# Synthesis and Study in Solution of a New Dansyl-Modified Azacryptand

Authors: Greta Bergamaschi; Ana Miljkovic; Stefania Marcheggiani; Antonio Poggi
Journal: International Journal of Inorganic Chemistry
 (2016)

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## Abstract

We report the synthesis of a new asymmetric azacryptand (L1), characterized by three p-xylyl spacers, one of which carries a dansyl side arm. The fluorescent sensor has been studied by potentiometric, UV-Vis, and emission studies in MeOH : water 3 : 2 mixture (0.07 M NaNO3), determining, in particular, the protonation constants of the free ligand and metal ion complexation equilibria. Interestingly, the obtained results revealed that the new receptor is fluorescent at neutral pH with a typical emission band of the dansyl group. Metal addition induced a partial quenching of the dansyl emission band; this behavior is more pronounced with Cu(II) that reduces the receptor’s emission by 60%. With all the studied cations, quenching follows the formation of a dimetallic complex. Similar studies on the model compoundL2confirmed that fluorescence quenching is mainly driven by a static mechanism, attributable to the formation of the inclusion dicopper complex [L1Cu2]4+. In order to test the stability of copper complexes under physiological conditions, spectrofluorimetric titrations with Cu(II) were performed in water buffered at pH = 8 (HEPES 0.07 M) and the values of binding constants, K11 and K12, were determined.


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## Body

## 1. Introduction

The detection of transition metal ions is a significant research field due to cations’ relevance in life science, medicine, biology, and chemistry [1–6]. For these reasons, many cation sensors have been described and synthesized; fluorescent chemosensors, in particular, are very intriguing thanks to the low detection limits of the fluorescence technique [7–11]. Functionalized polyamine macrocycles and macrobicycles are often used as receptors; however, by introducing fluorescent signaling units in the molecular skeleton (e.g., anthracene or naphthalene), they can be also converted into efficient chemosensors [12–15]. In this field, bistren azacryptands have been deeply investigated, due to the possibility of modulating their cavity shape [16–22]. Bistren ligands can include two transition metal ions (e.g., Cu2+or Zn2+), one of each bound to the four amine nitrogen atoms of a tris(2-aminoethyl)amine (tren) subunit. The unsaturated apical position of each Cu(II) cation can be occupied by a molecule of solvent or by a bidentate anion; in this way, the encapsulated Cu2+achieves a five-coordination geometry, according to an axially compressed trigonal bipyramidal geometry. Dimetallic bistren cryptands were synthesized for the first time by Lehn [23–25].In general, fluorescent azacryptands show a weak fluorescence at neutral pH; in fact, amino groups are able to quench the fluorophore emission by a photoinduced electron transfer (PET) mechanism [26]. Among the best known fluorescent fragments, the dansyl fluorophore (5-dimethylamino-1-naphthalene sulfonate) is characterized by an intense fluorescence emission in the visible spectrum, due to a charge-transfer excited state [27]. Moreover, high emission quantum yield and biological compatibility make the use of dansylated sensors very promising for application under physiological conditions [28–30]. In the present work, we report the synthesis and the characterization of the new asymmetric receptor containing a dansylated side arm (L1, see Scheme 1). In particular, the protonation constants of the free ligand and copper complexation equilibria in MeOH : water mixture have been investigated through potentiometric and spectrofluorometric experiments. The binding tendencies of the cage-like system towards copper (II) and zinc (II) have been also studied in MeOH and aqueous solution.Scheme 1
Formation of the dimetallic complex.


## 2. Experimental

### 2.1. Chemicals and Methods

All reagents for syntheses were purchased form Aldrich/Fluka or Alfa-Aesar Chemical Co. and used without further purification. All reactions were performed under nitrogen. The solutions used in titrations were prepared from freshly opened solvent bottles. Mass spectra were acquired on a Thermo-Finnigan ion-trap LCQ Advantage Max instrument equipped with an ESI source, and NMR spectra were recorded on a Bruker ADVANCE 400 spectrometer (operating at 9.37 T, 400 MHz). UV-Vis spectra were run on a Varian Cary 100 SCAN spectrophotometer with quartz cuvettes of the appropriate path length (0.1−1 cm) at 25.0 ± 0.1°C under inert conditions. Emission spectra were recorded on a Perkin-Elmer LS 50B instrument.


### 2.2. Synthesis ofL1 andL2

The synthesis of dialdehyde2 andL1 and is reported in Scheme 2, including H-labelling for NMR interpretation.Scheme 2
Step-by-step synthesis ofL1.


#### 2.2.1. Synthesis of 2-Dansyl-1,4-benzenedicarboxaldehyde2

The dialdehyde1 was obtained following the procedures reported in the literature [31]. Reagent2 was prepared by modifying a described procedure [32].2-Hydroxy-1,4-benzenedicarboxaldehyde (0.1 g, 0.68 mmol) and dansyl chloride (0.2 g, 0.68 mmol) were suspended in 2 mL CH2Cl2. 0.1 g of 1,4-diazabicyclooctane (0.93 mmol) in 1 mL of CH2Cl2 was added and the reaction mixture was stirred at room temperature for 48 hrs under an inert atmosphere. The crude product was purified by column chromatography (SiO2, hexane, hexane-AcOEt mixture 5%–25% gradient). A yellow solid was obtained (yield 52%).1H NMR (400 MHz, CDCl3, ppm): δ 3.1 (6H, s, Ha), 7.3 (1H, d, Hb), 7.4 (1H, d, Hh), 7.5 (1H, t, Hf), 7.7 (1H, t, Hc), 7.8 (1H, dd, Hj), 8.0 (1H, d, Hi), 8.1 (1H, dd, Hg), 8.5 (1H, d, Hd), 8.7 (1H, d, He), 9.9 (1H, s, Hk), 10.2 (1H, s, Hl).


#### 2.2.2. Synthesis ofL1

A solution of2 (0.10 g, 0.26 mmol) in 70 mL of MeOH was added dropwise to a stirred solution of the p-xylyl intermediate macrocycleL (0.13 g, 0.26 mmol, prepared following a published procedure [33]) in 120 mL of MeOH over 3 h at room temperature. After 24 h stirring, the mixture was heated to 50°C and hydrogenated with NaBH4 (0.2 g, 5.2 mmol). When the addition was complete, the stirring was continued at 50°C overnight. The solvent was removed; the residue was dissolved in basic water (20 mL, 3 M NaOH) and extracted with 15 mL of CH2Cl2 (×7). The collected organic phases were dried over Na2SO4and evaporated to dryness. An orange solid was obtained (yield 54%).MS (ESI, MeOH, pos.):m
/
z 425.2 [M + 2H]2+, 848.6 [M + H]+.1H NMR (400 MHz, CD3OD, ppm): δ 2.8 (24H, m, Hk, Hk’, Hj, Hj’), 2.9 (6H, s, Ha), 3.5 (4H, d, Hi), 3.7 (8H, d, Hi’), 6.8 (11H, m, Hh, Hh’), 7.2 (1H, d, Hb), 7.4 (1H, t, Hf), 7.6 (1H, t, Hc), 8.1 (1H, d, Hg), 8.4 (1H, d, Hd), 8.6 (1H, d, He).


