Syntheses, structures, and stabilities of aliphatic and aromatic fluorous iodine(I) and iodine(III) compounds: the role of iodine Lewis basicity

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1Department of Chemistry, Texas A&M University, P.O. Box 30012, College Station, Texas, 77842-3012, USA,
2Department of Chemistry, Texas A&M University at Qatar, P.O. Box 23874, Doha, Qatar
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§ Present address: Dr. Tathagata Mukherjee, Intel Corporation, Hillsboro, Oregon
Guest Editor: D. O'Hagan
Beilstein J. Org. Chem. 2017, 13, 2486–2501.
Received 23 Aug 2017, Accepted 25 Oct 2017, Published 23 Nov 2017
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The title molecules are sought in connection with various synthetic applications. The aliphatic fluorous alcohols RfnCH2OH (Rfn = CF3(CF2)n–1; n = 11, 13, 15) are converted to the triflates RfnCH2OTf (Tf2O, pyridine; 22–61%) and then to RfnCH2I (NaI, acetone; 58–69%). Subsequent reactions with NaOCl/HCl give iodine(III) dichlorides RfnCH2ICl2 (n = 11, 13; 33–81%), which slowly evolve Cl2. The ethereal fluorous alcohols CF3CF2CF2O(CF(CF3)CF2O)xCF(CF3)CH2OH (x = 2–5) are similarly converted to triflates and then to iodides, but efforts to generate the corresponding dichlorides fail. Substrates lacking a methylene group, RfnI, are also inert, but additions of TMSCl to bis(trifluoroacetates) RfnI(OCOCF3)2 appear to generate RfnICl2, which rapidly evolve Cl2. The aromatic fluorous iodides 1,3-Rf6C6H4I, 1,4-Rf6C6H4I, and 1,3-Rf10C6H4I are prepared from the corresponding diiodides, copper, and RfnI (110–130 °C, 50–60%), and afford quite stable RfnC6H4ICl2 species upon reaction with NaOCl/HCl (80–89%). Iodinations of 1,3-(Rf6)2C6H4 and 1,3-(Rf8CH2CH2)2C6H4 (NIS or I2/H5IO6) give 1,3,5-(Rf6)2C6H3I and 1,2,4-(Rf8CH2CH2)2C6H3I (77–93%). The former, the crystal structure of which is determined, reacts with Cl2 to give a 75:25 ArICl2/ArI mixture, but partial Cl2 evolution occurs upon work-up. The latter gives the easily isolated dichloride 1,2,4-(Rf8CH2CH2)2C6H3ICl2 (89%). The relative thermodynamic ease of dichlorination of these and other iodine(I) compounds is probed by DFT calculations.


A number of fluorous alkyl iodides, usually of the formula RfnCH2CH2I or RfnI (Rfn = CF3(CF2)n–1), are commercially available and have seen abundant use as building blocks in fluorous chemistry [1-3]. Fluorous aryl iodides, such as RfnC6H4I or Rfn(CH2)mC6H4I species, are also often employed as intermediates (typically m = 2, 3 and n ≥ 6 [1-3]), but only a few have been commercialized [4]. Many research groups have described the syntheses of other types of fluorous alkyl [5-8] and aryl [9-12] iodides [13-17]. The former are ubiquitous by virtue of the large number of perfluoroalkyl iodides RfnI that have been shown to undergo free radical additions to alkenes [7,8].

In previous papers, we have reported convenient preparations of a variety of fluorous alkyl iodides [13-15], aryl iodides [16,17], and hypervalent iodine(III) derivatives [16-19]. The latter have included aliphatic iodine(III) bis(trifluoroacetates) [18,19] and dichlorides [17], and aromatic iodine(III) bis(acetates) [16] and dichlorides [17]. The bis(carboxylates) have been employed as recyclable reagents for oxidations of organic substrates [16,18,19], and some of the dichlorides are depicted in Scheme 1. Others have described additional fluorous iodine(III) species [11,20-22].


Scheme 1: Some previously reported iodine(III) dichlorides relevant to this work.

Recently, our attention has been directed at two potential applications of iodine containing fluorous compounds. One involves new approaches to phosphorus–carbon bond formation using fluorous alkyl and aryl iodides [23,24]. The other involves the use of fluorous iodine(III) dichlorides for free radical chlorinations [25]. In this regard, phenyl iodine(III) dichloride (PhICl2) is an effective free radical chlorinating agent for hydrocarbons [26,27]. Importantly, the mechanism does not involve the liberation of Cl2, followed by the textbook sequence of steps. Rather, hydrogen abstraction is effected by a species other than the chlorine radical Cl·, presumably PhICl· [26,27].

One potential attraction of fluorous iodine(III) dichlorides as chlorinating agents would be the recovery and recycling of the fluorous iodide byproduct. Towards this end, higher fluorophilicities are usually advantageous. To a first approximation, these are maximized by increasing the lengths and quantities of the (CF2)n segments, and decreasing the lengths and quantities of any (CH2)m segments [1-3]. However, longer (CF2)n segments are often coupled with lower absolute solubilities [1,28], a logical consequence as one approaches the macromolecular limit of polytetrafluoroethylene. Fluorophilicities are typically quantified by fluorous/organic liquid/liquid phase partition coefficients [1-3]. The most common solvent combination is perfluoro(methylcyclohexane) (CF3C6F11) and toluene.

The objective of this study was to bridge several strategic gaps regarding highly fluorophilic building blocks for the formation of (1) phosphorus–carbon bonded species, and (2) iodine(III) dichloride reagents. For example, aliphatic species of the formula RfnCH2CH2ICl2 are unstable [17]. However, analogs with one less methylene group, RfnCH2ICl2, have been isolated for n = 8 and 10 as depicted in Scheme 1 [17,20]. Although partition coefficients are not available for the iodide Rf8CH2I (the byproduct that would form in most chlorination reactions), they would fall between those of Rf8I (88.5:11.5 for CF3C6F11/toluene [29]) and Rf8(CH2)3I (50.7: 49.3 [30]). These rather modest fluorophilicities would presumably be lower for the more polar dichlorides RfnCH2ICl2 – a possible disadvantage for reactions in fluorous solvents. In any case, higher homologs that would have more biased partition coefficients were sought.

