50 Rumus Kimia I Love You Too

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Jul 04, 2022 · Unsur kimia i love you. Sebuah atom terdiri atas inti atom (nukleus) dan dikelilingi oleh elektron. Source: keepcalm-o-matic.co.uk. Senyawa kimia i love you. Gunakan rumus ini u b r b2 r d b u r2 b2 r u2 r d2 l2 f2 l2 d nb. Source: www.gurupaud.my.id. Rumus kimia i love you… 0

Oct 17, 2020 I love you so much saya sangat mencintaimu 5. Kimia kelas x sma terdapat materi tentang molekul. Di makan was ate di lihat was see di buat are made dan lain sebagainya. Rumus kimia dasar unsur molekul rumus kimia gas oksigen yaitu o2 berarti rumus kimia … 1

Aug 31, 2021 · Rumus Kimia I Love You. Rumus kimia disebut juga rumus molekul karena penggambaran yang nyata dari jenis dan jumlah atom unsur penyusun senyawa yang bersangkutan. H2SO4 Asam sulfat 6. Kemudian sang wanita membalasnya langsung dengan kata i love you too. Gunakan rumus ini u b r b2 r d b u r2 b2 r u2 r d2 l2 f2 l2 d nb. THE WAY I LOVE YOU … 2

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all right good morning so we are one, more quiz through completing this course, successfully as much as I like to joke, you should fall behind early so you have, longer to catch up I know it's truly, hard to keep on top of things and one of, the reasons we have these quizzes is to, help in addition to integrating the, homework and the discussion sections is, to help us keep on top of the material, because 10 weeks really does go by very, very quickly well today we're going to, start on chapter 4 and begin discussing, alkanes in some ways alkanes are the, least interesting of organic molecules, but they're also going to serve as a, platform for beginning to discuss, stereochemistry and for discussing, confirmations of molecules the, three-dimensional shapes of molecules so, we're going to have a lot of meat in, this chapter this is the chapter that, you're going to start to use your, molecular models begin to play with them, like we've seen in the videos we're, going to be using rulers to help us and, to help integrate the exercises in the, chapter with the discussion section and, the midterm exam if you haven't already, done so you should get yourself a good, ruler that measures in centimeters one, that's a full 1 foot long 30 centimeters, in length so that you'll be prepared to, ask to answer questions that are asked, of you involving the molecular models, all right well let's begin what will be, 4 lectures on the chapter on alkanes so, alkanes are saturated hydrocarbons they, have a general formula of C and, in being an integral number of carbons h, 2 n plus 2 and we're also going to lump, into our discussion of Sacher of alkanes, we'll also lump in cyclo alkanes these, are saturated hydrocarbons with a ring, in them as such they have two fewer, hydrogen's you basically connect the end, of a chain together at a position where, two hydrogen's would be to get a ring so, you'll have a general formula cnh2n as, an example of an alkane I'll just take, octane you've heard of octane before of, course in terms of the octane number for, gasoline the octane numbers actually not, determined by the parent compound octane, but rather by a branched isomer of, octane what octane gives your car is not, power all of the hydrocarbons burn with, about the same amount of energy but, rather what octane are more specifically, this branched isomer of octane does is, it burns in a way that causes your, engine not to knock so on an octane, scale octane is a hundred and heck, heptane a seven carbon alkane has an, octane number of zero anyway octane and, all of its isomers have a formula c8h18, and by comparison we'll take as an, example for a cyclo alkane, take cyclohexane cyclohexane is going to, become a good friend of ours because it, has an interesting conformation and, interesting shape with very regular, properties and this ring can be found in, various steroids steroids of course are, both compounds that people take illness, Utley for sports performance but they're, also the estrogen and androgen sex, hormones, anyway cyclohexane itself has a formula, c6 h-12 hydrocarbons and alkanes in, particular come from petroleum there are, vast quantities under the ground and, unfortunately mostly they're used as, fuel burn 80% of the alkanes that are, produced and this is really a really a, shame given how valuable these are these, are the starting feedstocks for all, sorts of chemicals the plastics the, nylon in your backpack, the polyesters and the like and the, chairs that you're sitting on are all, ultimately derived from petroleum and, many of them from alkanes and from, cycloalkanes, so although they're mostly used as fuel, I'll write that they're important, feedstocks for chemicals and drugs, plastics as well I'll just write etc, because they're just about everything, you can think of as some component of, alkanes in it almost every chemical, compound you can