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A Novel Phosphorescent Iridium(III) Complex Bearing Formamide for Quantitative Fluorine Anion Detection

: Fluorine anion plays a critical role for human health, especially for the teeth and the skeletal system, and a deficiency or excess of fluorine anion will result in various diseases. Thus, the accurate and timely detection of fluorine content is of great importance. Herein, a novel and sensitive fluorine probe based on ionic iridium(III) complex using 5-formamide phenanthroline as an ancillary ligand was designed and synthesized rationally. The probe exhibited excellent performance for F − detection in organic solvents. H-bonding between the fluoride and the amide proton was formed, thus changing the photophysical properties of the probe and leading to significant phosphorescence quenching. Nuclear magnetic resonance titration and theoretical calculations were carried out to understand the mechanism in detail. This is the first report of an iridium(III) complex probe for F − detection based on the interaction between formamide and fluorine anion.


Introduction
Fluorine is an essential element for the human body. It is conducive to boosting the immune system and plays a vital physiological role in the health of bones, teeth, skin, and eyesight [1,2]. Fluorine mainly exists in the human body as a negative valence, such as fluoride anion (F − ) [3]. The deficiency or excess intake of fluorine is closely related to various diseases, such as tooth decay, osteoporosis, dental fluorosis, and skeletal fluorosis. Further research has shown that high fluoride concentrations in food may cause serious neurotoxicity [4][5][6]. Thus, it is of great importance to quantitatively detect fluoride anion.
Many methods have been utilized for F − detection, including mass spectrometry, 19 F nuclear magnetic resonance, atomic absorption spectroscopy, high performance liquid chromatography, sensor arrays, and so on [7][8][9]. Compared with the above methods, optical detection, especially luminescence detection, possesses unique advantages due to its high sensitivity, excellent selectivity, and low cost, making it suited to on-site analysis [10,11]. In addition, searching for a suitable probe is the key to F − detection. Phosphorescent transitional metal complexes, especially iridium (III) complex, have various unique advantages, such as tunable emission color, high quantum efficiency, rich excited states, and good photostability. Furthermore, the Ir(III) complex possesses a long emission lifetime from hundreds of nanoseconds to microseconds, which can eliminate the background fluorescent signal with short lifetime using a time-resolved photoluminescence technique, thereby enhancing the signal-to-noise ratio in detection [12][13][14][15][16][17]. F − , as a strong  Lewis base, is the smallest anion with high charge density and strong affinity to silicon atoms. In view of this, our group has reported a series of F − probes base on Ir(III) complexes using the tert-butyldiphenylsilyl moiety as the specific reaction site for F − [4,18,19]. However, these probes are all single use and cannot be reused. As we know, F − probes based on active hydrogen can be reused after the addition of a trace proton. In 2016 we developed a low-level water probe based on Ir(III) complex including formamide moiety. However, the influence of F − on the photophysical properties of the probe was not studied in depth [20].
Herein, a novel and sensitive F − probe based on Ir(III) complex containing formamide unit was designed and synthesized rationally. To increase the stability of the complex, chlorinated 2-phenyllepidine substituted with trifluoromethyl instead of fluorine was selected as the main ligand, and 5-formamide phenanthroline was chosen as the ancillary ligand [21][22][23]. The probe showed outstanding performance for F − detection in organic solvents. Importantly, the change of configuration for the excited states before and after the addition of F − was investigated systematically. Simultaneously, the emission lifetime of the probe changed greatly after the addition of F − , which enabled the potential application for F − detection using a time-resolved photoluminescence technique, thereby improving the signal-to-noise ratio. Moreover, density functional theory (DFT) and time-dependent density functional theory (TDDFT) calculations were carried out to fully understand the relationship between the structure and photophysical properties. To the best of our knowledge, this is the first report of a quantitative probe for F − based on a formamide group.
Instrumentation: Nuclear magnetic resonance (NMR) spectra and mass spectra were obtained by a Bruker AMX-500 NMR instrument and Bruker autoflex matrix-assisted laser desorption/ionization time of flight mass spectrometer (MALDI-TOF MS). The UV-vis absorption spectrum was recorded on a UV3600 UV-Vis spectrophotometer (Shimadzu, Japan). The emission spectra and the emission lifetime were performed on a FluoroMax-4 fluorescence spectrophotometer (Horiba, Japan). The absolute quantum efficiency (Φ) of solutions was measured by an integrating sphere. The cyclic voltammetry measurements were accomplished in CH3CN (5.0 × 10 −4 M) with a three-electrode system consisting of platinum working and counter electrodes and an Ag/AgNO3 (0.01 M in CH3CN) reference electrode at N2 atmosphere. Tetra-n-butylammonium hexafluorophosphate (0.1 M in CH3CN) was selected as the electrolyte. The scan rate was 100 mV/s and reported with the reference to the ferrocene/ferrocenium (Fc/Fc + ) redox couple.
Calculation method: The ground-state geometrical configuration of 4 was optimized by density functional theory (DFT) with B3LYP functional. Based on the optimized ground state molecular structure, the time-dependent DFT (TDDFT) approach associated with the polarized continuum model (PCM) in dichloromethane media was carried out to obtain the vertical excitation energies of triplet states (Tn). The calculation was performed using the Gaussian 16 B.01 suite of programs [24]. The SDD basis set was used to treat the iridium atom, whereas the 6-31 G* basis set was used to treat all other atoms. The contours of the highest occupied molecular orbital (HOMO) and lowest unoccupied molecular orbital (LUMO) were plotted by Multiwfn 3.8 program [25].

