CA2632868C - Electrolyte for lithium secondary battery comprising chelating agent and lithium secondary battery using the same - Google Patents
Electrolyte for lithium secondary battery comprising chelating agent and lithium secondary battery using the same Download PDFInfo
- Publication number
- CA2632868C CA2632868C CA2632868A CA2632868A CA2632868C CA 2632868 C CA2632868 C CA 2632868C CA 2632868 A CA2632868 A CA 2632868A CA 2632868 A CA2632868 A CA 2632868A CA 2632868 C CA2632868 C CA 2632868C
- Authority
- CA
- Canada
- Prior art keywords
- electrolyte
- chelating agent
- battery
- lithium secondary
- secondary battery
- Prior art date
- Legal status (The legal status is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the status listed.)
- Active
Links
Classifications
-
- 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
- H01M10/056—Accumulators with non-aqueous electrolyte characterised by the materials used as electrolytes, e.g. mixed inorganic/organic electrolytes
-
- 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
- H01M10/056—Accumulators with non-aqueous electrolyte characterised by the materials used as electrolytes, e.g. mixed inorganic/organic electrolytes
- H01M10/0564—Accumulators with non-aqueous electrolyte characterised by the materials used as electrolytes, e.g. mixed inorganic/organic electrolytes the electrolyte being constituted of organic materials only
- H01M10/0566—Liquid materials
- H01M10/0567—Liquid materials characterised by the additives
-
- 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
-
- 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
- H01M10/42—Methods or arrangements for servicing or maintenance of secondary cells or secondary half-cells
- H01M10/4235—Safety or regulating additives or arrangements in electrodes, separators or electrolyte
-
- 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
- H01M10/056—Accumulators with non-aqueous electrolyte characterised by the materials used as electrolytes, e.g. mixed inorganic/organic electrolytes
- H01M10/0564—Accumulators with non-aqueous electrolyte characterised by the materials used as electrolytes, e.g. mixed inorganic/organic electrolytes the electrolyte being constituted of organic materials only
- H01M10/0565—Polymeric materials, e.g. gel-type or solid-type
-
- Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
- Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
- Y02E—REDUCTION OF GREENHOUSE GAS [GHG] EMISSIONS, RELATED TO ENERGY GENERATION, TRANSMISSION OR DISTRIBUTION
- Y02E60/00—Enabling technologies; Technologies with a potential or indirect contribution to GHG emissions mitigation
- Y02E60/10—Energy storage using batteries
-
- Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
- Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
- Y02P—CLIMATE CHANGE MITIGATION TECHNOLOGIES IN THE PRODUCTION OR PROCESSING OF GOODS
- Y02P70/00—Climate change mitigation technologies in the production process for final industrial or consumer products
- Y02P70/50—Manufacturing or production processes characterised by the final manufactured product
Landscapes
- Chemical & Material Sciences (AREA)
- Engineering & Computer Science (AREA)
- Manufacturing & Machinery (AREA)
- Chemical Kinetics & Catalysis (AREA)
- Electrochemistry (AREA)
- General Chemical & Material Sciences (AREA)
- Inorganic Chemistry (AREA)
- Physics & Mathematics (AREA)
- Condensed Matter Physics & Semiconductors (AREA)
- General Physics & Mathematics (AREA)
- Secondary Cells (AREA)
- Battery Electrode And Active Subsutance (AREA)
Abstract
Disclosed herein is an electrolyte for lithium secondary batteries comprising:
a chelating agent, which forms complexes with transition metal ions in the battery, and at the same time does not react and coordinate with lithium ions;
a non-aqueous solvent; and an electrolyte salt, as well as a lithium secondary battery comprising the electrolyte. The chelating agent, which is contained in the electrolyte for lithium secondary batteries, can suppress a side reaction in which transition metal ions are reduced and deposited as transition metals on the anode. Also, the chelating agent can suppress internal short-circuits in the battery and the resulting voltage drop of the battery and a reduction in the safety and performance of the battery, which can occur when transition metals are deposited on the anode.
a chelating agent, which forms complexes with transition metal ions in the battery, and at the same time does not react and coordinate with lithium ions;
a non-aqueous solvent; and an electrolyte salt, as well as a lithium secondary battery comprising the electrolyte. The chelating agent, which is contained in the electrolyte for lithium secondary batteries, can suppress a side reaction in which transition metal ions are reduced and deposited as transition metals on the anode. Also, the chelating agent can suppress internal short-circuits in the battery and the resulting voltage drop of the battery and a reduction in the safety and performance of the battery, which can occur when transition metals are deposited on the anode.
Description
Description ELECTROLYTE FOR LITHIUM SECONDARY BATTERY
COMPRISING CHELATING AGENT AND LITHIUM
SECONDARY BATTERY USING THE SAME
Technical Field Ill The present invention relates to an electrolyte for lithium secondary batteries containing a chelating agent, and a lithium secondary battery comprising said electrolyte.
Background Art [21 Recently, the compact and lightweight construction of electronic equipment has been realized and the use of portable electronic devices has been generalized, and thus studies on secondary batteries having high energy density have been actively conducted.
[31 Lithium secondary batteries, which are currently mainly used, comprise cathode and anode made of materials capable of intercalating and deintercalating lithium ions, are fabricated by injecting a non-aqueous electrolyte between the cathode and anode, and produce electrical energy by oxidation and reduction reactions, which occur when lithium ions are intercalated into and deintercalated from the cathode and anode.
[41 When the secondary battery is charged and discharged, transition metal ions in the battery can cause side reactions and can result in a reduction in the performance of the battery. For example, when the cathode contains Fe impurities, Fe can be ionized, and deposited on the anode, resulting in voltage drop. Also, some Co, which is used as the cathode active material, can be dissolved out and deposited on the anode, and when spinel Mn is used for the cathode, Mn can be dissolved. In addition, when a Fe olivine material is used, Fe can be dissolved out. Such side reactions deteriorate the stability and performance of the battery.
[51 In a prior attempt to suppress side reactions, an expensive apparatus for purifying raw materials is used, the pretreatment of raw materials is performed, or other al-ternative materials having poor performance are used. However, such methods have problems in that they are expensive and deteriorate the performance of the battery.
Disclosure of Invention Technical Problem [61 It is an object of the present invention to provide an electrolyte for lithium secondary batteries containing a chelating agent, which forms complexes with transition metal ions and, at the same time, does not react and coordinate with lithium ions, and thus can improve the performance and safety of the battery by suppressing side reactions, in which some transition metals and transition metal ions such as Fe impurities, contained in a cathode, are oxidized and deposited on an anode when the battery is charged and discharged, as well as a lithium secondary battery comprising said electrolyte.
Technical Solution [71 To achieve the above object, the present invention provides an electrolyte for lithium secondary batteries, comprising: a chelating agent, which forms complexes with transition metal ions in the battery and, at the same time, does not react and coordinate with lithium ions; a non-aqueous solvent; and an electrolyte salt, as well as a lithium secondary battery comprising said electrolyte.
Brief Description of the Drawings [81 FIG. 1 is a graphic diagram showing the results of Fe electroplating experiments for batteries fabricated according to Example 1 of the present invention and Comparative Examples 1-3.
