# [MG49-LiClO4]:[TiO2-SiO2] Polymer Electrolytes: In Situ Preparation and Characterization

Authors: Oon Lee Kang; Azizan Ahmad; Nur Hasyareeda Hassan; Usman Ali Rana
Journal: International Journal of Polymer Science
 (2016)

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## Abstract

In the present research, [MG49-LiClO4]:[HNO3-THF/TiO2-SiO2] and [MG49-LiClO4]:[ClHNO2-THF/TiO2-SiO2] polymer electrolytes were first prepared through simple stepwise in situ techniques: sol-gel technique and solution-cast technique. [MG49-LiClO4]:[HNO3-THF/TiO2-SiO2] and [MG49-LiClO4]:[ClHNO2-THF/TiO2-SiO2] polymer electrolytes were then characterized through different experimental techniques. [MG49-LiClO4]:[HNO3-THF/TiO2-SiO2] and [MG49-LiClO4]:[ClHNO2-THF/TiO2-SiO2] polymer electrolytes had exhibited significant structural changes upon different salt concentrations. In the present investigation, [MG49-LiClO4]:[HNO3-THF/TiO2-SiO2] and [MG49-LiClO4]:[ClHNO2-THF/TiO2-SiO2] polymer electrolytes had attained maximum ionic conductivities (σ
~
10
-
7 S/cm at ambient temperature; 10−4 S/cm at 100°C) upon 25 wt.% salt insertion. [MG49-LiClO4]:[HNO3-THF/TiO2-SiO2] and [MG49-LiClO4]:[ClHNO2-THF/TiO2-SiO2] polymer electrolytes had exhibited distinct conduction mechanisms in similar experimental configuration. [MG49-LiClO4]:[HNO3-THF/TiO2-SiO2] and [MG49-LiClO4]:[ClHNO2-THF/TiO2-SiO2] polymer electrolytes had exhibited different stability characteristics over certain operational condition.


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## Body

## 1. Introduction

Nanocomposite polymer electrolytes are major breakthrough in solid-state electrochemical technologies [1]. PEO-LiClO4-α-alumina polymer electrolytes were first developed in the early 1980s; recent empirical studies have focused attention on solid-state electrochemical behavior [2, 3].Nanocomposite polymer electrolytes have shown tremendous potential in solid-state electrochemical applications. Nanocomposite polymer electrolytes are critical component in solid-state electrochemical systems [4]. Nanocomposite polymer electrolytes can serve important function as ionic conduction medium. Nanocomposite polymer electrolytes can serve another function as mechanical support barrier.Nanocomposite biopolymer electrolytes have attained precedence over conventional electrolytes [5]. Such predominant phenomenon is considered attributable to their characteristic properties: renewable; biodegradable; biocompatible; derivatizable; and so forth. Modified natural rubber-lithium salt-silica nanoparticle biopolymer electrolytes are often reported in the electrochemical literature [6]. Rice starch-ionic liquid-titania nanoparticle biopolymer electrolytes are also reported in the relevant literature [7].Nanocomposite biopolymer electrolytes are often characterized as high electrochemical performance [8]. Nanocomposite biopolymer electrolytes are custom tailored to specific electrochemical characteristics: adequate ionic conductivities; negligible electronic conduction; and insignificant activation energies. Even so, some practical limitations are still encountered in solid-state electrochemical applications [9].Nanocomposite biopolymer electrolytes are often obtained through ex situ techniques (i.e., dispersion techniques). Nanocomposite biopolymer electrolytes are also derived from sol-gel techniques [10].Nanocomposite biopolymer electrolytes are often considered as multicomponent structures. In the present case, 49% poly(methyl methacrylate) grafted natural rubber (MG49) is also selected as polymer host. MG49 is best regarded as superior host: excellent solvation capabilities; unique transportation properties; and superior mechanical properties [11]. Lithium perchlorate (LiClO4) is more favorable than other lithium salts. LiClO4 is therefore selected as dopant salt. LiClO4 is often identified as ideal ionic salt: superior dissociative abilities; insignificant resistive characteristics; and least electronegative characteristics. Titania-silica (TiO2-SiO2) nanoparticles are further implemented as ceramic filler. TiO2-SiO2 nanoparticles have significant roles in simultaneous stabilization and performance improvement. TiO2-SiO2 nanoparticles are not involved in lithium transportation process.[MG49-LiClO4]:[HNO3-THF/TiO2-SiO2] and [MG49-LiClO4]:[ClHNO2-THF/TiO2-SiO2] polymer electrolytes were first prepared through simple stepwise in situ technique: sol-gel technique and solution-cast technique. [MG49-LiClO4]:[HNO3-THF/TiO2-SiO2] and [MG49-LiClO4]:[ClHNO2-THF/TiO2-SiO2] polymer electrolytes were then characterized through different experimental techniques.


