IE801312L

IE801312L - Non-aqueous cell

Info

Publication number: IE801312L
Application number: IE801312A
Authority: IE
Original assignee: Union Carbide Corp
Priority date: 1979-06-25
Filing date: 1980-06-24
Publication date: 1980-12-25
Also published as: IE49844B1; CA1149447A; ES492687A0; MX153063A; DK270280A; BE883985A; ES8102423A1; IT1132123B; NO801877L; CH642779A5; HK33585A; JPS566383A; LU82543A1; SE8004657L; AU5956580A; NL8003660A; GB2054253B; GB2054253A; AU530502B2; DE3022977A1

Abstract

A nonaqueous cell comprising an active metal anode such as lithium, a manganese dioxide-containing cathode which contains less than 1 weight percent water in the manganese dioxide and a liquid organic electrolyte comprising 3-methyl- 2-oxazolidone in conjunction with a selected solute and optionally a cosolvent having a viscosity lower than that of the 3-methyl-2- oxazolidone. [GB2054253A]

Description

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 5 cathode materials, such as manganese dioxide. 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 10 cathodes, to turn to the Investigation of nonaqueous electrolyte systems and more particularly to nonaqueous organic electrolyte systems.

The term "nonaqueous organic electrolyte" in the prior art refers to an electrolyte which is composed of a solute, for example, a salt or complex salt of Group I-A, Group II-A or Group III-A elements of 15 the Periodic Table, dissolved in an appropriate nonaqueous organic solvent. Conventional solvents include propylene carbonate, ethylene carbonate or y-butyrolactone. The term "Periodic Table" as used herein refers to the Periodic Table of the Elements as set forth on the inside back cover of the Handbook of Chemistry and Physics, 48th Edition, the Chemical Rubber Co., Cleveland, Ohio, 1967-1968.

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 2 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 (MnOg), 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 absorbed and bound (adsorbed) 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 with not leak any electrolyte into the device being powered.

U.S. Patent No. 4 133 856 discloses a process for producing a Mn02 electrode (cathode) for nonaqueous cells whereby the MnOg is initially heated within a range of 350° to 430°C so as to substantially remove both the absorbed and bound water and then, after being formed into an electrode with a conductive agent and bonder, it is further heated in a range of 200° to 350°C prior to its assembly into a cell. British Patent No. 1 199 426 also discloses the heat treatment of MnOg in air at 250° to 450°C to substantially remove Its water component.

U.S. Patents Nos. 3 871 916; 3 951 685 and 3 999 069 disclose a nonaqueous cell employing a 3-methyl-2-oxazolidone-based electrolyte in cor\junction with a solid cathode selected from (CF ) » CuO, FeS2> Co304, V205, PbjO^, In2S3 and CoSg.

While the theoretical energy, i.e., the electical 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 it that it is practically impossible to predict in advance how well, if at all, a nonaqueous electrolyte will function with a selected couple. 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 manganese dioxide nonaqueous cell employing an active metal anode.

The invention provides a novel high energy density nonaqueous cell comprising a highly active metal anode, a manganese dioxide-containing cathode and a liquid organic electrolyte comprising 3-methyl-2-oxazolidone together with a conductive solute with or without at least one cosolvent having a viscosity lower than that of 3-methyl-2-oxazolidone and wherein the manganese dioxide has a water content of less than 1 weight percent based on the weight of the manganese dioxide. Preferably the water content should be lower than 0.5 weight percent and most preferably below 0.2 weight percent.

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 of 350°C 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 400°C in air. In oxygen atmosphere, higher temperatures may be employed. To make it suitable for use in the cell of this invention the manganese dioxide should be heated for a sufficient period of time to ensure that the water content is reduced below 1 weight percent, preferably below about 0.5 and most preferably below about 0.2 weight percent based on the weight of the manganese dioxide. An amount of water above about 1 weight percent would react with the highly active metal anode, such as lithium, and cause it to corrode thereby resulting in hydrogen evolution. As stated above this could result in physical distortion of the cell and/or electrolyte leakage from the cell during storage or discharge.

