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Article

Effects of Different Concentrations of Arsine on the Synthesis and Final Properties of Polypropylene

by
Joaquín Hernández-Fernández
1,*,
Yoleima Guerra
2,
Esneyder Puello-Polo
3 and
Edgar Marquez
4,*
1
Chemistry Program, Department of Natural and Exact Sciences, San Pablo Campus, University of Cartagena, Cartagena 130015, Colombia
2
Centro de Investigación en Ciencias e Ingeniería, CECOPAT&A, Cartagena 131001, Colombia
3
Grupo de Investigación en Oxi/Hidrotratamiento Catalítico Y Nuevos Materiales, Programa de Química-Ciencias Básicas, Universidad del Atlántico, Puerto Colombia 081001, Colombia
4
Grupo de Investigaciones en Química Y Biología, Departamento de Química Y Biología, Facultad de Ciencias Básicas, Universidad del Norte, Carrera 51B, Km 5, Vía Puerto Colombia, Barranquilla 081007, Colombia
*
Authors to whom correspondence should be addressed.
Polymers 2022, 14(15), 3123; https://doi.org/10.3390/polym14153123
Submission received: 20 June 2022 / Revised: 22 July 2022 / Accepted: 29 July 2022 / Published: 31 July 2022
(This article belongs to the Special Issue Synthesis, Processing, Structure and Properties of Polymer Materials)
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Versions Notes

Abstract

:
This article studies the effects of arsine on the synthesis and thermal degradation of 4 samples of virgin polypropylene (PP-virgin) and proposes reaction mechanisms that allow understanding of its behaviour. Different points are monitored during the polypropylene synthesis to perform TGA, DSC, FT-IR, RDX, and MFI analyses later. The content of AsH3 in polypropylene varies between 0.05 and 4.73 ppm, and of arsenic in virgin PP residues between 0.001 and 4.32 ppm for PP0 and PP10, increasing in fluidity index from 3.0 to 24.51. The origin of thermo-oxidative degradation is explained by the reaction mechanisms of the Molecule AsH3 with the active titanium center of the ZN catalyst and the subsequent oxidation to form radical complexes. OO-AsH-TiCl4-MgCl2 and (OO-as-OO)2 -TiCl4-MgCl2, which, by radical reactions, give rise to the formation of functional groups aldehyde, ketone, alcohol, carboxylic acid, CO, CO2, PP-Polyol, PP-Polyether, and PP-Isopropylethers. These species caused the TG and DTG curves to increase degradation peaks in pp samples.

1. Introduction

Arsine (AsH3) is a chemical compound of inorganic nature formed by an arsenic atom and three hydrogen atoms, and has a general structure ER3 (E = As, N, P, Sb, Bi, and R = H, alkyl, aryl, halogens) and a tetrahedral geometry, with the pair of non-shared electrons located in one of its vertices, which can act as a soft Lewis base [1,2]. In addition, it can bind to transition metals (M), specifically those that have partially filled d-orbitals and with vacant s and p orbitals, and form M-ER3 complexes using a covalent bond between the arsine and the metal [1,3]. The coordination of the metals of the d-block of these compounds is given two bonds at once: the donor bond σ and acceptor π. The donor bond σ is established between the pair of nonbonding electrons of the ER3 ligand, belonging to the HOMO orbital of the ligand (Highest Occupied Molecular Orbital) and the vacant orbitals of the metal (LUMO, Lowest Unoccupied Molecular Orbital). On the other hand, for the π bond, an action called retro bonding occurs between the filled or half-filled orbitals of the metal (HOMO of the metal) and the anti-bonding σ orbitals of the E-R ligand and/or the empty d orbitals of the heteroatom (E) [4,5]. Arsine complexes for use in catalytic processes are of interest for their organometallic characteristics [6,7,8,9,10], such as their oxidation state, metal coordination number, and the ease by which they can form vacant coordination sites, among others, thereby allowing us to understand its reactivity and behaviour in catalytic systems [11,12]. The use of analysis techniques such as FTIR, X-ray fluorescence, and NMR are necessary for studying these interactions between ligands and metals so that the oxidation of compounds can be evaluated [4,13,14,15].
The effect of AsH3 on the synthesis of PP is of importance since, in the polymerization stage of propylene, fundamental raw materials are required, such as Propylene, Ziegler catalyst Natta (ZN), triethylaluminium co-catalyst (TEAL), selectivity control people, hydrogen (H2), and nitrogen (N2) [16,17], where at least one can act as Lewis acid or have transition metals is its structure. PP synthesis begins with the initiation reaction, which is the activation of the double bond and the active site, followed by a polymerization stage and a polymerization completion stage [18]. The catalyst is titanium (IV) chloride (TiCl4), which is a compound with a tendency to form different complexes with a wide diversity of ligands as a result of being a strong Lewis acid [19,20]. In the catalytic system used for the synthesis of PP, the effect of impurities such as this and other components, such as inhibitors of PP polymerization, have been examined and quantified [15,21,22,23,24,25,26,27,28]. In this sense, AsH3 is an inhibitor of polymerization reactions. It is observed that its effect is irremediable to the catalytic system and its coordination reaction with the active center of Ti in the catalyst, as well as to the different surfaces of MgCl2 and with the alkyl co-catalyst [29,30,31].
In this research, the synthesis of 4 PP is conducted, and specific concentrations of AsH3 are dosed at each stage [32] to evaluate its impact on the efficiency of the catalyst. Regarding the PP production rate during the polymerization stage, the effect on the onset of thermal degradation of PP will be evaluated. The significant alterations in the physicochemical properties of PP are of great importance, and have not been observed in previous research. These must be studied so that adequate reaction mechanisms can be explained and proposed in order to help understand the effect of arsine.

2. Materials and Methods

2.1. Standards and Reagents

For the elaboration of this work, a fourth-generation spherical Ziegler-Natta catalyst with MgCl2 support with 3.6% by weight of Ti was used; Diisobutyl phthalate (DIBP) as an in-house donor supplied by Sudchemie, Germany. It was used as a triethylaluminium co-catalyst (98% purity TEAL) from Merck, Germany, diluted in n-heptane. As an external donor, cyclohexyl methyl dimethoxysilane (CMDS) acquired from Merck, Germany, was used. Shazand Petrochemical, Iran, provided polymer-grade propylene. The hydrogen and nitrogen used had a purity of 99.999% [33,34].
We worked with AsH3 at 99.999% purity and to guarantee the concentrations of 0.1 and 3.0 ppm in LPG balance, which were required for this research. A dilusor in line was used, which allowed for the creation of the mixtures of AsH3 and LPG in the required proportions.

