# Catalytic Hydrodechlorination of Trichlorobenzenes with Pd(Phen)Cl2 as Catalyst Precursor

Authors: Guanlin Zhang; Hu Xu; Yuehui Fan; Yuhong Wang; Lirong Zhang; Guanzhong Lu
Journal: Journal of Nanomaterials
 (2015)

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## Abstract

We reported the catalytic hydrodechlorination (HDC) of trichlorobenzenes by an organometallic compound Pd(Phen)Cl2 as a catalyst precursor. The catalyst precursor was prepared by chemical coordination reaction and characterized by FTIR and 1H NMR techniques. The HDC performance of Pd(Phen)Cl2 as catalyst precursor was evaluated on 1,2,3-, 1,2,4-, and 1,3,5-trichlorobenzenes (TCBs). All TCBs could be converted to dechlorination products with high conversion. Products distribution was closely related with the substrate structures and C-Cl bond energies. A reasonable reaction mechanism was also proposed.


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## Body

## 1. Introduction

Aryl chlorides are considered the persistent toxic pollutants because the environment does not possess a comparatively assimilative ability [1]. The dechlorination of aryl chlorides is becoming a global issue [2]. With the ever increasing concerns for environmental protection and human health, the safe disposal of aryl chlorides has attracted much attention [2, 3]. Various methods like incineration and thermal oxidation do degrade aryl chlorides, but incomplete oxidation usually leads to the formation of more toxic species such as dioxins and chlorine [4]. In contrast, catalytic hydrodechlorination (HDC) may become a promising treatment for these chlorinated compounds by means of an environmentally friendly way [5]. Although HDC process does not usually cause the complete destruction of pollutants, it can result in the convenient transformation to less toxic compounds. Other advantages of HDC reflect in high conversion levels, conducting at low temperature and pressure, and so forth [6].Catalytic HDC can be usually effectively performed in both liquid and vapor phases using the supported noble metal (Pd [2, 4, 6–8], Pt [9], and Ru [10]) or nonnoble metal (Ni [4, 11, 12] and Ni-Mo [11]) as catalysts, among which Pd-based catalysts are considered the most suitable for liquid phase HDC since it can selectively replace the chlorine element of substrate with hydrogen [7]. On the other hand, organometallic compounds are frequently selected as catalysts for the activation of carbon-halogen bonds [13]. Thus, it is reasonable to infer the utility of metal complexes in the catalytic HDC reactions if only the proper hydrogen sources and reducing agents are provided. In fact, the organometallic complexes containing Rh [14], Fe [15], and Ni [16] have been reported in the HDC of aryl chlorides with the appropriate reagents such as hydrogen [14], hydrides [17], alcohols [18], and Grignard reagents [19] as reducing agents. Recently, our group reported a nickel complexes Ni[Phen]2(PF6)2 catalyzed HDC of aryl chlorides in the presence of zinc and water and results found that the Ni complexes could be recycled six times without the evident deactivation [20]. However, the reports on palladium complexes used in catalytic HDC of aryl chlorides are still rarely studied. Powell et al. reported PdCl2(PhCN)2 together with bidentate phosphine ligands as catalyst system for the HDC of aryl chlorides in the presence of sodium formate and N,N-dimethyl-acetamide [21].Herein, we reported the further exploration of HDC of aryl chlorides by organometallic complex Pd(Phen)Cl2 as catalyst precursor. Under the special conditions, Pd(Phen)Cl2 could smoothly promote the HDC reactions of several TCBs to occur and different dechlorination products were detected. Products distribution was closely related with the substrate structures and C-Cl bond energies. The possible reaction pathway was also discussed.


## 2. Experimental

### 2.1. General

PdCl2, phenanthroline, and other chemicals were purchased from Sinopharm Chemical Reagent Company. 1H NMR spectra were acquired on a Bruker Avance III spectrometer (500 MHz). Transmission electron microscopy (TEM) investigations were performed with an FEI Tecnai G2 20 microscope operated at 200 kV. Before the detection, the catalyst was dispersed in ethanol and reduced by NaBH4 for 10 min until the color of the catalyst became black. To confirm that the catalyst distributed uniformly, the sample should be put into the ultrasonic vibration meter for another 30 min. Catalytic HDC activity of Pd catalysts was evaluated by gas chromatograph (GC-9790, Fuli, MD) equipped with a flame ionization detector (FID), a PEG-20 M capillary column (30 m × 0.25 mm × 0.5 μm), and N2 as carrier gas. The initial oven temperature was set at 50°C for 3 min and was then raised with a gradient of 10°C/min until 200°C and held for 5 min. The temperature of the FID and injection was settled at 250°C. The FTIR analysis was performed on Nicolet 380 spectrometer with a KBr tablet.


