How to use Newman projections to determine the most and least stable conformations of a compound.
Want to join the conversation?
- Is this molecule called 2,3-dimethylbutane?(14 votes)
- You´re right. It consists of 4 carbon-atoms, so it is butane. It has 2 methyl (one-carbon) groups, so it´s dimethylbutane. And the two methyl groups are at the second and third carbon, so the final name is:
- Any tips on how to draw the eclipse without the physical models, but with only the drawing. The staggered conformation was explain extremely well. However, the eclipsed conformation has me puzzled when approaching a problem.(5 votes)
- At0:20, when counting the carbons, can't we also count the carbons from the right? And also, At7:15, when we think about the energy, why don't we think about energies between hydrogen and methyl group? Sorry..(2 votes)
- Yes, because the molecule is symmetrical we could count from either end and get identical results.
I agree that this would be clearer if Jay discussed all of the interactions. However, when I rewatched the video on butane he shows (starting at 9 minutes) that the energy for the two methyl groups being gauche is ~3.8 kJ/mol greater than when they are anti.
I've done some searching and Jay's description seems to be widely accepted, so I guess we can interpret this as follows.
His calculations make sense if we set the energy for the staggered H <-> H and H <-> CH₃ interactions to zero and the staggered CH₃ <-> CH₃ (gauche) interaction to 3.8 kJ/mol. We therefore seem to able to ignore all staggered interactions that involve a hydrogen.
I think this was a good question - why are you apologizing?(3 votes)
- Wouldn't we consider gauche interactions for CH3 groups in eclipsed conformations?
After taking them into account, I'm getting incorrect answer.(2 votes)
- A Gauche conformation is a specific type of staggered conformation. If one is looking at an eclipsed conformation, then it's not staggered.
I think, though I'm not sure, that the higher energy (3.8 kJ/mol) of a gauche conformation (as opposed to a regular staggered) is a result of the same forces that cause higher energy (11 kJ/mol) of two eclipsed methyl groups. The gauche's energy cost is lower because the methyl groups are farther apart; if that's the case, then the cost has already been factored into the eclipsed conformation.(2 votes)
- What model set do you use or recommend for use in Organic Chemistry 1 and 2?(1 vote)
- http://www.amazon.com/Molymod-MMS-008-Organic-Chemistry-Molecular/dp/B007FAZOVS/ref=sr_1_1?ie=UTF8&qid=1440612600&sr=8-1&keywords=organic+chemistry+model+kit&pebp=1440612601792&perid=1S2JSHTM2P7SQVJX64Y1(4 votes)
- So which one is te most stable one on those because I think the most stable one is what we are give.........correct me if am wrong....(1 vote)
- Does he mean to write H3C instead of CH3 at time2:33and4:38on the first two NP diagrams but not the third?(1 vote)
- Wouldn't the energy value of a gauche methyl-methyl interaction be .8? Forgive me if I'm wrong, my professor told us this.(1 vote)
- At the beginning of the video (15sec), did you chose the direction you wanted the carbons to start from? Why did you label the back carbon as carbon 1 and not the front one as carbon one? ( the carbon to the farthest left rather than the carbon from the farthest right, in the longest chain)(1 vote)
- [Voiceover] Let's get some practice drawing Newman projections. Our goal is to look down the carbon two carbon three bond for this compound, and in part A our goal is to draw the most stable conformation. So let's number our carbons. This carbon we could say is number one, this carbon is number two. this carbon is number three, and this carbon is number four. If we're going to look down the C2-C3 bond, that's this bond right here. So we're going to put our eye along this axis. If I draw this out right here, we're going to put our eye right here, and we're going to stare down the carbon two carbon three bond, and we're going to draw what we see. Our goal is to find the most stable conformation, and we know from earlier videos that would be a staggered conformation, so we'll draw one staggered conformation, and then we'll draw the rest, and then we'll pick which one is the lowest energy, which one is the most stable. So here's carbon one, and then we have carbon two with a hydrogen coming out at us, and a methyl group going away from us in space. Attached to carbon three, we have a methyl group coming out at us in space and a hydrogen going away from us in space, and then we have carbon four. Our job is to stare down the carbon C2-C3 bond and draw our Newman projections. So if I rotate it so we're staring down that C2-C3 bond, we can see a Newman projection. We can see a staggered conformation for our compound. To get another staggered conformation, I could rotate the front carbon and keep the back carbon stationary, and that gives us another staggered conformation. And I could do it again. I could rotate the front carbon to get another possible staggered conformation. In the video, we stared down our C2-C3 bond so this bond right here. We put our eye here, and we looked at the possible staggered conformations for our compound. It's important to be able to draw the Newman projections without using a model set. So let's go