Maitri Patelab,
Kuldeep Mishrac,
N. A. Chaudharyd,
Vaishali Madhanie,
J. J. Chaudhariab and
Deepak Kumar
*af
aGujarat Technological University, Ahmedabad, Gujarat-382424, India. E-mail: deepak.kumar06@gov.in; fwtdrdeepakkumar@gmail.com
bVishwakarma Government Engineering College, Ahmedabad, Gujarat-382424, India
cSymbiosis Institute of Technology (SIT), Symbiosis International (Deemed University) (SIU), Pune-412115, India
dDepartment of Applied Physics, Faculty of Technology and Engineering, The Maharaja Sayajirao University of Baroda, Vadodara, Gujarat-390002, India
eDepartment of Applied Sciences (Physis), Parul University, Vadodara, Gujarat-391760, India
fRegional Institute of Education Mysuru, National Council of Educational Research and Training, Mysuru-570006, Karnataka, India
First published on 30th April 2024
For sodium batteries, the development of gel polymer electrolytes (GPEs) with remarkable electrochemical properties is in its early stage and persists to be a challenge. In this report we have synthesized a series of GPEs containing a poly(vinyllidene fluoride-co-hexafluoropropylene) (PVdF-HFP) and poly (methyl methacrylate) (PMMA) as blend polymer, sodium perchlorate (NaClO4) as ion-conducting salt and 1-ethyl-3-methylimidazolium tetrafluoroborate (EMIM-BF4) and tetra ethylene glycol dimethyl ether (TEGDME) as molecular solvents. The counter balance between EMIM-BF4 and TEGDME is maintained by the electrolyte, which is formed through the optimal weight ratio of 2:
1. GPEs have an advantageous set of properties, including stability window of 5 V, Na+ transference number of 0.20, and a room-temperature ionic conductivity of 5.8 × 10−3 S cm−1. According to enthalpy and entropy calculations, optimized GPE yields the highest amount of disorder or amorphicity and contributes to greatest conductivity. XRD analysis supports this argument. Thermal investigations show that optimized GPE may preserve gel phase up to 125 °C. The prototype sodium cell fabricated with optimize GPE has a specific capacity of 281 mA h g−1 and open circuit voltage of 2.5 V. The optimized GPE exhibits potential for future electrochemical applications.
Molecular solvents play a vital role in the GPEs. By decreasing crystallinity of polymer, plasticizer induces formation of an increased number of dissociated free cations and anions via the separation of ion pairs. Conductivity is exclusively observed in the amorphous region. Consequently, as the degree of amorphicity of the GPE increases, so its conductivity will also boost by inclusion of solvents.13 In addition to their stability and reduced flammability, electrolytes containing TEGDME feature high conductivity.14 It has many other advantageous characteristics, including a high boiling point and minimal volatility.15 Ionic liquids (ILs) have garnered significant attention in recent investigations owing to their distinctive physical and chemical characteristics, including incombustibility, miscibility with various organic solvents, and non-volatility. Due to their broad potential window and high ionic conductivity, ILs are viable electrolytes from an electrochemical aspect. ILs have garnered considerable curiosity in recognition of their promising utility in electrochemical capacitors and batteries.16–18 Numerous studies demonstrate the application of ionic liquid and glyme as molecular solvents for fabrication of GPEs for lithium and sodium based electrochemical application. Syali et al. reported