Synthesis, Characterization, and Crystal Structures of Imides Condensed with p-Phenylamino(Phenyl) Amine and Fluorescence Property

A series of aromatic diimide and monoimide compounds condensed with p-phenylamino(phenyl)amine were synthesized and confirmed by Proton Nuclear Magnetic Resonance (1H NMR), Carbon-13 Nuclear Magnetic Resonance (13C NMR), Fourier Transform Infrared Spectroscopy (FT-IR), Elemental Analysis (EA), and High Resolution Mass Spectroscopy (HRMS). Meanwhile, single crystal X-ray diffraction showed the existence of intermolecular N···O hydrogen bonds, which affected the thermal stabilities of corresponding compounds by the support of Thermalgravimetric Analysis (TGA) curves. The steady-state UV-vis absorption peaks of synthetic compounds 1–6 appeared in the range of 220–380 nm. Fluorescence emission spectra showed peaks in the range of 290–420 nm. Meanwhile, deep-blue or violet-blue emissions for 2, 4, and 5 in THF under excitations of 254 nm and 365 nm, respectively, were observed at room temperature in air. Furthermore, Differential pulse voltammetry (DPV) and cyclic voltammogram CV were conducted within −1.5–+1.5 V to show quasi-reversible behavior for conjugated compounds and irreversible behavior for less conjugated ones.

To investigate the binding process for small molecules to DNA motivated by discovering drugs, fluorescence property on both naphthalimide-based Schiff base derivatives, reported by Uddin [29], and 1,4,5,8-naphthalene diimide-spermine conjugate (NDIs), by Wang [30], was exploited. The latter case also revealed that hydrogen bonding interactions play an important role in fluorescence quenching. A

Materials and Methods
All commercially available starting materials, reagents, and solvents were purchased and used as supplied. p-Phenylamino(phenyl)amine, Naphthalene-1,4,5,8-tetracarboxylic dianhydride, Pyromellitic dianhydride, and 4,4 -Biphthalic anhydride were purchased from TCI (Shanghai, China). Bicyclo[2.2.2]oct-7-ene-2,3,5,6-tetracarboxylic dianhydride, 1,8-Naphthalene anhydride, and 3,3 ,4,4 -Benzophenonetetracarboxylic dianhydride were purchased from Alfa Aesar. Acetic acid was purchased from Greagent. Infrared spectra (KBr pellets) were measured on a Bruker MPA spectrometer (Billerica, MA, USA) between 400 and 4000 cm −1 . Thermogravimetric analysis (TGA) was measured under a nitrogen stream, at a flow rate of 50 cm 3 /min with a heating rate of 10 • C/min on Mettler TGA2 Thermogravimetric Analyzer (Zurich, Switzerland). 1 H NMR and 13 C NMR spectra were recorded on either a Bruker ADVANCE AV-300 or ADVANCE-500 spectrometer (Billerica, MA, USA). Elemental analysis data were obtained using an instrument of Vario EL cube Elementar (Hamburg, Germany). Fluorescence spectra were obtained using a Hitachi F-4600 fluorescence spectrophotometer (Tokyo, Japan). Photoluminescent quantum yields (PLQYs) were obtained using a Fluoromax-4C-L TCSPC spectrophotometer (Horiba, Kyoto, Japan) at room temperature in air. UV-vis absorption spectra were obtained using a Shimadzu UV-1750 spectrometer (Kyoto, Japan). High resolution mass spectra (HRMS) were obtained using an Agilent 1260-6230 sepectrometer (Santa Clara, CA, USA). Differential pulse voltammetry (DPV) and cyclic voltammogram (CV) spectra were conducted with a three-electrode system on a Pine WaveDriver200 electrochemical workstation (Phoenix, AZ, USA), with a scanning rate of 0.1 Vs −1 in 0.1 M TBAPF 6 DMF solutions. Pt wire and Pt disk were used as a counter electrode and a working electrode, respectively. Ag/AgCl was used as a reference electrode. Single crystal X-ray diffraction data were collected on a Bruker APEX-II diffractometer (Billerica, MA, USA) at 296 (2) K equipped with a CCD detector. The X-ray beam was generated using graphite monochromated Mo Kα radiation (λ = 0.71073 Å). All single crystal structures were solved by direct method with structure refinements being performed by the SHELXTL program [40]. Hydrogen atoms were introduced in calculated positions and refined according to the riding model. Figures related to crystal structures were generated by Mercury 3.10.2. The synthesis of compound 1 followed a modified procedure [41].

