Method for producing sulfide solid electrolyte, sulfide solid electrolyte, all solid state battery, and method for selecting raw material compound used for producing sulfide solid electrolyte

Abstract

To provide a method for producing a sulfide solid electrolyte capable of suppressing discharge of N to the outside of a system in a production process of the sulfide solid electrolyte, a method for selecting a raw material compound used for producing the sulfide solid electrolyte, an all-solid-state battery including the sulfide solid electrolyte, a sulfide solid electrolyte having improved thermal stability, a method for producing the sulfide solid electrolyte, and an all-solid-state battery including the sulfide solid electrolyte.SOLUTION: The sulfide solid electrolyte contains P, S, N, an element A, an element X, and an element M as constituent elements and has a crystal structure. Here, A represents at least one element selected from the group consisting of Li, Na, and K. X represents at least one element selected from the group consisting of Cl, Br, and I. M represents at least one element selected from the group consisting of Al, Ta, Si, Sc, Mg, Nb, B, Hf, C, P, Zr, and Ti. In the all-solid-state battery 10, a positive electrode substrate layer 7, a positive electrode mixture layer 6, a solid electrolyte layer 3, a negative electrode mixture layer 5, and a negative electrode substrate layer 4 are laminated in this order.SELECTED DRAWING: Figure 2

Description

[Technical Field]

[0001] The present invention relates to a method for producing a sulfide solid electrolyte, a sulfide solid electrolyte, an all-solid-state battery, and a method for selecting raw material compounds used in producing a sulfide solid electrolyte.

[0002] Due to their high energy density, non-aqueous electrolyte secondary batteries, typified by lithium ion non-aqueous electrolyte secondary batteries, are widely used in electronic devices such as personal computers and communication terminals, automobiles, etc. The non-aqueous electrolyte secondary batteries generally include an electrode assembly having a pair of electrically isolated electrodes and a non-aqueous electrolyte interposed between the electrodes, and are configured to charge and discharge by transferring ions between the electrodes.

[0003] In recent years, sulfide solid electrolytes have been attracting attention as non-aqueous electrolytes for non-aqueous electrolyte secondary batteries, and various studies have been conducted on them.

[0004] Patent Document 1 describes the production of a sulfide solid electrolyte having a composition of 75Li2S-25P2S5-yLi3N using Li2S, P2S5, and Li3N as starting materials. Patent Document 2 describes the production of a sulfide solid electrolyte using a raw material composition consisting of Li2S, P2S5, LiBr, LiI, and Li3N. [Prior art documents] [Patent documents]

[0005] [Patent Document 1] Patent Publication No. 2018-041671 [Patent Document 2] Patent Publication No. 2015-011898 [Patent Document 3] Patent Publication No. 2018-156735 Summary of the Invention [Problem to be solved by the invention]

[0006] Patent Document 1 describes that the atmospheric stability (water resistance) of a sulfide solid electrolyte can be improved by including N in the sulfide solid electrolyte. However, when LiN is used as a raw material for the sulfide solid electrolyte, there is a problem in that N is discharged outside the system.

[0007] Patent Document 2 describes that a high Li-ion conductive phase is precipitated by amorphizing a raw material composition containing Li2S, P2S5, LiI, and LiBr and then heat-treating it. However, if the heat-treatment temperature is too high, a low Li-ion conductive phase is precipitated. Patent Document 3 describes that the addition of Li3N can increase the difference in temperature between the formation of a high Li-ion conductive phase and the formation of a low Li-ion conductive phase. However, this difference is small, at most about 30°C, and further improvement is needed.

[0008] The present invention has been made in light of the above-mentioned circumstances, and an object of one aspect of the present invention is to provide a method for producing a sulfide solid electrolyte that can suppress the emission of N to the outside of the system during the production process of the sulfide solid electrolyte, a method for selecting raw material compounds used in the production of the sulfide solid electrolyte, and an all-solid-state battery including the sulfide solid electrolyte. Another object of the present invention is to provide a sulfide solid electrolyte having improved thermal stability, a method for producing the same, and an all-solid-state battery including the sulfide solid electrolyte. [Means for solving the problem]

[0009] One aspect of the present invention, which has been made to solve the above-mentioned problems, is a method for producing a sulfide solid electrolyte, comprising: preparing a composition containing P, S, N, element A, and element M; reacting the composition to obtain an intermediate; and heating the intermediate to obtain a sulfide solid electrolyte, wherein the composition comprises a raw material compound containing N, element A, and element M. A represents at least one element selected from the group consisting of Li, Na, and K. M represents at least one element selected from the group consisting of Al, Ta, Si, Sc, Mg, Nb, B, Hf, C, P, Zr, and Ti.

[0010] Another aspect of the present invention is a method for selecting raw material compounds used in the production of a sulfide solid electrolyte, comprising: As a candidate for the raw material compound, a candidate material containing N, element A', and element M' is selected, and the defect formation energy E of N in the candidate material is calculated using first-principles calculations. Ndefect and calculating E Ndefect is 4.00 eV or more, the candidate material is selected as the raw material compound.

[0011] Another aspect of the present invention is a sulfide solid electrolyte having a crystalline structure and containing, as constituent elements, P, S, N, element A, element X, and element M. Here, A represents at least one element selected from the group consisting of Li, Na, and K. X represents at least one element selected from the group consisting of Cl, Br, and I. M represents at least one element selected from the group consisting of Al, Ta, Si, Sc, Mg, Nb, B, Hf, C, P, Zr, and Ti. [Effects of the Invention]

[0012] According to the method for producing a sulfide solid electrolyte, the method for selecting raw material compounds used in the production of a sulfide solid electrolyte, and the sulfide solid electrolyte of one embodiment of the present invention, it is possible to suppress the emission of N to the outside of the system during the production process of a sulfide solid electrolyte. According to another aspect of the sulfide solid electrolyte of the present invention, it is possible to obtain a sulfide solid electrolyte having improved thermal stability. [Brief explanation of the drawings]

[0013] [Figure 1] FIG. 1 is a flowchart showing a process for producing a sulfide solid electrolyte according to one embodiment of the present invention. [Figure 2] FIG. 2 is a schematic cross-sectional view showing an all-solid-state battery according to one embodiment of the present invention. [Figure 3] FIG. 3 shows an XRD diffraction pattern of the sulfide solid electrolyte of the example. [Figure 4] FIG. 4 shows an XRD diffraction pattern of the sulfide solid electrolyte of the comparative example. [Figure 5] FIG. 5 shows DSC curves of intermediate sulfide solid electrolytes of Examples and Comparative Examples after milling treatment and before heat treatment. [Figure 6] FIG. 6 shows DSC curves of intermediate sulfide solid electrolytes of Examples and Comparative Examples after milling treatment and before heat treatment. DETAILED DESCRIPTION OF THE INVENTION

[0014] First, an outline of the method for producing the sulfide solid electrolyte disclosed in this specification will be described.

[0015] A method for producing a sulfide solid electrolyte according to one embodiment of the present invention includes the steps of preparing a composition containing P, S, N, element A, and element M, reacting the composition to obtain an intermediate, and heating the intermediate to obtain a sulfide solid electrolyte, wherein the composition includes a raw material compound containing N, element A, and element M. Here, A represents at least one element selected from the group consisting of Li, Na, and K. M represents at least one element selected from the group consisting of Al, Ta, Si, Sc, Mg, Nb, B, Hf, C, P, Zr, and Ti.

[0016] In the present invention, the term "composition" refers to a mixture of two or more compounds, and the term "raw material compound" refers to a specific compound that constitutes the composition.

[0017] The inventors have discovered that by using a raw material compound containing at least one element A selected from the group consisting of Li, Na, and K, at least one element M selected from the group consisting of Al, Ta, Si, Sc, Mg, Nb, B, Hf, C, P, Zr, and Ti, and N, it is possible to suppress the emission of N to the outside of the system in the production process of a sulfide solid electrolyte, and have arrived at the present invention.

[0018] According to this method for producing a sulfide solid electrolyte, it is possible to suppress the emission of N to the outside of the system during the production process of the sulfide solid electrolyte. This makes it easier to control the content of N in the sulfide solid electrolyte. Although the reason for this is not clear, the following reason is presumed. In the methods for producing a sulfide solid electrolyte using Li3N disclosed in Patent Documents 1 and 3, the defect formation energy of N in Li3N is small, and N2 gas is easily generated. In contrast, in the method for producing a sulfide solid electrolyte using a raw material compound containing N, element A, and element M, the defect formation energy of N is large, and N defects are unlikely to be formed during the synthesis of the sulfide solid electrolyte, so N gas is unlikely to be produced, which makes it possible to suppress the emission of N to the outside of the system during the production process of the sulfide solid electrolyte. The element M is calculated by first-principles calculations, which will be described later. α M β N is an element having a defect formation energy of 4.00 eV or more in a compound represented by N (α and β are values ​​that give a stoichiometric ratio depending on the type of element M). The defect formation energy of N will be defined later.

[0019] The raw material compound containing N, element A, and element M preferably contains Li, N, element A, and element M.

[0020] This allows for an increased mass energy density of an all-solid-state battery including a sulfide solid electrolyte produced by this production method, since Li has the smallest atomic weight and smallest ion size among alkali metal elements.

[0021] The raw material compound containing N, element A, and element M may be obtained by reacting a nitride of element M with a nitride of element A, or may be an industrially produced and commercially available compound.

[0022] The element M is preferably one element selected from the group consisting of Al, Ta, Si, Sc, Mg, Nb, B, Hf, C, and P. These elements are elements for which the N defect creation energy calculated by first-principles calculations described below is 4.10 eV or more.

[0023] This makes it possible to more reliably suppress the emission of N to the outside of the system during the production process of the sulfide solid electrolyte.

[0024] The element M is more preferably at least one element selected from the group consisting of Al, Ta, Si, Sc, Mg, Nb, and B. These elements are elements for which the N defect creation energy calculated by first-principles calculations described below is 4.35 eV or more.

[0025] This makes it possible to more reliably suppress the emission of N to the outside of the system during the production process of the sulfide solid electrolyte.

[0026] The composition preferably contains lithium sulfide, phosphorus sulfide, and raw material compounds containing N, element A, and element M. These compounds are easy to handle, and therefore can improve the productivity of the sulfide solid electrolyte.

[0027] In the composition, the element A preferably contains Li, the molar ratio of Li to P in the composition is 2.30 to 4.20, and the molar ratio of N to P in the composition is 0.0100 to 1.20. Furthermore, the element A more preferably contains Li, the molar ratio of Li to P in the composition is 2.77 to 3.38, and the molar ratio of N to P in the composition is 0.280 to 0.650. This makes it possible to provide a sulfide solid electrolyte that is excellent in atmospheric stability and has high ionic conductivity at 25°C.

[0028] The composition preferably contains an element X. X is at least one element selected from the group consisting of Cl, Br, and I.

[0029] It is known that a sulfide solid electrolyte containing Li, P, S, and an element X generates a metastable phase with high ionic conductivity (hereinafter also referred to as a high ion conduction phase (HICP)) (Patent Document 2). It is also known that when such a sulfide solid electrolyte contains N, the difference between the heat treatment temperature at which HICP precipitates and the heat treatment temperature at which the HICP undergoes a phase transition to another phase with low ionic conductivity (hereinafter also referred to as a low ion conduction phase (LICP)) widens (Patent Document 3). However, since the sulfide solid electrolyte in Patent Document 3 is produced using LiN, N is discharged outside the system during the production process of the sulfide solid electrolyte, and the effect of widening the heat treatment temperature range in which HICP is stable is not fully achieved. In contrast, the method for producing a sulfide solid electrolyte suppresses the emission of N to the outside of the system, thereby enabling the effect of improving the thermal stability of HICP to be fully exerted.

[0030] The composition preferably has a molar ratio of Li to P of 3.10 or more and 4.20 or less, a molar ratio of N to P of 0.0600 or more and 0.750 or less, and a molar ratio of X to P of 0.180 or more and 1.30 or less.

[0031] This makes it possible to provide a sulfide solid electrolyte with high thermal stability of HICP.

[0032] A sulfide solid electrolyte according to another aspect of the present invention is a sulfide solid electrolyte produced by the method for producing a sulfide solid electrolyte. Such a sulfide solid electrolyte suppresses the emission of N to the outside of the system during the production process of the sulfide solid electrolyte, and therefore can fully exhibit various effects due to the inclusion of N.

[0033] An all-solid-state battery according to another aspect of the present invention includes a sulfide solid electrolyte produced by the method for producing a sulfide solid electrolyte. In such an all-solid-state battery, N is prevented from being released from the system during the production process of the sulfide solid electrolyte, and therefore various effects attributable to the inclusion of N can be fully exhibited.

[0034] A method for selecting a raw material compound used in the production of a sulfide solid electrolyte according to another embodiment of the present invention is a method for selecting a raw material compound used in the production of a sulfide solid electrolyte, the method comprising the steps of: selecting a candidate material containing N, element A', and element M' as the raw material compound candidate; and calculating, using first-principles calculations, a defect formation energy E of N in the candidate material. Ndefect and calculating E Ndefect is 4.00 eV or more, the candidate material is selected as the raw material compound. If there are multiple N-occupied sites in the crystal structure of the candidate material, E Ndefect The lowest value is the E of the candidate material. Ndefect Used as.

[0035] The raw material compounds selected by this selection method have a large N defect formation energy, and N defects are less likely to be formed during the synthesis of the sulfide solid electrolyte, making it difficult to generate N gas. Therefore, when a sulfide solid electrolyte is produced using the above raw material compounds, it is possible to suppress the emission of N to the outside of the system during the production process of the sulfide solid electrolyte.

[0036] Above E Ndefect is 4.10 eV or more, the candidate material is preferably selected as the raw material compound.

[0037] This makes it possible to more reliably suppress the emission of N to the outside of the system during the production process of the sulfide solid electrolyte.

[0038] Above E Ndefect is 4.35 eV or more, it is more preferable to select the candidate material as the raw material compound.

[0039] This makes it possible to more reliably suppress the emission of N to the outside of the system during the production process of the sulfide solid electrolyte.

[0040] A method for producing a sulfide solid electrolyte according to another aspect of the present invention includes: preparing a composition containing raw material compounds selected by the method for selecting raw material compounds to be used in the production of the sulfide solid electrolyte; reacting the composition to obtain an intermediate; and heating the intermediate to obtain the sulfide solid electrolyte.

[0041] This makes it possible to suppress the discharge of N outside the system during the production process of the sulfide solid electrolyte, thereby facilitating the control of the N content in the sulfide solid electrolyte.

[0042] A sulfide solid electrolyte according to another aspect of the present invention is a sulfide solid electrolyte produced by the above-described production method. With such a sulfide solid electrolyte, the emission of N to the outside of the system during the production process of the sulfide solid electrolyte is suppressed, and therefore various effects due to the inclusion of N can be fully exhibited.

[0043] An all-solid-state battery according to another embodiment of the present invention includes a sulfide solid electrolyte produced using raw material compounds selected by the selection method. Such a sulfide solid electrolyte suppresses the emission of N to the outside of the system during the production process, and therefore can fully exhibit various effects due to the inclusion of N.

