U.S. patent application number 13/803382 was filed with the patent office on 2013-09-26 for high voltage rechargeable magnesium cells having a non-aqueous electrolyte.
This patent application is currently assigned to PELLION TECHNOLOGIES, INC.. The applicant listed for this patent is Robert Ellis Doe, Jaehee Hwang, Robert E. Jilek, George Hamilton Lane. Invention is credited to Robert Ellis Doe, Jaehee Hwang, Robert E. Jilek, George Hamilton Lane.
Application Number | 20130252114 13/803382 |
Document ID | / |
Family ID | 49212134 |
Filed Date | 2013-09-26 |
United States Patent
Application |
20130252114 |
Kind Code |
A1 |
Doe; Robert Ellis ; et
al. |
September 26, 2013 |
HIGH VOLTAGE RECHARGEABLE MAGNESIUM CELLS HAVING A NON-AQUEOUS
ELECTROLYTE
Abstract
A electrochemical cell having an non-aqueous electrolyte is
provided. The properties of the electrolyte include high
conductivity, high Coulombic efficiency, and an electrochemical
window that can exceed 3.5 V vs. Mg/Mg.sup.+2. The use of the
electrolyte promotes the electrochemical deposition and dissolution
of Mg without the use of any Grignard reagents, other
organometallic materials, tetraphenyl borate, or
tetrachloroaluminate derived anions. Other Mg-containing
electrolyte systems that are expected to be suitable for use in
secondary batteries are also described.
Inventors: |
Doe; Robert Ellis; (Norwood,
MA) ; Lane; George Hamilton; (St. Helens, AU)
; Jilek; Robert E.; (Belmont, MA) ; Hwang;
Jaehee; (Cambridge, MA) |
|
Applicant: |
Name |
City |
State |
Country |
Type |
Doe; Robert Ellis
Lane; George Hamilton
Jilek; Robert E.
Hwang; Jaehee |
Norwood
St. Helens
Belmont
Cambridge |
MA
MA
MA |
US
AU
US
US |
|
|
Assignee: |
PELLION TECHNOLOGIES, INC.
Cambridge
MA
|
Family ID: |
49212134 |
Appl. No.: |
13/803382 |
Filed: |
March 14, 2013 |
Related U.S. Patent Documents
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Application
Number |
Filing Date |
Patent Number |
|
|
61613063 |
Mar 20, 2012 |
|
|
|
Current U.S.
Class: |
429/337 ;
429/199; 429/341 |
Current CPC
Class: |
H01M 10/0568 20130101;
Y02E 60/10 20130101; H01M 10/0567 20130101; H01M 10/054 20130101;
H01M 10/056 20130101 |
Class at
Publication: |
429/337 ;
429/199; 429/341 |
International
Class: |
H01M 10/056 20060101
H01M010/056 |
Goverment Interests
STATEMENT REGARDING FEDERALLY FUNDED RESEARCH OR DEVELOPMENT
[0002] This invention was made with government support under award
number DE-AR0000062, awarded by Advanced Research Projects
Agency-Energy (ARPA-E), U.S. Department of Energy. The government
has certain rights in the invention.
Claims
1. A method of preparing a non-aqueous electrolyte solution for use
in an electrochemical cell, comprising the step of reacting a
magnesium halide and a magnesium salt of formula MgZ.sub.2, where Z
is a polyatomic monovalent anion, in a solvent.
2. The method of claim 1, wherein Z is a polyatomic monovalent
anion selected from the group of polyatomic monovalent anions
described in Table I, or mixtures thereof.
3. The method of claim 1, wherein said magnesium halide is
magnesium chloride, said magnesium salt is
Mg[N(CF.sub.3SO.sub.2).sub.2].sub.2, and said solvent is THF, DME,
ethyl diglyme, butyl diglyme, or a mixture thereof.
4. The method of claim 1, wherein a magnesium halide:MgZ.sub.2
ratio is in the range from 4:1 to 1:4.
5. The non-aqueous electrolyte solution of claim 1, wherein a
magnesium halide:MgZ.sub.2 ratio is in any proportion between 4:1
and 1:1.
6. The method of claim 1, further comprising the step of
conditioning said non-aqueous electrolyte solution by
electrochemical polarization.
7. An electrochemical cell, comprising: a non-aqueous electrolyte
solution comprising: at least one organic solvent; and at least one
electrolytically active, soluble, inorganic Magnesium (Mg) salt
complex represented by the formula Mg.sub.n+1X.sub.(2*n)Z.sub.2 in
which n is in the range from one-quarter to four, X is a halide,
and Z is an inorganic polyatomic monovalent anion; a magnesium
anode and a cathode capable of magnesium intercalation, conversion,
or displacement reaction.
8. The electrochemical cell of claim 7, wherein said magnesium
anode is selected from the group consisting of Mg metal, Anatase
TiO.sub.2, rutile TiO.sub.2, Mo.sub.6S.sub.8, FeS.sub.2, TiS.sub.2,
and MoS.sub.2.
9. The electrochemical cell of claim 7, wherein said Mg alloy is
selected from the group of Mg alloys consisting of AZ31, AZ61,
AZ63, AZ80, AZ81, AZ91, AM50, AM60, Elektron 675, ZK51, ZK60, ZK61,
ZC63, M1A, ZC71, Elektron 21, Elektron 675, Elektron, and
Magnox.
10. The electrochemical cell of claim 7, wherein said magnesium
intercalation cathode is selected from the group consisting of
Chevrel phase Mo.sub.6S.sub.8, MnO.sub.2, CuS, Cu.sub.2S,
Ag.sub.2S, CrS.sub.2, VOPO.sub.4, a layered structure compound, a
spinel structured compound, a zinc blende structure, a rock salt
structured compound, a NASICON structured compound, a Cadmium
iodide structured compound, an Olivine structured compound, a
Tavorite structured compound, a pyrophosphate, a monoclinic
structured compound, and a fluoride.
11. The electrochemical cell of claim 10, wherein said layered
structure compound is selected from the group consisting of
TiS.sub.2, V.sub.2O.sub.5, MgVO.sub.3, MoS.sub.2, MgV.sub.2O.sub.5,
and MoO.sub.3.
12. The electrochemical cell of claim 10, wherein said spinel
structured compound is selected from the group consisting of
CuCr.sub.2S.sub.4, MgCr.sub.2S.sub.4, MgMn.sub.2O.sub.4,
MgNiMnO.sub.4, and Mg.sub.2MnO.sub.4.
13. The electrochemical cell of claim 10, wherein said NASICON
structured compound is selected from the group consisting of
MgFe.sub.2(PO.sub.4).sub.3 and MgV.sub.2(PO.sub.4).sub.3.
14. The electrochemical cell of claim 10, wherein said Olivine
structured compound is selected from the group consisting of
MgMnSiO.sub.4 and MgFe.sub.2(PO.sub.4).sub.2.
15. The electrochemical cell of claim 10, wherein said Tavorite
structured compound is Mg.sub.0.5VPO.sub.4F.
16. The electrochemical cell of claim 10, wherein said
pyrophosphate is selected from the group consisting of
TiP.sub.2O.sub.7 and VP.sub.2O.sub.7.
