Electrolyte salts for rechargeable magnesium-ion batteries

Abstract

Magnesium salts suitable for use in an electrolyte for a magnesium ion electrochemical cell are described herein. The salts are magnesium tetra(perfluoroalkoxy)metalates, optionally solvated with up to seven ether molecules coordinated to the magnesium ion thereof. In one embodiment, the salt has the empirical formula: Mg(Z).sub.n.sup.2+[M(OCR.sub.3).sub.4.sup.].sub.2 (Formula (I)) wherein Z is an ether; n is 0 to about 7; M is Al or B; and each R independently is a perfluoroalkyl group (e.g., C.sub.1 to C.sub.10 perfluoroalkyl). The magnesium salts of Formula (I) are suitable for use as electrolyte salts for magnesium ion batteries (e.g., 5 V class magnesium batteries) and exhibit a wide redox window that is particularly compatible with magnesium anode. The salts are relatively cost effective to prepare by methods described herein, which are conveniently scalable to levels suitable for commercial production.

Claims

1. An electrochemical cell comprising an anode; a cathode; and a magnesium ion-containing electrolyte contacting the anode and the cathode; wherein the anode comprises metallic magnesium and the cathode comprises at least one compound selected from the group consisting of MoS.sub.2, Mo.sub.6S.sub.8, MoO.sub.3, TiS.sub.2, Ti.sub.2S.sub.4, V.sub.2O.sub.5, MnO.sub.2, MgM.sup.a.sub.2O.sub.4, MgM.sup.bXO.sub.4, Mg.sub.0.5M.sup.c.sub.2(PO.sub.4).sub.3, and Mg.sub.xM.sup.d(CN).sub.6yH.sub.2O; wherein: M.sup.a is one or more metal selected from the group consisting of Mn, Fe, Co, Ni, and Cr; M.sup.b is one or more metal selected from the group consisting of Fe, Mn, Co, and Ni; M.sup.c is one or more metal selected from the group consisting of Ti, Zr, V, and Fe; M.sup.d is one or more metal selected from the group consisting of Fe and Ni; X is one or more element selected from the group consisting of Si, P, and S; x is 0 or 1; and y is in the range of 0 to 9; the electrolyte comprises a magnesium salt dissolved in a nonaqueous solvent; the magnesium salt comprises a salt of Formula (I): Mg(Z).sub.n.sup.2+[M(OCR.sub.3).sub.4.sup.].sub.2; Z is an ether; n is 0 to 7; M is Al or B; and each R independently is a perfluoroalkyl group.

2. A battery comprising a plurality of the electrochemical cell of claim 1 electrically connected together.

3. The electrochemical cell of claim 1, wherein Z comprises at least one ether selected from the group consisting of a dialkyl ether and a cyclic ether.

4. The electrochemical cell of claim 1, wherein Z comprises at least one ether selected from the group consisting of diethyl ether and tetrahydrofuran.

5. The electrochemical cell of claim 1, wherein n is 7.

6. The electrochemical cell of claim 1, wherein M is Al.

7. The electrochemical cell of claim 1, wherein M is B.

8. The electrochemical cell of claim 1, wherein each R independently is a C.sub.1 to C.sub.10 perfluoroalkyl.

9. The electrochemical cell of claim 1, wherein each R is trifluoromethyl.

10. The electrochemical cell of claim 1, wherein M is Al, and each R is trifluoromethyl.

11. The electrochemical cell of claim 1, wherein M is Al, each R is trifluoromethyl, and Z is selected from the group consisting of diethyl ether and tetrahydrofuran.

12. The electrochemical cell of claim 1, wherein M is Al, each R is trifluoromethyl, Z is tetrahydrofuran, and n is 7.

13. The electrochemical cell of claim 1, wherein the nonaqueous organic solvent comprises at least one solvent selected from the group consisting of diethyl ether, tetrahydrofuran, 2-methyltetrahydrofuran, 2,5-dimethyltetrahydrofuran, dimethoxyethane, diglyme, triglyme, tetraglyme, sulfolane, 3-methylsulfolane, acetonitrile, propylene carbonate, butyrolactone, valerolactone, and glutaronitrile.

