# Preparation of Organic Zn-Phthalocyanine-Based Semiconducting Materials and Their Optical and Electrochemical Characterization

Authors: Amira Hajri; Sarra Touaiti; Bassem Jamoussi
Journal: Advances in OptoElectronics
 (2013)

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## Abstract

In order to increase the species of organic semiconductors, new Zn-phthalocyanines-based organic materials were synthesized and characterized. The new compounds have been characterized by1H and 13C using NMR, FTIR, and UV-Vis. The absorption, fluorescence, and electrochemical properties were also studied. Green photoluminescence was observed in dilute solutions. In solid thin films, π-π* interactions influenced the optical properties, and redshifted photoluminescence spectra were obtained; red emissions for ZnPAL (647 nm) and ZnPTr (655 nm) were found. By cyclic voltammetry, the electrochemical band gap was estimated to be 1.94 and 1.17 eV for ZnPAl and ZnPTr, respectively. Single-layer diode devices of an indium tin oxide/Zn-phthalocyanine/aluminum configuration were fabricated and showed relatively low turn-on voltages (3.3 V for ZnPAl and 3 V for ZnPTr).


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## Body

## 1. Introduction

Phthalocyanines and related macrocycles have drawn considerable attention as molecular materials that give rise to outstanding electronic and optical properties. These properties arise from their electronic delocalization and make these compounds applicable in different fields of materials science; they are particularly promising as building blocks in nanotechnology. Some of the potential uses for phthalocyanines include nonlinear optical materials [1], liquid crystals [2], Langmuir-Blodgett (LB) films [3], optical data storage (computer recordable DVDs) [4], as electrochromic substances [5], low dimensional metals [6], and gas sensors [7], as photosensitizers [8], in photoelectrochemical cells [9] and electrophotographic applications [10]. Substitution has a strong influence on the π-electron conjugation of the macromolecule, since it makes salvation easier [11]. In recent years reports predict that a suitable functionalization of the M(Pc) molecules permits realizing more charge transfer processes decreasing [12], thus, the difference between HOMO and LUMO orbital (gap energy). We described herein, the synthesis and characterization of novel Zn(II) phthalocyanine derivatives which contain a 1,2,3 triazole unit on each benzo group, and tetra-substituted alkynyl phthalocyanine was synthesis for comparison purpose. ZnPcs structures were characterized by Fourier Transform Infrared Spectrophotometry (FTIR); we studied their electrochemical, optical (by UV-Vis absorption and photoluminescence spectroscopy), and electrical properties.


## 2. Experimental

### 2.1. Materials and Measurement

N,N′-dimethylformamide (DMF) were freshly used; alcohols and initiator products were purchased from Aldrich.1H-nuclear magnetic resonance (NMR) spectra were obtained using Bruker spectra AC 300 MHz. FTIR spectra were acquired on a Mattson 1000 Fourier transform spectrometer as KBr pellets and UV-Vis spectra on a Unicam UV-Vis spectrometer. Thin layer chromatography (TLC) was performed on precoated silica gel plates (0.25 mm, Merck). Column chromatography was performed on Merck silica gel having size 0.063–0.200 mm.Cyclic voltammetry was recorded using a VoltaLab 10 apparatus from Radiometer driven by the Volta Master software.Single-layer device elaborated a sandwich structure between an aluminium (Al) cathode and an indium tin oxide (ITO) anode. The solution of phthalocyanine (210−6 M in DMF) was deeply coated onto ITO glass to obtain a film about 40 nm thick after 1 h of annealing at 100°C. A thin aluminium layer was deposited by thermal evaporation at 3.10−6 Torr.Devices were fabricated and characterized in air at room temperature.Photoluminescence (PL) spectra were obtained on a spectra physics spectrometer 3900S with 2017 as stability.


### 2.2. Synthesis

The synthesis of the macrocycle zinc(II) phthalocyanines ZnPAl and ZnPTr begins with the nitration in position4 of phthalimide followed by reaction of the amine hydroxide [13], to form the 4-nitrophthalimide 2; the dehydration by the thionyl chloride in N,N-dimethylformamide [14] leads to 4-nitrophthalonitrile 3 (Scheme 1).Scheme 1
Reaction conditions: (i) HNO3, H2SO4, 0°C, 5 h; (ii) NHOH 25%; (iii) DMF, SOCl2, 0–2°C, 5 h.The 4-nitrophthalonitrile3 reacted with commercial propargyl alcohol 4 to obtain compound 5 in a reasonable 57% yield, followed by the amidation reaction to afford benzyl azide 6 (Scheme 1). The 1,3-dipolar cycloaddition of phthalonitrile 5 with compound 6 was carried out in DMF at room temperature using CuBr as a catalyst and triethylamine as a base to prevent the degradation of Cu(I) (Scheme 2).Scheme 2
Reaction conditions: (iv) K2CO3, DMF, 50°C, 72 h; (v) NaN3, DMF, rt, 6 h.Zinc(II) phthalocyanines8 and 9 were prepared by cyclotetramerization of phthalonitriles 5 and 7, respectively, in the presence of anhydrous Zn(OAc)2, urea, and nitrobenzene (Scheme 4).


#### 2.2.1. Synthesis of 4-Nitrophthalimide (1)

4-nitrophthalimide1 was prepared by nitration of phthalimide. Nitric acid (15.1 mL, 0.27 v/v) was slowly added to sulfuric acid (90.1 mL) (6 : 1) in round-bottom flask cooled in an ice bath. The solution was stirred for approximately 30 minutes. Afterward, the ice bath was removed, and the acidic solution was allowed to warm to room temperature. The phthalimide was stirred into the acid solution and heated at 35°C until a clear, colorless, and homogenous solution was achieved. As the phthalimide dissolved, the reaction became yellow. The reaction solution was stirred for 4 hours. A powdery white solid was precipitated from ice water, collected via vacuum filtration, and washed with deionized water. The precipitant was stirred under ambient conditions for 12 hours; an 80% yield was obtained. RMN1H (DMSO-d6): δ: 8.003 (d, J=5.7 Hz, 1H); 8.342 (s, 1H); 8.540 (d, J=6.9 Hz, 1H); 11.761 (s, 1H). RMN 13C (DMSO-d6) δ: 118.16; 124.92; 129.87; 134.42; 137.66; 151.71; 167.61; 167.91.


