Cyclic Voltammetry Principle

Cyclic Voltammetry regulationCyclic voltammetry is the well-nigh widely employ technique for acquiring qualitative information ab come forth electro chemic chemical substance receptions 34, 35. The ability of cyclicalal voltammetry results from its ability to provide considerable information on the thermodynamicals and dynamics of compound negatron tilt replys 47, 48, and matesd chemical receptions 36, 37. It besides provides numeral analysis of an electron expatriation answer at an electrode 41, 49, 50.Basic Principle of Cyclic voltammetryAn electron beam play with a single measuring rod may be represented asO + ne R (2.1)where O and R be oxidized and reduced form of elector active species heedively, which either is soluble in solution or absorbed on the electrode come forth and are transported by diffusion al cardinal.Cyclic voltammetry consists of s idlerning li tight-fittingly the potence of a stationary working electrode (in an unstirred solution), us ing a 3-sided authorisation prosperform. Depending on the information sought, single or multiple cycles end be used. During the voltage dispute puff, the potentiostat measures the original resulting from the applied emf. The resulting plot of authoritative vs. possible is termed as cyclic voltammogram.The excitation signal in cyclic voltammetry is apt(p) in Fig. 2.1a. Initially the voltage of the electrode is Ei. therefore the probable is swept linearly at the reckon of volts per second. In cyclic voltammetry reversal technique is carried out by reversing direction of stare after a certain beat t = .The capableness at any cartridge holder E (t) is give byE (t) = Ei t tE (t) = Ei 2 + t t (2.2b)Here is rake treasure in V/s.The body-build of the resulting cyclic voltammogram peck be qualitatively explained as followsWhen voltage is append from the region where oxidized form O is stable, cathodic present-day(prenominal) starts to flux as potential approa ches E0 for R/O couple until a cathodic vertex is reached. After traversing the potential region in which the decline carry through takes fleck, the direction of potential sweep is twistd.The chemical reaction-taking place in the forward look butt joint be expressed asO + e- RDuring the move around s privy, R molecule (gene vaga stand byd in the forward one- half(a)(prenominal) cycle, and accumulated near the rebel) is reoxidized back to O and anodic tallness results.R O + e-In the forward scan as potential moves past Eo, the near-electrode concentration of O falls to zero, the mass transfer of O reaches a supreme evaluate, in unstirred solution, this regulate and then declines as the depletion of O come on and further from electrode takes place. Before trimping once again current passes through a maximum. coke of scan repeats the above sequence of events for the oxidation of electrochemically gene governd R that right off predominates in near-electrode regio n.The continuous change in the surface concentration is coupled with an expanding upon of the diffusion layer thickness (as expected in the quiescent solutions). The resulting current altitudes thus reflect the continuous change of the concentration gradient with time, and then, the increase to the visor current corresponds to the achievement of diffusion control, while the current drop (beyond the throwaway) exhibits a t-1/2 dependence ( free-lance of the applied potential). For the above reasons, the reversal current has the same shape as the forward one.electrochemical CellElectrochemical cell is a sealed vessel which is designed to prevent the first appearance of air. It has an inlet and outlet to allow the saturation of solution with an inert gas, N2 or Ar. Removal of O2 is usually necessary to prevent currents due to the reduction of O2 meddlesome with reaction from establishment under study. The type electrochemical cell consists of terce electrodes immersed in an e lectrolyteWorking electrode (WE)Reference electrode (RE)Counter electrode (CE)Working Electrode (WE)The performance of the voltammetric modus operandi is strongly influenced by the working electrode material. Since the reaction of interest (reduction or oxidation) takes place on working electrode, it should provide lavishly signal to noise characteristics, as well as a reproducible reaction. Thus, its selection depends primarily on ii factors the redox behaviour of the target analyte and the background current all over the potential region needful for the measurement. Other considerations include the potential window, electric conductivity, surface reproducibility, mechanical properties, cost, availability and toxicity. A range of materials thrust effectuate application as working electrodes for electroanalysis, the most popular are those involving mercury, speed of light or noble metals (particularly platinum and gold).Reference Electrode (RE)This