In the same vein, literature data prompted interest in certain fluorous aromatic iodine(III) dichlorides. For example, the non-fluorous iodine(III) dichloride II-Me (Scheme 1) [31], which features two strongly electron-withdrawing nitro groups and a mildly electron-donating methyl group, is easily isolated in analytically pure form from the reaction of the corresponding aryl iodide and Cl2, even though the nitro groups render the iodine atom less Lewis basic and thermodynamically less prone to oxidation. The Hammett σ values associated with CF2CF3 and CF2CF2CF3 substituents (σp 0.52; σm 0.47–0.52 [32]) suggest that Rfn groups are less electron withdrawing than nitro groups (σp 0.81; σm 0.71). Therefore, similar fluorous compounds of the formula (Rfn)2C6H3ICl2 were seen as realistic targets. The less fluorophilic homologs III and IV (Scheme 1), which feature three methylene or CH2CH2CH2 "spacers" that electronically insulate the arene ring from the perfluoroalkyl groups, have been previously isolated [17].

As described below, the pursuit of the preceding objectives has met with both success and some unanticipated speed bumps, for which parallel computational studies have provided valuable insight. Regardless, these efforts have resulted in a number of practical preparations that will soon be utilized in further applications [23], and defined various physical properties and stability limits that are useful guides for future research.


Syntheses and reactions, RfnCH2I (n = 11, 13, 15). To the authors' knowledge, no fluorous alkyl iodides of the formula RfnCH2I are commercially available. Thus, as shown in Scheme 2, a sequence previously employed for lower homologs (n = 8, 10 [13]) was investigated. The commercially available alcohols RfnCH2OH (n = 11, 13, 15) were first converted to the triflates RfnCH2OTf using pyridine and triflic anhydride (Tf2O) in (trifluoromethyl)benzene (CF3C6H5), an amphoteric solvent that is usually able to dissolve appreciable quantities of both fluorous and non-fluorous solutes [33]. The reactions with n = 11 and 13 were conducted at 0 °C, and work-ups gave the expected triflates in 60–61% yields. In contrast, only traces of product were obtained with n = 15, presumably due to the poor solubility of the alcohol in virtually any medium. However, the solubilities of fluorous compounds are often highly temperature dependent [28,34], and an analogous reaction at room temperature gave Rf15CH2OTf in 22% yield. The triflates were white solids with some solubility in acetone. They were characterized by IR and NMR (1H, 13C{1H}, 19F{1H}) spectroscopy and microanalyses as summarized in the experimental section.


Scheme 2: Syntheses of fluorous compounds of the formula RfnCH2X.

The triflates were treated with NaI in acetone at 75 °C. Over the course of 24 h, high conversions to the corresponding fluorous iodides RfnCH2I were realized, although at rates much slower than with non-fluorous analogs. Work-ups afforded the products as analytically pure white solids in 58–69% yields, which were characterized analogously to the triflates. All were to some degree soluble in acetone, but as the perfluoroalkyl group lengthened, appropriate cosolvents were required to achieve significant concentrations. In order to obtain 13C NMR spectra (n = 13, 15), C6F6 – which is technically a non-fluorous solvent [35] but is nonetheless often effective with fluorous solutes – was employed.

Importantly, these fluorous aliphatic iodides were more fluorophilic than those mentioned in the introduction. Representative partition coefficients were determined as described in the experimental section. Those for Rf15CH2I ranged from >99:<1 for CF3C6F11/toluene to 87:13 for CF3C6F11/acetone. The CF3C6F11/toluene partition coefficient of Rf11CH2I was also >99:<1.

Next, CH3CN/C6F6 solutions of the fluorous aliphatic iodides (n = 11, 13) were treated with aqueous NaOCl and conc. HCl. The combination of HCl and a mild oxidant generates Cl2, providing a "greener" synthetic approach to iodine(III) dichlorides [36-38]. Accordingly, the target molecules RfnCH2ICl2 precipitated in 33–81% yields. However, the poor solubilities of these pale yellow powders precluded further purification by the usual protocols. Microanalyses confirmed the presence of chlorine. When 1H NMR spectra were recorded in acetone-d6, new CH2 signals 1.37–1.38 ppm downfield of those of the precursors RfnCH2I were apparent. However, the NMR samples slowly became greenish yellow, suggestive of dissolved Cl2, and the starting iodides were usually evident. The use of Cl2 in place of NaOCl/HCl did not give better results.

Syntheses and reactions, RfOxCH2I (x = 2–5). There is an ongoing effort in fluorous chemistry to decrease reliance on perfluorooctyl containing building blocks, which are associated with a variety of environmental issues [39]. One approach is to switch to related ethereal phase tags or "ponytails" [40,41]. Accordingly, oligomeric fluorous ethers that terminate in CH2OH groups, CF3CF2CF2O(CF(CF3)CF2O)xCF(CF3)CH2OH, are commercially available. These are abbreviated RfOxCH2OH, and the ethereal oxygen atoms have essentially no Lewis base character. In some cases, CF2CF2OCF(CF3)CF2OCF(CF3)- segments have been found to impart higher fluorophilicites than similar perfluoroalkyl groups [42]. However, the multiple CF(CF3) stereocenters are disadvantageous, as they render such compounds mixtures of diastereomers, presenting an impediment to crystallization. In some cases, NMR spectra do not differentiate the diastereomers, and in other cases more complex signal patterns are evident.

As shown in Scheme 3, the oligomeric alcohols (x = 2–5) were elaborated as described for the non-ethereal alcohols RfnCH2OH and a previous report involving the lower non-oligomeric homolog RfO1CH2OH (x = 1 [5]). They were first converted to the triflates RfOxCH2OTf using pyridine and triflic anhydride (Tf2O). These were soluble in hexane/ethyl acetate and isolated as analytically pure colorless oils in 84–93% yields. Subsequent reactions with NaI in acetone (70–75 °C, x = 2,4,5) gave the corresponding iodides RfOxCH2I as colorless liquids in 81–91% yields. Unfortunately, efforts to oxidize these compounds to the corresponding iodine(III) dichlorides using the conditions in Scheme 1 and Scheme 2 were unsuccessful. NMR analyses of crude reaction mixtures showed only starting material.


