Abstract:
An electrolyte comprising at least one organic aprotic solvent, at least one salt and at least one chelatoborate additive. A method of forming an SEI layer in a cell comprising a positive electrode, a negative electrode and an electrolyte, said method comprising the step of overcharging the electrolyte prior to fabricating the cell, or said cell during the formation cycle.

Description:
[0001]     This Application is a continuation in part of application Ser. No. 11/300,287, filed on Dec. 15, 2005. application Ser. No. 11/300,287 claims the benefit of Provisional Application No. 60/642,815, filed Jan. 11, 2005. The disclosure of foregoing applications is hereby incorporated by reference. 
     
    
     STATEMENT REGARDING FEDERALLY SPONSORED RESEARCH OR DEVELOPMENT  
       [0002]     The Government has rights in this invention pursuant to Agreement 85N14 between the Argonne National Laboratory and Air Products And Chemicals, Inc. 
     
    
     BACKGROUND OF THE INVENTION  
       [0003]     Lithium and Lithium-ion secondary batteries, by virtue of the large reduction potential and low molecular weight of elemental lithium, offer a dramatic improvement in power density over existing primary and secondary battery technologies. Lithium secondary batteries are batteries containing metallic lithium as the negative electrode. Lithium ion secondary batteries contain a lithium ion host material as the negative electrode. By “secondary battery” it is meant a battery that provides for multiple cycles of charging and discharging with minimal capacity fade. The small size and high mobility of lithium cations allow for the possibility of rapid recharging. These advantages make lithium ion batteries ideal for portable electronic devices, e.g., cell phones and laptop computers. Recently, larger size lithium ion batteries have been developed and have application for use in automotive applications including the hybrid electric vehicle market.  
         [0004]     The following patents are representative of lithium batteries and electrochemical cells:  
         [0005]     U.S. Pat. No. 4,201,839 discloses electrochemical cells based upon alkali metal-containing anodes, solid cathodes, and electrolytes where the electrolytes are closoborane compounds carried in aprotic solvents.  
         [0006]     U.S. Pat. No. 5,849,432 discloses electrolyte solvents for use in liquid or rubbery polymer electrolyte solutions based upon boron compounds with Lewis acid characteristics, e.g., boron linked to oxygen, halogen atoms, and sulfur.  
         [0007]     U.S. Pat. No. 6,346,351 discloses secondary electrolyte systems for a rechargeable battery of high compatibility towards positive electrode structures based upon a salt and solvent mixture. Lithium tetrafluoroborate and lithium hexafluorophosphate are examples of salts.  
         [0008]     U.S. Pat. No. 6,159,640 discloses electrolyte systems for lithium batteries used in electronic equipment such as mobile phones, laptop computers, camcorders, etc based upon fluorinated carbamates.  
         [0009]     U.S. Pat. No. 6,537,697 discloses a lithium secondary battery using a nonaqueous electrolyte including lithium tetrakis(pentafluorophenyl)borate as an electrolyte salt.  
         [0010]     (D. Aurbach, A. Zaban, Y. Ein-Eli, I. Weissman, O. Chusid, B. Markovsky, M. Levi, E. Levi, A. Schechter, E. Granot) and (S. Mori, H. Asahina, H. Suzuki, A. Yonei, K. Yokoto) describe the phenomenon of anode passivation by electrolyte reduction in lithium metal and lithium ion batteries using a carbon host anode material, and its cause of irreversible capacity loss at the graphite anode in lithium ion battery applications. In general, for graphitic carbons some reduction of both solvent and salt occurs at the graphite surface at low potentials during charging of the cell. This forms a electrode/electrolyte interface layer, sometimes referred to as a solid electrolyte interface (SEI) layer, which in some cases is stable and prevents further capacity loss and in other cases is unstable. The layer is comprised of solvent and salt decomposition products. Use of ethylene carbonate as one of the cosolvents leads to stable passivation layers, while using high levels of propylene carbonate in the absence of ethylene carbonate leads to significant irreversible capacity loss due to exfoliation of the graphite.  
         [0011]     U.S. Pat. No. 5,626,981 describes the use of a small amount of vinylene carbonate to improve the passivation layer formed by ethylene carbonate (EC) and EC/propylene carbonate (PC) based solvents with standard electrolyte salts. The final reversible capacity is improved slightly with this additive.  
         [0012]     U.S. Pat. No. 5,571,635 discloses that high reversible capacity over multiple charge/discharge cycles is not obtainable in solvent systems which are predominantly propylene carbonate. Propylene carbonate, which is a desirable solvent because of its wide liquid range and high dielectric constant, gives continuous capacity fade by virtue of cointercalation/exfoliation reactions. This patent describes the use of chloroethylene carbonate as a cosolvent with propylene carbonate, which acts to form stable passivation films on crystalline graphites when used with standard electrolyte salts, such as LiPF 6 , LiBF 4 , lithium bis-oxalatoborate (LiBOB), LiCF 3 SO 3 , etc. It describes the use of chloroethylene carbonate as an additive for reducing irreversible capacity loss with ethylene carbonate/propylene carbonate solvent mixtures.  
         [0013]     The disclosure of the previously identified patents and publications is hereby incorporated by reference.  
         [0014]     A key challenge to the reversibility of cells has been the reactivity of the electrolyte solution components (salt and solvent); especially under the charging conditions. Heretofore, it has been observed that all electrolyte salts and solvents undergo some reduction at the negative electrode during at least the initial charging step. This reduction can either lead to a stable, conducting passivation layer or film also referred to as a Solid Electrolyte Interface or SEI layer, or reduction can continue with charge/discharge cycling eventually leaving no reversible capacity in the negative electrode.  
       BRIEF SUMMARY OF THE INVENTION  
       [0015]     The instant invention solves problems associated with conventional reversible or rechargeable cells employed in lithium secondary batteries by providing an electrolyte that provides a suitable SEI layer. The present invention can also provide an electrolyte which imparts improved thermal stability to lithium ion batteries compared to conventional electrolytes for lithium ion batteries. By thermal stability, it is meant that a battery retains at least about 80% of its original capacity while being cycled between charge and discharge conditions at a temperature of about 50° C. or greater.  
         [0016]     The invention further provides improved cell stability on overcharge  
         [0017]     This invention further provides an electrolyte as described above further comprising at least one additive.  
         [0018]     This invention further provides an electrolyte as described above where the additive selected from the chelato-borate salts.  
         [0019]     This invention further provides an electrolyte as described above where the additive comprises at least one lithium difluorooxalatoborate.  
         [0020]     The invention further provides a cell comprising a positive electrode, a negative electrode and an electrolyte, said electrolyte providing better high temperature charge/discharge cycling stability than conventional electrolytes for lithium ion batteries.  
         [0021]     This invention further provides electrolytes or cells as described above further comprising lithium.  
         [0022]     This invention further provides electrolytes or cells comprising lithium of the formula: 
 
