Fluorine-containing solvent for lithium batteries with increased security

In terms of environmental protection and economy, the development in the battery sector is clearly directed towards rechargeable (secondary) batteries. In the important sector of mobile electronics (high-quality camcorders, portable computers, cell phones and the like), lithium ion batteries are given great opportunities because their energy density is around twice as high as that of metal hydride cells and about three times higher than that of nickel / cadmium cells. Another interesting area is the use of secondary lithium-ion batteries for electric traction, for example for electrically powered city cars.

Currently, the safety standard of rechargeable lithium batteries is particularly problematic, since critical operating conditions such as overcharging, overdischarging or short-circuiting, which can lead to the cell opening under fire, have so far often only been avoided by electronic monitoring.

According to the current state of the art, organic solvents with strongly polarizing heteroatoms, such as nitrogen, oxygen or sulfur, are primarily used in secondary lithium batteries for the preparation of aprotic electrolyte solutions [see, for example, O. Popovych, RPT Tomkins, Nonaqueous Solution Chemistry, John Wiley & Sons (1981) or GJ Janz, RPT Tomkins, Nonaqueous Elektrolytes Handbook, Vol. I (1972), Vol. II (1973), Academic Press, New York]. Typical examples of such solvents are ethers (for example 1,2-dimethoxyethane or tetrahydrofuran), esters (for example propylene carbonate), nitriles (for example acetonitrile), but also lactones, sulfones and many others.

Some low volatility or little tendency to form explosive mixtures are some non-volatile, but unfortunately also highly viscous solvents such as propylene carbonate, ethylene carbonate or sulfolane (tetramethylene sulfone). Due to the high viscosity, the electrical conductivity of the electrolyte solutions produced with these solvents is low, especially at lower temperatures. In addition to ion migration, all other mass transfer processes in such solutions are slow.

In order to achieve high conductivities, solvent mixtures are generally used in industry which contain at least one strongly polar component which, because of its polarity, has a strongly dissociating effect on salts. The dielectric constant is an orientation measure for the dissociation ability. Since such highly polar solvents, such as propylene carbonate or ethylene carbonate, whose dielectric constants at 67 at 25 ° C or 90 at 40 ° C roughly correspond to that of water (78 at 25 ° C), are generally also quite highly viscous additionally one or more low-viscosity components as "thinners". Typical thinners are, for example, 1,2-dimethoxyethane or dimethyl carbonate, which, however, are characterized by very small values ​​for the dielectric constant (approximately 7 for 1,2-dimethoxyethane and approximately 3 for dimethyl carbonate).

A serious disadvantage of the "thinner" components is their volatility and the associated ignition and explosion behavior when entering air. Since electrochemical applications of electrolyte solutions are always associated with heating due to current flow and when errors occur (for example a short circuit inside or outside the electrochemical component) and also with the risk of ignition, this disadvantage is of considerable practical importance. For 1,2-dimethoxyethane, for example, the flash point is -6 ° C and the explosion limit is between 1.6 and 10.4 vol%.

The rechargeable lithium batteries usually contain a compound of lithium and a metal oxide as the cathode (for example Li_xMnO₂ or Li_xCoO₂) and lithium metal as the anode, the lithium preferably being used as an intercalation compound with graphite or in combination with carbon or graphite fibers. K. Brandt gives a good overview of the development of such batteries [Solid State Ionics 69 (1994), 173 to 183, Elsevier Science BV].

To increase safety, the cathode and anode compartments can be separated by a microporous separator membrane, which is designed in such a way that when a defined limit temperature is exceeded, the current flow is automatically interrupted by fusing of the pores. Suitable membranes of this type are included, for example, in the ®Celgard range from Hoechst Celanese Corporation. Furthermore, the safety of lithium batteries can be increased by means of pressure switches, which react, for example, to gas development during overcharging, and in general by means of complex monitoring and control electronics. Flame retardant additives containing phosphorus and halogen were also recommended.

