- Alcohols and phenols questions
- Alcohol nomenclature
- Properties of alcohols
- Biological oxidation of alcohols
- Oxidation of alcohols
- Oxidation of alcohols (examples)
- Protection of alcohols
- Preparation of mesylates and tosylates
- SN1 and SN2 reactions of alcohols
- Biological redox reactions of alcohols and phenols
- Aromatic stability of benzene
- Aromatic heterocycles
Created by Jay.
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- How is Phenol oxidation leading to benzoquinone? where is the extra carbonyl functional group coming from?(5 votes)
- I conducted a quick literature review and discovered that phenol can indeed be oxidized to benzoquinone, although this reaction requires the use of a structural catalyst in some cases. The additional oxygen is sourced from the oxidizing reagent, which was lead(II) oxide (PbO2) in one particular experiment that I read about. :)(4 votes)
- Shouldn't it take 2 NADHs to reduce the ubiquinone since we're reducing two ketones?(4 votes)
- I want to say that's why he specified NADH and H+ at the beginning of that reaction mechanism. The two H's present will reduce the two ketones.(0 votes)
- Why does the H attached to carbon not kick of its electrons to carbon while carbon gets oxidized at2:52?(2 votes)
- Because then carbon would have 5 pairs of electrons around it and that makes carbon molecules super unhappy. If the hydrogen's electrons didn't leave, then the oxygen atom wouldn't form the double bond and would just hold onto those electrons and take the negative charge before the carbon would take the negative charge (remember, oxygen is more electronegative than carbon is).(2 votes)
In this video, we're going to look at the biological redox reactions of alcohols and phenols. Over here on the left, we have the ethanol molecules. This is a two-carbon alcohol. The carbon that we're most concerned with is this carbon right here, which has one bond to this oxygen atom. And in the liver, ethanol is oxidized to ethanal. So over here on the right is the ethanal molecule, a two-carbon aldehyde. And once again, we're concerned with that carbon in yellow. And so one easy way to tell that ethanol was oxidized to ethanal is to see that on the left, we have one bond of that carbon to oxygen and over here on the right, we now have two bonds of that carbon to oxygen. So an increase in the number of bonds to oxygen is oxidation. You could also assign oxidation states to this carbon, and you will see that there's an increase in the oxidation state of that carbon. And then you could also think about electrons. So LEO the lion goes GER. Loss of electrons is oxidation; gain of electrons is reduction. And so if I think about these electrons here in magenta, you can see that those electrons are lost from the ethanol molecule. So loss of electrons is oxidation, ethanol is oxidized. If ethanol is oxidized, something else must be reduced. That's how redox reactions work. And what's reduced is NAD plus, over here on the left. So this is NAD plus, which stands for nicotinamide adenine dinucleotide. The adenine is hiding in this R portion. And we have a nitrogenous-based ring with an amide functional group over here on the right for the nicotinamide portion of the molecule. Plus 1 formal charge on this nitrogen gives us NAD plus. So this is nicotinamide adenine dinucleotide, NAD plus, and since ethanol is oxidized, NAD plus must be reduced. So reduction means gaining of electrons. And so NAD plus is going to gain those electrons in magenta from ethanol. So if we think about a possible mechanism, if I took these electrons between the oxygen and the hydrogen and move them in here, that would form our double bond between the carbon and the oxygen. But there'd be too many bonds to this carbon right here, so the electrons in magenta are going to move to this carbon down here on NAD plus, to this carbon. That would push these electrons over here, and that would push these electrons here off onto the nitrogen. So if we showed what happened with the movement of all of those electrons right over here on the right, this carbon right here at the top already had a hydrogen bonded to it, and it gained another hydrogen with two electrons. The two electrons were the ones in magenta right here. So this hydrogen right here is this hydrogen, and the electrons in magenta move over there to our ring. And then we would also have pi electrons moved over here. And then we had a lone pair of electrons move off onto the nitrogen, like that. And then we still had some pi electrons over here on the right. And so this molecule is called NADH. So it's gained the equivalent of a hydride, a hydrogen with two electrons. And so we can see that NAD plus gains two electrons, and gaining electrons is reduction. So NAD plus is reduced to NADH. Since NAD plus is reduced, it allows ethanol to be oxidized. And so we would refer to NAD plus as an oxidizing agent. It is the oxidizing agent for ethanol, even though it itself is being reduced. So that's