Advances in Materials Science and Engineering

Volume 2013 (2013), Article ID 137032, 7 pages

http://dx.doi.org/10.1155/2013/137032

Research Article

Structural and Electrochemical Investigation of Li1.02Mn1.92Al0.02Fe0.02Cr0.02 () Synthesized by Solid-State Method

Hai-Lang Zhang and Nanchun Xiang

School of Chemical and Material Engineering, Jiangnan University, Wuxi City, Jiangsu 214122, China

Received 31 May 2013; Accepted 4 October 2013

Academic Editor: Markku Leskela

Copyright © 2013 Hai-Lang Zhang and Nanchun Xiang. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

Abstract.

To improve the cycle performance of spinel LiMn₂O₄ as the cathode of 4-V-class lithium secondary batteries, spinel phases Li1.02Mn1.92Al0.02Fe0.02Cr0.02 (, 0.08) have been successfully prepared by a conventional solid-state method. The structure and physicochemical properties of this as-prepared powder were investigated by powder X-ray diffraction (XRD), electrochemical impedance spectroscopy (EIS), and galvanostatic charge-discharge test in detail. The results reveal that the multiple doping spinel Li1.02Mn1.92Al0.02Fe0.02Cr0.02O₄F0.08 have better electrochemical performance than the undoped or only metal-element doped material, which may be contributed to the multiple cation and anion doping to lead to a more stable spinel framework with good capacity retention rate.

1. Introduction

Spinel LiMn₂O₄ has been regarded as one of the most promising cathode materials for lithium-ion batteries in virtue of its obvious advantages such as the abundant and cheap resources, environmental benignity, safety, high voltage, and good rate of capability [1]. So it has been extensively investigated as a cathode material for lithium-ion batteries [2]. Although LiMn₂O₄ cycles well at room temperature, prolonged cycling at higher temperatures is accompanied by an unacceptable fading of capacity [3]. This severe capacity fading is mainly due to the Jahn-Teller distortion on the surface of spinel LiMn₂O₄ [4], the dissolution of manganese in the electrolyte solution [5, 6], the spinel LiMn₂O₄ with oxygen deficiency [7], and the decomposition of electrolyte solution on the electrode [8, 9]. To overcome this problem, many researchers have studied the mechanisms of capacity fading and many methods for the cyclability improvement of spinel cathodes have been suggested.

Doping is considered to be an effective path to improve the electrochemical performance of LiMn₂O₄, so several attempts have been made for improving synthesis of lithium manganese spinels by doping with various metals, such as Al, Mg, Co, Cr, Ni, Fe, and Cu. [10–15]. It may be expected that replacing part of the manganese with another metal could increase the stability of the spinel structure and improve the cycling performance of Li-Mn spinel when it is employed as the cathode active material [16]. Although such substitutions often result in enhanced stability of the spinel, the initial discharge capacity of the doped spinels decreases significantly and is lower than that of the parent compound. Single-ion-doped LiMn₂O₄ spinels could not counteract all the factors responsible for the capacity loss. The effect of multiple cation-substituted LiMn₂O₄ has been reported and it has been pointed out that codoping has a synergistic effect on the improvement of the cycling life of the materials as cathodes in lithium batteries [17]. It has been demonstrated that the cyclic stability of LiMn₂O₄ could be improved by doping anion F [18–21]. So in this work codoping cations and anion F has been designed to improve the properties of LiMn₂O₄.

In this work, the cathode materials LiMn₂O₄, Li1.02Mn1.92Al0.02Fe0.02Cr0.02O₄, and Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08 have been successfully prepared by the high temperature solid-state reaction. The physical characteristics and electrochemical properties of the synthesized products have also been investigated in detail.

2. Experimental Section

2.1. Materials Preparation

The spinel LiMn₂O₄, Li1.02Mn1.92Al0.02Fe0.02Cr0.02O₄, and Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08 powders were prepared by a simple solid-state reaction. A stoichiometric amount of Li₂CO₃, MnO₂, Al(NO₃)₃·6H₂O, HF, Cr(NO₃)₃·6H₂O, and Fe(NO₃)₃·6H₂O was thoroughly ground in an agate mortar and pelletized. The pellets were heated at 700°C for 12 h to drive off CO₂ and then calcined in a muffle at for 20 h in air. The heating rate was  min⁻¹ and the cooling rate to room temperature was −3°C min⁻¹. After cooling to room temperature, the pellets were ground again.

