BY-NC-ND 3.0 license Open Access Published by De Gruyter April 30, 2013

Electroanalytical chemistry of lanthanides and actinides

Paul D. Schumacher, Jamie L. Doyle, James O. Schenk and Sue B. Clark

Abstract

The electrochemical properties of lanthanides (Ln) and actinides (An) are reviewed. This review summarizes papers from 1986 to 2011 with a primary focus on the electrochemical and redox properties of Ln/An elements in aqueous solution and their responses to a variety of electrode materials including Hg, Hg films, solid electrodes, modified carbon paste, and microelectrodes. A section is also devoted to the electrochemical properties and responses of Ln and An in nonaqueous and mixed solvent systems.

Introduction

Electroanalytical chemistry is a general term covering a wide variety of techniques that investigate the electrical properties of an electroactive analyte in solution. Electroanalytical techniques have many advantages over other detection systems, namely low cost, low detection limits, tunability to specific oxidation states for an analyte, and characterization of electrochemical information for the system under study (Skoog etal. 1997). Some of the information includes, but is not limited to, kinetics, rates and amounts of adsorption, stoichiometry, and rates of electron transfer (Skoog etal. 1997). Conducting a literature search on the electrochemistry of f-elements yields relatively few references. The reason for this scarcity of research is that although lanthanides (Ln) and actinides (An) are electroactive, their electrochemical properties are challenging to exploit, especially in aqueous solutions (Gao 1986).

Historically, the separation of trivalent f-elements has been a challenge due to similarities in their chemical behavior, making the determination of individual members of the f-element group difficult by electroanalytical techniques with only a few exceptions (Gao 1986, Nash and Jensen 2000). Despite these difficulties, progress has been made; new radioelectroanalytical approaches developed in the last 20 years have focused on exploiting the redox behavior of Ln and An to facilitate their separation. A review of current knowledge regarding the electrochemical properties is thus warranted. There are a number of acronyms used throughout this article, and a list of all acronyms used is included in Table 1 to aid the reader.

Table 1

List of acronyms.

AcronymFull description
LnLanthanides
AnActinides
ILIonic liquids
H/SMDEHanging/static mercury drop electrode
DMEDropping mercury electrode
MFEMercury film electrode
CPCarbon paste
MCPModified carbon paste
18-Crown-61,4,7,10,13,16-Hexaoxacyclooctadecane
CVCyclic voltammetry
ASVAnodic stripping voltammetry
GCGlassy carbon
PVCPolyvinylchloride
LSVLinear sweep voltammetry
ISEIon-selective electrode
LODLimit of detection
MWCNTMultiwalled carbon nanotubes
HIBAα-Hydroxyisobutyric acid
TBAN-(1-Thia-2ylmethylene)-1,3-benzothiazole- 2-amine
HDEBHN′-(2-Hydroxy-1,2-diphenylethylidene) benzohydrazide
BMIM1-Butyl-3-methylimidazolium
EMITFSI1-Ethyl-3-methylimidazolium bis(trifluoromethylsulfonyl)imide
BMPTFSI1-n-Butyl-1-methylpyrrolidinium bis(trifluoromethylsulfonyl)imide
PIPESPiperazine-N,N′-bis(2-ethanesulfonic acid)

Summary of previous reviews of Ln and An electrochemistry

In 1966, the electrochemistry of Ln and An was reviewed by Ryabichicov and Ryabukhin, as translated by Aladjem (1970). In 1976, Herman and Rairden did an extensive review of Sc, Y, and Ln. Their review focused on the polarography in both aqueous and nonaqueous solutions along with polarographic characteristics and kinetic properties. O’Laughlin’s (1979) short review on the polarography of Ln focused on separation and determination techniques and concluded that polarography was not an ideal technique for separation given the similar chemistries. In 1986, Gao reviewed the polarography of rare earths, focusing on detection via the addition of complexing ligands. More recently, Binnenmans (2007) review discussed the effects of solution conditions in ionic liquids (ILs) on Ln and An electrochemistry. Information on the reaction of f-elements with water was also provided, which suggested that pure metals cannot be deposited electrochemically in ILs.

Mudring and Tang’s (2010) review covered the electrochemistry of Ln and An in ILs. Findings include deposit morphology, temperature dependence, deposition potential, and redox potentials for U along with other f-elements. In general, the review supports the use of ILs as electroanalytical solvents due to their wide electrochemical range, large ion conductivity, and ability to dissolve the f-elements. Because ILs were only recently reviewed, the focus of this review is to summarize the progress on electrochemistry of Ln and An since 1986, emphasizing aqueous and mixed solvent solutions.

Early voltammetric assessments of the f-elements

Since Professor Jaroslav Heyrovsky invented the polarographic method in 1922, Hg has been the electrode material of choice for investigations in the negative potential window (Galus and Meites 1975). Thus, nearly all early electroanalytical assessments of the f-elements were completed using pure mercury electrodes, typically a hanging mercury drop electrode (HMDE) or dropping mercury electrode (DME). These mercury electrodes were desirable for radiopolarographic analysis, a technique in which drops were collected and the concentration of analyte was determined via nuclear counting (Samhoun and David 1979, David etal. 1981). Mercury can be advantageous for these techniques, as these electrodes are known to provide a rapidly renewable and smooth surface and a high overpotential for hydrogen, thus extending the potential range in aqueous solutions, and it has the ability to form amalgams, or more specifically, alloys with one or more metals (Kowalski etal. 1987, Mikkelsen and Schroeder 2003). The overpotential value for hydrogen has been reported at -0.85 V in aqueous solution (Bard and Faulkner 2001). However, this value is dependent on solution conditions because each elementary step in an electrochemical mechanism is subject to contributions from resistance, concentration, ionization, and polarization overpotentials creating variability in measurements (Ammar and Hassanein 1960). The mercury overpotential was advantageous during aqueous f-element studies based on the inherent reduction potentials of these elements; however, most early works on Ln and An were not done in purely aqueous media. Early voltammetric analysis of these metals was done in the presence of a complexing ligand, such as 1,4,7,10,13,16-hexaoxacyclooctadecane (18-Crown-6) or acetate (Maly 1967, David and Bouissieres 1968, Sipos and Galus 1971, Herman and Rairden 1976, Yamana etal. 1983). The addition of complexing ligands allows for observations of the redox properties of f-element metals because the metals interact with the ligand at the electrode surface, typically at a less negative potential than would be observed for the f-element cation. Several works observed the existence of a divalent state and the ability of these metals to form amalgams in their presence (David and Bouissieres 1968, Herman and Rairden 1976). A review of the f-elements by Herman and Rairden (1976) indicated that the reduction of the Ln and An is not a simple process, with several references to works noting hydrogen gas formation and/or hydride and oxide formations, all with contributions to the voltammetric signals observed.

Later electroanalytical assessments shifted to new modified electrodes with better sensitivity, stability, and lower environmental toxicity. These electrodes included the mercury film electrode (MFE) and the modified carbon paste (MCP). Commonly, the MFE based on glassy carbon (GC) is chosen for electroanalytical studies due to the substance’s chemical inertness, useful potential range, low residual current, readily renewable surface, and low cost (Economou and Fielden 2003); however, other base materials have been and can be used for a wide variety of applications. Besides the utility of the electrode, the mercury content of solutions tested with this electrode held considerable lower mercury contamination, which became an important characteristic as electroanalysis of environmental samples became more prominent. As the desire to reduce mercury from electroanalysis arose, the MCP became more widely used. The many current utilities and modifications of carbon paste (CP) have been reviewed in the current millennium by Švancara etal. (2009). Similar to their pure mercury predecessors, both MFE and MCP have proven to be very effective in the determination of redox characteristics of the f-elements in a range of solution conditions. A summary of some of these applications and findings is presented later.

