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Newman projections

Newman Projections. Created by Sal Khan.

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  • blobby green style avatar for user Nicholas Ignacio Gargiulo
    anyone know if they appear in nature evenly? or is one more evident? is the staggered conformation more common then the eclipsed? or vice-versa? at he mentions the staggered are more stable, i guess this ? also applies to cis/trans, are the trans more common?
    (26 votes)
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  • leafers ultimate style avatar for user Roy Nehoran
    Is it possible to show double and triple bonds in the newman projection?
    (15 votes)
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  • blobby green style avatar for user Arjun Sharma Eldiablo
    i wanna ask one question, is the eclipsed conformation ,staggered conformation is come in the classification of saw horse projection or newman projection??
    (5 votes)
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    • purple pi purple style avatar for user Andrew Widener
      A saw-horse model simply refers to only drawing lines and using letters for the elements in the molecule. A Newman projection is basically a "head on" view of the molecule that uses the same saw-horse drawing scheme (lines and letters). Eclipsed and staggered conformations are two types of ways that a molecule organizes is atoms. These conformations would only be viewable in a Newman projection because from any other viewpoint you would not be able to see if the molecules lay on the same axises.
      (13 votes)
  • leaf green style avatar for user Ganesh Prasad
    why do we learn this?? is there any practical use of these projections?? because itz just the way you view it. i mean how do you particularly predict its projection??
    (4 votes)
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    • female robot amelia style avatar for user jg
      Structure = function. You need to know the shape of each molecule in order to predict its behavior and how it will likely react with other molecules or atoms (eg. nucleophiles).
      (12 votes)
  • marcimus pink style avatar for user lessdenmore
    It is eclisped from -, not staggered right?
    (2 votes)
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  • leaf green style avatar for user Akshay Raman
    Isn't the bond angle of the 2 C-h bonds 109 degrees. Then why does sal say the angle is 60 degrees.
    i think it should be 109/2 degrees..
    (2 votes)
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    • mr pants purple style avatar for user Ryan W
      When you’re considering it from a Newman projection that’s not the case.
      When you look down the C-C bond the 3 hydrogen atoms are at 120 degrees from one another. Remember this is NOT the bond angle, this is the three of them arranged essentially around a circle in a Y or ⅄ shape.

      If a circle has 360 degrees then 360/3 = 120. So in this orientation each H is 120 degrees around a circle.

      Then if you consider how offset the front hydrogens are from the back hydrogens in that specific configuration he mentioned, they are 120/2 = 60 degrees offset.

      Remember this is not the bond angles, it’s a geometry thing.
      This image may help: https://en.wikipedia.org/wiki/Conformational_isomerism#/media/File:Butane_conformations.jpg

      These things can be really hard to explain through text, it’s much easier to show with models.
      (3 votes)
  • blobby green style avatar for user jayantkumarz48
    the eclipse will come to staggered, fine. A slightly staggered will become optimized such that the dihedral angle is 60 degree, fine. But.... If its in eclipse, you need "Torque" to put it into staggered, and two linear forces (in this case the repulsion between the co-linear hydrogens) can only push them away, (or at worst, attract), but if there is no initial staggering, how can you generate torque? you need d (dist b/w point of application of force and rotation point) > 0, but here its not so
    (1 vote)
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    • leafers ultimate style avatar for user seth.sims
      The conformation changes constantly because of thermal motion. The staggered conformation is not locked in only energetically favored. So if you are analyzing groups molecules for conformation you will find mostly staggered. However if you followed the evolution of a particular molecule over time you would see it "cog" between the different staggered conformations. So once it gets enough energy to push it into an eclipsed conformation, it will quickly snap back into one of the two neighboring staggered conformations to minimize the repulsion. So the only way you can ever get them to stay in the perfect alignment required for the repulsion to be axial would be to cool the molecule to absolute zero(0K).