2.2. Structure and Morphology Characterization

The structure of products was characterized by an X-ray diffractometer (D/Max-3B, Japan) with CuKα radiation operating at 40.0 kV and 30.0 mA. XRD data were collected in the ranges from to .

2.3. Electrochemical Measurements

After mixing the active material (80 wt%) with acetylene black (12 wt%) and polyvinylidene fluoride (PVDF) binder (8 wt%) in N-methylpyrrolidinone (NMP) solvent, the mixed slurry was attained. The slurry was coated on an aluminum foil by a doctor balde technique in a vacuum oven at for 12 h. The cells were assembled in an Ar-filled glove box. The CR2032 coin cell comprises a cathode, a Celgard (2325) separator, and a Li-foil anode. The electrolyte was 1 M LiPF₆ in a 1 : 1 (volume ratio) mixture of ethylene carbonate (EC) and dimethyl carbonate (DMC). Charge-discharge characteristics were tested galvanostatically on a Land CT2001A (Wuhan, China) between 3.0 and 4.5 V (versus Li/Li⁺). Cyclic voltammetry measurements of the prepared powders were performed in the voltage range 3.0–4.5 V at a scan rate of 0.1 mV s⁻¹. The electrochemical impedance measurements were carried out in the frequency range from 100 KHz to 0.01 Hz with an AC voltage signal of ±5 mV.

3. Results and Discussion

3.1. X-Ray Diffraction

Figure 1 presents the XRD pattern of LiMn₂O₄, Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08, and Li1.02Mn1.92Al0.02Fe0.02Cr0.02O₄. All samples were identified as a pure spinel phase with a space group Fd3m where lithium ions occupy the tetrahedral sites (8a) and manganese and substituting metal ions reside at the octahedral (16d) sites [22]. This fact may indicate that the Mn site in LiMn₂O₄ is substituted fully by Al-, Cr-, and Fe-, respectively, and no other phase is formed.

Figure 1: The XRD patterns of (a) LiMn₂O₄, (b) Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08, and (c) Li1.02Mn1.92Al0.02Fe0.02Cr0.02O₄ obtained by the high temperature solid-state reaction.

The lattice parameters, which were calculated from the diffraction data through the least-squares method, and the unit cell volumes of the samples are given in Table 1. It could be found that all the substituted samples have lattice parameters values smaller than those of LiMn₂O₄. This is due to the smaller size of the substituting ions Li⁺ (0.059 nm), Al³⁺ (0.054 nm), Cr³⁺ (0.0615 nm), and Fe³⁺ (0.064 nm) as compared with the larger Mn³⁺ ion (0.066 nm) [23]. The decrease in cell volume should increase the stability of the spinel structure during the insertion and deinsertion of lithium [16], and thereby the electrochemical cycle stability of the sample could be improved. In addition, the Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08 has a little larger lattice parameter than the Li1.02Mn1.92Al0.02Fe0.02Cr0.02O₄, which is due to the fact that monovalent fluorine substitutes for divalent oxygen reduce Mn⁴⁺ to Mn³⁺ and thus increase the quantity of the larger trivalent manganese Mn³⁺. The increase of Mn³⁺ will slightly increase the unit cell volume of the Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08 compared to that of Li1.02Mn1.92Al0.02Fe0.02Cr0.02O₄ and elevate the initial specific capacity.

Table 1: Lattice parameters of samples.

Samples
Lattice parameters volume ()
Unit cell volume ()

Li₂Mn₂O₄
8.246
560.279

Li1.02Mn1.92Al0.02Fe0.02Cr0.02O₄
8.232
558.572

Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08
8.237
559.132

3.2. Charge-Discharge Characteristics

Figure 2 shows the initial charge-discharge curves of the prepared samples at room temperature and a constant current density of C/3 in the potential range from 3.0 to 4.5 V. It can obviously be seen that the charge-discharge curves of all the samples have two distinctive voltage plateaus, characteristic of the well-defined spinel LiMn₂O₄ cathode, which implies that there are two steps for lithium intercalating and deintercalating into the material [24]. Compared with the pure LiMn₂O₄, the charging plateau potential for the doped samples rises and the discharge plateau potential drops. This may mainly be due to the stronger chemical bond of Al–O, Fe–O, and Cr–O than Mn–O, which can reinforce the lattice energy of the doped samples, which needs expending more energy for lithium ions to extract or to insert.

