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.

1. Introduction

Conjugated organic class="Chemical">polymers and small molecules disclass="Chemical">play both charge and energy transfer class="Chemical">proclass="Chemical">perties through π–π or π–n–π, which are affected by intrinsic structures, class="Chemical">packing modes, and morclass="Chemical">phology [1,2,3]. Aclass="Chemical">pclass="Chemical">plications were found in organic nonvolatile memories (ONVMs) [4], organic field-effect transistors (OFETs) [5,6], single molecular switch [7], class="Chemical">photonics [8], organic solar cells (OSCs) [9], organic rechargeable class="Chemical">pan class="Chemical">lithium-/sodium ion batteries [10,11,12,13], and electrochromism [14,15,16]. Particularly, rylene diimides were widely studied, due to their high electron mobilities because of long range conjugation and high thermal and oxidative stabilities [17]. Moreover, multifunctional properties on rylene diimides were also explored as molecular imaging agents [18,19] and probes [20,21,22]. A few rylene diimides, such as perylene diimide dyes [23,24] and naphthalene diimide derivatives [25,26,27], showing fluorescence property in solid state were synthesized with non-arylamine, regardless of the aggregation-caused quenching (ACQ) effect, leading to weak or quenched fluorescence property in solid state [28].

To investigate the biclass="Chemical">nding class="Chemical">process for small molecules to DNA motivated by discovering drugs, fluorescence class="Chemical">proclass="Chemical">perty on both class="Chemical">pan class="Chemical">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 water-soluble fluorescent probe of naphthalene diimide combined with red and blue NDIs was reported by Freccero [31], which gave a red/NIR emission upon binding with G-quadruplex. Furthermore, conjugated aromatic compounds containing oxadiazole and pyridine units upon coordination with zinc ions by Diana [32] showed bright luminescence. In addition, Caruso reported a fluorescence sensor, pyridyl/phenolic/benzothiazole functionalized colorimetric receptors (BPAP), with high selectivity and excellent sensitivity towards zinc and cadium ions [33].

N, N′-bis[class="Chemical">p-phenylamino(phenyl)]-1,4,5,8-naclass="Chemical">phthalenetetracarboxylic class="Chemical">pan class="Chemical">diimide (DNTD) and N, N′-bis[p-phenylamino(phenyl)]-3,4,9,10-perylenetetracarboxylic diimide (DPTD) were reported by Cammarata [34,35,36] and Guo [37,38,39], respectively. Single crystal structures provide rich information about packing and weak interactions, including hydrogen bonds, π–π stacking, and the van der Waals force. Detailed structural data are not only useful to understand mechanisms but also important for guiding the design of new molecules. However, such conjugated imides have low solubility issues in many organic solvents.

In this work, we describe single crystal structures and thermal stability, fluorescence, and electrochemical properties based on synthesized class="Chemical">imide comclass="Chemical">pounds. Herein, a series of class="Chemical">pan class="Chemical">diimide compounds 1–5 and monoimide compound 6 condensed with p-phenylamino(phenyl)amine were successfully synthesized (Scheme 1). Of these, 2–6 are new compounds and single crystal structures of 1, 3, and 5 are firstly presented. Furthermore, the roles of intermolecular N···O hydrogen bonds on thermal stability and fluorescence properties are discussed accordingly.

Scheme 1

Synthesis of diimide and monoimide compounds.

2. Materials and Methods

All commercially available starting materials, reagents, and solvents were purchased and used as supplied. class="Chemical">p-Phenylamino(phenyl)amine, class="Chemical">pan class="Chemical">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 cm3/min with a heating rate of 10 °C/min on Mettler TGA2 Thermogravimetric Analyzer (Zurich, Switzerland). 1H NMR and 13C 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 TBAPF6 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].

