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Int. J. Mol. Sci. 2012, 13(9), 10986-10999; doi:10.3390/ijms130910986
Published: 5 September 2012
Abstract: The interactions between chemosensors, 3-amino-5-(4,5,6,7-tetrahydro-1H-indol-2-yl)isoxazole-4-carboxamide (AIC) derivatives, and different anions (F− Cl−, Br−, AcO−, and H2PO4−) have been theoretically investigated using DFT approaches. It turned out that the unique selectivity of AIC derivatives for F− is ascribed to their ability of deprotonating the host sensors. Frontier molecular orbital (FMO) analyses have shown that the vertical electronic transitions of absorption and emission for the sensing signals are characterized as intramolecular charge transfer (ICT). The study of substituent effects suggests that all the substituted derivatives are expected to be promising candidates for fluoride chemosensors both in UV-vis and fluorescence spectra except for derivative with benzo[d]thieno[3,2-b]thiophene fragment that can serve as ratiometric fluorescent fluoride chemosensor only.
The design and synthesis of receptors capable of binding and sensing anions selectively have received significant attention in recent years because anions play an important role in a wide range of biological, environmental, and chemical processes [1–6]. Especially, colorimetric and ratiometric chemosensors appear to be particularly attractive due to their simplicity, high sensitivity, and high selectivity [7,8]. For quantitative analyses, ratiometric chemosensors have the significant advantage of their dual emission system, which can minimize measurement errors caused by fluctuations of light scattering as well as reagent concentration . Colorimetric chemosensors provide an immediate qualitative signal, which allows direct naked-eye detection of anions because of a specific color change of solution upon anion complexation [10,11]. Among the range of biologically important anions, fluoride, the smallest anion, has unique chemical properties. It is of particular interest to recognize and detect it owing to its essential role in a broad range of biological, medical, and chemical processes of osteoporosis, fluorination of drinking water supplies, or even in chemical and nuclear warfare agents [12–14]. However, the chemosensors for F− are rather few, and there is a need for good anion sensors with an improved specific response, in particular, with a selectivity for F− in the presence of other anions. Furthermore, it is necessary to understand the unique host-guest interaction of the sensor with F− and other anions. Different signaling mechanisms have been suggested for F−, such as photoinduced electron transfer (PET) , excited state proton transfer (ESPT) , intramolecular charge transfer (ICT) [17,18], excimer and exciplex formation , and metal-ligand charge transfer (MLCT) , etc.
Recently, a fluoride chemosensor made of a derivative of pyrrole-isoxazole, 3-amino-5-(4,5,6, 7-tetrahydro-1H-indol-2-yl)isoxazole-4-carboxamide (AIC, Scheme I), has been reported . AIC shows both changes in its UV-vis absorption and fluorescence emission spectra upon the addition of F−, resulting in a higher selectivity for fluoride detection compared to other anions in CH3CN. Interactions of AIC with F− cause a red-shift in UV-vis absorption and a Stokes shift in fluorescence emission due to the deprotonation of the active pyrrole-NH moiety of AIC by F−. To the best of our knowledge, neither calculations of the host-guest interactions with the basis set superposition error (BSSE) corrections nor sophisticated level optimizations for the neutral, anion, and complexes forms of AIC derivatives in ground states (S0) and first excited singlet states (S1) have been reported so far.
Herein we report the investigation of both host-guest interaction and signaling properties from a theoretical point of view for this system. Further in-depth explanations for the experimental results have been discussed by the investigation of the optical and electronic properties of pyrrole-isoxazole derivatives. To investigate the substituent effect, several derivatives (1–5), as shown in Scheme I, have been designed by introducing functional groups to pyrrole-isoxazole to provide a demonstration for the rational design of new fluorescent and/or chromogenic chemosensors for fluoride anion.
2. Computational Details
All calculations were performed using Gaussian 09 code . Optimizations were carried out without symmetry constraints. The geometries of AIC and 1–5 and their anions in S0 were optimized by using the hybrid B3LYP functional with 6-31+G(d,p) basis set. Furthermore, complexes consisting of AIC and 1–5 and X− (X = F, Cl, Br, AcO, and H2PO4) were optimized at the same theoretical levels as above with the consideration of the BSSE correction using the counterpoise method . The unphysical long-range asymptote of the exchange part of popular functionals B3LYP makes them unsuitable for calculations of excited states having a large charge-transfer (CT) component [24,25]. Therefore, the S1 structures for AIC and 1–5 and their anions were optimized using the long-range corrected version of B3LYP using the Coulomb-attenuating method CAM-B3LYP functional, which contains 65% long-range HF exchange [25,26]. These range-separated functionals rely on a growing fraction of exact exchange when the interelectronic distance increases, subsequently providing a more physically sound model for long-range phenomena. It has been shown that the CAM-B3LYP functional proved efficient in the determination of the charge-transfer transition [27–31]. The harmonic vibrational frequency calculations using the same methods as for the geometry optimizations were used to ascertain the presence of a local minimum. Absorption and fluorescent properties of AIC and 1–5 and their anions were predicted using the TD-B3LYP/6-31+G(d,p) and TD-BLYP/6-31+G(d,p) methods based on the S0 and S1 optimized geometries, respectively. To investigate the influence of solvents on the optical properties for the S0 and S1 states of the molecular systems in CH3CN (dielectric constant: 35.688) solvent, we performed the polarized continuum model (PCM)  calculations at the TD-DFT level.
