# Patent

## Title
Anode material for ultrafast-charging lithium ion batteries and a method of its synthesis

## Abstract

An anode material for ultrafast-charging lithium ion batteries, the anode material comprising C—Li4Ti5O12. A method of synthesizing an anode material for ultrafast-charging lithium ion batteries, the method comprising the steps of: adding lithium to an organic alcohol to form a first solution; adding titanium via an organic titanium source to the first solution to form a second solution; adding water to the second solution to form a diluted second solution; heating the diluted second solution at a temperature ranging from about 80° C. to about 180° C. to obtain solid Li4Ti5O12; and annealing the solid Li4Ti5O12 in the absence of air to obtain the anode material comprising C—Li4Ti5O12.

## Background
CROSS-REFERENCE TO RELATED APPLICATIONS
This application is a filing under 35 U.S.C. 371 as the National Stage of International Application No. PCT/SG2013/000040, filed Jan. 31, 2013, entitled “AN ANODE MATERIAL FOR ULTRAFAST-CHARGING LITHIUM ION BATTERIES AND A METHOD OF ITS SYNTHESIS”, which claims the benefit of and priority to U.S. Application No. 61/593,600, filed Feb. 1, 2012, both of which are incorporated herein by reference in their entirety for all purposes.


TECHNICAL FIELD
This invention relates to an anode material for ultrafast-charging lithium ion batteries and a method of its synthesis.
BACKGROUND
Ultrafast charging lithium-ion batteries have huge potential market size on demand due to their shortened charging time which can be as quickly as refueling for gas-powered vehicles. However, high-rate recharge produces sudden heating, which gives rise to a fire hazard for high-power batteries with high-cost metallic lithium anode as well as new high-capacity anode materials, such as micro/nano silicon1, SnO22,3, or Co3O44. Compared with the progress of the high-performance cathode materials5-8, there is an urgent task to develop high-performance anode materials for safe high-power lithium ion batteries. Spinel Li4Ti5O12 (LTO) is an ideal host owing not only to its ‘zero-strain insertion’ structural characteristics, but also to its low cost, abundance and environmental benignity.9 However, the inherent insulating characteristic of LTO seriously limits its high-rate capability, which is a key parameter to obtaining high-power density in batteries.10 
In principle, the charging-rate capability of safe lithium ion batteries depends largely on the performance of anode for lithium storage. Although the addition of conductive additives could improve its surface electronic conductivity for achieving high rate capability15, the cost of LTO materials is increased due to complicated procedures and some expensive additives. On the other hand, LTO materials obtained by molten-salt method often need to undergo long-time and high-strength milling.16 The low surface area of sintered grains is also a crucial factor that hampers the improvement of rate performance and available capacities for LTO electrodes. Therefore, there still remains a challenging issue in developing novel structured LTO materials as suitable anodes for ultra-fast charging lithium ion batteries.
To solve the above problems, nanostructured electrode materials with a larger surface area and short path for lithium-ion migration were exploited for increasing the active material/electrolyte interface and shortening the time of Li-ion insertion/extraction. It has been demonstrated that nanostructured LTO materials, such as nanocrystals,17 nanowires,18 hierarchical structure19 as well as their composite with conductive additives,20 could help to fulfill such purpose and also facilitate the electrochemical insertion/extraction of lithium ions. However, although the addition of conductive additives could improve the high rate capability of LTO15-18, the cost of LTO materials is increased due to complicated procedures and some expensive additives.