### 2.2. The Preparation of Catalyst Precursor Pd(Phen)Cl2

Typically, a solution of PdCl2 (0.355 g, 2 mmol) in acetonitrile (50 mL) was heated to 70°C under stirring and maintained at this temperature for 2 h. During this process a clear solution appeared, which indicated the formation of Pd(CH3CN)2Cl2. Then the solvent was removed at reduced pressure and a pale yellow solid was obtained. The yellow solid was dissolved in 25 mL EtOH, to which a solution of 1,10-phenanthroline (0.396 g, 2 mmol) was dropwise added. With the addition of phenanthroline, the color of solution became gradually violent. Two hours of reaction resulted in the formation of a substantial white precipitate, which was collected by filtration and washed by EtOH (3 × 5 mL). The product was dried in vacuum drying oven at 50°C for 12 h to give the catalyst precursor Pd(Phen)Cl2 (0.580 g, 81.23%).


### 2.3. The Hydrodechlorination of Aryl Chlorides

Typically, hydrodechlorination reaction was carried out in a 150 mL three-necked, round-bottomed reactor equipped with a balloon for hydrogen supply (1 atm) at a temperature of 333 K. 0.25 mmol catalyst precursor was dispersed in 25 mL of MeOH by means of ultrasonation. To this dispersion the acid-binding agent triethylamine (15 mmol) and NaBH4 (0.02 g) were added. The reduction process was maintained for 1 h, after which the aryl chlorides substrates (5 mmol) were added and the HDC reaction started counting. The aliquots of reaction solution were taken every 30 min for GC analysis.


## 2.1. General

PdCl2, phenanthroline, and other chemicals were purchased from Sinopharm Chemical Reagent Company. 1H NMR spectra were acquired on a Bruker Avance III spectrometer (500 MHz). Transmission electron microscopy (TEM) investigations were performed with an FEI Tecnai G2 20 microscope operated at 200 kV. Before the detection, the catalyst was dispersed in ethanol and reduced by NaBH4 for 10 min until the color of the catalyst became black. To confirm that the catalyst distributed uniformly, the sample should be put into the ultrasonic vibration meter for another 30 min. Catalytic HDC activity of Pd catalysts was evaluated by gas chromatograph (GC-9790, Fuli, MD) equipped with a flame ionization detector (FID), a PEG-20 M capillary column (30 m × 0.25 mm × 0.5 μm), and N2 as carrier gas. The initial oven temperature was set at 50°C for 3 min and was then raised with a gradient of 10°C/min until 200°C and held for 5 min. The temperature of the FID and injection was settled at 250°C. The FTIR analysis was performed on Nicolet 380 spectrometer with a KBr tablet.


## 2.2. The Preparation of Catalyst Precursor Pd(Phen)Cl2

Typically, a solution of PdCl2 (0.355 g, 2 mmol) in acetonitrile (50 mL) was heated to 70°C under stirring and maintained at this temperature for 2 h. During this process a clear solution appeared, which indicated the formation of Pd(CH3CN)2Cl2. Then the solvent was removed at reduced pressure and a pale yellow solid was obtained. The yellow solid was dissolved in 25 mL EtOH, to which a solution of 1,10-phenanthroline (0.396 g, 2 mmol) was dropwise added. With the addition of phenanthroline, the color of solution became gradually violent. Two hours of reaction resulted in the formation of a substantial white precipitate, which was collected by filtration and washed by EtOH (3 × 5 mL). The product was dried in vacuum drying oven at 50°C for 12 h to give the catalyst precursor Pd(Phen)Cl2 (0.580 g, 81.23%).


## 2.3. The Hydrodechlorination of Aryl Chlorides

Typically, hydrodechlorination reaction was carried out in a 150 mL three-necked, round-bottomed reactor equipped with a balloon for hydrogen supply (1 atm) at a temperature of 333 K. 0.25 mmol catalyst precursor was dispersed in 25 mL of MeOH by means of ultrasonation. To this dispersion the acid-binding agent triethylamine (15 mmol) and NaBH4 (0.02 g) were added. The reduction process was maintained for 1 h, after which the aryl chlorides substrates (5 mmol) were added and the HDC reaction started counting. The aliquots of reaction solution were taken every 30 min for GC analysis.