(a)

(b)

(c)

Figure 2: The charge-discharge curves of cells (a) Li/LiMn₂O₄, (b) Li/Li1.02Mn1.92Al0.02Fe0.02Cr0.02O₄, and (c) Li/Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08.

The initial capacity of or is lower than that of pure LiMn₂O₄. The initial discharge capacity of , , and is 121.5, 115.6, and 117.8 mAh·g⁻¹, respectively. This decrease of initial capacity is because the composition of the substituting spinel can be written as and , respectively. Compared with the initial composition of , the number of ions in the substituted spinel phase is decreased. In fact, only the contributes to the charge-discharge capacity during the intercalation-deintercalation of in .

In order to study the influence of doping ions on the cyclability, the cells were tested at a charge-discharge current density of C/3 between 3.0 and 4.5 V. The variations of the discharge capacity with the cycle number for LiMn₂O₄, Li1.02Mn1.92Al0.02Fe0.02Cr0.02O₄, and Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08 are shown in Figure 3. It is obviously found that the cyclabilities of Li1.02Mn1.92Al0.02Fe0.02Cr0.02O₄ and Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08 have been significantly improved. Although the pure LiMn₂O₄ had the highest initial discharge capacity, its capacity retention ratio was 82.1% after 50th cycle. However, the capacity retention ratio of Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08 is 96.8% after 50th cycle. The capacity retention ratio of Li1.02Mn1.92Al0.02Fe0.02Cr0.02O₄ is 91.5% after the 50th cycle. Moreover, spinel Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08 shows better cycle performance and a slightly higher capacity than the spinel Li1.02Mn1.92Al0.02Fe0.02Cr0.02O₄ because the substitution of Mn by Cr, Fe, Al, and Li decreases the unit cell volume and the decrease of Mn³⁺ concentration reduces the Jahn-Teller distortion and also stabilizes the structure integrity of the active. In addition, the Cr, Fe, Al, Li, and F codoping in LiMn₂O₄ increases the binding energy in the octahedral MO₆ sites. Thus, the simultaneous cation and anion substitution of LiMn₂O₄ with Cr, Fe, Al, Li, and F improves the cycling performance of spinel LiMn₂O₄ more than cation-only substitution of LiMn₂O₄ with Cr, Fe, Al, and Li.

Figure 3: Cycle performance of cells (a) Li/, (b) Li/Li1.02Mn1.92Al0.02Fe0.02Cr0.02O₄, and (c) Li/Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08 at room temperature.

Figure 4 shows the cycling performance of the Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08 electrode at 25 and in voltage range of 3.0–4.5 V, respectively. To investigate the rate capability upon cycling, various current densities of C/3 and 1C were applied to the working electrode. From Figure 4, it can be seen that the synthesized Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08 material exhibits excellent cycling stability at room and elevated temperature even at high current densities. For the electrode cycled at , the initial discharge capacity is 117.5 and 111.8 mAh·g⁻¹ at C/3, 1C rate, respectively. At 55°C, the initial discharge capacity is 118.1 and 111.5 mAh·g⁻¹ at C/3, 1C rate, respectively. The capacity retention ratio is 96.8% and 91.7% after the 50th cycle at and at C/3 rate and 94.7% and 88.1% after the 90th cycle at 1C rate, respectively. It is well known that high rate discharge capability and cycle stability are the most important electrochemical parameters for battery applications [25]. Therefore, the results obtained above confirm that the Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08 sample is an attractive material for practical applications.

(a)

(b)

Figure 4: Cycling performance of the Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08 electrode at different current densities in voltage range of 3.0–4.5 V at and .