Description

BRIEF DESCRIPTION OF THE DRAWINGS

(1) FIG. 1 provides plots of current density (J, mA/cm.sup.2) versus potential (relative to Mg/Mg.sup.2+) demonstrating cathodic stability of Mg(AlPFTB.sub.4).sub.2 in triglyme (0.1 M: solid line; 0.4 M: dashed line) versus magnesium anode at first cycle of cyclic voltammetry; working electrode (WE): Pt; counter electrode (CE): Mg; reference electrode: Ag+/AgCl; 100 mV/s.

(2) FIG. 2 provides plots of current density (J, mA/cm.sup.2) versus potential (relative to Mg/Mg.sup.2+) demonstrating cathodic stability of Mg(AlPFTB.sub.4).sub.2 in triglyme (0.1 M: solid line; 0.4 M: dashed line) versus magnesium anode at 10th cycle; working electrode (WE): Pt; counter electrode (CE): Mg; reference electrode: Ag/AgCl; 100 mV/s.

(3) FIG. 3 provides plots of coulombic efficiency versus cycle number in cyclic voltammetry demonstrating cathodic stability of Mg(AlPFTB.sub.4).sub.2 in triglyme (0.1 M: square; 0.4 M: circle) versus magnesium anode; working electrode (WE): Pt; counter electrode (CE): Mg; reference electrode: Ag/AgCl; 100 mV/s.

(4) FIG. 4 shows a scanning electron micrograph (SEM) of Mg deposits on Pt from galvanostatic deposition of Mg(AlPFTB.sub.4).sub.2 in triglyme for 2.5 h at a current density of 1.5 mA/cm.sup.2; WE: Pt; CE: Mg; reference electrode: Ag/AgCl; Panel A shows 239magnification for deposits from 0.1 M solution. Panel B shows 1000magnification for deposits from 0.1 M solution. Panel C shows 250magnification for deposits from 0.4 M solution. Panel D shows 1000magnification for deposits from 0.4 M solution.

(5) FIG. 5 provides plots of current density (J, mA/cm.sup.2) versus voltage (V) for 0.1 M solution of Mg(AlPFTB.sub.4).sub.2 in 3-methylsulfolane, demonstrating anodic stability of Mg(AlPFTB.sub.4).sub.2 versus different current collectors: platinum (Pt: solid), gold (Au: dash), glassy carbon (GC: dot), molybdenum (Mo: dash-dot-dot), stainless steel (SS: dash-dot), aluminum (Al: short dot); working electrode (WE): Pt, Au, Mo, SS, Al, GC; counter electrode (CE): Mg; reference electrode: Ag/AgCl; 5 mV/s (Mo, SS, Al) or 20 mV/s (Pt, Au, GC). Panel A shows plots with Pt, Au and GC as WE. Panel B shows plots with Mo, SS and Al as WE.

(6) FIG. 6 provides plots of sample weight versus temperature for Mg(THF).sub.7(AlPFTB.sub.4).sub.2, demonstrating thermal stability up to about 240 C.

(7) FIG. 7 shows a plot of ionic conductivity versus concentration for Mg(AlPFTB.sub.4).sub.2 in triglyme solvent. Ionic conductivities of solutions of Mg(AlPFTB.sub.4).sub.2 in triglyme at various concentration were calculated from impedance values that were measured with AC impedance spectroscopy.

(8) FIG. 8 schematically illustrates an electrochemical cell.

(9) FIG. 9 schematically illustrates a battery comprising a plurality of an electrochemical cells electrically connected together.

