English

• 0.   Introduction

  During the past few years, the development of efficient sensors detecting metal ions has attracted wide attention. Some metal ions are strong toxic to the human body at very low concentration, such as mercury ions and palladium ions. Although some metal ions play a central part in our daily life and are widely used in industry, excessive uptake can also have harmful effects. Therefore, it is meaningful to selectively identify related ions for human health. At present, many ion detection sensor materials have been developed, such as ion recognition responsive materials based crown ether^[1], ion recognition materials based coordination compounds^[2-3], ion recognition materials based calix[4]arene^[4].

  Calix[4]arenes are highly applied into many fields, such as recognition, sensors, biomedicine^[5-9], because of their adjustable conformation and easy derivatization. Calix[4]arenes are especially prominent in sensors and selective receptors due to their func-tionalized structures and complexation possibilities^[10-12]. In the field of reco-gnition of ions, the design of highly selective and multifunctional calix[4]arene derivatives has become an important branch and is also an interesting aspect of supramolecular chemistry^[13-18]. Chemical modification of calix[4]arenes is one of the methods to prepare derivatives^[19-20]. Calix[4]arene derivatives modified by different functional moieties are obtained by introd-ucing characteristic groups, such as optical active groups and electrical active groups. Wong et al.^[21] investigated the property dependence of phenyl-calix[4]crown-4 on the upper rim substituent of methyl, fluorine or trimethylsilyl. Chawla et al.^[22] synthesized a series of para-substituted receptors which show selectivity to Cs⁺ and Rb⁺ ions by introducing arylazo, thiazolylazo, pyridylazo and β-naphthylazo groups into tetrathiacalix[4]arene. However, it was rarely reported that fluorine groups were introduced on the upper rim of calix[4]arene. It is due to the special properties of fluorine groups^[23-24] that few researchers synthesize fluorinated calix[4]arene derivatives. Herein, we synthesized fluorinated calix[4]arene derivatives by using Suzuki coupling reaction to modify the up-rim of calix[4]arenes and introduce fluorine and trifluoro-methyl groups into calix[4]arenes, and we studied their recognition properties.

  1.   Experimental

  1.1   General

  ¹H NMR spectra in CDCl₃ were detected on a Bruker 400 MHz spectrometer. FT-IR spectra were obtained by a Nicollet 6700 FT-IR spectrometer. UV-Vis spectral studies were carried out by using a TU-1901 spectrophotometer (Beijing Purkinje General Instrument). Fluorescence spectra were recorded on a Hitachi F-4600 fluorescence spectrometer. All the reagents and chemicals were commercially available and analytical pure.

  1.2   Synthesis of compound 1

  5, 11, 17, 23-Tetrabromo-25, 26, 27, 28-tetraethoxycalix[4]arene (a, 0.425 7 g, 0.5 mmol), 4-(trifluoromethyl)phenylboronic acid (0.372 5 g, 2.0 mmol) and sodium carbonate (0.424 0 g, 4 mmol) were mixed in the mixed solvent of toluene/ethanol/water (20 mL/10 mL/2 mL). The mixture was added tetrakis(triphenylphosphine)palladium((β-4)-platinum) after pumping vacuum and purging with nitrogen gas for three times. Subsequently, the mixture was heated at 80 ℃ to reflux under nitrogen protection and stirred for 24 h. The solution was stratified statically after the reaction completed. The inorganic layer was extracted with dichloromethane (6 mL×3), and the organic layer was washed with saturated salt water (6 mL×3). Successively, organic phases merged into one phase, which was dried with anhydrous sodium sulfate and concentrated by rotary evaporator. The raw solid was obtained. After the purification process by a silica gel column, the white solids of 5, 11, 17, 23-tetra(4-trifluoromethylphenyl)-25, 26, 27, 28-tetraethoxycalix[4]arene were obtained (0.110 g, Yield: 19.8%). Elemental Anal. Calcd. C₆₄H₅₂F₁₂O₄(%): C, 69.06; H, 4.70. Found(%): C, 70.20; H, 4.94. IR (KBr, cm^-1): ν_max 1 328(CF₃). ¹H NMR (400 MHz, CDCl₃): δ 7.39 (d, J=7.9 Hz, 4H, ArH), 7.27~7.18 (m, 5H, ArH), 6.95 (s, 4H, ArH), 4.59 (d, J=13.1 Hz, 2H, ArCH₂Ar), 4.12 (q, J=6.8 Hz, 4H, CH₂), 3.31 (d, J=13.2 Hz, 2H, ArCH₂Ar), 1.55 (t, J=6.7 Hz, 7H, CH₃).

