Patent Application
20100203370
The invention relates to a primary lithium cell having an anode preferably composed of lithium alloy and a cathode comprising iron disulfide.
Primary (non-rechargeable) electrochemical cells having an anode of lithium are known and are in widespread commercial use. The anode is comprised essentially of lithium metal. Such cells typically have a cathode comprising manganese dioxide, and electrolyte comprising a lithium salt such as lithium trifluoromethane sulfonate (LiCF3SO3) dissolved in an organic solvent. The cells are referenced in the art as primary lithium cells (primary Li/mnO2 cells) and are generally not intended to be rechargeable. Alternatively, primary lithium cells with lithium metal anodes but having different cathodes are also known. Such cells, for example, have cathodes comprising iron disulfide (FeS2) and are designated Li/FeS2 cells. The iron disulfide (FeS2) is also known as pyrite. The Li/MnO2 cells or Li/FeS2 cells are typically in the form of cylindrical cells, typically AA size or AAA size cells, but may be in other size cylindrical cells. The Li/MnO2 cells have a voltage of about 3.0 volts which is twice that of conventional Zn/MnO2 alkaline cells and also have higher energy density (watt-hrs per cm3 of cell volume) than that of alkaline cells. The Li/FeS2 cells have a voltage (fresh) of between about 1.2 and 1.8 volts which is about the same as a conventional Zn/MnO2 alkaline cell. However, the energy density (watt-hrs per cm3 of cell volume) of the Li/FeS2 cell is higher than a comparable size Zn/MnO2 alkaline cell. The theoretical specific capacity of lithium metal is high at 3861.4 mAmp-hr/gram and the theoretical specific capacity of FeS2 is 893.6 mAmp-hr/gram. The FeS2 theoretical capacity is based on a 4 electron transfer from 4Li per FeS2 molecule to result in reaction product of elemental iron Fe and 2Li2S. That is, 2 of the 4 electrons change the oxidation state of +2 for Fe+2 in FeS2 to 0 in elemental iron (Fe0) and the remaining 2 electrons change the oxidation state of sulfur from −1 in FeS2 to −2 in Li2S.
Overall the Li/FeS2 cell is much more powerful than the same size Zn/MnO2 alkaline cell. That is, for a given continuous current drain, particularly at higher current drain over 200 milliAmp, the voltage is flatter for longer periods for the Li/FeS2 cell than the Zn/MnO2 alkaline cell as may be evident in a voltage vs. time discharge profile. This results in a higher energy output obtainable from a Li/FeS2 cell compared to that obtainable for a same size alkaline cell. The higher energy output of the Li/FeS2 cell is more clearly and more directly shown in graphical plots of energy (Watt-hrs) versus continuous discharge at constant power (Watts) wherein fresh cells are discharged to completion at fixed continuous power outputs ranging from as little as 0.01 Watt to 5 Watt. (As the cell's voltage drops during discharge the load resistance is gradually decreased, raising the current drain to maintain a fixed constant power output.) The graphical plot Energy (Watt-Hrs) versus Power Output (Watt) for the Li/FeS2 cell is above that for the same size alkaline cell. This is despite that the starting voltage of both cells (fresh) is about the same, namely, between about 1.2 and 1.8 volt.
Thus, the Li/FeS2 cell has the advantage over same size alkaline cells, for example, AAA, AA, C or D size or any other size cell in that the Li/FeS2 cell may be used interchangeably with the conventional Zn/MnO2 alkaline cell and will have greater service life, particularly for higher power demands. Similarly the Li/FeS2 cell which is a primary (nonrechargeable) cell can also be used as a replacement for the same size rechargeable nickel metal hydride cell, which has about the same voltage (fresh) as the Li/FeS2 cell. Thus, the primary Li/FeS2 cell can be used to power digital cameras, which require operation at high pulsed power demands.
The cathode material for the Li/FeS2 cell may be initially prepared in a form such as a slurry mixture (cathode slurry), which can be readily coated onto the metal substrate by conventional coating methods. The electrolyte added to the cell must be a suitable organic electrolyte for the Li/FeS2 system allowing the necessary electrochemical reactions to occur efficiently over the range of high power output desired. The electrolyte must exhibit good ionic conductivity and also be sufficiently stable, that is non reactive, with the undischarged electrode materials (anode and cathode components) and also non-reactive with the discharge products. This is because undesirable oxidation/reduction side reactions between the electrolyte and electrode materials (either discharged or undischarged) could thereby gradually contaminate the electrolyte and reduce its effectiveness or result in excessive gassing. This in turn can result in a catastrophic cell failure. Thus, the electrolyte used in Li/FeS2 cell in addition to promoting the necessary electrochemical reactions, should also be stable to discharged and undischarged electrode materials. Additionally, the electrolyte should enable good ionic mobility and transport of the lithium ion (Li+) from anode to cathode so that it can engage in the necessary reduction reaction resulting in LiS2 product in the cathode.
An electrode composite is formed with a sheet of lithium, a sheet of cathode composite containing the FeS2 active material and separator therebetween. The electrode composite may be spirally wound and inserted into the cell casing, for example, as shown in the spirally wound lithium cell of U.S. Pat. No. 4,707,421. A cathode coating mixture for the Li/FeS2 cell is described in U.S. Pat. No. 6,849,360. A portion of the anode sheet is typically electrically connected to the cell casing which forms the cell's negative terminal. The cell is closed with an end cap which is insulated from the casing. The cathode sheet can be electrically connected to the end cap which forms the cell's positive terminal. The casing is typically crimped over the peripheral edge of the end cap to seal the casing's open end. The cell may be fitted internally with a PTC (positive thermal coefficient) device or the like to shut down the cell in case the cell is exposed to abusive conditions such as short circuit discharge or overheating.
The electrolyte used in a primary Li/FeS2 cells is formed of a “lithium salt” dissolved in an “organic solvent”. Representative lithium salts which may be used in electrolytes for Li/FeS2 primary cells are referenced in related art, for example, as in U.S. Pat. No. 5,290,414 and include such salts as: Lithium trifluoromethanesulfonate, LiCF3SO3 (LiTFS); lithium bistrifluoromethylsulfonyl imide, Li(CF3SO2)2N (LiTFSI); lithium iodide, LiI; lithium bromide, LiBr; lithium tetrafluoroborate, LiBF4; lithium hexafluorophosphate, LiPF6; lithium hexafluoroarsenate, LiAsF6; Li(CF3SO2)3C, and various mixtures. In the art of Li/FeS2 electrochemistry lithium salts are not always interchangeable as specific salts work best with specific electrolyte solvent mixtures, and specific solvent mixtures with certain lithium salts can lead to significantly improved performance.
In U.S. Pat. No. 5,290,414 (Marple) is reported use of a beneficial electrolyte for FeS2 cells, wherein the electrolyte comprises a lithium salt dissolved in a solvent comprising 1,3-dioxolane (DX) in admixture with a second solvent which is an acyclic (non cyclic) ether based solvent. The acyclic (non cyclic) ether based solvent as referenced may be dimethoxyethane (DME), ethyl glyme, diglyme and triglyme, with the preferred being 1,2-dimethoxyethane (DME). As given in the example the dioxolane and 1,2-dimethoxyethane (DME) are present in the electrolyte in substantial amount, i.e., 50 vol % 1,3-dioxolane (DX) and 40 vol % dimethoxyethane (DME) or 25 vol % 1,3-dioxolane (DX) and 75 vol. % dimethoxyethane (DME)(col. 7, lines 47-54). A specific lithium salt ionizable in such solvent mixture(s), as given in the example, is lithium trifluoromethane sulfonate, LiCF3SO3. Another lithium salt, namely lithium bistrifluoromethylsulfonyl imide, Li(CF3SO2)2N is also mentioned at col. 7, line 18-19. The reference teaches that a third solvent may optionally be added selected from 3,5-dimethylisoxazole (DMI), 3-methy-2-oxazolidone, propylene carbonate (PC), ethylene carbonate (EC), butylene carbonate (BC), tetrahydrofuran (THF), diethyl carbonate (DEC), ethylene glycol sulfite (EGS), dioxane, dimethyl sulfate (DMS), and sulfolane (claim 19), with the preferred being 3,5-dimethylisoxazole.
In U.S. Pat. No. 6,218,054 (Webber) is disclosed an electrolyte solvent system wherein dioxolane-based solvent and dimethoxyethane-based solvent are present in a weight ratio of about 1:3 (1 part by weight dioxolane to 3 parts by weight dimethoxyethane).
In U.S. Pat. No. 6,849,360 B2 (Marple) is disclosed an electrolyte for an Li/FeS2 cell, wherein the electrolyte comprises the salt lithium iodide dissolved in the organic solvent mixture comprising 1,3-dioxolane (DX), 1,2-dimethoxyethane (DME), and small amount of 3,5 dimethylisoxazole (DMI). (col. 6, lines 44-48.) This reference discloses an anode of lithium alloyed with aluminum.
