Search tips
Search criteria 


Logo of materialsLink to Publisher's site
Materials (Basel). 2009 September; 2(3): 857–868.
Published online 2009 July 27. doi:  10.3390/ma2030857
PMCID: PMC5445747

Nitrate-Melt Synthesized HT-LiCoO2 as a Superior Cathode-Material for Lithium-Ion Batteries


An electrochemically-active high-temperature form of LiCoO2 (HT-LiCoO2) is prepared by thermally decomposing its constituent metal-nitrates at 700 ºC. The synthetic conditions have been optimized to achieve improved performance with the HT-LiCoO2 cathode in Li-ion batteries. For this purpose, the synthesized materials have been characterized by powder X-ray diffraction, scanning electron microscopy, and galvanostatic charge-discharge cycling. Cathodes comprising HT-LiCoO2 exhibit a specific capacity of 140 mAhg-1 with good capacity-retention over several charge-discharge cycles in the voltage range between 3.5 V and 4.2 V, and can sustain improved rate capability in contrast to a cathode constituting LiCoO2 prepared by conventional ceramic method. The nitrate-melt-decomposition method is also found effective for synthesizing Mg-/Al- doped HT-LiCoO2; these also are investigated as cathode materials for Li-ion batteries.

Keywords: LiCoO2, synthesis, nitrate decomposition, Li-ion batteries

1. Introduction

Lithium cobalt oxide (LiCoO2) remains the most exploited cathode material for commercial Li-ion batteries [1]. LiCoO2 cathode exhibits high output-voltage, high specific-energy, long cycle-life and low self-discharge features that are central to batteries powering portable-electronic devices [1,2,3,4]. Electrochemical performance of LiCoO2 greatly depends on its crystallographic structure, as it exists in two different modifications, namely the high-temperature (HT) phase, crystallizing in an ideal layered-structure isomorphic to α-NaFeO2 (space group: R3m) with ordered cobalt and lithium ions resulting in hexagonal sheets of Li+- and Co3+- ions in alternate layers of (111) planes [5], and the low-temperature (LT) phase with spinel-like structure (space group: Fd3m) with about 6 % of Co3+ ions located at lithium sites [6]. Unlike LT-LiCoO2, HT-LiCoO2 exhibits excellent electrochemical stability on prolonged cycling [7,8]. The stability of HT phase originates from the structural durability of the material with the layered cation-ordering that remains well preserved even after repeated insertion and de-insertion of Li+-ions during the charge-discharge processes of the lithium-ion cell.

The structure and degree of cation ordering in LiCoO2 vary with the synthetic conditions that affect its electrochemical activity. Accordingly, the optimization of synthetic procedure for LiCoO2 is seminal for attaining its improved electrochemical behavior. To this end, various synthetic methods, such as ceramic method [9], oxalate method [10], hydroxide precipitation method [11], sol-gel method [12], molten salt method [13], hydrothermal method [14], template method [15], spray pyrolysis [16], polymer pyrolysis method [17], Pechini method [18] and combustion method [19], have been attempted in the literature for realizing electrochemically active LiCoO2.

This communication reports a rapid synthesis of LiCoO2 cathode material with high specific-capacity for Li-ion batteries. The method involves heating stoichiometric amounts of metal-nitrate precursors that on decomposing yield a crystalline oxide. Since the metal nitrates have low melting-point, their mixtures transform to a eutectic melt on heating to the eutectic temperature that on further heating yields nano-crystalline LiCoO2 with perfect layered-structure suitable for use as active cathode material in a lithium-ion rechargeable battery. The method is also useful for synthesizing Mg-/Al-ions doped LiCoO2 and related intercalation oxides. It is noteworthy that the present method is altogether novel and differs substantially from other nitrate-decomposition methods [18,19,20]. The method is simple and cost-effective for bulk synthesis of HT-LiCoO2.

