LITHIUM-OXYGEN BATTERIES INCORPORATING LITHIUM SUPEROXIDE

Abstract

A composition includes LiO2, reduced graphene oxide, and a metal catalyst or residue thereof.

Description

FIELD

The present technology is generally related to the production of lithium superoxide (LiO₂) which is free of other lithium-oxygen compounds.

BACKGROUND

There has been a significant interest in lithium superoxide (LiO₂), due to recent research into lithium-oxygen batteries, and the possibility that lithium superoxide may be an intermediate in the formation of lithium peroxide in lithium air cells. The first step in the oxygen reduction reaction (ORR) in a lithium air cell has been speculated to be the reduction of O₂ to O₂⁻, through a one-electron transfer, which is followed by the reaction with a lithium cation to form LiO₂ (Eqs. 1 and 2):

O₂+e⁻→O₂   (Eq. 1)

O₂⁻+Li⁺→LiO₂   (Eq. 2)

Lithium peroxide (Li₂O₂) can be then formed by the reaction of LiO₂ with Li⁺ through a second electron transfer, as shown in Eq. 3:

LiO₂+e⁻+Li⁺→Li₂O₂   (Eq. 3)

Alternatively, Li₂O₂ may be generated via the disproportionation reaction of LiO₂:

2 LiO₂→Li₂O₂+O₂   (Eq. 4)

SUMMARY

In one aspect, a composition includes LiO₂, reduced graphene oxide, and a metal catalyst or residue thereof. The composition may be free of Li₂O₂ and Li₂O. In any of the above embodiments, the metal catalyst includes a metal that forms an intermetallic phase with lithium, and the intermetallic phase has an orthorhombic structure. In any of the above embodiments, the metal catalyst includes Ir, Ru, Pt, or Pd. In any of the above embodiments, the metal catalyst includes Ir. In any of the above embodiments, the LiO₂ may be crystalline LiO₂. In any of the above embodiments, the intermetallic phase may be Ir₃Li.

In another aspect, an electrochemical cell includes an anode including lithium metal; a cathode including LiO₂ that is substantially free of Li₂O₂ and Li₂O; and an electrolyte. In some embodiments, the cathode may include a carbon-based material. In any of the above embodiments, the carbon-based material may include graphene oxide. The electrolyte may include at least a solvent and a lithium salt. In any of the above embodiments, the solvent may include an ether-based solvent, a fluorinated ether-based solvent, an oligo(ethylene oxide) solvent, or a mixture of any two or more thereof. In any of the above embodiments, the lithium salt may include LiCF₃CO₂, LiC₂F₅CO₂, LiClO₄, LiBF₄, LiAsF₆, LiPF₆, LiPF₂(C₂O₄)₂, LiPF₄C₂O₄, LiCF₃SO₃, LiN(CF₃SO₂)₂, LiC(CF₃SO₂)₃, LiN(SO₂C₂F₅)₂), lithium alkyl fluorophosphates, Li(C₂O₄)₂, LiBF₂C₂O₄, Li₂B₁₂X_12-pH_p, Li₂B₁₀X_10-yH_y, or a mixture of any two or more lithium salts, where X is OH, F, Cl, or Br; p is 0, 1, 2, 3, 4, 5, 6, 7, 8, 9, 10, 11, or 12; and y is 0, 1, 2, 3, 4, 5, 6, 7, 8, 9, or 10.

In another aspect, an electrochemical cell is provided. The cell may include an anode comprising lithium metal; a cathode comprising a solid phase oxygen generator; and an electrolyte. The solid phase oxygen generator may be LiO₂. In any such embodiments, the cathode may include a carbon-based material. In any such embodiments, the carbon-based material comprises graphene oxide. In any such embodiments, the electrolyte may include a solvent and a lithium salt. In any such embodiments, the cell may be a closed cell.

In another aspect, a process is provided for forming LiO₂. The process may include providing an electrochemical cell, the electrochemical cell comprising a porous oxygen carbon cathode, a lithium anode, a current collector, and an electrolyte; and discharging the electrochemical cell to form a discharge product. In such embodiments, the discharge product includes LiO₂, the porous oxygen carbon cathode includes reduced graphene oxide and a catalyst; and the discharge product is free of Li₂O and Li₂O₂.

BRIEF DESCRIPTION OF THE DRAWINGS

FIGS. 1A, 1B, 1C, and 1D are illustrations of cathode materials. FIG. 1A is an SEM image of a pristine rGO powder, according to the examples. FIG. 1B is an SEM image of an Ir-rGO composite, according to the examples. FIGS. 1C and 1D are TEM images of the Ir-rGO composite, showing Ir nanoparticles of less than 2 nm, according to the examples.

FIGS. 2A, 2B, 2C, and 2D are illustrations for rGO- and iridium-rGO-based cathodes. FIG. 2A is a voltage profile of an Ir-rGO cathode, according to the examples. FIG. 2B is a voltage profile of an rGO cathode, according to the examples. FIG. 2C is an SEM image of a discharge product of an Ir-rGO electrode, according to the examples. FIG. 2D is a TEM image of discharge product of an Ir-rGO, according to the examples. FIGS. 2C and 2 D are from the first discharge for the electrode. The current density is 100 mA/g, and the time control over 10 hrs.

