Patent Application
20120292560
This is a §371 of International Application No. PCT/JP2010/073880, with an international filing date of Dec. 24, 2010, which is based on Japanese Patent Application No. 2010-006183, filed Jan. 14, 2010, the subject matter of which is incorporated by reference.
This disclosure relates to a method for producing a positive active material for a secondary battery represented by a lithium-ion battery, and more particularly to a method for producing lithium iron phosphate.
With respect to miniaturized lithium-ion batteries which have become widespread mainly in the field of mobile apparatus, enhancement of performance has been realized through improvement of negative active material or development of an electrolytic solution or the like. On the other hand, with respect to a positive active material, no remarkable technical innovation has been made up to now from the time that commercialization of miniaturized lithium-ion batteries started. Lithium cobaltate (LiCoO2), which contains expensive rare metal, has been mainly used. Besides being expensive, the lithium cobaltate is not sufficient in thermal and chemical stability and emits oxygen under a high temperature of approximately 180° C. thus giving rise to a possibility of igniting an organic electrolytic solution whereby safety still remains a drawback.
Accordingly, in the development of the use of lithium-ion batteries which envisages the future use of the lithium-ion battery in a large-sized apparatus, development of a positive active material which is cheaper than conventionally used lithium cobaltate and is thermally and chemically stable to secure high safety is indispensable.
Currently, a material which is considered promising as a new positive active material capable of replacing the lithium cobaltate is olivine lithium iron phosphate (LiFePO4, simply referred to as “lithium iron phosphate” hereinafter) which is an iron-based active material and exhibits high safety in addition to less restriction in terms of resource problems and less toxicity. The lithium iron phosphate is a highly safe active material since the lithium iron phosphate does not emit oxygen up to approximately 400° C. because of strong P—O bonding in the crystalline structure, and is also an active material which exhibits excellent long-period stability and rapid charge characteristics.
In using the lithium iron phosphate as the positive active material, to allow the lithium iron phosphate to secure a high-speed charge/discharge characteristic which is a characteristic that the positive active material is requested to satisfy, it is necessary to improve electron conduction of the lithium iron phosphate and shorten the diffusion distance of lithium ions.
As a measure to cope with such problems, it is considered effective to cover surfaces of lithium iron phosphate particles with an electric conductive material and form the lithium iron phosphate particles into fine particles (approximately 100 nm or less) thus increasing the reaction surface area. Further, it has been also reported that doping the lithium iron phosphate with other elements is effective in improving electron conduction and stabilization of the crystalline structure.
Accordingly, as described above, development of a method for producing fine lithium iron phosphate particles whose surfaces are covered with the electric conductive material stably at a low cost becomes important to realize the practical use of the lithium iron phosphate as the positive active material.
As a method for synthesizing the lithium iron phosphate aimed at lowering cost, a method which uses inexpensive iron particles as an iron source has been known.
For example, in WO 2004/036671, a method is disclosed where metallic iron and a compound liberating a phosphoric acid ion are first reacted with each other in an aqueous solution and, thereafter, lithium carbonate or lithium hydroxide is added to the aqueous solution to prepare a precursor of the lithium iron phosphate. The precursor is then dried, the dried material is subject to primary baking at a temperature within a temperature range from 300 to 450° C., a substance from which conductive carbon is formed by thermo decomposition is added to the baking material, and the mixture is baked at a temperature of 500 to 800° C.
However, in the above-mentioned method, since the metallic iron of high purity of 99.9% or more reacts with phosphoric acid in preparing the precursor, aggregate particles of iron phosphate (Fe3(PO4)2.8H2O) which are a sparingly soluble bivalent iron compound are formed and grown and the solution becomes a creamy high-viscosity material which exhibits color ranging from white to light blue. As a result, agitation of the solution becomes insufficient thus giving rise to drawbacks including a drawback that unreacted metallic iron is liable to remain and raw materials are not uniformly mixed with each other. Further, an acid such as hydrochloric acid or oxalic acid is added to promote a reaction of the unreacted metallic iron. However, when the hydrochloric acid is added, the product is liable to be oxidized, while when the oxalic acid is added, it is difficult to uniformly prepare the precursor due to the formation of stable iron oxalate as a deposit in the form of a single body or the like. Further, it is difficult to uniformly mix carbon black or the like which is added as the conductive carbon to the precursor at an atomic level. Hence, the effect of the carbon black or the like as a reducing agent is small in the temperature range of the primary baking where the precursor is liable to be oxidized.
