Impact of Multiple Hydrogen Bonds with Fluoride on Catalysis: Insight from NMR Spectroscopy.

Hydrogen-bonding interactions have been explored in catalysis, enabling complex chemical reactions. Recently, enantioselective nucleophilic fluorination with metal alkali fluoride has been accomplished with BINAM-derived bisurea catalysts, presenting up to four NH hydrogen-bond donors (HBDs) for fluoride. These catalysts bring insoluble CsF and KF into solution, control fluoride nucleophilicity, and provide a chiral microenvironment for enantioselective fluoride delivery to the electrophile. These attributes encouraged a 1H/19F NMR study to gain information on hydrogen-bonding networks with fluoride in solution, as well as how these arrangements impact the efficiency of catalytic nucleophilic fluorination. Herein, NMR experiments enabled the determination of the number and magnitude of HB contacts to fluoride for thirteen bisurea catalysts. These data supplemented by diagnostic coupling constants 1hJNH···F- give insight into how multiple H bonds to fluoride influence reaction performance. In dichloromethane (DCM-d2), nonalkylated BINAM-derived bisurea catalyst engages two of its four NH groups in hydrogen bonding with fluoride, an arrangement that allows effective phase-transfer capability but low control over enantioselectivity for fluoride delivery. The more efficient N-alkylated BINAM-derived bisurea catalysts undergo urea isomerization upon fluoride binding and form dynamically rigid trifurcated hydrogen-bonded fluoride complexes that are structurally similar to their conformation in the solid state. Insight into how the countercation influences fluoride complexation is provided based on NMR data characterizing the species formed in DCM-d2 when reacting a bisurea catalyst with tetra-n-butylammonium fluoride (TBAF) or CsF. Structure-activity analysis reveals that the three hydrogen-bond contacts with fluoride are not equal in terms of their contribution to catalyst efficacy, suggesting that tuning individual electronic environment is a viable approach to control phase-transfer ability and enantioselectivity.

Introduction

Hydrogen bonding (HB) is an important force for molecular recognition and for shaping the three-dimensional structure of molecules as large as proteins. In the past decade, n class="Chemical">hydrogen-bond donors (HBD) have also found widespread applications in asymmetric catalysis offering an alternative to Brønsted and Lewis acid catalysts.[1] For example, dual HBD catalysts promote enantioselective nucleophilic additions through direct binding to neutral electrophiles[2] or via the formation of chiral ion pair intermediates.[3] In the latter scenario commonly referred to as anion-binding catalysis, an electrophile is ionized by a chiral HBD catalyst generating an ion pair, with the resulting anionic hydrogen-bonded species creating a chiral environment for the cation to react with an external nucleophile. These approaches that build on pioneering studies in non-asymmetric cases[4] have enabled a wide range of transformations involving heteroatom-stabilized cations including acyl-Pictet–Spengler reactions,[5a] acyl-Mannich reaction,[5b] and additions to oxocarbenium ions.[5c] In further developments, HBD and Lewis acid catalysts were combined for enantioselective reactions involving less-reactive electrophiles.[6] Specifically, chiral squaramides were used to activate silyl triflates via triflate abstraction, forming a highly Lewis acidic complex capable of generating oxocarbenium ion intermediates from acetals for enantioselective nucleophilic additions.[6a] Such a dual-catalyst system also enables activation of propargyl acetates into tertiary carbocationic intermediates that lack heteroatom stabilization for enantioconvergent catalytic SN1 reactions.[6b] An underdeveloped manifold in chiral ion pair organocatalysis consists of using the hydrogen-bonded anion itself as the nucleophile. Hydrogen bonding is expected to decrease nucleophilicity, a challenge that led to creative solutions.[7] For example, the combination of a chiral squaramide and pro-nucleophile bromotrimethylsilane (TMSBr) allowed for highly enantioselective ring-opening of oxetanes with in situ released bromide bound to the chiral HBD catalyst.[7a] Our laboratory disclosed an alternative approach for nucleophile activation whereby hydrogen bonding is merged with phase-transfer catalysis (Figure A). Specifically, an insoluble and unreactive inorganic salt selected as a nucleophile is solubilized by the chiral HBD that serves as a solid–liquid phase-transfer catalyst. The resulting, now soluble hydrogen-bonded anion can act as a competent nucleophile and undergo enantiocontrolled reaction with a cationic electrophilic partner (Figure B). This approach, coined hydrogen-bonding phase-transfer catalysis (HB-PTC), was applied to asymmetric C–F bond formation with CsF or KF in organic solvents.[8]

Figure 1

(A) Proposed mechanism for hydrogen-bonding phase-transfer catalysis (HB-PTC). (B) Asymmetric fluorination of β-bromosulfides under HB-PTC. (C) BINAM-derived bisurea catalysts 1 and 2 and solid-state structure of 2:TBAF from single-crystal X-ray diffraction.

(A) Proposed mechanism for hydrogen-bonding phase-transfer catalysis (HB-n class="Chemical">PTC). (B) Asymmetric fluorination of β-bromosulfides under HB-PTC. (C) BINAM-derived bisurea catalysts 1 and 2 and solid-state structure of 2:TBAF from single-crystal X-ray diffraction.

For HB-PTC, the chiral n class="Chemical">BINAM-derived bisurea catalysts 1 and 2 shown in Figure C were engineered to coordinate fluoride in a manner reminiscent of the naturally occurring fluorinase enzyme.[9] Highly enantioselective nucleophilic substitution of β-bromosulfides or β-chloramines was achieved via ring-opening of in situ formed meso-episulfonium or -aziridinium ions with metal alkali fluorides.[8a,8b] Enantioenriched γ-fluoroamines were also within reach from achiral azetidinium salts applying HB-PTC.[8c] For selected transformations, 2.5 mol % of the phase-transfer catalyst was sufficient to reach high yield and enantioselectivity. N-Alkylation of the bisurea catalyst improved performance, suggesting that this structural modification influences conformational preference and the ability of the catalyst to engage in hydrogen bonding with fluoride.

While fluoride binding to HBD is an active area of research in supramolecular chemistry,[10] applications to asymmetric catalytic fluorination have been overlooked for many years, and data on how the number, strength, and directionality of n class="Chemical">hydrogen bonds with fluoride influence its nucleophilicity have only recently appeared.[11] Valuable information on the spatial arrangement of the chiral tetrabutylammonium (TBA) N-isopropyl bisurea–fluoride complex 2:TBAF was obtained from a single-crystal X-ray diffraction measurement that revealed three distinct N–H···F– hydrogen-bonding interactions (Figure C).

A 1H/19F NMR study is ideally suited to define the precise nature of H-bonding to n class="Chemical">fluoride under conditions that simulate catalytic fluorination. Herein, we report the results of a detailed investigation performed on a selection of thirteen chiral bisurea catalysts enabling fluorinations under HB-PTC. The analyses of 1D NMR spectra and quantitative nuclear Overhauser effect (NOE) studies were used to study conformational changes of the catalysts upon binding to fluoride. Scalar couplings across hydrogen bonding, 1hJNH···F,[12] provide valuable information on the number and magnitude of catalyst–fluoride interactions. The characterization of the first bisurea–CsF complex in the solid state and in solution provides important insight on counterion effects, as well as on the species leading to successful catalytic fluorination with CsF under HB-PTC. This study unveils the existence of a range of multifurcated hydrogen-bonded fluoride complexes in solution and enables an analysis that correlates structural features with performance.

