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WO1999060638A2 - Materiaux pour cathodes de batterie - Google Patents

Materiaux pour cathodes de batterie Download PDF

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Publication number
WO1999060638A2
WO1999060638A2 PCT/US1999/010556 US9910556W WO9960638A2 WO 1999060638 A2 WO1999060638 A2 WO 1999060638A2 US 9910556 W US9910556 W US 9910556W WO 9960638 A2 WO9960638 A2 WO 9960638A2
Authority
WO
WIPO (PCT)
Prior art keywords
lithium
battery
precursor
less
cathode
Prior art date
Application number
PCT/US1999/010556
Other languages
English (en)
Other versions
WO1999060638A3 (fr
Inventor
Joseph E. Sunstrom, Iv
Enoch I. Wang
Original Assignee
Duracell Inc.
Priority date (The priority date is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the date listed.)
Filing date
Publication date
Application filed by Duracell Inc. filed Critical Duracell Inc.
Priority to AU39874/99A priority Critical patent/AU3987499A/en
Publication of WO1999060638A2 publication Critical patent/WO1999060638A2/fr
Publication of WO1999060638A3 publication Critical patent/WO1999060638A3/fr

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Classifications

    • 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
    • H01M4/58—Selection of substances as active materials, active masses, active liquids of inorganic compounds other than oxides or hydroxides, e.g. sulfides, selenides, tellurides, halogenides or LiCoFy; of polyanionic structures, e.g. phosphates, silicates or borates
    • H01M4/5825—Oxygenated metallic salts or polyanionic structures, e.g. borates, phosphates, silicates, olivines
    • 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
    • H01M4/505—Selection of substances as active materials, active masses, active liquids of inorganic oxides or hydroxides of manganese of mixed oxides or hydroxides containing manganese for inserting or intercalating light metals, e.g. LiMn2O4 or LiMn2OxFy
    • 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
    • H01M4/58—Selection of substances as active materials, active masses, active liquids of inorganic compounds other than oxides or hydroxides, e.g. sulfides, selenides, tellurides, halogenides or LiCoFy; of polyanionic structures, e.g. phosphates, silicates or borates
    • H01M4/582—Halogenides
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M10/00—Secondary cells; Manufacture thereof
    • H01M10/05—Accumulators with non-aqueous electrolyte
    • H01M10/052—Li-accumulators
    • 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