  1.3   Synthesis of compound 2

  Compound a (0.426 7 g, 0.5 mmol) and 4-fluorophenylboronic acid (0.826 9 g, 2 mmol) were stirred in 32 mL of mixed solvents (V_toluene:V_ethanol:V_water=10:5:1) at ambient temperature. The sodium carbonate solution (2 mL, 2 mol·L^-1) was added to the mixture. Then the mixture was added (β-4)-platinum after vacuuming and sparging nitrogen gas several times and heated at 80 ℃ to reflux for 24 h. Finally, the reaction mixture was extracted with CH₂C_l2 and washed with saturated salt water. The product was purified by a silica gel column to give compound 2 as a white solid (0.100 g, yield 21.92%). Elemental Anal. Calcd. for C₆₀H₅₂F₄O₄(%): C, 78.93; H, 5.74. Found(%): C, 79.95; H, 6.56. IR (KBr, cm^-1): ν_max 1 227 (Ar-F). ¹H NMR (400 MHz, CDCl₃): δ 7.04 (dd, J=8.5, 5.4 Hz, 2H, ArH), 6.86 (s, 2H, ArH), 6.80 (t, J=8.7 Hz, 2H, ArH), 4.55 (d, J=13.1 Hz, 1H, ArCH₂Ar), 4.08 (q, J=7.0 Hz, 2H, CH₂), 3.26 (d, J=13.2 Hz, 1H, ArCH₂Ar), 1.53 (dd, J=13.5, 6.4 Hz, 6H, CH₃).

  1.4   Synthesis of compound 3

  A mixture of a (0.851 2 g, 1.0 mmol) and 3, 5-bis(trifluoromethyl)benzeneboronic acid (1.038 8 g, 4 mmol) in the presence of Na₂CO₃ (2.218 9 g) as the templating base under nitrogen in mixed solvent was stirred. (β-4)-Platinum was added in the solution after vacuuming three times. After all reagents were added, the resulting mixture was refluxed at 90 ℃ under the protection of nitrogen for 24 h. The solution was extracted with CH₂C_l2 and washed with saturated salt water three times after reaction. The solution was dried with anhydrous sodium sulfate. Then, the crude product was obtained by concentrating with rotary evaporator. Compound 3 was obtained by the purifica-tion process (0.130 g, Yield: 9.40%). Elemental Anal. Calcd. for C₆₈H₄₈F₂₄O₄(%): C, 58.97; H, 3.49. Found(%): C, 59.03; H, 3.51. IR (KBr, cm^-1): ν_max 1 272 (CF₃). ¹H NMR (400 MHz, CDCl₃): δ 7.58 (s, 1H, ArH), 7.43 (s, 2H, ArH), 6.94 (s, 2H, ArH), 4.60 (d, J=13.2 Hz, 1H, ArCH₂Ar), 4.12 (q, J=7.0 Hz, 2H, CH₂), 3.35 (d, J=13.3 Hz, 1H, ArCH₂Ar), 1.63~1.50 (m, 8H, CH₃).

