Patent Application
20230015865
The present disclosure relates to a production method for producing a halide.
International Publication No. 2018/025582 discloses a production method for producing a halide solid electrolyte.
One non-limiting and exemplary embodiment provides a production method for producing a halide with industrially high productivity.
In one general aspect, the techniques disclosed here feature a production method for producing a halide, the method containing heat-treating a mixed material containing (NH4)aYα3+a, (NH4)bSmβ3+b, Liγ, and Caδ2 in an inert gas atmosphere, wherein α, β, γ, and δ are each independently at least one selected from the group consisting of F, Cl, Br, and I, and the following three formulas: 0≤a≤3, 0≤b≤3, and 0<a+b≤6, are satisfied.
The present disclosure provides a production method for producing a halide with industrially high productivity.
Additional benefits and advantages of the disclosed embodiments will become apparent from the specification and drawings. The benefits and/or advantages may be individually obtained by the various embodiments and features of the specification and drawings, which need not all be provided in order to obtain one or more of such benefits and/or advantages.
Embodiments will be described below with reference to the drawings.
The production method according to the first embodiment includes a heat treatment step S1000. In the heat treatment step S1000, a mixed material is heat-treated in an inert gas atmosphere.
The mixed material to be heat-treated in the heat treatment step S1000 includes (NH4)aYα3+a, (NH4)bSmβ3+b, Liγ, and Caδ2, wherein α, β, γ, and δ are each independently at least one selected from the group consisting of F, Cl, Br, and I. Furthermore, the formulas: 0≤a≤3, 0≤b≤3, and 0<a+b≤6 are satisfied.
The production method according to the first embodiment is a method for producing a halide with industrially high productivity. The method with industrially high productivity is, for example, a method enabling low-cost mass production. That is, by a simple and easy production method (i.e., heat treatment in an inert gas atmosphere), a halide containing Li (i.e., lithium), Y (i.e., yttrium), Sm (i.e., samarium), and Ca (i.e., calcium) can be produced.
In the production method according to the first embodiment, it is not necessary to use a vacuum-sealed tube and a planetary ball mill.
Since “(NH4)aYα3+a” included in the mixed material can be simply and easily synthesized from inexpensive Y2O3 and NH4α, the production cost can be further reduced.
Since “(NH4)bSmβ3+b” included in the mixed material can be simply and easily synthesized from inexpensive Sm2O3 and NH4β, the production cost can be further reduced.
In order to enhance the ionic conductivity of a halide, the formulas: 0.5≤a≤3, and 0.5≤b≤3 may be satisfied.
In order to enhance the ionic conductivity of a halide, the formulas: a=3, and b=3 may be satisfied.
In order to further enhance the ionic conductivity of a halide, α, β, γ, and δ may be each independently at least one selected from the group consisting of Cl and Br.
For example, in the case where the mixed material to be heat-treated in the heat treatment step S1000 includes (NH4)3YCl6, (NH4)3SmCl6, LiCl, and CaCl2, the reaction represented by the formula (1) below is considered to proceed.
0.5(NH4)3YCl6+0.5(NH4)3SmCl6+2.8LiCl+0.1CaCl2→Li2.8Ca0.1Y0.5Sm0.5Cl6+3NH3+3HCl (1)
By the reaction represented by the formula (1), Li2.8Ca0.1Y0.5Sm0.5Cl6 is obtained.
In the heat treatment step S1000, for example, powder of the mixed material may be placed in a container (e.g., a crucible) and heat-treated in a heating furnace. In this case, the state in which the mixed material is heated to a predetermined temperature in an inert gas atmosphere may be held for more than or equal to a predetermined time. The heat treatment time may be a time period that does not cause a compositional change of a heat-treated product due to volatilization of a halide or the like. The term “not causing a compositional change of a heat-treated product” means not impairing the ionic conductivity of the heat-treated product. In the production method according to the first embodiment, for example, it is possible to produce a halide having an ionic conductivity of greater than or equal to 3.1×10−10 S/cm at around room temperature.
