Classifications

• • H—ELECTRICITY
  • H01—ELECTRIC ELEMENTS
  • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
  • H01M10/00—Secondary cells; Manufacture thereof
  • H01M10/05—Accumulators with non-aqueous electrolyte
  • H01M10/056—Accumulators with non-aqueous electrolyte characterised by the materials used as electrolytes, e.g. mixed inorganic/organic electrolytes
  • H01M10/0564—Accumulators with non-aqueous electrolyte characterised by the materials used as electrolytes, e.g. mixed inorganic/organic electrolytes the electrolyte being constituted of organic materials only
  • H01M10/0566—Liquid materials
  • H01M10/0569—Liquid materials characterised by the solvents
• • H—ELECTRICITY
  • H01—ELECTRIC ELEMENTS
  • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
  • H01M6/00—Primary cells; Manufacture thereof
  • H01M6/14—Cells with non-aqueous electrolyte
  • H01M6/16—Cells with non-aqueous electrolyte with organic electrolyte
  • H01M6/162—Cells with non-aqueous electrolyte with organic electrolyte characterised by the electrolyte
  • H01M6/164—Cells with non-aqueous electrolyte with organic electrolyte characterised by the electrolyte by the solvent
• • Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
  • Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
  • Y02E—REDUCTION OF GREENHOUSE GAS [GHG] EMISSIONS, RELATED TO ENERGY GENERATION, TRANSMISSION OR DISTRIBUTION
  • Y02E60/00—Enabling technologies; Technologies with a potential or indirect contribution to GHG emissions mitigation
  • Y02E60/10—Energy storage using batteries

Definitions

• the present application claims priority rights based on U.S. Provisional Application Serial No. 60/006,207 filed November 3, 1995 and U.S. Provisional Application Serial No. 60/006,435 filed November 13, 1995.
• the present application claims priority rights based on U.S. Nonprovisional Application Serial No. , filed on October 31, 1996, which has the same title and inventors as the present application, has attorney identification number P30795, and was transmitted to the U.S. Patent and Trademark Office under Express Mail No. EH682355287US.
• the present application also claims priority rights based on U.S.
• This invention relates generally to electrolyte solvents for use in liquid or rubbery polymer electrolyte solutions as are used, for example, in electrochemical devices. More specifically, this invention is directed to boron-containing electrolyte solvents and boron-containing electrolyte solutions.
• Typical electrolyte solvents for use in liquid or polymer electrolyte solutions include alkyl ethers such as dimethyl ether, diethyl ether, dioxalane, diglyme and tetraglyme; and alkene carbonates such as ethylene carbonate (hereinafter “EC”) and propylene carbonate (hereinafter “PC”) . These solvents are used to dissolve electrolyte solutes and/or rubberizing polymer additives to form electrolyte solutions which may be used in electrochemical devices.
• alkyl ethers such as dimethyl ether, diethyl ether, dioxalane, diglyme and tetraglyme
• alkene carbonates such as ethylene carbonate (hereinafter “EC") and propylene carbonate (hereinafter “PC”) .
• EC ethylene carbonate
• PC propylene carbonate
• alkyl ethers and alkene carbonates present significant disadvantages as electrochemical solvents.
• alkyl ethers are relatively volatile, and therefore may evaporate over time. This is a disadvantage in any electrochemical device that is meant to operate for an extended period of time because evaporation of the solvent may change the electrical behavior of the device.
• solvents present fire hazards.
• alkyl ethers typically have low dielectric constants which discourage solvation of electrolyte salts. Therefore, alkyl ethers generally depend on cation chelation effects to dissolve signifi ⁇ cant amounts of electrolyte salts. Such compositions, containing limited amounts of electrolyte, tend to have a limited number of available charge carrier ions. Furthermore, when cation solvation is the driving force for forming a solution, the cation transport number will be low. Both paucity of charge carriers and low cation transport values may lead to undesirable polarization effects. Alkene carbonates have higher dielectric constants than alkyl ethers, and therefore are better electrolyte solvents for liquid or polymer electrolytes.
• PC is not a suitable solvent because it is unstable in the presence of alkali metals, and forms a passivating layer on lithium.