#### 2.2.3. Synthesis ofL2

In order to explain the coordination properties of the new fluorescent azacryptand, the model compoundL2 was synthesized (Scheme 3).L2 was prepared by modifying a described procedure [32]: phenol (0.1 g, 1.0 mmol) and dansyl chloride (0.3 g, 1.0 mmol) were dissolved in 2 mL CH2Cl2. 0.2 g of 1,4-diazabicyclooctane (1.8 mmol) in 1 mL of CH2Cl2 was added and the reaction mixture was stirred at room temperature for 24 hrs under an inert atmosphere. The crude product was purified by column chromatography (SiO2, hexane : AcOEt mixture 1 : 1). A yellow solid was obtained (yield 45%).Scheme 3
Synthesis ofL2.1H NMR (400 MHz, CDCl3, ppm): δ 2.9 (6H, s, Ha), 6.8 (3H, m, Hh, Hi, Hl), 7.1 (2H, m, Hj, Hk), 7.2 (1H, s, Hb), 7.4 (1H, t, Hf), 7.7 (1H, t, Hc), 8.1 (1H, dd, Hg), 8.5 (1H, d, Hd), 8.6 (1H, d, He).


### 2.3. Potentiometric Titrations

All titrations were performed at 25.0 ± 0.1°C. Protonation constants of ligandL1 were determined in a MeOH/water (3 : 2) mixture, 0.07 M in NaNO3. In a typical experiment, 10 mL of a 7 × 10−4 M ligand solution was treated with an excess of a 1.0 M HNO3 standard solution. Titrations were run by addition of 10 μL aliquots of carbonate-free standard 0.1 M NaOH, recording 80–100 points for each titration. Complexation constants were determined by carrying out a similar potentiometric titration experiment, with the additional presence of 2 eqv. of C
u
I
I(CF3SO3)2. Prior to each potentiometric titration, the standard electrochemical potential (E°) of the glass electrode was determined in the MeOH/water (1 : 4) mixture, by a titration experiment according to the Gran method [34, 35]. Protonation and complexation titration data (emf versus mL of NaOH) were processed with the Hyperquad® package [36] to determine the equilibrium constants (reported in Table 1). In the pH-spectrophotometric/spectrofluorimetric titration experiments, the UV-Vis/emission spectra of the solution were recorded after each addition of standard 0.1 M NaOH.Table 1
Logarithmic protonation and complex formation constants forL1 (standard deviations in parentheses).
log
⁡
β values
[
L1H1
]
+
8.63 (1)
[
L1H2
]
2+
16.75 (1)
[
L1H3
]
3+
23.89 (1)
[
L1H4
]
4+
29.95 (2)
[
L1H5
]
5+
35.76 (2)
[
L1H6
]
6+
38.79 (2)
[
L1H7
]
7+
40.49 (2)
[
L1H3Cu]
5+
30.13 (1)
[
L1H2Cu]
4+
25.56 (2)
[
L1Cu2
]
4+
17.87 (2)
[
L1Cu2(OH)]
3+
10.63 (2)


### 2.4. Spectrophotometric and Spectrofluorimetric Titrations

UV-Vis spectra of the azacryptand in the presence of metal ions were run on a Varian Cary 100 SCAN spectrophotometer with quartz cuvettes of the appropriate path length (0.1–1 cm) at 25.0 ± 0.1°C under inert conditions. In any case, the concentration of the ligand and the optical path were adjusted to obtain spectra with AU ~ 1.Titrations with metal ions were performed at 25.0 ± 0.1°C in pure water and in MeOH/water (3 : 2) mixture, buffered at pH 8 (0.07 M HEPES). In a typical experiment, the solution of the receptor was titrated with a 100-fold more concentrated solution of the trifluoromethanesulfonate salt of the envisaged transition metals. In spectrofluorimetric titrations, the sample was excited at a wavelength corresponding to an isosbestic point in the family of UV-Vis spectra. Titration data were processed with a nonlinear least-squares procedure (Hyperquad package) [36], in order to determine the equilibrium constants.


## 2.1. Chemicals and Methods

All reagents for syntheses were purchased form Aldrich/Fluka or Alfa-Aesar Chemical Co. and used without further purification. All reactions were performed under nitrogen. The solutions used in titrations were prepared from freshly opened solvent bottles. Mass spectra were acquired on a Thermo-Finnigan ion-trap LCQ Advantage Max instrument equipped with an ESI source, and NMR spectra were recorded on a Bruker ADVANCE 400 spectrometer (operating at 9.37 T, 400 MHz). UV-Vis spectra were run on a Varian Cary 100 SCAN spectrophotometer with quartz cuvettes of the appropriate path length (0.1−1 cm) at 25.0 ± 0.1°C under inert conditions. Emission spectra were recorded on a Perkin-Elmer LS 50B instrument.


## 2.2. Synthesis ofL1 andL2

The synthesis of dialdehyde2 andL1 and is reported in Scheme 2, including H-labelling for NMR interpretation.Scheme 2
Step-by-step synthesis ofL1.


### 2.2.1. Synthesis of 2-Dansyl-1,4-benzenedicarboxaldehyde2

The dialdehyde1 was obtained following the procedures reported in the literature [31]. Reagent2 was prepared by modifying a described procedure [32].2-Hydroxy-1,4-benzenedicarboxaldehyde (0.1 g, 0.68 mmol) and dansyl chloride (0.2 g, 0.68 mmol) were suspended in 2 mL CH2Cl2. 0.1 g of 1,4-diazabicyclooctane (0.93 mmol) in 1 mL of CH2Cl2 was added and the reaction mixture was stirred at room temperature for 48 hrs under an inert atmosphere. The crude product was purified by column chromatography (SiO2, hexane, hexane-AcOEt mixture 5%–25% gradient). A yellow solid was obtained (yield 52%).1H NMR (400 MHz, CDCl3, ppm): δ 3.1 (6H, s, Ha), 7.3 (1H, d, Hb), 7.4 (1H, d, Hh), 7.5 (1H, t, Hf), 7.7 (1H, t, Hc), 7.8 (1H, dd, Hj), 8.0 (1H, d, Hi), 8.1 (1H, dd, Hg), 8.5 (1H, d, Hd), 8.7 (1H, d, He), 9.9 (1H, s, Hk), 10.2 (1H, s, Hl).


