[Music] [Music] hey students a very very warm welcome to all of you so all my atoms i hope you all are feeling absolutely awesome your mom is welcoming you to the session and so many students were telling me that ma'am when i going to upload one short video of a chapter and uh cbse 10th class nam here you ma'am here you and this is the very first session that is chemical reaction sign equations one short video in this video ma'am is going to tell about all the important topics as well as the entire chapter so that when you're done with the chapter you can see this video and have a quick revision and can attempt all the important questions so happy excited a bit nervous that exam is coming soon do not worry white to fear your anubha mama is here keep following all the videos and chemistry abortion is going to be very easy and i'll take care of all the things that you'll get everything so let's start please follow this channel equally please subscribe to the channel and share it to your 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signs when you keep your milk open for some of the time you see that starts curdling up that is something that's giving you maybe paneer maybe cheese and maybe curd so what exactly is the reason behind it do you remember that do let me know in the comment section what about the iron nails uh even so there are so many iron objects in your home after few months that will turn like this reddish brown they will be rusted what exactly is the reason for the same and humid environment something now you're getting it that they are creating some chemical changes chemical changes means they react with some of the things and giving you new substances so students your day-to-day life is filled with so many day-to-day examples day-to-day life examples of chemical changes if i talk about your iron nail that turned reddish brown because it reacts with the humidity air and moisture to give hydrated iron oxide that's your rust when i talk about your milk milk is having a bacteria lactobacillus and after you know in that hot environment that will be giving what converting to lactic acid in the milk milk is having lactose of sugar that convert to lactic acid and that's how you got your curd so chemical reactions chemical changes new substances are forming and students there must be proper way to write each and every chemical reaction are you agree with me there must be a proper way every time we can't say this this this and making big big sentences so in this chapter we'll talk about how to uh define a chemical reaction how to write it and so many other types of the same so students if i talk about laboratory that you're going to laboratory and you're like let me see if i can perform a chemical reaction yes or no definitely the very simple example that's there in your text book is this if you're taking a magnesium ribbon and you start burning it in air what will happen your magnesium react with the atmospheric oxygen we have provide enough heat also giving you a new substance that's magnesium oxide how we are making sure that we got magnesium oxide a very bright white dazzling light is going to produce and the powder starts coming out of the same that white powder is nothing but magnesium oxide you got a new substance that's what a chemical reactions we perform in laboratory too yeah students got it so what i meant by this that how a chemical reaction happens in day-to-day life or in laboratory you are going to take two or more substances they are going to react with each other whatever substance are reacting is called as reactants they react with each other and give you some new substance with entirely new property and that substance is called as product okay that substance is called as product or products if more than one that's what a chemical reaction is okay i hope it's pretty simple and you got it a process in which one or more substances are going to react with each other to produce one or more new substances yeah with entirely different property and how you can make sure that when you go to laboratory you're like yes something has happened a chemical reaction has happened you can make sure by knowing some of the observable changes you'll see in the reaction and you're like yeah i got it yes completely i'm with you so the very first example in change in state that how a different substances with different physical state is going to combine to give a new substance with entirely new physical state the very common example and very famous one is in there is there in front of you i took ammonia gas i took hydrogen chloride gas you won't call it hydrochloric acid because if that will be acid you must have written aq aqueous acid shows acidic property in aqueous solution in water otherwise it's just a gas so these two gases are going to react with each other kind of combination they are going to combine to give a single substance that is ammonium chloride white color powder type of a substance in solid form so i observe by reacting to gases what did i got i get my ammonium chloride in solid form change in states best example now you see mama's writing every reaction with what writing something in the bracket and what is this students the physical state this is making your reaction more and more informative so you should prefer it okay second one is change in color that if i'm doing some of the chemical reaction if i got a new substance with a new color that is definitely you can say is a reaction where change in color is happening very famous example that you're knowing from your eighth class also if i'm not wrong that how if i put an iron nail into copper sulphate aqueous solution which is of blue color this is like a grayish white color i see a color change i got iron sulfate in the same solution