The nano-structured Li[Li0.2Co0.4Mn0.4]O2 cathode material is synthesized by a co-precipitation method. X-ray diffraction shows that the synthesized material has a hexagonal α-NaFeO2 type structure with a space group R-3m. Scanning electron microscopy and transmission electron microscopy images show the homogeneous distribution with 100-200 nm. X-ray photoelectron spectroscopy results indicate that the oxi-dation states of Co and Mn in Li[Li0.2Co0.4Mn0.4]O2 are present in trivalence and tetravalence, respectively. The charge-discharge curves and cycling performance are analyzed in detail. The initial charge and dis-charge capacities are respectively 236.5 mAh g-1 and 140.3 mAh g-1 at the current density of 100 mA g-1 in the voltage range of 2.0-4.6 V.
When you are citing the document, use the following link http://essuir.sumdu.edu.ua/handle/123456789/3520

Liu, G.R.

Lu, X.X.

Wei, X.

Zhang, S.C.

Electronic Sumy State University Institutional Repository

PROCEEDINGS OF THE INTERNATIONAL CONFERENCE  NANOMATERIALS: APPLICATIONS AND PROPERTIES Vol. 2 No 2, 02PCN27(3pp) (2013)   2304-1862/2013/2(2)02PCN27(3) 02PCN27-1  2013 Sumy State University Structure and Electrochemical Performance of Li[Li0.2Co0.4Mn0.4]O2 Cathode Material for Lithium Ion Battery by Co-precipitation Method  X. Wei, X. X. Lu, S. C. Zhang*, G. R. Liu  School of Materials Science and Engineering, Beihang University, Beijing 100191, PR China  (Received 09 June 2013; published online 02 September 2013)  The nano-structured Li[Li0.2Co0.4Mn0.4]O2 cathode material is synthesized by a co-precipitation method. X-ray diffraction shows that the synthesized material has a hexagonal α-NaFeO2 type structure with a space group R-3m. Scanning electron microscopy and transmission electron microscopy images show the homogeneous distribution with 100-200 nm. X-ray photoelectron spectroscopy results indicate that the oxi-dation states of Co and Mn in Li[Li0.2Co0.4Mn0.4]O2 are present in trivalence and tetravalence, respectively. The charge-discharge curves and cycling performance are analyzed in detail. The initial charge and dis-charge capacities are respectively 236.5 mAh g-1 and 140.3 mAh g-1 at the current density of 100 mA g-1 in the voltage range of 2.0-4.6 V.  Keywords: Li-ion battery; Li[Li0.2Co0.4Mn0.4]O2; Co-precipitation Method; Li-rich layered material; Cathode.   PACS numbers: 81.07.–b, 82.47.Jk                                                             * csc@buaa.edu.cn 1. INTRODUCTION  Lithium ion batteries were considered to be a promis-ing electric storage technology for electric vehicles. A vast series of Li-storage cathode materials had been ex-plored in the past two decades. LiCoO2 had been widely applied due to its good electrochemical performance and its ease of preparation. However, the concerns about high costs, toxicity and structural instability prompted a search for alternative cathode materials. Manganese substitution was considered because it was more abun-dant and cheaper than Cobalt. Li-rich cathode materials xLiCoO2·(1-x)Li2MnO3 have been studied in the recent past [1-3]. In these materials, Li2MnO3 existed with short-range order within a LiCoO2 matrix [4]. Li+ extrac-tion and oxygen loss from lattice were concurrent at the first charge process of Li-rich layered materials. A part of Mn4+ ions was activated to participate in the following electrochemical reactions, leading to a high discharge capacity [5]. Among the different stoichiometric ratio of xLiCoO2•(1-x)Li2MnO3 compounds, Li[Li0.2Co0.4Mn0.4]O2 have been studied by many authors. To improve the per-formance of Li[Li0.2Co0.4Mn0.4]O2 materials, some groups have recently adopted different synthetic methods, such as sol-gel method [6], solid state method [7, 8], oxalate-precursor method [9]. In this work, we developed a simple co-precipitation method to synthesize nano-structured Li[Li0.2Co0.4Mn0.4]O2 particles. The structure, morphology and electrochemical properties were thoroughly investi-gated.  