CHEM 125a: Freshman Organic Chemistry I
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Freshman Organic Chemistry I
CHEM 125a - Lecture 22 - Radical and Type Theories (1832-1850)
Chapter 1. Benzaldehyde and the Focus on Radicals [00:00:00]
Professor Michael McBride: So in 1832, as we saw at the end last time, Wöhler went to work for most of a month with Liebig, and together they worked on the oil of bitter almonds, which is making its way around — it’s benzaldehyde — which is making its way around here. So there’s the bottle that’s coming around. What did you notice about it? Where is it? What do you notice about it Devin?
Professor Michael McBride: Yeah.
Student: About the smell?
Professor Michael McBride: What does it smell like? Is it almonds? Turn it around, look at the — turn it upside down. What do you notice?
Student: There’s a little bit of solid in the bottom.
Professor Michael McBride: Yeah, it’s half solid. Benzaldehyde is the oil of bitter almonds; not the solid of bitter almonds. What does it say on the label, written by hand? Somebody’s initials, J.W.
Student: J.W., 11/29/95.
Professor Michael McBride: So it was opened in 1995, thirteen years ago. When it was opened it was a liquid. Now it’s half solid. How do you figure that? Well something must’ve happened. So what did it react with, in the bottle? Yoonjoo?
Professor Michael McBride: Oxygen. Okay? So oil of bitter almonds; they analyzed, C7H6O, and they found that it reacted with oxygen to get C7H6O2. Right? They also reacted it with bromine. The halogens were common, as we’ll see, for reagents in those days. Got C7H5OBr. They reacted it with chlorine, and also that product with potassium iodide, or ammonia, or lead sulfide. And they got all these compounds. And what did they do with them when they got them? They smelled them. Right? What was the main thing they did?
Student: Tasted it.
Professor Michael McBride: No that’s not the — it’s true that they probably tasted, that they tasted them, but that’s not the main thing they did that gave them unique information.
Professor Michael McBride: What about the weight? What was the main technique that we’ve been talking about all the time? Dana?
Student: The analysis of combustion.
Professor Michael McBride: They did an elemental analysis; ultimate analysis of what the ratio of the elements. So that’s what they had. Right? So big deal. What do you get from the analysis? What can you infer? Here were these guys; you could now compete with them, right? This is what they found out during that month of experimentation, and they came up with a theory that revolutionized organic chemistry, as of that time and for the next twenty years. So what did they notice? Claire?
Student: They noticed the carbon chains.
Professor Michael McBride: Pardon me?
Student: The carbon chains.
Professor Michael McBride: Well how would you know it’s a chain? The numbers don’t tell you it’s a chain. What?
Student: The presence of the hydrocarbons.
Professor Michael McBride: Well it’s, it’s got hydrogen and carbon in it. That’s true. But they also have oxygen and nitrogen, chlorine and other things. What could you make out of this? Brian?
Professor Michael McBride: Yeah. All of them have at least C7H5. Some of them have more hydrogen than that, but nothing has less than C7 or less than H5. Can anybody carry that any further?
Student: C7H5 is non-reactive.
Professor Michael McBride: Pardon me?
Student: It’s non — the C7H5 is the unreactive part.
Professor Michael McBride: Yeah. What would they have called it; the thing that you have it there and then it reacts and gives this, that, or the other thing? What did Lavoisier call it?
Student: The radical.
Professor Michael McBride: The base, or the radical. But actually the radical is more than C7H5, the thing that persists. What else?
[Students speak over one another]
Professor Michael McBride: O. So C7H5O persists through all these transformations. So it looks like that’s some sort of a core that gets modified. Okay? But it’s there all the time. It’s like a radical. Right? So it was called the benzoyl radical. They thought up that name at that time, and the idea of using the suffix -yl, to denote a radical. So if you denote the benzoyl radical by Bz — you see that you started, the oil of bitter almonds is BzH, and then the acid is BzOH, and the acid chloride is BzCl and Br and I and NH2 and two Bz’s, together with S, at the end. Okay? So a radical can be the base of more than just an acid. Right? Lavoisier had the idea that you react it with oxygen and you get an acid. But here you can react it with all sorts of different things and get different compounds. But the base is still there, the benzoyl radical. So this gave rise to the idea of organic dualism. Remember, we had this dualism last time. There were positive things and negative things and they could associate and trade partners. But maybe the difference in organic chemistry is that you have radicals, things that are plus or minus, but they’re more complicated than just single atoms. There are combinations of elements that function in organic chemistry; and that’s what makes it different from inorganic, according to this theory. So then the idea is to find all these organic radicals, that make organic chemistry special.