Results and Discussion

Conformational Properties of BINAM-Derived Bisurea Catalysts

Polar aromatic solvents such as 1,2-difluorobenzene are optimal for fluorination under HB-n class="Chemical">PTC; chlorinated solvents such as chloroform and dichloromethane are also effective. In this study, spectra were recorded in DCM-d2 because of its noncoordinating nature, optimal chemical shift dispersion, and favorable temperature range. When possible, the concentration was set to 25 mM to reflect the reaction conditions applied for enantioselective fluorination under HB-PTC.

Initially, BINAM bisurea 1 and its N-n class="Chemical">isopropylated analogue 2 served to investigate the effect of N-alkylation on conformational change to the catalyst. A combination of total correlation spectroscopy (TOCSY), heteronuclear single quantum coherence spectroscopy (HSQC), and heteronuclear multiple bond correlation spectroscopy (HMBC) (1H–13C and 1H–15N) allowed for unambiguous assignment of all proton and carbon resonances of 1 and 2.[13] Nonalkylated bisurea 1 shows uniformly sharp peaks in 1H and 13C NMR spectra (Figure , top). The chemical shifts are consistent with electronic environments, with NH(a) proximal to electron-deficient 3,5-bis(trifluoromethyl)phenyl groups deshielded with respect to NH(b), which are positioned close to the BINAM scaffold. In contrast to 1, line broadening was observed for selected peaks in the 1H and 13C NMR spectra of N-isopropyl bisurea 2 (Figure , bottom). The resonances assigned to NH(a) and NH(c) appear at 7.1 and 6.9 ppm, respectively; NH(b) overlaps with multiple peaks in a range of common deuterated solvents (DCM-d2, CDCl3, tetrahydrofuran (THF-d8), CD3CN, dimethyl sulfoxide (DMSO-d6), and MeOD) and, at first glance, was difficult to locate due to broadening (>70 Hz). In DCM-d2, the chemical shift of NH(b) was estimated at ∼7.6 ppm based on cross-peaks in 1H nuclear Overhauser effect spectroscopy (NOESY) and 1H–15N HSQC;13 this was unexpected as NH(b) is in a less electron-deficient environment than NH(a) and NH(c). In DMSO-d6,[14] NH(a) and NH(c) are deshielded (+1.5 and +0.8 ppm, respectively) likely due to hydrogen bonding with the solvent, while NH(b) is minimally affected (+0.2 ppm). This observation alludes to NH(b) engaging in intramolecular hydrogen bonding with O=C(9) (broad 13C signal deshielded at 156.2 ppm; Figure , inset).

Figure 2

(A) Detail of 1H and 13C NMR of 1. (B) Detail of 1H,13C NMR, and 1H–15N HSQC of 2 (DCM-d2, 25 mM, 298 K).

(A) Detail of 1H and n class="Chemical">13C NMR of 1. (B) Detail of 1H,13C NMR, and 1H–15N HSQC of 2 (DCM-d2, 25 mM, 298 K).

Peak line width (ν1/2 = half-height line width) is an important NMR observable correlating with the transverse relaxation rate R2 (R2 = 1/T2 ≈ ν1/2, Hz) and thereby with dynamic behavior of molecules in solution.[15] Specifically, signal broadening observed for H(3′), C(3′), C(2′), C(1′), and C(9) is consistent with a dynamic conformational exchange on the NMR time scale involving the hydrogen-bond interaction NH(b)···O=C(9). The n class="Chemical">1H NMR spectra of both 1 and 2 were also recorded at varying concentrations. Significant changes were observed for 1 between 2 and 64 mM, with all protons bound to carbons experiencing shielding (ΔδH(11) = −211 ppb), while deshielding was observed for the NH (Δδ NH(a) = +300 ppb, Δδ NH(b) = +227 ppb). This pattern suggests intermolecular aggregation. In contrast to 1, the 1H NMR spectra of 2 display minimal variations in chemical shifts at higher concentration, a result suggesting reluctance to form intermolecular aggregates.

Insight into the conformational preference of 2 in DCM-d2 was deduced from analysis of through-space correlations by means of high-resolution n class="Chemical">1H NOESY (Figure ). Strong correlations between the isopropyl protons H(15), H(16), H(17), and NH(c) are consistent with the N-iPr urea adopting an anti–anti conformation.[13] Nuclear Overhauser effect (NOE) between isopropyl and H(8′) indicates that the N-alkyl group is within close distance to naphthyl(I), while the NH(a) ⇔ H(11) interaction suggests that the two ureas are proximal to each other. The different orientations of the two ureas with respect to the BINAM scaffold explains the pronounced variations in chemical shifts between H(3′) and H(3) (8.47 vs. 7.56 ppm), with both positioned on the naphthyl group ortho to the urea substituent. The carbonyl group affects the chemical shifts of neighboring protons by means of anisotropic electron circulation; as a result H(3′), which is coplanar with the urea, is deshielded, whereas this is not the case for H(3) being out of plane. Together, these observations suggest that the two ureas are approximately perpendicular to each other. Magnetic anisotropy effects account for the shielding of the two diastereotopic methyls belonging to isopropyl. Protons 17 appear at 1.03 ppm as a sharp doublet, while H(15) pointing toward naphthyl(I) appears as a broad singlet at 0.68 ppm. Data in the solid state could not be secured because recrystallization of 2 afforded fine needles that were unsuitable for single-crystal X-ray diffraction studies.

Figure 3

Conformation of 2 based on 1H NOESY correlations (DCM-d2, 25 mM, 298 K).

Conformation of 2 based on 1H NOESY correlations (n class="Chemical">DCM-d2, 25 mM, 298 K).

A range of N-alkylated n class="Chemical">BINAM bisureas with various N-substituents and electronic patterns for the aryl rings were synthesized and analyzed by NMR spectroscopy in DCM-d2 (Figure A). The spectra of N-alkylated analogues 3–7 all featuring two 3,5-bis(trifluoromethyl)phenyl substituents were very similar to N-isopropyl bisurea 2, implying analogous conformational preference. For this series, all NH(b) are more deshielded than NH(a)/NH(c) and appear broader; the C(9) and H(3′) signals are also broader and deshielded compared to C(9′) and H(3), respectively. When the aryl group linked to the N-alkylated urea is the less electron-deficient phenyl group (R1 = Ph, catalyst 8), an additional hydrogen-bond interaction NH(a)···O=C is observed that is consistent with increased Lewis basicity of the carbonyl oxygen (Figure B, top). This interaction confers conformational rigidity, giving rise to sharp proton and carbon resonances. In contrast, when the aromatic ring of the nonalkylated urea is phenyl (R2 = Ph, catalyst 9), the 1H and 13C NMR spectra are broader, suggesting the existence of a more dynamic structure likely resulting from weaker intramolecular hydrogen-bonding interactions (Figure B, bottom).