However, all of these measures cannot rule out the fact that when defects occur, the volatile component of the liquid electrolyte solutions ultimately ignites and subsequently ignites the negative electrode, for example. In this case, a fire that can hardly be extinguished by conventional means arises, since, for example, burning lithium reacts violently not only with water, but also with the substances contained in common fire extinguishers (for example carbon dioxide).

Perfluorinated ethers and perfluoroalkanes for the electrolyte system of lithium batteries have already been proposed in earlier publications (JP-A 7-249432 and EP-A 631 339). Although these are generally very stable thermally and chemically, they are, however, difficult to mix with solvents customary in batteries. In addition, they generally have poor solubility for the common lithium conductive salts.

JP-A 7-249432 discloses the use of partially fluorinated ethers in electrolyte solutions for lithium secondary batteries. However, particularly preferred are ethers with a relatively low molecular weight (for example 1,1,1,5,5,5-hexafluoro-3-oxapentane), which experience has shown to have the following disadvantages: high vapor pressure, low boiling point, poor solubility for conductive lithium salts and generally also very low flash points. For example, the flash points of the compounds are ROCF₂CF₂H (R is methyl or ethyl) below 10 ° C and even the highly fluorinated ether of the formula HCF₂CF₂CH₂OCF₂CF₂H has a flash point of only 22 ° C. Mixtures of dimethyl carbonate or ethylene carbonate with 3,3,4,4-tetrafluoro-2,4-dioxa-hexane were tested with a 1M concentration of different lithium conducting salts in secondary lithium cells over three cycles and found to be useful (M. Winter, dissertation, Technical University Graz, "Film formation on lithium / carbon intercalation anodes", September 1995).

According to the current state of the art, reduced flammability of the electrolyte solution is achieved primarily by increasing the viscosity of the electrolyte solution by means of binders or fillers or by using polymer electrolytes which are practically solid at room temperature. For example, US-A 5 169 736 describes organic or inorganic thickeners (polyethylene oxide, SiO₂, Al₂O₃ and others) to solidify liquid electrolyte solutions. Polymeric electrolytes based on macromolecules with numerous polar groups, such as polyethylene oxides [see, for example, B. Scrosati, ed., 2nd International Symposium on Polymer Electrolytes, Elsevier, London and New York (1990)] are also much heavier due to their low volatility flammable. US Pat. No. 5,393,621 describes polymeric electrolytes whose polar macromolecules are formed by polymerizing organophosphorus compounds which are notable for particularly low flammability.

All these gel-like to solid electrolytes have in common that, due to their high viscosity, the mobility of the ions of the salts dissolved in them is far less than in liquid electrolyte solutions, so that, especially at lower temperatures, the required conductivities are no longer achieved, at least for most technical applications . For this reason, for example, alkali metal batteries with polymeric electrolytes have still not been able to achieve economic importance despite decades of very intensive research.

The aim of the present invention was to develop electrolyte solutions which are free from the abovementioned highly flammable and explosive, low-viscosity "thinners" and thus increase the safety of the electrolyte-containing devices, but nevertheless exhibit a viscosity and conductivity behavior which show their practical use even at low temperatures makes possible.

There was therefore an urgent need for stable solvents for lithium cells, which are characterized by the following substance properties:<ul id="ul0001" list-style="none" compact="compact"><li>1. High thermal stability.</li><li>2nd High flash point.</li><li>3rd Low vapor pressure or high boiling point.</li><li>4th Low viscosity.</li><li>5. Miscibility with common battery solvents, for example ethylene carbonate, propylene carbonate or α, ω-dialkyl glycol ethers.</li><li>6. Sufficient solubility for fluorine-containing lithium conductive salts, for example LiPF₆, LiN (SO₂CF₃)₂ or LiC (SO₂CF₃)₃.</li><li>7. High stability against metallic lithium.</li><li>8th. Good solvency for carbon dioxide: CO₂ accelerates the build-up of protective films on lithium or LiC_nAnodes.</li></ul>

