CA2298792C - Phosphonate additives for nonaqueous electrolyte in rechargeable cells - Google Patents
Phosphonate additives for nonaqueous electrolyte in rechargeable cells Download PDFInfo
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- CA2298792C CA2298792C CA002298792A CA2298792A CA2298792C CA 2298792 C CA2298792 C CA 2298792C CA 002298792 A CA002298792 A CA 002298792A CA 2298792 A CA2298792 A CA 2298792A CA 2298792 C CA2298792 C CA 2298792C
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- H—ELECTRICITY
- H01—ELECTRIC ELEMENTS
- H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
- H01M10/00—Secondary cells; Manufacture thereof
- H01M10/05—Accumulators with non-aqueous electrolyte
- H01M10/052—Li-accumulators
- H01M10/0525—Rocking-chair batteries, i.e. batteries with lithium insertion or intercalation in both electrodes; Lithium-ion batteries
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- 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
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- H—ELECTRICITY
- H01—ELECTRIC ELEMENTS
- H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
- H01M10/00—Secondary cells; Manufacture thereof
- H01M10/05—Accumulators with non-aqueous electrolyte
- H01M10/056—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
- H01M10/0569—Liquid materials characterised by the solvents
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- H—ELECTRICITY
- H01—ELECTRIC ELEMENTS
- H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
- H01M4/00—Electrodes
- H01M4/02—Electrodes composed of, or comprising, active material
- H01M4/13—Electrodes for accumulators with non-aqueous electrolyte, e.g. for lithium-accumulators; Processes of manufacture thereof
- H01M4/133—Electrodes based on carbonaceous material, e.g. graphite-intercalation compounds or CFx
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- H—ELECTRICITY
- H01—ELECTRIC ELEMENTS
- H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
- H01M10/00—Secondary cells; Manufacture thereof
- H01M10/05—Accumulators with non-aqueous electrolyte
- H01M10/058—Construction or manufacture
- H01M10/0587—Construction or manufacture of accumulators having only wound construction elements, i.e. wound positive electrodes, wound negative electrodes and wound separators
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- H—ELECTRICITY
- H01—ELECTRIC ELEMENTS
- H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
- H01M2300/00—Electrolytes
- H01M2300/0017—Non-aqueous electrolytes
- H01M2300/0025—Organic electrolyte
- H01M2300/0028—Organic electrolyte characterised by the solvent
- H01M2300/0037—Mixture of solvents
- H01M2300/0042—Four or more solvents
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- H—ELECTRICITY
- H01—ELECTRIC ELEMENTS
- H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
- H01M4/00—Electrodes
- H01M4/02—Electrodes composed of, or comprising, active material
- H01M4/13—Electrodes for accumulators with non-aqueous electrolyte, e.g. for lithium-accumulators; Processes of manufacture thereof
- H01M4/131—Electrodes based on mixed oxides or hydroxides, or on mixtures of oxides or hydroxides, e.g. LiCoOx
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- H—ELECTRICITY
- H01—ELECTRIC ELEMENTS
- H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
- H01M4/00—Electrodes
- H01M4/02—Electrodes composed of, or comprising, active material
- H01M4/36—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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- 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
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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
- 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
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- General Chemical & Material Sciences (AREA)
- Manufacturing & Machinery (AREA)
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- Secondary Cells (AREA)
Abstract
A lithium ion electrochemical cell having high charge/discharge capacity, long cycle life and exhibiting a reduced first cycle irreversible capacity, is described. The stated benefits are realized by the addition of at least one phosphonate additive to an electrolyte comprising an alkali metal salt dissolved in a solvent mixture that includes ethylene carbonate, dimethyl carbonate, ethylmethyl carbonate and diethyl carbonate. The preferred additive is an alkyl phosphonate compound.
Description
04645.0601 PHOSPHONATE ADDITIVES FOR NONAQUEOUS
ELECTROLYTE IN RECHARGEABLE CELLS
BACKGROUND OF INVENTION
The present invention generally relates to an alkali metal electrochemical cell, and more particularly, to a rechargeable alkali metal cell. Still more particularly, the present invention relates to a lithium ion electrochemical cell activated with an electrolyte having an additive provided to achieve high charge/discharge capacity, long cycle life and to minimize the first cycle irreversible~capacity. According to the present invention, the preferred 'additive to the activating electrolyte is a phosphonate compound. A phosphite compound is another name for a phosphonate compound and is also preferred for the present invention.
Alkali metal rechargeable cells typically comprise a carbonaceous anode electrode and a lithiated cathode electrode.
Due to the high potential of the cathode material (up to 4.3V vs.
Li/Li+ for Lil_xCo02) and the low potential of the carbonaceous anode material (0.01V vs. Li/Li+ for graphite) in a fully charged lithium ion cell, the choice of the electrolyte solvent system is limited. Since carbonate solvents have high oxidative stability toward typically used lithiated cathode materials and good kinetic stability toward carbonaceous anode materials, they are generally used in lithium ion cell electrolytes. To achieve ..
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ELECTROLYTE IN RECHARGEABLE CELLS
BACKGROUND OF INVENTION
The present invention generally relates to an alkali metal electrochemical cell, and more particularly, to a rechargeable alkali metal cell. Still more particularly, the present invention relates to a lithium ion electrochemical cell activated with an electrolyte having an additive provided to achieve high charge/discharge capacity, long cycle life and to minimize the first cycle irreversible~capacity. According to the present invention, the preferred 'additive to the activating electrolyte is a phosphonate compound. A phosphite compound is another name for a phosphonate compound and is also preferred for the present invention.
Alkali metal rechargeable cells typically comprise a carbonaceous anode electrode and a lithiated cathode electrode.
Due to the high potential of the cathode material (up to 4.3V vs.
Li/Li+ for Lil_xCo02) and the low potential of the carbonaceous anode material (0.01V vs. Li/Li+ for graphite) in a fully charged lithium ion cell, the choice of the electrolyte solvent system is limited. Since carbonate solvents have high oxidative stability toward typically used lithiated cathode materials and good kinetic stability toward carbonaceous anode materials, they are generally used in lithium ion cell electrolytes. To achieve ..
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- 3 - 04645.0601 cycle irreversible capacity, the lower the cell capacity in subsequent cycles and the lower the cell efficiency. Thus, it is desirable to minimize or even eliminate the first cycle irreversible capacity in lithium ion cells while at the same time maintaining the low temperature cycling capability of such cells.
According to the present invention, these objectives are achieved by providing an organic phosphonate or phosphite in the quaternary solvent electrolyte. Lithium ion cells activated with these electrolytes exhibit lower first cycle irreversible capacities relative to cells activated with the same quaternary solvent electrolyte devoid of the phosphonate additive. As a result, cells including the phosphonate additive present higher - subsequent cycling capacity than control cells. The cycleability of the present invention cells at room temperature, as well as at low temperatures, i.e., down to about -40~C, is as good as cells activated with the quaternary electrolyte devoid of a phosphonate additive.
SUMMARY OF THE INVENTION
It is commonly known that when an electrical potential is initially applied to lithium ion cells constructed with a carbon anode in a discharged condition to charge the cell, some permanent capacity loss occurs due to the anode surface passivation film formation. This permanent capacity loss is called first cycle irreversible capacity. The film formation process, however, is highly dependent on the reactivity of the electrolyte components at the cell charging potentials. The electrochemical properties of the passivation film are also dependent on the chemical composition of the surface film.