think of or material, you can think of probably has had some, component of alkanes and petroleum in, the making of them since we burn them, I'll write one chemical equation you're, actually not going to see that many, chemical reactions of alkanes this year, you'll see some halogenation reactions, but on a day to day use when you take, your car and you put a mixture of, hydrocarbons as well as a few ethers, that contain octane in your car and you, burn it with oxygen we get carbon, dioxide and water a lot of times in, organic chemistry we don't balance, equations but I can easily balance this, we generate eight molecules of carbon, dioxide we generate nine molecules of, water and in order to do this of course, we need twelve and a half molecules of, oxygen, all right I'd like to spend a few, minutes not too long talking about the, various alkanes and about the, nomenclature of alkanes that is how we, name them also we'll talk about the, properties, it seems that any basic cultural, literacy probably should know the, physical and chemical properties of the, first few alkanes we've talked about, methane ch4 before it's a gas very low, boiling gas I think I mentioned in the, past it has a boiling point of negative, 162 degrees Celsius so we move along in, the chain the series we get ethane right, out its molecular formula since we, talked about c2 CN h 2 n plus 2 ethane, is C 2 H 6 in other words it's ch3 ch3, ethane is a gas but it has more van der, Waals interactions so it boils at a, higher temperature the boiling point of, ethane is negative 89 moving along the, series oh and I should write out write, out the name here, moving along the series propane c8, whoops c3h8 in other words ch3 ch2 ch3, propane is also a gas but propane is, interesting because by the time you get, to propane if you apply enough pressure, at room temperature you can liquefy it, so you can put a lot of it in a gas tank, it's boiling point, is not so not so low it's negative 42, degrees Celsius which is temperatures, that you get on well you can get access, to one on earth but what that means the, fact that you can liquefy and the fact, that the boiling point isn't isn't too, low is that it's a gas at 10 atmospheres, a liquid at 10 atmospheres an atmosphere, is 15 pounds per square inch so if you, looked on your card tires if you go to, the gas station and you put air in your, car tires you're putting in about 30 psi, about two atmospheres of pressure if you, have a bicycle and you have racing tires, on it you may be putting in 90 psi or, more six atmospheres of pressure so the, pressure and a propane tank is not that, much higher than you would access from a, handheld bicycle pump continuing along, the series butane c4h10 we should get in, the habit of writing out these, structures in the skeletal notation so, I'm going to do that for butane butane, is also a gas but it's boiling point is, negative 1 degrees Celsius so now it, would liquefy in the freezer that you, might have in your home or in your dorm, room of course if you smoke you pry, butane lighters and you see liquid, butane in those lighters butane is a, liquid the two atmospheres at room, temperature so the pressure and those, butane lighters is the same as the, pressure in your car tires if we, continue along the series of alkanes, pentane, c5h12 now pentanes a liquid it's a low, boiling liquid so we've gone from a gas, to a liquid and adding one carbon but, his boiling point is just 36 degrees so, if I were to take a few ounces of, pentane and spill it on the floor here, it would evaporate in just about no time, not only is the boiling point low but, because we just have Van der Waals, forces between the molecules the heat of, vaporization is low that means it, doesn't take a lot of energy to boil an, ounce of it and turn it to gas it takes, a lot more energy to boil an ounce of, water and to turn it to gas because the, molecules stick together one of the, things we're getting as we see these, molecules is we're also getting the, names of them so the first four names, basically are trivial common names we, talked before about how butane comes, from butter ethane comes from ether from, the air methane it turns out has a, connection to wood but beyond that we, get to systemic roots derived from greek, or latin so pentane you can think, pentagon the next one hexane c4 c6h14, hexane you can think like a hexagon if, you want to remember these names the, names all become systematic it's a, liquid it's boiling point is 69 degrees, now the other cool thing is when you, have a series of numbers like this you, can start to come up with some, reasonable predictions so if I asked you, the boiling point of heptane you might, say well I don't know the boiling point, of heptane but I can see that as we're, moving through this series the, difference between the boiling points is, just a little over 32, and it's getting closer together so I, could probably extrapolate