So during the 1830s these compound radicals were discovered everywhere. For example, in Germany, Liebig found acetyl. And Bunsen, in Heidelberg, found cacodyl; which is named because it smells so awful. Right? Or Berzelius in Sweden found ethyl. Or Piria in Italy got salicyl. And Dumas got a whole bunch of them, in Paris: methyl, cinnamyl, cetyl, ethylene. All these radicals were discovered. So the thought was this is the way to organize organic chemistry. And that theory, the dualism applied to organic theory, the radical theory, survives today in our nomenclature. Right? So, for example, we talk about ethyl chloride. That’s not one word, it’s two words, with a space. Right? And the reason is it’s dualistic. It’s a positive ethyl and a minus chlorine. Right? So it’s two things that have come together.
Okay, now the -yl part, that Wöhler and Liebig thought up, comes from a Greek word, üleh, which means wood or matter. So it’s the substance of stuff. Okay, so now ether was something that had been known for a long time, and it came from a Greek root which means to shine. So in the 1700s it was — so it had been applied to the sky. It was transferred from the idea of shining, to the idea of the clear sky, and from that to a colorless liquid. So when they distilled something out of alcohol that had been treated with acid, and they got this clear stuff that was clear as the sky, they called it ether. Right? Which we call diethyl ether nowadays. So that’s where “ether” came from. So hence eth-yl was the matter that appears in ether. So it was like two benzoyl radicals with sulfur. Right? You can have two ethyl radicals with oxygen. Right? And that was then eth-yl — right? — the material of ether. Okay?
How about methyl? Well meth comes from the Greek word meaning wine or spirit. Right? And the -yl, that same root, but a different meaning this time. Remember, it can mean matter — that was the one before — or it can mean wood, and in this case it means wood. So what does it mean, meth-yl, if the -yl means not the substance of but means wood?
Student: From wood.
Professor Michael McBride: Pardon me?
Student: From wood.
Professor Michael McBride: From wood. What from wood?
Professor Michael McBride: The spirits, from wood. So you’ve heard methanol called wood alcohol — right? — because you get it from distilling it. But the first word was methylene, and ene is the Greek feminine patronymic; it means “the daughter of.” And ene, ine, one, all of those are like that; like Persephone, or Antigone means the “one who goes against her parents,” and so on. So ene was the Greek — so what did meth-yl-ene mean? It meant the daughter of wood spirits. So the theory was that wood spirits, that is, wood alcohol, was a combination of methylene plus water. So methylene thus, if wood alcohol is CH3OH, then methylene was CH2; which then you add water and you get wood alcohol. So that’s where the name methylene came from. Right?
So then in 1840 — that was 1835, so five years later — they decided that they needed the radical CH3. So they named it methyl, from methylene. Right? And then ethylene came; that name came in 1852, because it was related to ethyl, which had already been named, the same way that methylene was related to methyl. Okay? So that’s where these names came from. They all have their root in the radical theory. Now, that’s C1 and C2, methyl and ethyl. How about C3 and C4, do you know what they’re named? Roots? How about C3, do you know what C 3 alcohol is?
Professor Michael McBride: Propyl. And C4?
Professor Michael McBride: Butyl. So where do those names come from? Okay, C3H7 is propyl, and by the same reasoning as before, C3H6 is propylene; or propene, sometimes it shortened. Okay? And butyl and butylene, or butene. Okay, now butylene comes — the C4 acid is butyric acid, which had already been named, because it’s the stuff that makes rancid butter smell bad. Okay? So people worked it up and found butyric acid; so that’s where butyl comes from. But how about propyl? It has a very much more interesting origin. Okay, so protos means first, and pion means fat. So propion was the first fat. In what sense? Well these carboxylic acids came from fats, right? And they were called fatty acids. And they behaved like fats, they dissolved in organic solvents. Right? But the very — the ones with the fewest number of carbons, with just one carbon — that’s formic acid that you get by destructive distillation of ants, or acetic acid, from vinegar — those are miscible with water. But the C3 is the first one that’s not freely miscible with water; it behaves more like a fat. Right? So the first fatty acid is propionic acid. So propyl, propylene are the C3s. Okay, after that you get into numbers, the roots for numbers.
