CA1165813A - Electrochemical cell and electrolytic solution therefor - Google Patents
Electrochemical cell and electrolytic solution thereforInfo
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- CA1165813A CA1165813A CA000376610A CA376610A CA1165813A CA 1165813 A CA1165813 A CA 1165813A CA 000376610 A CA000376610 A CA 000376610A CA 376610 A CA376610 A CA 376610A CA 1165813 A CA1165813 A CA 1165813A
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- electrolytic solution
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- H—ELECTRICITY
- H01—ELECTRIC ELEMENTS
- H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
- H01M6/00—Primary cells; Manufacture thereof
- H01M6/14—Cells with non-aqueous electrolyte
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- Manufacturing & Machinery (AREA)
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- Chemical Kinetics & Catalysis (AREA)
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Abstract
ABSTRACT OF THE DISCLOSURE
An electrochemical cell having an oxidizable anode containing lithium and a cathode current collector. The cell includes an electrolytic solution in contact with the anode and the cathode current collector. The solu-tion includes a solvent which is also a reducible liquid cathode material, specifically SOCl2, and an electrolyte solute consisting of the reaction products of a salt of an oxyacid, specifically Li2SO3, constituting a Lewis base and a Lewis acid, specifically AlCl3, dissolved in the solvent.
An electrochemical cell having an oxidizable anode containing lithium and a cathode current collector. The cell includes an electrolytic solution in contact with the anode and the cathode current collector. The solu-tion includes a solvent which is also a reducible liquid cathode material, specifically SOCl2, and an electrolyte solute consisting of the reaction products of a salt of an oxyacid, specifically Li2SO3, constituting a Lewis base and a Lewis acid, specifically AlCl3, dissolved in the solvent.
Description
1:~6~3~3 `-220~:0 ~1--ELEC'.l.'ROC~lEMIC~I. CELL AND ELECT OLYTIC SOLUT OP THEREPOR
This invention relates to electrochemical cells.
More particularly, it is concerned with elec~rochemical cells employing non-aqueous electrslytic solutions and to electrolytic solutions cherefor.
A particularly effectiJe clas~ of elec~rochemica]
cells which employs soluble or liqui~ cathcde materials has undergone rapid development in recent years~ In these cells the active cathode material is usually a fluid solvent for an electrolyte solute which provi~es conductivity. The active anocle for these cells ;~.~
usual:Ly lithium or other hiyhly electropositi.-~e me-tal.
During discharge the sol~ent is electrochemicall~7 re~
duced on a cathode current collector to yi.elcl ions, e~g., halide i.ons, which react wit~ positive metal ions from the. anode to form insoluble metal salts, e.g., metal halides.
One particular type of elect.rochemical cell of the foregoing class which contains a lithium anode emplo~s a reducible liquid cathode of thion~l chloride. Typi-cally the electrolyte solute dissolvea n the thionyl chloride solvent is lithium tetrachloroaluminate. This salt is prepared from the Lewis acia alum.num chloride and the Lewis base lithium chloride. A Le~Jis acid is any compound capable of entering into a chemical reac~
tion by acceptinct an eletron pair to ~orm a covalent bon~, and a Lewi.~ base i~ any compound capable of entering i.nto a chemical reaction by ~onati.n~ arl 5 $3 ~ ~
.-22020 ~2-electron pair to form a covalent bond. Lithium/thionyl chloride elect~-ochemical cells have proven to have outstanding weight and volume energy density, long shelf lire, and unusually high power density when comparcd with other cells presently available.
Under unfavorable circumstances during prolonged stora~e or ~torage under extreme conditions, corrosion of the lithium anode in a cell causes a film of lithium chloride to grow on the anode sufficient to cause signl-Eicant polarization at the onse-t of discharge of the cell~ After operating at a reduced potential for a period of time, a cell may recover depending upon the ~severity of the condition. This initial polarization is ~ef~rred to as voltage delay and has been found particu-larl~ troublesome in cells which are required to operate at current densities higher than 1 mA/cm .
