Triphenylphosphine (PPh3), an important organic substance with a lone pair of electrons on phosphine, is a strong Lewis base and easy to form complexes with transition metals. PPh3 is ubiquitous for its nucleophilicity and reducing character. It is widely used in the synthesis of organic and organometallic compounds, such as Wittig reaction, Mitsunobu reaction, Mukaiyama-Corey lactonization, Appel reaction, Staudinger reaction, and as ligand in carbon-carbon bond formation reactions (e.g., Suzuki, Heck, and Negishi coupling)[1]. In the fields of fluorescent probes, PPh3 was often used for direct imaging of azide-bearing molecules based on bioorthogonal Staudinger ligation in living cells[2-4], which could form an stable amide bond in complex biological environment, such as in living cells and animals[5]. This reaction has been employed in a wide range of applications, including modification of cell surfaces[6], protein engineering[7], specific labeling of nucleic acids[8], proteomic studies, and as a general tool for bioconjugation[9,10]. Very recently, several PPh3-containing fluorescent probes for the discrimination of GSNO or HNO have been reported[11-16].
The extensive use of PPh3 is inevitable to cause phosphorous pollution to the environment and would pose a potential danger to human health. Traditionally, analysis of PPh3 in various matrices has been accomplished by spectrophotometric[17], titrimetric[18], chromatographic[19], and high performance liquid chromatography (HPLC)[20] methods. Unfortunately, those methods suffer limitations on the sensitivity and ease of use. A convenient and effective detection method for PPh3 is therefore desirable. Fluorescent techniques are extremely attractive due to their simplicity, high sensitivity and real-time detection[21]. However, little attention had been paid for the detecting of PPh3 in the research area of fluorescent probe. As a part of our continued effort for development of fluorescent probes for neutral organic substance[22-25], herein, we report the first fluorescent probe for PPh3 mimicking Staudinger ligation with a different arrangement of functionalities. As showed in Scheme 1, our design concept was to mask a hydroxyl-containing fluorophore as 2-azidophenylacetic ester. Such a latent fluorophore may react with PPh3 to undergo a rapid intramolecular acyl transfer through aza-ylide intermediate to release the fluorophore after hydrolysis[26].
All reagents were purchased from commercial suppliers and used without further purification. Solvents used were purified by standard methods prior to use. Acetonitrile in chromatographic purity and deionized water were used in detection. 1HNMR spectra were recorded on a VARIAN Mercury 400 MHz spectrometer. 1HNMR chemical shifts (δ) are given in ppm (s = singlet, d = doublet, t = triplet, q = quartet, m = multiplet) downfield from Me4Si, determined by chloroform (δ = 7.26 ppm) and dimethyl sulfoxide (δ = 2.5 ppm). 13CNMR spectra were recorded on a VARIAN Mercury 100 MHz spectrometer. 13CNMR chemical shifts (δ) are reported in ppm with the internal CDCl3 and d6-DMSO at 77.0 and 39.4 as standard, respectively. Mass spectrometric measurements were performed by AB SCIEX Triple TOFTM 5600+ mass spectrometry. Fluorescence spectra were recorded on FluoroSENS spectrophotometer. UV/Vis spectra were recorded on Perkin-Elmer Lambda 35 UV/Vis spectrophotometer at room temperature. All spectra were recorded at room temperature except for the fluorescence microscopic images.
1.2 Synthesis2-(2-Azidophenyl) acetic acid was prepared according to the reported method[27].
Probe 1: Under N2, a solution of 2-(2-azidophenyl) acetic acid (106 mg, 0.6 mmol), DCC (124 mg, 0.6 mmol), and DMAP (22 mg, 0.2 mmol) in 10 mL of CH2Cl2 were added dropwise in a solution of fluorescein (66 mg, 0.2 mmol) in 3 mL of CH2Cl2 at ambient temperature. The reaction mixture was stirred for 3 h. Solvent was evaporated in vacuo and the residue was put onto preparative silica gel plates (developed with CH2Cl2) to isolate probe 1 as a white solid after evaporation of solvent (75 mg, 83%).
1HNMR (400 MHz, CDCl3): 8.03 (d, 1H, J = 8.0 Hz), 7.65 (m, 2H), 7.38 (td, 2H, J = 8.0, 2.0 Hz), 7.31 (dd, 2H, J = 8.0 Hz, 1.0 Hz), 7.21 (d, 2H, J = 8.0 Hz), 7.15 (m, 3H), 7.09 (s, 2H), 6.82 (d, 4H, J = 4.0), 3.85 (s, 4H). 13CNMR (100 MHz, CDCl3): 169.20, 169.02, 153.01, 152, 16, 151.55, 138.83, 135.35, 131.56, 130.10, 129.21, 128.98, 126.06, 125.27, 125.03, 124.79, 124.05, 118.32, 117.69, 116.51, 110.34, 81.65, 36.84. HRMS-ESI: [M]+ calculated for C36H22N6O7Na+1: 673.1442; found: 673.1438.
