Skip to main content
NCBI home page
Wiley Open Access Collection logoLink to Wiley Open Access Collection
. 2022 Feb 9;28(14):e202104308. doi: 10.1002/chem.202104308

Synthesis, Reactivity and Structural Properties of Trifluoromethylphosphoranides

Oleg O Shyshkov 2, Alexander A Kolomeitsev 2, Berthold Hoge 3, Enno Lork 2, Axel Haupt 1,✉, Mira Keßler 3,✉, Gerd‐Volker Röschenthaler 1,✉
PMCID: PMC9305102  PMID: 35025112

Abstract

Phosphoranides are interesting hypervalent species which serve as model compounds for intermediates or transition states in nucleophilic substitution reactions at trivalent phosphorus substrates. Herein, the syntheses and properties of stable trifluoromethylphosphoranide salts are reported. [K(18‐crown‐6)][P(CF3)4], [K(18‐crown‐6)][P(CF3)3F], and [NMe4][P(CF3)2F2] were obtained by treatment of trivalent precursors with sources of CF3 − or F− units. These [P(CF3)4‐nFn]− (n=0–2) salts exhibit fluorinating (n=1–2) or trifluoromethylating (n=0) properties, which is disclosed by studying their reactivity towards selected electrophiles. The solid‐state structures of [K(18‐crown‐6)][P(CF3)4] and [K(18‐crown‐6)][P(CF3)3F] are ascertained by single crystal X‐ray crystallography. The dynamics of these compounds are investigated by variable temperature NMR spectroscopy.

Keywords: fluorine, fluorination, hypervalent compounds, phosphorus, trifluoromethylation

Different trifluoromethylated phosphoranides are accessible upon treatment of trifluoromethylated phosphanes, such as P(CF3)3, with a source of F− or CF3 − in presence of a stabilizing counterion. The hypervalent compounds have been investigated by NMR spectroscopic as well as X‐ray crystallographic methods, gaining insights into their stability and structural behavior. In addition, the phosphoranides have revealed fluorinating and trifluoromethylating properties towards electrophiles.

graphic file with name CHEM-28-0-g003.jpg

Introduction

To date, a number of hypervalent phosphorus compounds has been studied, including phosphoranides which feature a formally negatively charged, tetracoordinated phosphorus atom. They turned out to be useful models for the intermediates or transition states in nucleophilic substitution reactions at trivalent phosphorus substrates. [1] In general, phosphoranides are accessible by three major approaches, namely the addition of X− to a phosphorus(III) compound (Lewis acid‐base interaction), [2] deprotonation of a pentavalent phosphorane R4PH, [3] or oxidation of an anionic and monovalent species, such as [P(CN)2]− by Cl2 or Br2. [4] As a rule of thumb, phosphoranides have to be stabilized by electron‐withdrawing substituents X with a low tendency to function as leaving groups at the same time. The first phosphoranide to be isolated was [PBr4]−, followed by the chloro‐ and fluoro‐analogues [PCl4]− and [PF4]−.[ 2 , 5 , 6 ] However, tetraiodo phosphoranide [PI4]− has eluded observation so far, which is in line with the decreasing acceptor properties of the phosphanes within the homologous series. In solution, the equilibrium between PX3, X− and [PX4]− lies well on side of the educts for X=Br and to some extent on side of the educts for X=Cl, whereas it lies on side of the phosphoranide for X=F.[ 2 , 5 , 6 ] Structurally, the phosphoranides are derived from a trigonal bipyramid, with the sterically active lone‐pair in an equatorial position. Axial and equatorial substituents of the [PF4]− ion are interconverted via Berry pseudo rotation resulting in indifferent NMR resonances at room temperature. However, the exchange is slowed down at low temperatures, facilitating the differentiation of two types of substituents via NMR spectroscopy. [6] Apart from the aforementioned tetrahalophosphoranides, a few cyclic organophosphoranides have also been described.[ 3 , 7 ] Moreover, a few derivatives have been prepared containing both, organic residues and (pseudo‐)halide groups at the phosphorus atom, for example [PR(CN)2X]− with R=Me, Et, Ph, C6F5 and X=Cl, Br, I. [8] Basically, halide substituents at [PX4]− may be replaced by perfluoroalkyl functionalities. Thus, trifluoromethylated phosphoranides had been predicted to be relatively stable, long before their verification by experiment, [1] and the analogous pentafluoroethylated phosphoranides have been reported only recently. [9] The homoleptic tetrakis(trifluoromethyl)phosphoranide has been authenticated as an anion in the extremely unstable salt [(Me2N)3S][P(CF3)4] and in a slightly more stable, but nevertheless still very reactive and pyrophoric, tetramethylammonium derivative, [NMe4][P(CF3)4]. [10] A similar increase in stability has been observed for the corresponding salts [(Me2N)3S][P(CF3)3F] and [NMe4][P(CF3)3F]. The difluorobis(trifluoromethyl)‐phosphoranide [P(CF3)2F2]− results from difluorocarbene extrusion of [P(CF3)3F]− or by addition of NMe4F to the phosphine P(CF3)2F. [11] So far, detailed NMR‐spectroscopic and crystallographic examinations of these compounds have been thwarted by their instability. The most suitable starting material for the preparation of trifluoromethyl‐containing phosphoranides is P(CF3)3, which is well known as a ligand in transition metal coordination chemistry. [12] This phosphine may be prepared for example by treatment of CF3I with white phosphorus, by reaction of Cd(CF3)2 with PI3, by reduction of the phosphorane (CF3)3PF2, or by combining CF3Br with P(NEt2)3 and P(OPh)3. [13] The aforementioned methods, however, all have significant drawbacks, since they are either inconvenient, cost‐intensive or require the employment of toxic or environmentally harmful compounds. Thus, an alternate synthesis involving relatively non‐hazardous, commercially available reagents was developed. The reaction of triphenyl phosphite with Me3SiCF3 in the presence of an equimolar amount of CsF afforded P(CF3)3 in 98 % yield. Using only catalytic amounts of CsF, at least 90 % yield were accomplished. [14]