The formation of a surface film is unavoidable for alkali metal systems, and in particular, lithium metal anodes, and - 4 - 04645.0601 lithium intercalated carbon anodes due to the relatively low potential and high reactivity of lithium toward organic electrolytes. The ideal surface film, known as the solid-electrolyte interphase (SEI), should be electrically insulating and sonically conducting. While most alkali metal, and in particular, lithium electrochemical systems meet the first requirement, the second requirement is difficult to achieve. The resistance of these films is not negligible, and as a result;
impedance builds up inside the cell due to this surface layer formation which induces unacceptable polarization during the charge and discharge of the lithium ion cell. On the other hand, if the SEI film is electrically conductive, the electrolyte decomposition reaction on the anode surface does not stop due to the low potential of the lithiated carbon electrode.
Hence, the composition of the electrolyte has a significant influence on the discharge efficiency of alkali metal systems, and particularly the permanent capacity loss in secondary cells.
For example, when 1.0M LiPF6/EC:DMC=30:70 is used to activate a secondary cell, the first cycle irreversible capacity is approximately 35 mAh/g of graphite. However, under the same cycling conditions, the first cycle irreversible capacity is found to be approximately 65 mAh/g of graphite when 1. OM
LiPF6/EC:DMC:EMC:DEC=45:22:24.8:8.2 is used as the electrolyte.
Further, lithium ion cells activated with the binary solvent electrolyte of ethylene carbonate and dimethyl carbonate cannot be cycled at temperatures less than about -11°C. The quaternary solvent electrolyte of the previously referenced patent application, which enables lithium ion cells to cycle at much lower temperatures, is a compromise in terms of providing a wider temperature application with acceptable cycling efficiencies. It would be highly desirable to retain the benefits of a lithium ion - 5 - 04645.0601 cell capable of operating at temperatures down to as low as about -40aC while minimizing the first cycle irreversible capacity.
According to the present invention, this objective is achieved by adding a phosphonate additive in the above described quaternary solvent electrolytes. In addition, this invention may be generalized'to other nonaqueous organic electrolyte systems, such as binary solvent and ternary solvent systems,.as well as the electrolyte systems containing solvents other than mixtures of linear or cyclic carbonates. For example, linear or cyclic ethers or esters may also be included as electrolyte components.
Although the exact reason for the observed improvement is not clear, it is hypothesized that the phosphonate additive competes with the existing electrolyte components to react on the carbon anode surface during initial lithiation to form a beneficial SEI
film. The thusly formed SEI film is electrically more insulating than the film formed without the phosphonate additive and, as a consequence, the lithiated carbon electrode is better protected from reactions with other electrolyte components. Therefore, lower first cycle irreversible capacity is obtained.
The phosphonate or phosphate additives are defined herein as organic mono-alkyl alkyl or dialkyl alkyl phosphonate compounds or phosphorous acid (phosphonic acid) provided as a co-solvent with the other nonaqueous eletrolyte solvents. The organic phosphonate additives are in a condensed phase which makes them easy to handle in electrolyte preparation.
These and other objects of the present invention will become increasingly more apparent to those skilled in the art by reference to the following description and to the appended drawings.
According to the present invention, these objectives are achieved by providing an organic phosphonate or phosphite in the quaternary solvent electrolyte. Lithium ion cells activated with these electrolytes exhibit lower first cycle irreversible capacities relative to cells activated with the same quaternary solvent electrolyte devoid of the phosphonate additive. As a result, cells including the phosphonate additive present higher - subsequent cycling capacity than control cells. The cycleability of the present invention cells at room temperature, as well as at low temperatures, i.e., down to about -40~C, is as good as cells activated with the quaternary electrolyte devoid of a phosphonate additive.
SUMMARY OF THE INVENTION
It is commonly known that when an electrical potential is initially applied to lithium ion cells constructed with a carbon anode in a discharged condition to charge the cell, some permanent capacity loss occurs due to the anode surface passivation film formation. This permanent capacity loss is called first cycle irreversible capacity. The film formation process, however, is highly dependent on the reactivity of the electrolyte components at the cell charging potentials. The electrochemical properties of the passivation film are also dependent on the chemical composition of the surface film.
The formation of a surface film is unavoidable for alkali metal systems, and in particular, lithium metal anodes, and - 4 - 04645.0601 lithium intercalated carbon anodes due to the relatively low potential and high reactivity of lithium toward organic electrolytes. The ideal surface film, known as the solid-electrolyte interphase (SEI), should be electrically insulating and sonically conducting. While most alkali metal, and in particular, lithium electrochemical systems meet the first requirement, the second requirement is difficult to achieve. The resistance of these films is not negligible, and as a result;
impedance builds up inside the cell due to this surface layer formation which induces unacceptable polarization during the charge and discharge of the lithium ion cell. On the other hand, if the SEI film is electrically conductive, the electrolyte decomposition reaction on the anode surface does not stop due to the low potential of the lithiated carbon electrode.
Hence, the composition of the electrolyte has a significant influence on the discharge efficiency of alkali metal systems, and particularly the permanent capacity loss in secondary cells.
For example, when 1.0M LiPF6/EC:DMC=30:70 is used to activate a secondary cell, the first cycle irreversible capacity is approximately 35 mAh/g of graphite. However, under the same cycling conditions, the first cycle irreversible capacity is found to be approximately 65 mAh/g of graphite when 1. OM
LiPF6/EC:DMC:EMC:DEC=45:22:24.8:8.2 is used as the electrolyte.
Further, lithium ion cells activated with the binary solvent electrolyte of ethylene carbonate and dimethyl carbonate cannot be cycled at temperatures less than about -11°C. The quaternary solvent electrolyte of the previously referenced patent application, which enables lithium ion cells to cycle at much lower temperatures, is a compromise in terms of providing a wider temperature application with acceptable cycling efficiencies. It would be highly desirable to retain the benefits of a lithium ion - 5 - 04645.0601 cell capable of operating at temperatures down to as low as about -40aC while minimizing the first cycle irreversible capacity.
According to the present invention, this objective is achieved by adding a phosphonate additive in the above described quaternary solvent electrolytes. In addition, this invention may be generalized'to other nonaqueous organic electrolyte systems, such as binary solvent and ternary solvent systems,.as well as the electrolyte systems containing solvents other than mixtures of linear or cyclic carbonates. For example, linear or cyclic ethers or esters may also be included as electrolyte components.
Although the exact reason for the observed improvement is not clear, it is hypothesized that the phosphonate additive competes with the existing electrolyte components to react on the carbon anode surface during initial lithiation to form a beneficial SEI
film. The thusly formed SEI film is electrically more insulating than the film formed without the phosphonate additive and, as a consequence, the lithiated carbon electrode is better protected from reactions with other electrolyte components. Therefore, lower first cycle irreversible capacity is obtained.
The phosphonate or phosphate additives are defined herein as organic mono-alkyl alkyl or dialkyl alkyl phosphonate compounds or phosphorous acid (phosphonic acid) provided as a co-solvent with the other nonaqueous eletrolyte solvents. The organic phosphonate additives are in a condensed phase which makes them easy to handle in electrolyte preparation.
These and other objects of the present invention will become increasingly more apparent to those skilled in the art by reference to the following description and to the appended drawings.
6 - 04645.0601 BRIEF DESCRIPTION OF THE DRAWINGS
Fig. 1 is a graph showing trhe averaged discharge capacity through twenty cycles for twp groups of lithium-ion cells, one group activated with a quaternary carbonate solvent mixture devoid of a phosphonate additive in comparison to a similarly constructed cell group having the phosphonate electrolyte additive.