  1.5   General procedure for UV-Vis study and fluorescence study

  Standard stock solutions (0.01 mol·L^-1) of metal acetate salts and chloride salts (NaCl, KCl, CsCl, Cu(Ac)₂·H₂O, BaCl₂·2H₂O, Zn(Ac)₂, Mg(Ac)₂·4H₂O, Cd(Ac)₂·2H₂O, Mn(Ac)₂·4H₂O, Co(Ac)₂·4H₂O, Ni(Ac)₂ ·4H₂O, FeCl₃, CaCl₂) were prepared in CH₃OH. The stock solutions (0.1 mmol·L^-1) of compounds 1~3 were prepared with CH₂C_l2. The solution concentration of compounds 1~3 is 5 μmol·L^-1 with different concen-trations of metal ions in the mixed solvent (V_CH2Cl2: V_CH3OH=1:1) in the titration experiments for UV-Vis and fluorescent studies.

  1.6   X-ray diffraction data collection and refinement

  Crystallographic data for 1 and 2 were collected at room temperature on a Bruker Smart CCD area detector diffractometer equipped with a graphite monochromated Mo Kα radiation (λ=0.071 073 nm) by ω-2θ scan mode. All absorption corrections were applied using the SADABS program^[25]. The Lp factor and empirical absorption were performed to correct the data, and to restore the data and correct the unit cell parameters by using SANIT and SMART software. The structures were solved by direct method and refined on F² by full-matrix least-squares using the SHELXTL-97 program package^[26]. All non-hydrogen atoms were refined with anisotropic displacement parameters. All hydrogen atoms were placed geometrically and were refined in a riding-model approximation. The crystallographic data of compound 1 and 2 are summarized in Table 1.

  Table 1

  

  Table 1.  Crystallographic data for compounds 1 and 2

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  Compound	1	2
  Empirical formula	C64H52F12O4	C60H52F4O4
  Formula weight	1 113.06	913.02
  Temperature / K	293(2)	293(2)
  Crystal system	Triclinic	Monoclinic
  Space group	P1	C2/c
  a / nm	1.293 25(L)	1.371 7(3)
  b / nm	1.534 64(9)	1.835 8(4)
  c / nm	1.859 67(11)	1.899 4(4)
  α /(°)	83.141(2)
  β /(°)	86.122(2)	95.660(7)
  γ /(°)	71.506(2)
  Volume / nm3	3.473 4(4)	4.759 8(17)
  Z	2	4
  Dc / (g·cm-3)	1.064	1.274
  F(000)	1 152	1 920
  Absorption coefficient / mm-1	0.087	0.089
  θ range for data collection / (°)	1.10~27.56	2.07~27.89
  Reflection collected	54 847	24 449
  Unique reflection	15 893	5 497
  Rint	0.044 4	0.049 3
  Data, restraint, parameter	15 893, 2, 726	5 497, 0, 300
  Goodness-of-fit on F2	1.346	1.047
  R1 indices [I>2σ(I)]	0.128 5	0.066 3
  wR2 indices (all data)	0.4142	0.210 2
  Largest diff. peak and hole / (e·nm-3)	949 and -527	544 and -355

  2.   Results and discussion

  2.1   Synthesis of compounds 1~3

  Modifying up-rim of calix[4]arene was imple-mented according to the Scheme 1. Compound a as raw materials can be prepared by published procedure^[27]. Thus, the Suzuki coupling reaction of tetrabromocalix[4]arene with fluorine-containing phenylboronic acid produced fluorine-containing calix[4]arene derivatives. The structures of compounds 1~3 were proved by respective IR, X-ray diffraction and ¹HNMR spectra.

  Scheme 1

  

  Scheme 1.  Synthetic routes for compounds 1~3

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  ¹H NMR spectroscopy can be used as a marker to identify the conformation of calix[4]arene deriva-tives because there are different characteristics with different conformations in ¹H NMR spectra^[28-30]. The conical conformation of the compound 1 can be confirmed by the presence of doublets at δ of 3.31 and 4.59 as an AB type proton signal of ArCH₂Ar in the ¹H NMR spectra. In the ¹H NMR spectra of compound 2, there were two doublets at δ of 3.26 and 4.45 for ArCH₂Ar, which confirmed the compound 2 is in the cone conformation. Compound 3 adopts the cone conformation due to the proton signal of methylene bridges at δ of 3.35 and 4.60 in ¹H NMR spectra. The IR spectra of compounds 1~3 show characteristic bands at 1 328 cm^-1(CF₃), 1 227 cm^-1 (Ar-F) and 1 272 cm^-1 (CF₃), respectively.

