# Solid Solutions ofLiCo1−xNixO2

Authors: Kelimah Elong; Norlida Kamarulzaman; Roshidah Rusdi; Nurhanna Badar; Mohd Hilmi Jaafar
Journal: ISRN Condensed Matter Physics
 (2013)

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## Abstract

Pure, single-phase and layeredLiCo1−xNixO2 materials with good cation ordering are not easy to synthesize. In this work, solid solutions of LiCo1−xNixO2 (x = 0, 0.1, …, 0.9) are synthesized using a self-propagating combustion route and characterized. All the materials are observed to be phase pure giving materials of hexagonal crystal system with R-3m space group. The RIR and R factor values of stoichiometries of LiCo1−xNixO2 (x = 0.1, 0.2, 0.3, 0.4, and 0.5) show good cation ordering. Their electrochemical properties are investigated by a series of charge-discharge cycling in the voltage range of 3.0 to 4.3 V. It is found that some of the stoichiometries exhibit specific capacities comparable or better than those of LiCoO2, but the voltage plateau is slightly more slopping than that for the LiCoO2 reference material.


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## Body

## 1. Introduction

Layered oxides are more advantageous over those of the spinels due to their higher theoretical specific capacities which are about double those of the spinels. The present commercial cathode material, LiCoO2, suffers from three major restrictions which are toxicity, cost, and scarcity. Therefore, it is logical to produce materials with less Co content [1] for commercial applications. LiNiO2 has the advantage of being cheaper, but it is more difficult to synthesize and does not cycle well [1, 2]. It is thermodynamically as well as electrochemically unstable [3]. Thus, it is unsuitable for use in commercial Li-ion batteries. Cobalt substitution in LiNiO2 is, however, more stable than its pure form [1]. LiCo1-xNixO2 can be a potential commercial cathode if a relatively simple synthesis method yielding pure single-phase compounds is found.Many groups of researchers [4–8] have attempted to synthesize some stoichiometries of LiCo1-xNixO2, but their XRD results show the presence of impurities. Others such as Xie et al. [9] and Lu and Wang [10] have produced hexagonal structure but with poor cation ordering with high (104) peaks relative to the (003) peak.We present here a simple self-propagating combustion synthesis which produces pure, single-phase, and layered hexagonal-structured materials for the whole range of solid solutions ofLiCo1-xNixO2 (x=0,0.1,…,0.9) with relatively good cation ordering especially for materials with x≤0.4 stoichiometries. Electrochemical behaviour of the materials was investigated, and it was found that some stoichiometries show comparable performance to LiCoO2 reference material.


## 2. Experimental

LiCo
1
-
x
Ni
x
O
2 (x=0,0.1,…,0.9) materials were synthesized using a self propagating combustion method [11]. For the synthesis, lithium nitrate (LiNO3, Fluka), cobalt (II) nitrate hexahydrate (Co (NO3)3·6H2O, Aldrich), and nickel (II) nitrate (Ni(NO2)3·H2O, Fluka) were used as starting materials. Nine Ni-substituted samples of LiCo1-xNixO2 (x=0.1 to 0.9) were prepared, and LiCoO2 reference material was also prepared using the same synthesis route for a fair comparison. The starting materials were first dissolved in deionised water obtained from an ultrapure deionizing water system (TKA LabTower EDI: 15–10 MΩcm) whereby a combustant, citric acid, was added according to stoichiometry. The mixture was stirred until homogeneous and slow heated until it reached its ignition conditions whereby combustion occurs. The combustion reaction is very fast and is over in a few seconds. The precursors obtained were annealed at 700°C for 24 h. The final products were grinded until fine and characterized.Characterizations of the materials were done using X-ray diffraction (XRD) with CuKα radiation to identify the crystalline phase and purity of the materials. The XRD data was acquired with a PANalytical Xpert Pro powder diffraction equipment at room temperature and measured using the Bragg-Brentano optical configuration. The sample was prepared using the back loading method to minimise preferred orientation effects. The particle size and powder morphology of the synthesized materials were examined by scanning electron microscopy (SEM), using the JEOL JSM-7600F microscope.The cathode was prepared using 80 wt%LiCo1-xNixO2, 10 wt% polytetrafluoroethylene (PTFE) as binder, and 10 wt% Super P (a type of carbon) as an electronic conductor. The mixture was pressed onto metal grids, and the cathode was dried in an oven at 200°C for 24 h. The separator was a Celgard 2400 microporous polyethylene film, and lithium metal was used as anode. The electrolyte was 1.0 M lithium hexafluorophosphate, LiPF6 in 1 : 1 volume ratio of ethylene carbonate (EC) and dimethyl carbonate (DMC) from Mitsubishi Chemical Corporation. The cells were assembled in a glove box (Unilab Mbraun) with oxygen and water content of less than 0.1 ppm. The cells were tested using a battery tester, the WonATech (WBCS 3000) electrochemical testing equipment. The cells were cycled using a constant current of 43.5 mA g−1 at a voltage range of between 3.0 and 4.3 V.


