{'fraction_non_alphanumeric': 0.03157190635451505, 'fraction_numerical': 0.020133779264214047, 'mean_word_length': 4.853954581049335, 'pattern_counts': {'":': 0, '<': 0, '<?xml version=': 0, '>': 0, 'https://': 0, 'lorem ipsum': 0, 'www.': 0, 'xml': 0}, 'pii_count': 0, 'substrings_counts': 0, 'word_list_counts': {'cursed_substrings.json': 0, 'profanity_word_list.json': 0, 'sexual_word_list.json': 0, 'zh_pornsignals.json': 0}}
Aggregation‐induced Emission Properties of Triphenylamine Chalcone Compounds

Two triphenylamine chalcone derivatives 1 and 2 were synthesized through the Vilsmeier-Haack reaction and Claisen-Schmidt condensation reaction. Through ultraviolet absorption spectroscopy and fluorescence emission spectroscopy experiments, it was confirmed that these two compounds exhibited good aggregation-induced emission (AIE) behavior in ethanol/water mixtures. The solvent effect test showed with the increase of the orientation polarizability of the solvent, the Stokes shift in the solvent of compound 1 and compound 2 shows a linear change trend. Through solid state fluorescence test and universal density function theory (DFT), the existence of π-π stacking interaction in the solid state of the compound has been studied, resulting in weak fluorescence emission. pH has no effect on the fluorescence intensity of the aggregate state of excited state intramolecular proton transfer (ESIPT) molecules in an acidic environment, but greatly weakens its fluorescence intensity in an alkaline environment. Cyclic voltammetry (CV) test shows that compound 1 was more prone to oxidation reaction than compound 2. The results of thermal stability test show that the thermal stability of compound 1 was better than that of compound 2, indicating that triphenylamine chalcone derivatives can improve the thermal stability of compounds by increasing the number of branches.


Introduction
In recent years, AIE materials have been widely used in chemical sensing, biological imaging, organic light-emitting diodes (OLED) [1][2][3][4][5][6][7], etc.Based on a large number of experiments and theoretical studies, researchers have concluded that restriction of intramolecular rotations (RIR), excited state intramolecular proton transfer (ESIPT), etc. [8] inhibits the π-π accumulation in the molecule to achieve the AIE effect. Due to the widespread application of molecules based on the ESIPT mechanism of action [9][10][11], the behavior of AIE based on the ESIPT mechanism has gradually gained attention in the field of natural sciences.
Generally, a molecule with ESIPT characteristics was composed of a proton donor (such as -OH, -NH 2 ) and a proton acceptor (such as -N = C, C = O) [12]. Because of its π conjugated framework, the fluorescence emission of 2-hydroxychalcone derivatives was often affected by aggregation-caused quenching (ACQ). Triphenylamine was a molecule with a central N atom and three benzene rings connected around it to form a starshaped structure. Because of its special structure, it has larger steric hindrance and higher hole transport rate [13]. In addition, the structure of triphenylamine was easy to modified. Although the fluorescence emission efficiency of triphenylamine was not high, the modified triphenylamine derivatives were used in fluorescent probes [14][15][16], organic electroluminescent materials and organic solar cell materials [17,18] and other aspects have been widely used.

Materials and Methods
The raw materials required for the experiment such as trip hen ylam i ne, p hos pho rusv ox ych l orid e, N,Ndimethylformamide, 2-hydroxyacetophenone, 2-hydroxy-1naphthophenone, sodium hydroxide, ethanol, and chloroform. 1 H and 13 C-NMR spectra were recorded on a Avance 400 spectrometer in CDCl 3 with.
TMS as an internal standard. Mass spectrum was recorded on the Thermo Q-Exactive mass spectrometer. The melting point was measured on the XRC-1µ melting point instrument. The ultraviolet absorption was recorded on Cary50. The fluorescence test was recorded on the FE06CN-IF171(ZB) LD/LM luminescence spectrophotometer. Thermogravimetric analysis (TGA) was performed on Mettler STAR e System thermal analyser under nitrogen flushing at a heating rate of 10 min − 1 with sample weight of 3-4 mg. Cyclic voltammetry measurements were performed on a CHI660E electrochemical workstation at room temperature with three electrodes cell system in a solution of Bu 4 NPF 6 (0.1 M) in chloroform at a scanning rate of 100 mVs − 1 . Glassy carbon electrode acts as working electrode; platinum electrode used as a counter electrode and SCE (saturated calomel electrode) electrode as a reference electrode. The scanning electron microscope images of compound 1 and compound 2 in different ratios of ethanol and water as solvents were tested on Hitachi Regulus 8100 high-resolution cold field emission electron microscope.

