Metallate electrodes

Abstract

The invention relates to electrodes that contain active materials of the formula: A.sub.aM.sub.bX.sub.xO.sub.y wherein A is one or more alkali metals selected from lithium, sodium and potassium; M is selected from one or more transition metals and/or one or more non-transition metals and/or one or more metalloids; X comprises one or more atoms selected from niobium, antimony, tellurium, tantalum, bismuth and selenium; and further wherein 0<a6; b is in the range: 0<b4; x is in the range 0<x1 and y is in the range 2y10. Such electrodes are useful in, for example, sodium and/or lithium ion battery applications.

Claims

1. A positive electrode containing an active material of the formula:
A.sub.aM.sub.bX.sub.xO.sub.y wherein, A is one or more alkali metals comprising lithium; M is selected from one or more transition metals and/or one or more non-transition metals and/or one or more metalloids; X comprises one or more elements selected from the group consisting of niobium in oxidation state 5+, antimony in oxidation state 5+, tellurium in oxidation state 6+, tantalum in oxidation state 5+, bismuth in oxidation state 5+ and selenium in oxidation state 6+; and further wherein 0 <a6; b is in the range: 0 <b4; x is in the range 0.5 x1 and y is in the range 2 y10.

2. A positive electrode containing an active material according to claim 1 wherein M comprises one or more transition metals and/or one or more non-transition metals selected from titanium, vanadium, chromium, molybdenum, tungsten, manganese, iron, osmium, cobalt, nickel, palladium, platinum, copper, silver, gold, zinc, cadmium, magnesium, calcium, beryllium, strontium, barium, aluminum and boron.

3. A positive electrode containing an active material according to claim 1 wherein at least one of the one or more transition metals has an oxidation state of +2 and at least one of the one or more non-transition metals has an oxidation state of +2.

4. A positive electrode containing an active material according to claim 1 wherein at least one of the one or more transition metals has an oxidation state of either +2 or +3 and wherein at least one of the one or more non-transition metals has an oxidation state of +3.

5. A positive electrode containing an active material according to claim 1 wherein M is selected from one or more of copper, nickel, cobalt, manganese, aluminum, vanadium, magnesium and iron.

6. A positive electrode containing an active material according to claim 1 of the formula: A.sub.aM.sub.bSb.sub.xO.sub.y, wherein A is one or more alkali metals comprising lithium, and M is one or more metals selected from cobalt, nickel, manganese, iron, copper, aluminum, vanadium and magnesium.

7. A positive electrode containing an active material according to claim 1 of the formula: A.sub.aM.sub.bTe.sub.xO.sub.y, wherein A is one or more alkali metals comprising lithium, and M is one or more metals selected from cobalt, nickel, manganese, iron, copper, aluminum, vanadium and magnesium.

8. A positive electrode according to claim 1 used in conjunction with a counter electrode and one or more electrolyte materials.

9. A positive electrode according to claim 1 containing one or more active materials selected from: Li.sub.3Ni.sub.1.5Mg.sub.0.5SbO.sub.6, Li.sub.3Ni.sub.2SbO.sub.6, Li.sub.3Mn.sub.2SbO.sub.6, Li.sub.3Fe.sub.2SbO.sub.6, Li.sub.3Ni.sub.1.5Mg.sub.0.5SbO.sub.6, Li.sub.3Cu.sub.2SbO.sub.6, Li.sub.3Co.sub.2SbO.sub.6, Li.sub.2Co.sub.2TeO.sub.6, Li.sub.2Ni.sub.2TeO.sub.6, Li.sub.2Mn.sub.2TeO.sub.6, LiCoSbO.sub.4, LiNiSbO.sub.4, LiMnSbO.sub.4, Li.sub.3CuSbO.sub.5, Li.sub.2NiSbO.sub.5, Li.sub.4Fe.sub.3SbO.sub.9, Li.sub.5NiSbO.sub.6, Li.sub.4MnSbO.sub.6, Li.sub.3MnTeO.sub.6, Li.sub.3FeTeO.sub.6, Li.sub.4Fe.sub.1z(Ni.sub.0.5Ti.sub.0.5).sub.zSbO.sub.6 (0<z<1), Li.sub.4Fe.sub.0.5Ni.sub.0.25Ti.sub.0.25SbO.sub.6, Li.sub.4Fe.sub.1z(Ni.sub.0.5Mn.sub.0.5).sub.zSbO.sub.6 (0z1), Li.sub.4Fe.sub.0.5Ni.sub.0.25Mn.sub.0.25SbO.sub.6, Li.sub.5zNi.sub.1zFe.sub.zSbO.sub.6 (0z1), Li.sub.4.5Ni.sub.0.5Fe.sub.0.5SbO.sub.6, Li.sub.4FeSbO.sub.6 and Li.sub.4NiTeO.sub.6.

10. An energy storage device comprising a positive electrode according to claim 1.

11. An energy storage device according to claim 10 suitable for use as one or more of the following: a lithium ion-containing cell, a lithium metal containing cell, a non-aqueous electrolyte lithium ion-containing cell, an aqueous electrolyte lithium ion-containing cell.