Herein, we would like to report upon the synthesis, properties, and reactivity of stable trifluoromethyl phosphoranides derived from P(CF3)3.

Results and Discussion

P(CF3)3 (1) was obtained by treatment of P(OPh)3 with Me3SiCF3 in the presence of small amounts of NMe4F or KOPh in ethereal solvents, after a modified literature procedure. [14] The reaction is performed in the temperature range 20 to 50 °C, affording phosphine 1 in yields of 80–85 % (Scheme 1). [15] The starting materials are preferably used stoichiometrically to avoid contamination with by‐products. An excess of the phosphite leads to the formation of (CF3)P(OPh)2 and CF3H, whereas larger amounts of the silane mainly produce traces of CF3H. The product is easily pumped off and subsequently distilled at atmospheric pressure.

Scheme 1.

Scheme 1

Open in a new tab

Preparation of P(CF3)3 (1). Triglyme=2,5,8,11‐tetraoxadodecane.

Treatment of P(CF3)3 (1) with Me3SiCF3 in the presence of fluoride salts leads to the formation of corresponding [P(CF3)4]− salts. To obstruct the notorious tendency to decompose, the [NMe4]+ ion in [NMe4][P(CF3)4] [10] should be replaced by more bulky cations, such as [K(18‐crown‐6)]+ which previously allowed synthesis and X‐ray structural characterization of [K(18‐crown‐6)][P(CF3)2]. [16] Therefore, we attempted the preparation of stable phosphoranides [P(CF3)3F]− and [P(CF3)4]− by combination of P(CF3)3 with KF/18‐crown‐6 or KF/Me3SiCF3/18‐crown‐6, respectively. Compounds [K(18‐crown‐6)][P(CF3)4] (2) and [K(18‐crown‐6)][P(CF3)3F] (3) are accessible by this approach in 92 % and 98 % yield (Scheme 2). [15] Attempts to prepare pure salts of the difluorobis(trifluoromethyl)phosphoranide ion, [P(CF3)2F2]−, failed when P(CF3)2F was reacted with NMe4F or KF/18‐crown‐6. With large fluoride excess, a maximum of 60 % phosphoranide was achieved. In a consecutive reaction of [P(CF3)2F2]− with the starting phosphine, [P(CF3)2F3{P(CF3)2}]− was formed as a byproduct. The reaction is believed to proceed via an adduct formed by the phosphoranide and phosphine, [P(CF3)2F{P(CF3)2F2}]−, and subsequent fluoride transfer.

Scheme 2.

Scheme 2

Open in a new tab

Preparation of stable trifluoromethylated phosphoranides 2, 3 and 4.

Interestingly, [NMe4][P(CF3)2F2] (4) is formed, when the mono‐trifluoromethyl phosphine (CF3)PF2 is allowed to react with NMe4F in diethyl ether at room temperature (Scheme 2). [15] As a side product, PF3 is liberated, which implies a low affinity between PF3 and CF3 − and therefore rationalizes the preferred formation of [P(CF3)2F2]− instead of expected [P(CF3)F3]−. The latter mono‐trifluoromethylated species is still unknown and all our attempts to synthesize and detect this species failed. Thus, combination of (CF3)PF2 with NMe4F in CH3CN or treatment of PF3 with NMe4F and Me3SiCF3 did not give unambiguous evidence for the transient existence of [NMe4][P(CF3)F3].