like of this color pale green color is going to come and that copper that was free starts accumulating on that iron nail that's reddish brown so see that what did we get out of the same see the color changes isn't it amazing so yes students change in color is also an example to see whether the reaction has taken place and the characteristics of chemical reaction one more that's evolution of gas that how come when two or more substances are reacting we are getting a product that's in the gas form and gas is leaving your test tube or beaker okay and always remember whenever metal react with acid you'll always get metal salt and hydrogen gas metal salt and hydrogen gas so i took zinc metal and i put it into sulphuric acid and this is a very good example as you know the chapter already zinc being more reactive is kind of displacing hydrogen and telling to hydrogen hydrogen you go away be a loner okay so you got zinc sulphate a metal salt and along with that hydrogen gas what you're getting hydrogen gas and how you can check hydrogen gas if you put a funnel over it if you put a glass tube over it and two things you can do if you pass it through soap solution if you pass it this gas through soap solution soap bubbles are going to trap hydrogen gas and whenever you are going to take a burning candle near it or burning matt stick near it it will burn with a pop sound as simple as that so you can also detect your hydrogen gas not necessarily hydrogen gas i can show this reaction also that if i heat calcium carbonate what i'm going to get calcium oxide along with co2 gas co2 gas and how you can check that then the gas is co2 because that's turning your lime water milky yeah one uh example in front of you you can tell me other way to detect co2 gas in the comment section that is very easy eighth class thing okay even change in temperature is also one of the example that when you're performing the reaction if the beaker after some time became hot or if the beaker or flask whatever you have taken became cold that's also telling a change in temperature and definitely that a chemical reaction has taken place so there's one example in front of you that how ammonia is reacting with sulfuric acid again what did you see here that's i'm taking a concentrated sulphuric acid and that is doing what the product is like i'm getting uh a kind of a salt a kind of compound along with h2o water so ammonia with sulphuric acid i got ammonium sulphate it's like h two hydrogen and then sulphate so ammonia will give you ammonium sulphate i'll take two molecule of the same two nh4 it became two nh4 right and then so4 so i got ammonium sulphate along with h2o in this and what did we see in this reaction in front of you that when i touch it it is a bit hot exothermic that's release in energy what is exactly meaning of exothermic students reaction is of basically two type if i talk about change in temperature one is exothermic and one is endothermic all right one is exothermic and one is endothermic exo means outside yeah exo means outside and when i talk about endo endo means inside okay exo means outside and endo means inside thermal thermic means definitely heat thermal related to thermal related to heat so change in temperature reactions will be of two type outside heat if the reaction is releasing heat and the beaker will become hot endothermic inside heat if the reaction needed some amount of heat to perform they absorb the heat and the beaker will be a bit cold and i can definitely give you more example for better understanding students because that's what i want from you right so exothermic one more example all the combustion reactions are exothermic burning a substance magnesium burn in air that's an exothermic coal burning in air your lpg burning in air exothermic endo means inside heat and day to day life example photosynthesis that how your plants absorb sunlight to perform a chemical reaction okay very simple one i hope you got it there's one more that you can see that's formation of precipitate that how come when two or more aqua solutions are going to react in laboratory you see whenever these two aqueous solutions are reacting one of the product is in the solid form and settle down at the bottom of test tube very simple so it's like having two aqueous solution and what they'll do they're like we are bored of each other's company let's just exchange position so barium is like i'm going with sulfate sodium is like i'm going with chlorine do let me know in the comment section what this type of reaction is your comments are highly appreciated and making me figure out that you're learning everything so sodium chloride two molecules and then barium sulphate and what will i observe white precipitate white solid powder settling down at the bottom of test tube whenever you mix it so that's what is precipitate a solid in soluble product that i'm going to get look at this something like this so i hope it makes sense i hope revision is going absolutely fine and awesome yeah so now it's just chemical reaction should be written in a better way rather than writing big big word magnesium plus oxygen gives magnesium oxide so what we'll do that we write every chemical reaction in a better way in a simple way and what that simple way is writing a chemical reaction in terms of using symbols and formula so rather than writing magnesium and oxygen giving us magnesium oxide that's what my product is uh rather than writing in this site we'll write it in a better way that i'll use the symbol and formula that i will write what i will write magnesium reacting with oxygen to give magnesium oxide i know that you know this much now yeah using symbols and formulas of the elements and compounds that is there in the reaction okay so chemical equations i can