The inert gas atmosphere means, for example, an atmosphere in which the total concentration of gases other than the inert gas is less than or equal to 1% by volume. The inert gas is, for example, helium, nitrogen, or argon.
After the heat treatment step S1000, the heat-treated product may be pulverized. In this case, a pulverizing apparatus (e.g., a mortar or mixer) may be used.
The mixed material may be a material in which (NH4)aYα3+a, (NH4)bSmβ3+b, Liγ, and Caδ2 are mixed. That is, the mixed material may consist of (NH4)aYα3+a, (NH4)bSmβ3+b, Liγ, and Caδ2.
The mixed material may further include, in addition to (NH4)aYα3+a, (NH4)bSmβ3+b, Liγ, and Caδ2, a material different from (NH4)aYα3+a, (NH4)bSmβ3+b, Liγ, and Caδ2.
In at least one selected from the group consisting of (NH4)aYα3+a and (NH4)bSmβ3+b included in the mixed material, part of metal cations may be replaced with other metal cations. That is, part of Y and Sm may be replaced with other metal cations. Accordingly, the mixed material may further include a compound in which part of Y in (NH4)aYα3+a is replaced with other metal cations, or a compound in which part of Sm in (NH4)bSmβ3+b is replaced with other metal cations. Thus, it is possible to improve the properties (e.g., ionic conductivity) of the resulting halide. The cation substitution ratio of Y and Sm with other metal cations may be less than 50 mol %. Thus, a halide with a stabler structure can be obtained.
In at least one selected from the group consisting of Liγ and Caδ2 included in the mixed material, part of metal cations may be replaced with other metal cations. That is, part of Li and Ca may be replaced with other metal cations. Accordingly, the mixed material may further include a compound in which part of Li in Liγ is replated with other metal cations, or a compound in which part of Ca in Caδ2 is replaced with other metal cations. Thus, it is possible to improve the properties (e.g., ionic conductivity) of the resulting halide. The cation substitution ratio of Li and Ca with other metal cations may be less than 50 mol %. Thus, a halide with a stabler structure can be obtained.
In at least one selected from the group consisting of (NH4)aYα3+a and (NH4)bSmβ3+b included in the mixed material, part of metal cations may be, for example, replaced with at least one cation selected from the group consisting of Na, K, Mg, Sr, Ba, Zn, In, Sn, Bi, La, Ce, Pr, Nd, Pm, Sm, Eu, Tb, Dy, Ho, Er, Tm, Yb, and Lu.
In the heat treatment step S1000, the mixed material may be heat-treated at higher than or equal to 300° C. Thus, a halide having high ionic conductivity can be produced by a method with industrially high productivity. By setting the heat treatment temperature to be higher than or equal to 300° C., the mixed material can be reacted sufficiently. That is, (NH4)aYα3+a, (NH4)bSmβ3+b, Liγ, and Caδ2 can be reacted sufficiently. Here, the term “heat treatment temperature” refers to ambient temperature. In the case where the mixed material is heat-treated at higher than or equal to 300° C., it is possible to produce a halide having an ionic conductivity of greater than or equal to 6.7×10−7 S/cm at around room temperature.
In the heat treatment step S1000, the mixed material may be heat-treated at lower than or equal to 650° C. The mixed material may be heat-treated, for example, at higher than or equal to 300° C. and lower than or equal to 650° C. Thus, a halide having high ionic conductivity can be produced by a method with industrially high productivity. By setting the heat treatment temperature to be lower than or equal to 650° C., it is possible to suppress thermal decomposition of a halide formed by a solid phase reaction. Consequently, the ionic conductivity of a halide, which is a heat-treated product, can be enhanced. That is, a high-quality halide solid electrolyte can be obtained.