DETAILED DESCRIPTION

(10) An expansion of electrochemical window is needed to enable high-voltage (>5 V) Mg batteries that adopt Mg metal anodes in order to potentially replace Li-ion batteries. Fundamentally, chemical intuition suggests that installing electron-withdrawing groups into anions would enhance the oxidative stability by lowering the HOMO level of anions, but this would compromise reductive stability by lowering LUMO, hence hampering most synthetic attempts to expand the electrochemical window. Hypothetically, instead of pursuing thermodynamic stability of anions at both cathodic (low voltage) and anodic (high voltage) ends, kinetic inertness toward Mg can be introduced to thermodynamically and anodically stable anions by leveraging weak coordination to Mg.sup.2+ to shut down the key step in Mg.sup.2+-catalyzed reductive decomposition. Weakly coordinating anions have been widely used in catalysis, polymerization and recently in development of electrolytes in batteries to stabilize highly electrophilic, naked metal cations, which infer higher catalytic activities to molecular transition metal catalysts, faster intercalation/de-intercalation kinetics and solubility to cations in electrolytes. However, to the best of our knowledge, this concept has never been extended to kinetic inertness of anions for the expansion of electrochemical windows. Therefore, as a proof of concept, a highly electron-deficient, weakly coordinating anion tetrakis(perfluoro-tert-butoxy)aluminate ([TPFA].sup.=[Al{OC(CF.sub.3).sub.3}.sub.4].sup.) was prepared and electrochemically evaluated. The synthesis, characterization and electrochemical performances of perfluorinated magnesium tetra(alkoxy)aluminate Mg[TPFA].sub.2 are described herein.

(11) As described herein, magnesium salts suitable for use in an electrolyte for a magnesium ion electrochemical cell are magnesium tetra(perfluoroalkoxy)metalates, of Formula (I): Mg(Z).sub.n.sup.2+[M(OCR.sub.3).sub.4.sup.].sub.2, wherein Z is an ether; n is 0 to about 7; M is Al or B; and each R independently is a perfluoroalkyl group. In some preferred embodiments, M is aluminum.

(12) In some embodiments of Formula (I), each R independently is a C.sub.1 to C.sub.10 perfluoroalkyl group, e.g., a C.sub.1 to C.sub.8 perfluoroalkyl group, a C.sub.1 to C.sub.8 perfluoroalkyl group, a C.sub.1 to C.sub.6 perfluoroalkyl group, a C.sub.1 to C.sub.4 perfluoroalkyl group, or a C.sub.1 to C.sub.2 perfluoroalkyl group. The perfluoroalkyl groups can be linear or branched. Non-limiting examples of such perfluoroalkyl groups include trifluoromethyl, pentafluoroethyl, heptafluoro-1-propyl, heptafluoro-2-propyl, nonafluoro-1-butyl, nonafluoro-sec-butyl, nonafluoro-tert-butyl, undecafluorohexyl, pentadecafluorooctyl, and the like. In some preferred embodiments the perfluoroalkyl groups are independently selected from the group consisting of trifluoromethyl and pentafluoroethyl.

(13) The ether, Z, in Formula (I) preferably is at least one ether selected from the group consisting of diethyl ether, tetrahydrofuran, 2-methyltetrahydrofuran, 2,5-dimethyltetrahydrofuran, dimethoxyethane, diglyme, triglyme, and tetraglyme. In some preferred embodiments, the ether, Z, is selected from the group consisting of tetrahydrofuran, diethyl ether, and a combination thereof.

