Won Joon
Choi
a,
Sungkyu
Choi
b,
Kei
Ohkubo
c,
Shunichi
Fukuzumi
*c,
Eun Jin
Cho
*b and
Youngmin
You
*a
aDepartment of Advanced Materials Engineering for Information and Electronics, Kyung Hee University, Yongin, Gyeonggi-do 446-701, Korea. E-mail: odds2@khu.ac.kr
bDepartment of Applied Chemistry & Department of Bionanotechnology, Hanyang University, Ansan, Gyeonggi-do 426-791, Korea. E-mail: echo@hanyang.ac.kr
cDepartment of Material and Life Science, Graduate School of Engineering, Osaka University, ALCA, Japan Science and Technology Agency (JST), Suita, Osaka 565-0871, Japan. E-mail: fukuzumi@chem.eng.osaka-u.ac.jp
First published on 24th November 2014
The incorporation of a trifluoromethyl group into an existing scaffold can provide an effective strategy for designing new drugs and agrochemicals. Among the numerous approaches to trifluoromethylation, radical trifluoromethylation mediated by visible light-driven photoredox catalysis has gathered significant interest as it offers unique opportunities for circumventing the drawbacks encountered in conventional methods. A limited understanding of the mechanism and molecular parameters that control the catalytic actions has hampered the full utilization of photoredox catalysis reactions. To address this challenge, we evaluated and investigated the photoredox catalytic trifluoromethylation reaction using a series of cyclometalated Pt(II) complexes with systematically varied ligand structures. The Pt(II) complexes were capable of catalyzing the trifluoromethylation of non-prefunctionalized alkenes and heteroarenes in the presence of CF3I under visible light irradiation. The high excited-state redox potentials of the complexes permitted oxidative quenching during the cycle, whereas reductive quenching was forbidden. Spectroscopic measurements, including time-resolved photoluminescence and laser flash photolysis, were performed to identify the catalytic intermediates and directly monitor their conversions. The mechanistic studies provide compelling evidence that the catalytic cycle selects the oxidative quenching pathway. We also found that electron transfer during each step of the cycle strictly adhered to the Marcus normal region behaviors. The results are fully supported by additional experiments, including photoinduced ESR spectroscopy, spectroelectrochemical measurements, and quantum chemical calculations based on time-dependent density functional theory. Finally, quantum yields exceeding 100% strongly suggest that radical propagation significantly contributes to the catalytic trifluoromethylation reaction. These findings establish molecular strategies for designing trifluoromethyl sources and catalysts in an effort to enhance catalysis performance.
Photoredox catalysed trifluoromethylation reactions typically employ coordinatively saturated 4d or 5d transition metal complexes, such as Ru(II) polypyridine complexes53–66 and cyclometalated Ir(III) complexes,64,67–70 as the catalysts. Photoexcitation of these complexes promotes the formation of a long-lived triplet metal-to-ligand charge-transfer (3MLCT) transition state, in which the one-electron oxidized metal core and the one-electron reduced ligand act as the oxidant and reductant, respectively. A variety of reagents, such as CF3I,55,60–62,64,67,71,72 silver trifluoroacetate,73 triflyl chloride (CF3SO2Cl),54,69 the Langlois reagent,74 the Togni reagent,56,58,59,65,70 the Umemoto reagent,53,57,63,68,70 and the Shibata reagent,66 can serve as trifluoromethyl radical (˙CF3) sources,75 and the key step involves the reductive cleavage of these reagents under photoirradiation of the catalyst. Two possible routes to the reductive generation of ˙CF3 are available (Scheme 1). The photoexcited catalyst can directly deliver an electron to the ˙CF3 source (oxidative quenching pathway), followed by the reductive regeneration of the catalyst by an electron donor. Alternatively, the photoexcited catalyst may be preferentially reduced by an electron donor to a one-electron reduced species that subsequently transfers an extra electron to the ˙CF3 source (reductive quenching pathway). Although the net reactions are identical (i.e., CF3X + donor → ˙CF3 + donor˙+ + X−), each of two pathways involves reductants with distinct stabilities and thermodynamic driving forces