US20050089760A1 - Electrolyte additive for non-aqueous electrochemical cells - Google Patents

Electrolyte additive for non-aqueous electrochemical cells Download PDF

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US20050089760A1
US20050089760A1 US10/990,379 US99037904A US2005089760A1 US 20050089760 A1 US20050089760 A1 US 20050089760A1 US 99037904 A US99037904 A US 99037904A US 2005089760 A1 US2005089760 A1 US 2005089760A1
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electrolyte
ppm
aluminum
liclo
corrosion
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Jane Blasi
Nikolai Issaev
Michael Pozin
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Gillette Co LLC
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Gillette Co LLC
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    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M4/00—Electrodes
    • H01M4/02—Electrodes composed of, or comprising, active material
    • H01M4/64—Carriers or collectors
    • H01M4/66—Selection of materials
    • H01M4/661—Metal or alloys, e.g. alloy coatings
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M50/00—Constructional details or processes of manufacture of the non-active parts of electrochemical cells other than fuel cells, e.g. hybrid cells
    • H01M50/10—Primary casings; Jackets or wrappings
    • H01M50/116—Primary casings; Jackets or wrappings characterised by the material
    • H01M50/117—Inorganic material
    • H01M50/119—Metals
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M50/00—Constructional details or processes of manufacture of the non-active parts of electrochemical cells other than fuel cells, e.g. hybrid cells
    • H01M50/10—Primary casings; Jackets or wrappings
    • H01M50/14—Primary casings; Jackets or wrappings for protecting against damage caused by external factors
    • H01M50/145—Primary casings; Jackets or wrappings for protecting against damage caused by external factors for protecting against corrosion
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M6/00—Primary cells; Manufacture thereof
    • H01M6/14—Cells with non-aqueous electrolyte
    • H01M6/16—Cells with non-aqueous electrolyte with organic electrolyte
    • H01M6/162—Cells with non-aqueous electrolyte with organic electrolyte characterised by the electrolyte
    • H01M6/166—Cells with non-aqueous electrolyte with organic electrolyte characterised by the electrolyte by the solute
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M4/00—Electrodes
    • H01M4/02—Electrodes composed of, or comprising, active material
    • H01M4/36—Selection of substances as active materials, active masses, active liquids
    • H01M4/48—Selection of substances as active materials, active masses, active liquids of inorganic oxides or hydroxides
    • H01M4/50—Selection of substances as active materials, active masses, active liquids of inorganic oxides or hydroxides of manganese
    • H01M4/502—Selection of substances as active materials, active masses, active liquids of inorganic oxides or hydroxides of manganese for non-aqueous cells
    • Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
    • Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
    • Y02E—REDUCTION OF GREENHOUSE GAS [GHG] EMISSIONS, RELATED TO ENERGY GENERATION, TRANSMISSION OR DISTRIBUTION
    • Y02E60/00—Enabling technologies; Technologies with a potential or indirect contribution to GHG emissions mitigation
    • Y02E60/10—Energy storage using batteries
    • Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
    • Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
    • Y02P—CLIMATE CHANGE MITIGATION TECHNOLOGIES IN THE PRODUCTION OR PROCESSING OF GOODS
    • Y02P70/00—Climate change mitigation technologies in the production process for final industrial or consumer products
    • Y02P70/50—Manufacturing or production processes characterised by the final manufactured product
    • Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
    • Y10—TECHNICAL SUBJECTS COVERED BY FORMER USPC
    • Y10T—TECHNICAL SUBJECTS COVERED BY FORMER US CLASSIFICATION
    • Y10T29/00—Metal working
    • Y10T29/49—Method of mechanical manufacture
    • Y10T29/49002—Electrical device making
    • Y10T29/49108—Electric battery cell making

