Vinylene-Bridged Cyclic Dipyrrin and BODIPY Trimers

Abstract

Vinylene-bridged cyclic boron–difluoride complex of dipyrrin (BODIPY) trimers were successfully prepared from expanded dimethyl-vinylene bridged hexaphyrin(2.1.2.1.2.1) Me-Hex that has the structure of alternate dipyrrins and vinylene bridges. The hexaphyrin(2.1.2.1.2.1) Me-Hex can coordinate with boron ions to afford five kinds of cyclic BODIPYs given by step-by-step boron complexations. Crystal structures of all cyclic BODIPYs except for 3BF₂-Me-Hex(b) formed non-planar structures. The theoretical calculation predicted that mono-/bis-boron cyclic BODIPYs show the intramolecular charge transfer (ICT) characteristics, whereas tri-boron cyclic BODIPYs have no ICT characteristics. Reflecting these electronic properties, tri-boron cyclic BODIPYs exhibit weak fluorescence in the red region, but mono-/bis-boron cyclic BODIPYs exhibit no emission. Vinylene bridged cyclic dipyrrin trimer Me-Hex is the novel porphyrinoid ligand allowed to control the boron coordination under different reaction conditions to form various boron complexes.

1. Introduction

A boron–difluoride complex of dipyrrin (BODIPY) is an outstanding fluorescent dye with high fluorescence quantum yield and high chemical robustness [1,2,3,4]. BODIPYs have been used for many applications such as optical materials, solar cells, biological imaging, and sensitizers for photodynamic therapy [5,6,7]. Among BODIPY derivatives, cyclic BODIPY oligomers show distinct electronic and optical properties such as unique luminescent and lasing properties, cation recognition, and switchable near infrared (NIR) responses [8,9,10,11,12,13,14,15]. Shinokubo and co-workers developed the synthesis of planar BODIPY dimer and trimer (c-BODIPY-1), linked through butadiyne by sila-Glaser coupling reaction (Figure 1) [9]. These cyclic BODIPYs are stable anti-aromatic compounds with NIR absorbing properties. Nabeshima and co-workers also reported a series of cyclic BODIPY oligomers linked through meta- and para-phenylenes (c-BODIPY-2 and c-BODIPY-3) (Figure 1) [11,12,13,14,15]. Their results show that the expanded porphyrins containing π-conjugated bridging units could be excellent precursors for the preparation of cyclic BODIPY oligomers. However, research on cyclic BODIPY oligomers is still limited due to few efficient synthesis methods [8,9,10,11,12,13,14,15]. Moreover, the relationship between the number of coordinated boron atoms and molecular configuration/optical properties of expanded porphyrins is still unclear.

Recently, we developed the synthesis of expanded porphyrins that include alternate vinylene bonds and dipyrrin units [16,17,18,19]. These expanded porphyrins are flexible and switchable molecular frameworks because of containing the vinylene bridges that can isomerize by external stimuli. In addition, molecular configurations and electronic properties can be tuned by substitution on vinylene bridges. The pristine trans-vinylene-bridged hexaphyrin(2.1.2.1.2.1), Hex, forms a planar structure with the aromatic property, whereas diphenyl-vinylene bridged hexaphyrin(2.1.2.1.2.1), Ph-Hex, forms the highly distorted structure with the non-aromatic property. Ph-Hex has bulky phenyl groups and mixed configurations on vinylene bridges, resulting in the formation of the distorted structure. Interestingly, the configuration of Ph-Hex is changed to the cis-vinylene-bridged figure-of-eight structure with the aromatic property by insertion of copper ions [18]. These results indicate that the expanded porphyrins having vinylene-bridges are curious ligands to make metal complexes accompanied by changes in molecular configurations and electronic properties. In addition, they include the dipyrrin unit that is a useful bidentate mono-anionic ligand capable of preparing various metal complexes, including BODIPYs.

In this paper, we report the synthesis, crystal structure, and optical properties of vinylene-bridged expanded porphyrins and boron complexes, using the dimethyl-vinylene bridged hexaphyrin(2.1.2.1.2.1), Me-Hex. We found that Me-Hex is a suitable ligand for the preparation of five boron complexes. Distorted and flexible structures lead to adjusting the coordination structure to boron ions, and the small methyl group allows sufficient space. We will discuss the reactivity of Me-Hex for inserting boron ions, crystal structures, and optical and electrochemical properties.