• EC is also problematic because its melting point is above room temperature, and therefore it must be mixed with compounds that lower its melting temperature to obtain a liquid or rubbery electrolyte.
• both PC and EC form cloudy solutions with alkali metal salts, which are indicative of disadvantageous composition fluctuations or pre- passivation reaction products.
• Various unsuccessful attempts have also been made to use other organic molecules, such as ketones, as electrolyte solvents. These attempts were unsuccessful because these molecules exhibit poor chemical and electrochemical stability in the presence of alkali metals.
• boron electrolyte solvents Lewis acid boron-containing compounds
• the present invention relates to boron electrolyte solvents, boron electrolyte solvent mixtures and boron electrolyte solutions which all comprise at least one Lewis acid boron-containing compound.
• the present invention further relates to rechargeable batteries and other electrochemical devices which utilize such electrolyte solutions.
• the boron electrolyte solvents according to the present invention comprise one or more
• Such boron electrolyte solvents include those with boron linked to oxygen, halogen atoms, sulfur atoms or combinations thereof.
• the boron electrolyte solvent comprises a boron atom bound to two oxygen radicals and one halogen atom as shown below in formula (I) :
• R and R 2 may be straight or branched chain aliphatic or aromatic alkyl groups and X is a halogen atom. These alkyl groups may have various substituents (e.g. halides) which effectively vary the electronic charge density at the boron atom. It is further preferred for R x and R 2 to together form a heterocyclic ring containing an O-B-O linkage.
• Preferable boron electrolyte solvents are borate compounds which have at least one B0 3 group such as is shown below in formula (II) :
• R 1# R 2 and R 3 may be straight or branched chain aliphatic or aromatic alkyl groups . These alkyl groups may have various substituents (e.g. halides) , which effectively vary the electronic charge density at the boron atom. It is further preferred for R x and R 2 to together form a heterocyclic ring containing an O-B-O linkage. In one such preferred molecule (hereinafter "BEG-3") according to formula (II) , Rl and R2 together form a propyl group and R3 is an isopropyl group.
• BEG-3 preferred molecule
• the boron electrolyte solvents may comprise borate ethers dimers according to formula (III) below: , O O R 3
• R lf R 2 , R 3 and R 4 may be straight or branched chain aliphatic or aromatic alkyl groups. These alkyl groups may have various substituents (e.g. halides) which effectively vary the electronic charge density at the boron atoms. It is further preferred for R x and R 2 , and R 3 and R 4 , respectively, to together form two heterocyclic rings containing O-B-O linkages. In one such preferred molecule (hereinafter "BEG-2”) according to formula (III) , R 1 and R 2 , and R 3 and R 4/ respectively, together form two propyl groups.
• BEG-2 preferred molecule
• a most preferred class of borate ether-type boron electrolyte solvents has a B-O-Z-O-B linkage as shown below in formula (IV) :
• R l t R 2 , R 3 and R 4 may be straight or branched chain aliphatic or aromatic alkyl groups. These groups may be substituted with various substituents of differing electronegativity, (e.g. halides) which effectively vary the electronic charge density on the boron atoms. It is further preferred for R x and R 2 , and R 3 and R 4 , respectively to together form two heterocyclic rings containing O-B-O linkages. "Z” may be a straight or branched chain aliphatic or aromatic alkyl group which may also be substituted with various groups of different electronegativity. "Z” may also be a siloxane group such as dimethyl siloxane or another bivalent radical.
• BEG-1 In one such preferred molecule (hereinafter "BEG-1") according to formula (IV) , R t and R 2 , and R 3 and R 4 , respectively, together form two propyl groups, and Z is (CH 2 ) 3 .
• the chemical structure of BEG-1 is shown below:
• Boron electrolyte solvent mixtures according to the invention comprise a boron electrolyte solvent which functions as an electrolyte solvent together with a conventional electrolyte solvent (e.g., an alkene carbonate or an alkyl ether) .
• Boron electrolyte solutions comprise an electrolyte solute (such as an electrolyte salt) dissolved in a boron electrolyte solvent or in a boron electrolyte solvent mixture.