JP-A-2006-131485 discloses a method in which iron powder, a lithium salt and a phosphate compound are dissolved in an organic acid aqueous solution to prepare a precursor and, then, the precursor is dried by spraying and, thereafter, a dried material is baked at a temperature of 500° C. or more.
However, the above-mentioned method has a drawback that although an effective bivalent iron can be formed by oxidizing iron with an organic acid or a mixed organic acid, it is difficult to make the bivalent iron present in a stable state. Further, when the lithium salt is lithium nitrate, nitrate ion acts as an oxidant at the time of baking. Further, although it may be possible to use lithium acetate as the lithium salt, lithium acetate is an expensive raw material. Hence, use of lithium acetate is not effective in lowering cost. Further, although organic compounds which generate pyrolytic carbon are mixed in a precursor solution in the above-mentioned method, some organic compounds are carbonized alone at the time of baking so that the surfaces of the lithium iron phosphate particles cannot be effectively covered with the pyrolytic carbon.
JP-A-2007-305585 describes a method where iron powder first reacted in an aqueous solution containing a phosphoric acid and a citric acid, lithium hydroxide is added to the aqueous solution and, then, a precursor is prepared by adding metal oxide or a metal salt which is changed to conductive oxide by baking to the aqueous solution, and the precursor is dried and, finally, a dried product of the precursor is baked.
However, in the above-mentioned method, the citric acid does not effectively act as a chelating agent when the iron powder reacts with the phosphoric acid so that iron in the precursor is oxidized to trivalence to form ferric phosphate which is a trivalent iron compound. Further, the method describes an example where vanadium oxide V2O5 is added as the conductive oxide. However, in that method, the vanadium oxide is added after formation of the precursor of lithium iron phosphate. Hence, doping of vanadium is not effected and vanadium adheres to peripheries of the lithium iron phosphate particles.
JP-A-2008-4317 describes a method for producing lithium iron phosphate for batteries where the lithium iron phosphate is formed by baking a mixture which contains iron powder having an average particle size of 20 to 150 μm and apparent density of 2 g/cm3 or less, a phosphate compound and a lithium compound.
However, the method described in JP '317 also, in the same manner as the method described in JP '485, has a drawback that it is difficult to make the bivalent iron present in a stable state.
As described above, when iron particles are used as an iron source in a method for synthesizing lithium iron phosphate, the prior methods cannot sufficiently control the reaction of iron particles. Accordingly, because unreacted iron particles remain and the oxidation of iron excessively progresses so that a crystalline trivalent iron compound is formed or the like, a precursor of the lithium iron phosphate cannot be uniformly mixed and prepared at an atomic level whereby the lithium iron phosphate obtained as a final product cannot secure a sufficient discharge capacity. Further, in improving various characteristics of the lithium iron phosphate by doping lithium iron phosphate with other elements, the prior methods cannot dope the lithium iron phosphate with other elements uniformly.
It could therefore be helpful to provide a method for producing in a stable manner lithium iron phosphate which can acquire a positive active material made of inexpensive lithium iron phosphate possessing a high discharge capacity by preparing a precursor of the lithium iron phosphate where components are uniformly mixed at an atomic level by controlling a reaction of iron particles.
We discovered that, in producing high-performance lithium iron phosphate having a high discharge capacity as a positive active material using an inexpensive iron particle raw material, it is effective to determine an amount of oxygen chemically bonded to iron particles, to allow a carboxylic acid and a lithium source to coexist when the iron particles and the phosphoric acid are reacted with each other, and to cause the reaction in an oxidizing atmosphere. We also discovered that a chelate substance of the lithium iron phosphate which uniformly disperses in an aqueous solution is obtained by the above-mentioned reaction, and by drying the chelate substance of the lithium iron phosphate, a precursor of the lithium iron phosphate in which raw materials are uniformly mixed at an atomic level is obtained. Further, we discovered that, in improving various characteristics of the lithium iron phosphate by doping the lithium iron phosphate with other elements, by adding elements to be doped to an aqueous solution which contains a phosphoric acid, a carboxylic acid and a lithium source, the lithium iron phosphate which is uniformly doped with the elements can be obtained.