Li a Q 
 
 where Q comprises a monovalent or divalent borate or heteroborate cluster anion, a may be 1 or 2.
 
     
    
     BRIEF DESCRIPTION OF THE DRAWINGS  
       [0023]      FIG. 1  shows the voltage profile of an MCMB anode/Li 1.1 [Mn 1/3 Ni 1/3 Co 1/3 ] 0.9 O 2  cathode lithium ion cell during an  8 C-rate pulse overcharge experiment. The electrolyte was 1.2M LiPF 6  in EC/PC/DMC (1:1:3 by weight). MCMB refers to a synthetic graphite negative electrode material with a meso-carbon-micro-bead composite structure.  
         [0024]      FIG. 2  shows the voltage profile of a MCMB/Li 1.1 [Mn 1/3 Ni 1/3 Co 1/3 ] 0.9 O 2  lithium ion cell during an 8 C-rate pulse overcharge experiment. The electrolyte was 0.8 M LiB(C 2 O 4 )—LiBOB in EC/PC/DMC (1:1:3 by weight).  
         [0025]      FIG. 3  shows the voltage profile of a MCMB/Li 1.1 [Mn 1/3 Ni 1/3 Co 1/3 ] 0.9 O 2  lithium ion cell during an 8 C-rate pulse overcharge experiment. The electrolyte was 0.4 M Li 2 B 12 F 9 H 3  in EC/PC/DMC (1:1:3 by weight).  
         [0026]      FIG. 4  shows the voltage profile of a MCMB/Li 1.1 [Mn 1/3 Ni 1/3 Co 1/3 ] 0.9 O 2  lithium ion cell during an 8 C-rate pulse overcharge experiment. The electrolyte was 0.4 M Li 2 B 12 F 9 H 3  in EC/PC/DMC (1:1:3 by weight) with 2 wt. % LiBF 2 (C 2 O 4 )—LiDFOB as an additive.  
         [0027]      FIG. 5  shows the voltage profile of a MCMB/LiMn 2 O 4  lithium ion cell during an 1 C-rate pulse overcharge experiment. The electrolyte was 1.2M LiPF 6  in EC/PC/DMC (1:1:3 by weight).  
         [0028]      FIG. 6  shows the voltage profile of a MCMB/LiMn 2 O 4  lithium ion cell during an 1 C-rate pulse overcharge experiment. The electrolyte was 0.7M LiBOB in EC/PC/DMC (1:1:3 by weight).  
         [0029]      FIG. 7  shows the voltage profile of a MCMB/LiMn 2 O 4  lithium ion cell during an 5 C-rate pulse overcharge experiment. The electrolyte was 0.4 M Li 2 B 12 F 9 H 3  in EC/PC/DMC (1:1:3 by weight) with 2 wt. % LiBF 2 (C 2 O 4 )—LiDFOB as an additive.  
         [0030]      FIG. 8  shows the nominal capacity retention of MCMB/Li 1.1 [Mn 1/3 Ni 1/3 Co 1/3 ] 0.9 O 2  (L333) lithium ion cells cycled at 55° C. with a constant current of C/2, or 1.2 mA. The electrolyte used for the control cell was 1.2M LiPF 6  in EC/PC/3DEC by weight. The electrolyte used for the other cell was 0.4 M Li 2 B 12 F 9 H 3  in 3EC/7EMC (by weight) with 2 wt. % LiBF 2 (C 2 O 4 ) as an additive.  
         [0031]      FIG. 9  shows the electrochemical impedance spectra of MCMB/Li 1.1 [Mn 1/3 Ni 1/3 Co 1/3 ] 0.9 O 2  (L333) lithium-ion cells that were constant-voltage charged to 3.8 V with 0.4 M Li 2 B 12 F 9 H 3  in 3EC/7EMC (by weight) with different additive levels of LiBF 2 (C 2 O 4 ) as the electrolyte.  
         [0032]      FIG. 10  shows shows the area specific impedance of MCMB/Li 1.1 [Mn 1/3 Ni 1/3 Co 1/3 ] 0.9 O 2  (L333) lithium-ion cells with 0.4 M Li 2 B 12 F 9 H 3  in 3EC/7EMC (by weight) with different additive levels of LiBF 2 (C 2 O 4 ) as the electrolyte.  
         [0033]      FIG. 11  shows shows the discharge capacity retention of MCMB/Li 1.1 [Mn 1/3 Ni 1/3 Co 1/3 ] 0.9 O 2  (L333) lithium-ion cells cycled at 55° C. with a constant current of 1.0 mA, or C/2. The electrolytes used were 0.4 M Li 2 B 12 F 9 H 3  in 3EC/7EMC (by weight) with different levels of LiBF 2 (C 2 O 4 ) as an additive.  
         [0034]      FIG. 12  shows shows the discharge capacity retention of MCMB/Li 1.1 [Mn 1/3 Ni 1/3 Co 1/3 ] 0.9 O 2  (L333) lithium-ion cells cycled at 55° C. with a constant current of 1.0 mA, or C/2. The electrolyte used for the control cell was 1.2 M LiPF 6  in 3EC/7EMC (by weight). The electrolyte of the invention used in the other cell was 0.4 M Li 2 B 12 F 12  in 3EC/7EMC (by weight) with 2 wt. % LiBF 2 (C 2 O 4 ) as an additive.  
         [0035]      FIG. 13  shows shows the discharge capacity of carbon/LiMn 2 O 4  lithium-ion cells cycled at 55° C. with a constant current of 1 C, or 250 mA. The electrolyte used for the control cell was 1.2 M LiPF 6  in 3EC/7EMC (by weight). The electrolyte of the invention used in the other cell was 0.4 M Li 2 B 12 F 12  in 3EC/7EMC (by weight) with 2 wt. % LiBF 2 (C 2 O 4 ) as an additive. 
     
