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International Journal of Industrial Chemistry

, Volume 8, Issue 3, pp 329–343 | Cite as

Synthesis, characterization and electrochemical properties of poly(phenoxy-imine)s containing carbazole unit

  • İsmet Kaya
  • Sebra Çöpür
  • Hatice Karaer
Open Access
Research
  • 968 Downloads

Abstract

Several new Schiff base polymers were synthesized via oxidative polymerization method in an aqueous alkaline medium in the presence of NaOCl as an oxidant and were confirmed by FT-IR, 1H-NMR, 13C-NMR and UV–Vis spectroscopic techniques. Furthermore, cyclic voltammetry measurements were carried out and the HOMO–LUMO energy levels and electrochemical band gaps (E g′) were calculated. Additionally, the optical band gaps (E g) were determined using their UV–Vis spectra of the materials. The morphologic properties of the polymers were investigated by scanning electron microscopy. In addition, the number average molecular weight (M n), weight average molecular weight (M w) and polydispersity index values of the polymers were determined by gel permeation chromatography technique. Electrical conductivity measurements of the doped (with iodine) and undoped polymer related to doping time were carried out by four-point probe technique using a Keithley 2400 electrometer. Their thermal behaviors were determined by TG–DTA and DSC measurements. The synthesized compounds were soluble in common solvents such as DMF, THF and DMSO. Photoluminescence properties of the polymers were determined in different concentrations of DMF solvent.

Keywords

Carbazole Fluorescence Thermal analysis Poly(phenoxy-imine) Band gaps 

Introduction

Poly(imine)s, known as Schiff base polymers or poly(azomethine)s or also named polyazines (when hydrazine is used as diamine compound) [1] which are of great interest to researchers because of to their potential applications and advantageous properties. Recently, polyazomethines have attracted much attention of both industries and academia and they have been widely investigated for their electrochemical properties, thermal stability, fluorescence, intrinsic conductivity [2].

Polyimines conjugated polymers have claimed the attention of researchers because of their potentially advantageous electronic applications, such as their electrical properties and environmentally stability, with acceptable mechanical strength [3]. Polyazomethines are conducting polymers [4] that usually show an optical absorption band in the visible region owing to their extended delocalization of the π electrons along the polymer backbone. Upon doping with suitable dopants, charge carriers, namely bipolaron and polaron, are formed in the conjugated backbone. This class of polymers was primarily found to be electroactive as well as semiconductive materials [5, 6], and their conductivity could be increased by doping with a dopant like iodine [2]. Furthermore, Schiff base polymers have been become increasingly interesting in the field of optical materials since they possess great potential for device applications like light-emitting diodes, photovoltaic cells and thin film transistors [7].

Poly(azomethine)s including conjugated bonding and active hydroxyl group have been studied for more than 60 years, and used in several fields [8]. The oxidative polymerization method is simply the reaction of compounds including –OH groups and active functional groups (–CHO, –NH2, –COOH) in their structure with the oxidants like air oxygen NaOCl, H2O2 an in the aqueous alkaline medium [9].

Carbazole-containing polymers are of great interest owing to their several potential for applications in organic electronics, such as organic solar cells, organic field effect transistors (OFET) and organic light-emitting devices (OLED), etc. [10].

In this study, new Schiff bases were synthesized by condensation reaction of 4-diethylaminosalicylaldehyde, 3,4-dihydroxybenzaldehyde and 2,4-dihydroxybenzaldehyde compounds with 3-amino-9-ethyl-carbazole. Then, these products were polymerized via oxidative polycondensation method in an aqueous alkaline medium in the presence of NaOCl as an oxidant. The structures of all compounds were confirmed by FT-IR, UV–Vis, 1H-NMR and 13C-NMR measurements. Thermal stabilities of all compounds were determined by TG–DTA and DSC measurements. Also, the conductivity and photoluminescence (PL) properties of polymers were determined from four-point probe technique and spectrofluorophotometer measurements, respectively.

Experimental

Materials

3-Amino-9-ethyl-carbazole, ethyl alcohol, ethyl acetate, chloroform, N,N-dimethylacetamide, N,N-dimethylformamide, dimethyl sulfoxide, acetonitrile and sodium hypochlorite (NaOCl, 37%) were supplied from Merck Chemical Co. (Germany). 4-Diethylamino salicylaldehyde (Alfa Aesar), 3,4-dihydroxybenzaldehyde (Fluka) and 2,4-dihydroxybenzaldehyde were supplied from Acros.

