The Supramolecular Structural Chemistry of Pentafluorosulfanyl and Tetrafluorosulfanylene Compounds.

The analysis of crystal structures of SF5 - or SF4 -containing molecules revealed that these groups are often surrounded by hydrogen or other fluorine atoms. Even though fluorine prefers F⋅⋅⋅H over F⋅⋅⋅F contacts, the latter appeared to be important in many compounds. In a significant number of datasets, the closest F⋅⋅⋅F contacts are below 95 % of the van der Waals distance of two F atoms. Moreover, a number of repeating structural motifs formed by contacts between SF5 groups was identified, including different supramolecular dimers and infinite chains. Among SF4 -containing molecules, the study focused on SF4 Cl compounds, including the first solid-state structure analyses of these reactive species. Additionally, electrostatic potential surfaces of a series of Ph-SF5 derivatives were calculated, pointing out the substituent influence on the ability of F⋅⋅⋅X contact formation (X=F or other electronegative atom). Interaction energies were calculated for different dimeric arrangements of Ph-SF5 , which were extracted from experimental crystal structure determinations.

Introduction

Fluorinated organic compounds are widely used in various fields of application, for example, as pharmaceuticals, crop protectants, and radiomarkers (18F PET). Organofluorine chemistry is traditionally focused on fluorine directly bonded to carbon (e.g. in CF3, CF2, or aryl‐F groups), while functional groups having heteroatom‐bonded fluorine are less investigated. This is certainly due to the challenges associated with synthesizing stable substituents adorned with heteroatom‐fluorine bonds. In the past decade, synthetic strategies have been developed that have made the pentafluorosulfanyl (SF5)[ , , , , , , ] and tetrafluorosulfanylene (SF4)[ , , ] groups accessible to a broad chemical community. The SF5 moiety, in particular, has attracted attention as a sterically demanding, nonpolar, and electron‐poor group, which is sometimes regarded as “super‐trifluoromethyl group”. Additionally, both SF5 and SF4 compounds have found interesting applications in materials, such as liquid crystals.[ , ] Thus, an in‐depth structural understanding of such compounds seems timely. Organofluorine compounds with carbon‐bound fluorine atoms have been extensively studied regarding their solid‐state structures, which are often governed by attractive F⋅⋅⋅H or F⋅⋅⋅F interactions.[ , ] Such interactions are potentially important for the physical properties of materials, as it has been shown with the absorption of fluorinated molecules on solid materials or the gas capture ability of fluorinated metal‐organic frameworks.[ , ] Generally, a C−F group is both a poor hydrogen‐bond and halogen‐bond acceptor due to energetically low‐lying fluorine lone‐pairs and low polarizability of fluorine. For these reasons the interactions are relatively weak, but often important for crystal‐structure formation and stabilization. For F⋅⋅⋅F interactions, two different types are described in the literature. “Type I” interactions, which can be described as van der Waals interactions with minimal repulsion contribution, are characterized by similar C−F⋅⋅⋅F angles for both F atoms Figure 1, a). In contrast, “Type II” contacts (which are “real” halogen bonds according to the IUPAC definition ) are characterized by an l‐shaped structure, having a contact between the nucleophilic region of one F atom and the electrophilic region of the other one (Figure 1, b).

Figure 1

Different arrangements of F⋅⋅⋅F contacts: a) Type I (predominant van‐der‐Waals contacts), b) Type II (“real” halogen bonds according to IUPAC definition ).

Different arrangements of F⋅⋅⋅F contacts: a) Type I (predominant van‐der‐Waals contacts), b) Type II (“real” n class="Chemical">halogen bonds according to IUPAC definition ).

Except for few crystallographic and computational studies, the supramolecular structural chemistry of SF5 and SF4 compounds remained ln class="Chemical">argely unnoticed thus far, which motivated us to conduct a detailed study on the solid‐state structural chemistry of these compound classes. In November 2019, the Cambridge Structural Database (CSD) contained no more than 188 entries on compounds of hexavalent sulfur with fluorine substituents (duplicates and SF6 solvates excluded), comprising 161 SF5 and 27 SF4 compounds (see the Supporting Information for details). However, 65 % of all entries have been added during the past six years, attesting to an increasing interest in this young substance class (Figure 2). Similar interaction properties as known for carbon‐bonded fluorine can certainly be expected for sulfur‐fluorine analogues. However, the striking difference between SF5 and CF3 is the presence of two chemically inequivalent fluorine positions (four equatorial F atoms, Feq, and one axial F atom, Fax) in the former. Moreover, SF4 compounds can exist in two different diastereomeric forms, with the trans isomer being usually isolated and structurally characterized for acyclic compounds.[ , , , , , , ]

Figure 2

Numbers of SF5 (black) and SF4 (grey) crystal structures published in the CSD, sorted after publication year (until November 2019).