write in two way one is called a skeletal equation what is chemical equation uh writing a chemical reaction in symbol and formula symbolic representation skeleton equation is what when i'm just using what students when i'm just using symbols and formulas so in this reaction what did we see i took my potassium nitrate and when i heat it it is kind of decomposing to give me potassium nitrate is decomposing to give me potassium nitrite this is nitrate this is potassium nitrate decomposing to give us potassium nitrite more oxygen eight lesser oxygen eight with oxygen released now this is just a skeletal equation means i'm not very much sure that the number of atoms are equal on both the side and there is one more way that's a better way that's balanced chemical equation writing the chemical equation in what way a balanced way balance way means i'll make sure that i will see the number of atoms equal on the reactant and product side so when i take two potassium nitrate and wrote two potassium nitrite with oxygen the number of potassium the number of oxygen the number of uh nitrogen everything is same two nitrogen four and two six oxygen so this is a better way to write a chemical equation and that is writing a chemical equation in balance form okay why we have to balance a chemical equation just to justify law of conservation of mass which simply said what is law of conservation of mass that whenever i started the reaction whatever is the mass of reactant and when the reaction is completed the product the mass of product must be equal when i'm doing the reaction definitely in a closed system otherwise you will say now what if we will be getting some gases and gases will be evolving out no that's what you have to approach in a closed system mass can neither be created nor be destroyed i can't say some of the masses destroyed some of the mass came up on its own it must be same and to make mass same on both the side we have to make atoms equal on both the side because atoms are responsible for the masses and you know that right so the main way to balance a chemical reaction is to follow the law of conservation of mass and the one that's there in your syllabus the method that's hit and trial method we're hitting some number and we're trying it we are using it so what are the steps that we are going to follow follow these steps if the question will come in three mark you are not like i will not make any of the proper way and i'll just make a very chaotic representation and that's it no that's not the right way write all the possible steps if the question is for three mark one mark you can simply tell in very short first of all write a balanced uh chemical equation that how come my hydrogen is reacting with chlorine to give hcl how my hydrogen react with chlorine to give hcl okay students so this is just an unbalanced chemical equation second we'll count number of atoms on both the side counting number of atoms on both the side is very simple that i just make sure that i have two hydrogen and two chlorine on the reactant side and one hydrogen and one chlorine on the product side numbers are not equal i'm done and how did we do that multiply coefficient with subscript that's what we did multiply this coefficient uh i mean the coefficient that we write in very starting with my subscript then i can make the number of atoms equal that how would i know how to make atoms equal on both the side so that is what i'm telling you right away that you will write some coefficient and very starting coefficient is nothing but a whole number in such a way that when you multiply them with the subscript substitute that's we are writing here with the subscript the number of atoms will become equal on both the side coefficient into substrate will give you the total number of atoms and if your reaction is suppose you wrote it in this way two hydrogen two chlorine i got four hcl now look for this point if necessary reduce coefficient to lower possible ratio that i write it in simplest possible whole ratio so i divided it by two i got h2 cl2 to hcl did you get the point we'll write it in the simplest possible number okay update and double check that the atom and the reaction is balanced that's what will we do okay and how you make sure that uh yeah ma'am we are understanding it if you will do enough kind of examples because doing examples are very much important so at least you should practice 15 20 examples whatever is given at least in ncrt suppose i have to balance this this is very much easy uh coefficient is nothing but one if nothing is written means one that's giving two hydrogen two oxygen two hydrogen but one oxygen number of atoms are not equal on both the side how will i make it equal by writing some coefficient in the starting which makes the number of atoms equal now this became 4 and this became 2 so oxygen here is 2 2 but hydrogen here is 2 so how to make it 4 to make number of atoms equal i can also multiply this h2 with 2 as simple as that by writing simplest possible whole number yeah so is it clear not at all difficult i know that you got it it's not at all difficult so let's have one more example how come c6 x6 whenever going to react with oxygen produce co2 h2 and definitely energy this is nothing but your benzene i am burning benzene in air that's giving do remember whenever you have any hydrocarbon and whenever you try to burn a hydrocarbon that will always give co2 and water vapor let's see how to balance it number of carbon six number of carbon one i'll write it six here students how to approach it there is one thing that you should remember whatever the atoms include carbon hydrogen oxygen first go for that atom in balancing which is repeating the minimum number of time which i can see in the reaction minimum number of