In this video, I'm going to introduce all of the different reactions that can occur to benzene through an EAS mechanism. As previously discussed, benzene is going to require very strong electrophiles in order to react through EAS. Some of these reagents are going to require catalysts in order to become strong enough for the benzene to react with them. Let's just take the first one into account, EAS halogenation. Halogenation would be a reaction with a double bond and a diatomic halogen, so something like X2. But actually X2 is not a reactive enough electrophile to react with a benzene. Guess what? If you just put X2 in a mixture of benzene, you're not going anywhere. You're not going to make a substituted benzene. How do we get the X2 to react? We need a catalyst, guys. This is going to be a Lewis acid catalyst, FeX3. This is going to work for bromine. I'm going to put here where X is equal to specifically bromine or chlorine. You always want to make sure that when you're performing one of these EAS halogenations, that you're using the same halogen in your catalyst as you are in the actual electrophile. That's going to become important later when we look into the mechanism. As you can see, the product is now going to be a monohalogenated benzene, which is great. That's what we wanted. Now, it's important to distinguish this mechanism from another reaction we learned in the past just called halogenation. It's important that when you discuss this mechanism, you call it EAS halogenation, because specifically, this is the one that requires a Lewis acid catalyst.
Let's move on to the next one. It turns out that iodination is a little bit tricky. Iodine does not react with the Lewis acid catalyst of iron and 3 halogens to perform this EAS reaction. We're going to have to use nitric acid instead, HNO3. That's one little peculiar thing that you have to memorize that iodination, in order to put an iodine on a benzene, we're going to need to use nitric acid, not our iron Lewis acid catalyst.
Let's move on. The next one we want to discuss is nitration. A nitro group is not a group that we've discussed a whole lot at this point of the course. I do want to just help you guys understand what a nitro group is by drawing it. It would be something like this. We have a nitrogen with a double bond O and a single bond O, and there's going to be formal charges. The single-bonded O has a negative charge. The nitrogen since it has four bonds has a positive. But notice that this has no net charge because they cancel out. That's why when you draw NO2, you draw it neutral without charges even though those charges do exist. Now there are two different ways to add a nitro group to a benzene. But they're really the same thing. It's just that different websites, different textbooks like to use different combinations. The most common would be using nitric acid, HNO3 and sulfuric acid. A combination of sulfuric acid and nitric acid is going to react together to make the active electrophile, as we will see later when we go into the mechanism. But just keep in mind that you could also generate this electrophile just through using concentrated HNO3. In the first example, you have one acid reacting with another. When you use concentrated HNO3, it just reacts by itself. One HNO3 molecule reacts with another one and makes that active electrophile. Regardless of how you draw it, it's really going to produce the same product. That would be EAS Nitration. Also, one thing to keep in mind is that nitric acid can also be written differently. It can be written as HONO2. This is just a little technicality that actually could make you guys stumble on an exam because the same compound as nitric acid, HNO3, is just written differently. It's basically written on the connectivity in a condensed structure instead of just based on the molecular formula.
Let's go on to sulfonation, which is actually going to be the kind of the most special reaction we're going to talk about on this page because sulfonation is the only one with these two arrows. Let's discuss what that is. First of all, the product of sulfonation is it's going to make what we call a sulfonic acid group. That's what we have at the top. By the way, I forgot to write what the product of nitration would be. It would be a nitro group. You got nitro, and we've got sulfonic acid. These are literally functional groups that we just learned in this course. Sulfonic acid. The way that we do a sulfonation is to use sulfuric acid, so H2SO4 and O3, sulfur trioxide. It turns out that when you heat up H2