Results and Discussion
Diimide compounds 1-5 and monoimide compound 6 were synthesized by the condensation of p-phenylamino(phenyl)amine with dianhydrides/anhydride. 1 H NMR and 13 C NMR spectra along with HRMS spectra either by APCI or ESI confirmed target compounds (Figures S1-S18). For example, the NH proton positions in 1-6 were identified as singlet peaks in DMSO-d 6 between 8.32 and 8.40 ppm on a 500 MHz nuclear magnetic resonance spectrometer. Meanwhile, experimental values of mass-to-charge ratio (m/z, [M+H] + ) for each compound were obtained within experimental errors. In addition, single crystal structures of compounds 1, 3, and 5 were also obtained. Structural analyses are discussed in Section 3.1.

Description of Crystal Structures
Crystallographic data for 1, 3, and 5 are summarized in Table 1 and selected bond lengths and torsion angles are in Table 2. Compound 1 crystallized in monoclinic space group P2 1 /n with solvent DMF molecules embedded in the lattice. As shown in Figures 1 and 2, the crystal structure showed one rigid conjugated core and two p-phenylamino(phenyl) units interacting with neighbor molecules through intermolecular N···O hydrogen bonds. No interactions were observed for solvent DMF molecules in the solid state. Selected C-N bond lengths in 1 ( Figure 1 and Table 2) showed a longer distance for C10-N2 (1.444(3) Å) than both C1-N1 (1.385 (4) Å) and C7-N1 (1.389 (3) Å) due to twisted Ph-a/Imide ring angles and electron withdrawing imide groups. Meanwhile, the average bond length of carbon-carbon in Ph-t (C-C(Ph-t) av )-Ph-t represents the terminal phenyl unit relative to core-was 1.358(9) Å shorter than the average bond length of carbon-carbon that was 1.378 (3) Å in Ph-a (C-C(Ph-a) av ). Ph-a represents the adjacent phenyl unit was relative to core. The average carbon-carbon bond length in core, C-C(core) av , was 1.260(2) Å relatively shorter than either C-C(Ph-t) av or C-C(Ph-a) av .     The space filling diagram of 1 showed twisted connections between the imide rings and p-phenylamino(phenyl) units. The torsion angle of C9-C10-N2-C17 between the Ph-a and imide ring, ∠Ph-a/Imide ring, was 115.0(3)°. A dihedral angle of 64.419(0.099)° between ∠Ph-a/Imide ring was also obtained. In contrast, the torsion angle of C8-C7-N1-C1, ∠Ph-t/Ph-a, was 177.5(3)°. Together with a dihedral angle of 18.815(0.261)° between ∠Ph-t/Ph-a, these values indicate the co-planarity for Ph-t and Ph-a ( Figure 2 and Table 2). Compound 1 was linked together through one type of intermolecular N···O hydrogen bond (3.052(4) Å, ∠N1H1O2 = 155.1°) to form a large pore size 2D channel ( Figure 3). either slightly decreased to 104.0(5)° or significantly increased to 149.7(4)° due to the less conjugated core in a free rotation mode. In other words, the increased dihedral angles of ∠Ph-t/Ph-a, with 53.576(0.148)° and 41.781(0.150)° compared to 18.815(0.261)° in 1, were observed for 3. Dihedral angles of ∠Ph-a/Imide ring were either slightly decreased to 31.697(0.168)° or significantly increased to 69.870(0.174)°. Besides, compound 3 was linked together through two types of intermolecular N···O hydrogen bonds (2.980(5) Å, ∠N4H4AO1 = 145.3° and 3.054(4) Å, ∠N1H1O4 = 162.2°) to form a small pore size 1D chain (Figure 4). Compound 5 crystallized in the monoclinic space group P21/c. As shown in Figure 1, the structure contained a non-conjugated core and two p-phenylamino(phenyl) units without intermolecular N···O Table 2). The average bond lengths of C-C(Ph-t)av (1.378(3) and 1.381(6) Å) and C-C(Ph-a)av (1.376 (2) Å and 1.380 (9) Å) in 5 were comparable to the corresponding average carbon-carbon bond lengths in 1 and 3.
The space filling diagram of 5 showed twisted connections between the non-conjugated core and p-phenylamino(phenyl) units. The torsion angles of ∠Ph-t/Ph-a with −144.71 (17) Table 2). On the contrary, the torsion angles and dihedral angles of ∠Ph-a/Imide ring were almost equally changed by 10° either clockwise or anticlockwise. The highly bent non-conjugated core was likely to block the approach of neighbor molecules, which prevented the existence of intermolecular N···O hydrogen bonding interactions in 5. Table 2. Selected bond lengths (Å) and torsion angles (°) for 1, 3, and 5. The space filling diagram of 1 showed twisted connections between the imide rings and p-phenylamino(phenyl) units. The torsion angle of C9-C10-N2-C17 between the Ph-a and imide ring, ∠Ph-a/Imide ring, was 115.0(3) • . A dihedral angle of 64.419(0.099) • between ∠Ph-a/Imide ring was also obtained. In contrast, the torsion angle of C8-C7-N1-C1, ∠Ph-t/Ph-a, was 177.5(3) • . Together with a dihedral angle of 18.815(0.261) • between ∠Ph-t/Ph-a, these values indicate the co-planarity for Ph-t and Ph-a ( Figure 2 and Table 2). Compound 1 was linked together through one type of intermolecular N···O hydrogen bond (3.052(4) Å, ∠N1H1O2 = 155.1 • ) to form a large pore size 2D channel ( Figure 3).
Compound 3 crystallized in the triclinic space group P-1. As shown in Figures 1 and 2, the crystal structure showed one twisted core and two p-phenylamino(phenyl) units interacting with neighbor molecules through intermolecular N···O hydrogen bonds. Selected C-N bond lengths in 3 ( Figure 1 and Table 2 The space filling diagram of 3 showed a highly twisted configuration. The dramatically decreased torsion angles of ∠Ph-t/Ph-a, with 152.8(5) • and -140.8(5) • compared to 177.5(3) • in 1, were observed for 3 ( Figure 2 and Table 2). Furthermore, the torsion angles of ∠Ph-a/Imide ring were either slightly decreased to 104.0(5) • or significantly increased to 149.7(4) • due to the less conjugated core in a free rotation mode. In other words, the increased dihedral angles of ∠Ph-t/Ph-a,
The space filling diagram of 5 showed twisted connections between the non-conjugated core and p-phenylamino(phenyl) units. The torsion angles of ∠Ph-t/Ph-a with −144.71 (17) Table 2). On the contrary, the torsion angles and dihedral angles of ∠Ph-a/Imide ring were almost equally changed by 10 • either clockwise or anticlockwise. The highly bent non-conjugated core was likely to block the approach of neighbor molecules, which prevented the existence of intermolecular N···O hydrogen bonding interactions in 5.