  2.2   Single crystal structure

  We successfully obtained colorless single crystals of compounds 1 and 2 from the mixed solvent (ethyl acetate/petroleum ether) and collected their structure data by single crystal X-ray diffractometer. As shown in Fig. 1 and 2, X-ray diffraction analysis revealed that compound 1 and 2 adopts conical conformations. Single crystals suitable for X-ray diffraction analysis of 3 were not obtained presently.

  Figure 1

  

  Figure 1.  Crystal structure (a) and π-π stacking interaction (b) of compound 1

  50% thermal ellipsoids

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  Figure 2

  

  Figure 2.  Crystal structure (a) and π-π stacking interaction (b) of compound 2

  All hydrogen atoms are omitted for clarity; 50% thermal ellipsoids; Symmetry codes: A: 2-x, y, 1/2-z

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  Compound 1 shows an asymmetric distorted cone conformation, in which the relatively long distance between the aromatic ring C1…C6 and C29…C34 is about 1.44 nm, and the short distance between the aromatic ring C15…C20 and C43…C48 is about 0.37 nm (Fig. 1). The nearest distance (0.37 nm) is attributed to the strong π-π stacking interactions in 1. The distance about 0.49 nm between the aromatic ring C21…C26 and C49…C54 displays hardly the π-π stacking interactions. The aromatic ring C21…C26 are rotated relative to the aromatic ring C15…C20, and torsion angle of C19-C18-C21-C26 is 37.2°. Similarly, torsion angle of C45-C46-C49-C50 is 40.5°.

  Compound 2 with a cone conformation was obtained through substituents of 4-fluorophenyl groups on upper rim, similar to compound 1. The distance between the aromatic rings C1…C6 and C1A…C6A is about 0.35 nm, which results from strong π-π interactions in 2 (Fig. 2). Torsion occurs between fluorophenyl-substituted aromatic rings C1…C6 and C7…C12, and torsion angle of C3-C4-C7-C8 is about 45.3°.

  2.3   UV-Vis spectroscopic studies

  Calix[4]arenes are considered to be perfect compounds for forming stable complexation with metal ions, such as Fe³⁺, Ni²⁺, Cu²⁺. Therefore, we studied and explored the fluorinated calix[4]arene for binding ability. The titration experiments were implemented to explore the interplay of compounds 1~3 with various metal ions and investigate its selectivity.

  As shown in Fig. 3, it can be found that the maximum ultraviolet absorption wavelength of comp-ounds 1~3 are in a range of 220~270 nm in the mixed solvent (V_CH2Cl2: V_CH3OH=1:1). The ultraviolet spectrum of compound 1 displayed strong peaks at 230 and 270 nm owing to π→π^* and n→π^* transitions. There were two peaks at 232 and 2 nm in the ultraviolet spectrum of compound 2, and the UV-Vis spectrum of 3 exhibited strong peaks at 225 and 266 nm.

  Figure 3

  

  Figure 3.  3 UV-Vis spectra of compounds 1~3 in mixed solvent CH₂C_l2/CH₃OH

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  The selectivity of 1~3 in mixed solvent (5 μmol·L^-1) to different metal ions (0.5 mmol·L^-1, excepted Fe³⁺) was preliminarily measured by UV-Vis spectros-copy. The wavelength with maximum absorbance upon the metal ion addition was listed in Table 2. On the basis of titration experiments, compound 1 exhibited a new band at 361 nm after adding Fe³⁺ (10 equiv.) (Fig. 4). After adding copper ions (100 equiv.), the new band appeared at 246 nm while the original peaks disappeared as shown in Fig. 4. Compared with the compound 1 in the absence of metal ions, the absorbance of the band enhanced greatly. Other metal ions, unlike iron or copper ions, only caused slight changes in absorption bands. Moreover, the color of compound 1 changed to yellow green after adding Cu²⁺ for 24 h (Fig. 4). The result reflects that 1 is more selective for Cu²⁺ ions.

