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US3298935A - Preparation of reactive metal solutions by electrodeposition methods - Google Patents

Preparation of reactive metal solutions by electrodeposition methods Download PDF

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US3298935A
US3298935A US447923A US44792365A US3298935A US 3298935 A US3298935 A US 3298935A US 447923 A US447923 A US 447923A US 44792365 A US44792365 A US 44792365A US 3298935 A US3298935 A US 3298935A
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metals
molten
electrolyte
fluoride
cathode
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Thomas A Henrie
Donald G Kesterke
Morrice Edward
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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
    • C25C3/36—Alloys obtained by cathodic reduction of all their ions

Definitions

  • This invention relates to preparation of molten metal solutions suitable for use in preparation of alloys, as deoxidizers or nodularizers in ferroalloys, as intermediate products for preparation of pure reactive metals, etc.
  • this objective may be achieved by electrolytic reduction of metal oxides or other compounds in molten salt solution to form the desired molten metal solution on a nonconsumable metal cathode by simultaneous electrodeposition of the component metals.
  • the invention has been found to be particularly applicable to formation of molten solutions of one or more members of two groups of metals, i.e., (1) reactive metals such as thorium, uranium, titanium, yttrium, lanthanum and cerium and (2) conventional alloying metals such as nickel, copper and tin, as well as iron.
  • the metals are simultaneously electrodeposited on a solid non-reactive cathode such as tungsten, Where they form a liquid solution that drips off and collects at the bottom of the molten bath.
  • the product is easily recovered, dense, slag free and in a form suitable for addition to ferro-alloys and for use as a source of reactive metal for an electro-refining cell.
  • Processes for electrodeposition from fused salt baths are conventional and a Wide variety of materials have been used to form the molten bath in which the electrolysis is conducted.
  • the molten salt electrolyte components used in the instant invention are conventional; however, particular compositions may be optimum for deposition of particular combinations of metals.
  • Compositions comprising alkali metal or alkaline earth metal fluorides and fluorides of the metals to be deposited have been found to be particularly effective in the method of These compositions are, however, conventional and do not constitute the essence of the invention.
  • Similar molten bath compositions are disclosed in US. Patent 2,033,172 to Andrieuxthis patent discloses preparation of alloys of boron by deposition of the boron on a cathode of the metal to be alloyed. In some instances limited quantitie of chlorides may be substituted for the fluorides in the instant invention.
  • the source (feed materials) of the metals to be codeposited may be various compounds that are soluble in the molten bath. Most eflective and convenient sources are usually the oxides. Other compounds that maybe used are chlorides, nitrides, and fluorides.
  • proportions of the components of the molten bath and feed material will vary with the com-position and amount of the particular alloy or molten metal mixture to ice be formed and are best determined experimentally.
  • proportions of alkali or alkaline earth fluorides in the bath will range from about 15 to about 65 weight percent, with the fluorides of the metals to be deposited ranging from about 35 to about 85 percent.
  • the apparatus employed in the process of the invention is also conventional and consists of one or more anodes, usually carbon, and a non-consumable cathode, i.e., a cathode that does not react with the molten bath or the deposited metals at the operating temperature.
  • the molten electrolyte bath is generally contained in a graphite crucible. Tungsten has been found to be a verysatisfactory cathode material; other possible cathode materials are molybdenum, tantalum and graphite.
