Patent Application
20220352546
The present disclosure relates to a solid electrolyte material and a battery using it.
Japanese Unexamined Patent Application Publication No. 2011-129312 discloses an all solid state battery using a sulfide solid electrolyte. International Publication No. WO 2018/025582 discloses a solid electrolyte material represented by Li6-3zYzX6 (0<z<2 is satisfied, and X is Cl or Br).
One non-limiting and exemplary embodiment provides a solid electrolyte material having a low melting point and a high ion conductivity.
In one general aspect, the techniques disclosed here feature a solid electrolyte material comprising Li, Y, X, and O, here X is one selected from the group consisting of F, Cl, Br, and I, and the molar ratio of O to Y is greater than 0.01 and less than 0.52.
The present disclosure provides a solid electrolyte material having a low melting point and a high ion conductivity.
Additional benefits and advantages of the disclosed embodiments will become apparent from the specification and drawings. The benefits and/or advantages may be individually obtained by the various embodiments and features of the specification and drawings, which need not all be provided in order to obtain one or more of such benefits and/or advantages.
Hereinafter, embodiments of the present disclosure are described with reference to the drawings.
The solid electrolyte material according to a first embodiment comprises Li, Y, X, and O. Here, X is one selected from the group consisting of F, Cl, Br, and I. The molar ratio of O to Y is greater than 0.01 and less than 0.52. The solid electrolyte material according to the first embodiment has a low melting point. Furthermore, the solid electrolyte material according to the first embodiment has a high lithium ion conductivity. Here, a low melting point is, for example, 504° C. or less. That is, the solid electrolyte material according to the first embodiment can have a melting point of, for example, 504° C. or less. When the solid electrolyte material is a multiphase material, the melting point of the solid electrolyte material means the highest temperature in the melting points of the solid electrolyte material. The high lithium ion conductivity is, for example, 1×10−5 S/cm or more. That is, the solid electrolyte material according to the first embodiment can have, for example, a melting point of 504° C. or less and an ion conductivity of 1×10−5 S/cm or more.
The solid electrolyte material according to the first embodiment can be used for obtaining an all solid state battery having excellent charge and discharge characteristics. The all solid state battery may be a primary battery or a secondary battery.
The solid electrolyte material according to the first embodiment desirably does not contain sulfur. A solid electrolyte material not containing sulfur does not generate hydrogen sulfide, even if it is exposed to the atmosphere, and is therefore excellent in safety. The sulfide solid electrolyte disclosed in Japanese Unexamined Patent Application Publication No. 2011-129312 may generate hydrogen sulfide when it is exposed to the atmosphere.
The solid electrolyte material according to the first embodiment may consist of Li, Y, X, and O only.
In order to enhance the ion conductivity of the solid electrolyte material, the solid electrolyte material according to the first embodiment may further include at least one selected from the group consisting of Mg, Ca, Zn, Sr, Ba, Al, Sc, Ga, Bi, La, Zr, Hf, Ta, and Nb.
The transition metal included in the solid electrolyte material according to the present embodiment may be only Y excluding elements included as inevitable impurities.
X may be Cl. Such a solid electrolyte material has a low melting point and a high ion conductivity.
Hereinafter, a first example and a second example of the solid electrolyte material according to the first embodiment will be described. The first example of the solid electrolyte material according to the first embodiment is described as a “first solid electrolyte material”, and the second example of the solid electrolyte material according to the first embodiment is described as a “second solid electrolyte material”.
The X-ray diffraction pattern of the first solid electrolyte material can be measured using Cu-Kα rays. In the obtained X-ray diffraction pattern, peaks may be present in diffraction angle 2θ ranges of 15.2° or more and 16.4° or less, 16.7° or more and 18.6° or less, 30.8° or more and 31.9° or less, 33.2° or more and 34.3° or less, 40.3° or more and 41.4° or less, 48.2° or more and 49.3° or less, and 53.0° or more and 54.2° or less. Such a solid electrolyte material has a low melting point and a high ion conductivity.
In order to lower the melting point of the solid electrolyte material, the molar ratio of Li to Y may be 2.2 or more and 2.56 or less, and the molar ratio of X to Y may be 3.5 or more and 5.9 or less.
In order to further lower the melting point of the solid electrolyte material, the molar ratio of Li to Y may be 2.49 or more and 2.56 or less, and the molar ratio of X to Y may be 3.91 or more and 5.29 or less.
The molar ratio of O to Y may be, for example, 1.0 or less.
The upper limit and lower limit of the molar ratio of O to Y can be defined by any combination selected from the numerical values of 0.01, 0.04, 0.23, and 0.50.
In order to lower the melting point of the solid electrolyte material, the molar ratio of O to Y may be greater than 0.01 and 0.50 or less.
