electrochemical activities in li2mno3

Journal of The Electrochemical Society, 156 6 A417-A424 20090013-4651/2009/156 6 /A417/8/$25.00 The Electrochemical Society

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Electrochemical Activities in Li2MnO3Denis Y. W. Yu,*,z Katsunori Yanagida,* Yoshio Kato, and Hiroshi Nakamura*Mobile Energy Company, SANYO Electric Company, Limited, Kobe, Hyogo 651-2242, Japan Li2MnO3 is shown to be electrochemically active, with a maximum charge capacity of 350 mAh/g and a discharge capacity of 260 mAh/g at 25C. A total of 1 mole of Li can be extracted from Li Li1/3Mn2/3 O2, and the rst cycle efciency is 66% regardless of state of charge. Larger charge-discharge capacity is obtained from materials with smaller particle size and larger amount of stacking faults. Composition and structural analyses indicate that Li are removed from both the Li and transitional metal layers of the material during charging. Results from X-ray-absorption ne-structure measurements suggest that the valence of Mn remains at 4+ during charging but is reduced during discharging. Charging is accompanied by gas generation: at 25C, oxygen is the main gas detected, and the total amount accounts for 1/8 mole of O2 generation from Li Li1/3Mn2/3 O2. At an elevated temperature, amount of CO2 increases due to electrolyte decomposition. Li2MnO3 shows poor cycle performance, which is attributed to phase transformation and low charge-discharge efciency during cycling. Low rst-cycle efciency, gas generation, and poor cycle performance limit the usage of Li2MnO3 in practical batteries. 2009 The Electrochemical Society. DOI: 10.1149/1.3110803 All rights reserved. Manuscript submitted November 21, 2008; revised manuscript received February 4, 2009. Published April 3, 2009.

The study of Mn-based Li-excess layered cathode materials with a formula Li LixMnyMz O2 where M represents one or more transition metal elements has been gaining popularity because these materials can give a discharge capacity 200 mAh/g,1-16 much higher than practical discharge capacity of common cathode materials, such as LiCoO2 and LiMn2O4. Successful application of these materials can potentially increase energy density of Li-ion batteries. One challenge that researchers face in the study of Li LixMnyMz O2 materials is that there is almost an endless combination of systems, depending on the additional element or elements M and the ratio of cations in the layered material. A change in composition is sure to affect the electrochemical performance of the cathode material. In addition, modications such as acid treatment and surface coating can further change material behavior.4,8,17-20 It is therefore difcult to compare results from different publications due to differences in material composition and processing techniques. Though, all of the Li LixMnyMz O2 materials share a common feature: a plateau at 4.5 V vs Li/Li+ during initial charging which is similar to the behavior of Li2MnO3. We therefore think it would be benecial to reinvestigate the fundamental mechanism of Li2MnO3 to help further understanding of the properties of Mn-based Li-excess materials. Electrochemical properties of Li2MnO3 and acid-leached Li2MnO3 were previously reported in the literature.4,5,8,21-30 However, the described discharge capacity varies from publication to publication, with values ranging from a few to 200 mAh/g. The inconsistency in results is probably due to differences in synthesis condition and test condition.25,29,30 In theory, Li2MnO3 has a capacity of 458 mAh/g with respect to the initial mass of the sample if all Li can be extracted. In this study, we investigated the reasons for the limited capacity observed in experiments and studied the effect of physical parameters of Li2MnO3 on the discharge capacity of the material by methods such as X-ray diffractometry XRD and scanning electron microscopy SEM . It was originally thought that Li2MnO3 is electrochemically inactive because Mn has a valence of 4+, and it is unlikely that Mn will go to higher valence. Many researchers attributed the electrochemical activity of Li2MnO3 to the removal of Li2O from the active material.2,4,8,25-28 However, there are few discussions on what is the status of the oxygen atoms after charge-discharge. There is also a lack of quantitative analysis on the correlation between the amount of oxygen lost from the active material and the observed capacities, because direct measurement of oxygen stoichiometry is difcult. Armstrong et al.31 observed O2 gas generation from the initial

charging of Li Li0.2Ni0.2Mn0.6 O2 material using an in situ differential electrochemical mass spectroscopy. Though, the amount of oxygen gas cannot be determined by their method. In this study, we used a quantitative approach aiming to understand the fundamental mechanism of Li2MnO3, by tracking the amount of Li in the active material by inductively coupled plasma ICP atomic emission spectroscopy and the amount of oxygen gas generated by gas chromatography GC . The change in valence of Mn is studied qualitatively by X-ray absorption ne structure spectroscopy XAFS . The results are presented in this paper. In addition, the cycle performance of the active material and practical issues of Li2MnO3 will be discussed. Throughout the paper, the formula Li2MnO3 is used interchangeably with Li Li1/3Mn2/3 O2, a notation that gives more information about the structure of the material.