3.3. Cyclic Voltammetry

The cycle voltammogram properties of the cells LiMn₂O₄ and Li1.02Mn1.92Al0.02Fe0.02Cr0.02O₄F0.08 after 2 and 50 cycles were tested. Cyclic voltammograms with the sweep rate of 0.05 mV s⁻¹ in the potential region of 3.0–4.5 V are presented in Figures 5(a) and 5(b), respectively. For both cyclic voltagrams, there are two pairs of reversible peaks, oxidation and reduction peaks, corresponding to Li⁺ extraction and insertion, which reflect the typical Mn³⁺/Mn⁴⁺ redox process of the spinel structure in the 4 V domain [26].

(a)

(b)

Figure 5: Cyclic voltammograms of cells containing (a) LiMn₂O₄ and (b) Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08 after 2 and 50 cycles.

The difference between the two samples is that the redox peaks of the Li1.02Mn1.92Al0.02Fe0.02Cr0.02O₄F0.08 electrode are sharp and show well-defined splitting, which indicates that the Li1.02Mn1.92Al0.02Fe0.02Cr0.02O₄F0.08 powder is more crystalline than pure LiMn₂O₄. In addition, the peak current of pure electrode for the 50th cycle is much lower than that for the 2nd cycle, which indicates that the cycling leads to a distinct capacity fading. In comparison, the peak current of Li1.02Mn1.92Al0.02Fe0.02Cr0.02O₄F0.08 with cycling almost does not decrease, and the curve for the 50th cycle is approximately the same as that for the 2nd cycle. This strongly demonstrates that the cycling performance of the Li1.02Mn1.92Al0.02Fe0.02Cr0.02O₄F0.08 electrode is significantly improved.

3.4. EIS Studies the Spinel Electrodes

AC impedance spectroscopy is a powerful technique for determining the kinetic parameters of the electrode process [27]. The Nyquist plots obtained at the CV peak potential (4.16 V) for LiMn₂O₄, Li1.02Mn1.92Al0.02Fe0.02Cr0.02O₄, and Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08 spinels are shown in Figure 6. All the Nyquist plots show two semicircles and a Warburg impedance associated with the diffusion of lithium ions in the oxide matrix. The first semicircle is associated with the passivation layer on the electrode. The second one is associated with the charge-transfer resistance coupled with a capacitance at the surface film/cathode particle interface arising from surface-adsorbed species.

(a)

(b)

(c)

Figure 6: AC impedance experiments measured for the spinel (a) Li/LiMn₂O₄, (b) Li/Li1.02Mn1.92Al0.02Fe0.02Cr0.02O₄, and (c) Li/Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08 electrodes at the potential  V before and after 50 cycles.

From the Nyquist plots, it can be found that in comparison with semicircles of pure LiMn₂O₄, the first and second semicircles of doped LiMn₂O₄ decrease, which indicates that the surface layer resistance and the charge transfer resistance of doped LiMn₂O₄ are smaller than those of pure LiMn₂O₄. In addition, the minimum values of Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08 mean a lower electrochemical polarization, and this leads to a higher electrochemical performance. These EIS phenomena might be able to explain the excellent high rate performance of the spinel Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08 [28]. Also, it can be seen from Figure 6 that total resistance of LiMn₂O₄ and Li1.02Mn1.92Al0.02Fe0.02Cr0.02O₄ evidently increases after 50 cycles, especially for pure LiMn₂O₄. Compared with pure LiMn₂O₄, the resistance of the spinel Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08 almost does not change after 50 cycles. The electrochemical impedance is a major part of internal resistance of a battery and the cycle life of a battery decreases as its internal resistance increases after repeated charge and discharge. Hence, the electrochemical impedance characteristics of the spinel Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08 explains the enhanced cycle life of the multiple doping spinel compared to the pure one. Also, from the EIS property comparison, it could be concluded that Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08 has better electrochemical performance than Li1.02Mn1.92Al0.02Fe0.02Cr0.02O₄.

4. Conclusions

Spinel materilas LiMn₂O₄, Li1.02Mn1.92Al0.02Fe0.02Cr0.02O₄, and Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08 were successfully synthesized by the simple solid-state reaction. Among these synthesized materials, the Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08 sample shows the best cycle performance at room and elevated temperature even at high current densities. The improvement in cycling performance might be attributed to the stabilization in the spinel structure and the suppression of Jahn-Teller distortion by the codoped metal cations and anion F. In addition, the Cr, Fe, Al, Li, and F codoping in LiMn₂O₄ increases the binding energy in the octahedral MO₆ sites. It could be seen that codoping is an effective way to improve the stability of LiMn₂O₄. Li1.02Mn1.92Al0.02Fe0.02Cr0.02O3.92F0.08 is one promising cathode material for Li-ion battery.

