# A White-Light-Emitting Small Molecule: Synthesis, Crystal Structure, and Optical Properties

Authors: Sin-Kai Fang; Hsing-Yang Tsai; Jiun-Wei Hu; Kew-Yu Chen
Journal: International Journal of Photoenergy
 (2014)

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## Abstract

A white-light-emitting small molecule (1) was synthesized and characterized by single-crystal X-ray diffraction. Compound 1 undergoes an excited-state intramolecular proton transfer (ESIPT) reaction, resulting in a tautomer that is in equilibrium with the normal species and exhibiting a dual emission that covers almost all of the visible spectrum, and consequently generates white light. Furthermore, the geometric structures, the frontier molecular orbitals (MOs), and the potential energy curves for 1 in the ground and the first singlet excited state were fully rationalized by density functional theory (DFT) and time-dependent DFT calculations. The results show that the forward ESIPT and backward ESIPT may happen on the same timescale, enabling the excited-state equilibrium to be established.


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## Body

## 1. Introduction

Organic fluorescent molecules with excited-state intramolecular proton transfer (ESIPT) characteristics have been constantly drawing significant attention due to their peculiar optical properties [1–6]. An ESIPT reaction commonly involves the transfer of a hydroxyl (amino) proton to an acceptor such as imine nitrogen (carbonyl oxygen) through a preexisting hydrogen bonding configuration [7–9]. As shown in Figure 1, molecules that exhibit ESIPT in the ground state exist predominantly as enol (E) forms; however, upon photoexcitation, they undergo tautomerization into keto forms (E*→K*) via an ultrafast and irreversible ESIPT process occurring in the subpicosecond time domain [10]. The resulting proton-transfer tautomer is substantially different in structure and electronic configuration from its corresponding ground state, that is, a large Stokes shifted K*→K emission. This unusual optical property has many practical applications, typical examples of which are probes for solvation dynamics [11, 12] and biological environments [13, 14], photochromic materials [15], fluorescence microscopy imaging [16], chemosensors [17–20], near-infrared fluorescent dyes [21], nonlinear optical materials [22], and organic light emitting diodes (OLEDs) [23–25].Figure 1
Characteristic four-level photocycle scheme of the ESIPT process.Attempts at exploiting single-molecule-based white-light-emitting ESIPT chromophores as the white lighting materials have recently been an important issue of research, since the use of a single molecule can provide easy fabrication with perfect color reproducibility and stability [26, 27]. In 2009, Park and coworkers synthesized and characterized, for the first time, a white-light-emitting single molecule dyad, consisting of two noninteracting chromophores showing ESIPT [28]. Later in 2011, we paved a new and feasible avenue en route to white light generation based on a single ESIPT system [29]. Taking advantage of an adiabatic ESIPT reaction, we were able to show that broad blue emission from the excited starting material and broad red emission from an ESIPT molecule2 (Scheme 1) combined to generate white light as if there were two molecules present in the sample. However, due to its relatively low overall fluorescence quantum yield, the electroluminescent performance using2 as an active layer is only decent compared with the work mentioned early utilizing multi-ESIPT moieties [28, 30]. To expand the scope of the2-based chromophores available for designing systems for high performance single-molecule-based white-light-emitting OLEDs, the present research reports the synthesis of a new derivative of2with atert-butyl moiety attached to the naphthalene ring, that is, 8-tert-butyl-1-hydroxy-11H-benzo[b]fluoren-11-one (1).Its X-ray structure, as well as optical and electrochemical properties, and complementary time-dependent density functional theory (TD-DFT) calculations are also studied.Scheme 1
The synthetic route of1.


## 2. Experimental

### 2.1. Chemicals and Instruments

The starting materials such as 7-methoxy-2,3-dihydro-1H-inden-1-one (6),N-bromosuccinimide (NBS), 2,2′-azobisisobutyronitrile (AIBN), triethylamine, α,α,α′α′-tetrabromo-o-xylene, sodium iodide, boron tribromide,tert-butyl chloride, and aluminum trichloride were purchased from Merck, ACROS, and Sigma-Aldrich. Solvents were distilled freshly according to standard procedure. Column chromatography was performed using silica gel Merck Kieselgelsi 60 (40–63 mesh).1H NMR spectra were recorded in CDCl3 on a Bruker 400 MHz spectrometer. Mass spectra were recorded on a VG70-250S mass spectrometer. The absorption and emission spectra were measured using a Jasco V-570 UV-Vis spectrophotometer and a Hitachi F-4500 fluorescence spectrophotometer, respectively. The single-crystal X-ray diffraction data were collected on a Bruker Smart 1000 CCD area-detector diffractometer. The redox potentials were measured using cyclic voltammetry on a CHI 620 analyzer. The data were collected and analyzed using electrochemical analysis software. All measurements were carried out in dichloromethane containing 0.1 M tetrabutylammonium hexafluorophosphate (TBAPF6) as the supporting electrolyte under ambient conditions after purging for 15 min with N2. The conventional three-electrode configuration was employed, which consisted of a glassy-carbon working electrode, a platinum counter electrode, and a Ag/AgNO3 (0.1 M) reference electrode calibrated with ferrocene/ferrocenium (Fc/Fc+) as an internal reference.


### 2.2. Synthesis and Characterization

#### 2.2.1. Synthesis of 3-Bromo-7-methoxy-2,3-dihydro-1H-inden-1-one (5)

7-Methoxy-2,3-dihydro-1H-inden-1-one (1.0 g, 6.2 mmol) andN-bromosuccinimide (1.2 g, 6.8 mmol) were dissolved in 20 mL of CCl4 and 12 mg (1 mol%) of 2,2′-azobisisobutyronitrile (AIBN) was added. The mixture was slowly stirred and heated to 80°C for 2 hours. After cooling, the mixture was poured into cold water, extracted with CH2Cl2, and dried with anhydrous MgSO4. After the solvent was removed, the crude product was purified by silica gel column chromatography with eluent ethyl acetate/n-hexane (1/4) to afford5 (1.1 g, 74%). 1H NMR (CDCl3, ppm) 7.62 (t,J = 8.5 Hz, 1H), 7.20 (d,J = 8.0 Hz, 1H), 6.87 (d,J = 8.5 Hz, 1H), 5.52 (dd, J1 = 7.0 Hz, J2 = 2.0 Hz, 1H), 3.92 (s, 3H), 3.32 (dd, J1 = 18.5 Hz, J2 = 7.0 Hz, 1H), 2.97 (dd, J1 = 18.5 Hz, J2 = 2.0 Hz, 1H); MS (FAB) m/z 240 (M + H)+. HRMS calcd. for C10H10BrO2 240.9864, found 240.9866.


#### 2.2.2. Synthesis of 7-Methoxy-1H-inden-1-one (4)

3-Bromo-7-methoxy-2,3-dihydro-1H-inden-1-one (1.0 g, 4.1 mmol) in CCl4 was cooled in an ice bath, and 1.93 mL (1.4 g, 14.0 mmol) of triethylamine was added slowly. The reaction mixture was allowed to warm to room temperature and stir overnight. After the solvent was removed, the crude product was purified by silica gel column chromatography with eluent ethyl acetate/n-hexane (1/4) to afford4 (0.63 g, 95%). 1H NMR (CDCl3, ppm) 7.42 (d,J = 6.0 Hz, 1H), 7.34 (t,J = 8.0 Hz, 1H), 6.85 (d,J = 8.8 Hz, 1H), 6.70 (d,J = 8.0 Hz, 1H), 5.84 (d,J = 6.0 Hz, 1H), 3.95 (s, 3H); 13C NMR (100 MHz, CDCl3, ppm) 196.57, 156.50, 147.38, 147.03, 144.48, 136.02, 127.70, 115.65, 114.67, 55.89; MS (FAB) m/z 161 (M + H)+. HRMS calcd. for C10H9O2 161.0603, found 161.0608.


