# High-Active Metallic-Activated Carbon Catalysts for Selective Hydrogenation

Authors: Nicolás Carrara; Carolina Betti; Fernando Coloma-Pascual; María Cristina Almansa; Laura Gutierrez; Cristian Miranda; Mónica E. Quiroga; Cecilia R. Lederhos
Journal: International Journal of Chemical Engineering
 (2018)

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## Abstract

A series of low-loaded metallic-activated carbon catalysts were evaluated during the selective hydrogenation of a medium-chain alkyne under mild conditions. The catalysts and support were characterized by ICP, hydrogen chemisorption, Raman spectroscopy, temperature-programmed desorption (TPD), temperature-programmed reduction (TPR), X-ray diffraction (XRD), Fourier transform infrared spectroscopy (FTIR micro-ATR), transmission electronic microscopy (TEM), and X-ray photoelectronic spectroscopy (XPS). When studying the effect of the metallic phase, the catalysts were active and selective to the alkene synthesis. NiCl/C was the most active and selective catalytic system. Besides, when the precursor salt was evaluated, PdN/C was more active and selective than PdCl/C. Meanwhile, alkyne is present in the reaction media, and geometrical and electronic effects favor alkene desorption and so avoid their overhydrogenation to the alkane. Under mild conditions, nickel catalysts are considerably more active and selective than the Lindlar catalyst.


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## Body

## 1. Introduction

Olefins are of great academic and industrial interest. They are very important raw material for the synthesis of biologically active compounds, margarine, and lubricants, as well as in plastic industry [1]. Also, olefins present many applications in fine chemistry. The purification of olefins is a very important step in manufacturing polymers with a 0.35% content of impurities, as alkyne compounds, leading to a polymer with undesirable properties. There are several ways of purification of olefins stream, and the most common is solvent extraction, which is a nonecological friendly procedure. Another alternative for obtaining olefins is via the selective hydrogenation of alkynes. This catalytic process is the major challenge because they reduce the production costs and let obtaining good yields and high selectivities.Different noble metals as Pd, Pt, Ru, and Rh anchored on inorganic supports are highly active and selective for carbon-carbon multiple bond hydrogenations [2–7]. During the partial hydrogenation of alkynes to alkenes, or dienes to olefins, many authors found that supported palladium catalysts presented the highest catalytic activities [8, 9]. The most used catalyst for alkyne partial hydrogenation is the commercial Lindlar catalyst, that contains palladium poisoned with lead (Pd/CaCO3, 5 wt.% Pd modified with Pb(OAc)2) [10]. The cost of this noble metal has increased greatly in the last decade, and the world tendency is to develop cheaper catalysts by lowering the Pd content or by using cheaper metals.In previous papers [11, 12], we have studied the partial hydrogenation reaction of a medium-chain alkyne (1-heptyne) to obtain the corresponding olefin using monometallic catalysts using alumina and carbonaceous supports. In these papers, the influences of different supports, reaction, and reduction temperature and the metallic phase on the activity and the selectivity were evaluated.Activated carbonaceous surfaces have been studied during the last decades [13, 14] in different reactions showing that they are very complex. Carbonaceous supports are widely used because of their inertness, stability, high specific surface, low cost, and ability to easily recover the metallic phase after ending their useful life. Besides, during the synthesis of the catalysts, on the surface of activated carbon, different oxygenated and nitrogenized functional groups are found, and both can be easily modified when the material is physically or chemically pretreated [15, 16].The objectives of this work were to synthesize low-loaded Ru, Pd, and Ni catalysts using an activated carbon as support and evaluate their activities and selectivities during 1-heptyne selective hydrogenation reaction under mild conditions. The effect of the type of metal and the precursor salt on the activity and selectivity to the desired product (1-heptene) is also evaluated. The Lindlar catalyst was used as a reference.


## 2. Experimental

### 2.1. Catalyst Preparation

CNR-115 pelletized activated carbon provided by NORIT (SBET: 1503 m2·g−1, micropore volume: 0.738 mL·g−1, and total pore volume: 1.010 mL·g−1) was used as a support. Chloride acidic solutions of Ru, Pd, and Ni (purity >99.98%) at pH = 1 with HCl were used to prepare PdCl/C, RuCl/C, and NiCl/C catalysts by the incipient wetness technique. On the contrary, PdN/C was prepared from Pd(NO3)2 acidic solution (purity >99.98%) at pH = 1 with HNO3. Solutions have the necessary concentration to obtain 0.4 wt.% of each metal (M: Pd, Ni, and Ru) on the final catalyst. After impregnation, all samples were dried overnight at 373 K and reduced under a hydrogen stream, flow rate of 25 mL·min−1, at 393 K for 1 h before each catalytic evaluation.


### 2.2. Catalyst Characterization

Metal loadings of the catalysts were obtained by the ICP technique in PerkinElmer Optima 2100DV equipment, previous digesting the samples in aStart D Microwave Digestion system (Milestone).Dispersion values were obtained by hydrogen chemisorption in Micromeritics Accusorb 2100e equipment after reducing each sample at 393 K for 1 h under 5% v/v H2/Ar, and an atomic ratio H : M equal to 1 was assumed for all of the calculations as suggested by the other authors [17–19]. The particle diameter of the catalysts was calculated from the chemisorption results following the procedure reported by Paryjczac et al. [20, 21]. The adopted metallic surface area, σ value, was calculated from the average of the densities of the (100), (110), and (111) crystal planes [22, 23]; the values for Pd, Ru, and Ni were 1.27·1019, 1.63·1019, and 1.54·1019 atoms·m−2, respectively.Temperature-programmed desorption (TPD) allowed to determine the amount and type of oxygen-containing groups on the activated carbon surface. 10 mg of the sample were treated in a He stream at 100 mL·min−1 from 293 to 1273 K at 20 K·min−1. In the experiments, the effect of the thrust is corrected using a “white” curve. CO and CO2 desorptions were measured in a simultaneous TG-DTA (Mettler Toledo model TGA/SDTA851e/LF/1600) coupled to a quadrupole mass spectrometer (Pfeiffer Vacuum model Thermostar GSD301T).The FTIR micro-ATR technique was carried in a Shimadzu FTIR-8400 spectrophotometer which is based on the internal reflectance phenomenon. The FTIR micro-ATR technique is the most sensitive technique for surface analysis [24].The Raman spectra were recorded using a LabRam spectrometer (Horiba–Jobin–Yvon) coupled to an Olympus confocal microscope (a 100x objective lens was used for simultaneous illumination and collection) and equipped with a CCD detector cooled to about 200 K using the Peltier effect. The excitation wavelength was 532 nm in all cases (Spectra-Physics diode pump solid state laser). The laser power was set at 30 mW.X-ray diffraction (XRD) measurements of powdered samples were obtained using a Shimadzu XD-D1 instrument with CuKα radiation (λ = 1.5405 Å) in the 21 < 2θ < 49° at 0.25°·min−1 scan speed.The electronic state of superficial species and their atomic ratios were determined by X-ray photoelectron spectroscopy (XPS), following Pd and Ru 3d5/2, Ni and Cl 2p3/2, N, C, and O 1s peaks’ binding energy (BE) for catalysts and support. Measurements were acquired in VG-Microtech Multilab equipment, with MgKα (hν: 1253.6 eV) radiation and a pass energy of 50 eV. The analysis pressure during data acquisition was kept at 5.10−7 Pa. Samples were treated in situ in the presence of a H2 stream following the same pretreatment conditions for each catalyst. A careful deconvolution of the spectra was made, and the areas of the peaks were estimated by calculating the integral of each peak after subtracting a Shirley background and fitting the experimental peak to a combination of Lorentzian/Gaussian lines of 30–70% proportions. The reference binding energy (BE) was C 1s peak at 285.0 eV. Determinations of the superficial atomic ratios were made by comparing the areas under the peaks after background subtraction and corrections due to differences in escape depth and in photoionization cross sections [25].The reducibility of the surface species in all the catalysts was determined by temperature-programmed reduction (TPR) which was carried out in an Ohkura TP 2002 S instrument equipped with a thermal conductivity detector. Samples were pretreated at 373 K for 30 min under an argon stream, cooled up to room temperature under an argon flow, and then, the temperature was increased up to 1223 K at 10 K·min−1 in a 5% hydrogen/argon mixture stream.Transmission electronic microscopy (TEM) photographs were obtained using an electronic microscope JEOL JEM-2011 at 200 kV. The samples were reduced for 1 h at 393 K and dispersed in distilled water in order to obtain TEM images which are only used for comparative purposes.


