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Abstract

In this work, an insoluble three dimensional (3D) porous polymeric structure and their metal complexes were synthesised by the condensation reactions of meta(m)-phenylenediamine, para(p)-phenylenediamine and glutaraldehyde. The morphological and spectral features of the porous polymeric structures were determined using different analytical and spectroscopic methods, including field emission scanning electron microscopy, four-point probe electrical conductivity, photoluminescence spectroscopy, Fourier-transform infrared spectroscopy, surface area Brunauer–Emmett–Teller and magnetic and thermal behaviours. According to the obtained data, the shape, size and photoluminescence properties of the compounds, especially the conductivity, were clearly changed after the metalation processes.

Keywords

Coordination polymers electrical conductivity luminescence measurements

Introduction

Technological development and an increasing human population increase energy consumption rates. Fossil fuel–based energy sources create the emission of carbon dioxide in the atmosphere, which causes global warming. The increase in green gas emissions in the atmosphere is warning us to decrease carbon dioxide emissions through more environmentally friendly solutions.^1–3 One of the most likely solutions for solving this problem is the improvement of electric-based technologies.^4,5 Electrical vehicles, such as electric cars and smart portable devices, need an advanced energy storage system for high efficiency.⁶ Upon those demands for energy storage systems, the progression of battery technologies with power density, long life cycles, high-energy density and low costs has become one of the hottest topics for many research groups. Lithium (Li-ion) rechargeable batteries are one of the most important and likely solutions for the new generation of energy storage systems.⁶ However, morphological reconstruction after cycling of a battery causes new architectural structures of morphology, such as dendrite shapes that make a Li-ion battery inactive and responsible for short circuits.^7–9 To figure out the deterioration of the battery’s performance dependent on the surface fractures, the surface of the battery should be protected with solid electrodes. Transition metal oxide, porous carbon and conductive polymers have been widely investigated as solid electrodes to protect the battery’s surface from fractures.^8,10,11 Conductive polymers are one of the best potential materials for protection of the Li battery surfaces.^12–17 The morphological features of the polymers and their production methods, the number of donor atoms and centres, the kind of metals and their ionic charge, the hydrogen bond and the π-π stacking in the polymer and the steric hindrance are crucial for designing well-tuned and stable electrodes.^14,18–22 More specifically, the type of organic linker in the polymer is also one of the most significant points to achieve a targeted, efficient porous morphology because linker ligands, having a single C–C bond (sp³) and donor group, have the ability to give flexibility to each of the polymeric units.^6,23–27 Therefore, the coordination polymers can rotate around the flexible linkers. The morphology of the molecules in the polymeric structure can grow in different directions.^26,28-34 The 3D structure, the porosity of the coordination polymers and the conductivity are highly effective for application, such as in a flexible electrode for new generation battery technologies.^35–37 Polymers, such as polyaniline (PANI) and polypyroline (PPy), have been used as electrodes for enhancing the cycling stability and lifetime, but the swelling and shrinking of the polymeric structure after the charge and discharge of the battery deteriorates the polymer’s performance.^9,38,39 For this purpose, the beneficial modification of conductive polymers with some transition metals, Ni, Co, and Cu, plays a vital role in structural-electrochemical stability and conductivity.^{13,17,39–41} The transition metals contribute to the capability of the battery’s capacity by providing a high number of transferred electrons as intercalation. Furthermore, the production of the coordination polymers with the transition metals enables the fast charging of a battery and improves the stable-cycling number. Our previous experiences showed that the preparation of the coordination polymers containing N and O donor atoms allows for the tuning of porous structures depending on the preparation methods. ^35,36,42 In addition to the methods, the type of monomeric unit, preparation method and metalation process play a key role in the behaviour of the polymer.^43–47 The monomeric units as linkers are one of the most important cases for achieving targeted compositions because of electrical conductivity and a 3D structure. If the linker has double bonds that allows the delocalisation of electron, then the conductivity rises. However, the linker, including the longer carbon chain, exhibits unconventional behaviours that mitigates the conductivity but develops the 3D structures. Therefore, we believe that this work sheds light on the effective parameters for the designing of new functionalised polymeric structures for different applications.