In US 2007/0202409 A1 (Yamakawa) it is stated with reference to the electrolyte solvent for the Li/FeS2 cell at para. 33: “Examples of the organic solvent include propylene carbonate, ethylene carbonate, 1,2-dimethoxy ethane, γ-butyrolactone, tetrahydrofuran, 2-methyltetrahydrofuran, 1,3-dioxolane, sulfolane, acetonitrile, dimethyl carbonate, and dipropyl carbonate, and any one of them or two or more of them can be used independently, or in a form of a mixed solvent.” Such statement is misleading, since the art teaches only specific combinations of electrolyte solvents will be workable for the Li/FeS2 cell depending on the particular lithium salt to be dissolved in the solvent. (See, e.g. above U.S. Pat. No. 5,290,414 and U.S. Pat. No. 6,849,360) The reference Yamakawa does not teach which combination of solvents from the above list are to be used with any given lithium salt.
In U.S. 2006/0046152 (Webber) is disclosed an electrolyte system for a lithium cell which may have a cathode comprising FeS2 and FeS therein. The disclosed electrolyte contains lithium iodide salt dissolved in a solvent system comprising a mixture of 1,2-dimethoxypropane and 1,2-dimethoxyethane.
The choice of a particular organic solvent or mixture of different organic solvents for use in conjunction with any one or more lithium salts to produce a suitable electrolyte for the Li/FeS2 cell is challenging. This is not to say that the cell with various combinations of lithium salt and solvent mixtures may not work at all, but it may not work well enough to be practical. The challenge associated with such cells using an electrolyte formed with just any combination of lithium salt and known organic solvent suitable for dissolution and ionization of the salt is that the problems encountered will likely be very substantial, thus making the cell impractical for commercial usage. The history of development of lithium cells in general, whether lithium primary cells, e.g. non rechargeable Li/MnO2 or Li/FeS2 cells or rechargeable lithium or lithium ion cells reveals that just any combination of lithium salt and organic solvent cannot be expected to result in a good cell, that is, exhibiting good, reliable performance. Thus, references which merely provide long lists of possible organic solvents for Li/FeS2 cells do not necessarily teach combinations of solvents or combination of specific lithium salts in specific solvent mixtures, which exhibit particular or unexpected benefit.
Accordingly, it is desired to produce a Li/FeS2 cell employing an effective electrolyte therein which promotes ionization of the lithium salt in the electrolyte and is sufficiently stable that it does not degrade with time and does not degrade the anode or cathode components.
It is desired that the electrolyte comprising a lithium salt dissolved in an organic solvent provide for good ionic mobility of the lithium ions through the electrolyte so that the lithium ions may pass at good transport rate from anode to cathode through the separator.
It is desired to retard the formation of a deleterious passivation layer on the anode surface, which can interfere with obtaining best performance from the Li/FeS2 cell upon discharge.
It is desired to produce a primary (nonrechargeable) Li/FeS2 cell having good rate capability that the cell may be used in place of rechargeable batteries to power digital cameras.
The present invention is directed to a primary electrochemical cell having an anode comprising lithium metal, preferably a lithium alloy as anode active material and a cathode comprising iron disulfide (FeS2) as cathode active material. The cell is designated herein as a Li/FeS2 cell. It has been determined that there can be advantages in cell performance when the anode is composed of a lithium alloy instead of pure lithium metal.
The anode and cathode are typically spirally wound with a separator sheet therebetween to form an electrode assembly. An electrolyte solution is added to the cell after the wound electrode assembly is inserted into the cell casing. The electrolyte typically comprises a lithium salt dissolved in an organic solvent mixture. When the anode is composed of lithium alloy, a preferred electrolyte for the cell comprises a mixture of lithium iodide (LiI) salt dissolved in a mixture of dioxolane (DX) and dimethoxyethane (DME), preferably with small amount of component added to retard dioxolane polymerization. The lithium salt may be present in the electrolyte desirably at a concentration of between about 0.5 to 1.2 moles per liter, typically at about 0.8 moles per liter. A preferred electrolyte may be formed of a mixture of lithium iodide salt (0.5 to 1.2 moles per liter, typically about 0.8 moles per liter) in mixture with smaller amount lithium trifluoromethane sulfonate LiCF3SO3 (LiTFS) (between about 0.05 and 1 wt %, typically about 0.1 wt %) dissolved in the electrolyte solvent. The dioxolane is preferably 1,3-dioxolane. It shall be understood that the term dioxolane may include alkyl substituted dioxolanes. The preferred dimethoxyethane is 1,2-dimethoxyethane. The dioxolane and dimethoxyethane may be present in weight ratio of dioxolane to dimethoxyethane, for example, in a range between about 0.82 and 2.33. Typically, the solvent mixture comprises between about 50 and 90 percent by weight 1,3-dioxolane. A component which may be used to retard dioxolane polymerization may, for example, be 3,5-dimethylisoxazole, which can be added in amount between about 0.1 and 5 wt %, typically between about 0.1 and 1 percent by weight, for example, about 0.2 wt %, of the total electrolyte. Such component retards dioxolane polymerization and possibly also reacts with undesired materials in the cathode. Thus, when the Li/FeS2 cell anode (or at least the anode surface) is formed of a lithium alloy, a representative preferred electrolyte may be composed of a salt mixture of lithium iodide (0.8 moles per liter) and LiCF3SO3 (LiTFS) (about 0.1 wt %) dissolved in a solvent mixture of 1,3-dioxolane (DX) and 1,2-dimethoxyethane (DME) in weight ratio DX/DME of about 70/30 with about 0.2 wt % 3,5-dimethylisoxazole (DMI) added.
The anode may desirably be formed of lithium metal alloyed with small amounts of other metal, preferably metals or metal like elements from Groups IIA, IIIA, IVA of the periodic table, thus forming a lithium alloy. (The term alloy as used herein shall have its normal dictionary definition of a solid or liquid mixture of two or more metals or a solid or liquid mixture of metal with certain nonmetal. The term lithium alloy as used herein shall be understood to be a solid mixture or solid composite formed of a mixture of lithium metal and a smaller portion of other metal, typically other elemental metal or certain nonmetals.) For example, the lithium alloy may be formed of lithium metal alloyed with aluminum, calcium, barium, magnesium, tin, indium, gallium, tellurium. (Calcium and barium are technically classified as alkaline-earth elements.) The aluminum itself may be alloyed with common aluminum alloys such as magnesium, copper, and zinc. The lithium can be alloyed with two, three, or more metals. In some cases lithium can be alloyed with a metalloid (e.g. nonmetal or semiconductor component), for example silicon, germanium, or antimony. The lithium alloy can comprise lithium alloyed with one or more metalloids (nonmetal or semiconductor component), and one or more other metals. Small amount of elements alloyed with lithium preferably comprises less than about 1 or 2 wt. %, and even up to about 5 wt. % of the lithium alloy. The alloy element may comprise between about 0.05 and 5 wt %, for example, between about 0.1 and 5 wt %, typically between about 0.1 and 2 wt % of the lithium alloy. Typically, the alloy element or component will make up less than 0.5 wt % of the lithium alloy, if other elements are also in the lithium alloy. Thus, if other elements are also in the lithium alloy one of the alloy elements may comprise between about 0.05 and 0.5 wt %, for example, between about 0.1 and 0.5 wt % of the lithium alloy. The lithium alloy can be metallurgical in nature when the lithium alloy composition is uniform throughout the entire anode sheet. Alternatively, the lithium alloy may be plated or formed just on the surface of the lithium anode sheet. In that case the surface lithium alloy may be of different composition from the bulk of the anode, wherein the bulk of the anode may be of pure lithium (e.g. least 99.9% lithium) or of a different lithium alloy than the surface alloy. The anode may typically be in the form of a sheet or foil, usually intended to be wound.