Infrared Spectra
IR (infrared) spectra for 1-6 were recorded on a Bruker MPA spectrometer between 400 and 4000 cm −1 (KBr pellets). For compound 1, the observed semicircle stretch modes of para-substituted benzene ring appeared at 1509 and 1409 cm −1 , while the terminal benzene ring stretches appeared at 1496 and 1448 cm −1 and the conjugated carbon-carbon stretch for the NDI core was observed at 1581 cm −1 . The strong characteristic imide stretch modes were identified at 1712 and 1666 cm −1 . The carbon-nitrogen stretch modes were observed at 1328 and 1345 cm −1 [34,42]. Similar assignments for 2−6 were also observed in Figures S19 and S20.

Thermogravimetric Analyses
TGA data for 1-6 showed two stages for weight losses. The first stage experienced rapid minor weight losses below 100 • C that were assigned to lost solvents from corresponding solid samples, evidenced by steady curves after 100 • C. Sudden weight losses started at 395 • C for 5 and 391 • C for 6 during the second stage, that were assigned to broken bonds of the Ph-a and imide ring, which further evaporated to almost nothing. Decomposition temperatures for 1-4 were at higher temperatures of 453 • C for 1, 501 • C for 2, 517 • C for 3, and 463 • C for 4. Interestingly, unknown polymers, possibly high thermal stable polyimides, were formed, as evidenced by the steady curves ( Figure S21). Excellent thermal stabilities under the N 2 stream were also supported by the existence of hydrogen bonds. Based on the solved crystal structures of 1, 3, and 5, a conclusion was drawn that thermal stabilities for 1 and 3 were enhanced by hydrogen bonds, but this was not the case for 5, due to the absence of such interactions. Particularly, the two types of short hydrogen bonds were responsible for the most stable compound 3.