Results and Discussion

Analysis of the SF5 crystal structures deposited in the CSD for intermolecular interactions revealed that the SF5 group is often surrounded by C−H moieties, thus stabilizing the crystal structures through weak C−H⋅⋅⋅F interactions (Table 1 and Tables S1–S4 in the Supporting Information). The closest F⋅⋅⋅H distance is <260 pm in 56 % of all analyzed structures, being in the usual range of weak F⋅⋅⋅H n class="Chemical">hydrogen bonds[ , ] (for comparison, the sum of van der Waals radii of H and F is 257 pm ). Contacts to other hydrogen bond donors such as N−H are extremely rare. Generally, the total number of contacts to equatorial F atoms is significantly larger than to the axial one (Table 2). However, it is hard to differentiate if this is simply for statistical reasons since there are four times as many Feq atoms than Fax atoms per SF5 group, or if the Feq atoms are actually more potent hydrogen bond acceptors than Fax. The majority of F⋅⋅⋅H contacts has been observed in Ar‐SF5 compounds (67 %), while F⋅⋅⋅H contacts seem to be less favored in aliphatic R‐SF5 compounds (42 %). This finding could be attributed to 1) a higher hydrogen‐bond donor ability of aromatic H atoms as compared to aliphatic ones, and 2) the electronic properties of the additional substituent accompanying the SF5 group, thus influencing the hydrogen‐bond acceptor ability of the F atoms.

Table 1

General statistics on intermolecular SF⋅⋅⋅H and SF⋅⋅⋅F contacts in crystal structures of X‐SF5 and X‐SF4‐Y molecules, including CSD data as well as compounds 1–4 reported here (Duplicates, structures with disordered SF5 groups, and datasets with R 1 >0.075 omitted).

	Entries total	F⋅⋅⋅H<260 pm[a]	279.3 ppm<F⋅⋅⋅F<308.7 pm	F⋅⋅⋅F<279.3 pm
aryl−SF5	110	74 (67 %)	62 (56 %)	26 (24 %)
olefinic C(sp2)−SF5	14	5 (36 %)	7 (50 %)	5 (36 %)
C(sp3)−SF5	26	11 (42 %)[b]	11 (42 %)	6 (23 %)
X−SF5 (X=N or O group)	13	4 (31 %)[b]	10 (77 %)	–
trans‐X‐SF4‐Y	25	13 (52 %)	13 (52 %)	1 (4 %)
cis‐X‐SF4‐Y	4	–	2 (50 %)	1 (25 %)
sum	192	107 (56 %)	105 (55 %)	39 (20 %)

[a] Based on X‐ray crystallographic data and therefore on imprecise determination of hydrogen atomic coordinates. [b] The real abundance might be higher as the H atoms are missing in some datasets.

Table 2

Abundance of Feq⋅⋅⋅H and Fax⋅⋅⋅H contacts among 163 crystallographic datasets with intermolecular X−SF5⋅⋅⋅H contacts shorter than 260 pm.

X	Overall entries	Thereof relevant	Feq⋅⋅⋅H	Fax⋅⋅⋅H
aryl	110	74 (67 %)	48 (44 %)	27 (24 %)
olefinic C(sp2)	14	5 (36 %)	4 (29 %)	1 (7 %)
C(sp3)	26	11 (42 %)	9 (35 %)	2 (8 %)
N or O group	13	4 (31 %)	3 (23 %)	1 (8 %)
sum	163	94 (58 %)	63 (39 %)	31 (19 %)

–

–

[a] Based on X‐ray crystallographic data and therefore on imprecise determination of hydrogen atomic coordinates. [b] The real abundance might be higher as the n class="Disease">H atoms are missing in some datasets.

Since the hydrogen atom coordinates determined by X‐ray crystallography n class="Chemical">are not very reliable, we decided to forgo a detailed analysis of F⋅⋅⋅H contact geometries and focus on other F⋅⋅⋅X (X=F, O, N, …) interactions. Even though fluorine prefers F⋅⋅⋅H over F⋅⋅⋅F contacts, the latter turned out to be important in many SF5 crystal structures. This is not only the case for molecules not containing hydrogen atoms, but also for many highly functionalized organic molecules. In 20 % of all analyzed SF5 crystallographic datasets, the closest F⋅⋅⋅F contacts are below 279 pm, which is <95 % of the van der Waals distance of two F atoms; therefore, these contacts are regarded as significant attractive interactions. In an additional 55 % of SF5 datasets, the contacts are in a range of 95–105 % around the van der Waals distance of 294 pm, representing typical van‐der‐Waals contacts. Most of these F⋅⋅⋅F contacts are actually close to Type I geometry according to Figure 1, indicating a high percentage of van‐der‐Waals interaction. However, a number of compounds shows a significant tendency toward Type II behavior, or intermediate cases between both geometries (Tables 3 and S1–S6). Among the Ar‐SF5 crystal structures, most of the “strong” F⋅⋅⋅F contacts were observed for molecules where Ar is an electron‐poor or electron‐neutral aryl group, and much less in cases where Ar is a rather electron‐rich aryl group. This finding fits the picture that the halogen bonding ability of fluorine is enhanced by electron‐poor substituents, as it has been discussed earlier.[ , ] Actually, most of the observed F⋅⋅⋅F contacts (in both aromatic and aliphatic SF5 compounds) stem from equatorial F atoms, which can be expected to be better halogen bond acceptors than Fax, as they have another F atom in trans position, being more electron‐withdrawing than any other group (Table 4).

Table 3

Abundance of Type I and Type II SF5⋅⋅⋅F5S contacts shorter than 279.3 pm (=95 % of the vdW sum of two F atoms) among 163 crystallographic datasets of X−SF5 compounds, according to Figure 1.