As this review is broken down by electrode types, it is useful to include a table of working potential ranges for the different electrodes. Table 2 is a summary of the potential ranges. Upon observation, two points are worth noting. First, Hg has a larger negative potential window than the other elements, thus its wide usage with Ln and An. Second, the potential range expands when the electrode material is used in nonaqueous solvents.

Table 2

Summary of electrode potential ranges.

MaterialTypeConditionsE range (V)MetalsReferences
Mercury
HMDEAcetone/18-Crown-60.4 to -2.3EuGao and Guan 1988
HMDENaClO4-1.2 to -1.5YbXiaoquan etal. 2000
HMDEKMnO4-1.2 to -1.5YbXiaoquan etal. 2000
DMECCl4/TMACl-2 to -2.4AcYamana etal. 1983
DMEKMnO4-1.15 to -1.55YbXiaoquan etal. 2000
DMEMordant red/ammonium buffer-0.5 to -1TbLee etal. 1997
DMEAcetate buffer/mordant blue-0.2 to -1UWang and Zadeii 1987
DMEPIPES/SVRS-0.8 to -1.2YbWang and Zadeii 1986
DMEAqueous-2 to 1.84Cf/Gd/SmMusikas etal. 1981
Hg poolAcetate buffer5Cf/Es/FmMaly 1967
Hg poolAqueous-1.6 to -2.8LnYamana and Moriyama 1997
MFENafion/NH4Cl0 to-1.5EuUgo etal. 1991
MFENafion/NH4Cl or in NH4NO30 to -1.5YbUgo etal. 1991
MFEKNO3/chloranilic acid-0.05 to 0.25UPiech etal. 2007
MFELiCl-2.5 to 1.5LnSchumacher etal. 2010
Carbon
MCP-HIBALiCl0.8 to -0.4LnSchumacher etal. 2011a–c
Sal-SAMMSAcetate buffer or NH4Cl0 to -0.95EuYantasee etal. 2006
CPAcetate buffer-0.3 to -0.8HoLi etal. 2004
CPAcetate buffer-0.3 to -0.8CeLi etal. 2006
CPNaAc-Hac/KHP buffer-0.3 to -0.9CeLiu etal. 2005
MCP-MWCNTKCl-0.02 to 0.18TbGanjali etal. 2010
MCP-MWCNTKCl0.05 to 0.25ErNorouzi etal. 2010
MCP-MWCNTKCl-0.02 to 0.28HoGanjali etal. 2009
MCP-MWCNTKCl0 to 0.16HoFaridbod etal. 2010
GraphiteCs2NpCl6/HMPA0 to -2NpMartinot etal. 1995
GraphiteCs2NpCl6/DMF0 to -3.5NpMartinot etal. 1995
GCBMPTFSI or EMITFSI1 to -1.5EuYamagata etal. 2006
GCBMPTFSI0 to -2YbYamagata etal. 2006
GCBMPTFSI0 to -3SmYamagata etal. 2006
GCMolten NaCl-2CsCl-0.5 to -2.1UNagai etal. 2005
Carbon fiberHIBA/LiCl-0.5 to 1.5CeToyoshima etal. 2008
Carbon fiberLiCl-2.5 to 1.1LnSchumacher etal. 2011a–c
Platinum
PtThCl4/molten DMSO-0.15 to 0.65ThMartinot etal. 1995
PtCs2NpCl6/molten DMSO0 to -2.3NpMartinot etal. 1995
PtMolten DMSO2/Cs2UO2Cl40 to -1.5UO2Martinot etal. 1990
PtMolten DMSO2/Cs2UCl60 to -1.3UMartinot etal. 1990
Gold
Au fiberH3PO4-0.4 to 1.4LnPourjavid etal. 2009a,b
Au fiberH3PO4-1 to 2LnPourjavid etal. 2010
Au fiber0 to 0.14LnGanjali etal. 2007

Amalgamation studies of f-elements

Between the 1950s and the 1990s, most electroanalytical investigations of f-elements involved polarographic or radiopolarographic analysis of amalgams with an Hg pool serving as the working electrode or cathode. These studies were carried out in a controlled pH range of 2.0–4.0 (David and Bouissieres 1968, Musikas etal. 1981, Yamana etal. 1983, David etal. 1990a,b, Yamana and Moriyama 1997, 1998), except for David etal. 1990a,b, who conducted studies in the 6.0–7.0 range. Background electrolytes were typically 0.1–1.0 m alkali metal chlorides or perchlorates (David and Bouissieres 1968, Musikas etal. 1981, Yamana etal. 1983, David etal. 1990a,b, Yamana and Moriyama 1997). Several studies also used the complexing ligands of citrate and acetate (David and Bouissieres 1968, David etal. 1990a,b) or 18-Crown-6 (Yamana etal. 1983, Yamana and Moriyama 1997, 1998).

A few observations become apparent as a result of analyzing amalgamation studies. Several investigators discovered and confirmed the stable divalent oxidation states for various An because amalgamation techniques give the reduction potentials from the most stable oxidation state (David and Bouissieres 1968, Musikas etal. 1981, David etal. 1990a,b, Yamana and Moriyama 1997). In general, An were found to reduce via a two-step mechanism compared with a single-step process for Ln. A direct correlation was observed between the reduction potential of the metal and the stability constant of any metal-ligand complex in solution. Amalgamation was also observed to follow a first-order kinetic rate expression. As amalgamation techniques report reduction potentials from the most stable oxidation state in solution to amalgamated metallic states in mercury, one would expect to observe large negative potentials to overcome the stability of the metallic oxidation state of the f-element. Table 3 confirms that large negative potentials are required for Ln/An reduction. Table 3, which is a compilation of electrochemical information from Bard etal. (1985), David etal. (1990a,b), and Yamana and Moriyama (1997) shows that the reduction of the metals are well within the potential window for hydronium reduction, which leads to a large background current and makes operating in aqueous solutions challenging. Although general metal reduction schemes are proposed, it is noteworthy that these are based on the comparison of cyclic voltammetry (CV) and have not been subjected to a rigorous kinetic investigation for validation. As amalgamation experiments are time-consuming, i.e., hundreds of minutes, the technique is not ideally suited for kinetic measurements. However, other electroanalytical techniques that operate on shorter timescales could provide mechanistic information. Additionally, the CVs show that in the case of Ln, a potential mechanism for reduction based upon a previously reviewed work (Herman and Rairden 1976) is as follows (Musikas etal. 1981):

Table 3

Summary of electrochemical data of Ln and An with Hg electrodes.

