Redox kinetics of cyanoferrate(III) species adsorbed at an n-type ZnO multipod/electrolyte interface is explored
using electrochemical techniques like cyclic voltammetry and impedance spectroscopy. The electrochemical
impedance results are analyzed using a fluctuating energy level model, assuming isoenergetic tunneling of
majority carriers through the Helmholtz layer. A shift in the slope of Mott−Schottky plots (C
sc
-2 versus E)
together with evidence from cyclic voltammetry shows that the electron-transfer process is mediated by surface
states formed because of the adsorption of ferricyanide ions (as evident from the results of Fourier transform
infrared spectroscopy). More significantly, the pH of zero charge (point of zero zeta potential, pzzp) of ZnO
multipods is found to be 4.5 (from capacitance vs pH plots) compared to that of bulk ZnO (pH 9.5), which
could be explained on the basis of a lowering in the work function of the nanostructured semiconductor and
its consequent susceptibility to the formation of surface states. This is in excellent agreement with our earlier
observation of ultralow threshold field emission with this material in the light of the linear dependence of
pzzp with work function of the electrode material. The flat-band potential of the nanostructures is found to
be 200 mV more negative than that reported for bulk n-type ZnO electrodes, indicating a higher doping
density in the former. A three-dimensional mapping of charge distribution in the surface states is attempted
by correlating the capacitance response of the system subjected to a sinusoidal potential modulation to the
semiconductor electrode with that resulting from a systematic variation of the redox potential of the dissolved
acceptor (achieved by varying the pH of the electrolyte) which further reveals the polyenergetic nature of the
surface states.