17. The electrochemical cell of claim 10, wherein said fluoride is
selected from the group consisting of MgMnF.sub.4 and FeF.sub.3.
Description
CROSS-REFERENCE TO RELATED APPLICATIONS
[0001] This application claims priority to and the benefit of
co-pending U.S. provisional patent application Ser. No. 61/613,063,
filed Mar. 20, 2012, which application is incorporated herein by
reference in its entirety.
FIELD OF THE INVENTION
[0003] The invention relates to electrolytic solutions in general
and particularly to an electrolyte that comprises magnesium ions as
the charge carrier.
BACKGROUND
[0004] A variety of rechargeable, high energy density
electrochemical cells have been demonstrated although the most
widely utilized commercial system is that based upon Li-ion
chemistry because it displays very high energy density. Such cells
usually include a transition metal oxide or chalcogenide
cathode-active material, an anode-active lithium metal or lithium
intercalation or alloy compound such as graphitic carbon, tin and
silicon, and an electrolytic solution containing a dissolved
lithium-based salt in an aprotic organic or inorganic solvent or in
a polymer. Today there is great demand for energy storage devices
capable of storing more energy per unit volume or per unit mass,
e.g., Watt-hours per liter (Wh/l) or Watt-hours per kilogram
(Wh/kg), than premier rechargeable Li-ion batteries are capable of
delivering. Consequently an increasingly sought after route to
meeting this demand higher energy density is to replace the
monovalent cation lithium (Li) with divalent magnesium cations
(Mg.sup.2+) because magnesium can enable nearly twice the charge of
Li.sup.+ to be transferred, per volume. Furthermore the abundance
of Mg metal and readily available compounds containing Mg is
expected to offer significant cost reduction relative to Li-ion
batteries. Magnesium also offers superior safety and waste disposal
characteristics.
[0005] Electrolytes utilizing an alkali metal with organic ligands
from organometallic species have been described. Generally the use
of an alkaline earth metal anode such as magnesium would appear
disadvantageous relative to the use of an alkali metal such as
lithium because alkali metal anodes are much more readily ionized
than are alkaline earth metal anodes. In addition, on recharge the
cell should be capable of re-depositing the anode metal that was
dissolved during discharge, in a relatively pure state, and without
the formation of deposits that block the electrodes. One practiced
in the art would note this characteristic is not natural for Mg.
Despite this, there are numerous other disadvantages to alkali
batteries. Alkali metals, and lithium in particular, are expensive
and highly reactive. Alkali metals are also highly flammable, and
fire caused by the reaction of alkali metals with oxygen, water or
other reactive materials is extremely difficult to extinguish. As a
result, the use of alkali metals requires specialized facilities,
such as dry rooms, specialized equipment and specialized
procedures, and shipment of Lithium containing products (e.g.,
batteries) is tightly controlled. In contrast, magnesium metal and
its respective inorganic salts are easy to process and usually are
considered as benign. Magnesium metal is reactive, but it undergoes
rapid passivation of the surface, such that the metal and its
alloys are highly stable. Magnesium is inexpensive relative to the
alkali metals, and widely used as ubiquitous construction
materials.
[0006] Known electrolytes that enable reversible, electrochemical
deposition of Mg and that have potential use in a battery contain
organometallic materials. Most often these electrolytes contain
organometallic Grignard salts as the electrochemically active
component. However sustaining anodic limits greater than 1 Volt is
problematic or impossible with the usual intercalation cathodes
because of electrolyte decomposition and corresponding encrustation
and/or passivation of electrode surfaces. The anodic limit, or
anodic voltage, is a measure of an electrolytes stability limit;
represented as the highest voltage that can be applied to the
electrolyte prior to initiating oxidative decomposition of the
electrolyte at an electrode surface. Enhanced electrochemical
stability has been demonstrated by complexing Grignard reagents
with strong Lewis acids. For example, a cell comprised of a
magnesium metal anode, a molybdenum sulfide "Chevrel" phase active
material cathode, and an electrolyte solution derived from an
organometallic complex containing Mg is capable of the reversible,
electrochemical plating of magnesium metal from solutions with
about a 2 V anodic limit of the stability window. Under the same
principle similar results have also been shown when Magnesium
Chloride and organometallic Aluminum compounds complexes are
employed.
[0007] Such cells are low energy density due to a low difference in
operating potentials between a Chevrel cathode and Mg metal anode
and therefore are not commercially viable cells. Sustaining an
anodic voltage greater than 2 volts is problematic or impossible
with the usual intercalation cathodes and electrolytes based upon
Grignard reagents and other organometallic species. Magnesium
batteries operating at voltages greater than 1.5 volts are
particularly prone to electrolyte decomposition and to encrustation
and/or passivation of the electrode surface due to anodic limits of
the electrolyte. Furthermore electrolytes intended for use in
electrochemical cells in which the plating and stripping of Mg ions
is required include organometallic species among the ionic species
in the respective electrolytic solutions. There are many
disadvantages to organometallic species, relative to inorganic
salts. Practically, all organometallic species of the alkalis and
the earth alkalis are highly unstable in the presence of air and
water and thus are classified as pyrophoric. Organometallic species
of sufficient purity are quite expensive to produce. Organometallic
species introduce organic ligands into the electrolytic solution,
which will limit the chemical stability of the solution when in
contact with certain electrode active materials and other
electrochemical cell components. In general, handling, manipulation
and storing organometallic species of this sort are complicated,
hazardous and expensive.
[0008] In contrast one practiced in the art will recognize that
previous attempts to utilize inorganic magnesium salts failed to
enable substantial reversibility of magnesium deposition with high
Coulombic efficiency and low overpotential. In general it has been
shown that electrodeposition in previous inorganic magnesium salt
solutions corresponded with electrolyte consumption and resulted in
decomposition of the solution components. The decomposition
products passivate the electrode blocking in further
electrochemical reaction. Consequently no commercial Mg secondary
batteries have succeeded thus far.
[0009] The literature on Mg secondary batteries includes N. Amir et
al., "Progress in nonaqueous magnesium electrochemistry," Journal
of Power Sources 174 (2007) 1234-1240, published on line on Jun.
30, 2007; Y Gofer et al., "Magnesium Batteries (Secondary and
Primary)," published in Encyclopedia of Electrochemical Power
Sources 2009 285-301 Elsevier B.V.; and John Muldoon et al.,
"Electrolyte roadblocks to a magnesium rechargeable battery," 5
(2012) Energy & Environmental Science 5941-5950.
[0010] Also previously described is Aurbach et al. in U.S. Pat. No.
6,316,141, issued Nov. 13, 2001, which is said to disclose a cell
comprised of a Magnesium metal anode, a Molybdenum Sulfide
"Chevrel" phase active material cathode, and an electrolyte
solution derived from an organometallic complex containing Mg. The
critical aspect of that invention is the specification of an
electrolyte capable of the reversible, electrochemical plating of
Magnesium metal from solutions with a 2 V anodic limit. This was
demonstrated through the formation of complex electrolytically
active salts represented by the formula:
M'.sup.+m(ZR.sub.nX.sub.q-n).sub.m in which: M' is selected from a
group consisting of magnesium, calcium, aluminum, lithium and
sodium; Z is selected from a group consisting of aluminum, boron,
phosphorus, antimony and arsenic; R represents radicals selected
from the following groups: alkyl, alkenyl, aryl, phenyl, benzyl,
and amido; X is a halogen (I, Br, Cl, F); m=1-3; and n=0-5 and q=6
in the case of Z=phosphorus, antimony and arsenic, and n=0-3 and
q=4 in the case of Z=aluminum and boron.