2.2. Polymerization Process

The PP samples were synthesized by polymerization of propylene in the gas phase with the use of a ZN catalyst [35]. The process is shown in Figure 1, and this process consists of a fluidized bed reactor, where nitrogen was initially fed to purge the equipment; subsequently, the propylene and hydrogen that provide the fluidization and absorb the heat of the reaction were fed the catalyst, TEAL, the selectivity control agent, and the nitrogen, in order to carry out the polymerization in discontinuous mode; the quantities are shown in Table 1. This process was conducted at 70 °C and 27 bar pressure. Gases leaving the reactor passed through a compressor to be transported to a heat exchanger where they were cooled and recirculated to the reactor. The resin obtained passed to a purge tower fed with nitrogen and steam to remove traces of hydrocarbons that left the system to obtain a virgin resin [17].
During the process, sampling points were established, as shown in Figure 1. The first points correspond to the feed where samples of propylene were taken (A) that came from liquefied petroleum gases (LPG), nitrogen (B), hydrogen (C), and arsine (D), which came from the same as the propylene from LPG. The following points are those taken from within the reactor; these are composed of gas samples inside the reactor (E), catalyst inside the reactor (F), a sample of the catalytic system (G), and recirculated propylene (H). The last points were taken in the degassing stage, the resin sample that came out of the reactor (I), the gases that were synthesized and removed by virgin PP desorption (J), and the PP obtained from the process (K). Because this process was repeated several times with different concentrations of arsine, a number was assigned to each of them, with zero as the target.
Throughout the process, sampling points were established, as shown in Figure 1. These were found in the feed, in the reaction system, and in the degassing stage. Table 2 describes the sampling points and the identification of the samples; because this process was repeated several times with different concentrations of arsine, a number was assigned to each of them, with zero as the target.

2.3. Analysis

2.3.1. Thermogravimetric Analysis-TGA

To determine the effects of arsine on the thermal degradation of the PP samples obtained, the Perkin Elmer TGA7 equipment performed a thermogravimetric analysis (TGA) at a heating rate of 20 °C min−1 and under an N2 flow rate of 60 mL min−1. For this analysis, 10 mg samples were used to obtain the TG and DTG curves [36,37].

2.3.2. Differential Scanning Calorimetry Analysis-DSC

A differential heat scanning (DSC) analysis was performed on a DSC Standard Cell RC. To ensure an identical thermal history, the sample was heated from 0 °C to 230 °C at a rate of 10 °C min−1 and subsequently cooled from 230 °C to 0 °C at the same speed.

2.3.3. Melt Flow Index-MFI

The melt flow index (MFI) was measured using a Tinius Olsen MP1200 plastometer. The temperature inside the cylinder of the plastometer was 230 °C and a 2.16 kg piston was used to displace the melt. After the MFI data was obtained, the average molecular weight for each of the PP samples was evaluated using the Bremner approximation [38], which was obtained by correlations that were formulated by the study of commercial polypropylene samples with MI values between 0.7 and 12, measuring the variation in the molecular weight distribution by SEC, using differential refractive index and low-angle laser light scattering detectors [39].
MW3.7 = 1675/((MFI230 °C 2.16 kg) × 10−21)

2.3.4. X-ray Fluorescence

This analysis was performed on Malvern’s Axios FAST analytical equipment, which allowed us to see the concentration of arsenic and arsine present at the sample points.

2.3.5. Infrared Fourier Transform Analysis-FT-IR

Fourier transform infrared spectroscopy (FT-IR) was used to determine the most significant structural changes in the PP matrix and the ZN catalyst due to the reaction of ZN Ti with AsH3, and to evaluate how this interaction affected the thermal stability of PP. FT-IR analysis was performed using a Nicolet 6700 (Thermo Scientific) infrared spectrometer using the attenuated total reflectance (ATR) method. The samples were analyzed in the form of films; these films were obtained by compression moulding of the PP in a CARVER 3895 hot press to obtain 300 mm diameter films of ≈100 μm thickness.

2.3.6. Gas Chromatography Analysis with Selective Mass Detector (GC-MS)

A GC-MS 7890B from Agilent technologies was used for arsine analysis [36]. Figure 2 shows the chromatograms of the standards for AsH3.

2.3.7. Headspace-GC-MS

PP samples were analyzed using an Agilent 7694E Headspace Sampler with the following conditions, GC cycle time: 60 min, furnace: 150 °C, transfer line: 175 °C, loop: 175 °C, vial equilibrium time: 60 min, stirring speed: off, loop size: 1.0 mL, loop filling time: 0.2 min, loop equilibrium time: 0.02 min, injection time: 0.3 min, pressurization time: 0.4.

3. Results

3.1. Polymerization Process

Polymerization occurs in three stages. The first is the formation of the active site consisting of the alkylation of a pentacoordinate Ti (III) ion for the titanium atom that is on the surface of the layers of the α-TiCl3 [40,41] and the activation of the double bond of the monomer. This is given by the coordination of the monomer when establishing a giving bond of electrons p of the double bond with the empty orbital of the transition metal. During the reaction, an intermediate is formed where the unsubstituted carbon binds to the transition metal and the other to the alkyl group [18]. The second stage is the propagation of the monomer, where the active center is linked to the transition metal-alkyl, formed by the constitution of a coordination complex between the growth chain, the added monomer, and the active center of the catalyst [41]. The third stage is the culmination of polymerization, which can be achieved with the separation of hydrogen β, with the removal of a hydride, or by deactivation of the complex using H2 [41,42]. The addition of arsine during polymerization can affect this process due to its ability to bind to transition metals such as Ti present in the catalyst, inhibiting its effectiveness. Thus, in this work, samples are taken at strategic points that allow for the measurement of the content of this compound and for the proposition of a reaction mechanism, so that the behavior of the PP-virgin arsine and its effects can be determined.