that the, boiling point of heptane would be, somewhere just about a hundred degrees, Celsius so it's sort of cold you can, figure out the various trends all right, if we go through our name see seven age, 16 is heptane we saw c8h18 octane it's, probably worth knowing how to count to, about 12 and maybe knowing knowing 20, number 20 beyond that c9 age 20 is no, name NO in a and e c10 age 22 is decane, that's easy easy if you remember the C, when you're talking and writing deck, Cain's like 10 C 11 I'll just give you, two more and then I'll give you a number, 20 C 11 H 24 his undec pain and so you, see the principle becomes we're going to, add a prefix to specify that it's one, more than decane c12 h22 decane, and I'll give you one more just in case, you hear it, Aiko Sain is c20 H 22h 42 e IC OS am ii, in a couple of things that i should add, so our alkanes up through C 17 or, liquids they're light liquids so let me, let me jot this down over here so c5h12, pentane through heptad decane up above C, 17 they're solids they're kind of waxy, solids in fact if you push your finger, against them they're soft it's not a, surprise paraffin wax is a mixture of, high chain length long chain length, alkanes and in fact all of the alkanes, are known as the paraffins that's the, family of compounds to which they belong, the compounds are all light they're low, density, less than a gram per mil that means if, you put dodecane on water and water not, only will they not mix but the dodecane, will float to the surface, alright one of the things that alkanes, give us a chance to do is to introduce, ourselves to the concept of isomers, this concept already came up when we, started to look at Lewis structures of, various molecules and I remember when I, asked people the structure of methyl, azide a lot of people struggled to write, a structure and some people came up with, a lewis structure but it wasn't methyl, azide and this was the first chance we, got to see that there can be different, covalent connectivities of atoms, different what we call constitutional, isomers, so isomers are molecules with the same, molecular formula but different, structure and there are two main classes, of isomers one is constitutional isomers, constitutional isomers are isomers that, with different connectivity, we've already seen some examples but I'm, going to take us through and take us, through a little bit of systematic, thinking the other ones that are a, little harder to understand and we'll, get to them in just a couple of lectures, are stereoisomers and this is where your, models really shine for helping to get, things into your head stereoisomers have, the same connectivity but a different, three-dimensional structure, we'll get to this concept with, enantiomers and diastereomers but if you, want to know what I mean by the same, connectivity of it but a different, structure for now just look at your, right hand, and look at your left hand and both, hands have all of the fingers and thumb, connected in the same type of places and, yet they're not the same that's what I, mean by the same connectivity but a, different structure we'll also see, something that would be like with your, fingers pointing in different direction, and that's a type of type of, stereoisomer called a diastereomer what, you're seeing for your hands are a type, of stereoisomer called an enantiomer, all right so four isomers start with the, isomers of butane pentane and then we'll, talk about some other if we make a, linear chain ch3 ch2 ch2 ch3 or I draw, it as a zigzag structure of course you, have a molecule that's called butane, you'll sometimes see it referred to as, in butane in is a prefix that means, normal and so in butane is just a way of, saying yeah I mean butane not any isomer, of it I mean the straight chain compound, for contrast let me give you the one, isomer of butane CH 3 CH ch3 with a, methyl group off of the CH group off of, the what we call a methane group so if I, want to write this out in shorthand I'll, just write it like this, this isomer is not surprisingly called, isobutane since it's the only isomer of, butane we know what we're talking about, when you'd say isobutane these types of, names are what we call common names I've, mentioned them before the more, systematic name says oh this molecule, has a three carbon chain so it is a, derivative of protech propane we would, call it two methyl propane, now let's do the same thing with pentane, we're going to get three isomers for, pentane I'll write them out in shorthand, and what I want to get us used to is the, thought process for generating different, isomers, so pentane has three isomers and the way, I think about it is to say okay we have, pentane here or in pentane if I imagine, taking off one methyl group so I'm gonna, permute systematically through all the, different possibilities if I took off, one methyl group and I wanted to put it, somewhere where could