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Intermolecular Interactions in Functional Crystalline Materials: From Data to Knowledge

Crystals 2019, 9(10), 506; https://doi.org/10.3390/cryst9100506

Article
Noncovalent Bonds, Spectral and Thermal Properties of Substituted Thiazolo[2,3-b][1,3]thiazinium Triiodides
South Ural State University (National Research University) 76, Lenin Prospect, Chelyabinsk 454080, Russia
*
Author to whom correspondence should be addressed.
Received: 31 August 2019 / Accepted: 23 September 2019 / Published: 28 September 2019

Abstract

:
The interrelation between noncovalent bonds and physicochemical properties is in the spotlight due to the practical aspects in the field of crystalline material design. Such study requires a number of similar substances in order to reveal the effect of structural features on observed properties. For this reason, we analyzed a series of three substituted thiazolo[2,3-b][1,3]thiazinium triiodides synthesized by an iodocyclization reaction. They have been characterized with the use of X-ray diffraction, Raman spectroscopy, and thermal analysis. Various types of noncovalent interactions have been considered, and an S…I chalcogen bond type has been confirmed using the electronic criterion based on the calculated electron density and electrostatic potential. The involvement of triiodide anions in the I…I halogen and S…I chalcogen bonding is reflected in the Raman spectroscopic properties of the I–I bonds: identical bond lengths demonstrate different wave numbers of symmetric triiodide vibration and different values of electron density at bond critical points. Chalcogen and halogen bonds formed by the terminal iodine atom of triiodide anion and numerous cation…cation pairwise interactions can serve as one of the reasons for increased thermal stability and retention of iodine in the melt under heating.
Keywords:
chalcogen bond; halogen bond; triiodide anion; Raman spectroscopy; thermal analysis; thiazolo[2,3-b][1,3]thiazinium salts

1. Introduction

A great number of relatively strong noncovalent interactions in N- and S-heterocyclic polyiodides, such as halogen and chalcogen bonds, can not only promote the stability and diversity of possible polyiodide organization, but help in the organization of anion transport, chiral synthesis, and organocatalysis [1]. For electrostatically driven noncovalent bonds [2], the electrophilic site—the electron deficient region on the extension of the covalent bond of one atom—is orientated towards the nucleophilic fragment in another molecule. The International Union of Pure and Applied Chemistry (IUPAC) definition of halogen [3] and chalcogen bonds [4] is based on a series of quantitative features from structural, theoretical and spectral points of view. The development of noncovalent bond characterization in crystals includes the analysis of distribution features of the electrostatic potential [5], the quantum theory of atoms in molecules (QTAIM) methodology [6], electron localization function (ELF) [7], Laplacian of electron density [8], facilities of reduced density gradient (RDG) and analysis using the noncovalent interactions (NCI) method [9].
Variation of the N- and S-containing heterocyclic cations is useful for the investigation of bonding properties in organic polyiodide crystals. The chemistry of polyhalides has attracted particular attention due to the vast diversity of applicable properties related to the ability of halogens to form different types of contacts [10,11,12,13,14,15]. Polyiodides represent an absolute majority among polyhalide structures [16,17,18,19,20,21]. The interest in polyiodide derivatives is based on their enormous structural diversity of packing motives resulting in the formation of anionic ribbons, layers, channels and sheets [22,23,24]. The intense development of semiconductor [25,26,27,28] and nonlinear optical materials [29] based on polyiodides [30] necessitates obtaining and comprehensively investigating new molecular and crystal structures with specific properties. Structural investigation of the polarization effect or charge transfer in ionic complexes of thioamides with iodine is quite useful for explaning of the activity of some anti-thyroid drugs and antibiotics in vivo [31,32,33,34,35,36]. In all cases, the specific moiety responsible for biological activity is the released diiodine. The possibility of binding and releasing iodine from complex polyiodide structures finds its practical application in water disinfection [37] and the sorption of radioactive isotopes of iodine, such as I-131, and radiolabeling in vivo [38]. The particular significance of I3–/I·I2 interconversion is reflected in the tasks of the novel design of ionic liquids and iodine-containing solid electrolytes for dye-sensitized solar cells (DSSC) [39].
The use of such heterocyclic systems as thiazolo[2,3-a]isoquinolinium cations [40] is very promising in this regard. Syntheses of the related systems, such as 2H-benzo[4,5]thiazolo[2,3-b][1,3]thiazin-5-ium, are superficially described in the literature [41], and only a few examples of 3,5,6,7-tetrahydro-2H-thiazolo[2,3-b][1,3]thiazin-4-ium synthesis and transformation have been described [42,43,44] in the context of their biological activity.
The determination of crystal structure in polyiodide systems is highly necessary because of the ability of polyiodides to form mixtures of different compositions, to absorb excess iodine in a precipitate, and to form a melt or release iodine under storage conditions. Raman spectroscopy has earned a reputation as an extremely sensitive method [45] capable of distinguishing a variety of bonding peculiarities in the polyiodide anion [46]. It reliably characterizes polyiodides with various organic or inorganic cations, revealing typical structural units, such as the triiodide anion (100–120 cm−1), bound iodine (140–180 cm−1), and the pentaiodide anion (140–160 cm−1) [30]. The role of thermal analysis is very important in the field of iodophoric materials and DSSC device development, where the questions of thermal stability, features of source decomposition, and iodine release are of particular importance [47].
Sometimes, for the S…I interactions in N- and S-heterocyclic polyiodides, the main question is which atom delivers the electrophilic site for bonding. If the I atom acts as the electrophilic site provider, we can conclude that this is a halogen bond. If the S atom delivers the electrophilic site, then it is a chalcogen bond. Thus, the relatively strong and charge-assisted S…I interactions in organic polyiodide crystals can be interpreted as either halogen or chalcogen bonds depending on the electron density distribution and mutual orientation of their electrophilic and nucleophilic sites. In order to figure out how the polarization effect or charge redistribution are directed, it is important to understand which atom donates electrons and which one delivers the electrophilic site for bonding. The categorization of chalcogen and halogen bonds in debatable cases can be performed using previously suggested [48] electronic criterion: “along the line between bound atoms, the minimum of electrostatic potential is always located from the side of nucleophilic site; the minimum of electron density is closer to electrophilic site provider”.
Our research is focused on a series of thiazolo[2,3-b][1,3]thiazinium triiodides and on the study of how the spectral properties and thermal stability of these crystals are influenced by the type and features of the S…I noncovalent bond.