To gain an additional insight into the bonding characteristics of the studied complexes consisting of AIC and 1–5 and X− (X = F, Cl, Br, AcO, and H2PO4), we also used the atoms in molecules (AIM) [33,34] theory at the B3LYP/6-31+G(d,p) level. The charge distribution was performed using the natural bond orbital (NBO) approach, which has been proven to be very valuable in the study and characterization of hydrogen bonds and cooperative effects .
3. Results and Discussion
3.1. Host-Guest Interaction
In order to obtain an insight into the anion-sensing mechanism, the interactions between hosts and guests were investigated exploiting the density functional method. Table 1 presents the most important geometrical parameters with and without BSSE corrections for complexes AIC−·HF and AIC·X− (X = Cl, Br, AcO, and H2PO4). The corresponding geometrical parameters of complexes for 1–5 are given in Table SI, Supporting Information. According to the suggested geometry cutoffs for D–H···A hydrogen bond definition, i.e. H···A distances <3.0 Å and D–H···A angles >110° [36,37], the interaction between pyrrole N and H for complex AIC−·HF and between Cl, Br, AcO, and H2PO4 and pyrrole-NH in AIC·X− (X = Cl, Br, AcO, and H2PO4) can be identified as hydrogen bonds. Comparing the optimized geometries with and without BSSE correction, one may find that the deviations of the hydrogen bond length between pyrrole-N and H (RN·H) and the distance between H and F (RH–F) for complex AIC−·HF are 0.005 and 0.001 Å, respectively. The angles θN–H·F in complex AIC−·HF without BSSE correction is equal to that of with BSSE correction. For complexes AIC·X− (X = Cl, Br, AcO, and H2PO4), the deviations of RN–H and RH·X are within 0.004 and 0.15 Å, respectively. The corresponding deviations of angles θN–H·X are within 6°. Therefore, BSSE correction is necessary for the optimization of this kind of system to some extent. Compared with the H–N bond in AIC (1.025 Å), obviously, the H–N bond is broken (0.447 Å elongation) and RH···N = 1.4712 Å and RH–F = 1.030 Å forming AIC−·HF. Namely, the pyrrole-H can be efficiently deprotonated by F−. In the cases of Cl−, Br−, AcO−, and H2PO4−, however, RH–N values only change slightly (<0.044 Å elongation, see Table 1). This suggests that deprotonation indeed takes place from the acidic pyrrole-NH of the host chemosensor to form AIC− and HF in the presence of F−. However, for Cl−, Br−, AcO−, and H2PO4−, the host chemosensor prefers to form the hydrogen-bonded complexes between AIC and X− (X = Cl, Br, AcO, and H2PO4), rather than formation of the AIC− form. Similar phenomena are also found for 1–5 (see Table SI, Supporting Information).
The interaction energies with BSSE corrections for complexes n−·HF and n·X− (n = AIC and 1–5, X = Cl, Br, AcO, and H2PO4) are listed in Table 2. It is clear that the BSSE-corrected interaction energy (ΔEBSSE) of complex AIC−·HF is much more favorable for the distinct selectivity of F− than other anions. The ΔEBSSE of complex AIC−·HF is more than those of AIC·X− (X = Cl, Br, AcO, and H2PO4) by about 20 kcal/mol. Therefore, the sensors can easily detect F− in the presence of Cl−, Br−, AcO−, and H2PO4 −. These calculation results are in good agreement with the reported experimental observations that intermolecular proton transfer (IPT) between chemosensor substrate AIC and F− occurs when the concentration of F− reaches a certain level with the addition of F− to the sensor substrate solution . Similar phenomena are also found for 1–5. Thus, one can conclude that the host chemosensors have a much stronger affinity to F− than to Cl−, Br−, AcO−, and H2PO4− through intermolecular proton transfer, which leads to the formation of chemosensor anions by F−. The hydrogen bond acceptor F− is stronger than those of Cl−, Br−, AcO−, and H2PO4−. On the other hand, the more pronounced the proton transfer reaction, the higher the intensity of the hydrogen bond interaction and the higher the stability of the complex [37,38]. Furthermore, the ΔEBSSE, RH–N, and RH–X (X = F, Cl, Br, AcO, and H2PO4) values of the complexes also support the distinct selectivity for F− from Cl−, Br−, AcO−, and H2PO4−.
