Study on Electrochemical Behavior of La(III) and Preparation of Al−La Intermetallic Compound Whiskers in Chloride Melt

De-Bin Ji; Yong-De Yan; Mi-Lin Zhang; Pu Wang; Xue Yang; Xiao-Yan Jing; Yun Xue; Wei Han; Thomas Hartmann

doi:10.1149/2.0101602jes

Along with the development of the economy, the energy consumption issue and environmental protection have become the theme of the world. With this problem, the superlight materials have attracted much attention. Magnesium−lithium alloys are considered to the most promising new energy materials, which have drawn more and more attention by the industry of aerospace and microelectronic because of the advantages of the low density, high specific strength, good machinability, damping ability and high energetic particle penetration resistance.^1–4 Nevertheless, the widespread use of magnesium−lithium alloys is limited by the poor mechanical properties of alloy, especially the hardness.

The definition of the whisker was given by Cevans et al.:⁵ the crystal structure of the whisker is single-crystal structure, the ratio of the length to diameter is between 5 and 1000. The diameter of whisker is falling in 20 to 100 nanometer. Many researchers^6–9 have adopted the whiskers to improve the mechanical properties of magnesium−lithium alloys. On account of the binding force between the whisker and the magnesium−lithium alloys substrate is limited by the adscititious whisker, the mechanical properties of the magnesium−lithium alloy are not likely to see a great promotion. In our prior work, for the extraction of europium and formation of Al−Li−Eu alloy, most of needle-like precipitates can be formed in aluminum substrate.¹⁰ The needle-like precipitates grow through several grains and across grain boundaries. Such long needle-like precipitates should act as pins to increase the boundary strength and improve the properties of alloy. Therefore, the thought of whether the mechanical properties of the magnesium−lithium alloys can be improved by the formation of Al−RE intermetallic compound whiskers in magnesium−lithium alloy attracts our attention.

The traditional method of preparation magnesium−lithium based alloy is directly mixing and fusing the metallic element. However, many shortcomings exist in the production process:¹¹ a complex production process and a high energy consume. Therefore, the preparation of magnesium−lithium based alloys by electrochemical methods in molten salts draws an increasing attention. The advantages of molten salt electrolysis method are mainly including:¹² the alloy with different phases can be controlled by the electrochemical parameters; low-energy consume; more suitable for industrial mass production. In recently years, there are many reports about the preparation of alloys by molten salt electrolysis. The electrochemical behavior of Sm(III) in LiCl−KCl−SmCl₃¹³ and LiCl−KCl−SmCl₃−CoCl₃¹⁴ melts was reported by Ito et al. on the inert and active (Ni and Cu) electrodes, respectively. The Sm−Ni alloy containing Sm₂Ni phase and Sm−Co alloy containing SmCo₃ phase were prepared by potentiostatic/galvanostatic electrolysis. Nohira et al. studied the electrochemical behavior of Nd(III),¹⁵ Dy(III)¹⁶ and Pr(III)¹⁷ on the Mo and Ni electrodes in different molten salt systems, respectively. The Ni−Nd, Ni−Dy and Ni−Pr alloys were also successfully synthetized by molten salt electrolysis. Castrillejo et al.^18–26 and Smolenski et al.²⁷ investigated the electrochemical behavior of the Yb(III), Sm(III), Gd(III), Eu(III), Er(III), Ho(III), Pr(III), Dy(III) and Tm(III) on tungsten and aluminum electrodes in LiCl−KCl melts and prepared Al−RE alloy on an active aluminum plate. The electrochemical behavior of Sm(III), Dy(III), Th(IV), Eu(III), Gd(III) and Nd(III) had been investigated by Massot et al.^28–33 in fluorides melts on Mo, Ni, Cu and Al electrode and successfully prepared Ni−RE, Cu−RE and Al−RE alloys, respectively. For the past few years, the Mg−Li³⁴ alloy with different phases, Mg−Li−Al³⁵ alloy, Mg−Li−Al−Zn³⁶ alloy and Mg−Li−Zn³⁷ alloy were also successfully prepared by molten salts electrolysis in our group.