2. Materials and Methods

2.1. Synthesis

Thiazolo[2,3-b][1,3]thiazin-5-ium cations of compounds 2a–c (Figure 1) are formed via a halocyclization reaction by the action of the iodine molecule on an unsaturated bond of S-allylic or S-butenylic substituents. The compounds 3-iodo-4-phenyl-3,4-dihydro-2H-benzo[4,5]thiazolo[2,3-b][1,3]thiazin-5-ium (2a) and 4-(iodomethyl)-3,4-dihydro-2H-benzo[4,5]thiazolo[2,3-b][1,3]thiazin-5-ium triiodides (2b) were obtained for the first time. Compounds 2a,b with aromatic systems in their structures crystallized faster than triiodide 2c with a partially unsaturated cation. High quality crystals of compound 2c were obtained in the mixture with a corresponding monoiodide only after recrystallization.
The iodine solution was prepared as follows: anhydrous dioxane and CH2Cl2 were refluxed for half an hour with solid iodine. The solution was decanted from an excess of iodine and cooled. Te concentration of iodine was determined by titration with sodium thiosulphate solution in three replicates. The resulting concentration of iodine in dioxane was 73.9 ± 0.05 mg/mL, and 50.5 ± 0.05 mg/mL in CH2Cl2.
Benzothiazole-2-thione (2 g; 12 mmol) was dissolved in 20 mL i-PrOH with 12 mmol i-PrONa; then, 12 mmol alkenyl bromide (cinnamyl chloride or 4-bromobut-1-ene) was added dropwise. The mixture was stirred for 12 h at 298 K and filtered. The solution was diluted with 50 mL of water and extracted with three portions of CH2Cl2 (50 mL, 25 mL, and 25 mL). The extracts were combined, washed with 20 mL 5% H2SO4, 15 mL distilled water, and dried over CaCl2. The solvent was evaporated under reduced pressure, giving compounds 1a,b in the form of yellow oil.
The compound 2-(cinnamylsulfanyl)benzo[d]thiazole (1a) was analyzed by 1H NMR (CDCl3, ppm): 7.90 (d, J = 8.2 Hz, HAr); 7.74 (d, J = 7.9 Hz, HAr); 7.44–7.38 (m, HAr); 7.38–7.32 (m, 2HAr); 7.31–7.26 (m, HAr); 7.25–7.20 (m, HAr); 6.70 (d, J = 15.7 Hz, =CH–); 6.37 (dt, J = 15.0, 7.3 Hz, =CH–); 4.17 (2H, d, J = 7.3 Hz, –CH2–). It was also analyzed by 13C NMR (dimethyl sulfoxide-d6 (DMSO-d6), ppm): 166.21; 153.06; 136.31; 135.25; 134.27; 128.54 (2C); 127.87; 126.45 (2C); 126.04; 124.26; 123.45; 121.51; 120.96; 36.06. Elemental analysis calc. (%) for C16H13NS2: C, 67.81; H, 4.62; N, 4.94; found: C, 67.60; H, 4.71; N, 4.88.
The compound 2-(butenylsulfanyl)benzo[d]thiazole (1b) was analyzed by 1H NMR: (CDCl3, ppm): 7.86 (m, HAr); 7.75 (m, HAr); 7.41 (m, HAr); 7.29 (m, HAr); 5.89 (m, =CH); 5.13 (2H, m, =CH2); 3.43 (2H, t, J = 7.3 Hz, SCH2); 2.59 (2H, m, –CH2–). 13C NMR (DMSO-d6, ppm): 166.81; 153.28; 135.67; 135.18; 125.97; 124.14; 121.46; 120.90; 116.92; 33.31; 32.71. Elemental analysis calc. (%) for C11H11NS2: C, 59.69; H, 5.01; N, 6.33; found: C 59.60, H 5.15, N 6.35. The compound 2-(3-methylbutenyl)sulfanyl-4,5-dihydrothiazole (1c) was obtained as described elsewhere [49].