#### 2.2.2. Synthesis of 4-Nitrophthalimide (2)

4-Nitrophthalimide was stirred in 32% ammonia solution (70 mL) for 24 hours to obtain 4-nitrophthalimide2. The resulting deep yellow product was filtered and washed with cold water until the excess of ammonia could not be detected. The title compound was dried at 110°C, a 95% yield.RMN1H (DMSO-d6): δ: 7.636 (s, 2H); 7.704 (d, J=8.1, 1H); 8.020 (s, 1H); 8.079 (s, 1H); 8.297 (dd, J=2.4 Hz, J=8.7 Hz, 1H); 8.338 (d, J=2.1, 1H). RMN 13C (DMSO-d6) δ: 122.35; 124.38; 129.11; 137.19; 142; 65; 147.02; 167.67; 168.67.


#### 2.2.3. Synthesis of 4-Nitrophthalonitrile (3)

The 4-nitrophthalimide2 was converted to 4-nitrophthalonitrile via dehydration of the amide by using thionyl chloride and DMF as solvents.In a two-necked flask of 250 mL equipped with a mechanical stirrer, under nitrogen atmosphere and at a temperature 0–5°C, was placed 50 mL of N,N-dimethylformamide and was slowly added 20.87 mL of thionyl chloride (34 g, 0286 mole). To the reaction mixture 15 g of 4-nitrophthalimide was added, and the reaction was maintained for 18 hours to complete the dehydration reaction. The 4-nitrophthalonitrile was filtered after precipitation into a mixture of water-ice. the product was dried to yield 86% of pure product.RMN1H (DMSO-d6): δ: 8.439 (d, J=8.7, 1H); 8.685 (dd, J=2.1 Hz, J=8.4 Hz, 1H); 9.033 (d, J=2.1, 1H). RMN 13C (DMSO-d6) δ: 114.55; 114.86; 116.59; 120.22; 128.52; 128.81; 135.27; 149.69.FTIR: 3091 (C–H aromatic), 2242 (CN), 1534 (asymmetric N=O band), 1349 (symmetric N=O band), 853 (C–N).


#### 2.2.4. Synthesis of 4-(Propyn-3-yloxy) Phthalonitrile (5)

Yield 57%; 4-nitrophthalonitrile3 (0.5 g, 2.89 mmol) was dissolved in anhydrous DMF (25 mL) under nitrogen, and propargyl alcohol 4 (0.486 g, 8.67 mmol) was added. After stirring for 10 min, finely ground anhydrous K2CO3 (3.89 g, 28.9 mmol) was added in portions over 2 h with stirring. The reaction mixture was stirred at 50°C for 72 h under nitrogen. Then water (100 mL) was added, and the aqueous phase was extracted with chloroform. 1H nmr (DMSO-d6) δ: 3.75 (s, 1H, C≡CH); 5.01 (d, J=2.4 Hz, 2H, CH2–O–); 7.51 (dd, J=2.4 Hz, J=8.7 Hz, 1H); 7.82 (d, J=2.7 Hz, 1H); 8.11 (d, J=8.7 Hz, 1H). 13C nmr (DMSO-d6) δ: 56.6; 79.6; 115.5; 115.6; 116.4; 120.4; 120.6; 121.4; 135.8; 159.8.


#### 2.2.5. Synthesis of Benzyl Azide (6)

Yield 70%; NaN3 (1.54, 23.64 mmol) was added to a solution of benzyl chloride 4 (1 g, 8 mmol) in DMF, and the resulting mixture was stirred for 6 h at room temperature. The product was obtained after purification as a colorless oil. 1H nmr (CDCl3) δ: 4.40 (s, 2H, CH2N3); 7.40–7.49 (m, 5H, Ar). 13C nmr (CDCl3) δ: 54.8, 128.5, 128.6, 128.8, 128.8, 129.4, 153.5.


#### 2.2.6. Synthesis of 1-Benzyl-4-(3,4-dicyanophenoxymethyl)-1H-1,2,3-triazole (7)

Yield: 84%; a mixture of 4-(2-propyn-1-yn-oxy) phthalonitrile6 (0.695 g, 0.00374 mol), benzyl azide 5 (0.497 g, 0.00374 mol), triethylamine (0.377 g, 0.00374 mol), copper bromide (53 mg, 0.000374 mol), and 15 mL DMF was taken into round-bottom flask and stirred at room temperature for 24 h (Scheme 3). Progress of the reaction was monitored by TLC. After completion of the reaction, it was diluted with cold water, and the precipitate formed was filtered, washed with water and crystallized from methanol as white powder and recrystallized from methanol as white powder. 1H nmr (DMSO-d6) δ: 5.36 (s, 2H, CH2–O–), 5.64 (s, 2H, CH2–N), 7.36–7.57 (m, 6H, Ar), 7.88 (s, 1H, CH-Ar), 8.07 (s, 1H, CH-Ar), 8.66 (s, 1H, triazole). 13C nmr (DMSO-d6) δ: 52.9, 62.1, 106.3, 115.7 (2C), 120.5 (2C), 122.1, 128.0, 128.7 (4C), 135.8 (2C, CH2–O), 141.6 (C, CH2-arom), 143.6, 161.3 (C, O–CH2).Scheme 3
Reaction conditions: (vi) CuBr, Et3N, rt, 24 h.Scheme 4
Reaction conditions: (viii) ZnOAc2, nitrobenzene, urea, and ammonium molybdate.


#### 2.2.7. Synthesis of Zinc Tetrakis (Propyn-3-yloxy) Phthalocyanine (8)

Yield: 20% ZnPAl8 was prepared using compound 5 (0.179 g, 0.984 mmol), urea (0.174 g, 2.901 mmol), zinc acetate (0.053 g, 0.243 mmol), and ammonium molybdate and heated in nitrobenzene at 160°C for 8 h. After cooling, the reaction mixture was treated with water. the green dark product that precipitated was filtered off, successively washed with water and hot methanol. UV-Vis λmax in DMF (680 nm):1H nmr (DMSO-d6) δ: 2.34 (s, 4H, C≡CH); 3.49 (s, 8H, CH2–O–); 7.70 (m, 4H, Ar-H); 7.86 (m, 4H, Ar-H); 8.27 (m, 4H, Ar-H). FT-IR γ (cm−1): 3280 (H–C≡CH), 2800 (CH, aliphatic), 2200 (–C≡C–).


#### 2.2.8. Synthesis of Zinc Phthalocyanine (9)

Yield: 10%; Following a similar synthetic procedure, 1-benzyl-4-(3,4-dicyanophenoxy)-1H-1,2,3-triazole7 (0.155 g, 0.492 mmol), urea (0.087 g, 1,450 mmol), zinc acetate (0,026 g, 0,121 mmol), and ammonium molybdate (0,012 g, 0.01 mmol) were suspended in nitrobenzene (2 mL) and heated at 160°C for 8 h. Yield: (10%) UV-Vis λ max in DMF (700 nm); 1H nmr (DMSO-d6) δ: 5.13 (s, 8H, CH2–O–), 5.58 (s, 8H, CH2–N), 7.67–7.88 (m, 32H, Ar-H/Pc-H), 8.34 (s, 4H, triazole). FT-IR γ (cm−1): 3050 (CH, triazole), 3030 (CH, aromatic), 2850 (CH, aliphatic).


