JP3730861B2 - Electrolytes for electrochemical devices, electrolytes or solid electrolytes thereof, and batteries - Google Patents

Description

[0001]
BACKGROUND OF THE INVENTION
The present invention relates to an electrolyte, an electrolytic solution, or a solid electrolyte that exhibits excellent cycle characteristics used for electrochemical devices such as lithium batteries, lithium ion batteries, and electric double layer capacitors, and a battery using the same.
[0002]
[Prior art]
With the development of portable devices in recent years, the development of electrochemical devices using electrochemical phenomena such as batteries and capacitors as a power source has become active. Further, as an electrochemical device other than the power source, an electrochromic display (ECD) in which a color change is caused by an electrochemical reaction can be given.
[0003]
These electrochemical devices are generally composed of a pair of electrodes and an ionic conductor filling them. As the ionic conductor, a solution in which a salt (AB) composed of a cation (A ⁺ ) and an anion (B ⁻ ) called an electrolyte is dissolved in a solvent, a polymer, or a mixture thereof is used. When this electrolyte is dissolved, it dissociates into a cation and an anion, and conducts ions. In order to obtain the ionic conductivity necessary for the device, it is necessary that this electrolyte is dissolved in a sufficient amount in a solvent or a polymer. Actually, a solvent other than water is often used as a solvent, and there are currently only a few types of electrolytes having sufficient solubility in such organic solvents and polymers. For example, as an electrolyte for a lithium battery, LiClO ₄ , LiPF ₆ , LiBF ₄ , LiAsF ₆ , LiN (SO ₂ CF ₃ ) ₂ , LiN (SO ₂ C ₂ F ₅ ) ₂ , LiN (SO ₂ CF ₃ ) (SO ₂ C ₄ F ₉ ) and LiCF ₃ SO ₃ only. The cation portion is often determined by the device, such as the lithium ion of a lithium battery, but the anion portion can be used if the condition that the solubility is high is satisfied.
[0004]
While the application range of devices is diversifying, the optimum electrolyte for each application is being searched for, but at present, optimization is reaching its limit because there are few types of anions. Moreover, the existing electrolyte has various problems, and an electrolyte having a novel anion portion is desired. Specifically, ClO ₄ ions are explosive and AsF ₆ ions are toxic and cannot be used for safety reasons. The only practically used LiPF ₆ also has problems such as heat resistance and hydrolysis resistance. LiN (CF ₃ SO ₂ ) ₂ , LiN (SO ₂ C ₂ F ₅ ) ₂ , LiN (SO ₂ CF ₃ ) (SO ₂ C ₄ F ₉ ) and LiCF ₃ SO ₃ have high stability and ionic conductivity. It is a very excellent electrolyte because it is high, but it is difficult to use because the aluminum current collector in the battery is corroded in a state where a potential is applied.
[0005]
[Concrete means for solving the problem]
As a result of intensive studies in view of the problems of the prior art, the present inventors have found a system in which an electrolyte having a novel chemical structural feature and a conventional one are combined, and have reached the present invention.
[0006]
That is, the present invention relates to a compound comprising a chemical structural formula represented by general formula (1) and a compound comprising a chemical structural formula represented by general formula (2), general formula (3), or general formula (4). An electrolyte for at least one lithium battery and lithium ion battery ,
[0007]
[Chemical 2]
[0008]
M is B or P, A ^{a +} is Li ion, a is 1, b is 1, p is 1, m is 1 to 2 , n is 1 to 4 , q is 0 or 1 R ¹ represents C ₁ -C ₁₀ alkylene, C ₁ -C ₁₀ halogenated alkylene, C ₆ -C ₂₀ arylene, or C ₆ -C ₂₀ halogenated arylene (these alkylene and arylenes). May have a substituent or a hetero atom in the structure, and m R ¹ may be bonded to each other.), R ² is halogen, X ¹ and X ² are O, And x, y, and z are each independently an electrolyte for a lithium battery and a lithium ion battery , each representing 1 to 8, and the lithium battery and the lithium ion battery that are obtained by dissolving the electrolyte in a non-aqueous solvent . An electrolyte or a solution of the electrolyte in a polymer. A lithium battery and a solid electrolyte for a lithium ion battery , and at least a positive electrode, a negative electrode, an electrolytic solution or a solid electrolyte, and the battery containing the electrolyte according to claim 1 in the electrolytic solution or the solid electrolyte are provided.