ahead and do that. So if we're staring at carbon two, so this is carbon two right here, and our Newman projection, that's represented by a point, so I draw a point here. And then we'd have a hydrogen going up and to the right. So if your eye is right here, your hydrogen goes up and to the right from this perspective so hydrogen going up and to the right. We have a methyl group going up and to the left, so a CH3 up and to the left. And then, finally, we have another methyl group going straight down, so a CH3 going down. For carbon three, remember carbon three is this one right here, you can't see carbon three if your eye is right here. Carbon two is in the way, but in our Newman projection, we represent that with a circle, so this circle represents carbon three. And what's attached to carbon three? There's a methyl group going straight up. So, again, if your eye is here, this methyl group is up. So we have a CH3 going up. We have another CH3 going down and to the right, so this is going down and to the right, and then we have a hydrogen going down and to the left. So here is our Newman projection for a staggered conformation. Next, we rotated the front carbon and held the back carbon stationary to get another staggered conformation. So let's go ahead and do that. Let's hold the back carbon stationary. We're going to take this methyl group, and we're going to rotate it all the way over to this position. If we do that, then this hydrogen rotates all the way over to this position, and, finally, this methyl group would rotate over to this position. The back carbon's stationary, so let's go ahead and draw the back carbon a circle, and the CH3 is going to stay in the same spot. This CH3 stays in the same spot, and this hydrogen stays in the same spot. So we rotated the front carbon. It doesn't really matter if you rotate the front or the back carbon, but let's go ahead and draw in our groups here on our front carbon. So here's C2, and we moved the methyl group in magenta over to here. So let me go ahead and draw in that methyl group. That methyl group moved over to here. Next, the hydrogen in blue moved down here. So I can draw the hydrogen in blue here on my Newman projection. And then, finally, the methyl group over here in red moved over to this position, so the methyl group in red moved over to here, and now we have another staggered conformation. For our last staggered conformation, we're going to do the same thing. We're going to take the methyl group in magenta, rotate it over to here, and then that would cause the hydrogen right here to rotate over to this position and the methyl group in red to rotate over to this position. So we keep the back carbon stationary, so we draw that in as a circle. Again, we put in our CH3. We put in our CH3. We put in our hydrogen. Those aren't moving, and the methyl group in magenta is now down. So this is the methyl group in magenta. The hydrogen moved over to this position, and, finally, the methyl group in red moved over to this position. So now we have our staggered conformations, and we can double-check ourselves by comparing these Newman projections to what we saw in the video. So here are the staggered conformations. These are stills from the video, and you can see they match the Newman projections that we drew. Finally, we need to choose the most stable out of these three. So what is the most stable conformation? Well, we know that when we have this situation. Let me go ahead and use blue for this. So when we have a methyl group and methyl group here that are 60 degrees apart, this is a gauche interaction. So we have a methyl methyl gauche interaction. And from the video on butane, conformations on butane, we saw that a gauche interaction has 3.8 kilojoules per mole as an energy cost. So we have 3.8 kilojoules per mole for this gauche interaction. And we have another gauche interaction here so another 3.8 kilojoules per mole and another gauche interaction, so there are three gauche interactions for this conformation for a total of 11.4. So the total would be 11.4 kilojoules per mole as an energy cost, so 3.8 times three. What about this conformation? Well, here's a gauche interaction, here's a gauche interaction, and here's a gauche interaction, so, again, we have three gauche interactions. So for this conformation, the total energy cost is also 11.4 kilojoules per mole. What about this conformation, our first one? Well, here's a gauche interaction, so that's 3.8 kilojoules per mole, and here's a gauche interaction. We have only two for this conformation, so only two gauche interactions. That would be a total of 7.6 kilojoules per mole, which is the lowest energy, so this is the most stable conformation. In part B, our goal is to draw the least stable conformation, and we know that the least stable conformation is the one that's the highest in energy. So let's go to the video where I take the model set, and I go from the staggered conformation to an eclipsed conformation, and then we look at all the possible eclipsed conformations. One of them is going to be the least stable. Here we start with our staggered conformation, and if I rotate it a little bit, we get an eclisped conformation. I left it a little bit off, so you could still see the back bonds. I rotate again and get another