### 2.2.2. Synthesis ofL1

A solution of2 (0.10 g, 0.26 mmol) in 70 mL of MeOH was added dropwise to a stirred solution of the p-xylyl intermediate macrocycleL (0.13 g, 0.26 mmol, prepared following a published procedure [33]) in 120 mL of MeOH over 3 h at room temperature. After 24 h stirring, the mixture was heated to 50°C and hydrogenated with NaBH4 (0.2 g, 5.2 mmol). When the addition was complete, the stirring was continued at 50°C overnight. The solvent was removed; the residue was dissolved in basic water (20 mL, 3 M NaOH) and extracted with 15 mL of CH2Cl2 (×7). The collected organic phases were dried over Na2SO4and evaporated to dryness. An orange solid was obtained (yield 54%).MS (ESI, MeOH, pos.):m
/
z 425.2 [M + 2H]2+, 848.6 [M + H]+.1H NMR (400 MHz, CD3OD, ppm): δ 2.8 (24H, m, Hk, Hk’, Hj, Hj’), 2.9 (6H, s, Ha), 3.5 (4H, d, Hi), 3.7 (8H, d, Hi’), 6.8 (11H, m, Hh, Hh’), 7.2 (1H, d, Hb), 7.4 (1H, t, Hf), 7.6 (1H, t, Hc), 8.1 (1H, d, Hg), 8.4 (1H, d, Hd), 8.6 (1H, d, He).


### 2.2.3. Synthesis ofL2

In order to explain the coordination properties of the new fluorescent azacryptand, the model compoundL2 was synthesized (Scheme 3).L2 was prepared by modifying a described procedure [32]: phenol (0.1 g, 1.0 mmol) and dansyl chloride (0.3 g, 1.0 mmol) were dissolved in 2 mL CH2Cl2. 0.2 g of 1,4-diazabicyclooctane (1.8 mmol) in 1 mL of CH2Cl2 was added and the reaction mixture was stirred at room temperature for 24 hrs under an inert atmosphere. The crude product was purified by column chromatography (SiO2, hexane : AcOEt mixture 1 : 1). A yellow solid was obtained (yield 45%).Scheme 3
Synthesis ofL2.1H NMR (400 MHz, CDCl3, ppm): δ 2.9 (6H, s, Ha), 6.8 (3H, m, Hh, Hi, Hl), 7.1 (2H, m, Hj, Hk), 7.2 (1H, s, Hb), 7.4 (1H, t, Hf), 7.7 (1H, t, Hc), 8.1 (1H, dd, Hg), 8.5 (1H, d, Hd), 8.6 (1H, d, He).


## 2.2.1. Synthesis of 2-Dansyl-1,4-benzenedicarboxaldehyde2

The dialdehyde1 was obtained following the procedures reported in the literature [31]. Reagent2 was prepared by modifying a described procedure [32].2-Hydroxy-1,4-benzenedicarboxaldehyde (0.1 g, 0.68 mmol) and dansyl chloride (0.2 g, 0.68 mmol) were suspended in 2 mL CH2Cl2. 0.1 g of 1,4-diazabicyclooctane (0.93 mmol) in 1 mL of CH2Cl2 was added and the reaction mixture was stirred at room temperature for 48 hrs under an inert atmosphere. The crude product was purified by column chromatography (SiO2, hexane, hexane-AcOEt mixture 5%–25% gradient). A yellow solid was obtained (yield 52%).1H NMR (400 MHz, CDCl3, ppm): δ 3.1 (6H, s, Ha), 7.3 (1H, d, Hb), 7.4 (1H, d, Hh), 7.5 (1H, t, Hf), 7.7 (1H, t, Hc), 7.8 (1H, dd, Hj), 8.0 (1H, d, Hi), 8.1 (1H, dd, Hg), 8.5 (1H, d, Hd), 8.7 (1H, d, He), 9.9 (1H, s, Hk), 10.2 (1H, s, Hl).


## 2.2.2. Synthesis ofL1

A solution of2 (0.10 g, 0.26 mmol) in 70 mL of MeOH was added dropwise to a stirred solution of the p-xylyl intermediate macrocycleL (0.13 g, 0.26 mmol, prepared following a published procedure [33]) in 120 mL of MeOH over 3 h at room temperature. After 24 h stirring, the mixture was heated to 50°C and hydrogenated with NaBH4 (0.2 g, 5.2 mmol). When the addition was complete, the stirring was continued at 50°C overnight. The solvent was removed; the residue was dissolved in basic water (20 mL, 3 M NaOH) and extracted with 15 mL of CH2Cl2 (×7). The collected organic phases were dried over Na2SO4and evaporated to dryness. An orange solid was obtained (yield 54%).MS (ESI, MeOH, pos.):m
/
z 425.2 [M + 2H]2+, 848.6 [M + H]+.1H NMR (400 MHz, CD3OD, ppm): δ 2.8 (24H, m, Hk, Hk’, Hj, Hj’), 2.9 (6H, s, Ha), 3.5 (4H, d, Hi), 3.7 (8H, d, Hi’), 6.8 (11H, m, Hh, Hh’), 7.2 (1H, d, Hb), 7.4 (1H, t, Hf), 7.6 (1H, t, Hc), 8.1 (1H, d, Hg), 8.4 (1H, d, Hd), 8.6 (1H, d, He).


## 2.2.3. Synthesis ofL2

In order to explain the coordination properties of the new fluorescent azacryptand, the model compoundL2 was synthesized (Scheme 3).L2 was prepared by modifying a described procedure [32]: phenol (0.1 g, 1.0 mmol) and dansyl chloride (0.3 g, 1.0 mmol) were dissolved in 2 mL CH2Cl2. 0.2 g of 1,4-diazabicyclooctane (1.8 mmol) in 1 mL of CH2Cl2 was added and the reaction mixture was stirred at room temperature for 24 hrs under an inert atmosphere. The crude product was purified by column chromatography (SiO2, hexane : AcOEt mixture 1 : 1). A yellow solid was obtained (yield 45%).Scheme 3
Synthesis ofL2.1H NMR (400 MHz, CDCl3, ppm): δ 2.9 (6H, s, Ha), 6.8 (3H, m, Hh, Hi, Hl), 7.1 (2H, m, Hj, Hk), 7.2 (1H, s, Hb), 7.4 (1H, t, Hf), 7.7 (1H, t, Hc), 8.1 (1H, dd, Hg), 8.5 (1H, d, Hd), 8.6 (1H, d, He).