Next, we looked at the stability of the novel trifluoromethylphosphoranide salts 2 and 3 in comparison to the related [NMe4]+ compounds. Disregarding the nature of the counter ion, most of the trifluoromethylated phosphoranides suffer from facial difluorocarbene elimination, leading to a mixture of (trifluoromethyl)fluoro derivatives.

The facile loss of a CF3 group may be due to the axial 3‐center‐4‐electron bonding. Consistently, apical P−C bonds are weakened in comparison to 2‐center‐2‐electron P−C bonds. In stark contrast to the corresponding [NMe4]+ salts, the decomposition of which commences at about −45 °C in dimethoxyethane (DME) solution, derivative [K(18‐crown‐6)][P(CF3)4] (2) decomposes very slowly at ambient temperature. The stability of 2 is considerably improved in the presence of an equivalent amount of P(CF3)3 (1). Thus, 74 % of 2 remained intact after 24 h in DME solution mixed with 1. A similar behavior was encountered for DME solutions of [K(18‐crown‐6)][P(CF3)3F] (3) and the analogous [NMe4][P(CF3)3F]. [NMe4][P(CF3)3F] decomposed in DME solution at room temperature within two weeks, whereas 85 % of 3 remain unaffected under these conditions. In addition, storage of solid [NMe4][P(CF3)3F] at 20 °C for 12 days led to a 2 : 1 mixture of [NMe4][P(CF3)3F] and [NMe4][P(CF3)2F2].

Solid [NMe4][P(CF3)4] tends to spontaneously explode, whereas solid [K(18‐crown‐6)][P(CF3)4] (2) is relatively stable at room temperature. The remarkable instability of the ammonium salt may be rationalized by the reaction of the strong base CF3 − with [NMe4]+ which would result in the formation of the very reactive and unstable ammonium ylide Me3N+−CH2 −. [17] Analysis of the decomposition products revealed only traces of P(CF3)3, but significant amounts of CF3H and NMe3. We also found, that :CF2 preferentially inserts into α‐C−H bonds of ethereal solvents, as it has been described earlier. [18]

Clearly, all trifluoromethyl phosphoranides under discussion are thermally unstable and very reactive. The obtained products are colorless to pale yellow solids which are sensitive towards moisture and oxygen, the latter causing spontaneous ignition. Analytically pure compounds are only obtained by drying in vacuo at 0 to −30 °C. In contrast, drying at room temperature leads invariantly to impure samples. Moreover, the phosphoranides are not characterized by sharp melting points, since they always suffer from decomposition prior to liquefaction. Thereby, the [NMe4]+ salts decompose and melt at lower temperatures than the corresponding compounds 2 and 3, featuring cation [K(18‐crown‐6)]+. Pyrolysis of [NMe4]+ phosphoranides yields mixtures of PF3, P(CF3)3, CF3H and NMe3 in addition to an intractable black solid, whereas [K(18‐crown‐6)]+ salts mainly liberate P(CF3)3 as well as some PF3 and CF3H. Fast hydrolysis of the phosphoranides in wet DME yields [PH(CF3)(=O)O]−, whereby [P(CF3)3F]− is slightly less readily hydrolyzed than [P(CF3)4]−. The hydrolysis of [PH(CF3)(=O)O]− is very slow, and requires a few drops of aqueous NaOH to produce CF3H and HP(=O)(OH)2.

The remarkable reactivity of the phosphoranides under discussion is based upon the loss of an axial ligand which may be conveniently trapped by suitable electrophiles. In keeping with this, [P(CF3)4]− is a powerful trifluoromethylating reagent, whereas the anions [P(CF3)3F]− and [P(CF3)2F2]− behave as fluoride donors. This is nicely illustrated by the clean reaction of 2, 3, and 4 with Me3SiCl which furnished products Me3SiCF3 and Me3SiF, respectively.

The ammonium salt [NMe4][P(CF3)2ClF] is generated in quantitative yield, if [NMe4][P(CF3)2F2] is added to an equimolar amount of Me3SiCl at −30 °C. On the other hand, reactions of the phosphoranides [P(CF3)2F2]− and [P(CF3)3F]− with Me3SiCF3 yield [P(CF3)4]−. Upon warming of the reaction mixture from −60 °C to room temperature, the phosphoranides also react with SO2 and aryl sulfonyl chlorides Ar−SO2Cl under formation of [X‐SO2]− and Ar−SO2X, respectively (Scheme 3). [15] Moreover, boric esters and aldehydes are trifluoromethylated by [P(CF3)4]− with CF3H as a major side product. Thus, in the reaction of 2 with B(OMe)3, [K(18‐crown‐6)][B(OMe)3(CF3)] is formed. Treatment of 2 with benzaldehyde and subsequent aqueous workup yields PhCH(CF3)(OH).