cocktail GPEs by utilizing carbonate, glyme and ionic liquid molecular solvents for Na based batteries and EDLC application.19 Wu et al. designed GPEs with the combination of N-methoxyethyl-N-methylpyrrolidinium bis(trifluorome-thanesulfonyl)-imide (P1,2O1TFSI) and TEGDME for application in lithium–sulfur battery.20 Rao et al. fabricated Li–S cell by utilizing a GPE containing N-methyl-N-butylpiperidinium bis(trifluoromethanesulfonyl) imide (PPR14TFSI) and poly (ethylene glycol) dimethyl ether (PEGDME).21 Wu et al. synthesized Li–S battery by employing binary salt based GPE with Nmethoxyethyl-N-methylpyrrolidinium bis(trifluoromethanesulfonyl)-imide (Pyr1,2O1TFSI) TEGDME in ratio of 7:
3.22 Song et al. reported polymer electrolyte by utilizing 1-ethyl-3-methylimidazolium bis(fluorosulfonyl)imide and SiO2 nanoparticles with PEO matrix for Na metal batteries.23
Scientists are making efforts to discover a sodium–ion conducting gel polymer electrolyte that is commercially viable. Even though there are numerous reports on the development of GPEs, the authors have not found any report on the counterbalance between the solvents in order to advance the development of electrolytes for Na batteries. This study aims to address this gap found in the literature. By combining EMIM-BF4 and TEGDME, we proposed a novel ionic liquid-based GPE system for electrochemical application in this study that aims to amplify electrochemical properties of GPEs. The ether group present in ionic liquid confers a comparatively high level of conductivity. Ethers may serve as viable alternatives for co-solvents, thereby potentially enhancing the conductivity of GPEs. These properties are critical for optimizing the capacity and rate performance of any batteries.24 Although ethers with low molecular weights, such as diethylene glycol dimethyl ether (DEGDME) and 1,2-dimethoxyethane (DME), have a low viscosity, their low boiling and flashing points render them incompatible with safety regulations. TEGDME is chosen in the electrolyte without significantly compromising the intrinsic safety of the ionic liquid. Consequently, we investigate the possibility for a counterbalance between the TEGDME and the ether-functionalized ionic liquid in order to advance the development of Na batteries that exhibit commendable safety attributes.20 In various mass ratios, we utilized binary mixture consisting of 2 M NaClO4 + EMIM-BF4/TEGDME. The electrolyte mixes were analyzed for their physical and electrochemical characteristics. The optimal ratio for balancing the composition of EMIM-BF4/TEGDME mixed electrolytes was identified. Additionally, we examined the electrochemical behavior of Na based prototype cell utilizing the optimized electrolyte mixtures.
The composition and sample codes of the GPEs are detailed in Table 1.
Sample code | Composition |
---|---|
PNTE-1 | PVdF-HFP/PMMA + EMIMBF4![]() ![]() ![]() ![]() |
PNTE-2 | PVdF-HFP/PMMA + EMIMBF4![]() ![]() ![]() ![]() |
PNTE-3 | PVdF-HFP/PMMA + EMIMBF4![]() ![]() ![]() ![]() |
Fig. 2(b) illustrates Nyquist curves of optimized GPEs at 30, 40, 50 and 60 °C. Rb drops as temperature rises in GPE (Fig. 2(b)). The Rb is correlated with σ of GPE according to the subsequent relationship.
![]() | (1) |
The components of equivalent circuit of the cell have been determined using the EC-Lab software. Eqn (2) is used to fit complex impedance experimental data points into Randles Cell Circuit model, which is given in Fig. 2(a).
