Journal of Sustainable Metallurgy

, Volume 3, Issue 3, pp 627–637 | Cite as

Electrochemical Extraction of Rare Earth Metals in Molten Fluorides: Conversion of Rare Earth Oxides into Rare Earth Fluorides Using Fluoride Additives

  • Aida AbbasalizadehEmail author
  • Annelies Malfliet
  • Seshadri Seetharaman
  • Jilt Sietsma
  • Yongxiang Yang
Open Access
Research Article


In the present research on rare earth extraction from rare earth oxides (REOs), conversion of rare earth oxides into rare earth fluorides with fluoride fluxes is investigated in order to overcome the problem of low solubility of the rare earth oxides in molten fluoride salts as well as the formation of oxyfluorides in the fluorination process. Based on thermodynamic calculations, a series of experiments were performed for converting the rare earth oxides into rare earth fluorides using AlF3, ZnF2, FeF3, and Na3AlF6 as fluorinating agents in a LiF–Nd2O3 system. The formation of neodymium fluoride as a result of the reactions between these fluxes and neodymium oxide is confirmed. The rare earth fluoride thus formed can subsequently be processed through the electrolysis route in the same reactor, and rare earth metal can be produced as the cathodic deposit. In this concept, the REO dissolution in molten fluorides would become unnecessary due to the complete conversion of the oxide into the fluoride, REF3. The results of XRD and EPMA analysis of the reacted samples indicate that AlF3, ZnF2, and FeF3 can act as strong fluorinating agents for the neodymium oxide giving rise to a complete conversion of neodymium oxide into neodymium fluoride.


Rare earth oxides Rare earth fluorides Recycling Fluorination 


Rare earth oxides are among the most stable oxides of the elements in the periodic table. Oxygen removal from rare earth metals is therefore very difficult due to the strong affinity of these metals to oxygen.

Chen et al. [1] have developed a direct electrochemical process for the reduction of solid metal oxides into their metals in molten salts, the FFC process. This method has been extensively adopted in metal extraction for a number of elements including rare earth metals (RE = Gd, Tb, Dy, Er, and Ce) [2, 3, 4]. The direct electrochemical reduction of oxide into metal is influenced by a number of parameters such as duration of electrolysis, temperature, applied voltage, open porosity of the oxide pellet, and mode of electrolysis [5]. The efficiency of the oxygen removal by direct electrochemical reduction of oxides is mainly determined by the geometry of the samples, the surface area of the solid sample in contact with the molten salt, and the initial oxygen concentrations. The FFC process has not yet been commercialized, and one of the main challenges is the residual oxygen concentration in the reduced metal.

Electrowinning (molten salt electrolysis) is the dominating industrial method for rare earth metal extraction from their oxides in the salt extraction process [6, 7, 8]. It is generally considered that in an electrowinning process, it is the dissolved oxide in the electrolyte that is subjected to electrolysis [9]. Hence in fluoride systems, solubility of the oxide in fluoride electrolytes is an important parameter. Generally, molten fluorides have a low oxide solubility, except for cryolite, which has a high solubility for alumina (about 10 wt%); the solubility of neodymium oxide in molten alkali fluorides was reported to be 2–4 wt% [10, 11]. The concentration of dissolved oxide cannot be increased by adding excess oxide into the melt at a constant temperature and fixed salt composition. Nevertheless, addition of an excess quantity of oxide into the melt can increase the kinetics of the reactions. Besides the low solubility of rare earth oxides in molten fluorides, another problem for metals extraction that needs to be addressed is that these oxides can form rare earth oxyfluorides in the LiF–NdF3 molten salt. It has been reported that neodymium oxyfluorides cannot be reduced to neodymium metal [12]. It has been confirmed that neodymium oxyfluoride participates in the anodic reaction to generate oxygen [13]. However, the role of neodymium oxyfluoride in the anodic and cathodic reactions is not very clear and needs to be clarified further in detail [12, 13, 14, 15, 16].

In the present work, a new approach is proposed for solving the problem of low oxide solubility and oxyfluoride formation of rare earth oxides (REOs) in molten fluorides. Addition of fluorinating agents such as AlF3, ZnF2, and FeF3 to the LiF–Nd2O3 system changes the thermodynamic equilibrium and thus allows conversion of REOs into rare earth fluorides. Use of cryolite (Na3AlF6) as a fluorinating agent, and as a substitute for AlF3, was also investigated, due to its availability and cost advantages. By treatment with fluorinating agents, the rare earth oxide is converted into rare earth fluoride. The rare earth fluoride thus formed can subsequently be processed through the electrolysis route in the same reactor to extract rare earth metal as the cathodic deposit. In this concept, the REO dissolution in molten fluorides would become redundant due to the complete conversion of the oxide into the fluoride, REF3.