12. A rechargeable battery comprising a positive electrode according to claim 1.

13. An electrochemical device comprising a positive electrode according to claim 1.

14. An electrochromic device comprising a positive electrode according to claim 1.

Description

BRIEF DESCRIPTION OF THE DRAWINGS

(1) The present invention will now be described with reference to the following drawings in which:

(2) FIG. 1A is the XRD of Na.sub.3Ni.sub.2SbO.sub.6 prepared according to Example 1;

(3) FIG. 1B shows the Constant current cycling (Cell Voltage versus Cumulative Cathode Specific Capacity) of a Na-ion cell: Hard Carbon/Na.sub.3Ni.sub.2SbO.sub.6 prepared according to Example 1;

(4) FIG. 2 is the XRD for Na.sub.3Co.sub.2SbO.sub.6 prepared according to Example 2;

(5) FIG. 3 is the XRD for Na.sub.3Mn.sub.2SbO.sub.6 prepared according to Example 3;

(6) FIG. 4A is the XRD for Li.sub.3Cu.sub.2SbO.sub.6 prepared according to Example 22;

(7) FIG. 4B shows Constant current cycling (Electrode Potential versus Cumulative Specific Capacity) of Li.sub.3Cu.sub.2SbO.sub.6 prepared according to Example 22;

(8) FIG. 5A is the XRD of Na.sub.2Ni.sub.2TeO.sub.6 prepared according to Example 28;

(9) FIG. 5B shows the Constant current cycling (Electrode Potential versus Cumulative Specific Capacity) of Na.sub.2Ni.sub.2TeO.sub.6 prepared according to Example 28;

(10) FIG. 6A is the XRD of Li.sub.3Ni.sub.2SbO.sub.6 prepared according to Example 19;

(11) FIG. 6B shows the Constant current cycling (Electrode Potential versus Cumulative Specific Capacity) of Li.sub.3Ni.sub.2SbO.sub.6 prepared according to Example 19;

(12) FIG. 7A is the XRD of Na.sub.3Ni.sub.2-zMg.sub.zSbO.sub.6, where z=0.00, 0.25, 0.5, and 0.75, prepared according to method of Examples 34a, 34b, 34c, 34d respectively;

(13) FIG. 7B shows the Constant current cycling (Cell Voltage versus Cumulative Cathode Specific Capacity) of a Na-ion cell: Hard Carbon //Na.sub.3Ni.sub.1.5Mg.sub.0.5SbO.sub.6 prepared according to Example 34c;

(14) FIG. 8A is the XRD of Li.sub.3Ni.sub.1.5Mg.sub.0.5SbO.sub.6 prepared according to Example 17;

(15) FIG. 8B shows the Constant current cycling (Cell Voltage versus Cumulative Cathode Specific Capacity) of a Li-ion cell: Graphite//Li.sub.3Ni.sub.1.5Mg.sub.0.5SbO.sub.6 prepared according to Example 17;

(16) FIG. 9A is the XRD of Na.sub.3Ni.sub.1.75Zn.sub.0.25SbO.sub.6 prepared according to Example 35;

(17) FIG. 9B shows the long term Constant current cycling performance (cathode specific capacity versus cycle number) of a Na-ion Cell comprising Carbotron (Kureha Inc.) Hard Carbon//Na.sub.3Ni.sub.1.75Zn.sub.0.25SbO.sub.6 prepared according to Example 35;

(18) FIG. 10A is the XRD of Na.sub.3Ni.sub.1.75Cu.sub.0.25SbO.sub.6 prepared according to Example 36;

(19) FIG. 10B shows the long term constant current cycling performance (cathode specific capacity versus cycle number) of a Na-ion Cell comprising: Hard Carbon//Na.sub.3Ni.sub.1.75Cu.sub.0.25SbO.sub.6 prepared according to Example 36;

(20) FIG. 11A is the XRD of Na.sub.3Ni.sub.1.25Mg.sub.0.75SbO.sub.6 prepared according to Example 34d;

(21) FIG. 11B shows the long term constant current cycling performance (cathode specific capacity versus cycle number) of a Na-ion Cell comprising: Hard Carbon//Na.sub.3Ni.sub.1.25Mn.sub.0.75SbO.sub.6 prepared according to Example 34d;

(22) FIG. 12A is the XRD of Na.sub.3Ni.sub.1.50Mn.sub.0.50SbO.sub.6 prepared according to Example 37;

(23) FIG. 12B shows the long term constant current cycling performance (cathode specific capacity versus cycle number) of a Na-ion Cell comprising: Hard Carbon//Na.sub.3Ni.sub.1.50Mn.sub.0.50SbO.sub.6 prepared according to Example 37;

(24) FIG. 13A is the XRD of Li.sub.4FeSbO.sub.6 prepared according to Example 38;

(25) FIG. 13B shows the constant current cycling data for the Li.sub.4FeSbO.sub.6 active material prepared according to Example 38;

(26) FIG. 14A is the XRD of Li.sub.4NiTeO.sub.6 prepared according to Example 39;

(27) FIG. 14B shows the constant current cycling data for the Li.sub.4NiTeO.sub.6 active material prepared according to Example 39; and

(28) FIG. 15A is the XRD of Na.sub.4NiTeO.sub.6 prepared according to Example 40; and

(29) FIG. 15B shows the constant current cycling data for the Na.sub.4NiTeO.sub.6 prepared according to Example 40.

