CA2531003A1 - Low temperature refining and formation of refractory metals - Google Patents
Low temperature refining and formation of refractory metals Download PDFInfo
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- CA2531003A1 CA2531003A1 CA002531003A CA2531003A CA2531003A1 CA 2531003 A1 CA2531003 A1 CA 2531003A1 CA 002531003 A CA002531003 A CA 002531003A CA 2531003 A CA2531003 A CA 2531003A CA 2531003 A1 CA2531003 A1 CA 2531003A1
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- Prior art keywords
- metal
- low temperature
- titanium
- tio2
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- C—CHEMISTRY; METALLURGY
- C22—METALLURGY; FERROUS OR NON-FERROUS ALLOYS; TREATMENT OF ALLOYS OR NON-FERROUS METALS
- C22B—PRODUCTION AND REFINING OF METALS; PRETREATMENT OF RAW MATERIALS
- C22B34/00—Obtaining refractory metals
- C22B34/10—Obtaining titanium, zirconium or hafnium
- C22B34/12—Obtaining titanium or titanium compounds from ores or scrap by metallurgical processing; preparation of titanium compounds from other titanium compounds see C01G23/00 - C01G23/08
- C22B34/129—Obtaining titanium or titanium compounds from ores or scrap by metallurgical processing; preparation of titanium compounds from other titanium compounds see C01G23/00 - C01G23/08 obtaining metallic titanium from titanium compounds by dissociation, e.g. thermic dissociation of titanium tetraiodide, or by electrolysis or with the use of an electric arc
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- C—CHEMISTRY; METALLURGY
- C22—METALLURGY; FERROUS OR NON-FERROUS ALLOYS; TREATMENT OF ALLOYS OR NON-FERROUS METALS
- C22B—PRODUCTION AND REFINING OF METALS; PRETREATMENT OF RAW MATERIALS
- C22B34/00—Obtaining refractory metals
- C22B34/10—Obtaining titanium, zirconium or hafnium
- C22B34/12—Obtaining titanium or titanium compounds from ores or scrap by metallurgical processing; preparation of titanium compounds from other titanium compounds see C01G23/00 - C01G23/08
- C22B34/1263—Obtaining titanium or titanium compounds from ores or scrap by metallurgical processing; preparation of titanium compounds from other titanium compounds see C01G23/00 - C01G23/08 obtaining metallic titanium from titanium compounds, e.g. by reduction
- C22B34/1281—Obtaining titanium or titanium compounds from ores or scrap by metallurgical processing; preparation of titanium compounds from other titanium compounds see C01G23/00 - C01G23/08 obtaining metallic titanium from titanium compounds, e.g. by reduction using carbon containing agents, e.g. C, CO, carbides
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- C—CHEMISTRY; METALLURGY
- C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
- C25C—PROCESSES FOR THE ELECTROLYTIC PRODUCTION, RECOVERY OR REFINING OF METALS; APPARATUS THEREFOR
- C25C3/00—Electrolytic production, recovery or refining of metals by electrolysis of melts
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- C—CHEMISTRY; METALLURGY
- C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
- C25C—PROCESSES FOR THE ELECTROLYTIC PRODUCTION, RECOVERY OR REFINING OF METALS; APPARATUS THEREFOR
- C25C3/00—Electrolytic production, recovery or refining of metals by electrolysis of melts
- C25C3/26—Electrolytic production, recovery or refining of metals by electrolysis of melts of titanium, zirconium, hafnium, tantalum or vanadium
- C25C3/28—Electrolytic production, recovery or refining of metals by electrolysis of melts of titanium, zirconium, hafnium, tantalum or vanadium of titanium
Abstract
This invention discloses and claims the low temperature reduction and purification of refractory metals, metal compounds, and semi-metals. The reduction is accomplished using non~-aqueous ionic solvents in an electrochemical cell with the metal entity to be reduced. Using this invention, Ti02 is reduced directly to Ti metal at room temperature.
Description
LOW TEMPERATURE REFINING AND FORMATION OF REFRACTORY METALS
Technical Field This invention pertains to electrochemical reduction and purification of refractory metals, metal compounds and semi-metals at low temperatures in non-aqueous ionic solvents. Metals and semi-metals form oxides and they also have a significant oxygen solubility. Using the methods described herein below 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.
