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## Conformations of alkanes

Current time:0:00Total duration:6:24

# Conformational analysis of ethane

## Video transcript

- [Voiceover] Here we have
the eclipsed conformation of ethane, and if I turn it so we sight down the carbon carbon bond, we'll see the Newman projection for the eclipsed conformation. Notice I have some
hydrogens in green here, and that's just to help
us visualize rotation around the carbon carbon bond. So I'm going to rotate the front carbon and keep the back carbon stationary. So now we get the staggered
conformation of ethane. I'm gonna keep rotating 60 degrees. So I'm gonna rotate again, and now we have an eclipsed conformation. I rotate again, and
now we have a staggered conformation of ethane. I rotate another 60 degrees, and we get an eclipsed conformation. I rotate again, and we get a staggered, and you get the idea. One more rotation, and we get back to an eclipsed conformation. Here we have a graph of
the potential energies of the conformations that
we just saw in the video. So we started out right here with this eclipsed conformation of ethane, so we are at this
particular potential energy. As we rotate to get to this
staggered conformation, you can see there's a
decrease in potential energy. So this staggered conformation has a lower potential energy than the
eclipsed conformation. We rotate again, we get back up here to this eclipsed conformation. Notice that takes energy. So it takes energy to
go from this staggered conformation to this
eclipsed conformation. Going from the eclipsed to the staggered, that's a decrease in energy. Going from staggered up to this eclipsed, that's an increase in energy. Going from the eclipsed
down to the staggered again is a decrease, and finally, back to the original eclipsed conformation would be an increase in energy. Notice that all of our
eclipsed conformations here have the same potential energy. If I draw a line, this is all
the same potential energy. Whoops, I didn't draw
a very nice line there, but you get the idea. Therefore, we say that
these are degenerate in terms of energy. Same thing for the
staggered conformations. All of these staggered conformations, if I draw a line in here, have the same potential energy. So the staggered conformations are lower in energy than
the eclipsed conformations. Actually, the difference
is 12 kilojoules per mole. So if I write that in here, so 12 kilojoules per mole, that's talking about
the difference in energy between the eclipsed conformations and the staggered conformations. Lower in energy means more stable. The easy way of thinking about that is imagine these things as hills, if I have a boulder,
or a rock, or something down here at the bottom of the hill and I'm comparing that boulder or rock up here to a boulder
at the top of the hill. In physics, you can set
your potential energy equal to zero at the ground. So let's say that this is ground level. I say my potential energy, U, is equal to zero joules at this point. And so the boulder in this valley here, let's say it's 10 joules. Let's say this is 10
joules here at this point. And then it would take
energy to push this boulder up this hill to this point. Let's say the final potential energy of the boulder at this
point would be 22 joules. It takes energy in order to do that. This final position is less stable, and this is the higher potential energy. So higher in potential
energy means less stable. Lower in potential
energy means more stable. So why do we have a difference in energy between the staggered and
the eclipsed conformation? Well this is called torsional strain. So this difference in energy, this 12 kilojoules per mole, is called torsional strain. The source of torsional strain has been a topic of debate. One of the current theories has to do with molecular orbital theory. I'm gonna go with one of the older ones, which talks about the
electron pair repulsions. The electron pair repulsions are greatest when the bonds are eclipsed. So if you think about the electrons in this bond being close to the electrons in this bond, and you have that same thing over here and over here, so in space, these electron pairs, these bonding electron
pairs are closer together in the eclipsed conformation than they are in the staggered. If I go down here to the staggered, you can see if you're thinking
about these electron pairs they're relatively
further away than they are in the eclipsed conformation. We know that electrons will repel. So electron pair repulsions are greatest when the bonds are eclipsed, and therefore, that's higher energy and the electron pairs are further away from each other when you're
talking about staggered, therefore, more stable. The total energy cost
between the two conformations is 12 kilojoules per mole. We have three pairs of eclipsed hydrogens. If I go back up to here, here's one pair of eclipsed hydrogens, here's another pair, and here's another pair. So if the total energy is
12 kilojoules per mole, and I have three pairs
of eclipsed hydrogens, we could say that the energy cost for each pair of eclipsed hydrogens is four kilojoules per mole. So this would be four kilojoules per mole for this pair of eclipsed hydrogens, four kilojoules per mole for this one, and four kilojoules per mole for this one, adding up for a total of 12. So our total energy cost is 12, and now we can think about two hydrogens eclipsing each other as
having an energy cost of four kilojoules per mole. We've just seen that the
staggered conformation of ethane is more stable than the eclipsed conformation of ethane. If you want turn a staggered conformation into an eclipsed conformation, you would need energy. At room temperature, there's enough energy for the staggered conformation to turn into the eclipsed. Equilibrium is reached
between the two conformations, and at room temperature, approximately 99% of ethane molecules have an approximately staggered conformation, whereas only about 1% have an eclipsed conformation. Again, that's due to stability. Staggered is more stable than eclipsed.