For the compound 3-iodo-4-phenyl-3,4-dihydro-2H-benzo[4,5]thiazolo[2,3-b][1,3]thiazin-5-ium triiodide (2a), compound 1a (1 mmol) was dissolved in 1 mL anhydrous CH2Cl2, and 7.11 mL of a solution of iodine (50.5 ± 0.05 mg/mL) was added under stirring. The resulting mixture was kept at room temperature for 4 days. Dark brown crystals were filtered and dried in vacuo (yield 0.46 g, 98%). It was analyzed by 1H NMR (DMSO-d6, ppm): 8.46–8.42 (m, HAr); 7.90–7.84 (m, HAr); 7.78–7.69 (m, 2HAr); 7.50–7.43 (m, HAr); 7.38–7.24 (m, HAr); 7.01 (1H, s, 4-H); 5.69 (1H, dd, J = 5.9, 3.0 Hz, 3-H); 3.70 (1H, dd, J = 14.6, 3.4 Hz, 2-H); 3.40 (1H, dd, J = 14.6, 2.8 Hz, 2-H) and 13C NMR (DMSO-d6, ppm): 175.96; 140.67; 135.42; 129.60 (2C); 129.50; 129.18; 128.24; 127.43; 126.15 (2C); 124.53; 114.67; 66.33; 33.78; 17.19. Elemental analysis calc. (%) for C16H13I4NS2: C, 24.29; H, 1.66; N, 1.77; found: C, 24.31; H, 1.62; N, 1.83.
For the compounds 4-(iodomethyl)-3,4-dihydro-2H-benzo[4,5]thiazolo[2,3-b][1,3]thiazin-5-ium triiodide (2b) and 6-iodo-5,5-dimethyl-3,5,6,7-tetrahydro-2H-thiazolo[2,3-b][1,3]thiazin-4-ium triiodide (2c): compounds 1b,c (1 mmol) were dissolved in 0.8 mL anhydrous dioxane, and 7.35 mL of a solution of iodine (73.9 ± 0.05 mg/mL) was added under stirring. The resulting mixture was kept at room temperature for 19 days (2b) and 8 days (2c).
For 4-(iodomethyl)-3,4-dihydro-2H-benzo[4,5]thiazolo[2,3-b][1,3]thiazin-5-ium triiodide (2b): dark brown crystals were filtered and dried in vacuo (yield 0.6 g, 91%); analysis by 1H NMR (DMSO-d6, ppm): 8.34 (d, J = 7.7, HAr); 8.12 (d, J = 8.5 Hz, HAr); 7.89 (t, J = 7.9 Hz, HAr); 7.72 (t, J = 7.7 Hz, HAr); 5.58–5.51 (1H, m, 5-CH); 3.76–3.66 (2H, m, CH2I); 3.65–3.57 (2H, m, 3-CH2); 3.05–2.96 (1H, m, 4-CH2); 2.49–2.41 (1H, m, 4-CH2) and 13C NMR (DMSO-d6, ppm):: 173.63; 136.67; 126.58; 125.55; 124.89; 121.83; 119.48; 112.87; 53.15; 30.11; 21.41. Elemental analysis calc. (%) for C11H11I4NS2: C, 18.12; H, 1.52; N, 1.92; found: C, 18.10; H, 1.60; N, 1.89.
For 6-iodo-5,5-dimethyl-3,5,6,7-tetrahydro-2H-thiazolo[2,3-b][1,3]thiazin-4-ium triiodide (2c): the solvent was decanted and dark brown crystals with a matte surface (0.43 g) were isolated and dried in vacuo. A portion of the crystals (0.23 g) was recrystallized from a 5 mL mixture of i-PrOH – DMF (N,N-Dimethylformamide) (3:2). The mixture of small brown and yellow crystals (0.15 g) was filtered and dried in vacuo (Figure S1, see Supplementary Materials). The crystal structure of the brown prismatic crystals (2c) was determined using single crystal X-ray diffraction. The impurity of the yellow prismatic crystals, which should presumably relate to the corresponding monoiodide, was separated manually under a microscope, but still did not prove suitable for X-ray diffraction experiments (Figure S1).