    
     CROSS REFERENCE TO RELATED PATENTS AND PATENT APPLICATIONS  
       [0036]     The instant invention is related to U.S. patent application Ser. No. 10/655,476, filed Sep. 04, 2003; Ser. No. 10/910,529, filed Aug. 03, 2004; Ser. No. 10/924,293, filed Aug. 23, 2004; Ser. No. 11/097,810, filed Apr. 01, 2005 and U.S. Pat. No. 6,781,005. The disclosure of the previously identified patents and patent application is hereby incorporated by reference.  
       DETAILED DESCRIPTION OF THE INVENTION  
       [0037]     A secondary battery or cell capable of multiple cycles of charging and discharging, is dependent on an electrolyte carrying ions. The term electrolyte may refer to an electrolyte salt, electrolyte salt in a solvent, an electrolyte salt in a polymer or gel or an electrolyte salt in an ionic liquid or a fully formulated electrolyte within a battery. In cells having a full-charge potential of greater than 2V, electrolyte salts and solutions for such cells should provide: (a) a relatively high conductivity in a non-aqueous ionizing solution, (b) chemical stability to heat, e.g. cell temperatures of &gt;50° C., preferably &gt;80° C. and more preferably &gt;100° C., and stability toward hydrolysis and/or HF generation in the presence of water or alcohols, and electrochemical cycling over a wide potential range, e.g., 3 to 3.6V, preferably 3 to 4.2 V and more preferably 3 to &gt;4.2V, and/or (c) an ability of the electrolyte and/or additives therein to form a stable, passivating ion conducting interfacial or SEI layer at the electrode/electrolyte interface.  
         [0038]     A battery may comprise one or more electrochemical cells; however the terms battery and cell may be used interchangeably herein to mean a cell. Any reference to a voltage herein refers to voltage versus the lithium/lithium +  (Li/Li + ) couple.  
         [0039]     The electrolyte of this invention comprises at least one salt that is chemically very stable, not readily reduced and/or will not provide electrochemical passivation (passivation is achieved in the instant invention by the employing the compositions described herein). Electrochemical passivation is a process which results in the formation of a film on an electrode surface, which limits further reactivity of the electrolyte with the electrode. If passivation does not occur then the cell will undergo continuous capacity fade as active lithium in the negative electrode reacts with the electrolyte on each charging cycle.  
         [0040]     The salt can be any salt or mixture of salts. In one embodiment, the salt comprises lithium. In another embodiment, the salt comprises a lithium salt of the formula: 
 
Li a Q 
 
 where Q comprises a monovalent or divalent borate or heteroborate cluster anion, and a is 1 or 2. The group Q comprises at least one member selected from the following borate (i) and heteroborate (ii and iii) anions: 
        i) The closo-borate anion compositions of formula (B n Z n ) 2− , where Z comprises F, H, Cl, Br, and/or (OR), where R comprises H, C 1-8 , preferably C 1-3  alkyl or fluoroalkyl, and n is 8 to 12. The compositions are polyhedral clusters consisting of eight to twelve boron atoms where each boron is attached as defined to a hydrogen, a halogen atom or hydroxyl group.     ii) The closo-ammonioborate anion compositions of formula: 
 