[0009]
The alkyl, alkyl halide, aryl, and aryl halide used in the present invention include those having other functional groups such as a branch, a hydroxyl group, and an ether bond.
[0010]
Hereinafter, the present invention will be described in more detail.
[0011]
Here, first, specific examples of the compound represented by the general formula (1) used in the present invention are shown below.
[0012]
[Chemical 3]
[0013]
[Formula 4]
[0015]
[Chemical 6]
[0016]
Here, lithium ions may be mentioned as A ^{a +} .
[0018]
The electrolyte represented by the general formula (1), which is a part of the structure of the present invention, has an ionic metal complex structure, and M at the center thereof is a transition metal, group III, group IV of the periodic table, Or selected from group V elements. Preferably, any of Al, B, V, Ti, Si, Zr, Ge, Sn, Cu, Y, Zn, Ga, Nb, Ta, Bi, P, As, Sc, Hf, or Sb, and B or P is preferable. Although various elements can be used as the central M, Al, B, V, Ti, Si, Zr, Ge, Sn, Cu, Y, Zn, Ga, Nb, Ta, Bi, P, As , Sc, Hf, or Sb is relatively easy to synthesize. Further, in the case of B or P, in addition to the ease of synthesis, it has excellent properties in all aspects such as low toxicity, stability, and cost.
[0019]
Next, the part of the ligand that is a feature of the electrolyte (ionic metal complex) represented by the general formula (1) will be described. Hereinafter, the organic or inorganic part bonded to M is referred to as a ligand.
[0020]
R ¹ in the general formula (1) is selected from C _{1 to} C ₁₀ alkylene, C _{1 to} C ₁₀ halogenated alkylene, C _{6 to} C ₂₀ arylene, or C _{6 to} C ₂₀ halogenated arylene. These alkylenes and arylenes may have a substituent or a hetero atom in the structure. Specifically, instead of hydrogen on alkylene and arylene, halogen, chain or cyclic alkyl group, aryl group, alkenyl group, alkoxy group, aryloxy group, sulfonyl group, amino group, cyano group, carbonyl group, acyl group , An amide group, a hydroxyl group, and a structure in which nitrogen, sulfur, or oxygen is introduced in place of carbon on alkylene and arylene. Furthermore, plural R ^{1 s} may be bonded to each other, and examples thereof include a ligand such as ethylenediaminetetraacetic acid.
[0021]
R ² is preferably a halogen, preferably an electron-withdrawing group, particularly fluorine. When R ² is fluorine, the ion conductivity is very high due to the improvement in dissociation of the electrolyte due to its strong electron-withdrawing property and the effect of improving the mobility due to the reduction in size.
[0022]
X ¹ and X ² are each independently O, and the ligand is bonded to M through these heteroatoms. Here, it is not impossible to combine other than O, but it is very complicated in synthesis. Since this compound has a bond of M by X ¹ and X ² in the same ligand, these ligands constitute a chelate structure with M. Due to the effect of this chelate, the heat resistance, chemical stability, and hydrolysis resistance of this compound are improved. The constant q in this ligand is 0 or 1. Particularly, 0 is preferable because this chelate ring is a five-membered ring, so that the chelate effect is exerted most strongly and the stability is increased.
[0024]
The constants m and n related to the number of ligands described so far are determined by the type of M at the center, and m is preferably 1 to 2 and n is preferably 1 to 4 .
[0025]
Next, specific examples of the compounds represented by the general formula (2), the general formula (3), and the general formula (4) include LiCF ₃ SO ₃ , LiN (SO ₂ CF ₃ ) ₂ , LiN (SO ₂ C _{2). F 5) 2, LiN (SO} 2 CF 3) (SO 2 C 4 F 9), and _{LiC (SO 2 CF 3) 3} , include like. When these electrolytes are used alone, the aluminum current collector in the battery is corroded in a state where an electric potential is applied, so that there is a problem that the capacity decreases when the charge / discharge cycle is repeated. In the present invention, it is possible to prevent corrosion of the aluminum current collector by using the electrolyte having the sulfonyl group and the electrolyte of the general formula (1) in combination. Although the details of the principle are not clear, it is presumed that the electrolyte of the general formula (1) is slightly decomposed on the electrode surface to form a film composed of the ligand on the aluminum surface, thereby preventing the corrosion. .
