• We are sorry, but NCBI web applications do not support your browser and may not function properly. More information
Logo of nanoreslettspringer open web sitethis articlemanuscript submissionregistrationjournal front pagespringer open web site
Nanoscale Res Lett. 2012; 7(1): 60.
Published online Jan 5, 2012. doi:  10.1186/1556-276X-7-60
PMCID: PMC3271028

Synthesis and characterization of integrated layered nanocomposites for lithium ion batteries

Abstract

The series of Li[NixMxLi1/3-xMn2/3-x]O2 cathodes, where M is cobalt or chromium with a wide compositional range x from 0 to 0.33, were prepared by hydroxide coprecipitation method with subsequent quenching. The sample structures were investigated using X-ray diffraction results which were indexed completely on the basis of a trigonal structure of space group R3m¯ with monoclinic C2/m phase as expected. The morphologies and electrochemical properties of the samples obtained were compared as the value of x and substituted transition metal. The particle sizes of cobalt-substituted Li[NixCoxLi1/3-xMn2/3-x]O2 samples are much smaller than those of the Li[NixCrxLi1/3-xMn2/3-x]O2 system. The electrode containing Li[NixCoxLi1/3-xMn2/3-x]O2 with x = 0.10 delivered a discharge capacity of above 200 mAh/g after 10 cycles due to the activation of Li2MnO3.

PACS: 82.47.Aa; 82.47.-a; 82.45.Fk.

Keywords: lithium ion batteries, cathodes, nanocomposites, coprecipitation

Introduction

The development of rechargeable lithium ion batteries depends critically on the technological advances in electrode materials. Over the years, several compounds such as spinel LiMn2O4, olivine LiFePO4 [1], and layered LiCoO2 and LiNiO2 have been studied extensively by many researchers as cathode materials for lithium ion batteries. In fact, LiMn2O4 and LiFePO4 have distinct advantages of being cost-effective and environmentally benign. However, LiMn2O4 suffers from capacity fading due to the dissolution of manganese and Jahn-Teller distortion [2,3], while LiFePO4 delivers insufficient capacity and low electronic conductivity [4].

Commercially used LiCoO2 cathode has advantages of easy synthesis and excellent lithium ion mobility though challenging issues of stability, achieving practical capacities, and environmental risks need to be addressed [2]. The layer-structured rhombohedral LiMnO2 (R3m¯) attracts interest as a potential cathode due to its cost effectiveness and relatively high capacity, but it exhibits severe capacity fading during extended cycling. More precisely, its discharge behavior during electrochemical cycling needs significant improvement. The strategies to overcome such limitations in rhombohedral LiMnO2 have been focused on metal ion substitution [5,6]. Due to its higher theoretical capacity, LiNiO2 has also been investigated as an alternative cathode to commercial LiCoO2. However, it is complicated to synthesize a pure-layered structure with a well-ordered phase because of severe cationic disordering between nickel and lithium ions that occurs due to the ionic radii values of Ni2+(0.069 nm) and Li+(0.068 nm) being almost similar. Further, capacity fading occurs during discharge since the electronic state in low spin Ni3+ serves as the satisfactory condition for the Jahn-Teller distortion observed in the spinel LiMn2O4.

In light of the above discussions, many researchers have investigated on the strategies to replace LiCoO2. First, alien transition metal ions such as Ni, Mn, and Cr could be introduced in order to exploit their advantages of stable and high redox-couple properties. Second, by combining stable Li2MnO3 as an inactive frame with layered LiMO2, lithium-saturated solid solutions or nanocomposite xLi2MnO3·(1-x)LiMO2 with prolonged structural integrities have been researched to take advantage of their stable and rigid structure [7-11]. Here, Li2MnO3, which has a layered rock salt structure (space group R3m¯) with a monoclinic phase (C2/m), can be represented in layered form as Li[Li1/3Mn2/3]O2. Further, the nanocomposites can be represented by the notation, Li[M1-xLix/3 Mn2x/3]O2 with a layered structure [12-14]. Our earlier work was focused on investigating one such nanocomposite electrode namely, 0.4Li2MnO3·0.6LiMO2 (M = Ni1/3Co1/3Mn1/3 and Ni1/3Cr1/3Mn1/3) [13]. The encouraging results obtained from that study led us to investigate the physicochemical properties of the doped nanocomposites with a layered structure over a range of stoichiometric compositions.