Lanthanum, which is the first element of the lanthanides in periodic table of chemical elements, is one of the most cheap rare earth elements. In recent years, the studies about La(III) in molten salt have been reported by many researchers. Liu et al.³⁸ investigated the electrochemical behavior of La(III) on a Mo electrode and prepared Al−La alloy with different phases (Al₂La, Al₃La and Al₁₁La₃) on a Mo electrode assisted by AlCl₃. Vandarkuzhali et al.³⁹ reported the electrochemical behavior of La(III) on a Mo and an aluminum electrodes. The results illustrates that the reduction of La(III) to metal La on inert electrode is a single step reaction with transfer three electrons. Al−La alloy with Al₁₁La₃ phase was also obtained by potentiostatic electrolysis at 798 K. Masset et al.⁴⁰ reported the electrochemical behavior of La(III) on a W electrode and calculated the diffusion apparent standard potentials of lanthanum. Based on above professional foundations, the information about the electrochemical behavior of La(III) in LiCl−KCl−MgCl₂−AlCl₃ melts and preparation of Mg−Li−Al−La alloy with whiskers by molten salts electrolysis have never been reported till to now. Thus, the reduction behavior of La(III) was investigated by different electrochemical measurements on a W electrode, and Mg−Li−Al−La alloy with whiskers was prepared on liquid magnesium electrode. The micro hardness of Mg−Li−Al−La alloy with and without whiskers was characterized by Leitz micro hardness tester.

Experimental

Preparation and purification of the melts

The electrolyte was composed of LiCl and KCl. In order to remove excess water of the electrolyte, the LiCl–KCl mixture (LiCl:KCl = 50:50 (wt%), analytical grade) was dried under vacuum condition for more than 48 h at 523 K before it was added into an alumina crucible placed in a quartz cell located in an electric furnace. The temperature of the melts was measured by the nickel–chromium thermocouple which was sheathed by an alumina tube. To remove the impurity of the molten salts, the molten salts were carefully purified by pre-electrolysis for 4 h. Lanthanum, aluminum and magnesium elements were introduced into bath in the form of dehydrated LaCl₃, AlCl₃ and MgCl₂ powder, respectively.

Electrochemical apparatus and electrodes

All of the electrochemical measures were performed by Autolab electrochemical workstation (Zahner Co., Ltd.). The reference electrode was an Ag/AgCl electrode which composed by a Pyrex tube containing a solution of AgCl (1 wt%) in LiCl–KCl (50:50 wt%) melts. All of the potentials were referred to this Ag/AgCl couple. The counter electrode was a spectral pure graphite rod of 6 mm diameter. The tungsten wire (99.99%) which diameter is 1 mm was used as the working electrode. The working electrodes were polished thoroughly using SiC paper, then cleaned ultrasonically with ethanol prior to use. The surface of working electrode was determined by measuring the immersion depth of the electrode in molten salts after each experiment.

Auxiliary techniques

The preparation of Mg−Li−Al−La alloy (containing whiskers) was carried out via galvanostatic electrolysis in LiCl−KCl melts at 1023 K after the addition of LaCl₃ and AlCl₃ on liquid magnesium electrode. The deposits were analyzed by XRD (X^' Pert Pro; Philips Co., Ltd.) using Cu−Kα radiation at 40 kV and 40 mA. Scanning electron microscopy (SEM) (JSM−6480A; JEOL Co., Ltd.) with energy dispersive spectrometer (EDS) was used to observe the microstructure and micro−zone chemical analysis of the alloys. Transmission electron microscope (TEM) (JEOL, JEM−2010) with electron diffraction was employed to investigate the crystal structure of whisker. The TEM sample preparation steps were as follows: the samples with thickness of about 0.4 mm were made by line cutting, and then were abraded and polished to about 50 um thickness with 200#, 400# and 1500# SiC paper. After that, the sample was made into circular sheet which diameter was 3 mm, and was thinned by Precision Ion Polishing System (Gatan691). The Leitz micro hardness tester with the conditions of the loading force 50 N and holding pressure time 15 s was used to measure the micro hardness of the alloy.

