Electrochemical Study of Nd and Pr Co-Deposition onto Mo and W from Molten Oxyﬂuorides

: Electrodeposition processes of neodymium and praseodymium in molten NdF 3 + PrF 3 + LiF + 1 wt.%Pr 6 O 11 + 1 wt.%Nd 2 O 3 and NdF 3 + PrF 3 + LiF + 2 wt.%Pr 6 O 11 + 2 wt.%Nd 2 O 3 electrolytes at 1323 K were investigated. Cyclic voltammetry, square wave voltammetry, and open circuit potentiometry were applied to study the electrochemical reduction of Nd(III) and Pr(III) ions on Mo and W cathodes. It was established that a critical condition for Nd and Pr co-deposition in oxyﬂuoride electrolytes was a constant praseodymium deposition overpotential of ≈− 0.100 V, which was shown to result in co-deposition current densities approaching 6 mAcm − 2 . Analysis of the results obtained by applied electrochemical techniques showed that praseodymium deposition proceeds as a one-step process involving exchange of three electrons (Pr(III) → Pr(0)) and that neodymium deposition is a two-step process: the ﬁrst involves one electron exchange (Nd(III) → Nd(II)), and the second involves an exchange of two electrons (Nd(II) → Nd(0)). X-ray diffraction analyses conﬁrmed the formation of metallic Nd and Pr on the working substrate. Keeping the anodic potential to the glassy carbon working anode low results in very low levels of carbon oxides, ﬂuorine and ﬂuorocarbon gas emissions, which should qualify the studied system as an environmentally friendly option for rare earth metal deposition. The newly reported data for Nd and Pr metals co-deposition provide valuable information for the recycling of neodymium-iron-boron magnets.


Introduction
The growing demand for neodymium-iron-boron permanent magnets (Nd 2 Fe 14 B, or NdFeB), driven particularly by their use in wind turbines, high-tech products, etc., requires an ever increasing supply of rare earth based materials [1][2][3][4][5]. An NdFeB magnet, depending on the application, contains about 31-32 wt.% of rare earth elements (REEs), mainly neodymium and praseodymium (Nd + Pr) [6]. The combination of the supply shortage of rare earth minerals and increasing supply of rare earth solid wastes calls for a simple, inexpensive, and environmentally friendly recycling process for REEs in order to supplement current supply chains.
Interest in the recovery of the rare earth metals neodymium and praseodymium from their secondary sources, mainly from the end-of-life NdFeB magnet scrap, is becoming increasingly important for the sustainable rare earth industry [1,4,7]. Most of the recycling processes are in their development stages and require technology advances to achieve sustainable production. To find a solution for the growing environmental problems and

Materials and Methods
The used electrolytes were composed of neodymium fluoride (NdF 3 , ≥99.9%), praseodymium fluoride (PrF 3 , ≥99.9%), lithium fluoride (LiF, ≥99.5%), neodymium oxide (Nd 2 O 3 , ≥99.9%) and praseodymium oxide (Pr 6 O 11 , ≥99.9%). All the chemicals were purchased from Treibacher, Althofen, Austria. Two electrolytes were developed. The composition of each was as shown in Table 1. The key composition difference is in the oxide concentration. The two oxides made up 2 wt.% of the Electrolyte I and 4 wt.% of the Electrolyte II. Before being manually mixed, the fluorides were dried in a furnace for 24 h at 523 K. Mixed fluorides were melted in a high purity graphite crucible. This process was conducted in a vacuum induction furnace, which operated in overpressure condition in order to counteract the high vapour pressure of the fluorides under 1800 mbar of argon pressure at temperatures up to 1373 K. Before they were added to the electrolyte, neodymium and praseodymium oxides were also dried in a furnace for 24 h at 393 K.
Electrochemical experiments were conducted in a three-electrode steel cell, shown in Figure 1. As working electrodes, 2-mm-diameter, EWG 99.95% molybdenum or tungsten electrodes were used, with surface area of 1cm 2 exposed to contact with the melt. The potentials were referenced to the RE, which was made from tungsten (1 mm diameter, EWG 99.95%). The CEs were made from high purity glassy carbon (>99.99% HTW SIGRADUR ® G). Glassy carbon as chemically relatively stable compared to other types of carbon materials was chosen to be used in our experiments [26,27]. Prior to insertion in the cell, the surface of the electrodes used was polished thoroughly with SiC emery paper, rinsed with deionized water and ethanol, and dried in open air.

NdF3
PrF3 Before being manually mixed, the fluorides were dried in a furnace for 24 h at 523 K. Mixed fluorides were melted in a high purity graphite crucible. This process was conducted in a vacuum induction furnace, which operated in overpressure condition in order to counteract the high vapour pressure of the fluorides under 1800 mbar of argon pressure at temperatures up to 1373 K. Before they were added to the electrolyte, neodymium and praseodymium oxides were also dried in a furnace for 24 h at 393 K.
Electrochemical experiments were conducted in a three-electrode steel cell, shown in Figure 1. As working electrodes, 2-mm-diameter, EWG 99.95% molybdenum or tungsten electrodes were used, with surface area of 1cm 2 exposed to contact with the melt. The potentials were referenced to the RE, which was made from tungsten (1 mm diameter, EWG 99.95%). The CEs were made from high purity glassy carbon (>99.99% HTW SI-GRADUR ® G). Glassy carbon as chemically relatively stable compared to other types of carbon materials was chosen to be used in our experiments [26,27]. Prior to insertion in the cell, the surface of the electrodes used was polished thoroughly with SiC emery paper, rinsed with deionized water and ethanol, and dried in open air.