Therefore, the present work reports on the synthesis and systematic investigations on the structure, morphology, and electrochemical performances of an integrated layered nanocomposite system, viz Li[NixMxLi1/3-xMn2/3-x]O2, where M is cobalt or chromium with a wide compositional range x from 0 to 0.33. Ultimately, it is aimed to arrive at the optimized compositions (x) of Co and Cr in the integrated nanocomposite that exhibit impressive electrochemical properties.

Methods

Synthesis

Lithium hydroxide monohydrate (98.0% to approximately 102.0%; Junsei Chemical Co., Ltd., Chuo-ku, Tokyo, Japan), manganese acetate tetrahydrate (97%; Yakuri Pure Chemicals Co., Ltd., Kyoto, Japan), nickel acetate tetrahydrate (98.0%, Junsei Chemical Co., Ltd.), Cobalt acetate tetrahydrate (98.5%, Junsei Chemical Co., Ltd.) and Chromium acetate (22% as Cr, Wako Pure Chemical Industries, Ltd., Chuo-ku, Osaka, Japan) were used as precursors for the solution synthetic method. The samples with different stoichiometric compositions in the layered Li[NixMxLi1/3-xMn2/3-x]O2 system where x = 0, 0.05, 0.1, 0.17, 0.24, and 0.33 were prepared by coprecipitation method. In brief, the transition metal acetate precursors and lithium hydroxide were dissolved separately in distilled water. The aqueous solution of lithium hydroxide was then slowly dripped into the transition metal solution to facilitate hydroxide coprecipitation at room temperature for 24 h. The precipitated solution was subsequently dried in an oven at 85°C to evaporate residual water, and the dried powders were ground well before heating at 600°C for 3 h to eliminate undesired organic materials that remained. The heated powders were ground completely and then fired at 900°C for 12 h for crystallization. The resultant powders were obtained after quenching the fired powders using two copper plates in air and subsequent grinding. The final products were obtained after washing with distilled water to remove unwanted impurities such as Li2CrO4 and subsequent vacuum drying at 120°C.

Structural and physical characterization

The crystalline nature of the obtained samples in the Li[NixMxLi1/3-xMn2/3-x]O2 system were characterized by X-ray diffraction [XRD] using a Shimadzu X-ray diffractometer (Shimadzu Corporation, Nakagyo-ku, Kyoto, Japan) with Ni-filtered Cu-Kα radiation (λ = 1.5406 Å) operating at 40 kV and 30 mA within the scanning range angle from 10° to 80° (2θ). Inductively coupled plasma atomic emission spectrometer [ICP-AES] analysis utilizing PerkinElmer OPTIMA 4300 DV (PerkinElmer, Waltham, MA, USA) was performed to confirm the compositions of the obtained materials. The particle morphologies and sizes were observed by field-emission scanning electron microscopy [FE-SEM] using the HITACHI S-4700 instrument (Hitachi High-Tech, Minato-ku, Tokyo, Japan). The sample surface areas were measured by the Brunauer Emmett and Teller [BET] method using a surface area analyzer (ASAP 2020, Micromeritics Instrument Co., Norcross, GA, USA).

Electrochemical characterization

The electrochemical properties of the cathodes fabricated from the samples in the Li[NixMxLi1/3-xMn2/3-x]O2 system were evaluated using the NAGANO battery tester system 2004H equipment (NAGANO KEIKI Co., LTD, Ohta-ku, Tokyo, Japan). The fabricated cathode consisted of 72 wt.% active materials, 10 wt.% conductive carbon (Ketjen black), and 18 wt.% polytetrafluoroethylene as binder. The pasted film was then pressed onto a stainless steel mesh with a 2-cm2 area and dried under vacuum at 120°C for 12 h. The electrolyte employed was a 1:1 (v/v) mixture of ethylene carbonate and dimethyl carbonate containing 1 M LiPF6. A 2032 coin-type cell which consists of the cathode and lithium metal anode separated by a polymer membrane was fabricated in an Ar-filled glove box and aged for 12 h. The cells assembled were tested with 0.1 mA/cm2 of current density in the voltage range from 2.0 to 4.8 V.