2.2. X-ray Diffraction Refinement

X-ray diffraction study of single crystals 2a–c was carried out with a Bruker D8 QUEST diffractometer (Mo-Kα radiation, λ = 0.71073 Å, graphite monochromator). Collection, handling of data and refinement of the unit cell parameters, as well as accounting for absorption, were carried out using the SMART and SAINT-Plus programs [50]. All calculations were performed using SHELXTL/PC [51] and OLEX2 [52] software. The structure was solved by direct method and refined by the method of least squares in the anisotropic approximation for non-hydrogen atoms. Crystal data and structure refinement parameters can be found in Table 1. A full list of bond lengths and valence angles are shown in Tables S1 and S2. Full crystallographic data for the compounds can be obtained free of charge from The Cambridge Crystallographic Data Centre (CCDC) (1829960 (2a), 1589820 (2b), 1589819 (2c)).

2.3. Sample Characterization

The 1H NMR and 13C NMR spectra were recorded on a Bruker Avance-500 500 and 126 MHz apparatus (tetramethylsilane as an internal standard). The elemental compositions were determined with a Carlo Erba CHNS-O EA 1108 analyzer. Raman spectra were obtained with a NTEGRA Spectra spectrometer using a 632.8 nm line of the He–Ne+ laser for spectra excitation. The laser power on the sample surface was about 0.2 μW. We had to take into consideration that due to decreased thermal stability of higher polyiodides [53], the laser power should be thoroughly controlled in order to avoid decomposition under laser explosion. The thermal analysis data have been obtained in the temperature range of 25–700 °C using Netzsch STA F1 equipment at 10 K/min-1 heating rates in corundum crucibles in an air atmosphere. The masses of the analyzed samples were 2.0–2.2 mg.

2.4. Theoretical Calculations

Periodic Kohn–Sham calculations were performed in the CRYSTAL17 program package [54], employing the B3LYP exchange-correlation functional. K-point sampling was done using a Monkhorst–Pack grid of 8 × 8 × 8. The modified DZVP basis set was used for iodine atoms [55], and the 6-31G** Gaussian type basis sets were used for the C, H, N and S atoms from [56]. Calculations of the electron localization function (ELF) [7] distribution in the planes, in which the S...I interactions lay, were performed using the TOPOND program [57]. The values of the electron density (ED) and electrostatic potential (ESP) along the line between the S and I atoms were derived due to the additional output procedure in TOPOND approximating the interatomic line by 200 points.

3. Results and Discussion

3.1. Structural Characterization of Compounds 2a–c

The crystal structures of compounds 2a,b belong to the triclinic crystal system. The crystallographic cell consists of two ionic pairs of 2H-benzo[4,5]thiazolo[2,3-b][1,3]thiazin-5-ium cations with triiodide anions. Compound 2c crystallizes in a monoclinic lattice with four ionic pairs of 3,5,6,7-tetrahydro-2H-thiazolo[2,3-b][1,3]thiazin-4-ium cations with triiodide anions (Figure 2). The summary of geometric parameters of the S...I interactions and bond lengths within triiodide anions can be found in Table 2.