DETAILED DESCRIPTION OF THE PREFERRED EMBODIMENTS
A secondary electrochemical cell constructed according to the present invention includes an anode active material selected from Groups IA, IIA, or IIIB of the Periodic Table of Elements, including the alkali metals lithium, sodium, potassium, etc. The preferred anode active material comprises lithium.
In secondary electrochemical systems, the anode. electrode comprises a material capable of intercalating and de-intercalating the alkali metal, and preferably lithium. A
carbonaceous anode comprising any of the various forms of carbon (e. g., coke, graphite, acetylene black, carbon black, glassy carbon, etc.) which are capable of reversibly retaining the lithium species, is preferred. Graphite is particularly preferred due to its relatively high lithium-retention capacity.
Regardless of the form of the carbon, fibers of the carbonaceous material are particularly advantageous because the fibers have excellent mechanical properties which permit them to be fabricated into rigid electrodes that are capable of withstanding degradation during repeated charge/discharge cycling. Moreover, the high surface area of carbon fibers allows for rapid charge/discharge rates. A preferred carbonaceous material for the anode of a secondary electrochemical cell is described in U.S. Patent No. 5,443,928 to Takeuchi et al., which is assigned .i..k~1'C': C.fsi ':#.''~~~'i':f.': f~-::. :~~.i:'r.'.
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- 8 - 04645.0601 Metals such as nickel, aluminum, titanium and stainless steel in powder form are also useful as conductive diluents when mixed with the above listed active materials. The electrode further comprises a fluoro-resin binder, preferably in a powder form, such as PTFE, PVDF, ETFE, polyamides and polyimides, and mixtures thereof.
To discharge such secondary cells, the lithium ion comprising the cathode is intercalated into the carbonaceous anode by applying an externally generated electrical potential to recharge the cell. The applied recharging electrical potential serves to draw the alkali metal ions from the cathode material, through the electrolyte and into the carbonaceous anode to saturate the carbon comprising the anode. The resulting LiXC6 electrode can have an x ranging between 0.1 and 1Ø The cell is then provided with an electrical potential and is discharged in a normal manner.
An alternate secondary cell construction comprises intercalating the carbonaceous material with the active alkali material before the anode is incorporated into the cell. In this case, the cathode body can be solid and comprise, but not be limited to, such materials as manganese dioxide, silver vanadium oxide, copper silver vanadium oxide, titanium disulfide, copper oxide, copper sulfide, iron sulfide, iron disulfide and fluorinated carbon. However, this approach is compromised by the problems associated with handling lithiated carbon outside o~f the cell. Lithiated carbon tends to react when contacted by air.
The secondary cell of the present invention includes a separator to provide physical segregation between the anode and cathode active electrodes. The separator is of an electrically insulative material to prevent an internal electrical short circuit between the electrodes, and the separator material also ...,.. s~~"3,~'r;z,f~..~.:...~.yy wnza'.,F~.:,s,.~w,..,.~v'~.':
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uS,~.:..i%'~~3~ ,~;';<.~. :.W iv:~'=' s~~,>~~~".r'>~3.~,..~' :'~~'~i - 10 - 04645.0601 alkali metal salt dissolved in a quaternary mixture of organic carbonate solvents comprising dialkyl (non-cyclic) carbonates selected from dimethyl carbonate (DMC), diethyl carbonate (DEC), dipropyl carbonate (DPC), ethylmethyl carbonate (EMC), methylpropyl carbonate (MPC) and ethylpropyl carbonate (EPC), and mixtures thereof, and at least one cyclic carbonate selected from propylene carbonate (PC), ethylene carbonate (EC), butylene carbonate (BC) and vinylene carbonate (VC), and mixtures thereof.
Organic carbonates are generally used in the electrolyte solvent system for such battery chemistries because they exhibit high oxidative stability toward cathode materials and good kinetic stability toward anode materials.
Preferred electrolytes according to the present invention comprise solvent mixtures of EC:DMC:EMC:DEC. Most preferred volume percent ranges for the various carbonate solvents include EC in the range of about 10$ to about 50~; DMC in the range of about 5$ to about 75~; EMC in the range of about 5$ to about 50$;
and DEC in the range of about 3$ to about 450. Electrolytes containing this quaternary carbonate mixture exhibit freezing points below -50oC, and lithium ion cells activated with such mixtures have very good cycling behavior at room temperature as well as very good discharge and charge/discharge cycling behavior at temperatures below -20oC.
Known lithium salts that are useful as a vehicle for transport of alkali metal ions from the anode to the cathode, and back again include LiPFs, LiBF4, LiAsF6, LiSbF6, LiC104, LiA1C14, LiGaCl4, LiC (SOZCF3) 3, LiN03, LiN (SOZCF3) 2, LiSCN, Li03SCF2CF3, LiC6F5S03, LiOZCCF3, LiS03F, LiB (C6H5) 4 and LiCF3S03, and mixtures thereof. Suitable salt concentrations typically range between about 0.8 to 1.5 molar.
- 11 - 04645.0601 In accordance with the present invention, at least one organic phosphonate additive, preferably a mono-alkyl alkyl or a dialkyl alkyl phosphonate compound is provided as a co-solvent in the electrolyte solution of the previously described alkali metal ion or rechargeable electrochemical cell. The phosphonate additive is preferably an alkyl phosphonate compound having the general formula (R10) P (=0) (0R2) (R3) wherein R1, RZ and R3 are the same or different, and they can be a hydrogen atom or a saturated or unsaturated organic group containing 1 to 13 carbon atoms.
The greatest effect is found when dimethyl phosphonate, diethyl phosphonate, dipropyl phosphonate, dibutyl phosphonate, diphenyl phosphonate, dibenzyl phosphonate, dimethyl methylphosphonate, diethyl methylphosphonate, dipropyl methylphosphonate, dibutyl methylphosphonate, Biphenyl methylphosphonate, dibenzyl methylphosphonate, dimethyl benzylphosphonate, ethyl methylphosphonate, dimethyl diphenylmethylphosphonate and phosphourous acid or phosphonic acid, and mixtures thereof are used as additives in the electrolyte.
The above described compounds are only intended to be exemplary of those that are useful with the present invention, and are not to be construed as limiting. Those skilled in the art will readily recognize phosphonate compounds which come under the purview of the general formula set forth above and which will be useful as additives for the electrolyte to achieve high charge/discharge capacity, long cycle life and to minimize the first cycle irreversible capacity according to the present invention.
While not intending to be bound by any particular mechanism, i.t is believed that due to the presence of the P=0 bond in the -OP(=O)(R)O- functional group, the bond between oxygen and at least one of the group R1 and Rz is severed and the phosphonate ... ~.! ,.~
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- 13 - 04645.0601 electrochemical cell and is resistant to corrosion. The cathode lead is welded to the positive terminal pin in the glass-to-metal seal and the header is welded to the case containing the electrode stack. The cell is thereafter filled with the electrolyte solution comprising at least one of the phosphonate additives described hereinabove and hermetically sealed such as by close-welding a.stainless steel ball over the fill hole, but not limited thereto. ..
The above assembly describes a case-negative cell, which is the preferred construction of the exemplary cell of the present invention. As is well known to those skilled in the art, the exemplary electrochemical system of the present invention can also be constructed in a case-positive configuration.
The following examples describe the manner and process of an electrochemical cell according to the present invention, and set forth the best mode contemplated by the inventors of carrying out the invention, but are not construed as limiting.
EXAMPLE I
Six lithium ion cells were constructed as test vehicles.
The cells were divided into two groups of three cells. One group of cells was activated with a quaternary carbonate solvent system electrolyte devoid of a phosphonate additive while the remaining cells had the same electrolyte but including the phosphonate additive. Except for the electrolyte, the cells were the same.