[0044] A sulfide solid electrolyte according to another embodiment of the present invention is a sulfide solid electrolyte having a crystalline structure and containing, as constituent elements, P, S, N, element A, element X, and element M. Here, A represents at least one element selected from the group consisting of Li, Na, and K. X represents at least one element selected from the group consisting of Cl, Br, and I. M represents at least one element selected from the group consisting of Al, Ta, Si, Sc, Mg, Nb, B, Hf, C, P, Zr, and Ti.

[0045] Such a sulfide solid electrolyte can improve the thermal stability of the HICP compared to a sulfide solid electrolyte consisting only of Li, P, S, N, and the element X.

[0046] The element M is preferably at least one element selected from the group consisting of Al, Ta, Si, Sc, Mg, Nb, and B.

[0047] This can further increase the thermal stability of the HICP.

[0048] The above crystal structure preferably has diffraction peaks at 2θ=20.2°±0.5° and 23.6°±0.5° in X-ray diffraction measurement using CuKα radiation.

[0049] When the sulfide solid electrolyte has the above crystal structure, good Li-ion conductivity can be obtained.

[0050] An all-solid-state battery according to another embodiment of the present invention is an all-solid-state battery including a sulfide solid electrolyte having a crystalline structure and containing P, S, N, element A, element X, and element M as constituent elements.

[0051] One advantage of all-solid-state batteries over non-aqueous electrolyte batteries is their extremely high upper operating temperature limit, which is achieved by the high thermal stability of solid electrolytes. However, Patent Documents 2 and 3 describe that a sulfide solid electrolyte containing Li, P, S, N, Br, and I undergoes a phase transition from a high Li-ion conductive phase to a low Li-ion conductive phase when heated to a high temperature. In other words, the operating temperature of an all-solid-state battery including such a sulfide solid electrolyte is limited by the phase transition temperature of the high Li-ion conductive phase. In contrast, the sulfide solid electrolyte of the present invention has higher thermal stability of HICP than conventional sulfide solid electrolytes that do not contain element M. Therefore, an all-solid-state battery including the sulfide solid electrolyte of the present invention can fully enjoy the advantage of all-solid-state batteries, which can increase the upper limit of the operating temperature of the battery.

[0052] A sulfide solid electrolyte according to another embodiment of the present invention is a crystalline sulfide solid electrolyte containing P, S, N, element A, and element M. Here, A represents at least one element selected from the group consisting of Li, Na, and K. M represents at least one element selected from the group consisting of Al, Ta, Si, Sc, Mg, Nb, B, Hf, C, P, Zr, and Ti.

[0053] Such a sulfide solid electrolyte can improve atmospheric stability by suppressing the emission of N to the outside of the system during the production process of the sulfide solid electrolyte.

[0054] The element M is preferably at least one element selected from the group consisting of Al, Ta, Si, Sc, Mg, Nb, and B.

[0055] This more reliably suppresses the emission of N to the outside of the system during the production process of the sulfide solid electrolyte, thereby further improving the atmospheric stability and the like.

[0056] Hereinafter, a method for producing a sulfide solid electrolyte, a sulfide solid electrolyte, an all-solid-state battery, and a method for selecting raw material compounds used in producing a sulfide solid electrolyte according to one embodiment of the present invention will be described in detail. Matters other than those specifically mentioned in this specification that are necessary for carrying out the present invention can be understood as design matters for a person skilled in the art based on prior art in the relevant field. The present invention can be carried out based on the contents disclosed in this specification and common general technical knowledge in the relevant field.

[0057] <Method of manufacturing sulfide solid electrolyte> [Embodiment] A method for producing a sulfide solid electrolyte according to one embodiment of the present invention includes a preparation step of preparing a composition containing P, S, N, element A, and element M, a reaction step of reacting the composition to obtain an intermediate, and a heating step of heating the intermediate to obtain a sulfide solid electrolyte, the composition comprising a raw material compound containing N, element A, and element M. Here, A is at least one element selected from the group consisting of Li, Na, and K. M is at least one element selected from the group consisting of Al, Ta, Si, Sc, Mg, Nb, B, Hf, C, P, Zr, and Ti. In this embodiment, a method for producing the sulfide solid electrolyte will be described using an example in which Li is contained as element A. Fig. 1 is a flowchart showing an example of the method for producing the sulfide solid electrolyte according to this embodiment, and the following description will be made in accordance with this flowchart.

[0058] (preparation process) In this step, a composition containing Li, P, S, N, and element M is prepared. The composition is preferably a mixture of one or more raw material compounds containing N, Li, and the element M (hereinafter also referred to as Li-MN-containing compounds) and one or more raw material compounds containing Li, P, and S.

[0059] In Fig. 1, first, LiN and a nitride of element M are prepared and mixed in a mortar or the like. Next, pellets of the mixed raw material compounds are produced. Next, the pellets are heat-treated to produce a Li-MN-containing compound.

[0060] The Li-MN-containing compound may be prepared by other methods. For example, the raw materials for the Li-MN-containing compound may be two or more compounds containing N, Li, or element M. The Li-MN-containing compound may be prepared by mechanical milling. An industrially manufactured and commercially available MN-containing compound may also be prepared.

[0061] As the Li-MN-containing compound, a lithium composite nitride of element M is preferably used. Examples of the lithium composite nitride of element M include Li 3 / 2 Al 1 / 2 N, Li 3 / 2 B 1 / 2 N, Li 5 / 3 Si 1 / 3 N, Li 9 / 5 Si 3 / 10 N, Li 7 / 4 P 1 / 4 N, LiMgN, LiHf 1 / 2 N, Li 3 / 2 Sc 1 / 2 N, LiZr 1 / 2 N, Li 5 / 3 Ti 1 / 3 N, Li 4 / 3 Ta 1 / 3 N, Li 7 / 4 Ta 1 / 4 N, Li 7 / 4 Nb 1 / 4 N, LiC 1 / 2 Among these, Lithium nitrides such as LiN are the most popular because they are easily available. 3 / 2 Al 1 / 2 N, Li 3 / 2 B 1 / 2 N, and Li 5 / 3 Si 1 / 3 N is preferred. From the viewpoint of suppressing the precipitation of Li2S, Li 3 / 2 Al 1 / 2 N is particularly preferred, and Li is preferred from the viewpoint of improving the thermal stability of HICP. 3 / 2 B 1 / 2 N and Li 5 / 3 Si 1 / 3N is particularly preferred. From the viewpoint of suppressing the emission of N out of the system in the production process of the sulfide solid electrolyte, Li 3 / 2 Al 1 / 2 N and Li 3 / 2 B 1 / 2 N is particularly preferred.

[0062] Examples of raw material compounds containing element M include oxides of element M, sulfides of element M, nitrides of element M, and alloys of element M and Li. Examples of sulfides of element M include Al2S3 and SiS2. Examples of nitrides of element M include AlN, Si3N4, BN, and Mg3N2. Raw material compounds containing element M may be used singly or in combination of two or more.

[0063] The element M in the production method is not particularly limited as long as it is at least one element selected from the group consisting of Al, Ta, Si, Sc, Mg, Nb, B, Hf, C, P, Zr, and Ti. Among these, from the viewpoint of more reliably suppressing the emission of N to the outside of the system in the production process of the sulfide solid electrolyte, the element M is preferably any one of Al, Ta, Si, Sc, Mg, Nb, B, Hf, C, and P, and more preferably any one of Al, Ta, Si, Sc, Mg, Nb, and B. Furthermore, because of ease of availability, the element M is even more preferably any one of Al, Si, and B. In particular, the element M may be Al.

[0064] Examples of raw material compounds containing N include Li3N, PN, P3N5, S4N4, S2N2, and S4N2. Among these, Li3N is preferred. The raw material compounds containing N may be used alone or in combination of two or more.

[0065] Examples of raw material compounds containing Li (also referred to as Li compounds) include Li2S, Li2O, Li3N, Li2CO3, metallic lithium, etc. Among these, Li2S is preferred. One type of raw material compound containing Li may be used alone, or two or more types may be mixed and used.

[0066] Examples of raw material compounds containing P (also referred to as P compounds) include P2S3, P2S5, P2O5, P3N5, and elemental phosphorus. Among these, P2S3 and P2S5 are preferred, with P2S5 being particularly preferred. One type of raw material compound containing P may be used alone, or two or more types may be mixed and used.

[0067] Examples of raw material compounds containing S include Li2S, P2S3, P2S5, sulfides of element M, and elemental sulfur. The raw material compounds containing S may be used singly or in combination of two or more.

[0068] The composition preferably contains a Li compound, a P compound, and a Li-MN-containing compound, and more preferably, at least one of the Li compound and the P compound contains S. The Li compound, P compound, and Li-MN-containing compound include lithium sulfide, phosphorus sulfide, and compounds of the general formula Li α M β It is more preferable that the compound contains a compound represented by N (α and β are values ​​that give a stoichiometric ratio depending on the type of element M).

[0069] When the sulfide solid electrolyte contains a large amount of Li, Li2S precipitates, which reduces its atmospheric stability, while when it contains a small amount of Li, ionic conductivity may decrease. Also, when the N content is large, Li2S precipitates, which reduces its atmospheric stability, while when it contains a small amount of N, the effects of N, such as improved atmospheric stability, may not be fully realized. From these viewpoints, it is preferable that the element ratios in the composition in a mixed state simultaneously satisfy the following formulas in terms of molar ratio: 2.30 ≦ Li / P ≦ 4.20 0.0100≦N / P≦1.20 It is more preferable that the Li / P and N / P simultaneously satisfy the following formulae: 2.36 ≦ Li / P ≦ 4.12 0.0200 ≦ N / P ≦ 1.11 It is more preferable that the Li / P and N / P simultaneously satisfy the following formulae: 2.36 ≤ Li / P ≤ 4.00 0.0600 ≤ N / P ≤ 0.900 It is more preferable that the above Li / P and the above N / P simultaneously satisfy the following equations respectively. 2.60 ≤ Li / P ≤ 3.40 0.190 ≤ N / P ≤ 0.710 It is particularly preferable that the above Li / P and the above N / P simultaneously satisfy the following equations respectively. 2.77 ≤ Li / P ≤ 3.38 0.280 ≤ N / P ≤ 0.650

[0070] In addition, for the above composition, it is preferable that the molar ratios of each element of Li, P, S, N, and element M satisfy the general formula (100 - z)(yLi₂S·(1 - y)P₂S₅)·zLi α M β N (where 0 < z ≤ 40, 0.50 ≤ y ≤ 0.75, α and β are numerical values that give the stoichiometric ratio according to the type of element M). According to this, a sulfide solid electrolyte excellent in air stability and ionic conductivity at 25°C can be produced. Note that the above general formula indicates the content ratios of Li, S, P, N, and element M, and the above composition does not specify that it consists of Li₂S, P₂S₅, and Li α M β N.

[0071] In the above general formula, z is preferably more than 0 and 40 or less, and more preferably 1 or more and 30 or less. When z in the above general formula is within the above range, a sulfide solid electrolyte excellent in air stability and ionic conductivity can be produced. Furthermore, when 1 ≤ z ≤ 30, a sulfide solid electrolyte with increased ionic conductivity at 25°C can be produced. When 10 ≤ z ≤ 40, a so-called cross-linked sulfur P₂S₇ 4- (S₃P - S - PS₃) is reduced, and a sulfide solid electrolyte excellent in air stability that substantially does not contain Li₂S, which is likely to react with water, can be produced.

[0072] In the general formula, y is preferably 0.50 or more and 0.75 or less, and more preferably 0.67 or more and 0.70 or less. When the content ratios of Li2S and P2S5 in the composition are within the above ranges, a sulfide solid electrolyte having increased ionic conductivity at 25°C can be produced.

[0073] In the above general formula, α and β are numerical values ​​that give a stoichiometric ratio depending on the type of element M. The values ​​of α and β are not particularly limited, but may be, for example, 0.80≦α≦3.0 and 0.10≦β≦1.2.

[0074] (Reaction step) In this step, a composition containing Li, P, S, N, and element M is subjected to mechanical milling to react with the composition, thereby obtaining an intermediate. The method for obtaining the intermediate is not limited to this, and other methods may be used. For example, in FIG. 1, instead of mechanical milling, a melt quenching method or the like may be used.

[0075] Mechanical milling may be either dry or wet, but wet milling is preferred because it allows for more uniform mixing of the raw material compounds. Examples of mechanical milling include a container-driven mill, a media-agitating mill, milling using a high-speed rotary grinder, a roller mill, and a jet mill. Examples of container-driven mills include a rotary mill, a vibration mill, and a planetary mill. Examples of media-agitating mills include an attritor and a bead mill. Examples of milling using a high-speed rotary grinder include a hammer mill and a pin mill. Among these, a container-driven mill is preferred, and a planetary mill is particularly preferred.

[0076] The intermediate obtained in the reaction step may have a crystalline structure, but is preferably a sulfide glass. The term "sulfide glass" refers to a sulfide solid electrolyte containing an amorphous structure. When the intermediate is sulfide glass, a sulfide solid electrolyte containing a low amount of crystalline phases with low atmospheric stability, such as LiS, and highly dispersed elements such as N and M can be obtained.

[0077] (Heat treatment process) In this step, the intermediate is heat-treated at a temperature equal to or higher than the crystallization temperature to produce a sulfide solid electrolyte. The heat treatment may be carried out under reduced pressure or in an inert gas atmosphere. The crystallization temperature can be determined by measurement using a differential scanning calorimeter (DSC). For example, Li7P3S 11 To obtain the β-Li3PS4 crystal structure, the heat treatment temperature is preferably 250°C or higher and 400°C or lower. To obtain the β-Li3PS4 crystal structure, the heat treatment temperature is preferably 200°C or higher and 400°C or lower. Furthermore, to obtain the first crystal structure having diffraction peaks at 2θ = 17.9° ± 0.5°, 19.1° ± 0.5°, 29.1° ± 0.5°, and 29.8° ± 0.5° in X-ray diffraction measurement using CuKα radiation, the heat treatment temperature is preferably 250°C or higher and 400°C or lower. This is because heat treatment at a high temperature such as 500°C may result in a phase transition to the stable phase Li4P2S6.

[0078] [Variations] The method for producing a sulfide solid electrolyte according to the present invention is not limited to the above-described embodiment, and can be carried out in various forms, including the above-described forms, with various modifications and improvements.

[0079] In the above embodiment, a Li2S-P2S5-based sulfide solid electrolyte has been described as an example, but an LGPS-type sulfide solid electrolyte or an argyrodite-type sulfide solid electrolyte may also be produced by this production method. Examples of LGPS-type sulfide solid electrolytes include Li 10 GeP2S 12 Li 10 GeP2S 12 The crystal structure having the above crystalline phase has diffraction peaks at 2θ=14.4°±0.5°, 20.1°±0.5°, 20.4°±0.5°, 26.9°±0.5°, 29.5°±0.5°, and 47.3°±0.5° in X-ray diffraction measurement using CuKα radiation. An example of an argyrodite-type sulfide solid electrolyte is Li6PS5Cl. A crystalline structure having a Li6PS5Cl crystalline phase exhibits diffraction peaks at 2θ=15.6°±0.5°, 25.5°±0.5°, 30.0°±0.5°, 31.4°±0.5°, 45.0°±0.5°, and 52.5°±0.5° in X-ray diffraction measurement using CuKα radiation.

