Pechini Synthesis of Nanostructured Li_1.05M_0.02Mn_1.98O₄ (M = Al³⁺ or Ga³⁺)

Abstract

Doped Li_1.05M_0.02Mn_1.98O₄ (M = Ga³⁺ or Al³⁺) were prepared by Pechini synthesis using lithium and manganese acetates, citric acid, ethylene glycol, and the respective oxide or acetate of the doping ions in molar ratios of 2.00 (Mn_1.98 + M_0.02) to 1.05 Li. The TGA/DTA of the precursor gels showed weight loss/energy relative to crystallization below 450 ºC. From the XRD, a single cubic phase (F_d3m) was identified for the all-doped or undoped oxides after only 2 h calcination. The unit cell parameters a for both aluminum- and gallium-doped oxides calcined at 750 °C for 2 h (8.212 Å and 8.210 Å, respectively) were higher than that for the undoped oxide (8.199 Å). The crystallite sizes ranged from ~ 20 nm to 70 nm, conferring nanometric character. The specific capacities decreased in order: C_discharge (Li_1.05Mn₂O₄) >C_discharge (Li_1.05Ga_0.02Mn_1.98O₄) >C_discharge (Li_1.05Al_0.02Mn_1.98O₄), but with increasing capacity retention for the doped samples.

Keywords:
doped spinel; LiMn₂O₄; Jahn Teller effect; lithium-ion battery; Pechini method; nanostructured oxide

1 Introduction

Despite that electrical energy is indispensable today we must also consider the importance of portable power sources, especially the batteries, responsible for the operation of the main electronic marketed. Concern for the environment has increased significantly, many people recognize the importance of preserving natural resources. Thus, new and less-polluting products have been developed in an attempt to minimize the deleterious effect that is inherent to the industrial activity on the environment.

Materials, such as biodegradable plastics have been used more frequently; furthermore, recycling has gained importance, becoming an essential tool for reducing waste. Energy sources have also undergone major changes over the years and there is currently a range of clean energy sources as well as essential, renewable energy sources, such as wind¹, solar², and geothermal³ energies, which currently produce about 10% of the energy used in the world⁴.

Over the years, portable power sources and batteries, including AAA batteries, have undergone changes in terms of being reduced in size and improved in power capabilities, following a constant update of portable electronic items. It is estimated that over 10 billion batteries, including rechargeable batteries, are sold annually throughout the World⁵. From these, over 50% are incorrectly discarded in the regular trash. In Brazil, despite the creation of laws that assign obligations to businessmen and consumers, it is noted that these devices continue to be dispensed into the trash⁶.

The lack of inspection and awareness associated with impunity contributes to the noncompliance of laws and, consequently, to the contamination of the environment with the toxic metals from which these batteries are made. Among the metals, cobalt and lithium are present in so-called lithium-ion batteries, which represent secondary batteries that are most commonly consumed today. These batteries were introduced in the market in 1991 by Sony Energy Tech Incorporation⁷ and their charging involves the removal of lithium ions from a LiMO₂ electrode and their insertion into a lithiated carbon electrode, according to a process known as the "Rocking Chair"⁸.

The lithium-ion batteries have a lithiated graphite anode (LiC₆) and a cathode that, in current batteries, is composed of lithium cobaltate (LiCoO₂), which has a high charge capacity and high stability, increasing battery life. On the other hand, this cathode material represents about 30% of the world demand for cobalt, which caused the price to reach US$ 660.00 per kilogram in 2008^[9], making LiCoO₂ a very expensive material that, consequently, also makes their by-products expensive, as is the case for lithium-ion batteries¹⁰.

In addition to economic issues, both cobalt and lithium are toxic to living organisms and may accumulate in the environment, contaminating soil, water, plants, and animals, getting to man. In an organism, these metals may cause dysfunction, mainly in the respiratory system, causing decreased lung function, and may cause congestion, edema, and hemorrhage in the lungs¹¹.

In view of the neglect towards the environment and the high value LiCoO₂ has acquired¹², it is believed that the best alternative would be to replace the LiCoO₂ in batteries with of a less harmful material that could be more abundant, and consequently cheaper than cobalt-containing batteries. In this way, LiMn₂O₄ emerges as an interesting option for this issue, as many Mn reserves exist in the world (5.7 billion tons in 2006)¹³, and this, as well as its oxide, presents little risk to the environment.

