- freely available
Membranes 2013, 3(4), 298-310; doi:10.3390/membranes3040298
Published: 25 October 2013
Abstract: The electrochemical properties of a composite solid polymer electrolyte, consisting of poly(ethylene oxide) (PEO)-lithium bis(trifluoromethanesulfonyl)imide (LiTFSI) and tetraethylene glycol dimethyl ether (TEGDME) was examined as a protective layer between lithium metal and a water-stable lithium ion-conducting glass ceramic of Li1+x+y(Ti,Ge)2−xAlxP3−ySiyO12 (LTAP). The lithium ion conductivity and salt diffusion coefficient of PEO18LiTFSI were dramatically enhanced by the addition of TEGDME. The water-stable lithium electrode with PEO18LiTFSI-2TEGDME, as the protective layer, exhibited a low and stable electrode resistance of 85 Ω·cm2 at 60 °C, after 28 days, and low overpotentials of 0.3 V for lithium plating and 0.4 V for lithium stripping at 4.0 mA·cm−2 and 60 °C. A Li/PEO18LiTFSI-2TEGDME/LTAP/saturated LiCl aqueous solution/Pt, air cell showed excellent cyclability up to 100 cycles at 2.0 mAh·cm−2.
Aqueous lithium-air batteries have been considered as a promising electrochemical energy storage system for electric vehicles. The theoretical energy density for the cell reaction of 4Li + 6H2O + O2 = 4(LiOH·H2O) is 1910 Wh·kg−1, which is significantly higher than 387 Wh·kg−1 for typical lithium-ion batteries with a carbon anode and LiCoO2 cathode. The aqueous lithium-air battery system, proposed by Imanishi and co-workers, is composed of a lithium metal electrode, a lithium ion conducting polymer electrolyte based on poly(ethylene oxide) (PEO)x-lithium bis(trifluoromethanesulfonyl)imide (LiTFSI), a water-stable lithium ion-conducting glass ceramics of Li1+x+y(Ti,Ge)1−xAlxP3−ySiyO12 (LTAP), an aqueous electrolyte with saturated LiCl, and a carbon air electrode . At present, the only acceptable water-stable lithium ion conducting solid electrolyte is LTAP, which exhibits a lithium ion conductivity of higher than 10−4 S·cm−1 at ambient temperature, and is stable in saturated LiOH and LiCl aqueous solution, but exhibits poor chemical stability towards lithium metal . To construct a water-stable lithium electrode (WSLE) based on LTAP requires a chemically stable lithium conducting electrolyte interlayer between the lithium metal and LTAP. Some candidates for this interlayer have been adopted, such as lithium nitride , lithium phosphorous oxynitride , and polymer electrolytes . The two former materials are generally prepared by vapor deposition, which involves considerable cost and makes the preparation of large sized cells difficult. In contrast, the polymer electrolyte is stable in contact with lithium metal and large sized sheets can be easily fabricated.
In our previous studies [6,7,8], we have reported that the interface resistance between lithium metal and polymer electrolytes in a WSLE is the dominant part of the cell resistance and an important factor in initiating lithium dendrite formation. The addition of ionic liquids into PEO18LiTFSI reduced the interface resistance and suppressed lithium dendrite formation ; however, high overpotentials for lithium deposition and stripping reaction were observed at high current densities. The WSLE should be operated at the highest current density possible with low overpotentials to prevent the formation of lithium dendrites . The addition of low-molecular weight plasticizers to the PEO-based electrolyte is expected to improve the interface properties between lithium metal and the polymer electrolyte, and enhance the lithium ion transport number of the polymer electrolyte. Kim et al.  reported the use of low molecular weight oligomer ethers as a plasticizer to enhance the transport properties of polymer electrolytes, and Naoi et al. reported that the addition of poly(ethylene glycol) dimethyl ether (PEGDME) into propylene carbonate (PC) with LiClO4 suppressed dendrite formation . Moreover, Yoshida et al. reported that the oxidative stability of glyme molecules is enhanced by complex formation with LiTFSI in a molar ratio of 1:1 . Recently, Jung et al.  demonstrated a Li/tetraethylene glycol dimethyl ether (TEGDME)-LiCF3SO3/carbon, O2 cell capable of operating over many cycles with capacity and rate values as high as 5000 mAh·g−1 and 0.5 A·g−1, respectively. We have previously reported an increase in the lithium ion transport number and decreases in the interface resistance of the lithium metal and polymer electrolyte by the addition of PEGDME to PEO18LiTFSI, where the mean molecular weight of PEGDME was 500 . Naoi et al.  concluded that the Gibbs activation energy for the charge transfer reaction on the lithium metal surface in PC-PEGDME-LiClO4 decreased with a decrease in the molecular weight of PEGDME in the range of 90–400. In this study, the interface resistance between lithium and the polymer electrolyte, and the transport properties of the PEO18LiTFSI-xTEGDME (M = 222.28 g·mol−1) composite polymer electrolyte (CPE) are examined as a function of the amount of TEGDME (x). In addition, the electrochemical performance of a Li/PEO18LiTFSI-2TEGDME/LTAP/saturated LiCl aqueous solution/Pt, air cell is evaluated at 60 °C.
