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Materials Science » Polymers » "Conducting Polymers", book edited by Faris Yilmaz, ISBN 978-953-51-2691-1, Print ISBN 978-953-51-2690-4, Published: October 5, 2016 under CC BY 3.0 license. © The Author(s).

Chapter 11

Intercalation of Poly(bis-(methoxyethoxyethoxy)phosphazene) into Lithium Hectorite

By Iskandar Saada, Rabin Bissessur, Douglas C. Dahn and Matthieu Hughes
DOI: 10.5772/64580

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Structure of MEEP.
Figure 1. Structure of MEEP.
Structure of hectorite.
Figure 2. Structure of hectorite.
XRD data for (a) MEEP:Li-hectorite (0.5:1), (b) MEEP:Li-hectorite (2:1), and (c) MEEP:Li-hectorite (4:1).
Figure 3. XRD data for (a) MEEP:Li-hectorite (0.5:1), (b) MEEP:Li-hectorite (2:1), and (c) MEEP:Li-hectorite (4:1).
Schematic arrangement of MEEP in lithium hectorite (0.5:1).
Figure 4. Schematic arrangement of MEEP in lithium hectorite (0.5:1).
TGA data for (a) Li-MEEP:Li-hectorite (1:1), (b) MEEP:Li-hectorite(1:1), (c) MEEP, and (d) Li-MEEP.
Figure 5. TGA data for (a) Li-MEEP:Li-hectorite (1:1), (b) MEEP:Li-hectorite(1:1), (c) MEEP, and (d) Li-MEEP.
DSC data for (a) MEEP:Li-hectorite (1:1), (b) Li-MEEP:Li-hectorite (1:1), (c) MEEP, and (d) Li-MEEP.
Figure 6. DSC data for (a) MEEP:Li-hectorite (1:1), (b) Li-MEEP:Li-hectorite (1:1), (c) MEEP, and (d) Li-MEEP.
ATR results for (a) MEEP, (b) MEEP:Li-hectorite (1:1), (c) Li-MEEP, and (d) Li-MEEP:Li-hectorite(1:1).
Figure 7. ATR results for (a) MEEP, (b) MEEP:Li-hectorite (1:1), (c) Li-MEEP, and (d) Li-MEEP:Li-hectorite(1:1).
Complex-plane plot of Li-MEEP impedance at 300 K.
Figure 8. Complex-plane plot of Li-MEEP impedance at 300 K.
Variable-temperature ionic conductivity of Li-MEEP.
Figure 9. Variable-temperature ionic conductivity of Li-MEEP.

Intercalation of Poly(bis-(methoxyethoxyethoxy)phosphazene) into Lithium Hectorite

Iskandar Saada1, Rabin Bissessur1, Douglas C. Dahn2 and Matthieu Hughes2
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Poly(bis-(methoxyethoxyethoxy)phosphazene) (MEEP) intercalated into lithium hectorite was investigated for its potential application as a solid polymer electrolyte in lithium-ion polymer batteries. Varying amounts of MEEP were intercalated into lithium hectorite, and the physical properties of the nanocomposites were monitored using powder X-ray diffraction, thermogravimetric analysis, differential scanning calorimetry, and attenuated total reflectance spectroscopy. Alternating current (AC) impedance spectroscopy was used to determine the ionic conductivity of the nanocomposites when complexed with lithium triflate salt.

Keywords: lithium hectorite, poly(bis-(methoxyethoxyethoxy)phosphazene), nanocomposites, solid polymer electrolytes

1. Introduction

The electrolyte in a lithium-ion battery is the medium through which lithium ions flow between anode and cathode. It is electrically insulating, and thus prohibits the passage of electrons. Much work has been done to develop solid-state electrolyte materials such as solid polymer electrolytes (SPEs) which have the advantage of enhanced safety compared to conventional liquid organic electrolytes. Some of the most recent research on electrolyte materials has focused on utilizing polymers such as poly(ethylene oxide) (PEO) [1] and polyphosphazenes [2, 3]. Current research on polyphosphazenes focuses on exploiting their fire-resistant properties [4], ionic conductivity [5], and as phosphazene-based dye-sensitized solar cells [6]. Polyphosphazenes are amorphous polymers with low glass transition temperatures (Tg), which dictates their polymer-chain flexibility and aids in lithium-ion mobility [7].

