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Solid state electrolytes |
| RE31365 |
Solid state electrolytes
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| Patent Drawings: | |
| Inventor: |
Mellors |
| Date Issued: |
August 30, 1983 |
| Application: |
06/392,714 |
| Filed: |
June 28, 1982 |
| Inventors: |
Mellors; Geoffrey W. (North Royalton, OH)
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| Assignee: |
Union Carbide Corporation (Danbury, CT) |
| Primary Examiner: |
Walton; Donald L. |
| Assistant Examiner: |
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| Attorney Or Agent: |
O'Brien; Cornelius F. |
| U.S. Class: |
429/304; 429/321 |
| Field Of Search: |
429/191 |
| International Class: |
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| U.S Patent Documents: |
2718539; 3318734; 3657016; 3973990; 4118549 |
| Foreign Patent Documents: |
842829; 2330127 |
| Other References: |
Schoonman, A Solid State Galvanic Cell with Fluoride-Conducting Electrolytes, J. Electro. Chem. Science and Techno., Dec. 1976, p.1772.. |
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| Abstract: |
A solid state electrolyte comprising an ionically conducting product of a fused ternary mixture of lead fluoride, an alkali salt of sodium, potassium, rubidium or cesium in a range of 0.1 to 15.0 mole percent and a fluoride, nitrate or sulfate of magnesium, calcium, strontium or barium in a range of between 1 and 40 mole percent. |
| Claim: |
What is claimed is: .[.
1. A solid state cell electrolyte comprising an ionically conducting produce of a fused ternary mixture of lead fluoride, an alkali salt selected from the group consistingof sodium, potassium rubidium and cesium salts in a range of between about 1.0 and about 15.0 mole percent and a fluoride, nitrate or sulfate of magnesium, calcium, strontium or barium in a range between about 1 and about 40 mole percent..]. .[.2. Thesolid state cell electrolyte of claim 1 wherein the alkali salt is selected from the group consisting of potassium fluoride, rubidium fluoride, cesium fluoride, potassium carbonate, potassium sulfate and potassium nitrate..]. .[.3. The solid state cellelectrolyte of claim 1 wherein the fluoride is selected from the group consisting of strontium fluoride, calcium fluoride, barium fluoride and magnesium fluoride..]. .[.4. The solid state cell electrolyte of claim 1 wherein the nitrate is selected fromthe group consisting of calcium nitrate and strontium nitrate..]. .[.5. The solid state cell electrolyte of claim 1 wherein the sulfate is selected from the group consisting of calcium sulfate, barium sulfate and strontium sulfate..]. .[.6. The solidstate electrolyte of claim 1 wherein the ionically conducting produce is formed from the fused ternary mixture 88PbF.sub.2 -8SrF.sub.2 -4KF..]. .[.7. The solid state electrolyte of claim 1 wherein the ionically conducting product is formed from thefused ternary mixture 94PbF.sub.2 -3CaF.sub.2 -3KF..]. .[.8. The solid state electrolyte of claim 1 wherein the ionically conducting product is formed from the fused ternary mixture 95PbF.sub.2 -2CaF.sub.2 -3KF..]. .[.9. The solid state electrolyteof claim 1 wherein the ionically conducting product is formed from the fused ternary mixture 94PbF.sub.2 -2CaF.sub.2 -4KF..]. .[.10. The solid state electrolyte of claim 1 wherein the ionically conducting product is formed from the fused ternarymixture 86PbF.sub.2 -10SrF.sub.2 -4KF..]. .[.11. The solid state electrolyte of claim 1 wherein the ionically conducting product is formed from the fused ternary mixture 86PbF.sub.2 -10BaF.sub.2 -4KF..]. .[.12. The solid state electrolyte of claim 1wherein the ionically conducting product is formed from the fused ternary mixture 94PbF.sub.2 -2MgF.sub.2 -4KF..]. .Iadd.13. A solid state cell electrolyte comprising an ionically conducting product of a fused ternary mixture of lead fluoride, analkali salt selected from the group consisting of sodium salts, cesium salts and nonfluoride-containing salts of potassium and rubidium in a range of between about 1.0 and about 15.0 mole percent and a fluoride, nitrate or sulfate of magnesium, calcium,strontium or barium in a range of between about 1 and about 40 mole percent. .Iaddend. .Iadd.14. The solid state cell electrolyte of claim 13 wherein the alkali salt is selected from the group consisting of cesium fluoride, potassium carbonate,potassium
sulfate and potassium nitrate. .Iaddend. .Iadd.15. The solid state cell electrolyte of claim 13 wherein the fluoride is selected from the group consisting of strontium fluoride, calcium fluoride, barium fluoride and magnesium fluoride. .Iaddend. .Iadd.16. The solid state cell electrolyte of claim 13 wherein the nitrate is selected from the group consisting of calcium nitrate and strontium nitrate. .Iaddend. .Iadd.17. The solid state cell electrolyte of claim 13 wherein the sulfateis selected from the group consisting of calcium sulfate, barium sulfate and strontium sulfate. .Iaddend. |
| Description: |
FIELD OF THE INVENTION
The invention relates to a solid state electrolyte based on a fused ternary mixture containing lead fluoride.