## 2. Experimental

### 2.1. Material Preparation

MG49 was purchased from Green HPSC Malaysia Sdn Bhd. LiClO4 was purchased from Sigma-Aldrich Corporation. Metal precursors were purchased from Sigma-Aldrich Corporation. Chemical reagents were used as received unless stated otherwise.


### 2.2. Process Description

[MG49-x wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and [MG49-x wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes were prepared through simple stepwise in situ technique: sol-gel technique and solution-cast technique. TiO2-SiO2 (70 : 30) sol particles were prehydrolysed in different catalyst-solvent systems: HNO3-THF and ClHNO2-THF systems. TiO2-SiO2 (70 : 30) sol particles were introduced into preformed MG49-LiClO4 matrices. Resultant reaction mixtures were stirred 1/2 hours at ambient temperature. Homogeneous reaction mixtures were cast into Teflon petri dishes. Resultant thin films were dried in vacuum oven.


### 2.3. Polymer Electrolyte Characterization

XRD analyses were conducted on a Bruker D8 Advance diffractometer (Bruker AXS GmbH, Germany). XRD patterns were acquired in the Bragg-Brentano configuration. XRD patterns were recorded in the2
θ range (15–60°; step size 0.02°).IR analyses were conducted on a Perkin-Elmer Spectrum 400 spectrometer (Perkin Elmer, UK). Infrared spectra were acquired in the attenuated total reflectance (ATR) mode. Infrared spectra were recorded in the mid infrared range (4000–650 cm−1; spectral resolution 4 cm−1).EIS analyses were conducted on a Solartron Schlumberger SI 1286 potentiostat (Solartron Schlumberger, Farnborough, England). Impedance spectra were acquired in the alternative current (AC) modulation. Impedance spectra were recorded in the medium frequencies region (1 Hz–1 kHz).SEM analyses were conducted on a LEO 1450 VP instrument (Carl Zeiss, Oberkochen, Germany). SEM micrographs were acquired in the backscattered electrons (BSE) mode. SEM micrographs were taken at moderate acceleration voltage (15–20 kV).TGA analyses were conducted on a Shimadzu TGA-50 instrument (Shimadzu, Japan). TGA scans were recorded in a broad temperature range (room temperature to 600°C; scan rate 10°C min−1).DRA analyses were conducted on Anton Paar Physica MCR 501 rheometer (Anton Paar GmbH, Graz, Austria). DRA analyses were performed at isothermal condition. DRA responses were acquired in a dynamic oscillation mode.


## 2.1. Material Preparation

MG49 was purchased from Green HPSC Malaysia Sdn Bhd. LiClO4 was purchased from Sigma-Aldrich Corporation. Metal precursors were purchased from Sigma-Aldrich Corporation. Chemical reagents were used as received unless stated otherwise.


## 2.2. Process Description

[MG49-x wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and [MG49-x wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes were prepared through simple stepwise in situ technique: sol-gel technique and solution-cast technique. TiO2-SiO2 (70 : 30) sol particles were prehydrolysed in different catalyst-solvent systems: HNO3-THF and ClHNO2-THF systems. TiO2-SiO2 (70 : 30) sol particles were introduced into preformed MG49-LiClO4 matrices. Resultant reaction mixtures were stirred 1/2 hours at ambient temperature. Homogeneous reaction mixtures were cast into Teflon petri dishes. Resultant thin films were dried in vacuum oven.


## 2.3. Polymer Electrolyte Characterization

XRD analyses were conducted on a Bruker D8 Advance diffractometer (Bruker AXS GmbH, Germany). XRD patterns were acquired in the Bragg-Brentano configuration. XRD patterns were recorded in the2
θ range (15–60°; step size 0.02°).IR analyses were conducted on a Perkin-Elmer Spectrum 400 spectrometer (Perkin Elmer, UK). Infrared spectra were acquired in the attenuated total reflectance (ATR) mode. Infrared spectra were recorded in the mid infrared range (4000–650 cm−1; spectral resolution 4 cm−1).EIS analyses were conducted on a Solartron Schlumberger SI 1286 potentiostat (Solartron Schlumberger, Farnborough, England). Impedance spectra were acquired in the alternative current (AC) modulation. Impedance spectra were recorded in the medium frequencies region (1 Hz–1 kHz).SEM analyses were conducted on a LEO 1450 VP instrument (Carl Zeiss, Oberkochen, Germany). SEM micrographs were acquired in the backscattered electrons (BSE) mode. SEM micrographs were taken at moderate acceleration voltage (15–20 kV).TGA analyses were conducted on a Shimadzu TGA-50 instrument (Shimadzu, Japan). TGA scans were recorded in a broad temperature range (room temperature to 600°C; scan rate 10°C min−1).DRA analyses were conducted on Anton Paar Physica MCR 501 rheometer (Anton Paar GmbH, Graz, Austria). DRA analyses were performed at isothermal condition. DRA responses were acquired in a dynamic oscillation mode.