go awayal electrode has a unceasing potential so it can be used as base standard against which potential of other electrode present in the cell can be metrical. Commonly used case electrodes are silver-silver chloride or the mercurous chloride electrode.Counter of Auxiliary Electrode (CE)It is as well as termed as auxiliary electrode and serves as source or sink for electrons so that current can be passed from impertinent circuit through the cell.The potential at WE is monitored and controlled very precisely with view to RE via potentiostat. This may be controlled in turn via interfacing with a information processing system. The desired undulationform is imposed on the potential at the WE by a beckonform generator. The potential drop V is usually measured by the current flowing amidst the WE and CE across a underground R (from which (I=V/R), the latter connected in series with the ii electrodes. The resulting I/V trace, termed as a voltammogram is then either plot out via an XY chart record er or, where possible, retained in a computer to allow any desired data manipulation prior to austere copy being taken.Single electron Transfer buttlead types of single electron transfer process can be canvas. correctable processIr correctable processQuasi- correctable processBased on think of of electrochemical parameters, i.e. head potential Ep, half account potential (Ep/2), half wave potential (E1/2), peak current (ip), anodic peak potential Epa, cathodic peak potential Epc etc, it can be ascertained whether a reaction is reversible, irreversible or quasi-reversible. Ep is the potential corresponding to peak current ip, Ep/2 is the potential corresponding to 0.5 ip, E1/2 is the potential corresponding to 0.85 ip. Theseelectrochemical parameters can be graphically obtained from the voltammogram as shown in the Fig. 2.2. bilateral ProcessThe motley transfer of electron from an electrode to a reducible species and vice versaO + ne Ris a form of Nernstian electrode reaction with assumption that at the surface of electrode, rate of electron transfer is so rapid that a dynamic touch oniser is established and Nernstian condition holds i.e.CO(0,t) CR(0,t) = Exp(nFRT)(Ei-t-Eo) (2.3)In comparability (2.3), Co and CR are concentration of oxidized and reduced species at the surface of electrode as a function of time, Eo is the standard electrode potential, Ei is the initial potential and is the scan rate in volts per second. Under these conditions, the oxidized and reduced species involved in an electrode reaction are in equilibrium at the electrode surface and such(prenominal) an electrode reaction is termed as a reversible reaction.Current Expression collectable to difference in concentration of electroactive species at the surface of electrode and the concentration in the bulk, diffusion controlled mass transport takes place. Ficks second law can be applied to obtain time dependent concentration distribution in one dimension of expanding diffusion lay er.Ci(x, t) t = Di2Ci(x, t) x2 (2.4)Peak current is a characteristic quantity in reversible cyclic voltammetric process. The current smell is obtained by solving Ficks law 51.i = nFACo*(Doa)1/2 (at) (2.5)where i = current, n = number of electrons transferred, A is the area of electrode, Co* is the bulk concentration of oxidized species, Do is the diffusion coefficient, (at) is the current function and a = nF/RTAt 298K, function (at) and the current potential persuade reaches their maximum for the reduction process at a potential which is 28.5/n mV much negative than the half wave potential i.e. at n(Ep-E1/2) = 28.50 mV, 1/2(at) = 0.4463 ( Table 2.1). Then the current normal for the forward potential scan becomes(2.6)where ip is the peak current or maximum current.Using T=298K, Area (A) in cm2, Diffusion coefficient (Do) in cm2/s, concentration of species O (Co*) in moles dm-3 and Scan rate () in volts sec-1, equation (2.6) takes the adjacent form,(2.7)Equation (2.7) is called Randles Sevick equation 39, 40.Diagnostic Criteria of Reversibility received well-defined characteristic mensurates can be obtained from the voltammogram, for a reversible electrochemical reaction.Relationship amongst peak potential (Ep) and half wave potential (E1/2) for a reversible reaction is tending(p) by,(2.8a)(2.8b)Where E1/2 is potential corresponding to i = 0.8817ip 41.At 298 K(2.8c)From equations (2.8a) and (2.8b) one obtains,(2.9a)At 298K(2.9b)The peak voltage position does not alter as scan rate varies. In some cases, the precise design of peak potential Ep is not easy because the observed CV peak is somewhat broader. So it is some propagation more than convenient to report the potential at i = 0.5ip called half peak potential, which can be used for E1/2 determination 52.