As the counterpoise correction was unreliable for the H-bond with fluorine in some cases , we calculated the interaction energies of AIC−·HF and AIC·X− (X = Cl, Br, AcO, and H2PO4) at the MP2/6-31+G(d,p)//B3LYP/6-31+G(d,p) level. It turns out that the interaction energy of AIC−·HF (36.9 kcal/mol) is larger than that of ΔEBSSE by 6.2 kcal/mol. The corresponding values of AIC·X− (X = Cl, Br, AcO, and H2PO4) are larger than those of ΔEBSSE about 8–10 kcal/mol. However, the interaction energy of AIC−·HF is larger than those of complexes AIC·X−(X = Cl, Br, AcO, and H2PO4) by about 10 kcal/mol at the MP2/6-31+G(d,p) level, respectively. It suggests that the interaction energy values of complexes at MP2/6-31+G(d,p) level support the distinct selectivity for F− from Cl−, Br−, AcO−, and H2PO4−. Furthermore, we selected complexes AIC−·HF and AIC·X− (X = Cl and Br) as representatives. The geometrical structures of these complexes were optimized using the MP2 method with 6-31+G(d,p) basis set. The interaction energies were calculated using the same methods as for the geometry optimizations and compared with the BSSE-corrected interaction energy (ΔEBSSE) at the B3LYP/6-31+G(d,p) level. The main geometrical parameters and the interaction energies of complexes AIC−·HF and AIC·X− (X = Cl and Br) at the MP2/6-31+G(d,p) level are given in Table SII, Supporting Information. Comparing the results shown in Table SI with Table 1, one can find that the values of RH···N, RH–F, and angles θN–H·F of AIC−·HF at the MP2/6-31+G(d,p) level are similar to those of AIC−·HF with BSSE corrections at the B3LYP/6-31+G(d,p) level, the corresponding deviations are 0.004, 0.004 Å, and 4.0°, respectively. Similar phenomena are found for complexes AIC·X− (X = Cl and Br). The value of interaction energy for complex AIC−·HF (37.2 kcal/mol) is larger than that of ΔEBSSE by 6.5 kcal/mol. The corresponding interaction energies deviations for complexes AIC·X− (X = Cl and Br) are larger than that of complex AIC−·HF. However, the interaction energy of AIC−·HF is larger than those of complexes AIC·X− (X = Cl and Br) by 19 and 10 kcal/mol at the MP2/6-31+G(d,p) level, respectively. These results indicate that the RH–N, RH–X (X = F, Cl, and Br), and the interaction energy values of the complexes also support the distinct selectivity for F− from Cl− and Br−.
3.2. AIM and NBO Analysis
The AIM theory is often applied to study hydrogen bonds [40–42]. The characteristics of bond critical points (BCPs) are very useful to estimate the strength of hydrogen bonds. To gain a deeper insight into the fundamental nature of NH···X (X = F, Cl, Br, AcO, and H2PO4) hydrogen bonds, it is crucial to obtain reasonable estimates of their relative energies. In particular, the electron densities, ρ(r)bcp, and their Laplacians, ∇2ρ(r)bcp, evaluated at BCPs are frequently used as indicators of hydrogen bonds. More specifically, the kinetic G(r)bcp and potential V(r)bcp electron energy densities are often used to gain additional insight into the strength and nature of a given hydrogen bond. The local kinetic electron energy density can be evaluated from the values of ρ(r)bcp and ∇2ρ(r)bcp as :
The kinetic energy density G(r)bcp is in turn related to the potential energy density V(r)bcp through the local statement of the virial theorem :
The hydrogen bond energy EHB (defined as −De, where De is the hydrogen bond dissociation energy) in molecules can be estimated within the framework of the AIM analysis using the relationship :
The relationship (3) is used to estimate the energy of intermolecular hydrogen bonding. However, the values of the intramolecular hydrogen-bonding energy obtained by means of this equation are somewhat different from the real ones, particularly for intramolecular hydrogen transfer . One of the most reliable approaches to estimating the energy of intramolecular hydrogen bonding is the conformational method. Unfortunately, such a scheme cannot be applied in our calculations because of the lack of conformer. The second one by Musin and Mariam  is disposed to correlate EHB with the interatomic separation (in Å) from donor (D) to acceptor (A) according to the empirical relationship. However, this relationship does not suit the hydrogen bonds in the chemosensors under investigation. Because the pyrrole-NH of the chemosensors are deprotonated by F− and form complexes n−·HF (n = AIC and 1–5), the hydrogen bonds in complexes n−·HF can be regarded as intermolecular hydrogen bonds between chemosensors anions and HF. Therefore, the EHB are estimated by this relationship within the framework of the AIM analysis.