Background Art The Droll process and Hunter process are methods currently in use for the production of titanium metal from titanium dioxide. In these methods, Ti02 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 Droll 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.
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 TiOX forming an oxygenated Ca species, CaO, which is soluble in the melt forming Ca+~ and O-2. The second mechanism proposed was the direct electrochemical reduction of the TiOX 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 C02.
Disclosure of Invention We have established that a refractory metal oxide can be electrochemically reduced directly to the metal at room temperature. In this, Ti0 2 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 A1 wire was used as a reference electrode. After determining a voltage at which TiO 2 could be converted to Ti metal, a current was passed through the electrochemical system at the determined voltage to produce Ti metal.
Brief Description of Drawings 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 TiOz 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 Ti02 recorded on the reduced bulk Ti02 discussed below using the apparatus shown in Figure 2.
Figure 4 shows XPS spectra of TiOz Anatase.
Best Mode for Carrying Out the Invention In this invention, TiO2 has been 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 Ti02, current was passed through the system at a voltage predetermined to reduce the metal oxide. In this invention, a compound MX is reacted iri an electrochemical system to remove X from MX. X may be an element chemically combined with M as for instance Ti02, 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.
In this invention, M is a metal or a semi-metal, while MX is a metal compound, or a semi-metal compound or a metal or semi-metal with X being dissolved in M.
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 described by Chauvin et al, Chemtech, 26-28 (1995).
Technical Field This invention pertains to electrochemical reduction and purification of refractory metals, metal compounds and semi-metals at low temperatures in non-aqueous ionic solvents. Metals and semi-metals form oxides and they also have a significant oxygen solubility. Using the methods described herein below 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.
Background Art The Droll process and Hunter process are methods currently in use for the production of titanium metal from titanium dioxide. In these methods, Ti02 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 Droll 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.
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 TiOX forming an oxygenated Ca species, CaO, which is soluble in the melt forming Ca+~ and O-2. The second mechanism proposed was the direct electrochemical reduction of the TiOX 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 C02.
Disclosure of Invention We have established that a refractory metal oxide can be electrochemically reduced directly to the metal at room temperature. In this, Ti0 2 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 A1 wire was used as a reference electrode. After determining a voltage at which TiO 2 could be converted to Ti metal, a current was passed through the electrochemical system at the determined voltage to produce Ti metal.
Brief Description of Drawings 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 TiOz 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 Ti02 recorded on the reduced bulk Ti02 discussed below using the apparatus shown in Figure 2.
Figure 4 shows XPS spectra of TiOz Anatase.
Best Mode for Carrying Out the Invention In this invention, TiO2 has been 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 Ti02, current was passed through the system at a voltage predetermined to reduce the metal oxide. In this invention, a compound MX is reacted iri an electrochemical system to remove X from MX. X may be an element chemically combined with M as for instance Ti02, 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.
In this invention, M is a metal or a semi-metal, while MX is a metal compound, or a semi-metal compound or a metal or semi-metal with X being dissolved in M.
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 described by Chauvin et al, Chemtech, 26-28 (1995).
- The non-aqueous ionic liquids used in the reactions of this invention described above were either 1-ethyl-3-methylimidazolium tetrafluoroborate or 1-ethyl-3-methylimidazolium chloride (EMIC) and aluminum chloride. The latter solvent was prepared by mixing A1C13 with EMIC in a 0.8 to 1.0 mole ratio. Non-aqueous ionic liquids have been studied and reported upon by C.L. Hussey in Claemistfy of Nonaqueous Solutions, Mamantov and Popov, eds., VCH
publishers, chapter 4 (1994), and McEwen et al. Thermoc7Zemica 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 dialkylimidazolium 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 imidazolium compounds thus allowing for higher temperature use.
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, or alloys thereof or mixtures thereof.
The Symbol X is representative of ~, C, N, S, P, As, Sb, and halides.
Phosphorus, arsenic, and antimony are impurities particularly associated with the semi-metals Ge, and Si whose purity is critical to the function as semi-conductors.
