Is Li4Ti5O12 a Solid-Electrolyte-Interphase-Free Electrode Material in Li-Ion Batteries? Reactivity Between Li4Ti5O12 Electrode and Electrolyte (2014)

Li 4 Ti 5 O 12 with a cubic spinel structure (space group, F d 3(_) m ) has a high redox potential at around 1.5 V vs. Li + /Li with a theoretical capacity of 175 mA h g −1 . 2 The negligible structural difference between pristine Li 4 Ti 5 O 12 and lithiated Li 7 Ti 5 O 12 at the two-phase equilibrium junction guarantees an outstanding electrochemical reversibility during the charge/discharge process. 3 Furthermore, the high redox potential would prevent not only the lithium metal deposition on the anode at high current conditions but also the formation of the resistive solid electrolyte interphase (SEI) layer, which may lead to an active Li-ion loss and an increase of the cell impedance. 4 No SEI formation at the surface of Li 4 Ti 5 O 12 is a widely accepted argument from the literature point of view. However, in our previous report regarding the electrochemical study of the carbon-free Li 4 Ti 5 O 12 electrode, 5 we noticed the formation and dissolution of the SEI layer through the change in the intensity of Ti 2p XPS core peaks during the charge and discharge process. This fact led us to suspect the stability of Li 4 Ti 5 O 12 vis-à-vis to the electrolyte in spite of its high redox potential. Despite the interesting properties of Li 4 Ti 5 O 12 , only few literature studies were reported on its reactivity to the electrolyte. Based on a detailed XPS study on the electrolyte/electrode interfaces in LiMn 1.6 Ni 0.4 O 4 / Li 4 Ti 5 O 12 system, Dedryvère et al. have reported the formation of organic and inorganic species on the surface of Li 4 Ti 5 O 12 anode after cycling. 6 However, they concluded that those species were first formed at the cathode and then, adsorbed on the surface of Li 4 Ti 5 O 12 either by diffusion or by migration of organic cationic species. In addition, the lower voltage limit of Li 4 Ti 5 O 12 anode couldn’t be also guaranteed to be over 1 V in their study because measuring the voltage of Li 4 Ti 5 O 12 itself is impossible in two-electrode full cell. He et al. also pointed out the formation of SEI film on the Li 4 Ti 5 O 12 electrode cycled between 2.5 and ~ 0 V vs. Li + /Li., but they mainly focused on the SEI formation occurred below 1 V. 7 Moreover, in the aforementioned studies, the results were obtained only at room temperature cycling, and the effects of carbon conducting agent contained in the conventional Li 4 Ti 5 O 12 electrodes were neither considered nor clarified. In this report, for the first time, the Li 4 Ti 5 O 12 / electrolyte interface is investigated at room and high temperature using the carbon-free Li 4 Ti 5 O 12 electrode. The new electrode concept 5,8 allows us to examine the reactivity of Li 4 Ti 5 O 12 to the electrolyte and avoid any kind of parasite reaction which may be induced by the high-surface-area carbon conducting additive. Chemical changes at the surface of Li 4 Ti 5 O 12 were investigated using a step by step X-ray photoelectron spectroscopy (XPS) analysis during charge/discharge cycling. The time-of-flight secondary ion mass spectroscopy (ToF-SIMS) study and scanning electron microscopy (SEM) observation were carried out to examine a quantitative and qualitative change in the surface chemistry and the electrode morphology after cycling, respectively. The differences between the carbon-free and carbon-containing Li 4 Ti 5 O 12 electrodes in terms of stability and cyclability were also discussed. [1] S.S. Zhang, J. Power Sources , 2006, 161 , 1385. [2] T. Ohzuku, A. Ueda, N. Yamamoto, J. Electrochem. Soc. , 1995, 142 , 1431; L. Kavan, M. Gratzel, Electrochem. Solid State Lett. , 2002, 5 , A39. [3] K. Zaghib, M. Simoneua, A. Armand, M. Gauthier, J. Power Sources , 1999, 81-82 , 300; G. Armstrong, A. R. Armstrong, J. Canales, P. G. Bruce, Electrochem. Solid-State Lett. , 2006, 9 , A139; A. N. Jansen, A. J. Kahaian, K. D. Kepler, P. A. Nelson, K. Amine, D. W. Dees, D.R. Vissers, M. M. Thackeray, J. Power Sources , 1999, 81-82 , 902; T. Brousse, P. Fragnaud, R. Marchand, D. M. Schleich, O. Bohnke, K. West, J. Power Sources , 1997, 68 , 412; T. Ohzuku, A. Ueda, N. Yamamoto, J. Electrochem. Soc. , 1995, 142 , 1431. [4] J. Christensen, V. Srinivasan, J. Newman, J. Electrochem. Soc. , 2006, 153 , A560; M. Winter, W. K. Appel, B. Evers, T. Hodal, K. C. Moller, I. Schneider, M. Wachtler, M. R. Wagner, G. H. Wrodnigg, J. O. Besenhard, Monatsch. Chem. , 2001, 132 , 473. [5] M. S. Song, A. Benayad, Y. M. Choi and K. S. Park, Chem. Commun. , 2012, 48 , 516. [6] R. Dedryvère, D. Foix, S. Franger, S. Patoux, L. Daniel and D. Gonbeau, J. Phys. Chem. C, 2010, 114 , 10999. [7] Y. B. He, F. Ning, B. Li, Q. S. Song, W. Lv, H. Du , D. Zhai, F. Su, Q. H. Yang, F. Kang, J. of Power Sources, 2012, 202 , 253. [8] C. J. Kim, N. S. Norberg, C. T. Alexander, R. Kostecki and J. Cabana, Adv. Funct. Mater., 2013, 23 , 1214.