ElementMetallic radius (Å)aMediumbpHbE0, V vs. SHEcE1/2 vs. SHEbE1/2 vs. NHEaMechanismb
La1.88-2.38-1.75
Ce1.830.1 m LiClO42.2/3.2-2.34-1.84±0.01-1.833→0 irr
Pr1.83-2.35-1.88d
Nd1.82-2.32-1.83d
Pm1.81-2.29-1.79d
Sm1.800.1 m LiClO42.95/3.65-2.30-1.72±0.01-1.712→0 irr
Eu2.040.1 m LiClO43.0/5.8-1.99-1.71±0.01-1.702→0 r
Gd1.800.1 m LiClO44.0/5.5-2.28-1.78±0.01-1.783→0 irr
Tb1.780.1 m LiClO43.3/3.4-2.31-1.74±0.01-1.733→0 irr
Dy1.77-2.29-1.79d
Ho1.770.1 m LiClO4-2.33-1.78±0.01-1.773→0 irr
Er1.76-2.32-1.74d
Tm1.75-2.32-1.73d
Yb1.940.1 m LiClO42.0/3.5-2.22-1.81±0.01-1.812→0 irr
Lu1.740.1 m LiClO43.5-2.30∼-1.69-1.683→0 irr
Ac1.882.5/3.2-2.21e-1.96±0.02-1.913→0 irr
Th-1.83
Pa1 m HCle-1.47
U1.540.005 m (CH3)Cl41.5/3-1.65-1.65±0.05-1.653→0 irr
Np1.50-1.77e-1.78d
Pu1.52-2.00-1.99d
Am1.730.1 m LiCl1.8/2.25-2.07-1.60±0.01-1.723→0 irr
Cm1.740.1 m LiCl1.8/2.26-2.06-1.61±0.01-1.773→0 irr
Bk1.700.1 m LiCl1.8/2.27-2.00-1.63±0.01-1.633→0 irr
Cf1.690.1 m LiCl1.8/2.28-1.91-1.51±0.01-1.513→0 r
Es1.980.1 m LiCl1.8/2.29-1.98-1.46±0.01-1.463→0 r
Fm1.970.1 m LiCl2.4-2.07-1.49±0.01-1.473→0 irre
Md0.1 m LiCl2.4-1.74-1.51±0.013→0 irre
No-1.26e
Lr-2.06e

aYamana and Moriyama 1997.

bDavid etal. 1990a,b.

cBard etal. 1985.

dEstimated from Yamana and Moriyama 1997.

eUpdated from Edelstein etal. 2010.

irr, irreversible; r, reversible.

2Ln3+ + 2H2O + 2e- ↔ 2LnOH2+ + H2

LnOH2+ + 2H2O + 2e- ↔ Ln(OH)3 ↓ + H2

Although this potential mechanism accounts for many of the observations that occur in the reduction of Ln and An, to date, there is no consensus on the actual elementary steps of the mechanism. It may be stated, based on the previously mentioned reviews, that Ln reduce via a one-step 3 e- transfer (Herman and Rairden 1976). Another possibility is that charge transfer could potentially occur through a ligand bridge. The fact that halide anions can cause anion-induced adsorption on Hg is well known (Bard and Faulkner 2001). As seen in Tables 2 and 3, halide anions are used as supporting electrolyte, although other supporting anions such as perchlorate are also used. It would be worthwhile to explore the effects of supporting electrolyte on the reduction mechanism of Ln and An. Regardless, knowing the actual mechanism would greatly enhance our ability to develop an electrochemical separation technique, as technological advances allows us to work at ultratrace levels.

Electrochemistry of f-elements on Hg and Hg film electrodes

The next studies utilize a DME (Ugo etal. 1991, Tamrakar and Pitre 2000), hanging/static mercury drop electrode (H/SMDE) (Wang and Zadeii 1986, 1987, Lee etal. 1997, Xiaoquan etal. 2000, Piech etal. 2007), or MFE (Ugo etal. 1991, Piech etal. 2007, Schumacher etal. 2010, 2011b,c) to detect f-elements (Wang and Zadeii 1986, 1987, Ugo etal. 1991, Lee etal. 1997, Tamrakar and Pitre 2000, Xiaoquan etal. 2000, Piech etal. 2007) or pre-concentrate (Schumacher etal. 2010, 2011a–c) f-elements. Solution and sample compositions varied from environmental analysis to neat solutions. The pH range and background electrolyte concentration/composition, shown in Table 4, are in general agreement with amalgamation studies. The most prevalent technique used for detection of Ln and An was anodic stripping voltammetry (ASV), with sweep and potentiostatic techniques used in the pre-concentration studies (Schumacher etal. 2010, 2011a–c).

Table 4

Summary of electrochemical data of Ln and An on mercury films.

MetalElectrodeE (V)Background electrolyteDetection limit (m)WaveformReferences
YbDME/SMDE-1.480.1 m NaClO410-7LSPXiaoquan et al. 2000
Eu/YbMFE (Nafion)-0.67/-1.50.1 m NH4NO310-8DPVUgo etal. 1991
La, Eu, Tb, YbHMDE-0.7 to -0.81.0 m NH3 buffer10-10ASVLee etal. 1997
Y, Dy, Ho, YbHMDE-1.000.02 m PIPES10-10ASVWang and Zadeii 1986
La, Nd, Eu, Gd, Ho, LuMFE-2.200.1 m LiCl10-11LSVSchumacher etal. 2010
UDME-0.240.1 m KSCN10-12DPASVTamrakar and Pitre 2000
UHg(Ag) film-0.80.1 m KNO310-10DPSVPiech etal. 2007
UHMDE-0.560.05 m Ac buffer10-10ASVWang and Zadeii 1987

The general observations for DME, H/SMDE, and MFEs are that Ln and An exhibit linear accumulation at the surface of the electrode until saturation is achieved. In the case of Ln, the sequence of film formation in situ (i.e., the formation of the mercury film with the analyte present and adsorbing during film formation) vs. ex situ (i.e., the formation of the mercury film with no analyte present in solution and the analyte added to solution after film formation) lowered the detection limits by well over an order of magnitude in the case of ex situ (Schumacher etal. 2010, 2011a–c). Although this phenomenon was observed, the reason for this behavior is still under investigation. Changing the background electrolyte anion improved the detection limits for An (Tamrakar and Pitre 2000). Exploiting the electrochemistry of the complexing ligand improved the detection of Ln and An down to the ultratrace level at much higher pH range (6.0–9.0) (Wang and Zadeii 1986, 1987, Lee etal. 1997). Not unexpectedly, the use of ASV lowers the detection limit for both Ln and An by up to four orders of magnitude, and it is possible to detect down to the subnanomolar range (Wang and Zadeii 1986, 1987). Depending on solution conditions, sweep waveforms can be preferential to differential pulse. The use of DME, H/SMDE, or MFEs allows the timescale of analysis to dramatically decrease compared with amalgamation studies. Most experiments required only minutes to detect or pre-concentrate compared with hours for the amalgamation studies. One of the benefits of this decrease in experimental time is that it now allows for the kinetic study of the reduction mechanism. Although each of these electrochemical techniques is sensitive, it is not possible to determine any isotopic information via the use of electroanalytical techniques. If isotopic information is desired, as would be the case in nuclear forensic analysis, a follow-on detection method such as radiometric counting or mass spectrometry would be required to elucidate the isotopic abundances (Schumacher etal. 2010).

The role of pH is of concern when working with Ln and An. Above pH 5.0, metal hydrolysis and precipitation becomes the dominant reaction in solution when working with Ln and An in an aqueous solution (Nash and Jensen 2000). This limits the pH range in which electroanalytical measurements can be made. At low pH values, background current from water hydrolysis increases at the negative potentials required to reduce Ln and some An. This increase in background current can make analyte signal determination problematic and challenging. Additionally, H2 gas evolution also increases, which can cause disruptions in the formation of an Hg film. Some thought must therefore be given to determine the optimal pH to conduct experiments.

A final note on observable trends when working with Hg: the presence of O2 in solution will oxidize the surface of Hg, thus reducing the effective surface area available. All working solutions are typically purged with an inert gas, such as Ar, before conducting any experiments. During experiments, the inert gas is blown over the solution in the electrochemical cell to minimize O2 interference during the conduct of the experiment.

Solid electrodes

Given the inherent toxicity of Hg, there is growing interest in pre-concentrating and/or detecting and separating Ln and An with other electrode materials. Solid electrodes for detection of Ln and An include Pt-, Ti-, and C-based electrodes. Voltammetric responses vary with the electrode material used, thus opening a larger untapped field of study.