Furthermore, although ultrathin nanosheets are a desired framework for lithium storage owing to large exposed area and short path for Li ion transfer, smooth facets of the nanosheets are easily bonded when overlapping with each other at high temperatures, which leads to a decrease of surface area and affect the battery's performance. Although assembling the nanosheets into the hierarchical structure is an efficient way to increase their surface area, the high porosity of the electrode makes the power density low and the reported surface area of LTO or TiO2 nanosheets is no more than 140 m2 g−1.21 
SUMMARY
The anode materials with open channels and efficiently exposed facets have a direct influence on the battery's capacity and recyclability. Therefore, the corrugated 2D structure proposed in this project may retain big exposed surface area and improve its capacity. Improvement of surface performance may be achieved with the aid of sample and low-cost structure directing agents.
The present invention provides a facile and sustainable ‘co-hydrolysis’ route for low-cost and large-scale synthesis of novel wavelike spinel LTO nanosheets with ‘carbon joint’ and a promising surface properties, which successfully conquers the insulating characteristic of LTO. In this work, the corrugated spinel single-crystal Li4Ti5O12 nanosheets with high surface area were successfully synthesized using the shortest bifunctional structure-inducing agent. The material has an attractive architecture for the Li-ion battery electrode. Its capacity has a distinct increase owing to the pseudocapacitive effect. As a result, the 2D wavelike LTO with 0.6 wt. % ‘carbon joint’ exhibits excellent capacities of lithium storage at high discharge/charge rates of 10 C-100 C (1.7-17 A g−1) and its full discharging/charging time can be shortened to 1 minute or less. This novel anode material makes it possible to develop safe ‘one-minute charging’ lithium ion batteries and will significantly push forward progress of batteries for fast energy storage.
According to a first aspect, there is provided an anode material for ultrafast-charging lithium ion batteries, the anode material comprising C—Li4Ti5O12.
The anode material may comprise 0.6 wt. % carbon.
The anode material may have a lithium storage capacity of 180-122 mA h g−1.
The anode material may have a discharge/charge rate ranging from 1.7 to 17 A g−1.
The anode material may have a full discharging/charging time of less than or equal to one minute at a discharging/charging rate of 50 C.
The C—Li4Ti5O12 may comprise two-dimensional wavy Li4Ti5O12 nanosheets having carbon joints at adjacent Li4Ti5O12 interfaces between adjacent two-dimensional wavy Li4Ti5O12 nanosheets.
The carbon joints at adjacent Li4Ti5O12 interfaces may be alternated with open channels formed between adjacent two-dimensional wavy Li4Ti5O12nanosheets.
According to a second aspect, there is provided a method of synthesizing an anode material for ultrafast-charging lithium ion batteries, the method comprising the steps of: adding lithium to an organic alcohol to form a first solution; adding titanium via an organic titanium source to the first solution to form a second solution; adding water to the second solution to form a diluted second solution; heating the diluted second solution at a temperature ranging from about 80° C. to about 180° C. to obtain solid Li4Ti5O12; and annealing the solid Li4Ti5O12 in the absence of air to obtain the anode material comprising C—Li4Ti5O12.
The annealing may form carbon joints at adjacent Li4Ti5O12 interfaces between adjacent two-dimensional wavy Li4Ti5O12 nanosheets.
The carbon joints may be alternated with open channels formed between adjacent two-dimensional wavy Li4Ti5O12 nanosheets.
The organic alcohol may be dimethylethanolamine (DMEA).
The annealing may comprise carbonizing a single-molecule layer of the DMEA.