Various attempts have been made to overcome the problem of vol.tage delay upon startup. In one techni~ue desc.ci.bed in U.S. Patent No. 4,020,240 to Carl R.
Schlai~jer dated April 26, 1977, a lithium clovoborate salt such as Li2 BloCllo is enmployed as the electrolyte solute. In another l:echnique described by J. P~ Gabano in pa~er -,~27, presented at the Electrochemical Societ~ -~all ~ee-ki.ng, .ittsburgh, October 15-20, 1978, the electrolyte solute is a salt prepared by dissolving li.thium oxide in thionyl chloride containing aluminum chloride~ It is postulated that the salt produced by the reaction is Li2 (AlC130 AlC13). Although the solutes of SchlaiXjer and ~abano provide cells having i.rnproved startup characteristics, either they are ex-pensive, diEficu3.t to puri:Ey or l.ess conduct1ve than -220~0 ~-presently used materials.
Accordingly, the present invention provides an electrochemical cell eomprising an oxidizable anode material; a reducible cathode material; and an eleetrolyte solute in an electrolytic solution, the solute consisting of the reaction products of a salt of an oxyacid constituting a Lewis base and a Lewis acid dissolved in the solvent of ~he electrolytic solution.
Some e~odiments of the invention will now be described, by way of example, w.ith reference to the accompanying drawings in which: 5 FIG. 1 is a graph illustrating the conductivity of an electroly~ic solution in accordance with the presen-t inven-tion in comparison with other solutions;
FIG. 2 is an elevational view partially in cross
This invention relates to electrochemical cells.
More particularly, it is concerned with elec~rochemical cells employing non-aqueous electrslytic solutions and to electrolytic solutions cherefor.
A particularly effectiJe clas~ of elec~rochemica]
cells which employs soluble or liqui~ cathcde materials has undergone rapid development in recent years~ In these cells the active cathode material is usually a fluid solvent for an electrolyte solute which provi~es conductivity. The active anocle for these cells ;~.~
usual:Ly lithium or other hiyhly electropositi.-~e me-tal.
During discharge the sol~ent is electrochemicall~7 re~
duced on a cathode current collector to yi.elcl ions, e~g., halide i.ons, which react wit~ positive metal ions from the. anode to form insoluble metal salts, e.g., metal halides.
One particular type of elect.rochemical cell of the foregoing class which contains a lithium anode emplo~s a reducible liquid cathode of thion~l chloride. Typi-cally the electrolyte solute dissolvea n the thionyl chloride solvent is lithium tetrachloroaluminate. This salt is prepared from the Lewis acia alum.num chloride and the Lewis base lithium chloride. A Le~Jis acid is any compound capable of entering into a chemical reac~
tion by acceptinct an eletron pair to ~orm a covalent bon~, and a Lewi.~ base i~ any compound capable of entering i.nto a chemical reaction by ~onati.n~ arl 5 $3 ~ ~
.-22020 ~2-electron pair to form a covalent bond. Lithium/thionyl chloride elect~-ochemical cells have proven to have outstanding weight and volume energy density, long shelf lire, and unusually high power density when comparcd with other cells presently available.
Under unfavorable circumstances during prolonged stora~e or ~torage under extreme conditions, corrosion of the lithium anode in a cell causes a film of lithium chloride to grow on the anode sufficient to cause signl-Eicant polarization at the onse-t of discharge of the cell~ After operating at a reduced potential for a period of time, a cell may recover depending upon the ~severity of the condition. This initial polarization is ~ef~rred to as voltage delay and has been found particu-larl~ troublesome in cells which are required to operate at current densities higher than 1 mA/cm .
Various attempts have been made to overcome the problem of vol.tage delay upon startup. In one techni~ue desc.ci.bed in U.S. Patent No. 4,020,240 to Carl R.