The ρ(r)bcp, ∇2ρ(r)bcp, and EHB of the complexes AIC·HF− and AIC·X− (X = Cl, Br, AcO, and H2PO4) are given in Table 3. The corresponding topological parameters of the complexes n−·HF and n·X− (n = 1–5, X = Cl, Br, AcO, and H2PO4) are given in Table SIII, Supporting Information. As a general rule, hydrogen bonds are characterized by positive values of ∇2ρ(r)bcp and low ρ(r)bcp values. Covalent bonds (shared interactions) have negative ∇2ρ(r)bcp values and high values of ρ(r)bcp, whereas the values of ∇2ρ(r)bcp become positive when the bonds are of a ionic nature . The results displayed in Tables 3 and SIII reveal that the ρ(r)bcp and ∇2ρ(r)bcp values of H···N in n−·HF (n = AIC and 1–5) are about 0.09 and 0.06 au, respectively. This suggests that the interactions between N and H in n−·HF (n = AIC and 1–5) are hydrogen bonds in nature. The ρ(r)bcp and ∇2ρ(r)bcp values of H–F in n−·HF (n = AIC and 1–5) are about 0.25 and −1.1 au, respectively. Hence, H–F bonds of n−·HF (n = AIC and 1–5) are of a covalent bond nature. On the contrary, for complexes n·X− (n = AIC and 1–5, X = Cl, Br, AcO, and H2PO4), BCPs at H–N provides ∇2ρ(r)bcp < 0 (about −1.5 au) and high positive values for ρ(r)bcp (about 0.3 au), which are characteristics of covalent type interactions. For H···X bonds in complexes n·X− (n = 1–5, X = Cl, Br, AcO, and H2PO4), the values of ρ(r)bcp and ∇2ρ(r)bcp are about 0.04 and 0.06 au, respectively. This indicates that H···X bonds in complexes n·X− (n = 1–5, X = Cl, Br, AcO, and H2PO4) are of hydrogen bond nature. Furthermore, the EHB values of H···N and H···X in complexes confirm the expectation. The EHB values of H···N bonds in n−·HF (n = AIC and 1–5) are about 27 kcal/mol, while the H···X bonds in n·X− (n = AIC and 1–5, X = Cl, Br, AcO, and H2PO4) are 4–20 kcal/mol. The above results show qualitative agreement with the results based on their geometries.
It is well known that the electronic reorganization derived from the formation of a hydrogen bond is associated with a charge transfer between the two moieties of the complex . The overall NBO charge transfer has been evaluated by summing up the NBO atomic charges on the two moieties of each hydrogen-bonded complex (the host chemosensor and halides). We select the parent compound AIC as representative of the system under investigation. The calculated NBO charge densities for AIC−·HF and AIC·X− (X = Cl, Br, AcO, and H2PO4) are collected in Table SIV in supplementary information. It clearly shows that the sum of charges on the AIC− moiety is −0.856, while the corresponding value of HF is only −0.144 in complex AIC−·HF. The sum of charges on the AIC moiety and Cl− in AIC·Cl− are −0.098 and −0.902, respectively. The corresponding values in AIC·Br−, AIC·AcO−, and AIC·H2PO4− are −0.072 and −0.928, −0.120 and −0.88, and −0.060 and −0.933, respectively. Hence, the NBO charge analysis also indicates that the proton is almost completely abstracted by F−. In the cases of Cl−, Br−, AcO−, and H2PO4−, however, the host chemosensor prefers to form the hydrogen-bonded complexes between AIC and Cl−, Br−, AcO−, and H2PO4−, rather than the AIC− form.
3.2. Electronic Properties
It is useful to examine the frontier molecular orbitals (FMOs) of the compounds under investigation. The origin of the geometric difference introduced by excitation can be explained, at least in qualitative terms, by analyzing the change in the bonding character of the orbitals involved in the electronic transition for each pair of bonded atoms. An electronic excitation results in some electron density redistribution that affects the molecular geometry [49,50]. The qualitative molecular orbital representations of FMOs for AIC and AIC− in S0 are shown in Figure 1. The corresponding qualitative molecular orbital representations of FMOs for AIC and AIC− in S1 are shown in Figure SI, Supporting Information. The major assignments of the lowest electronic transitions for AIC and AIC− are mainly as HOMO→LUMO, which corresponds to a π–π* excited singlet state. From Figure 1, one can see that both the HOMO and LUMO of AIC and AIC− are spread over the whole conjugated molecule. A careful inspection of the results displayed in Figure 1 reveals that the vertical S0→S1 transition of AIC and AIC− shows the intramolecular charge transfer (ICT) in nature. Analysis of the FMOs for AIC and AIC− indicates that the excitation of the electron from the HOMO to LUMO makes the electronic density flow mainly from the 4,5,6,7-tetrahydro-1H-indole moiety (part A) to 3-aminoisoxazole-4-carboxamide moiety (part B). The HOMO of AIC has contributions of 69.2% and 30.8% on parts A and B, while the corresponding values of LUMO are 35.5% and 64.5%, respectively. The HOMO of AIC− has contributions of 68.9% and 31.1% on parts A and B, while the corresponding values of LUMO are 29.0% and 71.0%, respectively. Hence, the percentage of charge transfer from Parts A to B is 38.9% in AIC−, which is greater than that of 5.2% in AIC. It is obvious that deprotonation strengthens the electron-donating ability of part A, suggesting a stronger coupling between parts A and B. The molecular p-conjugation in AIC− becomes higher than that of AIC. As a consequence, the electron can move more fluently from parts A to B. This suggests that the charge-transfer character of AIC− is stronger than that of AIC. The ICT transition in the chemosensor system becomes much easier after deprotonation, resulting in a red shift between their UV-vis spectra. Similar phenomena are also found for S1 (see Figure SI). However, the intensity of fluorescence may be weak because the AIC− has a worse conjugation due to large twist angles between Parts A and B. The dihedral values of between Parts A and B for AIC and AIC− are 179.0 and 78.7° respectively, suggesting that the molecular p-conjugation in AIC− becomes lower than that of AIC. These results reveal that the deprotonation by F− has obvious effects on the distribution of FMOs, resulting in a red shift between their fluorescence spectra and decreasing the intensity of fluorescence.