Chapter 2. Dumas’s “Note on the Present State of Organic Chemistry” [00:12:52]
So Jean-Baptiste André Dumas was the successor of Gay-Lussac as the spokesman for French chemistry. You see, he was born on the 14th of July, a reasonable date for somebody to lead French chemistry, in 1800. So for eighty-four years — well, for part of eighty-four years, he was the leader of French chemistry. There he is with some decoration on him. I’m not sure what it is. I’d like to find out. So he was the Post-Napoleonic guardian of the French tradition of chemistry. The French had what most people regard as a terrible system, which is they had chairs, you know, for professors. But you could have more than one chair. So a single individual could tie up three different appointments, and you didn’t have as many people able to exercise their ingenuity in developing chemistry. So he had the chair at the Sorbonne; also the École Polytechnique and the École de Médicine. And he was a persistent opponent of Liebig and Berzelius. But in 1837, after this radical stuff got going — and he had discovered four radicals himself, of which he was quite pleased — he and Liebig happened to meet during a speaking tour in England, and they got in conversation, and Dumas decided, on the basis of that meeting — though not Liebig — that they were now great friends and could collaborate from here on in.
So he wrote this long thing, in flowery French, in 1837, “A Note on the Present State of Organic Chemistry.” So this is five years after the Radical Theory began. He said: “Sixty years have hardly passed since the ever memorable time when this same assembly” — he was speaking to the Paris Academy — “heard the first discussions of the fertile chemical doctrine which we owe to the genius of Lavoisier. This short span of time has sufficed to examine fully the most delicate questions of inorganic chemistry, and anyone can easily convince himself that this branch of our knowledge possesses almost everything that it can with the methods of observation available.” So check off inorganic chemistry, we’ve got that now. Okay? “There barely remain a few cracks here and there to fill in.” So this is the persistent myopia of leaders of science. As I mentioned before, when we were speaking of Lavoisier, this certainly persists ‘til today. So Dumas goes on: “In a word, how with the help of the laws of inorganic chemistry can” — incidentally, this is all one sentence, of course. This is “in a word”, right? So he really liked speaking, right?; flowery language. “How with the help of the laws of inorganic chemistry can one explain and classify such varied substances as one obtains from organic bodies, and which nearly always are formed only of carbon, hydrogen, and oxygen, to which elements nitrogen is sometimes joined?” So if it’s all in the analysis of what atoms are there, how can you have so many different things? Right? “This was the great and beautiful question of natural philosophy, a question well designed to excite the highest degree of competition among chemists.” Name two, right?
Great and beautiful questions to answer. It only remains to follow through the consequences; compounds which behave like elements. “Thus organic chemistry possesses in its own elements, which sometimes play the role of chlorine or oxygen” — what does he mean, play the role of chlorine and oxygen? How come radicals sometimes play the role of chlorine and oxygen? What would that role be?
Professor Michael McBride: Pardon me?
Professor Michael McBride: No. What roles do things play in this theory that he’s using? Lucas?
Student: Plus and minus.
Professor Michael McBride: Plus and minus. So sometimes they’re like chlorine or oxygen. What does that mean?
Professor Michael McBride: Sometimes they’re negative, right? “And sometimes, on the contrary, they play the role of metals.” Sometimes they’re positive.
So that is what everybody should do. Then you’ll know all about organic chemistry.
Right? So if everybody does what we say they should do, then we got it. Okay? “This is not an effort conceived for personal gain or in the interest of narrow vanity.” Far be it from us. “No, and in a collaboration which is perhaps unheard of in the history of science, this is an undertaking in which we hope to interest every chemist in Europe.” So everyone should work on this. So we’ll go to the funding agencies and tell them this is the only kind of research you should fund; forget these other guys out there. This is true love of science, right? And conceived in the same spirit and carried out by the same methods. So this is megalomania, and doesn’t show much imagination. Now, but there was a problem with dualism. So, for example, suppose you have benzoyl chloride, which remember was by reacting benzaldehyde or benzoyl hydride with chlorine, and you get benzoyl chloride and HCl as the other product. Now HCl is quite clear, it’s H+ and Cl-. What’s benzoyl chloride? It’s obviously benzoyl+ and Cl-. And what problem does that create? What, Russell?
