First, an explanation. This happened. So things at MOC have basically been on hold for a few weeks. Life is now returning to normal.
The following discussion has nothing to do with the above, other than the fact that my dad’s best friend wryly observed of him: “When he opened his wallet, moths flew out”. I suppose I share this trait with regard to a lot of things. But I do not scrimp on can openers. This is why.
About 10 years ago when I was living in Montreal I was very poor, and outfitted my kitchen with items available from the dollar store. Including a can opener I paid exactly $1.14 for (in Canada, they hit you hard with sales tax).
After taking this small financial hit, life was somewhat better. I could now eat canned Ravioli. However this state of affairs did not last long. Within the next week my $1.14 can opener had opened (poorly!) about three or four cans before flying apart while trying to pry open an 800 mL can of Bravo spaghetti sauce. So I was back to where I started: with no working can opener.
This time around I decided I wasn’t going to screw around, so I went to the local Canadian Tire and pulled out $6.99 . It was more painful to do this, but the can opener I received was of superior quality. And it did not fail me in the subsequent years that passed (although it did get a tad rusty).
So if we compare these two situations we get this:
Now what does this have to do with chemistry?
Well, it resembles a situation that occurs in the addition of strong acids (like hydrochloric acid, HCl) to certain dienes such as butadiene. Two products are possible: the 1,2-product and the 1,4-product.
- With butadiene, the addition of HCl leads to a resonance-stabilized carbocation. Note that the resonance form on the top bears the positive charge on the more substituted carbon, and will therefore have a higher contribution to the hybrid than the resonance form on the bottom, where the positive charge is borne by a primary carbon.
- In the attack of Cl– to the resonance stabilized carbocation, there are two possible sites of attack. In the transition state for attack at the carbon labelled C-2 [top] note that there is a partial double bond between C-3 and C-4, and that the positive charge is localized on C-2. In the transition state for attack at the carbon labelled C-4 [bottom] note that the partial double bond is between C-2 and C-3 and that positive charge is localized on C-4. The top transition state will be lower in energy because in it, positive charge is localized on the most substituted carbon.
- Now look at the final products. The product of the top transition state [1,2 addition] has a mono substituted alkene (one carbon substituent) while the bottom transition state [1,4 addition] leads to a disubstituted alkene. Since alkene stability increases with the number of carbon substituents, the bottom product will be more thermodynamically stable.
The reaction diagram looks like this.
Each reaction begins with diene A, and then progresses through a transition state (B) to form resonance stabilized carbocation C. , which undergo attack through transition states D to give final products E. The height of each step in the process is related to its overall energy.
- When temperature is low, there is enough energy to form the 1,2-product – and that’s it. The product ratio is determined by the reaction rate (i.e. the height of the transition state D). Such a reaction is said to be under kinetic control.
- When temperature is high, there is enough energy to form both the 1,2- and the 1,4-products. Furthermore, the reaction to form products is reversible (i.e. there is enough energy to go from E → D and thence back to C. In this case the ratio of products is determined by the relative thermodynamic stabilities (i.e. the height of E). Such a reaction is said to be under thermodynanic control.
So it’s a little bit like buying can openers. There’s a lower barrier for buying the cheapest one, but the more expensive one is often the more stable product overall.
As Benjamin Graham said, “Price is what you pay: value is what you get. “
1. The can opener analogy doesn’t go into the “reversibility” part of things. However if you had a large population of people who had to make the identical decision, the population of people with deluxe/crappy can openers should likewise segment according to cost and reliability as a function of available resources. Note that if the product is too stable, nobody ever buys a replacement and the company goes out of business. That’s where planned obsolescence comes in.
2. Not all additions to dienes follow this pattern. It is important to be able to evaluate the relative carbocation stabilities and alkene substitution patterns independently for each given diene. Don’t automatically assume that the “1,4” product is always the most stable (try cyclopentadiene, for instance). For a good time, also try 2,5-dimethyl-2, 4 hexadiene.
3. When you buy an item from the dollar store with moving parts, caveat emptor.