![]() | (2) |
τEDL = R2C2 | (3) |
τσ = R3C3 | (4) |
Sample code | Rb | R1 (Ω) | C2 (µF) | R2 (Ω) | C3 (µF) | R3 (Ω) | σ4 (Ω s−1/2) | τEDL (s) | τσ (s) |
---|---|---|---|---|---|---|---|---|---|
PNTE-1 | 19.66 | 18.19 | 10.11 | 229.1 | 11.61 | 7385 | 1332 | 0.002316 | 0.08574 |
PNTE-2 | 10.10 | 8.875 | 8.018 | 197.2 | 18.46 | 3324 | 1270 | 0.001581 | 0.06136 |
PNTE-3 | 6.69 | 4.316 | 4.183 | 236.6 | 7.169 | 8017 | 1269 | 0.000990 | 0.05747 |
Fig. 2(c) demonstrates the variation in log σ in relation to the reciprocal of the absolute temperature for GPEs with various concentrations of TEGDME and EMIMBF4 in temperature range 30 to 65 °C. Fig. 2(c) indicates that conductivity of the systems does not have a sudden increase with temperature, suggesting that GPEs have a fully amorphous structure.25 It is apparent from the graph that σ of each sample rises with increasing temperature, which is consistent with Arrhenius relation. The correlation between temperature and conductivity may be attributed to a reduction in viscosity, which consequently enhances the flexibility of the chain.26 This phenomenon can be elucidated by considering free volume model and the hopping of charge carriers between localized states.27 Polymer ionizes salt into anions and cations upon exposure to an applied electric field and temperature. By transitioning between localized states, these ions increase the ionic conductivity. When the temperature rises, a segment's vibrational energy becomes strong enough to overcome the hydrostatic pressure exerted by the atoms around it, creating a little area around its own volume where vibrational motion is possible. Consequently, an increase in conductivity is brought about by free volume around polymer, which also induces ion and polymer segment mobility. Because there is more free volume at a higher temperature, conductivity increases. A larger free volume is also provided in the polymer electrolyte system by rising amorphous content with temperature.28 Throughout the entire temperature range, the temperature-dependent ionic conductivity of PNTE-3 is greater than other counterpart GPEs of this study.
The thermodynamic parameters are crucial for understanding the temperature-dependent conductivity of polymer electrolytes include the change in activation energy (ΔEa), enthalpy of activation (ΔH), and entropy of activation (ΔS). These parameters are determined through experimental analysis by employing an Arrhenius-type relationship29,30, which establishes a correlation between conductivity and temperature. The experimental data utilized in this study indicates that σ of GPEs upsurges with temperature, suggesting a process of heat activation within the material. This phenomenon can be elucidated through the Arrhenius relationship, which correlates conductivity (σ) with temperature (T) as follows:
![]() | (5) |
![]() | (6) |
The Eyring–Polanyi equation provides a general linear form of the Arrhenius-like appearance by related conductivity to Gibb's function and calculating ΔH and ΔS is specified by eqn (7).
![]() | (7) |
The change in activation enthalpy (ΔH) and entropy (ΔS) is also expressed as32
![]() | (8) |
This can be written in the form of y = mx + c as given by eqn (8).
Where slope determines enthalpy of activation, () and intercept supply entropy, ΔS [intercept = (ΔS/R) + ln(k/h)].
Table 3 shows ionic conductivity, activation energy, enthalpy and entropy values for fabricated GPEs along with their sample code. ΔH and ΔS are obtained from linear plots of 1000/T vs. ln(σ/T). The enthalpy values obtained for samples PNTE-1, PNTE-2 and PNTE-3 are 23.06, 18.23 and 17.80 J mol−1 K−1. So, enthalpy value is decreased in GPE sample PNTE-3. The entropy values are about of −214.83, −226.75 and −236.66 J mol−1 K−1 for PNTE-1, PNTE-2 and PNTE-3 respectively. The optimized GPEs sample PNTE-3 carries the maximum conductivity and lowest activation energy. The lowest enthalpy and highest entropy of GPE PNTE-3 indicate that the GPE carry maximum amorphicity contributing to the faster polymer segmental motion and hence faster ionic mobility.
