WO2008107571A2 - Silicates mixtes de lithium. - Google Patents
Silicates mixtes de lithium. Download PDFInfo
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- WO2008107571A2 WO2008107571A2 PCT/FR2008/000148 FR2008000148W WO2008107571A2 WO 2008107571 A2 WO2008107571 A2 WO 2008107571A2 FR 2008000148 W FR2008000148 W FR 2008000148W WO 2008107571 A2 WO2008107571 A2 WO 2008107571A2
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- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
- C01B33/00—Silicon; Compounds thereof
- C01B33/20—Silicates
- C01B33/32—Alkali metal silicates
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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
- H01M10/00—Secondary cells; Manufacture thereof
- H01M10/05—Accumulators with non-aqueous electrolyte
- H01M10/052—Li-accumulators
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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
- H01M4/13—Electrodes for accumulators with non-aqueous electrolyte, e.g. for lithium-accumulators; Processes of manufacture thereof
- H01M4/131—Electrodes based on mixed oxides or hydroxides, or on mixtures of oxides or hydroxides, e.g. LiCoOx
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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
- H01M4/13—Electrodes for accumulators with non-aqueous electrolyte, e.g. for lithium-accumulators; Processes of manufacture thereof
- H01M4/139—Processes of manufacture
- H01M4/1391—Processes of manufacture of electrodes based on mixed oxides or hydroxides, or on mixtures of oxides or hydroxides, e.g. LiCoOx
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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
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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
- H01M4/50—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
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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
- H01M4/52—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
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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
- 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
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- 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
- the present invention relates to mixed lithium silicates, their preparation and their use as electrode active material.
- EP-I 134 826 describes the preparation of mixed silicates by a process consisting in mixing the solid precursors of the silicate, in stoichiometric proportions, in a high-energy mill, and in carrying out a heat treatment at a temperature of at least 800 0 C under controlled atmosphere. Such a process is therefore complicated to implement and unattractive because of the large amount of energy used. In addition, it provides the silicate in the form of particles of uncontrolled size, relatively large, of the order of 20 microns to 200 microns.
- the object of the invention is to provide a process for the preparation of mixed silicates of Li and a transition metal M (Fe, Co, Mn, Ni) which does not have the disadvantages of the method of the prior art. Accordingly, the present invention relates to a process for the preparation of mixed lithium silicates and transition metal, the silicates obtained, and their use as electrode active material in various electrochemical devices.
- the method of the present invention is a process for preparing a compound of the formula Li 2 M 11 J i X) M X 111 SiO 4 (OH) x (I) wherein 0 ⁇ x ⁇ 1 and M is Fe, Co, Mn or Ni, characterized in that it consists in: a) preparing an aqueous mixture of precursors of the compound (I); b) bringing the aqueous mixture to a temperature Tp between 60 ° C.
- the aqueous precursor solution is prepared by introducing into the water the precursor of M, the precursor of Si and the precursor of Li; the pH of the precursor solution is adjusted to a value of 10 to 14; steps a) and b) are carried out with stirring.
- the precursors of the silicate are chosen from compounds that are soluble in water.
- the aqueous mixture of silicate precursors is advantageously prepared at room temperature or at a higher temperature, depending on the solubility of the precursors.
- the precursors are preferably used in the form of a powder.
- the grain size is not critical.
- the precursor mixture is prepared by successively adding in water the M precursor, then the Si precursor and then the Li precursor.
- the precursor solution must be at a pH between 10 and 14. during steps a) and b). If necessary, the pH can be adjusted to this value by adding a base to the reaction medium, for example NaOH or KOH.
- iron As a precursor of iron, can be used a sulfate of Fe 11, Fe 11 chloride, oxalate Fe 11 or Fe 11 acetate, each in hydrated form or not.
- a precursor of manganese As a precursor of manganese can be used a sulfate Mn 11, Mn 11 a nitrate, a chloride of Mn 11, a Mn 11 oxalate, or an Mn 11 acetate, each in hydrated form or not.
- Ni As a precursor of nickel, one can use a sulfate of 11 Ni, 11 Ni chloride, oxalate Ni 11, or acetate of Ni 11, each in hydrated form or not.