2. EXPERIMENTAL  The Li[Li0.2Co0.4Mn0.4]O2 sample was synthesized by a co-precipitation method. The procedure was de-scribed as follows. The desired amount of Co(NO3)2·6H2O, MnCl2·4H2O were dissolved to form a aqueous solution. M(OH)2 (M = Co, Mn) precipitate was gained by slowly dripping the above solution and LiOH solution synchronously into a glass reactor with continuous strring. The pH value of the reactant solu-tion was adjusted by ammonia and was kept at 11. The hydroxide precipitate was filtrated, washed and dried. The mixture of precipitate and LiOH·H2O were ground and initially heat-treated at 500 °C for 5 h for the impregnation of Lithium into the matrix. The fi-nal product was finally obtained by sintering at 800 °C for 10 h and then quenching to room temperature.  X-ray diffraction (XRD, Rigaku D/Max-2400, Ja-pan) using Cu Kα radiation was used to identify the crystalline structure of the synthesized materials. Scanning electron microscopy (SEM, Hitachi S-4800, Japan), transmission electron microscopy (TEM, JEM-2100F, Japan) were engaged to observe morphology, size and distribution of as-prepared material. X-ray photoelectron spectroscopy (XPS) was obtained by using ESCALAB250 (Thermo Fisher Scientific) with monochromatic Al Kα anode source with pass energy of 20 eV and energy step of 0.1 eV. The chemical va-lence state of the transition metal elements was de-termined. The electrode slurry was prepared by mixing 80 wt.% active material, 10 wt.% carbon black, and 10 wt.% polyvinylidene fluoride (PVDF) with n-methyl-2-pyrrolidone (NMP). The prepared slurry was pasted onto an aluminum foil. The electrode was then dried in a vacuum oven at 100 °C for 2 h. The testing half-cells were assembled in an argon-filled glove box (MB-10-G with TP170b/mono, MBRAUN) with lithium metal as counter and reference electrode. Electrolyte was 1 M LiPF6 in a mixed solution of EC and DMC (1:1 in vol-ume ratio). The charge-discharge measurements were galvanostatically carried out by using a battery test system (NWEARE BTS-610, Neware Technology Co., Ltd., China). All the batteries were tested over a volt-age range between 2.0 V and 4.6 V vs. Li0/Li+ at room temperature.  3. RESULTS AND DISCUSSION   X. WEI, X. X. LU, S. C. ZHANG, G. R. LIU PROC. NAP 2, 02PCN27 (2013)   02PCN27-2 Fig. 1 shows the X-ray diffraction pattern of Li[Li0.2Co0.4Mn0.4]O2 sample. All the major diffraction peaks can be indexed as a layered oxide lattice based on a hexagonal α-NaFeO2 type structure with a space group R-3m [10]. The weak peaks between 21° and 25° are reflected by a monoclinic unit cell with a C2/m symmetry, due to a LiMn6 cation arrangement that occurs in the transition metal layers of Li2MnO3 re-gions [11]. Both (006)/(102) and (108)/(110) doublets are clear split, suggesting that the material crystallized in the layered structure without formation of any spinel structure [11].    Fig. 1 – X-ray diffraction pattern of Li[Li0.2Co0.4Mn0.4]O2 sample  Fig. 2 shows the SEM and TEM images of Li[Li0.2Co0.4Mn0.4]O2 sample. It can be observed that homogeneous particles with dimensions in a narrow range between 100 nm and 200 nm. Undoubtedly, such nano-sized particles must result in a high sur-face area and a short diffusion path for Li inser-tion/extraction and also for the diffusive transport of the oxygen ion vacancies, so as to enhance the electro-chemical performance, especially the high rate capaci-ty [12].     Fig. 2 – SEM and TEM images of Li[Li0.2Co0.4Mn0.4]O2 sample.  Fig. 3 shows Co2p and Mn2p XPS spectra of as-prepared material. The chemical valence state of the transition metal elements is determined. In Fig. 3A, the results show a Co2p3/2 main peak at 780.9 eV with a satellite peak at 790.3 eV and a Co2p1/2 main peak at 795.9 eV with a satellite peak at 805.2 eV. It confirms that the main oxidation state is Co3+ [13, 14]. In the Mn2p spectra (Fig. 3B), the major peak Mn2p3/2 at 643.1 eV confirms the Mn4+ oxidation states in this material, in accord with previous reports [15, 16].    