3.3. Optical Properties
The original color and emissions change upon addition of F− because of the formation of anions. The addition of F− leads to an intermolecular proton transfer (IPT) between chemosensor AIC and F− which forms the deprotonated anion AIC− and HF. This shifts the equilibrium from AIC towards AIC− (see Scheme I). Hence, the absorption and emission of AIC (340 and 340 nm) are decreased and a new absorption and emission of AIC− has been observed when adding enough amounts of fluoride to the sensor’s solution. In contrast, the addition of Cl−, Br−, AcO−, and H2PO4− leaves its absorption and emission spectra almost unchanged. Therefore, the absorption and emission bands can be assigned to AIC and AIC− before and after the addition of F−, respectively. The driving force for the changing of the color and emission is the intermolecular proton transfer. The bathochromic or hypsochromic shifts between the two characteristic absorptions and emissions of AIC and AIC− are chosen to calculate the colorimetric and ratiometric fluorescent fluoride anion chemosensor.
Table 4 presents the absorption λabs wavelengths, assignments, and the oscillator strength f for AIC and 1–5 and their anions in CH3CN at the TD-B3LYP/6-31+G(d,p) level. The predicted λabs values are in excellent agreement with experimental results . Namely, λabs = 340 and 375 nm before and after the addition of F−. The bathochromic shift between the two characteristic λabs values for AIC and AIC− is 34 nm, which is comparable to the experimental 35 nm. The values of oscillator strength f for AIC and AIC− are 0.67 and 0.55, respectively. This indicates that the intensity absorbance of AIC− is weaker than that of AIC after the addition of F−. However, with increasing F− concentration, the intensity of the absorbance for AIC at 340 nm decreases significantly and the intensity of a new absorption peak for AIC− increases because the formation of AIC− shifts the equilibrium from AIC towards AIC−. Furthermore, the higher molecular p-conjugation in AIC− enhances the intensity of absorption for AIC−. Thus, this result is found thanks to the computational approach, so appropriate electronic transition energies can be predicted at these levels for this kind of chemosensor. The successful simulations indicate that the observed colorimetric and fluorescent signals truly originate from the formation of AIC− anion.
In Table 4, one can see that the λabs of 1 shows a slightly hypsochromic shift, while 2, 3, and 5 have slight bathochromic shifts compared with that of the parent compound AIC, with the maximum deviation being less than 38 nm. However, 4 has a strong bathochromic shift compared with that of the parent compound AIC, the deviation being 348 nm. In general, a larger oscillator strength corresponds to a larger experimental absorption coefficient or stronger fluorescence intensity. The f values of 2 and 5 are larger, while the corresponding f values of 1, 3, and 4 are smaller than that of AIC, particularly for 4. This suggests that 2 and 5 correspond to more intensive spectra. For n− (n = 1–5) of the substituted derivatives, it is found that the λabs of 1− and 2− show slightly hypsochromic shifts, while 3− and 5− have slight bathochromic shifts compared with that of AIC−, the deviations are within 29 nm. However, 4− has a strong bathochromic shift compared with that of the parent compound AIC (the deviation being 82 nm). The f values of 1−–5− are larger than that of AIC− except that the value of f for 4 is less than that for AIC−. This clearly shows that the functional group in 4 has more influence on the shifts of λabs for the substituted derivative and its anion, while the functional groups in 1, 2, 3, and 5 do not significantly affect the λabs of the substituted derivatives and their anions. Furthermore, derivatives 1–5 and their anions show a more intensive spectrum than those of AIC and its anion except for 4.
On the basis of the results displayed in Table 4 and taking into account the ΔEBSSE, one can conclude that the substituted derivatives 1–4 are expected to be fluoride chemosensors. The bathochromic or hypsochromic shifts between the two characteristic λabs values of n and n− (n = 1–4, i.e., λabs values before and after the addition of F−) are 12, 9, 20, and 232 nm, respectively. Therefore, 1–5 show changes in their UV-vis absorption spectra upon the addition of F−, resulting in high selectivity for fluoride detection over other anions, such as Cl−, Br−, AcO−, and H2PO4 in CH3CN. However, 5 does not seem to be a chromogenic chemosensor because the shift between the two characteristic λabs values of 5 and 5− is only 4 nm and the original color of the solution of 5 has no obvious change to the naked eye upon addition of F−.
