Stereochemistry and Chirality
Chiral Allenes And Chiral Axes
Last updated: May 30th, 2019 |
All About Allenes, Chiral and Otherwise
This post is all about the structure of allenes, and how certain allenes can be chiral due to the presence of what we call an “axis of chirality”.
Table of Contents
- Allenes are “Cumulated” Dienes
- The Central Carbon In Allene Is sp Hybridized
- A 3-D “Fly-By” Of Allene Shows It Is Not Flat
- Examples of Substituted Allenes With Mirror Planes
- An Example of A Chiral, Di-Substituted Allene
- Chiral Allenes Have an “Axis of Chirality”
- Summary: How Do I Recognize A Chiral Allene vs. An Achiral Allene?
We’ve met alkenes before – right? Just in case you haven’t, let’s review the basics, because today’s post is going to depend on understanding a few of the most important concepts.
Alkenes contain both sigma [ σ] bonding formed through “head-on” orbital overlap [i.e. “single bonds”] and also pi [ π ] bonding where orbitals have “side-on” overlap [i.e. “multiple bonds”]
Alkenes like ethylene are flat [planar]. The p orbitals are at 90 degrees to this planar structure. If you’ve ever used graphite lubricant, you might know it’s slippery because graphite is made up of layered sheets of flat, pi-bonded carbon, and the sheets have very little friction between each layer. Graphene is the same idea, only it’s a single layer.
Now let’s draw something weird. What do we get when we extend a second double bond directly adjacent to the first one?
Does this look strange to you? The first time you see this, you’ll probably think – yes! You might wonder – do these even exist? The answer is also – Yes! This moleule is called allene, and is part of a family of molecules called cumulenes, so named because the double bonds are cumulative (consecutive).
Now let’s ask: what might the bonding in this molecule look like? In other words, what does it look like in 3D?
You might think – simple! It’s flat, like an alkene!
It’s actually not quite that simple! The key is that central carbon – it has TWO π bonds.
You might recall that acetylene has two π bonds as well, at 90 degrees to each other.
The same is true for allene, except that it’s only the central carbon that is involved in two pi bonds.
Here’s what the orbitals of this molecule look like.
The hybridization of that central carbon? It’s sp, just like the carbons in acetylene. The end carbons are sp2
The line diagram of allene really does not do it justice.
So here I present a 3D “fly-by” of allene. Note how the two CH2 groups are “offset” with respect to each other by 90 degrees.
Allene is not flat! [those white balls – imagine they are hydrogen]
Like so many things in organic chemistry, this simple fact leads to consequences that aren’t immediately apparent. Let’s pay attention to the mirror planes in this molecule. Note that there are two. Recall that in order for a molecule to be chiral it must not be superimposable on its mirror image. If the molecule has a mirror plane (plane of symmetry) then it will be superimposable on its mirror image [and therefore achiral].
With two mirror planes this is definitely an achiral molecule.
Now let’s start playing around a bit. What happens if we replace one of the hydrogens by another group? In the drawing I’ve arbitrarily made this atom Cl but in practice it can be anything except H in this case.
Here’s a line drawing of the molecule and a picture of its orbitals.
Now here’s what it looks like in 3D. Notice that we’ve lost one of the mirror planes! But it still has one, so it’s still achiral.
Now: what happens if we add a second group to the same carbon?
It’s still achiral! – in fact, we’ve gone back to having two mirror planes.
Now, finally, let’s change the position of that second group. Instead of making it so that there are two identical groups on the carbon, let’s change it so that there’s one on each carbon. Like this:
Here’s the 3D version.
Now I ask: where are the mirror planes?
THERE ARE NONE! If there are no mirror planes —> then we are looking at a chiral molecule.
Wait. You might ask -what trickery is this? We have no chiral centres. Don’t we need something to have a chiral centre to be chiral?
Actually you are very familiar with a chiral object that has no chiral centre.
Have you ever screwed before?
No, no, no! I mean, screwed using a screwdriver. This is a chemistry blog. Don’t expect anything lascivious here.
See, most screw threads are, to use a familiar mnemonic, “righty tighty, lefty loosey.” You have to turn the screwdriver clockwise to screw it in, and counterclockwise to loosen. Screws are chiral!
[By the way the enantiomer of that common screw thread would be… “lefty tighty, righty loosey” – those types of threads exist BTW – especially in gas barbecues, so as to prevent people from trying to connect things to them such as garden hoses or other idiotic things].
Here’s a representative picture of two chiral screws. You can also imagine these as spiral staircases. Imagine walking up each staircase. On the staircase labelled “left- hand” below, your right arm would be on the inside as you ascend. On the “right-hand” staircase, your left arm would be on the inside as you ascend. [see nerdy note below]
Instead of having a chiral centre, screws have what we refer to as a “chiral axis“. Other common examples of things with chiral axes: spiral staircases, snail shells and DNA.
Our disubstituted allene has a chiral axis – just like a screw.
Screws are chiral – and chiral objects have enantiomers. And just as screws have enantiomers, so do chiral molecules with a chiral axis.
What would the enantiomer of the allene look like?
Here is an enantiomeric pair of allenes. Can you see now how they are not superimposable?
[In other words, an allene with a chiral axis vs. an allene without a chiral axis]
You might ask, is there some kind of short cut for recognizing a chiral allene? Sure.
Examine both “ends” of the allene. If either of those ends is attached to two identical substituents, it is achiral – because it will have a mirror plane.
If neither of the ends are attached to two identical substituents, then it is chiral.
Bonus question: Would you expect this molecule to be chiral? Why or why not?
Nerdy note about staircases, possibly a myth. This may or may not be true, but I recall reading a book in my childhood about castles where it was said that castles were built with staircases that forced someone ascending them [an attacker, presumably] to have their right (sword) hand on the inside and a descending defender to have their sword hand on the outside. The idea being that there is much more freedom of motion if your sword hand is on the outside because you have to swing it across your body.