We thus provide:
(1) A method for producing lithium iron phosphate including:
(2) The method described in the above-mentioned (1), further includes a secondary baking step of mixing the lithium iron phosphate obtained in the primary baking step and a carbon source, and baking the mixture under a non-oxidizing atmosphere thus obtaining lithium iron phosphate whose surface is covered with carbon.
(3) The method described in the above-mentioned (1) or (2), wherein a content of the carboxylic acid is 0.18 to 0.5 mol for 1 mol of iron in the iron particles.
(4) The method described in any one of the above-mentioned (1) to (3), wherein a residual carbon rate of the carboxylic acid is 3 mass % or more.
(5) The method described in any one of the above-mentioned (1) to (4), wherein the carboxylic acid is at least one selected from the group consisting of a tartaric acid, a malic acid and a citric acid.
(6) The method described in any one of the above-mentioned (1) to (5), wherein metal or a compound which is an element to be doped is dissolved in the aqueous solution containing the phosphoric acid, the carboxylic acid and the lithium source in advance.
(7) The method described in any one of the above-mentioned (1) to (6), wherein the lithium iron phosphate is a positive active material for a secondary battery.
It is thus possible to produce lithium iron phosphate excellent in high-speed charge/discharge characteristics which are important characteristics to be satisfied by a positive active material at a low cost and in a stable manner.
Our method for producing lithium iron phosphate includes:
As the iron particles, it is possible to use reduced iron powder produced by reducing mill scales (ferric oxide) using coke, atomized iron powder produced by pulverizing and cooling molten steel using highly-pressurized water, electrolytic iron powder produced by precipitating on an anode by applying electrolysis to an aqueous ferric salt solution or the like. An average particle size of the iron powder may preferably be set to 100 μm or less. Although an average particle size of ordinary general-industry-use iron powder is 70 to 80 μm, the ordinary general-industry-use iron powder contains particles having a maximum particle size of 150 to 180 μm. Accordingly, the use of the iron powder after increasing a reaction surface by removing coarse particles using a sieve or turning the coarse particles into fine particles by mechanical milling or the like when necessary is advantageous for synthesizing chelate substances of the lithium iron phosphate while promoting a subsequent reaction of the iron powder with the phosphoric acid, the carboxylic acid and the lithium source.
The oxygen contained in the iron powder indicates oxygen which is chemically bonded to iron. It is a prerequisite that oxygen content is 0.5 mass % or more to synthesize the chelate substances of the lithium iron phosphate. The oxygen content may preferably be 0.6 to 2 mass %. When the oxygen content of the iron particles is less than 0.5 mass %, priority is assigned to a direct reaction between metallic iron and the phosphoric acid so that aggregate particles of iron phosphate (Fe3(PO4)2.8H2O) which are a sparingly soluble bivalent iron compound are formed and grown whereby the solution becomes a creamy high-viscosity material which exhibits color ranging from white to light blue. As a result, agitation of the aqueous solution becomes insufficient thus giving rise to drawbacks including such that unreacted metallic iron is liable to remain and raw materials are not uniformly mixed with each other. When the oxygen content of the iron particles is 2 mass % or less, there is no segregation of scales of ferric oxide on surfaces of the iron powder whereby the reaction between the iron powder and the aqueous solution of the phosphoric acid and the carboxylic acid is not impeded. Accordingly, the oxygen content of the iron particles may preferably be 2 mass % or less. The determination of the oxygen content in the iron particles is performed in accordance with a vacuum melting infrared absorbing method stipulated in JIS Z 613 (1992) using TC436 made by LECO Corporation.
To set the oxygen content of the iron particles to 0.5 mass % or more, in a case where the reduced iron powder is used as a raw material, for example, a temperature at which the mill scales (ferric oxide) are reduced using coke may be set to a temperature (about 800 to 1000° C.) which is lower than a usual temperature (1000 to 1200° C.).
Further, to use water atomized iron powder as a raw material, molten steel is pulverized and cooled using highly pressurized water and, thereafter, pulverized steel may be positively brought into contact with air in a drying step.
To elevate purity of the iron particles, usually, raw-material iron powder is subject to hydrogen reduction thus producing iron particles having oxygen content of approximately 0.4 mass % or less. Accordingly, the iron particles may be produced by adjusting the degree of hydrogen reduction.