In particular, the cathode was prepared by casting a LiCo02 cathode mix on aluminum foil. The cathode mix contained 91$ _.
LiCo02, 6~ graphite additive and 3$ PVDF binder, by weight. The anode was prepared by casting an anode mix containing 91.7°s - 14~ - 04645.0601 graphite and 8.3$ PVDF binder, by weight, on a copper foil. An electrode assembly was constructed by placing one layer of polyethylene separator between the cathode and the anode and spirally winding the electrodes to fit into an AA sized cylindrical stainless steel can. The cells were activated with an electrolyte of EC:DMC:EMC:DEC=45:22:24.8:8.2 having 1. OM LiPF6 dissolved therein (group 1). The group 2 cells fabricated according to the present invention further had 0.05M dibenzyl phosphonate (DBPI) dissolved therein. Finally, the cells were hermetically sealed.
All six cells were then cycled between 4.1V and 2.75V. The charge cycle was performed under a 100 mA constant current until the cells reach 4.1V. Then, the charge cycle was continued at 4.1V until the current dropped to 20 mA. After resting for 5 minutes, the cells were discharged under a 100 mA constant current to 2.75 V. The cells were rested for another 5 minutes before the next cycle.
The initial average charge and discharge capacities of both groups of cells are summarized in Table 1. The first cycle irreversible capacity was calculated as the difference between the first charge capacity and the first discharge capacity.
Table 1 First Cycle Capacities and Irreversible Capacities 1st Charge 1st Discharge Irreversible Group (mAh) (mAh) 1 641.4 ~ 1.5 520.2 ~ 9.5 121.2 ~ 10.7 2 635.1 ~ 13.9 541.7 ~ 4.3 93.4 ~ 18.2 - 15 - 04645.0601 The data in Table 1 clearly demonstrate that both groups of cells had similar first cycle charge capacities.
However, the first cycle discharge capacities are quite different. The group 2 cells activated with the electrolyte containing the dibenzyl phosphonate additive had significantly higher first cycle discharge capacities than that of the group 1 cells (approximately 4.1g higher). As a result, the group 2 cells also had about 23~ lower first cycle irreversible capacity than that of the group I cells.
EXAMPLE II
After the initial cycle, the cycling of the six cells continued for a total of 10 times under. the same cycling conditions as described in Example I. The discharge'capacities and the capacity retention of each cycle are summarized in Table 2. The capacity retention is defined as the capacity percentage of each discharge cycle relative to that of the first cycle discharge capacity.
Table 2 Cycling Discharge Capacity and Capacity Retention Group 1 Group 2 Capacity Retention Capacity Retention Cycle # (mAh) (~h) 1 520.2 100.0 541.7 100.0 2 510.2 98.1 534.1 98.6 _. 3 503.4 96.8 528.0 97.5 4 497.6 95.7 522.7 96.5 493.2 94.8 519.0 95.8 6 489.4 94.1 515.3 95.1 - 16 - 04645.0601 Group 1 Group 2 Capacity Retention Capacity Retention Cycle (mAh) ($) (mAh) #
Fig. 1 is a graph showing trhe averaged discharge capacity through twenty cycles for twp groups of lithium-ion cells, one group activated with a quaternary carbonate solvent mixture devoid of a phosphonate additive in comparison to a similarly constructed cell group having the phosphonate electrolyte additive.
DETAILED DESCRIPTION OF THE PREFERRED EMBODIMENTS
A secondary electrochemical cell constructed according to the present invention includes an anode active material selected from Groups IA, IIA, or IIIB of the Periodic Table of Elements, including the alkali metals lithium, sodium, potassium, etc. The preferred anode active material comprises lithium.
In secondary electrochemical systems, the anode. electrode comprises a material capable of intercalating and de-intercalating the alkali metal, and preferably lithium. A
carbonaceous anode comprising any of the various forms of carbon (e. g., coke, graphite, acetylene black, carbon black, glassy carbon, etc.) which are capable of reversibly retaining the lithium species, is preferred. Graphite is particularly preferred due to its relatively high lithium-retention capacity.
Regardless of the form of the carbon, fibers of the carbonaceous material are particularly advantageous because the fibers have excellent mechanical properties which permit them to be fabricated into rigid electrodes that are capable of withstanding degradation during repeated charge/discharge cycling. Moreover, the high surface area of carbon fibers allows for rapid charge/discharge rates. A preferred carbonaceous material for the anode of a secondary electrochemical cell is described in U.S. Patent No. 5,443,928 to Takeuchi et al., which is assigned .i..k~1'C': C.fsi ':#.''~~~'i':f.': f~-::. :~~.i:'r.'.
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- 8 - 04645.0601 Metals such as nickel, aluminum, titanium and stainless steel in powder form are also useful as conductive diluents when mixed with the above listed active materials. The electrode further comprises a fluoro-resin binder, preferably in a powder form, such as PTFE, PVDF, ETFE, polyamides and polyimides, and mixtures thereof.
To discharge such secondary cells, the lithium ion comprising the cathode is intercalated into the carbonaceous anode by applying an externally generated electrical potential to recharge the cell. The applied recharging electrical potential serves to draw the alkali metal ions from the cathode material, through the electrolyte and into the carbonaceous anode to saturate the carbon comprising the anode. The resulting LiXC6 electrode can have an x ranging between 0.1 and 1Ø The cell is then provided with an electrical potential and is discharged in a normal manner.
An alternate secondary cell construction comprises intercalating the carbonaceous material with the active alkali material before the anode is incorporated into the cell. In this case, the cathode body can be solid and comprise, but not be limited to, such materials as manganese dioxide, silver vanadium oxide, copper silver vanadium oxide, titanium disulfide, copper oxide, copper sulfide, iron sulfide, iron disulfide and fluorinated carbon. However, this approach is compromised by the problems associated with handling lithiated carbon outside o~f the cell. Lithiated carbon tends to react when contacted by air.
The secondary cell of the present invention includes a separator to provide physical segregation between the anode and cathode active electrodes. The separator is of an electrically insulative material to prevent an internal electrical short circuit between the electrodes, and the separator material also ...,.. s~~"3,~'r;z,f~..~.:...~.yy wnza'.,F~.:,s,.~w,..,.~v'~.':
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Organic carbonates are generally used in the electrolyte solvent system for such battery chemistries because they exhibit high oxidative stability toward cathode materials and good kinetic stability toward anode materials.
Preferred electrolytes according to the present invention comprise solvent mixtures of EC:DMC:EMC:DEC. Most preferred volume percent ranges for the various carbonate solvents include EC in the range of about 10$ to about 50~; DMC in the range of about 5$ to about 75~; EMC in the range of about 5$ to about 50$;
and DEC in the range of about 3$ to about 450. Electrolytes containing this quaternary carbonate mixture exhibit freezing points below -50oC, and lithium ion cells activated with such mixtures have very good cycling behavior at room temperature as well as very good discharge and charge/discharge cycling behavior at temperatures below -20oC.
Known lithium salts that are useful as a vehicle for transport of alkali metal ions from the anode to the cathode, and back again include LiPFs, LiBF4, LiAsF6, LiSbF6, LiC104, LiA1C14, LiGaCl4, LiC (SOZCF3) 3, LiN03, LiN (SOZCF3) 2, LiSCN, Li03SCF2CF3, LiC6F5S03, LiOZCCF3, LiS03F, LiB (C6H5) 4 and LiCF3S03, and mixtures thereof. Suitable salt concentrations typically range between about 0.8 to 1.5 molar.