The molar ratio A of O to Y in the surface region of the second solid electrolyte material may be greater than the molar ratio B of O to Y in the whole second solid electrolyte material. Such a solid electrolyte material has a low melting point and a high ion conductivity. As an example, the value of the molar ratio A may be greater than twice the value of the molar ratio B.
Here, the surface region of the second solid electrolyte material means the region from the surface of the second solid electrolyte material to a depth of about 5 nm in the inward direction.
In order for the solid electrolyte material to have a high ion conductivity, the molar ratio A may be 2.50 or less.
The X-ray diffraction pattern of the second solid electrolyte material can be measured using Cu-Kα rays. In the obtained X-ray diffraction pattern, peaks may be present in diffraction angle 2θ ranges of 15.2° or more and 16.3° or less, 16.7° or more and 18.5° or less, 30.8° or more and 31.9° or less, 33.1° or more and 34.2° or less, 40.3° or more and 41.4° or less, 48.2° or more and 49.3° or less, and 53.1° or more and 54.2° or less. Such a solid electrolyte material has a low melting point and a high ion conductivity.
In order for the solid electrolyte material to have a low melting point and a high ion conductivity, the molar ratio of O to Y in the whole second solid electrolyte material may be greater than 0.01 and 0.33 or less.
The shape of the solid electrolyte material according to the first embodiment is not limited. Examples of the shape are needle, spherical, and oval spherical shapes. The solid electrolyte material according to the first embodiment may be a particle. The solid electrolyte material according to the first embodiment may be formed so as to have a pellet or planar shape.
When the shape of the solid electrolyte material according to the first embodiment is a particulate shape (e.g., spherical), the solid electrolyte material according to the first embodiment may have a median diameter of 0.1 μm or more and 100 μm or less.
In order to enhance the ion conductivity of the solid electrolyte material according to the first embodiment and well disperse the solid electrolyte material according to the first embodiment and an active material, the median diameter may be 0.5 μm or more and 10 μm or less. The median diameter means the particle diameter at which the accumulated volume in a volume-based particle size distribution is equal to 50%. The volume-based particle size distribution can be measured with a laser diffraction measurement apparatus or an image analyzer.
In order to better disperse the solid electrolyte material according to the first embodiment and the active material, the solid electrolyte material according to the first embodiment may have a median diameter smaller than that of the active material.
The solid electrolyte material according to the first embodiment can be manufactured by the following method.
First, a plurality of halides as raw material powders are mixed.
As an example, when a solid electrolyte material consisting of Li, Y, Cl, and O is produced, a YCl3 raw material powder and a LiCl raw material powder are mixed. The resulting powder mixture is heat-treated in an inert gas atmosphere with an adjusted oxygen concentration and an adjusted moisture concentration (for example, an argon atmosphere having a dew point of −60° C. or less). The heat treatment temperature may be, for example, within a range of 200° C. or more and 650° C. or less. The resulting reaction product is left to stand in an atmosphere having a relatively high dew point (for example, an argon atmosphere having a dew point of −30° C.).
Subsequently, the reaction product is heat-treated at a temperature of the melting point or more (for example, 550° C.) in, for example, an inert gas atmosphere with an adjusted oxygen concentration and an adjusted moisture concentration (for example, an argon atmosphere having a dew point of −60° C. or less). O can be present in the whole material by the heat treatment at a temperature of the melting point or more. Alternatively, as another example, the reaction product may be heat-treated at a temperature of the melting point or less (for example, 400° C.) in an inert gas atmosphere with an adjusted oxygen concentration and an adjusted moisture concentration (for example, an argon atmosphere having a dew point of −60° C. or less). The ratio of O in the surface region of the solid electrolyte material is increased by the heat treatment at a temperature lower than the melting point.
The raw material powders may be mixed at a molar ratio adjusted in advance so as to offset a composition change that may occur in the synthesis process. The oxygen amount in a solid electrolyte material is determined by selecting the raw material powders, the oxygen concentration in the atmosphere, the moisture concentration in the atmosphere, and the reaction time. Thus, the solid electrolyte material according to the first embodiment is obtained.
The raw material powders may be an oxide and a halide. For example, as the raw material powders, Y2O3, NH4Cl, and LiCl may be used.
It is inferred that the oxygen constituting the solid electrolyte material according to the first embodiment is incorporated from the above-mentioned atmosphere having a relatively high dew point.
Hereinafter, a second embodiment will be described. The matters described in the first embodiment may be omitted.
The battery according to the second embodiment includes a positive electrode, a negative electrode, and an electrolyte layer. The electrolyte layer is disposed between the positive electrode and the negative electrode. At least one selected from the group consisting of the positive electrode, the electrolyte layer, and the negative electrode contains the solid electrolyte material according to the first embodiment. The battery according to the second embodiment contains the solid electrolyte material according to the first embodiment and therefore has excellent charge and discharge characteristics.