Definitions

  • This invention relates to non-aqueous electrochemical cells for batteries.
  • a battery contains a negative electrode, typically called the anode, and a positive electrode, typically called the cathode.
  • the anode contains an active material that can be oxidized; the cathode contains or consumes an active material that can be reduced.
  • the anode active material is capable of reducing the cathode active material.
  • anode and the cathode When a battery is used as an electrical energy source in a device, electrical contact is made to the anode and the cathode, allowing electrons to flow through the device and permitting the respective oxidation and reduction reactions to occur to provide electrical power.
  • An electrolyte in contact with the anode and the cathode contains ions that flow through the separator between the electrodes to maintain charge balance throughout the battery during discharge.
  • Aluminum can be used as a construction material in a battery. However, aluminum can corrode because the electrode potential of aluminum is lower than the normal operating potential of the positive electrode of the battery. This corrosion increases the internal impedance of a cell, leading to capacity loss and to a decrease in specific energy. When aluminum is coupled with metals of a different nature in the environment of an electrochemical cell, the aluminum can also be susceptible to corrosion degradation.
  • the invention relates to an electrochemical cell that includes parts made from aluminum or an aluminum-based alloy; these parts contact the electrolyte of the cell.
  • the cell also includes an additive to suppress aluminum corrosion.
  • the invention features a secondary electrochemical cell including a cathode, an anode, a current collector including aluminum, and an electrolyte containing a perchlorate salt and a second salt that is different from the perchlorate salt.
  • the second salt is not a perchlorate salt.
  • the electrolyte is essentially free of LiPF 6 .
  • the electrolyte can contain at least 5000 ppm by weight of the perchlorate salt or at least 10,000 ppm by weight of the perchlorate salt.
  • An example of the second salt is LiTFS.
  • the invention features an electrochemical cell including a cathode containing MnO 2 , an anode containing lithium, and an electrolyte containing a perchlorate salt.
  • the cell includes an aluminum surface in electrical contact with a second metal surface.
  • the surface is a portion of an object having at least one dimension greater than 0.5 mm, 1 mm, or 2 mm.
  • An “aluminum surface” can be the surface of an object made of pure aluminum, or a surface made of an aluminum-based alloy.
  • the second metal surface is different than the aluminum surface.
  • the different metal can be, e.g., steel, stainless steel, or nickel.
  • the different metal can also be a different alloy of aluminum. That is, different alloys of aluminum are considered to be different metals.
  • the cell is relatively light.
  • the cell also has low ohmic resistance under polarization, because aluminum is very conductive.
  • aluminum is less expensive than stainless steel. The aluminum is protected from corrosion by the addition of a perchlorate salt.
  • the cell can include a cathode current collector containing aluminum.
  • the electrolyte can contain about 500 to about 2500 ppm by weight of a perchlorate salt.
  • the perchlorate salt can be, e.g., LiClO 4 , Ca(ClO 4 ) 2 , Al(ClO 4 ) 3 , or Ba(ClO 4 ) 2 .
  • the electrolyte is essentially free of LiPF 6 .
  • the invention features an electrochemical cell including a cathode containing an aluminum current collector, an anode, and an electrolyte containing a lithium salt and a perchlorate salt.
  • the cell is a primary electrochemical cell. Primary electrochemical cells are meant to be discharged to exhaustion only once, and then discarded. Primary cells are not meant to be recharged.
  • the cathode can contain MnO 2 and the anode can contain lithium.
  • the electrolyte can contain at least 500 ppm by weight of the perchlorate salt, or at least. 1000, 1500, or 2500 ppm by weight of the perchlorate salt.
  • the electrolyte can also contain less than 20,000 ppm by weight of the perchlorate salt.
  • the perchlorate salt can be, e.g., LiClO 4 , Ca(ClO 4 ) 2 , Al(ClO 4 ) 3 , or Ba(ClO 4 ) 2 .
  • the electrolyte can also include LiPF 6 , e.g., at least 5000 ppm by weight LiPF 6 or at least 10,000 ppm by weight LiPF 6 . In other aspects, the electrolyte is essentially free of LiPF 6 .
  • the case of the cell can be aluminum, either in whole or in part.
  • the invention features an electrochemical cell comprising a cathode containing MnO 2 , an anode containing lithium, and an electrolyte containing about 500 ppm to about 2000 ppm of a perchlorate salt.
  • the perchlorate salt can be, e.g., LiClO 4 , Ca(ClO 4 ) 2 , Al(ClO 4 ) 3 , or Ba(ClO 4 ) 2 .
  • the invention features an electrochemical cell comprising a cathode containing MnO 2 , an anode containing lithium, and an electrolyte containing a perchlorate salt; the cell is a primary electrochemical cell and includes two pieces of aluminum in electrical contact with each other. The two pieces can be made of the same alloy of aluminum.
  • the invention features a method of inhibiting aluminum corrosion in a primary electrochemical cell.
  • the method includes: (a) adding a perchlorate salt to the electrolyte of the cell; and (b) placing the electrolyte, an anode containing Li, and a cathode containing MnO 2 and an aluminum current collector into a cell case.
  • the perchlorate salt can be, e.g., LiClO 4 , Ca(ClO 4 ) 2 , Al(ClO 4 ) 3 , or Ba(ClO 4 ) 2 .
  • FIG. 1 is a sectional view of a nonaqueous electrochemical cell.
  • FIG. 2 is a graph showing current density vs. potential of the aluminum in an electrode exposed to LiTFS, DME:EC:PC electrolytes containing different amounts of LiClO 4 .
  • FIG. 3 is a graph showing current density vs. time of the aluminum in an electrode exposed to LiTFS, DME:EC:PC electrolytes containing different amounts of LiClO 4 .
  • FIG. 4 is a graph showing current density vs. time of the aluminum in an electrode exposed to a LiTFS, DME:EC:PC electrolyte containing LiClO 4 .
  • FIG. 5 is a graph showing current density vs. potential of the aluminum in an electrode exposed to LiTFS+LiTFSI, DME:EC:PC electrolytes containing different amounts of LiClO 4 .
  • FIG. 6 is a graph showing current density vs. time of the aluminum in an electrode exposed to LiTFS+LiTFSI, DME:EC:PC electrolytes containing different amounts of LiClO 4 .
  • FIG. 7 is a graph showing current density vs. potential of the aluminum in an electrode exposed to LiTFS+LiPF 6 , DME:EC:PC electrolytes containing different amounts of LiClO 4 .
  • FIG. 8 is a graph showing current density vs. time of the aluminum in an electrode exposed to LiTFS+LiPF 6 , DME:EC:PC electrolytes containing different amounts of LiClO 4 .
  • FIG. 9 is a graph showing current density vs. potential of the aluminum in an electrode exposed to a LiTFS, DME:EC:PC electrolyte containing different amounts of LiClO 4 and different amounts of Al(ClO 4 ) 3 .
  • FIG. 10 is a graph showing current density vs. potential of the aluminum in an electrode exposed to a LiTFS, DME:EC:PC electrolyte containing different amounts of LiClO 4 and different amounts of Ba(ClO 4 ) 2 .
  • an electrochemical cell 10 includes an anode 12 in electrical contact with a negative lead 14 , a cathode 16 in electrical contact with a positive lead 18 , a separator 20 and an electrolytic solution.
  • Anode 12 , cathode 16 , separator 20 and the electrolytic solution are contained within a case 22 .
  • the electrolytic solution includes a solvent system and a salt that is at least partially dissolved in the solvent system.
  • Cathode 16 includes an active cathode material, which is generally coated on the cathode current collector.
  • the current collector is generally titanium, stainless steel, nickel, aluminum, or an aluminum alloy, e.g., aluminum foil.
  • the active material can be, e.g., a metal oxide, halide, or chalcogenide; alternatively, the active material can be sulfur, an organosulfur polymer, or a conducting polymer. Specific examples include MnO 2 , V 2 O 5 , CoF 3 , MoS 2 , FeS 2 , SOCl 2 , MoO 3 , S, (C 6 H 5 N) n , (S 3 N 2 ) n , where n is at least 2.
  • the active material can also be a carbon monofluoride.
  • An example is a compound having the formula CF x , where x is 0.5 to 1.0.
  • the active material can be mixed with a conductive material such as carbon and a binder such as polytetrafluoroethylene (PTFE).
  • PTFE polytetrafluoroethylene
  • An example of a cathode is one that includes aluminum foil coated with MnO 2 . The cathode can be prepared as described in U.S. Pat. No. 4,279,972.
  • Anode 12 can consist of an active anode material, usually in the form of an alkali metal, e.g., Li, Na, K, or an alkaline earth metal, e.g., Ca, Mg.
  • the anode can also consist of alloys of alkali metals and alkaline earth metals or alloys of alkali metals and Al.
  • the anode can be used with or without a substrate.
  • the anode also can consist of an active anode material and a binder.
  • an active anode material can include carbon, graphite, an acetylenic mesophase carbon, coke, a metal oxide and/or a lithiated metal oxide.
  • the binder can be, for example, PTFE.
  • the active anode material and binder can be mixed to form a paste which can be applied to the substrate of anode 12 .
  • Separator 20 can be formed of any of the standard separator materials used in nonaqueous electrochemical cells.
  • separator 20 can be formed of polypropylene, (e.g., nonwoven polypropylene or microporous polypropylene), polyethylene, and/or a polysulfone.
  • the electrolyte can be in liquid, solid or gel (polymer) form.
  • the electrolyte can contain an organic solvent such as propylene carbonate (PC), ethylene carbonate (EC), dimethoxyethane (DME), dioxolane (DO), tetrahydrofuran (THF), acetonitrile (CH 3 CN), gamma-butyrolactone, diethyl carbonate (DEC), dimethyl carbonate (DMC), ethyl methyl carbonate (EMC) dimethylsulfoxide (DMSO) methyl acetate (MA), methyl formiate (MF), sulfolane or combinations thereof.
  • PC propylene carbonate
  • EC ethylene carbonate
  • DME dimethoxyethane
  • DO dioxolane
  • THF tetrahydrofuran
  • CH 3 CN acetonitrile
  • EMC ethyl methyl carbonate
  • DMSO dimethylsulfoxide
  • the electrolyte can alternatively contain an inorganic solvent such as SO 2 or SOCl 2 .
  • the electrolyte also contains a lithium salt such as lithium trifluoromethanesulfonate (LiTFS) or lithium trifluoromethanesulfonimide (LiTFSI), or a combination thereof. Additional lithium salts that can be included are listed in U.S. Pat. No. 5,595,841, which is hereby incorporated by reference in its entirety.
  • the electrolyte may contain LiPF 6 ; in other embodiments, the electrolyte is essentially free of LiPF 6 .
  • the electrolyte also contains a perchlorate salt, which inhibits corrosion in the cell.
  • Suitable salts include lithium, barium, calcium, aluminum, sodium, potassium, magnesium, copper, zinc, ammonium, and tetrabutylammonium perchlorates. Generally, at least 500 ppm by weight of the perchlorate salt is used; this ensures that there is enough salt to suppress corrosion. In addition, less than about 20,000 by weight of the perchlorate salt is generally used. If too much perchlorate salt is used, the cell can be internally shorted under certain conditions during use.
  • separator 20 can be cut into pieces of a similar size as anode 12 and cathode 16 and placed therebetween as shown in FIG. 1 .
  • Anode 12 , cathode 16 , and separator 20 are then placed within case 22 , which can be made of a metal such as nickel, nickel plated steel, stainless steel, or aluminum, or a plastic such as polyvinyl chloride, polypropylene, polysulfone, ABS or a polyamide.
  • Case 22 is then filled with the electrolytic solution and sealed.
  • One end of case 22 is closed with a cap 24 and an annular insulating gasket 26 that can provide a gas-tight and fluid-tight seal.
  • Positive lead 18 which can be made of aluminum, connects cathode 16 to cap 24 .
  • Cap 24 may also be made of aluminum.
  • a safety valve 28 is disposed in the inner side of cap 24 and is configured to decrease the pressure within battery 10 when the pressure exceeds some predetermined value. Additional methods for assembling the cell are described in U.S. Pat. Nos. 4,279,972; 4,401,735; and 4,526,846.
  • battery 10 can also be used, including, e.g., the coin cell configuration.
  • the batteries can be of different voltages, e.g., 1.5V, 3.0V, or 4.0V.
  • An electrochemical glass cell was constructed having an Al working electrode, a Li reference electrode, and two Li auxiliary electrodes.
  • the working electrode was fabricated from a 99.999% Al rod inserted into a Teflon sleeve to provide a planar electrode area of 0.33 cm 2 .
  • the native oxide layer was removed by first polishing the planar working surface with 3 ⁇ m aluminum oxide paper under an argon atmosphere, followed by thorough rinsing of the Al electrode in electrolyte. All experiments were performed under an Ar atmosphere.
  • Corrosion current measurements were made according to a modified procedure generally described in X. Wang et al., Electrochemica Acta, vol. 45, pp. 2677-2684 (2000).
  • the corrosion potential of Al was determined by continuous cyclic voltammetry. In each cycle, the potential was initially set to an open circuit potential, then anodically scanned to +4.5 V and reversed to an open circuit potential. A scan rate of 50 mV/s was selected, at which good reproducibility of the corrosion potential of aluminum was obtained.
  • the corrosion potential of aluminum was defined as the potential at which the anodic current density reached 10 ⁇ 5 A/cm 2 at the first cycle.
  • Corrosion current measurements were made according to the procedure described in EP 0 852 072.
  • the aluminum electrode was polarized at various potentials vs. a Li reference electrode while the current was recorded vs. time.
  • Current vs. time measurements were taken during a 30-minute period.
  • the area under current vs. time curve was used as a measure of the amount of aluminum corrosion occurring.
  • the experiment also could be terminated in case the current density reached 3 mA/cm 2 before the 30 minute time period elapsed and no corrosion suppression occurred. Corrosion suppression occurred when the resulting current density was observed in the range of 10 ⁇ 6 A/cm 2 .
  • Curves “a” and “a′” in FIG. 2 show the corrosion potential of the aluminum in the electrolyte containing no LiClO 4 .
  • the addition of 500 ppm of LiClO 4 to the electrolyte shifted the potential of the aluminum 150 mV in the positive direction (curves “b” and “b′”); the addition of 1000 ppm of LiClO 4 to the electrolyte shifted the potential 300 mV (curves “c” and “c′”); and the addition of 2500 ppm of LiClO 4 to the electrolyte shifted the potential 600 mV (curves “d” and “d′”).
  • curve “a” shows a potentiostatic dependence (chronoamperogram) of the aluminum electrode exposed to the electrolyte containing LiTFS, DME:EC:PC with the addition of 500 ppm LiClO 4 ;
  • curve “b” shows the chronoamperogram taken in the same electrolyte with addition of 1000 ppm LiClO 4 ;
  • curve “c” shows the chronoamperogram taken in the electrolyte containing LiTFS, DME:EC:PC, and 2500 ppm LiClO 4 .
  • the aluminum corrosion at +3.6 V vs. a Li reference electrode
  • the corrosion current is less than 10 ⁇ 6 A/cm 2 after 30 minutes of measurement.
  • the electrochemical window of Al stability can be extended as high as +4.2 V (vs. a Li reference electrode) by increasing the concentration of LiClO 4 to 1% (10,000 ppm).
  • LiClO 4 concentration of 1% aluminum corrosion is effectively suppressed at 4.2 V.
  • the corrosion current after 30 minutes is 8-10 ⁇ A/cm 2 , and the current continues to fall over time.
  • the falling current indicates passivation of the Al surface.
  • the increased level of the resulting current (10 ⁇ A/cm 2 vs. 1 ⁇ A/cm 2 after 30 minutes of experiment) is due to the increased background current at these potentials.
  • curves “a”, “a′”, and “a′′” show the corrosion potential of an aluminum electrode subjected to an electrolyte containing a mixture of LiTFS and LiTFSI salts, DME:EC:PC, and no LiClO 4 .
  • curve “a” shows the chronoamperogram of the aluminum electrode exposed to the electrolyte containing a mixture of LiTFS and LiTFSI salts, DME:EC:PC, and 1000 ppm LiClO 4
  • curve “b” shows the chronoamperogram of the aluminum electrode exposed to the same electrolyte containing 2500 ppm LiClO 4 .
  • the aluminum corrosion at +3.6 V is effectively suppressed, and resulting corrosion current of the Al electrode is about 10 ⁇ 6 A/cm 2 after 30 minutes.
  • curve “a” shows the corrosion potential of the aluminum subjected to an electrolyte containing a mixture of LiTFS and LiPF 6 salts, DME:EC:PC, and no LiClO 4 .
  • the addition of 500 ppm of LiClO 4 to this electrolyte shifted the corrosion potential of the aluminum 125 mV in the positive direction (curve “b”); the addition of 2500 ppm of LiClO 4 to the electrolyte shifted the potential 425 mV (curve “c”); and the addition of 5000 ppm of LiClO 4 to the electrolyte shifted the potential 635 mV (curve “d”).
  • curve “a” shows a chronoamperogram of the aluminum electrode exposed to the electrolyte containing LiTFS, LiPF 6 , DME:EC:PC with no LiClO 4 ;
  • curve “b” shows a chronoamperogram taken in the same electrolyte with 2500 ppm LiClO 4 added;
  • curve “c” shows a chronoamperogram taken in the electrolyte containing LiTFS, LiPF 6 , DME:EC:PC, and 5000 ppm LiClO 4 .
  • the aluminum corrosion at +3.6 V vs. a Li reference electrode
  • the corrosion current is less than 10 ⁇ 6 A/cm 2 after 30 minutes of measurement.
  • Electrochemical glass cells were constructed as described in Example 1. Cyclic voltammetry and chromoamperometry were performed as described in Example 1.
  • curves “a”, “b”, and “c” show the corrosion potential of an aluminum electrode exposed to the electrolyte LiTFS, DME:EC:PC containing 0, 1000 and 2500 ppm of LiClO 4 , respectively.
  • Curves “a′”, “b′,” and “c′” show the corrosion potential of an aluminum electrode exposed to the electrolyte LiTFS, DME:EC:PC containing 0, 1000 and 2500 ppm of Al(ClO 4 ) 3 , respectively.
  • curves “a”, “b”, and “c” show the corrosion potential of an aluminum electrode exposed to the electrolyte LiTFS, DME:EC:PC containing 0, 1000 and 2500 ppm of LiClO 4 , respectively.
  • Curves “a′”, “b′” and “c′” show the corrosion potential of an aluminum electrode exposed to the electrolyte LiTFS, DME:EC:PC containing 0, 1000 and 2500 ppm of Ba(ClO 4 ) 2 , respectively.
  • the level of Al ions in the electrolyte indicates the rate of Al corrosion.
  • the background level of Al ions in solution is about 2 ppm.
  • the corrosion of a metal is said to be suppressed when, after the test described above is performed, the concentration of metal ions in the electrolyte is less than about 3 ppm, which is just above the background level.
  • the Al concentration in the electrolyte without LiClO 4 addition is high (the range is 19.4-23 ppm). Thus, part of the Al substrate has dissolved (corroded) under the potential of the applied active cathode material.
  • the analytical data were confirmed by the direct observation of Al surface after aging (under an optical microscope, at a magnification of 60 ⁇ ).
  • the electrodes stored in the electrolyte without LiClO 4 exhibited substantial corrosion, as viewed under the optical microscope.
  • the section stored in the electrolyte with added LiClO 4 showed virtually no corrosion.
  • Cathode Al cur. LiTFS, DME:EC:PC + ⁇ 1.0 ⁇ 1.0 ⁇ 1.0 collector with 2500 ppm LiClO 4 welded Ni tab
  • a high concentration of Ni (90.9 ppm) in the resulting electrolyte indicates the severe corrosion of the Ni tab coupled with Al (the Al corroded as well, as indicated by the presence of 20.5 ppm Al).
  • the assembled cells (2/3A size) were stored 20 days at 60° C. Electrolyte removed from the cells after storage was submitted for ICP analysis. The electrolyte did not show any traces of Al, Fe, or Ni (the concentrations were at the background level).
  • Two cathodes were prepared by coating aluminum foil substrates (1145 Al) with MnO 2 . Pieces of aluminum foil (3003 Al) were welded to the aluminum foil of each of the cathodes.
  • One cathode was stored for 20 days at 60° C. over LiTFS, DME:EC:PC electrolyte containing 2500 ppm of LiClO 4 .
  • the second cathode was stored for 20 days at 60° C. over LiTFS, DME:EC:PC electrolyte containing no LiClO 4 . After the 20-day period, the electrolytes were analyzed by ICP.
  • the first electrolyte (2500 ppm LiClO 4 in the electrolyte) contained less than 1 ppm Al, while the second electrolyte (no LiClO 4 in the electrolyte) contained 18 ppm Al.