It has now surprisingly been found that certain groups of partially fluorinated, aliphatic ethers meet the requirements mentioned under items 1 to 8 well to excellent. Basically, they are compounds which are characterized in that they contain alkylene groups which are linked via ether oxygen to partially fluorinated alkyl groups which, in addition to fluorine, may also contain hydrogen, chlorine and ether oxygen. Compounds within the meaning of this definition are ethers of the formulas (I) and (II) below         RO - [(CH₂)_mO]_n-CF₂-CFH-X (I)    wherein<dl id="dl0001" compact="compact"><dt>R</dt><dd>a straight-chain alkyl group with 1 to 10 C atoms or a branched alkyl group with 3 to 10 C atoms,</dd><dt>X</dt><dd>Is fluorine, chlorine or a perfluoroalkyl group with 1 to 6 carbon atoms, which can also contain ether oxygen,</dd><dt>m</dt><dd>a number from 2 to 6 and</dd><dt>n</dt><dd>is a number from 1 to 8,</dd></dl> and         X-CFH-CF₂O - [(CH₂)_mO]_n-CF₂-CFH-X (II)    wherein X, m and n have the meanings given above.

The invention thus relates to an electrolyte system for increasing the safety of lithium batteries, which contains compounds of the formulas (I) and / or (II) in an effective amount, the compounds with X fluorine or trifluoromethyl being preferred. Fluorine-containing ethers of the formula (I), in which R is a methyl group, X is fluorine, m 2 and n 1 to 3, and ethers of the formula (II) in which X is fluorine, m 2 and n 1 to 3 are particularly preferred.

In general, the compounds with m equal to 2 are preferred because they can be prepared from easily accessible and inexpensive ethylene glycol monoalkyl ethers or ethylene glycols. The compounds in which X is chlorine are less preferred because they can react at high temperatures with metallic lithium with the elimination of chlorine and fluorine to form the corresponding lithium halides.

The solution to the safety problem of secondary lithium batteries according to the invention is achieved by using compounds of the formulas (I) and / or (II) as an essential component of the electrolyte system, taking advantage of their surprisingly low viscosity. The substances of the formulas (I) and (II) can be used as diluents for flame-retardant, highly viscous components, for example ethylene carbonate and propylene carbonate. In this way, aprotic electrolyte systems can be produced that are practically hardly flammable. The content of ethers of the formulas (I) and / or (II) is usually 5 to 70% by volume, preferably 20 to 50% by volume, based on the total volume of the electrolyte system.

The partially fluorinated ethers according to formulas (I) and (II) also improve the solvency for non-polar or slightly polar gases, in particular CO₂, N₂, N₂O, SF₆, SO₂FCl or SO₂F₂. These gases can advantageously be used as protective gas in lithium batteries, since they have a positive effect on the reactions taking place at the negative electrode / electrolyte interface [see, for example, JO Besenhard, MW Wagner, M. Winter; J. Power Sources, 44 (1993), 413].

It is known that reactive impurities (for example water), even in very low concentrations, have drastic negative effects on the function of the lithium batteries. In practice, the sum of such contaminants should never exceed 50 ppm. A great advantage of the products defined by formulas (I) and (II) above is that they usually have boiling points so high that water and other reactive impurities can easily be removed completely by distillation.