3.2. Noncovalent Bonds Formed by Triiodide Anions: Electron Density Calculations

In crystal 2a, there is a typical halogen bond between the terminal iodine atom I4 of the triiodide anion and a covalently bound iodine atom I5 as part of the CH–I fragment. Both the I4 and I2 atoms of the triiodide anion in crystal 2a form the chalcogen bonds with S atoms of the heterocyclic cation. In the triiodide anion of crystal 2b, both terminal atoms form two S…I interactions with almost identical distances, but they differ in their C–S…I and S…I–I angle values (Table 2); the central I1 and terminal I2 atoms are also involved in the I1…H9 and I2…H9 hydrogen bonds. Crystal structure 2c represents a case of a typical chalcogen bond where the C8…S2–I3 angle tends to 180° and S2–I3–I1 is nearly a right angle, so that the mutual orientation of the electrophilic site of S2 and the nucleophilic region of I3 fits in the best way. Note that the terminal I atoms in the triiodide anions of 2c are involved in multiple noncovalent interactions, among which the most significant are chalcogen bonds S4…I3, S3…I8, S1…I6, S2…I1 and halogen bond I3…I5 with iodine atom I5 in the organic cation.
The representation of regions with a concentration and depletion of electron pairs in molecules and crystals can be done using the electron localization function (ELF) [7]. This function is dimensionless and is normalized from 0 to 1, where the value 0.5 corresponds to the case of uniformly distributed one-electron gas. It is particularly interesting in the case of halogen atoms, as it is known that their electron concentration regions form the belt in the equatorial part of an atom [58]. ELF for I atoms in the triiodide anions (Figure 3) clearly reveals the regions of electron accumulation (shown in orange) and electrophilic sites—regions of electron depletion on the extension of the I–I bond. However, for the bound S atom, the electrophilic site region is not always clearly seen in ELF, because it can be camouflaged by the electron concentration region that give a pronounced projection of high ELF values onto the considered plane of atomic interactions. This fact complicates the identification of the orientation of the bound S and I atoms. Accordingly, in such a case, we have applied the electronic criterion [48] that allows us to identify the atom (S or I) that has provided the electrophilic site and defined the name of interaction; in our case, it is either a halogen or chalcogen bond. The examples of the main considered S…I interactions in the studied crystals are presented in Figure 3 and Figure 4.
Let us consider the S…I and other interactions in the studied crystals from the calculated electron density and electrostatic potential point of view as this approach has already been proven to be demonstrative [59,60]. Figure 4 illustrates the examples of S…I chalcogen bonds in the considered crystals as well as the verification of non-covalent bonding type based on the electronic criteria. Within QTAIM [6], a zero-flux condition of the gradient vector field of electron density defines the boundaries of chemically bonded atoms, while basin boundaries in the electrostatic potential demarcate electrically neutral atomic fragments [61]. The map of the gradient field of electron density (Figure 4) allows us to recognize the boundaries of atomic basins. If this map is superimposed on the map of electrostatic potential distribution, it can be seen that the boundaries of electrically neutral atoms located using electrostatic potential do not coincide with the boundaries of atomic basins in electron density. This means that the fraction of electrons formally belonging to I atoms are attracted to S nuclei along the highlighted directions. This is the general feature of chalcogen bonding. The images in Figure 4 are accompanied by the bond critical points (bcp) with values of electron density given in Table S3.
As a simplification, the order of electron density and electrostatic potential minima along the S…I line can give a clue about the localization of the electrophilic site for typical and unobvious cases of halogen/chalcogen bonding. In this case, the formulation of previously suggested electronic criterion becomes more demonstrative. For the S1…I4 (2a), S2…I2 (2b) and S4…I3 (2c) bonds in Figure 5, the minima of electrostatic potential (ESP) are located at the side of the I atoms donating electrons; the minima of electron density (ED) are placed closer to the S atoms which deliver their electrophilic site for noncovalent bonding. The arrows in Figure 5 show the direction in which the electron density of the I atom is attracted to the electrophilic site of the S atom. Thus, for all the cases of illustrated I…S noncovalent bonds in 2a–2c, we ascribe such interactions to a chalcogen bonding.