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  • Engineering & Computer Science (AREA)
  • Inorganic Chemistry (AREA)
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  • Manufacturing & Machinery (AREA)
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Abstract

An electrochemical secondary cell is disclosed. The cell includes a cathode, an anode, a current collector including aluminum, and an electrolyte containing a perchlorate salt and a second salt. The electrolyte is essentially free of LiPF6.

Description

    BACKGROUND
  • This invention relates to non-aqueous electrochemical cells for batteries.
  • Batteries are commonly used electrical energy sources. A battery contains a negative electrode, typically called the anode, and a positive electrode, typically called the cathode. The anode contains an active material that can be oxidized; the cathode contains or consumes an active material that can be reduced. The anode active material is capable of reducing the cathode active material.
  • When a battery is used as an electrical energy source in a device, electrical contact is made to the anode and the cathode, allowing electrons to flow through the device and permitting the respective oxidation and reduction reactions to occur to provide electrical power. An electrolyte in contact with the anode and the cathode contains ions that flow through the separator between the electrodes to maintain charge balance throughout the battery during discharge.
  • Aluminum can be used as a construction material in a battery. However, aluminum can corrode because the electrode potential of aluminum is lower than the normal operating potential of the positive electrode of the battery. This corrosion increases the internal impedance of a cell, leading to capacity loss and to a decrease in specific energy. When aluminum is coupled with metals of a different nature in the environment of an electrochemical cell, the aluminum can also be susceptible to corrosion degradation.
    • SUMMARY
  • The invention relates to an electrochemical cell that includes parts made from aluminum or an aluminum-based alloy; these parts contact the electrolyte of the cell. The cell also includes an additive to suppress aluminum corrosion.
  • In one aspect, the invention features a secondary electrochemical cell including a cathode, an anode, a current collector including aluminum, and an electrolyte containing a perchlorate salt and a second salt that is different from the perchlorate salt. Preferably, the second salt is not a perchlorate salt. The electrolyte is essentially free of LiPF6. The electrolyte can contain at least 5000 ppm by weight of the perchlorate salt or at least 10,000 ppm by weight of the perchlorate salt. An example of the second salt is LiTFS.
  • In another aspect, the invention features an electrochemical cell including a cathode containing MnO2, an anode containing lithium, and an electrolyte containing a perchlorate salt. The cell includes an aluminum surface in electrical contact with a second metal surface. Preferably, the surface is a portion of an object having at least one dimension greater than 0.5 mm, 1 mm, or 2 mm. An “aluminum surface” can be the surface of an object made of pure aluminum, or a surface made of an aluminum-based alloy. The second metal surface is different than the aluminum surface. The different metal can be, e.g., steel, stainless steel, or nickel. The different metal can also be a different alloy of aluminum. That is, different alloys of aluminum are considered to be different metals.
  • Because aluminum weighs less than other metals, such as stainless steel, that are used in electrochemical cells, the cell is relatively light. The cell also has low ohmic resistance under polarization, because aluminum is very conductive. Furthermore, aluminum is less expensive than stainless steel. The aluminum is protected from corrosion by the addition of a perchlorate salt.
  • The cell can include a cathode current collector containing aluminum. The electrolyte can contain about 500 to about 2500 ppm by weight of a perchlorate salt. The perchlorate salt can be, e.g., LiClO4, Ca(ClO4)2, Al(ClO4)3, or Ba(ClO4)2. In some embodiments, the electrolyte is essentially free of LiPF6.
  • In another aspect, the invention features an electrochemical cell including a cathode containing an aluminum current collector, an anode, and an electrolyte containing a lithium salt and a perchlorate salt. The cell is a primary electrochemical cell. Primary electrochemical cells are meant to be discharged to exhaustion only once, and then discarded. Primary cells are not meant to be recharged. The cathode can contain MnO2 and the anode can contain lithium. The electrolyte can contain at least 500 ppm by weight of the perchlorate salt, or at least. 1000, 1500, or 2500 ppm by weight of the perchlorate salt. The electrolyte can also contain less than 20,000 ppm by weight of the perchlorate salt. The perchlorate salt can be, e.g., LiClO4, Ca(ClO4)2, Al(ClO4)3, or Ba(ClO4)2. The electrolyte can also include LiPF6, e.g., at least 5000 ppm by weight LiPF6 or at least 10,000 ppm by weight LiPF6. In other aspects, the electrolyte is essentially free of LiPF6. The case of the cell can be aluminum, either in whole or in part.
  • In another aspect, the invention features an electrochemical cell comprising a cathode containing MnO2, an anode containing lithium, and an electrolyte containing about 500 ppm to about 2000 ppm of a perchlorate salt. The perchlorate salt can be, e.g., LiClO4, Ca(ClO4)2, Al(ClO4)3, or Ba(ClO4)2.
  • In another aspect, the invention features an electrochemical cell comprising a cathode containing MnO2, an anode containing lithium, and an electrolyte containing a perchlorate salt; the cell is a primary electrochemical cell and includes two pieces of aluminum in electrical contact with each other. The two pieces can be made of the same alloy of aluminum.
  • In yet another aspect, the invention features a method of inhibiting aluminum corrosion in a primary electrochemical cell. The method includes: (a) adding a perchlorate salt to the electrolyte of the cell; and (b) placing the electrolyte, an anode containing Li, and a cathode containing MnO2 and an aluminum current collector into a cell case. The perchlorate salt can be, e.g., LiClO4, Ca(ClO4)2, Al(ClO4)3, or Ba(ClO4)2.
  • The details of one or more embodiments of the invention are set forth in the accompanying drawings and the description below. Other features, objects, and advantages of the invention will be apparent from the description and drawings, and from the claims.
    • DESCRIPTION OF DRAWINGS
  • FIG. 1 is a sectional view of a nonaqueous electrochemical cell.
  • FIG. 2 is a graph showing current density vs. potential of the aluminum in an electrode exposed to LiTFS, DME:EC:PC electrolytes containing different amounts of LiClO4.
  • FIG. 3 is a graph showing current density vs. time of the aluminum in an electrode exposed to LiTFS, DME:EC:PC electrolytes containing different amounts of LiClO4.
  • FIG. 4 is a graph showing current density vs. time of the aluminum in an electrode exposed to a LiTFS, DME:EC:PC electrolyte containing LiClO4.
  • FIG. 5 is a graph showing current density vs. potential of the aluminum in an electrode exposed to LiTFS+LiTFSI, DME:EC:PC electrolytes containing different amounts of LiClO4.
  • FIG. 6 is a graph showing current density vs. time of the aluminum in an electrode exposed to LiTFS+LiTFSI, DME:EC:PC electrolytes containing different amounts of LiClO4.
  • FIG. 7 is a graph showing current density vs. potential of the aluminum in an electrode exposed to LiTFS+LiPF6, DME:EC:PC electrolytes containing different amounts of LiClO4.
  • FIG. 8 is a graph showing current density vs. time of the aluminum in an electrode exposed to LiTFS+LiPF6, DME:EC:PC electrolytes containing different amounts of LiClO4.
  • FIG. 9 is a graph showing current density vs. potential of the aluminum in an electrode exposed to a LiTFS, DME:EC:PC electrolyte containing different amounts of LiClO4 and different amounts of Al(ClO4)3.
  • FIG. 10 is a graph showing current density vs. potential of the aluminum in an electrode exposed to a LiTFS, DME:EC:PC electrolyte containing different amounts of LiClO4 and different amounts of Ba(ClO4)2.
    • DETAILED DESCRIPTION
  • Referring to FIG. 1, an electrochemical cell 10 includes an anode 12 in electrical contact with a negative lead 14, a cathode 16 in electrical contact with a positive lead 18, a separator 20 and an electrolytic solution. Anode 12, cathode 16, separator 20 and the electrolytic solution are contained within a case 22. The electrolytic solution includes a solvent system and a salt that is at least partially dissolved in the solvent system.
  • Cathode 16 includes an active cathode material, which is generally coated on the cathode current collector. The current collector is generally titanium, stainless steel, nickel, aluminum, or an aluminum alloy, e.g., aluminum foil. The active material can be, e.g., a metal oxide, halide, or chalcogenide; alternatively, the active material can be sulfur, an organosulfur polymer, or a conducting polymer. Specific examples include MnO2, V2O5, CoF3, MoS2, FeS2, SOCl2, MoO3, S, (C6H5N)n, (S3N2)n, where n is at least 2. The active material can also be a carbon monofluoride. An example is a compound having the formula CFx, where x is 0.5 to 1.0. The active material can be mixed with a conductive material such as carbon and a binder such as polytetrafluoroethylene (PTFE). An example of a cathode is one that includes aluminum foil coated with MnO2. The cathode can be prepared as described in U.S. Pat. No. 4,279,972.
  • Anode 12 can consist of an active anode material, usually in the form of an alkali metal, e.g., Li, Na, K, or an alkaline earth metal, e.g., Ca, Mg. The anode can also consist of alloys of alkali metals and alkaline earth metals or alloys of alkali metals and Al. The anode can be used with or without a substrate. The anode also can consist of an active anode material and a binder. In this case an active anode material can include carbon, graphite, an acetylenic mesophase carbon, coke, a metal oxide and/or a lithiated metal oxide. The binder can be, for example, PTFE. The active anode material and binder can be mixed to form a paste which can be applied to the substrate of anode 12.
  • Separator 20 can be formed of any of the standard separator materials used in nonaqueous electrochemical cells. For example, separator 20 can be formed of polypropylene, (e.g., nonwoven polypropylene or microporous polypropylene), polyethylene, and/or a polysulfone.
  • The electrolyte can be in liquid, solid or gel (polymer) form. The electrolyte can contain an organic solvent such as propylene carbonate (PC), ethylene carbonate (EC), dimethoxyethane (DME), dioxolane (DO), tetrahydrofuran (THF), acetonitrile (CH3CN), gamma-butyrolactone, diethyl carbonate (DEC), dimethyl carbonate (DMC), ethyl methyl carbonate (EMC) dimethylsulfoxide (DMSO) methyl acetate (MA), methyl formiate (MF), sulfolane or combinations thereof. The electrolyte can alternatively contain an inorganic solvent such as SO2 or SOCl2. The electrolyte also contains a lithium salt such as lithium trifluoromethanesulfonate (LiTFS) or lithium trifluoromethanesulfonimide (LiTFSI), or a combination thereof. Additional lithium salts that can be included are listed in U.S. Pat. No. 5,595,841, which is hereby incorporated by reference in its entirety. In some embodiments, the electrolyte may contain LiPF6; in other embodiments, the electrolyte is essentially free of LiPF6. The electrolyte also contains a perchlorate salt, which inhibits corrosion in the cell. Examples of suitable salts include lithium, barium, calcium, aluminum, sodium, potassium, magnesium, copper, zinc, ammonium, and tetrabutylammonium perchlorates. Generally, at least 500 ppm by weight of the perchlorate salt is used; this ensures that there is enough salt to suppress corrosion. In addition, less than about 20,000 by weight of the perchlorate salt is generally used. If too much perchlorate salt is used, the cell can be internally shorted under certain conditions during use.
  • To assemble the cell, separator 20 can be cut into pieces of a similar size as anode 12 and cathode 16 and placed therebetween as shown in FIG. 1. Anode 12, cathode 16, and separator 20 are then placed within case 22, which can be made of a metal such as nickel, nickel plated steel, stainless steel, or aluminum, or a plastic such as polyvinyl chloride, polypropylene, polysulfone, ABS or a polyamide. Case 22 is then filled with the electrolytic solution and sealed. One end of case 22 is closed with a cap 24 and an annular insulating gasket 26 that can provide a gas-tight and fluid-tight seal. Positive lead 18, which can be made of aluminum, connects cathode 16 to cap 24. Cap 24 may also be made of aluminum. A safety valve 28 is disposed in the inner side of cap 24 and is configured to decrease the pressure within battery 10 when the pressure exceeds some predetermined value. Additional methods for assembling the cell are described in U.S. Pat. Nos. 4,279,972; 4,401,735; and 4,526,846.
  • Other configurations of battery 10 can also be used, including, e.g., the coin cell configuration. The batteries can be of different voltages, e.g., 1.5V, 3.0V, or 4.0V.
  • The invention is further described in the following examples, which do not limit the scope of the invention described in the claims.
    • EXAMPLE 1 Al Corrosion in Different Electrolytes with Addition of LiClO4
  • Glass Cell Experimentation
  • An electrochemical glass cell was constructed having an Al working electrode, a Li reference electrode, and two Li auxiliary electrodes. The working electrode was fabricated from a 99.999% Al rod inserted into a Teflon sleeve to provide a planar electrode area of 0.33 cm2. The native oxide layer was removed by first polishing the planar working surface with 3 μm aluminum oxide paper under an argon atmosphere, followed by thorough rinsing of the Al electrode in electrolyte. All experiments were performed under an Ar atmosphere.
    • Cyclic Voltammetry