The viscosity of mixtures of the ethers of the formulas (I) and (II) with propylene carbonate can be reduced by adding (at least) a low-viscosity, largely fluorinated solvent from the group of the hydroperfluoroalkanes or hydroperfluoroethers, in order to also at temperatures below 0 ° C to guarantee high conductivity. In such cases, the use of particularly easily dissociating conductive salts with large fluorine-containing anions, such as LiN (SO₂CF₃)₂ or LiC (SO₂CF₃)₃. The partially fluorinated ethers according to the invention act as phase mediators with respect to the more fluorinated solvents added. Particularly suitable agents for lowering the viscosity are, for example, 1H-perfluorohexane (kinematic viscosity at 20 ° C.: 0.55 mm²/ s, flash point&gt; 110 ° C) and 2,3-dihydro-perfluoro-5-methyl-pentane. These substances do not form explosive mixtures with air. This also applies to fluoroethers of the formula<chemistry id="chem0001" num="0001"><img file="EP0807986A1_D0001.tif" /></chemistry>    where n is 1 or 2.

As can be seen from Table 3, the compounds described by the formulas (I) and (II) tend to thermally decompose above 200 ° C. It has surprisingly been found that the partially fluorinated ethers can be stabilized very effectively with very small amounts of tertiary, aliphatic amines. Even small additions of the amine in the order of 0.1 to 1.0% by weight with respect to the partially fluorinated ether are sufficient to raise the temperature at which the ether begins to decompose by 60 to 100 ° C. The tertiary amine should be so high-boiling that it remains predominantly in the liquid phase even at temperatures above 100 ° C. Suitable tertiary amines are, for example, tri-n-butylamine, tri-n-octylamine or 1,6-bis (dimethylamino) hexane. Aromatic amines are less suitable because of their tendency to anodize.

Our invention thus also relates to a method for stabilizing compounds of the formulas (I) and (II) with tertiary, aliphatic amines.

Syntheses of partially fluorinated ethers:

Primary alcohols react base-catalyzed with various fluorine-containing alkenes to form partially fluorinated ethers [see Houben-Weyl, Methods of Organic Chemistry, 4th Edition, Volume VI / 3, (1965) 120/121, Georg Thieme Verlag Stuttgart and the literature cited therein] : <maths id="math0001" num=""><math display="block"><mrow><msub><mrow><mtext>ROH + F</mtext></mrow><mrow><mtext>2</mtext></mrow></msub><msub><mrow><mtext>C = CFX → RO-CF</mtext></mrow><mrow><mtext>2</mtext></mrow></msub><mtext>-CFHX,</mtext></mrow></math><img file="EP0807986A1_D0002.tif" /></maths>wherein R is a primary alkyl group and X is fluorine, chlorine or perfluoroalkyl (for example CF₃) is.

The ethers shown in Table 1 with 1H-tetrafluoroethyl groups were synthesized from the corresponding alcohols and tetrafluoroethylene (catalyst: KOH; solvent: N, N-dimethylformamide). The compound CH₃O (CH₂)₂OCF₂CFClH obtained with chlorotrifluoroethylene (boiling point: 146 to 147 ° C, 1013 hPa; GC purity: 99.4%).