time the minimum number is basically two there will be some specially oxygen that is written three times four times in all so we will do such atoms uh balancing in the last yeah so i'll approach carbon as it's repeating two times hydrogen also two times oxygen three times so i will balance carbon and hydrogen before but ma'am among carbon and hydrogen which one will i choose so choose one that's heavy that's one that's having more mass so first preference carbon second preference hydrogen third preference oxygen okay so six carbon six carbon all okay six hydrogen i will make six hydrogen by writing three hydrogen is also balanced let's see the number of oxygen 6 into 2 12 plus 3 that's 15 how to write 15 oxygen it's not 2 multiple you can write it either in this way 15 by 2 2 2 cancel 15 by 2 o 2 15 by 2 o2 and that if you'll do a half of 15 that means uh you will get the same number that's what we wanted that's 15 or there's one more way either i'll do this the reaction became balance the number of carbon the number of hydrogen and number of oxygen is balanced let me erase this and tell you one more way to write it in a better way because the thing is using a fractional number doesn't look nice what will i do to cancel this 2 i can multiply the whole equation by 2. so it's 2 3 6 x 6 plus 15 o 2 gives me 12 co2 and 2 into 3 6 h2o now we are done 12 carbon 12 carbon 10 hydrogen no that was 6 a mistake 12 hydrogen 12 hydrogen oxygen is like 30 12 into 2 24 plus 6 30 now it's correct way so please remember you can do that also it will give you 15 uh oh but the right way will be writing it into a whole number okay so this is the way you can balance i know nam had made so many videos on a monk 2.0 series please see the entire series if you'll be having any confusion we discuss so many examples over there as well and you can practice and let me know your problems okay now let's discuss different different types of chemical reaction it's like there will be million of chemical reactions and studying them one by one will be very difficult so they have classified the chemical reaction on some of the common types and according to it there will be five types of chemical reaction that we are going to study okay in which my reactants are somewhat having some atoms they're rearranging themselves to get new product that's what happens in a chemical reaction it's just a rearrangement of atoms to get new substances so the very first one that we need to discuss is combination reaction something that's getting combined and very simple a reaction in which a single product is formed when two or more reactants are going to combine okay so that's combination you can totally download this file you can have this pdf for quick revision that will be uploaded very soon on the description box okay so mom is showing you with the help of amazing gifs also that how come two or more things are coming reacting to give a single substance that's what combination also called a synthesis reaction so never get confused that these two are different synthesis and combination is same only very famous example in front of you that's how hydrogen came chlorine came you know hydrogen tiny h tiny atoms chlorine cl2 cl2 i mean cl2 big atoms they are just combining and see what is happening hcl hcl you are getting two molecule of hcl what exactly is this synthesis combination two or more things are combining to get a single substance right if i talk about decomposition name is giving you the answer that's opposite of your combination and what did we see here decomposition means breaking down a single substance to give more than one substance that's it breaking down of a single substance single heavy compound into simpler kind of a compound simple type of substances yeah so decomposition is also very simple breaking down of a single substance to give more than one substance yeah one example in front of you that they're showing here we have taken kclo3 potassium chlorate that was decomposed to give kcl potassium chloride and oxygen anyway you have to balance it 2 kcl 6 oxygen yeah i balance it also so that was the example that how we get kcl and oxygen in this by a single substance potassium chlorate now that's a three type students your decomposition is of three type and what exactly this that when a single substance breaks down with the help of heat given to it a substance will not break down on its own right you have to heat it i mean you have to give it energy either in form of heat either in form of light it will absorb light or in form of passing electricity these all are different different forms of energy only so there is one thing that's there in front of you that we have taken lead nitrate as a single substance we heat it for heating we can use this triangle symbol called as delta symbol also do remember whenever metal salts are going to be heated that will break down in such a way that your metal as it's heating in air will give you metal oxide look at this very famous and very good you got lead oxide and the rest over substance is going you some gases that is going to come out so do see that that's a white color substance decomposed to give lead oxide that's a yellow color a reddish brown fumes that's of no2 gas also oxygen released and what this is you can see that here also is thermal decomposition reaction why i call it thermal decomposition because decomposition due to heat so that is thermal decomposition now the second type is electrolysis means lysis means breakdown electro means electricity electricity lysis means breakdown okay when a substance is going to break down when electricity is passed through it very famous example that you know is electrolysis of water when i'm going to take water not normal distilled water i will put some two to