3.1.1. Quantification of Arsine at the Polymerization Stage

The variation of the concentrations of arsine presented in the samples taken at the different selected points of the polymerization process is shown in Figure 1, where the points detailing the presence of these components can be observed. Point D is the initial concentration of arsine introduced to the process, which varies from 0.05 to 4.73 ppm, referring to the presence of impurities not removed during the purification stage of the refinery grade propylene, which translates to a failure of the petrochemical plants that supply this compound. Point H refers to the recovered propylene; the values obtained are equal to 0, which means that AsH3 was adsorbed or absorbed during the polymerization reaction. Point E shows the gaseous propylene found in the reactor; the presence of AsH3 at this point indicates that the compound is part of the reaction or interacts in the formation of the polymer being adsorbed, which had been confirmed at point H. Therefore, there must be a reaction mechanism between the catalyst and the arsine that allows the latter to act as a component of the polymerization reaction, which is possible due to the arsine’s ability to form M-ER3 bonds, binding to the transition metal of the active center of the catalyst affecting the polymerization reaction, and due to the efficiency of the catalyst.

3.1.2. Reaction Mechanisms of AsH3 Proposed during Polymerization: Reaction of Residual AsH3 with TiCl4/MgCl2

In the mechanism proposed in Figure 3, AsH3 competes with the propylene monomer for the active site of Ti. First, a complex π is formed by coordinating the AsH3 with the Ti of the TiCl4/MgCl2 complex. The AsH3-Ti interaction is conducted via the interaction of the electropositive Ti with the free electron pair of arsenic, which predominates the electrons of the π bond of propylene. The formation of a complex π in Ti-propylene has no barriers and is accompanied by an energy gain less than that of AsH3-Ti, so the latter reaction is predominant. The propylene insertion barrier varies between 6–12 kcal mol−1 [43,44,45,46]. The high probability of occurrence of the insertion reaction is supported by thermodynamics, since a favoring of approximately 20 kcal mol−1 is observed [30,47,48]. In the PP synthesis process, the polymer chain’s propagation takes place by moving propylene into Ti-PP, where the PP-alkyl chain has the olefin inserted [47,49]. The PP chain’s growth is affected when Ti’s active centre reacts with inhibitors of different polarities. The occurrence of these reactions depends on energetic factors. The coordination of the different inhibitors to the Ti Center on the surface of MgCl2 is favored by 27.2 kcal mol−1 for Ti-H2O, 15.1 kcal mol−1 for Ti-H2S, 8.4 kcal mol−1 for Ti-CO2, 13.1 kcal mol−1 for Ti-O2, and 30.6 kcal mol−1 for Ti-CH3OH interactions [26]. Since AsH3 exhibits polarities intermediate to the poisons mentioned above, it is expected that its values are within the ranges discussed above. As shown in Figure 3, AsH3 interferes with the formation of propylene complexes and their insertion. It is worth mentioning that the interactions of these impurities, including AsH3 with the active centers of Ti, are reversible when these inhibitors are removed from the system, and thereafter, the active center of Ti resumes polymerization [50].

3.1.3. Discussion of FTIR Analysis

Figure 4 shows the catalyst’s infrared spectra with various arsine levels used during the synthesis of PP. The above identifies species of oxidized arsenic in the As-ZN complex, thus supporting the mechanisms prepositioned in Figure 3. Concerning the fundamental vibration As-O and As = O in FTIR, the force constants of an As-O bond estimated by the use of Gordy’s rule are 8.7 × 105 and 4.6 × 105 cm−1 dinas for a single bond and double bond, respectively [51]. When substituted in the fundamental equation for a harmonic oscillator, these values give VAs-O 964 and 776 cm−1 for a “pure” single bond and a double bond, respectively. The values for the fundamental vibration As-0 and As = O were, in most cases, within 10–40 cm−1 of 920 cm−1 the average of the frequencies calculated for a single and double bond [51,52]. The observed frequency suggests a higher bond order than one that may well result from the subsequent donation of the pπ electrons of the oxygen atom using the empty dπ orbitals of the arsenic atom. Figure 4 shows that the band’s growth between 800 and 970 cm−1 is associated with the increase in the concentration of oxidized arsenic atoms in the As-ZN complex, and an increase in the area of these peaks is observed, being greater for the K10 sample. This last catalyst sample was the one that was in contact with the highest levels of AsH3. The spectra indicate that the oxidized arsenic that is part of a chemical complex within the catalyst was higher when AsH3 levels increased.
Arsenic of AsH3-TiCl4-MgCl2 is oxidized in the presence of oxygen atoms to form a complex of radicals O-O-AsH2-TiCl4-MgCl2, which are the initiators of the degradation of wasting PP. In Figure 5, the effect of this complex of radicals O-O-AsH-TiCl4-MgCl2 is shown on the beginning of the degradation of PP, which consists of the abstraction of hydrogen in the PP-virgin, generating a stable tertiary radical, which, when reacting with a molecule O2, will produce a Peroxy-PP-virgin radical, which extracts hydrogen from a neighboring virgin-PP chain, thereby forming the virgin-PP-Hydroperoxide. The latter, after a homolytic rupture, will give rise to the Alkoxy-PP-Virgin radical [53,54,55,56]. The radical complex of O-O-ash-tiCl4-MgCl2, after the abstraction of hydrogen, forms the peroxy complex H-O-O-AsH-TiCl4-MgCl2 that, by hemolysis, forms the radical O-AsH-TiCl4-MgCl2. The latter can perform successive abstractions of hydrogen from the tertiary carbon of the PP-virgin chain to continue increasing its degradation or reaction with hydrogen radicals to end the radicalization process and form the stable complex HO-AsH-TiCl4-MgCl2. This last complex also participates in the radical reaction with PP-virgin and with oxygen atoms to form the radical tertiary polymer and the intermediate complex HO-As-OH-TiCl4-MgCl2 that, by dehydration, forms the new adduct O = As-TiCl4-MgCl2. Figure 3b shows the reaction of two molecules of AsH3 with the active center of Ti of the Catalyst ZN, to form the complex (AsH3)2-TiCl4-MgCl2 that subsequently oxidizes in the presence of oxygen atoms to form the radical complex (O-O-As-O-O-)2-TiCl4-MgCl2, which are the initiators of the degradation of PP-virgin residues by abstraction of multiple tertiary carbon protons, by the formation of multiple tertiary radicals of the PP-virgin chain and the intermediate complex HO-As-OH-TiCl4-MgCl2 that, by dehydration, forms the new adduct O = As-TiCl4-MgCl2.