[0011] In a different report Nakayama et. al., U.S. Patent
Application Publication No. 2010/0136439, published Jun. 3, 2010,
which is said to disclose a magnesium ion-containing nonaqueous
electrolytic solution comprising a magnesium ion and another kind
of a metal ion dissolved in an organic solvent, wherein solutions
may be obtained through combinations of inorganic Lewis Base
MgCl.sub.2 and organometallic Aluminum Lewis Acids such as
dimethylaluminum chloride or methylaluminum dichloride.
[0012] Also described is Yamamoto et al., U.S. Patent Application
Publication No. 2009/0068568, published Mar. 12, 2009, which is
said to disclose a magnesium ion containing non-aqueous electrolyte
in which magnesium ions and aluminum ions are dissolved in an
organic ethereal solvent, and which is formed by adding metal
magnesium, a halogenated hydrocarbon, an aluminum halide AlY.sub.3,
and a quaternary ammonium salt to an organic ethereal solvent and
applying a heating treatment while stirring them as a one-step
reaction to form the Grignard-based organometallic containing
complex solution species.
[0013] There is a need for improved non-aqueous electrolytes for
use in secondary batteries.
SUMMARY OF THE INVENTION
[0014] An electrolyte for use in electrochemical cells is provided.
The properties of the electrolyte include high conductivity, high
Coulombic efficiency, and an electrochemical window that can exceed
3.5 V vs. Mg/Mg.sup.+2. The use of the electrolyte promotes the
electrochemical deposition and dissolution of Mg without the use of
any Grignard reagents, organometallic materials, or Lewis acid
derived anions including tetrachloroaluminate or
tetraphenylborate.
[0015] According to further features in preferred embodiments
described below, the electrolyte is incorporated into specific
Mg-ion electrochemical cells comprised of said electrolyte and an
appropriate anode-cathode pair. In one aspect an appropriate
anode-cathode pair is a magnesium metal anode and a magnesium
insertion-compound cathode. In another aspect an appropriate
anode-cathode pair is a magnesium metal anode and a cathode capable
of conversion, or displacement reactions. In yet another aspect an
appropriate anode-cathode pair is a magnesium metal anode and a
catholyte.
[0016] In some specific embodiments described herein solutions
formed from combinations of Magnesium Chloride (MgCl.sub.2) and
Magnesium bis(trifluoromethylsulfonyl)imide (MgTFSI.sub.2) in
ethereal solvents such as THF and Glyme successfully address the
shortcomings of the previously reported Mg electrolytes and provide
a basis for the production of a viable, rechargeable magnesium
battery with a voltage exceeding a 2 Volt stability window.
[0017] The significantly wider electrochemical window obtained
using electrolytes described herein indicates improved stability
for the electrolytic solution and allows the use of more energetic
cathode materials, such that both the cycle life and the energy
density of the battery are substantially increased. Furthermore the
present invention enables cheaper, safer, and more chemically
stable materials to be utilized for these purposes.
[0018] According to one aspect, the invention relates to a method
of preparing a non-aqueous electrolyte solution. The method
comprises the step of reacting a magnesium halide and a magnesium
salt of formula MgZ.sub.2, where Z is a polyatomic monovalent
anion.
[0019] In one embodiment, Z is a polyatomic monovalent anion
selected from the polyatomic monovalent anions described in Table
I, and mixtures thereof.
[0020] In one embodiment, the magnesium halide is magnesium
chloride, the magnesium salt is
Mg[N(CF.sub.3SO.sub.2).sub.2].sub.2, and the solvent is THF, DME,
ethyl diglyme, butyl diglyme, or a mixture thereof.
[0021] In another embodiment, the magnesium halide:MgZ.sub.2 mole
ratio is in the range from 4:1 to 1:4.
[0022] In yet another embodiment, the magnesium halide:MgZ.sub.2
mole ratio is in any proportion between 4:1 and 1:1.
[0023] In yet another embodiment, the magnesium halide:MgZ.sub.2
mole ratio is in any proportion between 4:1 and 1:4.
[0024] In an additional embodiment, the method further comprises
the step of conditioning the non-aqueous electrolyte solution by
electrochemical polarization.
[0025] According to another aspect, the invention features an
electrochemical cell. The electrochemical cell comprises a
non-aqueous electrolyte solution comprising at least one organic
solvent; and at least one electrolytically active, soluble,
inorganic Magnesium (Mg) salt complex represented by the formula
Mg.sub.n+1X.sub.(2*n)Z.sub.2 in which n is in the range from
one-quarter to four, X is a halide, and Z is an inorganic
polyatomic monovalent anion; a magnesium anode and a cathode
capable of magnesium intercalation, conversion, or displacement
reaction.
[0026] In one embodiment, the magnesium anode is selected from the
group consisting of Mg metal, Anatase TiO.sub.2, rutile TiO.sub.2,
Mo.sub.6S.sub.8, FeS.sub.2, TiS.sub.2, and MoS.sub.2.
[0027] In another embodiment, the Mg alloy is selected from the
group of Mg alloys consisting of AZ31, AZ61, AZ63, AZ80, AZ81,
AZ91, AM50, AM60, Elektron 675, ZK51, ZK60, ZK61, ZC63, M1A, ZC71,
Elektron 21, Elektron 675, Elektron, and Magnox.
[0028] In yet another embodiment, the magnesium intercalation
cathode is selected from the group consisting of Chevrel phase
Mo.sub.6S.sub.8, MnO.sub.2, CuS, Cu.sub.2S, Ag.sub.2S, CrS.sub.2,
VOPO.sub.4, a layered structure compound, a spinel structured
compound, a zinc blende structure, a rock salt structured compound,
a NASICON structured compound, a Cadmium iodide structured
compound, an Olivine structured compound, a Tavorite structured
compound, a pyrophosphate, a monoclinic structured compound, and a
fluoride.
[0029] In still another embodiment, the layered structure compound
is selected from the group consisting of TiS.sub.2, V.sub.2O.sub.5,
MgVO.sub.3, MoS.sub.2, MgV.sub.2O.sub.5, and MoO.sub.3.
[0030] In a further embodiment, the spinel structured compound is
selected from the group consisting of CuCr.sub.2S.sub.4,
MgCr.sub.2S.sub.4, MgMn.sub.2O.sub.4, MgNiMnO.sub.4, and
Mg.sub.2MnO.sub.4.
[0031] In yet a further embodiment, the NASICON structured compound
is selected from the group consisting of MgFe.sub.2(PO.sub.4).sub.3
and MgV.sub.2(PO.sub.4).sub.3.
[0032] In an additional embodiment, the Olivine structured compound
is selected from the group consisting of MgMnSiO.sub.4 and
MgFe.sub.2(PO).sub.2.