It should be noted that within this field of solid electrodes, an entire series of studies that deal with Ln and An in organometallic complexes has been published. These ligands have multiple redox centers; thus, it is difficult to elucidate the electrochemical characteristics of the Ln and An from those of the ligands. Therefore, this review acknowledges this body of work, but it is excluded from further discussion here because they constitute an independent field of study.

The studies reviewed cover the solid electrodes graphite (Kayasth 1993), Ti (Kim etal. 1994), GC (Clark etal. 2006, Yuan etal. 2006, Liezers etal. 2009), and a polyvinylchloride (PVC)-based ion-selective electrode (ISE) (Tyagi etal. 2010). Solution compositions varied from seawater to blood serum and were generally in the acidic pH range (<6.0). One of the major findings is that in 4% NaCl solutions, Ln exhibit a tendency to electrodeposit on graphite electrodes at potentials much lower than predicted by the Nernst equation (Kayasth 1993). Clark etal. (2006) followed by Liezers etal. (2009) were able to pre-concentrate, separate, and detect attomolar levels of Pu and U on an anodized GC electrode using inductively coupled plasma mass spectrometry by exploiting the unique electrochemical properties of U and Pu. By modifying a GC electrode with carbon nanotubes and a Nafion coating, Yuan etal. (2006) detected Eu3+ in an environmental sample via the Eu3+/Eu2+ redox couple. The technique showed enhanced selectivity for Eu3+, although other rare earths also were adsorbed. Tyagi etal. (2010) developed a Eu3+ ISE utilizing p-tert-butylcalix[4]arene derivative (L) on a PVC-based electrode. This ISE was applicable over a large pH range and would operate both in aqueous and nonaqueous solutions.

These studies highlight that although the electrochemical properties of Ln and An in aqueous solution can be challenging to exploit, creative solutions abound. An interesting observation deserving further systematic investigation is the underpotential deposition, a term coined by Herzfeld in 1914 on graphite which was observed by Kayasth in 1993. Kayasth observed that more than 60% of Ln present was able to adsorb to a 2-mm graphite rod in a stirred solution of 4% NaCl at pH 1.5. The removal from the electrode was accomplished by stirring in 2 m HNO3. Although no kinetic parameters were measured, the rate of adsorption is slow, given the electrolysis time (∼15 h); however, if the mechanism of adsorption could be elucidated, then the possibility of potentially finding a catalyst to speed the reaction is available. The works of Clark etal. (2006) and Liezers etal. (2009) are good examples of how incorporating the electrochemical properties of An in an analytical process can greatly improve the chemical separations for follow on detection eliminating the need for multiple chemical separation steps. Yuan etal. (2006) is an excellent example of how modifications to an electrode can increase the sensitivity and selectivity for a particular analyte. By modifying the GC electrode with a carbon nanotube-Nafion film, the sensitivity to Eu3+ increased (Yuan etal. 2006). The properties of nanotubes will be discussed in the next section. In the case of Tyagi etal. (2010), incorporating a permselective membrane with an ionophore that is sensitive to Eu3+ opens a whole new avenue in the realm of sensor development for Ln and An,and will be discussed further in the following section.

Carbon and modified CP

CP electrodes are now widely used in electrochemical research. Many factors contribute to their popularity: low ohmic resistance, large potential window, and ease of modification, to name a few (Arrigan etal. 1994, Švancara etal. 2009, Vytras etal. 2009). Given the large negative reduction potentials required for Ln and An, one creative approach to pre-concentrate and/or detect f-elements is to exploit the redox properties of a metal-ligand complex through CP modification, which occurs in a more positive potential region as was highlighted earlier (Wang and Zadeii 1986, 1987, Lee etal. 1997); MCP electrodes are ideally suited for this type of approach (Li etal. 2004, 2006, Liu etal. 2005, Yantasee etal. 2006, Ganjali etal. 2009, 2010, Faridbod etal. 2010, Norouzi etal. 2010, Schumacher etal. 2011a–c). Table 5 summarizes the types of modifications and their results. CP electrodes can be modified in several ways including chemical pretreatment, in situ modification, dissolution in the binding liquid, or direct mechanical mixing of dry modifiers into the paste (Stozhko etal. 2008).

Table 5

Summary of electrochemical data of Ln from CP and MCP electrodes.

Metal(s)ElectrodeDetection level (m)Background electrolyteTime (s)References
LaMCP (HIBA)10-15LiCl300aSchumacher etal. 2011a–c
CebCP10-6HAc-NaAc/KHP120aLi etal. 2006
CebMCP (cetyltrimethylammonium)10-10HAc-NaAc/KHP120aLiu etal. 2005
EuScreen printed carbon sensors10-9NH4Cl180–600aYantasee etal. 2006
TbMCP ([BMIM]BF4, MWCNTs, L)c10-8Tb salts16Ganjali etal. 2010
HoMCP (ionophore, MWCNTs, nanosilica)10-8Ho salts10Ganjali etal. 2009
HoMCP (TBA, MWCNTs)b10-6Ho nitrate/acetonitrile13Faridbod etal. 2010
ErMCP (HDEBH, MWCNTs, [BMIM]BF4, nanosilica)c10-8Er salts16Norouzi etal. 2010
Sm, Eu, Tb, Ho, Yb, YbCP10-10HAc-NaAc120aLi etal. 2004

aCation pre-concentration; others represent detection time for sensor.

bSolution mixture of the cation(s) with alizarin complexone.

c L, N′-(2-Napthoyl)-8-(dimethylamino)naphthalene-2-sulfonohydrazide.

One major advantage of using an MCP electrode with f-elements is that it provides a more selective surface for separations. Work has been done using the preferential binding of Ln to the modifiers in MCPs; for example, Liu etal. (2005) created an MCP with two modifiers that increased the selectivity for Ce3+ when optimized to a limit of detection (LOD) for Ce3+ of 10-9m. In addition to increasing the selectivity for individual Ln, work has also been focused on production of ISEs for Ln using multiwalled carbon nanotubes (MWCNT), nanosilica, and room temperature ILs along with ionophores as modifiers (Ganjali etal. 2009, 2010, Faridbod etal. 2010, Norouzi etal. 2010). The use of MWCNTs is growing because there are many advantages to the use of these structures as modifiers, such as their unique electronic structures, electrical conductivity, high specific surface area, and strong adsorptive abilities (Yuan etal. 2006). Overall, these MCP electrodes display remarkable selectivity and serve as durable sensors for Ln.

Another advantage to MCP electrodes is their potential in pre-concentration and detection of Ln and An. Luckily, this topic is one ripe for exploration. Work has been done with a variety of ligands, pasting liquids, and electroanalytical techniques showing little variation in results due to carbon’s ability to be an inert conductor. Specifically, Schumacher etal. (2011) has done work using α-hydroxyisobutyric acid (HIBA) as a modifier that could pre-concentrate as little as 3.6×10-11mol/m3of an f-element mixture (Schumacher etal. 2011a–c). Although previous work has shown carbonaceous material to be just as effective in pre-concentration, the use of an MCP significantly reduces the time needed for reaction from hours of contact to minutes (Faridbod etal. 2010, Schumacher etal. 2011a–c). As a final note, although all of these experiments were done under aqueous conditions, MCP electrodes can be used in nonaqueous/mixed solvent environments as well, further expanding their usefulness in Ln and An electrochemical analysis.

Microelectrodes

Microelectrodes, conventionally defined as electrodes with active dimensions in the tens of micrometers or less, have gained wide acceptance within the field of electrochemistry, due to their distinct advantages over conventionally sized (∼3 mm) electrodes, namely, low ohmic drop, fast response times, and steady-state currents along with enhanced sensitivity due to mass transport by radial diffusion (Wightman 1981, Wehmeyer and Wightman 1985, Wojciechowski and Balcerzak 1990, Fungaro and Brett 1999). This enhanced sensitivity has led to applications for trace and ultratrace level analysis of metal cations in a large variety of solutions and volumes. The small size also allows for the development of electrode arrays that can further increase measurement sensitivity.