three drops of acid into it so i'll call it acidified water because acid is somehow helping water to dissociate into ions so that they can move towards respective electrode so positive terminal and negative terminal of the battery and negative terminal of battery is called as cathode because they attract cation and positive terminal is called as anode as they attract in ion why opposite attracts so on one of uh the electrode you will get hydrogen and one of the electrode you will get oxygen where students h is in the form of h positive that will go to the negative terminal so on cathode you will get hydrogen gas oxygen is negatively charged so you know that every time two hydrogen ion will move and one oxygen ion will go uh towards the positive terminal and give you oxygen gas the conclusion is when you take two molecule of water you get two molecule of hydrogen but one molecule of oxygen the amount of gases produced here is in the ratio of two is to one clear yeah students electrolysis breaking down a substance in presence of electricity and i would love to see some more example of electrolysis in the comment section give me reply all right now decomposition in presence of sunlight that is nothing but a photodecomposition or photolytic decomposition right breaking down in presence of light and now my silver compound some of the silver compounds are light sensitive like agcl and aj b are silver halides silver chloride silver bromide halides mean this halidus 17th group of the periodic table halogens okay so whenever you put them into sunlight you can use this symbol also ah h nu this is new new means frequency frequency of light light comes with the proper frequency and einstein told us that whenever energy comes energy comes in a packet and the every packet of energy is defined by h so that's what uh another representation though they won't give you it's like out of the box okay so you will get what product it will decompose to give silver and here chlorine and here bromine it's like your white silver pale uh yellow silver bromide decomposes to have a grayish substance left on your watch glass or your china dish and the gases will evolve out what example is this photonic decomposition breaking down in presence of light okay so these are the things that your substance are breaking down in presence of either heat light electricity that means they are needing energy they are absorbing energy in form of heat light and electricity and all your decomposition reactions are endothermic reaction what is endothermic reaction absorbing the heat that's what all the decomposition reactions are doing so now you have plenty of examples okay you have plenty of examples of endothermic and one more thing exothermic you can say combination combination reactions are exothermic okay like in general let's talk about displacement reaction now this is the third type of reaction what exactly is a displacement reaction when a single substance being highly reactive is going to displace a substance an element from its aqueous solution or its molten salt what exactly that's what mam said i'll repeat it again here the examples are there in your textbook in form of metal so when you have a reactive metal when you have a highly reactive metal that can displace a less reactive metal from its aqueous solution or from its molten salt reason to take in aqueous and molten so that ions will be dissociated ions will be free reaction is easy to perform so zinc is like i am displacing copper copper be a loner and you got zinc sulfate metal salt and again one metal in the free form yeah you got it i'll show you see that example in front of you magnesium i have combined with what silver nitrate no3 okay and magnesium agno3 yeah and magnesium is like i am more reactive than you silver go i will take this position you got magnesium nitrate and vegetaria silver lunar silver is free okay so this is your single displacement i hope it makes sense i hope you will remember the reactivity series because somehow this will help you this will help you to remember all the elements in an order that which one is more reactive and which one is less reactive in the entire reactivity series reactivity decreases down the group that means a highly reactive metal can displace a less from its salt solution one more example in front of you my iron being grayish white my copper sulphate copper and this is copper sulphate this is copper basically this is sulfate s o four okay iron is displacing uh copper and we are getting iron sulphate and copper now there's one more type of a reaction yeah yeah it is going to be a long one so stay tight because mom is helping you to revise the entire chapter that too properly so students now the example is our dd reaction what's dd reaction a d-day reaction is nothing but double displacement reaction two times displacement reaction and how that happens when you have two aqueous solution and they are exchanging their ions that's what a dt reaction is two aqueous solutions exchanging their ions like we are done let's exchange one sodium one positive two sodium two positive sulfate minus two charge barium plus two two chlorine minus two exchange of fines sodium is like i'm going with chlorine i am done barium is like okay i'm going with sulfate so barium sulfate and sodium chloride one of the substance and double displacement when the substances are not acid and base one of the substance in that case would be precipitate a solid insoluble product so what you will get you know that two aqueous solution exchanging their ions giving two new solutions if the two reactants are not acid in base one of the product we assume is precipitate one more example silver nitrate with kcl exchanging the ions silver is like i'm going with chlorine potassium is