FIGS. 3A, 3B, 3C, and 3D are illustrations of performance tests of iridium-rGO-based cathodes. FIG. 3A is an illustration of HE-XRD patterns of discharge products from Ir-rGO as a function of the aging time. FIG. 3B is a Raman spectra of a discharge product from Ir-rGO cathode from the 1^st and 2^nd discharges, according to the examples. FIG. 3C is a graph of voltage plots for the Ir-rGO cathode discharged first in O₂ to a capacity of 1000 mAh/g and then the discharged cathode was continuously discharged in Ar during which it attained a capacity 970 mAh/g. FIG. 3D is an HE-XRD pattern of cathode resulting from both discharges in the sample illustrated in FIG. 3C. FIG. 3E is a TEM image of an Ir agglomerate after 1^st discharge. FIG. 3F is an HR-TEM image of the Ir agglomerate surface, and FIG. 3G is the corresponding ED pattern, which provide the evidence of the formation of the Ir₃Li intermetallic. All of FIGS. 3 are according to the examples.

FIGS. 4A, 4B, 4C, and 4D are illustrative of density functional calculations. FIG. 4A is a barrier for desorption of an O₂ molecule from the (101) LiO₂ surface in vacuum, according to the examples. FIG. 4B includes ab initio molecular dynamics (MD) simulations showing the thermal stability of the (111) and (101) LiO₂ surfaces in vacuum at room temperature, according to the examples. FIG. 4C is a barrier for desorption of an O₂ molecule from an amorphous LiO₂ surface in vacuum, according to the examples. FIG. 4D illustrates density of states showing that bulk crystalline LiO₂ is a half-metal, according to the examples.

FIG. 5A is a secondary electron image of Ir-rGO, and FIG. 5B is a backscattering image of the sample, according to the examples.

FIG. 6 is a TGA curve of Ir-rGO, according to the examples.

FIG. 7A is an SEM image of a discharge product from a rGO cathode, and FIG. 7B is an XRD of a discharge product from the rGO cathode, according to the examples.

FIG. 8 is a calculation of a theoretical (LiO₂) XRD pattern derived from the DFT prediction of crystalline LiO₂, and experimental XRD patterns for crystalline Li₂O₂ and Ir at a wavelength of 0.11165 Å.

FIG. 9A illustrates the configuration (top and side view) of epitaxial growth of LiO₂ crystals (i.e. in P_nnm orthorhombic lattice) in a (111) orientation on a (121) facet of Ir₃Li (i.e. in the I_mm2 orthorhombic lattice) crystalline substrate, and FIG. 9B is a graph showing the basis of the preferred orientation growth of LiO₂ on Ir₃Li is supported by the low interfacial energy γ_interface (in eV/Ų) based on DFT calculations.

FIG. 10A is a lithium-metal anode converted to LiOH after the cell failed, and FIG. 10B is the voltage profile after replacement of the Li anode with a new one.

FIG. 11 is a Raman spectra of charged Ir-rGO cathode (from discharge cathode capacity=1000 mAh/g, current density=100 mAh/g) after 2, 8, and 30 cycles.

FIG. 12 is a graph of cycling data for a coin cell using the Ir-rGO cathode. The coin cell cycles for more than 80 cycles compared to the swagelok cell, which runs for about 40 cycles.

FIG. 13 is an SEM image of discharge product on deep discharge showing toroidal morphology.

FIG. 14A is a voltage profile for deep discharge (about 9500 mAH/g at a current density of 100 mA/g) on the Ir-rGO cathode. FIG. 14B is an XRD pattern for discharge product on deep discharge showing presence of Li₂O₂, LiO₂, and LiOH.

FIGS. 15A and 15B are FTIR spectra of (A) charged Ir-rGO cathode and (B) separators (from discharge cathode capacity of 1000 mAh/g, and a current density of 100 mAh/g) after 2, 8, 30 cycles.

DETAILED DESCRIPTION

Various embodiments are described hereinafter. It should be noted that the specific embodiments are not intended as an exhaustive description or as a limitation to the broader aspects discussed herein. One aspect described in conjunction with a particular embodiment is not necessarily limited to that embodiment and can be practiced with any other embodiment(s).

As used herein, “about” will be understood by persons of ordinary skill in the art and will vary to some extent depending upon the context in which it is used. If there are uses of the term which are not clear to persons of ordinary skill in the art, given the context in which it is used, “about” will mean up to plus or minus 10% of the particular term.

The use of the terms “a” and “an” and “the” and similar referents in the context of describing the elements (especially in the context of the following claims) are to be construed to cover both the singular and the plural, unless otherwise indicated herein or clearly contradicted by context. Recitation of ranges of values herein are merely intended to serve as a shorthand method of referring individually to each separate value falling within the range, unless otherwise indicated herein, and each separate value is incorporated into the specification as if it were individually recited herein. All methods described herein can be performed in any suitable order unless otherwise indicated herein or otherwise clearly contradicted by context. The use of any and all examples, or exemplary language (e.g., “such as”) provided herein, is intended merely to better illuminate the embodiments and does not pose a limitation on the scope of the claims unless otherwise stated. No language in the specification should be construed as indicating any non-claimed element as essential.

Although lithium superoxide (LiO₂) is believed to be an intermediate formed during lithium air battery discharge, ultimately becoming lithium peroxide, Li₂O₂, it is not believed that LiO₂ has ever been observed in its pure state at other than very low temperatures. Provided herein is a crystalline lithium superoxide that is free of both Li₂O₂ and lithium oxide (Li₂O). The lithium peroxide is formed on reduced graphene oxide (rGO). Metal catalysts may also be used to assist in the formation of the LiO₂. It has been found that LiO₂ may be formed as a discharge product from single electron transfer without further electron transfer or disproportionation to form Li₂O₂. High energy X-ray diffraction (HE-XRD) has been used to determine that there is no evidence of Li₂O₂ or Li₂O in the LiO₂ formed in the process. The HE-XRD studies as a function of time also shows that LiO₂ is stable in its crystalline form. The LiO₂ is stable for up to and at least one week of aging, in the presence of electrolyte. The results provide evidence that LiO₂ is stable enough that it can be repeatedly charged and discharged with a very low charge potential (about 3.2 V). Accordingly, in another aspect, a lithium superoxide-based battery is provided.