Results and Discussion

Cyclic voltammetry

The cyclic voltammetry was adopted to investigate the electrochemical behavior of La(III) in chloride melts. Fig. 1 illustrates the cyclic voltammograms obtained on a tungsten electrode at 1023 K in different molten salt systems. Only one pair of cathode/anode signals A/A^' (curve 1 in Fig. 1) which correspond to the formation and dissolution of metal Li in blank LiCl−KCl melts on a tungsten electrode can be observed before the additions of MgCl₂, AlCl₃ and LaCl₃. There are no others redox signals in the electrochemical window. This phenomenon indicates that blank LiCl−KCl melts apply for investigating the electrochemical behavior of La(III). After the addition of MgCl₂ (1 wt%), a new pair of cathode/anode signals B/B^' appear (curve 2 in Fig. 1). The cathode signal B at about −1.70 V is ascribed to the reduction of Mg²⁺, and anode signal B^' which is associated with the dissolution of the metal magnesium is detected at about −1.51 V. Curve 3 in Figure 1 exhibits the cyclic voltammogram obtained on a tungsten electrode in LiCl−KCl−MgCl₂ melts after the addition of AlCl₃ (1 wt%) at 1023 K. Except for the signals A/A^' and B/B^', a new pair of electro−signals C/C^' at around −0.90 V/-0.58 V are detected. The electro−signal C in negative−going scan is ascribed to the reduction of Al(III) and the corresponding oxidation signal C^' is interpreted as the dissolution of metal aluminum, respectively. Apart from these redox signals, a new oxidation signal D^' appears between the signals C^' and B^' in positive direction. Due to the reduction potential of Mg ions is more negative than that of Al ions on a tungsten electrode, the signal D^' may be caused by the dissolution of an Al−Mg alloy,⁴¹ which is formed by the underpotential deposition of Mg on an aluminum already deposited on the tungsten electrode.

**Figure 1.** The typical cyclic voltammograms obtained on a tungsten electrode (S = 0.322 cm²) at 1023 K in different molten salt systems, curve 1: LiCl−KCl melts, curve 2: LiCl−KCl−MgCl₂ (1 wt%) melts, curve 3: LiCl−KCl−MgCl₂ (1 wt%)−AlCl₃ (1 wt%) melts. Scan rate: 0.1 V·s⁻¹.

To verify our conjecture, the semi-empirically formula of ΔUp = αΔΦ⁴² was used to estimate whether the underpotential deposition occurs or not. ΔUp denotes the potential difference, ΔΦ ascribes the difference in the work functions of the substrate and deposited metal and α = 0.5 V eV⁻¹. The ΔUp is finally calculated to be 0.31 V.⁴³ Therefore, the underpotential deposition can be occurred under our experiment condition.

To investigate the corresponding relationship of C and C^' or D^', the different scanning ranges of cyclic voltammograms were obtained on a tungsten electrode at 1023 K in LiCl−KCl−MgCl₂ (1 wt%)−AlCl₃ (1 wt%) melts (Fig. 2). Curve 1 illustrates the cyclic voltammogram plotted from −0.25 V to −0.90 V. Two pairs of redox signals can be observed. The weak signal F at around −0.67 V is possibly ascribed to the formation of an Al−W alloy. The oxidation signal F^' belongs to the dissolution of an Al−W alloy. The similar phenomenon occurs in the process of the electrochemical extraction of europium¹⁰ and yttbium.⁴⁴ When the potential reaches to −0.75 V, the reduction signal C appears, and the corresponding oxidation signal C^' is detected at around −0.61 V. At this point, the oxidation signal D^' does not appear. When the scanning range of cyclic voltammogram is switched from 0 V to −1.1 V. The oxidation signal D^' is detected. Therefore, the redox signals C/C^' are related to the formation and dissolution of the metal aluminum, and the oxidation signal D^' corresponds to the dissolution of an Al−Mg alloy.

**Figure 2.** The different scanning ranges of cyclic voltammograms obtained on a tungsten electrode (S = 0.322 cm²) at 1023 K in LiCl−KCl−MgCl₂ (1 wt%)−AlCl₃ (1 wt%) melts. Scan rate: 0.1 V·s⁻¹.