A solid electrolyte material having a low melting point is soft compared to a solid electrolyte material having a higher melting point. Accordingly, the adhesion of the interface between a solid electrolyte material and another solid electrolyte material or the interface between a solid electrolyte material and another material (for example, an active material) is improved. As a result, since the battery resistance decreases, the charge and discharge characteristics of the battery are improved. Furthermore, even if the solid electrolyte material is heat-treated with another material (for example, an active material), the occurrence of side reaction can be prevented.
The battery 1000 includes a positive electrode 201, an electrolyte layer 202, and a negative electrode 203.
The positive electrode 201 contains a positive electrode active material particle 204 and a solid electrolyte particle 100.
The electrolyte layer 202 is disposed between the positive electrode 201 and the negative electrode 203.
The electrolyte layer 202 contains an electrolyte material (for example, a solid electrolyte material).
The negative electrode 203 contains a negative electrode active material particle 205 and a solid electrolyte particle 100.
The solid electrolyte particle 100 is a particle consisting of the solid electrolyte material according to the first embodiment or a particle containing the solid electrolyte material according to the first embodiment as a main component. Here, the particle containing the solid electrolyte material according to the first embodiment as a main component means a particle in which the most abundant component is the solid electrolyte material according to the first embodiment.
The positive electrode 201 contains a material that can occlude and release metal ions (for example, lithium ions). The material is, for example, a positive electrode active material (for example, the positive electrode active material particle 204).
Examples of the positive electrode active material are a lithium-containing transition metal oxide, a transition metal fluoride, a polyanionic material, a fluorinated polyanionic material, a transition metal sulfide, a transition metal oxyfluoride, a transition metal oxysulfide, and a transition metal oxynitride. Examples of the lithium-containing transition metal oxide are LiNi1-d-fCodAlfO2 (here, 0<d, 0<f, and 0<(d+<1) and LiCoO2.
In order to well disperse the positive electrode active material particle 204 and the solid electrolyte particle 100 in the positive electrode 201, the positive electrode active material particle 204 may have a median diameter of 0.1 μm or more. This good dispersion improves the charge and discharge characteristics of the battery 1000. In order to rapidly diffuse lithium in the positive electrode active material particle 204, the positive electrode active material particle 204 may have a median diameter of 100 μm or less. The battery 1000 can be operated at a high output due to the rapid diffusion of lithium. As described above, the positive electrode active material particle 204 may have a median diameter of 0.1 μm or more and 100 μm or less.
The positive electrode active material particle 204 may have a median diameter larger than that of the solid electrolyte particle 100 in order to well disperse the positive electrode active material particle 204 and the solid electrolyte particle 100 in the positive electrode 201.
In order to increase the energy density and output of the battery 1000, in the positive electrode 201, the ratio of the volume of the positive electrode active material particle 204 to the sum of the volume of the positive electrode active material particle 204 and the volume of the solid electrolyte particle 100 may be 0.30 or more and 0.95 or less.
In order to increase the energy density and output of the battery 1000, the positive electrode 201 may have a thickness of 10 μm or more and 500 μm or less.
The electrolyte layer 202 contains an electrolyte material. The electrolyte material may include the solid electrolyte material according to the first embodiment. The electrolyte layer 202 may be a solid electrolyte layer.
The electrolyte layer 202 may be constituted of the solid electrolyte material according to the first embodiment only. Alternatively, the electrolyte layer 202 may be constituted of only a solid electrolyte material that is different from the solid electrolyte material according to the first embodiment.
Examples of the solid electrolyte material that is different from the solid electrolyte material according to the first embodiment are Li2MgX′4, Li2FeX′4, Li(Al,Ga,In)X′4, Li3(Al,Ga,In)X′6, and LiI. Here, X′ is at least one selected from the group consisting of F, Cl, Br, and I.
The electrolyte layer 202 may contain not only the solid electrolyte material according to the first embodiment but also a solid electrolyte material that is different from the solid electrolyte material according to the first embodiment. The solid electrolyte material according to the first embodiment and the solid electrolyte material different from the solid electrolyte material according to the first embodiment may be uniformly dispersed. A layer made of the solid electrolyte material according to the first embodiment and a layer made of the solid electrolyte material different from the solid electrolyte material according to the first embodiment may be stacked along the stacking direction of the battery 1000.
In order to prevent short circuit between the positive electrode 201 and the negative electrode 203 and to increase the output of the battery 1000, the electrolyte layer 202 may have a thickness of 1 μm or more and 100 μm or less.
The negative electrode 203 contains a material that can occlude and release metal ions (for example, lithium ions). The material is, for example, a negative electrode active material (for example, the negative electrode active material particle 205).
