- About this Journal ·
- Abstracting and Indexing ·
- Advance Access ·
- Aims and Scope ·
- Annual Issues ·
- Article Processing Charges ·
- Articles in Press ·
- Author Guidelines ·
- Bibliographic Information ·
- Citations to this Journal ·
- Contact Information ·
- Editorial Board ·
- Editorial Workflow ·
- Free eTOC Alerts ·
- Publication Ethics ·
- Reviewers Acknowledgment ·
- Submit a Manuscript ·
- Subscription Information ·
- Table of Contents
Advances in Materials Science and Engineering
Volume 2013 (2013), Article ID 375074, 6 pages
Synthesis and Characterization of LiNi1/3Co1/3Mn1/3O2−xClx as Cathode Materials for Lithium Ion Batteries at 55°C
School of Chemical and Material Engineering, Jiangnan University, Wuxi, Jiangsu 214122, China
Received 14 May 2013; Revised 27 September 2013; Accepted 2 October 2013
Academic Editor: Dachamir Hotza
Copyright © 2013 Hai-Lang Zhang and Shuixiang Liu. 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.
A series of materials based on the LiNi1/3Co1/3Mn1/3 system were prepared by a sol-gel method, and their phase formation processes, crystal structures, and electrochemical performances were studied by thermogravimetric analyses (TG/DTG), X-ray diffraction (XRD), charge-discharge tests, and cyclic voltammetry (CV). The XRD patterns indicate that the LiNi1/3Co1/3Mn1/3 powders with better crystalline structure could be obtained at calcining temperature 850°C for 20 h under air atmosphere and show that the chlorine addition may induce the change of lattice parameters. The charge-discharge tests show that both the specific capacities and capacity retentions of Cl-doped materials increase compared to the undoped material, especially for the capacity retention at the high-voltage region. At 55°C, the LiNi1/3Co1/3Mn1/3O2-0.10Cl0.10 cathode material shows the highest initial discharge capacity of 180.1 mAh·g−1 and the best capacity retention with the value of 91.9% after 100 cycles in the region of 2.0–4.4 V at 0.1 C, while the initial discharge capacity is 208.2 mAh·g−1 when the charge cutoff voltage is up to 4.6 V.
Lithiumion batteries have been investigated extensively by people for their high working voltage, high energy density, and long cyclic life to be used in electronic devices and power tools. A significant challenge of lithiumion battery improvement is to find a proper cathode material as an attractive candidate of next-generation cathode materials to replace LiCoO2. Although LiCoO2 is the predominant cathode material, its high cost and toxicity limit its further development. Recently, several other positive electrode materials, such as LiNiO2, LiMn2O4, LiNi1/3Co1/3Mn1/3O2, and LiFePO4, have been researched [1–4]. However, LiNiO2 suffers from safety and stability problems; LiMn2O4 has serious capacity fading problem during cycling, especially at higher temperatures, and LiFePO4 suffers from lower conductivity [1–3]. Layer-structured LiNi1/3Co1/3Mn1/3O2 cathode material has attracted much attention for it integrates the features of LiCoO2, LiNiO2, and LiMn2O4 with higher structural stability, higher capacity, lower cost, higher safety, and so on. It has been found that the predominant oxidation states of Ni, Co, and Mn are +2, +3, and +4, respectively. Ni2+ and Co3+ are electrochemically active for redox reaction; however, Mn4+ is electrochemically inactive to stabilize the crystal structure [4, 5]. LiNi1/3Co1/3Mn1/3O2 has been studied extensively because it has fast capacity fading due to the electrolyte decomposition and the structural decay of the electrode itself [6–8]. Moreover, the degree of capacity fading increases with the increase of charge cutoff voltage, in which is mainly due to gradual decaying of electroactive Co . In general, it is believed that the valence of transition-metal ions changes during Li+ intercalation and deintercalation. Tsai et al.  reported that the whole Ni2+ ions are oxidized to Jahn-Teller active Ni3+ ions, which two-step redox reactions of Ni2+/Ni3+ and Ni3+/Ni4+ occur during cycling, and the initial irreversible capacity is mainly due to that a part of Ni3+ and Ni4+ cannot be reduced to Ni2+ and also proved that the function of oxygen is to be the electron donor at the end of charge. It may be an effective way that partial O2− substitution by F− would enhance the electrochemical performance [10–12]. However, the fluorine addition could lower the conductivity as F− is harder to lose electrons than O2−. Li et al.  reported that chlorine addition may increase the specific capacity and enhance the cyclic stability of LiNi0.7Co0.3O2, which is conductive for their electrochemical performance due to that Cl− is easier to lose electrons than O2−. Sun et al.  also reported that Cl-doping has improved the high-rate capability of LiFePO4 owing to the improvement of the Li+ ion diffusion.