The process of forming the LiO₂ utilizes an electrochemical cell. The electrochemical cell has a reduced graphene oxide-based air cathode containing a catalyst, a lithium anode, a current collector, and the electrolyte is an ether-based solvent with a lithium salt. The cell is cycled for a predetermined time, and at a predetermined capacity and current density.

For example, a single cycle of the cell may be conducted for greater than 1 hour. In some embodiments, the cycle is conducted for from 1 hour to 48 hours. In some embodiments, the cycle is conducted for from 2 hours to 24 hours. In some embodiments, the cycle is conducted for from 12 hours to 24 hours. In yet a further embodiment, the cycle is conducted for about 20 hours. Accordingly, cycling for 35 cycles, in some cases may be 35×20, or about 700 hours. In any of the above embodiments, the capacity at which the cycling is conducted by be from about 200 mAh/g to about 2500 mAh/g. This may include from about 500 mAh/g to about 1500 mAh/g, and about 1000 mAh/g. The current density for the cycling, in any of the above embodiments, may be from about 10 mA/h to about 500 mA/h. This may include, but is not limited to, from about 25 mA/h to about 250 mA/h, and about 100 mA/h.

The metal catalyst is a transition metal catalyst that upon discharge will form an intermetallic compound with lithium. The intermetallic compound that is formed may have an orthorhombic structure that that will facilitate epitaxial growth of lithium superoxide on the surface of the lattice of the intermetallic compound.

As noted above, the porous oxygen carbon cathode may include a metal catalyst. Illustrative metal catalysts may include, but are not limited to Rh, Ir, and Pt. In some embodiments, the metal catalyst is Ir.

The lithium superoxide produced may find application in lithium air batteries, as a cathode material for a closed Li-air battery systems without need for a source of oxygen for the storage of oxygen, in solid form with low molecular weight, and as a lithium storage material to pre-lithiate high-energy anodes.

In one aspect, a composition is provided including lithium superoxide (LiO₂), reduced graphene oxide, and a metal catalyst or residue thereof. As used herein, the residue of a catalyst is the spent catalyst. It may be the catalyst or a decomposition product thereof that may or may not be characterized. In some embodiments, the LiO₂ is crystalline.

In any of the embodiments described herein, the composition may be free of other lithium-oxygen compounds such as lithium peroxide (Li₂O₂) or lithium oxide (Li₂O). As used herein, the phrase “free-of' means that in the compositions, the Li₂O₂ or the Li₂O are undetectable using spectroscopic methods. In any of the above embodiments, “free of” may mean greater than 98% purity of the LiO₂. In any of the above embodiments, “free of” may mean greater than 99% purity of the LiO₂. In any of the above embodiments, “free of” may mean greater than 99.9% purity of the LiO₂. In any of the above embodiments, “free of” may mean 100% purity of the LiO₂.

The metal catalyst may be a metal, metal compound, or metal alloy that forms an intermetallic phase with lithium. The intermetallic phase may have an orthorhombic structure. Illustrative metal catalysts may include, but are not limited to, Ir, Ru, Os, Ni, Pt, or Pd. In any of the above embodiments, the metal catalyst may include Ir. Where the catalyst is Ir, the intermetallic phase that is formed may be Ir₃Li.

In another aspect, an electrochemical cell is provided. The electrochemical cell may include an anode, a cathode, and an electrolyte, where the anode may be lithium metal, and the cathode described above is porous for oxygen transport for reaction with lithium cations. As used herein, a solid phase oxygen generator is a material that upon discharge of the cell provides oxygen for consumption by the lithium metal anode.

In the electrochemical cells, the cathode may also include a carbon-based material. For example, a porous carbon-based material may be used. Illustrative materials for use as the carbon-based material include, but are not limited to, reduced graphene oxide.

Illustrative electrolytes are aprotic and may include a solvent and a lithium salt in addition to other additives that may be present. The solvent may be an aprotic solvent such as an ether-based solvent, a fluorinated ether-based solvent, an oligo(ethylene oxide) solvent, or a mixture of any two or more thereof. Illustrative solvents include, but are not limited to glyme, diglyme, tetrahydrofuran, tetraethyletheylene glycol dimethylether, tri(ethylene glycol)-substituted methyltrimethyl silane (1NM3), ethylene glycol-substituted methyltrimethyl silane (1NM1), and di(ethylene glycol)-substituted methyltrimethyl silane (1NM2). Other illustrative solvents include, but are not limited to, solvents such as acetonitrile (ACN), dimethyl sulfoxide (DMSO), dimethylformamide (DMF), triethyl phosphate, N,N-dimethylacetamide (DMA), N-methyl pyrrolidone (NMP), methoxybenzene, siloxanes, and ionic liquids.

Illustrative lithium salts include, but are not limited to, LiCF₃CO₂, LiC₂F₅CO₂, LiClO₄, LiBF₄, LiAsF₆, LiPF₆, LiPF₂(C₂O₄)₂, LiPF₄C₂O₄, LiCF₃SO₃, LiN(CF₃SO₂)₂, LiC(CF₃SO₂)₃, LiN(SO₂C₂F₅)₂), lithium alkyl fluorophosphates, Li(C₂O₄)₂, LiBF₂C₂O₄, Li₂B₁₂X_12-pH_p, Li₂B₁₀X_10-yH_y, or a mixture of any two or more lithium salts, where X is OH, F, Cl, or Br; p is 0, 1, 2, 3, 4, 5, 6, 7, 8, 9, 10, 11, or 12; and y is 0, 1, 2, 3, 4, 5, 6, 7, 8, 9, or 10.

