NONAQUEOUS CELL WITH A NOVEL ORGANIC ELECTROLYTE

Abstract: A nonaqueous cell employing an anode such as lithium, a cathode such as MnO₂ and a liquid organic electrolyte comprising a solute of lithium perchlorate and lithium tri­ fluoromethane sulfonate dissolved in a solvent mixture of propylene carbonate and dimethoxyethane.

Description: NONAQUEOUS CELL WITH A NOVEL ORGANIC ELECTROLYTE Technical Field The invention relates to an organic electrolyte for use in nonaqueous cells such as Li/MnO2, Li/polycarbon fluoride systems and the like. Background of the Art The development of high energy battery systems requires the compatibility of an electrolyte possessing desirable electrochemical properties with highly reactive anode materials. such as lithium. sodium, and the like and the efficient use of high energy density cathode materials. such as manganese dioxide. polycarbon fluorides such as (C2F) , (CF ) in which x is greater than 0 up to about xn 1.2, and the like. The use of aqueous electrolytes is precluded in these systems since the anode materials are sufficiently active to react with water chemically. It has therefore been necessary. in order to realize the high energy density obtainable through use of these highly reactive anodes and high energy density cathodes. to turn to the investigation of nonaqueous electrolyte systems and more particularly to nonaqueous organic electrolyte systems. A multitude of solutes is known and recommended for use but the selection of a suitable solvent has been particularly troublesome since many of those solvents which are used to prepare electrolytes sufficiently conductive to permit effective ion migration through the solution are reactive with the highly active anodes mentioned above. Most investigators in this area, in search of suitable solvents, have concentrated on aliphatic and aromatic nitrogen- and oxygen-containing compounds with some attention given to organic sulfur-. phosphorus- and arsenic-containing compounds. The results of this search have not been entirely satisfactory since many of the solvents investigated still could not be used effectively with high energy density cathode materials, such as manganese dioxide (MnO2). poly-carbon fluoride and the like, and were sufficiently corrosive to lithium anodes to prevent efficient performance over any length of time. Although manganese dioxide has been mentioned as a possible cathode for cell applications. manganese dioxide inherently contains an unacceptable amount of water, both of the adsorbed and bound types. which is sufficient to cause anode (lithium) corrosion along with its associated hydrogen evolution. This type of corrosion that causes gas evolution is a serious problem in sealed cells, particularly in miniature type button cells. In order to maintain overall battery-powered electronic devices as compact as possible. the electronic devices are usually designed with cavities to accommodate the miniature cells as their power source. The cavities are usually made so that a cell can be snugly positioned therein thus making electronic contact with appropriate terminals within the device. A major potential problem in the use of cell-powered devices of this nature is that if the gas evolution causes the cell to bulge then the cell could become wedged within the cavity. This could result in damage to the device. Also. if electrolyte leaks from the cell it could cause damage to the device. Thus it is important that the physical dimensions of the cell's housing remain constant during discharge and that the cell will not leak any electrolyte into the device during storage or discharge. US-A-4.133,856 discloses a process for producing an MnO2 electrode (cathode) for nonaqueous cells whereby the MnO2 is initially heated within a range of 3500C to 4300C so as to substantially remove both the adsorbed and bound water and then, after being formed into an electrode with a conductive agent and binder, it is further heated in a range of 2000C to 3500C prior to its assembly into a cell. GB-A-1,199,426 also discloses the heat treatment of MnO2 in air at 2500C to 4500C to substantially remove its water component. In U.S. Serial No. 384,222 filed in the name of Violeta Zilionis Leger on June 2. 