2. Experimental

Powder samples of LiCoO2 were prepared by rapidly heating the mixture of LiNO3 and Co(NO3)2.6H2O in the molar ratio of 1.1:1 with an excess of lithium stoichiometry (10 mol %) added to compensate for the lithium losses during the synthesis. In a typical preparation, 3.87 g of LiNO3 and 14.87 g of Co(NO3)2·6H2O were taken in a sintered alumina crucible and introduced to a preheated furnace at 350 ºC. Subsequently, the furnace was programmed for rapid heating to 700 ºC and held there for 1 h. The furnace was then fast cooled to 350 ºC in about 10 min and the crucible removed from the furnace. The sample was crushed and ground well to obtain a fine powder of LiCoO2. Similarly, Mg- or Al- doped HT-LiCoO2 with respective compositions of LiCo0.95Mg0.05O2 and LiCo0.95Al0.05O2 were prepared by taking corresponding metal nitrates in the required stoichiometry with 10 mol % extra lithium nitrate, followed by heating at 700 ºC for 1h. For comparison, HT-LiCoO2 was also prepared using the conventional solid-state method [9]; this sample is referred to as LiCoO2-SS in the text.

Powder X-ray diffraction patterns for the prepared samples were recorded using X’pert PRO-PANalytical Diffractometer with CuKα radiation. The morphology of the powder samples were examined under a Scanning Electron Microscope (HITACHI Model S-3000H). Chemical analyses of the samples were carried out using Perkin-Elmer Atomic Absorption Spectrometer (AAS). Electrochemical tests were conducted using Swagelok-typeTM cells assembled in an argon-filled glove box. The positive electrode comprised the ball-milled mixture of 85 wt.% active material with 15 wt.% Super-P Li Carbon (Timcal Belgium) as the conducting additive. Lithium electrode was prepared by pressing a piece of lithium metal onto a thin stainless steel disc. Electrolyte used was 1M LiPF6 solution in a mixture of ethylene carbonate and dimethyl carbonate in 1:1 ratio by volume. The cells thus fabricated were cycled galvanostatically between 3.5 V and 4.3 V versus lithium using a VMP3Z (Biologica) multi-channel potentiostat/galvanostat.

3. Results and Discussion

Figures 1(a-d) show the powder X-ray diffraction patterns for the products formed by heating the mixed-metal nitrates of lithium and cobalt in a 1.1:1 molar ratio at varying temperatures between 600 ºC and 900 ºC for 4 h. The diffraction pattern for the product obtained at 600 ºC could be indexed as rhombohedral R3m LiCoO2 along with small amounts of lithium-deficient LiCoO2 crystallizing in cubic Fm3m structure. X-ray powder diffraction pattern for the product obtained by heating at 700 ºC shows single-phase LiCoO2 as indexed on the basis of α-NaFeO2 structure (space group: R3m).

Figure 1
Powder X-ray diffraction patterns for LiCoO2 obtained by nitrate melt decomposition at varying temperatures (a) 600 ºC (b) 700 ºC (c) 800 ºC (d) 900 ºC. The peaks marked as (#) correspond to Co34 and (*) correspond ...

The lattice parameters obtained by Rietveld refinement of LiCoO2-700 sample agree well with those prepared by conventional solid-state method [21] and are given in Table 1. All diffraction patterns show clear (006)/(102) peaks and (018)/(110) split peaks indicating a perfect layered-structure for LiCoO2 [21]. The diffraction patterns of samples prepared at 800 ºC and 900 ºC comprise a major LiCoO2 phase crystallizing in rhombohedral structure with a small Co3O4 spinel phase marked with (*) in Figure 1 (c) and (d); the latter arising due to lithium evaporation from the parent compound at high temperatures. I(003)/I(104) intensity ratio decreases with increasing calcination temperature and is sensitive to the degree of cation mixing [22] that influences electrochemical properties substantially.

Table 1
Lattice parameters, c/a ratio and I(003)/I(104) intensity ratio for HT-LiCoO2 related phases.