for reductive cleavage. As shown in Scheme 1, the oxidative and reductive quenching pathways involve the photoexcited catalyst and one-electron reduced catalyst, respectively, as the reductants. In most cases, photoredox catalysts, such as [Ru(bpy)3]2+ and fac-Ir(ppy)3 (bpy = 2,2′-bipyridine and ppy = 2-phenylpyridinate), can promote both oxidative53,54,56–59,63,65,68–70 and reductive55,60–62,64,67,74 quenching cycles, due to the positive driving forces for electron transfer to typical ˙CF3 sources and from electron donors.7 The presence of two competing pathways hampers the elucidation and optimization of the molecular parameters associated with the catalysis. Further developments are needed to identify photoredox catalysts that select a single quenching process. This need prompted us to employ cyclometalated Pt(II) complexes as photoredox catalysts for trifluoromethylation reactions. The cyclometalated structure between a Pt(II) core and an anionic cyclometalating (C∧N) ligand can cathodically shift the excited-state redox potentials. This effect provides the thermodynamic conditions needed to suppress excited-state reduction while enabling excited-state oxidation of the Pt complex. Thus, the resulting photoredox catalysis reaction strictly follows an oxidative quenching cycle. The additional benefits of using Pt(II) complexes are enormous. The complexes can be easily modified, allowing the molecular parameters to be synthetically tailored. Control over the substituents in the C∧N ligands provides a viable approach to tuning the excited-state redox potentials and lifetimes of the complexes. Molecular design efforts can benefit from the rich knowledge established in previous studies of Pt(II) complexes in the context of electrophosphorescence and sensors.76–79 Taking advantage of these properties, photoredox catalytic applications of Pt(II) complexes in polymerization,80,81 hydrogen production,82 and oxidation reactions83,84 have been demonstrated. It is, however, noted that trifluoromethylation by a Pt(II) complex has yet to be established.
Here, we report the first demonstration of photoredox catalytic trifluoromethylation using cyclometalated Pt(II) complexes. Key intermediates in the photoredox catalytic cycle were monitored directly using spectroscopic techniques. The spectroscopic identification of catalytic intermediates in the visible light-driven trifluoromethylation reaction is unprecedented. Mechanistic studies revealed that the photoredox catalysis involves an oxidative quenching pathway. The kinetic parameters associated with each step of the catalytic cycle were determined, providing novel insights into enhancing the catalysis performance.
The UV-vis absorption spectra of the Pt(II) complexes (10 μM in CH3CN) featured characteristic MLCT transition bands at 380 nm (logε = 3.76; Ptdfppy), 386 nm (log
ε = 3.91; Ptppy), and 420 nm (log
ε = 3.78; PtOMe), with tails that approached the visible regions (Fig. 1a).85,87,88 Strong photoluminescence emission was observed upon photoexcitation of the MLCT bands at room temperature (see ESI, Fig. S1† for the photoluminescence spectra). The photoluminescence lifetimes (τobs) of the emission were on the order of submicroseconds or microseconds, indicating phosphorescence (Fig. 1b). It should be noted that the τobs value increased by two orders of magnitude as the electron richness of the C∧N ligand was increased (i.e., in PtOMe). The slow decay was indicative of weak MLCT contributions to the spin-forbidden electronic transition. Indeed, the MLCT character estimated by time-dependent density functional theory (CPCM(CH3CN)-TD-B3LYP/LANL2DZ:6-311+G(d,p)//B3LYP/LANL2DZ:6-311+G(d,p)) was significantly smaller in the PtOMe complex (15%) than in the Ptdfppy complex (28%) (Table 1). Therefore, the triplet state responsible for phosphorescence emission can be best described as an admixture of the MLCT, ligand-centered (LC) π–π*, and intraligand charge-transfer (ILCT) transitions. The large variations in τobs were useful for examining the notion of whether a long-lifetime catalyst could exhibit better photoredox catalytic performance (vide infra). The photophysical data, including the photoluminescence quantum yields (PLQY) and the triplet-state energies (ΔET) of the Pt(II) complexes are summarized in Table 1.