The goal of this work is to synthesize the Cl-doped LiNi1/3Co1/3Mn1/3O2 cathode materials and understand the effect of chlorine addition on the structure and electrochemical properties of LiNi1/3Co1/3Mn1/3O2, especially at higher temperature. Because more and reliable results could be obtained by measuring the high temperature charge-discharge performance. To our knowledge, this is the first time to report Cl-doped LiNi1/3Co1/3Mn1/3O2 cathode materials.
2.1. The Preparation of LiNi1/3Co1/3Mn1/3O2−xClx Powders
LiNi1/3Co1/3Mn1/3 powders were prepared via a sol-gel route using citric acid as chelating agent. A stoichiometric amount of LiCH3COO2H2O (AR), Ni(CH3COO)24H2O(AR), Mn(CH3COO)24H2O(AR), Co(CH3COO)24H2O(AR) and LiClH2O (AR) was dissolved in deionized water, and then the aqueous solution of citric acid was added to the mixture of metal ion solution. The pH was adjusted to 7~8 by ammonium hydroxide. The reagent solution was stirred continuously at 80°C until homogeneous sol-gel formed. The resulting gel was dried at 120°C for 8 h and then heated at 500°C for 6 h to eliminate the organic residues. The powders were thoroughly ground and then calciniated at 850°C for 20 h in air and followed by quenching to room temperature.
2.2. The Characterization of LiNi1/3Co1/3Mn1/3O2-xClx Powders
TG/DTG was used to analyze the thermal process and phase formation process of the gel precursor from 50°C to 1000°C at a rate of 10°C/min under a nitrogen atmosphere.
The X-ray diffraction (XRD) with Cu Kα radiation operated at 40 kV and 40 mA was used to analyze the crystalline structure of samples. The scan data were in the 2θ range from 10° to 90° in a step of 4°/min.
The electrochemical properties of samples were carried out using two-electrode coin cells (type CR2032) assembled in an argon filled glove box. The positive electrodes were prepared by blending 80% active material, 12% acetylene black, and 8% polyvinylidene fluoride in N-methyl-2-pyrrolidone (NMP). Then the slurry was spread on an aluminum foil as current collector using the Doctor-blade technique and dried at 80°C for 10 h in a vacuum oven. Microporous polypropylene membrane (Celgard 2325) was used as the separator. The electrolyte is LB-315 which consists of a 1 M LiPF6 solution in DMC : EMC : EC (1 : 1 : 1, v/v/v). The charge-discharge was tested in the potential range of 2.0~4.4 or 4.6 V at different rates at elevated temperature (55°C) by using the instrument Land2001T.
The cyclic voltammogram (CV) curves were obtained between the cutoff voltage ranges of 2.0~4.8 V on an IM6 electrochemical workstation at a scan rate of 0.1 mV/s.