DETAILED DESCRIPTION

(30) Active materials used in the present invention are prepared on a laboratory scale using the following generic method:

(31) Generic Synthesis Method:

(32) The required amounts of the precursor materials are intimately mixed together. The resulting mixture is then heated in a tube furnace or a chamber furnace using either a flowing inert atmosphere (e.g. argon or nitrogen) or an ambient air atmosphere, at a furnace temperature of between 400 C. and 1200 C. until reaction product forms. When cool, the reaction product is removed from the furnace and ground into a powder.

(33) Using the above method, active materials used in the present invention were prepared as summarised below in Examples 1 to 40

(34) TABLE-US-00001 TARGET COMPOUND STARTING FURNACE EXAMPLE (ID code) MATERIALS CONDITIONS 1 Na.sub.3Ni.sub.2SbO.sub.6 Na.sub.2CO.sub.3 Air/800 C., dwell time (X0328) NiCO.sub.3 of 8 hours. Sb.sub.2O.sub.3 2 Na.sub.3Co.sub.2SbO.sub.6 Na.sub.2CO.sub.3 Air/800 C., dwell time (X0325) CoCO.sub.3 of 8 hours. Sb.sub.2O.sub.3 3 Na.sub.3Mn.sub.2SbO.sub.6 Na.sub.2CO.sub.3 N.sub.2/800 C., dwell time (X0276) MnCO.sub.3 of 8 hours. Sb.sub.2O.sub.3 4 Na.sub.3Fe.sub.2SbO.sub.6 Na.sub.2CO.sub.3 N.sub.2/800 C., dwell time (X0240) Fe.sub.2O.sub.3 of 8 hours. Sb.sub.2O.sub.3 5 Na.sub.3Cu.sub.2SbO.sub.6 Na.sub.2CO.sub.3 Air/800 C., dwell time (X0247) CuO of 8 hours Sb.sub.2O.sub.3 6 Na.sub.2AlMnSbO.sub.6 Na.sub.2CO.sub.3 Air/800 C., dwell time (X0232) Al(OH).sub.3 of 8 hours MnCO.sub.3 Sb.sub.2O.sub.3 7 Na.sub.2AlNiSbO.sub.6 Na.sub.2CO.sub.3 Air/800 C., dwell time (X0233) Al(OH).sub.3 of 8 hours NiCO.sub.3 Sb.sub.2O.sub.3 8 Na.sub.2VMgSbO.sub.6 Na.sub.2CO.sub.3 N.sub.2/800 C., dwell time (X0245) V.sub.2O.sub.3 of 8 hours Mg(OH).sub.2 NaSbO.sub.33H.sub.2O 9 NaCoSbO.sub.4 Na.sub.2CO.sub.3 Air/800 C., dwell time (X0253) CoCO.sub.3 of 8 hours Sb.sub.2O.sub.33H.sub.2O 10 NaNiSbO.sub.4 Na.sub.2CO.sub.3, Air/800 C., dwell time (X0254) NiCO.sub.3. of 8 hours Sb.sub.2O.sub.3 11 NaMnSbO.sub.4 Na.sub.2CO.sub.3, Air/800 C., dwell time (X0257) MnCO.sub.3 of 8 hours Sb.sub.2O.sub.3 12 Na.sub.4FeSbO.sub.6 Na.sub.2CO.sub.3 Air/800 C., dwell time (X0260) Fe.sub.2O.sub.3 of 8 hours Sb.sub.2O.sub.3 13 Na.sub.0.8Co.sub.0.6Sb.sub.0.4O.sub.2 Na.sub.2CO.sub.3 Air/800 C., dwell time (X0263) CoCO.sub.3 of 8 hours Sb.sub.2O.sub.3 14 Na.sub.0.8Ni.sub.0.6Sb.sub.0.4O.sub.4 Na.sub.2CO.sub.3 Air/800 C., dwell time (X0264) NiCO.sub.3 of 8 hours Sb.sub.2O.sub.3 15 Na.sub.3Ni.sub.1.5Mg.sub.0.5SbO.sub.6 Na.sub.2CO.sub.3 Air/800 C., dwell time (X0336) NiCO.sub.3 of 14 hours Sb.sub.2O.sub.3 Mg(OH).sub.2 16 Na.sub.3Co.sub.1.5Mg.sub.0.5SbO.sub.6 Na.sub.2CO.sub.3 Air/800 C., dwell time (X0331) CoCO.sub.3 of 14 hours Sb.sub.2O.sub.3 Mg(OH).sub.2 17 Li.sub.3Ni.sub.1.5Mg.sub.0.5SbO.sub.6 Li.sub.2CO.sub.3 Air/800 C., dwell time (X0368) NiCO.sub.3 of 8 hours Sb.sub.2O.sub.3 Mg(OH).sub.2 18 Li.sub.3Co.sub.2SbO.sub.6 Na.sub.2CO.sub.3 Air/800 C., dwell time (X0222) CoCO.sub.3 of 8 hours Sb.sub.2O.sub.3 19 