• Boron electrolyte solutions according to the invention preferably comprise less than 50 mole percent, and more preferably less than 30 mole percent electrolyte solute.
• the boron electrolyte solvents and boron electrolyte solvent mixtures of the present invention exhibit unexpectedly superior electrochemical stability against anodic decomposition compared to conventional electrochemical solvents; (ii) exhibit unexpectedly superior chemical stability against degradation in the presence of alkali metals;
• (iii) are capable of dissolving large mole fractions of most electrolyte solutes, including alkali metal salts, to provide high room temperature conductivity boron electrolyte solutions;
• (iv) are glass-forming liquids (i.e. liquids which are resistant to crystallization with or without an electrolyte solute salt) at room temperature and down to the glass transition temperature of about -70°C, thus enabling use at low temperatures;
• (v) exhibit higher boiling points and correspondingly lower ambient temperature volatilities than most conventional electrolyte solvents, thus reducing the possibility of volatilization of the electrolyte solvent; and (vi) exhibit wide electrochemical windows, enabling use over a wide voltage range.
• a particularly effective boron electrolyte solvent mixture may be obtained by mixing together one or more of the above-described boron electrolyte solvents with an alkene carbonate.
• Such a boron electrolyte solvent mixture has a lower viscosity and remarkably improved electrochemical stability compared to a conventional electrolyte solvent which solely contains an alkene carbonate.
• Examples of such boron electrolyte solvent mixtures with alkene carbonates include, but are not limited to, a mixture of 1 part by weight BEG-1 mixed with 2 parts by weight EC (hereinafter "1:2 Mix BEG- 1:EC”) ; 1 part by weight BEG-2 mixed with 2 parts by weight EC (hereinafter “1:2 Mix BEG-2:EC”); and corresponding PC mixtures.
• the boron electrolyte solvent mixture or electrolyte solution of the invention may further comprise a polymer which imparts a rubbery consistency.
• a polymer which imparts a rubbery consistency are known as "gel electrolytes.”
• Figure 1 is a plot of log conductivity (Sem "1 ) versus reciprocal temperature (K) for various mole percentages of LiC10 4 dissolved in BEG-1.
• Figure 2 is a plot of log conductivity (Sem _1 ) versus mole fraction of dissolved LiC10 4 in BEG-1 at various temperatures (°C) .
• Figure 3 is a plot of log conductivity (Sem "1 ) versus reciprocal temperature (K) for various molarities of LiN(S0 2 CF 3 ) 2 dissolved in BEG-1.
• Figure 4 is an overlay of two cyclic voltammograms for the BEG-1 solvent, and for a 2.5M LiC10 4 solution in the 1:2 Mix BEG-1:EC solvent.
• Figure 5 is an overlay of three cyclic volta ⁇ mmograms for a 2.5M LiC10 4 solution in the 1:2 Mix BEG-1:EC solvent compared with a conventional l.OM LiC10 4 solution in a 1:1 mixture of dimethyl ether:EC and a conventional 3.IM LiC10 4 solution in EC.
• Figure 6 is an overlay plot of two cyclic voltammograms for a 1. OM LiC10 4 solution in 1:2 Mix BEG-1:PC compared with a conventional l.OM LiC10 4 solution in PC.
• Figure 7 is an overlay plot of log conductivity (Sem '1 ) versus reciprocal temperature (K) for a 2.5M LiC10 4 solution in 1:2 Mix BEG-1:EC solvent, and the same composition further containing 20 percent by weight polyvinyl acetate (PVAc) .
• Figure 8 is an overlay plot of log conductivity (Sem" 1 ) versus reciprocal temperature (K) for solutions of l.OM and 2.5M LiC10 4 , LiN(S0 2 CF 3 ) 2 and LiS0 3 CF 3 in 1:2 Mix BEG-1:EC.
• Figure 9 is an overlay plot of log conductivity
• Figure 10 is an overlay plot of three cyclic voltammograms for l.OM LiC10 4 solutions in 1:2 Mix BEG-1:EC, 1:2 Mix BEG-2:EC and 1:2 Mix BEG-3:EC.
