WO2005096417A1 - レドックス活性可逆電極およびそれを用いた二次電池 - Google Patents
レドックス活性可逆電極およびそれを用いた二次電池 Download PDFInfo
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- WO2005096417A1 WO2005096417A1 PCT/JP2005/005953 JP2005005953W WO2005096417A1 WO 2005096417 A1 WO2005096417 A1 WO 2005096417A1 JP 2005005953 W JP2005005953 W JP 2005005953W WO 2005096417 A1 WO2005096417 A1 WO 2005096417A1
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- H01M4/13—Electrodes for accumulators with non-aqueous electrolyte, e.g. for lithium-accumulators; Processes of manufacture thereof
- H01M4/136—Electrodes based on inorganic compounds other than oxides or hydroxides, e.g. sulfides, selenides, tellurides, halogenides or LiCoFy
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- H01M4/36—Selection of substances as active materials, active masses, active liquids
- H01M4/48—Selection of substances as active materials, active masses, active liquids of inorganic oxides or hydroxides
- H01M4/485—Selection of substances as active materials, active masses, active liquids of inorganic oxides or hydroxides of mixed oxides or hydroxides for inserting or intercalating light metals, e.g. LiTi2O4 or LiTi2OxFy
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- H01M4/36—Selection of substances as active materials, active masses, active liquids
- H01M4/58—Selection of substances as active materials, active masses, active liquids of inorganic compounds other than oxides or hydroxides, e.g. sulfides, selenides, tellurides, halogenides or LiCoFy; of polyanionic structures, e.g. phosphates, silicates or borates
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- H01M10/0525—Rocking-chair batteries, i.e. batteries with lithium insertion or intercalation in both electrodes; Lithium-ion batteries
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- H01M4/13—Electrodes for accumulators with non-aqueous electrolyte, e.g. for lithium-accumulators; Processes of manufacture thereof
- H01M4/131—Electrodes based on mixed oxides or hydroxides, or on mixtures of oxides or hydroxides, e.g. LiCoOx
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- H01M4/13—Electrodes for accumulators with non-aqueous electrolyte, e.g. for lithium-accumulators; Processes of manufacture thereof
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- H01M4/36—Selection of substances as active materials, active masses, active liquids
- H01M4/48—Selection of substances as active materials, active masses, active liquids of inorganic oxides or hydroxides
- H01M4/50—Selection of substances as active materials, active masses, active liquids of inorganic oxides or hydroxides of manganese
- H01M4/505—Selection of substances as active materials, active masses, active liquids of inorganic oxides or hydroxides of manganese of mixed oxides or hydroxides containing manganese for inserting or intercalating light metals, e.g. LiMn2O4 or LiMn2OxFy
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- H01M4/36—Selection of substances as active materials, active masses, active liquids
- H01M4/48—Selection of substances as active materials, active masses, active liquids of inorganic oxides or hydroxides
- H01M4/52—Selection of substances as active materials, active masses, active liquids of inorganic oxides or hydroxides of nickel, cobalt or iron
- H01M4/525—Selection of substances as active materials, active masses, active liquids of inorganic oxides or hydroxides of nickel, cobalt or iron of mixed oxides or hydroxides containing iron, cobalt or nickel for inserting or intercalating light metals, e.g. LiNiO2, LiCoO2 or LiCoOxFy
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- H01M4/62—Selection of inactive substances as ingredients for active masses, e.g. binders, fillers
- H01M4/624—Electric conductive fillers
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- Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
- Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
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- Y02T10/00—Road transport of goods or passengers
- Y02T10/60—Other road transportation technologies with climate change mitigation effect
- Y02T10/70—Energy storage systems for electromobility, e.g. batteries
Definitions
- the present invention relates to a redox activity (redox activity) used for an electrochemical device such as a battery.
- the present invention relates to a reversible electrode and a secondary battery using the same, and more particularly, to a redox active electrode having a redox active film on a conductive substrate capable of performing a rapid electron and charge transfer reaction, and a lithium secondary battery using the same.
- the present invention relates to a secondary battery and a magnesium secondary battery.
- the present invention particularly relates to a lithium secondary battery or a magnesium secondary battery suitable as a power source for a mobile phone or an electric vehicle requiring a high energy density, and a positive electrode used therein.