X	Overall entries	Thereof relevant	Type I	Type II	Undefined
aryl	110	26 (24 %)	20 (18 %)	3 (3 %)	3 (3 %)
olefinic C(sp2)	14	5 (36 %)	3 (21 %)	2 (14 %)	–
C(sp3)	26	6 (23 %)	6 (23 %)	–	–
N or O group	13	0 (0 %)	–	–	–
sum	163	37 (23 %)	29 (18 %)	5 (3 %)	3 (2 %)

Table 4

Abundance of different SF5⋅⋅⋅F contacts shorter than 279.3 pm (=95 % of the vdW sum of two F atoms ) among 163 crystallographic datasets of X−SF5 compounds (Fother=F atom of substituent other than SF5).

	Overall entries	Thereof relevant	Feq⋅⋅⋅Feq	Feq⋅⋅⋅Fax	Feq⋅⋅⋅Fother	Fax⋅⋅⋅Fax	Fax⋅⋅⋅Fother
aryl−SF5	110	26 (24 %)	16 (15 %)	6 (5 %)	1 (1 %)	2 (2 %)	1 (1 %)
olefinic C(sp2)−SF5	14	5 (36 %)	2 (14 %)	1 (7 %)	1 (7 %)	–	1 (7 %)
C(sp3)−SF5	26	6 (23 %)	4 (15 %)	–	1 (4 %)	1 (4 %)	–
N or O group	13	0 (0 %)	–	–	–	–	–
sum	163	37 (23 %)	22 (13 %)	7 (4 %)	3 (2 %)	3 (2 %)	2 (1 %)

–

–

–

–

–

–

–

–

–

–

–

–

–

–

Even though F⋅⋅⋅F interactions are expected to be relatively weak and therefore strongly impacted by other intermoleculn class="Chemical">ar interactions such as π–π stacking and hydrogen bonds, we identified a number of repeating structural motifs formed by contacts between SF5 groups. For more than 50 % of “strong” interactions and also for numerous structures with weak interactions, contacts between equatorial F atoms form supramolecular linear chains (Figure 3 a). Other possible architectures include twisted chains formed by Feq⋅⋅⋅Fax contacts (Figure 3 d) and different supramolecular dimers (Figure 3 b, c, e–g).

Figure 3

Observed supramolecular structural motifs in crystal structures of SF5‐substituted molecules: infinite chains (a, d), open‐chain dimers (b, e, g), and cyclic dimers* (c, f). Blue=Feq, Red=Fax. *syn or anti arrangement of the X groups is possible; shown is the respective syn isomer.

Observed supramolecular structural motifs in crystal structures of SF5‐substituted molecules: infinite chains (a, d), open‐chain dimers (b, e, g), and cyclic dimers* (c, f). Blue=Feq, Red=Fax. *syn or anti n class="Chemical">arrangement of the X groups is possible; shown is the respective syn isomer.

Analysis of datasets containing other fluorinated groups besides SF5 (accounting for ca. 20 % of all datasets) did not allow for a clear conclusion whether SF5 does prefer either another SF5 group for F⋅⋅⋅F interactions, or other fluorinated groups. The distribution of “strong” F⋅⋅F interactions between both groups is virtually equal, including SF5⋅⋅⋅X contacts with X being an n class="Chemical">aromatic or aliphatic C‐F, R‐AsF5 −, or PF6 −.

In the course of our ongoing investigation of perfluorinated main group compounds, we prepared the n class="Chemical">tetrafluoroiodyl compound F4I‐C6H4‐4‐SF5 (1, Figure 4; see the Supporting Information for details). In its crystal structure, the molecules are assembled through SF5⋅⋅⋅F5S and IF4⋅⋅⋅F4I contacts, while SF5⋅⋅⋅F4I contacts are not realized. The SF5 groups form typical supramolecular chains by Feq⋅⋅⋅Feq interactions, but in spite of the very high group electronegativity of the IF4 substituent, the interactions are relatively weak with separations of 288.8(3) pm. IF4⋅⋅⋅F4I contacts arise from direct I⋅⋅⋅F interactions and can therefore be estimated to be stronger than SF5⋅⋅⋅F5S interactions.

Figure 4

SF5‐ and SF4Cl‐substituted molecules that have been structurally characterized in the course of this work; note that 2 and 4 represent the first examples of SF4Cl‐substituted compounds characterized in the solid state.

The search for F⋅⋅⋅E interactions with E other than F in the CSD disclosed “strong” contacts (<95 % of the corresponding vdW sums) in only a small number of cases, including a n class="Chemical">diazonium salt (CSD refcode EQACIK; F⋅⋅⋅N 278(1) pm), a sulfonate salt (NALWIG; F⋅⋅⋅O 282.6(3) pm), and a polybrominated porphyrin complex (AGACAP; F⋅⋅⋅Br 301.9(6) pm). Additionally, weak van der Waals contacts between SF5 groups and N, O, S, Cl, or B atoms were observed in only 27 % of all cases where these heteroatoms are present, and therefore F⋅⋅⋅F contacts seem to be preferred over other F⋅⋅⋅E contacts. Many of these examples contain very electron‐poor contact groups such as ‐NO2, CO ligands, or ‐N2 +, suggesting that fluorine acts more likely as Lewis base rather than as Lewis acid.