Experimental Li2MnO3 powders were synthesized by a solid-state reaction with LiOH H2O and MnCO3 nH2O n 0.5 as precursors. The starting materials were thoroughly mixed by milling in acetone for 1 h and then dried at 60C. The resulting precursors were then annealed at temperatures between 400 and 1000C in air. Structure of the powders was studied by XRD using a Cu K source 50 kV, 300 mA . Morphology and particle size information were obtained from SEM. The surface area of the materials was determined using an AUTOSORB-1 equipment by Quantachrome: 0.5 g of material was rst dried at 150C for 1.5 h and then the surface area was determined by a ve-point BrunauerEmmettTeller BET method with nitrogen as the adsorbate gas. ICP atomic emission spectroscopy was used to study the amount of Li and Mn in the material before and after charge-discharge. For electrochemical evaluation, Li2MnO3 active material was mixed with acetylene black and polyvinyl diuoride PVdF in 1-methyl-2-pyrrolidone NMP with a weight ratio of 80:10:10 to form a slurry. The slurry was then coated onto a roughened aluminum current collector using a doctor blade. The electrodes were rolled with a calender press to a packing density of about 2.22.3 g/cm3, with a typical thickness of 2535 m. These electrodes were assembled in a glove box with Ar atmosphere using Li metal as the counter and reference electrodes with a layer of separator to make a at laminated test cell. 1 M LiPF6 in ethylene carbonate/diethylcarbonate EC/DEC = 3:7 by volume was the electrolyte used in the experiments. The electrodes were sandwiched between glass plates to maintain contact of the electrodes, and the cells were typically charged and discharged at room temperature 25C between 4.8 and 2 V vs Li/Li+ with a constant current rate

* Electrochemical Society Active Member.z

E-mail: [email protected]

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Journal of The Electrochemical Society, 156 6 A417-A424 2009

Table I. Electrochemical properties of Li2MnO3 synthesized at different temperatures. Annealing conditions C h 400 48 425 10 600 10 750 10 800 10 850 10 900 10 1000 10a

Charge capacity mAh/g 367.0 355.0 342.0 294.8 290.0 206.7 63.6 28.4

Discharge capacity mAh/g 258.7 251.8 232.4 197.2 191.6 135.4 43.8 22.7

Charge efciency % 70.5 70.9 68.0 66.9 66.1 65.5 68.9 79.9

fwhm 18.7 peak 001 plane 0.434 0.368 0.302 0.252 0.221 0.180 0.132 0.123

Avg. particle sizea nm 70 70 90 110 130 140 390 650

BET surface area m2 /g 20.2 18.0 15.9 10.7 9.0 6.6 2.2 1.5

Measured from SEM images.

of 10 mA/g, unless stated otherwise. Charge-discharge capacities were calculated with respect to the mass of Li2MnO3 before charging. To study gas generation from the sample, an in situ measurement was performed to monitor the change in cell thickness during charge-discharge. The cells were disassembled after charging, and the composition and total volume of the generated gas from the cells were measured by GC. Structural information of the material at different state of charges was further investigated by an ex situ XAFS with the MnK edge in transition mode using the BL08 beamline at SPring-8 in Hyogo Prefecture, Japan. X-ray absorption near-edge spectroscopy XANES was used to monitor the electronic structure of Mn and extended X-ray absorption ne-structure EXAFS was used to monitor the interaction of Mn with surrounding atoms. To interpret the XAFS results of Li2MnO3, XAFS of LiNi1/3Co1/3Mn1/3O2 and LiMn2O4 were taken as references. Average particle size and BET surface area of the reference materials were 10 m and 2.0 m2 /g for LiNi1/3Co1/3Mn1/3O2 and 13 m and 0.35 m2 /g for LiMn2O4, respectively. Results and Discussion Effect of synthesis conditions on electrochemical behavior of Li2MnO3. Annealing temperature was varied from 400 to 1000C to study the effect of synthesis condition on the electrochemical performance of Li2MnO3 see Table I . The materials were made into test cells, and their electrochemical properties were tested. First cycle charge-discharge proles with a rate of 10 mA/g at 25C of several Li2MnO3 samples are shown in Fig. 1. An initial charge plateau at 4.5 V vs Li/Li+ is observed for all samples. Reducing the synthesis temperature lowers the potential of the charge plateau and leads to higher charge and discharge capacities. A maximum charge capacity of about 350370 mAh/g is obtained, correspond5 4.5 Potential (V vs. Li/Li+) 4 3.5 3 2.5 2 1.5 0 100 200 Capacity (mAh/g) 300 400 10mA/g 1000C 900C 850C 800C 600C 400C first cycle

ing to the removal of 1 mole of Li out of Li Li1/3Mn2/3 O2. In return, a maximum discharge capacity of about 250260 mAh/g is obtained. First cycle efciency FCE is 66% for most of the samples, showing a reinsertion of only 2/3 of the extracted Li. The discharge capacity is rst of all limited by the charge capacity. Thus, a larger discharge capacity is obtained from a sample with larger charge capacity. In addition, the low FCE suggests that the discharge capacity i.e., the reinsertion of Li is limited by the structure of the material. This will be further discussed in a later section together with other analytical results. To understand how the change in synthesis condition leads to a change in electrochemical behavior of Li2MnO3, we rst studied the structure of the materials by XRD. XRD proles of the different samples are shown in Fig. 2. All samples show a layered structure with a c2/m space group, with alternating Li layers and transitional metal TM layers separated by oxygen layers. The superlattice peaks between 20 and 30 in the XRD prole with a Cu K source , which are not observed in other layered materials, are due to the ordering of Li/Mn in the TM layers. Figure 2 shows that below a synthesis temperature of 600C, only a single broad peak at 20.9 is observed. This broadening of the superlattice peak is attributed to an increase in the amount of stacking faults shifting of the TM layers perpendicular to the layered 001 direction with a lower synthesis temperature.32 The role of the stacking fault on the electrochemical properties of the active material is unclear. From thermodynamics, a material without defects has the lowest energy state. Introducing stacking faults and other defects in the material increases the energy state of the material, which may lower the activation barrier for Li diffusion and allow Li to be extracted at a lower potential. Further studies on the effect of defects on electrochemical performance are in progress. The effect of synthesis temperature on the particle size and morphology was studied by SEM. Figure 3 shows the SEM pictures of

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Figure 1. Color online First cycle charge-discharge proles of Li2MnO3 synthesized at different temperatures.

