US20220149427A1 - Powderous solid electrolyte compound for solid-state rechargeable lithium ion battery - Google Patents
Powderous solid electrolyte compound for solid-state rechargeable lithium ion battery Download PDFInfo
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- US20220149427A1 US20220149427A1 US17/431,728 US202017431728A US2022149427A1 US 20220149427 A1 US20220149427 A1 US 20220149427A1 US 202017431728 A US202017431728 A US 202017431728A US 2022149427 A1 US2022149427 A1 US 2022149427A1
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- 150000001875 compounds Chemical class 0.000 title claims abstract description 23
- HBBGRARXTFLTSG-UHFFFAOYSA-N Lithium ion Chemical compound [Li+] HBBGRARXTFLTSG-UHFFFAOYSA-N 0.000 title claims abstract description 12
- 229910001416 lithium ion Inorganic materials 0.000 title claims abstract description 12
- 239000007784 solid electrolyte Substances 0.000 title description 25
- 239000003792 electrolyte Substances 0.000 claims abstract description 42
- 239000006104 solid solution Substances 0.000 claims abstract description 41
- WHXSMMKQMYFTQS-UHFFFAOYSA-N Lithium Chemical compound [Li] WHXSMMKQMYFTQS-UHFFFAOYSA-N 0.000 claims description 32
- 229910052744 lithium Inorganic materials 0.000 claims description 32
- 238000002441 X-ray diffraction Methods 0.000 claims description 20
- 239000013078 crystal Substances 0.000 claims description 14
- 239000000843 powder Substances 0.000 claims description 14
- 239000002245 particle Substances 0.000 claims description 11
- 239000007774 positive electrode material Substances 0.000 claims description 10
- 239000010406 cathode material Substances 0.000 claims description 2
- 238000005245 sintering Methods 0.000 description 20
- 239000000203 mixture Substances 0.000 description 18
- 229910052751 metal Inorganic materials 0.000 description 15
- 239000002184 metal Substances 0.000 description 15
- 239000008188 pellet Substances 0.000 description 14
- 238000005259 measurement Methods 0.000 description 13
- 230000000052 comparative effect Effects 0.000 description 12
- 238000000034 method Methods 0.000 description 11
- 239000011244 liquid electrolyte Substances 0.000 description 10
- 239000000463 material Substances 0.000 description 10
- 101150088727 CEX1 gene Proteins 0.000 description 9
- 229910052732 germanium Inorganic materials 0.000 description 9
- GNPVGFCGXDBREM-UHFFFAOYSA-N germanium atom Chemical compound [Ge] GNPVGFCGXDBREM-UHFFFAOYSA-N 0.000 description 9
- 238000002156 mixing Methods 0.000 description 9
- QVGXLLKOCUKJST-UHFFFAOYSA-N atomic oxygen Chemical compound [O] QVGXLLKOCUKJST-UHFFFAOYSA-N 0.000 description 7
- 239000011888 foil Substances 0.000 description 7
- 229910052760 oxygen Inorganic materials 0.000 description 7
- 239000001301 oxygen Substances 0.000 description 7
- 239000000243 solution Substances 0.000 description 7
- 239000002904 solvent Substances 0.000 description 7
- MCMNRKCIXSYSNV-UHFFFAOYSA-N Zirconium dioxide Chemical compound O=[Zr]=O MCMNRKCIXSYSNV-UHFFFAOYSA-N 0.000 description 6
- YBMRDBCBODYGJE-UHFFFAOYSA-N germanium dioxide Chemical compound O=[Ge]=O YBMRDBCBODYGJE-UHFFFAOYSA-N 0.000 description 6
- 230000008569 process Effects 0.000 description 6
- 238000005033 Fourier transform infrared spectroscopy Methods 0.000 description 5
- VEXZGXHMUGYJMC-UHFFFAOYSA-N Hydrochloric acid Chemical compound Cl VEXZGXHMUGYJMC-UHFFFAOYSA-N 0.000 description 5
- VYPSYNLAJGMNEJ-UHFFFAOYSA-N Silicium dioxide Chemical compound O=[Si]=O VYPSYNLAJGMNEJ-UHFFFAOYSA-N 0.000 description 5
- 238000009826 distribution Methods 0.000 description 5
- 238000009616 inductively coupled plasma Methods 0.000 description 5
- 239000012535 impurity Substances 0.000 description 4
- 229910052909 inorganic silicate Inorganic materials 0.000 description 4
- 229910001386 lithium phosphate Inorganic materials 0.000 description 4
- 239000011164 primary particle Substances 0.000 description 4
- 239000000126 substance Substances 0.000 description 4
- 238000012360 testing method Methods 0.000 description 4
- 239000002227 LISICON Substances 0.000 description 3
- 238000004458 analytical method Methods 0.000 description 3
- 150000001768 cations Chemical class 0.000 description 3
- 230000002950 deficient Effects 0.000 description 3
- 239000008367 deionised water Substances 0.000 description 3
- 229910021641 deionized water Inorganic materials 0.000 description 3
- IEJIGPNLZYLLBP-UHFFFAOYSA-N dimethyl carbonate Chemical compound COC(=O)OC IEJIGPNLZYLLBP-UHFFFAOYSA-N 0.000 description 3
- 239000002223 garnet Substances 0.000 description 3
- 229910052746 lanthanum Inorganic materials 0.000 description 3
- XGZVUEUWXADBQD-UHFFFAOYSA-L lithium carbonate Chemical compound [Li+].[Li+].[O-]C([O-])=O XGZVUEUWXADBQD-UHFFFAOYSA-L 0.000 description 3
- 229910052808 lithium carbonate Inorganic materials 0.000 description 3
- 239000002243 precursor Substances 0.000 description 3
- 238000002360 preparation method Methods 0.000 description 3
- 239000007787 solid Substances 0.000 description 3
- 238000006467 substitution reaction Methods 0.000 description 3
- 238000002834 transmittance Methods 0.000 description 3
- TWQULNDIKKJZPH-UHFFFAOYSA-K trilithium;phosphate Chemical compound [Li+].[Li+].[Li+].[O-]P([O-])([O-])=O TWQULNDIKKJZPH-UHFFFAOYSA-K 0.000 description 3
- XLYOFNOQVPJJNP-UHFFFAOYSA-N water Chemical compound O XLYOFNOQVPJJNP-UHFFFAOYSA-N 0.000 description 3
- 229910052726 zirconium Inorganic materials 0.000 description 3
- CSCPPACGZOOCGX-UHFFFAOYSA-N Acetone Chemical compound CC(C)=O CSCPPACGZOOCGX-UHFFFAOYSA-N 0.000 description 2
- XKRFYHLGVUSROY-UHFFFAOYSA-N Argon Chemical compound [Ar] XKRFYHLGVUSROY-UHFFFAOYSA-N 0.000 description 2
- 229910007562 Li2SiO3 Inorganic materials 0.000 description 2
- 229910001290 LiPF6 Inorganic materials 0.000 description 2
- 238000003991 Rietveld refinement Methods 0.000 description 2
- 229910018557 Si O Inorganic materials 0.000 description 2
- 229910006937 Si0.5P0.5 Inorganic materials 0.000 description 2
- 229910052782 aluminium Inorganic materials 0.000 description 2
- 230000015572 biosynthetic process Effects 0.000 description 2
- 238000006243 chemical reaction Methods 0.000 description 2
- 238000000975 co-precipitation Methods 0.000 description 2
- 229910052681 coesite Inorganic materials 0.000 description 2
- 229910052906 cristobalite Inorganic materials 0.000 description 2
- 230000007423 decrease Effects 0.000 description 2
- MNNHAPBLZZVQHP-UHFFFAOYSA-N diammonium hydrogen phosphate Chemical compound [NH4+].[NH4+].OP([O-])([O-])=O MNNHAPBLZZVQHP-UHFFFAOYSA-N 0.000 description 2
- 229910000388 diammonium phosphate Inorganic materials 0.000 description 2
- 239000002019 doping agent Substances 0.000 description 2
- 230000000694 effects Effects 0.000 description 2
- 238000000157 electrochemical-induced impedance spectroscopy Methods 0.000 description 2
- ZZUFCTLCJUWOSV-UHFFFAOYSA-N furosemide Chemical compound C1=C(Cl)C(S(=O)(=O)N)=CC(C(O)=O)=C1NCC1=CC=CO1 ZZUFCTLCJUWOSV-UHFFFAOYSA-N 0.000 description 2
- 238000010438 heat treatment Methods 0.000 description 2
- 230000006872 improvement Effects 0.000 description 2
- INHCSSUBVCNVSK-UHFFFAOYSA-L lithium sulfate Chemical compound [Li+].[Li+].[O-]S([O-])(=O)=O INHCSSUBVCNVSK-UHFFFAOYSA-L 0.000 description 2
- 238000004519 manufacturing process Methods 0.000 description 2
- 230000001590 oxidative effect Effects 0.000 description 2
- 229910052698 phosphorus Inorganic materials 0.000 description 2
- 230000004044 response Effects 0.000 description 2
- 239000011163 secondary particle Substances 0.000 description 2
- 229910052710 silicon Inorganic materials 0.000 description 2
- 239000000377 silicon dioxide Substances 0.000 description 2
- LIVNPJMFVYWSIS-UHFFFAOYSA-N silicon monoxide Inorganic materials [Si-]#[O+] LIVNPJMFVYWSIS-UHFFFAOYSA-N 0.000 description 2
- 239000002002 slurry Substances 0.000 description 2
- 229910052682 stishovite Inorganic materials 0.000 description 2
- 229910052905 tridymite Inorganic materials 0.000 description 2
- RIUWBIIVUYSTCN-UHFFFAOYSA-N trilithium borate Chemical compound [Li+].[Li+].[Li+].[O-]B([O-])[O-] RIUWBIIVUYSTCN-UHFFFAOYSA-N 0.000 description 2
- 238000001238 wet grinding Methods 0.000 description 2
- 101100439211 Caenorhabditis elegans cex-2 gene Proteins 0.000 description 1
- KMTRUDSVKNLOMY-UHFFFAOYSA-N Ethylene carbonate Chemical compound O=C1OCCO1 KMTRUDSVKNLOMY-UHFFFAOYSA-N 0.000 description 1
- 238000001157 Fourier transform infrared spectrum Methods 0.000 description 1
- 229910007822 Li2ZrO3 Inorganic materials 0.000 description 1
- -1 Li3.5Si0.5P0.5O4 Chemical class 0.000 description 1
- 229910011790 Li4GeO4 Inorganic materials 0.000 description 1
- 229910002984 Li7La3Zr2O12 Inorganic materials 0.000 description 1
- QUGWHPCSEHRAFA-UHFFFAOYSA-K P(=O)([O-])([O-])[O-].[Ge+2].[Li+] Chemical compound P(=O)([O-])([O-])[O-].[Ge+2].[Li+] QUGWHPCSEHRAFA-UHFFFAOYSA-K 0.000 description 1
- 229910019142 PO4 Inorganic materials 0.000 description 1
- 239000002033 PVDF binder Substances 0.000 description 1
- BQCADISMDOOEFD-UHFFFAOYSA-N Silver Chemical compound [Ag] BQCADISMDOOEFD-UHFFFAOYSA-N 0.000 description 1
