Novel Fluorescent Tetrahedral Zinc (II) Complexes Derived from 4-Phenyl-1-octyl-1H-imidazole Fused with Aryl-9H-Carbazole and Triarylamine Donor Units: Synthesis, Crystal Structures, and Photophysical Properties

We present here the design, synthesis, and photophysical properties of two novel fluorescent zinc (II) complexes, ZnCl2(ImL1)2 and ZnCl2(ImL2)2, containing 4-(1-octyl-1H-imidazol-4-yl)-N,N-diphenyl-[1,1-biphenyl]-4-yl)-4-amine ImL1 and 9-(4-(1-octyl-1H-imidazol-4-yl)-[1,1-biphenyl]-4-yl)-9H-carbazole ImL2 ligands. The newly synthesized free ligands and their zinc (II) complexes were characterized using several spectroscopic techniques; their structures were identified by single-crystal X-ray diffraction; and their photophysical properties have been studied in the context of their chemical structure. The ZnCl2(ImL1)2 and ZnCl2(ImL2)2 complexes showed good thermal stability at 341 °C and 365 °C, respectively. Photophysical properties, including UV-Vis absorption spectra in ethanol solution and photoluminescence (PL) in both solid state and ethanol solution, were determined. UV-Vis adsorption data indicated that both free ligands had similar UV-Vis absorption properties, while their Zn (II) complexes had distinctive absorption characteristics. The fluorescence spectra show that both ligands and their corresponding Zn (II) complexes emit violet to cyan luminescence in the solid state at room temperature, while in ethanol solution at the same temperature, they exhibit efficient photoluminescence properties in the UV-A emission spectral region. Because of these photophysical properties, the synthesized ligands and their cognate Zn (II) complexes can be used as scaffolds for the potential development of optoelectronic materials.


Introduction
Many researchers have developed an interest in the design and synthesis of hybrid organic-inorganic systems as efficient optoelectronic materials because of their exciting potential for use in latent fingerprint (LFP) detection, organic light-emitting diodes (OLEDs), anti-counterfeiting, bio-imaging, and sensing applications [1][2][3][4][5]. The construction of these hybrid organic-inorganic systems with a fascinating range of structures and topologies is dependent on the organic ligands used and the nature of the metal ions. The careful choice of nitrogen (N)-containing organic ligands linked by a spacer and/or donors with a certain positional orientation is critical in building and controlling the architecture of complexes with desirable photophysical properties [6][7][8]. Several N-heterocyclic skeletons have been deemed building synthon ligands in organometallic and coordination chemistry because of their ability to serve as donor units, resulting in desirable properties [9][10][11][12][13].
Examples of N-heterocyclic systems, such as imidazole and its derivatives, have piqued the curiosity of researchers interested in developing hybrid organic-inorganic systems for various applications [2,[14][15][16][17][18]. The unique properties of imidazole-based complexes, such as excellent electrochemical and photoluminescent properties, excellent thermal properties, and ease of modification, were taken into account in the design of various host materials such as electron transport, fluorescent, or phosphorescent molecules [19][20][21][22][23]. Over the years, several articles have reported the coordination of imidazole-based synthons with a variety of metal ions, including cobalt, nickel, iron, zinc, copper, and iridium, leading to the preparation of stable organic metal complexes [9][10][11][12][13][24][25][26][27]. In particular, d 10 transition zinc (II) complexes have become the focus of an ever-growing research area owing to their attractive luminescence and the low cost of zinc metal sources [2,9,[27][28][29]. This posttransition metal ion can coordinate with four donor atoms, which can easily be increased to five and six, resulting in geometry ranging from tetrahedral to trigonal bipyramid, square pyramidal, and octahedral [2,9,[27][28][29]. As a result, the development of novel organic zinc (II) complexes has remained a key endeavor.