Figure 2. Color online XRD proles of Li2MnO3 synthesized at different temperatures.


Journal of The Electrochemical Society, 156 6 A417-A424 20092.0 Normalized intensity (a.u.) 1.8 1.6 1.4 1.2 1.0 0.8 0.6 0.4 0.2 0.0 6535 1s 3d 6540 6545 6550 Energy (eV) 6555 MnO6 connectivity Li2MnO3 450C 600C 750C 900C LiNi1/3Co1/3Mn1/3O2

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Figure 5. Color online XANES proles of Mn K-edge of Li2MnO3 synthesized at 450, 600, 750, and 900C, all four proles overlap on top of each other. XANES prole of LiNi1/3Co1/3Mn1/3O2 is also shown for comparison.

Figure 3. Color online SEM images of Li2MnO3 synthesized at different temperatures.

the sample annealed at different temperatures. Average particle size of the samples was determined by measuring the dimension of the particles from the SEM images, and the results are shown in Table I. Samples synthesized at a lower temperature have smaller particles size: Li2MnO3 synthesized at 400C has a particle size as small as 70 nm. Increasing temperature leads to larger particles. Signicant grain growth is observed for samples made at a temperature of 850C, particle size is 650 nm when the sample is annealed at 1000C. This is consistent with the decrease in the full width halfmaximum fwhm of the XRD peaks with increasing synthesis temperature see Table I . Figure 4 shows the relationship between discharge capacity and particle size, showing larger capacity from Li2MnO3 nanoparticles. We attribute this to a smaller diffusion path for smaller particles, which allows the material to be charged to a higher capacity. Another consequence of reducing the annealing temperature is an increase in surface area. The BET surface area of the Li2MnO3 samples was measured and the results are shown in Table I. An inverse relationship between surface area and particle size is obtained, the smaller the particle size, the larger the surface area. A simple geometrical calculation shows that surface area per unit mass A/m is related to the diameter of the particle d by A/m = 6/ d for spherical particles, where is the density of the material. Our result is consistent with the inverse proportionality between A/m and d, suggesting that the increase in surface area of our Li2MnO3

sample synthesized at a reduced temperature is a direct result of the decrease in particle size, and not from other contributions, such as surface roughening. The effect of annealing temperature on the local environment of Mn in as-made Li2MnO3 was studied by XAFS. Figure 5 shows the results of Mn K-edge XANES of Li2MnO3 samples synthesized at 450, 600, 750, and 900C. The double-peak near 6540 eV is attributed to a 1s-to-3d transition, which is expected to be weak for an octahedral coordination of Mn.33,34 The shoulder at 6548 eV is associated with the connectivity of the MnO6 octahedral.35 No signicant change in the XANES Mn K-edge is observed with annealing temperature. Similarly, EXAFS, which gives information about the interaction of Mn with neighboring atoms, does not depend on synthesis condition EXAFS of one of the pristine samples is shown in Fig. 12 . These results suggest that annealing temperature does not change the local environment of Mn. In summary, electrochemical activity of Li2MnO3 is enhanced by the reduction of particle size of the material and the increase in the amount of stacking faults in the structure. Effect of particle size is expected to be dominating since Li2MnO3 with poor crystallinity but only gives discharge capacity 100 mAh/g has been reported elsewhere.29,30 Though the effect of stacking faults cannot be ruled out because it was not possible to make small particles without stacking faults with the current synthesis method. Li2MnO3 sample synthesized at 425C, which can give a charge and discharge capacity of 350 and 250 mAh/g at 25C, respectively, is used in subsequent studies to investigate the charge-discharge mechanism of Li2MnO3. Tracking Li atoms and structural change during charge-discharge of Li2MnO3 at 25C. Li2MnO3 cells were charged and discharged to different capacities, and the cells were disassembled and their compositions were determined by ICP to correlate the measured capacities from electrochemical tests with the amount of Li in the material. Test results are shown in Table II. ICP results show that pristine samples have a Li/Mn ratio of 2:1, according to the stoichiometry of our starting precursors. By assuming that the amount of Mn in the active material remains constant after charge and discharge, we can calculate the amount of Li in the samples from ICP measurements. Figure 6 shows the relationship between measured capacity cumulative and the amount of Li in LixMn2/3O2. The dotted line in Fig. 6 represents the theoretical capacity at a given Li content if all extracted Li contribute to the capacity. When the electrochemical tests were performed at 25C, measured capacities coincide with the Li contents in the material according to calculation. This directly shows that the electrochemical activity of Li2MnO3 is accompanied by Li extraction/insertion. When charging was performed at 60C, the measured capacity is 50 mAh/g larger than

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Figure 4. Color online Relationship between particle size, BET surface area, and discharge capacity of Li2MnO3 samples.