2. Results and Discussion

Initially, we designed new hexaphyrin(2.1.2.1.2.1) with methyl groups on vinylene bridges as small substituents to make coordination spaces for preparing multi-boron complexes. The intermediate of dimethyl-dipyrrolylethenes (E/Z-1) was obtained from 2-acylpyrrole by McMurry coupling [11,12,13,14,15,16,17,18,20]. We and others reported that E/Z-dipyrroethenes undergo cis/trans isomerization in acidic conditions to prepare porphyrinoids [16,17,18,19,21]. Therefore, we used it as a mixture toward the next step. Treatment of E/Z-1 and pentafluorobenzaldehyde in the presence of BF₃•OEt₂ under condensation reactions and oxidation with 2,3-dichloro-5,6-dicyano-p-benzoquinone (DDQ) afforded three expanded porphyrins: Porphyrin(2.1.2.1), Me-Por, in 1%, hexaphyrin(2.1.2.1.2.1), Me-Hex, in 6%, and octaphyrin(2.1.2.1.2.1.2.1), Me-Oct, in 3% (Scheme 1). Characterization was conducted by matrix assisted Laser desorption/ionization-mass spectrometry (HR-MALDI-MS), X-ray crystallography, and ¹H and ¹⁹F nuclear magnetic resonance (NMR) spectroscopy. In the HR-MALDI-MS, corresponding molecular ion peaks of Me-Por at m/z = 724.1683 (calculated for C₃₈H₂₂F₁₀N₄ = 724.1685 [M]⁺), Me-Hex at m/z = 1086.2522 (calculated for C₅₇H₃₃F₁₅N₆ = 1086.2527 [M]⁺), and Me-Oct at m/z = 1448.3364 (calculated for C₇₆H₄₄F₂₀N₈ = 1448.3370 [M]⁺) were observed, respectively (Figures S1–S3).

The structures of these expanded porphyrins were determined by X-ray crystal structural analysis (Figure 2). Me-Por consists of two dipyrrin units connected through cis/cis-vinylene bridges, which make a saddle-shaped bent structure. This structure is similar to the structures of dibenzoporphyrin(2.1.2.1) and tetraphenylporphyrin(2.1.2.1) [16,18]. The compounds Me-Hex and Me-Oct also form distorted structures, mixing with cis- and trans-conformations at vinylene bridges. The compound Me-Hex comprises cis/trans/trans conformation at the vinylene bridges. The compound Me-Oct has a saddle-shaped distorted molecular structure consisting of cis/trans/cis/trans conformation at vinylene-bridges. All obtained porphyrins are categorized as having the same non-aromatic characteristic as Ph-Hex because of distorted structures [18].

The UV-vis absorption spectra of Me-Por, Me-Hex, and Me-Oct were measured in CH₂Cl₂. These compounds show two distinct absorptions with strong and weak broad bands, reflecting their non-aromaticity (Figure 3) [16,17,18,19]. Maximum absorption peaks are observed at 432 nm for Me-Por, 500 nm for Me-Hex, and 574 nm for Me-Oct, which are gradually red-shifted by increasing in the ring size from Me-Por to Me-Oct as similar to expanded porphyrins. Their highest occupied molecular orbital (HOMO)-lowest unoccupied molecular orbital (LUMO) energy differences were estimated by density functional theory (DFT) calculations at B3LYP/6-31G* level (Figures S4 and S5). With increasing the ring size, the HOMO and LUMO energies increase and decrease, respectively. The HOMO levels of Me-Por, Me-Hex, and Me-Oct are −5.27 eV, −4.87 eV, and −4.78 eV, and the LUMO levels are −2.51 eV, −3.00 eV, and −3.04 eV, resulting in the decreasing the HOMO-LUMO difference.