Examples of the negative electrode active material are a metal material, a carbon material, an oxide, a nitride, a tin compound, and a silicon compound. The metal material may be a single metal or an alloy. Examples of the metal material are a lithium metal and a lithium alloy. Examples of the carbon material are natural graphite, coke, graphitizing carbon, carbon fibers, spherical carbon, artificial graphite, and amorphous carbon. From the viewpoint of capacity density, suitable examples of the negative electrode active material are silicon (i.e., Si), tin (i.e., Sn), a silicon compound, and a tin compound.
In order to well disperse the negative electrode active material particle 205 and the solid electrolyte particle 100 in the negative electrode 203, the negative electrode active material particle 205 may have a median diameter of 0.1 μm or more. The good dispersion improves the charge and discharge characteristics of the battery. In order to rapidly disperse lithium in the negative electrode active material particle 205, the negative electrode active material particle 205 may have a median diameter of 100 μm or less. The battery can be operated at a high output due to the rapid diffusion of lithium. As described above, the negative electrode active material particle 205 may have a median diameter of 0.1 μm or more and 100 μm or less.
In order to well disperse the negative electrode active material particle 205 and the solid electrolyte particle 100 in the negative electrode 203, the negative electrode active material particle 205 may have a median diameter larger than that of the solid electrolyte particle 100.
In order to increase the energy density and output of the battery 1000, in the negative electrode 203, the ratio of the volume of the negative electrode active material particle 205 to the sum of the volume of the negative electrode active material particle 205 and the volume of the solid electrolyte particle 100 may be 0.30 or more and 0.95 or less.
In order to increase the energy density and output of the battery 1000, the negative electrode 203 may have a thickness of 10 μm or more and 500 μm or less.
In order to enhance the ion conductivity, chemical stability, and electrochemical stability, at least one selected from the group consisting of the positive electrode 201, the electrolyte layer 202, and the negative electrode 203 may contain the solid electrolyte material different from the solid electrolyte material according to the first embodiment.
Examples of the solid electrolyte material are a halide solid electrolyte, a sulfide solid electrolyte, an oxide solid electrolyte, and an organic polymer solid electrolyte.
Examples of the halide solid electrolyte are Li2MgX′4, Li2FeX′4, Li(Al,Ga,In)X′4, Li3(Al,Ga,In)X′6, and LiI. Here, X′ is at least one selected from the group consisting of F, Cl, Br, and I.
Examples of the sulfide solid electrolyte are Li2S—P2S5, Li2S—SiS2, Li2S—B2S3, Li2S—GeS2, Li3.25Ge0.25O0.75S4, and Li10GeP2S12.
Examples of the oxide solid electrolyte are:
(i) an NASICON-type solid electrolyte, such as LiTi2(PO4)3 and its element substitute;
(ii) a perovskite-type solid electrolyte, such as (LaLi)TiO3;
(iii) an LISICON-type solid electrolyte, such as Li14ZnGe4O16, Li4SiO4, LiGeO4, and its element substitute;
(iv) a garnet-type solid electrolyte, such as Li7La3Zr2O12 and its element substitute; and
(v) Li3PO4 and its N-substitute.
Examples of the organic polymer solid electrolyte are a polymer compound and a compound of a lithium salt. The polymer compound may have an ethylene oxide structure. A polymer compound having an ethylene oxide structure can contain a large amount of a lithium salt and can therefore further enhance the ion conductivity.
Examples of the lithium salt are LiPF6, LiBF4, LiSbF6, LiAsF6, LiSO3CF3, LiN(SO2CF3)2, LiN(SO2C2F5)2, LiN(SO2CF3)(SO2C4F9), and LiC(SO2CF3)3. One lithium salt selected from these salts may be used alone. Alternatively, a mixture of two or more lithium salts selected from these salts may be used.
At least one selected from the group consisting of the positive electrode 201, the electrolyte layer 202, and the negative electrode 203 may contain a nonaqueous electrolyte liquid, a gel electrolyte, or an ionic liquid for the purpose of facilitating the transfer of lithium ions and improving the output characteristics of the battery 1000.
The nonaqueous electrolyte liquid contains a nonaqueous solvent and a lithium salt dissolved in the nonaqueous solvent.
Examples of the nonaqueous solvent are a cyclic carbonate solvent, a chain carbonate solvent, a cyclic ether solvent, a chain ether solvent, a cyclic ester solvent, a chain ester solvent, and a fluorine solvent. Examples of the cyclic carbonate solvent are ethylene carbonate, propylene carbonate, and butylene carbonate. Examples of the chain carbonate solvent are dimethyl carbonate, ethyl methyl carbonate, and diethyl carbonate. Examples of the cyclic ether solvent are tetrahydrofuran, 1,4-dioxane, and 1,3-dioxolane. Examples of the chain ether solvent are 1,2-dimethoxyethane and 1,2-diethoxyethane. An example of the cyclic ester solvent is γ-butyrolactone. An example of the chain ester solvent is methyl acetate. Examples of the fluorine solvent are fluoroethylene carbonate, methyl fluoropropionate, fluorobenzene, fluoroethyl methyl carbonate, and fluorodimethylene carbonate.