## 3. Result and Discussion

### 3.1. Structural Characterization

X-ray diffraction patterns are shown in Figure1. Several broad humps were observed at 2
θ
=
15, 30, and 45°. Such broad humps are attributed to semicrystalline nature [12]. In fact, polyether side chain is still present in semicrystalline structure.Figure 1
X-ray diffraction patterns: (a) [MG49-x wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and (b) [MG49-x wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes.
(a)
(b)Characteristic broad hump (2
θ
=
15
°) had become flattened upon Li-salt insertion. Such predominant phenomenon is attributed to structural distortion. Characteristic broad hump is shifted upon Li-salt insertion. Characteristic broad hump is shifted to high 2-theta angle. Such predominant phenomenon is attributed to configurational alternation [13].LiClO4 diffraction peaks were apparent at high salt concentration (30 wt.% salt insertion). LiClO4 diffraction peaks were observed at 2
θ
=
13.5, 21.1, 23.3, 31.7, 33.1, 35.7, 39.5, 47.3, 49.3, 52.3, 58.1, and 63.1°. Such diffraction peaks are attributed to ionic association. In the literature, pure LiClO4 diffraction peaks were observed at 2
θ
=
12.1, 13.5, 21.1, 23.3, 31.7, 33.1, 35.7, 39.5, 47.3, 49.3, 52.3, 58.1, and 63.1°.LiClO4 diffraction signals are less intense in [MG49-x wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] polymer electrolytes. Such preference phenomenon is attributed to strong interfacial polarization. In general, Li+ cation solvation is dependent on interfacial interaction [14].IR absorption spectra are shown in Figure2. IR absorption spectra are comparable to earlier reports. Major absorption features were detected in such vibrational regions: 3400–3600 cm−1 (hydroxyl stretch); 2960–2860 cm−1 (methyl stretch); 1750–1730 cm−1 (carbonyl stretch); and 1250–950 cm−1 (ether stretch).Figure 2
IR absorption spectra: (a) [MG49-x wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and (b) [MG49-x wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes.
(a)
(b)Hydroxyl absorption band had become apparent upon Li-salt insertion. Hydroxyl absorption band had split into two distinct peaks (3560 and 3525 cm−1). Such interference phenomenon is attributed to intramolecular hydroxyl-hydroxyl interaction. Broad shoulder band was observed at 3380 cm−1. Such shoulder band is attributed to intermolecular hydroxyl-carbonyl interaction.Carbonyl absorption band had become broadened upon Li-salt insertion. Such preference phenomenon is attributed to significant C=O-Li+ complexation.Ether absorption bands were observed at different vibrational modes:ν(C-O), ν
s(C-O-C), ν
a
s(C-O-C), and δ(O-CH3) (as shown in Figure 3). Ether absorption band is shifted upon Li-salt insertion.Figure 3
Isoprene/methyl methacrylate monomeric structure.LiClO4 absorption bands were apparent at high salt concentration. LiClO4 absorption band was observed at 1065 cm−1. Such absorption bands are attributed to ionic association. In the literature, pure LiClO4 absorption bands were observed at 1150–1080 cm−1. Li+ absorption band was observed at 940 cm−1; C
l
O
4
- absorption band was observed at 625 cm−1. Surface hydroxyl absorption bands were apparent at high salt concentration. Surface hydroxyl absorption band was observed at 1630 cm−1. Such hydroxyl absorption band is attributed to hygroscopic properties.