λabsa (MLCT) (nm; log![]() |
PLQYb | MLCTc (%) | ΔETd (eV) | E ox (V vs. SCE) | E red (V vs. SCE) | E *ox (V vs. SCE) | E *red (V vs. SCE) | τ obs (μs) | |
---|---|---|---|---|---|---|---|---|---|
a 10 μM in acetonitrile solutions, 298 K. b Photoluminescence quantum yields determined relative to the fluorescein standard (0.1 N NaOH (aq), PLQY = 0.79). c MLCT contribution to the triplet transition estimated using AOMix based on the TD-DFT (CPCM(CH3CN)-TD-B3LYP/LANL2DZ:6-311+G(d,p)//B3LYP/LANL2DZ:6-311+G(d,p)) results. d Triplet-state energy determined from the phosphorescence spectra. e Determined using cyclic and differential pulse voltammetry. Conditions: scan rate = 100 and 0.4 mV s−1 for CV and DPV, respectively; 1.0 mM Pt complex in Ar-saturated acetonitrile containing the 0.10 M Bu4NPF6 supporting electrolyte; a Pt wire counter electrode and a Pt microdisc working electrode; the Ag/AgNO3 couple as the pseudo-reference electrode; qr = quasi-reversible; irr = irreversible. f Estimated using Ered = Eox − ΔEg, where ΔEg is the optical band gap energy: Ptdfppy, 3.08 eV; Ptppy, 2.95 eV; PtOMe, 2.72 eV. g E *ox = Eox − ΔET. h E *red = Ered + ΔET. i Photoluminescence lifetimes observed at λem = 465 nm (Ptdfppy), 483 nm (Ptppy), and 543 nm (PtOMe). The measurements were collected in triplicate. | |||||||||
Ptdfppy | 380 (3.76) | 0.31 | 28 | 2.73 | 0.62 (qr) | −2.46 | −2.11 | 0.27 | 0.382 ± 0.059 |
Ptppy | 386 (3.91) | 0.44 | 27 | 2.64 | 0.57 (irr) | −2.38 | −2.07 | 0.26 | 2.21 ± 0.14 |
PtOMe | 420 (3.78) | 0.74 | 15 | 2.45 | 0.52 (irr) | −2.20 | −1.93 | 0.25 | 11.6 ± 0.50 |
The ground-state redox potentials of the Pt(II) complexes were determined by cyclic voltammetry (CV), and were further verified using differential pulse voltammetry (DPV). Quasi-reversible (Ptdfppy) and irreversible (Ptppy and PtOMe) oxidation waves were measured at 0.52–0.62 V vs. SCE (see ESI, Fig. S2† for the voltammograms), corresponding to the PtIII/II redox couple.88 These oxidation potentials (Eox) were more positive than the Eox value (0.47 V vs. SCE) of N,N,N′,N′-tetramethylethylenediamine (TMEDA), a sacrificial electron donor. Because reduction was not observed until −1.8 V vs. SCE, the reduction potentials (Ered) for the Pt(II) complexes were calculated according to the relationship, Ered = Eox − ΔEg, where ΔEg is the optical band gap energy. As summarized in Table 1, the Ered value shifted cathodically as the electron density of the C∧N ligand decreased. The same trend was observed in the excited-state oxidation potential (E*ox = Eox − ΔET), whereas the excited-state reduction potential (E*red = Ered + ΔET) remained relatively unchanged across the series of the Pt(II) complexes (Table 1). The changes in the E*ox values were dominated by ΔET rather than Eox, as inferred from ΔΔET (0.28 eV) > eΔEox (0.10 eV; e is the elementary charge). The E*ox values (−2.11 to −1.93 V vs. SCE) were more negative than the Ered value of CF3I (−0.91 V vs. SCE,89 determined by DPV (ESI, Fig. S3†)), indicating that the photoexcited Pt complexes could donate an electron to CF3I under the driving force for the photoinduced electron transfer (−ΔGPeT = e[E*ox(Pt) − Ered(CF3I)]) of 1.02–1.20 eV. The photoexcited complexes could not be reduced by TMEDA, as indicated by the negative driving force (−ΔGPeT = e[Eox(TMEDA) − E*red(Pt)] = −0.20∼ −0.22 eV).