(2.10a)At 298 K(2.10b)(2.10c)From equations (2.8a) and (2.10a) we obtain,(2.11a)At 298K(2.11b)The diagnostic criterion of single electron transfer reversible reaction is often sufficient to get qu alitative as well as quantitative information about the thermodynamic and energizing parameters of the system.For a reversible system, should be independent of the scan rate, however, it is found that by and large increases with . This is due to presence of finite solution resistance amongst the reference and the working electrode.Irreversible ProcessFor a totally irreversible process, reverse reaction of the electrode process does not occur. Actually for this type of reaction the fool away transfer rate constant is quite small, i.e. ksh 10-5cm sec-1, hence weight down transfer is exceedingly low and current is mainly controlled by the rate of charge transfer reaction. Nernst equation is not applicable for such type of reaction.The process can be best described by the side by side(p) reactionO + ne RDelahay 51 and later on Mastuda, Ayabe 48, and Reinmuth 53 described the stationary electrode voltammetric curves of the irreversible process.Irreversibility can be diagnosed by three major criteria.A shift in peak potential occurs as the scan rate varies.Half peak width for an irreversible process is given by(2.12)Here is transfer coefficient and na is the number of electrons involved in rate determining step of charge transfer process.At 298K(2.13)Current port is given as,i = nFACo*(Dob)1/2 (bt) (2.14)The function (bt) goes through a maximum at 1/2(bt) = 0.4958.(Table 2.2).Introduction of this value in equation (2.14) yields the expression (2.15) for the peakcurrent.A plot of ln ip vs. (Ep-Eo) for different scan rates would be a straight line with a hawk proportional to -naF and an intercept proportional to ks,h.Quasi-reversible ProcessQuasi-reversible process is termed as a process which shows intermediate behaviour between reversible and irreversible processes. both charge transfer and mass transfer control current of the reaction. For quasi-reversible process value of standard diversified electron transfer rate constant, ks,h lies between 10-1 to 1 0-5 cm sec-142. Cyclic voltammogram for quasi-reversible process is shown in Fig. 2.3.An expression relating the current to potential dependent charge transfer rate was first provided by Matsuda and Ayabe 48.(2.17)where, ksh is the assorted electron transfer rate constant at standard potential Eo of redox system,is the transfer coefficient and = 1- .In this case, the shape of the peak and the various peak parameters are functions of and the dimensionless parameter , defined as 54(2.18)For quasi-reversible process current value is expressed as a function of.(2.19)where is expressed as(2.20)is shown in Fig. 2.4. It is observed that when 10, the behavior approaches that of a reversible system.It is observed that for a quasi-reversible reaction, ip is not proportional to 1/2. For half peak potential we haveat 298K (2.21)This implies,These parameters attain limiting set characteristic of reversible or totally irreversible processes as varies. For 10, (,) = 2.2 which gives Ep-Ep/2 = 56.5mV (value characteristic of a reversible wave). For Variation of with and is shown in Fig. 2.5.For three types of electrode processes Matsuda and Ayabe 48 suggested following zone boundaries.a) reversible (Nernstian)15 ksh 0.3 1/2cm s-1b) Quasi- reversible15 10-2 (1+) 0.3 1/2 ksh 2 10-5 1/2 cm s-1c) Totally Irreversible fount Bard, A.J. Faulkner, L.R. Electrochemical Methods, Fundamentals and Applications, tin can Wiley, New York, 1980, pp 225.Source Bard, A.J. Faulkner, L.R. Electrochemical Methods, Fundamentals and Applications, John Wiley, New York, 1980, pp 227.Multi negatron Transfer ProcessMulti-electron transfer process usually takes place in two separate steps. devil-steps tool, each step characterized by its own electrochemical parameters is called EE machine.Stepwise reversible EE mechanism is given by following reaction,A + n1e B (E10) (2.22a)B + n2e C (E20) (2.22b)where, A and B are electroactive species and n1 and n2 are the number of electrons i nvolved in successive steps. If A and B react at sufficiently separated potentials with A more easily reducible than B, the voltammogram for overall reduction of A to C consists of two separated waves. The first wave corresponds to the reduction of A to B with n1 electrons and in this potential range the fondness B diffuses into the solution. As potential is scanned towards more cathodic values, a second wave appears which is made up of two superimposed parts. The current related to substance A, which is still diffusing toward electrode increases since this species now is reduced directly to substance C by (n1+n2) electrons. In addition, substance B, which was the crossroad of the first wave, can be reduced in this potential region and a portion of this material diffuses back towards the electrode and reacts.Each heterogeneous electron transfer