 reactivity towards acid, CO plus N2 is producer gas, reactivity towards acid. See carbon has different reaction with hot and concentrated acid and with dilute acid, okay, cold attack. Right on, carbon reacts with hot concentrated S2 SO4 and get oxidized into CO2, get oxidized into CO2 and forms sulfur dioxide gas, SO2 it forms. Okay, reaction right on, C plus S2 SO4 gives CO2 plus SO2 plus SO2 plus SO2 plus SO2. Right on next, carbon reacts with hot dilute acid, dilute acid and forms a brown color substance, forms a brown color substance which is known as artificial tannin, T-A-W-N-I-N, not that important. Thing is the color, right with dilute it forms brown color concept, that is important, okay, name is not important. If you use, if you use HNO3, concentrated HNO3, then what gas evolves in this? HNO2, right, S2 SO4 gives SO2, HNO3 gives NO2, right. Next one right on, next one right on, it's, see when you have a carbon with, suppose they are using HNO3, means water is there. So this will be a complex of water that is a hydrocarbon will give, will have a compound of carbon and hydrogen. Depends upon what is the amount of HNO3 you are taking. So it may be any hydrocarbon of this, with water it forms a complex, that complex is tannin, artificial tannin. Okay, next one right down, carbides, carbides. Now we have discussed the preparation of these things, alkenes, alkynes, by what method? By hydrolysis of certain carbides. Carbides, right down, carbon when heated with metals, carbon when heated with metals forms carbides. For example, beryllium with carbon 2C gives BEC2, beryllium with carbon BEC2 very common form of carbide. Another one is MN plus C, manganese plus carbon it forms MN3C, manganese carbide, MN3C, manganese carbides. Okay, there are certain oxides right down, there are certain oxides, hydroxides, phosphates and sulphates, phosphates and sulphates, phosphates and sulphates which reacts with or heated with carbon to form carbides. One more example we will write down, certain oxides right down magnesium oxide, MgO, MgO plus 3C gives MgC2 plus CO, carbon monoxide, carbon monoxide, MgC2 plus 3C, sulphates right down calcium phosphate, Ca3PO4 whole twice, Ca3PO4 whole 2 plus carbon 14C forms calcium carbide CaC2 plus phosphorous plus carbon monoxide evolves, carbon monoxide CO, CaC2 plus phosphorous plus CO, carbon monoxide evolves. Next one, sulphate, BHSO4. Sir, is this an easy way of preparing eta-inferring? Hydrolysis of what? CSE2. CSE2 whole twice. What kind of form is this? Sir, you are getting calcium carbide. Then hydrolysis of this? Yes, sir but rather method is used to prepare calcium carbide requires high temperature. No, it is calcium carbide is only and then after hydrolysis of this. So, even calcium carbide is prepared by heating it to like 2000 degrees Celsius? Sir, isn't this very easy compared to that? No, you said the preparation of eta-inferring. Sir, that we need calcium carbide. Correct. That method we heat it to a very high temperature and then here it is this method. With this method also you can prepare. No, see it is like it is happening so easy you are looking at it right. But how is it possible? It looks like easy right but actually... It is happening at a lower temperature. No, it is not the temperature is not mentioned you never know what is happening. Temperature is not mentioned it is not mentioned lower or higher temperature. See the thing is easy or tough it depends upon what reaction, what energy it requires. How the reaction is behaving towards the heat? Whether the heat is coming out or getting you know consume into this. If heat comes out is very high what is the rate? There are many factors what is the rate of the reaction? If the rate of the reaction is also very fast it is very difficult to control the reaction. That is why in laboratory we do not use this method for the preparation of calcium carbide. Reason can be anything like I said high heat may above rate is very fast you cannot control the reaction. Many things are possible so we cannot say that. But yes whether you can prepare or not by this method we can prepare the calcium carbide also. So with the temperature is it less than that? See here very high temperature is not required. For this reaction very high temperature is not required otherwise you would have mentioned. At high temperature it gives this. Next right is Sunfin right? B.A.S.O4 plus Carbon C. Hydroxyl. Hydroxyl. Now what have I done? Cospite has been done. Mg. Mg has been oxidized and Hydroxyl has been oxidized. Sulfate right? B.A.S.O4 plus 2C gives B.A.C2 plus SO2 plus 4C. B.A.C2 plus SO2 plus 4C. What is left? Hydroxyl. Hydroxyl has been done and Mg was worldwide right? Mg was worldwide. Mg was worldwide. Plus 4C. Yes Mg C2 H2O2. Right on these carbides are reducing in nature. Right on alkali metal carbides are soft in nature. Are soft in nature. But the other carbides are hard. Silicon gas structure is given in NCRT? Yes. One more compound you write down then we will see. Carbonic acid what is the formula of carbonic acid? H2CO3. We call it strong acid. It is a weak acid. It is not organic but weak acid. H2CO3. Right on it is prepared by the reaction of CO2, CO2 and water. Reversible reaction CO2 plus water gives H2CO3. Right on and hence and hydride of H2CO3 is what? Carbon dioxide. We also call it as carbonic hydride CO2. CO2 is the carbonic hydride and hydride not hydride. Carbonic and hydride of H2CO3. It is a dimasic acid H2CO3. Dimasic acid and it is conjugate base. And it is conjugate base is stable because of