On the other hand, carbazole and diarylamine units are often regarded as important electron-donating units in donor-acceptor systems (D-A) due to their high triplet energies and good hole-transport properties [1,15,16,[30][31][32][33]. The diarylamine structure consists of two benzene groups directly attached to the central nitrogen atom, while the carbazole structure is a tricyclic ring skeleton with pyrrole rings attached to two aromatic rings. These high photoluminescence efficiency, electron-rich, and inexpensive starting materials can be easily modified by substituting the central nitrogen atom [1,15,16,[30][31][32][33][34][35]. Therefore, the carbazole and diarylamine frameworks remain good templates for the fabrication of OLED emitters and transparent optoelectronic materials.

NMR Characterization of the Free Ligands ImL1 and ImL2 as Well as and Their
Corresponding Zn(II) Complexes ZnCl 2 (ImL) 2 The 1 H and 13 C NMR spectra of both free ligands and their corresponding zinc (II) complexes supported the synthesized structures. It was found that ImL1, ImL2, and ZnCl 2 (ImL1) 2 were soluble in deuterated chloroform (CDCl 3 ), whereas ZnCl 2 (ImL2) 2 was soluble in deuterated dimethyl sulfoxide (DMSO-d 6 ). The total number of protons and carbons in the NMR spectra was congruent with the proposed title molecules; however, the proton spectra of the ImL1 and complex ZnCl 2 (ImL1) 2 showed different chemical shift signatures. The proton spectrum of the free ligand ImL1 in Figure S1 showed a signal from the 2-methine proton of the imidazole moiety overlapping between 7.48 and 7.50 ppm; this proton becomes downshifted to a chemical shift of 8.12 ppm upon zinc coordination in the ZnCl 2 (ImL1) 2 spectrum ( Figure S5). In addition, the 4-methine proton signal of the imidazole nucleus was also shown to overlap in the region of 6.98-7.02 ppm, which also shifts to 6.63 ppm as a result of zinc (II) ion coordination. The carbon-13 spectra of ImL1 and ZnCl 2 (ImL1) 2 had no significant chemical shift difference ( Figures S2 and S6 in Supplementary Materials). In the case of ImL2 and ZnCl 2 (ImL2) 2 , their solubility in different deuterated NMR solvents was a notable distinguishing feature. These NMR data demonstrate unequivocally that the ligands were effectively coordinated with the zinc (II) ion ( Figures S1-S8).
2.3. Fourier Transform Infrared Spectroscopy (FT-IR) Characterization of the Free Ligands ImL1 and ImL2 as Well as and Their Corresponding Zn(II) Complexes ZnCl 2 (ImL) 2 The FTIR spectra of the metal complexes were compared to those of the free ligands to investigate the structure of the zinc (II) complexes and the coordination mode of the ligands. The complete FTIR spectra of the free ligands and their associated Zn (II) complexes are displayed in Supplementary Figures S9-S12, while Figure 2 below presents the spectra across a selected frequency range of 1000-1800 cm -1 , and Table 1 summarizes the data. The FT-IR spectra of ligands ImL1 and ImL2 shown in Figures S9 and S10 displayed absorption bands in the range from 2851 to 3125 cm −1 , ascribed to C-H stretching vibrations of aromatic rings and alkyl groups, but these bands in the spectra of the Zn (II) complexes in Figure S11 weakened compared to their corresponding ligand. In addition, weak absorption peaks at 1705 and 1701 cm −1 were observed in the FTIR spectra of the free ligand in Figure 2a,b. However, these bands disappeared upon coordination of the ligands with the Zn (II) ion. Furthermore, ligand spectra show bands at wavenumbers 1612, 1589, and 1520 cm −1 for ImL1 and 1624, 1597, and 1520 cm −1 for ImL2, assigned to C=N and C=C functional groups. These bands at 1612 and 1624 cm −1 , however, completely disappeared in their respective complex spectra, while other bands were shifted to frequencies of 1588 and 1524 cm −1 for ZnCl 2 (ImL1) 2 and 1593 and 1524 cm −1 for ZnCl 2 (ImL2) 2 , respectively. Additionally, the spectra of both ligands show a band at 1188 cm −1 that is completely absent in the spectrum of the Zn (II) complex, further signifying the successful coordination of the ligands with the zinc metal ion. Table 1. FTIR signals of ligands ImL1 and ImL2 as well as their related ZnCl 2 (ImL) 2 complexes.

