The present embodiments relate to batteries. More specifically, the present embodiments relate to a new type of battery in which the metal that is transported across the separator may be different than the material that is oxidized/reduced at the electrodes.
Our society has come to rely on batteries to power a myriad of devices, including computers, cell phones, portable music players, lighting devices, as well as many other electronic components. Nevertheless, there is an ongoing need for further advances in battery technology. For example, there is still a significant need for economical batteries that can power automobiles or provide load-leveling capabilities for wind, solar or other energy technologies. Furthermore, the “information age” increasingly demands portable energy sources that provide lighter weight, higher energy, longer discharge times, more “cycles,” and smaller customized designs. To achieve these advances, technologists continue to work to develop batteries with higher and higher energy densities while still providing acceptable safety, power densities, cost, and other needed characteristics.
U.S. Pat. No. 8,012,621, which was filed by Joshi, et. al., is an example of battery technology that is currently being researched. (As noted above, this U.S. patent is expressly incorporated herein by reference.) U.S. Pat. No. 8,012,621 describes a battery cell where a metal hydride is the negative electrode and a nickel hydroxy-oxide electrode is the positive electrode. In both positive and negative electrode chambers, there is an alkaline electrolyte comprised of alkali metal hydroxide dissolved in a water solvent. The patent discloses a substantially nonporous alkali metal ion conductive ceramic membrane to separate the electrode compartments. In this patent, “substantially nonporous” means that at least a portion of the cross-section of the membrane has little or no through porosity such that transport across the membrane primarily must occur through the membrane lattice structure and channels rather than through pores. During operation of the cell described in this patent, an alkali cation carries the charge during charging/re-charging of the battery (rather than the hydroxyl ion that is used as part of the reaction at the electrode). Advantages of this system include a prevention of undesirable species migration from one electrode to another. This patent may also result in improved columbic efficiency as well as negligible self-discharge between cycles and during storage.
Additionally, U.S. patent application Ser. No. 12/022,381 represents another type of battery technology. (This patent application has been published as U.S. Patent Application Publication No. 2009/0189567, and as noted above, this patent application has been expressly incorporated herein by reference.) In U.S. patent application Ser. No. 12/022,381, a battery cell is described in which a zinc negative electrode is utilized with a multitude of different positive electrode materials (such as, for example, MnO2, AgO or Ag2O, NiOOH, O2, HgO, CdO, Cu2O). In all these cases, an alkaline electrolyte is utilized on both sides of the cell, and this alkaline electrolyte is understood to be a water-based material. This system provides the advantage of having a non-porous membrane separating anode and cathode, resulting in high columbic efficiency and a prevention of self discharge.
At the same time, the above-recited patent documents all utilize an aqueous (alkaline) electrolyte. However, there are candidate negative and positive electrode materials that are not compatible with aqueous electrolytes. These aqueous-incompatible electrode materials offer advantages in terms of cyclability, energy density and cost per energy unit. For example, magnesium is a relatively low cost and energy dense electrode material with a very negative reduction potential (relative to hydrogen). In fact, use of a magnesium electrode can result in a very low cost per energy unit when coupled with many candidate electrodes with higher reduction potentials. However, magnesium is not compatible with water since it reacts with water. Aluminum is another low cost electrode material candidate material with similar advantages to magnesium but also is not compatible with an alkaline, water-based electrolyte. Thus, magnesium and aluminum cannot be used as the electrode material in the above-recited systems.
Accordingly, there is a need in the industry for a new type of battery that does not require an aqueous electrolyte and can use materials, such as magnesium and aluminum, as the electrode material. Such a device is disclosed herein.
The present embodiments may be designed in which the charge carrier that transports across the membrane is a cation that is different from the cation formed/reacted at the surface of the electrode. By having the cation species that moves across the membrane be different than the species involved in the reaction, there is a reduction in the tendency of the cell to form dendrites that may penetrate the membrane. When a metal is formed at the negative electrode upon recharge of the battery, the cation that is used to form the metal may be derived from a salt dissolved in the electrolyte rather than from a cation that has transported across the membrane.