- cobalt precursor can be used a sulfate of Co 11, Co 11 a nitrate, a chloride 11 Co, 11 Co oxalate, or acetate of Co 11, each in hydrated form or not.
- the mixed silicate comprises the transition metal M in M 11 form and in M 111 form.
- the proportion of M 111 that is to say the value of x, depends inter alia on the oxidizable nature of M and the oxidoreductive properties of the species present in the reaction medium.
- a mixed silicate of Fe or Ni may contain a high content of Fe 111 or Ni 111 respectively.
- a reducing agent into the aqueous precursor mixture.
- Ascorbic acid or hydrazine can be used as the reducing agent.
- a powder of the metal M It is advantageous to use an iron or nickel powder having a small particle size.
- the aqueous precursor solution may simultaneously contain the metal powder and a reducing agent selected from ascorbic acid and hydrazine.
- the ascorbic acid or hydrazine content is advantageously from 0.007 to 0.013 mol. L -1 , preferably from 0.009 to 0.011 mol L -1 .
- the precursor solution contains metal powder M
- the metal content in the precursor mixture does not exceed the precursor salt concentration of the metal.
- the powder content of the metal M is of the same order as the concentration of metal precursor salt, that is to say a number of moles of insoluble metal per unit volume of aqueous medium such as 0.07 ⁇ [M 0 ] ⁇ 0.13. 4 f. . . . . .
- the precursor of Si is selected from those compounds of Si which are soluble in water and in which Si is at oxidation state IV.
- Si precursors mention may be made of sodium metasilicate, SiCl 4 , Si (OH) 4 or SiCl 2 F 2 , optionally in their hydrated form.
- the Li precursor is a soluble compound preferably chosen from LiOH, LiCl, LiNO 3 , Li 2 SO 4 , C 2 H 3 LiO 2 , Li 2 C 2 O 4 and Li 2 CO 3 , each in hydrated form or not. It is particularly advantageous to use a precursor of Li whose counterion is OH or a counterion identical to that of the precursor salt of the metal M.
- the water constituting the solvent of the aqueous mixture is degassed before the introduction of the precursors.
- Degassing is particularly useful when M is an easily oxidizable metal such as Fe or Ni.
- Degassing can be carried out by passing an inert gas (eg N 2 or Ar) in water with gentle agitation for at least 20 min, preferably at room temperature.
- the temperature Tp is preferably between 80 ° C. and the boiling temperature.
- the precipitate formed is separated by conventional means. Centrifugation is particularly appropriate. After separation, the precipitate is washed with a solvent to remove residual reagents and by-products that may be formed. The residues and by-products soluble in water are removed by washing with a polar solvent preferably protic, for example water, ethanol or methanol. A second wash with a polar solvent miscible with more volatile water allows the removal of water.
- a polar solvent for example, acetonitrile, acetone, or ethanol can be used.
- the inert atmosphere can be obtained by drying under nitrogen or argon. Vacuum drying can also be carried out.
- the silicates obtained by the process described above constitute another subject of the invention.
- a silicate according to the invention corresponds to the formula Li 2 M II ( i- X ) M III x SiO 4 (OH) x (I) in which O x x l 1 and M is Fe, Co, Mn or Ni, and it is characterized in that it is in the form of substantially spherical and non-coalesced particles having a size of 400 to 600 nm; it has a structure in the Pna2i space group and possibly in the Pccn space group.
- the silicate corresponds to the formula Li 2 Fe ⁇ d - X ) Fe 111 X SiO 4 (OH) x and has a 7 Li NMR spectrum which shows 3 components at 11, -8 and -83, respectively ppm.
- x ⁇ 0.6 the silicate structure of Fe and Li is in the Pna2 ⁇ space group.
- x> 0.6 the structure of the Fe and Li silicate is in the Pna2i space group or in the Pccn space group.
- the silicate corresponds to the formula Li 2 Mn 11 SiO 4 and its structure is in the space group Pna2i.
- M Mn
- the silicate corresponds to the formula Li 2 Ni 11 CL - X ) Ni 111 X SiO 4 (OH) x and its structure is in the space group Pna2i.