step is associated with its own electrochemical parameters i.e. ks,hi and i, where i =1, 2 for the 1st and 2nd electron transfer respectiv ely.Based on the value of Eo, we come across three different types of cases 50 as shown in the Fig. 2.6.Types of Two Electron Transfer Reactions 50Case 1 Separate PeaksWhen Eo -150mV the EE mechanism is termed as disproportionate mechanism 55. Cyclic voltammogram consists of two typical one-electron reduction waves. The heterogeneous electron transfer reaction may simultaneously be accompanied by homogenous electron transfer reactions, which in multi-electron system leads todisproportionation. Each disproportionation reaction can be described as,2R1 O+ R2 (2.23)The equilibrium constant K (disproportionation constant) is given by(2.24)It can be derived from the difference between the standard potentials using (2.25)Case 2 In this case, the soulfulness waves merge into one broad distorted wave whose peak tiptop and shape are no longer characteristics of a reversible wave. The wave is broadened similar to an irreversible wave, but can be distinguished from the irreversible voltammog ram, in that the distorted wave does not shift on the potential axis as a function of the scan rate.Case 3 = 0mV Single peakIn this case, in cyclic voltammogram, only a single wave would appear with peak current intermediate between those of a single step one electron and two electron transfer reactions and Ep-Ep/2 = 21 mV.Case 4 E1o If the energy required for the first second electron transfer is less than that for the first, one wave is observed having peak height equal to 23/2 times that of a single electron transfer process. In this case, Ep E1/2 = 14.25 mV. The hard-hitting E0 for the composite two electron wave is given by 50.Source Polcyn, D.S. Shain, I. J. Anal. Chem. 1966, 38, 370.Cyclic Voltammetric Methods for the Determination of Heterogeneous Electron Transfer Rate constant quantityCyclic voltammetry provides a systematic approach to solution of diffusion problems and determination of different kinetic parameters including ks,h. Various modes are reported in books t o determine heterogeneous rate constants. Nicholson 41, 42, Gileadi 56 and Kochi 37 developed different equations to calculate heterogeneous electron transfer rate constants.Nicholsons Method 41, 42Nicholson derived an expression for determination of heterogeneous electron transfer rate constant ksh. This method is based on correlation between and ks,h through a dimensionless parameter by following equation,(2.26)where is scan rate.for different values of Ep can be obtained from the Table 2.3. Hence, if Ep (Epa-Epc) is persistent from the voltammogram, can be known from Table 2.3. From the knowledge of, , ksh can be calculated using equation (2.27).If D o= DR then =1(2.27)This method is applied for voltammograms having peak separation in the range of 57mV to 250mV, and between this range, the electrode process progresses from reversible to irreversible. With increasing scan rate, the peak separation and hence decreases.It can be seen from the Table 2.3, that for reversible reacti ons i.e. for the current voltage curves and is independent of . For totally irreversible reaction i.e. for the back reaction becomes un classic, anodic peak and is not observed. For quasi-reaction i.e. for 0. 001Separation of cathodic and anodic peak potential as a function of the kinetic parameter in the cyclic voltammogram at room temperature.Kochis MethodKochi and Klinger 37 develop another correlation between the rate constant for heterogeneous electron transfer and peak separation.The expression for ksh given by Kochi was(2.28)The standard rate constant ksh can be calculated from the difference of peak potentials and the sweep rates directly. This equation applies only to sweep rates which are large enough to induce electrode irreversibility. The relation derived by Kochi is based on following expressions derived by Nicholson and Shain 41.(2.29a)(2.29b)where = 1- , and is the scan rate.Equations (2.29a) and (2.29b) yield(2.30)This expression is used for the determination of the transfer coefficient. Assuming that (for reversible reaction).We have,(2.31)Gileadis MethodGileadi 56 formulated a more sophisticated method for the determination of heterogeneous electron transfer rate constant, ks,h, using the idea of slender scan rate, c. This method can be used in the case where anodic peak is not observed.When reversible heterogeneous electron transfer process is studied at increasing scan rates, peak potential values in any case vary and process progresses towards irreversible. If are plotted against the logarithm of scan rates, a straight line at low scan rates and raise curve at higher scan rate is obtained. Extrapolation of both curves intersects them at a point known as toe. This toe corresponds to the logarithm of critical scan