BRIEF DESCRIPTION OF THE DRAWINGS
In order that the invention may be fully understood and readily put into practical effect there shall now be described by way of non-limitative example only exemplary embodiments, the description being with reference to the accompanying illustrative drawings. In the drawings:
FIG. 1 is a schematic illustration of an anode material of the present invention showing formation of a ‘carbon joint’ between overlapped wavelike or wavy LTO nanosheets;
FIGS. 2a and 2b are TEM images of wavelike Li4Ti5O12 nanosheets annealed at 773K;
FIG. 3a is a TEM image of wavelike Li4Ti5O12 nanosheet annealed at 500° C.;
FIG. 3b is an HRTEM image of the nanosheet of FIG. 3a and an inset of its fast Fourier transform pattern;
FIG. 3c is a three dimensional (3D) image of the image of FIG. 3b; 
FIG. 3d is a magnified lattice fringe of the image of FIG. 3b; 
FIGS. 4a and 4b are TEM images with schematic insets of single-layer and overlapped LTO nanosheets respectively;
FIG. 5a is a graph showing X-ray diffraction (XRD) patterns of LTO samples annealed at 623K, 673K, 773K, and 873K;
FIG. 5b is a graph showing X-ray diffraction (XRD) patterns of an LTO sample and a CLTO sample annealed at 873K;
FIG. 6a is a graph showing N2 adsorption-desorption isotherms of an LTO sample annealed at 773 K and the inset shows its pore size distribution;
FIG. 6b is a graph showing N2 adsorption isotherms of an LTO sample annealed at 873 K using measurement of multipoint BET;
FIG. 7 is a graph showing a Magic angle spinning solid-state Li NMR spectra of LTO samples annealed at 473 and 773 K;
FIG. 8 is a graph showing Cross polarization/magic angle spinning solid-state H NMR spectra of LTO samples;
FIG. 9 is a schematic illustration of a formation mechanism of wavelike LTO nanosheets;
FIG. 10 is a graph showing TGA curves of as-synthesized sample at a temperature-rise rate of 10 K min−1;
FIG. 11a is an STEM image of single wavelike LTO nanosheet;
FIGS. 11b, 11c and 11d are EDS elemental maps of Ti, C and O respectively;
FIG. 12a is a graph showing Carbon 1 s XPS spectra of a carbon coated LTO sample calibrated by adventitious carbon at 384 eV;
FIG. 12b is a graph showing Titanium 2 p XPS spectra of a carbon coated LTO sample calibrated by adventitious carbon at 384 eV;
FIG. 13a is a graph showing cyclic voltammogram of CLTO at a scan rate of 0.2 mV s−1;
FIG. 13b is a graph showing cyclic voltammogram of LTO nanosheets at a scan rate of 0.2 mV s−1;
FIG. 14a is a graph showing cycling performance of CLTO cycled at a constant current drain of 10 C and the corresponding Coulombic efficiency;
FIG. 14b is a graph showing cycling performance of CLTO at different charge/discharge rates (10 C-100 C);
FIG. 14c is a graph showing discharging/charging time needed at different charge/discharge rates (10 C-100 C);
FIG. 15 is a graph showing cycling performance of CLTO nanosheets at charge/discharge rate of 50 C;
FIG. 16 is a graph showing cycling performance of LTO nanosheets at different charge/discharge rates (10 C-100 C); and
FIG. 17 is a schematic diagram of a synthesis route of Li4Ti5O12nanosheets.