((R′R″R′″)NB n Z n-1 ) 1− ; 
    where N is bonded to B and each of R′, R″, and R′″ is independently selected from the group consisting of hydrogen, alkyl, aryl and/or a polymer, Z comprises F, H, Cl, Br, and/or (OR), where R comprises H, alkyl, fluoroalkyl or aryl; and n is 8 to 12. These anion compositions are also polyhedral boron clusters of 8 to 12 boron atoms, where one of the boron atoms is attached to an ammonia group (NR′R″R′″), with F, H, Cl, Br and OR groups attached to the remaining boron atoms. A description of these compositions may be found in U.S. Pat. No. 6,335,466 B1;        
 
         [0044]     incorporated herein by reference. The alkyl, and fluoroalkyl groups may be branched, cyclic or straight-chained groups having 1 to 20 carbon atoms, and if fluorinated may have 1 to 42 fluorine atoms. The term aryl refers to aromatic ring systems, usually containing 5 to 20 ring atoms. Polymers can comprise at least one member selected from the group consisting of polystyrene, polyethylene, polyethylene glycol, among others, which allow the anions to be bound to a polymeric support. 
        iii) The closo-monocarborate anion compositions of formula: (R″″CB n Z n ) 1− , where R″″ is bonded to C and selected from the group consisting of hydrogen, alkyl, cycloalkyl, aryl, and a polymer; Z comprises F, H, Cl, Br, and/or (OR), where R comprises H, alkyl or fluoroalkyl; and n is 7 to 11. These fluorinated closo-monocarborate anion compositions are also polyhedral clusters that comprise 7-11 boron atoms and a single carbon atom. Such anion compositions are described in U.S. Pat. No. 6,130,357; incorporated herein by reference. The alkyl, and fluoroalkyl groups may comprise branched, cyclic or straight-chained groups having 1 to 20 carbon atoms, and if fluorinated will have 1 to 42 fluorine atoms. The term aryl refers to aromatic ring systems, typically containing 5 to 20 ring atoms. Polymers comprise at least one member selected from the group consisting of polystyrene, polyethylene, polyethylene glycol, among others, which allow the anions to be bound to a polymeric support.        
 
         [0046]     Examples of lithium salts that can comprise the electrolyte salt of this invention are lithium fluoroborates represented by the formulas: 
 
Li 2 B 10 F x Z 10-x  
 
and 
 
Li 2 B 12 F x Z 12-x  
 
 wherein x is at least 1, or at least 3 for the decaborate salt, or at least 5, or at least 6, or at least 8 but less than or equal to 12, for the dodecaborate salts. Z represents H, Cl, Br, or OR, where R═H, C 1-8 , typically C 1-3  alkyl or fluoroalkyl. Useful compounds are Li 2 B 12 F 12 , and mixtures of Li 2 B 12 F x Z 12-x  where x is 6, 7, 8, 9, 10, 11 and 12. 
 