### 3.2. Electrochemical Characterization

Ionic conductivities were determined through electrochemical impedance technique. Ionic conductivities are correlated with Ohm’s law. Ionic conductivities are regulated through multiple parameters: carrier charge, carrier concentration, and carrier mobility. Ionic conductivities are presented in Table1. Ionic conductivities are derived from the formula: (1)
σ
=
1
R
B
×
l
A
,where σ is conductivity (S·cm−1); R
B is bulk resistance; l is thickness (cm); A is the cross-sectional area (cm2).Table 1
LiClO4 salt concentration-dependence ionic conductivities (S/cm) at room temperature.
LiClO4 (wt.%)
Ionic conductivity (S/cm)
[MG49-x wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2]
[MG49-x wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2]
0
1.19 × 10−11
1.19 × 10−11
5
1.63 × 10−11
1.74 × 10−11
10
1.35 × 10−10
2.04 × 10−10
15
4.69 × 10−9
1.08 × 10−9
20
3.09 × 10−7
1.60 × 10−8
25
5.86 × 10−7
4.83 × 10−7
30
6.01 × 10−9
4.24 × 10−9Impedance characteristic curves are shown in Figure4. Small distorted semicircle was observed in high frequency region. Such distorted semicircle is attributed to bulk properties, that is, bulk ionic resistance and/or grain boundary resistance. Single distorted semicircle is correlated with ionic contribution dominate. Slanted spike was observed in low frequency region. Slanted spike is attributed to electrode interface properties [15].Figure 4
Impedance characteristic curves: (a) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and (b) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes.
(a)
(b)Ionic conductivities had increased upon Li-salt insertion. Such predominant phenomenon is attributed to mobile charge carrier increment [16]. Ionic conductivities had attained maximum value at 25 wt.% salt insertion. Such preference phenomenon is ascribed to maximum C=O-Li+ complexation. In general, ionic transport process is mediated through strong hard-acid/hard-base interaction [17].Ionic conductivities had decreased beyond 25 wt.% salt insertion. Such predominant phenomenon is attributed to short interionic distance. In general, ionic transport process is hindered upon ionic aggregation, that is, ionic pairs (Li+⋯C
l
O
4
-) and/or ionic triplets formation. In addition, ionic transport process is hindered upon transient cross-link network formation.In this case, however, ionic conductivities were not comparable to previous reports. Ionic conductivities are suppressed upon rotational hindrance. Such predominant phenomenon is correlated with interparticle interaction. Ionic conductivities were also high in [MG49-x wt.% LiBF4]:[50 wt.% EC]:[6 wt.% TiO2] polymer electrolytes. Ionic conductivities are enhanced upon plasticization effect. Such predominant phenomenon is correlated with free volume increment.Ionic conductivities had increased upon temperature increment (as shown in Figure5). Such preference phenomenon is attributed to free volume increment. In general, ionic diffusional motion is enhanced upon free volume increment. In addition, local segmental relaxation is enhanced upon free volume increment. Main structural relaxation is subjected through rapid internal motion (i.e., significant rotational transition).Figure 5
Temperature-dependence ionic conductivities: (a) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and (b) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes.
(a)
(b)l
o
g
σ versus 1000/T plot is almost linear in [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] polymer electrolyte. In such a case, Arrhenius behavior is predominant throughout the entire temperature range. Arrhenius behavior is described through the relation: (2)
σ
=
σ
0
exp
⁡
-
E
a
R
T
,where σ is conductivity (S·cm−1); σ
0 is preexponential factor (S·cm−1); E
a is activation energy (J·mol−1); R is perfect gas constant (8.314 J·mol−1·K−1); and T is absolute temperature (K). In the present case, hysteresis phenomenon is not observed at high temperature range.Ionic transport process is mediated through point defect movement. Schematic diagram is shown in Figure6. Ionic transport process does take place in the empty sites, either vacant or interstitial sites.Figure 6
Grain lattice diffusion: (a) substitutional diffusion and (b) interstitial diffusion.
(a)
(b)l
o
g
σ versus 1000/T plot is polynomial in [MG49-25.0 wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolyte. In such a case, VTF behavior is revealed in the entire temperature range. VTF behavior is described through the relation: (3)
σ
=
σ
0
exp
⁡
-
B
T
-
T
0
,where σ is ionic conductivities (S·cm−1); σ
0 is preexponential factor (S·cm−1); B is pseudo activation energy (J·mol−1); T is experimental temperature (K); and T
0 is reference temperature (K). Continuous curvature is indicative to cooperative mechanisms: segmental relaxation and/or interfacial defect interaction.Ionic transport process is facilitated through segmental relaxation. Critical transport behavior is correlated with segmental Brownian motion. Schematic diagram is shown in Figure7. Ionic transport process does take place in amorphous region [18].Figure 7
Local segmental motion: (a) intrachain motion and (b) interchain motion.
(a)
(b)Ionic transport process is induced through interfacial defect interaction. Critical transport behavior is correlated with interfacial site percolation [19]. Schematic diagram is shown in Figure 8. Ionic transport process does take place in space charge regions.Figure 8
Grain boundary diffusion: (a) intrachain diffusion and (b) interchain diffusion.
(a)
(b)Distinct conductivities (P
>
0.05) were observed in [MG49-x wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and [MG49-x wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes. Distinct conductivities are attributed to several fundamental factors: heterophase interface structures and relative dissociation degree.Cyclic voltammetric curves are shown in Figure9. Pseudo-elliptic curve was observed in fast scan rate. Such feature is denoted as ideal capacitive properties. Redox peaks were not detected in the entire potential range (−0.5–0.5 Volts). Such feature is attributed to nonfaradic process.Figure 9
Cyclic voltammetric curves: (a) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and (b) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes.
(a)
(b)Broad coverage area was observed in [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] polymer electrolyte. Broad coverage area is attributed to large current efficiencies. Such preference phenomenon is associated with better capacitive behavior.