DETAILED DESCRIPTION OF EXEMPLARY EMBODIMENTS
An exemplary anode material 10 and a method 100 of its synthesis will be described with reference to FIGS. 1 to 17 below.
As shown in FIG. 1, the anode material 10 comprises C—Li4Ti5O12. In a preferred embodiment, the C—Li4Ti5O12 comprises two-dimensional wavy Li4Ti5O12nanosheets 12 having carbon joints 14 at adjacent Li4Ti5O12 interfaces. The carbon joints 14 may be alternated with open channels 16 formed between adjacent two-dimensional wavy Li4Ti5O12nanosheets. Each open channel 16 may arise due to a crest 18 in a wave of a first wavy Li4Ti5O12nanosheet 12-1 coinciding and aligning with a trough 28 in a wave of a second wavy Li4Ti5O12nanosheet 12-2.
Electron Microscopy Analysis
The morphology of the two-dimensional wavy Li4Ti5O12 nanosheet can be observed directly with the help of a transmission electron microscope (TEM). FIG. 2a clearly shows that annealed LTO sample is nanosheet-like structure with a rough surface. Some smaller nanocrystals take the role of pillars to avoid overlap to some extent at high temperature. The wavelike framework with non-periodic corrugation could be also seen, as shown in FIGS. 2a and 2b. In the high-magnification TEM image (FIG. 3b), it can be observed that one set of big-area lattices are present. Its fast Fourier transform pattern (the inset of FIG. 3b) indicates single-crystal framework corresponding to LTO planes zone. The wavelike framework is also supported by a 3D image (FIG. 3c) of LTO nanosheet obtained by Image J software analysis. The lattice on the exposed facet displays an equal interfringe spacing of 0.48 nm along the axis (FIG. 3d), which offers enough space for zero-strain insertion of lithium ions with a diameter of 0.12 nm. The overlapped nanosheets can still retain their exposed surface owing to the unique wavelike structure, which can be directly observed in overlapped LTO nanosheets as shown in FIG. 4.
XRD Patterns Analysis
The X-ray diffraction (XRD) patterns were obtained for the LTO samples annealed at 623, 673, 773 and 873 K, as shown in FIG. 5a All Bragg peaks are consistent with those of spinel Li4Ti5O12 phase (space group Fd/3m (227); JCPDS no. 049-0207). The crystal size increases while increasing temperature based on full width at half maximum of peak (111). There were no significant differences concerning the XRD pattern between LTO and CLTO at high crystallization temperature of 873 K (FIG. 5b). The crystal size is  ̃10 nm after calcination at 500° C. (LTO-500), which is used for subsequence analysis.
Surface Properties Analysis
Surface properties of LTO were also detected via N2 adsorption-desorption method. Its N2 adsorption-desorption isotherms and pore size distribution were measured for LTO sample LTO-500 (FIG. 6). N2 adsorption isotherm is similar with the type III of IUPAC classifications, which describes adsorption on the adsorbent with N2-adsorbent interaction with the absorbed N2 volume of 1200 cm3 g−1. The surface area and total pore volume of LTO-500 nanosheets are 206 m2 g−1 and 0.166 cm3 g−1 respectively, which were obtained from N2 adsorption-desorption isotherm at 77 K using the DFT (density functional theory) method (FIG. 6a). To our best knowledge, this surface area is the largest among all reported results of LTO nanosheets annealed at 773 K. From the pore size distribution curve of LTO, three peaks are present at 1.1, 2.9, 4.6 nm respectively, which are corresponding to its TEM image with different corrugation spacing. Even annealing at 873 K, the sample still has a big surface area of 172 m2 g−1, which was calculated by multipoint Brunauer-Emmet-Teller (BET) method (FIG. 6b). The possible reason is that the overlapped nanosheets can still retain their exposed surface owing to the unique wavelike surface structure, which can be directly observed in overlapped LTO nanosheets as shown in FIG. 4.
Solid-State NMR Analysis