  • Temperature of the bath must be sufficient to maintain both the bath and deposited metals in a molten condition but not high enough to affect the cathode. Temperatures of from about 1050 C. to 1250 C. are usually satisfactory, although again optimum values may vary with dilferent bath ingredients and feed materials. Cathode current density is also not critical; values will generally range from about 30 to 65 amperes per square inch. Use of an inert atmosphere, such as helium, is also usually desirable to prevent undesired contamination from the atmosphere.
  • Example 1 In this example a thorium-nickel alloy was prepared. The experiment was conducted in a controlled atmosphere of helium.
  • the electrode configuration consisted of two vertical 1% inch diameter carbon anodes and one vertical inch diameter tungsten cathode, positioned in a 9 inch inside diameter graphite crucible.
  • the electrolyte composition in weight-percent was percent thorium fluoride, 2 percent nickel fluoride, 13 percent calcium fluoride, and 15 percent sodium fluoride.
  • the electrolyte was melted by heat from a graphite resistor located immediately below the crucible. The electrolysis was begun at a bath temperature of 1150 C. and continued for about 2 hours at about 1170" C.
  • an oxide mixture composed of 62 weight-percent thorium oxide and 38 weight-percent nickel oxide was fed to the cell in the vicinity of the anodes at a controlled rate. Electrodeposition of the two metals on the cathode formed a liquid alloy that dripped into a boron nitride-lined tungsten cup collection zone on the bottom of the cell. At the conclusion of the electrolysis the cell was heated to 1250" C. to insure a fluid alloy, then the cup was lifted from the cell and its contents poured into a mold. The resulting product contained 89 weight-percent thorium and 11 percent nickel.
  • Example 2 In this example a thorium-iron alloy was prepared. Experimental conditions were similar to those of Example 1 except that the electrolyte was composed of 35 weightpercent ThF 60 weight-percent BaF and 5 weight-percent LiF.
  • the oxide feed mixture consisted of 77 Weightpercent thorium oxide and 23 weight-percent ferric oxide. The resulting product contained 88 Weight-percent thorium and 12 weight-percent iron.
  • Example 3 In this example an iron-yttrium alloy was prepared.
  • the electrode arrangement consisted of two vertical 0.75 inch diameter carbon anodes and one vertical 0.20 inch diameter tungsten cathode.
  • the electrolyte mixture 85 Weight-percent YF and 15 percent LiF, was packed into a 5-inch diameter graphite crucible.
  • the electrolyte was melted by passing alternating current through a graphite resistor submerged between the anodes in the powdered electrolyte. When the electrolyte reached a temperature of 1050 C., the anodes were raised ofl the resistor and direct current turned on. During electrolysis alternating current was passed between the anodes as supplementary power.
  • a process for the electrolytic preparation of a molten solution of at least two metals comprising:
  • said molten salt electrolyte comprising a fluoride of at least one of said at least two metals and a fluoride selected from the group consisting of alkali metal fluoride and alkaline earth metal fluorides;
  • a process for the preparation of a molten solution of thorium and nickel from a source material of oxides of said thorium and nickel comprising electro-codepositing said thorium and nickel on a tungsten electrode from a molten salt electrolyte bath containing said oxides dissolved therein, said bath comprising thorium fluoride, nickel fluoride, calcium fluoride and sodium fluoride.
  • a process for the preparation of a molten solution of thorium and iron from a source material of oxides of said thorium and iron comprising electro-codepositing said thorium and iron on a tungsten electrode from a molten salt electrolyte bath containing said oxides dissolved therein, said bath comprising thorium fluoride, barium fluoride and lithium fluoride.
  • a process for the preparation of a molten solution of yttrium and iron from a source material of oxides of said yttrium and iron comprising electro-codepositing said yttrium and a iron on a tungsten electrode from a molten salt electrolyte bath containing said oxides dissolved therein, said bath comprising yttrium fluoride and lithium fluoride.

