Dienes and MO Theory
s-cis and s-trans
Last updated: October 24th, 2019 |
“s-cis and s-trans conformations of dienes.” What does those terms mean?
As we’ll soon see, in the Diels-Alder reaction, it’s important that the diene be in the “s–cis” conformation, otherwise the two reacting ends are too far apart. The “s–cis” is a conformation where both double bonds are on the same side of a sigma bond. Recall that there is free rotation about sigma bonds, so we say, “s-cis” and “s-trans” to distinguish it from “cis” and “trans” configurations which are locked.
Table of Contents
- Recall That Cis- And Trans– Isomers (“Geometric Isomers” Cannot Interconvert Without Breaking Bonds
- s-cis and s-trans Conformations In Butadiene
- The s-trans Conformation Is Lower In Energy
- Some Dienes Are “Locked” In The s-cis or s-trans Orientation
- Conformations In Amides: (Z) and (E)
1. Recall That Cis- And Trans– Isomers (“Geometric Isomers” Cannot Interconvert Without Breaking Bonds
Recall cis and trans. The reason Aldrich Chemical Co. can sell 99% cis-2-butene and 99% trans-2-butene in separate bottles is because of restricted rotation about the C-C pi bond. Rotation is energetically disfavored since it would destroy the overlap of the adjacent p-orbitals.
We use the terms “cis” and “trans” to distinguish the different configurations of hydrogens across the C-C pi bond.
In contrast to pi bonds, rotation about single (sigma) bonds happens all the time – thousands of times per second, in fact.
You might recall that we refer to the different shapes of a molecule that arise through these rotations, “conformations“.
For reasons that will soon become clear, it’s sometimes helpful to borrow the “cis” and “trans” terminology for naming particularly important conformations.
A particularly important case comes up with dienes. In butadiene, the two individual pi bonds may be either on the opposite side of the single bond or on the same side of the single bond. It would be incorrect to refer to these as strictly trans and cis since these are conformations (dynamic!), not configurations (static). But we can get the best of both worlds if we cheat a bit and use the prefix “s” (for “sigma” , or “single” if you prefer).
Voila: s-cis and s-trans conformations!
A video says a thousand words. Pay attention to the two blue hydrogens of the diene below (butadiene) and their orientation about the central C-C single (“sigma”) bond. In one conformation, they’re oriented “trans” across the C-C single bond, and in the other conformation, they’re oriented “cis” across the C-C single bond.
That’s really all there is to it.
But while we’re on the topic of s-cis and s-trans for dienes, let’s look at a few more details.
Which conformation is lower energy?
Note that in the s-cis conformation, the “inside” hydrogens on C-1 and C-4 are in close proximity to each other. This leads to some Van Der Waals repulsion, and the result is that the s-cis conformation is about 2.3 kcal/mol less stable. At any one time, about 96% of butadiene is in the s-trans conformation.
There are situations where dienes are locked in a particular orientation. For example, in 1,3-cyclohexadiene and cyclopentadiene, the two pi bonds are locked in a s-cis orientation, while the diene bottom right is locked in the s-trans orientation.
This will become more relevant in the next post, when we introduce the Diels Alder reaction.
One final note. It’s also useful to borrow the terms for amides, which have free (if somewhat restricted) rotation about the C-N bond.
Here, we can refer to s-E or s-Z conformations of the amide (see below).
That’s really it for this topic. Did I forget anything? Feel free to leave a comment!