Results and discussion

The Li[NixCoxLi1/3-xMn2/3-x]O2 system

Figure Figure11 shows the XRD patterns of layered nanocomposite powders obtained by coprecipitation and belonging to the Li[NixCoxLi1/3-xMn2/3-x]O2 system. All diffraction peaks of the prepared samples were assigned to the expected reflections of trigonal (R3m¯) and monoclinic (C2/m) phases simultaneously, except for the sample with composition x = 0. Particularly, a magnified view of the scanning angles ranging from 2θ = 19° to 34° indicate peaks arising due to the super-lattice ordering of Li+ and Mn4+ occurring in the transition metal layers. Li2MnO3 can be represented as Li[Li1/3Mn2/3]O2, a layered phase possessing long-range ordering in the transition metal layers. Such a cation ordering can correspond to well-resolved characteristic peaks at specific angles in the XRD patterns. These peaks indicating long-range ordering are distinctly visible and sharper in pure Li2MnO3 (x = 0), when compared with the other samples in this system. As the XRD patterns of the samples with increasing concentrations of x are viewed progressively, the characteristic peaks corresponding to cation ordering undergo a significant variation in their intensities. In fact, the peaks which indicate the cation ordering in transition metal layer disappear gradually, as we observe the characteristic peaks of the samples with increasing concentrations of x in the magnified image. To confirm the stoichiometric composition of the synthesized materials, ICP-AES analysis was performed, and the results are summarized in Table Table1.1. The ICP results revealed that the observed stoichiometric composition for transition metals in all the samples matched well with the calculated values. Despite the fact that an excess 3 wt.% lithium precursor was used as starting material, the experimental lithium content in all samples was slightly lower than the corresponding theoretical values. This lower lithium content most probably resulted from the evaporation loss of lithium during heat treatment at elevated temperatures. The possibilities for such lithium losses during high temperature synthesis of layered electrodes have been reported [12,15].

Figure 1
XRD patterns of Li[NixCoxLi1/3-xMn2/3-x]O2 system synthesized by coprecipitation and magnified image in the 19° to 34°(2θ) region.
Table 1
The ICP data confirming the stoichiometries of the prepared Co-doped samples and the corresponding BET values.

The morphology and size distribution of the Li[NixCoxLi1/3-x-Mn2/3-x]O2 system were examined by FE-SEM and is shown in Figure Figure2.2. From the SEM results, it is observed that the average particle size of the parent Li2MnO3 (sample with x = 0) is in the range of 4 μm. On doping with Co , the particle sizes of the doped samples tend to decrease, which might probably be due to the comparatively smaller ionic radius of Co3+ (0.053 nm) than that of Ni2+ (0.07 nm). A similar trend observed by researchers has been reported for Cr-doping in layered lithium manganese oxides [16,17]. The surface areas pertaining to the prepared samples which were calculated using the BET method indicate that the obtained values for the doped samples exceed those of the parent sample by an order of magnitude, as evidenced from Table Table1.1. This trend clearly further indicates that Co-doped samples possess smaller particle sizes than the undoped sample. However, among the doped samples, the surface area values undergo a marginal increase in the same order of magnitude for higher dopant concentrations until the value experiences a slight decline for the highest doping concentration of x = 0.33. Nevertheless, further investigations are required to understand the correlation between particle size and concentration of Co dopant. As observed from the well-developed crystal facets of the particles, the tetrakai-dodecahedral morphology is confirmed in the doped samples. The particle sizes are observed to roughly vary between 200 and 500 nm. The absence of a noticeable variation in the obtained morphologies of the doped samples indicates that varying the concentration of Co doping hardly introduces significant changes in the particle morphologies.

Figure 2
FE-SEM images of Li[NixCoxLi1/3-xMn2/3-x]O2 system synthesized by coprecipitation.