[0080] [Variation 1] As Modification 1, an embodiment for producing an LGPS-type sulfide solid electrolyte will be described. By adding a raw material compound containing Ge to the composition in the preparation step, an LGPS-type sulfide solid electrolyte can be produced. Examples of the raw material compound containing Ge include GeS2. When producing an LGPS-type sulfide solid electrolyte, it is preferable that the composition simultaneously satisfies the following formula in terms of molar ratio of elements: 5.01 ≦ Li / P ≦ 5.61 0.0051 ≦ N / P ≦ 0.41 By setting the content ratio of elements in the composition to the above range, Li 10 GeP2S 12 It is possible to produce a sulfide solid electrolyte having a crystalline phase of the above and high ionic conductivity at 25°C.

[0081] [Variation 2] As Modification 2, an embodiment will be described in which a sulfide solid electrolyte having a crystalline structure containing, as constituent elements, Li, P, S, N, an element X, and an element M. X is at least one element selected from the group consisting of Cl, Br, and I.

[0082] In Modification 2, a raw material compound containing element X is added to the above composition to produce a crystalline sulfide solid electrolyte containing Li, P, S, N, element X, and element M. This makes it possible to produce a sulfide solid electrolyte having HICPs and improved thermal stability of the HICPs.

[0083] Examples of raw material compounds containing element X include lithium halide, sulfur halide, phosphorus halide, M η X σ (where η=1 or 2, and σ=an integer of 1 to 10). Examples of lithium halides include LiCl, LiBr, and LiI. Examples of sulfur halides include SCl2, S2Cl2, SBr2, S2Br2, SI2, and S2I2. Examples of phosphorus halides include PCl3, PCl5, POCl3, PBr3, PBr5, POBr3, PI3, PCI4, and P2I4. Examples of the halide of element M include AlBr3, BBr3, AlCl3, AlBr3, AlI3, SiCl3, SiCl4, SiBr4, SiI4, SiBrI3, SiBr2I2, SiBr3I, BCl3, BBr3, and BI3. Among these, lithium halides and phosphorus halides are preferred, and lithium halides are more preferred. As the lithium halides, LiBr and LiI are preferred. The raw material compound containing the element X may be used alone or in combination of two or more. The composition may contain either one element X alone or two or more elements X. In particular, from the viewpoint of increasing ionic conductivity at 25°C, it is preferable that the element X contains Br or I alone, and it is more preferable that the element X contains Br alone. It is also preferable that the element X contains both Br and I simultaneously.

[0084] In Variant 2, when the composition simultaneously contains Br and I, the Br content relative to the total amount of Br and I in the composition is preferably 1 mol% or more and 99 mol% or less, and more preferably 5 mol% or more and 80 mol% or less.

[0085] When the content of Li is high, Li2S precipitates, resulting in a decrease in air stability. When the content of Li is low, there is a risk that HICP will not precipitate. Also, when the content of N is high, Li2S precipitates, leading to a decrease in air stability. When the content of N is low, there is a risk that the effect of containing N cannot be fully exerted. Further, when the content of element X is high, a crystal phase of lithium halide may remain in the sulfide solid electrolyte, which may reduce the ionic conductivity. When the content of element X is low, there is a risk that the effect of containing element X cannot be fully exerted. From these viewpoints, it is preferable that the composition in the preparation process of the modified example 2 simultaneously satisfies the following formulas in terms of the elemental ratio in the mixed state, each in molar ratio. 3.10 ≦ Li / P ≦ 4.20 0.0600 ≦ N / P ≦ 0.750 0.180 ≦ X / P ≦ 1.30 Moreover, it is more preferable that the above Li / P, the above N / P, and the above X / P simultaneously satisfy the following formulas. 3.10 ≦ Li / P ≦ 3.90 0.0900 ≦ N / P ≦ 0.750 0.180 ≦ X / P ≦ 1.00

[0086] The above composition preferably satisfies the molar ratio of each element of Li, P, S, N, element X, and element M in the general formula (100 - z){(1 - y)[xLi2S·(1 - x)P2S5]·yLi α M β N}·zLiX (where 0.50 ≦ x ≦ 0.80, 0 < y ≦ 0.50, 5 ≦ z ≦ 40, α and β are numerical values giving the stoichiometric ratio according to the type of element M). More preferably, x, y, and z are 0.67 ≦ x ≦ 0.73, 0.10 ≦ y ≦ 0.30, and 10 ≦ z ≦ 30, respectively. Thereby, the thermal stability of HICP can be improved. Moreover, when the above composition contains two types of elements X1 and X2 as element X, the above general formula is (100 - z1 - z2){(1 - y)[xLi2S·(1 - x)P2S5]·yLi α M βN}·z1LiX1·z2LiX2 (where 0.50 ≦ x ≦ 0.80, 0 < y ≦ 0.50, 5 ≦ (z1 + z2) ≦ 40, and α and β are numerical values that give the stoichiometric ratio according to the type of element M), and in this case, it is preferable that x, y, z1, and z2 are 0.67 ≦ x ≦ 0.73, 0.10 ≦ y ≦ 0.30, and 10 ≦ (z1 + z2) ≦ 30, respectively. Note that the above general formula indicates the content ratios of Li, S, P, N, element M, and element X, and the above composition does not specify that it consists of Li2S, P2S5, Li α M β N, and LiX.

[0087] In the above general formula, when element M is either Al or B, α = 2 / 3 and β = 1 / 2 may be used. In this case, it is preferable that x, y, and z are 0.50 ≦ x ≦ 0.80, 0 < y ≦ 0.50, and 5 ≦ z ≦ 40, respectively, more preferably 0.60 ≦ x ≦ 0.75, 0.050 ≦ y ≦ 0.40, and 10 ≦ z ≦ 30, and even more preferably 0.67 ≦ x ≦ 0.73, 0.10 ≦ y ≦ 0.30, and 15 ≦ z ≦ 25.

[0088] The raw materials used in the reaction process of Modified Example 2 preferably include a Li compound, a P compound, a halogen compound, and a Li-M-N-containing compound, and it is more preferable that at least one of the above Li compound and the above P compound contains an S element. Further, as the above Li compound, the above P compound, the above halogenated compound, and the above Li-M-N-containing compound, lithium sulfide, phosphorus sulfide, lithium halide, and a compound represented by the general formula Li α M β N (α and β are numerical values that give the stoichiometric ratio according to the type of element M) are more preferably contained.

[0089] In the heat treatment step of Modified Example 2, a sulfide solid electrolyte is produced by heat-treating the intermediate at a temperature not lower than the crystallization temperature. The heat treatment may be performed under a reduced pressure atmosphere or under an inert gas atmosphere. The crystallization temperature can be determined by measurement using a differential scanning calorimeter (DSC).

[0090] In Modification 2, a sulfide solid electrolyte containing HICP is produced. HICP is presumed to undergo a phase transition to either LICP or specific crystal structure C, and then further to β-Li3PS4. Of these crystal phases, HICP has the highest ionic conductivity. Therefore, in the heat treatment step of the second modification, the lower limit of the heat treatment temperature is the HICP generation temperature T H The upper limit of the heat treatment temperature is preferably the temperature T β It is preferable that the temperature is equal to or lower than the LICP generation temperature T L or the temperature T at which a specific crystal structure C is formed C It is more preferable that it is equal to or less than T H , T L , T C and T β can be determined by XRD measurement. The sulfide solid electrolyte produced in Modification 2 is T β -T H But, T β -T H ≧40°C, and T β -T H More preferably, T β -T H More preferably, T is ≥ 60°C. β -T H It is particularly preferred that it is ≧70°C.

[0091] The sulfide solid electrolyte produced by Modification 2 has a wide heat treatment temperature range in which ionic conductivity does not decrease. In other words, even if the heat treatment temperature deviates from the intended temperature in the heat treatment step, there is little risk of the ionic conductivity of the produced sulfide solid electrolyte decreasing. Therefore, Modification 2 has the advantage that a sulfide solid electrolyte with high ionic conductivity can be produced without requiring strict temperature control in the heat treatment step.

[0092] "HICP" refers to a crystalline phase having diffraction peaks at 2θ=20.2°±0.5° and 23.6°±0.5° in X-ray diffraction measurement using CuKα radiation. This crystalline structure is a crystalline phase described in Patent Document 2 and the like, and is a crystalline phase with high Li-ion conductivity. "LICP" refers to a crystalline phase having diffraction peaks at 2θ=21.0°±0.5° and 28.0°±0.5° in X-ray diffraction measurement using CuKα radiation. This crystalline structure is a crystalline phase described in Patent Document 2 and the like, and is a crystalline phase with low Li-ion conductivity. "Specific crystalline structure C" refers to a crystalline phase having diffraction peaks at 2θ=17.5°±0.5° and 24.9°±0.5° in X-ray diffraction measurement using CuKα radiation. "β-Li3PS4" represents a crystalline phase having diffraction peaks at 2θ=17.5°±0.5°, 18.1°±0.5°, 29.1°±0.5°, 29.9°±0.5°, and 31.2°±0.5° in X-ray diffraction measurement using CuKα radiation.

[0093] X-ray diffraction measurements using CuKα radiation in this specification are performed according to the following procedure. A solid electrolyte powder to be measured is filled into an airtight X-ray diffraction sample holder in an argon atmosphere with a dew point of -50°C or lower. Powder X-ray diffraction measurements are performed using an X-ray diffractometer (Rigaku's "MiniFlex II"). The radiation source is CuKα radiation, the tube voltage is 30 kV, and the tube current is 15 mA. Diffracted X-rays are passed through a 30 μm-thick Kβ filter and detected by a high-speed one-dimensional detector (model number: D / teX Ultra 2). The sampling width is 0.01°, the scan speed is 5° / min, the divergence slit width is 0.625°, the receiving slit width is 13 mm (open), and the scattering slit width is 8 mm.

[0094] <How to select raw material compounds> According to the method for producing a sulfide solid electrolyte of the present invention, by using a raw material compound containing N, element A, and element M, it is possible to prevent N from being released outside the system during the production process of the sulfide solid electrolyte. In selecting the elements A and M that provide such effects, the present inventors used first-principles calculations. Hereinafter, a method for selecting raw material compounds used in the production of a sulfide solid electrolyte according to one embodiment of the present invention will be described.

[0095] In this embodiment, raw material compounds are selected according to the procedures (1) to (3). (1) A candidate material containing N, an element A', and an element M', in which the first nearest neighbor atoms of the element A' and the element M' are N, is selected. (2) Using first-principles calculations, we estimate the defect formation energy E of N in the above candidate materials. Ndefect Calculate. (3) E above Ndefect is 4.00 eV or more, the candidate material is selected as the raw material compound.

[0096] First-principles calculations are a computational method for predicting physical properties non-empirically, and are a technique that can calculate the total energy and electron energy band structure of a model containing atoms whose atomic numbers and spatial coordinates are known. Calculating the forces acting on atoms enables structural optimization, and also allows calculation of lattice constants, stable structures at 0 K, band gaps, etc. Calculation methods can be broadly divided into two types: "wave function theory" and "density functional theory." The calculation method used in this specification is based on density functional theory.

[0097] Defect formation energy E of N Ndefect is the energy value required to remove N from the crystal structure and generate a defect. The defect formation energy of N is the total energy E of the crystal structure without defects. perfect and the total energy E of the crystal structure containing the N defect Nvacancy and the chemical potential μ of the N atom N and is defined by the following formula (1). E Ndefect = ( E Nvacancy + μ N ) - E perfect Formula (1) That is, the defect formation energy of N, E Ndefect The procedure for calculating is as follows: (a) Obtain the composition and crystal structure of the candidate material. (b) Chemical potential μ of the N atom desorbed as a defect N Calculate. (c) The total energy E of a defect-free crystal structure perfect is calculated by structural optimization calculation. (d) Total energy E of a crystal structure containing N defects Nvacancy is calculated by structural optimization calculation. (e) The defect formation energy E of N according to equation (1) Ndefect Calculate. If there are multiple N-occupied sites in the crystal structure of the candidate material, E Ndefect The lowest value is the E of the candidate material. Ndefect Used as. The composition and crystal structure of the candidate material can be arbitrarily selected from those available in publicly known publications, databases, etc. The candidate material is not particularly limited as long as it is a compound containing N, element A', and element M', but is preferably a compound that is stable at room temperature and normal pressure.

[0098] In this embodiment, the element A' is a metal element. The element M' is an element other than nitrogen that belongs to any of Groups 2 to 15 of the periodic table and is different from the element A'. N is a nitrogen element. The element A' is not particularly limited, but is preferably any one of an alkali metal element, an alkaline earth metal element, and an aluminum element, more preferably at least one element selected from Li, Na, K, Mg, Ca, and Al, and even more preferably Li, which makes it easier to operate the sulfide solid electrolyte as a battery.

[0099] In this embodiment, Li α M´ βThe defect formation energy of N was calculated for candidate materials represented by N (α and β are values ​​that give the stoichiometric ratio depending on the type of element M) and Li3N. That is, Li was selected as element A'. As elements M', B, Mg, Al, Si, P, Ca, Sr, Ti, V, Cr, Mn, Fe, Co, Ni, Zn, Ga, Ge, Sr, Y, Zr, Nb, In, Sn, Ce, Hf, Ta, and C were evaluated. The first-principles calculations were performed using the Vienna Ab-initio Simulation Package (VASP) software. The calculation conditions were as follows: The k-point was set so that the k-resolution value was approximately 1000. The k-resolution is the product of the number of atoms in the model and the k-points in the a, b, and c-axis directions. Cutoff energy of plane wave basis functions: 520 eV Approximation method for exchange-correlation interaction: GGA+U Pseudopotential: PAW(PBEsol) k point:k-resolution≒1000 Convergence condition for SCF calculation: 10 -4 eV Occupancy rate of each atomic site (Occ.): 1 The 3d orbital is the outermost orbital, and in the state of a cation with a stable valence, the 3d orbital is not a closed shell, and electrons exist in the 3d orbital. For the first-principles calculation of materials containing V, Cr, Mn, Fe, Co, and Ni, which are transition metal elements, the Hubbard U eff The values ​​used as calculation conditions were the Hubbard U values ​​shown in Table 1, which reflect the localization effect of electrons in the d orbitals. eff The values ​​are taken from the calculation conditions of first-principles calculations carried out in the crystal structure database Materials Project (https: / / materialsproject.org / #search / materials) (as of August 22, 2019). By searching the database for materials containing V, Cr, Mn, Fe, Co, and Ni, the U eff The value was obtained.

[0100] [Table 1]

[0101] In addition, in step (d) above, in order to reduce interactions between N defects, the calculation model cell was designed so that the lattice constants a, b, and c were all approximately 10 Å, with the total number of atoms not exceeding 200. Table 2 shows the lattice constants used in the calculations for some of the candidate materials.