The differences in the formation of boron complexes of compound Me-Hex depending on the reaction conditions are summarized in Scheme 2. We optimized the reaction conditions of the boron complexation of Me-Hex. The treatment of Me-Hex with 40 eq. triethylamine (TEA) and 80 eq. BF₃•OEt₂ in CH₂Cl₂ at room temperature for 12 h mainly gave a mono-boron complex BF₂-Me-Hex in 60% yield. ¹H NMR spectrum of BF₂-Me-Hex shows twelve sets of doublet peaks corresponding to pyrrolic β-protons and two broadened peaks at 13.26 and 13.07 ppm, corresponding to NH protons (Figure 4a). This result indicates that the first boron ion is coordinated into dipyrrin at the next to the cis-vinylene bridge as the asymmetric position. When an increase of reaction temperatures from room temperature to the reflux condition in CH₂Cl₂, two kinds of bis-boron complexes 2BF₂-Me-Hex(a) and 2BF₂-Me-Hex(b) that can be separated by silica gel column chromatography were generated in 20% and 28%, respectively (Scheme 2). The insertion positions of the second boron ion of 2BF₂-Me-Hex(a) and 2BF₂-Me-Hex(b) were confirmed by ¹H NMR spectroscopy (Figure 4b,c) and X-ray crystallography (vide infra). 2BF₂-Me-Hex(a) shows twelve sets of doublet peaks of pyrrolic β-protons and six methyl protons (Figure 4b). This structure is close to freebase Me-Hex and BF₂-Me-Hex. In contrast, 2BF₂-Me-Hex(b) shows the half number peak sets compared with 2BF₂-Me-Hex(a) (Figure 4c). This means that 2BF₂-Me-Hex(b) forms a 2-hold symmetric structure resulting in the formation of the bis-boron complex. Tri-boron complex was obtained from Me-Hex in the reaction with 40 eq. TEA and 120 eq. BF₃•OEt₂ in toluene at 80 °C. Unexpectedly, two types of tri-boron complexes, 3BF₂-Me-Hex(a) and 3BF₂-Me-Hex(b), were isolated in 5% and 2% yields, respectively, after separation by silica gel column chromatography. Additionally, these tri-boron complexes 3BF₂-Me-Hex(a) and 3BF₂-Me-Hex(b) were obtained from 2BF₂-Me-Hex(a) and 2BF₂-Me-Hex(b) under the same reaction conditions. The spectrum pattern of ¹H NMR of 3BF₂-Me-Hex(a) is similar to that of 2BF₂-Me-Hex(b), indicating that the addition of boron ion in the last coordination site into 2BF₂-Me-Hex(a) and 2BF₂-Me-Hex(b) (Figure 4d). Interestingly, the other 3BF₂-Me-Hex(b) shows a different peak pattern, which means that 3BF₂-Me-Hex(b) has a different molecular configuration (Figure 4e). In the HR-MALDI-MS, corresponding molecular ion peaks of all boron complexes were observed (Figures S6–S10). Although the compounds Me-Por and Me-Oct reacted with BF₃•OEt₂ in the presence of TEA in CH₂Cl₂, boron complexes of Me-Por and Me-Oct could not be isolated. The reason is that the cavity space of compounds Me-Por and Me-Oct is insufficient to coordinate boron ions because of steric hindrances and less structural flexibilities.

Molecular configurations of all boron complexes were determined by X-ray crystallography. BF₂-Me-Hex, 2BF₂-Me-Hex(a), 2BF₂-Me-Hex(b), and 3BF₂-Me-Hex(a) maintain distorted structures with cis/cis/trans geometry at vinylene bridges, which molecular frameworks are comparable to those of freebase Me-Hex (Figure 2 and Figure 5). The boron of BF₂-Me-Hex is coordinated on the dipyrrin unit, which is located to the next to cis-vinylene bridge. This is consistent with the result of NMR (Figure 4a). The bis-boron complexes, 2BF₂-Me-Hex(a) and 2BF₂-Me-Hex(b), clearly show that positions of the second boron are different. The second boron of 2BF₂-Me-Hex(a) is bonded to dipyrrin, which is sandwiched between trans-vinylene bridges, whereas the second boron of 2BF₂-Me-Hex(b) is bonded to another site of dipyrrin. Triboron complex of 3BF₂-Me-Hex(a) coordinates boron in all coordination sites and forms the distorted structure. In contrast, 3BF₂-Me-Hex(b) has a different molecular structure with the trans-vinylene bridges and a co-planar structure.

To investigate the selectivity of boron complexation to Me-Hex, the electrostatic potential of Me-Hex was calculated by Gaussian 09 (Figure 6) [22]. The dipyrrin units are named as coordination site 1, site 2, and site 3, which are depicted in Figure 6. Site 1 shows the most negative potential (red-colored position) compared with the other dipyrrin sites. This means that site 1 dominantly produces the deprotonated dipyrrin species that can react with BF₃•OEt₂ to give BF₂-Me-Hex.

The absorption spectra of boron complexes are shown in Figure 7. All boron complexes show a strong absorption band around 450 to 550 nm, and a weak broad band around 600 to 850 nm. The strong bands of approximately 500 nm become sharpened and increase the absorption coefficient with an increase in the number of boron ions. Bis-boron complexes 2BF₂-Me-Hex(a) and 2BF₂-Me-Hex(b) exhibit similar absorption shapes, indicating that the position of boron ions does not strongly perturb the optical properties because they form similar molecular structures. In contrast, tri-boron complexes 3BF₂-Me-Hex(a) and 3BF₂-Me-Hex(b) exhibit slightly different absorption shapes, reflecting their different molecular structures. The emission spectra of all boron complexes were measured in CH₂Cl₂ (Figure S11). Freebase, mono, and bis-boron complexes have no fluorescence, even at low temperatures. In contrast, two tri-boron complexes exhibit a weak fluorescence in the red region (3BF₂-Me-Hex(a): λ_em = 650 nm, Φ_F = 1.0%; 3BF₂-Me-Hex(b): λ_em = 650 nm, Φ_F = 1.4%). These fluorescence quantum yields were obtained by comparison with meso-tetraphenylporphyrin (Φ_F = 0.12 in CH₂Cl₂) used as a standard [23,24].

