# Patent

## Title
Lithium salt

## Abstract

The principal object of the invention is to provide a lithium salt having excellent ion conductivity. The invention solves the problem by providing a lithium salt having a structure represented by the general formula (1): in which “M” represents B, Si, Ge, P, As or Sb; “X” represents the valence of “M”; “R1” represents —CmH2m— whereupon “m” is an integer of 1 to 4; “R2” represents —CkH2k+1 whereupon “k” is an integer of 1 to 8; and “n” represents 0 to 12.

## Background
CROSS-REFERENCE TO RELATED APPLICATIONS
This application is a national phase application of International Application No. PCT/JP2007/067862, filed Sep. 13, 2007, and claims the priority of Japanese Application No. 2006-248539, filed Sep. 13, 2006, the contents of both of which are incorporated herein by reference.
TECHNICAL FIELD
The present invention relates to a lithium salt which can give a lithium ionic liquid with low viscosity and high ion conductivity.
BACKGROUND ART
Lithium salts which have conventionally been used in electrolytes etc. in lithium secondary batteries are solids having a highly dissociative chemical structure and do not show ion conductivity by themselves. Accordingly, the lithium salts have conventionally been used after dissolution in a suitable solvent in order to confer ion conductivity thereon.
Solvents used in dissolving lithium salts are generally non-aqueous solvents from the viewpoint of suppressing a reaction with an electrode active material. General non-aqueous solvents are combustible, and thus use of such non-aqueous solvents is preferably avoided in lithium secondary batteries widely usable for consumer application.
For withholding the use of non-aqueous solvents, a lithium ionic liquid having lithium ion conductivity and high dissociation property (self-dissociation property) by the lithium salt itself has been proposed. For example, Patent Document 1 discloses a lithium ionic liquid having a lithium cation and a quaternary anion having the XIII group element (B, Al, Ga, In, Ti) as the central element. However, there is the case where the lithium ionic liquid disclosed in Patent Document 1 cannot attain sufficiently excellent ion conductivity.
Patent Document 2 discloses a lithium ionic liquid represented by LiAlXn(OY)4-n wherein “X” is an electron-withdrawing substituent and “Y” is an oligoether group. However, the dissociation property of the lithium ionic liquid disclosed in Patent Document 2 is not high, and depending on the type of the electron-withdrawing group “X”, its viscosity may increase, and as a result, oligoether groups involved in conduction of lithium cations are hardly contacted with one another, thus failing to attain sufficiently excellent ion conductivity in some cases.
Patent Document 3 discloses a non-aqueous electrolyte for electrochemical element including a fluorine compound and an ambient temperature molten salt consisting of an onium cation and a non-aluminate anion. The addition of LiBF3(CF3), LiBF3(C2F5) and LiBF3(C3F7) etc., as lithium salts is also disclosed. However, the non-aqueous electrolyte for electrochemical element disclosed in Patent Document 3 includes various ions to make the system complex so that the movement of lithium cations may be inhibited.

    Patent Document 1: Japanese Patent Application Laid-Open (JP-A) No. 2004-307481
    Patent Document 2: JP-A No. 2003-146941
    Patent Document 3: JP-A No. 2005-229103


DISCLOSURE OF INVENTION
Problem to be Solved by the Invention
The present invention has been completed in view of the problem described above, and the principal object of the present invention is to provide a lithium salt excellent in ion conductivity. Particularly, the present invention provides a lithium salt which can give a lithium ionic liquid with high dissociation property, low viscosity and high ion conductivity.
Means for Solving Problem
To solve the problem, the present invention provides a lithium salt having a structure represented by the general formula (1).




In the above-mentioned general formula (1), “M” represents B, Si, Ge, P, As or Sb; “X” represents the valence of “M”; “R1” represents —CmH2m— whereupon “m” is an integer of 1 to 4; “R2” represents —CkH2k+1 whereupon “k” is an integer of 1 to 8; and “n” represents 0 to 12.
According to the present invention, the atoms bound to the central atom (M) of the anion moiety are an ether chain and F only, and thus the molecular weight of the anion moiety can be decreased. Accordingly, when the lithium salt of the present invention is a lithium ionic liquid for example, the liquid can have low viscosity and high ion conductivity.
In the present invention, it is preferable that M−Fx is B−F3 in the general formula (1). This is because a lithium salt with high ion conductivity can be obtained.
In the present invention, it is preferable that M−Fx is B−F3, “R1” is —C2H4—, and R2 is —CH3 in the general formula (1). Thereby, a lithium salt with high conductivity can be obtained.
The present invention provides a method for producing a lithium salt, which comprises carrying out the following reaction formulae (1) and (2).