- AENRKZLCRZIUKO-UHFFFAOYSA-N [P]=O.[Si].[Li] Chemical compound [P]=O.[Si].[Li] AENRKZLCRZIUKO-UHFFFAOYSA-N 0.000 description 1
- XAGFODPZIPBFFR-UHFFFAOYSA-N aluminium Chemical compound [Al] XAGFODPZIPBFFR-UHFFFAOYSA-N 0.000 description 1
- 239000012736 aqueous medium Substances 0.000 description 1
- 229910052786 argon Inorganic materials 0.000 description 1
- 238000000498 ball milling Methods 0.000 description 1
- 230000008901 benefit Effects 0.000 description 1
- 230000005540 biological transmission Effects 0.000 description 1
- 238000001354 calcination Methods 0.000 description 1
- 230000008859 change Effects 0.000 description 1
- 238000012512 characterization method Methods 0.000 description 1
- 239000004020 conductor Substances 0.000 description 1
- 230000001186 cumulative effect Effects 0.000 description 1
- 238000000354 decomposition reaction Methods 0.000 description 1
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- 238000010790 dilution Methods 0.000 description 1
- 239000012895 dilution Substances 0.000 description 1
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- 239000011363 dried mixture Substances 0.000 description 1
- 230000005518 electrochemistry Effects 0.000 description 1
- 238000005430 electron energy loss spectroscopy Methods 0.000 description 1
- 238000006056 electrooxidation reaction Methods 0.000 description 1
- 238000002474 experimental method Methods 0.000 description 1
- 238000010304 firing Methods 0.000 description 1
- 238000009472 formulation Methods 0.000 description 1
- 239000000446 fuel Substances 0.000 description 1
- 229910052733 gallium Inorganic materials 0.000 description 1
- QZQVBEXLDFYHSR-UHFFFAOYSA-N gallium(III) oxide Inorganic materials O=[Ga]O[Ga]=O QZQVBEXLDFYHSR-UHFFFAOYSA-N 0.000 description 1
- 239000011521 glass Substances 0.000 description 1
- 238000000227 grinding Methods 0.000 description 1
- 230000035876 healing Effects 0.000 description 1
- 238000000265 homogenisation Methods 0.000 description 1
- 238000001453 impedance spectrum Methods 0.000 description 1
- GLXDVVHUTZTUQK-UHFFFAOYSA-M lithium;hydroxide;hydrate Chemical compound [Li+].O.[OH-] GLXDVVHUTZTUQK-UHFFFAOYSA-M 0.000 description 1
- 230000014759 maintenance of location Effects 0.000 description 1
- 230000005012 migration Effects 0.000 description 1
- 238000013508 migration Methods 0.000 description 1
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- 230000005855 radiation Effects 0.000 description 1
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- 238000009877 rendering Methods 0.000 description 1
- 238000011160 research Methods 0.000 description 1
- 229910052709 silver Inorganic materials 0.000 description 1
- 239000004332 silver Substances 0.000 description 1
- 238000004611 spectroscopical analysis Methods 0.000 description 1
- 229910001220 stainless steel Inorganic materials 0.000 description 1
- 239000010935 stainless steel Substances 0.000 description 1
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- 239000004575 stone Substances 0.000 description 1
- 239000004094 surface-active agent Substances 0.000 description 1
- 229910052723 transition metal Inorganic materials 0.000 description 1
- 150000003624 transition metals Chemical class 0.000 description 1
- 238000000411 transmission spectrum Methods 0.000 description 1
- 238000010947 wet-dispersion method Methods 0.000 description 1
- 238000009736 wetting Methods 0.000 description 1
Images
Classifications
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- H—ELECTRICITY
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- H01M10/00—Secondary cells; Manufacture thereof
- H01M10/05—Accumulators with non-aqueous electrolyte
- H01M10/052—Li-accumulators
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- H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
- H01M10/00—Secondary cells; Manufacture thereof
- H01M10/05—Accumulators with non-aqueous electrolyte
- H01M10/052—Li-accumulators
- H01M10/0525—Rocking-chair batteries, i.e. batteries with lithium insertion or intercalation in both electrodes; Lithium-ion batteries
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- H—ELECTRICITY
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- H01M10/05—Accumulators with non-aqueous electrolyte
- H01M10/056—Accumulators with non-aqueous electrolyte characterised by the materials used as electrolytes, e.g. mixed inorganic/organic electrolytes
- H01M10/0561—Accumulators with non-aqueous electrolyte characterised by the materials used as electrolytes, e.g. mixed inorganic/organic electrolytes the electrolyte being constituted of inorganic materials only
- H01M10/0562—Solid materials
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- H01M4/04—Processes of manufacture in general
- H01M4/0471—Processes of manufacture in general involving thermal treatment, e.g. firing, sintering, backing particulate active material, thermal decomposition, pyrolysis
-
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- H01M4/02—Electrodes composed of, or comprising, active material
- H01M4/13—Electrodes for accumulators with non-aqueous electrolyte, e.g. for lithium-accumulators; Processes of manufacture thereof
- H01M4/131—Electrodes based on mixed oxides or hydroxides, or on mixtures of oxides or hydroxides, e.g. LiCoOx
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- H01M4/02—Electrodes composed of, or comprising, active material
- H01M4/13—Electrodes for accumulators with non-aqueous electrolyte, e.g. for lithium-accumulators; Processes of manufacture thereof
- H01M4/139—Processes of manufacture
- H01M4/1391—Processes of manufacture of electrodes based on mixed oxides or hydroxides, or on mixtures of oxides or hydroxides, e.g. LiCoOx
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- H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
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- H01M4/02—Electrodes composed of, or comprising, active material
- H01M4/36—Selection of substances as active materials, active masses, active liquids
- H01M4/38—Selection of substances as active materials, active masses, active liquids of elements or alloys
- H01M4/381—Alkaline or alkaline earth metals elements
- H01M4/382—Lithium
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- H—ELECTRICITY
- H01—ELECTRIC ELEMENTS
- H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
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- H01M4/02—Electrodes composed of, or comprising, active material
- H01M4/36—Selection of substances as active materials, active masses, active liquids
- H01M4/48—Selection of substances as active materials, active masses, active liquids of inorganic oxides or hydroxides
- H01M4/50—Selection of substances as active materials, active masses, active liquids of inorganic oxides or hydroxides of manganese
- H01M4/505—Selection of substances as active materials, active masses, active liquids of inorganic oxides or hydroxides of manganese of mixed oxides or hydroxides containing manganese for inserting or intercalating light metals, e.g. LiMn2O4 or LiMn2OxFy
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- H01M4/36—Selection of substances as active materials, active masses, active liquids
- H01M4/48—Selection of substances as active materials, active masses, active liquids of inorganic oxides or hydroxides
- H01M4/52—Selection of substances as active materials, active masses, active liquids of inorganic oxides or hydroxides of nickel, cobalt or iron
- H01M4/525—Selection of substances as active materials, active masses, active liquids of inorganic oxides or hydroxides of nickel, cobalt or iron of mixed oxides or hydroxides containing iron, cobalt or nickel for inserting or intercalating light metals, e.g. LiNiO2, LiCoO2 or LiCoOxFy
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- H01M4/62—Selection of inactive substances as ingredients for active masses, e.g. binders, fillers
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- H01M50/00—Constructional details or processes of manufacture of the non-active parts of electrochemical cells other than fuel cells, e.g. hybrid cells
- H01M50/40—Separators; Membranes; Diaphragms; Spacing elements inside cells
- H01M50/409—Separators, membranes or diaphragms characterised by the material
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- H01M2004/026—Electrodes composed of, or comprising, active material characterised by the polarity
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- H01M2220/20—Batteries in motive systems, e.g. vehicle, ship, plane
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- H01M2300/00—Electrolytes
- H01M2300/0017—Non-aqueous electrolytes
- H01M2300/0065—Solid electrolytes
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- Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
- Y02E—REDUCTION OF GREENHOUSE GAS [GHG] EMISSIONS, RELATED TO ENERGY GENERATION, TRANSMISSION OR DISTRIBUTION
- Y02E60/00—Enabling technologies; Technologies with a potential or indirect contribution to GHG emissions mitigation
- Y02E60/10—Energy storage using batteries
Definitions
- This invention relates to a solid electrolyte (SE) for solid-state rechargeable lithium-ion batteries suitable for electric vehicle (EV) applications.