like i'm going with nitrate i am getting white precipitate of silver chloride here and the other one will be the aqua solution so that's very easy and some of the students is like how to remember that practice students practice will make you perfect that's what mam is trying to help you over there yeah so one of the form of dd reaction is your precipitation reaction where you get one of the product as precipitate lead nitrite with lead nitrate with ki potassium iodide aqueous ions i mean in aqueous solution they'll exchange their ions lead iodide potassium nitrate do remember about the valency part also do not write the formula incorrect otherwise the whole equation will be you know uh balance in the wrong way so that's not the right way take it i hope that's fine so precipitation is done adam let's see i got a lead iodide yellow color precipitate very awesome and very good to see that yes students and the second type is of your dd reaction is nothing but neutralization reaction what is neutralization reaction reacting in acid in base to give salt and water very famous example given in front of you two that's reaction of hydrochloric acid and your sodium hydroxide this is your acid this is your base and as you know acids are bases acids and bases are also having ions and there are also exchange ones uh so h is like i'm going with oh n is like i'm going with cl i got nacl along with h that's your water i got salt i got water how did we get that exchange of ions dda reaction is of two type one that is the precipitation reaction the other one is your neutralization reaction okay got it students check check okay let's talk about this again which is going to be very very important that's a redox reaction the fifth one redox is a combination of two words that's red plus ox red came from reduction ox came from oxidation so redox reaction are a reaction a set of reactions or i'll say a reaction in which oxidation and reduction takes place simultaneously okay a reaction it's like oxidation and reduction are telling to each other we will live together always so that happens simultaneously but let's understand first of all what is oxidation and reduction so that you will understand red ox that will explain with the help of a very famous activity given in your ncrt also that i took copper reddish brown substance and i'm heating it in air so what will happen in this uh example students my copper as we are heating it in air is giving us copper oxide and my brown color my reddish brown color copper turned black so what exactly we observe in this reaction my copper is taking oxygen and making copper oxide so can you explain this why this has happened now i can explain it totally yeah why exactly this happened because oxygen is added and if oxygen is added to a substance that is called as oxidation in very simple word okay copper with oxygen giving you copper oxide really sorry for the same there is like after downloading the file some of the arrows are going here and there but what we concern is our concept must be clear and mama is doing the same so do remember students earlier oxidation reduction concept came to us in terms of oxygen only oxidation is addition of oxygen and reduction is something that's removing that's removal of oxygen okay so let's understand that with the help of this example when we take copper with hydrogen and we are heating it copper oxide with hydrogen we are heating it i got copper with water so look at this example if hydrogen gas is passed over the heated copper oxide the black coating on the surface this is of black color so the black coating turned brown as the reverse reaction takes place as hydrogen gas is passed it will again turn to copper and the black layer is again gone of copper oxide i got my reddish brown copper back i got my reddish brown copper back so what we observe that this is removal of oxygen so this is called as reduction earlier definition was limited to this earlier definition was limited to only this that oxidation is addition to oxygen to any element but hydrogen is like no i'm not very happy with the same so what in terms of hydrogen removal of hydrogen from a substance is also oxidation uh opposite job that it is doing in oxidation removal of hydrogen and that's something more important i'll tell with an analogy also losing electron to gain higher oxidation state like a simple example suppose you have sodium you know configuration of sodium is 281 for getting stability sodium is losing an electron right and becoming positive so a substance will lose its electron and get positive charge that's also oxidation you can remember in the term leo nam is leo2 loss of electron is oxidation leo that's leo loss of electron is oxidation okay in the same case uh we have understand different kind of example that adding oxygen i got copper oxide that's one of the example of oxidation we see here as well that if we took if we took copper oxide let me change the color if we took copper oxide and pass hydrogen gas back what did i get my copper oxide removed its oxygen so this is what reduction on the other hand one more thing we saw hydrogen here took oxygen right what do you need to see from reactant to product what exactly is happening to the substance gain of oxygen that's oxidation right gain of oxygen that's oxidation removal of hydrogen that's also oxidation so please remember that okay losing electron i've already explained to you with one more example i'm telling look at this my magnesium is like having two a two this is the configuration every chlorine is like i am two with seven so my magnesium having two extra electron in what says if it loses these two electron it will be stable so magnesium is telling to two chlorine you need electron i have it don't worry at all magnesium