[0102] [Table 2]

[0103] Table 3 shows the element M´, the chemical composition of each candidate material, and the defect formation energy E Ndefect Shows.

[0104] [Table 3]

[0105] From Table 3, the defect formation energy E of N in Li3N, which is prone to N defect formation, Ndefect is found to be 2.94 eV. In addition, the elements V, Y, Ga, Ca, Ce, Sn, Zn, Ge, Cr, Mn, Sr, In, Co, Ni, and Fe are α M´ β Defect formation energy E of N in N Ndefect It can be seen that the value is small, at 3.88 eV or less. Therefore, in a candidate material containing any of V, Y, Ga, Ca, Ce, Sn, Zn, Ge, Cr, Mn, Sr, In, Co, Ni, and Fe as the element M', N defects are likely to be generated, and it is predicted that the effect of the present invention of suppressing the emission of N to the outside of the system in the production process of a sulfide solid electrolyte will not be obtained, or the effect will be small. On the other hand, the elements Al, Ta, Si, Sc, Mg, Nb, B, Hf, C, P, Zr, and Ti are α M´ β Defect formation energy E of N in N NdefectIt can be seen that the difference is large, at 4.00 eV or more. Therefore, it is predicted that if the candidate material contains any of Al, Ta, Si, Sc, Mg, Nb, B, Hf, C, P, Zr, and Ti as the element M', N defects are unlikely to be generated, and the effect of the present invention, which suppresses the emission of N to the outside of the system in the production process of a sulfide solid electrolyte, is highly likely to be exhibited.

[0106] The candidate materials have the defect formation energy E Ndefect It is predicted that the larger the value of , the less likely N defects are to be generated, and the more likely it is that N will be released from the system during the production process of the sulfide solid electrolyte. Ndefect is 4.00 eV or more, preferably 4.10 eV or more, more preferably 4.20 eV or more, even more preferably 4.30 eV or more, and particularly preferably 4.35 eV or more.

[0107] In this embodiment, calculations were performed for the case where element A' contained Li. α M´ β The first-principles calculation was performed using N as a model. However, the present invention is not limited to this. The element A' may be any metal element. For example, a candidate material containing any of Na, K, Mg, Ca, and Al may be selected as the element A', and a raw material compound may be selected using the first-principles calculation.

[0108] <Sulfide solid electrolyte> [Embodiment 1] A sulfide solid electrolyte according to one embodiment of the present invention is a composition containing P, S, N, element A, and element M, and is produced by a production method including: preparing raw material compounds containing N, element A, and element M; reacting the composition to obtain an intermediate; and heating the intermediate to obtain a sulfide solid electrolyte. Hereinafter, the sulfide solid electrolyte will be described using an example in which element A contains Li.

[0109] The sulfide solid electrolyte has a crystalline structure. "Having a crystalline structure" means that, in an X-ray diffraction measurement, peaks attributable to the crystalline structure of the sulfide solid electrolyte are observed in the X-ray diffraction pattern. The sulfide solid electrolyte may contain an amorphous portion.

[0110] Examples of the crystal structure of the sulfide solid electrolyte include HICP, LGPS, argyrodite, and Li7P3S 11 Among these, the crystal structure is preferably HICP, LGPS, argyrodite, or Li7P3S from the viewpoint of lithium ion conductivity. 11 Among these, Li7P3S is preferred because it has high stability against Li. 11 From the viewpoint of stability to the atmosphere, it is preferable that the material contains a crystal structure having a crystalline phase of Li4P2S6 or β-Li3PS4, or a first crystal structure having diffraction peaks at 2θ=17.9°±0.5°, 19.1°±0.5°, 29.1°±0.5°, and 29.8°±0.5° in X-ray diffraction measurement using CuKα radiation, and among these, the first crystal structure having diffraction peaks at 2θ=17.9°±0.5°, 19.1°±0.5°, 29.1°±0.5°, and 29.8°±0.5° in X-ray diffraction measurement using CuKα radiation is more preferable because of its high lithium ion conductivity.

[0111] The first crystal structure may include specific crystal structure A having diffraction peaks at 2θ=17.9°±0.5°, 19.1°±0.5°, 29.1°±0.5°, 29.8°±0.5°, and 30.9°±0.5° in the X-ray diffraction measurement, or specific crystal structure B having diffraction peaks at 2θ=17.9°±0.5°, 19.1°±0.5°, 29.1°±0.5°, and 29.8°±0.5° but no diffraction peak at 30.9°±0.5° in the X-ray diffraction measurement. The above configuration provides a sulfide solid electrolyte that can increase the initial coulombic efficiency of an all-solid-state battery including the solid electrolyte.

[0112] The diffraction peak of the first crystal structure may have a 2θ range within ±0.3° or within ±0.1°.

[0113] The above Li7P3S 11 The crystal structure having the above crystalline phase has diffraction peaks at 2θ=17.8°±0.5°, 18.5°±0.5°, 23.7°±0.5°, 29.6°±0.5°, and 30.0°±0.5° in X-ray diffraction measurement using CuKα radiation.

[0114] The LGPS-type sulfide solid electrolyte may be, for example, Li 10 GeP2S 12 Li 10 GeP2S 12 The crystal structure having the above crystalline phase has diffraction peaks at 2θ=14.4°±0.5°, 20.1°±0.5°, 20.4°±0.5°, 26.9°±0.5°, 29.5°±0.5°, and 47.3°±0.5° in X-ray diffraction measurement using CuKα radiation.

[0115] An example of the argyrodite-type sulfide solid electrolyte is Li6PS5Cl. A crystalline structure having a Li6PS5Cl crystalline phase exhibits diffraction peaks at 2θ=15.6°±0.5°, 25.5°±0.5°, 30.0°±0.5°, 31.4°±0.5°, 45.0°±0.5°, and 52.5°±0.5° in X-ray diffraction measurement using CuKα radiation.

[0116] The crystal structure having the above Li4P2S6 crystalline phase has diffraction peaks at 2θ=16.9°±0.5°, 27.1°±0.5°, 32.1°±0.5°, and 32.5°±0.5° in X-ray diffraction measurement using CuKα radiation.

[0117] The crystal structure having the β-Li3PS4 crystalline phase has diffraction peaks at 2θ=17.5°±0.5°, 18.1°±0.5°, 29.1°±0.5°, 29.9°±0.5°, and 31.2°±0.5° in X-ray diffraction measurement using CuKα radiation.

[0118] The sulfide solid electrolyte preferably contains a so-called ortho-composition anion structure as a main component. For example, when the sulfide solid electrolyte is a Li2S-P2S5-based solid electrolyte, PS4 3- It is preferable that the polymer contains the structure as a main component. Here, "main component" means that the proportion of a specific component in all components is 50 mol % or more.

[0119] When the sulfide solid electrolyte contains an anionic structure with an ortho composition as a main component, the content of the anionic structure with an ortho composition relative to all anionic structures constituting the sulfide solid electrolyte is 50 mol% or more and less than 100 mol%, preferably 60 mol% or more and less than 100 mol%, more preferably 70 mol% or more and less than 100 mol%, even more preferably 80 mol% or more and less than 100 mol%, and particularly preferably 90 mol% or more and less than 100 mol%.

[0120] The sulfide solid electrolyte preferably does not substantially contain bridging sulfur. Because bridging sulfur reacts with water to produce hydrogen sulfide, atmospheric stability can be improved by substantially not containing bridging sulfur. For example, when the sulfide solid electrolyte is a Li2S-P2S5-based solid electrolyte, it preferably does not substantially contain an S3P-S-PS3 structure. The substantial absence of bridging sulfur can be confirmed by the absence of a peak corresponding to a bridging sulfur structure when a Raman spectrum is measured using a laser with an excitation wavelength of 532 nm. For example, the substantial absence of an S3P-S-PS3 structure can be confirmed by the absence of a peak corresponding to a bridging sulfur structure when a Raman spectrum is measured using a laser with an excitation wavelength of 532 nm. -1 This can be confirmed by the absence of a peak. The sulfide solid electrolyte may contain a small amount of bridging sulfur. In this case, the intensity I of the peak attributed to the anion structure of the ortho-composition in Raman spectroscopy measurement is O Intensity of the peaks attributed to bridging sulfur, I P Ratio of I P / I Ois preferably 0.7 or less, more preferably 0.5 or less, and even more preferably 0.35 or less. For example, when the sulfide solid electrolyte is a Li2S-P2S5-based solid electrolyte, PS4 3- 417cm due to structure -1 The peak intensity at I O corresponds to 402cm originating from the S3PS-PS3 structure. -1 The peak intensity at I P is equivalent to

[0121] The sulfide solid electrolyte preferably contains substantially no Li2S. Because Li2S reacts with water to produce hydrogen sulfide, atmospheric stability can be improved by being substantially free of Li2S. Here, "substantially free of Li2S" means that the solid electrolyte does not contain a crystalline structure having diffraction peaks at 2θ=27.0±0.5°, 31.2±0.5°, 44.8±0.5°, and 53.1±0.5° in X-ray diffraction measurement using CuKα radiation.

[0122] When the sulfide solid electrolyte contains a large amount of Li, Li2S precipitates, which reduces its atmospheric stability, while when it contains a small amount of Li, ionic conductivity may decrease. Also, when the N content is large, Li2S precipitates, which reduces its atmospheric stability, while when it contains a small amount of N, the effects of N, such as improved atmospheric stability, may not be fully realized. From these viewpoints, it is preferable that the sulfide solid electrolyte simultaneously satisfies the following formulas in terms of element ratios in terms of molar ratios: 2.30 ≦ Li / P ≦ 4.20 0.0100≦N / P≦1.20 It is more preferable that the Li / P and N / P simultaneously satisfy the following formulae: 2.36 ≦ Li / P ≦ 4.12 0.0200 ≦ N / P ≦ 1.11 It is more preferable that the Li / P and N / P simultaneously satisfy the following formulae: 2.36 ≦ Li / P ≦ 4.00 0.0600 ≦ N / P ≦ 0.900 It is more preferable that the above Li / P and the above N / P simultaneously satisfy the following formulas respectively. 2.60 ≦ Li / P ≦ 3.40 0.190 ≦ N / P ≦ 0.710 It is particularly preferable that the above Li / P and the above N / P simultaneously satisfy the following formulas respectively. 2.77 ≦ Li / P ≦ 3.38 0.280 ≦ N / P ≦ 0.650

[0123] As the sulfide solid electrolyte, it preferably has a composition represented by the general formula (100 - z)(yLi₂S·(1 - y)P₂S₅)·zLi α M β N (where 0 < z ≦ 40, 0.50 ≦ y ≦ 0.75, α and β are numerical values giving the stoichiometric ratio according to the type of element M). By having the sulfide solid electrolyte have a composition represented by the above general formula, the air stability and the ionic conductivity at 25°C can be improved. Note that the above general formula shows the content ratios of Li, S, P, N, and element M, and the above composition does not specify that the composition consists of Li₂S, P₂S₅, and Li α M β N.

[0124] As the lower limit of the ionic conductivity of the sulfide solid electrolyte at 25°C, 0.4×10 -3 S / cm is preferable, 1.0×10 -3 S / cm is more preferable, and 1.5×10 -3 S / cm is even more preferable. By having the ionic conductivity of the sulfide solid electrolyte at 25°C within the above range, the rate characteristics of the all-solid-state battery can be improved.

[0125] The ionic conductivity of the sulfide solid electrolyte at 25°C was determined by measuring AC impedance using the following method. In an argon atmosphere with a dew point of -50°C or lower, 120 mg of sample powder was placed in a powder molder with an inner diameter of 10 mm, and then uniaxially pressed using a hydraulic press at a pressure of 50 MPa or less per sample area. After the pressure was released, SUS316L powder was placed on the top and bottom of the sample as current collectors, and then uniaxially pressed for 5 minutes at a pressure of 360 MPa per pellet area to obtain a pellet for ionic conductivity measurement. This pellet for ionic conductivity measurement was inserted into a Hohsen HS cell, and AC impedance measurement was performed. The measurement conditions were an applied voltage amplitude of 20 mV, a frequency range of 1 MHz to 100 mHz, and a measurement temperature of 25°C.

[0126] Thus, the sulfide solid electrolyte can be suitably used as a solid electrolyte for all-solid-state batteries.

[0127] [Embodiment 2] A sulfide solid electrolyte according to another embodiment of the present invention contains Li, P, S, N, an element X, and an element M. The element X represents at least one element selected from the group consisting of Cl, Br, and I.

[0128] The sulfide solid electrolyte may contain one element selected from the group consisting of Al, B, and Si as the element M, or may contain Al as the element M.

[0129] If the sulfide solid electrolyte contains a large amount of Li, Li2S precipitates, reducing its atmospheric stability, while if the Li content is low, HICP may not precipitate. Furthermore, if the N content is high, Li2S precipitates, reducing its atmospheric stability, while if the N content is low, the effects of including N may not be fully realized. Furthermore, if the content of element X is high, a lithium halide crystalline phase may remain in the sulfide solid electrolyte, reducing ionic conductivity, while if the content is low, the effects of including element X may not be fully realized. Due to these circumstances, it is preferable that the sulfide solid electrolyte simultaneously satisfies the following equations in molar ratios for the content ratios of Li to P (Li / P), N to P (N / P), and X to P (X / P) with respect to P above. 3.10 < Li / P < 4.20 0.0600 < N / P < 0.750 0.180 < X / P < 1.30 Moreover, it is more preferable that Li / P, N / P, and X / P simultaneously satisfy the following equations. 3.10 < Li / P < 3.90 0.0900 < N / P < 0.750 0.180 < X / P < 1.00

[0130] The sulfide solid electrolyte preferably has a composition represented by the general formula (100 - z){(1 - y)[xLi2S·(1 - x)P2S5]·yLi α M β N}·zLiX (where 0.50 ≤ x ≤ 0.80, 0 < y ≤ 0.50, 5 ≤ z ≤ 40, α and β are numerical values giving the stoichiometric ratio according to the type of element M), and more preferably, x, y, and z are 0.67 ≤ x ≤ 0.73, 0.10 ≤ y ≤ 0.30, and 10 ≤ z ≤ 30, respectively. By having the composition represented by the above general formula, the thermal stability of HICP can be improved. Moreover, when the sulfide solid electrolyte contains two types of elements X1 and X2 as element X, the above general formula can also be represented as (100 - z1 - z2){(1 - y)[xLi2S·(1 - x)P2S5]·yLi α M β N}·z1LiX1·z2LiX2 (where 0.50 ≤ x ≤ 0.80, 0 < y ≤ 0.50, 5 ≤ (z1 + z2) ≤ 40, α and β are numerical values giving the stoichiometric ratio according to the type of element M), and in this case, x, y, z1, and z2 are preferably 0.67 ≤ x ≤ 0.73, 0.10 ≤ y ≤ 0.30, and 10 ≤ (z1 + z2) ≤ 30, respectively. The above general formula indicates the content ratios of Li, S, P, N, element M, and element X. The above composition does not specify that it consists of Li2S, P2S5, Li α M β N, and LiX.