Definitions

  • BATTERY CATHODE MATERIALS The invention relates to battery cathode materials. Batteries are commonly used as energy sources. Typically, a battery includes a negative electrode, called the anode, a positive electrode, called the cathode, and an electrolyte. The battery can further include one or more layers of material, called the separator, that electrically isolate the anode from the cathode when the battery is not in use.
  • the anode and the cathode can be electrically connected through an external path so that electrons can flow from the anode to the cathode along the external path. This can cause the anode material to be oxidized while the cathode material can be reduced. During this process, ions can flow between the electrodes through the electrolyte.
  • lithium ion battery One type of battery is called a lithium ion battery.
  • lithium ions can be transferred from the anode through the electrolyte to the cathode during battery use.
  • lithium ions can flow from the cathode through the electrolyte to the anode.
  • lithium ion batteries can heat up.
  • the invention relates to materials that can be used as cathodes in lithium ion batteries.
  • the materials have good thermal stability, release limited amounts of oxygen upon heating and can exhibit good cyclability.
  • the invention features a battery cathode formed of a material having the empirical formula Li x M M' , O 2.z A z .
  • M and M' are different metals, and A is a halogen, x can have a value of from about 0.9 to about 1.2.
  • y can have a value of from greater than zero to less than 1 , and z can have a value of from greater than zero to less than 2.
  • the battery cathode can be used in a battery that further contains an anode and a separator disposed between the cathode and the anode.
  • the material has a substantially uniform distribution of fluorine atoms across its cross-section.
  • the oxidation state of nickel is low relative to nonfluorinated lithium metal oxides.
  • the invention features a battery cathode having a peak power of less than about 100 Joules per gram-minute. Peak power is measured according to the peak power test described below.
  • the invention features a method of making a lithium metal oxide material. The method includes combining spherical nickel hydroxide, a lithium precursor, a cobalt precursor and a fluorine precursor.
  • spherical nickel hydroxide refers to nickel hydroxide in the form of generally spherical particles as measured using scanning electron microscopy. Typically, spherical nickel hydroxide particles have a diameter of from about 5 microns to about 50 microns as measured by light scattering.
  • the invention features a method of making a material having a peak power of less than about 100 Joules per gram-minute.
  • the method includes combining a nickel precursor, a lithium precursor, a cobalt precursor and a fluorine precursor.
  • the figure is a sectional view of a lithium ion battery.
  • the figure shows a lithium ion battery 10 that 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 electrolyte.
  • Anode 12, cathode 16 and separator 20 are contained within a case 22.
  • case 22 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 connects anode 16 to cap 24.
  • 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.
  • Cathode 16 can include a lithium metal oxide material.
  • This material can have the empirical formula Li M y M l . y 0 2 or the formula Li x M y M' 1 . y O 2 . z A z .
  • the material has a substantially uniform distribution of fluorine atoms across its cross-section.
  • M and M' are different metals.
  • M is Sc, Ti, V, Cr, Mn, Fe, Ni, Cu, Zn, Al or Mg, and more preferably M is Ni.
  • M' is Sc, Ti, V, Cr, Mn, Fe, Ni, Co, Cu, Zn, Al or Mg, and more preferably M' is Co.
  • A can be a halogen, including fluorine, chlorine, bromine or iodine.
  • A is fluorine.
  • x is preferably from about 0.9 to about 1.2, more preferably from about 1 to about 1.1, and most preferably from about 1 to about 1.05.
  • y can have a value of greater than zero and less than 1.
  • y is from about 0.4 to about 0.95, more preferably y is from about 0.75 to about 0.85, and most preferably y is about 0.8.
  • z can have a value of greater than zero and less than 2.
  • z is from about 0.001 to about 0.4, more preferably from about 0.03 to about 0.2, and most preferably from about 0.05 to about 0.1.
  • the preferred lithium metal oxide has a low peak power and a low maximum rate of mass loss, corresponding to a material having good thermal stability.
  • the lithium metal oxide can have a peak power of less than about 100 Joules per gram-minute.
  • the lithium metal oxide from which cathode 16 is formed has a peak power of less than about 70 Joules per gram- minute, more preferably less than about 40 Joules per gram-minute, and most preferably less than about 30 Joules per gram-minute to about 40 Joules per gram- minute.
  • the peak power test is conducted as follows. 2.7 grams of lithium metal oxide is mixed with 0.15 grams of carbon black (Shawinigan Black, Chevron, located in California) and 0.15 grams of Teflon (DuPont, located in Wilmington,