## 2.1. Materials and Measurement

N,N′-dimethylformamide (DMF) were freshly used; alcohols and initiator products were purchased from Aldrich.1H-nuclear magnetic resonance (NMR) spectra were obtained using Bruker spectra AC 300 MHz. FTIR spectra were acquired on a Mattson 1000 Fourier transform spectrometer as KBr pellets and UV-Vis spectra on a Unicam UV-Vis spectrometer. Thin layer chromatography (TLC) was performed on precoated silica gel plates (0.25 mm, Merck). Column chromatography was performed on Merck silica gel having size 0.063–0.200 mm.Cyclic voltammetry was recorded using a VoltaLab 10 apparatus from Radiometer driven by the Volta Master software.Single-layer device elaborated a sandwich structure between an aluminium (Al) cathode and an indium tin oxide (ITO) anode. The solution of phthalocyanine (210−6 M in DMF) was deeply coated onto ITO glass to obtain a film about 40 nm thick after 1 h of annealing at 100°C. A thin aluminium layer was deposited by thermal evaporation at 3.10−6 Torr.Devices were fabricated and characterized in air at room temperature.Photoluminescence (PL) spectra were obtained on a spectra physics spectrometer 3900S with 2017 as stability.


## 2.2. Synthesis

The synthesis of the macrocycle zinc(II) phthalocyanines ZnPAl and ZnPTr begins with the nitration in position4 of phthalimide followed by reaction of the amine hydroxide [13], to form the 4-nitrophthalimide 2; the dehydration by the thionyl chloride in N,N-dimethylformamide [14] leads to 4-nitrophthalonitrile 3 (Scheme 1).Scheme 1
Reaction conditions: (i) HNO3, H2SO4, 0°C, 5 h; (ii) NHOH 25%; (iii) DMF, SOCl2, 0–2°C, 5 h.The 4-nitrophthalonitrile3 reacted with commercial propargyl alcohol 4 to obtain compound 5 in a reasonable 57% yield, followed by the amidation reaction to afford benzyl azide 6 (Scheme 1). The 1,3-dipolar cycloaddition of phthalonitrile 5 with compound 6 was carried out in DMF at room temperature using CuBr as a catalyst and triethylamine as a base to prevent the degradation of Cu(I) (Scheme 2).Scheme 2
Reaction conditions: (iv) K2CO3, DMF, 50°C, 72 h; (v) NaN3, DMF, rt, 6 h.Zinc(II) phthalocyanines8 and 9 were prepared by cyclotetramerization of phthalonitriles 5 and 7, respectively, in the presence of anhydrous Zn(OAc)2, urea, and nitrobenzene (Scheme 4).


### 2.2.1. Synthesis of 4-Nitrophthalimide (1)

4-nitrophthalimide1 was prepared by nitration of phthalimide. Nitric acid (15.1 mL, 0.27 v/v) was slowly added to sulfuric acid (90.1 mL) (6 : 1) in round-bottom flask cooled in an ice bath. The solution was stirred for approximately 30 minutes. Afterward, the ice bath was removed, and the acidic solution was allowed to warm to room temperature. The phthalimide was stirred into the acid solution and heated at 35°C until a clear, colorless, and homogenous solution was achieved. As the phthalimide dissolved, the reaction became yellow. The reaction solution was stirred for 4 hours. A powdery white solid was precipitated from ice water, collected via vacuum filtration, and washed with deionized water. The precipitant was stirred under ambient conditions for 12 hours; an 80% yield was obtained. RMN1H (DMSO-d6): δ: 8.003 (d, J=5.7 Hz, 1H); 8.342 (s, 1H); 8.540 (d, J=6.9 Hz, 1H); 11.761 (s, 1H). RMN 13C (DMSO-d6) δ: 118.16; 124.92; 129.87; 134.42; 137.66; 151.71; 167.61; 167.91.


### 2.2.2. Synthesis of 4-Nitrophthalimide (2)

4-Nitrophthalimide was stirred in 32% ammonia solution (70 mL) for 24 hours to obtain 4-nitrophthalimide2. The resulting deep yellow product was filtered and washed with cold water until the excess of ammonia could not be detected. The title compound was dried at 110°C, a 95% yield.RMN1H (DMSO-d6): δ: 7.636 (s, 2H); 7.704 (d, J=8.1, 1H); 8.020 (s, 1H); 8.079 (s, 1H); 8.297 (dd, J=2.4 Hz, J=8.7 Hz, 1H); 8.338 (d, J=2.1, 1H). RMN 13C (DMSO-d6) δ: 122.35; 124.38; 129.11; 137.19; 142; 65; 147.02; 167.67; 168.67.


### 2.2.3. Synthesis of 4-Nitrophthalonitrile (3)

The 4-nitrophthalimide2 was converted to 4-nitrophthalonitrile via dehydration of the amide by using thionyl chloride and DMF as solvents.In a two-necked flask of 250 mL equipped with a mechanical stirrer, under nitrogen atmosphere and at a temperature 0–5°C, was placed 50 mL of N,N-dimethylformamide and was slowly added 20.87 mL of thionyl chloride (34 g, 0286 mole). To the reaction mixture 15 g of 4-nitrophthalimide was added, and the reaction was maintained for 18 hours to complete the dehydration reaction. The 4-nitrophthalonitrile was filtered after precipitation into a mixture of water-ice. the product was dried to yield 86% of pure product.RMN1H (DMSO-d6): δ: 8.439 (d, J=8.7, 1H); 8.685 (dd, J=2.1 Hz, J=8.4 Hz, 1H); 9.033 (d, J=2.1, 1H). RMN 13C (DMSO-d6) δ: 114.55; 114.86; 116.59; 120.22; 128.52; 128.81; 135.27; 149.69.FTIR: 3091 (C–H aromatic), 2242 (CN), 1534 (asymmetric N=O band), 1349 (symmetric N=O band), 853 (C–N).