[0026]
The usage ratio of these electrolytes is preferably in the following range in consideration of the cycle characteristics of the electrochemical device and the effect of improving the storage stability. The molar ratio of the electrolyte of general formula (1) and the electrolytes of general formula (2), general formula (3), and general formula (4) is 5:95 to 95: 5, preferably 30:70 to 70:30. It is. When the electrolyte of the general formula (1) is less than 5, since the effect of preventing corrosion of aluminum is small, the cycle characteristics and storage stability are deteriorated, and when it is larger than 95, the general formula (2), general The high ion conductivity and electrochemical stability of the formula (3) and the general formula (4) cannot be sufficiently exhibited.
[0027]
When an electrochemical device is constituted using the electrolyte of the present invention, its basic components are composed of an ion conductor, a negative electrode, a positive electrode, a current collector, a separator, a container, and the like.
[0028]
As the ionic conductor, a mixture of an electrolyte and a non-aqueous solvent or polymer is used. If a non-aqueous solvent is used, this ionic conductor is generally called an electrolytic solution, and if a polymer is used, it becomes a polymer solid electrolyte. The polymer solid electrolyte includes those containing a non-aqueous solvent as a plasticizer.
[0029]
The non-aqueous solvent is not particularly limited as long as it is an aprotic solvent capable of dissolving the electrolyte of the present invention, and examples thereof include carbonates, esters, ethers, lactones, nitriles, amides, sulfones. Can be used. Moreover, not only a single solvent but 2 or more types of mixed solvents may be sufficient. Specific examples include propylene carbonate, ethylene carbonate, diethyl carbonate, dimethyl carbonate, methyl ethyl carbonate, dimethoxyethane, acetonitrile, propionitrile, tetrahydrofuran, 2-methyltetrahydrofuran, dioxane, nitromethane, N, N-dimethylformamide, dimethyl sulfoxide. , Sulfolane, and γ-butyrolactone.
[0030]
However, when two or more kinds of mixed solvents are used, in the case of an electrolyte in which A ^{a + in} the general formula (1) is Li ion, among these nonaqueous solvents, an aprotic solvent having a dielectric constant of 20 or more and a dielectric constant Is preferably dissolved in a mixed solvent composed of 10 or less aprotic solvents. In particular, this lithium salt has low solubility in an aprotic solvent having a dielectric constant of 10 or less, such as diethyl ether, dimethyl carbonate, etc., and sufficient ionic conductivity cannot be obtained by itself, and conversely, an aprotic property having a dielectric constant of 20 or more. Although the solvent alone has high solubility, its viscosity is also high, so that ions do not easily move and sufficient ionic conductivity cannot be obtained. If these are mixed, appropriate solubility and mobility can be ensured, and sufficient ionic conductivity can be obtained.
[0031]
The polymer that dissolves the electrolyte is not particularly limited as long as it is an aprotic polymer. Examples thereof include polymers having polyethylene oxide in the main chain or side chain, homopolymers or copolymers of polyvinylidene fluoride, methacrylic acid ester polymers, polyacrylonitrile and the like. When a plasticizer is added to these polymers, the above-mentioned aprotic non-aqueous solvent can be used. Mixing the electrolyte concentration of the present invention in these ion conductors in the, 0.1 mol / dm ³ or more, the saturation concentration or less, preferably, 0.5 mol / dm ³ or more and 1.5 mol / dm ³ or less. If the concentration is lower than 0.1 mol / dm ³ , the ion conductivity is low, which is not preferable.
[0032]
Although it does not specifically limit as a negative electrode material, In the case of a lithium battery, the alloy of lithium metal and lithium and another metal is used. In the case of a lithium ion battery, a material using a phenomenon called intercalation such as carbon, natural graphite, or metal oxide obtained by firing a polymer, an organic substance, pitch or the like is used. In the case of an electric double layer capacitor, activated carbon, porous metal oxide, porous metal, conductive polymer, or the like is used.
[0033]
As the cathode material is not particularly limited, a lithium battery and a lithium ion battery, for _{example, LiCoO 2, LiNiO 2, LiMnO} 2, lithium-containing oxides such as _{LiMn 2 O 4, TiO 2,} V 2 O 5, MoO Oxides such as ₃ , sulfides such as TiS ₂ and FeS, or conductive polymers such as polyacetylene, polyparaphenylene, polyaniline, and polypyrrole are used. In the case of an electric double layer capacitor, activated carbon, porous metal oxide, porous metal, conductive polymer, or the like is used.