The initial charge/discharge profiles for all the prepared electrodes in the Li[NixCoxLi1/3-xMn2/3-x]O2 system and their cycleabilities are shown in Figure Figure3.3. The charge capacities tend to increase until the intermediate concentrations of Co and the values tend to reach saturation for higher Co contents. However, a different trend follows for the obtained discharge capacities. As the Co content (x) in the nanocomposite increased, a distinct improvement in the discharge capacities was observed until x = 0.24; beyond which, a drop in the discharge capacity occurred. Hence, the coulombic efficiencies in the doped samples were apparently higher (> 70%) than those observed in the pure sample (66%) which suggests that the higher efficiencies are probably associated with Co doping. The smaller the particle size, the higher the electrode/electrolyte interfacial areas; hence, shorter are the Li-ion diffusion paths. The reduced ion migration pathways lead to effective ion diffusion and ultimately enhance material properties/performances. However, the significant initial irreversible capacities observed in the voltage profiles of such layered nanocomposites arise mainly from the oxygen loss occurring at extended charge cycling (> 4.5 V) [12,14]. A maximum initial discharge and charge capacities of 270 and 220 mAh/g were registered for the sample with the composition x = 0.24. The specific capacity drop beyond this particular composition is most probably associated with the particular compositional ratio of the nanocomposite. In fact, beyond this composition, the Li2MnO3 content decreases, as seen from the XRD result. The electrochemically inactive Li2MnO3 in conjunction with the appropriate LiMO2 composition enhances the electrochemical properties of the final nanocomposite though other factors such as particle size and distribution need to be considered. Although the highest charge and discharge capacities were observed for the sample with the composition x = 0.24, the values steadily declined after few initial cycles. However, the capacities of the sample with low Co content (x = 0.05 and 0.10) increased gradually and steadied under subsequent cycling. On cycling the electrodes for 35 cycles, the capacities maintained by the latter samples were far better than those of the former. For instance, the capacity of the sample with high Co content underwent a decline from the initial value of 214 mAh/g to a final value of 127.12 mAh/g after the first 35 cycles. In contrast, the sample with a lower concentration of Co (x = 0.10), which delivered an initial capacity of 108.12 mAh/g, registered a higher capacity of 189.46 mAh/g after 35 cycles, the value achieved being 49% higher than that attained by the former under the same electrochemical conditions. The gradual rise in the capacities in the sample with low Co content has been attributed to the activation of these electrodes on repeated cycling. These results led us to conclude that the sample with Co content (x) varying between 0.05 and 0.10 in the Li[NixCoxLi1/3-xMn2/3-x]O2 system displayed an optimized electrochemical performance compared to the other counterparts.

Figure 3
Electrochemical properties of Li[NixCoxLi1/3-xMn2/3-x]O2 system with initial charge and discharge profiles (a) and cycleabilities (b).

The Li[NixCrxLi1/3-xMn2/3-x]O2 system

The XRD profiles, ICP-AES results, SEM images, and electrochemical properties of Li[NixCrxLi1/3-xMn2/3-x]O2 system, where x = 0, 0.05, 0.1, 0.17, 0.24, and 0.33, were obtained to compare with the results obtained for the cobalt-containing nanocomposite system, viz Li[NixCoxLi1/3-xMn2/3-x]O2. The XRD patterns of the Cr-doped samples, depicted in Figure Figure4,4, follow a similar trend to those observed in the Co-doped system; hence, the explanation of the XRD results holds valid for the Cr-doped system as in the case of the former system. The obtained ICP data, summarized in Table Table2,2, confirm the stoichiometries, excepting the evaporation losses in the case of lithium. The FE-SEM images of the Cr-doped nanocomposites are shown in Figure Figure5.5. It appears that the doping of Cr leads to a slight reduction in the particle size, and the BET surface area values in Table Table22 tend to confirm the observation. However, on comparison of the SEM images of the Co-doped and Cr-doped layered composites in Figures Figures22 and and5,5, respectively, it is observed that the particle sizes of the Li[NixCrxLi1/3-xMn2/3-x]O2 system are larger, with diameters of 300 nm to 1 μm, than those of the Li[NixCoxLi1/3-xMn2/3-x]O2 system. This might probably be due to the apparently smaller ionic radius of Co3+ (0.053 nm) than of Cr3+ (0.061 nm), and this observation is in congruence with our earlier report on Co/Cr-doped layered nanocomposites [13]. The electrochemical properties in Figure Figure66 of the Cr-substituted nanocomposite system exhibited apparently lower performances compared with those in the Co-contained nanocomposite system. In the Li[NixCrxLi1/3-xMn2/3-x]O2 system, the highest initial discharge capacity of 155 mAh/g was observed for the sample with the Cr composition x = 0.17. However, on completion of the initial 35 cycles, a capacity retention of 71% was observed (120 mAh/g). Whereas the sample with a low Cr content (x = 0.05), which delivered a lower initial discharge capacity of 87.46 mAh/g, registered higher capacities for 10 consecutive cycles and stabilized thereafter at 150 mAh/g, the value being 33% much higher than that observed under similar electrochemical conditions for the sample with the highest initial discharge capacity (x = 0.17). This behavior is similar to the case observed for the samples in the Co-doped nanocomposite system. Further, the enhanced electrochemical abilities of the Co-doped system may probably be due to the smaller particle sizes achieved by the coprecipitation process.