Scheme 3.

Scheme 3

Open in a new tab

Fluorination and trifluoromethylation by trifluoromethylated phosphoranides.

Interestingly, trifluoromethyl phosphoranides do not react with neutral 1,3‐dimethyl‐2,2‐difluoroimidazolidine (DFI). However, the corresponding imidazolium triflate is trifluoromethylated by [P(CF3)4]− or fluorinated by [P(CF3)3F]− under liberation of P(CF3)3 (Scheme 3).

Furthermore, trifluoromethylated phosphoranides are prone to oxidation. Thus, high yields of sixfold coordinated trifluoromethyl phosphates [P(CF3)3XY2]− (X=CF3, F; Y=Cl; F) are generated upon oxidation of the phosphoranides with Cl2 or Deoxo‐Fluor® ((MeOCH2)2NSF3) at low temperature. However, treatment of the phosphoranides with hexafluoroacetone does not lead to the oxidation of the phosphorus center. Transfer of CF3 − or F− anions to the ketone under formation of [(F3C)3CO]− or [F(F3C)2CO]− was observed, instead.

Methylation of the phosphoranides yields pentavalent trifluoromethyl phosphates (Scheme 4). In case of [P(CF3)4]−, methyl transfer is achieved by MeOTf in DME at −40 °C. For the methylation of [P(CF3)3F]−, MeI has been used in DME solution at room temperature. [15] Since the initially formed phosphoranes are strong Lewis acids, they cannot be isolated but immediately abstract CF3 − or F− from a second equivalent of the starting phosphoranide. Here should be stated that the conceivable addition of the CF3 − anion on a phosphorane is limited by steric hindrance, and fluoride addition to the phosphorane is preferred. Thus, methylation of [P(CF3)4]− yields [P(CH3)(CF3)4F]− and methylation of [P(CF3)3F]− yields [P(CH3)(CF3)3F2]−.

Scheme 4.

Scheme 4

Open in a new tab

Methylation of trifluoromethylated phosphoranides and subsequent reaction with a second equivalent phosphoranide.

Elucidation of the solid‐state structures of the compounds [K(18‐crown‐6)][P(CF3)3F] (3) (Figure 1) and [K(18‐crown‐6)][P(CF3)4] (2) (Figure 2) were effected by means of single crystal X‐ray crystallography. [19] [P(CF3)3F]− salt 3 crystallizes in the triclinic space group P‐1, whereas [P(CF3)4]− salt 2 crystallizes in the monoclinic space group P21/c with three geometrically nonequivalent anions, therefore average values of structural parameters of 2 are given hereinafter. In both cases, the coordination geometry of the phosphoranide anions is based on distorted trigonal bipyramids, where the lone pair at the phosphorus center is sterically active and occupies one of the equatorial positions. For both compounds, a few structural similarities are observed. The axial bonds in the phosphoranides (3: d(P‐CF3ax)=1.97(2) Å, d(P−F)=1.79(1) Å; 2: d(P‐CF3ax)=2.049 Å) are elongated with respect to the neutral species PF3 (d(P−F)=1.570(1) Å, gas phase electron diffraction – GED) [20] and P(CF3)3 (1) (d(P‐CF3)=1.93(2) Å, GED) [21] due to the 3‐center‐4‐electron bonding. The axial P−F bond is significantly shorter than the axial P−C bond in the [P(CF3)3F]− anion of compound 3, as could be expected. The equatorial P−CF3 bonds of 2 are 1.894 Å on average and thus, comparable to the P−C bonds in the neutral compounds P(CF3)3 (1) (1.93(2) Å, GED) [21] or (F3C)2P−P(CF3)2 (1.886(4) and 1.880(4) Å via X‐Ray; 1.90 Å via GED). [22]

Figure 1.

Figure 1

Open in a new tab

Solid‐state packing of [K(18‐crown‐6)][P(CF3)3F] (3) exhibiting zig‐zag chains along the a‐axis. The equatorial CF3 groups are disordered. Ellipsoids are at a probability level of 50 %, hydrogen atoms are omitted for clarity.

Figure 2.

