WO2006009700A2

WO2006009700A2 - Low temperature refining and formation of refractory metals

Info

Publication number: WO2006009700A2
Application number: PCT/US2005/020994
Authority: WO
Inventors: William E. O'grady; Graham T. Cheek
Original assignee: US Naval Research Laboratory NRL; Government of the United States of America
Current assignee: US Naval Research Laboratory NRL; Government of the United States of America
Priority date: 2004-06-16
Filing date: 2005-06-15
Publication date: 2006-01-26
Anticipated expiration: 2006-12-16
Also published as: WO2006009700A3; WO2006009700B1

Abstract

A low temperature method for reducing and purifying refractory metals, metal compounds, and semi-metals using a catalyst. Using this invention, TiO2 can be reduced directly to Ti metal at room temperature. The catalyst is an ion in an electrolyte that catalyzes the rate of the reduction of a compound MX to M, wherein M is a metal or a semi-metal; MX is a metal compound, a semi-metal compound, or a metal or semi-metal dissolved as an impurity in M; and X is an element chemically combined with or dissolved in M.

Description

LOW TEMPERATURE REFINING AND FORMATION OF REFRACTORY METALS

This application claims the benefit of U.S. Application No. 10/868,273 filed on 06/16/2004 which is a continuation of U.S. Application No. 10/602,056 filed on 06/24/2003.

Technical Field

[0001] The present application relates to refining and formation of refractory metals and, more specifically, to electrochemical reduction and purification of refractory metals, metal compounds, and semi- metals at low temperatures in non-aqueous ionic solvents using catalysts.

Background Art

[0002] The Kroll process and Hunter process are methods currently in use for the production of titanium metal from titanium dioxide. In these methods, TiO₂ is reacted with chlorine gas to produce titanium tetrachloride, a volatile corrosive liquid. This is reduced to titanium metal by reacting with metallic magnesium in the Kroll process or with sodium in the Hunter process. Both processes are carried out at high temperatures in sealed reactors. Following this, a two-step refining process is carried out which includes two high temperature vacuum distillations to remove the alkali metal and its chloride from titanium metal. [0003] The refining of titanium by electrochemical means has long been a sought after process. It has been shown in the literature that oxygen could be removed from titanium and titanium alloys using an electrochemical high temperature molten salt method. This has led to the development of a possible new method of extracting and refining titanium directly from the oxide ore and was published by G. Z. Chen, D.J. Fray and T. W. Farthing in Nature 407, 361 (2002), and PCT international application publication number WO 99/64638,16 December 1999. This process involves electrochemistry in a high temperature molten salt, molten CaCl₂ at -800° C. In these publications, two different mechanisms are proposed for the reduction of titanium oxides. In the first mechanism, it is proposed that the Ca⁺² ions are reduced to metallic Ca at the cathode. Then the Ca metal chemically reacts with the TiO_x forming an oxygenated Ca species, CaO, which is soluble in the melt forming Ca⁺² and O^"2. The second mechanism proposed was the direct electrochemical reduction of the TiO_x to Ti metal and an oxygen species such as O^"2. This is followed by the migration of the O^'2 to the carbon anode where it forms a volatile species such as CO or CO₂.

Disclosure of Invention

[0004] The current technology of refining and formation of refractory metals is improved by the present invention wherein a low temperature electrochemical method is used for the reduction and purification of refractory metals, metal compounds, and semi-metals using one or more catalysts, the catalyst being an ion in an electrolyte that catalyzes the rate of the reduction of a compound MX to M. [0005] A refractory metal oxide can be electrochemically reduced directly to the metal at room temperature. To do this, TiO₂ was immersed in a non-aqueous ionic solvent in an electrochemical cell in which a highly oxidized titanium strip is the cathode, a Pt wire the anode, and an Al wire was used as a reference electrode. After determining a voltage at which TiO₂ could be converted to Ti metal, a current was passed through the electrochemical system at the determined voltage to produce Ti metal. The addition of a catalyst in the form of metal ions in the electrolyte can substantially catalyze the rate of the reduction of a metal oxide, in this case TiO₂.

[0006] The present invention has several advantages. Using the methods described herein it is possible to produce metals such as titanium from bulk titanium dioxide at significant cost savings. Further, it is possible to reduce or remove the oxides on highly oxidized titanium metal surfaces.