Synthesis
The synthetic routes of Ir(III) complex are shown in Figure 1. First, the main ligand was synthesized by Suzuki cross-coupling reaction using palladium catalyst. The auxiliary ligand was obtained by the formylation of 5-amido-1,10-phenanthroline using formic acid as the reaction reagent and solvent. μ-dichloro bridged Ir(III) dimer complex and the end product Ir(III) complex were then fabricated by classic methods reported in the literature [26,27]. The structures of the compounds were confirmed through 1 H NMR (500 MHz), 13 C NMR (126 MHz), 31 P NMR (202 MHz) spectra and mass spectra. The photophysical properties of the complex were characterized via UV/vis absorption spectrometry, and steady-state and transient phosphorescence spectrometry. 3 mmol) were added into a 150 mL flask. The mixture system was evacuated under vacuum and flushed with dry nitrogen three times. Degassed toluene (45 mL) was then injected. The system was heated to 85 °C and stirred for 18 h, and then cooled to room temperature. Next, 50 mL dichloromethane was added into the flask, the system was filtered, and the filtrate was collected; the solvent was then removed by rotary evaporator. The crude product was purified by flash chromatography (silica gel, ethyl acetate/petroleum ether, 75/1 to 60/1, v/v), yielding a yellow solid. 1

Synthesis of auxiliary ligand 2
We added 5-amine-1,10-phenanthrolin (1.0 g, 5.1 mmol) into the solvent formic acid (50 mL), and the mixture was then heated to 100 °C for 7 h. After cooling the system, the residual formic acid was removed by rotary evaporator, and a red-orange solid was then

Synthesis of μ-dichloro bridged Ir(III) dimer complex 3
The μ-dichloro bridged Ir(III) dimer complex 3 was synthesized according to the published literature [27]. IrCl3·3H2O (1.23 g, 3.5 mmol) and ligand 1 (2.25 g, 7.0 mmol) were added into a mixture of 2-ethoxyethanol and deionized water (60 mL, 3:1 v/v). The system was then heated to 110 °C under N2 atmosphere for 15 h. After the system was cooled, the orange solid was obtained by filtering the solution and then washed with deionized water and methanol. The solid was then dried using a vacuum drying oven.

Synthesis of Ir(III) complex 4
μ-dichloro bridged Ir(III) dimer complex 3 (1.0 g, 0.58 mmol), and auxiliary ligand 2 (0.28 g, 1.27 mmol) were added into a mixture of degassed dichloromethane and methanol (60 mL, 1:1 v/v), which was then stirred at room temperature for 5 h under nitrogen atmosphere. The solvent was then removed by rotary evaporator. The crude product was purified by column chromatography using dichloromethane/methanol as eluent. 1

Structural Characterization
As for compound 2, formamide has two isomeric forms, cis and trans. These two isomers can be distinguished by coupling constant in 1 H NMR; the coupling constants between -NH and -CHO for the cis and trans forms are 0-2.2 Hz and 8.0-10.0 Hz, respectively [28,29]. The 1 H NMR spectrum of 2 is shown in Figure S1, the peak at 10.73 ppm in low field was doublet splitting with the coupling constant of 9.95 Hz, which can be ascribed to -NH in trans isomer; meanwhile, the singlet peak at 10.59 ppm can be ascribed to -NH in cis isomer. The integral proportion for the two peaks reflected the molar ratio of the two isomers, which is about 0.45:1.0. However, the 1 H NMR spectrum ( Figure S2) of compound 4 suggested that there were no isomers in the Ir(III) complex, and the singlet peak at 9.44 ppm in low field can be assigned to -NH in the cis form. The attribution of -NH will be beneficial to analyzing the interaction between F − and Ir(III) complex.