- a mixed silicate according to the present invention is particularly useful as a positive electrode active material in an electrochemical device, in particular in a rechargeable lithium ion battery, or a lithium battery with a polymer electrolyte.
- a positive electrode for an electrochemical device is constituted by a composite material that contains:
- the silicate content is preferably from 80 to 90% by weight.
- the binder content is preferably less than 10% by weight.
- the content of compound conferring electronic conduction is preferably between 5 and 15% by weight.
- the ionically conductive compound content is preferably less than 5% by weight.
- the binder may be a non-solvating polymer, a solvating polymer or a mixture of solvating polymer and non-solvating polymer. It may further contain one or more aprotic polar liquid compounds.
- the non-solvating polymer may be chosen from homopolymers and copolymers of vinylidene fluoride, copolymers of ethylene, of propylene and of a diene, homopolymers and copolymers of tetrafluoroethylene, homopolymers and copolymers of N-vinylpyrrolidone, homopolymers and copolymers of acrylonitrile and 1 homopolymers and copolymers of methacrylonitrile ..
- the solvating polymer may be chosen for example from polyethers of linear structure, comb or block, forming or not a network, based on poly (ethylene oxide); copolymers containing the ethylene oxide or propylene oxide or allylglycidyl ether unit; polyphosphazenes; crosslinked networks based on polyethylene glycol crosslinked with isocyanates; copolymers of oxyethylene and epichlorohydrin 1; and networks obtained by polycondensation and bearing groups that allow the incorporation of crosslinkable groups.
- the aprotic polar compound may be chosen from linear or cyclic carbonates, linear or cyclic ethers, linear or cyclic esters, linear or cyclic sulphones, sulphonamides and nitriles.
- the compound conferring electronic conduction may be chosen for example from carbon blacks, graphites, carbon fibers, carbon nanowires, or carbon nanotubes.
- the compound conferring ionic conduction is a lithium salt, advantageously chosen from LiClO 4 , LiPF 6 ,
- a composite positive electrode according to the invention may be prepared by mixing the silicate, a binder in a suitable solvent, a material conferring electronic conduction, and optionally a lithium salt, by spreading the mixture obtained on a metal disc serving as a collector (for example an aluminum disk), then evaporating the solvent under an inert atmosphere.
- the solvent is chosen according to the binder used.
- a positive electrode can be further elaborated by extruding a mixture of its constituents.
- a positive electrode according to the invention can be used in a battery whose operation is ensured by the reversible circulation of lithium ions in the electrolyte between the positive electrode and the negative electrode.
- Another object of the present invention is therefore a battery in which the electrolyte comprises a lithium salt dissolved in a solvent, the positive electrode being an electrode according to the present invention.
- the electrolyte comprises at least one lithium salt in solution in a solvent, said salt being able to be chosen, for example and without limitation, from among the lithium salts mentioned above as constituent of the composite material electrode.
- the solvent of the electrolyte may consist of one or more aprotic polar compounds chosen from linear or cyclic alkyl carbonates, linear or cyclic ethers, linear or cyclic esters, linear or cyclic sulphones, sulphonamides and nitriles. .
- the solvent of the electrolyte may further be a solvating polymer, selected for example from among those mentioned above as constituent of the electrode composite material.
- the solvent of the electrolyte may further be a mixture of a polar aprotic liquid compound selected from aprotic polar compounds and a solvating polymer.
- the solvent of the electrolyte may also be a mixture of an aprotic polar compound or a solvating polymer, and a non-solvating polar polymer comprising units containing at least one heteroatom selected from sulfur, oxygen, oxygen and the like. nitrogen and fluorine.
- the negative electrode of the battery may consist of lithium metal or a lithium alloy which may be chosen from ⁇ -LiAl, ⁇ -LiAl, Li-Pb alloys (for example Li 7 Pb 2 ), Li-Cd- Pb, Li-Sn, Li-Sn-Cd, Li-Sn in various matrices, in particular oxygen matrices or metal matrices (for example Cu, Ni, Fe, Fe-C), Li-Al-Mn.
- the battery is then called "lithium battery”.
