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Electrocatalytic activity of common noble metal (platinum, bimetallic platinum-ruthenium and palladium) nanoparticles (both unsupported and supported on Vulcan carriers) toward electrooxidation of formic acid in acid medium (0.5 mol dm–3 H2SO4) can be significantly enhanced by dispersing them over thin film of zirconia (ZrO2). The enhancement effects concern increases of the electrocatalytic current densities (normalized against the mass of noble metal catalysts) recorded under both cyclic voltammetric and chronoamperometric conditions. The observations can be rationalized in terms of the ability of zirconia nanostructures to provide active hydroxyl groups capable of inducing the removal of the inhibiting COOH or CO type adsorbates from their surfaces. The role of Vulcan carriers is in improving electronic conductivity, in addition to facilitating distribution of catalytic metal sites at the electrocatalytic interface. Regarding dissimilar mechanisms for HCOOH oxidations at Pt, PtRu and Pd nanoparticles, the activating capabilities of zirconia differ depending on the potential applied thus reflecting distinct nature of electronic or chemical interactions. Specific interactions between the zirconia support and noble metal nanoparticles are also possible, particularly in the case of Pd-based catalysts where the enhancement effects are the most pronounced. Finally, it should be emphasized that, historically, representatives of Russian school of electrochemistry, including V.S. Bagotsky, were one of the first world-wide who investigated the formic acid oxidation and emphasized the importance of metal—support interactions during electrooxidation of small organic molecules at noble metal nanoparticles.

Carbon is nonmetal and lead is a typical metal, while silicon and germanium exhibit semiconducting properties. Compounds with hydrogen are stable and common for carbon, but the number of such compounds for silicon and germanium becomes limited, and for lead, only one unstable compound of that type is known. The chemistry of the divalent state is more important for heavier elements and the basicity of oxides increases from carbon to lead. Carbon forms a great number of compounds with different oxidation states. The characteristic feature of carbon is significant stability in both the +4 and -4 valence state compounds. Only the potentials of those compounds of carbon that are traditionally grouped with inorganic substances. The electrode reactions of silicon species are slow under normal conditions, which may follow from the fact that the bonds of silicon with other atoms are quite strong.

Over 200 years of development of modern electrochemistry was divided into five periods. Period I from the beginning up to the end of nineteenth century, Period II from 1901 to 1945, Period III from 1946 to 1965, Period IV from 1966 to 1990, and the last Period V from 1991 till the present. This division is based on (1) use of different research methods in these periods, as well as (2) different intensity and organization of research work. In each period, the main research interests were briefly characterized, followed by short discussion of the main achievements. The expected trends of future development of electrochemistry were also briefly discussed.

The preparation of copper(II) hexacyanoferrate (CuHCF) films on the surface of gold electrodes as well as their characterization in solutions of various alkali metal and NH 4 + cations and in the presence of thallium(I) are described. The electrochemical quartz crystal microbalance and cyclic voltammetric techniques were used. In 0.50 M lithium nitrate, even at submillimolar concentration of Tl(I), the formal potential of CuHCF was shifted to more positive values. At higher Tl(I) concentrations, the formal potential of the CuHCF redox reaction changed linearly with the logarithm of Tl(I) concentration (in the 0.50 M solution of lithium or another alkali metal nitrate). From such dependencies, selectivity coefficients K Tl/M were calculated, and they show that the CuHCF film on the gold electrode interacts preferentially with Tl(I). High affinity of Tl(I) to copper hexacyanoferrate, that was observed in the presence of alkali metal cations, was explained by relatively strong donor–acceptor interactions of Tl(I) ions with nitrogen in CN groups of the CuHCF film. It was also shown for simple M 4 [Fe(CN) 6 ] metal ferrocyanate salts (where M = Li + , Na + , K + , Rb + , Cs + and Tl + ) that there is a preferential interaction of Tl + with CN group consistent with formation of a Tl–NC–Fe bridge.

Research carried out in the Laboratory of Professor Wiktor Kemula and his coworkers at the University of Warsaw in time of a divided world is described briefly. The description starts from the early works of Professor at the University of Jan Kazimierz in Lvov and ends around 1990, when important political transformations occured in Europe. Difficulties in research work, resulting from a divided world, of this laboratory and other electrochemical laboratories in Poland are presented.