The graphite crucible, filled with the salt mixture, was placed into the steel electrochemical cell; the lid was closed, and the cell was placed into a resistance furnace. The working temperature of 1323 K was controlled by a type K thermocouple controller. To protect the seals of the Swagelok system, which makes the swaps of the electrodes during the experiment possible, the lid of the cell must be water-cooled. Thus, the cell operates in an airtight environment, which on one hand prevents the toxic gases from leaking out of the cell and on the other hand prevents the electrolyte from oxidizing. The cell is also kept under argon atmosphere. The exhaust gases were discharged in a controlled manner, washed with sodium hydroxide solution and fed into the exhaust system. A certain amount of the off-gas is taken by the off-gas measurement system-Gasmet DX4000 Fourier transformation infrared spectrometer (FTIR, Ansyco, Karlsruhe, Germany)-for an online analysis displayed every 5 s. The graphite crucible, filled with the salt mixture, was placed into the steel electrochemical cell; the lid was closed, and the cell was placed into a resistance furnace. The working temperature of 1323 K was controlled by a type K thermocouple controller. To protect the seals of the Swagelok system, which makes the swaps of the electrodes during the experiment possible, the lid of the cell must be water-cooled. Thus, the cell operates in an airtight environment, which on one hand prevents the toxic gases from leaking out of the cell and on the other hand prevents the electrolyte from oxidizing. The cell is also kept under argon atmosphere. The exhaust gases were discharged in a controlled manner, washed with sodium hydroxide solution and fed into the exhaust system. A certain amount of the off-gas is taken by the off-gas measurement system-Gasmet DX4000 Fourier transformation infrared spectrometer (FTIR, Ansyco, Karlsruhe, Germany)-for an online analysis displayed every 5 s. All electrochemical measurements: cyclic voltammetry (CV), chronopotentiometry, square wave voltammetry (SWV) and open circuit chronopotentiometry, were controlled by an IviumStat potentiostat (5 A/10 V; Ivium Technologies Eindhoven, Netherlands). The cyclic voltammograms obtained, started from potential E I , usually 0.050 V negative to the working electrode open circuit potential (measured against the tungsten reference electrode), changed to a chosen cathodic end potential, E C , and back with various sweep rates. Long-term experiments were carried out for up to 90 min at constant overpotentials to provide adequate time for the metal to deposit on the working electrode. The surfaces of the samples and deposits were initially examined by an optical microscope (Keyence; model VH-Z100R, Osaka, Japan). Solidified deposits were mechanically removed from the working electrode and subsequently analysed by X-ray diffraction (XRD) with Philips PW 1050 powder diffractometer (Philips, Delft, The Netherlands) at room temperature with Ni filtered CuKα radiation (λ = 1.54178 Å), scintillation detector within 20-85 • 2θ range in steps of 0.05 • , and scanning time of 5 s per step.

Results and Discussion
The cyclic voltammetry technique was used to help identify possible redox reactions taking part on Mo and W working electrodes in both electrolytes. Cathodic end potential, E C , was gradually swept from the initial potential, E I , towards more negative values. A typical result is presented in Figure 2. Clear indications of four redox processes were obtained in the potential range up to 1.000 V negative to the open circuit of the working Mo or W electrode in Electrolyte I. They were represented as four reduction (cathodic) current waves (C 1 , C 2 , C 3 and C 4 ) and four oxidation (anodic) counterparts (A 1 , A 2 , A 3 and A 4 ). Comparing the current wave peak potentials shown in Figure 2 to the similar current wave potentials obtained in our previous study from NdF 3 + LiF + 2 wt.%Nd 2 O 3 electrolyte on W and Mo electrodes under the same conditions for the neodymium deposition and dissolution, helped attribution of C 1 /A 1 and C 2 /A 2 to the deposition and dissolution of neodymium and C 4 /A 4 to the deposition and dissolution of lithium [12,15]. According to the data published in our earlier work, in the fluoride electrolyte, neodymium reduces to the metal form in two steps, seen as C 1 and C 2 in Figure 2 [12,15]. Therefore, the electrode reaction corresponding to the current waves C 3 /A 3 can be assigned to possible deposition and dissolution of praseodymium. All electrochemical measurements: cyclic voltammetry (CV), chronopotentiometry, square wave voltammetry (SWV) and open circuit chronopotentiometry, were controlled by an IviumStat potentiostat (5 A/10 V; Ivium Technologies Eindhoven, Netherlands). The cyclic voltammograms obtained, started from potential EI, usually 0.050 V negative to the working electrode open circuit potential (measured against the tungsten reference electrode), changed to a chosen cathodic end potential, EC, and back with various sweep rates. Long-term experiments were carried out for up to 90 min at constant overpotentials to provide adequate time for the metal to deposit on the working electrode. The surfaces of the samples and deposits were initially examined by an optical microscope (Keyence; model VH-Z100R, Osaka, Japan). Solidified deposits were mechanically removed from the working electrode and subsequently analysed by X-ray diffraction (XRD) with Philips PW 1050 powder diffractometer (Philips, Delft, The Netherlands) at room temperature with Ni filtered CuKα radiation (λ = 1.54178 Å), scintillation detector within 20-85° 2θ range in steps of 0.05°, and scanning time of 5 s per step.

Results and Discussion
The cyclic voltammetry technique was used to help identify possible redox reactions taking part on Mo and W working electrodes in both electrolytes. Cathodic end potential, EC, was gradually swept from the initial potential, EI, towards more negative values. A typical result is presented in Figure 2. Clear indications of four redox processes were obtained in the potential range up to 1.000 V negative to the open circuit of the working Mo or W electrode in Electrolyte I. They were represented as four reduction (cathodic) current waves (C1, C2, C3 and C4) and four oxidation (anodic) counterparts (A1, A2, A3 and A4). Comparing the current wave peak potentials shown in Figure 2 to the similar current wave potentials obtained in our previous study from NdF3 + LiF + 2wt.%Nd2O3 electrolyte on W and Mo electrodes under the same conditions for the neodymium deposition and dissolution, helped attribution of C1/A1 and C2/A2 to the deposition and dissolution of neodymium and C4/A4 to the deposition and dissolution of lithium [12,15]. According to the data published in our earlier work, in the fluoride electrolyte, neodymium reduces to the metal form in two steps, seen as C1 and C2 in Figure 2 [12,15]. Therefore, the electrode reaction corresponding to the current waves C3/A3 can be assigned to possible deposition and dissolution of praseodymium. Cyclic voltammetry with different scan rates (50 and 300 mVs −1 ) was employed to study the electrochemical reactions related to Nd and Pr redox transitions on W and Mo Cyclic voltammetry with different scan rates (50 and 300 mV·s −1 ) was employed to study the electrochemical reactions related to Nd and Pr redox transitions on W and Mo working electrodes. Figure 3a within the applied potential range, the voltammograms, exhibited three distinct current waves C 1 , C 2 and C 3 in the cathodic sections and corresponding anodic counterparts A 1 , A 2 and A 3 in the anodic sections of the scanned potential range. working electrodes. Figure 3a,b show voltammograms obtained on each of the working electrode substrates (Mo and W) in the molten Electrolyte I, at 1323 K. On both substrates, within the applied potential range, the voltammograms, exhibited three distinct current waves C1, C2 and C3 in the cathodic sections and corresponding anodic counterparts A1, A2 and A3 in the anodic sections of the scanned potential range.