In order to produce a halide having higher ionic conductivity by a method with industrially high productivity, the mixed material may be heat-treated at higher than or equal to 350° C. The mixed material may be heat-treated, for example, at higher than or equal to 350° C. and lower than or equal to 650° C. By setting the heat treatment temperature to be higher than or equal to 350° C., a halide, which is a heat-treated product, has higher crystallinity. Consequently, the ionic conductivity of a halide, which is a heat-treated product, can be further enhanced. That is, a higher-quality halide solid electrolyte material can be obtained.
In order to produce a halide having higher ionic conductivity by a method with industrially high productivity, the mixed material may be heat-treated at higher than or equal to 450° C. The mixed material may be heat-treated, for example, at higher than or equal to 450° C. and lower than or equal to 650° C. By setting the heat treatment temperature to be higher than or equal to 450° C., a halide, which is a heat-treated product, has higher crystallinity. Consequently, the ionic conductivity of a halide, which is a heat-treated product, can be further enhanced. That is, a higher-quality halide solid electrolyte material can be obtained.
In order to produce a halide having higher ionic conductivity by a method with industrially high productivity, the mixed material may be heat-treated for more than or equal to 1 hour and less than or equal to 72 hours. By setting the heat treatment time to be more than or equal to 1 hour, the mixed material can be reacted sufficiently. That is, (NH4)aYα3+a, (NH4)bSmβ3+b, Liγ, and Caδ2 can be reacted sufficiently. By setting the heat treatment time to be less than or equal to 72 hours, volatilization of a halide, which is a heat-treated product, can be suppressed. That is, it is possible to obtain a halide having a target compositional ratio. Consequently, it is possible to suppress a decrease in ionic conductivity of a halide due to a compositional change. That is, a higher-quality halide solid electrolyte material can be obtained.
As shown in
The mixing step S1100 is carried out before the heat treatment step S1000.
In the mixing step S1100, (NH4)aYα3+a, (NH4)bSmβ3+b, Liγ, and Caδ2 serving as starting materials are mixed. Thus, a mixed material is obtained. That is, a material to be heat-treated in the heat treatment step S1000 is obtained.
In order to mix the starting materials, a commonly known mixing apparatus (e.g., a mortar, blender, or ball mill) may be used.
For example, in the mixing step S1100, powders of the starting materials may be prepared and mixed. In this case, in the heat treatment step S1000, a mixed material in the form of powder may be heat-treated. The mixed material in the form of powder obtained in the mixing step S1100 may be shaped into pellets by pressing. Alternatively, in the heat treatment step S1000, a mixed material in the form of pellets may be heat-treated.
In the mixing step S1100, by further mixing, in addition to (NH4)aYα3+a, (NH4)bSmβ3+b, Liγ, and Caδ2, a starting material different from (NH4)aYα3+a, (NH4)bSmβ3+b, Liγ, and Caδ2, a mixed material may be obtained.
In the mixing step S1100, a starting material containing (NH4)aYα3+a as a main component, a starting material containing (NH4)bSmβ3+b as a main component, a starting material containing Liγ as a main component, and a starting material containing Caδ2 as a main component may be mixed. The term “main component” refers to a component having the highest content by molar ratio.
In the mixing step S1100, (NH4)aYα3+a, (NH4)bSmβ3+b, Liγ, and Caδ2 may be prepared and mixed so as to have a target composition.
For example, (NH4)3YCl6, (NH4)3SmCl6, LiCl, and CaCl2 may be mixed so as to satisfy the molar ratio of (NH4)3YCl6:(NH4)3SmCl6:LiCl:CaCl2=0.5:0.5:2.8:0.1. Thus, a halide having the composition represented by Li2.8Ca0.1Y0.5Sm0.5Cl6 can be produced.
The molar ratio of (NH4)aYα3+a, (NH4)bSmβ3+b, Liγ, and Caδ2 may be adjusted beforehand so as to cancel out a compositional change that may occur in the heat treatment step S1000.
