WO2002089234A1 - Improved cathode compositions for lithium-ion batteries - Google Patents

Improved cathode compositions for lithium-ion batteries Download PDF

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Publication number
WO2002089234A1
WO2002089234A1 PCT/US2002/007251 US0207251W WO02089234A1 WO 2002089234 A1 WO2002089234 A1 WO 2002089234A1 US 0207251 W US0207251 W US 0207251W WO 02089234 A1 WO02089234 A1 WO 02089234A1
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cathode
lithium
examples
cathode composition
composition according
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English (en)
French (fr)
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Zhonghua Lu
Jeffrey R. Dahn
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3M Innovative Properties Co
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3M Innovative Properties Co
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Priority to DE60233219T priority Critical patent/DE60233219D1/de
Priority to KR10-2003-7013935A priority patent/KR20040015142A/ko
Priority to AT02719184T priority patent/ATE438934T1/de
Priority to HK04105217.2A priority patent/HK1063381B/en
Priority to KR1020137023557A priority patent/KR20130103830A/ko
Application filed by 3M Innovative Properties Co filed Critical 3M Innovative Properties Co
Priority to JP2002586424A priority patent/JP4544821B2/ja
Priority to EP02719184A priority patent/EP1390994B1/en
Priority to KR1020147033121A priority patent/KR20150002881A/ko
Publication of WO2002089234A1 publication Critical patent/WO2002089234A1/en
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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
    • H01M4/36—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
    • H01M4/485—Selection of substances as active materials, active masses, active liquids of inorganic oxides or hydroxides of mixed oxides or hydroxides for inserting or intercalating light metals, e.g. LiTi2O4 or LiTi2OxFy
    • 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
    • H01M4/52—Selection of substances as active materials, active masses, active liquids of inorganic oxides or hydroxides of nickel, cobalt or iron
    • H01M4/525—Selection of substances as active materials, active masses, active liquids of inorganic oxides or hydroxides of nickel, cobalt or iron of mixed oxides or hydroxides containing iron, cobalt or nickel for inserting or intercalating light metals, e.g. LiNiO2, LiCoO2 or LiCoOxFy
    • 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
    • H01M10/0525—Rocking-chair batteries, i.e. batteries with lithium insertion or intercalation in both electrodes; Lithium-ion batteries
    • 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
    • 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
    • H01M2004/026—Electrodes composed of, or comprising, active material characterised by the polarity
    • H01M2004/028—Positive electrodes
    • 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