In the reaction of alcohols with hexafluoropropene under basic conditions, HF elimination occurs in some cases, so that ethers of the formula RO-CF = CF-CF are also by-products₃ (E / Z isomers) form. This side reaction can be largely suppressed by carrying out the reaction under high pressure [H. Kokelenberg and R. Pollet, Tenside Detergents 22 (1985), 1]. The CF₃CFHCF₂-O (CH₂CH₂O)₂-CF₂CFHCF₃ prepared (GC purity: 98.7%).<tables id="tabl0001" num="0001"><img file="EP0807986A1_D0003.tif" /></tables><tables id="tabl0002" num="0002"><table frame="all"><title>Table 2</title><tgroup cols="4" colsep="1" rowsep="0"><colspec colnum="1" colname="col1" colwidth="39.37mm" /><colspec colnum="2" colname="col2" colwidth="39.37mm" /><colspec colnum="3" colname="col3" colwidth="39.37mm" /><colspec colnum="4" colname="col4" colwidth="39.37mm" /><thead valign="top"><row rowsep="1"><entry namest="col1" nameend="col4" align="left">Safety tests on partially fluorinated ethers</entry></row><row rowsep="1"><entry namest="col1" nameend="col1" align="left">Test substance</entry><entry namest="col2" nameend="col2" align="center">Ignition test with burning wood chips</entry><entry namest="col3" nameend="col3" align="center">Condition after trial</entry><entry namest="col4" nameend="col4" align="center">Stability against lithium *)</entry></row></thead><tbody valign="top"><row><entry namest="col1" nameend="col1" align="left">CH₃OCF₂CF₂OCH₃</entry><entry namest="col2" nameend="col2" align="left">burns, yellow flame</entry><entry namest="col3" nameend="col3" align="center">Etched glass</entry><entry namest="col4" nameend="col4" align="left">no reaction</entry></row><row><entry namest="col1" nameend="col1" align="left">CH₃OCH₂CH₂OCF₂CF₂H</entry><entry namest="col2" nameend="col2" align="left">burns, yellow flame</entry><entry namest="col3" nameend="col3" align="center">Etched glass</entry><entry namest="col4" nameend="col4" align="left">no reaction</entry></row><row><entry namest="col1" nameend="col1" align="left">CH₃CH₂OCH₂CH₂OCF₂CF₂H</entry><entry namest="col2" nameend="col2" align="left">burns, yellow flame</entry><entry namest="col3" nameend="col3" align="center">Etched glass</entry><entry namest="col4" nameend="col4" align="left">no reaction</entry></row><row><entry namest="col1" nameend="col1" align="left">CH₃O (CH₂CH₂O)₃CF₂CF₂H</entry><entry namest="col2" nameend="col2" align="left">non-flammable</entry><entry namest="col3" nameend="col3" align="center">---</entry><entry namest="col4" nameend="col4" align="left">no reaction</entry></row><row><entry namest="col1" nameend="col1" align="left">HCF₂CF₂OCH₂CH₂OCF₂CF₂H</entry><entry namest="col2" nameend="col2" align="left">non-flammable</entry><entry namest="col3" nameend="col3" align="center">---</entry><entry namest="col4" nameend="col4" align="left">no reaction</entry></row><row><entry namest="col1" nameend="col1" align="left">HCF₂CF₂O (CH₂CH₂O)₂CF₂CF₂H</entry><entry namest="col2" nameend="col2" align="left">non-flammable</entry><entry namest="col3" nameend="col3" align="center">---</entry><entry namest="col4" nameend="col4" align="left">no reaction</entry></row><row><entry namest="col1" nameend="col1" align="left">HCF₂CF₂O (CH₂CH₂O)₃CF₂CF₂H</entry><entry namest="col2" nameend="col2" align="left">non-flammable</entry><entry namest="col3" nameend="col3" align="center">---</entry><entry namest="col4" nameend="col4" align="left">no reaction</entry></row><row><entry namest="col1" nameend="col1" align="left">CF₃CFHCF₂O (CH₂CH₂O)₂CF₂CFHCF₃</entry><entry namest="col2" nameend="col2" align="left">non-flammable</entry><entry namest="col3" nameend="col3" align="center">---</entry><entry namest="col4" nameend="col4" align="left">no reaction</entry></row><row rowsep="1"><entry namest="col1" nameend="col1" align="left">CH₃OCH₂CH₂OCF₂CFClH</entry><entry namest="col2" nameend="col2" align="left">burns, yellow flame</entry><entry namest="col3" nameend="col3" align="center">Etched glass</entry><entry namest="col4" nameend="col4" align="left">Vapor, smoke formation</entry></row></tbody></tgroup><tgroup cols="4" colsep="0" rowsep="0"><colspec colnum="1" colname="col1" colwidth="39.37mm" /><colspec colnum="2" colname="col2" colwidth="39.37mm" /><colspec colnum="3" colname="col3" colwidth="39.37mm" /><colspec colnum="4" colname="col4" colwidth="39.37mm" /><tbody valign="top"><row><entry namest="col1" nameend="col4" align="justify">*) Test conditions: An apparatus consisting of a 20 ml quartz glass flask with an attached, heated dropping funnel is carefully heated in a high vacuum with a power blow dryer. After cooling and filling with argon, the flask is charged with about 1 g of lithium, then the dropping funnel with 5 ml of the test compound saturated with argon. The lithium is melted in a heating bath at 190 ° C and the ether preheated to approximately 100 ° C is slowly added dropwise. Only the chlorine-containing ether reacts with lithium, producing LiCl and LiF.</entry></row></tbody></tgroup></table></tables>