[Chemical Formula 2]

LiCpH2p+1+R2(OR1)nOH→R2(OR1)nOLi+CpH2p+2↑  (Reaction Formula 1)

R2(OR1)nOLi+MFxCompound→LiMFxO(R1O)nR2  (Reaction Formula 2)

In the above-mentioned reaction formulae (1) and (2), “p” represents an integer of 1 to 4; “R1” represents —CmH2m— whereupon “m” is an integer of 1 to 4; “R2” represents —CkH2k+1 whereupon “k” is an integer of 1 to 8; “n” represents 0 to 12; “M” represents B, Si, Ge, P, As or Sb; and “X” represents the valence of “M”.
The present invention has an advantage that a lithium salt can be easily obtained by using an alkyl lithium and an MFx compound.
Effect of the Invention
In the present invention, there is brought about an effect of obtaining a lithium salt excellent in ion conductivity.



BRIEF DESCRIPTION OF DRAWINGS
FIG. 1 is a graph showing an IR spectrum of the lithium ionic liquid obtained in Example 1.
FIG. 2 is a graph showing a 1H-NMR spectrum of the lithium ionic liquid obtained in Example 1.
FIG. 3 is a graph showing a 13C-NMR spectrum of the lithium ionic liquid obtained in Example 1.
FIG. 4 is a graph showing the results of ion conductivity measurement of the lithium ionic liquids obtained in Examples 1 to 3.
FIG. 5 is a graph showing the result of CV measurement of the lithium ionic liquid obtained in Example 1.
FIG. 6 is a graph showing the charge-discharge properties of a coin-cell type secondary battery using the lithium ionic liquid obtained in Example 1.