3. Results and Discussion
3.1. TG-DTG Analysis
TG-DTG curves of the gel precursor of LiNi1/3Co1/3Mn1/3O2 and LiNi1/3Co1/3Mn1/3O2-0.10Cl0.10 are shown in Figure 1. There is little change in the two profiles. The first weight loss occurs at the range of 100–200°C, which corresponds to the removal of water molecules staying in the gel surface and the crystallization water of the acetates. The second weight loss is due to the decomposition of citric acid and the decomposition of anhydrous acetate to produce and metal carbonates in the temperature region of 200°C –400°C . A slow weight loss could be observed between 400–800°C in the curve, which is attributed to conversion of the metal carbonates into , , and . There is little weight loss to be observed over 800°C, which indicates that the LiNi1/3Co1/3Mn1/3 phase has formed at around 800°C.
3.2. X-Ray Diffraction Analysis
Figure 2 shows the typical X-ray diffraction patterns of LiNi1/3Co1/3Mn1/3 (, 0.05, 0.10, 0.15) cathode materials by calcining at 850°C for 20 h in air atmosphere. The XRD patterns of samples show that no impurity phase exists, which indicates that the samples have the hexagonal α-NaFeO2 structure (space group, Rm). The clear peak splits of (006)/(102) and (108)/(110) doublets exhibit a high degree of ordered hexagonal layered structure. Table 1 presents the lattice parameters of LiNi1/3Co1/3Mn1/3O2−xClx (, 0.05, 0.10, 0.15) cathode materials. The integrated intensity ratio of (003)/(104) peak is more than 1.2 for all samples, and the biggest ratio 1.38 is obtained when the chlorine content is 0.10, suggesting that a small amount of Cl− substitution for O2− could suppress occupancy of Li+ layers by Ni2+ and be conducive to the performance during electrochemical cycling . The crystal structure has a little difference after chlorine doping, indicating the heteroelement has been incorporated into the LiNi1/3Co1/3Mn1/3O2 structure [17, 18]. The increase of lattice parameter may be attributed to the valence balance by the chlorine doping leading to Mn4+ (0.53 Å) transform to Mn3+ (0.58 Å) or Co3+ (0.545 Å) transform to Co2+ (0.65 Å) in these compounds , while the increase of lattice parameter may be due to the difference of radius between Cl− (1.81 Å) and O2− (1.40 Å). Furthermore, the c/a ratio is greater than 4.9, which reveals a high cation ordering of the synthesized compounds .
3.3. Electrochemical Studies
The initial charge-discharge curves of LiNi1/3Co1/3Mn1/3, 0.05, 0.10, 0.15) over a voltage range of 2.0–4.4 V at 55°C are shown in Figure 3. As for the initial discharge capacity, the materials exhibit 170.2, 178.9, 180.1, and 179.7 mAhg−1, respectively, and the initial coulombic efficiencies are 90.4%, 93.3%, 93.0%, and 95.7%, respectively, for to 0.15 at a current rate of 0.1 C. The 95.7% initial coulombic efficiency may be the highest value for LiNi1/3Co1/3Mn1/3O2 in the world as we have known.
That the Cl-doped materials have higher discharge capacities than bare materials is attributed to the valence balance caused by chlorine addition, which may lead Ni3+ and Ni4+ to almost be completely reduced to Ni2+, decreasing the initial irreversible capacity . Another reason is due to that Cl-doped materials have lower electronstatic repulsions between O–M–O interlayers in the process of Li+ insertion/deinsertion for Cl− has one valence electron less than O2−, which is beneficial for the removal of Li+ insertion/deinsertion . Furthermore, the initial irreversible capacity loss of the materials also may be involved with the formation of surface electrolyte interphase (SEI) film .