Table 5 presents the fluorescence λfl wavelengths, assignments, and the oscillator strength f for AIC and 1–5 and their anions in CH3CN at the TD-BLYP/6-31+G(d,p) level. The predicted λfl values are in agreement with experimental results . Namely, λfl = 400 and 432 nm before and after the addition of F−, respectively. The bathochromic shift between the two characteristic λfl values for AIC and AIC− is 56 nm, which is comparable to the experimental 32 nm. From Table 5, one can deduct that the λfl values of 2 and 3 have slight bathochromic shifts, while the corresponding values of 1, 4, and 5 show strong hypsochromic shifts compared with that of AIC. The f values of 2 and 5 are larger while the f values of 1 and 3 are smaller than that of AIC. The f value of 4 is the smallest among the substituted derivatives. For n− (n = 1–5) of the substituted derivatives, the λfl values of 1−and 5− have hypsochromic shifts, while the corresponding values of 2−–4− show more bathochromic shifts compared with that of AIC−. Furthermore, the f values of AIC− and 2−–4− are small (<0.1), indicating that the intensity of fluorescence for AIC− and 2−–4− is weak. The results displayed in Table 5 and the ΔEBSSE values indicate that all the substituted derivatives n (n = 1–5) are expected to be promising candidates for fluorescent fluoride chemosensors. The bathochromic or hypsochromic shifts between the two characteristic λfl values of n and n− (i.e., λfl values before and after the addition of F−) are 62, 308, 111, 65, and 24 nm, respectively. Therefore, the original emissions of 1–5 may be quenched and new weak emissions appear upon the addition of F−.
Our calculated results for both the host-guest interaction and the nature of UV-vis and fluorescent signaling for AIC in the presence of F− are in good agreement with the reported experimental observations. The host chemosensor AIC has a much stronger affinity to F− than to Cl−, Br−, AcO−, and H2PO4− through intermolecular proton transfer, which leads to the formation of chemosensor anions by F−. The AIM theory and NBO charge analysis of the complexes consisting of AIC and X− (X = F, Cl, Br, AcO, and H2PO4) confirm that the protons are almost completely abstracted by F−. FMOs analyses have shown that the vertical electronic transitions of absorption and emission for AIC and AIC− forms corresponding to the sensing signals are characterized as intramolecular charge transfer (ICT). The ICT transition becomes much more efficient when the chemosensor is deprotonated by F−. However, the intensity of fluorescence of AIC− is weak because the AIC− has a worse conjugation due to large twisted angles between 4,5,6,7-tetrahydro-1H-indol moiety and the 3-aminoisoxazole-4-carboxamide moiety. The study of substituent effects suggests that all the substituted derivatives are expected to be promising candidates for fluoride chemosensors both in UV-vis and fluorescence spectra except for the substituted derivative with benzo[d]thieno[3,2-b]thiophene fragment that can serve as ratiometric fluorescent fluoride chemosensor only.
Financial support was received from the Natural Science Foundation of Inner Mongolia Autonomous Region (No. 2011ZD02).
- Bianchi, A.; Bowman-James, K.; Garcia-Espana, E. Supramolecular Chemistry of Anions; Wiley-VCH: New York, NY, USA; p. 1997.
- Deng, Y.; Chen, Y.; Cao, D.; Liu, Z.; Li, G. A cationic triarylborane as water-tolerant fluorescent chemosensor for fluoride anions. Sensors Actuator B-Chem 2010, 149, 165–169. [Google Scholar]
- Li, J.Q.; Li, X.Y. Multichannel photoinduced intramolecular electron-transfer excitations in a bis-naphthalimide spermine conjugate by time-dependent density functional theory. Phys. Chem. A 2007, 111, 13061–13068. [Google Scholar]
- Hagihara, S.; Tanaka, H.; Matile, S. Boronic acid converters for reactive hydrazide amplifiers: Polyphenol sensing in green tea with synthetic pores. J. Am. Chem. Soc 2008, 130, 5656–5657. [Google Scholar]
- Yoon, J.; Kim, S.K.; Singh, N.J.; Kim, K.S. Imidazolium receptors for the recognition of anions. Chem. Soc. Rev 2006, 35, 355–360. [Google Scholar]
- Gale, P.A. Structural and molecular recognition studies with acyclic anion receptors. Acc. Chem. Res 2006, 39, 465–475. [Google Scholar]
- Callan, J.F.; de Silva, A.P.; Magri, D.C. Luminescent sensors and switches in the early 21st century. Tetrahedron 2005, 61, 8551–8588. [Google Scholar]
- Martinez-Manez, R.; Sancanon, F. Fluorogenic and chromogenic chemosensors and reagents for anions. Chem. Rev 2003, 103, 4419–4476. [Google Scholar]
- Valeur, B. Molecular Fluorescence; Wiley-VCH: Weinhein, Germany; p. 2002.