2. Results and Discussion
2.1. Evaluation of CPEs
The electrical conductivities of PEO18LiTFSI-xG4 (TEGDME abbreviated as G4 hereafter) were measured as a function of x (the molar ratio of G4 to ethylene oxide). Figure 1 presents Arrhenius plots for the conductivity of PEO18LiTFSI-xG4. The conductivity increases significantly with increasing x up to 2 and there is little difference in conductivity between the samples with x = 2 and 3. The electrical conductivity of PEO18LiTFSI-2G4 at 25 °C is almost one order of magnitude higher and that at 60 °C is three times higher than that of PEO18LiTFSI. TEGDME loosens the coordination of lithium ions with EO units in the PEO matrix and thus enhances the mobility of ions, and could also enable lithium ions to decouple from ion pairs, as shown by Kriz et al. . The activation energies for conduction in PEO18LiTFSI-xG4 at high temperature decrease with increasing x. That of PEO18LiTFSI-2G4 was calculated to be 25.3 kJ·mol−1, in the range of 55 to 80 °C, which is lower than that for PEO18LiTFSI (38.8 kJ·mol−1) and that for PEO18LiTFSI-2.0 N-methyl-N-propylpiperdinium bis(fluorosulfonyl) imide (PP13FSI) (33.8 kJ·mol−1) .
The overpotentials between lithium metal and polymer electrolytes for lithium deposition and stripping generally increase with current density and undergo a sudden increase with the polarization period at a current density (limiting current density). When the ionic concentration in the vicinity of cathode drops to zero, the limiting current density is reached and dendrite growth is initiated (Sand time) . To operate the Li/PEO18LiTFSI/LTAP/Pt, air cell at high current density, it is necessary to enhance the limiting current density of lithium-ion conducting PEO-based polymer electrolytes (Il), which is proportional to the salt diffusion coefficient and lithium ion transference number, as shown by Equation (1):
Lithium ion transference numbers for PEO18LiTFSI-xG4 were measured using the method reported by Evans and Vincent . Figure 3 shows a typical cell current decay curve upon application of a DC bias of 20 mV and impedance profiles for the Li/PEO18LiTFSI-2G4/Li cell. From these results, ta was calculated using the Evans and Vincent equation, and the results are summarized in Table 1. Significant increase of the lithium ion transport number (i.e., decrease of the anion transport number) was observed by addition of G4 into PEO18LiTFSI. The lithium ion transport number for PEO18LiTFSI-2G4 is slightly higher than that for LiTFSI-2G4. Based on these results for D and ta, the limiting current density (Il) for PEO18LiTFSI-xG4 was calculated and the results are summarized in Table 1, where the thickness (L) was 100 μm. PEO18LiTFSI-2G4 exhibits the highest Il of 15.8 mA·cm−2, which is higher than that for PEO18LiTFSI by a factor of approximately 15. The high limiting current density of PEO18LiTFSI-2G4 suggests that a WSLE with PEO18LiTFSI-2G4 could be operated at a high current density.