- LiCoO lithium cobaltate
- Li nickelate lithium nickelate
- Lithium-based inorganic metal oxides such as lithium (LiNiO) and lithium manganate (LiMnO)
- the cathode material is 100 to 150 AhZkg, while the anode material is more than three times (370 to 800 AhZkg for carbon material)!
- a sulfur-based material exhibits redox reaction activity, has a high energy density, and has a high energy storage capacity. This is because the atomic weight of the sulfur atom at the center of the redox is 32, smaller than that of cobalt (59), nickel (59), and manganese (55), and its oxidation number ranges from -2 to +6. The possibility of using a multi-electron transfer reaction.
- thiols are often electrochemically active among the sulfur conjugates.
- a thiol one electron is reversibly transferred / received per sulfur atom.
- an organic compound containing two or more thiol groups in one molecule is oxidized with an electrode in a state of being dissolved in an electrolyte solution, the organic compound is superposed through an SS bond. Combined and deposited on the electrode.
- This oxidized body has a property of depolymerizing by reduction to return to the original monomer.
- An example is 2,5-dimercapto-1,3,4-thiadiazole (DMcT), which has two thiol groups per molecule and therefore can transfer two electrons.
- DcT 2,5-dimercapto-1,3,4-thiadiazole
- the theoretical capacity of an energy density of 362 Ah per kilogram of DMcTl can be obtained from the redox reaction of DMcT.
- a sulfur-based material as it is as a positive electrode material for the following several reasons. The first is that smooth charge / discharge characteristics cannot be obtained due to the slow electron transfer reaction at room temperature. Second, in the form of a thin-film electrode using such a sulfur-based substance as a redox reaction active layer, the redox reaction between the dithiol and the SS bond does not always occur smoothly.
- the polyarline is complex because protons participate in the oxidation-reduction response, and its catalytic ability for the oxidation-reduction reaction of the sulfur-based compound is greatly affected by the acidity of the electrolyte, that is, the proton concentration. Therefore, it was difficult to select optimal conditions for the reaction.
- polypyrrole and polythiophene were selected as candidates among the electron conductive polymer substances, and two electron-donating oxygen atoms were coupled to the thiophene ring.
- the organic sulfur-based compound is characterized by having a high energy density, it has been difficult to increase the electric energy per unit weight of the battery and to repeatedly perform electron transfer at a high speed.
- the present invention is to provide a positive electrode material that can effectively utilize the high energy density of a sulfur-based compound and overcome the above-mentioned conventional problems, and in particular, to provide a positive electrode for a lithium secondary battery.
- a positive electrode material that can effectively utilize the high energy density of a sulfur-based compound and overcome the above-mentioned conventional problems, and in particular, to provide a positive electrode for a lithium secondary battery.
- Another object of the present invention is to provide a non-lithium-based positive electrode for a secondary battery from which a large current can be obtained relatively instantaneously by using it in combination with a non-lithium-based material negative electrode.
- a redox-active sulfur-containing ring having at least one or more aromatic rings and a ring containing at least one disulfide bond and having a side of the aromatic ring on the side of the disulfide-containing ring is provided.
- the disulfide-containing ring of which does not open there is provided a redox active reversible electrode comprising a redox active film containing a sulfur-containing substance having a property capable of reciprocally transferring and receiving the above electrons on the surface of a conductive substrate.
- a positive electrode, a lithium-based negative electrode or a non-lithium-based negative electrode, and an electrolyte layer disposed between the positive electrode and the negative electrode are provided.
- a lithium secondary battery or a non-lithium secondary battery constituted by electrodes is also provided.
- FIG. 1 is a graph showing CV characteristics of the cathode material of Example 1 in a dissolved state of a target substance.
- FIG. 2 is a graph showing CV characteristics of a positive electrode material of Example 2.
- FIG. 3 is a graph showing CV characteristics of a positive electrode material of Example 4.
- FIG. 4 is a graph showing CV characteristics of a positive electrode material of Example 5.
- FIG. 5 is a graph showing CV characteristics of a positive electrode material of Example 8.
- the redox active reversible electrode of the present invention has a redox active film on the surface of a conductive substrate.
- the redox active membrane of the present invention contains a redox active sulfur-containing substance.
- the redox-active sulfur-containing substance used in the present invention is a compound having at least one or more aromatic rings and one or more rings containing a disulfide bond, and having the side of the aromatic ring on the side of the disulfide-containing ring.