Schlai~jer dated April 26, 1977, a lithium clovoborate salt such as Li2 BloCllo is enmployed as the electrolyte solute. In another l:echnique described by J. P~ Gabano in pa~er -,~27, presented at the Electrochemical Societ~ -~all ~ee-ki.ng, .ittsburgh, October 15-20, 1978, the electrolyte solute is a salt prepared by dissolving li.thium oxide in thionyl chloride containing aluminum chloride~ It is postulated that the salt produced by the reaction is Li2 (AlC130 AlC13). Although the solutes of SchlaiXjer and ~abano provide cells having i.rnproved startup characteristics, either they are ex-pensive, diEficu3.t to puri:Ey or l.ess conduct1ve than -220~0 ~-presently used materials.
Accordingly, the present invention provides an electrochemical cell eomprising an oxidizable anode material; a reducible cathode material; and an eleetrolyte solute in an electrolytic solution, the solute consisting of the reaction products of a salt of an oxyacid constituting a Lewis base and a Lewis acid dissolved in the solvent of ~he electrolytic solution.
Some e~odiments of the invention will now be described, by way of example, w.ith reference to the accompanying drawings in which: 5 FIG. 1 is a graph illustrating the conductivity of an electroly~ic solution in accordance with the presen-t inven-tion in comparison with other solutions;
FIG. 2 is an elevational view partially in cross
2~ section of an electrochemical cell in aecGrdance with the present invention;
FIG. 3 is a graph illustrating the startup charac-ter-istics of electrochemical cells of previously known type; and 5 FIG. 4 i.s a graph illustrating the startup character-istics o~ eleetrochemical cells in accordance with the present invention.
For a better understanding of the present invention, together.with other and further objects, advantages, and ,~ ~ 1 6 22020 -~-capabilities thereof, reference is made to the following discussion and appended claims in connection with the above described drawings.
The present invention relates to non-aqueous elec-trolytic solutions containing an electrolyte salt pro-duced by the react~on of a salt of an oxyacid which cons'itutes a L,ew;s base with a Lewis acid. 5alts of oxyac~ds which may be em~loyed in electroly-tic solutions of the invention pro~ide a cation of an alkali metal, alkaline earth matal, ammonium, alkyl ammonium, pyridini-um, alkyl pvridinium, scandium, yttrium, or a rare earth.
Suitable oxyacid salts provide an anion such as orthob~-xa5:e, metaborate, aluminate, C03 , SiO3 , GeO
~n3 ~ N03 , P03 , P04 , AsO3 , As04 , S03 , SO~ , SeO4 , TeO4 , TeO4 , S204 ~ S26 ~ P
thiosulfate, molybdate, phosphomalybdate, tungstate, _ C103 , C104 , BrO3 , BrO4 , I03 , and I04 Th~ oxyacid sa~t is reacted wi.th a Lewis acid such as AlC13, AlBr3, AlI3~ BC13~ BF~ BBr3~ BI3~ PF5~ AsF5~ ~bF5~ SbC15, SnC14~ TiC14~ ZrC14~ Ga~l3~ GaF3~ GaBr3~ GaI3, InC~3, In~3~ IrlBr3, InI3~ TlC13, TlE'39 SiF4~ ana GeC14-The solute is produced by the reac-tion obtained by dissolving the salt of an oxyacid and a Lewis acid in a solvent. The solvent may be an electrochemically redu-cible liquid such as an oxyhalide of sulfur, phosphorus, or selenium. It may also be a fluid non-metallic oxide, or a fluid non-me~allic halide, or mixtures thereo-f~
Qther classes of solvellt which may be utilized include 30 aliphatic ether~;, alicylic ethers, este.rs, cyclic es~ers, j '. ` ~
, ? ~ f3 1~
-22020 ~5-cyclic lactone.q, anhydrides, nitriles, amides, and ureas~
Electrochemical cells utilizing electrolytic solu~
tions in accordance with th~ present invention May also employ oxidizable anode materials other than lithl-lm.
The anode material may be another alkali metal, an alka-line earth metal, scandium, yttrium, or a rare earth.