Structural Characterization by
Single Crystal X-ray Diffraction of the Free Ligands ImL1 and ImL2 as Well as and the Corresponding Zn (II) Complex ZnCl 2 (ImL1) 2 2.4.1. Description of the X-ray Crystal Structures the Free Ligands ImL1 and ImL2 The ligand ImL1 crystals suitable for X-ray crystallography were prepared by reheating the ligand ImL1 precipitates in a 50:50 mixture of THF and ethanol until the precipitate dissolved, followed by cooling and slowly evaporating the solvent for several days, yielding colourless crystals of ImL1. On the contrary, colourless ImL2 crystals were produced after heating the ImL2 precipitate in acetone and progressively evaporating the solvent for several days. The crystal structures for the free ligands ImL1 and ImL2 were solved by single crystal X-ray diffraction, and a summary of crystallographic data is presented in Table 2. For a complete collection of single-crystal X-ray diffraction data for ImL1 and ImL2, see the Supplementary Materials from Tables S1-S10. Table 2. Crystal data of ligands ImL1 and ImL2 as well as zinc (II) complex, ZnCl 2 (ImL1) 2 .

Ligand ImL1
Ligand ImL2 ZnCl 2 (ImL1) 2   Ligand ImL2 crystallized as triclinic with space group P-1, while the ligand ImL2 crystallized as monoclinic with space group P 21/c. Figures 3 and 4 depict the general arrangement and labeling of the atoms in the free ligands ImL1 and ImL2, respectively, while Table 3 lists the chosen bond lengths and angles. ImL2's three C-N bond lengths range from 1.318 to 1.368 Å, whereas ImL1's three C-N bond lengths range from 1.338 to 1.384 Å, which is comparable to previously reported imidazole derivatives [38,39]. Furthermore, the C-N bond lengths linking an alkyl group and the nitrogen (N2) atom of the imidazole moiety are 1.384 Å for ImL1 and 1.386Å for ImL2, while the C-N bond length connecting three aromatic carbon atoms to the nitrogen (N3) atom was found to be about 1.  27) could be attributed to the fact that two aromatic rings in the carbazole moiety in ImL2 adopt a planar shape, while the structure of the two aromatic rings in ImL1 resembles propeller blades.
The ImL1 ligand's crystal packing is stabilized by two-hydrogen bonding ( Figure 5), resulting in the development of a two-dimensional chain parallel to the crystallographic c-axis. The first intermolecular hydrogen bonding occurs between the imidazole rings' nitrogen (N1) atom and one of the hydrogen atoms linked to the carbon (C28) atom of the methylene moiety, which is directly attached to the nitrogen (N2) atom of the imidazole rings. A second intermolecular hydrogen bonding occurs between the hydrogen (H18) atom bound to the carbon (C18) atom of the aromatic ring, similar to propeller shafts, and the carbon (C12) atom of the aromatic ring sandwiched between the nitrogen (N3) atom and the aromatic ring carbon bonded directly to the imidazole unit.   The crystal packing of the ImL2 ligand, on the other hand, is also stabilized by twohydrogen bonding ( Figure 6), but the intermolecular hydrogen bonding occurs between the nitrogen (N1) atom of the imidazole rings and the hydrogen (H1) atom attached to the carbon (C1) atom of the neighbouring imidazole units. The difference in intramolecular interaction between ImL1 and ImL2 could be explained by the fact that the N-phenylcarbazole motif has a carbon-carbon linkage that forces two phenyl rings into planarity, whereas the two-phenyl rings of the triphenylamine unit have a propeller-like structure. This was reflected in the different bond angles of the N-phenylcarbazole motif [C16-N3-C27 with 108.04(13) • and C13-N3-C27 with 127.25 (14) • ] in comparison to the bond angles of the triphenylamine unit [116.6(3) • for C16-N3-C22 and 118.5 (3) • for C13-N3-C22] (see Table 3).     (14) C (27) The ZnCl 2 (ImL1) 2 crystals for X-ray examination were grown in the same way as Ligand L1 and obtained as pale yellow crystals. The crystallographic data and refinement information for the ZnCl 2 (ImL1) 2 complex are given in Table 2. The overall view and selected labelling of the atoms for clarity in the ZnCl 2 (ImL1) 2 complex are displayed in Figure 7, whereas the designated bond lengths and angles are tabulated in Table 4. A complete collection of single-crystal X-ray diffraction data for the ZnCl 2 (ImL1) 2 complex is given in the Supplementary Materials from Tables S11-S15. The single X-ray crystal structure of the ZnCl 2 L1 2 complex revealed that the complex crystallized as a monoclinic with space group C2. The ZnCl 2 (ImL1) 2 complex has a distorted tetrahedral environment in the zinc (II) ion center, with two coordination sites occupied by the bidentate chelation of two ImL1 ligands through the nitrogen atom of each ligand and the remaining two coordination sites occupied by two chlorine atoms. The Zn-N bond lengths between the nitrogen atoms of two ligands and the zinc ion were presented to be at distances of 2.029(2) Å and 2.030(2) Å, which are characteristic of Zn(II) complexes with neutral N donors, while the Zn-Cl length was exhibited to be at 2.2274(8) Å and 2.2453(8) Å, respectively. In addition, the N-Zn-N angles around Zn were found to be around the tetrahedral standard of 104.43 (9) • , while the Cl-Zn-Cl angle of 110.74(3) • is also centered on the tetrahedral standard, which confirmed that the Zn center forms a tetrahedral coordination geometry. The N-Zn-Cl angles are shown to be 107,24(7) • for N(1)-Zn(1)-Cl(1), 113.76 (7) • for N(4)-Zn(1)-Cl(1) • , 114.91(7) • for N(1)-Zn(1)-Cl(2), and 105.77 (7) • for N(4)-Zn(1)-Cl(2), respectively. Furthermore, the N-C-N bond angles for the two imidazole moieties of the complex were at 116.6(3) • for N(1)-C(1)-N(2) and 111.6(2) • for N(4)-C(36)-N(5), while the C-N-C bond angles of the same systems ranged from 1056(3) • to 126.5(3) • . The N-Zn-N and Cl-Zn-Cl bond lengths fall within the range of bond lengths in complexes of tetrahedral coordinated Zn with two N-coordinated ligands and two halide atoms previously reported [39][40][41][42].

Bond Lengths [Å]
Bond The optical properties of the free ligands and their corresponding complexes were studied by UV-Vis absorption in ethanol solution recorded at room temperature (at a concentration of 2 × 10 −4 mol/dm 3 ) and PL emission spectroscopy in both solid and ethanol solutions. The absorption and emission spectra, including the corresponding extinction coefficients, are shown in Figures 8-10, while their numerical data are tabulated in Table 5. The UV-Vis absorption spectra in Figure 8a,b of the free ligands show four bands of similar profile, each with a shoulder peak at 210 nm for ImL1 (black dotted curve) and 215 nm for ImL2 (blue dotted curve), which could be attributed to the π-π* transition of the benzene rings, and a second absorption peak at 230 nm for both ligands, which could be attributed to electronic π-π* transfers of the imidazole moieties [43][44][45]. Further, each ligand showed a third shoulder band centering around 295 nm and a fourth main peak at 340, which might be attributed to the usual n-π* transition of the N-phenylcarbazole and triphenylamine moieties [46][47][48][49]. The more intense π-π* transitions of the ligands have extinction coefficients (ε) ranging from 31,660 to 119,415 M −1 cm −1 , with ImL1 (blue curve in Figure 8c) having the highest value and ImL2 having the lowest (orange curve in Figure 8c). A high ε results indicate that the compounds absorb light well at the specified wavelength.   (Figure 9c, red curve) correspond to those in the free ligands, which could therefore be assigned to an intraligand (IL) 1 π-π* transition, whereas the shoulder at 235 and 335 nm for the ZnCl 2 (ImL1) 2 complex as well as 260 and 315 nm for the ZnCl 2 (ImL2) 2 complex could be assigned to a metal perturbed ligand π-π* transition. The results demonstrate that the complex, ZnCl 2 (ImL2) 2 , absorbs more and reflects less than ImL1 and ImL2, as well as ZnCl 2 (ImL1) 2 .  Figure 10. Emission spectra (a) of the free ligands (left), ImL1 (Blue) and ImL2 (orange) as well as (b) their zinc (II) complexes (right), ZnCl 2 (ImL1) 2 (red) and ZnCl 2 (ImL2) 2 (green) in the solid state at room temperature. Table 5. UV-Vis absorption in ethanol, molar extinction coefficient (ε), as well as photoluminescent, decay lifetimes (τ), CIE (x, y) coordinates data in the solid state and ethanol of ImL1, ImL2, ZnCl 2 (ImL1) 2 , and ZnCl 2 (ImL2) 2  The study of solid-state luminescence is intriguing because of the potential use of luminescent materials in the fabrication of transparent optoelectronic materials [50,51]. The solid-state photoluminescence of the free ligands and their corresponding Zn (II) complexes at room temperature were investigated, and their data are presented in Figure 10, and the photophysical data are summarized in Table 5. When the samples were excited with a photon source of 300 nm wavelength, emissions ranging from 350 to 800 nm were recorded in the solid state. It is worth mentioning that the intensity of the recorded emission was attenuated by a factor of 100 to prevent detector saturation. The free ligand ImL1 (Figure 10a, blue curve) displays structured cyan emission with wavelength maxima centered at 488 nm, while the emission spectrum of ImL2 (Figure 10a, orange curve) is intensely structured in the violet region with wavelength maxima centered at 411 nm.
The luminescence lifetimes of the free ligands in the solid state at room temperature were also measured. The measured luminescence time profiles of the free ligands and their corresponding Zn (II) complexes were well matched with one exponential decay component, and the resulting decay lifetimes (τ) are presented in Table 5 and Supplementary Figures S13-S16. The lifetimes of ImL1 and ImL2 were measured to be 1.07 and 7.81 nanoseconds, respectively.
It was observed that the related Zn (II) complexes in the solid state exhibit violet fluorescence emission characteristics, with ZnCl 2 (ImL1) 2 (Figure 10b, red curve) emitting at 410 nm with a fluorescence decay lifetime of 9.42 nanoseconds, whereas ZnCl 2 (ImL2) 2 (Figure 10b, green curve) emitting at 395 nm with a fluorescence decay lifetime of 4.61 nanoseconds. The luminescence in the violet region could be attributed to π-π* intraligand charge transfer (ILCT) transition. Additionally, the fluorescence intensity values of Zn ; (II) complexes were observed to be much larger than those of their corresponding free ligands, which is consistent with the complexes' homoleptic nature.