Improvement in cell performance can be realized when the Li/FeS2 cell has an anode composed of lithium alloy instead of pure (e.g. 99.9 wt % pure lithium). Lithium is thermodynamically unstable when in contact with organic electrolyte (or electrolyte impurities). Therefore, an interface coating, termed solid electrolyte interface (SEI), can be gradually formed on the surface of the lithium in contact with the organic electrolyte during cell storage and discharge. The solid electrolyte interface (SEI) can interfere with achieving the rate of lithium oxidation needed during cell discharge, especially when the electrolyte contains traces of water. The formation of a deleterious solid electrolyte interface layer (passivation layer) on the lithium surface can thus noticeably interfere with achieving optimum cell performance. It has been determined that when the lithium is alloyed with other metals, even though the alloy metal may be present in small amount, e.g. less than about 5 wt %, typically less than about 2 wt %, the presence of the alloy metal can reduce the chemical activity of the lithium. This in effect reduces the tendency of the lithium to react with the organic electrolyte (or electrolyte impurities) in turn slowing the rate of formation of deleterious solid electrolyte interface (SEI) on the surface of the lithium anode. It is further theorized that the presence of the alloy metal may even effect the composition and nature of the solid electrolyte interface, rendering it less deleterious in impeding the rate of lithium oxidation during cell discharge. The studies herein reported show an advantage in employing a lithium-aluminum alloy instead of pure lithium metal for the anode of a Li/FeS2 cell for the indicated electrolyte. These studies have reinforced a theoretical basis for postulating that the lithium in the anode of Li/FeS2 cells may also be alloyed with other metals as herein described, to help obtain enhanced cell performance.
Another aspect of the invention, in which there is also disclosed herein common subject matter with commonly assigned U.S. Ser. No. 12/069,953 filed Feb. 14, 2008, is also directed to a primary electrochemical cell having an anode comprising lithium or lithium alloy as anode active material and a cathode comprising iron disulfide (FeS2) as cathode active material. The anode and cathode are typically spirally wound with a separator sheet therebetween to form an electrode assembly. An electrolyte solution is added to the cell after the wound electrode assembly is inserted into the cell casing. The electrolyte typically comprises a lithium salt dissolved in an organic solvent mixture. A preferred electrolyte solution may comprise a mixture of lithium iodide (LiI) salt dissolved in a mixture of dioxolane (DX), dimethoxyethane (DME) and sulfolane. The dioxolane is preferably 1,3-dioxolane. It shall be understood that the term dioxolane may include alkyl substituted dioxolanes. The preferred dimethoxyethane is 1,2-dimethoxyethane. Although sulfolane is a preferred solvent, other solvents with similarly high dielectric constant can be employed in place of sulfolane. Such solvents are propylene carbonate, ethylene carbonate, 3-methy-2-oxazolidone, γ-butyrolactone, dimethylsulfoxide, dimethylsulfite, ethylene glycol sulfite, acetonitrile, N-methylpyrrolidinone or combinations thereof. The application of an anode of lithium alloy can also be used advantageously with the above indicated electrolyte formulation which includes sulfolane.
In an aspect of the invention wherein sulfolane is one of the electrolyte solvents, the electrolyte comprises a lithium iodide salt dissolved in a solvent mixture comprising dioxolane, dimethyoxyethane, and sulfolane, wherein the weight ratio of dioxolane to dimethoxyethane is in a range between about 0.82 and 9.0, desirably between about 0.82 and 2.3. The dioxolane is preferably 1,3-dioxolane but may include alkyl substituted dioxolanes as well. The preferred dimethoxyethane is 1,2-dimethoxyethane, but other glymes also can be employed. The sulfolane content in the electrolyte formulation of the invention preferably comprises greater than about 4.8 wt % of the solvent mixture. Preferably, the sulfolane comprises between about 4.8 and 6.0 wt % of the solvent mixture. However, the sulfolane may also be present in higher amount, for example, up to about 25 wt % of the above indicated solvent mixture wherein the weight ratio of dioxolane to dimethoxyethane is in a range between about 0.82 and 9.0. The electrolyte also optionally includes 3,5-dimethylisoxazole (DMI) in amount between about 0.1 and 1 wt. % of the solvent mixture. (The dimethylisoxazole similar to other Lewis bases is helpful in retarding polymerization of dioxolane.) The lithium iodide is typically present in the solvent mixture at a concentration of about 0.8 moles per liter. The electrolyte has a viscosity desirably between about 0.9 and 1.5 centipoise.
The water content in the electrolyte of the invention for the Li/FeS2 cell may typically be less than about 100 parts water per million parts total electrolyte. However, based on favorable test results reported herein utilizing the electrolyte formulation of the invention, water content in the total electrolyte may be greater than 100 ppm. Also it is believed that water (deionized) may be added to the electrolyte solvents so that the water content in the electrolyte for the Li/FeS2 cell may be up to about 1000 ppm and even up to about 2000 ppm. (See commonly assigned patent application Ser. No. 12/009,858, Filed Jan. 23, 2008.) Thus, it is believed that the water content in the electrolytes herein presented may be between about 100 and 1000 ppm, for example, between about 200 and 1000 ppm, or between about 300 and 1000 ppm and up to about 2000 ppm. Specifically, when the anode of the Li/FeS2 cell is a formed of a lithium alloy (or at least the anode surface is formed of a lithium alloy) water may be added to the electrolytes herein presented so that the water content in the electrolyte may be between about 100 and 2000 ppm, for example, between about 200 and 1000 ppm, or between about 300 and 1000 ppm. Typically the water content may be between about 100 and 500 ppm, or between about 200 and 500 ppm, or between about 300 and 450 ppm.
In an aspect of the invention the Li/FeS2 cell has a cathode comprising the cathode active material iron disulfide (FeS2), commonly known as “pyrite”. The cell may be in the form of a button (coin) cell or flat cell. Desirably the cell may be in the form of a spirally wound cell comprising an anode sheet and a cathode composite sheet spirally wound with separator therebetween. The cathode sheet is produced using a slurry process to coat a cathode mixture comprising iron disulfide (FeS2) and carbon particles onto a substrate, preferably a conductive metal substrate. The FeS2 and carbon particles are bound to the substrate using desirably an elastomer, preferably, a styrene-ethylene/butylene-styrene (SEES) block copolymer such as Kraton G1651 elastomer (Kraton Polymers, Houston, Tex.). This polymer is a film-former, and possesses good affinity and cohesive properties for the FeS2 particles as well as for conductive carbon particle additives in the cathode mixture. The polymer resists chemical attack by the electrolyte.
The cathode is formed from a cathode slurry comprising iron disulfide (FeS2) powder, conductive carbon particles, binder material, and solvent. (The term “slurry” as used herein will have its ordinary dictionary meaning and thus be understood to mean a wet mixture comprising solid particles.) The wet cathode slurry is coated onto a substrate which is preferably conductive such as a sheet of aluminum or stainless steel. The substrate functions as a cathode current collector. The solvent is then evaporated leaving a cathode composite formed of a dry cathode coating mixture comprising the iron disulfide material and carbon particles preferably including carbon black adhesively bound to each other and with the dry coating bound, preferably to the both sides of the substrate. An electrode assembly is then formed comprising a sheet of lithium or lithium alloy, the cathode composite sheet, and separator therebetween. The electrode assembly is preferably spirally wound and inserted into the cell casing. The electrolyte solution is then poured into the cell casing and the cell crimped closed over an end cap.
The Li/FeS2 cell of the invention may be in the form of a flat button cell 100 or a spirally wound cell 10. A button (coin) cell 100 configuration for use as a testing cell comprises a lithium anode 150 and a cathode 170 comprising iron disulfide (FeS2) with separator 160 therebetween is shown in the
The Li/FeS2 cell as in cell 100 has the following basic discharge reactions (one step mechanism):
Anode:
4Li=4Li++4e− Eq. 1
Cathode:
FeS2+4Li++4e−=Fe+2Li2S Eq. 2
Overall:
FeS2+4Li=Fe+2Li2S Eq. 3
The Li/FeS2 button cell 100 shown in
A cathode current collector 115 comprising a metallic grid can be inserted into the cell so that it abuts the inside surface of the closed end 138 of the housing 130. The cathode current collector 115 may desirably be composed of a sheet of expanded stainless steel metal foil, having a plurality of openings therein, thus forming a stainless steel grid or screen. The expanded stainless steel metal foil is available as EXMET foil 316L-SS from Dexmet Corp. Preferably, however, the cathode current collector 115 is composed of a sheet of aluminum, which is more conductive. (The cathode current collector 115 may be a sheet of aluminum alloyed with common aluminum alloy metals such as magnesium, copper, and zinc.) Such aluminum current collector sheet 115 may also have a plurality of small openings therein, thus forming an aluminum grid. The cathode current collector 115 can be welded onto the inside surface of the closed end 138 of the housing 130. (Optionally, the same type of current collector grid, preferably of expanded stainless steel metal foil with openings therein, may be welded to the inside surface of the closed end of the anode cover 120.) An optional conductive carbon base layer 172 comprising a mixture of graphite and polytetrafluoroethylene (PTFE) binder can be compressed into the cathode current collector 115. The cathode material 170 comprising the FeS2 active particles may then be pressed into such conductive base layer 172. This may be termed a “staged” cathode construction.