In the mixing step S1100, in at least one selected from the group consisting of (NH4)aYα3+a and (NH4)bSmβ3+b, part of metal cations may be replaced with other metal cations. That is, part of Y and Sm may be replaced with other metal cations. A mixed material may be obtained by further mixing a compound in which part of Y in (NH4)aYα3+a is replaced with other metal cations, or a compound in which part of Sm in (NH4)bSmβ3+b is replaced with other metal cations. The cation substitution ratio of Y and Sm with other metal cations may be less than 50 mol %.
In the mixing step S1100, in at least one selected from the group consisting of Liγ and Caδ2, part of metal cations may be replaced with other metal cations. That is, part of Li and Ca may be replaced with other metal cations. A mixed material may be obtained by further mixing a compound in which part of Li in Liγ is replated with other metal cations, or a compound in which part of Ca in Caδ2 is replaced with other metal cations. The cation substitution ratio of Li and Ca with other metal cations may be less than 50 mol %.
As shown in
The preparation step S1200 is carried out before the mixing step S1100.
In the preparation step S1200, (NH4)aYα3+a and (NH4)bSmβ3+b are prepared. In the preparation step S1200, Liγ and Caδ2 may be further prepared. That is, materials to be mixed in the mixing step S1100 may be prepared.
In the preparation step S1200, a starting material, such as (NH4)aYα3+a, (NH4)bSmβ3+b, Liγ, or Caδ2, may be synthesized. Alternatively, in the preparation step S1200, commonly known, commercially available products (e.g., materials with a purity of greater than or equal to 99%) may be used.
Materials to be prepared may be dry.
Materials to be prepared may be, for example, in the form of crystals, aggregates, flakes, or powder. In the preparation step S1200, starting materials in the form of powder may be obtained by pulverizing starting materials in the form of crystals, aggregates, or flakes.
In order to reduce production cost, in the preparation step S1200, (NH4)aYα3+a may be synthesized from inexpensive Y2O3 and NH4α.
In order to reduce production cost, in the preparation step S1200, (NH4)bSmβ3+b may be synthesized from inexpensive Sm2O3 and NH4β.
(NH4)aYα3+a is, for example, synthesized as follows.
Y2O3 and NH4α, as starting materials, are mixed, for example, at a molar ratio of Y2O3:NH4α=1:12 to obtain a mixture. The mixture is heat-treated, for example, at higher than or equal to 150° C. and lower than or equal to 350° C. The value of a can vary depending on the heat treatment temperature.
For example, in the case where α is Cl, i.e., in the case where Y2O3 and NH4Cl are mixed and heat-treated, the reactions represented by the formulas (2) and (3) below are considered to proceed.
Y2O3+12NH4Cl→2(NH4)3YCl6+6NH3+3H2O (2)
2(NH4)3YCl6→2(NH4)0.5YCl3.5+5NH4Cl (3)
When the mixture containing Y2O3 and NH4Cl is heat-treated, for example, at about 200° C., the reaction represented by the formula (2) takes place. As a result, (NH4)3YCl6 is obtained as a main product. When the mixture is heat-treated, for example, at about 350° C., the reaction represented by the formula (3) takes place. As a result, (NH4)0.5YCl3.5 is obtained as a main product. In this way, when the heat treatment temperature changes, the value of a can also change.
Note that, in order to make the reaction proceed satisfactorily, NH4α may be prepared in an excessive amount with respect to Y2O3. For example, the amount of NH4α prepared is 5 to 15 mol % in excess with respect to Y2O3.
The heat treatment may be performed in an inert gas (e.g., helium, nitrogen, or argon) atmosphere or in a reduced pressure atmosphere.
(NH4)bSmβ3+b is, for example, synthesized as follows.
Sm2O3 and NH4β, as starting materials, are mixed, for example, at a molar ratio of Sm2O3:NH4β=1:12 to obtain a mixture. The mixture is heat-treated, for example, at higher than or equal to 150° C. and lower than or equal to 350° C. The value of b can vary depending on the heat treatment temperature.