  • TECHNICAL FIELD This invention relates to preparing compositions useful as cathodes for lithium-ion batteries.
  • Lithium-ion batteries typically include an anode, an electrolyte, and a cathode that contains lithium in the form of a lithium-transition metal oxide.
  • transition metal oxides that have been used include cobalt dioxide, nickel dioxide, and manganese dioxide. None of these materials, however, exhibits an optimal combination of high initial capacity, high thermal stability, and good capacity retention after repeated charge- discharge cycling.
  • the invention features a cathode composition for a lithium-ion battery having the formula Li[M 1 (1 . x) Mn x ]O 2 where 0 ⁇ x ⁇ 1 and M 1 represents one or more metal elements, with the proviso that M 1 is a metal element other than chromium.
  • the composition is in the form of a single phase having an 03 crystal structure that does not undergo a phase transformation to a spinel crystal structure when incorporated in a lithium-ion battery and cycled for 100 full charge-discharge cycles at 30°C and a final capacity of 130 mAh/g using a discharge current of 30 mA/g.
  • the invention also features lithium-ion batteries incorporating these cathode compositions in combination with an anode and an electrolyte.
  • the resulting cathode composition has the formula Li[Li (1-2y y 3 M y Mn (2 _ y)/3 ]O 2 .
  • the resulting cathode composition has the formula Li[Li (1-y y 3 M 3 y Mn (2-
  • the resulting cathode composition has the formula Li[M y M 5 1-2y Mn y ]O 2 .
  • the invention provides cathode compositions, and lithium-ion batteries incorporating these compositions, that exhibit high initial capacities and good capacity retention after repeated charge-discharge cycling.
  • the cathode compositions do not evolve substantial amounts of heat during elevated temperature abuse, thereby improving battery safety.
  • FIG. 1 is an exploded perspective view of an electrochemical cell used to test various electrode compositions.
  • FIGS. 2(a)-(e) are plots of voltage versus' capacity and capacity versus cycle number for the samples described in Examples 1 and 3-6 cycled between 4.4 V and 3.0 V.
  • FIGS. 3(a)-(e) are plots of voltage versus capacity and capacity versus cycle number for the samples described in Examples 1 and 3-6 cycled between 4.8 V and 2.0 V.
  • FIGS. 4(a)-(d) are x-ray diffraction patterns for the samples described in Examples 3 and 7-9.
  • FIGS. 5(a)-(d) are x-ray diffraction patterns for the samples described in Examples 5 and 10-12.
  • FIGS. 6(a)-(d) are x-ray diffraction patterns for the samples described in Examples 6 and 16-18.
  • FIGS. 7(a)-(d) are plots of voltage versus capacity and capacity versus cycle number for the samples described in Examples 6 and 16-18 cycled between 4.4 V and 3.0 V.
  • FIGS. 8(a)-(d) are plots of voltage versus capacity and capacity versus cycle number for the samples described in Examples 6 and 16-18 cycled between 4.8 V and 2.0 V.
  • FIGS. 9(a)-(b) are plots of voltage versus capacity for the samples described in Examples 19 and 20.
  • FIG. 10 is a plot of capacity versus cycle number for the sample described in Example
  • Fig. 11 is a plot of capacity versus cycle number for the sample described in Example
  • Fig. 12 is a plot of capacity versus cycle number for the sample described in Example
  • Fig. 13 is a plot of capacity versus discharge current density for the sample described in Example 1 measured at 30°C to a 2.5 V cutoff.
  • the cathode compositions preferably adopt an O3 crystal structure featuring layers generally arranged in the sequence lithium-oxygen-metal-oxygen-lithium. This crystal structure is retained when the cathode composition is incorporated in a lithium-ion battery and cycled for 100 full charge-discharge cycles at 30°C and a final capacity of 130 mAh/g using a discharge current of 30 mA/g, rather than transforming into a spinel-type crystal structure under these conditions.
  • the metal elements in the lithium layers. It is further preferred that at least one of the metal elements be oxidizable within the electrochemical window of the electrolyte incorporated in the battery.
  • the cathode compositions may be synthesized by jet milling or by combining precursors of the metal elements (e.g., hydroxides, nitrates, and the like), followed by heating to generate the cathode composition. Heating is preferably conducted in air at temperatures of at least about 600°C, more preferably at least 800°C. In general, higher temperatures are preferred because they lead to materials with increased crystallinity. The ability to conduct the heating process in air is desirable because it obviates the need and associated expense of maintaining an inert atmosphere. Accordingly, the particular metal elements are selected such that they exhibit appropriate oxidation states in air at the desired synthesis temperature.
  • precursors of the metal elements e.g., hydroxides, nitrates, and the like
  • the synthesis temperature may be adjusted so that a particular metal element exists in a desired oxidation state in air at that temperature.
  • suitable metal elements for inclusion in the cathode composition include Ni, Co, Fe, Cu, Li, Zn, V, and combinations thereof.
  • Particularly preferred cathode compositions are those having the following formulae:
  • the cathode compositions are combined with an anode and an electrolyte to form a lithium-ion battery.
  • suitable anodes include lithium metal, graphite, and lithium alloy compositions, e.g., of the type described in Turner, U.S. 6,203,944 entitled “Electrode for a Lithium Battery” and Turner, WO 00/03444 entitled “Electrode Material and Compositions.”
  • the electrolyte may be liquid or solid.
  • solid electrolytes include polymeric electrolytes such as polyethylene oxide, polytetrafluoroethylene, fluorine-containing copolymers, and combinations thereof.