The data available for compounds bearing SF4 groups did not show clen class="Chemical">ar trends as identified for SF5 compounds. This is due to 1) the much lower number of published datasets and 2) the tendency of X‐SF4‐Y compounds toward secondary F⋅⋅⋅H and F⋅⋅⋅F bonding, which seems to be lower than for SF5 in general. The latter finding might be attributable to steric shielding of the SF4 core by the two organic substituents. Moreover, an SF4 fragment is always less electron‐deficient than an SF5 one, and the F atoms should therefore exhibit a lower tendency toward halogen bonding. Consequently, only 45 % of the analyzed structures contain an F⋅⋅⋅H contact below 260 pm, and only two out of 27 structures (CSD refcodes JOPFID and RESHUV) feature a very close F⋅⋅⋅F contact at 267.6(2) pm. A reasonable comparison between cis‐ and trans‐SF4 derivatives was not feasible since most of the available datasets are trans‐SF4 compounds.

Among X‐SF4‐Y molecules, we were particuln class="Chemical">arly interested in X‐SF4Cl compounds, which are important intermediates for the synthesis of X‐SF5 as well as other X‐SF4‐Y compounds.[ , , , , , , ] Due to their high reactivity, this compound class resisted structural characterization through X‐ray diffraction thus far. We report here the first two crystal structure analyses of such compounds together with their SF5 counterparts (2–5), allowing for a direct comparison of the supramolecular structural behavior of SF5 and SF4Cl (see the Supporting Information for details). The S−Feq bond lengths in 2 (159.2(2)‐161.1(2) pm) and 4 (158.3(3)‐161.3(3) pm) are slightly longer than in their SF5 analogues 3 (155(1)‐160(2) pm) and 5 (157.5(3)‐160.4(2) pm), respectively. The S−Cl bonds in 2 (206.5(1) pm) and 4 (209.3(2) pm) are within the range observed for other sulfur chlorides in the CSD (ca. 190–210 pm for tetravalent sulfur; values for hexavalent sulfur are not available). The fingerprint plots illustrate that the solid‐state structures of the SF5‐ and SF4Cl‐substituted molecules are fundamentally different (Figures S13 and S14). The SF4Cl group in 2 displays Cl⋅⋅⋅Cl−C and Cl⋅⋅⋅O=C contacts, while in 3 corresponding contacts involving the axial F atom are not present. Instead, compound 3 shows a very close Fax⋅⋅⋅Fax contact at 262.6(3) pm. The intermolecular interaction patterns in the 4’‐chlorobiphenyl derivatives 4 and 5 are more similar than seen with 2 and 3, displaying a rather close contact of the axial halogen atom to the aryl‐bonded Cl atom (both of Type I geometry), while F⋅⋅⋅F contacts are weak to negligible. The S−Cl⋅⋅⋅Cl−C contact in 4 is 338.8(2) pm (vdW distance: 350 pm ), and the Fax⋅⋅⋅Cl−C contact in 5 measures 313.7(4) pm (vdW distance: 322 pm ). Additionally, a supramolecular structural similarity for both SF4Cl/SF5 pairs is that the equatorial F atoms are involved in F⋅⋅⋅H−C hydrogen bonding.

In order to support our crystallographic findings with computational studies, we calculated the electrostatic potential surfaces of a series of simple SF5 molecules (see Figure S15 in the Supporting Information). A Hammett plot for a series of simple Ph‐SF5 derivatives met the expectation that the magnitude of the σ‐hole at the axial F atom increases with the rising electronegativity of the aryl group (Figure 5). The value of −4.4 kcal mol−1, reached for F5S‐C6H4‐4‐CN, seems to be the ln class="Chemical">argest value possible; even the extremely electron‐withdrawing IF4 group in 1 does not reinforce the σ‐hole at Fax any more. The substituent influence on the equatorial F atoms was harder to quantify since these atoms do not show a well‐defined σ‐hole. Due to the proximity to the phenyl group and its positive potential, no distinctly localized area of less negative potential was observed. Generally, the trend seems to be similar as for the axial F atom, but significantly weaker. This finding is in agreement with the fact that the Feq atoms have always another F atom in the trans position, and the trans substituent has a stronger influence on the electronic properties than the cis ones.

Figure 5

Hammett plot on the σ‐hole at the axial F atom in substituted Ph‐SF5 molecules (electrostatic potential surfaces calculated at SCS‐MP2/aug‐cc‐pVTZ level and at a 0.001 electron bohr−3 isovalue surface of the electron density). The IF4‐substituted molecule (compound 1) was omitted from the linear regression.

Hammett plot on the σ‐hole at the axial F atom in substituted Ph‐SF5 molecules (electrostatic potential surfaces calculated at SCS‐MP2/aug‐cc‐pVTZ level and at a 0.001 electron bohr−3 isovalue surface of the electron density). The IF4‐substituted molecule (compound 1) was omitted from the linen class="Chemical">ar regression.