Fig. 3 – Co2p (A) and Mn2p (B) XPS spectra of Li[Li0.2Co0.4Mn0.4]O2 sample  Fig. 4 shows the 1st (A) and 2nd (B) cycles charge-discharge curves for Li[Li0.2Co0.4Mn0.4]O2 sample be-tween 2.0 and 4.6 V at the current density of 100 and 200 mA g-1. In the first charge process, the slope of 4.0-4.4 V corresponds to the oxidation of the transition metal (Co3+ → Co3.6) [1], and a long plateau at ~4.5 V corresponds to oxygen loss with Li extraction, attrib-uting to active process of Li2MnO3 (Li2MnO3 → 2Li+ + 2e- + 0.5O2 + MnO2) [17]. The long plateau vanishes during the subsequent charge cycles. After this irre-versible structural transformation, both Co3.6+ and Mn4+ can be reduced in the first discharge process. The sample delivers the first charge capacity of 236.5 mAh g-1 and the first discharge capacity of 140.3 mAh g-1 at the current density of 100 mA g-1, with the coulombic efficiency of 59.3%. The sample delivers the first charge capacity of 126.5 mAh g-1 and the first discharge capac-ity of 76.6 mAh g-1 at the current density of 200 mA g-1, with the coulombic efficiency of 60.5%. The 2nd charge capacities are respectively 158.2 and 88.8 mAh g-1 and discharge capacities are respectively 143.8 and 77.3 mAh g-1, corresponding to the current density of 100 and 200 mA g-1, respectively, with the coulombic effi-ciency of 90.9% and 87.0%. After 100th cycles (Fig. 5), the retained discharge capacities are respectively 119.1 and 95.9 mAh g-1, which are 83.2%, and 124.1% of their 2nd discharge capacities, corresponding to the current density of 100 and 200 mA g-1. The cycling process ac-companies with activation process of Li2MnO3 compo-nent and capacity decay. Activation process undergoes a longer duration with higher current density. It can be observed that the discharge capacity ascends in the beginning several cycles and then descends in the sub- STRUCTURE AND ELECTROCHEMICAL PERFORMANCE OF… PROC. NAP 2, 02PCN27 (2013)   02PCN27-3 sequent cycles from two profiles. The activation process of Li2MnO3 component plays a main role in the ascend-ing part. The descending part may be ascribed to the irreversible capacity loss caused by structural collapse during intercalation/deintercalation of Li+. The degree of decline enlarges at lower current density, probably due to the more serious structure damage during the deeper charge and discharge process.     Fig. 4 – The 1st (A) and 2nd (B) cycles charge-discharge curves of Li[Li0.2Co0.4Mn0.4]O2 sample at the current density of 100 and 200 mA g-1.   Fig. 5 – Galvanostatic cycling performance of Li[Li0.2Co0.4Mn0.4]O2 sample for 100 cycles.  4. CONCLUSIONS  The nano-sized material Li[Li0.2Co0.4Mn0.4]O2 was synthesized by a co-precipitation method. After 100th cycles, the retained discharge capacities are respective-ly 119.1 and 95.9 mAh g-1, which are 83.2%, and 124.1% of their 2nd discharge capacities, corresponding to the current density of 100 and 200 mA g-1. Much work needs to be done in order to meet its commercial application.  AKNOWLEDGEMENTS  This work was supported by the National Basic Re-search Program of China (973 Program) (2013CB934001), National Natural Science Foundation of China (51074011 and 51274017) and National 863 Program (2007AA03Z231 and 2011AA11A257).   REFERENCES  1. T. A. Arinkumar, Y. Wu and A. Manthiram, Chem. Mater. 19, 3067 (2007). 2. Y. Wu and A. Manthiram, Solid. State. Ionics 180, 50 (2009). 3. G. Singh, W. C. West, J. Soler and R. S. Katiyar, J. Power Sources 218, 34 (2012). 4. S. H. Kang, C. S. Johnson, J. T. Vaughey, K. Amine and M. M. Thackeray, J. Electrochem. Soc. 153, A1186 (2006). 5. M. M. Thackeray, S. H. Kang, C. S. Johnson, J. T. Vaughey, R. Benedek and S. A. Hackney, J. Mater. Chem. 17, 3112 (2007). 6. Z. Li, Y. Wang, X. Bie, K. Zhu, C. Wang, G. Chen and Y. Wei, Electrochem. Commun. 13, 1016 (2011). 7. J. Bareno, M. Balasubramanian, S. H. Kang, J. G. Wen, C. H. Lei, S. V. Pol, I. Petrov and D. P. Abraham, Chem. Mater. 23, 2039 (2011). 8. J. G. Wen, J. Bareno, C. H. Lei, S. H. Kang, M. Balasubramanian, I. Petrov and D. P. Abraham, Solid. State. Ionics 182, 98 (2011). 9. D. Luo, G. S. Li, X. F. Guan, C. Yu, J. Zheng, X. H. Zhang and L. P. Li, J. Mater.Chem. A 1, 1220 (2013). 10. J. Gao and A. Manthiram, J. Power Sources 191, 644 (2009). 11. Z. H. Lu, L. Y. Beaulieu, R. A. Donaberger, C. L. Thomas and J. R. Dahn, J. Electrochem. Soc. 149, A778 (2002). 12. B. H. Song, Z. W. Liu, M. O. Lai and L. Lu, Phys. Chem. Chem. Phys. 14, 12875 (2012). 13. J. Zheng, S. N. Deng, Z. C. Shi, H. J. Xu, H. Xu, Y. F. Deng, Z. Zhang and G. H. Chen, J. Power Sources 221, 108 (2013). 14. K. J. K. Beng Jit Tan, Peter M. A. Sherwood, J. Am. Chem. Soc., 113, 855 (1991). 15. C. J. Jafta, K. I. Ozoemena, M. K. Mathe and W. D. Roos, Electrochim. Acta 85, 411 (2012). 16. J. S. Park, K. C. Roh, J. W. Lee, K. Song, Y. I. Kim and Y. M. Kang, J. Power Sources, 230, 138 (2013). 17. B. H. Song, M. O. Lai and L. Lu, Electrochim. Acta 80, 187 (2012).    