  • liquid electrolytes examples include ethylene carbonate, diethyl carbonate, propylene carbonate, and combinations thereof.
  • the electrolyte is provided with a lithium electrolyte salt.
  • suitable salts include LiPF 6 , LiBF , and LiClO .
  • Electrodes were prepared as follows. About 21 wt. % active cathode material (prepared as described below), 5.3 wt. % Kynar Flex 2801 (a vinylidene fluoride- hexafluoropropylene copolymer commercially available from Atochem), 8.4 wt. % dibutyl phthalate, 2.1 wt. % Super S carbon black (commercially available from MMM Carbon, Belgium), and 63.2 * wt. % acetone were mechanically shaken for 1-2 hours in a mixing vial to which a zirconia bead (8 mm diameter) had been added to form a uniform slurry.
  • the slurry was then spread in a thin layer (about 150 micrometers thick) on a glass plate using a notch-bar spreader. After evaporating the acetone, the resulting film was peeled from the glass and a circular electrode measuring 1.3 cm in diameter was punched from the film using an electrode punch, after which the electrode was soaked in diethyl ether for about 10 minutes to remove dibutyl phthalate and to form pores in the electrode. The ether rinse was repeated two times. The electrodes were then dried at 90°C overnight. At the conclusion of the drying period, the circular electrode was weighed and the active mass (the total weight of the circular electrode multiplied by the fraction of the electrode weight made up of the active cathode material) determined. Typically, the electrodes contained 74% by weight active material. The electrodes were then taken into an argon- filled glove box where the electrochemical cell was constructed.
  • FIG. 1 An exploded perspective view of the electrochemical cell 10 is shown in FIG. 1.
  • a stainless steel cap 24 and special oxidation resistant case 26 contain the cell and serve as the negative and positive terminals respectively.
  • the cathode 12 was the electrode prepared as described above.
  • the anode 14 was a lithium foil having a thickness of 125 micrometers; the anode also functioned as a reference electrode.
  • the cell featured 2325 coin-cell hardware, equipped with a spacer plate 18 (304 stainless steel) and a disc spring 16 (mild steel). The disc spring was selected so that a pressure of about 15 bar would be applied to each of the cell electrodes when the cell was crimped closed.
  • the separator 20 was a Celgard #2502 microporous polypropylene film (Hoechst-Celanese), which had been wetted with a IM solution of LiPF 6 dissolved in a 30:70 volume mixture of ethylene carbonate and diethyl carbonate (Mitsubishi Chemical).
  • a gasket 27 was used as a seal and to separate the two terminals.
  • each sample was accurately weighed on a microbalance (to 1 ⁇ g) into a 50 mL glass class A volumetric flask. 2 mL hydrochloric acid and 1 mL nitric acid were then added to form a salt. Once the salt had dissolved, the solution was diluted to 50 mL with deionized water and the solution shaken to mix. This solution was diluted further 10 times. Next, a 5 mL aliquot was removed with a glass class A volumetric pipet and diluted to 50 mL in a glass class A volumetric flask with 4 % HC1 and 2 % nitric acid.
  • the diluted solution were analyzed on a Jarrell-Ash 6 IE ICP using standards of 0, 1, 3, 10, and 20 ppm Co, Ni, Mn, Li, and Na in 4 % HC1 / 2% HNO3.
  • a 5 ppm standard of each element was used to monitor the stabilityof the calibration. All standards were prepared from a certified stock solution and with class A volumetric glassware. Prior to analysis of the elements, the injector tube of the ICP was cleaned to remove any deposits. All element calibration curves exhibited r 2 values in excess of 0.9999. The analytical results were measured in weight percent. These values were then converted to atomic percent and then ultimately to a stoichiometry where the oxygen content had been normalized to a stoichiometry of 2.
  • the pellets were heated in air at 480°C for 3 hours, after which they were quenched to room temperature, combined, and re-ground into powder. New pellets were pressed and heated in air to 900°C for 3 hours. At the conclusion of the heating step, the pellets were quenched to room temperature and again ground to powder to yield the cathode material.
  • Elemental analysis of the cathode material revealed that the composition had the following stoichiometry: Li[Lio . o 6 io. 3 3 Mno. 5 i]O 2, which is in close agreement with the target stoichiometry of Li[Li 0 .o6Nio. 42 Mn 0.53 ]O 2.
  • a powder x-ray diffraction pattern for each sample was collected using a Siemens D5000 diffractometer equipped with a copper target X-ray tube and a diffracted beam monochromator. Data was collected between scattering angles of 10 degrees and 130 degrees.
  • the crystal structure of each sample was determined based upon the x-ray diffraction data as described in (a) C. J. Howard and R. J. Hill, Australian Atomic Energy Commission Report No. Ml 12 (1986); and (b) D. B. Wiles and R. A. Young, J. Appl. Cryst., 14:149-151 (1981).
  • Lattice parameters were determined using the Rietveld refinement. The lattice parameters for each sample are reported in Table 1. The crystal structure of each sample could be described well by the O3 crystal structure type.
  • Electrochemical cells were constructed according to the above-described procedure using the material of Examples 1 and 3-6 as the cathode. Each cell was charged and discharged between 4.4 V and 3.0 V at 30°C using computer-controlled discharge stations from Moli Energy Ltd. (Maple Ridge, B.C., Canada) and a current of 10 mA/g of active material.
  • Fig. 3 is a plot of voltage versus capacity and capacity versus cycle number for each cell.
  • Example 1 shows an irreversible capacity of only about 15 mAh/g and a reversible capacity of about 230 mAh/g.