- the solid electrolyte according to the invention has an improved lithium ionic conductivity.
- additional requirements rendering a battery eligible for EV applications should therefore include: high capacity, longer cycle lives, lower cost, and better safety.
- Solid electrolyte-based batteries are considerably safer and can be an alternative to liquid electrolyte-based batteries for the power source of electric vehicles. Since the decomposition temperature of SE is higher than the liquid electrolyte, an EV comprising such a SE-based battery, instead of a liquid electrolyte-based battery, would be safer and its battery manufacturing would also be safer. Aside from the clear advantage that a SE-based battery is much safer than a liquid electrolyte-based battery, a SE-based battery is also more compact than liquid electrolyte-based batteries, and therefore lead to higher power densities
- a SE compared to liquid electrolyte, has a lower lithium ionic conductivity (typically included between 10 ⁇ 7 to 10 ⁇ 6 S/cm).
- the lower lithium ionic conductivity in a SE is due to the higher migration energy of lithium ions.
- La, Zr comprising garnet
- LSPO lithium silicon phosphorus oxide
- LISICON lithium superionic conductor
- electrolyte having a general formula: Li 4 ⁇ x Si 1 ⁇ x P x O 4 .
- the La, Zr comprising garnet, especially the cubic garnet (Li 7 La 3 Zr 2 O 12 ), shows a high conductivity.
- those materials are expensive due to the La and Zr content.
- This compound also needs to be synthesized at a temperature higher than 1000° C. which is not desired because of the volatility of lithium at the high temperature.
- the LSPO is well-known for its high chemical and electrochemical stability, high mechanical strength, and high electrochemical oxidation voltage, making such an electrolyte a promising candidate for EV applications.
- LSPO compounds like Li 3.5 Si 0.5 P 0.5 O 4 , have a relatively low lithium ionic conductivity.
- Li 3.5 Si 0.5 P 0.5 O 4 is a solid solution of Li 4 SiO 4 and Li 3 PO 4 having a crystal structure of ⁇ -Li 3 PO 4 with orthorhombic unit cell and tetrahedrally coordinated cations.
- a solid solution also called solid-state solution refers to a multi-component solid-state solution as a result of a mixture of one or more solutes in a solvent.
- the solutes can be atoms or groups of atoms (or compounds).
- Such a multi-component system is considered a solution rather than a compound when the crystal structure of the solvent remains unchanged by addition of the solutes, and when the chemical components remain in a single homogeneous phase.
- the solvent usually is a component with the largest portion and in this case is Li 3 PO 4 .
- the crystal structure of the solvent component is maintained after blending whereas the other component (solute, e.g. Li 4 SiO 4 ) dissolves in the solvent structure instead of forming a distinct compound having a structure that deviates from the structure of the solvent.
- Burmakin et. al. in Russian Journal of Electrochemistry (2010), 46, No. 2, 243-246 discloses a lithium germanium phosphate solid electrolyte doped with a tetravalent cation, Zr like: Li 3.75 Ge 0.70 Zr 0.05 P 0.25 O 4 , Li 3.50 Zn 0.125 Ge 0.75 P 0.25 O 4 , respectively.
- the Ge content in these formulation would not allow the obtention of a solid solution in a LSPO-based SE.
- Metallic Li can be used in the scope of the present invention as an anode of a SSB comprising the electrolyte according to the invention.
- the SE according to the present invention can be destined to be contacted to a Li metal-based anode, it must therefore be compatible to said Li metal-based anode of the SSB, meaning that the SE while contacting said anode must remain chemically stable.
- a solid electrolyte having an improved lithium ionic conductivity whilst retaining a solid solution and being chemically and thermally stable while contacting a Li metal anode is achieved by providing a solid solution according to claim 1 which comprises a LSPO-based electrolyte comprising germanium (Ge) up to 60 mol %.
- a Ge doped LSPO is referenced hereunder as “LSPGO”.
- a LSPGO-based electrolyte comprises Ge of superior to 60 mol %, it comprises at least one impurity phase (i.e. Li 2 SiO 3 ), and such a Li 2 SiO 3 -bearing LSPGO-based electrolyte is not a solid solution according to the present invention.
- impurity phase is observed in Burmakin et. al. (Li 2 ZrO 3 in this case) for a high content of Ge.
- the electrolyte according to the present invention is stable in presence of a Li metal foil, confirming its suitability in a SSB wherein a Li metal foil is used as an anode.
- a solid solution electrolyte suitable for solid-state rechargeable lithium ion battery comprising a compound having a general formula Li (3.5+L+x) Si (0.5+s ⁇ x) P (0.5+p ⁇ x) Ge 2x O 4+a wherein ⁇ 0.10 ⁇ L ⁇ 0.10, ⁇ 0.10 ⁇ s ⁇ 0.10, ⁇ 0.10 ⁇ p ⁇ 0.10, ⁇ 0.40 ⁇ a ⁇ 0.40, and 0.00 ⁇ x ⁇ 0.30.
- the solid solution electrolyte according to any of the preceding embodiments having a lithium ionic conductivity measured at 25° C. superior or equal to 2.0 ⁇ 10 ⁇ 5 S/cm and inferior or equal to 3.0 ⁇ 10 ⁇ 5 S/cm, preferably superior or equal to 2.5 ⁇ 10 ⁇ 5 S/cm and inferior or equal to 3.0 ⁇ 10 ⁇ 5 S/cm.
- the solid solution electrolyte according to any of the preceding embodiments comprising a crystal structure having an XRD pattern measured at 25° C. and at a wavelength of 1.5418 ⁇ comprising a first peak having a first intensity and a second peak having a second intensity, said first and second peaks being present in a range of 2 ⁇ superior or equal to 27.5 and inferior or to 30.0 ⁇ 0.5°, said XRD pattern being furthermore free of peaks at 2 ⁇ >37.0 ⁇ 0.5° having an intensity superior to said first or second intensity.
- the solid solution electrolyte according to any of the preceding embodiments comprising a crystal structure having an XRD pattern measured at 25° C. and at a wavelength of 1.5418 ⁇ comprising a first peak having a first intensity and a second peak having a second intensity, said first and second peaks being present in a first range of 2 ⁇ superior or equal to 27.5 and inferior or to 30.0 ⁇ 0.5°, wherein in a second range of 2 ⁇ superior or equal to 21.0 and inferior or to 25.0 ⁇ 0.5° said XRD pattern has no more than three additional peaks, each of said three additional peaks having an intensity superior to said first or second intensity.
- the solid solution electrolyte according to any of the preceding embodiments comprising a crystal structure having an XRD pattern measured at 25° C. and at a wavelength of 1.5418 ⁇ comprising a first peak having a first intensity and a second peak having a second intensity, said first and second peaks being present in a first range of 2 ⁇ superior or equal to 27.5 and inferior or to 30.0 ⁇ 0.5°, wherein in a second range of 2 ⁇ superior or equal to 34.0 and inferior or to 36.0 ⁇ 0.5°, said XRD pattern has no more than three additional peaks, each of said three additional peaks having an intensity superior to said first or second intensity.
- a solid-state rechargeable lithium ion battery comprising the solid solution electrolyte according to any of the previous embodiments.
- a solid-state rechargeable lithium ion battery comprising a negative electrode having a Li metal-base anode contacting the solid solution electrolyte according to any of the embodiments 1 to 9.
- FIG. 1 Comparison of Electrochemical Impedance Spectra (EIS) for sample with various Ge dopants (x in Li (3.5+x) Si (0.5 ⁇ x) P (0.5 ⁇ x) Ge 2x O 4+a ) in Example 1 and Comparative Example 1
- FIG. 2 Variation of lithium ionic conductivity versus the amount of Ge dopants (x in Li (3.5+x) Si (0.5 ⁇ x) P (0.5 ⁇ x) Ge 2x O 4+a ) in Example 1 and Comparative Example 1
- FIG. 3 Comparison of X-ray diffraction pattern of Example 1 and Comparative Example 1
- FIG. 4 Fourier-transform infrared spectrum of EX1-A, EX1-B, EX1-C, and Comparative Example 1 showing transmittance in (%) and wavenumber in (cm ⁇ 1 )
- FIG. 5 Comparison of X-ray diffraction pattern of Comparative Examples 1 and 2
- FIG. 6 Comparison of X-ray diffraction pattern of LSPO (a) before exposure to molten Li metal at 250° C. and (b) after 15 minutes exposure
- FIG. 7 Comparison of voltage vs. capacity graph of EX2-CAT-A and CEX3-CAT-B
- This invention discloses a germanium bearing LSPO compounds having a general formula Li (3.5+x) Si (0.5 ⁇ x) P (0.5 ⁇ x) Ge 2x O 4+a (LSPGO) wherein 0.00 ⁇ x ⁇ 0.30 and ⁇ 0.40 ⁇ a ⁇ 0.40. It is a solid solution of Li 4 GeO 4 , Li 3 PO 4 , and Li 4 SiO 4 .