### 2.3. Catalytic Evaluation

The reaction test accessed was 1-heptyne selective hydrogenation, carried out at 303 K, 150 kPa, and 800 rpm during 180 min. The possibility of external and internal diffusional limitations during the catalytic tests was discarded using a previously described procedure [26]. Experiments were performed in a stainless steel stirred tank reactor equipped with a magnetically driven stirrer with two blades in counterrotation. The inner wall of the reactor was completely coated with PTFE in order to neglect the catalytic action of the steel of the reactor found by other authors [27]. Samples of 0.75 g of the catalyst were used in a total volume of 75 mL of 5% (v/v) solution of 1-heptyne (Fluka, Cat. no. 51950) in toluene (Merck, Cat. no. TX0735-44).Blank tests were obtained using CNR and CNR-N activated carbons, and no conversion of 1-heptyne was observed. The commercialLindlar catalyst (Aldrich Cat. no. 20,573-7) was used as a reference, maintaining constant S : M (1-heptyne/metal molar ratio). Reactant and products were analyzed by gas chromatography using a flame ionization detector and a HP INNOWax polyethyleneglycol capillary column.


## 2.1. Catalyst Preparation

CNR-115 pelletized activated carbon provided by NORIT (SBET: 1503 m2·g−1, micropore volume: 0.738 mL·g−1, and total pore volume: 1.010 mL·g−1) was used as a support. Chloride acidic solutions of Ru, Pd, and Ni (purity >99.98%) at pH = 1 with HCl were used to prepare PdCl/C, RuCl/C, and NiCl/C catalysts by the incipient wetness technique. On the contrary, PdN/C was prepared from Pd(NO3)2 acidic solution (purity >99.98%) at pH = 1 with HNO3. Solutions have the necessary concentration to obtain 0.4 wt.% of each metal (M: Pd, Ni, and Ru) on the final catalyst. After impregnation, all samples were dried overnight at 373 K and reduced under a hydrogen stream, flow rate of 25 mL·min−1, at 393 K for 1 h before each catalytic evaluation.


## 2.2. Catalyst Characterization

Metal loadings of the catalysts were obtained by the ICP technique in PerkinElmer Optima 2100DV equipment, previous digesting the samples in aStart D Microwave Digestion system (Milestone).Dispersion values were obtained by hydrogen chemisorption in Micromeritics Accusorb 2100e equipment after reducing each sample at 393 K for 1 h under 5% v/v H2/Ar, and an atomic ratio H : M equal to 1 was assumed for all of the calculations as suggested by the other authors [17–19]. The particle diameter of the catalysts was calculated from the chemisorption results following the procedure reported by Paryjczac et al. [20, 21]. The adopted metallic surface area, σ value, was calculated from the average of the densities of the (100), (110), and (111) crystal planes [22, 23]; the values for Pd, Ru, and Ni were 1.27·1019, 1.63·1019, and 1.54·1019 atoms·m−2, respectively.Temperature-programmed desorption (TPD) allowed to determine the amount and type of oxygen-containing groups on the activated carbon surface. 10 mg of the sample were treated in a He stream at 100 mL·min−1 from 293 to 1273 K at 20 K·min−1. In the experiments, the effect of the thrust is corrected using a “white” curve. CO and CO2 desorptions were measured in a simultaneous TG-DTA (Mettler Toledo model TGA/SDTA851e/LF/1600) coupled to a quadrupole mass spectrometer (Pfeiffer Vacuum model Thermostar GSD301T).The FTIR micro-ATR technique was carried in a Shimadzu FTIR-8400 spectrophotometer which is based on the internal reflectance phenomenon. The FTIR micro-ATR technique is the most sensitive technique for surface analysis [24].The Raman spectra were recorded using a LabRam spectrometer (Horiba–Jobin–Yvon) coupled to an Olympus confocal microscope (a 100x objective lens was used for simultaneous illumination and collection) and equipped with a CCD detector cooled to about 200 K using the Peltier effect. The excitation wavelength was 532 nm in all cases (Spectra-Physics diode pump solid state laser). The laser power was set at 30 mW.X-ray diffraction (XRD) measurements of powdered samples were obtained using a Shimadzu XD-D1 instrument with CuKα radiation (λ = 1.5405 Å) in the 21 < 2θ < 49° at 0.25°·min−1 scan speed.The electronic state of superficial species and their atomic ratios were determined by X-ray photoelectron spectroscopy (XPS), following Pd and Ru 3d5/2, Ni and Cl 2p3/2, N, C, and O 1s peaks’ binding energy (BE) for catalysts and support. Measurements were acquired in VG-Microtech Multilab equipment, with MgKα (hν: 1253.6 eV) radiation and a pass energy of 50 eV. The analysis pressure during data acquisition was kept at 5.10−7 Pa. Samples were treated in situ in the presence of a H2 stream following the same pretreatment conditions for each catalyst. A careful deconvolution of the spectra was made, and the areas of the peaks were estimated by calculating the integral of each peak after subtracting a Shirley background and fitting the experimental peak to a combination of Lorentzian/Gaussian lines of 30–70% proportions. The reference binding energy (BE) was C 1s peak at 285.0 eV. Determinations of the superficial atomic ratios were made by comparing the areas under the peaks after background subtraction and corrections due to differences in escape depth and in photoionization cross sections [25].The reducibility of the surface species in all the catalysts was determined by temperature-programmed reduction (TPR) which was carried out in an Ohkura TP 2002 S instrument equipped with a thermal conductivity detector. Samples were pretreated at 373 K for 30 min under an argon stream, cooled up to room temperature under an argon flow, and then, the temperature was increased up to 1223 K at 10 K·min−1 in a 5% hydrogen/argon mixture stream.Transmission electronic microscopy (TEM) photographs were obtained using an electronic microscope JEOL JEM-2011 at 200 kV. The samples were reduced for 1 h at 393 K and dispersed in distilled water in order to obtain TEM images which are only used for comparative purposes.