  • HAT refers to the heat treatment temperature
  • "a” and "c” represent lattice parameters.
  • An asterisk means "not tested.”
  • Example 1 Another electrochemical cell was assembled using the material of Example 1 and cycled between 3.0 V and 4.4 V using a current of 30 mA/g. Some cycles were collected at 30°C, while other cycles were collected at 55°C. The results are reported in Fig. 12. The capacity of the material was maintained even at 55°C after extended cycling, demonstrating that the material did not exhibit phase separation after extended cycling.
  • X-ray diffraction patterns for each sample were collected and are shown in Fig. 3, along with an x-ray diffraction pattern for Example 3 prepared at 900°C.
  • the lattice parameters were also determined and are set forth in Table 2, along with the data for Example 3. The data demonstrate that as the heating temperature increases, the peak widths in the diffraction patterns become narrower, indicating increased crystallinity. All peaks can be understood based on the 03 crystal structure.
  • HAT refers to the heat treatment temperature
  • "a” and "c” represent lattice parameters.
  • X-ray diffraction patterns for each sample were collected and are shown in Fig. 4, along with an x-ray diffraction pattern for Example 5 prepared at 900°C.
  • the lattice parameters were also determined and are set forth in Table 3, along with the data for Example 5. The data demonstrate that as the heating temperature increases, the peak widths in the diffraction patterns become narrower, indicating increased crystallinity. All peaks can be understood based on the 03 crystal structure.
  • Electrochemical cells were constructed using material from Examples 10 and 12 as the cathode, as cycled as described above. The reversible and irreversible capacities are also reported in Table 3, along with data for Example 5. All samples performed well. TABLE 3
  • HAT refers to the heat treatment temperature
  • "a” and "c” represent lattice parameters.
  • An asterisk means "not tested.”
  • HAT refers to the heat treatment temperature
  • "a” and “c” represent lattice parameters. Examples 16-18
  • X-ray diffraction patterns for each sample were collected and are shown in Fig. 6, along with an x-ray diffraction pattern for Example 6 prepared at 900°C.
  • the lattice parameters were also determined and are set forth in Table 5, along with the data for Example 6. The data demonstrate that as the. heating temperature increases, the peak widths in the diffraction patterns become narrower, indicating increased crystallinity. All peaks can be understood based on the 03 crystal structure.
  • Electrochemical cells were constructed using material from Examples 16-18 as the cathode, as cycled as described above.
  • the reversible and irreversible capacities are also reported in Table 5, along with data for Example 6.
  • Fig. 7 reports voltage versus capacity and capacity versus cycle number for each cell, as well as a cell constructed using Example 6, when cycled between 4.4 V and 3.0 V.
  • Fig. 8 reports voltage versus capacity and capacity versus cycle number for each cell, as well as a cell constructed using Example 6, when cycled between 4.8 V and 2.0 V. All samples performed well, with samples prepared at higher temperatures exhibiting the best capacity retention and lowest irreversible capacity.
  • HAT refers to the heat treatment temperature
  • "a” and “c” represent lattice parameters. Examples 19-20
  • the procedure described in Examples 1-6 was followed except that the following reactants were used: 10.918 g of Ni(NO 3 ) 2 -6H 2 O, 9.420 g of Mn(NO 3 ) 2 -4H 2 O, and 7.280 g of Co(NO 3 ) 2 -6H 2 O.
  • the dried transition metal hydroxide was mixed with
  • Elemental analysis of the material revealed that the composition had the following stoichiometry: Li 1 .o 3 [Nio .2 3 Coo. 51 Mno. 25 ]O 2i which is in close agreement with the target stoichiometry of Li[Ni 0.25 Coo. 5 Mno. 5 ]O 2 .
  • Electrochemical cells were constructed using material from Examples 19-20 as the cathode, as cycled as described above.
  • Fig. 9 reports voltage versus capacity for each cell when cycled between 2.5 V and 4.8 V. Both samples performed well.
  • a second set of electrochemical cells was constructed using material from Examples 19- 20 and cycled as described above between 2.5 V and 4.4 V using a current of 40 mA/g.
  • the cathode material from Example 19 was further analyzed using differential scanning calorimetry (DSC).
  • the sample cell was a 3.14 mm outer diameter, type 304 stainless steel seamless tube having a wall thickness of 0.015 mm that had been cut into an 8.8 mm long piece (MicroGroup, Medway, MA).
  • the cell was cleaned, after which one end was flattened. The flattened end was then welded shut by tungsten inert gas welding using a Miller Maxstar 91 ARC welder equipped with a Snap Start II high frequency ARC starter.
  • the tube was loaded in an argon-filled glove box with 2 mg of the cathode material from Example 19 taken from a 2325 coin cell that had been charged to 4.2 V using the procedure described above. The electrolyte was not removed from the cathode sample. After the sample was loaded, the tube was crimped and welded shut.
  • the DSC measurements were performed using a TA Instruments DSC 910 instrument.
  • the DSC sweep rate was 2°C/minute. Both the onset temperature and the total heat evolved were recorded. The onset temperature corresponds to the temperature at which the first major exothermic peak occurs.
  • the results are shown in Table 6.
  • data from cathodes prepared using LiNiO and LiCoO 2 is included as well. The results demonstrate that cathodes prepared using the material from Example 19 exhibited a higher onset temperature and evolved less heat than cathodes prepared using LiNiO 2 and LiCoO 2 .