Figure 2

Open in a new tab

Extract of the solid‐state packing of [K(18‐crown‐6)][P(CF3)4] (2) revealing zig‐zag chains along the c‐axis (left) and structure of a [P(CF3)4]− anion (right). Ellipsoids are at a probability level of 50 %, hydrogen atoms are omitted for clarity.

Furthermore, the CPC‐angles between the two equatorial CF3‐groups are almost identical in 2 and 3 (104.06(2) to 105.05(1)°), but slightly larger than the corresponding CPC‐angle in the neutral phosphine P(CF3)3 (1) (100(3)°, GED). The angles between the apical substituents are smaller than 180° and amount to 170.47(1)° for 3 and 174.74(1) to 176.02(1)° for 2. The reasons for this distortion are repulsive interactions of the axial substituents with the lone pair, which is especially pronounced for the apical fluorine substituent in compound 3. Thus, the CPC angles between axial and equatorial CF3‐groups in both anions are virtually identical (90.79(1)° and 89.94(1)° in 3 and on average, 89.1° in 2).

The phosphoranide salts 3 and 2 differ in their solid‐state packing, since [P(CF3)4]− in 2 forms zig‐zag chains along the c‐axis. The chains are composed of K+ centers which are symmetrically surrounded by 18‐crown‐6 and two phosphoranide anions. The bridging between two K‐centers is realized by two fluorine atoms of each a single axial CF3 group of the phosphoranide. In each cell, there are three geometrically inequivalent anions. In contrast, [P(CF3)3F]− in compound 3 has two ion‐pairs per unit cell and exhibits a comparably simple arrangement, resulting in zig‐zag chains along the a‐axis of the unit cell. Here, bridging between the cations is realized by the two axial substituents of the phosphoranide anion, i. e. the axial fluorine atom and one of the fluorine atoms of the axial CF3 group. For both phosphoranide salts 2 and 3, the geometry of the cations and anions is determined by the pursuit for a maximum number of K−F contacts with preferably minimal distances. Since one observes rather large K−P distances of 4.454(3) to 5.436(7) Å (2) and 3.649(9) Å (3), respectively, this indicates in both cases a packing of well‐isolated ions.

Furthermore, trifluoromethyl phosphoranides 2 and 3 were studied by variable temperature NMR spectroscopy. Their spectra are compared with those of the corresponding tetramethylammonium derivatives. Phosphoranides may undergo inter‐ and intramolecular exchange processes. They tend to form an equilibrium with their precursors in solution, and pseudorotation may lead to an exchange of equatorial and axial substituents. In keeping with this, the 31P NMR spectrum of [NMe4][P(CF3)3F] shows a slightly broadened decet at −38 °C in acetonitrile solution, whereas the 19F NMR spectrum is characterized by a broad singlet and a doublet in the ratio 1 : 9. The lack of fine coupling implies a fast exchange process. Upon addition of excess NMe4F this exchange is considerably slowed down, so that a doublet of quartets of septets can be distinguished in the 31P NMR spectrum. In contrast, the exchange is very slow in DME solution, which allows differentiation of the axial and equatorial CF3 groups. However, a slow exchange remains as evidenced by slightly broad signals. Again, these dynamics can be suppressed by addition of small amounts NMe4F resulting in a well resolved 31P NMR resonance at room temperature. Cooling a DME solution of [NMe4][P(CF3)3F] to −60 °C in absence of NMe4F leads to the same observation. A fast exchange process takes place in DME above 60 °C, which can be identified by variable temperature 31P NMR spectroscopy. At −50 °C the 31P NMR signal is fully resolved (Figure 3), whereas a broad multiplet is found at about 50–60 °C, finally resulting in a broad decet at 80 °C. Consequently, the CF3 groups give rise to two broad singlets in the 19F NMR spectrum at 50 °C which fuse to one broad singlet at 60 °C.

Figure 3.

Figure 3

Open in a new tab

Experimental (top) and simulated [23] (bottom) 31P NMR resonance of [NMe4][P(CF3)3F] at −50 °C. The splitting may be described as a doublet of septets of quartets. Simulation yields the coupling constants 1 J(P−F)=385 Hz; 2 J(P‐CF 3eq.)=85 Hz and 2 J(P‐CF 3ax.)=29 Hz.

In contrast, 19F and 31P NMR spectra of [K(18‐crown‐6)][P(CF3)3F] (3) in DME at −90 °C do not allow a differentiation between axial and equatorial CF3 groups. The appearance of the spectra points to a fast exchange process similar to that observed in MeCN solution. We investigated the influence of the counterions on the spectra in DME in greater detail. If a mixture of KF/18‐crown‐6 is added to a DME solution of [NMe4][P(CF3)3F], no changes in the NMR resonances take place. In contrast, the addition of NMe4F to [K(18‐crown‐6)][P(CF3)3F] (3) results in dramatic transformations in the spectrum. Exchange processes are significantly slowed down, so that partially resolved signals are observable in the same way as for [NMe4][P(CF3)3F] in MeCN at −60 °C.