In this study, we present the production of imine-based polymers and their morphological, electrical and photoluminescent properties after the metalation processes. The produced compounds were characterised through elemental analysis, Fourier-transform infrared spectroscopy (FT-IR), thermogravimetric analysis (TGA), inductively coupled plasma (ICP), field emission scanning electron microscopy (FESEM), four-point probe conductivity (FPP), Brunauer–Emmett–Teller (BET), powder X-ray diffraction (PXRD) analysis, luminescent properties and magnetic susceptibility measurements. The results showed that the conductivity behaviours significantly changed after the metalation processes. Furthermore, the linkers play an important role in producing different 3D morphological and surface structures. This unique application opens new pathways for tuning a polymeric structure in the production of advanced materials.

Experiment

Materials

p- and m-phenylenediamine, glutaraldehyde (25% water solution), CoCl₂.6H₂O, NiCl₂.6H₂O, CuCl₂.2H₂O, ethanol, methanol and dichloromethane were commercially purchased. The pH values of the reactions were measured using the Hanna 211 pH metre. The infrared spectra were obtained on a Perkin-Elmer RX-1 (Potassium Bromide [KBr] disk; 4000–400 cm⁻¹) FT-IR spectrometer. The surface morphologies of the compounds were determined by Carl Zeiss, SUPRA-55. The TGA was performed with a Perkin-Elmer Pyris Diamond TG/DTA N₂ (30–900°C) at a heating rate of 10°C/min. A Perkin-Elmer Optima 2100 DV ICP-OES instrument was used for the ICP analysis. A Rigaku MiniFlex system with CuKα radiation (λ = 1.54,059 Å) was used for the PXRD studies. The single-photon fluorescence spectra of the compounds were collected on a Perkin-Elmer LS55 luminescence spectrometer. The magnetic susceptibility measurements were performed by using Sherwood Scientific magnetic susceptibility. The FPP electrical conductivity device and manual hydraulic pressure of 20,000.0 kg/cm² was used. The melting point of the produced materials was measured using the melting point apparatus B450 Buchi.

Methods

Synthesis of polymeric ligands

The polymeric ligands were prepared by the refluxing of (1.081 g, 10 mmol) for p-phenylenediamine and (1.081 g, 10 mmol) for m-phenylenediamine with corresponding glutaraldehyde (4.005 g in water solution, 10 mmol) in methanol (50 mL) for 3 h. The dark brown solution was filtered, and an insoluble solid was washed three times with 20 mL methanol. The produced polymer and metal complexes were dried under a 20-mbar vacuum for 12 h. The yields were calculated as 91.5% for P-1 and 94.6% for P-2, respectively (Figure 1) (P-1): Colour: light brown. Melting point (MP): <300^°C. Anal. Calcd. For C₁₂H₁₄N₂: C, 75.82; H, 8.10; N, 16.08. Found: C, 75.73; H, 7.64; N, 15.52%. FT-IR (KBr pellet, cm⁻¹): 3442–3342 υ(O-H) aromatic or water, 2942 υ(C-H) aliphatic, 1615 υ(CH = N), 1497 υ(C–C) aromatic.

Figure 1.

The structure of the polymeric ligands and the predicted metal complexes.

(P-2): Colour: dark brown. MP: <300^°C. Anal. Calcd. For C₁₂H₁₄N₂: C, 75.82; H, 8.10; N, 16.08. Found: C, 76.04; H, 8.17; N, 15.45%. FT-IR (KBr pellet, cm⁻¹): 3335 υ(O-H) aromatic or water, 2930 υ(C-H) aliphatic, 1656 υ(CH = N), 1505 υ(C–C) aromatic.

Synthesis of polymeric complexes

The polymeric complexes were prepared using the following template technique: p-phenylenediamine (1.081 g, 10 mmol) or m-phenylenediamine (1.081 g, 10 mmol) were dissolved in methanol (30 mL) at room temperature. After the dissociation of the monomer was completed, the metal salt was added to the solution. An appropriate amount of metal salt (0.238 g, 1 mmol) for CoCl₂.6H₂O; (0.237 g, 1 mmol), for NiCl₂.6H₂O; (0.170 g, 1 mmol) and for CuCl₂.2H₂O was dissolved in CH₃OH (20 mL) and added to the monomers solution. These reaction mixtures were heated under reflux for 1 h; the glutaraldehyde was added (4.005 g from 25% water solution, 10 mmol) in the reaction medium; and they were boiled for 3 hours. All of the polymeric metal complexes were collected by filtration, washed with MeOH and dried under a vacuum for 12 h (Figure 1).