  Table 2

  

  Table 2.  Maximum absorbance wavelength of compounds 1~3 after titration with metals ions

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  Compound	λmax / nm
  	Blank	Na+	K+	Cs+	Ba2+	Cu2+	Zn2+	Mg2++	Cd2+	Mn2+	Co2+	Ni+	Fe3+	Ca2+
  1	230	234	234	234	234	246	232	232	232	232	232	232	234	229
  	270	270	270	270	270		277	276	271	271	274	270	267	268
  													361
  2	232	228	230	227	229	237	230	230	230	229	228	228	229	229
  	258	258	258	258	258	240	258	258	258	258	258	258	257	258
  3	225	227	227	227	229	246	230	230	230	230	226	226	226	230
  	266	267	267	267	267		268	267	267	266	266	266	262	267
  													362
  *c1~c3=5 μmol·L-1, cFe3+=50 μmol·L-1, concentration of other metal ions: 0.5 mmol·L-1

  Figure 4

  

  Figure 4.  UV-Vis spectra of 1 with different metal ions (100 equiv. excepted Fe³⁺) in the mixed solvent CH₂C_l2/CH₃OH

  V_CH2Cl2: V_CH3OH; Inset: color changes: (a) 1, (b) 1 with Cu²⁺, (c) Cu²⁺ (0.5 mmol·L^-1)

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  The UV-Vis spectrum of compound 2 exhibited a significant increase of absorbance with the addition of Cu²⁺ (Fig. 5), and the bands shifted to 237 nm. The change of bands indicates that compound 2 has the ability to interact with copper ions. With the addition of nickel ions, the absorbance of compound 3 enhanced remarkably at 226 nm and decreased at 266 nm, although the absorption bands did not shift significantly (Fig. 6). In the presence of iron ions, the spectra showed gentle absorption peaks. In addition, it was visible that the new absorption band appeared at 246 and 362 nm, respectively, after copper and iron ions were added in the solution of compound 3 as shown in Fig. 6. The results show that copper ions, iron ions and nickel ions can interact with compound 3, especially copper ions have the most pronounced response.

  Figure 5

  

  Figure 5.  UV-Vis spectra of compound 2 with different metal ions (100 equiv., excepted Fe³⁺) in the mixed solvent CH₂C_l2/CH₃OH

  V_CH2Cl2: V_CH3OH=1:1; Inset: enlarged drawing of wavelength range of 200~350 nm

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  Figure 6

  

  Figure 6.  UV-Vis spectra of compound 3 with different metal ions (100 equiv., excepted Fe³⁺) in the mixed solvent CH₂C_l2/CH₃OH

  V_CH2Cl2: V_CH3OH=1:1; Inset: UV-Vis spectra of 3 alone, 3 with Cu²⁺, 3 with Ni²⁺, 3 with Fe³⁺

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  Compounds 1~3 show different binding abilities to metal ions, which possibly result from the following two factors: different substituents and substitution sites on the upper edge of calix[4]arenes. It can be seen that the factors affecting the selectivity of ligands to metal ions are not only the hard or soft properties of metal ions, but also the radius of ions, the size of holes and even the conformation of compounds. Many factors lead to the selectivity of different compounds to specific ions^[31-35].

  The selectivity of compounds 1~3 to copper ions was tested in existence of interfering ions by experi-ments adding Cu²⁺ ions and the other ions (1:1) (Fig. 7~9). It was found that other ions did not obviously interfere absorption spectra of the compounds with Cu²⁺. In addition, the interference of other ions on the binding of compound 3 to iron ions was also examined (Fig. 10). Other ions except Cu²⁺ did not affect the absorption spectra of compound 3 with iron ions. Adding copper ions broke down the binding of compound 3 to iron ions, which may be due to the higher binding efficiency of compound 3 to copper ions.