References

H.-L. Zhu, Z.-Y. Chen, S. Ji, and V. Linkov, “Influence of different morphologies on electrochemical performance of spinel LiMn₂O₄,” Solid State Ionics, vol. 179, no. 27–32, pp. 1788–1793, 2008.

X. Li, Y. Xua, and C. Wang, “Suppression of Jahn-Teller distortion of spinel LiMn₂O₄ cathode,” Journal of Alloys and Compounds, vol. 479, no. 1-2, pp. 310–313, 2009.

R. Thirunakaran, K. Kim, Y. Kang, C. Seo, and J. Young-Lee, “Adipic acid assisted, sol-gel route for synthesis of LiCrxMn2-xO₄ cathode material,” Journal of Power Sources, vol. 137, no. 1, pp. 100–104, 2004.

Y. P. Fu, C. H. Lin, Y. H. Su, and S. Wu, “Electrochemical characteristic of LiMn1.925M0.075O₄ (, Co) cathode materials synthesized by the microwave-induced combustion method,” Journal of Power Sources, vol. 159, no. 1, pp. 215–218, 2006.

S.-W. Lee, K.-S. Kim, H.-S. Moon et al., “Electrochemical and structural characteristics of metal oxide-coated lithium manganese oxide (spinel type): part I. In the range of 2.5–4.2 V,” Journal of Power Sources, vol. 130, no. 1-2, pp. 227–232, 2004.

R. Thirunakaran, A. Sivashanmugama, S. Gopukumar, C. W. Dunnill, and D. H. Gregory, “Phthalic acid assisted nano-sized spinel LiMn₂O₄and LiCrxMn2−xO₄ () via sol-gel synthesis and its electrochemical behaviour for use in Li-ion-batteries,” Materials Research Bulletin, vol. 43, no. 8-9, pp. 2119–2129, 2008.

M. Takahashi, T. Yoshida, A. Ichikawa et al., “Effect of oxygen deficiency reduction in Mg-doped Mn-spinel on its cell storage performance at high temperature,” Electrochimica Acta, vol. 51, no. 25, pp. 5508–5514, 2006.

R. J. Gummow, A. de Kock, and M. M. Thackeray, “Improved capacity retention in rechargeable 4 V lithium/lithium-manganese oxide (spinel) cells,” Solid State Ionics, vol. 69, no. 1, pp. 59–67, 1994.

G. G. Amatucci, C. N. Schmutz, A. Blyr et al., “Materials' effects on the elevated and room temperature performance of C/LiMn₂O₄ Li-ion batteries,” Journal of Power Sources, vol. 69, no. 1-2, pp. 11–25, 1997.

T. Yi, X. Hu, and K. Gao, “Synthesis and physicochemical properties of LiAl0.05Mn1.95O₄ cathode material by the ultrasonic-assisted sol-gel method,” Journal of Power Sources, vol. 162, no. 1, pp. 636–643, 2006.

H.-J. Choi, K.-M. Lee, and J.-G. Lee, “LiMn1.95M0.05O₄ (M : Al, Co, Fe, Ni, Y) cathode materials prepared by combustion synthesis,” Journal of Power Sources, vol. 103, no. 1, pp. 154–159, 2001.

W. Lu, I. Belharouak, S. H. Park, Y. K. Sun, and K. Amine, “Isothermal calorimetry investigation of Li1+xMn2-yAlzO₄ spinel,” Electrochimica Acta, vol. 52, no. 19, pp. 5837–5842, 2007.

L. Zhang, T. Yabu, and I. Taniguchi, “Synthesis of spherical nanostructured LiMxMn2−xO₄ (M = Ni²⁺, Co³⁺, and Ti⁴⁺; ) via a single-step ultrasonic spray pyrolysis method and their high rate charge-discharge performances,” Materials Research Bulletin, vol. 44, no. 3, pp. 707–713, 2009.