#### 2.2.3. Synthesis of 7-Methoxy-1H-inden-1-one (3)

A mixture of solution ofα,α,α′α′-tetrabromo-o-xylene (1.3 g, 3.1 mmol), 7-methoxy-1H-inden-1-one (0.5 g, 3.1 mmol), sodium iodide (1.8 g, 12 mmol), and dry DMF (30 mL) was stirred at 65°C for 24 hours. The reaction mixture was poured into cold water (70 mL) containing sodium bisulfite (1.0 g). The yellow precipitate was purified by silica gel column chromatography with eluent ethyl acetate/n-hexane (1/4) to afford3 (0.73 g, 90%). 1H NMR (CDCl3, ppm) 8.14 (s, 1H), 7.79~7.88 (m, 3H), 7.43~7.54 (m, 3H), 7.31 (d,J = 7.6 Hz, 1H), 6.85 (d,J = 8.4 Hz, 1H), 3.99 (s, 3H); 13C NMR (100 MHz, CDCl3, ppm) 191.06, 158.54, 146.83, 137.56, 136.96, 136.50, 133.76, 133.10, 130.58, 128.68, 128.59, 126.78, 125.01, 122.74, 119.03, 113.26, 112.37, 55.89; MS (FAB) m/z 261 (M + H)+. HRMS calcd. for C18H13O2 261.0916, found 261.0918.


#### 2.2.4. Synthesis of 1-Hydroxy-11H-benzo[b]fluoren-11-one (2)

1-Methoxy-11H-benzo[b]fluoren-11-one (300 mg, 1.1 mmol) was dissolved in 10 mL of dichloromethane in a 50 mL round-bottom flask, and the flask was placed in an ice bath at 0°C. A solution of boron tribromide (0.25 mL, 1.0 M solution in dichloromethane) was added carefully to the stirred solution under a nitrogen atmosphere. After 4 hours, the reaction was cooled and the reaction mixture was then hydrolyzed by carefully shaking it with 10 mL of water and extracted twice with 10 mL of dichloromethane. The combined organic phases were then dried over magnesium sulfate, filtered, and evaporatedin vacuo; the crude product was purified by silica gel column chromatography with eluent ethyl acetate/n-hexane (1/10) to afford2 (269 mg, 95%). 1H NMR (CDCl3, ppm) 8.64 (s, 1H), 8.07 (s, 1H), 7.84 (d,J = 7.5 Hz, 1H), 7.78 (s, 1H), 7.77 (d,J = 9.0 Hz, 1H), 7.54 (t,J = 7.5 Hz, 1H), 7.38~7.46 (m, 2H), 7.15 (d,J = 7.0 Hz, 1H), 6.76 (d,J = 8.0 Hz, 1H); 13C NMR (100 MHz, CDCl3, ppm) 195.51, 157.66, 144.25, 137.99, 137.81, 136.74, 133.41, 132.68, 130.78, 129.13, 128.85, 127.08, 125.54, 120.16, 120.01, 117.40, 113.00; MS (FAB) m/z 247 (M + H)+. HRMS calcd. for C17H11O2 247.0759, found 247.0755.


#### 2.2.5. Synthesis of 8-tert-Butyl-1-hydroxy-11H-benzo[b]fluoren-11-one (1)

1-Hydroxy-11H-benzo[b]fluoren-11-one (200 mg, 0.8 mmol) was added totert-butyl chloride (5 mL). The flask was kept at 0°C with an ice bath and all inlets were protected by drying tubes. Anhydrous aluminum chloride (280 mg, 2.1 mmol) was added dropwise over 1 h and the mixture was allowed to stir for another hour. H2O (20 mL) was added to the flask and the mixture was allowed to stir for 10 min. The mixture was extracted with dichloromethane and dried with magnesium sulfate; the crude product was purified by silica gel column chromatography with eluent ethyl acetate/n-hexane (1/8) to afford1 (208 mg, 85%). Yellow parallelepiped-shaped crystals suitable for the crystallographic studies reported here were isolated over a period of six weeks by slow evaporation from a dichloromethane solution. 1H NMR (CDCl3, ppm) 8.68 (s, 1H), 8.11 (s, 1H), 7.81 (s, 2H), 7.77 (d,J = 8.0 Hz, 1H), 7.64 (d,J = 8.0 Hz, 1H), 7.43 (t,J = 8.0 Hz, 1H), 7.18 (d,J = 8.0 Hz, 1H), 6.77 (d,J = 8.0 Hz, 1H), 1.40 (s, 9H); 13C NMR (100 MHz, CDCl3, ppm) 195.7, 157.7, 150.2, 144.5, 137.7, 137.6, 134.9, 133.5, 132.7, 128.6, 128.0, 126.2, 125.7, 120.2, 119.6, 117.2, 112.9, 34.9, 31.1; MS (FAB) m/z 303 (M + H)+. HRMS calcd. for C21H19O2 303.1385, found 303.1389.


#### 2.2.6. Crystal Structural Determination

A single crystal of1 with dimensions of 0.41 mm × 0.39 mm × 0.10 mm was selected. The lattice constants and diffraction intensities were measured with a Bruker Smart 1000 CCD area detector radiation (λ=0.71073 Å) at 297(2) K. An ω-2θ scan mode was used for data collection in the range of 2.38≦θ≦26.36°. A total of 19859 reflections were collected and 3158 were independent (Rint⁡=0.0320), of which 2455 were considered to be observed with I>2σ(I) and used in the succeeding refinement. The structure was solved by direct methods with SHELXS-97 [31] and refined on F2 by full-matrix least-squares procedure with Bruker SHELXL-97 packing [32]. All nonhydrogen atoms were refined with anisotropic thermal parameters. The hydrogen atoms refined with riding model position parameters isotropically were located from difference Fourier map and added theoretically. At the final cycle of refinement, R=0.0488 and wR=0.1163(w=1/[σ2(Fo2)+(0.0551P)2+0.6249P], where P=(Fo2+2Fc2)/3), S=1.028, (Δ/σ)max⁡=0.002, (Δ/ρ)max⁡=0.162, and (Δ/ρ)min⁡=-0.191 e/Å3.


### 2.3. Computational Methods

The Gaussian 03 program was used to perform theab initio calculation on the molecular structure [33]. Full geometry optimizations of compound1 were carried out with the 6-31G** basis set to the B3LYP functional. The hybrid DFT functional B3LYP has proven to be a suitable DFT functional to describe hydrogen bond [34]. Vibrational frequencies were also performed to check whether the optimized geometrical structures for1 were at energy minima, transition states, or higher order saddle points. After obtaining the converged geometries, the TD-B3LYP/6-31G** was used to calculate the vertical excitation energies. Emission energies were obtained from TD-DFT/B3LYP/6-31G** calculations performed on S1 optimized geometries. The phenomenon of photoinduced proton transfer (PT) reaction in1 can be most critically addressed and assessed by evaluating the potential energy curve (PEC) for the PT reaction. For the S0 state all of the other degrees of freedom are relaxed without imposing any symmetry constraints. The excited-state (S1) PEC for the ESIPT reaction in1 has been constructed on the basis of TD-DFT optimization method.