Presumably, [NMe4][P(CF3)3F] exists as a tight pair of contact ions in DME, which leads to decelerated exchange processes. The [NMe4]+ cation probably interacts with the phosphorus atom, leading to the formation of P−F bonds. On the other hand, the [K(18‐crown‐6)]+ cation rather interacts with the axial fluorine atom of the anion than with the phosphorus atom, as evident from the molecular structure, facilitating a fast exchange process.

The resonances of the axial and equatorial CF3 groups of [K(18‐crown‐6)][P(CF3)4] (2) are fully resolved at −50 °C. Upon warming an intermediate behavior is observed at 0 °C, whereas a fast exchange process occurs at 80 °C. In comparison, [NMe4][P(CF3)4] exhibits fully resolved spectra at −45 °C but it cannot be observed above 10 °C due to its thermal instability.

In solution, [P(CF3)4]− and [P(CF3)3F]− are generally stabilized by the addition of P(CF3)3 (1). Since phosphoranides and their precursors form an equilibrium in solution, the addition of one of the reactants entails a shift of this equilibrium to the side of the phosphoranide. Thus, [K(18‐crown‐6)][P(CF3)4] (2) already exhibits resolved 19F NMR spectra with fine splitting at −30 °C in the presence of P(CF3)3 (1). The NMR resonances of [K(18‐crown‐6)][P(CF3)3F] (3), on the other hand, are broadened, which might arise from interactions of the axial fluorine substituent of the phosphoranide with the phosphine.

Conclusion

In conclusion, we have demonstrated that stable trifluoromethylated phosphoranides are accessible upon treatment of trifluoromethyl phosphines with a source of F− or CF3 −, respectively. The anionic species are efficiently stabilized by crown ether‐coordinated K+ cations. The [K(18‐crown‐6)]+ salts have been isolated as solids and are thus significantly more stable than the known [NMe4]+ derivatives. As a general trend, trifluoromethylated phosphoranides tend to decompose under formal liberation of difluorocarbene, giving rise to mixed fluoro(trifluoromethyl)phosphoranides. The typical reactivity of [P(CF3)4‐nFn]− (n=0‐2) is determined by the tendency to donate one of the axial substituents, thus they serve as trifluoromethylating (n=0) and fluorinating agents (n=1‐2) which has been demonstrated by reactions with several different electrophiles. Moreover, the trivalent phosphoranides are oxidized by chlorine or Deoxo‐Fluor® to give pentavalent trifluoromethylphosphates. Solid‐state structures of [K(18‐crown‐6)][P(CF3)4] and [K(18‐crown‐6)][P(CF3)3F] have been elucidated. The examined phosphoranide anions exhibit a distorted trigonal bipyramidal geometry, where the sterically active lone pair leads to a decrease of the bond angle between the axial substituents. Elongated distances to the axial substituents are evident, due to the 3‐center‐4‐electron bonding. Finally, the solid‐state packing of the trifluoromethyl phosphoranides [K(18‐crown‐6)][P(CF3)4] and [K(18‐crown‐6)][P(CF3)3F] reveals zig‐zag chains, which are formed by an alternating arrangement of anions and cations, bridged by K−F interactions. Apart from that, variable temperature NMR experiments in different solvents disclose exchange processes in the phosphoranides.

Conflict of interest

The authors declare no conflict of interest.

1.

Supporting information

As a service to our authors and readers, this journal provides supporting information supplied by the authors. Such materials are peer reviewed and may be re‐organized for online delivery, but are not copy‐edited or typeset. Technical support issues arising from supporting information (other than missing files) should be addressed to the authors.

Supporting Information

Click here for additional data file. (1.1MB, pdf)

Acknowledgements

A. H. and G.‐V. R. are grateful for support by Jacobs University Bremen gGmbH and the University of Bremen. Open Access funding enabled and organized by Projekt DEAL.

In memoriam Alexander A. Kolomeitsev.

O. O. Shyshkov, A. A. Kolomeitsev, B. Hoge, E. Lork, A. Haupt, M. Keßler, G.-V. Röschenthaler, Chem. Eur. J. 2022, 28, e202104308.

Contributor Information

Dr. Axel Haupt, Email: a.haupt@jacobs-university.de.

Mira Keßler, Email: mira.kessler@uni-bielefeld.de.

