Advanced Search
RSS LinkedIn Twitter

Journal Archive

Platinum Metals Rev., 2004, 48, (4), 159


Iridium-Based Hexacyanometallate Thin Films in Aqueous Electrolytes


  • Kasem K. Kasem*
  • Leslie Huddleston
  • Department of Natural, Mathematical and Information Sciences,
  • Indiana University Kokomo, Kokomo, IN 46904-9003, U.S.A.
  • Email:

Article Synopsis

Thin films of metal-hexacyanoiridium(III) (MHCI), KxMy[Ir(CN)6]z, where M = Ru, Fe were electrochemically prepared and used as surface modifiers for glassy carbon electrodes. The redox behaviour of the counter/central ions of these films was investigated in aqueous electrolytes using cyclic voltammetry, chronocoulometry and electrochemical impedance spectroscopy. An electrochemical synthesis of zeolite-like films of KxMy[Ir(CN)6]z and KxFey[Fe(CN)6]z (Prussian blue) was also undertaken using the cyclic voltammetric technique. Porous multi-film assemblies of Prussian blue and MHCI were formed either by the direct electrodeposition of Prussian blue over MHCI or Prussian blue over MHCI during repetitive potential cycling, or by electrochemically-driven insertion-substitution methods. In acidic aqueous KCl, iron hexacyano iridate (FeHCI) displays two redox waves with formal potential Eof ≈ 0.35 and 0.6 V vs. Ag/AgCl. The electrochemical behaviour of FeHCI was compared with that of related hexacyanometallate compounds, such as KRux[Ru(CN)6]y, KRux[Fe(CN)6]y and KFex[Fe(CN)6]y. In addition, evidence for the catalytic behaviour of MHCI films towards the reduction of iodate, IO3, is reported.

Immobilised mixed-valence hexacyanometallates (HCM) or hexahalometallates, for example KFex[Fe(CN)6]y or M X6−y, respectively, (where X = Cl, Br, M = iron (Fe), iridium (Ir), ruthenium (Ru), etc. and y is the charge) and related compounds are an important class of polynuclear compounds. Their ability to form a conducting polymer that resembles zeolitic or intercalation material, as well as redox organic polymers, has attracted the attention of many investigators (115). Prussian blue is an excellent example of an HCM compound. Earlier studies of Prussian blue were carried out more than two decades ago (2,4) and substantiate the interest in further research of related compounds. As transition metals with different formal oxidation states occupy the counter ion and the central ion sites, different redox centres are created within host thin films.

Two major characteristics of this class of inorganic redox film promote its usefulness for possible applications:

  • first, the oxidation or reduction of these solid films can proceed without dissolution of the solid compound as the film maintains its neutrality by an ion diffusion process, and

  • second, the formation of a bi- or multilayered structure is possible using an insertion-substitution mechanism.

Hexacyanometallates also possess these characteristic features of redox active solid films. The composition, thickness and structure of HCM thin films can also be manipulated to serve a desired use and to expand some features that can be used in industrial applications. Multilayered (810) insoluble films of HCM have important applications in membrane chemistry. Some of the studies cited here focus on the preparation of multilayered films, carried out either by electrodeposition of one film over the other, or by mechanical mixing of two insoluble HCMs.

In addition, several studies have been carried out on HCMs in which the central atoms were Ru (1619), cobalt (1), nickel (12), vanadium (20) or chromium (21). A limited number of studies (2225) have been performed on Kx[Ir(CN)6]y, but with no mention of the redox behaviour of this compound. Like most of the platinum metals, iridium oxide shows great electrocatalytic activity. This indicates that iridium compounds possess promising features as electron acceptors/donors or depolarisers in biological membranes, and more investigations are needed to understand the redox behaviour of Ir-based HCMs.

This paper reports new studies into the electrochemical behaviour of multilayered film assemblies where iron and iridium are the redox centres in KMx[Ir(CN)6]y. Furthermore, as ruthenium hexacyanoferrate has a zeolite-like structure (26), KFex[Ir(CN)6]y deposits are expected to have similar structure. An alternate method for the preparation of zeolite-like multifilm assemblies of iridium-based HCMs with bi-, or trivalent cations substituted as counter ions is discussed. Evidence for the catalytic activities of these assemblies on the electrode surfaces is presented.