Figure 4

(A) Structures of the BINAM-derived bisurea catalysts 3–13. (B) 1H NMR of 8 (top) and 9 (bottom) (DCM-d2, 25 mM, 298 K).

(A) Structures of the BINAM-derived n class="Chemical">bisurea catalysts 3–13. (B) 1H NMR of 8 (top) and 9 (bottom) (DCM-d2, 25 mM, 298 K).

Complexation of Bisureas with TBAF

Formation of a hydrogen-bonded n class="Chemical">bisurea–fluoride complex is the cornerstone for successful enantioselective fluorinations with metal alkali fluoride under HB-PTC. Structural insight of these complexes in solution is therefore crucial for further development. The binding affinities of bisurea 1 and N-isopropyl bisurea 2 for fluoride were investigated by spectrophotometry (Figure ). UV titrations carried out with 1 or 2 (1.2 and 1.4 μM, respectively) were performed in DCM by adding a solution of tetra-n-butylammonium fluoride of exact concentration quantified by 19F NMR (TBAF·3H2O in DCM, 0.1 mM).[13] Upon addition of an increasing amount of TBAF (0–15 equiv), UV spectra showed a bathochromic shift with the buildup of a new maximum of absorption (λmax) at 273–275 nm. The binding constants and energies were calculated from the titration profiles at λmax via nonlinear least-squares regression using dedicated software.[16] Both 1:1 and 2:1 binding modes were considered, with 1:1 giving superior fitting results. A 1:1 binding mode was also consistent with the clean isosbestic points observed. Association constants in the range of 106 M–1 denote strong and similar binding affinities of 1 and 2 to fluoride (Table ).

Figure 5

Stacked UV spectra recorded for the titration of 1 (1.2 μM) and 2 (1.4 μM) with TBAF·3H2O (0.1 mM) in DCM at 298 K. On the right, titration profiles at the λmax (red dots) and fitting functions (red lines).[13]

Table 1

Association Constants (Ka), log(Ka), and Free Energies (ΔG) for the Formation of 1:1 Bisurea–TBAF Complexes Derived from Bisureas 1 and 2a

U	Ka (1:1) (M–1)	log(Ka (1:1))	ΔG (1:1) (kJ/mol)
1	0.92 ± 0.02 × 106	5.96 ± 0.01	–34.01 ± 0.06
2	1.43 ± 0.04 × 106	6.16 ± 0.01	–35.10 ± 0.08

Ka are calculated by nonlinear regression using DynaFit 4 and expressed as the average of two experiments.

Stacked UV spectra recorded for the titration of 1 (1.2 μM) and 2 (1.4 μM) with TBAF·3H2O (0.1 mM) in n class="Chemical">DCM at 298 K. On the right, titration profiles at the λmax (red dots) and fitting functions (red lines).[13]

Next, 1H NMR titrations were performed at 3 mM concentration in n class="Chemical">DCM-d2. Addition of a TBAF solution (TBAF·3H2O in DCM-d2, 55 mM) to 1 led to line broadening in 1H NMR, indicating on–off equilibration. Sharp spectra were gradually recovered when approaching 1 equiv of added fluoride. Noticeable changes in 1H and 19F chemical shifts were observed between 0 and 1 equiv, after which the chemical shift of all resonances became invariant. Over the course of the titration, proton signals were shielded between 0 and 0.5 equiv of fluoride and deshielded between 0.5 and 1.0 equiv before reaching a plateau at >1 equiv. A signal assigned to NH(a) appeared in 1H NMR at 13.5 ppm after 1 equiv of fluoride was added, while NH(b) was observed at 7.6 ppm (Figure , left). Addition of TBAF to 2 also led to line broadening until quantitative binding was reached. At 1 equiv of fluoride, all NH are deshielded by ∼5 ppm with respect to unbound bisurea 2 (Figure , right). The titration of both catalysts 1 and 2 reflects a scenario not limited to 1:1 complexation.[17] More likely, a dimeric species or higher coordinated fluorides dominate at low F– concentration, which then equilibrate toward the more stable [UF]− 1:1 complex (U = 1 or 2) over the course of the titration (Ka(1:1) ≫ Ka(2:1)). The variation of chemical shift for diagnostic resonances was plotted against the concentration of added fluoride, and the data were analyzed. Initial attempts to fit the data to a 1:1 binding mode resulted in poor fit and nonsensical data. When a 2:1 binding mode was considered and Ka(1:1) values secured from UV titration were taken into account, a good agreement with the experimental data was found. This allowed the calculation of 2:1 binding associations Ka(2:1) (∼103 M–1) and binding energies for both 1 and 2 (Table ). In our previous report on diarylurea–fluoride complexes [UF]− and [U2F]−,[11d] the binding constants were 250–500 M–1 for Ka(2:1) and 12 000–85 000 M–1 for Ka(1:1). These were measured in CD3CN, a solvent in which hydrogen-bonding interactions are expected to be weaker.

Figure 6

Stacked 1H NMR spectra for the titration of 1 (left) and 2 (right) with TBAF·3H2O (55 mM) in DCM-d2 at 298 K. Below, titration profiles for diagnostic protons (black dots) and fitted function (red lines).[13]

Table 2

Association Constant (Ka), log(Ka), and Free Energies (ΔG) for the Formation of 2:1 Bisurea–TBAF Complexesa

U	Ka (2:1) (M–1)	log(Ka(2:1))	ΔG(2:1) (kJ/mol)
1	600 ± 100	2.80 ± 0.08	–16.0 ± 0.5
2	3100 ± 900	3.5 ± 0.1	–20.0 ± 0.7

Ka are calculated by nonlinear regression using DynaFit 4 and expressed as the average of two experiments.

Stacked 1H NMR spectra for the titration of 1 (left) and 2 (right) with n class="Chemical">TBAF·3H2O (55 mM) in DCM-d2 at 298 K. Below, titration profiles for diagnostic protons (black dots) and fitted function (red lines).[13]

Hydrogen-Bond Coupling 1hJNH···F

The three NH of 2:TBAF are deshielded compared to 2 (ΔδNH ≈ +5 ppm), as are n class="Gene">H(11), H(11′), and H(3′). In contrast, H(13) and H(13′) on the 3,5-bis(trifluoromethyl)phenyl group, as well as H(6′), H(7′), and H(8′) belonging to naphthyl(I), are shielded. The sharp lines in the 1H and 13C NMR spectra indicate that 2:TBAF is dynamically stable (Figure ).