Synthesis of the monomers (DEACIMP, ACIMB and ACIBM)

The synthesis of 5-(diethylamino)-2-[(3-amino-9-ethyl-carbazole) imino methyl] phenol (DEACIMP) was synthesized according to the literature [11] (Scheme 1) as follows: 4-diethylamino salicylaldehyde (1.77 g) and 3-amino-9-ethyl-carbazole (1.95 g) were dissolved in 20 mL absolute ethanol in two separate beakers, which were then mixed. This mixture was refluxed for 5 h in a two-necked flask and cooled to room temperature. The precipitate formed was filtered, washed with ethanol and then dried under reduced pressure. The same procedure was used to obtain 4-[(3-amino-9-ethyl-carbazole) imino methyl] benzene-1,2-diol (ACIMB) and 4-[(3-amino-9-ethyl-carbazolyl) benzene imine methyl]-1,3-diol (ACIBM) the 3,4-dihydroxybenzaldehyde (1.38 g), 3-amino-9-ethyl-carbazole (1.95 g) and 2,4-dihydroxybenzaldehyde (1.38 g), 3-amino-9-ethyl-carbazole (1.95 g) were used for synthesis the ACIMB and ACIBM, respectively. The yields of DEACIMP, ACIMB and ACIBM compounds were found to be 80, 85, 89, respectively.
Scheme 1

Syntheses of Schiff bases and their polymers

General synthesis procedure of P-DEACIMP, P-ACIMB and P-ACIBM polymers

P-DEACIMP, P-ACIMB and P-ACIBM were synthesized through the oxidative polycondensation of DEACIMP, ACIMB and ACIBM with aqueous solution of NaOCl (10%). P-DEACIMP was synthesized through oxidative polycondensation of 5-(diethylamino)-2-[(3-amino-9-ethyl-carbazole) imino methyl] phenol using aqueous solution of NaOCl (10%). The 5-(diethylamino)-2-[(3-amino-9-ethyl-carbazole) imino methyl] phenol (0.385 g) was dissolved in an aqueous solution of 25 mL KOH (1.0 M) placed into a 100-mL three-necked round-bottom flask, which was fitted with a condenser, thermometer. Furthermore, a funnel containing NaOCl, which was added dropwise over about 30 min, was equipped. The reaction mixture was stirred at 100 °C for 24 h, cooled to room temperature and then 25 mL HCl (1.0 M) was added to solution. The P-DEACIMP was washed with water for the separation from mineral salt. The polymers were dried at 60 °C in an oven for 24 h [8, 12, 13].

The same procedure was used to obtain the P-ACIMB and P-ACIBM but the 4-[(3-amino-9-ethyl-carbazole) iminemethylbenzene]-1,2-diol (ACIMB) (0.33 g) and 4-[(3-amino-9-ethyl-carbazole) iminomethylbenzene]-1,3-diol (ACIBM) (0.33 g) were used for synthesis the P-ACIMB and P-ACIBM, respectively (Scheme 1). The yields of P-DEACIMP, P-ACIMB and P-ACIBM compounds were found to be 70, 72, 76, respectively.