(a) (b) Furthermore, it was apparent that there were in fact three redox reactions (C1/A1, C2/A2 and C3/A3), because each cathodic current wave was a prerequisite for its anodic counterpart.
The small difference between the voltammograms obtained on Mo and W was recorded in the peak potentials of the recorded current waves. On W working electrode, the current wave C1, starting at ≈ −0.550 V vs. W, should reflect the reduction of Nd(III) to Nd(II), and the anodic peak A1 in the reverse scan at ≈ −0.300 V vs. W, should reflect the oxidation of Nd(II) to Nd(III) [12,15,20]. At more cathodic potentials ≈ −0.700 V vs. W, the reduction current wave C2 should be assigned to further reduction of Nd(II) to Nd(0), and the anodic counterpart current wave A2 should represent the oxidation of Nd(0) to Nd(II). In other words, the reduction process of Nd(III) ions to Nd metal takes place in two steps, Nd(III) → Nd(II) and Nd(II) → Nd(0), which is in accordance with the results reported in molten fluorides with Nd2O3 added [12,15,20]. At the potentials negative to −0.700 V vs. W, a third reduction current wave was observed. Since the C3 current wave potentials are cathodic with respect to the reduction potential of Nd(II), cathodic peak C3 (starting from around −0.800 V vs. W) should be associated with the electroreduction of Pr(III) to Pr(0). In the anodic scan, starting at around −0.670 V vs. W, the oxidation current wave A3, should then correspond to the dissolution of Pr metal that was previously deposited on the working electrode, e.g., Pr(0) to Pr(III). It appeared that the electroreduction of Pr(III) ions to Pr metal in this system is a single one-step process, Pr(III) → Pr(0), which is in agreement with the results observed in similar molten fluoride electrolytes [5,17,28]. On the basis of experimental results in this study, the cathodic peak potential values C2 and C3, as seen on CVs in Figure 3a and b, reflecting the electroreduction potentials of Nd(II) ions into Nd metal (C2), are more positive than the electroreduction potential of Pr(III) ions (C3), which is consistent with the results seen in the literature [17]. Additionally, due to close values of the reduction potentials for reactions: Nd(II) + 2e − → Nd(0), and Pr(III) + 3e − → Pr(0), it was difficult to obtain ideally shaped individual current waves by cyclic voltammetry, particularly at higher scan rates. As recorded in voltammograms obtained on Mo and W cathodes, potentials of cathodic current waves on the Mo substrate are slightly shifted toward more positive values compared to the W substrate, whereas the Furthermore, it was apparent that there were in fact three redox reactions (C 1 /A 1 , C 2 /A 2 and C 3 /A 3 ), because each cathodic current wave was a prerequisite for its anodic counterpart.
The small difference between the voltammograms obtained on Mo and W was recorded in the peak potentials of the recorded current waves. On W working electrode, the current wave C 1 , starting at ≈−0.550 V vs. W, should reflect the reduction of Nd(III) to Nd(II), and the anodic peak A 1 in the reverse scan at ≈−0.300 V vs. W, should reflect the oxidation of Nd(II) to Nd(III) [12,15,20]. At more cathodic potentials ≈−0.700 V vs. W, the reduction current wave C 2 should be assigned to further reduction of Nd(II) to Nd(0), and the anodic counterpart current wave A 2 should represent the oxidation of Nd(0) to Nd(II). In other words, the reduction process of Nd(III) ions to Nd metal takes place in two steps, Nd(III) → Nd(II) and Nd(II) → Nd(0), which is in accordance with the results reported in molten fluorides with Nd 2 O 3 added [12,15,20]. At the potentials negative to −0.700 V vs. W, a third reduction current wave was observed. Since the C 3 current wave potentials are cathodic with respect to the reduction potential of Nd(II), cathodic peak C 3 (starting from around −0.800 V vs. W) should be associated with the electroreduction of Pr(III) to Pr(0). In the anodic scan, starting at around −0.670 V vs. W, the oxidation current wave A 3 , should then correspond to the dissolution of Pr metal that was previously deposited on the working electrode, e.g., Pr(0) to Pr(III). It appeared that the electroreduction of Pr(III) ions to Pr metal in this system is a single one-step process, Pr(III) → Pr(0), which is in agreement with the results observed in similar molten fluoride electrolytes [5,17,28]. On the basis of experimental results in this study, the cathodic peak potential values C 2 and C 3 , as seen on CVs in Figure 3a,b, reflecting the electroreduction potentials of Nd(II) ions into Nd metal (C 2 ), are more positive than the electroreduction potential of Pr(III) ions (C 3 ), which is consistent with the results seen in the literature [17]. Additionally, due to close values of the reduction potentials for reactions: Nd(II) + 2e − → Nd(0), and Pr(III) + 3e − → Pr(0), it was difficult to obtain ideally shaped individual current waves by cyclic voltammetry, particularly at higher scan rates. As recorded in voltammograms obtained on Mo and W cathodes, potentials of cathodic current waves on the Mo substrate are slightly shifted toward more positive values compared to the W substrate, whereas the anodic current waves are similar in values. Therefore, it can be assumed that in the Electrolyte I system, W and Mo working electrodes behave almost identically. Similar results were observed with Mo and W WEs in NdF 3 + LiF + 2 wt.%Nd 2 O 3 melts [15].
To investigate the redox reactions further, the CVs recorded at different scan rates on Mo and W electrodes in molten NdF 3 + PrF 3 + LiF + 1 wt.%Pr 6 O 11 + 1 wt.%Nd 2 O 3 electrolyte (Figure 3a,b) were recorded and analysed. It was observed that with an increase in scan rates (50-300 mV·s −1 ), reduction current densities for peaks C 1 , C 2 and C 3 and oxidation current densities for peaks A 3 , A 2 and A 1 increased. Attempts were made to recognize the possible reversibility of the recorded redox reactions or their parts. The reversibility was examined by plotting the influence of the scan rates applied to the current wave peak potentials recorded. Figure 4 shows graphical representations of the plots derived from the data in Figure 3a: anodic current waves are similar in values. Therefore, it can be assumed that in the Electrolyte I system, W and Mo working electrodes behave almost identically. Similar results were observed with Mo and W WEs in NdF3 + LiF + 2wt.%Nd2O3 melts [15].