Fig. 3 exhibits the cyclic voltammogram obtained in LiCl−KCl−MgCl₂ (1 wt%)−AlCl₃ (1 wt%) melts after the addition of LaCl₃ (3 wt%) on a tungsten electrode at 1023 K. As the same as the cyclic voltammogram obtained in LiCl−KCl−MgCl₂ (1 wt%)−AlCl₃ (1 wt%) molten salts system, the redox signals A/A^', B/B^' and C/C^' are also obtained. The reduction signals A, B and C in cathodic direction are ascribed to the formation of the metals Li, Mg and Al, respectively. And the corresponding oxidation signals A^', B^' and C^' in reverse direction are related to the dissolution of the metals Li, Mg and Al, respectively. Apart from the three pairs of electrochemical signals, a new pair of redox signals G/G^' is obtained. The reduction signal G, which is detected at around −1.37 V, may be ascribed to the formation of an Al−La intermetallic compound. And the corresponding oxidation signal G^', which is detected at around −1.22 V, is related to the dissolution of an Al−La intermetallic compound. Meanwhile, in the anode direction, an oxidation signal E^' detected at about −1.42 V, between the oxidation signals B^' and G^', is probably caused by the dissolution of another kind of Al−La intermetallic compound. Nevertheless, the corresponding reduction signal E is not detected. The reasons for this phenomenon may be as follows: the reduction potential of signal E is very close to the reduction potential of the magnesium ions. Consequently, the signal E is covered by signal B. It is easy to find signal G in Fig. 3 is too wide. Therefore, another possibility is that the signal E is covered by signal G. It is worth noticing that the redox signals of the Mg−La intermetallic compound are not observed between the reduction/oxidation signals A/A^' and B/B^'. This interesting phenomenon can be explained by the electronegativity difference, which can be used to predict the formation of the intermetallic compound, between the two kinds of different elements.⁴¹ With the electronegativity difference increasing between the two elements, the formation of intermetallic compound will be easier. Therefore, the Al−La intermetallic compound will be formed under this experiment condition when the electronegativily difference between aluminum and lanthanum is larger than that between magnesium and lanthanum.

**Figure 3.** The typical cyclic voltammogram obtained on a tungsten electrode (S = 0.322 cm²) at 1023 K in LiCl−KCl−MgCl₂ (1 wt%)−AlCl₃ (1 wt%)−LaCl₃ (3 wt%) melts. Scan rate: 0.1 V·s⁻¹.

Some voltammetric data were also employed to illustrate the Al−La alloy formation directly. Fig. 4a shows the typical cyclic voltammograms obtained on a tungsten electrode (S = 0.322 cm²) at 1023 K in different molten salt systems. Two pairs of cathode/anode signals A/A^' and H/H^' (curve 1 in Fig. 4a) which correspond to the formation and dissolution of metal Li and La in LiCl−KCl−LaCl₃ (3 wt%) melts on a tungsten electrode can be observed, respectively. After the addition of MgCl₂ (1 wt%), three oxidation signals appear. Curve 2 exhibits the cyclic voltammogram obtained in LiCl−KCl−LaCl₃−MgCl₂ melts on a tungsten electrode, and Fig. 4b shows the partial enlarged view of curve 2. Except for the cathode/anode signals H/H^', oxidation signals I^', II^' and III^' can be seen in Fig. 4b. The oxidation signals I^', II^' and III^' correspond to the dissolution of three kinds of Mg−La intermetallic compounds. The cathode/anode signals B/B^' are ascribed to the formation and dissolution of metal Mg. Curve 3 in Fig. 4a exhibits the cyclic voltammogram obtained on a tungsten electrode in LiCl−KCl−LaCl₃−MgCl₂ melts after the addition of AlCl₃ (1 wt%) at 1023 K. After the addition of AlCl₃, an interesting phenomenon occurs. The oxidation signals of I^', II^' and III^' corresponding to the dissolution of three kinds of Mg−La intermetallic compounds disappear. In the meanwhile, a pair of redox signals (G/G^') and an oxidation signal E^' which are related to the formation and dissolution of two kinds of Al−La intermetallic compounds can be observed. This phenomenon successfully validates our conjecture that the Al−La intermetallic compounds will be easily formed than the Mg−La intermetallic compounds under our experiment condition.