BACKGROUND OF THE INVENTION
Ionic conductivity is usually associated with the flow of ions through an aqueous solution of metallic salts. In the vast majority of practical uses of ionic conductors, i.e., as electrolytes for dry cell batteries, the aqueous solution isimmobilized in a paste or gelled matrix to overcome the difficulties associated with handling and packaging a liquid. However, even after immobilization, the system is still subject to possible leakage, has a limited shelf life due to drying out orcrystallization of the salts and is suitable for use only within a limited temperature range corresponding to the liquid range of the electrolyte. In addition, the necessity of including a large volume of immobilizing material has hindered the aims ofminiaturization.
In attempting to overcome the shortcomings of liquid systems, investigators have surveyed a large number of solid compounds hoping to find compounds which are solid at room temperature and have specific conductances approaching those exhibited bythe commonly used liquid system. Most solids have specific conductances at room temperature (20.degree. C.) in the range of 10.sup.-6 to 10.sup.-15 ohm.sup.-1 cm..sup.-1 as compared to aqueous solutions of salts which nominally have a specificconductance of 0.5 to 0.8 ohm.sup.-1 cm..sup.-1.
In addition to the shortcomings of liquid systems, improved microelectronic circuit designs have generally decreased the current requirements for electronic devices. This in turn has enhanced the applicability of solid electrolyte power sourceswhich usually can only deliver currents in the microampere range. These solid electrolyte systems have the inherent advantages of being free of electrolyte leakage and internal gassing problems due to the absence of a liquid phase and corrosionphenomena. In addition, they also have a much longer shelf life than the conventional liquid power sources.
Solid electrolytes must be essentially electronic insulators so as not to internally short the cell while at the same time they must allow ionic movement in the crystal lattice for the cell to operate. It has been discovered that certainmetallic salts which are solids at room temperatures have specific conductances sufficiently high to permit their use in practical battery applications. For example, U.S. Pat. No. 3,723,185 discloses solid state electrolytes of compounds conforming tothe general formula AgI-MCN-AgCN or modifications thereof wherein M is potassium, rubidium, cesium of mixtures thereof.
Filed concurrently herewith by applicant and incorporated herein by reference in U.S. application Ser. No. 973,554 titled Solid State Electrolyte disclosing a relatively highly conducting solid state electrolyte made from a binary mixture oflead fluoride and a 0.1 to 15.0 mole percent of a selected alkali salt of sodium, potassium, rubidium and cesium.
It is an object of the present invention to provide a novel ionically conductive product that is solid at room temperature and has a high conductance to permit its use as a solid state electrolyte for battery applications.
Another object of the present invention is to provide a novel solid state electrolyte for battery applications that is essentially an electronic insulator so as not to internally short the cell in which it is to be used while at the same time itwill allow ionic movement in the crystal lattice.
Another object of the present invention is to provide a novel solid state electrolyte of a fused ternary mixture containing lead fluoride as its major component and having a highly stable ionic conductivity at room temperature thus making itadmirably suitable for battery applications.
It is another object of the present invention to provide a highly conducting solid electrolyte based on lead fluoride.
The foregoing and additional objects will become more fully apparent from the following description.
SUMMARY OF THE INVENTION
The invention relates to a solid state electrolyte comprising an ionically conductive product of a fused ternary mixture of lead fluoride (PbF.sub.2), an alkali salt selected from the group of sodium (Na), potassium (K), rubidium (Rb) and cesium(Cs) salts in a range of between about 1.0 and about 15.0 mole percent and a fluoride, nitrate or sulfate of magnesium, calcium, strontium or barium in a range between about 1 and about 40 mole percent. Preferably the range of the former should bebetween about 1 and about 5 and the range of the latter should be between about 3 and about 10 mole percent based on the electrolyte.