[91 FIG. 2 is a graphic diagram showing the results of Fe electroplating experiments for batteries fabricated according to Examples 1-5 of the present invention and Comparative Example 1.
[101 FIG. 3 is a graphic diagram showing the high-temperature storage characteristics of batteries fabricated according to Examples 6 and 7 of the present invention and Comparative Example 4.
[11] FIG. 4 is a graphic diagram showing the C-rate characteristics of batteries fabricated according to Examples 6 and 7 of the present invention and Comparative Example 4.
[121 FIG. 5 is a graphic diagram showing the cycle characteristics of batteries fabricated according to Examples 6 and 7 of the present invention and Comparative Example 4.
Mode for the Invention [131 Hereinafter, the present invention will be described in further detail.
[141 The present invention is characterized in that a chelating agent, which is not reactive with lithium ions and does not form coordinate bonds with lithium ions and thus does not form complexes with lithium ions, is selected and the selected chelating agent is used in a lithium secondary battery.
[151 The cathode of the lithium secondary battery generally contains lithium transition-metal oxides and, in some cases, Fe as an impurity. When this secondary battery is charged and discharged, side reactions can occur, in which transition metals such as Co, Mn and Ni, which can be contained in the cathode, or transition metals such as Fe impurities, are ionized, dissolved out from the cathode, and deposited on the anode.
COMPRISING CHELATING AGENT AND LITHIUM
SECONDARY BATTERY USING THE SAME
Technical Field Ill The present invention relates to an electrolyte for lithium secondary batteries containing a chelating agent, and a lithium secondary battery comprising said electrolyte.
Background Art [21 Recently, the compact and lightweight construction of electronic equipment has been realized and the use of portable electronic devices has been generalized, and thus studies on secondary batteries having high energy density have been actively conducted.
[31 Lithium secondary batteries, which are currently mainly used, comprise cathode and anode made of materials capable of intercalating and deintercalating lithium ions, are fabricated by injecting a non-aqueous electrolyte between the cathode and anode, and produce electrical energy by oxidation and reduction reactions, which occur when lithium ions are intercalated into and deintercalated from the cathode and anode.
[41 When the secondary battery is charged and discharged, transition metal ions in the battery can cause side reactions and can result in a reduction in the performance of the battery. For example, when the cathode contains Fe impurities, Fe can be ionized, and deposited on the anode, resulting in voltage drop. Also, some Co, which is used as the cathode active material, can be dissolved out and deposited on the anode, and when spinel Mn is used for the cathode, Mn can be dissolved. In addition, when a Fe olivine material is used, Fe can be dissolved out. Such side reactions deteriorate the stability and performance of the battery.
[51 In a prior attempt to suppress side reactions, an expensive apparatus for purifying raw materials is used, the pretreatment of raw materials is performed, or other al-ternative materials having poor performance are used. However, such methods have problems in that they are expensive and deteriorate the performance of the battery.
Disclosure of Invention Technical Problem [61 It is an object of the present invention to provide an electrolyte for lithium secondary batteries containing a chelating agent, which forms complexes with transition metal ions and, at the same time, does not react and coordinate with lithium ions, and thus can improve the performance and safety of the battery by suppressing side reactions, in which some transition metals and transition metal ions such as Fe impurities, contained in a cathode, are oxidized and deposited on an anode when the battery is charged and discharged, as well as a lithium secondary battery comprising said electrolyte.
Technical Solution [71 To achieve the above object, the present invention provides an electrolyte for lithium secondary batteries, comprising: a chelating agent, which forms complexes with transition metal ions in the battery and, at the same time, does not react and coordinate with lithium ions; a non-aqueous solvent; and an electrolyte salt, as well as a lithium secondary battery comprising said electrolyte.
Brief Description of the Drawings [81 FIG. 1 is a graphic diagram showing the results of Fe electroplating experiments for batteries fabricated according to Example 1 of the present invention and Comparative Examples 1-3.
[91 FIG. 2 is a graphic diagram showing the results of Fe electroplating experiments for batteries fabricated according to Examples 1-5 of the present invention and Comparative Example 1.
[101 FIG. 3 is a graphic diagram showing the high-temperature storage characteristics of batteries fabricated according to Examples 6 and 7 of the present invention and Comparative Example 4.
[11] FIG. 4 is a graphic diagram showing the C-rate characteristics of batteries fabricated according to Examples 6 and 7 of the present invention and Comparative Example 4.
[121 FIG. 5 is a graphic diagram showing the cycle characteristics of batteries fabricated according to Examples 6 and 7 of the present invention and Comparative Example 4.
Mode for the Invention [131 Hereinafter, the present invention will be described in further detail.
[141 The present invention is characterized in that a chelating agent, which is not reactive with lithium ions and does not form coordinate bonds with lithium ions and thus does not form complexes with lithium ions, is selected and the selected chelating agent is used in a lithium secondary battery.
[151 The cathode of the lithium secondary battery generally contains lithium transition-metal oxides and, in some cases, Fe as an impurity. When this secondary battery is charged and discharged, side reactions can occur, in which transition metals such as Co, Mn and Ni, which can be contained in the cathode, or transition metals such as Fe impurities, are ionized, dissolved out from the cathode, and deposited on the anode.
[161 When the electrolyte of the lithium secondary battery contains a chelating agent, the chelating agent will form coordinate bonds with the metal ions such as Co, Mn, Ni and Fe to form metal-containing cyclic complexes known as chelates. Also, the chelating agent, which is included in the inventive electrolyte, does not deteriorate the performance of the battery because it does not react and coordinate with lithium ions, so that it does not form complexes with lithium ions.
[171 Thus, because the chelating agent forms complexes with transition metal ions except for lithium ions in the battery, it significantly reduces the reactivity of the transition metal ions, so that it can suppress side reactions in which the transition metal ions are reduced and deposited as transition metals on the anode. Also, the chelating agent can suppress internal short-circuits in the battery and the resulting voltage drop of the battery and a reduction in the safety and performance of the battery, which can occur when transition metals are deposited on the anode.
[181 Also, in the present invention, complexes formed between the chelating agent and the transition metal ions are preferably insoluble in the electrolyte. When the complexes between the chelating agent and the transition metal ions are well soluble in the electrolyte, the complexes can migrate to the anode and can be reduced and deposited as transition metals on the surface of the anode.
[191 The chelating agent, which is contained in the inventive electrolyte for lithium secondary batteries, can be at least one selected from the group consisting of EDTA
(ethylene diamine tetraacetic acid), NTA (nitrilotriacetic acid), DCTA
(trans-1,2-diaminocyclohexanetetraacetic acid), DTPA (diethylene-triaminepentaacetic acid), and EGTA (ethylene glycol bis(2-aminoethyl ether)-N,N,N',N'-tetraacetic acid).
[201 The chelating agent can be contained in an amount of 2-200 mM relative to the electrolyte. If the chelating agent is contained in the electrolyte in an amount of less than 2 mM, it will be insignificant with respect to the effects of forming complexes by coordinate bonds between the chelating agent and the transition metal ions and suppressing the side reaction in which transition metals are deposited in the anode. On the other hand, if the chelating agent is contained in an amount of more than 200 mM, it will not have any further effect resulting from an increase in the amount of use of the chelating agent.