## 3. Results and Discussion

### 3.1. The Characterization of Catalyst Precursor Pd(Phen)Cl2

Catalyst precursor Pd(Phen)Cl2 was firstly characterized by FTIR technique (Figure 1(a)). The bands at 1619, 1560, 1510, and 1421 cm−1 assigned to the skeletal vibration of Phen unit were shifted towards high frequency region (located at 1631, 1581, 1515, and 1425 cm−1) after complexation, which was ascribed to the sterohindrance effect. In addition, the signals of C-H bending vibration of aryl rings were shifted from 854, 735 cm−1 to 840, 707 cm−1 after complexation, respectively [22]. These data preliminarily implied the formation of Pd catalyst precursor. In order to provide the more definitive information for Pd(Phen)Cl2 complex, 1H NMR analysis was performed. Compared with free ligand Phen, the signals of protons on aryl rings of Pd(Phen)Cl2 were significantly shifted downfield by 0.24~0.48 ppm due to the coordination of N atoms of Phen to Pd2+ (Figure 1(b)), which definitely indicated the formation of catalyst precursor. Then, TEM was employed to examine the structure and Pd distribution of the materials. The catalyst sample was dispersed in ethanol by ultrasonic vibration, coordinated with phenanthroline ligand. We can see that, after the reduction with NaBH4, the particle was uniformly  distributed (Figure 1(c)). For estimation of particle size, at least more than 50 individual particles were counted for each catalyst (Figure 1(d)). From the figure of particle size distribution, we can see that most particles (more than 75 percentage points) distributed in the intervals 3 to 4 and the distribution of the eight intervals approached Gaussian distribution; it shows that the particle size was very small and it distributed uniformly.Figure 1
Comparison of FTIR spectra (a) and1H NMR spectra in [D6]DMSO (b) of free Phen ligand and Pd(Phen)Cl2. (Asterisks in 1H NMR spectra denote the residual solvents signals.) The TEM of the reduzate of Pd(phen)Cl2 (c). Particle size was calculated to analyse the distribution (d).
(a)
(b)
(c)
(d)


### 3.2. Effect of Temperature and Kinetic Analysis

In order to investigate the effect of reaction temperature, we performed the HDC reaction at 303, 313, 323, and 333 K, respectively, by the use of the synthesized catalyst precursor. Plots in Figure2 show the conversion of 1,3,5-TCB as a function of time under the different temperatures condition. Repeated experiments gave the similar results showing considerable reproducibility. For all cases, 1,3,5-TCB conversion always went up with time extension and reached the plateau at different reaction time (longer time for 303, 313 K and shorter time for 323, 333 K). Generally, increasing temperature is always beneficial for chemical reactions. The catalytic HDC of 1,3,5-TCB in the present study was in good accord with this rule. For the reaction temperature we studied, high temperature always provided the higher conversion than those obtained at lower temperature under the same reaction conditions. By plotting ln
⁡
(
c
0
/
c
) against reaction time (t), we could get a straight line showing a first order feature for the catalytic HDC of 1,3,5-TCB, which was similar to the previous result [23]. From the lines in Figure 2 and ln
⁡
(
c
0
/
c
)
=
k
t, we had calculated the values of rate constant k that were listed in Table 1. Higher reaction temperature was k that corresponded to a larger value implying the dependence of reaction rate on reaction temperature. According to Arrhenius equation, the overall apparent activation energy in the range 303–333 K was estimated to be 89.0 kJ/mol. The similar temperature effect was also observed in the HDC reactions of 1,2,3-TCB and 1,2,4-TCB and the corresponding activation energy values for these two reactions were estimated to be 49.5 and 39.8 kJ/mol, respectively.Table 1
Rate constants (k) values for HDC of 1,3,5-TCB at different reaction temperatures.
Temperature (K)
Reaction rate equation
k (h−1)
R
2
303
ln
⁡
(
c
0
/
c
) = 0.4497x  −  0.4158
0.4497
0.9937
313
ln
⁡
(
c
0
/
c
) = 0.5382x  −  0.4147
0.5382
0.9928
323
ln
⁡
(
c
0
/
c
) = 0.9283x  −  0.6100
0.9283
0.9904
333
ln
⁡
(
c
0
/
c
) = 1.6570x  −  1.4708
1.6570
0.9915Figure 2
Temporal 1,3,5-TCB conversion profiles at 303, 313, 323, and 333 K using Pd(Phen)Cl2 as catalyst precursor.


