# Synthesis and Characterization of LiNi1/3Co1/3Mn1/3O2−xClx as Cathode Materials for Lithium Ion Batteries at 55°C

Authors: Hai-Lang Zhang; Shuixiang Liu
Journal: Advances in Materials Science and Engineering
 (2013)

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## Abstract

A series of materials based on the LiNi1/3Co1/3Mn1/3O2-xClx
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 LiNi1/3Co1/3Mn1/3O2-xClx
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.


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## Body

## 1. Introduction

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 [4]. In general, it is believed that the valence of transition-metal ions changes during Li+ intercalation and deintercalation. Tsai et al. [9] 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. [13] 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. [14] 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. Experimental

### 2.1. The Preparation of LiNi1/3Co1/3Mn1/3O2−xClx Powders

LiNi1/3Co1/3Mn1/3O2-xClx(x=0.00,0.05,0.10,0.15) powders were prepared via a sol-gel route using citric acid as chelating agent. A stoichiometric amount of LiCH3COO·2H2O (AR),  Ni(CH3COO)2·4H2O(AR), Mn(CH3COO)2·4H2O(AR), Co(CH3COO)2·4H2O(AR) and LiCl·H2O (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.


## 2.1. The Preparation of LiNi1/3Co1/3Mn1/3O2−xClx Powders

LiNi1/3Co1/3Mn1/3O2-xClx(x=0.00,0.05,0.10,0.15) powders were prepared via a sol-gel route using citric acid as chelating agent. A stoichiometric amount of LiCH3COO·2H2O (AR),  Ni(CH3COO)2·4H2O(AR), Mn(CH3COO)2·4H2O(AR), Co(CH3COO)2·4H2O(AR) and LiCl·H2O (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 CH3COCH3(g) and metal carbonates in the temperature region of 200°C –400°C [15]. A slow weight loss could be observed between 400–800°C in the curve, which is attributed to conversion of the metal carbonates into MO(s), CO2(g), and CO(g). There is little weight loss to be observed over 800°C, which indicates that the LiNi1/3Co1/3Mn1/3O2-xClx phase has formed at around 800°C.TG/DTG curves of the gel precursor of (a) LiNi1/3Co1/3Mn1/3O2 and (b) LiNi1/3Co1/3Mn1/3O2-0.10Cl0.10.
(a)
(b)


### 3.2. X-Ray Diffraction Analysis

Figure2 shows the typical X-ray diffraction patterns of LiNi1/3Co1/3Mn1/3O2-xClx   (x=0.00, 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, R3-m). 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 (x=0.00, 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 [16]. 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 a 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 [19], while the increase of lattice parameter c 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 [20].Table 1
Lattice parameters of theLiNi1/3Co1/3Mn1/3O2-xClx cathode material.
X
a (Å)
c (Å)
c
/
a
V (Å3)
I
003
/
I
104
0.00
2.858
14.228
4.978
100.61
1.32
0.05
2.861
14.231
4.974
100.89
1.38
0.10
2.861
14.249
4.980
101.01
1.37
0.15
2.862
14.254
4.980
101.11
1.37Figure 2
XRD patterns of LiNi1/3Co1/3Mn1/3O2-xClx cathode materials.


### 3.3. Electrochemical Studies

The initial charge-discharge curves of LiNi1/3Co1/3Mn1/3O2-xClx(x=0.00, 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 mAh·g−1, respectively, and the initial coulombic efficiencies are 90.4%, 93.3%, 93.0%, and 95.7%, respectively, for x=0.00 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.Figure 3
Initial charge-discharge curves of LiNi1/3Co1/3Mn1/3O2-xClx cathode materials.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 [9]. 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 [13]. Furthermore, the initial irreversible capacity loss of the materials also may be involved with the formation of surface electrolyte interphase (SEI) film [21].The cyclic performance and rate capability of LiNi1/3Co1/3Mn1/3O2-xClx(x=0.00, 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 mAh·g−1, which are 70.6%, 83.7%, 91.9%, and 85.5% of the 11th cycle at 0.5 C for x=0.00 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.Figure 4
Cyclic performance of LiNi1/3Co1/3Mn1/3O2-xClx cathode materials at different rates.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. [13] 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 c andV and the other may be due to valence balance. So the capacity retention for x=0.15 is lower than that with the chlorine content of 0.10.Figure5 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 mAh·g−1, respectively, and the initial coulombic efficiencies are 83.4%, 86.0%, 85.6% and 91.1% for x=0.00 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 LiNi1/3Co1/3Mn1/3O2-xClx(x=0.00, 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 mAh·g−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 x=0.00 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. [19] 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.Figure 5
Initial charge-discharge curves of LiNi1/3Co1/3Mn1/3O2-xClx cathode materials.Figure 6
Cyclic performance of LiNi1/3Co1/3Mn1/3O2-xClx cathode materials at different rates.