[0033] In one more embodiment, the Tavorite structured compound is
Mg.sub.0.5VPO.sub.4F.
[0034] In still a further embodiment, the pyrophosphate is selected
from the group consisting of TiP.sub.2O.sub.7 and
VP.sub.2O.sub.7.
[0035] In one embodiment, the fluoride is selected from the group
consisting of MgMnF.sub.4 and FeF.sub.3.
[0036] The foregoing and other objects, aspects, features, and
advantages of the invention will become more apparent from the
following description and from the claims.
BRIEF DESCRIPTION OF THE DRAWINGS
[0037] The objects and features of the invention can be better
understood with reference to the drawings described below, and the
claims. The drawings are not necessarily to scale, emphasis instead
generally being placed upon illustrating the principles of the
invention. In the drawings, like numerals are used to indicate like
parts throughout the various views.
[0038] FIG. 1 is a graph displaying a typical cyclic voltammogram
of the all-inorganic Mg complex resulting from reaction of
MgCl.sub.2 and Mg(TFSI).sub.2 dissolved in a mixture of
1,2-dimethoxymethane (DME) and tetrahydrofuran (THF).
[0039] FIG. 2 is a graph displaying comparison of typical cyclic
voltammograms of the inorganic magnesium salt complex resulting
from reaction of MgCl.sub.2 and Mg(TFSI).sub.2 when the mole ratio
is varied between the two reactants.
[0040] FIG. 3 is a graph displaying a typical macrocoulometry
cycling data for the inorganic magnesium salt complex
Mg.sub.3Cl.sub.4(TFSI) resulting from reaction of 2MgCl.sub.2 and
1Mg(TFSI).sub.2 in a mixed solution of 1,2-dimethoxymethane (DME)
and
N,N-propyl-methyl-pyrrolidinium-bis(trifluoromethylsulfonyl)imide
(P13-TFSI) ionic liquid.
[0041] FIG. 4 is a graph displaying a typical cyclic voltammograms
of the inorganic magnesium salt complex resulting from reaction of
MgCl.sub.2 and Mg(TFSI).sub.2 when the solvent utilized is a
combination of butyl diglyme and the ionic liquid
N,N-propyl-methyl-pyrrolidinium-bis(trifluoromethylsulfonyl)imide.
DETAILED DESCRIPTION
[0042] An electrolyte is described for use in electrochemical cells
that transfer Mg-ions between electrodes. The properties of the
electrolyte include high conductivity, high Coulombic efficiency,
and an electrochemical window that can exceed 3.5 V vs.
Mg/Mg.sup.2+. The use of an inorganic salt complex in an
electrolyte promotes the substantially reversible deposition of
magnesium metal on the anode current collector and the reversible
intercalation of magnesium in the cathode material. It is expected
that the systems, materials, and methods described will provide an
improved non-aqueous electrolyte that allows the production of a
practical, rechargeable magnesium battery which is expected to be
safer and cleaner, and more durable, efficient and economical than
heretofore known.
[0043] We now provide example electrolytes that are expected to be
suitable for Mg-based secondary battery systems. In particular,
materials contemplated for use in the electrolytes of the invention
can be described by the general formula Mg.sub.2X.sub.3Z, where X
is a monovalent negative ion such as a halide (e.g., F.sup.-1,
Cl.sup.-1, Br.sup.-1, I.sup.-1), and Z is a polyatomic monovalent
negative ion. Examples of polyatomic monovalent anions that are
believed to be useful in practicing the invention include, but are
not limited to, those described in Table I, and mixtures
thereof
TABLE-US-00001 TABLE I Acro- Chemical name nym Formula
bis(perfluoroalkylsulfonyl)imides
N((CxF.sub.2x+1).sub.xSO.sub.2).sub.2.sup.-1
bis(fluorosulfonyl)imide FSI N(SO.sub.2F).sub.2.sup.-1 (x = 0)
bis(trifluoromethanesulfonyl)imide TFSI
N(CF.sub.3SO.sub.2).sub.2.sup.-1 (x = 1)
bis(perfluoroethylsulfonyl)imide BETI
N(C.sub.2F.sub.5SO.sub.2).sub.2.sup.-1 (x = 2) Dicyanamide DCA
N(CN).sub.2.sup.-1 Tricyanomethide TCM C(CN).sub.3.sup.-1
tetracyanoborate TCB B(CN).sub.4.sup.-1 2,2,2,-trifluoro-N-
N(CF.sub.3SO.sub.2) (trifluoromethylsulfonyl)acetamide
(CF.sub.3CO).sup.-1 tetrafluoroborate BF.sub.4.sup.-1
hexafluorophosphate PF.sub.6.sup.-1 triflate
CF.sub.3SO.sub.3.sup.-1 bis(oxalate)borate BOB
B(C.sub.2O.sub.4).sub.2.sup.-1 perchlorate ClO.sub.4.sup.-1
hexafluoroarsenate AsF.sub.6.sup.-1 Hexafluoroantimonate
SbF.sub.6.sup.-1 Perfluorobutylsulfonate
(C.sub.4F.sub.9SO.sub.3).sup.-1
Tris(trifluoromethanesulfonyl)methide
C(CF.sub.3SO.sub.2).sub.3.sup.-1 trifluoroacetate
CF.sub.3CO.sub.2.sup.-1 heptafluorobutanoate
C.sub.3F.sub.7CO.sub.2.sup.-1 thiocyanate SCN.sup.-1 triflinate
CF.sub.3SO.sub.2.sup.-1
Example 1
[0044] FIG. 1 is a graph displaying a typical cyclic voltammogram
of the Mg.sub.2Cl.sub.3-TFSI complex resulting from reaction of
MgCl.sub.2 and Mg(TFSI).sub.2. Solutions utilize a mixture of
1,2-dimethoxymethane (DME) and tetrahydrofuran (THF) as the solvent
and Platinum as the working electrode while Magnesium serves as
both the auxiliary and reference electrodes.
[0045] The data depicted in FIG. 1 shows the potentiodynamic
behavior of Mg.sub.2Cl.sub.3-TFSI complex salt obtained with
DME/THF solution from the reaction of
3MgCl.sub.2+Mg[N(CF.sub.3SO.sub.2).sub.2].sub.2. The experiment
utilized a scan rate of 25 mV/s, a platinum working electrode, and
Mg for the counter and reference electrodes. The anodic stability
of the solution is about 3.5 V vs. the onset of Mg dissolution.
This is significantly higher than previous electrolytic solutions
capable of reversibly plating Mg. The peak displaying maximum
current density at -1.3 V is attributed to the deposition of
magnesium metal while the peak with maximum current density at
about 1.8 V is attributed to the subsequent electrochemical
dissolution of the magnesium metal. The electrochemical window
obtained with this system exceeds 3.5 V vs. the onset of Mg
dissolution. Mg.sub.2Cl.sub.3-TFSI is one preferred embodiment of a
complex salt useful in an electrolyte according to principles of
the invention.