## 2.1. Chemicals and Instruments

The starting materials such as 7-methoxy-2,3-dihydro-1H-inden-1-one (6),N-bromosuccinimide (NBS), 2,2′-azobisisobutyronitrile (AIBN), triethylamine, α,α,α′α′-tetrabromo-o-xylene, sodium iodide, boron tribromide,tert-butyl chloride, and aluminum trichloride were purchased from Merck, ACROS, and Sigma-Aldrich. Solvents were distilled freshly according to standard procedure. Column chromatography was performed using silica gel Merck Kieselgelsi 60 (40–63 mesh).1H NMR spectra were recorded in CDCl3 on a Bruker 400 MHz spectrometer. Mass spectra were recorded on a VG70-250S mass spectrometer. The absorption and emission spectra were measured using a Jasco V-570 UV-Vis spectrophotometer and a Hitachi F-4500 fluorescence spectrophotometer, respectively. The single-crystal X-ray diffraction data were collected on a Bruker Smart 1000 CCD area-detector diffractometer. The redox potentials were measured using cyclic voltammetry on a CHI 620 analyzer. The data were collected and analyzed using electrochemical analysis software. All measurements were carried out in dichloromethane containing 0.1 M tetrabutylammonium hexafluorophosphate (TBAPF6) as the supporting electrolyte under ambient conditions after purging for 15 min with N2. The conventional three-electrode configuration was employed, which consisted of a glassy-carbon working electrode, a platinum counter electrode, and a Ag/AgNO3 (0.1 M) reference electrode calibrated with ferrocene/ferrocenium (Fc/Fc+) as an internal reference.


## 2.2. Synthesis and Characterization

### 2.2.1. Synthesis of 3-Bromo-7-methoxy-2,3-dihydro-1H-inden-1-one (5)

7-Methoxy-2,3-dihydro-1H-inden-1-one (1.0 g, 6.2 mmol) andN-bromosuccinimide (1.2 g, 6.8 mmol) were dissolved in 20 mL of CCl4 and 12 mg (1 mol%) of 2,2′-azobisisobutyronitrile (AIBN) was added. The mixture was slowly stirred and heated to 80°C for 2 hours. After cooling, the mixture was poured into cold water, extracted with CH2Cl2, and dried with anhydrous MgSO4. After the solvent was removed, the crude product was purified by silica gel column chromatography with eluent ethyl acetate/n-hexane (1/4) to afford5 (1.1 g, 74%). 1H NMR (CDCl3, ppm) 7.62 (t,J = 8.5 Hz, 1H), 7.20 (d,J = 8.0 Hz, 1H), 6.87 (d,J = 8.5 Hz, 1H), 5.52 (dd, J1 = 7.0 Hz, J2 = 2.0 Hz, 1H), 3.92 (s, 3H), 3.32 (dd, J1 = 18.5 Hz, J2 = 7.0 Hz, 1H), 2.97 (dd, J1 = 18.5 Hz, J2 = 2.0 Hz, 1H); MS (FAB) m/z 240 (M + H)+. HRMS calcd. for C10H10BrO2 240.9864, found 240.9866.


### 2.2.2. Synthesis of 7-Methoxy-1H-inden-1-one (4)

3-Bromo-7-methoxy-2,3-dihydro-1H-inden-1-one (1.0 g, 4.1 mmol) in CCl4 was cooled in an ice bath, and 1.93 mL (1.4 g, 14.0 mmol) of triethylamine was added slowly. The reaction mixture was allowed to warm to room temperature and stir overnight. After the solvent was removed, the crude product was purified by silica gel column chromatography with eluent ethyl acetate/n-hexane (1/4) to afford4 (0.63 g, 95%). 1H NMR (CDCl3, ppm) 7.42 (d,J = 6.0 Hz, 1H), 7.34 (t,J = 8.0 Hz, 1H), 6.85 (d,J = 8.8 Hz, 1H), 6.70 (d,J = 8.0 Hz, 1H), 5.84 (d,J = 6.0 Hz, 1H), 3.95 (s, 3H); 13C NMR (100 MHz, CDCl3, ppm) 196.57, 156.50, 147.38, 147.03, 144.48, 136.02, 127.70, 115.65, 114.67, 55.89; MS (FAB) m/z 161 (M + H)+. HRMS calcd. for C10H9O2 161.0603, found 161.0608.


### 2.2.3. Synthesis of 7-Methoxy-1H-inden-1-one (3)

A mixture of solution ofα,α,α′α′-tetrabromo-o-xylene (1.3 g, 3.1 mmol), 7-methoxy-1H-inden-1-one (0.5 g, 3.1 mmol), sodium iodide (1.8 g, 12 mmol), and dry DMF (30 mL) was stirred at 65°C for 24 hours. The reaction mixture was poured into cold water (70 mL) containing sodium bisulfite (1.0 g). The yellow precipitate was purified by silica gel column chromatography with eluent ethyl acetate/n-hexane (1/4) to afford3 (0.73 g, 90%). 1H NMR (CDCl3, ppm) 8.14 (s, 1H), 7.79~7.88 (m, 3H), 7.43~7.54 (m, 3H), 7.31 (d,J = 7.6 Hz, 1H), 6.85 (d,J = 8.4 Hz, 1H), 3.99 (s, 3H); 13C NMR (100 MHz, CDCl3, ppm) 191.06, 158.54, 146.83, 137.56, 136.96, 136.50, 133.76, 133.10, 130.58, 128.68, 128.59, 126.78, 125.01, 122.74, 119.03, 113.26, 112.37, 55.89; MS (FAB) m/z 261 (M + H)+. HRMS calcd. for C18H13O2 261.0916, found 261.0918.


### 2.2.4. Synthesis of 1-Hydroxy-11H-benzo[b]fluoren-11-one (2)

1-Methoxy-11H-benzo[b]fluoren-11-one (300 mg, 1.1 mmol) was dissolved in 10 mL of dichloromethane in a 50 mL round-bottom flask, and the flask was placed in an ice bath at 0°C. A solution of boron tribromide (0.25 mL, 1.0 M solution in dichloromethane) was added carefully to the stirred solution under a nitrogen atmosphere. After 4 hours, the reaction was cooled and the reaction mixture was then hydrolyzed by carefully shaking it with 10 mL of water and extracted twice with 10 mL of dichloromethane. The combined organic phases were then dried over magnesium sulfate, filtered, and evaporatedin vacuo; the crude product was purified by silica gel column chromatography with eluent ethyl acetate/n-hexane (1/10) to afford2 (269 mg, 95%). 1H NMR (CDCl3, ppm) 8.64 (s, 1H), 8.07 (s, 1H), 7.84 (d,J = 7.5 Hz, 1H), 7.78 (s, 1H), 7.77 (d,J = 9.0 Hz, 1H), 7.54 (t,J = 7.5 Hz, 1H), 7.38~7.46 (m, 2H), 7.15 (d,J = 7.0 Hz, 1H), 6.76 (d,J = 8.0 Hz, 1H); 13C NMR (100 MHz, CDCl3, ppm) 195.51, 157.66, 144.25, 137.99, 137.81, 136.74, 133.41, 132.68, 130.78, 129.13, 128.85, 127.08, 125.54, 120.16, 120.01, 117.40, 113.00; MS (FAB) m/z 247 (M + H)+. HRMS calcd. for C17H11O2 247.0759, found 247.0755.