For example, in the case where β is Cl, i.e., in the case where Sm2O3 and NH4Cl are mixed and heat-treated, the reactions represented by the formulas (4) and (5) below are considered to proceed.
Sm2O3+12NH4Cl→2(NH4)3SmCl6+6NH3+3H2O (4)
2(NH4)3SmCl6→2(NH4)0.5SmCl3.5+5NH4Cl (5)
When the mixture containing Sm2O3 and NH4Cl is heat-treated, for example, at about 200° C., the reaction represented by the formula (4) takes place. As a result, (NH4)3SmCl6 is obtained as a main product. When the mixture is heat-treated, for example, at about 350° C., the reaction represented by the formula (5) takes place. As a result, (NH4)0.5SmCl3.5 is obtained as a main product. In this way, when the heat treatment temperature changes, the value of b can also change.
In order to make the reaction proceed satisfactorily, NH4Cl may be prepared in an excessive amount with respect to Sm2O3. For example, the amount of NH4β prepared is 5 to 15 mol % in excess with respect to Sm2O3.
The heat treatment may be performed in an inert gas (e.g., helium, nitrogen, or argon) atmosphere or in a reduced pressure atmosphere.
In at least one selected from the group consisting of (NH4)aYα3+a and (NH4)bSmβ3+b, which are prepared in the preparation step S1200, part of metal cations may be replaced with other metal cations. That is, part of Y and Sm may be replaced with other metal cations. That is, a compound in which part of Y in (NH4)aYα3+a is replaced with other metal cations, or a compound in which part of Sm in (NH4)bSmβ3+b is replaced with other metal cations may be further prepared. The cation substitution ratio of Y and Sm with other metal cations may be less than 50 mol %.
The halide produced by the production method of the present disclosure can be used as a solid electrolyte material. The solid electrolyte material may be, for example, a solid electrolyte having lithium ion conductivity. The solid electrolyte material is used, for example, in all-solid-state lithium-ion secondary batteries.
The present disclosure will be described in more detail below.
Halides produced by the production method of the present disclosure described below were evaluated as solid electrolyte materials.
First, (NH4)3YCl6 and (NH4)3SmCl6 serving as starting materials for a solid electrolyte material were synthesized.
As starting materials for (NH4)3YCl6, Y2O3 and NH4Cl were prepared so as to satisfy the molar ratio of Y2O3:NH4Cl=1:13.2. That is, the preparation was made so that the amount of NH4Cl was 10 mol % in excess with respect to Y2O3. These materials were pulverized in a mortar made of agate and mixed. The resulting mixture was placed in a crucible made of alumina, and heat-treated, in a nitrogen atmosphere, at 200° C. for 15 hours. Thus, (NH4)3YCl6 was obtained.
As starting materials for (NH4)3SmCl6, Sm2O3 and NH4Cl were prepared so as to satisfy the molar ratio of Sm2O3:NH4Cl=1:13.2. That is, the preparation was made so that the amount of NH4Cl was 10 mol % in excess with respect to Sm2O3. These materials were pulverized in a mortar made of agate and mixed. The resulting mixture was placed in a crucible made of alumina, and heat-treated, in a nitrogen atmosphere, at 150° C. for 15 hours. Thus, (NH4)3SmCl6 was obtained.
Next, in an argon atmosphere with a dew point of lower than or equal to −60° C. and an oxygen concentration of less than or equal to 0.0001% by volume (hereinafter, referred to as “a dry argon atmosphere”), (NH4)3YCl6, (NH4)3SmCl6, LiCl, LiBr, and CaBr2 were prepared so as to satisfy the molar ratio of (NH4)3YCl6:(NH4)3SmCl6:LiCl:LiBr:CaBr2=0.8:0.2:0.5:2.3:0.1. These materials were pulverized and mixed with a mortar made of agate. The resulting mixture was placed in a crucible made of alumina, and heat-treated, in a dry argon atmosphere, at 500° C. for 1 hour. The resulting heat-treated product was pulverized in a mortar made of agate. Thus, a solid electrolyte material according to Sample 1 containing Li, Ca, Y, Sm, Br, and Cl was obtained.