Thermal analysis of the stability of partially fluorinated ethers:

The thermal stability of typical partially fluorinated ethers was investigated using DSC (Differential Scanning Calorimetry). The heating rate, starting at 20 ° C, was 10 ° C / min.<tables id="tabl0003" num="0003"><table frame="all"><title>Table 3</title><tgroup cols="4" colsep="1" rowsep="0"><colspec colnum="1" colname="col1" colwidth="39.37mm" /><colspec colnum="2" colname="col2" colwidth="39.37mm" /><colspec colnum="3" colname="col3" colwidth="39.37mm" /><colspec colnum="4" colname="col4" colwidth="39.37mm" /><thead valign="top"><row rowsep="1"><entry namest="col1" nameend="col1" align="left">substance</entry><entry namest="col2" nameend="col2" align="center">Start of decomposition [° C]</entry><entry namest="col3" nameend="col3" align="center">Maximum [° C]</entry><entry namest="col4" nameend="col4" align="center">Tone of heat [kJ / mol]</entry></row></thead><tbody valign="top"><row><entry namest="col1" nameend="col1" align="left">CH₃OCH₂CH₂OCF₂CF₂H</entry><entry namest="col2" nameend="col2" align="right">208</entry><entry namest="col3" nameend="col3" align="right">226</entry><entry namest="col4" nameend="col4" align="right">-67</entry></row><row><entry namest="col1" nameend="col1" align="left">CH₃CH₂OCH₂CH₂OCF₂CF₂H</entry><entry namest="col2" nameend="col2" align="right">200</entry><entry namest="col3" nameend="col3" align="right">220</entry><entry namest="col4" nameend="col4" align="right">-51</entry></row><row><entry namest="col1" nameend="col1" align="left">CH₃CH₂OCH₂CH₂OCF₂CF₂H + 1% N (nC₄H₉)₃</entry><entry namest="col2" nameend="col2" align="right">282</entry><entry namest="col3" nameend="col3" align="right">295</entry><entry namest="col4" nameend="col4" align="right">-49</entry></row><row><entry namest="col1" nameend="col1" align="left">HCF₂CF₂O (CH₂CH₂O)<maths id="math0002" num=""><math display="inline"><mrow><msub><mrow><mtext>​</mtext></mrow><mrow><mover accent="true"><mrow><mtext>n</mtext></mrow><mo>¯</mo></mover></mrow></msub></mrow></math><img file="EP0807986A1_D0004.tif" /></maths>CF₂CF₂H, <maths id="math0003" num=""><math display="inline"><mrow><mover accent="true"><mrow><mtext>n</mtext></mrow><mo>¯</mo></mover></mrow></math><img file="EP0807986A1_D0005.tif" /></maths> = 6,4</entry><entry namest="col2" nameend="col2" align="right">240</entry><entry namest="col3" nameend="col3" align="right">250</entry><entry namest="col4" nameend="col4" align="right">-75</entry></row><row><entry namest="col1" nameend="col1" align="left">HCF₂CF₂O (CH₂CH₂O)<maths id="math0004" num=""><math display="inline"><mrow><msub><mrow><mtext>​</mtext></mrow><mrow><mover accent="true"><mrow><mtext>n</mtext></mrow><mo>¯</mo></mover></mrow></msub></mrow></math><img file="EP0807986A1_D0006.tif" /></maths>CF₂CF₂H + 1% N (nC₄H₉)₃, <maths id="math0005" num=""><math display="inline"><mrow><mover accent="true"><mrow><mtext>n</mtext></mrow><mo>¯</mo></mover></mrow></math><img file="EP0807986A1_D0007.tif" /></maths> = 6,4</entry><entry namest="col2" nameend="col2" align="right">300</entry><entry namest="col3" nameend="col3" align="right">315</entry><entry namest="col4" nameend="col4" align="right">-70</entry></row><row><entry namest="col1" nameend="col1" align="left">CF₃CFHCF₂O (CH₂CH₂O)₂CF₂CFHCF₃</entry><entry namest="col2" nameend="col2" align="right">210</entry><entry namest="col3" nameend="col3" align="right">222</entry><entry namest="col4" nameend="col4" align="right">-73</entry></row><row rowsep="1"><entry namest="col1" nameend="col1" align="left">CF₃CFHCF₂O (CH₂CH₂O)₂CF₂CFHCF₃ + 1% N (nC₄H₉)₃</entry><entry namest="col2" nameend="col2" align="right">290</entry><entry namest="col3" nameend="col3" align="right">303</entry><entry namest="col4" nameend="col4" align="right">-70</entry></row></tbody></tgroup></table></tables>