Li.sub.3Ni.sub.2SbO.sub.6 Na.sub.2CO.sub.3 Air/800 C., dwell time (X0223) NiCO.sub.3 of 8 hours Sb.sub.2O.sub.3 20 Li.sub.3Mn.sub.2SbO.sub.6 Na.sub.2CO.sub.3 Air/800 C., dwell time (X0239) MnCO.sub.3 of 8 hours Sb.sub.2O.sub.3 21 Li.sub.3Fe.sub.2SbO.sub.6 Li.sub.2CO.sub.3 N.sub.2 /800 C., dwell time (X0241) Fe.sub.2O.sub.3 of 8 hours Sb.sub.2O.sub.3 22 Li.sub.3Cu.sub.2SbO.sub.6 Li.sub.2CO.sub.3 Air/800 C., dwell time (X0303) CuO of 8 hours Sb.sub.2O.sub.3 23 LiCoSbO.sub.4 Li.sub.2CO.sub.3 Air/800 C., dwell time (X0251) CoO.sub.3 of 8 hours Sb.sub.2O.sub.3 24 LiNiSbO.sub.4 Li.sub.2CO.sub.3 Air/800 C., dwell time (X0252) NiCO.sub.3 of 8 hours Sb.sub.2O.sub.3 25 LiMnSbO.sub.4 Li.sub.2CO.sub.3 Air/800 C., dwell time (X0256) MnCO.sub.3 of 8 hours Sb.sub.2O.sub.3 26 Li.sub.3CuSbO.sub.5 Li.sub.2CO.sub.3 Air/800 C., dwell time (X0255) CuO of 8 hours Sb.sub.2O.sub.3 27 Na.sub.2Co.sub.2TeO.sub.6 Na.sub.2CO.sub.3 Air/800 C., dwell time (X0216) CoCO.sub.3 of 8 hours TeO.sub.2 28 Na.sub.2Ni.sub.2TeO.sub.6 Na.sub.2CO.sub.3 Air/800 C., dwell time (X0217) NiCO.sub.3 of 8 hours TeO.sub.2 29 Na.sub.2Mn.sub.2TeO.sub.6 Na.sub.2CO.sub.3 Air/800 C. (X0234) MnCO.sub.3 TeO.sub.2 30 Na.sub.2Fe.sub.2TeO.sub.6 Na.sub.2CO.sub.3 N.sub.2/800 C., dwell time (X0236) Fe.sub.2O.sub.3 of 8 hours TeO.sub.2 31 Li.sub.2Co.sub.2TeO.sub.6 Li.sub.2CO.sub.3 Air/800 C., dwell time (X0218) CoCO.sub.3 of 8 hours TeO.sub.2 32 Li.sub.2Ni.sub.2TeO.sub.6 Li.sub.2CO.sub.3 Air/800 C., dwell (X0219) NiCO.sub.3 time of 8 hours TeO.sub.2 33 Li.sub.2Mn.sub.2TeO.sub.6 Li.sub.2CO.sub.3 Air/800 C., dwell time (X0235) MnCO.sub.3 of 8 hours TeO.sub.2 34 Na.sub.3Ni.sub.2zMg.sub.zSbO.sub.6 Na.sub.2CO.sub.3 Air/800 C., dwell time 34a Z = 0.00 (X0221) = E.g. 1 NiCO.sub.3 of 8-14 hours 34b Z = 0.25 (X0372) Mg(OH).sub.2 34c Z = 0.5 (X0336) = E.g. 15 Sb.sub.2O.sub.3 34d Z = 0.75 (X0373) 35 Na.sub.3Ni.sub.1.75Zn.sub.0.25SbO.sub.6 Na.sub.2CO.sub.3, NiCO.sub.3, Air/800 C., dwell (X0392) Sb.sub.2O.sub.3, ZnO time of 8 hours 36 Na.sub.3Ni.sub.1.75Cu.sub.0.25SbO.sub.6 Na.sub.2CO.sub.3, NiCO.sub.3, Air/800 C., dwell (X0393) Sb.sub.2O.sub.3, CuO time of 8 hours 37 Na.sub.3Ni.sub.1.50Mn.sub.0.50SbO.sub.6 Na.sub.2CO.sub.3, NiCO.sub.3, Air/800 C., dwell (0380) Sb.sub.2O.sub.3, MnO.sub.2 time of 8 hours 38 Li.sub.4FeSbO.sub.6 Li.sub.2CO.sub.3, Fe.sub.2O.sub.3, Air/800 C., dwell (1120A) Sb.sub.2O.sub.3 time of 8 hours followed by 800 C., for a further 8 hours 39 Li.sub.4NiTeO.sub.6 Li.sub.2CO.sub.3, NiCO.sub.3, Air/800 C., dwell (X1121) TeO.sub.2 time of 8 hours 40 Na.sub.4NiTeO.sub.6 Na.sub.2CO.sub.3, NiCO.sub.3, Air/800 C., dwell (X1122) TeO.sub.2 time of 8 hours
Product Analysis Using XRD

(35) All of the product materials were analysed by X-ray diffraction techniques using a Siemens D5000 powder diffractometer to confirm that the desired target materials had been prepared and to establish the phase purity of the product material and to determine the types of impurities present. From this information it is possible to determine the unit cell lattice parameters.