The contents per unit weight of Li, Ca, Y, and Sm in the entire solid electrolyte material according to Sample 1 were measured by an inductively coupled plasma atomic emission spectrochemical analysis method using an inductively coupled plasma atomic emission spectrochemical analysis device (Thermo Fisher Scientific K.K., iCAP7400). On the basis of the contents of Li, Ca, Y, and Sm measured, a molar ratio of Li:Ca:Y:Sm was calculated. As a result, the molar ratio of Li:Ca:Y:Sm was 2.8:0.1:0.8:0.2.
The pressure-molding die 200 included an upper punch 201, a die 202, and a lower punch 203. The die 202 was made of insulating polycarbonate. The upper punch 201 and the lower punch 203 were made of electronically conductive stainless steel.
Using the pressure-molding die 200 shown in
In a dry atmosphere with a dew point of lower than or equal to −60° C., the pressure-molding die 200 was filled with the solid electrolyte material according to Sample 1. Inside the pressure-molding die 200, a pressure of 300 MPa was applied to the solid electrolyte material according to Sample 1 (i.e., powder 101 of the solid electrolyte material in
With the pressure being applied, the upper punch 201 and the lower punch 203 were connected to a potentiostat (Princeton Applied Research, VersaSTAT4) equipped with a frequency response analyzer. The upper punch 201 was connected to a working electrode and a potential measurement terminal, The lower punch 203 was connected to a counter electrode and a reference electrode. The impedance of the solid electrolyte material was measured by an electrochemical impedance measurement method at room temperature.
In
σ=(RSE×S/t)−1 (6)
where σ represents the ionic conductivity. S represents the contact area between the solid electrolyte material and the upper punch 201 (equal to the area of a hollow portion of the die 202 in
The ionic conductivity of the solid electrolyte material according to Sample 1 measured at 25° C. was 3.1×10−3 S/cm.
Samples 2 to 16 will be described below.
Solid electrolyte materials according to Samples 2 to 8 were obtained as in Sample 1 except for the heat treatment temperature and the heat treatment time. The heat treatment temperature and the heat treatment time are shown in Table 1.
First, (NH4)0.5SmCl3.5 serving as a starting material for a solid electrolyte material was synthesized.
As starting materials for (NH4)0.5SmCl3.5, Sm2O3 and NH4Cl were prepared so as to satisfy the molar ratio of Sm2O3:NH4Cl=1:13.2. That is, the preparation was made so that the amount of NH4Cl was 10 mol % in excess with respect to Sm2O3. These materials were pulverized in a mortar made of agate and mixed. The resulting mixture was placed in a crucible made of alumina, and heat-treated, in a nitrogen atmosphere, at 350° C. for 15 hours. Thus, (NH4)0.5SmCl3.5 was obtained.
Next, in a dry argon atmosphere, (NH4)3YCl6, (NH4)0.5SmCl3.5, LiCl, LiBr, and CaBr2 were prepared so as to satisfy the molar ratio of (NH4)3YCl6:(NH4.5SmCl3.5:LiCl:LiBr:CaBr2=0.8:0.2:0.5:2.3:0.1.
As in Sample 1 except for the items described above, a solid electrolyte material according to Sample 9 was obtained.
First, SmCl3 serving as a starting material for a solid electrolyte material was synthesized.