Preferably the ionic conductivity of the solid state electrolyte of this invention should be at least 10.sup.-5 ohm.sup.-1 centimeter.sup.-1.
Suitable alkali salts would be potassium fluoride, rubidium fluoride, cesium fluoride, potassium carbonate, potassium sulfate and potassium nitrate. Suitable fluorides would be strontium fluoride, calcium fluoride, barium fluoride and magnesiumfluoride. Suitable nitrates would be calcium nitrate and strontium nitrate. Suitable sulfates would be calcium sulfate, barium sulfate and strontium sulfate.
While both alpha-PbF.sub.2 and beta-PbF.sub.2 are anionic conductors, the beta-PbF.sub.2 is more conductive but, nonetheless, neither is of the low resistivity that would be highly desirable in a solid electrolyte application. Beta-PbF.sub.2 hasa specific resistivity of about 5.times.10.sup.6 ohm-cm, while that of alpha-PbF.sub.2 is about 5.times.10.sup.7 ohm-cm. If ordinary lead fluoride is heated for a short time above about 350.degree. C. and then cooled, it is entirely converted to thebeta form with a characteristic X-ray pattern. However, it has been observed that when this material is compressed to make a pellet for a conductivity measurement, it transforms partially to the alpha form. Although the resistivity of beta-PbF.sub.2 isat levels marginally useful as a solid electrolyte in battery applications, the instability and reversion to the alpha form manifests itself in an increasing resistivity with increase of pressure such as would be employed in the fabrication of a solidelectrolyte battery and with increase of temperature and age such as might be experienced during storage of a battery.
It has been discovered that, with the addition of the above-referred to alkali salts in a range between about 0.1 and about 15.0 mole percent and the above-referred to fluorides, nitrates and sulfates in the range of 1 to 40 mole percent to thelead fluoride, the product of the fused ternary mixture produced will have a high ionic conductivity thereby making it suitable for use in battery applications as a solid state electrolyte. It was also unexpectedly found that the addition of theabove-referred to materials to lead fluoride had a very beneficial stabilizing effect on the ionic conductivity of the lead fluoride. As used herein, the term "stability" when referring to ionic conductivity shall mean the constancy of ionicconductivity with pressure, temperature and age. As stated above, stability of the ionic conductivity of a solid anionically conductive material is necessary if it is to be used as a solid state electrolyte in battery applications.
EXAMPLE I
Several lead fluoride-containing solid state electrolytes were prepared in the following manner. Lead fluoride along with the specific additions shown in Table I were separately vacuum dried at 140.degree. C. for about an hour. The materialswere then intimately mixed, placed in a platinum boat contained in a quartz vessel flushed with argon, and slowly heated up to as high as 850.degree. C. to melt the materials. In the case of easily decomposable or volatile salts, slow heating was usedto the minimum temperature necessary to melt the mixture. The melt was thereafter held at this temperature for 15 to 20 minutes to insure a homogeneous mixture. The solidified material was easily removed from the boat on cooling, transferred to a drybox and crushed in an agate mortar. The materials were thereafter formed into pellets measuring 1 sq. cm. cross section by 0.5 to 1.0 cm thick using a Carver Laboratory press operating at 45,000 psi. The resistivity of each pellet was measured andthe results obtained are shown in Table I. As evident from the data shown in Table I, the resistivity of lead fluoride which is from 10.sup.6 to 10.sup.7 ohm-cm decreased with the addition of the materials shown to values as low as 642 ohm-cm.