Figure 4
XRD patterns of Li[NixCrxLi1/3-xMn2/3-x]O2 system synthesized by coprecipitation and magnified image in the 19° to 34°(2θ) region.
Table 2
The ICP data confirming the stoichiometries of the prepared Cr-doped samples and the corresponding BET values.
Figure 5
FE-SEM images of Li[NixCrxLi1/3-xMn2/3-x]O2 system synthesized by coprecipitation.
Figure 6
Electrochemical properties of Li[NixCrxLi1/3-xMn2/3-x]O2 system with initial charge and discharge profiles (a) and cycleabilities (b).

Conclusions

In summary, structurally integrated nanocomposite materials belonging to the system, Li[NixMxLi1/3-xMn2/3-x]O2 where M is Co or Cr, were synthesized by hydroxide coprecipitation method and subsequent quenching process. The XRD patterns of all the prepared nanocomposite samples were well indexed to the trigonal (R3m) structure and monoclinic (C2/m) phase. However, obtaining the target stoichiometric composition is not trivial due to the reactivity of lithium at elevated temperatures. The average particle size of the crystallites in the Li[NixMxLi1/3-xMn2/3-x]O2 system is dependent on whether the transition metal of M is Co or Cr. In the case of the Co-substituted system, particle sizes were much smaller than those in the Li[NixCrxLi1/3-xMn2/3-x]O2 system. Consequently, impressive electrochemical properties were attained since discharge capacities as high as 200 mAh/g and above were registered after the initial 10 cycles for the sample with x = 0.10 in the Li[NixCoxLi1/3-xMn2/3-x]O2 system. Further studies focused not only on the co-existence of R3m and C2/m, but also investigation on the local structure characterization will be required in detail using advanced analysis such as transmission electron microscopy and nuclear magnetic resonance.

Competing interests

The authors declare that they have no competing interests.

Authors' contributions

JKK directed the research. JG analyzed the results and wrote the paper. JS, HP, JWK, and KK participated in the characterization of samples and carried out experiments. VM contributed to the technical discussions. All the authors have read and approved the final manuscript.

Acknowledgements

This work was supported by the Korea Research Foundation grant (KRF-2007-313-D00950) and by the Basic Research Laboratories Program of National Research Foundation of Korea (NRF). In addition, this research was also supported by the Human Resources Development of Korea Institute of Energy Technology Evaluation and Planning (KETEP) with the grant funded by the Korean government's Ministry of Knowledge Economy (20114010203100).