The cathode material 170 comprising iron disulfide (FeS2) or any mixture including iron disulfide (FeS2) as active cathode material, may thus be inserted over optional conductive base layer 172 so that it overlies current collector sheet 115. The cathode active material, that is, the material undergoing useful electrochemical reactions, in cathode layer 170 can be composed entirely of iron disulfide (FeS2). The cathode 170 comprising iron disulfide (FeS2) powder dispersed therein can be prepared in the form of a slurry which may be coated on both sides of a conductive metal foil, preferably an aluminum or stainless steel foil. Such aluminum or stainless steel foil may have openings therethrough, thus forming a grid or screen. Alternatively, the cathode 170 comprising iron disulfide (FeS2) powder dispersed therein can be prepared in the form of a slurry which is coated on just the side of an aluminum or stainless steel foil facing separator 160. In either case a conductive base layer 172, as above described, may be employed in which case cathode 170 is inserted in the cell so that it overlies conductive base layer 172 as shown in
Alternatively, the cathode 170 comprising iron disulfide (FeS2) powder dispersed therein can be prepared in the form of a slurry which may be coated directly onto a conductive substrate sheet 115 to form a cathode composite. Preferably conductive substrate sheet 115 is formed of a sheet of aluminum (or aluminum alloy), as above described, and may have a plurality of small apertures therein, thus forming a grid. Alternatively, the conductive substrate sheet 115 may be a sheet of stainless steel, desirably in the form of expanded stainless steel metal foil, having a plurality of small apertures therein.
The cathode slurry comprises 2 to 4 wt % of binder (Kraton G1651 elastomeric binder from Kraton Polymers, Houston Tex.); 50 to 70 wt % of active FeS2 powder; 4 to 7 wt % of conductive carbon (carbon black and graphite); and 25 to 40 wt % of solvent(s). (The carbon black may include in whole or in part acetylene black carbon particles. Thus, the term carbon black as used herein shall be understood to extend to and include carbon black and acetylene black carbon particles.) The Kraton G1651 binder is an elastomeric block copolymer (styrene-ethylene/butylene (SEBS) block copolymer) which is a film-former. This binder possesses sufficient affinity for the active FeS2 and carbon black particles to facilitate preparation of the wet cathode slurry and to keep these particles in contact with each other after the solvents are evaporated. The FeS2 powder may have an average particle size between about 1 and 100 micron, desirably between about 10 and 50 micron. A desirable FeS2 powder is available under the trade designation Pyrox Red 325 powder from Chemetall GmbH, wherein the FeS2 powder has a particle size sufficiently small that of particles will pass through a sieve of Tyler mesh size 325 (sieve openings of 0.045 mm). (The residue amount of FeS2 particles not passing through the 325 mesh sieve is 10% max.) The graphite is available under the trade designation Timrex KS6 graphite from Timcal Ltd. Timrex graphite is a highly crystalline synthetic graphite. (Other graphites may be employed selected from natural, synthetic, or expanded graphite and mixtures thereof, but the Timrex graphite is preferred because of its high purity.) The carbon black is available under the trade designation Super P conductive carbon black (BET surface area of 62 m2/g) from Timcal Co.
The solvents preferably include a mixture of C9-C11 (predominately C9) aromatic hydrocarbons available as ShellSol A100 hydrocarbon solvent (Shell Chemical Co.) and a mixture of primarily isoparaffins (average M.W. 166, aromatic content less than 0.25 wt. %) available as ShellSol OMS hydrocarbon solvent (Shell Chemical Co.). The weight ratio of ShellSol A100 to ShellSol OMS solvent is desirably at a 4:6 weight ratio. The ShellSol A100 solvent is a hydrocarbon mixture containing mostly aromatic hydrocarbons (over 90 wt % aromatic hydrocarbon), primarily C9 to C11 aromatic hydrocarbons. The ShellSol OMS solvent is a mixture of isoparaffin hydrocarbons (98 wt. % isoparaffins, M.W. about 166) with less than 0.25 wt % aromatic hydrocarbon content. The slurry formulation may be dispersed using a double planetary mixer. Dry powders are first blended to ensure uniformity before being added to the binder solution in the mixing bowl.
A preferred cathode slurry mixture is presented in Table 1:
The wet cathode slurry 170 is applied to the current collector 115 using intermittent roll coating technique. This same or similar wet cathode slurry mixture (electrolyte not yet added to the cell) is disclosed in commonly assigned application Ser. No. 11/516,534, filed Sep. 6, 2006. The total solids content of the wet cathode slurry mixture 170 as shown in above Table 1 is 66.4 wt. %. Thus, the acetylene black content in the dry cathode would be 2.26 wt. % and the graphite content in the dry cathode would be 6.02 wt. %.
As above indicated current collector sheet 115 is optionally precoated with a carbon base layer 172 before the wet cathode slurry is applied. The cathode slurry coated on the metal substrate 115 is dried gradually adjusting or ramping up the temperature from an initial temperature of 40° C. to a final temperature of about 130° C. in an oven until the solvent has all evaporated. (Drying the cathode slurry in this manner avoids cracking.) This forms a dry cathode coating 170 comprising FeS2, carbon particles, and binder on the metal substrate 115. The coated cathode is then passed between calendering rolls to obtain the desired cathode thicknesses. A representative desirable thickness of dry cathode coating 170 is between about 0.172 and 0.188 mm, preferably about 0.176 mm. The dry cathode coating 170 thus has the following desirable formulation: FeS2 powder (89 wt. %); Binder (Kraton G1651), 3 wt. %; Graphite (Timrex KS6), 6 wt. %, and Carbon Black (Super P), 2 wt %. The carbon black (Super P carbon black) develops a carbon network which improves conductivity.
The cathode composite comprising current collector sheet 115, cathode base layer 172, and dry cathode coating 170 thereon may then be inserted into cathode housing 130. A separator sheet 160 preferably comprising a microporous polypropylene may then be inserted over the cathode coating 170.
The electrolyte for the Li/FeS2 cell may then be added so that it fully penetrates through separator sheet 160 and cathode layer 170. An electrolyte mixture can be added so that it becomes absorbed into the separator and cathode coating. The electrolyte comprises a lithium salt or mixture of lithium salts dissolved in an organic solvent. The electrolyte mixture is desirably added on the basis of about 4 gram electrolyte solution per gram FeS2 facing the anode.
The electrolyte of the invention for the above cell comprises a lithium iodide salt dissolved in a solvent mixture comprising dioxolane, dimethyoxyethane, and sulfolane, wherein the weight ratio of dioxolane to dimethoxyethane is in a range between about 0.82 and 9.0, desirably between about 0.82 and 2.3. The dioxolane is preferably 1,3-dioxolane but may include alkyl-substituted dioxolanes as well. The preferred dimethoxyethane is 1,2-dimethoxyethane. The sulfolane preferably comprises greater than about 4.8 wt % of the solvent mixture. Preferably, the sulfolane comprises between about 4.8 and 6.0 wt % of the solvent mixture. The electrolyte has a viscosity desirably between about 0.9 and 1.5 centipoise.
A layer of anode material 150, typically a sheet of lithium or lithium alloy may then be placed over separator sheet 160. The anode cover 120, formed preferably from nickel-plated steel, is inserted into open end 132 of housing 130 and peripheral edge 135 of housing 130 is crimped over the exposed insulator edge 142 of insulating member 140. The peripheral edge 135 bites into insulator edge 142 closing housing 130 and tightly sealing the cell contents therein. The anode cover 120 also functions as the negative terminal of the cell and housing 130 at the closed end 138 functions as the positive terminal of the cell.
Experimental test Li/FeS2 coin cells 100 (
A coin shaped cathode housing 130 of nickel plated steel and a coin shaped anode housing (cover) 120 of nickel plated steel is formed of a similar configuration shown in
In forming each cell 100, an Arbor press with a 0.780-inch die was used to punch out two stainless steel grids (316L-SS EXMET expanded metal foil). One stainless steel grid was centered inside of coin cell cathode housing 130 forming cathode current collector sheet 115. The other stainless steel grid (not shown) was resistance welded to the inside surface of closed end of the anode housing (cover) 120. The grids were welded to their respective housings using a Hughes opposing tip tweezers welder. The welder was set at 20 watts-seconds and a medium pulse. The welds that were formed were evenly spaced around the perimeters of the grids over intersecting points of mesh strands. For each cell, six to eight welds were formed per grid. Anode 150 used in experimental cells was made out of pure lithium metal foil having thickness about 0.03 inches (0.76 mm).
A plastic insulating disk (grommet) 140 was then attached to the edge of anode cover 120 (
A microporous polypropylene separator 160 (Celgard CG2400 separator from Celgard, Inc.) was cut into eight-inch strips and punched out using a hand punch having a diameter of 0.9375 inch and set aside.