One nonaqueous solvent selected from these solvents may be used alone. Alternatively, a mixture of two or more nonaqueous solvents selected from these solvents may be used.
Examples of the lithium salt are LiPF6, LiBF4, LiSbF6, LiAsF6, LiSO3CF3, LiN(SO2CF3)2, LiN(SO2C2F5)2, LiN(SO2CF3)(SO2C4F9), and LiC(SO2CF3)3. One lithium salt selected from these salts may be used alone. Alternatively, a mixture of two or more lithium salts selected from these salts may be used.
The concentration of the lithium salt is, for example, within a range of 0.5 mol/L or more and 2 mol/L or less.
As the gel electrolyte, a polymer material impregnated with a nonaqueous electrolyte liquid may be used. Examples of the polymer material are polyethylene oxide, polyacrylonitrile, polyvinylidene fluoride, polymethyl methacrylate, and a polymer having an ethylene oxide bond.
Examples of the cation included in the ionic liquid are:
(i) an aliphatic chain quaternary salt, such as tetraalkylammonium and tetraalkylphosphonium;
(ii) aliphatic cyclic ammonium, such as pyrrolidiniums, morpholiniums, imidazoliniums, tetrahydropyrimidiniums, piperaziniums, and piperidiniums; and
(iii) a nitrogen-containing heterocyclic aromatic cation, such as pyridiniums and imidazoliums.
Examples of the anion included in the ionic liquid are PF6−, BF4−, SbF6−, AsF6−, SO3CF3−, N(SO2CF3)2−, N(SO2C2F5)2−, N(SO2CF3)(SO2C4F9)−, and C(SO2CF3)3−.
The ionic liquid may contain a lithium salt.
At least one selected from the group consisting of the positive electrode 201, the electrolyte layer 202, and the negative electrode 203 may contain a binder for the purpose of improving the adhesion between individual particles.
Examples of the binder are polyvinylidene fluoride, polytetrafluoroethylene, polyethylene, polypropylene, an aramid resin, polyamide, polyimide, polyamideimide, polyacrylonitrile, polyacrylic acid, polyacrylic acid methyl ester, polyacrylic acid ethyl ester, polyacrylic acid hexyl ester, polymethacrylic acid, polymethacrylic acid methyl ester, polymethacrylic acid ethyl ester, polymethacrylic acid hexyl ester, polyvinyl acetate, polyvinylpyrrolidone, polyether, polyether sulfone, hexafluoropolypropylene, styrene butadiene rubber, and carboxymethyl cellulose.
A copolymer may also be used as the binder. Examples of such the binder are copolymers of two or more materials selected from the group consisting of tetrafluoroethylene, hexafluoroethylene, hexafluoropropylene, perfluoroalkyl vinyl ether, vinylidene fluoride, chlorotrifluoroethylene, ethylene, propylene, pentafluoropropylene, fluoromethyl vinyl ether, acrylic acid, and hexadiene. A mixture of two or more selected from these materials may be used as the binder.
At least one selected from the positive electrode 201 and the negative electrode 203 may contain a conductive assistant for the purpose of enhancing the electron conductivity.
Examples of the conductive assistant are:
(i) graphites, such as natural graphite and artificial graphite;
(ii) carbon blacks, such as acetylene black and Ketjen black;
(iii) conductive fibers, such as carbon fibers and metal fibers;
(iv) carbon fluoride;
(v) metal powders, such as aluminum;
(vi) conductive whiskers, such as zinc oxide and potassium titanate;
(vii) a conductive metal oxide, such as titanium oxide; and
(viii) a conductive polymer compound, such as polyanion, polypyrrole, and polythiophene.
In order to reduce the cost, the conductive assistant of the above (i) or (ii) may be used.
Examples of the shape of the battery according to the second embodiment are coin type, cylindrical type, square type, sheet type, button type, flat type, and stack type.
The battery according to the second embodiment may be manufactured by, for example, preparing a material for forming a positive electrode, a material for forming an electrolyte layer, and a material for forming a negative electrode, and producing a stack of a positive electrode, an electrolyte layer, and a negative electrode arranged in this order by a known method.
The present disclosure will now be described in more detail with reference to Examples.
YCl3 and LiCl were prepared as raw material powders such that the YCl3:LiCl molar ratio was 1:3 in an argon atmosphere having a dew point of −60° C. or less and an oxygen concentration of 0.0001 vol % or less (hereinafter, referred to as “dry argon atmosphere”). These raw material powders were pulverized and mixed in a mortar. The resulting mixture was heat-treated at 550° C. for 1 hour in an alumina crucible and was then pulverized in a mortar. The resulting reaction product was left to stand in an argon atmosphere having a dew point of −30° C. and an oxygen concentration of 20.9 vol % for about 10 minutes. The reaction product was further heat-treated in a dry argon atmosphere at 550° C. for 1 hour and then pulverized in a mortar. Thus, a solid electrolyte material of Example 1 was obtained.