Voltocoulometric, chronocoulometric and cyclic voltammetric studies of the electrode reactions of the Pb(2,2,2) 2+ , Pb(2,2,1) 2+ and Pb(2,2) 2+ complexes were described ((2,2)-1,7,10,16-tetraoxa-4,13-diazacyclooctadecane, (2,2,1)-4,7,13,16,21-pentaoxa-1,10-12 diazabicyclo[5.8.8]tricosane, (2,2,2)-4,7,13,16,21,24-hexaoxa-1,10diazabicyclo[8.8.8]hexacosane). It was found that such Pb(L) 2+ complexes are adsorbed on the Hg electrode. The analysis of adsorption data for Pb(2,2,2) 2+ in the presence of excess of ligand (2,2,2) shows that the complex is adsorbed according to the competitive adsorption mechanism. Electroreduction processes of the studied complexes proceed via two parallel pathways: from the solution and from the adsorbed state. The electrode kinetic parameters of lead(II) complexes free of adsorption influence were found by analysis of the normal pulse voltocoulometric curves recorded with a 1 ms delay after application of the short potential pulse. From the analysis of kinetic parameters it follows that the electroreduction of Pb(L) 2+ is a two-step CE process with the rate determining step preceded by complex dissociation. The rate constants of the studied Pb(L) 2+ /Pb(Hg) systems are considerably lower than the rate constant of noncomplexed Pb 2+ ion in aqueous solution. We have found that the reaction rate constants of the systems Pb(L) 2+ /Pb(Hg) decrease linearly with increasing stability of the complexes. This dependence is also obeyed by cadmium and thallium complexes with the same ligands.

Electrodeposition of well-adhering polypyrrole-based hybrid films containing hexacyanoferrate(II,III) anions from neutral solutions of pyrrole and potassium hexacyanoferrate(II) on medium carbon (0.48% C) steel has been described. The resulting polypyrrole coatings that are doped with hexacyanoferrate(II,III) anions show protective properties against pitting corrosion of carbon steel substrates in strongly acidic media containing chlorides (0.1 mol dm−3 HCl + 0.4 mol dm−3 NaCl). Polypyrrole acts as a stable host matrix for inorganic anions. The presence of negatively charged species (hexacyanoferrates) in the polymer backbone tends to block the access of pitting-causing anions (chlorides) to the surface of steel. The Fe(CN)63-/4− anions existing in the vicinity of steel substrate stabilizes its surface by forming an overcoating in the form of sparingly soluble metal hexacyanoferrate, mostly Prussian blue (PB), microstructures. It has been demonstrated that by applying cyclic voltammetry and X-ray photoelectron spectroscopy, the presence of traces of free cyanide anions promotes the formation of PB on carbon steel surface which results in increasing the adherence of polypyrrole-based films to the metallic substrate. Morphology of the protective composite films is also addressed.

Electrochemical and electrochemical quartz crystal microbalance (EQCM) methods were used for the analysis of the growth and dissolution processes of sparingly soluble deposits. As a model of a sparingly soluble film, uranyl-hexacyanoferrate was selected. Additionally the rate of Prussian blue deposition was studied. We have shown that coupling of the EQCM technique with standard electrochemical methods may be useful in the study of mechanisms of electrodeposition phenomena when the solubility of the product of the electrode reaction is limited. The transformation of mass–time data into current–time dependences allows an analysis of the reaction in terms of electrocrystallization steps while other masking processes are superimposed during the polarization of the electrode. This approach may have general value and may be applied not only to hexacyanoferrate deposition but also to deposition of other products of the electrode reaction, which exhibit limited solubility. Analysis of growth of uranyl-hexacyanoferrate on the Au/quartz electrode under potentiostatic and cyclic voltammetry conditions, taken as an instance, reveals that the first step, limited by the growth of the crystallization nuclei, is clearly separated from the uniform growth, limited by diffusion. For thicker films, the slope of the frequency–charge dependence is dominated by the insertion/removal process of potassium ions, to and from the film. During the dissolution of the uranyl-hexacyanoferrate deposits, two clearly separated steps were observed. During the first, relatively fast oxidation of the deposit is observed which is accompanied by removal of potassium ions from the film. The second step corresponds to a chemical dissolution of the oxidized film. The rate coefficients corresponding to both steps were determined. Based on the gravimetric and electrochemical data, the molar mass of the deposited uranyl-hexacyanoferrate was estimated as equal to 690 ± 90 g/mol. From these and the EDX data, a chemical formula of the deposited uranyl-hexacyanoferrate was proposed as: K2(UO2)[Fe(CN)6].

The electrochemical behaviour of mixtures of phenazine (P) with iodine (I2) in the solid state was investigated. Three types of electrochemical experiments were conducted: (i) EMF measurements of the Ag/AgI/I2:P system for various I2 : P ratios, (ii) cyclic voltammetric (CV) experiments and (iii) potentiometric measurements of the open cell potentials after different cathodic charges were injected into the I2 : P pellets. In the first case, a detailed analysis of the observed electromotive force was presented. The Gibbs free energy of the I2 : P complex determined was in good agreement with earlier results. In the second case, the CV curves corresponding to the electrode processes of phenazine mixed with graphite in the solid state indicate that the mass and charge transfer, which occur in the pellets, are faster than expected. The potentiometric experiments confirm this conclusion. Additional experiments, conducted with pellets of different thickness, indicate that although, in comparison with an equilibrated pellet, the concentration profiles are modified in small layers (diffusion layers) neighbouring the electrodes, the electrode reaction probably occurs in the whole pellet. A tentative mechanism of these processes is discussed. Copyright © 2003 John Wiley & Sons, Ltd.