### 3.4. Cyclic Voltammetry (CV)

Figure7 presents the first cyclic voltammogram curves of LiNi1/3Co1/3Mn1/3O2 and LiNi1/3Co1/3Mn1/3O2-xClx 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. [4] 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.Cyclic voltammograms for the first curves obtained from LiNi1/3Co1/3Mn1/3O2-xClx for (a) x=0.00; (b) x=0.05; (c) x=0.10; (d) x=0.15.
(a)
(b)
(c)
(d)


## 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 CH3COCH3(g) and metal carbonates in the temperature region of 200°C –400°C [15]. A slow weight loss could be observed between 400–800°C in the curve, which is attributed to conversion of the metal carbonates into MO(s), CO2(g), and CO(g). There is little weight loss to be observed over 800°C, which indicates that the LiNi1/3Co1/3Mn1/3O2-xClx phase has formed at around 800°C.TG/DTG curves of the gel precursor of (a) LiNi1/3Co1/3Mn1/3O2 and (b) LiNi1/3Co1/3Mn1/3O2-0.10Cl0.10.
(a)
(b)


## 3.2. X-Ray Diffraction Analysis

Figure2 shows the typical X-ray diffraction patterns of LiNi1/3Co1/3Mn1/3O2-xClx   (x=0.00, 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, R3-m). 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 (x=0.00, 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 [16]. 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 a 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 [19], while the increase of lattice parameter c 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 [20].Table 1
Lattice parameters of theLiNi1/3Co1/3Mn1/3O2-xClx cathode material.
X
a (Å)
c (Å)
c
/
a
V (Å3)
I
003
/
I
104
0.00
2.858
14.228
4.978
100.61
1.32
0.05
2.861
14.231
4.974
100.89
1.38
0.10
2.861
14.249
4.980
101.01
1.37
0.15
2.862
14.254
4.980
101.11
1.37Figure 2
XRD patterns of LiNi1/3Co1/3Mn1/3O2-xClx cathode materials.


## 3.3. Electrochemical Studies

The initial charge-discharge curves of LiNi1/3Co1/3Mn1/3O2-xClx(x=0.00, 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 mAh·g−1, respectively, and the initial coulombic efficiencies are 90.4%, 93.3%, 93.0%, and 95.7%, respectively, for x=0.00 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.Figure 3
Initial charge-discharge curves of LiNi1/3Co1/3Mn1/3O2-xClx cathode materials.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 [9]. 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 [13]. Furthermore, the initial irreversible capacity loss of the materials also may be involved with the formation of surface electrolyte interphase (SEI) film [21].The cyclic performance and rate capability of LiNi1/3Co1/3Mn1/3O2-xClx(x=0.00, 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 mAh·g−1, which are 70.6%, 83.7%, 91.9%, and 85.5% of the 11th cycle at 0.5 C for x=0.00 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.Figure 4
Cyclic performance of LiNi1/3Co1/3Mn1/3O2-xClx cathode materials at different rates.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. [13] 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 c andV and the other may be due to valence balance. So the capacity retention for x=0.15 is lower than that with the chlorine content of 0.10.Figure5 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 mAh·g−1, respectively, and the initial coulombic efficiencies are 83.4%, 86.0%, 85.6% and 91.1% for x=0.00 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 LiNi1/3Co1/3Mn1/3O2-xClx(x=0.00, 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 mAh·g−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 x=0.00 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. [19] 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.Figure 5
Initial charge-discharge curves of LiNi1/3Co1/3Mn1/3O2-xClx cathode materials.Figure 6
Cyclic performance of LiNi1/3Co1/3Mn1/3O2-xClx cathode materials at different rates.


## 3.4. Cyclic Voltammetry (CV)

Figure7 presents the first cyclic voltammogram curves of LiNi1/3Co1/3Mn1/3O2 and LiNi1/3Co1/3Mn1/3O2-xClx 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. [4] 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.Cyclic voltammograms for the first curves obtained from LiNi1/3Co1/3Mn1/3O2-xClx for (a) x=0.00; (b) x=0.05; (c) x=0.10; (d) x=0.15.
(a)
(b)
(c)
(d)


## 4. Conclusions

The LiNi1/3Co1/3Mn1/3O2-xClx(x=0.00, 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 c, and V. LiNi1/3Co1/3Mn1/3O1.90Cl10 cathode material shows higher initial discharge capacity of 180.1 mAh·g−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 mAh·g−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.



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*Source: 375074-2013-12-23.xml*