N, N′-bis[

class="Chemical">Naphthalene-1,4,5,8-tetracarboxylic dianhydride (1.34 g, 5 mmol) was directly added to 120 mL glacial class="Chemical">pan class="Chemical">acetic acid dissolved with p-phenylamino(phenyl)amine (2.76 g, 15 mmol) and then heated to reflux for 12 h. The solution was cooled down to room temperature and poured into methanol (250 mL), resulting in a precipitate. The crude product was collected by filtration then suspended in 250 mL methanol. Under sonication for five minutes, the purified solid was recollected by filtration. This operation was repeated three times to obtain a purple product (2.70 g, 4.50mmol, 90%). Purple crystals were obtained by evaporation of CH3CN/DMF (1:4) at room temperature. 1H NMR (500 MHz, DMSO-d6, ppm): 8.72 (s, 2H, CoreH), 8.37 (s, 1H, NH), 7.25–7.31 (m, 4H, ArH), 7.19 (t, 4H, ArH), 6.89 (t, 1H, ArH); 13C NMR (300 MHz, DMSO-d6/TFA-d, ppm): 140.79, 140.37, 138.83, 136.58, 135.32, 134.92, 134.81, 131.32, 130.77, 128.50, 126.32, 124.24, 120.48, 116.72, 112.97; FT-IR (KBr pellet, cm−1): 1666(s), 1592(s), 1581(m), 1532(s), 1509(m), 1496(s), 1448(m), 1409(w), 1345(m), 1328(s); HRMS(APCI) m/z calcd: 601.1876 [M+H]+, found 601.1851; Anal. calcd for C38H24N4O4 (%): C 75.99; H 4.03; N 9.33, found: C 74.55; H 4.03; N 9.14.

N, N′-bis[

A similar method as described above was employed by the substitution of class="Chemical">naphthalene-1,4,5,8-tetracarboxylic dianhydride with 3,3′,4,4′-benzoclass="Chemical">phenonetetracarboxylic diclass="Chemical">pan class="Chemical">anhydride (1.61 g, 5 mmol). A brick red product was obtained (3.05 g, 4.66 mmol, 93%). 1H NMR (500 MHz, DMSO-d6, ppm): 8.39 (s, 1H, NH), 8.25 (d, 1H, CoreH), 8.16 (d, 2H, CoreH), 7.28 (t, 4H, ArH), 7.14–7.19 (m, 4H, ArH), 6.89 (t, 1H, ArH); 13C NMR (300 MHz, DMSO-d6/TFA-d, ppm): 199.38, 145.82, 140.70, 139.42, 138.69, 138.43, 136.85, 135.20, 134.78, 134.51, 134.40, 132.65, 129.28, 128.65, 127.59, 126.02, 124.00, 120.24, 116.48, 112.72; FT-IR (KBr pellet, cm−1): 1715(s), 1654(m), 1603(m), 1527(m), 1504(w), 1494(w), 1347(w), 1322(m); HRMS(APCI) m/z calcd: 655.1981 [M+H]+, found 655.1965; Anal. calcd for C41H26N4O5 (%): C 75.22; H 4.00; N 8.56, found: C 75.70; H 3.95; N 8.56.

N, N′-bis[

A similar method as described above was employed by the substitution of class="Chemical">naphthalene-1,4,5,8-tetracarboxylic dianhydride with 4,4′-biclass="Chemical">phthalic class="Chemical">pan class="Chemical">anhydride (1.47 g, 5 mmol). An orange red product was obtained (2.90 g, 4.63 mmol, 93%). Orange crystals were obtained by the evaporation of CH3CN/DMF (1:4) at room temperature. 1H NMR (500 MHz, DMSO-d6, ppm): 8.40 (s, 1H, NH), 8.37 (s, 2H, CoreH), 8.07 (d, 1H, CoreH), 7.29 (t, 4H, ArH), 7.15–7.19 (m, 4H, ArH), 6.89 (t, 1H, ArH); 13C NMR (300 MHz, DMSO-d6/TFA-d, ppm): 150.25, 139.31, 138.73, 138.26, 137.03, 135.74, 134.76, 134.49, 134.39, 134.28, 132.77, 128.94, 127.56, 126.95, 126.02, 124.01, 120.25, 116.48, 112.72; FT-IR (KBr pellet, cm−1): 1712(s), 1592(m), 1517(m), 1494(m), 1451(w), 1327(m), 1309(m); HRMS(APCI) m/z calcd: 627.2032 [M+H]+, found 627.2025; Anal. calcd for C40H26N4O4 (%): C 76.67; H 4.18; N 8.94, found: C 77.14; H 4.16; N 8.87.