However, when excited at 340 nm in ethanol solution at room temperature, both the free ligands and their corresponding zinc (II) complexes exhibited UV-A emission, with wavelength maxima occurring at 366 nm for ImL1 (Figure 8a, black solid curve), 350 nm for ImL2 (Figure 8b, blue solid curve), 372 nm for ZnCl 2 (ImL1) 2 (Figure 9b, purple solid curve), and 345 nm for ZnCl 2 (ImL2) 2 (Figure 9b, orange solid curve). Furthermore, it was observed that the maximum wavelength emission of the ZnCl 2 (ImL1) 2 complex at 372 nm (Figure 9b, violet solid curve) was accompanied by an additional shoulder emission band in a violet region at 399 nm. The free ligands exhibited a small Stokes shift of 26 nm and 10 nm for ImL1 and ImL2, respectively. It is worth mentioning that the complexes hypsochromic emission shift had little effect on the Stokes shift, as demonstrated by stroke shifts of 32 nm for ZnCl 2 (ImL1) 2 and 10 nm for ZnCl 2 (ImL2) 2 , which were equivalent to those of the free ligands. Figure 11a shows the Commission Internationale de l'Éclairage (CIE) 1931 colour space of the PL emission in the solid state of the free ligands and the corresponding Zn (II) complexes. The ImL1 ligand emits cyan light with CIE x and y coordinates of 0.27 and 0.333, while the ImL2 ligand exhibits violet light with CIE coordinates of 0.196 and 0.152 in solid form. Both Zn (II) complexes produce violet light colours, with CIE coordinates of (0.239, 0.224) for ZnCl 2 (ImL1) 2 and (0.21, 0.193) for ZnCl 2 (ImL2) 2 , respectively. In the solution phase, however, the colours of both free ligands and their corresponding Zinc (II) complexes change to violet, with CIE coordinates of (0.239, 0.216) for ImL1, (0.308, 0.23) for ImL2, (0.303, 0.219) for ZnCl 2 (ImL1) 2 , and (0.342, 0.313) for ZnCl 2 (ImL1) 2 (Figure 11b).

Thermal Stability Studies
The thermal stability of the zinc (II) complexes ZnCl 2 (ImL1) 2 and ZnCl 2 (ImL 2 ) 2 was investigated using thermogravimetric analysis (TGA). TGA tests were carried out in an inert environment at a heating rate of 10 • C per minute throughout a temperature range of 23-900 • C. The extraordinary heat stability of the zinc (II) complex is overcome by the beginning of complex disintegration (Td), which corresponds to a 2% weight loss. The TGA profile for the ZnCl 2 (ImL1) 2 complex in Figure 12a shows a two-step profile: the first decomposition phase takes place at 341 • C, losing 2% of the composite's weight, while the second step occurs at 500 • C, demonstrating the loss of the entire organic moiety with 32.5% of the complex's total weight. Despite having a similar TGA profile to the ZnCl 2 (ImL1) 2 , the ZnCl 2 (ImL2) 2 complex in Figure 12b had a 2% weight decomposition at 365 • C, followed by a 32.5% weight loss at 514 • C due to the disintegration of entire organic units. A convoluted pattern of weight losses began during the second stage of the TGA profiles for the complexes, and it lasted until all was lost at 656 • C for ZnCl 2 (ImL2) 2 and 861 • C for ZnCl 2 (ImL1) 2 .

General Methods
All chemical reagents were bought from Merck and used without additional purification. All dried solvents were used directly from an LC-Tech SP-1 argon gas-stored solvent purifier. Unless otherwise stated, all reactions were monitored by analytical thin layer chromatography (TLC) using precoated Merck silica gel F254 plates and visualized under UV light (254 nm). Unless otherwise stated, the products were separated by column chromatography using Merck Silica Gel 60 [particle size 0.040-0.063 mm (230-400 mesh)] using various ratio of ethyl acetate to hexane. FTIR data were acquired using an Attenuated Total Reflectance (ATR) Fourier Transform Infrared spectroscope (Thermo Nicolet 5700 FTIR). NMR data were obtained at 298 K with a 400 MHz Bruker Avance spectrometer equipped with a BBI 5 mm probe. The solvent peaks for proton NMR of 7.26 (CDCl 3 ) and 2.50 (DMSO-d 6 ) and 77.0 (CDCl 3 ) and 39.52 (DMSO-d 6 ) for