Characterization techniques

A PerkinElmer spectrum one FT-IR system was used to determine the chemical structure of the monomers and polymers. Measurements were performed in solid powder form at room temperature using universal ATR sampling accessory within the wavelengths of 4000–650 cm−1. UV–Vis spectroscopy, was used to study the electronic transition in the UV–Vis region of the all compounds. Measurements were performed by an AnalytikJena Specord 210 Plus with wavelength range of 190–900 nm by ethyl alcohol solvent at 25 °C. 1H and 13C NMR spectra (Bruker AV400 FT-NMR spectrometer operating at 400.1 and 100.6 MHz, respectively) were also recorded in DMSO-d6 at 25 °C. The tetramethylsilane was used as internal standard. Thermal data were obtained by using a PerkinElmer diamond thermal analysis system. TGA–DTA measurements were performed between 20 and 1000 °C (in N2, rate 10 °C min−1). DSC analyses of polymers were carried out by a PerkinElmer Pyris sapphire DSC. DSC measurements were conducted between 25 and 450 °C (in N2, rate 10 °C min−1). The number average molecular weight (M n), weight average molecular weight (M w) and polydispersity index (PDI) were determined by gel permeation chromatography-light scattering (GPC-LS) device by Malvern Viscotek GPC Dual 270 max. For GPC investigations a medium 300 × 8.00 mm dual column light scattering detector (LS) and a refractive index detector (RID) were used to analyze the products at 55 °C. LiBr (40 mM) was added to the DMF mobile phase to dissociate molecular aggregates of polymer during GPC analysis. Surface morphology of the polymers was determined by scanning electron microscope (SEM) (JEOL, JSM-7100 model). Cyclic voltammetry (CV) measurements were carried out with a CH 660 C Electrochemical Analyzer (CH Instruments, Texas, USA) at a potential scan rate of 20 mV/s. A Shimadzu RF-5301PC spectrofluorophotometer was used in fluorescence measurements. Emission spectra of the synthesized polymers were obtained in different concentration of DMF solvent. Also, to obtain maximal emission intensity values of polymers were investigated in different concentrations of DMF solutions.

Results and discussion

Structural characterization of the monomers and polymers

The structures of the monomers and polymers were confirmed by FT-IR, 1H and 13C-NMR spectra. FT-IR spectra of the monomers and polymers are shown in Fig. 1. According to these spectra, the characteristic peaks such as etheric groups, aromatic and aliphatic C–H stretching peaks are observed, as expected. The peaks related to Ar–O bonds are in the range of 1217–1235 cm−1 [14], indicating that the polymerization was achieved. The bands due to hydroxyl groups (–OH) are observed at around 3300–3670 cm−1 (Fig. 1) [15].
Fig. 1

FT-IR spectra of the monomers and polymers

Aromatic –CH peaks were observed at around 2980 cm−1 for all the compounds. Furthermore, peaks at 1450–1650 cm−1 were assigned to benzene ring and (C=C) moiety and those at 1522–1590 cm−1 were attributed to (C–O) stretching [16] while peaks for aliphatic group were seen at 2900–2940 cm−1.

The peak at 1600–1620 cm−1 corresponds to –CH=N stretching vibration of imine moiety. The peaks of vibration bonding are also shown in Table 1. As seen in Fig. 1, peaks of polymers were broader than that of monomers after the polycondensation reaction owing to their polyconjugated structures. Other characteristic absorption bands are also presented in Table 1.
Table 1

FT-IR spectral data of monomers and polymers

Compounds

Wave number (cm−1)

–OH

C–H (aromatic)

C–H (aliphatic)

–C=N

C=C (aromatic)

C–O

DEACIMP

3300

2973

2936

1600

1587, 1522

P-DEACIMP

2978

2927

1604

1532, 1486

1227

ACIMB

3665

2976

2905

1615

1495, 1473

P-ACIMB

2979

2895

1602

1489, 1460

1223

ACIBM

3393

2983

2911

1608

1492, 1476

P-ACIBM

2976

2908

1608

1544, 1463

1217

Furthermore, the edged peaks of P-DEACIMP, P-ACIMB and P-ACIBM were broader and decreased numerically due to the increase in molecular weight after polymerization reactions [17], confirming polymerization of DEACIMP, ACIMB and ACIBM.

1H NMR and 13C NMR spectra of the monomers and polymers were recorded in DMSO-d6. 1H data of the monomers and polymers are listed in Table 2 and the spectrum of a representative polymer P-DEACIMP and DEACIMP are shown in Fig. 2. The 1H and 13C NMR spectra of DEACIMP and P-DEACIMP data are given in Figs. 2 and 3. 1H and 13C NMR data results of the synthesized compounds are listed in Table 2 except for DEACIMP and P-DEACIMP. When phenol-based Schiff bases were polymerized by oxidative polycondensation, they were combined by C–C binding at ortho and/or para position of the ring or alternatively C–O–C binding through oxygen atom of –OH moiety (Scheme 1) [2, 18]. 1H-NMR spectra of the polymers contained three types of signals assigned as follows: the singlet at 8.05–8.98 ppm, –CH=N–; the multiple at 6.40–8.50 ppm, aromatic protons. The proton resonances of hydroxyl (–OH) groups were observed at 12.01, 10.25 and 14.08, 10.24 and 14.07 ppm for DEACIMP, ACIMB and ACIBM, respectively. The proton signal of hydroxyl (–OH) groups were observed at 12.85, 11.02 and 13.20, 11.00 and 13.00 ppm for P-DEACIMP, P-ACIMB and P-ACIBM, respectively. Meanwhile, the FT-IR spectra of polymers show bands in 1217, 1223 and 1227 cm−1 is assignable to the phenolic C–O stretching vibration [2].
Table 2