rate, c. as shown in Fig. 2.7. Hence critical scan rate can be calculated experimentally.ks,h can be calculated as,(2.32)where c is the critical scan rate, is a dimensionless parameter, called transfer coefficient and Do i s the diffusion coefficient. mate Chemical ReactionsAlthough charge transfer processes are an important part of entire spectrum of chemical reactions, they seldom occur as isolated elementary steps. Electron transfer reactions coupled with new bond formation or bond breaking steps are very frequent. The occurrence of such chemical reactions, which directly affect the available surface concentration of the electroactive species, is common to redox processes of many important organic and inorganic compounds. Changes in the shape of the cyclic voltammogram resulting from the chemical competition for the electrochemical reactantor product, can be extremely useful for elucidating the reaction pathways and for providing reliable chemical information about reactive intermediates 35.It is convenient to classify the different possible reaction schemes in which athe likes of reactions are associated with the heterogeneous electrons transfer steps by using garner to signify the nature of th e step. E represents an electron transfer at the electrode surface, and C represents a homogenous chemical reaction. While O and R shew oxidized and reduced forms of the electroactive species, other non electroactive species which result from the coupled chemical branching are indicated by W, Y, Z, etc 57. The order of C with respect to E then follows the chronological order in which the two events occur 58. So correspond to sequence of step, the systems are classified as EC, ECE, CE etc. These reactions are further classified on terms of reversibility. For exemplification, subclasses of EC reactions can be distinguished depending on whether the reactions are reversible (r), quasi-reversible (q), or irreversible (i), for example Er Cr, ErCi, EqCi, etc.Two Steps Coupled Chemical ReactionsIn two steps reactions, a variety of possibilities exist, which include chemical reactions following or antecedent a reversible or an irreversible electron transfer 59, 60, 61, 62. The chemical reactions themselves may be reversible or irreversible.a) forward Chemical Reactions (CE)In a prior chemical reaction, the species O is the product resulting from a chemical reaction. Such a reaction influences the amount of O to be reduced so forward peak is perturbed. For a foregoing chemical reaction, two mechanisms are possible, depending on whether the electron transfer is reversible CrEr or irreversible CrEi 58.Reversible Electrode Process Preceded by a Reversible Chemical Reaction(CrEr Reaction)The process in which a homogeneous chemical reaction precedes a reversible electron transfer is schematized as follows(2.33)where Y represents the non electroactive species and O and R are the electroactive congeners.Since the supply of electroactive species O results from the chemical reaction, it is important to know that how much of O is formed during the time scale of cyclic voltammogram. In this connection, it must be noted that the time scale of voltammetry is measured by the parametera = nF/RT for a reversible processand b = naF/RT for a quasi reversible or an irreversible processIt agent that the time scale of cyclic voltammetry is a function of the scan rate, in the sense that higher the scan rate, the higher is the competition of the voltammetric intervention with respect to the rate of chemical complication.The limit at which the chemical complication can proceed is governed either by the equilibrium constant K or the kinetics of the homogeneous reaction (l = kf+kr). In this regard, it is convenient to distinguish three limiting cases depending on the rate of chemical complication 41. relax preceding chemical reaction (kf+kr When K is large (i.e. K 20) most of O will already be present in solution, the solvent is apparently not disturbed by the latter, i.e. it appears as a simple-minded reversible electron transfer.When K is small, the small electron transfer again appears as a simple reversible process except that the peak current will be smal ler than is expected on the basis of quantity of Y in the solution. This results because the concentration of the electroactive species CO, being determined by the equilibrium of the preceding reaction is equal to a fraction of species Y placed in the solution.where C* = CO (x,0) +CY(x,0)Fast preceding chemical reaction (kf+kr nF/RT)When K is large, once again the response appears as a simple reversible electron transfer, but the measured standard potential Eo/* is shifted toward more negative values compared to the standard potential Eo/ of the couple O/ R by a factor of .When K is small, because of the unfaltering continuous maintaining of the small equilibrium amount of O, the complete depletion of O at the electrode surface will never be reached, so that the forward visibility no longer maintains the peak shape form, rather assumes a sigmoid S-shaped curve, the height of which remains constant at all scan rates. mediocre preceding chemical reaction (kf+kr = nF/RT)In this case , the kinetics can be studied using the ratio between the kinetic and the disseminative currents according to the relationship(2.34)Irreversible Electrode Process Preceded by a Reversible Chemical Reaction(CrEi Reaction)This process is schematizes as.