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Table II. Measured charge-discharge capacities and LiMn ratios. Test temperature C 25 25 25 25 25 25 25 60 Charge capacity mAh/g 50.0 99.7 150.0 248.8 337.5 336.2 335.4 429.2 Discharge capacity mAh/g 125.0 210.0 Cumulative capacitya mAh/g 0 50.0 99.7 150.0 248.8 337.5 211.2 125.4 429.2 x in LixMn2/3O2 calculated 1.33 1.16 1.10 0.88 0.64 0.31 0.70 0.98 0.27

Samples Pristine A1 A2 A3 A4 A5 A6 A7 B1a

Li/Mn ICP results 2.00 1.75 1.66 1.32 0.95 0.47 1.05 1.47 0.40

Cumulative capacity = charge capacity discharge capacity.

that corresponding to Li extraction. Other mechanisms, such as electrolyte decomposition, contribute to the excess capacity at an elevated temperature. To further study the electrochemical behavior of Li2MnO3, the electrodes were charged to different capacities and then discharged. Figure 7 shows the charge and discharge curves of electrodes that are initially charged to 0, 50, 150, 250, and 350 mAh/g fully charged cutoff capacities during charging are marked by X . An electrode that is initially discharged without charging gives a capacity of 20 mAh/g, suggesting that the as-made material can accommodate some amount of Li. The amount of Li accommodated from initial discharge decreases with synthesis temperature, with a capacity of 2 mAh/g for Li2MnO3 synthesized at 900C. We suspect the initial discharge capacity originates from either a surface500

Cummulative capacity (mAh/g)

450 400 350 300 250 200 150 100 50 0 0 0.2 discharge charge

electrolyte decompositio

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25C charge 25C discharge

theoretical capacity of Li[Li1/3Mn2/3]O2 pristine sample x=4/3

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Figure 6. Color online Plot of cumulative capacity with respect to Li content in LixMn2/3O2 dotted line represents the theoretical capacity at a given Li content .5 4.5 Potential (V vs. Li/Li+) 4 3.5 3 2.5 2 1.5 0 0 50 mAh/g mAh/g 50 100 150 mAh/g 150 250 mAh/g 200 350 mAh/g 250 300 charged to 350 400 X X X X 1st cycle 10mA/g

effect, such as the presence of additional active sites on the large surface, or from accommodation of Li in the grain boundary or defects such as stacking faults. When the charge capacity is increased, the discharge capacity also increases accordingly. At 25C, a maximum charge capacity of 350 mAh/g is obtained, which corresponds to the extraction of 1 mole of Li out of Li Li1/3Mn2/3 O2. Not all of the Li can be extracted from the active material. During discharge, a maximum capacity of 250 mAh/g is obtained, in which 229 mAh/g can be accounted for by the 4+/3+ transition of Mn. The remaining 21 mAh/g most likely corresponds to the capacity from Li accommodated on surface or defect sites, same as that obtained when the material is initially discharged. The discharge capacities of Li2MnO3 obtained from different states of charge during rst cycle is summarized in Fig. 8; all data points lie on a straight line with a slope close to 0.66. This indicates that the charge-discharge mechanism of Li2MnO3 is the same throughout the entire rst cycle, regardless of the state of charge. For every three Li extracted out of the lattice, only two can be reinserted back into the lattice. This suggests that there is a structural limitation on the amount of Li reinserted, instead of a chemical limitation from the redox reaction of Mn. In addition, Li extraction is most likely not uniform throughout the particles, resulting in reacted and not reacted regions, similar to a two-phase transformation. The plateau at 4.5 V vs Li/Li+ observed during charging supports this hypothesis. The change in structure of Li2MnO3 during charging and discharging was monitored by XRD. A summary of the XRD proles at different charged states is shown in Fig. 9. Upon charging, the overall intensity of XRD peaks decreases. The peak at 18.7, which correspond to the 001 plane, is shifted to a larger angle, indicating

3001st discharge capacity (mAh/g)

slope = 1 250 200 150 100 Li2MnO3 50 0 0 50 100 150 200 250 300 350 400 1st charge capacity (mAh/g) slope = 0.66

Capacity (mAh/g)

Figure 7. Color online Charge-discharge curves of Li2MnO3 by limiting the state of charge to 0, 50, 150, 250, and 350 mAh/g marked by X .

Figure 8. Color online First cycle discharge capacity of Li2MnO3 by limiting the charge capacity.


Journal of The Electrochemical Society, 156 6 A417-A424 20092.0 Normalized intensity (a.u.) 1.8 1.6 1.4 1.2 1.0 0.8 0.6 0.4 0.2 0.0 6543 6548 6553 Energy (eV) 6558 charge discharge pristine charged * discharged pristine LiNi1/3Co1/3Mn1/3O2

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Figure 9. Color online XRD proles of Li2MnO3 at different stages of charge. C1, C2, C3, and C4 correspond to a state of charge of 0, 150, 250, and 350 mAh/g, respectively. D1 and D2 correspond to a discharge of 125 and 210 mAh/g from a fully charged electrode.