[211 The non-aqueous solvent, which is contained in the inventive electrolyte for lithium secondary batteries, is not specifically limited as long as it is generally used as a non-aqueous solvent for non-aqueous electrolytes. Examples of the non-aqueous solvent, which can be used in the present invention, include cyclic carbonate, linear carbonate, lactone, ether, ester, and ketone.
[221 Examples of the cyclic carbonate include ethylene carbonate (EC), propylene carbonate (PC), and butylene carbonate (BC), and examples of the linear carbonate include diethyl carbonate (DEC), dimethyl carbonate (DMC), dipropyl carbonate (DPC), ethyl methyl carbonate (EMC), and methyl propyl carbonate (MPC).
Examples of the lactone include gamma-butyrolactone (GBL), and examples of the ether include dibutyl ether, tetrahydrofuran, 2-methyl tetrahydrofuran, 1,4-dioxane, and 1,2-dimethoxyethane. Also, examples of the ester include methyl acetate, ethyl acetate, methyl propionate, and methyl pivalate, and examples of the ketone include poly-methylvinyl ketone. These non-aqueous solvents can be used alone or in a mixture of two or more thereof.
[231 The electrolyte salt, which is contained in the inventive electrolyte for lithium secondary batteries, is not specifically limited as long as it is generally used as an electrolyte salt for non-aqueous electrolytes. Non-limiting examples of the electrolyte salt include salts having a structure such as AAB-, wherein A+ represents an alkali metal cation such as Li+, Na+, K+, or a combination thereof, and if represents an anion such as PF -, BF -,CI-, Br,I-,CIO -, AsF -, CH CO -, CF SO -,N(CFSO) -,C(CFSO) -, or a combination thereof. Particularly, a lithium salt is preferred. These electrolyte salts can be used alone or in a mixture of two or more thereof.
[241 The lithium secondary battery according to the present invention can employ said electrolyte for lithium secondary batteries. Specifically, the lithium secondary battery according to the present invention can comprise a cathode; an anode; a separator; and said electrolyte for lithium secondary batteries.
[251 The lithium secondary battery of the present invention can be fabricated according to a conventional method known in the art by interposing a porous separator between the cathode and the anode, and placing said electrolyte into the resulting structure.
However, the method of fabricating the lithium secondary battery, which can be used in the present invention, is not limited to any particular method.
[261 The cathode active material, which is used in the secondary battery of the present invention, can consist of any one or a mixture of two or more selected from among a variety of lithium transition-metal composite oxides (e.g., lithium manganese composite oxide, lithium nickel oxide, lithium cobalt oxide, and the foregoing oxides wherein part of manganese, nickel and cobalt is replaced with other transition metals and the like such as LiCoO , LiNiO , LiMnO , LiMn 0 , Li(Ni Co Mn )O (0 < a <
1, 2 2 2 2 4 a b c 2 0 < b < 1, 0 < c < 1, a+b+c=1), LiNi 1-Y Co Y 0 2, LiCo 1-Y Mn Y 0 2 , LiNi 1-Y Mn Y 0 2 (0-Y < 1), Li(Ni Co Mn )O (0<a<2, 0 < b < 2, 0 < c < 2, a+b+c=2), LiMn Ni O , LiMn CoO
a b c 4 2-z z 4 2-z z 4 (0< Z < 2), LiCoPO4 or LiFePO4, or a lithium-containing vanadium oxide and the like), and chalcogen compounds (such as manganese dioxide, titanium disulfide, molybdenum disulfide and the like).
[271 The anode active material, which can be used in the present invention, can consist of a carbon material, a lithium metal or an alloy thereof, which can absorb and release lithium ions. In addition, it is possible to use a metal oxide such as TiO z or SnO z, which can absorb and release lithium ions and has a potential of less than 2V
for lithium. Particularly, a carbon material such as graphite is preferred.
[281 Although the porous separator, which can be used in the present invention, is not limited to any particular separator, a porous separator can be used, examples of which include polypropylene-based, polyethylene-based, and polyolefin-based porous separators.
[291 In addition, although the shape of the lithium secondary battery is not limited to any particular shape, it can have a cylindrical shape, a prismatic shape, a pouch shape or a coin shape.
[301 Hereinafter, the present invention will be described in further detail with reference to examples. It is to be understood, however, that these examples are illustrative only, and the scope of the present invention is not limited thereto.
[311 Example 1: Preparation of electrolyte and battery, containing EDTA as chelating agent [321 An electrolyte was prepared by dissolving LiPF6 in ethylene carbonate (EC): ethyl methyl carbonate (EMC)=1:2(v/v) to a concentration of 1M, and then adding each of Fe ions (FeC13) and EDTA as a chelating agent to a concentration of 50 mM.
[331 A battery was fabricated by using a nitric acid-treated silver wire as a reference electrode, a Pt wire as a counter electrode, a copper foil as a working electrode, and the above-prepared electrolyte as an electrolyte.
[341 Comparative Example 1: Preparation of electrolyte and battery containing no chelating agent [351 An electrolyte and a battery were prepared according to the same method as Example 1, except that the chelating agent (EDTA) was not added.
[361 Comparative Example 2: Preparation of electrolyte and battery containing 18-crown-6 as chelating agent [371 An electrolyte and a battery were prepared according to the same method as Example 1, except that 18-crown-6 (crown ether) was used instead of EDTA as a chelating agent.
[381 Comparative Example 3: Preparation of electrolyte and battery containing dibenzo-18-crown-6 as chelating agent [391 An electrolyte and a battery were prepared according to the same method as Example 1, except that dibenzo- 1 8-crown-6 (crown ether) was used instead of EDTA
as a chelating agent.
[401 Experiment 1: Test of Fe electroplating (reduction of Fe ions) [411 In order to observe reactions in which Fe ions in the electrolytes of batteries prepared in Example 1 and Comparative Examples 1-3 are reduced on the surface of the anode, electroplating experiments were carried out, and the experimental results are shown in FIG. 1.
[421 As can be seen in FIG. 1, in the case where crown ether was used as the chelating agent, Fe ions reacted well with the crown ether to form complexes, but it seems that the complexes were dissolved well in the electrolyte due to the property of the crown ether soluble in the organic solvent, so that they rather helped the Fe ions migrate to the anode and were reduced on the surface of the anode. As a result, this case was not different from the case where the chelating agent was not used. However, in the case where EDTA was used as the chelating agent, a reaction of less than 2V with respect to Li/Li+ ions did not substantially appear, suggesting that the EDTA effectively suppressed the reduction of Fe ions.
[431 Examples 2-5: Preparation of electrolytes and batteries containing EDTA
[441 Electrolytes and batteries were prepared according to the same method as Example 1, except that EDTA was added in amounts of 2 mM, 5 mM, 10 mM and 200 mM, re-spectively.