Since the first report on poly(bis-(methoxyethoxyethoxy)phosphazene) (MEEP), Figure 1, an array of phosphazene-based polymers have been synthesized with diverse alkyl ether and alkoxy side groups, ultimately yielding ionically conductive polymers that are flexible. When polyphosphazenes such as MEEP are complexed with lithium salts (e.g., lithium triflate), they have been shown to possess enhanced ionic conductivity compared to PEO-based SPEs [8, 9]. Previous studies have reported that (MEEP)4LiCF3SO3 yields ionic conductivity in the range of 2 × 10−5 to 1 × 10−4 S/cm at ambient temperatures [10, 11]. However, the dimensional stability of MEEP is low, so it leaks out of cells at ambient temperatures. Researchers have attempted to enhance the dimensional stability of polyphosphazenes by investigating polymer blends with PEO [12], inducing cross-linking via 60Co-gamma irradiation [8] and preparing of polyphosphazene-silicate networks [13]. One other promising approach is the intercalation of polyphosphazenes into layered structures, which act as hosts for the polymers. Due to the weak electrostatic interactions holding the layers of two-dimensional structures, the layers may be exfoliated allowing for the intercalation of ionically conductive polymers. This yields nanocomposite materials with ionically conductive properties, along with enhanced mechanical and thermal durability provided by the layered structure. Intercalation of MEEP into two-dimensional layered structures has been investigated using layered structures such as graphite oxide [10], molybdenum disulfide [14], sodium montmorillonite [15], and sodium hectorite [16], and has typically yielded ionically conductive nanocomposite materials with enhanced physical properties. In this chapter, we report on the intercalation of various amounts of MEEP into lithium hectorite.


Figure 1.

Structure of MEEP.

Hectorite belongs to the family of smectite clays, and has a 2:1 structural arrangement composed of two tetrahedral silicate layers (Td) encompassing an octahedral layer (Oh), as shown in Figure 2 [17]. Their industrial applications range from pharmaceutical drug additives [18] to automobile parts [19], and potentially as SPEs in batteries [20, 21]. Hectorite has negatively charged layers, which are compensated with cations such as Na+ and Li+ to balance the overall charge. Hectorite is an appealing layered structure for the intercalation of MEEP due to its high thermal stability, high surface area, exfoliating/restacking capability, and high cation exchange capacity [22]. In this chapter, we exploit the cation exchange capability of hectorite by driving out the naturally lying sodium ions with lithium ions, and working with the lithiated form of hectorite [23]. The intercalation of varying stoichiometric molar ratios of MEEP was conducted with the lithiated form of hectorite.


Figure 2.

Structure of hectorite.

The aim of this chapter is to present the effects that varying polymeric molar ratios to Li-hectorite have on the physical properties of the synthesized nanocomposites, and to investigate the ionic conductivity of the salt-complexed nanocomposites. The synthesized nanocomposites were characterized using thermogravimetric analysis (TGA), differential scanning calorimetry (DSC), powder X-ray diffraction (XRD), and attenuated total reflectance (ATR). The ionic resistance of the materials was determined using AC impedance spectroscopy.

2. Experimental

2.1. Purification and lithiation of hectorite

Sodium hectorite (SHCa-1) was purchased from Source Clays Repository. Since the fine powder has calcium carbonate and other impurities, a purification process was performed as outlined in the literature [16]. When the purification process was complete, a cation exchange was done in order to replace the sodium ions with lithium ions [23]. This process was carried out twice to ensure maximum substitution of lithium ions. Elemental analysis was used to monitor the sodium- and lithium-ion content at Guelph Chemical Laboratories Ltd. Ontario, Canada. The data indicated an increase in lithium-ion proportion from Li0.5 Na0.8 Si1 (sodium hectorite) to Li3 Na0.4 Si1 (lithium hectorite).

2.2. Synthesis of MEEP and MEEP-salt complex

The synthesis of MEEP was performed as described in the literature [24]. (MEEP)4 LiCF3SO3 has been found to exhibit high ionic conductivity compared to other polymer:salt ratios [13, 25], so this polymer:salt ratio was used in this work. The synthesized polymer was stored in a vacuum desiccator, and salt-polymer complexes were used as soon as they were prepared in order to minimize exposure to humidity. Hereafter, the pure (uncomplexed) polymer will be referred to as MEEP, while the salt-complexed polymer will be referred to as Li-MEEP.