         [0047]     Specific examples of lithium fluoroborate compounds comprise at least one member selected from the group consisting of Li 2 B 12 F 8-12 Z 0-4  where Z comprises Cl, Br, or OR where R comprises C 1-8 , usually C 1-3 . Typically, the salts comprise at least one member selected from the group consisting of Li 2 B 10 F 10 , Li 2 B 12 F 12 , Li 2 B 12 F 10-12 (OH) 0-2 , Li 2 B 12 F 10-12 (Cl) 2 , Li 2 B 12 F 8-10 (H) 0-2 , Li 2 B 12 F 8-12 (OCF 3 ) 0-4 , and Li 2 B 10 F 8-10 Br 0-2 .  
         [0048]     The electrolyte further comprises a solvent or carrier, referred to collectively as solvent, to provide an electrolyte solution. The solvent or carrier may be an aprotic polar organic solvent. Typically, these aprotic solvents are anhydrous, forming anhydrous electrolyte solutions. By “anhydrous” it is meant that the solvent or carrier as well as the electrolyte comprises less than about 1,000 ppm water and normally less than about 500 to 100 ppm. Examples of aprotic organic solvents or carriers for forming the electrolyte solutions comprise at least one member selected from the group consisting of organic carbonates, such as ethylene carbonate (EC), propylene carbonate (PC), dimethyl carbonate (DMC), ethyl methyl carbonate (EMC), diethyl carbonate (DEC), methyl propyl carbonate (MPC), ethyl propyl carbonate (EPC), dipropyl carbonate (DPC), bis(trifluoroethyl)carbonate, bis(pentafluoropropyl)carbonate, trifluoroethyl methyl carbonate, pentafluoroethyl methyl carbonate, heptafluoropropyl methyl carbonate, perfluorobutyl methyl carbonate, trifluoroethyl ethyl carbonate, pentafluoroethyl ethyl carbonate, heptafluoropropyl ethyl carbonate, perfluorobutyl ethyl carbonate, etc., esters, such as gamma butyrolactone, methyl acetate, methyl propionate, methyl butyrate, among others, ethers such as dimethyl ether, or glymes, fluorinated oligomers, dimethoxyethane, tetraethyleneglycol, polyethylene glycols, sulfones, and gamma-butyrolactone (GBL). The solvent or carrier can also comprise at least one ionic liquid. By ionic liquid it is meant any room temperature molten salt. Examples of suitable ionic liquids comprise at least one member selected from the group consisting of asymmetric tetraalkyl ammonium salts of weakly coordinating anions such as butyl-trimethylammonium tetrafluoroborate, hexyl-trimethylammonium trifluoromethanesulfonimide, N-alkylpiperidium salts of weakly coordinating anions including N-methyl piperidinium tetrafluoroborate, N-ethylpiperidinium trifluoromethane sulfonate, N-butyl piperidinium trifluoromethanesulfonimide, among others, including those which do not contain active or reducible hydrogens in the cation of the liquid. The amount of any given solvent component in an electrolyte formulation normally ranges from about 5% to about 95 wt % of the electrolyte.  
         [0049]     In another embodiment, the electrolyte of the present invention can comprise an aprotic gel polymer carrier/solvent. Suitable gel polymer carrier/solvents can comprise at least one member selected from the group consisting of polyethers, polyethylene oxides, polyimides, polyphosphazines, polyacrylonitriles, polysiloxanes, polyether grafted polysiloxanes, derivatives of the foregoing, copolymers of the foregoing, crosslinked and network structures of the foregoing, blends of the foregoing, among others, to which is added an appropriate ionic electrolyte salt. Other gel-polymer carrier/solvents can comprise those prepared from polymer matrices derived from at least one member selected from the group consisting of polypropylene oxides, polysiloxanes, sulfonated polyimides, perfluorinated membranes (Nafion™ resins), divinyl polyethylene glycols, polyethylene glycol-bis-(methyl acrylates), polyethylene glycol-bis(methyl methacrylates), derivatives of the foregoing, copolymers of the foregoing, crosslinked and network structures of the foregoing. The aprotic gel polymer carrier may contain any of the aprotic liquid carriers described in the preceding paragraph.  
         [0050]     If the electrolyte comprises the electrolyte salt in a solution, typically the concentration of salt will be from about 0.05 to about 2 molar or from about 0.1 to about 1.2 molar, or from about 0.2 to about 0.5 molar. Higher concentrations tend to become too viscous and, the bulk conductivity characteristics of a cell using the electrolyte may be adversely affected.  
         [0051]     The electrolyte salts of this invention have been shown to provide overcharge protection as described in US 20050227143A1; hereby incorporated by reference, which is an advantage in use in lithium ion batteries. The chemical stability of the salts in the electrolytes of this invention, for example, Li 2 B 12 F 12  and Li 2 B 12 F 9 H 3 , which also makes them desirable as electrolyte salts for battery applications, may prevent their participation in reductive passivation chemistry. When standard formation charging cycle(s) are used, a stable passivation film is not formed by the salts or solutions of these salts, e.g., such as described in U.S. Pat. No. 6,346,351; hereby incorporated by reference. Formation cycle(s) are the initial charge/discharge cycle or cycles of an assembled cell designed to form the SEI layer, and otherwise conditioning the cell for use. Typically, the charge/discharge formation cycle(s) is(are) performed at a slower rate than the charge/discharge rate under the normal operating conditions of the cell. The optimum conditions of the formation cycle can be determined experimentally for each electrolyte and battery. The term “formation cycle” will be used herein to mean either one or more than one charge/discharge cycle to form the SEI layer. Without a stable SEI layer, the cell typically undergoes continual capacity fade on charging and discharging. We have found that if the electrolytes of formula (1) are combined with small amounts of another salt(e.g., to form an enhanced SEI layer), the charge/discharge cycle life of cells using this electrolyte can be improved over standard electrolytes, particularly at cell temperatures &gt;50° C. Thus a cell which has better stability at elevated temperature and under overcharging conditions can be designed if the electrolytes of this invention are used.  