Figure 7

δ 1H NMR variations of 2 after F– complexation. 2:TBAF was generated by adding 1 equiv of a TBAF·3H2O solution (55 mM in DCM-d2) to 2 (3 mM in DCM-d2) at 298 K.[13]

Each NH appears as a doublet in 1H NMR, and F– appears as a double–double doublet (ddd) in 19F NMR; the three NH collapsed into singlets in the n class="Chemical">fluorine decoupled 1H NMR, and the splitting of the fluoride peak disappeared when 19F NMR was acquired with proton decoupling. This signal multiplicity represents a case of scalar coupling that develops across hydrogen bonds (hydrogen-bond coupling, HBC). These couplings provide unambiguous proof of hydrogen-bonding interactions between NH and F– for the complex in solution and a measure of their strength. Because HBC results from overlap of H-bond donor and acceptor wave functions, the magnitude of the coupling depends exponentially on donor–acceptor distances, as well as geometry.[18] Studies by both Grzesiek and Bax demonstrated that the empirical relationship between HBC and internuclear distances can be exploited for the structural assignment of nucleobases and proteins.[19] For HBC to be observable, the hydrogen-bonding network must be rigid, which is often the case for biomolecules held together by multiple hydrogen bonds but is less common in small molecules.[20] For hydrogen bonds involving the fluoride ion, pioneering work from Shenderovich and Limbach determined 1hJFH in [F(HF)]− clusters measured at ultralow temperature,[21] while only a few organic molecules such as calix[4]pyrrols and amido cryptand receptors display HBC with fluoride.[22] The 1H NMR spectrum of 2:TBAF stands out with three resonances displaying hydrogen-bond scalar couplings with fluoride clearly visible. This offers the possibility of measuring correlation spectra across the hydrogen bridge, a feature more often applied to covalently linked nuclei. The clean in phase-HSQC (CLIP-HSQC) sequence was introduced for the direct measurement of one-bond couplings without phase distortions.[23] Here, we applied this sequence for 1H–19F detection to measure 1hJNH···F coupling constants, an experiment allowing for the four nuclei involved in the hydrogen-bonding network of 2:TBAF to be observed (Figure ). The 1H chemical shifts are seen on the horizontal axis, and the 19F chemical shift is seen on the vertical axis with the magnitude of 1hJNH···F determined from cross-peak distances (which matched those visible in the 1H spectrum). The three HBC constants measured for 2:TBAF (DCM-d2, 3 mM, 298 K) are 1hJNH(a)···F = 61 Hz, 1hJNH(c)···F = 51 Hz, and 1hJNH(b)···F = 34 Hz.

Figure 8

1H–19F CLIP-HSQC of 2:TBAF (500 MHz, DCM-d2, 3 mM, 298 K).

1H–19F CLIP-HSQC of 2:n class="Chemical">TBAF (500 MHz, DCM-d2, 3 mM, 298 K).

In DCM-d2, the peak of F– at −90 ppm for 2:n class="Chemical">TBAF is deshielded compared to TBAF·3H2O, which resonates at −118 ppm.[24] The F– longitudinal relaxation time constant (T1) would be expected to vary upon formation of a hydrogen-bonded fluoride complex because T1 depends on the motions of the molecule in solution (and hence its size) as well as the proximity of neighboring protons as relaxation sources. Accordingly, T1 measured for 19F via inversion recovery experiments (magnet field strength = 11.7 T) was found to decrease from 1430 ms for TBAF·3H2O to 313 ms for 2:TBAF, which is consistent with the formation of a larger, H-bonded molecular complex. The magnitude of the HBC constant for each NH inversely correlates with the NH···F internuclear distance measured from the solid-state structure of 2:TBAF (determined by single-crystal X-ray diffraction), with NH(a)···F– being the shortest HB contact with fluoride. To correlate 1hJNH···F and hydrogen-bond distances in solution, the NOE developed between fluoride and NH was investigated by 1H–19F heteronuclear Overhauser spectroscopy (HOESY). NOE buildup curves were determined using mixing times between 10 and 600 ms, and NH–F distances relative to NH(a)–F were calculated (Figure ).[13] The distance of NH to fluoride increased in the following order: NH(a) ≈ NH(c) < NH(b), with NH(c)···F– being 2% longer than NH(a)···F–, and NH(b)···F– being 12% longer. Larger coupling constants 1hJNH···F therefore correspond to shorter HB distance. An additional NOE correlation between the ortho-aromatic proton H(11) with fluoride was observed, although of smaller magnitude. Taken together, these data concur with the relative distances seen in the solid state from single-crystal X-ray diffraction studies, although the values for NH(b)···F– and H(11)···F– are shorter than those from solution studies.

Figure 9

Relative H···F– distances calculated for 2:TBAF from HOESY (DCM-d2, 10 mM, 298 K, τm = 10–600 ms) and comparison with single-crystal X-ray diffraction and 1hJNH···F.

Relative H···F– distances calculated for 2:TBAF from HOESY (n class="Chemical">DCM-d2, 10 mM, 298 K, τm = 10–600 ms) and comparison with single-crystal X-ray diffraction and 1hJNH···F.

Next, we studied N-isopropyl bisurea 13 featuring 3,5-difluorophenyl groups as this substituent features n class="Chemical">vicinal hydrogen and fluorine of known distance (2.60 Å).[25] Similarly to 2:TBAF, the distances in 13:TBAF calculated from HOESY experiments with a single mixing time of 30 ms, were found to be inversely proportional to the size of the HB coupling constants (absolute distance for NH(a)···F– = 1.83 Å, NH(c)···F– = 1.91 Å, and NH(b)···F– = 2.05 Å) (Figure ).

Figure 10

Quantitative 1H–19F HOESY of 13:TBAF (DCM-d2, 3 mM, 298 K, τm = 30 ms).

Quantitative 1H–19F HOESY of 13:n class="Chemical">TBAF (DCM-d2, 3 mM, 298 K, τm = 30 ms).

To gain insight into the conformational preference of 2:TBAF, n class="Chemical">1H NOESY cross-peak volumes were converted into absolute distances by calibration with the distance of the vicinal protons H(3′) and H(4′) (2.47 Å).[25] This allowed for a quantitative mapping analysis of H–H internuclear distances for 2:TBAF (Figure A).[26] Correlation H(16) ⇔ H(8′) indicates that the isopropyl C–H bond points toward naphthyl(I) with a distance between the two protons of 2.6 Å. In contrast to unbound bisurea 2, the protons belonging to the N-iPr group do not correlate with NH(c), which instead shows two NOE with H(11) and NH(b) (2.7 and 2.5 Å), suggesting that the N-isopropyl urea underwent an anti–anti to syn–anti conformational change upon fluoride binding. NH(a) and NH(b) belonging to the same urea display strong NOE (2.0 Å). NH(a) also presents correlation with H(11′) (2.7 Å) and H(11) (3.5 Å). These NOE interactions indicate that the three NH are in close proximity. Deshielding of H(3′) upon fluoride binding indicates more pronounced coplanarity between H(3′) and the adjacent urea carbonyl with respect to unbound 2. The internuclear distances measured by NMR are in keeping with those determined for the solid-state structure using single-crystal X-ray diffraction (Figure B).