For example, the present embodiments may be designed in which a magnesium or aluminum electrode is used in conjunction with a sodium conductive membrane (such as a NASICON membrane). In this system, sodium ions within the electrolyte will act as a charge carrier that will be transported across the membrane. These sodium ions may be from an alkali metal salt that is dissolved (at least partially) in the electrolyte solution. This alkali metal salt may be, for example, sodium chloride, sodium hydroxide, sodium triflate or the like or combinations thereof. This electrolyte solution may include a solvent. The solvent may be one of many polar organic solvents which do not react with magnesium/aluminum such as propanol, ethylene glycol, glycerine, dimethyl sulfoxide, acetronitrile or combinations of such solvents. Alternatively ionic liquids such as 1-Butyl-3-methylimidazolium hexafluorophosphate (BMIM-PF6) or Trioctylmethylammonium bis(trifluoromethyl-sulfonyl) imide may be used. During discharge of the battery, magnesium/aluminum halide or magnesium/aluminum hydroxide or magnesium/aluminum triflate form as the magnesium/aluminum metal on the electrode surface oxidizes. As part of this process, sodium ions from the electrolyte solution will transport across the membrane. During a recharging reaction, the opposite chemical reactions occur. Rather than having the magnesium/aluminum ions transported across the membrane, such magnesium/aluminum ions are dispersed throughout the negative electrode compartment (within the electrolyte solution). Sodium ions transport across the membrane (and not the magnesium/aluminum ions), thereby reducing the likelihood of dendrite formation. Dendrite formation can be further minimized or impeded by the addition of polymers stable with the electrode material and solvent, for example polytetrafluoroethylene (PTFE), Polyvinylidene Fluoride (PVDF) or the like.
Examples of a negative or first electrode discharge reaction (using magnesium as the example) are given below. During this discharge reaction, the metal is oxidized into an ionic state:
Mg+2NaOH or 2NaCl→MgCl2 or Mg(OH)2+2Na++2e−.
More generalized, these reactions can be written as follows:
A+2MeX→AX2+2Me++2e− (where A is a divalent metal), or
A+MeX→AX+Me++e− (where A is a monovalent metal), or
A+3MeX→AX3+3Me++3e− (where A is a trivalent metal).
If A is a divalent metal, this metal at the first electrode forms divalent cations upon oxidation (such as Mg, Ca, Zn or Be). If A is a monovalent metal, this metal at the first electrode forms monovalent cations upon oxidation (such as Li, Na, and K). If A is a trivalent metal, this metal at the first electrode forms trivalent cations upon oxidation (such as Al). Me is the alkali metal and MeX is the alkali metal salt, Me+ is the alkali metal ion that may conduct through the membrane, and X is the anion which may be a halide, or hydroxyl ion.
Examples of a negative or first electrode recharge reaction (using magnesium as the example) are given below. During this recharge reaction, the metal is regenerated.
MgCl2 or Mg(OH)2+2Na++2e−→Mg+2NaOH or 2NaCl.
More generalized, these reactions can be written as follows:
AX2+2Me++2e−→A+2MeX (where A is a divalent metal), or
AX+Me++e−→A+MeX (where A is a monovalent metal), or
AX3+3Me++3e−→A+3MeX (where A is a trivalent metal).
Of course, in an electrolytic cell, there must be a positive or second electrode that is used with the first electrode. A variety of different materials may be used as the second electrode, including sulfur, iodine, chloride, etc. During discharge, some of these reactions may be written as follows:
3S+2Na++2e−→Na2S3;
I2+2Na++2e−→2NaI;
NiCl2+2Na++2e−→2NaCl+Ni;
S+H2O+2e−→OH−+HS−; or
NiO2+H2O+e−→NiOOH+OH−
The first three of these second electrode reactions do not require the presence of water. Accordingly for these reactions, polar organic solvents or ionic liquids may be used to at least partially dissolve the forming salt (e.g., Na2S3, NaI, or NaCl). Ethylene glycol and N-methyl formamide, dimethyl sulfoxide, etc., are examples of solvents which effectively dissolve the salt, but are not water-based. In the last two electrode reactions indicated above, water may be used as the solvent. In fact, in such reactions, water is used as a reactant to form hydroxyl ion that is part of the chemical reaction occurring at the electrode. Of course many other electrode materials may be used for the positive or second electrode including MnO2, AgO, Ag2O, O2, CdO, Cu2O, FeS2.