Figure 10. Color online XANES proles of Mn K-edge LiNi1/3Co1/3Mn1/3O2 during charging to 4.3 V and discharging.

in

a decrease in lattice spacing between the layers with Li extraction. In addition, the intensity of superlattice peak between 20 and 25 is reduced gradually upon charging, indicating that the Li/Mn ordering in the transition metal layer is disrupted. This suggests that Li is extracted not only from the Li layer but also from the TM layer during charging. Because the charge mechanism is thought to be the same throughout the charging process, as shown in Fig. 8, we suspect Li are extracted from both Li layer and TM layer at the same time. At a fully charged state, almost all of Li atoms in the TM layer are removed, as the superlattice can hardly be seen. During discharging, there is a general shift for all major peaks to smaller angles, indicating an increase in lattice constants with Li insertion. The fully discharged state has a different XRD prole than that of the pristine sample: e.g., 001 peak of the fully discharged state is at a smaller angle and only one single peak is observed at 65. These results suggest a change in lattice structure after discharge, with a XRD prole similar to a spinel structure. Intensity of the superlattice peak remains small after discharge. Because only 2/3 of the extracted Li can be reinserted, we suspect the atoms reenter the Li layer, leaving Li vacancies in the TM layer. Status of Mn during charge-discharge. XAFS measurement was carried out to study the change in local environment of Mn during charging and discharging. LiNi1/3Co1/3Mn1/3O2 is used as a reference to help interpret the XANES prole of Li2MnO3. The reason for using LiNi1/3Co1/3Mn1/3O2 as a reference is that Li2MnO3 and LiNi1/3Co1/3Mn1/3O2 shows similar Mn K-edge XANES proles because both materials have a layered structure with Mn in an octahedral coordination as shown in Fig. 5 . After charge-discharge, the cells were disassembled and the cathode materials were removed from the Al collector for XAFS measurements. Figure 10 shows the change in XANES prole of the reference LiNi1/3Co1/3Mn1/3O2 material after charge and discharge. When charged to 4.3 V, disappearance of the shoulder at 6548 eV and the shift in the peak top to higher energy are attributed to the change in the local environment of Mn from Li extraction, with the valence of Mn remaining 4+.34,36 The change in the shape and position of the Mn XANES prole is reversible upon discharge. Quantitative analysis of the XANES prole is difcult because of the shape change during charge-discharge. An absorption intensity of 0.4 is marked in Fig. 10 as a qualitative guide for the eye to show the shift or the lack of shift of the proles. Figure 11 shows the corresponding XANES prole of Li2MnO3. During charging, a disappearance of the shoulder around 6548 eV and a gradual shift to higher energy of the peak top, similar to that of LiNi1/3Co1/3Mn1/3O2, are also observed. The edge position at = 0.4 hardly moves. These results suggest that the effect of charging of Li2MnO3 on the local environment of Mn is similar to that of

LiNi1/3Co1/3Mn1/3O2 i.e., that the valence of Mn remains 4+ . After discharge, as opposed to LiNi1/3Co1/3Mn1/3O2, the XANES prole of Li2MnO3 does not return to the original position. The overall edge both the peak top and the edge position at = 0.4 is shifted to a lower energy, indicating a decrease in valance of Mn during discharge. Shape of the discharged prole is similar to that of LiMn2O4, as opposed to Li2MnO3. At this point, further quantitative investigation on the change of valence of Mn is needed to further understand the charge-discharge mechanism. In addition, in situ XAFS measurements should be conducted to minimize reaction between the environment and the charged and discharged electrodes. EXAFS proles of Li2MnO3 show that charging is accompanied with a reduction of both Mn-O and MnMn Fourier transformation FT peaks see Fig. 12 and this reduction in FT is also not reversible upon discharge. We attributed the results to a distortion around the Mn atoms associated with the removal of Li from the Li and TM layers and the reduction of coordination number due to removal of oxygen from the lattice. Attempts to model the EXAFS results by simulations codes, such as FEFF, are in progress to clarify the origin of the large change. Oxygen evolution during charge-discharge. XAFS results suggest that Mn valence remains 4+ during the charging of Li Li1/3Mn2/3 O2. But ICP results show that Li atoms are removed from the active material. If charge compensation is accompanied by oxygen removal, as suggested by various researchers,2,4,8,25-28 the extraction of one mole of Li from Li Li1/3Mn2/3 O2 corresponds to a change in oxygen stoichiometry from 2 to 1.5. In this study, we investigated how much of the change can be explained by gas generation.

2.0 Normalized intensity (a.u.) 1.8 1.6 1.4 1.2 1.0 0.8 0.6 0.4 0.2 0.0 6543 6548 discharge charge pristine charged * discharged LiMn2O4

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Figure 11. Color online XANES proles of Mn K-edge in Li2MnO3 during charging to 4.8 V and discharging.


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Figure 12. Color online EXAFS proles of Mn K-edge FT of Li2MnO3 during charging and discharging.

Figure 14. Color online Volume of gases collected from Li2MnO3 cells with 1 M LiPF6 in EC/DEC = 3:7 charged at 25, 45, and 60C.

First, a simple in situ test to monitor the change in cell thickness of a at laminated Li2MnO3 cell during charge-discharge was performed. Figure 13 shows the variation of cell thickness and applied current with time. The cell was initially charged at a rate of 30, 20, and 10 mA/g with intermittent rest. Afterward, the not-yet-fullycharged cell was discharged at 20 mA/g for 2 h and then recharged again for 4 h. During initial charging, thickness of the test cell increases with charging and remains unchanged during rest. The larger the applied current, the larger is the rate of thickness change i.e., rate of gas generation see Fig. 13 . Thus, gas generation is an integral part of the charging process of Li2MnO3. Gas generation is only observed during the initial charge of the active material. During discharge, thickness does not change. Upon recharging, no change in thickness is observed for the rst 2 h which corresponds to the removal of Li that was inserted in the previous discharge step . After 2 h, cell thickness increases again from the charging of the not reacted Li2MnO3. This supports the hypothesis that Li is not extracted uniformly throughout the particles during rst charge, as suggested from the charge efciency results in Fig. 8. To determine the type of gases and the total volume generated, cells were charged to a capacity of 150, 250, and 350 mAh/g at 25C and the gas was collected and analyzed by GC. The results are shown in Fig. 14 and summarized in Table III. H2, O2, CO, and CO2 are detected within the collected gas. The amounts of H2, CO, and