(36) The general operating conditions used to obtain the XRD spectra are as follows:

(37) Slits sizes: 1 mm, 1 mm, 0.1 mm

(38) Range: 2=5-60

(39) X-ray Wavelength=1.5418 ) (Cu K)

(40) Speed: 0.5 or 1.0 second/step

(41) Increment: 0.015 or 0.025

(42) Electrochemical Results

(43) The target materials were tested in a lithium metal anode test electrochemical cell to determine their specific capacity and also to establish whether they have the potential to undergo charge and discharge cycles. A lithium metal anode test electrochemical cell containing the active material is constructed as follows:

(44) Generic Procedure to Make a Lithium Metal Test Electrochemical Cell

(45) The positive electrode is prepared by solvent-casting a slurry of the active material, conductive carbon, binder and solvent. The conductive carbon used is Super P (Timcal). PVdF co-polymer (e.g. Kynar Flex 2801, Elf Atochem Inc.) is used as the binder, and acetone is employed as the solvent. The slurry is then cast onto glass and a free-standing electrode film is formed as the solvent evaporates. The electrode is then dried further at about 80 C. The electrode film contains the following components, expressed in percent by weight: 80% active material, 8% Super P carbon, and 12% Kynar 2801 binder. Optionally, an aluminium current collector may be used to contact the positive electrode. Metallic lithium on a copper current collector may be employed as the negative electrode. The electrolyte comprises one of the following: (i) a 1 M solution of LiPF.sub.6 in ethylene carbonate (EC) and dimethyl carbonate (DMC) in a weight ratio of 1:1; (ii) a 1 M solution of LiPF.sub.6 in ethylene carbonate (EC) and diethyl carbonate (DEC) in a weight ratio of 1:1; or (iii) a 1 M solution of LiPF.sub.6 in propylene carbonate (PC) A glass fibre separator (Whatman, GF/A) or a porous polypropylene separator (e.g. Celgard 2400) wetted by the electrolyte is interposed between the positive and negative electrodes.

(46) Generic Procedure to Make a Hard Carbon Na-Ion Cell

(47) The positive electrode is prepared by solvent-casting a slurry of the active material, conductive carbon, binder and solvent. The conductive carbon used is Super P (Timcal). PVdF co-polymer (e.g. Kynar Flex 2801, Elf Atochem Inc.) is used as the binder, and acetone is employed as the solvent. The slurry is then cast onto glass and a free-standing electrode film is formed as the solvent evaporates. The electrode is then dried further at about 80 C. The electrode film contains the following components, expressed in percent by weight: 80% active material, 8% Super P carbon, and 12% Kynar 2801 binder. Optionally, an aluminium current collector may be used to contact the positive electrode.

(48) The negative electrode is prepared by solvent-casting a slurry of the hard carbon active material (Carbotron P/J, supplied by Kureha), conductive carbon, binder and solvent. The conductive carbon used is Super P (Timcal). PVdF co-polymer (e.g. Kynar Flex 2801, Elf Atochem Inc.) is used as the binder, and acetone is employed as the solvent. The slurry is then cast onto glass and a free-standing electrode film is formed as the solvent evaporates. The electrode is then dried further at about 80 C. The electrode film contains the following components, expressed in percent by weight: 84% active material, 4% Super P carbon, and 12% Kynar 2801 binder. Optionally, a copper current collector may be used to contact the negative electrode.

(49) Generic Procedure to Make a Graphite Li-Ion Cell

(50) The positive electrode is prepared by solvent-casting a slurry of the active material, conductive carbon, binder and solvent. The conductive carbon used is Super P (Timcal). PVdF co-polymer (e.g. Kynar Flex 2801, Elf Atochem Inc.) is used as the binder, and acetone is employed as the solvent. The slurry is then cast onto glass and a free-standing electrode film is formed as the solvent evaporates. The electrode is then dried further at about 80 C. The electrode film contains the following components, expressed in percent by weight: 80% active material, 8% Super P carbon, and 12% Kynar 2801 binder. Optionally, an aluminium current collector may be used to contact the positive electrode.

(51) The negative electrode is prepared by solvent-casting a slurry of the graphite active material (Crystalline Graphite, supplied by Conoco Inc.), conductive carbon, binder and solvent. The conductive carbon used is Super P (Timcal). PVdF co-polymer (e.g. Kynar Flex 2801, Elf Atochem Inc.) is used as the binder, and acetone is employed as the solvent. The slurry is then cast onto glass and a free-standing electrode film is formed as the solvent evaporates. The electrode is then dried further at about 80 C. The electrode film contains the following components, expressed in percent by weight: 92% active material, 2% Super P carbon, and 6% Kynar 2801 binder. Optionally, a copper current collector may be used to contact the negative electrode.

(52) Cell Testing

(53) The cells are tested as follows using Constant Current Cycling techniques.

(54) The cell is cycled at a given current density between pre-set voltage limits. A commercial battery cycler from Maccor Inc. (Tulsa, Okla., USA) is used. On charge, sodium (lithium) ions are extracted from the active material. During discharge, sodium (lithium) ions are re-inserted into the active material.

(55) Results:

(56) Na.sub.3Ni.sub.2SbO.sub.6 Prepared According to Example 1.