Instrumentation and Methods

Experiments were carried out using a conventional three-electrode type electrochemical cell. The reference electrode was a Ag/AgCl (saturated KCl) half-cell of potential −45 mV vs. SCE. The counter (auxiliary) electrode was a platinum (Pt) wire, and the working electrode was a glassy carbon disk electrode (GCE) of surface area 0.071 cm2. The working electrode was cleaned by polishing with 1 µm α-alumina paste and rinsed with water and acetone prior to use. An electrochemical analyser was used to perform the electrochemical studies and X-ray photoelectron spectra (XPS) with typical depth analysis of 5–50 Å were recorded. The deposited films on the electrode surfaces were examined by scanning electron microscopy.

Impedance Measurement

Electrochemical impedance spectroscopy (EIS) studies were carried out. Faradic impedance measurements were performed within a frequency range of 0.1 mHz to 1 kHz. The current response was monitored and the data were analysed by a Fourier transformation algorithm.


Experiments were performed with pulses of width 50 ms. All the electrochemical experiments were carried out by deoxygenation in a nitrogen (N2 99.99%) atmosphere at room temperature (25.1°C).

Electrode Modification

Thin solid films of KFex[Ir(CN)6]y were electrodeposited via oxidative electropolymerisation on the glassy carbon electrode surfaces by repetitive potential cycling of a GCE between −0.30 and +1.2 V vs. Ag/AgCl, in freshly prepared aqueous solutions containing an equiv. 0.5 mM of K3[Ir(CN)6].2H2O, either FeCl3 or RuCl3, and 40 mM KCl (pH 2). Scans were carried out at a sweep rate of 100 mV s−1. The electrodes were then rinsed thoroughly and transferred to reactant-free electrolyte where their electrochemical response was examined. The electrode surface coverage (Γ) of this thin film was determined by integrating the areas under the voltammetric i-E curves.

A sheathing (overlaying) procedure was used to form a multifilm assembly. This included depositing KxFey[Ir(CN)6]z on the electrode surface to form the inner layer followed by deposition of KxFey[Fe(CN)6]z over the modified electrode using a similar method to that used to deposit the inner layer.

Results and Discussion

Electrodeposition of KFexIII[IrIII(CN)6]y

Evidence of formation of KFexIII[IrIII(CN)6]y can be detected from the cyclic voltammograms shown in Figure 1 for the GCE in aqueous solutions containing equiv. 0.5 mM of K3[Ir(CN)6].2H2O, and FeCl3 and 40 mM of KCl (pH 2). The growth of the redox wave as successive scanning took place is indicative of the build-up of redox potential film. Notice that the anodic current is always greater than the cathodic current. Such behaviour can be attributed to the difference in the kinetics of the oxidation and reduction processes in the film.

Fig. 1

Repetitive cyclic voltammetry at 0.1V s −1 of a glassy carbon electrode (GCE) in equivalent 1 mM of K3[Ir(CN) 6] and FeCl 3 in 50 mM KCl/HCl (pH = 2). Scan started at −0.20 V vs. Ag/AgCl

1A Plot of anodic peak current (ipa) vs. number of cycles

1B Anodic peak potential (Epa) vs. number of cycles

Repetitive cyclic voltammetry at 0.1V s −1 of a glassy carbon electrode (GCE) in equivalent 1 mM of K3[Ir(CN) 6] and FeCl 3 in 50 mM KCl/HCl (pH = 2). Scan started at −0.20 V vs. Ag/AgCl1A Plot of anodic peak current (ipa) vs. number of cycles1B Anodic peak potential (Epa) vs. number of cycles

Rate of K+FexII[IrIII(CN)6]y Deposition

The slope of the plot of ipa (anodic peak current) vs. the number of cycles as a function of time (Figure 1A) averages 1.04 × 10−6 µC/cycle. Considering the effective time of deposition per cycle is 2 seconds, the rate of film build up is 0.52 µC s−1. This rate is equivalent to a surface coverage of 7.7 × 10−11 mol cm−2/cycle. Figure 1A also shows that ipa reached a maximum after 17 cycles and then became steady. This suggests that 20 cycles are enough to make a stable film with better mechanical properties than thicker films.