NMR spectra data of the monomers and polymers

Compounds

NMR spectra data

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1H NMR (DMSO-d6, ppm, δ): 10.25 and 14.08 (s, –OH), 1.30 (t, Ar–He), 4.43 (m, Ar–Hd), 6.48–8.20 (m, Ar–H), 8.25 (s, –CH=N)

13C NMR (DMSO-d6, ppm, δ): 118 (C1-H), 121 (C2-H and C3-H), 126 (C4-ipso), 133 (C5-ipso), 109 (C6-H), 107 (C7-ipso), 138 (C8-ipso), 38 (C9-H), 14 (C10-H), 112 (C11-H), 160 (C12-ipso), 162 (C13-H), 139 (C14-ipso), 156 (C15-H), 140 (C16-H), 161 (C17-ipso), 129 (C18-H), 115 (C19-H), 122 (C20-H and C21-H)

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1H NMR (DMSO-d6, ppm, δ): 11.02 and 13.20 (s, –OH), 1.27 (t, Ar–He), 4.38 (q, Ar–Hd), 7.40–8.03 (m, Ar–H), 8.05 (s, –CH=N)

13C NMR (DMSO-d6, ppm, δ): 133 (C1-H), 110 (C2-H), 121 (C3-H), 118 (C4-H), 120 (C5-H), 126 (C6-ipso), 105 (C7-ipso), 135 (C8-ipso), 36 (C9-H), 14 (C10-H), 111 (C11-H), 160 (C12-ipso), 165 (C13-H), 118 (C14-ipso), 107 (C15-H), 126 (C16-ipso), 161 (C17-ipso), 123 (C18-ipso), 139 (C19-ipso), 125 (C20-H), 112 (C23-H)

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1H NMR (DMSO-d6, ppm, δ): 10.24 and 14.07 (s, –OH), 1.31 (t, Ar–He), 4.45 (m, Ar–Hd), 6.48–8.20 (m, Ar–H), 8.96 (s, –CH=N)

13C NMR (DMSO-d6, ppm, δ): 121 (C1-H), 119 (C2-H), 122 (C3-H and C4-H), 126 (C5-ipso), 109 (C6-H), 102 (C7-ipso), 133 (C8-ipso), 39 (C9-H), 15 (C10-H), 112 (C11-H), 140 (C12-ipso), 160 (C13-H), 118 (C14-ipso), 162 (C15-ipso and C18-ipso), 107 (C16-H), 118 (C17-H), 109 (C19-H), 121 (C20-H)

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1H NMR (DMSO-d6, ppm,) δ): 11.00 and 13.00 (s, –OH), 7.22–8.33 (m, Aromatic protons), 8.87 (s, –CH=N), 1.30 (t, Ar–He), 4.43 (m, Ar–Hd). 13C NMR (DMSO-d6, ppm, δ): 126 (C1-ipso), 107 (C2-H), 120 (C3-H), 116 (C4-H), 120 (C5-H), 125 (C6-ipso), 103 (C7-ipso), 127 (C8-ipso), 40 (C9-H), 14 (C10-ipso), 112 (C11-H), 140 (C12-ipso), 160 (C13-H), 110 (C14-ipso), 129 (C15-H), 116 (C16-ipso), 164 (C17-ipso), 126 (C18-ipso), 156 (C19-ipso), 112 (C20-H), 125 (C21-H)

Fig. 2

1H NMR spectra of DEACIMP and P-DEACIMP

Fig. 3

13C NMR spectra of DEACIMP and P-DEACIMP

The azomethine protons are observed in 8.84, 8.25 and 8.96 ppm for DEACIMP, ACIMB and ACIBM monomers, 8.90, 8.05 and 8.87 ppm for P-DEACIMP, P-ACIMB and P-ACIBM polymers, respectively. The 1H NMR spectra of polymers shows broad signals for aromatic protons which confirm the participation of aromatic ring in polymerization [2, 19]. New signals were observed in the region of 169, 162 and 168 ppm in the 13C NMR spectra of P-DEACIMP, P-ACIMB and P-ACIBM, respectively, due to –C–O–C– coupling, confirming polymerization occurred via –OH moiety [20].