  Figure 7

  

  Figure 7.  Interference test of other ions on compound 1 with Cu²⁺ in the mixed solvent CH₂C_l2/CH₃OH

  V_CH2Cl2: V_CH3OH=1:1

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  Figure 8

  

  Figure 8.  Interference test of other ions on compound 2 with Cu²⁺ in the mixed solvent CH₂C_l2/CH₃OH

  V_CH2Cl2: V_CH3OH=1:1

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  Figure 9

  

  Figure 9.  Interference test of other ions on compound 3 with Cu²⁺ in the mixed solvent CH₂C_l2/CH₃OH

  V_CH2Cl2: V_CH3OH=1:1

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  Figure 10

  

  Figure 10.  Interference test of other ions on compound 3 with Fe³⁺ in the mixed solvent CH₂C_l2/CH₃OH

  V_CH2Cl2: V_CH3OH=1:1

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  2.4   Fluorescence studies

  The fluorescence spectra of compounds 1~3 (5 μmol·L^-1) were measured as shown in Fig. 11. The emission peak of 1 was 360.4 nm under the excitation of 294 nm, and there was a fluorescence peak of 2 at 348.4 nm when the exciting wavelength is 289 nm, while that of 3 was at 383.0 nm with excitation at 292 nm. The results from the fluorescence spectroscopy show that there is similarity in the optimum excitation wavelengths of the compounds.

  Figure 11

  

  Figure 11.  Fluorescence spectra of compounds 1~3 in the mixed solvent CH₂C_l2/CH₃OH

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  The binding of compounds 1~3 (5 μmol·L^-1) towards various ions (100 equiv., excepted Fe³⁺) was tested by fluorescence spectroscopy as showed in Fig. 12~14. The results of tests are consistent with those of ultraviolet spectra. The fluorescence intensity of compound 1 decreased sharply after adding copper ions, and there was obvious quenching in emission. The intensity of compound 2 decreased obviously in the existence of Cu²⁺ ions, while the other ions did not lead to remarkable changes. In the existence of copper and iron ions, the fluorescence intensity of compound 3 decreased. The intensity of compound 3 towards Cu²⁺ showed stronger quenching than that of compound 3 to Fe³⁺. Compound 3 is more compatible to Cu²⁺ than Fe³⁺. Upon addition of metal ions (100 equiv., except Fe³⁺), all metal ions more or less affect the emission intensity of compounds 1~3 despite no changing in the band of compound 1~3. In particular, the addition of copper and iron ions causes remarkable quenching in emission intensity. These results indicate that 1 and 2 only show high selectivity to Cu²⁺, and 3 is highly selective to iron and copper ions due to their different groups.

  Figure 12

  

  Figure 12.  Selectivity of compound 1 towards Cu²⁺ upon addition of various metal ions

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  Figure 13

  

  Figure 13.  Selectivity of compound 2 towards Cu²⁺ upon addition of various metal ions

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  Figure 14

  

  Figure 14.  Selectivity of compound 3 towards Cu²⁺ and Fe³⁺ upon addition of various metal ions

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  The selectivity of compounds 1~3 towards Cu²⁺ is further studied. The fluorescence quenching of compound 2 is more prominent, i.e. "Off state" (Fig. 13), compared to "On state" (Fig. 11), which has the highest selectivity to copper ions among compounds 1~3. Quenching of fluorescence in emission caused by Cu²⁺ is owing to reverse photo-induced electron transfer (reverse PET)^[36-37].

  In order to further observe the practical applicability of compounds 1~3 as fluorescent sensors for Cu²⁺ or Fe³⁺, we explored the interference of other ions. The competitive experiments were carried out on compounds 1~3 in the presence of copper ions (100 equiv.) or iron ions (10 equiv.) with an equal proportion of co-existing ions (Fig. 15~18). The results show that the fluorescence responses of compounds 1~3 to copper ions do not change significantly in the existence of other ions, and the fluorescence response of compound 3 to iron ions except copper ions shows small changes.