eclipsed conformation. Now for this one, if I turn to the side, you can see these methyl groups are really close together in space, and so that steric hindrance would destabilize this conformation. So if we go back to the eclipsed conformation, we rotate again, we get to the final eclipsed conformation. Here are the pictures of the eclipsed conformations from the video, and our goal is to pick the least stable, but just for practice, let's try drawing all of them as Newman projections. So we'll start with the one on the left here, and we're staring at C2, so that's C2, which we represent by a point. And then C2 has a methyl group going up, and I drew it a little bit to the right just so we can see what's going on behind it. And then we have a hydrogen going down and to the right, so there's a hydrogen bond to C2 going down to the right. And then over here is another methyl group, so to the left is a CH3. For the back carbon, even though we can't see it, we represent it with a circle so the back carbon right there, which is C3. What's bonded to C3? Let me use a different color and, hopefully, you can see there's a methyl group back here bonded to C3, so let's draw that in in red. And then there's another methyl group over here, so this is a methyl group. I'll draw that one in, a CH3. And then we have a hydrogen down here, so here is the hydrogen. So that would be the Newman projection for this eclipsed conformation. Let's move on to the next picture so this eclipsed conformation. So we're staring at C2, so that's our dot here. And then we can see there's a methyl group going up and to the right so a little bit to the right, so there's a CH3 going that way. There's a CH3 going down so this CH3 going down. And then we have a hydrogen going to the left so hydrogen going to the left here. And then in the back, we have our carbon three, and we held the back carbon stationary in the videos, so there's no change. You can see there is a methyl group straight up here in the back, so CH3, and then there's a methyl group going to the right back here, so a CH3, and then there's a hydrogen going to the left, so this is hydrogen here. So here's the Newman projection for this conformation. And to go from the one on the left to the one on the right, we rotated the front carbon. So let me go ahead and show which carbon is which. So if you took this carbon and, this methyl group, I should say, and rotated it over here, that methyl group in magenta becomes this methyl group. The hydrogen right here in blue gets rotated over to this position, so that's this hydrogen. And then, finally, this methyl group right here in green would get rotated over to this position, so that's this methyl group. For our last eclipsed conformation over here, we're staring at C2, so let's draw that C2 here. We have a hydrogen, hydrogen going up a little bit to the right. We have a methyl group going down, so we draw in that CH3. And then I have a methyl group going in this direction, so a CH3 here. Draw in the back carbon, so there is C3. Again, we didn't change anything, so, again, there's a methyl group going straight up, so CH3, a methyl group going this way, so that one right here, and then a hydrogen going this way, so here's our hydrogen. If we show going from this conformation to this conformation, again, we'll start with the one in magenta, so this one in magenta was moved over to here, so that's this CH3. The hydrogen in blue is rotated over to this position, so that's this hydrogen, and, finally, the methyl group in green was rotated over to here. And so now we have our eclipsed conformations, and let's analyze them and determine which one is the highest in energy. If we start with our first Newman projection, so this one right here, we have a methyl group eclipsing a hydrogen, and we know from earlier videos that's an energy cost of six kilojoules per mole. Here we have another situation with a hydrogen and a methyl group eclipsing each other, so that's six kilojoules per mole. Finally, a methyl group eclipsing a methyl group, which we know is 11 kilojoules per mole, so that's a total of 23 kilojoules per mole, the energy cost for this eclipsed conformation. Let me go ahead and write that here. That's 23 kilojoules per mole. Let's go to the one on the right next because you can see it's the same thing. We have a methyl group eclipsing a hydrogen, so that's six. We have another situation with the hydrogen and the methyl group eclipsing each other, so that's six, and we have a methyl group eclipsing a methyl group, so that's 11, so this one's also 23 kilojoules per mole. If we look at the one in the middle, it's a little bit different,. We have a pair of hydrogens eclipsing each other. We've already seen that's four kilojoules per mole, so that's four here. We have a methyl group eclipsing a methyl, which is 11, and then we have another methyl group eclipsing a methyl, which is another 11. So what is 11 plus 11 plus four? That's a total of 26 kilojoules per mole, so this is the highest in energy. This is the least stable conformation, the one where the methyl groups are the closet together in space because these relatively bulky methyl groups, these destabilized this conformation. So you want to get the bulky groups as far away from each other as you possibly can.