**Figure 4.** The typical cyclic voltammograms obtained on a tungsten electrode (S = 0.322 cm²) at 1023 K in different molten salt systems (a) curve 1: LiCl−KCl−LaCl₃ (3 wt%) melts, curve 2: LiCl−KCl−LaCl₃ (3 wt%)−MgCl₂ (1 wt%) melts, curve 3: LiCl−KCl−LaCl₃ (3 wt%)−MgCl₂ (1 wt%)−AlCl₃ (1 wt%) melts (b) the partial enlarged view of curve 2. Scan rate: 0.1 V·s⁻¹.

From the comparative diagrams of cyclic voltammograms (Fig. 1 and Fig. 3), when cathode potential is more negative than −2.0 V, the rapid increasing of cathode current density is easily recognized. This phenomenon may be caused by the formation of a kind of Mg−Li alloy, which is formed by the underpotential deposition of Li(I) on magnesium already deposited on a tungsten electrode.

Square wave voltammetry

Square wave voltammetry, a more sensitive electrochemical method than cyclic voltammetry, was also adopted to further investigate the electrochemical behavior of La(III). Fig. 5 exhibits the comparative diagram of the square wave voltammograms obtained in LiCl−KCl−MgCl₂ (curve 1) and LiCl−KCl−MgCl₂ (1 wt%)−AlCl₃ (1 wt%)−LaCl₃ (3 wt%) (curve 2) melts. In curve 1, two electro−signals A and B can be observed. The signal B is associated with the reduction of magnesium ions on a tungsten electrode, which is beginning at around −1.59 V. With the increasing of the cathode potential, another electro−signal A appears. The huge cathode signal A may be caused by the formation of a Mg−Li alloy, which is in accordance with the situation of the cyclic voltammetry. From curve 1, the asymmetry of the signal B exists. This can be probably explained by the nucleation effect. An overpotential is required during a new phase formation process on a tungsten electrode, which results in the deposition potential going negative. Therefore, the left side of peak B is wider than the right one. Curve 2 displays square wave voltammogram in LiCl−KCl−MgCl₂ (1 wt%)−AlCl₃ (1 wt%) melts after the addition of LaCl₃ (3 wt%) on a tungsten electrode at 1023 K. Four new electro−signals (E, G, C and F) are obtained, which are in accordance with these obtained in cyclic voltammogram. In addition, the peak potential of signal B (curve 2) is more negative than that in curve 1. The reason is that the volume of the electrolyte increases after the addition of the LaCl₃. Therefore, the concentration of the Mg(II) decreases and results in the reduction potential going negative. Furthermore, the current density of the signal B from curve 2 is larger than that in curve 1. This phenomenon may be caused by the reason that the numbers of free ions in the electrolyte system increase after the addition of LaCl₃ and the conductivity of the electrolyte enhances.

**Figure 5.** Square wave voltammograms obtained on a tungsten electrode (S = 0.322 cm²) at 1023 K in different melts 1: LiCl−KCl−MgCl₂ (1 wt%) melts, 2: LiCl−KCl−MgCl₂ (1 wt%)−AlCl₃ (1 wt%)−LaCl₃ (3 wt%) melts, with the conditions of pulse height: 25 mV; potential step: 1 mV; frequency: 10 Hz.