- Such sulfur-containing materials include a sulfur-containing material having an aromatic moiety containing at least one aromatic ring and at least one disulfide-containing heterocycle containing at least one disulfide bond having at least one side of the aromatic ring as a common side.
- organic sulfur compounds having a ring site.
- the aromatic ring and the disulfide-containing heterocycle share at least one side of each ring.
- the aromatic ring and the disulfide-containing heterocyclic ring have at least two carbon atoms as shared atoms.
- the aromatic moiety includes a condensed polycyclic skeleton having at least one benzene ring or a nitrogen-containing heterocyclic ring.
- the condensed polycyclic skeleton include polyacenes such as naphthalene, naphthacene, tetracene and hexacene, and hydroforms thereof. (Eg, dihydrohexacene, tetrahydrohexacene), and condensed polycycles such as perylene.
- nitrogen-containing heterocyclic ring examples include pyrrole.
- the polysulfide in the case of a polysulfide bond in which n (n ⁇ 3) sulfur atoms are continuously bonded, the polysulfide may contain (n ⁇ 1) disulfide bonds. Will be considered
- the sulfur-containing substance does not open or close due to the redox reaction of the sulfur site, and is positively monovalent, and Z or positive divalent, and Z or mymus monocyclic per ring. It is preferable that the organic sulfur-containing substance be charged to a valence. It is a substance in which one disulfide-containing ring in a neutral state is not two-electron reduced and the sulfur active site is not a thiol group.
- the potential at which the redox reaction of the sulfur-containing substance occurs is preferably between +2.0 and 4.5 volts with a lithium metal electrode as a reference electrode.
- Some of the sulfur-containing substances used in the present invention dielectronically reduce the disulfide-containing ring at potentials of 1.9 volts or less, turning the sulfur active site into a thiol group. In this case, as described above, the redox reaction between the thiol group and the SS bond does not occur smoothly in the molecule, and the irreversibility is lost. That is, in the above-mentioned U.S. Pat. No.
- the following compounds (1) to (11) and the following compounds (12) to (14) are preferable.
- the aromatic ring site may be substituted with one or more of a halogen atom, a nitro group, an alkyl group, a hydroxyl group, a sulfonic acid group, a carboxylic acid group, and an amino group. Good. Furthermore, a compound (polymer) obtained by introducing a polymerizable side chain such as a butyl group or an atalylate group into the aromatic ring site and polymerizing the same may be used.
- the compound having the above substituent can be represented, for example, by the following formulas (A) to (C).
- X represents the above substituent.
- m and n are each independently 1 or 2
- p and q are each independently 1 to 4 Is an integer.
- the compounds (1) to (11) may be in the form of a polymer in which two or more thereof are linked via a thioether bond (-S-) at the benzene ring at both ends! .
- a polymer can be represented, for example, by the following formula (D).
- each Z represents S, and n is 2 to 200.
- Such polymers are
- a polymer bonded at the ⁇ and ⁇ 'sites of the heteroaromatic ring is preferable.
- One or more of an alkyl group, a hydroxyl group, a sulfonic acid group, a carboxylic acid group, and an amino group may be contained in the site of the ring containing the magus disulfide.
- compounds (1) to (11) may be used in any form of a monomer or a polymer.
- compounds (12) to (14) a powder obtained by chemical oxidation polymerization using an oxidizing agent, or a powder or thin film obtained by oxidizing polymerization by electrolysis can be used.
- This redox active film shows a redox wave corresponding to the reversible redox response of the sulfur-containing substance.
- the redox active film of the present invention is obtained by adding a carbon-based conductive particle to the solid powder of the organic sulfur-containing substance described above, adding an appropriate amount of a binder, and mixing the mixture. It can be manufactured by coating on a substrate and press-molding. From the initial stage of charge and discharge, a large current suitable for practical use, for example, a current of 0.1 to 3 mAZcm 2 can be obtained from the initial stage of charging and discharging at room temperature.
- the carbon-based conductive particles include carbon black, Ketjen black, acetylene black, graphite, carbon nanotubes, and the like.
- the conductive carbon particles can be used at a ratio of 1 to 30 parts by weight per 100 parts by weight of the organic sulfur-containing substance.
- the redox active film of the present invention may contain a metal oxide and a metal complex.