- Li 4 GeO 4 Li 3 PO 4
- Li 4 SiO 4 Li 4 SiO 4 .
- the lithium ionic conductivity of the compound according to claim 1 significantly increases (reaching at least 10 ⁇ 5 S/cm) for x values higher or equal to 0.10.
- the conductivity of the compound according to claim 1 is unexpectedly higher (higher than 2.0 10 ⁇ 5 S/cm) for the narrow range: 0.20 ⁇ x ⁇ 0.30, in particular for 0.25 ⁇ x ⁇ 0.30.
- this narrower range leads to an increase of the lithium ionic conductivity by a 1.5 to 3.0 factor, which is remarkable.
- This invention is also inclusive of a catholyte compound made from a mixture of a NMC type of positive electrode active material and the germanium bearing LSPO compound according to the present invention.
- a “monolithic” morphology refers here to a morphology where a secondary particle contains basically only one primary particle. In the literature they are also called single crystal material, mono-crystal material, and one-body material. The preferred shape of the primary particle could be described as pebble stone shaped. The monolithic morphology can be achieved by using a high sintering temperature, a longer sintering time, and the use of a higher excess of lithium.
- a “polycrystalline” morphology refers to a morphology where a secondary particle contains more than one primary particles.
- the (solid-state) catholyte material is prepared by mixing the germanium bearing LSPO compound with the NMC composition so as to produce the catholyte which is subjected to a heat treatment at 600° C. ⁇ 800° C. for 1 ⁇ 20 hours under oxidizing atmosphere.
- the method for producing said catholyte is a co-sintering-based process wherein the germanium bearing LSPO and the NMC compositions are blended so as to provide a mixture which is then sintered.
- each of the compositions of the germanium bearing LSPO and NMC positive electrode active material in the catholyte There are several ways to obtain each of the compositions of the germanium bearing LSPO and NMC positive electrode active material in the catholyte. Whereas the difference of the median particle sizes (D50) between the solid electrolyte and positive electrode active material in the catholyte is superior or equal to 2 ⁇ m, they can be separated using a classifier such the elbow jet air classifier (https://elcanindustries.com/elbow-jet-air-classifier/). The compositions of separate particles are measured according to the protocol disclosed in the section F) Inductively Coupled Plasma method so as to determine each of the compositions of the germanium bearing LSPO material and NMC positive electrode active material in the catholyte.
- a classifier such the elbow jet air classifier (https://elcanindustries.com/elbow-jet-air-classifier/).
- the compositions of separate particles are measured according to the protocol disclosed
- EELS Electron Energy Loss Spectroscopy
- TEM Transmission Electron Microscope
- a cylindrical pellet is prepared by following procedure. 0.175 g of a powderous solid electrolyte compound sample is put on a mold having a diameter of 1.275 cm. A pressure of 230 MPa is applied to the mold. The pellet is sintered at 700° C. for 3 hours in oxygen atmosphere. Silver paste is painted on both sides of the pellet to have a sample configuration of Ag/pellet/Ag in order to allow EIS measurements. Standard deviation of this measurement is 2.0 ⁇ 10 ⁇ 8 .
- EIS is performed using an Ivium-n-Stat instrument, a potentiostat/galvanostat with an integrated frequency response analyzer.
- This instrument is common to be used in the battery/fuel cell-testing to collect impedance response against frequency sweep.
- the measurement frequency range is from 10 6 Hz to 10 ⁇ 1 Hz.
- the setting point/decade is 10 and the setting voltage is 0.05V. Measurement is conducted at room temperature (at 25° C.).
- the lithium ionic conductivity is calculated by below equation:
- L is the thickness of the pellet
- A is the area of the sample
- R is the resistance obtained by the electrochemical impedance spectroscopy.
- a cylindrical pellet is prepared by following procedure. 0.175 g of a powderous solid electrolyte compound sample is put on a mold having a diameter of 1.275 cm. A pressure of 230 MPa is applied to the mold. The pellet is sintered at 700° C. for 3 hours in oxygen atmosphere.
- the X-ray diffraction pattern of the pellet sample is collected with a Rigaku X-Ray Diffractometer (D/MAX-2500/PC) using a Cu K ⁇ radiation source emitting at a wavelength of 1.5418 ⁇ .
- the instrument configuration is set at: 1° Soller slit (SS), 1° divergence slit (DS) and 0.15 mm reception slit (RS).
- Diffraction patterns are obtained in the range of 10-70° (2 ⁇ ) with a scan speed of 4° per a minute.
- Obtained XRD patterns are analyzed by the Rietveld refinement method using X'Pert HighScore Plus software.
- the software is a powder pattern analysis tool with reliable Rietveld refinement analysis results.
- FTIR transmission spectrum for the LSPGO powder is collected using Thermo Scientific FTIR Spectrometer (Nicolet iS 50) in the wave number range of 1200 to 500 cm ⁇ 1 , with a resolution of 4 cm ⁇ 1 , and scan cycle of 32 scan.
- the catholyte powder samples used in the particle-size distribution (psd) measurements are prepared by hand grinding the catholyte powder samples using agate mortar and pestle.
- the psd is measured by using a Malvern Mastersizer 3000 with Hydro MV wet dispersion accessory after having dispersed each of the catholyte powder samples in an aqueous medium.
- D50 and D99 are defined as the particle size at 50% and 99% of the cumulative volume % distributions obtained from the Malvern Mastersizer 3000 with Hydro MV measurements.
- a catholyte containing 0.16 g of NMC, 0.03 g conductor (Super P), and 0.125 g of 8 wt % PVDF binder are mixed in NMP solvent using a planetary centrifugal mixer (Thinky mixer) for 20 minutes.
- the homogenized slurry is spread on one side of an aluminum foil using a doctor blade coater with a 15 ⁇ m gap.
- the slurry-coated foil is dried and punched as 8 mm diameter circular shape.
- a Swagelok cell is assembled in an argon-filled glove box with the configuration of positive electrode, separator having a diameter of 13 mm, and lithium foil having a diameter of 11 mm as a negative electrode.
- ICP Inductively Coupled Plasma
- composition of a positive electrode active material, a solid electrolyte, and a catholyte is measured by the inductively coupled plasma (ICP) method using an Agillent ICP 720-ES.
- ICP inductively coupled plasma
- 1 gram of a powder sample is dissolved into 50 mL high purity hydrochloric acid (at least 37 wt % of HCl with respect to the total amount of solution) in an Erlenmeyer flask.
- the flask is covered by a watch glass and heated on a hot plate at 380° C. until complete dissolution of the powder. After being cooled to room temperature, the solution from the Erlenmeyer flask is poured into a 250 mL volumetric flask.
- the volumetric flask is filled with deionized water up to the 250 mL mark, followed by a complete homogenization.
- An appropriate amount of solution is taken out by a pipette and transferred into a 250 mL volumetric flask for a second dilution, where the volumetric flask is filled with internal standard and 10% hydrochloric acid up to the 250 mL mark and then homogenized. Finally, this solution is used for ICP measurement.
- CEX1 having a general formula Li 3.50 Si 0.50 P 0.60 O 4 was prepared by the following steps:
- Pulverization 1.4 g of calcined powder was put on a 45 ml bottle with 30 ml of acetone and 3.4 g of Y doped ZrO 2 balls having a dimeter of 1 mm. The bottle was rotated in a conventional ball mill equipment with 500 RPM for 6 hours. The pulverized powder was dried at 70° C. for 6 hours.
- Ge doped LSPO samples having a general formula Li (3.5+x) Si (0.5 ⁇ x) P (0.5 ⁇ x) Ge 2x O 4 were prepared in the same manner as CEX1 except that different amount of GeO 2 was added and the amount of Li 2 CO 3 , SiO 2 , and (NH 4 ) 2 HPO 4 were adjusted in the mixing step according to the target molar ratios.
- EX1-A, EX1-B, EX1-C, EX1-D, EX1-E, and EX1-F had the x of 0.05, 0.10, 0.15, 0.20, 0.25, and 0.30, respectively.
- CEX2-A1 and CEX2-A2 having a general formula Li (3.5 ⁇ 30 x) Si (0.5 ⁇ x) P (0.5 ⁇ x) S 2x O 4+a were prepared in the same manner as samples in the Example 1 except that different amount of Li 2 SO 4 was added instead of GeO 2 .
- CEX2-A1 and CEX2-A2 had the x of 0.05 and 0.10, respectively.
- Ga doped LSPO sample CEX2-B having a general formula Li (3.5 ⁇ 30 x) Si (0.5 ⁇ x) P (0.5 ⁇ x) Ga 2x O 4+a was prepared in the same manner as samples in the Example 1 except that Ga 2 O 3 was added instead of GeO 2 .
- CEX2-B had the x of 0.05.
- the plot is composed of real part of impedance in X axis and imaginary part in Y axis.
- High frequency measurement appears on the left side of the graph forms a semicircle that is followed by a low angle spike as the result of the low frequency measurement.
- the semicircle formation corresponded to the lithium conduction in SE.
- the lithium ionic conductivity of CEX1 is 4.4 ⁇ 10 ⁇ 6 at room temperature that is comparable with the earlier published works on LSPO.
- the reduction of the semicircle diameter with the higher Ge amount indicating lower resistance of sample suggesting a better conductivity.
- FIG. 2 shows the improvement of lithium ionic conductivity where the value increases proportionally with more Ge in the structure.
- x is 0.30, the value reduces to 2.4 ⁇ 10 ⁇ 5 , concluding that 0.25 is an optimal concentration.