- the negative electrode of the battery may further consist of a composite material comprising a binder and a material capable of reversibly inserting lithium ions with low redox potential (hereinafter referred to as insertion material).
- the battery is then called "lithium ion battery".
- the insertion material may be chosen from carbon materials, natural or synthetic. These carbonaceous materials may be for example a petroleum coke, a graphite, a graphite whisker, a carbon fiber, a micro-grain carbon meso (usually referred to as meso carbon micro bead), a pitch coke (usually referred to as pitch coke), a needle coke (usually referred to as needle coke).
- the insert material may further be selected from oxides such as for example Li x MoO 2, Li x WO 2, Li x Fe 2 O 3, Li 4 Ti 5 O 2, Li x TiO 2 or from sulfides such as for example LigMo ⁇ S ⁇ and LiTiS 2 or among oxysulfides.
- oxides such as for example Li x MoO 2, Li x WO 2, Li x Fe 2 O 3, Li 4 Ti 5 O 2, Li x TiO 2 or from sulfides such as for example LigMo ⁇ S ⁇ and LiTiS 2 or among oxysulfides.
- the binder is an electrochemically stable organic binder in the operating range of the negative electrode.
- nitrides e.g., Li 2, 6 - ⁇ C ⁇ o, 4 N, Li 2+ x FeN 2 , Li 7 + x MnN 4
- phosphides for example Lig- x VP 4
- arsenides for example Li 9 _ x VAs 4
- reversible decomposition oxides for example CoO, CuO, Cu 2 O.
- the binder is an electrochemically stable organic binder in the operating range of the negative electrode.
- homopolymers of polyvinylidene fluoride or an ethylene propylene diene copolymer there may be mentioned homopolymers of polyvinylidene fluoride or an ethylene propylene diene copolymer.
- ascorbic acid (As.Ac) marketed by Acros Organics under the name L (+) -Ascorbic acid (99%, 50-81-7), particle size ⁇ 2 mm .
- iron sulphate FeSO 4 , 7H 2 O sold by Aldrich under the name Iron (II) sulfate heptahydrate (99%, 7782-63-0), particle size "2 mm.
- sodium metasilicate Na 2 SiO 3 , 5 H 2 O sold by Acros Organics under the name Sodium metasilicate penldhydrid (10213-79-3), particle size ⁇ 2 mm.
- the synthesis of the mixed Fe and Li silicate was carried out in a reactor equipped with a reflux system, a stirring system and a device allowing the passage of argon in the medium.
- iron sulphate FeSO 4 7 H 2 O 5.5602 g sodium metasilicate Na 2 SiO 3 , 5H 2 O 5.2505 g - lithium hydioxydide LiOH, H 2 O 12.7175 g
- Example 1 The procedure of Example 1 was repeated using the following compounds: ascorbic acid (As.Ac) 0, 2201 g Iron metal 1, 3987 g - iron sulphate FeSO 4 , 7 H 2 O 5, 5602 g metasilicate of sodium Na 2 SiOa, 5H 2 O 5, 2505 g lithium hydroxide LiOH, H 2 O 12, 7175 g
- Example 1 The procedure of Example 1 was repeated using the following compounds: ascorbic acid (As.Ac) 0, 2201 g
- Iron metal 1 3987 g - iron chloride FeCl 2 , 4 H 2 O 5, 5602 g - sodium metasilicate Na 2 SiO 3 , 5H 2 O 5, 2505 g lithium hydroxide LiOH, H 2 O 12, 7175 g
- Metallic iron was introduced at the same time as ascorbic acid. Iron chloride was introduced in place of iron sulphate.
- Example 4 The procedure of Example 4 was repeated, but the final drying of the Fe and Li silicate under vacuum was carried out.
- FIG. 1 represents two views by scanning electron microscope (SEM) of the compound obtained according to the method of example 1. It shows that the compound obtained is in the form of unsintered particles, monodisperse in size (from 400 to 600 nm), and of regular shape substantially spherical. The result is identical for the compounds obtained according to Examples 2 to 5.