UV-Vis Absorption and Fluorescence Spectra
Steady-state UV-vis absorption and fluorescence emission spectra for 1-6 were recorded in THF, DCM, EtOH, and CH 3 CN, respectively. UV-vis absorption spectra for 1-6 in THF showed that all peaks appeared below 400 nm ( Figure 5). Major absorption peaks appeared at 287 nm for 1, 299 nm for 2, 307 nm for 3, 300 nm for 4, 297 nm for 5, and 291 nm for 6. These peaks were assigned to π-π* transitions from conjugated aromatic units, while the rest of the lower energy peaks in the spectra were assigned to ICT transitions [43]. Similar absorption peaks recorded in DCM, EtOH, and CH 3 CN were also obtained ( Figures S22-S25).
CH3CN with the increasing of polarity. An emission peak at 317 nm in EtOH was sharp and resolved compared to the broad and overlapped peaks in other solvents. A similar trend was also observed for 2, 3, 4 and 6. For 5, the emission profile was quite different from 1, 2, 3, 4, and 6, also matching with polarity effect. The dramatic difference was tentatively attributed to the existence of a non-conjugated core only in 5. Therefore, aromatic conjugation greatly contributed to emission profiles and peak positions. Moreover, the characterized crystal structure for 5 revealed the absence of intermolecular N···O hydrogen bonds, which might be responsible for the decreased chances of forming types of hydrogen-bonded superstructures. To some extent, the existence of hydrogen bonds led to complicated emission profiles, non-radiative decay, energy transfer, and quenched fluorescence For compound 1, an emission peak appeared at 319 nm under the excitation of 265 nm, which matched well with the corresponding excitation peak at 267 nm ( Figure 5). Similarly, an emission peak appeared at 318 nm under the excitation of 273 nm for 6. In contrast, a shoulder peak appeared at 312 nm for 2, except for the major emission peak at 331 nm. Shoulder emission peaks at 311 nm for 3, 335 nm for 4, and 306 nm for 5, along with major emission peaks at 333 nm, 306 nm, and 342 nm, were observed accordingly.
The structured emission spectra for 1-6 indicated a function of a UV filter. The more harmful UV lights from 265 nm to 300 nm, UV-C to UV-B, were absorbed by such compounds, giving lights from 306 nm to 342 nm, in the range of UV-B to UV-A [44]. Bright deep-blue or violet-blue emissions for 2, 4, and 5 in diluted THF solutions were observed under excitations of 365 nm and 254 nm at room temperature in air ( Figure 6). Solvent effects on the steady-state emission spectra for 1-6 in CH 3 CN, EtOH, THF, and DCM at room temperature in air were also studied ( Figure 7, Figures S26-S31). For 1, major fluorescence peaks were red-shifted from 332 nm in DCM to 398 nm in CH 3 CN with the increasing of polarity. An emission peak at 317 nm in EtOH was sharp and resolved compared to the broad and overlapped peaks in other solvents. A similar trend was also observed for 2, 3, 4 and 6. For 5, the emission profile was quite different from 1, 2, 3, 4, and 6, also matching with polarity effect. The dramatic difference was tentatively attributed to the existence of a non-conjugated core only in 5.
Therefore, aromatic conjugation greatly contributed to emission profiles and peak positions. Moreover, the characterized crystal structure for 5 revealed the absence of intermolecular N···O hydrogen bonds, which might be responsible for the decreased chances of forming types of hydrogen-bonded superstructures. To some extent, the existence of hydrogen bonds led to complicated emission profiles, non-radiative decay, energy transfer, and quenched fluorescence [45][46][47][48][49] . For 1 and 3, intermolecular N···O hydrogen bonds were observed in characterized structures that could induce weak or quenched fluorescence in solid state. In solution state, freely moving molecules still have opportunities to form hydrogen bonds due to the existence of N-H and imide units in 1-6.  [45][46][47][48][49] . For 1 and 3, intermolecular N···O hydrogen bonds were observed in characterized structures that could induce weak or quenched fluorescence in solid state. In solution state, freely moving molecules still have opportunities to form hydrogen bonds due to the existence of N-H and imide units in 1-6. Fluorescence spectra for 1-6 in the solid state were also obtained under excitations of 250 nm and 280 nm at room temperature in air ( Figures S32-S34). Accordingly, emission peaks appeared at 440 nm, 400 nm, and 360 nm for 1, 4, and 5. It is a common phenomenon that aggregation-caused quenching (ACQ) occurs in conjugated molecules due to intermolecular interactions within a short range, which leads to the enhancement of non-radiative decay pathways [28,50]. Therefore, the less conjugated compound 5 without intermolecular N···O hydrogen bonds in solid state was brighter than the intermolecular N···O hydrogen bonded compounds of 1 and 3. In addition, PLQYs of 2 (PLQY = 4.69% in solid; PLQY = 7.67% in THF solution), 4 (PLQY = 5.43% in solid; PLQY = 1.28% in THF solution), and 5 (PLQY = 6.39% in solid; PLQY = 0.74% in THF solution) were obtained at room temperature in air. A potential application of 2, 4, and 5 can be considered for deep-blue or violet-blue emitters in solid state according to studies of blue OLEDs [43,51,52]. The exploration of being probes in solution state is also interesting.   Fluorescence spectra for 1-6 in the solid state were also obtained under excitations of 250 nm and 280 nm at room temperature in air (Figures S32-S34). Accordingly, emission peaks appeared at 440 nm, 400 nm, and 360 nm for 1, 4, and 5. It is a common phenomenon that aggregation-caused quenching (ACQ) occurs in conjugated molecules due to intermolecular interactions within a short range, which leads to the enhancement of non-radiative decay pathways [28,50]. Therefore, the less conjugated compound 5 without intermolecular N···O hydrogen bonds in solid state was brighter than the intermolecular N···O hydrogen bonded compounds of 1 and 3. In addition, PLQYs of 2 (PLQY = 4.69% in solid; PLQY = 7.67% in THF solution), 4 (PLQY = 5.43% in solid; PLQY = 1.28% in THF solution), and 5 (PLQY = 6.39% in solid; PLQY = 0.74% in THF solution) were obtained at room temperature in air. A potential application of 2, 4, and 5 can be considered for deep-blue or violet-blue emitters in solid state according to studies of blue OLEDs [43,51,52]. The exploration of being probes in solution state is also interesting.  Fluorescence spectra for 1-6 in the solid state were also obtained under excitations of 250 nm and 280 nm at room temperature in air (Figures S32-S34). Accordingly, emission peaks appeared at 440 nm, 400 nm, and 360 nm for 1, 4, and 5. It is a common phenomenon that aggregation-caused quenching (ACQ) occurs in conjugated molecules due to intermolecular interactions within a short range, which leads to the enhancement of non-radiative decay pathways [28,50]. Therefore, the less conjugated compound 5 without intermolecular N···O hydrogen bonds in solid state was brighter than the intermolecular N···O hydrogen bonded compounds of 1 and 3. In addition, PLQYs of 2 (PLQY = 4.69% in solid; PLQY = 7.67% in THF solution), 4 (PLQY = 5.43% in solid; PLQY = 1.28% in THF solution), and 5 (PLQY = 6.39% in solid; PLQY = 0.74% in THF solution) were obtained at room temperature in air. A potential application of 2, 4, and 5 can be considered for deep-blue or violet-blue emitters in solid state according to studies of blue OLEDs [43,51,52]. The exploration of being probes in solution state is also interesting.