Entry | Product | Yieldb (%; E/Z ratioc) | |
---|---|---|---|
a An oven-dried resealable test tube equipped with a magnetic stirrer bar was charged with an alkene (0.50 mmol), sealed with a screw-cap, and degassed by alternating between putting under vacuum and backfilling with argon. A solution of Ptppy (1.0 mol%, 0.0050 mmol) in CH3CN (2.0 mL, 0.25 M) and DBU (1.0 mmol) was then added to the tube under argon. CF3I (1.5 mmol) was then delivered to the reaction mixture using a gastight syringe. The test tube was placed under blue LEDs (7 W) at room temperature for 5–10 h, and the progress of each reaction was monitored by TLC or gas chromatography. b The given yields are isolated yields reported as the average of two runs, except for 2b (entry 2), which was monitored using 19F NMR due to the volatility of the product. c The E/Z ratio was determined by 1H NMR spectroscopy and gas chromatography. | |||
1 | 2a |
![]() |
97 (25![]() ![]() |
2 | 2b |
![]() |
82 (25![]() ![]() |
3 | 2c |
![]() |
85 (30![]() ![]() |
4 | 2d |
![]() |
95 (25![]() ![]() |
5 | 2e |
![]() |
95 (25![]() ![]() |
6 | 2f |
![]() |
94 (25![]() ![]() |
7 | 2g |
![]() |
88 (only E) |
8 | 2h |
![]() |
89 (40![]() ![]() |
9 | 2i |
![]() |
96 (25![]() ![]() |
10 | 2j |
![]() |
89 (25![]() ![]() |
Entry | Product | Yieldb (%) | |
---|---|---|---|
a An oven-dried resealable test tube equipped with a magnetic stirrer bar was charged with an acetonitrile solution (2.0 mL) containing heteroarene (0.50 mmol), TMEDA (1.0 mmol), and Ptppy (2.0 mol%, 0.010 mmol), and sealed with a screw-cap. The reaction mixture was degassed by alternating between putting under vacuum and backfilling with argon, after which CF3I (1.5 mmol) was delivered using a gastight syringe. The test tube was placed under blue LEDs (7 W) at room temperature for 10–24 h, while the progress of each reaction was monitored by TLC. b The given yields are isolated yields obtained by taking the average of two runs, except for 4a (entry 1), which was monitored using 19F NMR due to the volatility of the product. c Trifluoromethylation at the phenyl moiety of indole occurred at <10% (19F NMR and GC). | |||
1 | 4a |
![]() |
95 |
2 | 4b |
![]() |
75 |
3 | 4c |
![]() |
70 |
4 | 4d |
![]() |
68 |
5 | 4e |
![]() |
67c |
Scheme 2 illustrates the proposed mechanism underlying the photoredox catalytic trifluoromethylation reaction in the presence of the cyclometalated Pt(II) complex (PtII(C∧N) hereafter) catalysts. Photoexcitation of PtII(C∧N) promoted an electronic transition to a singlet MLCT (1MLCT) state, which underwent ultrafast intersystem crossing to a 3MLCT state (i.e., 3[PtIII(C∧N)˙−]*). Diffusional collision of 3[PtIII(C∧N)˙−]* with CF3I led to the reversible formation of an encounter complex ([3[PtIII(C∧N)˙−]* CF3I]; path B in Scheme 2). Oxidative electron transfer from the Pt catalyst to CF3I in the encounter complex generated a geminate radical ion pair, [[PtIII(C∧N)]+ CF3I˙−]. It should be noted that ligand oxidation (i.e., [PtII(C∧N)˙+]+) could not be excluded, because the triplet state of the Pt(II) complex contained significant LC character (vide supra). An encounter complex formed between the photoexcited catalyst and an electron donor, such as TMEDA, could also have been generated (path A in Scheme 2); however, the negative driving force abrogated the formation of a geminate radical ion pair (vide supra). Two pathways were available to the [[PtIII(C∧N)]+ CF3I˙−] species: the first pathway involved quenching to the original species (i.e., PtII(C∧N) and CF3I) by back electron transfer (BeT), and the other pathway involved dissociation into [PtIII(C∧N)]+ and CF3I˙−. In the latter path, prompt cleavage of the C–I bond in CF3I˙− resulted in the formation of ˙CF3. Radical addition of ˙CF3 to substrates formed trifluoromethylated radical species. The photocatalytic cycle was completed by the reductive regeneration of PtII(C∧N) with sacrificial electron donors, such as TMEDA and DBU. Alternatively, PtII(C∧N) was recovered through the radical-polar mechanism, which involved oxidation of radical species of the trifluoromethylated substrate to the cation (path C in Scheme 2). In this case, the resulting cationic species of the trifluoromethylated substrate was trapped by the strong nucleophile, I−. It should be noted that the compound bearing both iodide and trifluoromethyl groups could also be produced by radical propagation between the CF3I and radical species of the trifluoromethylated substrate (path D in Scheme 2). In both cases (i.e., paths C and D), E2 elimination assisted by TMEDA or DBU furnished the desired product, with the stoichiometric generation of ammonium iodide salts.