Scheme 3: Syntheses of fluorous compounds of the formula CF3CF2CF2O(CF(CF3)CF2O)xCF(CF3)CH2X'.

Attempted syntheses of RfnICl2. Prior to the efforts described in the previous sections, iodine(III) dichlorides derived from perfluoroalkyl iodides RfnI were considered as targets. Since these lack sp3 carbon–hydrogen bonds, they are not susceptible to possible chlorination or other degradation under free radical chlorination conditions. However, no reactions were observed when RfnI were treated with Cl2 or NaOCl/HCl.

Nonetheless, perfluoroalkyl iodides RfnI (n = 6–8, 10, 12) can be oxidized using various recipes (e.g., 80% H2O2 in trifluoroacetic acid anhydride) to the iodine(III) bis(trifluoroacetates) RfnI(OCOCF3)2 in high isolated yields [18,19,21]. It was thought that these might, in turn, react with TMSCl as sketched in Scheme 4 to provide "back door" entries to the target compounds RfnICl2. Indeed, when these reactions were carried out, the samples exhibited the appropriate characteristic bright yellow colors (n = 6, 8). However, upon work-up only the original perfluoroalkyl iodides RfnI were isolated. Hence, it is concluded that the target compounds are thermodynamically and kinetically unstable with respect to Cl2 elimination, consistent with the failure of the direct reaction and a lower Lewis basicity of the iodine atom as compared to RfnCH2I.


Scheme 4: Attempted syntheses of aliphatic fluorous iodine(III) dichlorides RfnICl2.

After these experiments were carried out, we became aware of the isolation of CF3ICl2 (Rf1ICl2) from the reaction of CF3IClF and TMSCl at −40 °C [43]. This route is conceptually similar to that shown in Scheme 4, and a crystal structure of CF3ICl2 could even be obtained. However, consistent with our observations, the compound decomposed above −35 °C.

Syntheses and reactions, aryl iodides with one perfluoroalkyl group. Aromatic compounds are challenging to render highly fluorophilic [16,30,44]. For example, the singly-phase-tagged arene C6H5CH2CH2CH2Rf8 gives a 49.5:50.5 CF3C6F11/toluene partition coefficient. Values for doubly tagged analogs fall into the range (90.7–91.2):(9.3–8.8) (o, m, p-isomers), and that for the triply tagged species 1,3,5-C6H3(CH2CH2CH2Rf8)3 is >99.7:<0.3 [30]. As noted above, longer perfluoroalkyl segments increase fluorophilicities, as do shorter methylene segments (compare the partition coefficients of C6H5Rf8 (77.5:22.5) or 1,4-(Rf8)2C6H4 (99.3:0.7) with the preceding examples [29]). Thus, in considering various fluorous aryliodine(III) dichloride targets, initial efforts were directed at systems with at least two Rfn substituents per arene ring. Given the ready isolation of the dinitro-substituted aryliodine(III) dichloride II-Me in Scheme 1 [31], this was seen as a surefire objective.

However, this was not to be, so the results in this and the following section are presented in inverse chronological order, focusing first on arenes with one Rfn substituent. As shown in Scheme 5 (top), the commercially available meta diiodide 1,3-C6H4I2 was treated with copper (1.0 equiv) and Rf6I (0.5 equiv; a deficiency to help suppress dialkylation) in DMSO at 110 °C. Similar recipes have previously been used to couple aryl iodides and RfnI building blocks [45,46]. Work-up gave the target compound 1,3-Rf6C6H4I in 60% yield (based upon limiting Rf6I). Some of the previously reported dialkylation product 1,3-(Rf6)2C6H4 was also formed [47,48], but was easily separated due to its differential fluorophilicity (extraction of a CH3CN solution with perfluorohexane). An analogous procedure with Rf10I gave the higher homolog 1,3-Rf10C6H4I in 50% yield [9], and a lesser amount of what was presumed to be the dialkylation product. The analogous para diiodide 1,4-C6H4I2 gave parallel chemistry, as illustrated by the reaction with Rf6I to give 1,4-Rf6C6H4I (50% [4,12]) in Scheme 5 (bottom).


Scheme 5: Syntheses of aromatic fluorous compounds with one perfluoroalkyl group.

The three aryl iodides RfnC6H4I thus obtained were treated with NaOCl/HCl per the sequence in Scheme 2. As shown in Scheme 5, work-ups gave the corresponding iodine(III) dichlorides RfnC6H4ICl2 as pale yellow powders in 80–89% yields. Although these were clean by NMR, only one gave a correct microanalysis. As illustrated in Figure S1 (Supporting Information File 1), CDCl3/C6F6 solutions of 1,3-Rf6C6H4ICl2 and 1,4-Rf6C6H4ICl2 containing an internal standard were monitored by 1H NMR. Slow partial evolution of Cl2 to give the iodides 1,3-Rf6C6H4I and 1,4-Rf6C6H4I was observed (7% and 27% conversion over 60 h, respectively).

Syntheses and reactions, aryl iodides with two perfluoroalkyl groups. In a previously reported procedure [48], the diiodide 1,3-C6H4I2 was treated with copper (5.1 equiv) and Rf6I (2.2 equiv) in DMSO at 140 °C. As shown in Scheme 6 (top), the bis(perfluorohexyl) adduct 1,3-(Rf6)2C6H4, which was the undesired byproduct in Scheme 5 (top), was isolated in 75% yield. Subsequent iodination using NIS in fuming H2SO4/CF3CO2H afforded the "all meta" iodide 1,3,5-(Rf6)2C6H3I in 77% yield. The substitution pattern was evident from the 1H NMR spectrum.


Scheme 6: Syntheses of aromatic fluorous compounds with two perfluoroalkyl groups.