Sample | Ionic conductivity (σ) (S cm−1) | Activation energy (Ea) (kJ mol−1) | Enthalpy (ΔH) (J mol−1 K−1) | Entropy (ΔS) (J mol−1 K−1) |
---|---|---|---|---|
PNTE-1 | 2.4 × 10−3 | 22.08 | 23.06 | −214.83 |
PNTE-2 | 4.1 × 10−3 | 20.46 | 18.23 | −226.75 |
PNTE-3 | 5.8 × 10−3 | 19.63 | 17.80 | −236.66 |
Fig. 2(d) displays the plot of ac conductivity against frequency for GPEs namely PNTE-1, PNTE-2 and PNTE-3. At lower frequencies, the alternating current signal is active for longer periods, leading to anticipated polarizing effects at interface between the electrolyte and electrode. Lower values of ac conductivity indicate that polarization effects are more prominent at lower frequencies. At the electrolyte/electrode interface, polarizing effects will occur due to the increased duration of the ac signal at low frequencies. At lower frequency values, polarization effects predominate, as indicated by the lower values of ac conductivity (σac). A decrease in polarizing effects is observed as the frequency increases, leading to an increase in conductivity values. The σac patterns begin to flatten for frequencies greater than 103 Hz; consequently. This means that σ values are identical across the whole plateau area. This flat zone indicates ionic transport occurs by hopping, and observed σ values in this zone are identical to σ values obtained using eqn (1). σac values for optimized GPE (PNTE-3) rise with temperature, but the overall behavior stays constant over the whole frequency range (Fig. 2(e)). Hence, throughout the operational temperature range of the GPE, hopping behaviour is observed at high frequencies and polarizing effects are observed at low frequencies.
ε* = ε′ − jε″ | (9) |
By utilizing the dielectric constant (ε′), one can examine ion conduction and relaxation mechanisms of GPEs system. The ε′of GPEs influences its polarization. The dielectric constant (ε′) of an electrolyte system represents the capacity for electric charge storage and dipole alignment per unit volume. It can be mathematically represented as follows:
![]() | (10) |
The dielectric constant of all GPEs system at RT is illustrated in Fig. 3(a). Additionally, Fig. 3(b) illustrates the frequency dependence of the dielectric constant of PNTE-3 across different temperatures.
Fig. 3(a) shows the change in ε′ for all the samples at RT. The plot of ε′ shows high values at lower frequencies due to the very higher interfacial capacitance and the buildup of ionic charge at the electrode-GPEs interface. At low frequencies, the system has great energy storage capabilities and experiences maximum energy loss. The reduction in ε′ with increasing frequency demonstrates the polar character of the system. When the applied field direction is reversed at high frequency, the charges are unable to keep up, leading to a drop in polarization and a fall in the ε′ value.33
At temperatures higher than room temperature, dipoles can readily align, although highly cross-linked materials may make orientation challenging at times. Fig. 3(b) shows the changes in ε′ of PNTE-3 sample at different temperatures. It is evident that as the frequency increases, the ε′ declines steadily and reaches a plateau at high frequencies after a certain point. The increased ε′ at high temperatures in low frequency is due to polarization of the electrode and space charge.34
Electric modulus assessments (M″) have been carried out to differentiate electrode polarization and other interfacial characteristics. Analysis on modulus is helpful in discovering materials that have similar resistances but varying capacitances.35,36 The M″ may be mathematically characterized as:
![]() | (11) |
Fig. 3(c) illustrates alteration in M″ vs. frequency at RT for GPEs: PNTE-1, PNTE-2, and PNTE-3. A negligible response, close to zero, is seen in low frequency owing to electrode/electrolyte interfacial interaction. This observation further indicates the extensive migration of ions over long distances and the slight impact of polarization effects in small frequency. The existence of an elongated tail in area of lower-frequency indicates that electrodes possess a substantial capacitance. Fig. 3(c) displays that GPE sample PNTE-3 has the lowest M″ in high frequency, when compared to GPE PNTE-1 and PNTE-2. Minor values of M″at high frequencies enable elevated σ and boosted ion dynamics, as shown by the study.33
The graph in Fig. 3(d) illustrates the change in M″ vs. frequency for PNTE-3 at various temperatures. When temperature goes from 303 K to 333 K, the onset swings to the higher frequency, which shows that relaxation process is happening. Moreover, the shift of this modulus towards higher frequencies with increasing temperature might be attributed to enhanced motion of ions inside tailored GPEs. Fig. 3(d) shows that when the temperature increases, there is a drop in values at higher frequencies. The commencement of peak height lowers with increasing temperature as a result of a reduction in Rb of GPE. In conclusion, modulus measurements corroborated the findings of ionic conductivity and dielectric studies, showing that electrolyte specimen PNTE-3, has superior conductivity, dielectrics, and modulus values when compared to GPEs specimens PNTE-1 and PNTE-2 respectively.