## 2.3. Catalytic Evaluation

The reaction test accessed was 1-heptyne selective hydrogenation, carried out at 303 K, 150 kPa, and 800 rpm during 180 min. The possibility of external and internal diffusional limitations during the catalytic tests was discarded using a previously described procedure [26]. Experiments were performed in a stainless steel stirred tank reactor equipped with a magnetically driven stirrer with two blades in counterrotation. The inner wall of the reactor was completely coated with PTFE in order to neglect the catalytic action of the steel of the reactor found by other authors [27]. Samples of 0.75 g of the catalyst were used in a total volume of 75 mL of 5% (v/v) solution of 1-heptyne (Fluka, Cat. no. 51950) in toluene (Merck, Cat. no. TX0735-44).Blank tests were obtained using CNR and CNR-N activated carbons, and no conversion of 1-heptyne was observed. The commercialLindlar catalyst (Aldrich Cat. no. 20,573-7) was used as a reference, maintaining constant S : M (1-heptyne/metal molar ratio). Reactant and products were analyzed by gas chromatography using a flame ionization detector and a HP INNOWax polyethyleneglycol capillary column.


## 3. Results and Discussion

### 3.1. Catalysts and Support Characterization

A way to know the number and nature of oxygen functional groups present on the carbon surface is by the temperature-programmed desorption (TPD) technique. It is well known [15, 16] that the treatment of the catalysts with a strong oxidant acid, such as nitric acid, modifies the oxygen amount and the kind of superficial groups in the carbon surface. For this purpose, a sample of the carbon support (CNR) was treated with HNO3 (CNR-N), and both were analyzed and compared by TPD. This allows studying the effect of nitric acid, which was used during the catalyst preparation step, on the CNR surface.In Figures1(a) and 1(b), the concentration profiles of CO and CO2 as a function of temperature, respectively, for CNR and CNR-N samples are shown. During the TPD experiments, the samples analyzed showed highly different behaviors, mainly during the CO2 desorption (Figure 1(b)) due to the decomposition of carboxyl and lactone groups. It can be seen that these surface groups had highly increased in the carbon sample treated with the oxidizing acid (HNO3).Figure 1
TPD spectra: (a) CO and (b) CO2 desorption profiles as a function of temperature for CNR and CNR-N samples.
(a)
(b)The quantitative results from TPD-MS analysis for the CNR and CNR-N supports are presented in Table1. The amount of surface oxygen groups of carbonaceous supports, estimated by CO, CO2, and O2 evolved in TPD experiments (Table 1), shows that the oxidizing treatment with HNO3 produces a large amount of surface oxygenated complexes, with 175% higher amount of carboxylic-type groups that decompose to give CO2 under the heat treatment [28]. This enhancement is also observed in the TPD profile in Figure 1(b).Table 1
Quantitative results of the TPD-MS analysis for carbon samples.
CO (µmol/g)
CO2 (µmol/g)
O (µmol/g)
CNR
2349
1394
5136
CNR-N
2621
2442
7504The FTIR micro-ART spectra are given in Figure2(a) for the supports CNR and CNR-N and in Figure 2(b), for the catalysts PdCl/C, PdN/C, NiCl/C, and RuCl/C. On the one hand, in Figure 2(a), it can be seen that the CNR carbonaceous support did not show new bands in the support treated with nitric acid (CNR-N). The bands at 665, 1583, and 3346 cm−1 correspond to ring deformation and C-O stretching vibrations in phenolic groups, but in general, the lack of parallel behavior between the growth of bands in 1000–1350 cm−1 is attributed to primarily C-O stretching of ether groups, possibly furans, to C-OH species [29], and to O-H or C-N stretching [30].Figure 2
FTIR micro-ART spectra for the supports (a) CNR and CNR-N and for the catalysts (b) PdCl/C, PdN/C, NiCl/C, and RuCl/C.
(a)
(b)On the other hand, in Figure2(b), for all the catalysts, PdN/C, PdCl/C, NiCl/C, and RuCl/C, the following peaks can be seen in general: (i) a broad band centered at 3444 cm−1 which was assigned mainly to O-H stretching, associated with the water absorbed on the surface of the material and hydroxylated groups; (ii) a NH2 stretching band located at 3600–3100 cm−1; and (iii) a C-H stretching band between 3000 and 2800 cm−1 [31]. In the 1350–1000 cm−1 range, the growth of bands for the PdN/C catalyst can be attributed mainly to C-N stretching [32] because of the support treatment with nitric acid during the synthesis of the catalyst.Figure3 shows the Raman spectra of the catalysts and carbon support in the range of 100–2000 cm−1. The profile of all catalysts analyzed is very similar to the CNR support spectrum. Two intense bands at ca. 1600 cm−1 and ca. 1350 cm−1 are observed, which are the typical signals of the graphite spectrum. The first signal is known as the G band associated with the graphitic order, and the second is named the D band and is attributed to structural defects [32].Figure 3
Raman spectroscopy for PdN/C, PdCl/C, and NiCl/C catalysts.PdN/C, PdCl/C, RuCl/C, NiCl/C, and the CNR support diffractograms are shown in Figure4. In this figure, it can be seen that there are no defined signals for the metallic samples or to the support, which could indicate the absence of the crystalline phases in all samples, or the crystals were very small (<100 Å). The absence of the crystalline phase is a consequence of the low-metallic loadings of the samples, 0.4 wt.%, low below the detection limit of the XRD equipment.Figure 4
DRX diffractograms of PdN/C, PdCl/C, RuCl/C, and NiCl/C catalysts treated in H2 at 393 K and the CNR support.Figure5 shows temperature-programmed reduction profiles of PdN/C, PdCl/C, RuCl/C, and NiCl/C catalysts. In this figure, the TPR profile of CNR carbon is also presented for a comparative way. As can be seen in Figure 5, the support and the catalysts profiles present a broad peak with a maximum at ca. 870 K, which can be attributed to the gasification of the carbonaceous support, the decomposition of chloride or nitrogen species, the reduction of superficial oxygenated groups of the support, or due to the possible presence of impurities (5-6%), producing CH4, CO, and/or CO2 [33–35]. de Miguel et al. [36], for carbonaceous supports, found these types of consumption at very high temperatures, between 923 and 1223 K, associated with decomposition of superficial oxygenated groups (C[O]) that can liberate CO in the presence of a reductive stream. In Figure 5, it can be seen that, at temperatures higher than 700 K, all metallic catalysts samples present very similar profile due to the reduction of surface groups of the carbonaceous support.Figure 5
