Precursor of Li-ion cathode material, the preparation method thereof and Li-ion cathode material

Abstract

Li-ion cathode materials with improved performance characteristics and precursors to prepare such materials are disclosed. The precursors consist of complex, mixed alkali transition metal oxides of the formula Li.sub.xA.sub.y(Mn.sub.aNi.sub.bM.sub.c)O.sub.2+d, where M represents one or more selected from transition metal elements beside Ni and Mn, and the groups IIA and IIIA elements of the periodic table, x is between 1 and 1.4, y is between 0.1 and 0.5, and x+y is between 1.1 and 1.5, a+b+c=1, the value of d depends on the proportions and average oxidation states of the cation elements Li, A, Mn, Ni and M such that the combined positive charge of the cation elements is balanced by the number of oxygen anions, A represents one or more elements selected from Na, K and Cs. The Li-ion cathode materials are produced by exchange of element(s) A for Li under mild conditions to limit the degree of structural reorganization that occurs during the reaction.

Claims

1. A method for preparing a precursor to a Li-ion cathode material containing at least Li, A, Ni and Mn and layered phase Li.sub.2MnO.sub.3 with a composition of Li.sub.xA.sub.y(Mn.sub.aNi.sub.bM.sub.c)O.sub.2+d, where M represents one or more elements selected from transition metal elements beside Ni and Mn, and the groups IIA and IIIA elements of the periodic table, x is between 1 and 1.4, y is between 0.1 and 0.5, and x+y is between 1.1 and 1.5, a+b+c=1, the value of d depends on the proportions and average oxidation states of the cation elements Li, A, Mn, Ni and M such that the combined positive charge of the cation elements is balanced by the number of oxygen anions, and A represents one or more elements selected from Na, K and Cs comprising: (1) dissolving soluble salts of Ni, Mn and M in water to obtain a solution of mixed cations; (2) combining the solution of mixed cations with a basic solution of lithium hydroxide or lithium carbonate to obtain a solid precipitate; and (3) mixing the solid precipitate with a combination of lithium carbonate and/or lithium hydroxide and at least one of other carbonates and/or hydroxides of Na, K, and/or Cs, and then firing the mixture.

2. The method of claim 1 wherein M represents one or more elements selected from B, Mg, Al, Ti, Fe, and Co.

Description

BRIEF DESCRIPTION OF THE DRAWINGS

(1) FIG. 1 shows x-ray diffraction data for a baseline Li.sub.1.2Ni.sub.0.2Mn.sub.0.6O.sub.2 and several analogues of identical nominal composition synthesized via ion-exchange chemistry from precursors with different alkali substitutions.

(2) FIG. 2 is graph comparing specific energy (mWh/g) and resistance (mOhm) of various baseline materials to their analogues synthesized by ion-exchange, which are plotted to the right of the relevant baseline.

(3) FIG. 3 is graph showing the C/3 rate specific energy and resistance determined from current interrupts at 80% DOD for a series of low (0.1 mol equivalent) and high (1.0 mol equivalent) level substituted IE-HENM materials compared to a baseline material of the same final composition.

(4) FIG. 4 is a plot demonstrating the relative cycling stability in Lithium metal coin cells for Baseline HE-NM and various chemical (IE) ion-exchange synthesized materials.

(5) FIG. 5 shows comparisons of voltage profile evolution over 72 cycles for two pairs of baseline vs. IE HE-NM materials.

(6) FIG. 6 is a plot of relative cycling stability in full Li-ion coin cells using a graphite anode for Baseline HE-NM and ion-exchange synthesized materials from precursors of differing Na-substitution levels.