Conclusions:

<ul id="ul0002" list-style="none"><li>1. The thermal decomposition of the partially fluorinated ethers listed in Table 3 is basically exothermic.</li><li>2nd The partially fluorinated ethers can be efficiently stabilized by small amounts of a tertiary amine.</li></ul>

Conductivity measurements on electrolyte systems which contain an ether according to the invention:

Figures 1 to 6 show the conductivity as a function of temperature in the range from +40 to approximately -50 ° C. In the case of solvent mixtures, the proportions of the components are given in percent by volume. The lithium conducting salt was used in 1M concentration.

Abbreviations:

<dl id="dl0002" compact="compact"><dt>EC:</dt><dd>Ethylene carbonate</dd><dt>PC:</dt><dd>Propylene carbonate</dd><dt>Imid:</dt><dd>Li⁺[N (SO₂CF₃)₂]^-</dd></dl>

The invention is explained in more detail in the following examples.

Embodiments

To produce the electrolyte, the solvent components used are first prepared as follows:

Ethylene carbonate (&gt; 99%, Merck company) is distilled in an oil pump vacuum (boiling point 85 to 95 ° C) and dewatered over activated molecular sieve (Roth company, pore size 4 angstroms) at 150 ° C for 3 days under a dry argon atmosphere [Argon, 99.996%, company AGA was first removed to remove traces of oxygen at 150 ° C with argon W5 (mixture of 95% argon and 5% hydrogen, technical purity, AGA) reduced copper (I) oxide (BASF) and then dried over activated molecular sieve] stored at 60 ° C.

Propylene carbonate (purum, Aldrich company) is distilled in an oil pump vacuum over a 1.5 m long, mirrored packed column (boiling point 64 to 66 ° C.) and stored over an activated molecular sieve under a dried argon atmosphere at room temperature. After cleaning and drying, the residual water content of the solvents is determined using the Karl Fischer method (for example with the Mitsubishi CA 05 automatic titration device). The water content should be below 10 ppm.

The fluorinated solvent component is dried for a few days over an activated molecular sieve under a dried argon atmosphere at room temperature.

The production of the electrolyte solutions takes place with the so-called Schlenk technology in a dried argon flow, whereby the glass devices used with a protective gas connection are freed of adhering moisture before use in the illuminated Bunsen burner flame with repeated changes of argon purge and oil pump vacuum.

example 1

Manufacture of a safety battery electrolyte based on ethylene carbonate as a film-forming component in lithium-ion batteries.