The contents of Li and Y per unit weight of the solid electrolyte material of Example 1 were measured with a high-frequency inductively coupled plasma emission spectrometer (iCAP7400, manufactured by Thermo Fisher Scientific, Inc.) by high-frequency inductively coupled plasma emission spectrometry. The content of Cl in the solid electrolyte material of Example 1 was measured with an ion chromatography apparatus (ICS-2000, manufactured by Dionex) by an ion chromatography method. The Li:Y:Cl molar ratio was calculated based on the contents of Li, Y, and Cl obtained from these measurement results. As a result, the solid electrolyte material of Example 1 had a Li:Y:Cl molar ratio of 2.56:1.00:5.29.
The mass proportion of O relative to the whole solid electrolyte material of Example 1 was measured with an oxygen nitrogen hydrogen analyzer (EMGA-930, manufactured by HORIBA, Ltd.) by a nondispersive infrared absorption method. As a result, the mass proportion of O was 0.22%. Based on this, the Y:O molar ratio was calculated. As a result, the solid electrolyte material of Example 1 had a Y:O molar ratio of 1.00:0.04.
In the composition analysis, elements of which the molar proportions relative to Y are 0.001% or less are recognized as impurities.
The melting point was measured using a thermal analyzer (Q1000, manufactured by TA Instruments). The solid electrolyte material (about 5 mg) of Example 1 was weighed in a nitrogen atmosphere and was heated from 300° C. to 530° C. at a temperature increase rate of 10 K/min. The endothermic peak at that time was observed. Based on the obtained data, a two-dimensional graph was created with the horizontal axis as temperature and the vertical axis as calorific value. The two points on the graph where the solid electrolyte material did not generate heat or absorb heat were connected by a straight line, and the line was used as the baseline. The intersection of the tangent at the inflection point of the endothermal peak and the baseline was defined as the melting point. As a result, the melting point of the solid electrolyte material of Example 1 was 500.6° C. The result of thermal analysis of the solid electrolyte material of Example 1 is shown in the graph of
The crystal structure of the solid electrolyte material was analyzed with an X-ray diffractometer (MiniFlex 600, RIGAKU Corporation). The X-ray diffraction pattern of the solid electrolyte material of Example 1 was measured in a dry atmosphere having a dew point of −45° C. or less. As the X-ray source, Cu-Kα rays (wavelength: 1.5405 angstrom and 1.5444 angstrom) were used.
As the results of the X-ray diffraction measurement, there were peaks at 15.83°, 18.03°, 31.37°, 33.72°, 40.85°, 48.74°, and 53.58°. The X-ray diffraction pattern of the solid electrolyte material of Example 1 is shown in the graph of
The compression molding dies 300 included a punch upper part 301, a die 302, and a punch lower part 303. The die 302 was formed from insulating polycarbonate. The punch upper part 301 and the punch lower part 303 were both formed from electron-conductive stainless steel.
The ion conductivity of the solid electrolyte material of Example 1 was measured using the compression molding dies 300 shown in
A powder 101 of the solid electrolyte material of Example 1 was loaded in the compression molding dies 300 in a dry argon atmosphere. A pressure of 400 MPa was applied to the solid electrolyte material of Example 1 inside the compression molding dies 300 using the punch upper part 301 and the punch lower part 303.
While applying the pressure, the punch upper part 301 and the punch lower part 303 were connected to a potentiostat (VersaSTAT4, Princeton Applied Research). The punch upper part 301 was connected to the working electrode and the potential measurement terminal. The punch lower part 303 was connected to the counter electrode and the reference electrode. The impedance of the solid electrolyte material of Example 1 was measured by an electrochemical impedance measurement method at room temperature.
In
σ=(RSE×S/t)−1 (1).
Here, a represents ion conductivity; S represents the contact area of a solid electrolyte material with the punch upper part 301 (equal to the cross-sectional area of the hollow part of the die 302 in
The ion conductivity of the solid electrolyte material of Example 1 measured at 25° C. was 2.4×10−4 S/cm.
The solid electrolyte material of Example 1 and LiCoO2 as an active material were prepared at a volume ratio of 70:30 in a dry argon atmosphere. These materials were mixed in an agate mortar. Thus, a mixture was obtained.
The solid electrolyte material (100 mg) of Example 1, the above mixture (10.0 mg), and an aluminum powder (14.7 mg) were stacked in this order in an insulating tube having an inner diameter of 9.5 mm. A pressure of 300 MPa was applied to this stack to form a first electrode and a solid electrolyte layer. The solid electrolyte layer had a thickness of 500 μm.