### 3.3. Morphological Characterization

SEM micrographs are shown in Figure10. SEM micrographs were taken at 10,000x magnification. Uneven structure was observed throughout entire fracture surface. Uneven structure is ascribed to polymer-salt complexation.Figure 10
SEM micrographs: (a) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and (b) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes.
(a)
(b)Irregular aggregate structure was observed throughout entire fracture surface. Irregular aggregate structure is discerned in uniform bright contrast. Irregular aggregate structure is distributed in a random fashion.Nanoparticle dispersion state can exert influence on microstructure growth. Distinct morphological features were observed in [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and [MG49-25.0 wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes. Continuous phase structure was observed in [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] polymer electrolyte. Continuous phase structure is attributed to crystallization retardation. Fine crack structure was observed in [MG49-25.0 wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolyte. Fine crack structure is attributed to salt aggregation.


### 3.4. Thermal Characterization

Thermal stabilities are important parameter in performance appraisal [20]. Thermal stabilities were investigated through simultaneous thermogravimetric and differential thermal analysis.Thermal degradation curves are shown in Figure12. Similar degradation pattern was observed in [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and [MG49-25.0 wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes.Initial degradation stage was observed around 80–100°C. Such degradation stage is ascribed to moisture (and residual solvent) elimination. Large mass loss is not detected until irreversible decomposition. In this case, however, minor mass loss was observed at lower temperature range. Such interference phenomenon is associated with TiO2-SiO2 catalytic effects.Distinct degradation phases were detected at high temperature region (as shown in DTG curves). Such endothermic peaks are ascribed to thermal oxidative decomposition. First degradation step was observed around 270–290°C. Such degradation step is attributed to polymer chain decomposition. Transient degradation process is initiated through different chemical mechanisms: random-chain scission; end-chain scission; stripe formation; and cross-link formation. In the present case, thermal degradation temperature was much lower than neat MG49 decomposition (as shown in Figure11). Such interference phenomenon is attributed to polymer-salt interaction.Figure 11
Thermal degradation curves: (a) neat MG49 and (b) pure LiClO4.
(a)
(b)Figure 12
Thermal degradation curves: (a) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and (b) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes.
(a)
(b)Second degradation step was observed around 420–440°C. Such degradation step is attributed to LiClO4 decomposition: (4)
L
i
C
l
O
4
s
⟶
L
i
C
l
s
+
2
O
2
gIn the present case, thermal degradation temperature was much lower than pure LiClO4 decomposition (as shown in Figure 11). Such interference phenomenon is attributed to polymer-salt interaction.


### 3.5. Rheological Characterization

Strain sweep tests were performed at a fixed angular frequencyω
=
1 rad/s. Strain sweep profiles are shown in Figure 13.Figure 13
Strain sweep curves: (a) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and (b) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes.
(a)
(b)G
′ and G
′
′ moduli had remained constant over small strain change. Such predominant phenomenon is attributed to elastic energy absorption. G
′ and G
′
′ moduli had sloped downward at moderate strain level. Such predominant phenomenon is attributed to network deformation. G
′ and G
′
′ moduli had declined above critical strain level. Such predominant phenomenon is attributed to network breakdown (as shown in Figure 14). In general, finite chain extensibility is associated with network breakdown.Figure 14
Stress-strain relations.
(a)
(b)
(c)G
′
/
G
′
′ modulus was observed in [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] polymer electrolyte. G
′ modulus is dominant at low strain range. Such predominant phenomenon is attributed to high stiffness properties, that is, homogeneous reinforcement dispersion and/or significant stress transfer.G
′
/
G
′
′ modulus was not observed in [MG49-25.0 wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolyte. G
′
′ modulus is dominant over the entire strain range. Such predominant phenomenon is attributed to the viscous effects.Frequency sweep tests were performed in the linear viscoelastic range. Frequency sweep profiles are shown in Figure15. Rectangular hyperbola curves were obtained in the linear viscoelastic region. Plateau modulus does not appear in low frequency range. Such predominant phenomenon is related to partial intercalative structure. l
o
g
G
′ versus l
o
g
ω slope is close to 2. Such predominant phenomenon is related to heterogeneous structure.Figure 15
Frequency sweep curves: (a) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and (b) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes.
(a)
(b)G
′
/
G
′
′ modulus was observed in [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and [MG49-25.0 wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes. G
′ modulus is dominant at high frequency range. Such predominant phenomenon is attributed to rotational hindrance. In general, individual segmental relaxation is restricted upon rotational hindrance [21]. In contrast, local chain motion is not affected upon rotational hindrance. Local chain motion is governed through translational diffusion.