### 2.2.5. Synthesis of 8-tert-Butyl-1-hydroxy-11H-benzo[b]fluoren-11-one (1)

1-Hydroxy-11H-benzo[b]fluoren-11-one (200 mg, 0.8 mmol) was added totert-butyl chloride (5 mL). The flask was kept at 0°C with an ice bath and all inlets were protected by drying tubes. Anhydrous aluminum chloride (280 mg, 2.1 mmol) was added dropwise over 1 h and the mixture was allowed to stir for another hour. H2O (20 mL) was added to the flask and the mixture was allowed to stir for 10 min. The mixture was extracted with dichloromethane and dried with magnesium sulfate; the crude product was purified by silica gel column chromatography with eluent ethyl acetate/n-hexane (1/8) to afford1 (208 mg, 85%). Yellow parallelepiped-shaped crystals suitable for the crystallographic studies reported here were isolated over a period of six weeks by slow evaporation from a dichloromethane solution. 1H NMR (CDCl3, ppm) 8.68 (s, 1H), 8.11 (s, 1H), 7.81 (s, 2H), 7.77 (d,J = 8.0 Hz, 1H), 7.64 (d,J = 8.0 Hz, 1H), 7.43 (t,J = 8.0 Hz, 1H), 7.18 (d,J = 8.0 Hz, 1H), 6.77 (d,J = 8.0 Hz, 1H), 1.40 (s, 9H); 13C NMR (100 MHz, CDCl3, ppm) 195.7, 157.7, 150.2, 144.5, 137.7, 137.6, 134.9, 133.5, 132.7, 128.6, 128.0, 126.2, 125.7, 120.2, 119.6, 117.2, 112.9, 34.9, 31.1; MS (FAB) m/z 303 (M + H)+. HRMS calcd. for C21H19O2 303.1385, found 303.1389.


### 2.2.6. Crystal Structural Determination

A single crystal of1 with dimensions of 0.41 mm × 0.39 mm × 0.10 mm was selected. The lattice constants and diffraction intensities were measured with a Bruker Smart 1000 CCD area detector radiation (λ=0.71073 Å) at 297(2) K. An ω-2θ scan mode was used for data collection in the range of 2.38≦θ≦26.36°. A total of 19859 reflections were collected and 3158 were independent (Rint⁡=0.0320), of which 2455 were considered to be observed with I>2σ(I) and used in the succeeding refinement. The structure was solved by direct methods with SHELXS-97 [31] and refined on F2 by full-matrix least-squares procedure with Bruker SHELXL-97 packing [32]. All nonhydrogen atoms were refined with anisotropic thermal parameters. The hydrogen atoms refined with riding model position parameters isotropically were located from difference Fourier map and added theoretically. At the final cycle of refinement, R=0.0488 and wR=0.1163(w=1/[σ2(Fo2)+(0.0551P)2+0.6249P], where P=(Fo2+2Fc2)/3), S=1.028, (Δ/σ)max⁡=0.002, (Δ/ρ)max⁡=0.162, and (Δ/ρ)min⁡=-0.191 e/Å3.


## 2.2.1. Synthesis of 3-Bromo-7-methoxy-2,3-dihydro-1H-inden-1-one (5)

7-Methoxy-2,3-dihydro-1H-inden-1-one (1.0 g, 6.2 mmol) andN-bromosuccinimide (1.2 g, 6.8 mmol) were dissolved in 20 mL of CCl4 and 12 mg (1 mol%) of 2,2′-azobisisobutyronitrile (AIBN) was added. The mixture was slowly stirred and heated to 80°C for 2 hours. After cooling, the mixture was poured into cold water, extracted with CH2Cl2, and dried with anhydrous MgSO4. After the solvent was removed, the crude product was purified by silica gel column chromatography with eluent ethyl acetate/n-hexane (1/4) to afford5 (1.1 g, 74%). 1H NMR (CDCl3, ppm) 7.62 (t,J = 8.5 Hz, 1H), 7.20 (d,J = 8.0 Hz, 1H), 6.87 (d,J = 8.5 Hz, 1H), 5.52 (dd, J1 = 7.0 Hz, J2 = 2.0 Hz, 1H), 3.92 (s, 3H), 3.32 (dd, J1 = 18.5 Hz, J2 = 7.0 Hz, 1H), 2.97 (dd, J1 = 18.5 Hz, J2 = 2.0 Hz, 1H); MS (FAB) m/z 240 (M + H)+. HRMS calcd. for C10H10BrO2 240.9864, found 240.9866.


## 2.2.2. Synthesis of 7-Methoxy-1H-inden-1-one (4)

3-Bromo-7-methoxy-2,3-dihydro-1H-inden-1-one (1.0 g, 4.1 mmol) in CCl4 was cooled in an ice bath, and 1.93 mL (1.4 g, 14.0 mmol) of triethylamine was added slowly. The reaction mixture was allowed to warm to room temperature and stir overnight. After the solvent was removed, the crude product was purified by silica gel column chromatography with eluent ethyl acetate/n-hexane (1/4) to afford4 (0.63 g, 95%). 1H NMR (CDCl3, ppm) 7.42 (d,J = 6.0 Hz, 1H), 7.34 (t,J = 8.0 Hz, 1H), 6.85 (d,J = 8.8 Hz, 1H), 6.70 (d,J = 8.0 Hz, 1H), 5.84 (d,J = 6.0 Hz, 1H), 3.95 (s, 3H); 13C NMR (100 MHz, CDCl3, ppm) 196.57, 156.50, 147.38, 147.03, 144.48, 136.02, 127.70, 115.65, 114.67, 55.89; MS (FAB) m/z 161 (M + H)+. HRMS calcd. for C10H9O2 161.0603, found 161.0608.


## 2.2.3. Synthesis of 7-Methoxy-1H-inden-1-one (3)

A mixture of solution ofα,α,α′α′-tetrabromo-o-xylene (1.3 g, 3.1 mmol), 7-methoxy-1H-inden-1-one (0.5 g, 3.1 mmol), sodium iodide (1.8 g, 12 mmol), and dry DMF (30 mL) was stirred at 65°C for 24 hours. The reaction mixture was poured into cold water (70 mL) containing sodium bisulfite (1.0 g). The yellow precipitate was purified by silica gel column chromatography with eluent ethyl acetate/n-hexane (1/4) to afford3 (0.73 g, 90%). 1H NMR (CDCl3, ppm) 8.14 (s, 1H), 7.79~7.88 (m, 3H), 7.43~7.54 (m, 3H), 7.31 (d,J = 7.6 Hz, 1H), 6.85 (d,J = 8.4 Hz, 1H), 3.99 (s, 3H); 13C NMR (100 MHz, CDCl3, ppm) 191.06, 158.54, 146.83, 137.56, 136.96, 136.50, 133.76, 133.10, 130.58, 128.68, 128.59, 126.78, 125.01, 122.74, 119.03, 113.26, 112.37, 55.89; MS (FAB) m/z 261 (M + H)+. HRMS calcd. for C18H13O2 261.0916, found 261.0918.