Thermodynamics of the Process

The standard Gibbs free energies (\( \Delta G^{ \circ } \) ) for the formation of the reacted fluorides and oxides at 1223 K (950 °C), calculated using FactSage, are given in Table 1. A decrease in the stability of fluorides formed was observed in the following order: CaF2 > LiF > NaF > KF. The decomposition voltages of rare earth fluorides and the alkali fluorides are also compared in Table 1. It can be seen that only CaF2 and LiF are more stable than NdF3 and DyF3. Thus, for the electrochemical decomposition of REOs into fluorides, the most suitable solvents among fluorides need to be based on CaF2 and LiF.
Table 1

Standard Gibbs energies and decomposition voltages of different fluoride salts and REOs and REF3 (RE = Nd, Dy)


\( \Delta G^{ \circ } \) (kJ/mol) at 1223 K (950 °C)

Decomposition potential (V) at 1223 K (950 °C)

\( \Delta G^{ \circ } \) (kJ/mol) at 298 K (25 °C)

\( {\text{CaF}}_{ 2} \rightleftarrows {\text{Ca}} + {\text{F}}_{ 2} \)




\( {\text{LiF}} \rightleftarrows {\text{Li}} + 1/ 2 {\text{F}}_{ 2} \)




\( {\text{NaF}} \rightleftarrows {\text{Na}} + 1/ 2 {\text{F}}_{ 2} \)




\( {\text{KF}} \rightleftarrows {\text{K}} + 1/ 2 {\text{F}}_{ 2} \)




\( {\text{NdF}}_{ 3} \left( {\text{s}} \right) \rightleftarrows {\text{Nd}}\left( {\text{s}} \right) + 3/ 2 {\text{F}}_{ 2} \left( {\text{g}} \right) \)




\( {\text{DyF}}_{ 3} \left( {\text{s}} \right) \rightleftarrows {\text{Dy}}\left( {\text{s}} \right) + 3/ 2 {\text{F}}_{ 2} \left( {\text{g}} \right) \)




\( {\text{Nd}}_{ 2} {\text{O}}_{ 3} \left( {\text{s}} \right) \rightleftarrows 2 {\text{Nd}}\left( {\text{s}} \right) + 3/ 2 {\text{O}}_{ 2} \left( {\text{g}} \right) \)




\( {\text{Dy}}_{ 2} {\text{O}}_{ 3} \left( {\text{s}} \right) \rightleftarrows 2 {\text{Dy}}\left( {\text{s}} \right) + 3/ 2 {\text{O}}_{ 2} \left( {\text{g}} \right) \)




In the present work, AlF3, ZnF2, FeF3, and Na3AlF6 are tested as candidates for the fluorination of REOs prior to electrolysis in molten fluoride bath. From the calculated standard Gibbs energies of the reactions (1)–(4) at 1223 K (950 °C)
$$ \begin{aligned} {\text{Nd}}_{ 2} {\text{O}}_{ 3} + {\text{ 2AlF}}_{ 3} \left( {\text{salt}} \right) \rightleftarrows 2 {\text{NdF}}_{ 3} + {\text{ Al}}_{ 2} {\text{O}}_{ 3} \hfill \\ \Delta G^{ \circ } = \, - 1 7 7 {\text{ kJ}}/{\text{mol}} \hfill \\ \end{aligned} $$
$$ \begin{aligned} {\text{Nd}}_{ 2} {\text{O}}_{ 3} + {\text{ 3ZnF}}_{ 2} \left( {\text{salt}} \right) \rightleftarrows 2 {\text{NdF}}_{ 3} + {\text{ 3ZnO}} \hfill \\ \Delta G^{ \circ } = \, - 2 7 4 {\text{ kJ}}/{\text{mol}} \hfill \\ \end{aligned} $$
$$ \begin{aligned} {\text{Nd}}_{ 2} {\text{O}}_{ 3} + {\text{ 2FeF}}_{ 3} \left( {\text{salt}} \right) \rightleftarrows 2 {\text{NdF}}_{ 3} + {\text{ Fe}}_{ 2} {\text{O}}_{ 3} \hfill \\ \Delta G^{ \circ } = \, - 2 2 2 {\text{ kJ}}/{\text{mol}} \hfill \\ \end{aligned} $$
$$ \begin{aligned} {\text{Nd}}_{ 2} {\text{O}}_{ 3} + {\text{ Na}}_{ 3} {\text{AlF}}_{ 6} \left( {\text{salt}} \right) \rightleftarrows {\text{NdF}}_{ 3} + {\text{ Al}}_{ 2} {\text{O}}_{ 3} + {\text{ 3NaF}} \hfill \\ \Delta G^{ \circ } = \, - 2 3. 4 {\text{ kJ}}/{\text{mol}} \hfill \\ \end{aligned} $$
it is evident that these metal fluorides can react with REOs to form rare earth fluorides, and the formed NdF3 can further be reduced at the cathode. The metal oxides Al2O3, ZnO, and Fe2O3 are formed in the system during the formation of NdF3. It should be noted that in argon atmosphere and at low oxygen pressure, in reaction (3), it is expected that, instead of Fe2O3, FeO could be formed which means that Fe2O3 will be in the form of FeO and O2 under experimental conditions.
NdF3, formed as a result of the reaction between Nd2O3 and MF x (M = Al, Zn, Fe) or Na3AlF6, will be subjected to electrolysis. In this process, in theory, the main cathodic reaction would be
$$ {\text{Nd}}^{ 3+ } + {\text{ 3e}}^{ - } \rightleftarrows {\text{Nd}} $$