- SEM scanning electron microscope
- FIGS. 2a, 3a, 4a, 5a and 6a respectively represent the Mossbauer spectra of the iron of each of the silicates of Examples 1 to 5.
- the spectrum obtained is the sum of two characteristic doublets of Fe (II) and Fe (III) in coordination with 4.
- the spectra are simulated with two components to describe the Fe (III) doublet and a single component for Fe (II).
- the curve (a) represents the experimental spectrum
- the curve (b) represents the calculated spectrum
- - the curve (c) represents the doublet Fe (II)
- the curve (d) represents the doublet Fe (III ) # 1
- curve (e) represents the doublet Fe (III) # 2.
- the quadrupole difference and the isomeric displacement are constant for all the examples, namely: Fe (II): 0.95 mm. s "1 and 2.6 mm s ' 1 ,
- Fe (III) # 2 0.3 mm. s "1 and 0.7 mm s ' 1 . Only the ratio of the intensities of the Fe (III) / Fe (II) doublets, from which the value of x can be determined, varies.
- FIGS. 2c, 3c, 4c, 5c and 6c respectively show the X-ray diffractogram of each of the silicates of Examples 1 to 5.
- (a) corresponds to the positions of the Bragg peaks for indexing in the group. of space Pna2i
- (b) corresponds to the positions of the Bragg peaks for indexing in the space group Pccn.
- the values of the mesh parameters are given in the table below.
- the structure is of type Pna2i.
- the crystal is built by twinning which affects the diffractogram of X-rays.
- it will be necessary to adopt the space group Pccn.
- This twinning is the consequence of the superposition of 3 lattice planes belonging to the Pna2i space group in the (001) direction with a rotation of 0 °, 120 ° and 240 °.
- An apparent space group is then formed which is visible in X-ray diffraction under the space group Pccn.
- the 7 Li NMR signal was measured by a Nuclear Magnetic Resonance spectrometer with a 4.7 Tesla Bruker magnet equipped with an Appolo Tecmag console. The acquisition was performed on a 2.5 mm Bruker probe by the magic angle spinning method at 33 kHz with a 2.5 mm diameter Zirconium rotor. The measurement was performed by a 90 ° pulse sequence followed by the acquisition and a relaxation time of 250 ⁇ s.
- FIGS. 2b, 3b, 4b, 5b and 6b respectively show the 7 Li NMR spectra of each of the silicates of Examples 1 to 5.
- curve (a) represents the experimental NMR 7 Li spectrum
- - curve (b) represents the calculated spectrum
- curve (c) represents the lithium site # 1
- curve (d) represents the lithium site # 2
- curve (e) represents the lithium site # 3.
- (# 1) represents the absolute area of the lithium 1 site
- (# 2) represents the absolute area of the lithium 2 site
- (# 3) represents the absolute area of the lithium site 3, - the projection on the axis of x, the position of the numbers 1, 2, 3, 4 and 5 inscribed at the top of the figure indicates the value of x respectively for each of the silicates prepared in Examples 1 to 5.
- the characteristics of the five silicates prepared according to Examples 1 to 5 are reported in the table below. They show that the OH content decreases from 1 toward the 5 th example. The lowest level is obtained with iron chloride as precursor, in the presence of a reducing agent (ascorbic acid) and Fe 0 , using small particle size reagents obtained by grinding commercial products, and performing vacuum drying.
- a reducing agent ascorbic acid
- Fe 0 small particle size reagents obtained by grinding commercial products, and performing vacuum drying.
- the electrochemical test was carried out in an electrochemical cell of the Swagelok® type assembled in a dry box under a controlled atmosphere.
- This cell comprises a positive electrode whose active material is a Fe and Li silicate obtained by the method of Example 5, a negative electrode consisting of a 1 cm 2 metal lithium foil, and a fiber sheet.
- borosilicate glass type GF / D, supplied by the company Whatman impregnated with a solution of LiPF ⁇ IM in a mixture of ethyl carbonate / dimethyl carbonate ECrDMC (1: 1 by mass), said impregnated sheet being placed between the two electrodes.
- the material constituting the positive electrode is prepared by mixing the silicate with carbon "Ketjen Black” (compressed to 50%, 99.9% pure, marketed by Alfa) in amounts such that the carbon represents 16.7 % by weight of the electrode.