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  • Chemical & Material Sciences (AREA)
  • Engineering & Computer Science (AREA)
  • Chemical Kinetics & Catalysis (AREA)
  • Electrochemistry (AREA)
  • Materials Engineering (AREA)
  • Metallurgy (AREA)
  • Organic Chemistry (AREA)
  • Electrolytic Production Of Metals (AREA)

Description

r the invention.
United States Patent PREPARATION OF REACTIVE METAL SOLUTIONS BY ELECTRODEPOSITION METHODS Thomas A." Henrie, Donald G. Kesterke, and Edward Moi-rice, all of Reno, Nev., assignors to the United States of America as represented by the Secretary of the Interior No Drawing. Filed Apr. 13, 1965, Ser. No. 447,923 4 Claims. (Cl. 204-15) The invention herein described and claimed may be manufactured and used by or for the Government of the United States of America for governmental purposes without the payment of royalties thereon or therefor.
This invention relates to preparation of molten metal solutions suitable for use in preparation of alloys, as deoxidizers or nodularizers in ferroalloys, as intermediate products for preparation of pure reactive metals, etc.
The conventional technique for preparing alloys of this nature is that of melting the metals together. This technique, however, is complicated by the precautions necessary to avoid impurities such as oxygen, nitrogen, and carbon.
It is therefore an object of the present invention to provide a reliable, economical process for preparing molten metal solutions that are low in deleterious impurities.
It has now been found that this objective may be achieved by electrolytic reduction of metal oxides or other compounds in molten salt solution to form the desired molten metal solution on a nonconsumable metal cathode by simultaneous electrodeposition of the component metals.
The invention has been found to be particularly applicable to formation of molten solutions of one or more members of two groups of metals, i.e., (1) reactive metals such as thorium, uranium, titanium, yttrium, lanthanum and cerium and (2) conventional alloying metals such as nickel, copper and tin, as well as iron. The metals are simultaneously electrodeposited on a solid non-reactive cathode such as tungsten, Where they form a liquid solution that drips off and collects at the bottom of the molten bath. The product is easily recovered, dense, slag free and in a form suitable for addition to ferro-alloys and for use as a source of reactive metal for an electro-refining cell.
Processes for electrodeposition from fused salt baths are conventional and a Wide variety of materials have been used to form the molten bath in which the electrolysis is conducted. The molten salt electrolyte components used in the instant invention are conventional; however, particular compositions may be optimum for deposition of particular combinations of metals. Compositions comprising alkali metal or alkaline earth metal fluorides and fluorides of the metals to be deposited have been found to be particularly effective in the method of These compositions are, however, conventional and do not constitute the essence of the invention. Similar molten bath compositions are disclosed in US. Patent 2,033,172 to Andrieuxthis patent discloses preparation of alloys of boron by deposition of the boron on a cathode of the metal to be alloyed. In some instances limited quantitie of chlorides may be substituted for the fluorides in the instant invention.
The source (feed materials) of the metals to be codeposited may be various compounds that are soluble in the molten bath. Most eflective and convenient sources are usually the oxides. Other compounds that maybe used are chlorides, nitrides, and fluorides.
Optimum. proportions of the components of the molten bath and feed material will vary with the com-position and amount of the particular alloy or molten metal mixture to ice be formed and are best determined experimentally. Generally, proportions of alkali or alkaline earth fluorides in the bath will range from about 15 to about 65 weight percent, with the fluorides of the metals to be deposited ranging from about 35 to about 85 percent.
The apparatus employed in the process of the invention is also conventional and consists of one or more anodes, usually carbon, and a non-consumable cathode, i.e., a cathode that does not react with the molten bath or the deposited metals at the operating temperature. The molten electrolyte bath is generally contained in a graphite crucible. Tungsten has been found to be a verysatisfactory cathode material; other possible cathode materials are molybdenum, tantalum and graphite.
Temperature of the bath must be sufficient to maintain both the bath and deposited metals in a molten condition but not high enough to affect the cathode. Temperatures of from about 1050 C. to 1250 C. are usually satisfactory, although again optimum values may vary with dilferent bath ingredients and feed materials. Cathode current density is also not critical; values will generally range from about 30 to 65 amperes per square inch. Use of an inert atmosphere, such as helium, is also usually desirable to prevent undesired contamination from the atmosphere.
Although the theoretical explanation for success of the process of the invention is not known with certainty, it is believed that codeposition of the metals, despite large differences in free energy of formation of their oxides, results from the limited solubility of the oxides or other feed materials in the molten bath. As a result, the two metals codeposit in about the same proportion as their concentration in the electrolyte.