      @jayantkumarz48
      It can hit any conformation naturally. But if the molecule is in eclipsed confirmation and is even slightly above 0k then it will soon wiggle, and fall back to a staggered conformation because the forces are no longer axial. A perfect eclipsed formation is an unstable equilibria like a needle standing on it's point. The slightest disturbance will cause it to tip over, and fall toward the lower energy equlibria of the staggered conformation. But even if it's in a "perfect" staggered confirmation it can get enough energy to wiggle into an eclipsed confirmation. It's just spends less time there for the reasons listed.
      (5 votes)
  • starky ultimate style avatar for user ST
    How do you draw methane by itself?
    (1 vote)
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    • piceratops seed style avatar for user Alex Carrasquillo
      In skeletal form, the methane molecule would just be a dot. The 4 hydrogens are implied because the octet of the carbon atom must be complete. Just as ethane was represented by a single line, which indicated the presence of 2 carbons. The line implied 3 additional hydrogens attached to each carbon. There wouldn't be a Newman Projection for methane as Newman Projections discuss molecules of at least two carbons. There's no need to discuss methane in a Newman Projection because there isn't any strain energy associated with the molecule.
      (2 votes)
  • duskpin sapling style avatar for user christine.chen.94
    Might be a little off topic but how do you draw methane with the line method because there is only 1 carbon? Do you just draw a dot?
    (1 vote)
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  • starky ultimate style avatar for user fDash
    when we talk about molecules rotating about a s bond we know that they do so but how often do they do it?is there a measure for that.? and if it occurs too often than why don't we observe things moving as as everything is ultimately made up of molecules. Just curious!!
    (1 vote)
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    • orange juice squid orange style avatar for user awemond
      At room temperature, most sigma bonds will be rotating many many times per second. Many things can affect this rate of rotation: steric hindrance, lower temperatures, and intermolecular H-bonding, for example, would all slow down sigma bond rotation. Despite the fact that molecules are constantly rotating and vibrating at room temperature, we can't see these movements because they are much too small for our eyes to distinguish.
      (2 votes)