Cathode conductive base layer 172 was prepared as follows:
Add 75 g of graphite (Timrex KS6 graphite) and 25 g of tetrafluoroethylene (Teflon) powder to a tumbler (with weights) and let run overnight in hood. Add contents to a blender (˜10 g at a time) and blend on high for 1 minute. Pour blended contents into a container, label, and store until ready for use. When ready for application of cathode base layer 172, the cathode housing 130 was placed in a die. The cathode base layer 172 (0.500 g) was impacted onto a stainless steel grid 115 by using a ram connected to a Carver hydraulic press. The cathode base layer 172 had the composition 75 wt. % graphite and 25% Teflon powder.
A cathode slurry was then prepared and coated over both sides of an aluminum sheet (not shown). The components of the cathode slurry comprising iron disulfide (FeS2) were mixed together in the following proportion:
FeS2 powder (58.9 wt. %); Binder, styrene-ethylene/butylene-styrene elastomer (Kraton G1651)(2 wt. %); Graphite (Timrex KS6) (4.0 wt %), Carbon Black (Super P carbon black) (1.5 wt %), Hydrocarbon Solvents, ShellSol A100 solvent (13.4 wt %) and ShellSol OMS solvent (20.2 wt %).
The wet cathode slurry on the aluminum sheet (not shown) was then dried in an oven between 40° C. and 130° C. until the solvent in the cathode slurry all evaporated, thus forming a dry cathode coating 170 comprising FeS2, conductive carbon and elastomeric binder on a side of the aluminum sheet. The aluminum sheet carrying cathode coating 170 was an aluminum foil of 20 micron thickness. The same composition of wet cathode slurry was then coated onto the opposite side of the aluminum sheet and similarly dried. The dried cathode coatings on each side of the aluminum sheet was calendered to form a dry cathode 170 having a total final thickness of about 0.176 mm, which includes the 20 micron thick aluminum foil. The dry cathode coating 170 had the following composition:
FeS2 powder (88.71 wt. %); Binder Kraton G1651 elastomer (3.01 wt. %); conductive carbon particles, graphite Timrex KS6 (6.02 wt. %) and carbon black, Super P (2.26 wt %).
The composite of the dry cathode coating 170 coated on both sides of the aluminum sheet was then die punched into the cathode housing 130 onto carbon base layer 172. This was done by placing cathode housing 130 within a die. A cut to size composite of aluminum sheet coated on both sides with dry cathode coating 170 was then aligned directly over cathode base layer 172 within housing 130. A ram was then inserted into the die holding housing 130, and the die was moved to a hydraulic press. Four metric tons of force was applied using the press to punch the composite into the cathode housing 130 so that it was impacted against cathode base layer 172. The die was then inverted and the housing 130 gently removed from the die. The surface of the exposed cathode layer 170 had a smooth, consistent texture. The finished cathode coin was then placed in a vacuum oven and was heated at 150° C. for 16 hours.
A Control Cell Group and Test Cell Group of button (coin) cells 100 were made as described above. The control group of cells had the following electrolyte:
Control Cell Group with Control Electrolyte:
Lithium bistrifluoromethylsulfonyl imide, Li(CF3SO2)2N referenced herein as LiTFSI, yielding a concentration of 0.8 moles/liter was dissolved in a solvent mixture comprising 1,3-dioxolane (DX) (80 vol %), sulfolane (20 vol %), and pyridine (PY) 800 ppm. The electrolyte contained less than 50 parts by weight water per million parts by weight (ppm) electrolyte.
The cells of first test group, that is, Test Cell Group I were identical (including the control cells) in construction and anode/cathode composition (coin cells 100) except that different electrolyte formulation was used in Test Cell Group I compared to the Control Cell Group. The Test Cell Group I of coin cells 100 had the following different electrolyte formulation of the invention:
Test Cell Group I With Electrolyte Formulation I:
Electrolyte Formulation I: Lithium iodide (LiI) yielding a concentration of 0.8 moles/liter was dissolved in a solvent mixture comprising 1,3-dioxolane (DX) (42.6 wt %), 1,2-dimethoxyethane (DME) (52.1 wt %), and sulfolane (5.3 wt %). The solvent mixture also contained 3,5-dimethylisoxazole (DMI) (0.2 wt %). The cells were made with water content in the total electrolyte of about 120 parts by weight water per million parts by weight electrolyte (ppm) as a result of adding deionized water to the solvent mixture.
The cells of second test group, namely Test Cell Group II were identical to Test Cell Group I and the Control cells except that different electrolyte formulation was used in Test Cell Group II. The Test Cell Group II was made with the following different electrolyte formulation of the invention:
Test Cell Group II With Electrolyte Formulation II:
Electrolyte Formulation II: Lithium iodide (LiI) yielding a concentration of 0.8 moles/liter was dissolved in a solvent mixture comprising 1,3-dioxolane (DX) (66.5 wt %), 1,2-dimethoxyethane (DME) (28.5 wt %), and sulfolane (5.0 wt %). The solvent mixture also contained 3,5-dimethylisoxazole (DMI) (0.2 wt %). The cells were made with water content in the total electrolyte of about 270 parts by weight water per million parts by weight electrolyte (ppm) by adding deionized water to the solvent mixture.
Thus, the electrolyte for all cells, that is Control Cells and Test Cell Group in Experiment 2 was: Lithium iodide (LiI) yielding a concentration of 0.8 moles/liter was dissolved in a solvent mixture comprising 1,3-dioxolane (DX) (42.6 wt %), 1,2-dimethoxyethane (DME) (52.1 wt %), and sulfolane (5.3 wt %). The solvent mixture also contained 3,5-dimethylisoxazole (DMI) (0.2 wt %). The cells were made with water content in the total electrolyte of about 120 ppm by adding deionized water to the solvent mixture. Enough electrolyte was added to saturate the separator 160 and cathode 170.
Predischarge (Limited Drain) Protocol For Experiment #1 Cells (Control Group Cells, Test Cell Group I, and Test Cell Group II):
All fresh cells for Experiment #1, that is, the Control Cell Group, Test Cell Group I and Test Cell Group II of Experiment #1 were subjected to the following predischarge schedule. The predischarged schedule was a series 27 discharge pulse cycles, where each pulse cycle consisted of a pulse at 35 mAmp for 7 seconds, followed by an intermittent pulse rest of 22 seconds. This predischarge schedule was applied within about one day after the fresh coin cells 100 was made. Thus, the term “predischarge protocol” as it is used herein is a limited drain protocol which is applied to the cell soon after the fresh cell is made, namely, within about one day after the cell is made. Thus the predischarge (limited drain) protocol is applied within about one day after the fresh cell is made and before the cell is made available for commercial usage.
Predischarge (Limited Drain) Protocol For Experiment #2 Control Group of Cells:
Fresh control cells were predischarged per schedule described above: This predischarge schedule was a series 27 discharge pulse cycles, where each pulse cycle consisted of a pulse at 35 mAmp for 7 seconds, followed by an intermittent pulse rest of 22 seconds. This predischarge schedule was applied within about one day after the fresh coin cells 100 was made.
Fresh Test Cells of Experiment #2 were predischarged by constant current of 0.6 mAmp for 3 hours to remove about the same capacity (mAmp-hrs) as was removed by pulse predischarge schedule for the control cells. This predischarge schedule was applied within about one day after the fresh coin cells 100 was made.
After subjecting fresh cells to the above indicated respective predischarge protocols, each of the cell groups, namely, the Control Cell Group of Experiment #1, and Control Cell Group of Experiment #2 as well as all Test Cells for Experiment #1 and all Test Cells of Experiment #2 were subjected to accelerated storage (5 days at 60° C.).
The Control Cell Group and Test Cell Group of Experiment #2 after accelerated storage were subjected to complex impedance measurements. Both control cells and test cells had same electrolyte as above indicated in description of Experiment #2, namely:
Lithium iodide (LiI) yielding a concentration of 0.8 moles/liter was dissolved in a solvent mixture comprising 1,3-dioxolane (DX) (42.6 wt %), 1,2-dimethoxyethane (DME) (52.1 wt %), and sulfolane (5.3 wt %). The solvent mixture also contained 3,5-dimethylisoxazole (DMI) (0.2 wt %). The cells were made with water content in the total electrolyte greater than 100 parts by weight water per million parts by weight electrolyte (ppm).
Complex impedance of each coin cell was measured by using Solartron Electrochemical Interface 1287 with Frequency Response Analyzer 1255. This measurement allows the calculation of the resistance of the lithium passive layer. The cell's impedance reflects the internal resistance of the cell and thus the resistance of the lithium passivation layer.
All the cells as described in above Experiments 1 and 2 were subjected to the digital camera accelerated simulation test which consisted of the following pulsed test protocol: Each pulsed cycle consisted of: 2 intermediate cycles consisting of both a 26 milliWatt pulse for 2 seconds followed immediately by a 12 milliWatt pulse for 28 seconds. These pulsed cycles were repeated until a cut off voltage of 1.05 Volt is reached.