It should be noted that the present embodiments may provide an advance with respect to the use of magnesium and/or aluminum in batteries. For example, batteries using magnesium were difficult to use because the magnesium ions often caused a failure to occur at the cathode. Specifically, the magnesium ions may be incompatible with the cathode solvent, may form undesirable compounds at the cathode, and/or may be inculcated (incorporated) into the electrode or the membrane, etc. However, the present embodiments address the difficulty associated with magnesium ions at the cathode by essentially converting the system into one that uses sodium ions, rather than magnesium ions, at the cathode. In other words, it is sodium ions, not magnesium ions, that will transport across the membrane and will be reacted at the cathode. Thus, the cathode is separated from magnesium ions, thereby making the cell less prone to failure and/or less prone to the problems associated with the use of magnesium ions at the cathode.
Referring now to
The separator 120 that is used in the battery 100 may be an alkali-ion conductive substantially non-porous separator 120 that is disposed between the first and second electrodes 104, 108. As used herein, the term “substantially nonporous” means that at least a portion of the cross-section of the separator 120 has little or no through porosity such that transport across the separator 120 primarily must occur through the separator's lattice structure and channels rather than through pores. Because the separator 120 is “alkali-ion conductive,” alkali metal ions (such as, for example, sodium ions, lithium ions, potassium ions, etc.) may pass through the separator 120. In other words, the alkali metal ions may pass through the separator 120 from the first compartment 114 to the second compartment 118 (and vice versa). Generally, the separator 120 will be a “specific alkali ion conductor,” meaning that it is specifically designed to transport a certain, specific alkali metal ion across the membrane (such as, for example, specifically transporting sodium ions across the separator 120, specifically transporting lithium ions across the separator, etc.).
In some embodiments, the separator 120 is a substantially non-porous, electronically insulating, ceramic separator material. In other embodiments, the separator 120 is a substantially non-porous glass separator material. In other embodiments, the separator 120 comprises a material having the formula Me1+xZr2SixP3−xO12 where 0.1≤x≤3, where Me is Na, K, or Li. In further embodiments, the separator 120 comprises a material having the formula Na1+xZr2SixP3−xO12 where 0.1≤x≤3. Yet additional embodiments may be made in which the separator 120 comprises a material having the formula Me5RESi4O12 where Me is Na, K, or Li, where RE is Y, Nd, Dy, or Sm, or any mixture thereof. Other embodiments are designed in which the separator 120 comprises a non-stoichiometric alkali-deficient material having the formula (Me5RESi4O12)1−δ, (RE2O3.2SiO2)δ, where Me is Na, K, or Li, where RE is Nd, Dy, or Sm, or any mixture thereof and where δ is the measure of deviation from stoichiometry. Additional embodiments may be designed in which the separator 120 comprises a material with the formula Li1+xAlxTi2−x(PO4)3 or Li1.3Al0.3Ti1.7(PO4)3. It should be noted that regardless of the particular material used to construct the separator 120, this separator 120 may be a monolithic flat plate, a monolithic tube, a monolithic honeycomb, or supported structures of the foregoing. In further embodiments, the separator 120 may comprise a layered alkali ion conducting ceramic-polymer composite membrane. This type of ceramic-polymer composite membrane may comprise alkali ion-selective polymers layered on alkali ion conducting ceramic solid electrolyte materials. Yet additional embodiments may be designed in which the separator 120 is a NaSICON, KS ICON or LiSICON membrane obtained from Ceramatec, Inc., which is located in Salt Lake City, Utah. Other types of alkali-ion conductive substantially non-porous separators may also be used in the present embodiments.