Microenvironments of LTO samples were further explored by solid-state NMR. 7Li magic angle spinning (MAS) spectra of LTO samples annealed at 473 and 773 K were recorded on a JNM-ECA400 spectrometer at 100.5 MHz and chemical shifts were referenced to a 1.0 M lithium chloride aqueous solution. As shown in FIG. 7, the resonance of LTO annealed at 473 K is actually composed of two resonances, a broad resonance due to Li on 16 d and a narrow resonance due to Li on 8 a.22 With increasing the temperature, Li on 16 d jumped on 8 a and the broad resonance (Li on 16 d) disappears. Meanwhile, the spinel Li4Ti5O12 could be obtained from amorphous lithium titanate. The cubic local environment of the 8 a is consistent with the XRD analysis of cubic spinel LTO. The reversible capacity of electrode material is limited by the amounts of protons attached to the surface or the bulk, which is irreversibly replaced by lithium ion when discharging the battery.23 In fact, different amount of protons were present in the LTO nanosheet samples as proved by CP/MAS 1H NMR spectra of LTO samples (FIG. 8). With increasing the temperature, the amount of proton residue decreased. It gives a possible way to improve the reversible capacity of LTO samples which were synthesized in a watery environment.
Formation of Wavelike or Wavy LTO Nanosheets
The actual formation mechanism of the wavelike LTO nanosheets is not yet clarified. A possible one is proposed and schematically illustrated in FIG. 9. First, amorphous lithium titanate can be fast formed because of the co-hydrolysis of lithium and Titanium resources. And what is more, low-cost dimethylethanolamine (DMEA) acts as an effective difunctional structure directing agent with the ammonium group (big head) and hydroxyl group (small tail). The two kinds of functional groups could easily form strong intermolecular hydrogen bonds with Ti—OH groups, which may form a curve by well-organized organic molecular structure and lead to the formation of wavelike structure. Then wavelike amorphous titanate nanosheets were formed along 2D plane direction due to growth along 2D plane direction to form large-scale wavelike nanosheet. The role of DMEA makes it possible to fabricate the wavelike framework with retained high surface area upon overlapping.
After removal of solvent, a single-molecule layer of DMEA is still firmly held on the surface of amorphous titanate nanosheets below 523 K and is decomposed at 573 K or above, which is supported by thermogravimetry (FIG. 10). Therefore, after crystallized in air, white powder is obtained due to the removal of the organic layer. However, the obtained sample is a gray powder after annealed in the absence of air. We hypothesized that ‘carbon joint’ was formed owing to the carbonization of single-molecule DMEA layer. The 0.6 wt. % of exact carbon content is detected by trace elemental analysis. However, the ‘carbon joint’ of 0.6 wt. %, which stemmed from the carbonization of single-molecule DMEA layer, is so low and thin that it is hardly detected by HRTEM image.
Detection of Carbon
To detect the position of carbon, elemental maps of Ti, C and O in CLTO were collected using high-angle annular dark-field scanning transmission electron microscopy (HAADF-STEM) and energy-dispersive X-ray spectroscopy (EDS) technologies. FIG. 11a is STEM image of single LTO nanosheet and its shape is consistent with the elemental maps of Ti and O in FIG. 11b and FIG. 11d. In FIG. 11c, the carbon distribution on the directly exposed 2D LTO surface (oval 2) is close to that on blank part (oval 3), that is, no carbon exists on the directly exposed LTO interface. Luckily, the carbon content at the joint part (oval 1) is higher than that in oval 2 and 3, which confirms our speculation that the carbon exists in the joint of particles. To facilitate the understanding, we provided the schematic formation of ‘carbon joint’ between the overlapped wavelike LTO nanosheets in the absence of air as shown in FIG. 1.
To further confirm the microenvironment of C and Ti, the surface chemical compositions of LTO samples were determined by X-ray photo-electron spectrometer (XPS). The carbon content of CLTO has a significant increase than adventitious carbon at 384 eV (FIG. 12a) as an auxiliary evidence for carbon analysis. The exact contents of carbon cannot be obtained, because the intensity depends not only on the amount of carbon in the sample but also on the amount of loading sample. Moreover, in FIG. 12b, two kinds of Ti4+ peaks on CLTO at 457.1 eV and 457.5 eV are due to the different microenvironment between big exposed surface and inner crystal, which may improve the surface performance for lithium storage. No Ti3+ was detected in CLTO sample.[16]
Electrochemical Studies