## 3.1. Structural Characterization

X-ray diffraction patterns are shown in Figure1. Several broad humps were observed at 2
θ
=
15, 30, and 45°. Such broad humps are attributed to semicrystalline nature [12]. In fact, polyether side chain is still present in semicrystalline structure.Figure 1
X-ray diffraction patterns: (a) [MG49-x wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and (b) [MG49-x wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes.
(a)
(b)Characteristic broad hump (2
θ
=
15
°) had become flattened upon Li-salt insertion. Such predominant phenomenon is attributed to structural distortion. Characteristic broad hump is shifted upon Li-salt insertion. Characteristic broad hump is shifted to high 2-theta angle. Such predominant phenomenon is attributed to configurational alternation [13].LiClO4 diffraction peaks were apparent at high salt concentration (30 wt.% salt insertion). LiClO4 diffraction peaks were observed at 2
θ
=
13.5, 21.1, 23.3, 31.7, 33.1, 35.7, 39.5, 47.3, 49.3, 52.3, 58.1, and 63.1°. Such diffraction peaks are attributed to ionic association. In the literature, pure LiClO4 diffraction peaks were observed at 2
θ
=
12.1, 13.5, 21.1, 23.3, 31.7, 33.1, 35.7, 39.5, 47.3, 49.3, 52.3, 58.1, and 63.1°.LiClO4 diffraction signals are less intense in [MG49-x wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] polymer electrolytes. Such preference phenomenon is attributed to strong interfacial polarization. In general, Li+ cation solvation is dependent on interfacial interaction [14].IR absorption spectra are shown in Figure2. IR absorption spectra are comparable to earlier reports. Major absorption features were detected in such vibrational regions: 3400–3600 cm−1 (hydroxyl stretch); 2960–2860 cm−1 (methyl stretch); 1750–1730 cm−1 (carbonyl stretch); and 1250–950 cm−1 (ether stretch).Figure 2
IR absorption spectra: (a) [MG49-x wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and (b) [MG49-x wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes.
(a)
(b)Hydroxyl absorption band had become apparent upon Li-salt insertion. Hydroxyl absorption band had split into two distinct peaks (3560 and 3525 cm−1). Such interference phenomenon is attributed to intramolecular hydroxyl-hydroxyl interaction. Broad shoulder band was observed at 3380 cm−1. Such shoulder band is attributed to intermolecular hydroxyl-carbonyl interaction.Carbonyl absorption band had become broadened upon Li-salt insertion. Such preference phenomenon is attributed to significant C=O-Li+ complexation.Ether absorption bands were observed at different vibrational modes:ν(C-O), ν
s(C-O-C), ν
a
s(C-O-C), and δ(O-CH3) (as shown in Figure 3). Ether absorption band is shifted upon Li-salt insertion.Figure 3
Isoprene/methyl methacrylate monomeric structure.LiClO4 absorption bands were apparent at high salt concentration. LiClO4 absorption band was observed at 1065 cm−1. Such absorption bands are attributed to ionic association. In the literature, pure LiClO4 absorption bands were observed at 1150–1080 cm−1. Li+ absorption band was observed at 940 cm−1; C
l
O
4
- absorption band was observed at 625 cm−1. Surface hydroxyl absorption bands were apparent at high salt concentration. Surface hydroxyl absorption band was observed at 1630 cm−1. Such hydroxyl absorption band is attributed to hygroscopic properties.