|Table 1. Ionic transport properties of PEO18LiTFSI-xTEGDME.|
|PEO18LiTFSI- xTEGDME||25 °C(×106 S·cm−1)||60 °C(×104 S·cm−1)||Ea (kJ·mol−1)||D (×107 cm2·s−1)||tLi+||Il (mA cm−2) L = 100 μm|
|σ||σLi+||σ||σLi+||Low temp. region||High temp. region|
|x = 0||5.64||1.35||5.29||1.27||115.7||38.8||0.36||0.24||1.02|
|x = 1.0||28.0||12.0||10.7||4.60||99.8||30.7||1.05||0.43||3.97|
|x = 1.5||40.7||18.3||12.5||5.62||82.4||27.1||1.50||0.45||5.87|
|x = 2.0||60.8||32.8||16.5||8.91||78.2||25.3||3.37||0.54||15.8|
|x = 3.0||68.3||39.6||16.4||9.51||72.9||25.0||2.27||0.58||11.6|
Low and stable interface resistance between lithium metal and polymer electrolytes is essential for the electrochemical performance of WSLEs and to reduce lithium dendrite formation . Figure 4 shows the impedance profile changes for the Li/PEO18LiTFSI-xG4/Li cells at 60 °C as a function of storage time. PEO18LiTFSI-G4 and PEO18LiTFSI-1.5G4 show a significant increase of interface resistance with storage time; the initial cell resistance of 69 Ω·cm2 increased to 141 Ω·cm2 for PEO18LiTFSI-G4 after 28 days. However, low interface resistance was obtained for PEO18LiTFSI-2G4 and PEO18LiTFSI-3G4. After 28 days, PEO18LiTFSI-2G4 and PEO18LiTFSI-3G4 showed interface resistances of 34 and 74 Ω·cm2, respectively, which are much lower than 253 Ω·cm2 for PEO18LiTFSI after storage for 28 days . The interface resistance behavior for PEO18LiTFSI-2G4 was unusual, where the interfacial resistance increased during the initial seven days and then decreased continuously to a value lower than the original. A similar change in the interface resistance was reported for the Li/PEGDME-LiTFSI/Li cell by Bernhard et al. , which could be attributed to the solid electrolyte interphase (SEI) formation-re-dissolution process . These impedance profiles show a diminished semicircle, which is associated with the resistance of a passivation film (SEI) formed on the lithium electrode surface by the reaction of lithium with the polymer electrolyte and the charge transfer resistance. Figure 5 shows the temperature dependence of the inverse of the passivation film resistance and the charge transfer resistance for the Li/PEO18LiTFSI-xG4/Li cells as a function of x. The activation energy for the inverse of the passivation film resistance (Rp) decreased from 76.2 kJ·mol−1 for PEO18LiTFSI to 54.7 kJ·mol−1 for PEO18LiTFSI-2G4. A decrease was also observed for PEO18LiTFSI-G4 and PEO18LiTFSI-3G4, but it was not as significant as that for PEO18LiTFSI-2G4. The activation energies for the inverse of the charge transfer resistance (Rc) decreased with increasing x. The lowest value of 63.4 kJ·mol−1 was calculated for PEO18LiTFSI-3G4, in comparison with 81.7 kJ·mol−1 for PEO18LiTFSI and 68.1 kJ·mol−1 for PEO18LiTFSI-2G4. These results suggest that the low-molecular weight oligomer ether G4 could reduce the resistance of the SEI and facilitate the charge transfer reaction at the interface. The former role is similar to other additives, such as nanofillers and ionic liquids, whereas the latter role is only performed by G4.