To effectively remove the undesirable water from Mn02, or Mn02 mixed with a conductive agent and a suitable binder, to the level necessary to practice this invention, it is believed necessary that both the absorbed and bound water be substantially removed. After the water removal treatment 5 has been completed, it is essential that the manganese dioxide be shielded to prevent absorption 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 10 heat treated to remove water that could have been absorbed from the atmosphere.

Preferably, the manganese dioxide should be heat treated to remove its water content to below 1 weight percent and then it can be mixed with a conductive agent such as a graphite, or carbon and a binder such as 15 Teflon (trade mark for polytetrafluoroethylene) or ethylene acrylic acid polymer to produce a solid cathode electrode. If desired, a small amount of electrolyte can be incorporated into the manganese dioxide mix.

An added possible benefit in the removal of substantially all the water from manganese dioxide is that if small amounts of water are present 20 in the cell's electrolyte then the manganese dioxide will absorb the main portion of that water from the electrolyte and thereby prevent or substantially delay the reaction of the water with the anode such as lithium. In this situation, the manganese dioxide will act as an extracting agent for the water impurities in the organic solvents. 25 The electrolyte for use in this invention is a 3-methyl-2- oxazolidone-based electrolyte. Liquid organic 3-methyl-2-oxazolidone material, (3Me20X) 6 49B41 1 1 CH2-CH2-0-C0-N-CH3, is an excellent nonaqueous solvent because of its high dielectric constant, chemical inertness to battery components, wide liquid range and low toxicity.

However, it has been found that when metal salts are dissolved in liquid 3Me20x for the purpose of improving the conductivity of 3Me20x, the viscosity of the solution may be too high for its efficient use as an electrolyte for some nonaqueous cell applications other than those requiring very low current drains. Thus, in some applications in accordance with this invention, the addition of a low viscosity cosolvent would be desirable if 3Me20x is to be used as an electrolyte for nonaqueous cells which can operate or perform at a high energy density level. Specifically, in order to obtain a high energy density level in accordance with this invention, it is essential to use a heat-treated Mn02 cathode along with a highly active metal anode. Thus this invention is directed to a novel high energy density cell having a highly active metal anode, such as lithium, a heat-treated Mn02 cathode, and an electrolyte comprising 3Me20x in combination with a conductive solute with or without at least one low viscosity cosolvent.

The low viscosity cosolvents if used in this invention include tetrahydrofuran (THF), dioxolane (DIOX), dimethoxyethane (DME), propylene carbonate (PC), dimethyl isoxazole (DM1), diethyl carbonate (DEC), ethylene glycol sulfite (EGS), dioxane and dimethyl sulfite (DMS). Dimethoxyethane (DME), dioxolane (DIOX) and propylene carbonate (PC) are preferred cosolvents because of their compatibility with metal salts dissolved in liquid 3Me20x and their chemical inertness to cell components. Specifically, the total amount of the low viscosity cosolvent added could be between about 202 and about 80% based on total solvent volume, i.e. exclusive of solute, so as to lower 5 the viscosity to a level suitable for use in a high drain cell.

Conductive solutes (metal salts) for use in this invention with the liquid 3Mfc20x may be selected from MCF^SOj, MBF^, MCIO^, and MM'Fg wherein M is lithium, sodium or potassium, and M' is phosphorus, arsenic or antimony. The addition of the solute is necessary to improve 10 conductivity of 3Me20x so that said 3Me20x can be used as the electrolyte in nonaqueous cell applications. Thus the particular salt selected has to be compatible and nonreactive with 2Me20x and the electrodes of the cell. The amount of solute to be dissolved in the liquid 3Me20x should be sufficient to provide good conductivity, 15 e.g. at least 10"* ohnf^cm"^. Generally an amount of at least 0.5 molar would be sufficient for most cell applications.

Highly active metal anodes suitable for this invention include • lithium (Li), potassium (K), sodium (Na), calcium (Ca), magnesium (Mg), aluminium (Al), and their alloys. Of these active metals, 20 lithium would be preferred because in addition to being a ductile, soft metal that can easily be assembled in a cell, it possesses the highest energy-to-weight ratio of the group of suitable anode metals.