N, N′-bis[

A similar method as described above was employed by the substitution of class="Chemical">naphthalene-1,4,5,8-tetracarboxylic dianhydride with class="Chemical">pan class="Chemical">pyromellitic dianhydride (1.09 g, 5 mmol). An orange product was obtained (2.56g, 4.65 mmol, 93%). 1H NMR (500 MHz, DMSO-d6, ppm): 8.40 (s, 1H, NH), 8.32 (s, 1H, CoreH), 7.27-7.33 (m, 4H, ArH), 7.15–7.19 (m, 4H, ArH), 6.90 (t, 1H, ArH); 13C NMR (300 MHz, DMSO-d6/TFA-d, ppm): 140.90, 139.50, 136.70, 134.44, 134.33, 132.46, 127.63, 126.02, 124.00, 123.69, 120.24, 116.48, 112.72; FT-IR (KBr pellet, cm−1): 1720(s), 1603(m), 1526(m), 1504(w), 1494(w), 1469(w), 1453(w), 1320(m), 1307(m); HRMS(APCI) m/z calcd: 551.1719 [M+H]+, found 551.1721; Anal. calcd for C34H22N4O4 (%): C 74.17; H 4.03; N 10.18, found: C 74.18; H 3.94; N 10.06.

N, N′-bis[

(pan class="Gene">DCTD) 5

A similar method as described above was employed by the substitution of class="Chemical">naphthalene-1,4,5,8-tetracarboxylic dianhydride with class="Chemical">pan class="Chemical">bicyclo[2.2.2]oct-7-ene-2,3,5,6-tetracarboxylic dianhydride (1.24 g, 5 mmol). A light pink product was obtained (2.48 g, 4.27 mmol, 86%). Light pink crystals were obtained by the evaporation of CH3CN at room temperature. 1H NMR (500 MHz, DMSO-d6, ppm): 8.32 (s, 1H, NH), 7.26 (t, 2H, ArH), 7.09–7.11 (d-d, 4H, ArH), 6.96 (d, 2H, ArH), 6.87 (t, 1H, ArH); 6.28 (t, 1H, eneH), 3.52 (s, 1H, R3CH), 3.37 (s, 2H, (C = O)CH); 13C NMR (300 MHz, DMSO-d6/TFA-d, ppm): 140.03, 138.58, 136.59, 135.02, 134.32, 134.21, 132.53, 127.73, 125.98, 124.02, 120.25, 116.49, 112.72, 46.63, 37.76; FT-IR (KBr pellet, cm−1): 1705(s), 1597(m), 1520(m), 1500(m), 1321(m), 1303(m); HRMS(ESI) m/z calcd: 581.2189 [M+H]+, found 581.2209; Anal. calcd for C36H28N4O4 (%): C 74.47; H 4.86; N 9.65, found: C 74.92; H 4.66; N 9.58.

N-

A similar method as described above was employed by the substitution of class="Chemical">naphthalene-1,4,5,8-tetracarboxylic dianhydride with class="Chemical">pan class="Chemical">1,8-naphthalene anhydride (0.99 g, 5 mmol). A yellow product was obtained (1.13 g, 3.10 mmol, 62%). 1H NMR (500 MHz, DMSO-d6, ppm): 8.49-8.51 (m, 4H, CoreH), 8.32 (s, 1H, NH), 7.90 (t, 2H, CoreH), 7.28 (t, 2H, ArH), 7.15–7.20 (m, 6H, ArH), 6.87 (t, 1H, ArH); 13C NMR (300 MHz, DMSO-d6/TFA-d, ppm): 140.77, 140.35, 140.12, 136.87, 135.63, 135.07, 134.32, 134.20, 132.08, 130.88, 127.98, 126.04, 124.41, 124.01, 120.25, 116.48, 112.71; FT-IR (KBr pellet, cm−1):1697(m), 1658(s), 1625(w), 1608(w), 1589(s), 1535(m), 1510(m), 1494(m), 1342(m), 1329(m); HRMS(ESI) m/z calcd: 365.1290 [M+H]+, found 365.1304; Anal. calcd for C24H16N2O2 (%): C 79.11; H 4.43; N 7.69, found: C 79.21; H 4.29; N 7.64.