- 11 - 04645.0601 In accordance with the present invention, at least one organic phosphonate additive, preferably a mono-alkyl alkyl or a dialkyl alkyl phosphonate compound is provided as a co-solvent in the electrolyte solution of the previously described alkali metal ion or rechargeable electrochemical cell. The phosphonate additive is preferably an alkyl phosphonate compound having the general formula (R10) P (=0) (0R2) (R3) wherein R1, RZ and R3 are the same or different, and they can be a hydrogen atom or a saturated or unsaturated organic group containing 1 to 13 carbon atoms.
The greatest effect is found when dimethyl phosphonate, diethyl phosphonate, dipropyl phosphonate, dibutyl phosphonate, diphenyl phosphonate, dibenzyl phosphonate, dimethyl methylphosphonate, diethyl methylphosphonate, dipropyl methylphosphonate, dibutyl methylphosphonate, Biphenyl methylphosphonate, dibenzyl methylphosphonate, dimethyl benzylphosphonate, ethyl methylphosphonate, dimethyl diphenylmethylphosphonate and phosphourous acid or phosphonic acid, and mixtures thereof are used as additives in the electrolyte.
The above described compounds are only intended to be exemplary of those that are useful with the present invention, and are not to be construed as limiting. Those skilled in the art will readily recognize phosphonate compounds which come under the purview of the general formula set forth above and which will be useful as additives for the electrolyte to achieve high charge/discharge capacity, long cycle life and to minimize the first cycle irreversible capacity according to the present invention.
While not intending to be bound by any particular mechanism, i.t is believed that due to the presence of the P=0 bond in the -OP(=O)(R)O- functional group, the bond between oxygen and at least one of the group R1 and Rz is severed and the phosphonate ... ~.! ,.~
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- 13 - 04645.0601 electrochemical cell and is resistant to corrosion. The cathode lead is welded to the positive terminal pin in the glass-to-metal seal and the header is welded to the case containing the electrode stack. The cell is thereafter filled with the electrolyte solution comprising at least one of the phosphonate additives described hereinabove and hermetically sealed such as by close-welding a.stainless steel ball over the fill hole, but not limited thereto. ..
The above assembly describes a case-negative cell, which is the preferred construction of the exemplary cell of the present invention. As is well known to those skilled in the art, the exemplary electrochemical system of the present invention can also be constructed in a case-positive configuration.
The following examples describe the manner and process of an electrochemical cell according to the present invention, and set forth the best mode contemplated by the inventors of carrying out the invention, but are not construed as limiting.
EXAMPLE I
Six lithium ion cells were constructed as test vehicles.
The cells were divided into two groups of three cells. One group of cells was activated with a quaternary carbonate solvent system electrolyte devoid of a phosphonate additive while the remaining cells had the same electrolyte but including the phosphonate additive. Except for the electrolyte, the cells were the same.
In particular, the cathode was prepared by casting a LiCo02 cathode mix on aluminum foil. The cathode mix contained 91$ _.
LiCo02, 6~ graphite additive and 3$ PVDF binder, by weight. The anode was prepared by casting an anode mix containing 91.7°s - 14~ - 04645.0601 graphite and 8.3$ PVDF binder, by weight, on a copper foil. An electrode assembly was constructed by placing one layer of polyethylene separator between the cathode and the anode and spirally winding the electrodes to fit into an AA sized cylindrical stainless steel can. The cells were activated with an electrolyte of EC:DMC:EMC:DEC=45:22:24.8:8.2 having 1. OM LiPF6 dissolved therein (group 1). The group 2 cells fabricated according to the present invention further had 0.05M dibenzyl phosphonate (DBPI) dissolved therein. Finally, the cells were hermetically sealed.
All six cells were then cycled between 4.1V and 2.75V. The charge cycle was performed under a 100 mA constant current until the cells reach 4.1V. Then, the charge cycle was continued at 4.1V until the current dropped to 20 mA. After resting for 5 minutes, the cells were discharged under a 100 mA constant current to 2.75 V. The cells were rested for another 5 minutes before the next cycle.
The initial average charge and discharge capacities of both groups of cells are summarized in Table 1. The first cycle irreversible capacity was calculated as the difference between the first charge capacity and the first discharge capacity.
Table 1 First Cycle Capacities and Irreversible Capacities 1st Charge 1st Discharge Irreversible Group (mAh) (mAh) 1 641.4 ~ 1.5 520.2 ~ 9.5 121.2 ~ 10.7 2 635.1 ~ 13.9 541.7 ~ 4.3 93.4 ~ 18.2 - 15 - 04645.0601 The data in Table 1 clearly demonstrate that both groups of cells had similar first cycle charge capacities.
However, the first cycle discharge capacities are quite different. The group 2 cells activated with the electrolyte containing the dibenzyl phosphonate additive had significantly higher first cycle discharge capacities than that of the group 1 cells (approximately 4.1g higher). As a result, the group 2 cells also had about 23~ lower first cycle irreversible capacity than that of the group I cells.
EXAMPLE II
After the initial cycle, the cycling of the six cells continued for a total of 10 times under. the same cycling conditions as described in Example I. The discharge'capacities and the capacity retention of each cycle are summarized in Table 2. The capacity retention is defined as the capacity percentage of each discharge cycle relative to that of the first cycle discharge capacity.
Table 2 Cycling Discharge Capacity and Capacity Retention Group 1 Group 2 Capacity Retention Capacity Retention Cycle # (mAh) (~h) 1 520.2 100.0 541.7 100.0 2 510.2 98.1 534.1 98.6 _. 3 503.4 96.8 528.0 97.5 4 497.6 95.7 522.7 96.5 493.2 94.8 519.0 95.8 6 489.4 94.1 515.3 95.1 - 16 - 04645.0601 Group 1 Group 2 Capacity Retention Capacity Retention Cycle (mAh) ($) (mAh) #
7 486.1 93.4 512.4 94.6 8 483.2 92.9 '509.8 94.1 9 480.2 92.3 507. 4 93.7 478.2 91.9 505.5 X3.3 The data in Table 2 demonstrate that the group 2 cells with the dibenzyl phosphonate additive consistently presented higher discharge capacities in all cycles. In addition, this higher capacity was not realized at the expense of lower cycle life. The group 1 and 2 cells had essentially the same cycling capacity retention throughout the various cycles.
EXAMPLE III
After the above cycle testing described in Example II, the cells were charged according to the procedures described in Example I. Then, the cells were discharged under a 1000 mA
constant current to 2.75 V then a five minute open circuit rest, followed by a 500 mA constant current discharge to 2.75 V then a five minute open circuit rest, followed by a 250 mA con.stant current discharge to 2.75 V then a five minute open circuit rest and, finally, followed by a 100 mA constant current discharge to 2.75 V then a five minute open circuit rest. The averaged total capacities under each discharge rate are summarized in Table 3 and the comparison of averaged discharge efficiency (defined as $
capacity of a 100 mA constant current discharge) under the various constant currents are summarized in Table 4. In Table 3, - 17 - 04645.0601 the discharge capacities are cumulative from one discharge current to the next.