Some observations from these studies involving microelectrodes include validation of one proposed mechanism for Ln reduction at a mercury film using a mercury film microelectrode (Schumacher etal. 2011c). Others include the quantitative determination of Ln with an Au microelectrode, the examination of current changes due to adsorption at high scan rates (Pourjavid etal. 2009a,b), and the development of an electrochemical flow-through cell for rapid analysis of heavy elements using a Nafion-coated carbon fiber (Toyoshima etal. 2008). The flow-through cell was validated with 1010 Ce3+/Ce4+ atoms in solution. Lastly, the development of a Lu3+ microsensor that exhibited characteristics similar to previously discussed ISEs (Ganjali etal. 2009, 2010, Norouzi etal. 2010), with the LOD lowered by two orders of magnitude and the validation of sensor operation in aqueous and binary solutions (Ganjali etal. 2007).

The unique characteristics of microelectrodes facilitate detailed investigations into mechanisms and electrochemical properties of Ln and An that are not easily obtained with conventionally sized electrodes. Using a microelectrode allows the researcher to operate in small volumes with enhanced sensitivity providing a wider array of experiments with radionuclides at lower concentration levels and in a larger variety of solution compositions. Conversely, operating at low levels requires a much larger emphasis on minimizing sample contamination; however, the benefits outweigh the effort required. The ability to incorporate a microelectrode electrochemical detector to a separation technique as discussed by Toyoshima etal. (2008) and Pourjavid etal. (2009a,b) has numerous potential applications within the field.

Although electrochemical detection is already widely used for separation instruments, microelectrodes provide for more rapid analysis with higher sensistivity and could prove potentially useful in examining the redox properties of shorter-lived radionuclides where relatively small amounts of material are produced. Implied in the previous statement is the understanding that a method exists to transfer the radionuclides from a production chamber to an electroanalytical apparatus. Toyoshima etal. (2008) provides a good starting description of how such an apparatus might operate.

Electrochemical studies in nonaqueous and mixed solvent solutions

A modest amount of research has been conducted on the electrochemical properties of Ln and An in nonaqueous solvents as a result of developing new methods for the reprocessing of spent nuclear fuels (Martinot etal. 1990) and in mitigating the large background signal from H3O+ reduction (Chlistunoff and Galus 1985). Although one drawback to nonaqueous solvents is the lack of solubility of inorganic cations in organic solvents, one of the greatest inherent advantages is the expansion of the electrochemical window, which can easily reach 5.0 V in the case of hexamethylphosphoramine (Martinot etal. 1990). Table 6 lists the variation in solutions and the observed reduction potentials. When compared with the previous tables, a clear shift in potentials is observed. Choosing a nonaqueous solvent requires a balance between a high enough donor number to allow the properties of the solvent to be compared from the standpoint of ion solvation (Elzanowska etal. 1983) while ensuring that shift in cathodic potential does not exceed the solvent limit.

Table 6

Summary of electrochemical data of Ln and An in nonaqueous solution.

MetalE (V)aBackground electrolyteMechanismTemperature (°C)ElectrodeReferences
Ce-1.752BMIM Cl3 to 070PtRao etal. 2010
Sm-1.41BMIM Cl3 to 070PtRao etal. 2010
Eu-0.3EMITFSI3 to 225GCEYamagata etal. 2006
Eu-0.269BMPTFSI3 to 225GCEYamagata etal. 2006
Eu-1.762BMIM Cl3 to 270PtRao etal. 2010
Yb-0.993BMPTFSI3 to 225GCEYamagata etal. 2006
Th-1.8[(n-C4H9)(CH3)3N]-[Tf2N]4 to 025GCEBinnenmans 2007
Tb-2.359LiCl-KCl eutectic4 to 0450GCEBinnenmans 2007
U-1.481NaCl-2CsCl4 to 3650GCENagai etal. 2005

aPotentials are temperature dependent.

One advantage to working in nonaqueous media is the observed potential shift. Elzanowska etal. (1983) suggested that the donor number is directly correlated to the shift. The larger donor number correlated with an increase in reorganization energy (λ). The activation energy for reduction is increased as a result of the increased λ and larger potentials are necessary for the reduction of Ln and An. Many others have observed this shift in their work (Gao and Guan 1988, Martinot etal. 1990). One study by Chlistunoff and Galus (1985) found that the addition of DMF to an aqueous solution resulted in a cathodic shift, with slight alterations in slope and shape of Eu voltammograms. Although the addition of a non-aqueous solvent altered the voltammograms by changing solution conditions, Trubachev (2003) suggested that the correlation between the donor and the coordination number and redox shifts could be used to predict changes in specified solution conditions.

Besides shifting the redox potentials of Ln and An, nonaqueous solvents have been shown to support the presence of oxidation states not normally observed under aqueous conditions. The presence of these species has been attributed to the complexation with either the nonaqueous solvent itself or with an added complexing ligand. Gao and Guan (1988) found that addition of 18-Crown-6 produced a greater stability of the Eu2+ state. Another example is the disproportion of U(V), which readily occurs in an aqueous solution is stabilized in organic solvents and leads to a decrease in the rates of reaction (Martinot etal. 1992, Suzuki etal. 2007). Other work citing this phenomenon with uranium include discussions on kinetic parameters and changes in pH or acid (Martinot etal. 1992, 2002, Suzuki etal. 2007, Elkechai etal. 2009).

Alternative f-element oxidation states

A majority of An can exhibit stable oxidation states different from the expected trivalent state of Ln with the exception of Eu and Ce. Although other states are possible, only a few are commonly observed. Trivalent states are common for Ac, Am, Cm, Bk, Cf, Es, Fm, Md, and Lr in aqueous solution, whereas the tetravalent state is common for Th, U, and Pu. Other An, such as Pa, U, Np, and No, can be stable in aqueous solutions in higher or lower oxidation states (Cotton 2006). The less common oxidation states can be observed experimentally under the specified conditions. Radiopolarographic studies performed in aqueous media observed slopes above the expected 20 mV for Fm, suggesting a mechanism that exchanges two electrons per mole, leading to the identification of divalent Fm as a stable oxidation state (Samhoun and David 1979). Similarly, divalent Md was identified by slope analysis (David etal. 1981).

To confirm the existence of alternate oxidation states in solution, complexing agents and/or alternative nonaqueous medium can be used. David et al. (1981) confirmed the divalent state of Fm by citrate complexation. In the presence of citrate, the half-wave potentials of Fm are shifted similarly to Mn2+-citrate complexation, increasing the likelihood of the Fm divalent state. Additionally, the differences between a trivalent and divalent citrate complex can be discerned based on the ion’s affinity for complexation. Besides complexation with a ligand, the interactions of these metals in non-aqueous media can stabilize alternative oxidation states. Uranium metal can be observed from electrochemical reduction in γ-BL/THF (Martinot etal. 2002). The oxidation of U(III) to (IV) and (IV) to (V) was observed in THF and Bu4NPF6 with a platinum electrode. Although the oxidation was reversible, the evidence of the existence of the (V) state was detected (Elkechai etal. 2009). The U(V) state was also observable in perchloric acid solution and noticeably stable in the presence of malonic and oxalic acid (Suzuki etal. 2007). Lastly, working in nonaqueous solutions allows for a greater potential window, which allows for the more negative reduction potentials to be attained, increasing the accessibility of alternative An oxidation states (Cotton 2006).