[0034]
【Example】
EXAMPLES Hereinafter, although an Example demonstrates this invention concretely, this invention is not limited by this Example.
[0035]
Example 1
In a mixed solvent of 50% by volume of ethylene carbonate and 50% by volume of dimethyl carbonate,
[0036]
[Chemical 7]
[0037]
An electrolyte solution prepared by dissolving 0.05 mol / l of a lithium borate derivative having the structure: 0.95 mol / l of LiN (SO ₂ C ₂ F ₅ ) ₂ was prepared, and the ionic conductivity was measured using an AC bipolar cell. Was measured. As a result, the ionic conductivity at 25 ° C. was 7.2 mS / cm.
[0038]
Next, a corrosion test of the aluminum current collector was performed using this electrolytic solution. The test cell was a beaker type having aluminum as a working electrode, a counter electrode and lithium metal as a reference electrode. When the working electrode was held at 5 V (Li / Li ⁺ ), no current flowed. After the test, the surface of the working electrode was observed with SEM, but no change was observed compared to before the test.
[0039]
Furthermore, using this electrolytic solution, a half cell was produced using LiCoO ₂ as a positive electrode material, and a battery charge / discharge test was actually performed. The test cell was produced as follows. To 90 parts by weight of LiCoO ₂ powder, 5 parts by weight of polyvinylidene fluoride (PVDF) as a binder and 5 parts by weight of acetylene black as a conductive material were mixed, and N, N-dimethylformamide was further added to form a paste. The paste was applied on an aluminum foil and dried to obtain a test positive electrode body. Lithium metal was used for the negative electrode. Then, using the glass fiber filter as a separator, an electrolyte was immersed in the separator to assemble a cell.
[0040]
Next, a constant current charge / discharge test was performed under the following conditions. Both charging and discharging were performed at a current density of 0.35 mA / cm ² , charging was performed at 4.2 V, and discharging was performed up to 3.0 V (vs. Li / Li ⁺ ). As a result, the initial discharge capacity was 118 mAh / g (capacity of the positive electrode). Moreover, although charging / discharging was repeated 100 times, the capacity | capacitance of the 100th time obtained the result of 95% of the first time.
[0041]
Example 2
In a mixed solvent of 50 vol% propylene carbonate and 50 vol% diethyl carbonate, 0.10 mol / l of a lithium borate derivative having the same structure as in Example 1 and 0.90 mol / l of LiN (SO ₂ CF ₃ ) ₂ Was prepared, and the ionic conductivity was measured with an AC bipolar cell. As a result, the ionic conductivity at 25 ° C. was 8.8 mS / cm.
[0042]
Next, in the same manner as in Example 1, a corrosion test of the aluminum current collector was performed using this electrolytic solution. When the working electrode was held at 5 V (Li / Li ⁺ ), no current flowed. After the test, the surface of the working electrode was observed with SEM, but no change was observed compared to before the test.
[0043]
Furthermore, a half cell using LiCoO ₂ as a positive electrode material was produced in the same manner as in Example 1 using this electrolytic solution, and a constant current charge / discharge test was performed under the following conditions. Both charging and discharging were performed at a current density of 0.35 mA / cm ² , charging was performed at 4.2 V, and discharging was performed up to 3.0 V (vs. Li / Li ⁺ ). As a result, the initial discharge capacity was 115 mAh / g (positive electrode capacity). Moreover, although charging / discharging was repeated 100 times, the capacity | capacitance of the 100th time obtained the result of 88% of the first time.
[0044]
Example 3
In a mixed solvent of 50% by volume of ethylene carbonate and 50% by volume of dimethyl carbonate, 0.05 mol / l of lithium borate derivative having the same structure as in Example 1 and LiN (SO ₂ CF ₃ ) (SO ₂ C ₄ F ₉ ) Was dissolved in 0.95 mol / l, and the ionic conductivity was measured with an AC bipolar cell. As a result, the ionic conductivity at 25 ° C. was 6.5 mS / cm.
[0045]
Next, in the same manner as in Example 1, a corrosion test of the aluminum current collector was performed using this electrolytic solution. When the working electrode was held at 5 V (Li / Li ⁺ ), no current flowed. After the test, the surface of the working electrode was observed with SEM, but no change was observed compared to before the test.