BEST MODE FOR CARRYING OUT THE INVENTION
Hereinafter, the lithium salt and the method for producing a lithium salt of the present invention are described in detail.
A. Lithium Salt
First, the lithium salt of the present invention is described. The lithium salt of the present invention is characterized by having a structure represented by the general formula (1) above.
According to the present invention, the atoms bound to the central atom (M) of the anion moiety are an ether chain and F only, and thus the molecular weight of the anion moiety can be decreased. Accordingly, when the lithium salt of the present invention is a lithium ionic liquid for example, the liquid can have low viscosity and high ion conductivity. Lithium cations are conductive usually through an ether chain, and lithium ions are estimated to diffuse easily with decreasing viscosity to increase ion conductivity. Although the conventional lithium salts have a property of easily solidifying and hardly liquefying with a decreasing molecular weight, a lithium ionic liquid stable with a relatively low molecular weight can be obtained in the present invention.
Conventionally, a lithium ionic liquid wherein an electron-withdrawing substituent is bound to an atom bound to the central atom (M) in the anion portion thereof is known, but the electron-withdrawing substituent of such lithium ionic liquid has a large molecular weight, thus increasing the viscosity of the lithium ionic liquid, resulting in failure to demonstrate sufficient ion conductivity in some cases. The lithium salt of the present invention, on the other hand, has a structure wherein the central atom (M) in the anion portion binds to fluorine atoms besides an ether chain represented by —O(R1O)nR2. Accordingly, a lithium ionic liquid having a low molecular weight, low viscosity and high ion conductivity can be obtained. The lithium salt of the present invention is useful for example as an electrolyte for lithium secondary battery.
Hereinafter, each constitution of the lithium salt of the present invention is described.
In the general formula (1), “M” represents B (boron), Si (silicon), Ge (germanium), P (phosphorus), As (arsenic) or Sb (antimony). Particularly, in the present invention, “M” is preferably B, Si or P, and particularly preferably B. In the general formula (1), “X” represents the valence of “M” and indicates the number of F (fluorine), which depending on the type of “M”, bound to “M”. Specifically, M−Fx in the general formula (1) represents B−F3, Si−F4, Ge−F4, P−F5, As−F5 or Sb−F5. In the present invention, M−Fx is particularly preferably B−F3.
In the general formula (1), “R1” represents —CmH2m— wherein “m” is an integer of 1 to 4. It is preferable that “m” is an integer in the range of 2 to 3, and particularly preferably to be 2. That is to say, in the present invention, “R1” is particularly preferably —C2H4—. In the general formula (1), “R2” represents —CkH2k+1 wherein “k” is an integer of 1 to 8. Furthermore, “k” is preferably an integer in the range of 1 to 3, and particularly preferably to be 1. That is to say, in the present invention, “R2” is particularly preferably —CH3.
In the general formula (1), “n” represents 0 to 12. Particularly, in the present invention, “n” is preferably a numerical value at which the lithium salt of the present invention can be converted into a lithium ionic liquid. Such a numerical value differs significantly depending on the constitution of the lithium salt of the present invention, and for example, “n” is preferably in the range of 3 to 12.
The nature of the lithium salt of the present invention varies significantly depending on properties such as the molecular weight of —(R1O)nR2 in the general formula (1). Specifically, when the molecular weight of —(R1O)nR2 is increased, the nature of —(R1O)nR2 in the lithium salt is dominating, and thus the lithium salt changes from solid to liquid. From the viewpoint of ion conductivity, the lithium salt of the present invention is preferably a lithium ionic liquid. The molecular weight of —(R1O)nR2 is preferably in the range of 150 to 540 for example. This is because when the molecular weight is less than the above range, the lithium salt may not form a lithium ionic liquid, while when the molecular weight is higher than the above range, the viscosity of the lithium salt may increase to reduce ion conductivity.
Particularly, in the present invention, —(R1O)nR2 is preferably —(C2H4O)nCH3. In this case, “n” represents 0 to 12 as described above and is preferably in the range of 1 to 12, more preferably in the range of 3 to 12, even more preferably 5 to 9. This is because, when “n” is 1 or more, ion conductivity can be improved; when “n” is 3 or more, the lithium salt of the present invention can form a lithium ionic liquid; and further, when “n” is in the range of 5 to 9, a lithium ionic liquid having suitable viscosity can be obtained. When the lithium salt wherein —(R1O)nR2 is —(C2H4O)nCH3 is to be obtained, CH3 (OC2H4)nOH (polyethylene glycol monomethyl ether) described later may be used as a raw material, and in this case, “n” means the average polymerization degree of the ethylene oxide group.
The ratio (O/Li) of the number of oxygen atoms to the number of lithium atoms, derived from (R1O)nR2, is not particularly limited, and is for example preferably in the range of 2/1 to 90/1, still more preferably in the range of 6/1 to 30/1, and even more preferably 10/1 to 18/1.
The lithium salt of the present invention may be either solid or liquid, but is preferably liquid from the viewpoint of ion conductivity. When the lithium salt of the present invention is solid, it can be dissolved in a suitable solvent to form a liquid electrolyte. The solvent is not particularly limited as long as it can dissolve the lithium salt of the present invention. Examples of the solvent include ethylene carbonate, propylene carbonate, diethyl carbonate, dimethyl carbonate, γ-butyrolactone, diethylene glycol dimethyl ether, and ethylene glycol dimethyl ether. These solvents may be used singly or as a mixed solvent of two or more thereof.
A method for producing the lithium ion represented by the general formula (1) is not particularly limited, and specifically the method described in “B. Method for Producing Lithium Salt” can be mentioned.
B. Method for Producing Lithium Salt
Next, the method for producing a lithium salt of the present invention is described. The method for producing a lithium salt of the present invention comprises carrying out the following reaction formulae (1) and (2), thereby yielding the lithium salt.