To investigate the redox reactions further, the CVs recorded at different scan rates on Mo and W electrodes in molten NdF3 + PrF3 + LiF + 1wt.%Pr6O11 + 1wt.%Nd2O3 electrolyte (Figure 3a,b) were recorded and analysed. It was observed that with an increase in scan rates (50-300 mVs −1 ), reduction current densities for peaks C1, C2 and C3 and oxidation current densities for peaks A3, A2 and A1 increased. Attempts were made to recognize the possible reversibility of the recorded redox reactions or their parts. The reversibility was examined by plotting the influence of the scan rates applied to the current wave peak potentials recorded. Figure 4 shows graphical representations of the plots derived from the data in Figure 3a: a) A1 anodic peak current density values as a function of square root of the scan rates applied, and b) the logarithms of A1 anodic peak current values as a function of the peak potentials recorded for different potential scan rates applied (log iP = f(EP)). The first plot appears to be linear and does not pass through the origin, Figure 4a. This should indicate that the oxidation process Nd(II) ↔ Nd(III) is reversible and under mixed control, as was shown in the earlier work done in neodymium oxyfluoride melts under very similar con- (a) A 1 anodic peak current density values as a function of square root of the scan rates applied, and (b) the logarithms of A 1 anodic peak current values as a function of the peak potentials recorded for different potential scan rates applied (log i P = f(E P )).
The first plot appears to be linear and does not pass through the origin, Figure 4a. This should indicate that the oxidation process Nd(II) (c) Figure 4. Plots of anodic peak A1: (a) current densities vs. square root of scan rate calculated from Figure 3a; (b) logarithm of the peak current density vs. peak potential from the same anodic peak in Figure 3a; (c) plots of peaks A3/C3, anodic and cathodic peak current densities vs. square root of scan rates derived from Figure 3b. a) A1 anodic peak current density values as a function of square root of the scan rates applied, and b) the logarithms of A1 anodic peak current values as a function of the peak potentials recorded for different potential scan rates applied (log iP = f(EP)). The first plot appears to be linear and does not pass through the origin, Figure 4a. This should indicate that the oxidation process Nd(II) ↔ Nd(III) is reversible and under mixed control, Nd(III) is reversible and under mixed control, as was shown in the earlier work done in neodymium oxyfluoride melts under very similar conditions [12,15,20]. The relationship presented in Figure 4b is linear for the whole range of the scan rates applied, which made it possible for the number of exchanged electrons in the Nd(II)→Nd(III) reaction to be calculated. The calculation was performed using the equation often employed in electrodeposition studies that defining the slope (K) as a function of log i P = f(E PEAK ) and the number of electrons involved in the reaction (z) [12,15,20]. It was found that the slope K of the linear function from Figure 4b was 2.39, and the corresponding electron transfer number therefore should be 1.25, so close to 1. This directly confirmed the oxidation reaction recorded as an oxidation process A 1 (Figure 3a) involves one electron exchange in electrochemical oxidation of Nd(II) to Nd(III). Thus, it was confirmed that the redox reaction reflected as a current wave pair C 1 /A 1 was Nd(II)  anodic peak current value potentials recorded for different potential scan rates applied (l appears to be linear and does not pass through the origin, Figu that the oxidation process Nd(II) ↔ Nd(III) is reversible a Nd(0) as a redox reaction [12,20].
The data presented in Figure 4c, where the maximum cathodic current densities for peak C 3 and its anodic counterpart peak A 3 from Figure 3b are plotted versus the square root of the scan rates applied, indicated a linear relationship that did not pass through the origin. The results were implying that the redox process recorded as the C 3 /A 3 current wave pair (Pr(III) a) A1 anodic peak current density values as a function of square root of the scan rates applied, and b) the logarithms of A1 anodic peak current values as a function of the peak potentials recorded for different potential scan rates applied (log iP = f(EP)). The first plot appears to be linear and does not pass through the origin, Figure 4a. This should indicate that the oxidation process Nd(II) ↔ Nd(III) is reversible and under mixed control, Pr(0)) was reversible and under mixed control: by mass transfer of the complexed prase-odymium ions in the molten NdF 3 + PrF 3 + LiF + 1 wt.%Pr 6 O 11 + 1 wt.%Nd 2 O 3 and that the rate of the charge transfer step was likely complicated by the dismantling structure of the praseodymium oxyfluoride complexes [25,29].
Although values of the peak potentials for the redox pairs C 3 /A 3 , C 2 /A 2 and C 1 /A 1 in the voltammograms, Figure 3a,b, were slightly different from when the scan rates applied were varied, the observed should be attributed to the reversible reactions under mixed control as shown above and in our previous studies [12,15]. These conclusions apply for both Mo and W working electrodes.