Example 2
[0046] FIG. 2 is a graph displaying a typical cyclic voltammograms
of the inorganic magnesium salt complex resulting from reaction of
MgCl.sub.2 and Mg(TFSI).sub.2 when the mole ratio is varied between
the two reactants. Solutions utilize 1,2-dimethoxymethane (DME) as
the solvent. The experiment utilized a scan rate of 25 mV/s, a
platinum working electrode, and Mg for the counter and reference
electrodes. The mole ratio of MgCl.sub.2 to Mg(TFSI).sub.2 ranges
from 1:2 to 2.5:1 in this salt solution. A high degree of
reversibility and Coulombic efficiency is present in each
composition depicted in FIG. 2. Furthermore the Mg deposition and
stripping occurs with low overpotential. Table II below
demonstrates that solutions of mole ratio for MgCl.sub.2 to
Mg(TFSI).sub.2 ranging from 1:2 to 2.5:1 exhibit high solution
conductivity; all samples being greater than 1 mS/cm at this
molarity of magnesium and room temperature. Electrolyte solutions
for secondary magnesium batteries, which are the product of
magnesium halide (e.g., MgCl.sub.2) and another inorganic salt
(e.g., Mg(TFSI).sub.2) containing an inorganic polyatomic
monovalent anion is one preferred embodiment of a complex salt
useful in an electrolyte according to principles of the invention.
In another preferred embodiment these inorganic Magnesium halide
complex solutions display high conductivity of >1 mS/cm at 25
degrees Celsius.
TABLE-US-00002 TABLE II Mole Ratio of MgCl2 to MgTFSI2 Conductivity
1:4 2.90 mS/cm @ 28.0 C. 1:2 3.73 mS/cm @ 28.5 C. 2:3 4.16 mS/cm @
28.5 C. 1:1 5.04 mS/cm @ 28.0 C. 3:2 5.31 mS/cm @ 28.5 C. 2:1 5.55
mS/cm @ 28.3 C. 2.5:1 5.80 mS/cm @ 28.2 C.
Example 3
[0047] FIG. 3 is a graph displaying a typical macrocoulometry
cycling data for the inorganic magnesium salt complex
Mg.sub.3Cl.sub.4(TFSI) resulting from reaction of 2MgCl.sub.2 and
1Mg(TFSI).sub.2 in a mixed solution of 1,2-dimethoxymethane (DME)
and
N,N-propyl-methyl-pyrrolidinium-bis(trifluoromethylsulfonyl)imide
(P13-TFSI) ionic liquid. The two-electrode experiment utilized
galvanostatic cycling at 1 mA/cm.sup.2 to deposit about 2 microns
of Magnesium onto a platinum working electrode from an Mg counter
electrode. Subsequently 20% of the Mg layer is stripped and
re-electrodeposited for 50 cycles prior to stripping the remaining
80% of Mg. The Coulometric efficiency of this process mimics deep
cycling in a commercial cell. In FIG. 3 the average Coulometric
efficiency over 50 cycles is 98.92%. Furthermore the cycling occurs
with low overpotential to Mg deposition and Mg stripping. The high
Coulombic efficiency, high degree of reversibility, and low
polarization depicted in FIG. 3 is typical for preferred
embodiments of these solutions. According to principles of the
invention, inorganic magnesium electrolyte solutions for secondary
magnesium batteries with Coulombic efficiency >98%, which are
the product of magnesium halide (e.g., MgCl.sub.2) and another
inorganic salt (e.g., Mg(TFSI).sub.2) containing an inorganic
polyatomic monovalent anion is one preferred embodiment of a
complex salt.
Example 4
[0048] FIG. 4 is a graph displaying a typical cyclic voltammograms
of the inorganic magnesium salt complex resulting from reaction of
MgCl.sub.2 and Mg(TFSI).sub.2 when the solvent utilized is a
combination of butyl diglyme and the ionic liquid
N,N-propyl-methyl-pyrrolidinium-bis(trifluoromethylsulfonyl)imide.
The experiment utilized a scan rate of 25 mV/s, a platinum working
electrode, and Mg for the counter and reference electrodes. The
mole ratio of MgCl.sub.2 to Mg(TFSI).sub.2 is about 2:1 in this
inorganic salt solution. To one practiced in the art, the
voltammogram in FIG. 4 shows a high degree of reversibility and
Coulombic efficiency, and the Mg deposition and stripping occurs
with low overpotential. Such solutions are expected to provide much
improved safety over previous organometallic-based Mg electrolytes
due to not only the inorganic nature of the salt complex, but also
the favorable vapor pressure and flash point of the solvents
utilized.
Example 5
[0049] The formation of an electrochemically active
Mg.sub.2Cl.sub.3-TFSI solution can be dependent upon ascertaining
proper conditions for some or all of the following non-limiting
examples of solution variables: the mole ratio of Mg:Cl:TFSI (or
other anodically stable anion), overall molarity, solvent
properties, precursor and solvent purity, and reaction conditions.
In one preferred embodiment, a suitable complex is prepared by
reacting MgCl.sub.2 with a compound containing
bis(trifluoromethanesulfonyl)imide. In a typical preparation of an
electrochemically active Mg.sub.2Cl.sub.3-TFSI solution such as
0.25 M Mg.sub.2Cl.sub.3-TFSI, one may perform the following
reaction:
3MgCl.sub.2+1Mg[N(CF.sub.3SO.sub.2).sub.2].sub.2.fwdarw.2Mg.sub.2Cl.sub.-
3[N(CF.sub.3SO.sub.2).sub.2] Eq. (1)
Place both 1.758 g MgCl.sub.2 powder (99.99%) and .about.2.016 g
Mg[N(CF.sub.3SO.sub.2).sub.2].sub.2 (min. 97%) into a single glass
container with a stir bar under inert atmosphere. Thereafter add
30.0 ml of tetrahydrofuran (THF, anhydrous<20 ppm H.sub.2O) and
20.0 ml of 1,2-dimethoxymethane (DME, anhydrous<20 ppm
H.sub.2O). Subsequently stir for a time in the range from one to
twenty-four hours at a temperature above room temperature after
which solution may be returned to room temperature. In some cases
it is preferential to heat the sample to 30.0.degree. Celsius or
more while stirring in order to facilitate reaction of the
materials. The resulting solution is clear or slightly cloudy or
translucent with no precipitation. In some embodiments it is
preferable to rigorously stir over Mg metal powder in order to
condition the solution for improved electrochemical response by
reducing residual water and other impurities.
[0050] The product can be described as
Mg.sub.2Cl.sub.3[N(CF.sub.3SO.sub.2).sub.2] salt or more generally
as a magnesium halide cation complex or more specifically as a
Mg.sub.2Cl.sub.3-TFSI complex solution. In some embodiments it may
be preferable to note the coordination solvent molecules to the
complex cation. The product of this reaction enables reversible,
facile electrochemical plating and stripping of Mg ions onto an
electrode while maintaining a high anodic stability, and these
advantageous electrochemical characteristics are achieved without
the use of Grignard reagents, organometallic materials, or Lewis
acid derived anions including tetrachloroaluminate or
tetraphenylborate.
[0051] If X represents a halide, and Z represents an inorganic
polyatomic monovalent ion, such as the non-limiting examples of
anions listed in Table I, it is possible to generalize formulas the
complexes or compounds that are expected to be useful in
electrolytes for secondary Mg batteries, for electrochemical cells
having a Mg electrode and in energy storage devices having a Mg
electrode. Such generalized formulas are given in Table III, along
with specific examples for different integer values of the variable
n.