I put it well I, could put it here or I could put it here, no matter where I put it I get the same, one I get the same molecule this, molecule is called isopentane, systematically it would be two methyl, butane and if you continue to think well, I can't take off an ethyl group and do, anything cuz if I take off an ethyl, group that's just gonna get me back to, two isopentane if I reconnect it but if, I take off another methyl group in other, words cut our chain down from 5 to 4 and, then from 4 to 3 the only place I can, put the methyl group to get something, unique is this molecule we've seen this, molecule before it's called neopentane, and it's systematic name as I've written, before is 2 to dimethyl propane, so as we go along the alkanes the number, of isomers increases dramatically butane, I'm gonna write this all out just so you, can see the whole trend butane has two, constitutional isomers pentane we saw a, three hexane as five heptane as nine and, if you want a good exercise this is one, that's worth doing in your next class if, it's boring is to try to write out in, this one in the last five minutes if, we're boring to try to write out all, nine constitutional isomers of of, heptane I did this yesterday at the, blackboard as I was thinking about what, I was going to say today and starting to, realize though I need to scratch my head, for a moment but yep there are nine of, them and it's a good exercise because, it's just the right number not to be, tedious and to get you into the right, mental processes if we go up to octane, now we have 18 the numbers really, increase and I mentioned this before, about organic chemistry this is what's, so amazing that just a few atoms can be, put together in so many different ways, the petroleum companies love these and, they are trying to catalog every known, isomer of all the molecules you can, found fighted petroleum sighs just, talking to my colleague and they paid, him vast his laboratory vast sums of, money for a few milligrams of obscure, hydrocarbons dodecane has 355 I won't, ask you to try to write all of those out, and I Kasane has a whopping three, hundred and thirty six thousand three, hundred ninety, isomers definitely not something to end, up writing out, so, we've already used the isomers of, pentane as a platform to talk about van, der Waals interactions and I just want, to bring this out again now that I've, laid them all in the open pentane I said, has a boiling point of 36 degrees all of, the other isomers both of the other, isomers have the exact same amount of, stuff in them and yet they're more, compact and as a result you get fewer, Van der Waals interactions isopentane, has a boiling point of 30 degrees, neopentane a boiling point of 9 degrees, so this is just an illustration of the, concept that we had before all right I, want to take a last moment to talk about, describing the various carbons in, hydrogen atoms and let me take as an, example isopentane 2-methylbutane as an, example so that we can start to see what, chemists refer to for the types of, groups and hydrogen's and carbons in the, molecule so here's our isopentane i'm, going to write it out explicitly and so, the terms that you will hear for the ch3, group we've used before a methyl group, the ch2 group we referred to as a, methylene group in the CH group we refer, to as a methane group, these types of names are not just, nomenclature they also give sense and, structure to the molecules and lend, sense to the reactivity of the molecules, there's a related way of naming things, and something that you should be aware, of and so I'll take our isobutane again, as an example or isopentane again as an, example and we talked about the types of, carbons and hydrogen's in the molecule, we describe a carbon with one other, carbon as a primary carbon you'll often, see this is one not one degree carbon, and the hydrogen that's attached to it, described as a primary hydrogen this, type of distinction is important because, primary hydrogen's and secondary, hydrogen's and tertiary hydrogen's have, different reactivity carbon with two, carbons attached is the secondary carbon, so again we'll use two not as the, abbreviation carbon and in turn the, hydrogen is a secondary hydrogen, and on this molecule the methane group, the CH group we refer to the carbon as a, tertiary carbon so I'll use three naught, and the hydrogen as a tertiary hydrogen, now not exemplified in this molecule but, exemplified in neopentane there's one, last type of carbon for which of course, you won't have a hydrogen and that's a, high a carbon with four carbons attached, to it and we refer to it as a quaternary, carbon alright well that is what I would, like to say about alkanes for today, tomorrow we're going to earn Wednesday, we're going to pick up with some, systematic nomenclature and then we'll, move on to some other aspects of alkanes

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