CO2 remain almost the same regardless of charge capacity, where as the amount of O2 increases with charge capacity. This conrms that oxygen gas is generated during charging of Li2MnO3. About 44 mL of gas per active-material mass is detected by GC when the electrode is charged to a capacity of 350 mAh/g equivalent to the evolution of 1/8 mole of O2 gas during the removal of one mole of Li from Li Li1/3Mn2/3 O2 . This corresponds to a change in oxygen stoichiometry from 2 to 1.75. Our result shows that the amount of oxygen gas can account for half of the charge compensation. The remaining oxygen atoms, if they are removed from the active material, may have reacted with electrolyte or formed Li2O at the anode and are therefore not accounted for in this study. A certain amount of proton exchange may have also occurred during charging, resulting in a smaller change in oxygen stoichiometry. A better tracing of oxygen and hydrogen atoms in the system is needed to clarify the full process. Effect of test temperature on charge mechanism of Li2MnO3. Li2MnO3 cells were charged to 350 mA/g at 25, 45, and 60C and the composition of the resulting gas was determined by GC to study the effect of test temperature on charge mechanism. The results are shown in Fig. 14 and summarized in Table III. At 25C, the main gas after charging is O2. With increasing test temperature, a signicant reduction in the amount of O2 and an increase in the amount of CO2 are observed. At 60C, a small amount of CH4 is also detected, but the signal overlapped with the O2 signal and therefore cannot be isolated. CO2 generation is associated with electrolyte decomposition, and therefore, the test results suggest that there is a change in charge mechanism of Li2MnO3 with temperature, from an oxygenloss process to the decomposition of electrolyte at a higher temperature. The change in mechanism is also reected in the material structure after charging. Li2MnO3 active materials were collected after charging at 25 and 60C to 350 mAh/g and examined by XRD, and the proles are shown in Fig. 15. Li2MnO3 charged at 25C shows a slight shift in the main peak from 18.68 18.80 the 001 plane . This shift corresponds to the shrinking of the lattice plane distance after Li is extracted from the layer. Material charged at 60C shows a larger shift of the main peak from 18.68 19.02 together with the growth of a peak at 38.3 marked by x in Fig. 15 . These features are characteristics of a P3 structure associated with hydrogen bonding between adjacent oxide layers,25,26 originated from the exchange of Li+ and H+ ions in the active material, that are also seen after acid treatment of Li2MnO3.4,8,37 The protons are likely to be generated from electrolyte decomposition. Note that the total amount of gas detected from the charged cell is smaller at a higher test temperature see Table III . This is consistent with electrolyte decomposition and proton exchange because the interchange of H+ and Li+ does not involve oxygen loss, and a larger portion of the gas is absorbed in the electrolyte since the solubility of CO2 is higher than that of O2.38,39

rest Current (mA/g) 30 20 10 0 -10 -20 0.8 0.6 0.4 0.2 0 0 2 slope =0.240

rest

rest

rest

rest

Thickness change (mm)

2hrs

2hrs

slope =0.080 slope =0.145 4 6 8 Time (hour) 10 12

slope =0.145

14

Figure 13. Color online Change in Li2MnO3 cell thickness with charge and discharge.



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Table III. Volume of detected gas per active material mass from charged Li2MnO3 cells at 25, 45, and 60C (bracketed values refer to the percentage). Charge temperature Charge capacity Total detected volume mL/g H2 O2 CO CO2a

25C 150 mAh/g 16.3 1.2 12.3 0.8 2.0 7.2% 75.6% 4.8% 12.4% 250 mAh/g 30.5 1.4 26.4 0.8 2.0 4.5% 86.5% 2.6% 6.4% 350 mAh/g 44.2 0.7 39.8 0.9 2.9 1.5% 90.0% 2.0% 6.5%

45C 350 mAh/g 41.3 1.4 28.2 1.5 10.1 3.4% 68.4% 3.7% 24.4%

60Ca 350 mAh/g 22.7 1.3 2.6 3.3 15.4 5.8% 11.3% 14.7% 67.8%

Small amount of CH4 is measured at 60C but the signal overlaps with O2 signal from GC.