### 3.3. Catalytic Activity and Product Distribution

Figure3 shows the product distribution of 1,3,5-TCB obtained by catalyst precursor Pd(Phen)Cl2 at 323 K as a function of reaction time. From this figure, we can see that dichlorobenzene (DCB) as one of the main products appeared at the beginning of the reaction and its yield increased quickly in the first 2 h of reaction time (yield up to 56%). Other products including chlorobenzene (CB) and benzene were always present in the reaction mixture and their yields gradually increased in the first 3 h but their contents were relatively low (<17%). It was interesting that the content of CB in product mixture at 3 h of reaction time became almost constant (about 15%), while the amounts of 1,3-DCB and benzene went along the reverse directions. Benzene content was drifting higher and 1,3-DCB’s continued to decline. This significantly suggested a dynamic equilibrium during HDC reaction of 1,3,5-TCB. After full conversion of 1,3,5-TCB, the sustained decrease of 1,3-DCB content as well as the increase of benzene synergistically contributed to the relative constant CB amount. From the conversion of 1,3,5-TCB (Figure 2), the dechlorination mainly occurred at the first 4 h of reaction (for HDC reactions at 323 and 333 K) and the conversion extent of TCB was fairly large (up to 95%). In the subsequent stage, the reaction rate was sharply decreased and the conversion was almost near to the maximum (98% at 5 h of reaction). Combining the above results, the HDC of 1,3,5-TCB by Pd(Phen)Cl2 catalyst precursor could smoothly proceed in the first 3 h of reaction and the main dechlorination product was 1,3-DCB. The poor HDC performance at later stage (several chloro-containing products rather than the final product benzene) could be attributed to the deactivation of Pd catalyst. The deactivation of Pd catalysts generally originated from HCl formed during HDC reaction, which increased the acidity and caused the poisoning of catalysts.Figure 3
Product yields of 1,3,5-TCB as a function of time at 323 K using Pd(Phen)Cl2 as catalyst precursor.In order to make sure of the role of Pd(Phen)Cl2 as a catalyst precursor, we performed the control experiments under the same conditions using 1,3,5-TCB as substrate. The HDC reactions in the presence of free Phen ligand or PdCl2 salt instead of Pd(Phen)Cl2 did not undergo the dechlorination and no dechlorination products were detectable. However, when Phen and PdCl2 (in 1 : 1 mole ratio) were individually added at the same time, a measurable conversion (32% at 1.5 h of reaction time) was observed (Figure 4). Thus we deduced that Phen and PdCl2 partly took part in the coordination reaction to form Pd(Phen)Cl2 during the reduction process, which served as catalyst precursor to participate in the subsequent HDC reaction. Two factors could contribute to the moderate substrate conversion. One was that the amount of Pd(Phen)Cl2 formed in reduction stage or that really participated in HDC was not as much as the cases by the direct use of Pd(Phen)Cl2 as catalyst precursor. The other reason was the formed HCl in HDC, which poisoned the formed Pd(Phen)Cl2 and weakened the coordination ability of Phen by acid-base reaction to steadily produce complex Pd(Phen)Cl2. Therefore, after the maximum conversion 32% at 1.5 h appeared no further substrate conversion was observable. All these results inferred indirectly the role of Pd(Phen)Cl2 as catalyst precursor, which really participated in the HDC reaction of aryl chlorides.Figure 4
Temporal 1,3,5-TCB conversion profiles at 323 K in the coexistence of Phen and PdCl2 (1 : 1 mole ratio).Figure5(a) shows the overall HDC conversion profiles of 1,2,3-, 1,2,4-, and 1,3,5-TCB. No significant difference could be distinguished. As shown by 1,3,5-TCB, HDC of 1,2,3- and 1,2,4-TCB by Pd(Phen)Cl2 as catalyst precursor also gave the similar products yields tendency except for 1,2,4-TCB case with two DCB products (Figures 5(b) and 5(c)). In the initial reaction stage (2-3 h), DCB converted directly from the corresponding TCBs always served as the main products that existed in corresponding reaction mixtures and their contents were steadily going up with reaction time. After the almost full conversion of the original chlorinated substrates (ca. 2-3 h of reaction time), DCB primarily underwent the further dechlorination to afford CB or benzene due to the lack of the sustained production of DCB and thus the relative DCB amounts started to decline. In addition, CB appeared at the beginning of the reaction, but the yields passed through a maximum at 4 h of reaction time and then began to drop. As the final dechlorination product, benzene was always present in the reaction mixture but the contents were relatively low. Although the amount of benzene in these two cases always kept rising, the yields were in the range from 35% to 45% even extending to 12 h of reaction time. This phenomenon implied that the deactivation of catalyst was equally encountered in the HDC of 1,2,3- and 1,2,4-TCB.Figure 5
Temporal conversion profiles of 1,2,3-, 1,2,4-, and 1,3,5-TCB (a) and product yields of 1,2,3-TCB (b) and 1,2,4-TCB (c) as a function of time at 323 K using Pd(Phen)Cl2 as catalyst precursor.
(a)
(b)
(c)For the DCB products distribution in the HDC reactions of 1,2,3- and 1,2,4-TCB, the C-Cl bond energy as well as the steric hindrance effect of C-Cl bonds could give a reasonable explanation. It is well known that the insertion reaction between C-Cl bond and active catalyst center (Pd(0) in our case) forming oxidative adduct complex is the rate determining step for the dechlorination [23]. For polychloride, producing what type of oxidative adduct complex depends not only on the C-Cl bond energy, but also on the steric hindrance of C-Cl position. Generally, the C-Cl bond with the relatively low C-Cl bond energy (having the equivalent steric hindrance compared with other C-Cl bonds) or small steric hindrance (possessing the equivalent C-Cl bond energy compared with other C-Cl bonds) prefers to afford the corresponding oxidative adduct complex. For 1,2,3-TCB in our case, the bigger steric hindrance of C(2)-Cl bond together with the equivalent bond energies of three C-Cl bonds (the bond energies of C(1)-Cl, C(2)-Cl, and C(3)-Cl bonds were 325.6, 325.7, and 325.6 kJ/mol [24], resp.) was responsible for the sole 1,2-DCB production. In contrast, the bond energy of C-Cl bond played a dominant role for producing what type of DCB products in the case of 1,2,4-TCB. Although the steric hindrance on C(1)-Cl and C(2)-Cl bonds was slightly bigger than that on C(4)-Cl bond, much difference in bond energies between C(4)-Cl (336.8 kJ/mol), C(1)-Cl (331.6 kJ/mol), C(2)-Cl (329.4 kJ/mol) bonds caused the insertion reaction to occur in C(1)-Cl or C(2)-Cl bonds, which resulted in the production of 1,3- and 1,4-DCB rather than 1,2-DCB.In the HDC reactions of 1,2,3-, 1,2,4-, and 1,3,5-TCB, the corresponding DCB as the main products appeared from the beginning of the reaction and their yields passed through a maximum and then were gradually declined. This phenomenon implied that DCB would be a reaction intermediate. In order to determine whether DCBs were the intermediates, we studied the reactivity of 1,2-, 1,3-, and 1,4-DCB under the same conditions (Figure6(a)). The results indicated that three DCBs were smoothly dechlorinated and converted into the dechlorination products CB and benzene (Figure 6(b)), which verified the feature of DCBs as an intermediate. The difference in C-Cl bond energy and steric hindrance could account for the reactivity difference of 1,2-, 1,3-, and 1,4-DCB. 1,3-DCB with moderate steric hindrance and lowest C-Cl bond energy (376.1 kJ/mol) [25] demonstrated the best reactivity. The crowded surrounding of two neighbored C-Cl bonds together with the higher C-Cl bond energy (385.8 kJ/mol) [25] made 1,2-DCB exhibit the worst HDC performance. The most preferred spatial situation and the highest C-Cl bond energy (392.0 kJ/mol) [25] allowed 1,4-DCB to have the mediated reactivity.Figure 6
Temporal conversion profiles of 1,2-, 1,3-, and 1,4-DCB (a) and product yields of 1,3-DCB (b) as a function of time using Pd(Phen)Cl2 as catalyst precursor at 323 K. Only the product yields of 1,3-DCB were depicted as atypical since the similar results were observed in the cases of 1,2- and 1,4-DCB.
(a)
(b)