Appearance of the new short resonances at 109,148 and 135,139 ppm obviously indicate polymerization of DEACIMP, ACIMB and ACIBM, respectively, i.e., –C–C binding occurs at ortho or para position of phenol by distribution of the phenoxy radical to the ring. The azomethine and aromatic carbon signals were observed at 159 and 97–163, 162 and 107–161, 160 and 102–162 ppm in the 13C NMR spectra of DEACIMP, ACIMB and ACIBM, respectively. Thus, we can easily conclude that the NMR data confirming the structures of the aimed products.

GPC analysis of polymers

Gel permeation chromatography (GPC) analyses of compounds (P-DEACIMP, P-ACIBM and P-ACIMB) were performed at 55 °C by DMF as eluent at a flow rate of 1.0 mL min−1. The number average molecular weight (M n), weight average molecular weight (M w) and polydispersity index (PDI, M w/M n) values of compounds were calculated according to a polystyrene standard calibration curve. The weight average molecular weight (M w) and polydispersity index (PDI, M w/M n) values of P-DEACIMP, P-ACIBM and P-ACIMB were found to be 8350, 6400, and 9200 and 1.25, 1.22 and 1.27, respectively. These results also agree with the solubility tests. P-ACIBM had lower molecular weight than P-DEACIMP and P-ACIMB polymers. So it was a fine-soluble polymer in common organic solvents and the others had lower solubilities owing to their high-molecular weighted structures.

Optical properties of compounds

UV–Vis spectra of the compounds recorded in ethyl alcohol at room temperature are given in Fig. 4. Their optical band gaps (E g) were calculated as in the literature [21] and results are shown in Table 3.
$$E_{\text{g}} = 1242/\lambda_{\text{onset}} ,$$
(1)
where λ onset is the onset wavelength which may be determined by intersection of two tangents on the absorption edges. λ onset also indicates the electronic transition start wavelength. According to results, one can easily conclude that the polymers have low optical band gaps. Because of monomers and polymers compounds to be having the same functional groups, some UV–V is absorption bands of their were observed as similar.
Fig. 4

Absorption spectra of the monomers and polymers (conc.: 100 mg L−1 in ethyl alcohol solvent)

Table 3

Optical electronic structure parameters of the monomers and polymers

Compound

E g a (eV)

λ onset (nm)

E ox b (eV)

E red c (eV)

HOMOd (eV)

LUMOe (eV)

E gf (eV)

DEACIMP

2.43

510

1.44

−1.73

−5.83

−2.66

3.17

P-DEACIMP

2.41

515

1.28

−1.30

−5.67

−3.09

2.58

ACIMB

2.60

478

1.32

−1.29

−5.71

−3.10

2.60

P-ACIMB

3.13

396

1.29

−1.23

−5.68

−3.16

2.51

ACIBM

3.05

406

0.92

−1.33

−5.31

−3.06

2.25

P-ACIBM

3.01

412

0.80

−0.74

−5.19

−3.65

1.54

aOptical band gap

bOxidation peak potential

cReduced peak potential

dHighest occupied molecular orbital

eLowest unoccupied molecular orbital

fElectrochemical band gap

It is known that the solubility behavior is very advantageous for the processing of these materials for technological applications [4]. Thus, the solubility properties of the polymers and monomers were tested in different solvents by using 1 mg of compound in 1 mL solvent and shown in Table 4.
Table 4