Student: The benzoyl is minus before, but hydrogen —
Professor Michael McBride: Ah ha. But how do you get benzoyl hydride, plus, plus? Right? So there’s something weird going on. So this is a problem.
Chapter 3. The Mystery of the Chlorinated Candle [00:21:39]
In the 1840s and 1850s, the French discovered a competing theory — or invented, I should say — a competing theory called the substitution theory, or the type theory, or the unitary theory, as opposed to the dualistic theory, the plus, minus idea. So these began to compete with one another. And it started at a ball in the Tuileries Palace in 1830. This picture is from 40 years later, or 37 years later. But what happened is they got the ball started, all the people came dressed up fancy, and they began to cough and choke because the room was filled with some noxious gas. And when they discovered it came from the candles, they asked Dumas to look into it. And he identified the culprit as HCl, because it turned out that the candles were very white. The wax had been bleached with chlorine, and when they were burned HCl was given off. So the question is, what is it that holds chlorine? How did this fat, in the candles, fix chlorine gas? Well you’re in a position to understand that now. We can think about mechanisms; in fact, two ways that the hydrocarbon could fix chlorine. Now, suppose we try — there’s chlorine that is being used to bleach the stuff. Let’s try for a HUMO/LUMO approach. What makes chlorine reactive? High HOMO or low LUMO? What’s unusual about chlorine?
Student: Low LUMO.
Professor Michael McBride: Pardon me?
Student: Low LUMO.
Professor Michael McBride: Why do you say so Claire? What is the low LUMO?
Student: It’s the Cl-Cl bond.
Professor Michael McBride: Right, the σ* of Cl-Cl, which is low because chlorine has a high nuclear charge. Okay, now we need a HOMO to react with it. Now, one of the more interesting hydrocarbons, in this regard, is one that had been known already, for fourty years, to react with chlorine. And it was because of that reaction it was called the “olefiant gas,” and was by this time known to be C2H4. Right? So we would write it with a double bond. “Olefiant,” because ole, oil, and fiant, to make; so it’s the stuff that makes oil. Right? And we’ll see the reaction that makes oil here, its reaction with chlorine. So what makes the olefiant gas reactive? Kevin?
Student: Poor overlap.
Professor Michael McBride: Right, so poor overlap makes a high HOMO. And remember the name of it?
Professor Michael McBride: π. So the π electrons because of poor overlap are a high HOMO. So we can use those electrons to mix with the low LUMO; and again, one of these make-and-break situations. And chloride leaves and you get this thing, which has a positive charge. Now that thing itself is reactive. What do you make — where is a low LUMO in this one? Pardon me?
Student: On the positive charge.
Professor Michael McBride: Speak up please.
Student: On the positive charge.
Professor Michael McBride: Where the positive charge is. There’s a vacant orbital on carbon, an atomic orbital of carbon that’s not shared. So there’s a low LUMO. Where’s a high HOMO? Have you got that too Virginia?
Student: On Cl.
Professor Michael McBride: Chlorine has unshared pairs, right. Bingo! So, in fact, both those things happen at once. It’s not that one happens and then the other. Both those things happen at once. And you can see it by looking at molecular orbitals. So there’s the HOMO of the ethylene or olefiant gas, and the σ* LUMO. So those things mix. The blue orbitals overlap and mix, shift electrons toward the other one; the chloride breaks away. But at the same time the HOMO of the chlorine mixes with the LUMO of the ethylene. So you’re making two bonds at once, two pairs of electrons. So you make that three-membered ring, with two new bonds, and the chloride, as we said, breaks away. Okay, so we’ve got that substance now. And now it itself is reactive. Can you see what would be reactive about that cation intermediate? What are you probably looking for, a LUMO or a HOMO?
Student: A LUMO.
Professor Michael McBride: A LUMO. Angela, do you have an idea of what could be a LUMO here?
Student: The chlorine has a positive charge.
Professor Michael McBride: It’s true that the chlorine has a positive charge. Does it have a vacant orbital, an unoccupied molecular orbital?