The present invention of a high energy density cell with a 3-Me20x-based electrolyte, a solid ffo^-containing cathode having 25 less than 1 weight percent water and a highly active metal anode will be further illustrated in the following examples. 8 «»S44 EXAMPLE 1 Thermogravimetric analyses (TGA) were made of various samples of connercial manganese dioxide. Some of the samples were analyzed as obtained, other samples were heat treated at 350°C for 8 hours, 5 and other samples were heated treated at 350°C for 8 hours and then blended with carbon and Teflon to produce cathode mixes. The data obtained from the thermogravimetric analyses (TGA) are shown in Table 1. The data clearly show that commercial types of manganese dioxide contain large amounts of water. In addition, the data 10 show that even after the manganese dioxide had been heat treated as specified above, it will absorb water from the atmosphere even after only a small period of time. 9 TABLE 1 Percent Weight Loss at Various Temperatures as Indicated by TGA Total % Weight Loss at Temp. "C (Cumulative) Sample Description 100 200 250 300 350 400 'Tekkosha MnOJ( as received 1.0 2.1 2.7 3.5 4.4 .1 Tekkosha as above, but dried at 350*C., 8 hrs; exposed to room atmosphere 5 mins. in sample transfer 0.2 0.3 0.3 0.3 0.4 0.6 '"Cathode mix taken directly from dry box; exposed to room atmosphere 5 mins. in sample transfer 0.3 0.4 0.5 0.7 1.1 Cathode mix exposed to room atmosphere 0.3 0.5 0.5 — — — Cathode mix same as above but exposed to room atmosphere an additional 17 hrs.**" 0.6 0.8 0.8 0.9 1.1 1.9 "'Sedema Mn02 1.4 2.1 2.4 2.6 2.9 3.7 'Tekkosha Mn02 is commercial electrolytic Mn02.

"Cathode mix—heat treated Tekkosha Mn02 + carbon black + graphite + Teflon *"Sedema Mn02 is commercial chemical Mn02 ""Room humidity, 35-50% EXAMPLE II Each of two falt-type cells was constructed utilizing a nickel metal base having therein a shallow depression into which the cell contents were placed and over which a nickel metal cap was placed to close the cell. The contents of each sample cell consisted of 1.0 inch (2.54 cm) diameter lithium discs consisting of five sheets of lithium foil having a total thickness of 0.10 inch (0.254 cm), about 4 ml of an electrolyte consisting of about 40 vol. % dioxolane, about 30 vol.% dimethoxyethane (DME), about 30 vol.% 3Me20x plus about 0.1% dimethelisoxazole (DM1) and containing 1M LiCF-jSO^, a 1.0 inch (2.54 cm) diameter porous nonwoven polypropylene separator having a thickness of 0.01 inch (0.0254 cm) which absorbed some of the electrolyte and two grams of cathode mix compressed to form a cathode having an apparent interfacial area of 5 square centimeters. In the first cell the cathode mix consisted of Tekkosha electrolytic Mn02 heat treated at 350°C for 20 hours, carbon black, and Teflon. The second cell employed the same type of components as in the first cell except that the Tekkosha Mn02 was untreated. Each cell was discharged across a 1200-ohm load to a 1-volt cutoff and the cathode efficiences assuming a 1-electron reaction were calculated along with the overall energy densities. The data obtained are shown in Table II.