(P¹-Cu): Yield: 89.6%, Colour: dark brown. MP: >300^°C. Anal. Calcd. For C₁₁H₁₃Cl₂N₂Cu: C, 42.94; H, 4.26; Cl, 21.97; Cu, 20.65; N, 9.10%; found: C, 41.60; H, 4.81; Cl, 19.56; Cu, 15.69; N, 8.60%. FT-IR (KBr pellet, cm⁻¹): 3434 and 3314 υ(O-H) water, 2960 υ(C-H) aliphatic, 1614 υ(CH = N), 1527 υ(C–C) aromatic, 583 υ(Cu-N).

(P¹-Co): Yield: 93.9%, Colour: dark brown. MP: >300^°C. Anal. Calcd. For C₁₁H₁₇Cl₂N₂O₂Co: C, 38.96; H, 5.05; Cl, 20.91; Co, 17.38; N, 8.26%; found: C, 40.90; H, 5.23; Cl, 18.94; Co, 15.12; N, 8.03%. FT-IR (KBr pellet, cm⁻¹): 3549 and 3330 υ(O-H) water, 2942 υ(C-H) aliphatic, 1611 υ(CH = N), 1498 υ(C–C) aromatic, 690 υ(Co-N).

(P¹-Ni): Yield: 92.4%, Colour: Brown. MP: >300^°C. Anal. Calcd. For C₁₁H₁₇Cl₂N₂O₂Ni: C, 38.99; H, 5.06; Cl, 20.92; Ni, 17.32; N, 8.27%; found: C, 40.37; H, 5.31; Cl, 19.76; Ni, 16.25; N, 7.51%. FT-IR (KBr pellet, cm⁻¹): 3320–3218 υ(O-H) water, 2930–2832 υ(C-H) aliphatic, 1610 υ(CH = N), 1497 υ(C–C) aromatic, 590 υ(Ni-N).

(P²-Cu): Yield: 91.7%, Colour: Brown. MP: >300^°C. Anal. Calcd. For C₁₁H₁₃Cl₂N₂Cu: C, 42.94; H, 4.26; Cl, 21.97; Cu, 20.65; N, 9.10%; found: C, 40.89; H, 5.04; Cl, 19.56; Cu, 15.69; N, 8.37%. FT-IR (KBr pellet, cm⁻¹): 3438 and 3317 υ(O-H) water, 2970 υ(C-H) aliphatic, 1610 υ(CH = N), 1505 υ(C–C) aromatic, 618 υ(Cu-N).

(P²-Co): Yield: 91.2%, Colour: dark brown. MP: >300^°C. Anal. Calcd. For C₁₁H₁₇Cl₂N₂O₂Co: C, 38.96; H, 5.05; Cl, 20.91; Co, 17.38; N, 8.26%; found: C, 40.43; H, 5.41; Cl, 18.94; Co, 15.12; N, 7.15%. FT-IR (KBr pellet, cm⁻¹): 3308 and 3240 υ(O-H) water, 2957 υ(C-H) aliphatic, 1601 υ(CH = N), 1506 υ(C–C) aromatic, 680 υ(Co-N).

(P²-Ni): Yield: 90.8%, Colour: brown. MP: >300^°C. Anal. Calcd. For C₁₁H₁₇Cl₂N₂O₂Ni: C, 38.99; H, 5.06; Cl, 20.92; Ni, 17.32; N, 8.27%; found: C, 40.28; H, 6.02; Cl, 19.76; Ni, 16.25; N, 8.49%. FT-IR (KBr pellet, cm⁻¹): 3299–3248 υ(O-H) water, 2940 υ(C-H) aliphatic, 1600 υ(CH = N), 1516 υ(C–C) aromatic, 624 υ(Ni-N).

Results and discussion

The physical and analytical properties of all the compounds were summarised in Table 1. According to the obtained elemental analysis data, the amount of the calculated hydrogen is lower than the theoretical calculation results. They overlapped with the TG/DTA results because of water molecules on the porous morphological structure or in the nano sized channel. As a consequence of the adsorbed water on the porous polymers, the other elements, such as C and N, have a lower value than the theoretical calculations. One other reason may concern the molecular structure of the polymer having a low coordination number; hence, the transition metals coordinated less than the theoretical calculation. The melting point of all the polymers and metal complexes was higher than 300^°C.

Table 1.

The ICP, elemental analysis and reaction yields of the compounds.