Fig. 4(a) shows the CV curvatures for prepared GPEs. The electrolyte breakdown voltage, wherein no oxidation or reduction occurs, is determined by the irreversible onset of the current. This value provides insight into the electrochemical stability of the system. The current gradually increases as the voltage across the cells rises. At first, there is a steady flow of electric current through the electrodes. However, once the voltage surpasses a certain threshold, there is a sudden and significant change in the current. This change defines the voltage range within which the membrane operates.38 At voltages below 2.5 V, there is a consistent flow of current across the electrodes in all samples. However, as the voltage increases, the current increases gradually, followed by a sudden transition that correlates with the starting point of the electrolyte's decomposition process. This mild current of up to 2.5 V could potentially be ascribed to the altering of the SS surface.39 The absence of any adverse reaction and the stability of the GPEs are indicated by the almost negligible current values observed in range of −2.5 V to +2.5 V for all three sample, representing window of approximately 5.2 V, 5.4 V and 5 V for PNTE-1, PNTE-2 and PNTE-3 GPEs respectively, as illustrated in Fig. 4(a). From the standpoint of device application, this operating voltage range is adequate, especially when utilized as the electrolyte in sodium batteries.
![]() | ||
Fig. 4 Cyclic voltammetry curvatures (a) with SS/electrolyte/SS for PNTE-1,2,3 (b) with Na–Hg/PNTE-3/Na–Hg (c) tion number for PNTE-3 (d) tNa+ number for PNTE-3. |
Cyclic voltammetry (CV) is used to verify the migration of sodium ions in optimized GPE PNTE-3, using a symmetric reversible cell arrangement, namely Na–Hg|PNTE-3|Na–Hg. The CV plot revealed in Fig. 4(b) displays two peaks in the anodic and cathodic directions, indicating the deposition of sodium ions at the anodic site and the removal of sodium ions at the cathodic site. Therefore, the anodic and cathodic redox processes occur efficiently at the interface between sodium and mercury in the presence of an electrolyte, suggesting the transfer of sodium ions from the anodic site to the cathodic site and vice versa when a little voltage is applied. With evidence of sodium ion plating/stripping at the respective electrodes, the CV studies indicate that an ESW of approximately 5 V is satisfactory from an application standpoint for sodium batteries. A multitude of studies have shown analogous sodium–ion migration by using GPEs and a reversible sodium electrode setup.40,5,41
The performance of Transference Number Measurement (TNM) relies on characteristics of blocking or non-blocking electrodes. The blocking electrodes selectively allow only electrons to enter and traverse through them, whereas non-blocking electrodes let both electrons and ions (cations or anions) to enter, but only electrons can traverse through them. The determination of TNM may be accomplished through two approaches, namely Wagner's polarization and Bruce–Vincent methods.42 In order to determine the type of species that contribute to conductivity in the current electrolyte system, the transport numbers were measured. These numbers provide a quantitative assessment of the extent to which ions and electrons contribute to the overall conductivity. This measurement was done by utilizing Wagner's dc polarization and by applying potential of 0.75 V across the cell. The cell has been polarized using a dc voltage. A decline in electric current over time is seen. The initial high current is due to transfer of ions and electrons. By eliminating ability of ions to travel through the external circuit, the SS electrodes hamper the flow of current solely. As a consequence of the electrode polarization effect, the current diminishes progressively with all-time. Consequently, the observed ultimate constant current can be elucidated exclusively through the electron contribution.43 The following expressions are utilized:36