- Coll, C.; Marínez-Máñez, R.; Dolores, M.M.; Sancenón, F.; Soto, J. A simple approach for the selective and sensitive colorimetric detection of anionic surfactants in water. Angew. Chem. Int. Ed 2007, 46, 1675–1678. [Google Scholar]
- Evans, L.S.; Gale, P.A.; Light, M.E.; Quesada, R. Anion binding vs deprotonation in colorimetric pyrrolylamidothiourea based anion sensors. Chem. Commun 2006, 965–967. [Google Scholar]
- Kirk, K.L. Biochemistry of the Halogens and Inorganic Halides; Plenum Press: New York, NY, USA, 1991. [Google Scholar]
- Kleerekoper, M. The role of calcitonin in the prevention of osteoporosis. Endocrin. Metab. Clin. North. Am 1998, 27, 414–418. [Google Scholar]
- Zhang, S.W.; Swager, T.M. Fluorescent detection of chemical warfare agents: Functional group specific ratiometric chemosensors. J. Am. Chem. Soc 2003, 125, 3420–3421. [Google Scholar]
- Kim, S.K.; Yoon, J. A new fluorescent PET chemosensor for fluoride ions. Chem. Commun 2002, 770–771. [Google Scholar]
- Peng, X.; Wu, Y.; Fan, J.; Tian, M.; Han, K. Colorimetric and ratiometric fluorescence sensing of fluoride: Tuning selectivity in proton transfer. J. Org. Chem 2005, 70, 10524–10531. [Google Scholar]
- Li, Z.; Zhang, J. An efficient theoretical study on host–guest interactions of a fluoride chemosensor with F−, Cl−, and Br−. Chem. Phys 2006, 331, 159–163. [Google Scholar]
- Thiagarajan, V.; Ramamurthy, P. Specific optical signalling of anions via intramolecular charge transfer pathway based on acridinedione fluorophore. J. Lumin 2007, 126, 886–892. [Google Scholar]
- Kim, S.K.; Bok, J.H.; Bartsch, R.A.; Lee, J.Y.; Kim, J.S. A fluoride-selective PCT chemosensor based on formation of a static pyrene excimer. Org. Lett 2005, 7, 4839–4842. [Google Scholar]
- Chow, C.F.; Chiu, B.K.W.; Lam, M.H.W.; Wong, W.Y. A trinuclear heterobimetallic Ru(II)/Pt(II) complex as a chemodosimeter selective for sulfhydryl-containing amino acids and peptides. J. Am. Chem. Soc 2003, 125, 7802–7803. [Google Scholar]
- Yang, Z.; Zhang, K.; Gong, F.; Li, S.; Chen, J.; Ma, J.S.; Sobenina, L.N.; Mikhaleva, A.I.; Yang, G.; Trofimov, B.A. A new fluorescent chemosensor for fluoride anion based on a pyrrole–isoxazole derivative. Beilstein. J. Org. Chem 2011, 7, 46–52. [Google Scholar]
- Frisch, M.J.T.; Trucks, G.W.; Schlegel, H.B.; Scuseria, G.E.; Robb, M.A.; Cheeseman, J.R.; Scalmani, G.; Barone, V.; Mennucci, B.; Petersson, G.A.; et al. Gaussian 09; Gaussian Inc: Wallingford, CT, USA; p. 2009.
- Simon, S.; Duran, M.; Dannenberg, J.J. How does basis set superposition error change the potential surfaces for hydrogen-bonded dimers? J. Chem. Phys 1996, 105, 11024–11031. [Google Scholar]
- Handy, N.C. The molecular physics lecture 2004: (i) Density functional theory; (ii) Quantum Monte Carlo. Mol. Phys 2004, 102, 2399–2499. [Google Scholar]
- Tawada, Y.; Tsuneda, T.; Yanagisawa, S.; Yanai, T.; Hirao, K. A long-range-corrected time-dependent density functional theory. J. Chem. Phys 2004, 120, 8425–8433. [Google Scholar]
- Yanai, T.; Tew, D.P.; Handy, N.C. A new hybrid exchange–correlation functional using the coulomb-attenuating method (CAM-B3LYP). Chem. Phys. Lett 2004, 393, 51–57. [Google Scholar]
- Kobayashi, R.; Amos, R.D. The application of CAM-B3LYP to the charge-transfer band problem of the zincbacteriochlorin–bacteriochlorin complex. Chem. Phys. Lett 2006, 420, 106–109. [Google Scholar]
- Kerkines, I.S.K.; Petsalakis, I.D.; Theodorakopoulos, G. Excited-state intramolecular proton transfer in hydroxyoxime-based chemical sensors. J. Phys. Chem. A 2011, 115, 834–840. [Google Scholar]
- Rostov, I.V.; Amos, R.D.; Kobayashi, R.; Scalmani, G.; Frisch, M.J. Studies of the ground and excited-state surfaces of the retinal chromophore using CAM-B3LYP. J. Phys. Chem. B 2010, 114, 5547–5555. [Google Scholar]
- Liu, X.; Zhang, X.; Hou, Y.; Teng, F.; Lou, Z. Theoretical investigation on properties of the ground and lowest excited states of a red emitter with donor-p-acceptor structure. Chem. Phys 2011, 381, 100–104. [Google Scholar]
- Monari, A.; Assfeld, X.; Beley, M.; Gros, P.C. Theoretical study of new ruthenium-based dyes for dye-sensitized solar cells. J. Phys. Chem. A 2011, 115, 3596–3603. [Google Scholar]
- Cornard, J.P.; Lapouge, C. Absorption spectra of caffeic acid, caffeate and their 1:1 complex with Al(III): Density functional theory and time-dependent density functional theory investigations. J. Phys. Chem. A 2006, 110, 7159–7166. [Google Scholar]