Experimental To establish the efficacy of the invention described and claimed herein, the following experiments were conducted. Titanium foil 10 cm long by 2 mm wide by 0.25 mm thick was oxidized in a furnace at 550 °Cin air for 140 hours. A simple test tube type electrochemical cell as illustrated in Figure 2 was used, and experiments were carned out in a dry box. The cell contained a non-aqueous ionic liquid comprising aluminum chloride and 1-ethyl-methyimidazolium chloride (EMIC) in a mole ratio of 0.8:1.0 respectively giving a mole fraction of A1C13 of 0.44. A sample of the Ti02 prepared above was placed in the cell so that ~l cm was immersed in the electrolyte. The TiOz 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 TiOa strip was removed in a short time at ambient temperature. Figure 1 shows the voltammograms recorded at a sweep rate of SOmV/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 -1.6V for 15 minutes, then the sweep was continued. The first full sweep after the 15 minute reaction is shown in 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 occurnng in this peak.
In another experiment to determine if bulk Ti~Z could be reduced to Ti, a basket was made of 40 mesh titanium gauze, and then ~1 mm diameter particles of Ti02 anatase obtained from Alfa Aesar were placed in the basket. The basket and particles were then placed in a fresh vial of EMIC-A1C13 electrolyte and the electrolysis was carried out again with the setup shown in Figure 2. After 14 hours at an applied voltage of -1.~V, the sample basket was removed from the cell and the Ti~2 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.
X-ray photoelectron spectroscopy (XPS) was carned out on the isolated samples after reduction to determine if the titanium oxide had been reduced to titanium metal. The XFS data for the electrolyzed sample is shown in Figure 3. The data show two sets of peaks, one for Ti and one for unreduced Ti02. 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 Ti02, 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 Ti02. Hence the actual yield of titanium metal from the electroreduction of Ti02 would be greater than the 12% found in the analysis. The reference spectrum for the initial sample of Ti02 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%.
While the experiments above are demonstrations that MX can be transformed to M, as in Ti02 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.
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 M~i to M.
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.
publishers, chapter 4 (1994), and McEwen et al. Thermoc7Zemica 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 dialkylimidazolium 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 imidazolium compounds thus allowing for higher temperature use.
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, or alloys thereof or mixtures thereof.
The Symbol X is representative of ~, C, N, S, P, As, Sb, and halides.
Phosphorus, arsenic, and antimony are impurities particularly associated with the semi-metals Ge, and Si whose purity is critical to the function as semi-conductors.
Experimental To establish the efficacy of the invention described and claimed herein, the following experiments were conducted. Titanium foil 10 cm long by 2 mm wide by 0.25 mm thick was oxidized in a furnace at 550 °Cin air for 140 hours. A simple test tube type electrochemical cell as illustrated in Figure 2 was used, and experiments were carned out in a dry box. The cell contained a non-aqueous ionic liquid comprising aluminum chloride and 1-ethyl-methyimidazolium chloride (EMIC) in a mole ratio of 0.8:1.0 respectively giving a mole fraction of A1C13 of 0.44. A sample of the Ti02 prepared above was placed in the cell so that ~l cm was immersed in the electrolyte. The TiOz 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 TiOa strip was removed in a short time at ambient temperature. Figure 1 shows the voltammograms recorded at a sweep rate of SOmV/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 -1.6V for 15 minutes, then the sweep was continued. The first full sweep after the 15 minute reaction is shown in 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 occurnng in this peak.
In another experiment to determine if bulk Ti~Z could be reduced to Ti, a basket was made of 40 mesh titanium gauze, and then ~1 mm diameter particles of Ti02 anatase obtained from Alfa Aesar were placed in the basket. The basket and particles were then placed in a fresh vial of EMIC-A1C13 electrolyte and the electrolysis was carried out again with the setup shown in Figure 2. After 14 hours at an applied voltage of -1.~V, the sample basket was removed from the cell and the Ti~2 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.