The invention will be more specifically illustrated by the following examples.
Example 1 In this example a thorium-nickel alloy was prepared. The experiment was conducted in a controlled atmosphere of helium. The electrode configuration consisted of two vertical 1% inch diameter carbon anodes and one vertical inch diameter tungsten cathode, positioned in a 9 inch inside diameter graphite crucible. The electrolyte composition in weight-percent was percent thorium fluoride, 2 percent nickel fluoride, 13 percent calcium fluoride, and 15 percent sodium fluoride. The electrolyte was melted by heat from a graphite resistor located immediately below the crucible. The electrolysis was begun at a bath temperature of 1150 C. and continued for about 2 hours at about 1170" C. During electrolysis an oxide mixture composed of 62 weight-percent thorium oxide and 38 weight-percent nickel oxide was fed to the cell in the vicinity of the anodes at a controlled rate. Electrodeposition of the two metals on the cathode formed a liquid alloy that dripped into a boron nitride-lined tungsten cup collection zone on the bottom of the cell. At the conclusion of the electrolysis the cell was heated to 1250" C. to insure a fluid alloy, then the cup was lifted from the cell and its contents poured into a mold. The resulting product contained 89 weight-percent thorium and 11 percent nickel.
Example 2 In this example a thorium-iron alloy was prepared. Experimental conditions were similar to those of Example 1 except that the electrolyte Was composed of 35 weightpercent ThF 60 weight-percent BaF and 5 weight-percent LiF. The oxide feed mixture consisted of 77 Weightpercent thorium oxide and 23 weight-percent ferric oxide. The resulting product contained 88 Weight-percent thorium and 12 weight-percent iron.
Example 3 In this example an iron-yttrium alloy was prepared. The electrode arrangement consisted of two vertical 0.75 inch diameter carbon anodes and one vertical 0.20 inch diameter tungsten cathode. The electrolyte mixture, 85 Weight-percent YF and 15 percent LiF, was packed into a 5-inch diameter graphite crucible. The electrolyte was melted by passing alternating current through a graphite resistor submerged between the anodes in the powdered electrolyte. When the electrolyte reached a temperature of 1050 C., the anodes were raised ofl the resistor and direct current turned on. During electrolysis alternating current was passed between the anodes as supplementary power. Approximately 170 grams of a mixture of 72 weight-percent Y O 14 percent F and 14 percent Fel was fed to the bath. The electrolysis was conducted at a bath temperature of approximately 1100 C. for 1 /2 hours. The bath was allowed to solidify, the electrolyte was crushed, and the iron-yttrium nodules recovered. Analyses showed the nodules to contain from 28 to 34 percent iron with 0.02 percent carbon as the major impurity. Typical operating conditions of this example, as well as examples 1 and 2, are given in the following table:
TABLE 1.-OPERATIONAL DATA FOR THE PREPARATION OF VARIOUS METAL SOLUTIONS BY ELECTRODEP OSITION METHODS What is claimed is:
1. A process for the electrolytic preparation of a molten solution of at least two metals comprising:
(a) dissolving metal oxides of said at least two metals in a molten salt electrolyte, one of said at least two metals selected from the group consisting of thorium, uranium, titanium, yttrium, lanthanum and cerium, and another of said at least two metals selected from the group consisting of nickel, copper, tin and iron,
said molten salt electrolyte comprising a fluoride of at least one of said at least two metals and a fluoride selected from the group consisting of alkali metal fluoride and alkaline earth metal fluorides;
(b) electrolytically reducing said metal oxides dissolved in said electrolyte;
(c) ele-ctro-codepositing said reduced metal oxides as a molten solution of said at least two metals on a nonreactive cathode in contact with said molten salt electrolyte, said electrolyte being maintained at a temperature sufliciently high enough to maintain said deposited metals in a molten condition;
(d) passing said molten metal solution which deposits on said cathode to a collection zone.
2. A process for the preparation of a molten solution of thorium and nickel from a source material of oxides of said thorium and nickel comprising electro-codepositing said thorium and nickel on a tungsten electrode from a molten salt electrolyte bath containing said oxides dissolved therein, said bath comprising thorium fluoride, nickel fluoride, calcium fluoride and sodium fluoride.
3. A process for the preparation of a molten solution of thorium and iron from a source material of oxides of said thorium and iron comprising electro-codepositing said thorium and iron on a tungsten electrode from a molten salt electrolyte bath containing said oxides dissolved therein, said bath comprising thorium fluoride, barium fluoride and lithium fluoride.
4. A process for the preparation of a molten solution of yttrium and iron from a source material of oxides of said yttrium and iron comprising electro-codepositing said yttrium and a iron on a tungsten electrode from a molten salt electrolyte bath containing said oxides dissolved therein, said bath comprising yttrium fluoride and lithium fluoride.
References Cited by the Examiner UNITED STATES PATENTS 1,835,026 12/1931 Driggs 204-292 X 2,752,303 6/1956 Cooper 204 71 X 2,902,415 9/1959 Niedrach et al. 204 71 X 2,951,793 9/1960 Hansen 204-71 X 2,986,503 5/1961 Pruvot et al. 204 -71 X 3,062,727 11/1962 Pokorny 204- 71 X 3,087,873 4/1963 Slatin 204 71 REUBEN EPSTEIN, Primary Examiner.