.More specifically, an electrolytic solu~ion parti-cularly useful in electrochemical cells employiny ].ithium and thionyl. chloride was obtained by reacting aluminum chloride (AlC13), a Lewis acid, with lithi.um sul~ite (Li2503), which constitutes a Lewis base. A 1 M solution of AlC13 in SOC12 was stirred while bei.ng hea-ted under reflux with enough solid Li2S03 -..o provide a stoich.o-metxic ratio of AlC13 to Li2S03 of 2 to 1.1. The con-ductivity of the solution was tested at various tempera-tures and the curve of conductivity versus temperature i9 plotted in FIG~ 1. Curves illustrating the conducti-vity of a l.OM soluti.on of LiAlC14 in SOC12, a 0.5 ~
solution of Li.~BloCllo in SOCl2, and a 4 M solution of AlC13 in SOCl~ are also shown in FIG. 1. Also shown i~ a curve illll.strating the.conductivity of a 0.5 M Li2 ~.~].C130AlCl3) solution in ~OCl~. It is postulaked that this is the salt produced by dissolving Li20 in SOCl2 ~5 containing AlCl3 in accordance with the teaching3 in the aforementioned al~ticle by Gabano. As can be seen from the curves of FIG. ~ the conductivity of applicants' solution cornpares favorably with that of lithium tetrachloroaluminate and is significantly highe~ tharl that of solutiGns contai.nillg Lithium clo~oborate ~n~ the sal.ts prepared in accordance with the technique of:
Gabano.
i 1 6~8 ~. 3 ~-22020 -6-The properties of the electrolytic so:lution of -the present inventlon indicate that a soluble lithium salt is a product of the reaction of the Li2SO3 and AlC13 in SOC12~ It may be that the Li2So3~ actiny as a Lewis base, forms an adduct salt wi-th the AlC13, a Lewis acid.
Several electrochemical cells as illustrated in FIG.
2 were constructed. Some were filled with an electrolytic solution containing lithium tetrachloroaluminate as a solute and some were filled with an electroly~ic solution in accordance with the present invention. The cells were about the size of commercial AA cells, approximately 1-7/8 inches long and 1/2 inch in diameter. The cases 10 were of stainless steel. Anodes 11 of lithium metal were pressed to the inside walls of the cases 10. Concentric bobbin cathodes 13 of Shawinigan (trade mark) carbon black and Teflon (trade mark) formed as an aqueous dispersion and dried were placed in the cases encircled by separators 12 of insulating material. After being filled with an electrolytic solution, each case was sealed with a ~over 15 having a conductive lead 16 to the cathode 13 through a glass-to~metal seal 17, Some of the cells were filled with a 1.8 M solution of LiAlC14 in SOC12. Other cells were illed with an electrolytic solution in accordance with the present 2S invention. The solution was prepared by refluxing a solution of AlC13 in SOC12 with excess Li2SO3 for sixteen days. The mixture was then filtered and diluted such that the concentration of aluminum was reduced to about
FIG. 3 is a graph illustrating the startup charac-ter-istics of electrochemical cells of previously known type; and 5 FIG. 4 i.s a graph illustrating the startup character-istics o~ eleetrochemical cells in accordance with the present invention.
For a better understanding of the present invention, together.with other and further objects, advantages, and ,~ ~ 1 6 22020 -~-capabilities thereof, reference is made to the following discussion and appended claims in connection with the above described drawings.
The present invention relates to non-aqueous elec-trolytic solutions containing an electrolyte salt pro-duced by the react~on of a salt of an oxyacid which cons'itutes a L,ew;s base with a Lewis acid. 5alts of oxyac~ds which may be em~loyed in electroly-tic solutions of the invention pro~ide a cation of an alkali metal, alkaline earth matal, ammonium, alkyl ammonium, pyridini-um, alkyl pvridinium, scandium, yttrium, or a rare earth.
