# Chemical Polymerization Kinetics of Poly-O-Phenylenediamine and Characterization of the Obtained Polymer in Aqueous Hydrochloric Acid Solution Using K2Cr2O7 as Oxidizing Agent

Authors: S. M. Sayyah; A. B. Khaliel; Ahmed A. Aboud; S. M. Mohamed
Journal: International Journal of Polymer Science
 (2014)

---

## Abstract

The oxidative chemical polymerization of o-phenylenediamine (OPDA) was studied in hydrochloric acid solution using potassium dichromate as oxidant at 5°C. The effects of potassium dichromate, hydrochloric acid, and monomer concentrations on the polymerization reaction were investigated. The order of reaction with respect to potassium dichromate, hydrochloric acid, and monomer concentration was found to be 1.011, 0.954, and 1.045, respectively. Also, the effect of temperature on the polymerization rate was studied and the apparent activation energy of the polymerization reaction was found to be 63.658 kJ/mol. The obtained polymer was characterized using XPS, IR, UV-visible, and elemental analysis. The surface morphology of the obtained polymers was characterized by X-ray diffraction and transmission electron microscopy (TEM). The TGA analysis was used to confirm the proposed structure and number of water molecules in each polymeric chain unit. The ac conductivity(
σ
ac
) of (POPDA) was investigated as a function of frequency and temperature. The ac conductivity was interpreted as a power law of frequency. The frequency exponent (s) was found to be less than unity and decreased with the increase of temperature, which confirms that the correlated barrier hopping model was the dominant charge transport mechanism.


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## Body

## 1. Introduction

Polyaniline as an electrically conductive polymer has attracted considerable attention, because of its excellent environmental stability in the electroconducting form and electrical and optical properties [1, 2]. It has various potential applications in many high performance devices [3–9]. A common feature of conducting polymer is conjugation of π-electrons extending over the length of the polymer backbone [10]. Polymerization of conducting polymer may be performed by chemical [11] or electrochemical [12] methods. Various chemical oxidizing agents, such as potassium dichromate [13], potassium iodate [14], hydrogen peroxide [15], ferric chloride, or ammonium persulphate, were used [16]. The applications of polyaniline are limited due to its poor processability [17], which is true for most conducting polymers. Several studies have been done in order to improve the solubility of polyaniline; among them is using functionalized protonic acids as dopant, like p-toluene-sulphonic acid, octyl-benzene-sulphonic acid, dodecyl benzene-sulphonic acid [18], poly(styrene) sulphonic acid [19], and phosphoric acid esters [20]. An alternative method to obtain soluble conductive polymers is the polymerization of aniline derivatives. The studied aniline derivatives are alkyloxy, hydroxy, and chloroaniline and substitution at the nitrogen atom was reported by Sayyah et al. [21–24] to improve the solubility of polyaniline. The substituted group of aniline affects not only the polymerization reaction but also the properties of the polymer obtained. The kinetics of chemical polymerization of 3-methylaniline, 3-chloroaniline, 3-hydroxyaniline, 3-methoxyaniline, and N-methyl aniline in hydrochloric acid solution using sodium dichromate as oxidant and characterization of the polymer obtained by IR, UV-visible and elemental analysis, X-ray diffraction, scanning electron microscopy, TGA-DTA analysis, and ac conductivity have been investigated by Sayyah et al. [25–28].The present work intends to study the kinetics of the oxidative chemical polymerization of o-phenylenediamine in aqueous HCl medium and potassium dichromate as oxidant. The obtained polymer is characterized by XPS, IR, UV-visible, TGA, elemental analysis, X-ray, transmission electron microscopy (TEM), and ac conductivity measurements.


## 2. Experimental

### 2.1. Materials

O-phenylenediamine was provided by Aldrich chemical Co. (Germany). Concentrated hydrochloric acid, pure grade product, was provided by El-Nasr pharmaceutical chemical Co., Egypt. Potassium dichromate was provided by Sigma-Aldrich chemical Co. (Germany). Doubly distilled water was used to prepare all the solutions needed in the kinetic studies.


### 2.2. Oxidative Aqueous Polymerization of O-Phenylenediamine Monomer

The polymerization reaction was carried out in a well-stoppered conical flask of 250 mL capacity; addition of OPDA amount in 25 mL HCl of known molarity was followed by the addition of the required amount of potassium dichromate as oxidant in water (25 mL) to the reaction mixture. The orders of addition of substances were kept constant in all the performed experiments. The stoppered conical flasks were then placed in an automatically controlled thermostat at the required temperature. The flasks were shaken (15 shakings/10 s/15 min) by using an automatic shaker. The flasks were filtrated using a Buchner funnel; then the obtained polymer was washed with distilled water and finally dried till constant weight in vacuum oven at 60°C.


### 2.3. Elemental Analysis, Infrared, and Ultraviolet Spectroscopy

The carbon, hydrogen, and nitrogen contents of the prepared polymer were carried out in the microanalytical laboratory at Cairo University by using oxygen flask combustion and a dosimat E415 titrator (Switzerland).The infrared spectroscopic analysis of the prepared polymer was carried out in the microanalytical laboratory at Cairo University by using a Shimadzu FTIR-430 Jasco spectrophotometer and KBr disc technique.The ultraviolet-visible absorption spectra of the monomer and the prepared polymer sample were measured using Shimadzu UV spectrophotometer (M 160 PC) at room temperature in the range 200–400 nm using dimethylformamide as a solvent and reference.


### 2.4. X-Ray Photoelectron Spectroscopy (XPS)

An XPS spectrum was obtained on XPS-thermo scientific spectrometer, Model: K-ALDH in Central metallurgical research and development institute (CMRDI). Polymer was mounted on a standard sample holder using double-sided adhesive tape. Survey and XPS spectra were obtained with Al Kα monochromatic X-ray with the resolution of 0.7 eV.


### 2.5. Thermal Gravimetric Analysis (TGA), Transmission Electron Microscopy (TEM), and X-Ray Analysis

Thermal gravimetric analysis (TGA) of the polymer sample was performed using a SHIMADZU DT-30 thermal analyzer. The weight loss was measured from ambient temperature up to 600°C at rate of 20°C/min to determine the rate of degradation of the polymer.The X-ray diffractometer type Philips 1976 Model 1390 was used to investigate the phase structure of the polymer powder under the following condition which kept constant during the analysis processes: Cu: X-ray tube, scan speed = 8/min, current = 30 mA, voltage = 40 kv, and preset time = 10 s.The inner cavity and wall thickness of the prepared polymer were investigated using transmission electron microscopy (TEM) JEOL JEM-1200 EX П (Japan).


### 2.6. Conductivity Measurements

The ac conductivity was measured using Philips RCL bridge (digital and computerized) at a frequency range 0.1–100 kHz and over temperature range 30–80°C. The temperature was controlled by the use of a double wound electric oven.The ac conductivityσ
ac value was calculated using the relation
(1)
σ
ac
=
ε
′′
ω
ε
o
,
where ω
=
2
π
f and f is the applied frequency.


## 2.1. Materials

O-phenylenediamine was provided by Aldrich chemical Co. (Germany). Concentrated hydrochloric acid, pure grade product, was provided by El-Nasr pharmaceutical chemical Co., Egypt. Potassium dichromate was provided by Sigma-Aldrich chemical Co. (Germany). Doubly distilled water was used to prepare all the solutions needed in the kinetic studies.


## 2.2. Oxidative Aqueous Polymerization of O-Phenylenediamine Monomer

The polymerization reaction was carried out in a well-stoppered conical flask of 250 mL capacity; addition of OPDA amount in 25 mL HCl of known molarity was followed by the addition of the required amount of potassium dichromate as oxidant in water (25 mL) to the reaction mixture. The orders of addition of substances were kept constant in all the performed experiments. The stoppered conical flasks were then placed in an automatically controlled thermostat at the required temperature. The flasks were shaken (15 shakings/10 s/15 min) by using an automatic shaker. The flasks were filtrated using a Buchner funnel; then the obtained polymer was washed with distilled water and finally dried till constant weight in vacuum oven at 60°C.


## 2.3. Elemental Analysis, Infrared, and Ultraviolet Spectroscopy

The carbon, hydrogen, and nitrogen contents of the prepared polymer were carried out in the microanalytical laboratory at Cairo University by using oxygen flask combustion and a dosimat E415 titrator (Switzerland).The infrared spectroscopic analysis of the prepared polymer was carried out in the microanalytical laboratory at Cairo University by using a Shimadzu FTIR-430 Jasco spectrophotometer and KBr disc technique.The ultraviolet-visible absorption spectra of the monomer and the prepared polymer sample were measured using Shimadzu UV spectrophotometer (M 160 PC) at room temperature in the range 200–400 nm using dimethylformamide as a solvent and reference.


## 2.4. X-Ray Photoelectron Spectroscopy (XPS)

An XPS spectrum was obtained on XPS-thermo scientific spectrometer, Model: K-ALDH in Central metallurgical research and development institute (CMRDI). Polymer was mounted on a standard sample holder using double-sided adhesive tape. Survey and XPS spectra were obtained with Al Kα monochromatic X-ray with the resolution of 0.7 eV.


## 2.5. Thermal Gravimetric Analysis (TGA), Transmission Electron Microscopy (TEM), and X-Ray Analysis

Thermal gravimetric analysis (TGA) of the polymer sample was performed using a SHIMADZU DT-30 thermal analyzer. The weight loss was measured from ambient temperature up to 600°C at rate of 20°C/min to determine the rate of degradation of the polymer.The X-ray diffractometer type Philips 1976 Model 1390 was used to investigate the phase structure of the polymer powder under the following condition which kept constant during the analysis processes: Cu: X-ray tube, scan speed = 8/min, current = 30 mA, voltage = 40 kv, and preset time = 10 s.The inner cavity and wall thickness of the prepared polymer were investigated using transmission electron microscopy (TEM) JEOL JEM-1200 EX П (Japan).


## 2.6. Conductivity Measurements

The ac conductivity was measured using Philips RCL bridge (digital and computerized) at a frequency range 0.1–100 kHz and over temperature range 30–80°C. The temperature was controlled by the use of a double wound electric oven.The ac conductivityσ
ac value was calculated using the relation
(1)
σ
ac
=
ε
′′
ω
ε
o
,
where ω
=
2
π
f and f is the applied frequency.