When Cl2 gas was sparged through a CF3C6H5 solution of 1,3,5-(Rf6)2C6H3I at −30 °C to −35 °C, the sample turned bright yellow. Two aliquots were removed. The 1H NMR spectrum of one (Figure 1b) showed two downfield shifted signals (cf. Figure 1a), which were attributed to the target molecule 1,3,5-(Rf6)2C6H3ICl2. Integration indicated 77:23 and 75:25 ArICl2/ArI ratios prior to and after solvent removal (room temperature, rotary evaporation). The isolated material was redissolved in CF3C6H5 and kept at −35 °C. After 7 d, the solvent was again removed by rotary evaporation, giving a 65:35 ArICl2/ArI mixture (Figure 1d). The solvent was removed from the second aliquot by oil pump vacuum at −40 °C. This gave a 35:65 ArICl2/ArI mixture as a pale white solid (Figure 1c). A variety of attempts to achieve higher conversions or isolate pure 1,3,5-(Rf6)2C6H3ICl2 were unsuccessful. It was concluded that 1,3,5-(Rf6)2C6H3ICl2 was much more labile with respect to Cl2 evolution than the fluorous aryliodine(III) dichlorides shown in Scheme 5, and that the 75–80% conversions reflected a thermodynamic limit.


Figure 1: Partial 1H NMR spectra (sp2 CH, 500 MHz, CDCl3) relating to the reaction of 1,3,5-(Rf6)2C6H3I and Cl2 in CF3C6H5 at −30 to −35 °C: (a) starting 1,3,5-(Rf6)2C6H3I; (b) aliquot taken after 24 h and removing nearly all CF3C6H5 (* = residual signals) by rotary evaporation (75:25 ArICl2/ArI); (c) aliquot taken after 24 h and removing all solvents by oil pump vacuum at −40 °C (35:65 ArICl2/ArI); (d) the sample from b, which was redissolved in CF3C6H5, kept at −35 °C for 7 d, and worked up as in b (65:35 ArICl2/ArI). The signals for the protons para and ortho to the iodine atoms are denoted ° and ◊ (red = ArI; blue = ArICl2).

Next, analogs of 1,3,5-(Rf6)2C6H3ICl2 with less electron-deficient iodine atoms were sought. As shown in Scheme 1, related fluorous aryliodine(III) dichlorides with three-methylene spacers, (Rf8CH2CH2CH2)2C6H3ICl2, had been isolated (the isomers III, IV) [17]. Recently, a potential precursor with two-methylene spacers, 1,3-(Rf8CH2CH2)2C6H4, became readily available [49]. Accordingly, it could be iodinated with I2/H5IO6 as shown in Scheme 6 (bottom) to give 1,2,4-(Rf8CH2CH2)2C6H3I [50] in 93% yield after work-up. The 1H NMR spectrum clearly indicated the regioisomer in which the iodide is ortho and para to the two alkyl substituents. This contrasts with the iodination of 1,3-(Rf6)2C6H4, in which the substituents function as meta directing groups.

As shown in Scheme 6, reactions of C6F6 or perfluoroheptane solutions of 1,2,4-(Rf8CH2CH2)2C6H3I and NaOCl/HCl gave the corresponding iodine(III) dichloride 1,2,4-(Rf8CH2CH2)2C6H3ICl2 [50] as a white powder in 89% yield. This material was stable at room temperature and gave a microanalysis consistent with a monohydrate. Hence, the iodine atom in benzenoid compounds with two Rf8CH2CH2 substituents is sufficiently Lewis basic to support a dichloride, but analogs with two Rf6 substituents are not.

Structural and computational data. Crystal structures of fluorous compounds were virtually unknown 20 years ago [51], so opportunities to acquire structural data are usually seized. Crystals of 1,3,5-(Rf6)2C6H3I could be grown as described in the experimental section. X-ray data were collected, and the structure determined, as summarized in Table 1 and the experimental section. Two views of the molecular structure and key metrical parameters are provided in Figure 2. Two perspectives of the unit cell (Z = 8) are provided in Figure 3. There are some unusual features associated with the packing and space group, and these are treated in the discussion section.

Table 1: Summary of crystallographic data for 1,3,5-(Rf6)2C6H3I.

empirical formula C18H3F26I
formula weight 840.10
diffractometer Bruker GADDS X-ray (three-circle)
temperature [K] 110(2)
wavelength [Å] 1.54178
crystal system tetragonal
space group I4
unit cell dimensions  
a [Å] 29.6474(9)
b [Å] 29.6474(9)
c [Å] 5.5976(2)
α [°] 90
β [°] 90
γ [°] 90
V3] 4920.1(3)
Z 8
ρcalcd [Mg/m3] 2.268
µ [mm−1] 12.238
F(000) 3184
crystal size [mm3] 0.40 × 0.02 × 0.02
θ limit [°] 2.11 to 59.94
index ranges [h, k, l] −33, 32; −33, 33; −6, 5
reflections collected 53384
independent reflections 3568
R(int) 0.0540
completeness (%) to θ (°) 99.8 (59.94)
max. and min. transmission 0.7919 and 0.0843
data/restraints/parameters 3568/1/407
goodness-of-fit on F2 0.991
R indices (final) [I > 2σ(I)]  
R1 0.0156
wR2 0.0355
R indices (all data)  
R1 0.0172
wR2 0.0357
largest diff. peak and hole [eÅ−3] 0.227 and −0.532

Figure 2: Two views of the molecular structure of 1,3,5-(Rf6)2C6H3I with thermal ellipsoids at the 50% probability level. Key bond lengths (Å) and angles (°): C1–I1 2.099(3), C1–C2 1.391(4), C2–C3 1.386(4), C3–C4 1.393(4), C4–C5 1.387(4), C5–C6 1.393(4), C6–C1 1.394(4), C3–C7 1.501(4), C5–C13 1.508(4), average of 10 CF–CF 1.545(5), I1–C1–C2 119.0(2), C1–C2–C3 118.8(3), C2–C3–C4 121.0(3), C3–C4–C5 119.2(3), C4–C5–C6 121.1(3), C5–C6–C1 118.5(3), C6–C1–C2 121.4(3), C6–C1–I1 119.5(2), C2–C3–C7 119.7(2), C4–C3–C7 119.3(2), C4–C5–C13 119.6(2), C6–C5–C13 119.3(2), average of 8 CF–CF–CF 115.0(10).