### 3.4. Possible Mechanism of HDC of Aryl Chlorides

In order to better understand the nature of HDC of aryl chlorides by the Pd catalyst precursor Pd(Phen)Cl2, we proposed a reasonable mechanism (Figure 7). For palladium-mediated dehalogenation reactions, the palladium (0) is widely considered as the catalytic active specie that promoted the formation of the oxidative adduct complex. In our case, the complex Pd(Phen)Cl2 was reduced by reducing agent NaBH4 to form the really active catalyst center Pd(0) (1). In the presence of hydrogen, active center1 was further converted into palladium-hybrid complex2. The control experiment using nitrogen instead of hydrogen could not give any dechlorination product, which suggested the real hydrogen source was coming from hydrogen gas rather than the solvent methanol. Then, complex2 reacted with aryl chloride to afford the oxidative adduct complex3 as mentioned above. With the aid of acid-binding reagent, complex3 was further transformed to compound4 by the release of HCl. Undergoing a beta hydride elimination compound4 afforded the expected hydrodechlorination product and regenerated the active Pd(0) species. The successive HDC of polychlorinated aryl gave various products. Generally, it is believed that the rate determining step for dechlorination is the oxidative addition of aryl chlorides and the electron-rich ligands are beneficial for this step. The relative high electron donating feature of Phen ligand partly accounted for the relatively fast conversion of chlorinated substrates.Figure 7
Proposed mechanism of HDC of aryl chlorides by Pd(Phen)Cl2 catalyst precursor.