Photophysical Properties
The photophysical properties of 4 were studied by UV-Vis absorption spectrometry and steady-state luminescence spectrometry, as shown in Figure 2a. The ultraviolet-visible (UV-Vis) absorption spectrum (1.0 × 10 −5 M, green line) showed an intense peak at 278 nm, which can be ascribed to the ligand-centered (LC) transition, the absorption band at 325-350 nm was attributed to π-π* transitions of the cyclometalating ligands. In addition, the weak absorption peak between 375 to 450 nm can be assigned to spin-allowed singlet metal-to-ligand charge transfer ( 1 MLCT) and ligand-to-ligand charge transfer ( 1 LLCT) transitions [30]. The emission spectrum (Figure 2a, red line) of 4 in solid state exhibited a maximum peak at 577 nm and a shoulder peak at 550 nm, and a large full width at half maximum of 136 nm, because of the difference of aggregate state compared with the solution state. The lifetime ( Figure S4) and absolute quantum efficiency were 123 ns and 13.76%, respectively.
Complex 4 in dichloromethane solution exhibited a bright yellow emission visible by naked eye when excited at 365 nm, as shown in Figure 2b (inset). The emission spectra of 4 in dichloromethane solution at different concentrations under ambient conditions were investigated, as shown in Figure 2b, and they all possessed a maximum phosphorescent peak at 535 nm and a shoulder peak at 569 nm, respectively. The similar profile of the spectra indicated that there existed extremely weak or no intermolecular interaction between the molecules in dilute solution. The emission lifetime and absolute luminescent efficiency in degassed dichloromethane solution at room temperature are 2.1 μs ( Figure  S5) and 15.36%, indicative of the phosphorescent nature of emission. The phosphorescent behaviors of 4 in various solutions (1,4-dioxane, 2-ethoxyethanol, methanol, acetonitrile, tetrahydrofuran, N,N-dimethyl formamide, dimethylsulfoxide, and ethyl acetate) were then studied, as shown in Figure 2c; the similar peaks at 535 and 569 nm indicated that solvents with different polarities had no obvious influence on the emission spectra, and phosphorescent emission may have originated from the LC excited state. Next, the phosphorescence spectrum at 77 K for 4 was measured in 2-methyltetrahydrofuran (2-MeTHF), and compared with the emission spectra at room temperature, the low temperature spectrum exhibited slight blue-shift, peaking at 530, 567 and 617 nm, respectively, along with fine structures of vibronic bands (Figure 2d). The triplet energy of the triplet state (T1) of 4 was calculated from the emission spectra at 77 K according to the highest energy-vibronic band, and it possessed a modest T1 energy at 2.35 eV. The photophysical data are summarized in Table 1. The electrochemical behaviors of complex 4 in the N2-saturated acetonitrile solution at concentrations of 1.0 × 10 −5 M were studied using cyclic voltammetry ( Figure S6). The cyclic voltammetry curve exhibited an irreversible oxidation wave at the potential of 1.75 V, which may be attributed to the oxidation of the iridium center [13].
Next, chemical stability and photostability of complex 4 were carried out by adding different anions, including Cl − , Br − , NO3 − , CH3COO − , HCO3 − , CO3 2− , SO4 2− , to the dichloromethane solution (1.0 × 10 −5 M) and illuminating at 365 nm (15 mW cm −2 ), respectively, as shown in Figures 3a and S9. The detailed experimental steps are presented in the Experimental Section in Supporting Information. With the exception of CH3COO − , the phosphorescent intensity at 535 nm exhibited little change, which indicated that 4 possessed excellent chemical stability and photostability. Subsequently, F − was added into the solution with different anions and the intensity dropped rapidly, suggesting the selectivity for F − in complex systems. However, the phosphorescent intensity of the samples containing CH3COO − dropped about 50 percent. Although the dissociation constant of HCO3 − (4.7 × 10 −11 ) is far less than that of HF (3.53 × 10 −4 ) and CH3COOH (1.8 × 10 −5 ) in aqueous solution, the factors of solubility and basicity of the salts in CH2Cl2 solution should be considered simultaneously. In addition, the MS spectra of complex 4 containing CO3 2− and CH3COO − are presented in Figures S7 and S8, respectively. The molecular weight exhibited no change, peaking at 1056 m/z, the same as Figure S3, which suggested that the addition of CO3 2− , CH3COO − showed almost no influence on the structure of the complex. Figure S9 was completed by recording the emission intensity at 535 nm, and the very little change of intensity revealed that complex 4 exhibited good photostability.

Fluoride Anion Detection
The phosphorescent response behaviors of complex 4 to F − in dichloromethane solution under ambient conditions were investigated in detail by titrations, as shown in Figures 3b,c, and S10. The detailed experimental steps are presented in the Experimental Section in Supporting Information. The results suggested that the intensity of the phosphorescence at 535 nm declined gradually with the addition of fluoride anion; meanwhile, the emission lifetime also decreased gradually. The quenching efficiency η (η = (I0 − I)/I0, I0, and I were the phosphorescent intensity before and after the titration of F − , respectively) can represent the responsiveness of the complex for F − . When F − reached 100 μM, the intensity dropped by nearly 98 percent compared with that of the absence of F, as shown in Figure 3d. There is a proximate linear relationship between the concentration of F − and phosphorescent intensity ratio (I/I0). The detection limit (LOD = 3σ/k) was calculated to be (3.9 × 10 −2 μM), which revealed that complex 4 was a potential candidate for the detection of low content of fluorine anion organic phases.