[451 Experiment 2: Reduction of Fe ions at varying EDTA concentrations [461 The reduction reactions of the batteries fabricated in Examples 1-5 and Comparative Example 1 on the surface of a copper foil and the amount of the resulting Fe electroplating were measured, and the measurement results are shown in FIG.
2.
[471 After Fe was electroplated while changing the amount of EDTA, the amount of Fe on the copper foil was analyzed using ICP. As a result, it could be seen that an increase in the amount of EDTA led to a decrease in the amount of the plated Fe. The values in brackets in FIG. 2 are the analyzed amounts of Fe, and it could be seen that, even though the amount of EDTA in the electrolytes was as low as ten times the amount of Fe ions, EDTA was significantly effective in inhibiting the reduction of Fe ions.
[481 Example 6: Preparation of electrolyte and polymer battery containing EDTA
[491 An electrolyte was prepared by adding EDTA to an electrolyte (EC/EMC=1/2(v/v), 1M LiPF6) for use in cylindrical batteries to a concentration of 2 mM.
[501 A cathode slurry was prepared by mixing together 90 wt% of LiCoO2 as a cathode active material, 5 wt% of acetylene black as a conductive agent, and 5 wt% of PVDF
as a binder, and then adding the mixture to NMP (N-methyl-2-pyrrolidone).
Then, the cathode slurry was applied on an aluminum (Al) current collector and dried, thus preparing a cathode.
[511 An anode slurry was prepared by adding a mixture of 95 wt% of graphite as an anode active material and 5 wt% of PVDF as a binder to NMP. Then, the anode slurry was applied on a copper (Cu) current collector and dried, thus preparing an anode.
[521 A polyolefin-based separator was interposed between the prepared cathode and anode, and then the electrolyte was injected into the resulting structure, thus fabricating an ICP563443 polymer battery (5.6 mm thick, 34 mm wide and 43 mm long) having a nominal capacity of 900 mAh.
[531 Example 7: Preparation of electrolyte and polymer battery containing EDTA
[541 An electrolyte and a polymer battery were prepared according to the same method as Example 6, except that EDTA was added to a concentration of 10 mM in the preparation of the electrolyte.
[551 Comparative Example 4: Preparation of electrolyte and polymer battery containing no EDTA
[561 An electrolyte and a polymer battery were prepared according to Example 6, except that EDTA was not added in the preparation of the electrolyte.
[571 Experiment 3: Evaluation of high-temperature storage characteristics of battery [581 Each of the batteries fabricated in Examples 6 and 7 and Comparative Example 4 was fully charged to 4.2 V, and placed in a constant-temperature chamber, in which the batteries were heated to 90 C over one hour, maintained at 90 C for 4 hours, cooled over one hour, and then maintained at room temperature. During this process, a change in the thickness of each of the batteries was measured, and the measurement results are shown in FIG. 3.
[591 The thickness of a battery during high-temperature generally becomes thicker due to the generation of gas resulting from the reaction of the electrolyte or the electrolyte additives on the electrode surface. However, an increase in the generation of gas, caused by the use of EDTA, could not be seen in the results of this Experiment. In other words, it could be found that the batteries containing EDTA and the battery containing no EDTA showed similar changes in the thickness thereof, and thus dete-rioration in the storage characteristics of the batteries caused by the use of EDTA, did not occur.
[601 Experiment 4: Evaluation of C-rate characteristics of batteries [611 The rate capabilities of the batteries fabricated in Examples 6 and 7 and Comparative Example 4 were measured at a charge condition of 0.5C and varying discharge currents, and the measurement results are shown in FIG. 4.
[621 In the case where EDTA was added, some deterioration in the performance of the batteries occurred at a high rate of 2 C, but was insignificant, and also had little variation between the batteries.
[631 Experiment 5: Evaluation of cycle characteristics of batteries [641 The cycle characteristics of the batteries fabricated in Examples 6 and 7 and Comparative Example 4 were tested, and the experimental results are shown in FIG. 5.
[651 As can be seen in FIG. 5, the batteries showed substantially the same behavior regardless of the amount of EDTA in 0.5C charge/iC discharge conditions and also showed good cycle characteristics.
[171 Thus, because the chelating agent forms complexes with transition metal ions except for lithium ions in the battery, it significantly reduces the reactivity of the transition metal ions, so that it can suppress side reactions in which the transition metal ions are reduced and deposited as transition metals on the anode. Also, the chelating agent can suppress internal short-circuits in the battery and the resulting voltage drop of the battery and a reduction in the safety and performance of the battery, which can occur when transition metals are deposited on the anode.
[181 Also, in the present invention, complexes formed between the chelating agent and the transition metal ions are preferably insoluble in the electrolyte. When the complexes between the chelating agent and the transition metal ions are well soluble in the electrolyte, the complexes can migrate to the anode and can be reduced and deposited as transition metals on the surface of the anode.
[191 The chelating agent, which is contained in the inventive electrolyte for lithium secondary batteries, can be at least one selected from the group consisting of EDTA
(ethylene diamine tetraacetic acid), NTA (nitrilotriacetic acid), DCTA
(trans-1,2-diaminocyclohexanetetraacetic acid), DTPA (diethylene-triaminepentaacetic acid), and EGTA (ethylene glycol bis(2-aminoethyl ether)-N,N,N',N'-tetraacetic acid).
[201 The chelating agent can be contained in an amount of 2-200 mM relative to the electrolyte. If the chelating agent is contained in the electrolyte in an amount of less than 2 mM, it will be insignificant with respect to the effects of forming complexes by coordinate bonds between the chelating agent and the transition metal ions and suppressing the side reaction in which transition metals are deposited in the anode. On the other hand, if the chelating agent is contained in an amount of more than 200 mM, it will not have any further effect resulting from an increase in the amount of use of the chelating agent.
[211 The non-aqueous solvent, which is contained in the inventive electrolyte for lithium secondary batteries, is not specifically limited as long as it is generally used as a non-aqueous solvent for non-aqueous electrolytes. Examples of the non-aqueous solvent, which can be used in the present invention, include cyclic carbonate, linear carbonate, lactone, ether, ester, and ketone.
[221 Examples of the cyclic carbonate include ethylene carbonate (EC), propylene carbonate (PC), and butylene carbonate (BC), and examples of the linear carbonate include diethyl carbonate (DEC), dimethyl carbonate (DMC), dipropyl carbonate (DPC), ethyl methyl carbonate (EMC), and methyl propyl carbonate (MPC).
Examples of the lactone include gamma-butyrolactone (GBL), and examples of the ether include dibutyl ether, tetrahydrofuran, 2-methyl tetrahydrofuran, 1,4-dioxane, and 1,2-dimethoxyethane. Also, examples of the ester include methyl acetate, ethyl acetate, methyl propionate, and methyl pivalate, and examples of the ketone include poly-methylvinyl ketone. These non-aqueous solvents can be used alone or in a mixture of two or more thereof.