DETAILED DESCRIPTION

(7) The present invention relates to a precursor of Li-ion cathode materials with a composition of Li.sub.xA.sub.y(Mn.sub.aNi.sub.bM.sub.c)O.sub.2+d, where x is between 1 and 1.4, y is between 0.1 and 0.5, and x+y is between 1.1 and 1.5, a+b+c=1, the value of d depends on the proportions and average oxidation states of the cation elements Li, A, Mn, Ni and M such that the combined positive charge of the cation elements is balanced by the number of oxygen anions. The precursor contains at least Li, A, Ni, and Mn, that is to say, the values of a and b are more than 0, and the value of c may be equal to 0. In a preferred embodiment, y is between 0.1 and 0.2, and x+y is between 1.1 and 1.3.

(8) In the precursor of the present invention, large cation A is selected from one or more of Na, K, and Cs. Preferably, A is selected from even larger cations such as K and/or Cs.

(9) In the precursor of the present invention, element M represents one or more selected from transition metal elements beside Ni and Mn, and the groups IIA and IIIA elements of the periodic table, and preferably selected from B, Mg, Al, Ti, Fe, and Co.

(10) In the present invention, the precursor can be prepared via a two-step co-precipitation/solid state synthesis process. In particular, the preparation method of the precursor of the present invention comprises the following steps: (1) dissolving soluble salts of Ni, Mn and M in water to obtain a solution of mixed cations, wherein M represents one or more elements selected from the transition metals beside Ni and Mn, and the groups IIA and IIIA elements of the periodic table; (2) combining the solution of mixed cations with a basic solution of lithium hydroxide or lithium carbonate to obtain a solid precipitate; and (3) mixing the solid precipitate with a combination of lithium and at least one of other alkali metal carbonates and/or hydroxides, and then firing the mixture.

(11) In one embodiment, the method starts with the selection of the ratio of metal oxides to be used in the final active material. These are generally a mixture of transition metals which can include nickel, manganese, and other elements. To achieve the best mixing of these metals, they are weighed out, and dissolved in water as the sulfate salts. This solution of the mixed sulfate salts is slowly pumped into a stirred reactor pre-charged with a hot aqueous solution of dilute lithium hydroxide or lithium carbonate. Simultaneously, an aqueous solution of lithium hydroxide or lithium carbonate is pumped in to cause the simultaneous co-precipitation of the mixed hydroxides and/or carbonates. In the case of lithium hydroxide is to be used, the reaction proceeds according to the following equation:
MSO.sub.4(aq)+2LiOH(aq).fwdarw.M(OH).sub.2+Li.sub.2SO.sub.4(aq)

(12) The mixture is agitated and heated for a period of time and then allowed to cool and settle. The insoluble hydroxides and/or carbonates are washed and vacuum filtered. The filter cake is heated in a vacuum oven to dry it and then ground finely and sieved to give a dry metal hydroxide and/or carbonate precursor.

(13) This precursor is then mixed with an appropriate amount of a combination of lithium and other alkali metal carbonates and/or hydroxides. This mixture is calcined twice, with an optional grinding step in between to improve mixing and formation of the desired crystalline structure.

(14) The Li-ion cathode material of the present invention is synthesized by ion-exchange from the precursor of the present invention. This ion-exchange process may be carried out by treatment of the precursor with a liquid phase reagent containing mobile Li.sup.+ ions. For example, the use of an excess of an alcoholic lithium bromide solution proceeds according to the following equation:
Li.sub.1.2(x+y+z)Na.sub.xK.sub.yCs.sub.zMO.sub.2+Li.sup.++Br.sup..fwdarw.Li.sub.1.2MO.sub.2+xNaBr+yKBrzCsBr

(15) The alkali metal oxides are refluxed in the alcoholic lithium bromide solution. By picking the appropriate alcohol, the lithium bromide has a higher solubility than the other alkali metal bromides, which will then precipitate, thus driving the reaction to the right. The reaction products are allowed to cool, washed to remove excess bromide salts, and then vacuum dried. Preferably, the washing step is conducted using methanol and/or water. The product so derived can then be used as is in an electrochemical cell or thermally annealed first at a temperature below the melting point of the product. This material is then ground and sieved to obtain a Li-ion cathode material suitable for use in conventional Li-ion electrode manufacturing processes.