TPR profiles of PdN/C, PdCl/C, RuCl/C, and NiCl/C catalysts and the CNR support.The palladium catalysts (PdN/C and PdCl/C) presented at high temperatures a much wider peak profiles with respect to the support, as can be observed in Figure5, with a maximum at ca. 875 K. No peaks are present at low reduction temperature, and this is because the palladium can be reduced by carbon at low temperature, even at room temperature as was observed by other authors [37]. In Figure 5, it can be seen that the peak above 700 K is more intense for PdN/C and NiCl/C catalysts. Besides, the TPR profile of the NiCl/C sample shows a small peak at 610 K attributed to the reduction of NiO to Ni° species, which indicates a weak metal-support interaction [38–40]. Lastly, for the ruthenium catalyst (RuCl/C), the TPR profile presents a signal with maximum at 610 K, related to the reduction of ruthenium, Ru3+ → Ru2+ → Ru°, assigned to the reduction of the ruthenium chloride species [16, 35].As an early conclusion, at the reduction temperature used during the preparation step of the catalysts (393 K, marked in Figure5), the palladium metals on PdCl/C and PdN/C could be mostly as Pd° species on the catalyst surface; meanwhile, nickel and ruthenium are present as Ni2+ and Ru3+ species.Table2 summarizes all the catalysts under study, the results of ICP, dispersion and particle diameter by hydrogen chemisorption, XPS, initial reaction rate, and activity TOF values. For a comparative study, the Lindlar catalyst was also included in Table 2. The metal loadings of the synthetized catalysts are ca. 0.4 wt.% in the final catalyst, while a concentration of 5 wt.% of Pd was corroborated for commercial Lindlar. Dispersion values show the following order PdCl/C > PdN/C > RuCl/C, while NiCl/C and Lindlar catalysts present extremely low D values (lower than 5%). Higher dispersions are favored by low loadings of the metallic precursor and by low pretreatment conditions used during the preparation of the catalysts [41]; besides, high surface areas and large pore volume of the carbonaceous materials usually favor very high dispersion of an active phase. All these factors avoid the sintering of the active phase. In our case, the highest dispersion of the Pd catalyst prepared from chlorinated precursor can be due to the presence of complex oxychlorinated species formed during the pretreatment step. The presence of these species improves the metal dispersion due to the greater interaction between these oxychlorinated species and the support as compared to the weaker one displayed by palladium(II) oxide (PdO) [42–44]. Furthermore, the PdN/C catalyst presents a dispersion of ca. 50% attributed to the high concentration of carboxylic-type groups on the surface, as observed by TPD-MS analysis, that exert an electronic and geometrical effect over the nitrate precursor used. On the contrary, due to the high surface area, ruthenium particles would also be highly dispersed on these carbon supports [45]. However, there is no simple relationship between the value of the surface area of the activated carbon and the metal dispersion of the catalysts supported on activated carbon [46]. Some authors [47–51] reported the inhibition and drawbacks due to the use of RuCl3 as a precursor salt because the chloride from this salt is a poison for CO and H2 chemisorptions and may be partitioned between the metal and the support. In our case, the high degree of sintering of the ruthenium metal particles could be due to the fact that, during the pretreatment process, no oxychlorinated species interacting with the support are formed, as noted earlier while studying ruthenium catalysts of different metal contents over the alumina support [12, 21]. The low dispersion of nickel is a characteristic when this metal is used to prepare inorganic or carbonaceous catalysts [52, 53].Table 2
Metal loading, dispersion, particle diameter, XPS, initial reaction rate, and activity (TOF) results for the catalysts.
Catalysts
Metal loading (%)
D (%)
d (nm)
XPS
r° (mol·gM−1·s−1)
TOF (s−1)
M 3d5/2 BE (eV)
Cl/M (at/at)
PdN/C
0.39
48
2.4
335.2
—
0.077
17.0
PdCl/C
0.42
62
1.9
335.2
1.56
0.050
8.6
RuCl/C
0.41
20
5.3
282.1
2.96
0.056
28.5
NiCl/C
0.41
4
25.2
857.3
2.05
0.026
38.9
Lindlar
5
2.5
46.4
337.2
—
0.003
13.5From the H2 chemisorption results, the metal particle size (d) was determined on assuming a spherical particle in accordance with Badano et al. [21]. The particle size order is PdCl/C < PdN/C < RuCl/C ≪ NiCl/C ≪ Lindlar. The smallest particle size of PdCl/C catalysts is due to the higher surface interaction between Pdδ+OxCly and oxygenated groups of the carbonaceous support, as observed earlier when alumina was used as a support [21]. The higher particle size of NiCl/C could be related with the higher structural defects observed by the Raman spectra in Figure 3.Figure6 shows the XPS spectra of the Pd 3d5/2 band for PdN/C and PdCl/C, Ru 3d5/2 band for RuCl/C, and Ni 2p3/2 band for the NiCl/C catalyst. Besides, the XPS spectra of the catalysts prepared from chlorine precursors (PdCl/C, RuCl/C, and NiCl/C) show a Cl 2p3/2 peak at ca. 199.4 eV that corresponds to surface chloride species [54] that were not completely eliminated after reduction because of the high adsorption capacity of the carbonaceous material used. The maximum binding energy (BE) of Pd and Ru 3d5/2, Ni 2p3/2 peaks, and Cl/M atomic ratios are also listed in Table 2.Figure 6
XPS spectra of BE Pd 3d for (a) PdN/C, (b) PdCl/C, (c) RuCl/C, and (d) NiCl/C catalysts treated in H2 at 393 K.
(a)
(b)
(c)
(d)XPS results in Figure6 show that both palladium catalysts present a Pd 3d5/2 peak at 335.2 eV, which can be attributed to Pdδ+ (δ ≈ 0) [16, 54]. Figure 6 also shows the spectra of palladium catalysts and the 3d3/2 peak doublet shifted 5.2 eV with respect to the 3d5/2 peak. No nitrogen was detected by XPS on the Pd catalyst prepared from the nitrate precursor. On the contrary, for the PdCl/C sample, the Cl/Pd atomic ratio was 1.56, confirming that chloride is present even after the reduction treatment. This could be attributed to the high absorption capacity of the carbon support. The chlorine content does not affect the palladium surface as it is totally reduced on the PdCl/C catalyst.In the case of ruthenium, the BE reference is difficult because the Ru 3d peaks appear at the same region than the C 1s peak. There are also discrepancies in the BE reported in the literature for ruthenium compounds. The Ru 3d5/2 signal for the RuCl/C catalyst was observed at 282.1 eV corresponding to ruthenium electrodeficient species as RuCl3 [54]. For this catalyst, after the temperature pretreatments, the superficial atomic ratio Cl/Ru was 2.96.According to the bibliography [54, 55], the Ni 2p3/2 signal appears at 852.5 eV for Ni° species. For the NiCl/C catalyst, the two signals were observed in the spectrum of Figure 6 at 857.3 and 862.7 eV. The first peak could be assigned to the electrodeficient nickel species (Nin+, with n → 2), probably corresponding to nickel interacting with the support [54–56], while the second peak corresponds to the characteristic shake-up satellite structure of Ni (II) [55, 57, 58]. This catalyst also presents a high Cl/Ni atomic ratio (2.05) as a consequence of the adsorption capacity or the carbonaceous support.For the Lindlar catalyst, in Table2, the main peaks at 335.2 eV (69%, at/at) and 336.9 eV (31%, at/at) are also registered, assigned to Pdδ+ and electrodeficient Pdn+ species (with δ → 0 and n → 2), respectively [53]. On the contrary, on the Lindlar catalyst, also two peaks of the Pb 4f7/2 spectrum at 136.8 eV (20%, at/at) and 138.6 (80%, at/at) were attributed to Pb and Pb(OAc)2, respectively [53].In Figure7, TEM micrographs of the carbonaceous catalysts are shown. The metal particle size for the PdCl/C catalyst is between 1 and 4 nm, presenting a high concentration of 2 nm Pd particles on the carbon surface. For PdN/C, the main palladium particle size is between 4 and 8 nm. The particle sizes of Ru on RuCl/C are mainly between 1 and 5 nm, although several bigger particles were observed on the micrographs. Besides, the NiCl/C catalyst presented the highest particle sizes between 25 and 40 nm.Figure 7
TEM Images for (a) PdN/C, (b) PdCl/C, (c) RuCl/C, and (d) NiCl/C catalysts.
(a)
(b)
(c)
(d)