In some embodiments, the separator 120 is selected from the group consisting of a glass separator material, an electronically insulating, ceramic separator material, and a layered alkali ion conducting ceramic-polymer composite membrane comprising alkali ion-selective polymers layered on alkali ion conducting ceramic solid electrolyte material.
The first and second electrodes 104, 108 will now be described. The first electrode 104 comprises a metal. This metal is designed as metal “A” 104a. This metal may be, for example, magnesium or aluminum. More generally, the metal may be Li, Na, Mg, Al, Zn, Ca, Fe, Zn, Be or K. During discharge of the battery 100, the metal at the first electrode 104 will be converted from its metallic state to its ionic state. These reactions may be represented as follows:
A+2MeX→AX2+2Me++2e− (where A is a divalent metal), or
A+MeX→AX+Me++e− (where A is a monovalent metal), or
A+3MeX→AX3+3Me++3e− (where A is a trivalent metal).
For example, if magnesium is the metal, this discharge reaction may be written as follows:
Mg+2NaOH or 2NaCl→MgCl2 or Mg(OH)2+2Na++2e−.
As noted above, the battery 100 may also be recharged. During this recharge reaction, the metal is regenerated.
AX2+2Me++2e−→A+2MeX (where A is a divalent metal), or
AX+Me++e−→A+MeX (where A is a monovalent metal), or
AX3+3Me++3e−→A+3MeX (where A is a trivalent metal).
For example, if magnesium is the metal, this recharging reaction may be written as follows:
MgCl2 or Mg(OH)2+2Na++2e−→Mg+2NaOH or 2NaCl.
As described herein, the charging/discharging reactions of the first electrode 104 will produce or consume ions of the metal 104a. These ions are present in the first compartment 114 (as shown by “A” ions 142). More specifically, as shown in
The first electrolyte 134 also comprises a quantity of an alkali metal salt, as represented in
The first electrolyte 134 may also comprise a solvent 154, such as a polar solvent. The salt MeX 144, as well as the ions 142, 144a, 144b, will be at least partially soluble in the solvent 154. In some embodiments, the solvent is designed such that it will not react with metal ions (“A” ions). In some embodiments, the solvent may be propanol, ethylene glycol, glycerine, dimethyl sulfoxide, acetronitrile or combinations of such solvents. Alternatively ionic liquids such as 1-Butyl-3-methylimidazolium hexafluorophosphate (BMIM-PF6) or Trioctylmethylammonium bis(trifluoromethyl-sulfonyl) imide may be used as the solvent 154.
The second electrode 108 will now be described. The second electrode 108 comprises an oxidized material that is capable of being electrochemically reduced by the metal of the first electrode 104 (during the discharging reaction). A variety of different materials may be used as the material for the second electrode 108. For example, embodiments may be constructed in which one or more of the following materials are used as the second electrode:
MnO2; AgO; Ag2O; FeS2; O2; NiOOH; NiCl2; HgO; CdO; and Cu2O.
A second electrolyte 138 will also be positioned within the second compartment 118 (proximate the second electrode 108.) The second electrolyte 138 contacts the second electrode 108. This second electrolyte 138 will at least partially dissolve the reduced material 162 that is being produced as part of the electrochemical reduction reaction (which is designated as Reduced Material 162 in
The second electrolyte 138 may further comprise a quantity of the alkali metal ions (Me+) 144a. These ions 144a may be conducted through the separator 120 (such as, for example, during a recharging reaction in which the reduced material 162 is oxidized back onto the second electrode 108 and alkali metal ions are produced). This conduction of the ions 144a through the separator 120 is shown by arrow 155.
It should be noted that in some embodiments, the metal that is used as the “A” metal 104a of the first electrode 104 is not an alkali metal. For example, the “A” metal 104a may be magnesium or aluminum. In such embodiments, the “A” ions 142 that are produced/consumed during the charging/discharging of the battery 100 are not the ions that will be transported across the separator 120. Rather, alkali metal ions 144a are transmitted across the separator 120. Such alkali metal ions 144a are not reacted at the electrodes 104, 108 during charging or recharging. Having the materials at the electrodes be different than the alkali metal that flows across the separator 120 may be advantageous in that it limits or reduces the possibility of dendrite formation. Specifically, because the materials that are oxidized/reduced at the electrodes do not “flow” into another compartment, the likelihood that such materials will form a dendrite that penetrates the separator 120 is substantially reduced and/or eliminated.