TABLE I ______________________________________ Mixture Specific Resistivity Composition (Molar) (ohm-cm) at Room Temp. ______________________________________ 86PbF.sub.2 -10CaF.sub.2 -4KF 1578 81PbF.sub.2 -15CaF.sub.2 -4KF 2750 76PbF.sub.2 -20CaF.sub.2 -4KF 2200 71PbF.sub.2 -25CaF.sub.2 -4KF 2500 66PbF.sub.2 -35CaF.sub.2 -4KF 1730 61PbF.sub.2 -35CaF.sub.2 -4KF 1800 79PbF.sub.2 -6KF-15SrF.sub.2 10778 77PbF.sub.2 -8KF-15SrF.sub.2 1736 75PbF.sub.2 -10KF-15SrF.sub.2 3000 86PbF.sub.2 -10BaF.sub.2 -4KF 1100 81PbF.sub.2 -15BaF.sub.2 -4KF 2800 76PbF.sub.2 -20BaF.sub.2 -4KF 4400 71PbF.sub.2 -25BaF.sub.2 -4KF 14000 66PbF.sub.2 -30BaF.sub.2 -4KF 113000 61PbF.sub.2 -35BaF.sub.2 -4KF 132000 56PbF.sub.2-40BaF.sub.2 -4KF 483000 86PbF.sub.2 -10SrF.sub.2 -4RbF 2660 86PbF.sub.2 -10SrF.sub.2 -4KF 1477 81PbF.sub.2 -15SrF.sub.2 -4KF 2413 76PbF.sub.2 -20SrF.sub.2 -4KF 3544 71PbF.sub.2 -25SrF.sub.2 -4KF 9310 66PbF.sub.2 -30SrF.sub.2 -4KF 26000 61PbF.sub.2 -35SrF.sub.2 -4KF 70000 56PbF.sub.2 -40SrF.sub.2 -4KF 269000 88PbF.sub.2 -8SrF.sub.2 -4LiF 380000 88PbF.sub.2 8SrF.sub.2 -4NaF 20000 88PbF.sub.2 8SrF.sub.2 -4RbF 5700 88PbF.sub.2 -8SrF.sub.2 -4CsF 63000 88PbF.sub.2 8SrF.sub.2-4RbCl 4100 76PbF.sub.2 -20CaF.sub.2 -4RbF 5200 76PbF.sub.2 -20BaF.sub.2 -4RbF 6500 81PbF.sub.2 -15SrF.sub.2 -4KBr 5200 81PbF.sub.2 -15SrF.sub.2 -4K.sub.2 CO.sub.3 7100 81PbF.sub.2 -15SrF.sub.2 -4K.sub.2 SO.sub.4 8500 76PbF.sub.2 -20SrF.sub.2-4KBr 7500 76PbF.sub.2 -20SrF.sub.2 -4K.sub.2 CO.sub.3 9800 76PbF.sub.2 -20SrF.sub.2 -4K.sub.2 SO.sub.4 18400 96PbF.sub.2 -2CaF.sub.2 -2KF 1326 94PbF.sub.2 -3CaF.sub.2 -3KF 827 95PbF.sub.2 -2CaF.sub.2 -3KF 766 94PbF.sub.2 -2CaF.sub.2 -4KF 642 95PbF.sub.2 -3CaF.sub.2 -2KF 1134 94PbF.sub.2 -1CaF.sub.2 -5RbCl 3450 96PbF.sub.2 -2MgF.sub.2 -2KF 3630 94PbF.sub.2 -1MgF.sub.2 -5KF 2430 94PbF.sub.2 -2MgF.sub.2 -4KF 1108 96PbF.sub.2 -2MgF.sub.2 -2K.sub.2 CO.sub.3 4400 94PbF.sub.2-1MgF.sub.2 -5K.sub.2 CO.sub.3 1047 94PbF.sub.2 -1MgF.sub.2 -4K.sub.2 CO.sub.3 1161 88PbF.sub.2 -8MgF.sub.2 -4KF 26400 86PbF.sub.2 -10MgF.sub.2 -4KF 21900 76PbF.sub.2 -20MgF.sub.2 -4KF 40200 90PbF.sub.2 -5SrF.sub.2 -5KF 848 88PbF.sub.2-8SrF.sub.2 -2K.sub.2 CO.sub.3 1970 90PbF.sub.2 -8SrF.sub.2 -2K.sub.2 CO.sub.3 1202 86PbF.sub.2 -10CaF.sub.2 -2K.sub.2 CO.sub.3 1815 86PbF.sub.2 -10SrF.sub.2 -2K.sub.2 CO.sub.3 1405 96PbF.sub.2 -2Sr(NO.sub.3).sub.2 -2KNO.sub.3 1078 86PbF.sub.210Sr(NO.sub.3).sub.2 -4KNO.sub.3 8290 86PbF.sub.2 -10SrF.sub.2 4KNO.sub.3 1450 *88PbF.sub.2 -8SrF.sub.2 -4KF 857 90PbF.sub.2 -6SrF.sub.2 -4KF 1034 94.5PbF.sub.2 -0.5CaSO.sub.4 -5.0KF 1136 94.5PbF.sub.2 -0.5CaSO.sub.4 -5.0K.sub.2 CO.sub.3 1164 88PbF.sub.2 -8SrF.sub.2 -4K.sub.2 SO.sub.4 5700 88PbF.sub.2 -8SrF.sub.2 -4KNO.sub.3 1900 88PbF.sub.2 -8SrF.sub.2 -4KCl 20000 88PbF.sub.2 -8SrF.sub.2 -4KBr 2500 88PbF.sub.2 -8SrF.sub.2 -4K.sub.2 CO.sub.3 1700 88PbF.sub.2 -8BaF.sub.2 -4KF 1050 88PbF.sub.2 -8BaF.sub.2 -4K.sub.2 SO.sub.4 5900 88PbF.sub.2 -4CaF.sub.2 -4SrF.sub.2 -4KF 4000 88PbF.sub.2 -4CaF.sub.2 -4SrF.sub.2 -4K.sub.2 SO.sub.4 15600 ______________________________________ *The ionically conducting product formed from thisternary mixture was analyzed and found to contain the following: 78.63 wt./percent lead, 3.07 wt./percent strontium, 15.97 wt./percent fluorine and 0.60 wt./percent potassium.