2.2. Electrochemical Performance of WSLEs
The high lithium ionic diffusion coefficient and low interface resistance with lithium metal for PEO18LiTFSI-2G4 motivated us to examine its role as the protective layer in a WSLE. The impedance of the Li/PEO18LiTFSI-2G4/LTAP/sat. LiCl aqueous solution/Pt, air cell was measured at 60 °C, using a platinized platinum reference electrode. Figure 6 presents the impedance spectra of this cell for various storage times. The open circuit voltage (OCV) was stabilized at 3.48 V after one week, which is comparable with that reported previously (3.43 V)  and slightly lower than that of the calculated OCV (3.59 V). After 28 days, a stable cell resistance of 84 Ω·cm2 was obtained, which is comparable with those reported previously; the cell resistance for the Li/PEO18LiTFSI/LTAP/1 M LiCl/Pt, air cell was 539 Ω·cm2 , 118 Ω·cm2 for the Li/PEO18LiTFSI-40 nm BaTiO3/LTAP/1 M LiCl aqueous solution/Pt, air cell  and 130 Ω·cm2 for the Li/PEO18LiTFSI-1.44 N-methyl-N-propylpiperdinium-bis(trifluromethanesulfonyl)imide/LTAP/1 M LiCl aqueous solution/Pt, air cell . An equivalent circuit proposed in our previous study was utilized to analyze the impedance spectra, which consists of the total resistances of the polymer electrolyte and the LTAP plate (Rb), the interfacial resistance between the polymer electrolyte and lithium metal electrode (Rf1), the interfacial resistance between the polymer electrolyte and the LTAP plate (Rf2), the charge-transfer resistance (Rc), and the Warburg impedance (W1) . Rb was quite stable at around 38 Ω·cm2 during the storage period. The fitting results suggest that Rf2 increased from 19.4 to 29.3 Ω·cm2, Rc decreased from 18.0 to 7.4 Ω·cm2, and Rf1 increased from 3.8 to 5.8 Ω·cm2 over the 28-day storage period.
The electrochemical performance of a WSLE protected by PEO18LiTFSI-2G4 and LTAP was investigated in an aqueous electrolyte using platinized platinum electrodes as the counter and reference electrodes. Figure 7 shows the change in potential over time for the Li/PEO18LiTFSI-2G4/LTAP/1 M LiCl-4 mM LiOH aqueous solution/Pt, air cell at current densities in the range of 0.5 to 4.0 mA·cm−2 at 60 °C. This WSLE exhibited quite low lithium plating and stripping overpotentials at high current densities up to 4.0 mA·cm−2. The lithium stripping and plating overpotentials at 1.5 mA·cm−2 were 0.10 and 0.15 V, respectively, which are lower than the best results obtained for the Li/PEO18LiTFSI-18 wt % PEGDME/LTAP/1 M LiCl-4 mM LiOH aqueous solution/Pt, air cell (0.29 V for plating and 0.21 V for stripping) in our previous studies . The low overpotentials of the cell at high current densities could be attributed to the high lithium ion diffusion coefficient, high lithium ion transport number, and low interfacial resistance of PEO18LiTFSI-2G4.
To study the lithium dendrite formation at the interface of Li and PEO18LiTFSI-2G4, a long period of lithium deposition at a constant current of 1 mA·cm−2 was performed using the Li/PEO18LiTFSI-2G4/LTAP/saturated LiCl aqueous solution/Pt, air cell, where the thickness of PEO18LiTFSI-2G4 was around 100 μm and the impedance of the WSLE was measured at every 4 h polarization. Figure 8a shows cell potential versus time curves as a function of the polarization period. The lithium electrode potential increased suddenly after a 25 h polarization. This potential increase may be due to lithium deposition on LTAP by lithium dendrite formation, which would result in the formation of a high resistance layer by the reaction of lithium and LTAP . Figure 8b shows the impedance profiles as a function of the polarization period. The WSLE resistance increased gradually with the polarization period up to 13 h and then decreased up to 22 h polarization. The decrease of electrode resistance may be due to lithium dendrite formation. Finally, the WSLE resistance was increased to 220 Ω·cm2 by the short circuit of the lithium metal electrode with LTAP. The short circuit period of 25 h is approximately 2.6 times longer than that measured for a Li/PEO18LiTFSI/LTAP/10 M LiCl-4 mM LiOH aqueous solution/Pt, air cell . The long short circuit period for the Li/PEO18LiTFSI-2G4/LTAP/saturated LiCl aqueous solution/Pt, air cell could be explained by the high lithium ion transport number, high salt diffusion coefficient, and low interface resistance [17,23].