### 3.2. Catalytic Tests

The catalytic performance during the selective hydrogenation of 1-heptyne for PdN/C, PdCl/C, RuCl/C, and NiCl/C catalysts is shown in Figure8. 1-heptyne total conversion (%) and selectivity to 1-heptene (%) as a function of time (min) were plotted in this figure for all the studied catalysts. All the catalysts were active during the hydrogenation of 1-heptyne and presented high selectivity to 1-heptene, the desired product.Figure 8
Total conversion (a) and selectivity to 1-heptene (b) versus time (min) for PdN/C, PdCl/C, RuCl/C, and NiCl/C catalysts pretreated in H2 at 393 K.
(a)
(b)Besides, in Figure9, 1-heptyne total conversion (%) and selectivity to 1-heptene (%) as a function of time (min) for the commercial Lindlar catalyst used as a reference is shown.Figure 9
Total conversion () and selectivity to 1-heptene () versus time (min) for the Lindlar catalyst (reproduced from Lederhos et al. [52], under the Creative Commons Attribution License/public domain).According to Figures8 and 9 the order of selectivities to the corresponding alkene was:(1)PdCl/C<PdN/C≅RuCl/C<Lindlar<NiCl/CIn order to compare the performance of the catalytic systems, the initial reaction rate of hydrogenation of 1-heptyne (rA0) was estimated for all the catalysts using the following formula:(2)rA0=V⋅CA0WM⋅∂XA∂tt=0,where rA0 is the initial 1-heptyne reaction rate (mol·gM−1·s−1), ∂XA/∂tt=0 is the tangent value of the 1-heptyne total conversion versus time curve at t=0, CA0 is the initial concentration of 1-heptyne (mol·L−1), WM is the mass of the metal (Pd, Ru, or Ni) in the catalyst (g), V is the reaction volume (L), and t is the reaction time (s).From these initial reaction rates of 1-heptyne hydrogenation, TOF values were calculated for all the catalysts and are summarized in Table2. For hydrogenation reactions, TOF values between 10−2 and 102 indicate a structure-insensitive system, not influenced by particle size [59, 60], so the differences in activities and selectivities between the catalysts may be associated with geometrical and/or geometrical effects. The order of activities of low-loaded catalysts is(3)PdCl/C<Lindlar<PdN/C<RuCl/C<NiCl/CThe effect of the precursor salt was studied by comparing PdCl/C and PdN/C catalysts. The results obtained for these catalysts show differences in both activity and selectivity. For the catalyst synthetized from palladium nitrate as the precursor salt, the obtained TOF was 17 s−1 versus the activity of palladium chloride precursor salt 8.6 s−1. That is, each active site of the PdN/C catalyst is almost two times more active than that of PdCl/C. As observed by XPS and RTP, both catalysts have Pdδ+ (with δ ≅ 0) as the active site, so no electronic effects are generated by the metallic phase; besides as observed by Raman, quite higher structural effects were found on PdN/C than on the PdCl/C sample. When comparing the catalytic behavior of the different Pd precursors, higher selectivities to 1-heptene were obtained when palladium nitrate was used, ca. 86% at 180 min, while for PdCl/C selectivities, ca. 70% was obtained.In Figure10, the main superficial groups present on carbonaceous supports are summarized. Between them carboxylic groups by heterolytic rupture of the O-H bond, could favor the adsorption of the cationic metallic precursors Mn+. In our case, the higher distribution of carboxylic and lactone groups on the surface of PdN/C could favor the adsorption of Pd2+, and its reduction to Pd° (as detected by XPS and TPR) during the pretreatment step: for 1 h at 393 K under a hydrogen stream. Also, the high concentration of carboxylic groups favors the high dispersion of the active sites and the small particle sizes. So, the observed differences in activity between PdN/C and PdCl/C could be originated, at least in part, by geometrical effects due to higher structural defects (as noted in D-bands on the Raman spectra) and electronic effects originated by the high concentration of carboxylic superficial groups on PdN/C (the favorable effect) and high remnants of chloride on PdCl/C catalysts (the negative effect). Besides, differences in selectivity between the PdN/C and PdCl/C catalysts could be caused on the one hand to the electronic and geometrical effects that favors the formation of 1-heptene and on the other hand to higher amount of carbonaceous superficial groups that favors the desorption of the alkene, avoiding its overhydrogenation, while alkyne is present in the reaction media.Figure 10
Schematic representation of the main superficial groups found on a carbonaceous supports.When analyzing the effect of the metal type used to synthesize the carbonaceous catalysts, PdCl/C, RuCl/C, and NiCl/C, the highest activity and selectivity were achieved when the supported metal is nickel, a very low cost precursor salt. The high activity and selectivity of NiCl/C could be related to electronic or geometrical effects of active sites, which would control the dissociative adsorption of hydrogen being this the controlling step [61], and/or to the aromatic superficial groups of the support that would preferentially adsorb remaining 1-heptyne desorbing 1-heptene from the reaction media, so avoiding its total hydrogenation to the alkane.