3.2. Effects of Arsine on the Properties of PP

3.2.1. Effects of Arsenic Content on Virgin PP MFI

The effects of the arsenic content in the samples are reflected in the change of the MFI obtained for each of them, presenting a linear correlation with an R2 of 0.99786; where the concentration of income of AsH3 increases, so does the MFI, as shown in Figure 5. This means that the arsine from impurities (point A) participates in the polymerization reaction, forming a stable complex present in the polymer chain that changes some properties of the resin obtained, including the Mw of the samples, which was calculated using the formula proposed by Brenner. Its variation is shown in Figure 5, demonstrating that as the arsenic content present in the resins increases, the MFI decreases.
Consequently, small chain scissors and fractures of the polymer structure during degradation are very frequent, occurring as the average molecular weight decreases and the MFI increases. It should be noted that the residue contents of the catalyst, such as Ti, Al, Cl, and Fe, do not present significant differences, thus the changes presented in this paragraph are not generated by residues other than arsine, as has been presented in other studies [36,57].
From these data, it can be inferred that, during the reaction, the arsine reacts with the ZN catalyst. During the development of this work, a reaction mechanism was proposed where it was evident that the arsine competed with the propylene molecule in the polymerization stage, reacting with the active center of the ZN that influences the growth of the polymer chain and presenting evidence of the high reactivity of the catalyst.

3.2.2. Degradation of Residual PP

The thermal degradation of the samples was evaluated by TGA and DSC, the data obtained show a decrease of the thermal stability of the material as the arsenic content increases. These results are presented in Figure 6. The thermal behavior of the K0 sample does not have a significant variation, as presented in the literature [19]. K0 and K1, which have a zero and very low content of arsenic, respectively, in their matrix, have a peak rupture at 390 and 430 °C with a mass loss of 22%.
The addition of AsH3 in the polymerization implies marked changes in the performance and macromolecular structure of the final material obtained, demonstrating that their molecular weight and thermal stability are too low to have functional groups different from the hydrocarbon. Previous research has demonstrated a link between the polymer’s low molecular weight and photooxidative degradation, as indicated by the carbonyl index in the 1712 cm−1 band of FTIR (Figure 7), which is impacted when the concentration of arsine and arsenic in the sample increases [57,58,59]. To understand this behavior, a reaction mechanism is proposed to explain the reduction in the physicochemical properties of PP when it has arsine content.

3.3. Degassing Process

The degassing process is the second stage of the process, in which the resin passes when leaving the reactor. This consists of the purge tower, where nitrogen and value are fed to remove the hydrocarbons, and the adsorption or absorption of arsine by the resin obtained is confirmed [35].

3.3.1. Identification and Quantification of Arsine in the Degassing Stage of PP Resin

Table 3 shows the concentrations obtained from the different compounds during the degassing stage taken at the available sampling points together with the input data for the overall process. Point I: the samples obtained from this point are of newly polymerized resin, which contains arsine either absorbed or adsorbed. Point J: volatile compounds are removed, having values equal to 0 for the arsine content, which allows us to rule out the absorption of both arsine and arsenic at the interface of the polymer. At this point, the other compounds formed during polymerization that are purged are also determined, which allows us to determine the effect of the arsine on their composition. Finally, point K: showing that the resin obtained has the content of the two compounds, therefore, the products obtained from these processes are considered waste and may present variations concerning virgin resins that can contribute to the degradation of the material, thermal stability, and fluidity index, among others. The study of the effects on these properties allows us to determine applications for these generated residues.
The compounds determined during this stage present a significant increase concerning the target; this increase may be related to the increase in the content of arsine fed in the polymerization stage. If we take point J as a reference, where most of these gaseous compounds are removed, it can be seen that the values are 3.5 to 5.27 times higher for the sample J1 concerning the white (J0); in the case of the J10 sample, the values are between 9.29 and 20.4 times higher with respect to the white, being alcohol the compound, where the greatest increase is shown. In addition, as the arsine content in the feed increases, the formation of CO production is promoted.

3.3.2. Mechanisms of Reaction of Peroxy Radicals in Arsenic Complexes to Form the VOCs Identified in PP

The Alkoxy-PP-virgin radical that has formed undergoes a homolytic rupture of the simple bond adjacent to the carbon of the oxygenated radical. This homolysis forms the methyl-PP-virgin ketone and the radical PP, as seen in Figure 8. The radical O-AsH-TiCl4-MgCl2 attacks the tertiary carbon of the methyl-PP-virgin ketone, to abstract the hydrogen atom and thus propagate the oxidation of the more stable carbon [58]. This new radical reacts with the oxygen atom to form the β-Hydroxyperoxy Methyl-PP-virgin Ketone, 2,4-pentanedione, 1-Hydroxy-2-propanone, and acetone. The latter two are formed after homolytic cleavage of another tertiary carbon bond, the formation of the acetone radical, and subsequent reactions with the hydroxyl and hydrogen radicals. On the other hand, the PP radical at the end of the chain reacts with O2, giving rise to PP-hydroperoxide, to the PP-Alkoxy radical, and then to methanol-PP-virgin, which, by abstraction of the tertiary carbon proton by the radical O-AsH-TiCl4-MgCl2, forms an intermediate radical that, when reacting with O2, decomposes into methanol and formaldehyde. Methanol-PP-virgin gives rise to Aldehyde-PP-virgin that, by homolysis of the H-C bond of the terminal carbonyl group, forms the Carbonyl-PP-virgin radical, which in turn, by reactions with hydroxyl radicals and hydrogen, gives rise to CO, CO2 and formic acid, as shown in Figure 8.
The strong relationship between the concentration of AsH3 residues and the arsenic content within the PP-virgin matrix with the MFI, TG, and DTG shows that increasing the concentration of AsH3 drastically decreases the stability of PP, allowing us to propose an alternative reaction mechanism to that shown in Figure 3; a mechanism that comes even closer to the behavior of K10. Figure 8 shows the reaction of two Molecules AsH3 with the active center of Ti of the catalyst ZN, to form the complex (AsH3)2-TiCl4-MgCl2 that is subsequently oxidized in the presence of oxygen atoms to form the radical complex (O-O-As-O-O-)2-TiCl4-MgCl2, which are the initiators of the degradation of PP-virgin waste by abstraction of multiple tertiary carbon protons, by the formation of multiple tertiary radicals of the virgin-PP chain. These will react with the oxygen atoms by forming PP-Virgin poly peroxide that supports increased PP fluidity and low TG and DTG values. The poly peroxide of PP-Virgin, due to its chemical structure, has the appropriate stereochemistry to form hydrogen bonds with another poly peroxide of the PP-Virgin to give rise to a macromolecule of greater polarity, and in an acid medium, creates polyols of PP-virgin. Figure 8 also shows that PP-virgin polyoxide, by the effect of hydrogen and hydroxyl radicals, forms PP-virgin polyols with a carboxyl group at the end of the chain. The latter experiences homolytic ruptures and dehydration. In homolysis, it gives rise to acetone, 1-Hydroxy-2-propanone, isopropyl alcohol, and 1,2-Propanediol, and in dehydration, it forms stable tertiary carbocations, which, when reacting with different alcohols and polyols, gives rise to macromolecules of PP-virgin ether type.
This study showed the impact that certain contaminants may have on the manufacture of polymers such as polypropylene. The selection and analysis of raw materials is critical to preventing this sort of reaction from happening during the industrial synthesis of PP. With this research, we expect that the purity of any raw materials will be thoroughly examined before application.