- FIG. 3 shows the XRD patterns of CEX1 (undoped electrolyte) and EX1-A to EX1-F. It is observed that Ge bearing LSPO samples have a single LISICON phase without impurity, demonstrating that Ge is well doped. In all graphs, the ⁇ -Li 3 PO 4 structure is maintained, indicated by the characteristic double peak at 28°-29° representing (121) and (200) planes as well as four consecutive peaks at 34°-36° correspond to (220), (131), (211), and (002) planes. The shifted peak positions to the left related with the larger crystal volume showed in Table 1. The observed single phase also acts as an evidence of solid solution formation for the Ge bearing LSPO.
- FTIR measurement is displayed in FIG. 4 with the vibration bands of P—O, Si—O, and Ge—O marked.
- the vibration bands at 580 cm ⁇ 1 , 910 cm ⁇ 1 , and around 1050 cm ⁇ 1 correspond to the vibration modes of tetrahedron P—O while band in area of 985-1005 cm ⁇ 1 corresponds to the vibration modes of Si—O, also in tetrahedral structure. All bands show transmittance signal increase along with the addition of Ge in the structure. On the other hand, transmittance of 790 cm ⁇ 1 band which corresponds to Ge—O vibration decreases with the more Ge in the structure. It is concluded that the atomic substitution of Ge successfully occurred at Si and P sites without changing the structure. This observation matches with that of XRD where the structure of LSPO is maintained upon doping.
- CEX2-A S bearing LSPO structure
- CEX2-B Ga bearing LSPO structure
- LSPGO pellet XRD diffraction pattern after exposure with molten Li metal is compared with the original pattern before exposure as displayed in FIG. 6 . Both measurement produced diffractogram with the same peak location indicating the structure remain the same (there is no structural change as the result of reaction with Li metal). The pellet is also observed to be very stable upon contact without thermal runaway or any exothermic reaction.
- a M-NMC622 compound having the target formula of Li(Ni 0.60 Mn 0.20 Co 0.20 )O 2 and a monolithic morphology is obtained through a double sintering process and a wet milling process running as follows:
- 1 st sintering the 1 st blend is sintered at 935° C. for 10 hours under an oxygen containing atmosphere.
- 2 nd sintering the 2 nd blend is sintered at 890° C. for 10 hours in an oxygen containing atmosphere in a roller hearth kiln (RHK). The sintered blocks are crushed by a jaw crushing equipment.
- a catholyte material EX2-CAT-A is made by mixing M-NMC622 and EX1-B (Li 3.60 Si 0.40 P 0.40 Ge 0.20 O 4 ) according to a mixing ratio of 1:1 by weight, followed by a heat treatment at 700° C. for 3 hours in an oxygen atmosphere (i.e. like air).
- EX1-B has a median particle size (D50) of 2 ⁇ m.
- a catholyte material EX2-CAT-B is obtained through a similar manner as the preparation of EX2-CAT-A except that the mixture is heated at 600° C.
- CEX3-CAT-A and CEX3-CAT-B are obtained through a similar manner as the preparation of EX2-CAT-A except that the mixture is heated at 500° C., 900° C., respectively, as displayed in Table 2.
- EX2-CAT-A, EX2-CAT-B, CEX3-CAT-A, and CEX3-CAT-B have a similar D50 at around 10.2-10.5 ⁇ m.
- the D99 values are larger at the higher co-sintering temperature.
- the D99 of EX2-CAT-A (resulting from a sintering at 700° C.) is 34.7 ⁇ m
- the D99 of CEX3-CAT-B (resulting from a co-sintering at 900° C.) is 143.0 ⁇ m.
- the coin cell characterization of EX2-CAT-A and CEX3-CAT-B as displayed in FIG. 7 shows the effect of the co-sintering temperature to the electrochemical performance.
- CEX3-CAT-B sintered at 900° C. clearly shows a lower discharge capacity comparing to EX2-CAT-A sintered at 700° C.
- co-sintering temperature lower than 600° C. is also unpreferable.
- the ionic conductivity data provided in Table 2 also demonstrate that the ionic conductivity of the catholyte depends upon the co-sintering temperature, wherein the catholyte is more conductive at a higher co-sintering temperature.
- EX2-CAT-A which results from a co-sintering prepared at 700° C. has an ionic conductivity of 10 ⁇ 5 S/cm while CEX3-CAT-A (resulting from a co-sintering at 500° C.) has an ionic conductivity of 10 ⁇ 7 S/cm, i.e. a decrease of ⁇ 100 is observed for this sample with respect to CEX3-CAT-A's ionic conductivity.
Abstract
Description
- This invention relates to a solid electrolyte (SE) for solid-state rechargeable lithium-ion batteries suitable for electric vehicle (EV) applications. The solid electrolyte according to the invention has an improved lithium ionic conductivity.
- Along with the developments of EVs, it comes also a demand for lithium-ion batteries as a possible constant source of power for such applications.
- Aside the zero-emission aspect, additional requirements rendering a battery eligible for EV applications should therefore include: high capacity, longer cycle lives, lower cost, and better safety.
- Most of the past and ongoing research on batteries usually emphasizes on the use of a liquid electrolyte, since such an electrolyte has a high lithium ionic conductivity of around 10−2 S/cm at room temperature (measured for an electrolyte composed of ethylene carbonate/dimethyl carbonate EC/DMC 1M LiPF6) and provides a good contact with electrodes through wetting. However, batteries containing liquid electrolytes imply concerns since liquid electrolytes are usually flammable.
- Solid electrolyte-based batteries are considerably safer and can be an alternative to liquid electrolyte-based batteries for the power source of electric vehicles. Since the decomposition temperature of SE is higher than the liquid electrolyte, an EV comprising such a SE-based battery, instead of a liquid electrolyte-based battery, would be safer and its battery manufacturing would also be safer. Aside from the clear advantage that a SE-based battery is much safer than a liquid electrolyte-based battery, a SE-based battery is also more compact than liquid electrolyte-based batteries, and therefore lead to higher power densities
- However, it is also true that, compared to liquid electrolyte, a SE has a lower lithium ionic conductivity (typically included between 10−7 to 10−6 S/cm). The lower lithium ionic conductivity in a SE is due to the higher migration energy of lithium ions.
- Well-known (inorganic) types of SE suitable for solid-state rechargeable lithium-ion batteries (SSB) which have been mainly explored are the La, Zr comprising garnet and the LSPO (lithium silicon phosphorus oxide) LISICON (lithium superionic conductor) electrolyte having a general formula: Li4±xSi1−xPxO4. The La, Zr comprising garnet, especially the cubic garnet (Li7La3Zr2O12), shows a high conductivity. However, those materials are expensive due to the La and Zr content. This compound also needs to be synthesized at a temperature higher than 1000° C. which is not desired because of the volatility of lithium at the high temperature. The LSPO is well-known for its high chemical and electrochemical stability, high mechanical strength, and high electrochemical oxidation voltage, making such an electrolyte a promising candidate for EV applications.
- LSPO compounds, like Li3.5Si0.5P0.5O4, have a relatively low lithium ionic conductivity. Li3.5Si0.5P0.5O4, is a solid solution of Li4SiO4 and Li3PO4 having a crystal structure of γ-Li3PO4 with orthorhombic unit cell and tetrahedrally coordinated cations. In the scope of the present invention, a solid solution (also called solid-state solution) refers to a multi-component solid-state solution as a result of a mixture of one or more solutes in a solvent. In particular, the solutes can be atoms or groups of atoms (or compounds). Such a multi-component system is considered a solution rather than a compound when the crystal structure of the solvent remains unchanged by addition of the solutes, and when the chemical components remain in a single homogeneous phase. In the system, the solvent usually is a component with the largest portion and in this case is Li3PO4. The crystal structure of the solvent component is maintained after blending whereas the other component (solute, e.g. Li4SiO4) dissolves in the solvent structure instead of forming a distinct compound having a structure that deviates from the structure of the solvent.
- In Solid State Ionics (2015), 283, 109-114, Wang, Dawei et al. studied the enhancement of lithium ionic conductivity of LSPO by an addition of Li3BO3. The highest lithium ionic conductivity was 6.5×10−6 S/cm at 20% of Li3BO3 addition compared to 3.6×10−6 S/cm for 0% addition. Another study conducted by Choi, Ji-won et al. in Solid State Ionics (2016), 289, 173-179, explored the effect of Al cation substitution in 0.7Li4SiO4+0.3Li3PO4 solid solution system. The lithium ionic conductivity of 7.7×10−6 S/cm was achieved at room temperature by the addition of 10 mol % Al.
- Sokseiha et al. in Chem. Mater. (2018), 30, 5573-5582 and Kamphorst et. al. in Solid State Ionics (1980), 1, 187-197 specify that LÍ4SÍO4-U3PO3 solid solutions have a lower conductivity than Li4GeO4—Li3PO3 teaching away from a possible substitution of Ge with Si.
- Burmakin et. al. in Russian Journal of Electrochemistry (2010), 46, No. 2, 243-246 discloses a lithium germanium phosphate solid electrolyte doped with a tetravalent cation, Zr like: Li3.75Ge0.70Zr0.05P0.25O4, Li3.50Zn0.125Ge0.75P0.25O4, respectively. The Ge content in these formulation would not allow the obtention of a solid solution in a LSPO-based SE.
- Although noticeable, these attempts to achieve a solid solution of a LSPO-based electrolyte are still below a desired threshold of at least 0.50×10−5 (or 5.0×10−6) S/cm required so that a solid-state battery made from said electrolyte is a tangible alternative to current liquid electrolyte-based batteries.