CV performed on Mo electrode in the same molten fluoride while applying different holding times at chosen cathodic end potentials, E C = −0.630 V vs. W, before returning to the starting potential, E I , is shown in Figure 5. C 2 /A 2 and C 1 /A 1 identify the redox signals that occurred within this potential window. The same electrochemical reactions associated with C 2 /A 2 and C 1 /A 1 redox couples were observed in previous studies and described as neodymium electrochemical deposition/dissolution in two steps on/from Mo working electrode under given conditions [12,15,20]. In a separate set of experiments, the cathodic end potential of the Mo working electrode was held at −0.850 V vs. W, Figure 6a, and the W working electrode at −0.900 V vs. W, Figure 6b, for 60, 180 and 300 s, before letting the potential return to positive values. On the basis of the above mentioned results, in Figures 2, 3 and 5, the chosen cathodic end potential has proven to be negative enough to sustain the praseodymium and neodymium electrodeposition but not too much to induce lithium deposition. With an increase in deposition time, the maximum peak current at the E C potential increased, and the charge encompassed by the anodic current waves (A 3 , A 2 , A 1 ), was substantially enlarged. The increased charge encompassed by anodic current waves with increased deposition time indicated more praseodymium and neodymium metal being dissolved. The conclusion had to be that the electroreduction processes of Nd and Pr in the fluoride bath made of Electrolyte I, on both W and Mo working substrates were taking place in a very similar way. To further clarify the electrochemical reduction of neodymium and praseodymium in the molten Electrolyte I, square wave voltammetry (SWV) was employed. SWV is characterised by advanced sensitivity and high resolution and can be applied to estimate the number of exchanged electrons involved in reduction processes [30,31]. A set of square wave voltammograms showing application of different frequencies to the Mo working electrode are presented in Figure 7. The peaks II and III detected at potentials ≈ −0.505 V vs. W and ≈ −0.640 V vs. W are in good agreement within the range of the cathodic current wave potentials C2 and C3 recorded in the voltammograms presented in Figures 3a and 5a and ascribed to the reduction of Nd(II) → Nd(0) and Pr(III) → Pr(0), respectively. For a reversible electrode reaction, mathematical analysis enables us to use a simple equation connecting the width of the half-peak, W1/2, recorded in a SW voltammogram with the number of the exchanged electrons [17,30]: where W1/2 is the half-peak width (V), T is the temperature (K), R represents the universal gas constant (J·mol −1 ·K −1 ), n is the number of exchanged electrons, and F is the Faraday constant (96485 C·mol −1 ). Application of Equation (1) for reversible systems is possible if the criterion of linearity for the peak current density vs. the square root of the frequency To further clarify the electrochemical reduction of neodymium and praseodymium in the molten Electrolyte I, square wave voltammetry (SWV) was employed. SWV is characterised by advanced sensitivity and high resolution and can be applied to estimate the number of exchanged electrons involved in reduction processes [30,31]. A set of square wave voltammograms showing application of different frequencies to the Mo working electrode are presented in Figure 7. The peaks II and III detected at potentials ≈ −0.505 V vs. W and ≈ −0.640 V vs. W are in good agreement within the range of the cathodic current wave potentials C2 and C3 recorded in the voltammograms presented in Figures 3a and 5a and ascribed to the reduction of Nd(II) → Nd(0) and Pr(III) → Pr(0), respectively. For a reversible electrode reaction, mathematical analysis enables us to use a simple equation connecting the width of the half-peak, W1/2, recorded in a SW voltammogram with the number of the exchanged electrons [17,30]: where W1/2 is the half-peak width (V), T is the temperature (K), R represents the universal gas constant (J·mol −1 ·K −1 ), n is the number of exchanged electrons, and F is the Faraday constant (96485 C·mol −1 ). Application of Equation (1) for reversible systems is possible if the criterion of linearity for the peak current density vs. the square root of the frequency To further clarify the electrochemical reduction of neodymium and praseodymium in the molten Electrolyte I, square wave voltammetry (SWV) was employed. SWV is characterised by advanced sensitivity and high resolution and can be applied to estimate the number of exchanged electrons involved in reduction processes [30,31]. A set of square wave voltammograms showing application of different frequencies to the Mo working electrode are presented in Figure 7. The peaks II and III detected at potentials ≈−0.505 V vs. W and ≈−0.640 V vs. W are in good agreement within the range of the cathodic current wave potentials C 2 and C 3 recorded in the voltammograms presented in Figures 3a and 5a and ascribed to the reduction of Nd(II) → Nd(0) and Pr(III) → Pr(0), respectively. For a reversible electrode reaction, mathematical analysis enables us to use a simple equation connecting the width of the half-peak, W 1/2 , recorded in a SW voltammogram with the number of the exchanged electrons [17,30]: where W 1/2 is the half-peak width (V), T is the temperature (K), R represents the universal gas constant (J·mol −1 ·K −1 ), n is the number of exchanged electrons, and F is the Faraday constant (96,485 C·mol −1 ). Application of Equation (1) for reversible systems is possible if the criterion of linearity for the peak current density vs. the square root of the frequency is fulfilled [17,31]. The linear relationship for the obtained SWV was proven by plotting peak current density vs. the square root of frequency, as can be seen from Figure 7b,c. The relationship can be used to calculate the electrons involved in reactions of the frequency range examined [17,31]. A Gaussian fitting model was applied to calculate the half-peak width, which was used to determine the number of the transferred electrons.
Metals 2021, 11, x FOR PEER REVIEW 9 of 17 is fulfilled [17,31]. The linear relationship for the obtained SWV was proven by plotting peak current density vs. the square root of frequency, as can be seen from Figure 7b,c. The relationship can be used to calculate the electrons involved in reactions of the frequency range examined [17,31]. A Gaussian fitting model was applied to calculate the half-peak width, which was used to determine the number of the transferred electrons. The results derived from Equation (1) for peak II revealed the exchange electron number as 2.37, close to 2. The conclusion had to be that the current wave II (C2) should reflect the reduction of neodymium Nd(II) into metal Nd, after two electrons were exchanged. After application of Equation (1) to the current wave III in Figure 7a, it was found that the number of electrons exchanged in the reduction was 3.42, close to 3. This indicated that the reduction of praseodymium, Pr(III) in the used electrolyte takes place in only one electrochemical step involving three electron exchange, namely Pr(III) → Pr(0). The number of electrons involved in the Pr electroreduction process calculated in the present study corresponds very well with the average oxidation state of Pr in Pr6O11, which is in alignment to the available data 3.667 [32].
The electrochemical reduction processes of Nd and Pr in Electrolyte I were verified by multiple electrochemical techniques. However, in order to further study the ongoing The results derived from Equation (1) for peak II revealed the exchange electron number as 2.37, close to 2. The conclusion had to be that the current wave II (C 2 ) should reflect the reduction of neodymium Nd(II) into metal Nd, after two electrons were exchanged. Figure 7a, it was found that the number of electrons exchanged in the reduction was 3.42, close to 3. This indicated that the reduction of praseodymium, Pr(III) in the used electrolyte takes place in only one electrochemical step involving three electron exchange, namely Pr(III) → Pr(0). The number of electrons involved in the Pr electroreduction process calculated in the present study corresponds very well with the average oxidation state of Pr in Pr 6 O 11 , which is in alignment to the available data 3.667 [32].

After application of Equation (1) to the current wave III in
The electrochemical reduction processes of Nd and Pr in Electrolyte I were verified by multiple electrochemical techniques. However, in order to further study the ongoing reaction mechanism, and adjust the deposition parameters to potentially improve the efficiency of the Nd and Pr electrolysis process, the percentage of rare earth oxide that was added to the base electrolyte was changed.