## 3. Results and Discussion

### 3.1. Determination of the Optimum Polymerization Conditions

To optimize the condition for polymerization of o-phenylenediamine, the concentrations of potassium dichromate, hydrochloric acid, and monomer were investigated with keeping the total volume of the reaction mixture constant at 50 mL.


#### 3.1.1. Effect of Potassium Dichromate Concentration

Both of the monomer and HCl concentrations are fixed at 0.1 M while the oxidant concentrations were varied from 0.04 to 0.5 M at5
±
0.2°C to investigate the optimum polymerization condition of K2Cr2O7. The yield-time curve was represented in Figure 1, from which it is clear that the obtained yield increased with the increase of K2Cr2O7 reaching maximum value at 0.3 M. From the left part of the curve it is clear that the polymer yield increases from 0.04 M to 0.3 M then decreases from 0.3 M to 0.5 M. This could be due to the fact that, in the first part of the curve, the produced initiator ion radical moieties activate the backbone and simultaneously produced the o-phenylenediamine ion radical, which takes place immediately, and, therefore, yield increases with the increase of potassium dichromate concentration up to 0.3 M. But in the second part of the curve, the polymer yield decreases with increasing K2Cr2O7 concentration, may be due to a high concentration of oxidant promote the formation of low molecular weight oxidation product and also degrade the product polymer which easily soluble in water [13].Figure 1
Yield-K2Cr2O7 concentration effect on the aqueous oxidative polymerization of poly-o-phenylenediamine (POPDA).


#### 3.1.2. Effect of HCl Concentration

The effect of HCl concentration on the aqueous oxidative polymerization of OPDA was investigated using constant concentration of K2Cr2O7 at 0.3 M and monomer concentration at 0.1 M and using different concentration of HCl at 5
±
0.2°C. The yield-time data was represented in Figure 2, from which it is clear that the obtained yield increases in the acid concentration range from 0.04 to 0.2 then decreases gradually up to 0.5 M. This behavior may be due to, at higher concentration of HCl, the degradation of the polymer in the early stages of the reaction, which may be due to the hydrolysis of polyemeraldine chain [13].Figure 2
Yield-HCl concentration effect on the aqueous oxidative polymerization of poly-o-phenylenediamine (POPDA).


#### 3.1.3. Effect of O-Phenylenediamine Concentration

The effect of monomer concentration on the polymerization efficiency was investigated in the range of monomer concentration from 0.02 to 0.5 M and the data was represented in Figure3, from which it is clear that the optimum yield formation is obtained at 0.1 M of the monomer concentration.Figure 3
Yield-monomer concentration effect on the aqueous oxidative polymerization of poly-o-phenylenediamine (POPDA).


### 3.2. The Kinetic Study of the Polymerization Reaction

#### 3.2.1. Effect of Potassium Dichromate Concentration

The aqueous polymerization of OPDA (0.1 mol) was carried out in 25 mL of HCl solution (0.2 mol) in the presence of 25 mL potassium dichromate as oxidant of different molarities at 5°C for different time intervals. The yield-time curves were plotted for different oxidant concentrations and the data are graphically represented in Figure4(a). The initial and overall reaction rates were determined using the following equation:
(2)
Rate
(
R
i
)
=
P
V
×
M
×
t
,
where P is the weight of the obtained polymer, t is the time in seconds, M is the molecular weight of the monomer, and V is the reaction volume in liter.(a) Yield-time curve for the effect of potassium dichromate concentration on the polymerization (POPDA) at different time intervals. (b) Double logarithmic plot of the initial rate and oxidant concentration of POPDA.
(a)
(b)The initial and overall reaction rates of the polymerization reaction increase with the increase of oxidant concentration in the range between 0.05 and 0.3 mol/L. The oxidant exponent was determined from the relation between logarithm of the initial rate of polymerization Log (R
i) and logarithm of the oxidant concentration. A straight line was obtained which has a slope of 1.011 as represented in Figure 4(b). This means that the polymerization reaction of OPDA is a first-order reaction with respect to the oxidant.


#### 3.2.2. Effect of Hydrochloric Acid Concentration

The polymerization of OPDA (0.1 mol) in 25 mL of HCl with different molarities was carried out by addition of 25 mL potassium dichromate (0.3 mol/L) as oxidant at 5°C for different time intervals. The concentration of the monomer and oxidant were kept constant during the study of HCl effect on the polymerization reaction. The experiments were carried out as described in Section2.2, and the yield-time curve was plotted for each acid concentration used. The data are graphically represented in Figure 5(a), from which it is clear that both the initial and overall reaction rates of the polymerization reaction increase with the increasing of HCl concentrations in the range between 0.05 and 0.2 mol/L. The HCl exponent determined from the slope of the straight line represented in Figure 5(b) was found to be 0.954, which means that the polymerization order with respect to the HCl concentration is a first-order reaction.(a) Yield-time curve for the effect of HCl concentration on the aqueous oxidative polymerization of (POPDA) at different time intervals. (b) Double logarithmic plot of the initial rate and HCl concentration of POPDA.
(a)
(b)


#### 3.2.3. Effect of Monomer (OPDA) Concentration

The aqueous polymerization of OPDA was carried out in 25 mL of HCl solution (0.2 mol/L) in the presence of 25 mL potassium dichromate (0.3 mol/L) as oxidant at 5°C for different time intervals. The yield-time curve was plotted for each monomer concentration used. The data are graphically represented in Figure6(a). The monomer exponent was determined from the slope of the straight line represented in Figure 6(b) for the relation between log R
i and logarithm of the monomer concentration. The slope of this linear relationship was found to be 1.045. This means that the polymerization reaction with respect to the monomer concentration is a first-order reaction.(a) Conversion-monomer/mol concentration effect on the aqueous oxidative polymerization of (POPDA) at different time intervals. (b) Double logarithmic plot of the initial rate and monomer concentration of POPDA.
(a)
(b)


### 3.3. Calculation of the Thermodynamic Activation Parameters

The polymerization of OPDA (0.1 mol/L) in 25 mL of 0.2 mol/L HCl in presence of 25 mL potassium dichromate (0.3 mol/L) as oxidant solution was carried out at 5, 10, and 15°C for different time periods. The yield-time curves were graphically represented in Figure7, from which it is clear that both of the initial and overall reaction rates increase with raising the reaction temperature. The apparent activation energy (E
a) of the aqueous polymerization reaction of o-phenylenediamine was calculated using the following Arrhenius equation:
(3)
Log
(
K
)
=
-
E
a
2.303
R
T
+
C
,
where K is the rate, R is the universal gas constant, T is the reaction temperature, and C is constant.Figure 7
Yield-time curve for the effect of temperature on the aqueous oxidative polymerization of POPDA.By plotting logR
i against 1
/
T, which gave a straight line as shown in Figure 8, and from the slope we can calculate the activation energy. The apparent activation energy for this system is 63.658 kJ/mol. The Enthalpy and entropy of activation for the polymerization reaction can be calculated by the calculation of K
2 from the following equation:
(4)
Reaction
Rate
=
K
2
[
oxidant
]
1.011
[
HCl
]
0.954
[
monomer
]
1.045
.Figure 8
The relation between the logarithm of initial rate and (1
/
T) for aqueous oxidative polymerization of POPDA.The values ofK
2 at 5, 10, and 15°C were 6.131 × 10−6, 1.054 × 10−5, and 1.594 × 10−5, respectively. The enthalpy (Δ
H
*) and entropy (Δ
S
*) of activation associated with K
2 were calculated using Eyring equation
(5)
K
2
=
(
R
T
N
h
)
e
Δ
S
*
/
R
·
e
-
Δ
H
*
/
R
T
,
where K
2 is the rate constant, N is the Avogadro’s number, R is the universal gas constant, and h is planks constant.By dividing the above equation byT and taking its natural logarithm we obtain the following equation:
(6)
Ln
(
K
2
T
)
=
ln
⁡
⁡
(
R
N
h
)
+
Δ
S
*
R
+
-
Δ
H
*
R
T
.Figure9 shows the relation between K
2/T versus 1/T, which gives a linear relationship with (-
Δ
H
*)/R and intercept line (ln R/N
h + Δ
S
*/R) from the slops and intercept; the values of Δ
H
* and Δ
S
* were found to be 61.48 kJmol−1 and 29.95 Jmol-1K−1, respectively.Figure 9
The relation between logK
2/T and 1/T for poly-o-phenylenediamine (POPDA).The intramolecular electron transfer steps for the oxidation reaction are endothermic as indicated by the value ofΔ
H
*. The contributions of Δ
H
* and Δ
S
* to the rate constant seem to compensate each other. This fact suggests that the factors controlling Δ
H
* must be closely related to those controlling Δ
S
*. Therefore, the salvation state of the encounter compound could be important in determination of Δ
H
*. Consequently, the relatively small enthalpy of activation can be explained in terms of the formation of more solvated complex.