Structure of KFexIII[IrIII(CN)6]y

Because of the small difference in radius among transition metal ions, calculation of the unit cell dimensions was performed as previously described in the literature (9). The calculated unit cell dimensions suggest that the monolayer thickness is ≈ 10.4 Å. This corresponds to a molar volume of 677.16 cm3 mol−1. The calculated monolayer equivalence based on the dimension of 10.4 Å is 10.75 × 10−10 mol cm−2. Accordingly, this means that approximately 14 cycles are needed to cover the electrode surface with the first layer.

The effect of this structure on the interfacial potential between the modified electrode and the solution is demonstrated in Figure 1B which shows an irregular-linear relationship between the recorded anodic peak potential and the number of cycles up to 25 cycles, after which it maintains constant value. Such behaviour indicates that the electrode/electrolyte interface was in steady change and reached constant structure after 25 cycles. This causes multi-interface systems, consisting of native GCE/[Ir(CN)6]3− and immobilised [Ir(CN)6]3−/free [Ir(CN)6]3−, to coexist. However, after the first 14 cycles the surface coverage of immobilised [Ir(CN)6]3− was sufficient to create one monolayer structure of immobilised [Ir(CN)6]3−. This monolayer was insufficient to create an interface that would give steady current and potential (Figures 1B and 1A) as both the current and potentials kept changing.

The steady rise in the current, see Figure 1A, could be evidence for film porosity, as a one monolayer film allowed redox ions through its network structure to be in contact with the active sites on the native electrode surface.

Spectroscopic Characterisation

Figure 2 is a scanning electron micrograph of the film formed on the GCE substrate. Figure 2 shows a highly crystalline deposit of cubic shape with dimensions of ∼ 200 nm. The discontinuity of this crystalline structure as well as its disordered packing makes film porosity highly likely. The XPS spectrum of the film formed (Figure 2) is shown in Figure 3. In Figure 3, the peaks corresponding to the trivalent iridium are identifiable by several peaks between 60 and 66 eV, at 105 eV, and between 300 and 500 eV. In particular, the signals at 495 eV support the Ir–O bonding that can be attributed to Ir(III) being surrounded by 6 O atoms. However, signals appearing between 705 and 725 eV indicate mixed valence Fe atoms coordinated with oxygen (Fe–O). This is evidence for the coexistence of Fe(II)–O and Fe(III)–O. The peak at 290 eV corresponds to C in the CN group, while the N peak is at 400 eV. It has been previously reported that multivalent oxides of transition metals can be codeposited from cyanometallate solutions at pH 2 (1,27).

Fig. 2

Scanning electron micrograph of polynuclear hexacyanoiridium(III) films on a GCE surface. The accelerating voltage is 0.8 kV

Scanning electron micrograph of polynuclear hexacyanoiridium(III) films on a GCE surface. The accelerating voltage is 0.8 kV

Fig. 3

X-ray photoelectron spectra (XPS) showing the binding energies and intensities of peaks of the aggregates shown in Figure 2

X-ray photoelectron spectra (XPS) showing the binding energies and intensities of peaks of the aggregates shown in Figure 2

Redox Behaviour of KFexIII[IrIII(CN)6]y Films

The general formula of hexacyanometallates (HCMs) can be written as MMAX[MBY(CN)6]Z; M represents main group metals, while MAX and MBY are generally transition metals. The reduction of the fixed counter cations of these compounds can take place via electron/cation addition according to the Equation:

while oxidation of the central atom can take place by electron loss followed by the anion addition needed for charge balance without affecting the coordination number/sphere (2):

As the deposited redox centres are totally immobilised, the charge transfer process is controlled by the mobility of the K or Cl ions (from the supporting electrolyte) and by electron hopping.

Scanning the potential of a GCE, modified with KFexIII[IrIII(CN)6]y at 200 mV s−1 between −0.40 and 1.20 V in 0.1M KCl, produced the solid line cyclic voltammogram shown in Figure 4. The cathodic scan (upper part) shows a broader reduction peak at 0.520 V, while two anodic peaks (lower part) at 0.520 and 0.80 V are shown in the anodic scan. Such behaviour depends on the scan rate. The dotted and dashed cyclic voltammogram in Figure 4 indicates that by decreasing the scan rate both the reduction and oxidation peaks become well defined. Notice that the reduction of Fe(III) as a counter ion becomes more identifiable at a lower scan rate. Unlike the formal redox wave reported for immobilised iron hexacyanoruthenate, KxFey[Ru(CN)6]z (7), the formal redox wave of iron counter ions appears at a more positive potential (∼ 0.375 V) and at a very low scan rate. Furthermore, the formal potential of the central Ir atom in the [Ir(CN)6]3− redox wave was at ∼ 0.680 V which is 100 mV less positive than that reported for IrCl63− (28).