(14) The salts of Formula (I) can be utilized in an electrolyte for a magnesium electrochemical cell, in which the salt is dissolved in a non-aqueous organic solvent, such as at least one solvent, which can be, e.g., an ether, a sulfolane compound, a nitrile, a carbonate, a lactone, or a combination of two or more thereof. In some preferred embodiments the solvent comprises at least one material selected from the group consisting of diethyl ether, tetrahydrofuran, 2-methyltetrahydrofuran, 2,5-dimethyltetrahydrofuran, dimethoxyethane, diglyme, triglyme, tetraglyme, sulfolane, 3-methylsulfolane, acetonitrile, propylene carbonate, butyrolactone, valerolactone, and glutaronitrile. In an electrochemical cell, the electrolyte is in contact with an anode (e.g., metallic Mg) and a cathode, preferably with a porous magnesium permeable membrane situated between the anode and the cathode to prevent direct contract of the anode with the cathode. The cathode can be any cathode material suitable for use in a magnesium electrochemical cell or battery. For example, the cathode can comprise at least one compound selected from the group consisting of MoS.sub.2, Mo.sub.6S.sub.8, MoO.sub.3, TiS.sub.2, Ti.sub.2S.sub.4, V.sub.2O.sub.5, MnO.sub.2, MgM.sup.a.sub.2O.sub.4. MgM.sup.bXO.sub.4, Mg.sub.0.5M.sup.c.sub.2(PO.sub.4).sub.3, and Mg.sub.xM.sup.d(CN).sub.6yH.sub.2O; wherein: M.sup.a is one or more metal selected from the group consisting of Mn, Fe, Co, Ni, and Cr; M.sup.b is one or more metal selected from the group consisting of Fe, Mn, Co, and Ni; M.sup.c is one or more metal selected from the group consisting of Ti, Zr, V, and Fe; M.sup.d is one or more metal selected from the group consisting of Fe and Ni; X is one or more element selected from the group consisting of Si, P, and S; x is 0 or 1; and y is in the range of 0 to 9.

(15) Salts of Formula (I) can be prepared by (a) contacting a lithium metal hydride of formula LiMH.sub.4 with at least four molar equivalents of a tertiary alcohol of formula HOCR.sub.3 in a hydrocarbon solvent to form a lithium salt of formula LiM(OCR.sub.3).sub.4; (b) contacting the salt of formula LiM(OCR.sub.3).sub.4 with gaseous hydrochloric acid in a nonaqueous solvent comprising diethyl ether to afford a compound of formula H(O(CH.sub.2CH.sub.3).sub.2).sub.2M(OCR.sub.3).sub.4; and (c) contacting the compound of formula H(O(CH.sub.2CH.sub.3).sub.2).sub.2M(OCR.sub.3).sub.4 with a magnesium salt in an ether solvent to afford the salt of Formula (I); wherein Z is an ether; n is 0 to 7; M is Al or B; and each R independently is a perfluoroalkyl group. Non-limiting examples of magnesium salts for use in step (c) include, e.g., magnesium bis(hexamethyldisilazide), dibutylmagnesium, dimethylmagnesium, diphenylmagnesium, and the like.

(16) The magnesium salts of Formula (I) are suitable for use as electrolyte salts for magnesium ion batteries (e.g., 5 V class magnesium batteries) and exhibit a wide redox window that is particularly compatible with magnesium anode. The salts are relatively cost effective to prepare by methods described herein, which are conveniently scalable to levels suitable for commercial production.

(17) The following non-limiting examples are provided to illustrate certain features and characteristics of the compositions and methods described herein.

EXAMPLE 1

Synthesis of Mg[AlPFTB.SUB.4.].SUB.2..

(18) Mg[AlPFTB.sub.4].sub.2 was synthesized in three steps (Scheme 1). The lithium analog Li[AlPFTB.sub.4] was first synthesized from alcoholysis of LiAlH.sub.4 by (CF.sub.3).sub.3COH in a substantially quantitative yield. Li.sup.+/H.sup.+ cation metathesis of Li[AlPFTB.sub.4] with HCl in CH.sub.2Cl.sub.2 and Et.sub.2O afforded [H(Et.sub.2O).sub.2] [AlPFTB.sub.4] in 93% yield. Finally, protonolysis of Mg(HMDS).sub.2 by about 2 equivalents (equiv) of [H(Et.sub.2O).sub.2][AlPFTB.sub.4] in THF and subsequent recrystallization from diffusion of Et.sub.2O to the THF solution yielded the THF adduct Mg[AlFTB.sub.4].sub.27 THF in 96% yield. The recrystallized compound was characterized by IR and NMR spectroscopy, and the purity and stoichiometry were supported by elemental analysis and .sup.1H NMR analysis using ferrocene as an internal standard.