Finally, we conducted interaction energy calculations for different Ph‐SF5 dimers, based on the structures given in Figure 3. These were extracted from real aryl‐SF5 crystal structures, with any substituents replaced by n class="Chemical">hydrogen atoms (see the Supporting Information for details). Due to the increased flexibility of a gas phase dimer compared to the crystal environment, full relaxation of the structures leads to new F−H and F−Ph contacts for all structural motives except for dimers in Figure 3f and g. Therefore, only the phenyl groups were relaxed, keeping the S and F coordinates fixed. Subsequent energy calculations revealed estimated interaction energies between −0.1 and −13.5 kJ mol−1, with the largest values for contacts between equatorial F atoms (Table 5). This result fits well with our findings from the crystal structure analyses, where Feq⋅⋅⋅Feq appeared most frequently. In order to verify the contribution of non‐F⋅⋅⋅F interactions to the observed interaction energies, we also performed calculations on corresponding acetylene‐SF5 systems. The resulting energies are significantly smaller than for the Ph‐SF5 dimers, suggesting that the latter are additionally stabilized by F⋅⋅⋅H interactions involving the ortho‐C−H moieties close to the SF5 groups, or π–π stacking in the case of the cisoid Feq⋅⋅⋅Feq contact (motif b). However, the single Feq⋅⋅⋅Feq and the dual Feq⋅⋅⋅Feq contact (Figure 3 b and c, respectively) still show the most negative bonding energies, corroborating the assumption that the contacts between equatorial F atoms are most favorable.

Table 5

Interaction energies in kJ mol−1 for the R−SF5 dimers shown in Figure 3, calculated at SCS‐MP2‐F12 level using a cc‐pVTZ‐F12 basis set and counterpoise corrections in order to account for the basis set superposition error.

Contact	F⋅⋅⋅F [pm]	R=Ph	R=‐C≡CH
Feq⋅⋅⋅Feq (b), anti	269.3	−10.1	−5.9
Feq⋅⋅⋅Feq (b), syn	258.8	−9.3	±0.0
dual Feq⋅⋅⋅Feq (c)	289.4	−13.5	−8.0
Feq⋅⋅⋅Fax (e)	272.1	−4.6	−1.7
dual Feq⋅⋅⋅Fax (f)	293.2	−2.1	−2.7
Fax⋅⋅⋅Fax (g)	285.8	−0.1	−0.9

Conclusions

In summary, SF5 is a nonpoln class="Chemical">ar, bulky, relatively inflexible group,[ , ] whose structural chemistry involves mainly weak secondary bonding interactions. Even though these interactions are strongly impacted by other intermolecular interactions, we could observe some significant trends:

The equatorial F atoms show a stronger tendency town class="Chemical">ards F⋅⋅⋅F contact formation than the axial one; this can be traced back to the strongly electron‐withdrawing fluorine substituent in the trans position, while the axial F atom usually has an organic group trans to it.

F⋅⋅⋅F contacts usually exhibit “Type I” geometry, indicating a large percentage of van‐der‐Waals interaction.

Electron‐poor substituents on aryl‐SF5 compounds seem to promote F⋅⋅⋅F bond formation; the influence on the axial F atom is thereby ln class="Chemical">arger than on the equatorial ones.

F⋅⋅⋅E contacts with E other than F also exist, where E is usually an electron‐poor N or O group.

Among the related SF4 compounds, SF4Cl compounds show the richest supramoleculn class="Chemical">ar structural chemistry, since Cl exerts minimal steric shielding of the SF4 core and is a better halogen bond acceptor than F.

Experimental Section

General information

Unless otherwise stated, all reactions were carried out under strictly anhydrous conditions and n class="Chemical">Ar or N2 atmosphere. All solvents were dried and distilled using standard methods. Trichloroisocyanuric acid was used without prior drying or purification. Spray‐dried KF was always weighed out under N2 atmosphere in a glove box. All 1H, 19F, and 13C NMR spectra were acquired on either a 300, 400, or 500 MHz spectrometer. For 19F NMR yield determination, trifluorotoluene was introduced after each reaction as an internal standard, and the d1 relaxation delay was increased to 10 s during data collection. The 1H, 13C, and 19F NMR chemical shifts are given in parts per million (ppm) and calibrated to either residual solvent signal (1H and 13C), α,α,α‐trifluorotoluene (19F, δ=−63.10 ppm in CD3CN), or CFCl3 (19F, δ=−0.65 ppm in CDCl3). NMR data are reported in the following format: chemical shift (integration, multiplicity (s=singlet, d=doublet, t=triplet, q=quartet, quintet=quint, m=multiplet), coupling constants (Hz)). IR data were collected on a Thermo Fischer Scientific Nicolet 6700 FT‐IR equipped with a PIKE technologies GladiATR or a PerkinElmer BX II using ATR FT‐IR technology and absorption maxima are reported in cm−1. GC/MS was performed on a Thermo Fischer Trace GC 2000 equipped with a flame ionization detector, using a ZB‐5 column with guardian (L: 30 m, i.d.: 0.25 mm, DF=0.25 μm) and helium as the carrier gas with a constant flow of 1.1 mL min−1 and a Shimadzu‐QP 2010 Ultra using HP‐5 column with a parallel MS and FID detection. HRMS data were collected by MoBiAS—the MS‐service of the “Laboratorium für Organische Chemie der ETH Zürich”. Single‐crystal X‐ray diffraction data were collected on a XtaLAB Synergy Dualflex Pilatus 300 K Diffractometer, at T=100(2) K. Absorption correction was applied on the intensity data using the multi‐scan method.