Subsequently, metal In foil was stacked on the solid electrolyte layer. The solid electrolyte layer was sandwiched between the metal In foil and the first electrode. The metal In foil had a thickness of 200 μm. Subsequently, a pressure of 80 MPa was applied to the metal In foil to form a second electrode.
A current collector made of stainless steel was attached to the first electrode and the second electrode, and current collecting lead was then attached to the current collector. Finally, the inside of the insulating tube was isolated from the outside atmosphere using an insulating ferrule to seal the inside of the tube. Thus, a battery of Example 1 was obtained.
The battery of Example 1 was placed in a thermostat of 25° C. The battery of Example 1 was charged with a current density of 86 μA/cm2 until the voltage reached 3.7 V. The current density corresponded to 0.05 C rate. Subsequently, the battery of Example 1 was discharged similarly at a current density of 86 μA/cm2 until the voltage reached 1.9 V.
As the results of the charge and discharge test, the battery of Example 1 had an initial discharge capacity of 536 μAh.
A solid electrolyte material of Example 2 was obtained as in Example 1 except that the time during which the reaction product was left to stand in an atmosphere having a dew point of −30° C. was set to 30 minutes instead of about 10 minutes.
A solid electrolyte material of Example 3 was obtained as in Example 1 except that the time during which the reaction product was left to stand in an atmosphere having a dew point of −30° C. was set to 9 hours instead of about 10 minutes.
The element ratio (molar ratio), melting point, oxygen amount, X-ray diffraction, and ion conductivity of each of the solid electrolyte materials of Examples 2 and 3 were measured as in Example 1. The measurement results are shown in Tables 1 and 2. The X-ray diffraction patterns of the solid electrolyte materials of Examples 2 and 3 are shown in the graph of
Batteries of Examples 2 and 3 were obtained as in Example 1 using the solid electrolyte materials of Examples 2 and 3.
The charge and discharge test was implemented as in Example 1 using the batteries of Examples 2 and 3. The batteries of Examples 2 and 3 were well charged and discharged as in the battery of Example 1.
In a dry argon atmosphere, YCl3 and LiCl were prepared as raw material powders such that the YCl3:LiCl molar ratio was 1:3. These raw material powders were pulverized and mixed in a mortar. The resulting mixture was heat-treated at 550° C. for 1 hour in an alumina crucible and was then pulverized in a mortar. Thus, a solid electrolyte material of Comparative Example 1 was obtained.
The element ratio (molar ratio), melting point, oxygen amount, X-ray diffraction, and ion conductivity of the solid electrolyte material of Comparative Example 1 were measured as in Example 1. The measurement results are shown in Tables 1 and 2. The X-ray diffraction pattern of the solid electrolyte material of Comparative Example 1 is shown in the graph of
As obvious from Table 1, the solid electrolyte materials of Examples 1 to 3 have melting points lower than that of the solid electrolyte material of Comparative Example 1. Furthermore, the solid electrolyte materials of Examples 1 to 3 each have a high ion conductivity of 1×10−5 S/cm or more at around room temperature.
The batteries according to Examples 1 to 3 were charged and discharged at 25° C.
Since the solid electrolyte materials of Examples 1 to 3 do not contain sulfur, hydrogen sulfide does not occur.
In a dry argon atmosphere, YCl3 and LiCl were prepared as raw material powders such that the YCl3:LiCl molar ratio was 1:3. These raw material powders were pulverized and mixed in a mortar. The resulting mixture was heat-treated at 550° C. for 1 hour in an alumina crucible and was then pulverized in a mortar. The resulting reaction product was left to stand in an argon atmosphere having a dew point of −30° C. and an oxygen concentration of 20.9 vol % for about 10 minutes. The reaction product was further heat-treated in a dry argon atmosphere at 400° C. for 1 hour and then pulverized in a mortar. Thus, a solid electrolyte material of Example 4 was obtained.
The contents of Li, Y, and Cl in the whole solid electrolyte material of Example 4 were measured as in Example 1, and the Li:Y:Cl molar ratio was calculated. As a result, the solid electrolyte material of Example 4 had a Li:Y:Cl molar ratio of 2.56:1.00:5.16.
The mass proportion of O relative to the whole solid electrolyte material of Example 4 was measured as in Example 1. As a result, the mass proportion of O was 0.29%. Based on this, the Y:O molar ratio was calculated. As a result, the solid electrolyte material of Example 4 had a Y:O molar ratio of 1.00:0.06.
The molar ratio of O to Y in the surface region of the solid electrolyte material of Example 4 was measured with a scanning X-ray photoelectron spectrometer (PHI Quantera SXM, manufactured by Ulvac-Phi, Inc.) by an X-ray photoelectron spectroscopy. As the X-ray source, Al-Kα rays were used. As a result, the solid electrolyte material of Example 4 had a Y:O molar ratio of 1.00:0.15 in the surface region. The surface region in the present disclosure means the thus-measured region. The thickness of the surface region of the solid electrolyte material of Example 4 was about 5 nm from the surface of the solid electrolyte material in the inward direction.