The optical properties of boron complexes were predicted by DFT and time dependent (TD)-DFT calculations at B3LYP/6-31G* level and cam-B3LYP/6-31G*// B3LYP/6-31G*, respectively. The HOMO of mono and bis-boron complexes of Me-Hex is located at the free-base dipyrrin unit, whereas their LUMO is mainly located at BODIPY units (Figures S12 and S13). In contrast, HOMO and LUMO of two tri-boron complexes 3BF₂-Me-Hex(a) and 3BF₂-Me-Hex(b) are equally delocalized on three BODIPY units. To deeper understand the optical properties of boron complexes, TD-DFT calculation was examined (Figure S14 and Table S1). The S₀–S₁ transitions of absorption of BF₂-Me-Hex, 2BF₂-Me-Hex(a), and 2BF₂-Me-Hex(b) clearly exhibit an intramolecular charge transfer (ICT) transition from the free-base dipyrrin as the donor unit to the BODIPY unit as the acceptor [24,25,26]. In contrast, 3BF₂-Me-Hex(a) and 3BF₂-Me-Hex(b) exhibit a π-π transition. The electron density difference map (EDDM) represents the difference in electron densities upon electronic transitions (Figure 8) [27]. EDDMs of 3BF₂-Me-Hex(a) and 3BF₂-Me-Hex(b) are delocalized on the whole molecules, whereas the location of EDDMs for the lowest HOMO-LUMO transitions of BF₂-Me-Hex, 2BF₂-Me-Hex(a), and 2BF₂-Me-Hex(b) is shifted from the free base dipyrrin units to the BODIPY units. The predicted ICT characteristics of BF₂-Me-Hex, 2BF₂-Me-Hex(a), and 2BF₂-Me-Hex(b) are consistent with their non-emissive behavior in solution upon photoexcitation [25,26,27]. Generally, BODIPY compounds show strong emission. Actually, the c-BODIPY-3 is the emissive compound with high fluorescence quantum yield [14]. Unfortunately, although the lowest transition of Me-Hex is the π-π transition, 3BF₂-Me-Hex(a) and 3BF₂-Me-Hex(b) exhibit only weak fluorescence. There are two possible reasons. The first reason is that the S₀-S₁ transition of 3BF₂-Me-Hex(a) and 3BF₂-Me-Hex(b) is forbidden, inducing the low emissive property. The second reason is that molecular skeleton of Me-Hex is highly flexible, caused by the rotation of the vinylene bridges in the solution. It is advantageous to give high reactivity, but it induces the nonradiative deactivation. Therefore, to achieve the preparation of the high emissive cyclic BODIPYs, substituents on vinylene bridges of hexaphyrin(2.1.2.1.2.1) should be carefully chosen with the combination of reactivity and rigid molecular frameworks.

The redox properties of BF₂-Me-Hex, 2BF₂-Me-Hex(a), 2BF₂-Me-Hex(b), 3BF₂-Me-Hex(a), and 3BF₂-Me-Hex(b) were measured by cyclic voltammetry (CV) in CH₂Cl₂ with 0.1 M TBAPF₆ as an electrolyte (Figure 9). The free base Me-Hex shows one irreversible oxidation and three reversible reduction potentials at 0.20, −1.40, −1.55, and −1.98 V (vs. Fc/Fc⁺). The cyclic BODIPYs also show similar redox properties. The oxidation and reduction potentials are gradually shifted positively because of the electron-withdrawing properties of boron–difluoride units [19].

3. Materials and Methods

3.1. General

¹H NMR and ¹⁹F NMR spectra were recorded on a JNM-ECX 400 spectrometer (operating as 400 MHz for ¹H and 376 MHz for ¹⁹F) using the residual solvent as the internal reference for ¹H (δ = 7.26 ppm in CDCl₃, δ = 5.32 ppm in CD₂Cl₂) and CF₃COOH as the external reference for ¹⁹F (δ = −76.5 ppm). The ¹H NMR and ¹⁹F NMR spectra of all compounds are shown in Figures S15–S32. HR-MALDI−TOF mass spectra were recorded on a Bruker Daltonics autoflex MALDI−TOF MS spectrometer. UV/Vis/NIR absorption spectra were measured using a JASCO UV/Vis/NIR Spectrophotometer V-670. CV measurements were conducted in a solution of 0.1 M TBAPF₆ in dichloromethane at a scan rate of 0.1 V s⁻¹ in an argon-filled cell. A glassy carbon electrode and a platinum wire were used as working and counter electrodes, respectively. An Ag/AgNO₃ electrode was used as a reference electrode, which was normalized with the half-wave potential of ferrocene/ferrocenium (Fc/Fc⁺) redox couple. All solvents and chemicals were reagent grade quality, obtained commercially, and used without further purification, except as noted. For spectral measurements, spectral grade dichloromethane was purchased from Nacalai Tesque Co. Thin-layer chromatography (TLC), flush column chromatography, and gravity column chromatography were performed on Art. 5554 (Merck KGaA, Darmstadt, Germany), Silica Gel 60 (Merck KGaA, Darmstadt, Germany), and Silica Gel 60N (Kanto Chemical Co., Tokyo, Japan), respectively.