[Chemical Formula 3]

LiCpH2p+1+R2(OR1)nOH→R2(OR1)nOLi+CpH2p+2↑  (Reaction Formula 1)

R2(OR1)nOLi+MFxCompound→LiMFxO(R1O)nR2  (Reaction Formula 2)

In the above-mentioned reaction formulae (1) and (2), “p” represents an integer of 1 to 4, “R1” represents —CmH2m— whereupon “m” is an integer of 1 to 4; “R2” represents —CkH2k+1 whereupon “k” is an integer of 1 to 8; “n” represents 0 to 12; “M” represents B, Si, Ge, P, As or Sb; and “X” represents the valence of “M”.
The present invention has an advantage that a lithium salt can be obtained by using an alkyl lithium and an MFx compound. In the conventional method for producing lithium salts, LiBH4, LiAlH4 etc. have been generally used as the starting materials, but these reagents easily react with water and thus have the problem of difficult handling and poor workability during production of the lithium salt. In the method for producing the lithium salt according to the present invention, on the other hand, the lithium salt can be obtained under relatively moderate conditions by using an alkyl lithium such as butyl lithium and an MFx compound such as BF3 gas or BF3 complex.
Next, the method for producing the lithium salt of the present invention is described by reference to the respective reactions.
1. Reaction Formula (1)
In the reaction formula (1), LiCpH2P+1 represents an alkyl lithium. This compound serves as a lithium source for the lithium salt obtained by the present invention. What “p” represents is an integer of 1 to 4, any of which may be similarly used to yield the objective compound, but “p” is preferably 4 which is an integer in the most common alkyl lithium. That is, LiCpH2P+1 is preferably normal butyl lithium (n-LiBu).
In the reaction formula (1), R2 (OR1)nOH is an OH derivative of the group represented by —(R1O)nR2 in the general formula (1). A description of “R1”, “R2” and “n” in R2(OR1)nOH is omitted because they are the same as described above in “A. Lithium Salt”. In the present invention, R2 (OR1)nOH is preferably CH3 (OCH2CH2)nOH.
Although the amounts of LiCpH2P+1 and R2(OR1)nOH used are not particularly limited, the molar ratio thereof is usually LiCpH2P+1:R2(OR1)nOH=1:1.
In the reaction formula (1), LiCpH2P+1 and R2(OR1)nOH described above are dissolved and reacted in a suitable solvent. Such solvent is not particularly limited as long as it can dissolve the above compounds and does not react with LiCpH2P+1. Examples of such solvent include tetrahydrofuran (THF), and dioxane. Although the reaction temperature in the reaction formula (1) is not particularly limited as long as side reactions can be inhibited, the reaction temperature is usually 0° C. or less, more preferably −20° C. or less.
By the reaction represented by the reaction formula (1), R2(OR1)nOLi can be obtained. By the reaction represented by the reaction formula (1), CpH2p+2 gas is usually generated. For example, when LiC4H8 is used, C4H9 gas is generated according to the reaction formula (1). Generation of C4H9 gas can be confirmed by gas chromatography (GC).
2. Reaction Formula (2)
In the reaction formula (2), R2(OR1)nOLi is obtained by the reaction represented by the reaction formula (1). The MFx compound is a compound giving the M−Fx moiety in the general formula (1). A description of “M” is omitted because it is the same as described above in “A. Lithium Salt”. The MFx compound refers specifically to a BF3 compound, an SiF4 compound, a GeF4 compound, a PF5 compound, an AsF5 compound or an SbF5 compound.
The BF3 compound, although not particularly limited as long as it gives a lithium salt represented by the general formula (1), includes for example BF3 and a BF3 complex. Because BF3 is gaseous at ordinary temperature and pressure, the reaction represented by the reaction formula (2) can be carried out by blowing BF3 gas into the reaction solution. On the other hand, the BF3 complex, although not particularly limited as long as it is a complex having an unshared electron pair coordinated and bonded with boron of BF3, includes for example BF3Et2O, BF3Me2O, BF3-THF, etc. Among them, BF3Et2O is preferable. Because the BF3 complex is usually liquid, the reaction represented by the reaction formula (2) can be carried out by adding a solution including the BF3 complex.
Although the amounts of R2(OR1)nOLi and MFx compound used are not particularly limited, the molar ratio thereof is usually in the range of R2(OR1)nOLi:MFx compound=1:1 to 1:2.
In the reaction formula (2), R2 (OR1)nOLi and the MFx compound are dissolved and reacted in a suitable solvent. Such solvent is not particularly limited as long as it can dissolve the above compounds. A description of the solvent is omitted because its specific examples are the same as used in the reaction formula (1). Although the reaction temperature in the reaction formula (2) is not particularly limited as long as side reactions can be inhibited, a description of the reaction temperature is omitted because the temperature is the same as used in the reaction formula (1).
In the present invention, it is preferable that the reactions represented by the reaction formulae (1) and (2) are successively conducted. That is, it is preferable that LiCpH2P+1 is reacted with R2(OR1)nOH (reaction formula (1)) and then the MFx compound is added to and reacted with the reaction solution (reaction formula (2)). By removing the solvent etc. from the resulting reaction solution, LiMFxO(R1O)nR2 represented by the general formula (1) is obtained.
The present invention is not limited to the embodiments described above. The embodiments described above are mere illustrative, and those having substantially the same constitution and the same working effect as in the technical idea described in the claims of the present invention are included in the technical scope of the present invention.
EXAMPLES
Hereinafter, the present invention is described in more detail by reference to the Examples.
Example 1
A lithium salt was prepared according to the following reaction formulae (i) and (ii):