giving one electron here one electron here and very happy what happened to magnesium loss of two electron got plus two charge here magnesium got oxidized look at the chlorine opposite job so you remember it in this way leo goes to girl leo goes to girl so gain of electron is reduction look at both the chlorine they accepted one one electron from magnesium and total two chlorine accepted two electrons or minus two charge so magnesium here is getting oxidized chlorine here is getting reduced magnesium oxidized chlorine reduce as simple as that so i hope now oxidation and reduction is also very much clear that how come reduction is addition of hydrogen opposite and then removal of oxygen and then gain of electron yes we can understand this also with the help of different different example my nitrogen here became nh3 by addition of hydrogen and addition of hydrogen is nothing but reduction that's pretty much clear removal of oxygen example in front of you i had iron oxide and i pass coke out of the same coke is what coke powder is pure form of carbon itself and what did we see students i'm not balancing it carbon here is helping iron oxide to lose its oxygen and iron oxide converted to iron and loss of oxygen is nothing but reduction gain of hydrogen is also reduction and now gain of electron i told you any substance taking electron suppose here is f2 two fluorine every fluorine to a i mean two seven two seven two electron we have given one here and one here both of the chlorine accepted one one electron so what did we get every chlorine is having a negative charge gain of electron is reduction every chlorine two fluorine this chlorine became negative this fluorine also became negative by accepting one one electron i hope you got it that how gain of electron is also reduction now redox must be properly cleared in your mind that redox reaction is nothing but combination of oxidation and reduction a reaction where a substance is getting oxidized and the other is getting reduced that's what your redox reaction so some example in front of you look at this my iron with oxygen is giving iron oxide and this is oxidation my iron is getting oxidized because it's adding oxygen into it my oxygen is getting reduced in what sense students my oxygen i can explain that in terms of electron because that's a better method how come any substance in elemental form is having zero charge i hope there is no denying in the same in0 charge oxygen zero charge when i take any element sodium lithium any of the element of periodic table every atom is having zero charge because number of proton and electron is same positive and negative the same so my oxygen here is in the elemental form not carrying any charge but here it makes a compound and compound is made when your metal losing electron and non-metal accepting it so if you remember every ion is having a valency i can check the valency iron iii oxygen two every ion is having a valency of plus three every oxygen is having a valency of minus two so in the same what did we observe students my oxygen from zero became minus two and how come minus charge by gain of electron my oxygen was zero now it became minus two by acceptance of two electron every electron minus one minus one gain of electron what exactly is this reduction so students sometime you might get confused in the oxidation and reduction in terms of oxygen and hydrogen but this concept is a better one that's the gain and loss of my electron simple example in front of you iron oxide two iron loss of oxygen reduction carbon dioxide i mean carbon monoxide to carbon dioxide gain of oxygen that's oxidation so one reaction where oxidation and reduction is taking place simultaneously there is one important note i hope you miss that but do remember that all of the reactions are not redox because sometimes we think every substance is somehow related to this that redox reaction and that's true also most of the reaction that we understood in combination decomposition also single displacement also is kind of redox also but neutralization reactions are not redox reaction dd reactions our dd reactions are in general dd reaction i should say are in general not redox at all because they are just exchanging their ions their ions their charts remain same it just exchange of ions no loss of electron no gain of electron so they are the ones that's not redox look at this h positive c l negative n a positive h negative exchange of ions i got nacl again and for any positive cl negative what is water h positive o h negative every ions are just same it's just position r exchange i hope you got it so this is your neutralization which is not at all a redox reaction okay before moving ahead one thing is a miss let me tell you here itself that is also an important question can be asked in exam what is my ra and what is my oa what is my reducing agent and what is my oxidizing agent so i'll tell you right away reducing agent is an agent that does reduction okay and how it can perform reduction of the other substance by oxidizing itself this is a very important thing i'm telling a question can definitely come oxidizing agent that does oxidation of other substance how by reducing itself it's like you do not need to think much but do one thing just see what a substance is doing to itself and the reverse action it will show it's like my iron oxide is giving you iron that's loss of oxygen it's reduction so if a substance is getting reduced because it's helping the other to get oxidized it's helping the other to give oxygen so this is my oxidizing agent look at the reactant site what they are doing what job they are doing my carbon monoxide is getting oxidized to co2 they are taking oxygen they are getting oxidized by reducing the other substance by taking its oxygen