carbon-13 NMR were used as internal reference, chemical shifts are expressed in parts per million (ppm). Single X-ray crystallography data on intensity were collected using an Oxford Cryostream 600 cooler on a Bruker D8 Venture Microfocus with Photon III CCD area detector diffractometer with graphite-monochromator MoKα 1 (λ = 0.71073 Å) radiation at 173 K. SAINT+, version 6.02 [52], was used to reduce the data, and SADABS [50] was used to make empirical absorption corrections. XPREP [52] was used to create space group assignments. The structure was solved using SHELXT [51] and refined using full-matrix least-squares or difference Fourier techniques on F2 using SHELXL-2017 in the WinGX [53] Suite of tools [54]. All C-bound hydrogen atoms were idealized and refined as riding atoms with isotropic characteristics that were 1.2 or 1.5 times those of their parent atoms. ORTEP-3 [54] and PLATON [55] were used to create diagrams and publication content. The absorbance properties of the free ligands and their reacting complexes were measured employing a Thermo Logical Multiskan GO UV/Vis spectrophotometer. Information was collected on tests kept in 1-cm plastic cuvettes with ethanol as the reference solvent. The molar extinction coefficient was calculated using the formula in Equation (1): where A is the absorbance, ε is the molar extinction coefficient, b is the path length of the incident photon and c is the concentration of the material in solution. Photoluminescence was measured in quartz cuvettes (1 cm path length) employing a xenon light (150 W) and ethanol as the reference solvent, utilizing Perkin Elmer LS photoluminescence spectroscopy. Steady-state PL spectra were acquired at room temperature using a Horiba QM8000 spectrofluorometer with a Xenon lamp. An excitation wavelength of 300 nm was used for all four powder samples. The luminescence was attenuated by a Neutral Density filter with Optical Density 2 (ND2) in order to prevent saturation of the detector due to the intensity of the luminescence. The lifetimes of the samples were measured using the TCSPC mode of the same instrument and a pulsed diode laser at 377 nm as the excitation source. The CIE 1931 (x, y) chromaticity diagram was plotted using an online interactive CIE 1931 chromaticity diagram application developed by the department of physics at the University of the Free State [56]. Thermogravimetric investigation (TGA) was performed on a Perkin Elmer Pyris 6 TGA from 23 • C up to 900 • C beneath a nitrogen environment (stream rate 20 mL/min) with a warming rate of 10 • C/min. Crystallographic data reported in this article has been deposited with the Cambridge Crystallographic Data Center, under deposition codes 2,270,110 for ImL1, 2,270,107 for ImL2, and 2,270,111 for ZnCl 2 (ImL1) 2 . In a two-necked round-bottom flask containing a mixture of 4-(4-bromophenyl)-1Himidazole 1 (2.15 g, 9.17 mmol), 1-bromooctane 2 (3.4 mL, 19.5 mmol), NaOH (50% in H 2 O, 10 mL, 0.54 mol), and benzyltetraethylammonium chloride (1.43 g, 6.28 mmol), was added toluene (30 mL). After 24 h of heating at 110 • C, the mixture was cooled to room temperature. It was then poured into water and extracted with ethyl acetate after cooling. The organic extracts were dried with anhydrous MgSO 4 after being rinsed with a brine solution. The crude product was separated by silica gel chromatography (eluting with 1% ethyl acetate in a hexane ratio) to give 4-(4-bromophenyl)-1-octyl-1H-imidazole 3 as a white solid (2.77 g, 90%). 1  To this was added water (1 mL), and the reaction mixture was heated to 100 • C for 20 h. The cooled reaction mixture was diluted with water (250 mL), acidified with HCl (2 M), and extracted with ethyl acetate (4 × 100 mL). The organic layer was filtered through celite, dried over MgSO 4 , filtered, and concentrated under reduced pressure to afford brown solids. This solid was purified by column chromatography over silica (eluent: 20-100% (1:9 EtOAc: Hexane)), and clean fractions were combined and concentrated under reduced pressure to give 4 -(1-octyl-1Himidazol-4-yl)-N,N-diphenyl-[1,1 -biphenyl]-4-yl)-4-amine ImL1 as a yellow solid (1.3 g, 49.6% yield). 