Our results show that oxygen loss is the dominating process at 25C and electrolyte decomposition is more prominent at a higher temperature, conrming the results of Robertson and Bruce.25 Both mechanisms occurs at a similar potential of 4.54.6 V vs Li/Li+, and therefore, a small change in test temperature can tip the balance in favor of one mechanism over another. We suspect the contribution from electrolyte decomposition will be reduced if a more oxidationresistant electrolyte is used in the cell and further tests are being done to verify this. Cycle performance of Li2MnO3 with different states of charge. Li2MnO3 electrodes were tested with different state of charges xed by charge capacity , and the cycle performance was monitored see Fig. 16 . Electrodes charged to 4.8 V vs Li/Li+ or with a charge cutoff of 250 mAh/g show poor cycle performance, where the capacity reduces to below 100 mAh/g after 10 cycles. By reducing the state of charge to 150 mAh/g, the cycle life can be prolonged, but the discharge capacity eventually decays after 15 cycles. The cycle efciency ratio of discharge and charge capacities is 90% when the electrode is charged to 150 mAh/g. This suggests that Li2MnO3 keeps on losing Li with cycling and eventually runs out of Li that leads to a capacity fade. Cycle performance can be improved by reducing the utilization of the electrode. For example, an electrode with a charge cutoff of 50 mAh/g shows good cycle performance with a cycle efciency of close to 100%. However, this is not a practical solution to improve cycle performance because we end up sacricing the capacity. The charge-discharge curves of a cycled electrode with a cutoff capacity of 150 mAh/g are shown in Fig. 17. Discharge capacity increases during the rst few cycles, and the formation of discharge plateaus around 4.0 and 2.9 V vs Li/Li+ is observed. These plateaus are characteristics of spinel Mn, suggesting that there is a layered-

to-spinel phase transformation during cycling, consistent with other reports.25,29,30 The phase transformation is most likely facilitated by the poor crystallinity of our sample, together with the removal of oxygen from the lattice and the formation of Li vacancies in the TM layer during charge-discharge. Issues of Li2MnO3. We have shown that Li2MnO3 made at a low temperature is electrochemically active, with a discharge capacity as large as 250260 mAh/g. However, Li2MnO3 shows the following characteristics: rst cycle efciency is 66%; gas is generated during the initial charging process; electrolyte decomposition is observed at elevated temperature; and cycle performance is poor. These limit the usage of phase-pure Li2MnO3 in practical Li-ion batteries. Methods to increase rst cycle efciency, reduce gas generation and improve cycle performance are needed. One such method that has been explored by numerous researches is to stabi-

300 Discharge capcaity (mAh/g) 250 200 150 100 50 0 0 5 10 15 20 25 Cycle number 50mAh/g cut 4.8V cut 250mAh/g cut

150mAh/g cut

18.68Intensity (a.u.)

18.80 19.02

Figure 16. Color online Cycle performance of Li2MnO3 with limited charge capacity.5 Potential (V vs. Li/Li+) 4.5 4 3.5 3 2.5 2 1.5 increase of plateau with cycling 0 50 100 Capacity (mAh/g) 1st 2nd 5th 8th 150 200 1st 2nd 5th 8th 10mA/g 150mAh/g charge cutoff

Intensity (a.u.)

x

17

18

19

20 2

21

22

23

pristine 25C charge 60C charge

15

25

35

45 2 ()

55

65

75

Figure 15. Color online XRD of Li2MnO3 materials charged at 25 and 60C to 350 mAh/g.

Figure 17. Color online Charge-discharge curves of Li2MnO3 with a 150 mAh/g cutoff.