3. Results and Discussion

class="Chemical">Diimide comclass="Chemical">pounds 1–5 and class="Chemical">pan class="Chemical">monoimide compound 6 were synthesized by the condensation of p-phenylamino(phenyl)amine with dianhydrides/anhydride. 1H NMR and 13C 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-d6 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.

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 class="Gene">P21/n with solvent class="Chemical">pan class="Chemical">DMF molecules embedded in the lattice. As shown in Figure 1 and Figure 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.

Table 1

Crystallographic data for 1, 3, and 5.

	1	3	5
Empirical formula	C38H24N4O4 ·2DMF	C40H26N4O4	C36H28N4O4
CCDC	1859060	1859059	1859058
Formula weight	746.80	626.65	580.62
Temperature (K)	296(2)	296(2)	296(2)
λ (Å)	0.71073	0.71073	0.71073
Crystal system	Monoclinic	Triclinic	Monoclinic
Space group	P21/n	P-1	P21/c
a (Å)	13.917(7)	8.3054(19)	9.457(10)
b (Å)	5.811(3)	12.394(3)	25.27(3)
c (Å)	22.797(11)	14.874(3)	12.610(14)
α (°)	90	103.340(4)	90
β (°)	97.101(8)	91.546(4)	109.546(13)
γ (°)	90	94.871(4)	90
V (Å3)	1829.7(15)	1482.6(6)	2840(5)
Z	2	2	4
Dcalcd (mg·m−3)	1.356	1.404	1.358
μ (mm−1)	0.092	0.092	0.090
F (000)	784	652	1216
θ (°)	2.913–27.570	2.446–25.000	2.285–27.618
Reflections /unique	10894/4195	7779/5157	17897/6511
GOF on F2	0.959	0.855	1.042
R1a, wR2b [I > 2σ(I)]	0.0665, 0.1697	0.0662, 0.1294	0.0432, 0.1090
Rint	0.0621	0.0636	0.0332

a R1=∑||Fo|−|Fc||/∑|Fo|. b wR2 = [∑w(Fo2−Fc2)2/∑w(Fo2)2]½.

Table 2

Selected bond lengths (Å) and torsion angles (°) for 1, 3, and 5.

1		3		5
	Bond Length		Bond Length		Bond Length
C1–N1	1.385(4)	C1–N1	1.402(5)	C31–N1	1.406(2)
C7–N1	1.389(3)	C7–N1	1.389(5)	C28–N1	1.408(2)
		C35–N4	1.417(6)	C4–N4	1.391(2)
		C32–N4	1.406(5)	C7–N4	1.398(2)
C10–N2	1.444(3)	C10–N2	1.436(5)	C25–N2	1.434(2)
		C29–N3	1.440(5)	C10–N3	1.435(2)
C–C(Ph-t)av	1.359(0)	C–C(Ph-t)av	1.379(4)	C–C(Ph-t)av	1.378(3)
C–C(Ph-a)av	1.378(3)	C–C(Ph-a)av	1.385(9)	C–C(Ph-a)av	1.376(2)
C–C(Core)av	1.260(2)	C–C(Core)av	1. 387(9)
		C–C(Ph-t)av	1.382(8)	C–C(Ph-t)av	1.381(6)
		C–C(Ph-a)av	1.380(5)	C–C(Ph-a)av	1.380(9)
		C–C(Core)av	1. 386(8)
	Torsion Angle		Torsion Angle		Torsion Angle
C8–C7–N1–C1	177.5(3)	C12–C7–N1–C1	152.8(5)	C27–C28–N1–C31	−126.89(17)
C9–C10–N2–C17	115.0(3)	C11–C10–N2–C13	104.0(5)	C26–C25–N2–C23	105.76(16)
		C33–C32–N4–C35	−140.8(5)	C8–C7–N4–C4	−144.71(17)
		C34–C29–N3–C27	149.7(4)	C9–C10–N3–C16	126.76(17)