Solvent Effect
In order to investigate the influence of different solvents on the ESIPT behavior of compound 1 and compound 2, the UVvisible absorption spectrum and fluorescence emission spectrum behavior of compound 1 and compound 2 in acetone, ethanol, dichloromethane, tetrahydrofuran, toluene, and chloroform were studied. It can be seen from Fig. 2(a) and 2(b) that the absorption wavelength maximum was shorter in the protic solvent ethanol. The absorption wavelength was longer in aprotic solvents. As was shown in Fig. 2(c), the maximum emission peak of fluorescence spectrum gradually shifted to long wavelength in toluene, chloroform, tetrahydrofuran, dichloromethane and acetone. In the Fig. 2(d), this change is not observed, which may be caused by different substituents on the triphenylamine group. To understand the effect of solvent polarity on the optical properties of substances, the relationship between the oriented polarizability (Δf) and the corresponding Stokes (Δv Fig. 3 Lippert mataga plot of compounds 1 and 2 in different solvents cm − 1 ) of toluene, chloroform, dichloromethane, tetrahydrofuran and ethanol solvents was studied [36]. From Fig. 3 and Table S1, it can be seen that with the increase of the orientation polarizability of the solvent, the Stokes shift in the solvent of compound 1 and compound 2 shows a linear change trend [37].
Where, the v abs and v flu are the wavelengths corresponding to the peak of the absorption and emission spectra, respectively. the h was the Planck constant, the c was the speed of light, and the a was the cavity radius. Δµ was the difference between the excited state dipole moment and the ground state dipole moment. ε and η were the dielectric constant and the refractive index of the solvent, respectively.

AIE Behavior
Chalcone compounds were soluble in ethanol solution and insoluble in water. In order to study whether compound 1 and compound 2 have aggregation-induced emission behavior, the UV absorption spectra and fluorescence emission spectra of chalcone compounds 1 and 2 in different proportions of ethanol/water mixtures were studied. As shown in Fig. 4(a), with the increase of water volume fractions in ethanol/ water mixtures, compounds 1 and 2 show different degrees of decrease of absorption intensity and horizontal trailing phenomenon. The reason for the decrease of absorption intensity may be the light scattering of suspension in aggregate state [38].
Meanwhile, the change of fluorescence intensity caused by the volume content of different water in ethanol/water mixtures was determined at an excitation wavelength of 450nm. As shown in Fig. 4(b), when the volume fraction of water in the ethanol/ water mixtures of Compound 1 was less than 40 %, the fluorescence intensity was not change substantially. When the volume fraction of water was higher than 40 %, the fluorescence intensity gradually increases. As shown in Fig. 5, Compound 2 exhibited similar behavior to compound 1 in ethanol/water mixtures. When the volume fractions of water in ethanol/water mixtures was less than 50 %, the fluorescence intensity was very weak. It may be due to the free rotation of the sigma bond of the benzene ring in the molecule and the distortion of the charge transfer in the molecule, which leads to the destruction of the proton transfer in the excited state [39]. When the volume fractions of water in the ethanol/water mixtures was higher than 50 %, the gradual increase in fluorescence intensity may be due to the carbonyl structure (-C = O) on the chalcone group and the hydroxyl structure (-OH) on the benzene ring undergo an excited state intramolecular proton transfer to form a stable hydrogen bond in aggregate state, which inhibits free rotation within the molecule and enhances fluorescence [40,41]. Meanwhile, the fluorescence emission behavior of compound 1 and compound 2 in the solid state was also studied. As was shown in Fig. 6, the emission peaks of Compound 1 and Compound 2 in the solid state were 610 nm and 620 nm, respectively. While compounds 1 and 2 had emission peaks of 550 nm and 541 nm in ethanol solvent, respectively. The fluorescence maximum emission peak in the solid state has a red shift of 60nm and 79nm, respectively, relative to the fluorescence maximum emission peak in ethanol solvent. It was caused by the π-π stacking between molecules in the solid state. As was shown in Fig. 7, Under 365nm UV light, the solid state emission of compound 1 was weaker than (E)-3-(4-(diphenylamino)phenyl)-1-(2-hydroxyphenyl)prop-2-en-1-one reported in literature [42]. This phenomenon was Fig. 7 Photographs of compound1 and compound 2 under daylight and 365nm UV irradiation Fig. 8 The fluorescence intensity of compound 1 and compound 2 in ethanol/water mixtures (f w =90 %) changes with pH due to the increase of π-conjugated system, which causes the increase of π-π stacking.