Open circuit chronopotentiometry

Open circuit chronopotentiometry, as an appropriate electrochemical technique to probe mechanism of the formation and dissolution of alloy,^18,19,45 was employed to survey the equilibrium potential of alloy. First, a thin layer of the specimen was synthesized by potentiostatic electrolysis for 10 s at −2.5 V on a tungsten electrode. Then, the current was cut up and a series of electrochemical curves were obtained. Fig. 6 shows a group of open circuit chronopotentiograms obtained in different molten salt systems on a tungsten electrode at 1023 K. Before the additions of AlCl₃ and LaCl₃ in LiCl−KCl−MgCl₂ melts, two potential plateaus can be observed. The first potential plateau A at around −2.27 V is ascribed to the formation potential of metal Li on a tungsten electrode. With the extension of time, a second potential plateau B at around −1.61 V corresponds to the equilibrium potential of Mg(II)/Mg. Curve 2 exhibits the open circuit chronopotentiogram obtained in LiCl−KCl−MgCl₂ melts after the addition of AlCl₃ (1 wt%) on a tungsten electrode. Two new potential plateaus F and C are obtained. The plateau F at around −1.40 V is probably associated with the equilibrium potential of Al−Mg alloy, which is formed by the underpotential deposition of Mg on an aluminum−coated tungsten electrode. The potential plateau C at about −0.86 V is ascribed to the equilibrium potential of Al(III)/Al. After the addition of LaCl₃ in LiCl−KCl−MgCl₂−AlCl₃ melts, potential plateaus G and E appear (curve 3). The plateaus G and E at around −1.26 V and −1.47 V are probably ascribed to the equilibrium potentials of two kinds of different Al−La intermetallic compounds, respectively. To further verify whether the plateaus G (−1.26 V) and E (−1.47 V) are the equilibrium potentials of Al−La intermetallic compounds, the open circuit chronopotentiogram was measured in LiCl−KCl−AlCl₃ (1 wt%)−LaCl₃ (3 wt%) melts on a tungsten electrode at 1023 K (as shown in Fig. 7). Five plateaus are obtained. Among them, plateaus H, I and K at around −1.47 V, −1.26 V and −1.12 V are ascribed to the equilibrium potentials of the three kinds of different Al−La intermetallic compounds, respectively. And the equilibrium potentials of H and I are in accordance with the equilibrium potential of E and G, which are obtained in LiCl−KCl−MgCl₂−AlCl₃−LaCl₃ molten salt system. Till then, the plateau E in curve 3 from Fig. 6 corresponds to the equilibrium potential of Al−La intermetallic compound.

**Figure 6.** Open circuit chronopotentiograms obtained in different molten salt systems, 1: LiCl−KCl−MgCl₂ (1 wt%) melts, 2: LiCl−KCl−MgCl₂ (1 wt%)−AlCl₃ (1 wt%) melts, 3: LiCl−KCl−MgCl₂ (1 wt%)−AlCl₃ (1 wt%)−LaCl₃ (3 wt%) melts, with the conditions of potentiostatic electrolysis 10 s at −2.5 V on a tungsten electrode (S = 0.322 cm²) at 1023 K.

**Figure 7.** Comparison diagram of the open circuit chronopotentiograms obtained in the different molten salt systems, 3: LiCl−KCl−MgCl₂ (1 wt%)−AlCl₃ (1 wt%)−LaCl₃ (3 wt%) melts, 4: LiCl−KCl−AlCl₃ (1 wt%)−LaCl₃ (3 wt%) melts, with the conditions of potentiostatic electrolysis 10 s at −2.5 V on a tungsten electrode (S = 0.322 cm²) at 1023 K.

Chronopotentiometry

Chronopotentiometry is a suitable method to investigate the co-deposition mechanism of Mg(II), Li(I), Al(III) and La(III) ions in LiCl−KCl melts on a tungsten electrode in our experiment condition.⁴⁶ Fig. 8 illustrates a series of chronopotentiograms obtained on a tungsten electrode at 1023 K under the different current intensities in LiCl−KCl−MgCl₂−AlCl₃−LaCl₃ melts. With changing the current intensity, five plateaus are obtained. When the current intensity is −15 mA, first plateau C appears, which is associated with the reduction of aluminum ions on a tungsten electrode. When the current intensity reaches to −30 mA and −35 mA, the plateaus G and E are obtained, which are ascribed to the formation of two different Al−La intermetallic compounds, respectively. When the current intensity is 40 mA, the plateau B which is related to the reduction of Mg(II) appears. The last plateau A is obtained when the current intensity is more negative than −190 mA. This plateau is attributed to the reduction of Li(I). That is to say, the co-deposition of the Mg(II), Li(I), Al(III) and La(III) ions will be realized when the current intensity is more negative than −190 mA. From the chronopotentiograms, with the increasing of the current intensity, the transition time of the plateaus C and B decreases. This phenomenon indicates that the reduction of aluminum and magnesium ions is controlled by the mass transfer.^35,41,47

**Figure 8.** Chronopotentiograms with different current intensities measured on a tungsten electrode in LiCl−KCl−MgCl₂ (1 wt%)−AlCl₃ (1 wt%)−LaCl₃ (3 wt%) melts at 1023 K.