Student: No it doesn’t.
Professor Michael McBride: No, it turns out it’s got two unshared pairs. So it doesn’t have any — it’s not like the carbon plus was. But the plus will make orbitals low in energy. So what’s a vacant orbital of this thing? All it’s got is σ bonds. But what makes — suppose all you have in your molecule is σ bonds, but you want to have an unusually low energy vacant orbital. Right? The plus charge will help. But what orbital will you have?
Professor Michael McBride: σ*. Now you got two choices. You got carbon-carbon or carbon-chlorine. Which one’s more likely to be low energy?
Professor Michael McBride: Why?
Student: Because the chlorine —
Professor Michael McBride: Say it —
Student: Chlorine has a high effective nuclear charge.
Professor Michael McBride: Right, chlorine has a high nuclear charge. So a σ* carbon-chlorine, would it be big on carbon or big on chlorine, Sam?
Student: Big on carbon.
Professor Michael McBride: Big on carbon, because the bonding orbital was big on chlorine. Right? This is the kind of stuff we’re talking about. So σ*. And there it is. Okay, there’s a localized σ*. Big on carbon, the black one; small on chlorine; and antibonding between them. Now what are you going to — there’s the low LUMO. What do you have for a high HOMO, to react with it? You have to think back to what’s been happening. Sherwin?
Student: The chlorine one.
Professor Michael McBride: The chloride that you had at the beginning, that you lost in the first step. Okay, so we bring it over here. So it’ll have good overlap. It comes up, makes a new bond; that make and break. And you get that. And that was the reaction in 1795 that resulted in ethylene being called the olefiant gas. Because this is the oil that was made, by reacting it with chlorine. So that was already a very old reaction at this time; the “oil of Dutch chemists”, because it was four Dutch chemists who reported that oil. Okay, so there’s one way that you can fix chlorine, make it part of a hydrocarbon molecule. It’s addition to an alkene. So if the hydrocarbons are unsaturated, if they have some double-bonds, then they’ll react with chlorine to fix the chlorine. So that’s one possibility. But how about if you don’t have a double bond? How about if you have methane? What’s the problem now, in doing an analogous reaction? Sherwin?
Student: You don’t have the π in there.
Professor Michael McBride: Pardon me?
Student: We don’t have the π in there.
Professor Michael McBride: You don’t have a π. You don’t have a low LUMO. So you can’t do a HOMO/LUMO reaction. Right? These are our model, saturated alkanes, like methane, our model of things that aren’t unusually high or unusually low. So you have to have another trick. And here’s the trick; that the chlorine-chlorine bond is weak. It’s only 58 kilocalories per mole. And one of the reasons for that is that the chlorine has so many unshared pairs. So you mix — if you were trying to form a π orbital in chlorine, you have two electrons in the p orbital here, two electrons in the p orbital here. They overlap. Is that going to be bonding, if you mix these two orbitals? You’ll obviously mix them. When you mix two orbitals you get a lower one and a higher one. Will it be bonding? This one will be bonding but this one is anti-bonding. Everybody with me on this? Now, so Kate, what would you say? Is it going to be net favorable or unfavorable? Two electrons went down in energy, two electrons went up in energy. But the ones that went up, went up a little more than the down went down. So that’s unfavorable. So having so many unshared pairs weakens the single bond. So chlorine has a weak bond. Now still it’s worth 58 kilocalories per mole, which is plenty strong. It doesn’t just break. You got to do something to help it to break. And what you can do is — I’ve made it in this weird color, which is hard to see. Why? Anybody know?
Student: The color of chlorine.
Professor Michael McBride: Pardon me?
Student: It’s the color of chlorine.
Professor Michael McBride: That’s the color of chlorine. It absorbs visible light. Now how does it take on energy, when it absorbs visible light? Where does the energy go, in the molecule? Does anybody know? Dana?
Student: Electrons are promoted.
Professor Michael McBride: Can’t hear very well.
