Equilibrium constants
for the associations of 17 diaryliodonium
salts Ar2I+X– with 11 different
Lewis bases (halide ions, carboxylates, p-nitrophenolate,
amines, and tris(p-anisyl)phosphine) have been investigated
by titrations followed by photometric or conductometric methods as
well as by isothermal titration calorimetry (ITC) in acetonitrile
at 20 °C. The resulting set of equilibrium constants K
I covers 6 orders of magnitude and can be expressed
by the linear free-energy relationship lg K
I = s
I LAI + LBI, which characterizes iodonium ions by the Lewis acidity parameter
LAI, as well as the iodonium-specific affinities of Lewis
bases by the Lewis basicity parameter LBI and the susceptibility s
I. Least squares minimization with the definition
LAI = 0 for Ph2I+ and s
I = 1.00 for the benzoate ion provides Lewis acidities
LAI for 17 iodonium ions and Lewis basicities LBI and s
I for 10 Lewis bases. The lack
of a general correlation between the Lewis basicities LBI (with respect to Ar2I+) and LB (with respect
to Ar2CH+) indicates that different factors
control the thermodynamics of Lewis adduct formation for iodonium
ions and carbenium ions. Analysis of temperature-dependent equilibrium
measurements as well as ITC experiments reveal a large entropic contribution
to the observed Gibbs reaction energies for the Lewis adduct formations
from iodonium ions and Lewis bases originating from solvation effects.
The kinetics of the benzoate transfer from the bis(4-dimethylamino)-substituted
benzhydryl benzoate Ar2CH–OBz to the phenyl(perfluorophenyl)iodonium
ion was found to follow a first-order rate law. The first-order rate
constant k
obs was not affected by the
concentration of Ph(C6F5)I+ indicating
that the benzoate release from Ar2CH–OBz proceeds
via an unassisted S
N1-type mechanism followed
by interception of the released benzoate ions by Ph(C6F5)I+ ions.