(19) ##STR00001##

(20) Exchange of hydrogen for magnesium was accomplished by combining about 1 equiv [H(Et.sub.2O).sub.2][AlPFTB.sub.4] (1.06 g, 0.95 mmol) and 0.52 eqiuv Mg(HMDS).sub.2 (168 mg, 0.49 mmol) in a 20 mL scintillation vial, and adding THF (5 mL) to the mixture (resulting in a concentration of about 200 mg [H(Et.sub.2O).sub.2][AlPFTB.sub.4]/1 mL THF). After about 5 min, a clear solution was formed. Recrystallization by diffusion of Et.sub.2O into the THF solution (v/v=1/1) afforded colorless crystals. The crystals were collected, washed with minimal amount of Et.sub.2O by filtration and dried at 100 mTorr at room temperature for about 2.5 h to afford Mg[AlPFTB.sub.4].sub.27 THF as a white solid (1.10 g, 0.46 mmol, 96%). The Mg(AlPFTB.sub.4).sub.2 is soluble in THF, and is thermally stable below about 240 C. Mg(AlPFTB.sub.4).sub.2 also is electrochemically stable when cycled with a magnesium electrode, and is oxidatively stable up to about 5.4 V versus Mg.

EXAMPLE 2

Electrochemical Physical Property Evaluation of Mg[AlPFTB.SUB.4.].SUB.2..

(21) Mg[AlPFTB.sub.4].sub.2 was evaluated by cyclic voltammetry (CV). FIG. 1 provides plots of current density (J) versus potential (relative to Mg/Mg.sup.2+) demonstrating cathodic stability of Mg(AlPFTB.sub.4).sub.2 in triglyme (0.1 M: solid line; 0.4 M: dashed line) versus magnesium anode at first cycle of cyclic voltammetry; working electrode (WE): Pt; counter electrode (CE): Mg; reference electrode: Ag/AgCl; 100 mV/s, while FIG. 2 provides plots of current density (J) versus potential (relative to Mg/Mg.sup.2+) demonstrating cathodic stability of Mg(AlPFTB.sub.4).sub.2 in triglyme (0.1 M: solid; 0.4 M: dash) versus magnesium anode at 10th cycle; working electrode (WE): Pt; counter electrode (CE): Mg; reference electrode: Ag/AgCl; 100 mV/s. FIG. 3 provides plots of coulombic efficiency versus cycle number in cyclic voltammetry demonstrating cathodic stability of Mg(AlPFTB.sub.4).sub.2 in triglyme (0.1 M: square; 0.4 M: circle) versus magnesium anode; working electrode (WE): Pt; counter electrode (CE): Mg; reference electrode: Ag/AgCl; 100 mV/s.

(22) Electrodeposition and dissolution of Mg was clearly observed during cycling. The nucleation overpotential, defined as the potential at which electrodeposition begins in the cathodic sweep, was 370 mV in the first cycle, while the dissolution overpotential, defined as the onset potential of the dissolution of deposited Mg into the solution, was 260 mV in the first cycle (FIG. 1). These values improved to 270 mV and 60 mV, respectively, at the 10th cycle and remained approximately constant thereafter (FIG. 2). These observed improvements suggest that a conditioning process occurred during the first 10 cycles. The coulombic efficiency for the first cycle was 96% and decreased slightly to 90% at 10th cycle (FIG. 3). Nonetheless, these results show that the 0.1 M solution of Mg(AlPFTB.sub.4).sub.2 in triglyme possesses sufficient cathodic stability for supporting electrodeposition/dissolution of Mg.