### 2.2.4. Synthesis of 4-(Propyn-3-yloxy) Phthalonitrile (5)

Yield 57%; 4-nitrophthalonitrile3 (0.5 g, 2.89 mmol) was dissolved in anhydrous DMF (25 mL) under nitrogen, and propargyl alcohol 4 (0.486 g, 8.67 mmol) was added. After stirring for 10 min, finely ground anhydrous K2CO3 (3.89 g, 28.9 mmol) was added in portions over 2 h with stirring. The reaction mixture was stirred at 50°C for 72 h under nitrogen. Then water (100 mL) was added, and the aqueous phase was extracted with chloroform. 1H nmr (DMSO-d6) δ: 3.75 (s, 1H, C≡CH); 5.01 (d, J=2.4 Hz, 2H, CH2–O–); 7.51 (dd, J=2.4 Hz, J=8.7 Hz, 1H); 7.82 (d, J=2.7 Hz, 1H); 8.11 (d, J=8.7 Hz, 1H). 13C nmr (DMSO-d6) δ: 56.6; 79.6; 115.5; 115.6; 116.4; 120.4; 120.6; 121.4; 135.8; 159.8.


### 2.2.5. Synthesis of Benzyl Azide (6)

Yield 70%; NaN3 (1.54, 23.64 mmol) was added to a solution of benzyl chloride 4 (1 g, 8 mmol) in DMF, and the resulting mixture was stirred for 6 h at room temperature. The product was obtained after purification as a colorless oil. 1H nmr (CDCl3) δ: 4.40 (s, 2H, CH2N3); 7.40–7.49 (m, 5H, Ar). 13C nmr (CDCl3) δ: 54.8, 128.5, 128.6, 128.8, 128.8, 129.4, 153.5.


### 2.2.6. Synthesis of 1-Benzyl-4-(3,4-dicyanophenoxymethyl)-1H-1,2,3-triazole (7)

Yield: 84%; a mixture of 4-(2-propyn-1-yn-oxy) phthalonitrile6 (0.695 g, 0.00374 mol), benzyl azide 5 (0.497 g, 0.00374 mol), triethylamine (0.377 g, 0.00374 mol), copper bromide (53 mg, 0.000374 mol), and 15 mL DMF was taken into round-bottom flask and stirred at room temperature for 24 h (Scheme 3). Progress of the reaction was monitored by TLC. After completion of the reaction, it was diluted with cold water, and the precipitate formed was filtered, washed with water and crystallized from methanol as white powder and recrystallized from methanol as white powder. 1H nmr (DMSO-d6) δ: 5.36 (s, 2H, CH2–O–), 5.64 (s, 2H, CH2–N), 7.36–7.57 (m, 6H, Ar), 7.88 (s, 1H, CH-Ar), 8.07 (s, 1H, CH-Ar), 8.66 (s, 1H, triazole). 13C nmr (DMSO-d6) δ: 52.9, 62.1, 106.3, 115.7 (2C), 120.5 (2C), 122.1, 128.0, 128.7 (4C), 135.8 (2C, CH2–O), 141.6 (C, CH2-arom), 143.6, 161.3 (C, O–CH2).Scheme 3
Reaction conditions: (vi) CuBr, Et3N, rt, 24 h.Scheme 4
Reaction conditions: (viii) ZnOAc2, nitrobenzene, urea, and ammonium molybdate.


### 2.2.7. Synthesis of Zinc Tetrakis (Propyn-3-yloxy) Phthalocyanine (8)

Yield: 20% ZnPAl8 was prepared using compound 5 (0.179 g, 0.984 mmol), urea (0.174 g, 2.901 mmol), zinc acetate (0.053 g, 0.243 mmol), and ammonium molybdate and heated in nitrobenzene at 160°C for 8 h. After cooling, the reaction mixture was treated with water. the green dark product that precipitated was filtered off, successively washed with water and hot methanol. UV-Vis λmax in DMF (680 nm):1H nmr (DMSO-d6) δ: 2.34 (s, 4H, C≡CH); 3.49 (s, 8H, CH2–O–); 7.70 (m, 4H, Ar-H); 7.86 (m, 4H, Ar-H); 8.27 (m, 4H, Ar-H). FT-IR γ (cm−1): 3280 (H–C≡CH), 2800 (CH, aliphatic), 2200 (–C≡C–).


### 2.2.8. Synthesis of Zinc Phthalocyanine (9)

Yield: 10%; Following a similar synthetic procedure, 1-benzyl-4-(3,4-dicyanophenoxy)-1H-1,2,3-triazole7 (0.155 g, 0.492 mmol), urea (0.087 g, 1,450 mmol), zinc acetate (0,026 g, 0,121 mmol), and ammonium molybdate (0,012 g, 0.01 mmol) were suspended in nitrobenzene (2 mL) and heated at 160°C for 8 h. Yield: (10%) UV-Vis λ max in DMF (700 nm); 1H nmr (DMSO-d6) δ: 5.13 (s, 8H, CH2–O–), 5.58 (s, 8H, CH2–N), 7.67–7.88 (m, 32H, Ar-H/Pc-H), 8.34 (s, 4H, triazole). FT-IR γ (cm−1): 3050 (CH, triazole), 3030 (CH, aromatic), 2850 (CH, aliphatic).


## 2.2.1. Synthesis of 4-Nitrophthalimide (1)

4-nitrophthalimide1 was prepared by nitration of phthalimide. Nitric acid (15.1 mL, 0.27 v/v) was slowly added to sulfuric acid (90.1 mL) (6 : 1) in round-bottom flask cooled in an ice bath. The solution was stirred for approximately 30 minutes. Afterward, the ice bath was removed, and the acidic solution was allowed to warm to room temperature. The phthalimide was stirred into the acid solution and heated at 35°C until a clear, colorless, and homogenous solution was achieved. As the phthalimide dissolved, the reaction became yellow. The reaction solution was stirred for 4 hours. A powdery white solid was precipitated from ice water, collected via vacuum filtration, and washed with deionized water. The precipitant was stirred under ambient conditions for 12 hours; an 80% yield was obtained. RMN1H (DMSO-d6): δ: 8.003 (d, J=5.7 Hz, 1H); 8.342 (s, 1H); 8.540 (d, J=6.9 Hz, 1H); 11.761 (s, 1H). RMN 13C (DMSO-d6) δ: 118.16; 124.92; 129.87; 134.42; 137.66; 151.71; 167.61; 167.91.


## 2.2.2. Synthesis of 4-Nitrophthalimide (2)

4-Nitrophthalimide was stirred in 32% ammonia solution (70 mL) for 24 hours to obtain 4-nitrophthalimide2. The resulting deep yellow product was filtered and washed with cold water until the excess of ammonia could not be detected. The title compound was dried at 110°C, a 95% yield.RMN1H (DMSO-d6): δ: 7.636 (s, 2H); 7.704 (d, J=8.1, 1H); 8.020 (s, 1H); 8.079 (s, 1H); 8.297 (dd, J=2.4 Hz, J=8.7 Hz, 1H); 8.338 (d, J=2.1, 1H). RMN 13C (DMSO-d6) δ: 122.35; 124.38; 129.11; 137.19; 142; 65; 147.02; 167.67; 168.67.