### 3.4. Polymerization Mechanism

The aqueous oxidative polymerization of o-phenylenediamine is described in the Experimental section and follows three steps [29].The Initial Step. Potassium dichromate in acidified aqueous solution produces chromic acid as shown in
(7)
K
2
Cr
2
O
7
+
H
2
O
+
2
H
+
=
2
K
+
+
2
H
2
CO
4
.This reaction is controlled by the change in pH; the orange red dichromate ions (Cr2O7)2- are in equilibrium with the (HCrO4)- in the range of pH-values between 2 and 6, but at pH below 1 the main species is (H2CrO4) and the equilibria can occur as follows:
(8)
(
HCrO
4
)
-
⇌
(
CrO
4
)
2
-
+
H
+
K
=
10
-
5.9
(9)
(
H
2
CrO
4
)
⇌
(
HCrO
4
)
-
+
H
+
K
=
4.1
(10)
2
(
HCrO
4
)
-
⇌
(
Cr
2
O
7
)
2
-
+
H
2
O
K
=
10
-
2
.
2
.
The chromic acid withdraws one electron from each protonated OPDA and probably forms a metastable complex as shown in (11):(11)The complex undergoes dissociation to form monomer cation radical as shown in (12):(12)Generally, the initial step is rapid and may occur in short time, 0–5 min (autocatalytic reaction); no polymeric product is being obtained. After 5 min of the polymerization reaction, the polymeric products are obtained.Propagation Step. This step involves the interaction between the formed radical cation and the monomer to form a dimer radical cation. In the case of Cr(VI) oxidation of the organic compounds, Cr(VI) is reduced to Cr(IV) first and then to Cr(III) [29]. Transfer of two electrons from two monomer ions radical by H2CrO4 produces para semidine salt along with chromous acid H2Cr2O3 (Cr(IV)). The intermediately produced Cr(IV) oxidises para semidine to pernigraniline salt (PS) at suitable low pH and the PS acts as a catalyst for conversion of OPDA to POPDA:(13)(14)This reaction is followed by further reaction of the formed dimmer radical cations with monomer molecules to form trimer radical cations and so on. The degree of polymerization depends on different factors such as dichromate concentration, HCl concentration, monomer concentration, and temperature. By adding (7), (11), (12), (13), and (14),(15)
(16)
12
OPDA
+
5
K
2
Cr
2
O
7
+
34
H
+
=
6
PS
+
10
Cr
3
+
+
10
K
+
+
35
H
2
O
.Termination Step. Termination of the reaction occurs by the addition of ammonium hydroxide solution in an equimolar amount to HCl present in the reaction medium (till pH = 7), which leads to cessation of the redox reaction. The reaction could occur as follows:(17)


### 3.5. Characterization of the Obtained Polymer

#### 3.5.1. The Solubility

The solubility of POPDA was investigated in N-methyl pyrrolidone, dimethylformamide (DMF), acetone, methanol, iso propanol, benzene, hexane, and chloroform. The solubility values are listed in Table1. The complete solubility was found in N-methyl pyrrolidone, then in DMF 2.235 g/L followed by acetone 1.67 g/L, then in methanol 1.074 g/L then followed by iso propanol 0.879 g/L at 20°C but not soluble in benzene, hexane, and chloroform.Table 1
Solubility of poly-o-phenylenediamine (POPDA) in different solvents at 20°C.
Solvent
Solubility of (POPDA) in (g/L)
N-methyl-2-pyrrolidone
Completely soluble
Dimethylformamide
2.235
Acetone
1.679
Methanol
1.074
Iso propanol
0.879


#### 3.5.2. The Elemental Analysis

The data obtained from elemental analysis using oxygen flask combustion and a dosimat E415 titrator shows that the found carbon content of (POPDA) is lower than the calculated value. This is due to the formation of chromium carbide during step of heating and measuring process while the found values of nitrogen and hydrogen are 20.91 and 4.37, respectively, which are in good agreement with the calculated one for the suggested structure present in Scheme1. By measuring another sample of the (POPDA) which was prepared by using ammonium persulfate as oxidant, the found value of carbon is higher than sample which is prepared by using potassium dichromate as oxidant. For more information about the chemical composition of (POPDA), the XPS study was conducted as mentioned under point 3.5.2.Scheme 1
Structure of the prepared (POPDA).


#### 3.5.3. X-Ray Photoelectron Spectroscopy (XPS) Characterization

(
1) XPS Survey Elemental Composition. X-ray photoelectron spectroscopy (XPS) is used to study the composition of materials, which detect elements starting from Li (Z = 3) and higher elements. Hydrogen (Z = 1) and helium (Z = 2) cannot be detected due to the low probability of electron emission. XPS survey begins from 0 to 1400 (eV) as shown in Figure 10. The XPS survey scan spectrum of the prepared polymer shows the presence of C, N, O, Cl, and Cr. The Cl was present as doping anion in the prepared polymer. Chrome was found due to the polymer prepared using potassium dichromate as oxidant. It is possible for chromium ion (Cr+3) to present between polymer chains as a sandwich-bonded C6H6–C6H6 groups as shown in Scheme 1 and the usual formation procedure is hydrolyzing the reaction mixture with dilute acid which gives the cation (C6H6)2Cr3+ [30, 31].Figure 10
X-ray photoelectron spectroscopy (XPS) survey elemental composition of poly-o-phenylenediamine (POPDA).The XPS elemental analysis of the prepared polymer is given in Table2. The data shows that there is a good agreement with the calculated one for the suggested structures present in Scheme 1.Table 2
The XPS elemental analysis of poly-o-phenylenediamine (POPDA).
C%
N%
Cl%
O%
Cr%
Calc.
Found
Calc.
Found
Calc.
Found
Calc.
Found
Calc.
Found
57.21
56.11
22.25
21.89
7.05
6.94
3.18
3.02
10.31
10.11(
2) XPS Spectra of Poly(OPDA). Four main peaks were obtained for C1s spectra of poly(OPDA) as shown in Figure 11(a). The sharp peak appearing at 283.98 eV is attributed to C–H (C1) bond, while the peak appearing at 284.18 eV is attributed to C–C (C2) bond. The peak appearing at 285.08 eV is assigned to C–N (C3) bond while the peak appearing at 287.58 eV is attributed to C–O or C–N+ (C4) bond [32–34].X-ray photoelectron spectroscopy (XPS) spectra of (POPDA).
(a)
(b)
(c)
(d)
(e)N1s Figure11(b) shows the XPS N1s spectrum of poly(OPDA) which has three distinct curves. The first two peaks are assigned to imine (–N=) at 398.58 eV and amine (–NH–) at 399.23 eV. Moreover, the peak that appears at 400.58 eV is due to positively charged nitrogen atom (N+).Two distinct oxygen species contribute to the oxygen 1 s signals in the conducting polymers (Figure11(c)). The distinct energy peaks at 530.68 and 533.12 eV could be attributed to Cr2O3 and C–OH, respectively.The Cl 2p spectrum of poly(OPDA) is shown in Figure11(d). In order to estimate the anion Cl at the surface, Cl 2p peaks are fitted with a number of spin-orbit doublets (Cl 2p1/2 and Cl 2p3/2) with the B.E. for the C12p3/2 peaks at about 197.36, 198.34, and 200.1 eV. The lowest and the highest B.E. components are attributable to the ionic and covalent chlorine species (Cl- and –Cl), respectively. The chlorine species (Cl*) with the intermediate appear at B.E. of 198.34 eV. The lower B.E. value of the Cl* species compared to the Cl species suggests the presence of chloride anion in a more positive environment, probably arising from an increase in the number of positively charged nitrogen in the polymer chain associated with the formation of polarons and bipolarons.The Cr spectrum of (POPDA) is shown in Figure11(e). The main components corresponding to different chemical chromium species were observed in the high-resolution Cr2p3/2 spectrums. The first peak at 576.18 eV ± 0.2 eV was assigned to Cr2O3 which is in agreement with what was found by Chowdhury and Saha [13] and Stefanov et al. [35], also indicated by a distinct O1s peak at 530.68 eV typical for Cr2O3 which may be adsorbed on polymer surface during chromous acid H2Cr2O3 oxidation process. There is also a component visible that corresponds to Cr2p1/2 at 586.08 eV, which was attributed to Cr3+. This data reveal that chromium ion is present between benzene rings of polymeric chain as shown in Scheme 1.


#### 3.5.4. The Infrared Spectroscopic Analysis of (OPDA) Monomer and Its Analogs Polymer

The IR spectra of the OPDA and its polymer (POPDA) are represented in Figure12, while the absorption band values and their assignments are summarized in Table 3. The medium absorption band appearing at 453 cm−1, which could be attributed to bending deformation of N–H group attached to benzene ring in case of monomer, appears at 518 cm−1 with slight shift in case of polymer. The broad absorption band appearing at 778 cm−1 in case of monomer, which could be attributed to out of plane deformation of CH for 1,2-disubstituted benzene, appears at 748 cm−1 with slight shift in case of polymer. A series of absorption bands appear in the region from 924 to 1152 cm−1 which could be attributed to the out of plane C–H deformation of 1,2-disubistuition benzene ring in case of monomer and 1,2,4 tri-substituted of benzene ring, in case of polymer. The sharp absorption bands appear at 1336 cm−1 in case of the monomer, which could be attributed to symmetric stretching vibration of C–N, appears at 1362 cm−1 with slight shift in case of polymer. The sharp absorption band appearing at 1490 cm−1 in case of the monomer may be attributed to C=C aromatic stretching vibration, which appears at 1500 cm−1 with slight shift in case of polymer. The sharp absorption band appearing at 1630 cm−1 in case of the monomer, which may be attributed to C=C deformation of benzene ring, appears at 1621 cm−1 with slight shift in case of polymer. The shoulder absorption band appears at 3032 cm−1 in case of the monomer which could be attributed to symmetric stretching vibration of C–H in aromatic ring and disappears in case of polymer. The triplet absorption bands appearing at 3190, 3281, and 3370 cm−1 in case of monomer could be attributed to asymmetric stretching vibration for NH group, but in case of polymer a broad absorption band that appears at 3354 cm−1 could be attributed to asymmetric stretching vibration for NH group and OH group present in the polymer structure.Table 3
Infrared absorption bands and their assignments of o-phenylene-diamine monomer (OPDA) and its analogs polymer (POPDA).
Wave number (cm−1)
Assignments
(OPDA)Monomer
(POPDA)Polymer
453m
—
Bending deformation of NH in primary aromatic amines
—
518m
748b
—
Out-of-plane bending deformation of CH in 1,2 disubstituted in benzene ring
—
761b
810s
—
Out-of-plane deformation showing 1,4-disubistuition  in the benzene ring
—
833sh
924s
—
Plane C–H deformation of 1,2-disubistuition of benzene ring
—
1044w
1056m
—
1117s
—
—
1133w
1152
—
1336s
1362sh
Symmetric stretching vibration for C–O or C–N group
1490s
1500b
Symmetric stretching vibration for C–C aromatic
1590s
—
Stretching vibration of C–N or combination band for protonated primary aromatic amine
1630s
1621b
N–H deformation of secondary amine
3032sh
—
Symmetric stretching vibration of N–H
3281s
3354m
Asymmetric stretching vibration for NH
2930sh
3354b
Asymmetric stretching vibration for CH group in aliphatic chain
3370s
—
Symmetric stretching vibration of =C–H
s: sharp; m: medium; w: weak; b: broad; sh: shoulder.Figure 12
The infrared spectrum of o-phenylenediamine (OPDA) (a) and it analogous polymer (POPDA) (b).