Figure 3: Ball-and-stick and space filling representations of the unit cell of 1,3,5-(Rf6)2C6H3I.

In order to help interpret the accessibilities and/or stabilities of the various iodine(III) dichlorides described above, the gas phase free energies of chlorination


were computed by DFT methods as described in the experimental section and summarized in Table S1 (Supporting Information File 1). The data are presented in "ladder format" in Figure 4, with the substrates that undergo more exergonic chlorinations placed higher. The energy difference between any pair of compounds is equal to that expressed by the corresponding isodesmic equation:


The validity of the data was supported by the good agreement of the computed structure of 1,3,5-(Rf6)2C6H3I with the crystal structure (Figure 2). An overlay, provided in Figure S2 (Supporting Information File 1), shows only very slightly increasing conformational differences as the perfluorohexyl groups extend from the arene. For the aliphatic compounds (RfnI, RfnCH2I, RfOxCH2ICl2), the free energies of chlorination were calculated for a series of chain lengths. As summarized in Figure 4 and tabulated in Table S1 (Supporting Information File 1), the ΔG values within each series varied by less than 0.5 kcal/mol. In all cases, vertical ionization potentials (not presented) followed analogous trends.


Figure 4: Free energies of chlorination of relevant aryl and alkyl iodides to the corresponding iodine(III) dichlorides in the gas phase (kcal/mol), presented in a ladder format (each iodide is more Lewis basic than that shown below it).

The iodine(III) dichlorides formed in the more exergonic reactions (upper portion of Figure 4) would be expected to be more stable with respect to Cl2 evolution. Thus, the data are consistent with the stability order RfnCH2ICl2 >> RfnICl2 evident from Scheme 2 and Scheme 4. However, they also imply that the ethereal systems RfOxCH2ICl2 (Scheme 3; −0.65 kcal/mol, x = 1) should be more stable than RfnCH2ICl2 (−0.53 to −0.59 kcal/mol, n = 4–8). All attempts to generate the former have been unsuccessful to date. Hence, there is either a kinetic barrier to the formation of RfOxCH2ICl2 that is not overcome under the conditions of Scheme 3, or an unrecognized, presumably non-electronic, destabilizing feature.

In the same vein, there must be a mitigating factor, such as solubility, that allows the isolation of the dinitro-substituted aryliodine(III) dichloride II-Me in pure form (Scheme 1), but not the bis(perfluorohexyl) species 1,3,5-(Rf6)2C6H3ICl2 (Scheme 6, Figure 1). The latter is derived from a more Lewis basic aryl iodide, with Cl2 addition 0.83 kcal/mol more favorable. The ortho methyl group in II-Me plays a moderately stabilizing role, with Cl2 addition to I-Me 0.73 kcal/mol more favorable than I. Otherwise, the computations (carried out with Rf6 groups to aid comparability) nicely predict the relative stabilities of the fluorous aryliodine(III) dichlorides (1,2,4-(Rf8CH2CH2)2C6H3ICl2 [50] > 1,4-Rf6C6H4ICl2 > 1,3-Rf6C6H4ICl2 > 1,3,5-(Rf6)2C6H3ICl2).


The preceding experimental data define the stability limits associated with a broad range of fluorous aliphatic and aromatic iodine(III) dichlorides. Aliphatic compounds of the formula RfnICl2 are clearly very unstable with respect to Cl2 loss, although there is literature precedent for their synthesis and isolation from other iodine(III) precursors under exacting low temperature conditions [43]. When an insulating methylene group is introduced between the fluorous moiety and the ICl2 group, the situation improves. Compounds of the formula RfnCH2ICl2 can generally be isolated, although they are somewhat labile towards Cl2 loss. In contrast, efforts to prepare the ethereal systems RfOxCH2ICl2 by the chlorination of RfOxCH2I have been unsuccessful. This poses a conundrum with respect to the DFT calculations; they seemingly possess sufficient Lewis basicity (Figure 4), but there appears to be a kinetic barrier.

In contrast, fluorous aromatic iodine(III) dichlorides bearing a single perfluoroalkyl group, RfnC6H4ICl2, are easily isolated in analytically pure form (Scheme 5), although they are still subject to slow Cl2 loss in solution (Figure S1, Supporting Information File 1). However, it has not yet proved possible to quantitatively generate analogs with two perfluoroalkyl groups by chlorinations of iodine(I) precursors (Scheme 6, top); 75–80% conversions are the maximum realized to date. In contrast, chlorinations of the doubly substituted substrates (Rfn(CH2)m)2C6H3I (m = 2, 3) go to completion, as exemplified in Scheme 1 (bottom) and Scheme 6 (bottom). The intervening methylene groups partially insulate the iodine atoms from the electron-withdrawing perfluoroalkyl segments, enhancing Lewis basicities.

However, it has not yet proved possible to access related compounds with three Rfn(CH2)m groups, at least when two of them are ortho to the iodine atom, as exemplified by V in Scheme 1 [17]. To probe this point, the DFT calculations were extended to the Rf6 homologs of the precursors of the three aryliodine(III) dichlorides in Scheme 1. These correspond to VII, VIII, and IX in Scheme 7 (top). The ΔG values obtained were −3.40, −3.75, and −4.15 kcal/mol, respectively. Thus, the third Rfn(CH2)3 substituent enhances the exergonicity of Cl2 addition. Hence, the failure to observe a reaction must represent a kinetic phenomenon. A second "ladder", augmented with the additional alkyl and aryl iodides analyzed in the discussion section, is provided in Figure S3 (Supporting Information File 1).


Scheme 7: Other relevant fluorous compounds and reactions.