## 2.2.4. Synthesis of 1-Hydroxy-11H-benzo[b]fluoren-11-one (2)

1-Methoxy-11H-benzo[b]fluoren-11-one (300 mg, 1.1 mmol) was dissolved in 10 mL of dichloromethane in a 50 mL round-bottom flask, and the flask was placed in an ice bath at 0°C. A solution of boron tribromide (0.25 mL, 1.0 M solution in dichloromethane) was added carefully to the stirred solution under a nitrogen atmosphere. After 4 hours, the reaction was cooled and the reaction mixture was then hydrolyzed by carefully shaking it with 10 mL of water and extracted twice with 10 mL of dichloromethane. The combined organic phases were then dried over magnesium sulfate, filtered, and evaporatedin vacuo; the crude product was purified by silica gel column chromatography with eluent ethyl acetate/n-hexane (1/10) to afford2 (269 mg, 95%). 1H NMR (CDCl3, ppm) 8.64 (s, 1H), 8.07 (s, 1H), 7.84 (d,J = 7.5 Hz, 1H), 7.78 (s, 1H), 7.77 (d,J = 9.0 Hz, 1H), 7.54 (t,J = 7.5 Hz, 1H), 7.38~7.46 (m, 2H), 7.15 (d,J = 7.0 Hz, 1H), 6.76 (d,J = 8.0 Hz, 1H); 13C NMR (100 MHz, CDCl3, ppm) 195.51, 157.66, 144.25, 137.99, 137.81, 136.74, 133.41, 132.68, 130.78, 129.13, 128.85, 127.08, 125.54, 120.16, 120.01, 117.40, 113.00; MS (FAB) m/z 247 (M + H)+. HRMS calcd. for C17H11O2 247.0759, found 247.0755.


## 2.2.5. Synthesis of 8-tert-Butyl-1-hydroxy-11H-benzo[b]fluoren-11-one (1)

1-Hydroxy-11H-benzo[b]fluoren-11-one (200 mg, 0.8 mmol) was added totert-butyl chloride (5 mL). The flask was kept at 0°C with an ice bath and all inlets were protected by drying tubes. Anhydrous aluminum chloride (280 mg, 2.1 mmol) was added dropwise over 1 h and the mixture was allowed to stir for another hour. H2O (20 mL) was added to the flask and the mixture was allowed to stir for 10 min. The mixture was extracted with dichloromethane and dried with magnesium sulfate; the crude product was purified by silica gel column chromatography with eluent ethyl acetate/n-hexane (1/8) to afford1 (208 mg, 85%). Yellow parallelepiped-shaped crystals suitable for the crystallographic studies reported here were isolated over a period of six weeks by slow evaporation from a dichloromethane solution. 1H NMR (CDCl3, ppm) 8.68 (s, 1H), 8.11 (s, 1H), 7.81 (s, 2H), 7.77 (d,J = 8.0 Hz, 1H), 7.64 (d,J = 8.0 Hz, 1H), 7.43 (t,J = 8.0 Hz, 1H), 7.18 (d,J = 8.0 Hz, 1H), 6.77 (d,J = 8.0 Hz, 1H), 1.40 (s, 9H); 13C NMR (100 MHz, CDCl3, ppm) 195.7, 157.7, 150.2, 144.5, 137.7, 137.6, 134.9, 133.5, 132.7, 128.6, 128.0, 126.2, 125.7, 120.2, 119.6, 117.2, 112.9, 34.9, 31.1; MS (FAB) m/z 303 (M + H)+. HRMS calcd. for C21H19O2 303.1385, found 303.1389.


## 2.2.6. Crystal Structural Determination

A single crystal of1 with dimensions of 0.41 mm × 0.39 mm × 0.10 mm was selected. The lattice constants and diffraction intensities were measured with a Bruker Smart 1000 CCD area detector radiation (λ=0.71073 Å) at 297(2) K. An ω-2θ scan mode was used for data collection in the range of 2.38≦θ≦26.36°. A total of 19859 reflections were collected and 3158 were independent (Rint⁡=0.0320), of which 2455 were considered to be observed with I>2σ(I) and used in the succeeding refinement. The structure was solved by direct methods with SHELXS-97 [31] and refined on F2 by full-matrix least-squares procedure with Bruker SHELXL-97 packing [32]. All nonhydrogen atoms were refined with anisotropic thermal parameters. The hydrogen atoms refined with riding model position parameters isotropically were located from difference Fourier map and added theoretically. At the final cycle of refinement, R=0.0488 and wR=0.1163(w=1/[σ2(Fo2)+(0.0551P)2+0.6249P], where P=(Fo2+2Fc2)/3), S=1.028, (Δ/σ)max⁡=0.002, (Δ/ρ)max⁡=0.162, and (Δ/ρ)min⁡=-0.191 e/Å3.


## 2.3. Computational Methods

The Gaussian 03 program was used to perform theab initio calculation on the molecular structure [33]. Full geometry optimizations of compound1 were carried out with the 6-31G** basis set to the B3LYP functional. The hybrid DFT functional B3LYP has proven to be a suitable DFT functional to describe hydrogen bond [34]. Vibrational frequencies were also performed to check whether the optimized geometrical structures for1 were at energy minima, transition states, or higher order saddle points. After obtaining the converged geometries, the TD-B3LYP/6-31G** was used to calculate the vertical excitation energies. Emission energies were obtained from TD-DFT/B3LYP/6-31G** calculations performed on S1 optimized geometries. The phenomenon of photoinduced proton transfer (PT) reaction in1 can be most critically addressed and assessed by evaluating the potential energy curve (PEC) for the PT reaction. For the S0 state all of the other degrees of freedom are relaxed without imposing any symmetry constraints. The excited-state (S1) PEC for the ESIPT reaction in1 has been constructed on the basis of TD-DFT optimization method.


## 3. Results and Discussion

### 3.1. Synthesis and Characterization

Scheme1 shows the chemical structure and the synthetic route of1. The synthesis of1 started from a conventional bromination of 7-methoxy-2,3-dihydro-1H-inden-1-one (6), followed by the elimination of the bromo adduct (5), giving a reactive dienophile4. The naphthalene moiety can then be fused onto the C(2)–C(3) double bond by placing4 through a reaction with α,α,α′α′-tetrabromo-o-xylene [29], yielding3. Subsequently, compound3 was subjected to the deprotection with BBr3 to give2. Finally, the fried-craft alkylation at the 8-position of2 was carried out by the reaction of2 withtert-butyl chloride and aluminum trichloride, giving1 with an overall product yield of 51%. The presence of a singletert-butyl substituent of1 can be verified by the presence of a signal at δ 1.40 ppm (9H) and eight signals at δ 6.7–8.1 ppm (8H) in the 1H NMR spectrum.


### 3.2. Hydrogen Bond Studies

The dominance of an enol-normal form for1, namely, the intramolecular hydrogen-bond formation between O(1)–H and O(2), is firmly supported by a combination of 1H NMR and X-ray single-crystal analyses (Figure 2). In the 1H NMR studies, the existence of an intramolecular hydrogen bond between O(1)–H and O(2) is evidenced by the observation of a substantial downfield shift of the proton peak at 8.68 ppm (in CDCl3). The hydrogen bonding energy (ΔE in kcal/mol) can be empirically calculated by introducing Schaefer’s correlation [35], expressed as Δδ=(-0.4±0.2)+ΔE, where Δδ is given in parts per million for the difference between chemical shift in the O–H peak of1and that in phenol (δ 4.29). Accordingly, the hydrogen-bonding energy is calculated to be 4.79±0.2 kcal/mol and is in good agreement with the theoretical calculations (6.27 kcal/mol). Note that compound1 has a weaker intramolecular hydrogen bond than most other ESIPT molecules [36, 37], which may account for its unique dual emission feature (vide infra).Figure 2
Displacement ellipsoid representation of1with the labelling scheme. The ellipsoids are drawn at the 50% probability level and the H atoms are drawn as spheres of arbitrary radii. The blue dashed line denotes the intramolecular hydrogen bond.