As starting materials for SmCl3, Sm2O3 and NH4Cl were prepared so as to satisfy the molar ratio of Sm2O3:NH4Cl=1:13.2. That is, the preparation was made so that the amount of NH4Cl was 10 mol % in excess with respect to Sm2O3. These materials were pulverized in a mortar made of agate and mixed. The resulting mixture was placed in a crucible made of alumina, and heat-treated, in a nitrogen atmosphere, at 450° C. for 15 hours. Thus, SmCl3 was obtained.
Next, in a dry argon atmosphere, (NH4)3YCl6, SmCl3, LiCl, LiBr, and CaBr2 were prepared so as to satisfy the molar ratio of (NH4)3YCl6:SmCl3:LiCl:LiBr:CaBr2=0.8:0.2:0.5:2.3:0.1.
As in Sample 1 except for the items described above, a solid electrolyte material according to Sample 10 was obtained.
First, (NH4)0.5YCl3.5 serving as a starting material for a solid electrolyte material was synthesized.
As starting materials for (NH4)0.5YCl3.5, Y2O3 and NH4Cl were prepared so as to satisfy the molar ratio of Y2O3:NH4Cl=1:13.2. That is, the preparation was made so that the amount of NH4Cl was 10 mol % in excess with respect to Y2O3. These materials were pulverized in a mortar made of agate and mixed. The resulting mixture was placed in a crucible made of alumina, and heat-treated, in a nitrogen atmosphere, at 350° C. for 15 hours. Thus, (NH4)0.5YCl3.5 was obtained.
Next, in a dry argon atmosphere, (NH4)0.5YCl3.5, (NH4)3SmCl6, LiCl, LiBr, and CaBr2 were prepared so as to satisfy the molar ratio of (NH4)0.5YCl3.5:(NH4)3SmCl6:LiCl:LiBr:CaBr2=0.8:0.2:0.5:2.3:0.1.
As in Sample 1 except for the items described above, a solid electrolyte material according to Sample 11 was obtained.
First, YCl3 serving as a starting material for a solid electrolyte material was synthesized.
As starting materials for YCl3, Y2O3 and NH4Cl were prepared so as to satisfy the molar ratio of Y2O3:NH4Cl=1:13.2. That is, the preparation was made so that the amount of NH4Cl was 10 mol % in excess with respect to Y2O3. These materials were pulverized in a mortar made of agate and mixed. The resulting mixture was placed in a crucible made of alumina, and heat-treated, in a nitrogen atmosphere, at 450° C. for 15 hours. Thus, YCl3 was obtained.
Next, in a dry argon atmosphere, YCl3, (NH4)3SmCl6, LiCl, LiBr, and CaBr2 were prepared so as to satisfy the molar ratio of YCl3:(NH4)3SmCl6:LiCl:LiBr:CaBr2=0.8:0.2:0.5:2.3:0.1.
As in Sample 1 except for the items described above, a solid electrolyte material according to Sample 12 was obtained.
In a dry argon atmosphere, (NH4)3YCl6, (NH4)3SmCl6, LiCl, LiBr, and CaCl2 were prepared so as to satisfy the molar ratio of (NH4)3YCl6:(NH4)3SmCl6:LiCl:LiBr:CaCl2=0.8:0.2:0.3:2.5:0.1.
As in Sample 1 except for the items described above, a solid electrolyte material according to Sample 13 was obtained.
First, (NH4)3YBr6 serving as a starting material for a solid electrolyte material was synthesized.
As starting materials for (NH4)3YBr6, Y2O3 and NH4Br were prepared so as to satisfy the molar ratio of Y2O3:NH4Br=1:13.2. That is, the preparation was made so that the amount of NH4Br was 10 mol % in excess with respect to Y2O3. These materials were pulverized in a mortar made of agate and mixed. The resulting mixture was placed in a crucible made of alumina, and heat-treated, in a nitrogen atmosphere, at 200° C. for 15 hours. Thus, (NH4)3YBr6 was obtained.