[231 The electrolyte salt, which is contained in the inventive electrolyte for lithium secondary batteries, is not specifically limited as long as it is generally used as an electrolyte salt for non-aqueous electrolytes. Non-limiting examples of the electrolyte salt include salts having a structure such as AAB-, wherein A+ represents an alkali metal cation such as Li+, Na+, K+, or a combination thereof, and if represents an anion such as PF -, BF -,CI-, Br,I-,CIO -, AsF -, CH CO -, CF SO -,N(CFSO) -,C(CFSO) -, or a combination thereof. Particularly, a lithium salt is preferred. These electrolyte salts can be used alone or in a mixture of two or more thereof.
[241 The lithium secondary battery according to the present invention can employ said electrolyte for lithium secondary batteries. Specifically, the lithium secondary battery according to the present invention can comprise a cathode; an anode; a separator; and said electrolyte for lithium secondary batteries.
[251 The lithium secondary battery of the present invention can be fabricated according to a conventional method known in the art by interposing a porous separator between the cathode and the anode, and placing said electrolyte into the resulting structure.
However, the method of fabricating the lithium secondary battery, which can be used in the present invention, is not limited to any particular method.
[261 The cathode active material, which is used in the secondary battery of the present invention, can consist of any one or a mixture of two or more selected from among a variety of lithium transition-metal composite oxides (e.g., lithium manganese composite oxide, lithium nickel oxide, lithium cobalt oxide, and the foregoing oxides wherein part of manganese, nickel and cobalt is replaced with other transition metals and the like such as LiCoO , LiNiO , LiMnO , LiMn 0 , Li(Ni Co Mn )O (0 < a <
1, 2 2 2 2 4 a b c 2 0 < b < 1, 0 < c < 1, a+b+c=1), LiNi 1-Y Co Y 0 2, LiCo 1-Y Mn Y 0 2 , LiNi 1-Y Mn Y 0 2 (0-Y < 1), Li(Ni Co Mn )O (0<a<2, 0 < b < 2, 0 < c < 2, a+b+c=2), LiMn Ni O , LiMn CoO
a b c 4 2-z z 4 2-z z 4 (0< Z < 2), LiCoPO4 or LiFePO4, or a lithium-containing vanadium oxide and the like), and chalcogen compounds (such as manganese dioxide, titanium disulfide, molybdenum disulfide and the like).
[271 The anode active material, which can be used in the present invention, can consist of a carbon material, a lithium metal or an alloy thereof, which can absorb and release lithium ions. In addition, it is possible to use a metal oxide such as TiO z or SnO z, which can absorb and release lithium ions and has a potential of less than 2V
for lithium. Particularly, a carbon material such as graphite is preferred.
[281 Although the porous separator, which can be used in the present invention, is not limited to any particular separator, a porous separator can be used, examples of which include polypropylene-based, polyethylene-based, and polyolefin-based porous separators.
[291 In addition, although the shape of the lithium secondary battery is not limited to any particular shape, it can have a cylindrical shape, a prismatic shape, a pouch shape or a coin shape.
[301 Hereinafter, the present invention will be described in further detail with reference to examples. It is to be understood, however, that these examples are illustrative only, and the scope of the present invention is not limited thereto.
[311 Example 1: Preparation of electrolyte and battery, containing EDTA as chelating agent [321 An electrolyte was prepared by dissolving LiPF6 in ethylene carbonate (EC): ethyl methyl carbonate (EMC)=1:2(v/v) to a concentration of 1M, and then adding each of Fe ions (FeC13) and EDTA as a chelating agent to a concentration of 50 mM.
[331 A battery was fabricated by using a nitric acid-treated silver wire as a reference electrode, a Pt wire as a counter electrode, a copper foil as a working electrode, and the above-prepared electrolyte as an electrolyte.
[341 Comparative Example 1: Preparation of electrolyte and battery containing no chelating agent [351 An electrolyte and a battery were prepared according to the same method as Example 1, except that the chelating agent (EDTA) was not added.
[361 Comparative Example 2: Preparation of electrolyte and battery containing 18-crown-6 as chelating agent [371 An electrolyte and a battery were prepared according to the same method as Example 1, except that 18-crown-6 (crown ether) was used instead of EDTA as a chelating agent.
[381 Comparative Example 3: Preparation of electrolyte and battery containing dibenzo-18-crown-6 as chelating agent [391 An electrolyte and a battery were prepared according to the same method as Example 1, except that dibenzo- 1 8-crown-6 (crown ether) was used instead of EDTA
as a chelating agent.
[401 Experiment 1: Test of Fe electroplating (reduction of Fe ions) [411 In order to observe reactions in which Fe ions in the electrolytes of batteries prepared in Example 1 and Comparative Examples 1-3 are reduced on the surface of the anode, electroplating experiments were carried out, and the experimental results are shown in FIG. 1.
[421 As can be seen in FIG. 1, in the case where crown ether was used as the chelating agent, Fe ions reacted well with the crown ether to form complexes, but it seems that the complexes were dissolved well in the electrolyte due to the property of the crown ether soluble in the organic solvent, so that they rather helped the Fe ions migrate to the anode and were reduced on the surface of the anode. As a result, this case was not different from the case where the chelating agent was not used. However, in the case where EDTA was used as the chelating agent, a reaction of less than 2V with respect to Li/Li+ ions did not substantially appear, suggesting that the EDTA effectively suppressed the reduction of Fe ions.
[431 Examples 2-5: Preparation of electrolytes and batteries containing EDTA
[441 Electrolytes and batteries were prepared according to the same method as Example 1, except that EDTA was added in amounts of 2 mM, 5 mM, 10 mM and 200 mM, re-spectively.
[451 Experiment 2: Reduction of Fe ions at varying EDTA concentrations [461 The reduction reactions of the batteries fabricated in Examples 1-5 and Comparative Example 1 on the surface of a copper foil and the amount of the resulting Fe electroplating were measured, and the measurement results are shown in FIG.
2.
[471 After Fe was electroplated while changing the amount of EDTA, the amount of Fe on the copper foil was analyzed using ICP. As a result, it could be seen that an increase in the amount of EDTA led to a decrease in the amount of the plated Fe. The values in brackets in FIG. 2 are the analyzed amounts of Fe, and it could be seen that, even though the amount of EDTA in the electrolytes was as low as ten times the amount of Fe ions, EDTA was significantly effective in inhibiting the reduction of Fe ions.
[481 Example 6: Preparation of electrolyte and polymer battery containing EDTA
[491 An electrolyte was prepared by adding EDTA to an electrolyte (EC/EMC=1/2(v/v), 1M LiPF6) for use in cylindrical batteries to a concentration of 2 mM.
[501 A cathode slurry was prepared by mixing together 90 wt% of LiCoO2 as a cathode active material, 5 wt% of acetylene black as a conductive agent, and 5 wt% of PVDF
as a binder, and then adding the mixture to NMP (N-methyl-2-pyrrolidone).
Then, the cathode slurry was applied on an aluminum (Al) current collector and dried, thus preparing a cathode.
[511 An anode slurry was prepared by adding a mixture of 95 wt% of graphite as an anode active material and 5 wt% of PVDF as a binder to NMP. Then, the anode slurry was applied on a copper (Cu) current collector and dried, thus preparing an anode.
[521 A polyolefin-based separator was interposed between the prepared cathode and anode, and then the electrolyte was injected into the resulting structure, thus fabricating an ICP563443 polymer battery (5.6 mm thick, 34 mm wide and 43 mm long) having a nominal capacity of 900 mAh.