Figure 11

(A) Structure of 2:TBAF and internuclear distances calculated from 1H NOESY (600 MHz, DCM-d2, 3 mM, 298 K, τm = 300 ms) and comparison with X-ray structure data. (B) Solid-state structure from single-crystal X-ray diffraction studies of 2:TBAF.

(A) Structure of 2:TBAF and internuclear distances calculated from n class="Chemical">1H NOESY (600 MHz, DCM-d2, 3 mM, 298 K, τm = 300 ms) and comparison with X-ray structure data. (B) Solid-state structure from single-crystal X-ray diffraction studies of 2:TBAF.

1hJNH···F Studies of Bisurea–TBAF Complexes

With a robust NMR experiment correlating 1hJNH···F and internuclear distances in place, we studied how n class="Chemical">fluoride positioned itself within the pocket of a range of BINAM-derived bisurea catalysts. Thirteen complexes were formed by addition of 1 equiv of TBAF·3H2O to a solution of bisurea, and the coupling constants 1hJNH···F were measured. For each catalyst–fluoride complex, 1H NMR, 19F NMR, and CLIP-HSQC were recorded at 273 K and at low concentration (3 mM) to minimize proton exchange with water, which we had observed to mask 1hJ couplings via spin-exchange decoupling. Complexation of nonalkylated BINAM bisurea 1 with TBAF·3H2O led to deshielding of all NH resonances indicative of fluoride binding, but no coupling with fluoride was observed at 3 mM. At lower concentration (0.58 mM), HBC was observed for the pair of equivalent NH(a) linked to 3,5-bis(trifluoromethyl)phenyl with 1hJNH(a)···F = 65 Hz, and ΔδNH(a) = +6 ppm compared to unligated 1 (Figure ).[13]

Figure 12

1H NMR of 1:TBAF (DCM-d2, 0.58 mM, 273 K); (inset) 19F NMR of 1:TBAF showing fluoride splitting.

1H NMR of 1:n class="Chemical">TBAF (DCM-d2, 0.58 mM, 273 K); (inset) 19F NMR of 1:TBAF showing fluoride splitting.

This dependence on concentration suggests a higher rate of proton exchange with water compared to 2:n class="Chemical">TBAF. Faster on–off fluoride complexation could also be responsible for the line broadening observed at a higher concentration. In 19F NMR, fluoride appears as a triplet at −86 ppm. The NH(b) pair is only slightly deshielded upon fluoride complexation, ΔδNH(b) = +1 ppm. The number of proton signals indicate that 1:TBAF retains its C2 symmetry. Taken together, these observations suggest that 1 in DCM-d2 forms a bidentate complex with fluoride bound to NH(a) away from the binaphthyl system. Catalysts 3–7 that are N-alkylated with different hydrocarbon chains display 1hJNH···F values between 59–61 Hz for NH(a), 48–54 Hz for NH(c), and 33–34 Hz for NH(b), which are highly similar to those for 2:TBAF (Table , entries 3–7). NH(c)···F– varies the most with a difference of up to 6 Hz for 1hJNH···F. A series of N-isopropyl bisurea–fluoride complexes with different 3,5-substituted aromatic rings was examined next. Electron-poor aryl groups are expected to increase NH acidity and therefore hydrogen-bond strength with fluoride; conversely, electron-rich aromatic rings would weaken NH···F– hydrogen-bonding interactions. This offers a platform to control the positioning of fluoride within the catalyst pocket, possibly tune its nucleophilicity, and influence the enantioselective delivery. Catalysts 8 (R1 = H, R2 = CF3) and 11 (R1 = F, R2 = CF3) resulted in 1hJNH(c)···F values of 39 and 44 Hz, respectively, indicating reduced interaction between NH(c) and fluoride (Table , entries 8 and 11). Catalysts 9 (R1 = CF3, R2 = H), 10 (R1 = CF3, R2 = Me), and 12 (R1 = CF3, R2 = F) displayed weaker hydrogen bonding between fluoride and NH(a), with 1hJNH(c)···F values increased and even exceeding 1hJNH(a)···F for 10 (Table , entries 9, 10, and 12). Fluoride is equally shared between NH(a) and NH(c) for 9 and 10 despite the electronic character of the rings expected to favor NH(c). Catalyst 13 (R1 = R2 = F) presents similar 1hJ values to 2 for NH(a) and NH(b) but a more pronounced variation in NH(c), which is reduced by 4 Hz (Table , entry 13).

Table 3

HBC Constants 1hJNH···F and 19F Chemical Shifts of Bisurea–Fluoride Complexesa

entry	catalyst	R	R1	R2	1hJNH(a)···F– (Hz)	1hJNH(c)···F– (Hz)	1hJNH(b)···F– (Hz)	δ 19F (ppm)
1b	1	H	CF3		65			–86.40
2	2	iPr	CF3		60	50	33	–90.53
3	3	Me	CF3		60	54	34	–89.41
4	4	Et	CF3		61	54	34	–88.64
5	5	nPr	CF3		60	53	33	–88.79
6	6	cPentyl	CF3		59	48	34	–91.33
7	7	3-Pentyl	CF3		61	52	34	–89.20
8	8	iPr	H	CF3	63	39	34	–93.87
9	9	iPr	CF3	H	53	52	33	–93.87
10	10	iPr	CF3	Me	52	53	34	–90.15
11	11	iPr	F	CF3	60	44	33	–89.79
12	12	iPr	CF3	F	59	51	33	–91.59
13	13	iPr	F		59	46	34	–91.17

The fluoride complexes were generated by addition of 1 equiv of TBAF·3H2O (solution in DCM-d2 of known concentration) to the bisurea (3 mM in DCM-d2) and measured at 273 K.

In DCM/DCM-d2, 0.58 mM.

The fluoride complexes were generated by addition of 1 equiv of n class="Chemical">TBAF·3H2O (solution in DCM-d2 of known concentration) to the bisurea (3 mM in DCM-d2) and measured at 273 K.

In DCM/n class="Chemical">DCM-d2, 0.58 mM.

These data are informative at various levels:

• In solution, all three NH of N-alkylated bisurea catalysts bind n class="Chemical">fluoride with the N-alkylated urea undergoing anti–anti to syn–anti isomerization. This contrasts with the nonalkylated catalyst 1, which does not engage all four NH groups in hydrogen bonding with fluoride; the two NH bound to fluoride are the ones substituted by the trifluoromethylated aryl groups, and 1hJ values are of large magnitude (65 Hz). Complex 1:TBAF is less dynamically stable than 2:TBAF as reflected by the broad line and unresolved 1hJ coupling at 3 mM concentration.

• For all catalysts, NH(a)···F– is the dominant hydrogen-bonding interaction in n class="Chemical">DCM-d2, even when programmed to be weaker by tuning its electronic environment; this is likely due to more favorable geometrical arrangement for hydrogen bonding. NH(c)···F– is the hydrogen bond that varies the most, and NH(b) provides the weakest HB contribution with 1hJ values of 33–34 Hz.