[0131] In the above general formula, when element M is any one of Al, B, and Sc, α may be 2 / 3 and β may be 1 / 2. In this case, x, y, and z are preferably 0.50 ≦ x ≦ 0.80, 0 < y ≦ 0.50, and 5 ≦ z ≦ 40, more preferably 0.60 ≦ x ≦ 0.75, 0.050 ≦ y ≦ 0.40, and 10 ≦ z ≦ 30, and even more preferably 0.67 ≦ x ≦ 0.73, 0.10 ≦ y ≦ 0.30, and 15 ≦ z ≦ 25.

[0132] The sulfide solid electrolyte preferably contains Br or I alone as element X, and more preferably contains Br alone. It is also preferable to contain Br and I simultaneously. When the sulfide solid electrolyte contains Br and I simultaneously, the content of Br with respect to the total amount of Br and I contained in the sulfide solid electrolyte is preferably 1 mol% or more and 99 mol% or less, and more preferably 5 mol% or more and 80 mol% or less.

[0133] The sulfide solid electrolyte preferably contains HICP. That is, it preferably contains a crystal structure having diffraction peaks at 2θ = 20.2° ± 0.5° and 23.6° ± 0.5° in X-ray diffraction measurement using CuKα radiation.

[0134] The sulfide solid electrolyte preferably does not contain LICP. That is, it preferably does not contain a crystal structure having diffraction peaks at 2θ = 21.0° ± 0.5° and 28.0° ± 0.5° in X-ray diffraction measurement using CuKα radiation. The sulfide solid electrolyte may contain a small amount of LICP. In this case, the diffraction peak intensity I at 2θ = 20.2° ± 0.5° in X-ray diffraction measurement using CuKα radiation H with respect to the diffraction peak intensity I at 2θ = 21.0° ± 0.5° LDiffraction peak intensity ratio I L / I H is 0 L / I H <3.2 is preferred, and 0 L / I H <2.5 is more preferable, 0 L / I H <2.0 is more preferable, and 0 L / I H It is even more preferable that the diffraction peak intensity ratio I is less than 1.0. L / I H indicates the abundance ratio of HICP and LICP contained in the sulfide solid electrolyte. In other words, the diffraction peak intensity ratio I L / I H A small value indicates that the amount of LICP is relatively small compared to HICP.

[0135] The ionic conductivity of the sulfide solid electrolyte of embodiment 2 at 25°C is 2.0 × 10 -3 S / cm or more is preferable, and 2.5×10 -3 S / cm or more is more preferable, and 3.0×10 -3 S / cm or more is more preferable, and 4.0×10 -3 The above-mentioned structure can improve the high-rate discharge performance of an all-solid-state battery including the sulfide solid electrolyte.

[0136] <All-solid-state battery> The all-solid-state battery includes an anode layer, a solid electrolyte layer, and a cathode layer. FIG. 2 is a schematic cross-sectional view showing an all-solid-state battery according to one embodiment of the present invention. An all-solid-state battery 10, which is a secondary battery, includes an anode layer 1 and a cathode layer 2 arranged with a solid electrolyte layer 3 interposed therebetween. The anode layer 1 includes an anode substrate layer 4 and an anode mixture layer 5, with the anode substrate layer 4 being the outermost layer of the anode layer 1. The cathode layer 2 includes a cathode substrate layer 7 and a cathode mixture layer 6, with the cathode substrate layer 7 being the outermost layer of the cathode layer 2. In the all-solid-state battery 10 shown in FIG. 2, the cathode mixture layer 6, the solid electrolyte layer 3, the anode mixture layer 5, and the anode substrate layer 4 are stacked in this order on the cathode substrate layer 7.

[0137] ​​​​In the all-solid-state battery, the anode layer 1, the solid electrolyte layer 3, the cathode layer 2, or a combination thereof contains the sulfide solid electrolyte. In the all-solid-state battery, the anode layer 1, the solid electrolyte layer 3, the cathode layer 2, or a combination thereof contains the sulfide solid electrolyte, and therefore the initial coulombic efficiency is excellent. Because the sulfide solid electrolyte has excellent resistance to reduction, it is preferable that the anode layer 1 and / or the solid electrolyte layer 3 contain the sulfide solid electrolyte. With the above configuration, the effects of the present invention are further improved.

[0138] The all-solid-state battery may also use a solid electrolyte other than the sulfide solid electrolyte, which may be a sulfide solid electrolyte other than the sulfide solid electrolyte, an oxide-based solid electrolyte, a dry polymer electrolyte, a gel polymer electrolyte, or a quasi-solid electrolyte.

[0139] As sulfide solid electrolytes other than the sulfide solid electrolyte, those having high Li ion conductivity are preferred, and examples thereof include Li2S-P2S5, Li2S-P2S5-LiI, Li2S-P2S5-LiCl, Li2S-P2S5-LiBr, Li2S-P2S5-Li2O, Li2S-P2S5-Li2O-LiI, Li2S-P2S5-Li3N, Li2S-SiS2, Li2S-SiS2-LiI, Li2S-SiS2-LiBr, Li2S-SiS2-LiCl, Li2S-SiS2-B2S3-LiI, Li2S-SiS2-P2S5-LiI, Li2S-B2S3, and Li2S-P2S5-Z. m S 2n (where m and n are positive numbers, and Z is Ge, Zn, or Ga.), Li2S-GeS2, Li2S-SiS2-Li3PO4, Li2S-SiS2-Li δ XO ε (where δ and ε are positive numbers, and X is one of P, Si, Ge, B, Al, Ga, and In.) Li 10 GeP2S 12 Among these, Li2S-P2S5 and Li 10 GeP2S 12etc. Li2S-P2S5 is preferably xLi2S·(100-x)P2S5 (70≦x≦80).

[0140] [Negative electrode layer] The negative electrode layer 1 includes a negative electrode substrate layer 4 and a negative electrode mixture layer 5 laminated on the surface of the negative electrode substrate layer 4. The negative electrode layer 1 may have an intermediate layer (not shown) between the negative electrode substrate layer 4 and the negative electrode mixture layer 5.

[0141] (Negative electrode base material layer) The negative electrode substrate layer 4 is a conductive layer. There are no particular limitations on the material of the negative electrode substrate layer 4 as long as it is a conductor. Examples of the material include one or more metals selected from the group consisting of copper, aluminum, titanium, nickel, tantalum, niobium, hafnium, zirconium, zinc, tungsten, bismuth, antimony, gold, silver, iron, platinum, chromium, tin, indium, alloys containing one or more of these metals, and stainless steel alloys.

[0142] The lower limit of the average thickness of the negative electrode substrate layer 4 is preferably 3 μm, more preferably 5 μm, and even more preferably 8 μm. The upper limit of the average thickness of the negative electrode substrate layer 4 is preferably 200 μm, more preferably 100 μm, and even more preferably 50 μm. By setting the average thickness of the negative electrode substrate layer 4 to the above lower limit or more, the strength of the negative electrode substrate layer 4 can be sufficiently increased, and the negative electrode layer 1 can be formed well. By setting the average thickness of the negative electrode substrate layer 4 to the above upper limit or less, the volume of the other components can be sufficiently secured.

[0143] (Negative electrode mixture layer) The negative electrode mixture layer 5 can be formed from a so-called negative electrode mixture containing a negative electrode active material. The negative electrode mixture may contain a negative electrode mixture or a negative electrode composite containing a negative electrode active material and the sulfide solid electrolyte. The negative electrode mixture may contain optional components such as a solid electrolyte other than the sulfide solid electrolyte, a conductive agent, a binder, a filler, etc., as needed.

[0144] <Negative electrode active material> As the negative electrode active material, a material capable of absorbing and releasing lithium ions is usually used. Specific examples of the negative electrode active material include metallic lithium, metals or semimetals such as Si and Sn, metal oxides or semimetal oxides such as Si oxide and Sn oxide, polyphosphate compounds, carbon materials such as graphite and non-graphitic carbon (easily graphitizable carbon or non-graphitizable carbon), and lithium metal composite oxides such as lithium titanate.

[0145] The lower limit of the content of the negative electrode active material in the negative electrode mixture is preferably 10% by mass, more preferably 15% by mass. The upper limit of the content of the negative electrode active material is preferably 60% by mass, more preferably 70% by mass, even more preferably 80% by mass, particularly preferably 90% by mass, and may even be 95% by mass. By setting the content of the negative electrode active material within the above range, the electrical capacity of the all-solid-state battery can be increased.

[0146] <Negative electrode mixture or negative electrode composite> The negative electrode mixture is a mixture prepared by mixing the negative electrode active material and the sulfide solid electrolyte by mechanical milling, etc. For example, the mixture of the negative electrode active material and the sulfide solid electrolyte can be obtained by mixing particulate negative electrode active material and particulate sulfide solid electrolyte. Examples of the negative electrode composite include a composite in which the negative electrode active material and the sulfide solid electrolyte are chemically or physically bonded, a composite in which the negative electrode active material and the sulfide solid electrolyte are mechanically combined, etc. The composite is one in which the negative electrode active material and the sulfide solid electrolyte are present in a single particle, and examples of the composite include one in which the negative electrode active material and the sulfide solid electrolyte form an aggregated state, and one in which the sulfide solid electrolyte-containing coating is formed on at least a portion of the surface of the negative electrode active material. The negative electrode mixture or negative electrode composite may contain a solid electrolyte other than the sulfide solid electrolyte. The negative electrode active material contained in the negative electrode mixture and the sulfide solid electrolyte constitute a negative electrode mixture or a negative electrode composite, which can improve ionic conductivity.

[0147] When the negative electrode mixture contains a solid electrolyte, the lower limit of the content of the solid electrolyte in the negative electrode mixture may be 5% by mass, and preferably 10% by mass. The upper limit of the content of the solid electrolyte in the negative electrode mixture is preferably 90% by mass, more preferably 85% by mass, even more preferably 80% by mass, and particularly preferably 75% by mass. By setting the content of the solid electrolyte within the above range, the electric capacity of the all-solid-state battery can be increased. The negative electrode mixture may contain the sulfide solid electrolyte, or may contain a solid electrolyte other than the sulfide solid electrolyte.

[0148] <Other optional ingredients> The conductive agent is not particularly limited. Examples of such conductive agents include natural or artificial graphite, carbon black such as furnace black, acetylene black, and ketjen black, metals, and conductive ceramics. The conductive agent may be in the form of powder or fiber. The content of the conductive agent in the negative electrode mixture may be, for example, 0.5% by mass or more and 30% by mass or less. The negative electrode mixture may not contain a conductive agent.

[0149] The binder (binding agent) is not particularly limited, and examples thereof include thermoplastic resins such as fluororesins (polytetrafluoroethylene (PTFE), polyvinylidene fluoride (PVDF), etc.), polyethylene, polypropylene, polyimide, and polyacrylic acid; elastomers such as ethylene-propylene-diene rubber (EPDM), sulfonated EPDM, styrene-butadiene rubber (SBR), and fluororubber; and polysaccharide polymers.

[0150] The filler is not particularly limited, and examples of the main component of the filler include polyolefins such as polypropylene and polyethylene, silica, alumina, zeolite, glass, and carbon.

[0151] The lower limit of the average thickness of the negative electrode mixture layer 5 is preferably 30 μm, more preferably 60 μm. The upper limit of the average thickness of the negative electrode mixture layer 5 is preferably 1000 μm, more preferably 500 μm, and even more preferably 200 μm. By setting the average thickness of the negative electrode mixture layer 5 to the above lower limit or more, an all-solid-state battery having a high energy density can be obtained. By setting the average thickness of the negative electrode mixture layer 5 to the above upper limit or less, an all-solid-state battery having a negative electrode with excellent rate characteristics and high active material utilization can be obtained.

[0152] (middle class) The intermediate layer is a coating layer on the surface of the negative electrode substrate layer 4, and contains conductive particles such as carbon particles to reduce the contact resistance between the negative electrode substrate layer 4 and the negative electrode mixture layer 5. The configuration of the intermediate layer is not particularly limited, and the intermediate layer can be formed, for example, from a composition containing a resin binder and conductive particles.

[0153] [Positive electrode layer] The positive electrode layer 2 includes a positive electrode substrate layer 7 and a positive electrode mixture layer 6 laminated on the surface of the positive electrode substrate layer 7. Similar to the negative electrode layer 1, the positive electrode layer 2 may have an intermediate layer between the positive electrode substrate layer 7 and the positive electrode mixture layer 6. This intermediate layer may have the same configuration as the intermediate layer of the negative electrode layer 1.

[0154] (Positive electrode substrate layer) The positive electrode substrate layer 7 can have the same configuration as the negative electrode substrate layer 4. The material of the positive electrode substrate layer 7 is not limited as long as it is a conductor. For example, it can be one or more metals selected from the group consisting of copper, aluminum, titanium, nickel, tantalum, niobium, hafnium, zirconium, zinc, tungsten, bismuth, antimony, gold, silver, iron, platinum, chromium, tin, indium, alloys containing one or more of these metals, and stainless steel alloys.

[0155] The lower limit of the average thickness of the positive electrode substrate layer 7 is preferably 3 μm, more preferably 5 μm. The upper limit of the average thickness of the positive electrode substrate layer 7 is preferably 200 μm, more preferably 100 μm, and even more preferably 50 μm. By making the average thickness of the positive electrode substrate layer 7 equal to or greater than the above lower limit, the strength of the positive electrode substrate layer 7 can be sufficiently increased, allowing the positive electrode layer 2 to be formed satisfactorily. By making the average thickness of the positive electrode substrate layer 7 equal to or less than the above upper limit, sufficient volume for the other components can be ensured.

[0156] (Positive electrode mixture layer) The positive electrode mixture layer 6 can be formed from a so-called positive electrode mixture containing a positive electrode active material. The positive electrode mixture may contain a positive electrode mixture or a positive electrode composite containing a positive electrode active material and a solid electrolyte. The sulfide solid electrolyte may be used as the solid electrolyte. Like the negative electrode mixture, the positive electrode mixture forming the positive electrode mixture layer 6 may contain optional components such as a solid electrolyte, a conductive agent, a binder, and a filler, as necessary. Note that the positive electrode mixture layer may not contain a solid electrolyte.

[0157] <Cathode active material> The positive electrode active material contained in the positive electrode mixture layer 6 can be a known material that is commonly used in all-solid-state batteries. x M e O y (Me represents at least one transition metal) x CoO2, Li x NiO2, Li x MnO3, Li x Ni α Co (1-α) O2, Li x Ni α Mn β Co (1-α-β) Li with spinel-type crystal structure, such as O2 x Mn2O4, Li x Ni α Mn (2-α) O4, etc.), Li w Me x (AO y ) z(Me represents at least one transition metal, and A represents, for example, P, Si, B, V, etc.) polyanion compounds (LiFePO4, LiMnPO4, LiNiPO4, LiCoPO4, Li3V2(PO4)3, Li2MnSiO4, Li2CoPO4F, etc.) in which the elements or polyanions in these compounds may be partially substituted with other elements or anion species. In the positive electrode active material layer, one of these compounds may be used alone, or two or more may be used in combination.