The literature presents claims that increased weight percentage of Nd 2 O 3 in the neodymium fluoride electrolyte has a significant impact on Nd metal production [1,22]. Based on our previous work, it appears that better neodymium yield on the cathode is achieved when 2 wt.% of Nd 2 O 3 is added to the original neodymium fluoride melt. With the Nd 2 O 3 added in the fluoride bath, the oxide will react with NdF 3 or LiF to form different oxyfluorides complexes, namely NdOF or [NdOF 5 ] 4− [1,12,33,34]. Due to the excess of Fions in fluoride molten salts, both complexes coexist, and which complex will be reduced into metallic Nd during the electrodeposition of Nd from Nd(III) depends on the neodymium oxyfluoride/neodymium fluoride ion molar ratio, electrode potential and applied current density [12,34,35]. However, the data on the subject of dissolution of praseodymium oxide, especially Pr 6 O 11 , in fluoride molten bath are rather limited [1,18,25,29]. During preparation of rare earth fluoride electrolytes, praseodymium oxide is dissolved in neodymium fluoride or corresponding praseodymium fluoride molten electrolyte. As a result, of the chemical exchange between the praseodymium oxide and rare earth fluorides, praseodymium oxyfluoride complexes are formed. The knowledge gathered around this subject suggests substantial similarity between the Nd and Pr complexes formed in the melts containing their fluorides, LiF, Nd 2 O 3 and Pr 6 O 11 [1,29]. Controlled addition of rare earth oxides to fluoride melts should increase the conductivity of the electrolyte and provide a source of rare earth metals for the electrolysis [18].
Since the objective was to maximize the quantity of Nd and Pr electrodeposited on the working electrode substrates (Mo and W), the experiments were repeated, applying the same set of experimental techniques but in NdF 3 + PrF 3 + LiF + 2 wt.%Pr 6 O 11 + 2 wt.%Nd 2 O 3 electrolyte instead. The voltammograms in Figure 8 reflect the results of the CVs applied on a Mo cathode in the Electrolyte II at 1323 K. They exhibit three current waves in the cathodic run (namely C 1 , C 2 and C 3 ) showing peak potentials at ≈−0.400 V, ≈−0.550 V and ≈−0.800 V vs. W, respectively, and three anodic current waves with peak potentials at around ≈−0.600 V, ≈−0.350 V and ≈−0.200 V vs. W, respectively. Compared to the voltammograms obtained for Electrolyte I under the same conditions, the current densities recorded were up to five times higher in the electrolyte with higher oxide weight percentages. Otherwise, the current wave pairs C 1 /A 1 , C 2 /A 2 and C 3 /A 3 in Figure 8 should correspond to the electrochemical redox processes, which were found to be Nd(III)/Nd(II), Nd(II)/Nd(0) and Pr(III)/Pr(0). Figure 9 shows CVs similar to those described above for Electrolyte I (Figure 6a,b). These were recorded while applying different holding times at chosen cathodic end potentials, E C , on Mo working electrode in the electrolyte with higher oxides concentration. By using the same procedures as those employed for Electrolyte I, prolonged deposition at potentials cathodic to the peak potential C 3 induced increased amounts of charge encompassed by the anodic current waves, A 3 and A 2 , which clearly suggested an increased quantity of dissolved praseodymium and neodymium, which were previously deposited during the application of the E C cathodic potential. −0.550 V and ≈ −0.800 V vs. W, respectively, and three anodic current waves with peak potentials at around ≈ −0.600 V, ≈ −0.350 V and ≈ −0.200 V vs. W, respectively. Compared to the voltammograms obtained for Electrolyte I under the same conditions, the current densities recorded were up to five times higher in the electrolyte with higher oxide weight percentages. Otherwise, the current wave pairs C1/A1, C2/A2 and C3/A3 in Figure 8 should correspond to the electrochemical redox processes, which were found to be Nd(III)/Nd(II), Nd(II)/Nd(0) and Pr(III)/Pr(0).   Figure 9 shows CVs similar to those described above for Electrolyte I (Figure 6a,b). These were recorded while applying different holding times at chosen cathodic end potentials, EC, on Mo working electrode in the electrolyte with higher oxides concentration. By using the same procedures as those employed for Electrolyte I, prolonged deposition at potentials cathodic to the peak potential C3 induced increased amounts of charge encompassed by the anodic current waves, A3 and A2, which clearly suggested an increased quantity of dissolved praseodymium and neodymium, which were previously deposited during the application of the EC cathodic potential. To support the proposition that current wave pairs C1/A1, C2/A2 and C3/A3 recorded in the voltammograms presented in Figures 8 and 9 are the results of praseodymium (C3/A3) and neodymium (C1/A1, C2/A2), metal phase formation and dissolution open circuit potentiometry was conducted. Nd and Pr were electrodeposited on working electrode substrates by applying a constant potential negative to the peak of the C3 potential for a short period of time, and then the resulting transient curve for the open circuit working electrode potential was recorded. The open circuit chronopotentiograms obtained in Electrolyte II on a Mo working electrode after potentiostatic electrodeposition at −0.900 V vs. W at 1323 K is presented in Figure 10. The chronopotentiogram shows the plateaux I ≈ −0.750 V, II ≈ −0.600 V and III ≈ −0.350 V vs. W, respectively, pointing out that the number of inflection points agreed with the number of anodic current waves (A1, A2 and A3) seen in the previously presented voltammograms. Relatively stable plateaux I and II reflect two phases (metal Pr and metal Nd) in equilibrium with individual ions in the surrounding electrolyte under the given conditions. The fading potential of the inclined plateau III should reflect declining equilibrium between Nd(III) ↔ Nd(II) ions. To support the proposition that current wave pairs C 1 /A 1 , C 2 /A 2 and C 3 /A 3 recorded in the voltammograms presented in Figures 8 and 9 are the results of praseodymium (C 3 /A 3 ) and neodymium (C 1 /A 1 , C 2 /A 2 ), metal phase formation and dissolution open circuit potentiometry was conducted. Nd and Pr were electrodeposited on working electrode substrates by applying a constant potential negative to the peak of the C 3 potential for a short period of time, and then the resulting transient curve for the open circuit working electrode potential was recorded. The open circuit chronopotentiograms obtained in Electrolyte II on a Mo working electrode after potentiostatic electrodeposition at −0.900 V vs. W at 1323 K is presented in Figure 10. The chronopotentiogram shows the plateaux I ≈ −0.750 V, II ≈ −0.600 V and III ≈ −0.350 V vs. W, respectively, pointing out that the number of inflection points agreed with the number of anodic current waves (A 1 , A 2 and A 3 ) seen in the previously presented voltammograms. Relatively stable plateaux I and II reflect two phases (metal Pr and metal Nd) in equilibrium with individual ions in the surrounding electrolyte under the given conditions. The fading potential of the inclined plateau III should reflect declining equilibrium between Nd(III) Metals 2021, 11, x FOR PEER REVIEW anodic current waves are similar in values. Therefore, it can be assumed that in trolyte I system, W and Mo working electrodes behave almost identically. Simil were observed with Mo and W WEs in NdF3 + LiF + 2wt.%Nd2O3 melts [15].