2.3. Preparation of nanocomposites

A general procedure was employed for the intercalation of MEEP into Li-hectorite. Li-hectorite (0.10 g, 2.6 × 10-4 mol) was suspended in deionized water and left to stir until fully suspended in water (typically 30 min). The polymer with molar ratio of 0.5, 1, 2, or 4 to Li-hectorite was dissolved in 5 mL of deionized water. A pipette was used to transfer the polymer solution to the Li-hectorite suspension at a rate of one drop per second. The progress of the reactions was monitored via XRD. The products were then isolated via freeze drying, and stored in a vacuum desiccator.

2.4. Materials characterization

Powder X-ray diffraction was conducted on a Bruker AXS D8 Advance diffractometer. The instrument is equipped with a graphite monochromator, variable divergence slit, variable antiscatter slit, and a scintillation detector. Cu (kα) radiation (λ = 1.542 Å) was utilized and the data were collected at room temperature on glass substrates.

Thermogravimetric analysis (TGA) was performed on a TA Q500 using a heating rate of 10°C/min, with the use of platinum pans under dry-compressed air. Samples were freeze dried prior to TGA analysis in order to minimize their moisture content.

Differential scanning calorimetry (DSC) was performed on a TA Q100 using heat/cool/heat cycles. Samples were crimped in aluminum pans, and ran under nitrogen flow at a rate of 50 mL/min.

Attenuated total reflectance spectroscopy (ATR) data were collected using a Bruker Alpha A-T (resolution 0.9, 128 scans).

AC impedance spectroscopy (IS) was conducted to determine the ionic conductivity of the salt-complexed materials [26]. The samples were tested using rectangular glass substrates with two rectangular stainless steel electrodes on the opposite ends of the substrates. For the intercalated nanocomposites, samples were cast onto the substrates, between the electrodes, after 3 days of reaction time in order to ensure complete intercalation. Typical samples had a width of about 9 mm, were 20–90-μm thick, and had a length between the electrodes in the direction of current of about 6 mm. In most cases, the films were not uniform in thickness, and this was the main source of uncertainty in the ionic conductivity values that were obtained. The frequency range used was 10 kHz to 0.01 Hz. In order to remove moisture, the samples were placed under vacuum for at least 24 h at room temperature prior to the data collection. The temperature of the samples was controlled using a Cryodyne 350CP refrigerator and a Lakeshore 321 temperature controller. The data collection was performed using a Solartron 1250 frequency response analyzer and a home-built accessory circuit for high-impedance samples. The conductivity was then determined by fitting the IS data to an equivalent circuit model using LEVMW [27].

3. Results and discussion

3.1. MEEP/Lithium hectorite

3.1.1. Powder X-ray diffraction

Powder X-ray diffraction was used to monitor the intercalation process and the effect of the molar ratio of MEEP to Li-hectorite on the polymer loading in the layered structure.


Figure 3.

XRD data for (a) MEEP:Li-hectorite (0.5:1), (b) MEEP:Li-hectorite (2:1), and (c) MEEP:Li-hectorite (4:1).

The diffractograms for MEEP:Li-hectorite (0.5:1), MEEP:Li-hectorite (2:1), and MEEP:Li-hectorite (4:1) nanocomposites are displayed in Figure 3 to illustrate the enhancement in basal spacing (d-spacing) of the layered host upon the intercalation of MEEP. The net interlayer expansion is obtained by subtracting the basal spacing of dry Li-hectorite heated to 650°C (d-spacing = 9.5 Å) from the basal spacing of the synthesized nanocomposite. For example, MEEP:Li-hectorite (0.5:1) nanocomposite has a basal spacing of 18.9 Å, which corresponds to an interlayer expansion of 9.40 Å. The XRD data for all the nanocomposites are summarized in Table 1.

MaterialBasal spacing (Å)Net expansion (Å)Average crystallite size (Å)
MEEP:Li-hectorite (0.5:1)18.99.4073
MEEP:Li-hectorite (1:1)21.712.274
MEEP:Li-hectorite (2:1)36.426.9126
MEEP:Li-hectorite (4:1)41.532.0135
Dry Li- hectorite9.50182

Table 1.