The phosphoric acid may preferably be an aqueous solution of an orthophosphoric acid (H3PO4). However, an aqueous solution of higher-order condensed phosphoric acid (Hn+2PnO3n+1) may be also used as the phosphoric acid. The orthophosphoric acid which amounts to 75 to 85 mass % can be usually used as an industrial product. An addition amount of the phosphoric acid is 1 mol for 1 mol of iron in terms of a stoichiometric equivalent. However, there is no problem even when the addition amount of the phosphoric acid exceeds 1 mol by approximately 0.1 mol.
The carboxylic acid indicates an organic compound having a carboxyl group, and functions as a chelating agent at the time of synthesizing the chelate substances of the lithium iron phosphate. As the above-mentioned carboxylic acid, a carboxylic acid which exhibits a strong chelating force for iron, for example, a tartaric acid, a malic acid, a citric acid and the like can be named. Among these carboxylic acids, it is particularly preferable to use citric acid which exhibits a strong chelating force and forms a hardly-oxidized chelating substance.
Further, carbon remains at the time of baking. Hence, the carboxylic acid also functions as a reducing agent. To allow the carboxylic acid to exhibit such a function, it is desirable to set a residual carbon ratio of the carboxylic acid to 3 mass % or more. When the residual carbon ratio of the carboxylic acid is 3 mass % or more, there exists no possibility that the precursor is oxidized with oxygen existing in the non-oxidizing atmosphere. The non-oxidizing atmosphere means an inert gas atmosphere of nitrogen, argon or the like where oxygen concentration is 1000 ppm or less or an inert gas atmosphere containing a reducing gas such as hydrogen or carbon monoxide.
Further, it is preferable to set the above-mentioned residual carbon ratio to 20 mass % or less. When the residual carbon ratio exceeds 20 mass %, a residual carbon content after baking becomes excessive. With respect to the residual carbon ratio of the above-mentioned carboxylic acid, the residual carbon ratio is 7 mass % in the case of tartaric acid, the residual carbon ratio is 12 mass % in the case of malic acid, the residual carbon ratio is 7 mass % in the case of citric acid hydrate, and the residual carbon ratio is less than 1 mass % in the case of oxalic acid dehydrate, acetic acid or the like.
“Residual carbon ratio” is a value obtained such that residual carbon after baking is determined in accordance with a high-frequency induction heating furnace combustion-infrared absorption method stipulated in JIS G 1211 (1995), and the residual carbon is divided by an initial amount of the carboxylic acid.
A content of the carboxylic acid may preferably be set to 0.18 to 0.5 mol for 1 mol of iron, and may more preferably be set to 0.2 to 0.4 mol for 1 mol of iron. When the content of the carboxylic acid is less than 0.18 mol, the above-mentioned chelating effect derived from the carboxylic acid is decreased. Hence, the metallic iron and phosphoric acid ion directly react with each other and aggregate particles of sparingly soluble iron phosphate are formed and grown whereby the aqueous solution becomes a creamy high-viscosity material which exhibits color ranging from white to light blue. As a result, agitation of the aqueous solution becomes insufficient thus giving rise to drawbacks such that unreacted metallic iron is liable to remain and raw materials are not uniformly mixed with each other. On the other hand, when the above-mentioned content of the carboxylic acid exceeds 0.5 mol, synthesized chelate substances of the lithium iron phosphate are uniformly dispersed in the aqueous solution (raw materials being mixed uniformly). However, the residual carbon content after baking becomes excessive. As a result, an apparent discharge capacity of the lithium iron phosphate obtained as a final product is lowered.
As the lithium source, any kind of lithium may be used provided that the lithium is a water-soluble salt. However, it is particularly preferable to use lithium hydroxide or lithium carbonate which does not generate a poisonous gas at the time of baking.
As an atmosphere where the reaction is made by adding the iron particles to the aqueous solution which contains the phosphoric acid, the carboxylic acid and the lithium source, it is necessary to set the oxidizing atmosphere. It is because when a chelating reaction progresses and the oxygen or the surfaces of the iron particles is consumed, the chelating reaction cannot be sustained. Hence, priority is assigned to the direct reaction between the metallic iron and the phosphoric acid ion whereby the sparing soluble aggregate particles of the iron phosphate are formed and grown.