According to reactions (1)–(4), during the Nd2O3 conversion into NdF3 by AlF3, ZnF2, FeF3, or Na3AlF6, the corresponding oxides Al2O3, ZnO, FeO, and Al2O3, respectively, are formed in the salt. Since the stability of these oxides is lower than that of NdF3, parts of Al2O3, ZnO, and FeO might dissolve in the fluoride melt and get subjected to the electrolysis process. The solubility of alumina in the molten fluorides is 6 mol% [17]. Based on the density of the LiF containing different concentrations of NdF3 [18], an estimation shows that the density of LiF-5 mol% NdF3 is 4 g/cm3 (aluminum oxide density is 3.95 g/cm3). This means that the critical composition in which the aluminum oxide will start floating is LiF-5 mol% NdF3. The floating oxide can be then removed from the top of the liquid. The density of the LiF–NdF3 system can go up to 5 g/cm3 when NdF3 reaches 50 mol%. Yet ZnO and FeO have higher density (5.6 and 5.74 g/cm3, respectively), so the oxide formed will sink in the liquid and should be removed. If the newly formed oxide could be removed before electrolysis, the co-deposition could be minimized. For the separation of newly formed oxide solids from the molten salt (for electrolysis), a two-chamber inter-connected furnace system can be designed: NdF3 conversion chamber-1 and NdF3 electrolysis chamber-2. By arranging the connection channel in the middle or the bottom level (depending on the density of the newly formed oxide), the new oxide particles can be removed from the top or bottom, before entering the electrolysis chamber.

The decomposition voltages of these oxides as well as their corresponding fluorides are compared with neodymium fluorides as shown in Fig. 1. These data are calculated for pure substances at their standard states at the specified temperatures. In the real system, the activity values of the fluorides and the oxides will deviate from unity (standard state) due to the dissolution in the salt bath. Yet these data are crucial for the comparison of the different fluorides.
Fig. 1

Decomposition voltages of metal oxides and fluorides calculated by FactSage

Based on the stability line of the different compounds in Fig. 1, addition of AlF3, ZnF2, FeF3, and Na3AlF6 to the LiF–Nd2O3 system and subsequent electrolysis (with a cell voltage of ~4.8 V at T = 950 °C, without considering the overpotential) would enable the extraction of neodymium from neodymium fluoride. It is also expected that Al, Zn and Fe will be co-deposited on the cathode, forming Nd–Al, Nd–Zn and Nd–Fe alloys if there are remaining AlF3, ZnF2 or FeF3 in the salt or the Al2O3, ZnO or Fe2O3 that are formed are dissolved in the salt and participate in the electrochemical reactions. In the case of using cryolite, Na deposition on cathode is also expected. Hence, along with the reaction (4), one of the following reactions can take place at the cathode:
$$ {\text{Al}}^{ 3+ } + {\text{ 3e}}^{ - } \rightleftarrows {\text{Al}} $$
$$ {\text{Zn}}^{ 2+ } + {\text{ 2e}}^{ - } \rightleftarrows {\text{Zn}} $$
$$ {\text{Fe}}^{ 3+ } + {\text{ 3e}}^{ - } \rightleftarrows {\text{Fe}} $$
$$ {\text{Na}}^{ + } + {\text{ e}}^{ - } \rightleftarrows {\text{Na}} $$
The following anodic reactions will take place if a graphite anode is used:
$$ {\text{O}}^{ 2- } \left( {\text{salt}} \right) \, + {\text{ C}}\left( {\text{anode}} \right) \rightleftarrows {\text{CO}}\left( {\text{g}} \right) \, + {\text{ 2e}}^{ - } $$
$$ 2 {\text{O}}^{ 2- } \left( {\text{salt}} \right) + {\text{ C}}\left( {\text{anode}} \right) \rightleftarrows {\text{CO}}_{ 2} \left( {\text{g}} \right) \, + {\text{ 4e}}^{ - } $$
$$ 2 {\text{F}}^{ - } \left( {\text{salt}} \right) \rightleftarrows {\text{F}}_{ 2} \left( {\text{g}} \right) \, + {\text{ 2e}}^{ - } $$
A schematic diagram of the salt extraction process including the fluorinating step and the electrochemical RE extraction step is shown in Fig. 2.
Fig. 2