Suitable oxyacid salts provide an anion such as orthob~-xa5:e, metaborate, aluminate, C03 , SiO3 , GeO
~n3 ~ N03 , P03 , P04 , AsO3 , As04 , S03 , SO~ , SeO4 , TeO4 , TeO4 , S204 ~ S26 ~ P
thiosulfate, molybdate, phosphomalybdate, tungstate, _ C103 , C104 , BrO3 , BrO4 , I03 , and I04 Th~ oxyacid sa~t is reacted wi.th a Lewis acid such as AlC13, AlBr3, AlI3~ BC13~ BF~ BBr3~ BI3~ PF5~ AsF5~ ~bF5~ SbC15, SnC14~ TiC14~ ZrC14~ Ga~l3~ GaF3~ GaBr3~ GaI3, InC~3, In~3~ IrlBr3, InI3~ TlC13, TlE'39 SiF4~ ana GeC14-The solute is produced by the reac-tion obtained by dissolving the salt of an oxyacid and a Lewis acid in a solvent. The solvent may be an electrochemically redu-cible liquid such as an oxyhalide of sulfur, phosphorus, or selenium. It may also be a fluid non-metallic oxide, or a fluid non-me~allic halide, or mixtures thereo-f~
Qther classes of solvellt which may be utilized include 30 aliphatic ether~;, alicylic ethers, este.rs, cyclic es~ers, j '. ` ~
, ? ~ f3 1~
-22020 ~5-cyclic lactone.q, anhydrides, nitriles, amides, and ureas~
Electrochemical cells utilizing electrolytic solu~
tions in accordance with th~ present invention May also employ oxidizable anode materials other than lithl-lm.
The anode material may be another alkali metal, an alka-line earth metal, scandium, yttrium, or a rare earth.
.More specifically, an electrolytic solu~ion parti-cularly useful in electrochemical cells employiny ].ithium and thionyl. chloride was obtained by reacting aluminum chloride (AlC13), a Lewis acid, with lithi.um sul~ite (Li2503), which constitutes a Lewis base. A 1 M solution of AlC13 in SOC12 was stirred while bei.ng hea-ted under reflux with enough solid Li2S03 -..o provide a stoich.o-metxic ratio of AlC13 to Li2S03 of 2 to 1.1. The con-ductivity of the solution was tested at various tempera-tures and the curve of conductivity versus temperature i9 plotted in FIG~ 1. Curves illustrating the conducti-vity of a l.OM soluti.on of LiAlC14 in SOC12, a 0.5 ~
solution of Li.~BloCllo in SOCl2, and a 4 M solution of AlC13 in SOCl~ are also shown in FIG. 1. Also shown i~ a curve illll.strating the.conductivity of a 0.5 M Li2 ~.~].C130AlCl3) solution in ~OCl~. It is postulaked that this is the salt produced by dissolving Li20 in SOCl2 ~5 containing AlCl3 in accordance with the teaching3 in the aforementioned al~ticle by Gabano. As can be seen from the curves of FIG. ~ the conductivity of applicants' solution cornpares favorably with that of lithium tetrachloroaluminate and is significantly highe~ tharl that of solutiGns contai.nillg Lithium clo~oborate ~n~ the sal.ts prepared in accordance with the technique of:
Gabano.
i 1 6~8 ~. 3 ~-22020 -6-The properties of the electrolytic so:lution of -the present inventlon indicate that a soluble lithium salt is a product of the reaction of the Li2SO3 and AlC13 in SOC12~ It may be that the Li2So3~ actiny as a Lewis base, forms an adduct salt wi-th the AlC13, a Lewis acid.
Several electrochemical cells as illustrated in FIG.
2 were constructed. Some were filled with an electrolytic solution containing lithium tetrachloroaluminate as a solute and some were filled with an electroly~ic solution in accordance with the present invention. The cells were about the size of commercial AA cells, approximately 1-7/8 inches long and 1/2 inch in diameter. The cases 10 were of stainless steel. Anodes 11 of lithium metal were pressed to the inside walls of the cases 10. Concentric bobbin cathodes 13 of Shawinigan (trade mark) carbon black and Teflon (trade mark) formed as an aqueous dispersion and dried were placed in the cases encircled by separators 12 of insulating material. After being filled with an electrolytic solution, each case was sealed with a ~over 15 having a conductive lead 16 to the cathode 13 through a glass-to~metal seal 17, Some of the cells were filled with a 1.8 M solution of LiAlC14 in SOC12. Other cells were illed with an electrolytic solution in accordance with the present 2S invention. The solution was prepared by refluxing a solution of AlC13 in SOC12 with excess Li2SO3 for sixteen days. The mixture was then filtered and diluted such that the concentration of aluminum was reduced to about
3 M. For both electrolytic solutions the SOC12 solvent was the reducible liquid cathode material of the cells.
Three cells containing LiAlC14 as a solute and three cells with Li2SO3 and LiC13 were stored for four days at .~, .