We describe the electrochemical behavior of solid copper hexacyanoferrate (powder) investigated in the absence of contact with a liquid external supporting electrolyte. In addition to a typical hexacyanoferrate(III,II) redox transition, the system is characterized by a second electrode process which appears at more negative potentials. Diagnostic experiments, which include spectrochemical and solid-state voltammetric characterization, support our view that the latter redox reaction most likely originates from reduction of the system's lattice copper(II) ions. The overall dynamics of charge transport in the material, when discussed in terms of effective diffusion, is moderately high (on the level of 10 −8 cm 2 s −1 ). Comparison has been also made to the electrochemical behavior of solid Prussian blue and to the voltammetric characteristics of conventional electrodes modified with thin films of copper hexacyanoferrate.

The electrochemical analysis of the properties of the adsorbed reactant state for the case when it is energetically close to the nonadsorbed state of the electroactive species is presented. The method of separation of thecorresponding adsorption and adsorption-free contributions to the overall faradaic response, which may also supply the voltammetric properties of adsorbed state, is given. It is based on recording, for a given solution, two normal pulse, charge-potential (voltocoulometric) curves. The first curve is obtained by integration of the faradaic current over the entire duration of the potential pulse t (Q t -E curve). For the second curve the charge is measured with the exclusion of the first millisecond after the application of the potential pulse (Q t - 1 vs E curve). The numerical model of such dependencies proves that the shape of their difference AQ = Q t - Q t - 1 as a function of the electrode potential satisfactorily approximates the electrochemical properties of the adsorption state. Such an approach is recommended as a simple way of analysis of the properties of the adsorption state of electroactive substances which do not yield a distinct separate faradaic response from the adsorption state.

Composite nickel/thallium hexacyanoferrates were prepared as thin films on electrode surfaces. Electrodeposition of composite films was achieved by potential cycling in the solution for modification containing, in addition to potassium salt electrolyte, nickel(II), thallium(I), and hexacyanoferrate(III). Depending on the relative amounts of thallium to nickel, either a mixed phase with respect to interstitial ions was formed in which Tl(I) cations substitute potassium countercations at interstitial positions of nickel hexacyanoferrate or mixed phases of hexacyanoferrates of nickel and thallium were produced. Due to large differences in ionic radii of Ni(II) and Tl(I), formation of heteronuclear nickel/thallium hexacyanoferrate, in which both nickel(II) and thallium(I) are nitrogen-coordinated within the cyanometallate lattice, was rather unlikely. On basis of the stripping-like determinations, we propose a stoichiometric formula, K 2− z Tl I z Ni II [Fe II (CN)] 6 ( z ≤1), for the system in which interstitial K + was substituted with Tl(I); and a more general K x Tl I z Ni II y [Fe II (CN)] 6 formula that also reflects the possibility of codeposition of separate nickel hexacyanoferrate and thallium hexacyanoferrate microstructures during the film growth. Mixed nickel/thallium hexacyanoferrate films showed good stability during voltammetric potential cycling. In addition to potassium salt electrolytes, well-defined and reversible cyclic voltammetric responses were also obtained in sodium and cesium electrolytes.

The temperature dependences of the four transfer coefficients for cathodic and anodic electrode reactions of two different types of systems, namely Cr(III)/Cr(II) and Cr(II)/Cr(Hg), were determined in 5.0 M NaClO 4 solution. The results were obtained for a wide range of temperatures from −20 to 90°C. The α parameter determined from the log k fh on E dependence corresponding to the Cr 3+ +e − →Cr 2+ electrode process shows the highest dependence on temperature (∂ α /∂ T =1.1±0.3×10 −3 K −1 ), whereas the β parameter corresponding to the Cr 2+ →Cr 3+ +e − electrode process is virtually independent of temperature (∂ β /∂ T =0). The same results were obtained when the transfer coefficients were determined from dependence of the enthalpy and entropy of activation on overpotential. The observed temperature dependence of α is attributed to the changes of the ϕ 2 potential. The transfer coefficients for the Cr 2+/0 electrode reaction also show some dependence on temperature (∂ α /∂ T =8.7±2.0×10 −4 K −1 and ∂ β /∂ T =3.2±1.4×10 −4 K −1 ), which probably results from the influence of the ϕ 2 potential.

The electroreduction of nitromethane and 1-nitrohexane in both the absence and in the presence of n-octanol and n-decanol was studied. It was found that, under comparable conditions at smaller concentrations of inhibitors, nitromethane is inhibited more strongly than 1-nitrohexane by the n-alcohol adsorbed monolayer on the mercury electrodes. This was explained by the larger affinity of nitrohexane to the alcohol-rich surface phase and of nitromethane to the aqueous solution phase. Through the increased affinity of both reactants to the electrode surface phase at the inhibitor concentration, c/cs, exceeding 0.6, the independence of the electroreduction rate constant of both reactants was explained. When the bulk concentration of inhibitors approached saturation even the increase of the rate constant was observed. The change of the solvent composition, from pure water to 10 vol. % ethanol, increases the inhibition by increasing the affinity of the reactant to the solution phase.