Compounds	Yield %	% Metal (ICP)	% Elemental Analysis
Compounds	Yield %	M_Cal./M_Found	C_Cal./C_Found	H_Cal./H_Found	N_Cal./N_Found
P ¹	91.5	—	75.82/75.73	8.10/7.64	16.08/15.52
P ¹ -Co	93.9	17.32/16.08	38.96/40.90	5.05/5.23	8.26/8.03
P ¹ -Ni	92.4	17.41/16.03	38.99/40.37	5.06/5.31	8.27/7.51
P ¹ -Cu	89.6	17.38/16.20	42.94/41.60	4.26/4.81	9.10/8.60
P ²	94.6	—	75.82/76.04	8.10/8.17	16.08/15.45
P ² -Co	91.2	17.32/16.48	38.96/40.43	5.05/5.41	8.26/7.15
P ² -Ni	90.8	17.32/16.48	38.99/40.28	5.06/6.02	8.27/8.49
P ² -Cu	91.7	17.38/15.28	42.94/40.89	4.26/5.04	9.10/8.37

*Cal: Calculated.

ICP: Inductively coupled plasma.

FT-IR Spectra

The FT-IR spectra of the polymeric ligands and their complexes are presented in Table 2 and Supplementary Figures S1–S8. A strong and broad absorption band at 1656 cm⁻¹ for P² and 1615 cm⁻¹ for P¹, as shown by the ligands, is attributable to the υ(C = N) stretching. In all the complexes, this band shifted the lower frequencies, indicating the coordination of azomethine nitrogen to the metal.^44,48 The donation of electrons through the azomethine nitrogen diminishes the (C = N) bond electron density, and hence, the υ(C = N) stretching shift of the lower frequencies. This is supported by the appearance of a new band in the 583–690 cm⁻¹ region due to the metal ligand bonding.⁴³ The broad absorption bands relative to the υ(O-H) stretching bands in the range of 3549–3218 cm⁻¹ are attributed to the coordination of water to metal for the polymeric metal complexes.

Table 2.

FT-IR spectral bands (cm⁻¹) and the magnetic susceptibility values of the compounds.

Compound	υ(OH)	υ(C = N)	υ(M-N)	M _eff (B.M.)	n
P ¹	3442–3342	1615	—	—	—
P ¹ -Cu	3434–3314	1614	583	1.91	1
P ¹ -Co	3549–3330	1611	690	5.19	3
P ¹ -Ni	3320–3218	1610	590	2.77	2
P ²	3335	1656	—	—	—
P ² -Cu	3438–3317	1610	618	1.97	1
P ² -Co	3308–3240	1601	680	4.36	3
P ² -Ni	3299–3248	1600	624	3.34	2

Magnetic properties of the complexes

According to the magnetic moment results (Table 2), the complex (P¹-Cu) and (P²-Cu) have tetrahedral or square planar geometry, but the other complexes (P¹-Co), (P¹-Ni), (P²-Co) and (P²-Ni) have octahedral geometries. The experimental μ_eff values for the polymeric complexes are within the range found for the polymeric complexes d⁹ for [(Cu(P¹)Cl₂].2H₂O (P¹-Cu), d⁷ for [Co(P¹)Cl₂(H₂O)₂] (P²-Cu), d⁸ for [Ni(P¹)Cl₂(H₂O)₂] (P¹-Ni), d⁹ for [Cu(P²)Cl₂].2H₂O] (P²-Cu), d⁷ for [Co(P²)Cl₂(H₂O)₂] (P²-Co) and d⁸ for [Ni(P²)Cl₂(H₂O)₂] (P²-Ni).

Thermogravimetric analysis

The TG/DTA curves of the compounds and explanations are given in Supplementary Figures S5–S7 in the supplementary data. The objective of this section is to analyse the thermal behaviour of the complexes. The confirmation of the composition of the polymeric structures and the evaluation of the crystal water molecules. The TG/DTA results were investigated in three parts. The first step is described as leaving the coordinated water molecules in the polymeric structures. Interesting results were observed from P¹Ni and P²Co that exothermic degradation of metalated polymers. The exothermic degradation causes the temperature rises than the program rate; therefore, the small peaks were discovered on the TG/DTA curves (Supplementary Figures S11 and S13).^49,50 The decomposition of the aromatic group from the polymers is the second part of the degradation of the polymeric structures depending on the monomeric unit. In the final step, the remaining substances are attributed as metal oxides depending on the metals and monomers.