Stabilizing and observing less common An oxidation states can also be done with alternative analytical techniques. For environmental samples, oxidation states can be determined by ion chromatography (Coates etal. 2001). In a few cases, certain oxidation states cannot be differentiated, particularly if the matrix conditions do not support one state. An and Ln compounds in unusual oxidation states can also be formed through specified synthetic routes. The use of superoxidizers and superacids has been shown to produce Pu(VI) and Pr(IV) compounds, and oxidation states of VI, V, IV, and III have been stabilized for multiple An in perovskite complexes (Eller and Penneman 1987). In general, the higher and lower uncommon oxidation states can be stabilized in cubic complexes or polymer-type structures, such as ternary oxides, binary oxides, binary fluorides, and oxyfluorides (Eller and Penneman 1987).

Conclusion

Since the mid-1980s, much progress has been made on determining the electrochemical properties of Ln and An in both aqueous and nonaqueous solutions. In both solvents, large negative potentials are required to reduce these elements to their metallic state. These electrochemical properties are susceptible to variances in the solution conditions that need to be carefully controlled. Because of the similarity of electrochemical properties, the separation and detection of individual Ln and An within a mixture are difficult to achieve solely by electroanalytical techniques; however, advances in technology have facilitated the development of separations in some circumstances when combining electroanalytical techniques with other separation techniques. CP electrodes represent a very appealing avenue to pursue in terms of pre-concentration, individual detection and/or separation within a mixture due to their ease of modification, and the large variety of ligands that can be incorporated into the paste. Advances in microelectrode technology allow for electrochemical analysis on a per-atom basis, which provide promise in furthering separation and detection research regarding Ln and An. It will be interesting to see what advances are made within the fields of radiochemistry and electroanalytical chemistry as technology and knowledge increase.


Corresponding author: Sue B. Clark, Department of Chemistry, Washington State University, Pullman, WA 99164, USA

P.D.S. acknowledges the support of the US Army while in residence at Washington State University. All the authors acknowledge funding from the Academic Research Initiative of the Joint Domestic Nuclear Detection Office, Department of Homeland Security, and the National Science Foundation, for funding under grant numbers ECCS-0833548 and DN-077-ARI-03302. In addition, S.B.C. acknowledges support from the US Department of Energy, Office of Science, Heavy Elements Program, grant number DE-SC-0004102. We also gratefully acknowledge two reviewers whose constructive comments helped us to improve this manuscript significantly.

References

Aladjem, A. Analytical Chemistry of Yttrium and the Lanthanide Elements; Ann-Humphrey Science: Michigan, 1970. Search in Google Scholar

Ammar, I. A.; Hassanein, M. Hydrogen overpotential on Cadmium. J. Phys. Chem. 1960, 64, 558–560. Search in Google Scholar

Arrigan, D. W. M.; Svehla, G.; Harris, S. J.; McKervey, M. A. Use of calixarenes as modifiers of carbon paste electrodes for voltammetric analysis. Electroanalysis1994, 6, 97–106. Search in Google Scholar

Bard, A. J.; Faulkner, L. R. Electrochemical Methods: Fundamentals and Applications; Wiley: New York, 2001. Search in Google Scholar

Bard, A. J.; Parsons, R.; Jordan, J. Standard Potentials in Aqueous Solutions; Dekker: New York, 1985. Search in Google Scholar

Binnenmans, K. Lanthanides and actinides in ionic liquids. Chem. Rev.2007, 107, 2592. Search in Google Scholar

Chlistunoff, J.; Galus, Z. Electrode reactions at extremely negative potentials. J. Electroanal. Chem.1985, 193, 175–191. Search in Google Scholar

Clark, W. J.; Park, S. H.; Bostick, D. A.; Duckworth, D. C.; Van Berkel, G. J. Electrochemically modulated separation, concentration and detection of plutonium using an anodized glassy carbon electrode and inductively coupled plasma mass spectrometry. Anal. Chem.2006, 78, 8535–8542. Search in Google Scholar

Coates, J. T.; Fjeld, R. A.; Paulenova, A.; DeVol, T. Evaluation of a rapid technique for measuring actinide oxidation states in ground water simulant. J. Radioanal. Nucl. Chem.2001, 248, 501–506. Search in Google Scholar

Cotton, S. Lanthanide and Actinide Chemistry; John Wiley & Sons: West Sussex, UK, 2006. Search in Google Scholar

David, F.; Bouissieres, G. Comparative formation of amalgams of transuranium elements and rare earths by electrolysis. Inorg. Nucl. Chem. Lett.1968, 4, 153–159. Search in Google Scholar

David, F.; Samhoun, K.; Hulet, E. K.; Baisden, P. A.; Dougan, R.; Landrum, J. H.; Lougheed, R. W.; Wild, J. F.; O’Kelle, G. D. Radiopolarography of mendelebium in aqueous solutions. J. Inorg. Nucl. Chem.1981, 43, 2941–2945. Search in Google Scholar

David, F.; Maslennikov, A. G.; Peretrukhin, V. P. Electrochemical reduction of actinide ions in aqueous solution. J. Radioanal. Nucl. Chem.1990a, 143, 415–426. Search in Google Scholar

David, F.; Peretrukin, V. F.; Maslennikov, A. G.; Fourest, B. Electrochemical reduction of actinides to amalgams in aqueous solutions and some examples of its application. Radiochim. Acta1990b, 50, 39–46. Search in Google Scholar

Economou, A.; Fielden, P. Mercury film electrodes: developments, trends and potentialities for electroanalysis. Analyst2003, 128, 205–212. Search in Google Scholar

Edelstein, N. M.; Fuger, J.; Katz, J. J.; Morss, L. R. Summary and Comparison of Properties of the Actinide and Tranactinide Elements. In: The Chemistry of the Actinide and Transactinide Elements Edition; 3rd Edition. Morss, L.; Edelstein, N. M.; Fuger, J., Eds. Springer: The Netherlands, 2010, 3, p. 1779. Search in Google Scholar

Elkechai, A.; Boucekkine, A.; Belkhiri, L.; Amarouche, M.; Clappe, C.; Hauchard, D. A DFT and experimental investigation of the electron affinity of the triscyclopentadienyl uranium complexes Cp3UX. Dalton Trans.2009, 15, 2843–2849. Search in Google Scholar

Eller, P. G.; Penneman, R. A. Stabilization of actinides and lanthanides in unusual oxidation states. J. Less Common Metals1987, 127, 19–33. Search in Google Scholar

Elzanowska, H.; Galus, Z.; Borkowska, Z. Electro-donicity of the solvents and kinetics of simple electrode reactions. The Eu(III)/Eu(II) couple in common solvents. J. Electroanal. Chem. 1983, 157, 251–268. Search in Google Scholar

Faridbod, F.; Ganjali, M. R.; Larijani, B.; Hosseini, M.; Norouzi, P. Ho3+ carbon paste sensor based on luti-walled carbon nanotubes: applied for determination of holmium content in biological and environmental samples. Mater. Sci. Eng.2010, 30, 555–560. Search in Google Scholar

Fungaro, D. A.; Brett, C. M. A. Microelectrode arrays: application in batch-injection analysis. Anal. Chim. Acta1999, 385, 257–264. Search in Google Scholar

Galus, Z.; Meites, L. Electrochemical behaviors of metal amalgams. Crit. Rev. Anal. Chem.1975, 4, 359–422. Search in Google Scholar

Ganjali, M. R.; Norouzi, P.; Adergani, B. A.; Riahi, S.; Larijani, B. An asymmetric lutetium(III) microsensor based on N-(2-furylmethylene) pyridine-2,6-diamine for determination of lutetium(III) ions. Anal. Lett.2007, 40, 1923–1938. Search in Google Scholar