3.2. X-ray Analysis

All the single crystals except Me-Oct were obtained by the solvent diffusion method. The solvents are described in the Tables S2–S9 in the supporting information. Single crystals of Me-Oct were obtained by recrystallization from toluene. X-ray crystallographic data for BF₂-Me-Hex, 2BF₂-Me-Hex(b), and 3BF₂-Me-Hex(b) were recorded at 90 K using a BRUKER-APEXII X-Ray diffractometer using a Mo-Kα radiation equipped with a large area CCD detector and X-ray crystallographic data for Me-Por, Me-Hex, Me-Oct, 2BF₂-Me-Hex(a), and 3BF₂-Me-Hex(a) were recorded at 103 K on a Rigaku R-AXIS RAPID/S imaging plate diffractometer using Mo-Kα radiation. The structures were solved by direct methods and refined on F² by full−matrix least−squares using the CrystalClear and SHELXS−97 and SHELXT−2014/5 programs. CCDC: 1830225, 1830228, 1830229, 1830230, 1830231, 1848201, 1830232, and 1830233 contain the supplementary crystallographic data for Me-Por, Me-Hex, Me-Oct, BF₂-Me-Hex, 2BF₂-Me-Hex(a), 2BF₂-Me-Hex(b), 3BF₂-Me-Hex(a), and 3BF₂-Me-Hex(b), respectively. These data can be obtained free of charge from the Cambridge Crystallographic Data Centre via www.ccdc.cam.ac.uk/data_request/cif.

3.3. Theoretical Calculations

All density functional theory calculations were achieved with the Gaussian 09 program package. The geometry was optimized at the Becke’s three-parameter hybrid functional combined with the Lee−Yang−Parr correlation functional abbreviated as the B3LYP level of density functional theory with the 6-31G(d) basis set.

3.4. Synthesis of Dimethyl-Dipyrrolylethane (E/Z-1)

TiCl₄ (3.5 mL) was added dropwise to a solution of Zn powder (2.73 g) and CuCl (273 mg) in THF (75 mL) at 0 °C under argon. The reaction mixture was heated at reflux for 2 h. 2-Acetylpyrrole (600 mg, 5.5 mmol) in THF (10 mL) was added dropwise to the reaction mixture, and then the solution was heated at reflux for another 2 h. The reaction was carefully quenched with aqueous sodium acetate and the resulting mixture was extracted with CH₂Cl₂. The organic layer was washed with water and brine, and dried over anhydrous Na₂SO₄. After removal of the solvent, the crude product was purified by silica gel column chromatography (CH₂Cl₂/hexane = 3/2) to give Z-1 in 23% (120 mg, 0.6 mmol) and E-1 in 10% (51 mg, 0.3 mmol). Z-1: ¹H NMR (400 MHz, CDCl₃, 298 K) δ = 7.74 (brs, 2H), 6.60 (m, 2H, pyrrole), 6.18–6.17 (m, 4H, pyrrole), 2.12 (s, 6H, methyl) ppm. E-1: ¹H NMR (400 MHz, CDCl₃, 298 K) δ = 8.17 (brs, 2H, NH), 6.81–6.80 (m, 2H, pyrrole), 6.28–6.26 (m, 2H, pyrrole), 6.24–6.23 (m, 2H, pyrrole), 2.22 (s, 6H, methyl) ppm.

3.5. Synthesis of Me-Por, Me-Hex, and Me-Oct

To a solution of E/Z-1 (186 mg, 1.0 mmol) and pentafluorobenzaldehyde (196 mg, 1.0 mmol) in CH₂Cl₂ (150 mL) was added BF₃•Et₂O (4.3 mg, 0.03 mmol) under argon. After stirring for 2 h at room temperature, DDQ (227 mg, 1.0 mmol) was added to the reaction mixture, which was stirred for 1 h. After removal of the solvent, the residue was purified by alumina chromatography (hexane/CH₂Cl₂ = 5/1) and silica gel column chromatography (CH₂Cl₂). The first eluted yellow fraction was evaporated to give Me-Por in 1% (3.5 mg, 0.0048 mmol) as a deep purple solid. The second red fraction was evaporated to give Me-Hex in 6% (21.5 mg, 0.02 mmol) as a dark red solid, and the third green fraction was evaporated to give Me-Oct in 3% (10.5 mg, 0.0075 mmol) as a dark red solid.