Claims (1)

1. A PROCESS FOR THE ELECTROLYTIC PREPARATION OF A MOLTEN SOLUTION OF AT LEAST TWO METALS COMPRISING: (A) DISSOLVING METAL OXIDES OF SAID AT LEAST TWO METALS IN A MOLTEN SALT ELECTROLYTE, ONE OF SAID AT LEAST TWO METALS SELECTED FROM THE GROUP CONSISTING OF THORIUM, URANIUM, TITANIUM, YTTRIUM, LANTHANUMM AND CERIUM, AND ANOTHER OF SAID AT LEAST TWO METALS SELECTED FROM THE GROUP CONSISTING OF NICKEL, COPPER, TIN AND IRON, SAID MOLTEN SALT ELECTROLYTE COMPRISING A FLUORIDE OF AT LEAST ONE OF SAID AT LEAST TWO METALS AND A FLUORIDE SELECTED FROM THE GROUP CONSISTING OF ALKALI METAL FLUORIDE AND ALKALINE EARTH METAL FLUORIDES; (B) ELECTROLYTICALLY REDUCING SAID METAL OXIDES DISSOLVED IN SAID ELECTROLYTE; (C) ELECTRO-CODEPOSITING SAID REDUCED METAL OXIDES AS A MOLTEN SOLUTION OF SAID AT LEAST TWO METALS ON A NONREACTIVE CATHODE IN CONTACT WITH SAID MOLTEN SALT ELECTROLYTE, SAID ELECTROLYTE BEING MAINTAINED AT A TEMPERATURE SUFFICIENTLY HIGH ENOUGH TO MAINTAIN SAID DEPOSITED METALS IN A MOLTEN CONDITION; (D) PASSING SAID MOLTEN METAL SOLUTION WHICH DEPOSITS ON SAID CATHODE TO A COLLECTION ZONE.
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Cited By (7)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US3524800A (en) * 1968-04-04 1970-08-18 Us Interior Method for the production of samarium alloys
US4684448A (en) * 1984-10-03 1987-08-04 Sumitomo Light Metal Industries, Ltd. Process of producing neodymium-iron alloy
US4747924A (en) * 1984-10-03 1988-05-31 Sumitomo Light Metal Industries, Ltd. Apparatus for producing neodymium-iron alloy
US5024737A (en) * 1989-06-09 1991-06-18 The Dow Chemical Company Process for producing a reactive metal-magnesium alloy
US5131988A (en) * 1991-04-12 1992-07-21 Reynolds Metals Company Method of extracting lithium from aluminum-lithium alloys
US20080023321A1 (en) * 2006-07-31 2008-01-31 Donald Sadoway Apparatus for electrolysis of molten oxides
GB2556944A (en) * 2016-11-28 2018-06-13 Richard Scott Ian Use of decay heat from spent nuclear fuel processed by electro-reduction

Citations (7)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US1835026A (en) * 1930-04-17 1931-12-08 Westinghouse Lamp Co Electrode material
US2752303A (en) * 1954-09-02 1956-06-26 Walter M Weil Fused bath electrolysis of metal chlorides
US2902415A (en) * 1956-10-03 1959-09-01 Leonard W Niedrach Purification of uranium fuels
US2951793A (en) * 1957-10-09 1960-09-06 Wilford N Hansen Electrolysis of thorium and uranium
US2986503A (en) * 1956-03-20 1961-05-30 Sobertiz Soc De Brevets D Expl Production of titanium and zirconium by the electrolytic refining of their alloys
US3062727A (en) * 1958-12-10 1962-11-06 Metallurg De Hoboken Soc Gen Manufacture of niobium by fusion electrolysis
US3087873A (en) * 1960-06-15 1963-04-30 Timax Associates Electrolytic production of metal alloys

Patent Citations (7)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US1835026A (en) * 1930-04-17 1931-12-08 Westinghouse Lamp Co Electrode material
US2752303A (en) * 1954-09-02 1956-06-26 Walter M Weil Fused bath electrolysis of metal chlorides
US2986503A (en) * 1956-03-20 1961-05-30 Sobertiz Soc De Brevets D Expl Production of titanium and zirconium by the electrolytic refining of their alloys
US2902415A (en) * 1956-10-03 1959-09-01 Leonard W Niedrach Purification of uranium fuels
US2951793A (en) * 1957-10-09 1960-09-06 Wilford N Hansen Electrolysis of thorium and uranium
US3062727A (en) * 1958-12-10 1962-11-06 Metallurg De Hoboken Soc Gen Manufacture of niobium by fusion electrolysis
US3087873A (en) * 1960-06-15 1963-04-30 Timax Associates Electrolytic production of metal alloys

Cited By (8)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US3524800A (en) * 1968-04-04 1970-08-18 Us Interior Method for the production of samarium alloys
US4684448A (en) * 1984-10-03 1987-08-04 Sumitomo Light Metal Industries, Ltd. Process of producing neodymium-iron alloy
US4747924A (en) * 1984-10-03 1988-05-31 Sumitomo Light Metal Industries, Ltd. Apparatus for producing neodymium-iron alloy
US5024737A (en) * 1989-06-09 1991-06-18 The Dow Chemical Company Process for producing a reactive metal-magnesium alloy
US5131988A (en) * 1991-04-12 1992-07-21 Reynolds Metals Company Method of extracting lithium from aluminum-lithium alloys
US20080023321A1 (en) * 2006-07-31 2008-01-31 Donald Sadoway Apparatus for electrolysis of molten oxides
WO2008016526A3 (en) * 2006-07-31 2008-03-20 Massachusetts Inst Technology Apparatus for electrolysis of molten oxides
GB2556944A (en) * 2016-11-28 2018-06-13 Richard Scott Ian Use of decay heat from spent nuclear fuel processed by electro-reduction

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