Differential Pulse Voltammetry (DPV) and Cyclic Voltammogram (CV)
Peaks from DPV at 0.47 V and 1.01 V, together with oxidation peaks by CV at around 0.50 V and 1.10 V for compound 1 suggest the formation of diphenylbenzidene after two subsequent 1 e oxidation reactions. E 1/2 values at −0.50 V and −1.00 V were consistent with DPV peaks appearing at −0.55 V and −1.02 V for the two 1 e reductions of the NDI core ( Figure 8) [34,35,37,38]. Similarly, two 1 e reductions of the 4,4 -biphthalic core in 3 were observed at potentials of −1.27 V and −1.17 V by DPV, which were consistent with E 1/2 values at −1.33 V and −1.14 V by CV. On the contrary, only one 1 e reduction of the 1,8-naphthalene unit in 6 at −1.27 V by DPV with an E 1/2 value at −1.24 V by CV were observed ( Figures S35-S39). Meanwhile, oxidation and reduction potentials for 1-6 were not obviously affected either by oxidation run first or reduction run first.

Differential Pulse Voltammetry (DPV) and Cyclic Voltammogram (CV)
Peaks from DPV at 0.47 V and 1.01 V, together with oxidation peaks by CV at around 0.50 V and 1.10 V for compound 1 suggest the formation of diphenylbenzidene after two subsequent 1 e oxidation reactions. E1/2 values at −0.50 V and −1.00 V were consistent with DPV peaks appearing at −0.55 V and −1.02 V for the two 1 e reductions of the NDI core ( Figure 8) [34,35,37,38]. Similarly, two 1 e reductions of the 4,4′-biphthalic core in 3 were observed at potentials of −1.27 V and −1.17 V by DPV, which were consistent with E1/2 values at −1.33 V and −1.14 V by CV. On the contrary, only one 1 e reduction of the 1,8-naphthalene unit in 6 at −1.27 V by DPV with an E1/2 value at −1.24 V by CV were observed (Figures S35-39). Meanwhile, oxidation and reduction potentials for 1-6 were not obviously affected either by oxidation run first or reduction run first.

Conclusions
In summary, a series of diimide and monoimide compounds condensed with p-phenylamino(phenyl)amine were successfully synthesized and confirmed. Single crystal structures showed one type of intermolecular N···O hydrogen bond in 1, forming 2D large pore size channels, and two types of intermolecular N···O hydrogen bonds in 3, forming a 1D chain. All compounds showed high thermal stabilities. Particularly, the two types of intermolecular N···O hydrogen bonds in 3 play a vital role for thermal stability property. Fluorescence studies conducted both in solution and in solid states indicated that intermolecular N···O hydrogen bonding interactions quenched fluorescence. Diimide compounds 2, 4, and 5 were potential deep-blue or violet-blue emitters in solid state. The exploration of such compounds in areas of probes, electrochromic materials, information security, and semiconductors are worthy of consideration.
Supplementary Materials: The following are available online at www.mdpi.com/xxx/s1, spectroscopic data for 1-6 were provided as supplementary information. CCDC 1859058, 1859059, and 1859060 contain the supplementary crystallographic data for this paper. These data can be obtained free of charge via www.ccdc.cam.ac.uk/data_request/cif, or by emailing data_request@ccdc.cam.ac.uk, or by contacting The Cambridge Crystallographic Data Centre, 12 Union Road, Cambridge CB2 1EZ, UK; fax: +44 1223 336033. Figure S1: 1 H NMR for 1 in DMSO-d6 recorded on a 500M Hz spectrometer at 303 K.; Figure S2: 13 C NMR for 1 in DMSO-d6/TFA-d solvents recorded on a 300M Hz spectrometer at 303 K. Figure S3: 1 H NMR for 2 in DMSO-d6 recorded on a 500M Hz spectrometer at 303 K. Figure S4: 13 C NMR for 2 in DMSO-d6/TFA-d solvents recorded on a 300M Hz spectrometer at 303 K. Figure S5: 1 H NMR for 3 in DMSO-d6 recorded on a 500M Hz spectrometer