The cyclability of the Li/PEO18LiTFSI-2G4/LTAP/saturated LiCl aqueous solution/Pt, air cell for lithium deposition and stripping at a constant current density of 1.0 mA·cm−2 was measured at 60 °C, where the current was passed for 2 h. The cell voltage versus time profile is shown in Figure 9. After 100 cycles, the overpotential for lithium deposition and stripping slightly increased from 0.10 to 0.15 V and from 0.08 to 0.13 V, respectively. This excellent cycling performance could be ascribed to the low and stable resistance for the SEI formed between lithium metal and PEO18LiTFSI-2G4.
3. Experimental Section
PEO (Sigma-Aldrich, Mv ≈ 600,000 g·mol−1) and LiTFSI (Wako Chemicals, Japan) were dried overnight under vacuum at 50 and 160 °C, respectively, and then transferred to an Ar-filled glove box without exposure to air. G4 (Kishida Chemical, M = 222.28 g·mol−1) was immersed into activated 0.3 nm molecular sieves for 1 week and the same pretreatment by molecular sieves was performed 3 times before G4 was stored in a glove box. The composite polymer electrolytes of PEO18LiTFSI-xTEGDME in the range of x = 0–3 were prepared using a casting method . LiTFSI (Wako Chemicals, Japan) and G4 were added to an acetonitrile (AN) solution of PEO (Li/O = 1/18). The mixed solution was stirred at room temperature for 12 h and then cast into a clean Teflon dish. The AN solvent was evaporated slowly at room temperature in a Ar-filled dry glove box. After evaporation of the AN, the Teflon dish was transferred to a vacuum oven and dried at 80 °C for 24 h to remove residual AN. The resultant CPEs were ca. 100 μm thick.
Electrical conductivity measurements of the CPEs were performed using sandwich cells of Au/CPE/Au with gold foil electrodes. The cell impedances were measured using a frequency response analyzer (Solartron 1250) in the frequency range from 0.1 Hz to 1 MHz at temperatures in the range of 25–80 °C. Z-plot software was employed for data analysis.
The LTAP plate (ca. 250 μm thick) was supplied by Ohara Inc., Japan. The electrical conductivity of the LTAP plate at 60 °C was 1.4 × 10−3 S·cm−1. A Li/CPE/Li cell was assembled to investigate the interfacial resistance between lithium and the CPE. The active surface area was 1.00 cm2. The WSLE was prepared by sandwiching lithium metal foil (200 μm thick) with a Cu thin film lead, CPE, and the LTAP plate in a plastic envelope. The envelope was evacuated, heat-sealed apart from a 0.35 × 0.35 cm2 area, and then subjected to an isostatic pressure of 150 MPa for 15 min to ensure good contact. The WSLE was immersed into an aqueous solution of 1 M (or 10 M) LiCl with 4 mM LiOH. A platinized Pt electrode was used as both the counter and reference electrodes. Electrochemical measurements were conducted using a multichannel potentiostat-galvanostat (Biologic Science Instruments VMP3). The lithium ion transport number tLi+, was determined using the Li/CPE/Li cell with a combination of AC impedance spectroscopy and the DC polarization method, as originally proposed by Evans and Vincent, and later refined by Abraham and Jiang [19,25]. The cell potentials were measured after polarization for at least 4 h to obtain steady-state current data. The diffusion coefficient was estimated using a method proposed by Ma et al. . The Li/CPE/Li cell was polarized at 50 mV under potentiostatic mode for a few hours to achieve steady-state, after which the potential was interrupted and monitored at 60 °C.
The PEO18LiTFSI-2G4 electrolyte exhibited a high lithium ion conductivity of 8.91 × 10−4 S·cm−1, a high diffusion coefficient of 3.37 × 10−7 cm2·S−1 at 60 °C, and a low interfacial resistance in contact with lithium metal. The Li/PEO18LiTFSI-2G4/LTAP/saturated LiCl aqueous solution/Pt, air cell exhibited excellent cyclability. The overpotentials for lithium deposition and stripping at 2.0 mAh·cm−2 for 2 h polarization at 60 °C were increased slightly from 0.10 to 0.15 V and from 0.08 to 0.13 V after 100 cycles, respectively. Therefore, the CPE is an attractive material for the interlayer between lithium metal and LTAP for the water stable lithium electrode in lithium-air batteries.