The electrode reaction of the Cd2+ complex with acetylacetone (Acac) was studied on mercury electrodes in the absence and in the presence of n-pentanol and n-octanol. In the inhibitor free solution and under conditions where Cd(Acac)2 complex predominated, the standard rate constant of the cadmium reaction was found to be 6.2×10−2 cm s−1. In the presence of inhibitors, it was determined from cathodic and anodic reaction orders with respect to Acac, that the Cd(I)(Acac) species reacted directly with the electrode. In the presence of n-pentanol and n-octanol adsorbed on electrodes, the electrode reaction of the Cdaq2+ | Cd(Hg) system with hydrated Cd2+ ions proceeds more than one order of magnitude slower than the reaction of Cd-acetylacetone complexes. The ionophoretic effect of Acac is postulated to be due to the interaction of the reactant with the adsorbed surface layer.

The kineticsand mechanism of the electrode process Cr II ) + 2e − = Cr(Hg) was investigated in LiBr + LiClO 4 solutions having constant water activity equal to 0.764. The concentration of LiBr was changed from 0 to 4.0 M. On the basis of the results obtained, the equilibrium constant of the CrBr + complex ( K 1 = 0.3 ± 0.1 M) was calculated. This value is higher than that of the chloride and lower than that of the iodide complex, which proves that the Cr 2+ ion is a soft cation. During electroreduction of the Cr 2+ ion in solutions of different water activity in the presence and in the absence of bromide ions, the following cathodic reaction orders were observed: −7.2, −5.9 and −1 for water in the absence of bromide ions, water in the presence of bromide ions and bromide ions, respectively. Since the hydration number determined was equal to 9.2 in bromide-free solutions, therefore the complex which undergoes a direct reduction at the electrode is weakly hydrated Cr(H 2 O) 2 2+ . A comparison of the rate constants of the Cr(II)|Cr(Hg) electrode reaction in solutions of perchlorate, chlorides, bromides and iodides, with various water activity reveals that the water activity is the most important factor which determines the rate constant of this process.

The electroreduction of 3-nitrophthalic acid anion on the mercury electrode in water + HMPA mixtures was studied with 0.5 M NaClO 4 and 0.05 M NaOH as electrolytes. A detailed kinetic study concerned one-electron reduction of 3-nitrophthalic acid anion to free radical. The change of the determined rate constants of this process on water + HMPA mixture composition was interpreted in terms of the solvent adsorption on the electrode and reagent solvation. An equation is proposed which describes the observed change of the kinetics.

Two different methods for solid-state electrochemical measurements in the absence of liquid electrolyte are discussed. The simplest approach is based on a two-electrode sandwich cell (without reference electrode), and it is suitable for ionically-conducting materials containing stable and chemically identifiable, mixed-valence redox sites (eg Fe(III,II) in Prussian Blue or Berlin Green). The second two-electrode design utilizes an ultramicrodisk working electrode which faces a large surface area silver-disk semireference/counter electrode. In order to discuss usefulness and limitations of these methods, we consider the following inorganic materials: Prussian Blue, Berlin Green, and silicotungstic acid single crystals. These structures contain mobile countercations (hydrated K + or H + ) in concentrations extensive enough to support diffusive transport of electrons hopping between Fe(III,II) or W(VI,V) centers (redox conduction). In the latter case, combination of potential step measurements in short-time and long-time experimental regimes provides an absolute electroanalytical method for determinations of redox centers and an effective diffusion coefficient for charge propagation.

The standard hydrogen electrode (SHE) acts as a primary reference in electrochemistry. The standard potentials of all other reference electrodes are linked to that of the SHE at the same temperature. The SHE contribution to the cell potential is by convention zero at all temperatures (see Chap. 1).

The electrooxidation of in situ produced electrolytically radical anion of 3-nitrophthalic acid in various water—ethanol solutions containing 0.5 M NaCIO4, 0.05 M NaOH and inhibitor has been studied. The inhibition of the electrode kinetics in the presence of n-octanol and n-decanol, used as inhibitors, at relative concentrations not exceeding c/cs ≤ 0.5 could be interpreted in terms of the competitive monolayer adsorption of reactant, inhibitor and solvent on the electrode surface. At c/cs > 0.8, on the capacitance-potential curves, a subtle minima caused by formation of two layers adsorbed on the mercury electrode were observed. The kinetics of the electrooxidation of the 3-nitrophthalic acid anion radical was additionaly influenced by this multilayer. An equation which describes the inhibition of the electrode process by two adsorbed layers of inhibitor is presented and used in the estimation of the surface coverage in the second layer.

The formal potentials and kinetic parameters for the electrode process Cr2+ + 2e−⇄Cr0 occurring at mercury electrode in solutions of LiClO4 + LiCl(aH2O = 0.741) and LiClO4 + LiI(aH2O = 0.853) were determined from analysis of irreversible anodic and cathodic chronocoulometric charge-potential curves. The interaction of Cr(II) with I− ions was found to be stronger (K1 = 1.6 M−1) than the very weak interaction with Cl− ions (K1 < 0.1 M−1). Double-layer properties were established for the solutions studied. On the basis of the rate constants, transfer coefficients, electrode reaction orders, double-layer properties and charges of the activated complex determined, a mechanism for the electrode reaction of the Cr2+/Cr(Hg) redox couple was proposed.