what kind of resonance is there? No that is conjugation. It is conjugate base is stable by equal resonance. CO3 2 minus CO2 plus water. CO3 2 minus CO2 plus equal resonance. So it is conjugate base is highly stable because of equal resonance. And hence it is a good acid. However it is weaker than all those H2CO4, H2CO3, H2CO3. Okay next write down compounds of silicon. Compounds of silicon. First one. SiCl4 carbon tetrachloride. SiCl4 silicon tetrachloride. Yes write down it is prepared by SiCl4. It is prepared by passing tri-chlorine tri-Cl2 over heated silicon. Tri-Cl2. Tri-Cl2. Tri-Cl2. Si plus 2Cl2. Water we do not use here because then it forms hydroxide. Tri-Cl2 plus 2Cl2 forms SiCl4. Second method of preparation is by heating magnesium silicide empty Si. Magnesium silicide Cl2 forms SiCl4 plus empty silicide. So heating magnesium silicide. Yes write down SiCl4 easily hydrolyze to form silicic acid. Si NiCiC. Silicic acid. Si NiCiC. Silicic acid. The formula is SiOH. On hydrolysis it gives SiOH. Okay. Silicon has vacant the orbital. Vacant the orbital. Okay. Silicon has vacant the orbital. Vacant the orbital. And hence it accepts the loom pair of electron from water. Accepts roll pair from water and releases H plus ion. So basically you see SiCl4 has a tetrahedral structure. Right. Now with water what happens H2O. It has vacant the orbital. And accepts one pair of electron from this. And then what happens this H plus and this Cl minus comes out forms. We will get what SiCl3. Similarly the same reaction we have three more times. Okay one by one. So we are using four moles of this total. And eventually you will end up getting SiOH4. For how many moles of HCl? Three moles of HCl here. Total four. Total four HCl. For last reaction is right out. SiCl4 goes under reduction reaction with hydrogen. Goes under reduction reaction with hydrogen. And forms silicon pure silicon. So SiCl4 plus H2O gives Si plus HCl. Si plus HCl. Okay next compound right out carbon random. SiC carbon random. This is the which compound. Carbon random SiC. Silicon carbide. It is obtained when a mixture of silica. It is obtained when a mixture of silica and carbon. Is strongly heated. Reaction is right out. SiO2 plus C gives SiC plus CO. SiC plus CO. Right out next properties. Pure carbon random is colorless. Is colorless. Very hard. But less than, hardness is less than diamond. But it is also very hard. Chemically inert. The structure of carbon random is similar to that of diamond. Okay. Very hard chemically inert. Even it is not attacked by HF also. HF is a very strong oxidizing agent. But it is not getting attacked by HF. The structure is similar to that of diamond. Does it look like a diamond? Not exactly. It does not look like diamond. The structure is same. It is not that shiny. Why is it yellow? Why is it yellow? SiC if you see. The structure, entire structure if you see. So the entire structure is stable at normal condition. This normal condition you are talking about. So the electron present in the shell, which is bonded with the carbon atom. It does not go to the excited state of normal condition. That is why it does not react easily. But again, if you use very high heat here, or very high temperature, then maybe some excitation is possible in the reaction process. Okay. So next we write down. Next. One last one. Silicone. Wait on. These are the hydrides of silicon. Hydrides of silicon are silicone. It is look like diamond only. Diamond texture we have no SiC. So you see. Silicone will be there in the center. And carbon will be like this. And it is associated molecule. So it is associated with another silicon. The entire crystal is like this. So silins are what? These are the hydrides of silicon. It may exist as a straight chain. A straight chain. Or branch chain. It is prepared by. It is prepared by acid hydrolysis of magnesium silicide. Acid hydrolysis of magnesium silicide. Magnesium silicide. Which gives a mixture of silins. Which gives a mixture of silins. This is the reaction. Mg2Si. When reacts with HCl. It forms SiH4. It can also form Si2 and Si3H8 like that. SiH4. Si2 and Si6. Si3H8 and so on. Mixer of silins we get here. Which can be separated by fractional distillation. Which is not there in our syllabus. Little bit we will discuss in solution chapter. What is distillation and fractional distillation? So this can be separated by that. But since we are getting mixture of compounds here. Then this method is not that useful. So other method we use for the preparation of silins. And that is. In this right on magnesium silicide Mg2Si. Is allowed to react with. Ammonium chloride in presence of liquid H3. Mg2Si. Plus NH4Cl. Liquid H3. It gives you SiH4. SiH4. Pure form of this. SiH4. Some other compounds will also get ammonia. This is the pure form. Another method of preparation you write down. By the reduction of. By the reduction of silicon halides. That is SiCl4. SiCl4. With LiClH4. Lithium, aluminium. Right. SiCl4. Reacts with LiH4. LiClH4. In presence of ether. Ether is a solvent here. Okay. It forms as LiCl. Plus. AlCl3. Plus SiH4. This reaction is important. We will get pure form of silicon. Okay fine. So there are few structure of silicates. Okay. Structure of silicates. For that I will share the nodes with you. Okay. That we need to go through the structure and memorize that. Sometimes they ask me like that. But not that important. Okay. Silicon. Overall silicon is not important in this chapter. A little bit of structure of silicon. Silicons. Okay guys. I will share the nodes with you. Thank you.