Table 3 Discharge Capacities (mAh) under Various Currents Group 1000 mA 500 mA 250 mA 100 mA
1 277.8 439.8 459.8 465.9 2 231.6 460.9 484.2 492.3 Table 4 Discharge Efficiency (~) under Various Currents Group 1000 mA 500 mA 250 mA 100 mA
1 59.7 94.4 98.7 100.0 2 47.0 93.6 98.3 100.0 The data in Table 3 indicate that the group 2 cells with phosphonate additive delivered increased discharge capacity in comparison to the group 1 control cells under a discharge rate equal to or less than 500 mA (approximately a 1C rate). Under a higher discharge rate (1000 mA, approximately a 2C rate), however, the group 1 control cells delivered higher capacity than that of the group 2 cells. The same trends are also shown in Table 4. Under a 500 mA or lower discharge current, the group 2 cells presented similar discharge efficiencies than that of the group 1 cells. Under a higher discharge current (i.e. 1000 mA), - 18 - 04645.0601 the group 1 control cells afforded a higher discharge efficiency than that of the group 2 cells.
EXAMPLE IV
After the above discharge rate capability test, all the cells were fully charged according to the procedure described in Example I. The six test cells were then stored on open circuit voltage (OCV) at 37°C for two weeks. Finally, the cells were discharged and cycled for eight more times. The ~ of self-discharge and the capacity retention were calculated and are shown in Table 5.
Table 5 Rates of Self-Discharge and After Storage Capacity Retention Group Self-Discharge ($) Capacity Retention 1 12.6 93.4 2 15.0 93.6 The data in Table 5 demonstrate that both groups of cells exhibited similar self-discharge rates and similar after storage capacity retention rates. However, since the group 2 cells had higher discharge capacities than that of the group 1 cells, the capacities of the group 2 cells were still higher than that of the group 1 cells, even though they presented similar self-discharge and capacity retention rates. A total of 20 cycles were obtained and the results are summarized in Fig. 1. In .. -: w> w ,~c~~~::1.E:F>. .... , C'3_3:: :f' :.~'s 's~;:3.i~
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'~' ~' ~ t f. . ~, :'... ~,:. ~'f' .... _ . , n ,. y '~.,.. .i, ,t'.....: J, :: ~.'r.~ i':::'.'. 'i':.'i,;' s.).~'. ~v . ~, . . ;,,:~ ~~ ;i'~, a. %%.i't :.:; ~: v: ,~ .., r~ ~~~- ~; ~: ::~ 3y~:; :.
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- 20 - 04645.0601 the carbon anode surface. Therefore, for lithium ion cells, at least one of the R groups in the phosphonate additive having the general formula (R10) P (=O) (0R2) (R3) should be either hydrogen (acidic proton) or a saturated or unsaturated organic group containing 1 to 13 carbon atoms.
While not intended to be bound by any particular theory, it is believed that due to the presence of the -OP(=0)(R)0-functional group, the reductive cleavage of at least owe of the ORland ORZ bonds in the phosphonate additives of the present invention may produce lithium phosphonate or the lithium salt of a phosphonate reduction product of the general formula 0=P(O-Li)"(OR)m (n = 1 or 2; m = 0 or 1) deposited on the anode surface.
This anode surface film is ionically more conductive than the film formed in the absence of the additives and is responsible for the improved performance of the lithium-ion cells.
The concentration limit for the phosphonate additive is preferably about O.OO1M to about 0.40M. The beneficial effect of the phosphonate additive will not be apparent if the additive concentration is less than about O.OO1M. On the other hand, if the additive concentration is greater than about 0.40M, the beneficial effect of the additive will be canceled by the detrimental effect of higher internal cell resistance due to the thicker anode surface film formation and lower electrolyte conductivity.
It is appreciated that various modifications to the inventive concepts described herein may be apparent to those of ordinary skill in the art without departing from the spirit and scope of the present invention as defined by the appended claims.
EXAMPLE III
After the above cycle testing described in Example II, the cells were charged according to the procedures described in Example I. Then, the cells were discharged under a 1000 mA
constant current to 2.75 V then a five minute open circuit rest, followed by a 500 mA constant current discharge to 2.75 V then a five minute open circuit rest, followed by a 250 mA con.stant current discharge to 2.75 V then a five minute open circuit rest and, finally, followed by a 100 mA constant current discharge to 2.75 V then a five minute open circuit rest. The averaged total capacities under each discharge rate are summarized in Table 3 and the comparison of averaged discharge efficiency (defined as $
capacity of a 100 mA constant current discharge) under the various constant currents are summarized in Table 4. In Table 3, - 17 - 04645.0601 the discharge capacities are cumulative from one discharge current to the next.
Table 3 Discharge Capacities (mAh) under Various Currents Group 1000 mA 500 mA 250 mA 100 mA
1 277.8 439.8 459.8 465.9 2 231.6 460.9 484.2 492.3 Table 4 Discharge Efficiency (~) under Various Currents Group 1000 mA 500 mA 250 mA 100 mA
1 59.7 94.4 98.7 100.0 2 47.0 93.6 98.3 100.0 The data in Table 3 indicate that the group 2 cells with phosphonate additive delivered increased discharge capacity in comparison to the group 1 control cells under a discharge rate equal to or less than 500 mA (approximately a 1C rate). Under a higher discharge rate (1000 mA, approximately a 2C rate), however, the group 1 control cells delivered higher capacity than that of the group 2 cells. The same trends are also shown in Table 4. Under a 500 mA or lower discharge current, the group 2 cells presented similar discharge efficiencies than that of the group 1 cells. Under a higher discharge current (i.e. 1000 mA), - 18 - 04645.0601 the group 1 control cells afforded a higher discharge efficiency than that of the group 2 cells.
EXAMPLE IV
After the above discharge rate capability test, all the cells were fully charged according to the procedure described in Example I. The six test cells were then stored on open circuit voltage (OCV) at 37°C for two weeks. Finally, the cells were discharged and cycled for eight more times. The ~ of self-discharge and the capacity retention were calculated and are shown in Table 5.
Table 5 Rates of Self-Discharge and After Storage Capacity Retention Group Self-Discharge ($) Capacity Retention 1 12.6 93.4 2 15.0 93.6 The data in Table 5 demonstrate that both groups of cells exhibited similar self-discharge rates and similar after storage capacity retention rates. However, since the group 2 cells had higher discharge capacities than that of the group 1 cells, the capacities of the group 2 cells were still higher than that of the group 1 cells, even though they presented similar self-discharge and capacity retention rates. A total of 20 cycles were obtained and the results are summarized in Fig. 1. In .. -: w> w ,~c~~~::1.E:F>. .... , C'3_3:: :f' :.~'s 's~;:3.i~
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- 20 - 04645.0601 the carbon anode surface. Therefore, for lithium ion cells, at least one of the R groups in the phosphonate additive having the general formula (R10) P (=O) (0R2) (R3) should be either hydrogen (acidic proton) or a saturated or unsaturated organic group containing 1 to 13 carbon atoms.
While not intended to be bound by any particular theory, it is believed that due to the presence of the -OP(=0)(R)0-functional group, the reductive cleavage of at least owe of the ORland ORZ bonds in the phosphonate additives of the present invention may produce lithium phosphonate or the lithium salt of a phosphonate reduction product of the general formula 0=P(O-Li)"(OR)m (n = 1 or 2; m = 0 or 1) deposited on the anode surface.
This anode surface film is ionically more conductive than the film formed in the absence of the additives and is responsible for the improved performance of the lithium-ion cells.
The concentration limit for the phosphonate additive is preferably about O.OO1M to about 0.40M. The beneficial effect of the phosphonate additive will not be apparent if the additive concentration is less than about O.OO1M. On the other hand, if the additive concentration is greater than about 0.40M, the beneficial effect of the additive will be canceled by the detrimental effect of higher internal cell resistance due to the thicker anode surface film formation and lower electrolyte conductivity.
It is appreciated that various modifications to the inventive concepts described herein may be apparent to those of ordinary skill in the art without departing from the spirit and scope of the present invention as defined by the appended claims.