Solubility characteristics of the monomers and polymers (1 mg mL−1) at 25 °C

Solvent

DEACIMP

ACIMB

ACIBM

P-DEACIMP

P-ACIMB

P-ACIBM

DMF

+

+

+

+

+

+

DMA

+

+

+

+

+

+

DMSO

+

+

+

+

+

+

THF

+

+

+

+

+

+

Ethyl acetate

+

+

+

Chloroform

+

+

+

Acetone

+

+

+

Ethanol

+

+

+

Acetonitrile

+

+

+

+

(+), soluble; (⊥), partially soluble; (−), insoluble

Fluorescence properties of the synthesized compounds are determined using DMF solutions at different concentrations [22]. Also, the optimization of the concentrations to obtain maximal emission intensity is investigated in DMF. Concentration effects on the fluorescence properties are shown in Fig. 5. Maximum emission intensity values of the compounds are also given in Table 5. When concentration of DEACIMP, P-DEACIMP, ACIMB were decreased, they showed bathochromic shift in the range 14–35 nm. On the other hand, a significant change in the emission wavelength of these polymers was not observed. As seen in Table 5, these results showed that P-ACIMB polymer has higher emission intensity values at 9.76 × 10−6 and 1.95 × 10−5 g mL−1 than the other synthesized polymers and monomers. But P-DEACIMP and ACIBM have the lowest emission intensity as polymer and monomer, respectively.
Fig. 5

Emission spectra of the synthesized monomers and polymers in different concentrations (PL intensity photoluminescence intensity, slit width: 3 nm, in DMF solvent)

Table 5

The maximum emission intensity values that obtained from fluorescence spectra of the monomers and polymers as a function of concentration

Compounds

Concentration (mg mL−1)

a ƛ ex (nm)

b ƛ em (nm)

c ƛ max(ex) (nm)

d ƛ max(em) (nm)

e Ι ex

f Ι em

gΔƛ ST

DEACIMP

6.250 × 10−5

460

496

450

495

305

260

35

3.125 × 10−5

460

496

467

495

378

332

35

1.563 × 10−5

460

496

473

495

412

140

35

P-DEACIMP

1.250 × 10−3

513

555

498

561

272

200

48

6.250 × 10−4

513

555

512

561

264

258

48

3.125 × 10−4

513

555

532

561

247

34

48

ACIMB

6.250 × 10−4

475

514

460

515

243

117

60

3.125 × 10−4

475

514

474

515

237

241

60

1.563 × 10−4

475

514

484

515

233

204

60

P-ACIMB

3.90 × 10−5

416

478

385

447

574

302

31

1.95 × 10−5

416

478

380

447

>1000

338

31

9.75 × 10−6

416

478

375

447

>1000

317

31

ACIBM

2.250 × 10−3

528

568

526

561

233

204

33

1.125 × 10−3

528

568

519

561

237

117

33

5.625 × 10−4

528

568

518

561

243

241

33

P-ACIBM

7.80 × 10−4

384

449

381

445

224

589

61

3.90 × 10−4

384

449

380

445

602

586

61

1.95 × 10−4

384

449

379

445

572

558

61

aExcitation wavelength for emission

bEmission wavelength for excitation

cMaximum emission wavelength

dMaximum excitation wavelength

eMaximum excitation intensity

fMaximum emission intensity

gStokes shift

Stokes shift (Δλ ST) is the difference between positions of the band maxima of emission and excitation spectra of the same electronic transition. This knowledge offers significant conformational differences between ground state (S 0) and the first excited state (S 1). If the Δλ ST value is too small, the emission and excitation spectra will overlap more. So the emitted light will be self-absorbed and the photoluminescence efficiency will decrease. Δλ ST values are listed in Table 5. Δλ ST values of P-DEACIMP, P-ACIMB and P-ACIBM are calculated as 48, 31 and 61, respectively. According to Δλ ST values, the synthesized P-ACIBM can be used for the production of fluorescence sensor owing to high Δλ ST value [23]. It can be seen from Fig. 5 that with increase in the concentrations of the solutions, the absorption spectra of the compounds were observed to shift to the visible region.