Conflicts of Interest
The authors declare no conflict of interest.
- Zhang, T.; Imanishi, N.; Hasegawa, S.; Hirano, A.; Xie, J.; Takeda, Y.; Yamamoto, O.; Sammes, N. Li/polymer electrolyte/water stable lithium-conducting glass ceramics composite for lithium-air secondary batteries with an aqueous electrolyte. J. Electrochem. Soc. 2008, 155, A965–A969. [Google Scholar]
- Shimonishi, Y.S.Y.; Zhang, T.; Imanishi, N.; Im, D.; Lee, D.J.; Hirano, A.; Takeda, Y.; Yamamoto, O.; Sammes, N. A study on lithium/air secondary batteries-stability of the NASICON-type lithium ion conducting solid electrolyte in alkaline aqueous solutions. J. Power Sources 2011, 196, 5128–5132. [Google Scholar] [CrossRef]
- Visco, S.J.; Nimon, N.; Katz, B.; Jonghe, L.C.D.; Chu, M.Y. The Development of High Energy Density Lithium/Air and Lithium/Water Batteries with No Self-Discharge. In Proceedings of the 210th Electrochemical Society Meeting, Cancun, Mexico, 2 November 2006.
- Imanishi, N.; Hasegawa, S.; Zhang, T.; Hirano, A.; Takeda, Y.; Yamamoto, O. Lithium anode for lithium-air secondary batteries. J. Power Sources 2008, 185, 1392–1397. [Google Scholar] [CrossRef]
- Wang, X.; Hou, Y.; Zhu, Y.; Wu, Y.; Holze, R. An aqueous rechargeable lithium battery using coated Li metal as anode. Sci. Rep. 2013, 3, 1401. [Google Scholar] [CrossRef]
- Zhang, T.; Imanishi, N.; Shimonishi, Y.; Hirano, A.; Takeda, Y.; Yamamoto, O.; Sammes, N. A novel high energy density rechargeable lithium/air battery. Chem. Commun. 2010, 46, 1661–1663. [Google Scholar]
- Liu, S.; Wang, H.; Imanishi, N.; Zhang, T.; Hirano, A.; Takeda, Y.; Yamamoto, O.; Yang, J. Effect of co-doping nano-silica filler and N-methyl-N-propylpiperidinium bis(trifluoromethanesulfonyl)imide into polymer electrolyte on Li dendrite formation in Li/poly(ethylene oxide)-Li(CF3SO2)2N/Li. J. Power Sources 2011, 196, 7681–7686. [Google Scholar] [CrossRef]
- Zhang, T.; Imanishi, N.; Hirano, A.; Takeda, Y.; Yamamoto, O. Stability of Li/polymer electrolyte-ionic liquid composite/lithium conducting glass ceramics in an aqueous electrolyte. Electrochem. Solid-State Lett. 2011, 14, A45–A48. [Google Scholar] [CrossRef]
- Christensen, J.; Albertus, P.; Sanchez-Carrera, R.S.; Lohmann, T.; Kozinsky, B.; Liedtke, R.; Ahmed, J.; Kojic, A. A critical review of Li/air batteries. J. Electrochem. Soc. 2012, 159, R1–R30. [Google Scholar] [CrossRef]
- Kim, Y.-T.; Smotkin, E.S. The effect of plasticizers on transport and electrochemical properties of PEO-based electrolytes for lithium rechargeable batteries. Solid State Ion. 2002, 149, 29–37. [Google Scholar] [CrossRef]
- Naoi, K.; Mori, M.; Inoue, M.; Wakabayashi, T.; Yamauchi, K. Modification of the lithium metal surface by nonionic polyether surfactants. Ii. Investigations with microelectrode voltammetry and in situ quartz crystal microbalance. J. Electrochem. Soc. 2000, 147, 813–819. [Google Scholar] [CrossRef]
- Yoshida, K.; Nakamura, M.; Kazue, Y.; Tachikawa, N.; Tsuzuki, S.; Seki, S.; Dokko, K.; Watanabe, M. Oxidative-stability enhancement and charge transport mechanism in glyme–lithium salt equimolar complexes. J. Am. Chem. Soc. 2011, 133, 13121–13129. [Google Scholar] [CrossRef]