         [0052]     In one embodiment of this invention, the electrolyte further comprises such an SEI forming salt as an additive to aid passivation layer (SEI layer) formation. The additive can function to form a stable passivation layer. The passivation layer may contain reduction products of the solvent, and/or additive, and/or electrolyte salt. The additive will typically be an organic material, inorganic salt or mixtures thereof.  
         [0053]     Additives that are organic compounds that can function to form the passivation layer can comprise at least one member selected from the group consisting of chloroethylene carbonate, vinylene carbonate (VC), vinylethylenecarbonate (VEC), and non-carbonate species such as ethylene sulfite, propane sulfone, propylene sulfite, as well as substituted carbonates, sulfites and butyrolactones, such as phenylethylene carbonate, phenylvinylene carbonate, catechol carbonate, vinyl acetate, vinylethylene carbonate, dimethyl sulfite, fluoroethylene carbonate, trifluoropropylene carbonate, bromo gamma-butyrolactone, fluoro gamma-butyrolactone, among others which provide organic salts on reduction at the at least one electrode, particularly the negative electrode.  
         [0054]     Additives that are inorganic compounds or salts that may be useful in this invention can comprise at least one compound containing boron, phosphorous, sulfur or fluorine, among others. Additives that are useful in this embodiment of the invention can comprise at least one member selected from the group consisting of lithium chelato-borate salts (e.g., Li difluorooxalatoborate, LiBF 2 (C 2 O 4 ) or LiDFOB, LiB(C 2 O 3 CF 3 ) 2 , LiBF 2 (C 2 O 3 CF 3 ), and LiB(C 3 H 2 O 3 (CF 3 ) 2 ) 2 as described in U.S. Pat. No. 6,407,232, EP 139532B1 and JP2005032716 A; hereby incorporated by reference). Examples of suitable additives and methods for making these additives are also described in U.S. Pat. Nos. 6,783,896 and 6,849,752; both hereby incorporated by reference.  
         [0055]     For a lithium containing electrolyte, the passivation layer (SEI layer) formed by the additives listed herein may comprise lithium alkyl carbonates and Li 2 CO 3  (from the electrolyte solvent/organic additive reduction), LiF, and salt reduction products, including the reduction products of the oxalatoborate salts with the solvents (e.g., B(OCO 2 R) 3 , where R is a lithium alkyl carbonate salt derived from solvent oxidation). The SEI layer will typically be about 5 nm to about 1000 nm in thickness. The SEI layer can be formed upon the negative electrodes described herein. While the SEI layer will normally be formed in situ upon the negative electrode, if desired, the negative electrode can be pre-treated with the SEI layer composition.  
         [0056]     The additive can be present in the electrolyte in an amount which forms an effective SEI layer. In some embodiments, the additive may be present in an amount between about 0.1 and about 5% of the total weight of the electrolyte. The battery or cell of this invention comprises any negative electrode and positive electrode, and the electrolyte of this invention. In one embodiment, the positive and negative electrodes of the battery are any using lithium containing materials, or materials that are capable of “hosting” ions in reduced or oxidized form, such as lithium. “Hosting” means that the material is capable of reversibly sequestering the ions, for example, lithium ions. The negative electrodes for the batteries of this invention can comprise at least one member selected from the group consisting of lithium metal, carbonaceous materials, such as amorphous carbon, including hard carbon or graphites (natural or artificial, including MCMB [available from Osaka Gas]), tin, tin oxide, silicon, or germanium compounds or metal oxides or derivatives of those materials (e.g., lithium titanate). The positive electrodes for use in batteries of this invention may be based upon a lithium composite oxide with a transition metal such as cobalt, nickel, manganese, mixtures thereof, among others, or a lithium composite oxide, part of whose lithium sites or transition metal sites is replaced with at least one member selected from the group consisting of cobalt, nickel, manganese, aluminum, boron, magnesium, iron, copper, or the like, or iron complex compounds such as iron phosphates and iron phosphosilicates. Specific examples of lithium composites for use as positive electrodes comprise at least one of lithium iron phosphate, LiFePO4, Li 1.1 [Mn 1/3 Ni 1/3 Co 1/3 ] 0.9 O 2 , LiNi 1-x Co x O 2  and lithium manganese spinel, LiMn 2 O 4 , LiNi 0.8 Co 0.15 Al 0.05 O 2 , LiCoO 2 , LiNiO 2 , LiNi 1-x-y Co x Mn y O 2    