On the other hand, LiMn₂O₄ presents a problem in terms of maintaining its ability to charge storage as compared to LiCoO₂. The Jahn–Teller effect occurs because of a structural anisotropic distortion in the d orbitals from Mn³⁺, changing the compact cubic symmetry to tetragonal symmetry. This local distortion is related to the vacancy/occupancy of the e_g antibonding orbital of the Mn³⁺ ion during successive charge and discharge cycles^14-17. The gradual loss of specific capacity leads to a decrease in the useful life time of these batteries, which could represent huge financial losses. This problem can be minimized by reducing the Mn³⁺ amount in the spinel structure and increasing the Mn⁴⁺ amount, which do not suffer Jahn–Teller distortion. In order to achieve that, one can dope, that is, replace a certain amount of trivalent manganese (in proportions less than 5%) in the lithium manganate structure with other trivalent cations that have similar ionic radii and do not present the Jahn–Teller distortion¹⁸.

Furthermore, it is known that the charge-storage capacity of these materials is strongly influenced by the surface characteristics and particle size of the oxides that are influenced by the synthetic route. Thus, using the Pechini method can contribute towards achieving nanostructured oxides with unique crystallographic phases that present electrochemical activity. The principle of this method consists of chelate formation among metallic cations and a carboxylic acid (citric acid) with subsequent esterification reaction between the formed chelate and a polyalcohol (ethylene glycol), giving rise to a polymer precursor¹⁹. The formed substance will yield a homogeneous oxide after thermal treatment. The Pechini method can be realized at low temperatures, allowing stoichiometric control of the atoms in the crystalline structure and the obtainment of highly pure and nanometric powders, making it a valuable method for obtaining cathodic materials²⁰.

Considering this, the main objectives of this work were to investigate the efficiency of the Pechini methodology for the production of stoichiometric Li_1.05Mn₂O₄ and to assess its doping with gallium and aluminum, analyzing whether there is an improvement in the electrochemical behavior of the doped samples compared with the undoped samples. The purpose of this synthesis route was to produce materials to be used as cathodes in environmentally less-harmful lithium-ion batteries that present a minimized Jahn–Teller effect.

2 Material and Methods

2.1 Preparation of the dopant precursor

The following precursors were used in the synthesis of the doped Li_1.05M_0.02Mn_1.98O₄ oxides (M = Ga³⁺ or Al³⁺): Ga₂O₃ (Aldrich, PA) and Al(C₂H₃O₂)₂ (Aldrich, PA). The doped oxides were prepared by Pechini synthesis with the precursors in the molar ratios of 2.00 (Mn_1.98 + M_0.02), 1.05 Li, and 1.00 (citric acid).

Doping with gallium was performed using gallium hydroxide, which was obtained by dissolving Ga₂O₃ (Aldrich, PA) in hydrochloric acid (Merck, PA). After dissolution, the pH of the solution was adjusted to 4.5 by addition of 2.0% ammonium hydroxide (Mallinckrodt, PA). More simply, the aluminum dopant was obtained by direct addition of basic aluminum acetate, requiring no treatment with hydrochloric acid.

2.2 Synthesis of Li1.05M0.02Mn1.98O4 (M=Ga3+ or Al3+)21-23

To obtain a homogeneous material with the same stoichiometric control, the molar ratio of precursors were 1.05:1.98 for lithium and manganese acetates (Aldrich, PA), 0.02 of the doping metal (aluminum or gallium) (Aldrich, PA), and 1:4 citric acid (Synth, PA) to ethylene glycol (Synth, PA). Doping was performed by adding gallium hydroxide in deionized water whilst stirring and heating. Subsequently, citric acid was added under constant stirring. The pH of the solution was increased to 10.0 with the addition of 2.0% NH₄OH, forming a translucent yellow-colored solution. This clear solution was added to ethylene glycol (Vetec, PA). The ratio used to prepare these samples was calculated from the molar ratio 1:4 citric acid to ethylene glycol. The solution was stirred and heated to obtain a viscous resin. The undoped oxide was also synthesized for comparative purposes. First, citric acid was dissolved in distilled water, followed by addition of lithium, manganese, and gallium acetates; NH₄OH (Aldrich, PA) was used to adjust the pH to between 9 and 10. Then, ethylene glycol was added drop-wise, stirring to form a viscous liquid that was heated up to 140 °C in order to form a gelatinous material (polymer precursor).

