high ionic charges Third most important availability of D Orbital Electrons for Bond Formation Electrons are needed to form a bond falls and we see that our D Those in the block have Na in the d orbital unpaired electrons are present and these In unpaired electron bond formation So dear children, let's talk now We are going to talk about catalytic properties Catalytic properties of transition metals What are catalysts A catalyst is a substances that are present in any chemical It increases the speed of reaction but He himself remains unchanged during the reaction I neither consume nor do I do anything It happens that they themselves remain absolutely unchanged but it increases the rate of that reaction it is like a guy came who gave two I started a fight between friends The speed of the fight suddenly increased But he himself remained the same as he was When I slowly walked away from there, something like this this is what happens as a catalyst okay now our These are transition metals, aren't they known? are there any catalytic properties yes Meaning this knot is an expert in instigating fights Exactly this is to speed up the reaction why is it so because of their Unique Ability to Form how does this complexion Both of these are complexion states Any reaction due to the properties To get this done, it is very easy for anyone to any thing together with an intermediate In the Haber process as a complexification Finally, it works as a catalyst Divided Iron Iron What is a transition Metal is catalytic in hydrogenation Nickel acts as a catalyst What is it, if it is from D block then kids What did I just say, this transition Metal ice is a very unique feature of these Or the special thing is that it reduces its oxidation You can change the status in these has variable oxidation state and corresponding Because these are very effective catalysts There are a lot of best I will give example with fe3 p that is Iron which acts as a catalyst When we have iodide and sulphate ions First let's see the reaction between Let's look at this reaction, say iodide i- but sulphate means S2O2 - both of these When a reaction occurs between we get what do we get i2 + so4 2 - Can you see any iron anywhere here? but look now when we look at this Check what is happening inside the reaction if we do then we will know that there is a critical role playing fe3 p ok Let's see step by step first We will notice that on fe3 with i- reacts to form i2 + fe2 and this fe2 reacts further with s2o 2 - and makes fe3p + so4 2 - okay now Look at both the steps if you take them together Observe both the steps then you What did you get in the output? Output has a so you got i2 second you got so4 2 - and during this whole reaction You started with f 3+ in the last round too only fe3 p was found i.e. the fe3 p which is Iron is what remained unchanged during this reaction but what did iron do in this reaction got it speeded up because this is iron's He had a special ability to react with everyone because of that it quickly got in the middle made intermediates because of which these reaction speed has increased but if iron key If we talk about it, it remained the same as it was Right till the end, you understood it here But in this reaction, how does iron Like a really amazing catalyst from Our transition metals are working What are interstitial compounds When are interstitial compounds formed? Interstitial compounds are formed when very small atoms such as carbon nitrogen Hydrogen gets trapped in these lattices inside a large lattice inside a structure when These small atoms get trapped then Interstitial compounds are formed like this The compounds are neither typical ionic neither typically Kovalenko is hometro as an example Let us suppose it is made of titanium and carbon TC is made of manganese and nitrogen mn4 n is made up of iron and hydrogen fe3h so these are all the examples These are called interstitial compounds Why do we call them compounds because lattices the spaces between the structures of which are the interstitial spaces Those spaces are occupied by atoms because They have got this name due to this nature of theirs They got their name due to their composition. has become interstitial compounds if we Characteristics of interstitial compounds Speaking of which, these are very hard they have high melting points Infact higher than pure metal These are metallic melting points retains conductivity in a way that Metals are good conductors in the same way These compounds are also good conductors Not only this, these chemicals are inert Inert means inecto reacts so much Don't do this to others, child Party, with this we have arrived at this Till the end of the video so D block with this The story of the elements ends but The story of F block is yet to come my friend So I'll see you soon in another one With shot video in which we have details I will discuss about the F block elements and after watching this video If the concept of d block elements is If it is crystal clear then definitely post in the comments Write and tell me as usual that the concept happened crystal clear and I'll see you one New video with a bang video of Till then stay home stay safe take take care ba bye