TABLE-US-00003 TABLE III Equivalent Example in Which Value Compound
Cation and X = Cl and Formula of n or Complex Anion Species Z =
TFSI Mg.sub.n+1X.sub.2nZ.sub.2 0 MgZ.sub.2 Mg.sup.2+ + 2Z.sup.-
Mg.sup.2+ + 2(TFSI).sup.- 1 Mg.sub.2X.sub.2Z.sub.2 2MgX.sup.+ +
2Z.sup.- 2MgCl.sup.+ + 2(TFSI).sup.- 2 Mg.sub.3X.sub.4Z.sub.2
MgX.sup.+ + MgCl.sup.+ + Mg.sub.2X.sub.3.sup.+ + 2Z.sup.-
Mg.sub.2Cl.sub.3.sup.+ + 2(TFSI).sup.- 3 Mg.sub.4X.sub.6Z.sub.2
2Mg.sub.2X.sub.3.sup.+ + 2Mg.sub.2Cl.sub.3.sup.+ + 2Z.sup.-
2(TFSI).sup.- 4 Mg.sub.5X.sub.8Z.sub.2 MgX.sub.2 + MgCl.sub.2 +
2Mg.sub.2X.sub.3.sup.+ + 2Mg.sub.2Cl.sub.3.sup.+ + 2Z.sup.-
2(TFSI).sup.-
[0052] The non-aqueous electrolyte solution including
Mg.sub.2Cl.sub.3-TFSI can employ MgCl.sub.2 and
Mg[N(CF.sub.3SO.sub.2).sub.2].sub.2 over a range of proportions to
provide formation of Mg.sup.2+, Mg.sub.2Cl.sub.3.sup.+, MgCl.sup.+
and MgCl.sub.2, or mixtures thereof. In certain embodiments, the
MgCl.sub.2:Mg(TFSI).sub.2 ratio is in the ratio of 1:4 to 5:1 with
preferable ratios being 4:1, 3:1, 2:1 or any ratio between. For
example, any non-whole number proportion in the range from 5:1 to
1:1 may also be used. In one or more embodiments, the electrolyte
salt complex can have an Mg concentration of greater than 0.1 M for
Mg.
[0053] In one or more embodiments a non-aqueous electrolyte for use
in an electrochemical cell includes at least one organic solvent
and at least one electrolytically active, soluble, magnesium (Mg)
salt complex represented by the formula
Mg.sub.n+1Cl.sub.(2*n)Z.sub.2, in which Z is selected from the
group of monovalent negative complex ions described in Table I or
mixtures thereof; and n is in the range from one to four. The
electrolyte salt complex can be used at any concentration; however,
in certain embodiments, the Mg molarity, e.g., concentration,
ranges up to 1 M. In one or more embodiments, the electrolyte salt
complex is expected to have a Mg concentration of about 0.25 to
about 0.5 M. In a few additional embodiments, the electrolyte salt
complex is expected to have a Mg concentration of greater than 1
M.
[0054] Surprisingly, it has been proposed that the voltage at which
the anodic electrolyte decomposition occurs is set by the breaking
of metal-organic bonds. In addition, chlorinated anions such as
tetrachloroaluminate limit the anodic stability to .about.3 V vs.
Mg/Mg.sup.2+. In order to surpass the energy density limitations of
current state-of-the-art one needs an electrolyte capable of higher
voltage stability while maintaining the ability to
electrochemically deposit and strip Mg-ions in facile, reversible
manner.
[0055] While not being bound by any particular mode of operation,
it is hypothesized that the capability for reversible Mg deposition
is accomplished via the formation of MgCl.sup.+ and/or
Mg.sub.2Cl.sub.3.sup.+ and/or Mg.sub.3Cl.sub.4.sup.+ clusters in
solution. Cationic species using other halides, such as MgBr.sup.+
and/or Mg.sub.2Br.sub.3.sup.+ clusters, and MgF.sup.+ and/or
Mg.sub.2F.sub.3.sup.+ clusters may also be suitable for reversible
Mg deposition.
[0056] Although MgCl.sub.2 is generally regarded as insoluble or
poorly soluble in many organic solvents, it is possible to prepare
non-aqueous electrolyte solution including magnesium chloride
complexes and in particular using Mg.sub.2Cl.sub.3-TFSI, wherein
the Mg molarity, e.g., concentration, ranging up to 2 M, and for
example at about 0.1 to about 0.5 M for Mg.
[0057] Other anions with high anodic stability may be used, as long
as they meet the requirements of electrochemical stability
throughout the voltage window of cell operation.
[0058] A variety of organic solvents are suitable for use in the
electrolyte of the present invention. The organic solvents can be
used alone or in combination. Whether a solvent comprises a single
organic composition or a plurality of organic compositions, for the
purposes of further exposition, the organic solvent will be
referred to as "the solvent" in the singular. In order to provide
for the reversible dissolution and plating of Mg, the solvent
advantageously should provide appreciable solubility by
coordination of the constituent inorganic salts of Mg. Further the
solvent preferably should not reduce above the Mg plating
potential, so as to form products which inhibit migration of Mg
from solution to the electrode surface. In various embodiments,
suitable solvents include ethers and tertiary amines, and may also
include organic carbonates, lactones, ketones, glymes, nitriles,
ionic liquids, aliphatic and aromatic hydrocarbon solvents and
organic nitro solvents. More specifically, suitable solvents
include THF, 2-methyl THF, dimethoxyethane, diglyme, triglyme,
tetraglyme, diethoxyethane, diethylether, proglyme, ethyl diglyme,
butyl diglyme, dimethylsulfoxide, dimethylsulfite, sulfolane, ethyl
methyl sulfone, acetonitrile, hexane, toluene, nitromethane, 1-3
dioxalane, 1-3 dioxane, 1-4 dioxane, trimethyl phosphate, tri-ethyl
phosphate, hexa-methyl-phosphoramide (HMPA),
N,N-propyl-methyl-pyrrolidinium-bis(trifluoromethylsulfonyl)imide
(P13-TFSI), N,N-propyl-methyl-pyrrolidinium-diacetamide (P13-DCA),
propyl-methyl-pyrrolidinium-bis(fluorosulfonyl)imide (P13-FSI),
ethyl-dimethyl-propyl-ammonium-bis(trifluoromethylsulfonyl)imide
(PDEA-TFSI), and
1-(methoxyethyl)-1-methylpiperidinium-bis(trifluoromethylsulfonyl)imide
(MOEMPP-TFSI).
[0059] In one or more embodiments, the solvent that enables
reversible, electrochemical deposition and stripping of Mg from a
solution containing the reaction product(s) of MgCl.sub.2 and
Mg(TFSI).sub.2 is a THF, dimethoxyethane, ethyl diglyme, butyl
diglyme, or a mixture thereof.