(57) Referring to FIG. 1B. The Cell #202071 shows the constant current cycling data for the Na.sub.3Ni.sub.2SbO.sub.6 active material (X0328) made according to Example 1 in a Na-ion cell where it is coupled with a Hard Carbon (Carbotron P/J) anode material. The electrolyte used a 0.5 M solution of NaClO.sub.4 in propylene carbonate. The constant current data were collected at an approximate current density of 0.05 mA/cm.sup.2 between voltage limits of 1.80 and 4.00 V. To fully charge the cell the Na-ion cell was potentiostatically held at 4.0 V at the end of the constant current charging process. The testing was carried out at room temperature. It is shown that sodium ions are extracted from the cathode active material, Na.sub.3Ni.sub.2SbO.sub.6, and inserted into the Hard Carbon anode during the initial charging of the cell. During the subsequent discharge process, sodium ions are extracted from the Hard Carbon and re-inserted into the Na.sub.3Ni.sub.2SbO.sub.6 cathode active material. The first discharge process corresponds to a specific capacity for the cathode of 86 mAh/g, indicating the reversibility of the sodium ion extraction-insertion processes. The generally symmetrical nature of the charge-discharge curves further indicates the excellent reversibility of the system, and the low level of voltage hysteresis (i.e. the voltage difference between the charge and discharge processes) is extremely small, and this also indicates the excellent kinetics of the extraction-insertion reactions. This is an important property that is useful for producing a high rate active material.

(58) Na.sub.3Cu.sub.2SbO.sub.6 Prepared According to Example 22.

(59) Referring to FIG. 4B. The Cell #202014 shows the constant current cycling data for the Li.sub.3Cu.sub.2SbO.sub.6 active material (X0303) made according to Example 22. The electrolyte used a 1.0 M solution of LiPF.sub.6 in ethylene carbonate (EC) and diethyl carbonate (DEC). The constant current data were collected using a lithium metal counter electrode at an approximate current density of 0.02 mA/cm.sup.2 between voltage limits of 3.00 and 4.20 V. The upper voltage limit was increased by 0.1 V on subsequent cycles. The testing was carried out at room temperature. It is shown that lithium ions are extracted from the active material during the initial charging of the cell. A charge equivalent to a material specific capacity of 33 mAh/g is extracted from the active material. The re-insertion process corresponds to 14 mAh/g, indicating the reversibility of the ion extraction-insertion processes. The generally symmetrical nature of the charge-discharge curves further indicates the excellent reversibility of the system. In addition, the level of voltage hysteresis (i.e. the voltage difference between the charge and discharge processes) is extremely small, indicating the excellent kinetics of the extraction-insertion reactions. This is an important property that is useful for producing a high rate active material.

(60) Na.sub.2Ni.sub.2TeO.sub.6 Prepared According to Example 28.

(61) Referring to FIG. 5B. The Cell #201017 shows the constant current cycling data for the Na.sub.2Ni.sub.2TeO.sub.6 active material (X0217) made according to Example 28. The electrolyte used a 0.5 M solution of NaClO.sub.4 in propylene carbonate. The constant current data were collected using a lithium metal counter electrode at an approximate current density of 0.02 mA/cm.sup.2 between voltage limits of 3.00 and 4.20 V. The upper voltage limit was increased by 0.1 V on subsequent cycles. The testing was carried out at room temperature. It is shown that sodium ions are extracted from the active material during the initial charging of the cell. A charge equivalent to a material specific capacity of 51 mAh/g is extracted from the active material.

(62) It is expected from thermodynamic considerations that the sodium extracted from the Na.sub.2Ni.sub.2TeO.sub.6 active material during the initial charging process, enters the electrolyte, and would then be displacement plated onto the lithium metal anode (i.e. releasing more lithium into the electrolyte). Therefore, during the subsequent discharging of the cell, it is assumed that a mix of lithium and sodium ions is re-inserted into the active material. The re-insertion process corresponds to 43 mAh/g; indicating the reversibility of the ion extraction-insertion processes. The generally symmetrical nature of the charge-discharge curves further indicates the excellent reversibility of the system. In addition, the level of voltage hysteresis (i.e. the voltage difference between the charge and discharge processes) is extremely small, indicating the excellent kinetics of the extraction-insertion reactions. This is an important property that is useful for producing a high rate active material.

(63) Li.sub.3Ni.sub.2SbO.sub.6 Prepared According to Example 19.

(64) Referring to FIG. 6B. The Cell #201020 shows the constant current cycling data for the Li.sub.3Ni.sub.2SbO.sub.6 active material (X0223) made following Example 19. The electrolyte used a 1.0 M solution of LiPF.sub.6 in ethylene carbonate (EC) and diethyl carbonate (DEC). The constant current data were collected using a lithium metal counter electrode at an approximate current density of 0.02 mA/cm.sup.2, between voltage limits of 3.00 and 4.20 V. The upper voltage limit was increased by 0.1 V on subsequent cycles. The testing was carried out at room temperature. It is shown that lithium ions are extracted from the active material during the initial charging of the cell. A charge equivalent to a material specific capacity of 130 mAh/g is extracted from the active material. The re-insertion process corresponds to 63 mAh/g and indicates the reversibility of the ion extraction-insertion processes. The generally symmetrical nature of the charge-discharge curves further indicates the excellent reversibility of the system. In addition, the level of voltage hysteresis (i.e. the voltage difference between the charge and discharge processes) is extremely small, indicating the excellent kinetics of the extraction-insertion reactions. This is an important property that is useful for producing a high rate active material.