Ganjali, M. R.; Kazemi, N. M.; Norouzi, P.; Khoee, S. A modified Ho3+ carbon paste electrode based on multi-walled carbon nanotubes (MWCNTs) and nanosilica. Int. J. Electrochem. Sci.2009, 4, 906–913. Search in Google Scholar

Ganjali, M. R.; Ganjali, H.; Hosseini, M.; Norouzi, P. A novel nano-composite Tb3+ carbon paste electrode. Int. J. Electrochem. Sci.2010, 5, 967–977. Search in Google Scholar

Gao, X. Polarographic Analysis of the Rare Earths. In: Handbook on Physics and Chemistry of Rare Earths; Gschneidner, K. A.; Eyring, L., Eds. Elsevier: New York, 1986, pp. 163–201. Search in Google Scholar

Gao, X.; Guan, F. Electrochemical studies on the complexation of rare earth elements with crown ethers. Kexue Tongbao1988, 33, 748–752. Search in Google Scholar

Herzfeld, K. F. Physik Z.1914, 14, 29. Search in Google Scholar

Herman, H. B.; Rairden, J. R. Scandium, Yttrium and the Lanthanides. In: Encyclopedia of Electrochemistry of the Elements; Bard, A. J. Eds. Dekker: New York, 1976, pp. 33–62. Search in Google Scholar

Kayasth, S. Electrodeposition studies of rare earths. J. Radioanal. Nucl. Chem.1993, 173, 351–356. Search in Google Scholar

Kim, K. W.; Kim, J. D.; Aoyagi, H.; Yoshida, Z. Kinetics of reduction of uranium (VI) to uranium (IV) at titanium electrode in nitric acid and hydrazine media. J. Nucl. Sci. Technol.1994, 31, 329–334. Search in Google Scholar

Kowalski, Z.; Wong, K. H.; Osteryoung, R. A.; Osteryoung, J. Controlled-growth mercury drop electrode. J. Anal. Chem.1987, 59, 2216–2218. Search in Google Scholar

Lee, S. K.; Chung, T. D.; Kim, H. Indirect voltammetric determination of lanthanides in the presence of mordant red 19. Electroanalysis1997, 9, 527–532. Search in Google Scholar

Li, J.; Liu, S.; Mao, X.; Gao, P.; Yan, Z. Trace determination of rare earths by adsorption voltammetry at a carbon paste electrode. J. Electroanal. Chem.2004, 561, 137–142. Search in Google Scholar

Li, J.; Liu, S.; Yan, Z.; Mao, X.; Gao, P. Adsorptive voltammetric studies on the cerium(III)-Alizarin complexon complex at a carbon paste electrode. Microchim. Acta2006, 154, 241–246. Search in Google Scholar

Liezers, M.; Lehn, S. A.; Olsen, K. B.; Farmer, O. T.; Duckworth, D. C. Determination of plutonium isotope ratios at very low levels by ICP-MS using on-line electrochemically modulated separations. J. Radioanal. Nucl. Chem.2009, 282, 299–304. Search in Google Scholar

Liu, S.; Li, J.; Zhang, S.; Zhao, J. Study on the adsorptive stripping voltammetric determination of trace cerium at a carbon paste electrode modified in situ with cetyltrimethylammonium bromide. Appl. Surf. Sci.2005, 252, 2078–2084. Search in Google Scholar

Maly, J. The amalgamation behavior of heavy elements: 1. Observation of anomalous preference in formation of amalgams of californium, einsteinium and fermium. Inorg. Nucl. Chem. Lett.1967, 3, 373–381. Search in Google Scholar

Martinot, L.; Laeckmann, D.; Materne, T.; Muller, V. Contribution to the knowledge of the electrochemical properties of actinides in non-aqueous media. I: The reduction of tetravalent uranium in various organic solvents. J. Less Common Metals1990, 163, 185–197. Search in Google Scholar

Martinot, L.; Laeckmann, D.; Lopes, L.; Materne, T.; Muller, V. Contribution to the knowledge of the electrochemical properties of actinides in non-aqueous media. II: The reduction of hexavalent uranium in various organic solvents. J. Alloy Cmpd.1992, 185, 151–162. Search in Google Scholar

Martinot, L.; Licour, C.; Lopes, L. Contribution to the knowledge of the electrochemical properties of actinides in non-aqueous media. III. The reduction of tetravalent thorium and tetravalent neptunium in various organic solvents. J. Alloy Cmpd.1995, 228, 6–12. Search in Google Scholar

Martinot, L.; Lopes, L.; Marien, J.; Jerome, C. Electrochemistry of lanthanum and uranium chlorides in organic media: deposition of lanthanum and uranium. J. Radioanal. Nucl. Chem.2002, 253, 407–412. Search in Google Scholar

Mikkelsen, O.; Schroeder, K. H. Amalgam electrodes for electroanalysis. Electroanalysis2003, 15, 679–687. Search in Google Scholar

Mudring, A. V.; Tang, S. Ionic liquids for lanthanide and actinide chemistry. Eur. J. Inorg. Chem.2010, 18, 2569–2581. Search in Google Scholar

Musikas, C.; Haire, R. G.; Peterson, J. R. Electrochemical studies of trivalent californium and selected trivalent lanthanides in aqueous solution. J. Inorg. Nucl. Chem.1981, 43, 2935–2940. Search in Google Scholar

Nagai, T.; Uehara, A.; Fujii, T.; Shirai, O.; Sato, N.; Yamana, H. Redox equilibrium of U4+/U3+ in molten NaCl-2CsCl by UV-Vis spectrophotometry and cyclic voltammetry. J. Nucl. Sci. Technol.2005, 42, 1025–1031. Search in Google Scholar

Nash, K.; Jensen, M. Analytical Separations of the Lanthanides: Basic Chemistry and Methods. In: Handbook on Physics and Chemistry of Rare Earths; Gschneidner, K. A.; Eyring, L., Eds. Elsevier: New York, 2000, 28, pp. 311–372. Search in Google Scholar

Norouzi, P.; Sarmazdeh, Z. R.; Faridbod, F.; Adibi, M.; Ganjali, M. R. Er3+ carbon paste electrode based on new nano-composite. Int. J. Electrochem. Sci.2010, 5, 367–376. Search in Google Scholar

O’Laughlin, J. W. Chemical Spectrophotometric and Polarographic Methods. In: Handbook on Physics and Chemistry of Rare Earths; Gschneidner, K. A.; Eyring, L., Eds. Elsevier: New York, 1979, 4, pp. 341–355. Search in Google Scholar

Piech, R.; Bas, B.; Kubiak, W. W. The cyclic renewable mercury film silver based electrode for determination of uranium(VI) traces using adsorptive stripping voltammetry. Electroanalysis2007, 19, 2342–2350. Search in Google Scholar

Pourjavid, M. R.; Norouzi, P.; Ganjali, M. R. Light lanthanides determination by fast Fourier transform continuous cyclic voltammetry after separation by ion-exchange chromatography. Int. J. Electrochem. Sci.2009a, 4, 923–942. Search in Google Scholar

Pourjavid, M. R.; Norouzi, P.; Ganjali, M. R.; Nemati, A.; Zamani, H. A.; Javaheri, M. Separation and determination of medium lanthanides: a new experiment with use of ion-exchange separation and fast Fourier transform continuous cyclic voltammetry. Int. J. Electrochem. Sci.2009b, 4, 1650–1671. Search in Google Scholar