3.3. Raman Spectroscopy Data

Experimental Raman spectra of the studied crystals are presented in Figure 6. On the spectrum of crystal 2c, we clearly see two overlapping bands corresponding to the two symmetrically independent triiodide anions in the crystallographic cell. As both of them are symmetric, we see only the band of symmetric stretching vibration of the triiodide anion at 112.1 cm−1 and 113.7 cm−1 and do not see the band of antisymmetric vibration, usually observed in the range of 120–140 cm−1 [30].
The spectra of crystals 2a and 2b are very similar and have weak bands at 138 cm−1, 149 cm−1 and 168 cm−1, which are not attributed to the anionic vibrations and relate to libration and deformational vibrations of the tricyclic dihydrobenzothiazolo[2,3-b]thiazin-5-ium system. The intense triiodide vibration bands are located at 118 cm−1 (2a) and 115 cm−1 (2b).
The correlation between the I–I bond lengths in the triiodide anion and the observed experimental wavenumbers of symmetric vibration is not so clear and evident as in case of iodine complexes [62,63]. For example, one of the triiodide anions in the crystal 2c has the same bond length as in 2a (2.9170 Å), but its wavenumber is much lower: 113 cm−1 (2c) and 118 cm−1 (2a), respectively. Such a spectral difference may reveal the effects that are beyond the geometric contribution on the level of bond length analysis and may be due to the effect of noncovalent interactions and crystal surrounding. Thus, as the isolated triiodide in 2c demonstrates a lower wavenumber, it has weaker I–I bonding within the triiodide anion in comparison to the anion in crystal 2a, demonstrating the band at 118 cm−1.
Such features of bonding strength in triiodide anions according to spectral data are also reflected in quantum-topological analysis of electron density. The electron density value at the bond critical point of the I–I bond in the triiodide anion is slightly higher in crystal 2a (0.0433 a.u.) than in crystal 2c (0.0419 a.u.), although the calculated equilibrium distances in these structures are identical (Table 2).
This fact is in agreement with the experimental spectral data and electron density values at the I–I bond critical point. Thus, the combination of experimental Raman characteristics together with calculated electron density descriptors can enrich the understanding of bond properties within the triiodide anion beyond the geometric approach based on bond length analysis.

3.4. Thermal Analysis Data

Thermoanalytical curves of TG-DSC analysis for crystals 2a–c are presented in Figure 7. The summary of the decomposition characteristics can be found in Table 3. All samples demonstrate multistep decomposition and rather high thermal stability for polyiodides; decomposition in all cases starts above 150 °C.
We can attempt to compare thermal decomposition and melting temperatures in the series of heterocyclic derivatives with the thiazolo-thiazinium fragment and with the same anion composition in order to try and find some trends due to differences in noncovalent interactions in the analyzed structures. A comparison of the data listed in Table 2 and Table 3 shows that melting points decrease in the row 2a > 2b > 2c (Table 1). The structural complexity of cations reduces in the order 2a – 2b – 2c from the tricyclic system with the voluminous phenyl substituent (2a) to the same tricyclic system but with the small –CH2I substituent (2b) to the bicyclic thiazolo-thiazinium system (2c), leading to a lower melting point for structure 2c.
All studied triiodides tend to decompose only in the melt (no mass loss is observed before the melting point), although here the universal trend is not so evident: structure 2b demonstrates remarkably high thermal stability (222 °C, almost a 100 °C stability range of the melt), which is significantly higher than that for the other two structures. This fact may be due to the existence of four S…I interactions involving both the terminal iodine atoms of triiodide anion in 2b, organized in such a way that the anion is trapped into the cage of four neighboring organic cations (Figure 3b). This fact can lead to a higher retention of iodine in the melt, as typically the first decomposition stage of polyiodides usually includes the loss of I2 from the triiodide anion [64,65]. Similar conclusions concerning melting and decomposition of crystals with C–Se…O/N chalcogen bonds were found in a recent study [66].
The crystal structures of compounds 2a and 2c are similar to the zigzag-like location of triiodide anions, while the crystal structure of 2b demonstrates layered packing of organic cations, as the benzothiazolo-thiazinuim cycle is flatter than the corresponding thiazolo-thiazinium and especially than phenyl-substituted 2a. Such layered organization in crystal 2b can lead to more effective capsulation of triiodide anions in the cage of the cations, which can be one of possible reasons for comparatively higher retention of iodine in the melt in the row of triiodides 2a – 2b – 2c. Based on quantum-topological analysis of the electron density properties (Tables S3 and S4) and thermal analysis data, we can make some inferences. Firstly, both triiodides in structure 2b are relatively weakly bound with crystalline surrounding; the only rather strong chalcogen bond S…I (3.7208 Å, the value of electron density at the bond critical point (rbcp) = 0.008 a.u.) dominates. Secondly, in structure 2a, we observe a moderate number of bond critical points but only for one symmetrically independent triiodide anion. The other is weakly bound to the crystal surrounding. Thirdly, in structure 2c, the numerous weak I…H interactions are formed with each of the triiodide anions; one relatively short and strong I…H hydrogen bond (2.8940 Å, (rbcp) = 0.0114 a.u.) stands out from all others. Chalcogen S…I and halogen I…I bonds between the cation and anion are also observed. In general, the 2a > 2b > 2c melting point order is reversed for the overall density in the bond critical points of cation…cation (H…H, C…I, S…H, C…C) interactions.

