Patent Application
20070269715
The invention relates to lithium-borate complex salts, to the production thereof and to the use thereof as electrolytes in galvanic cells, in particular as conducting salts in lithium-ion batteries.
Mobile electronic appliances require ever more efficient rechargeable batteries for their independent power supply. Suitable for this purpose, besides nickel/cadmium and nickel/metal-hydride accumulator batteries, are rechargeable lithium batteries, which in comparison with the nickel batteries have a significantly higher energy density. The conventional systems on the market have a terminal voltage of about 3 V; the consequence of this potential is that water-based electrolyte systems cannot be used in lithium batteries. Instead, non-aqueous, mostly organic electrolytes (i.e. solutions of a lithium salt in organic solvents such as carbonates, ethers or esters) find application in liquid systems.
In the battery design that is dominant at the present time—lithium-ion batteries with liquid electrolytes—lithium hexafluorophosphate (LiPF6) is used practically exclusively as conducting salt. This salt possesses the necessary prerequisites for use in high-energy cells—i.e. it is readily soluble in aprotic solvents, it results in electrolytes having high conductivities, and it exhibits a high degree of electrochemical stability. Oxidative decomposition occurs only at potentials >approx. 4.5 V. However, LiPF6 has serious disadvantages, which can mainly be attributed to its lack of thermal stability (decomposition above approx. 130° C.). In addition, corroding and toxic hydrogen fluoride is released in the event of contact with moisture, which, on the one hand, makes handling difficult and, on the other hand, attacks and damages integral parts of the battery, e.g. the cathode.
Against this background, intense efforts are being made to develop alternative conducting salts. Above all, lithium salts with perfluorinated organic residues have been tested as such. In this connection it is a question of lithium trifluoromethanesulfonate (‘Li triflate’), lithium imides (lithium bis(perfluoralkylsulfonyl)imides) and also lithium methides (lithium tris(perfluoralkylsulfonyl)methides). All these salts require relatively elaborate production processes, are therefore relatively expensive, and have other drawbacks, such as corrosivity with respect to aluminium, or poor conductivity.
Lithium organoborates have been investigated as a further class of compounds for use as conducting salt in rechargeable lithium batteries. However, on account of their low oxidative stability and on account of misgivings as regards safety in connection with the handling of triorganoboranes, they do not come into consideration for commercial systems.
A significant advance is represented by the lithium complex salts of the type ABL2 (where A signifies lithium or a quaternary ammonium ion, B signifies boron, and L signifies a bidentate ligand which is bound to the boron atom via oxygen atoms) which are proposed in EP 698 301 for use in galvanic cells. However, the proposed salts, the ligands of which contain at least one aromatic residue, exhibit sufficient electrochemical stability only when the aromatic hydrocarbon is substituted with electron-attracting residues, typically fluorine, or exhibits at least one nitrogen atom in the ring. Such chelate compounds are not commercially available and can only be produced with high costs. The proposed products have therefore been unable to gain acceptance on the market.
Quite similar boron compounds are proposed in EP 907 217 as constituents in organic electrolyte cells. By way of boron-containing conducting salt, compounds of the general formula LiBXX′ are proposed, wherein the ligands X and X′ may be the same or different and each ligand contains an electron-attracting group containing oxygen, which binds to the boron atom. However, the listed compounds (lithium boron disalicylate and a special imide salt) exhibit the disadvantages already mentioned above.
The lithium bis(oxalato)borate (LiBOB) described for the first time in DE 198 29 030 is the first boron-centred complex salt described for use as an electrolyte that uses a dicarboxylic acid (in this case, oxalic acid) as chelate component. The compound is easy to produce, is non-toxic, and is electrochemically stable up to about 4.5 V, which makes its use in lithium-ion batteries possible. A disadvantageous aspect, however, is the fact that it can hardly be employed in new battery systems with cell voltages>3 V. For electrochemical storage batteries of such a type, salts having stabilities≧approx. 5 V are required. A further disadvantageous aspect is the fact that lithium bis(oxalato)borate does not admit of any possibilities for structural variation without the basic framework being destroyed.
In EP 1 035 612 additives of the formula
Li+B−(OR1)m(R2)p
are named,
with m and p=0, 1, 2, 3 or 4, where m+p=4, and
A=alkyl residue with 1 to 6 C atoms, which may be monohalogenated to trihalogenated.