1982 a nonaqueous cell is discloseS which comprises a highly active metal anode such as lithium, a manganese dioxide-containing cathode wherein the manganese dioxide has a water content of less than 1 weight percent based on the weight of the manganese dioxide, and a liquid organic electrolyte comprising lithium trifluoromethane sulfonate dissolved in propylene carbonate and dimethoxyethane. JP'A-54/110429 discloses a nonaqueous cell employing an electrolyte to improve the low temperature performance of the cell, said electrolyte employing an organic solvent, such as a mixture of propylene carbonate and dimethoxyethane. in which is dissolved two inorganic salts, one of which contains an anion different from that of the main solute. Examples in this application use LiClO as the main solute 4 along with LiBF4, LiAlC14, LiPF6. LiAsF or 6 KPF6 as the added inorganic salt in a mixture of propylene carbonate and dimethoxyethane as the solvent. Although specific solutes and solvents have been mentioned as good electrolyte solutions for certain cell systems. it is not always possible to predict whether combinations of these components would effectively and efficiently function in other cell systems. Thus while. the theoretical energy. i.e.. the electrical energy potentially available from a selected anode-cathode couple, is relatively easy to calculate, there is a need to choose a nonaqueous electrolyte for a couple that permits the actual energy produced by an assembled battery to approach the theoretical energy. The problem usually encountered is that it is practically impossible to predict in advance how well, if at all, a conductive nonaqueous electrolyte will function with a selected couple with regard to stability and corrosion behavior. Thus a cell must be considered as a unit having three parts: a cathode, an anode. and an electrolyte. and it is to be understood that the parts of one cell are not predictably interchangeable with parts of another cell to produce an efficient and workable cell. It is an object of the present invention to provide a nonaqueous cell employing an electrolyte solution of lithium perchlorate and lithium trifluoromethane sulfonate dissolved in a mixture of propylene carbonate and dimethoxyethane which provides excellent low temperature performance characteristics and excellent shelf life characteristics, It is another object of the present invention to provide a nonaqueous cell employing an electrolyte solution of lithium perchlorate and lithium trifluoromethane sulfonate dissolved in a mixture of propylene carbonate and dimethoxyethane, said electrolyte solution being stable in the cell and inhibiting corrosion of the cell components. It is another object of the present invention to provide a Li/MnO2 nonaqueous cell employing a liquid organic electrolyte comprising lithium perchlorate and lithium trifluoromethane sulfonate dissolved in a mixture of propylene carbonate and dimethoxyethane. It is another object of the present invention to provide a Li/polycarbon fluoride nonaqueous cell employing a liquid organic electrolyte comprising lithium perchlorate and lithium trifluoromethane sulfonate dissolved in a mixture of propylene carbonate and dimethoxyethane. The foregoing and additional objects will become more fully apparent from the following description. Summary of the Invention The invention is directed to a nonaqueous cell comprising an active metal anode. a cathode and a nonaqueous electrolyte solution comprising a solute of lithium perchlorate and lithium trifluoromethane sulfonate dissolved in a solvent mixture of propylene carbonate and dimethoxyethane. It has been found that an electrolyte solution of lithium perchlorate (LC10 ) dissolved 4 in a mixture of propylene carbonate (PC) and dimethoxyethane (DME) can be used in a nonaqueous cell to provide excellent shelf life and high rate capability