### 3.3. X-Ray Structures

The structure of1was further confirmed by single-crystal X-ray diffraction analysis. Compound1 crystallizes in the monoclinic space groupP21/c, witha = 15.7248(9),b = 6.0166(3),c = 17.5500(8) Å, α = 90°, β = 110.515(2)°, and γ = 90°. As shown in Figure 2, the molecular structure of1 is nearly planar (except fortert-butyl group), which is also confirmed by geometry optimization in our DFT calculation (Table 1 and Figure 4). This, together with 2.919 Å of O(1)–O(2) distance, supports the existence of a six-membered-ring intramolecular hydrogen bond. Additionally, the longer O(1)–O(2) distance in1than that (O(1)–O(2) < 2.7 Å) in most other ESIPT molecules [36, 37]supports that compound1has a weaker intramolecular hydrogen bond. This is possible due to the fact that the carbonyl oxygen O(2) locates at the five-membered-ring cyclopenta-2,4-dienone moiety (Figure 2), such that the ∠O(1)–H–O(2) angle is expected to be deviated from 120°, a perfect six-member-ring hydrogen bonding formation. This viewpoint is confirmed by the ∠O(1)–H–O(2) angle of 144.8°, according to the X-ray structure analysis. Careful examination of the crystal structure also indicates that there is no substantial π-π stacking between the tetracyclic plane and its adjacent one. Thus, we can ascertain that thetert-butyl group not only largely increases the solubility of1 compared with2 but also reduces intermolecular contact and aggregation.Table 1
Comparison of the experimental and optimized geometric parameters of1.
X-ray
DFT
Bond lengths (Å)
C(1)–O(1)
1.357(2)
1.348
C(7)–O(2)
1.222(2)
1.233
C(1)–C(2)
1.390(3)
1.407
C(3)–C(4)
1.396(3)
1.409
C(4)–C(5)
1.376(2)
1.387
C(5)–C(6)
1.399(2)
1.409
C(7)–C(8)
1.495(2)
1.492
C(9)–C(10)
1.361(2)
1.370
C(11)–C(12)
1.426(2)
1.433
C(15)–C(16)
1.419(2)
1.423
C(18)–C(19)
1.538(3)
1.539
Bond angles (°)
O(1)–C(1)–C(6)
121.7(2)
121.3
C(6)–C(1)–C(2)
118.1(2)
117.8
C(4)–C(5)–C(6)
120.3(2)
119.6
C(7)–C(8)–C(9)
108.1(2)
108.3
C(10)–C(11)–C(12)
119.9(2)
120.1
C(14)–C(15)–C(16)
117.0(2)
117.2
C(10)–C(11)–C(17)
122.3(2)
122.1
C(15)–C(18)–C(19)
111.5(2)
109.4
Torsion angles (°)
O(1)–C(1)–C(2)–C(3)
−178.8(2)
−179.9
C(3)–C(4)–C(5)–C(9)
179.6(2)
179.9
C(6)–C(5)–C(9)–C(10)
179.1(2)
179.9
C(17)–C(11)–C(12)–C(13)
−178.2(2)
−179.9


### 3.4. Photophysical Properties

Figure3 reveals the steady state absorption and emission spectra of1 in cyclohexane, and pertinent photophysical data is given in Table 2. Compound1exhibits the lowest lying absorption band maximized at 430 nm with vibronic structures, attributed to a π→π* transition, which is also supported by the calculated frontier orbitals shown in Figure 5. In addition, the absorption spectrum of1is almost identical with that of2 [29], which indicates that the introduction of thetert-butyl group does not significantly affect the bandgap energy of1 compared with that of2. As shown in Figure 3, dual emission is well resolved in the steady-state measurement of1, which is composed of a normal emission band (enol form), justified by its mirror image with respect to the lowest lying absorption, and a large Stokes shifted (5834 cm−1) emission band maximized at 457 and 574 nm, respectively. Accordingly, the assignment of a 574 nm emission for1 in cyclohexane to a proton-transfer tautomer emission is unambiguous, and ESIPT takes place from the phenolic proton (O(1)–H) to the O(2) oxygen, forming the keto-tautomer species depicted in Figure 4. Incidentally, the dual emission achieves a nearly white-light generation with CIE (0.28, 0.26). The overall quantum yield of1 is measured to be 0.07 and is about three times larger than that of2, which can be explained by the fact that the bulkytert-butyl group reduces the intermolecular π-π stacking of1 so that the quantum yield can be improved.Table 2
Calculated and experimental parameters for1.
Compound
λ
abs
a
λ
em
a
Φb
E
g
c
E(1)d
E(−1)d
E
HOMO/ELUMOe
E
HOMO/ELUMOf
E
g
g
1
430
457, 574
0.07
2.88
1.34
−1.28
−5.96/−3.08
−5.88/−2.25
2.99
aMeasured in cyclohexane (in nm).
bDetermined with 2 as [29].
cAt absorption maxima (Eg = 1240/λmax⁡, in eV).
dMeasured in a solution of 0.1 M tetrabutylammonium hexafluorophosphate (TBAPF6) in dichloromethane versus SCE (in V).
eCalculated from EHOMO = −4.88 − (Eoxd − EFc/Fc+) and ELUMO = EHOMO+ Eg  (in eV).
fCalculated by DFT/B3LYP (in eV).
gCalculated by TD-DFT/B3LYP (in eV).Figure 3
Normalized absorption (black line) and emission (red line) spectra of1 in cyclohexane.Figure 4
The optimized geometric structures of enol (E) and keto (K) form for1 in the ground and the first singlet excited state together with the intramolecular hydrogen bond lengths.Figure 5
The frontier molecular orbitals of1 for E, E*, K, and K*.