#### 3.5.5. The UV-Visible Spectroscopic Study of OPDA Monomer and Its Analogs Polymer

The UV-visible spectra of OPDA and its polymer are represented in Figure13; the spectra show the following absorption bands:(1)
in case of monomer, two absorption bands appear atλ
max
⁡ = 219 and 240 nm which may be attributed to π-π* transition (E2-band) of the benzene ring and the β-band (A
1
g
-
B
2
u);
(2)
in case of polymer, two absorption bands appear atλ
max
⁡ = 221 and 243 nm which may be attributed to π-π* transition showing a bathochromic shift. Beside these two bands, broad absorption band appears in the visible region at λ
max
⁡ = 417 nm which may be due to the high conjugation of the aromatic polymeric chain.Figure 13
UV-visible spectra of o-phenylenediamine (OPDA) (A) and it analogous polymer (POPDA) (B).


#### 3.5.6. Thermal Gravimetric Analysis (TGA) of Poly O-Phenylenediamine

Thermogravimetric analysis (TGA) for the prepared polymer has been investigated and the TGA-curve is represented in Figure14. The calculated and found data for the prepared polymers are summarized in Table 4. The thermal degradation steps are summarized as follows:(1)
the first stage includes the loss of one water molecule in the temperature range between 29.5 and 122.6°C; the weight loss of this step was found to be 3.21% which is in a good agreement with the calculated one;
(2)
in the second stage, in the temperature range between 122.6 and 203.8°C, the weight loss was found to be 6.65%, which could be attributed to the loss of one HCl molecule. The calculated weight loss is in good agreement with the found one;
(3)
in the third stage, in the temperature range between 203.8 and 320.3°C, the weight loss was found to be 11.79%, which is attributed to the loss of four (NH2) groups. The calculated weight loss for this stage is equal to 12.11%;
(4)
in the fourth stage, in the temperature range between 320.3 and 400.0°C, the weight loss was found to be 16.95%, which could be attributed to the loss of one molecule of C6H3–NH. The calculated weight loss of this stage is equal to 17.22%;
(5)
in the fifth stage, in the temperature range between 400.0 and 523.4°C, the weight loss was found to be 13.78%, which is attributed to the loss of one molecule of phenyl ring. The calculated weight loss of this stage is equal to 14.19%;
(6)
in the last stage, above 523.38°C, the remaining polymer molecule was found to be 47.62% including the metallic residue, but the calculated one was found to be 46.46%.Table 4
Thermogravimetric data of poly-o-phenylenediamine (POPDA).
Name
Temperaturerange °C
Weight loss (%)
The removedmolecule
Calc.
Found
Poly(POPDA)
29.5–122.6
3.41
3.212
H2O
122.6–203.8
6.91
6.652
HCl
203.8–320.3
12.11
11.791
4NH2
320.3–400.00
17.22
16.952
C6H3–NH
400–523.40
14.19
13.778
C6H3
Remaining weight (%) above 600
46.17
47.62
—Figure 14
The thermal gravimetric analysis (TGA) for (POPDA).


#### 3.5.7. The X-Ray Diffraction Analysis and Transmission Electron Microscope

The X-Ray diffraction patterns of the prepared polymer are represented in Figure15. The figure shows that the prepared poly o-phenylenediamine is completely amorphous.Figure 15
X-ray poly-o-phenylenediamine (POPDA).Morphology of poly o-phenylenediamine was characterized by transmission electron microscope. Figure16 shows TEM image of poly o-phenylenediamine which nearly spherical or ellipsoidal particles with approximate diameter 60–120 nm either separated or linked with each other.Figure 16
The transmission electron microscope of POPDA.


### 3.6.  ac  Conductivity (σ
a
c)

Figure17 represent the variation in ac conductivity (σ
ac) for (POPDA) as a function of frequency and temperature. It is observed that the value of ac conductivity increases with the increase of frequency. This behavior is in good agreement with the random free energy model proposed by Dyre [36]. According to this model, conductance increases as a function of frequency in many solids, including polymers, which can be explained on the basis of any hopping model. The rise in conductivity upon increasing the frequency and temperature is common for disordered conducting polymer. As can be seen, each curve displays a conductivity dispersion, which is strongly dependent on frequency and shows weaker temperature dependant.Figure 17
ac conductivity versus angular frequency for poly-o-phenylenediamine (POPDA) with frequency at different temperatures.The recorded conductivity value at room temperature of POPDA was found 0.0352 S/cm which is higher than conductivity of polyaniline-polyvinyl alcohol blends 10.5 × 10−5 S cm−1 [37] and ac conductivity of HCl doped polyaniline synthesized by the interfacial polymerization technique 6.2 × 10−5 S cm−1 [38]. Also, the ac conductivity of POPDA is higher than polyaniline loaded with 10% molybdenum trioxide composites 0.025 s/cm [39] but lower than the determined value of ac conductivity polyaniline prepared by K2Cr2O7 as oxidant 1.922 S cm−1. Such difference could be attributed to the different disorder of each composite, substituted function group, and different used dopant.In general, for amorphous conducting material, disordered systems, low mobility polymers, and even crystalline materials, the ac conductivity (σ
ac) as a function of frequency can obey a power law with frequency [40]. The ac conductivity (σ
ac) over a wide range of frequencies can be expressed as
(18)
σ
ac
(
ω
)
=
A
ω
s
,
where A is a complex constant and the index (s) is frequency exponent and ω is the angular frequency (ω
=
2
π
f).Figure17 shows the relation between Ln σ
ac and Ln ω at different temperatures. The value of (s) at each temperature has been calculated from the slope of ln σ(ω) versus ln (ω) plot. As shown in Figure 18 the calculated values of (s) for (POPDA) sample are less than unity. The microscopic conduction mechanisms of disordered systems are governed by two physical processes such as classical hopping or quantum mechanical tunneling of charge carries over the potential barrier separating two energetically favorable centers in a random distribution. The exact nature of charge transport is mainly obtained experimentally from the temperature variation of exponent (s) [41]. The temperature exponent(s) dependences for (POPDA) sample reveal that the frequency exponent(s) decreases with the increase of temperature. This behavior is only observed in the correlated barrier hopping model proposed by Elliott [42].Figure 18
Frequency exponent (s) versus temperature for poly-o-phenylenediamine (POPDA).


## 3.1. Determination of the Optimum Polymerization Conditions

To optimize the condition for polymerization of o-phenylenediamine, the concentrations of potassium dichromate, hydrochloric acid, and monomer were investigated with keeping the total volume of the reaction mixture constant at 50 mL.


### 3.1.1. Effect of Potassium Dichromate Concentration

Both of the monomer and HCl concentrations are fixed at 0.1 M while the oxidant concentrations were varied from 0.04 to 0.5 M at5
±
0.2°C to investigate the optimum polymerization condition of K2Cr2O7. The yield-time curve was represented in Figure 1, from which it is clear that the obtained yield increased with the increase of K2Cr2O7 reaching maximum value at 0.3 M. From the left part of the curve it is clear that the polymer yield increases from 0.04 M to 0.3 M then decreases from 0.3 M to 0.5 M. This could be due to the fact that, in the first part of the curve, the produced initiator ion radical moieties activate the backbone and simultaneously produced the o-phenylenediamine ion radical, which takes place immediately, and, therefore, yield increases with the increase of potassium dichromate concentration up to 0.3 M. But in the second part of the curve, the polymer yield decreases with increasing K2Cr2O7 concentration, may be due to a high concentration of oxidant promote the formation of low molecular weight oxidation product and also degrade the product polymer which easily soluble in water [13].Figure 1
Yield-K2Cr2O7 concentration effect on the aqueous oxidative polymerization of poly-o-phenylenediamine (POPDA).


### 3.1.2. Effect of HCl Concentration

The effect of HCl concentration on the aqueous oxidative polymerization of OPDA was investigated using constant concentration of K2Cr2O7 at 0.3 M and monomer concentration at 0.1 M and using different concentration of HCl at 5
±
0.2°C. The yield-time data was represented in Figure 2, from which it is clear that the obtained yield increases in the acid concentration range from 0.04 to 0.2 then decreases gradually up to 0.5 M. This behavior may be due to, at higher concentration of HCl, the degradation of the polymer in the early stages of the reaction, which may be due to the hydrolysis of polyemeraldine chain [13].Figure 2
Yield-HCl concentration effect on the aqueous oxidative polymerization of poly-o-phenylenediamine (POPDA).


### 3.1.3. Effect of O-Phenylenediamine Concentration

The effect of monomer concentration on the polymerization efficiency was investigated in the range of monomer concentration from 0.02 to 0.5 M and the data was represented in Figure3, from which it is clear that the optimum yield formation is obtained at 0.1 M of the monomer concentration.Figure 3
Yield-monomer concentration effect on the aqueous oxidative polymerization of poly-o-phenylenediamine (POPDA).


## 3.1.1. Effect of Potassium Dichromate Concentration

Both of the monomer and HCl concentrations are fixed at 0.1 M while the oxidant concentrations were varied from 0.04 to 0.5 M at5
±
0.2°C to investigate the optimum polymerization condition of K2Cr2O7. The yield-time curve was represented in Figure 1, from which it is clear that the obtained yield increased with the increase of K2Cr2O7 reaching maximum value at 0.3 M. From the left part of the curve it is clear that the polymer yield increases from 0.04 M to 0.3 M then decreases from 0.3 M to 0.5 M. This could be due to the fact that, in the first part of the curve, the produced initiator ion radical moieties activate the backbone and simultaneously produced the o-phenylenediamine ion radical, which takes place immediately, and, therefore, yield increases with the increase of potassium dichromate concentration up to 0.3 M. But in the second part of the curve, the polymer yield decreases with increasing K2Cr2O7 concentration, may be due to a high concentration of oxidant promote the formation of low molecular weight oxidation product and also degrade the product polymer which easily soluble in water [13].Figure 1
Yield-K2Cr2O7 concentration effect on the aqueous oxidative polymerization of poly-o-phenylenediamine (POPDA).


## 3.1.2. Effect of HCl Concentration

The effect of HCl concentration on the aqueous oxidative polymerization of OPDA was investigated using constant concentration of K2Cr2O7 at 0.3 M and monomer concentration at 0.1 M and using different concentration of HCl at 5
±
0.2°C. The yield-time data was represented in Figure 2, from which it is clear that the obtained yield increases in the acid concentration range from 0.04 to 0.2 then decreases gradually up to 0.5 M. This behavior may be due to, at higher concentration of HCl, the degradation of the polymer in the early stages of the reaction, which may be due to the hydrolysis of polyemeraldine chain [13].Figure 2
Yield-HCl concentration effect on the aqueous oxidative polymerization of poly-o-phenylenediamine (POPDA).