- Certainly, there is a need for improving the lithium ionic conductivity of LSPO-based electrolyte so as to render the use of solid-state batteries made from such an electrolyte more performant and therefore more attractive in the field of EV applications.
- It is therefore an object of the present invention to provide a LSPO-based SE having an improved lithium ionic conductivity whilst retaining a solid solution, which is a prerequisite for the use of such a SE in a solid-state secondary battery suitable for EV applications.
- Metallic Li can be used in the scope of the present invention as an anode of a SSB comprising the electrolyte according to the invention.
- Provided that the SE according to the present invention can be destined to be contacted to a Li metal-based anode, it must therefore be compatible to said Li metal-based anode of the SSB, meaning that the SE while contacting said anode must remain chemically stable.
- A solid electrolyte having an improved lithium ionic conductivity whilst retaining a solid solution and being chemically and thermally stable while contacting a Li metal anode is achieved by providing a solid solution according to
claim 1 which comprises a LSPO-based electrolyte comprising germanium (Ge) up to 60 mol %. A Ge doped LSPO is referenced hereunder as “LSPGO”. - If a LSPGO-based electrolyte comprises Ge of superior to 60 mol %, it comprises at least one impurity phase (i.e. Li2SiO3), and such a Li2SiO3-bearing LSPGO-based electrolyte is not a solid solution according to the present invention. A similar impurity phase is observed in Burmakin et. al. (Li2ZrO3 in this case) for a high content of Ge.
- In the framework of the present invention, it has been observed that by integrating up to 60 mol % of Ge in a solid solution of LSPO-based electrolyte it was possible to preserve said solid solution property together with a noticeable improvement of the lithium ionic conduction to a minimal value of 0.50×10−5 S/cm, which constitutes a significant contribution to what is currently known from the prior art.
- It has also been demonstrated that the electrolyte according to the present invention is stable in presence of a Li metal foil, confirming its suitability in a SSB wherein a Li metal foil is used as an anode.
- The present invention concerns the following embodiments:
- 1. —A solid solution electrolyte suitable for solid-state rechargeable lithium ion battery comprising a compound having a general formula Li(3.5+L+x)Si(0.5+s−x)P(0.5+p−x)Ge2xO4+a wherein −0.10≤L≤0.10, −0.10≤s≤0.10, −0.10≤p≤0.10, −0.40≤a≤0.40, and 0.00<x≤0.30.
- In a first aspect of the
embodiment 1, 0.05≤x≤0.30, preferably 0.10≤x≤0.30. - In a second aspect of the
embodiment 1, 0.15≤x≤0.30, preferably 0.20≤x≤0.30. - 2. —The solid solution electrolyte according to
embodiment 1 wherein said compound has a general formula: Li(3.5+x)Si(0.5−x)P(0.5−x)Ge2xO4. - 3. —The solid solution electrolyte according to the
embodiment 1 or 2, having a lithium ionic conductivity of at least 10−5 S/cm at 25° C. - 4. —The solid solution electrolyte according to any of the preceding embodiments, wherein 0.25≤x≤0.30.
- 5. —The solid solution electrolyte according to any of the preceding embodiments, having a lithium ionic conductivity measured at 25° C. superior or equal to 2.0×10−5 S/cm and inferior or equal to 3.0×10−5 S/cm, preferably superior or equal to 2.5×10−5 S/cm and inferior or equal to 3.0×10−5 S/cm.
- 6. —The solid solution electrolyte according to any of the preceding embodiments, comprising a crystal structure having an XRD pattern measured at 25° C. and at a wavelength of 1.5418 Å comprising a first peak having a first intensity and a second peak having a second intensity, said first and second peaks being present in a range of 2θ superior or equal to 27.5 and inferior or to 30.0±0.5°, said XRD pattern being furthermore free of peaks at 2θ>37.0±0.5° having an intensity superior to said first or second intensity.
- 7. —The solid solution electrolyte according to any of the preceding embodiments, comprising a crystal structure having an XRD pattern measured at 25° C. and at a wavelength of 1.5418 Å comprising a first peak having a first intensity and a second peak having a second intensity, said first and second peaks being present in a first range of 2θ superior or equal to 27.5 and inferior or to 30.0±0.5°, wherein in a second range of 2θ superior or equal to 21.0 and inferior or to 25.0±0.5° said XRD pattern has no more than three additional peaks, each of said three additional peaks having an intensity superior to said first or second intensity.
- 8. —The solid solution electrolyte according to any of the preceding embodiments, comprising a crystal structure having an XRD pattern measured at 25° C. and at a wavelength of 1.5418 Å comprising a first peak having a first intensity and a second peak having a second intensity, said first and second peaks being present in a first range of 2θ superior or equal to 27.5 and inferior or to 30.0±0.5°, wherein in a second range of 2θ superior or equal to 34.0 and inferior or to 36.0±0.5°, said XRD pattern has no more than three additional peaks, each of said three additional peaks having an intensity superior to said first or second intensity.
- 9. —A solid-state rechargeable lithium ion battery comprising the solid solution electrolyte according to any of the previous embodiments.
- 10. —A solid-state rechargeable lithium ion battery comprising a negative electrode having a Li metal-base anode contacting the solid solution electrolyte according to any of the
embodiments 1 to 9. - 11. —Use of the solid-state battery according to the
embodiment 9 or 10 in an electric vehicle, in particular in an electric car, wherein the operating voltage of said battery is superior or equal to 200 V and inferior or equal to 500 V. - 12. —A catholyte comprising the solid solution electrolyte according to any of the preceding embodiments and a cathode material having the general formula: Li1+kM′1−kO2 where M′=Ni1−x′−y′−z′Mnx′Coy′Az′ with −0.05≤k≤0.05, 0≤x′≤0.40, 0.05≤y′≤0.40, and 0≤z′≤0.05, wherein A is a doping element which is different to Li, M′ and O, said positive active material powder comprising particles having a layered R-3m crystal structure, said catholyte having a D99≤50 μm and an ionic conductivity of at least 1.0×10−6 S/m
-
FIG. 1 . Comparison of Electrochemical Impedance Spectra (EIS) for sample with various Ge dopants (x in Li(3.5+x)Si(0.5−x)P(0.5−x)Ge2xO4+a) in Example 1 and Comparative Example 1 -
FIG. 2 . Variation of lithium ionic conductivity versus the amount of Ge dopants (x in Li(3.5+x)Si(0.5−x)P(0.5−x)Ge2xO4+a) in Example 1 and Comparative Example 1FIG. 3 . Comparison of X-ray diffraction pattern of Example 1 and Comparative Example 1 -
FIG. 4 . Fourier-transform infrared spectrum of EX1-A, EX1-B, EX1-C, and Comparative Example 1 showing transmittance in (%) and wavenumber in (cm−1) -
FIG. 5 . Comparison of X-ray diffraction pattern of Comparative Examples 1 and 2 -
FIG. 6 . Comparison of X-ray diffraction pattern of LSPO (a) before exposure to molten Li metal at 250° C. and (b) after 15 minutes exposure -
FIG. 7 . Comparison of voltage vs. capacity graph of EX2-CAT-A and CEX3-CAT-B - In the following detailed description, preferred embodiments are detailed so as to enable practice of the invention. Although the invention is described with reference to these specific preferred embodiments, it will be understood that the invention is not limited to these embodiments. To the contrary, the invention includes numerous alternatives, modifications and equivalents as will become apparent from consideration of the following detailed description.
- This invention discloses a germanium bearing LSPO compounds having a general formula Li(3.5+x)Si(0.5−x)P(0.5−x)Ge2xO4+a (LSPGO) wherein 0.00<x≤0.30 and −0.40≤a≤0.40. It is a solid solution of Li4GeO4, Li3PO4, and Li4SiO4. When Ge equally substitutes Si and P in a LSPO compound, it is observed that the lithium ionic conductivity of the compound according to
claim 1 significantly increases (reaching at least 10−5 S/cm) for x values higher or equal to 0.10. Moreover, the conductivity of Li(3.5+x)Si(0.5−x)P(0.5−x)Ge2xO4+a wherein 0.10≤x≤0.30 gradually increases and it is maximized when x is 0.30. In particular, the conductivity of the compound according toclaim 1 is unexpectedly higher (higher than 2.0 10−5 S/cm) for the narrow range: 0.20<x≤0.30, in particular for 0.25≤x≤0.30. Compared to the broader range of Ge content ofclaim 1, this narrower range leads to an increase of the lithium ionic conductivity by a 1.5 to 3.0 factor, which is remarkable. - Such a high conductivity of at least 10−5 S/cm has never been reported yet for solid solution LSPO type of electrolytes.
- In addition, compatibility of the electrolyte according to the present invention with a Li metal anode.
- This invention is also inclusive of a catholyte compound made from a mixture of a NMC type of positive electrode active material and the germanium bearing LSPO compound according to the present invention.
- Both polycrystalline and monolithic NMC can be used as a positive electrode active material in the catholyte according to the present invention. A “monolithic” morphology refers here to a morphology where a secondary particle contains basically only one primary particle. In the literature they are also called single crystal material, mono-crystal material, and one-body material. The preferred shape of the primary particle could be described as pebble stone shaped. The monolithic morphology can be achieved by using a high sintering temperature, a longer sintering time, and the use of a higher excess of lithium. A “polycrystalline” morphology refers to a morphology where a secondary particle contains more than one primary particles.