[531 Example 7: Preparation of electrolyte and polymer battery containing EDTA
[541 An electrolyte and a polymer battery were prepared according to the same method as Example 6, except that EDTA was added to a concentration of 10 mM in the preparation of the electrolyte.
[551 Comparative Example 4: Preparation of electrolyte and polymer battery containing no EDTA
[561 An electrolyte and a polymer battery were prepared according to Example 6, except that EDTA was not added in the preparation of the electrolyte.
[571 Experiment 3: Evaluation of high-temperature storage characteristics of battery [581 Each of the batteries fabricated in Examples 6 and 7 and Comparative Example 4 was fully charged to 4.2 V, and placed in a constant-temperature chamber, in which the batteries were heated to 90 C over one hour, maintained at 90 C for 4 hours, cooled over one hour, and then maintained at room temperature. During this process, a change in the thickness of each of the batteries was measured, and the measurement results are shown in FIG. 3.
[591 The thickness of a battery during high-temperature generally becomes thicker due to the generation of gas resulting from the reaction of the electrolyte or the electrolyte additives on the electrode surface. However, an increase in the generation of gas, caused by the use of EDTA, could not be seen in the results of this Experiment. In other words, it could be found that the batteries containing EDTA and the battery containing no EDTA showed similar changes in the thickness thereof, and thus dete-rioration in the storage characteristics of the batteries caused by the use of EDTA, did not occur.
[601 Experiment 4: Evaluation of C-rate characteristics of batteries [611 The rate capabilities of the batteries fabricated in Examples 6 and 7 and Comparative Example 4 were measured at a charge condition of 0.5C and varying discharge currents, and the measurement results are shown in FIG. 4.
[621 In the case where EDTA was added, some deterioration in the performance of the batteries occurred at a high rate of 2 C, but was insignificant, and also had little variation between the batteries.
[631 Experiment 5: Evaluation of cycle characteristics of batteries [641 The cycle characteristics of the batteries fabricated in Examples 6 and 7 and Comparative Example 4 were tested, and the experimental results are shown in FIG. 5.
[651 As can be seen in FIG. 5, the batteries showed substantially the same behavior regardless of the amount of EDTA in 0.5C charge/iC discharge conditions and also showed good cycle characteristics.
Industrial Applicability [66] As can be seen from the foregoing, the chelating agent, which is contained in the inventive electrolyte for lithium secondary batteries, forms complexes with transition metal ions in the battery and, at the same time, does not react and coordinate with lithium ions, and thus can suppress a side reaction in which transition metal ions are reduced and deposited as transition metals on the anode. Also, the chelating agent can suppress internal short-circuits in the battery and the resulting voltage drop of the battery, and a reduction in the safety and performance of the battery, which can occur when transition metals are deposited on. the anode.
[67] Although the preferred embodiment of the present invention has been described for illustrative purposes, those skilled in the art will appreciate that various modifications, additions and substitutions are possible, without departing from the scope of the invention as disclosed in the accompanying claims.
[67] Although the preferred embodiment of the present invention has been described for illustrative purposes, those skilled in the art will appreciate that various modifications, additions and substitutions are possible, without departing from the scope of the invention as disclosed in the accompanying claims.
Claims (4)
1. An electrolyte for lithium secondary batteries comprising: a chelating agent, which forms complexes with transition metal ions in the battery, and at the same time does not react and coordinate with lithium ions; a non-aqueous solvent; and an electrolyte salt, wherein the chelating agent is at least one selected from the group consisting of NTA
(nitrilotriacetic acid), DCTA (trans-1,2-diaminocyclohexanetetraacetic acid), DTPA (diethylene-triaminepentaacetic acid), and EGTA (ethylene glycol bis(2-aminoethyl ether)-N,N,N',N'-tetraacetic acid).
(nitrilotriacetic acid), DCTA (trans-1,2-diaminocyclohexanetetraacetic acid), DTPA (diethylene-triaminepentaacetic acid), and EGTA (ethylene glycol bis(2-aminoethyl ether)-N,N,N',N'-tetraacetic acid).
2. The electrolyte of Claim 1, wherein the complexes are insoluble in the electrolyte.
3. The electrolyte of Claim 1, wherein the chelating agent is contained in an amount of 2 to 200 mM relative to the electrolyte.
4. A lithium secondary battery comprising an electrolyte according to any one of Claims 1-3.
Applications Claiming Priority (3)
| Application Number | Priority Date | Filing Date | Title |
|---|---|---|---|
| KR10-2005-0116827 | 2005-12-02 | ||
| KR1020050116827A KR20070057405A (en) | 2005-12-02 | 2005-12-02 | Electrolyte for lithium secondary battery containing chelating agent and lithium secondary battery using same |
| PCT/KR2006/005152 WO2007064170A1 (en) | 2005-12-02 | 2006-12-01 | Electrolyte for lithium secondary battery comprising chelating agent and lithium secondary battery using the same |
Publications (2)
| Publication Number | Publication Date |
|---|---|
| CA2632868A1 CA2632868A1 (en) | 2007-06-07 |
| CA2632868C true CA2632868C (en) | 2011-09-20 |
Family
ID=38092460
Family Applications (1)
| Application Number | Title | Priority Date | Filing Date |
|---|---|---|---|
| CA2632868A Active CA2632868C (en) | 2005-12-02 | 2006-12-01 | Electrolyte for lithium secondary battery comprising chelating agent and lithium secondary battery using the same |
Country Status (7)
| Country | Link |
|---|---|
| US (2) | US7745056B2 (en) |
| JP (1) | JP5507083B2 (en) |
| KR (1) | KR20070057405A (en) |
| CN (1) | CN101322277B (en) |
| CA (1) | CA2632868C (en) |
| TW (1) | TWI344713B (en) |
| WO (1) | WO2007064170A1 (en) |
Families Citing this family (38)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| AU2010266488B2 (en) * | 2009-07-01 | 2014-05-29 | Energizer Brands, Llc | Removal of impurities from lithium-iron disulfide electrochemical cells |