4. Conclusions

The synthesized crystal structures of 2H-benzo[4,5]thiazolo[2,3-b][1,3]thiazin-5-ium and 3,5,6,7-tetrahydro-2H-thiazolo[2,3-b][1,3]thiazin-4-ium triiodides were characterized using single crystal X-ray diffraction, Raman spectroscopy, and thermal analysis. The type of noncovalent bonds were described on the basis of periodic quantum-chemical calculations revealing cation…anion chalcogen S…I bonds and halogen I…I bonds. In the cases of ambiguous mutual orientation of noncovalently bound atoms, the electronic criterion of the disposition of electron density and electrostatic potential minima was used; all considered S…I interactions were categorized as chalcogen bonds. Raman spectra and local properties of electron density allowed us to reveal the influence of noncovalent bonds on the properties of triiodide anions with equal bond length: the more bound iodine atoms was the reason for a stronger I–I bond within the triiodide anion. The thermal analysis data showed that the layered packing of benzothiazolo-thiazinium triiodide promoted effective capsulation of triiodide anions due to hydrogen and chalcogen bonding and might act as a stabilizing factor, providing comparatively higher thermal stability and iodine retention in the melt.

Supplementary Materials

The following are available online at https://www.mdpi.com/2073-4352/9/10/506/s1, Table S1: Bond lengths for triiodides 2a, 2b and 2c, Table S2: Bond angles for triiodides 2a, 2b and 2c, Figure S1: Crystal habit of triiodide 2c (ruby red) and corresponding monoiodide (light yellow) under 4× microscope magnification, Table S3: Local properties at bond critical points (bcp) of noncovalent interactions formed by triiodide anions in 2a, 2b and 2c crystals, Table S4: Local properties at bond critical points of noncovalent interactions formed by organic cations in 2a, 2b and 2c.

Author Contributions

Conceptualization, E.B.; Funding acquisition, D.K., V.S. and E.B.; Investigation, I.Y., N.T. and V.S.; Methodology, E.B.; Project administration, D.K. and E.B.; Resources, N.T.; Supervision, D.K. and E.B.; Validation, I.Y. and E.B.; Visualization, I.Y. and E.B.; Writing—original draft, I.Y., N.T.; Writing—review and editing, E.B.

Funding

The work was supported by The Government of Russian Federation decree №211, agreement № 02.A03.21.0011 and by the Ministry of Education and Science of the Russian Federation: grant 4.9665.2017/8.9 (N.T. and D.K.), grant 4.6151.2017/8.9 (V.S.) and 4.1157.2017/4.6 (I.Y. and E.B.).

Conflicts of Interest

The authors declare no conflict of interest.