         [0057]     The separator for the lithium battery can comprise a microporous polymer film. Examples of polymers for forming films comprise at least one member selected from the group consisting of nylon, cellulose, nitrocellulose, polysulfone, polyacrylonitrile, polyvinylidene fluoride, polypropylene, polyethylene, polybutene, mixtures thereof, among others. Ceramic separators, based on silicates, alumino-silicates, and their derivatives, among others, may also be used. Surfactants may be added to the separator or electrolyte to improve electrolyte wetting of the separator. Other components or compounds known to be useful in electrolytes or cells may be added.  
         [0058]     In one embodiment, the battery is comprised of a carbonaceous lithium ion hosting negative electrode, a positive electrode, a separator, and a lithium-based electrolyte salt carried in an aprotic solvent, gel polymer or polymer matrix. Examples of carbonaceous negative electrodes include graphites.  
         [0059]     In another embodiment, the battery comprises an electrolyte comprising a polar organic solvent, a salt comprising Li 2 B 12 F x Z 12-x  wherein x is at least 5 but less than or equal to 12 and Z represents H, Cl, or Br; an LiBF 2 (C 2 O 4 ) additive, an anode comprising graphite or hard carbon, and a cathode comprising Li 1.1 [Mn 1/3 Ni 1/3 Co 1/3 ] 0.9 O 2 , or doped or undoped LiMn 2 O 4 . This battery can have a suitable SEI layer as well as thermal stability.  
         [0060]     The electrolytes of this invention, together with additives which form stable SEI layers, such as LiBF 2 (C 2 O 4 ), can provide very stable cell performance at elevated temperature, such that the charge/discharge capacity retention at &gt;50° C. remains &gt;than 80% for more than twice as many cycles as cells based on standard LiPF 6  electrolytes. The electrolytes of this invention can be employed in a wide range of electrochemical devices including secondary batteries, capacitors, hybrid capacitors, fuel cells and electrolyzers among other applications.  
         [0061]     The following examples are intended to illustrate various embodiments of the invention and do not limit the scope of the claims appended hereto.  
       EXAMPLES  
     Control Example 1a  
       [0062]      FIG. 1  shows the cell voltage of a MCMB/Li 1.1 [Mn 1/3 Ni 1/3 Co 1/3 ] 0.9 O 2  (L333) lithium-ion cell that was pulse-overcharged. The electrolyte used was 1.2 M LiPF 6  in EC/PC/DMC (1:1:3 by weight, EC stands for ethylene carbonate, PC stands for propylene carbonate, and DMC stands for dimethyl carbonate.). The cell was pulse-overcharged at an 8 C rate (20 mA) for 18 seconds every 60 minutes.  FIG. 1  clearly shows that the cell voltage steadily increased with the number of pulse current applied. Only in 4 pulses, the peak voltage of the cell increased to 4.95 V, which is high enough to trigger the decomposition of the positive electrode and the non-aqueous electrolytes.  
       Control Example 1b  
       [0063]      FIG. 2  shows the cell voltage of a MCMB/Li 1.1 [Mn 1/3 Ni 1/3 Co 1/3 ] 0.9 O 2  (L333) lithium-ion cell that was pulse-overcharged. The electrolyte used was 0.8 M LiBOB in EC/PC/DMC (1:1:3 by weight). The cell was pulse-overcharged at an 8 C rate (20 mA) for 18 seconds every 60 minutes.  FIG. 2  clearly shows that the cell voltage steadily increased with the number of pulse current applied. Only in 4 pulses, the peak voltage of the cell increased to 4.95 V, which is high enough to trigger the decomposition of the positive electrode and the non-aqueous electrolytes.  
       Control Example 1c  
       [0064]      FIG. 3  shows the cell voltage of a MCMB/Li 1.1 [Mn 1/3 Ni 1/3 Co 1/3 ] 0.9 O 2  (L333) lithium-ion cell that was pulse-overcharged. The electrolyte used was 0.4 M Li 2 B 12 F 9 H 3  (AP-F9) in EC/PC/DMC (1:1:3 by weight). The cell was pulse-overcharged at an 8 C rate (20 mA) for 18 seconds every 60 minutes.  FIG. 3  clearly shows that the salt AP-F9 has the redox shuttle capability to carry charge through the lithium-ion cell and hence improve the pulse overcharge tolerance of the cell.  
       Example 1  
       [0065]      FIG. 4  shows the cell voltage of a MCMB/Li 1.1 [Mn 1/3 Ni 1/3 Co 1/3 ] 0.9 O 2  (L333) lithium-ion cell that was pulse-overcharged. The electrolyte used was 0.4 M Li 2 B 12 F 9 H 3  (AP-F9) in EC/PC/DMC (1:1:3 by weight) with 2 wt % lithium difluoro(oxalato)borate (LiDFOB). The cell was pulse-overcharged at an 8 C rate (20 mA) for 18 seconds every 60 minutes for 100 pulses.  FIG. 4  clearly shows that the cell comprising 0.4 M AP-F9 and 2.0 wt % LiDFOB as the additive had excellent pulse overcharge tolerance. The cell voltage was stabilized at about 4.8 V after the overcharge pulses.  
       Control Example 2a  
       [0066]      FIG. 5  shows the cell voltage of a MCMEI/LiMn 2 O 4  lithium-ion cell that was pulse-overcharged. The electrolyte used was 1.2 M LiPF 6  in EC/PC/DMC (1:1:3 by weight). The cell was pulse-overcharged at a 1 C rate (1 mA) for 18 seconds every 60 minutes.  FIG. 5  clearly shows that the cell voltage steadily increased with the number of pulse current applied. In 25 pulses, the peak voltage of the cell increased to 4.95 V, which is high enough to trigger the decomposition of the positive electrode and the non-aqueous electrolytes.  
       Control Example 2b  