(23) At a higher concentration of 0.4 M in triglyme, where the formation of [Mg(AlPFTB.sub.4)].sup.+ ion-pairs was strongly implied by IR and NMR spectroscopy, Mg deposition/dissolution was also observed, but the electrochemical behavior of this solution was drastically different from that of a 0.1 M solution. The nucleation overpotential started and stayed at 260 mV throughout cycling, in sharp contrast with that of 0.1 M solution (see above), and dissolution overpotential started at 170 mV in the first cycle but dropped to 25 mV at the end of 10.sup.th cycle. The constant and lower nucleation overpotential observed for a more concentrated electrolyte argues against desorption of adsorbed Mg.sub.x[AlPFTB.sub.4].sub.y.sup.n/n species, which has been attributed to the higher initial overpotential and impedance as reported for other electrolytes stored at open-circuit potential before cycling as the origin of conditioning of Pt electrode observed for the 0.1 M solution. The coulombic efficiency (CE) of the first cycle was 54%,which was significantly lower than that with 0.1 M solution, and increased to 85% after 10 cycles. These observations are consistent with more favored formation of an SEI on the Pt electrode at a higher concentration, leading to decreased overpotentials. Similar concentration-dependent effects on coulombic efficiency have reported for Mg(TFSI).sub.2 in diglyme and attributed to ion-pairing, and recently noted for Mg[B{OCH(CF.sub.3).sub.2}.sub.4].sub.2 without explanation. All this information and data collectively suggest increased reductive decomposition of the electrolyte, which resulted in an initially lower CE with a higher concentration of [Mg][TPFA].sub.2. The decomposed products could form an SEI on the working electrode, which conditioned the Pt electrode and led to lower overpotentials to avoid further decomposition as in Li-ion batteries.

(24) FIG. 4 shows a scanning electron micrograph (SEM) of Mg deposits on Pt from galvanostatic deposition of Mg(AlPFTB.sub.4).sub.2 in triglyme for 2.5 h at a current density of 1.5 mA/cm.sup.2; WE: Pt; CE: Mg; reference electrode: Ag/AgCl; Panel A shows 239magnification for deposits from 0.1 M solution. Panel B shows 1000magnification for deposits from 0.1 M solution. Panel C shows 250magnification for deposits from 0.4 M solution. Panel D shows 1000magnification for deposits from 0.4 M solution. Images of the deposits obtained from the 0.1 M solution via scanning electron microscopy (SEM) show randomly dispersed globular islands (FIG. 4, Panel A), which were composed of densely packed, crystalline platelets of 20100 m in size (FIG. 4, Panel B). The morphology of these deposits is different from the commonly observed smooth and continuous film, but this morphology is not unprecedented. Prior XRD, SEM and STM studies on Mg deposition from solutions of R.sub.2-mMgCl.sub.m (R=Et, Bu; m=0, 1) and R.sub.3-nAlCl.sub.n in ethereal solvents (R=Me, Et; n=1, 2) suggest that nucleation of Mg.sup.0 starts randomly with similar island formation as observed here according to a local concentration gradient of active species. The nucleation process is strongly dependent on the applied current density as a result of competitive kinetics between charge transfer and mass transfer, as well as the structure of adsorbed Mg.sup.2 species. Interestingly, SEM images of the deposits obtained from the 0.4 M solution show similar globular macrostructures (FIG. 4, Panel C); however, these aggregates were highly amorphous (FIG. 4, Panel D).