4. Conclusions

After the analysis of the samples obtained, it is possible to define the effect that the arsine has on thermal stability and other properties of PP, in addition to defining how an increase of the content of this chemical compound can further enlarge the difference in thermal stability, molecular weight, and MFI between the samples and standard; the first two decreasing and the last increasing. Likewise, the possible reaction mechanisms that occur between the arsine with the active titanium center of the ZN catalyst and the subsequent oxidation to form radical complexes of O-O-AsH-TiCl4-MgCl2 and (O-O-As-O-O-) 2-TiCl4-MgCl2, which, by radical reactions, give formation to aldehydes, ketones, alcohols, carboxylic acids of functional groups, CO, CO2, PP-Polyol, PP-ethers, and PP-Isopropyl ethers, can be defined.

Author Contributions

Conceptualization, J.H.-F.; methodology, J.H.-F. and E.P.-P.; validation, E.P.-P. and E.M.; formal analysis, J.H.-F. and Y.G.; investigation, Y.G. and J.H.-F.; writing—original draft preparation, Y.G.; writing—review and editing, E.M.; E.P.-P. and Y.G.; supervision, J.H.-F. and E.M.; project administration, J.H.-F. All authors have read and agreed to the published version of the manuscript.

Funding

This research received no external funding.

Institutional Review Board Statement

Not applicable.

Informed Consent Statement

Not applicable.

Data Availability Statement

The data presented in this study are available on request from the corresponding author.

Conflicts of Interest

The authors declare no conflict of interest.