[0060] The reaction described above is motivated by an effort to
surpass the high voltage and safety limitations of previous
organometallic-based electrolytic solutions. However, it would
appear that the result observed comes as a surprise to one of
ordinary skill in the relevant art, for three reasons: First,
electrolyte solutions previously shown to reversibly electrodeposit
Mg metal at or near room temperature generally required the
utilization of Grignard reagent, or another organometallic reagent
with metal-organic bonds. One practiced in the art will recognize
that previous attempts to utilize inorganic magnesium salts failed
to enable substantial reversibility of magnesium deposition with
high Coulombic efficiency and low overpotential, but instead
resulted in decomposition of the solution components. Second, the
low solubility of MgCl.sub.2 in various solvents led others to
conclude co-dissolution and reaction was not favorable. And third,
MgCl.sub.2 is a chemically inert inorganic magnesium salt. It does
not dissociate in based on aprotic organic solvents to appreciable
extent and displays little to no conductivity in ethereal solution.
Furthermore, MgCl.sub.2 alone is electrochemically inactive in such
ethereal solutions, enabling only negligible Mg deposition,
dissolution or intercalation.
[0061] The magnesium electrolyte salt can be prepared by combining
a source of magnesium cation, e.g., a magnesium halide, and a
source of an anion stable at high voltage, based on the anion Z in
the electrolyte solvent with stirring and heating. Exemplary
reaction times include 1, 5, 10, 12, 24, 48 and 72 hours; exemplary
reaction temperatures include between 20 and 50 degrees Celsius.
Heating under inert or reduced atmosphere is preferred to avoid
water contamination and formation of oxide species.
[0062] In some embodiments, it is preferable to condition the
solution prior to use in an electrochemical cell, by elimination or
mitigation of harmful species inevitable found in the raw materials
and/or the as-prepared solution. In some embodiments, additives are
provided in the electrolyte to mitigate the deleterious species,
without the production of side reaction or unwanted, harmful
chemicals. Water, oxygen, and peroxide(s) are non-limiting examples
of deleterious species.
Solution Conditioning
[0063] Solution conditioning is accomplished by control of
variables including, but not limited to, cation:anion ratio,
constituent molarity, choice of solvent or solvents, precursor and
solvent purity, impurity removal, reaction temperature, time,
mixing, and electrochemical conditions can yield a solution
containing an all inorganic salt capable of reversible deposition
of Mg. The electrolyte can be conditioned using a variety of
processes, including physical, chemical and electrochemical
process.
[0064] The process of conditioning includes the following
non-limiting examples.
[0065] Physical processes that enable a high degree of Mg complex
formation and removal of deleterious species/impurities including:
heating, freezing, distillation, maintaining an
MgCl.sub.2:MgZ.sub.2 ratio between 1:1 and 4:1, maintaining
molarities that saturate the solution, etc. In some embodiments,
the electrolyte solution is heated to help the dissolution of the
Mg salts. In some embodiments, the MgCl.sub.2:MgZ.sub.2 ratio is
adjusted so that a saturated electrolyte solution with high
concentration of the electrolytically active Mg salt complex is
obtained. In some specific embodiments, the MgCl.sub.2:MgZ.sub.2
ratio is 1:1, 2:1, 3:1, or 4:1 or any non-integer value in between.
Similarly, in the case where Z is an anion other than
bis(trifluoromethylsulfonyl)imide, the MgCl.sub.2:MgZ.sub.2 ratio
can be adjusted to result in a high concentration of
electrolytically active Mg salt complex. Non-limiting examples of
the MgCl.sub.2:MgZ.sub.2 with any ratio between 4:1 and 1:4.
[0066] Chemical processes in order to remove deleterious species
such as addition of minute quantities of proton/water scavengers,
such as Grignard reagents, AlCl.sub.3, organoaluminum, molecular
sieves, gamma-alumina, silica, Magnesium metal, etc.
[0067] Electrochemical processes like potentiostatic,
potentiodynamic or galvanostatic electrolysis that enable a high
degree of Mg complex formation and removal of deleterious
species/impurities. This can be accomplished at reducing or
oxidizing potentials, which reduce or oxidize deleterious species
and/or drive the reaction of reactants to products. It can be
exercised with inert electrodes, sacrificial electrodes, like Mg
or, within a complete cell, with an auxiliary electrode or with the
cathode serving as the working electrode. In some specific
embodiments, the electrolyte is subjected to multiple cycles of
potentiostatic, potentiodynamic or galvanostatic electrolysis. In
some specific embodiments, the electrolyte is potentiostatically
polarized for 5 cycles, 10 cycles, 15 cycles, 20 cycles, or 30
cycles.
[0068] In one or more embodiments, the electrolyte salt solution is
conditioned to improve the electrochemical properties through
electrochemical polarization.
[0069] In one or more embodiments, the electrolyte salt solution is
conditioned to improve the electrochemical properties by reacting
with insoluble active metals, such as metallic Mg, Al, Ca, Li, Na,
or K, and/or reacting with insoluble acids/bases, and by being
exposed to adsorbing agents such as molecular sieves, CaH.sub.2,
alumina, silica, MgCO.sub.3, and similar absorptive materials.
[0070] In one or more embodiments, the electrolyte salt solution is
conditioned to improve the electrochemical properties by providing
additives to scavenge contaminants. The contaminants that can be
scavenged include but are not limited to organo-Mg compounds,
organo-Al compounds, organo-B compounds, organometallics, trace
water, oxygen, CO.sub.2, and protic contaminants such as acids.
[0071] As described above, the electrochemical window of a cell
with an electrolyte as described herein and an appropriate
anode-cathode pair has been observed to be 3.5-3.6 volts.
[0072] It is expected that the electrolytic solutions described and
contemplated herein can be used in such devices as electrochemical
cells, secondary (e.g., rechargeable) batteries, and energy storage
devices that include, in addition to the electrolyte, an anode and
a cathode. In some embodiments, an electrochemical cell can include
a metal anode and an intercalation cathode.
[0073] In one or more embodiments, a secondary battery includes the
electrolyte according to the present invention, a magnesium metal
anode and a magnesium insertion compound cathode.
[0074] In one or more embodiments, a secondary battery includes the
electrolyte according to the present invention, a magnesium metal
anode and a conversion, or displacement compound cathode.
[0075] In one or more embodiments, the magnesium insertion-compound
cathode includes a magnesium-Chevrel intercalation cathode of the
formula, Mo.sub.6S.sub.8.
[0076] The electrolyte composition of the present invention
includes an organic solvent and electrochemically-active, soluble,
inorganic salt complex represented by the formula
Mg.sub.n+1Cl.sub.(2*n)Z.sub.2, in which Z is selected from the
compounds described in Table I or mixtures thereof; and n is in the
range from one to four.
[0077] Inorganic salts of this form may, in certain cases, be
combined with compatible organometallic salts or with compatible
inorganic salts of other forms.
[0078] Intercalation cathodes used in conjunction with the
electrolyte according to the present invention preferably include
transition metal oxides, transition metal oxo-anions,
chalcogenides, and halogenides and combinations thereof.