## 3.1.3. Effect of O-Phenylenediamine Concentration

The effect of monomer concentration on the polymerization efficiency was investigated in the range of monomer concentration from 0.02 to 0.5 M and the data was represented in Figure3, from which it is clear that the optimum yield formation is obtained at 0.1 M of the monomer concentration.Figure 3
Yield-monomer concentration effect on the aqueous oxidative polymerization of poly-o-phenylenediamine (POPDA).


## 3.2. The Kinetic Study of the Polymerization Reaction

### 3.2.1. Effect of Potassium Dichromate Concentration

The aqueous polymerization of OPDA (0.1 mol) was carried out in 25 mL of HCl solution (0.2 mol) in the presence of 25 mL potassium dichromate as oxidant of different molarities at 5°C for different time intervals. The yield-time curves were plotted for different oxidant concentrations and the data are graphically represented in Figure4(a). The initial and overall reaction rates were determined using the following equation:
(2)
Rate
(
R
i
)
=
P
V
×
M
×
t
,
where P is the weight of the obtained polymer, t is the time in seconds, M is the molecular weight of the monomer, and V is the reaction volume in liter.(a) Yield-time curve for the effect of potassium dichromate concentration on the polymerization (POPDA) at different time intervals. (b) Double logarithmic plot of the initial rate and oxidant concentration of POPDA.
(a)
(b)The initial and overall reaction rates of the polymerization reaction increase with the increase of oxidant concentration in the range between 0.05 and 0.3 mol/L. The oxidant exponent was determined from the relation between logarithm of the initial rate of polymerization Log (R
i) and logarithm of the oxidant concentration. A straight line was obtained which has a slope of 1.011 as represented in Figure 4(b). This means that the polymerization reaction of OPDA is a first-order reaction with respect to the oxidant.


### 3.2.2. Effect of Hydrochloric Acid Concentration

The polymerization of OPDA (0.1 mol) in 25 mL of HCl with different molarities was carried out by addition of 25 mL potassium dichromate (0.3 mol/L) as oxidant at 5°C for different time intervals. The concentration of the monomer and oxidant were kept constant during the study of HCl effect on the polymerization reaction. The experiments were carried out as described in Section2.2, and the yield-time curve was plotted for each acid concentration used. The data are graphically represented in Figure 5(a), from which it is clear that both the initial and overall reaction rates of the polymerization reaction increase with the increasing of HCl concentrations in the range between 0.05 and 0.2 mol/L. The HCl exponent determined from the slope of the straight line represented in Figure 5(b) was found to be 0.954, which means that the polymerization order with respect to the HCl concentration is a first-order reaction.(a) Yield-time curve for the effect of HCl concentration on the aqueous oxidative polymerization of (POPDA) at different time intervals. (b) Double logarithmic plot of the initial rate and HCl concentration of POPDA.
(a)
(b)


### 3.2.3. Effect of Monomer (OPDA) Concentration

The aqueous polymerization of OPDA was carried out in 25 mL of HCl solution (0.2 mol/L) in the presence of 25 mL potassium dichromate (0.3 mol/L) as oxidant at 5°C for different time intervals. The yield-time curve was plotted for each monomer concentration used. The data are graphically represented in Figure6(a). The monomer exponent was determined from the slope of the straight line represented in Figure 6(b) for the relation between log R
i and logarithm of the monomer concentration. The slope of this linear relationship was found to be 1.045. This means that the polymerization reaction with respect to the monomer concentration is a first-order reaction.(a) Conversion-monomer/mol concentration effect on the aqueous oxidative polymerization of (POPDA) at different time intervals. (b) Double logarithmic plot of the initial rate and monomer concentration of POPDA.
(a)
(b)


## 3.2.1. Effect of Potassium Dichromate Concentration

The aqueous polymerization of OPDA (0.1 mol) was carried out in 25 mL of HCl solution (0.2 mol) in the presence of 25 mL potassium dichromate as oxidant of different molarities at 5°C for different time intervals. The yield-time curves were plotted for different oxidant concentrations and the data are graphically represented in Figure4(a). The initial and overall reaction rates were determined using the following equation:
(2)
Rate
(
R
i
)
=
P
V
×
M
×
t
,
where P is the weight of the obtained polymer, t is the time in seconds, M is the molecular weight of the monomer, and V is the reaction volume in liter.(a) Yield-time curve for the effect of potassium dichromate concentration on the polymerization (POPDA) at different time intervals. (b) Double logarithmic plot of the initial rate and oxidant concentration of POPDA.
(a)
(b)The initial and overall reaction rates of the polymerization reaction increase with the increase of oxidant concentration in the range between 0.05 and 0.3 mol/L. The oxidant exponent was determined from the relation between logarithm of the initial rate of polymerization Log (R
i) and logarithm of the oxidant concentration. A straight line was obtained which has a slope of 1.011 as represented in Figure 4(b). This means that the polymerization reaction of OPDA is a first-order reaction with respect to the oxidant.


## 3.2.2. Effect of Hydrochloric Acid Concentration

The polymerization of OPDA (0.1 mol) in 25 mL of HCl with different molarities was carried out by addition of 25 mL potassium dichromate (0.3 mol/L) as oxidant at 5°C for different time intervals. The concentration of the monomer and oxidant were kept constant during the study of HCl effect on the polymerization reaction. The experiments were carried out as described in Section2.2, and the yield-time curve was plotted for each acid concentration used. The data are graphically represented in Figure 5(a), from which it is clear that both the initial and overall reaction rates of the polymerization reaction increase with the increasing of HCl concentrations in the range between 0.05 and 0.2 mol/L. The HCl exponent determined from the slope of the straight line represented in Figure 5(b) was found to be 0.954, which means that the polymerization order with respect to the HCl concentration is a first-order reaction.(a) Yield-time curve for the effect of HCl concentration on the aqueous oxidative polymerization of (POPDA) at different time intervals. (b) Double logarithmic plot of the initial rate and HCl concentration of POPDA.
(a)
(b)


## 3.2.3. Effect of Monomer (OPDA) Concentration

The aqueous polymerization of OPDA was carried out in 25 mL of HCl solution (0.2 mol/L) in the presence of 25 mL potassium dichromate (0.3 mol/L) as oxidant at 5°C for different time intervals. The yield-time curve was plotted for each monomer concentration used. The data are graphically represented in Figure6(a). The monomer exponent was determined from the slope of the straight line represented in Figure 6(b) for the relation between log R
i and logarithm of the monomer concentration. The slope of this linear relationship was found to be 1.045. This means that the polymerization reaction with respect to the monomer concentration is a first-order reaction.(a) Conversion-monomer/mol concentration effect on the aqueous oxidative polymerization of (POPDA) at different time intervals. (b) Double logarithmic plot of the initial rate and monomer concentration of POPDA.
(a)
(b)


## 3.3. Calculation of the Thermodynamic Activation Parameters

The polymerization of OPDA (0.1 mol/L) in 25 mL of 0.2 mol/L HCl in presence of 25 mL potassium dichromate (0.3 mol/L) as oxidant solution was carried out at 5, 10, and 15°C for different time periods. The yield-time curves were graphically represented in Figure7, from which it is clear that both of the initial and overall reaction rates increase with raising the reaction temperature. The apparent activation energy (E
a) of the aqueous polymerization reaction of o-phenylenediamine was calculated using the following Arrhenius equation:
(3)
Log
(
K
)
=
-
E
a
2.303
R
T
+
C
,
where K is the rate, R is the universal gas constant, T is the reaction temperature, and C is constant.Figure 7
Yield-time curve for the effect of temperature on the aqueous oxidative polymerization of POPDA.By plotting logR
i against 1
/
T, which gave a straight line as shown in Figure 8, and from the slope we can calculate the activation energy. The apparent activation energy for this system is 63.658 kJ/mol. The Enthalpy and entropy of activation for the polymerization reaction can be calculated by the calculation of K
2 from the following equation:
(4)
Reaction
Rate
=
K
2
[
oxidant
]
1.011
[
HCl
]
0.954
[
monomer
]
1.045
.Figure 8
The relation between the logarithm of initial rate and (1
/
T) for aqueous oxidative polymerization of POPDA.The values ofK
2 at 5, 10, and 15°C were 6.131 × 10−6, 1.054 × 10−5, and 1.594 × 10−5, respectively. The enthalpy (Δ
H
*) and entropy (Δ
S
*) of activation associated with K
2 were calculated using Eyring equation
(5)
K
2
=
(
R
T
N
h
)
e
Δ
S
*
/
R
·
e
-
Δ
H
*
/
R
T
,
where K
2 is the rate constant, N is the Avogadro’s number, R is the universal gas constant, and h is planks constant.By dividing the above equation byT and taking its natural logarithm we obtain the following equation:
(6)
Ln
(
K
2
T
)
=
ln
⁡
⁡
(
R
N
h
)
+
Δ
S
*
R
+
-
Δ
H
*
R
T
.Figure9 shows the relation between K
2/T versus 1/T, which gives a linear relationship with (-
Δ
H
*)/R and intercept line (ln R/N
h + Δ
S
*/R) from the slops and intercept; the values of Δ
H
* and Δ
S
* were found to be 61.48 kJmol−1 and 29.95 Jmol-1K−1, respectively.Figure 9
The relation between logK
2/T and 1/T for poly-o-phenylenediamine (POPDA).The intramolecular electron transfer steps for the oxidation reaction are endothermic as indicated by the value ofΔ
H
*. The contributions of Δ
H
* and Δ
S
* to the rate constant seem to compensate each other. This fact suggests that the factors controlling Δ
H
* must be closely related to those controlling Δ
S
*. Therefore, the salvation state of the encounter compound could be important in determination of Δ
H
*. Consequently, the relatively small enthalpy of activation can be explained in terms of the formation of more solvated complex.