Thermal properties of the polymers

Thermal degradation data (TGA–DTA and DTG) are listed in Table 6. TGA curves of the synthesized monomers and polymers are also shown in Fig. 6. According to the TGA results, the initial degradation temperatures (T on) of the monomers are higher than their polymers, expect for P-ACIBM. This could be explained by the formation of C–O etheric bond during polymerization. This weak bond is easily broken at mild temperatures and makes the polymer thermally unstable [21, 22]. Furthermore, when % char amounts are compared, % char of ACIMB was higher than other compounds at 1000 °C. In addition, Table 6 exhibits listed temperatures corresponding to 5, 10, 20 and 50% weight losses of the all compounds. T on values of monomers and polymers were found between 219–320 and 201–230 °C, respectively. According to TG curves of ACIMB, ACIBM, P-DEACIMP, P-ACIMB, and P-ACIBM, the losses of absorbed water were found to be 2, 1.7, 2.7, 5.1 and 3.9%, respectively, between 20 and 150 °C. DEACIMP monomer was degraded at the one step between 320 and 540 °C and its weight loss was 86.5% at this step. ACIMB and ACIBM monomers were degraded in two steps: between 220–385 and 219–308 for the first step; 385–690 and 308–665 °C for the second step and their weight losses were 23, 16; 21 and 35% at these steps, respectively. P-DEACIMP, P-ACIMB and P-ACIBM polymers were degraded in two steps: between 230–370, 209–380 and 201–620 for the first step; 370–570, 380–600 and 620–1000 °C for the second step and their weight losses were 53, 37, 50; 25, 22 and 14% at these steps, respectively.
Table 6

Thermal stabilities of the monomers and polymers

TGA/DTG DTA

Compounds

a T on

b T max

c T 5 (°C)

d T 10 (°C)

e T 20 (°C)

f T 50 (°C)

g% char

Endo (°C)

DEACIMP

320

367

330

348

359

376

9.5

127, 373

P-DEACIMP

230

270, 425

236

248

269

345

20.0

129

ACIMB

220

302, 478

235

263

351

54.0

P-ACIMB

209

316, 432

216

247

298

424

23.0

ACIBM

219

244, 419

232

248

315

534

43.0

223

P-ACIBM

201

412, 862

234

298

380

542

35.0

aThe onset temperature

bTemperature of the peak maxima

cTemperature corresponding to 5% weight loss

dTemperature corresponding to 10% weight loss

eTemperature corresponding to 20% weight loss

fTemperature corresponding to 50% weight loss

g% char at 1000 °C

Fig. 6

TGA–DTA–DTG curves of the monomers and polymers (heating rate: 10 C min−1; N2 atmosphere)

According to DSC measurements of polymers, the T g and C p values of P-DEACIMP, P-ACIMB, and P-ACIBM were found to be 123, 105 and 104 °C and 2.083, 0.086, and 0.075 J g−1 K−1, respectively. The results indicated that P-DEACIMP has the highest T g.

Morphologic properties

Morphological properties of the polymers are obtained by SEM technique. SEM images of compounds were recorded using a Jeol JSM-7100F Schottky instrument in a powder form. Polymers were prepared by sprinkling on double-sided adhesive tape mounted on a carbon stub and then they coated with a thin gold/palladium film by a sputter coater.

SEM photographs of P-DEACIMP, P-ACIBM and P-ACIMB are given in Fig. 7. According to the SEM images, P-ACIBM consists of different, nano-sized particles, while P-ACIMB has sharp edges with the form of rods. Surface of P-DEACIMP has the folds in the form of brain.
Fig. 7

SEM images of polymers

Electrochemical and conductivity properties

The voltammetric measurements were performed in acetonitrile. All the experiments were performed in a dry box filled with Ar at room temperature. The electrochemical potential of Ag was calibrated with respect to the ferrocene/ferrocenium (Fc/Fc+) couple. The half-wave potential (E1/2) of (Fc/Fc+) measured in 0.1 M tetrabutylammoniumhexafluorophosphate (TBAPF6) acetonitrile solution is 0.39 V with respect to Ag wire or 0.38 V with respect to saturated calomel electrolyte (SCE). The voltammetric measurements were carried out for all monomer compounds by acetonitrile and added to extra 1 mL DMF for polymers.