## 3.1. The Characterization of Catalyst Precursor Pd(Phen)Cl2

Catalyst precursor Pd(Phen)Cl2 was firstly characterized by FTIR technique (Figure 1(a)). The bands at 1619, 1560, 1510, and 1421 cm−1 assigned to the skeletal vibration of Phen unit were shifted towards high frequency region (located at 1631, 1581, 1515, and 1425 cm−1) after complexation, which was ascribed to the sterohindrance effect. In addition, the signals of C-H bending vibration of aryl rings were shifted from 854, 735 cm−1 to 840, 707 cm−1 after complexation, respectively [22]. These data preliminarily implied the formation of Pd catalyst precursor. In order to provide the more definitive information for Pd(Phen)Cl2 complex, 1H NMR analysis was performed. Compared with free ligand Phen, the signals of protons on aryl rings of Pd(Phen)Cl2 were significantly shifted downfield by 0.24~0.48 ppm due to the coordination of N atoms of Phen to Pd2+ (Figure 1(b)), which definitely indicated the formation of catalyst precursor. Then, TEM was employed to examine the structure and Pd distribution of the materials. The catalyst sample was dispersed in ethanol by ultrasonic vibration, coordinated with phenanthroline ligand. We can see that, after the reduction with NaBH4, the particle was uniformly  distributed (Figure 1(c)). For estimation of particle size, at least more than 50 individual particles were counted for each catalyst (Figure 1(d)). From the figure of particle size distribution, we can see that most particles (more than 75 percentage points) distributed in the intervals 3 to 4 and the distribution of the eight intervals approached Gaussian distribution; it shows that the particle size was very small and it distributed uniformly.Figure 1
Comparison of FTIR spectra (a) and1H NMR spectra in [D6]DMSO (b) of free Phen ligand and Pd(Phen)Cl2. (Asterisks in 1H NMR spectra denote the residual solvents signals.) The TEM of the reduzate of Pd(phen)Cl2 (c). Particle size was calculated to analyse the distribution (d).
(a)
(b)
(c)
(d)


## 3.2. Effect of Temperature and Kinetic Analysis

In order to investigate the effect of reaction temperature, we performed the HDC reaction at 303, 313, 323, and 333 K, respectively, by the use of the synthesized catalyst precursor. Plots in Figure2 show the conversion of 1,3,5-TCB as a function of time under the different temperatures condition. Repeated experiments gave the similar results showing considerable reproducibility. For all cases, 1,3,5-TCB conversion always went up with time extension and reached the plateau at different reaction time (longer time for 303, 313 K and shorter time for 323, 333 K). Generally, increasing temperature is always beneficial for chemical reactions. The catalytic HDC of 1,3,5-TCB in the present study was in good accord with this rule. For the reaction temperature we studied, high temperature always provided the higher conversion than those obtained at lower temperature under the same reaction conditions. By plotting ln
⁡
(
c
0
/
c
) against reaction time (t), we could get a straight line showing a first order feature for the catalytic HDC of 1,3,5-TCB, which was similar to the previous result [23]. From the lines in Figure 2 and ln
⁡
(
c
0
/
c
)
=
k
t, we had calculated the values of rate constant k that were listed in Table 1. Higher reaction temperature was k that corresponded to a larger value implying the dependence of reaction rate on reaction temperature. According to Arrhenius equation, the overall apparent activation energy in the range 303–333 K was estimated to be 89.0 kJ/mol. The similar temperature effect was also observed in the HDC reactions of 1,2,3-TCB and 1,2,4-TCB and the corresponding activation energy values for these two reactions were estimated to be 49.5 and 39.8 kJ/mol, respectively.Table 1
Rate constants (k) values for HDC of 1,3,5-TCB at different reaction temperatures.
Temperature (K)
Reaction rate equation
k (h−1)
R
2
303
ln
⁡
(
c
0
/
c
) = 0.4497x  −  0.4158
0.4497
0.9937
313
ln
⁡
(
c
0
/
c
) = 0.5382x  −  0.4147
0.5382
0.9928
323
ln
⁡
(
c
0
/
c
) = 0.9283x  −  0.6100
0.9283
0.9904
333
ln
⁡
(
c
0
/
c
) = 1.6570x  −  1.4708
1.6570
0.9915Figure 2
Temporal 1,3,5-TCB conversion profiles at 303, 313, 323, and 333 K using Pd(Phen)Cl2 as catalyst precursor.