## 3.4. Polymerization Mechanism

The aqueous oxidative polymerization of o-phenylenediamine is described in the Experimental section and follows three steps [29].The Initial Step. Potassium dichromate in acidified aqueous solution produces chromic acid as shown in
(7)
K
2
Cr
2
O
7
+
H
2
O
+
2
H
+
=
2
K
+
+
2
H
2
CO
4
.This reaction is controlled by the change in pH; the orange red dichromate ions (Cr2O7)2- are in equilibrium with the (HCrO4)- in the range of pH-values between 2 and 6, but at pH below 1 the main species is (H2CrO4) and the equilibria can occur as follows:
(8)
(
HCrO
4
)
-
⇌
(
CrO
4
)
2
-
+
H
+
K
=
10
-
5.9
(9)
(
H
2
CrO
4
)
⇌
(
HCrO
4
)
-
+
H
+
K
=
4.1
(10)
2
(
HCrO
4
)
-
⇌
(
Cr
2
O
7
)
2
-
+
H
2
O
K
=
10
-
2
.
2
.
The chromic acid withdraws one electron from each protonated OPDA and probably forms a metastable complex as shown in (11):(11)The complex undergoes dissociation to form monomer cation radical as shown in (12):(12)Generally, the initial step is rapid and may occur in short time, 0–5 min (autocatalytic reaction); no polymeric product is being obtained. After 5 min of the polymerization reaction, the polymeric products are obtained.Propagation Step. This step involves the interaction between the formed radical cation and the monomer to form a dimer radical cation. In the case of Cr(VI) oxidation of the organic compounds, Cr(VI) is reduced to Cr(IV) first and then to Cr(III) [29]. Transfer of two electrons from two monomer ions radical by H2CrO4 produces para semidine salt along with chromous acid H2Cr2O3 (Cr(IV)). The intermediately produced Cr(IV) oxidises para semidine to pernigraniline salt (PS) at suitable low pH and the PS acts as a catalyst for conversion of OPDA to POPDA:(13)(14)This reaction is followed by further reaction of the formed dimmer radical cations with monomer molecules to form trimer radical cations and so on. The degree of polymerization depends on different factors such as dichromate concentration, HCl concentration, monomer concentration, and temperature. By adding (7), (11), (12), (13), and (14),(15)
(16)
12
OPDA
+
5
K
2
Cr
2
O
7
+
34
H
+
=
6
PS
+
10
Cr
3
+
+
10
K
+
+
35
H
2
O
.Termination Step. Termination of the reaction occurs by the addition of ammonium hydroxide solution in an equimolar amount to HCl present in the reaction medium (till pH = 7), which leads to cessation of the redox reaction. The reaction could occur as follows:(17)


## 3.5. Characterization of the Obtained Polymer

### 3.5.1. The Solubility

The solubility of POPDA was investigated in N-methyl pyrrolidone, dimethylformamide (DMF), acetone, methanol, iso propanol, benzene, hexane, and chloroform. The solubility values are listed in Table1. The complete solubility was found in N-methyl pyrrolidone, then in DMF 2.235 g/L followed by acetone 1.67 g/L, then in methanol 1.074 g/L then followed by iso propanol 0.879 g/L at 20°C but not soluble in benzene, hexane, and chloroform.Table 1
Solubility of poly-o-phenylenediamine (POPDA) in different solvents at 20°C.
Solvent
Solubility of (POPDA) in (g/L)
N-methyl-2-pyrrolidone
Completely soluble
Dimethylformamide
2.235
Acetone
1.679
Methanol
1.074
Iso propanol
0.879


### 3.5.2. The Elemental Analysis

The data obtained from elemental analysis using oxygen flask combustion and a dosimat E415 titrator shows that the found carbon content of (POPDA) is lower than the calculated value. This is due to the formation of chromium carbide during step of heating and measuring process while the found values of nitrogen and hydrogen are 20.91 and 4.37, respectively, which are in good agreement with the calculated one for the suggested structure present in Scheme1. By measuring another sample of the (POPDA) which was prepared by using ammonium persulfate as oxidant, the found value of carbon is higher than sample which is prepared by using potassium dichromate as oxidant. For more information about the chemical composition of (POPDA), the XPS study was conducted as mentioned under point 3.5.2.Scheme 1
Structure of the prepared (POPDA).


### 3.5.3. X-Ray Photoelectron Spectroscopy (XPS) Characterization

(
1) XPS Survey Elemental Composition. X-ray photoelectron spectroscopy (XPS) is used to study the composition of materials, which detect elements starting from Li (Z = 3) and higher elements. Hydrogen (Z = 1) and helium (Z = 2) cannot be detected due to the low probability of electron emission. XPS survey begins from 0 to 1400 (eV) as shown in Figure 10. The XPS survey scan spectrum of the prepared polymer shows the presence of C, N, O, Cl, and Cr. The Cl was present as doping anion in the prepared polymer. Chrome was found due to the polymer prepared using potassium dichromate as oxidant. It is possible for chromium ion (Cr+3) to present between polymer chains as a sandwich-bonded C6H6–C6H6 groups as shown in Scheme 1 and the usual formation procedure is hydrolyzing the reaction mixture with dilute acid which gives the cation (C6H6)2Cr3+ [30, 31].Figure 10
X-ray photoelectron spectroscopy (XPS) survey elemental composition of poly-o-phenylenediamine (POPDA).The XPS elemental analysis of the prepared polymer is given in Table2. The data shows that there is a good agreement with the calculated one for the suggested structures present in Scheme 1.Table 2
The XPS elemental analysis of poly-o-phenylenediamine (POPDA).
C%
N%
Cl%
O%
Cr%
Calc.
Found
Calc.
Found
Calc.
Found
Calc.
Found
Calc.
Found
57.21
56.11
22.25
21.89
7.05
6.94
3.18
3.02
10.31
10.11(
2) XPS Spectra of Poly(OPDA). Four main peaks were obtained for C1s spectra of poly(OPDA) as shown in Figure 11(a). The sharp peak appearing at 283.98 eV is attributed to C–H (C1) bond, while the peak appearing at 284.18 eV is attributed to C–C (C2) bond. The peak appearing at 285.08 eV is assigned to C–N (C3) bond while the peak appearing at 287.58 eV is attributed to C–O or C–N+ (C4) bond [32–34].X-ray photoelectron spectroscopy (XPS) spectra of (POPDA).
(a)
(b)
(c)
(d)
(e)N1s Figure11(b) shows the XPS N1s spectrum of poly(OPDA) which has three distinct curves. The first two peaks are assigned to imine (–N=) at 398.58 eV and amine (–NH–) at 399.23 eV. Moreover, the peak that appears at 400.58 eV is due to positively charged nitrogen atom (N+).Two distinct oxygen species contribute to the oxygen 1 s signals in the conducting polymers (Figure11(c)). The distinct energy peaks at 530.68 and 533.12 eV could be attributed to Cr2O3 and C–OH, respectively.The Cl 2p spectrum of poly(OPDA) is shown in Figure11(d). In order to estimate the anion Cl at the surface, Cl 2p peaks are fitted with a number of spin-orbit doublets (Cl 2p1/2 and Cl 2p3/2) with the B.E. for the C12p3/2 peaks at about 197.36, 198.34, and 200.1 eV. The lowest and the highest B.E. components are attributable to the ionic and covalent chlorine species (Cl- and –Cl), respectively. The chlorine species (Cl*) with the intermediate appear at B.E. of 198.34 eV. The lower B.E. value of the Cl* species compared to the Cl species suggests the presence of chloride anion in a more positive environment, probably arising from an increase in the number of positively charged nitrogen in the polymer chain associated with the formation of polarons and bipolarons.The Cr spectrum of (POPDA) is shown in Figure11(e). The main components corresponding to different chemical chromium species were observed in the high-resolution Cr2p3/2 spectrums. The first peak at 576.18 eV ± 0.2 eV was assigned to Cr2O3 which is in agreement with what was found by Chowdhury and Saha [13] and Stefanov et al. [35], also indicated by a distinct O1s peak at 530.68 eV typical for Cr2O3 which may be adsorbed on polymer surface during chromous acid H2Cr2O3 oxidation process. There is also a component visible that corresponds to Cr2p1/2 at 586.08 eV, which was attributed to Cr3+. This data reveal that chromium ion is present between benzene rings of polymeric chain as shown in Scheme 1.


### 3.5.4. The Infrared Spectroscopic Analysis of (OPDA) Monomer and Its Analogs Polymer

The IR spectra of the OPDA and its polymer (POPDA) are represented in Figure12, while the absorption band values and their assignments are summarized in Table 3. The medium absorption band appearing at 453 cm−1, which could be attributed to bending deformation of N–H group attached to benzene ring in case of monomer, appears at 518 cm−1 with slight shift in case of polymer. The broad absorption band appearing at 778 cm−1 in case of monomer, which could be attributed to out of plane deformation of CH for 1,2-disubstituted benzene, appears at 748 cm−1 with slight shift in case of polymer. A series of absorption bands appear in the region from 924 to 1152 cm−1 which could be attributed to the out of plane C–H deformation of 1,2-disubistuition benzene ring in case of monomer and 1,2,4 tri-substituted of benzene ring, in case of polymer. The sharp absorption bands appear at 1336 cm−1 in case of the monomer, which could be attributed to symmetric stretching vibration of C–N, appears at 1362 cm−1 with slight shift in case of polymer. The sharp absorption band appearing at 1490 cm−1 in case of the monomer may be attributed to C=C aromatic stretching vibration, which appears at 1500 cm−1 with slight shift in case of polymer. The sharp absorption band appearing at 1630 cm−1 in case of the monomer, which may be attributed to C=C deformation of benzene ring, appears at 1621 cm−1 with slight shift in case of polymer. The shoulder absorption band appears at 3032 cm−1 in case of the monomer which could be attributed to symmetric stretching vibration of C–H in aromatic ring and disappears in case of polymer. The triplet absorption bands appearing at 3190, 3281, and 3370 cm−1 in case of monomer could be attributed to asymmetric stretching vibration for NH group, but in case of polymer a broad absorption band that appears at 3354 cm−1 could be attributed to asymmetric stretching vibration for NH group and OH group present in the polymer structure.Table 3
Infrared absorption bands and their assignments of o-phenylene-diamine monomer (OPDA) and its analogs polymer (POPDA).
Wave number (cm−1)
Assignments
(OPDA)Monomer
(POPDA)Polymer
453m
—
Bending deformation of NH in primary aromatic amines
—
518m
748b
—
Out-of-plane bending deformation of CH in 1,2 disubstituted in benzene ring
—
761b
810s
—
Out-of-plane deformation showing 1,4-disubistuition  in the benzene ring
—
833sh
924s
—
Plane C–H deformation of 1,2-disubistuition of benzene ring
—
1044w
1056m
—
1117s
—
—
1133w
1152
—
1336s
1362sh
Symmetric stretching vibration for C–O or C–N group
1490s
1500b
Symmetric stretching vibration for C–C aromatic
1590s
—
Stretching vibration of C–N or combination band for protonated primary aromatic amine
1630s
1621b
N–H deformation of secondary amine
3032sh
—
Symmetric stretching vibration of N–H
3281s
3354m
Asymmetric stretching vibration for NH
2930sh
3354b
Asymmetric stretching vibration for CH group in aliphatic chain
3370s
—
Symmetric stretching vibration of =C–H
s: sharp; m: medium; w: weak; b: broad; sh: shoulder.Figure 12
The infrared spectrum of o-phenylenediamine (OPDA) (a) and it analogous polymer (POPDA) (b).