2 Results and DiscussionThe implementation of our design concept was exemplified by the fluorescein-based probe 1 as showed in scheme 2. Fluorescein is a well-known highly fluorescent dye and is non-fluorescent when the two hydroxyl groups were both acylated. In this study, fluorescein reacted with excess of 2-azidophenylacetic acid in the presence of DCC and DMAP to generate the desired masked fluorophore. Probe 1 may react with PPh3 in a sequential manner to release highly fluorescent mono-deprotected fluorescein and fluorescein. It is known that even mono-deprotected species of probe 1 is also strong fluorescent with almost identical emission maxima[28].
Probe 1 does not have obvious absorption band around 490 nm and is almost non-fluorescent. When probe 1 (1 mol/L) was subjected to PPh3 (10 mol/L, 10 equiv) in DMSO/PBS buffer (0.5:100, V/V, 10 mmol/L, pH 7.4) at 25 ℃, there were distinct changes in the absorption and emission of probe 1 (Figure 1). Upon addition of PPh3, the absorption at 490 nm increased with increasing time, fluorescence intensity at 515 nm enhanced concurrently and reached the maximum after about 60 min. These preliminary results indicated that the expected chemical reaction between the PPh3 and probe 1 released fluorescein.
With the positive results obtained, we then carried out concentration-dependent fluorescence response studies toward various concentrations of PPh3. Upon incremental addition of PPh3 with concentration range of 0-20 μmol/L to DMSO/PBS buffer (0.5:100, V/V, 10 mmol/L, pH7.4) solution of probe 1 (1 μmol/L) at 25 ℃ and allowed to react for 60 min, a concurrently increased fluorescence at 515 nm was observed (Figure 2a). Further studies suggested a concentration-dependent response with linear character of probe 1 toward PPh3 ranged from 1×10-7 mol/L to 8×10-7 mol/L. The detection limit for PPh3 was estimated to be 10 nmol/L based on the signal-to-noise ratio (S/N=3), which suggested that our probe was fairly sensitive to detect PPh3.
To investigate the selectivity, various potential interfering species were tested. Probe 1 was initially investigated in the presence of various metallic ions in DMSO/PBS buffer (0.5:100, V/V, 10 mmol/L, pH 7.4) at 25 ℃ by adding PPh3 (10 μmol/L) or 100 μmol/L of metallic ion to the solution of probe 1 (1 μmol/L) and incubated for 60 min prior to follow the fluorescence at 515 nm (Figure 3a). None of the metallic ion used caused any noticeable fluorescence enhancement, only PPh3 induced significant fluorescence (Figure 3a). Further investigations on competitive experiments wherein a mixture of PPh3 (10 μmol/L) and individual metallic ion (100 μmol/L) were incubated in DMSO/PBS buffer (0.5:100, V/V, 10 mmol/L, pH 7.4) at 25 ℃ for 60 min suggested that only PPh3 turned on obvious fluorescence (Figure 3b).
We subsequently tested more potential interfe-ring analytes of biothiols, nucleophiles, and various anions and the results are shown in Figure 4. Both incubation of probe 1 with individual analyte and competitive experiments with mixture of PPh3 and the applied interfering analyte provided evidence that only PPh3 elicited obvious fluorescence turn-on (Figure 4). Notably, although aryl azide functiona-lity is known to be reduced by NaSH or Na2S to produce aniline, we did not observe obvious fluorescence increment presumably due to the low nucleophilicity of aniline compared with aza-ylide species. Thus, we can conclude that probe 1 displayed excellent selectivity toward PPh3, namely, only strong fluorescence was visualized when probe 1 exposed to PPh3, which was not disturbed by other substances.
The effect of pH on the fluorescence intensity and reactivity of probe 1 (1 μmol/L) was examined in the absence and presence of PPh3 in DMSO/PBS buffer (0.5:100, V/V, 10 mmol/L) at 25 ℃ for 60 min (Figure 5). Probe 1 is stable in pH range of 0.0-10.0. However, at high pH greater than 10.0, the ester bond of probe 1 started to be cleaved. In the presence of PPh3, the increased reaction rate at high pH environment was observed and the preferred pH range was 6.0-10.0.
The above investigations revealed that probe 1 was superior to detect PPh3 with excellent sensitivity and selectivity. The big off-to-on (φ: 0→1) contrast ratio and dramatic change of fluorescence upon addition of PPh3 allow sensitive identification of PPh3 even with "naked eye" as shown in Figure 6. When probe 1 (1 μmol/L) was treated with PPh3 (10 μmol/L) in comparison with various metallic ions, anions, amino acids, reductants or oxidants (100 μmol/L each) in water containing 0.5% DMSO solution, only PPh3 resulted strong green fluorescence without any interference from other analyte.
In summary, we have developed a novel fluorescent probe 1 with high selectivity and sensitivity for PPh3 by attaching 2-azidophenylacetyl functionality to fluorescein mimicking Staudinger ligation. Probe 1 is promising for the sensitive detection of PPh3, and the detection limit is about 1×10-8 mol/L measured in DMSO/PBS buffer. The sensitive detection of PPh3 can be viewed with "naked eye" in aqueous solution containing 0.5% DMSO.
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