Schematic diagram of the salt extraction process for extraction of RE from REOs


Lithium fluoride (98.5%-Alfa Aesar) was mixed with neodymium oxide (Rhodia) in a glove box. A fluorinating agent of aluminum fluoride (99+%-Alfa Aesar), zinc fluoride (99%-Alfa Aesar), iron fluoride (97%-Alfa Aesar), or cryolite (97%-Sigma Aldrich) was added to the mixture separately, and the mixture was charged into a graphite crucible. The ratio of neodymium fluoride to fluorinating agent were prepared based on the stoichiometry of Eqs. 14; Nd2O3:2AlF3, Nd2O3:3ZnF2, Nd2O3:2AlF3 and Nd2O3:Na3AlF6. No excessive fluorinating agents were added more than the theoretical requirement. LiF concentration was determined assuming that after reaching the complete conversion of Nd2O3 to NdF3, the eutectic composition of LiF-23 mol% NdF3 [19] is formed in the system. The total amount of the mixture for all the systems was about 30 g. The mixtures were heated at 1223 K (950 °C) for 3 h in a purified argon atmosphere. The Ar gas was purified by passing through KOH flakes in order to remove sulfur and also through silica gel and P2O5 to remove moisture. The gas was passed through a tube furnace containing Ti sponges which was held at 1123 K (850 °C) in order to remove the traces of O2. The samples were quenched in liquid nitrogen after the experiment.

The samples were analyzed by X-ray diffractometry (XRD) as well as electron probe microanalysis (EPMA), in order to determine the phases that are formed during the experiments. For the EPMA analyses, WDS point analyses or mappings were performed at either 15 kV–15 nA or at 5 kV–15 nA. For quantification, standards were used. The EPMA quantification data are within 1% error.


AlF3 in LiF–Nd2O3 System

The XRD analysis results of the sample from the LiF–Nd2O3–AlF3 mixture after fluorination treatment are shown in Fig. 3, illustrating the formation of NdF3, LiF, AlNdO3, and Al2O3 phases. These results thus confirm the formation of NdF3 based on reaction (1).
Fig. 3

XRD pattern of LiF–Nd2O3–AlF3 sample after fluorination treatment with identified phases

Al, Nd, and oxygen distributions shown by EPMA mapping in Fig. 4 provide further evidence for the formation of Al–Nd–O phase, which is identified as AlNdO3 in XRD. Formation of AlNdO3 could inhibit the complete conversion of Nd2O3 into NdF3. Furthermore, Nd is distributed in the fluorine areas, which indicates neodymium fluoride formation. The dark phase in the sample is possibly LiF, since the fluorine concentration is very high in this area. Lithium, being a light element, could not be measured by EPMA. The microstructure of the liquid nitrogen-quenched sample is shown in Fig. 5. With the help of the EPMA point analysis, different phases present in the samples were identified and are marked. The dark phase with high fluorine concentration is identified as lithium fluoride, and the fibrous phase is NdF3. Fibrous pattern of NdF3–LiF eutectic structure is shown in this image. The large light grains correspond to oxides (Al2O3, AlNdO3). Both aluminum oxide and aluminum neodymium oxide were identified by XRD. The EPMA analysis shows the distribution of neodymium, aluminum, and oxygen in the same areas which can be referred to AlNdO3 phase.
Fig. 4

EPMA mapping images of LiF–Nd2O3–AlF3 sample after fluorination treatment (Color figure online)

Fig. 5

BSE image and EPMA quantification result of the LiF–Nd2O3–AlF3 sample in at% after fluorination treatment, showing the presence of NdF3 and AlNdO3

Point analysis of the LiF–Nd2O3–AlF3 sample shows the presence of 77 at% fluorine and 19 at% neodymium, forming NdF3 phase, a fluorine-rich phase (LiF), and AlNdO3 (20 at% aluminum, 17 at% neodymium, and 62 at% oxygen). Al2O3 was not identified in the EPMA. This could be due to the fact that EPMA point analysis is limited to certain areas, whereas the XRD analysis detects the whole sample, wherein the Al2O3 phase was identified.