for the cell. However, in some cell applications, the performance of a cell employing this electrolyte in a low temperature environment. i.e., about -100C and lower. can be rather poor. It was found that if lithium trifluoromethane sulfonate (LiCF3 SC3) is added to the electrolyte solution, the low temperature performance of the cell can be greatly improved, i.e., the cell will operate at a higher voltage, particularly on pulse discharge. in the low temperature environment while maintaining excellent shelf life. In general it has been found that the electrolyte, particularly the LiClO4 component, will passivate metal surfaces of the cell thereby protecting the surfaces from attack by corrosion-initiating species. The molar concentration of lithium trifluoromethane sulfonate can vary between about 0.25 to about 1.5 and the molar concentration of lithium perchlorate can vary between about 0.1 and about 1.0. Preferably, the molar concentration of the lithium trifluoromethane sulfonate should be between about 0.35 and about 0.7 and the molar concentration of lithium perchlorate should be between about 0.25 and about 0.5. In applications where the cell would be operating at low temperatures then a larger amount of lithium trifluoromethane sulfonate would be used. In applications where the cell would be stored at 200C for a long period of time or where high rate capability is desired, then a larger amount of lithium perchlorate would be used. Thus by using an appropriate mixture of these two salts dissolved in a solvent mixture of PC and DME. an electrolyte solution can be obtained that will have the desirable characteristics of each salt component. i.e., good low temperature performance due to the presence of LiCF3SO3 and improved shelf life and high rate capability due to the presence of LiClO4. The ratio of propylene carbonate to dimethoxyethane based on the solvent volume can vary from about 80:20 to 20:80 and is preferably about 50:50. The lithium perchlorate and lithium trifluoromethane sulfonate mixture can vary from about 0.5 molar up to their saturation in the electrolyte solution at the lowest expected operating temperature and preferably is about 1 molar in concentration. Generally, the conductivity should be at least 10-3 ohm-1 cm-1 Cathodes suitable for use with the electrolyte solution of the this invention would include manganese dioxide, poly-carbon fluoride, iron sulfide, Coo , Bi 203,Ag2CrO4, Pb304, CuS, CuO and TiS2. The water inherently contained in both electrolytic and chemical types of manganese dioxide can be substantially removed by various treatments. For example, the manganese dioxide can be heated in air or an inert atmosphere at a temperature up to 3800C for about 8 hours or at a lower temperature for a longer period of time. Care should be taken to avoid heating the manganese dioxide above its decomposition temperature which is about 4000C in air. In oxygen atmospheres. higher temperatures may be employed. In accordance with this invention the manganese dioxide should be heated for a sufficient period of time to insure that the water content is reduced preferably below about 1 weight percent. more preferably below about 0.5 and most preferably below about 0.2 weight percent based on the weight of the manganese dioxide. An excessive amount of water would react with the highly active metal anode, such as lithium, and cause it to corrode thereby resulting in hydrogen evolution. After the water removal treatment has been completed, the manganese dioxide should be shielded to prevent adsorption of water from the atmosphere. This could be accomplished by handling the treated manganese dioxide in a dry box or the like. Alternatively, the treated manganese dioxide or the manganese dioxide combined with a conductive agent and a suitable binder could be heat treated to remove water that could have been adsorbed from the atmosphere. Preferably, the manganese dioxide to be used with the electrolyte of this invention would be heat treated to remove its water content preferably below about 