(25) Elemental mapping for Al, F, and Mg was performed using Energy-dispersive X-ray spectroscopy (EDS) on the crystalline aggregates from the 0.1 M solution. Mg was the sole element detected in the deposit (no Al, C or F atoms were detected). These results are consistent with CV data that Mg could be electrodeposited from Mg(AlPFTB.sub.4).sub.2in triglyme, and minimal decomposition of the [TPFA].sup. anion on Mg surface during constant-current electrodeposition at the concentration of 0.1 M. EDS analysis of the deposits from the 0.4 M solution still shows Mg as the major element; however, the deposits also contained significant amounts of C and F atoms and to a lesser extent Al atoms, which is indicative of increased decomposition of the [AlPFTB.sub.4].sup. anion. These results strongly suggest that galvanostatic deposition of Mg in a more concentrated solution of Mg(AlPFTB.sub.4).sub.2 leads to electrodeposition of Mg that was accompanied by increased decomposition of [AlPFTB.sub.4].sup. anion to form the observed amorphous mixtures. These comparative SEM/EDS results are also consistent with CV results, where a lower initial coulombic efficiency of Mg deposition/dissolution in the 0.4 M solution was observed. Together with CV studies, these results strongly indicate that at 0.4 M, where ion-pairs are formed, increased reductive decomposition occurred relative to 0.1 M where little coordination of [AlPFTB.sub.4].sup. to Mg.sup.2+ was present

(26) FIG. 5 provides plots of current density (J, mA/cm.sup.2) versus voltage (V) for 0.1 M solution of Mg(AlPFTB.sub.4).sub.2 in 3-methylsulfolane, demonstrating anodic stability of Mg(AlPFTB.sub.4).sub.2 versus different current collectors: platinum (Pt: solid), gold (Au: dash), glassy carbon (GC: dot), molybdenum (Mo: dash-dot-dot), stainless steel (SS: dash-dot), and aluminum (Al: short dot).; working electrode (WE): Pt, Au, Mo, SS, Al, GC; counter electrode (CE): Mg; reference electrode: Ag/AgCl; 5 mV/s (Mo, SS, Al) or 20 mV/s (Pt, Au, GC). Panel A shows plots with Pt, Au and GC as WE. Panel B shows plots with Mo, SS and Al as WE. In order to gauge the anodic stability of Mg(AlPFTB.sub.4).sub.2, the compound was dissolved in 3-methylsulfolane and residual THF was removed under vacuum at 55 C. overnight. .sup.1H NMR and GC-MS of the solution indicate removal of THF to an undetectable level.

(27) The anodic stability of a 0.1 M solution of Mg(AlPFTB.sub.4).sub.2 in 3-methylsulfolane was investigated by CV using glassy carbon (GC), Au, and Pt electrodes. The electrodes were immersed in the solution at 2.0 V (0 V vs reference electrode) and cycled between 2.0 and 5.7 V at a rate of 20 mV/s for 3 consecutive cycles (FIG. 5, Panel A). Broadly speaking, bulk oxidation occurred at potentials above 5.4 V on all three electrode materials (defined as J>0.1 mA/cm.sup.2). Similarly, bulk oxidation >5 V was also observed for Al and stainless steel electrodes when these were immersed at their open-circuit potential (FIG. 5, Panel B). These results suggest high thermodynamic stability of in 3-methylsulfolane.

(28) The thermal stability of Mg(AlPFTB.sub.4).sub.2 was investigated by thermogravimetric analysis (TGA). FIG. 6 provides plots of sample weight versus temperature for Mg(THF).sub.7(AlPFTB.sub.4).sub.2, demonstrating thermal stability up to about 240 C. The analysis shows that the compound is stable until 150 C., after which the sample lost 5.7% of its weight (1.38 mg) from 150 and 210 C., and 7.19% (1.74 mg) from 210 to 240 C. Above 240 C., almost the entire mass was rapidly lost presumably via sublimation. While little is known about the possible chemical changes during sublimation, these results show that the compound was stable up to 240 C. without sublimation.

(29) Ionic conductivities of solutions of Mg(AlPFTB.sub.4).sub.2 in triglyme at various concentration were calculated from impedance values that were measured with AC impedance spectroscopy. FIG. 7 shows a plot of ionic conductivity versus concentration for Mg(AlPFTB.sub.4).sub.2 in triglyme solvent. This analysis shows that the ionic conductivity initially increases with concentration, peaks at about 0.3 M, and then decreases thereafter. The maximum solubility of the compound in triglyme is 0.4 M. These results suggest that ion association occurs at concentration above 0.2 M in triglyme, which reduces the amount of free ions in the solution.