Prof. Dr. Gerd‐Volker Röschenthaler, Email: g.roeschenthaler@jacobs-university.de.

Data Availability Statement

The data that support the findings of this study are available from the corresponding author upon reasonable request.

References

  • 1.For a review on phosphoranides see: Dillon K. B., Chem. Rev. 1994, 94, 1441–1456. [Google Scholar]
  • 2. Dillon K. B., Waddington T. C., J. Chem. Soc. D 1969, 1317. [Google Scholar]
  • 3. Granoth I., Martin J. C., J. Am. Chem. Soc. 1978, 100, 7434–7436. [Google Scholar]
  • 4. Schmidpeter A., Zwaschka F., Angew. Chem. Int. Ed. 1979, 18, 411–412; [Google Scholar]; Angew. Chem. 1979, 91, 441–442. [Google Scholar]
  • 5. Dillon K. B., Platt A. W. G., Schmidpeter A., Zwaschka Z., Sheldrick W. S., Z. Anorg. Allg. Chem. 1982, 488, 7–26. [Google Scholar]
  • 6. Christe K. O., Dixon D. A., Mercier H. P. A., Sanders J. C. P., Schrobilgen G. J., Wilson W. W., J. Am. Chem. Soc. 1994, 116, 2850–2858. [Google Scholar]
  • 7. Schomburg D., Storzer W., Bohlen R., Kuhn W., Röschenthaler G.-V., Chem. Ber. 1983, 116, 3301–3308. [Google Scholar]
  • 8. 
  • 8a. Deng R. M. K., Dillon K. B., Platt A. W. G., Phosphorus Sulfur Relat. Elem. 1983, 18, 93–96; [Google Scholar]
  • 8b. Deng R. M. K., Dillon K. B., Sheldrick W. S., J. Chem. Soc. Dalton Trans. 1990, 551–554; [Google Scholar]
  • 8c. Dillon K. B., Drury C. J., Straw T. A., Polyhedron 1994, 13, 2605–2609; [Google Scholar]
  • 8d. Ali R., Dillon K. B., Phosphorus Sulfur Relat. Elem. 1987, 30, 139–142; [Google Scholar]
  • 8e. Ali R., Dillon K. B., J. Chem. Soc. Dalton Trans. 1990, 2593–2596. [Google Scholar]
  • 9. 
  • 9a. Allefeld N., Neumann B., Stammler H.-G., Röschenthaler G.-V., Ignat'ev N., Hoge B., Chem. Eur. J. 2014, 20, 7736–7745; [DOI] [PubMed] [Google Scholar]
  • 9b. Keßler M., Neumann B., Stammler H.-G., Hoge B., Z. Anorg. Allg. Chem. 2020, 646, 784–789; [Google Scholar]
  • 9c. Keßler M., Neumann B., Stammler H.-G., Hoge B., Z. Anorg. Allg. Chem. 2021, 647, 225–230; [Google Scholar]
  • 9d. Keßler M., Stammler H.-G., Neumann B., Röschenthaler G.-V., Hoge B., Inorg. Chem. 2021, 60, 16466–16473. [DOI] [PubMed] [Google Scholar]
  • 10. Kolomeitsev A., Görg M., Dieckbreder U., Lork E., Röschenthaler G.-V., Phosphorus Sulfur Silicon Relat. Elem. 1996, 109, 597–600. [Google Scholar]
  • 11. 
  • 11a. Burg A. B., Brendel G., J. Am. Chem. Soc. 1958, 80, 3198–3202; [Google Scholar]
  • 11b. Ang H. G., Schmutzler R., J. Chem. Soc. A 1969, 702–703; [Google Scholar]
  • 11c.G.-V. Röschenthaler, A. A. Kolomeitsev, unpublished results.
  • 12. 
  • 12a. Burg A. B., Inorg. Chem. 1986, 25, 4751–4755; [Google Scholar]
  • 12b. Ang H.-G., Koh C.-H., Koh L.-L., Kwik W.-L., Leong W.-K., Leong W.-Y., J. Chem. Soc. Dalton Trans. 1993, 847–855. [Google Scholar]
  • 13. 
  • 13a. Bennett F. W., Brandt G. R. A., Emeléus H. J., Haszeldine R. N., Nature 1950, 166, 225; [DOI] [PubMed] [Google Scholar]
  • 13b. Bennett F. W., Emeléus H. J., Haszeldine R. N., J. Chem. Soc. 1953, 1565–1571; [Google Scholar]
  • 13c. Krause L. J., Morrison J. A., J. Am. Chem. Soc. 1981, 103, 2995–3001; [Google Scholar]
  • 13d. Kampa J. J., Nail J. W., Lagow R. J., Angew. Chem. Int. Ed. 1995, 34, 1241–1244; [Google Scholar]; Angew. Chem. 1995, 107, 1334–1337; [Google Scholar]
  • 13e. Görg M., Röschenthaler G.-V., Kolomeitsev A. A., J. Fluorine Chem. 1996, 79, 103–104; [Google Scholar]