The electrochemical studies of the CLTO and LTO annealed at 873 K were obtained using two-electrode Swagelok-type cells with Li metal slices serving as both the counter and reference electrodes at room temperature. The working electrode was composed of 70 wt % of the active material, 20 wt % of conductivity agent (carbon black, Super-P-Li), and 10 wt % of binder (polyvinylidene difluoride, PVDF, Aldrich). The electrolyte used was 1 M LiPF6 in a 1:1 (w/w) mixture of ethylene carbonate and diethyl carbonate. Cell assembly was carried out in an Argon-filled glove box. Cyclic voltammetry (CV, 0.8-2.5 V, 0.2 mV s−1) was performed using an electrochemical workstation (CHI 760D). Galvanostatic charge/discharge cycling was conducted using a battery tester (NEWAER) at different current rates of 10 C-100 C, where 1 C=170 mA g−1. The cyclic voltammetric curve (FIG. 13a) of electrode made of CLTO was determined at a scanning rate of 0.2 mV s−1. The typical current peaks of LTO are obvious at voltages of  ̃1.47 V and  ̃1.66 V. Its insertion-deinsertion peak separation of 0.19 V is smaller than 0.24 V of LTO (FIG. 13b) at the same scan rate, which reflects that CLTO has low polarization.
The cycling performance and needed time of CLTO was studied as a high-rate anode material. FIG. 14a shows the cycling performance of the CLTO at a current drain of 10 C. After 300 charge/discharge cycles, a reversible discharge capacity as high as 151 mAh g−1 can still be retained and its Coulombic efficiency almost approaches 100%. The improvement of capacity at high rate is due to large electrolyte/electrode interface (grain boundaries) that leads to pseudocapacitive insertion/extraction.25 The rate performance of the CLTO at 10 C-100 C was further investigated as shown in FIG. 14b and clearly demonstrates excellent cycling performance at all current rates. At 20 C and 30 C, the discharge capacities are around 171 mAh g−1 and 164 mAh g−1 respectively, which is very close to its LTO theoretical capacity.26 It can still retain 151 mAh g−1 at 50 C. Even at the highest rate of 100 C (17 A g−1), a capacity of 122 mAh g−1 can be held. Evidently, the electrochemical performance of CLTO is one of best results in all reported LTO and TiO2 nanomaterials. Charge/discharge experiment at 50 C was conducted to investigate its high-rate capacities and cycling performance (FIG. 15). After 100 full charge/discharge cycles, their discharge capacity of 148 mAh g−1 can be remained and its Coulombic efficiency also approaches 100%. The electrochemical studies demonstrated that the wavelike CLTO nanosheets exhibit an excellent reversible capacity, stable cycling performance, and superior high-rate capability. The discharging/charging time of CLTO nanosheets shows that this material is ideal anode for ultrafast charging lithium-ion batteries (FIG. 14c). Its full charging time at 10 C, 20 C, 30 C are shortened to  ̃6.5, 3, 2 minutes respectively. At higher rates, the charging time needed is only 1 minute (at 50 C) or less.
As a comparison task, the electrochemical performance of LTO was also studied at high rates from 10 C to 100 C (FIG. 16). It exhibits a high capacity of 165, 147, 129, 101 and 75 mAh g−1 at high discharge/charge rates of 10 C, 20 C, 30 C, 50 C, 80 C respectively, which is superior to the most recently reported LTO materials without any additive.15c, 24, 27 Therefore, the unique surface properties of LTO are conducive to overcoming its insulating characteristic. Compared with LTO nanosheets, the improvement of high-rate performance of CLTO should owe to the ‘carbon joint’ formed at adjacent interface of LTO, by which the surface insulating characteristic of LTO may be significantly improved with the assistance of ‘carbon-joint’. However, the carbon joint, which stemmed from the carbonization of single-molecule DMEA layer, is so thin that it is hardly detected by HRTEM.
On the basis of the above analysis, the wavelike CLTO nanosheets can provide a short path for lithium-ion migration and a big electrolyte/electrode interface for lithium insertion. We believe that wavelike LTO materials with ‘carbon joint’ have extensive application prospect for ultrafast charging lithium-ion batteries and hybrid super-capacitors. We believe that the ‘co-hydrolysis’ method is an alternative approach to develop new high-performance electrode materials.
Method of Synthesis
Compared with traditional molten-salt method,16a amorphous lithium titanate can be obtained at lower temperature due to the uniform distribution of lithium and titanium formed by rapid hydrolysis according to equations (1) and (2) below, which avoid high-temperature melt salts and long-time milling for mixing and reducing grain size.

