Are strong Bronsted acids necessarily strong Lewis acids?

Abstract

The Broensted and Lowry acid base theory is based on the capacity of proton donation or acceptance (in the presence or absence of a solvent) whereas the Lewis acid base theory is based on the propensity of electron pair acceptance or donation. We explore through DFT calculation the obvious question whether these two theories are in conformity with each other. We use pK_a as the descriptor for the Broensted and Lowry acidity. The DFT descriptors like ionization potential, electron affinity, electronegativity, hardness and global electrophilicity are computed for 58 organic and inorganic acids. The fractional electron transfer, Δ(N) and the associated energy change, Δ(E) for the reaction of these acids with trimethyl amine (a strong base) are used as the possible descriptors for the Lewis acidity. A near exponential decrease in Δ(N) and (-Δ(E)) values is observed in general with an increase in pK_a values. The findings reveal that a stronger Broensted acid in most cases behaves as a stronger Lewis acid as well. However it is not necessarily true for all acids.