### 3.5. Quantum Chemistry Computation

The optimized geometric structures and the corresponding hydrogen bond lengths of enol and keto form for1 in the ground and the first singlet excited state were calculated using DFT and TD-DFT with the B3LYP functional and the 6-31G** basis set (Figure 4). From E (K*) to E* (K), we can see that the intramolecular hydrogen bond length decreases from 1.99 (1.81) Å to 1.89 (1.75) Å, whereas the other bond lengths do not change. The results clearly provide the evidence for the strengthening of the intramolecular hydrogen bond from S0 → S1 (S1 → S0), which is consistent with previous studies [38]. Therefore, there is no doubt that the decrease of intramolecular hydrogen bond lengths from E (K*) to E* (K) is a very important positive factor for the ESIPT (GSIPT: ground state intramolecular proton transfer) reaction.Figure5 shows the highest occupied molecular orbitals (HOMOs) and the lowest unoccupied molecular orbitals (LUMOs) of enol and keto form of1, both of which are strongly delocalized over the entire π-conjugated system. It also reveals that the electron density around the intramolecular hydrogen binding site is mainly populated at hydroxyl oxygen and carbonyl oxygen at HOMO and LUMO, respectively. The results clearly demonstrate that, upon electronic excitation of1, the hydroxyl proton (O(1)–H) is expected to be more acidic, whereas the carbonyl oxygen O(2) is more basic with respect to their ground state, driving the proton transfer reaction (forward ESIPT). After the forward ESIPT (E*→K*), the electron density located on O(1) increases while that on O(2) decreases, which shows the conspicuous intramolecular charge transfer from O(2) to O(1). This may supply the driving force for the proton transfer from O(2) to O(1) (backward ESIPT), so that the excited-state equilibrium can be created. Moreover, the absorption and emission spectra of1 were calculated by time-dependent DFT calculations (Franck-Condon principle, Figure 5). The calculated excitation, normal emission, and tautomer emission wavelengths for the S0→ S1 (S1→ S0) transitions are 414 nm, 476 nm,and 578 nm, respectively, which is very close to the experimental results (Table 2).The potential energy curves of1 as a function of the O(1)–H bond length were also studied (Figure 6). On the one hand, the full geometry optimization based on the B3LYP/6-31G** theoretical level reveals that the normal form (E) of1in the ground state is more stable than the corresponding proton-transfer tautomer (K) by 13.7 kcal/mol. As a result, proton transfer from K to E is populated in the ground states. On the other hand (for the first singlet excited state), one can clearly see that the potential energy barriers of the forward (8.0 kcal/mol) and the backward (2.7 kcal/mol) ESIPT are in the same order of magnitude, which is in good agreement with previous theoretical results of2 [38]. Accordingly, the forward and the backward ESIPT may happen on the same timescale and consequently leads to the rapidly established excited-state equilibrium.Figure 6
Potential energy curves (PECs) from enol form (E) to keto form (K) of1 at the ground state and excited state. The calculations are based on the optimized ground state geometry (S0 state) at the B3LYP/6-31G**/level using Gaussian 03W.


### 3.6. Electrochemical Properties

The cyclic voltammogram of1 is illustrated in Figure 7. When placed in dichloromethane and subjected to modest potentials, compound1 shows one oxidation and two reduction waves that all are chemically irreversible. The first oxidation and reduction potentials of1 are nearly identical to those of2 [29], showing that the alkylation of2 has no significant impact on both their electrochemical properties and their optical properties. Table 2 summarizes the redox potentials and the HOMO and LUMO energy levels estimated from cyclic voltammetry (CV) for1[39]. The HOMO/LUMO energy levels of1 are estimated to be −5.96/−3.08 eV and are in good agreement with the theoretical calculations.Figure 7
The cyclic voltammogram of1measured in dichloromethane solution with ferrocenium/ferrocene, at 200 mV/s.


## 3.1. Synthesis and Characterization

Scheme1 shows the chemical structure and the synthetic route of1. The synthesis of1 started from a conventional bromination of 7-methoxy-2,3-dihydro-1H-inden-1-one (6), followed by the elimination of the bromo adduct (5), giving a reactive dienophile4. The naphthalene moiety can then be fused onto the C(2)–C(3) double bond by placing4 through a reaction with α,α,α′α′-tetrabromo-o-xylene [29], yielding3. Subsequently, compound3 was subjected to the deprotection with BBr3 to give2. Finally, the fried-craft alkylation at the 8-position of2 was carried out by the reaction of2 withtert-butyl chloride and aluminum trichloride, giving1 with an overall product yield of 51%. The presence of a singletert-butyl substituent of1 can be verified by the presence of a signal at δ 1.40 ppm (9H) and eight signals at δ 6.7–8.1 ppm (8H) in the 1H NMR spectrum.


## 3.2. Hydrogen Bond Studies

The dominance of an enol-normal form for1, namely, the intramolecular hydrogen-bond formation between O(1)–H and O(2), is firmly supported by a combination of 1H NMR and X-ray single-crystal analyses (Figure 2). In the 1H NMR studies, the existence of an intramolecular hydrogen bond between O(1)–H and O(2) is evidenced by the observation of a substantial downfield shift of the proton peak at 8.68 ppm (in CDCl3). The hydrogen bonding energy (ΔE in kcal/mol) can be empirically calculated by introducing Schaefer’s correlation [35], expressed as Δδ=(-0.4±0.2)+ΔE, where Δδ is given in parts per million for the difference between chemical shift in the O–H peak of1and that in phenol (δ 4.29). Accordingly, the hydrogen-bonding energy is calculated to be 4.79±0.2 kcal/mol and is in good agreement with the theoretical calculations (6.27 kcal/mol). Note that compound1 has a weaker intramolecular hydrogen bond than most other ESIPT molecules [36, 37], which may account for its unique dual emission feature (vide infra).Figure 2
Displacement ellipsoid representation of1with the labelling scheme. The ellipsoids are drawn at the 50% probability level and the H atoms are drawn as spheres of arbitrary radii. The blue dashed line denotes the intramolecular hydrogen bond.


## 3.3. X-Ray Structures

The structure of1was further confirmed by single-crystal X-ray diffraction analysis. Compound1 crystallizes in the monoclinic space groupP21/c, witha = 15.7248(9),b = 6.0166(3),c = 17.5500(8) Å, α = 90°, β = 110.515(2)°, and γ = 90°. As shown in Figure 2, the molecular structure of1 is nearly planar (except fortert-butyl group), which is also confirmed by geometry optimization in our DFT calculation (Table 1 and Figure 4). This, together with 2.919 Å of O(1)–O(2) distance, supports the existence of a six-membered-ring intramolecular hydrogen bond. Additionally, the longer O(1)–O(2) distance in1than that (O(1)–O(2) < 2.7 Å) in most other ESIPT molecules [36, 37]supports that compound1has a weaker intramolecular hydrogen bond. This is possible due to the fact that the carbonyl oxygen O(2) locates at the five-membered-ring cyclopenta-2,4-dienone moiety (Figure 2), such that the ∠O(1)–H–O(2) angle is expected to be deviated from 120°, a perfect six-member-ring hydrogen bonding formation. This viewpoint is confirmed by the ∠O(1)–H–O(2) angle of 144.8°, according to the X-ray structure analysis. Careful examination of the crystal structure also indicates that there is no substantial π-π stacking between the tetracyclic plane and its adjacent one. Thus, we can ascertain that thetert-butyl group not only largely increases the solubility of1 compared with2 but also reduces intermolecular contact and aggregation.Table 1
Comparison of the experimental and optimized geometric parameters of1.
X-ray
DFT
Bond lengths (Å)
C(1)–O(1)
1.357(2)
1.348
C(7)–O(2)
1.222(2)
1.233
C(1)–C(2)
1.390(3)
1.407
C(3)–C(4)
1.396(3)
1.409
C(4)–C(5)
1.376(2)
1.387
C(5)–C(6)
1.399(2)
1.409
C(7)–C(8)
1.495(2)
1.492
C(9)–C(10)
1.361(2)
1.370
C(11)–C(12)
1.426(2)
1.433
C(15)–C(16)
1.419(2)
1.423
C(18)–C(19)
1.538(3)
1.539
Bond angles (°)
O(1)–C(1)–C(6)
121.7(2)
121.3
C(6)–C(1)–C(2)
118.1(2)
117.8
C(4)–C(5)–C(6)
120.3(2)
119.6
C(7)–C(8)–C(9)
108.1(2)
108.3
C(10)–C(11)–C(12)
119.9(2)
120.1
C(14)–C(15)–C(16)
117.0(2)
117.2
C(10)–C(11)–C(17)
122.3(2)
122.1
C(15)–C(18)–C(19)
111.5(2)
109.4
Torsion angles (°)
O(1)–C(1)–C(2)–C(3)
−178.8(2)
−179.9
C(3)–C(4)–C(5)–C(9)
179.6(2)
179.9
C(6)–C(5)–C(9)–C(10)
179.1(2)
179.9
C(17)–C(11)–C(12)–C(13)
−178.2(2)
−179.9