Figure 1

Schematic diagrams of intermolecular N···O hydrogen bonding interactions that appeared in diimide compounds for 1 (top left), 3 (middle left), and 5 (bottom left). ORTEP structures of 1 (top right), 3 (middle right), and 5 (bottom right) were presented with intermolecular N···O hydrogen bonding interactions. Solvent DMF molecules in 1 were deleted for clarity. Ph-t represented the terminal phenyl unit and Ph-a represented the adjacent phenyl unit relative to core.

Figure 2

Space filling diagrams (left) with listed torsion angles and dihedral angles (right) were presented. Top left and right diagrams are for 1, middle left and right diagrams are for 3; bottom left and right are for 5.

The space filling diagram of 1 showed twisted connections between the class="Chemical">imide rings and class="Chemical">pan class="Chemical">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).

Figure 3

Perspective views for 1 formed by intermolecular N···O hydrogen bonds (a–d) are presented. A large pore was formed by four molecules with equivalent one type of N···O hydrogen bonds (a). Views of embedded solvent DMF molecules (b), solvent free 2D network (c), and channels (d) are presented. The greenish blue dashed line represents the intermolecular N···O hydrogen bonds. The red dashed line represents hanging contacts.

Compound 3 crystallized in the triclinic space group class="Gene">P-1. As shown in Figure 1 and Figure 2, the crystal structure showed one twisted core and two class="Chemical">pan class="Chemical">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) showed longer distances for C10–N2 (1.436(5) Å) and C29–N3 (1.440(5) Å) than C1–N1 (1.402 (5) Å), C7–N1 (1.389 (5) Å), C35–N4 (1.417 (6) Å), and C32–N4 (1.406 (5) Å) in p-phenylamino(phenyl) units due to similar reasons as compound 1. In addition, lower symmetry was observed in 3 than in 1. Interestingly, the average bond length of 1.387(4) Å for C–C(core)av was comparable to both C–C(Ph-t)av (1.379(4) and 1.382(8) Å) and C–C(Ph-a)av (1.385(9) and 1.380(5) Å).

The space filling diagram of 3 showed a highly twisted configuration. The dramatically decreased torsion angles of ∠class="Chemical">Ph-t/class="Chemical">pan class="Gene">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, 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).

Figure 4

Perspective views for 3 formed by intermolecular N···O hydrogen bonds (a–d) are presented. A small pore was formed by two molecules with non-equivalent two types of N···O hydrogen bonds (a). Views of a single 1D chain (c), and double chains (b,d) for 3 are presented. The greenish blue dashed line represents intermolecular N···O hydrogen bonds.

Compound 5 crystallized in the monoclinic space group class="Gene">P21/c. As shown in Figure 1, the structure contained a non-conjugated core and two class="Chemical">pan class="Chemical">p-phenylamino(phenyl) units without intermolecular N···O hydrogen bonds. Selected C–N bond lengths in 5 showed longer distances for C25–N2 (1.434(2) Å) and C10–N3 (1.435(2) Å) than C31–N1 (1.406 (2) Å), C28–N1(1.408 (2) Å), C4–N4 (1.391 (2) Å), and C7–N4 (1.398 (2) Å) in p-phenylamino(phenyl) units (Figure 1 and 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 class="Chemical">p-phenylamino(phenyl) units. The torsion angles of ∠class="Chemical">pan class="Chemical">Ph-t/Ph-a with −144.71(17)° (a dihedral angle of 46.397(0.087)°) and (−126.89(17)°(a dihedral angle of 61.583(0.089)°) were also significantly decreased contrast to 177.5(3)° (a dihedral angle of 18.815(0.261)°) in 1 (Figure 2 and 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.