1 weight percent and then it would be mixed with a conductive agent such as graphite. carbon or the like and a binder such as Teflon (trademark for polytetrafluoroethylene), ethylene acrylic acid polymer or the like to produce a solid cathode electrode. If desired, a small amount of the electrolyte can be incorporated into the manganese dioxide cathode mix. The poly-carbon fluoride cathodes for use with the electrolyte of this invention can be composed of carbon and fluorine in which the carbon includes graphitic and non-graphitic forms of carbon, such as coke. charcoal or activated carbon and have the formula (C F )n wherein y is 1 or yxn 2, x is greater than 0 up to about 1.2 and n refers to the number of monomer units which can vary widely. Preferably, the poly-carbon fluoride would be those having a y of 1 and an x between about 0.8 and 1.0. and poly-dicarbon monofluoride (C2F)n. Fluorinated carbon cathodes are disclosed in US-A-3,636,532, US-A-3,2a0,502 and US-A 4,271,242 as having the formula (CF ) wherein x xn varies from 0.5 to about 1.0. US-A 4.139,474 discloses (C2F)n material suitable for use as cathodes. The disclosure of these U.S. P-a tents are incorporated by reference as if set out in full text. A benefit of the novel electrolyte solution of this invention, when employed with a Li/polycarbon fluoride system, is that the metal components of the cell are protected from corrosion by any unbonded fluoride associated with the polycarbon fluoride material. Highly active anodes for use in nonaqueous systems employing the novel electrolyte according to this invention would be consumable metals and include aluminum, the alkali metals, alkaline earth metals and alloys of alkali metals or alkaline earth metals with each other and other metals. The term "alloys" as used herein and in the appended claims is intended to include mixtures. solid solutions, such as lithium-magnesium. and the intermetallic compounds, such as lithium monoaluminide. The preferred anode materials are lithium. sodium, potassium. calcium, magnesium and alloys thereof. Of the preferred anode materials, lithium would be the best because. in addition to being a ductile metal that can be easily assembled in a cell, it possesses the highest energy-to-weight ratio of the group of suitable anodes. ExamPle 1 Several cylindrical cells (33 mm high and 16,4 mm in diameter) were constructed employing a cathode of 6.2 grams mix containing 88% by weight heat-treated Mono2, 9% by weight graphite, and 3% by weight polytetrafluoroethylene: a lithium anode (0.45 gram); two layers of separator material (nonwoven polypropylene and microporous polypropylene) and about 2.6 grams of an electrolyte solution of LiClO4 and/or LiCF3SO3 in the approximate molar concentrations shown in Table 1 in a 50:50 volume ratio of PC to DME. Some cells were discharged at 200C across a 60-ohm load to a 1.8 volt cutoff. Other cells were stored for various time periods at 600C and then discharged at 200C across a 60-ohm load to a 1.8 volt cutoff. The data obtained are shown in Table 1. TABLE 1 Discharge time to 1.8 volts (hours) LiClO4 to LiCF3SO3 Sample Approximate Storage time at 60 C (days) Cell Molar Conc. Fresh 20 40 60 80 A 0.5: 0.5 30.0 27.7 28.2 29.1 27.3 B 0.3: 0.7 29.7 25.8 26.9 27.9 23.3 C 0: 1 28.8 27.5 16.8 11.5 9.7 Some cells were either stored at 200C for various time periods or stored at 600C for various time periods and then the open circuit voltage (CCV), closed circuit voltage (CCV) and impedance (Imp) were measured for each cell. The closed circuit voltage was taken across a 25-ohm load for 2 seconds. The impedance was measured at 1000 Hz. The data observed are shown in Table 2. As evident from the data, the cells employing a mixture of LiC104 and LiCF3 SO3 in the electrolyte solution exhibited better shelf characteristics after being stored at 600C for 40 days or more than the cells that contained only LCF SO in the electrolyte solution. Several of each type of cells were examined after disassembly and the cells containing the combination of LiC104 