In another aspect, a process is provided for forming LiO₂. The process includes providing an electrochemical cell, where the electrochemical cell includes a porous oxygen carbon cathode, a lithium anode, a current collector, and an electrolyte. The porous oxygen carbon cathode may include both reduced graphene oxide and a metal catalyst. The following step is discharging of the electrochemical cell form a discharge product. The discharge product includes the LiO₂, and the LiO₂ is free of Li₂O and Li₂O₂.

As noted above, “free of” indicates, at least in some embodiments, that the LiO₂ is spectroscopically pure. Accordingly, the LiO₂ may exhibit a Raman absorption peak at 1123 cm⁻¹. In addition, to further clarify “free of” x-ray diffraction may be used to evidence the purity of the LiO₂. For example, the x-ray diffraction may have peaks of 2θ of 2.530; 2.590; 2.710; 3.000; 3.060; 3.250; 3.500; 3.750; and/or 4.120. Alternatively, a pure sample of LiO₂ may be void peaks of 2θ of 2.321, 2.464, 2.851, 3.400, 4.020, and 4.747.

The discharging may further include cycling of the electrochemical cell, i.e. discharging and charging cycles. As illustrated above, a single cycle may be from 1 hour to 48 hours, or multiple cycles may endure for hundreds of hours. The cycling may also be conducted at a predetermined capacity. For example, the capacity may be greater than 100 mAh/g. This may include, but is not limited to, a capacity from 100 mAH/g to about 2000 mAh/g, or a capacity of about 1000 mAh/g. The cycling may also include cycling the electrochemical cell at a predetermined current density. For example, the current density may be greater than 10 mA/h. This may include, but is not limited to cycling at a current density of 10 mA/h to 500 mA/h, or cycling the electrochemical cell at a current density of about 100 mA/h.

The present invention, thus generally described, will be understood more readily by reference to the following examples, which are provided by way of illustration and are not intended to be limiting of the present invention.

EXAMPLES

Example 1

Preparation and Electrochemical Evaluation of rGO (reduced graphene oxide) and Ir-rGO cathodes (reduced graphene oxide having nanoparticulate iridium). Graphene oxide was prepared by a modified Hummers method. See Hummers, W. S. et al. J. Am. Chem. Soc. 80, 1339 (1958) and Xu, Y. et al. ACS Nano 4, 4324 (2010). The graphene oxide was then dispersed (1 mg/ml) in ethylene glycol (EG) with the aid of horn sonication for 1 hour. The pH of the graphene oxide dispersion was adjusted to 13 with NaOH (2.5 M in EG). The temperature of the dispersion was then increased to 120° C., and NaBH₄ dissolved in EG was injected slowly. The resultant reduced solution was held at temperature for 1 hour, and then cooled to room temperature. The precipitate was filtered, washed, and dried under vacuum.

IrCl₃.H₂O was then added to 100 ml of an aqueous dispersion of the reduced graphene oxide (0.67 mg/ml) from above, and the resultant mixture was stirred for 2 hours. The solution was then transferred to a Teflon®-lined autoclave and reacted hydrothermally at 180° C. for 12 hours. The precipitate, Ir-rGO (iridium—reduced graphene oxide), was filtered, washed, and dried under vacuum.

Electrochemical characterization of the Ir-rGO was carried out using a Swagelok-type cell. The cell included a lithium metal anode, an electrolyte (1M LiCF₃SO₃ in tetraethylene glycol dimethyl ether (TEGDME) impregnated into a glass fiber separator), and a porous cathode ( 7/16 inch diameter). The cells were sealed except for the aluminum grid window that exposed the porous cathode to 1 bar O₂ pressure. The electrochemical measurements were carried out using a MACCOR cycler. The discharge-charge performance was conducted over the voltage range of 2.2V to 4.5V, at a constant current of 100 mA/g, and where the cell was maintained in 1 bar O₂ atmosphere to avoid negative effects of humidity and CO₂.

Characterization. SEM images of the rGO and Ir-rGO composite (FIGS. 1A and 1B, respectively) reveal porous 3-dimensional (3D) networks of rGO composed of wrinkled 2D rGO sheets. FIGS. 1C and 1D show TEM images of the Ir nanoparticles on rGO, indicating that the well-dispersed Ir nanoparticles decorated on rGO are very small (<2 nm), with evidence for the presence of some small Ir clusters (circled in FIG. 1D), and possibly even atoms. A backscattering image (see FIG. 5B) shows some scattered larger Ir particles of about 500 nm in size, which may be due to an agglomeration of smaller nanoparticles.

Performance. The performance of the rGO and Ir-rGO cathodes was examined using a Swagelok-type cell composed of a lithium metal anode, electrolyte (1M LiCF₃SO₃ in tetraethylene glycol dimethyl ether (TEGDME) impregnated into a glass fiber separator, and a porous cathode (see supplementary materials). A current density of 100 mA/g is used for both discharge and charge and the cell was run under time control of 10 hours (capacity of 1000 mAh/g). It should be pointed out that the expression of the specific capacity (mAh/g) and the current density (mA/g) are based on the active materials of the O₂ electrodes. FIGS. 2A and 2B show voltage profiles for the Ir-rGO and rGO cathode architectures, respectively. The Ir-rGO discharge product shows a very low charge potential of about 3.2 V that rises to 3.5 V over 40 cycles leading to over 85% efficiency in this system (FIG. 2A). The voltage profile of the rGO cathode shows a much larger charge potential of about 4.2 V with lower efficiency of 67% (FIG. 2B).