In view of such a circumstance, by bringing the above-mentioned atmosphere at the time of reaction into the oxidizing atmosphere, oxygen is supplemented by properly oxidizing the surfaces of the iron particles thus sustaining the chelating reaction. The oxidizing atmosphere indicates a state where the surfaces of the iron particles in the aqueous solution can be properly oxidized. Such a state is obtained, for example, by bringing an interface of the aqueous solution and an oxygen containing gas into contact with each other, by introducing bubbles or nano-bubbles of dissolved oxygen or oxygen containing gases in the aqueous solution or the like. Further, as a specific manipulation, agitation under an air atmosphere, bubbling of air or the like can be named.
In the above-mentioned chelating reaction, an aqueous solution temperature may preferably be controlled within a range from 10 to 40° C., and may be more preferably controlled within a range from 20 to 30° C. By controlling the aqueous solution temperature within the range from 10 to 40° C., the surfaces of the iron particles which newly appear due to the consumption of the oxygen by the above-mentioned chelating reaction are properly oxidized as being brought into contact with the dissolved oxygen, the air bubbles or the like in the aqueous solution whereby the chelate substances of the lithium iron phosphate can be continuously formed. When the aqueous solution temperature is below 10° C., the chelating reaction of the iron particles becomes slow. Hence, it takes a long time before the reaction is completely finished. On the other hand, when the aqueous solution temperature exceeds 40° C., the oxidation for supplementing the oxygen to the surfaces of the iron particles where the oxygen is consumed cannot catch up with the consumption of oxygen. Accordingly, priority is assigned to the direct reaction between the metallic iron and the phosphoric acid so that the aggregate particles of the sparingly soluble iron phosphate are formed and grown thus giving rise to a possibility that the aqueous solution becomes a creamy high-viscosity material which exhibits color ranging from white to light blue.
When the iron particles are added to the aqueous solution which contains the phosphoric acid, the carboxylic acid and the lithium source, and the aqueous solution is exposed to the oxidizing atmosphere, the carboxylic acid chelates iron by way of oxygen or a hydroxy group present on the surfaces of the iron particles, and the iron phosphate is formed due to bonding of the phosphoric acid with iron by oxidation whereby some hydrogen in a carboxylic group is replaced with lithium. As a result, it is estimated that chelate substances of the lithium iron phosphate expressed by Formula 1 are synthesized, and a reaction liquid in which the chelate substances are uniformly dispersed is obtained.
Although the chelate substances of the lithium iron phosphate are present in the reaction liquid in a dispersed state, there may be a case where some chelate substances are present in the form of aggregate particles and become a deposit. In such a case, to make the precursor solution uniform, it is desirable to wet the aggregate particles fine by mechanical milling. As a wet milling method, a beads mill, a wet jet mill, an ultrasonic irradiation or the like is named.
Further, when an X ray diffraction analysis is applied to a dried product obtained by drying the reaction liquid (precursor of lithium iron phosphate), no crystalline compound is detected, and an amorphous phase derived from chelate substances which are mixed uniformly at an atomic level is confirmed.
In doping the lithium iron phosphate with other elements, by dissolving in advance a metal or compound which is an element to be doped into the aqueous solution which contains the phosphoric acid, the carboxylic acid and the lithium source, the element to be doped can be uniformly mixed into the aqueous solution. For example, as such metal or compound of the element to be doped, Ti(OH)4, TiOSO4.H2O are named in the case of titanium, FeV, V2O5, VOSO4.2H2O are named in the case of vanadium, Mg, MgO, Mg(OH)2 are named in the case of magnesium, WO3, H2WO4 are named in the case of tungsten, and MnCO3.nH2O, Mn(CH3COO)2 are named in the case of manganese. Here, in the case where a doped element which is dissolved in advance in the aqueous solution containing the phosphoric acid and the carboxylic acid is reduced due to the addition of the iron particles so that the doped element is brought into a low oxidized state, it is expected that the doped element acts as an electron donor. Although the doping amount may depend on the kind of element, in general, replacement of 0.1 mol % or more of the iron element is preferable, and particularly replacement of 0.5 mol % or more of the iron element is more preferable. When the doping amount is less than 0.1 mol % of the iron element, the doping effect can be hardly acquired. An upper limit of the doping amount is largely changed due to factors such as ion radius, valency, coordination number of the element to be doped. Hence, the upper limit of the doping amount cannot be necessarily decided. However, when the doping amount exceeds a threshold value, there exists a tendency that characteristics are deteriorated due to localization of electrons due to formation of an impurity phase or a change of the band structure.