[0046]
Furthermore, a half cell using LiCoO ₂ as a positive electrode material was produced in the same manner as in Example 1 using this electrolytic solution, and a constant current charge / discharge test was performed under the following conditions. Both charging and discharging were performed at a current density of 0.35 mA / cm ² , charging was performed at 4.2 V, and discharging was performed up to 3.0 V (vs. Li / Li ⁺ ). As a result, the initial discharge capacity was 120 mAh / g (capacity of the positive electrode). Moreover, although charging / discharging was repeated 100 times, the capacity | capacitance of the 100th time obtained the result of 91% of the first time.
[0047]
Example 4
In a mixed solvent of 50% by volume of ethylene carbonate and 50% by volume of dimethyl carbonate, 0.95 mol / l of lithium borate derivative having the same structure as in Example 1 and LiN (SO ₂ CF ₃ ) (SO ₂ C ₄ F ₉ ) Was dissolved in 0.05 mol / l, and the ionic conductivity was measured with an AC bipolar cell. As a result, the ionic conductivity at 25 ° C. was 6.9 mS / cm.
[0048]
Next, in the same manner as in Example 1, a corrosion test of the aluminum current collector was performed using this electrolytic solution. When the working electrode was held at 5 V (Li / Li ⁺ ), no current flowed. After the test, the surface of the working electrode was observed with SEM, but no change was observed compared to before the test.
[0049]
Furthermore, a half cell using LiCoO ₂ as a positive electrode material was produced in the same manner as in Example 1 using this electrolytic solution, and a constant current charge / discharge test was performed under the following conditions. Both charging and discharging were performed at a current density of 0.35 mA / cm ² , charging was performed at 4.2 V, and discharging was performed up to 3.0 V (vs. Li / Li ⁺ ). As a result, the initial discharge capacity was 120 mAh / g (capacity of the positive electrode). Moreover, although charging / discharging was repeated 100 times, the capacity | capacitance of the 100th time obtained the result of 93% of the first time.
[0050]
Example 5
Acetonitrile was added to 70 parts by weight of polyethylene oxide having an average molecular weight of 10000 to prepare a solution, and 5 parts by weight of a lithium borate derivative having the same structure as in Example 1, LiN (SO ₂ CF ₃ ) (SO ₂ C ₄ F ₉ ) was added in an amount of 25 parts by weight, which was cast on glass and dried to remove the solvent acetonitrile, thereby preparing a polymer solid electrolyte membrane.
[0051]
Next, a corrosion test of the aluminum current collector was performed using this polymer solid electrolyte membrane. This film was sandwiched between an aluminum electrode and a lithium electrode as working electrodes, and measured by pressure bonding. When the working electrode was held at 5 V (Li / Li ⁺ ), no current flowed. After the test, the surface of the working electrode was observed with SEM, but no change was observed compared to before the test.
[0052]
Next, using this polymer solid electrolyte membrane as an electrolyte and a separator, a half cell using LiCoO ₂ as a positive electrode material was produced in the same manner as in Example 1, and constant current charge / discharge was performed at 70 ° C. under the following conditions. The test was conducted. Both charging and discharging were performed at a current density of 0.1 mA / cm ² , charging was performed at 4.2 V, and discharging was performed up to 3.0 V (vs. Li ^/ Li ⁺ ). As a result, the initial discharge capacity was 120 mAh / g (capacity of the positive electrode). Moreover, although charging / discharging was repeated 100 times, the capacity | capacitance of the 100th time obtained the result of 91% of the first time.
[0053]
Comparative Example 1
An electrolytic solution in which 1.0 mol / l of LiN (SO ₂ C ₂ F ₅ ) ₂ was dissolved in a mixed solvent of 50% by volume of ethylene carbonate and 50% by volume of dimethyl carbonate was prepared. Was used to conduct corrosion tests on aluminum current collectors. When the working electrode was held at 5 V (Li / Li ⁺ ), a corrosion current was observed. Further, when the surface of the working electrode was observed with an SEM after the test, many pits that were thought to be due to corrosion were observed on the surface.
[0054]
Next, a half cell using LiCoO ₂ as a positive electrode material was prepared in the same manner as in Example 1 using this electrolytic solution, and a constant current charge / discharge test was performed under the following conditions. Both charging and discharging were performed at a current density of 0.35 mA / cm ² , charging was performed at 4.2 V, and discharging was performed up to 3.0 V (vs. Li / Li ⁺ ). As a result, the initial discharge capacity was 117 mAh / g (capacity of the positive electrode). Moreover, although charging / discharging was repeated 100 times, the capacity | capacitance of the 100th time obtained the result of 69% of the first time.