- . . . , ~ . . . . .. .. .
.
~ ~ 3 ~; 5 ~
22020 -7~
72 C, The startup charactsristi.cs o~ these cells at room temperature under a load of $0 ohms and current densities at about 408 mA/crn were recorded. The result-ing curves of output voltage versus time for the cells employing LiAlC14 in SOC12 are shown in FIG~ 3. Output voltage ve.rsus time for the three cells containing the reaction products of Li2S03 and LiC13 in SOC12 are shown in FIG. 4. As indicated by FIGS. 3 and 4 electrochemical cells employing an electrolvtic solution in accordance with the present invention operate at full operating - potential immediately upon startup withou~ the voltage delay problem encountered with previously known de~ices.
While there has been shown and described what are considered preferred embodiments of the present inven.tion, it will be obvious to those skilled in the art that va~i-ous changes and modifications may be made therein withoutdeparting from the invention as de-ined by the appende~ ..
claims. .
' . ~ , ' .. ' ' ' '~ .
Three cells containing LiAlC14 as a solute and three cells with Li2SO3 and LiC13 were stored for four days at .~, .
- . . . , ~ . . . . .. .. .
.
~ ~ 3 ~; 5 ~
22020 -7~
72 C, The startup charactsristi.cs o~ these cells at room temperature under a load of $0 ohms and current densities at about 408 mA/crn were recorded. The result-ing curves of output voltage versus time for the cells employing LiAlC14 in SOC12 are shown in FIG~ 3. Output voltage ve.rsus time for the three cells containing the reaction products of Li2S03 and LiC13 in SOC12 are shown in FIG. 4. As indicated by FIGS. 3 and 4 electrochemical cells employing an electrolvtic solution in accordance with the present invention operate at full operating - potential immediately upon startup withou~ the voltage delay problem encountered with previously known de~ices.
While there has been shown and described what are considered preferred embodiments of the present inven.tion, it will be obvious to those skilled in the art that va~i-ous changes and modifications may be made therein withoutdeparting from the invention as de-ined by the appende~ ..
claims. .
' . ~ , ' .. ' ' ' '~ .
Claims (12)
PROPERTY OR PRIVILEGE IS CLAIMED ARE DEFINED AS FOLLOWS:
1. An electrochemical cell comprising an oxidizable anode material;
a reducible cathode material; and an electrolyte solute in an electrolytic solution, the solute consisting of the reaction products of a salt of an oxyacid constituting a Lewis base and a Lewis acid dissolved in the solvent of the electrolytic solution.
a reducible cathode material; and an electrolyte solute in an electrolytic solution, the solute consisting of the reaction products of a salt of an oxyacid constituting a Lewis base and a Lewis acid dissolved in the solvent of the electrolytic solution.
2. An electrochemical cell in accordance with Claim 1 wherein the salt of an oxyacid constituting a Lewis base has a cation selected from the group consisting of alkali metals, alkaline earth metals, ammonium, alkyl ammonium, pyridinium, alkyl pyridinium, scandium, yttrium, and the rare earths, and has an oxygen containing anion selected from the group consisting of orthoborates, metaborates, aluminates, , polythionates, thiosulfates, molybdates, phosphomolybdates, tungstates, C1O3-, ClO4-, BrO3-, BrO4, lO3-, and IO4-; and the Lewis acid is selected from the group consisting of AlCl3, AlBr3, AlI3, BCl3, BF3, BBr3, BI3, PF5, AsF5, SbF5, SbCl5, SnCl4, TiCl4, ZrCl4, GaCl3, GaF3, GaBr3, GaI3, InCl3, InF3, InBr3, InI3, TlCl3, TlF3, SiF4, and GeCl4.