• Figure 11 is a plot of cell voltage versus time for the first discharge/charging cycle for a Li/2.5M LiN(S0 2 CF 3 ) 2 in 1:2 Mix BEG-1:EC gel electrolyte (containing 20 weight percent PVAc)/Li x Mn 2 0 4 battery.
• Figure 12 is a plot of cell voltage versus time for several discharge/charging cycles for a Li/2.5M LiN(S0 2 CF 3 ) 2 in 1:2 Mix BEG-1:EC gel electrolyte (containing 20 weight percent PVAc)/Li x Mn 2 0 4 battery.
• boron electrolyte solvent refers to a Lewis acid boron-containing compound, with one or more 3-coordinated boron atoms, which is capable of dissolving an electrolyte solute.
• boron electrolyte solvent mixture refers to a mixture of two or more electrolyte solvents which comprises at least one boron electrolyte solvent according to the present invention.
• the term “electrolyte solute” refers to a conductive species, such as a salt, which behaves as an electrolyte (i.e., transports an electric current via long range motion of ions) , and may be dissolved in the boron electrolyte solvent or boron electrolyte solvent mixture.
• the term “boron electrolyte solution” refers to a combination of an electrolyte solute and a boron electrolyte solvent or boron electrolyte solvent mixture.
• electrochemical device is meant to refer to any apparatus that uses an electrolyte.
• the boron electrolyte solvent comprises a compound accord ⁇ ing to formula (I) below:
• R-. and R 2 may be straight or branched chain aliphatic or aromatic alkyl groups and X is a halogen atom. These alkyl groups may have various substituents (e.g. halides) which effectively vary the electronic charge density at the boron atom. It is further preferred for R x and R 2 to together form a heterocyclic ring containing an O-B-O linkage.
• boron electrolyte solvents are borate compounds according to formula (II) below:
• R l t R 2 and R 3 may be straight or branched chain aliphatic or aromatic alkyl groups. These alkyl groups may have various substituents (e.g. halides) , which effectively vary the electronic charge density at the boron atom. It is further preferred for R 1 and R 2 to together form a heterocyclic ring containing an O-B-O linkage. It may also be possible to synthesize advantageous boron electrolyte solvents analogous to those of formula (II) wherein the oxygen atoms are replaced by sulfur.
• borate compounds according to formula (II) are preferably synthesized by reacting B 2 0 3 with an OH group-containing molecule such as an alcohol or a diol. More preferable borate ethers according to formula (II) are synthesized by reacting B 2 0 3 with 1,2-propane diol or 1,3-propane diol.
• the boron electrolyte solvents may comprise borate ether dimers according to formula (III) below:
• R l t R 2 , R 3 and R 4 may be straight or branched chain aliphatic or aromatic alkyl groups. These alkyl groups may have various substituents (e.g. halides) which effectively vary the electronic charge density at the boron atoms. It is still further preferred for R 1 and R 2 , and R 3 and R 4 , respectively, to together form two heterocyclic rings containing O-B-O linkages.
• a boron electrolyte solvent according to formula (III) is synthesized by reacting B 2 0 3 with 1,3-propane diol as described in example 5.
• the product formed is the boron ether shown below:
• the boron electrolyte solvents may be borate ether dimers according to formula (IV) below:
• R lf R 2 , R 3 and R 4 may be straight or branched chain aliphatic or aromatic alkyl groups. These groups may be substituted with various substituents of differing electronegativity, (e.g. halides) which effectively vary the electronic charge density on the boron atoms. It is further preferred for R and R 2 , and R 3 and R 4 , respectively, together to form heterocyclic rings containing O-B-O linkages.
• "Z” may be a straight or branched chain aliphatic or aromatic alkyl group, which may also be substituted with various groups of different electronegativity.
• “Z” may also be a siloxane group such as dimethyl siloxane or another bivalent radical.
• a preferred electrolyte solvent according to formula IV is synthesized by reacting (CH 3 ) 2 Si (OH) 2 with H 3 B0 3 and 1,3-propane diol as shown in Example 4.