  • cathode sample 0.12 grams of the cathode sample is pressed into one half of an aluminum coin cell can (2430 size) and dried in a vacuum for about four hours at about 150°C. An excess of lithium metal (anode sample) is pressed onto the other half of the aluminum coin cell can. Once the cathode sample is dry, both the cathode sample and anode sample are immediately placed into an argon atmosphere drybox. One layer of separator material (HiPore H-4030V, Asahi Chemicals, Japan) is placed on the cathode sample, and one layer of polypropylene oxide (Pellon) is placed on the anode sample.
  • separator material HiPore H-4030V, Asahi Chemicals, Japan
  • Both the cathode sample and the anode sample are soaked with a one molar solution of LiPF 6 in ethylene carbonate and dimethyl carbonate (50:50 by volume), assembled together with a plastic grommet to prevent shorting, and crimped.
  • the coin cell is then charged at about 0.5 milliamps to about 4.8 volts until full delithiation occurred.
  • the charged cell is pumped in the drybox and disassembled in the drybox without shorting the cell.
  • the cathode sample is placed into a gold sample pan.
  • the cathode sample is soaked in about two microliters of a solution of one molar LiPF 6 in ethylene carbonate and dimethyl carbonate (50:50 by volume).
  • the pan is then hermetically sealed with a gold lid.
  • the cathode sample is taken from the drybox and placed into a DSC instrument (TA Instruments model 2010, Wilmington, DE), and the temperature of the cathode sample is increased from room temperature to about 300°C at a rate of about 5°C per minute. During this temperature ramp, the cathode sample is kept under a flow of argon gas (about 50 cubic centimeters per minute).
  • the heat given off by the cathode sample is measured as the temperature of the cathode sample is increased, commonly referred to as an exotherm.
  • the time over which this heat is given off is determined by the point where the exotherm begins to deviate from the baseline by more than the noise level to the point where the exotherm returns to within the noise level of the baseline.
  • the total amount of heat given off by the cathode sample during this time is divided by the time and the mass of the cathode sample. To compensate for the fact that a portion of the mass of the sample was carbon and/or Teflon, the measured value is multiplied by 0.9.
  • the lithium metal oxide from which cathode 16 is made can have a maximum rate of mass loss of less than about 0.3% per °C.
  • the lithium metal oxide from which cathode 16 is formed has a maximum rate of mass loss of less than about 0.25% per °C, more preferably less than about 0.2% per °C, and most preferably less than about 0.15% per °C.
  • the maximum rate of mass loss can be measured as follows. 1.9 grams of lithium metal oxide is mixed with 0.1 grams of carbon black (Shawinigan Black, Chevron) to form a cathode sample. 50 to 100 milligrams of the cathode sample is pressed into an aluminum coin cell can (2430 size) having an aluminum mesh attached to it and dried under vacuum for about four hours at about 150°C. An excess of lithium metal (anode sample) is pressed onto the other half of the aluminum coin cell can. Once the cathode is dried, both the cathode sample and the anode sample are immediately placed into an argon atmosphere drybox.
  • One layer of separator material (Asahi) is placed on the cathode sample, and one layer of polypropylene oxide (Pellon) is placed on the anode sample.
  • Both the cathode sample and the anode sample are soaked with a solution of one molar LiPF 6 in ethylene carbonate and dimethyl carbonate (50:50 by volume), assembled together with a plastic grommet to prevent shorting, and crimped.
  • the coin cell is then charged at about 0.2 milliamps to about 4.8 volts until full delithiation occurred.
  • the charged cell is pumped in the drybox and disassembled in the drybox without shorting the cell.
  • the aluminum mesh is pried away from the can and the cathode sample is washed into a centrifuge tube using dimethyl carbonate.
  • the cathode sample is then washed with excess dimethyl carbonate and allowed to settle in the centrifuge tube. Most of the dimethyl carbonate is decanted, and the cathode sample is dried under vacuum at room temperature overnight. The dried sample is placed in a thermal gravimetry analysis (TGA) instrument (TA Instruments model 2950) under an argon atmosphere, and the rate of mass loss is measured as the sample is heated at a rate of about 10°C per minute to a temperature of about 500°C.
  • TGA thermal gravimetry analysis
  • the lithium metal oxide material can be made by combining and heating a nickel precursor, a cobalt precursor, a lithium precursor and a halogen precursor.
  • the precursors can be ground in a mortar and pestle to form a homogenized mixture and heated in a furnace.
  • the peak temperature used when heating the combined precursors can be, for example, from about 600°C to about 800°C. Preferably, the peak temperature is from about 650°C to about 720°C.
  • the nickel precursor can be any material which, upon being heated to at least about 600°C, readily decomposes to provide nickel atoms that can be incorporated into the lithium metal oxide material.
  • Nickel precursors include nickel hydroxide, spherical nickel hydroxide, nickel carbonate, nickel oxide and nickel acetate.