The orientation of adsorbed aliphatic alcohols on mercury electrode surface is discussed on the basis of literature data concerning steric factors of electrochemical reactions inhibited by these alcohols and on quantum chemical calculations using the mopac program. Steric factors were evaluated from dependences of rate constants of electrochemical reactions of several model systems on alcohol concentration at total surface coverage. Theoretical calculations were made for a single alcohol molecule interacting with a 28-atomic mercury cluster. These two sets of data point to a vertical orientation of adsorbed alcohol molecules, even at incomplete coverage of the electrode surface.

The influence of temperature over the range from −30 to 25°C on the electrochemical properties of solid iron(III) hexacyanoferrate(II/III) containing various amounts of water has been studied by means of cyclic voltammetry and impedance spectroscopy. The system studied is a water-insoluble mixed-valence coordination compound. The experiments have shown in major role for water molecules in the charge transport across this solid system. An attempt has been made to understand the experimental data on the basis of an existing model of redox conductance in solid mixed-valence transition metal hexacyanoferrates. The activation energy of charge migration in a partially dehydrated system and the activation energy of charge diffusion in a well-hydrated system have been determined.

The electrochemistry of wet solid Berlin green (BG) containing Na+ and K+ has been studied by voltammetry and chronoamperometry. It has been found that the reactions of both electroactive systems in BG, FeII/III cyanide complex and Fe2+/3+, are diffusion controlled. The charge diffusion coefficients in BG containing K+ are high and have been estimated as 2.2 × 10−8 cm2s−1 and 1.1 × 10−7 cm2s−1 under transient and steady-state conditions respectively. Evidence is provided that almost all redox sites in BG are electroactive. BG has been found to be nearly 1:1 mixed hexacyanoferrate(II)/(III).

The kinetics of the [Mn(CN) 6 ] 4− + e − ⇌ [Mn(CN) 6 ] 5− system at mercury electrodes has been investigated using cyclic voltammetry, chronocoulometric and faradaic impedance methods. The standard heterogeneous rate constant k s of this process in 1 mol dm −3 NaCN is 0.26 ± 0.01 5 cm s −1 and the cathodic transfer coefficient α is 0.59 ± 0.01, similar to the kinetic characteristics of the [Cr(CN) 6 ] 3− /[Cr(CN) 6 ] 4− system. The diffusion coefficient of [Mn(CN) 6 ] 4− in 1 mol dm −3 NaCN is (5.6 ± 0.8) × 10 −6 cm 2 s −1 . The role of the composition of the inner coordination sphere of manganese complexes in their electroreduction mechanism and the possibility of the further electroreduction process [Mn(CN) 6 ] 5− + e − → [Mn(CN) 6 ] 6− at mercury electrodes are discussed using literature data.

Intermetallic compounds of Pd with Hg were produced by simultaneous electrodeposition of palladium and mercury on platinum and carbon paste electrodes. Chronopotentiometric and linear potential scan voltammetric oxidation of such deposits revealed that oxidation of the individual compounds formed (PdHg, Pd 2 Hg 5 and PdHg 4 ) occurs in separate steps or peaks. It was proved that the whole deposit, not just its surface layers, is oxidized. Kinetic limitations were observed at higher current densities and scan rates. Oxidation of PdHg 4 and Pd 2 Hg 5 was found to proceed with the formation of PdHg as an intermediate. The Gibbs energies, enthalpies and entropies of formation of PdHg, Pd 2 Hg 5 and PdHg 4 were calculated from their deposition potentials determined at different temperatures.

Mercury hemispherical ultramicroelectrodes were used, in chronoamperometric studies, for the determination of the diffusion coefficient of thallium in its concentrated amalgams up to 1.2 M. The determination was based (1) on the amalgam oxidation limiting current density vs. time dependence and (2) on electroreduction of thallium (I) from its 0.1 M solution at potentials corresponding to the foot of voltammetric curves. In both cases the dependences of I 1 ( I ) vs. time were linear, with a slope dependent only on the diffusion coefficient and the square of the electrode radius. The diffusion coefficient values obtained are reliable.

The role of reactant size in the electrochemical kinetics of the series of europium complexes with nitrilo- N , N , N -triacetic acid (NTA), trans -1,2-diaminocyclohexane- N , N , N ′, N ′-tetraacetic acide (DCTA) and ethylenediamino- N , N , N ′, N ′-tetraacetic acid (EDTA) was studied in the presence of n -butanol and n -pentanol adsorbed on a mercury electrode surface. A rise in reactant size causes an increase in inhibiting influence of the adsorbate, expressed in the value r ≠ / r i , the steric factor. The orientation of non-symmetric reactant molecules, under such conditions, is that providing the smallest cross-sectional area on the electrode surface.