and LiCF3SO3 (cell samples A and B) showed no evidence of corrosion of cell components while control cells (sample C) showed visual evidence of corrosion reaction products on the anode surface. This confirms visually the evidence of corrosion demonstrated by the decline in open circuit voltage (CCV) of the control cells. Table 2 Storage at 200C - (days) Storage at 600C - (days) Sample Cell Test 7 90 20 40 60 80 A OCV (volts) 3.53 3.39 3.39 3.36 3.33 3.33 A -CCV (volts) 2.96 3.04 2.94 2.74 2.64 2.11 A Imp (ohms) 2.2 1.7 3.7 3.5 4.0 5.3 B CCV (volts) 3.54 3.36 3.39 3.38 3.34 3.34 B CCV (volts) 2.89 3.04 2.88 2.55 2.58 2.21 B Imp (ohms) 2.1 1.6 4.8 4.8 4.4 5.8 C CCV (volts) 3.43 3.31 3.15 3.09 2.84 2.81 C CCV (volts 2.98 3.04 2.81 2.42 1.95 1.21 C Imp (ohms) 2.0 1.3 3.7 3.9 7.4 24.8 Example 2 Several cylindrical cells were constructed as in Example 1 using the same components and amounts, varying only the LiC104 and LiCF SO3 4 3 molar concentrations in a 50:50 volume ratio of PC to DME. Some cells were discharged at various temperatures across a 60-ohm load to a 1.8 volt cutoff. Other cells were stored for various time periods at 600C and discharged across a 60-ohm load to a 1.8 volt cutoff. The data obtained are shown in Table 3. As evident from the data, the cells employing a mixture of LiC104 and LiCF3SO3 in the electrolyte solution performed better at low temperatures than the cells that contained only 1iC104 in the electrolyte solution. TABLE 3 Discharge time to 1.8 volts (hours) LiClO4 to LiCF3SO3 Fresh Cells Discharge Temp. *Stored at Sample Approximate 60 C (days) Cell Molar Conc. 20 C 0 C -10 C -20 C 20 40 D 0.5: 0.5 25.8 26.6 25.5 15.8 27.2 26.8 E 0.75: .25 27.9 **NT 22.0 0 **NT 27.5 F 1.0: 0 27.2 26.8 22.0 0 28.3 27.1 *Discharged at 20 C **NT = Not tested Some cells were stored for various time periods at various temperatures and then the open circuit voltage (CCV), closed circuit voltage (CCV) and impedance (Imp) were measured for each cell at ambient temperature. The closed circuit voltage was taken across a 25-ohm load for 2 seconds. The impedance was measured at 1000 Hz. The data observed are shown in Table 4. As evident from the data, cells employing a mixture of LiClO4 and LiCF3SO3 in the electrolyte solution in which the molar concentration of LiClO4 was 0.5 up to 1.0 exhibited good shelf characteristics at 600C. Table 4 Stored at Stored at Stored at Sample 20 C for 20 C for 20 C for Cell Test Fresh 26 weeks 20 days 40 days D OCV (volts) 3.47 3.40 3.40 3.38 D CCV (volts) 3.16 2.86 2.81 2.81 D Imp (ohms) 1.8 1.5 2.0 4.2 E OCV (volts) 3.47 3.40 3.40 3.38 E CCV (volts) 3.12 2.67 2.95 2.88 E Imp (ohms) 1.5 1.2 NT 3.4 F OCV (volts) 3.47 3.37 3.40 3.37 F CCV (volts) 3.24 2.62 2.85 2.70 F Imp (ohms) 1.5 1.8 2.7 3.6 Example 3 Several cylindrical cells were constructed as in Example 1 using the same components and amounts, varying only the LiC104 and LiCF3SO3 molar concentrations in a 50:50 volume ratio of PC to DME. Some cells were discharged at 200C across a 60-ohm load to a 1.8 volt cutoff. Other cells were stored for various time periods at 600C and then discharged across a 60-ohm load to a 1.8 volt cutoff. The data obtained are shown in Table 5. Table 5 Discharge time to 1.8 volts (hours) LiClO4 to Storage time LiCF3SO3 at 60 C (days) Sample Approximate Cell Molar Conc. Fresh* 20 40 60 **0 C **-20 C G 1.0:0 27.7 26.4 24.5 26.0 27.8 0 H 0.5:0.5 28.8 27.5 NT NT 27.5 15.5 I 0:1.0 25.0 27.6 25.3 22.2 NT NT *Discharge temperature = 20 C **Temperature at which cells were discharged NT=Not Tested Some additional cells were either stored at 200C for various time periods or stored at 600C for various time periods and then the open circuit voltage (CCV) and closed circuit voltage (CCV) were measured for each cell at ambient temperature. The closed circuit voltage was taken across a 25-ohm load for 2 seconds. The data observed are shown in Table 6. As evident from the data. the cells employing a mixture of LiClO and LiCF SO3 in 4 3 the electrolyte solution performed better after being stored at 600C for 