(65) Na.sub.3Ni.sub.1.5Mg.sub.0.5SbO.sub.6 Prepared According to Example 34C.

(66) Referring to FIG. 7B. The Cell #203016 shows the constant current cycling data for the Na.sub.3Ni.sub.1.5Mg.sub.0.5SbO.sub.6 active material (X0336) made following Example 34c in a Na-ion cell where it is coupled with a Hard Carbon (Carbotron P/J) anode material. The electrolyte used a 0.5 M solution of NaClO.sub.4 in propylene carbonate. The constant current data were collected at an approximate current density of 0.05 mA/cm.sup.2 between voltage limits of 1.80 and 4.20 V.

(67) To fully charge the cell the Na-ion cell was potentiostatically held at 4.2 V at the end of the constant current charging process. The testing was carried out at room temperature. It is shown that sodium ions are extracted from the cathode active material, Na.sub.3Ni.sub.1.5Mg.sub.0.5SbO.sub.6, and inserted into the Hard Carbon anode during the initial charging of the cell. During the subsequent discharge process, sodium ions are extracted from the Hard Carbon and re-inserted into the Na.sub.3Ni.sub.1.5Mg.sub.0.5SbO.sub.6 cathode active material. The first discharge process corresponds to a specific capacity for the cathode of 91 mAh/g, indicating the reversibility of the sodium ion extraction-insertion processes. The generally symmetrical nature of the charge-discharge curves further indicates the excellent reversibility of the system. In addition, the level of voltage hysteresis (i.e. the voltage difference between the charge and discharge processes) is extremely small, indicating the excellent kinetics of the extraction-insertion reactions. This is an important property that is useful for producing a high rate active material.

(68) Li.sub.3Ni.sub.1.5Mg.sub.0.5SbO.sub.6 Prepared According to Example 17.

(69) Referring to FIG. 8B. The Cell #203018 shows the constant current cycling data for the Li.sub.3Ni.sub.1.5Mg.sub.0.5SbO.sub.6 active material (X0368) made according to Example 17 in a Li-ion cell where it is coupled with a Crystalline Graphite (Conoco Inc.) anode material. The electrolyte used a 1.0 M solution of LiPF.sub.6 in ethylene carbonate (EC) and diethyl carbonate (DEC). The constant current data were collected at an approximate current density of 0.05 mA/cm.sup.2 between voltage limits of 1.80 and 4.20 V. To fully charge the cell the Li-ion cell was potentiostatically held at 4.2 V at the end of the constant current charging process. The testing was carried out at room temperature. It is shown that lithium ions are extracted from the cathode active material, Li.sub.3Ni.sub.1.5Mg.sub.0.5SbO.sub.6, and inserted into the Graphite anode during the initial charging of the cell. During the subsequent discharge process, lithium ions are extracted from the Graphite and re-inserted into the Li.sub.3Ni.sub.1.5Mg.sub.0.5SbO.sub.6 cathode active material. The first discharge process corresponds to a specific capacity for the cathode of 85 mAh/g, indicating the reversibility of the lithium ion extraction-insertion processes. The generally symmetrical nature of the charge-discharge curves further indicates the excellent reversibility of the system. In addition, the level of voltage hysteresis (i.e. the voltage difference between the charge and discharge processes) is extremely small, indicating the excellent kinetics of the extraction-insertion reactions. This is an important property that is useful for producing a high rate active material.

(70) Na.sub.3Ni.sub.1.75Zn.sub.025SbO.sub.6 Prepared According to Example 35.

(71) FIG. 9B (Cell#203054) shows the long term constant current cycling performance (cathode specific capacity versus cycle number) of a Na-ion Cell comprising Carbotron (Kureha Inc.) Hard Carbon//Na.sub.3Ni.sub.1.75Zn.sub.0.25SbO.sub.6 (Material=X0392) using a 0.5 M NaClO.sub.4propylene carbonate (PC) electrolyte. The constant current cycling test was carried out at 25 C. between voltage limits of 1.8 and 4.2 V. To fully charge the cell, the Na-ion cell was held at a cell voltage of 4.2 V at the end of the constant current charging process until the cell current had decayed to one tenth of the constant current value. During the charging of the cell, sodium ions are extracted from the cathode active material, and inserted into the Hard Carbon anode. During the subsequent discharge process, sodium ions are extracted from the Hard Carbon and re-inserted into the cathode active material. The initial cathode specific capacity (cycle 1) is 70 mAh/g. The Na-ion cell cycles more than 50 times with low capacity fade.

(72) Na.sub.3Ni.sub.1.75Cu.sub.0.25SbO.sub.6 Prepared According to Example 36.

(73) FIG. 10B (Cell#203055) shows the long term constant current cycling performance (cathode specific capacity versus cycle number) of a Na-ion Cell comprising: Hard Carbon//Na.sub.3Ni.sub.1.75Cu.sub.0.25SbO.sub.6 (Material=X0393) using a 0.5 M NaClO.sub.4propylene carbonate (PC) electrolyte. The constant current cycling test was carried out at 25 C. between voltage limits of 1.8 and 4.2 V. To fully charge the cell, the Na-ion cell was held at a cell voltage of 4.2 V at the end of the constant current charging process until the cell current had decayed to one tenth of the constant current value. During the charging of the cell, sodium ions are extracted from the cathode active material, and inserted into the Hard Carbon anode. During the subsequent discharge process, sodium ions are extracted from the Hard Carbon and re-inserted into the cathode active material. The initial cathode specific capacity (cycle 1) is 62 mAh/g. The Na-ion cell cycles 18 times with low capacity fade.

