For each pair of compounds below, identify the more acidic compound:
Alright, so let's take a look at the acidity of these molecules and figure out which one is the more acidic one. So let's take a look. Here we've got our benzene, right? With our alcohol coming off and look we've got five methyl groups, right? One, two, three, four, five and the difference between this group-, this molecule over here and this one is that instead of having those metals, right? Those extra carbons, what we've got is chlorine, so we've got five chlorines, and we know that each one of these is going to be pulling electron density away from the benzene, right? So, we know that by effect we're going to be pulling electron density also away from that oxygen, that's holding that hydrogen, okay? So what we know is that, guys, in one molecule we're not really going to have a ton of electron density to hold that hydrogen there, and the other one, we're going to have a little bit more electron density to hold that hydrogen. If we can hold that hydrogen there, we're not going to be as acidic right? If we-, if our hydrogen is more freely taking off, right? We know that's going to be more acidic. So, guys which molecule do you think is going to be more acidic? It's definitely going to be this one over here, because of the inductive effect, right? And you can get some extra resonates from the chlorine but really here what's important is the inductive effect, alright? Let's move on.