- the mixing is carried out by an intimate grinding of 5 minutes by mechanical grinding with an SPEX 8000 type grinder.
- a galvanostatic measurement was carried out by subjecting the electrochemical cell to charge discharge cycles on a "Macpile" type automatic cycler (Biology Co , SA, Claix, France) at 75 ° C and a C / 37 regime.
- Figure 8 shows the cycling curves and the lithium level y. It shows a charge at 3 V during the first cycle and 2.8 V for subsequent cycles. 90% of lithium is extracted with a reversibility on 0.8 lithium.
- the polarization of the battery due to the material is low.
- the capacity of the electrode is related to the value of x. Indeed, the material will be electrochemically active only on (1-x) lithium. On the other hand, the presence of hydroxyl groups is likely to generate water molecules, harmful to the operation of the battery.
- a solid Fe and Li silicate was prepared according to the prior art, and the silicate obtained was characterized. Silicate preparation
- Example 2 of EP-I 134 826 a mixture of 71.8 g of FeO and 89.9 g of Li 2 SiO 3 was subjected to high energy milling in a ball mill for 4 hours, then the resulting mixture was transferred to a quartz bulb in which iron shot was added.
- the ampoule kept at 200 ° C. was placed under secondary vacuum and sealed. Then, it was brought to 800 0 C and maintained at this temperature for 4 hours. After cooling, the bulb was opened under argon and the shot was removed magnetically.
- Figure 9 shows two SEM micrographs of the compound obtained. It shows that the compound has a large disparity in size and morphology. It consists of sintered and agglomerated particles of heterogeneous form, whose size is between 5 microns and 200 microns.
- the 7 Li NMR signal was measured by a Nuclear Magnetic Resonance spectrometer with a Bruker magnet of 4.7
- the acquisition was carried out on a 2.5 mm Bruker probe by the method of the magic angle rotation at 33 kHz with a rotor in
- the measurement was performed by a 90 ° pulse sequence followed by the acquisition and a relaxation time of 250 ⁇ s.
- the NMR spectrum Li 7 is shown in FIG. 10, in which: the inset represents an enlarged view of the central peak - the curve (a) represents the experimental NMR 7 Li spectrum, the curve (b) the calculated spectrum, the curve (c) represents the lithium site # 1, the curve (d) represents the lithium site # 2.
- the NMR spectrum shows the existence of two lithium sites at -6 and -64 ppm. The integration of these sites gives a distribution of 1 and 2 lithium respectively.
- Electrochemical test II was carried out according to the procedure described in Example 6, replacing the silicate according to the invention by the same amount of silicate prepared according to the prior art as described in the present example.
- Figure 12 shows the cycling curves and the y-rate of lithium at 75 ° C and a C / 37 regime. It shows a charge at 3 V during the first cycle and 2.8 V for subsequent cycles. 45% of the lithium is extracted with a reversibility on 0.35 lithium.
- the grain structure of the silicate of the invention is different from that of the silicate of the prior art
- the silicate grains of the invention are thinner and more regular than the silicate grains of the prior art
- the NMR 7 Li spectrum shows that the sites and the chemical shift of the lithium in a silicate of the prior art are different from the sites and the displacement of lithium in a silicate according to the present invention, which shows that the respective environment lithium is different.
- Example 8 Li 2 Mn 11 SiO 4
- reaction mixture was brought to 100 ° C. over a period of 1 h, this temperature was maintained for 24 h, and then the reaction mixture was allowed to return to room temperature. At room temperature, the supernatant was removed by centrifugation, the compound was washed with acetone, and the resulting compound was dried.
- the X-ray diffractogram shown in Figure 13 was recorded on a Philips powder diffractometer with a copper anticathode. It shows that the compound has a very good crystallinity.
- reaction mixture was brought to 100 ° C. over a period of 1 h, this temperature was maintained for 24 h, and then the reaction mixture was allowed to return to room temperature. At room temperature, the supernatant was removed by centrifugation, the compound was washed with acetone, and the resulting compound was dried under argon.