[0158] Positive electrode active materials include lithium alloys such as Li-Al, Li-In, Li-Sn, Li-Pb, Li-Bi, Li-Ga, Li-Sr, Li-Si, Li-Zn, Li-Cd, Li-Ca, and Li-Ba, as well as compounds other than those represented by the above general formula, such as MnO2, FeO2, TiO2, V2O5, and VO 13 A material having a redox potential higher than that of the negative electrode material, such as TiS2, can be used.

[0159] The lower limit of the content of the positive electrode active material in the positive electrode mixture is preferably 10% by mass, more preferably 15% by mass. The upper limit of the content of the positive electrode active material is preferably 60% by mass, more preferably 70% by mass, even more preferably 80% by mass, particularly preferably 90% by mass, and may even be 95% by mass. By setting the content of the positive electrode active material within the above range, the electrical capacity of the all-solid-state battery can be increased.

[0160] <Positive Electrode Mixture or Positive Electrode Composite> As in the case of the negative electrode, the positive electrode mixture is a mixture prepared by mixing a positive electrode active material, a solid electrolyte, etc. by mechanical milling, etc. For example, the mixture of a positive electrode active material and a solid electrolyte, etc. can be obtained by mixing a particulate positive electrode active material and a particulate solid electrolyte, etc. As in the case of the negative electrode, the positive electrode composite may be a composite having a chemical or physical bond between the positive electrode active material and the solid electrolyte, etc., or a composite obtained by mechanically combining the positive electrode active material and the solid electrolyte, etc. The composite is one in which the positive electrode active material and the solid electrolyte, etc. are present within a single particle, and examples thereof include a composite in which the positive electrode active material and the solid electrolyte, etc. are in an aggregated state, and a composite in which a coating containing the solid electrolyte, etc. is formed on at least a portion of the surface of the positive electrode active material. The positive electrode mixture or positive electrode composite may contain a solid electrolyte other than the sulfide solid electrolyte. The positive electrode active material, solid electrolyte, and the like contained in the positive electrode mixture constitute a positive electrode mixture or a positive electrode composite, which can improve ionic conductivity.

[0161] When the positive electrode mixture contains a solid electrolyte, the lower limit of the solid electrolyte content may be 5 mass %, preferably 10 mass %. The upper limit of the solid electrolyte content in the positive electrode mixture is preferably 90 mass %, more preferably 85 mass %, even more preferably 80 mass %, and particularly preferably 75 mass %. By setting the solid electrolyte content within the above range, the electrical capacity of the all-solid-state battery can be increased.

[0162] The lower limit of the average thickness of the positive electrode mixture layer 6 is preferably 30 μm, more preferably 60 μm. The upper limit of the average thickness of the positive electrode mixture layer 6 is preferably 1000 μm, more preferably 500 μm, and even more preferably 200 μm. By setting the average thickness of the positive electrode mixture layer 6 to be equal to or greater than the above lower limit, an all-solid-state battery having a high energy density can be obtained. By setting the average thickness of the positive electrode mixture layer 6 to be equal to or less than the above upper limit, an all-solid-state battery having excellent high-rate discharge performance and a negative electrode with a high active material utilization rate can be obtained.

[0163] [Solid electrolyte layer] The solid electrolyte layer 3 contains an electrolyte for the solid electrolyte layer. In addition to the sulfide solid electrolyte described above, examples of the electrolyte for the solid electrolyte layer include oxide-based solid electrolytes, other sulfide solid electrolytes, dry polymer electrolytes, gel polymer electrolytes, and pseudo-solid electrolytes. Among these, sulfide solid electrolytes are preferred, and sulfide solid electrolytes are more preferred, from the viewpoints of good ionic conductivity and ease of interface formation. When the solid electrolyte layer 3 contains the sulfide solid electrolyte, the solid electrolyte layer can exhibit high ionic conductivity, thereby reducing the internal resistance of the all-solid-state battery.

[0164] The content of the sulfide solid electrolyte relative to the total amount of solid electrolyte contained in the all-solid-state battery is preferably 50% by mass to 100% by mass, more preferably 70% by mass to 100% by mass, even more preferably 80% by mass to 100% by mass, and even more preferably 90% by mass to 100% by mass. In particular, it is preferable that the solid electrolyte contained in the all-solid-state battery is composed solely of the sulfide solid electrolyte. In particular, since the sulfide solid electrolyte containing the element X has high thermal stability, by configuring the all-solid-state battery as described above, it is possible to fully enjoy the advantage of the all-solid-state battery, which is that the upper limit of the operating temperature of the battery can be increased.

[0165] The electrolyte for the solid electrolyte layer may have a crystalline structure or may be amorphous without a crystalline structure. The electrolyte for the solid electrolyte layer may contain an oxide such as Li3PO4, a halogen, a halogen compound, or the like.

[0166] The average thickness of the solid electrolyte layer 3 is preferably 1 μm or more and 50 μm or less, and more preferably 3 μm or more and 20 μm or less. By setting the average thickness of the solid electrolyte layer 3 within the above range, it becomes possible to increase the energy density of the all-solid-state battery while reliably insulating the positive electrode and the negative electrode.

[0167] <Manufacturing method for all-solid-state batteries> The manufacturing method of the all-solid-state battery mainly includes, for example, a sulfide solid electrolyte preparation step, a negative electrode mixture preparation step, a solid electrolyte layer preparation step, a positive electrode mixture preparation step, and a lamination step of laminating the negative electrode layer, the solid electrolyte layer, and the positive electrode layer.

[0168] (Sulfide solid electrolyte manufacturing process) In this step, for example, a sulfide solid electrolyte is produced by the method for producing a sulfide solid electrolyte.

[0169] (Negative electrode mixture production process) In this step, an anode mixture for forming the anode layer is prepared. When the anode mixture contains a mixture or composite including an anode active material and the sulfide solid electrolyte, this step includes mixing the anode active material and the sulfide solid electrolyte by, for example, mechanical milling to prepare a mixture or composite of the anode active material and the sulfide solid electrolyte.

[0170] (Electrolyte manufacturing process for solid electrolyte layer) In this step, the above-mentioned solid electrolyte layer electrolyte for forming the solid electrolyte layer is prepared. In this step, the predetermined material for the solid electrolyte layer electrolyte can be obtained by processing the predetermined material for the solid electrolyte layer electrolyte by a mechanical milling method. The predetermined material for the solid electrolyte layer electrolyte may be prepared by a melt quenching method, where the predetermined material for the solid electrolyte layer electrolyte is heated to above its melting temperature, melt-mixed in a predetermined ratio, and then quenched. Other methods for synthesizing the solid electrolyte layer electrolyte include, for example, a solid-phase method in which the solid electrolyte layer electrolyte is sintered under reduced pressure, a liquid-phase method such as solution deposition, a vapor-phase method (PLD), and mechanical milling followed by sintering in an argon atmosphere. Note that when the solid electrolyte layer electrolyte is a sulfide solid electrolyte, the above-mentioned sulfide solid electrolyte preparation step is performed in the preparation step for the solid electrolyte layer electrolyte.

[0171] (Positive electrode mixture production process) In this step, a cathode mixture for forming a cathode layer is prepared. The method for preparing the cathode mixture is not particularly limited and can be appropriately selected depending on the purpose. Examples include compression molding of a cathode active material, mechanical milling of a predetermined material for the cathode mixture, and sputtering using a target material for the cathode active material. When the cathode mixture contains a mixture or composite containing a cathode active material and the sulfide solid electrolyte, this step includes mixing the cathode active material and the sulfide solid electrolyte using, for example, mechanical milling to prepare a mixture or composite of the cathode active material and the sulfide solid electrolyte.

[0172] (Lamination process) In this step, an anode layer having an anode substrate layer and an anode mixture layer, a solid electrolyte layer, and a cathode layer having a cathode substrate layer and a cathode mixture layer are laminated. In this step, the anode layer, the solid electrolyte layer, and the cathode layer may be formed sequentially or in reverse, and the order of forming the layers is not particularly important. The anode layer is formed by pressure molding the anode substrate and the anode mixture, the solid electrolyte layer is formed by pressure molding an electrolyte for the solid electrolyte layer, and the positive electrode layer is formed by pressure molding the positive electrode substrate and the cathode mixture.

[0173] The anode layer, the solid electrolyte layer, and the positive electrode layer may be laminated by simultaneously pressure-molding the anode substrate, the anode mixture, the electrolyte for the solid electrolyte layer, the cathode substrate, and the positive electrode mixture. The positive electrode layer, the anode layer, or these layers may be molded in advance, and then pressure-molded together with the solid electrolyte layer to laminate them.

[0174] <Other embodiments> The present invention is not limited to the above-described embodiment, and can be implemented in various other forms, including those described above, with various modifications and improvements.

[0175] In the above embodiment, the source compound containing N, element A, and element M is described as containing only N, Li, and element M. However, the present invention is not limited to this. For example, the source compound containing N, element A, and element M may further contain other elements as long as it does not interfere with solving the problems of the present invention.

[0176] The configuration of the all-solid-state battery according to the present invention is not particularly limited, and may include layers other than the negative electrode layer, the positive electrode layer, and the solid electrolyte layer, such as an intermediate layer or an adhesive layer. [Example]

[0177] The present invention will be explained in more detail below by means of demonstration experiments, but the present invention is not limited to the following examples.

[0178] First, Example 1, Example 2, Comparative Example 1, Comparative Example 2, and Comparative Example 3 show the effect of the method for producing a sulfide solid electrolyte according to one embodiment of the present invention in suppressing the emission of N to the outside of the system. [Example 1] By the following process, 80(0.70Li2S·0.30P2S5)·20Li 3 / 2 Al 1 / 2 N was synthesized. (preparation process) LiN and AlN were weighed out to a molar ratio of 1.2:1, mixed in a mortar, and then pelletized. Then, the mixture was heat-treated at 750°C for 1 hour to obtain LiN. 3 / 2 Al 1 / 2 N was prepared. 3 / 2 Al 1 / 2 XRD measurement revealed that the main phase of N is Li. 3 / 2 Al 1 / 2 It was confirmed that N. Next, Li2S (99.98%, Aldrich), P2S5 (99%, Aldrich), and Li 3 / 2 Al 1 / 2 After weighing out N so that the molar ratio was 56:24:20, the components were mixed in a mortar to prepare a composition containing Li, P, S, N, and Al. (Reaction step) The composition was placed in a sealed 80 mL zirconia pot containing 160 g of 4 mm diameter zirconia balls, and milled for 45 hours at a revolution speed of 510 rpm using a planetary ball mill (FRITSCH, Model No. Premium Line P-7) to obtain an intermediate. (Heat treatment process) The intermediate was heat-treated for 2 hours to obtain a sulfide solid electrolyte. This heat treatment was carried out at a temperature equal to or higher than the crystallization temperature but not higher than 100°C above the crystallization temperature. The crystallization temperature was determined by DSC measurement. The DSC measurement was carried out under the following conditions: a DSC device (Rigaku Thermo Plus DSC8230) was used, and a sealed SUS pan was used, and the temperature was increased from room temperature to 400°C at a rate of 10°C / min. The composition prepared by the above synthesis procedure was designated as sample a, the intermediate as sample b, and the sulfide solid electrolyte as sample c.

[0179] [Example 2] 80(0.70Li2S 0.30P2S5) 20Li was prepared in the same manner as in Example 1, except for the following changes in the preparation process: 3 / 2 B 1 / 2 N was synthesized. (preparation process) LiN and BN were weighed in a molar ratio of 1.1:1, mixed in a mortar, and then pelletized. Then, the mixture was heat-treated at 800°C for 10 minutes to obtain LiN. 3 / 2 B 1 / 2 N was prepared. 3 / 2 B 1 / 2 XRD measurement revealed that the main phase of N is Li. 3 / 2 B 1 / 2 It was confirmed that N. Next, Li2S (99.98%, Aldrich), P2S5 (99%, Aldrich), and Li 3 / 2 B 1 / 2 The components were weighed out so that the molar ratio of Li, P, S, N, and B was 56:24:20, and then mixed in a mortar to prepare a composition containing Li, P, S, N, and B.

[0180] [Comparative Example 1] 56.8Li2S·27.0P2S5·16.2Li3N was synthesized in the same manner as in Example 1, except that the preparation process was changed as follows. (preparation process) Li2S (99.98%, Aldrich), P2S5 (99%, Aldrich), and Li3N were weighed in a molar ratio of 56.8:27.0:16.2 in a glove box with an argon atmosphere and a dew point of −50°C or less, and then mixed in a mortar to prepare a composition containing Li, P, S, and N.

[0181] Comparative Example 2 80(0.70Li2S 0.30P2S5) 20Li was prepared in the same manner as in Example 1, except for the following changes in the preparation process: 3 / 2 Al 1 / 2 N was synthesized. (preparation process) In a glove box with an argon atmosphere and a dew point of −50°C or less, Li2S (99.98%, Aldrich), P2S5 (99%, Aldrich), Li3N, and AlN were weighed out to a molar ratio of 56:24:10:10 and mixed in a mortar to prepare a composition containing Li, P, S, N, and Al.

[0182] Comparative Example 3 80(0.70Li2S 0.30P2S5) 20Li was prepared in the same manner as in Example 1, except for the following changes in the preparation process: 7 / 4 V 1 / 4 N was synthesized. (preparation process) LiN and VN were weighed in a molar ratio of 3:1, mixed in a mortar, and then pelletized. Then, the mixture was heat-treated at 750°C for 10 hours to obtain Li 7 / 4 V 1 / 4 N was prepared. 7 / 4 V 1 / 4 XRD measurement revealed that the main phase of N is Li. 7 / 4 V 1 / 4 It was confirmed that N. Next, Li2S (99.98%, Aldrich), P2S5 (99%, Aldrich), and Li 7 / 4 V 1 / 4 The components were weighed out so that the molar ratio of Li, P, S, N, and V was 56:24:20, and then mixed in a mortar to prepare a composition containing Li, P, S, N, and V.

[0183] [evaluation] (1) XRD X-ray diffraction measurements were performed using the following method. An airtight sample holder for X-ray diffraction measurements was filled with the sulfide solid electrolyte powders of the examples and comparative examples in an argon atmosphere with a dew point of -50°C or lower. Powder X-ray diffraction measurements were performed using an X-ray diffractometer ("miniFlex II" manufactured by Rigaku). The radiation source was CuKα radiation, the tube voltage was 30 kV, and the tube current was 15 mA. Diffracted X-rays were passed through a 30 μm-thick Kβ filter and detected with a high-speed one-dimensional detector (model number: D / teX Ultra2). The sampling width was 0.01°, the scan speed was 5° / min, the divergence slit width was 0.625°, the receiving slit width was 13 mm (open), and the scattering slit width was 8 mm.

[0184] (2) Ionic conductivity (σ) Ionic conductivity (σ 25 The ionic conductivity at 25°C was determined by measuring AC impedance using a Bio-Logic VMP-300 in the manner described above. For some examples and comparative examples, the ionic conductivity was also measured at temperatures of -30°C, -20°C, -10°C, 0°C, and 50°C, and the activation energy (E a ) was calculated.