Student: Electrons get promoted to higher —
Professor Michael McBride: Electrons go from orbitals to higher orbitals. So you can put — and the next higher orbital is σ*. And what happens if you take an electron and put it in σ*? It breaks the bond. Right? That’s what happened up at the top, when the chlorine broke, right? You put electrons into σ*. So you can do it with light, as well as with some HOMO attacking. Okay, so we have — in fact, I said LUMO when I was talking about ethylene; I meant HOMO up above, I think, some three or four minutes ago. Okay, so the bond breaks. But it doesn’t break into ions. It breaks one electron going each way, because that’s easier. Okay? And notice that we draw curved arrows for that too, but you draw arrows with a single barb rather than a double barb, when it’s just one electron rather than a pair of electrons that’s executing the motion we’re talking about. Okay, so now we have two chlorine atoms. And now we can do the trick with the chlorine atom, because we have this SOMO, and it can mix with the C-H bond to make a new bond; that is, one electron in the C-H bond now goes each way. One goes to complete the pair, to make HCl, and the other one is left on carbon. Right? So it’s very much like the reaction above, but it’s single electrons that are doing the moving instead of electron pairs. And the nice thing about this is you still have a radical. It must be so. If you start with something with an odd number of electrons, and react it with something with an even number of electrons, you must be left, at the end, with an odd number of electrons. Right? So CH3 is such a radical, and it can react with something, to break another bond, and it reacts with the weakest bond, chlorine. Right? So now you have methyl chloride — you’ve incorporated chlorine into the alkane — and you have a chlorine atom. Why is it neat, that you have a chlorine atom? What’s great about that?
Professor Michael McBride: Dana, what did you say?
Student: That was what you started with.
Professor Michael McBride: That’s what you needed at the beginning. That’s why you used light, in order to get that. But you don’t need any more light now. Right? That can go back and start over again. So it’s a “chain” reaction. It’s called a free-radical chain reaction. And so you can get lots of products from just one initial photon of light, that started this chain along. So these are two completely different ways. The first, the top is an “addition” of chlorine to an alkene, and the bottom is called free-radical “substitution” of chlorine for hydrogen, and involves SOMOs, rather than HOMOs and LUMOs. Chris?
Student: If you have a second chlorine radical from the first breaking…
Professor Michael McBride: Yeah.
Student: …why does it break a second chlorine molecule, rather than using the other —
Professor Michael McBride: Because they have to find one another. Right? They’ve gone off — it’ll take forever before they by chance encounter one another in solution. They’ll react with many molecules. If you try to generate too many chlorine radicals, so the concentration gets high, then their concentration will drop again, or not get so high, because they find one another and combine. But as long as they’re rare, they can survive. You know what the license plate of New Hampshire says on it? “Live free or die.” Okay? I use that joke later on. Okay, 1830s to 1850s, we have this substitution or type or unitary theory. It doesn’t involve the plus/minus stuff. Max?
Student: Is that kind of like how CFCs work?
Professor Michael McBride: Is it kind of like what?
Student: How CFCs destroy the ozone.
Professor Michael McBride: I couldn’t hear clearly.
Student: Is that how CFCs break down the ozone?
Professor Michael McBride: Yeah, they involve — that’s a free-radical chain reaction, the ozone reduction. Yeah. We’ll talk about that a little bit later, I hope.
Chapter 4. Further Development of the Law of Substitution and the Theory of Types [00:35:00]
Okay, so there’s more trouble for radicals, from Dumas in 1839. And that is that they had this — remember, acetyl radical had been discovered by Liebig. So there was this great element that would survive from reaction to reaction. But here was a reaction with chlorine, of this kind that Dumas had been studying, where you start with acetic acid, acetyl OH, react it with chlorine, and you get a chloroacetyl. So the element has been changed. It’s been transmuted. It doesn’t go unchanged from reaction to reaction. Right? And, in fact, it goes even further. It can react again to give dichloroacetyl or trichloroacetyl. All the hydrogens can be substituted, as we now know by the kind of mechanism, the SOMO mechanism, we just studied; free-radical chlorination, chain reaction. So hydrogen can be substituted by an equivalent amount of halogen, or oxygen, right? But all these things you get, when you change a radical into something else, when you transmute it, have similar properties. All of these acids — acetic acid, chloroacetic, dichloroacetic, trichloroacetic, are all acids; they all taste sharp and so on. Right? So they’re similar. So they don’t change the type. That’s where this idea of Type theory came on. You get the same type of molecule, even after you have a substitution.