It is clear from the aforesaid X-ray diffraction studies that 700 ºC is the optimal temperature for obtaining pure LiCoO2 in ordered rock-salt superstructure. In order to determine the optimal duration, the synthesis was carried out with varying heating durations between 15 min and 4 h at 700 ºC. The X-ray diffraction patterns for the products formed at different time intervals are presented in Figure 2. It is seen from the diffractograms that the sample prepared at 700 ºC for as low as 15 min matches well with HT-LiCoO2 pattern with R3m space group; the intensity ratio of I(003)/I(104) <1.2 indicating a considerable extent of cation mixing in the crystal lattice. By contrast, the samples synthesized at 700 ºC for 1 h (or more) exhibit I(003)/I(104) >1.2 indicating the absence of cation mixing. On increasing the heating duration beyond 1 h, little change is observed in the diffraction pattern with increase in overall peak intensity owing to the improved crystallinity of the sample.

Figure 2
Powder X-ray diffraction patterns for LiCoO2 obtained by heating nitrates at 700 °C for varying durations.

The increase in crystallinity of the sample with longer heating duration is further corroborated from morphological studies by scanning electron microscopy (SEM). The SEM image for the samples heated at 700 ºC for 1 h shown in Figure 3(a) depicts agglomerates of smaller crystallites of ~1 μm. The sample obtained by heating at 700 ºC for 4 h shows well defined crystals of platelet-like morphology of ~ 50 μm [Figure 3(b)]. The chemical compositions of the prepared samples obtained from AAS analysis of Li and Co suggest cation stoichiometry to be strongly dependent on the synthesis temperature. LiCoO2 prepared at 600 ºC shows a slight excess of lithium stoichiometry corresponding to Li1.09CoO2 and closure to the initial stoichiometry of nitrates taken, suggesting little loss of Li during heating. It is noteworthy that impurity peaks corresponding to lithium salts are absent in the X-ray diffractogram. The sample prepared at 700 ºC has its nominal composition as LiCoO2 while the samples prepared at 800 ºC and above reflect Co3O4 as impurity in the diffractogram albeit the use of 10 mol % excess Li salt in the synthesis. This suggests substantial amount of Li loss at high temperatures. Chemical analyses of these samples were not possible owing to the insolubility of Co3O4 in acids. From the fore going, it is clear that the synthetic conditions have a seminal role in controlling structural as well as compositional aspects of LiCoO2 that affect its electrochemical activity.

Figure 3
Scanning Electron Micrographs for HT-LiCoO2 obtained by heating corresponding metal nitrates at 700 °C in air for (a) 1 h and (b) 4 h.

The metal-nitrates-melt decomposition method has added advantage in relation to solution methods as the former results in homogeneously mixed metal ions leading to their effective substitution in the end product. It has been possible to synthesize about 5-6 atom % of Mg- or Al- doped LiCoO2. Figure 4 shows powder X-ray diffraction patterns for LiCo0.95Mg0.05O2 and LiCo0.95Al0.05O2 samples along with the XRD pattern for pristine LiCoO2. All these XRD patterns could be indexed to a layered α-NaFeO2 structure (space group: R3m). The samples are phase pure and no impurity peaks corresponding to Li2CO3 and metal oxides are present. The refined lattice parameters for LiCo0.95Mg0.05O2 and LiCo0.95Al0.05O2 are presented in Table 1 which agrees well with those reported in the literature for similar compositions [23,24]. Substitution of Co3+ by larger Mg2+-ion increases the a and c lattice parameters with c/a ratio of 4.99 while substitution by smaller Al3+-ion decreases the a-lattice parameter and increases the c-lattice parameter resulting in an increased c/a ratio of 5.004.

Figure 4
Powder X-ray diffraction patterns for (a) pristine LiCoO2, (b) LiCo0.95Mg0.05O2 and (c) LiCo0.95Al0.05O2.

The electrochemical performances of all the LiCoO­2 samples, prepared at different temperatures with varying heat durations, have been evaluated using Swagelok-type cells. The voltage-composition curves for galvanostatic charge/discharge cycling of Li/LiCoO2-700 cells at 1 Li/5 h in different voltage ranges are shown in Figures 5(a) and (b) as representative examples.

Figure 5
The voltage-composition curve for a Li/LixCoO2-700 cell cycled galvanostatically at 1 Li/5 h rate between the voltage window (a) 3.5 - 4.2 V and (b) 3.5 - 4.3 V at room temperature (~30 ºC).