## 3.3. Catalytic Activity and Product Distribution

Figure3 shows the product distribution of 1,3,5-TCB obtained by catalyst precursor Pd(Phen)Cl2 at 323 K as a function of reaction time. From this figure, we can see that dichlorobenzene (DCB) as one of the main products appeared at the beginning of the reaction and its yield increased quickly in the first 2 h of reaction time (yield up to 56%). Other products including chlorobenzene (CB) and benzene were always present in the reaction mixture and their yields gradually increased in the first 3 h but their contents were relatively low (<17%). It was interesting that the content of CB in product mixture at 3 h of reaction time became almost constant (about 15%), while the amounts of 1,3-DCB and benzene went along the reverse directions. Benzene content was drifting higher and 1,3-DCB’s continued to decline. This significantly suggested a dynamic equilibrium during HDC reaction of 1,3,5-TCB. After full conversion of 1,3,5-TCB, the sustained decrease of 1,3-DCB content as well as the increase of benzene synergistically contributed to the relative constant CB amount. From the conversion of 1,3,5-TCB (Figure 2), the dechlorination mainly occurred at the first 4 h of reaction (for HDC reactions at 323 and 333 K) and the conversion extent of TCB was fairly large (up to 95%). In the subsequent stage, the reaction rate was sharply decreased and the conversion was almost near to the maximum (98% at 5 h of reaction). Combining the above results, the HDC of 1,3,5-TCB by Pd(Phen)Cl2 catalyst precursor could smoothly proceed in the first 3 h of reaction and the main dechlorination product was 1,3-DCB. The poor HDC performance at later stage (several chloro-containing products rather than the final product benzene) could be attributed to the deactivation of Pd catalyst. The deactivation of Pd catalysts generally originated from HCl formed during HDC reaction, which increased the acidity and caused the poisoning of catalysts.Figure 3
Product yields of 1,3,5-TCB as a function of time at 323 K using Pd(Phen)Cl2 as catalyst precursor.In order to make sure of the role of Pd(Phen)Cl2 as a catalyst precursor, we performed the control experiments under the same conditions using 1,3,5-TCB as substrate. The HDC reactions in the presence of free Phen ligand or PdCl2 salt instead of Pd(Phen)Cl2 did not undergo the dechlorination and no dechlorination products were detectable. However, when Phen and PdCl2 (in 1 : 1 mole ratio) were individually added at the same time, a measurable conversion (32% at 1.5 h of reaction time) was observed (Figure 4). Thus we deduced that Phen and PdCl2 partly took part in the coordination reaction to form Pd(Phen)Cl2 during the reduction process, which served as catalyst precursor to participate in the subsequent HDC reaction. Two factors could contribute to the moderate substrate conversion. One was that the amount of Pd(Phen)Cl2 formed in reduction stage or that really participated in HDC was not as much as the cases by the direct use of Pd(Phen)Cl2 as catalyst precursor. The other reason was the formed HCl in HDC, which poisoned the formed Pd(Phen)Cl2 and weakened the coordination ability of Phen by acid-base reaction to steadily produce complex Pd(Phen)Cl2. Therefore, after the maximum conversion 32% at 1.5 h appeared no further substrate conversion was observable. All these results inferred indirectly the role of Pd(Phen)Cl2 as catalyst precursor, which really participated in the HDC reaction of aryl chlorides.Figure 4
Temporal 1,3,5-TCB conversion profiles at 323 K in the coexistence of Phen and PdCl2 (1 : 1 mole ratio).Figure5(a) shows the overall HDC conversion profiles of 1,2,3-, 1,2,4-, and 1,3,5-TCB. No significant difference could be distinguished. As shown by 1,3,5-TCB, HDC of 1,2,3- and 1,2,4-TCB by Pd(Phen)Cl2 as catalyst precursor also gave the similar products yields tendency except for 1,2,4-TCB case with two DCB products (Figures 5(b) and 5(c)). In the initial reaction stage (2-3 h), DCB converted directly from the corresponding TCBs always served as the main products that existed in corresponding reaction mixtures and their contents were steadily going up with reaction time. After the almost full conversion of the original chlorinated substrates (ca. 2-3 h of reaction time), DCB primarily underwent the further dechlorination to afford CB or benzene due to the lack of the sustained production of DCB and thus the relative DCB amounts started to decline. In addition, CB appeared at the beginning of the reaction, but the yields passed through a maximum at 4 h of reaction time and then began to drop. As the final dechlorination product, benzene was always present in the reaction mixture but the contents were relatively low. Although the amount of benzene in these two cases always kept rising, the yields were in the range from 35% to 45% even extending to 12 h of reaction time. This phenomenon implied that the deactivation of catalyst was equally encountered in the HDC of 1,2,3- and 1,2,4-TCB.Figure 5
Temporal conversion profiles of 1,2,3-, 1,2,4-, and 1,3,5-TCB (a) and product yields of 1,2,3-TCB (b) and 1,2,4-TCB (c) as a function of time at 323 K using Pd(Phen)Cl2 as catalyst precursor.
(a)
(b)
(c)For the DCB products distribution in the HDC reactions of 1,2,3- and 1,2,4-TCB, the C-Cl bond energy as well as the steric hindrance effect of C-Cl bonds could give a reasonable explanation. It is well known that the insertion reaction between C-Cl bond and active catalyst center (Pd(0) in our case) forming oxidative adduct complex is the rate determining step for the dechlorination [23]. For polychloride, producing what type of oxidative adduct complex depends not only on the C-Cl bond energy, but also on the steric hindrance of C-Cl position. Generally, the C-Cl bond with the relatively low C-Cl bond energy (having the equivalent steric hindrance compared with other C-Cl bonds) or small steric hindrance (possessing the equivalent C-Cl bond energy compared with other C-Cl bonds) prefers to afford the corresponding oxidative adduct complex. For 1,2,3-TCB in our case, the bigger steric hindrance of C(2)-Cl bond together with the equivalent bond energies of three C-Cl bonds (the bond energies of C(1)-Cl, C(2)-Cl, and C(3)-Cl bonds were 325.6, 325.7, and 325.6 kJ/mol [24], resp.) was responsible for the sole 1,2-DCB production. In contrast, the bond energy of C-Cl bond played a dominant role for producing what type of DCB products in the case of 1,2,4-TCB. Although the steric hindrance on C(1)-Cl and C(2)-Cl bonds was slightly bigger than that on C(4)-Cl bond, much difference in bond energies between C(4)-Cl (336.8 kJ/mol), C(1)-Cl (331.6 kJ/mol), C(2)-Cl (329.4 kJ/mol) bonds caused the insertion reaction to occur in C(1)-Cl or C(2)-Cl bonds, which resulted in the production of 1,3- and 1,4-DCB rather than 1,2-DCB.In the HDC reactions of 1,2,3-, 1,2,4-, and 1,3,5-TCB, the corresponding DCB as the main products appeared from the beginning of the reaction and their yields passed through a maximum and then were gradually declined. This phenomenon implied that DCB would be a reaction intermediate. In order to determine whether DCBs were the intermediates, we studied the reactivity of 1,2-, 1,3-, and 1,4-DCB under the same conditions (Figure6(a)). The results indicated that three DCBs were smoothly dechlorinated and converted into the dechlorination products CB and benzene (Figure 6(b)), which verified the feature of DCBs as an intermediate. The difference in C-Cl bond energy and steric hindrance could account for the reactivity difference of 1,2-, 1,3-, and 1,4-DCB. 1,3-DCB with moderate steric hindrance and lowest C-Cl bond energy (376.1 kJ/mol) [25] demonstrated the best reactivity. The crowded surrounding of two neighbored C-Cl bonds together with the higher C-Cl bond energy (385.8 kJ/mol) [25] made 1,2-DCB exhibit the worst HDC performance. The most preferred spatial situation and the highest C-Cl bond energy (392.0 kJ/mol) [25] allowed 1,4-DCB to have the mediated reactivity.Figure 6
Temporal conversion profiles of 1,2-, 1,3-, and 1,4-DCB (a) and product yields of 1,3-DCB (b) as a function of time using Pd(Phen)Cl2 as catalyst precursor at 323 K. Only the product yields of 1,3-DCB were depicted as atypical since the similar results were observed in the cases of 1,2- and 1,4-DCB.
(a)
(b)