Research on pH Responsiveness
In order to evaluate the effect of pH on the aggregation state of ESIPT molecules, the pH responsiveness of it was studied in an ethanol/water mixtures (f w =90 %). As was shown in Fig. 8, when the pH was less than 7, compound 1 and compound 2 were maintained in a stable range, without causing much change in fluorescence intensity. It was because the chalcone phenol hydroxyl group was acidic as an acidic proton donor and was insensitive to pH under acidic conditions.When the pH was greater than 7, the fluorescence intensity of compounds 1 and 2 decreased significantly with the increase of pH. It was because the increase of OH − in the solution deprives the hydrogen protons on the phenolic hydroxyl group, making it unable to form a stable hydrogen bond, resulting in low fluorescence intensity in the aggregate state.

Theoretical Calculation
In order to have a comprehensive understanding of compound 1 and compound 2 at the molecular level, Gaussian09 software was used to optimize the structure of compounds 1 and 2 with B3LYP/6-31G(d) as the method and basis set. As was shown in Fig. 9, the electron cloud of the highest occupied molecular orbital (HOMO) of compound 1 and compound 2 was mainly distributed in the triphenylamine part, and the electron cloud of the lowest unoccupied molecular orbital (LUMO) was mainly distributed in the corresponding chalcone part. The calculated energy values of the HOMO and LUMO of compound 1 were − 5.11 eV and − 1.95 eV, respectively. The energy values of HOMO and LUMO of compound 2 were − 5.20 eV and − 2.21 eV, respectively. The HOMO-LUMO energy gap (ΔEg) of compound 1 and compound 2 were 3.16 eV and 2.99 eV, respectively. It can be seen from the figure that the optimized spatial configuration of the molecule tends to be planar and fails to effectively prevent π-π stacking, so the fluorescence emission in the solid state was weak.

Electrochemical and Optical Properties
The electrochemical behavior of compound 1 and compound 2 was carried out with CHCl 3 as the solvent and tetrabutylammonium hexafluorophosphate as the supporting electrolyte, the electrochemical window is from − 1.8 V to 1.8 V, and the scanning speed was 100mV/s [43]. As was shown in Fig. 10(a), compound 1 and compound 2 were dissolved in chloroform solution, the abscissa of the intersection of the initial line of the absorption wavelength and the long-range absorption spectrum measured by the UV-visible spectrometer was the initial incident wavelength λ onset . Then calculated the energy value of the optical band gap by the formula E opt =1240/λ onset . The energy values(E opt ) of the optical band gap of compound 1 and compound 2 were 2.24 eV and 2.35 eV, respectively, which may be caused by the different degree of molecular conjugation [44] ( Table 1). As was shown in Fig. 10(b), the formation of the oxidation peak may be due to the electron donation of triphenylamine. The initial oxidation potentials of compound 1 and compound 2 were 1.06 V and 1.08 V, respectively. The initial oxidation potential of compound 1 was slightly lower than that of compound 2, indicating that compound 1 was easier to oxidize than compound 2. Calculated by the formula E HOMO =-e(E onset ox +4.4)(eV), the potentials of the highest occupied molecular orbitals of compound 1 and compound 2 were − 5.46 eV and − 5.48 eV, respectively. The potential of the lowest unoccupied molecular orbital of compound and compound 2 was obtained according to the formula E LUMO =E HOMO + E opt (eV).

Thermal Stability
In order to study the thermal stability of compound 1 and compound 2, the two compounds were tested by thermogravimetric analysis. The 10 % loss of compound mass was defined as the initial value of the thermal decomposition temperature. As was shown in the Fig. 11, the initial thermal decomposition temperature (T d ) of compound 1 and compound 2 were 410 and 340 , respectively. The initial thermal decomposition temperature of compound 1 was higher than that of compound 2, indicating that the derivatives of triphenylamine chalcone can be increased by the number of branches to improve thermal stability. These test results showed that compound 1 and compound 2 have good thermal stability.

Conclusions
Two triphenylamine chalcone derivatives were synthesized in this chapter, which showed good AIE behavior in ethanol/ water mixtures, respectively. The Stokes shift of the solvent shows a linear trend with the increase of the solvent orientation polarizability. Different pH environments will affect the fluorescence intensity of the compound in the aggregate state. Both the solid state fluorescence test and the generalized density function theory show that the two compounds have π-π stacking effect in solid state, which makes the fluorescence emission weak in solid state. Compound 1 is more prone to oxidation than compound 2, and the thermal stability was better than compound 2.
Author Contributions Ying-Peng Zhang, contributed to the conception of the study; Qi Teng, performed the experiment and wrote the manuscript; Yun-Shang Yang, contributed significantly to analysis and manuscript preparation; Jing-Qi Cao, performed the data analyses; Ji-Jun Xue, helped perform the analysis with constructive discussions.
Data Availability The 1 H NMR, 13 C NMR HR-ESI-Ms of the 1 and 2 are detailed in the Supporting information. These materials are available free of charge via the Internet.
Code Availability Not applicable.

Declarations
Conflict of Interest The authors declare that they have no conflict of interest.