The smooth charge-discharge curves between 3.5 V and 4.2V show the absence of spinel-phase formation during cycling with the plateau due to Co3+/Co4+ redox process at ~3.9 V. A higher capacity of 150 mAhg-1 is obtained when the cells are cycled between 3.5 V and 4.3 V but the irreversible capacity loss, polarisability and capacity fade are higher compared to cells cycled between 3.5 V and 4.2 V. This is probably due to the change in crystal structure associated with the higher lithium extraction during higher voltage windows.

Figure 6 shows the specific capacity values versus cycle number for Li/LiCoO2 cells with LiCoO2 samples prepared at different temperatures. The first charge/discharge capacities of the samples prepared at 600 °C, 700 °C and 800 °C are 106/91, 132/122 and 131/114 mAhg-1, respectively. As obvious from the data, the sample obtained by heating at 600 ºC shows lower capacity and retains only 92% of its initial capacity after 25 cycles, presumably due to the absence of perfect-layered structure as revealed by its X-ray diffraction pattern. By contrast, the sample prepared at 700 °C shows a maximum capacity with an irreversible capacity loss of about 10 mAh/g; the sample retains a capacity value of ~ 116mAhg-1 after 25 cycles with a capacity loss of only ~ 5%. The initial charge capacity for the sample synthesized at 800 °C is comparable to the sample prepared at 700 °C but its irreversible capacity loss in the first cycle is 17 mAhg-1 that pushes its specific capacity to ~114 mAhg-1. This is due to the Li-deficiency in the sample brought about by lithium loss at higher temperature. Accordingly, the sintering temperature clearly affects electrochemical behavior of the samples. In this study, the optimum electrochemical performance is observed for stoichiometric LiCoO2 prepared at 700 °C.

Figure 6
Discharge capacity versus cycle number for Li/LiCoO2 cells cycled between 3.5-4.2 V at room temperature ( ~30 ºC ) with LiCoO2 prepared at different temperatures: -●- 800 ºC, -▲- 700 ºC and -■-600 ºC. ...

In order to compare the electrochemical performance of HT-LiCoO2 prepared by nitrate-melt method with conventionally prepared samples, the cells of LiCoO2 prepared by solid state (LiCoO2-SS) and nitrate-melt (LiCoO2-700) methods have been subjected to cycling at varying rates. The capacity Vs cycle number plot is shown in Figure 7. The data reflect that the sample derived by nitrate-melt method exhibits higher capacity and better rate capability as compared to the sample prepared by conventional ceramic method.

Figure 7
Rate capability plot for Li/LiCoO2 cells for nitrate derived (-●-) and solid-state prepared (-○-) samples.

Further, we have also evaluated electrochemical performances of Mg- or Al-doped LiCoO2 samples prepared by nitrate-melt-decomposition method. Figures 8(a) and (b) show the voltage versus composition curves for Li/LiCo0.95Mg0.05O2 and Li/LiCo0.95Al0.05O2 cells, respectively. The corresponding plots of capacity versus cycle number are shown as insets to Figures 8 (a) and (b).

Figure 8
The voltage versus composition curves for (a) Li/LiCo0.95Mg0.05O2 and (b) Li/LiCo0.95Al0.05O2 cells in the voltage window 3.5-4.3 V. Corresponding capacity versus cycle number data are shown as insets.

The Mg-doped samples show good reversibility during charge/discharge cycling with first cycle capacity as high as 146 mAhg-1, a value comparable to un-doped LiCoO2. As expected, Mg doping enhances the structural stability with good capacity retention between 3.5 V and 4.3 V in relation to pristine LiCoO2. Interestingly, Li/LiCo0.95Al0.05O2 cell shows very high initial capacity of ~ 154 mAhg-1 but has poor capacity retention

We have demonstrated that nitrate-melt-decomposition route leads to electrochemically active pristine and doped LiCoO2. Although, synthesis of electrochemically active LiCoO2 through nitrate precursors followed by combustion, sol-gel or flame pyrolysis methods have been reported previously [18,19,20], these methods require a fuel or chelating agent in addition with metal precursors. Generally, the product obtained using these methods have residual carbonaceous matter which requires high-temperature heating for long duration. Besides, in many cases, the product formed is amorphous and requires further calcination for crystallization. In this context, the metal-nitrate-melt-decomposition route is attractive and new. The method is simple as well as cost effective for synthesizing battery grade LiCoO2 in bulk.