Fig. 4

A Cyclic voltammogram of a GCE modified with KxFey[Ir(CN)6]z in 50 mM KCl/HCl at scan rates:

0.05 V s−1 (‐‐‐); 0.50 V s−1 (‐‐‐); 0. 200 V s−1 (—)

4 B Nyquist plot at 0.7 V; 4 C Nyquist plot at 0.5 V

Units: (1E + 5 ohm) = 1 × 105 ohm; (1E + 4 ohm) = 1 × 104 ohm

A Cyclic voltammogram of a GCE modified with KxFey[Ir(CN)6]z in 50 mM KCl/HCl at scan rates:0.05 V s−1 (‐‐‐); 0.50 V s−1 (‐‐‐); 0. 200 V s−1 (—)4 B Nyquist plot at 0.7 V; 4 C Nyquist plot at 0.5 VUnits: (1E + 5 ohm) = 1 × 105 ohm; (1E + 4 ohm) = 1 × 104 ohm

The phenomena of such ill-defined redox waves in KFexIII[IrIII(CN)6]y at scan rates faster than 10 mV s−1 distinguish it from other studied HCM. Figure 4 shows at scan rates faster than 10 mV s−1, that total overlapped waves having a formal redox centre closer to that of the central Ir ion occur. This indicates there is slow charge transfer in the counter Fe ion centre. Obtaining a well-defined Fe redox wave at (∼ 0.375 V) at a slow scan rate confirms this conclusion. The fact that the compact (3d) orbital in Fe has less metal-donor atom bonding than the more expanded (5d) orbital in the Ir ion makes Ir ions soft acids. Unlike the Ru in KxFey[Ru(CN)6]z no Ir oxides are being formed. The fact that KxFey[Ru(CN)6]z shows similar electrochemical behaviour to KxFey[Fe(CN)6]z, but different to that of KFexIII[IrIII(CN)6]y may indicate the effect of expanded (5d) orbitals in the Ir ions.

The Nyquist plots, which predict the stability and performance of a closed-loop system by observing its open-loop behaviour, see Figures 4B and 4C for a 1.49 nm film, show combined diffusional behaviour (mass transfer is the significant factor) with no sign of charge saturation, and a kinetically controlled charge transfer process. The greater Z in Figure 4C (at 0.5 V) compared to that in Figure 4B (at 0.7 V) reflects the importance of Cl ions in charge balance when both iron and iridium are in their highest stable oxidation states. However, when impedance measurements are carried out at 0.5 V, only the counter ion Fe is oxidised (d5 Fe3+). As the counter ion occupies the interstitial sites of octahedral [Ir(CN)6]3, the charge balance to these sites requires the removal of K+ ions and the diffusion of Cl ions. The kinetics of this process may affect the magnitude of the impedance measured at this potential. The equivalent circuit for the film assembly can be pictured as an ohmic resistance (RΩ) in series with a paralleled double layer capacitor (Cdl) with charge transfer resistance (Rct), see inset in Figure 4. At 0.7 V, when both the Ir and Fe cations involved in the network structure of this assembly are in their highest oxidation states, the number of K+ ions needed for charge balance in the film assembly is reduced. This will hinder self diffusion in the film. Calculations from the impedance measurement showed that the diffusion coefficent (Dct) was 2.2 × 10−9 cm2 s−1. This quantity is in agreement with Dct determined for IrCl62−or [Fe(CN)6]3− immobilised in poly Ru(vbpy)32+ at the saturation level where the ratio of surface coverage of M (ΓM) to that of the polymer (ΓPoly) is (ΓMPoly ≥ 0.3) (29).

Stability of KFex[Ir(CN)6]y Film

Cu2+-Substituted KFex[Ir(CN)6]y

GCEs modified with a thin film of KFex[Ir(CN)6]y undergo structural alteration by substitution of the counter Fe3+ ion by Cu2+ (d9). This is achieved by cycling the potential of the GCE modified with KFex[Ir(CN)6]y thin film in the desired metal ion acidic solution. The results, see Figures 5A and 5B, indicate that Cu2+ partially substituted the Fe counter ions in the film.