  • the nickel precursor is spherical nickel hydroxide.
  • the lithium precursor can be any material which, upon being heated to at least about 600°C, readily decomposes to provide lithium atoms that can be incorporated into the lithium metal oxide material.
  • Lithium precursors include lithium carbonate, lithium hydroxide, lithium acetate and lithium oxalate.
  • the lithium precursor is lithium hydroxide.
  • the cobalt precursor can be any material which, upon being heated to at least about 600°C, readily decomposes to provide cobalt atoms that can be incorporated into the lithium metal oxide material.
  • Cobalt precursors include CoO 4 , C0 3 O 4 , Co 2 O 3 , CoO, cobalt carbonate and cobalt acetate.
  • the cobalt precursor is Co 3 O 4 .
  • the halogen precursor can be any material which, upon being heated to at least about 600°C, readily decomposes to provide halogen atoms that can be incorporated into the lithium metal oxide material.
  • Halogen precursors include lithium fluoride, nickel fluoride, cobalt fluoride, ammonium fluoride, fluorine gas, lithium chloride, nickel chloride, cobalt chloride, ammonium chloride, chlorine gas, lithium bromide, nickel bromide, cobalt bromide, ammonium bromide, lithium iodide, nickel iodide, cobalt iodide, and ammonium iodide.
  • the halogen precursor is nickel fluoride.
  • the lithium metal oxide has the empirical formula Li ⁇ M v M', .y O 2 A z
  • the lithium metal oxide can be formed by flowing fluorine gas over material having the empirical formula Li ⁇ M M',. y O 2 at temperature of at least about 600°C, preferably from about 600°C to about 800°C.
  • Anode 12 can include any materials suitable for use in the anode of a lithium ion battery.
  • anode 12 can be formed of a highly porous sintered, felt, or foam substrate having a coating of anode material thereon.
  • the anode material can be formed of an active material and a binder.
  • the binder can be, for example, a polymeric binder.
  • the active anode material can include lithium, carbon, graphite, acetylenic mesophase carbons, coke, polyacenic semiconductors, metal oxides, and lithiated metal oxides having an electrochemical potential that is greater than the electrochemical potential of the cathode.
  • Separator 20 can be formed of any of the standard separator materials used in lithium ion batteries.
  • separator 20 can be formed of polypropylene, polyethylene, a polyamide (e.g., a nylon), a polysulfone and/or a poly vinyl chloride.
  • Separator 20 preferably has a thickness of from about 0.1 millimeters to about 2 millimeters, and more preferably from about 0.2 millimeters to about 0.5 millimeters.
  • Separator 20 can be cut into pieces of a similar size as anode 12 and cathode 16 and placed therebetween as shown in the figure.
  • Anode 12, cathode 16 and separator 20 can then be placed within case 22 which can be made of a metal such as nickel or nickel plated steel, or a plastic such as polyvinyl chloride, polypropylene, a polysulfone, ABS or a polyamide.
  • battery 10 can also be used, including the coin cell configuration or the classic (Leclanche) configuration.
  • Case 22 containing anode 12, cathode 16 and separator 20 can be filled with the electrolyte, which can be any electrolyte appropriate for use in lithium ion batteries.
  • the electrolyte includes one or more solvents and one or more lithium salts.
  • Solvents include ethylene carbonate, propylene carbonate, dimethyl carbonate, ethylmethyl carbonate diethyl ether, dimethyl ether, methyl propionate, ethyl propionate, methyl butryate, gamma butyrolactone, dimethoxy ethane, diethoxy ethane, triethyl phosphate and trimethyl phosphate.
  • Lithium salts include LiPF 6 , LiAsF 6 , Lil, LiBr, LiBF 4 , LiAlCl 4 , LiClO 4 and LiCFSO 3 .
  • the electrolyte is a 1 molar solution of LiPF 6 in a 50:50 mixture (by volume) of ethylene carbonate and dimethyl carbonate.
  • cap 24 After disposing the electrolyte in can 22, it can be sealed with cap 24 and annular insulating gasket 26.
  • Example I About 29.478 grams of LiOH»H 2 O (available from Alfa Aesar, located in Ward Hill, MA), about 51.530 grams of spherical Ni(OH) 2 (available from Tanaka Chemicals, located in Osaka, Japan), about 2.822 grams of NiF 2 »4H 2 O (available from Alfa Aesar) and about 10.742 grams of Co 3 O 4 (available from Alfa Aesar) were mixed and ground using a mortar and pestle.
  • the reactants were put into alumina crucibles and placed in a tube furnace.
  • the reactants were heated to about 700°C over about three hours, kept at a temperature of about 700°C for about eight hours, and ambiently cooled to room temperature.
  • the reaction mixture was removed from the furnace, reground in a mortar and pestle, and placed back into the furnace.
  • the mixture was heated to about 700°C over about three hours, kept at a temperature of about 700°C for about eight hours, cooled to about 300°C over about eight hours, and then ambiently cooled to room temperature. This yielded about 31.93 grams of material having the empirical formula Li, 05 Ni 08 Co 02 O, 95 F 005 .
  • Example II About 14.739 grams of LiOH «H 2 0 (Alfa Aesar), about 24.825 grams of spherical Ni(OH) 2 (Tanaka), and about 5.371 grams of Co 3 O 4 (Alfa Aesar) were weighed mixed and ground using a mortar and pestle.