- The (solid-state) catholyte material is prepared by mixing the germanium bearing LSPO compound with the NMC composition so as to produce the catholyte which is subjected to a heat treatment at 600° C.˜800° C. for 1˜20 hours under oxidizing atmosphere. In particular, the method for producing said catholyte is a co-sintering-based process wherein the germanium bearing LSPO and the NMC compositions are blended so as to provide a mixture which is then sintered.
- There are several ways to obtain each of the compositions of the germanium bearing LSPO and NMC positive electrode active material in the catholyte. Whereas the difference of the median particle sizes (D50) between the solid electrolyte and positive electrode active material in the catholyte is superior or equal to 2 μm, they can be separated using a classifier such the elbow jet air classifier (https://elcanindustries.com/elbow-jet-air-classifier/). The compositions of separate particles are measured according to the protocol disclosed in the section F) Inductively Coupled Plasma method so as to determine each of the compositions of the germanium bearing LSPO material and NMC positive electrode active material in the catholyte.
- The use of an Electron Energy Loss Spectroscopy (EELS) in a Transmission Electron Microscope (TEM) is another example for obtaining each of the compositions of the germanium bearing LSPO material and NMC positive electrode active material in the catholyte. The elements and their atomic amount can be obtained directly by measuring the EELS of cross-sectional germanium bearing LSPO particles and NMC positive electrode active material particles separately.
- The following analysis methods are used in the Examples:
- A) Electrochemical Impedance Spectroscopy (EIS)
- A cylindrical pellet is prepared by following procedure. 0.175 g of a powderous solid electrolyte compound sample is put on a mold having a diameter of 1.275 cm. A pressure of 230 MPa is applied to the mold. The pellet is sintered at 700° C. for 3 hours in oxygen atmosphere. Silver paste is painted on both sides of the pellet to have a sample configuration of Ag/pellet/Ag in order to allow EIS measurements. Standard deviation of this measurement is 2.0×10−8.
- EIS is performed using an Ivium-n-Stat instrument, a potentiostat/galvanostat with an integrated frequency response analyzer. This instrument is common to be used in the battery/fuel cell-testing to collect impedance response against frequency sweep. The measurement frequency range is from 106 Hz to 10−1 Hz. The setting point/decade is 10 and the setting voltage is 0.05V. Measurement is conducted at room temperature (at 25° C.). The lithium ionic conductivity is calculated by below equation:
-
- where L is the thickness of the pellet, A is the area of the sample, and R is the resistance obtained by the electrochemical impedance spectroscopy.
- B) X-Ray Diffraction Test
- A cylindrical pellet is prepared by following procedure. 0.175 g of a powderous solid electrolyte compound sample is put on a mold having a diameter of 1.275 cm. A pressure of 230 MPa is applied to the mold. The pellet is sintered at 700° C. for 3 hours in oxygen atmosphere.
- The X-ray diffraction pattern of the pellet sample is collected with a Rigaku X-Ray Diffractometer (D/MAX-2500/PC) using a Cu Kα radiation source emitting at a wavelength of 1.5418 Å. The instrument configuration is set at: 1° Soller slit (SS), 1° divergence slit (DS) and 0.15 mm reception slit (RS). Diffraction patterns are obtained in the range of 10-70° (2θ) with a scan speed of 4° per a minute. Obtained XRD patterns are analyzed by the Rietveld refinement method using X'Pert HighScore Plus software. The software is a powder pattern analysis tool with reliable Rietveld refinement analysis results.
- C) Fourier-Transform Infrared (FTIR) Spectrometry
- FTIR transmission spectrum for the LSPGO powder is collected using Thermo Scientific FTIR Spectrometer (Nicolet iS 50) in the wave number range of 1200 to 500 cm−1, with a resolution of 4 cm−1, and scan cycle of 32 scan.
- D) Particle Size Distribution
- The catholyte powder samples used in the particle-size distribution (psd) measurements are prepared by hand grinding the catholyte powder samples using agate mortar and pestle. The psd is measured by using a Malvern Mastersizer 3000 with Hydro MV wet dispersion accessory after having dispersed each of the catholyte powder samples in an aqueous medium. In order to improve the dispersion of the catholyte powder, sufficient ultrasonic irradiation and stirring is applied, and an appropriate surfactant is introduced. D50 and D99 are defined as the particle size at 50% and 99% of the cumulative volume % distributions obtained from the Malvern Mastersizer 3000 with Hydro MV measurements.
- E) Coin Cell Test
- For the preparation of a positive electrode, a catholyte containing 0.16 g of NMC, 0.03 g conductor (Super P), and 0.125 g of 8 wt % PVDF binder are mixed in NMP solvent using a planetary centrifugal mixer (Thinky mixer) for 20 minutes. The homogenized slurry is spread on one side of an aluminum foil using a doctor blade coater with a 15 μm gap. The slurry-coated foil is dried and punched as 8 mm diameter circular shape. A Swagelok cell is assembled in an argon-filled glove box with the configuration of positive electrode, separator having a diameter of 13 mm, and lithium foil having a diameter of 11 mm as a negative electrode. 1M LiPF6 in EC/DMC (1:1 wt %) is used as electrolyte. Each cell is cycled at 25° C. using automatic battery cycler Wonatech-WBCS3000. The coin cell testing at 0.1 C in the 4.3˜2.5V/Li metal window range.
- F) Inductively Coupled Plasma (ICP)
- The composition of a positive electrode active material, a solid electrolyte, and a catholyte is measured by the inductively coupled plasma (ICP) method using an Agillent ICP 720-ES. 1 gram of a powder sample is dissolved into 50 mL high purity hydrochloric acid (at least 37 wt % of HCl with respect to the total amount of solution) in an Erlenmeyer flask. The flask is covered by a watch glass and heated on a hot plate at 380° C. until complete dissolution of the powder. After being cooled to room temperature, the solution from the Erlenmeyer flask is poured into a 250 mL volumetric flask. Afterwards, the volumetric flask is filled with deionized water up to the 250 mL mark, followed by a complete homogenization. An appropriate amount of solution is taken out by a pipette and transferred into a 250 mL volumetric flask for a second dilution, where the volumetric flask is filled with internal standard and 10% hydrochloric acid up to the 250 mL mark and then homogenized. Finally, this solution is used for ICP measurement.
- The invention is further exemplified in the examples below. The following samples were prepared:
- CEX1 having a general formula Li3.50Si0.50P0.60O4 was prepared by the following steps:
- 1) Mixing: Li2CO3, SiO2, and (NH4)2HPO4 with total weight of around 6.0 g according to the corresponding molar ratio were put on a 250 ml bottle with 140 ml of deionized water and each 100 g of Y doped ZrO2 balls having 3, 5, and 10 mm diameter. The bottle was rotated in a conventional ball mill equipment with 300 RPM for 24 hours. The homogeneously mixed slurry was dried at 90° C. for 12 hours.
- 2) Calcination: the dried mixture was calcined at 900° C. for 6 hours in Ar atmosphere.
- 3) Pulverization: 1.4 g of calcined powder was put on a 45 ml bottle with 30 ml of acetone and 3.4 g of Y doped ZrO2 balls having a dimeter of 1 mm. The bottle was rotated in a conventional ball mill equipment with 500 RPM for 6 hours. The pulverized powder was dried at 70° C. for 6 hours.
- 4) Sintering: The dried powder was sintered at 700° C. for 3 hours in oxygen atmosphere to get the final LSPO solid electrolyte compound.
- Ge doped LSPO samples having a general formula Li(3.5+x)Si(0.5−x)P(0.5−x)Ge2xO4 were prepared in the same manner as CEX1 except that different amount of GeO2 was added and the amount of Li2CO3, SiO2, and (NH4)2HPO4 were adjusted in the mixing step according to the target molar ratios. EX1-A, EX1-B, EX1-C, EX1-D, EX1-E, and EX1-F had the x of 0.05, 0.10, 0.15, 0.20, 0.25, and 0.30, respectively.
- S doped LSPO samples CEX2-A1 and CEX2-A2 having a general formula Li(3.5−30 x)Si(0.5−x)P(0.5−x)S2xO4+a were prepared in the same manner as samples in the Example 1 except that different amount of Li2SO4 was added instead of GeO2. CEX2-A1 and CEX2-A2 had the x of 0.05 and 0.10, respectively.
- Ga doped LSPO sample CEX2-B having a general formula Li(3.5−30 x)Si(0.5−x)P(0.5−x)Ga2xO4+a was prepared in the same manner as samples in the Example 1 except that Ga2O3 was added instead of GeO2. CEX2-B had the x of 0.05.
- To examine the stability of electrolyte with Li metal, LSPGO samples of EX1-B is directly contacted with molten Li metal under Ar atmosphere. To this end, pellet of EX1-B is made by pressing 0.175 g of EX1-A powder under 2349.7 kgf/cm2 pressure, followed by a sintering at 700° C. for 3 h under 02 atmosphere. A stripe of Li foil is placed on a stainless-steel plate heated on 250° C. hot plate (under controlled non-oxidizing atmosphere). The obtained molten Li is directly poured on the prepared EX1-B pellets and the pellets are observed for 15 minutes. This explanatory experiment is conducted in a glove box with Ar atmosphere. The pellet is visually observed/monitored so as to detect an eventual thermal runaway and the structure is examined using X-Ray Diffraction.