Me-Por: ¹H NMR (CDCl₃, 400 MHz, 298 K) δ = 11.82 (brs, 2H), 6.23 (d, J = 4 Hz, 4H), 6.12 (d, J = 4 Hz, 4H), 2.16 (s, 12H) ppm. ¹⁹F NMR (CDCl₃, 376 MHz, CF₃COOH) δ = −152.98–−153.10 (t, 2F), −161.26–−161.40 (m, 2F), −161.49–−161.62 (m, 2F) ppm. HR-MALDI-MS: Calculated for C₃₈H₂₂F₁₀N₄: 724.1685 [M⁺], Found: 724.1683. UV-vis-NIR (in CH₂Cl₂) λ [nm] (ε[M⁻¹cm⁻¹]): 431 (58,000) 507 (sh.) (4300).

Me-Hex: ¹H NMR (CDCl₃, 400 MHz, 298 K) δ = 14.14 (brs, 1H), 13.62 (brs, 1H), 13.25 (brs, 1H), 6.75 (d, J = 4 Hz, 1H), 6.66 (d, J = 4 Hz, 1H), 6.59 (d, J = 4 Hz, 1H), 6.51 (d, J = 4 Hz, 1H), 6.48 (d, J = 4 Hz, 1H), 6.45 (d, J = 4 Hz, 1H), 6.43 (d, J = 4 Hz, 1H), 6.39 (d, J = 4 Hz, 1H), 6.36 (d, J = 4 Hz, 1H), 6.03 (d, J = 4 Hz, 1H), 5.96 (d, J = 4 Hz, 1H), 5.56 (d, J = 4 Hz, 1H), 2.71 (s, 3H), 2.57 (s, 3H), 2.45 (s, 3H), 2.40 (s, 3H), 2.29 (s, 3H), 1.95 (s, 3H) ppm. ¹⁹F NMR (CDCl₃, 376 MHz, CF₃COOH) δ = −136.84–−138.37 (m, 6F), −152.23–−153.37 (m, 3F), −160.92–−161.38 (m, 6F) ppm. HR-MALDI-MS: Calculated for C₅₇H₃₃F₁₅N₆: 1086.2527 [M⁺], Found: 1086.2522. UV-vis-NIR (in CH₂Cl₂) λ [nm] (ε [M⁻¹ cm⁻¹]): 506 (84,000), 645 (sh) (9700).

Me-Oct: ¹H NMR (400 MHz, CDCl₃, 298 K) δ = 12.49 (brs, 4H), 6.43 (s, 4H), 6.33 (d, J = 4 Hz, 4H), 6.23 (s, 8H), 2.33 (s, 12H), 2.29 (s, 12H) ppm. ¹⁹F NMR (376 MHz, CDCl₃): δ = −137.84–−137.90 (m, 8F), −152.78–−152.90 (m, 4F), −161.15–−161.26 (m, 8F) ppm. HR-MALDI-MS: Calculated for C₇₆H₄₄F₂₀N₈: 1448.3370 [M⁺], Found: 1448.3370. UV-vis-NIR (in CH₂Cl₂) λ [nm] (ε [M⁻¹ cm⁻¹]): 438 (43,000), 570 nm (72,000).

3.6. Synthesis of Boron Complexes of Me-Hex

Method A: To a solution of Me-Hex (11 mg, 0.01 mmol) in CH₂Cl₂ (20 mL) and triethylamine (TEA) (40 mg, 0.4 mmol) was added BF₃•Et₂O (113 mg, 0.8 mmol) under argon. After stirring at room temperature for 12 h, the reaction mixture was extracted with CH₂Cl₂. The organic phase was washed with aqueous NaHCO₃, water and brine, and dried over Na₂SO₄. After removal of the solvent, the crude product was purified by silica gel column chromatography (hexane/CH₂Cl₂ = 3/1) to give BF₂- Me-Hex (7 mg, 0.006 mmol) in 60% yield.

Method B: To a solution of Me-Hex (11 mg, 0.01 mmol) in CH₂Cl₂ (20 mL) and triethylamine (TEA) (40 mg, 0.4 mmol) was added BF₃•Et₂O (169 mg, 1.2 mmol) under argon. After stirring at reflux for 12 h, the reaction mixture was extracted with CH₂Cl₂. The organic phase was washed with aqueous NaHCO₃, water and brine, and dried over Na₂SO₄. After removal of the solvent, the resulting crude product was purified by silica gel column chromatography (hexane/CH₂Cl₂ = 3/2) to give 2BF₂-Me-Hex(a) (2.4 mg, 0.002 mmol) in 20% and 2BF₂-Me-Hex(b) (3.4 mg, 0.0028 mmol) in 28%.