i am getting it so this is acting as my ra this is acting as my ra my reducing agent because that's what it is doing to iron oxide reducing it by taking its oxygen this is my way this is oxidizing co by giving its oxygen so reverse job they'll do please do remember okay so that's also clear 90 percent of your chemical reactions and equations is complete now the main part is this oxidation will not leave us very see we see in our day-to-day life that's not in a good way okay that's corrosion and rancidity two problems that we face due to this oxidation so students this process is corrosion and something that you know from eighth class i'm pretty sure about the same what exactly is corrosion is just eating up of your metal your metal is getting degraded basically with this oxygen that it is taking from atmosphere yeah there are other gases also that's equally responsible but oxygen here is the main villain not every time a villain though so what exactly is corrosion kind of a natural process that how your metal is getting degraded mostly when it reacts with atmospheric gases water vapor also with diluted acids okay and the very famous one you know that let me tell you the one that's very famous is irons corrosion yeah that my iron is getting oxidized let me tell you the reaction my iron is getting oxidized with some water molecule x molecule of water i got iron oxide with some x molecule of water and i will call it hydrated iron oxide that's nothing but a fancy name but your rust yeah so rusting is definitely eating up your iron metal with this moisture and harming so much to our economy every year so many uh iron objects has to be replaced so many bridges and all because yeah that's not a good thing right see look at that statue of liberty that was supposed to be now that looks also nice but yeah that's not a good thing your copper that was reddish brown turned to this green color because copper is taking atmospheric oxygen along with water vapor it's like moisture along with co2 gas and making a combination making a mixture of two products that's copper hydroxide and copper carbonate copper hydroxide and copper carbonate and simple bird we can also call it basic copper carbonate which will behave as a hydroxyl ion release means it's a base basic copper carbonate all right basic copper carbonate so we got a mixture of copper hydroxide and copper carbonate basic copper carbonate of green color that's what corrosion of copper do let me know your silver is also getting uh silver is also getting corroded when hydrogen sulfide gas the one that's coming out of sewage is affecting it and giving a set of products so what will be the product when your silver is getting reacting with your hydrogen sulfide okay do let me know your answer students okay so i hope this is pretty much clear there is no denying in that yay and do let me know what are the prevention method we can use for the same so let's talk about a rancidity that's rancidity what exactly is rancidity students look at your fresh oil and that's your rancid oil your fats and oils are getting oxidized due to oxygen present in the atmosphere and will give you a foul smell and bad taste if you use the same so you know that when your favorite food after some time it happens so many times that when you taste it oh that tastes bad pathetic the reason is generally this not like that was made bad okay because the oil used was getting oxidized and converted to this rancid form that's giving false melon bad taste this process is called as rancidity this is a picture of avocado see because it's having so much of fat into it oil into it that's getting oxidized yes so how you can prevent your substances and food from rancidity uh rancidities because of oxidation right so if you're preventing this process of oxidation that will be good what you can do you can put some antioxidants in your food that's what generally those the packets that you got is carrying it they have some antioxidants that is allowed one antioxidant that is preventing your oxidation apart from that flushing nitrogen gas also sometimes they do this they took oxygen out and put nitrogen gas kind of inert and preventing your oxygen to react with the fat and oil so that food will last longer and keeping it in airtight container keeping your food in refrigerator because in the cold temperature your process of transitivity will be slowed down not like completely away yeah so these are the methods that you can prefer to prevent your rancidity and i hope all of my hard work will not going to wane and you get the entire lecture uh it was a big one but i try to set the entire picture in front of you in this chapter so students happy happy that chemical reactions and equations absolutely done da nadan so come and see the way we work in vedanta platform there is a link given in description box just click on that select your grade 10th select your target cbsc and take your subscription for one month three months and six months choice is yours it's just the amount of discount you are going to get after applying a coupon code that's a g e p r o anova nam code is a g e p r o apply it you can say from 20 to 43 percent one month just give it a try two one five nine three months will be the best one at that moment of time because almost 3-4 months are left in your exam and you can save 31 on mrp do not forget to apply the coupon code do not forget to visit the link do not forget to like share and subscribe to the channel and support it equally this is like a must video do not forget it okay students so i'll take a leave i hope after the session is done we can still have some uh 7 800 likes that is like important so i'll see you next time students until then take care of yourself bye bye have fun keep revising happy learning