2.3 Calcination of the polymeric precursor

The resulting gel was calcined for various times (30, 60, 120, and 360 min) and at various temperatures (500, 600, 700, and 750 °C). A sample obtained by solid-state reaction at 750 °C for 24 h (2880 min) was used as a reference. The particle size of the calcined oxides was controlled by deagglomeration in mortar by passing the sample through a #325 mesh sieve (smaller than 45 μm).

2.4 Thermal characterization by TGA/DTA

Thermogravimetric analysis (TGA/DTA) were performed on DTG-60H Shimadzu equipment, Simultaneous DTA-TG apparatus. The heating routine occurred from room temperature (approximately 25 °C) to 1000 °C at 10 °C min^–1 using N₂.

2.5 Structural characterization by XRD

The structural characterization was performed by X-ray diffraction (XRD) using a Shimadzu diffractometer (Model 6000, radiation Cu Kα, λ = 1.5406 Ǻ) with a voltage of 40 kV, current of 30 mA, at 2θ min^–1 from 10° to 80°. The crystallite sizes were calculated using the Scherrer equation^24-30, the full width–half maximum (FWHM), were calculated from the widening of the basal XRD peak (d₁₁₁), the unit cell parameters, a, were calculated using the Unit Cell Win program, with the adjustment of the XRD peaks previously made on the Peak Fit software.

2.6 Morphological characterization by SEM

SEM images were obtained using a Hitachi electronic scanning microscope, Model 3000, enlarging the images 1000 and 5000 times with acceleration voltages of 5 and 10 kV.

2.7 Specific surface area determination by B.E.T.

The specific Brunauer–Emmett–Teller (B.E.T.) surface areas were determined by the Micromeritics ASAP 2020 apparatus from nitrogen adsorption isotherms at 77 K. Prior to the analysis, the samples were degassed overnight at 150 °C with a heating rate of 10 °C min^–1.

2.8 Cell assembly and electrochemical characterization by Cyclic Voltammetry and Charge/Discharge

For the electrochemical evaluation, electrodes were made with 85% of the synthesized oxide (by mass), 10% acetylene black (Vulcan XC 72-GP 2800, Cabot Corp., USA), and 5% polyvinylidene fluorine (PVDF) (Aldrich, PA) dispersed in cyclohexanone (Aldrich, PA). The sludge containing the electrode material was painted on the platinum.

The electrodes containing the synthesized oxide were then submitted to cyclic voltammetry measurements in a potential range of –0.5 to 1.30 V vs. Ag/AgCl at 0.5 mV s^–1, using a disassembled cellular telephone battery (LiC₆) as the counter electrode and conventional liquid organic solvent used in lithium batteries, EC/DMC (ethyl carbonate/ dimethyl carbonate) containing LiClO₄ 1 mol L^-1 (as electrolyte) using an Autolab potentiostat 302 N, interfaced with a microcomputer using GPES software version 4.9.

Chronoamperometry tests to evaluate the charge-storage capacity of the cathodes were carried out using an anodic current of 40 µA (C/1) up to 4.35 V (vs. Li/Li⁺) and 80 µA (C/2) up to 3.60 V (vs. Li/Li⁺), in a dry Labconco chamber (Model 50600) with controlled humidity (< 10 ppm of H₂O) by passage of argon (Air Liquid, 99.999%).

3 Results and Discussion

3.1 Thermal characterization by TGA/DTA

Figure 1a, b show the DTA/TGA curves of the precursor gels used in the Pechini synthesis for doped and undoped LiMn₂O₄ powders. There was heat absorption (endothermic reaction) at the approximate temperatures of 100, 200, and 450 °C. These thermal reactions can be related to water evaporation, organic residue elimination, and sample crystallization, respectively, according to Suryakala et al.²⁵. Similarly to the DTA, the mass losses at temperatures of 100, 200 and 450 °C correspond to water elimination, organic compound elimination, and crystallization of the sample, respectively. These results are in agreement with those obtained by Huang, as he also identified three well-defined mass-loss phases during LiMn₂O₄ synthesis using the solid-state reaction²⁶. After 500 °C, there was no further mass loss, nor release or heat absorption, allowing us to confirm that, after this temperature, no further reaction occurred. However, the samples calcined at 500 °C did not show satisfactory electrochemical profiles and, therefore, although the samples are already crystallized at this temperature, they did not acquire an ideal spinel structure for lithium-ion intercalation and deintercalation, as can be seen in Figure 2.

Figure 1
DTA (a) / TGA (b) curves of the precursor gel of Pechini synthesis.