(16) A number of compositional variables relating to the present invention have been explored at Farasis. They include the transition metal content and ratios, the total alkali metal to transition metal ratio, and other alkali metal substituent and substituent levels for lithium. A simplified notation is used in this write up to describe the various compositions. Details and several relevant examples are given below: HEHigh Energy NCM and indicates that the final cathode material has a greater level of Li stoichiometrically than other metals, i.e. it is lithium rich (e.g. Li.sub.1.2(M).sub.1.0O.sub.2+d). IEThe final cathode material was prepared via an ion-exchange reaction. (Na0.1)0.1 mol Na substitution for lithium in the ion-exchange precursor material. Baseline HE-NM1.0Li.sub.1.2(Ni.sub.0.25Mn.sub.0.75).sub.1.0O.sub.2 Conventional solid state synthesis, no ion-exchange, Ni and Mn transition metals, Transition metal to alkali metal ratio 1.0/1.2 Baseline HE-NCM0.8Li.sub.1.2(Ni.sub.0.219Co.sub.0.125Mn.sub.0.656).sub.0.8O.sub.2 Conventional synthesis, no ion-exchange, Ni, Co and Mn transition metals, transition metal to alkali metal ratio 0.8/1.2 Baseline HE-NCM1.0Li.sub.1.2(Ni.sub.0.219Co.sub.0.125Mn.sub.0.656).sub.1.0O.sub.2 Transition metal to alkali metal ratio 1.0/1.2, no ion-exchange (Na1.0) IE-HE-NM1.0Li.sub.1.2(Ni.sub.0.25Mn.sub.0.75).sub.1.0O.sub.2 Ion exchange synthesis from Na.sub.1.0Li.sub.0.2(Ni.sub.0.25Mn.sub.0.75).sub.1.0O.sub.2, Only Ni and Mn transition metals, Transition metal to alkali metal ratio 1.0/1.2, 1.0 mol Na substitution for lithium in precursor. (K0.1) IE-HE-NM0.8Li.sub.1.2(Ni.sub.0.25Mn.sub.0.75).sub.0.8O.sub.2 Ion exchange synthesis from K.sub.0.1Li.sub.1.1(Ni.sub.0.25Mn.sub.0.75).sub.0.8O.sub.2, Only Ni and Mn transition metals, Transition metal to alkali metal ratio 0.8/1.2, 0.1 mol K substitution for lithium in precursor.

(17) Table 1 lists a selection of precursor- and ion-exchanged materials synthesized that are representative of the present invention. Additionally, several compositions labelled Baseline have been synthesized according to conventional solid state cathode material synthesis methods (i.e., without ion-exchange) to serve as comparative examples to demonstrate the advantages of the present invention.

(18) TABLE-US-00001 TABLE 1 Precursor Composition Li A Ni Co Mn Ion Exchange Method(s) Identifier Baseline 1.20 0.18 0.10 0.52 No ion-exchange Baseline HE-NCM0.8 A = Na 0.20 1.00 0.18 0.10 0.52 LiBr in refluxing 1-hexanol (Na1.0) IE-HE-NCM0.8 Baseline 1.2 0.20 0.00 0.60 No ion-exchange Baseline HE-NM0.8 A = Na 0.20 1.00 0.20 0.00 0.60 LiBr in refluxing 1-hexanol (Na1.0) IE-HE-NM0.8 A = K 0.20 1.00 0.20 0.00 0.60 LiBr in refluxing 1-hexanol (K1.0)IE-HE-NM0.8 Baseline 1.20 0.00 0.25 0.00 0.75 No ion-exchange Baseline HE-NM1.0 A = Na 0.20 1.00 0.25 0.00 0.75 LiBr in refluxing 1-hexanol (Na1.0)IE-HE-NM1.0 A = K 0.20 1.00 0.25 0.00 0.75 LiBr in refluxing 1-hexanol (K1.0)IE-HE-NM1.0 X = Cs 0.20 1.00 0.25 0.00 0.75 LiBr in refluxing 1-hexanol (Cs1.0)IE-HE-NM1.0 A = Na 0.20 1.00 0.25 0.00 0.75 LiBr in refluxing 1-hexanol (Na1.0)IE-HE-NM1.0 (fired) A = Na 0.20 1.00 0.25 0.00 0.75 LiBr in refluxing 1-hexanol (Na1.0)IE-HE-NM1.0 (washed/fired) A = Na 0.20 1.00 0.25 0.00 0.75 LiBr in refluxing 1-hexanol (Na1.0)IE-HE-NM1.0 (AlF.sub.3 coated)