## 3.1. Catalysts and Support Characterization

A way to know the number and nature of oxygen functional groups present on the carbon surface is by the temperature-programmed desorption (TPD) technique. It is well known [15, 16] that the treatment of the catalysts with a strong oxidant acid, such as nitric acid, modifies the oxygen amount and the kind of superficial groups in the carbon surface. For this purpose, a sample of the carbon support (CNR) was treated with HNO3 (CNR-N), and both were analyzed and compared by TPD. This allows studying the effect of nitric acid, which was used during the catalyst preparation step, on the CNR surface.In Figures1(a) and 1(b), the concentration profiles of CO and CO2 as a function of temperature, respectively, for CNR and CNR-N samples are shown. During the TPD experiments, the samples analyzed showed highly different behaviors, mainly during the CO2 desorption (Figure 1(b)) due to the decomposition of carboxyl and lactone groups. It can be seen that these surface groups had highly increased in the carbon sample treated with the oxidizing acid (HNO3).Figure 1
TPD spectra: (a) CO and (b) CO2 desorption profiles as a function of temperature for CNR and CNR-N samples.
(a)
(b)The quantitative results from TPD-MS analysis for the CNR and CNR-N supports are presented in Table1. The amount of surface oxygen groups of carbonaceous supports, estimated by CO, CO2, and O2 evolved in TPD experiments (Table 1), shows that the oxidizing treatment with HNO3 produces a large amount of surface oxygenated complexes, with 175% higher amount of carboxylic-type groups that decompose to give CO2 under the heat treatment [28]. This enhancement is also observed in the TPD profile in Figure 1(b).Table 1
Quantitative results of the TPD-MS analysis for carbon samples.
CO (µmol/g)
CO2 (µmol/g)
O (µmol/g)
CNR
2349
1394
5136
CNR-N
2621
2442
7504The FTIR micro-ART spectra are given in Figure2(a) for the supports CNR and CNR-N and in Figure 2(b), for the catalysts PdCl/C, PdN/C, NiCl/C, and RuCl/C. On the one hand, in Figure 2(a), it can be seen that the CNR carbonaceous support did not show new bands in the support treated with nitric acid (CNR-N). The bands at 665, 1583, and 3346 cm−1 correspond to ring deformation and C-O stretching vibrations in phenolic groups, but in general, the lack of parallel behavior between the growth of bands in 1000–1350 cm−1 is attributed to primarily C-O stretching of ether groups, possibly furans, to C-OH species [29], and to O-H or C-N stretching [30].Figure 2
FTIR micro-ART spectra for the supports (a) CNR and CNR-N and for the catalysts (b) PdCl/C, PdN/C, NiCl/C, and RuCl/C.
(a)
(b)On the other hand, in Figure2(b), for all the catalysts, PdN/C, PdCl/C, NiCl/C, and RuCl/C, the following peaks can be seen in general: (i) a broad band centered at 3444 cm−1 which was assigned mainly to O-H stretching, associated with the water absorbed on the surface of the material and hydroxylated groups; (ii) a NH2 stretching band located at 3600–3100 cm−1; and (iii) a C-H stretching band between 3000 and 2800 cm−1 [31]. In the 1350–1000 cm−1 range, the growth of bands for the PdN/C catalyst can be attributed mainly to C-N stretching [32] because of the support treatment with nitric acid during the synthesis of the catalyst.Figure3 shows the Raman spectra of the catalysts and carbon support in the range of 100–2000 cm−1. The profile of all catalysts analyzed is very similar to the CNR support spectrum. Two intense bands at ca. 1600 cm−1 and ca. 1350 cm−1 are observed, which are the typical signals of the graphite spectrum. The first signal is known as the G band associated with the graphitic order, and the second is named the D band and is attributed to structural defects [32].Figure 3
Raman spectroscopy for PdN/C, PdCl/C, and NiCl/C catalysts.PdN/C, PdCl/C, RuCl/C, NiCl/C, and the CNR support diffractograms are shown in Figure4. In this figure, it can be seen that there are no defined signals for the metallic samples or to the support, which could indicate the absence of the crystalline phases in all samples, or the crystals were very small (<100 Å). The absence of the crystalline phase is a consequence of the low-metallic loadings of the samples, 0.4 wt.%, low below the detection limit of the XRD equipment.Figure 4
DRX diffractograms of PdN/C, PdCl/C, RuCl/C, and NiCl/C catalysts treated in H2 at 393 K and the CNR support.Figure5 shows temperature-programmed reduction profiles of PdN/C, PdCl/C, RuCl/C, and NiCl/C catalysts. In this figure, the TPR profile of CNR carbon is also presented for a comparative way. As can be seen in Figure 5, the support and the catalysts profiles present a broad peak with a maximum at ca. 870 K, which can be attributed to the gasification of the carbonaceous support, the decomposition of chloride or nitrogen species, the reduction of superficial oxygenated groups of the support, or due to the possible presence of impurities (5-6%), producing CH4, CO, and/or CO2 [33–35]. de Miguel et al. [36], for carbonaceous supports, found these types of consumption at very high temperatures, between 923 and 1223 K, associated with decomposition of superficial oxygenated groups (C[O]) that can liberate CO in the presence of a reductive stream. In Figure 5, it can be seen that, at temperatures higher than 700 K, all metallic catalysts samples present very similar profile due to the reduction of surface groups of the carbonaceous support.Figure 5
TPR profiles of PdN/C, PdCl/C, RuCl/C, and NiCl/C catalysts and the CNR support.The palladium catalysts (PdN/C and PdCl/C) presented at high temperatures a much wider peak profiles with respect to the support, as can be observed in Figure5, with a maximum at ca. 875 K. No peaks are present at low reduction temperature, and this is because the palladium can be reduced by carbon at low temperature, even at room temperature as was observed by other authors [37]. In Figure 5, it can be seen that the peak above 700 K is more intense for PdN/C and NiCl/C catalysts. Besides, the TPR profile of the NiCl/C sample shows a small peak at 610 K attributed to the reduction of NiO to Ni° species, which indicates a weak metal-support interaction [38–40]. Lastly, for the ruthenium catalyst (RuCl/C), the TPR profile presents a signal with maximum at 610 K, related to the reduction of ruthenium, Ru3+ → Ru2+ → Ru°, assigned to the reduction of the ruthenium chloride species [16, 35].As an early conclusion, at the reduction temperature used during the preparation step of the catalysts (393 K, marked in Figure5), the palladium metals on PdCl/C and PdN/C could be mostly as Pd° species on the catalyst surface; meanwhile, nickel and ruthenium are present as Ni2+ and Ru3+ species.Table2 summarizes all the catalysts under study, the results of ICP, dispersion and particle diameter by hydrogen chemisorption, XPS, initial reaction rate, and activity TOF values. For a comparative study, the Lindlar catalyst was also included in Table 2. The metal loadings of the synthetized catalysts are ca. 0.4 wt.