Figure 2
Cyclic voltammograms of the electrodes: (a) Li_1.05Mn₂O₄; (b) Li_1.05Ga_0.02Mn_1.98O₄; (c) Li_1.05Al_0.02Mn_1.98O₄, calcined at 600 °C or 750 °C for 120 min; in EC/DMC LiClO₄ 1 mol L^–1 at 0.5 mV s^–1.

3.2 Structural characterization by XRD

The XRD patterns of the oxides subjected to different thermal treatments show that the samples calcined at 750 °C formed structures similar to the pattern in JCPDS 35-0782, as shown in Figure 3a, b. However, the obtained structures at 700 °C already showed significant structural similarities with few interferences, which can mainly be observed in the doped samples, with aluminum showing higher phase ordering and crystallinity. Furthermore, it is possible to note that the undoped samples showed a large amount of interferences, which may be related to the insufficient calcination time, as these additional peaks are not observed in the XRD patterns of the samples calcined for longer periods, as shown in Figure 4.

Figure 3
XRD patterns of the: (a) Li_1.05Mn₂O₄; (b) Li_1.05Ga_0.02Mn_1.98O₄ and (c) Li_1.05Al_0.02Mn_1.98O₄, calcined for 120 min at different temperatures.

Figure 4
XRD patterns of the: (a) Li_1.05Mn₂O₄; (b) Li_1.05Ga_0.02Mn_1.98O₄; (c) Li_1.05Al_0.02Mn_1.98O₄, calcined at 750 °C for different times.

Regarding the calcination time, it was observed that at longer times, the oxide structures presented unique phases and were more organized (Figure 4), which shows the differences between the XRD patterns of the calcined doped and undoped Li_1.05Mn₂O₄ samples at different times. Besides, the XRD patterns of the samples doped with aluminum showed a higher ordering of the phase and less impurities at all times evaluated. Figure 4 shows well-defined diffraction peaks for the samples calcined for more than 120 min, presenting structures similar to that of the stoichiometric spinel LiMn₂O₄(JCPDS 35-782) with a cubic unit cell belonging to the F_d3m. However, the samples calcined for 360 min were more organized and crystalline, as evidenced by the FWHM (Figure 5).

Figure 5
FWHM of the Li_1.05Mn₂O₄, Li_1.05Ga_0.02Mn_1.98O₄ and Li_1.05Al_0.02Mn_1.98O₄ as a function of the: (a) temperature calcination (for 120 min); (b) time calcination (at 750 °C).

3.2.1 FWHM

According to Manev et al.²⁷ and Lee et al.²⁸, the position and FWHM of the (400) plane peak are important factors, indicating the crystallinity degree of a spinel powder. The narrow shape of the reflections, quantified by the full width at half maximum (FWHM) of the main reflections considered as signs of high crystallinity and well-ordered structure. It can be seen in Figure 5a, b that FWHM values were gradually decreased from 0.55º to 0.15º (average values). It indicates the crystallinity of oxide is gradually improved with enhancing the calcination temperature and time. That the synthesized samples are as crystalline as those with higher calcination times. All samples presented high crystallinity at calcination times of 1440 min (XRD does not show); however, the samples doped with aluminum showed, even after 60 min, higher crystallinity than the other samples; therefore, it is expected that a higher insertion of lithium ions occurs in these samples²⁹. When comparing the variation of the FWHM as a function of the temperature, it is also possible to observe that the crystallinity of the samples increases as the temperature increases (Figure 5). Moreover, it can be noted that the temperature is the factor that most affects the crystallinity, as the FWHM decreases abruptly.

3.2.2 Unit cell parameter

In order to evaluate the influence of the doping on the crystalline lattice of the obtained spinel oxides, the unit cell parameter a was calculated from the XRD data by the least-squares method. Figure 6a, b show the unit cell parameter of the samples calcined at different times and temperatures, which presented higher crystallinity and resemblance to the standard stoichiometric LiMn₂O₄ (a = 8.247 Å, JCPDS 35-0782). Amatucci et al.³⁰ reported a value of a = 8.235 Å for Li_xMn₂O₄ (x = 1.03) obtained by solid-state reaction at 800 °C for 24 h. In general, doped samples showed similar values than the undoped samples, suggesting effective doping, as this process is associated with the substitution of Mn³⁺ ions (ionic radius of 0.65 Å) in octahedral sites (16d) by cations of the same oxidation state and smaller ionic radius (Al³⁺ or Ga³⁺ with ionic radius of 0.53 or 0.63 Å, respectively)³¹. Thus, it is possible to justify the higher values for the samples doped with Ga³⁺. However, these reduced values suggest that the oxides suffer less deformation during cycling, which results in a lower specific-capacity loss.