The discharge product resulting from the Ir-rGO cathode was examined using SEM, HE-XRD, TEM and Raman with the results shown in FIGS. 2C/D and 3C/D. The SEM image in FIG. 2C shows the Ir-rGO cathode after discharge (2.75 V) from the first cycle (1000 mAh/g capacity). This image indicates that the discharge product resulting from the Ir-rGO-based cathode has mainly nanoparticles with needle-like or rod-like morphology, although other shapes such as cubic cannot be ruled out. This is also observed by the TEM image of a part of the discharge product that appears to be on the Ir-rGO nanostructures (FIG. 2D). The discharge product from the rGO-based cathode has a range of morphologies including toroids and nanoparticles (See FIG. 13).

FIG. 14A is a voltage profile for deep discharge (about 9500 mAH/g at a current density of 100 mA/g) on the Ir-rGO cathode. FIG. 14B is an XRD pattern for discharge product on deep discharge showing presence of Li₂O₂, LiO₂, and LiOH. When the Ir-rGO cell is run to deep discharge of 2.2 V and about 9,500 mAh/g capacity the HE-XRD data shows evidence for the presence of LiO₂, Li₂O₂, and LiOH with a toroidal morphology. FIGS. 15A and 15B are FTIR spectra of (A) charged Ir-rGO cathode and (B) separators (from discharge cathode capacity of 1000 mAh/g, and a current density of 100 mAh/g) after 2, 8, 30 cycles.

FIG. 7A shows that when rGO is used without the Ir nanoparticles, the discharge product has Li₂O₂, LiO₂, and LiOH. This confirms the role of Ir in LiO₂ formation. The morphology is different—also toroids (FIG. 7) rather than nanoneedles/nanorods for LiO₂. In FIG. 3A the peroxide is listed as well as in 7B. Without being bound by theory, while the material initially includes LiO₂ without contamination, FIG. 3A illustrates that the peroxide appears after 7 days of aging due to disproportionation. Additionally, the peroxide appears after degradation of the catalyst.

The XRD pattern in FIG. 3A for the discharge product on the Ir-rGO cathode (1000 mAh/g capacity) during the first cycle shows peaks corresponding to crystalline LiO₂ [(101), (111), (120)], and no evidence for peaks corresponding to Li₂O₂. The identification of the LiO₂ peaks is based on a theoretical XRD pattern derived from the DFT predicted crystalline LiO₂ structure (See FIG. 8) from Lau et al. J. Phys. Chem. C 115, 23625 (2011), and Zhuravlev et al. J. Struct. Chem. 51, 1005 (2010), as no experimental XRD pattern has been reported. LiO₂ may be characterized by 2θ peaks according to the following table:

XRD Peak 2θ (degree)
(011)    2.530
(020)    2.590
(101)    2.710
(111)    3.000
(120)    3.060
(200)    3.250
(210)    3.500
(121)    3.750
(211)    4.120
(130)    4.220
(002)    4.340
(031)    4.450
(221)    4.690
(131)    4.740
(112)    4.810
(022)    5.050
(230)    5.070

At a λ=0.11165 Å, Li₂O₂ crystals are characterized according to the following table (P63_mmc):

XRD Peak	2 θ (degree)	Intensity (rel)
(100)	2.321	33.70
(101)	2.464	100.00
(102)	2.851	29.96
(004)	3.313	4.18
(103)	3.400	18.46
(110)	4.020	51.21
(104)	4.045	13.23
(112)	4.348	3.65
(200)	4.643	2.37
(201)	4.716	7.62
(105)	4.747	29.54
(202)	4.929	5.01
(006)	4.970	2.40

Iridium is characterized according to the following x-ray diffraction data:

XRD Peak	2 θ (degree)	Intensity (rel)
(111)	2.87	100.00
(200)	3.31	51.76
(220)	4.69	39.99

The LiO₂ structure is orthorhombic and is similar to that of NaO₂, but different from KO₂, which is in tetragonal phase at room temperature. The standard Li₂O₂ XRD pattern was used to determine the absence of Li₂O₂. The Raman spectra of the discharge product of the Ir-rGO cathode in FIG. 3B features a peak at 1123 cm⁻¹, consistent with the signature of LiO₂, and a peak at 1505 cm⁻¹ that is attributed to the strong interaction between LiO₂ and graphitic carbon surface. No evidence of lithium peroxide was found. Evidence for the stability of the lithium superoxide is seen in the XRD pattern 48 hours later, as it remains unchanged from original XRD patterns. In contrast, the XRD pattern (See FIG. 7B) for the discharge product on the rGO cathode without Ir added (1000 mAh/g capacity) during the first cycle shows peaks corresponding to both crystalline LiO₂ [(101), (111), (120)] and Li₂O₂ [(101), (102), (103) and (110)].

Further evidence that the discharge product is LiO₂ from the Ir-rGO cathode was obtained by an experiment in which Li was electrochemically added to the discharge product without the presence of O₂ (i.e. the O₂ was replaced by Ar). The voltage profile is shown in FIG. 3C for this discharge process, along with that of the initial discharge process (to 1000 mAh/g). The XRD of the resulting product with no O₂ in the cell is shown in FIG. 3D and reveals strong peaks for Li₂O₂, thus indicating a conversion of LiO₂ to Li₂O₂ (Li⁺+e⁻+LiO₂→Li₂O₂) with 96% of the theoretical capacity for this reaction is attained. This is clear evidence that a reaction involving one-electron per O₂ in the first cycle for 1000 mAh/g capacity is being observed, and that no Li₂O₂, crystalline or amorphous, forms on this capacity limited discharge.

The stability of the LiO₂ was investigated by carrying out XRD measurements on Ir-rGO cathodes aged for different times in the presence of the electrolyte (FIG. 3A). After twelve hours at the end of both the first and second discharges they show only evidence for crystalline LiO₂. When the discharge product is allowed to sit for seven days under the same conditions, both samples still show mostly signature of LiO₂ with a small presence of crystalline Li₂O₂. Thus, the XRD measurements indicate that the crystalline LiO₂ formed with the Ir-rGO cathode is surprisingly stable for a relatively long period of time. In addition, LiO₂ is still the dominant discharge product on the 20^th discharge cycle indicating that LiO₂ is stable enough that it can be repeatedly charged and discharged for about 40 cycles with a very low charge potential (about 3.2 V).