  • Corrosion current measurements were made according to a modified procedure generally described in X. Wang et al., Electrochemica Acta, vol. 45, pp. 2677-2684 (2000). The corrosion potential of Al was determined by continuous cyclic voltammetry. In each cycle, the potential was initially set to an open circuit potential, then anodically scanned to +4.5 V and reversed to an open circuit potential. A scan rate of 50 mV/s was selected, at which good reproducibility of the corrosion potential of aluminum was obtained. The corrosion potential of aluminum was defined as the potential at which the anodic current density reached 10−5 A/cm2 at the first cycle.
    • Chronoamperometry
  • Corrosion current measurements were made according to the procedure described in EP 0 852 072. The aluminum electrode was polarized at various potentials vs. a Li reference electrode while the current was recorded vs. time. Current vs. time measurements were taken during a 30-minute period. The area under current vs. time curve was used as a measure of the amount of aluminum corrosion occurring. The experiment also could be terminated in case the current density reached 3 mA/cm2 before the 30 minute time period elapsed and no corrosion suppression occurred. Corrosion suppression occurred when the resulting current density was observed in the range of 10−6 A/cm2.
  • Referring to FIG. 2, cyclic voltammograms taken in the electrolyte containing LiTFS and DME:EC:PC showed significant shifts in the corrosion potential of the Al electrode. The addition of LiClO4 to the electrolyte shifted the potential of aluminum in the positive direction, which indicates corrosion suppression.
  • Curves “a” and “a′” in FIG. 2 show the corrosion potential of the aluminum in the electrolyte containing no LiClO4. The addition of 500 ppm of LiClO4 to the electrolyte shifted the potential of the aluminum 150 mV in the positive direction (curves “b” and “b′”); the addition of 1000 ppm of LiClO4 to the electrolyte shifted the potential 300 mV (curves “c” and “c′”); and the addition of 2500 ppm of LiClO4 to the electrolyte shifted the potential 600 mV (curves “d” and “d′”). These results demonstrate that the addition of increasing amounts of LiClO4 to the electrolyte containing LiTFS salt and mixture of DME:EC:PC results in increasing degrees of corrosion protection of the aluminum electrode.
  • Referring to FIG. 3, curve “a” shows a potentiostatic dependence (chronoamperogram) of the aluminum electrode exposed to the electrolyte containing LiTFS, DME:EC:PC with the addition of 500 ppm LiClO4; curve “b” shows the chronoamperogram taken in the same electrolyte with addition of 1000 ppm LiClO4; curve “c” shows the chronoamperogram taken in the electrolyte containing LiTFS, DME:EC:PC, and 2500 ppm LiClO4. As shown in FIG. 3, at a LiClO4 concentration of 2500 ppm, the aluminum corrosion at +3.6 V (vs. a Li reference electrode) is effectively suppressed, and the corrosion current is less than 10−6 A/cm2 after 30 minutes of measurement.
  • Referring to FIG. 4, the electrochemical window of Al stability can be extended as high as +4.2 V (vs. a Li reference electrode) by increasing the concentration of LiClO4 to 1% (10,000 ppm). At a LiClO4 concentration of 1%, aluminum corrosion is effectively suppressed at 4.2 V. The corrosion current after 30 minutes is 8-10 μA/cm2, and the current continues to fall over time. The falling current indicates passivation of the Al surface. The increased level of the resulting current (10 μA/cm2 vs. 1 μA/cm2 after 30 minutes of experiment) is due to the increased background current at these potentials.
  • Referring to FIG. 5, curves “a”, “a′”, and “a″” show the corrosion potential of an aluminum electrode subjected to an electrolyte containing a mixture of LiTFS and LiTFSI salts, DME:EC:PC, and no LiClO4. The addition of 500 ppm of LiClO4 to this electrolyte shifted the corrosion potential of the aluminum 150 mV in the positive direction (curves “b” and “b′”); the addition of 1000 ppm of LiClO4 to the electrolyte shifted the potential 280 mV (curves “c” and “c′”); and the addition of 2500 ppm of LiClO4 to the electrolyte shifted potential 460 mV (curves “d” and “d′”). These results demonstrate that the addition of increasing amounts of LiClO4 to the electrolyte containing the mixture of LiTFS and LiTFSI salts and DME:EC:PC results in increasing degrees of corrosion protection of the aluminum electrode.
  • Referring to FIG. 6, curve “a” shows the chronoamperogram of the aluminum electrode exposed to the electrolyte containing a mixture of LiTFS and LiTFSI salts, DME:EC:PC, and 1000 ppm LiClO4; and curve “b” shows the chronoamperogram of the aluminum electrode exposed to the same electrolyte containing 2500 ppm LiClO4. As shown in FIG. 5, at a LiClO4 concentration of 2500 ppm in LiTFS, LiTFSI, DME:EC:PC electrolyte, the aluminum corrosion at +3.6 V is effectively suppressed, and resulting corrosion current of the Al electrode is about 10−6 A/cm2 after 30 minutes.
  • Referring to FIG. 7, curve “a” shows the corrosion potential of the aluminum subjected to an electrolyte containing a mixture of LiTFS and LiPF6 salts, DME:EC:PC, and no LiClO4. The addition of 500 ppm of LiClO4 to this electrolyte shifted the corrosion potential of the aluminum 125 mV in the positive direction (curve “b”); the addition of 2500 ppm of LiClO4 to the electrolyte shifted the potential 425 mV (curve “c”); and the addition of 5000 ppm of LiClO4 to the electrolyte shifted the potential 635 mV (curve “d”). These results demonstrate that the addition of increasing amounts of LiClO4 to the electrolyte containing the mixture of LiTFS, LiPF6 salts, and DME:EC:PC results in increasing degrees of corrosion protection of the aluminum electrode.
  • Referring to FIG. 8, curve “a” shows a chronoamperogram of the aluminum electrode exposed to the electrolyte containing LiTFS, LiPF6, DME:EC:PC with no LiClO4; curve “b” shows a chronoamperogram taken in the same electrolyte with 2500 ppm LiClO4 added; curve “c” shows a chronoamperogram taken in the electrolyte containing LiTFS, LiPF6, DME:EC:PC, and 5000 ppm LiClO4. As shown in FIG. 8, at a LiClO4 concentration of 5000 ppm, the aluminum corrosion at +3.6 V (vs. a Li reference electrode) is effectively suppressed, and the corrosion current is less than 10−6 A/cm2 after 30 minutes of measurement.
    • EXAMPLE 2 Al Corrosion in Electrolytes Containing LiTFS, DME:EC:PC, with the Addition of Different Perchlorates
  • Electrochemical glass cells were constructed as described in Example 1. Cyclic voltammetry and chromoamperometry were performed as described in Example 1.
  • Referring to FIG. 9, curves “a”, “b”, and “c” show the corrosion potential of an aluminum electrode exposed to the electrolyte LiTFS, DME:EC:PC containing 0, 1000 and 2500 ppm of LiClO4, respectively. Curves “a′”, “b′,” and “c′” show the corrosion potential of an aluminum electrode exposed to the electrolyte LiTFS, DME:EC:PC containing 0, 1000 and 2500 ppm of Al(ClO4)3, respectively. These results demonstrate that the addition of Al(ClO4)3 salt, like the addition of LiClO4 salt, suppressed the corrosion of Al.
  • Referring to FIG. 10, curves “a”, “b”, and “c” show the corrosion potential of an aluminum electrode exposed to the electrolyte LiTFS, DME:EC:PC containing 0, 1000 and 2500 ppm of LiClO4, respectively. Curves “a′”, “b′” and “c′” show the corrosion potential of an aluminum electrode exposed to the electrolyte LiTFS, DME:EC:PC containing 0, 1000 and 2500 ppm of Ba(ClO4)2, respectively. These results demonstrate that the addition of Ba(ClO4)2 salt, like the addition of LiClO4 salt, suppressed the corrosion of Al.
  • The shifts in the corrosion potential that result from the addition of LiClO4, Al(ClO4)3, and Ba(ClO4)2 to an electrolyte containing LiTFS and DME:EC:PC are summarized below in Table 1.
    TABLE 1
    Anodic shift of corrosion
    potential (mV)
    Additive 0 ppm 1000 ppm 2500 ppm
    Al(ClO4)3 0 170 450
    Ba(ClO4)2 0 170 400
    LiClO 4 0 300 600
    • Example 3 Al Corrosion in Electrolyte Containing LiTFS, DME:EC:PC, (Vial Storage Test)
    • The following test conditions were used:
      • Electrodes: EMD (electrochemically synthesized manganese dioxide) based cathodes applied on the Al current collector
      • Electrolyte (10 mL per sample): LiTFS, DME:EC:PC with and without addition of LiClO4 salt
      • Aging conditions: 60° C. for 20 days
    • Direct determination of Al corrosion was performed in one of two ways:
      • Analytical determination of Al ions in the electrolyte after aging (ICP method)
      • Direct observation of the Al surface (optical microscopy) after aging
  • Measurements of Al corrosion were performed by measuring the Al ions in the electrolyte after aging of the EMD based cathodes with an Al current collector. Analytical results (ICP) are summarized in Table 2.
    TABLE 2
    Al concentration
    Sample Electrolyte after storage (ppm)
    None LiTFS, DME:EC:PC 1.94 ± 0.20
    EMD based cathode on LiTFS, DME:EC:PC 21.55 ± 1.58 
    Al current collector
    EMD based cathode on LiTFS, DME:EC:PC + 2.16 ± 0.18
    Al current collector 2500 ppm LiClO4
  • The level of Al ions in the electrolyte indicates the rate of Al corrosion. As shown above, the background level of Al ions in solution is about 2 ppm. As referred to herein, the corrosion of a metal is said to be suppressed when, after the test described above is performed, the concentration of metal ions in the electrolyte is less than about 3 ppm, which is just above the background level.
  • The Al concentration in the electrolyte without LiClO4 addition is high (the range is 19.4-23 ppm). Thus, part of the Al substrate has dissolved (corroded) under the potential of the applied active cathode material.
  • On the other hand, the samples which were stored in the electrolytes with added LiClO4 did not show any corrosion (the resulting Al concentration in the electrolyte is at the background level 1.9-2.3 ppm). These data confirm results of the electrochemical measurements in a glass cell: 2500 ppm of LiClO4 completely suppresses the corrosion of Al at the potential of the EMD cathode.
  • The analytical data were confirmed by the direct observation of Al surface after aging (under an optical microscope, at a magnification of 60×). The electrodes stored in the electrolyte without LiClO4 exhibited substantial corrosion, as viewed under the optical microscope. The section stored in the electrolyte with added LiClO4 showed virtually no corrosion.
    • EXAMPLE 4 Al Current Collector Coupled with Other Metals, (Vial Storage Test)
  • The same cathodes on the Al substrate as described above were used in this experiment. In this case, the Al substrates were welded to stainless steel (SS) or nickel (Ni) tabs. A description of the samples and analytical results is presented in Table 3.
    TABLE 3
    Ni Al Fe
    Sample Electrolyte (ppm) (ppm) (ppm)
    None LiTFS, DME:EC:PC <1.0 <1.0 <1.0
    Cathode (Al cur. LiTFS, DME:EC:PC <1.0 24.4 5.3
    collector with
    welded SS tab)
    Cathode (Al cur. LiTFS, DME:EC:PC 90.9 20.5 <1.0
    collector with
    welded Ni tab)
    Cathode (Al cur. LiTFS, DME:EC:PC + <1.0 <1.0 <1.0
    collector with 2500 ppm LiClO4
    welded SS tab)
    Cathode (Al cur. LiTFS, DME:EC:PC + <1.0 <1.0 <1.0
    collector with 2500 ppm LiClO4
    welded Ni tab)
  • The highest corrosion rate was observed on the sample welded to the SS tab and stored in the electrolyte without added LiClO4 (the resulting solution contains the residue colored as a rust, and the SS tab is separated from the Al substrate). The presence of iron (5.3 ppm of Fe ions in the resulting electrolyte) indicates a high rate of SS corrosion as well as Al corrosion (24.4 ppm of the Al in the resulting electrolyte).
  • A high concentration of Ni (90.9 ppm) in the resulting electrolyte (Al current collector with welded Ni tab, electrolyte without LiClO4) indicates the severe corrosion of the Ni tab coupled with Al (the Al corroded as well, as indicated by the presence of 20.5 ppm Al).
  • On the other hand, the samples stored in the electrolytes with added LiClO4 did not show any corrosion (the resulting Al, Ni, Fe concentrations in the electrolyte were at the background level of <1 ppm).
    • EXAMPLE 5 Al Corrosion in Electrolyte Containing LiTFS, DME:EC:PC and 2500 ppm of LiClO4, (2/3A Cell Tests)
  • Cells were assembled with investigated parts and electrolytes according to the standard procedure with Al current foil applied as the cathode substrate.
  • The assembled cells (2/3A size) were stored 20 days at 60° C. Electrolyte removed from the cells after storage was submitted for ICP analysis. The electrolyte did not show any traces of Al, Fe, or Ni (the concentrations were at the background level).
    • EXAMPLE 6 Corrosion Tests Using Different Aluminum Alloys, (Vial Storage Test)
  • Two cathodes were prepared by coating aluminum foil substrates (1145 Al) with MnO2. Pieces of aluminum foil (3003 Al) were welded to the aluminum foil of each of the cathodes. One cathode was stored for 20 days at 60° C. over LiTFS, DME:EC:PC electrolyte containing 2500 ppm of LiClO4. The second cathode was stored for 20 days at 60° C. over LiTFS, DME:EC:PC electrolyte containing no LiClO4. After the 20-day period, the electrolytes were analyzed by ICP. The first electrolyte (2500 ppm LiClO4 in the electrolyte) contained less than 1 ppm Al, while the second electrolyte (no LiClO4 in the electrolyte) contained 18 ppm Al. These results indicate that the presence of LiClO4 can suppress corrosion when two different alloys of aluminum are in electrical contact in the presence of electrolyte.
  • All publications, patents, and patent applications mentioned in this application are herein incorporated by reference to the same extent as if each individual publication, patent, or patent application was specifically and individually indicated to be incorporated by reference.
    • OTHER EMBODIMENTS
  • A number of embodiments of the invention have been described. Nevertheless, it will be understood that various modifications may be made without departing from the spirit and scope of the invention. For example, although the examples described above relate to batteries, the invention can be used to suppress aluminum corrosion in systems other than batteries, in which an aluminum-metal couple occurs. Other embodiments are within the scope of the following claims.