- the synthesis of the mixed Co and Li silicate was carried out in a reactor equipped with a reflux system, and a stirring system.
- reaction mixture was heated to 100 ° C over 1 hour, maintained at this temperature for 24 hours, and the reaction mixture was allowed to warm to room temperature.
- the supernatant was removed by centrifugation, the compound was washed with acetone, and the resulting compound was dried.
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Abstract
Description
Claims
Priority Applications (3)
Application Number | Priority Date | Filing Date | Title |
---|---|---|---|
EP08761851A EP2118007A2 (fr) | 2007-02-09 | 2008-02-07 | Silicates mixtes de lithium. |
CA002677711A CA2677711A1 (fr) | 2007-02-09 | 2008-02-07 | Silicates mixtes de lithium |
JP2009548714A JP2010517913A (ja) | 2007-02-09 | 2008-02-07 | 混合されたケイ酸リチウム |
Applications Claiming Priority (2)
Application Number | Priority Date | Filing Date | Title |
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FR0700932 | 2007-02-09 | ||
FR0700932A FR2912398B1 (fr) | 2007-02-09 | 2007-02-09 | Silicates mixtes de lithium |
Publications (2)
Publication Number | Publication Date |
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WO2008107571A2 true WO2008107571A2 (fr) | 2008-09-12 |
WO2008107571A3 WO2008107571A3 (fr) | 2009-06-25 |
Family
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Family Applications (1)
Application Number | Title | Priority Date | Filing Date |
---|---|---|---|
PCT/FR2008/000148 WO2008107571A2 (fr) | 2007-02-09 | 2008-02-07 | Silicates mixtes de lithium. |
Country Status (6)
Country | Link |
---|---|
EP (1) | EP2118007A2 (fr) |
JP (1) | JP2010517913A (fr) |
CN (1) | CN101652321A (fr) |
CA (1) | CA2677711A1 (fr) |
FR (1) | FR2912398B1 (fr) |
WO (1) | WO2008107571A2 (fr) |
Cited By (5)
Publication number | Priority date | Publication date | Assignee | Title |
---|---|---|---|---|
JP2010225378A (ja) * | 2009-03-23 | 2010-10-07 | Toyota Central R&D Labs Inc | リチウム二次電池 |
WO2011108464A1 (fr) * | 2010-03-01 | 2011-09-09 | 古河電気工業株式会社 | Substance de matériau actif de cathode, cathode, batterie rechargeable et leurs procédés de production |
WO2011108465A1 (fr) * | 2010-03-01 | 2011-09-09 | 古河電気工業株式会社 | Composite particulaire, agrégat de matière active, substance pour matière active cathodique, cathode, batterie secondaire, et leurs procédés de fabrication |
WO2012001060A1 (fr) | 2010-06-30 | 2012-01-05 | Höganäs Ab | Matériau de cathode en silicate double de lithium et fer et sa production |
US8999282B2 (en) | 2010-02-22 | 2015-04-07 | Massachusetts Institute Of Technology | Carbophosphates and related compounds |
Families Citing this family (7)
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CN101920972B (zh) * | 2010-06-28 | 2011-12-14 | 宁波大学 | 一种用于锂离子电池的硅酸钴锂正极材料的制备方法 |
WO2012127762A1 (fr) * | 2011-03-23 | 2012-09-27 | ヤマハ発動機株式会社 | Composition électriquement conductrice, système de dispersion, procédé de production d'une composition électriquement conductrice et batterie à électrolyte solide |
JP5754808B2 (ja) * | 2011-10-13 | 2015-07-29 | 太平洋セメント株式会社 | 二次電池用正極活物質及びその製造方法 |
WO2014155408A1 (fr) * | 2013-03-25 | 2014-10-02 | 株式会社豊田自動織機 | Composé de silicate de lithium contenant de l'hydrogène, son procédé de production, matériau actif positif pour batterie secondaire à électrolyte non aqueux, électrode positive pour batterie secondaire à électrolyte non aqueux et batterie secondaire à électrolyte non aqueux |