The cyclic performance and rate capability of LiNi1/3Co1/3Mn1/3, 0.05, 0.10, 0.15) cathode materials are illustrated in Figure 4. All cells were operated by the steps of 2 cycles at 0.1 C, 3 cycles at 0.15 C, 5 cycles at 0.25 C, 87 cycles at 0.5 C, and the final 3 cycles at 0.1 C between 2.0 V and 4.4 V. At the 97th cycle the discharge capacities at 0.5 C are 101.2, 125.7, 139.1, and 129 mAhg−1, which are 70.6%, 83.7%, 91.9%, and 85.5% of the 11th cycle at 0.5 C for to 0.15, respectively. And after 100 cycles the capacities at 0.1 C are 82.4%, 89.9%, 91.8%, and 89.3% of the initial discharge capacity at 0.1 C, respectively.
It is worth noting that Cl-doped materials exhibit high discharge specific capacity, excellent cyclic stability, and good rate performance. The ion radius of Cl− is larger than O2−, expanding pathway for Li+ to intercalate and deintercalate. Moreover, Li et al.  reported that Li+ can be more freely deintercalated due to that Cl− is easier to lose electron than O2−. However, the structural stability slightly decreases with the increase of chlorine content; one reason may be for larger lattice parameters and and the other may be due to valence balance. So the capacity retention for is lower than that with the chlorine content of 0.10.
Figure 5 shows the initial charge-discharge curves when the charge cutoff potential is up to 4.6 V at 0.1 C. The initial discharge capacities are 202.1, 206.2, 208.2, and 207.7 mAhg−1, respectively, and the initial coulombic efficiencies are 83.4%, 86.0%, 85.6% and 91.1% for to 0.15, respectively. The initial coulombic efficiency decreases with the increase of charge cutoff potential. Figure 6 shows the cyclic performances and rate capabilities of LiNi1/3Co1/3Mn1/3, 0.05, 0.10, 0.15) cathode materials between 2.0 V and 4.6 V. All cells were operated by the steps of 2 cycles at 0.1 C, 3 cycles at 0.15 C, 5 cycles at 0.25 C, and the final 50 cycles at 0.5 C. The discharge capacities of the 11th cycle at 0.5 C are 166.4, 170.9, 175.6, and 171.1 mAhg−1, respectively; and at the 60th cycle the discharge capacities are 71.2%, 83.4%, 92.2% and 80.6% of the 11th cycle at 0.5 C for to 0.15, respectively. It is worthy to note that the discharge capacity increases but leads to fast capacity fading with the increasing of cutoff voltage, especially for the bare material. Kim et al.  have reported that the capacity fading is mainly due to the Co dissolution during cycling in high voltage cutoff. However, the Cl− doping leads to improvement in capacity retention at the high-voltage region, which indicates that chlorine addition has enhanced the electrochemical performance.
3.4. Cyclic Voltammetry (CV)
Figure 7 presents the first cyclic voltammogram curves of LiNi1/3Co1/3Mn1/3O2 and LiNi1/3Co1/3Mn1/3 cathode materials in the voltage range of 2.0–4.8 V at a scan rate of 0.1 mV/s. Evidently two redox peaks at 4.078/3.632 V and 4.608/4.497 V are found in the curve of bare sample, indicating that two phase transitions occurred in the charge-discharge process. Shaju et al.  have reported that the large redox peak and the small redox peak are corresponding to Ni2+/4+ and Co3+/4+, respectively. It is reported that the capacity fade of the layer-structured cathode materials is associated with structural transitions from hexagonal to monoclinic to hexagonal modifications at potentials above 4.1 V [22, 23]. There is only one redox peak in the curves of Cl-doped materials, which means that Cl−, as a doping material, suppresses the structure transitions from hexagonal to monoclinic structure.