It was observed that an Ir₃Li intermetallic phase formed on the large iridium agglomerates seen in the backscattering image (See FIG. 5B), as shown in FIGS. 3F/G. Nanoparticles (needle-lke or rod-like) formed on the surface of these agglomerates during the 1^st discharge (FIG. 3E). It is interesting to point out that the Ir₃Li intermetallic phase has a similar crystallographic space group (orthorhombic) to that of LiO₂. Without being bound by theory, it is believed that the Ir₃Li intermetallic phase supports LiO₂ formation by templating the growth of the crystalline LiO₂, due to a lattic matching.

Density functional theory (DFT) calculations were carried out on the interface between LiO₂ and Ir₃Li. FIG. 9A illustrates the configuration (top and side view) of epitaxial growth of LiO₂ crystals (i.e. in P_nnm orthorhombic lattice) in a (111) orientation on a (121) facet of Ir₃Li (i.e. in the I_mm2 orthorhombic lattice) crystalline substrate. From DFT calculations, the lattice mismatch between the LiO₂ crystalline film and the Ir₃Li substrate is only about 0.25 Å in both the a and b lattice of LiO₂ (or about +6.3% and −5.1% in the a and b lattice of LiO₂ crystal). FIG. 9B is a graph showing the basis of the preferred orientation growth of LiO₂ on Ir₃Li is supported by the low interfacial energy γ_interface (in eV/Ų) based on DFT calculations. As shown in 9B, the average interface energy γ_interface is about −0.12 eV/Ų based on different thicknesses of LiO₂ film on two different Ir₃Li substrates (i.e. stoichiometric and Li-rich). Based on the DFT calculated γ_interface (interface energy), γ_substrate (substrate surface energy) and γ_film (film surface energy), we found γ_substrate≧γ_film+γ_interface, which follows the Frank-van der Merwe mode in epitaxial growth model (J. H. van der Merwe, in R. Vanselow (ed.), Chemistry and Physics of Solid Surfaces, CRC Press, Boca Raton, Fla., 1979, p. 209).

The kinetic stability of crystalline and amorphous LiO₂ was investigated using ab initio molecular dynamics (AIMD) and density functional theory (DFT) with the results shown in FIG. 4. The disproportionation rate will depend on several factors. One factor is the rate at which the O₂ leaves the surface. The DFT results in FIG. 4A indicate that the initial step of O₂ leaving the clean surface into vacuum has a barrier of about 0.9 eV, based on one of the low energy LiO₂ surfaces. FIG. 4B shows that crystalline LiO₂ surfaces (i.e. (101) and (111)) are thermally stable in vacuum at room temperature. For an amorphous surface, the barrier is less (about 0.3 eV) than for the crystalline surface as shown in FIG. 4C. From AIMD simulations, the presence of electrolyte molecules adsorbed on the amorphous LiO₂ surface reduces O₂ desorption. This suggests that adsorbed electrolyte on the LiO₂ surface may prevent disproportionation of the crystalline phase. The other factor controlling the disproportionation rate is the barrier to reorganization of the LiO₂ atomic positions allowing for O₂ diffusion to the surface to replace the missing surface O₂. The barriers for this are likely to be large in a crystal lattice, which can also contribute to the unexpected stability of crystalline LiO₂.

The Ir-rGO cathode also exhibits a low charge potential, which may be due to several factors. As shown in FIG. 4D, crystalline LiO₂ is a half metal based on density functional calculations, and, thus, will have good electronic conduction in contrast to insulating bulk Li₂O₂. Ir is a good oxygen evolution catalyst and it interacts strongly with LiO₂ to form a good interface for electrical contact. These properties may explain why the discharge product formed on just rGO has a large charge potential, i.e., it lacks the Ir nanoparticles. The lithium air cell based on Ir-rGO cathode material also can cycle for as much as 40 cycles before failure (FIG. 2A), similar to what has been found for Li₂O₂ based Li—O₂ cells, indicating that the lithium superoxide is not any more reactive towards the electrolyte than lithium peroxide. In addition, the low charge potential will lead to less side reactions. The failure of the cell could be due to both oxygen crossover to the anode resulting in the anode being converted to LiOH (See FIG. 10) and poisoning of Ir metal catalyst with cycling.

Characterization. The phase structures of the discharge products were identified using high energy X-ray diffraction (HE-XRD) with a wavelength of 0.11165 Å, performed at beamline 11ID-C of Sector 11 at the Advanced Photon Source (APS) of Argonne National Laboratory. The X-ray specimens were sealed with Kapton tape as a protective film in the glove box to avoid side reactions with air. The XRD patterns were collected in the transmission mode. During the course of the measurements, a high-energy X-ray beam hit the sample horizontally, and a 2D detector (Perkin Elmer large area detector) was used to collect the X-ray diffraction profiles using transmission mode. The 2D patterns were then integrated into conventional 1D patterns (intensity vs. 2θ) for final data analysis using the Fit2d software.

Scanning transmission electron microscopy (TEM, JEOL JEM-2100F FEG FasTEM with an accelerating voltage of 80 kV) was employed to evaluate the morphology and particle size of the Ir catalysts and the discharge products on the porous cathodes. Spherical and chromatic aberration correction enables the microscope to reach the information limit better than 0.1 nm (measured by Young's fringes) at 80 kV. To prepare the TEM specimens, a dilute suspension was prepared by ultrasonically dispersing the samples in ethanol for 5 min, and a drop of the suspension was placed onto a copper grid and dried. Particle size histograms were generated from the TEM images using software ImageJ. Field-emission scanning electron microscopy (SEM, Hitachi S-4700) coupled with backscattering electron imaging (BSE) was employed to determine the morphology and estimate the particle size of Ir catalyst and discharge products.