So by 1853, four types were recognized as prevalent. One was water, another was hydrogen, another was hydrochloric acid, and another was ammonia. So, for example, you could have these structures; and this drawing with a curly bracket like this was the notation used by the people who did Type theory. So you have water, hydrochloric acid, hydrogen and ammonia. And you could exchange, make exchanges, for the hydrogen. Right? Substitution. So, for example with ammonia, you can substitute ethyl for hydrogen and you could get ethylamine, diethylmanine, or triethylamine. But these were all basic. Why would we say they’re basic, in the sense of acid base? Why do we say they’re basic? They react with acids, why? Sherwin?
Student: The unshared pair.
Professor Michael McBride: Yeah, they all have the unshared pair on nitrogen, we would say. But they said they’re just the same Type of molecule. Okay? Or you could have ethyl alcohol, which is of the water type. Or the potassium salt thereof, which they would say is the potassium-ethyl analog of water. Or of the HCl, you could have ethyl iodide, where you exchanged hydrogen with ethyl, and exchanged chloride with iodine. Okay, but in fact these two things could react with one another to give this ether; which is another thing that’s still like water, clear liquid and so on. Okay? Fairly unreactive. So this particular reaction was named for the work, in 1850, of Williamson in England. So it’s called the Williamson Ether Synthesis. And we’ll talk about that again later. But it’s quite an old reaction.
So how about the theory of these types? So notice it’s unitary, not dualistic. They’re just things that are holistic, right? Not plus/minus. Dumas said that molecules are like planetary systems, like the sun and its planets, “held together by a force resembling gravitation, but acting in accord with much more complicated laws.” He didn’t think it was gravity, but it was some force holds this assemblage together. And Williamson, Alexander William Williamson, who we just mentioned making ether, said this is something new. And notice it’s because it’s a very young guy that has a new idea, not like these imagination-starved older people. At this time Dumas was 40-years-old. He’s 4/7ths as old as I am, right? So he was really getting over the hill. “A formula” — the young guy says — “may be used as an actual image of what we rationally suppose to be the arrangement of constituent atoms.” This is entirely new. Formulas, at least since Dalton, were only what the elements were and what ratios they’re in; not how they’re arranged. Right? But he said, “We can think that they’re like an orrery, which is an image of what we conclude to be the arrangement of our planetary system.” Do you know what an orrery is? It’s a thing like this, you know, where you have a mechanical model of the solar system and you turn a crank and the moon goes around the earth, the earth goes around the sun, and a bunch of moons go around Saturn and so on. Have you seen these devices? Okay, that was very popular. There was a show of Joseph Wright of Derby here at Yale last summer.
So butyl bromide, you remember, is a residue of radical dualism, right?; plus-butyl, minus-bromide. But there’s another name for butyl bromide. Do you know what it is? You know the other name for butyl bromide? We haven’t talked about systematic nomenclature yet, so you probably don’t. But it’s also called bromobutane. But bromobutane is not two words, it’s one word. Right? And that’s a relic of the unitary theory, the substitution theory, that it’s butane in which a hydrogen has been replaced by bromine. Okay, so Berzelius, in 1838 when these things came along, said: “By reacting chlorine with ordinary ether [Dumas] produced a very interesting compound which he reckoned, according to the theory of substitutions, to be an ether in which 4 atoms of chlorine replaced 4 atoms of hydrogen.” Right? So Dumas says that in these types you can replace hydrogen by chlorine. What would Berzelius think about that? What kind of theory is he advocating? Remember, we talked last time about Berzelius. He was the originator of dualism, plus/minus. What would he think of replacing hydrogen by chlorine? Lucas?
Student: It’s impossible. If chlorine is minus, hydrogen is plus.
Professor Michael McBride: Right. So here’s what he said: “An element as eminently electronegative as chlorine would never be able to enter into an organic radical. This idea is contrary to the first principles of chemistry.” Okay? And in that same paper, in 1838, he talked about tartrate losing an atom of water — but you mean it’s a molecule — at 190°. But the interesting thing about that, it’s not transformation, but that this is the first time the letter R was used, to talk about a generic radical; “R” stands for radical. Right? So we still use that. So, so much of what we do nowadays derives from this period. Okay? So the principal journal at that time, in chemistry, was the Annalen der Chemie und Pharmacie, which was originally the Annalen der Pharmacie; but Chemie was added. And you see who put it out. It says: “With the collaboration of Dumas in Paris and Graham in London.” And Graham is one of the guys out in front of the building here. Edited by Wöhler and Liebig; but actually it was Liebig, he was the one. And later the journal came to be called Liebig’s Annalen. Right? So he was the one in charge, but he’d added these other people, just sort of for show.
