Concept: Concept: Aromatic hydrocarbon acidity6m
Generally speaking, aromatic molecules are not acidic at all. But the concept of aromaticity can cause certain molecules to become acidic. Let's go ahead and explore how that happens.
As I said, aromatic compounds are not naturally acidic. The pKa of benzene which is your most common aromatic molecule, is if you guys member, 44. Is that a good pKa? Is that a good acid? No. It’s actually one of the worst acids possible. That’s obviously not going to be a great proton donor. But what we do find is that if a hydrocarbon can become aromatic by giving away a proton, basically being an acid, donating a proton. If that makes it become aromatic because it's becoming a conjugate base, then it's going to be uniquely acidic. Our stereotypical example here is cyclopentadiene. Cyclopentadiene is a hydrocarbon. You would expect it to have pKas of 44, something around there. But it's got these two hydrogens up here.
What’s special about these hydrogens? This is right now not a fully conjugated molecule. This is what we would consider non-aromatic because it fails one of Huckel’s Rule criteria. It fails one of the four tests because it's not fully conjugated. But check this out. What if a base were to come along and pull off a proton? What kind of charge would that carbon now get? Make bond, break a bond. I would wind up getting a new compound that looks like this – double bond, double bond, negative charge.
What can you tell me about that molecule? What’s the aromaticity of that molecule? This is aromatic. We learned about the four tests. We learned about Huckel’s Rule. This would be an aromatic molecule. The definition of a good acid is that after donating a proton, it becomes a stable conjugate base. Would you say that this conjugate base is pretty stable? Hell yeah! It's aromatic. Aromatic molecules are awesome at being stable. That’s what they do the best.
It turns out that you guys might have not memorized this. Maybe you've never heard of this before but it's okay. Cyclopentadiene is actually one of the most acidic hydrocarbons there is. These hydrogens at the top have a pKa of 15. Isn’t that a huge difference? That means that cyclopentadiene is even more acidic than water and alcohol. It's a better proton donor than even those because it can become aromatic after it donates that proton. Makes sense so far?
The opposite idea can apply for molecules that become anti-aromatic when donating protons. Let's look at this molecule. If a hydrocarbon becomes anti-aromatic after donating a proton, then it’s uniquely nonacidic. Cycloheptatriene, same thing. We don't expect it to be very acidic. But what if a base were to come along and pull off this proton? What kind of charge would it now receive? It would become negatively charged. I’d have double bond, double bond, double bond, negative charge.
The original molecule was what? Nonaromatic just like my previous example because it’s not fully conjugated. But afterwards, what’s the aromaticity of this molecule? This one is forced to become anti-aromatic which sucks. This is like the worst acid-base reaction ever. It’s saying “Why do they do this?” If you can imagine, the pKa of a normal sp3 hybridized CH bond is the pKa is usually 50. It’s one of the worst acids known to man.
What do you think the pKa of this specific molecule will be? Do you think it will be greater than 50 or less than 50? Because of the fact that this is making an anti-aromatic molecule, not just a normal carbanion. Carbanions already suck but it's not only a carbanion, it’s an anti-aromatic carbanion. You can't get a worse conjugate base than this. This is the conjugate base from hell. Instead of being a pKa of 50, this is going to be a pKa of 60 to 70. It's going to be very, very high. Remember this is on a log scale. This is impossibly difficult to remove that proton because that proton would make it anti-aromatic, removing that proton.
As you can see, aromatic molecules are not great acids or bases but the concept of aromaticity can be what is behind the motivating factor behind some really common acids like cyclopentadiene.
We're going to do some examples. I want you to read through them first. Try to answer them and then I'll go ahead and explain them for you. Start on the first one.
Concept: Example 1: Determining hydrocarbon acitidy2m
What do you guys think about this acid? Would it be especially good would it be especially bad. So in order to answer this question we have to draw the conjugate base we have to see what would it look like after it donates a proton so we can just use the letter B and a negative charge to stand for base after it extracts this proton, what does this molecule look like? The conjugate base now looks like this, so what's the stability of that molecule? Guys this would be antiaromatic right. So the answer here would be that and I mean this is I guess a free response answer so it's going to be essay style, you do not have to write these exact words I'm just kind of paraphrasing this idea which is that this molecule would be unique non acidic due to an antiaromatic conjugate base.
That's it just explaining ourselves how this is not a good acid it's actually going to be a terrible acid, so now here's another one this one requires a little bit more thinking a little more thought will the following two hydrocarbons be expected to have similar acidities explain your reasoning. So go for that one and then I'll answer it.
Concept: Example 2: Comparing hydrocarbon acidity3m
Alright guys, so the only way to solve this is just to draw the conjugate bases of both and see what they look like, so at this point we've done this a few times I'm just going to draw the negative charge because we know that after you donate a proton you get an electron pair. So you would get a negative charge here, that's fair and then notice that on this molecule we actually have two different sites that are not fully conjugated, so it could actually have come the negative charge could be on the top or on the bottom either one you choose is fine but no matter what that's where you would want to draw the negative charge to compare the sights now what I would ask is are the stabilities of these molecule similar at this point, what do you think? The stability of the first one could be categorised as let's say this is molecule A it's what kind of molecule? It's aromatic, and then molecule B is what kind of molecule, what do you think? Is it also aromatic? No guys this can't be aromatic because one of the carbon is still S P 3 hybridized with 2 hydrogen's with 4 bonds 4 signal bonds so this is still going to be nonaromatic.
So even though that negative charge might have helped with huckel's rule we're still missing a fully conjugated ring so this is still nonaromatic. So the answer is no, no right they would not be expected to have similar acidities. No molecule A is more acidic due to having an aromatic conjugate base. I don't have to mention the conjugate base for molecule B because it's assumed that it's not going to be aromatic molecule A is, I will take myself out of the screen more a second. Molecule A is the one that has an aromatic conjugate base, molecule B doesn't have that so it must not be as stable. So anyway guys, I hope that helps to clarify the rule of aromaticity and acidity. So let's move on to the next topic.
For the reaction below, draw the structure of the appropriate compound in the box provided. Indicate stereochemistry where it is pertinent. For Friedel Crafts reactions, assume that the major product is the least sterically hindered one.
Based on arguments of aromaticity, would you expect the following compound to be one of the world's strongest acids or one of the world's strongest bases?
Which one of the following compounds is most acidic?
Which of the following compounds would you expect to be most acidic?
Circle the most acidic hydrogens (or hydrogens) in each molecule below and place them in order of their acidity with #1 being the most acidic and #4 being the least acidic. Work carefully. There will be no partial credit or regrades on this problem.
A student was searching the web for the pKa value of fluorene (see below). He found two contradicting numbers: 2 and 22. Since this is probably a typographical error, he will need to decide which value is correct. Help the student decide. Provide a short explanation and a chemical equation to support it.
Which of the following bases would be strong enough to completely deprotonate compound 1? Lets assume ‘fully deprotonate’ means more than 50% deprotonated.
Which hydrocarbon is least acidic?