3. An electrochemical cell comprising an oxidizable anode material;
a cathode current collector; and an electrolytic solution, in contact with the anode material and the cathode current collector, comprising a reducible liquid cathode material and an electrolyte solute consisting of the reaction products of a salt of an oxyacid constituting a Lewis base and a Lewis acid dissolved in the liquid cathode material.
a cathode current collector; and an electrolytic solution, in contact with the anode material and the cathode current collector, comprising a reducible liquid cathode material and an electrolyte solute consisting of the reaction products of a salt of an oxyacid constituting a Lewis base and a Lewis acid dissolved in the liquid cathode material.
4. An electrochemical cell in accordance with Claim 3 wherein the salt of an oxyacid constituting a Lewis base has a cation selected from the group consist-ing of alkali metals, alkaline earth metals, ammonium, alkyl ammonium, pyridinium, alkyl pyridinium, scandium, yttrium, and the rare earths, and has an oxygen containing anion selected from the group consisting of orthobo-rates, metaborates, aluminates, polythionates, thio-sulfates, molybdates, phosphomolybdates, tungstates, CIO3-, ClO4-, BrO3-, BrO4-, IO3-, and IO4-; and the Lewis acid is selected from the group consisting of AlCl3, AlBr3, AlI3, BCl3, BF3, BBr3, BI3, PF5, AsF5, SbF5, SbCl5, SnCl4, TiCl4, ZrCl4, GaCl3, GaF3, GaBr3, GaI3, InCl3, InF3, InBr3, InI3, TlCl3, TlF3, SiF4, and GeCl4.
5. An electrochemical cell in accordance with Claim 4 wherein the reducible liquid cathode material is selected from the group consisting of fluid oxyhalides, fluid non-metallic oxides, fluid non-metallic halides, and mixtures thereof; and the oxidizable anode material is selected from the group consisting of alkali metals, alkaline earth metals, scandium, yttrium, and rare earths.
6. An electrochemical cell in accordance with claim 5 wherein the reducible liquid cathode material is selected from the group consisting of oxyhalides of sulfur, phosphorus and selenium;
the salt of any oxyacid constituting a Lewis base is lithium sulfite;
the Lewis acid is aluminum chloride; and the oxidizable anode material is lithium metal.
the salt of any oxyacid constituting a Lewis base is lithium sulfite;
the Lewis acid is aluminum chloride; and the oxidizable anode material is lithium metal.
7. An electrochemical cell in accordance with claim 6 wherein the reducible liquid cathode material is thionyl chloride.
8. An electrolytic solution including in combination a liquid electrochemically reducible solvent selected from the group consisting of fluid oxyhalides, fluid non-metallic oxides, fluid non-metallic halides, and mixtures thereof; and an electrolyte solute consisting of the reaction products of a salt of an oxyacid constituting a Lewis base and a Lewis acid dissolved in the solvent.
9. An electrolytic solution in accordance with claim 8 wherein the salt of an oxyacid constituting a Lewis base has a cation selected from the group consisting of alkali metals, alkaline earth metals, ammonium, alkyl ammonium, pyridinium, alkyl pyridinium, scandium, yttrium, and the rare earths, and has an oxygen containing anion selected from the group consisting of orthoborates, metaborates, aluminates, , polythionates, thiosulfates, molybdates, phospho-molybdates, tungstates, ClO3-, ClO4-, BrO3-, BrO4-, IO3-, and IO4-; and the Lewis acid is selected from the group consisting of AlCl3, AlBr3, AlI3, BCl3, BF3, BBr3, BI3, PF5, AsF5, SbF5, SbCl5, SnCl4, TiCl4, ZrCl4, GaCl3, GaF3, GaBr3, GaI3, InCl3, InF3, InBr3, InI3, TlCl3, TlF3, SiF4, and GeCl4.