Figure 6
Unit cell parameters of the Li_1.05Mn₂O₄, Li_1.05Ga_0.02Mn_1.98O₄ and Li_1.05Al_0.02Mn_1.98O₄ (Å) as a function of the: (a) temperature calcination (for 120 min); (b) time calcination (at 750 °C).

3.2.3 Crystallite size

According to the values shown in Figure 7a, b, the crystallite sizes were found to increase as the calcination temperature and time increases. These results are in agreement with those obtained by Chaves³² that used the Pechini method for obtaining cerium and nickel oxide. This increase in the crystallite size can be explained by the reduction of internal stresses that occur with the increase in temperature that allows further growth of the crystallites³³. However, it is also possible to observe that the crystallite size increases as the calcination time increases, as shown in Figure 7b, due to the decrease in surface tension. The crystallite sizes of the oxides increased from ∼20 nm to ∼70 nm, indicating that the crystallinity of LiMn₂O₄ is gradually improved with enhancing the time and temperature, tendency also reported by Zhan et al.³⁴ using the solid state reaction to produce stoichometric LiMn₂O₄. But in this work, the crystallite sizes were smaller than those obtained by solid state reaction, indicating character nanometric of the particles.

Figure 7
Crystallite sizes of the Li_1.05Mn₂O₄, Li_1.05Ga_0.02Mn_1.98O₄ and Li_1.05Al_0.02Mn_1.98O₄as a function of the: (a) temperature calcination (for 120 min); (b) time calcination (at 750 °C).

3.3 Morphological characterization by SEM

The SEM images of the Li_1.05Mn₂O₄, Li_1.05Ga_0.02Mn_1.98O₄, and Li_1.05Al_0.02Mn_1.98O₄ samples calcined at 750 °C for 120 min showed that, in general, the undoped samples presented a greater uniformity in terms of the size of their particles compared to the doped samples (Figure 8). Furthermore, for all samples, the formation of large cluster numbers can be observed, as also reported by Chaves³², which is a typical feature of nanostructured particles, due to the intense attractive van der Waals forces acting among the particles³⁵. Furthermore, it was observed that these clusters have symmetrical geometric form and a wide particle distribution, similar for spinel MgAl₂O₄ oxides.

Figure 8
SEM images of the: (a) and (d) Li_1.05Mn₂O₄; (b) and (e) Li_1.05Ga_0.02Mn_1.98O₄; (c) and (f) Li_1.05Al_0.02Mn_41.98O₄; calcined at750 °C for 120 min.

3.4 Specific surface area determination by B.E.T.

Table 1 shows the specific surface area data determined by the BET method for the different LiMn₂O₄ oxides obtained by different synthesis routes. It can be seen that the surface area for the oxides synthesized by the Pechini method were higher than those by solid-state reaction (even when subjected to further mechanical ball milling)¹⁸. However, these values were lower than those obtained by combustion synthesis (~ 8.88 m² g^–1)^36,37, probably because of the large volume of gases released by the combustion method during the synthesis. Higher B.E.T. surface area values were found for LiMn₂O₄ obtained by other authors by sonochemical (6.8 m² g^–1)³⁸, but lower values by sol gel methods (1.08 m² g^–1)³⁹. In general, the values found in this study were higher than the average found in literature. This surface area confirmed the reduced crystallite size and the existence of clusters consisting of nanometric particles⁴⁰.

Table 1
Specific surface area data (B.E.T.) for Li_1.05Mn₂O₄ obtained by different synthesis methods.

oxides	B.E.T. (Solid State Reaction) [18]/ m2 g–1	oxides	B.E.T. (Pechini)/ m2 g–1
Li1.05Mn2O4 750°C / 24 h	2.23	Li1.05Mn2O4/ 750 °C 2 h	4.67
Li1.05Mn2O4 750 °C / 24 h + 15 min ball milling	4.55	Li1.05Al0.02Mn1.98O4 /750 °C 2 h	5.59
Li1.05Mn2O4 750 °C / 24 h + 30 min ball milling	4.53	Li1.05Ga0.02Mn1.98O4/ 750 °C 2 h	5.14