Summary XRD data of hectorites and MEEP:Li-hectorite nanocomposites.

The synthesized nanocomposites are crystalline as indicated by XRD, and a significant increase in basal spacing is observed as the ratio of MEEP to Li-hectorite is increased. From the XRD diffractograms of the nanocomposites, the average crystallite size was determined using the Scherrer formula [28]. The crystallite size appeared to increase upon increasing the MEEP molar ratio to Li-hectorite, which is possibly due to the significant enhancement in basal spacing upon loading of the polymer into the layered structure.


Figure 4.

Schematic arrangement of MEEP in lithium hectorite (0.5:1).

The dimensions of MEEP were estimated using Spartan ’08. The average dimension was determined for the largest possible distance between the ether oxygens on the R-groups in MEEP, and was found to be approximately 7.9 Å for one unit of MEEP [29]. This indicates that a single layer of MEEP is inserted between the Li-hectorite sheets for the MEEP:Li-hectorite (0.5:1) nanocomposite, which had a net layer expansion of 9.40 Å. The difference of 1.5 Å between the observed basal spacing of the 0.5:1 nanocomposite and the calculated dimensions of MEEP could be due to the manner in which MEEP is oriented within the layers. MEEP is a highly flexible polymer and may not necessarily be oriented within the layers as depicted in Figure 4. For example, a helical conformation may also be possible.

3.1.2. Thermogravimetric analysis

Thermogravimetric analysis was used to compare the thermal stability of MEEP, MEEP:Li-hectorite, Li-MEEP, and Li-MEEP:Li-hectorite. This was completed in order to monitor the thermal stability of nanocomposites with different polymer concentrations and to compare the stability of salt-complexed materials with their uncomplexed counterparts. The MEEP:Li-hectorite thermograms were also used to calculate the stoichiometry of the synthesized nanocomposites.

The thermogram of pristine MEEP (Figure 5(c)) shows that it undergoes a major decomposition between 230 and 350°C, followed by an onward gradual weight loss. Once MEEP is complexed with lithium triflate (LiCF3SO3), its decomposition is slightly compromised due to the presence of the inorganic salt, which appeared to decrease the polymer onset decomposition temperature by approximately 30°C; thereafter, complete decomposition of the triflate salt is observed at 420°C (Figure 5(d)).


Figure 5.

TGA data for (a) Li-MEEP:Li-hectorite (1:1), (b) MEEP:Li-hectorite(1:1), (c) MEEP, and (d) Li-MEEP.

Upon polymer intercalation, the nanocomposite thermograms appeared to have three weight loss steps, where the thermogram of, for example, MEEP:Li-hectorite (1:1) (Figure 5(b)) illustrates a small loss of water near 100°C, followed by the decomposition at 178°C corresponding to the presence of externally lying MEEP. The final decomposition is the gradual decomposition of the intercalated MEEP occurring at 305°C. This is quite similar to the thermal behavior of Li-MEEP:Li-hectorite (1:1) (Figure 5(a)), except for the decomposition of the salt which occurs at around 420°C. The TGA data are summarized in Table 2.

MaterialTa (°C)Tb (°C)ΔTc (°C)
MEEP:Li-hectorite (0.5:1)20531272
MEEP:Li-hectorite (1:1)17830565
MEEP:Li-hectorite (2:1)17631575
MEEP:Li-hectorite (4:1)17032484

Table 2.

Thermogravimetric data.

Ta, onset decomposition temperature of pure MEEP or externally lying MEEP in nanocomposite; Tb, onset decomposition temperature of intercalated MEEP in nanocomposite; and ΔTc, difference in decomposition temperature of the intercalated MEEP and pristine MEEP.

As shown in Table 2, the onset decomposition temperatures of the externally lying MEEP (Ta) in the nanocomposites were lower than that of the bulk polymer, which occurs at 240°C. However, the onset decomposition temperatures of the intercalated MEEP (Tb) in the nanocomposites are significantly higher than that of the pure polymer, indicating enhancement in the thermal stability of polymer when sandwiched between the layers of hectorite.