To be mentioned as particularly preferred additives are lithium bis[1,2-benzenediolato(2-)O,O′]borate(1-), lithium bis[3-fluoro-1,2-benzenediolato(2-)O,O′]borate(1-), lithium bis[2,3-naphthalenediolato(2-)O,O′]borate(1-), lithium bis[2,2-biphenyldiolato(2-)O,O′]borate(1-), lithium bis[salicylato(2-)O,O′]borate(1-), lithium bis[2-olato-benzenesulfonato(2-)O,O′]borate(1-), lithium bis[5-fluoro-2-olato-benzenesulfonato(2-)O,O′]borate(1-), lithium phenolate and lithium-2,2-biphenolate. These are all symmetrical lithium chelatoborates of the Li[BL2] type.
Lithium bis(malonato)borate, which is supposed to exhibit an electrochemical window of up to 5 V, has been described by C. Angell as an electrochemically particularly stable, simple lithium (chelato)borate compound. The compound considered has the disadvantage that it is practically insoluble in the conventional battery solvents (e.g. only 0.08 molar in propylene carbonate), so that it can be dissolved and characterised only in DMSO and similar solvents that are prohibitive for batteries (Wu Xu and C. Austen Angell, Electrochem. Solid-State Lett. 4, E1-E4, 2001).
In DE 101 08 592 mixed boron chelate complexes of the general formula
are described, with either X≡—C(R1R2)— or —C(R1R2)—C(═O)—, wherein
A disadvantageous aspect of these compounds is their frequently unsatisfactory solubility in organic solvents such as propylene carbonate, for example. Therefore the electrical conductivity of such solutions is, as a rule, lower than that of established lithium salts (such as LiPF6 or LiBOB, for example).
For this reason, liquid electrolytes that exclusively contain one of the mixed boron chelate complex salts disclosed in DE 101 08 592 cannot be employed for powerful high-performance batteries.
The synthesis as described in DE 101 08 592 and in DE 101 08 608 is also not free from disadvantages: in the course of the production of mixed salts—starting from an oxidic boron raw material, for example boric acid or boron oxide, and two differing complex ligands L1 and L2 in a molar ratio of 1:1:1—not only does the desired mixed complex salt arise but also the homo compounds [BL12]− and [BL22]−. In DE 101 08 608 the following examples are mentioned:
*DE 101 08 592
The undesirable homo compounds have varying physicochemical properties, especially an electrochemical stability differing from that of the mixed compound; therefore they have to be separated out by recrystallisation or by a similar purification process, which is relatively costly.
WO 01/99209 also discloses the production of mixed lithium-borate salts such as lithium (malonato oxalato)borate (Examples 6 and 7). Two possibilities for synthesis are described, which both yield the desired salt as main product, but contaminations by homo complex compounds cannot be avoided (Example 6: 4.5% lithium bis(oxalato)borate).
In EP 1 095 942 complex salts of the formula
Li+B−(OR1)m(OR2)p
are described (with respect to the significance of R1, R2, m and p, see above in connection with EP 1 035 612). They serve as conducting salts in electrolytes for electrochemical cells. They may also be used in proportions between 1% and 99% in combination with other conducting salts. Suitable are conducting salts from the group comprising LiPF6, LiBF4, LiClOF4, LiAsF6, LiCF3SO3, LiN(CF3SO2)2 or LiC(CF3SO2)3 and mixtures thereof. These are all fluorinated conducting salts.
The object of the present invention is to overcome the disadvantages of the state of the art and to find, in particular, fluorine-free conducting salts that are capable of being produced easily and inexpensively for lithium-ion batteries, and to demonstrate the synthesis thereof. Moreover, the conducting salts are to be capable of being adapted to the material-specific and application-specific properties and are to have a forming function and an overcharge-protection function.
The object is achieved in that salt mixtures containing lithium bis(oxalato)borate (‘LiBOB’) and also mixed lithium-borate salts of the type
are employed by way of conducting salt, the proportion of compound (I) in the salt mixture amounting to 0.01 mol. % to 20 mol. %. X in formula (I) is a bridge which is linked to the boron by two oxygen atoms and which is selected from
wherein
These new, fluorine-free mixtures of substances may, for example, be produced in a manner analogous to a production process described in DE 101 08 592. In this process, the 1:1:1:1 stoichiometry (boron compound (e.g. boric acid)/oxalic acid/chelating agent L2/lithium compound) has to be departed from in such a manner that at most 20 mol. % of the chelating agent L2, relative to oxalic acid, is employed. The molar ratio of the substances employed (boron compound/mixture of oxalic acid and chelating agent L2/lithium compound) is 1:2:1, the mixture of oxalic acid and chelating agent L2 containing a maximum of 20 mol. % chelating agent L2. In this case L2 is, for example, a dicarboxylic acid (not oxalic acid), hydroxycarboxylic acid or salicylic acid (which may also be maximally disubstituted). Further possibilities for the chelating agent L2 are listed below in connection with the description of compound part X.