## 2.3. Potentiometric Titrations

All titrations were performed at 25.0 ± 0.1°C. Protonation constants of ligandL1 were determined in a MeOH/water (3 : 2) mixture, 0.07 M in NaNO3. In a typical experiment, 10 mL of a 7 × 10−4 M ligand solution was treated with an excess of a 1.0 M HNO3 standard solution. Titrations were run by addition of 10 μL aliquots of carbonate-free standard 0.1 M NaOH, recording 80–100 points for each titration. Complexation constants were determined by carrying out a similar potentiometric titration experiment, with the additional presence of 2 eqv. of C
u
I
I(CF3SO3)2. Prior to each potentiometric titration, the standard electrochemical potential (E°) of the glass electrode was determined in the MeOH/water (1 : 4) mixture, by a titration experiment according to the Gran method [34, 35]. Protonation and complexation titration data (emf versus mL of NaOH) were processed with the Hyperquad® package [36] to determine the equilibrium constants (reported in Table 1). In the pH-spectrophotometric/spectrofluorimetric titration experiments, the UV-Vis/emission spectra of the solution were recorded after each addition of standard 0.1 M NaOH.Table 1
Logarithmic protonation and complex formation constants forL1 (standard deviations in parentheses).
log
⁡
β values
[
L1H1
]
+
8.63 (1)
[
L1H2
]
2+
16.75 (1)
[
L1H3
]
3+
23.89 (1)
[
L1H4
]
4+
29.95 (2)
[
L1H5
]
5+
35.76 (2)
[
L1H6
]
6+
38.79 (2)
[
L1H7
]
7+
40.49 (2)
[
L1H3Cu]
5+
30.13 (1)
[
L1H2Cu]
4+
25.56 (2)
[
L1Cu2
]
4+
17.87 (2)
[
L1Cu2(OH)]
3+
10.63 (2)


## 2.4. Spectrophotometric and Spectrofluorimetric Titrations

UV-Vis spectra of the azacryptand in the presence of metal ions were run on a Varian Cary 100 SCAN spectrophotometer with quartz cuvettes of the appropriate path length (0.1–1 cm) at 25.0 ± 0.1°C under inert conditions. In any case, the concentration of the ligand and the optical path were adjusted to obtain spectra with AU ~ 1.Titrations with metal ions were performed at 25.0 ± 0.1°C in pure water and in MeOH/water (3 : 2) mixture, buffered at pH 8 (0.07 M HEPES). In a typical experiment, the solution of the receptor was titrated with a 100-fold more concentrated solution of the trifluoromethanesulfonate salt of the envisaged transition metals. In spectrofluorimetric titrations, the sample was excited at a wavelength corresponding to an isosbestic point in the family of UV-Vis spectra. Titration data were processed with a nonlinear least-squares procedure (Hyperquad package) [36], in order to determine the equilibrium constants.


## 3. Results and Discussion

### 3.1. Synthesis

Bistren symmetric cryptands are usually synthesized through Schiff base condensation of two molecules of tris(2-aminoethyl)amine (tren) and three molecules of the desired dialdehyde [37, 38] followed by reduction with NaBH4of the imine groups. The new asymmetric azacryptand presented in this work required a multistep synthesis (see Scheme 2 in Section 2) recently described by our group [26, 31, 33]. In particular, 1 mol of mono-BOC-protected tren was first reacted with 1 mol of the 1,4-p-xylyl dialdehyde, obtaining the intermediate polyimine macrocycle1. After reduction with NaBH4 and deprotection of the secondary amine groups, precursor1 was reacted with 2-dansyl-1,4-benzenedicarboxaldehyde (2), in a 1 : 1 ratio. Reduction of the imine groups yieldedL1 without further purification (see Section 2 for details). Thanks to this approach, we obtained a new fluorescent receptor with a fluorescent dansyl group covalently linked on one of the three p-xylyl spacers.