- metal oxides include layered metal oxides capable of fixing a sulfur-containing substance between layers, such as vanadium pentoxide.
- metal oxides include lithium cobalt oxide (LiCoO), lithium nickelate (LiNiO), and lithium manganate (LiMn O 2).
- the redox active film of the present invention is formed of metal-based conductive fine particles such as metals such as copper, iron, silver, nickel, palladium, gold, platinum, indium, and tungsten, indium oxide, and tin oxide.
- metal-based conductive fine particles such as metals such as copper, iron, silver, nickel, palladium, gold, platinum, indium, and tungsten, indium oxide, and tin oxide.
- a conductive metal oxide may be mixed.
- These conductive fine particles are preferably formed of silver, nordium, nickel, gold or copper, and can be used as a mixture of different conductive ultrafine particles.
- the substrate (current collector) supporting the redox active film of the present invention includes at least a redox active film.
- This substrate can be formed of a conductive material such as a metal, a conductive metal oxide, or carbon, but is preferably formed of copper, carbon, gold, aluminum, or an alloy thereof.
- a substrate body formed of another material may be coated with these conductive materials.
- the substrate may have irregularities on its surface or may have a net-like shape!
- the redox active film can contain an electron conductive polymer.
- an electron conductive polymer For example, in a material in which a redox-active sulfur-containing substance is doped into a polythiophene-based electron-conductive polymer to form a composite, the redox reaction of a sulfide-based compound is accelerated by an electron transfer reaction, so that the inside of the redox-active film and the redox reaction are increased. A rapid electron transfer reaction can be achieved at the interface between the active film and the current collector.
- the redox active film of the present invention may contain a metal complex such as lithium iron phosphate (lithium olivine).
- the redox active film has a thickness of 10 to: LOO m. Further, it is preferable that the particles (electroconductive polymer material, sulfur compound, conductive fine particles, etc.) used in the present invention are smaller than the thickness of the redox active film.
- the redox active reversible electrode of the present invention is particularly preferably used as a positive electrode of a lithium secondary battery.
- a lithium secondary battery includes a positive electrode and a lithium-based negative electrode, and an electrolyte layer is disposed between them.
- the positive electrode is constituted by the redox active reversible electrode of the present invention.
- the lithium-based negative electrode can be composed of a lithium-based metal material such as metallic lithium or a lithium alloy (for example, Li-A1 alloy), or a lithium intercalated carbon material.
- the lithium-based metal material is preferably used in the form of a foil from the viewpoint of light weight of the battery.
- the electrolyte layer interposed between the positive electrode and the negative electrode is preferably composed of a polymer gel containing an electrolyte solution (polymer gel electrolyte).
- polymer gel electrolyte As the electrolyte contained in the polymer electrolyte, CF SO Li, C F SO Li, (CF SO Li
- Lithium salts such as NLi, (CF SO) CLi, LiBF, LiPF, LiCIO can be used.
- the solvent in which these electrolytes are dissolved is preferably a non-aqueous solvent.
- non-aqueous solvents include chain carbonates, cyclic carbonates, cyclic esters, nitrile compounds, acid anhydrides, amide compounds, phosphate compounds, amine compounds and the like.
- Non-aqueous solvent Specific examples include ethylene carbonate, propylene carbonate, getyl carbonate, dimethoxyethane, butyrolataton, N methylpyrrolidinone, N, N 'dimethyl acetoamide, a mixture of propylene carbonate and dimethoxyethane, ethylene carbonate and getyl.
- the polymer gel it is preferable to use a copolymer of acrylonitrile and methyl acrylate or methacrylic acid.
- the polymer gel electrolyte can be obtained by immersing the polymer in an electrolyte solution, or by polymerizing a component (monomer Z compound) of the polymer in the presence of the electrolyte solution.
- This gel is a non-crosslinked polymer gel in which about 10% by mole of polyethylene is grafted with a compound containing an oligomer of polyethylene oxide such as polyethylene glycol.
- This polymer has completely different physical properties from non-daraphtodon polyethylene, and has the ability to absorb a large amount of organic electrolyte solution, to gelate, and to retain the absorption solution. Therefore, a gel electrolyte can be obtained by immersing the polymer in an electrolyte solution. Further, a reaction mixture obtained by adding a crosslinkable monomer to a solution in which the above-mentioned non-crosslinkable polymer is dissolved in an electrolyte solution in an organic solvent is applied to a substrate, and subjected to reaction conditions for crosslinking and polymerizing the crosslinkable monomer. It is also possible to produce a polymer gel electrolyte integrally formed with the material.