Luminescence properties

The solid state emission and excitation studies of the polymers (P¹ and P²) and their metalated versions were investigated. The obtained data are given in Figure 2.

Figure 2.

Emission and excitation spectra of the ligands and complexes.

The photoluminescence properties of the ligands and their complexes were investigated in a solid state because of the insolubility of the polymers and the metalated polymers (Supplementary Table S1). The polymeric structure and its metal complexes have higher fluorescent intensive peaks. If they were compared with the previous studies, it could be explained by the polymeric structures consisting of a high number of the repeated units, such as benzene, the imine groups as a linker. The photoluminescent behaviours of the polymeric structures results from the benzene ring, the imine groups, π-π*, the ligand metal charge transfer (LMCT) and the metal ligand charge transfer (MLCT), respectively. Furthermore, the metalated polymeric structures in particular have multiple unpredictable inter-/intra-molecular interaction, which gives a unique rigidity, and the special crinkly shape of the polymers can be clearly seen in the FESEM images (Figures 3 and 4).⁵¹ Inter-/intra-molecular interactions and the induced-strain polymeric structure restricts the ability of the C–C bond rotation and the decreased regulated benzene π-π stacking on the polymeric structure. Therefore, the radiationless vibrational relaxation channels clearly reduce, and the fluorescent intensity of the polymers slightly increases without quenching.^37,52,53 Additionally, even the polymeric structure rigidity and the emission wavelength of the metalated polymers show a very small red shift towards the 5–6 nm lower energies. The photoluminescent properties of P¹ and P² and their metalated complexes have mostly overlapped excited and emission peaks that are located very intensively at approximately 290–300 nm and 590–615 nm, respectively. The main peaks seen at 300 nm are attributed to an intra-ligand transition π-π* backbone of the polymers, and the others appearing at around 600 nm are assigned to the mixture of the intra-ligand transition, the ligand metal charge transfer (LMCT) and the metal ligand charge transfer (MLCT).^54–57 If one of the interesting spectrums, which belongs to the P²-Co_em complexes, is compared with P², it reveals that they overlapped and shifted peaks at the 302 and 307 nm regions. These data also matche the FT-IR results (Table 2) of the imine group, where the metalated polymers have a lower frequency than the backbone of the polymers. It is especially seen that the imine peak exhibits a 56 cm⁻¹ red shift from the P² to P²-Co complex. This red shift is associated with the ligand metal charge transfer (LMCT) from the imine nitrogen to the metal d orbitals.^48,57

Figure 3.

Field emission scanning electron microscopy images of P¹ and their complexes.

Figure 4.

Field emission scanning electron microscopy images of P2 and their complexes.

The morphological analysis

The surface morphological structures of the compounds were inspected with FESEM.

The perspective descriptions of the polymeric ligands, P¹ and P², have an almost well-uniformed spherical shape, while the average size of P¹(a) is nearly 230 nm and 420 nm for P²(b), according to the size distribution results. It is clearly seen with the FESEM pictures that both the orientation of the polymeric structure slightly decreased to smaller sizes and diverse shapes after the metal complexes (Figures 3 and 4). Clearly, the polymeric complexes are also differentiated from each other depending on the transition metal, such as P²-Ni being a much smaller particle size of 21.6 nm. The P²-Cu is similar to the worm shape with a 120 nm length and 23.4 nm thickness. However, the P²-Co is almost 100 nm average sizes with the spherical shape. On the other hand, even though P¹ and P² are also spherical, the shape of the P¹ metal complexes slightly differs from P¹ and P². In addition to the difference between P¹ and P², each of the metal complexes has variety of the shape and size. For example, P¹-Co has a spherical shape with a 200 nm size and P¹-Cu is mostly angular shaped with an 18 nm size; however, P¹-Ni has round plate shape with the 20 nm average size. In comparing the P¹ complexes with the P², one of the biggest distinctions can be interestingly discovered between the shape of P¹-Cu, which is like a worm, and P²-Cu, which is angular. Thus, the FESEM results demonstrated that the polymers exhibit different shapes and sizes after the metalation processes.

Electrical conductivity

The FPP electrical conductivity values of the polymeric compounds were measured via the four-probe technique from the sample pellets, which designed 1 mm thick and 1.0 cm in diameter under a hydraulic pressure of 10 tons. The electrical conductivity test was calculated undoped with iodine during the experimental parts.