Conclusions
In summary, a series of diimide and monoimide compounds condensed with p-phenylamino(phenyl)amine were successfully synthesized and confirmed. Single crystal structures showed one type of intermolecular N···O hydrogen bond in 1, forming 2D large pore size channels, and two types of intermolecular N···O hydrogen bonds in 3, forming a 1D chain. All compounds showed high thermal stabilities. Particularly, the two types of intermolecular N···O hydrogen bonds in 3 play a vital role for thermal stability property. Fluorescence studies conducted both in solution and in solid states indicated that intermolecular N···O hydrogen bonding interactions quenched fluorescence. Diimide compounds 2, 4, and 5 were potential deep-blue or violet-blue emitters in solid state. The exploration of such compounds in areas of probes, electrochromic materials, information security, and semiconductors are worthy of consideration.  Figure  S1: 1 H NMR for 1 in DMSO-d 6 recorded on a 500M Hz spectrometer at 303 K.; Figure S2: 13 C NMR for 1 in DMSO-d 6 /TFA-d solvents recorded on a 300M Hz spectrometer at 303 K. Figure S3: 1 H NMR for 2 in DMSO-d 6 recorded on a 500M Hz spectrometer at 303 K. Figure S4: 13 C NMR for 2 in DMSO-d 6 /TFA-d solvents recorded on a 300M Hz spectrometer at 303 K. Figure S5: 1 H NMR for 3 in DMSO-d 6 recorded on a 500M Hz spectrometer at 303 K. Figure S6: 13 C NMR for 3 in DMSO-d 6 /TFA-d solvents recorded on a 300M Hz spectrometer at 303 K. Figure S7: 1 H NMR for 4 in DMSO-d 6 recorded on a 500M Hz spectrometer at 303 K. Figure S8: 13 C NMR for 4 in DMSO-d 6 /TFA-d solvents recorded on a 300M Hz spectrometer at 303 K. Figure S9: 1 H NMR for 5 in DMSO-d 6 recorded on a 500M Hz spectrometer at 303 K. Figure S10: 13 C NMR for 5 in DMSO-d 6 /TFA-d solvents recorded on a 300M Hz spectrometer at 303 K. Figure S11: 1 H NMR for 6 in DMSO-d 6 recorded on a 500M Hz spectrometer at 303 K. Figure S12: 13 C NMR for 6 in DMSO-d 6 /TFA-d solvents recorded on a 500M Hz spectrometer at 303 K. Figure S13: APCI for 1. Figure S14: APCI for 2. Figure S15: APCI for 3. Figure S16: APCI for 4. Figure S17: ESI for 5. Figure S18: ESI for 6. Figure S19: FT-IR spectra of 1, 2, and 3 (KBr pellets). Figure S20: FT-IR spectra of 4, 5, and 6 (KBr pellets). Figure S21: TGA curves for 1-6. Figure S22: UV-vis spectra for 1-6 in DCM. Figure  S23: UV-vis spectra for 1-6 in THF. Figure S24: UV-vis spectra for 1-6 in EtOH. Figure S25: UV-vis spectra for 1-6 in CH 3 CN. Figure S26: Normalized emission spectra of 2 were excited at 290 nm in CH 3 CN (black), EtOH (red), THF (blue), and DCM (greenish blue), respectively at room temperature in air. Figure S27: Normalized emission spectra of 3 were excited at 286 nm in CH 3 CN (black), EtOH (red), THF (blue), and DCM (greenish blue), respectively at room temperature in air. Figure S28: Normalized emission spectra of 4 were excited at 284 nm in CH 3 CN (black), EtOH (red), THF (blue), and DCM (greenish blue), respectively at room temperature in air. Figure S29: Normalized emission spectra of 5 were excited at 290 nm in CH 3 CN (black), EtOH (red), THF (blue), and DCM (greenish blue), respectively at room temperature in air. Figure S30: Normalized emission spectra of 6 were excited at 290 nm in CH 3 CN (black), EtOH (red), THF (blue), and DCM (greenish blue), respectively at room temperature in air. Figure S31: Emission photographs for 1-6 in DCM (top), EtOH (middle), and CH 3 CN (bottom) excited at 254 nm (left) and 365 nm (right), respectively at room temperature in air. Figure S32: Solid state emission spectra excited at 250 nm for 1-6 at room temperature in air. Figure S33: Solid state emission spectra excited at 280 nm for 1-6 at room temperature in air. Figure S34: Emission photographs for 1-6 in solid state with regular light (top), excited at 365 nm (middle), and 254nm (bottom), respectively at room temperature in air. Figure S35: DPV in black dashed line and CV of 2 were measured in DMF with 0.1 M TBAPF 6 . CV of 2-Oxi in red solid line indicated oxidation run first and 2-Red in blue solid line indicated reduction run first. Pt wire, Pt disk, and Ag/AgCl were used for measurements with a scan rate of 0.1 Vs −1 . Figure S36: DPV in black dashed line and CV of 3 were measured in DMF with 0.1 M TBAPF 6 . CV of 3-Oxi in red solid line indicated oxidation run first and 3-Red in blue solid line indicated reduction run first. Pt wire, Pt disk, and Ag/AgCl were used for measurements with a scan rate of 0.1 Vs −1 . Figure S37: DPV in black dashed line and CV of 4 were measured in DMF with 0.1 M TBAPF 6 . CV of 4-Oxi in red solid line indicated oxidation run first and 4-Red in blue solid line indicated reduction run first. Pt wire, Pt disk, and Ag/AgCl were used for measurements with a scan rate of 0.1 Vs −1 . Figure S38: DPV in black dashed line and CV of 5 were measured in DMF with 0.1 M TBAPF 6 . CV of 5-Oxi in red solid line indicated oxidation run first and 5-Red in blue solid line indicated reduction run first. Pt wire, Pt disk, and Ag/AgCl were used for measurements with a scan rate of 0.1 Vs −1 . Figure

Conflicts of Interest:
The authors declare no conflict of interest.