something that confuses some general chemistry students sometimes. All right. So now, over here, we have the NADH molecule. And this reaction is catalyzed by an enzyme. And the enzyme is alcohol dehydrogenase. So this is catalyzed by the alcohol dehydrogenase enzyme, like that. And this reaction is reversible. So if we think about the reverse reaction, we think about ethanal being reduced to ethanol. And so if ethanal is reduced to ethanol, NADH would be oxidized to NAD plus. And so let's think about a mechanism where we could oxidize NADH and reduce the ethanal. If I took this lone pair of electrons in the nitrogen and move it back in here, that would push these electrons off over here. And now the electrons in magenta on this bond right here would attack this carbon right here. So the electrons in magenta, we could think about the electrons in magenta as being right here. And you could think about that as being a hydride. So a hydrogen with two electrons, giving it a negative 1 a formal charge. And even though we've seen in some earlier videos that hydride isn't necessarily the best nucleophile, you could think about this as being a nucleophilic attack if it makes it easier for you. Because this carbon right up here would be partially positive. So the negatively-charged electrons would attack that carbon. And in doing so, that would push these pi electrons off to then grab this proton here. And that would give you your ethanol molecule. And that would convert NADH back into NAD plus. So you could think about NADH as being oxidized. It is losing two electrons, the electrons in magenta. Loss of electrons is oxidation. And since NADH is the agent for the reduction of ethanal to ethanol, you would say that NADH would be the reducing agent for this example. And the best way to remember that NADH is the reducing agent is it is the one that has the hydrogen on it. So it has the hydride which is capable of being the agent for the reduction. So therefore, NADH is the reducing agent. This NAD plus NADH conversion, and vice versa, is extremely important in biochemistry. This happens in numerous biochemical reactions. And so it's important to understand what's happening with those electrons on these molecules. Let's look at another biochemical example of redox. And here we have on the left phenol. So this is our phenol molecule. And once again, we're most concerned about this carbon, the one that's attached to this oxygen. And there are many ways to oxidize phenols. So if we oxidize phenol like-- so like the Jones reagent was sodium dichromate, sulfuric acid, and water, would be capable of oxidizing phenol to this molecule over here on the right, which we call benzoquinone. This right here is a benzoquinone molecule. And just real fast, you can see that this carbon right now has two bonds of carbon to oxygen, so it has been oxidized. So phenol can be oxidized to benzoquinone using numerous organic reagents. Once you make benzoquinone, you could reduce that to this molecule over here on the right, which is called hydroquinone. So there are several, again, organic reagents that can reduce benzoquinone to hydroquinone. Hydroquinone, let me change that spelling there. And then from hydroquinone, you could oxidize hydroquinone back to benzoquinone pretty easily. And so once again, in organic chemistry, there are lots of reagents that can do these redox conversions. And in the body, you're usually talking about the NAD plus NADH system. So we've just studied that. And if we look here at this molecule, you can see it's a quinone. So you can see the benzoquinone portion of this molecule. And this is called ubiquinone. Ubi referring to the fact that this is ubiquitous. This compound is found in everywhere. It's found in all the cells in nature. And the other name for this would be coenzyme Q. And so this is a very important part of the electron transport chain. And if we look at ubiquinone, going to this molecule over here on the right, you can see this is like a hydroquinone analog here. So this is ubiquinol. So these carbons are being reduced from this chemical reaction that I've drawn here. So ubiquinone is being reduced to ubiquinol. And so if ubiquinone is being reduced, something else must be oxidized. And so the NADH is being oxidized to NAD plus. And so the NADH, it's the one that has this hydride on here, which can serve as the reducing agent. So here, NADH is acting as the reducing agent, the agent for the reduction of ubiquinone to the ubiquinol molecule over here on the right. And so this is just an oversimplification of part of the electron transport chain, where you're transporting electrons, which eventually leads to oxidative phosphorylation and also ATP synthesis. Which of course, gives us energy. And so this isn't meant to be an exhaustive detail of those biochemical processes, but it's just to show you how you can analyze biochemistry using a simple knowledge of organic chemistry, and the importance of NAD plus and NADH in biological systems.