Figures 5A and 5B show the redox wave of the film after 2 hours of Cu substitution (Figure 5B). This has not only affected the Fe redox wave, but has also decreased the total amount of redox active materials by ∼ 25% of the initial amount. Unlike Prussian blue, which is fully substituted in under 2 hours, KFex[Ir(CN)6]y is less susceptible to substitution.

Fig. 5

A Cyclic voltammogram at 0.05 V s−1 of a GCE modified with KxFey[Ir(CN) 6]z in 50 mM KCl/HCl

5B Cyclic voltammogram after the GCE was immersed in Cu2+ for 120 minutes

A Cyclic voltammogram at 0.05 V s−1 of a GCE modified with KxFey[Ir(CN) 6]z in 50 mM KCl/HCl5B Cyclic voltammogram after the GCE was immersed in Cu2+ for 120 minutes

Formation of Zeolite-Like Bilayer Film Assembly

Formation of Multi-Film Assemblies

The sheathing method previously described was performed and the results are shown in Figure 6. Figure 6A shows the cyclic voltammogram obtained for a modified GCE with an assembly of KxFey[Fe(CN)6]z (Prussian blue) as the inner layers and KxFey[Ir(CN)6]z as the outer/upper layers in a 1:1 ratio (equal surface coverage of 1.97 × 10−9 mol cm−2). The redox waves of the Ir-related centres overlap with that of the central Fe atom in Prussian blue at 0.75 V. The redox wave at 0.20 V is due to the counter Fe atom in the Prussian blue inner layer, while the redox wave of the counter Fe atom in the upper layer has an ill-developed anodic peak at 0.4 V. The fact that this redox wave exists suggests that the counter Fe ions in this assembly have two different redox potentials depending upon the central ion with which they associate. Due to the structure of the bi-film (which includes both Ir and Fe as central ions) two redox potentials of central Fe and Ir ions coexist and overlap. Figure 6B shows the cyclic voltammogram obtained for a modified GCE with an assembly of KxFey[Ir(CN)6]z as the inner layers and KxFey[Fe(CN)6]z (Prussian blue) as the outer/upper layers in a 1:1 ratio.

Fig. 6

A Cyclic voltammogram of a GCE modified with Prussian blue under KxFey[Ir(CN) 6]z in KCl/HCl

6B Cyclic voltammogram of a GCE modified with KxFey[Ir(CN) 6]z under Prussian blue in KCl/HCl.

Scan rates: (‐‐‐) at 0.005 V s−1, (—) at 0.01V s−1

A Cyclic voltammogram of a GCE modified with Prussian blue under KxFey[Ir(CN) 6]z in KCl/HCl6B Cyclic voltammogram of a GCE modified with KxFey[Ir(CN) 6]z under Prussian blue in KCl/HCl.Scan rates: (‐‐‐) at 0.005 V s−1, (—) at 0.01V s−1

The order in which the layers are placed or formed affects the magnitude of the capacitive current. It also affects the shape of the collective redox waves in the assembly with very little change in the formal potentials of these redox waves, as observed when comparing the cyclic voltammograms in Figures 6A and 6B. The fact that the redox wave at ∼ 0.75 V is much larger in Figure 6B than in Figure 6A may indicate that the upper KxFey[Ir(CN)6]z layer is more porous than Prussian blue. This will allow more transport of ions needed for electrical neutrality when both the central ions in Prussian blue and KxFey[Ir(CN)6]z are oxidised or reduced. The cyclic voltammogram for the film assembly created indicates perfect surface waves with smaller double layer capacitive current.

Evidence of Catalytic Activity

The catalytic activity of KxFey[Ir(CN)6]z was tested using the IO3 as a soft base with +7 oxidation state iodine atom. There was no technological significance behind the choice of that anion in this study. Modified GCEs with thin films of KxFey[Ir(CN)6]z exhibited electrocatalytic activities towards the reduction/oxidation of IO3. Evidence for such catalytic behaviour can be seen in the cyclic voltammograms obtained in an acidic solution of KIO3 (Eof = 0.4 V vs. Ag/AgCl), see Figure 7A. A carbon paste electrode of the same apparent geometrical area was used to confirm that the reduction peaks shown in Figure 6 were not due to an increase in electrode surface area.