## 3.2. Electrochemical Characterization

Ionic conductivities were determined through electrochemical impedance technique. Ionic conductivities are correlated with Ohm’s law. Ionic conductivities are regulated through multiple parameters: carrier charge, carrier concentration, and carrier mobility. Ionic conductivities are presented in Table1. Ionic conductivities are derived from the formula: (1)
σ
=
1
R
B
×
l
A
,where σ is conductivity (S·cm−1); R
B is bulk resistance; l is thickness (cm); A is the cross-sectional area (cm2).Table 1
LiClO4 salt concentration-dependence ionic conductivities (S/cm) at room temperature.
LiClO4 (wt.%)
Ionic conductivity (S/cm)
[MG49-x wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2]
[MG49-x wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2]
0
1.19 × 10−11
1.19 × 10−11
5
1.63 × 10−11
1.74 × 10−11
10
1.35 × 10−10
2.04 × 10−10
15
4.69 × 10−9
1.08 × 10−9
20
3.09 × 10−7
1.60 × 10−8
25
5.86 × 10−7
4.83 × 10−7
30
6.01 × 10−9
4.24 × 10−9Impedance characteristic curves are shown in Figure4. Small distorted semicircle was observed in high frequency region. Such distorted semicircle is attributed to bulk properties, that is, bulk ionic resistance and/or grain boundary resistance. Single distorted semicircle is correlated with ionic contribution dominate. Slanted spike was observed in low frequency region. Slanted spike is attributed to electrode interface properties [15].Figure 4
Impedance characteristic curves: (a) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and (b) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes.
(a)
(b)Ionic conductivities had increased upon Li-salt insertion. Such predominant phenomenon is attributed to mobile charge carrier increment [16]. Ionic conductivities had attained maximum value at 25 wt.% salt insertion. Such preference phenomenon is ascribed to maximum C=O-Li+ complexation. In general, ionic transport process is mediated through strong hard-acid/hard-base interaction [17].Ionic conductivities had decreased beyond 25 wt.% salt insertion. Such predominant phenomenon is attributed to short interionic distance. In general, ionic transport process is hindered upon ionic aggregation, that is, ionic pairs (Li+⋯C
l
O
4
-) and/or ionic triplets formation. In addition, ionic transport process is hindered upon transient cross-link network formation.In this case, however, ionic conductivities were not comparable to previous reports. Ionic conductivities are suppressed upon rotational hindrance. Such predominant phenomenon is correlated with interparticle interaction. Ionic conductivities were also high in [MG49-x wt.% LiBF4]:[50 wt.% EC]:[6 wt.% TiO2] polymer electrolytes. Ionic conductivities are enhanced upon plasticization effect. Such predominant phenomenon is correlated with free volume increment.Ionic conductivities had increased upon temperature increment (as shown in Figure5). Such preference phenomenon is attributed to free volume increment. In general, ionic diffusional motion is enhanced upon free volume increment. In addition, local segmental relaxation is enhanced upon free volume increment. Main structural relaxation is subjected through rapid internal motion (i.e., significant rotational transition).Figure 5
Temperature-dependence ionic conductivities: (a) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and (b) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes.
(a)
(b)l
o
g
σ versus 1000/T plot is almost linear in [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] polymer electrolyte. In such a case, Arrhenius behavior is predominant throughout the entire temperature range. Arrhenius behavior is described through the relation: (2)
σ
=
σ
0
exp
⁡
-
E
a
R
T
,where σ is conductivity (S·cm−1); σ
0 is preexponential factor (S·cm−1); E
a is activation energy (J·mol−1); R is perfect gas constant (8.314 J·mol−1·K−1); and T is absolute temperature (K). In the present case, hysteresis phenomenon is not observed at high temperature range.Ionic transport process is mediated through point defect movement. Schematic diagram is shown in Figure6. Ionic transport process does take place in the empty sites, either vacant or interstitial sites.Figure 6
Grain lattice diffusion: (a) substitutional diffusion and (b) interstitial diffusion.
(a)
(b)l
o
g
σ versus 1000/T plot is polynomial in [MG49-25.0 wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolyte. In such a case, VTF behavior is revealed in the entire temperature range. VTF behavior is described through the relation: (3)
σ
=
σ
0
exp
⁡
-
B
T
-
T
0
,where σ is ionic conductivities (S·cm−1); σ
0 is preexponential factor (S·cm−1); B is pseudo activation energy (J·mol−1); T is experimental temperature (K); and T
0 is reference temperature (K). Continuous curvature is indicative to cooperative mechanisms: segmental relaxation and/or interfacial defect interaction.Ionic transport process is facilitated through segmental relaxation. Critical transport behavior is correlated with segmental Brownian motion. Schematic diagram is shown in Figure7. Ionic transport process does take place in amorphous region [18].Figure 7
Local segmental motion: (a) intrachain motion and (b) interchain motion.
(a)
(b)Ionic transport process is induced through interfacial defect interaction. Critical transport behavior is correlated with interfacial site percolation [19]. Schematic diagram is shown in Figure 8. Ionic transport process does take place in space charge regions.Figure 8
Grain boundary diffusion: (a) intrachain diffusion and (b) interchain diffusion.
(a)
(b)Distinct conductivities (P
>
0.05) were observed in [MG49-x wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and [MG49-x wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes. Distinct conductivities are attributed to several fundamental factors: heterophase interface structures and relative dissociation degree.Cyclic voltammetric curves are shown in Figure9. Pseudo-elliptic curve was observed in fast scan rate. Such feature is denoted as ideal capacitive properties. Redox peaks were not detected in the entire potential range (−0.5–0.5 Volts). Such feature is attributed to nonfaradic process.Figure 9
Cyclic voltammetric curves: (a) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and (b) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes.
(a)
(b)Broad coverage area was observed in [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] polymer electrolyte. Broad coverage area is attributed to large current efficiencies. Such preference phenomenon is associated with better capacitive behavior.


## 3.3. Morphological Characterization

SEM micrographs are shown in Figure10. SEM micrographs were taken at 10,000x magnification. Uneven structure was observed throughout entire fracture surface. Uneven structure is ascribed to polymer-salt complexation.Figure 10
SEM micrographs: (a) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and (b) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes.
(a)
(b)Irregular aggregate structure was observed throughout entire fracture surface. Irregular aggregate structure is discerned in uniform bright contrast. Irregular aggregate structure is distributed in a random fashion.Nanoparticle dispersion state can exert influence on microstructure growth. Distinct morphological features were observed in [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and [MG49-25.0 wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes. Continuous phase structure was observed in [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] polymer electrolyte. Continuous phase structure is attributed to crystallization retardation. Fine crack structure was observed in [MG49-25.0 wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolyte. Fine crack structure is attributed to salt aggregation.