• the product (hereinafter "BEG-4") formed is shown below:
• a most preferred boron electrolyte solvent according to formula IV is synthesized by reacting B(OH) 3 with a diol compound as shown in Example 3. Most preferable diols are 1,2-propane diol and 1,3 propane diol.
• BEG-1 1,3-propane diol
• an electrolyte solute is added to a boron electrolyte solvent or solvent mixture to form a boron electrolyte solution.
• Preferable electrolyte solutes include ionic salts such as LiAlCl 4 , LiC10 4 , LiN(S0 2 CF 3 ) 2 , LiS0 3 CF 3 , and their corresponding sodium analogues.
• Boron electrolyte solutions containing LiC10 4 are desirable because they produce very high conductivity electrolytes.
• solutions of LiN(S0 2 CF 3 ) 2 are more preferable for consumer applications because
• LiN(S0 2 CF 3 ) 2 is chemically more stable than LiC10 4 , and presents no explosion hazard, as does LiC10 4 .
• LiN(S0 2 CF 3 ) 2 -containing boron electrolyte solutions also exhibit relatively high conductivities.
• LiC10 4 is dissolved in BEG-l.
• Figs. 1 and 2 show that room temperature conductivities of a 9.1 mole percent LiC10 4 solution in BEG-l may approach IO "4 Sem "1 at room temperature.
• Figure 8 shows that a 1.OM LiC10 4 solution in 1:2 Mix BEG-1:EC has a conductivity of about IO "23 Sem "1 at room temperature.
• LiAlCl 4 was dissolved in a mixture of BEG-l and EC. Although LiAlCl 4 decomposes in most organic solvents and in pure BEG-l, it does not decompose in mixtures of BEG-l and EC.
• BEG-l and BEG-2 have symmetrical structures, and therefore may have small dielectric constants. However, BEG-l and BEG-2 are very good solvents for alkali metal salt electrolyte solutes. For example, BEG-1 dissolves up to 50 mole percent of LiC10 4 at ambient temperature to yield a viscous solution.
• Solutions of LiC10 4 in BEG-l and BEG-2 tend to be substantially transparent, which indicates that LiC10 4 may dissolve better in BEG-l and BEG-2 than in known ether or carbonate solvents, which often yield cloudy solutions. Cloudy electrolyte solutions are unsuitable for some applications, such as optical displays.
• a conventional solvent such as an alkene carbonate or an alkyl ether may be added to a boron electrolyte solvent to form a boron electrolyte solvent mixture.
• the preferred electrolyte solvent mixture "1:2 Mix BEG-2:EC” is formed by mixing 1 part by weight BEG-2 with 2 parts EC.
• the most preferred electrolyte solvent mixture "1:2 Mix BEG-l:EC” is formed by mixing 1 part BEG-l with 2 parts EC.
• high molecular weight polymers may also be added to electrolyte solutions to form gel electrolytes which exhibit more desirable rubbery behavior. It is preferable to use polymers with sufficiently high molecular weight to impart a rubbery consistency to the electrolyte.
• Preferred polymers include high molecular weight polyethylene oxide having a molecular weight of at least about IO 8 and polyvinyl acetate having a molecular weight of more than 50,000.
• polymer oils may be synthesized by reacting boron electrolyte solvents such as BEG-l with silicates as shown in Example 14.
• polymeric Lewis acid borate compounds may be synthesized as shown in Example 15.
• Ionic conductivities of the boron electrolyte solutions according to the present invention were determined from complex impedance plots obtained using twin platinum electrode dip-type cells with cell constants of about 1-2 cm "1 .
• the complex impedance plots were generated using a HEWLETT-PACKARD Model HP4192A-Frequency Analyzer. Measurements were automated to cover a predetermined temperature range at a sequence of temperatures controlled by a EUROTHERM temperature controller.
• Figs. 4-6 and 10 The cyclic voltammograms shown in Figs. 4-6 and 10 were obtained using a PAR Potentiometer. All scans were performed at room temperature with a scan speed of lOmV/s. A platinum pseudo-reference electrode was used for all the scans.
• boron electrolyte solvents and boron electrolyte solutions described herein are useful in all manner of electrochemical devices which require electrolytes.