The LiNi1/3Co1/3Mn1/3, 0.05, 0.10, 0.15) cathode materials have been successfully synthetized by a sol-gel method. Partial O2− substitution by Cl− increases the lattice parameters , and . LiNi1/3Co1/3Mn1/3O1.90Cl10 cathode material shows higher initial discharge capacity of 180.1 mAhg−1 at 0.1 C in a voltage range of 2.0–4.4 V, and the capacity retention was 91.9% after 100 cycles at 55°C, while for the undoped material they are 170.2 mAhg−1 and 82.4%, respectively. It should be confirmed that a small amount of Cl doping could improve the cyclic property of LiNi1/3Co1/3Mn1/3O2 a great deal and also increase the discharge capacity. Although the initial discharge capacity increases when the charge cutoff voltage is up to 4.6 V, the capacity retention and rate capability for the bare material decrease. Chlorine addition has improved the electrochemical performance in the higher charge cutoff voltage. CV shows that only one redox peak is observed for Cl-doped materials, which means that there is no structural transition from hexagonal to monoclinic in this area. Chlorine doping has been demonstrated to be a good way for improving the property of LiNi1/3Co1/3Mn1/3O2. LiNi1/3Co1/3Mn1/3O1.90Cl10 would be a promising candidate cathode material for next generation Li-ion battery.
- C. Delmas, J. P. Pérès, A. Rougier et al., “On the behavior of the LixNiO2 system: an electrochemical and structural overview,” Journal of Power Sources, vol. 68, no. 1, pp. 120–125, 1997.
- 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.
- A. S. Andersson and J. O. Thomas, “The source of first-cycle capacity loss in LiFePO4,” Journal of Power Sources, vol. 97-98, pp. 498–502, 2001.
- K. M. Shaju, G. V. Subba Rao, and B. V. R. Chowdari, “Performance of layered Li(Ni1/3Co1/3Mn1/3)O2 as cathode for Li-ion batteries,” Electrochimica Acta, vol. 48, no. 2, pp. 145–151, 2002.
- Y.-J. Shin, W.-J. Choi, Y.-S. Hong, S. Yoon, K. S. Ryu, and S. H. Chang, “Investigation on the microscopic features of layered oxide Li[Ni1/3Co1/3Mn1/3]O2 and their influences on the cathode properties,” Solid State Ionics, vol. 177, no. 5-6, pp. 515–521, 2006.
- Y. Koyama, N. Yabuuchi, I. Tanaka, H. Adachi, and T. Ohzuku, “Solid-state chemistry and electrochemistry of LiCo1/3Ni1/3Mn1/3O2 for advanced lithium-ion batteries I. First-principles calculation on the crystal and electronic structures,” Journal of the Electrochemical Society, vol. 151, no. 10, pp. A1545–A1551, 2004.
- H. Liu and L. Tan, “High rate performance of novel cathode material Li1.33Ni1/3Co1/3Mn1/3O2 for lithium ion batteries,” Materials Chemistry and Physics, vol. 129, pp. 729–732, 2011.
- S. H. Park, C. S. Yoon, S. G. Kang, H.-S. Kim, S.-I. Moon, and Y.-K. Sun, “Synthesis and structural characterization of layered Li[Ni1/3Co1/3Mn1/3]O2 cathode materials by ultrasonic spray pyrolysis method,” Electrochimica Acta, vol. 49, no. 4, pp. 557–563, 2004.
- Y. W. Tsai, B. J. Hwang, G. Ceder, H. S. Sheu, D. G. Liu, and J. F. Lee, “In-situ X-ray absorption spectroscopic study on variation of electronic transitions and local structure of LiNi1/3Co1/3Mn1/3O2 cathode material during electrochemical cycling,” Chemistry of Materials, vol. 17, no. 12, pp. 3191–3199, 2005.
- D. C. Li, Y. Sasaki, K. Kobayakawa, H. Noguchi, and Y. Sato, “Preparation, morphology and electrochemical characteristics of LiNi1/3Mn1/3Co1/3O2 with LiF addition,” Electrochimica Acta, vol. 52, no. 2, pp. 643–648, 2006.
- Y. S. He, L. Pei, X. Z. Liao, and Z. F. Ma, “Synthesis of LiNi1/3Co1/3Mn1/3O2-zFz cathode material from oxalate precursors for lithium ion battery,” Journal of Fluorine Chemistry, vol. 128, pp. 139–143, 2007.