| US8785054B2 (en) | 2009-12-18 | 2014-07-22 | GM Global Technology Operations LLC | Lithium ion battery |
| JP2011192634A (en) * | 2010-02-17 | 2011-09-29 | Sanyo Electric Co Ltd | Nonaqueous electrolyte secondary battery |
| US8765301B2 (en) | 2010-10-01 | 2014-07-01 | GM Global Technology Operations LLC | Lithium ion battery |
| CN102569723A (en) * | 2012-02-13 | 2012-07-11 | 华为技术有限公司 | Lithium ion battery positive electrode material and preparation method thereof, positive electrode and lithium ion battery |
| JP6206639B2 (en) | 2012-04-02 | 2017-10-04 | 日産自動車株式会社 | Electrolyte for lithium ion secondary battery and lithium ion secondary battery |
| US9382274B2 (en) | 2012-07-27 | 2016-07-05 | Lockheed Martin Advanced Energy Storage, Llc | Aqueous redox flow batteries featuring improved cell design characteristics |
| US8753761B2 (en) | 2012-07-27 | 2014-06-17 | Sun Catalytix Corporation | Aqueous redox flow batteries comprising metal ligand coordination compounds |
| US9559374B2 (en) | 2012-07-27 | 2017-01-31 | Lockheed Martin Advanced Energy Storage, Llc | Electrochemical energy storage systems and methods featuring large negative half-cell potentials |
| US9865893B2 (en) | 2012-07-27 | 2018-01-09 | Lockheed Martin Advanced Energy Storage, Llc | Electrochemical energy storage systems and methods featuring optimal membrane systems |
| US9692077B2 (en) | 2012-07-27 | 2017-06-27 | Lockheed Martin Advanced Energy Storage, Llc | Aqueous redox flow batteries comprising matched ionomer membranes |
| US9899694B2 (en) | 2012-07-27 | 2018-02-20 | Lockheed Martin Advanced Energy Storage, Llc | Electrochemical energy storage systems and methods featuring high open circuit potential |
| US9768463B2 (en) | 2012-07-27 | 2017-09-19 | Lockheed Martin Advanced Energy Storage, Llc | Aqueous redox flow batteries comprising metal ligand coordination compounds |
| US10164284B2 (en) | 2012-07-27 | 2018-12-25 | Lockheed Martin Energy, Llc | Aqueous redox flow batteries featuring improved cell design characteristics |
| US8691413B2 (en) | 2012-07-27 | 2014-04-08 | Sun Catalytix Corporation | Aqueous redox flow batteries featuring improved cell design characteristics |
| CN103413968A (en) * | 2012-11-20 | 2013-11-27 | 浙江普耐德新能源科技有限公司 | Lithium battery electrolyte and lithium battery comprising same |
| DK3224266T3 (en) | 2014-11-26 | 2021-04-26 | Lockheed Martin Energy Llc | Metal complexes of substituted catecholates and redox flow batteries containing these |
| US10253051B2 (en) | 2015-03-16 | 2019-04-09 | Lockheed Martin Energy, Llc | Preparation of titanium catecholate complexes in aqueous solution using titanium tetrachloride or titanium oxychloride |
| CN104900916A (en) * | 2015-06-26 | 2015-09-09 | 广州天赐高新材料股份有限公司 | Electrolyte solution for high-capacity lithium-ion battery, preparation method and lithium-ion battery |
| US10316047B2 (en) | 2016-03-03 | 2019-06-11 | Lockheed Martin Energy, Llc | Processes for forming coordination complexes containing monosulfonated catecholate ligands |
| US10644342B2 (en) | 2016-03-03 | 2020-05-05 | Lockheed Martin Energy, Llc | Coordination complexes containing monosulfonated catecholate ligands and methods for producing the same |
| US9938308B2 (en) | 2016-04-07 | 2018-04-10 | Lockheed Martin Energy, Llc | Coordination compounds having redox non-innocent ligands and flow batteries containing the same |
| US10343964B2 (en) | 2016-07-26 | 2019-07-09 | Lockheed Martin Energy, Llc | Processes for forming titanium catechol complexes |
| US10377687B2 (en) | 2016-07-26 | 2019-08-13 | Lockheed Martin Energy, Llc | Processes for forming titanium catechol complexes |
| US10065977B2 (en) | 2016-10-19 | 2018-09-04 | Lockheed Martin Advanced Energy Storage, Llc | Concerted processes for forming 1,2,4-trihydroxybenzene from hydroquinone |
| US10930937B2 (en) | 2016-11-23 | 2021-02-23 | Lockheed Martin Energy, Llc | Flow batteries incorporating active materials containing doubly bridged aromatic groups |
| EP3555939B1 (en) * | 2016-12-13 | 2025-02-05 | Henkel AG & Co. KGaA | Improved secondary li ion battery and li capacitor electrode compositions |
| US10497958B2 (en) | 2016-12-14 | 2019-12-03 | Lockheed Martin Energy, Llc | Coordinatively unsaturated titanium catecholate complexes and processes associated therewith |
| US10741864B2 (en) | 2016-12-30 | 2020-08-11 | Lockheed Martin Energy, Llc | Aqueous methods for forming titanium catecholate complexes and associated compositions |
| US10320023B2 (en) | 2017-02-16 | 2019-06-11 | Lockheed Martin Energy, Llc | Neat methods for forming titanium catecholate complexes and associated compositions |
| KR102039336B1 (en) * | 2019-07-31 | 2019-11-01 | 주식회사 로브 | Eco-friendly method for manufacturing Ni-Co-Mn composite precursor using organic chelating agent |
| EP4088334A4 (en) * | 2020-01-06 | 2025-01-08 | L3Harris Open Water Power, Inc. | ELECTROLYTE ENGINEERING PROCESSES AND SYSTEMS |
| JP6930641B1 (en) | 2020-07-16 | 2021-09-01 | 住友大阪セメント株式会社 | Metal adsorbent-supporting carbon material for lithium-ion secondary batteries, positive electrode material for lithium-ion secondary batteries, positive electrode for lithium-ion secondary batteries, lithium-ion secondary batteries |
| KR102843861B1 (en) * | 2020-11-30 | 2025-08-06 | 주식회사 엘지화학 | A solid electrolyte material for all solid-state battery and an all solid-state battery comprising the same |
| CN112626344A (en) * | 2020-12-16 | 2021-04-09 | 武汉工程大学 | Method for recovering Li and Co in lithium battery positive electrode material by using polyethylene glycol dicarboxylic acid |
| EP4318631A4 (en) | 2021-03-31 | 2025-01-22 | Panasonic Intellectual Property Management Co., Ltd. | NEGATIVE ELECTRODE FOR NONAQUEOUS ELECTROLYTE SECONDARY BATTERIES, SEPARATOR FOR NONAQUEOUS ELECTROLYTE SECONDARY BATTERIES, AND NONAQUEOUS ELECTROLYTE SECONDARY BATTERY |
| US20230095171A1 (en) * | 2021-09-01 | 2023-03-30 | Enevate Corporation | Organic acid additives for silicon-based li ion batteries |
| KR20240064423A (en) * | 2022-11-04 | 2024-05-13 | 주식회사 엘지에너지솔루션 | Lithium secondary battery |
Family Cites Families (12)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| US4670363A (en) | 1986-09-22 | 1987-06-02 | Duracell Inc. | Non-aqueous electrochemical cell |