Claims (15)

1-42. (canceled)
43. A method of inhibiting aluminum corrosion in an electrochemical cell, the method comprising:
(a) adding a lithium perchlorate salt and a lithium salt selected from the group consisting of LiTFS, LiTFSI, and LiPF6 to an electrolyte; and
(b) placing the electrolyte, an anode, a cathode, and an aluminum current collector into a cell case to form the cell, wherein the cell is a primary electrochemical cell.
44-47. (canceled)
48. The method of claim 43, wherein the anode contains lithium.
49. The method of claim 43, wherein the cathode contains MnO2.
50. The method of claim 43, wherein the method comprises adding at least 500 ppm by weight of the lithium perchlorate to the electrolyte.
51. The method of claim 43, wherein the method comprises adding at least 1000 ppm by weight of the lithium perchlorate to the electrolyte.
52. The method of claim 43, wherein the method comprises adding at least 1500 ppm by weight of the lithium perchlorate to the electrolyte.
53. The method of claim 43, wherein the method comprises adding at least 2500 ppm by weight of the lithium perchlorate to the electrolyte.
54. The method of claim 43, wherein the method comprises adding less than 20,000 ppm by weight of the lithium perchlorate to the electrolyte.
55. The method of claim 43, wherein the cell case comprises aluminum.
56. The method of claim 55, wherein the cell case consists essentially of aluminum.
57. The method of claim 43, wherein the method comprises adding at least 5000 ppm by weight of LiPF6 to the electrolyte.
58. The method of claim 43, wherein the method comprises adding at least 10,000 ppm by weight of LiPF6 to the electrolyte.
59. The method of claim 43, wherein the method does not comprise adding LiPF6 to the electrolyte, and the electrolyte is essentially free of LiPF6.
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Publication number Priority date Publication date Assignee Title
US20070059588A1 (en) * 2005-09-15 2007-03-15 Lee Ho C Additives for non-aqueous electrolytes and electrochemical device using the same
US20070202409A1 (en) * 2006-02-24 2007-08-30 Sony Corporation Lithium/iron disulfide primary cell

Families Citing this family (41)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US20030113622A1 (en) * 2001-12-14 2003-06-19 Blasi Jane A. Electrolyte additive for non-aqueous electrochemical cells
US20030162099A1 (en) * 2002-02-28 2003-08-28 Bowden William L. Non-aqueous electrochemical cell
JP2004014306A (en) * 2002-06-07 2004-01-15 Mitsui Mining & Smelting Co Ltd Electrolytic solution for alkaline battery and alkaline battery using this electrolytic solution
US7033698B2 (en) * 2002-11-08 2006-04-25 The Gillette Company Flexible cathodes
US7459234B2 (en) * 2003-11-24 2008-12-02 The Gillette Company Battery including aluminum components
US7279250B2 (en) * 2003-11-24 2007-10-09 The Gillette Company Battery including aluminum components
US7544384B2 (en) * 2003-11-24 2009-06-09 The Gillette Company Methods of making coated battery components
US10629947B2 (en) 2008-08-05 2020-04-21 Sion Power Corporation Electrochemical cell
US7459237B2 (en) * 2004-03-15 2008-12-02 The Gillette Company Non-aqueous lithium electrical cell
JP2005276872A (en) * 2004-03-23 2005-10-06 Sanyo Electric Co Ltd Electric double layer capacitor and electrolyte battery
US7285356B2 (en) * 2004-07-23 2007-10-23 The Gillette Company Non-aqueous electrochemical cells
US7479348B2 (en) * 2005-04-08 2009-01-20 The Gillette Company Non-aqueous electrochemical cells
EP1879252A4 (en) * 2005-04-19 2010-06-23 Panasonic Corp Nonaqueous electrolyte solution, electrochemical energy storage device using same, and nonaqueous electrolyte secondary battery
US7867553B2 (en) * 2006-08-23 2011-01-11 The Gillette Company Method of making cathode including iron disulfide
US20080050654A1 (en) * 2006-08-23 2008-02-28 Maya Stevanovic Battery
FR2913530B1 (en) * 2007-03-09 2009-06-05 Accumulateurs Fixes ELECTRICAL TERMINAL FOR WATERPROOF ACCUMULATOR.
US20090081545A1 (en) * 2007-06-28 2009-03-26 Ultralife Corporation HIGH CAPACITY AND HIGH RATE LITHIUM CELLS WITH CFx-MnO2 HYBRID CATHODE
US20100239914A1 (en) * 2009-03-19 2010-09-23 Sion Power Corporation Cathode for lithium battery
AU2008317471B2 (en) * 2007-10-19 2012-08-30 Energizer Brands, Llc Lithium-Iron Disulfide Cell Design
EP2240973B1 (en) * 2008-01-08 2018-03-28 Sion Power Corporation Porous electrodes and associated methods
US20090202910A1 (en) * 2008-02-08 2009-08-13 Anglin David L Alkaline Batteries
US20100068609A1 (en) * 2008-09-15 2010-03-18 Ultralife Corportion Hybrid cell construction for improved performance
US8088511B2 (en) * 2009-06-12 2012-01-03 Tesla Motors, Inc. Cell cap assembly with recessed terminal and enlarged insulating gasket
CN102640327B (en) * 2009-08-27 2015-11-25 永备电池有限公司 There is the Lithium-iron disulfide cathode formulation of high sulfide pyrite content and low electric conductivity additive
IN2012DN02063A (en) 2009-08-28 2015-08-21 Sion Power Corp
US20110206992A1 (en) * 2009-08-28 2011-08-25 Sion Power Corporation Porous structures for energy storage devices
US11081721B2 (en) 2009-11-24 2021-08-03 Duracell U.S. Operations, Inc. Secondary electrochemical cells with separator and electrolyte combination
KR101807911B1 (en) 2011-06-17 2017-12-11 시온 파워 코퍼레이션 Plating technique for electrode
US9252400B2 (en) 2011-09-07 2016-02-02 Tesla Motors, Inc. Battery cap assembly with high efficiency vent
US8936870B2 (en) 2011-10-13 2015-01-20 Sion Power Corporation Electrode structure and method for making the same
CN104041014B (en) 2012-01-09 2017-12-01 加速有限公司 HFC cable systems with broad-band communication path and coaxial cable domain node
WO2013123131A1 (en) 2012-02-14 2013-08-22 Sion Power Corporation Electrode structure for electrochemical cell
US20130236756A1 (en) * 2012-03-09 2013-09-12 Ultralife Corporation Lithium bobbin cell with cathode using wrapped metal grid as current collector
EP2936594B1 (en) 2012-12-19 2017-02-22 Basf Se Electrode structure and method for making same
US9692038B2 (en) 2013-11-25 2017-06-27 Tesla, Inc. Cap for electrochemical cell
US9711784B2 (en) 2014-05-01 2017-07-18 Sion Power Corporation Electrode fabrication methods and associated systems and articles
US10615457B2 (en) 2015-02-25 2020-04-07 Ses Holdings Pte. Ltd. Electrolyte system for high voltage lithium ion battery
JP6879214B2 (en) * 2015-11-19 2021-06-02 三洋電機株式会社 Non-aqueous electrolyte secondary battery
CN106099164B (en) * 2016-08-23 2018-08-17 辽宁九夷锂能股份有限公司 A kind of three electrode assembly of cylindrical battery and its assemble method
JP6996172B2 (en) * 2017-09-04 2022-01-17 株式会社豊田自動織機 Manufacturing method of lithium ion secondary battery
EP4106096B1 (en) * 2021-04-30 2024-10-23 Contemporary Amperex Technology (Hong Kong) Limited Connection member, battery cell, battery, and electrical device

