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Explain why compound $ extbf{A}$ is much more stable than compound $ extbf{B}$....

Question

Explain why compound $ extbf{A}$ is much more stable than compound $ extbf{B}$.

Explain why compound $\textbf{A}$ is much more stable than compound $\textbf{B}$.



Answers

Explain why compound $\textbf{A}$ is much more stable than compound $\textbf{B}$.

Hillary wanted to redo Chapter 19 problem. 46 minutes for Masses. Explain why the P K of compound is lower than a P K's of both Compound B and C, so let's look at Compound Ace. Remember, lower the peaky and stronger the assets. So obviously, Compound A has the lowest P case. It wasn't a strong is acid and what we know about the acidic strength will and stronger the acid that more stable conjuring base the ways you can stabilize the contract bases of three ways Number one Putting a negative charge Intellectual negative auction. Adam Look on all of them. Do Resident Lee stabilizing the negative charge through the car boxful group, which all of them do a number three inductive stabilization off the negative charge to inductive. Pull a left tendency towards some sort of electoral negative Adam that is, in close proximity to this car box Late group, which all of them also exhibits. So then, what's the difference in acidity? Well, we see that the karmic selic acid in and see our place in the same position they are next to the left. A negative Adam option Major Jin. So why's a more acidic than see Well, it's because oxygen is more election withdrawn and more electoral, electoral negative than nitrogen. Therefore, oxygen will have a greater electron. Withdrawing, inducted, effects and stabilization of his contrary face been in this molecule. See? So that explains why A's more acidic than see. But I would be well, pull them have oxygen's. But now the position of this car looks LaGrassa Group is different. This one and B is one carbon away, while the one in a is directly adjacent to one another. So the difference in the Andes is very simple. It's just because the distance is greater towards this election of drying. Group is goingto have, in a less of an effect inductive destabilizing the contract base than in a so because it has this further away, it's gonna be less efficient in stabilizing the continent base as compared to a

This is the answer to Chapter 10. Problem number 71 Fromthe Smith Organic chemistry textbook. Ah, and this problem gives us these two molecules called A and B. Um, and we're asked to explain why a is a stable compound, but B is not. Ah, and so basically, these two molecules differ only in the placement of the double bond. Uh, and so we should remember that, Um ah, the bond angles around ah, double bond, Uhm ideally are 120 degrees. So it's a tribunal. Plainer geometry, 120 degree bond angles. Um, and the further that we get from that 120 degrees, the less stable, um, Bond and therefore molecule was going to be so when we look at the two carbons that are involved in the double bond here in a, um, there are only only two carbons. Um, and they, uh, are probably, um, the angles of these bonds are close to 120 degrees. So close, close enough to 120 degrees. At least that way is gonna be stable. Ah, but when we look at B, what we see is that, um, b has this double bond so that one of the carbons is at a juncture of both of these rings. And so that is gonna really stress, uh, the geometry here. So, uh, the bond angles at that carbon are gonna be not close to 120 degrees. So not close to 120 degrees. And so that's gonna make it unstable. The ring forces by these molecules or forces these atoms into a certain confirmation on, then the presence of a double bond. There really tries to force the atoms into a different confirmation on. And so those two, I guess you could say forces are opposing one another. You have the ring strain imposed by the junction of the two rings there on. And then you have the strain caused by the fact that the ideal geometry around a double bond is 120 degrees. Ah, and so the the atoms in the double wander going to try to approximate that. Ah. And so the end result is that these two forces make this molecule very, very unstable. Um, and you'll you'll never find, uh, something like this in her life. I don't think, uh and so that's the answer to Chapter 10. Problem number 71

Here. The question is why is most suitable as cover to be? Would our elkins and die substituted at the carbon carbon double booked even then, why gays more stable as cover? Trippy. So first reason is in Gay Double Wound is present. He's in six members, man. It is interesting. He's less s comfort to be because one more reason that carbon carbon Carmen Angry Day mission from Norman Normal that is 100 in 9.5 TD is no so no string easiness and it is formally more stable as comfort of the into some P. The wound is present in four members ring and the angle of division from the Norman that his 109.5 is very less very high in case off full member thing. And that is where the molecule is under constant. And it will be less general s comfort to e

This is the answer to chat there. Three Problem number 55 from the Smith Organic Chemistry textbook. Ah, and in this problem were given molecules A and B. Um, and we're told that a is less water soluble than be I'm and were asked to explain why this is the case. Even though they have the exact same functional groups on drily, there are only different, um, bye. Placement of those functional groups on DSO. The answer is that a in a, uh the alcohol and the oxygen of the Alba hide are so close together that the Alba hide oxygen. One of its lone pairs can intra molecularly hydrogen bond with the hydrogen of the alcohol. And so that hydrogen bond takes place like that. I've drawn it with a green dash line there. And so the end result of this is that, um, so this molecule can still hydrogen bond with water so we can draw some water here. We can put a water here, Um, and we can put a water here on then guess what's put in all of the lone pairs. Okay. And so, um, so this oxygen iss is still gonna hydrogen bond this oxygen has another loan paired, starving hydrogen bond on and then the hydrogen on the alcohol here could probably still, um, weekly hydrogen bond with with a water molecule there. But it's not great because it's it's already hydrogen bond. And then So when we look to be, ah, what we see is that b, um, essentially has has more hydrogen bonding available to it. Um, because it's not hydrogen bonding, interim molecularly with itself. And so that is gonna look like this so we could draw like this again. Put in all the lone pairs on all these oxygen's Okay, Uh, so as you can hopefully see from the way that I've drawn this year, there's going to be a lot more hydrogen bonding opportunities with water molecules and B um, and so enhanced hydrogen bonding is gonna mean enhanced water soluble ity. Um, and so that is why be is more water soluble? Been a because it has more opportunities to hydrogen bond. And that's the answer to Chapter three. Problem number 50


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