Structure and Electrochemical Performance of Li[Li0.2Co0.4Mn0.4]O2 Cathode Material for Lithium Ion Battery by Co-precipitation Method

SocioEconomic Challenges Journal (Sumy State University)

PROCEEDINGS OF THE INTERNATIONAL CONFERENCE  
NANOMATERIALS: APPLICATIONS AND PROPERTIES 
Vol. 2 No 2, 02PCN27(3pp) (2013) 
 
 
2304-1862/2013/2(2)02PCN27(3) 02PCN27-1  2013 Sumy State University 
Structure and Electrochemical Performance of Li[Li0.2Co0.4Mn0.4]O2 Cathode Material for 
Lithium Ion Battery by Co-precipitation Method 
 
X. Wei, X. X. Lu, S. C. Zhang*, G. R. Liu 
 
School of Materials Science and Engineering, Beihang University, Beijing 100191, PR China 
 
(Received 09 June 2013; published online 02 September 2013) 
 
The nano-structured Li[Li0.2Co0.4Mn0.4]O2 cathode material is synthesized by a co-precipitation method. 
X-ray diffraction shows that the synthesized material has a hexagonal α-NaFeO2 type structure with a 
space group R-3m. Scanning electron microscopy and transmission electron microscopy images show the 
homogeneous distribution with 100-200 nm. X-ray photoelectron spectroscopy results indicate that the oxi-
dation states of Co and Mn in Li[Li0.2Co0.4Mn0.4]O2 are present in trivalence and tetravalence, respectively. 
The charge-discharge curves and cycling performance are analyzed in detail. The initial charge and dis-
charge capacities are respectively 236.5 mAh g-1 and 140.3 mAh g-1 at the current density of 100 mA g-1 in 
the voltage range of 2.0-4.6 V. 
 
Keywords: Li-ion battery; Li[Li0.2Co0.4Mn0.4]O2; Co-precipitation Method; Li-rich layered material; Cathode. 
 