% in the final catalyst, while a concentration of 5 wt.% of Pd was corroborated for commercial Lindlar. Dispersion values show the following order PdCl/C > PdN/C > RuCl/C, while NiCl/C and Lindlar catalysts present extremely low D values (lower than 5%). Higher dispersions are favored by low loadings of the metallic precursor and by low pretreatment conditions used during the preparation of the catalysts [41]; besides, high surface areas and large pore volume of the carbonaceous materials usually favor very high dispersion of an active phase. All these factors avoid the sintering of the active phase. In our case, the highest dispersion of the Pd catalyst prepared from chlorinated precursor can be due to the presence of complex oxychlorinated species formed during the pretreatment step. The presence of these species improves the metal dispersion due to the greater interaction between these oxychlorinated species and the support as compared to the weaker one displayed by palladium(II) oxide (PdO) [42–44]. Furthermore, the PdN/C catalyst presents a dispersion of ca. 50% attributed to the high concentration of carboxylic-type groups on the surface, as observed by TPD-MS analysis, that exert an electronic and geometrical effect over the nitrate precursor used. On the contrary, due to the high surface area, ruthenium particles would also be highly dispersed on these carbon supports [45]. However, there is no simple relationship between the value of the surface area of the activated carbon and the metal dispersion of the catalysts supported on activated carbon [46]. Some authors [47–51] reported the inhibition and drawbacks due to the use of RuCl3 as a precursor salt because the chloride from this salt is a poison for CO and H2 chemisorptions and may be partitioned between the metal and the support. In our case, the high degree of sintering of the ruthenium metal particles could be due to the fact that, during the pretreatment process, no oxychlorinated species interacting with the support are formed, as noted earlier while studying ruthenium catalysts of different metal contents over the alumina support [12, 21]. The low dispersion of nickel is a characteristic when this metal is used to prepare inorganic or carbonaceous catalysts [52, 53].Table 2
Metal loading, dispersion, particle diameter, XPS, initial reaction rate, and activity (TOF) results for the catalysts.
Catalysts
Metal loading (%)
D (%)
d (nm)
XPS
r° (mol·gM−1·s−1)
TOF (s−1)
M 3d5/2 BE (eV)
Cl/M (at/at)
PdN/C
0.39
48
2.4
335.2
—
0.077
17.0
PdCl/C
0.42
62
1.9
335.2
1.56
0.050
8.6
RuCl/C
0.41
20
5.3
282.1
2.96
0.056
28.5
NiCl/C
0.41
4
25.2
857.3
2.05
0.026
38.9
Lindlar
5
2.5
46.4
337.2
—
0.003
13.5From the H2 chemisorption results, the metal particle size (d) was determined on assuming a spherical particle in accordance with Badano et al. [21]. The particle size order is PdCl/C < PdN/C < RuCl/C ≪ NiCl/C ≪ Lindlar. The smallest particle size of PdCl/C catalysts is due to the higher surface interaction between Pdδ+OxCly and oxygenated groups of the carbonaceous support, as observed earlier when alumina was used as a support [21]. The higher particle size of NiCl/C could be related with the higher structural defects observed by the Raman spectra in Figure 3.Figure6 shows the XPS spectra of the Pd 3d5/2 band for PdN/C and PdCl/C, Ru 3d5/2 band for RuCl/C, and Ni 2p3/2 band for the NiCl/C catalyst. Besides, the XPS spectra of the catalysts prepared from chlorine precursors (PdCl/C, RuCl/C, and NiCl/C) show a Cl 2p3/2 peak at ca. 199.4 eV that corresponds to surface chloride species [54] that were not completely eliminated after reduction because of the high adsorption capacity of the carbonaceous material used. The maximum binding energy (BE) of Pd and Ru 3d5/2, Ni 2p3/2 peaks, and Cl/M atomic ratios are also listed in Table 2.Figure 6
XPS spectra of BE Pd 3d for (a) PdN/C, (b) PdCl/C, (c) RuCl/C, and (d) NiCl/C catalysts treated in H2 at 393 K.
(a)
(b)
(c)
(d)XPS results in Figure6 show that both palladium catalysts present a Pd 3d5/2 peak at 335.2 eV, which can be attributed to Pdδ+ (δ ≈ 0) [16, 54]. Figure 6 also shows the spectra of palladium catalysts and the 3d3/2 peak doublet shifted 5.2 eV with respect to the 3d5/2 peak. No nitrogen was detected by XPS on the Pd catalyst prepared from the nitrate precursor. On the contrary, for the PdCl/C sample, the Cl/Pd atomic ratio was 1.56, confirming that chloride is present even after the reduction treatment. This could be attributed to the high absorption capacity of the carbon support. The chlorine content does not affect the palladium surface as it is totally reduced on the PdCl/C catalyst.In the case of ruthenium, the BE reference is difficult because the Ru 3d peaks appear at the same region than the C 1s peak. There are also discrepancies in the BE reported in the literature for ruthenium compounds. The Ru 3d5/2 signal for the RuCl/C catalyst was observed at 282.1 eV corresponding to ruthenium electrodeficient species as RuCl3 [54]. For this catalyst, after the temperature pretreatments, the superficial atomic ratio Cl/Ru was 2.96.According to the bibliography [54, 55], the Ni 2p3/2 signal appears at 852.5 eV for Ni° species. For the NiCl/C catalyst, the two signals were observed in the spectrum of Figure 6 at 857.3 and 862.7 eV. The first peak could be assigned to the electrodeficient nickel species (Nin+, with n → 2), probably corresponding to nickel interacting with the support [54–56], while the second peak corresponds to the characteristic shake-up satellite structure of Ni (II) [55, 57, 58]. This catalyst also presents a high Cl/Ni atomic ratio (2.05) as a consequence of the adsorption capacity or the carbonaceous support.For the Lindlar catalyst, in Table2, the main peaks at 335.2 eV (69%, at/at) and 336.9 eV (31%, at/at) are also registered, assigned to Pdδ+ and electrodeficient Pdn+ species (with δ → 0 and n → 2), respectively [53]. On the contrary, on the Lindlar catalyst, also two peaks of the Pb 4f7/2 spectrum at 136.8 eV (20%, at/at) and 138.6 (80%, at/at) were attributed to Pb and Pb(OAc)2, respectively [53].In Figure7, TEM micrographs of the carbonaceous catalysts are shown. The metal particle size for the PdCl/C catalyst is between 1 and 4 nm, presenting a high concentration of 2 nm Pd particles on the carbon surface. For PdN/C, the main palladium particle size is between 4 and 8 nm. The particle sizes of Ru on RuCl/C are mainly between 1 and 5 nm, although several bigger particles were observed on the micrographs. Besides, the NiCl/C catalyst presented the highest particle sizes between 25 and 40 nm.Figure 7
TEM Images for (a) PdN/C, (b) PdCl/C, (c) RuCl/C, and (d) NiCl/C catalysts.
(a)
(b)
(c)
(d)