References

  1. Quinteros, J.G. Sintesis y Aplicaciones de Ligandos Arsinas. Estudios de Sistemas Catalíticos de Pd y Au; Universidad Nacional de Córdoba: Córdoba, Spain, 2016. [Google Scholar]
  2. Gras, R.; Luong, J.; Hawryluk, M.; Monagle, M. Analysis of part-per-billion level of arsine and phosphine in light hydrocarbons by capillary flow technology and dielectric barrier discharge detector. J. Chromatogr. A 2010, 1217, 348–352. [Google Scholar] [CrossRef] [PubMed]
  3. Zhang, J.; Li, X. Hydrogen bonding in the complexes formed by arsine and H-X molecules: A theoretical study. Chem. Phys. Lett. 2019, 735, 136767. [Google Scholar] [CrossRef]
  4. Burt, J.; Levason, W.; Reid, G. Coordination chemistry of the main group elements with phosphine, arsine and stibine ligands. Coord. Chem. Rev. 2014, 260, 65–115. [Google Scholar] [CrossRef] [Green Version]
  5. Green, J. Transition Metals in the Synthesis of Complex Organic Molecules. J. Am. Chem. Soc. 2010, 132, 1443. [Google Scholar] [CrossRef]
  6. Orpen, A.G.; Connelly, N.G. Structural systematics: The role of PA. sigma.* orbitals in metal-phosphorus .pi.-bonding in redox-related pairs of M-PA3 complexes (A = R, Ar, OR; R = alkyl). Organometallics 1990, 9, 1206–1210. [Google Scholar] [CrossRef]
  7. Crabtree, R.H. The Organometallic Chemistry of the Transition Metals; John Wiley & Sons, Inc.: Hoboken, NJ, USA, 2014. [Google Scholar] [CrossRef]
  8. McCleverty, J.A.; Meyer, T.J. Comprehensive Coordination Chemistry II: From Biology to Nanotechnology. J. Am. Chem. Soc. 2004, 126. [Google Scholar] [CrossRef]
  9. Treichel, P.M. Phosphine, Arsine, and Stibine Complexes of the Transition Elementes; Elsevier Scientific Publishing Co.: Amsterdam, The Netherlands, 1979; Volume 9. [Google Scholar] [CrossRef]
  10. Wilkinson, G.; Gillard, R.D.; McCleverty, J.A. Comprehensive Coordination Chemistry: The Synthesis, Reactions, Properties and Applications of Coordination Compounds; Pergamon Press: Oxford, UK, 1987; Available online: https://inis.iaea.org/search/search.aspx?orig_q=RN:19039703 (accessed on 1 November 2021).
  11. Rodríguez, M.E. Funcionalización de Ligandos Coordinados; Universidad de Coruña: Coruña, Spain, 2017. [Google Scholar]
  12. Hernández-Fernández, J. Quantification of arsine and phosphine in industrial atmospheric emissions in Spain and Colombia. Implementation of modified zeolites to reduce the environmental impact of emissions. Atmos. Pollut. Res. 2021, 12, 167–176. [Google Scholar] [CrossRef]
  13. Carrizo, D.S. Estudios Computacionales en Catálisis Homogénea con Metales de Transición: Reacción de Stille, Activación de Enlaces C-H y β-Eliminación; Universidad Nacional de Córdoba: Córdoba, Spain, 2016. [Google Scholar]
  14. Arlinghaus, R.T.; Andrews, L. Infrared spectra of the PH3, AsH3, and SbH 3-HX hydrogen bonded complexes in solid argon J. Chem. Phys. 1984, 81, 4341–4351. [Google Scholar] [CrossRef]
  15. Joaquin, H.-F.; Juan, L. Quantification of poisons for Ziegler Natta catalysts and effects on the production of polypropylene by gas chromatographic with simultaneous detection: Pulsed discharge helium ionization, mass spectrometry and flame ionization. J. Chromatogr. A 2020, 1614, 460736. [Google Scholar] [CrossRef]
  16. Kurahashi, E.; Wada, T.; Nagai, T.; Chammingkwan, P.; Terano, M.; Taniike, T. Synthesis of polypropylene functionalized with a trace amount of reactive functional groups and its utilization in graft-type nanocomposites. Polymer 2018, 158, 46–52. [Google Scholar] [CrossRef]
  17. Karol, F.J.; Jacobson, F.I. Catalysis and the Unipol Process. In Studies in Surface Science and Catalysis; Elsevier: Amsterdam, The Netherlands, 1986; Volume 25. [Google Scholar] [CrossRef]
  18. Mier, J.; Artiaga, R.; Soto, L.G. Síntesis de Polímeros. Pesos moleculares. Conformación y configuración. Elementos Estructurales con Materiales Polímeros: Ferrol; Universidad de Coruña: Coruña, Spain, 1997; pp. 11–48. [Google Scholar]
  19. Bailar, J.C.; Emeléus, H.J.; Nyholm, R.; Trotman-Dickenson, A.F. Comprehensive Inorganic Chemistry; Elsevier: Amsterdam, The Netherlands, 1973; Volume 3. [Google Scholar] [CrossRef]
  20. Nikolaeva, M.; Mikenas, T.; Matsko, M.; Zakharov, V. Effect of AlEt3 and an External Donor on the Distribution of Active Sites According to Their Stereospecificity in Propylene Polymerization over TiCl4/MgCl2 Catalysts with Different Titanium Content. Macromol. Chem. Phys. 2016, 217, 1384–1395. [Google Scholar] [CrossRef]
  21. Panchenko, V.N.; Vorontsova, L.V.; Zakharov, V.A. Ziegler-Natta catalysts for propylene polymerization—Interaction of an external donor with the catalyst. Polyolefins J. 2017, 4, 87–97. [Google Scholar] [CrossRef]
  22. Vizen, E.I.; Rishina, L.A.; Sosnovskaja, L.N.; Dyachkovsky, F.S.; Dubnikova, I.L.; Ladygina, T.A. Study of hydrogen effect in propylene polymerization on (with) the MgC12- Supported Ziegler-Natta catalyst-Part 2. Effect of Cs2 on polymerization centres. Eur. Polym. J 1994, 30, 1315–1318. [Google Scholar]
  23. Kallio, K.; Wartmann, A.; Reichert, K.-H. Reactivation of a Poisoned Metallocene Catalyst by Irradiation with Visible Light. Macromol. Rapid Commun. 2002, 23, 187–190. [Google Scholar] [CrossRef]
  24. Bahri-Laleh, N. Interaction of different poisons with MgCl2/TiCl4 based Ziegler-Natta catalysts. Appl. Surf. Sci. 2016, 379, 395–401. [Google Scholar] [CrossRef]
  25. Asynkiewicz, S.P. Reactions of organoaluminium compounds with electron donors. Pure Appl. Chem. 1972, 30, 509–522. [Google Scholar] [CrossRef]
  26. Hernández-Fernández, J. Quantification of oxygenates, sulphides, thiols and permanent gases in propylene. A multiple linear regression model to predict the loss of efficiency in polypropylene production on an industrial scale. J. Chromatogr. A 2020, 1628, 461478. [Google Scholar] [CrossRef] [PubMed]
  27. Li, Z.; Yin, Y.; Wang, X.; Tu, D.M.; Kao, K.C. Formation and inhibition of free radicals in electrically stressed and aged insulating polymers. J. Appl. Polym. Sci. 2003, 89, 3416–3425. [Google Scholar] [CrossRef]