## 3.4. Thermal Characterization

Thermal stabilities are important parameter in performance appraisal [20]. Thermal stabilities were investigated through simultaneous thermogravimetric and differential thermal analysis.Thermal degradation curves are shown in Figure12. Similar degradation pattern was observed in [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and [MG49-25.0 wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes.Initial degradation stage was observed around 80–100°C. Such degradation stage is ascribed to moisture (and residual solvent) elimination. Large mass loss is not detected until irreversible decomposition. In this case, however, minor mass loss was observed at lower temperature range. Such interference phenomenon is associated with TiO2-SiO2 catalytic effects.Distinct degradation phases were detected at high temperature region (as shown in DTG curves). Such endothermic peaks are ascribed to thermal oxidative decomposition. First degradation step was observed around 270–290°C. Such degradation step is attributed to polymer chain decomposition. Transient degradation process is initiated through different chemical mechanisms: random-chain scission; end-chain scission; stripe formation; and cross-link formation. In the present case, thermal degradation temperature was much lower than neat MG49 decomposition (as shown in Figure11). Such interference phenomenon is attributed to polymer-salt interaction.Figure 11
Thermal degradation curves: (a) neat MG49 and (b) pure LiClO4.
(a)
(b)Figure 12
Thermal degradation curves: (a) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and (b) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes.
(a)
(b)Second degradation step was observed around 420–440°C. Such degradation step is attributed to LiClO4 decomposition: (4)
L
i
C
l
O
4
s
⟶
L
i
C
l
s
+
2
O
2
gIn the present case, thermal degradation temperature was much lower than pure LiClO4 decomposition (as shown in Figure 11). Such interference phenomenon is attributed to polymer-salt interaction.


## 3.5. Rheological Characterization

Strain sweep tests were performed at a fixed angular frequencyω
=
1 rad/s. Strain sweep profiles are shown in Figure 13.Figure 13
Strain sweep curves: (a) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and (b) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes.
(a)
(b)G
′ and G
′
′ moduli had remained constant over small strain change. Such predominant phenomenon is attributed to elastic energy absorption. G
′ and G
′
′ moduli had sloped downward at moderate strain level. Such predominant phenomenon is attributed to network deformation. G
′ and G
′
′ moduli had declined above critical strain level. Such predominant phenomenon is attributed to network breakdown (as shown in Figure 14). In general, finite chain extensibility is associated with network breakdown.Figure 14
Stress-strain relations.
(a)
(b)
(c)G
′
/
G
′
′ modulus was observed in [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] polymer electrolyte. G
′ modulus is dominant at low strain range. Such predominant phenomenon is attributed to high stiffness properties, that is, homogeneous reinforcement dispersion and/or significant stress transfer.G
′
/
G
′
′ modulus was not observed in [MG49-25.0 wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolyte. G
′
′ modulus is dominant over the entire strain range. Such predominant phenomenon is attributed to the viscous effects.Frequency sweep tests were performed in the linear viscoelastic range. Frequency sweep profiles are shown in Figure15. Rectangular hyperbola curves were obtained in the linear viscoelastic region. Plateau modulus does not appear in low frequency range. Such predominant phenomenon is related to partial intercalative structure. l
o
g
G
′ versus l
o
g
ω slope is close to 2. Such predominant phenomenon is related to heterogeneous structure.Figure 15
Frequency sweep curves: (a) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and (b) [MG49-25.0 wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes.
(a)
(b)G
′
/
G
′
′ modulus was observed in [MG49-25.0 wt.% LiClO4]:[8.0 wt.% HNO3-THF/TiO2-SiO2] and [MG49-25.0 wt.% LiClO4]:[8.0 wt.% ClHNO2-THF/TiO2-SiO2] polymer electrolytes. G
′ modulus is dominant at high frequency range. Such predominant phenomenon is attributed to rotational hindrance. In general, individual segmental relaxation is restricted upon rotational hindrance [21]. In contrast, local chain motion is not affected upon rotational hindrance. Local chain motion is governed through translational diffusion.


## 4. Conclusion

Different measurement techniques were further implemented in microstructural characterization. XRD analysis had revealed remarkable crystalline reduction upon structural alternation. FTIR analysis had confirmed C=O-Li+ complex formation upon coordinative interaction. EIS analysis had demonstrated unique transport mechanism upon interfacial interaction. CV analysis had indicated significant redox stabilization upon interfacial interaction. TGA analysis had indicated rapid oxidative degradation upon structural alternation. DRA analysis had revealed noticeable rheological stabilization upon interparticle interaction.



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*Source: 9838067-2016-08-04.xml*