(CH3)2N(CH2)2OLi+H2O→(CH3)2N(CH2)2OH+LiOH  (1)

Ti(OC4H9)4+4H2O→Ti(OH)4+4C4H9OH  (2)

Furthermore, solvents can be easily removed and reused for a next cycle. After annealing in air and in absence of air, LTO and carbon coated LTO (CLTO) can be facilely obtained in a large scale respectively.
As shown in FIG. 17, the method 100 comprises placing lithium (Li) in an organic solvent such as an organic alcohol (ROH) to form a first solution of ROLi in excess ROH, 102. The organic alcohol ROH also functions as a surfactant without requiring the provision of another template. Titanium (Ti) is added to the first solution of ROLi in ROH solution, via an organic titanium source such as Ti(OR)4, to form a second solution, 104. Water is added to the second solution to form a diluted second solution, 106, followed by heating the diluted second solution at a temperature ranging between 80-180° C., 108. After the heating, a solid intermediate product of wavy Li4Ti5O12nanosheets is obtained together with unused solvent ROH. The unused solvent ROH may be reused in a subsequent cycle of synthesis. Wavy Li4Ti5O12 nanosheets are obtained after annealing the solid intermediate product in air. To obtain the C—Li4Ti5O12, the solid intermediate product is then annealed in the absence of air.
In a first exemplary embodiment of the method 100 of synthesis described above, metal Li is put into dimethylethanolamine (DMEA) immersed in an ice-bath to form a solution A (0.5 mol of Li in 200 g DMEA). Tetrabutyl titanate (0.625 mol,  ̃213 g) is then added into solution A to form solution B. The solution B is placed in a Teflon-lined stainless steel reactor and H2O is added to form a diluted solution B (4-5 ml of H2O needed per 15 ml of solution B), followed by heating of the diluted solution B at 433 K for 10 to 24 hours. Solid product from the reaction in the steel reactor can be directly annealed at temperatures ranging from 623K to 873K for 1 to 2 hours respectively, and remaining liquid including DMEA and n-butanol can be reused for a next cycle of synthesis.
In a second exemplary embodiment of the method 100 of synthesis described above, 16 metal Li is put into dimethylethanolamine (DMEA) immersed in an ice-bath to form a solution A (0.5 mol of Li in 200 g DMEA). Tetrabutyl titanate of 0.625 mol ( ̃213 g) was then added into solution A to form a solution B. The solution B is placed in a Teflon-lined stainless steel reactor and H2O is added to form a diluted solution B (4-5 ml of H2O needed per 15 ml solution B), followed by heating of the diluted solution B at temperatures ranging from 80-180° C. for 24 hours. After reaction, white amorphous lithium titanate is obtained due to the uniform distribution of lithium and titanium formed by rapid hydrolysis (as given by equations (1) and (2) above), which avoid high-temperature melt salts and long-time milling for reducing grain size.
The white solid products (LTOs) can be obtained by directly annealing at 350-700° C. for 2 hours and the obtained samples are gray powder (CLTOs) when annealing in the absence of air. Remaining liquid including DMEA and n-butanol can be reused for a next cycle of synthesis.
Sample Characterizations
XRD patterns were performed with a D8 diffractometer with Cu—Kα radiation (λ=1.54056 Å). TEM were obtained with JEOL JEM-1400 and JEOL 2100F. Elemental maps were collected using a JEM 2100F with a HAADF-STEM detector and an Oxford EDS. N2 adsorption-desorption isotherms were conducted at 77 K on a Micromeritics Tristar 3000 analyzer. The BET surface areas and pore-size distribution curves were concluded using adsorption data. 7Li, and 1H Cross Polarization/Magic-Angle Spinning (CP/MAS) or MAS NMR measurements, a JNM-ECA400 spectrometer was used at 100.5 and 400.0 MHz, respectively. X-ray photoelectron spectroscopic (XPS, KRATOS, AXIS ULTRA DLD) measurements were carried out by using a monochromated Al Kα (1486.7 eV) X-ray source at power of 150 W (15 kV×10 mA). The XPS analysis was carried out at room temperature under a typical pressure in the range of 1.0 e−9 Torr—5.0 e−9 Torr, at take-off angle relative to the surface holder of about 90°. Thermogravimetric analysis was determined using a thermal gravity analyzer (TGA) at a temperature-rise rate of 10 K min−1 from room temperature to 1073 K under a continuous air flow. Carbon trance analysis is determined using EuroVector Euro EA elemental analyzer
Compared with other reported methods for titanium based anode materials, the low-cost material of the present invention exhibits the best performance as shown in Table 1 below.