Video transcript

In the video on sp3 hybridized orbitals, we went in pretty good detail about how a methane molecule looks. But just as a bit of a review, it's the tetrahedral shape. You have a carbon in the middle, and then you would have a hydrogen-- you can imagine I'm drawing it like this because this hydrogen is poking out of the page. Then maybe you have another hydrogen that's in the page. You have one above the carbon, and you have one that's behind the page. You could imagine it's like a tripod with a pole sticking out of the top of the tripod. Or if you were to imagine the shape another way, if you were to connect the hydrogens, you would have a four-sided pyramid with a triangle as each of the sides. So it would to look something like this. I'm trying my best to draw-- the pyramid would look something like this if you could see through it. So this would be one side, another side would be over here, and then the backside would be over here, and then the fourth side is actually the side that's transparent out front. So the fourth side would be the actual kind of thing that we're looking through when we look at this pyramid. It would be this front side right over here. So you can imagine it different ways, this was the case with methane. Now let's extend this into a slightly more complex molecule, and that's ethane. So the way we've been drawing it so far-- I guess the simplest way to draw ethane, is just like that. By implication this is ethane. By implication you have a carbon there, and a carbon there, and they'll each have three hydrogens bonded to it. And we've drawn it something like this. Three hydrogens bonded to each of these guys. But now we know that carbon has these sp3 hybridized orbitals, that it likes to form more of a tetrahedral shape when it bonds. So an ethane molecule would actually look more like this. Let me draw the carbons. So I'll do the carbons in orange. So if that's the carbon and that's the carbon. So you can imagine you have a carbon molecule here. I'll draw it as this little circle. And then if we have some perspective, so the carbon-carbon bond is going to look like that. And then you have another carbon molecule right over there. So that's that bond over here. And we want both the carbons, all of their bonds to be kind of in a tetrahedral shape. So then you could imagine this bond over here going like this. This bond going like that. And you have your hydrogen at the end. Let's make the green circles the hydrogens. So you have that hydrogen, and then-- or actually just the circles, we'll call them hydrogen-- and then you can imagine this one, maybe it's coming out of the page a little bit. That is that hydrogen. Let me label the hydrogens, actually. I'm doing it in all different colors so you can see what I'm talking about. And then this hydrogen is going right below it, maybe pointed back a little bit. So that hydrogen is right over there. So you can see this carbon, its bonds have a tetrahedral shape. Or, if you just looked at this part of it, these would be the base of the tripod and this would be the thing sticking up. Now for this carbon it would be very similar idea. This hydrogen right here, might be sticking down like this. And I'll stop switching colors soon enough. It takes a lot of time. That hydrogen over there, it's pointing out in that direction like that. And then you would have, let's see what colors do I have left? Well, I'll just do yellow. That hydrogen right there, maybe it's pointing out like that. So this is a possible configuration for ethane. And the way that I've drawn this right now, and you can actually have a model that has this, where you have little wooden sticks with balls and this, the balls to represent the actual atoms, this is called a ball and stick model. And this is a ball and stick model for ethane. Now a simpler way we could have drawn this, this is called a horse shoe projection-- or actually it's a sawhorse production. I always say horse shoe. A sawhorse projection. It would look like this. This exact same configuration of ethane in a sawhorse projection. And you know what a sawhorse looks like, well, it looks like what I'm about to draw. It looks like this. So you could, well I could draw it exactly the way I drew it here. So you have the carbon, carbon, and then you have the hydrogen, hydrogen, hydrogen, and then you have a-- well, the way I've drawn it up here is more like this. Just so we see the parallel and then we can rotate things around. The way I drew it up here, you have a hydrogen, hydrogen, and hydrogen. And then over here you have a hydrogen, hydrogen, and hydrogen. This is a sawhorse projection. Now, either way you depict it, I mean, these are really the same way. This is kind of just like the lazier way of doing it on some level. You're not drawing all of these circles and all of that, and you're putting a little less care into actually showing the angle, how things are angled away from the carbon and showing the tetrahedral shape. But in either case, when you start visualizing the molecule in this way, you start to realize there's, well, there's actually infinite ways that these things can be configured. And it all comes from the notion that this is just a sigma bond right here. We learned that in the video on sp3 hybridization and sigma and pi bonds. This is just a sigma bond. And so we can rotate around the bonds. One of these carbons could rotate around the axis of that bond without the other carbon having to necessarily rotate with it. If this was a double bond, if this was a pi bond, they would have to rotate together. So you could have a situation like I've drawn here or you could have a situation where they're kind of rotated the inverse of each other. And this is what I mean. So I'll do a ball and stick. So let's say this is our front carbon, that is our back carbon, and we'll compare it to this one over here. So let me draw this guy the exact same way. So he's got a hydrogen down here, he's got a hydrogen up there, and then he's got a hydrogen up here. So that part of the ethane looks identical. Now what I'm going to do is I'm going to flip the other side of the ethane. I want you to pay close attention, because hopefully you'll see the difference between the two. So instead of doing this blue ethane down here-- this blue hydrogen down here-- I'm going to do it on top. So this blue one, I want to do that in blue, this blue hydrogen, put it on top. So I'm just rotating this around. So the blue hydrogen's on top. So I've rotated it so the blue one's on top now. And now the green one is going to go over here. So now the green hydrogen is now over here. And then this purple, or this magenta hydrogen, the way I've rotated it, is now going