## 3. Results and Discussions

The most obvious advantage of using this combustion route is the ease of the method and speed of the reaction which is over in a few seconds. The precursors are already in dry form, and, subsequently, the thermal annealing can be done directly without further drying or precalcination process. Therefore, the synthesis method has the advantage of producing homogeneous materials with the resulting final products free from impurities, even for the Ni-rich stoichiometries. Thus, a whole range of solid solutions ofLiCo1-xNixO2 (x=0,0.1,…,0.9) materials are obtainable as pure, single-phase compounds. So far, no researchers have shown that all the solid solutions of LiCo1-xNixO2 (x=0,0.1,…,0.9) materials in pure form are obtainable by using one synthesis method. For example, Ohzuku et al. [12], Makimura and Ohzuku [13], Julien et al. [14], Saadoune and Delmas [15], Nayoze et al. [16], all show only one stoichiometry with their respective synthesis methods. The others produce LiCo1-xNixO2 materials that are not pure, containing minor phases [17], or materials that do not show good layered structures [18].The XRD patterns of theLiCo1-xNixO2 (x=0,0.1,…,0.9) materials are shown in Figure 1. They are taken with high counts in order to show that there are no minor phases and impurity peaks present in the samples. The samples are all pure, layered compounds. This means that the Ni-ions have been successfully substituted in the LiCoO2 structure. It can be clearly observed that all of the fingerprint peaks, namely, (003), (101), (006), (012), (104), (018), and (110) are easily identifiable in all of the XRD patterns. All the diffraction peaks can be indexed with α-NaFeO2-type structure based on the hexagonal crystal system with R-3m space group. They are isostructural with LiNiO2 and LiCoO2 phases as compared with the XRD patterns in the ICDD database corresponding to patterns number 98-000-9674 and 98-001-1288, respectively. The XRD patterns also show sharp peaks in the spectra indicating a high degree of crystallinity of the materials. Clear peak splittings of the (006)/(012) and the (008)/(110) doublets are an indication of highly layered structure [19, 20]. It is observed in our samples that the (006)/(012) and the (008)/(110) peak splittings are more distinct in the lesser Ni content materials of the LiCo1-xNixO2 which are an indication that high nickel content reduces the layered characteristics of the compounds. The reference intensity ratio (RIR) and R factor are given by the following expressions:
(1)RIR=I(003)I(104),R=I(006)+I(012)I(101),
and they are taken as a measure of the cation ordering of the materials [17, 21]. A high RIR of 1.2 and above indicates good cation ordering [21]. As for the R factor, values of less than 1.0 indicate good cation ordering [18, 22]. Our data indicates high RIR values of above 1.2 and very low R factor values for the materials x=0.1 to 0.5 of the LiCo1-xNixO2 cathode materials corresponding to the respective compounds to reveal the splitting of the (006)/(012) peaks. Ionic radius plays an important role in the cation mixing phenomenon [17]. The Li+, Co3+, Ni3+, and Ni2+ ionic radii are 0.76 Å´, 0.55 Å´, 0.56 Å´, and 0.69 Å´ (in coordination 6), respectively [23]. It can be seen that the Ni2+ ion is quite similar in size to the Li+ ion; therefore, cation mixing between these two ions is more likely especially in the high Ni content materials. There is also more likelihood of Ni to exist in the Ni2+ oxidation state for the Ni-rich samples. Our results indicate that for x≤0.5 in the LiCo1-xNixO2 materials, the cation ordering is very good, and these materials are expected to perform well in the electrochemical tests.XRD patterns of (a) LiCo0.1Ni0.9O2, (b) LiCo0.2Ni0.8O2, (c) LiCo0.3Ni0.7O2, (d) LiCo0.4Ni0.6O2, (e) LiNi0.5Co0.5O2, (f) LiCo0.6Ni0.4O2, (g) LiCo0.7Ni0.3O2, (h) LiCo0.8Ni0.2O2, (i) LiCo0.9Ni0.1O2, and (j) LiCoO2 and enlargement of the XRD patterns at 30° and 50° for (k) to (t) materials.Cyclic voltammograms of theLiCo1-xNixO2 materials are shown in Figure 2. The oxidation peaks seem to increase as the Ni content increases in the materials. The oxidation and reduction peaks are listed in Table 1. There seem to be two broad reduction peaks in the Ni-substituted materials compared to those of the pure LiCoO2 material. This is attributed to the redox couples Ni4+/Ni3+ and Ni3+/Ni2+ [24] and is reflected by the double or triple plateaus of the charge-discharge curves of the heavier Ni content materials in Figure 3. It is believed that the Ni-rich materials have both Ni3+ and Ni2+ ions. The lower voltage plateaus are attributed to the Ni3+/Ni2+ redox couple. One consequence for the existence of Ni2+ ions in the sample is that there will be the existence of Co4+ in the sample to balance the charge. The existence of Co4+ is detrimental to the electrochemical performance of the materials because Co4+ is not electroactive. This may be one of the reasons why the heavier Ni content samples, LiCo1-xNixO2 (x=0.9 to 0.8), do not show good electrochemical charge-discharge as seen later.Table 1
Electrochemical performances ofLiCo1-xNixO2 (x=0, 0.1, …0.9) and LiCoO2 annealed at 700°C for 24 h.
Material700°C, 24 h
Theoretical value
1st discharge capacity (mAh g−1)
2nd discharge capacity (mAh g−1)
30th discharge capacity (mAh g−1)
Capacity loss after 30th cycles (%)
Oxidation peak (V)
Reduction peak (V)
RIRI(003)/I(104)
R factor [I(006) + I(012)]/I(101)
LiCo0.1Ni0.9O2
274.43
66
61
56
15.15
5.18
2.80
0.94
1.00
LiCo0.2Ni0.8O2
274.36
95
90
86
9.47
5.11
2.76
1.07
0.83
LiCo0.3Ni0.7O2
274.35
146
141
113
22.6
5.15
2.82
1.17
0.62
LiCo0.4Ni0.6O2
274.23
152
150
132
13.16
5.10
2.92
1.32
0.62
LiCo0.5Ni0.5O2
274.16
162
158
136
16.05
4.99
2.63
1.33
0.54
LiCo0.6Ni0.4O2
274.10
165
162
138
16.36
4.89
3.22
1.38
0.51
LiCo0.7Ni0.3O2
274.03
155
150
138
10.97
4.65
3.35
1.40
0.53
LiCo0.8Ni0.2O2
273.96
145
140
134
6.94
4.92
3.14
1.42
0.49
LiCo0.9Ni0.1O2
273.89
143
138
129
9.79
4.99
3.12
1.46
0.43
LiCoO2
273.83
149
146
134
9.46
5.04
2.95
1.58
0.43Cyclic voltammogram of (a)LiCo1-xNixO2 (x=0.9 to 0.5) and (b) LiCo1-xNixO2 (x=0.4 to 0) in voltage range 0.5 to 5.6 V at a scan rate of 3 mVs−1.
(a)
(b)Charge-discharge capacities of 1st and 30th cycles of (a) LiCo0.1Ni0.9O2, (b) LiCo0.2Ni0.8O2, (c) LiCo0.3Ni0.7O2, (d) LiCo0.4Ni0.6O2, (e) LiNi0.5Co0.5O2, (f) LiCo0.6Ni0.4O2, (g) LiCo0.7Ni0.3O2, (h) LiCo0.8Ni0.2O2, (i) LiCo0.9Ni0.1O2, and (j) LiCoO2.
(a)
(b)The first cycle and thirtieth cycle charge-discharge curves of the materials are shown in Figure3. It can be seen that via this synthesis route, LiCoO2 shows a specific capacity of 149 mAh g−1 which is better than the commercial value of about 120 mAh g−1.As was discussed earlier, the combustion synthesis results in highly ordered layered compounds that show good electrochemical performance. The discharge profile of the LiCoO2 material exhibiting a flat plateau at a high average voltage of about 3.9 V illustrates why LiCoO2 is a very popular commercial