Preparation and characterization of Mg−Li−Al−La alloy containing whiskers

In this experiment, the main purpose is to prepare Al−La intermetallic compound whiskers in magnesium substrate and characterize the mechanical properties of the Mg−Li−Al−La alloy containing whiskers. However, it is difficult to obtain the bulk alloy during the co-deposition process. Therefore, the preparation of Mg−Li−Al−La alloy containing whisker was implemented by galvanostatic electrolysis on liquid magnesium electrode at 1023 K in LiCl−KCl−AlCl₃−LaCl₃ (3 wt%) melts. In consideration of the volatilization of AlCl₃, 2 g AlCl₃ powder was poured into the melts per 30 minutes. The current intensity for galvanostatic electrolysis was selected from chronopotentiograms. When the current intensity was more negative than −0.19 A, the co-deposition of the Mg(II), Li(I), Al(III) and La(III) ions could be realized. Thus, −0.20 A (S = 1.76 cm²) was employed for applying current. After electrolysis for 4.5 h, Mg−Li−Al−La alloy was cooled to the room temperature (the cooling rate is 2°C/min). Then, the Mg−Li−Al−La alloy was taken out and laid in glove box until their analysis. Fig. 9 exhibits the X-ray diffraction (XRD) of Mg−Li−Al−La alloy obtained by galvanostatic electrolysis for 4.5 h on a liquid magnesium electrode. The XRD pattern illustrates that only Al₄La and Mg phases are detected in Mg−Li−Al−La alloy. In XRD pattern, the diffraction peaks of aluminum are not observed. The reason should be that the element aluminum exists in magnesium substrate in the form of the Al−La intermetallic compound.⁴¹

**Figure 9.** X-ray diffraction pattern of Mg−Li−Al−La alloy obtained on a liquid magnesium electrode at 1023 K in LiCl−KCl−AlCl₃−LaCl₃ (3 wt%) molten salt system.

Fig. 10 exhibits the scanning electron microscope of the Mg−Li−Al−La alloy obtained on a liquid magnesium electrode at 1023 K after galvanostatic electrolysis for 4.5 h. Lots of needle-like precipitates orderly distribute in magnesium substrate. These needle-like precipitates probably are Al−La intermetallic compounds. The gray zone on cross−sectional may mainly be magnesium

**Figure 10.** SEM with EDS mapping analysis of Mg−Li−Al−La alloy obtained on liquid magnesium electrode at 1023 K in LiCl−KCl−AlCl₃−LaCl₃ (3 wt%) melts.

substrate. To certify our conjecture, the EDS mapping analysis was employed to investigate the distribution of the elements magnesium, aluminum and lanthanum. From the EDS mapping analysis spectra, it is obvious to find that the elements aluminum and lanthanum mainly distribute on needle-like precipitates, and the element magnesium mainly distributes on gray zone. In addition, the distribution of aluminum is similar to that of element lanthanum. It further verifies the view that element aluminum mainly distributes on needle-like precipitate in the form of Al−La intermetallic compound. The EDS quantitative analysis was also employed to further examine the distribution of the magnesium, aluminum and lanthanum elements (Fig. 11). Points 1 and 2 were selected from the needle-like precipitate and point 3 was selected from the gray zone. The quantitative analysis exhibits that the needle-like precipitates dissolve more aluminum and lanthanum elements than the gray zone. The element with atomic number less than 4 cannot be detected by EDS. Thus, inductive coupled plasma atomic emission spectrometer was directly used to examine the percentage composition of each element of Mg−Li−Al−La alloy. The result shows that the compositions of these elements are: 84.1 wt% Mg, 1.2 wt% Li, 8.4 wt% Al and 6.3 wt% La, respectively.

**Figure 11.** SEM with EDS quantitative analysis of Mg−Li−Al−La alloy obtained on the liquid magnesium electrode at 1023 K in LiCl−KCl−AlCl₃−LaCl₃ (3 wt%) melts.