Claims (37)
1. An electrochemical cell, which comprises:
a) a negative electrode which intercalates with an alkali metal;
b) a positive electrode comprising an electrode active material which intercalates with the alkali metal;
c) a nonaqueous electrolyte activating the negative and the positive electrode; and d) a phosphonate additive having the formula:
(R1O)P(=O)(OR2)(R1) provided in the electrolyte, wherein R3 is a hydrogen atom and wherein at least one, but not both of R1 and R2 is a hydrogen atom or at least one of R1 and R2 is a saturated organic group containing 1 to 13 carbon atoms.
a) a negative electrode which intercalates with an alkali metal;
b) a positive electrode comprising an electrode active material which intercalates with the alkali metal;
c) a nonaqueous electrolyte activating the negative and the positive electrode; and d) a phosphonate additive having the formula:
(R1O)P(=O)(OR2)(R1) provided in the electrolyte, wherein R3 is a hydrogen atom and wherein at least one, but not both of R1 and R2 is a hydrogen atom or at least one of R1 and R2 is a saturated organic group containing 1 to 13 carbon atoms.
2. The electrochemical cell of claim 1 wherein the phosphonate additive is selected from the group consisting of dimethyl phosphonate, diethyl phosphonate, dipropyl phosphonate, dibutyl phosphonate, diphenyl phosphonate, dibenzyl phosphonate, ethyl methylphosphonate, and mixtures thereof.
3. The electrochemical cell of claims 1 wherein the phosphonate additive is present in the electrolyte in a range of about 0.001 M to about 0.40M.
4. The electrochemical cell of claim 1 wherein the phosphonate additive is dibenzyl phosphonate present in the electrolyte at a concentration up to about 0.05M.
5. The electrochemical cell of claim 1 wherein the electrolyte includes a quaternary, nonaqueous carbonate solvent mixture.
6. The electrochemical cell of claim 1 wherein the electrolyte comprises at least one linear carbonate selected from the group consisting of dimethyl carbonate, diethyl carbonate, dipropyl carbonate, ethylmethyl carbonate, methyl propyl carbonate and ethylpropyl carbonate, and mixtures thereof.
7. The electrochemical cell of claim 6 wherein the electrolyte comprises at least three of the linear carbonates.
8. The electrochemical cell of claim 1 wherein the electrolyte comprises at least one cyclic carbonate selected from the group consisting of ethylene carbonate, propylene carbonate, butylene carbonate and vinylene carbonate, and mixtures thereof.
9. The electrochemical cell of claim 1 wherein the electrolyte comprises ethylene carbonate, dimethyl carbonate, ethylmethyl carbonate and diethyl carbonate.
10. The electrochemical cell of claim 9 wherein the ethylene carbonate is in the range of about 10% about 50%, the dimethyl carbonate is in the range of about 5% to about 75%, the ethylmethyl carbonate is in the range of about 5% to about 50%, and the diethyl carbonate is in the range of about 3% to about 45%, by volume.
11. The electrochemical cell of claim 1 wherein the electrolyte includes an alkali metal salt selected from the group consisting of LiPF6, LiBF4, LiAsF6, LiSbF6, LiClO4, LiAlCl4, LiGaCl4, LiNO3, LiC(SO2CF3)3, LiN(SO2CF3)2, LiSCN, LiO3SCF2CF3, LiC6F5SO3, LiO2CCF3, LiSO3F, LiB(C6H5)4 and LiCF3SO3, and mixtures thereof.
12. The electrochemical cell of claim 11 wherein the alkali metal is lithium.
13. The electrochemical cell of claim 1 wherein the negative electrode comprises a negative electrode active material selected from the group consisting of coke, carbon black, graphite, acetylene black, carbon fibers and glassy carbon, and mixtures thereof.
14. The electrochemical cell of claim 1 wherein the negative electrode active material is mixed with a fluoro-resin binder.
15. The electrochemical cell of claim 1 wherein the positive electrode comprises a positive electrode active material selected from the group consisting of lithiated oxides, lithiated sulfides, lithiated selenides and lithiated tellurides of the group selected from vanadium, titanium, chromium, copper, molybdenum, niobium, iron, nickel, cobalt and manganese, and mixtures thereof.
16. The electrochemical cell of claim 15 wherein the positive electrode active material is mixed with a fluoro-resin binder.
17. The electrochemical cell of claim 15 wherein the positive electrode active material is mixed with a conductive additive selected from the group consisting of acetylene black, carbon black, graphite, nickel powder, aluminum powder titanium powder and stainless steel powder, and mixtures thereof.
18. An electrochemical cell, which comprises:
a) a negative electrode which intercalates with lithium;
b) a positive electrode comprising an electrode active material and which intercalates with lithium; and c) an electrolyte solution activating the anode and the cathode, the electrolyte including an alkali metal salt dissolved in a quaternary, nonaqueous carbonate solvent mixture of ethylene carbonate, dimethyl carbonate, ethylmethyl carbonate and diethyl carbonate; and d) a phosphonate additive having the formula:
(R1O)P(=O)(OR2)(R3) provided in the electrolyte, wherein R3 is a hydrogen atom and wherein at least one, but not both of R1 and R2 is a hydrogen atom or at least one of R1 and R2 is saturated organic group containing 1 to 13 carbon atoms.
a) a negative electrode which intercalates with lithium;
b) a positive electrode comprising an electrode active material and which intercalates with lithium; and c) an electrolyte solution activating the anode and the cathode, the electrolyte including an alkali metal salt dissolved in a quaternary, nonaqueous carbonate solvent mixture of ethylene carbonate, dimethyl carbonate, ethylmethyl carbonate and diethyl carbonate; and d) a phosphonate additive having the formula:
(R1O)P(=O)(OR2)(R3) provided in the electrolyte, wherein R3 is a hydrogen atom and wherein at least one, but not both of R1 and R2 is a hydrogen atom or at least one of R1 and R2 is saturated organic group containing 1 to 13 carbon atoms.
19. The electrochemical cell of claim 18 wherein the phosphonate additive is selected from the group consisting of dimethyl phosphonate, diethyl phosphonate, dipropyl phosphonate, dibutyl phosphonate, diphenyl phosphonate, dibenzyl phosphonate, ethyl methylphosphonate, and mixtures thereof are used as additives in the electrolyte.
20. The electrochemical cell of claim 18 wherein the ethylene carbonate is in the range of about 10% to about 50%, the dimethyl carbonate is in the range of about 5% to about 75%, the ethylmethyl carbonate is in the range of about 5% to about 50%, and the diethyl carbonate is in the range of about 3% to about 45%, by volume.
21. The electrochemical cell of claim 18 wherein the electrolyte includes an alkali metal salt selected from the group consisting of LiPF6, LiBF4, LiAsF6, LiSbF6, LiClO~, LiAlCl4, LiGaCl4, LiNO3, LiC(SO2CF3)3, LiN(SO2CF3)2, LiSCN, LiO3SCF2CF3, LiC6F5SO3, LiO2CCF3, LiSO3F, LiB(6H5)4 and LiCF3SO3, and mixtures thereof.