![]() | (12) |
te = (1 − tion) × 100% | (13) |
For the optimal GPE PNTE-3, the time-dependent variation of polarization current is illustrated in Fig. 4(c). It is determined that the value of tion for PNTE-3 sample is 99.08%. More precisely, te is equal to 0.92%. It is evident from this observation that the ion transport number exceeds that of the electron transport number. This observation implies that in the GPE sample that is reported, ions are the predominant species accountable for electrical conduction.41
The assessment of the sodium transport number (tNa+) is an essential variable utilized to determine the proportion of sodium ions that contribute to overall σ in GPEs. By employing combined ac and dc method, tNa+ of PNTE-3 is computed utilizing the Vincent method. In this methodology, Na–Hg| PNTE-3|Na–Hg cell is polarized for a duration of 2 h through the application of a voltage, ΔV = 20 mV. The final and initial currents are subsequently tracked (Fig. 4(d)). Moreover, the cells undergo a.c. impedance measurements both before and after the polarization as a vital aspect of the approach. The electrode–electrolyte contact resistance values are subsequently estimated based on the impedance plots (Fig. 4(d)). The following equation can be utilized to determine sodium–ion transport number (tNa+)
![]() | (14) |
The tNa+ value for PNTE-3, as determined through eqn (14), is ∼0.20. The observed Na+ transport number value in GPE indicate that anionic species play a substantial role in facilitating ion conduction within the electrolyte system.
TGA is done to check thermal stability of GPEs films that were prepared. Fig. 5(b) illustrates the TGA thermograms of prepared GPEs namely PNTE-1, PNTE-2 and PNTE-3 in the temperature range from RT to 600 °C. The GPE films composed of PVdF-HFP/PMMA blend decompose in a four-step process, as observed. The initial phase of decomposition was detected at a temperature marginally ∼100 °C, potentially due to the evaporation of surface or residual moisture present in the specimen. The second stage of decomposition occurred between 100–200 °C and is associated with the thermal evaporation of the TEGDME/EMIMBF4 solvent and followed by third stage in the range of 200–300 °C due to breakdown of the polymer's main chain. At greater temperatures, mass loss is occurred above 300 °C in fourth stage of decomposition occurred caused by the breakdown of NaClO4 salt. The inclusion of NaClO4/EMIM-BF4/TEGDME in PVdF-HFP/PMMA blending resulted in a reduction in weight loss for the constructed GPEs films, suggesting that the thermal stability of the electrolytes was enhanced and is adequate to support their potential use as electrolyte in electrochemical devices.45,46
![]() | ||
Fig. 6 FTIR band for PVdF-HFP, PMMA and PNTE-1,2,3 in wavenumber (a) 700–2000 cm−1 and (b) 2000–4000 cm−1, and (c) XRD plots for PVdF-HFP, PMMA and PNTE-1,2,3. |
Materials | IR bands (cm−1) | Assignment | Reference |
---|---|---|---|
PMMA | 747 | Rocking deformation vibrations | 48 |
805 | C–O–C symmetric stretching mode | 48 | |
838 | Methylene rocking mode | 48 | |
1242 | Antisymmetric C–C–O stretch | 49 | |
1386 | OCH3 deformations | 49 | |
1443 | CH3 stretching | 49 | |
1726 | C![]() |
50 | |
2951 | CH3 asymmetric stretching | 50 | |
PVdF-HFP | 762 | α-Phase | 51 |
834 | γ-Phase | 51 | |
876 | Combined CF2 and C–C symmetric stretching vibrations and amorphous-HFP | 51 | |
1064 | C–C skeletal vibrations and CF3 out of plane deformation | 52 | |
1175 | antisymmetric CF2 stretching | 52 | |
1400 | CH2 wagging | 52 | |
TEGDME | 944 | Asymmetrical CH2 rocking | 19 |
1242 | Asymmetric CH2 twisting | 19 | |
1456 | CH2 scissoring | 19 | |
EMIMBF4 | 752 | C![]() |
19 |
1175 | Ring in-plane deformation | 19 | |
1572 | C–H, C–N (ring) stretching | 19 |
When TEGDME and EMIMBF4 are introduced in varying ratios to the blended polymer matrix PMMA:
PVdF-HFP, certain absorption bands vanish or shift in the developed samples. There are noticeable changes in the intensity of certain bands. These outcomes definitely show that blended GPEs based on glyme and IL successfully synthesised. The absorption bands detected in 756–698 cm−1 of pure PMMA is owed to the presence of bending, ring out of plane or rocking deformation vibrations of PMMA, while band at 762 cm−1 in PVdF-HFP polymer corresponds to α-phase of crystalline PVdF. The band at 805, 838 cm−1 in pure PMMA polymer is assigned to C–O–C symmetric stretching and methylene rocking. The band 834, 877 cm−1 are due to γ-phase of PVdF and combined CF2 and C–C symmetric stretching vibrations and amorphous-HFP. The peaks of pure PMMA and PVdF-HFP at 762, 747 cm−1 begin to merge and weaken when TEGDME and EMIMBF4 have been added to the blend polymer matrix of PMMA
:
PVdF-HFP. The peak has been shifted to 752 cm−1 of C
C–H of EMIMBF4. Other characteristic bands at 838 cm−1 of PMMA as well as bands at 834 and 876 cm−1 is found to be lifted to 836 and 881 cm−1. The peak at 949 cm−1 in PNTE-1 and PNTE-2 samples corresponds to asymmetrical CH2 rocking in TEGDME plasticizer which has disappeared in PNTE-3 sample. The band at 1064 cm−1 of PVDF-HFP is of C–C skeletal vibrations and CF3 out of plane deformation are getting broadened and lifted to 1069 cm−1, specifying interaction between polymers, plasticizers and salt. The absorption band at 1175, 1400 cm−1 corresponds to antisymmetric CF2 stretching and CH2 wagging of PVdF-HFP gets reduced in intensity on addition of TEGDME and EMIMBF4. The band at 1175 cm−1 links to ring in-plane deformation of IL. The band at 1242 cm−1 is allotted to asymmetric CH2 twisting of TEGDME. The peaks at 1456, 1572 cm−1 corresponds to CH2 scissoring and C–H, C–N (ring) stretching of glyme and IL. The PMMA polymer's characteristic peak, which was previously located at 1726 cm−1, has now moved to the higher frequency side at 1731 cm−1. The addition of plasticizers has also drastically decreased the peak's intensity. The butyl chain of IL (which also causes the polymer backbone stretching) and the imidazolium cation ring of IL are responsible for the C–H stretching vibrations that cause the peaks in the spectral range of 3200−2800 cm−1. The peaks found between 3650 and 3000 cm−1 indicate the presence of OH and –OOH groups. The peak at 2951 cm−1 is owed to presence of CH3 asymmetric stretching of methylene group which has been shifted to lower frequency side and has become weak by incorporating TEGDME and EMIMBF4. Based on this, the constructed samples consisting PMMA, PVdF-HFP, NaClO4, TEGDME, and EMIMBF4 exhibit shifting and lack of vibrational bands, suggesting that the polymer, salt, and plasticizer interactions are favourable to form blended GPEs.48,49,51–55
In a GPEs, XRD is an effective method to characterize crystalline phase transitions and alterations.56 The XRD patterns of (PVdF-HFP: PMMA) and NaClO4-based GPE at different TEGDME-EMIMBF4 concentrations are shown in Fig. 6(c). The semicrystalline character of PVdF-HFP is revealed by peaks at 2θ ∼18.5° and ∼20°, along with small intensity peak at ∼39°. The (100) + (020) and (021) planes of the non-polar crystalline phase of PVdF are represented by peaks on ∼18.5° and ∼39°, respectively. The (110) plane of the polar crystalline phase of PVdF-HFP is reflected by peak on ∼20°.57 The XRD peaks that were detected are compared to the standard JCPDS data (Card No. 00-038-1638), which provides confirmation of the creation of the semi-crystalline phase of the PVdF-HFP copolymer.58 The pure PMMA pattern has a broad as well, less prominent peak at 2θ ∼13.8°, indicating the PMMA film's entire amorphous nature.57 The amorphous hump of PMMA at 2θ ∼13.8° is found vanished, and the dominant peaks of PVdF-HFP at 2θ ∼20° and 39° are reduced in intensity together with the broadening on addition of TEGDME