A model is proposed and supported with experimental data to describe solid-state electrochemical responses of transition metal hexacyanoferrate powders: K2NiIIFeII(CN)6/KNiIIFeIII(CN)6, KlnIIIFeII(CN)6/InIIIFeIII(CN)6 and Berlin Green (K1-x{FeIII[FeIII(CN)6]}x·{FeIII[FeII(CN)6]}1-x, where x

In this article, the chemical properties and thermodynamics of lead and its electrochemically important compounds are briefly described. Electrochemical behavior of lead and its technologically significant compounds, mainly oxides, in different media is reviewed, with special emphasis on voltammetric characteristics. More attention was paid to lead–acid batteries: construction, electrochemical properties, performance limitations, and new trends in the development of lead batteries.

The rate of the interfacial charge transfer in the V(III)/V(II) system at the mercury electrode in H2O+DMPU 1 +0.4 mol dm−3 HClO4 mixtures was found to increase when x DMPU was raised from 0.1 to 0.8. The solvatochromism of the electronic d-d transitions within the vanadium ions was used to leam about their resolvation with DMPU molecules. It was found that, under the experimental conditions used, the charge transfer occurs at the electrode surface which is already largely covered by DMPU (θDMPU = 0.9 to 1.0) and the interfacial kinetics are determined mainly by the solvation state of reactant in the bulk solution. Our observation of a close correspondence between log ks, and the reactant inner-shell composition can be considered as a result of the prevailing non-continuum contributions to the activation energy arising from the elimination of specific short-range, quo-ligand-solvent (hydrogen bond) interactions by coordinated DMPU molecules which are not hydrogen-bond donors. It seems that generally such effects could be kinetically significant also in other aqueous solutions of aprotic solvents (e.g. DMF, AN, HMPA).

The parameters α, β and γ of the equation WΔsGf(MX) = αBKT + βET + γ were calculated and analysed for different salts (MX) in pure solvents and in non-aqueous solvent–water mixtures (S). Among 109 different equations, only 64 were taken for the final analysis since in the case of 38 equations the parameters BKT and ET were highly correlated. After a statistical analysis and normalization, on the basis of the coefficients α and β obtained, it was found that the ions analysed may be divided into three classes characterized by the different dependences of α on β: class I, H+, Li+, Na+, Rb +, Cs+, Me4N+, Cl−, Br− and I−, where αN = 1.074βN + 1.639; class II, Ag+, Cl−, Br−, I−, OAc−, SCN− and N where αN = 2.057βN + 2.147; and class III, Ph4As+, BPh, Ph4C and Ph4Ge, where αN is variable and βN is almost constant. Two main conclusions can be drawn out from the results obtained: the behaviour of ions considered as Lewis acids and bases reflects different hard–soft properties of the ions, and the behaviour of the Ph4As+ ion is different from that of BPh.

The electroreduction of cadmium(II) at a mercury electrode and the oxidation of cadmium amalgam in 4.0 M NaCl at pressures ranging from 0.001 to 10 kbar, using cyclic voltammetry and chronoamperometry, revealed a moderate decrease in the limiting currents and diffusion coefficients of CdII in solution and Cd in mercury. The partial molar volume of the diffusion activation calculated from these dependences is equal to 1.1–1.2 and 0.93 cm3 mol−1 for diffusion in 4.0 M NaCl and in mercury, respectively. The formal potentials of the CdII/Cd(Hg) system expressed versus the ferrocene-ferricinium ion electrode as a function of pressure led to a value of 10.7 cm3 mol−1 for the volume of the electroreduction reaction of CdII.

The influence of single and mixed solvents on the rate of electrode reactions is discussed.

The mechanism of Ni2(CN)64− electro-oxidation at mercury electrodes is investigated using cyclic voltanunetric and chronocoulometric methods. Ni2(CN)64− (existing presumably in the form of various ion-pairs {Ni2(CN)64−, x Na+}) is surface-active and manifests itself by the formation of an anodic adsorption wave. In the absence of an excess of free ligand, surface-active nickel cyanide was formed as one of the products of Ni2(CN)64− electro-oxidation on mercury. It was found that one cyanide ion was consumed in the rate-determining step of the electrooxidation of each Ni2(CN)64− particle. Within the potential range of mercury oxidation to Hg(CN)p(2−p)+ and in the presence of both CN− and Ni2(CN)64− ions, small latent limiting currents are caused by the reaction 2 Ni(I) + Hg(II) → 2 Ni(II) + Hg(0) The scheme proposed for the participation of CN− ions in Ni2(CN)64− electro-oxidation was confirmed by the results of digital simulation of an appropriate model system.

The discharge of the lead citrate complex (PbL2−) on a mercury electrode covered by n-hexanol or n-heptanol molecules has been investigated by means of polarographic and chronocoulometric methods. The relation between the bulk surfactant concentration and the rate of the electrode reaction was examined. An average value of the steric factor r≠/ri equal to 4.0 ±0.2 was found for the cathodic electrode reaction occurring in aqueous solutions of sodium citrate containing aliphatic alcohols. The kinetic and mechanistic implications of an increase in the reactant size under such conditions are discussed.