3.5 Electrochemical characterization by Cyclic Voltammetry and Charge/Discharge

Figure 9 shows the stabilized cyclic voltammograms (3^rd cycles) of the oxides calcined at 750 °C for 60 or 120 min. The voltammetric profiles of the samples calcined for 120 min were similar to those obtained for stoichiometric LiMn₂O₄, showing that the redox processes occur in two stages, at 1.10/0.87 V ( I/IV in Figure 9) and 1.15/1.00 V ( II/III) vs. Ag/AgCl, corresponding to the desintercalation/intercalation of the first lithium ion in the Li_xMn₂O₄ structure (0 ≤ x ≤ 1) in the octahedral sites¹⁶. It was observed that the sample doped with gallium and aluminum showed redox peaks that were better defined, indicating a higher charge-storage capability in this potential range. However, these redox processes were not evidenced for oxides calcined at 750 °C for 60 min. Furthermore, the desintercalation/intercalation of the second lithium ion in the Li_xMn₂O₄ structure (1 ≤ x ≤ 2) occurred in one stage at 0.20/–0.35 V ( V/VI), suggesting a higher charge storage in the tetrahedral sites¹⁶. Although, the calcination time influenced the electrochemical profiles, it was also possible to observe higher variations in the voltammetric profiles of the samples calcined at 600 and 750 °C for 120 min, indicating that a higher calcination temperature is necessary (Figure 2).

Figure 9
Cyclic voltammograms of the electrodes: (a) Li_1.05Mn₂O₄; (b) Li_1.05Ga_0.02Mn_1.98O₄; (c) Li_1.05Al_0.02Mn_1.98O₄, calcined at 750 °C for 60 or 120 min; in EC/DMC LiClO₄ 1 mol L^–1 at 0.5 mV s^–1.

Figure 10 shows the specific discharge capacity calculated for the samples calcined at 750 °C for 120 min. It was observed that after ten cycles, the specific discharge capacity was kept between 105 and 100 mA h g^–1 for all samples, which are closer to the practical capacities of 120 mA h g^-1 (80% of the theoretical values), indicating that lithium-ion intercalation/deintercalation processes were favored in the oxide structure, due to the higher ordering of the phase and the fewer impurities present in the oxide for this investigated calcination time and temperature.

Figure 10
Discharge specific capacities of the electrodes of the oxides calcined at 750 °C for 120 min, in EC/DMC LiClO₄ 1 mol L^–1 ati_c= 40 µA (C/1) and i_a= 80 µA (C/2).

4 Conclusions

It was possible to obtain a doped lithiated manganese oxide in the stoichiometric spinel phase with a cubic structure by the Pechini method at low calcination temperatures and times. Thus, LiMn₂O₄ doped with aluminum and gallium resulted in a single cubic phase at 750 °C for only 120 min of calcination. The crystallite sizes ranged from ~20 nm to ~70 nm, conferring nanometric character of the synthetized oxide particles. The unit cell parameter a calculated for doped spinel samples calcined with aluminum and gallium for 2 h at 750 °C (8.212–8.210 Å) were higher than for the undoped samples (8.199 Å). The temperature increase and the varied calcination times provided samples with higher crystallinity and crystals organization that favored lithium-ion insertion and extraction in the oxide structure. The SEM images of the oxides showed symmetrical geometric forms with a wide particle distribution. The voltammetric profiles of the samples calcined for 120 min were similar to those obtained for LiMn₂O₄, showing that the redox processes occurred in two stages, corresponding to lithium-ion deintercalation/intercalation in the Li_xMn₂O₄ structure (0 ≤ x ≤ 1). It was observed that the sample doped with gallium and aluminum showed more well-defined redox peaks, indicating a higher charge-storage capability in this potential range. However, these redox processes were not evidenced for oxides calcined at 750 °C for 60 min. Thus, the oxides calcined at 750 °C for 120 min showed high specific capacity values (80% of the theoretical values), decreasing in the order C_discharge (Li_1.05Mn₂O₄) >C_discharge (Li_1.05Ga_0.02Mn_1.98O₄) >C_discharge. (Li_1.05Al_0.02Mn_1.98O₄), but with a greater conservation of the discharge capacity for the doped samples after ten charge and discharge cycles.

Acknowledgments

We acknowledge MIZUMO (Jacto group). This work is a collaboration research project of members of the Rede Mineira de Química (RQ-MG) supported by FAPEMIG (Project: APQ 2279/2010).

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Publication Dates

• Publication in this collection
  17 Nov 2015
• Date of issue
  Dec 2015

History

• Received
  15 Dec 2014
• Reviewed
  30 Aug 2015