The crystal structure of the whisker is single-crystal structure. The ratio of length to diameter is between 10 and 1000. And the diameter of the whisker is falling in 20 to 100 nanometer. From the SEM images, all of characteristic can be satisfied, except the crystal structure. Consequently, the TEM with electron diffraction was employed to investigate whether the needle-like precipitate is single crystal structure. Fig. 12 exhibits the TEM image and electron diffraction image of Mg−Li−Al−La alloy obtained by galvanostatic electrolysis for 4.5 hours at 1023 K on liquid magnesium electrode in LiCl−KCl−AlCl₃−LaCl₃ (3 wt%) melts. Lots of needle-like precipitates orderly distribute in magnesium substrate in image a. The ratio of length to diameter is between 10 and 1000, and the diameter of the needle-like precipitate falling in 20 to 100 nanometer can also be observed from image a. The point A is taken from random area of needle-like precipitates for the electron diffraction experiment. Image b exhibits the electron diffraction pattern of needle-like precipitates. The electron diffraction image shows that the diffraction spots arrange in an orderly manner, which can be used to explain the fact that the crystal structure of needle-like precipitates is single–crystal structure, and needle-like precipitates are intermetallic compound whisker.

**Figure 12.** TEM image (a) and electron diffraction pattern (b) of Mg−Li−Al−La alloy containing whiskers obtained by galvanostatic electrolysis for 4.5 hours at 1023 K on liquid magnesium electrode in LiCl−KCl−AlCl₃−LaCl₃ (3 wt%) melts.

The test of the hardness

To verify the improvement of mechanical properties of alloy with the help of Al₄La intermetallic compound whiskers, the micro hardness of alloy was measured by the micro hardness tester. Originally, two kinds of alloys with the same compositions of Mg, Li, Al and La were prepared with the same experiment condition except for the cooling rate. Fig. 13 exhibits the comparison diagram of micro hardness of the Mg−Li−Al−La alloys with and without whiskers. The column diagram 1 shows the micro hardness of Mg−Li−Al−La alloy containing whiskers obtained in LiCl–KCl–AlCl₃−LaCl₃ (3 wt%) melts at 973 K on a liquid magnesium electrode. The micro hardness is 71.25 HV. The column diagram 2 illustrates the micro hardness of Mg−Li−Al−La alloy without whiskers. The micro hardness is 63.75 HV. It is easy to find that the hardness of Mg−Li−Al−La alloy containing whiskers is higher than the alloy without whiskers.

**Figure 13.** Comparison diagram of micro hardness of Mg−Li−Al−La alloys with (column 1) and without (column 2) whiskers.

Conclusions

The electrochemical behavior of La(III) was investigated by cyclic voltammetry, square wave voltammetry, chronopotentiometry and open circuit chronopotentiometry in LiCl–KCl–MgCl₂–AlCl₃–LaCl₃ melts on a tungsten electrode at 1023 K. The results illustrate Mg−La intermetallic compound cannot be formed under this experiment condition. This interesting phenomenon maybe caused by the electronegativity difference between the two kinds of different elements. Al−La intermetallic compound can be formed while the electronegativity difference between aluminum and lanthanum is larger than that between magnesium and lanthanum. Chronopotentiometry shows that co-deposition of the Mg(II), Li(I) Al(III) and La(III) ions occurs when the current intensity is more than –190 mA. The Al−La intermetallic compound whiskers are formed in magnesium substrate after galvanostatic electrolysis for 4.5 h, and Al₄La intermetallic compound is identified via XRD. The SEM with EDS (map analysis and quantitative analysis) illustrates that elements aluminum and lanthanum mainly distribute on needle-like precipitates and element magnesium mainly distributes on gray area. The SEM and TEM show that the ratio of length to diameter is between 10 and 1000, and the diameter of the whisker is falling in 20 to 100 nanometers. The electron diffraction pattern exhibits the diffraction spots arrange in an orderly manner and the needle-like precipitates are Al−La intermetallic compound whiskers. Compared with Mg−Li−Al−La alloy without whiskers, the micro hardness of Mg−Li−Al−La alloy containing whiskers improves 11.68%.

Acknowledgments

The work was financially supported by the China Scholarship Council, the National Natural Science Foundation of China (21103033, 21101040, 91226201 and 51574097), the Fundamental Research funds for the Central Universities (HEUCF20151007), the Foundation for University Key Teacher of Heilongjiang Province of China and Harbin Engineering University (1253G016 and HEUCFQ1415), and the Special Foundation Heilongjiang Postdoctoral Science Foundation (LBH–TZ0411).

Study on Electrochemical Behavior of La(III) and Preparation of Al−La Intermetallic Compound Whiskers in Chloride Melt

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