Raman spectra of the discharged cathode were obtained using a Renishaw 2000 or in Via microscope spectrometer with a HeNe laser at exciting wavelength of 633 nm. The sample was loaded inside of a glove box to a gas-tight Raman cell with glass or quartz window. Raman spectrum collection was set up in a 180° reflective mode. Roughly 10% of the maximum 13 mW laser intensity was applied. Collection time constant setting varied from 30 seconds to about 100 seconds. There is no evidence of any significant side reactions in the Raman data for the first discharge cycle (FIG. 3) or from Raman and FTIR data for after charging for up to 30 cycles (See FIGS. 11 and 15A/B). These also confirm that the discharge product is consumed upon charging.

Theoretical calculations. To study the stability of LiO₂ systems (i.e. crystal, crystalline surfaces, amorphous-like thin films) and its interface with an electrolyte, we carried out Density Functional Theory (DFT) calculations with plane wave basis sets as implemented in the VASP code. P. Hartmann et al., Nat. Mater. 12, 228 (2013). All calculations were spin-polarized and carried out using the gradient corrected exchange-correlation functional of Perdew, Burke and Ernzerhof (PBE) under the projector augmented wave (PAW) method, with plane wave basis sets up to a kinetic energy cutoff of 400 eV. X. Ren, Y. Wu, J. Am. Chem. Soc. 135, 2923 (2013). The PAW method was used to represent the interaction between the core and valence electrons, and the Kohn-Sham valence states (i.e. is for H, 2s for Li, 2s 2p for C and O) are expanded in plane wave basis sets. Laoire et al. J. Phys. Chem. C 113, 20127 (2009). For the geometry optimization and Nudge Elastic Band calculations, the convergence criterion of the total energy was set to be within 1×10⁻⁵ eV for the K-point integration, and all the atoms and geometries were optimized until the residual forces became less than 1×10⁻² eV/Å.

For LiO₂ crystals, the calculation is based on a mesh of 9×9×9 in K-point grid. For both the crystalline and amorphous-like LiO₂ thin film surfaces, the K-point grid of 6×6×1 was used. For the Ab Initio Molecular Dynamics (AIMD) simulations, all the calculations were carried out with the convergence criterion of the total energy set to be within 1×10⁻⁴ eV in kinetic energy cutoff of 300 eV. For the simulations of LiO₂ surfaces with the electrolyte molecules, the Van der Waals method of Grimme (i.e. DFT-D2) is used throughout both the DFT and AIMD calculations. Abraham et al. J. Electrochem. Soc. 143, 1 (1996). For the simulation of the electrolyte, a smaller ether solvent molecule, i.e. dimethoxy ethane (DME) is used instead of TEGDME in order to reduce the computational cost. To investigate the thermodynamic stability of the system at room temperature, all the structures from the DFT optimizations were then thermally equilibrated at T=300K using AIMD simulations based on an Nose-Hoover NVT-ensemble with a time step of 1 femtosecond.

FIG. 5 shows SEM images of the Ir-rGO cathode. FIG. 5A is the secondary electron image, while FIG. 5B is the backscattering image.

FIG. 6 is thermogravimetric analysis (TGA) curves of Ir-rGO. The iridium content of the Ir-rGO composite was determined to be 49 wt % Ir. The Brunauer-Emmett-Teller (BET) specific surface area of the pristine rGO powder and the Ir-rGO composite is 51.7 m²/g and 342 m²/g, respectively. The pore volume is 0.049 cm³/g and 0.3136 cm³/g for the corresponding samples. Because the Ir nanoparticles supported on rGO can prevent the re-stacking of rGO sheets during the drying process, the Ir-rGO composite shows higher porosity. FIG. 7A is an SEM image of a discharge product from the rGO cathode, while FIG. 7B is an XRD of the discharge product from rGO cathode. The results in FIG. 7 provide additional evidence that Ir nanoparticles are responsible for the LiO2 in the discharge product

FIG. 8 provides the theoretical (LiO₂) XRD pattern derived from the DFT predicted crystalline LiO₂, and experimental XRD patterns for crystalline Li₂O₂ and Ir under the wavelength 0.11165 Å. FIG. 9A is an illustration of the AIMD time evolution of total energy of an amorphous-like LiO₂ thin film surface thermally equilibrated at 300K for 2 picoseconds in simulation time. As shown, the under-coordinated superoxide (O₂) bonded on the amorphous-like LiO₂ surface tends to desorb as an O₂ molecule (resulting in disproportionation) when exposed to a vacuum. In FIG. 9B the AIMD time evolution of total energy of the amorphous-like LiO₂ thin film surface covered by a thin layer of dimethoxy ethane (DME) molecules thermally equilibrated at 300K for 2 ps in simulation time. In contrast to the bare surface in FIG. 9A, the adsorbed DME molecules (ΔE about −0.6 eV/DME-molecule) seem to suppress the under-coordinated superoxide (O₂⁻) species bonded on the amorphous-like LiO₂ surface from desorption (which would result in disproportionation). There is no O₂ molecule release during the simulation. Finally, FIG. 10 is a photograph of a lithium metal anode converted to LiOH after cell failure.

While certain embodiments have been illustrated and described, it should be understood that changes and modifications can be made therein in accordance with ordinary skill in the art without departing from the technology in its broader aspects as defined in the following claims.