In the composition analysis, elements of which the molar proportions relative to Y are 0.001% or less are recognized as impurities.
The melting point of the solid electrolyte material of Example 4 was measured as in Example 1. As a result, the melting point of the solid electrolyte material of Example 4 was 498.8° C. The result of the thermal analysis of the solid electrolyte material of Example 4 is shown in the graph of
The X-ray diffraction pattern of the solid electrolyte material of Example 4 was measured as in Example 1.
As the results of the X-ray diffraction measurement, there were peaks at 15.79°, 17.99°, 31.33°, 33.67°, 40.84°, 48.74°, and 53.56°. The X-ray diffraction pattern of the solid electrolyte material of Example 4 is shown in the graph of
A battery of Example 4 was obtained as in Example 1 using the solid electrolyte material of Example 4.
The battery of Example 4 was placed in a thermostat of 25° C. The battery of Example 4 was charged with a current density of 83 μA/cm2 until the voltage reached 3.7 V. The current density corresponded to 0.05 C rate. Subsequently, the battery of Example 4 was discharged similarly at a current density of 83 μA/cm2 until the voltage reached 1.9 V.
As the results of the charge and discharge test, the battery of Example 4 had an initial discharge capacity of 642 μAh.
A solid electrolyte material of Example 5 was obtained as in Example 4 except that the time during which the reaction product was left to stand in an atmosphere having a dew point of −30° C. was set to 30 minutes instead of about 10 minutes.
A solid electrolyte material of Example 6 was obtained as in Example 4 except that the time during which the reaction product was left to stand in an atmosphere having a dew point of −30° C. was set to 2 hours instead of about 10 minutes.
The element ratio (molar ratio), melting point, oxygen amount, X-ray diffraction, and ion conductivity of each of the solid electrolyte materials of Examples 5 and 6 were measured as in Example 4. The measurement results are shown in Tables 3 and 4. The X-ray diffraction patterns of the solid electrolyte materials of Examples 5 and 6 are shown in the graph of
Batteries of Examples 5 and 6 were obtained as in Example 1 using the solid electrolyte materials of Examples 5 and 6.
The charge and discharge test was implemented as in Example 4 using the batteries of Examples 5 and 6. The batteries of Examples 5 and 6 were well charged and discharged as in the battery of Example 4.
A solid electrolyte material of Comparative Example 2 was obtained as in Example 4 except that the time during which the reaction product was left to stand in an atmosphere having a dew point of −30° C. was set to 9 hours instead of about 10 minutes.
The element ratio (molar ratio), melting point, oxygen amount, X-ray diffraction, and ion conductivity of each of the solid electrolyte materials of Comparative Examples 1 and 2 were measured as in Example 4. The measurement results are shown in Tables 3 and 4. The X-ray diffraction patterns of the solid electrolyte materials of Comparative Examples 1 and 2 are shown in the graph of
A battery of Comparative Example 2 was obtained as in Example 4 using the solid electrolyte material of Comparative Example 2.
The charge and discharge test was implemented as in Example 4 using the battery of Comparative Example 2, but the initial discharge capacity was 1 mAh or less, and the battery of Comparative Example 2 was neither charged nor discharged.
As obvious from Table 3, the solid electrolyte materials of Examples 4 to 6 have melting points lower than that of the solid electrolyte material of Comparative Example 1. Furthermore, the solid electrolyte materials of Examples 4 to 6 each have a high ion conductivity of 1×10−5 S/cm or more at around room temperature. In contrast, the solid electrolyte material of Comparative Example 2 has an ion conductivity lower than 1×10−5 S/cm.
As obvious from Table 3, when the molar ratio of O to Y in the whole solid electrolyte material is greater than 0.01 and 0.33 and or less, the solid electrolyte material has a low melting point and a high ion conductivity.
The batteries of Examples 4 to 6 were charged and discharged at 25° C.
Since the solid electrolyte materials of Examples 4 to 6 do not contain sulfur, hydrogen sulfide does not occur.
As described above, the solid electrolyte material of the present disclosure has a low melting point and a high lithium ion conductivity and is suitable for providing a battery that can be well charged and discharged.
The solid electrolyte material of the present disclosure is used in, for example, an all solid lithium ion secondary battery.
| Number | Date | Country | Kind |
|---|---|---|---|
| 2020-012969 | Jan 2020 | JP | national |
| 2020-012973 | Jan 2020 | JP | national |
| Number | Date | Country | |
|---|---|---|---|
| Parent | PCT/JP2020/043705 | Nov 2020 | US |
| Child | 17810840 | US |