- the redox-active reversible electrode of the present invention is combined with a negative electrode of a conductive carbon material such as a conductive polymer material or an activated carbon material that reversibly doped with non-lithium ions in addition to the positive electrode of a lithium secondary battery. It can be used as a positive electrode of a non-lithium-based battery (for example, a magnesium secondary battery).
- the secondary battery has a positive electrode and a non-lithium negative electrode, and an electrolyte layer is disposed between them.
- the electrolyte layer interposed between the positive electrode and the negative electrode is preferably composed of a polymer gel containing an electrolyte solution (polymer gel electrolyte).
- electrolyte salt magnesium ion BF-salt, PF-salt, dodecyl salt
- An benzene sulfonate and a tosylate salt can be used.
- the solvent for dissolving these electrolytes is preferably a non-aqueous solvent.
- the polymer gel electrolyte the materials described above in the lithium secondary battery can be used.
- NMP N-methylpyrrolidinone
- Ketjen black of conductive carbon powder and a polymer of binder are converted into a katen ⁇ paste-like liquid.
- a working electrode was produced by coating.
- a lithium metal electrode was used as a counter electrode, and a silver Z silver ion electrode was used as a reference electrode.
- the CV measurement was performed in the potential range of -0.2 to +0.2 V vs. silver ion electrode (+3.5 to +3.9 V vs. lithium electrode) for 20 mVZ seconds. Made at sweep speed.
- PC Propylene carbonate
- lithium perchlorate was used as the electrolyte salt to prepare a PC solution containing 0.1 M lithium perchlorate.
- Figure 2 shows the CV behavior.
- an acid-reduction current response with good reversibility was obtained near OV.
- the current response only decreased gradually with repeated potential sweeps. The cause of this decrease was due to the dissolution of the active material from the film into the solution. This reduction could be prevented by using a polymer gel as the electrolyte.
- the potential sweep is extended in the range of 13.0 to 10.8V (+0.7 to + 4.2V vs. lithium electrode) while applying force, the current response due to repetition of CV is remarkable. It became worse, and it was shown that reversibility was lost when the disulfide ring was opened.
- the compound (1) is sulfonated with concentrated sulfuric acid (H SO), and the redox response of the coated electrode is measured.
- sulfonidani was carried out by a general method in which 1 gram of the compound (1) was dissolved in 10 ml of concentrated sulfuric acid and stirred at 60 ° C for 1 hour. The dark green paste-like liquid turned reddish purple with the lapse of stirring time. 30 ml of distilled water was added to the liquid to obtain a precipitate. The precipitate was filtered, then washed repeatedly with distilled water and finally with acetone. The washed precipitate was dried at 60 ° C. under vacuum.
- a known amount of the obtained compound is dissolved and dispersed in NMP, and the Ketjen Black conductive carbon powder and the polymer of the binder are converted into a paste-like liquid, which is coated on a GC electrode and dried.
- Working electrodes were fabricated. A lithium metal electrode was used as a counter electrode, and a silver Z silver ion electrode was used as a reference electrode. The CV measurements were performed at a sweep rate of 20 mVZ seconds over the potential range of -1.0 to +0.5 V vs. silver Z silver ion electrode (+1.7 to +4.2 V vs. lithium electrode).
- a propylene carbonate (PC) was used as an electrolyte for performing CV measurement, and a lithium perchlorate was used as an electrolyte salt.
- a PC solution containing 0.1 M lithium perchlorate was prepared and used.
- an oxidizing reduction current response having good reversibility was obtained.
- the potential range of the redox response was widened, and the repetition stability was significantly increased.
- the potential sweep expands to the range of ⁇ 3.0 to +0.5 V (+0.7 to +4.2 V vs. the lithium electrode), the current response due to the repetition of CV is poor. It was shown that reversibility was lost when the disulfide ring was opened.
- the compound was synthesized according to N. R. Ayyangar et al, Indian J. Chem., B16, 673 (1978).
- the compound was dissolved and dispersed in NMP, and the ketjen black of the conductive carbon powder and the polymer of the binder were converted into a katen ⁇ paste-like liquid.