Fig. 7

Electrolytic catalytic activities towards the reduction of IO3 in aqueous KCl (pH = 1); scan rate 0.01 V s−1

7A 1 Naturally occurring/Native GCE in 0.05 M KIO3 (KCl/HCl)

 2 GCE modified with KxFey[Ir(CN)6]z in KCl/HCl

 3 GCE modified with KxFey[Ir(CN)6]z in 0.05 M KIO3

7B 2 GCE modified with Kx −1RhyFe[Ir(CN)6]z in KCl/HCl

 3 GCE modified with Kx − 1RhyFe[Ir(CN)6]z in 0.5 M KIO3

Electrolytic catalytic activities towards the reduction of IO3− in aqueous KCl (pH = 1); scan rate 0.01 V s−17A 1 Naturally occurring/Native GCE in 0.05 M KIO3 (KCl/HCl) 2 GCE modified with KxFey[Ir(CN)6]z in KCl/HCl 3 GCE modified with KxFey[Ir(CN)6]z in 0.05 M KIO37B 2 GCE modified with Kx −1RhyFe[Ir(CN)6]z in KCl/HCl 3 GCE modified with Kx − 1RhyFe[Ir(CN)6]z in 0.5 M KIO3

Native GCE shows a reduction peak at 0.430 V (Figure 7A, line 1) whereas modified GCE with KxFey[Ir(CN)6]z (Figure 7A, line 3) shows reduction peaks with greater cathodic currents at 0.6 and 0.45 V. The larger cathodic current is due to the catalytic effect of KxFey[Ir(CN)6]z. Furthermore, doping the film with an element from the same group as Ir (Rh) did not improve the catalytic activity. This can be concluded from Figure 7B (line 3), which represents the behaviour of GCEs modified with Kx−1RhyFe[Ir(CN)6]z under the same experimental conditions. It can be noted that less catalytic current is generated from doped film than from undoped film. The observed catalytic current in Figure 7 is due to the reduction of iodate to iodide according to the Equation:


This study shows evidence of the efficient manipulation of Ir-HCM film structures to a desired composition and porosity. The redox behaviour of thin films of iridium-based HCMs differs from those of (3d) and (4d) metals-based HCM. The formation of higher oxidation state oxides in proximity to cyanide complexes was noticed with (3d) or (4d) metals. This was not the case for Ir-based HCM. The expanded valence shell of the Ir ion in which its (5d) electrons are preceded by 4f14 create a soft acid nature for Ir (II or III) ions as a central atom. The reactivity of its 6-π acceptor ligand (CN) with Ir ions may be considered when comparing the redox behaviour of (5d) metal-based HCM with those of (3d) or (4d) metal-based HCMs. The catalytic activity of Ir-based HCM agrees with that of most of the studied HCM and can be explained on the basis of an electron/proton transfer process.