• The complexes display 19F chemical shifts between −86 and −94 ppm, which represents a deshielding of ∼30 ppm compared to unbound TBAF·3H2O in n class="Chemical">DCM-d2.[27]

Complexation with CsF

Fluorinations under HB-PTC are carried out with n class="Chemical">alkali metal fluorides (MFs), requiring the formation of a soluble bisurea–MF complex as a reaction intermediate. The spectroscopic characterization of a representative bisurea–MF complex would therefore provide valuable information. With the prospect of carrying out 133Cs NMR, we selected 2:CsF for this study. Because of the limited solubility of CsF, the complex was generated in a sealed NMR tube by sonication of N-isopropylated bisurea 2 and solid CsF (50 equiv) in DCM-d2 (25 mM).[13] The 1H NMR spectrum at room temperature showed extensive line broadening, indicating that equilibration of several species took place. Low-temperature experiments (298–243 K) gave three sets of signals diagnostic for isopropyl H(16); these were in mutual chemical exchange as revealed by the sign of ROESY cross-peaks. The presence of at least seven NH doublets denoted the presence of multiple species in solution (Figure ). The 19F NMR spectrum (298–243 K) showed two signals, with the major resonating at −65 ppm and the minor resonating at −96 ppm (Figure C). T1 relaxation was measured by inversion recovery experiments for both fluoride resonances at room temperature (magnet field strength 11.7 T) and found to be 145 and 5 ms for the major and minor species, respectively. These T1 values are substantially shorter than those of 2:TBAF (313 ms) and TBAF in DCM-d2 (1430 ms), suggesting slower tumbling due to the species in solution being larger in size and/or increased contributions from local relaxation sources. 133Cs NMR shows a wide peak (Figure C, inset) broadened as a result of its quadrupolar moment, as well as dynamic averaging of more than one cesium fluoride complex. The 133Cs signal is recorded at −14 ppm at room temperature, which is significantly more shielded than previously observed for the ion pair formed from Cs+ and the weakly coordinating [H2NB2(C6F5)6]− anion (17 ppm), a rare example of 133Cs NMR for a Cs+ salt measured in DCM-d2.[28]

Figure 13

(A) 1H NMR after mixing 2 with CsF (DCM-d2, 25 mM) recorded at 298 K (overlaid, gray line) and 243 K (black line); (B) detail of ROESY spectrum recorded at 273 K showing chemical exchange cross-peaks; (C) 19F NMR and 133Cs NMR (inset).

(A) 1H NMR after mixing 2 with n class="Gene">CsF (DCM-d2, 25 mM) recorded at 298 K (overlaid, gray line) and 243 K (black line); (B) detail of ROESY spectrum recorded at 273 K showing chemical exchange cross-peaks; (C) 19F NMR and 133Cs NMR (inset).

Proton diffusion experiments (1H DOSY) were performed at 243 K and revealed that the three sets of peaks assigned to isopropyl CH(16) belong to two species. The minor species had a smaller diffusion coefficient (D = 1.9 × 10–10 m2 s–1), denoting a larger molecular complex, while the major species displayed faster diffusion (D = 2.4 × 10–10 m2 s–1).[13] These data support the presence of a 1:1 bisurea–fluoride complex as the major species and a minor nonsymmetrical 2:1 complex. 19F NMR indicated that the 1:1 to 2:1 ratio was 85:15 at room temperature.

The NH signals for both species were unambiguously identified using NOESY (EXSY) and ROESY correlations (measured, respectively, at 273 and 243 K); 1hJNH···F coupling constants together with n class="Chemical">1H–19F NOE gave insight into binding modes. The chemical shifts for the NH protons of the 1:1 complex (2:CsF) were comparable to those observed for 2:TBAF, with NH(a) being the most deshielded (δNH(a) = 11.46 ppm), followed by NH(c) (δNH(c) = 10.52 ppm) and NH(b) (δNH(b) = 10.26 ppm). Complex 2:CsF displayed 1hJNH···F splitting of 52 Hz for NH(a), 37 Hz for NH(c), and 34 Hz for NH(b). These values differ from those for 2:TBAF, which shows larger HB coupling constants for both NH(a) and NH(c) (cf. 2:TBAF: 1hJNH(a)···F = 61 Hz, 1hJNH(c)···F = 51 Hz, and 1hJNH(b)···F = 34 Hz, measured at 298 K). 1hJNH(c)···F stands out for being reduced by 14 Hz. The 2:1 complex Cs[(2)2:F] shows five NH···F correlations in 1H–19F CLIP-HSQC and 1H–19F HOESY. In Cs[(2)2:F], one of the two bisureas exhibited tridentate binding to fluoride (1hJNH(a)···F = 40 Hz, 1hJNH(b)···F = 37 Hz, and 1hJNH(c)···F = 14 Hz), while the other featured two HB contacts engaging its nonalkylated urea submotif (1hJNH(a)′···F = 58 Hz and 1hJNH(b)′···F = 21 Hz). NH(c)′ appeared as a shielded singlet at 5.8 ppm and did not interact with fluoride (Figure ).

Figure 14

NMR parameters measured for NH resonances and F– of 2:CsF and Cs[(2)2:F].

NMR parameters measured for NH resonances and F– of 2:CsF and n class="Chemical">Cs[(2)2:F].

We noted important differences in fluoride chemical shifts. The observed shifts were −96 and −65 ppm for Cs[(2)2:F] and 2:CsF, respectively. This large difference suggests no interaction between fluoride and Cs+ in Cs[(2)2:F]; in contrast, for 2:CsF, Cs+ likely forms a contact ion pair with F– in DCM-d2. No data are available in the literature on fluoride chemical shift for CsF in apolar solvent likely due to the difficulties of solubilizing the salt; strongly deshielded F–, however, has been observed in solid-state NMR of CsF.[29]

The crystallization of bisurea 13 in the presence of n class="Gene">CsF gave a single crystal suitable for X-ray diffraction studies.[30] In the solid state, 13:CsF formed columnar superstructures, where Cs+ was bridged between F– and the two carbonyls of a second bisurea molecule, with each pair of bisurea being oriented in a head-to-tail arrangement (Figure ). The complex showed 1:1 binding to fluoride, which was itself hydrogen-bonded to all three NH groups. The structure of the BINAM scaffold is highly similar to that of 2:TBAF; however, in 13:CsF NH(c)···F– showed the longest hydrogen-bonding distance (Table ). A distinctive cation−π interaction between Cs+ and naphthyl(II) (distance of 3.3283(4) Å) was also prominent. Compared with the NH···F– distances of 13:TBAF determined by NMR in DCM-d2 (Table ), an elongation of NH(c)···F– and shortening of NH(b)···F– were observed. NH(a)···F– displayed a similar HB distance in solution and in the solid state. The Cs···F distance for 13:CsF was 2.742(3) Å,[31] and Cs+ displayed short-distance contacts with the two carbonyls of a neighboring bisurea, a multimeric arrangement likely reinforced by solid-state packing. In solution, the shielding for 133Cs resonance was consistent with an interaction with fluoride as well as a cation−π interaction with naphthyl. From these insights, it appears that Cs+ in place of TBA+ does not drastically affect the structure of the 1:1 catalyst–fluoride complex, apart from weakening NH(a)···F– and NH(c)···F– interactions. The π–cation interaction of Cs+ with BINAM directly contributes to the positioning of Cs+ and indirectly to that of fluoride and its HB interactions. An analogous cation−π contact between the positively charged episulfonium ion and naphthyl was found to be a key noncovalent interaction in the transition state (TS) leading to product formation.[8a]

Figure 15

Solid-state structure of 13:CsF from single-crystal X-ray diffraction (solvent omitted for clarity).