[0185] Table 4 shows the XRD patterns and ionic conductivities (σ) at 25°C for Example 1, Example 2, Comparative Example 1, Comparative Example 2, and Comparative Example 3. 25) is shown. As shown in Table 4, peaks were observed in the XRD spectrum of the sulfide solid electrolytes of all Examples and Comparative Examples, and it was confirmed that they had specific crystalline structure A. Note that specific crystalline structure A is a crystalline structure having diffraction peaks at 2θ = 17.9° ± 0.5°, 19.1° ± 0.5°, 29.1° ± 0.5°, 29.8° ± 0.5°, and 30.9° ± 0.5° in X-ray diffraction measurement. It was also confirmed that the sulfide solid electrolytes of Example 1, Example 2, and Comparative Example 3 exhibited similar ionic conductivities. Therefore, it can be said that Example 1, Example 2, Comparative Example 1, Comparative Example 2, and Comparative Example 3 have similar structures.

[0186] [Table 4]

[0187] For each sample of Example 1, Example 2, Comparative Example 1, and Comparative Example 2, the contents of Li, B, Al, and P in the sample were determined using an ICP atomic emission spectrometer. Furthermore, for each sample of Example 1, Example 2, and Comparative Examples 1 to 3, the content of N in the sample was determined using an oxygen / nitrogen / hydrogen analyzer. From the analysis results, the rate of change in the N content in the sample was calculated. Table 5 shows the analysis results. In the table, "no change" indicates that the rate of change in the N content relative to sample a was ±5% by mass or less.

[0188] [Table 5]

[0189] Table 5 shows that there is almost no change in the N content ratios of Sample a, Sample b, and Sample c in Examples 1 and 2. That is, in Examples 1 and 2, there is almost no change in the N content ratios even after going through the reaction step and the heat treatment step, and it is understood that the release of N to the outside of the system was suppressed. On the other hand, in Comparative Examples 1, 2, and 3, it can be seen that the N content in Sample a, Sample b, and Sample c decreases in the order of Sample a, Sample b, and Sample c. In other words, it can be seen that in Comparative Examples 1, 2, and 3, the N content decreases with each step of the reaction step and heat treatment step, and N is discharged outside the system. From the above, it was demonstrated that Al and B, which were selected based on the prediction of their N emission suppression effect using first-principles calculations, actually have an effect. Furthermore, it was also demonstrated that V, which was predicted using first-principles calculations to have no effect on N emission suppression, actually does not have an effect.

[0190] Next, Examples 3 to 20 and Comparative Examples 4 to 8 will demonstrate the effect of improving the thermal stability of the sulfide solid electrolyte according to one embodiment of the present invention. [Example 3] The following treatment yielded the compound with the formula 85(0.80(0.70Li2S 0.30P2S5) 0.20Li 3 / 2 Al 1 / 2 A sulfide solid electrolyte represented by the formula (N)·10LiBr·5LiI was synthesized. LiN and AlN were weighed out to a molar ratio of 1.2:1, mixed in a mortar, and then pelletized. Then, the mixture was heat-treated at 750°C for 1 hour to obtain LiN. 3 / 2 Al 1 / 2 N was prepared. 3 / 2 Al 1 / 2 XRD measurement revealed that the main phase of N is Li. 3 / 2 Al 1 / 2 It was confirmed that N. Next, Li2S (99.98%, Aldrich), P2S5 (99%, Aldrich), LiBr (99.999%, Aldrich), LiI (99.999%, Aldrich), and Li were dissolved in an argon atmosphere in a glove box with a dew point of -50 °C or less. 3 / 2 Al 1 / 2The sulfide solid electrolyte of Example 3 was obtained by weighing out N to a molar ratio of 47.6:20.4:10:5:17 and then mixing them in a mortar. This mixed sample was placed in a sealed 80 mL zirconia pot containing 160 g of zirconia balls with a diameter of 4 mm. A planetary ball mill (FRITSCH, Model No. Premium Line P-7) was used for milling at a revolution speed of 510 rpm for 45 hours. Heat treatment at 245°C for 2 hours yielded the sulfide solid electrolyte of Example 3. The heat treatment temperature was set to be equal to or higher than the crystallization temperature but not higher than 100°C above the crystallization temperature. The crystallization temperature was determined by taking a portion of the milled sample and subjecting it to DSC measurement. The DSC measurement was performed under the following conditions: A DSC apparatus (Rigaku, Thermo Plus DSC8230) was used, and a stainless steel sealed pan was used, and the temperature was increased from room temperature to 400°C at a rate of 10°C / min.

[0191] [Comparative Examples 4 and 5] The sulfide solid electrolytes of Comparative Examples 4 and 5 were synthesized in the same manner as in Example 3, except that the composition of the sulfide solid electrolyte was changed to 85(0.75LiS 0.25P2S5) 10LiBr 5LiI and 85(0.72Li2S 0.25P2S5 0.020Li3N) 10LiBr 5LiI, and the heat treatment temperature was set to 225°C in both cases.

[0192] [Examples 4 to 7, Comparative Example 6] The composition of the sulfide solid electrolyte was 80(0.80(0.70Li2S 0.30P2S5) 0.20Li 3 / 2 Al 1 / 2 N)·12LiBr·8LiI, 80(0.70(0.67Li2S·0.33P2S5)·0.30Li 3 / 2 Al 1 / 2 N)·12LiBr·8LiI, 80(0.80(0.70Li2S·0.30P2S5)·0.20Li 3 / 2 B 1 / 2 N)·12LiBr·8LiI, 80(0.80(0.70Li2S·0.30P2S5)·0.20Li 5 / 3 Si 1 / 3The sulfide solid electrolytes of Examples 4 to 7 and Comparative Example 6 were synthesized in the same manner as in Example 3, except that the catalyst used was changed to 80(0.6975LiS 0.25P2S 0.035LiN)·12LiBr 8LiI, and 80(0.6975LiS 0.25P2S 0.035LiN)·12LiBr 8LiI, and the heat treatment temperatures were changed to 255°C, 275°C, 270°C, 270°C, and 250°C, respectively. In addition to the sulfide solid electrolyte of Example 4, samples were synthesized at heat treatment temperatures of 215°C, 230°C, 275°C, 290°C, and 310°C, in addition to the sample heat-treated at 255°C. In addition to the sulfide solid electrolyte of Example 5, samples were synthesized at heat treatment temperatures of 235°C, 290°C, 310°C, and 330°C, in addition to the sample heat-treated at 275°C. In addition to the sulfide solid electrolyte of Example 6, samples were synthesized at heat treatment temperatures of 230°C, 270°C, 290°C, 310°C, and 330°C, in addition to the sample heat-treated at 270°C. In addition to the sulfide solid electrolyte of Example 7, samples were synthesized at heat treatment temperatures of 230°C, 290°C, 310°C, and 330°C. In addition to the sulfide solid electrolyte of Comparative Example 6, samples heat-treated at 250°C were also synthesized, with samples heat-treated at 210°C and 230°C. The sulfide solid electrolytes synthesized at each heat treatment temperature are named, in order of decreasing heat treatment temperature, as Examples 4-1 to 4-6, 5-1 to 5-5, 6-1 to 6-5, 7-1 to 7-5, and Comparative Examples 6-1 to 6-3, respectively.

[0193] [Example 8, Comparative Example 7] The composition of the sulfide solid electrolyte was 75(0.80(0.70Li2S 0.30P2S5) 0.20Li 3 / 2 Al 1 / 2 The sulfide solid electrolytes of Example 8 and Comparative Example 7 were synthesized in the same manner as in Example 1, except that the catalyst used was changed to 75(0.72LiS 0.25P2S 0.020LiN)·15LiBr·10LiI and 75(0.72LiS 0.25P2S 0.020LiN)·15LiBr·10LiI, and the heat treatment temperatures were changed to 215°C and 195°C, respectively.

[0194] [Examples 9 to 11, Comparative Example 8] The composition of the sulfide solid electrolyte was 90(0.80(0.70Li2S 0.30P2S5) 0.20Li 3 / 2 Al 1 / 2 N)·10LiBr, 80(0.80(0.70Li2S·0.30P2S5)·0.20Li 3 / 2 Al 1 / 2 N)·20LiBr, 70(0.80(0.70Li2S·0.30P2S5)·0.20Li 3 / 2 Al 1 / 2 The sulfide solid electrolytes of Examples 9, 10, and 11 and Comparative Example 8 were synthesized in the same manner as in Example 3, except that the composition of the sulfide solid electrolyte was changed to 90(0.72LiS 0.25P2S 0.020LiN)·30LiBr and 90(0.72LiS 0.25P2S 0.020LiN)·10LiBr and the heat treatment temperatures were changed to 265°C, 250°C, 240°C, and 225°C, respectively.

[0195] [Examples 12 and 13] The composition of the sulfide solid electrolyte was 90(0.80(0.70Li2S 0.30P2S5) 0.20Li 3 / 2 Al 1 / 2 N)·10LiI, 80(0.80(0.7Li2S·0.30P2S5)·0.20Li 3 / 2 Al 1 / 2 The sulfide solid electrolytes of Examples 12 and 13 were synthesized in the same manner as in Example 3, except that the catalyst was changed to (N)·20LiI and the heat treatment temperatures were changed to 255°C and 240°C, respectively.

[0196] [Examples 14 to 17] The composition of the sulfide solid electrolyte was 80(0.97(0.745Li2S 0.255P2S5) 0.03Li 3 / 2 B 1 / 2 N)·12LiBr·8LiI, 80(0.95(0.74Li2S·0.26P2S5)·0.05Li 3 / 2 B 1 / 2 N)·12LiBr·8LiI, 80(0.90(0.73Li2S·0.27P2S5)·0.10Li 3 / 2 B 1 / 2 N)·12LiBr·8LiI, 80(0.85(0.715Li2S·0.285P2S5)·0.15Li 3 / 2 B1 / 2 The sulfide solid electrolytes of Examples 14 to 17 were synthesized in the same manner as in Example 3, except that the catalyst was changed to (N)·12LiBr·8LiI and the heat treatment temperature was changed to 250°C.

[0197] [Examples 18 to 20] The composition of the sulfide solid electrolyte was 75(0.80(0.70Li2S 0.30P2S5) 0.20Li 3 / 2 B 1 / 2 N)·15LiBr·10LiI, 70(0.80(0.70Li2S·0.30P2S5)·0.20Li 3 / 2 B 1 / 2 N)·17LiBr·13LiI, 65(0.80(0.70Li2S·0.30P2S5)·0.20Li 3 / 2 B 1 / 2 The sulfide solid electrolytes of Examples 18 to 20 were synthesized in the same manner as in Example 3, except that the catalyst used was changed to (N)·20LiBr·15LiI and the heat treatment temperatures were changed to 230°C, 195°C, and 185°C, respectively.

[0198] The sulfide solid electrolytes of Examples 3 to 20 were prepared using a sulfide-based solid electrolyte having a general formula (100-z1-z2){(1-y)[xLi2S·(1-x)P2S5]·yLi α M β The sulfide solid electrolytes of Comparative Examples 5 to 7 are represented by the general formula (100-z1-z2){(x-1.5y)Li2S (1-x)P2S5 yLi3N} z1LiX1 z2LiX2.

[0199] Tables 6 to 12 show the crystal structures identified from the XRD patterns of Examples 3 to 20 and Comparative Examples 4 to 8. Table 13 shows the crystal structures identified from the XRD patterns of Examples 4-1 to 4-6, Examples 5-1 to 5-5, Examples 6-1 to 6-5, Examples 7-1 to 7-5, and Comparative Examples 6-1 to 6-3. In the table, "HICP" represents a crystalline phase having diffraction peaks at 2θ = 20.2° ± 0.5° and 23.6° ± 0.5° in X-ray diffraction measurement using CuKα radiation. "LICP" represents a crystalline phase having diffraction peaks at 2θ = 21.0° ± 0.5° and 28.0° ± 0.5° in X-ray diffraction measurement using CuKα radiation. "Specific crystalline structure C" represents a crystalline phase having diffraction peaks at 2θ = 17.5° ± 0.5° and 24.9° ± 0.5° in X-ray diffraction measurement using CuKα radiation. "β-Li3PS4" represents a crystalline phase having diffraction peaks at 2θ = 17.5° ± 0.5°, 18.1° ± 0.5°, 29.1° ± 0.5°, 29.9° ± 0.5°, and 31.2° ± 0.5° in X-ray diffraction measurement using CuKα radiation. "Unknown" indicates a peak whose crystal phase is unknown. 3 shows the XRD patterns of Examples 4-1 to 4-6, and FIG. 4 shows the XRD patterns of Comparative Examples 6-1 to 6-3.

[0200] Tables 6 to 12 show the ionic conductivities (σ) at 25° C. for Examples 3 to 20 and Comparative Examples 4 to 8. 25 ) and activation energy (E a Table 13 shows the ionic conductivities (σ) at 25° C. of Examples 4-1 to 4-6, Examples 5-1 to 5-5, Examples 6-1 to 6-5, Examples 7-1 to 7-5, and Comparative Examples 6-1 to 6-3. 25 ) and activation energy (E a ) is shown.

[0201] (3) DSC DSC measurements were carried out as follows: Using a DSC device (Rigaku Thermo Plus DSC8230), a sealed SUS pan was used, and the temperature was increased from room temperature to 400°C at a rate of 10°C / min.

[0202] The intermediates after milling and before heat treatment were subjected to DSC measurement for the sulfide solid electrolytes of Examples 4 to 7, Examples 14 to 17, and Comparative Example 6. DSC curves for these samples are shown in Figures 5 and 6.

[0203] Table 6

[0204] Table 7

[0205] Table 8

[0206] Table 9

[0207] Table 10

[0208] Table 11

[0209] Table 12

[0210] Table 13

[0211] Table 6 shows that in the sulfide solid electrolytes of Comparative Examples 4 and 5, LICPs are generated when the heat treatment temperature is set to 225°C, and the ionic conductivity at 25°C is reduced. On the other hand, the sulfide solid electrolyte of Example 3, which contains Li, P, S, N, Br, I, and Al, does not generate LICPs and exhibits high ionic conductivity, despite being heat-treated at a higher temperature than the sulfide solid electrolytes of Comparative Examples 4 and 5. In other words, it can be seen that the lower limit of the heat treatment temperature at which the ionic conductivity decreases is higher in the sulfide solid electrolyte of Example 3 than in the sulfide solid electrolytes of Comparative Examples 4 and 5.

[0212] Table 7 shows that the sulfide solid electrolytes of Examples 4 to 7 exhibit high ionic conductivity without producing LICPs, despite being heat-treated at a higher temperature than the sulfide solid electrolyte of Comparative Example 6. In other words, it can be seen that the sulfide solid electrolytes of Examples 4 to 7 have a higher lower limit of the heat treatment temperature at which the ionic conductivity decreases than the sulfide solid electrolyte of Comparative Example 6.

[0213] Table 8 shows that the sulfide solid electrolyte of Example 8 exhibits higher ionic conductivity despite being heat-treated at a higher temperature than the sulfide solid electrolyte of Comparative Example 7. In other words, it can be seen that the sulfide solid electrolyte of Example 8 has a higher lower limit of the heat treatment temperature at which the ionic conductivity decreases than the sulfide solid electrolyte of Comparative Example 7. This is thought to be because the phase transition from HICP to LICP is suppressed in the sulfide solid electrolyte of Example 8.