To investigate the redox reactions further, the CVs recorded at different scan Mo and W electrodes in molten NdF3 + PrF3 + LiF + 1wt.%Pr6O11 + 1wt.%Nd2O3 e (Figure 3a,b) were recorded and analysed. It was observed that with an increas rates (50-300 mVs −1 ), reduction current densities for peaks C1, C2 and C3 and o current densities for peaks A3, A2 and A1 increased. Attempts were made to reco possible reversibility of the recorded redox reactions or their parts. The reversib examined by plotting the influence of the scan rates applied to the current w potentials recorded. Figure 4 shows graphical representations of the plots deri the data in Figure 3a:  Figure 3a; (b) logarithm of the peak current density vs. peak potential from the same an in Figure 3a; (c) plots of peaks A3/C3, anodic and cathodic peak current densities vs. squ scan rates derived from Figure 3b. a) A1 anodic peak current density values as a function of square root of the s applied, and b) the logarithms of A1 anodic peak current values as a function of potentials recorded for different potential scan rates applied (log iP = f(EP)). The appears to be linear and does not pass through the origin, Figure 4a. This should that the oxidation process Nd(II) ↔ Nd(III) is reversible and under mixed Nd(II) ions. In the oxide richer Electrolyte II, SWV measurements resulted in more distinct results in terms of the deposition of neodymium and praseodymium. An example of the typical SWV on a Mo working electrode is presented in Figure 11. Two well-pronounced cathodic peaks were recorded in the potential range applied. Half-peak width was established, and after applying a Gaussian fitting model, the exchange electron number was calculated using Equation (1), after proving the linear relationship; Figure 11b. Reduction peak II identified at around −0.600 V vs. W was processed, and the number of transferred electrons was found to be 2.23, which implied the exchange of two electrons, i.e., the reduction process of Nd(II) into Nd metal. As for the reduction peak III identified at ≈−0.820 V, the number of exchanged electrons was determined to be 3.43, which can be explained as a three-electron exchange in the one-step reduction process of Pr(III) to Pr metal. SWV obtained with different frequencies on Mo cathode in both electrolytes confirmed the already suggested corresponding potentials of the cathodic reactions C 2 and C 3 and the number of exchanged electrons involved in each reaction. V vs. W; sweep rate 100 mVs .
To support the proposition that current wave pairs C1/A1, C2/A2 and C3/A3 recorded in the voltammograms presented in Figures 8 and 9 are the results of praseodymium (C3/A3) and neodymium (C1/A1, C2/A2), metal phase formation and dissolution open circuit potentiometry was conducted. Nd and Pr were electrodeposited on working electrode substrates by applying a constant potential negative to the peak of the C3 potential for a short period of time, and then the resulting transient curve for the open circuit working electrode potential was recorded. The open circuit chronopotentiograms obtained in Electrolyte II on a Mo working electrode after potentiostatic electrodeposition at −0.900 V vs. W at 1323 K is presented in Figure 10. The chronopotentiogram shows the plateaux I ≈ −0.750 V, II ≈ −0.600 V and III ≈ −0.350 V vs. W, respectively, pointing out that the number of inflection points agreed with the number of anodic current waves (A1, A2 and A3) seen in the previously presented voltammograms. Relatively stable plateaux I and II reflect two phases (metal Pr and metal Nd) in equilibrium with individual ions in the surrounding electrolyte under the given conditions. The fading potential of the inclined plateau III should reflect declining equilibrium between Nd(III) ↔ Nd(II) ions. In the oxide richer Electrolyte II, SWV measurements resulted in more distinct results in terms of the deposition of neodymium and praseodymium. An example of the typical SWV on a Mo working electrode is presented in Figure 11. Two well-pronounced cathodic peaks were recorded in the potential range applied. Half-peak width was established, and after applying a Gaussian fitting model, the exchange electron number was calculated using Equation (1), after proving the linear relationship; Figure 11b. Reduction peak II identified at around −0.600 V vs. W was processed, and the number of transferred electrons was found to be 2.23, which implied the exchange of two electrons, i.e., the reduction process of Nd(II) into Nd metal. As for the reduction peak III identified at ≈ −0.820 V, the number of exchanged electrons was determined to be 3.43, which can be explained as a three-electron exchange in the one-step reduction process of Pr(III) to Pr metal. SWV obtained with different frequencies on Mo cathode in both electrolytes confirmed the already suggested corresponding potentials of the cathodic reactions C2 and C3 and the number of exchanged electrons involved in each reaction.
(a) (b) Figure 11. (a) SWV obtained on Mo WE in NdF3 + PrF3 + LiF + 2wt.%Pr6O11 + 2wt.%Nd2O3 electrolyte with different frequency, pulse amplitude = 25mV, potential step = 1mV; (b) Variation of the peak current density versus the square root of the frequency in Figure 11a for the peak III.
Thus, taking into account similar behaviour of molybdenum and tungsten in the common Nd-Pr fluoride electrolytes with 2wt.% and 4wt.% REO added, one should assume that on both electrodes at potentials more negative than the reduction potential of Pr(III) ions, Nd metal and Pr metal can be co-deposited.
Literature is very scarce regarding Nd and Pr metal being identified on an inert cathode (Mo and W) surface by a deposition similar to the potentiostatic deposition from an oxide fluoride molten salt electrolyte [25]. There are, however, reports showing Nd and Pr being deposited from fluoride melts, but only in the form of alloys [17,23].
To confirm the presence of Nd and Pr metal on an inert working substrate, potentiostic electrolysis was conducted at −0.900 V vs. W on Mo working electrode for 60 and 90 Figure 11. (a) SWV obtained on Mo WE in NdF 3 + PrF 3 + LiF + 2 wt.%Pr 6 O 11 + 2 wt.%Nd 2 O 3 electrolyte with different frequency, pulse amplitude = 25 mV, potential step = 1 mV; (b) Variation of the peak current density versus the square root of the frequency in Figure 11a for the peak III.
Thus, taking into account similar behaviour of molybdenum and tungsten in the common Nd-Pr fluoride electrolytes with 2 wt.% and 4 wt.% REO added, one should assume that on both electrodes at potentials more negative than the reduction potential of Pr(III) ions, Nd metal and Pr metal can be co-deposited.
