Now we're going to move on to drawing and recognizing functional groups with hydrogen in them. These are going to be alcohols and amines. The first thing we want to focus on is probably the granddaddy of all absorptions and that's alcohol. Alcohols, as we said, are one of the broadest absorptions there is, and they absorb from 32100 all the way to 36100 in their absorption. So this thing is massive. Remember that I told you that an alcohol almost looks like a parabola. That 'OH' is going to look huge. The official name for this type of absorption is that it's strong and broad. That should tell you strong—it's moving all the way down to the floor and broad—it's very, very wide. Now on top of that, because of the fact that I'm always including an alkene component, what other peak should we always be drawing? We should always be drawing our sp3 CH bonds as well because all of these molecules are going to have those. But notice that I have C-C single bonds which I'm excluding. I also have C-O single bond which I'm excluding as well. I don't have to worry about anything else. I'm just going to draw those 2 absorptions. Let's go ahead. I've got my fingerprint. Who cares? Now I move all the way to 29100 and once again, I'm going to draw my sp3. At this point, you guys should be pretty good at drawing these sp3. Go crazy. You know, I expect different shapes coming up at this point. Okay? You got your choppy sp3 peaks. But what's going to happen? Well, when we get to 3200, it gets real. This alcohol is going to be huge. It's going to do something like this. Boom. Okay? Now in this, spectrum, I actually went past 36100 so I probably drew it a little bit too big but it's not a big deal. The whole point is that I just want you to know that it's a huge massive peak that takes up pretty much the entire 3,000 area and that can actually make it kind of challenging because alcohols are so large in terms of their absorption that they tend to block out things that are behind them. Remember that I told you, for example, what's an absorption that you can think of that happens between 3,203,600? Remember our triple bonds, are 33100 alkyne. So imagine that you have an alcohol, but you also have a terminal alkyne that has a sharp peak around 33100. You might barely see it. In fact, what it might look like is you might have an alcohol that looks like this. It's coming down and then it has this sharp little thing and then it keeps going. Because you could almost think of an IR spectrum as a silhouette. It's almost like a shadow of all the peaks. So you can't see multiple layers or multiple dimensions here. If there truly was a sp hybridized CH along with an alcohol, you might only see a little peak like that popping out, just popping right out of the alcohol peak. My whole point here is that alcohols can make reading the 3,000 region a little bit challenging because they take up so much space and there's really nothing we can do about it. One of the limitations of IR spectroscopy.
Now let's move on to amines. What you'll notice is that I've got primary amines and secondary amines and they're going to result differently. Let's start off with primary amines and then move on to secondaries. Then I'll explain why tertiaries are not on this page. The general rule for amines is that you're going to draw as many peaks, same number of absorptions as hydrogens that you have in your amine. So a primary amine has how many hydrogens? 2. That means that we would expect it to have 2 absorptions. In general, these absorptions are going to be weaker and sharper than alcohol. Okay. So if you guys recall, the range of amines was somewhere between like 33030-3500. That means that amines could completely get covered by an alcohol if it was present. Now thankfully, your class is not going to go into that much complexity where you have to figure out what's behind the alcohol. But just letting you know that there's a lot of overlap between these ranges and really the only way that you could tell the difference is by the shape because it's weaker and it's sharper. Now you might be wondering why does it have these 2 different absorptions. I'm just going to tell you quickly this is beyond the scope of the course. You don't necessarily need to know this. But basically, there's 2 types of there's 2 types of vibrations that are going to be happening with your amine. When we talked about how there's stretching, wagging, rocking and all of those are under the umbrella of vibrations, well, when you have those 2 hydrogens present on the amine, you're going to have a type of vibration called symmetrical stretching and you're going to have a type of vibration called asymmetrical stretching. I'll tell you where I'm going with this in a second. Symmetrical looks like this, that both of them are stretching exactly the same. Asymmetrical is where one is stretching in a different direction than the other. Because you have these 2 different vibrations that are kind of vibrating at different frequencies, one is going to be higher than the other. The symmetrical stretch is going to be right around 33100. The asymmetrical stretch is going to be a little higher. It's going to be around 34100. That's why when you have 2 hydrogens present on the amine, we're going to expect double peaks. That's enough for now. Let's go ahead and draw it and then I'll explain why this is important. We're going to go ahead and do nothing, nothing, nothing, nothing. We get to 29100 and we draw our choppy sp3. So much fun. And then we get to around 33100 and this is where we draw our amine peaks. So we're going to get a weak, weaker, sharper peak around 33100 and then a