Interestingly, isodesmic reactions corresponding to Equation 2 in the preceding section can actually be carried out. For example, Cl2 can be transferred from the fluorous aliphatic iodine(III) dichloride Rf1CH2ICl2 (CF3CH2ICl2) to phenyl iodide as shown in Scheme 7 (middle) [52]. The ΔG value for the addition of Cl2 to phenyl iodide is computed to be −3.86 kcal/mol, as compared to −0.72 kcal/mol for Rf1CH2I. Curiously, the introduction of two Rfn(CH2)3 substituents that are ortho/para or meta/para to iodine is thermodynamically deactivating for Cl2 addition (VII/III and VIII/IV; −3.40 to −3.75 kcal/mol), whereas the introduction of three that are ortho/para/ortho is activating (IX/V; −4.15 kcal/mol) but kinetically inhibiting for steric reasons.

As noted in the introduction, a long-standing goal has been to realize highly fluorophilic aliphatic and aromatic iodine(I) compounds and iodine(III) dichlorides. The preceding results raise the question, "quo vadis?" When the compounds RfnCH2I and RfnCH2ICl2 reach n = 15 (Scheme 2), they are close to approaching a practical solubility limit, although the former gives a highly biased CF3C6F11/toluene liquid/liquid partition coefficient. Branched analogs may be more tractable. However, DFT calculations show that chlorinations of substrates such as (Rfn)3CCH2I X (Scheme 7) would be strongly endergonic (ΔG = 3.36 kcal/mol, n = 6). Related species, such as (1) (Rfn)3CCF2CF2CH2I, which features a more remote branch site, or (2) (RfnCH2)3CCH2I, which features additional insulating methylene groups, would be more likely to give stabile iodine(III) dichlorides. Nonetheless, these types of species have never been described in the literature. Silicon has been used as a locus for branching, as exemplified by a variety of highly fluorophilic compounds of the formula (RfnCH2CH2)3SiZ (see XI in Scheme 7, Z = 4-C6H5X [53,54]). However, these feature silicon–carbon and sp3 carbon–hydrogen bonds that may be sensitive towards Cl2.

The fluorous aryl iodides that are precursors to III and IV have rather modest fluorophilicities (CF3C6F11/toluene partition coefficients (69.5–74.7):(30.5–25.3) [16]), and simply lengthening the Rf8 segments to Rf10 or even longer is unlikely to achieve biases of >99:<1. The same goes for 1,2,4-(Rf8CH2CH2)2C6H3I in Scheme 6. Accordingly, we suggest that branched fluorous aryl iodides of the formula (Rfn)3CC6H4I (XII, Scheme 7) have particular promise. DFT calculations establish exergonic chlorinations, with ΔG values of −1.93 and −1.59 kcal/mol for n = 6 and 8. This implies that the corresponding iodine(III) dichlorides should have good stabilities, equal to or better than those of 1,3- and 1,4-Rf6C6H4ICl2 in Scheme 5. However, this represents a currently unknown type of compound, and the synthesis is potentially challenging.

The following analysis of the crystal structure of 1,3,5-(Rf6)2C6H3I is kept brief, as this compound crystallizes in the same space group and crystal system (I4, tetragonal) as the corresponding bromide 1,3,5-(Rf6)2C6H3Br reported earlier [48]. The unit cell dimensions of the latter are virtually identical, with the cell volume ca. 1.5% lower (4851.7(4) vs 4920.1(3) Å3), apropos to the smaller bromine atom. The space group is both chiral and polar, and the unit cell dimensions of both compounds feature c values (5.5976(2)–5.5624 Å) that are much smaller than the a and b values (29.6474(9)–29.5335(13) Å). As noted earlier and illustrated in Figure 2 (bottom), the sixteen perfluorohexyl groups associated with the eight molecules in the unit cell lie roughly in the a/b plane. They largely segregate, as seen for most fluorous molecules [44,51,55,56], into fluorous domains.

The eight arene rings in the unit cell tilt distinctly out of the a/b plane (average angle 49.1°). Furthermore, the eight iodine atoms are oriented on the same "side" or a/b face of the unit cell. In the neighboring unit cell that adjoins the a/b face, the iodine atoms are found on the opposite side (c direction). This represents the molecular basis for the polar nature of the crystal. Also, the C–C–C–C and F–C–C–F segments in the perfluorohexyl groups do not exhibit the idealized antiperiplanar and gauche conformations associated with saturated alkanes. Rather, the torsion angles for the roughly anti linkages average 164.4(1.6)° and 166.0(3.6)°, respectively. This leads to helical motifs as shown in Figure 5, which are furthermore reproduced by the computations. The basis for this deviation, as well as a more detailed presentation of the torsional relationships, is provided elsewhere [57-59]. In a given molecule, the C6F13 groups exhibit opposite helical chiralities (see Figure S2, Supporting Information File 1), affording a meso stereoisomer.


Figure 5: Views of the helical motif of the perfluorohexyl segments in crystalline 1,3,5-(Rf6)2C6H3I (left) and the structure computed by DFT calculations (right).

Finally, attempts have been made to extend the preceding chemistry in several directions. In screening experiments, all of the fluorous iodine(III) dichlorides assayed, as well as PhICl2, were competent for the free radical chlorination of methane [25]. Under certain conditions, uncommon selectivities were apparent, but the fluorophilicities of the dichlorides or precursor iodides studied were insufficient for certain target recycling strategies. As discussed above, it is not clear how to meet these challenges at this time, although the couple Rf13CH2ICl2/Rf13CH2I would be one of several with promise. Regardless, the fluorous iodides reported herein have numerous other uses, some of which will be communicated in the near future [23].


The preceding experimental and computational data have established a strong correlation between iodine atom Lewis basicity and the feasibility of oxidizing fluorous and non-fluorous aliphatic and aromatic iodides to the corresponding iodine(III) dichlorides. Although a few surprises are noted, these are attributed to special phenomena that can drive equilibria, such as precipitation (e.g., the conversion of I-Me to II-Me in Scheme 1), or kinetic barriers (inertness of RfOxCH2I in Scheme 3 or the precursor to V in Scheme 1). With the fluorous iodides, the extent of chlorination generally provides a measure of the degree to which the electron-withdrawing perfluoroalkyl or perfluoroether segments are insulated from the Lewis basic site.


