Revisiting the initial irreversible capacity loss of LiNi0.6Co0.2Mn0.2O2 cathode material batteries
Graphical abstract
Introduction
Layered transition metal oxides, such as LiCoO2, are the predominant cathode materials for Li-ion batteries (LIBs) that dominate portable applications, electric vehicles (EVs) and stationary energy storage, because of their high energy density and considerably long cycling life [1], [2], [3], [4]. Ni-rich layered cathodes have drawn great attention for application in automobile batteries, primarily driven by the relatively lower cost of nickel than cobalt and the potential unlock more reversible capacity by raising their upper cutoff potential (up to 4.5 V vs. Li+/Li). LiNi0.6Co0.2Mn0.2O2 (NCM622), LiNi0.8Co0.1Mn0.1O2 (NCM811), LiNi0.8Co0.15Al0.05O2 (NCA) and even Co-free layered cathodes are the current hotspots [[5], [6], [7], [8], [9]]. Researchers are committed to addressing the severe challenges to improve their production and application, including a sensitivity to the environment, great reactivity with the electrolyte, fatal thermal abuse, and these challenges become more serious with Ni content increasing [[10], [11], [12], [13], [14]]. Besides the effort mentioned above, researchers also try to increase the charge voltage for the layered cathode materials with medium high Ni content to obtain higher specific energy density. For example, 4.6V-NCM622 (NCM622 charged to 4.6V vs. Li+/Li) can deliver 10% higher theoretical specific energy density than 4.3V-NCM811, while the challenges need to be addressed are similar or less severe than that of 4.3V-NCM811 (see Fig. S1 for a comparison of specific energy density at the material level). Given that the capacity loss during the first cycle is around 10–30% [15,16], another opportunity to significantly increase the energy density of these cathodes can be achievable by mitigating the capacity loss in the first cycle [15].
The reported explanations for this initial loss are as follows: (1) parasitic electrochemical reactions occurring on the surface of the cathode materials with electrolyte; [17], [18], [19], [20] (2) loss of Li-site due to irreversible structural changes; [21], [22], [23] (3) slow kinetics for lithium intercalation [15,24,25]. It is widely accepted that the parasitic side reactions and phase transitions are absolutely irreversible, while the capacity loss due to Li+ diffusion kinetics is conditional, varying with conditioning temperature and applied current density. In fact, the large capacity loss in the first cycle was once reported by Chen et al., it mainly occurs under 3.8V and kept almost constant when the charging potential was below 4.0V (vs. Li+/Li). In addition, this loss was observed only during the first cycle and the subsequent cycles achieved close to 100% coulombic efficiency [25]. This indicated that the parasitic reactions on the interface between cathode and electrolyte might not the main contributor for the initial capacity loss at low potential range. Zhou et al. recently showed that the slow lithium kinetics at high lithium contents was highly related with the initial cycle capacity loss of NCM 811, as Li+ diffusion coefficient dropped nearly by 2, 3 orders of magnitude from Li0.7Ni0.8Co0.1Mn0.1O2 to LiNi0.8Co0.1Mn0.1O2 during lithiation [15,16]. Increasing the temperature from 25°C to 45°C to accelerate Li+ diffusion, the capacity loss of NCM811 decreased from 12.1 to 8.4 mAh g−1. Decreasing C-rates also resulted in less charge-discharge asymmetry with better Li+ intercalation kinetics and higher initial coulombic efficiency [26]. To clarify the onset potential of parasitic electrochemical reaction, Robert et al. studied operando differential electrochemical mass spectrometry (DEMS) and revealed that CO2 gas is not continuously released from the very beginning of charging. CO2 generation started at ∼4V (vs. Li+/Li) in the first charging, which corresponding to the oxidative decomposition of the carbonate electrolyte [27]. Meanwhile, Zeng et al. used a home-built high-precision leakage current measuring system and also clearly stated that no obvious electrochemical reaction and chemical reaction occurred when the cut-off potential was lower than 4.0V (vs. Li+/Li) [28]. Hence, the capacity loss caused by parasitic electrochemical reaction below 4V (vs. Li+/Li) can be ignored. It is of great significance to investigate the causes of initial capacity loss in the low voltage (≤4V, vs. Li+/Li), and the investigation may guide the upside space for layered cathode material with higher specific capacity.