 PACS numbers: 81.07.–b, 82.47.Jk 
 
 
                                                          
* csc@buaa.edu.cn 
1. INTRODUCTION 
 
Lithium ion batteries were considered to be a promis-
ing electric storage technology for electric vehicles. A 
vast series of Li-storage cathode materials had been ex-
plored in the past two decades. LiCoO2 had been widely 
applied due to its good electrochemical performance and 
its ease of preparation. However, the concerns about 
high costs, toxicity and structural instability prompted a 
search for alternative cathode materials. Manganese 
substitution was considered because it was more abun-
dant and cheaper than Cobalt. Li-rich cathode materials 
xLiCoO2·(1-x)Li2MnO3 have been studied in the recent 
past [1-3]. In these materials, Li2MnO3 existed with 
short-range order within a LiCoO2 matrix [4]. Li+ extrac-
tion and oxygen loss from lattice were concurrent at the 
first charge process of Li-rich layered materials. A part 
of Mn4+ ions was activated to participate in the following 
electrochemical reactions, leading to a high discharge 
capacity [5]. Among the different stoichiometric ratio of 
xLiCoO2•(1-x)Li2MnO3 compounds, Li[Li0.2Co0.4Mn0.4]O2 
have been studied by many authors. To improve the per-
formance of Li[Li0.2Co0.4Mn0.4]O2 materials, some groups 
have recently adopted different synthetic methods, such 
as sol-gel method [6], solid state method [7, 8], oxalate-
precursor method [9]. 
In this work, we developed a simple co-
precipitation method to synthesize nano-structured 
Li[Li0.2Co0.4Mn0.4]O2 particles. The structure, morphology 
and electrochemical properties were thoroughly investi-
gated. 
 
2. EXPERIMENTAL 
 
The Li[Li0.2Co0.4Mn0.4]O2 sample was synthesized 
by a co-precipitation method. The procedure was de-
scribed as follows. The desired amount of 
Co(NO3)2·6H2O, MnCl2·4H2O were dissolved to form a 
aqueous solution. M(OH)2 (M = Co, Mn) precipitate 
was gained by slowly dripping the above solution and 
LiOH solution synchronously into a glass reactor with 
continuous strring. The pH value of the reactant solu-
tion was adjusted by ammonia and was kept at 11. 
The hydroxide precipitate was filtrated, washed and 
dried. The mixture of precipitate and LiOH·H2O were 
ground and initially heat-treated at 500 °C for 5 h for 
the impregnation of Lithium into the matrix. The fi-
nal product was finally obtained by sintering at 800 
°C for 10 h and then quenching to room temperature.  
X-ray diffraction (XRD, Rigaku D/Max-2400, Ja-
pan) using Cu Kα radiation was used to identify the 
crystalline structure of the synthesized materials. 
Scanning electron microscopy (SEM, Hitachi S-4800, 
Japan), transmission electron microscopy (TEM, JEM-
2100F, Japan) were engaged to observe morphology, 
size and distribution of as-prepared material. X-ray 
photoelectron spectroscopy (XPS) was obtained by 
using ESCALAB250 (Thermo Fisher Scientific) with 
monochromatic Al Kα anode source with pass energy 
of 20 eV and energy step of 0.1 eV. The chemical va-
lence state of the transition metal elements was de-
termined. 
The electrode slurry was prepared by mixing 80 
wt.% active material, 10 wt.% carbon black, and 10 
wt.% polyvinylidene fluoride (PVDF) with n-methyl-2-
pyrrolidone (NMP). The prepared slurry was pasted 
onto an aluminum foil. The electrode was then dried in 
a vacuum oven at 100 °C for 2 h. The testing half-cells 
were assembled in an argon-filled glove box (MB-10-G 
with TP170b/mono, MBRAUN) with lithium metal as 
counter and reference electrode. Electrolyte was 1 M 
LiPF6 in a mixed solution of EC and DMC (1:1 in vol-
ume ratio). The charge-discharge measurements were 
galvanostatically carried out by using a battery test 
system (NWEARE BTS-610, Neware Technology Co., 
Ltd., China). All the batteries were tested over a volt-
age range between 2.0 V and 4.6 V vs. Li0/Li+ at room 
temperature. 
 
3. RESULTS AND DISCUSSION 
 
 X. WEI, X. X. LU, S. C. ZHANG, G. R. LIU PROC. NAP 2, 02PCN27 (2013) 
 
 
02PCN27-2 
Fig. 1 shows the X-ray diffraction pattern of 
Li[Li0.2Co0.4Mn0.4]O2 sample. All the major diffraction 
peaks can be indexed as a layered oxide lattice based 
on a hexagonal α-NaFeO2 type structure with a space 
group R-3m [10]. The weak peaks between 21° and 25° 
are reflected by a monoclinic unit cell with a C2/m 
symmetry, due to a LiMn6 cation arrangement that 
occurs in the transition metal layers of Li2MnO3 re-
gions [11]. Both (006)/(102) and (108)/(110) doublets are 
clear split, suggesting that the material crystallized in 
the layered structure without formation of any spinel 
structure [11]. 
 