Deposition numbers 2013886 (for contain the supplementary crystallographic data for this paper. These data n class="Chemical">are provided free of charge by the joint Cambridge Crystallographic Data Centre and Fachinformationszentrum Karlsruhe Access Structures service. Crystallographic data and details on structure refinement for the compounds are reported in Table 6.

Table 6

Crystal data and details on structure refinement for the compounds 1–4.

Compound	1	2	3[a]	4[b]
CCDC	2013886	2013887	2013888	2013889
molecular formula sum	C6H4F9IS	C7H6ClF4NO2S	C7H6F5NO2S	C12H8Cl2F4S
formula weight [g mol−1]	406.05	279.64	263.19	331.14
crystal system	orthorhombic	monoclinic	monoclinic	triclinic
space group	Pbca	P21/c	P21/m	P1‾
a [Å]	6.9632(2)	6.1797(1)	6.2352(4)	7.8901(6)
b [Å]	8.8136(2)	21.2904(4)	19.7193(16)	8.4624(7)
c [Å]	32.914(1)	7.8226(2)	12.2091(11)	10.5314(9)
α [°]	90	90	90	106.565(8)
β [°]	90	105.680(2)	103.599(3)	108.756(7)
γ [°]	90	90	90	94.523(7)
V [Å3]	2020.0(1)	990.91(4)	1459.1(2)	626.8(1)
molecules per cell z	8	4	6	2
electrons per cell F 000	1520	560	792	332
ρ calcd [g cm−3]	2.670	1.874	1.797	1.754
μ [mm−1] (radiation)	3.484 (MoKα)	5.900 (CuKα)	0.394	6.549 (CuKα)
crystal shape and color	colorless block	colorless needle	colorless plank	colorless plate
crystal size [mm]	0.08×0.06×0.04	0.22×0.04×0.02	0.28×0.09×0.07	0.22×0.10×0.02
θ range [Mo]	3.177 … 34.741	4.153 … 79.748	3.947 … 27.497	4.696 … 79.990
reflns collected	28 728	10776	17079	11743
reflns unique	3982	2116	3375	2629
reflns with I>2σ(I)	3388	1941	2877	2242
completeness of dataset	99.8 %	100 %	98.3 %	99.7 %
R int	0.0333	0.0440	0.0418	0.0447
parameters; restraints	154; 0	146; 0	256; 57	172; 6
R 1 (all data, I>2σ(I))	0.0422; 0.0338	0.0661; 0.0625	0.0464; 0.0382	0.0918; 0.0843
wR 2 (all data, I>2σ(I))	0.0718; 0.0697	0.1740; 0.1714	0.1093; 0.1058	0.2593; 0.2512
GooF (F 2)	1.137	1.076	1.144	1.068
max. residual peaks	−1.680; 1.590	−0.911; 0.903	−0.616; 0.339	−1.129; 1.410

[a] Twinned sample; HKLF5 used for final refinement. One molecule is disordered over a mirror plane. This measurement represents the best of many attempts; crystals were always very small and decomposed or redissolved rather quickly, especially after the vessel had been opened. Apart from these problems the refinement quality indicators are reasonable and the structural parameters are very similar to comparable compounds published in the CSD. [b] The moderate data quality is due to the fact that the crystals showed a layered platelet structure. The highest residual peaks hint at a full‐molecule disorder (pseudorotation about 180°), with very low occupancy of the second orientation. It cannot be excluded that the disordered part is a similar but different species. Aryl‐SF3, and to some extent, aryl‐SOF3 and aryl‐SO2F have been repeatedly observed in the product solution, so it is likely one of these compounds has co‐crystallized on the same position. However, none of these could be modelled as a disorder, which is plausible due to the low contribution and partial overlap of atomic positions. This would lead to collisions between adjacent cells, but crystal morphology hints at multicrystallinity or a form of twinning which could simulate disorder. The unmodelled disorder causes ambiguities in the Hirshfeld test for S and Cl, as well as some residual peaks and a relatively high wR 2 value.

3

P

[a] Twinned sample; HKLF5 used for final refinement. One molecule is disordered over a mirror plane. This measurement represents the best of many attempts; crystals were always very small and decomposed or redissolved rather quickly, especially after the vessel had been opened. Apart from these problems the refinement quality indicators n class="Chemical">are reasonable and the structural parameters are very similar to comparable compounds published in the CSD. [b] The moderate data quality is due to the fact that the crystals showed a layered platelet structure. The highest residual peaks hint at a full‐molecule disorder (pseudorotation about 180°), with very low occupancy of the second orientation. It cannot be excluded that the disordered part is a similar but different species. Aryl‐SF3, and to some extent, aryl‐SOF3 and aryl‐SO2F have been repeatedly observed in the product solution, so it is likely one of these compounds has co‐crystallized on the same position. However, none of these could be modelled as a disorder, which is plausible due to the low contribution and partial overlap of atomic positions. This would lead to collisions between adjacent cells, but crystal morphology hints at multicrystallinity or a form of twinning which could simulate disorder. The unmodelled disorder causes ambiguities in the Hirshfeld test for S and Cl, as well as some residual peaks and a relatively high wR 2 value.