MEEP:Li-hectorite (mol ratio)Stoichiometry
0.5:1(H2O)0.61 (MEEPExt)0.17 (MEEPIn)0.023(Li-hectorite)
1:1(H2O)0.42 (MEEPExt)0.44 (MEEPIn)0.073(Li-hectorite)
2:1(H2O)0.48 (MEEPExt)0.71(MEEPIn)0.12(Li-hectorite)
4:1(H2O)0.34 (MEEPExt)0.84 (MEEPIn)0.14(Li-hectorite)

Table 3.

Stoichiometry of MEEP:Li-hectorite nanocomposites.

Since the nanocomposites displayed three decomposition steps, the stoichiometry was calculated in order to compare the spread between externally lying and intercalated polymer. It is important to note that the stoichiometry was calculated only for the MEEP:Li-hectorite nanocomposites, and not for the Li-MEEP:Li-hectorite nanocomposites due to the presence of lithium salt. The stoichiometry data of the nanocomposites are displayed in Table 3.

As shown in Table 3, when the molar ratio of MEEP is increased with respect to Li-hectorite, there is an increase in the amount of the externally lying polymer and intercalated polymer. These observations are in agreement with the XRD data (Table 1), which indicate that the basal spacing of the intercalated nanocomposite increases when the amount of MEEP is increased. In fact, MEEP:Li-hectorite (4:1) has almost twice as much of the intercalated polymer compared to MEEP:Li-hectorite (1:1).

3.1.3. Differential scanning calorimetry

Differential scanning calorimetry was used to monitor the glass transition temperature (Tg) of pristine MEEP, Li-MEEP, and their corresponding synthesized nanocomposites (Figure 6).


Figure 6.

DSC data for (a) MEEP:Li-hectorite (1:1), (b) Li-MEEP:Li-hectorite (1:1), (c) MEEP, and (d) Li-MEEP.

Material(Tg, oC)
MEEP:Li-hectorite (0.5:1)
MEEP:Li-hectorite (1:1)
MEEP:Li-hectorite (2:1)
MEEP:Li-hectorite (4:1)

Table 4.

Summary of DSC data.

The DSC of pure MEEP indicates a Tg of −71°C, which is in fairly good agreement with the previously reported literature value of −83°C [30]. Upon complexing MEEP with lithium triflate (LiCF3SO3), the glass transition temperature (Tg) significantly increases to −28°C due to the crystalline nature of lithium triflate. However, upon intercalation of pristine MEEP or Li-MEEP into Li-hectorite, a Tg is not observed for the ratios used. Due to the lack of glass transition temperatures in both Li-MEEP:Li-hectorite and MEEP:Li-hectorite nanocomposites, it is believed that (1) the oxygen atoms of the polymer are potentially interacting with the tetrahedrally coordinated silicon atoms in the hectorite sheets and restricting chain mobility or (2) the polymer is no longer flexible when it is intercalated in the layers of hectorite. The glass transition temperatures are displayed in Table 4.

3.1.4. Attenuated total reflectance

ATR spectroscopy was used to monitor the bond vibrations in MEEP, MEEP:Li-hectorite, Li-MEEP, and Li-MEEP:Li-hectorite. More specifically, it was important to determine whether intercalating MEEP or Li-MEEP into Li-hectorite hinders the flexibility of the polymer, and ultimately its ionic conductivity (Figure 7).


Figure 7.

ATR results for (a) MEEP, (b) MEEP:Li-hectorite (1:1), (c) Li-MEEP, and (d) Li-MEEP:Li-hectorite(1:1).

Major vibrations (cm−1)MEEPMEEP:Li-hectorite(1:1)Li-MEEPLi-MEEP:Li-hectorite(1:1)
HOH stretchN/A3686N/A3624
Sp3 C-H stretch/bend2877/14572883/14572896/14572887/1457
C-O-C ether1199–104312011170–10361189
PNP skeletal849/803/753848/801/757855/766798/768
C-F deformationN/AN/A638638
SO3 asymmetric bendN/AN/A573573
SO3 symmetric bendN/AN/A518518

Table 5.

Summary of IR data.

From the IR data, it is observed that the P = N vibration in the pure polymer occurs at 1243 cm-1. Upon complexation with lithium triflate, the P = N vibration of the polymer shifts to 1251 cm-1, and to 1257 cm-1 in the synthesized nanocomposites. This increase in vibrational energy of the P = N bond is indicative of the increased rigidity of the polymer backbone. The P-O-C vibration in MEEP shifts from 959 to 967 cm-1 upon intercalation into Li-hectorite, indicating increased rigidity of the polymer side chains. Thus, the IR data support lack of polymer flexibility upon intercalation, and are in very good agreement with the DSC results. The IR data are summarized in Table 5 [8].