- Lithium metal electrodes were used for the counter and reference electrodes.
- the CV measurements were made at a potential range of +3.0 to +4.2 V (vs. lithium electrode) at a sweep rate of lmVZ seconds. 1.
- sulfonidani was performed by a general method in which 1 gram of the compound (4) was dissolved in 10 ml of concentrated sulfuric acid and stirred at 60 ° C for 3 hours. Upon addition of concentrated sulfuric acid, the pasty liquid immediately turned deep red. After stirring for 3 hours, 30 ml of distilled water was added to the liquid to obtain a precipitate. The precipitate was filtered, then washed repeatedly with distilled water and finally with acetone. The washed precipitate was dried at 60 ° C. under vacuum.
- the organic compound was dissolved and dispersed in NMP, and Ketjen black of conductive carbon powder and a binder polymer were converted into a Kagami ⁇ paste.
- a working electrode was prepared by coating the solution on a GC electrode and drying it.
- a lithium metal electrode was used as a counter electrode and a reference electrode.
- the CV measurement was performed at a sweep rate of lmVZ seconds in the potential range of +3.0 to + 4.2V (for the lithium electrode).
- the compound was synthesized according to Indian J. Chem. B16, 673 (1978) described above.
- the compound was dissolved and dispersed in NMP, and the ketjen black of the conductive carbon powder and the polymer of the binder were converted into a katen ⁇ paste-like liquid.
- Lithium metal electrodes were used for the counter and reference electrodes.
- the CV measurement was performed in the potential range of +2.7 to +4.2 V (with respect to the lithium electrode) at a sweep speed of lmVZ seconds. 1.
- sulfonidani was performed by a general method in which 1 gram of the compound (5) was dissolved in 10 ml of concentrated sulfuric acid and stirred at 60 ° C. for 15 hours. Even when concentrated sulfuric acid was added, the paste-like liquid remained dark green and remained intact. After stirring for 15 hours, 30 ml of distilled water was added to the liquid to obtain a precipitate. The precipitate was filtered, then washed repeatedly with distilled water and finally with acetone. The washed precipitate was dried at 60 ° C. under vacuum.
- the material was dissolved and dispersed in NMP, and Ketjen Black, a conductive carbon powder, and a binder polymer were converted into a paste-like liquid, which was coated on a GC electrode and dried to prepare a working electrode.
- a lithium metal electrode was used as a counter electrode and a reference electrode.
- the CV measurement was performed at a sweep rate of lmVZ seconds in the potential range of +2.7 to + 4.2V (for lithium electrode). 1.
- Figure 5 shows the CV behavior of the electrode coated with compound (12) in the same electrolyte solution as V without compound (12). From these results, it was concluded that the membrane polymerized by the above-mentioned method had excellent redox activity having a reversible oxidation-reduction peak potential value of -0.4V.
- the current response of the electrode coated with this compound (12) shows that the response does not deteriorate even if the potential sweep range is extended to 3.0 to 0 V (+0.7 to +3.7 V vs. the lithium electrode). I got it. Even when the compounds (13) and (14) were used, these compound-coated electrodes exhibited reversible redox responses having an oxidation reduction peak potential value of 0.25 V and ⁇ 0.20 V, respectively. Behavior similar to that of compound (12) was obtained. Was.
- TTN-4C1 site power of naphthalene ring of compound (2) 3,4,7,8-tetrachloronaphtho [1,8-cd: 4,5-c, d,] bis [ [1, 2] dithiol (abbreviated as TTN-4C1) was synthesized according to E. Klingsberg, Tetrahedron, 28, 963 (1972). 15 g of otatachloronaphthalene and 6 g of sulfur were placed in a 200 ml flask, and the temperature was increased to 310 ° C under a nitrogen stream. Although there was a large amount of sulfur generated during the process, the temperature was kept at 310 ° C for about 20 minutes and then allowed to cool to room temperature.
- TTN-4C1 could be obtained in a yield of 75%.
- the compound was dissolved and dispersed in NMP, and the ketjen black of conductive carbon powder and the polymer of the binder were converted into a kato paste solution. This was coated on a GC electrode and dried to produce a working electrode. A lithium metal electrode was used as a counter electrode and a reference electrode. The CV measurement was performed at a sweep rate of lmVZ seconds in the potential range of +2.7 to + 4.2V (for lithium electrode).