KR101527286B1 (ko) * | 2013-09-30 | 2015-06-09 | 고려대학교 산학협력단 | 리튬 이차 전지용 음극의 형성 방법 |
CN110127712A (zh) * | 2019-05-15 | 2019-08-16 | 浙江工业大学 | 常压水解法制备具有微纳结构的介孔硅酸锂空心球的方法 |
CN118039890B (zh) * | 2024-01-18 | 2025-02-14 | 深圳新源邦科技有限公司 | 一种硅钼酸锂材料及其制备方法和应用 |
Family Cites Families (3)
Publication number | Priority date | Publication date | Assignee | Title |
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JPS58110414A (ja) * | 1981-12-23 | 1983-07-01 | Tokuyama Soda Co Ltd | 無機酸化物及びその製造方法 |
CA2320661A1 (fr) * | 2000-09-26 | 2002-03-26 | Hydro-Quebec | Nouveau procede de synthese de materiaux limpo4 a structure olivine |
GB0229630D0 (en) * | 2002-12-20 | 2003-01-22 | Rockwood Additives Ltd | Process for the production of synthetic magnesium silicate compositions |
-
2007
- 2007-02-09 FR FR0700932A patent/FR2912398B1/fr not_active Expired - Fee Related
-
2008
- 2008-02-07 EP EP08761851A patent/EP2118007A2/fr not_active Withdrawn
- 2008-02-07 JP JP2009548714A patent/JP2010517913A/ja active Pending
- 2008-02-07 CN CN200880010766A patent/CN101652321A/zh active Pending
- 2008-02-07 CA CA002677711A patent/CA2677711A1/fr not_active Abandoned
- 2008-02-07 WO PCT/FR2008/000148 patent/WO2008107571A2/fr active Application Filing
Cited By (10)
Publication number | Priority date | Publication date | Assignee | Title |
---|---|---|---|---|
JP2010225378A (ja) * | 2009-03-23 | 2010-10-07 | Toyota Central R&D Labs Inc | リチウム二次電池 |
US8999282B2 (en) | 2010-02-22 | 2015-04-07 | Massachusetts Institute Of Technology | Carbophosphates and related compounds |
WO2011108464A1 (fr) * | 2010-03-01 | 2011-09-09 | 古河電気工業株式会社 | Substance de matériau actif de cathode, cathode, batterie rechargeable et leurs procédés de production |
WO2011108465A1 (fr) * | 2010-03-01 | 2011-09-09 | 古河電気工業株式会社 | Composite particulaire, agrégat de matière active, substance pour matière active cathodique, cathode, batterie secondaire, et leurs procédés de fabrication |
JP2011181331A (ja) * | 2010-03-01 | 2011-09-15 | Furukawa Electric Co Ltd:The | 正極活物質材料、正極、2次電池及びこれらの製造方法 |
JP2011178601A (ja) * | 2010-03-01 | 2011-09-15 | Furukawa Electric Co Ltd:The | 微粒子混合物、活物質凝集体、正極活物質材料、正極、2次電池及びこれらの製造方法 |
US8696949B2 (en) | 2010-03-01 | 2014-04-15 | Furukawa Electric Co., Ltd. | Particulate mixture, active material aggregate, cathode active material, cathode, secondary battery and methods for producing the same |
US9136535B2 (en) | 2010-03-01 | 2015-09-15 | Furukawa Electric Co., Ltd. | Cathode active material, cathode, secondary battery and manufacturing methods for the same |
WO2012001060A1 (fr) | 2010-06-30 | 2012-01-05 | Höganäs Ab | Matériau de cathode en silicate double de lithium et fer et sa production |
US20130207032A1 (en) * | 2010-06-30 | 2013-08-15 | Höganas AB (publ) | Lithium iron silicate cathode material and its production |
Also Published As
Publication number | Publication date |
---|---|
JP2010517913A (ja) | 2010-05-27 |
CA2677711A1 (fr) | 2008-09-12 |
FR2912398B1 (fr) | 2009-04-24 |
FR2912398A1 (fr) | 2008-08-15 |
WO2008107571A3 (fr) | 2009-06-25 |
EP2118007A2 (fr) | 2009-11-18 |
CN101652321A (zh) | 2010-02-17 |
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