  28. Cavallo, L.; Del Piero, S.; Ducéré, J.M.; Fedele, R.; Melchior, A.; Morini, G.; Piemontesi, F.; Tolazzi, M. Key interactions in heterogeneous Ziegler-Natta catalytic systems: Structure and energetics of TiCL4-lewis base complexes. J. Phys. Chem. C 2007, 111, 4412–4419. [Google Scholar] [CrossRef]
  29. Bahri-Laleh, N.; Nekoomanesh-Haghighi, M.; Mirmohammadi, S.A. A DFT study on the effect of hydrogen in ethylene and propylene polymerization using a Ti-based heterogeneous Ziegler-Natta catalyst. J. Organomet. Chem. 2012, 719, 74–79. [Google Scholar] [CrossRef]
  30. Correa, A.; Bahri-Laleh, N.; Cavallo, L. How well can DFT reproduce key interactions in Ziegler-Natta systems? Macromol. Chem. Phys. 2013, 214, 1980–1989. [Google Scholar] [CrossRef]
  31. Joaquin, H.-F.; Juan, L.-M. Autocatalytic influence of different levels of arsine on the thermal stability and pyrolysis of polypropylene. J. Anal. Appl. Pyrolysis 2022, 161, 105385. [Google Scholar] [CrossRef]
  32. Arshouee, G.H.; Zarand, S.M.G. Determination of Catalyst Residence Time, Heat Generation, and Monomer Conversion via Process Variables during Propylene Polymerization by a Mathematical Model. Theor. Found. Chem. Eng. 2021, 55, 140–152. [Google Scholar] [CrossRef]
  33. Hernández-Fernandez, J.; Rodríguez, E. Determination of phenolic antioxidants additives in industrial wastewater from polypropylene production using solid phase extraction with high-performance liquid chromatography. J. Chromatogr. A 2019, 1607, 460442. [Google Scholar] [CrossRef] [PubMed]
  34. Hernández-Fernández, J.; Lopez-Martinez, J.; Barceló, D. Quantification and elimination of substituted synthetic phenols and volatile organic compounds in the wastewater treatment plant during the production of industrial scale polypropylene. Chemosphere 2021, 263, 128027. [Google Scholar] [CrossRef] [PubMed]
  35. Hernández-Fernández, J.; López-Martínez, J. Experimental study of the auto-catalytic effect of triethylaluminum and TiCl4 residuals at the onset of non-additive polypropylene degradation and their impact on thermo-oxidative degradation and pyrolysis. J. Anal. Appl. Pyrolysis 2021, 155, 105052. [Google Scholar] [CrossRef]
  36. Zhang, S.; Li, B.; Lin, M.; Li, Q.; Gao, S.; Yi, W. Effect of a novel phosphorus-containing compound on the flame retardancy and thermal degradation of intumescent flame retardant polypropylene. J. Appl. Polym. Sci. 2011, 122, 3430–3439. [Google Scholar] [CrossRef]
  37. Hernández-Fernández, J.; Rayón, E.; López, J.; Arrieta, M.P. Enhancing the Thermal Stability of Polypropylene by Blending with Low Amounts of Natural Antioxidants. Macromol. Mater. Eng. 2019, 304, 1900379. [Google Scholar] [CrossRef]
  38. Bremner, T.; Rudin, A.; Cook, D.G. Melt flow index values and molecular weight distributions of commercial thermoplastics. J. Appl. Polym. Sci. 1990, 41, 1617–1627. [Google Scholar] [CrossRef]
  39. Ivin, K.J.; Rooney, J.J.; Stewart, C.D.; Green, M.L.H.; Mahtab, R. Mechanism for the stereospecific polymerization of olefins by Ziegler–Natta catalysts. J. Chem. Soc. Chem. Commun. 1978, 14, 604–606. [Google Scholar] [CrossRef]
  40. Padilla Paz, R.M. Síntesis y Estudio de Cpmplejos Organometálicos de Iridio con N-Aril-4,5-dimetilen-1,3-oxazolidin-2-onas y Complejos de Cobre con Furoiltioureas; Universidad Autónoma del estado de Hidalgo: Hidalgo, Mexico, 2006. [Google Scholar]
  41. Castro, C.A.; Eguren, L.; Korswagen, R.P. Catalizadores Ziegler-Natta utilizados para polimerizar propileno y etileno. Rev. De Química 1987, 1, 5–13. [Google Scholar]
  42. Natta, G.; Pasquon, I.; Giachetti, E. Kinetics of the stereospecific polymerization of polypropylene to isotactic polymers. In Stereoregular Polymers and Stereospecific Polymerizations; Elsevier: Amsterdam, The Netherlands, 1967. [Google Scholar] [CrossRef]
  43. Chien, J.C.W.; Bres, P. Magnesium Chloride Supported High Mileage Catalysts for Olefin Polymerization. XIII. Effect of External Lewis Base on Ethylene Polymerization. J. Polym. Sci. Part A Polym. Chem. 1986, 24, 1967–1988. [Google Scholar] [CrossRef]
  44. Bhaduri, S.; Mukhopadhyay, S.; Kulkarni, S.A. Role of titanium oxidation states in polymerization activity of Ziegler-Natta catalyst: A density functional study. J. Organomet. Chem. 2006, 691, 2810–2820. [Google Scholar] [CrossRef]
  45. Mukhopadhyay, S.; Kulkarni, S.A.; Bhaduri, S. Density functional study on the role of electron donors in propylene polymerization using Ziegler-Natta catalyst. J. Organomet. Chem. 2005, 690, 1356–1365. [Google Scholar] [CrossRef]
  46. Jensen, V.R.; Borve, K.J.; Ystenesg, M. Ziegler-Natta Ethylene Insertion Reaction for a Five-Coordinate Titanium Chloride Complex Bridged to an Aluminum Hydride Cocatalyst. J. Am. Chem. Soc. 1995, 117, 4109–4117. [Google Scholar] [CrossRef]
  47. Zakharov, I.I.; Zakharov, V.A.; Zhidomirov, G.M. Quantum chemical studies of propene, ethylene, acetylene and dihydrogen reactivity in the insertion reaction into the titanium-alkyl bond. Macromol. Theory Simul. 1996, 5, 837–843. [Google Scholar] [CrossRef]
  48. Cavallo, L.; Guerra, G.; Corradini, P. Mechanisms of Propagation and Termination Reactions in Classical Heterogeneous Ziegler−Natta Catalytic Systems: A Nonlocal Density Functional Study. J. Am. Chem. Soc. 1998, 120, 2428–2436. [Google Scholar] [CrossRef]
  49. Cheremisinoff, N.P. Handbook of Polymer Science and Technology: Synthesis and Properties; John Wiley & Sons Ltd.: London, UK, 1989. [Google Scholar]
  50. Gordy, W. A Relation between Bond Force Constants, Bond Orders, Bond Lengths, and the Electronegativities of the Bonded Atoms. J. Chem. Phys. 1946, 14, 305–320. [Google Scholar] [CrossRef]
  51. Myneni, S.C.B.; Traina, S.J.; Waychunas, G.A.; Logan, T.J. Vibrational spectroscopy of functional group chemistry and arsenate coordination in ettringite. Geochim. Cosmochim. Acta 1998, 62, 3499–3514. [Google Scholar] [CrossRef]