- a mixture of ethylene carbonate (EC) and ethynolecarbonate (DEC) (weight ratio 1: 3) as the electrolyte for CV measurement, and a 1.0M concentration using lithium tetrafluoroborate as the electrolyte salt was prepared.
- EC ethylene carbonate
- DEC ethynolecarbonate
- the coating film on the coated electrode prepared in the same manner as described above was dried, and then a perfluoro ion exchanger, naphion
- the film surface was further covered with an appropriate amount of a mixed solution containing 5% by weight of water and an alcoholic solution, followed by drying to prepare a working electrode.
- a lithium metal electrode was used as a counter electrode and a reference electrode.
- the CV measurement was performed at a sweep rate of lmVZ seconds in the potential range of +3.0 to + 4.2V (vs. lithium electrode).
- ethylene carbonate (EC) and ethynolecarbonate (DEC) Using a mixed solution (1: 3 by weight) and lithium tetrafluoroborate as an electrolyte salt, a 1.OM concentration electrolyte solution was prepared.
- An oxidation wave with peak potentials around 3.8V and 3.9V, and two sharp reduction waves with peak potentials near 3.8 and 3.7V were obtained. In this case, the response did not decrease even with a sweep of 4 hours or more, and the repetition stability of the redox response was significantly increased as compared with the case of Example 11.
- Example 11 In order to examine the redox response of a polymer in which the a ;, ⁇ , and moieties of the naphthalene ring of compound (2) were linked by a thioether (one S—), the compound was prepared according to the method described in Example 11 ⁇ . Klingsberg, Tetrahedron, 28 , 963 (1972) with a new process. In this method, the TTN-4C1 described in Example 11 was reacted at 310 ° C. for 20 minutes without isolation, and then the flask was cooled to 100 ° C. and contained TTN-4C1 in a flask containing TTN-4C1. 5 g of the hydrate was added. Then, the temperature was raised again to 330 ° C and held for about 30 minutes.
- Chlorine remaining in the black powder of the present invention obtained by adding sodium sulfide during the reaction is present in an amount of 1% or less according to the result of elemental analysis and the result of X-ray photoelectron spectroscopy (ESCA). It was confirmed that. Furthermore, the sulfur fraction is 1.5 to 1.6 times the value obtained with the force TTN-4C1, which varies with the amount of sodium sulfide added during the reaction. In other words, it became clear that an average of two sulfur atoms were newly introduced into the naphthalene ring unit and used for polymerization.
- the compound was dissolved and dispersed in NMP, and Ketjen black of conductive carbon powder and a polymer of the binder were mixed with Kagami paste.
- a working liquid was prepared by coating the liquid on a GC electrode and drying it.
- a lithium metal electrode was used as a counter electrode and a reference electrode.
- the CV measurement was performed at a sweep rate of lmVZ seconds in the potential range of +2.7 to + 4.2V (for lithium electrode). 1.
- OM concentration using a mixture of ethylene carbonate (EC) and ethynolecarbonate (DEC) (weight ratio 1: 3) as electrolyte for CV measurement and lithium tetrafluoroborate as electrolyte salt was prepared. Its CV response behavior is two superposed oxidation waves with peak potential values around 4.0 to 4.IV, and two sharp reduction waves with peak potential values around 4.0 to 3.8V. was gotten. The response stability did not decrease even with a very good potential sweep for several hours.