- Results
-
TABLE 1 List of Examples and Comparative Examples with their properties Sample Conductivity Volume Examples ID Composition x - (S/cm) (As) Comparative CEX1 Li3.50Si0.50P0.50O4 0.00 4.4 × 10−6 324.15 example 1 Example 1 EX1-A Li3.55Si0.45P0.45Ge0.10O4 0.05 7.2 × 10−6 327.11 EX1-B Li3.60Si0.40P0.40Ge0.20O4 0.10 1.0 × 10−5 329.96 EX1-C Li3.65Si0.35P0.35Ge0.30O4 0.15 1.4 × 10−5 332.93 EX1-D Li3.70Si0.30P0.30Ge0.40O4 0.20 1.5 × 10−5 335.73 EX1-E Li3.75Si0.25P0.25Ge0.50O4 0.25 2.7 × 10−5 338.83 EX1-F Li3.75Si0.25P0.25Ge0.50O4 0.30 2.4 × 10−5 340.76 Comparative CEX2- Li3.35Si0.45P0.45S0.10O4 0.05 2.3 × 10−6 324.27 A1 example 2 CEX2- Li3.20Si0.40P0.40S0.20O4 0.10 3.9 × 10−7 323.58 A2 CEX2-B Li3.65Si0.45P0.45S0.10O4 0.05 3.5 × 10−6 No solid solution (*x in CEX1 and EX1-A to EX1-F with formula Li(3.5x)Si(0.5-x)P(0.5-x)Ge2×04, in CEX2-A1 and CEX2-A2 with formula Li(3.5-3x)Si(0.5-x)P(0.5-x)S2xO4, and in CEX2-B with formula Li(3.5+303x)Si(0.5-x)P(0.5-x)Ga2xO4.) - Enhanced Conductivity of the LSPGO According to the Present Invention
- Table 1 summarizes the list of example and comparative example samples. It can be seen that LSPGO samples at x=0.05-0.30 (EX1-A to EX1-F) have higher lithium ionic conductivity than the LSPO sample (CEX1). As for S and Ga bearing LSPO (CEX2-A1, CEX2-A2, and CEX2-B), the lithium ionic conductivities are lower.
-
FIG. 1 shows a typical Nyquist plot from EIS measurement Li(3.5+x)Si(0.5−x)P(0.5−x)Ge2xO4+a (x=0.00 to 0.30). The plot is composed of real part of impedance in X axis and imaginary part in Y axis. High frequency measurement appears on the left side of the graph forms a semicircle that is followed by a low angle spike as the result of the low frequency measurement. The semicircle formation corresponded to the lithium conduction in SE. The lithium ionic conductivity of CEX1 is 4.4×10−6 at room temperature that is comparable with the earlier published works on LSPO. The reduction of the semicircle diameter with the higher Ge amount indicating lower resistance of sample suggesting a better conductivity. -
FIG. 2 shows the improvement of lithium ionic conductivity where the value increases proportionally with more Ge in the structure. The highest lithium ionic conductivity is 2.7×10−5 at x=0.25 which is about 6 times of CEX1. When x is 0.30, the value reduces to 2.4×10−5, concluding that 0.25 is an optimal concentration. - Retention of the Solid Solution in the Ge-Doped LSPO According to the Invention
-
FIG. 3 shows the XRD patterns of CEX1 (undoped electrolyte) and EX1-A to EX1-F. It is observed that Ge bearing LSPO samples have a single LISICON phase without impurity, demonstrating that Ge is well doped. In all graphs, the γ-Li3PO4 structure is maintained, indicated by the characteristic double peak at 28°-29° representing (121) and (200) planes as well as four consecutive peaks at 34°-36° correspond to (220), (131), (211), and (002) planes. The shifted peak positions to the left related with the larger crystal volume showed in Table 1. The observed single phase also acts as an evidence of solid solution formation for the Ge bearing LSPO. - Additionally, FTIR measurement is displayed in
FIG. 4 with the vibration bands of P—O, Si—O, and Ge—O marked. The vibration bands at 580 cm−1, 910 cm−1, and around 1050 cm−1 correspond to the vibration modes of tetrahedron P—O while band in area of 985-1005 cm−1 corresponds to the vibration modes of Si—O, also in tetrahedral structure. All bands show transmittance signal increase along with the addition of Ge in the structure. On the other hand, transmittance of 790 cm−1 band which corresponds to Ge—O vibration decreases with the more Ge in the structure. It is concluded that the atomic substitution of Ge successfully occurred at Si and P sites without changing the structure. This observation matches with that of XRD where the structure of LSPO is maintained upon doping. - XRD of CEX2 are compared with CEX1 in
FIG. 5 . The S bearing LSPO structure (CEX2-A) is still well maintained while Ga bearing LSPO structure (CEX2-B) has multiple impurity peaks marked with (*) in the graph. This indicating Ga is not easy to be doped in the LSPO system and solid solution is failed to form for CEX2-B. - Chemical Stability of the LSPGO with a Li Metal Foil
- Chemical stability of LSPGO with Li metal was examined through a direct contact with the molten Li metal.
- LSPGO pellet XRD diffraction pattern after exposure with molten Li metal is compared with the original pattern before exposure as displayed in
FIG. 6 . Both measurement produced diffractogram with the same peak location indicating the structure remain the same (there is no structural change as the result of reaction with Li metal). The pellet is also observed to be very stable upon contact without thermal runaway or any exothermic reaction. - A M-NMC622 compound having the target formula of Li(Ni0.60Mn0.20Co0.20)O2 and a monolithic morphology is obtained through a double sintering process and a wet milling process running as follows:
- 1) Co-precipitation: mixed transition metal hydroxides with D50 of around 4 μm are prepared by the process described in KR101547972B1 (from
page 6line 25 to page 7 line 32). - 2) 1st blending: to obtain a lithium deficient sintered precursor, Li2CO3 and the co-precipitation product are homogenously blended with a Li/M′ ratio of 0.85 in a Henschel mixer for 30 minutes so as to obtain a 1st blend.
- 3) 1st sintering: the 1st blend is sintered at 935° C. for 10 hours under an oxygen containing atmosphere. The product obtained from this step is a powderous lithium deficient sintered precursor with Li/M′=0.85.
- 4) Blending: the lithium deficient sintered precursor is blended with LiOH.H2O to correct the Li stoichiometry to Li/M′=1.01. The blending is performed in a mixer for 30 minutes so as to obtain a 2nd blend.
- 5) 2nd sintering: the 2nd blend is sintered at 890° C. for 10 hours in an oxygen containing atmosphere in a roller hearth kiln (RHK). The sintered blocks are crushed by a jaw crushing equipment.
- 6) Wet milling: To break the agglomerated intermediate particles into monolithic primary particles, a wet ball milling process is applied. 5 L bottle is filled with 1 L of deionized water, 5.4 kg ZrO2 balls, and 1 kg of 2nd sintering product from
process number 5. The bottle is rotated on a commercial ball mill equipment. - 7) Healing firing step (3rd sintering): The wet milled product is heated at 750° C. for 10 hours under oxygen containing atmosphere in a furnace. The sintered compound is sieved.
- A catholyte material EX2-CAT-A is made by mixing M-NMC622 and EX1-B (Li3.60Si0.40P0.40Ge0.20O4) according to a mixing ratio of 1:1 by weight, followed by a heat treatment at 700° C. for 3 hours in an oxygen atmosphere (i.e. like air). EX1-B has a median particle size (D50) of 2 μm.
- A catholyte material EX2-CAT-B is obtained through a similar manner as the preparation of EX2-CAT-A except that the mixture is heated at 600° C.
- CEX3-CAT-A and CEX3-CAT-B are obtained through a similar manner as the preparation of EX2-CAT-A except that the mixture is heated at 500° C., 900° C., respectively, as displayed in Table 2.
-
TABLE 2 Particle size distribution and ionic conductivity of EX2 and CEX3 material Co-sintering Ionic First discharge Sample temperature D50 D99 conductivity capacity ID* (° C.) (μm) (μm) (S/cm) (mAh/g) EX2-CAT- A 700 10.2 34.7 1 × 10−5 176.4 EX2-CAT- B 600 10.3 31.0 2 × 10−6 _** CEX3-CAT- A 500 10.4 28.1 1 × 10−7 _** CEX3-CAT- B 900 10.5 143.0 9 × 10−4 133.8 *-CAT- stands for “catholyte”. ** - : not measured. - The results of the size distribution measurement as displayed in the Table 2 show that EX2-CAT-A, EX2-CAT-B, CEX3-CAT-A, and CEX3-CAT-B have a similar D50 at around 10.2-10.5 μm. However, the D99 values are larger at the higher co-sintering temperature. For instance, the D99 of EX2-CAT-A (resulting from a sintering at 700° C.) is 34.7 μm while the D99 of CEX3-CAT-B (resulting from a co-sintering at 900° C.) is 143.0 μm. The coin cell characterization of EX2-CAT-A and CEX3-CAT-B as displayed in
FIG. 7 shows the effect of the co-sintering temperature to the electrochemical performance. Here, CEX3-CAT-B sintered at 900° C. clearly shows a lower discharge capacity comparing to EX2-CAT-A sintered at 700° C. - On the other hand, co-sintering temperature lower than 600° C. is also unpreferable. The ionic conductivity data provided in Table 2 also demonstrate that the ionic conductivity of the catholyte depends upon the co-sintering temperature, wherein the catholyte is more conductive at a higher co-sintering temperature. EX2-CAT-A which results from a co-sintering prepared at 700° C. has an ionic conductivity of 10−5 S/cm while CEX3-CAT-A (resulting from a co-sintering at 500° C.) has an ionic conductivity of 10−7 S/cm, i.e. a decrease of ×100 is observed for this sample with respect to CEX3-CAT-A's ionic conductivity.
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