### 3.2. Potentiometric/pH-Spectrophotometric Studies in Aqueous Mixture

In order to study the acid-base behavior of the new receptor, potentiometric titrations have been performed on the asymmetric azacryptand (L1) in H2O : MeOH 3 : 2 mixture (0.07 M NaNO3, at 25°C) by addition of standard acid. The use of a solvent mixture is fundamental to guarantee solubility in the whole pH range (2.5–11). Experimental results were fitted with Hyperquad package [36] and the obtained protonation constants are reported in Table 1.In the pH range considered, only seven protonation constants could be determined, attributable to the protonation of the six secondary amines of the azacryptand and the tertiary amino group of the dansyl moiety. Notably, the protonation of the receptor’s tertiary amino groups was not observed in these conditions. The obtained protonation constant of the NMe2 groups, log
⁡
K
=
1.7, is comparable to that of the system reported by Prodi and coworkers [39].pH-spectrophotometric experiments confirmed these results; Figure1 shows the family of spectra taken over the course of the pH-spectrophotometric titration ofL1(0.5 mM) in MeOH : H2O mixture (0.07 M NaNO3).Figure 1
Family of UV-Vis spectra taken over the pH-spectrophotometric titration ofL1 (0.5 mM,T = 25°C, 0.07 M NaNO3). Long dash line: initial spectrum at pH = 2.5; solid line: spectrum at pH = 11.At acidic pH values, the receptor shows the typical UV/Vis spectrum of the naphthyl group [40] with an intense band at λmax = 288 nm (black dashed line spectrum). Upon deprotonation of the dansyl moiety, the absorption at 288 nm decreases and a new band appears at 340 nm. This new band is attributable to the typical charge transfer of the dansyl group (NMe2→ naphthyl) [27]. The titration profiles obtained at 288 and 340 nm well fit the distribution diagram of the species shown in Figure 2.Figure 2
Distribution diagram of the species (% abundance versus pH) obtained upon potentiometric titration ofL1 in H2O : MeOH 3 : 2 mixture (0.5 mM, 0.07 M NaNO3, at 25°C). The corresponding protonation constants are shown in Table 1. Triangles: profiles of Mol Abs (×10−3, M−1 cm−1) at 288 nm (black) and 340 nm (white), respectively, obtained upon pH-spectrophotometric titration (right vertical axes, see Figure 1).Analogous experiments have been carried out in the presence of 2 equiv. ofC
u
I
I(CF3SO3)2. For cryptandL1, the best data fitting was obtained by assuming the formation of the following copper species on increasing pH: [L1H3Cu]5+, [L1H2Cu]4+, [L1Cu2]4+, and [L1Cu2(OH) ]3+. The formation constants of the copper species are reported in Table 1 and the corresponding distribution diagrams are reported in Figure 3.Figure 3
Distribution diagram of the species (% abundance versus pH) obtained upon potentiometric titration ofL1 (0.5 mM), in the presence of 2 equiv. Cu(CF3SO3)2 (0.07 M NaNO3, H2O : MeOH 3 : 2 at 25°C). The corresponding constants are shown in Table 1. Black triangles: profile of Mol Abs (×
10
-
3, M−1 cm−1) at 300 nm versus pH, obtained upon pH-spectrophotometric titration ofL1 (0.5 mM), in the presence of 2 equiv. Cu(CF3SO3)2 (right vertical axis, see Figure 4).Figure 4
UV-Vis spectra taken upon pH-spectrophotometric titration ofL1(0.5 mM), in the presence of 2 eqv. Cu(CF3SO3)2 (in H2O : MeOH 3 : 2, 0.07 M NaNO3, at 25°C). Long dash line: initial spectrum at pH 2.4; short dash line: spectrum at pH 6.4, corresponding to the maximum of the [Cu2
L1]4+ species; solid line: pH 11, spectrum corresponding to the hydroxide complex [Cu2
L1(OH)]3+.Between pH 2 and pH 4, the azacryptand is in the polyprotonated forms (i.e.,L
1
H
7
7
+, L
1
H
6
6
+, and L
1
H
5
5
+) in which both the secondary amino groups of the azacryptand and the dansyl tertiary amino group are protonated. On increasing pH, the formation of copper-containing species occurs: [CuL1H3]5+(39% at pH = 4.5) and [CuL1H2]4+(68% at pH = 5.1, see Figure 3). The dicopper complex, [Cu2
L1]4+, is the major species in solution at pH 6.4 (78%). In [Cu2
L1]4+, each Cu(II) ion occupies one of thetren units, adopting the typical trigonal bipyramidal geometry imposed by tripodal ligands. The apical positions on the metal ions, left free by the receptor, are occupied by water molecules. Upon further addition of NaOH, the deprotonation of coordinated water occurs, leading to the stable hydroxide complex [Cu2
L1(OH)]3+. Due to its high stability, this species predominates in solution (>90%) over the wide pH range of 8.5–11.Figure4 shows the family of spectra taken over the course of the pH-spectrophotometric titration ofL1 (0.5 mM) in the presence of 2 eqv. Cu(CF3SO3)2. The formation of copper-containing species is accompanied by the development of a band around 300 nm, attributable to a ligand to metal charge transfer (i.e., N(amine) → Cu(II)). The LMCT band develops at pH = 3.5 with the formation of the monometallic complex [CuL1H3]5+and reaches its maximum intensity at pH = 6.8, in the presence of the dicopper species [Cu2
L1]4+. Upon deprotonation of the metal coordinated water molecule, the charge-transfer band undergoes a slight blue shift (see Figure 4 solid black spectrum) due to the different coordinative sphere of the copper(II) cation. The profile obtained at 300 nm well fits the distribution diagram of the Cu(II) species shown in Figure 3.


### 3.3. pH Spectrofluorimetric Studies in Aqueous Mixture

Thanks to the presence of the dansyl fragment close to the receptor’s cavity, the formation of copper-containing species could be followed by emission studies. The fluorescence emission ofL1 is pH dependent; therefore, pH spectrofluorimetric experiments on the asymmetric azacryptand (L1) were performed in an H2O : MeOH 3 : 2 mixture (0.07 M NaNO3, at 25°C) by addition of standard NaOH 0.1 M. Emission spectra were recorded after each addition of standard 0.1 M NaOH; the excitation wavelength was chosen at 314 nm, corresponding to an isosbestic point in the pH-spectrophotometric titration (see Figure 1). The family of the emission spectra taken over the course of the titration ofL1 (0.05 mM) is reported in Figure 5.Figure 5
Family of emission spectra recorded during the pH-spectrophotometric titration ofL1 (0.05 mM,T = 25°C, 0.07 M NaNO3). Long dash line: initial spectrum at pH = 2.5; solid line: spectrum at pH = 10.5.Noticeably, on increasing pH, a fluorescent band centered at 500 nm develops; this behavior is attributable to the formation of a CT band following the deprotonation of the dansyl tertiary amino group [41, 42]. The observed emission band is typical of the dansyl fluorophore, characterized by an intense broad luminescence band.Generally, the emission intensity of fluorescent polyammonium azacryptands decreases with pH; as an example, our group recently reported a fluorescent azacryptand with a 9,10-anthracenyl unit embedded in the receptor’s framework [26]. The anthracenyl emission intensity was maximum at acidic pH (2 < pH < 4 interval) when the secondary amino groups were fully protonated. At pH > 4, the deprotonation of the ammonium groups occurred, leading to the quenching of the anthracenyl fluorophore by a photoinduced electron transfer mechanism, from the free amine groups to the excited anthracene.Very interestingly, in the case ofL1, fluorescent emission increases with the pH, in particular between pH 3 and pH 5, reaching the maximum intensity over pH 7 (see Figure 6). The deprotonation of ammonium groups has no effect on the fluorophore emission because the dansyl group dangles out of the receptor’s cavity, far from the amino groups. The photoinduced electron transfer is therefore disfavored by the distance between the fluorophore and the receptor’s amines.Figure 6
Normalized intensity versus pH at 500 nm obtained upon pH spectrofluorimetric titration ofL1 (0.05 mM) (see Figure 5, λexc = 314 nm).