## 3.2. Catalytic Tests

The catalytic performance during the selective hydrogenation of 1-heptyne for PdN/C, PdCl/C, RuCl/C, and NiCl/C catalysts is shown in Figure8. 1-heptyne total conversion (%) and selectivity to 1-heptene (%) as a function of time (min) were plotted in this figure for all the studied catalysts. All the catalysts were active during the hydrogenation of 1-heptyne and presented high selectivity to 1-heptene, the desired product.Figure 8
Total conversion (a) and selectivity to 1-heptene (b) versus time (min) for PdN/C, PdCl/C, RuCl/C, and NiCl/C catalysts pretreated in H2 at 393 K.
(a)
(b)Besides, in Figure9, 1-heptyne total conversion (%) and selectivity to 1-heptene (%) as a function of time (min) for the commercial Lindlar catalyst used as a reference is shown.Figure 9
Total conversion () and selectivity to 1-heptene () versus time (min) for the Lindlar catalyst (reproduced from Lederhos et al. [52], under the Creative Commons Attribution License/public domain).According to Figures8 and 9 the order of selectivities to the corresponding alkene was:(1)PdCl/C<PdN/C≅RuCl/C<Lindlar<NiCl/CIn order to compare the performance of the catalytic systems, the initial reaction rate of hydrogenation of 1-heptyne (rA0) was estimated for all the catalysts using the following formula:(2)rA0=V⋅CA0WM⋅∂XA∂tt=0,where rA0 is the initial 1-heptyne reaction rate (mol·gM−1·s−1), ∂XA/∂tt=0 is the tangent value of the 1-heptyne total conversion versus time curve at t=0, CA0 is the initial concentration of 1-heptyne (mol·L−1), WM is the mass of the metal (Pd, Ru, or Ni) in the catalyst (g), V is the reaction volume (L), and t is the reaction time (s).From these initial reaction rates of 1-heptyne hydrogenation, TOF values were calculated for all the catalysts and are summarized in Table2. For hydrogenation reactions, TOF values between 10−2 and 102 indicate a structure-insensitive system, not influenced by particle size [59, 60], so the differences in activities and selectivities between the catalysts may be associated with geometrical and/or geometrical effects. The order of activities of low-loaded catalysts is(3)PdCl/C<Lindlar<PdN/C<RuCl/C<NiCl/CThe effect of the precursor salt was studied by comparing PdCl/C and PdN/C catalysts. The results obtained for these catalysts show differences in both activity and selectivity. For the catalyst synthetized from palladium nitrate as the precursor salt, the obtained TOF was 17 s−1 versus the activity of palladium chloride precursor salt 8.6 s−1. That is, each active site of the PdN/C catalyst is almost two times more active than that of PdCl/C. As observed by XPS and RTP, both catalysts have Pdδ+ (with δ ≅ 0) as the active site, so no electronic effects are generated by the metallic phase; besides as observed by Raman, quite higher structural effects were found on PdN/C than on the PdCl/C sample. When comparing the catalytic behavior of the different Pd precursors, higher selectivities to 1-heptene were obtained when palladium nitrate was used, ca. 86% at 180 min, while for PdCl/C selectivities, ca. 70% was obtained.In Figure10, the main superficial groups present on carbonaceous supports are summarized. Between them carboxylic groups by heterolytic rupture of the O-H bond, could favor the adsorption of the cationic metallic precursors Mn+. In our case, the higher distribution of carboxylic and lactone groups on the surface of PdN/C could favor the adsorption of Pd2+, and its reduction to Pd° (as detected by XPS and TPR) during the pretreatment step: for 1 h at 393 K under a hydrogen stream. Also, the high concentration of carboxylic groups favors the high dispersion of the active sites and the small particle sizes. So, the observed differences in activity between PdN/C and PdCl/C could be originated, at least in part, by geometrical effects due to higher structural defects (as noted in D-bands on the Raman spectra) and electronic effects originated by the high concentration of carboxylic superficial groups on PdN/C (the favorable effect) and high remnants of chloride on PdCl/C catalysts (the negative effect). Besides, differences in selectivity between the PdN/C and PdCl/C catalysts could be caused on the one hand to the electronic and geometrical effects that favors the formation of 1-heptene and on the other hand to higher amount of carbonaceous superficial groups that favors the desorption of the alkene, avoiding its overhydrogenation, while alkyne is present in the reaction media.Figure 10
Schematic representation of the main superficial groups found on a carbonaceous supports.When analyzing the effect of the metal type used to synthesize the carbonaceous catalysts, PdCl/C, RuCl/C, and NiCl/C, the highest activity and selectivity were achieved when the supported metal is nickel, a very low cost precursor salt. The high activity and selectivity of NiCl/C could be related to electronic or geometrical effects of active sites, which would control the dissociative adsorption of hydrogen being this the controlling step [61], and/or to the aromatic superficial groups of the support that would preferentially adsorb remaining 1-heptyne desorbing 1-heptene from the reaction media, so avoiding its total hydrogenation to the alkane.


## 4. Conclusions

The effect of metallic salt and the kind of metal was studied using a carbonaceous support. A series of low-loaded catalysts supported on an activated carbon (ca. 0.4 wt.%) were synthetized by the incipient wetness technique. Nanoparticles of palladium, ruthenium, and nickel were deposited using Pd(NO3)2, PdCl2, RuCl3, and NiCl2 aqueous acidic solutions as precursor salts. The catalysts were pretreated under moderate conditions.PdN/C, PdCl/, RuCl/C, and NiCl/C were characterized by ICP, TPD, FTIR micro-ATR, Raman, XRD, TPR, hydrogen chemisorption, XPS, and TEM.All the catalytic systems were assessed during the selective hydrogenation of 1-heptyne, a medium-chain alkyne under moderate operational conditions: 303 K, 150 kPa, and 800 rpm during 180 min. The catalysts were active and selective to 1-heptene. The order of activity and selectivity found was NiCl/C > RuCl/C > PdCl/C. Geometrical and electronic effects over the NiCl/C catalyst favors alkyne adsorption and 1-heptene desorption in the reaction media, avoiding alkyne total hydrogenation to the alkane. Besides, the PdN/C catalyst is more active and selective than PdCl/C due to geometrical and electronic effects, and the first ones are caused by structural defects (observed by Raman), while the seconds ones are originated by the high loading of carboxylic superficial on PdN/C and the chloride remnants on PdCl/C catalysts (as observed by TPD-MS and XPS, resp.).



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