## 3.4. Photophysical Properties

Figure3 reveals the steady state absorption and emission spectra of1 in cyclohexane, and pertinent photophysical data is given in Table 2. Compound1exhibits the lowest lying absorption band maximized at 430 nm with vibronic structures, attributed to a π→π* transition, which is also supported by the calculated frontier orbitals shown in Figure 5. In addition, the absorption spectrum of1is almost identical with that of2 [29], which indicates that the introduction of thetert-butyl group does not significantly affect the bandgap energy of1 compared with that of2. As shown in Figure 3, dual emission is well resolved in the steady-state measurement of1, which is composed of a normal emission band (enol form), justified by its mirror image with respect to the lowest lying absorption, and a large Stokes shifted (5834 cm−1) emission band maximized at 457 and 574 nm, respectively. Accordingly, the assignment of a 574 nm emission for1 in cyclohexane to a proton-transfer tautomer emission is unambiguous, and ESIPT takes place from the phenolic proton (O(1)–H) to the O(2) oxygen, forming the keto-tautomer species depicted in Figure 4. Incidentally, the dual emission achieves a nearly white-light generation with CIE (0.28, 0.26). The overall quantum yield of1 is measured to be 0.07 and is about three times larger than that of2, which can be explained by the fact that the bulkytert-butyl group reduces the intermolecular π-π stacking of1 so that the quantum yield can be improved.Table 2
Calculated and experimental parameters for1.
Compound
λ
abs
a
λ
em
a
Φb
E
g
c
E(1)d
E(−1)d
E
HOMO/ELUMOe
E
HOMO/ELUMOf
E
g
g
1
430
457, 574
0.07
2.88
1.34
−1.28
−5.96/−3.08
−5.88/−2.25
2.99
aMeasured in cyclohexane (in nm).
bDetermined with 2 as [29].
cAt absorption maxima (Eg = 1240/λmax⁡, in eV).
dMeasured in a solution of 0.1 M tetrabutylammonium hexafluorophosphate (TBAPF6) in dichloromethane versus SCE (in V).
eCalculated from EHOMO = −4.88 − (Eoxd − EFc/Fc+) and ELUMO = EHOMO+ Eg  (in eV).
fCalculated by DFT/B3LYP (in eV).
gCalculated by TD-DFT/B3LYP (in eV).Figure 3
Normalized absorption (black line) and emission (red line) spectra of1 in cyclohexane.Figure 4
The optimized geometric structures of enol (E) and keto (K) form for1 in the ground and the first singlet excited state together with the intramolecular hydrogen bond lengths.Figure 5
The frontier molecular orbitals of1 for E, E*, K, and K*.


## 3.5. Quantum Chemistry Computation

The optimized geometric structures and the corresponding hydrogen bond lengths of enol and keto form for1 in the ground and the first singlet excited state were calculated using DFT and TD-DFT with the B3LYP functional and the 6-31G** basis set (Figure 4). From E (K*) to E* (K), we can see that the intramolecular hydrogen bond length decreases from 1.99 (1.81) Å to 1.89 (1.75) Å, whereas the other bond lengths do not change. The results clearly provide the evidence for the strengthening of the intramolecular hydrogen bond from S0 → S1 (S1 → S0), which is consistent with previous studies [38]. Therefore, there is no doubt that the decrease of intramolecular hydrogen bond lengths from E (K*) to E* (K) is a very important positive factor for the ESIPT (GSIPT: ground state intramolecular proton transfer) reaction.Figure5 shows the highest occupied molecular orbitals (HOMOs) and the lowest unoccupied molecular orbitals (LUMOs) of enol and keto form of1, both of which are strongly delocalized over the entire π-conjugated system. It also reveals that the electron density around the intramolecular hydrogen binding site is mainly populated at hydroxyl oxygen and carbonyl oxygen at HOMO and LUMO, respectively. The results clearly demonstrate that, upon electronic excitation of1, the hydroxyl proton (O(1)–H) is expected to be more acidic, whereas the carbonyl oxygen O(2) is more basic with respect to their ground state, driving the proton transfer reaction (forward ESIPT). After the forward ESIPT (E*→K*), the electron density located on O(1) increases while that on O(2) decreases, which shows the conspicuous intramolecular charge transfer from O(2) to O(1). This may supply the driving force for the proton transfer from O(2) to O(1) (backward ESIPT), so that the excited-state equilibrium can be created. Moreover, the absorption and emission spectra of1 were calculated by time-dependent DFT calculations (Franck-Condon principle, Figure 5). The calculated excitation, normal emission, and tautomer emission wavelengths for the S0→ S1 (S1→ S0) transitions are 414 nm, 476 nm,and 578 nm, respectively, which is very close to the experimental results (Table 2).The potential energy curves of1 as a function of the O(1)–H bond length were also studied (Figure 6). On the one hand, the full geometry optimization based on the B3LYP/6-31G** theoretical level reveals that the normal form (E) of1in the ground state is more stable than the corresponding proton-transfer tautomer (K) by 13.7 kcal/mol. As a result, proton transfer from K to E is populated in the ground states. On the other hand (for the first singlet excited state), one can clearly see that the potential energy barriers of the forward (8.0 kcal/mol) and the backward (2.7 kcal/mol) ESIPT are in the same order of magnitude, which is in good agreement with previous theoretical results of2 [38]. Accordingly, the forward and the backward ESIPT may happen on the same timescale and consequently leads to the rapidly established excited-state equilibrium.Figure 6
Potential energy curves (PECs) from enol form (E) to keto form (K) of1 at the ground state and excited state. The calculations are based on the optimized ground state geometry (S0 state) at the B3LYP/6-31G**/level using Gaussian 03W.


## 3.6. Electrochemical Properties

The cyclic voltammogram of1 is illustrated in Figure 7. When placed in dichloromethane and subjected to modest potentials, compound1 shows one oxidation and two reduction waves that all are chemically irreversible. The first oxidation and reduction potentials of1 are nearly identical to those of2 [29], showing that the alkylation of2 has no significant impact on both their electrochemical properties and their optical properties. Table 2 summarizes the redox potentials and the HOMO and LUMO energy levels estimated from cyclic voltammetry (CV) for1[39]. The HOMO/LUMO energy levels of1 are estimated to be −5.96/−3.08 eV and are in good agreement with the theoretical calculations.Figure 7
The cyclic voltammogram of1measured in dichloromethane solution with ferrocenium/ferrocene, at 200 mV/s.


## 4. Conclusions

In conclusion, we have successfully synthesized a new ESIPT-based white-light-emitting small molecule (1). Compound1 undergoes an intramolecular proton transfer reaction in the excited state, resulting in a tautomer that is in equilibrium with the normal species, exhibiting a dual emission that generates white light. Analysis of the geometric structures clearly indicates that the intramolecular hydrogen bond length is shortened upon the photoexcitation, which is regarded as a very important factor for ESIPT. Furthermore, the potential energy curves suggest that the forward ESIPT and backward ESIPT may happen on the same timescale and leads to the rapidly established excited-state equilibrium. Research on its application to single-molecule-based white-light-emitting OLEDs is currently in progress.



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*Source: 124753-2014-05-26.xml*