(74) Na.sub.3Ni.sub.1.25Mg.sub.0.75SbO.sub.6 Prepared According to Example 34d.

(75) FIG. 11B (Cell#203047) shows the long term constant current cycling performance (cathode specific capacity versus cycle number) of a Na-ion Cell comprising: Hard Carbon//Na.sub.3Ni.sub.1.25Mg.sub.0.75SbO.sub.6 (Material=X0373) using a 0.5 M NaClO.sub.4propylene carbonate (PC) electrolyte. The constant current cycling test was carried out at 25 C. between voltage limits of 1.8 and 4.0 V. To fully charge the cell, the Na-ion cell was held at a cell voltage of 4.0 V at the end of the constant current charging process until the cell current had decayed to one tenth of the constant current value. During the charging of the cell, sodium ions are extracted from the cathode active material, and inserted into the Hard Carbon anode.

(76) During the subsequent discharge process, sodium ions are extracted from the Hard Carbon and re-inserted into the cathode active material. The initial cathode specific capacity (cycle 1) is 83 mAh/g. The Na-ion cell cycles more than 40 times with low capacity fade.

(77) Na.sub.3Ni.sub.1.50Mn.sub.0.50SbO.sub.6 Prepared According to Example 37.

(78) FIG. 12B (Cell#203029) shows the long term constant current cycling performance (cathode specific capacity versus cycle number) of a Na-ion Cell comprising: Hard Carbon//Na.sub.3Ni.sub.1.50Mn.sub.0.50SbO.sub.6 (Material=X0380) using a 0.5 M NaClO.sub.4propylene carbonate (PC) electrolyte. The constant current cycling test was carried out at 25 C. between voltage limits of 1.8 and 4.2 V. To fully charge the cell, the Na-ion cell was held at a cell voltage of 4.2 V at the end of the constant current charging process until the cell current had decayed to one tenth of the constant current value. During the charging of the cell, sodium ions are extracted from the cathode active material, and inserted into the Hard Carbon anode. During the subsequent discharge process, sodium ions are extracted from the Hard Carbon and re-inserted into the cathode active material. The initial cathode specific capacity (cycle 1) is 78 mAh/g. The Na-ion cell cycles 13 times with low capacity fade.

(79) Li.sub.4FeSbO.sub.6 Prepared According to Example 38.

(80) FIG. 13B (Cell #303017) shows the constant current cycling data for the Li.sub.4FeSbO.sub.6 active material (X1120A). The electrolyte used a 1.0 M solution of LiPF.sub.6 in ethylene carbonate (EC) and diethyl carbonate (DEC). The constant current data were collected using a lithium metal counter electrode at an approximate current density of 0.04 mA/cm.sup.2 between voltage limits of 2.50 and 4.30 V. The testing was carried out at 25 C. It is shown that lithium ions are extracted from the active material during the initial charging of the cell. A charge equivalent to a material specific capacity of 165 mAh/g is extracted from the active material. The re-insertion process corresponds to 100 mAh/g, indicating the reversibility of the ion extraction-insertion processes. The generally symmetrical nature of the charge-discharge curves further indicates the excellent reversibility of the system.

(81) Li.sub.4NiTeO.sub.6 Prepared According to Example 39

(82) FIG. 14B (Cell #303018) shows the constant current cycling data for the Li.sub.4NiTeO.sub.6 active material (X1121). The electrolyte used a 1.0 M solution of LiPF.sub.6 in ethylene carbonate (EC) and diethyl carbonate (DEC). The constant current data were collected using a lithium metal counter electrode at an approximate current density of 0.04 mA/cm.sup.2 between voltage limits of 2.50 and 4.40 V. The testing was carried out at 25 C. It is shown that lithium ions are extracted from the active material during the initial charging of the cell. A charge equivalent to a material specific capacity of 168 mAh/g is extracted from the active material. The re-insertion process corresponds to 110 mAh/g, indicating the reversibility of the alkali ion extraction-insertion processes. The generally symmetrical nature of the charge-discharge curves further indicates the excellent reversibility of the system.

(83) Na.sub.4NiTeO.sub.6 Prepared According to Example 40.

(84) FIG. 15B (Cell #303019) shows the constant current cycling data for the Na.sub.4NiTeO.sub.6 active material (X1122). The electrolyte used a 1.0 M solution of LiPF.sub.6 in ethylene carbonate (EC) and diethyl carbonate (DEC). The constant current data were collected using a lithium metal counter electrode at an approximate current density of 0.04 mA/cm.sup.2 between voltage limits of 2.50 and 4.30 V. The testing was carried out at 25 C. It is shown that sodium ions are extracted from the active material during the initial charging of the cell. A charge equivalent to a material specific capacity of 75 mAh/g is extracted from the active material. The re-insertion process corresponds to 30 mAh/g, indicating the reversibility of the alkali ion extraction-insertion processes. The generally symmetrical nature of the charge-discharge curves further indicates the excellent reversibility of the system.