3.1.5. AC impedance spectroscopy

Impedance measurements were conducted on Li-MEEP and the Li-MEEP:Li-hectorite nanocomposites. Since the DSC and IR data indicated that the polymer-chain flexibility was restricted in the nanocomposites, it was necessary to investigate the ionic conductivity properties of Li-MEEP prior to intercalation, and post-intercalation. A complex plane plot of the impedance of an Li-MEEP sample is given in Figure 8. High-frequency data (10 kHz) is near the origin, and low-frequency (0.01 Hz) at the upper right.


Figure 8.

Complex-plane plot of Li-MEEP impedance at 300 K.

As shown in Figure 8, Li-MEEP demonstrates a curve typical for an ionic conductor. The value of Re(Z) at which Im(Z) goes through a minimum (about 7 × 107 Ω in Figure 8) corresponds approximately to the resistance (R) of the sample. The value of R and the dimensions of the polymeric film were used to calculate the ionic conductivity of the sample. In order to obtain more accurate values of R from the impedance data, a complex nonlinear least-squares fit was done with an equivalent circuit model using the program LEVMW [27]. A three-component equivalent circuit consisting of a resistor (R), a constant-phase element (CPE) that models the effects of the blocking electrodes, and a parallel capacitor (C) was used and is shown in the inset of Figure 8. Using the resistance value R and the dimensions of the polymeric film, the ionic conductivity of Li-MEEP was calculated.

Ionic conductivity measurements were performed within the temperature range of 220–310 K, and the results for a typical Li-MEEP sample are displayed in Figure 9. As is typical for ionically conducting polymers, the conductivity drops rapidly as the temperature is reduced, and for this sample it was too small to be measured with our system below 260 K.


Figure 9.

Variable-temperature ionic conductivity of Li-MEEP.

The room temperature ionic conductivity of Li-MEEP samples ranged from about 4 × 10-6 to 1.3 × 10-5 S/cm, which is in agreement with the literature [11, 12]. However, upon intercalation of Li-MEEP into Li-hectorite, the conductivity of the resulting nanocomposite material was below our detection limit, which in the case of these cast film samples is about 10-7 S/cm. These observations further indicate that there is an interaction occurring between the polymer and the layered structure that is ultimately inhibiting the nanocomposites from conducting lithium ions.

4. Conclusions

MEEP has been intercalated into Li-hectorite. A series of nanocomposites have been created by varying the mole ratio of the polymer with respect to the clay. The nanocomposites were characterized by TGA, DSC, FTIR, XRD, and AC impedance spectroscopy. XRD data confirm the successful and complete intercalation of MEEP into the layered silicate. TGA data confirm that increasing the molar ratio of MEEP with respect to the Li-hectorite results in a larger amount of the polymer within the layers. In fact, MEEP:Li-hectorite (4:1) has approximately twice the amount of intercalated polymer versus MEEP:Li-hectorite (1:1). TGA also indicates an enhancement in thermal stability of the intercalated polymer versus the pristine polymer for all nanocomposites. For instance, the intercalated polymer in MEEP:Li-hectorite (1:1) is thermally stable up to 305°C, while the pure polymer decomposes at 240°C. The room temperature ionic conductivity of Li-MEEP was determined to be about 1 × 10-5 S/cm; however, the polymer-salt complex displayed high ionic resistance when intercalated into Li-hectorite, and hence the ionic conductivity of the nanocomposites was too small to be determined (below about 10-7 S/cm). The impedance data are in good agreement with the DSC results, where no glass transition temperature has been detected for all the synthesized nanocomposites. ATR spectroscopy also confirms that the rigidity of the polymer backbone increases upon complexation with lithium triflate, and when the lithium complexed MEEP is intercalated into Li-hectorite.


The authors are grateful for the financial support from the Natural Sciences and Engineering Research Council (NSERC) of Canada, Canada Foundation for Innovation (CFI), Atlantic Innovation Fund of Canada (AIF), and UPEI.


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