• electrochemical devices which require electrolytes include batteries, fuel cells, photochromic displays, photovoltaic cells and gas sensors. This list is merely exemplary, and is not meant to limit the invention to any particular electrochemical device.
• BEG-5 (hereinafter "BEG-5") is shown below:
• BEG-5 was prepared by the following procedure disclosed by A. Finch, J.C. Lockhart and E.J. Pearn in J. Org. Chem. , 26, pp. 3250-53 (1961) . 15.2 grams (0.20 moles) of 1,3-propanediol (Aldrich, 98%) was added dropwise to a solution of 23.5 grams (0.20 moles) boron trichloride (Aldrich, IM in heptane) diluted in 60 mL methylene chloride (Baker) at 5°-10°C. Nitrogen was bubbled through the flask to remove HCl generated by the reaction. The reaction was allowed to proceed for 6 hours. Vacuum-distillation at 30°-31°C/0.15 mmHg yielded 15.9 grams of the product shown above (yield 66% based on BC1 3 ) .
• BEG-3 (hereinafter "BEG-3") is shown below:
• BEG-3 BEG-3 was prepared by the following procedure. 13.92 grams (0.20 mole) of B 2 0 3 (Aldrich, 99.98%) and 30.40 grams (0.40 mole) of 1, 3-propanediol (Aldrich, 98%) were mixed in approximately 50 mL toluene and refluxed in a flask equipped with water separation apparatus until no further water was generated. The total amount of water separated at this stage was approximately 7.3 mL. Then 26.40 grams (0.44 mole) of isopropanol (Aldrich, 99%) was added, and an additional 3.6 mL of water was collected. The resultant product was then refluxed in the presence of lithium overnight. Vacuum-distillation at 67°-68°C/0.4 mmHg yielded 38.0 grams of the product shown above (yield 66% based on B 2 0 3 ) .
• BEG-1 is a viscous, glass-forming liquid with a T g of -80°C and a boiling point of 125-128°C/0.05 mmHg, implying 380°C at 760 mmHg.
• a previous report of the preparation of this substance reports a boiling point of 165-169°C at 10.6 mmHg, implying 390°C at 760 mmHg. See H. Steinberg, Organoboron Chemistry. Vol. 1, Ch 5, (1964) .
• a preferred boron electrolyte solvent according to formula (IV) was synthesized as follows. 14.2 grams (0.11 mole, Aldrich, 99%) of (CH 3 ) 2 SiCl 2 was hydrolyzed by adding it to 30 mL of deionized water, and the product was extracted with 60 mL of ethyl ether. The organic phase was washed with deionized water until the pH reached 7, followed by evaporation of the ethyl ether. 1, 3-propanediol (16.8 grams, 0.
• a preferred boron electrolyte solvent according to formula (III) was synthesized as follows. 13.92 grams (0.20 mole) of B 2 0 3 (Aldrich, 99.98%-) and 30.40 grams (0.40 mole) of 1, 3-propanediol (Aldrich, 98%) were reacted in a similar manner to that described in Example 2. The amount of water finally separated was 7.3 mL. During vacuum-distillation the fraction of 138°-143°C/0.05 mmHg was collected with yield of 27.84 grams (75% based on B 2 0 3 ) .
• a boron electrolyte solvent mixture was prepared by mixing 1 part by weight BEG-l prepared according to
• Example 3 with two parts ethylene carbonate.
• a second boron electrolyte solvent mixture was prepared by mixing 1 part by weight BEG-l with two parts by weight propylene carbonate.
• a third boron electrolyte solvent mixture was prepared by mixing 1 part by weight BEG-l with one part by weight of acetone, which is a simple type of ketone. All reagents were mixed and weighed out in a dry box.
• Vials containing pieces of shiny lithium foil immersed in the above-described electrolyte solvent mixtures were sealed tightly and put aside for observa ⁇ tion.
• Control samples were prepared by immersing pieces of shiny lithium foil in the ethylene carbonate, propylene carbonate and acetone-containing solvent mixtures.
• the acetone-containing vials were left overnight at ambient temperature.
