Heteroatom Chemistry
Volume 2019 (2019), Article ID 7680264, 6 pages
https://doi.org/10.1155/2019/7680264

Research Article

A Thermochemical Parameters and Theoretical Study of the Chlorinated Compounds of Thiophene

Ibrahim A. M. Saraireh,¹ Mohammednoor Altarawneh,2,3 Jibril Alhawarin,¹ and Mansour H. Almatarneh4,5

¹Department of Chemistry, Al-Hussein Bin Talal University, Ma’an, Jordan
²Department of Chemical Engineering, Al-Hussein Bin Talal University, Ma’an, Jordan
³School of Engineering and Information Technology, Murdoch University, 6150 WA, Australia
⁴Department of Chemistry, University of Jordan, Amman 11942, Jordan
⁵Department of Chemistry, Memorial University, St. John’s, Newfoundland and Labrador, Canada A1B 3X7

Correspondence should be addressed to Ibrahim A. M. Saraireh; dribrahim9997@gmail.com

Received 17 October 2018; Accepted 18 December 2018; Published 9 January 2019

Academic Editor: Mariateresa Giustiniano

Copyright © 2019 Ibrahim A. M. Saraireh et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

Abstract.

This contribution sets out to compute thermochemical and geometrical parameters of the complete series of chlorinated isomers of thiophene based on the accurate chemistry model of CBS-QB3. Herein, we compute standard entropies, standard enthalpies of formation, standard Gibbs free energies of formation, and heat capacities. Our calculated enthalpy values agree with available limited experimental values. The DFT-based reactivity descriptors were used to elucidate the site selectivity for the chlorination sequence of thiophene. The relative preference for chlorination was found to be in accord with the thermodynamic stability trends inferred based on the H scale. Calculated Fukui indices predict a chlorination sequence to ensue as follows: 2-chloro → 2,5-dichloro → 2,3,5-trichloro → 2,3,4,5-tetrachlorothiophene.

1. Introduction

Thiophene (C₄H₄S) is a heterocyclic organic compound with a five-membered ring similar to cyclopentadiene with replacement of a -CH₂- group by sulfur atom [1]. Thiophene and its derivatives can be found in some natural resources such as petroleum and coal and in several pharmacologically active compounds [2]. Thiophene has high potential for bioactivation which in some cases has been linked to toxicity [3]. Medicinal chemistry approaches to minimize the bioactivation potential of thiophenes often include substitution at the α-carbon position to provide a potential site for metabolism. Such thiophene derivative that is often used in medicinal chemistry is the α-chlorothiophene, and there are several examples of marketed drugs containing this moiety such as tioconazole, lornoxicam, and rivaroxaban [4].

Halothiophenes and their secondary products are intermediate compounds in the synthesis of drugs and plant protection agents [5]. Chlorothiophene isomers may be used in the synthesis of many important organic compounds [6–8]. Experimentally, nine isomers of chlorothiophene could be produced by chlorination of thiophene in several methods [9] and all isomers were isolable. Monochlorothiophene was formed in high percent during substitution reaction of chlorine with thiophene. Similarly [10], chlorination of 2-chlorothiophene yielded a dichlorothiophene fraction composed of high percent of 2,5-dichloro thiophene and 2,3-dichlorothiophene, 2,3-, 2,4-, and 3,4-dichlorothiophenes were formed largely by dehydrohalogenation of 2,3,4,5-tetrachlorothiolane and not by substitution. 2,5-Dichlorothiophene was formed by substitution. On the other hand 2,3,4-trichlorothiophene was prepared by low temperature chlorination and was formed largely after the chlorination by the action of alkali on 2,2,3,4,5-pentachlorothiolane. 2,3,5-Trichlorothiophene was prepared by high temperature chlonation and was formed both by the substitution of 2,5-dichlorothiophene and by the pyrolysis of pentachlorothiolane. Tetrachlorothiophene was formed both by substitution of 2,3,5-trichlorothiophene and by pyrolytic or alkaline dehydrohalogenation of 2,2,3,4,5,5-hexachlorothiolane [11, 12]. 2,5-dichlorothiophene was used in the preparation of chalcones compounds which have been evaluated for antimicrobial activity [13]. The effects of the number and the position of the chlorine atoms on the properties of the thiophene ring for the chlorothiophenes have been studied theoretically by the CBS-QB3 composite method [14]. It is well-established that this method performs very well in predicting thermochemistry in general applications pertinent to halogenated systems. In previous studies, we have demonstrated the accuracy of the CBS-QB3 methodology against analogous experimental values and calculated parameters by CBS-QB3 in these studies span kinetics reaction rate constants [15], pka values [16], and bond dissociation enthalpies [17]. The focus in this study is on acquiring standard entropies, heat capacities, enthalpy, and the free energy barrier for the addition of Cl to the ring-carbon sites at selected temperature for the optimized structures of chlorinated thiophene compounds which are calculated.