(19) Hereinafter, the present invention will be described by way of examples. However, it will be recognized by the skilled in the art that these examples are provided for the purpose of illustration rather than limitation to the range of the present invention.

Example 1

(20) The precursor sodium-lithium-transition metal oxide Li.sub.0.2Na.sub.1.0Mn.sub.0.6Ni.sub.0.2O.sub.2+d was prepared by ball-milling sodium and lithium carbonates together with a co-precipitated Mn.sub.0.75Ni.sub.0.25CO.sub.3 precursor; the mixture of starting materials was analyzed by TGA-DTA and demonstrated that the majority of carbonate decomposition occurs around 500 C., with slow continued mass loss at higher temperatures. The solid state reaction was carried out by heating the powder mixture at 850 C. for 6 h (heating rate: 1.5 C./min), regrinding, and firing a second time at 850 C. for 12 h. Based on the mass difference of starting materials and products the value of d can be estimated as approximately 0.1-0.2. The product was ground and sieved to furnish about 20 g of the desired precursor as a black powder. The same procedure was used to synthesize all of the precursor materials described in Table 1.

Example 2

(21) The precursor sodium-lithium-transition metal oxide Li.sub.0.2Na.sub.1.0Mn.sub.0.6Ni.sub.0.2O.sub.2+d, prepared as described in Example 1 was ion-exchanged by stirring 10 g of the precursor in a refluxing solution of 17.4 g LiBr in 80 g of 1-hexanol (approximate temperature 160 C.). The mixture was cooled and filtered to isolate the product as a black powder. The crude product was washed with sufficient methanol and water to remove residual bromide salts and allowed to dry, then ground and sieved to obtain 6 g of final product as a black powder. Powder X-ray diffraction patterns for representative materials after ion exchange (A1.0)IE-HE-NM1.0 for A=Na, K and Cs are displayed in FIG. 1. The results indicate that all of the materials have similar d-space shifts and line broadening features associated with the formation of the high performance IE-HENCM cathode materials. Similar results were observed for the IE materials made using a low level of substitution of large cation.

Example 3

(22) The Li-ion cathode material prepared according to Example 2 can optionally be thermally annealed to improve its performance characteristics. A sample of the powder is annealed at approximately 500 C. for 12 h and allowed to cool naturally. Data for materials treated in this manner are presented in FIG. 2 with the label fired appended to their identifier.

Example 4

(23) As is known in the art, surface treatment of Li-ion cathode materials with various oxides and fluorides can lead to improved performance in electrochemical cells derived from such materials. As an example of this technique applied to ion-exchange products described above, the (Na1.0)IE-HE-NM1.0 material was treated as follows: A suitably sized reactor was charged with 67 g of Al(NO.sub.3).sub.3.9H.sub.2O and 10 L of deionized water and the mixture was stirred until all solids dissolved. 1 kg of the ion-exchanged product was then added to the reactor and the mixture was stirred for 5 min. Next, a solution of 20 g NH.sub.4F in 200 mL deionized water was slowly added and the bath temperature of the reactor was maintained at 65 C. for 5 h. The reactor charge was allowed to cool and the crude product was isolated by filtration and thoroughly washed with deionized water. This crude material was annealed in an Ar atmosphere at 400 C. for 5 h to furnish the final product.