and EMIMBF4, indicating a rise in the films' amorphicity (Fig. 6(c)). The aforementioned analyses show that adding TEGDME-EMIMBF4 can decrease the polymer membrane's crystallinity, speed up the mobility of the chain segments within the polymer, and increase the pace at which sodium ions migrate.59 With XRD analysis, the degree of crystallinity has been computed to determine if the prepared samples' amorphocity has increased or decreased. The pure PVdF-HFP polymer possesses the degree of crystallinity of 34.40%. When TEGDME and EMIMBF4 are added to the blended polymer matrix to obtain electrolyte films PNTE-1 and PNTE-2, the degree of crystallinity further reduces to 22.13 and 16.34% respectively. The crystallinity calculations reveals that the electrolyte sample PNTE-3 has the lowest degree of crystallinity of 13.72%, indicating that the presence of higher content of EMIMBF4 ionic liquid inculcate more disordering the polymeric structure than other solvent combinations used in PNTE-1 and PNTE-2. Therefore, it should have the most flexible polymeric chain enabling the faster segmental mobility promoting the higher ionic conductivity in the GPE.60
![]() | ||
Fig. 7 (a) OCV plot for Na cell (b) charge–discharge profile ((inset): coulombic efficiency vs. cycle no.) (c) discharge capacity vs. cycle number. |
The charge–discharge characteristic of the prototype for various cycles under 50 mA g−1 current are illustrated in Fig. 7(b). The cell delivers an initial specific discharge capacity of ∼281 mA h g−1. The capacity of the cell significantly declines during subsequent charge–discharge cycles, and by the twentieth discharge, it seems to have retained no more than 21.35% of its initial capacity. The two major possible reasons for the above observed capacity deterioration are the formation of passivation layer depositing at the electrolyte/electrode interface at the Na–Hg anode and the inadequate conductivity of the P–C electrode,61 which indeed display scope for tailoring electrodes. The coulombic efficiency (CE) of the prototype cell is illustrated in the inset of Fig. 7(b). In this instance, the CE was calculated as the proportion of stripping Na+ to plating Na utilized in each cycle.62 The initial CE of cell is comparatively low, which is potentially due to the decomposition of NaClO4 or the loss of a large amount of sodium due to the formation of solid–electrolyte interface (SEI). Over 20 cycles, the Na–Hg/PNTE-3/P–C maintained a steady coulombic efficiency (CE) of around 94%. As illustrated in Fig. 7(c), the discharge capacity decreases with the number of charge–discharge cycles. During the second discharge, the cell experiences a capacity loss of approximately 35.24%, resulting in a measured capacity of 99 mA h g−1. Following the second discharge, the rate of capacity diminishing decelerates, with the discharge capacities of approximately 75, 65, 64.5, and 60 mA h g−1 observed for the 5th, 10th, 15th and 20th discharges, respectively.
Although the designed PNTE-3 GPE displays a favourable σ, ESW, and tNa+, the capacity fading of the proto-type sodium cell might be caused by other cell components such as the anode and cathode. The selection of substance for the electrode and the electrolyte/electrode contact are two critical factors in determining the cycling parameters of the cell. During cycling, the GPE may be reduced at the Na–Hg anode and oxidized at the P–C cathode, eventually increasing the size of the passivating solid electrolyte inter-phase (SEI).63 This layer may be accountable for consumption of a portion of the cathode's sodium ions, reducing discharge capacity. Another probable explanation is the volume enlargement at the anode portion of the proto-type during cycling, which may increase the charge-transfer resistance at the electrolyte/electrode interface and therefore the internal resistance of the prototype.64,65
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