### 3.5.5. The UV-Visible Spectroscopic Study of OPDA Monomer and Its Analogs Polymer

The UV-visible spectra of OPDA and its polymer are represented in Figure13; the spectra show the following absorption bands:(1)
in case of monomer, two absorption bands appear atλ
max
⁡ = 219 and 240 nm which may be attributed to π-π* transition (E2-band) of the benzene ring and the β-band (A
1
g
-
B
2
u);
(2)
in case of polymer, two absorption bands appear atλ
max
⁡ = 221 and 243 nm which may be attributed to π-π* transition showing a bathochromic shift. Beside these two bands, broad absorption band appears in the visible region at λ
max
⁡ = 417 nm which may be due to the high conjugation of the aromatic polymeric chain.Figure 13
UV-visible spectra of o-phenylenediamine (OPDA) (A) and it analogous polymer (POPDA) (B).


### 3.5.6. Thermal Gravimetric Analysis (TGA) of Poly O-Phenylenediamine

Thermogravimetric analysis (TGA) for the prepared polymer has been investigated and the TGA-curve is represented in Figure14. The calculated and found data for the prepared polymers are summarized in Table 4. The thermal degradation steps are summarized as follows:(1)
the first stage includes the loss of one water molecule in the temperature range between 29.5 and 122.6°C; the weight loss of this step was found to be 3.21% which is in a good agreement with the calculated one;
(2)
in the second stage, in the temperature range between 122.6 and 203.8°C, the weight loss was found to be 6.65%, which could be attributed to the loss of one HCl molecule. The calculated weight loss is in good agreement with the found one;
(3)
in the third stage, in the temperature range between 203.8 and 320.3°C, the weight loss was found to be 11.79%, which is attributed to the loss of four (NH2) groups. The calculated weight loss for this stage is equal to 12.11%;
(4)
in the fourth stage, in the temperature range between 320.3 and 400.0°C, the weight loss was found to be 16.95%, which could be attributed to the loss of one molecule of C6H3–NH. The calculated weight loss of this stage is equal to 17.22%;
(5)
in the fifth stage, in the temperature range between 400.0 and 523.4°C, the weight loss was found to be 13.78%, which is attributed to the loss of one molecule of phenyl ring. The calculated weight loss of this stage is equal to 14.19%;
(6)
in the last stage, above 523.38°C, the remaining polymer molecule was found to be 47.62% including the metallic residue, but the calculated one was found to be 46.46%.Table 4
Thermogravimetric data of poly-o-phenylenediamine (POPDA).
Name
Temperaturerange °C
Weight loss (%)
The removedmolecule
Calc.
Found
Poly(POPDA)
29.5–122.6
3.41
3.212
H2O
122.6–203.8
6.91
6.652
HCl
203.8–320.3
12.11
11.791
4NH2
320.3–400.00
17.22
16.952
C6H3–NH
400–523.40
14.19
13.778
C6H3
Remaining weight (%) above 600
46.17
47.62
—Figure 14
The thermal gravimetric analysis (TGA) for (POPDA).


### 3.5.7. The X-Ray Diffraction Analysis and Transmission Electron Microscope

The X-Ray diffraction patterns of the prepared polymer are represented in Figure15. The figure shows that the prepared poly o-phenylenediamine is completely amorphous.Figure 15
X-ray poly-o-phenylenediamine (POPDA).Morphology of poly o-phenylenediamine was characterized by transmission electron microscope. Figure16 shows TEM image of poly o-phenylenediamine which nearly spherical or ellipsoidal particles with approximate diameter 60–120 nm either separated or linked with each other.Figure 16
The transmission electron microscope of POPDA.


## 3.5.1. The Solubility

The solubility of POPDA was investigated in N-methyl pyrrolidone, dimethylformamide (DMF), acetone, methanol, iso propanol, benzene, hexane, and chloroform. The solubility values are listed in Table1. The complete solubility was found in N-methyl pyrrolidone, then in DMF 2.235 g/L followed by acetone 1.67 g/L, then in methanol 1.074 g/L then followed by iso propanol 0.879 g/L at 20°C but not soluble in benzene, hexane, and chloroform.Table 1
Solubility of poly-o-phenylenediamine (POPDA) in different solvents at 20°C.
Solvent
Solubility of (POPDA) in (g/L)
N-methyl-2-pyrrolidone
Completely soluble
Dimethylformamide
2.235
Acetone
1.679
Methanol
1.074
Iso propanol
0.879


## 3.5.2. The Elemental Analysis

The data obtained from elemental analysis using oxygen flask combustion and a dosimat E415 titrator shows that the found carbon content of (POPDA) is lower than the calculated value. This is due to the formation of chromium carbide during step of heating and measuring process while the found values of nitrogen and hydrogen are 20.91 and 4.37, respectively, which are in good agreement with the calculated one for the suggested structure present in Scheme1. By measuring another sample of the (POPDA) which was prepared by using ammonium persulfate as oxidant, the found value of carbon is higher than sample which is prepared by using potassium dichromate as oxidant. For more information about the chemical composition of (POPDA), the XPS study was conducted as mentioned under point 3.5.2.Scheme 1
Structure of the prepared (POPDA).


## 3.5.3. X-Ray Photoelectron Spectroscopy (XPS) Characterization

(
1) XPS Survey Elemental Composition. X-ray photoelectron spectroscopy (XPS) is used to study the composition of materials, which detect elements starting from Li (Z = 3) and higher elements. Hydrogen (Z = 1) and helium (Z = 2) cannot be detected due to the low probability of electron emission. XPS survey begins from 0 to 1400 (eV) as shown in Figure 10. The XPS survey scan spectrum of the prepared polymer shows the presence of C, N, O, Cl, and Cr. The Cl was present as doping anion in the prepared polymer. Chrome was found due to the polymer prepared using potassium dichromate as oxidant. It is possible for chromium ion (Cr+3) to present between polymer chains as a sandwich-bonded C6H6–C6H6 groups as shown in Scheme 1 and the usual formation procedure is hydrolyzing the reaction mixture with dilute acid which gives the cation (C6H6)2Cr3+ [30, 31].Figure 10
X-ray photoelectron spectroscopy (XPS) survey elemental composition of poly-o-phenylenediamine (POPDA).The XPS elemental analysis of the prepared polymer is given in Table2. The data shows that there is a good agreement with the calculated one for the suggested structures present in Scheme 1.Table 2
The XPS elemental analysis of poly-o-phenylenediamine (POPDA).
C%
N%
Cl%
O%
Cr%
Calc.
Found
Calc.
Found
Calc.
Found
Calc.
Found
Calc.
Found
57.21
56.11
22.25
21.89
7.05
6.94
3.18
3.02
10.31
10.11(
2) XPS Spectra of Poly(OPDA). Four main peaks were obtained for C1s spectra of poly(OPDA) as shown in Figure 11(a). The sharp peak appearing at 283.98 eV is attributed to C–H (C1) bond, while the peak appearing at 284.18 eV is attributed to C–C (C2) bond. The peak appearing at 285.08 eV is assigned to C–N (C3) bond while the peak appearing at 287.58 eV is attributed to C–O or C–N+ (C4) bond [32–34].X-ray photoelectron spectroscopy (XPS) spectra of (POPDA).
(a)
(b)
(c)
(d)
(e)N1s Figure11(b) shows the XPS N1s spectrum of poly(OPDA) which has three distinct curves. The first two peaks are assigned to imine (–N=) at 398.58 eV and amine (–NH–) at 399.23 eV. Moreover, the peak that appears at 400.58 eV is due to positively charged nitrogen atom (N+).Two distinct oxygen species contribute to the oxygen 1 s signals in the conducting polymers (Figure11(c)). The distinct energy peaks at 530.68 and 533.12 eV could be attributed to Cr2O3 and C–OH, respectively.The Cl 2p spectrum of poly(OPDA) is shown in Figure11(d). In order to estimate the anion Cl at the surface, Cl 2p peaks are fitted with a number of spin-orbit doublets (Cl 2p1/2 and Cl 2p3/2) with the B.E. for the C12p3/2 peaks at about 197.36, 198.34, and 200.1 eV. The lowest and the highest B.E. components are attributable to the ionic and covalent chlorine species (Cl- and –Cl), respectively. The chlorine species (Cl*) with the intermediate appear at B.E. of 198.34 eV. The lower B.E. value of the Cl* species compared to the Cl species suggests the presence of chloride anion in a more positive environment, probably arising from an increase in the number of positively charged nitrogen in the polymer chain associated with the formation of polarons and bipolarons.The Cr spectrum of (POPDA) is shown in Figure11(e). The main components corresponding to different chemical chromium species were observed in the high-resolution Cr2p3/2 spectrums. The first peak at 576.18 eV ± 0.2 eV was assigned to Cr2O3 which is in agreement with what was found by Chowdhury and Saha [13] and Stefanov et al. [35], also indicated by a distinct O1s peak at 530.68 eV typical for Cr2O3 which may be adsorbed on polymer surface during chromous acid H2Cr2O3 oxidation process. There is also a component visible that corresponds to Cr2p1/2 at 586.08 eV, which was attributed to Cr3+. This data reveal that chromium ion is present between benzene rings of polymeric chain as shown in Scheme 1.