2. Computational Details

The Gaussian 09 [18] suite of programs carries out all structural optimization and energy estimations for the complete series of chlorinated congeners of thiophene at the composite chemistry model of CBS-QB3 [19]. CBS-QB3 performs structural optimization and frequency calculations at the B3LYP/6-311+G(d,p) theoretical level. This is followed by several subsequent single point energies at higher theoretical levels including MP2 and CCSD(T) methodologies. We have shown in our previous studies that the CBS-QB3 method performs very well in estimating thermos-kinetics parameters for general applications of halogenated hydrocarbons [17, 20, 21]. The DMol³ software [22] was deployed to acquire Fukui () [23] indices of electrophilic attack. The values are then used to underpin the preferred chlorination sequence of thiophene.

We compute standard via utilizing our calculated standard entropies (Table 3) and the standard entropies of elements (C, H, N, and Cl) in their standard state according to

Calculating Gibbs free energies of formation in the aqueous phase, , requires estimation of the energy of solvation, :

Standard entropies and heat capacities are computed based on vibrational frequencies and moments of inertia via the ChemRate code [24].

3. Result and Discussion

3.1. The Optimized Geometries

Optimized structures for all chlorinated isomers are presented in Figure 1. Change in the position and the extent of chlorination exerts rather minimal changes in the structural parameters when contrasted with analogous values in the unsubstituted thiophene molecule. For instance, all C-C distances in the chlorinated isomers of thiophene are within 0.007 Å. Likewise, all C-C-C and C-S-C angles in the chlorinated isomers of thiophene reside with of the corresponding angles of the thiophene molecule.

Figure 1: Optimized structures at the B3LYP/6-311+G(d,p) level of theory for chlorinated isomers of thiophene.

3.2. Sequence of Chlorination

Chlorination of thiophene occurs via electrophilic aromatic substitution (Scheme 1). These substitutions ensue by an initial electrophile addition, followed by a hydrogen atom loss from the intermediate forming the aromatic ring.

Scheme 1: Resonance stabilization of 2-substitution intermediate is greater than that of the 3-substitution intermediate.

We have previously utilized Fukui indices for electrophilic substitution to reproduce the experimentally observed halogenation patterns for chlorinated several aromatic compounds [25]. Herein, we adapt the same approach to calculate the chlorination pattern of chlorinated compounds of thiophene.

Calculated values in Figure 2 predict the chlorination sequence as follows: 2-chloro → 2,5-dichloro → 2,3,5-trichloro → 2,3,4,5-tetrachlorothiophene. This sequence of chlorination allows less repulsion between the chlorine atoms. Experimentally, chlorination of thiophene is preferred at the C-2 (α-position) of the ring. An explanation for the α-selectivity of this substitution reaction is apparent from the mechanism in Scheme 1. The intermediate that is formed by electrophile attack at C-2 is stabilized by charge delocalization to a greater degree than the intermediate from C-3 attack.

Figure 2: Chlorination sequence of thiophene predicted based on Fukui indices of electrophilic attack, (r).

3.3. Standard Enthalpies of Formation

The standard entropies, heat capacities, enthalpy, and the free energy barrier for the addition of Cl to the ring-carbon sites at selected temperature for these reactions were calculated. The results are given in Tables 1, 2, and 3. We calculated standard enthalpies of formation () based on two isodesmic reactions shown in Scheme 2.

Table 1: Values of standard entropy () and heat capacity at constant pressure () at selected temperatures for chlorinated thiophene isomers. in cal/(mol K) and (T) in cal/(mol K).

298.15K
300K
500K
800K
1000K
1500K

Thiophene
70.566
17.895
18.006
27.771
35.679
38.827
43.453

2-Chlorothiophene
77.534
21.624
21.730
26.875
37.967
40.709
44.612

3-Chlorothiophene
78.109
21.685
21.792
30.929
38.022
40.738
44.614

2,3-Dichlorothiophene
85.559
25.327
25.429
33.915
40.280
42.608
45.776

2,4-Dichlorothiophene
85.716
25.431
25.533
33.995
40.320
42.630
45.781

2,5-Dichlorothiophene
85.860
25.354
25.455
33.881
40.257
42.595
45.775

3,4-Dichlorothiophene
85.377
25.379
25.483
34.024
40.344
42.645
45.784

2,3,4-Trichlorothiophene
92.799
29.059
29.158
37..041
42.625
44.532
46.956

2,3,5-Trichlorothiophene
93.197
29.067
29.163
36.968
42.573
44.497
46.942

2,3,4,5-Tetrachlorothiophene
100.252
32.697
32.789
40..005
44.875
46.395
48.114

Table 2: (kcal/mol) for chlorinated thiophene isomers.

