the result that proton transfer often accompanies electron transfer, particularly in aqueous solution. In less
polar organic solvents, H-bonding also can play an important role. While it is generally appreciated that
proton transfer will have a greater effect on the overall reaction than H-bonding, it is not always straight
forward to distinguish between the two, and, despite a considerable amount of research, a complete,
quantitative understanding of the relative roles that the two play in the voltammetry that is observed upon
addition of acids or bases to organic redox couples in non-aqueous solution remains elusive.
This study focuses on the electrochemistry of p-tetramethylphenylenediamine, H 2 PD, in acetonitrile in the
presence of pyridine bases. In acetonitrile, this compound undergoes a reversible one electron oxidation
to the radical cation, H 2 PD + , followed by a second reversible oxidation to the strongly acidic quinoidal
dication, H 2 PD 2+ . With the addition of 1 equivalent of the pyridine base, no significant change in the first
oxidation is observed, but there is a large negative shift in the E 1/2 of the second oxidation with no loss in
reversibility. Subsequent additions show a smaller, incremental negative shift, still with no loss in
reversibility. We believe that this behavior signals proton transfer is occurring between the pyridine, pyr,
and the H 2 PD 2+ , so that the overall reaction occurring in the second oxidation corresponds to H 2 PD + + pyr
= HPD + + Hpyr + + e-. In this case, the observed E 1/2 should depend linearly on the pK a of the Hpyr + with a
slope of −60 mV/pH unit. To test this hypothesis, the voltammetry of H 2 PD was studied with different
pyridines that cover a range of pK a values. A plot of E 1/2 of the wave observed with 1 eq pyridine vs. pKa is
indeed linear with close to the predicted slope. Furthermore, it is found that the continued shift in E 1/2 of
the second oxidation with increasing concentrations of pyridine is well-accounted for simply by applying
the Nernst equation to the overall reaction. However, while proton transfer can explain the potentials of
the CV waves in the presence of added pyridine, simulations of the voltammetry show that proton transfer
by itself cannot explain the observed reversibility of the second oxidation wave in the presence of
increasing amounts of added pyridine. This is where H-bonding can play a role. By including H-bonding
steps, and allowing electron transfer and proton transfer to occur through the H-bond complex formed
between H 2 PD + /pyr and HPD + /Hpyr + , the simulations nicely explain both the observed potential shifts and
the reversibility of the waves.
The next question is whether the electron and proton transfer within the H-bonding complex is concerted
or step wise. To test this, CV’s were run with 10:1 cyanopyridine:H2PD in 2% D 4 -methanol/acetonitrile or
2% H 4 -methanol/acetonitrile. If the second oxidation involved concerted electron-proton transfer, a
significant deuterium isotope effect would be expected, causing a larger ΔE p in the deuterated solvent
resulting from slower electron transfer. However, no significant difference was observed. Therefore,
there is no evidence that the electron-proton transfer is concerted. This result does not by any means
rule out the hypothesis that the proton-electron transfer is occurring within the H-bond complex, it merely
indicates that it is likely that the proton and electron transfer occur in a step-wise fashion within the H-
bond complex, and that facilitation of proton-electron transfer by H-bonding can happen even if the
process is not concerted.