EXAMPLE II
A lead disc anode, a solid electrolyte made from the molar mixture of 88PbF.sub.2 -8SrF.sub.2 -4KF and a cathode consisting of a 1:1 molar mixture of MnF.sub.3 and PbO.sub.2 which was further diluted with about 30 wt. % of the electrolyte wascompressed together in a cavity of 1-cm.sup.2 cross section at about 12,000 psi. The open circuit voltage of the cell so produced was 1.60 volts and when discharged across a 500-K-ohm resistor, the initial closed circuit voltage was 1.56 volts.
EXAMPLE III
A cell was prepared as in Example II with the exception that the cathode was a 1:1 molar mixture of CoF.sub.3 and PbO.sub.2. The open circuit voltage of the cell so produced was 1.9 volts and fell to 1.88 volts initially when a 100-K-ohmresistor was connected across the cell.
EXAMPLE IV
To further test the solid state electrolyte of this invention in a cell, a sheet-lead anode, a solid electrolyte made from the molar mixture 88PbF.sub.2 -8SrF.sub.2 -4KF and a lead dioxide (PbO.sub.2) cathode were assembled together to form acell. The open circuit voltage of the cell so produced was 1.192 volts and when discharged across a 500-K-Ohm resistor, the initial closed circuit voltage was 1.170 volts. Under this load condition, the initial current density was calculated to be 2.3.mu.A/cm.sup.2. Thus the solid state electrolyte of this invention is admirably suited for battery applications.
EXAMPLE V
A cell was constructed as described in Example IV with the exception that the cathode was electrolytic manganese dioxide mixed with the electrolyte made from the molar mixture 88PbF.sub.2 -8 SrF.sub.2 -4KF. The open circuit voltage of the cellso produced was 1.088 volts and when discharged across a 500-K-ohm resistor, the initial closed circuit voltage was 1.082 volts.
EXAMPLE VI
Several additional cells were prepared using an anode of lead, a solid electrolyte made from the molar mixture 88PbF.sub.2 -8SrF.sub.2 -4FK and a cathode as shown in Table II. The open circuit voltage of each cell produced was measured and isshown in Table II. From the data shown in Table II it is evident that the solid state electrolytes of this invention can be admirably suited for battery applications.
TABLE II ______________________________________ Cathode O.C.V. Cathode O.C.V. Material (Volts) Material (Volts) ______________________________________ HgF.sub.2 + graphite 1.20 CF.sub.x 0.50 AgF.sub.2 + graphite 1.90 EMD(MnO.sub.2)/HgO 1.05 BiF.sub.3 + graphite 0.86 CoF.sub.3.MnO.sub.2 1.23 CoF.sub.3 + graphite 1.35 BrF.sub.3.PbO.sub.2 1.11 MnF.sub.3 + graphite 0.26 MnF.sub.3.PbO.sub.2 1.71 PbO.sub.2 1.04 CoF.sub.3.PbO.sub.2 1.90 YF.sub.3 + graphite 0.95TaF.sub.5.PbO.sub.2 1.80 AuF.sub.3 + graphite 1.24 V.sub.2 O.sub.5 0.85 FeF.sub.2 + graphite 1.04 FeS.sub.2 0.53 FeF.sub.3 + graphite 0.66 WO.sub.3 0.185 EMD(MnO.sub.2) 1.09 CoF.sub.3.HlO.sub.3 1.625 MnF.sub.3 /MnO.sub.2 1.30 TaF.sub.5 +graphite 0.69 CuF.sub.2 + graphite 0.80 TaF.sub.5.MnF.sub.3 + graphite 1.52 ______________________________________
As evident from the examples above the solid state electrolyte of this invention can be used with various cell systems employing an anode such as lead or any metal more noble than lead and fluoride-containing solid cathodes.
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