- K.-H. Dai, Y.-T. Xie, Y.-J. Wang, Z.-S. Song, and Q. Qilu, “Effect of fluorine in the preparation of Li(Ni1/3Co1/3Mn1/3)O2 via hydroxide co-precipitation,” Electrochimica Acta, vol. 53, no. 8, pp. 3257–3261, 2008.
- X. L. Li, F. Y. Kang, W. C. Shen, and X. D. Bai, “Improvement of structural stability and electrochemical activity of a cathode material LiNi0.7Co0.3O2 by chlorine doping,” Electrochimica Acta, vol. 53, no. 4, pp. 1761–1765, 2007.
- C. S. Sun, Y. Zhang, X. J. Zhang, and Z. Zhou, “Structural and electrochemical properties of Cl-doped LiFePO4/C,” Journal of Power Sources, vol. 195, no. 11, pp. 3680–3683, 2010.
- C. Nithya, V. S. Syamala Kumari, and S. Gopukumar, “Synthesis of high voltage (4.9 V) cycling LiNixCoyMn1-x-yO2 cathode materials for lithium rechargeable batteries,” Physical Chemistry Chemical Physics, vol. 13, no. 13, pp. 6125–6132, 2011.
- R. Santhanam, P. Jones, A. Sumana, and B. Rambabu, “Influence of lithium content on high rate cycleability of layered Li1+xNi0.30Co0.30Mn0.40O2 cathodes for high power lithium-ion batteries,” Journal of Power Sources, vol. 195, no. 21, pp. 7391–7396, 2010.
- S.-T. Myung, K. Izumi, S. Komaba, Y.-K. Sun, H. Yashiro, and N. Kumagai, “Role of alumina coating on Li-Ni-Co-Mn-O particles as positive electrode material for lithium-ion batteries,” Chemistry of Materials, vol. 17, no. 14, pp. 3695–3704, 2005.
- S.-T. Myung, K. Izumi, S. Komaba et al., “Functionality of oxide coating for Li[Li0.05Ni0.4Co0.15Mn0.4]O2 as positive electrode materials for lithium-ion secondary batteries,” Journal of Physical Chemistry C, vol. 111, no. 10, pp. 4061–4067, 2007.
- G.-H. Kim, J.-H. Kim, S.-T. Myung, C. S. Yoon, and Y.-K. Sun, “Improvement of high-voltage cycling behavior of surface-modified Li[Ni1/3Co1/3Mn1/3]O2 cathodes by fluorine substitution for Li-ion batteries,” Journal of the Electrochemical Society, vol. 152, no. 9, pp. A1707–A1713, 2005.
- J.-W. Lee, J.-H. Lee, T. T. Viet, J.-Y. Lee, J.-S. Kim, and C.-H. Lee, “Synthesis of LiNi1/3Co1/3Mn1/3O2 cathode materials by using a supercritical water method in a batch reactor,” Electrochimica Acta, vol. 55, no. 8, pp. 3015–3021, 2010.
- Z.-D. Huang, X.-M. Liu, S.-W. Oh, B. Zhang, P.-C. Ma, and J.-K. Kim, “Microscopically porous, interconnected single crystal LiNi1/3Co1/3Mn1/3O2 cathode material for Lithium ion batteries,” Journal of Materials Chemistry, vol. 21, no. 29, pp. 10777–10784, 2011.
- G. T.-K. Fey, Y. Y. Lin, and T. Prem Kumar, “Enhanced cyclability and thermal stability of LiCoO2 coated with cobalt oxides,” Surface and Coatings Technology, vol. 191, no. 1, pp. 68–75, 2005.
- H. Cao, Y. Zhang, J. Zhang, and B. Xia, “Synthesis and electrochemical characteristics of layered LiNi0.6Co0.2Mn0.2O2 cathode material for lithium ion batteries,” Solid State Ionics, vol. 176, no. 13-14, pp. 1207–1211, 2005.