 
 
Fig. 1 – X-ray diffraction pattern of Li[Li0.2Co0.4Mn0.4]O2 sample 
 
Fig. 2 shows the SEM and TEM images of 
Li[Li0.2Co0.4Mn0.4]O2 sample. It can be observed that 
homogeneous particles with dimensions in a narrow 
range between 100 nm and 200 nm. Undoubtedly, 
such nano-sized particles must result in a high sur-
face area and a short diffusion path for Li inser-
tion/extraction and also for the diffusive transport of 
the oxygen ion vacancies, so as to enhance the electro-
chemical performance, especially the high rate capaci-
ty [12].  
 
 
 
Fig. 2 – SEM and TEM images of Li[Li0.2Co0.4Mn0.4]O2 sample. 
 
Fig. 3 shows Co2p and Mn2p XPS spectra of as-
prepared material. The chemical valence state of the 
transition metal elements is determined. In Fig. 3A, 
the results show a Co2p3/2 main peak at 780.9 eV with 
a satellite peak at 790.3 eV and a Co2p1/2 main peak at 
795.9 eV with a satellite peak at 805.2 eV. It confirms 
that the main oxidation state is Co3+ [13, 14]. In the 
Mn2p spectra (Fig. 3B), the major peak Mn2p3/2 at 
643.1 eV confirms the Mn4+ oxidation states in this 
material, in accord with previous reports [15, 16]. 
 
 
 
Fig. 3 – Co2p (A) and Mn2p (B) XPS spectra of 
Li[Li0.2Co0.4Mn0.4]O2 sample 
 
Fig. 4 shows the 1st (A) and 2nd (B) cycles charge-
discharge curves for Li[Li0.2Co0.4Mn0.4]O2 sample be-
tween 2.0 and 4.6 V at the current density of 100 and 
200 mA g-1. In the first charge process, the slope of 4.0-
4.4 V corresponds to the oxidation of the transition 
metal (Co3+ → Co3.6) [1], and a long plateau at ~4.5 V 
corresponds to oxygen loss with Li extraction, attrib-
uting to active process of Li2MnO3 (Li2MnO3 → 2Li+ + 
2e- + 0.5O2 + MnO2) [17]. The long plateau vanishes 
during the subsequent charge cycles. After this irre-
versible structural transformation, both Co3.6+ and 
Mn4+ can be reduced in the first discharge process. The 
sample delivers the first charge capacity of 236.5 mAh 
g-1 and the first discharge capacity of 140.3 mAh g-1 at 
the current density of 100 mA g-1, with the coulombic 
efficiency of 59.3%. The sample delivers the first charge 
capacity of 126.5 mAh g-1 and the first discharge capac-
ity of 76.6 mAh g-1 at the current density of 200 mA g-1, 
with the coulombic efficiency of 60.5%. The 2nd charge 
capacities are respectively 158.2 and 88.8 mAh g-1 and 
discharge capacities are respectively 143.8 and 77.3 
mAh g-1, corresponding to the current density of 100 
and 200 mA g-1, respectively, with the coulombic effi-
ciency of 90.9% and 87.0%. After 100th cycles (Fig. 5), 
the retained discharge capacities are respectively 119.1 
and 95.9 mAh g-1, which are 83.2%, and 124.1% of their 
2nd discharge capacities, corresponding to the current 
density of 100 and 200 mA g-1. The cycling process ac-
companies with activation process of Li2MnO3 compo-
nent and capacity decay. Activation process undergoes 
a longer duration with higher current density. It can be 
observed that the discharge capacity ascends in the 
beginning several cycles and then descends in the sub-
 STRUCTURE AND ELECTROCHEMICAL PERFORMANCE OF… PROC. NAP 2, 02PCN27 (2013) 
 
 
02PCN27-3 
sequent cycles from two profiles. The activation process 
of Li2MnO3 component plays a main role in the ascend-
ing part. The descending part may be ascribed to the 
irreversible capacity loss caused by structural collapse 
during intercalation/deintercalation of Li+. The degree 
of decline enlarges at lower current density, probably 
due to the more serious structure damage during the 
deeper charge and discharge process. 
 