The XRD (Supplementary Figures S15 and S16), the FESEM and the BET results showed that the coordination of the nitrogen atom to the metals changed the direction of the monomeric unit in the polymer. Furthermore, according to the FT-IR data complexation of the polymer breaks of the π-π stacking on the polymer chain, which is seen as a red shift after the metalation, the electrical conductivity (Table 3) slightly decimated after the metalation processes.^57–63 The electrical conductivity is carried out through intra-molecular and inter-molecular interactions.⁶⁴ Conversely to P¹, P² has higher electrical conductivity, which could be illustrated by the intermolecular resonance through the polymeric structure. The resonance structures of the para position electrons are permitted to the delocalisation along with the polymeric structures, while the double-bond electrons on the meta position in the benzene ring are disallowed for the delocalisation on the polymer.^51,65,66 Therefore, the delocalisation of the electrons on the polymeric structures improves the conductivity.⁵ The intra-molecular forces, the π-π stacking and the hydrogen bonding of the nitrogen atoms on the imine group also contribute to the higher conductivity for the P² para position.^{14,63,64,67–69} Moreover, the very dark colour of the polymer and the metalated complexes correspond to the extended π system, and the polymers have higher conductivity than the monomeric structures.^60,70 The transition metals, which are π-d-conjugated coordination polymers, increase the conductivity. The diminishment of conductivity can be depending on the low coordination numbers.^{5,12,14–16,40,71} According to the experimental results, the amount of metal is lower than the theoretical calculation, which can be because the metals have a low coordination number on the polymeric structure.^72–74 The ICP, FT-IR and the conductivity results match perfectly because the number of the donated electrons change depending on the valance electron configuration of Co(d⁷), Ni(d⁸) and Cu(d⁹). The decrescent of the conductivity from Co(d⁷) and Ni(d⁸) to Cu(d⁹), respectively, is meaningful, which agrees with the electronic configuration of the transition metals. In a consequence of electronic configuration, the Co has higher electron deficiency if it is compared with the Ni and Cu; hence, the Co-metalated polymers perform the lowest conductivity. In addition to the previous data, the XRD pattern of the polymers and the metalated polymers were investigated (Supplementary Figures S15 and S16). The results demonstrated that new diffraction peaks appear after the metalation of the polymers, depending on the increasing crystallinity. However, the contribution of crystallinity on conductivity is still uncertain for our current XRD results, so it is not discussed in here.

Table 3.

Electrical conductivity and surface area results of the compounds.

Sample	Conductivity (S/cm)	BET Surface Area (m²/g)
P ¹	1.06x10⁻⁴	2.2593
P¹-Co	6.5x10⁻⁶	4.8402
P¹-Ni	6.6x10⁻⁶	0.9227
P¹-Cu	6.8x10⁻⁶	2.9936
P ²	1.5x10⁻¹	0.8163
P²-Co	2.2x10⁻⁵	1.8763
P²-Ni	6.6x10⁻⁵	2.6536
P²-Cu	7.3x10⁻⁵	1.0529

Conclusions

The insoluble and high-temperature melting point polymer that is more than 300^°C and its metalated complexes were successfully synthesised. According to the FESEM data, the coordination bonds during the metalation processes have revealed modification on the morphology of the polymers, shape and size. Similar to the FESEM and FT-IR data, the electrical conductivity of the polymer clearly diminished after metalation. The electrical conductivity showed a remarkable decrease because the new coordination bond breaks the π-π stacking and the delocalisation electrons on the polymeric structure. A similar effect is also shown for the surface area data increases after the metalation processes. Additionally, the data and all the other results also support and demonstrate that the coordination bond during the metalation processes causes a new morphological structure of the polymer; therefore, all of the properties changed slightly after the metalation processes.

Supplemental Material

sj-pdf-1-ppc-10.1177_09673911211048287 – Supplemental Material for The effect of metalation processes on polymer morphology and conductivity properties

Supplemental Material, sj-pdf-1-ppc-10.1177_09673911211048287 for The effect of metalation processes on polymer morphology and conductivity properties by Oğuz Yunus Sarıbıyık, İlyas Gönül, Burak Ay and Serkan Karaca in Polymers and Polymer Composites

Footnotes

Declaration of conflicting interests

The author(s) declared no potential conflicts of interest with respect to the research, authorship, and/or publication of this article.

Funding

The author(s) received no financial support for the research, authorship, and/or publication of this article.

ORCID iD

Oğuz Yunus Sarıbıyık

Supplementary material

Supplementary Material for this article is available online.

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