General procedure for the synthesis of aryl tetrafluoro‐λ6‐sulfanyl chloride compounds

Trichloroisocyanuric acid (0.958 g, 4.1 mmol, 18 equiv) was added to an oven‐dried microwave vial equipped with a stir bn class="Chemical">ar; the vessel was then transported inside a glove box under N2 atmosphere. Spray‐dried potassium fluoride (0.425 g, 7.3 mmol, 32 equiv) and the corresponding disulfide (0.23 mmol, 1.0 equiv) were added to the reaction vessel, followed by 4 mL MeCN and trifluoroacetic acid (1.8 μL, 0.02 mmol, 0.1 equiv). The vessel was then sealed with a cap with septum using a crimper, and the reaction mixture was stirred vigorously at room temperature overnight (ca. 18 h). Upon reaction completion, an aliquot of the reaction mixture was passed through a PTFE syringe filter, and an NMR sample was prepared with 0.4 mL of the filtered aliquot and adding 0.1 mL internal standard solution (made immediately prior to use with defined amounts of α,α,α‐trifluorotoluene and CD3CN) for 19F NMR yield determination.

In order to remove KF and TCICA (and its byproducts), the reaction vessel atmosphere and solvent was purged with n class="Chemical">Ar and transported into the glove box. Subsequently, the crude reaction mixture was filtered into a PFA vessel via syringe filter and concentrated in vacuo. Then, the crude reaction mixture was diluted with n‐hexane, filtered into a PFA vessel, and concentrated in vacuo. (Note that repeating dilution/filtration/concentration 3–4 times will provide better results due to limited solubility of the aryl‐SF.) The crude material consisted of mostly the aryl‐SF4Cl product (amount quantified by 19F NMR) and was carried forward without further purification.

General procedure A for the synthesis of pentafluorosulfanyl compounds

The aryl‐n class="Chemical">SF4Cl compound (0.12 mmol, 1.0 equiv) was added to a PFA vessel under N2 atmosphere in a glove box. Subsequently, AgF (0.36 mmol, 3.0 equiv) was added, and the vessel was sealed and removed from the glovebox. The sealed vessel was heated to 120 °C for ca. 2 days. Upon cooling, the vessel was rinsed with copious amounts of CH2Cl2 and H2O into a separatory funnel. The reaction mixture was extracted with CH2Cl2. The combined organic layers were dried with MgSO4, filtered through Celite, and concentrated. The crude reaction mixture was purified via gradient column chromatography on silica gel on a Teledyne‐Isco Combiflash instrument, eluting with hexanes:EtOAc.

General procedure B for the synthesis of pentafluorosulfanyl compounds

The aryl‐n class="Chemical">SF4Cl compound (0.046 mmol, 1.0 equiv) was added to a PFA vessel under N2 atmosphere in a glove box. Subsequently, AgF (0.287 mmol, 6.2 equiv) was added, and the vessel was sealed and removed from the glovebox. The sealed vessel was placed in a sand bath and heated to 130 °C (at the bottom of the vessel) for 48 h to avoid sublimation of the substrate to the lid. Upon reaction completion, to the reaction mixture 10.0 μL (11.9 mg, 0.0814 mmol) of α,α,α‐trifluorotoluene were added for 19F NMR yield determination. The reaction mixture was extracted with n‐pentane and n‐hexane. The residue was further subjected to column chromatography.

Procedure for synthesis of pentafluoro(4‐(tetrafluoro‐λ5‐ iodanyl)phenyl)‐λ6‐sulfane (1)

Trichloroisocyanuric acid (0.350 g, 1.5 mmol, 4.0 equiv) was added to an oven‐dried microwave vial equipped with a stir bn class="Chemical">ar; the vessel was then transported inside a glove box under N2 atmosphere. Spray‐dried potassium fluoride (0.131 g, 2.3 mmol, 6.0 equiv) and pentafluoro(4‐iodophenyl)‐λ6‐sulfane (0.124 g, 0.38 mmol, 1.0 equiv) were added to the reaction vessel, followed by 4 mL MeCN. The vessel was then sealed with a cap with septum using a crimper and removed from the glove box. The reaction mixture was stirred vigorously at 40 °C for ca. 48 h. Upon reaction completion, an aliquot of the reaction mixture was passed through a PTFE syringe filter, and an NMR sample was prepared with 0.4 mL of the filtered aliquot + 0.1 mL internal standard solution (made immediately prior to use with x g of either trifluorotoluene or fluorobenzene in y mL CD3CN) for 19F NMR yield determination.

In order to remove KF and TCICA (and its byproducts), the reaction vessel atmosphere and solvent was purged with n class="Chemical">Ar and transported into the glove box. Subsequently, the crude reaction mixture was filtered into a PFA vessel, washed with dry MeCN, and then concentrated in vacuo. Then, the crude reaction mixture was diluted with n‐hexane, filtered into a PFA vessel, and concentrated in vacuo. (Note that repeating dilution/filtration/concentration 3–4 times will provide better results due to limited solubility of the aryl‐IF.) The crude material consisted of mostly the aryl‐IF4 product and was carried forward without further purification.