22. The method for providing an electrochemical cell, comprising the steps of:
a) providing a negative electrode which intercalates with an alkali metal;
b) providing a positive electrode comprising an electrode active material which intercalates with the alkali metal;
c) activating the negative and positive electrodes with a nonaqueous electrolyte; and d) providing a phosphonate additive having the formula:
(R1O)P(=O) (OR2) (R3) in the electrolyte, wherein R1 is a hydrogen atom and wherein at least one, but not both of R1 and R2 is a hydrogen atom of at least one of R1 and R2 is a saturated organic group containing 1 to 13 carbon atoms.
a) providing a negative electrode which intercalates with an alkali metal;
b) providing a positive electrode comprising an electrode active material which intercalates with the alkali metal;
c) activating the negative and positive electrodes with a nonaqueous electrolyte; and d) providing a phosphonate additive having the formula:
(R1O)P(=O) (OR2) (R3) in the electrolyte, wherein R1 is a hydrogen atom and wherein at least one, but not both of R1 and R2 is a hydrogen atom of at least one of R1 and R2 is a saturated organic group containing 1 to 13 carbon atoms.
23. The method of claim 22 including selecting the phosphonate additive from the group consisting of dimethyl phosphonate, diethyl phosphonate, dipropyl phosphonate, dibutyl phosphonate, diphenyl phosphonate, dibenzyl phosphonate, ethyl methylphosphonate, and mixtures thereof are used as additives in the electrolyte.
24. The method of claim 22 wherein the phosphonate additive is present in the electrolyte in a range of about 0.001 M to about 0.40M.
25. The method of claim 22 wherein the phosphonate additive is dibenzyl phosphonate present in the electrolyte at a concentration up to about 0.05M.
26. The method of claim 22 including providing the electrolyte comprising a quaternary, nonaqueous carbonate solvent mixture.
27. The method of claim 22 wherein the electrolyte comprises at least one linear carbonate selected from the group consisting of dimethyl carbonate, diethyl carbonate, dipropyl carbonate, ethylmethyl carbonate, methylpropyl carbonate and ethylpropyl carbonate, and mixtures thereof.
28. The method of claim 27 wherein the electrolyte comprises at least three of the linear carbonates.
29. The method of claim 22 wherein the electrolyte comprises at least one cyclic carbonate selected from the group consisting of ethylene carbonate, propylene carbonate, butylene carbonate and vinylene carbonate, and mixtures thereof.
30. The method of claim 22 wherein the electrolyte comprises ethylene carbonate, dimethyl carbonate, ethylmethyl carbonate and diethyl carbonate.
31. The method of claim 30 wherein the ethylene carbonate is in the range of about 10% to about 50%, the dimethyl carbonate is in the range of about 5% to about 75%, the ethylmethyl carbonate is in the range of about 5% to about 50%, and the diethyl carbonate is in the range of about 3% to about 45%, by volume.
32. The method of claim 22 wherein the electrolyte includes an alkali metal salt selected from the group consisting of LiPF6, LiBF4, LiAsF5, LiSbF6, LiClO4, LiAlCl4, LiGaCl4, LiNO3, LiC(SO2CF3)3, LiN(SO2CF3)2, LiSCN, LiO3SCF2CF3, LiC6F5SO3, LiO2CCF3, LiSO3F, LiB(C6H5)4 and LiCF3SO3, and mixtures thereof.
33. The method of claim 22 including providing the alkali metal as lithium.
34. The method of claim 22 including providing the positive electrode comprising a positive electrode active material selected from the group consisting of lithiated oxides, lithiated sulfides, lithiated selenides and lithiated tellurides of the group selected from vanadium, titanium, chromium, copper, molybdenum, niobium, iron, nickel, cobalt and manganese, and mixtures thereof.
35. The method of claim 22 including providing the negative electrode comprising a negative electrode active material selected from the group consisting of coke, carbon black, graphite, acetylene black, carbon fibers and glassy carbon, and mixtures thereof.
36. An electrochemical cell, which comprises:
a) a negative electrode which intercalates with an alkali metal;
b) a positive electrode comprising an electrode active material which intercalates with an alkali metal;
c) a nonaqueous electrolyte activating the negative and the positive electrodes; and d) dibenzyl phosphonate provided in the electrolyte at a concentration up to about 0.05M.
a) a negative electrode which intercalates with an alkali metal;
b) a positive electrode comprising an electrode active material which intercalates with an alkali metal;
c) a nonaqueous electrolyte activating the negative and the positive electrodes; and d) dibenzyl phosphonate provided in the electrolyte at a concentration up to about 0.05M.
37. The method for providing an electrochemical cell, comprising the steps of:
a)providing a negative electrode which intercalates with an alkali metal;
b)providing a positive electrode comprising an electrode active material which intercalates with the alkali metal;
c) activating the negative and positive electrodes with a nonaqueous electrolyte; and d) providing dibenzyl phosphonate in the electrolyte at a concentration up to about 0.05M.
a)providing a negative electrode which intercalates with an alkali metal;
b)providing a positive electrode comprising an electrode active material which intercalates with the alkali metal;
c) activating the negative and positive electrodes with a nonaqueous electrolyte; and d) providing dibenzyl phosphonate in the electrolyte at a concentration up to about 0.05M.
Applications Claiming Priority (2)
| Application Number | Priority Date | Filing Date | Title |
|---|---|---|---|
| US09/324,268 | 1999-06-02 | ||
| US09/324,268 US6200701B1 (en) | 1999-01-25 | 1999-06-02 | Phosphonate additives for nonaqueous electrolyte in rechargeable cells |
Publications (2)
| Publication Number | Publication Date |
|---|---|
| CA2298792A1 CA2298792A1 (en) | 2000-12-02 |
| CA2298792C true CA2298792C (en) | 2004-04-27 |
Family
ID=23262842
Family Applications (1)
| Application Number | Title | Priority Date | Filing Date |
|---|---|---|---|
| CA002298792A Expired - Fee Related CA2298792C (en) | 1999-06-02 | 2000-02-11 | Phosphonate additives for nonaqueous electrolyte in rechargeable cells |
Country Status (4)
| Country | Link |
|---|---|
| KR (1) | KR20010006797A (en) |
| CA (1) | CA2298792C (en) |
| IL (1) | IL136367A0 (en) |
| TW (1) | TW484245B (en) |
Families Citing this family (4)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| KR100863887B1 (en) * | 2007-06-21 | 2008-10-15 | 성균관대학교산학협력단 | Organic electrolyte for lithium-ion battery and lithium-ion battery comprising the same |
| KR101130726B1 (en) * | 2010-01-05 | 2012-03-28 | 성균관대학교산학협력단 | Electrolyte for lithium-ion battery and lithium-ion battery comprising the same |
| JP6520064B2 (en) | 2014-11-19 | 2019-05-29 | セントラル硝子株式会社 | Electrolyte for non-aqueous electrolyte battery and lithium non-aqueous electrolyte battery |
| KR20210031158A (en) * | 2019-09-11 | 2021-03-19 | 주식회사 엘지화학 | Non-aqueous electrolyte for lithium secondary battery and lithium secondary battery comprising the same |
-
2000
- 2000-02-11 CA CA002298792A patent/CA2298792C/en not_active Expired - Fee Related
- 2000-03-14 KR KR1020000012716A patent/KR20010006797A/en not_active Application Discontinuation
- 2000-04-17 TW TW089107149A patent/TW484245B/en active
- 2000-05-25 IL IL13636700A patent/IL136367A0/en unknown
Also Published As
| Publication number | Publication date |
|---|---|
| IL136367A0 (en) | 2001-06-14 |
| CA2298792A1 (en) | 2000-12-02 |
| KR20010006797A (en) | 2001-01-26 |
| TW484245B (en) | 2002-04-21 |
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Legal Events
| Date | Code | Title | Description |
|---|---|---|---|
| EEER | Examination request | ||
| MKLA | Lapsed | ||
| MKLA | Lapsed |
Effective date: 20060213 |