Referring now to
The discharge and charge reactions of this Mg system are summarized below:
Discharge:
Mg+2NaOH or 2NaCl→MgCl2 or Mg(OH)2+2Na++2e−
Charge:
MgCl2 or Mg(OH)2+2Na++2e−→Mg+2NaOH or 2NaCl
With respect to the second electrode 108, this electrode 108 may be a sulfur electrode that reacts according to the following equations:
Discharge:
3S+2Na++2e−→Na2S3
Charge:
Na2S3→3S+2Na++2e−
In this embodiment, the “reduced material” that is formed upon the oxidation of the magnesium metal is Na2S3 162. The solvent 158 is selected such that it will at least partially dissolve the formed Na2S3.
This particular battery 200 has significant advantages. For example, the use of Mg metal is desirable as this material is very inexpensive and provides a good electric potential and battery performance. Also, the Mg may be used in the battery 200 because there is no water (or very minimal water) in the system. Further, the Mg2+ ions that are formed upon oxidation of the first electrode 104 are not transported across the separator 120; rather, it is the sodium ions 144a 144a that are carried across the NaSICON membrane.
Additionally, the present battery 200 shown in
Referring now to
The discharge and charge reactions of this Al system are summarized below:
Discharge:
Al+3NaOH or 3NaCl→AlCl3 or Al(OH)3+3Na++3e−
Charge:
AlCl3 or Al(OH)3+3Na++3e−→Al+3NaOH or 3NaCl
With respect to the second electrode 108, this electrode 108 may be a sulfur electrode that reacts according to the following equations:
Discharge:
4.5 S+3Na++3e−→1.5 Na2S3
Charge:
1.5Na2S3→4.5S+3Na++3e−
Thus, in this embodiment, the “reduced material” that is formed upon the oxidation of the magnesium metal is Na2S3 162. The solvent 158 is selected such that it will at least partially dissolve the formed Na2S3.
This particular battery 300 has significant advantages. For example, the use of Al metal is desirable as this material is very inexpensive and provides a good electric potential and battery performance. Also, the Al may be used in the battery because there is no water (or very minimal water) in the system. Further, the Al ions that are formed upon oxidation of the first electrode 104 are not transported across the separator 120; rather, it is the sodium ions 144a that are carried across the membrane.
Additionally, the present battery 300 shown in
Referring now to all of the Figures generally, the present embodiments also provide for a method of charging or discharging a battery. Specifically, a battery is obtained, which may be any of the batteries 100, 200, 300 described herein. The charging of the battery will occur when an electric charging potential (voltage) is supplied by the source 126. This application of the potential causes the following reactions to occur:
if A is a divalent metal: AX2+2Me++2e−→A+2MeX;
if A is a trivalent metal: AX3+3Me++3e−→A+3MeX; and
if A is a monovalent metal: AX+Me++e−→A+MeX.
Additionally, wherein applying the electric charging potential also causes oxidation at the second electrode 108 resulting in the release of alkali metal ions, Me+, from the solvent 158 and conducting Me+ ions 144a across the alkali ion conducting separator 120 from the second electrode 108 to the first electrode 104.
The present embodiments also provide for a method of discharging a battery. Specifically, a battery is obtained, which may be any of the batteries 100, 200, 300 described herein. As part of the discharging process, an electric potential between the first and second electrodes 104, 108 is generated at least in part due to the following reaction occurring at the first electrode 104:
A+2MeX→AX2+2Me++2e−, if A is a divalent metal,
A+MeX→AX+Me++e−, if A is a monovalent metal,
A+3MeX→AX3+3Me++3e−, if A is a trivalent metal.