ZnF2 in LiF–Nd2O3 System

The XRD analysis result for LiF–Nd2O3–ZnF2 after fluorination is shown in Fig. 6. The identified phases are NdF3, LiF, and ZnO. This confirms the complete conversion of Nd2O3 into NdF3 based on reaction (2).
Fig. 6

XRD pattern of LiF–Nd2O3-ZnF2 sample after fluorination treatment with identified phases

Very strong peaks of neodymium fluoride indicate that neodymium oxide is converted into neodymium fluoride after reaction with ZnF2. Oxygen is detected only in the zinc oxide phase, and there were no peaks corresponding to the remaining neodymium oxide in the sample. Hence neodymium oxide is considered to have been completely converted into neodymium fluoride. It should be noted that no oxyfluoride phase was detected by XRD analysis.

The EPMA mapping images in Fig. 7 also clearly show the formation of NdF3 and ZnO as separate phases. Mapping (a) was analyzed at 15 kV voltage; however, for more details and a clear distinction between the two phases, mapping (b) was performed at a lower voltage level of 5 kV. The LiF–NdF3 eutectic microstructure, lamellar NdF3 phase in the LiF phase, is visibly shown in this image. In this figure, it is clearly shown that neodymium is distributed in the lamellar phase and fluorine is found in both microstructural constituents. The level of fluorine in the black phase is twice that of the lamellar phase which is a reflection of the presence of LiF as the basic salt constituent (solvent).
Fig. 7

EPMA mapping images of LiF–Nd2O3–ZnF2 sample after fluorination treatment: a analyzed at 15 kV and b at 5 kV (Color figure online)

The EPMA point analysis of the LiF–Nd2O3–ZnF2 sample after fluorination treatment with the elemental quantification is shown in Fig. 8. The results show the presence of dark gray ZnO grains in a lamellar LiF–NdF3 eutectic matrix. The quantifications show that no oxyfluoride phase is formed and that all neodymium oxide has been converted into neodymium fluoride. The lamellar light gray phase having fluorine and neodymium in a 3:1 atomic ratio proves the formation of neodymium fluoride. NdF3–LiF eutectic structure is clearly shown in the EBS image. Measurement of NdF x phase indicates (referring to the table under Fig. 8) that the fluorine concentration is relatively high (nine times the Nd concentration). High concentration value for fluorine can be due to the fact that this data is obtained using area analysis with the radius of 7 µm wihich contains both NdF3 and LiF. Li cannot be detected by EPMA. The small gray grains correspond to the presence of the ZnO phase (Zn 52 at% and O 47 at%).
Fig. 8

BSE image and EPMA quantification result of LiF–Nd2O3–ZnF2 sample in at% after fluorination treatment showing the presence of NdF3 and ZnO

FeF3 in LiF–Nd2O3 System

The result of the XRD analysis of the LiF–Nd2O3–FeF3 sample is shown in Fig. 9. The strong peaks of neodymium fluoride prove the oxide-to-fluoride conversion. FeO is formed during the reaction between iron fluoride and neodymium oxide. As mentioned earlier, in the Ar ambient and low oxygen pressure atmosphere, hematite (Fe2O3) will not be formed or, depending upon the prevailing oxygen pressure, the formed Fe2O3 would be decomposed to Fe3O4 and FeO. At temperatures higher than the eutectoid temperature (ca. 560 °C) for FeO in equilibrium with metallic iron and Fe3O4, the stable oxide is wüstite (FeO). Furthermore, three peaks were detected in the XRD pattern corresponding to the presence of NdOF phase.
Fig. 9

XRD pattern of LiF–Nd2O3–FeF3 sample after fluorination treatment with identified phases

In the EPMA mapping, the distribution of iron and oxygen is clearly shown. Based on the mapping images, neodymium is highly concentrated around the FeO grain boundaries. Oxygen and fluorine are also present in these areas at very low concentrations (Fig. 10). Hence neodymium oxyfluoride is found in these areas, which was detected by XRD. Based on the mapping images, the lamellar phase is NdF3 in the LiF, indicating the LiF–NdF3 eutectic microstructure.
Fig. 10

EPMA mapping of LiF–Nd2O3–FeF3 sample after fluorination treatment showing the presence of NdF3 and FeO (Color figure online)

The BSE images and EPMA quantification results are shown in Fig. 11. In this figure, the presence of FeO (45 at% Fe and 54 at% O) grains is seen. This phase can be a mixture of FeO and Fe2O3, since concentration can also be related to magnetite phase (Fe3O4). From reaction (3), Fe2O3 formation is expected, but as both XRD and EPMA results show, the oxide of iron formed is wüstite or non-stoichiometric FeO x . However, oxygen measurement by EPMA at 15 kV is not precise.
Fig. 11