Citations (89)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US345124A (en) * 1886-07-06 Briel bailhache
US2993946A (en) * 1957-09-27 1961-07-25 Rca Corp Primary cells
US3732124A (en) * 1970-07-01 1973-05-08 Accumulateurs Fixes Electrochemical cells comprising current collector member embedded into the protruding edges of the electrodes
US3761314A (en) * 1970-06-23 1973-09-25 Accumulateurs Fixes High discharge rate electric cells and batteries
US3905851A (en) * 1972-05-08 1975-09-16 Union Carbide Corp Method of making battery separators
US4129691A (en) * 1977-01-19 1978-12-12 Saft-Societe Des Accumulateurs Fixes Et De Traction Organic solvent electrolytes for high specific energy primary cells
US4181778A (en) * 1974-02-15 1980-01-01 Polaroid Corporation Novel battery anode
US4279972A (en) * 1979-08-27 1981-07-21 Duracell International Inc. Non-aqueous electrolyte cell
US4401735A (en) * 1979-12-28 1983-08-30 Duracell International Inc. Non-aqueous Li/MnO2 cell
US4499160A (en) * 1980-06-05 1985-02-12 Matzliach Babai Cathode and electrochemical cell containing same
US4526846A (en) * 1982-06-14 1985-07-02 Duracell Inc. Corrosion prevention additive
US4529675A (en) * 1984-11-21 1985-07-16 General Electric Company Rechargeable electrochemical cell having improved current collector means
US4555457A (en) * 1983-09-28 1985-11-26 Acr Electronics Inc. Battery cell containing potassium monoperoxysulfate in the cathode mix
US4755440A (en) * 1986-02-04 1988-07-05 Ramot University For Applied Research And Industrial Development Ltd. Electrochemical cell
US4803137A (en) * 1987-05-19 1989-02-07 Bridgestone Corporation Non-aqueous electrolyte secondary cell
US4863817A (en) * 1987-10-13 1989-09-05 Bridgestone Corporation Nonaqueous electrolyte cell
US4865932A (en) * 1987-05-12 1989-09-12 Bridgestone Corporation Electric cells and process for making the same
US4925751A (en) * 1989-04-26 1990-05-15 Shackle Dale R High power solid state electrochemical laminar cell
US4957833A (en) * 1988-12-23 1990-09-18 Bridgestone Corporation Non-aqueous liquid electrolyte cell
US4971686A (en) * 1988-12-28 1990-11-20 Pitney Bowes Inc. Mail handling machine with mis-sealed envelope detector
US5077152A (en) * 1989-09-25 1991-12-31 Ricoh Company, Ltd Negative electrode for secondary battery
US5114811A (en) * 1990-02-05 1992-05-19 W. Greatbatch Ltd. High energy density non-aqueous electrolyte lithium cell operational over a wide temperature range
US5176968A (en) * 1990-12-27 1993-01-05 Duracell Inc. Electrochemical cell
US5204196A (en) * 1991-02-25 1993-04-20 Osaka Gas Company Limited Solid state and conductive polymer composition
US5225296A (en) * 1989-11-21 1993-07-06 Ricoh Company, Ltd. Electrode and method of producing the same
US5240794A (en) * 1990-12-20 1993-08-31 Technology Finance Corporation (Proprietary) Limited Electrochemical cell
US5262255A (en) * 1991-01-30 1993-11-16 Matsushita Electric Industrial Co., Ltd. Negative electrode for non-aqueous electrolyte secondary battery
US5272022A (en) * 1990-09-28 1993-12-21 Kabushiki Kaisha Toshiba Non-aqueous electrolyte secondary battery
US5278005A (en) * 1992-04-06 1994-01-11 Advanced Energy Technologies Inc. Electrochemical cell comprising dispersion alloy anode
US5418084A (en) * 1992-11-23 1995-05-23 Eveready Battery Company, Inc. Electrochemical cell having a safety vent closure
US5462820A (en) * 1993-11-02 1995-10-31 Fuji Photo Film Co., Ltd. Non-aqueous battery with a block copolymer sealing member
US5523073A (en) * 1994-03-31 1996-06-04 Mitsui Mining & Smelting Co., Ltd. Manganese dioxide for lithium primary battery and method of producing the same
US5541022A (en) * 1992-08-06 1996-07-30 Hitachi, Ltd. Composite anode for nonaqueous secondary battery and method for producing the same
US5554462A (en) * 1993-12-22 1996-09-10 Saft Carbon anode for a lithium rechargeable electrochemical cell and a process for its production
US5567548A (en) * 1994-08-19 1996-10-22 Tracor Applied Sciences, Inc. Lithium ion battery with lithium vanadium pentoxide positive electrode
US5569558A (en) * 1995-06-05 1996-10-29 Wilson Greatbatch Ltd. Reduced voltage delay additive for nonaqueous electrolyte in alkali metal electrochemical cell
US5580683A (en) * 1993-11-01 1996-12-03 Wilson Greatbatch Ltd. high pulse power cell
US5595841A (en) * 1995-04-19 1997-01-21 Fuji Photo Film Co., Ltd. Nonaqueous secondary battery
US5639577A (en) * 1996-04-16 1997-06-17 Wilson Greatbatch Ltd. Nonaqueous electrochemical cell having a mixed cathode and method of preparation
US5654114A (en) * 1994-03-25 1997-08-05 Fuji Photo Film Co., Ltd. Nonaqueous secondary battery
US5691081A (en) * 1995-09-21 1997-11-25 Minnesota Mining And Manufacturing Company Battery containing bis(perfluoroalkylsulfonyl)imide and cyclic perfluoroalkylene disulfonylimide salts
US5750277A (en) * 1996-04-10 1998-05-12 Texas Instruments Incorporated Current interrupter for electrochemical cells
US5773734A (en) * 1995-12-21 1998-06-30 Dana Corporation Nitrided powdered metal piston ring
US5811205A (en) * 1994-12-28 1998-09-22 Saft Bifunctional electrode for an electrochemical cell or a supercapacitor and a method of producing it
US5834133A (en) * 1995-07-28 1998-11-10 Sanyo Electric Co., Ltd. Laser-sealed battery
US5851693A (en) * 1995-03-20 1998-12-22 Matsushita Electric Industrial Co., Ltd. Organic electrolyte batteries
US5958625A (en) * 1996-09-23 1999-09-28 Gnb Technologies, Inc. Positive lead-acid battery grids and cells and batteries using such grids
US5989745A (en) * 1994-11-28 1999-11-23 Mitsubishi Cable Industries, Ltd. Lithium secondary battery
US6001509A (en) * 1996-11-08 1999-12-14 Samsung Display Devices Co., Ltd. Solid polymer electrolytes
US6017656A (en) * 1996-11-27 2000-01-25 Medtronic, Inc. Electrolyte for electrochemical cells having cathodes containing silver vanadium oxide
US6025096A (en) * 1990-08-27 2000-02-15 Hope; Stephen F. Solid state polymeric electrolyte for electrochemical devices
US6030728A (en) * 1997-08-20 2000-02-29 International Business Machines Corporation High performance lithium polymer electrolyte battery
US6030422A (en) * 1997-11-03 2000-02-29 Wilson Greatbatch Ltd. Method for modifying the electrochemical surface area of a cell using a perforated film
US6045950A (en) * 1998-06-26 2000-04-04 Duracell Inc. Solvent for electrolytic solutions
US6053953A (en) * 1997-02-14 2000-04-25 Fuji Photo Film Co., Ltd. Nonaqueous secondary battery and process for preparation thereof
US6090506A (en) * 1996-08-02 2000-07-18 Fuji Photo Film Co. Ltd. Nonaqueous secondary battery
US6106977A (en) * 1995-10-30 2000-08-22 Mitsubishi Chemical Corporation Lithium secondary cells and methods for preparing active materials for negative electrodes
US6165644A (en) * 1994-11-23 2000-12-26 Polyplus Battery Company, Inc. Methods and reagents for enhancing the cycling efficiency of lithium polymer batteries
US6168889B1 (en) * 1998-12-10 2001-01-02 Micron Technology, Inc. Battery electrolytes and batteries
US6190803B1 (en) * 1996-07-26 2001-02-20 Fuji Photo Film Co., Ltd. Nonaqueous secondary battery
US6218055B1 (en) * 1998-06-05 2001-04-17 Mine Safety Appliances Company Electrochemical power cells and method of improving electrochemical power cell performance
US20010008146A1 (en) * 1998-07-17 2001-07-19 Georges Guarneri Gas pressure-regulating device for dispensing working fluid
US6287719B1 (en) * 1998-06-15 2001-09-11 Eveready Battery Company, Inc. Battery including a non-aqueous multi-cell spiral-wound electrode assembly
US20010028871A1 (en) * 1997-12-09 2001-10-11 Limtech Process for the purification of lithium carbonate
US20010033964A1 (en) * 1999-12-10 2001-10-25 Merck Patent Gesellschaft Mit Beschrankter Haftung Alkylspiroborate salts for use in electrochemical cells
US6316145B1 (en) * 1997-03-10 2001-11-13 Sanyo Electric Co., Ltd. Non-aqueous electrolyte battery and charging method therefor
US6322928B1 (en) * 1999-09-23 2001-11-27 3M Innovative Properties Company Modified lithium vanadium oxide electrode materials and products
US6352793B2 (en) * 1997-10-14 2002-03-05 Ngk Insulators, Ltd. Lithium secondary battery
US20020028389A1 (en) * 2000-07-17 2002-03-07 Matsushita Electric Industrial Co., Ltd. Non-aqueous electrolyte and electrochemical device comprising the same
US6447957B1 (en) * 1999-04-05 2002-09-10 Toyo Aluminum Kabushiki Kaisha Metal foil for collector and method of manufacturing the same, collector for secondary battery and secondary battery
US20020136949A1 (en) * 2001-03-21 2002-09-26 Hong Gan Electrochemical cell having an electrode with a dicarbonate additive in the electrode active mixture
US20030003356A1 (en) * 2000-02-02 2003-01-02 Quallion Llc Bipolar electronics package
US6506516B1 (en) * 1998-06-30 2003-01-14 Metallgesellschaft Aktiengesellschaft Lithium bisoxalatoborate, the production thereof and its use as a conducting salt
US6521374B1 (en) * 1998-09-02 2003-02-18 Sanyo Electric Co., Ltd. Lithium secondary cell
US20030113622A1 (en) * 2001-12-14 2003-06-19 Blasi Jane A. Electrolyte additive for non-aqueous electrochemical cells
US20030118906A1 (en) * 2001-11-19 2003-06-26 Bowden William L. Primary lithium electrochemical cell
US20030143112A1 (en) * 2000-03-21 2003-07-31 Board Of Trustees Of The University Of Illinois Colorimetric artificial nose having an array of dyes and method for artificial olfaction
US20030186110A1 (en) * 2002-01-09 2003-10-02 Sloop Steven E. System and method for removing an electrolyte from an energy storage and/or conversion device using a supercritical fluid
US20040005267A1 (en) * 1998-07-16 2004-01-08 Boryta Daniel Alfred Production of lithium compounds directly from lithium containing brines
US6689511B2 (en) * 1999-12-09 2004-02-10 Sharp Kabushiki Kaisha Secondary battery and electronic instrument using it
US20040053138A1 (en) * 2002-09-16 2004-03-18 Ralph Otterstedt Overcharge protection of nonaqueous rechargeable lithium batteries by cyano-substituted thiophenes as electrolyte additives
US20040096746A1 (en) * 2000-09-27 2004-05-20 Ulrich Wietelmann Method for drying organic liquid electrolytes
US6780543B2 (en) * 2001-02-14 2004-08-24 Sanyo Electric Co., Ltd. Aluminum or aluminum alloy-based lithium secondary battery
US20050019670A1 (en) * 2003-07-17 2005-01-27 Khalil Amine Long life lithium batteries with stabilized electrodes
US20050112467A1 (en) * 2003-11-24 2005-05-26 Berkowitz Fred J. Battery including aluminum components
US20050191545A1 (en) * 2004-02-26 2005-09-01 Qinetiq Limited Electrode assembly
US20050202320A1 (en) * 2004-03-15 2005-09-15 Totir Dana A. Non-aqueous electrochemical cells
US20060216597A1 (en) * 2002-11-08 2006-09-28 The Gillette Company, A Delaware Corporation Flexible cathodes
US7285356B2 (en) * 2004-07-23 2007-10-23 The Gillette Company Non-aqueous electrochemical cells