## 2.2.3. Synthesis of 4-Nitrophthalonitrile (3)

The 4-nitrophthalimide2 was converted to 4-nitrophthalonitrile via dehydration of the amide by using thionyl chloride and DMF as solvents.In a two-necked flask of 250 mL equipped with a mechanical stirrer, under nitrogen atmosphere and at a temperature 0–5°C, was placed 50 mL of N,N-dimethylformamide and was slowly added 20.87 mL of thionyl chloride (34 g, 0286 mole). To the reaction mixture 15 g of 4-nitrophthalimide was added, and the reaction was maintained for 18 hours to complete the dehydration reaction. The 4-nitrophthalonitrile was filtered after precipitation into a mixture of water-ice. the product was dried to yield 86% of pure product.RMN1H (DMSO-d6): δ: 8.439 (d, J=8.7, 1H); 8.685 (dd, J=2.1 Hz, J=8.4 Hz, 1H); 9.033 (d, J=2.1, 1H). RMN 13C (DMSO-d6) δ: 114.55; 114.86; 116.59; 120.22; 128.52; 128.81; 135.27; 149.69.FTIR: 3091 (C–H aromatic), 2242 (CN), 1534 (asymmetric N=O band), 1349 (symmetric N=O band), 853 (C–N).


## 2.2.4. Synthesis of 4-(Propyn-3-yloxy) Phthalonitrile (5)

Yield 57%; 4-nitrophthalonitrile3 (0.5 g, 2.89 mmol) was dissolved in anhydrous DMF (25 mL) under nitrogen, and propargyl alcohol 4 (0.486 g, 8.67 mmol) was added. After stirring for 10 min, finely ground anhydrous K2CO3 (3.89 g, 28.9 mmol) was added in portions over 2 h with stirring. The reaction mixture was stirred at 50°C for 72 h under nitrogen. Then water (100 mL) was added, and the aqueous phase was extracted with chloroform. 1H nmr (DMSO-d6) δ: 3.75 (s, 1H, C≡CH); 5.01 (d, J=2.4 Hz, 2H, CH2–O–); 7.51 (dd, J=2.4 Hz, J=8.7 Hz, 1H); 7.82 (d, J=2.7 Hz, 1H); 8.11 (d, J=8.7 Hz, 1H). 13C nmr (DMSO-d6) δ: 56.6; 79.6; 115.5; 115.6; 116.4; 120.4; 120.6; 121.4; 135.8; 159.8.


## 2.2.5. Synthesis of Benzyl Azide (6)

Yield 70%; NaN3 (1.54, 23.64 mmol) was added to a solution of benzyl chloride 4 (1 g, 8 mmol) in DMF, and the resulting mixture was stirred for 6 h at room temperature. The product was obtained after purification as a colorless oil. 1H nmr (CDCl3) δ: 4.40 (s, 2H, CH2N3); 7.40–7.49 (m, 5H, Ar). 13C nmr (CDCl3) δ: 54.8, 128.5, 128.6, 128.8, 128.8, 129.4, 153.5.


## 2.2.6. Synthesis of 1-Benzyl-4-(3,4-dicyanophenoxymethyl)-1H-1,2,3-triazole (7)

Yield: 84%; a mixture of 4-(2-propyn-1-yn-oxy) phthalonitrile6 (0.695 g, 0.00374 mol), benzyl azide 5 (0.497 g, 0.00374 mol), triethylamine (0.377 g, 0.00374 mol), copper bromide (53 mg, 0.000374 mol), and 15 mL DMF was taken into round-bottom flask and stirred at room temperature for 24 h (Scheme 3). Progress of the reaction was monitored by TLC. After completion of the reaction, it was diluted with cold water, and the precipitate formed was filtered, washed with water and crystallized from methanol as white powder and recrystallized from methanol as white powder. 1H nmr (DMSO-d6) δ: 5.36 (s, 2H, CH2–O–), 5.64 (s, 2H, CH2–N), 7.36–7.57 (m, 6H, Ar), 7.88 (s, 1H, CH-Ar), 8.07 (s, 1H, CH-Ar), 8.66 (s, 1H, triazole). 13C nmr (DMSO-d6) δ: 52.9, 62.1, 106.3, 115.7 (2C), 120.5 (2C), 122.1, 128.0, 128.7 (4C), 135.8 (2C, CH2–O), 141.6 (C, CH2-arom), 143.6, 161.3 (C, O–CH2).Scheme 3
Reaction conditions: (vi) CuBr, Et3N, rt, 24 h.Scheme 4
Reaction conditions: (viii) ZnOAc2, nitrobenzene, urea, and ammonium molybdate.


## 2.2.7. Synthesis of Zinc Tetrakis (Propyn-3-yloxy) Phthalocyanine (8)

Yield: 20% ZnPAl8 was prepared using compound 5 (0.179 g, 0.984 mmol), urea (0.174 g, 2.901 mmol), zinc acetate (0.053 g, 0.243 mmol), and ammonium molybdate and heated in nitrobenzene at 160°C for 8 h. After cooling, the reaction mixture was treated with water. the green dark product that precipitated was filtered off, successively washed with water and hot methanol. UV-Vis λmax in DMF (680 nm):1H nmr (DMSO-d6) δ: 2.34 (s, 4H, C≡CH); 3.49 (s, 8H, CH2–O–); 7.70 (m, 4H, Ar-H); 7.86 (m, 4H, Ar-H); 8.27 (m, 4H, Ar-H). FT-IR γ (cm−1): 3280 (H–C≡CH), 2800 (CH, aliphatic), 2200 (–C≡C–).


## 2.2.8. Synthesis of Zinc Phthalocyanine (9)

Yield: 10%; Following a similar synthetic procedure, 1-benzyl-4-(3,4-dicyanophenoxy)-1H-1,2,3-triazole7 (0.155 g, 0.492 mmol), urea (0.087 g, 1,450 mmol), zinc acetate (0,026 g, 0,121 mmol), and ammonium molybdate (0,012 g, 0.01 mmol) were suspended in nitrobenzene (2 mL) and heated at 160°C for 8 h. Yield: (10%) UV-Vis λ max in DMF (700 nm); 1H nmr (DMSO-d6) δ: 5.13 (s, 8H, CH2–O–), 5.58 (s, 8H, CH2–N), 7.67–7.88 (m, 32H, Ar-H/Pc-H), 8.34 (s, 4H, triazole). FT-IR γ (cm−1): 3050 (CH, triazole), 3030 (CH, aromatic), 2850 (CH, aliphatic).