Discharge of the cells was performed on Maccor 4000 cycling equipment. The cells were discharged to the same cut off voltage of 1.05 volts using the above indicated digital camera accelerated simulation discharge test. The test results are reported as follows:
The following are the mean average pulsed cycles achieved for the Experiment #1 Control Cell Group, Test Cell Group I and Test Cell Group II as the cells were discharged to 1.05 with the above described digital camera simulation test. These cells were all discharged after being subjected to above described predischarge and accelerated storage protocols for the Experiment #1 cells. (Each cell group was made up of about 5 to 7 cells.)
Control Cell Group: 540.7 pulsed cycles (mean average) to 1.05 Volt cut off.
Test Cell Group I: 582.8 pulsed cycles (mean average) to 1.05 Volt cut off.
Test Cell Group II: 569.4 pulsed cycles (mean average) to 1.05 Volt cut off.
The following are the mean average pulsed cycles achieved for the Experiment #2 Control Cell Group and Test Cell Group as the cells were discharged to 1.05 with the above described digital camera simulation test. These cells were all discharged after being subjected to above described predischarge and accelerated storage protocols for the Experiment #2 cells. (Each cell group was made up of 6 to 7 cells.)
Control Cell Group: 582.8 pulsed cycles (mean average) to 1.05 Volt cut off.
Test Cell Group: 555.6 pulsed cycles (mean average) to 1.05 Volt cut off.
Resistance of the lithium anode passive layer is reflected by the cell impedance measurements, which is a measure of the cell's internal resistance. The cell impedance was recorded as follows for the Experiment #2 cells:
Control Cell Group: Impedance—Resistance of Anode Passive Layer: 5.8 Ohms (mean impedance); number of pulsed cycles in digital camera accelerated simulation discharge test 582.8 (mean average) to 1.05 V cut off.
Test Cell Group: Impedance—Resistance of Anode Passive Layer for Test Cell Group 24.8 Ohms; number of pulsed cycles in digital camera accelerated simulation discharge test 555.6 to 1.05 V cut off.
In Experiment #1 the test results indicate better discharge performance (accelerated discharge simulation test) for the Test Cell Groups I and II compared to the Control Cell Group. As above indicated the Control Cell Group as well as both Test Cell Groups I and II were subjected to the same predischarge (limited drain) protocol and same accelerated storage protocol. The mean pulsed cycles for Test Cell Group I and Test Cell Group II were 582.8 pulsed cycles and 569.4 pulsed cycles to 1.05 volt cutoff compared to the Control Cell Group which had a mean of 540.7 pulsed cycles to 1.05 volt cutoff. Both test cell groups (Test Cell Group I and II) had high water content in the electrolyte, namely greater than 100 ppm water in the electrolyte compared to the control cells which had less than 50 ppm water. Nevertheless, the test cells showed better discharge performance than the control cells as the cells were subjected to the accelerated discharge simulation test.
Thus, it would appear that the electrolyte formulation in Test Cell Groups I and II in Experiment #1, namely, Electrolyte Formulation I and Electrolyte Formulation II, respectively was a more effective electrolyte than the control electrolyte.
The Electrolyte Formulation I was as follows: Lithium iodide (LiI) yielding a concentration of 0.8 moles/liter dissolved in a solvent mixture comprising 1,3-dioxolane (DX) (42.6 wt %), 1,2-dimethoxyethane (DME) (52.1 wt %), and sulfolane (5.3 wt %). The solvent mixture also contained 3,5-dimethylisoxazole (DMI) (0.2 wt %). The Electrolyte Formulation II comprised 1,3-dioxolane (DX) (66.5 wt %), 1,2-dimethoxyethane (DME) (28.5 wt %) and sulfolane (5.0 wt %). The solvent mixture also contained 3,5-dimethylisoxazole (DMI) (0.2 wt %). The Electrolyte Formulations I and II also contained greater than 100 parts by weight water per million parts by weight electrolyte (ppm). Specifically, deionized water was added to the electrolyte Formulations I and II so that the water content in Electrolyte Formulation I was 120 ppm water and the water content in Electrolyte Formulation II was 270 ppm water. By contrast the electrolyte in the control cells was comprised of a mixture of LiTFSI salt dissolved in a solvent mixture comprising 1,3-dioxolane (DX) and sulfolane with less than 50 ppm water present. The above electrolyte formulation I and II comprising 1,3-dioxolane (DX) (42-67 wt %), 1,2-dimethoxyethane (DME) (28-52 wt %), and sulfolane (5-6 wt %) may be more effective as a result of better mass transport properties of the electrolyte mixture as a whole. It is possible that the added water in these electrolyte formulations resulting in a water content of greater than 100 ppm water may also be contributing to the improved conductivity of the electrolyte, thereby, helping to achieve the better cell discharge performance.
In Experiment #2 the electrolyte in both control cell group and test cell group were the same, namely, lithium iodide (LiI) yielding a concentration of 0.8 moles/liter dissolved in a solvent mixture comprising 1,3-dioxolane (DX) (42.6 wt %), 1,2-dimethoxyethane (DME) (52.1 wt %), and sulfolane (5.3 wt %), and also 3,5-dimethylisoxazole (DMI) (0.2 wt %). The cells were made with water content in the total electrolyte was about 120 parts by weight water per million parts by weight electrolyte (ppm).
The test results with respect to Experiment #2 cells indicate that the pulsed predischarge (pulsed limited drain) protocol employed with respect the fresh control cells, reduces the buildup of deleterious passivation layer on the lithium anode compared to the same fresh cells with same electrolyte, namely the test cell group, which was only subjected to a constant current predischarge protocol removing the same amount of cell capacity. This beneficial effect of the pulsed predischarge (pulsed limited drain) protocol is reflected in the above experimental data, wherein the internal impedance (resistance of the anode passivation layer) for the control cells subjected to pulsed predischarge was only 5.8 ohm, which was much lower compared to the test cells subjected to constant current predischarge, wherein the average impedance was 24.8 ohm. (The predischarge protocol also reduces the tendency for the cell's OCV (open cell voltage) to rise soon after, that is, within about one day after the cell is made.) It is inferred from the data that the presence of water in the control cells electrolyte (>100 ppm water in the total electrolyte) in combination with subjecting these cells to a pulsed predischarge protocol helps to achieve lower anode passive layer resistance. It is conjectured that the pulsed predischarge protocol in combination with the presence of water in the electrolyte in the control cells may result in a change in composition of the passive layer or retard its rate of buildup, thereby reducing the passive layer resistance in these cells. The net result is better cell discharge performance, which is verified by the higher number of pulsed cycles obtained for the control cells (mean average 582.8) than the test cells (mean average 555.6) as measured to 1.05 volt cutoff.
The cylindrical cell 10 may have a spirally wound electrode assembly 70 (
For a spirally wound cell, a preferred shape of the cell casing (housing) 20 is cylindrical as shown in
The electrode composite 13 (
The wet cathode slurry mixture having the composition shown above in Table 1 comprising iron disulfide (FeS2), binder, conductive carbon and solvents is prepared by mixing the components shown in Table 1 until a homogeneous mixture is obtained.
The above quantities of components (Table 1) of course can be scaled proportionally so that small or large batches of cathode slurry can be prepared. The wet cathode slurry thus preferably has the following composition: FeS2 powder (58.9 wt. %); Binder, Kraton G1651 (2 wt. %); Graphite, Timrex KS6 (4.0 wt %), Acetylene Black, Super P (1.5 wt %), Hydrocarbon Solvents, ShellSol A100 (13.4 wt %) and ShellSol OMS (20.2 wt %).
The FeS2 powder (Pyrox Red 325) may be used directly as obtained from the supplier, Chemetall GmbH. Such product may be obtained from the supplier with a CaCO3 additive already mixed into the FeS2 powder. The CaCO3 may typically comprise up to 1.5 wt. % of the FeS2 powder. The CaCO3 (or CaCO3 containing compound) is added by the supplier to raise the pH of the FeS2 in order to extend its storage life. That is, the elevated pH of FeS2 resulting from the addition of CaCO3 is intended to retard the rate of buildup of acidic contaminants within or on the surface of the FeS2 particles as the FeS2 is exposed to or stored in ambient air.
When it is desired to prepare the wet cathode slurry, the premix of FeS2 powder and acetylene carbon black, is removed from storage and readied for admixture with binder and solvent solution. The mixture is stirred with graphite, binder and solvent as above described until a homogenous mixture is obtained, thus forming the wet cathode slurry.