  Figure 15

  

  Figure 15.  Competitive selectivity of compound 1 towards Cu²⁺ in the presence of different cations in the mixed solvent CH₂C_l2/CH₃OH

  c₁=5 μmol·L^-1, V_CH2Cl2: V_CH3OH=1:1

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  Figure 16

  

  Figure 16.  Competitive selectivity of compound 2 towards Cu²⁺ in the presence of different cations in the mixed solvent CH₂C_l2/CH₃OH

  c₂=5 μmol·L^-1, V_CH2Cl2: V_CH3OH=1:1

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  Figure 17

  

  Figure 17.  Competitive selectivity of compound 3 towards Cu²⁺ in the presence of different cations in the mixed solvent CH₂C_l2/CH₃OH

  c₃=5 μmol·L^-1, V_CH2Cl2: V_CH3OH=1:1

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  Figure 18

  

  Figure 18.  Competitive selectivity of compound 3 towards Fe³⁺ in the presence of different cations in the mixed solvent CH₂C_l2/CH₃OH

  c₃=5 μmol·L^-1, V_CH2Cl2: V_CH3OH=1:1

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  3.   Conclusions

  In conclusion, we synthesized fluorinated calix[4]arene derivatives 1~3 in the cone conformation. The calix[4]arene derivatives were characterized by ¹H NMR, FT-IR, UV-Vis, fluorescence spectra analysis and so on. Compounds 1~3 show high significant selective nature to copper ions, which is indicated by UV-Vis and fluorescence techniques. The ultraviolet intensity of compounds 1~3 increased, new bands appeared and fluorescence quenching occurred in the presence of copper ions. At the same time, compound 3 exhibits higher selectivity to copper ions than iron ions. This kind of molecular switch may be utilized as a Cu²⁺ selective sensor.

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  Scheme 1  Synthetic routes for compounds 1~3

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  Figure 1  Crystal structure (a) and π-π stacking interaction (b) of compound 1

  50% thermal ellipsoids

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  Figure 2  Crystal structure (a) and π-π stacking interaction (b) of compound 2

  All hydrogen atoms are omitted for clarity; 50% thermal ellipsoids; Symmetry codes: A: 2-x, y, 1/2-z

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  Figure 3  3 UV-Vis spectra of compounds 1~3 in mixed solvent CH₂C_l2/CH₃OH

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  Figure 4  UV-Vis spectra of 1 with different metal ions (100 equiv. excepted Fe³⁺) in the mixed solvent CH₂C_l2/CH₃OH

  V_CH2Cl2: V_CH3OH; Inset: color changes: (a) 1, (b) 1 with Cu²⁺, (c) Cu²⁺ (0.5 mmol·L^-1)

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  Figure 5  UV-Vis spectra of compound 2 with different metal ions (100 equiv., excepted Fe³⁺) in the mixed solvent CH₂C_l2/CH₃OH

  V_CH2Cl2: V_CH3OH=1:1; Inset: enlarged drawing of wavelength range of 200~350 nm

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  Figure 6  UV-Vis spectra of compound 3 with different metal ions (100 equiv., excepted Fe³⁺) in the mixed solvent CH₂C_l2/CH₃OH

  V_CH2Cl2: V_CH3OH=1:1; Inset: UV-Vis spectra of 3 alone, 3 with Cu²⁺, 3 with Ni²⁺, 3 with Fe³⁺

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  Figure 7  Interference test of other ions on compound 1 with Cu²⁺ in the mixed solvent CH₂C_l2/CH₃OH

  V_CH2Cl2: V_CH3OH=1:1

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  Figure 8  Interference test of other ions on compound 2 with Cu²⁺ in the mixed solvent CH₂C_l2/CH₃OH

  V_CH2Cl2: V_CH3OH=1:1

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  Figure 9  Interference test of other ions on compound 3 with Cu²⁺ in the mixed solvent CH₂C_l2/CH₃OH