1   A solution of 4-(4-bromophenyl)-1-octyl-1H-imidazole 3 (3.00 g; 5.97 mmol), 9H-Carbazole-9-(4-phenyl) boronic acid pinacol ester 5 (1.76 g; 5.97 mmol), XPhos Pd G3 (202.29 mg; 0.24 mmol), and potassium carbonate (5.84 g; 17.92 mmol) in anhydrous 1,4-dioxane (60.00 mL) were sonicated under argon for 5 min. To this was added water (1.00 mL), and the reaction mixture was heated to 100 • C for 20 h. The cooled reaction mixture was diluted with water (250 mL), acidified with HCl (2 M), and extracted with ethyl acetate (4 × 100 mL). The organic layer was filtered through celite, dried over MgSO 4 , filtered, and concentrated under reduced pressure to afford brown solids. This solid was purified by column chromatography over silica (eluent: 20-100% (1:9 EtOAc: Hexane)), and clean fractions were combined and concentrated under reduced pressure to give-(4 -(1-octyl-1H-imidazol-4-yl)-[1,1 -biphenyl]-4-yl)-9H-carbazole ImL2 as a pale yellow solid (1.3 g, 49.6% yield). 1  A mixture of zinc (II) chloride (41 mg, 0.30 mmol) and 4-(1-octyl-1H-imidazol-4yl)-N,N-diphenyl-[1,1-biphenyl]-4-yl)-4-Amine ImL1 (300 mg, 0.60 mmol) in methanol (10 mL) was refluxed for 24 h. The reaction mixture was allowed to cool and kept at room temperature for three days. The resulting precipitates were separated by filtration, washed with water (2 × 3 mL), and air dried to obtain the desired novel ZnCl 2 (ImL1) 2 complex as pale yellow solids. Yield: 375 mg, 55% based on ligand ImL1. 1  A mixture of zinc (II) chloride (35 mg, 0.256 mmol) and 9-(4'-(1-octyl-1H-imidazol-4yl)-[1,1'-biphenyl]-4-yl)-9H-carbazole ImL2 (255 mg, 0.512 mmol) in methanol (10 mL) was refluxed for 24 h. The reaction mixture was allowed to cool and kept at room temperature for three days. The resulting precipitates were separated by filtration, washed with water (2 × 3 mL), and air dried to obtain the desired novel ZnCl 2 (ImL2) 2 complex as white solids. Yield: 342 mg, 59% based on ligand ImL2. 1

Conclusions
Two new fluorescent ligands, 4-(1-octyl-1H-imidazol-4-yl)-N,N-diphenyl-[1,1-biphenyl]-4-yl)-4-amine ImL1 and 9-(4 -(1-Octyl-1H-imidazol-4-yl)-[1,1-biphenyl]-4-yl)-9H-carbazole ImL2 were synthesized in 74% and 66% yields, respectively. These ligands were later treated with zinc chloride to give their corresponding zinc (II) chloride complexes, ZnCl 2 (ImL1) 2 and ZnCl 2 (ImL2) 2 , in up to 59% yield. FTIR, 1 H, and 13 C-NMR confirmed the molecular structures of the free ligands and their corresponding Zn (II) complexes. The crystal structure analysis shows that the ImL1 ligand and the ZnCl 2 (ImL1) 2 complex crystallized in triclinic with space groups P-1 and C2, respectively, while the ImL2 ligand crystallized in monoclinic with space group P 21/c. In addition, the ZnCl 2 (ImL1) 2 complex shows a distorted tetrahedron geometry with two coordination sites occupied by the bidentate chelation of two ImL1 ligands through the nitrogen atom of each ligand and the remaining two coordination sites occupied by two chlorine atoms. Both zinc complexes are thermally stable at 341 • C for ZnCl 2 (ImL1) 2 and 365 • C for ZnCl 2 (ImL2) 2 , corresponding to 2% weight loss. Both the free ligands and their complexes display efficient photoluminescence properties in the violet to cyan spectral range from 410 to 488 nm in the solid state at room temperature, with fluorescence decay lifetimes ranging from 1 to 9 nanoseconds, as well as good photoluminescence properties in the UV-A emission area from 345 to 372 nm in ethanol solutions. Because of these potential photophysical features, additional research is being conducted to assess these products as optoelectronic materials.

Data Availability Statement:
The data presented in this study are available on request from the corresponding author.