Brief Description of Drawings

[0007] These and other objects, features, and advantages of the invention, as well as the invention itself, will become better understood by reference to the following detailed description, appended claims, and accompanying drawings where: Figure 1 shows the voltage window for the production of Ti from TiO₂ in a non-aqueous ionized solvent;

Figure 2 shows the apparatus used to demonstrate the invention and produce the results shown in Figure 1;

Figure 3 shows XPS data for Ti, and TiO₂ recorded on the reduced bulk TiO₂ discussed below using the apparatus shown in Figure 2; and

Figure 4 shows XPS spectra OfTiO₂ Anatase.

Best Mode for Carrying Out the Invention

[0008] In the parent application, it was shown that TiO₂ can be reduced to Ti at room temperature using an electrochemical electrolysis system and a non-aqueous ionic solvent. To accomplish the reduction, or the removal of oxygen from TiO₂ , current was passed through the system at a voltage predetermined to reduce the metal oxide. In this invention, a compound MX is reacted in an electrochemical system to remove X from MX. X may be an element chemically combined with M as for instance TiO₂, or dissolved in M. For instance O may react with M to form oxides, or it may also be dissolved as an impurity in M. [0009] M is a metal or a semi-metal, while MX is a metal compound, a semi-metal compound, or a metal or semi-metal with X being dissolved in M.

[0010] The non-aqueous ionic liquid solvent electrolytes used in this invention are mono- and dialkylimidazolium salts mixed with aluminum chloride. This is a class of compounds known as organochloroaluminates. This class of compounds has been found to posses a wide electrochemically stable window, good electrical conductivity, high ionic mobility and a broad range of room temperature liquid compositions, negligible vapor pressure and excellent chemical and thermal stability. These compounds have been described by Chauvin et al, Chemtech, 26-28 (1995).

[0011] The non-aqueous ionic liquids used in the reactions of this invention were either l-ethyl-3- methylimidazolium tetrafluoroborate or l-ethyl-3-methylimidazolium chloride (EMIC) and aluminum chloride. The latter solvent was prepared by mixing AlCl₃ with EMIC in a 0.8 to 1.0 mole ratio. Non-aqueous ionic liquids have been studied and reported upon by CL. Hussey in Chemistry of Nonaqueous Solutions, Mamantov and Popov, eds., VCH publishers, chapter 4 (1994), and McEwen et al. Thermochemica Acta, 357-358, 97-102 (2000). The articles describe a plurality of non-aqueous ionic liquids based particularly on alkylimidazolium salts, which are useful in the instant invention. The temperature stability of these compounds makes them particularly attractive for this application because they are stable over a considerable range up to 200° C, and encompassing room temperature (20° C to 25° C) The preferred compounds for use as the ionic liquids are the dialkylimidazohum compounds In addition, the substitution of alkyl groups for hydrogen atoms on carbon atoms in the ring increases the electrochemical and thermal stability of the resulting lmidazohum compounds thus allowing for higher temperature use [0012] In a preferred embodiment, the metals and semi-metals represented by the symbol M comprise Ti,

Si, Ge, Zr, Hf, Sm, U, Al, Mg, Nd, Mo, Cr, Li, La, Ce, Y, Sc, Be, V or Nb, alloys thereof, or mixtures thereof [0013] In a further preferred embodiment, the symbol X is representative of O, C, N, S, P, As, Sb, and hahdes Phosphorus, arsenic, and antimony are impurities particularly associated with the semi-metals Ge, and Si whose purity is cπtical to the function as semi-conductors [0014] This continuation-m-part application addresses a new best mode not contemplated m the parent application, that being the use of one or more catalysts, the catalyst being an ion m the electrolyte, regardless of the temperature or nature of the electrolyte (e g molten salt, ionic-liquid, aqueous), that catalyzes the reduction rate of a compound MX to M [0015] The ion chosen to act as a catalyst must have the property of having a lower reduction potential than the reduction potential of the compound, MX, being reduced In the example discussed below, the Ag⁺ ion is reduced to Ag metal at -1 2 V while T1O₂ is reduced at -1 8 V The mechanism for this process is the reduction of the silver, in this case, to form metallic particles on the surface of the T1O₂ This causes a voltage drop between these particles and the oxide, and the oxide around the particle is reduced to Ti metal Then the Ti also begins to act as an electrode for the reduction and hence the oxide is very rapidly completely reduced starting at the outside of the oxide particle and moving inward