- Jung, H.G.; Hassoun, J.; Park, J.B.; Sun, Y.K.; Scrosati, B. An improved high-performance lithium-air battery. Nat. Chem. 2012, 4, 579–585. [Google Scholar] [CrossRef]
- Wang, H.; Im, D.; Lee, D.J.; Matsui, M.; Takeda, Y.; Yamamoto, O.; Imanishi, N. A composite polymer electrolyte protect layer between lithium and water stable ceramics for aqueous lithium-air batteries. J. Electrochem. Soc. 2013, 160, A728–A733. [Google Scholar] [CrossRef]
- Kříž, J.; Abbrent, S.; Dybal, J.; Kurková, D.; Lindgren, J.; Tegenfeldt, J.; Wendsjö, Å. Nature and dynamics of lithium ion coordination in oligo(ethylene glycol) dimethacrylate-solvent systems: NMR, Raman, and quantum mechanical study. J. Phys. Chem. A 1999, 103, 8505–8515. [Google Scholar] [CrossRef]
- Wang, H.; Imanishi, N.; Hirano, A.; Takeda, Y.; Yamamoto, O. Electrochemical properties of the polyethylene oxide–Li(CF3SO2)2N and ionic liquid composite electrolyte. J. Power Sources 2012, 219, 22–28. [Google Scholar] [CrossRef]
- Brissot, C.; Rosso, M.; Chazalviel, J.N.; Lascaud, S. Dendritic growth mechanisms in lithium/polymer cells. J. Power Sources 1999, 81, 925–929. [Google Scholar]
- Ma, Y.P.; Doyle, M.; Fuller, T.F.; Doeff, M.M.; Dejonghe, L.C.; Newman, J. The measurement of a complete set of transport-properties for a concentrated solid polymer electrolyte solution. J. Electrochem. Soc. 1995, 142, 1859–1868. [Google Scholar] [CrossRef]
- Evans, J.; Vincent, C.A. Electrochemical measurement of transference numbers in polymer electrolytes. Polymer 1987, 28, 2324–2328. [Google Scholar] [CrossRef]
- Bernhard, R.; Latini, A.; Panero, S.; Scrosati, B.; Hassoun, J. Poly(ethylene glycol)dimethylether-lithium bis(trifluoromethanesulfonyl)imide, PEG500DME-LiTFSI, as high viscosity electrolyte for lithium ion batteries. J. Power Sources 2013, 226, 329–333. [Google Scholar] [CrossRef]
- Aurbach, D. Review of selected electrode-solution interactions which determine the performance of Li and Li ion batteries. J. Power Sources 2000, 89, 206–218. [Google Scholar] [CrossRef]
- Zhang, T.; Imanishi, N.; Takeda, Y.; Yamamoto, O. Aqueous lithium/air rechargeable batteries. Chem. Lett. 2011, 40, 668–673. [Google Scholar] [CrossRef]
- Chazalviel, J.N. Electrochemical aspects of the generation of ramified metallic electrodeposits. Phys. Rev. A 1990, 42, 7355–7367. [Google Scholar] [CrossRef]
- Scrosati, B. Lithium Ion Plastic Batteries. In Lithium Ion Batteries: Fundamentals and Performance; Wakihara, M., Yamamoto, O., Eds.; Kodansha Ltd.: Tokyo, Japan, 1998; p. 221. [Google Scholar]
- Abraham, K.M.; Jiang, Z.; Carroll, B. Highly conductive PEO-like polymer electrolytes. Chem. Mater. 1997, 9, 1978–1988. [Google Scholar] [CrossRef]
© 2013 by the authors; licensee MDPI, Basel, Switzerland. This article is an open access article distributed under the terms and conditions of the Creative Commons Attribution license (http://creativecommons.org/licenses/by/3.0/).