[Chemical Formula 4]

n-BuLi+CH3(OCH2CH2)nOH→CH3(OCH2CH2)nOLi+C4H10↑  (Reaction Formula i)

CH3(OCH2CH2)nOLi+BF3Et2O→LiBF3O(CH2CH2O)nCH3+Et2O  (Reaction Formula ii)

A solution of 7.2 mmol n-butyl lithium (n-BuLi) dissolved in 10 mL tetrahydrofuran (THF), a solution of 7.2 mmol polyethylene glycol monomethyl ether (PEGMME, average molecular weight 350, average polymerization degree 7.2) dissolved in 10 mL THF, and a solution of 7.2 mmol BF3Et2O dissolved in 10 mL tetrahydrofuran (THF), were added in this order to a reaction container cooled at about −20° C. in an acetone bath and mixed with each other to yield a yellow liquid. Then, the reaction solution was returned gradually to room temperature and stirred overnight. Thereafter, the solvent was distilled away, and the reaction mixture was dried at 30° C. for 24 hours under reduced pressure to give a brown viscous liquid. A lithium metal piece was introduced into it and stirred for one day at room temperature, and then a trace amount of impurities reacting with the lithium metal were removed, whereby a brown viscous liquid (lithium ionic liquid) was obtained.
When an infrared absorption spectrum (IR spectrum) and nuclear magnetic resonance spectrum (NMR spectrum) of the resulting lithium ionic liquid were measured, it was confirmed that the objective product had been synthesized. The result of the IR spectrum is shown in FIG. 1, the result of the 1H-NMR spectrum is shown in FIG. 2, and the result of the 13C-NMR spectrum is shown in FIG. 3. From the result of IR spectrum, a B—O bond could be confirmed, and it was suggested that the objective product had been synthesized. From the result of 1H-NMR spectrum and 13C-NMR spectra, it was suggested that the objective product had been synthesized.
Example 2
A lithium ionic liquid was obtained in the same manner as in Example 1 except that PEGMME having an average polymerization degree of 3 was used in place of the PEGMME having an average polymerization degree of 7.2. When the obtained IR spectrum, 1H-NMR spectrum and 13C-NMR spectrum were measured, it was suggested that the objective product had been synthesized.
Example 3
A lithium ionic liquid was obtained in the same manner as in Example 1 except that PEGMME having an average polymerization degree of 11.8 was used in place of the PEGMME having an average polymerization degree of 7.2. When the obtained IR spectrum, 1H-NMR spectrum and 13C-NMR spectrum were measured, it was suggested that the objective product had been synthesized.
Evaluation
(1) Measurement of Ion Conductivity
The electrolyte was injected into between 2 stainless metal blocking electrodes and measured for its alternating-current impedance at 0 to 80° C. with a frequency response analyzer (FRA, trade name: Solartron 1260, manufactured by Solartron), to measure the ion conductivity of the electrolyte.
FIG. 4 is a graph showing the results of ion conductivity measurement of the lithium ionic liquids obtained in Examples 1 to 3. The solid line in the figure is obtained by subjecting the experimental data to a nonlinear least-squares method by a VTF equation. As shown in FIG. 4, the lithium ionic liquids obtained in Examples 1 to 3 were revealed to show excellent ion conductivity.
(2) Cyclic Voltammetry Measurement
Cyclic voltammetry measurement (CV measurement) of the electrolyte was carried out at 50° C. by using Solartron 1260 (potentiostat/galvanostat, manufactured by Solartron) and a 3-electrode cell (counter electrode and reference electrode: lithium foils, working electrode: stainless steel (surface area 0.01 cm2)).
FIG. 5 is a graph showing the result of CV measurement of the lithium ionic liquid obtained in Example 1. The sweep velocity was 2 mV/s. As shown in FIG. 5, the lithium ionic liquid obtained in Example 1 was revealed to have a broad potential window.
(3) Charge-Discharge Properties
Preparation of A Coin Cell-Type Secondary Cell
First, a cathode of a coin cell-type secondary battery was prepared. As a binder, PVDF (poly(vinylidene fluoride)) was prepared and dissolved in 1-pyrrolidinone to yield a uniform PVDF solution. Next, LiNi0.8Co0.2O2 (obtained by heating a mixture of Li2O, NiO and CoO at 720° C. for 24 hours) was prepared as a cathode active material, and acetylene black (AB) was prepared as a conductive material, and these materials were ground and then added gradually to the above PVDF solution. Thereafter, this mixture was stirred vigorously for 24 hours to yield highly viscous slurry. Thereafter, this slurry was applied onto an aluminum substrate prepared as a collector and dried to produce a cathode. The starting materials were prepared such that LiNi0.8Co0.2O2:PVDF:AB=80:10:10.
Then, an Li metal foil was prepared as an anode of a coin cell-type secondary battery. Thereafter, a coin cell-type secondary battery having a constitution of the cathode/electrolyte-charged Celgard/anode in a glove box filled with argon was prepared.
Method of Evaluating Charge-Discharge Properties
The charge-discharge properties of the coin cell-type secondary battery were evaluated by galvanostatic measurement at a current density of 0.1 mA/cm2 with a battery charging and discharging device (HJ-SM8 system, manufactured by Hokuto Denko Corporation).
Results
FIG. 6 is a graph showing the charge-discharge properties of the coin cell-type secondary battery using the lithium ionic liquid obtained in Example 1. FIG. 6 shows charge-discharge properties in second discharge charge (cutoff voltage: 2.5 to 3.9 V). As shown in FIG. 6, it was revealed that when the lithium ionic liquid obtained in Example 1 was used, a lithium secondary battery having excellent charge-discharge properties could be obtained.