(2.35)In this case, not only the thermodynamic K (kf / kr) and kinetic (kf + kr) parameters of preceding chemical reaction but also the kinetic parameters of the electron transfer (, k0) play a role. Obviously the neglect of reverse peak is immediately apparent, due to the irreversibility of the charge transfer. The curves are also more drawn out because of the electron transfer coefficient, .Slow preceding chemical reaction (kf+kr In this case, the process appears as a simple irreversible electron transfer. The peak height of the process depends on the equilibrium constant because, as mentioned in the previous case, the concentration of the active species CO is a fraction of the amount C* put in the solutionFast preceding chemical re action (kf+kr nF/RT)If preferably the reaction kinetics is fast, there are two possibilitiesIf K is large, again the response appears as if the preceding chemical reaction would be absent. However, the peak potential is shifted towards more negative values than those that would be recorded in the absence of the chemical complication by a factor equal to .If K is small, as in the preceding case, an easily recognizable S-like curve voltammogram is obtained having a limiting current independent from the scan rate(2.36) mean(a) preceding chemical reaction (kf+kr = nF/RT)Here again, the kinetics can be studied using the ratio between the kinetic and disseminative currents according to the relationship(2.37)b) Following Chemical Reactions (EC)The process in which the primary product of an electron transfer becomes involved in a chemical reaction is indicated by EC mechanism. It can be represented byO + ne RR Z (2.38)where O and R are the electroactive congeners and Z represents the non electroactive species.Several situations are possible depending on the result of electrochemical reversibility of the electron transfer and on the reversibility or irreversibility of the chemical reaction following the electron transfer.As a general criterion, in cyclic voltammetry, the presence of a following reaction has little influence on the forward peak, whereas it has a considerable effect on the reverse peak.Reversible Electrode Process Followed by a Reversible Chemical Reaction(ErCr Reaction)ErCr mechanism can be written as(2.39)Once again the voltammetric response will differ to a greater or lesser conclusion with respect to a simple electron transfer depending on the values of either the equilibrium constant, K, or the kinetics of the chemical complication (kf+kr) 58.analogously to that discussed for preceding equilibrium reactions, three limiting cases can be distinguished.Slow following chemical reaction (kf+kr If the rate of chemical reaction is low, it has a lit tle effect on the process, thus reducing it a simple reversible electron transfer.Fast following chemical reaction (kf+kr nF/RT)If the rate of the chemical complication is high, the system will perpetually be in equilibrium and the voltammogram will apparently look like a non complicated reversible electron transfer. However, as a final result of the continual partial removal of the species R from the electrode surface, the reduction occurs at potential values less negative than that of a simple electron transfer by an amount of .Due to the fast kinetics of the chemical complication, the potential will remain at this value regardless of the scan rate. negociate following chemical reaction (kf+kr=nF/RT)If the kinetics of the chemical reaction are intermediate with the scan rate the response gradually shifts from previous value for a fast chemical reaction which was more anodic by w.r.t. to value of the couple O/R towards the Eo/ value assuming more and more the values predicted by the relationship(2.40)In other words, the response (which for the fast kinetics is more anodic compared to E0/) due to the competitive do of the potential scan rate moves towards more cathodic values by 30/n (mV) for every ten fold increase in the scan rate. However, it is noted that at the same time, the reversible peak tends to disappear, in that on increasing the scan rate, the species Z does not have time to restore R. This is demonstrated by the current ratio which is about one at low scan rates, but it tends to zero at high scan rates.Reversible Electrode Process Followed by an Irreversible Chemical R