TABLE II Cathode Energy Cathode Efficiency* Density 1-electron (Wh/in^) Heat Treated Mn02 Unheated Mn02 81. OX 72.8 ,993.1 48.2% .2 7,732.9 *Coulombic 11 48844 EXAMPLE III Ten miniature button cells were constructed using a lithium anode, an electrolyte consisting of about 40 vol.% dioxolane, about 30 vol.% DME, about 30 vol.%.3Me20x plus about 0.1% DM1 and containing 1 M LiCF3S03, 5 and a cathode containing 80 wt.% unheated or heat-treated MnOg, 1.5 wt.% carbon black, 13.5 wt.% graphite and 5.0 wt.% ethylene acrylic acid binder. The heat-treated MnOg was heated at a temperature of 350°C for 18 hours under an argon atmosphere. Each cell (0.452 inch (1.148 cm) diameter; 0.166 inch (0.422 cm) height) contained 0.3045 gram of the 10 untreated Mn02-containing cathode mix, or 0.3036 gram of the heat-treated Mn02~containing cathode^ mix, 0.037 gram of lithium, a polypropylene separator, and 140 yl of the electrolyte. Each cell was placed on a continuous 6200-ohm background load and was pulsed on a 250-ohm load for 2 seconds once a week. Upon reaching a cutoff voltage 15 of 1 volt, the cell capacity and cathode coulombic efficiency for each cell were calculated and are shown in Table III. 12 TABLE III Cell Sample Mn02 Cell Capability (mAh) Cathode Efficiency 1 Heat Treated 37.6 50.0 2 Heat Treated .2 40.3 3 Heat Treated 39.2 52.2 4 Heat Treated 46.0 61.4 Heat Treated 41.4 55.3 6 Not Heated 6.1 8.2 7 Not Heated 26.4 .5 8 Not Heated 34.2 45.7 9 Not Heated .9 14.5 Not Heated 4.9 6.6 EXAMPLE IV Two cells were constructed similar to cells in Example II except that 1.5 ml of the electrolyte was used and in the first cell the cathode mix (33% porosity) consisted of 80 wt.% Tekkosha Mn02> 10 wt.% carbon black and 10% Teflon, and in the second cell the cathode mix (45% porosity) was the same except that the Mn02 was electrolytic Mn02 made by Union Carbide Corporation. The Mn02 in each cell was heat treated and then blended into cathode pellets which were dried at 120°C in vacuum. The nominal interfacial electrode area for each electrode was 2 square centimeters. The cells were continuously discharged across a 3000-ohm load and the cathode coulombic efficiency of utilization to a 13 2.0 volt cutoff was calculated to be 88% for the Tekkosha Mn02 containing cell and 99% for the other cell.

EXAMPLE V Several 0.455 inch (1.156 cm) diameter, 0.165 inch (0.419 cm) high 5 cells were constructed using 0.36 gram of cathode mix containing 86 wt.% Tekkosha Mn02, 8.5 wt.% carbon black, 2.5 wt.% graphite, and 3.0 wt.% Teflon; 0.03 gram lithium anode; and 140 yl of the electrolyte used in Example III. The Mn02, prior to forming the cathode mix, was heat treated at 350°C for 8 hours. Thereafter the moulded cathode 10 mix pellets were exposed to various levels of humidity for various lengths of time and then assembled into cells. The bulge measurements, if any, and the leakage, if any, after storage for various periods of time as shown in Table IV. The bulge measurement is the deviation in mils or milliiieters of the height of the cell from the original 15 height of the cell due to anode corrosion and/or gas evolution within the cell. Leakage is any electrolyte visually observable at the seal area of the cell. The cells were then discharged across a 15,000 ohm load until the voltage dropped to 2.4 volts. The average milliampere hours capacity delivered by the cells in each sample group is also shown 20 in Table IV.