Characterization data

Pentafluoro(4‐(tetrafluoro‐λ): The reaction was run according to the procedure outlined above, and the product was formed in 90 % yield by 19F NMR analysis. 19F NMR (282 MHz, CD3CN): δ=+80.76 (1F, quint, J=149.0 Hz), +61.79 (4F, d, J=149.0 Hz), −26.05 (4F, br s). After extracting the product, colorless crystals suitable for single‐crystal X‐ray diffraction were obtained via slow solvent evaporation of a n class="Chemical">diisopropyl ether solution under inert atmosphere.

Methyl 6‐(chlorotetrafluoro‐λ: The reaction was run according to the general procedure A, and the product was formed in 65 % yield by 19F NMR analysis. 19F NMR (282 MHz, CD3CN): +123.52 (4F, s). After extracting the product, colorless crystals suitable for single‐crystal X‐ray diffraction were obtained via slow solvent evaporation of a 9:1 n‐hexane:n class="Chemical">CH2Cl2 solution under inert atmosphere.

Methyl 6‐(pentafluoro‐λ: The reaction was run under the conditions of the general procedure B. The residue was further subjected to column chromatography (Alumina–Brockmann grade I, n‐pentane to 7:3 (dichloromethane:n‐pentane), R f=0.5 in n class="Chemical">dichloromethane:n‐Pentane (7:3). The product was obtained in 6 % yield by 19F‐NMR analysis. 1H NMR (400 MHz, Chloroform‐d): δ=9.18–9.13 (m, 1 H), 8.55–8.48 (m, 2 H), 7.85 (dd, J=8.5, 0.8 Hz, 1 H), 4.01 ppm (s, 3 H). 19F NMR (376 MHz, Chloroform‐d): δ=76.66 (quint, J=150.3 Hz), 51.98 ppm (d, J=150.1 Hz). 13C NMR (100 MHz, Chloroform‐d) 167.40 (Cq), 163.60 (Cq), 149.77 (CHAr), 140.15 (CHAr), 128.85 (Cq), 121.41 (CHAr), 53.17 (CH3). GC/MS (EI): calcd for C7H6F5NO2S [M]+: 263.0, found 263.0. Crystals suitable for single‐crystal X‐ray diffraction were obtained via extraction of the crude reaction mixture with n‐pentane and n‐hexane. The solvent was condensed off under atmospheric pressure and −78 °C in a sealed condensation apparatus. Crystals of the product were obtained as low‐melting colorless needles and have been mounted at a temperature of −30 °C.

Chloro(4′‐chloro‐[1,1′‐biphenyl]‐4‐yl)tetrafluoro‐λ: The reaction was run according to the general procedure A, and the product was formed in 64 % yield by 19F NMR analysis. 19F NMR (282 MHz, CD3CN): +137.13 (4F, s). After extracting the product, colorless crystals suitable for single‐crystal X‐ray diffraction were obtained via slow solvent evaporation of a 9:1 n‐hexane:n class="Chemical">CH2Cl2 solution under inert atmosphere.

(4′‐Chloro‐[1,1′‐biphenyl]‐4‐yl)pentafluoro‐λ: The reaction was run according to the general procedure A, and the product was obtained in 77 % isolated yield (29 mg, 0.09 mmol) as a white solid; m.p. 82.8–84.8 °C. 19F NMR (471 MHz, CDCl3): +84.60 (1F, quint, J=150.2 Hz), +63.24 (4F, d, J=150.2 Hz); n class="Chemical">1H NMR (500 MHz, CDCl3): 7.83 (2 H, dm, J=8.6 Hz), 7.62 (2 H, br d, J=8.6 Hz), 7.52 (2 H, dm, J=8.6 Hz), 7.45 (2 H, dm, J=8.6 Hz); 13C{1H} NMR (126 MHz, CDCl3): 153.1 (quint, J=17.5 Hz), 143.3, 137.5, 134.8, 129.3, 128.5, 127.1, 126.6 (quint, J=4.6 Hz). max (ATR‐IR): 840 cm−1 (br), 813 cm−1. HRMS (EI): calcd for C12H8ClF5S [M]+: 313.9950, found 313.9947. Colorless crystals suitable for single‐crystal X‐ray diffraction were obtained via sublimation.

Computational studies

All calculations were performed using the TURBOMOLE program package, version 7.3. Structures were optimized at the SCS‐MP2 level of theory using the aug‐cc‐pVTZ basis set for all atoms (aug‐cc‐pVTZ‐PP and the corresponding ECP for I ) and the corresponding auxiliary basis sets.[ , ] SCF was converged to energy changes below 10−8 a.u., structures were optimized to a ln class="Chemical">argest Cartesian gradient component below 10−4 a.u. For the substituted monomers, the electrostatic potential and the density were calculated at the same level of theory. All electrostatic potential maps show the electrostatic potential projected on a density iso‐surface of 0.001 a.u. in a range from −15 kcal mol−1 (blue) to +15 kcal mol−1 (red). All pictures were created using the Jmol package. To estimate the interaction energies of the dimer structures roughly, only the phenyl and the acetylene moieties were optimized, the S and F positions were taken from experimental data. For the computation of the interaction energies, we used the obtained fragments without further re‐optimization. The energies were calculated at the SCS‐MP2‐F12 level of theory using cc‐pVTZ‐F12 basis sets and the corresponding auxiliary basis sets.[ , ] To correct for basis set superposition errors, the counterpoise correction was applied.

Conflict of interest

The authors declare no conflict of interest.

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Supplementary

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