Example 1

[0016] To establish the efficacy of the invention described and claimed herein the following expeπments were conducted Titanium foil 10 cm long by 2mm wide by 0 25mm thick was oxidized in a furnace at 55O⁰Cm air for 140 hours A simple test tube type electrochemical cell as illustrated in Figure 2 was used and expeπments were carried out m a dry box The cell contained a non-aqueous ionic liquid comprising aluminum chloride and l-ethyl-3-methyimidazohum chloπde (EMIC) m a mole ratio of 0 8 1 0 respectively giving a mole fraction of AlCl₃ of 0 44 A sample of the TiO₂ prepared above was placed in the cell so that ~1 cm was immersed in the electrolyte The TiO₂ strip acts as the cathode, a platinum wire was used as the counter electrode or anode, and an aluminum wire was used as a reference electrode Voltage was applied to the electrolysis cell and controlled by a Princeton Applied Research 283 potentiostat through a computer controlled interface By controlling the voltage it was demonstrated that the oxide on the TiO₂ strip was removed in a short time at ambient temperature Figure 1 shows the voltammograms recorded at a sweep rate of 50mV/sec for the oxidized Ti strip after it was introduced into the electrolyte The initial sweep toward more negative voltages exhibits two clearly-defined reduction waves past -0 5 V After several cycles, the resistivity of the oxide film decreases as the titanium oxide film is reduced to the metal This is evidenced by a decrease in the overall slope of the current - voltage curve Further, the anodic peak observed in the solid curve at -0 5 V is indicative of metal dissolution, the metal having been formed in the original cathodic sweep For more extensive reduction, the voltage was held at -1 6 V This value was chosen because that voltage lies beyond the reduction waves observed in the initial cycle in Figure 1 The oxidized Ti strip was held at a voltage of -1 6 V for 15 minutes, then the sweep was continued The first full sweep after the 15 minute reaction is shown m Figure 1 with the filled dotted line. The area between the solid line and the top of the filled dotted line is the charge used to reduce the thermally grown oxide on Ti. Further, the anodic peak at -0.5 V is now considerably larger and better defined than in the initial sweep. This indicates that a substantial amount of fresh titanium metal was available for the oxidation occurring in this peak. [0017] The advocacy of a catalyst was tested by adding Ag BF₄ to form silver ions (Ag⁺) in the electrolyte

(l-ethyl-3-methylimidazolium tetrafluoroborate) in which the oxide on a fresh air oxidized titanium strip was being reduced. The potential was then held at -1.8V. Black spots appeared immediately on the surface of the electrode and grew until the entire surface was covered, about 10 minutes, when the current dropped. The sample was removed from the electrolyte and rinsed in benzene followed by acetone. The entire surface that had been submerged in the electrolyte was covered by a loosely adherent uniform black coating. The sample was then wiped with a lab wipe and all the black material came off on the lab wipe leaving a shiny metallic titanium surface while the remainder of the sample remained white covered with titanium oxide.

Example 2

[0018] Another experiment was conducted to determine if bulk TiO₂ could be reduced to Ti. A Ti basket was made of 40 mesh titanium gauze and then ~lmm diameter particles of TiO₂ anatase obtained from Alfa Aesar were placed in the basket. The basket and particles were then placed in a fresh vial of EMIC-AlCl₃ electrolyte and the electrolysis was carried out again with the setup shown in Figure 2. After 14 hours at an applied voltage of -1.8V, the sample basket was removed from the cell and the TiO₂ particles which were initially white were now dark gray. The particles were rinsed with benzene to remove the electrolyte, and the sample sealed in a vial and removed from the dry box in which the electrolysis experiments were carried out. When the titanium reaction particles were removed from the vial they were initially dark gray-almost black, but in time turned light gray with a blue cast.

[0019] X-ray photoelectron spectroscopy (XPS) was carried out on the isolated samples after reduction to determine if the titanium oxide had been reduced to titanium metal. The XPS data for the electrolyzed sample is shown in Figure 3. The data show two sets of peaks, one for Ti and one for unreduced TiO₂. Analysis showed that ~12% of the Ti observed in the data is metallic titanium. In order to obtain good XPS data, the sample was washed with water and rinsed with isopropyl alcohol. The sample for analysis was prepared using a standard preparation technique. After grinding several of the particles of the reduced TiO₂, the resulting powder was pressed into a piece of indium foil and introduced into the XPS spectrometer where the data were recorded. The grinding processes further exposes the Ti metal to air which would produce more TiO₂. Hence the actual yield of titanium metal from the electroreduction of TiO₂ would be greater than the 12% found in the analysis. The reference spectrum for the initial sample of TiO₂ is shown in figure 4. This shows that there is no metallic titanium in the reference sample. This experiment was repeated using a platinum basket made from 50 mesh gauze. Following the reduction, the powder resulting from the grinding was pressed into a gold foil. The yield of Ti in this experiment was ~20%.