Mechanism Analysis
To understand the mechanism of the quenching behaviors in depth, NMR titration and theoretical calculations were carried out, as shown in Figure S11. As we know, fluoride has a strong binding capacity with reactive protons, and the addition of F − to the iridium can change the configuration of the excited states, thus leading to a quenching effect. The 1 H NMR spectra showed that the peak at 9.44 ppm assigned to -NH shifted to low field and dwindled gradually along with the addition of F − , along with splitting into a doublet peak, the coupling constants are 8.05 Hz (mid spectrum) and 8.35 Hz (bottom spectrum). The different coupling constants may be due to the different distance between the hydrogen atom and fluorine atom. Thus, we speculate that when adding F − into the mixture system, H-bonding between the fluoride and the amide proton was formed (Figure 4).
The geometrical configuration of 4 optimized via B3LYP is shown in Figure 5, and the results suggested that 4 adopted a slightly twisting hexa-coordinate octahedron structure, leading to no or weak intermolecular interactions, which was consistent with the similar profile of emission spectra at different concentrations. The frontier molecular orbital (FMO) was calculated by TDDFT, as shown in Table 2. The results revealed that the HOMO primarily distributed on the iridium center and π orbital of quinolone unit of the main ligand, simultaneously, the LUMO was primarily distributed on the phenanthroline. Particularly, LUMO + 2 and HOMO-1 were principally located on the main ligand, without the auxiliary ligand. HOMO-1-LUMO + 2 and HOMO-LUMO transitions took up a large proportion, and the excited states of 4 were attributed to the mixture of MLCT transitions and LLCT transitions. We then simulated the molecular configuration of complex 4 with fluoride, as shown in Figure S12; because of the strong affinity of the fluorine and hydrogen, the distance between fluorine and hydrogen is 0.9735 Å, far shorter than that between nitrogen and hydrogen (1.6722 Å). Thus, the unit of F-H has little effect on the physical properties of the complex. Next, the calculation of FMO for complex 4 + F − was carried out based on the removal of hydrogen by fluorine. The results showed that, provided -NH was snatched by the fluoride anion, FMO would present a significant change. HOMO, LUMO + 2 and LUMO + 3 were primarily distributed on the auxiliary ligand, and LUMO was mainly located on the iridium center and main ligand. The proportion of the HOMO-LUMO transition is much lower than that of HOMO-LUMO + 2 and HOMO-LUMO + 3 transitions, and the excited states were assigned to the LLCT transition, leading to a red-shift of the spectrum and efficiency drop and even luminescence quenching, which demonstrated well the quenching effect when adding F − into complex 4.

Conclusions
In summary, a novel phosphorescent Ir(III) complex probe based on formamide for F − detection with low LOD was achieved successfully. The probe exhibited excellent recognition capability for quantitative analysis of fluorine anion in complex systems. Moreover, the working mechanism was calculated by TDDFT in detail, after the addition of F − , the excited states of the complex decay to LLCT transition, resulting in the quenching effect. In addition, the long emission lifetime of the complex allowed the probe to be a promising candidate with high signal to noise ratio via time-resolved technique. Next, we will focus on the development of a water-soluble near-infrared probe for F − detection and imaging in vivo.

Supplementary Materials:
The following are available online at www.mdpi.com/article/10.3390/cryst11101190/s1, Figure S1: The 1 H spectrum of auxiliary ligand 2. Figure S2: The 1 H spectrum of complex 4. Figure S3: MALDI-TOF spectrum of complex 4. Figure S4: The decay curve of phosphorescent lifetime for complex 4 in solid state. Figure S5: The decay curve of phosphorescent lifetime for complex 4 in CH2Cl2. Figure S6: The cyclic voltammograms of 4 under a scan rate of 100 mV/s in CH3CN. Figure S7: MALDI-TOF spectrum of complex 4 containing CO3 2− . Figure S8: MALDI-TOF spectrum of complex 4 containing HCO3 − . Figure S9: The photostability of complex 4 excited at 365 nm. Figure S10: The emission spectra for the response of complex 4 to fluoride anion in dichloromethane. Figure S11: The 1 H NMR titration for complex 4. Figure S12: The molecular configuration of complex 4 with fluorinion. Figure S13: The 1 H spectrum of main ligand. Figure S14: The 13 C spectrum of complex 4. Figure S15:

Data Availability Statement:
The data presented in this study are available upon request from the the first author or the corresponding authors.