Example 5

(24) The evaluation for the electrochemical performance of the cathode materials is performed in Lithium metal coin cells. The ion-exchanged products were processed into laminate electrodes by mixing with carbon black, PVDF binder, and NMP solvent to create a slurry that is then coated onto Al foil current collector. The composite film composition was 82% active material, 8% PVDF binder, and 8% carbon black for all materials tested. Coin cells (2032) were built with Li metal counter electrodes, microporous polyolefin film separator, and 1.2 M LiPF.sub.6 in EC/EMC (3:7) electrolyte. The coin cells are charged to 4.9V vs Lithium in the first cycle and cycled between 2.0 V and 4.55 V in subsequent cycles. The first (formation) cycle was performed at a C/20 rate (100% charge in 20 hours) while subsequent cycling was carried out at C/5 charge rate and a C/3 discharge rate; a C/20 charge and C/20 discharge cycle are inserted in every 25 cycles for reference purposes. During discharge, 30 second current interrupts are used every 5 minutes to be used to calculate the resistance of the cells.

(25) From the electrochemical testing the specific energy for the first discharge and the average cell resistance were determined. For Li-ion cathode materials derived from precursors with a full equivalent of alkali substitution this data is plotted in FIG. 2. As can be seen from this Figure, the ion-exchanged materials exhibited higher specific energy and lower impedance than the corresponding baseline materials, excepting the (Cs1.0)IE-HE-NM1.0 sample. Similar data comparing compounds of different alkali substitution levels are presented in FIG. 3. For all large alkali substitutions tested, the lower levels of substitution produced cathode materials with superior performance relative to high levels of alkali substitution or the baseline. The results clearly show that the same or better performance benefits associated with high levels of substitution and ion-exchange can be achieved while decreasing the amount of ion-exchange necessary by at least 90% with corresponding reductions in processing costs.

(26) FIG. 4 shows a set of typical Lithium coin cell cycling data for a series of Na-substituted precursor-based IE materials compared to a baseline for the HE-NCM0.8 composition. The amount of Na substitution in the precursor is indicated on the chart. In addition to a higher energy density, the ion-exchanged cathodes consistently exhibited greater cycling stability relative to the baseline compositions. Also the greater difference in capacity between C/20 and C/3 rates for the baseline compositions is another indication of the lower impedance and higher rate capability of the IE materials. Finally, it can be found that the best cycling, highest performance cathode materials are those made from IE precursors using low levels of Na substitution (Na=0.2 or 0.1 mol equivalent).

(27) FIG. 5 shows comparisons of select discharge voltage curves, with Cycle 1 and Cycle 72 as end-members, for two sets of Baseline vs. IE-synthesized materials, HE-NCM0.8 vs, (Na0.1)IE-HE-NCM0.8 and HE-NM1.0 vs. (Na0.1)IE-HE-NM1.0. The change in the voltage profiles is associated with ongoing structural changes during cycling that are characteristic of the HE-NCM materials as a class. Based on the Figure, it can be seen that the magnitude of the decrease of the average cell voltage was significantly less for the ion exchange materials relative to the corresponding baseline materials across cathodes with both transition metal compositions.

Example 6

(28) In addition to evaluating the materials in coin cells with Li-metal anodes, the same electrodes were also evaluated against more commercially relevant graphite anodes. FIG. 6 shows data for secondary Li-ion cells made from cathode materials derived from precursors with three different Na-substitution levels. Save for the anode composition, the cell construction and cycling conditions were otherwise identical to those of Example 5. The performance reflected what we observed in lithium half cells with the ion exchange cells exhibiting both higher utilization and energy, lower impedance, and better cycle life than the corresponding baseline material. In particular, the cathode materials derived from precursors with low levels of alkali substitution exhibited better performance than the higher levels of substitution and also exhibited better performance than the baseline material made without an ion-exchange step.