  1.  Z. Gao, G. Wang, P. Li and Z. Zhao, Electrochim. Acta, 1991, 36, 147 LINK doi:10.1016/0013-4686(91)85193-B
  2.  K. Itaya, H. Akahoshi and S. Toshima, J. Electrochem. Soc., 1985, 128, (7), 1498
  3.  L. M. Siperko and T. Kuwana, J. Electrochem. Soc., 1983, 130, 396
  4.  V. D. NeffJ. Electrochem. Soc., 1978, 125, 886
  5.  K. K. Kasem, J. Appl. Electrochem., 1999, 29, 1473 LINK doi:10.1023/A:1003806808008
  6.  T. R. Cataldi, C. E. de Benedetto and C. Campa, J. Electroanal. Chem., 1997, 437, 93 LINK doi:10.1016/S0022-0728(97)00117-4
  7.  K. K. Kasem, Mater. Sci. Eng., 2001, B83, 97 LINK doi:10.1016/S0921-5107(01)00503-7
  8.  A. Dostal, M. Hermes and F. Scholtz, J. Electroanal. Chem., 1996, 415, 133 LINK doi:10.1016/S0022-0728(96)04709-2
  9.  S. J. Reddy, A. Dostal and F. Scholtz, J. Electroanal. Chem., 1996, 403, 209 LINK doi:10.1016/0022-0728(95)04380-2
  10.  K. Kasem, R. Hazen and R. M. Spaulding, Interface Sci., 2002, 10, 261 LINK doi:10.1023/A:1020848711982
  11.  D. Olaf, L. Sabine, H. Frank and B. Michael. J. Exp. Bot., 1990, 41, (230), 1055
  12.  L. Hartwig and B. Michael, Plant Physiol., 1988, 86, (4), 1044
  13.  K. K. Kasem, J. Appl. Electrochem., 2001, 31, 1125 LINK doi:10.1023/A:1012222415364
  14.  S. Ohkoski, A. Fujishima and K. Hashimoto, J. Am. Chem. Soc., 1998, 120, 5349 LINK doi:10.1021/ja980732f
  15.  J. A. Cox and R. K. Kulkarni, Talanta, 1986, 33, (11), 911 LINK doi:10.1016/0039-9140(86)80222-3
  16.  J. A. Cox and P. J. Kulesza, Anal. Chem., 1988, 5, (16), 1021
  17.  J. A. Cox, J. Electroanal. Chem., 1987, 233, (1–2), 87 LINK doi:10.1016/0022-0728(87)85008-8
  18.  P. J. Kulesza, J. Electroanal. Chem., 1987, 220, (2), 295 LINK doi:10.1016/0022-0728(87)85116-1
  19.  T. R. Cataldi, C. E. De Benedetto and C. Campa, J. Electroanal. Chem., 1998, 458, 149 LINK doi:10.1016/S0022-0728(98)00327-1
  20.  Y. Wang, G. Zhu and E. Wang, J. Electroanal. Chem., 1997, 430, 127 LINK doi:10.1016/S0022-0728(97)00104-6
  21.  J. P. Eaton and D. Nicholls, Trans. Met., 1981, 6, 203
  22.  N. M. Pinhal and N. V. Vugman, Hyperfine Interact., 1989, 52, (1), 89
  23.  N. V. Vugman and N. M. Pinhal, Report, 1983, (UFRJ-IF-10/83), AN 1984, 156787
  24.  N. V. Vugman and N. M. Pinhal, Mol. Phys., 1983, 49, (6), 1315–1319
  25.  N. V. Vugman, R. P. A. Muniz and J. J. Danon, J. Chem. Phys., 1972, 57, (3), 1297 LINK doi:10.1063/1.1678390
  26.  K. Kasem, F. R. Steldt, T.J. Miller and A. N. Zimmerman, Microporous, Mesoporous Mater., 2003, 66, 133 LINK doi:10.1016/j.micromeso.2003.09.006
  27.  W. Gorski and J. A. Cox, Anal. Chem., 1994, 66, 736
  28.  W. Sun, H. Liu, J. Kong, G. Xie and J. Deng, J. Electroanal Chem., 1997, 437, 67 LINK doi:10.1016/S0022-0728(97)00356-2
  29.  K. Kasem and F. A. Schultz, J. Inorg. Organomet. Polym., 1994, 4, (4), 377

Supplementary Material

Details of Experimental Procedure and Equipment

Chemicals used were reagent grade; K3[Ir(CN)6].2H2O, FeCl3, RuCl3, and KCl were obtained from Aldrich Chemical Co. All other reagents were of at least reagent grade and were used without further purification.

The GCE was from Bioanalytical Systems (surface area 0.071 cm2); the electrochemical analyser was a BAS 100B electrochemical analyser (Bioanalytical Systems).

X-ray photoelectron spectra were recorded with a Perkin Elmer 5500 ESCA (aluminium filament source), with a typical depth analysis of 5-50 Å. The XPS were calibrated using silver line standards. Scanning electron micrographs of the deposited films on the electrode surfaces were obtained using an Amray 1000A Scanning Electron Microscope at an accelerating voltage of 8 kV. Electrochemical impedance spectroscopy studies were carried out using a Bioanalytical Systems impedance module.

The Author

Kasem K. Kasem is a Professor of Chemistry at Indiana University Kokomo, U.S.A. He is interested in developments in the field of applied electrochemistry, especially in physical and analytical applications of chemically-modified electrodes. He also has interests in semiconductor electrochemistry, the electrochemical behaviour of polymeric thin films, activation and metallisation of polymers, and the electrodeposition of metals and alloys.

Leslie Huddleston was an undergraduate at Indiana University Kokomo, U.S.A. when she worked on this project. She obtained her BS in chemistry at Kokomo and is currectly working in industry.

Read more from this issue »