After the wet cathode slurry is formed (Table 1), the wet slurry is then coated onto a side of the conductive substrate 65. The conductive substrate 65 with wet cathode slurry coated thereon is then dried in conventional convective oven (or in inert gas) to evaporate the solvents in the slurry, thereby forming a dry cathode coating 60 on one side of conductive substrate 65 (
The anode 40 can be prepared from a solid sheet of lithium metal (typically 99.8% pure). However, the lithium metal in anode 40 may be alloyed with small amounts of other metal, preferably metals or metal like elements from Groups IIA, IIIA, IVA of the periodic table, thus forming a lithium alloy. For example, the lithium alloy may be formed of lithium metal alloyed with aluminum, calcium, barium, magnesium, tin, indium, gallium, tellurium, bismuth. The aluminum itself may be alloyed with common aluminum alloys such as magnesium, copper, and zinc. The lithium can be alloyed with two, three, or more metals. In some cases lithium can be alloyed with metalloid (e.g. nonmetal or semiconductor component), for example silicon, germanium, or antimony. The lithium alloy can comprise lithium alloyed with one or more metalloids (nonmetal or semiconductor component), and one or more other metals. Small amount of elements alloyed with lithium preferably comprises less than about 1 or 2 wt. %, and even up to about 5 wt. % of the lithium alloy. The alloy element may comprise between about 0.05 and 5 wt %, for example, between about 0.1 and 5 wt %, typically between about 0.1 and 2 wt % of the lithium alloy. Typically, the alloy element or component will make up less than 0.5 wt % of the lithium alloy, if other elements are also in the lithium alloy. Thus, if other elements are also in the lithium alloy, one of the alloy elements may comprise between about 0.05 and 0.5 wt %, for example between about 0.1 and 0.5 wt % of the lithium alloy. The lithium alloy can be metallurgical in nature when the lithium alloy composition is uniform throughout the entire anode sheet.
Alternatively, the lithium alloy may be plated or formed just on the surface of the lithium anode sheet. In that case the surface lithium alloy may be of different composition than the bulk of the anode, wherein the bulk of the anode may be of pure lithium metal or of a different lithium alloy. The anode may typically be in the form of a sheet or foil, usually intended to be wound.
Since the metal or component which may be alloyed with lithium to form anode 40 is generally of small amount, as above indicated, the lithium alloy upon cell discharge functions electrochemically essentially as pure lithium. The lithium sheet forming anode 40 does not require a substrate. The lithium anode 40 can be advantageously formed from an extruded sheet of lithium metal having a thickness of between about 0.09 and 0.20 mm desirably between about 0.09 and 0.19 mm for the spirally wound cell.
For an AA size Li/FeS2 cell 10 there may typically be between about 4.5 and 5.0 grams of cathode active material, e.g. FeS2 in the cathode. The amount of anode active material, namely, lithium or lithium alloy is determined by balancing the cell based on its theoretical capacity. In general the theoretical capacity of the anode involves computing the ideal capacity (mAmp-hrs) of all the anode active materials therein, and the theoretical capacity of the cathode involves computing the ideal capacity (mAmp-hrs) of all the cathode active materials therein. It shall be understood that the use of such terms theoretical capacity of anode and theoretical capacity of cathode as used in the present application shall be so defined. The “anode active” materials and “cathode active” materials are defined as the materials in the anode and cathode, respectively, which are capable of useful electrochemical discharge. (Only those portions of the anode and cathode with separator therebetween are considered.) That is, the “anode active materials” and “cathode active materials” promote current flow between the cell's negative and positive terminals when an external circuit between these terminals is connected and the cell is used in normal manner. In a wound cylindrical cell 10 wherein the anode active material is lithium metal (or lithium alloy) and the cathode active material is FeS2 the theoretical specific capacity of the anode may be based on lithium at 3861.4 mAmp-hrs/g and the theoretical specific capacity of the cathode may be based on FeS2 at 893.5 mAmp-hrs/g. The wound cylindrical cell 10 utilizing the electrolyte formulation of the invention may be balanced so that either the theoretical capacity (mAmp-hrs) of the anode or cathode is in excess or both are the same.
Individual sheets of electrolyte permeable separator material 50, preferably of microporous polypropylene or polyethylene having a thickness of about 0.025 mm or less (0.020 mm, 0.016 mm, or 0.012 mm) is inserted on each side of the lithium anode sheet 40 (
When the winding is completed separator portion 50b appears within the core 98 of the wound electrode assembly 70 as shown in
The electrolyte can be added to the cell casing after the wound electrode spiral 70 is inserted. The electrolyte typically comprises a lithium salt dissolved in an organic solvent mixture. The electrolyte mixture may be added typically on the basis of about 0.4 gram electrolyte solution per gram FeS2 for the spirally wound cell (
When the Li/FeS2 cell anode (or at least the anode surface) is formed of a lithium alloy, a representative preferred electrolyte may be composed of a salt mixture of lithium iodide (0.8 moles per liter) and LiCF2SO2 (LiTFS) (about 0.1 wt %) dissolved in a solvent mixture of 1,3-dioxolane (DX) and 1,2-dimethoxyethane (DME) in weight ratio DX/DME of about 70/30 with about 0.2 wt % 3,5-dimethylisoxazole (DMI) added.
The water content in the electrolyte of the invention for the wound cell 10 may typically be less than about 100 parts water per million parts total electrolyte. However, it is believed that water (deionized) may be added to the electrolyte solvents so that the water content in the electrolyte may be up to about 1000 ppm and even up to about 2000 ppm. (See commonly assigned patent application Ser. No. 12/009,858, filed Jan. 23, 2008.) Thus, it is believed that the water content in the electrolytes herein presented may be between about 100 and 1000 ppm, for example, between about 200 and 1000 ppm, or between about 300 and 1000 ppm and up to about 2000 ppm, for example, between about 300 and 2000 ppm.
Specifically, when the anode of the Li/FeS2 cell is a formed of a lithium alloy (or at least the anode surface is formed of a lithium alloy) water may be added to the electrolytes herein presented so that the water content in the electrolyte may be between about 100 and 2000 ppm, for example, between about 200 and 1000 ppm, or between about 300 and 1000 ppm. Typically the water content may be between about 100 and 500 ppm, or between about 200 and 500 ppm, or between about 300 and 450 ppm.
An end cap 18 forming the cell's positive terminal 17 may have a metal tab 25 (cathode tab) which can be welded on one of its sides to inside surface of end cap 18. Metal tab 25 is preferably of aluminum or aluminum alloy. A portion of the cathode substrate 65 extends into portion 64 extending from the top of the wound spiral as shown in
A metal tab 44 (anode tab), preferably of nickel, or nickel plated steel, can be pressed into a portion of the lithium metal anode 40. Anode tab 44 can be pressed into the lithium metal at any point within the spiral, for example, it can be pressed into the lithium metal at the outermost layer of the spiral as shown in
The primary lithium cell 10 may optionally also be provided with a PTC (positive thermal coefficient) device 95 located under the end cap 18 and connected in series between the cathode 60 and end cap 18 (
The following is an example showing a comparison in Digicam Test Results and Cell Impedance (Internal Resistance) between a control AA size wound Li/FeS2 cell and test AA size Li/FeS2 wound cell. The control cells had an anode of lithium metal and the test cells had an anode of lithium alloyed with aluminum (1500 ppm aluminum). (The water content in the control and test cells were at least 350 ppm water.)
Test AA size cylindrical cells were made in accordance with the preceding description and are representative of a specific embodiment of the invention. Three Groups B,C, and D of cells were tested. The control cells in each case was the cell Group B which had an anode sheet 40 of lithium metal and the test cells group C and D all had a lithium anode sheet 40 of lithium alloyed with 1500 ppm aluminum. The electrolyte for each group of cells was the same except that the Groups B and C had 350 ppm water added to the electrolyte and the D cells had 425 ppm water added to the electrolyte. The cells otherwise had the same contents and the made according to the same specifications.
The AA cells were all identical and made according to the following specifications.
The cathode was coated in the form of a wet cathode slurry as earlier described herein onto both sides of an aluminum foil substrate 65. The aluminum foil had a thickness of about 15 micron. The wet cathode slurry was coated first on one side of foil substrate 65 and then dried as described herein. The wet cathode slurry was then coated onto the opposite side of substrate 65 and then dried. The dried cathode coatings 60 were then calendered to compress the coating thickness, thus forming a dry coating 60 on both sides of substrate 65 resulting in cathode composite 62. The cathode composite 62 had a total thickness of about 0.13 mm, which includes the thickness of substrate 65 (15 micron) and dry cathode coating 60 on both sides of substrate 65. The dry cathode loading was 24 milligram per square centimeter per side of substrate 65. The FeS2 loading in the dry cathode coating 60 was 21.3 milligram per square centimeter per side of substrate 65. FeS2 powder (Pyrox Red 325) 88.7 wt. %, acetylene black (Super P from Timcal Co.) 2.3 wt. %, graphite (Timrex KS6 from Timcal Co.) 6.0 wt. %, binder (Kraton G1651 from Kraton Polymers) 3.0 wt. %. The FeS2 powder in the cathode had a loading of about 0.0144 g/cm2 per side, which is equivalent to a theoretical capacity of about 12.86 mAmp-Hr/cm2 per side. The cells had a total anode/cathode interfacial area of about 150 cm2 per side of substrate 65 or 300 cm2 total. (At high rate drain at 1 Amp this corresponds to a current density of about 0.0033 Amp/cm2.)