The conversion is preferably undertaken in such a manner that the raw-material components are suspended in a medium (e.g. toluene, xylene, methylcyclohexane, perfluorinated hydrocarbons with more than 6 C atoms) that is suitable for azeotropic removal of water, and the water is removed azeotropically in known manner.
It is also possible to perform the synthesis in aqueous solution. In this case the components are charged into water in arbitrary sequence and are concentrated by evaporation, subject to stirring, preferably at reduced pressure. After removal of the bulk of the water, a solid reaction product forms which, depending upon the specific product properties, is subjected to final drying at temperatures between 100° C. and 180° C. and at reduced pressure (e.g. 10 mbar). Besides water, alcohols and other polar organic solvents are also suitable as reaction media.
Lastly, production of the product may also be undertaken without addition of any solvent, i.e. the commercial raw materials are mixed and are then heated by supply of heat, and are dehydrated, under preferably reduced pressure.
In the course of implementation of the process a mixture forms that contains at least 80 nmol. % LiBOB in addition to at most 20 mol. % of the mixed lithium-borate salt (I). Surprisingly, no detectable quantities of the homo complex compound
are present in synthesis mixtures of such a type. The conducting-salt mixture that is obtained has the advantage, in comparison with pure LiBOB, that in the event of overcharge a decomposition reaction sets in at the cathode, which slows down the rise in cell voltage. As a result, dangerous consequent reactions of the cathode material with constituents of the electrolyte can be avoided or lessened.
Preferred examples of compound part X are 1,3-dicarboxylic acids formally lessened by two OH groups, such as malonic acid and alkylmalonic acids (malonic acid substituted with an alkyl group with preferably 1 to 5 C atoms). (The O atoms binding to the boron are already contained in formula (I); the 1,3-dicarboxylic acids correspond to L2.)
Further preferred examples of compound part X are 1,2- or 1,3-hydroxycarboxylic acids formally lessened by two OH groups, such as glycolic acid or lactic acid. (The 1,2- or 1,3-hydroxycarboxylic acids correspond to L2.) Compound part X may also preferably be constituted by saturated C2 chains or saturated C3 chains, this being derivable formally from 1,2- or 1,3-diols lessened by two OH groups. (The 1,2- or 1,3-diols correspond to L2.)
Further preferred examples of compound part X are 1,2-bisphenols, (such as pyrocatechol) or 1,2-carboxyphenols (such as salicylic acid) or aromatic or heteroaromatic 1,2-dicarboxylic acids (such as phthalic acid or pyridine-2,3-diol), these compounds having been formally lessened by two OH groups. The listed 1,2-bisphenols, 1,2-carboxyphenols or aromatic 1,2-dicarboxylic acids correspond to L2.
The subject-matter of the invention will be elucidated in more detail on the basis of the following Examples:
In a 250 ml round-bottom flask made of glass 23.95 g oxalic acid dehydrate, 6.81 g boric acid and 1.38 g salicylic acid (10 mol. %, relative to boric acid) were suspended in 50 ml water and, subject to stirring, added to 4.06 g lithium carbonate. After the evolution of gas (CO2 from the neutralisation reaction) had flattened out, the suspension was refluxed for 1 hour at an oil-bath temperature of 115° C. In this process a clear, colourless solution was formed. This solution was totally concentrated by evaporation in a vacuum in a rotary evaporator at an oil-bath temperature of 125° C.
The solids left behind were precrushed with a nickel spatula under protective-gas atmosphere (argon) and were finely triturated in a porcelain mortar. The powder was then recharged into a glass round-bottom flask and subjected to final drying in a rotary evaporator at 150° C. and, lastly, at 13 mbar.
Yield: 17.3 g (88% of the theoretical value; losses due to baked-on deposits in the glass flask)
Analysis: lithium 3.60% (nominal: 3.54%)
Purity: In the 11B NMR spectrum (solvent THF/C6D6) it is not possible for the homo compound lithium bis(salicylato)borate (literature shift 4.0 ppm) to be detected; recognisable only are the signals of the expected products lithium bis(oxalato)borate (7.6 ppm), abbreviated to LiBOB, and of the mixed salt lithium (salicylato, oxalato)borate (5.6 ppm), abbreviated to LiSOB, see
| Number | Date | Country | Kind |
|---|---|---|---|
| 10 2004 011 522.2 | Mar 2004 | DE | national |
| Filing Document | Filing Date | Country | Kind | 371c Date |
|---|---|---|---|---|
| PCT/EP05/02439 | 3/8/2005 | WO | 8/14/2007 |