• the ethylene carbonate and propylene carbonate-containing vials were heated to 90°C in an oven overnight.
• BEG-l prepared according to Example 3 was mixed with two parts by weight EC to form a boron electrolyte solvent mixture "1:2 Mix BEG-l:EC.”
• BEG-l prepared according to Example 3 was mixed with two parts by weight PC to form a boron electrolyte solvent mixture "1:2 Mix BEG-l:PC.”
• BEG-2 prepared according to Example 5 was mixed with two parts by weight EC to form a boron electrolyte solvent mixture "1:2 Mix BEG-2:EC.”
• Example 8 One part by weight BEG-3 prepared according to Example 2 was mixed with two parts by weight EC to form a boron electrolyte solvent mixture "1:2 Mix BEG-3:EC.”
• Example 8 One part by weight BEG-3 prepared according to Example 2 was mixed with two parts by weight EC to form a boron electrolyte solvent mixture "1:2 Mix BEG-3:EC.”
• Various concentrations of LiC10 4 boron electrolyte solutions were prepared by dissolving LiC10 4 in BEG-l, which was prepared according to Example 3. All mate ⁇ rials were weighed out in a glove box.
• Fig. l shows a plot of the log of conductivity versus reciprocal temperature for these electrolytes.
• Fig. 2 shows a plot of the log of conductivity versus mole fraction LiC10 4 at 30°C, 50°C, 100°C and 150°C.
• the solution with the highest room temperature conductivity contained 9.1% LiC10 4 , and has a conductivity below 10 "4 Sem "1 .
• Fig. 1 shows that the solution of 75 mole percent LiC10 4 in BEG-l was only thermodynamically stable as a liquid above 80°C.
• Fig. 4 shows an overlay of two cyclic volta ⁇ mmograms obtained for a 2.5 M LiC10 4 Mix BEG-l:EC boron electrolyte solution and for pure BEG-l solvent.
• the cyclic voltammogram for the boron electrolyte solution indicates that lithium can be deposited and stripped back into the solution in an almost reversible fashion. This property is important for rechargeable electro ⁇ chemical devices using these electrolytes.
• Fig. 4 also shows that the 2.5 M LiC10 4 1:2 Mix
• BEG-l:EC electrolyte solution solvent exhibited a wide electrochemical window of about 5.3 volts. This observed voltage window is believed to be limited by the stability of the C10 4 " anion and the Li + cation in the solution, rather than by the solvent.
• Fig. 3 shows a plot of the log of conductivity versus reciprocal temperature for these boron electrolyte solutions.
• Fig. 3 indicates that the highest ambient temperature conductivities corresponded to the 0.5 or l.OM boron electrolyte solutions, which show conductivities of IO "38 Sem 1 .
• Fig. 3 further showed that the conductivity of the 0.5 and l.OM solutions remained above 10 "5 Sem "1 down to 0°C.
• a 2.5M LiC10 4 solution in 1:2 Mix BEG-l:EC was prepared by dissolving an appropriate amount of LiC10 4 in a 1:2 Mix BEG-L:EC boron electrolyte solvent mixture prepared in accordance with Example 7.
• a 1.0M LiC10 4 solution was prepared by dissolving LiC10 4 in a
• a 3.IM LiCl0 4 solution was prepared by dissolving an appropriate amount of LiC10 4 in EC. All materials were weighed out in a glove box.
• Fig. 5 shows an overlay of three cyclic voltammograms for these three electrolyte solutions. Fig. 5 shows that the electrochemical window was much wider for the 1:2 Mix BEG-l:EC solvent than for the dimethyl ether/EC solvent or the EC solvent.
• a l.OM LiC10 4 boron electrolyte solution in 1:2 Mix BEG-l:PC was prepared by dissolving an appropriate amount of LiC10 4 in a 1:2 Mix BEG-l:PC boron electrolyte solvent mixture prepared in accordance with Example 7.
• a l.OM LiC10 4 :PC solution was prepared by dissolving an appropriate amount of LiC10 4 in PC.