## Claims

1. A lithium salt comprising a structure represented by the general formula (1):



and in the general formula (1), “M” represents B, Si, Ge, P, As or Sb; “X” represents a valence of “M”; “R1” represents —CmH2m— in which “m” is an integer of 1 to 4; “R2” represents —CkH2k+1 in which “k” is an integer of 1 to 8; and “n” represents 7 to 12.

2. The lithium salt according to claim 1, wherein M−Fx is B−F3 in the general formula (1).

3. The lithium salt according to claim 1, wherein M−Fx is B−F3, “R1” is —C2H4—, and “R2” is —CH3 in the general formula (1).

4. A method for producing a lithium salt, comprising steps of carrying out the following reactions (1) and (2):


[Chemical Formula 2]



LiCpH2p+1+R2(OR1)nOH→R2(OR1)nOLi+CpH2p+2↑  (Reaction Formula 1)



R2(OR1)nOLi+MFxCompound→LiMFxO(R1O)nR2  (Reaction Formula 2)

and in the reaction formulae (1) and (2), “p” represents an integer of 1 to 4; “R1” represents —CmH2m— in which “m” is an integer of 1 to 4; “R2” represents —CkH2k+1 in which “k” is an integer of 1 to 8; “n” represents 0 to 12; “M” represents B, Si, Ge, P, As or Sb; and “X” represents a valence of “M”.

5. A lithium salt comprising a structure represented by the general formula (1a):



and in the general formula (1a), “M” represents B, Si, Ge, P, As or Sb; “X” represents a valence of “M”; and “n” represents 5 to 12.

6. The lithium salt according to claim 5, wherein M−Fx is B−F3 in the general formula (1a).