The photoredox catalytic cycle described above involved three key electron-transfer steps: forward photoinduced electron transfer (PeT), BeT, and reductive regeneration of the catalyst. The electron-transfer processes and their intermediate species generated during the photoredox catalytic trifluoromethylation reaction had not been directly observed to date. No kinetic information about electron transfer was available in the literature.
k r (104 s−1) | k nr (104 s−1) | k PeT (108 M−1 s−1) | k BeT (1010 M−1 s−1) | k regen (108 M−1 s−1) | |
---|---|---|---|---|---|
a Radiative rate constant. b Non-radiative rate constant. c Rate constant for photoinduced electron transfer. d Rate constant for back electron transfer. e Rate constant for regeneration of the Pt(II) complex photocatalyst by reductive electron transfer from TMEDA. | |||||
Ptdfppy | 81.2 | 181 | 8.8 | 2.2 | 7.7 |
Ptppy | 1.99 | 25.3 | 7.9 | 1.4 | 5.0 |
PtOMe | 6.38 | 2.24 | 4.4 | 0.57 | 3.4 |
After oxidative quenching by PeT, BeT could occur in the geminate radical ion pair to restore [PtII(C∧N)] and CF3I. The BeT process was monitored according to the [PtIII(C∧N)]+ decay signals in the microsecond regime. Fig. 4a presents the transient absorption spectra of a deaerated acetonitrile solution containing 100 μM PtOMe and 50 mM CF3I after nanosecond photoexcitation at 355 nm (O.D. = 0.52). The spectra display a visible absorption band at 770 nm, and similar visible absorption signatures are also observed for Ptdfppy (740 nm) and Ptppy (730 nm) (ESI, Fig. S8†). These absorption bands can be reasonably ascribed to [PtIII(C∧N)]+ because chemical oxidation of 50 μM Ptdfppy by 50 μM [FeIII(bpy)3]3+ produced a visible absorption band around 700 nm (ε = 3200 M−1 cm−1; ESI, Fig. S9†), although the irreversible oxidation of Ptppy and PtOMe hampered our ability to measure the visible absorption bands. As shown in Fig. 4a, the visible absorption spectrum of [PtIII(C∧N)]+ can be reproduced using quantum chemical simulation methods based on time-dependent density functional theory (CPCM(CH3CN)-TD-B3LYP/LANL2DZ:6-311+G(d,p)//B3LYP/LANL2DZ:6-311+G(d,p)). The molar absorbances (ε) of the one-electron oxidized species of PtOMe and Ptppy were thus estimated based on the simulated spectra. The decay trace of the one-electron oxidized species of PtOMe was monitored at 770 nm, and the rate constant for BeT (kBeT) was determined from the second-order linear fit of the decay traces to be 2.2 × 1010 M−1 s−1 (Fig. 4b; see ESI, Fig. S8† for other complexes). The kBeT value was approximately one order of magnitude greater than the kPeT values (Table 4), and was comparable to the diffusion rate constant (kdiff) in CH3CN at 298 K, 1.93 × 1010 M−1 s−1, calculated according to the Stokes–Einstein–Smoluchowski equation, kdiff = (8kBNAT)/(3η), where kB, NA, T, and η are the Boltzmann constant, Avogadro's number, the absolute temperature, and the viscosity of the solvent, respectively. A significant fraction of the CF3I˙− species returned to CF3I via BeT prior to escaping the solvent cage. This result revealed the importance of controlling the molecular structure to suppress BeT.
