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 PDF

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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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ByoungWoo Kang
Seung-Jun WOO
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Umicore NV SA
Academy Industry Foundation of POSTECH
Umicore Korea Ltd
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Academy Industry Foundation of POSTECH
Umicore Korea Ltd
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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
    • H01M10/00—Secondary cells; Manufacture thereof
    • H01M10/05—Accumulators with non-aqueous electrolyte
    • H01M10/052—Li-accumulators
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • 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
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • 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
    • H01M10/056—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
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M4/00—Electrodes
    • H01M4/02—Electrodes composed of, or comprising, active material
    • 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
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M4/00—Electrodes
    • 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
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M4/00—Electrodes
    • 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
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M4/00—Electrodes
    • 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
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M4/00—Electrodes
    • 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
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M4/00—Electrodes
    • 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
    • H01M4/52—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
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M4/00—Electrodes
    • H01M4/02—Electrodes composed of, or comprising, active material
    • H01M4/62—Selection of inactive substances as ingredients for active masses, e.g. binders, fillers
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • 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
    • H01M50/431—Inorganic material
    • H—ELECTRICITY
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    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M4/00—Electrodes
    • H01M4/02—Electrodes composed of, or comprising, active material
    • H01M2004/026—Electrodes composed of, or comprising, active material characterised by the polarity
    • H01M2004/028—Positive electrodes
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M2220/00—Batteries for particular applications
    • H01M2220/20—Batteries in motive systems, e.g. vehicle, ship, plane
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M2300/00—Electrolytes
    • H01M2300/0017—Non-aqueous electrolytes
    • H01M2300/0065—Solid electrolytes
    • H01M2300/0068—Solid electrolytes inorganic
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M2300/00—Electrolytes
    • H01M2300/0017—Non-aqueous electrolytes
    • H01M2300/0065—Solid electrolytes
    • H01M2300/0068—Solid electrolytes inorganic
    • H01M2300/0071—Oxides
    • Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
    • 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.

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