4. Conclusions

Electrochemically active HT-LiCoO2 has been prepared by heating nitrate precursors for duration as short as 15 min. LiCoO2 prepared using this method exhibits varying degrees of cation mixing and crystallinity depending on the synthetic conditions. The samples prepared at 700 ºC for shorter durations are nano-crystalline in nature and exhibit increased rate capability. On increasing the reaction temperature above 700 ºC, samples are found to be lithium deficient. HT-LiCoO2 obtained by nitrate-melt decomposition at 700 ºC results in a superior cathode material for lithium-ion batteries. The method is also effective for synthesizing Mg- or Al- doped LiCoO2. The nitrate-melt decomposition method is simple, cost effective and convenient for large-scale synthesis of LiCoO2 with better electrochemical performance.


Financial support from the Council of Scientific and Industrial Research, New Delhi under the EFYP is gratefully acknowledged.


1. Ozawa K. Lithium-ion rechargeable batteries with LiCoO2 and carbon electrodes - the LiCoO2 system. Solid State Ionics. 1994;69:212–221. doi: 10.1016/0167-2738(94)90411-1. [Cross Ref]
2. Sadoway D.R., Mayes A.M. Portable power: Advanced rechargeable lithium batteries. MRS Bull. 2002;27:590–592.
3. Nazri G.A. Issues in energy storage for electric-based transportation. MRS Bull. 2002;27:628–631. doi: 10.1557/mrs2002.200. [Cross Ref]
4. Tarascon J.M., Armand M. Issues and challenges facing rechargeable lithium batteries. Nature. 2001;414:359–367. doi: 10.1038/35104644. [PubMed] [Cross Ref]
5. Kang S.G., Kang S.Y., Ryu K.S., Chang S.H. Electrochemical and structural properties of HT-LiCoO2 and LT-LiCoO2 prepared by the citrate sol-gel method. Solid State Ionics. 1999;120:155–161. doi: 10.1016/S0167-2738(98)00559-1. [Cross Ref]
6. Gummow R.J., Liles D.C., Thackeray M.M., David W.I.F. A Reinvestigation of the structures of lithium cobalt oxides with neutron diffraction data. Mater. Res. Bull. 1993;28:1177–1184. doi: 10.1016/0025-5408(93)90098-X. [Cross Ref]
7. Garcia B., Farcy J., Pereira-Ramos J.P., Baffier N. Electrochemical properties of low temperature crystallized LiCoO2. J. Electrochem.Soc. 1997;144:1179–1184. doi: 10.1149/1.1837569. [Cross Ref]
8. Antolini E. LiCoO2: Formation, structure, lithium and oxygen nonstoichiometry, electrochemical behaviour and transport properties. Solid State Ionics. 2004;170:159–171. doi: 10.1016/j.ssi.2004.04.003. [Cross Ref]
9. Mizushima K., Jones P.C., Wiseman P.J., Goodenough J.B. LixCoO2 (0<x~1): A new cathode material for batteries of high energy density. Mater. Res. Bull. 1980;15:783–789.
10. Caballero A., Cruz M., Hernán L., Melero M., Morales J., Castellón E.R. Nanocrystalline materials obtained by using a simple, rapid method for rechargeable lithium batteries. J. Power Sources. 2005;150:192–201. doi: 10.1016/j.jpowsour.2005.02.013. [Cross Ref]
11. Huang B., Jang Y-I., Chiang Y-M., Sadoway D.R. Electrochemical evaluation of LiCoO2 synthesized by decomposition and intercalation of hydroxides for lithium-ion battery applications. J. Appl. Electrochem. 1998;28:1365–1369.