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PCT/US2002/007251 2001-04-27 2002-03-11 Improved cathode compositions for lithium-ion batteries Ceased WO2002089234A1 (en)

Priority Applications (8)

Application Number Priority Date Filing Date Title
KR1020147033121A KR20150002881A (ko) 2001-04-27 2002-03-11 리튬 이온 배터리용 개선된 캐쏘드 조성물
KR10-2003-7013935A KR20040015142A (ko) 2001-04-27 2002-03-11 리튬 이온 배터리용 개선된 캐쏘드 조성물
AT02719184T ATE438934T1 (de) 2001-04-27 2002-03-11 Verbesserte kathodenzusammensetzungen für lithiumionenbatterien
HK04105217.2A HK1063381B (en) 2001-04-27 2002-03-11 Improved cathode compositions for lithium-ion batteries
KR1020137023557A KR20130103830A (ko) 2001-04-27 2002-03-11 리튬 이온 배터리용 개선된 캐쏘드 조성물
DE60233219T DE60233219D1 (de) 2001-04-27 2002-03-11 Verbesserte kathodenzusammensetzungen für lithiumionenbatterien
JP2002586424A JP4544821B2 (ja) 2001-04-27 2002-03-11 リチウムイオン電池用の改善されたカソード組成物
EP02719184A EP1390994B1 (en) 2001-04-27 2002-03-11 Improved cathode compositions for lithium-ion batteries

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Application Number Priority Date Filing Date Title
US09/845,178 2001-04-27
US09/845,178 US6964828B2 (en) 2001-04-27 2001-04-27 Cathode compositions for lithium-ion batteries

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CN (2) CN100403585C (https=)
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JP2004006267A (ja) * 2002-03-25 2004-01-08 Sumitomo Chem Co Ltd 非水二次電池用正極活物質の製造方法
WO2003015198A3 (en) * 2001-08-07 2004-04-01 3M Innovative Properties Co Cathode compositions for lithium ion batteries
WO2004084330A3 (en) * 2003-03-14 2005-10-20 3M Innovative Properties Co Method of producing lithium ion cathode materials
US7211237B2 (en) 2003-11-26 2007-05-01 3M Innovative Properties Company Solid state synthesis of lithium ion battery cathode material
US8241791B2 (en) 2001-04-27 2012-08-14 3M Innovative Properties Company Cathode compositions for lithium-ion batteries
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US9017841B2 (en) 2005-08-19 2015-04-28 Lg Chem, Ltd. Electrochemical device with high capacity and method for preparing the same

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KR100628797B1 (ko) * 2000-11-16 2006-09-26 히다치 막셀 가부시키가이샤 리튬 함유 복합 산화물을 포함하는 양극 활물질
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JP4510331B2 (ja) * 2001-06-27 2010-07-21 パナソニック株式会社 非水電解質二次電池
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JP4836371B2 (ja) * 2001-09-13 2011-12-14 パナソニック株式会社 正極活物質およびこれを含む非水電解質二次電池
JP3827545B2 (ja) * 2001-09-13 2006-09-27 松下電器産業株式会社 正極活物質、その製造方法および非水電解質二次電池
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