Thiophene
+ 52.200

2-Chlorothiophene
+ 46.507

3-Chlorothiophene
+ 47.330

2,3-Dichlorothiophene
+ 45.846

2,4-Dichlorothiophene
+ 45.077

2,5-Dichlorothiophene
+ 44.403

3,4-Dichlorothiophene
+ 45.395

2,3,4-Trichlorothiophene
+ 41.334

2,3,5-Trichlorothiophene
+ 43.119

2,3,4,5-Tetrachlorothiophene
+ 40.366

Table 3: The calculated properties of chlorinated thiophene at 298 K: the Gibbs free energies in the gas phase (g), the Gibbs free energies for solvation (), and the standard and relative Gibbs free energies in aqueous phase (aq). All are in kcal/mol.

G(g)
Δ
(aq)

Thiophene
-40.656
-2.028
-42.683

2-Chlorothiophene
-48.723
-1.949
-50.670

3-Chlorothiophene
-51.070
-2.272
-53.342

2,3-Dichlorothiophene
-56.867
-2.144
-59.011

2,4-Dichlorothiophene
-57.083
-1.936
-59.019

2,5-Dichlorothiophene
-54.600
-1.636
-56.236

3,4-Dichlorothiophene
-60.464
-2.506
-62.970

2,3,4-Trichlorothiophene
-68.030
-2.128
-70.158

2,3,5-Trichlorothiophene
-66.363
-1.551
-67.914

2,3,4,5-Tetrachlorothiophene
-74.512
-1.511
-76.023

Scheme 2: Hypothetical reaction between thiophene and chlorobenzene.

Based on the of chlorobenzene (13.01 ± 0.50 kcal/mol) [26], benzene (19.8 ± 0.2 kcal/mol) [27], thiophene (52.20 kcal/mol) [28], and the for the selected chlorothiophene compounds were estimated using CBS-QB3 along with the selected isodesmic reaction Scheme 2 (Table 2).

Similarly, the for the 2-chlorothiophene calculated at 46.507 kcal/mol is less than 3-chlorothiophene isomer (47.330 kcal/mol). This indicates that the 2-chlorothiophene isomer is more stable than the 3-chlorothiophene isomer. Along the same line of discussion, the of 2,5-dichlorothiophene (44.403 kcal/mol) is less than the other dichloro isomers. This infers that the 2,5-dichloro isomer is more stable than the other dichloro isomers. Such finding is attributed the S-atom that separates between the two chlorine atoms in thiophene. These positions are denoted as α-positions with respect to sulfur atom. Obviously, higher thermodynamic stability for this isomer stems from a smaller enthalpic penalty associated with the repulsion between the chlorine atoms.

It is noticed that the heat of formation of the chlorothiophene compounds decreases with the addition of the number of chlorine atoms. To the contrary and as expected, entropies (Sο) and the heat capacities at constant pressure () for chlorothiophene compounds increase with the addition of chlorine atoms. Table 1 lists calculated standard entropies and heat capacities at selected temperatures.

3.4. Gaseous and Aqueous Gibbs Free Energies of Formation

The polarizable continuum model (PCM) [29] is used to estimate values of . This approach utilizes a continuum surface charge formalism that incorporates a robust and a smooth perturbing reaction field. Values of are modestly negative indicating an exothermic nature for dissolving of pyridine and its chlorinated compounds in water. Values of randomly vary among isomers but reside in the narrow range of -1.5 and ~ 2.25 kcal/mol. Nevertheless, no conclusive observation can be drawn regarding the effect of degree and pattern of chlorination on computed values of . Values of and highlight a highly spontaneous nature for the formation of chlorinated compounds of thiophene in the gas phase as well as in the aqueous medium. Water is a polar solvent so the solvation effect depends on the dipole moments of chlorinated thiophenes: 3,4-dichlorothiophene should have the greatest dipole moment and, thus, the greatest interaction with polar solvent. This explains why this isomer acquires lower G(aq) among other dechlorinated congeners. Calculating polarizability effects on the selected chlorinated thiophene using various other solvents will be investigated in a due course.

4. Conclusion

The thermochemical and the optimized geometrical parameters are presented for the selected chlorothiophene isomers. Isodesmic reactions were used to estimate standard enthalpies of formation. The standard enthalpies of formation decrease as the degree of chlorination increases in both the gaseous and aqueous media. No trend can be deduced with respect to the effect of degree and pattern of chlorination on the computed solvation energies. Similarly, geometries of chlorinated isomers of thiophene exhibit to a large extent the analogous structural parameters in the thiophene molecule. The degree and pattern of chlorination indices a minor in.

Data Availability

The data used to support the findings of this study are included within the article.

Conflicts of Interest

The authors declare that they have no conflicts of interest.

Acknowledgments

This study has been supported by a grant of computing time from the Australian Centre of Australian national Computational Infrastructure (NCI) in Canberra.

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