Five syntheses that are representative of the types of transformations in this study are detailed in the main article. The remaining preparations are described in Supporting Information File 1, together with data on the solvents, starting materials, and instrumentation employed.

Rf11CH2OTf. A Schlenk flask was flame dried, allowed to cool, charged with Rf11CH2OH (5.10 g, 8.52 mmol) and anhydrous CF3C6H5 (50 mL) under a N2 flow, capped, and placed in an ice bath. Then pyridine (1.0 mL, 1.0 g, 13 mmol) and (after 30 min) Tf2O (3.0 mL, 5.3 g, 14 mmol) were added dropwise by syringe with stirring. The ice bath was allowed to warm to room temperature. After 16 h, H2O (60 mL) was added. After 30 min, the organic phase was separated and dried (MgSO4). The solvent was removed by rotary evaporation. The residue was dissolved in petroleum ether/ethyl acetate (4:1 v/v). The solution was filtered through a silica pad (3 × 5 cm) and the solvent was removed by rotary evaporation to give Rf11CH2OTf as a white solid (3.82 g, 5.21 mmol, 61%), mp 77.2–79.9 °C (capillary). Anal. calcd for C13H2F26O3S: C, 21.33; H, 0.28; F, 67.46; S, 4.38; found: C, 21.44; H, 0.31; F, 67.21; S, 4.15; 1H NMR (500 MHz, acetone-d6) δ 5.55 (t, 3JHF = 13 Hz, 2H, CH2); 19F{1H} NMR (470 MHz, acetone-d6) δ −75.5 (s, 3F, SO2CF3), −81.7 (t, 4JFF = 10 Hz [60-62], 3F, CF3), −120.2 (m, 2F, CF2), −122.2 (m, 12F, 6CF2), −123.2 (m, 4F, 2CF2), −126.7 (m, 2F, CF2); 13C{1H} NMR (125 MHz, acetone-d6, partial) δ 70.0 (t, 2JCF = 28 Hz, CH2); IR (powder film, cm−1): 2924 (w), 2855 (w), 1418 (m), 1202 (s), 1140 (s), 1103 (w), 1023 (m), 854 (m), 822 (m).

Rf11CH2I. A round bottom flask was charged with Rf11CH2OTf (3.01 g, 4.11 mmol), NaI (10.2 g, 68.0 mmol), and acetone (30 mL), and fitted with a condenser. The flask was placed in a 75 °C oil bath and the mixture was stirred. After 1 d, the bath was removed and the mixture was allowed to cool. The solvent was removed by rotary evaporation. Then Et2O (50 mL) and H2O (40 mL) were added with stirring. After 5 min, the dark brown organic phase was separated, washed with saturated aqueous Na2S2O3 until it became colorless, and dried (Na2SO4). The solvent was removed by rotary evaporation and the residue was dissolved in hexanes/ethyl acetate (20:1 v/v). The solution was kept at −35 °C until a precipitate formed. The solid was collected by filtration and washed with cold hexanes to give Rf11CH2I as a white solid (2.00 g, 2.82 mmol, 69%), mp (capillary): 97.8–98.2 °C. Anal. calcd for C12H2F23I: C, 20.30; H, 0.28; F, 61.54; I, 17.87; found: C, 20.20; H, 0.16; F, 61.29; I, 17.68; 1H NMR (500 MHz, acetone-d6) δ 4.06 (t, 3JHF = 19 Hz, 2H, CH2); 19F{1H} NMR (470 MHz, acetone-d6) δ −81.6 (t, 4JFF = 10 Hz [60-62], 3F, CF3), −107.0 (m, 2F, CF2), −122.2 (m, 14F, 7CF2), −123.2 (m, 2F, CF2), −126.7 (m, 2F, CF2); 13C{1H} NMR (125 MHz, acetone-d6, partial) δ −3.8 (t, 2JCF = 25 Hz, CH2); IR (powder film, cm−1): 2986 (w), 2874 (w), 1422 (w), 1373 (w), 1348 (w), 1234 (s), 1200 (s), 1140 (s), 1040 (m), 858 (m).

Rf11CH2ICl2. A round bottom flask was charged with Rf11CH2I (1.01 g, 1.42 mmol), C6F6 (1.4 mL), and CH3CN (14 mL) with stirring. Aqueous NaOCl (2.5% w/w, 21 mL) and then conc. HCl (10 mL) were slowly added. After 2 h, a pale yellow precipitate began to form. After 5 h, the mixture was filtered. The filter cake was washed with hexane (10 mL) and air dried (4–5 h) to give Rf11CH2ICl2 as a pale yellow powder (0.90 g, 1.15 mmol, 81%), mp 122.1–125.4 °C (capillary). Anal. calcd for C12H2F23Cl2I: C, 18.46; H, 0.26; F, 55.96; Cl, 9.08; found: C, 16.76; H, 1.16; F, 50.15; Cl, 7.98 [63]; 1H NMR (500 MHz, acetone-d6) δ 5.44 (t, 3JHF = 17 Hz, 2H, CH2); 19F{1H} NMR (470 MHz, acetone-d6, partial) δ −106.7 (m, 2F, CF2); IR (powder film, cm−1): 3030 (w), 2970 (w), 1392 (w), 1373 (w), 1348 (w), 1315 (w), 1202 (s), 1148 (s), 1046 (m), 860 (m).