![]() | ||
Fig. 4 Determination of the rate constant for back electron transfer (kBeT) by nanosecond laser flash photolysis (λex = 355 nm) for a deaerated acetonitrile solution containing 100 μM PtOMe (O.D. at 355 nm = 0.52) and 50 mM CF3I. (a) Transient absorption spectra recorded at 4 μs (red), 8 μs (blue), and 252 μs (black) after photoexcitation. The dotted grey line and grey bars are the simulated (CPCM(CH3CN)-TD-B3LYP/LANL2DZ:6-311+G(d,p)//B3LYP/LANL2DZ:6-311+G(d,p)) absorption spectrum and calculated absorbance, respectively, of the one-electron oxidized species of PtOMe. (b) Plot of ε/absorbance of the 770 nm band vs. time. The kBeT value was determined from the second-order linear fit (red). The results obtained from other Pt(II) complexes are shown in the ESI, Fig. S8.† |
The photoredox cycle was completed by the one-electron reduction of [PtIII(C∧N)]+. Regeneration was accomplished primarily by electron transfer from a sacrificial electron donor, such as TMEDA, as determined based on the positive driving force (−ΔGeT = e[Eox(TMEDA) − Eox(Pt)] = 0.05–0.15 eV). This process was monitored by acquiring the decay traces of [PtIII(C∧N)]+ under various concentrations of TMEDA. Fig. 5a shows the decay traces of the 770 nm absorption band for the deaerated acetonitrile solutions containing 100 μM PtOMe and 50 mM CF3I in the presence and absence of TMEDA. The half-life of the decay trace decreased from 70 μs to 25 μs upon the addition of 50 μM TMEDA. This behavior was ascribed to the reductive regeneration of PtOMe by TMEDA. The regeneration rate was calculated from the relationship, 1/τ(TMEDA) − 1/τ, where τ(TMEDA) and τ are the half-lives of the 770 nm decay traces in the presence and absence of TMEDA, respectively. The pseudo-first order linear fit of the regeneration rates vs. the concentration of TMEDA yielded the rate constants for regeneration (kregen) in the range of 3.4 to 7.7 × 108 M−1 s−1. As shown in Table 4, these values are comparable to the kPeT values but are approximately one order of magnitude smaller than kBeT.
The classical Marcus theory for adiabatic outer-sphere electron transfer provided a valuable basis for correlating the kinetic parameters (i.e., kPeT, kBeT, and kregen) to the driving force. The electron transfer steps could be best described using eqn (1) with consideration for the diffusion process:92,93
![]() | (1) |
As shown in Fig. 6, the kPeT values adhere well to the theoretical curve calculated using the Marcus theory of electron transfer, with a λ value of 2.7 eV. The large reorganization energy indicates bond scission in CF3I after electron transfer. The positive dependence of kPeT on −ΔGPeT points to the occurrence of PeT in the Marcus normal region (i.e., −ΔGPeT < λ). The Marcus normal behavior suggests two possible strategies for accelerating PeT: (1) raising E*ox of the photoredox catalyst by incorporating ligands with wide band gap energies (i.e., high ΔET) and weak π-backbonding abilities (i.e., cathodically shifting Eox), and (2) using ˙CF3 sources with large (more positive) Ered values, such as the Shibata reagent.66 The former approach involves a tradeoff because the effect may be offset by a reduction in the visible absorption cross-section.
![]() | ||
Fig. 6 Plots of the log(rate constant) (log![]() |
The analyses using eqn (1) revealed a positive dependence of kBeT on −ΔGBeT, with a λ value of 2.7 eV. This λ value was identical to that obtained under PeT, as expected for forward and reverse electron transfer. One potential strategy for retarding the hazardous BeT involves raising the Eox of the photoredox catalysts using ligands with weak π-accepting or strong σ-donating properties. Alternatively, the use of ˙CF3 sources with large (more positive) Ered values may be advantageous.