## 3.4. Possible Mechanism of HDC of Aryl Chlorides

In order to better understand the nature of HDC of aryl chlorides by the Pd catalyst precursor Pd(Phen)Cl2, we proposed a reasonable mechanism (Figure 7). For palladium-mediated dehalogenation reactions, the palladium (0) is widely considered as the catalytic active specie that promoted the formation of the oxidative adduct complex. In our case, the complex Pd(Phen)Cl2 was reduced by reducing agent NaBH4 to form the really active catalyst center Pd(0) (1). In the presence of hydrogen, active center1 was further converted into palladium-hybrid complex2. The control experiment using nitrogen instead of hydrogen could not give any dechlorination product, which suggested the real hydrogen source was coming from hydrogen gas rather than the solvent methanol. Then, complex2 reacted with aryl chloride to afford the oxidative adduct complex3 as mentioned above. With the aid of acid-binding reagent, complex3 was further transformed to compound4 by the release of HCl. Undergoing a beta hydride elimination compound4 afforded the expected hydrodechlorination product and regenerated the active Pd(0) species. The successive HDC of polychlorinated aryl gave various products. Generally, it is believed that the rate determining step for dechlorination is the oxidative addition of aryl chlorides and the electron-rich ligands are beneficial for this step. The relative high electron donating feature of Phen ligand partly accounted for the relatively fast conversion of chlorinated substrates.Figure 7
Proposed mechanism of HDC of aryl chlorides by Pd(Phen)Cl2 catalyst precursor.


## 4. Conclusions

In this work, we investigated the HDC performance of Pd(Phen)Cl2 as catalyst precursor using TCBs as substrates. All TCBs could be fully converted under the described conditions, but they could not be degraded completely to produce the final dechlorination product benzene, which was ascribed to the deactivation of catalyst. Products distribution was closely related to the substrate structures and C-Cl bond energies. The possible reaction pathway was also discussed.



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*Source: 912104-2015-08-27.xml*