40% by volume of monoglycol-bis-tetrafluoroethyl ether (HC.) Are added to 50% by volume of ethylene carbonate and 10% by volume of propylene carbonate₂F₄OCH₂CH₂OC₂F₄H) given. This solvent mixture is stirred with 287.1 g (1 mol) of lithium bis (trifluoromethanesulfone) imide [LiN (CF₃SO₂)₂,&gt; 99.5%, 3M Company, dried for 4 days in a high vacuum at 110 ° C.] and made up to 1 liter. The electrolyte produced in this way consists of 50% by volume of ethylene carbonate, 40% by volume of monoglycol-bis-tetrafluoroethyl ether (HC₂F₄OC₂H₄OC₂F₄H) and 10 vol .-% propylene carbonate and is 1 M at LiN (CF₃SO₂)₂. The electrolyte is characterized by favorable low-temperature behavior down to -50 ° C without crystallization of the ethylene carbonate component with good conductivity (Figure 2), is stable in a wide "electrochemical window", behaves favorably with the intercalation of lithium in carbon and is extremely difficult to ignite. A solution of the imide in ethylene carbonate without the addition of fluorether is unsuitable for low temperatures (see FIG. 1).

Example 2

Production of a safety battery electrolyte based on propylene carbonate with lithium bis (trifluoromethanesulfone) imide [LiN (CF₃SO₂)₂] as a conductive salt.

30% by volume of monoglycol-bis-tetrafluoroethyl ether (HC₂F₄OCH₂CH₂OC₂F₄H) given. This solvent mixture is stirred with 287.1 g (1 mol) of lithium bis (trifluoromethanesulfone) imide [LiN (CF₃SO₂)₂,&gt; 99.5%, 3M Company, dried for 4 days in a high vacuum at 110 ° C.] and made up to 1 liter. The electrolyte produced consists of 70 vol .-% propylene carbonate, 30 vol .-% monoglycol-bis-tetrafluoroethyl ether (HC₂F₄OC₂H₄OC₂F₄H) and is 1 M at imide [LiN (CF₃SO₂)₂]. The electrolyte is characterized by favorable low-temperature behavior down to -50 ° C with good conductivity (Figure 3), is stable in a wide "electrochemical window", behaves favorably with the intercalation of lithium in carbon and is extremely difficult to ignite. The solvents can be mixed with one another in any ratio [FIG. 4 shows the temperature dependence of the conductivity of an electrolyte which consists of 30 vol.% Propylene carbonate and 70 vol.% Monoglycol-bis-tetrafluoroethyl ether (HC₂F₄OCH₂CH₂OC₂F₄H) and 1 M lithium bis (trifluoromethanesulfone) imide [LiN (CF₃SO₂)₂ is].

Example 3

Production of a safety battery electrolyte based on propylene carbonate with lithium hexafluorophosphate (LiPF₆) as a conductive salt.

30% by volume of monoglycol-bis-tetrafluoroethyl ether (HC₂F₄OCH₂CH₂OC₂F₄H) given. With stirring, this solvent mixture becomes 151.9 g (1 mol) of lithium hexafluorophosphate (LiPF₆,&gt; 99.9%, company Merck or Hashimoto, can be used without prior drying) and made up to 1 liter. The electrolyte produced consists of 70 vol .-% propylene carbonate, 30 vol .-% monoglycol-bis-tetrafluoroethyl ether (HC₂F₄OC₂H₄OC₂F₄H) and is 1 M lithium hexafluorophosphate. The electrolyte is characterized by favorable low-temperature behavior down to -50 ° C with good conductivity (Figure 5), is stable in a wide "electrochemical window", behaves favorably with the intercalation of lithium in carbon and is extremely difficult to ignite.

Example 4

A 1M solution is prepared from 30% by volume of propylene carbonate and 70% by volume of monoglycol-bis-tetrafluoroethyl ether and the imide already mentioned. See Figure 6 for conductivity measurement.