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Journal of The Electrochemical Society, 156 6 A417-A424 20096. 7. 8. 9. 10. 11. 12. 13. 14. 15. 16. 17. 18. 19. 20. 21. 22. 23. 24. 25. 26. 27. 28. 29. 30. 31. 32. 33. 34. 35. 36. 37. 38. 39. D. A. R. Barkhouse and J. R. Dahn, J. Electrochem. Soc., 152, A746 2005 . T. A. Arunkumar, Y. Wu, and A. Manthiram, Chem. Mater., 19, 3067 2007 . C. S. Johnson, J. Power Sources, 165, 559 2007 . S.-H. Kang, P. Kempgens, S. Greenbaum, A. J. Kropf, K. Amine, and M. M. Thackeray, J. Mater. Chem., 17, 2069 2007 . J.-M. Kim, S. Tsuruta, and N. Kumagai, Electrochem. Commun., 9, 103 2007 . C. W. Park, S. H. Kim, I. R. Mangani, J. H. Lee, S. Boo, and J. Kim, Mater. Res. Bull., 42, 1374 2007 . S.-H. Park, S.-H. Kang, C. S. Johnson, K. Amine, and M. M. Thackeray, Electrochem. Commun., 9, 262 2007 . M. Tabuchi, Y. Nabeshima, K. Ado, M. Shikano, H. Kageyama, and K. Tatsumi, J. Power Sources, 174, 554 2007 . M. M. Thackeray, S.-H. Kang, C. S. Johnson, J. T. Vaughey, R. Benedek, and S. A. Hackney, J. Mater. Chem., 17, 3112 2007 . Y. Wu and A. Manthiram, Electrochem. Solid-State Lett., 10, A151 2007 . J. Kikkawa, T. Akita, M. Tabuchi, M. Shikano, K. Tatsumi, and M. Kohyama, Electrochem. Solid-State Lett., 11, A183 2008 . S.-H. Kang, C. S. Johnson, J. T. Vaughey, K. Amine, and M. M. Thackeray, J. Electrochem. Soc., 153, A1186 2006 . Y. Wu and A. Manthiram, Electrochem. Solid-State Lett., 9, A221 2006 . Y. Wu, A. V. Murugan, and A. Manthiram, J. Electrochem. Soc., 155, A635 2008 . J. M. Zheng, J. Li, Z. R. Zhang, X. J. Guo, and Y. Yang, Solid State Ionics, 179, 1794 2008 . M. H. Rossouw and M. M. Thackeray, Mater. Res. Bull., 26, 463 1991 . Y. Shao-Horn, Y. Ein-Eli, A. D. Robertson, W. F. Averill, S. A. Hackney, and W. F. Howard Jr., J. Electrochem. Soc., 145, 16 1998 . P. Kalyani, S. Chitra, T. Mohan, and S. Gopukumar, J. Power Sources, 80, 103 1999 . C. S. Johnson, S. D. Korte, J. T. Vaughey, M. M. Thackeray, T. E. Bonger, Y. Shao-Horn, and S. A. Hackney, J. Power Sources, 81-82, 491 1999 . A. D. Robertson and P. G. Bruce, Chem. Mater., 15, 1984 2003 . A. R. Armstrong, A. D. Robertson, and P. G. Bruce, J. Power Sources, 146, 275 2005 . C. Gan, H. Zhan, X. Hu, and Y. Zhou, Electrochem. Commun., 7, 1318 2005 . Y.-S. Hong, Y. J. Park, K. S. Ryu, and S. H. Chang, Solid State Ionics, 176, 1035 2005 . S.-H. Park, Y. Sato, J.-K. Kim, and Y.-S. Lee, Mater. Chem. Phys., 102, 225 2007 . S.-H. Park, H. S. Ahn, G. J. Park, J. Kim, and Y.-S. Lee, Mater. Chem. Phys., 112, 696 2008 . A. R. Armstrong, M. Holzapfel, P. Novak, C. S. Johnson, S. Kang, M. M. Thackeray, and P. G. Bruce, J. Am. Chem. Soc., 128, 8694 2006 . J. Brger, M. Jiang, N. Dupr, Y. S. Meng, Y. Shao-Horn, G. Ceder, and C. P. Grey, J. Solid State Chem., 178, 2575 2005 . M. Morcrette, P. Barboux, J. Perrire, T. Brousse, A. Traverse, and J. P. Boilot, Solid State Ionics, 138, 213 2001 . W.-S. Yoon, C. P. Grey, M. Balasubramanian, X.-Q. Yang, D. A. Fischer, and J. McBreen, Electrochem. Solid-State Lett., 7, A53 2004 . Y. J. Park, Y.-S. Hong, X. Wu, M. G. Kim, K. S. Ryu, and S. H. Chang, Bull. Korean Chem. Soc., 25, 511 2004 . P.-Y. Liao, J. G. Duh, J.-F. Lee, and H. S. Sheu, Electrochim. Acta, 53, 1850 2007 . S. Venkatraman and A. Manthiram, J. Solid State Chem., 177, 4244 2004 . J. Read, K. Mutolo, M. Ervin, W. Behl, J. Wolfenstine, A. Driedger, and D. Foster, J. Electrochem. Soc., 150, A1351 2003 . P. Kol, H. Nakata, J.-W. Shen, A. Tsuboi, H. Suzuki, and M. Ue, Fluid Phase Equilib., 228-229, 59 2005 .

lize the Li2MnO3 phase by the formation of a composite, similar to that in Li LixMnyMz O2 materials. Yoon et al. reported that the presence of Co in the material allows some charge compensation through the generation of electron holes in the O 2p state;34 thus, the charge mechanism could potentially be changed by the addition of elements and components into the material. Further studies are being conducted to extend our knowledge of Li2MnO3 to Li LixMnyMz O2 materials. Conclusions Li2MnO3 with a maximum discharge capacity of 260 mAh/g was synthesized by solid-state reaction. Electrochemical performance of the material is found to depend strongly on synthesis conditions. Reducing particle size and increasing the amount of stacking faults enable Li2MnO3 to be charged at a lower potential to a higher capacity. ICP measurements conrmed that Li is extracted and reinserted into the material, consistent with electrochemical capacity, during charge-discharge. Ex situ XANES results suggest that Mn valence remains the same during charging and is reduced during discharging. Further study to quantify the valence of Mn and investigate the stability of the charged/discharged electrodes in air is needed. GC measurements conrmed the generation of O2 during charging. The total amount of O2 gas detected corresponds to 1/8 mole of O2 per mole of Li extracted from Li Li1/3Mn2/3 O2 at 25C. This can account for half of the charge compensation. Some of the oxygen lost from the active material may exist in other forms other than oxygen gas in the cell. In addition, H+ /Li+ exchange is also expected to take part during charging, especially at high potential and at high temperature. On the basis of our results, we speculate that vacancies are left in the lattice after oxygen is removed from the active material. The structure after charging is not in an equilibrium state, and the rearrangement of atoms within the material leads to a gradual transformation to spinel structure with cycling. Further analyses are in progress to clarify the charge-discharge mechanism.Sanyo Electric Company, Limited assisted in meeting the publication costs of this article.

References1. Z. Lu, D. D. MacNeil, and J. R. Dahn, Electrochem. Solid-State Lett., 4, A191 2001 . 2. Z. Lu and J. R. Dahn, J. Electrochem. Soc., 149, A815 2002 . 3. J.-S. Kim, C. S. Johnson, J. T. Vaughey, M. M. Thackeray, S. A. Hackney, W. Yoon, and C. P. Grey, Chem. Mater., 16, 1996 2004 . 4. C. S. Johnson, J.-S. Kim, C. Leef, N. Li, J. T. Vaughey, and M. M. Thackeray, Electrochem. Commun., 6, 1085 2004 . 5. C. S. Johnson, N. Li, J. T. Vaughey, S. A. Hackney, and M. M. Thackeray, Electrochem. Commun., 7, 528 2005 .


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