3.2. Infrared Spectra

IR (infrared) spectra for 1–6 were recorded on a Bruker Mclass="Chemical">PA sclass="Chemical">pectrometer between 400 and 4000 cm−1 (KBr class="Chemical">pellets). For comclass="Chemical">pound 1, the observed semicircle stretch modes of class="Chemical">pan class="Chemical">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.

3.3. 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 correspoclass="Chemical">nding solid samclass="Chemical">ples, 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 class="Chemical">pan class="Gene">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 N2 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.

3.4. UV-Vis Absorption and Fluorescence Spectra

Steady-state class="Disease">UV-vis absorption and fluorescence emission sclass="Chemical">pectra for 1–6 were recorded in class="Chemical">pan class="Chemical">THF, DCM, EtOH, and CH3CN, 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 CH3CN were also obtained (Figures S22–S25).

Figure 5

UV-vis absorption spectra (top), excitation spectra (bottom left, dashed line) and emission spectra of 1–6 (bottom right, solid line) in THF (2 × 10−5 M) were recorded at room temperature in air. Excitation wavelengths of 265 nm for 1, 277 nm for 2, 274 nm for 3, 300 nm for 4, 278 nm for 5, and 273 nm for 6 were applied to obtain emission spectra.

For compound 1, an emission peak appeared at 319 nm under the excitation of 265 nm, which matched well with the correspopan class="Chemical">nding excitation class="Chemical">peak at 267 nm (Figure 5). Similarly, an emission class="Chemical">peak aclass="Chemical">pclass="Chemical">peared at 318 nm under the excitation of 273 nm for 6. In contrast, a shoulder class="Chemical">peak aclass="Chemical">pclass="Chemical">peared at 312 nm for 2, exceclass="Chemical">pan class="Chemical">pt 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 iclass="Chemical">ndicated 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 comclass="Chemical">pounds, giving lights from 306 nm to 342 nm, in the range of UV-B to UV-A [44]. Bright deeclass="Chemical">p-blue or violet-blue emissions for 2, 4, and 5 in diluted class="Chemical">pan class="Chemical">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 CH3CN, 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 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.

Figure 6

Emission photographs of solvent THF (most left) and 1–6 in THF, excited at 254 nm (top) and 365 nm (bottom), were recorded at room temperature in air.

Figure 7

Normalized emission spectra of 1 were excited at 286 nm in CH3CN (black), EtOH (red), THF (blue), and DCM (greenish blue) at room temperature in air.

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 class="Chemical">hydrogen bonds, which might be resclass="Chemical">ponsible for the decreased chances of forming tyclass="Chemical">pes of class="Chemical">pan class="Chemical">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.

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 (class="Chemical">ACQ) occurs in conjugated molecules due to intermolecular interactions within a short range, which leads to the enhancement of non-radiative decay class="Chemical">pathways [28,50]. Therefore, the less conjugated comclass="Chemical">pound 5 without intermolecular N···O class="Chemical">pan class="Chemical">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.

3.5. Differential Pulse Voltammetry (DPV) and Cyclic Voltammogram (CV)

class="Chemical">Peaks from class="Chemical">pan class="Chemical">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–S39). Meanwhile, oxidation and reduction potentials for 1–6 were not obviously affected either by oxidation run first or reduction run first.

Figure 8

Differential pulse voltammetry (DPV) in the black dashed line and a cyclic voltammogram (CV) of 1 were measured in DMF with 0.1 M TBAPF6. The CV of 1-Oxi in the red solid line indicates that oxidation was run first and the 1-Red in the blue solid line indicates that reduction was run first. Pt wire, Pt disk, and Ag/AgCl were used for measurements with a scan rate of 0.1 Vs−1.

4. Conclusions

In summary, a series of class="Chemical">diimide and class="Chemical">pan class="Chemical">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.