Family Cites Families (40)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
FR1415519A (en) 1963-07-18 1965-10-29 Accumulateurs Fixes Process for the arrangement of electrolytic cells and electric accumulators, and cells and accumulators obtained by this process
EP0138056B1 (en) † 1983-09-19 1987-12-23 Eveready Battery Company, Inc. Nonaqueous cell with a novel organic electrolyte
US4740433A (en) 1986-09-29 1988-04-26 American Telephone And Telegraph Co., At&T Bell Laboratories Nonaqueous battery with special separator
US4971868A (en) * 1986-11-03 1990-11-20 Eveready Battery Company, Inc. Hermetically sealed nonaqueous cell with positive terminal pin and perchlorate electrolyte
EP0270264B1 (en) 1986-11-13 1993-05-12 Seiko Electronic Components Ltd. An organic electrolyte cell
JPS63241867A (en) * 1987-03-30 1988-10-07 Sanyo Electric Co Ltd Nonaqueous electrolytic battery
JPS63119160A (en) * 1987-09-24 1988-05-23 Sanyo Electric Co Ltd Nonaqueous electrolyte cell
JPH01227990A (en) 1988-03-09 1989-09-12 Hitachi Ltd Nuclear fuel assembly
JPH069140B2 (en) * 1988-06-08 1994-02-02 富士電気化学株式会社 Spiral type non-aqueous electrolyte battery
JPH0256849A (en) * 1988-08-23 1990-02-26 Matsushita Electric Ind Co Ltd Organic electrolytic battery
JPH02204976A (en) 1989-01-23 1990-08-14 Moli Energ Ltd Electrochenical battery and its manufacture
US4963446A (en) 1989-04-05 1990-10-16 Eveready Battery Co., Inc. Inwardly indented edge electrode assembly
JPH0384858A (en) 1989-08-28 1991-04-10 Toshiba Battery Co Ltd Manufacture of organic solvent cell
JP2970086B2 (en) 1991-06-28 1999-11-02 ソニー株式会社 Non-aqueous electrolyte battery
JPH05174873A (en) 1991-12-24 1993-07-13 Sanyo Electric Co Ltd Nonaqueous electrolyte secondary battery resistant to overcharging
JPH0737572A (en) 1993-07-22 1995-02-07 Japan Storage Battery Co Ltd Lithium battery
JP3249305B2 (en) 1994-08-25 2002-01-21 三洋電機株式会社 Non-aqueous electrolyte battery
JP3384625B2 (en) * 1994-08-25 2003-03-10 三洋電機株式会社 Non-aqueous electrolyte battery
US5525441A (en) † 1994-09-13 1996-06-11 Power Conversion, Inc. Folded electrode configuration for galvanic cells
JPH0950823A (en) * 1995-06-01 1997-02-18 Ricoh Co Ltd Secondary battery
JPH0945373A (en) 1995-07-31 1997-02-14 Sanyo Electric Co Ltd Lithium secondary battery
JP3632968B2 (en) 1996-04-01 2005-03-30 日本電池株式会社 Nonaqueous electrolyte secondary battery
JPH09306443A (en) * 1996-05-20 1997-11-28 Haibaru:Kk Non-aqueous electrolyte battery
JPH10116633A (en) 1996-08-22 1998-05-06 Matsushita Electric Ind Co Ltd Non-aqueous electrolyte secondary battery
JPH10199493A (en) * 1997-01-10 1998-07-31 Japan Storage Battery Co Ltd Secondary battery
JP3464750B2 (en) 1997-01-21 2003-11-10 東芝電池株式会社 Lithium secondary battery
JP3030263B2 (en) 1997-05-09 2000-04-10 三洋電機株式会社 Non-aqueous electrolyte secondary battery
JPH1186906A (en) † 1997-09-16 1999-03-30 Central Glass Co Ltd Ion conductive medium composition
EP1100135A4 (en) † 1998-06-25 2006-06-14 Mitsubishi Electric Corp Cell and method of producing the same
US6060184A (en) * 1998-07-09 2000-05-09 Wilson Greatbatch Ltd. Inorganic and organic nitrate additives for nonaqueous electrolyte in alkali metal electrochemical cells
JP2000294231A (en) * 1999-02-04 2000-10-20 Toshiba Battery Co Ltd Organic electrolyte battery
DE19951804A1 (en) † 1999-10-28 2001-05-03 Merck Patent Gmbh Complex salts for use in electrochemical cells
JP2001143753A (en) * 1999-11-10 2001-05-25 Furukawa Electric Co Ltd:The Lithium ion secondary cell
KR100325866B1 (en) * 2000-01-25 2002-03-07 김순택 Lithium secondary battery
JP4644899B2 (en) * 2000-02-23 2011-03-09 ソニー株式会社 Electrode and battery, and manufacturing method thereof
EP1279199A2 (en) * 2000-04-25 2003-01-29 Rayovac Corporation Extended temperature operating range electrochemical cells
JP2002151065A (en) * 2000-11-07 2002-05-24 Sony Corp Negative electrode active material and non-aqueous electrolyte battery
US6447657B1 (en) * 2000-12-04 2002-09-10 Roche Diagnostics Corporation Biosensor
CN1235307C (en) * 2001-08-24 2006-01-04 日本电池株式会社 Non-aqueous electrolyte secondary battery
JP2003249208A (en) 2002-02-25 2003-09-05 Sanyo Electric Co Ltd Battery with electric parts