40 days or more than the cells that contained only LiCF3SO3 in the electrolyte solution. Table 6 Stored at 60 C - days Sample Cell Test Fresh 20 40 60 180 360 G OCV (volts) 3.47 3.38 3.34 3.29 3.38 3.35 G CCV (volts) 3.23 2.85 2.72 2.64 2.79 3.09 H OCV (volts) 3.46 3.38 NT NT 3.42 3.39 H CCV (volts) 3.27 2.85 NT NT 2.73 3.02 I OCV (volts) 3.44 3.30 3.13 3.05 3.20 NT I CCV (volts) 3.16 2.46 2.56 2.28 2.41 NT NT = Not Tested *Stored at ambiant room temperature Example 4 Several cylindrical cells ( 22,99 mm high and 13,5 mm in diameter) were constructed employing a cathode of 1.02 grams mix containing 80% by weight (CFx)n where x was about 1.0, 10% by weight acetylene black and 10% by weight polytetrafluoroethylene; a lithium anode (0.24 gram): two layers of separator material (microporous polypropylene and nonwoven polypropylene); and about 1.10 grams of an electrolyte solution of LiC104 and/or LCF SO in the molar concentrations shown in Table 7 in a 50:50 volume ratio of PC to DME. The open circuit voltage (CCV). closed circuit voltage (CCV) and impedance (Imp) of each cell were measured when fresh and after storage at 600C for 20 and 40 days. The closed circuit voltage was taken across a 50-ohm load for 2 seconds. The impedance was measured at 1000 Hz. The data observed are shown in Table 7. Several of each type of cells were examined after disassembly and the cells containing the combination of LiClO4 and LiCF3SO3 (cell sample K) showed substantially less evidence of corrosion reaction products on the anode surface than the control cell (cell sample J). This confirms visually the evidence of corrosion demonstrated by the greater decline in open circuit voltage (CCV) of the control cells. Table 7 60 C Storage Sample Approximate Cell Molar Conc. Fresh 20 days 40 days OCV CCV Imp OCV CCV Imp OCV CCV Imp (volts) (volts) (ohms) (volts) (volts) (ohms) (volts) (volts) (ohms) J 1M LiCF3SO3 3.32 2.67 3.5 3.00 2.32 6.9 2.95 2.3 8.0 K 0.5 M LiClO4 3.39 2.76 3.5 3.29 2.17 9.4 3.11 2.06 10.9 0.5 M LiCF3SO3 As evident from the data. the use of mixtures of LiC104 and LiCF3 SO3 as the solute for the electrolyte solution of the cell provided the cells with both good low temperature performance characteristics and good shelf life characteristics.

Claims: CLAIMS: 1. A nonaqueous cell comprising an active metal anode, a cathode and a nonaqueous electrolyte solution, characterized in that the nonaqueous electrolyte solution comprises a solute of lithium perchlorate and lithium trifluoromethane sulfonate dissolved in a solvent mixture of propylene carbonate and dimethoxyethane. 2. The nonaqueous cell of claim 1 wherein the molar concentration of lithium perchlorate is between about 0.1 and about 1.0 and the molar concentration of lithium trifluoromethane sulfonate is between about 0.25 and about 1.5. 3. The nonaqueous cell of claim 2 wherein the molar concentration of lithium perchlorate is between about 0.25 and about 0.5 and the molar concentration of lithium trifluoromethane sulfonate is between about 0.35 and about 0.7. 4. The nonaqueous cell of 3 wherein the molar concentration of lithium perchlorate is about 0.5 and the molar concentration of lithium trifluoromethane sulfonate is about 0.5. 5. The nonaqueous cell of claim 2 wherein the volume ratio of propylene carbonate to dimethoxyethane is between about 80:20 and 20:80. 6. The nonaqueous cell of claim 1 wherein the volume ratio of propylene carbonate to dimethoxyethane is about 50:50. 7. The nonaqueous cell of claim 1 wherein the total concentration of the lithium perchlorate and the lithium trifluoromethane sulfonate in the electrolyte solution varies from about 0.5 molar up to their saturation in the electrolyte solution. 6. The nonaqueous cell of claim 1 wherein the total concentration of the lithium perchlorate and lithium trifluoromethane sulfonate in the electrolyte solution is about 1 molar.

Inventors: MARPLE, JACK WILLIAM, O'HARA, III, THOMAS JAMES
Applicants: EVEREADY BATTERY COMPANY, INC.
Application year: 1984
Main classification: H01M6
IPC codes: H01M6