## 3.5.4. The Infrared Spectroscopic Analysis of (OPDA) Monomer and Its Analogs Polymer

The IR spectra of the OPDA and its polymer (POPDA) are represented in Figure12, while the absorption band values and their assignments are summarized in Table 3. The medium absorption band appearing at 453 cm−1, which could be attributed to bending deformation of N–H group attached to benzene ring in case of monomer, appears at 518 cm−1 with slight shift in case of polymer. The broad absorption band appearing at 778 cm−1 in case of monomer, which could be attributed to out of plane deformation of CH for 1,2-disubstituted benzene, appears at 748 cm−1 with slight shift in case of polymer. A series of absorption bands appear in the region from 924 to 1152 cm−1 which could be attributed to the out of plane C–H deformation of 1,2-disubistuition benzene ring in case of monomer and 1,2,4 tri-substituted of benzene ring, in case of polymer. The sharp absorption bands appear at 1336 cm−1 in case of the monomer, which could be attributed to symmetric stretching vibration of C–N, appears at 1362 cm−1 with slight shift in case of polymer. The sharp absorption band appearing at 1490 cm−1 in case of the monomer may be attributed to C=C aromatic stretching vibration, which appears at 1500 cm−1 with slight shift in case of polymer. The sharp absorption band appearing at 1630 cm−1 in case of the monomer, which may be attributed to C=C deformation of benzene ring, appears at 1621 cm−1 with slight shift in case of polymer. The shoulder absorption band appears at 3032 cm−1 in case of the monomer which could be attributed to symmetric stretching vibration of C–H in aromatic ring and disappears in case of polymer. The triplet absorption bands appearing at 3190, 3281, and 3370 cm−1 in case of monomer could be attributed to asymmetric stretching vibration for NH group, but in case of polymer a broad absorption band that appears at 3354 cm−1 could be attributed to asymmetric stretching vibration for NH group and OH group present in the polymer structure.Table 3
Infrared absorption bands and their assignments of o-phenylene-diamine monomer (OPDA) and its analogs polymer (POPDA).
Wave number (cm−1)
Assignments
(OPDA)Monomer
(POPDA)Polymer
453m
—
Bending deformation of NH in primary aromatic amines
—
518m
748b
—
Out-of-plane bending deformation of CH in 1,2 disubstituted in benzene ring
—
761b
810s
—
Out-of-plane deformation showing 1,4-disubistuition  in the benzene ring
—
833sh
924s
—
Plane C–H deformation of 1,2-disubistuition of benzene ring
—
1044w
1056m
—
1117s
—
—
1133w
1152
—
1336s
1362sh
Symmetric stretching vibration for C–O or C–N group
1490s
1500b
Symmetric stretching vibration for C–C aromatic
1590s
—
Stretching vibration of C–N or combination band for protonated primary aromatic amine
1630s
1621b
N–H deformation of secondary amine
3032sh
—
Symmetric stretching vibration of N–H
3281s
3354m
Asymmetric stretching vibration for NH
2930sh
3354b
Asymmetric stretching vibration for CH group in aliphatic chain
3370s
—
Symmetric stretching vibration of =C–H
s: sharp; m: medium; w: weak; b: broad; sh: shoulder.Figure 12
The infrared spectrum of o-phenylenediamine (OPDA) (a) and it analogous polymer (POPDA) (b).


## 3.5.5. The UV-Visible Spectroscopic Study of OPDA Monomer and Its Analogs Polymer

The UV-visible spectra of OPDA and its polymer are represented in Figure13; the spectra show the following absorption bands:(1)
in case of monomer, two absorption bands appear atλ
max
⁡ = 219 and 240 nm which may be attributed to π-π* transition (E2-band) of the benzene ring and the β-band (A
1
g
-
B
2
u);
(2)
in case of polymer, two absorption bands appear atλ
max
⁡ = 221 and 243 nm which may be attributed to π-π* transition showing a bathochromic shift. Beside these two bands, broad absorption band appears in the visible region at λ
max
⁡ = 417 nm which may be due to the high conjugation of the aromatic polymeric chain.Figure 13
UV-visible spectra of o-phenylenediamine (OPDA) (A) and it analogous polymer (POPDA) (B).


## 3.5.6. Thermal Gravimetric Analysis (TGA) of Poly O-Phenylenediamine

Thermogravimetric analysis (TGA) for the prepared polymer has been investigated and the TGA-curve is represented in Figure14. The calculated and found data for the prepared polymers are summarized in Table 4. The thermal degradation steps are summarized as follows:(1)
the first stage includes the loss of one water molecule in the temperature range between 29.5 and 122.6°C; the weight loss of this step was found to be 3.21% which is in a good agreement with the calculated one;
(2)
in the second stage, in the temperature range between 122.6 and 203.8°C, the weight loss was found to be 6.65%, which could be attributed to the loss of one HCl molecule. The calculated weight loss is in good agreement with the found one;
(3)
in the third stage, in the temperature range between 203.8 and 320.3°C, the weight loss was found to be 11.79%, which is attributed to the loss of four (NH2) groups. The calculated weight loss for this stage is equal to 12.11%;
(4)
in the fourth stage, in the temperature range between 320.3 and 400.0°C, the weight loss was found to be 16.95%, which could be attributed to the loss of one molecule of C6H3–NH. The calculated weight loss of this stage is equal to 17.22%;
(5)
in the fifth stage, in the temperature range between 400.0 and 523.4°C, the weight loss was found to be 13.78%, which is attributed to the loss of one molecule of phenyl ring. The calculated weight loss of this stage is equal to 14.19%;
(6)
in the last stage, above 523.38°C, the remaining polymer molecule was found to be 47.62% including the metallic residue, but the calculated one was found to be 46.46%.Table 4
Thermogravimetric data of poly-o-phenylenediamine (POPDA).
Name
Temperaturerange °C
Weight loss (%)
The removedmolecule
Calc.
Found
Poly(POPDA)
29.5–122.6
3.41
3.212
H2O
122.6–203.8
6.91
6.652
HCl
203.8–320.3
12.11
11.791
4NH2
320.3–400.00
17.22
16.952
C6H3–NH
400–523.40
14.19
13.778
C6H3
Remaining weight (%) above 600
46.17
47.62
—Figure 14
The thermal gravimetric analysis (TGA) for (POPDA).


## 3.5.7. The X-Ray Diffraction Analysis and Transmission Electron Microscope

The X-Ray diffraction patterns of the prepared polymer are represented in Figure15. The figure shows that the prepared poly o-phenylenediamine is completely amorphous.Figure 15
X-ray poly-o-phenylenediamine (POPDA).Morphology of poly o-phenylenediamine was characterized by transmission electron microscope. Figure16 shows TEM image of poly o-phenylenediamine which nearly spherical or ellipsoidal particles with approximate diameter 60–120 nm either separated or linked with each other.Figure 16
The transmission electron microscope of POPDA.


## 3.6.  ac  Conductivity (σ
a
c)

Figure17 represent the variation in ac conductivity (σ
ac) for (POPDA) as a function of frequency and temperature. It is observed that the value of ac conductivity increases with the increase of frequency. This behavior is in good agreement with the random free energy model proposed by Dyre [36]. According to this model, conductance increases as a function of frequency in many solids, including polymers, which can be explained on the basis of any hopping model. The rise in conductivity upon increasing the frequency and temperature is common for disordered conducting polymer. As can be seen, each curve displays a conductivity dispersion, which is strongly dependent on frequency and shows weaker temperature dependant.Figure 17
ac conductivity versus angular frequency for poly-o-phenylenediamine (POPDA) with frequency at different temperatures.The recorded conductivity value at room temperature of POPDA was found 0.0352 S/cm which is higher than conductivity of polyaniline-polyvinyl alcohol blends 10.5 × 10−5 S cm−1 [37] and ac conductivity of HCl doped polyaniline synthesized by the interfacial polymerization technique 6.2 × 10−5 S cm−1 [38]. Also, the ac conductivity of POPDA is higher than polyaniline loaded with 10% molybdenum trioxide composites 0.025 s/cm [39] but lower than the determined value of ac conductivity polyaniline prepared by K2Cr2O7 as oxidant 1.922 S cm−1. Such difference could be attributed to the different disorder of each composite, substituted function group, and different used dopant.In general, for amorphous conducting material, disordered systems, low mobility polymers, and even crystalline materials, the ac conductivity (σ
ac) as a function of frequency can obey a power law with frequency [40]. The ac conductivity (σ
ac) over a wide range of frequencies can be expressed as
(18)
σ
ac
(
ω
)
=
A
ω
s
,
where A is a complex constant and the index (s) is frequency exponent and ω is the angular frequency (ω
=
2
π
f).Figure17 shows the relation between Ln σ
ac and Ln ω at different temperatures. The value of (s) at each temperature has been calculated from the slope of ln σ(ω) versus ln (ω) plot. As shown in Figure 18 the calculated values of (s) for (POPDA) sample are less than unity. The microscopic conduction mechanisms of disordered systems are governed by two physical processes such as classical hopping or quantum mechanical tunneling of charge carries over the potential barrier separating two energetically favorable centers in a random distribution. The exact nature of charge transport is mainly obtained experimentally from the temperature variation of exponent (s) [41]. The temperature exponent(s) dependences for (POPDA) sample reveal that the frequency exponent(s) decreases with the increase of temperature. This behavior is only observed in the correlated barrier hopping model proposed by Elliott [42].Figure 18
Frequency exponent (s) versus temperature for poly-o-phenylenediamine (POPDA).


## 4. Conclusions

In the present work POPDA polymer incorporated with potassium dichromate and HCl has been successfully achieved. The optimum yield formation of POPDA is obtained at 0.3 M potassium dichromate 0.1 M of the monomer and 0.2 M hydrochloric acid concentrations. The initial and overall rate of polymerization reaction increases with increasing the oxidant, monomer, and HCl concentrations. The exponent of oxidant, monomer, and HCl was found to be 1.011, 1.045, and 0.954, respectively. The chrome is present between polymer chains as sandwich-bonded C6H6–C6H6 groups and the usual formation procedure hydrolyzes the reaction mixture with dilute acid which gives the cation (C6H6)2Cr3+. The ac conductivity increases with the increase of frequency and temperature. The microscopic conduction mechanism of charge which carries over the potential barrier in polymer backbone is classical hopping model.



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*Source: 520910-2014-06-12.xml*