Method C: To a solution of Me-Hex (10.8 mg, 0.01 mmol) in toluene (20 mL) and triethylamine (TEA) (40 mg, 0.4 mmol) was added BF₃•Et₂O (169 mg, 1.2 mmol) under argon. After stirring at 80 °C for 12 h, the reaction mixture was extracted with CH₂Cl₂. The organic phase was washed with aqueous NaHCO₃, water, and brine, and dried over Na₂SO₄. After removal of the solvent, the resulting crude product was purified by silica gel column chromatography (hexane/CH₂Cl₂ = 1/1) to give 3BF₂-Me-Hex(a) (0.63 mg, 0.0005 mmol) in 5% and 3BF₂-Me-Hex(a) (0.25 mg, 0.0002 mmol) in 2%, 2BF₂-Me-Hex(a) in 20% (2.4 mg, 0.002 mmol), and 2BF₂-Me-Hex(b) in 28% (3.4 mg, 0.0028 mmol).

BF₂-Me-Hex: ¹H NMR (400 MHz, CDCl₃, 298 K) δ = 13.26 (brs, 1H), 13.07 (brs, 1H), 6.75 (d, J = 4 Hz, 2H), 6.69 (d, J = 4 Hz, 1H), 6.65 (d, J = 4 Hz, 1H), 6.60 − 6.59 (m, J = 4 Hz, 2H), 6.54 (d, J = 4 Hz, 1H), 6.49 (d, J = 4 Hz, 1H), 6.45 (d, J = 4 Hz, 1H), 6.28 (d, J = 4 Hz, 1H), 6.24 (d, J = 4 Hz, 1H), 6.22 (d, J = 4 Hz, 1H), 2.73 (s, 3H), 2.47 (s, 3H), 2.42 (s, 3H), 2.21 (s, 3H), 2.18 (s, 3H), 1.96 (s, 3H) ppm. ¹⁹F NMR (376 MHz, CDCl₃): δ = −135.60 (m, 1F), −136.56 (m, 2F), −137.68 (m, 1F), −137.95 (m, 2F), −141.50 (brs, 2F), −150.02 (t, J = 41 Hz, 1F), −152.46 (t, J = 42 Hz, 1F), −152.69 (t, J = 41 Hz, 1F), −159.67 (m, 2F), −160.78 (m, 2), −161.15 (m, 2F) ppm. HR-MALDI-MS: Calculated for C₅₇H₃₂BF₁₇N₆ = 1134.2510 [M]⁺, Found: 1134.2505. UV-vis-NIR (in CH₂Cl₂) λ [nm] (ε [M⁻¹cm⁻¹]): 492 (54,000), 518 (58,000).

2BF₂-Me-Hex(a): ¹H NMR (400 MHz, CDCl₃, 298 K) δ = 6.76 (d, J = 4 Hz, 1H), 6.71 (d, J = 4 Hz, 1H), 6.66 (d, J = 4 Hz, 1H), 6.62 (d, J = 4 Hz, 1H), 6.47 (m, 2H), 6.41 (m, 2H), 6.38 (d, J = 4 Hz, 1H), 6.34 (d, J = 4 Hz, 1H), 6.31 (d, J = 4 Hz, 1H), 6.23 (d, J = 4 Hz, 1H), 2.66 (s, 3H), 2.26 (s, 3H), 2.24 (s, 3H), 2.15(s, 3H), 2.14 (s, 3H), 1.95 (s, 3H) ppm. ¹⁹F NMR (376 MHz, CDCl₃): δ = −135.14 (m, 1F), −136.01 (m, 1F), −136.45 (m, 2F), −136.85 (m, 1F), −138.06 (m, 1F), −138.07 (brs, 1F), −138.72 (brs, 1F), −144.69 (brs, 1F), −146.38 (brs, 1F), −150.01 (t, J = 42 Hz, 1F), −150.20 (t, J = 42 Hz, 1F), −152.86 (t, J = 42 Hz, 1F), −159.61 (m, 3F), −159.95 (m, 1F), −161.33 (m, 2F) ppm. HR-MALDI-MS: Calculated for C₅₇H₃₁B₂F₁₉N₆Na = 1205.2391 [M+Na]⁺, Found: 1205.2391. UV-vis-NIR (in CH₂Cl₂) λ [nm] (ε [M⁻¹cm⁻¹]): 510 (11,4000).