BSE image and EPMA quantification result of LiF–Nd2O3–FeF3 sample in at% after fluorination treatment showing the presence of NdF3 and FeO

In Fig. 11, the presence of needle-shaped grains of neodymium fluoride is seen. No neodymium oxyfluoride phase was detected by EPMA in the selected area of the sample. However, in XRD results of the same sample (Fig. 9), small peaks corresponding to NdOF phase could be detected. Considering the fact that XRD analysis is valid for the whole sample while EPMA analysis is limited to certain areas, it is assumed that NdOF is formed as a result of the chemical reaction. The EPMA quantitative analysis shows the presence of 26 at% Nd and 72 at% F.

Na3AlF6 in LiF–Nd2O3 System

Figure 12 shows the XRD results of the LiF–Nd2O3–Na3AlF6 system after fluorination. It can be seen that unlike the NdF3 formation in other systems, in this system Na1.5Nd1.5F6 compound is formed. It seems that neodymium from neodymium oxide reacts with cryolite and gets substituted in place of aluminum in the cryolite. Therefore, peaks corresponding to AlNdO3 and also three peaks—an unexpected result—related to aluminum metal were observed. This observation is inexplicable at this stage and thus is not discussed further in this study.
Fig. 12

XRD pattern of LiF–Nd2O3–Na3AlF6 sample after fluorination treatment with identified phases

The EPMA analysis results depicted in Fig. 13 show the distribution of fluorine and neodymium in the same areas, indicating the presence of neodymium fluoride. It can be seen that large grains in the sample (indicated in the picture) consist of aluminum, oxygen, and neodymium, which show the presence of AlNdO.
Fig. 13

EPMA mapping of LiF–Nd2O3–Na3AlF6 sample after fluorination treatment showing the presence of NdF3 (Color figure online)

The BSE image and the EPMA quantification results of LiF–Nd2O3–Na3AlF6 sample shown in Figure 14 indicate the formation of Nd1.5Na1.5F6 lamellar structure containing 18 at% Nd, 11 at% Na, and 70 at% F and the AlNdO phase with 21 at% Nd, 22 at% Al, and 54 at% O. These results are in line with the results of XRD obtained for the same sample.
Fig. 14

BSE images and EPMA quantification result of LiF–Nd2O3–Na3AlF6 sample in at% after fluorination treatment showing the presence of Nd1.5Na1.5F6 and NdAlO


Among the four fluorides used as fluorinating agents, complete conversion of rare earth oxide into rare earth fluoride is observed only in the case when ZnO is used. According to the Gibbs formation energy of reactions (1)–(4) at 950 °C, formation of NdF3 as a result of reaction of Nd2O3 with ZnO is the most favorable reaction since it has the lowest Gibbs energy under standard conditions.

The reaction related to cryolite has the highest Gibbs energy and hence has the lowest tendency for the formation of NdF3. Instead of neodymium fluoride, Na1.5Nd1.5F6 is formed. Some of the oxide phase is also found in the form of AlNdO3. In the next step of the process, which is electrochemical reduction of the rare earth on cathode, neodymium should be extracted from Na1.5Nd1.5F6. Na was also expected to get co-deposited with Nd on the cathode.

Results of the LiF–Nd2O3–AlF3 system show that neodymium from neodymium oxide gets substituted for aluminum, resulting in the formation of neodymium fluoride. But the complete conversion was obviously not attained since some neodymium was detected in the oxide phase in AlNdO3. Adding an excess amount of AlF3 to the system can result in the complete conversion of neodymium oxide, which needs to be proved in the future research.

In the case of FeF3, three small peaks in XRD, corresponding to the neodymium oxyfluoride phase, were identified; in the EPMA mapping of this system, neodymium was found to be highly concentrated around the FeO grain boundaries, whereas oxygen and fluorine are were found at very low concentrations. This led to the conclusion that a small fraction of oxyfluoride is present in this system; however, most of the neodymium oxide got converted into neodymium fluoride.

In-situ formation of REF3 is very important since the solubility of REOs is very low in molten fluorides [20]. Further, an additional advantage is that the formation of rare earth oxyfluoride is likely to be inhibited. Stefanidaki et al. [20] have studied the oxide solubility and Raman spectra of Nd2O3 in the molten alkali fluorides. The authors have reported that the octahedral [NdF6]3− anion is the dominant complex in the eutectic NdF3–LiF melt system. With the addition of Nd2O3, complexes that are likely to be formed in the melt would be [NdOF4]3− and [NdOF5]4−. These authors have suggested reaction (14) for the solubility of neodymium oxide in the LiF–NdF3 eutectic melt. Taxil et al. [15] showed that the oxyfluoride is an insoluble compound. The controversy of the present results demands for the further investigation on the impact of the oxyfluoride; hence further research is needed on the solubility of the formed oxyfluoride and the possible reduction mechanism.