TABLE 1








Capacities atdifferent charging rates




(1 C = 170 mA g−1)/mA h g−1













Materials
10 C
20 C
30 C
50 C
Reference















CLTO
180
170
160
150
This work


Titanate
155
145
125
100
Adv. Mater. 2011, 23, 998


nanosheets







TiO2 nanosheets
120
98


J. Am. Soc. Chem. 2010, 132, 6124


LTO
160
120


Electrochem. Commun., 2011, 13,







650


Mesoporous
125

91

Adv. Mater. 2007, 19, 2087


TiO2







Li4Ti5O12/C
130
125


Energy Environ. Sci., 2011,







DOI:10.1039/C1EE01680F


Li4Ti5O12/C
110



Energy Environ. Sci., 2011, 4, 1345









As described above, wavelike LTO nanosheet can be formed having a big exposed surface area of 205 m2 g−1 for lithium insertion. The ‘carbon joint’ of 0.6 wt. % can be synthesized in situ without other additives. The CLTO product can be prepared on a large scale and it can endure high-rate charge from 10 C to 100 C (1.7-17 A g−1), while the needed charging time can be shortened to 1 minute or less.
Whilst there has been described in the foregoing description exemplary embodiments of the present invention, it will be understood by those skilled in the technology concerned that many variations in details of design, construction and/or operation may be made without departing from the present invention. For example, the method can also be used to synthesize many other materials, such as cobalt, zirconium doped C—Li4Ti5O12, silica and zirconia based materials.
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## Claims

1. An anode material for ultrafast-charging lithium ion batteries, the anode material comprising C—Li4Ti5O12 having a nanosheet structure.

2. The anode material of claim 1, wherein the anode material comprises 0.6 wt. % carbon.

3. The anode material of claim 1, having a lithium storage capacity of 180-122 mA h g−1.

4. The anode material of claim 1, having a discharge/charge rate ranging from 1.7 to 17 A g−1.

5. The anode material of claim 1, having a full discharging/charging time of less than or equal to one minute at a discharging/charging rate of 50C.

6. The anode material of claim 1, wherein the C—Li4Ti5O12 comprises two-dimensional wavy Li4Ti5O12 nanosheets having carbon joints at adjacent Li4Ti5O12 interfaces between adjacent two-dimensional wavy Li4Ti5O12 nanosheets.

7. The anode material of claim 6, wherein the carbon joints at adjacent Li4Ti5O12 interfaces are alternated with open channels formed between adjacent two-dimensional wavy Li4Ti5O12 nanosheets.

8. A method of synthesizing an anode material for ultrafast-charging lithium ion batteries, the method comprising the steps of:
adding lithium to an organic alcohol to form a first solution;
adding titanium via an organic titanium source to the first solution to form a second solution;
adding water to the second solution to form a diluted second solution;
heating the diluted second solution at a temperature ranging from about 80° C. to about 180° C. to obtain solid Li4Ti5O12; and
annealing the solid Li4Ti5O12 in the absence of air to obtain the anode material comprising C—Li4Ti5O12 having a nanosheet structure.

9. The method of claim 8, wherein the annealing forms carbon joints at adjacent Li4Ti5O12 interfaces between adjacent two-dimensional wavy Li4Ti5O12 nanosheets.

10. The method of claim 9, wherein the carbon joints are alternated with open channels formed between adjacent two-dimensional wavy Li4Ti5O12 nanosheets.

11. The method of claim 8, wherein the organic alcohol is dimethylethanolamine (DMEA).

12. The method of claim 11, wherein the annealing comprises carbonizing a single-molecule layer of the DMEA.