EXAMPLE 3

Exemplary Electrochemical Cell and Battery

(30) FIG. 8 schematically illustrates a cross-sectional view of Mg-ion electrochemical cell 10 comprising cathode 12 (e.g., comprising metallic or carbon current collector coated with a material capable of reversibly accepting and releasing magnesium ions), and anode 14 (e.g., Mg), with a porous separator 16 (e.g., a polypropylene microporous separator, a polyethylene/polypropylene/polyethylene microporous separator, a polyethylene microporous separator; a poly(vinylidene-difluoride)-polyacrylonitrile graft copolymer microporous separator; and the like) between cathode 12 and anode 14. Electrolyte 18, comprising a solution of a Mg salt described herein in a non-aqueous solvent contacts electrodes 12 and 14 and separator 16. Optionally, the cathode can comprise a particulate carbon material (e.g., graphite or carbon black) intermixed with the material capable of reversibly accepting and releasing magnesium ions in a binder compound, such as poly(vinylidene difluoride). The electrodes, separator and electrolyte are sealed within housing 19. FIG. 9 schematically illustrates a magnesium-ion battery comprising a first array 20 consisting of three series-connected electrochemical cells 10, and a second array 22 consisting of three series-connected electrochemical cells 10, in which first array 20 is electrically connected to second array 22 in parallel.

(31) All references, including publications, patent applications, and patents, cited herein are hereby incorporated by reference to the same extent as if each reference were individually and specifically indicated to be incorporated by reference and were set forth in its entirety herein.

(32) The use of the terms a and an and the and similar referents in the context of describing the invention (especially in the context of the following claims) are to be construed to cover both the singular and the plural, unless otherwise indicated herein or clearly contradicted by context. The terms comprising, having, including, and containing are to be construed as open-ended terms (i.e., meaning including, but not limited to,) unless otherwise noted. The terms consisting of and consists of are to be construed as closed terms, which limit any compositions or methods to the specified components or steps, respectively, that are listed in a given claim or portion of the specification. In addition, and because of its open nature, the term comprising broadly encompasses compositions and methods that consist essentially of or consist of specified components or steps, in addition to compositions and methods that include other components or steps beyond those listed in the given claim or portion of the specification. Recitation of ranges of values herein are merely intended to serve as a shorthand method of referring individually to each separate value falling within the range, unless otherwise indicated herein, and each separate value is incorporated into the specification as if it were individually recited herein. All numerical values obtained by measurement (e.g., weight, concentration, physical dimensions, removal rates, flow rates, and the like) are not to be construed as absolutely precise numbers, and should be considered to encompass values within the known limits of the measurement techniques commonly used in the art, regardless of whether or not the term about is explicitly stated. All methods described herein can be performed in any suitable order unless otherwise indicated herein or otherwise clearly contradicted by context. The use of any and all examples, or exemplary language (e.g., such as) provided herein, is intended merely to better illuminate certain aspects of the invention and does not pose a limitation on the scope of the invention unless otherwise claimed. No language in the specification should be construed as indicating any non-claimed element as essential to the practice of the invention.

(33) Preferred embodiments of this invention are described herein, including the best mode known to the inventors for carrying out the invention. Variations of those preferred embodiments may become apparent to those of ordinary skill in the art upon reading the foregoing description. The inventors expect skilled artisans to employ such variations as appropriate, and the inventors intend for the invention to be practiced otherwise than as specifically described herein. Accordingly, this invention includes all modifications and equivalents of the subject matter recited in the claims appended hereto as permitted by applicable law. Moreover, any combination of the above-described elements in all possible variations thereof is encompassed by the invention unless otherwise indicated herein or otherwise clearly contradicted by context.