| JP2871065B2 (en) * | 1990-10-29 | 1999-03-17 | 松下電器産業株式会社 | Metal oxide-hydrogen storage battery |
| JP3028622B2 (en) * | 1991-03-14 | 2000-04-04 | 松下電器産業株式会社 | Method for producing hydrogen storage electrode and metal oxide-hydrogen storage battery |
| JPH07211351A (en) * | 1994-01-20 | 1995-08-11 | Sony Corp | Non-aqueous electrolyte for secondary batteries |
| JP2000195548A (en) * | 1998-10-19 | 2000-07-14 | Shin Kobe Electric Mach Co Ltd | Non-aqueous electrolyte secondary battery |
| JP3498905B2 (en) | 1999-08-02 | 2004-02-23 | セントラル硝子株式会社 | Electrolyte for electrochemical devices |
| JP2001210366A (en) * | 2000-01-26 | 2001-08-03 | Matsushita Electric Ind Co Ltd | Non-aqueous electrochemical device and its electrolyte |
| KR100422942B1 (en) * | 2001-05-22 | 2004-03-18 | 주식회사 엘지화학 | Non-aqueous electrolyte additive enhancing safety and lithium ion secondary battery comprising the same |
| JP2004063123A (en) | 2002-07-25 | 2004-02-26 | Japan Storage Battery Co Ltd | Non-aqueous electrolyte secondary battery |
| JP4522683B2 (en) * | 2003-10-09 | 2010-08-11 | 住友大阪セメント株式会社 | Method for producing electrode material powder, electrode material powder and electrode, and lithium battery |
| JP2005259635A (en) | 2004-03-15 | 2005-09-22 | Japan Storage Battery Co Ltd | Nonaqueous electrolyte secondary battery |
| KR101191636B1 (en) | 2005-02-28 | 2012-10-18 | 삼성에스디아이 주식회사 | Electrolyte for lithium battery and lithium battery comprising same |
-
2005
- 2005-12-02 KR KR1020050116827A patent/KR20070057405A/en not_active Ceased
-
2006
- 2006-12-01 CA CA2632868A patent/CA2632868C/en active Active
- 2006-12-01 JP JP2008543203A patent/JP5507083B2/en active Active
- 2006-12-01 CN CN2006800453185A patent/CN101322277B/en active Active
- 2006-12-01 WO PCT/KR2006/005152 patent/WO2007064170A1/en not_active Ceased
- 2006-12-01 US US12/095,845 patent/US7745056B2/en active Active
- 2006-12-01 TW TW095144632A patent/TWI344713B/en active
-
2010
- 2010-03-08 US US12/719,138 patent/US20100159321A1/en not_active Abandoned
Also Published As
| Publication number | Publication date |
|---|---|
| CN101322277A (en) | 2008-12-10 |
| CA2632868A1 (en) | 2007-06-07 |
| TWI344713B (en) | 2011-07-01 |
| JP2009517836A (en) | 2009-04-30 |
| KR20070057405A (en) | 2007-06-07 |
| CN101322277B (en) | 2011-02-16 |
| US7745056B2 (en) | 2010-06-29 |
| WO2007064170A1 (en) | 2007-06-07 |
| JP5507083B2 (en) | 2014-05-28 |
| TW200723572A (en) | 2007-06-16 |
| US20100159321A1 (en) | 2010-06-24 |
| US20080280211A1 (en) | 2008-11-13 |
Similar Documents
| Publication | Publication Date | Title |
|---|---|---|
| CA2632868C (en) | Electrolyte for lithium secondary battery comprising chelating agent and lithium secondary battery using the same | |
| KR102633527B1 (en) | Non-aqueous electrolyte for lithium secondary battery and lithium secondary battery comprising the same | |
| CN101297433B (en) | Inhibitor of redox interaction additive life cycle reduction and nonaqueous electrolyte and secondary battery containing the same | |
| JP7713540B2 (en) | Electrochemical and Electronic Devices | |
| KR102117622B1 (en) | Electrolyte for lithium secondary battery and lithium secondary battery comprising the same | |
| US20100190064A1 (en) | Nonaqueous electrolyte secondary battery | |
| JP2021501978A (en) | Non-aqueous electrolyte solution for lithium secondary battery and lithium secondary battery containing it | |
| JP2010153258A (en) | Nonaqueous electrolyte battery | |
| US20100248022A1 (en) | Nonaqueous electrolyte secondary battery | |
| JP2003282055A (en) | Non-aqueous electrolyte secondary battery | |
| JP2005235624A (en) | Method for producing non-aqueous electrolyte secondary battery | |
| US9337479B2 (en) | Nonaqueous electrolyte secondary battery | |
| EP2284934B1 (en) | Electrode assembly and lithium secondary battery including the same | |
| JP2014067629A (en) | Nonaqueous electrolyte secondary battery | |
| EP2259375B1 (en) | Nonaqueous electrolytic solution and lithium secondary battery | |
| KR102940360B1 (en) | Nonaqueous electrolyte for lithium secondary battery and lithium secondary battery comprising the same | |
| EP1961068B1 (en) | Non-aqueous electrolyte and secondary battery comprising the same | |
| US20140203787A1 (en) | Nonaqueous electrolyte secondary battery | |
| EP1734607A1 (en) | Nonaqueous electrolyte secondary battery | |
| JP2010238451A (en) | Nonaqueous electrolyte secondary battery | |
| KR20200080170A (en) | Electrolyte for lithium secondary battery and lithium secondary battery comprising the same | |
| KR100725704B1 (en) | Non-aqueous electrolyte additive and secondary battery using same | |
| JP4826760B2 (en) | Non-aqueous electrolyte and lithium secondary battery using the same | |
| JP5070780B2 (en) | Non-aqueous electrolyte and lithium secondary battery using the same | |
| JP2008097954A (en) | Electrolyte and battery |
Legal Events
| Date | Code | Title | Description |
|---|---|---|---|
| EEER | Examination request | ||
| MPN | Maintenance fee for patent paid |
Free format text: FEE DESCRIPTION TEXT: MF (PATENT, 18TH ANNIV.) - STANDARD Year of fee payment: 18 |
|
| U00 | Fee paid |
Free format text: ST27 STATUS EVENT CODE: A-4-4-U10-U00-U101 (AS PROVIDED BY THE NATIONAL OFFICE); EVENT TEXT: MAINTENANCE REQUEST RECEIVED Effective date: 20241120 |
|
| U11 | Full renewal or maintenance fee paid |
Free format text: ST27 STATUS EVENT CODE: A-4-4-U10-U11-U102 (AS PROVIDED BY THE NATIONAL OFFICE); EVENT TEXT: MAINTENANCE FEE PAYMENT DETERMINED COMPLIANT Effective date: 20241120 Free format text: ST27 STATUS EVENT CODE: A-4-4-U10-U11-U102 (AS PROVIDED BY THE NATIONAL OFFICE); EVENT TEXT: MAINTENANCE FEE PAYMENT PAID IN FULL Effective date: 20241120 |
|
| MPN | Maintenance fee for patent paid |
Free format text: FEE DESCRIPTION TEXT: MF (PATENT, 19TH ANNIV.) - STANDARD Year of fee payment: 19 |
|
| U00 | Fee paid |
Free format text: ST27 STATUS EVENT CODE: A-4-4-U10-U00-U101 (AS PROVIDED BY THE NATIONAL OFFICE); EVENT TEXT: MAINTENANCE REQUEST RECEIVED Effective date: 20251125 |
|
| U11 | Full renewal or maintenance fee paid |
Free format text: ST27 STATUS EVENT CODE: A-4-4-U10-U11-U102 (AS PROVIDED BY THE NATIONAL OFFICE); EVENT TEXT: MAINTENANCE FEE PAYMENT PAID IN FULL Effective date: 20251125 |