The
kinetics of aqueous outer-sphere electron-transfer (ET) reactions
are determined in large part by noncovalent electrostatic interactions
that originate from the surrounding electrolyte solution. In this
work, we examine the role of spectator cations in modifying the rate
of heterogeneous ET for an [Fe(CN)6]3–/[Fe(CN)6]4– redox pair. We combine
the results of electrochemical measurement, in situ surface-enhanced infrared absorption spectroscopy (SEIRAS), classical
molecular dynamics simulation, and theoretical modeling to demonstrate
how changing the identity of the spectator cation species over a series
that includes Li+, Na+, K+, Rb+ to Cs+ influences the solvation properties and
ET kinetics of the redox species. By analyzing the results in the
context of the Marcus–Hush–Chidsey (MHC) theory, we
find that the solvent reorganization energy increases systematically
as the cationic radius decreases. The trend can be attributed to cation-dependent
coordination environments of the redox species, whereby more cations
of less charge density such as Cs+ than Li+ are
present in the redox solvation shell in bulk and at the electrified
interface, promoting weaker hydrogen bonds and lowering the effective
interfacial static dielectric constant. We discuss the implications
of these findings for enabling the tunability of reaction thermodynamics
and rates in electrochemical processes.