References

  • Padhi AK, Nanjundaswamy KS, Goodenough JB. Phospho-olivines as positive-electrode materials for rechargeable lithium batteries. J Electrochem Soc. 1997;144:1188–1194. doi: 10.1149/1.1837571. [Cross Ref]
  • Croguennec L, Deniard P, Brec R. Electrochemical cyclability of orthorhombic LiMnO2. J Electrochem Soc. 1997;144:3323–3330. doi: 10.1149/1.1838013. [Cross Ref]
  • Davidson IJ, McMillan RS, Murray JJ. Rechargeable cathodes based on Li2CrxMn2-xO4. J Power Sources. 1995;54:205–208. doi: 10.1016/0378-7753(94)02067-D. [Cross Ref]
  • Jang YI, Huang B, Chiang YM, Sadoway DR. Stabilization of LiMnO2 in the a-NaFeO2 structure type by LiAlO2 addition. Electrochem Solid State Lett. 1998;1:13–16.
  • Thackeray MM, Johnson CS, Vaughey JT, Li N, Hackney SA. Advances in manganese-oxide 'composite' electrodes for lithium-ion batteries. J Mater Chem. 2005;15:2257–2267. doi: 10.1039/b417616m. [Cross Ref]
  • Feng L, Chang Y, Wu L, Lu T. Electrochemical behavior of spinel LiMn2O4 as positive electrode in rechargeable lithium cells. J Power Sources. 1996;63:149–152. doi: 10.1016/S0378-7753(96)02458-5. [Cross Ref]
  • Wakihara M. Recent developments in lithium ion batteries. Mater Sci Eng. 2001;33:109–134. doi: 10.1016/S0927-796X(01)00030-4. [Cross Ref]
  • Kang SH, Park SH, Johnson CS, Amine K. Effects of Li content on structure and properties of Li1+x(Ni0.5Mn0.5)1-xO2 (0 ≤ x ≤ 0.15) electrodes in lithium cells (1.0-4.8 V) J Electrochem Soc. 2007;154:A268–A274. doi: 10.1149/1.2436624. [Cross Ref]
  • Park SH, Kang SH, Belharouak I, Sun YK, Amine K. Physical and electrochemical properties of spherical Li1+x(Ni1/3Co1/3Mn1/3)1-xO2 cathode materials. J Power Sources. 2008;177:177–183. doi: 10.1016/j.jpowsour.2007.10.062. [Cross Ref]
  • Kim JM, Kumagai N, Chung HT. Improved electrochemical properties and structural stability of overlithiated Li1+x(Ni1/3Co1/3Mn1/3)1-xO2 prepared by spray-drying method. Electrochem Solid-State Lett. 2006;9:A494–A498. doi: 10.1149/1.2336988. [Cross Ref]
  • Todorov YM, Numata K. Effects of the Li:(Mn + Co + Ni) molar ratio on the electrochemical properties of LiMn1/3Co1/3Ni1/3O2 cathode material. Electrochim Acta. 2004;50:495–499. doi: 10.1016/j.electacta.2004.05.050. [Cross Ref]
  • Deng Q, Manthiram A. Influence of cationic substitutions on the oxygen loss and reversible capacity of lithium-rich layered oxide cathodes. J Phys Chem C. 2011;115:7097–7103. doi: 10.1021/jp200375d. [Cross Ref]
  • Kim D, Gim J, Lim J, Park S, Kim J. Synthesis of xLi2MnO3 (1-x)LiMO2 (M = Cr, Mn, Co, Ni) nanocomposites and their electrochemical properties. Mater Res Bull. 2010;45:252–255. doi: 10.1016/j.materresbull.2009.12.027. [Cross Ref]
  • Arunkumar TA, Wu Y, Manthiram A. Factors influencing the irreversible oxygen loss and reversible capacity in layered Li[Li1/3Mn2/3]O2-Li[M]O2 (M = Mn0.5-yNi0.5-yCo2yand Ni1-yCoy) solid solutions. Chem Mater. 2007;19:3067–3073. doi: 10.1021/cm070389q. [Cross Ref]
  • Johnson CS, Li N, Lefief C, Vaughey JT, Thackeray MM. Synthesis, characterization and electrochemistry of Lithium battery electrodes: (1-x) LiMn0.333Ni0.333Co0.333O2 (0 ≤ x ≤ 0.7) Chem Mater. 2008;20:6095–6106. doi: 10.1021/cm801245r. [Cross Ref]
  • Jiao LF, Zhang M, Yuan HT, Zhao M, Guo J, Wang W, Zhou XD, Wang YM. Effect of Cr doping on the structural, electrochemical properties of Li[Li0.2Ni0.2-x/2Mn0.6-x/2Crx]O2 (x = 0, 0.02, 0.04, 0.06, 0.08) as cathode materials for lithium secondary batteries. J Power Sources. 2007;167:178–184. doi: 10.1016/j.jpowsour.2007.01.070. [Cross Ref]
  • Yi TF, Li Cy, Zhu YR, Shu J, Zhu RS. Comparison of structure and electrochemical properties for 5 V LiNi0.5Mn1.5O4 and LiNi0.4Cr0.2Mn1.4O4 cathode materials. J Solid State Electrochem. 2009;13:913–919. doi: 10.1007/s10008-008-0628-x. [Cross Ref]

Articles from Nanoscale Research Letters are provided here courtesy of Springer
PubReader format: click here to try

Formats:

Related citations in PubMed

See reviews...See all...

Cited by other articles in PMC

See all...

Links

  • MedGen
    MedGen
    Related information in MedGen
  • Nucleotide
    Nucleotide
    Published Nucleotide sequences
  • PubMed
    PubMed
    PubMed citations for these articles