K. Suryakala, G. P. Kalaignan, and T. Vasudevan, “Synthesis and characterization of Cr-doped LiMn2-xCrxO₄ () cathode for Li-ion battery,” Materials Chemistry and Physics, vol. 104, no. 2-3, pp. 479–482, 2007.

K.-S. Lee, H. J. Bang, S.-T. Myung, J. Prakash, K. Amine, and Y.-K. Sun, “Synthesis and electrochemical properties of spherical spinel Li1.05M0.05Mn1.9O₄ (M = Mg and Al) as a cathode material for lithium-ion batteries by co-precipitation method,” Journal of Power Sources, vol. 174, no. 2, pp. 726–729, 2007.

B.-L. He, W.-J. Zhou, Y.-Y. Liang, S. J. Bao, and H. L. Li, “Synthesis and electrochemical properties of chemically substituted LiMn₂O₄ prepared by a solution-based gel method,” Journal of Colloid and Interface Science, vol. 300, no. 2, pp. 633–639, 2006.

F. Bonino, S. Panero, D. Satolli, and B. Scrosati, “Synthesis and characterization of Li₂MxMn4-xO₈ (M = Co, Fe) as positive active materials for lithium-ion cells,” Journal of Power Sources, vol. 97-98, pp. 389–392, 2001.

G. G. Amatucc, N. Pereira, T. Zheng, and J. M. Taraseon, “Failure mechanism and improvement of the elevated temperature cycling of LiMn₂O₄ compounds through the use of the LiAlxMn2-xO4-zFz solid solution,” Journal of The Electrochemical Society, vol. 148, no. 2, pp. A171–A182, 2001.

J. T. Son and H. G. Kim, “New investigation of fluorine-substituted spinel LiMn₂O4-xFx by using sol-gel process,” Journal of Power Sources, vol. 147, no. 1-2, pp. 220–226, 2005.

Y.-J. Kang, J.-H. Kim, and Y.-K. Sun, “Structural and electrochemical study of Li-Al-Mn-O-F spinel material for lithium secondary batteries,” Journal of Power Sources, vol. 146, no. 1-2, pp. 237–240, 2005.

Sh.-J. Bao, Y.-Y. Liang, W.-J. Zhou, B.-L. He, and H.-L. Li, “Enhancement of the electrochemical properties of LiMn₂O₄ through Al³⁺ and F-co-substitution,” Journal of Colloid and Interface Science, vol. 291, no. 2, pp. 433–437, 2005.

Y. Ito, Y. Idemoto, Y. Tsunoda, and N. Koura, “Relation between crystal structures, electronic structures, and electrode performances of LiMn2-xMxO₄ (M = Ni, Zn) as a cathode active material for 4 V secondary Li batteries,” Journal of Power Sources, vol. 119–121, pp. 733–737, 2003.

I. Taniguchi, “Powder properties of partially substituted LiMxMn2-xO₄ (M = Al, Cr, Fe and Co) synthesized by ultrasonic spray pyrolysis,” Materials Chemistry and Physics, vol. 92, no. 1, pp. 172–179, 2005.

Y. Xie, R. Yang, L. Yan, L. Qi, K. Dai, and P. He, “Synthesis and electrochemical characterization of Li1.05RExCryMn2-x-yO₄ spinel as cathode material for rechargeable Li-battery,” Journal of Power Sources, vol. 168, no. 1, pp. 272–277, 2007.

S. H. Ye, J. Y. Lv, X. P. Gao, F. Wu, and D. Y. Song, “Synthesis and electrochemical properties of LiMn₂O₄ spinel phase with nanostructure,” Electrochimica Acta, vol. 49, no. 9-10, pp. 1623–1628, 2004.

X. Li and Y. Xu, “Novel method to enhance the cycling performance of spinel LiMn₂O₄,” Electrochemistry Communications, vol. 9, no. 8, pp. 2023–2026, 2007.

F. Orsini, M. Dolle, and J.-M. Tarascon, “Impedance study of the Li°/electrolyte interface upon cycling,” Solid State Ionics, vol. 135, no. 1–4, pp. 213–221, 2000.

X. Wang, O. Tanaike, M. Kodama, and H. Hatori, “High rate capability of the Mg-doped Li-Mn-O spinel prepared via coprecipitated precursor,” Journal of Power Sources, vol. 168, no. 1, pp. 282–287, 2007.