The cyclic voltammetry (CV) results for the LiF–Nd2O3 system showed that the neodymium oxyfluoride is not reduced to neodymium metal; hence this system is unsuitable for neodymium production [12]. In the voltammetric characterization of the LiF–NdF3–Nd2O3 system, the same voltammogram is found for the LiF–NdF3 system [12]. It is concluded that neodymium is reduced on the cathode by electroreduction of neodymium fluorides (present in the form of [NdF6]3−), while oxygen is generated on the glassy carbon anode by the oxidation of neodymium oxyfluorides (present in the form of [NdOF5]4−), producing CO and CO2 gases. According to Taxil et al. [15], RE fluorides in the presence of the metal oxides will form rare earth oxyfluoride which is an insoluble product and thus it cannot participate in the electrochemical reactions. Dysinger and Murphy [21] have explained that the formation of neodymium oxyfluoride could be one factor to decrease the current efficiency. Hence the formation of rare earth oxyfluoride as an insoluble product is a significant drawback in the extraction of rare earth in molten salts, since they do not participate in the cathodic reactions and thereby lower the current efficiency. However, conversion of neodymium oxide into neodymium fluoride preempts the formation of neodymium oxyfluoride, since neodymium fluoride formation is thermodynamically favorable and it is formed directly as a result of the chemical reaction between neodymium oxide and fluorinating agents.


The maximum conductivity of the electrolyte is usually observed at the eutectic compositions of the fluoride salts. In all the experiments in this work, the stoichiometry of neodymium oxide and the fluorinating agent was calculated based on theoretical values of reactions 14, assuming that if complete conversion of neodymium oxide occurs, then LiF–NdF3 forms the eutectic composition. The eutectic composition of LiF–NdF3 system was experimentally determined to be 0.23 mol fraction of NdF3 [19] and was calculated to be about 0.25 mol fraction of NdF3 by van der Meer et al. [22]. The LiF–NdF3 phase diagram determined by the same researchers using the experimental data is shown in Fig. 15.
Fig. 15

The optimized LiF–NdF3 phase diagram: (filled square) experimental data liquidus; (filled triangle) experimental data solidus [19, 22]

In the case of many systems, the microstructure is dependent on the growth conditions; thus the cooling rate and conditions. Hence it does not resemble the molten state of the salt. However, the volume fraction ratio of the two eutectic phases can lead to the formation of lamellar, fibrous, or mixed microstructures. In general, when both phases have comparable volume fractions, a lamellar structure is formed [23].

Due to the fast cooling using liquid nitrogen in all four systems, a fine eutectic structure with small alternations LiF and NdF3 lamellar is formed (Figs. 5, 8, 11, 14). In LiF–Nd2O3–ZnF2 and LiF–Nd2O3–FeF3 systems, XRD analysis shows that most of the neodymium oxide is converted into neodymium fluoride. Hence the composition of the LiF–NdF3 mixture would be close to the eutectic. The lamellar microstructure of the NdF3 light phase in the LiF dark phase shown in Figs. 7, 8, 10, and 11 infers that the volume fraction of LiF and NdF3 is close to the eutectic composition. Also in the case of the system LiF–Nd2O3–Nd2Al3F6, the lamellar microstructure is observed; however, in this system Nd1.5Na1.5F6 is formed instead of NdF3. There are insufficient data in the literature for this system, but the microstructure observations show that LiF–Nd1.5Na1.5F6 behaves very similar to the eutectic composition of LiF–NdF3 system. In the LiF–Nd2O3–AlF3 system, the presence of NdAlO3 shows that not all the neodymium oxide is converted into neodymium fluoride. Hence the volume fraction of NdF3 is expected to be lower than 0.25. With decrease in the volume fraction of one
$$ {\text{Nd}}_{2} {\text{O}}_{3} + {\text{NdF}}_{3} + 3\left( {x - 1} \right){\text{LiF}} \rightleftarrows \varvec{ }3{\text{NdOF}}_{x}^{{\left( {x - 1} \right) - }} + 3\left( {x - 1} \right){\text{Li}}^{ + } \;\;\;\; x = { 4},{ 5} $$
phase below 0.29, the microstructure forms the fibrous pattern. Fibrous microstructure in Fig. 5 indicates that the microstructure corresponds to a non-eutectic phase. With the increasing growth velocity, the dimensions of the two phases are expected to decrease [23, 24].