Literature is very scarce regarding Nd and Pr metal being identified on an inert cathode (Mo and W) surface by a deposition similar to the potentiostatic deposition from an oxide fluoride molten salt electrolyte [25]. There are, however, reports showing Nd and Pr being deposited from fluoride melts, but only in the form of alloys [17,23].
To confirm the presence of Nd and Pr metal on an inert working substrate, potentiostic electrolysis was conducted at −0.900 V vs. W on Mo working electrode for 60 and 90 min in the electrolyte made of NdF 3 + PrF 3 + LiF + 2 wt.%Pr 6 O 11 + 2 wt.%Nd 2 O 3 .
The applied potential was approximately 100 mV more negative than the peak potential value of the cathodic current wave C 3 , which reflects the reduction process Pr(III) into Pr(0); Figures 2,5,6,8 and 9. After the deposition ended, a solidified electrolyte film from the Mo working electrode surface was mechanically removed. The film-free surface was then analysed by optical microscopy, Figures 12a and 13a, and by XRD, Figures 12b and 13b. The scratches observed were remains of the mechanical preparation of the electrode surface.         [24]. The anodic working potentials, governed by the applied cathodic potentials were obviously high enough to sustain oxidation processes on the GC anode by oxygen and fluoride ions at longer reaction times, prior to the partial passivation of the anode occurs. Similar observation was reported by other researchers in the field, claiming that only oxygen containing species are taking part in partial passivation and CF 4 emission starts only later at higher anodic potentials [24]. The quantity of recorded CF4 was almost negligible; the average values during the electrochemical experiments were below 5 ppm and during the potentiostatic Pr/Nd deposition around 0.02 ppm, which should be attributed to the relatively low applied deposition overpotential (and therefore small anodic overpotential). At the same time, C2F6 was not detected under the potential regime applied. According to Zhang et al. [38], and taking into account the off-gas results obtained during voltammetry measurements in this study, it appears that in the positive scan the PFC gases are being adsorbed on the anode and are forming an insulating layer which reduces the anode oxidation current. During the reverse scan PFC are rapidly desorbed from the graphite anode and the desorption potential is more negative than the adsorption potential, thus reducing the PFC emission to a great extent and keeping the process in a green process window [38,39].

Conclusions
1) Praseodymium and neodymium were successfully electrodeposited from NdF3 + PrF3 + LiF + 1wt.%Pr6O11 + 1wt.%Nd2O3 and NdF3 + PrF3 + LiF + 2wt.%Pr6O11 + 2wt.%Nd2O3 molten electrolytes at 1323 K on inert Mo and W electrodes. The results recorded by electrochemical techniques confirm that optimal conditions for the co-deposition were constant overpotential of ≈ −0.100 V of praseodymium deposition potential (−0.700 V to −0.800 V vs. W on Mo electrode and −0.750 V to −0.850 V vs. W on W electrode), which should provide deposition current densities of around 6 mAcm −2 in the fluoride molten salt.
2) Analysis of the results obtained by applied electrochemical techniques have shown that praseodymium deposition proceeds in one step involving three electrons exchange (Pr(III) → Pr(0)). The same techniques previously confirmed earlier propositions that neodymium deposition includes two steps: the first involving exchange of one electron (Nd(III) → Nd(II)) and the second involving exchange of two electrons (Nd(II) → Nd(0)).
3) It was established that Pr and Nd co-deposition performed under relatively small praseodymium deposition overpotentials in the used electrolytes and at applied temperatures on the inert Mo and W cathodes was very successful because: a) lithium deposition was disabled, and b) it allowed only very small evolution of the greenhouse gases due to the low anodic potential. 4) Such low levels of carbon oxides, fluorine and fluorocarbon gas evolution from the glassy carbon anode indicates this process to be an environmentally friendly technique for rare earth metal deposition. Thus, this process has the potential to recycle the rare The quantity of recorded CF 4 was almost negligible; the average values during the electrochemical experiments were below 5 ppm and during the potentiostatic Pr/Nd deposition around 0.02 ppm, which should be attributed to the relatively low applied deposition overpotential (and therefore small anodic overpotential). At the same time, C 2 F 6 was not detected under the potential regime applied. According to Zhang et al. [38], and taking into account the off-gas results obtained during voltammetry measurements in this study, it appears that in the positive scan the PFC gases are being adsorbed on the anode and are forming an insulating layer which reduces the anode oxidation current. During the reverse scan PFC are rapidly desorbed from the graphite anode and the desorption potential is more negative than the adsorption potential, thus reducing the PFC emission to a great extent and keeping the process in a green process window [38,39].

Conclusions
(1) Praseodymium and neodymium were successfully electrodeposited from NdF 3 + PrF 3 + LiF + 1 wt.%Pr 6 O 11 + 1 wt.%Nd 2 O 3 and NdF 3 + PrF 3 + LiF + 2 wt.%Pr 6 O 11 + 2 wt.%Nd 2 O 3 molten electrolytes at 1323 K on inert Mo and W electrodes. The results recorded by electrochemical techniques confirm that optimal conditions for the co-deposition were constant overpotential of ≈−0.100 V of praseodymium deposition potential (−0.700 V to −0.800 V vs. W on Mo electrode and −0.750 V to −0.850 V vs. W on W electrode), which should provide deposition current densities of around 6 mAcm −2 in the fluoride molten salt.
(2) Analysis of the results obtained by applied electrochemical techniques have shown that praseodymium deposition proceeds in one step involving three electrons exchange (Pr(III) → Pr(0)). The same techniques previously confirmed earlier propositions that neodymium deposition includes two steps: the first involving exchange of one electron (Nd(III) → Nd(II)) and the second involving exchange of two electrons (Nd(II) → Nd(0)).
(3) It was established that Pr and Nd co-deposition performed under relatively small praseodymium deposition overpotentials in the used electrolytes and at applied temperatures on the inert Mo and W cathodes was very successful because: (a) lithium deposition was disabled, and (b) it allowed only very small evolution of the greenhouse gases due to the low anodic potential.
(4) Such low levels of carbon oxides, fluorine and fluorocarbon gas evolution from the glassy carbon anode indicates this process to be an environmentally friendly technique for rare earth metal deposition. Thus, this process has the potential to recycle the rare earth elements of a neodymium iron boron magnet if they are first separated from the magnet in oxide form. If Nd and Pr are deposited simultaneously as an alloy without emitting a large amount of greenhouse gases, it should be possible to use this alloy directly in magnet production.