## 3. Results and Discussion

### 3.1. Optical Properties

#### 3.1.1. Electronic Absorption Spectra

The ground state electronic spectra are especially useful to identify the structure of the phthalocyanines. Generally, UV-Vis spectra of phthalocyanines show typical electronic spectra with two strong absorption bands known as Q and B bands. The Q band in the visible region at ca. 600–750 nm is attributed to theπ-π* transition from the highest occupied molecular orbital (HOMO) to the lowest unoccupied molecular orbital (LUMO) of the Pc ring and the B band in the UV region at 300–400 nm [15, 16]. The ground state electronic absorption spectra of the peripherally tetra-substituted phthalocyanine complexes showed monomeric behavior evidenced by a single (narrow) Q band, typical of nonaggregated metallophthalocyanine complexes in THF and DMF.The electronic spectra of Zn-phthalocyanine compounds (ZnPAl, ZnPTr) in DMF and THF are given in Figure1.Figure 1
UV-Visible absorption spectra of ZnPAl (red line) and ZnPTr (green line) in DMF solution, ZnPAl (black line) and ZnPTr (blue line) in THF solution (410−5M).The UV-Vis absorption spectra of ZnPAl and ZnPTr in DMF showed intense Q absorption at 685 and 700 nm, respectively. The Q band absorptions were also observed at 670 nm and 683 nm, respectively, for ZnPAL and ZnPTr in THF. In addition, the intense B band absorptions in DMF were observed at 349 nm for ZnPAl and 381 nm for ZnPTr but 340 nm for ZnPAl and 352 nm for ZnPTr in THF (Figure1).The electronic absorption transitions of these compounds are strongly dependent on the type of the substituent (withdrawing or donating groups) as well as the type of the metal ion and its position (in the centre or on peripheral position) [17].Peripheral substitution of phthalocyanine by triazole chains gave bathochromic shifts of the Q band [18–20] in both studied solvents, which can be explained by the concomitant effect of the presence of triazole ring which possesses three nitrogen atoms and, thus, can serve as a ligand to coordinate metals or as a hydrogen bond acceptor and donor.The optical band gaps were estimated from the absorption onset of the phtalocyanines solutions. Table1 summarizes these spectral data.Table 1
Optical data for ZnPAl and ZnPTr.
λ
max (nm)
λ
onset (nm )
Optical band gapEgap (ev)
B band
Q band
Dilute solution in DMF
ZnPAl
349
685
707
1.75
ZnPTr
381
700
760
1.63
Dilute solution in THF
ZnPAl
340
670
693
1.79
ZnPTr
352
683
705
1.76
λ
max: wavelength of maximum absorption;
λonset: wavelength of absorption onset; Egap: optical energy gap.


#### 3.1.2. Fluorescence Spectra

The fluorescence behavior of zinc phthalocyanine complexes was studied in solution in DMF and in thin solid films, excitation wavelength (λexc) = 488 nm. Samples show emission in green region at 533 and 553 nm for ZnPAl and ZnPTr, respectively (Figure 2).Figure 2
PL spectra of ZnPAl and ZnPTr (dilute solutions in DMF 210−6M,  λexc = 488 nm).Theπ-π* stacking of conjugated phthalocyanines also influenced the film emission, and broad, red shifted PL spectra were obtained as a result to excimer formation [21] in comparison with the solution spectra (Figure 2). An important redshift was observed (647 nm) and (655 nm), respectively, for ZnPAl and ZnPTr, and a red emission was obtained (Figure 3).Figure 3
PL spectra of ZnPAl and ZnPTr in thin films 40 nm (λexc = 488 nm).


### 3.2. Electrochemistry

#### 3.2.1. Cyclic Voltammetry

Electrochemistry provides valuable insight into the electronic properties of molecules. This technique provides information on the position of the energy levels; in particular the highest occupied molecular orbital (HOMO) and the lowest unoccupied molecular orbital (LUMO) are easily discernible from these measurements.The glass ITO was used as working electrode and scanned in LiClO4/dimethylformamide. The voltammograms obtained are shown in Figure 4.Cyclic voltammograms of ZnPAl and ZnPTr in 0.1 M LiclO4/DMF (scan rate: 100 mVs−1 working electrode = ITO, auxiliary electrode = platinum wire, and reference electrode = ECS).
(a)
(b)ZnPAl exhibits two creversible oxidations peaks at 1.05 and 1.32 V. ZnPTr exhibits two quasi-reversible oxidations at 0.9 and 1.35 V and a reversible reduction peak at −0.79 V (Figure4).The position of the HOMO of a molecule is probed by determining its anodic potential, while the position of the LUMO is determined by its cathodic potential. These positions can be referenced with respect to the vacuum level by adding 4.8 eV to the onset of the peak (oxidation/reduction) with respect to the ferrocene/ferrocenium (Fc/Fc+) redox couple [22]. All processes are ring based since the central Zn metal is electroinactive [23, 24].The HOMO energy level (EHOMO), LUMO energy level (ELUMO), and the electrochemical gap (Egapel) were calculated as follows:
(1)EHOMO=-(Vonsetox-VFOC+4.8)eV,ELUMO=-(Vonsetred-VFOC+4.8)eV,Egapel=(ELUMO-EHOMO)eV,
where VFOC is the ferrocene half-wave potential (0.9 V), Vonsetox is the material oxidation onset, and Vonsetred is the material reduction onset, all measured versus SCE. The calculated EHOMO, ELUMO, and Egapel values are summarized in Table 2.Table 2
SpecificEHOMO (V), ELUMO (V), and electrochemical band gap (ev) of ZnPAl and ZnPTr.
Phthalocyanines
E
HOMO
E
LUMO
E
gap
ZnPAl
−4.49
−2.55
1.94
ZnPTr
−4.49
−3.32
1.17


### 3.3. Current-Voltage Measurements

Two single-layer devices with an ITO/ZnPc/aluminum configuration were fabricated to investigate the current-voltage characteristics of the phtalocyanine-based materials. As shown in Figure5, the current-voltage curves indicate typical diode behavior with relatively low turn-on voltages of 3 and 3.3 V for ZnPTr and ZnPAl, respectively. Nevertheless, no electroluminescence could be recorded for these simple devices. The reason was probably unbalanced charge injection, which increased the probability of radiation less exciton quenching at the electrode phthalocyanine interface [25, 26].Current-voltage curves for ITO/Zn-phthalocyanine/aluminum diodes.
(a)
(b)Therefore, we believe that the device turn-on voltage indicates the threshold of a hole governed unipolar injection. Work is in progress to build electroluminescent multilayer devices.