Electrode processes involving the formation of a heterogeneous amalgam of iron during the electroreduction of Fe(II) ions on mercury and the oxidation of the iron amalgam were investigated by cyclic voltammetry, chronoamperometry and cyclic chronopotentiometry. The hanging mercury drop electrode and an iron plate placed on a mercury pool electrode were used in the experiments as working electrodes. It was established that particles of the electrodeposited iron are wetted by mercury and penetrate into the bulk of mercury electrodes forming a suspension. However, during electroreduction of Fe(II) ions from concentrated CaCl2 and Ca(ClO4)2 solutions a small amount of metallic iron remains on the surface of mercury. Oxidation of the heterogeneous amalgam of iron occurs at potentials about 100–150 mV less positive than the onset potential of mercury oxidation in the solutions studied. At these potentials oxidation of mercury may become significant enough to uncover some parts of the iron microcrystals. These iron particles become partially passivated and their surface energy at the Fe/solution interface decreases; consequently, the spreading coefficient of mercury on iron decreases, microcrystals of iron are expelled from mercury and finally oxidized.

The coordination model of ion solvation in mixed solvents was applied to evaluate solvation numbers of cations and reaction orders with respect to the organic solvent for electrode reactions in non-aqueous media. These values were calculated from linear dependences of the Gibbs energy of transfer and logarithms of electrochemical rate constants plotted against the logarithm of organic solvent activity. This method gives credible results, but only for highly basic solvents.

The sections in this article are Double-layer Properties of Cadmium Electrodes Electrochemical Properties and Kinetics of the Cd(II)/Cd(Hg) Systems Electrochemistry in Aqueous Solutions Kinetics of Simple Ions Influence of a Catalyst Influence of Inhibitors Electrochemistry in Mixed and Nonaqueous Solvents Electrochemical Properties of the Cadmium Complexes Determination of Stability Constants Electrochemical Preparation of Cadmium Complexes Preparation and Electrochemical Properties of Cadmium Chalcogenides CdS CdSe CdTe Properties of Cadmium Intermetallic Compounds Cadmium Underpotential Deposition and Electrodeposition on Solid Electrodes Deposition of Cd on Cadmium Electrode Electrodeposition of Cd on Other Solid Substrates Gold Platinum Silver Copper Silicon Other Substrates Passivation and Corrosion of Cadmium Passivation of Cadmium Electrode Corrosion of Cadmium Applied Electrochemistry Batteries Cadmium–Mercuric Oxide Primary Cells Cadmium–Nickel Oxide (Ni–Cd) Secondary Cells Cadmium–Silver Oxide Secondary Cells Application in Electrochemical Sensors Potentiometric Sensors Amperometric-voltammetric Sensors

The sections in this article are Double-layer Properties of Pb Electrodes Properties of Solid Electrodes Properties of Liquid Electrodes Adsorption on Solid Electrodes Electrochemical Properties and Kinetics of Lead and Lead Compounds Pb(II)/Pb(Hg) System Studies in the Presence of Inhibitors and Organic Solvents Other Phenomena Complexes of Pb(II) and Related Phenomena Electrochemical Processes of Liquid Lead in Molten Salts Voltammetric Behavior of Lead Sulfuric Acid Solutions Nitric Acid Solutions Phosphoric Acid Solutions Sodium Hydroxide Solutions Different Salt Solutions Voltammetric Behavior of Several Lead Compounds PbO PbO2 Pb chalcogenides Electrodeposition and Underpotential Deposition of Lead on Solid Substrates Platinum Gold Silver Copper Carbon Silicon Germanium Other Materials Corrosion and Passivation Applied Electrochemistry Lead-acid Batteries Electrocatalytic Properties Pb PbO2 Electrochemical Sensors Potentiometric Sensors Amperometric/Voltammetric Sensors

The sections in this article are Double-layer Properties of Zinc Electrodes Pc-Zinc in Aqueous Solutions Zn Single Crystals in Aqueous Solutions Electrochemical Properties and Kinetics of the Zn(II)/Zn(Hg) and Zn(II)/Zn Systems Electrochemistry in Aqueous Solutions Electrochemistry in Water-organic Solvent Mixtures Electrochemistry in Nonaqueous Solvents The Influence of Organic Compounds on the Electrode Processes The Electrochemical Properties of the Zinc Complexes Properties of Zinc Oxide Electrode Electrode Processes in Molten Salts Deposition and Underpotential Deposition of Zn on Solid Electrodes Underpotential Deposition of Zinc Zn UPD on Pt Zn UPD on Au Zinc Electrodeposition on Solid Electrodes Electrodeposition on Zn Electrodes Electrodeposition on Other Electrodes Passivation and Corrosion of Zinc Anodic Dissolution and Passivation of Zinc Corrosion Applied Electrochemistry Batteries Ni–Zn Cells Zn–Air Batteries Zn–MnO2 Batteries Zn–Ag Batteries Other Cells Electrowinning Zinc Electroplating Zinc Alloys Electroplating Electrochemical Sensors and Modified Electrodes Potentiometric Sensors Voltammetric/Amperometric Sensors Modified Electrodes