to go over here. So what's the difference between this configuration and this configuration right here? And we could have had every other configuration in between. But what's the real difference here? Well, here the hydrogen, you could imagine that hydrogen is kind of, if you were looking from that direction, that hydrogen is directly behind that hydrogen, that hydrogen is directly behind that hydrogen, that hydrogen is directly behind that. This is called an eclipsed configuration, or eclipsed conformation. So eclipsed conformation. And this right here, nothing is behind anything. If you went straight back from this guy, you'd get to this point. And no one's behind it. And if you went straight forward from this guy you'll get-- So in no way are any of the guys in the back-- once again, if your viewing from this direction-- are they blocked by any of the people here. So we call this a staggered conformation. Now, why do we even care? OK, I can twist around this back molecule. What's that even going to do for our actual-- why does it even matter? Well, one, it's just interesting that you can actually change, that this thing can twist around without changing the front-- without the front molecule having to twist with it. But even more important, these have different energy levels, so you can kind of think of them as you're kind of twisting a spring and the spring might want to go back to one conformation or another. And to visualize it a little better, I'll draw what's called a Newman Projection. So I'm going to draw this exact thing, but with a Newman Projection, you draw the carbon molecules directly in front or directly behind each other. So in this situation, you would draw the carbon molecule in front, would just be the intersection of these bonds. So for a Newman Projection-- let me draw that out. So it's a Newman Projection and I'll start with the Newman Projection for the staggered conformation. So in the front-- we'll consider this carbon the front carbon-- we have our hydrogen pointing straight down like that. And we have a hydrogen coming out to the top left, like that. And then we have this hydrogen over here coming up to the right. I want to do that in that same color. So the front carbon is implicitly at the intersection of the bonds of these three hydrogens. And then the back carbon-- I said the front carbon is the intersection of the bonds of these three hydrogens-- the back carbon you represented as a circle. So the circle represents the back of carbon. The front carbon is kind of that point there. This is a way of visualizing it. But if we were to draw it this way, the back carbon now has that blue hydrogen popping off of it. So it has that blue hydrogen, this green hydrogen, and then this magenta hydrogen. And when you look at it like this, it is more clear that it's staggered. We're just looking straight on to this ethane molecule. When we look straight on, the front carbon, they're obviously blocking each other. But this way you can see the front carbon's hydrogens are staggered relative to the back ones. So this is right here, once again, this is staggered. Now let's draw the eclipsed conformation as a Newman Projection. So as a Newman Projection the front's going to look the same. You have a hydrogen there, you have this hydrogen, you have that hydrogen, and then you have that blue, or I guess that purple hydrogen, down here. So that's the front of it. But the back, they're right behind it's. So let me draw the back carbon. The front carbon is kind of represented by just that dot. The back carbon we'll represent like that. And the staggered conformation, if this guy's really behind that, you're going to have to draw it like, right there, like right behind it. But since that's a little bit messy, normally when people draw a staggered projection-- an eclipsed conformation, as a Newman Projection. Instead of directly eclipsing that last, that back hydrogen, they'll put it to the right a little, or they'll push it off a little bit. So that's that hydrogen. That magenta hydrogen is right there. It's really right behind the front one, but this is just so you can actually see that it's there. And then finally you have this blue one down there. So that blue one is going to be right over here. So this is the eclipsed conformation as a Newman Projection. And as you can see, it's eclipsed. The back hydrogens are eclipsed by the front ones. If I were to draw it perfectly, they would be right behind it. Now there's one other piece of, I guess one more idea, I want to introduce you to, and that's the notion of the angle between the different hydrogens. So if you wanted to say, well, what is this angle? What is this angle between the blue hydrogen and this pink hydrogen right here? Now, when you actually think of it in three dimensions, it's like, wow, you can't really say the angle over here between blue and the pink. But on a Newman Projection, when you're just saying how much are they rotated away from each other, this angle right here is called a dihedral angle. Sometimes it's just said, you know, this hydrogen relative to that hydrogen has a DA of, in this case, 60 degrees. In this case, this hydrogen relative to that hydrogen has a dihedral angle of zero degrees. And it's a way of saying, how staggered, or how eclipsed, you are. Now, one last thing I touched on the idea, so again, why do we even care? Well, all of these hydrogens have electron clouds around them, and all of these bonds have electron clouds around them. And electron clouds, they're all negative, so they want to get as far away from each other as possible. And they're all stable now, because they've bonded in ways that they have nice stable structures. Everyone feels like they have full valence shells, full orbitals. And so the electron clouds want to get away from each other. Now in this situation, in the eclipsed conformation, this hydrogen and this hydrogen-- let me do it in-- this hydrogen and this hydrogen are closer to each other than when you go to the staggered conformation. The staggered conformation, the closest hydrogen to this guy is going to be either that hydrogen or that hydrogen. But they're both further away than this hydrogen was in the eclipsed conformation. So in general, the staggered conformation is going to be more stable. It's going to have a lower potential energy. You can imagine that if you start with an eclipsed conformation, these guys are all going to want to get away from each other. So it's kind of like this is the wound conformation. It has higher potential energy. So it'll want to unwind and it'll want to unwind to a staggered conformation, because in this conformation, all of the hydrogens have gotten as far away from each other.