## 3.1. Optical Properties

### 3.1.1. Electronic Absorption Spectra

The ground state electronic spectra are especially useful to identify the structure of the phthalocyanines. Generally, UV-Vis spectra of phthalocyanines show typical electronic spectra with two strong absorption bands known as Q and B bands. The Q band in the visible region at ca. 600–750 nm is attributed to theπ-π* transition from the highest occupied molecular orbital (HOMO) to the lowest unoccupied molecular orbital (LUMO) of the Pc ring and the B band in the UV region at 300–400 nm [15, 16]. The ground state electronic absorption spectra of the peripherally tetra-substituted phthalocyanine complexes showed monomeric behavior evidenced by a single (narrow) Q band, typical of nonaggregated metallophthalocyanine complexes in THF and DMF.The electronic spectra of Zn-phthalocyanine compounds (ZnPAl, ZnPTr) in DMF and THF are given in Figure1.Figure 1
UV-Visible absorption spectra of ZnPAl (red line) and ZnPTr (green line) in DMF solution, ZnPAl (black line) and ZnPTr (blue line) in THF solution (410−5M).The UV-Vis absorption spectra of ZnPAl and ZnPTr in DMF showed intense Q absorption at 685 and 700 nm, respectively. The Q band absorptions were also observed at 670 nm and 683 nm, respectively, for ZnPAL and ZnPTr in THF. In addition, the intense B band absorptions in DMF were observed at 349 nm for ZnPAl and 381 nm for ZnPTr but 340 nm for ZnPAl and 352 nm for ZnPTr in THF (Figure1).The electronic absorption transitions of these compounds are strongly dependent on the type of the substituent (withdrawing or donating groups) as well as the type of the metal ion and its position (in the centre or on peripheral position) [17].Peripheral substitution of phthalocyanine by triazole chains gave bathochromic shifts of the Q band [18–20] in both studied solvents, which can be explained by the concomitant effect of the presence of triazole ring which possesses three nitrogen atoms and, thus, can serve as a ligand to coordinate metals or as a hydrogen bond acceptor and donor.The optical band gaps were estimated from the absorption onset of the phtalocyanines solutions. Table1 summarizes these spectral data.Table 1
Optical data for ZnPAl and ZnPTr.
λ
max (nm)
λ
onset (nm )
Optical band gapEgap (ev)
B band
Q band
Dilute solution in DMF
ZnPAl
349
685
707
1.75
ZnPTr
381
700
760
1.63
Dilute solution in THF
ZnPAl
340
670
693
1.79
ZnPTr
352
683
705
1.76
λ
max: wavelength of maximum absorption;
λonset: wavelength of absorption onset; Egap: optical energy gap.


### 3.1.2. Fluorescence Spectra

The fluorescence behavior of zinc phthalocyanine complexes was studied in solution in DMF and in thin solid films, excitation wavelength (λexc) = 488 nm. Samples show emission in green region at 533 and 553 nm for ZnPAl and ZnPTr, respectively (Figure 2).Figure 2
PL spectra of ZnPAl and ZnPTr (dilute solutions in DMF 210−6M,  λexc = 488 nm).Theπ-π* stacking of conjugated phthalocyanines also influenced the film emission, and broad, red shifted PL spectra were obtained as a result to excimer formation [21] in comparison with the solution spectra (Figure 2). An important redshift was observed (647 nm) and (655 nm), respectively, for ZnPAl and ZnPTr, and a red emission was obtained (Figure 3).Figure 3
PL spectra of ZnPAl and ZnPTr in thin films 40 nm (λexc = 488 nm).


## 3.1.1. Electronic Absorption Spectra

The ground state electronic spectra are especially useful to identify the structure of the phthalocyanines. Generally, UV-Vis spectra of phthalocyanines show typical electronic spectra with two strong absorption bands known as Q and B bands. The Q band in the visible region at ca. 600–750 nm is attributed to theπ-π* transition from the highest occupied molecular orbital (HOMO) to the lowest unoccupied molecular orbital (LUMO) of the Pc ring and the B band in the UV region at 300–400 nm [15, 16]. The ground state electronic absorption spectra of the peripherally tetra-substituted phthalocyanine complexes showed monomeric behavior evidenced by a single (narrow) Q band, typical of nonaggregated metallophthalocyanine complexes in THF and DMF.The electronic spectra of Zn-phthalocyanine compounds (ZnPAl, ZnPTr) in DMF and THF are given in Figure1.Figure 1
UV-Visible absorption spectra of ZnPAl (red line) and ZnPTr (green line) in DMF solution, ZnPAl (black line) and ZnPTr (blue line) in THF solution (410−5M).The UV-Vis absorption spectra of ZnPAl and ZnPTr in DMF showed intense Q absorption at 685 and 700 nm, respectively. The Q band absorptions were also observed at 670 nm and 683 nm, respectively, for ZnPAL and ZnPTr in THF. In addition, the intense B band absorptions in DMF were observed at 349 nm for ZnPAl and 381 nm for ZnPTr but 340 nm for ZnPAl and 352 nm for ZnPTr in THF (Figure1).The electronic absorption transitions of these compounds are strongly dependent on the type of the substituent (withdrawing or donating groups) as well as the type of the metal ion and its position (in the centre or on peripheral position) [17].Peripheral substitution of phthalocyanine by triazole chains gave bathochromic shifts of the Q band [18–20] in both studied solvents, which can be explained by the concomitant effect of the presence of triazole ring which possesses three nitrogen atoms and, thus, can serve as a ligand to coordinate metals or as a hydrogen bond acceptor and donor.The optical band gaps were estimated from the absorption onset of the phtalocyanines solutions. Table1 summarizes these spectral data.Table 1
Optical data for ZnPAl and ZnPTr.
λ
max (nm)
λ
onset (nm )
Optical band gapEgap (ev)
B band
Q band
Dilute solution in DMF
ZnPAl
349
685
707
1.75
ZnPTr
381
700
760
1.63
Dilute solution in THF
ZnPAl
340
670
693
1.79
ZnPTr
352
683
705
1.76
λ
max: wavelength of maximum absorption;
λonset: wavelength of absorption onset; Egap: optical energy gap.