The sections in this article are Double-layer Properties of Hg/Water Interface Potential of Zero Charge Surface Charge Density and Capacitive Current Experimental and Theoretical Studies of the Hg/Water Interface Double-layer Properties of Hg/Nonaqueous Media Interface Adsorption and Electrode Reactions at Hg Surface Deposition and Underpotential Deposition of Hg on Various Electrodes Underpotential Deposition of Mercury on Gold Electrodes Film Electrodes and Related Hg Electrodes Adsorption and Electrode Reactions of Inorganic Ions and Coordination Compounds of Metal Ions Analytical Applications Adsorption and Electrode Reactions Involving Organic Compounds Organic Compounds Containing Sulfur, Selenium, and Tellurium Organic Nitrogen Compounds Indicators and Dyes Vitamins and Antibiotics Enzymes and Coenzymes Other Organic Compounds Analytical Aspects of Adsorption of Organic Compounds Ammonium and Quaternary-substituted Ammonium Amalgams

The sections in this article are Preparation of Au Surfaces and Double-layer Properties Polycrystalline (pc-Au) and Single-crystal Au/H2O Interface pc-Au and Single-crystal Au/Nonaqueous Solutions Interface Adsorption of Inorganic Compounds on Gold Electrodes Sulfate Hydroxide Nitrate Chloride Bromide Iodide Cyanide Thiocyanate Other Inorganic Species Adsorption of Organic Compounds on Gold Electrodes Adsorption of Sulfur-containing Compounds Adsorption of Thiols Adsorption of Modified Thiols Adsorption of Thiourea Adsorption of Disulfides and Related Compounds Other Sulfur Compounds and Complex Adsorption Layers Adsorption of Selenium-containing Compounds Adsorption of Nitrogen-containing Compounds Pyridine and its Derivatives Pyrazine Amines and Other Nitrogen-containing Compounds Adsorption of Other Organic Compounds Alcohols Aminoacids Other Organic Acids Nucleic Bases and Other Biochemical Compounds Other Compounds Reconstruction of the Surface of Gold Electrodes Formation of Oxides on Gold Electrodes Underpotential Deposition of Various Metals on Au Cu Cd Pd S, Se, and Te Sulfur Selenium Tellurium Bi Pt Ni Co Sb Sn Al Tl Pb Zn Ge Rh Li Fe Ag Hg Electrochemistry of Coordination Compounds of Gold. Electrodissolution and Electrodeposition of Au Au Electrodeposition Au Electrodissolution Gold Clusters

The sections in this article are Properties of Ag Electrodes Polycrystalline Ag Electrodes Preparation Surface and Double-layer Properties Single-crystal Ag Electrodes Preparation Surface and Double-layer Properties Surface Dynamics Affinity of Water and Nonaqueous Solvent Molecules to Ag Surfaces Adsorption of Inorganic Species on Ag Electrodes Halide Ions pc-Ag Electrodes Single-crystal Ag Electrodes Pseudohalide Oxygen and its Compounds Sulfur Compounds Inorganic Carbon Compounds Fullerenes Other Inorganic Compounds Metalocenes Adsorption of Organic Species on Ag Electrodes Hydrocarbons Pyridine and Other Nitrogen Compounds Carboxylic Acids Alcohols Sulfur Compounds Thiourea (TU) Alkanethiols and Self-assembled Monolayers Biochemically Important Compounds Adsorption on Modified Ag Electrodes Other Organic Compounds Electrode Processes with Participation of Silver Electrodes Reactions Involving Oxidation of Ag Surface Oxygen and its Compounds Sulfur Compounds Carbon Compounds Electrode Reactions of Selected Organic Compounds, Adsorbed on Ag Electrodes Biochemically Important Species Underpotential Deposition Processes Ag UPD on Ag Ag UPD on Au and Pt Pb Tl Ni Chalcogenides Other Elements and Compounds Electrodeposition and Electrodissolution Processes of Ag Electrodeposition Processes Electrodissolution Processes Silver Compounds at the Oxidation States Higher Than I

Voltocoulometric, chronocoulometric and cyclic voltammetric studies of the electrode reaction of Tl(2,2,2)+ cryptate at mercury electrodes are described. This process occurs via two parallel pathways – from the solution and from the adsorbed states which are energetically close. The kinetic and adsorption parameters of thallium(I) cryptate electroreduction were found by analysis of the normal pulse voltocoulometric curves recorded with a 1 ms delay after the application of the potential pulse. Such Qt−1-E dependences are characterized by a maximum that originates from the electroreduction of the adsorbed reactant. The model for numerical simulation of such curves was developed. Comparison of experimental and simulated curves allowed to determine apparent standard rate constant of Tl(2,2,2)+/Tl(Hg) couple as equal to 8×10−3 cm s−1, thus significantly lower than that for noncomplexed Tl+ /Tl(Hg) system. The stability constant of the Tl(2,2,2)+ complex (log K=6.70) and the surface coverage of the electrode by Tl+ were determined.