Non-limiting examples of positive electrode active material for the
Mg battery include Chevrel phase Mo.sub.6S.sub.8, MnO.sub.2, CuS,
Cu.sub.2S, Ag.sub.2S, CrS.sub.2, VOPO.sub.4, layered structure
compounds such as TiS.sub.2, V.sub.2O.sub.5, MgVO.sub.3, MoS.sub.2,
MgV.sub.2O.sub.5, MoO.sub.3, Spinel structured compounds such as
CuCr.sub.2S.sub.4, MgCr.sub.2S.sub.4, MgMn.sub.2O.sub.4,
MgNiMnO.sub.4, Mg.sub.2MnO.sub.4, NASICON structured compounds such
as MgFe.sub.2(PO.sub.4).sub.3 and MgV.sub.2(PO.sub.4).sub.3,
Olivine structured compounds such as MgMnSiO.sub.4 and
MgFe.sub.2(PO.sub.4).sub.2, Tavorite structured compounds such as
Mg.sub.0.5VPO.sub.4F, pyrophosphates such as TiP.sub.2O.sub.7 and
VP.sub.2O.sub.2, and fluorides such as MgMnF.sub.4 and
FeF.sub.3.
[0079] In some embodiments, the positive electrode layer further
comprises an electronically conductive additive. Non-limiting
examples of electronically conductive additives include carbon
black, Super P, Super C65, Ensaco black, Ketjen black, acetylene
black, synthetic graphite such as Timrex SFG-6, Timrex SFG-15,
Timrex SFG-44, Timrex KS-6, Timrex KS-15, Timrex KS-44, natural
flake graphite, carbon nanotubes, fullerenes, hard carbon, or
mesocarbon microbeads.
[0080] In some embodiments, the positive electrode layer further
comprises a polymer binder. Non-limiting examples of polymer
binders include poly-vinylidene fluoride (PVdF), poly(vinylidene
fluoride-co-hexafluoropropene) (PVdF-HFP), Polytetrafluoroethylene
(PTFE), Kynar Flex 2801, Kynar Powerflex LBG, and Kynar HSV 900, or
Teflon.
[0081] Negative electrodes used in conjunction with the present
invention comprise a negative electrode active material that can
accept Mg-ions. Non-limiting examples of negative electrode active
material for the Mg battery include Mg, Mg alloys such as AZ31,
AZ61, AZ63, AZ80, AZ81, AZ91, AM50, AM60, Elektron 675, ZK51, ZK60,
ZK61, ZC63, M1A, ZC71, Elektron 21, Elektron 675, Elektron, Magnox,
or insertion materials such as Anatase TiO2, ruble TiO2,
Mo.sub.6S.sub.8, FeS.sub.2, TiS.sub.2, MoS.sub.2.
[0082] In some embodiments, the negative electrode layer further
comprises an electronically conductive additive. Non-limiting
examples of electronically conductive additives include carbon
black, Super P, Super C65, Ensaco black, Ketjen black, acetylene
black, synthetic graphite such as Timrex SFG-6, Timrex SFG-15,
Timrex SFG-44, Timrex KS-6, Timrex KS-15, Timrex KS-44, natural
flake graphite, carbon nanotubes, fullerenes, hard carbon, or
mesocarbon microbeads.
[0083] In some embodiments, the negative electrode layer further
comprises a polymer binder. Non-limiting examples of polymer
binders include poly-vinylidene fluoride (PVdF), poly(vinylidene
fluoride-co-hexafluoropropene) (PVdF-HFP), Polytetrafluoroethylene
(PTFE), Kynar Flex 2801, Kynar Powerflex LBG, and Kynar HSV 900, or
Teflon.
[0084] In some embodiments, the Mg battery used in conjunction with
the electrolyte described herein comprises a positive electrode
current collector comprising carbonaceous material, or a current
collector comprising a metal substrate coated with an over-layer to
prevent corrosion in the electrolyte. In some embodiments, the Mg
battery described herein comprises a negative electrode current
collector comprising carbonaceous material. In other embodiments,
the Mg battery described herein comprises positive and negative
electrode current collectors comprising carbonaceous material.
[0085] In some embodiments, the Mg battery disclosed herein is a
button or coin cell battery consisting of a stack of negative
electrode, porous polypropylene or glass fiber separator, and
positive electrode disks sit in a can base onto which the can lid
is crimped. In other embodiments, the Mg battery used in
conjunction with the electrolyte disclosed herein is a stacked cell
battery. In other embodiments, the Mg battery disclosed herein is a
prismatic, or pouch, cell consisting of one or more stacks of
negative electrode, porous polypropylene or glass fiber separator,
and positive electrode sandwiched between current collectors
wherein one or both current collectors comprise carbonaceous
materials, or a metal substrate coated with an over-layer to
prevent corrosion in the electrolyte. The stack(s) are folded
within a polymer coated aluminum foil pouch, vacuum and heat dried,
filled with electrolyte, and vacuum and heat sealed. In other
embodiments, the Mg battery disclosed herein is a prismatic, or
pouch, bi-cell consisting of one or more stacks of a positive
electrode which is coated with active material on both sides and
wrapped in porous polypropylene or glass fiber separator, and a
negative electrode folded around the positive electrode wherein one
or both current collectors comprise carbonaceous materials. The
stack(s) are folded within a polymer coated aluminum foil pouch,
dried under heat and/or vacuum, filled with electrolyte, and vacuum
and heat sealed. In some embodiments of the prismatic or pouch
cells used in conjunction with the electrolyte described herein, an
additional tab composed of a metal foil or carbonaceous material of
the same kind as current collectors described herein, is affixed to
the current collector by laser or ultrasonic welding, adhesive, or
mechanical contact, in order to connect the electrodes to the
device outside the packaging.
[0086] In other embodiments, the Mg battery used in conjunction
with the electrolyte disclosed herein is a wound or cylindrical
cell consisting of wound layers of one or more stacks of a positive
electrode which is coated with active material on one or both
sides, sandwiched between layers of porous polypropylene or glass
fiber separator, and a negative electrode wherein one or both
current collectors comprise carbonaceous materials. The stack(s)
are wound into cylindrical roll, inserted into the can, dried under
heat and/or vacuum, filled with electrolyte, and vacuum and welded
shut. In some embodiments of the cylindrical cells described
herein, an additional tab composed of a metal foil or carbonaceous
material of the same kind as current collectors described herein,
is affixed to the current collector by laser or ultrasonic welding,
adhesive, or mechanical contact, in order to connect the electrodes
to the device outside the packaging.
Theoretical Discussion
[0087] Although the theoretical description given herein is thought
to be correct, the operation of the devices described and claimed
herein does not depend upon the accuracy or validity of the
theoretical description. That is, later theoretical developments
that may explain the observed results on a basis different from the
theory presented herein will not detract from the inventions
described herein.
[0088] Any patent, patent application, or publication identified in
the specification is hereby incorporated by reference herein in its
entirety. Any material, or portion thereof, that is said to be
incorporated by reference herein, but which conflicts with existing
definitions, statements, or other disclosure material explicitly
set forth herein is only incorporated to the extent that no
conflict arises between that incorporated material and the present
disclosure material. In the event of a conflict, the conflict is to
be resolved in favor of the present disclosure as the preferred
disclosure.
[0089] While the present invention has been particularly shown and
described with reference to the preferred mode as illustrated in
the drawing, it will be understood by one skilled in the art that
various changes in detail may be affected therein without departing
from the spirit and scope of the invention as defined by the
claims.
* * * * *