       [0067]      FIG. 6  shows the cell voltage of a MCMB/LiMn 2 O 4  lithium-ion cell that was pulse-overcharged. The electrolyte used was 0.8 M LiBOB in EC/PC/DMC (1:1:3 by weight). The cell was pulse-overcharged at a 1 C rate (1 mA) for 18 seconds every 60 minutes.  FIG. 6  clearly shows that the cell voltage steadily increased with the number of pulse current applied. Only in 11 pulses, the peak voltage of the cell increased to 4.95 V, which is high enough to trigger the decomposition of the positive electrode and the non-aqueous electrolytes.  
       Example 2  
       [0068]      FIG. 7  shows the cell voltage of a MCMB/LiMn 2 O 4  lithium-ion cell that was pulse-overcharged. The electrolyte used was 0.4 M Li 2 B 12 F 9 H 3  (AP-F9) in EC/PC/DMC (1:1:3 by weight) with 2 wt % lithium difluoro(oxalato)borate (LiDFOB). The cell was pulse-overcharged at a 5 C rate (5 mA) for 18 seconds every 60 minutes for 100 pulses.  FIG. 7  clearly shows that the cell comprising 0.4 M AP-F9 and 2.0 wt % LiDFOB as the additive had excellent pulse overcharge tolerance. The cell voltage was stabilized at about 4.7 V after the overcharge pulses.  
       Example 3  
     Cell Performance of a Conventional Electrolyte (1 M LiPF 6  in EC/PC/3DMC) vs. 0.4 M Li 2 B 12 F 9 H 3  in 3EC/7EMC  
       [0069]      FIG. 8  shows the nominal capacity retention of MCMB/Li 1.1 [Mn 1/3 Ni 1/3 Co 1/3 ] 0.9 O 2  (L333) lithium ion cells cycled at 55° C. with a current of C/2, or 1.2 mA. The electrolyte used for the control cell was 1.2M LiPF 6  in EC/PC/3DEC by weight. The electrolyte used for the other cell was 0.4 M Li 2 B 12 F 9 H 3  in 3EC/7EMC (by weight) with 2 wt. % LiBF 2 (C 2 O 4 ) as an additive. The cells with the electrolyte of this invention show improved capacity retention than that using the conventional electrolyte.  
       Example 4  
     Effect of LiBF 2 (C 2 O 4 ) as an Additive on the Electrochemical and Area Specific Impedances of Cells with 0.4 M Li 2 B 12 F 9 H 3  in 3EC/7EMC  
       [0070]      FIG. 9  shows the electrochemical impedance spectra of MCMB/Li 1.1 [Mn 1/3 Ni 1/3 Co 1/3 ] 0.9 O 2  (L333) lithium-ion cells that were constant-voltage charged to 3.8 V with 0.4 M Li 2 B 12 F 9 H 3  in 3EC/7EMC (by weight) with different additive levels of LiBF 2 (C 2 O 4 ) as the electrolyte.  FIG. 2  shows that the cell impedance initially decreased with the content of the added LiBF 2 (C 2 O 4 ) and the cell impedance remained almost unchanged when more than 1.5% LiBF 2 (C 2 O 4 ) was added. Similar results are seen in  FIG. 10  for area specific impedance tests of these cells. The area specific impedance initially decreased with the content of the added LiBF 2 (C 2 O 4 ) and the cell impedance remained almost unchanged when more than 1.5%.  
       Example 5  
     Cycling stability of MCMB/Li 1.1 [Mn 1/3 Ni 1/3 Co 1/3 ] 0.9 O 2  (L333) lithium-ion cells with electrolytes containing Li 2 B 12 F 12  and varying amounts of LiBF 2 (C 2 O 4 )  
       [0071]      FIG. 11  shows the discharge capacity retention of MCMB/Li 1.1 [Mn 1/3 Ni 1/3 Co 1/3 ] 0.9 O 2  (L333) lithium-ion cells cycled at 55° C. with a constant current of 1.0 mA, or C/2. The electrolytes used were 0.4 M Li 2 B 12 F 9 H 3  in 3EC/7EMC (by weight) with different levels of LiBF 2 (C 2 O 4 ) as an additive.  FIG. 11  shows that &gt;1% LiBF 2 (C 2 O 4 ) is useful as an additive to achieve good capacity retention with Li 2 B 12 F 9 H 3 .  
       Example 6  
     Cell Performance of a Conventional Electrolyte (1.2 M LiPF 6  in 3EC/7EMC) vs. 0.4 M Li 2 B 12 F 12  in 3EC/7EMC  
       [0072]      FIG. 12  shows the discharge capacity retention of MCMB/Li 1.1 [Mn 1/3 Ni 1/3 Co 1/3 ] 0.9 O 2  (L333) lithium-ion cells cycled at 55° C. with a constant current of 1.0 mA, or C/2. The electrolyte used for the control cell was 1.2 M LiPF 6  in 3EC/7EMC (by weight). The electrolyte of the invention used in the other cell was 0.4 M Li 2 B 12 F 12  in 3EC/7EMC (by weight) with 2 wt. % LiBF 2 (C 2 O 4 ) as an additive. The cells with the electrolyte of this invention show improved initial discharge capacity and capacity retention than that using the conventional LiPF 6 -based electrolyte.  
       Example 7  
     Cell Performance of a Conventional Electrolyte (1.2 M LiPF 6  in 3EC/7EMC) vs. 0.4 M Li 2 B 12 F 12  in 3EC/7EMC  
       [0073]      FIG. 13  shows the discharge capacity of carbon/LiMn 2 O 4  lithium-ion cells cycled at 55° C. with a constant current of 1 C, or 250 mA. The electrolyte used for the control cell was 1.2 M LiPF 6  in 3EC/7EMC (by weight). The electrolyte of the invention used in the other cell was 0.4 M Li 2 B 12 F 12  in 3EC/7EMC (by weight) with 2 wt. % LiBF 2 (C 2 O 4 ) as an additive. The cells with the electrolyte of this invention show improved initial discharge capacity and capacity retention than that using the conventional LiPF 6 -based electrolyte.  
         [0074]     Examples 1a-2 show that the electrolytes of this invention can provide improved cell stability to lithium ion cells under conditions in which the cell are subjected to short overcharging events above the cells normal, upper operating potential.  
         [0075]     Examples 3-7 show that the electrolytes of this invention can provide improved cell charge/discharge cycling stability at temperatures above 50° C. than standard LiPF 6 -based electrolytes. The electrolytes of this invention enable &gt;80% of the initial charge/discharge capacity to be retained for more than twice as many charge discharge cycles at &gt;50° C. than standard LiPF 6 -based electrolytes.  
         [0076]     This invention has been described with reference to certain aspects or embodiments, but other aspects and embodiments are apparent to persons of skill in the art, and are included within the scope of the claims.