  • 13f. Dieckbreder U., Röschenthaler G.-V., Kolomeitsev A. A., Heteroat. Chem. 2002, 13, 650–653. [Google Scholar]
  • 14. Murphy-Jolly M. B., Lewis L. C., Caffyn A. J. M., Chem. Commun. 2005, 35, 4479–4480. [DOI] [PubMed] [Google Scholar]
  • 15.For experimental details and spectroscopic data, please see the Supporting Information.
  • 16. 
  • 16a. Hoge B., Thösen C., Inorg. Chem. 2001, 40, 3113–3116; [DOI] [PubMed] [Google Scholar]
  • 16b. Hoge B., Thösen C., Herrmann T., Pantenburg I., Inorg. Chem. 2003, 42, 3633–3641. [DOI] [PubMed] [Google Scholar]
  • 17. 
  • 17a. Cristau J., Plenat F., Bayssade S., J. Organomet. Chem. 1999, 592, 29–33; [Google Scholar]
  • 17b. Musker W. K., Stevens R. R., J. Am. Chem. Soc. 1968, 90, 3515–3521. [Google Scholar]
  • 18. Hu C.-M., Qing F.-L., Shen C.-X., J. Chem. Soc. Perkin Trans. 1 1993, 335–338. [Google Scholar]
  • 19.Crystallographic data: 2 (CCDC 2100145), colourless block, 0.8 x 0.5 x 0.4 mm3, monoclinic, P 21/c, a=14.633(2), b=35.255(6), c=14.619(6), β=98.39(3), V=7461(4) Å3, ρcalcd =1.630, Z=12, Mo-Kα radiation, λ=0.71073 Å, T=163(2) K, μ=0.398 mm−1, Θmax =12.53°, 14417 measured reflexions, 12345 crystallographic independent reflexions, Rint =0.0172, 974 parameters, GOOF=1.031, R1 =0.0465, wR2 =0.1205; 3 (CCDC 2100146), colourless block, 0.6 x 0.4 x 0.4 mm3, triclinic, P −1, a=8.897(4), b=9.544(2), c=14.965(3), α=90.552(14), β=93.19(2), γ=115.168(17), V=1147.4(6) Å3, ρcalcd =1.622, Z=2, Mo-Kα radiation, λ=0.71073 Å, T=173(2) K, μ=0.411 mm−1, Θmax =16.59°, 5396 measured reflexions, 4413 crystallographic independent reflexions, Rint =0.0335, 355 parameters, GOOF=1.064, R1 =0.0674, wR2 =0.2140. Deposition Number(s) 2100145 (for 2) and 2100146 (for 3) contain(s) the supplementary crystallographic data for this paper. These data are provided free of charge by the joint Cambridge Crystallographic Data Centre and Fachinformationszentrum Karlsruhe Access Structures service.
  • 20. Morino Y., Kuchitsu K., Moritani T., Inorg. Chem. 1969, 8, 867–871. [Google Scholar]
  • 21. Bowen H. J. M., Trans. Faraday Soc. 1954, 50, 463–470. [Google Scholar]
  • 22. Becker G., Golla W., Grobe J., Klinkhammer K. W., Le Van D., Maulitz A. H., Mundt O., Oberhammer H., Sachs M., Inorg. Chem. 1999, 38, 1099–1107. [DOI] [PubMed] [Google Scholar]
  • 23.High-order NMR spectra were calculated using the program gNMR: P. H. M. Budzelaar, gNMR version 4.1, Cherwell Scientific, Oxford/UK 1998.

Associated Data

This section collects any data citations, data availability statements, or supplementary materials included in this article.

Supplementary Materials

As a service to our authors and readers, this journal provides supporting information supplied by the authors. Such materials are peer reviewed and may be re‐organized for online delivery, but are not copy‐edited or typeset. Technical support issues arising from supporting information (other than missing files) should be addressed to the authors.

Supporting Information

Click here for additional data file. (1.1MB, pdf)

Data Availability Statement

The data that support the findings of this study are available from the corresponding author upon reasonable request.

Articles from Chemistry (Weinheim an Der Bergstrasse, Germany) are provided here courtesy of Wiley

RESOURCES