To dry the reaction liquid, it is preferable to adopt a spray dry method which exhibits favorable dry efficiency. In the spray dry method, a specimen solution is dried by spraying the specimen solution in high-temperature heated air. Hence, powder having a uniform shape can be manufactured. In adopting the spray dry method, it is preferable to set an inlet temperature (heating air temperature) in a spray dry device to 150 to 250° C. by taking a fact that an oxidizing temperature of a precursor (of the lithium iron phosphate) is approximately 250° C. into consideration. When the inlet temperature is set to 150 to 250° C., a reaching temperature of a formed dried product becomes approximately 100 to 150° C. although the reaching temperature depends on a balance with a liquid feeding amount. The lithium iron phosphate precursor which is the formed dried product takes a powdery form. The particle size of the precursor is preferably 100 μm or less, is more preferably 80 μm or less, and is still more preferably 50 μm or less. In the case where the particle size of the precursor exceeds 100 μm, coarse particles remain when milling performed after baking is insufficient, while when an electrode is formed using the precursor as a positive active material, there exists a possibility that a current collector is damaged.
By baking the lithium iron phosphate precursor at a temperature of 300° C. or above under the non-oxidizing atmosphere, H2O, CO2, H2 contained in the lithium iron phosphate precursor are eliminated through thermal decomposition, and the dried product having the amorphous phase is crystallized whereby a crystalline body of the lithium iron phosphate having the olivine structure is obtained. The baking temperature is preferably 300° C. or above, more preferably 350 to 700° C. When the baking temperature is below 300° C., elimination of CO2, H2 which are volatile components, through thermal decomposition becomes insufficient, and also crystallization cannot be acquired. On the other hand, with respect to an upper limit of the baking temperature, when the upper limit exceeds 700° C., the coarseness of obtained crystal particles progresses. Accordingly, the upper limit of the baking temperature is preferably 700° C. or below. Baking is performed under the non-oxidizing atmosphere to prevent oxidization of the lithium iron phosphate precursor.
Next, using the lithium iron phosphate which is the above-mentioned baked product as a primary baked product, a carbon source is mixed into the primary baked product and, then, the mixture is subjected to secondary baking. Due to such secondary baking, crystallinity of the lithium iron phosphate may be enhanced and, at the same time, conductivity of the lithium iron phosphate can be enhanced by covering a surface of the lithium iron phosphate with carbon or by adhering carbon to the surface of the lithium iron phosphate.
As the carbon source to be mixed to the lithium iron phosphate, a substance which forms carbon through thermal decomposition at the time of secondary baking or conductive carbon is used. The substance which forms carbon through thermal decomposition at the time of secondary baking may preferably be a substance which is melted at the time of secondary baking and wets the surfaces of the lithium iron phosphate particles. For example, a saccharide such as glucose, fructose, maltose, sucrose, ascorbic acid or erythorbic acid, carboxymethylcellulose, acenaphthylene, quinoline insoluble-less pitch (quinoline insoluble ≦0.1 mass %, ash ≦0.01 mass %) or the like can be used. As the conductive carbon, for example, carbon black, acetylene black, Ketjen black, VGCF, carbon nano fiber, fullerene or the like can be used. These substances can be used in a single form or in a combination of the plurality of substances.
As a method for mixing the carbon source into the primary baked product, a method where the carbon source is added to the primary baked product before or after the primary baked product is pulverized by wet or dry milling, and the mixture is pulverized using a ball mill, a jet mill or the like can be named. The addition amount of the carbon source is preferably set such that an amount of carbon contained in the lithium iron phosphate after the secondary baking is 1 to 5 mass %, and the addition amount of the carbon source may more preferably be set such that such the carbon content is 1.5 to 4 mass %. When the carbon content is less than 1 mass %, conductivity of the lithium iron phosphate is insufficient thus giving rise to the possibility that performance of the lithium iron phosphate particles which constitute the positive active material cannot be sufficiently taken out. On the other hand, when the carbon content exceeds 5 mass %, there exists a tendency where apparent discharge capacity is lowered. When secondary baking is performed, primary baking is preferably performed under a non-oxidizing atmosphere at a temperature of 350 to 400° C. Although the lithium iron phosphate is surely crystallized by baking at a temperature of 350° C. or above, the lithium iron phosphate particles grow along with the elevation of temperature. Hence, it is sufficient to perform primary baking at a temperature of 400° C.