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  • Chemical & Material Sciences (AREA)
  • Inorganic Chemistry (AREA)
  • Chemical Kinetics & Catalysis (AREA)
  • Electrochemistry (AREA)
  • General Chemical & Material Sciences (AREA)
  • Crystallography & Structural Chemistry (AREA)
  • Battery Electrode And Active Subsutance (AREA)
  • Secondary Cells (AREA)

Abstract

L'invention concerne des matériaux représentés par la formule empirique LixMyM'1-yO2-zAz. M et M' sont des métaux différents, et A est un halogène. x peut prendre une valeur comprise entre 0,9 environ et 1,2 environ. y peut prendre une valeur supérieure à zéro et inférieure à 1, et z peut prendre une valeur supérieure à zéro et inférieure à deux. La répartition des atomes de fluor peut être sensiblement uniforme dans toute la section transversale des matériaux. Ces matériaux peuvent être utilisés dans des cathodes (16) de batteries au lithium.
PCT/US1999/010556 1998-05-15 1999-05-13 Materiaux pour cathodes de batterie WO1999060638A2 (fr)

Priority Applications (1)

Application Number Priority Date Filing Date Title
AU39874/99A AU3987499A (en) 1998-05-15 1999-05-13 Battery cathode materials

Applications Claiming Priority (2)

Application Number Priority Date Filing Date Title
US7994798A 1998-05-15 1998-05-15
US09/079,947 1998-05-15

Publications (2)

Publication Number Publication Date
WO1999060638A2 true WO1999060638A2 (fr) 1999-11-25
WO1999060638A3 WO1999060638A3 (fr) 2000-04-06

Family

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Application Number Title Priority Date Filing Date
PCT/US1999/010556 WO1999060638A2 (fr) 1998-05-15 1999-05-13 Materiaux pour cathodes de batterie

Country Status (3)

Country Link
AU (1) AU3987499A (fr)
TW (1) TW442993B (fr)
WO (1) WO1999060638A2 (fr)

Cited By (15)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
WO2007049215A1 (fr) * 2005-10-26 2007-05-03 The Gillette Company Cathodes pour batteries
WO2012039893A2 (fr) 2010-09-22 2012-03-29 Envia Systems, Inc. Revêtements d'halogénure de métal sur des matériaux électrode positive de batterie lithium-ion et batteries correspondantes
WO2012061191A3 (fr) * 2010-11-02 2012-07-12 Envia Systems, Inc. Batteries lithium-ion avec lithium supplémentaire
US8389160B2 (en) 2008-10-07 2013-03-05 Envia Systems, Inc. Positive electrode materials for lithium ion batteries having a high specific discharge capacity and processes for the synthesis of these materials
US8475959B2 (en) 2009-08-27 2013-07-02 Envia Systems, Inc. Lithium doped cathode material
US8535832B2 (en) 2009-08-27 2013-09-17 Envia Systems, Inc. Metal oxide coated positive electrode materials for lithium-based batteries
US8741484B2 (en) 2010-04-02 2014-06-03 Envia Systems, Inc. Doped positive electrode active materials and lithium ion secondary battery constructed therefrom
US8928286B2 (en) 2010-09-03 2015-01-06 Envia Systems, Inc. Very long cycling of lithium ion batteries with lithium rich cathode materials
US9070489B2 (en) 2012-02-07 2015-06-30 Envia Systems, Inc. Mixed phase lithium metal oxide compositions with desirable battery performance
US9552901B2 (en) 2012-08-17 2017-01-24 Envia Systems, Inc. Lithium ion batteries with high energy density, excellent cycling capability and low internal impedance
US9843041B2 (en) 2009-11-11 2017-12-12 Zenlabs Energy, Inc. Coated positive electrode materials for lithium ion batteries
US9960424B2 (en) 2008-12-11 2018-05-01 Zenlabs Energy, Inc. Positive electrode materials for high discharge capacity lithium ion batteries
WO2018187531A1 (fr) * 2017-04-07 2018-10-11 The Regents Of The University Of California Oxydes métalliques de lithium à désordre cationique et substitution fluor et procédés de fabrication associés
US10115962B2 (en) 2012-12-20 2018-10-30 Envia Systems, Inc. High capacity cathode material with stabilizing nanocoatings
US10170762B2 (en) 2011-12-12 2019-01-01 Zenlabs Energy, Inc. Lithium metal oxides with multiple phases and stable high energy electrochemical cycling

Family Cites Families (5)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
JPH06243871A (ja) * 1993-02-16 1994-09-02 Sanyo Electric Co Ltd 非水系二次電池
US5773168A (en) * 1995-08-23 1998-06-30 Kabushiki Kaisha Toshiba Nonaqueous electrolyte secondary battery and method for manufacturing the same
CA2163695C (fr) * 1995-11-24 2000-08-01 Qiming Zhong Methode de preparation de li1+xmn2-x-ymyo4 pour des piles au lithium
US5674645A (en) * 1996-09-06 1997-10-07 Bell Communications Research, Inc. Lithium manganese oxy-fluorides for li-ion rechargeable battery electrodes
US5759720A (en) * 1997-06-04 1998-06-02 Bell Communications Research, Inc. Lithium aluminum manganese oxy-fluorides for Li-ion rechargeable battery electrodes