1,3-Rf6C6H4I. A Schlenk tube was charged with copper (1.26 g, 20.0 mmol) and DMSO (30 mL) and placed in a 105 °C oil bath. The mixture was sparged with N2 with stirring (30 min), and 1,3-diiodobenzene (6.60 g, 20.0 mmol) was added. After a second sparge, Rf6I (4.48 g, 10.0 mmol) was added in portions over 30 min under a N2 flow with stirring. The tube was sealed and placed in a 110 °C oil bath. After 4 d, the mixture was cooled to room temperature and poured into H2O (100 mL). Then Et2O (100 mL) was added with stirring. After 1 h, the aqueous phase was separated and extracted with Et2O (5 × 50 mL). The combined organic phases were dried (Na2SO4) and the solvent was removed by rotary evaporation. The residue was dissolved in CH3CN (10 mL). The sample was extracted with perfluorohexane (5 × 5 mL). The fluorous layers were combined, concentrated to 2 mL, and extracted with acetone (5 × 3 mL). The solvent was removed from the extracts by oil pump vacuum to give 1,3-Rf6C6H4I as a colorless oil (3.16 g, 6.05 mmol, 60% based upon Rf6I). Anal. calcd for C12H4F13I: C; 27.61; H, 0.77; F, 47.31; found: C, 28.09; H, 0.67; F, 48.59 [63]. The solvent was removed from the concentrated perfluorohexane extract by oil pump vacuum to give 1,3-(Rf6)2C6H4 as a light yellow oil (1.07 g, 1.51 mmol, 15%) [48]. The 1H NMR spectrum matched those in the literature [47,48]. 1H NMR (500 MHz, CD2Cl2) δ 8.01 (s, 1H), 7.96 (d, 3JHH = 8 Hz, 1H), 7.61 (d, 3JHH = 8 Hz, 1H), 7.26 (t, 3JHH = 8 Hz, 1H); 19F{1H} (470 MHz, CD2Cl2) δ −82.0 (t, 4JFF = 9 Hz [60-62], 3F, CF3), −111.7 (t, 4JFF = 15 Hz [60-62], 2F, CF2), −122.1 (m, 2F, CF2), −122.3 (m, 2F, CF2), −123.5 (m, 2F, CF2), −127.0 (m, 2F, CF2); 13C{1H,19F} (125 MHz, CD2Cl2) δ 141.9, 136.4, 130.8, 126.8, 118.0 (5 × s, C6H4), 116.1, 115.8, 112.0, 111.5, 111.1, 109.3 (5 × s, 5CF2/CF3), 94.4 (s, CI).

1,3-Rf6C6H4ICl2. A round bottom flask was charged 1,3-Rf6C6H4I (0.523 g, 1.00 mmol), C6F6 (1 mL), and CH3CN (10 mL) with stirring. Aqueous NaOCl (2.5% w/w, 10 mL) followed by conc. HCl (10 mL) were slowly added. After 30 min, a pale yellow precipitate began to form. After 3 h, the mixture was filtered. The filter cake was washed with H2O (5 mL) and hexane (10 mL) and air dried (2 d) to give 1,3-Rf6C6H4ICl2 as a pale yellow powder (0.477 g, 0.804 mmol, 80%). Anal. calcd for C12H4F13Cl2I: C, 24.31; H, 0.68; F, 41.65; found: C, 23.89; H, 0.38; F, 49.81 [63]; 1H NMR (500 MHz, CDCl3/C6F6) δ 8.54–8.52 (m, 2H), 7.94 (d, 3JHH = 8 Hz, 1H), 7.79 (t, 3JHH = 8 Hz, 1H); 19F{1H} NMR (470 MHz, CDCl3/C6F6) δ −82.3 (t, 4JFF = 9 Hz [60-62], 3F, CF3), −112.0 (t, 4JFF = 15 Hz [60-62], 2F, CF2), −124.4 (m, 4F, 2CF2), −123.7 (m, 2F, CF2), −127.3 (m, 2F, CF2).

Partition coefficients. The following is representative. A 20 mL vial was charged with a CF3C6F11 solution of RfnCH2I (n = 11, 15; 5.0 × 10−2 M, 4.0 mL) and toluene (4.0 mL), capped, and vigorously stirred. After 10 min at room temperature (24 °C), aliquots were removed from the fluorous (2.0 mL) and organic (2.0 mL) phases. The solvent was evaporated from each, and the residues were dried under vacuum. A solution of Ph2SiMe2 (internal standard; 0.0055 mL) in acetone-d6/CF3C6H5 (1:1 v/v; 10.0 mL) was prepared. Each residue was dissolved in 1.00 mL of this solution and 1H NMR spectra were recorded. The relative peak integrations gave the corresponding partition coefficients.

Crystallography. A solution of 1,3,5-(Rf6)2C6H3I (ca. 0.05 g) in CHCl3/C6F6 (1.0 mL, 4:1 v/v) in an NMR tube was allowed to concentrate. After 2 d, colorless needles with well defined faces were obtained. Data were collected as outlined in Table 1. Integrated intensity information for each reflection was obtained by reduction of the data frames with the program APEX2 [64]. Data were corrected for Lorentz and polarization factors, and using SADABS [65] for absorption and crystal decay effects. The structure was solved by direct methods using SHELXTL/XS [66,67]. Non-hydrogen atoms were refined with anisotropic thermal parameters. Hydrogen atoms were placed in idealized positions and refined using a riding model. The structure was refined (weighted least squares refinement on F2) to convergence [66-68].

Calculations. Computations were performed with the Gaussian09 program package, employing the ultrafine grid (99,590) to enhance accuracy [69]. Geometries were optimized using density functional theory (DFT). The B3LYP [70-72] functional was employed with an all-electron 6-311+G(d,p) [73] basis set on all atoms except iodine, which was treated using an effective core potential, SDD [74]. The optimized structures were subjected to frequency calculations (using the same functional and basis set as before) to confirm that all structures were local minima and to obtain the free energies of chlorination (Figure 4 and Table S1, Supporting Information File 1).

Supporting Information

Full details and product characterization for all the syntheses described in Schemes 2, 3, 5, and 6, information on the solvents, starting materials, and instrumentation employed, and additional spectroscopic, structural, and computational data, including a molecular structure file that can be read by the program Mercury [75] and contains the optimized geometries of all computed structures [76].

Supporting Information File 1: Experimental section continued.
Format: PDF Size: 525.6 KB Download
Supporting Information File 2: Molecular structure file.
Format: MOL2 Size: 119.2 KB Download


The authors thank the Qatar National Research Fund for support (project number 5-848-1-142), the Laboratory for Molecular Simulation and Texas A&M High Performance Research Computing for resources, Prof. Michael B. Hall and Dr. Lisa M. Pérez for helpful discussions, and Dr. Markus Jurisch for preliminary studies of Rf13CH2OTf and Rf13CH2I.


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