Okay, so in 1840, there were a series of papers published. The first of them was by his so-called collaborator, Dumas, On the Law of Substitution and the Theory of Types. This was a 40-page paper. And it begins with this question, number one there: “Can one substitute the elements that play their role in any simple or compound substance equivalent for equivalent?” So can you make a new atom take the role of an old atom? And you won’t be surprised that in 40 pages he concludes the answer is yes. But immediately following this is a note from the editor, which says “Remarks on the Previous Paper.” And it’s by J.L. at the bottom, Justus Liebig. And he says, begins: “I am a far cry from sharing the ideas that Monsieur Dumas has linked to the so-called laws of the substitution theory.” And then there’s another paper, by another Frenchman, Pelouze, on “The Substitution Law of Monsieur Dumas.” And after that lengthy paper, there’s a letter, “On the Law of Substitution and the Theory of Types,” with a footnote that says it was a letter to Justus Liebig. And you notice it’s dated Paris. And it’s the only paper that’s in French, in his particular issue. And there’s another page. It’s got some curious formulas in them that have a lot of chlorine. We’ll come back to that in just a second. And it’s by a chemist that no one had heard of before called S.C.H. Windler — this letter to Liebig. And then the next paper is also “On the Reaction of Chlorine with the Chlorides of Ethanol and Methanol, and Several Points of the Ether Theory,” by Regnault, who was a French chemist. Now this is that letter, translated.
So it starts — it’s got a complicated description of all the — light that was used sometimes and the various distillations and crystallizations, and the crystals are described. But he started with manganese acetate, which had this formula with the acetyl radical in it, and was able to chlorinate — to substitute the hydrogens with chlorine. So there’s already a validation of the substitution theory. But it went further. A subsequent reaction exchanged the O in manganese oxide with chlorine, and a further reaction replaced the manganese itself with chlorine. And then the final reaction, the pièce de résistance, replaced the carbon with chlorine and the oxygen with chlorine, but still it preserved its type. Right? So it was the same kind of substance still, even though it was entirely chlorine.
And there’s a footnote, which says: “I have learned that there is already in the London shops a cloth of chlorine thread, which is very much sought after and preferred above all others for night caps, underwear, etc.” Now this is, you’ll not be surprised a pun, because the name is pronounced schvindler or swindler. So where do you think this came from? Liebig didn’t have enough sense of humor to do such a thing. Who was the joker?
Professor Michael McBride: Wöhler. So Wöhler had sent this in a letter to Berzelius, and Berzelius thought it was so fun that he forwarded it to Liebig. And to Wöhler’s consternation, Liebig published it. Right? [Laughter] Which didn’t make Dumas any happier. Right? So this was a — Liebig at least thought it was funny, I guess.
Chapter 5. Kolbe and the First Free Methyl Radical [00:47:36]
Okay, so in 1849 Kolbe prepared the free methyl radical, the actual element, which had never been prepared before, CH3. He did it by electrolysis. So when you electrolyze acetic acid it turns out you can get hydrogen, hydrogen gas, and CO2, and what analyzed for CH3. Right? So he had prepared the actual radical. Now, of course, it was discovered ten years later that he hadn’t prepared CH3. It had that analysis, but actually it was C2H6; it was the dimer of CH3. Okay, but at the time it was thought to be justification of the radical theory. So these two theories were competing with one another. And ironically, both the theories were supported by reactions that actually did involve radicals. So the oxygenation of benzaldehyde, the first reaction that generated benzoyl, did in fact involve benzoyl. It was a SOMO reaction in which a hydrogen atom was abstracted. And the chlorination, as we’ve already seen, of a hydrocarbon like methane, involves pulling a hydrogen atom off. And that electrolysis did indeed generate the methyl radicals, but they were so reactive, they found one another and dimerized to C2H6. So it’s just sort of curious that all these reactions did indeed involve free radicals, but no one was truly aware of it. So next time we’ll see what resolved all this.
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