00:01
We have two sets of compounds, that we have to rate in order of acidity, from least acidic to most acidic.
00:08
And each sec shares similarities between the compounds, which makes comparison fairly straightforward.
00:15
So this first set, we have this carboxylic acid here.
00:19
That's going to be our acidic group, and specifically this proton here would be the label proton, or the one that, or the acidic proton.
00:34
So this is a proton that would be lost.
00:37
So we're considering these protons as the losing protons.
00:42
And so if we're looking at these structures, they're all very similar, with the exception of a chlorine added to these two, and nothing but hydrogens on this one.
00:52
And so what are chlorines? well, chlorines are electron with a drawing group.
01:04
And so they pull electrons to, them.
01:13
So they're not strong as like fluorine is in this job rule, but basically they draw electrons to go towards them.
01:20
Electrons want to go towards chlorine here.
01:23
And so if we're looking at the deprotent state of these molecules, we have in the basic form after we lost that proton a negative charge, which means extra electrons.
01:41
So the ability of let me make some more space here.
01:51
The stability of this has to deal with the ability of these electrons to be shared throughout the molecule.
01:58
And so corpuxulc acid by itself is pretty good at this and that's why we call it acid, because it shares those electrons up and through this oxygen chain.
02:10
You end up creating a resonance structure here where this double molecule can go back and forth, and that distributes the electrons between.
02:17
Between these two oxygens.
02:21
The electrons don't really want to go down the carbon chain very much because you have these two options here they're fairly electronegative.
02:28
They're whole electrons pretty tight.
02:31
But when we start adding chlorine here, well, we can share that electrons between the two oxygens, but we can now start sharing them with that chlorine.
02:42
We can pass the burden of those electrons off to the chlorine.
02:46
So the reason why this is so powerful, being able to share electrons is monocles tend to like to tend to like to be neutral and so if you reduce the high concentration electrons throughout the entire molecule it's going to behave more neutral like and it's going to be more stable so the ability to share these electrons um so spread electron or negative as another way to look at it um burden increases molecule stability.
03:31
The takeaway that is more likely to form.
03:36
The more stable a molecule is, the more likely it is to form.
03:40
And so the acidity of these molecules is directly tied to the stability and then charged negative state.
03:48
And so taking away from then, the molecule of the chlorine closes towards that negative charge in the base state is going to be the most stable.
03:57
And so this has the chlorine closest, so this will be the most stable.
04:06
This has a chlorine on the molecule, although it's pretty far away, this will be second stable, and this will, without any chlorine, will be the least stable.
04:17
Electron density is entirely localized.
04:20
On this end here, electron density is spread throughout this molecule here, and it's spread throughout this molecule too, but to lesser extent, because the chlorine doesn't have as much pull on those electron density, so it's going to spend less time on the chlorine than it would over here...