Table 4

Relevant Internuclear Distances of 13:F–a

	X-ray 13:CsF			NMR 13:TBAF
DH···A	d D–H (Å)	d D···A (Å)	d H···A (Å)	d H···Ab (Å)
NH(a)···F–	0.85	2.641(7)	1.88	1.83
NH(b)···F–	0.87	2.727(6)	1.93	2.05
NH(c)···F–	0.85	2.837(6)	2.10	1.91
CH(11)···F–	0.93	3.119(7)	2.52

D = HB donor, A = HB acceptor.

Determined by NMR from HOESY experiments on 13:TBAF.

The observation that Cs+ interacts with n class="Chemical">fluoride in the solid state and in solution has implications for catalytic fluorination under HB-PTC because the process requires ion metathesis between Cs+ and the electrophile (E+). Also, under catalytic conditions, the formation of Cs[(2)2:F] will depend on the rate of formation (phase transfer) and consumption (fluoride delivery) of 2:CsF. For fast fluorination involving highly reactive electrophiles, the formation of Cs[(2)2:F] will be kinetically unfavorable. However, under conditions favoring aggregation such as high concentration, low temperature, or poorly reactive electrophiles, one would assume that Cs[(2)2:F] is present in solution.

Further information was gained on reactivity. To a solution of 2:CsF/n class="Chemical">Cs[(2)2:F] generated in situ by sonication of 2 and CsF in DCM-d2, β-bromosulfide 1a (2 equiv) was added as a solid, and the sample was briefly agitated. This resulted in the instantaneous formation of a precipitate assigned as CsBr. 1H and 19F NMR analyses showed the presence of β-fluorosulfide 3a formed with an enantiomeric ratio (e.r.) of 86.5:13.5, which is consistent with the enantioselectivity measured for the catalytic reaction (cf. e.r. = 88:12). This experiment unambiguously demonstrated that 2:CsF (in equilibrium with Cs[(2)2:F]) is effective for the enantioselective fluorination of 1a, an observation that supports our mechanistic hypothesis (Figure A).

Impact of Multiple H Bonds to Fluoride on Catalytic Fluorination

Preliminary computational studies suggested that 2:F– participates in the enantiodetermining step for the fluorination of meso-episulfonium ions under HB-n class="Chemical">PTC;[8a] striking structural similarities were found for the bisurea–fluoride anionic component featured in the TS and complex 2:TBAF in its ground state (in the solid state and in DCM-d2). The structure and conformation of bisurea–fluoride complexes in their ground state could therefore provide valuable information to understand catalyst performance. Catalysts 1–13 were tested with the fluorination of β-bromosulfide 1a with CsF in DCM or 1,2-difluorobenzene (1,2-DFB) at room temperature for 1.5 h (Table ). Initially, yields and enantioselectivities were determined for catalysts 3–7 bearing different N-alkyl groups and compared with the results obtained with the nonalkylated bisurea 1 and N-iPr bisurea 2 (Table , entries 1–7). All catalysts 1–7 provided excellent yields (>95%), implying that the 3,5-bis(trifluoromethyl)phenyl substituents ensure strong binding with fluoride and thus effective solid–liquid phase transfer for CsF. The nonalkylated BINAM urea 1 led to a lower e.r. compared to all N-alkylated analogues (entry 2, 86:14 e.r.) (ΔΔG⧧ = 1.07 kcal/mol). For catalysts 4–6, the level of enantioselectivity achieved is highly similar to that for 2 (e.r. 89.5:10.5–90:10); only the N-methylated catalyst 3 provided (S,S)-3a in slightly lower e.r. (entry 3, e.r. 88:12). N-(3-Pentyl) catalyst 7 on the other hand led to slight improvement (entry 7, 91:9 e.r.) (ΔΔG⧧ = 1.4 kcal/mol).

Table 5

Evaluation of Catalytic Performance of Bisurea Catalystsa

						1,2-DFB		DCM
entry	catalyst	R	R1	R2	1hJNH(a,c,b)···F– (Hz)	yieldb (%)	e.r.c	yieldb(%)	e.r.c
1	2	iPr	CF3		60, 50, 33	>95	90:10	>95	88:12
2	1	H	CF3		65	>95	86:14	>95	82:18
3	3	Me	CF3		60, 54, 34	>95	88:12	>95	83.5:16.5
4	4	Et	CF3		61, 54, 34	>95	90:10	>95	87.5:12.5
5	5	nPr	CF3		60, 53, 33	>95	89.5:10.5	>95	88:12
6	6	cPentyl	CF3		59, 48, 34	>95	89:11	>95	87.5:12.5
7	7	3-Pentyl	CF3		61, 52, 34	>95	91:9	>95	89.5:10.5
8	8	iPr	H	CF3	63, 39, 34	18	76.5:23.5	36	77:23
9	9	iPr	CF3	H	53, 52, 33	75	86.5:13.5	85	84:16
10	10	iPr	CF3	Me	52, 53, 34	48	87.5:12.5	80	84.5:15.5
11	11	iPr	F	CF3	60, 44, 33	68	81:19	18	79:21
12	12	iPr	CF3	F	59, 51, 33	>95	88.5:11.5	>95	86:14
13	13	iPr	F		59, 46, 34	>95	72:28	>95	74:26

General conditions:[8a] substrate (0.05 mmol), catalyst (0.005 mmol), and CsF (0.15 mmol) in 200 μL of solvent stirred at 1200 rpm for the indicated time.

Determined by 19F NMR using 4-fluoroanisole as the internal standard.

e.r. was determined by high-performance liquid chromatography (HPLC) analysis using a chiral stationary phase; 1,2-DFB = 1,2-difluorobenzene.

e.r. was determined by high-performance liquid chromatography (HPLC) analysis using a chiral stationary phase; 1,2-DFB = n class="Chemical">1,2-difluorobenzene.