2BF₂-Me-Hex(b): ¹H NMR (400 MHz, CDCl₃, 298 K) δ = 6.69 (d, J = 4 Hz, 2H), 6.61 (d, J = 4 Hz, 2H), 6.53 (d, J = 4 Hz, 4H), 6.36 (d, J = 4 Hz, 2H), 6.34 (d, J = 4 Hz, 2H), 2.41 (s, 6H), 2.26 (s, 6H), 2.06 (s, 6H) ppm. ¹⁹F NMR (376 MHz, CDCl₃, 213 K): δ = −133.07 (brs, 1F), −135.15 (m, 1F), −135.02 (m, 1F), −135.53 (m, 1F), −136.13 (m, 1F), −137.12 (m, 1F), −137.90 (m, 1F), −139.10 (brs, 1F), −143.15 (brs, 1F), −149.11 (t, J = 42 Hz, 1F), −149.83 (brs, 1F), −151.55 (t, J = 42 Hz, 1F), −158.93 (m, 3F), −159.83 (m, 1F), −160.16 (m, 2F) ppm. HR-MALDI-MS: Calculated for C₅₇H₃₁B₂F₁₉N₆Na = 1205.2391 [M+Na]⁺, Found: 1205.2397. UV-vis-NIR (in CH₂Cl₂) λ [nm] (ε [M⁻¹ cm⁻¹]): 500 (12,3000).

3BF₂-Me-Hex(a): ¹H NMR (400 MHz, CDCl₃, 298 K) δ = 6.70 (d, J = 4 Hz, 2H), 6.63 (d, J = 4 Hz, 2H), 6.50 (d, J = 4 Hz, 2H), 6.45 (d, J = 4 Hz, 2H), 6.43 (d, J = 4 Hz, 2H), 6.29 (d, J = 4 Hz, 2H), 2.32 (s, 3H), 2.29 (s, 3H), 2.22 (s, 3H) ppm. ¹⁹F NMR (376 MHz, CDCl₃): δ = −128.81 (brs, 2F), −132.02 (brs, 1F), −135.13 (m, 2F), −136.34 (m, 1F), −136.71 (m, 3F), −149.10 (brs, 1F), −150.09 (t, J = 41 Hz, 1F), −150.32 (t, J = 43 Hz, 2F), −151.50 (brs, 1F), −159.88 (m, 6F) ppm. HR-MALDI-MS: Calculated for C₅₇H₃₀B₃F₂₁N₆Na = 1253.2393 [M+Na]⁺, Found: 1253.2399. UV-vis-NIR (in CH₂Cl₂) λ [nm] (ε [M⁻¹cm⁻¹]): 525 nm (18,7000).

3BF₂-Me-Hex(b): ¹H NMR (400 MHz, CDCl_3, 298 K) δ = 6.76 − 6.73 (m, 6H), 6.36 − 6.31 (m, 6H), 2.13 (s, 6H), 2.11 (s, 6H,), 2.03 (s, 3H), 2.02 (s, 3H) ppm. ¹⁹F NMR (376 MHz, CDCl₃): δ = −136.37 (m, 6F), −139.86 (m, 2F), −143.61 (brs, 2F), −147.17 (brs, 2F), −150.10 (m, 3F), −159.64 (m, 6F) ppm. HR-MALDI-MS: Calculated for C₅₇H₃₀B₃F₂₁N₆Na = 1253.2393 [M+Na]⁺, Found: 1253.2393. UV-vis-NIR (in CH₂Cl₂) λ [nm] (ε [M⁻¹ cm⁻¹]): 512 (16,7000).

4. Conclusions

Five cyclic BODIPYs were synthesized from dimethyl-vinylene bridged hexaphyrin Me-Hex as effective expanded porphyrin-like ligand. The BF₂-Me-Hex, 2BF₂-Me-Hex(a), 2BF₂-Me-Hex(b), and 3BF₂-Me-Hex(a) form the distorted structure reflecting the molecular structure of Me-Hex. Alternatively, 3BF₂-Me-Hex(b) forms the co-planar structure, meaning that the transformation of the molecular skeleton of Me-Hex occurs during boron complexation. Optical property of cyclic BODIPYs affects their molecular structures. The macrocycles BF₂-Me-Hex, 2BF₂-Me-Hex(a) and 2BF₂-Me-Hex(b) having both the dipyrrin and BODIPY units exhibit no fluorescence because of ICT characteristics. In contrast, cyclic BODIPY trimers that consist only of BODIPY units show weak fluorescence. In addition, we experimentally revealed that the number of boron ions on cyclic BODIPYs is an important factor for the determination of their optical and electronic properties. Currently, we have been developing the chemistry of cyclic dipyrrins that are promising ligands for preparing cyclic BODIPY, which will take us to the next step for research on optical and electronic materials.