Commercial NCM622 attracts many attentions due to the highest energy density, good rate performance [24,29] and moderate cost among the layered oxide cathode materials when the cut-off potential is raised to 4.6 V (vs. Li+/Li) or above. In this work, we choose commercial LiNi0.6Mn0.2Co0.2O2 (NCM622) in the voltage range of 2.7–4.0V (vs. Li+/Li) as a model system. The structural evolution of NCM622 at different temperature (25°C, 45°C and 60°C) and different rate (0.1C, 0.01C, 1C=120 mA g−1) are investigated using operando X-ray diffraction. Combining these results, the correlation between structural evolutions and Li+ diffusion kinetics are revealed. Our results clearly demonstrate that 46% of the initial capacity loss of NCM622 is due to the slow Li+ diffusion kinetics, another 46% of the capacity loss is caused by the irreversible O3/H1-3 phase transition, and only 8% is attributed to the surface changes in the material and/or CEI formation during the first charging.
Section snippets
Electrode preparation
NCM622 single-crystal particles were provided by Beijing Easpring Material Technology Co. Ltd, China. The working electrodes were prepared by casting the slurry of active material (80 wt%), conductive carbon black C45 (10 wt%) and poly(vinylidene-fluoride) (10 wt%) on a porous aluminum foil, followed by drying at 80°C under vacuum overnight. The loading of active material was controlled within the range between 5.0 and 6.0 mg cm−2.
Half-cell assembly
The NCM622|Li half-cell tests were conducted using coin-type
Results and discussion
Figs. S2a and c display the initial XRD patterns of NCM622|Li-O at RT and 60°C, all the diffraction peaks can be well-indexed to the α-NaFeO2 layer structure with space group of R-3m, no other obvious diffraction peaks can be detected except some peaks corresponding to the Be and Al. The cell parameters and other information obtained by Rietveld refinement are listed in Table S1, with a small fitting deviation (Rwp) of 4.3% (RT), and 5.1% (60°C). The calculated Li/Ni mixing ratio of this sample
Conclusions
In conclusion, the causes for low ICE of NCM622 in the first charge–discharge process are deeply investigated in the low voltage 2.7–4.0V (vs. Li+/Li), and the correlation between structural evolution and Li+ diffusion kinetics is revealed by operando XRD and galvanostatic charge-discharge cycling. It is clarified that 46% of the initial capacity loss of NCM622 is affected by the slow Li+ kinetics, another 46% of the capacity loss is caused by irreversible O3/H1-3 phase transition, the
Declaration of Competing Interest
The authors declare that they have no known competing financial interests or personal relationships that could have appeared to influence the work reported in this paper.
Acknowledgement
We would like to show gratitude to the Ministry of Science and Technology of China (No. 2021YFB2501900, 2019YFA0705703 and 2019YFE0100200), the National Natural Science Foundation of China (No. U1564205 and 51706117) and the Tsinghua University Initiative Scientific Research Program (No. 2021THFS0216). The authors also thank Argonne National Laboratory at U.S. and China – Clean Energy Research Center (CERC-CVC2.0, 2016-2020), and thank Tsinghua University-Zhangjiagang Joint Institute for
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2023, Journal of Power SourcesCitation Excerpt :(Fig. 7a and b) shows the EIS measurements of the original NCM-(0, 3, 5, 7) electrodes to reveal the interfacial reaction kinetics of the material [46]. The obtained Nyquist diagram consists of two parts: a semicircle in the high frequency part and a straight line in the low frequency part [47]. Fig. 7a shows the EIS spectra obtained from equivalent circuit simulations, including Rs, Rct, Zw (solution resistance, charge-transfer resistance, Warburg impedance) [48].