The data shown in Table IV demonstrate that the cells in which the heat-treated Mn02 cathodes have been exposed to substantial levels of humidity begin to show bulging within 24 hours. Some decrease in bulge with time may be due to some of the gas escaping through the 25 cover/gasket/container interface when leakage occurs. 14 TABLE IV (METRIC) Group Sample % Humidity Mn02 Cathode Exposure Time Average Bulge (millimiters) after storage Leakage* mAh 1 day 7 days 1 month 2 months 3 months 1 <1 2 hrs. ____ 0 -0.025 0 0/100 65 2 3 + 2 hrs. + 0.076 + 0.25 + 0.051 + 0.025 + 0.2 0/45 61 3 2.7 2 hrs. -0.018 - 0.025 + 0.0051 0 - 0.025 /16 72 4 14 mins. + 0.25 + 0.15 + 0.1 + 0.1 + 0.076 /20 66 14 2 hrs. + 0.36 + 0.3 + 0.23 + 0.2 + 0.18 6/20 62 6 mins. + 0.3 + 0.15 + 0.076 — + 0.076 — — 7 19 50 mins. + 0.47 + 0.57 + 0.41 + 0.36 + 0.33 27/46 29 8 26 mins. + 0.28 + 0.15 + 0.1 + 0.1 + 0.076 7/20 68 9 26 2 hrs. + 0.43 + 0.38 + 0.25 + 0.28 + 0.25 6/19 58 27 40 mins. + 0.53 + 0.53 + 0.38 + 0.25 + 0.28 27/47 36 11 69 -30 mins. + 0.58 + 0.56 + 0.46 + 0.41 + 0.38 7/19 41 12 72 45 mins + 0.53 + 0.61 + 0.43 + 0.36 + 0.1 37/50 31 *the first number is the number of cell where second number is the total number of cells in electrolyte was observed and the the group.

Claims

1. A nonaqueous cell comprising an active metal anode, a manganese dioxide-containing cathode and a liquid organic electrolyte comprising 3-methyl-2-oxazolidone together with a solute and wherein the manganese dioxide has a water content of less than 1 weight percent based on the weight of the manganese dioxide.

2. A nonaqueous cell as claimed in claim 1 wherein the water content is less than 0.5 weight percent based on the weight of the manganese dioxide.

3. A nonaqueous cell as claimed in claim 2 wherein the water content is less than 0.2 weight percent based on the weight of the manganese dioxide.

4. A nonaqueous cell as claimed in any one of claims 1 to 3 wherein the cathode comprises manganese dioxide, a conductive agent and a binder.

5. A nonaqueous cell as claimed in claim 4 wherein the conductive agent is carbon or graphite and the binder is polytetrafluorethylene or ethylene acrylic acid polymer.

6. A nonaqueous cell as claimed in any one of claims 1 to 5 wherein at least one cosolvent is contained in the liquid organic electrolyte.

7. A nonaqueous cell as claimed in claim 6 wherein said solvent is selected from tetrahydrofuran, dioxolane, dimethoxyethane, dimethyl isoxazole, diethyl carbonate, propylene carbonate, ethylene glycol sulfite, dioxane and dimethyl sulfite.

8. A nonaqueous cell as claimed in any one of claims 1 to 7 wherein said solute is selected from MCF^SO-j, MBF^, MCIO^, and MM'Fg wherein M is lithium, sodium or potassium and M' is phosphorus, arsenic or antimony. 16

9. A nonaqueous cell as claimed in any one of claims 1 to 8 wherein said active metal anode is selected from lithium, potassium, sodium, calcium, mangnesium, aluminium and alloys thereof.

10. A nonaqueous cell as claimed in any one of claims 1 to 6 wherein the anode is lithium and the electrolyte is LiCF^SO-j dissolved in 3-methyl-2-oxazolidone, dioxolane, dimethoxyethane and dimethyl isoxazole

11. A nonaqueous cell as claimed in any one of claims 1 to 6 wherein the anode is lithium and the electrolyte is LiBF^ dissolved in 3-methyl-2-oxazolidone and dimethoxyethane.

12. A nonaqueous cell as claimed in any one of claims 1 to 6 wherein the anode is lithium and the electrolyte is LiCF^SO^ dissolved in 3-methyl-2-oxazolidone and dimethoxyethane.

13. A nonaqueous cell as claimed in any one of claims 1 to 6 wherein the anode is lithium and the electrolyte is LiCFjSO^ dissolved in 3-methyl-2-oxazolidone and propylene carbonate.

14. A nonaqueous cell substantially as hereinbefore described with reference to any one of the Examples II to IV. Dated this 24th day of June, 1980, TOMKINS & CO., Applicants' Agents, (signed) DUBLIN 6 17