The reductive regeneration by TMEDA was found to be essential because the trifluoromethylated products could not be obtained if TMEDA was replaced with a Brønsted base, such as K3PO4, K2HPO4 or KOtBu (ESI, Tables S1 and S2†). As shown in Fig. 6, the regeneration by TMEDA followed a typical Rehm–Weller behavior with a λ value of 1.2 eV. The large positive dependence indicated that the rate of regeneration increased using catalysts with large Eox values; however, predicting the influence of kregen on the overall cycle was not straightforward due to the presence of an additional regeneration path involving radical species generated on the trifluoromethylated substrate (path C in Scheme 2). The above analyses based on the Marcus theory of electron transfer established that the photoredox catalysis performance could be improved by implementing the following molecular controls: (1) Eox of the catalyst should be as small as possible to speed up PeT and to slow down BeT; (2) Eox of the catalyst should be more positive than Eox of the sacrificial electron donor to warrant regeneration; (3) the value of ΔET for the catalyst may be optimized, since larger values of ΔET will accelerate oxidative PeT but very large ΔET values eventually initiate competing reductive quenching.
Having established the photoredox catalytic cycle, we sought to understand the influence of the C∧N ligand structures on the overall catalytic performance. The quantum yields of the three Pt(II) complexes for trifluoromethylation (QY) of 1-dodecene and N-methylpyrrole were determined using standard ferrioxalate actinometry (6.0 mM K3[Fe(C2O4)3], quantum yield = 1.1 at 420 nm; see the ESI† for experimental details). As summarized in Table 5, the QY values exceeded 100% in all cases. These results strongly indicated the significant involvement of radical propagation (path D in Scheme 2). This hypothesis was supported by the observation of a dark-state reaction after shutting off photoirradiation (ESI, Fig. S10†). It is noted that the Pt(II) catalyst prepared with an electron-poor C∧N ligand produced a larger value of QY for the alkene, whereas the QY values for the heteroarene exhibited an opposite trend. Because the radical propagation and subsequent steps, including iodination and E2 elimination, were independent of the identity of the photoredox catalyst, variations in QY could be explained in terms of the photoredox cycle. Obviously, the QYs for 1-dodecene followed a trend opposite to those of f and kBeT for the series of Pt(II) complexes, suggesting that the effects of f and kBeT would be marginal. One possible explanation for the QY trend is that regeneration is the limiting step in the overall catalytic performance. Of note, in Table 5 are the greater QY values of the Pt(II) complexes over those of the well-established Ir(III) and Ru(II) catalysts. The improved photon economy of the Pt(II) catalysts is likely due to elimination of the hazardous reductive quenching pathway that exists in the Ir(III) and Ru(II) catalyst systems.
Ptdfppy | Ptppy | PtOMe | fac-Ir(ppy)3 | [Ir(ppy)2(dtbbpy)]PF6 | [Ru(bpy)3]Cl2 | |
---|---|---|---|---|---|---|
a Quantum yields for trifluoromethylation of 1-dodecene. b Quantum yields for trifluoromethylation of N-methylpyrrole. The quantum yields were determined using standard ferrioxalate actinometry (6.0 mM K3[Fe(C2O4)3], QY = 1.1 at 420 nm (light intensity = 6.7 × 10−10 Einstein s-1)). | ||||||
QYalkenea | 18 | 17 | 16 | 12 | 10 | 6.5 |
QYheterob | 2.4 | 3.9 | 4.8 | 3.0 | 2.5 | 0.67 |
Footnote |
† Electronic supplementary information (ESI) available: Experimental details and the syntheses of the Pt(II) catalysts; Fig. S1–S55, showing the phosphorescence spectra, femto- and nanosecond laser flash photolysis results, cyclic and differential pulse voltammograms, phosphorescence quenching experiment results, photoinduced ESR spectrum, spectroelectrochemical UV-vis-NIR absorption spectrum, dark-state reaction results, and 1H, 13C, and 19F NMR spectra; Scheme S1, presenting the synthetic routes to the Pt(II) complexes; Tables S1–S6, listing optimization results for the trifluoromethylation of 1-dodecene, 3-methylindole and N-methylpyrrole, and the Cartesian coordinates for the optimized geometries of one-electron oxidized species of the Pt complexes. See DOI: 10.1039/c4sc02537g |
This journal is © The Royal Society of Chemistry 2015 |