Secondary baking is preferably performed at a temperature of 550 to 750° C. under a non-oxidizing atmosphere, and secondary baking is more preferably performed at a temperature of 600 to 700° C. When a substance which generates pyrolytic carbon is used as the carbon source, generation of the pyrolytic carbon becomes insufficient at a temperature below 550° C. thus giving rise to the possibility that conductivity of the lithium iron phosphate obtained after the secondary baking cannot be sufficiently exhibited. On the other hand, when the secondary baking is performed at a temperature exceeding 750° C., there is the possibility that the lithium iron phosphate particles become coarse.
As described above, the lithium iron phosphate precursor in which the raw materials are uniformly mixed at an atomic level is obtained such that the iron particles containing 0.5 mass % or more of oxygen are added to the aqueous solution containing the phosphoric acid, the carboxylic acid and the lithium source, the chelate substances of the lithium iron phosphate are synthesized by causing these elements to react with each other under the oxidizing atmosphere, and the chelate substances of the lithium iron phosphate are dried. Then, by baking the lithium iron phosphate precursor, the lithium iron phosphate having high performance can be obtained as an inexpensive positive active material.
We filed PCT/JP 2010/001691 on a method for producing lithium iron phosphate which includes the following steps:
In our method here, two steps, that is the first forming step of forming the first reaction liquid and the second forming step of forming the second reaction liquid in PCT/JP 2010/001691 are carried out in one synthesizing step:
Accordingly, this has advantages compared to the method described in PCT/JP 2010/001691:
Although our methods are specifically explained using examples hereinafter, this disclosure is not limited to these examples.
10 mol of phosphoric acid of 85 mass %, 2 mol of citric acid hydrate and 5 mol of lithium carbonate were dissolved in 2000 g of distilled water, 10 mol of iron powder (produced by JFE Steel Corporation, oxygen content: 0.68 mass %, average particle size: 80 μm, apparent density: 3.18 g/cm3) was added to the mixture solution, and a reaction between these materials was continued for 1 day while agitating these materials under an air atmosphere at a liquid temperature of 25 to 30° C. Then, the reaction liquid was dried by a spray dryer (FOC16 made by OHKAWARA KAKOHKI CO., LTD.) at an inlet temperature of 200° C. thus obtaining dried powder having an average particle size of approximately 30 μm in SEM observation. Primary baking was applied to the dried powder in a nitrogen gas flow at a temperature of 400° C. for 5 hours. Then, as a carbon source, 40 g of ascorbic acid was added to the whole primary baking product, and the primary baking product was subjected to wet milling and mixing using a ball mill. Subsequently, the obtained mixture was dried and, thereafter, secondary baking was applied to the obtained mixture in a nitrogen gas flow at a temperature of 700° C. for 10 hours. Finally, the baking mixture was subjected to screening using a sieve having meshes of 75 μm thus preparing lithium iron phosphate.
The oxygen content of the iron powder was determined using TC436 made by LECO Corporation.
The apparent density of the iron powder is measured in accordance with JIS Z 2504 (2000).
Lithium iron phosphate was prepared in the same manner as the Example 1 except for that 2 mol of malic acid was used in place of the citric acid hydrate in the Example 1.
Lithium iron phosphate was prepared in the same manner as the Example 1 except for that 2 mol of tartaric acid was used in place of the citric acid hydrate in the Example 1.
Lithium iron phosphate was prepared in the same manner as the Example 1 except for that an amount of the citric acid hydrate was set to 2.5 mol, and the ascorbic acid was not added to the primary baking product in the Example 1.
Lithium iron phosphate was prepared in the same manner as the Example 1 except for that iron powder (produced by KISHIDA CHEMICAL Co., Ltd., oxygen content: 1.55 mass %, average particle size: 70 μm, apparent density: 2.47 g/cm3) was used in the Example 1.
Lithium iron phosphate was prepared in the same manner as the Example 1 except for that 0.05 mol (replacing 1 mol % of iron element) of vanadium pentoxide V2O5 which is a vanadium source was added to and dissolved in the mixed solution containing the phosphoric acid, the citric acid hydrate and the lithium carbonate, and 9.9 mol of iron powder equal to the iron powder used in the Example 1 was added to the mixed solution in the Example 1.
Lithium iron phosphate was prepared in the same manner as the Example 1 except for that 0.15 mol (replacing 1 mol % of iron element) of titanyl sulfate which is a titanium source was added to and dissolved in the mixed solution containing the phosphoric acid, the citric acid hydrate and the lithium carbonate, and 9.9 mol of iron powder equal to the iron powder used in the Example 1 was added to the mixed solution in the Example 1.