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Figure 1. Iodocyclization of compounds 1a–c resulting in corresponding triiodides 2a–c.
Figure 1. Iodocyclization of compounds 1a–c resulting in corresponding triiodides 2a–c.
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Figure 2. Crystal packing of 2a (a); 2b (b) and 2c (c) with thermal ellipsoids of 50% probability, view along the b crystallographic axis.
Figure 2. Crystal packing of 2a (a); 2b (b) and 2c (c) with thermal ellipsoids of 50% probability, view along the b crystallographic axis.
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Figure 3. Electron localization function (ELF) distribution in S…I motives in the structures (a) 2a (plane I4-–I2…S2); (b) 2b (plane I1–I2…S2); and (c) 2c (plane I3–I2…S4).
Figure 3. Electron localization function (ELF) distribution in S…I motives in the structures (a) 2a (plane I4-–I2…S2); (b) 2b (plane I1–I2…S2); and (c) 2c (plane I3–I2…S4).
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Figure 4. ORTEP diagrams of crystal structures illustrating the typical S…I chalcogen bond (on top); on bottom: gradient fields, atomic basins and bond critical points of electron density (red lines and points), electrostatic potential distributions (blue lines) for typical chalcogen bonds (a) 2a (plane I4––I2…S2); (b) 2b (plane I2–I1…S2); and (c) 2c (plane I3–I2…S4).
Figure 4. ORTEP diagrams of crystal structures illustrating the typical S…I chalcogen bond (on top); on bottom: gradient fields, atomic basins and bond critical points of electron density (red lines and points), electrostatic potential distributions (blue lines) for typical chalcogen bonds (a) 2a (plane I4––I2…S2); (b) 2b (plane I2–I1…S2); and (c) 2c (plane I3–I2…S4).
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Figure 5. One-dimensional distributions of electron density (ED) and electrostatic potential (ESP) functions (a.u.) along the S…I chalcogen bonds in 2a (a), 2b (b) and 2c (c) illustrating that the positions of electron density minimum (EDmin) are closer to the S atoms; interatomic distances are in Bohr.
Figure 5. One-dimensional distributions of electron density (ED) and electrostatic potential (ESP) functions (a.u.) along the S…I chalcogen bonds in 2a (a), 2b (b) and 2c (c) illustrating that the positions of electron density minimum (EDmin) are closer to the S atoms; interatomic distances are in Bohr.
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Figure 6. Experimental Raman spectra of crystals 2a–c in the low-frequency region.
Figure 6. Experimental Raman spectra of crystals 2a–c in the low-frequency region.
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Figure 7. Thermogravimetric (TG), differential scanning calorimetry (DSC) and differential thermogravimetric (DTG) curves of crystals: 2a (a), 2b (b) and 2c (c).
Figure 7. Thermogravimetric (TG), differential scanning calorimetry (DSC) and differential thermogravimetric (DTG) curves of crystals: 2a (a), 2b (b) and 2c (c).
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Table 1. Crystal data and structure refinement for triiodides 2a–c.
Table 1. Crystal data and structure refinement for triiodides 2a–c.
Structure2a2b2c
Empirical formulaC16H13NS2I4,C11H11NS2I4, C8H13NS2I4
Temperature (K)293293296.15
Crystal systemtriclinictriclinicmonoclinic
Space groupP-1P-1P21/n
a (Å)9.775(7)7.913(5)12.1447(7)
b (Å)9.868(6)7.994(5)10.2762(5)
c (Å)12.890(8)14.883(11)13.9862(7)
α (°)96.416(19)101.68(3)90
β (°)98.49(2)96.33(3)108.053(2)
γ (°)117.72(4)101.22(3)90
Volume (Å3)1065.24893.291659.57(15)
Z224
Density (g/cm3)2.4662.7102.781
µ, (mm1)6.0457.1957.74
F(000)720.0653.41242.9
Crystal size (mm)0.25 × 0.14 × 0.110.77 × 0.27 × 0.220.47 × 0.29 × 0.17
2θ range of data collection (deg)5.9 to 59.225.66 to 66.486.12 to 79.2
Range of refraction indices–13 ≤ h ≤ 13,
–13 ≤ k ≤ 13,
–17 ≤ l ≤ 17
–12 ≤ h ≤ 12,
–12 ≤ k ≤ 12,
–22 ≤ l ≤ 22
–21 ≤ h ≤ 21,
–18 ≤ k ≤ 18,
–24 ≤ l ≤ 25
Measured reflections470575239681480
Independent reflections5968 (Rint = 0.0346,
Rsigma = 0.0186
6839 (Rint = 0.0357,
Rsigma = 0.0208)
9984 (Rint = 0.0432,
Rsigma = 0.0315)
Refinement variables211165142
Goodness-of-fit on F21.0391.0491.104
R factors for F2 > 2σ(F2)R1 = 0.0283,
wR2 = 0.0623
R1 = 0.0450,
wR2 = 0.1007
R1 = 0.0543,
wR2 = 0.117
R factors for all reflectionsR1 = 0.0431
wR2 = 0.0683
R1 = 0.0611
wR2 = 0.1098
R1 = 0.1107
wR2 = 0.1171
Residual electron density (min/max) (e3)0.61/−1.291.98/−2.243.13/−3.71
Table 2. Experimental geometric parameters of S…I interactions in 2a–c crystal structures.
Table 2. Experimental geometric parameters of S…I interactions in 2a–c crystal structures.
Distance S…I, ÅC–S…I Angle, °S…I–I Angle, °I–I in I3, Å
2aS2…I2: 3.707C1–S2…I2: 142.27S2…I2–I4: 110.542.917; 2.917
2bS2…I2: 3.775C1–S2…I2: 161.54S2…I2–I1: 110.53; I3 (1): 2.912; 2.912
S2b…I2: 3.778C10–S2b…I2: 153.69S2b…I2–I1: 32.93I3 (2): 2.931; 2.931
2cS4…I3: 3.910C9–S4…I3: 165.72S4…I3–I2: 96.39I3 (1): 2.904; 2.936
S3…I8: 3.699C9–S3…I8: 166.14S3…I8–I7: 96.41
S2…I1: 3.902C1–S2…I1: 172.07S2…I1–I2: 77.78I3 (2): 2.931; 2.933
S1…I6: 3.734C1–S1…I6: 165.23S1…I6–I7: 96.74
Table 3. Thermal decomposition features of crystals 2a–c.
Table 3. Thermal decomposition features of crystals 2a–c.
2a2b2c
Melting Point (°C)141127122.5
Decomposition start (°C)162*smooth222160
DTG peak 1 (°C)180–210249215
DTG peak 2 (°C)277310252
Mass loss, peak 1 and 2 (%)83.489.990.3

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