Pourjavid, M. R.; Norouzi, P.; Rashedi, H.; Ganjali, M. R. Separation and direct determination of heavy lanthanides using new ion-exchange chromatography: fast Fourier transform continuous cyclic voltammetry system. J. Appl. Electrochem.2010, 40, 1593–1603. Search in Google Scholar

Rao, C. J.; Venkatesan, K. A.; Nagarajan, K.; Srinivasan, T. G.; Rao, P. R. V. Electrochemical an thermodynamic properties of europium (III), samarium (III), and cerium (III) in 1-butyl-3-methylimidazolium chloride ionic liquid. J. Nucl. Mater. 2010, 399, 81–16. Search in Google Scholar

Ryabichicov, D. I.; Ryabukhin, V. A. Analytical Chemistry of Rare Earth Elements; Institute of Geochemistry and Analytical Chemistry: Moscow, 1966. Search in Google Scholar

Samhoun, K.; David, F. Electrochemical reduction by radiopolarography of some transplutonium aqueous ions. J. Inorg. Nucl. Chem.1979, 41, 357–363. Search in Google Scholar

Schumacher, P. D.; Woods, N. A.; Schenk, J. O.; Clark, S. B. Rapid pre-concentration of trivalent lanthanide elements on a mercury film from aqueous solution using rotating disk electrode voltammetry. Anal. Chem.2010, 82, 5663–5668. Search in Google Scholar

Schumacher, P. D.; Fitzgerald, K. A.; Schenk, J. O.; Clark, S. B. Preconcentration of f-elements from aqueous solution utilizing a modified carbon paste electrode. Anal. Chem.2011a, 83, 1388–1393. Search in Google Scholar

Schumacher, P. D.; Miley, S. M.; Schenk, J. O.; Clark, S. B. Optimization of Nd(III) pre-concentration on a rotating disk mercury film electrode in aqueous solution. Proc. Radiochim. Acta2011b, 1, 21–25. Search in Google Scholar

Schumacher, P. D.; Woods, N. A.; Doyle, J. L.; Schenk, J. O.; Clark, S. B. Cathodic pre-concentration of f-elements on a mercury film carbon fiber microelectrode. Anal. Chem.2011c, 83, 4788–4793. Search in Google Scholar

Sipos, L.; Galus, Z. Redox processes of uranium (VI), (V), (IV) and (III) in acetate buffers. Inorg. Nucl. Chem. Lett.1971, 7, 299–304. Search in Google Scholar

Skoog, D. A.; Holler, F. J.; Nieman, T. A. Principles of Instrumental Analysis; 5th Edition. Brooks Cole: New York, 1997. Search in Google Scholar

Stozhko, N. Y.; Malakhova, N. A.; Fyodorov, M. V.; Brainina, K. Z. Modified carbon-containing electrodes in stripping voltammetry of metals. J. Solid State Electrochem. 2008, 12, 1185–1204. Search in Google Scholar

Suzuki, Y.; Nankawa, T.; Ozaki, T.; Ohnuki, T.; Francis, A. J.; Enokida, Y.; Yamamoto, I. electrochemical studies on uranium in the presence of organic acids. J. Nucl. Sci. Technol.2007, 44, 1227–1232. Search in Google Scholar

Švancara, I.; Walcarius, A.; Kalcher, K.; Vytras, K. Carbon paste electrodes in the new millennium. Cent. Eur. J. Chem.2009, 7, 598–656. Search in Google Scholar

Tamrakar, P. K.; Pitre, K. S. Voltammetric trace analysis of uranium and other metals in meta rhyolite rock samples. Anal. Sci.2000, 16, 951–955. Search in Google Scholar

Toyoshima, A.; Kasamatsu, Y.; Kitatsuji, Y.; Tsukada, K.; Haba, H.; Shinohara, A.; Nagame, Y. Development of an electrochemistry apparatus for the heaviest elements. Radiochim. Acta2008, 96, 323–326. Search in Google Scholar

Trubachev, A. V. Voltammetry of p-, d- and f-block elements in mineral-organic supporting electrolytes. J. Anal. Chem.2003, 58, 1132–1138. Search in Google Scholar

Tyagi, S.; Agarwal, H.; Ikram, S. A dynamic electrochemical sensor for europium(III). Ind. J. Chem.2010, 49A, 1325–1331. Search in Google Scholar

Ugo, P.; Ballarin, B.; Daniele, S.; Mazzocchin, G. A. Determination of trace amounts of Eu3+ and Yb3+ ions at Nafion-coated thin mercury films. Anal. Chim. Acta1991, 244, 29–38. Search in Google Scholar

Vytras, K.; Švancara, I.; Metelka, R. Carbon paste electrodes in the new millennium. Cen. Euro. J. Chem.2009, 7, 598–656. Search in Google Scholar

Wang, J.; Zadeii, J. M. Trace determination of yttrium and some heavy rare-earths by adsorptive stripping voltammetry. Talanta1986, 33, 321–324. Search in Google Scholar

Wang, J.; Zadeii, J. M. Adsorptive stripping voltammetric measurements of trace levels of uranium following chelation with mordant blue 9. Talanta1987, 34, 247–251. Search in Google Scholar

Wehmeyer, H. R.; Wightman, R. M. Cyclic voltammetry and anodic stripping voltammetry with mercury ultramicroelectrodes. Anal. Chem.1985, 57, 1989–1993. Search in Google Scholar

Wightman, R. M. Microvoltammetric electrodes. Anal. Chem.1981, 53, 1125A–1134A. Search in Google Scholar

Wojciechowski, M.; Balcerzak, J. Microvolume electrochemical cell employing cylindrical graphite fiber microelectrodes. Anal. Chim. Acta1990, 237, 127–133. Search in Google Scholar

Xiaoquan, L.; Xiaorong, M.; Jingwan, K.; Jinzhang, G. Study on electoanalytical chemistry of rare earths. Part 1: Catalytic wave of Yb3+-MnO4-HClO4 system. J. Rare Metal2000, 19, 21–26. Search in Google Scholar

Yamagata, M.; Katayama, Y.; Miura, T. Electrochemical behavior of samarium, europium, ytterbium in hydrophobic room-temperature molten salt systems. J. Electrochem. Soc.2006, 153, E5–E9. Search in Google Scholar

Yamana, H.; Moriyama, H. Feasibility of the separation of americium, curium and lanthanides by electrolytic amalgamation technique. J. Nucl. Sci. Technol.1997, 34, 288–297. Search in Google Scholar

Yamana, H.; Moriyama, H. Characteristics of the electrolytic amalgamation of trivalent f-elements and its application. J. Alloy Cmpd.1998, 275, 898–902. Search in Google Scholar

Yamana, H.; Mitsugashira, T.; Shiokawa, Y.; Sato, A.; Suzuki, S. Possibility of the existence of divalent actinium in aqueous solution. J. Radioanal. Chem.1983, 76, 19–26. Search in Google Scholar

Yantasee, W.; Fryxell, G. E.; Lin, Y. Voltammetric analysis of europium at screen-printed electrodes modified with salicylamide self-assembled on mesoporous silica. Analyst2006, 131, 1342–1346. Search in Google Scholar

Yuan, S.; He, Q.; Yao, S.; Hu, S. Mercury-free detection of europium (III) at a glassy carbon electrode modified with carbon nanotubes by adsorptive stripping voltammetry. Anal. Lett.2006, 39, 373–385. Search in Google Scholar

Received: 2012-9-4
Accepted: 2013-2-13
Published Online: 2013-04-30
Published in Print: 2013-05-01

©2013 by Walter de Gruyter Berlin Boston

This article is distributed under the terms of the Creative Commons Attribution Non-Commercial License, which permits unrestricted non-commercial use, distribution, and reproduction in any medium, provided the original work is properly cited.