• Fig. 6 shows an overlay of two cyclic voltammograms for these two electrolyte solutions. Fig. 6 shows that the PC solution began to decompose at about 4.5 volts positive with respect to Li + /Li. However the boron electrolyte solution did not begin to decompose until about 5.6 volts positive with respect to LiVLi-
• LiCl0 4 , LiN(S0 2 CF 3 ) 2 and LiS0 3 CF 3 were prepared by dissolving appropriate quantities of these salts in 1:2
• Fig. 5 shows that an electrochemical decomposition process attributed to EC began at +1 volts with respect to a platinum pseudo-reference electrode.
• Fig. 10 shows that the onset of the electrochemical decompo- sition process attributed to EC was not affected by
• BEG-3-containing boron electrolyte solutions but was not observed until more positive voltages than +1 volts were applied to BEG-2-containing, BEG-4-containing and BEG-l-containing boron electrolyte solutions. Most remarkably, decomposition attributed to EC was completely suppressed in BEG-l-containing boron electrolyte solutions.
• Electrolytes must exhibit rubbery behavior to be useful in solid state electrochemical devices. Rubbery behavior may be imparted to a boron electrolyte solution by adding a high molecular weight polymer.
• a 1.3M LiC10 4 boron electrolyte solution was prepared by dissolving LiC10 4 in a 1:2 Mix BEG-l:EC solvent mixture prepared according to Example 7.
• a gel electrolyte was similarly prepared by further adding 20% polyvinyl acetate (molecular weight of about 50,000) respectively.
• Fig. 7 is an overlay plot of log conductivity versus reciprocal temperature which compares the conductivity of the gel electrolyte to the reference boron electrolyte solution which does not contain the polymer.
• Fig. 7 shows that the addition of 20 weight percent polyvinyl acetate somewhat reduced the room temperature conductivity of the solution. However, it is likely that higher conductivities could have been achieved by adding a smaller percentage of higher molecular weight polymer.
• Another electrolyte solution was prepared by adding 5 percent polyethylene oxide (MW about 10 8 ) to the above-described 1.3 M LiC10 4 boron electrolyte solution.
• the resultant composition was a high stretch rubbery material which may be useful as an electrolyte for solid state electrochemical devices.
• a polymer oil was generated by reacting BEG-l prepared according to example 3 with tetramethyl ortho ⁇ silicate. Specifically, 4.88 grams (0.02 mole) of BEG-l and 0.608 grams (0.004 mole, Aldrich, 99+%) of tetramethyl orthosilicate were sealed in a strong vial, and heated at 250°C overnight. As a result, a polymer oil with a somewhat complicated structure was obtained. This oil may be used as a solvent for non-aqueous electrolytes.
• a polymeric borate compound according to the following formula was synthesized O B O R
• a voltaic cell was formed using a Li foil anode and a cathode made from LiMn 2 0 4 , carbon black, and a binder, separated by a gel electrolyte containing 2.5M
• a Rechargeable Li Battery Incorporating a Boron Electrolyte Solution A voltaic cell was formed using a carbon anode and a LiCo0 2 cathode, separated by a gel electrolyte containing l.OM LiC10 4 dissolved in 1:2 Mix BEG-LiEC electrolyte and 20 weight percent poly (methyl methacrylate) .
• a composite cathode was prepared by mixing LiCo0 2 (Alpha, 98%) , carbon black, and the above described gel electrolyte in weight ratios of 72:8:20, respectively. The resulting slurry was pressed onto Ni foil.
• the carbon anode was constructed from 80 weight percent carbon and 20 weight percent boron electrolyte gel used as a binder.
• the assembled battery was charged, and then cycled between, 2.5 and 4.4 volts. As shown in Fig. 13, after 14 cycles, the cycling voltage limit was increased to 4.5 volts. The cell continued to cycle reversibly, and showed a significant increase in capacity

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• 1996
  • 1996-11-01 JP JP9517555A patent/JPH11514790A/ja active Pending
  • 1996-11-01 AU AU77198/96A patent/AU7719896A/en not_active Abandoned
  • 1996-11-01 WO PCT/US1996/017490 patent/WO1997016862A1/en not_active Application Discontinuation

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