### 3.4. Studies onL1 andL2with Metal Ions

In order to explore the binding tendencies ofL1 towards metal ions, spectrofluorimetric titrations with Cu(II) and Zn(II) triflate salts have been performed.The family of spectra taken over the course of the titration ofL1 (0.02 M) in MeOH with Cu(CF3SO3)2 and Zn(CF3SO3)2 are shown in Figures 7(a) and 7(b), respectively. The emission spectrum of the free receptorL1 shows the intense CT band at 500 nm (λexc = 350 nm) of the dansyl moiety.Figure 7
Spectrofluorometric titration ofL1 (0.02 mM) with C
u
I
I(CF3SO3)2 3.37 mM (a), Z
n
I
I(CF3SO3)2 3.83 mM (b), andL2 (0.02 mM) with C
u
I
I(CF3SO3)2 2.00 mM (c) in MeOH (λexc = 350 nm). Solid black line: initial spectrum of the free ligandL1; dashed black line: final spectrum. (d) Profiles of the normalized emission intensity (I
/
I
0) at 540 nm versus number of equivalents of added metal ion. Black triangles:L1(0.02 mM) with C
u
I
I(CF3SO3)2, grey triangles:L1(0.02 mM) with Z
n
I
I(CF3SO3)2, and white triangles:L2(0.025 mM) with C
u
I
I(CF3SO3)2 2 mM.
(a)
(b)
(c)
(d)Metal complexation generally affects the dansyl fluorescent band. Figure7(a) shows the changes in the fluorescence ofL1, observed over the course of the titration with copper. Cu(II) addition induced a partial quenching of dansyl emission (by about 60% of the initial intensity); the obtained titration profile I
/
I
0 at 538 nm is shown in Figure 7(d) (black triangles). Quenching follows the formation of a dicopper complex with a 2 : 1 C
u
I
I : L stoichiometry; in fact, the quenching profile reaches aplateau upon the addition of 2 eqv. Cu(II). ReceptorL1can include two C
u
I
I ions, one for each tren subunit. The encapsulated Cu(II) metal centers (d9) easily quench the excited state of the fluorophore through a static quenching mechanism (electron transfer or energy transfer process). In order to prove that receptor’s quenching was due to the formation of a stable dicopper complex, emission experiments were also performed on the model compoundL2(Figure 7(c)).L2 shows the typical band of the dansyl fluorophore. Notably, the addition of Cu(II) to a solution ofL2 had no effect on the emission (even at a Cu(II) concentration 5-fold higher thanL2; white triangles in Figure 7(d)). This result confirms that, in the case ofL1, fluorescence quenching is manly driven by a static mechanism, associated with the coordination of copper ions within the receptor’s cavity.Binding studies onL1were performed also with Zn(II) in the same experimental conditions. Upon addition of zinc, the emission band ofL1undergoes a blue shift and a small decrease in intensity (Figure 7(b)). The titration profile (normalized intensity at 540 nm versus equivalents of Zn(II)) in Figure 7(d) (grey triangles) shows that Zn(II) quenches the emission of the receptor by only 20% of the initial intensity. The maximum variation of the fluorescent emission was obtained upon addition of 2 equivalents of metal ion, revealing the formation of a 2 : 1 Zn(II):L1 complex. Even if zinc has no redox properties, the coordination of Zn(II) induces a weak decrease of the fluorescence emission, indicating the existence of a chelating enhancement of the quenching [30].In order to evaluate the stability of the copper complex in physiological conditions, complexation was also investigated in pure water. In particular, spectrofluorimetric titrations were performed onL1 (0.015 mM) with aqueous Cu(II) at pH = 8 (HEPES), where the [Cu2
L1(OH)]3+ complex is the predominant species (85%) in solution.Figure8(a) displays the family of emission spectra recorded over the course of the titrationL1 (0.015 M), adjusted to pH 8 with HEPES buffer (0.07 M), with a solution of 2.5 mM of Cu(CF3SO3)2. On copper addition, the receptor’s fluorescence is progressively quenched (by about 40% of the initial intensity), proving the interaction ofL1with Cu(II). The best fitting of the experimental data was obtained by assuming the formation of two species in solution with 1 : 1 and 2 : 1 C
u
I
I : L stoichiometry; the corresponding binding constants are reported in Table 2.Table 2
log
⁡
K values for the equilibria in water (HEPES 0.07 M pH = 8, 25°C). In parentheses, standard deviations are shown.
Equilibrium
log
⁡
K values
L1 + Cu2+
⇆
[L1Cu]
2+
K
11
=
5.34 (1)
[L1Cu]
2+ + Cu2+
⇆
[L1Cu2
]
4+
K
12
=
5.25 (1)Figure 8
Spectrofluorimetric titration ofL1 (0.015 mM) with C
u
I
I(CF3SO3)2 2.5 mM (a) in H2O (0.07 M HEPES pH = 8) (λexc = 340 nm). (b) Distribution diagrams of the species present at the equilibrium; white triangles, normalized intensity of the emission at 540 nm, right vertical axis.
(a)
(b)Figure8(b) shows the distribution diagram of the species obtained from the values of K11 and K12 reported in Table 2. The emission intensity profile versus eqv. of Cu(II) (Figure 8(b)) well fits the concentration profile of the free ligand (solid line). Noticeably, the formation of the dicopper complex causes a partial quenching of the dansyl emission band.


## 3.1. Synthesis

Bistren symmetric cryptands are usually synthesized through Schiff base condensation of two molecules of tris(2-aminoethyl)amine (tren) and three molecules of the desired dialdehyde [37, 38] followed by reduction with NaBH4of the imine groups. The new asymmetric azacryptand presented in this work required a multistep synthesis (see Scheme 2 in Section 2) recently described by our group [26, 31, 33]. In particular, 1 mol of mono-BOC-protected tren was first reacted with 1 mol of the 1,4-p-xylyl dialdehyde, obtaining the intermediate polyimine macrocycle1. After reduction with NaBH4 and deprotection of the secondary amine groups, precursor1 was reacted with 2-dansyl-1,4-benzenedicarboxaldehyde (2), in a 1 : 1 ratio. Reduction of the imine groups yieldedL1 without further purification (see Section 2 for details). Thanks to this approach, we obtained a new fluorescent receptor with a fluorescent dansyl group covalently linked on one of the three p-xylyl spacers.