Lithium iron phosphate was prepared in the same manner as the Example 1 except for that 0.1 mol (replacing 1 mol % of iron element) of magnesium oxide which is a magnesium source was added to and dissolved in the mixed solution containing the phosphoric acid, the citric acid hydrate and the lithium carbonate, and 9.9 mol of iron powder equal to the iron powder used in the Example 1 was added to the mixed solution in the Example 1.
Lithium iron phosphate was prepared in the same manner as the Example 1 except for that 0.1 mol (replacing 1 mol % of iron element) of manganese acetate which is a manganese source was added to and dissolved in the mixed solution containing the phosphoric acid, the citric acid hydrate and the lithium carbonate, and 9.9 mol of iron powder equal to the iron powder used in the Example 1 was added to the mixed solution in the Example 1.
Lithium iron phosphate was prepared in the same manner as the Example 1 except for that iron powder (produced by JFE Steel Corporation, oxygen content: 0.41 mass %, average particle size: 80 μm, apparent density: 2.55 g/cm3) was used in the Example 1.
Lithium iron phosphate was prepared in the same manner as the Example 1 except for that the agitation of the solution after the iron powder was added was performed under a nitrogen atmosphere in the Example 1.
Lithium iron phosphate was prepared in the same manner as the Example 1 except for that 2 mol of oxalic acid dehydrate was used in place of the citric acid hydrate in the Example 1.
With respect to respective lithium iron phosphates prepared by Examples 1 to 9 and Comparative Examples 1 to 3, identification analysis based on an X-ray diffraction analysis and quantitative analysis of carbon were performed. Primary particle sizes were also measured with respect to the respective lithium iron phosphates. The X-ray diffraction analysis was performed using UltimalV (X-Ray: Cu—Kα1) made by Rigaku Corporation. The quantitative analysis of carbon was performed using EMIA-620 made by HORIBA, Ltd. by determining the carbon content of the lithium iron phosphate. The primary particle size was obtained by X-ray diffraction analysis using the Scherrer equation.
Further, with respect to the respective lithium iron phosphates prepared by Examples 1 to 9 and Comparative Examples 1 to 3, discharge capacity was measured using the following method. A cathode was prepared such that a paste having a composition consisting of lithium iron phosphate, acetylene black, polyvinylidene fluoride (KFL #1320 made by KUREHA CORPORATION) at a mass ratio of 86:4:10 was applied to a current collector formed of an aluminum foil by coating at 10 mg/cm2. An anode was prepared by assembling a half cell (made by Hohsen Corp.) using metallic lithium. An electrolyte having a composition consisting of 1M-LiPF6/EC (ethylene carbonate) and EMC (ethylmethyl carbonate) at a mass ratio of 3:7 was used. A measuring condition was set such that the discharge capacity is obtained by performing a constant current charge up to 4.0 V at 0.2 mA/cm2 and, thereafter, by performing a constant current discharge down to 2.5 V at 0.2 mA/cm2.
The result of measurement of the above-mentioned identification analysis, carbon content, primary particle size and discharge capacity is shown in Table 1. As can be clearly understood from Table 1, in all Examples 1 to 9, the carbon content is 1.5 mass % or more, and the primary particle size is 100 nm or less, and olivine lithium iron phosphate possessing high discharge capacity was obtained. Particularly, the discharge capacity in the Examples 6 to 9 is slightly larger than the discharge capacity in the Examples 1 to 5. Hence, it is believed that such a discharge capacity enhancing effect is brought about by doping. On the other hand, Comparative Examples 1 to 3 cannot obtain lithium iron phosphate possessing sufficient discharge capacity. It is believed that phosphorus, iron and lithium are not mixed uniformly at an atomic level in Comparative Examples 1 to 3.
We provide a method for producing lithium iron phosphate possessing a high discharge capacity as an inexpensive positive active material by using inexpensive iron particles as an iron source.
| Number | Date | Country | Kind |
|---|---|---|---|
| 2010-006183 | Jan 2010 | JP | national |
| Filing Document | Filing Date | Country | Kind | 371c Date |
|---|---|---|---|---|
| PCT/JP2010/073880 | 12/24/2010 | WO | 00 | 8/6/2012 |