[0055]
Comparative Example 2
An electrolyte solution in which 1.0 mol / l of LiN (SO ₂ CF ₃ ) ₂ was dissolved in a mixed solvent of 50 vol% propylene carbonate and 50 vol% diethyl carbonate was prepared, and this electrolyte solution was used in the same manner as in Example 1. The corrosion test of the aluminum current collector was conducted. When the working electrode was held at 5 V (Li / Li ⁺ ), a corrosion current was observed. Further, when the surface of the working electrode was observed with an SEM after the test, many pits that were thought to be due to corrosion were observed on the surface.
[0056]
Next, a half cell using LiCoO ₂ as a positive electrode material was prepared in the same manner as in Example 1 using this electrolytic solution, and a constant current charge / discharge test was performed under the following conditions. Both charging and discharging were performed at a current density of 0.35 mA / cm ² , charging was performed at 4.2 V, and discharging was performed up to 3.0 V (vs. Li / Li ⁺ ). As a result, the initial discharge capacity was 112 mAh / g (positive electrode capacity). Moreover, although charging / discharging was repeated 100 times, the capacity | capacitance of the 100th time obtained the result of 67% of the first time.
[0057]
Comparative Example 3
An electrolyte solution in which 1.0 mol / l of LiN (SO ₂ CF ₃ ) (SO ₂ C ₄ F ₉ ) was dissolved in a mixed solvent of 50% by volume of ethylene carbonate and 50% by volume of dimethyl carbonate was prepared. In addition, a corrosion test of the aluminum current collector was performed using this electrolytic solution. When the working electrode was held at 5 V (Li / Li ⁺ ), a corrosion current was observed. Further, when the surface of the working electrode was observed with an SEM after the test, many pits that were thought to be due to corrosion were observed on the surface.
[0058]
Next, a half cell using LiCoO ₂ as a positive electrode material was prepared in the same manner as in Example 1 using this electrolytic solution, and a constant current charge / discharge test was performed under the following conditions. Both charging and discharging were performed at a current density of 0.35 mA / cm ² , charging was performed at 4.2 V, and discharging was performed up to 3.0 V (vs. Li / Li ⁺ ). As a result, the initial discharge capacity was 118 mAh / g (capacity of the positive electrode). Moreover, although charging / discharging was repeated 100 times, the capacity | capacitance of the 100th time obtained the result of 74% of the first time.
[0059]
【The invention's effect】
The present invention is an electrolyte having excellent cycle characteristics and storage characteristics as compared with conventional electrolytes used for electrochemical devices such as lithium batteries, lithium ion batteries, and electric double layer capacitors. In addition, a battery using these is made possible.

Claims (5)

It consists of at least one of the compound consisting of the chemical structural formula shown by the general formula (1) and the compound consisting of the chemical structural formula shown by the general formula (2), the general formula (3), or the general formula (4). Electrolyte for lithium battery and lithium ion battery .
M is B or P,
A ^{a +} is Li ion,
a is 1,
b is 1,
p is 1,
m is 1-2 ,
n is 1 to 4 ,
q represents 0 or 1 respectively;
R ¹ is C ₁ -C ₁₀ alkylene, C ₁ -C ₁₀ halogenated alkylene, C ₆ -C ₂₀ arylene, or C ₆ -C ₂₀ halogenated arylene (these alkylene and arylene are in the structure) May have a substituent or a hetero atom, and m R ¹ may be bonded to each other.)
R ² is halogen,
X ¹ and X ² are O,
x, y, and z are each independently 1 to 8; An electrolyte for lithium batteries and lithium ion batteries, comprising the electrolyte according to claim 1 dissolved in a non-aqueous solvent. 3. The electrolysis for lithium battery and lithium ion battery according to claim 2 , wherein the non-aqueous solvent is a mixed solvent comprising an aprotic solvent having a dielectric constant of 20 or more and an aprotic solvent having a dielectric constant of 10 or less. liquid. A solid electrolyte for a lithium battery and a lithium ion battery, comprising the electrolyte according to claim 1 dissolved in a polymer.   A battery comprising at least a positive electrode, a negative electrode, an electrolyte solution or a solid electrolyte, wherein the electrolyte solution or solid electrolyte contains the electrolyte according to claim 1.