Alloy Formation

The neodymium fluoride which is formed will be dissolved in the molten LiF and will be subjected to electrolysis when the appropriate voltage is applied. As shown in Fig. 1, the voltage needed for NdF3 electrolysis would be higher than the decomposition voltage of the other oxides which are present in the system. Hence the dissolved Al2O3, ZnO, and FeO will also participate in the electro-decomposition process, and the co-deposition of Al, Zn, and Fe will occur at the cathode. Therefore, removal of the undissolved oxides so as to minimize their side effect on cathodic deposition of Nd is a challenging task. A new design of a two-chamber furnace system is one way for removing the undissolved oxides. The density difference between the formed oxide and the fluoride bath could also be used to separate the oxides from the molten salt.

At the carbon anode, there is likely to be a competition between oxygen gas and fluorine gas evolution. In the former case, oxidation reactions between the carbon anode and the oxygen gas lead to the formation of CO or CO2 gas (reactions 1112) and in the latter case, reaction between fluorine gas and the carbon anode results in the formation of fluorocarbon compounds (reaction 13), such as CF4 and C2F6 [25]. CO and CO2 evolutions have more negative potentials than fluorocarbon or fluorine gas evolution. According to Stefanidaki et al. [12], fluorocarbon generation on the anode can be inhibited by controlling the cell voltage. However, in order to avoid fluorine gas formation, the use of an alternative anode is proposed which will be explained in a further study as the electro-decomposition part of the same project which will follow.

Regarding the cathodic reactions, formation of Nd–Fe alloy is desirable since it can be used as a master alloy for magnet production. In this regard, using FeF3 as the fluorinating agent would be a great advantage.

In general, RE-Al can be applied to improve the magnetic properties of the RE magnets. Dy–Ni–Al eutectic alloy is used in grain boundary diffusion treatment in neodymium magnets in order to improve coercivity [26]. Alloying pure aluminum with rare earth elements is also an effective means to reduce the defect formation in films which are used to interconnect lines in large-scale integration circuits [27].

In the case when cryolite is used, Nd2O3 is converted into Na1.5Nd1.5F6 instead of NdF3. In the electrolysis step, Na reduction with Nd from Na1.5Nd1.5F6 and Al reduction from Al2O3 are expected. Hence Nd–Al–Na alloy is formed at the cathode. In order to avoid Na reduction, AlF3 should be used instead of Na3AlF6.

Nd–Zn alloy can be used for magnesium alloying in the production of novel composites. Zn is the major alloying element of the magnesium materials, and it has been proven that rare earth elements are the most effective alloying elements used to improve the strength and corrosion behavior of zinc [28, 29].


The results of XRD and EPMA analyses show that AlF3, ZnF2, and FeF3 can act as strong fluorinating agents for neodymium oxide. In all these systems, neodymium oxide was converted into neodymium fluoride. By the addition of AlF3, ZnF2, and FeF3 to the LiF–Nd2O3 system, aluminum oxide, zinc oxide, and iron oxide are formed, respectively. In the case of Na3AlF6, Na1.5Nd1.5F6 was formed instead of NdF3. Also as a result of the conversion reaction, instead of Al2O3, AlNdO3 is formed. In general, cryolite has the least tendency for the formation of NdF3 compared to other fluorinating agents that are studied in this research.

The reaction related to cryolite has the highest Gibbs energy and hence has the lowest tendency for the formation of NdF3.

The results of this study indicate the feasibility of the conversion of the rare earth oxide into rare earth fluoride using fluorinating agents (Fig. 2). Conversion of neodymium oxide into neodymium fluoride solves the problem of low solubility of the neodymium oxide in molten fluorides, to a large extent. Once neodymium fluoride is formed, it can subsequently be electrolyzed and extracted on the cathode. The electrolysis process will be discussed in a separate paper in the future.



This research has received funding from the European Community’s Seventh Framework Programme ([FP7/2007-2013]) under Grant Agreement No 607411 (MC-ITN EREAN: European Rare Earth Magnet Recycling Network, Project website: This publication reflects only the authors’ view, exempting the Community from any liability. The authors would also like to thank Ruud Hendrikx and Richard Huizenga for the XRD analyses.


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Open AccessThis article is distributed under the terms of the Creative Commons Attribution 4.0 International License (, which permits unrestricted use, distribution, and reproduction in any medium, provided you give appropriate credit to the original author(s) and the source, provide a link to the Creative Commons license, and indicate if changes were made.

Authors and Affiliations

  1. 1.Department of Materials Science and EngineeringDelft University of TechnologyDelftThe Netherlands
  2. 2.Department of Materials EngineeringKU LeuvenLeuvenBelgium
  3. 3.Royal Institute of Technology (KTH)StockholmSweden

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