X-ray photoelectron spectroscopy (XPS) was carned out on the isolated samples after reduction to determine if the titanium oxide had been reduced to titanium metal. The XFS data for the electrolyzed sample is shown in Figure 3. The data show two sets of peaks, one for Ti and one for unreduced Ti02. 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 Ti02, 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 Ti02. Hence the actual yield of titanium metal from the electroreduction of Ti02 would be greater than the 12% found in the analysis. The reference spectrum for the initial sample of Ti02 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%.
While the experiments above are demonstrations that MX can be transformed to M, as in Ti02 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.
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 M~i to M.
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 (10)
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 a non-aqueous ionic liquid electrolyte;
B. passing a current through said system at a voltage determined to remove X
from MX;
C. isolating the reaction product resulting from removal of X from MX.
A. forming an electrolysis system comprising a MX cathode, an anode, and a non-aqueous ionic liquid electrolyte;
B. passing a current through said system at a voltage determined to remove X
from MX;
C. isolating the reaction product resulting from removal of X from MX.
2. The method according to claim 1, where M is selected from the group consisting of a metal, a metal compound, or a semi-metal compound.
3. The method according to claim 1, 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 or Nb, or alloys thereof or mixtures thereof.
4. The method of claim 1 or 10, wherein X is selected from the group consisting of O, C, N, S, F, As, Sb, or a halide.
5. The method according to claim 1 or 10, wherein X is oxygen.
6. The method according to claim 1 or 10, wherein said non-aqueous solvent is a chloroaluminate system based on nitrogen heterocyclic cations or functional equivalent thereof.
7. The method according to claim 1 or 10, wherein said non-aqueous solvent is selected from the group consisting of mono and dialkylimidazolium salts.
8. The method according to claim 1 or 10, wherein said non-aqueous solvent is a mixture of 1-ethyl-3-methylimidazolium chloride and aluminum chloride.
9. The method according to claim 1 or 10, wherein said solvent is 1-ethyl-3-methylimidazolium tetrafluoroborate.
10. 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 a non-aqueous ionic liquid electrolyte;
B. passing a current through said system at a voltage selected to remove O
from said TiO2;
C. isolating the reaction product resulting from the removal of O from TiO2.
A. forming an electrolysis system comprising a TiO2 cathode, an anode, and a non-aqueous ionic liquid electrolyte;
B. passing a current through said system at a voltage selected to remove O
from said TiO2;
C. isolating the reaction product resulting from the removal of O from TiO2.
Applications Claiming Priority (3)
| Application Number | Priority Date | Filing Date | Title |
|---|---|---|---|
| US10/602,056 US6958115B2 (en) | 2003-06-24 | 2003-06-24 | Low temperature refining and formation of refractory metals |
| US10/602,056 | 2003-06-24 | ||
| PCT/US2004/008815 WO2005010238A1 (en) | 2003-06-24 | 2004-03-17 | Low temperature refining and formation of refractory metals |
Publications (1)
| Publication Number | Publication Date |
|---|---|
| CA2531003A1 true CA2531003A1 (en) | 2005-02-03 |
Family
ID=33539479
Family Applications (1)
| Application Number | Title | Priority Date | Filing Date |
|---|---|---|---|
| CA002531003A Abandoned CA2531003A1 (en) | 2003-06-24 | 2004-03-17 | Low temperature refining and formation of refractory metals |
Country Status (4)
| Country | Link |
|---|---|
| US (1) | US6958115B2 (en) |
| EP (1) | EP1649082A4 (en) |
| CA (1) | CA2531003A1 (en) |
| WO (1) | WO2005010238A1 (en) |
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| US7510680B2 (en) * | 2002-12-13 | 2009-03-31 | General Electric Company | Method for producing a metallic alloy by dissolution, oxidation and chemical reduction |