[0214] It can be seen from Table 9 that the sulfide solid electrolytes of Examples 9 to 11 all exhibit higher ionic conductivities than the sulfide solid electrolyte of Comparative Example 8, despite being heat-treated at higher temperatures. It can also be seen that the effect of the present invention, which is to improve the thermal stability of the high Li-ion conductive phase of the sulfide solid electrolyte, can be obtained even when the sulfide solid electrolyte contains only Br as the element X. Furthermore, comparing Example 9 and Comparative Example 8, which have the same Br content, it can be seen that neither HICPs nor LICPs were produced in Comparative Example 8, whereas HICPs were produced in Example 9. In other words, when the sulfide solid electrolyte contains Li, P, S, N, the element X, and the element M, it was found that HICPs could be produced with a smaller content of the element X than when the element M was not contained.

[0215] Table 10 shows that even when the sulfide solid electrolyte contains only I as the element X, a sulfide solid electrolyte containing HICP can be obtained.

[0216] Table 11 shows that the sulfide solid electrolytes of Examples 6 and 15 to 17 exhibited the presence of HICPs and high ionic conductivity despite being heat-treated at a temperature higher than that of the sulfide solid electrolyte of Comparative Example 6. In other words, it can be seen that the sulfide solid electrolytes of these Examples have a higher lower limit of the heat treatment temperature at which the ionic conductivity decreases than the sulfide solid electrolyte of Comparative Example 6. 6 also shows that the sulfide solid electrolytes of Examples 6 and 14 to 17 have a larger temperature difference between the crystallization peak presumed to be derived from HICP and the crystallization peak presumed to be derived from β-Li3PS4, compared to the sulfide solid electrolyte of Comparative Example 6. For example, in Comparative Example 6, the crystallization peak presumed to be derived from HICP and the crystallization peak presumed to be derived from β-Li3PS4 were observed near 190°C and 260°C, respectively, whereas in Example 14, they were observed near 190°C and 280°C, respectively. This shows that the sulfide solid electrolytes of the Examples have a wider temperature range in which HICP stably exists, improving the thermal stability of the high Li-ion conductive phase. 6, the crystallization peaks presumed to be derived from HICP indicate peaks observed in the range of approximately 180° C. to 220° C. The crystallization peaks derived from β-Li3PS4 in FIG. 6 indicate peaks observed around 345° C., 280° C., 300° C., 310° C., 335° C., and 260° C. in Example 6, Examples 14 to 16, and Comparative Example 6, respectively. From the above, it can be seen that the effect of improving the thermal stability of the high Li-ion conductive phase can be obtained even when the content ratio N / P of N to P of the sulfide solid electrolyte is 0.060, 0.10, 0.21, 0.31, or 0.42.

[0217] Table 12 shows that a sulfide solid electrolyte containing HICP can be obtained even when the content ratio X / P of the element X to P in the sulfide solid electrolyte is 0.52, 0.70, 0.90, or 1.12.

[0218] From Comparative Examples 6-1 to 6-3 shown in Table 13, it can be seen that the sulfide solid electrolyte of Comparative Example 6 undergoes a phase transition from HICP to LICP and β-Li3PS4 when the heat treatment temperature is 250°C or higher. It can also be seen that this causes a significant decrease in ionic conductivity at 25°C. On the other hand, it is clear from Examples 4-1 to 4-6 that in the sulfide solid electrolyte of Example 4, HICPs exist even when the heat treatment temperature is increased to 290° C., and high ionic conductivity can be maintained. Moreover, it is clear from Examples 5-1 to 5-5 that the sulfide solid electrolyte of Example 5 also has HICPs over a wide temperature range and can maintain high ionic conductivity. Furthermore, from Examples 6-1 to 6-5 and Examples 7-1 to 7-5, it can be seen that even when B and Si are contained instead of Al as the element M, the effect of the present invention of maintaining high ionic conductivity over a wide temperature range can be obtained. That is, it can be seen from Table 13 that the sulfide solid electrolytes of Examples 4 to 7 have a wider heat treatment temperature range in which ionic conductivity does not decrease. Furthermore, a comparison of Examples 6 and 7 with Examples 4 and 5 in Table 13 reveals that when the sulfide solid electrolyte contains either Si or B as the element M, the heat treatment temperature range in which ionic conductivity does not decrease extends over at least a range of 80°C, demonstrating particularly excellent thermal stability of the high Li-ion conductive phase. The peaks near 210°C in the DSC curves of Examples 6 and 7 in FIG. 5 are crystallization peaks presumably derived from HICP. Therefore, it can be inferred that in Examples 6 and 7, the heat treatment temperature range in which ionic conductivity does not decrease extends over a range of 100°C. While the reason for these results is unclear, it is thought that, for example, the strength of the bond energy between either Si or B and N was a value suitable for achieving the effects of the present invention.

[0219] As is clear from Tables 6 to 13, it was confirmed that the sulfide solid electrolytes of the examples had a higher lower limit of the heat treatment temperature at which ionic conductivity decreased, and a wider heat treatment temperature range over which ionic conductivity did not decrease. In other words, the sulfide solid electrolytes containing Li, P, S, N, element X, and element M had excellent thermal stability of HICP. This is thought to be because the release of N to the outside of the system during the production process was suppressed, and the thermal stability-improving effect of N contained in the sulfide solid electrolyte was fully exerted.

[0220] It has been suggested that the method for producing a sulfide solid electrolyte according to one embodiment of the present invention can suppress not only the discharge of N out of the system but also the precipitation of Li2S. Suppressing the precipitation of Li2S is preferable because it improves the atmospheric stability of the sulfide solid electrolyte.

[0221] That is, Examples 21 to 41, Comparative Examples 9 and 10 suggest that the method for producing a sulfide solid electrolyte according to one embodiment of the present invention can suppress the precipitation of Li2S.

[0222] [Example 21] By the following treatment, the composition formula (100-z)(yLi2S·(1-y)P2S5)·zLi α M βLi in N α M β N is Li 3 / 2 Al 1 / 2 N, z = 1, y = 0.70, i.e., 99(0.7Li2S 0.3P2S5) 1Li 3 / 2 Al 1 / 2 N was synthesized. LiN and AlN were weighed out to a molar ratio of 1.2:1, mixed in a mortar, and then pelletized. Then, the mixture was heat-treated at 750°C for 1 hour to obtain LiN. 3 / 2 Al 1 / 2 N was produced. Next, Li2S (99.98%, Aldrich), P2S5 (99%, Aldrich), and Li 3 / 2 Al 1 / 2 The sulfide solid electrolyte of Example 1 was obtained by weighing N to a molar ratio of 69.3:29.7:1.0 and then mixing them in a mortar. This mixed sample was placed in a sealed 80 mL zirconia pot containing 160 g of zirconia balls with a diameter of 4 mm. A planetary ball mill (FRITSCH, model number Premium line P-7) was used for milling at a revolution speed of 510 rpm for 45 hours. Heat treatment was performed for 2 hours at a temperature equal to or higher than the crystallization temperature but not higher than 100°C above the crystallization temperature. The crystallization temperature was determined by DSC measurement. The DSC measurement was performed under the following conditions: A DSC apparatus (Rigaku, Thermo Plus DSC8230) was used, and a sealed SUS pan was used, and the temperature was increased from room temperature to 400°C at a rate of 10°C / min.

[0223] [Examples 22 to 29] The composition formula of sulfide solid electrolyte is (100-z)(yLi2S·(1-y)P2S5)·zLi α M β The sulfide solid electrolytes of Examples 22 to 29 were synthesized in the same manner as in Example 21, except that the value of z in N was changed to 5, 7, 10, 15, 20, 25, 30, or 40.

[0224] [Examples 30 to 32] The composition formula of sulfide solid electrolyte is (100-z)(yLi2S·(1-y)P2S5)·zLi α M β The sulfide solid electrolytes of Examples 30 to 32 were synthesized in the same manner as in Example 21, except that in N, y=0.67 and the value of z was changed to 20, 25, and 30, respectively.

[0225] [Examples 33 to 36] LiN and BN were weighed out to a molar ratio of 1.1:1, mixed in a mortar, pelletized, and then heat-treated at 800°C for 10 minutes to obtain Li 3 / 2 B 1 / 2 N was prepared. 3 / 2 B 1 / 2 Regarding N, XRD measurement revealed that the main phase was Li 3 / 2 B 1 / 2 It was confirmed that N. The composition formula of sulfide solid electrolyte is (100-z)(yLi2S·(1-y)P2S5)·zLi α M β Li in N α M β N to Li 3 / 2 B 1 / 2 The sulfide solid electrolytes of Examples 33 to 36 were synthesized in the same manner as in Example 21, except that N was changed to 0, and the value of z was changed to 1, 10, 20, or 30.

[0226] [Examples 37 to 41] Li3N and Si3N4 were weighed out to a molar ratio of 5.1:1, mixed in a mortar, pelletized, and then heat-treated at 800°C for 10 minutes to obtain Li 5 / 3 Si 1 / 3 N was produced. The Li 5 / 3 Si 1 / 3 Regarding N, XRD measurement revealed that the main phase was Li5 / 3Si 1 / 3 It was confirmed that N. The composition formula of sulfide solid electrolyte is (100-z)(yLi2S·(1-y)P2S5)·zLi α M β Li in N α M β N to Li5 / 3 Si 1 / 3 The sulfide solid electrolytes of Examples 37 to 41 were synthesized in the same manner as in Example 21, except that N was changed to 0.01 and the value of z was changed to 1.5, 15, 20, 30, and 45.

[0227] Comparative Example 9 The composition formula of sulfide solid electrolyte is (100-z)(yLi2S·(1-y)P2S5)·zLi α M β Li in N α M β A sulfide solid electrolyte of Comparative Example 9 was synthesized in the same manner as in Example 21, except that N was changed to Li 3 N and the value of z was changed to 20.

[0228] [Comparative Example 10] The composition formula of sulfide solid electrolyte is (100-z)(yLi2S·(1-y)P2S5)·zLi α M β A sulfide solid electrolyte of Comparative Example 10 was synthesized in the same manner as in Comparative Example 9, except that in N, y=0.68 and the value of z was changed to 16.

[0229] [evaluation] (1) XRD, ionic conductivity (σ) X-ray diffraction measurements were carried out using the method described above. In addition, the ionic conductivity (σ 25 ) was determined by measuring AC impedance using a Bio-Logic VMP-300 according to the method described above.

[0230] (2) Raman spectroscopy The Raman spectrum was measured using a laser Raman spectrophotometer (Horiba Ltd., "LabRAM HR Revolution") at 100 cm under the conditions of an excitation laser wavelength of 532 nm (YAG laser) and a grating of 600 gr / mm. -1 From 1800cm -1 Raman spectroscopy was performed in the wavenumber range of

[0231] Table 14 shows the ionic conductivity at 25°C of Examples 21 to 41, Comparative Example 9, and Comparative Example 10, as well as the crystal structure identified from the XRD pattern and Raman spectrum. In the table, "Specific Crystal Structure A" refers to a crystalline phase having diffraction peaks at 2θ = 17.9° ± 0.5°, 19.1° ± 0.5°, 29.1° ± 0.5°, 29.8° ± 0.5°, and 30.9° ± 0.5° in X-ray diffraction measurement using CuKα radiation. "Specific Crystal Structure B" refers to a crystalline phase having diffraction peaks at 2θ = 17.9° ± 0.5°, 19.1° ± 0.5°, 29.1° ± 0.5°, and 29.8° ± 0.5° in X-ray diffraction measurement using CuKα radiation. "-" indicates that measurement was not performed.

[0232] [Table 14]

[0233] Only the peak attributable to the crystal structure of Li2S was observed in the sulfide solid electrolyte of Comparative Example 9. This result shows that when Li3N is used, Li2S is likely to precipitate. The reason for this result is unclear, but it is thought to be due to the dramatic reaction of Li3N with other raw material compounds to precipitate Li2S.

[0234] No Li2S peak was observed in Examples 21 to 35 and Examples 37 to 40. In particular, a comparison of Examples in which z = 20 and y = 0.70 (Examples 26, 35, 39, and Comparative Example 9) confirmed that the precipitation of Li2S was suppressed in the sulfide solid electrolytes of the Examples.

[0235] Furthermore, in the sulfide solid electrolytes of Examples 27 to 29, 32, 39, and 40, no Li2S peak was observed, despite the fact that the ratio of Li to P (Li / P) was higher than that of the sulfide solid electrolyte of Comparative Example 10. In particular, in Example 29, the ratio of Li to P was 4.00, which was a higher value than that of Comparative Examples 9 and 10, but no Li2S peak was observed. In the sulfide solid electrolytes of Examples 26 and 35, no Li2S peak was observed, despite the fact that the Li / P was approximately the same as that of the sulfide solid electrolyte of Comparative Example 10. The sulfide solid electrolyte of Example 32 had approximately the same value of y as Comparative Example 10, and the Li / P ratio was also the same, but no Li2S peak was observed. In sulfide solid electrolytes, when the Li content is high, LiS tends to precipitate. The above results suggest that the production method of the sulfide solid electrolyte of the example suppresses the precipitation of LiS.

[0236] That is, a comparison of Examples 28, 29, 36, 40, and 41 suggests that when Al is contained as the element M, the precipitation of Li2S is significantly suppressed.

[0237] From the above, it is suggested that the precipitation of Li2S is suppressed in the manufacturing method of the sulfide solid electrolyte of the example. The reason why the precipitation of Li2S can be suppressed by the sulfide solid electrolyte containing the element M is thought to be as follows. When Li3N is used as the starting material for the sulfide solid electrolyte containing N, Li3N and P2S5 react dramatically, releasing N2 and causing the precipitation of Li2S. This is thought to be because the defect formation energy of N in Li3N is small. In contrast, in the present invention, Li α M β Because the defect formation energy of N in N is greater than that of N in Li3N, the reaction proceeds slowly during the synthesis of the sulfide-based solid electrolyte, suppressing the release of N2 and the precipitation of Li2S.

[0238] Although the present invention has been described in detail above, the above-described embodiments are merely examples, and the invention disclosed herein includes various modifications and alterations of the above-described specific examples. [Industrial Applicability]

[0239] An all-solid-state battery including a sulfide solid electrolyte according to the present invention is suitably used as, for example, a lithium-ion all-solid-state battery for HEVs. [Explanation of symbols]

[0240] 1. Negative electrode layer 2 Positive electrode layer 3 Solid electrolyte layer 4 Negative electrode base material layer 5. Negative electrode mixture layer 6 Positive electrode mixture layer 7 Positive electrode substrate layer 10 All-solid-state battery

Claims

[Claim 1] A sulfide solid electrolyte having a crystalline structure and containing P, S, N, element A, element X, and element M as constituent elements, wherein A represents at least one element selected from the group consisting of Li, Na, and K. X represents at least one element selected from the group consisting of Cl, Br, and I. M represents at least one element selected from the group consisting of Al, Ta, Si, Sc, Mg, Nb, B, Hf, C, P, Zr, and Ti.

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