## 3.2. Potentiometric/pH-Spectrophotometric Studies in Aqueous Mixture

In order to study the acid-base behavior of the new receptor, potentiometric titrations have been performed on the asymmetric azacryptand (L1) in H2O : MeOH 3 : 2 mixture (0.07 M NaNO3, at 25°C) by addition of standard acid. The use of a solvent mixture is fundamental to guarantee solubility in the whole pH range (2.5–11). Experimental results were fitted with Hyperquad package [36] and the obtained protonation constants are reported in Table 1.In the pH range considered, only seven protonation constants could be determined, attributable to the protonation of the six secondary amines of the azacryptand and the tertiary amino group of the dansyl moiety. Notably, the protonation of the receptor’s tertiary amino groups was not observed in these conditions. The obtained protonation constant of the NMe2 groups, log
⁡
K
=
1.7, is comparable to that of the system reported by Prodi and coworkers [39].pH-spectrophotometric experiments confirmed these results; Figure1 shows the family of spectra taken over the course of the pH-spectrophotometric titration ofL1(0.5 mM) in MeOH : H2O mixture (0.07 M NaNO3).Figure 1
Family of UV-Vis spectra taken over the pH-spectrophotometric titration ofL1 (0.5 mM,T = 25°C, 0.07 M NaNO3). Long dash line: initial spectrum at pH = 2.5; solid line: spectrum at pH = 11.At acidic pH values, the receptor shows the typical UV/Vis spectrum of the naphthyl group [40] with an intense band at λmax = 288 nm (black dashed line spectrum). Upon deprotonation of the dansyl moiety, the absorption at 288 nm decreases and a new band appears at 340 nm. This new band is attributable to the typical charge transfer of the dansyl group (NMe2→ naphthyl) [27]. The titration profiles obtained at 288 and 340 nm well fit the distribution diagram of the species shown in Figure 2.Figure 2
Distribution diagram of the species (% abundance versus pH) obtained upon potentiometric titration ofL1 in H2O : MeOH 3 : 2 mixture (0.5 mM, 0.07 M NaNO3, at 25°C). The corresponding protonation constants are shown in Table 1. Triangles: profiles of Mol Abs (×10−3, M−1 cm−1) at 288 nm (black) and 340 nm (white), respectively, obtained upon pH-spectrophotometric titration (right vertical axes, see Figure 1).Analogous experiments have been carried out in the presence of 2 equiv. ofC
u
I
I(CF3SO3)2. For cryptandL1, the best data fitting was obtained by assuming the formation of the following copper species on increasing pH: [L1H3Cu]5+, [L1H2Cu]4+, [L1Cu2]4+, and [L1Cu2(OH) ]3+. The formation constants of the copper species are reported in Table 1 and the corresponding distribution diagrams are reported in Figure 3.Figure 3
Distribution diagram of the species (% abundance versus pH) obtained upon potentiometric titration ofL1 (0.5 mM), in the presence of 2 equiv. Cu(CF3SO3)2 (0.07 M NaNO3, H2O : MeOH 3 : 2 at 25°C). The corresponding constants are shown in Table 1. Black triangles: profile of Mol Abs (×
10
-
3, M−1 cm−1) at 300 nm versus pH, obtained upon pH-spectrophotometric titration ofL1 (0.5 mM), in the presence of 2 equiv. Cu(CF3SO3)2 (right vertical axis, see Figure 4).Figure 4
UV-Vis spectra taken upon pH-spectrophotometric titration ofL1(0.5 mM), in the presence of 2 eqv. Cu(CF3SO3)2 (in H2O : MeOH 3 : 2, 0.07 M NaNO3, at 25°C). Long dash line: initial spectrum at pH 2.4; short dash line: spectrum at pH 6.4, corresponding to the maximum of the [Cu2
L1]4+ species; solid line: pH 11, spectrum corresponding to the hydroxide complex [Cu2
L1(OH)]3+.Between pH 2 and pH 4, the azacryptand is in the polyprotonated forms (i.e.,L
1
H
7
7
+, L
1
H
6
6
+, and L
1
H
5
5
+) in which both the secondary amino groups of the azacryptand and the dansyl tertiary amino group are protonated. On increasing pH, the formation of copper-containing species occurs: [CuL1H3]5+(39% at pH = 4.5) and [CuL1H2]4+(68% at pH = 5.1, see Figure 3). The dicopper complex, [Cu2
L1]4+, is the major species in solution at pH 6.4 (78%). In [Cu2
L1]4+, each Cu(II) ion occupies one of thetren units, adopting the typical trigonal bipyramidal geometry imposed by tripodal ligands. The apical positions on the metal ions, left free by the receptor, are occupied by water molecules. Upon further addition of NaOH, the deprotonation of coordinated water occurs, leading to the stable hydroxide complex [Cu2
L1(OH)]3+. Due to its high stability, this species predominates in solution (>90%) over the wide pH range of 8.5–11.Figure4 shows the family of spectra taken over the course of the pH-spectrophotometric titration ofL1 (0.5 mM) in the presence of 2 eqv. Cu(CF3SO3)2. The formation of copper-containing species is accompanied by the development of a band around 300 nm, attributable to a ligand to metal charge transfer (i.e., N(amine) → Cu(II)). The LMCT band develops at pH = 3.5 with the formation of the monometallic complex [CuL1H3]5+and reaches its maximum intensity at pH = 6.8, in the presence of the dicopper species [Cu2
L1]4+. Upon deprotonation of the metal coordinated water molecule, the charge-transfer band undergoes a slight blue shift (see Figure 4 solid black spectrum) due to the different coordinative sphere of the copper(II) cation. The profile obtained at 300 nm well fits the distribution diagram of the Cu(II) species shown in Figure 3.


## 3.3. pH Spectrofluorimetric Studies in Aqueous Mixture

Thanks to the presence of the dansyl fragment close to the receptor’s cavity, the formation of copper-containing species could be followed by emission studies. The fluorescence emission ofL1 is pH dependent; therefore, pH spectrofluorimetric experiments on the asymmetric azacryptand (L1) were performed in an H2O : MeOH 3 : 2 mixture (0.07 M NaNO3, at 25°C) by addition of standard NaOH 0.1 M. Emission spectra were recorded after each addition of standard 0.1 M NaOH; the excitation wavelength was chosen at 314 nm, corresponding to an isosbestic point in the pH-spectrophotometric titration (see Figure 1). The family of the emission spectra taken over the course of the titration ofL1 (0.05 mM) is reported in Figure 5.Figure 5
Family of emission spectra recorded during the pH-spectrophotometric titration ofL1 (0.05 mM,T = 25°C, 0.07 M NaNO3). Long dash line: initial spectrum at pH = 2.5; solid line: spectrum at pH = 10.5.Noticeably, on increasing pH, a fluorescent band centered at 500 nm develops; this behavior is attributable to the formation of a CT band following the deprotonation of the dansyl tertiary amino group [41, 42]. The observed emission band is typical of the dansyl fluorophore, characterized by an intense broad luminescence band.Generally, the emission intensity of fluorescent polyammonium azacryptands decreases with pH; as an example, our group recently reported a fluorescent azacryptand with a 9,10-anthracenyl unit embedded in the receptor’s framework [26]. The anthracenyl emission intensity was maximum at acidic pH (2 < pH < 4 interval) when the secondary amino groups were fully protonated. At pH > 4, the deprotonation of the ammonium groups occurred, leading to the quenching of the anthracenyl fluorophore by a photoinduced electron transfer mechanism, from the free amine groups to the excited anthracene.Very interestingly, in the case ofL1, fluorescent emission increases with the pH, in particular between pH 3 and pH 5, reaching the maximum intensity over pH 7 (see Figure 6). The deprotonation of ammonium groups has no effect on the fluorophore emission because the dansyl group dangles out of the receptor’s cavity, far from the amino groups. The photoinduced electron transfer is therefore disfavored by the distance between the fluorophore and the receptor’s amines.Figure 6
Normalized intensity versus pH at 500 nm obtained upon pH spectrofluorimetric titration ofL1 (0.05 mM) (see Figure 5, λexc = 314 nm).