| US7169285B1 (en) * | 2003-06-24 | 2007-01-30 | The United States Of America As Represented By The Secretary Of The Navy | Low temperature refining and formation of refractory metals |
| WO2005103338A1 (en) * | 2004-04-27 | 2005-11-03 | Technological Resources Pty. Limited | Production of iron/titanium alloys |
| US7531021B2 (en) | 2004-11-12 | 2009-05-12 | General Electric Company | Article having a dispersion of ultrafine titanium boride particles in a titanium-base matrix |
| WO2006074523A1 (en) * | 2005-01-13 | 2006-07-20 | Commonwealth Scientific And Industrial Research Organisation | Recovery of metals |
| AU2007212481A1 (en) * | 2006-02-06 | 2007-08-16 | E. I. Du Pont De Nemours And Company | Method for electrolytic production of titanium and other metal powders |
| EP3561091A1 (en) | 2011-12-22 | 2019-10-30 | Universal Achemetal Titanium, LLC | A method for extraction and refining of titanium |
| CN102943182B (en) * | 2012-11-30 | 2014-06-11 | 上海大学 | Electrochemical deoxidization method for refining titanium and titanium alloy solution |
| CN102995065B (en) * | 2012-12-07 | 2015-01-14 | 山东理工大学 | Method for preparing metal titanium by taking ionic liquid as electrolyte and performing electro-deoxidization at room temperature |
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| WO2015069703A1 (en) | 2013-11-06 | 2015-05-14 | Bristol-Myers Squibb Company | Immunotherapeutic dosing regimens and combinations thereof |
| CN104150650A (en) * | 2014-08-15 | 2014-11-19 | 攀钢集团工程技术有限公司 | Method for electrochemically treating vanadium oxide production process wastewater |
| JP2017537927A (en) | 2014-12-04 | 2017-12-21 | ブリストル−マイヤーズ スクイブ カンパニーＢｒｉｓｔｏｌ−Ｍｙｅｒｓ Ｓｑｕｉｂｂ Ｃｏｍｐａｎｙ | Combination of anti-CS1 and anti-PD1 antibodies to treat cancer (myeloma) |
| CN104499002A (en) * | 2014-12-10 | 2015-04-08 | 上海大学 | Method for preparing copper-iron nano plated layer from low-grade sulfide ore through direct electro-deposition |
| HRP20211478T1 (en) | 2015-06-29 | 2021-12-24 | Bristol-Myers Squibb Company | Immunotherapeutic dosing regimens comprising pomalidomide and an anti-cs1 antibody for treating cancer |
| CN105154916B (en) * | 2015-08-13 | 2017-09-12 | 长沙矿冶研究院有限责任公司 | A kind of method of impurity content of magnesium in fractional precipitation reduction electrolytic manganese system |
| CN106400058B (en) * | 2016-09-14 | 2018-05-29 | 闽南师范大学 | A kind of preparation method of water solubility germanium nano-particle |
| BR112019005038B1 (en) | 2016-09-14 | 2022-12-20 | Universal Achemetal Titanium, Llc | A METHOD TO PRODUCE TITANIUM-ALUMINUM-VANADIUM ALLOY |
| CA3049769C (en) | 2017-01-13 | 2023-11-21 | Universal Achemetal Titanium, Llc | Titanium master alloy for titanium-aluminum based alloys |
| CN112267031B (en) * | 2020-10-10 | 2022-11-01 | 青海民族大学 | Method for extracting lithium by using phosphate ionic liquid |
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| US5552241A (en) * | 1995-05-10 | 1996-09-03 | Electrochemical Systems, Inc. | Low temperature molten salt compositions containing fluoropyrazolium salts |
| GB9812169D0 (en) * | 1998-06-05 | 1998-08-05 | Univ Cambridge Tech | Purification method |
| US6368486B1 (en) * | 2000-03-28 | 2002-04-09 | E. I. Du Pont De Nemours And Company | Low temperature alkali metal electrolysis |
| US6527938B2 (en) * | 2001-06-21 | 2003-03-04 | Syntheon, Llc | Method for microporous surface modification of implantable metallic medical articles |
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- 2004-03-17 WO PCT/US2004/008815 patent/WO2005010238A1/en active Application Filing
- 2004-03-17 EP EP04801778A patent/EP1649082A4/en not_active Withdrawn
- 2004-03-17 CA CA002531003A patent/CA2531003A1/en not_active Abandoned
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| EP1649082A1 (en) | 2006-04-26 |
| US20040262166A1 (en) | 2004-12-30 |
| WO2005010238A1 (en) | 2005-02-03 |
| EP1649082A4 (en) | 2007-03-21 |
| US6958115B2 (en) | 2005-10-25 |
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