Patent Citations (90)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US345124A (en) * 1886-07-06 Briel bailhache
US2993946A (en) * 1957-09-27 1961-07-25 Rca Corp Primary cells
US3761314A (en) * 1970-06-23 1973-09-25 Accumulateurs Fixes High discharge rate electric cells and batteries
US3732124A (en) * 1970-07-01 1973-05-08 Accumulateurs Fixes Electrochemical cells comprising current collector member embedded into the protruding edges of the electrodes
US3905851A (en) * 1972-05-08 1975-09-16 Union Carbide Corp Method of making battery separators
US4181778A (en) * 1974-02-15 1980-01-01 Polaroid Corporation Novel battery anode
US4129691A (en) * 1977-01-19 1978-12-12 Saft-Societe Des Accumulateurs Fixes Et De Traction Organic solvent electrolytes for high specific energy primary cells
US4279972A (en) * 1979-08-27 1981-07-21 Duracell International Inc. Non-aqueous electrolyte cell
US4401735A (en) * 1979-12-28 1983-08-30 Duracell International Inc. Non-aqueous Li/MnO2 cell
US4499160A (en) * 1980-06-05 1985-02-12 Matzliach Babai Cathode and electrochemical cell containing same
US4526846A (en) * 1982-06-14 1985-07-02 Duracell Inc. Corrosion prevention additive
US4555457A (en) * 1983-09-28 1985-11-26 Acr Electronics Inc. Battery cell containing potassium monoperoxysulfate in the cathode mix
US4529675A (en) * 1984-11-21 1985-07-16 General Electric Company Rechargeable electrochemical cell having improved current collector means
US4755440A (en) * 1986-02-04 1988-07-05 Ramot University For Applied Research And Industrial Development Ltd. Electrochemical cell
US4865932A (en) * 1987-05-12 1989-09-12 Bridgestone Corporation Electric cells and process for making the same
US4803137A (en) * 1987-05-19 1989-02-07 Bridgestone Corporation Non-aqueous electrolyte secondary cell
US4863817A (en) * 1987-10-13 1989-09-05 Bridgestone Corporation Nonaqueous electrolyte cell
US4957833A (en) * 1988-12-23 1990-09-18 Bridgestone Corporation Non-aqueous liquid electrolyte cell
US4971686A (en) * 1988-12-28 1990-11-20 Pitney Bowes Inc. Mail handling machine with mis-sealed envelope detector
US4925751A (en) * 1989-04-26 1990-05-15 Shackle Dale R High power solid state electrochemical laminar cell
US5077152A (en) * 1989-09-25 1991-12-31 Ricoh Company, Ltd Negative electrode for secondary battery
US5225296A (en) * 1989-11-21 1993-07-06 Ricoh Company, Ltd. Electrode and method of producing the same
US5114811A (en) * 1990-02-05 1992-05-19 W. Greatbatch Ltd. High energy density non-aqueous electrolyte lithium cell operational over a wide temperature range
US6025096A (en) * 1990-08-27 2000-02-15 Hope; Stephen F. Solid state polymeric electrolyte for electrochemical devices
US5272022A (en) * 1990-09-28 1993-12-21 Kabushiki Kaisha Toshiba Non-aqueous electrolyte secondary battery
US5240794A (en) * 1990-12-20 1993-08-31 Technology Finance Corporation (Proprietary) Limited Electrochemical cell
US5176968A (en) * 1990-12-27 1993-01-05 Duracell Inc. Electrochemical cell
US5262255A (en) * 1991-01-30 1993-11-16 Matsushita Electric Industrial Co., Ltd. Negative electrode for non-aqueous electrolyte secondary battery
US5204196A (en) * 1991-02-25 1993-04-20 Osaka Gas Company Limited Solid state and conductive polymer composition
US5278005A (en) * 1992-04-06 1994-01-11 Advanced Energy Technologies Inc. Electrochemical cell comprising dispersion alloy anode
US5541022A (en) * 1992-08-06 1996-07-30 Hitachi, Ltd. Composite anode for nonaqueous secondary battery and method for producing the same
US5418084A (en) * 1992-11-23 1995-05-23 Eveready Battery Company, Inc. Electrochemical cell having a safety vent closure
US5580683A (en) * 1993-11-01 1996-12-03 Wilson Greatbatch Ltd. high pulse power cell
US5462820A (en) * 1993-11-02 1995-10-31 Fuji Photo Film Co., Ltd. Non-aqueous battery with a block copolymer sealing member
US5554462A (en) * 1993-12-22 1996-09-10 Saft Carbon anode for a lithium rechargeable electrochemical cell and a process for its production
US5654114A (en) * 1994-03-25 1997-08-05 Fuji Photo Film Co., Ltd. Nonaqueous secondary battery
US5523073A (en) * 1994-03-31 1996-06-04 Mitsui Mining & Smelting Co., Ltd. Manganese dioxide for lithium primary battery and method of producing the same
US5567548A (en) * 1994-08-19 1996-10-22 Tracor Applied Sciences, Inc. Lithium ion battery with lithium vanadium pentoxide positive electrode
US6165644A (en) * 1994-11-23 2000-12-26 Polyplus Battery Company, Inc. Methods and reagents for enhancing the cycling efficiency of lithium polymer batteries
US5989745A (en) * 1994-11-28 1999-11-23 Mitsubishi Cable Industries, Ltd. Lithium secondary battery
US5811205A (en) * 1994-12-28 1998-09-22 Saft Bifunctional electrode for an electrochemical cell or a supercapacitor and a method of producing it
US5851693A (en) * 1995-03-20 1998-12-22 Matsushita Electric Industrial Co., Ltd. Organic electrolyte batteries
US5595841A (en) * 1995-04-19 1997-01-21 Fuji Photo Film Co., Ltd. Nonaqueous secondary battery
US5569558A (en) * 1995-06-05 1996-10-29 Wilson Greatbatch Ltd. Reduced voltage delay additive for nonaqueous electrolyte in alkali metal electrochemical cell
US5834133A (en) * 1995-07-28 1998-11-10 Sanyo Electric Co., Ltd. Laser-sealed battery
US5691081A (en) * 1995-09-21 1997-11-25 Minnesota Mining And Manufacturing Company Battery containing bis(perfluoroalkylsulfonyl)imide and cyclic perfluoroalkylene disulfonylimide salts
US6106977A (en) * 1995-10-30 2000-08-22 Mitsubishi Chemical Corporation Lithium secondary cells and methods for preparing active materials for negative electrodes
US5773734A (en) * 1995-12-21 1998-06-30 Dana Corporation Nitrided powdered metal piston ring
US5750277A (en) * 1996-04-10 1998-05-12 Texas Instruments Incorporated Current interrupter for electrochemical cells
US5639577A (en) * 1996-04-16 1997-06-17 Wilson Greatbatch Ltd. Nonaqueous electrochemical cell having a mixed cathode and method of preparation
US6190803B1 (en) * 1996-07-26 2001-02-20 Fuji Photo Film Co., Ltd. Nonaqueous secondary battery
US6090506A (en) * 1996-08-02 2000-07-18 Fuji Photo Film Co. Ltd. Nonaqueous secondary battery
US5958625A (en) * 1996-09-23 1999-09-28 Gnb Technologies, Inc. Positive lead-acid battery grids and cells and batteries using such grids
US6001509A (en) * 1996-11-08 1999-12-14 Samsung Display Devices Co., Ltd. Solid polymer electrolytes
US6017656A (en) * 1996-11-27 2000-01-25 Medtronic, Inc. Electrolyte for electrochemical cells having cathodes containing silver vanadium oxide
US6053953A (en) * 1997-02-14 2000-04-25 Fuji Photo Film Co., Ltd. Nonaqueous secondary battery and process for preparation thereof
US6316145B1 (en) * 1997-03-10 2001-11-13 Sanyo Electric Co., Ltd. Non-aqueous electrolyte battery and charging method therefor
US6030728A (en) * 1997-08-20 2000-02-29 International Business Machines Corporation High performance lithium polymer electrolyte battery
US6352793B2 (en) * 1997-10-14 2002-03-05 Ngk Insulators, Ltd. Lithium secondary battery
US6030422A (en) * 1997-11-03 2000-02-29 Wilson Greatbatch Ltd. Method for modifying the electrochemical surface area of a cell using a perforated film
US20010028871A1 (en) * 1997-12-09 2001-10-11 Limtech Process for the purification of lithium carbonate
US6218055B1 (en) * 1998-06-05 2001-04-17 Mine Safety Appliances Company Electrochemical power cells and method of improving electrochemical power cell performance
US6287719B1 (en) * 1998-06-15 2001-09-11 Eveready Battery Company, Inc. Battery including a non-aqueous multi-cell spiral-wound electrode assembly
US6045950A (en) * 1998-06-26 2000-04-04 Duracell Inc. Solvent for electrolytic solutions
US6506516B1 (en) * 1998-06-30 2003-01-14 Metallgesellschaft Aktiengesellschaft Lithium bisoxalatoborate, the production thereof and its use as a conducting salt
US20040005267A1 (en) * 1998-07-16 2004-01-08 Boryta Daniel Alfred Production of lithium compounds directly from lithium containing brines
US20010008146A1 (en) * 1998-07-17 2001-07-19 Georges Guarneri Gas pressure-regulating device for dispensing working fluid
US6521374B1 (en) * 1998-09-02 2003-02-18 Sanyo Electric Co., Ltd. Lithium secondary cell
US6168889B1 (en) * 1998-12-10 2001-01-02 Micron Technology, Inc. Battery electrolytes and batteries
US6447957B1 (en) * 1999-04-05 2002-09-10 Toyo Aluminum Kabushiki Kaisha Metal foil for collector and method of manufacturing the same, collector for secondary battery and secondary battery
US6322928B1 (en) * 1999-09-23 2001-11-27 3M Innovative Properties Company Modified lithium vanadium oxide electrode materials and products
US6689511B2 (en) * 1999-12-09 2004-02-10 Sharp Kabushiki Kaisha Secondary battery and electronic instrument using it
US20010033964A1 (en) * 1999-12-10 2001-10-25 Merck Patent Gesellschaft Mit Beschrankter Haftung Alkylspiroborate salts for use in electrochemical cells
US20030003356A1 (en) * 2000-02-02 2003-01-02 Quallion Llc Bipolar electronics package
US20030143112A1 (en) * 2000-03-21 2003-07-31 Board Of Trustees Of The University Of Illinois Colorimetric artificial nose having an array of dyes and method for artificial olfaction
US20020028389A1 (en) * 2000-07-17 2002-03-07 Matsushita Electric Industrial Co., Ltd. Non-aqueous electrolyte and electrochemical device comprising the same
US20040096746A1 (en) * 2000-09-27 2004-05-20 Ulrich Wietelmann Method for drying organic liquid electrolytes
US6780543B2 (en) * 2001-02-14 2004-08-24 Sanyo Electric Co., Ltd. Aluminum or aluminum alloy-based lithium secondary battery
US20020136949A1 (en) * 2001-03-21 2002-09-26 Hong Gan Electrochemical cell having an electrode with a dicarbonate additive in the electrode active mixture
US20030118906A1 (en) * 2001-11-19 2003-06-26 Bowden William L. Primary lithium electrochemical cell
US20030124421A1 (en) * 2001-12-14 2003-07-03 Issaev Nikolai N. Non-aqueous electrochemical cells
US20030113622A1 (en) * 2001-12-14 2003-06-19 Blasi Jane A. Electrolyte additive for non-aqueous electrochemical cells
US20030186110A1 (en) * 2002-01-09 2003-10-02 Sloop Steven E. System and method for removing an electrolyte from an energy storage and/or conversion device using a supercritical fluid
US20040053138A1 (en) * 2002-09-16 2004-03-18 Ralph Otterstedt Overcharge protection of nonaqueous rechargeable lithium batteries by cyano-substituted thiophenes as electrolyte additives
US20060216597A1 (en) * 2002-11-08 2006-09-28 The Gillette Company, A Delaware Corporation Flexible cathodes
US20050019670A1 (en) * 2003-07-17 2005-01-27 Khalil Amine Long life lithium batteries with stabilized electrodes
US20050112467A1 (en) * 2003-11-24 2005-05-26 Berkowitz Fred J. Battery including aluminum components
US20050191545A1 (en) * 2004-02-26 2005-09-01 Qinetiq Limited Electrode assembly
US20050202320A1 (en) * 2004-03-15 2005-09-15 Totir Dana A. Non-aqueous electrochemical cells
US7285356B2 (en) * 2004-07-23 2007-10-23 The Gillette Company Non-aqueous electrochemical cells

Cited By (3)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US20070059588A1 (en) * 2005-09-15 2007-03-15 Lee Ho C Additives for non-aqueous electrolytes and electrochemical device using the same
US7824578B2 (en) 2005-09-15 2010-11-02 Lg Chem, Ltd. Additives for non-aqueous electrolytes and electrochemical device using the same
US20070202409A1 (en) * 2006-02-24 2007-08-30 Sony Corporation Lithium/iron disulfide primary cell

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US20030124421A1 (en) 2003-07-03
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AR038015A1 (en) 2004-12-22
AU2002360562A1 (en) 2003-06-30
US7927739B2 (en) 2011-04-19
EP2204869A2 (en) 2010-07-07
EP1527488B2 (en) 2017-07-19
US20030113622A1 (en) 2003-06-19
CN1630959A (en) 2005-06-22
US20080261110A1 (en) 2008-10-23
US20120096708A1 (en) 2012-04-26
EP1527488B1 (en) 2013-11-20
JP2005538498A (en) 2005-12-15
EP1527488A2 (en) 2005-05-04
EP2204869B1 (en) 2012-05-23
WO2003052845A2 (en) 2003-06-26
CN1320674C (en) 2007-06-06
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WO2003052845A3 (en) 2005-03-03
JP4623965B2 (en) 2011-02-02

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