10. An electrolytic solution in accordance with claim 9 wherein the liquid electrochemically reducible solvent is selected from the group consisting of fluid oxyhalides, fluid non-metallic oxides, fluid non-metallic halides, and mixtures thereof.
11. An electrolytic solution in accordance with claim 10 wherein the liquid electrochemically reducible solvent is selected from the group consisting of oxyhalides of sulfur, phosphorus, and selenium;
the salt of an oxyacid constituting a Lewis base is lithium sulfite; and the Lewis acid is aluminum chloride.
the salt of an oxyacid constituting a Lewis base is lithium sulfite; and the Lewis acid is aluminum chloride.
12. An electrolytic solution in accordance with claim 11 wherein the liquid electrochemically reducible solvent is thionyl chloride.
Applications Claiming Priority (2)
| Application Number | Priority Date | Filing Date | Title |
|---|---|---|---|
| US14798580A | 1980-05-08 | 1980-05-08 | |
| US147,985 | 1980-05-08 |
Publications (1)
| Publication Number | Publication Date |
|---|---|
| CA1165813A true CA1165813A (en) | 1984-04-17 |
Family
ID=22523742
Family Applications (1)
| Application Number | Title | Priority Date | Filing Date |
|---|---|---|---|
| CA000376610A Expired CA1165813A (en) | 1980-05-08 | 1981-04-30 | Electrochemical cell and electrolytic solution therefor |
Country Status (3)
| Country | Link |
|---|---|
| JP (1) | JPS573373A (en) |
| CA (1) | CA1165813A (en) |
| DE (1) | DE3117760A1 (en) |
Cited By (1)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| CN116435591A (en) * | 2023-04-24 | 2023-07-14 | 湖南添越能源科技有限公司 | Lithium ion battery electrode material suitable for working under ultralow temperature condition |
Families Citing this family (10)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| JPS58121563A (en) * | 1982-01-12 | 1983-07-19 | Hitachi Maxell Ltd | Inorganic electrolyte battery |
| JPS58200745A (en) * | 1982-05-17 | 1983-11-22 | 井浦 忠 | Transfer bed for disabled person |
| JPH0647409B2 (en) * | 1983-12-03 | 1994-06-22 | 株式会社島津製作所 | Object transfer device |
| JPS60185553A (en) * | 1984-03-06 | 1985-09-21 | 工業技術院長 | Movable deck support structure in patient carrying apparatus |
| JPS6129726U (en) * | 1984-07-12 | 1986-02-22 | 東陽精工株式会社 | Victim movement equipment |
| JPS6126518U (en) * | 1984-07-20 | 1986-02-17 | オ−ジ−技研株式会社 | patient transfer |
| DE3448420C2 (en) * | 1984-12-17 | 1992-12-17 | Stierlen Maquet Ag | Device for moving objects or people |
| JPS61135826U (en) * | 1985-02-12 | 1986-08-23 | ||
| DK155560C (en) * | 1985-06-17 | 1989-09-18 | Hellesens As | ELECTRICAL BATTERY |
| US4752541A (en) * | 1987-03-09 | 1988-06-21 | Amoco Corporation | Electrolyte for lithium-sulfur dioxide electrochemical cell |
-
1981
- 1981-04-30 CA CA000376610A patent/CA1165813A/en not_active Expired
- 1981-05-05 DE DE19813117760 patent/DE3117760A1/en not_active Withdrawn
- 1981-05-07 JP JP6774181A patent/JPS573373A/en active Pending
Cited By (2)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| CN116435591A (en) * | 2023-04-24 | 2023-07-14 | 湖南添越能源科技有限公司 | Lithium ion battery electrode material suitable for working under ultralow temperature condition |
| CN116435591B (en) * | 2023-04-24 | 2024-02-23 | 湖南添越能源科技有限公司 | Lithium ion battery electrode material suitable for working under ultralow temperature condition |
Also Published As
| Publication number | Publication date |
|---|---|
| JPS573373A (en) | 1982-01-08 |
| DE3117760A1 (en) | 1982-05-13 |
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| MKEX | Expiry |