Additionally, generation of the electric potential also causes reduction at the second electrode 108 resulting in anions which form salts with alkali metal ions, Me+; and resulting in conducting Me+ ions across the alkali ion conducting separator 120 from the first electrode 104 to the second electrode 108.
A method of inhibiting dendrite formation is also taught herein. This method involves obtaining a battery. This battery may be any of the batteries 100, 200, 300 taught herein. The batteries 100, 200, 300 may have a first electrode 104 comprising metal and a second electrode 108 comprising an oxidized material capable of electrochemical reduction by the metal. The method further comprises the step of disposing an alkali-ion conductive, substantially non-porous separator 120 disposed between the first and second electrodes and where a first electrolyte 134 contacting the first electrode 104 comprised of a polar solvent 154 which is non-reactive with the metal and a salt bearing the alkali-ion where the salt is at least partially soluble in the polar solvent 154, and second electrolyte 138 contacting the second electrode 108, the second electrolyte 138 comprising a solvent 158 which at least partially dissolves the alkali salt that forms upon reduction of the second electrode.
As described in the systems of
A Zn/Zn(OH)2 anode was utilized with sodium hydroxide electrolyte, while at the cathode, Ni(OH)2/NiOOH was utilized also with sodium hydroxide electrolyte. A nonporous NaSICON sodium ion conducting membrane separated anode from cathode.
This application claims the benefit of U.S. Provisional Patent Application Ser. No. 61/484,406 filed May 10, 2011, entitled “Alkali Metal Ion Battery Using Alkali Metal Conductive Ceramic Separator.” This application is also a continuation-in-part of U.S. patent application Ser. No. 12/022,381 filed Jan. 30, 2008, entitled “Battery Using Alkali Ion Conducting Separator.” This application is also a continuation-in-part of U.S. patent application Ser. No. 13/364,169 filed Feb. 1, 2012, which, in turn, is a continuation-in-part of U.S. Pat. No. 8,012,621. All of these prior patent documents are expressly incorporated herein by reference.
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Number | Date | Country |
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2935655 | Oct 2015 | EP |
2973832 | Jan 2016 | EP |
2301108 | Sep 1976 | FR |
2518320 | Jun 1983 | FR |
1361377 | Jul 1974 | GB |
21599661 | Dec 1985 | GB |
59-75985 | Apr 1984 | JP |
5975985 | Apr 1984 | JP |
62186470 | Aug 1987 | JP |
07-282860 | Oct 1995 | JP |
08-507637 | Aug 1996 | JP |
08321322 | Dec 1996 | JP |
10162807 | Jun 1998 | JP |
2001-307709 | Nov 2001 | JP |
2001307709 | Nov 2001 | JP |
2002-245847 | Aug 2002 | JP |
2013-541825 | Nov 2003 | JP |
2005-322551 | Nov 2005 | JP |
2008-293678 | Dec 2008 | JP |
2008293678 | Dec 2008 | JP |
2008300173 | Dec 2008 | JP |
201181971 | Apr 2011 | JP |
09-508490 | Aug 2017 | JP |
2004047664 | Jun 2004 | KR |
100651246 | Aug 2005 | KR |
20070021110 | Feb 2007 | KR |
20070021110 | Feb 2007 | KR |
2007028588 | Mar 2007 | KR |
WO2012061823 | Aug 1992 | WO |
WO9416468 | Jul 1994 | WO |
WO-2005038953 | Apr 2005 | WO |
WO2005038953 | Apr 2005 | WO |
WO-2005091946 | Oct 2005 | WO |
WO-2011057135 | Aug 2011 | WO |
WO-2012061823 | May 2012 | WO |
WO-2012061823 | Jul 2012 | WO |
WO2013154349 | Oct 2013 | WO |
WO2014159542 | Oct 2014 | WO |
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Number | Date | Country | |
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20120235644 A1 | Sep 2012 | US |
Number | Date | Country | |
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61484406 | May 2011 | US |
Number | Date | Country | |
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Parent | 12022381 | Jan 2008 | US |
Child | 13466844 | US | |
Parent | 13364169 | Feb 2012 | US |
Child | 12022381 | US |