The anode 40 was formed from a sheet of lithium metal in the control cells or lithium metal alloyed with 1500 ppm aluminum in the test cells. The anode 40 sheet had a thickness of about 0.165 mm. This corresponds to a lithium loading in the anode of about 8.9 milligram per square centimeter. (The anode 40 can be formed of alloy of lithium alloyed with up to about 5000 ppm aluminum, but the test cells (Groups C and D) for this example were formed of lithium alloyed with 1500 ppm aluminum.) The separator was formed of a sheet of microporous polyethylene having a thickness of about 0.016 mm. The electrolyte added to the B and C cells were identical and comprised a mixture of lithium iodide (LiI) (1.0 moles per liter) with LiCF3SO3 (LiTFS) (0.1 wt/%) dissolved in a solvent mixture of 1,3 dioxolane (DX) and 1,2-dimethoxyethane (DME) in a weight ratio of 70:30 with 0.2 wt % 3,5-dimethylisoxazole (DMI). The Group D cells electrolyte was about the same but had a slightly higher concentration of LiI salt. The Group D cells electrolyte comprised a mixture of lithium iodide (LiI) (1.2 moles per liter) with LiCF3SO3 (LiTFS) (0.1 wt/%) dissolved in a solvent mixture of 1,3 dioxolane (DX) and 1,2-dimethoxyethane (DME) in a weight ratio of 70:30 with 0.2 wt % 3,5-dimethylisoxazole (DMI). Additionally, the control Group B Cells and test cell Group C cells had a water content of 350 ppm (parts per million by weight) and the Group D cells had a water content of 425 ppm.
After the AA cells (Groups B,C, and D cells) were filled, they were predischarged slightly to a depth of discharge of about 3 percent of the cell's capacity and then stored at room temperature for about 3 days (fresh cells) and then subjected to the Digicam test below. These cells are referred to as fresh cells. The same tests were repeated with the same groups of cells except that these cells were stored for 20 days at a temperature of 60° C. and then subjected to the Digicam test described below. These cells are referred to as stored cells. The tests were all performed with eight cells in each group (B,C, and D) of fresh cells and eight cells in each group (B,C, and D) of stored cells. The test results reported in the following tables reflect a mean average of the results from each of the groups of fresh and stored cells.
The Test AA cells were discharged to a cutoff voltage of about 1.05 Volts using a digital camera discharge test (Digicam test).
The digital camera test (Digicam test) consists of the following pulse test protocol wherein each test cell was drained by applying pulsed discharge cycles to the cell: Each cycle consists of both a 1.5 Watt pulse for 2 seconds followed immediately by a 0.65 Watt pulse for 28 seconds. These cycles are repeated 10 times followed by 55 minutes rest. Then the cycles are repeated until the cutoff voltage is reached. The cycles are continued until a cutoff voltage of 1.05V is reached. The total number of the 1.5 Watt pulses required to reach these cutoff voltages were recorded. The results are reported in Table II (below). The Digicam test results (Table II) clearly show that that the cells with anode of lithium alloyed with aluminum (Li—Al anode), namely, the Group C and D cells had service life (number of 1.5 watt pulses to cut off voltage of 1.05V) greater than the control Group B cells with lithium metal anode. These greater service for the Group C and D cells compared to the control B Cells were apparent regardless of whether the tests were performed on fresh cells or stored cells.
The Impedance Tests (Cell's Internal Resistance, milliohm) as reported in Table III similarly showed that that the cells having anode of lithium alloyed with aluminum (Li—Al anode, namely, the Group C and D cells, showed a smaller internal resistance, milliohm, than the control B cell having an anode of lithium metal. The Table III also shows that the difference in the cell's internal resistance between fresh cells and stored cells is less for the test C and D cells as compared to the control B cells.
The test data for the Li/FeS2 wound cells comparing the effect of anode of lithium vs. anode of lithium alloyed with aluminum is presented in the following Tables II and III.
1Lithium alloyed with 1500 ppm aluminum.
2Cells stored for 3 days at room temperature before Digicam test was applied.
3Cells stored for 20 days at 60° C. before Digicam test was applied.
4Electrolyte was a mixture of LiI (1.0 Molar) and LiCF3SO3 (LiTFS) (0.1 wt %) dissolved in a solvent mixture of 1,3 dioxolane (DX) and 1,2- dimethoxyethane (DME) in weight ratio of 70/30 with 0.2 wt % 3,5-dimethylisoxazole (DMI) and 350 ppm water added.
5Electrolyte was a mixture of LiI (1.2 Molar) and LiCF3SO3 (LiTFS) (0.1 wt %) dissolved in a solvent mixture of 1,3 dioxolane (DX) and 1,2- dimethoxyethane (DME) in weight ratio of 70/30 with 0.2 wt % 3,5-dimethylisoxazole (DMI) and 425 ppm water added.
1Lithium alloyed with 1500 ppm aluminum.
2Cells stored for 3 days at room temperature before internal impedance was measured.
3Cells stored for 20 days at 60° C. before internal impedance was measured.
4Electrolyte was a mixture of LiI (1.0 Molar) and LiCF3SO3 (LiTFS) (0.1 wt %) dissolved in a solvent mixture of 1,3 dioxolane (DX) and 1,2-dimethoxyethane (DME) in weight ratio of 70/30 with 0.2 wt % 3,5-dimethylisoxazole (DMI) and 350 ppm water added.
5Electrolyte was a mixture of LiI (1.2 Molar) and LiCF3SO3 (LiTFS) (0.1 wt %) dissolved in a solvent mixture of 1,3 dioxolane (DX) and 1,2-dimethoxyethane (DME) in weight ratio of 70/30 with 0.2 wt % 3,5-dimethylisoxazole (DMI) and 425 ppm water added.
The basic conclusions drawn from the data shown in Tables II and III are:
1. The service life of the Li/FeS2 cells as measured by the pulsed Digicam test is greater (higher number of pulses to 1.05V cut off) for the Li/FeS2 cells with anodes of lithium alloyed with aluminum compared to the control Li/FeS2 cells with anode of lithium metal.
2. The cell's internal resistance are lower for the Li/FeS2 cells with anodes of lithium alloyed with aluminum compared to the control Li/FeS2 cells with anode of lithium metal.
3. The differences in internal resistance between the stored cells and the fresh cells are smaller for the Li/FeS2 cells with anodes of lithium alloyed with aluminum compared to the Li/FeS2 control cells with anode of lithium metal.
4. These performance advantages are reported herein for the Li/FeS2 cells having lithium alloyed with aluminum despite that the electrolyte used in the test and control cells have a water content of at least 350 ppm by weight.
5. Based on obtained experimental data it is expected that the application of a lithium-aluminum (Li—Al) alloy as an anode for Li/FeS2 primary button cell or wound cell will enhance performance of an electrolyte containing the lithium salt bistrifluoromethylsulfonyl imide, Li(CF3SO2)2N, e.g. at concentration of about 0.8 moles per liter in a solvent mixture comprising 1,3-dioxolane (DX) (80 vol %), sulfolane (20 vol. %), pyridine (750-950 ppm), and water between about 100 and 2,000 ppm. It is expected that the water content in the electrolyte, for example, may be between about 200 and 1000 ppm, or between about 300 and 1000 ppm, or between about 300 and 600 ppm. The 1,3-dioxolane (DX) may typically be between about 70 and 90 vol % and the sulfolane between about 10 and 30 vol. %. The bistrifluoromethylsulfonyl imide, Li(CF3SO2)2N salt may, for example, be at a concentration of between about 0.3 and 1.4 moles per liter in the solvent mixture. The aluminum content in the Li—Al alloy anode may, for example, be between about 0.1 and 2 percent by weight or even up to about 5 percent by weight.
The studies herein reported show an advantage in employing a lithium-aluminum alloy instead of pure lithium metal for the anode of a Li/FeS2 cell. This data has reinforced a theoretical basis for postulating that the lithium in the anode of Li/FeS2 cells may be alloyed with other metals as herein described, to help obtain enhanced cell performance.
Although the invention has been described with reference to specific embodiments, it should be appreciated that other embodiments are possible without departing from the concept of the invention and are thus within the claims and equivalents thereof.