The embodiments, illustratively described herein may suitably be practiced in the absence of any element or elements, limitation or limitations, not specifically disclosed herein. Thus, for example, the terms “comprising,” “including,” “containing,” etc. shall be read expansively and without limitation. Additionally, the terms and expressions employed herein have been used as terms of description and not of limitation, and there is no intention in the use of such terms and expressions of excluding any equivalents of the features shown and described or portions thereof, but it is recognized that various modifications are possible within the scope of the claimed technology. Additionally, the phrase “consisting essentially of” will be understood to include those elements specifically recited and those additional elements that do not materially affect the basic and novel characteristics of the claimed technology. The phrase “consisting of” excludes any element not specified.

The present disclosure is not to be limited in terms of the particular embodiments described in this application. Many modifications and variations can be made without departing from its spirit and scope, as will be apparent to those skilled in the art. Functionally equivalent methods and compositions within the scope of the disclosure, in addition to those enumerated herein, will be apparent to those skilled in the art from the foregoing descriptions. Such modifications and variations are intended to fall within the scope of the appended claims. The present disclosure is to be limited only by the terms of the appended claims, along with the full scope of equivalents to which such claims are entitled. It is to be understood that this disclosure is not limited to particular methods, reagents, compounds compositions or biological systems, which can of course vary. It is also to be understood that the terminology used herein is for the purpose of describing particular embodiments only, and is not intended to be limiting.

In addition, where features or aspects of the disclosure are described in terms of Markush groups, those skilled in the art will recognize that the disclosure is also thereby described in terms of any individual member or subgroup of members of the Markush group.

As will be understood by one skilled in the art, for any and all purposes, particularly in terms of providing a written description, all ranges disclosed herein also encompass any and all possible subranges and combinations of subranges thereof. Any listed range can be easily recognized as sufficiently describing and enabling the same range being broken down into at least equal halves, thirds, quarters, fifths, tenths, etc. As a non-limiting example, each range discussed herein can be readily broken down into a lower third, middle third and upper third, etc. As will also be understood by one skilled in the art all language such as “up to,” “at least,” “greater than,” “less than,” and the like, include the number recited and refer to ranges which can be subsequently broken down into subranges as discussed above. Finally, as will be understood by one skilled in the art, a range includes each individual member.

All publications, patent applications, issued patents, and other documents referred to in this specification are herein incorporated by reference as if each individual publication, patent application, issued patent, or other document was specifically and individually indicated to be incorporated by reference in its entirety. Definitions that are contained in text incorporated by reference are excluded to the extent that they contradict definitions in this disclosure.

Other embodiments are set forth in the following claims.

Claims

1. A composition comprising LiO2, reduced graphene oxide, and a metal catalyst or residue thereof.

2. The composition of claim 1, which is free of Li2O2 and Li2O.

3. The composition of claim 1, wherein the metal catalyst comprises a metal that forms an intermetallic phase with lithium, and the intermetallic phase has an orthorhombic structure.

4. The composition of claim 1, wherein the metal catalyst comprises Ir, Ru, Pt, or Pd.

5. The composition of claim 1, wherein the metal catalyst comprises Ir.

6. The composition of claim 1, wherein the LiO2 is crystalline LiO2.

7. The composition of claim 3, wherein the intermetallic phase is Ir3Li.

8. An electrochemical cell comprising: an anode comprising lithium metal;a cathode comprising LiO2 that is substantially free of Li2O2 and Li2O; andan electrolyte.

9. The electrochemical cell of claim 8, wherein the cathode further comprises a carbon-based material.

10. The electrochemical cell of claim 9, wherein the carbon-based material comprises graphene oxide.

11. The electrochemical cell of claim 8, wherein the electrolyte comprises a solvent and a lithium salt.

12. The electrochemical cell of claim 11, wherein the solvent comprises an ether-based solvent, a fluorinated ether-based solvent, an oligo(ethylene oxide) solvent, or a mixture of any two or more thereof.

13. The electrochemical cell of claim 11, wherein the lithium salt comprises LiCF3CO2, LiC2F5CO2, LiClO4, LiBF4, LiAsF6, LiPF6, LiPF2(C2O4)2, LiPF4C2O4, LiCF3SO3, LiN(CF3SO2)2, LiC(CF3SO2)3, LiN(SO2C2F5)2), lithium alkyl fluorophosphates, Li(C2O4)2, LiBF2C2O4, Li2B12X12-pHp, Li2B10X10-yHy, or a mixture of any two or more lithium salts, where X is OH, F, Cl, or Br; p is 0, 1, 2, 3, 4, 5, 6, 7, 8, 9, 10, 11, or 12; and y is 0, 1, 2, 3, 4, 5, 6, 7, 8, 9, or 10.

14. An electrochemical cell comprising: an anode comprising lithium metal;a cathode comprising a LiO2; andan electrolyte.

15. The electrochemical cell of claim 14, wherein the cathode further comprises a carbon-based material.

16. The electrochemical cell of claim 15, wherein the carbon-based material comprises graphene oxide.

17. The electrochemical cell of claim 14, wherein the electrochemical cell is a closed electrochemical cell.

18. A process of forming LiO2, the process comprising: providing an electrochemical cell, the electrochemical cell comprising a porous oxygen carbon cathode, a lithium anode, a current collector, and an electrolyte; anddischarging the electrochemical cell to form a discharge product;wherein: the discharge product comprises LiO2;the porous oxygen carbon cathode comprises reduced graphene oxide and a catalyst; andthe discharge product is free of Li2O and Li2O2.

19. The process of claim 15, wherein the LiO2 exhibits a Raman absorption peak at 1123 cm−1, and x-ray diffraction (2θ) peaks of 2.530, 2.590, 2.710, and 3.000 while being void of (2θ) peaks of 2.321, 2.464, 2.851, 3.400, 4.020, and 4.747.