  V_CH2Cl2: V_CH3OH=1:1

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  Figure 10  Interference test of other ions on compound 3 with Fe³⁺ in the mixed solvent CH₂C_l2/CH₃OH

  V_CH2Cl2: V_CH3OH=1:1

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  Figure 11  Fluorescence spectra of compounds 1~3 in the mixed solvent CH₂C_l2/CH₃OH

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  Figure 12  Selectivity of compound 1 towards Cu²⁺ upon addition of various metal ions

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  Figure 13  Selectivity of compound 2 towards Cu²⁺ upon addition of various metal ions

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  Figure 14  Selectivity of compound 3 towards Cu²⁺ and Fe³⁺ upon addition of various metal ions

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  Figure 15  Competitive selectivity of compound 1 towards Cu²⁺ in the presence of different cations in the mixed solvent CH₂C_l2/CH₃OH

  c₁=5 μmol·L^-1, V_CH2Cl2: V_CH3OH=1:1

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  Figure 16  Competitive selectivity of compound 2 towards Cu²⁺ in the presence of different cations in the mixed solvent CH₂C_l2/CH₃OH

  c₂=5 μmol·L^-1, V_CH2Cl2: V_CH3OH=1:1

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  Figure 17  Competitive selectivity of compound 3 towards Cu²⁺ in the presence of different cations in the mixed solvent CH₂C_l2/CH₃OH

  c₃=5 μmol·L^-1, V_CH2Cl2: V_CH3OH=1:1

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  Figure 18  Competitive selectivity of compound 3 towards Fe³⁺ in the presence of different cations in the mixed solvent CH₂C_l2/CH₃OH

  c₃=5 μmol·L^-1, V_CH2Cl2: V_CH3OH=1:1

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  Table 1.  Crystallographic data for compounds 1 and 2

  Compound	1	2
  Empirical formula	C64H52F12O4	C60H52F4O4
  Formula weight	1 113.06	913.02
  Temperature / K	293(2)	293(2)
  Crystal system	Triclinic	Monoclinic
  Space group	P1	C2/c
  a / nm	1.293 25(L)	1.371 7(3)
  b / nm	1.534 64(9)	1.835 8(4)
  c / nm	1.859 67(11)	1.899 4(4)
  α /(°)	83.141(2)
  β /(°)	86.122(2)	95.660(7)
  γ /(°)	71.506(2)
  Volume / nm3	3.473 4(4)	4.759 8(17)
  Z	2	4
  Dc / (g·cm-3)	1.064	1.274
  F(000)	1 152	1 920
  Absorption coefficient / mm-1	0.087	0.089
  θ range for data collection / (°)	1.10~27.56	2.07~27.89
  Reflection collected	54 847	24 449
  Unique reflection	15 893	5 497
  Rint	0.044 4	0.049 3
  Data, restraint, parameter	15 893, 2, 726	5 497, 0, 300
  Goodness-of-fit on F2	1.346	1.047
  R1 indices [I>2σ(I)]	0.128 5	0.066 3
  wR2 indices (all data)	0.4142	0.210 2
  Largest diff. peak and hole / (e·nm-3)	949 and -527	544 and -355

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  Table 2.  Maximum absorbance wavelength of compounds 1~3 after titration with metals ions

  Compound	λmax / nm
  	Blank	Na+	K+	Cs+	Ba2+	Cu2+	Zn2+	Mg2++	Cd2+	Mn2+	Co2+	Ni+	Fe3+	Ca2+
  1	230	234	234	234	234	246	232	232	232	232	232	232	234	229
  	270	270	270	270	270		277	276	271	271	274	270	267	268
  													361
  2	232	228	230	227	229	237	230	230	230	229	228	228	229	229
  	258	258	258	258	258	240	258	258	258	258	258	258	257	258
  3	225	227	227	227	229	246	230	230	230	230	226	226	226	230
  	266	267	267	267	267		268	267	267	266	266	266	262	267
  													362
  *c1~c3=5 μmol·L-1, cFe3+=50 μmol·L-1, concentration of other metal ions: 0.5 mmol·L-1

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