The so-called E2 elimination mechanism is another one of those mainstays of organic chemistry. It is important because it introduces the principle that anti-periplanarity of the reacting atoms is favoured over other orientations such as the syn-periplanar form; Barton used this principle to great effect in developing the theory of conformational analysis. Here I explore its origins.
The concerted bimolecular nature of the elimination (E2) is revealed by the intrinsic reaction coordinate (IRC). Notice the peculiar goings on for the spp geometry at IRC = -15, during which the initial gauche conformation of the chloroethane rotates into an eclipsed orientation to allow the synperiplanar transition state to develop. The app isomer has no need to do this.
Time to explain what is going on. This will be done by obtaining a form of localised bond orbital known as the NBO. In fact, a pair of them, one bonding, the other antibonding. The former is known as the donor, and the latter the acceptor. Such a take was used in an earlier post to explain why 1,2-difluoroethane adopts a gauche rather than antiperiplanar conformation. Such localised orbitals are useful to probe specific bonds in a molecule, and why they might be reacting in the way that they do. The theory behind this is shown below. Basically an occupied (donor) orbital can interact (be perturbed by) an empty (acceptor) orbital, the result being a stabilisation energy E2. This energy depends on two specific factors; the energy gap between the donor and acceptor orbitals (the smaller the gap the better) and the overlap between the two orbitals (the larger the overlap the better).
For chloroethane, these two criteria are satisfied by virtue of the C-Cl bond being a good acceptor (due to the electronegative chlorine) whilst the C-H bond is a reasonable donor. The overlap is shown below (click on the image to get a rotatable model). The colour scheme is purple/orange for the two phases of the donor orbital, which derives from the H-C bond, and blue/red for the acceptor orbital, which derives from the C-Cl bond. The colours can be equivalenced; purple=blue, and orange=red, meaning that any overlap between purple and blue or orange and red is positive and stabilising, and the larger this overlap, the larger is E2. At the start of the reaction (IRC=9), E2 = 7.0 cal/mol.As the reaction proceeds, so E2 gets slowly bigger. At IRC +6, E2 has climbed to 11 kcal/mol, by IRC +2.5 it is 31 and at IRC =0 (the transition state) it is 111 kcal/mol. This is induced by the action of the base (Cl–in this case) making the C-H a better donor and the increasing overlap between the donor and acceptor orbitals. At the transition state, the two overlapping orbitals are morphing from C-H and C-Cl* σ-type orbitals into one π-type orbital of the product alkene. At the product I(IRC= -15) the π-π overlap is complete and now corresponds to a fully fledged bond.
The syn-periplanar transition state in contrast shows a smaller value of E2 = 63 kcal/mol at the transition state due to a smaller positive overlap of the donor/acceptor orbitals at this geometry.
To conclude, the relatively small and subtle bond/antibondorbital overlaps that are used in conformational analysis to explain the equilibrium conformations of species such as 1,2-difluoroethane also apply to considering the transition states involving elimination. The overlap of the donor orbital (with two electrons) with an (empty) acceptor orbital directly morphs as the reaction proceeds into a new orbital in the product.