Next, in a dry argon atmosphere, (NH4)3YBr6, (NH4)3SmCl6, LiCl, LiBr, and CaCl2 were prepared so as to satisfy the molar ratio of (NH4)3YBr6:(NH4)3SmCl6:LiCl:LiBr:CaCl2=0.8:0.2:2.7:0.1:0.1.
As in Sample 1 except for the items described above, a solid electrolyte material according to Sample 14 was obtained.
First, (NH4)3SmBr6 serving as a starting material for a solid electrolyte material was synthesized.
As starting materials for (NH4)3SmBr6, Sm2O3 and NH4Br were prepared so as to satisfy the molar ratio of Sm2O3:NH4Br=1:13.2. That is, the preparation was made so that the amount of NH4Br was 10 mol % in excess with respect to Sm2O3. These materials were pulverized in a mortar made of agate and mixed. The resulting mixture was placed in a crucible made of alumina, and heat-treated, in a nitrogen atmosphere, at 200° C. for 15 hours. Thus, (NH4)3SmBr6 was obtained.
Next, in a dry argon atmosphere, (NH4)3YCl6, (NH4)3SmBr6, LiCl, LiBr, and CaCl2 were prepared so as to satisfy the molar ratio of (NH4)3YCl6:(NH4)3SmBr6:LiCl:LiBr:CaCl2=0.8:0.2:0.9:1.9:0.1.
As in Sample 1 except for the items described above, a solid electrolyte material according to Sample 15 was obtained.
As in Sample 1 except for the heat treatment temperature, a solid electrolyte material according to Sample 16 was obtained.
Ionic conductivities of the solid electrolyte materials according to Samples 2 to 16 were measured as in Sample 1. The measurement results are shown in Table 1.
In Table 1, the starting material 1 is a halide containing Y. The starting material 2 is a halide containing Sm. The starting material 3 is LiCl. The starting material 4 is LiBr. The starting material 5 is a halide containing Ca.
3.1 × 10−10
As is clear from Samples 1 to 16, the solid electrolyte materials produced by the production method of the present disclosure have, at around room temperature, an ionic conductivity of greater than or equal to 3.1×10−10 S/cm. As is clear from Samples 1 to 15, when the heat treatment temperature is higher than or equal to 300° C. and lower than or equal to 650° C., the resulting solid electrolyte material has, at around room temperature, a high ionic conductivity of greater than or equal to 6.7×10−7 S/cm. The reason for this is considered to be that, when the heat treatment temperature is 300° C., a solid phase reaction proceeds sufficiently.
As is clear from comparison of Samples 1 and 3 to 8 with Sample 2, when the heat treatment temperature is higher than or equal to 350 and lower than or equal to 650° C., the ionic conductivity of the solid electrolyte material is further enhanced.
As is clear from comparison of Samples 1 and 5 to 8 with Samples 3 and 4, when the heat treatment temperature is higher than or equal to 450 and lower than or equal to 650° C., the ionic conductivity of the solid electrolyte material is still further enhanced.
As is clear from comparison of Samples 1, 6, and 7 with Samples 5 and 8, when the heat treatment temperature is higher than or equal to 500° C. and lower than or equal to 600° C., the ionic conductivity of the solid electrolyte material is still further enhanced. The reason for this is considered to be that the solid electrolyte material has higher crystallinity.
As described above, the halide produced by the production method of the present disclosure has high lithium ion conductivity. Furthermore, the production method of the present disclosure is a simple and easy method and a method with industrially high productivity. The method with industrially high productivity is, for example, a method enabling low-cost mass production.
The production method of the present disclosure is, for example, used as a method for producing a solid electrolyte material. The solid electrolyte material produced by the production method of the present disclosure is used, for example, in all-solid-state lithium-ion secondary batteries.
| Number | Date | Country | Kind |
|---|---|---|---|
| 2020-064815 | Mar 2020 | JP | national |
| Number | Date | Country | |
|---|---|---|---|
| Parent | PCT/JP2021/003305 | Jan 2021 | US |
| Child | 17933098 | US |