## 3.1.2. Fluorescence Spectra

The fluorescence behavior of zinc phthalocyanine complexes was studied in solution in DMF and in thin solid films, excitation wavelength (λexc) = 488 nm. Samples show emission in green region at 533 and 553 nm for ZnPAl and ZnPTr, respectively (Figure 2).Figure 2
PL spectra of ZnPAl and ZnPTr (dilute solutions in DMF 210−6M,  λexc = 488 nm).Theπ-π* stacking of conjugated phthalocyanines also influenced the film emission, and broad, red shifted PL spectra were obtained as a result to excimer formation [21] in comparison with the solution spectra (Figure 2). An important redshift was observed (647 nm) and (655 nm), respectively, for ZnPAl and ZnPTr, and a red emission was obtained (Figure 3).Figure 3
PL spectra of ZnPAl and ZnPTr in thin films 40 nm (λexc = 488 nm).


## 3.2. Electrochemistry

### 3.2.1. Cyclic Voltammetry

Electrochemistry provides valuable insight into the electronic properties of molecules. This technique provides information on the position of the energy levels; in particular the highest occupied molecular orbital (HOMO) and the lowest unoccupied molecular orbital (LUMO) are easily discernible from these measurements.The glass ITO was used as working electrode and scanned in LiClO4/dimethylformamide. The voltammograms obtained are shown in Figure 4.Cyclic voltammograms of ZnPAl and ZnPTr in 0.1 M LiclO4/DMF (scan rate: 100 mVs−1 working electrode = ITO, auxiliary electrode = platinum wire, and reference electrode = ECS).
(a)
(b)ZnPAl exhibits two creversible oxidations peaks at 1.05 and 1.32 V. ZnPTr exhibits two quasi-reversible oxidations at 0.9 and 1.35 V and a reversible reduction peak at −0.79 V (Figure4).The position of the HOMO of a molecule is probed by determining its anodic potential, while the position of the LUMO is determined by its cathodic potential. These positions can be referenced with respect to the vacuum level by adding 4.8 eV to the onset of the peak (oxidation/reduction) with respect to the ferrocene/ferrocenium (Fc/Fc+) redox couple [22]. All processes are ring based since the central Zn metal is electroinactive [23, 24].The HOMO energy level (EHOMO), LUMO energy level (ELUMO), and the electrochemical gap (Egapel) were calculated as follows:
(1)EHOMO=-(Vonsetox-VFOC+4.8)eV,ELUMO=-(Vonsetred-VFOC+4.8)eV,Egapel=(ELUMO-EHOMO)eV,
where VFOC is the ferrocene half-wave potential (0.9 V), Vonsetox is the material oxidation onset, and Vonsetred is the material reduction onset, all measured versus SCE. The calculated EHOMO, ELUMO, and Egapel values are summarized in Table 2.Table 2
SpecificEHOMO (V), ELUMO (V), and electrochemical band gap (ev) of ZnPAl and ZnPTr.
Phthalocyanines
E
HOMO
E
LUMO
E
gap
ZnPAl
−4.49
−2.55
1.94
ZnPTr
−4.49
−3.32
1.17


## 3.2.1. Cyclic Voltammetry

Electrochemistry provides valuable insight into the electronic properties of molecules. This technique provides information on the position of the energy levels; in particular the highest occupied molecular orbital (HOMO) and the lowest unoccupied molecular orbital (LUMO) are easily discernible from these measurements.The glass ITO was used as working electrode and scanned in LiClO4/dimethylformamide. The voltammograms obtained are shown in Figure 4.Cyclic voltammograms of ZnPAl and ZnPTr in 0.1 M LiclO4/DMF (scan rate: 100 mVs−1 working electrode = ITO, auxiliary electrode = platinum wire, and reference electrode = ECS).
(a)
(b)ZnPAl exhibits two creversible oxidations peaks at 1.05 and 1.32 V. ZnPTr exhibits two quasi-reversible oxidations at 0.9 and 1.35 V and a reversible reduction peak at −0.79 V (Figure4).The position of the HOMO of a molecule is probed by determining its anodic potential, while the position of the LUMO is determined by its cathodic potential. These positions can be referenced with respect to the vacuum level by adding 4.8 eV to the onset of the peak (oxidation/reduction) with respect to the ferrocene/ferrocenium (Fc/Fc+) redox couple [22]. All processes are ring based since the central Zn metal is electroinactive [23, 24].The HOMO energy level (EHOMO), LUMO energy level (ELUMO), and the electrochemical gap (Egapel) were calculated as follows:
(1)EHOMO=-(Vonsetox-VFOC+4.8)eV,ELUMO=-(Vonsetred-VFOC+4.8)eV,Egapel=(ELUMO-EHOMO)eV,
where VFOC is the ferrocene half-wave potential (0.9 V), Vonsetox is the material oxidation onset, and Vonsetred is the material reduction onset, all measured versus SCE. The calculated EHOMO, ELUMO, and Egapel values are summarized in Table 2.Table 2
SpecificEHOMO (V), ELUMO (V), and electrochemical band gap (ev) of ZnPAl and ZnPTr.
Phthalocyanines
E
HOMO
E
LUMO
E
gap
ZnPAl
−4.49
−2.55
1.94
ZnPTr
−4.49
−3.32
1.17


## 3.3. Current-Voltage Measurements

Two single-layer devices with an ITO/ZnPc/aluminum configuration were fabricated to investigate the current-voltage characteristics of the phtalocyanine-based materials. As shown in Figure5, the current-voltage curves indicate typical diode behavior with relatively low turn-on voltages of 3 and 3.3 V for ZnPTr and ZnPAl, respectively. Nevertheless, no electroluminescence could be recorded for these simple devices. The reason was probably unbalanced charge injection, which increased the probability of radiation less exciton quenching at the electrode phthalocyanine interface [25, 26].Current-voltage curves for ITO/Zn-phthalocyanine/aluminum diodes.
(a)
(b)Therefore, we believe that the device turn-on voltage indicates the threshold of a hole governed unipolar injection. Work is in progress to build electroluminescent multilayer devices.


## 4. Conclusion

In summary, two semiconductors Zn-phthalocyanines were successfully synthesized and optically and electrochemically characterized. It was shown that the extension of phthalocyanine by triazole ring can increase the absorption bands to 700 nm. In dilute solutions, these complexes presented green emissions. In thin solid films, the interchainπ-π* interactions influenced the optical behavior, and redshifted PL spectra were obtained. The current-voltage characteristics of the devices with an ITO/phthalocyanine/aluminum configuration demonstrated typical diode behavior and relatively low turn-on voltages. All these features make these complexes promising active materials for phthalocyanine-based OLEDs.



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*Source: 321563-2013-05-02.xml*