cathode material hard to match by other cathode materials. Four of the materials, LiCo0.4Ni0.6O2, LiCo0.5Ni0.5O2, LiCo0.6Ni0.4O2, and LiCo0.7Ni0.3O2, all show better initial capacities than LiCoO2. The stoichiometry of LiCo0.6Ni0.4O2 shows the best specific capacity of 165 mAh g−1 over the voltage range of 4.3 to 3.0 V in the first cycle. The voltage plateau, however, is lower than that of LiCoO2 and slopping down more drastically to 3.0 V. This means that the energy density of the material is slightly lowered due to the lower voltage plateau. This material also suffers from the most capacity loss at the 30th cycle (16.3%) as given in Table 1. LiCoO2, on the other hand, only lost 9.5% capacity at the 30th cycle. Another material that seems to show good performance with higher average voltage than LiCo0.6Ni0.4O2 is LiCo0.7Ni0.3O2. This material shows specific capacity of 155 mAh g−1 and 138 mAh g−1 for the 1st and 30th cycles, respectively. At the 30th cycle, LiCo0.3Ni0.7O2 seems to perform better than LiCo0.6Ni0.4O2 with only about 11% lost in capacity. The discharge plateau is also quite similar to that of LiCoO2. The good performance of the materials is believed to be attributable to several factors such as those of highly ordered crystal structure and smaller particle size as discussed later.The SEM images of LiCoO2 and LiCo1-xNixO2 (x=0,0.1,…,0.9) are displayed in Figure 4. The images show that all samples are well-formed polycrystalline materials. The images show that the introduction of Ni in the LiCoO2 lattice immediately decreases the crystallite size of the LiCo1-xNixO2 materials. The crystal size of LiCoO2 seem larger compared to the Ni-substituted materials. All the materials have mostly polyhedral-type crystals. Samples (a), (b), and (c) have larger crystallite sizes of about 50 to 300 nm but smaller than LiCoO2 crystallite size which is about a few microns in size. Samples (d), (e), and (f) have very similar crystallite size of about 50 to 200 nm which are bigger than those of samples (g), (h), and (i). Samples (g), (h), and (i) have the smallest range of crystallite sizes of about 50 to 100 nm. Some of the crystals seem to aggregate slightly into larger particles. It is clear here that the smaller crystallite size of nm range of the samples, LiCo0.7Ni0.3O2, LiCo0.8Ni0.2O2, and LiCo0.9Ni0.1O2, contributes to better performance in terms of specific capacity as well as capacity retention of the materials [25]. The high surface area to volume ratio of nanocrystals increased the efficiency of the electrochemical process which is a surface-dependent phenomenon.SEM images of (a) LiCo0.1Ni0.9O2, (b) LiCo0.2Ni0.8O2, (c) LiCo0.3Ni0.7O2, (d) LiCo0.4Ni0.6O2, (e) LiNi0.5Co0.5O2, (f) LiCo0.6Ni0.4O2, (g) LiCo0.7Ni0.3O2, (h) LiCo0.8Ni0.2O2, (i) LiCo0.9Ni0.1O2, and (j) LiCoO2.
(a)
(b)
(c)
(d)
(e)
(f)
(g)
(h)
(i)
(j)


## 4. Conclusion

LiCo
1
-
x
Ni
x
O
2 (x=0,0.1,…,0.9) materials, via the self propagating combustion method, have been successfully synthesized and show single-phase, pure products with high crystallinity. The LiCo1-xNixO2 (x=0.1,…,0.5) materials show good cation ordering and exhibit high specific capacities with slightly lower and slopping discharge plateaus. In conclusion, the self-propagating combustion synthesis is a good synthesis method for getting well-ordered structures of LiCo1-xNixO2 materials with electrochemical performance comparable to LiCoO2.



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*Source: 568191-2013-02-11.xml*