## 3.4. Studies onL1 andL2with Metal Ions

In order to explore the binding tendencies ofL1 towards metal ions, spectrofluorimetric titrations with Cu(II) and Zn(II) triflate salts have been performed.The family of spectra taken over the course of the titration ofL1 (0.02 M) in MeOH with Cu(CF3SO3)2 and Zn(CF3SO3)2 are shown in Figures 7(a) and 7(b), respectively. The emission spectrum of the free receptorL1 shows the intense CT band at 500 nm (λexc = 350 nm) of the dansyl moiety.Figure 7
Spectrofluorometric titration ofL1 (0.02 mM) with C
u
I
I(CF3SO3)2 3.37 mM (a), Z
n
I
I(CF3SO3)2 3.83 mM (b), andL2 (0.02 mM) with C
u
I
I(CF3SO3)2 2.00 mM (c) in MeOH (λexc = 350 nm). Solid black line: initial spectrum of the free ligandL1; dashed black line: final spectrum. (d) Profiles of the normalized emission intensity (I
/
I
0) at 540 nm versus number of equivalents of added metal ion. Black triangles:L1(0.02 mM) with C
u
I
I(CF3SO3)2, grey triangles:L1(0.02 mM) with Z
n
I
I(CF3SO3)2, and white triangles:L2(0.025 mM) with C
u
I
I(CF3SO3)2 2 mM.
(a)
(b)
(c)
(d)Metal complexation generally affects the dansyl fluorescent band. Figure7(a) shows the changes in the fluorescence ofL1, observed over the course of the titration with copper. Cu(II) addition induced a partial quenching of dansyl emission (by about 60% of the initial intensity); the obtained titration profile I
/
I
0 at 538 nm is shown in Figure 7(d) (black triangles). Quenching follows the formation of a dicopper complex with a 2 : 1 C
u
I
I : L stoichiometry; in fact, the quenching profile reaches aplateau upon the addition of 2 eqv. Cu(II). ReceptorL1can include two C
u
I
I ions, one for each tren subunit. The encapsulated Cu(II) metal centers (d9) easily quench the excited state of the fluorophore through a static quenching mechanism (electron transfer or energy transfer process). In order to prove that receptor’s quenching was due to the formation of a stable dicopper complex, emission experiments were also performed on the model compoundL2(Figure 7(c)).L2 shows the typical band of the dansyl fluorophore. Notably, the addition of Cu(II) to a solution ofL2 had no effect on the emission (even at a Cu(II) concentration 5-fold higher thanL2; white triangles in Figure 7(d)). This result confirms that, in the case ofL1, fluorescence quenching is manly driven by a static mechanism, associated with the coordination of copper ions within the receptor’s cavity.Binding studies onL1were performed also with Zn(II) in the same experimental conditions. Upon addition of zinc, the emission band ofL1undergoes a blue shift and a small decrease in intensity (Figure 7(b)). The titration profile (normalized intensity at 540 nm versus equivalents of Zn(II)) in Figure 7(d) (grey triangles) shows that Zn(II) quenches the emission of the receptor by only 20% of the initial intensity. The maximum variation of the fluorescent emission was obtained upon addition of 2 equivalents of metal ion, revealing the formation of a 2 : 1 Zn(II):L1 complex. Even if zinc has no redox properties, the coordination of Zn(II) induces a weak decrease of the fluorescence emission, indicating the existence of a chelating enhancement of the quenching [30].In order to evaluate the stability of the copper complex in physiological conditions, complexation was also investigated in pure water. In particular, spectrofluorimetric titrations were performed onL1 (0.015 mM) with aqueous Cu(II) at pH = 8 (HEPES), where the [Cu2
L1(OH)]3+ complex is the predominant species (85%) in solution.Figure8(a) displays the family of emission spectra recorded over the course of the titrationL1 (0.015 M), adjusted to pH 8 with HEPES buffer (0.07 M), with a solution of 2.5 mM of Cu(CF3SO3)2. On copper addition, the receptor’s fluorescence is progressively quenched (by about 40% of the initial intensity), proving the interaction ofL1with Cu(II). The best fitting of the experimental data was obtained by assuming the formation of two species in solution with 1 : 1 and 2 : 1 C
u
I
I : L stoichiometry; the corresponding binding constants are reported in Table 2.Table 2
log
⁡
K values for the equilibria in water (HEPES 0.07 M pH = 8, 25°C). In parentheses, standard deviations are shown.
Equilibrium
log
⁡
K values
L1 + Cu2+
⇆
[L1Cu]
2+
K
11
=
5.34 (1)
[L1Cu]
2+ + Cu2+
⇆
[L1Cu2
]
4+
K
12
=
5.25 (1)Figure 8
Spectrofluorimetric titration ofL1 (0.015 mM) with C
u
I
I(CF3SO3)2 2.5 mM (a) in H2O (0.07 M HEPES pH = 8) (λexc = 340 nm). (b) Distribution diagrams of the species present at the equilibrium; white triangles, normalized intensity of the emission at 540 nm, right vertical axis.
(a)
(b)Figure8(b) shows the distribution diagram of the species obtained from the values of K11 and K12 reported in Table 2. The emission intensity profile versus eqv. of Cu(II) (Figure 8(b)) well fits the concentration profile of the free ligand (solid line). Noticeably, the formation of the dicopper complex causes a partial quenching of the dansyl emission band.


## 4. Conclusions

In this work, we report the synthesis of the new asymmetric fluorescent azacryptandL1, characterized by a dansylated fragment anchored to one of the p-xylyl spacers. The sensor was fully characterized by potentiometric, UV-Vis, and emission studies in MeOH : water 3 : 2 mixture (0.07 M NaNO3). Interestingly, the obtained results revealed that the new receptor is fully fluorescent at neutral pH, with the typical dansyl emission band. Notably, fluorescent azacryptands are usually quenched at neutral pH due to the photoinduced electron transfer (PET) from amino groups to the fluorophore. The binding tendencies ofL1towards copper (II) and zinc (II) were studied in MeOH and aqueous solution. Metal addition induced a partial quenching ofL1’s emission; this behavior was more pronounced with Cu(II), which reduces the emission intensity by about 60%. The profiles obtained in these studies with metal ions pointed out the formation of a dimetallic species with a 2 : 1 M
I
I:L stoichiometry. Studies on the model fluorophoreL2confirmed that, in the case ofL1, the quenching is mainly driven by the formation of an inclusion complex. The coordination properties towards Cu2+ have been also tested under physiological conditions. Spectrofluorimetric titrations in water at pH = 8 with Cu2+ allowed for the determination of the formation constants of both mono- and dicopper complexes.



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*Source: 3415690-2016-10-10.xml*