The small variation in e.r. for catalysts bearing different N-alkyl groups suggests that this structural variation does not play a prominent role in differentiating between the TSs leading to one or the other enantiomer. This is corroborated by NMR conformational analyses, X-ray structures, and DFT calculations, which indicate that the n class="Chemical">N-alkyl substituent points away from the catalyst pocket that binds fluoride. These data also inform that the tridentate fluoride binding mode of N-alkylated catalysts 2–7 is beneficial over bidentate binding to ensure higher e.r. as demonstrated with the lower performance of 1, which lacks an N-alkyl group. Next, N-isopropyl bisureas 8–13 served the purpose of investigating the influence of NH-aryl substitution on both yields and e.r. (Table , entries 8–13). In this series, only catalysts 12 and 13 featuring fluorine substitution on both aryl rings afforded 3a in >95% yield, offering optimal performance as a phase-transfer catalyst for CsF and the ability to release fluoride for C–F bond construction. The replacement of 3,5-bis(trifluoromethyl)phenyl for phenyl or meta-xylyl, as shown with catalysts 8–10, was detrimental as yields plummeted as low as 18%, indicating poor phase-transfer capability. The most drastic effect was encountered when the aryl group attached to NH(c) lacked electron-deficient substituents (catalyst 8). Reactivity is dependent on the solvent, with catalysts 8–10 affording higher yields in DCM and catalyst 11 being much more effective in 1,2-DFB. The trends in enantioselectivity are similar in both solvents, with 1,2-DFB giving more often higher enantiomeric ratios. In this series, catalyst 13 is the least effective in terms of enantiocontrol. In all cases, no side products were detected in the crude mixture based on 1H NMR analysis.

The NMR data of the best-performing catalyst–TBAF complexes indicate that n class="Chemical">bisureas having stronger NH(c)···F– contribution (larger 1hJNH(c)···F) typically lead to a superior reaction outcome, suggesting that NH(c)···F– is a key interaction for achieving high yield and enantioselectivity. The striking role of NH(c) was highlighted in our original report, which presented intrinsic reaction coordinates to shed light on the mechanism of the reaction.[8a] The calculations showed that the three NH···F– hydrogen bonds elongated during fluoride delivery to the episulfonium ion as a consequence of charge neutralization; however, the elongation of NH(c)···F– occurred faster compared to those of NH(a)···F– and NH(b)···F–.

Conclusion

This investigation has unveiled important information on the conformation of BINAM-derived bisureas and their ability to bind fluoride in solution. Analysis of a set of bisureas featuring up to four NH groups enabled us to draw conclusions on the effect of multiple hydrogen bonds to fluoride on catalytic nucleophilic fluorination. The key findings are summarized hereafter.

• In DCM-d2 (25 mM), n class="Chemical">N-alkylated BINAM-derived bisureas with three NH groups exist as equilibrating structures resulting from an intramolecular time-dependent hydrogen bond that involves the two urea motifs. The corresponding nonalkylated BINAM bisurea with four HB donor NHs does not display such intramolecular interaction but undergoes aggregation when the concentration increases.

• Nonalkylated and alkylated bisureas bind n class="Chemical">fluoride in DCM-d2, resulting in the formation of two equilibrating species: a 2:1 bisurea–F– complex at low TBAF stoichiometry and a more stable 1:1 complex dominant when TBAF stoichiometry is >1 equiv. Conformational analysis by quantitative NOESY informed that N-alkylated bisureas underwent anti–anti to syn–anti isomerization of the N-alkylated urea upon addition of TBAF. This conformational change led to a dynamically stable 1:1 complex, allowing all three NHs to bind fluoride, an arrangement similar to the conformation observed for this complex in the solid state. The corresponding nonalkylated bisurea binds fluoride, engaging two of its four NH groups.

• Hydrogen-bond coupling constants (n class="Chemical">1hJNH···F) were observed and measured by 1H–19F CLIP-HSQC experiments, providing insight into the hydrogen-bonding network around fluoride, with distances calculated from 1H–19F NOE experiments. All N-alkylated bisurea catalysts bind fluoride, with all three NHs participating in hydrogen bonding. NH(a), located on the nonalkylated urea submotif and away from naphthyl, was the dominant contributor to the HB network (1hJNH(a)···F ≈ 60 Hz), while NH(c), belonging to the N-alkylated urea, varied significantly as a function of its electronic environment (1hJNH(c)···F ≈ 40–50 Hz). Hydrogen bonding with NH(b) located inside the cavity of the catalyst was the weakest interaction (1hJNH(b)···F ≈ 33–34 Hz). In contrast, only two of the four NH groups of nonalkylated BINAM bisurea 1 displayed HB with fluoride (1hJNH(a)···F = 65 Hz); the NHs involved are those proximal to the 3,5-bis(trifluoromethyl)phenyl rings.

• A bisurea–n class="Chemical">fluoride complex prepared from CsF was characterized in solution and in the solid state. Low-temperature NMR and 1H diffusion experiments revealed two species in equilibrium, a 1:1 bisurea–CsF complex as the main species along with a less-abundant 2:1 complex (85:15 at 298 K). 1hJNH···F detection provided information on the binding mode, with the 1:1 species showing a four-centered trifurcated HB with fluoride (1hJNH(a)···F = 52 Hz, 1hJNH(c)···F = 37 Hz, and 1hJNH(b)···F = 34 Hz). The 2:1 bisurea–CsF led to a six-centered hydrogen-bond network, engaging both bisureas as hydrogen-bond donors (1hJNH(a)···F = 40 Hz, 1hJNH(b)···F = 37 Hz, 1hJNH(c)···F = 14 Hz, 1hJNH(a′)···F = 58 Hz, and 1hJNH(b′)···F = 21 Hz). Spectroscopic studies of the 1:1 complex agreed with the solid-state structure from single-crystal X-ray diffraction, indicating that the Cs+ ion interacted both with naphthyl via a cation−π interaction and with F–. These interactions resulted in some reorganization of the HB network in the catalytic pocket, with NH(a)···F– and NH(c)···F– interactions reduced compared to those observed in the corresponding TBAF complex. The reaction of the preformed bisurea–CsF complex with a model β-bromosulfide led to instantaneous formation of the expected enantioenriched β-fluorosulfide; this experiment demonstrated that this bisurea–CsF complex enabled asymmetric fluorination with fast fluoride delivery.

• Catalytic fluorinations carried out with thirteen bisurea catalysts all characterized by NMR spectroscopy provided additional insight. Excellent reactivity was observed for all catalysts with electron-withdrawing substituents on the N-aryl groups, suggesting that this electronic pattern was necessary for the catalyst to act as a phase-transfer agent for n class="Gene">CsF. The resulting bisurea–fluoride complexes remained competent nucleophiles and provided the necessary chiral environment for enantioselective fluoride delivery. The data show that the hydrogen-bond interaction NH(c)···F– was critical to ensure good control over enantioselectivity. The nonalkylated bisurea gave the desired product in high yield, indicating that the formation of a three-centered bifurcated fluoride complex was sufficient for phase-transfer but not optimal for enantioselectivity.

In this study, we demonstrated that 1H/19F NMR spectroscopy is a powerful tool to analyze multiple H-bonding interactions with n class="Chemical">fluoride, thereby offering insight into catalyst performance for enantioselective nucleophilic fluorination under HB-PTC. Considering the importance of hydrogen-bonding interactions in catalysis, we anticipate that the analytical approach described herein would encourage further investigations with a multitude of catalyst candidates featuring multiple hydrogen-bond donor functionalities that are capable of anion binding.