12. Yoon W.S., Kim K.B. Synthesis of LiCoO2 using acrylic acid and its electrochemical properties for Li secondary batteries. J. Power Sources. 1999;81-82:517–523.
13. Chen H., Grey C.P. Molten salt synthesis and high rate performance of the “Desert- Rose” form of LiCoO2. Adv. Mater. 2008;20:2206–2210. doi: 10.1002/adma.200702655. [Cross Ref]
14. Okubo M., Hosono E., Kim J., Enomoto M., Kojima N., Kudo T., Zhou H., Honma I. Nanosize effect on high-rate Li-ion intercalation in LiCoO2 electrode. J. Am. Chem. Soc. 2007;129:7444–7452. doi: 10.1021/ja0681927. [PubMed] [Cross Ref]
15. Jiao F., Shaju K.M., Bruce P.G. Synthesis of nanowire and mesoporous low-temperature LiCoO2 by a post-templating reaction. Angew. Chem. Intl. Edn. 2005;44:6550–6553. doi: 10.1002/anie.200501663. [PubMed] [Cross Ref]
16. Kim D.Y., Ju S.H., Kang Y.C. Fine-sized LiCoO2 particles prepared by spray pyrolysis from polymeric precursor solution. Mater. Res. Bull. 2007;42:362–370. doi: 10.1016/j.materresbull.2006.05.024. [Cross Ref]
17. Xiao L., Yang Y., Zhao Y., Ai X., Yang H., Cao Y. Enhanced electrochemical performance of submicron LiCoO2 synthesized by polymer pyrolysis method. J. Solid State ElectroChem. 2008;12:149–153. doi: 10.1007/s10008-007-0373-6. [Cross Ref]
18. Tennakoon T.M.T.N., Lindbergh G, Bergman B. Performance of LiCoO2 cathodes, prepared using the Pechini method, in molten carbonate fuel cells. J. Electrochem. Soc. 1997;144:2296–2301. doi: 10.1149/1.1837807. [Cross Ref]
19. Rodrigues S., Munichandraiah N., Shukla A.K. Novel solution-combustion synthesis of LiCoO2 and its characterization as cathode material for lithium-ion cells. J. Power Sources. 2001;102:322–325. doi: 10.1016/S0378-7753(01)00770-4. [Cross Ref]
20. Maly E.N., Dedov N.V., Kutyavin E.M., Sennikov Yu, Soloviov A.I., Stepanov I.A., Makeev A.A., Lyubimova L.L. Production of superdispersed powders for cathode masses of lithium-ionic rechargeable batteries by thermal decomposition of salt solutions in plasma jet (in Russian) Izv. Vuz. Cvet. Metall. 2004;1:57–62.
21. Jeong W.T., Lee K.S. Synthesis and structural characteristics of LiCoO2 powders prepared by mechanical alloying of LiOH.H2O and Co(OH)2. J. Alloys Comp. 2001;322:205–210. doi: 10.1016/S0925-8388(00)01431-6. [Cross Ref]
22. Amatucci G.G., Tarascon J.M., Larcher D., Klein L.C. Synthesis of electrochemically active LiCoO2, and LiNiO2, at 100 °C. Solid State Ionics. 1996;84:169–180. doi: 10.1016/0167-2738(96)00031-8. [Cross Ref]
23. Levasseur S., Me´ne´trier M., Delmas C. On the dual effect of Mg doping in LiCoO2 and Li1+äCoO2: Structural, electronic properties, and 7Li-MAS NMR studies. Chem. Mater. 2002;14:3584–3590. doi: 10.1021/cm021107j. [Cross Ref]
24. Jang Y.I., Huang B., Wang H.F., Maskaly G.R., Ceder G., Sadoway D.R., Chiang Y.M., Liu H., Tamura H. Synthesis and characterization of LiAlyCo1-yO 2 and LiAl yNi1-yO2. J. Power Sources. 1999;81:589–593. doi: 10.1016/S0378-7753(99)00104-4. [Cross Ref]

Articles from Materials are provided here courtesy of Multidisciplinary Digital Publishing Institute (MDPI)