]0020] While the experiments above are demonstrations that MX can be transformed to M, as in TiO₂ to

Ti metal, it should be clear that for any non-aqueous ionic liquid electrolyte having the proper stable electrochemical voltage window, that any MX can be converted to M. [0021] Commercially, the electrochemical cell would consist of the MX cathode, the non-aqueous ionic electrolyte, and an anode selected and compatible with the voltage required for the reaction of converting MX to M. It is possible to carry out this process in a packed bed reactor or a fluidized bed reactor. [0022] The above description is that of a preferred embodiment of the invention. Various modifications and variations are possible in light of the above teachings. It is therefore to be understood that, within the scope of the appended claims, the invention may be practiced otherwise than as specifically described. Any reference to claim elements in the singular, e.g. using the articles "a," "an," "the," or "said" is not construed as limiting the element to the singular.

Claims

ClaimsWhat is claimed:

1. A low temperature electrochemical method for removing specie X from compound MX, comprising the steps of: A. forming an electrolysis system comprising a MX cathode, an anode, and an electrolyte that includes at least one catalyst;

B. passing a current through said system at a voltage determined to remove X from MX; and

C. isolating the reaction product resulting from removal of X from MX.

2. The method according to claim 1, wherein said electrolyte is a non-aqueous ionic-liquid electrolyte.

3. The method according to claim 1 or 2, where M is selected from the group consisting of metals, metal compounds, semi-metal compounds, and any combination thereof.

4. The method according to claim 1 or 2, where M is selected from the group consisting of Ti, Si, Ge, Zr, Hf, Sm, U, Al, Mg, Nd, Mo, Cr, Li, La, Ce, Y, Sc, Be, V, Nb, any alloy thereof, and any combination thereof.

5. The method of claim 1 or 2, wherein X is selected from the group consisting of O, C, N, S, and halides.

6. The method according to claim 1 or 2, wherein X is O.

7. A low temperature electrochemical method for removing O from TiO₂, comprising the steps of: A. forming an electrolysis system comprising a TiO₂ cathode, an anode, and an electrolyte that includes at least one catalyst;

B. passing a current through said system at a voltage selected to remove O from said TiO₂; and

C. isolating the reaction product resulting from the removal of O from TiO₂.

8. The method according to claim 1, 2 or 7, wherein said electrolyte is a non-aqueous chloroaluminate system based on nitrogen heterocyclic cations or the functional equivalent thereof.

9. The method according to claim 1, 2 or 7, wherein said electrolyte is a non-aqueous solvent selected from the group consisting of mono and dialkylimidazolium salts.

10. The method according to claim 1, 2 or 7, wherein said electrolyte is a non-aqueous solvent mixture of l-ethyl-3-methylimidazolium chloride and aluminum chloride.

11. The method according to claim 1, 2 or 7, wherein said electrolyte is l-ethyl-3-methylimidazolium tetrafluoroborate.

12. The method according to claim 1, 2 or 7, wherein said electrolyte is selected from the group consisting of nitriles, ethers, sulfones, sulfoxides, and amides together with a salt selected from the group consisting of tetraalkylammonium salts, triflouromethanesulfonate salts and tetraflouroborate salts.

13. The method according to claim 1, 2, or 7, wherein said catalyst is selected from the group of materials which are reduced at less negative reducing potentials than M in MX in claim 1 or 2 or Ti in claim 7. 14 The method according to claim 1, 2, or 7, wherein said catalyst is a metal ion selected from the group of metals which are reduced at less negative reducing potentials than M in MX in claim 1 or 2 or Ti in claim 7

15 The method according to claim 1, 2, or 7, wherein said catalyst is a metal ion added to the electrolyte as a compound containing the desired metal ion or a metal or alloy that produces the desired metal ion in the electrolyte with said metal ion being selected from the group of metals which are reduced at less negative reducing potentials than M in MX in claim 1 or 2 or Ti in claim 7

16 The method according to claim 1, 2, or 7, wherein said catalyst is a metal ion added to the electrolyte by adding a soluble salt containing the metal ion, wherein said metal ion is selected from the group of metals which are reduced at less negative reducing potentials than M m MX in claim 1 or 2 or Ti in claim 7

17 The method according to claim 7, wherein said catalyst is Ag

18 The method according to claim 1, 2, or 7, wherein said electrolysis occurs in a fluidized bed reactor or a packed bed reactor

19 A method of adding at least one catalyst to an electrolyte system, comprising depositing the catalyst onto the surface of a material being reduced regardless of the temperature or nature of the electrolyte, wherein said catalyst acts to reduce the supporting mateπal

20 The method of claim 19, wherein the electrolyte is selected from the group consisting of molten salts, ionic liquids, aqueous solutions, and any combination thereof.