Cited By (26)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
JP2009512992A (ja) * 2005-10-26 2009-03-26 ザ ジレット カンパニー 電池カソード
US7858230B2 (en) 2005-10-26 2010-12-28 The Gillette Company Battery cathodes
WO2007049215A1 (fr) * 2005-10-26 2007-05-03 The Gillette Company Cathodes pour batteries
US8257863B2 (en) 2005-10-26 2012-09-04 The Gillette Company Method of making electrode
US8389160B2 (en) 2008-10-07 2013-03-05 Envia Systems, Inc. Positive electrode materials for lithium ion batteries having a high specific discharge capacity and processes for the synthesis of these materials
US9960424B2 (en) 2008-12-11 2018-05-01 Zenlabs Energy, Inc. Positive electrode materials for high discharge capacity lithium ion batteries
US8741485B2 (en) 2009-08-27 2014-06-03 Envia Systems, Inc. Layer-layer lithium rich complex metal oxides with high specific capacity and excellent cycling
US8475959B2 (en) 2009-08-27 2013-07-02 Envia Systems, Inc. Lithium doped cathode material
US8535832B2 (en) 2009-08-27 2013-09-17 Envia Systems, Inc. Metal oxide coated positive electrode materials for lithium-based batteries
US9843041B2 (en) 2009-11-11 2017-12-12 Zenlabs Energy, Inc. Coated positive electrode materials for lithium ion batteries
US8741484B2 (en) 2010-04-02 2014-06-03 Envia Systems, Inc. Doped positive electrode active materials and lithium ion secondary battery constructed therefrom
US8928286B2 (en) 2010-09-03 2015-01-06 Envia Systems, Inc. Very long cycling of lithium ion batteries with lithium rich cathode materials
WO2012039893A2 (fr) 2010-09-22 2012-03-29 Envia Systems, Inc. Revêtements d'halogénure de métal sur des matériaux électrode positive de batterie lithium-ion et batteries correspondantes
US8663849B2 (en) 2010-09-22 2014-03-04 Envia Systems, Inc. Metal halide coatings on lithium ion battery positive electrode materials and corresponding batteries
EP3285315A1 (fr) 2010-09-22 2018-02-21 Zenlabs Energy, Inc. Revêtements d'halogénure métallique sur des matériaux à électrode positive de batterie au lithium-ion et batterie correspondante
US9166222B2 (en) 2010-11-02 2015-10-20 Envia Systems, Inc. Lithium ion batteries with supplemental lithium
WO2012061191A3 (fr) * 2010-11-02 2012-07-12 Envia Systems, Inc. Batteries lithium-ion avec lithium supplémentaire
US9923195B2 (en) 2010-11-02 2018-03-20 Zenlabs Energy, Inc. Lithium ion batteries with supplemental lithium
CN103190026A (zh) * 2010-11-02 2013-07-03 安维亚系统公司 具有额外锂的锂离子电池
US11380883B2 (en) 2010-11-02 2022-07-05 Zenlabs Energy, Inc. Method of forming negative electrode active material, with lithium preloading
US10170762B2 (en) 2011-12-12 2019-01-01 Zenlabs Energy, Inc. Lithium metal oxides with multiple phases and stable high energy electrochemical cycling
US9070489B2 (en) 2012-02-07 2015-06-30 Envia Systems, Inc. Mixed phase lithium metal oxide compositions with desirable battery performance
US9552901B2 (en) 2012-08-17 2017-01-24 Envia Systems, Inc. Lithium ion batteries with high energy density, excellent cycling capability and low internal impedance
US10115962B2 (en) 2012-12-20 2018-10-30 Envia Systems, Inc. High capacity cathode material with stabilizing nanocoatings
WO2018187531A1 (fr) * 2017-04-07 2018-10-11 The Regents Of The University Of California Oxydes métalliques de lithium à désordre cationique et substitution fluor et procédés de fabrication associés
US12278365B2 (en) 2017-04-07 2025-04-15 The Regents Of The University Of California Fluorine substituted cation-disordered lithium metal oxides and methods of making same

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Publication number Publication date
WO1999060638A3 (fr) 2000-04-06
TW442993B (en) 2001-06-23
AU3987499A (en) 1999-12-06

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