 
 
 
Fig. 4 – The 1st (A) and 2nd (B) cycles charge-discharge 
curves of Li[Li0.2Co0.4Mn0.4]O2 sample at the current density of 
100 and 200 mA g-1. 
 
 
Fig. 5 – Galvanostatic cycling performance of 
Li[Li0.2Co0.4Mn0.4]O2 sample for 100 cycles. 
 
4. CONCLUSIONS 
 
The nano-sized material Li[Li0.2Co0.4Mn0.4]O2 was 
synthesized by a co-precipitation method. After 100th 
cycles, the retained discharge capacities are respective-
ly 119.1 and 95.9 mAh g-1, which are 83.2%, and 
124.1% of their 2nd discharge capacities, corresponding 
to the current density of 100 and 200 mA g-1. Much 
work needs to be done in order to meet its commercial 
application. 
 
AKNOWLEDGEMENTS 
 
This work was supported by the National Basic Re-
search Program of China (973 Program) 
(2013CB934001), National Natural Science Foundation 
of China (51074011 and 51274017) and National 863 
Program (2007AA03Z231 and 2011AA11A257). 
 
 
REFERENCES 
 
1. T. A. Arinkumar, Y. Wu and A. Manthiram, Chem. Mater. 
19, 3067 (2007). 
2. Y. Wu and A. Manthiram, Solid. State. Ionics 180, 50 
(2009). 
3. G. Singh, W. C. West, J. Soler and R. S. Katiyar, J. Power 
Sources 218, 34 (2012). 
4. S. H. Kang, C. S. Johnson, J. T. Vaughey, K. Amine and 
M. M. Thackeray, J. Electrochem. Soc. 153, A1186 (2006). 
5. M. M. Thackeray, S. H. Kang, C. S. Johnson, J. T. 
Vaughey, R. Benedek and S. A. Hackney, J. Mater. Chem. 
17, 3112 (2007). 
6. Z. Li, Y. Wang, X. Bie, K. Zhu, C. Wang, G. Chen and Y. 
Wei, Electrochem. Commun. 13, 1016 (2011). 
7. J. Bareno, M. Balasubramanian, S. H. Kang, J. G. Wen, C. 
H. Lei, S. V. Pol, I. Petrov and D. P. Abraham, Chem. 
Mater. 23, 2039 (2011). 
8. J. G. Wen, J. Bareno, C. H. Lei, S. H. Kang, M. 
Balasubramanian, I. Petrov and D. P. Abraham, Solid. 
State. Ionics 182, 98 (2011). 
9. D. Luo, G. S. Li, X. F. Guan, C. Yu, J. Zheng, X. H. Zhang 
and L. P. Li, J. Mater.Chem. A 1, 1220 (2013). 
10. J. Gao and A. Manthiram, J. Power Sources 191, 644 
(2009). 
11. Z. H. Lu, L. Y. Beaulieu, R. A. Donaberger, C. L. Thomas 
and J. R. Dahn, J. Electrochem. Soc. 149, A778 (2002). 
12. B. H. Song, Z. W. Liu, M. O. Lai and L. Lu, Phys. Chem. 
Chem. Phys. 14, 12875 (2012). 
13. J. Zheng, S. N. Deng, Z. C. Shi, H. J. Xu, H. Xu, Y. F. 
Deng, Z. Zhang and G. H. Chen, J. Power Sources 221, 108 
(2013). 
14. K. J. K. Beng Jit Tan, Peter M. A. Sherwood, J. Am. Chem. 
Soc., 113, 855 (1991). 
15. C. J. Jafta, K. I. Ozoemena, M. K. Mathe and W. D. Roos, 
Electrochim. Acta 85, 411 (2012). 
16. J. S. Park, K. C. Roh, J. W. Lee, K. Song, Y. I. Kim and Y. 
M. Kang, J. Power Sources, 230, 138 (2013). 
17. B. H. Song, M. O. Lai and L. Lu, Electrochim. Acta 80, 187 
(2012). 
 
 
 


https://essuir.sumdu.edu.ua/bitstream/123456789/35203/1/princon_2013_2_2_29.pdf

Structure and Electrochemical Performance of Li[Li0.2Co0.4Mn0.4]O2 Cathode Material for Lithium Ion Battery by Co-precipitation Method

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