The values of electrochemical band gaps (E g′) are given in Table 3. These data were estimated by using the oxidation onset (E ox) and reduction onset (E red) values, as given in Fig. 8 for the compounds where E ox is the oxidation peak potential and E red is the reduction peak potential. The calculations were performed by using the following equations [24]:
$$E_{\text{HOMO}} = - \, \left( {4.39 + E_{\text{ox}} } \right)$$
(2)
$$E_{\text{LUMO}} = - \left( {4.39 + E_{\text{red}} } \right)$$
(3)
$$E_{\text{g}}^{\prime } = E_{\text{LUMO}} {-}E_{\text{HOMO}} .$$
(4)
To understand the electronic structure of conjugated polymers it is essential to establish the relative positions of the characteristic electronic energy levels such as the highest occupied molecular orbital (HOMO or п level), the lowest unoccupied molecular orbital (LUMO or п), and the associated energy parameters [25, 26].
Fig. 8

Cyclic voltammograms of the monomers and polymers

The oxidation peaks in cyclic voltammograms probably correspond to the oxidation of hydroxyl groups to form phenoxy radicals. The reduction peaks were presumably due to the reduction of the azomethine linkages via protonation of azomethine nitrogen [23].

According to the Table 3, the order of the electrochemical band gap values of the polymer changes are as follows: P-ACIBM > P-ACIMB > P-DEACIMP. This was a result of the polyconjugated structures of the polymers, which increase HOMO and decrease LUMO energy levels, resulting in lower electrochemical band gaps [23].

Conductivity was measured by a Keithley 2400 Electrometer (Keithley, Ohio, USA). The pellets were pressed on hydraulic press at 1687.2 kg/cm2. Iodine doping was carried out by exposing the pellets to iodine vapor at atmospheric pressure and room temperature in a desiccator. Solid-state conductivities of the polymers measured under air atmosphere were shown in a graph plotted versus time. The measurements for the polymers were carried out in pure form and then polymers were exposed to iodine vapor in a desiccator, and the change in their conductivities depending on time was measured at specific time intervals by doping. In the doping process, electron emitting amine nitrogen and electron pulling iodine coordinate, and the formation of radical cation (polaron) structure in polymer chain (on amine nitrogen) is enabled [27].

Electrical conductivities of the polymers and the changes of these values as a function of doping time with iodine were determined and shown in Fig. 9. Diaz et al. [28] suggested the doping mechanism of Schiff base polymers. According to doping mechanism, nitrogen, being a very electronegative element, is capable of coordinating with an iodine molecule (Scheme 2). Consequently, a charge-transfer complex between imine compound and dopant iodine forms and thus conductivity increases [29].
Fig. 9

Electrical conductivity changes of the polymers I2-doped at 25 °C

Scheme 2

The nitrogen atom coordination of iodine to the P-ACIBM

The conductivity values of the undoped P-DEACIMP, P-ACIBM, P-ACIMB polymers were about 4.35 10−8, 4.2 × 10−7 and 5.3 × 10−7 S cm−1, respectively. After 120 h doping, the conductivity of P-DEACIMP, P-ACIBM, P-ACIMB polymers were found to be around 1.78 × 10−5, 5.13 × 10−5 and 2.65 × 10−5 S cm−1, respectively. According to these results, increasing of the conductivity values of polymers were observed as connected iodine doping time.

Conclusions

Schiff base with different position of –OH group was oxidatively polymerized in aqueous alkaline medium by NaOCl as oxidant. The structures of the monomers and polymers were confirmed by UV–Vis, FT-IR, 1H, and 13C NMR spectroscopic techniques. According to 1H-NMR and 13C-NMR spectra, Schiff bases were polymerized by C–O–C or C–C binding. Iodine vapor-doped polymer P-DEACIMP gave the maximum electrical conductivity. The synthesized polymers have lower band gaps than the monomers because of polyconjugated structures. According to char % at 1000 °C, the thermal stability of the polymers was in the order P-ACIBM > P-ACIMB > P-DEACIMP. The synthesized compounds were all soluble in common solvents such as DMF, THF and DMSO. Because of carbazole units in the structures of these polymers, both conductivity and thermal properties were better than that of other imine polymers in literature. Electrochemical band gap values of P-DEACIMP, P-ACIBM and P-ACIMB were found to be 2.58, 1.54 and 2.51 eV, respectively.

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Authors and Affiliations

  1. 1.Polymer Synthesis and Analysis Laboratory, Department of ChemistryÇanakkale Onsekiz Mart UniversityÇanakkaleTurkey
  2. 2.Department of Chemistry, Faculty of SciencesDicle UniversityDiyarbakırTurkey

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