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Abstract
Description
Claims
Priority Applications (5)
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EP05727636A EP1744388A4 (en) | 2004-03-30 | 2005-03-29 | ACTIVE REDOX REVERSIBLE ELECTRODE AND SECONDARY BATTERY INCLUDING SAID ELECTRODE |
CA002561915A CA2561915A1 (en) | 2004-03-30 | 2005-03-29 | Redox active reversible electrode and secondary battery including the same |
JP2005518605A JPWO2005096417A1 (ja) | 2004-03-30 | 2005-03-29 | レドックス活性可逆電極およびそれを用いた二次電池 |
CN2005800100827A CN1938885B (zh) | 2004-03-30 | 2005-03-29 | 氧化还原活性可逆电极和使用该电极的二次电池 |
US11/544,437 US20070026310A1 (en) | 2004-03-30 | 2006-09-29 | Redox-active reversible electrode and secondary battery using the same |
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JP2004-101018 | 2004-03-30 | ||
JP2004101018 | 2004-03-30 |
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US11/544,437 Continuation US20070026310A1 (en) | 2004-03-30 | 2006-09-29 | Redox-active reversible electrode and secondary battery using the same |
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WO2005096417A1 true WO2005096417A1 (ja) | 2005-10-13 |
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US (1) | US20070026310A1 (ja) |
EP (1) | EP1744388A4 (ja) |
JP (2) | JPWO2005096417A1 (ja) |
KR (1) | KR100854837B1 (ja) |
CN (1) | CN1938885B (ja) |
CA (1) | CA2561915A1 (ja) |
TW (1) | TWI250679B (ja) |
WO (1) | WO2005096417A1 (ja) |
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WO2007086519A1 (ja) * | 2006-01-27 | 2007-08-02 | Fuji Jukogyo Kabushiki Kaisya | 硫黄含有芳香族ポリマーの製造方法 |
JP2007227186A (ja) * | 2006-02-24 | 2007-09-06 | Osaka Univ | 分子結晶性二次電池 |
JP2008066125A (ja) * | 2006-09-07 | 2008-03-21 | Fuji Heavy Ind Ltd | 電極材料およびその製造方法ならびにそれを用いた蓄電池 |
CN100384911C (zh) * | 2006-05-26 | 2008-04-30 | 武汉大学 | 一种芳酸酐硫化聚合物的制备方法 |
JP2010118320A (ja) * | 2008-11-14 | 2010-05-27 | Denso Corp | 二次電池 |
US7816679B2 (en) * | 2004-06-16 | 2010-10-19 | Sony Corporation | Organic compound crystal and field-effect transistor |
JP2011028949A (ja) * | 2009-07-23 | 2011-02-10 | Toyota Central R&D Labs Inc | 蓄電デバイス及び電極活物質の製造方法 |
JP2012150934A (ja) * | 2011-01-18 | 2012-08-09 | Toyota Industries Corp | 硫黄系正極活物質とその製造方法及びリチウムイオン二次電池用正極 |
WO2012147242A1 (ja) * | 2011-04-27 | 2012-11-01 | 株式会社豊田自動織機 | ナトリウム二次電池 |
WO2013084445A1 (ja) * | 2011-12-08 | 2013-06-13 | 株式会社豊田自動織機 | 非水電解質二次電池 |
WO2018143048A1 (ja) * | 2017-01-31 | 2018-08-09 | パナソニックIpマネジメント株式会社 | 電気化学デバイス用正極および電気化学デバイス、ならびにこれらの製造方法 |
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JP6554645B2 (ja) * | 2015-07-13 | 2019-08-07 | 本田技研工業株式会社 | 電解液及びマグネシウム二次電池 |
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- 2005-03-29 JP JP2005518605A patent/JPWO2005096417A1/ja active Pending
- 2005-03-29 CA CA002561915A patent/CA2561915A1/en not_active Abandoned
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JPWO2007086519A1 (ja) * | 2006-01-27 | 2009-06-25 | 富士重工業株式会社 | 硫黄含有芳香族ポリマーの製造方法 |
JP2007227186A (ja) * | 2006-02-24 | 2007-09-06 | Osaka Univ | 分子結晶性二次電池 |
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JP2008066125A (ja) * | 2006-09-07 | 2008-03-21 | Fuji Heavy Ind Ltd | 電極材料およびその製造方法ならびにそれを用いた蓄電池 |
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Also Published As
Publication number | Publication date |
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EP1744388A4 (en) | 2010-08-25 |
JP2011060777A (ja) | 2011-03-24 |
CA2561915A1 (en) | 2005-10-13 |
JPWO2005096417A1 (ja) | 2008-02-21 |
TW200536163A (en) | 2005-11-01 |
TWI250679B (en) | 2006-03-01 |
KR20060131941A (ko) | 2006-12-20 |
CN1938885A (zh) | 2007-03-28 |
JP5377464B2 (ja) | 2013-12-25 |
CN1938885B (zh) | 2010-12-08 |
KR100854837B1 (ko) | 2008-08-27 |
US20070026310A1 (en) | 2007-02-01 |
EP1744388A1 (en) | 2007-01-17 |
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