  52. Mowery, D.M.; Assink, R.A.; Derzon, D.K.; Klamo, S.B.; Clough, R.L.; Bernstein, R. Solid-State 13C NMR Investigation of the Oxidative Degradation of Selectively Labeled Polypropylene by Thermal Aging and γ-Irradiation. Macromolecules 2005, 38, 5035–5046. [Google Scholar] [CrossRef]
  53. Hamid, S.H. Handbook of Polymer Degradation, 2nd ed.; Marcel Dekker: New York, NY, USA, 2000. [Google Scholar]
  54. Carlsson, D.J.; Wiles, D.M. The Photooxidative Degradation of Polypropylene. Part I. Photooxidation and Photoinitiation Processes. J. Macromol. Sci. Part C Polym. Rev. 1976, 14, 65–106. [Google Scholar] [CrossRef]
  55. Rangaraj, V.M.; Singh, S.; Devaraju, S.; Wadi, V.S.; Alhassan, S.; Anjum, D.H.; Mittal, V. Polypropylene/phosphazene nanotube nanocomposites: Thermal, mechanical, and flame retardation studies. J. Appl. Polym. Sci. 2020, 137, 49525. [Google Scholar] [CrossRef]
  56. Kurt, G.; Kasgoz, A. Effects of molecular weight and molecular weight distribution on creep properties of polypropylene homopolymer. J. Appl. Polym. Sci. 2021, 138, 50722. [Google Scholar] [CrossRef]
  57. Schoolenberg, G.E.; Vink, P. Ultra-violet degradation of polypropylene: 1. Degradation profile and thickness of the embrittled surface layer. Polymer 1991, 32, 432–437. [Google Scholar] [CrossRef]
  58. Rouillon, C.; Bussiere, P.O.; Desnoux, E.; Collin, S.; Vial, C.; Therias, S.; Gardette, J.L. Is carbonyl index a quantitative probe to monitor polypropylene photodegradation? Polym. Degrad. Stab. 2016, 128, 200–208. [Google Scholar] [CrossRef]
  59. Zhang, T.; Chen, K.; Zhang, Z.; Shi, R. Quantitative relationship between melting peak temperature and carbonyl index of polypropylene during UV aging based on date fitting. IOP Conf. Ser. Mater. Sci. Eng. 2018, 322, 022016. [Google Scholar] [CrossRef]
Polymers 14 03123 g001 550
Figure 1. Diagram of the polymerization process and sampling points.
Figure 1. Diagram of the polymerization process and sampling points.
Polymers 14 03123 g001
Polymers 14 03123 g002 550
Figure 2. Arsine chromatogram.
Figure 2. Arsine chromatogram.
Polymers 14 03123 g002
Polymers 14 03123 g003a 550Polymers 14 03123 g003b 550
Figure 3. Reaction mechanism of residual AsH3 with TiCl4/MgCl2.
Figure 3. Reaction mechanism of residual AsH3 with TiCl4/MgCl2.
Polymers 14 03123 g003aPolymers 14 03123 g003b
Polymers 14 03123 g004 550
Figure 4. Infrared spectra of the catalyst with distinct levels of arsine.
Figure 4. Infrared spectra of the catalyst with distinct levels of arsine.
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Polymers 14 03123 g005 550
Figure 5. Relationship between the arsenic content in the PP and the MFI, and the variation of the Mw.
Figure 5. Relationship between the arsenic content in the PP and the MFI, and the variation of the Mw.
Polymers 14 03123 g005
Polymers 14 03123 g006 550
Figure 6. TGA and DTG of PP samples.
Figure 6. TGA and DTG of PP samples.
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Polymers 14 03123 g007 550
Figure 7. Carbonyl index of PP samples.
Figure 7. Carbonyl index of PP samples.
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Polymers 14 03123 g008 550
Figure 8. Mechanisms of reaction of peroxy radicals in arsenic complexes to form VOCs.
Figure 8. Mechanisms of reaction of peroxy radicals in arsenic complexes to form VOCs.
Polymers 14 03123 g008
Table
Table 1. Reagents for polymerization.
Table 1. Reagents for polymerization.
RunCatalyst
[kg/h]		Propylene
[TM/h]		TEAl
1
[kg/h]		Hydrogen
[g/h]		NitrogenArsine
[ppm]		Selectivity Control Agent
[mol/h]		T [°C]Pressure
[bar]
051.20.2530.017027
151.20.2530.0.0517027
551.20.2530.0.8417027
1051.20.2530.4.7317027
1 triethylaluminium co-catalyst.
Table
Table 2. Identification and sampling points.
Table 2. Identification and sampling points.
StagePointSubstanceState of OriginIdentification
FeedingAPropyleneLPGA0, A1, A5, A10
BNitrogenGasB0, B1, B5, B10
CHydrogenGasC0, C1, C5, C10
DArsineLPGD0, D1, D5, D10
ReactionEGasesInside the reactorE0, E1, E5, E10
FCatalystInside the reactorF0, F1, F5, F10
GCatalystCatalytic systemG0, G1, G5, G10
HPropyleneRecoveredH0, H1, H5, H10
DegassingIResinExits the reactorI0, I1, I5, I10
JGasesRetired in the purgeJ0, J1, J5, J10
KPolypropyleneDustK0, K1, K5, K10
Table
Table 3. Compounds determined in the degassing stage.
Table 3. Compounds determined in the degassing stage.
Compound (ppm)Point IPoint JPoint K
I0I1I5I10J0J1J5J10K0K1K5K10
AsH3000000000000
Alcohol10.150.281.5180.115.280.2100310.15.17.520.150.5
Ketone19.580.2160.1220.130.2130.1220280.74.510.631.545.5
Aldehydes13.260.1121.5242.725.291.5172270.17.111.722.321.2
Acid20.197.1210.1351.732.1161.2308425.14.523.441.533.3
CO000.21.1000.43.20000.1
CO20.11.55.511.31.22.1820.200.11.21.9
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Hernández-Fernández, J.; Guerra, Y.; Puello-Polo, E.; Marquez, E. Effects of Different Concentrations of Arsine on the Synthesis and Final Properties of Polypropylene. Polymers 2022, 14, 3123. https://doi.org/10.3390/polym14153123

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Hernández-Fernández J, Guerra Y, Puello-Polo E, Marquez E. Effects of Different Concentrations of Arsine on the Synthesis and Final Properties of Polypropylene. Polymers. 2022; 14(15):3123. https://doi.org/10.3390/polym14153123

Chicago/Turabian Style

Hernández-Fernández, Joaquín, Yoleima Guerra, Esneyder Puello-Polo, and Edgar Marquez. 2022. "Effects of Different Concentrations of Arsine on the Synthesis and Final Properties of Polypropylene" Polymers 14, no. 15: 3123. https://doi.org/10.3390/polym14153123

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Hernández-Fernández, J., Guerra, Y., Puello-Polo, E., & Marquez, E. (2022). Effects of Different Concentrations of Arsine on the Synthesis and Final Properties of Polypropylene. Polymers, 14(15), 3123. https://doi.org/10.3390/polym14153123

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