- Bader, R.F.W. A bond path: A universal indicator of bonded interactions. J. Phys. Chem. A 1998, 102, 7314–7323. [Google Scholar]
- Biegler-König, F. AIM2000; University of Applied Sciences Bielefeld: Bielefeld, Germany, 2000. [Google Scholar]
- Hobza, P.; Havlas, Z. Blue-shifting hydrogen bonds. Chem. Rev 2000, 100, 4253–4264. [Google Scholar]
- Steiner, T.; Desiraju, G.R. Distinction between the weak hydrogen bond and the van der waals interaction. Chem. Commun 1998, 891–892. [Google Scholar]
- Steiner, T. The hydrogen bond in the solid state. Angew. Chem. Int. Ed 2002, 41, 48–76. [Google Scholar]
- Amendola, V.; Esteban-Gómez, D.; Fabbrizzi, L.; Licchelli, M. What anions do to N–H-containing receptors. Acc. Chem. Res 2006, 39, 343–353. [Google Scholar]
- Schwenke, D.W.; Truhlar, D.G. Systematic study of basis set superposition errors in the calculated interaction energy of two HF molecules. J. Chem. Phys 1985, 82, 2418–2426. [Google Scholar]
- Sidorkin, V.F.; Doronina, E.P.; Chipanina, N.N.; Aksamentova, T.N.; Shainyan, B.A. Bifurcate hydrogen bonds. Interaction of intramolecularly H-bonded systems with Lewis bases. J. Phys. Chem. A 2008, 112, 6227–6234. [Google Scholar]
- Nagaraju, M.; Narahari, S.G. Effect of alkyl substitution on H-bond strength of substituted amide-alcohol complexes. J. Mol. Model 2011, 17, 1801–1816. [Google Scholar]
- Karabıyık, H.; Sevinçek, R.; Petek, H.; Aygün, M. Aromaticity balance, π-electron cooperativity and H-bonding properties in tautomerism of salicylideneaniline: The quantum theory of atoms in molecules (QTAIM) approach. J. Mol. Model 2011, 7, 1295–1309. [Google Scholar]
- Abramov, Y.A. On the possibility of kinetic energy density evaluation from the experimental electron-density distribution. Acta. Crystallogr. A 1997, 53, 264–272. [Google Scholar]
- Bader, R.F.W. Atoms in Molecules: A Quantum Theory; Clarendon Press: Oxford, UK; p. 1994.
- Espinosa, E.; Molins, E.; Lecomte, C. Hydrogen bond strengths revealed by topological analyses of experimentally observed electron densities. Chem. Phys. Lett 1998, 285, 170–173. [Google Scholar]
- Coppens, P.; Abramov, Y.; Carducci, M.; Korjov, B.; Novozhilova, I.; Alhambra, C.; Pressprich, M.R. Experimental charge densities and intermolecular interactions: Electrostatic and topological analysis of dl-histidine. J. Am. Chem. Soc 1999, 121, 2585–2593. [Google Scholar]
- Musin, R.N.; Mariam, Y.H. An integrated approach to the study of intramolecular hydrogen bonds in malonaldehyde enol derivatives and naphthazarin: Trend in energetic versus geometrical consequences. J. Phys. Org. Chem 2006, 19, 425–444. [Google Scholar]
- Nakanishi, W.; Hayashi, S.; Narahara, K. Atoms-in-molecules dual parameter analysis of weak to strong interactions: Behaviors of electronic energy densities versus laplacian of electron densities at bond critical points. J. Phys. Chem. A 2008, 112, 13593–13599. [Google Scholar]
- Forés, M.; Duran, M.; Solà, M.; Adamowicz, L. Excited-state intramolecular proton transfer and rotamerism of 2-(2′-hydroxyvinyl)benzimidazole and 2-(2′-hydroxyphenyl)imidazole. J. Phys. Chem. A 1999, 103, 4413–4420. [Google Scholar]
- Helal, A.; Rashid, M.H.O.; Choi, C.-H.; Kim, H.-S. Chromogenic and fluorogenic sensing of Cu2+ based on coumarin. Tetrahedron 2011, 67, 2794–2802. [Google Scholar]
|Table 1. The distances of RN–H and RH·X (in angstroms) and angles of θO–H·X (in deg) with and without basis set superposition error (BSSE) corrections (in kcal/mol) for complexes AIC−·HF and AIC·X− (X = Cl, Br, AcO, and H2PO4) at the B3LYP/6-31+G(d,p) level.|
|without BSSE||with BSSE|
|Table 2. The interaction energies with BSSE corrections ΔEBSSE (in kcal/mol) of complexes n−·HF, n·Cl−, n·Br−, n·AcO−, and n·H2PO4− (n = AIC and 1–5) at the B3LYP/6-31+G(d,p) level.|
|Table 3. Electronic density at bond critical points (BCP) ρ(r)bcp, the Laplacian ∇2ρ(r)bcp (all in au), and the bond energy EHB (in kcal/mol) of complexes AIC−·HF and AIC·X− (X = Cl, Br, AcO, and H2PO4) at the B3LYP/6-31+G(d,p) level.|
|Table 4. Absorption (λabs) wavelengths (in nm), the oscillator strength f, and assignments (coefficient) for AIC and 1–5 and their anions in CH3CN at the TD-BLYP/6-31+G(d,p) level, along with available experimental data.|
|Compounds||λabs||f||Assignments||Exp *||λabs||f||Assignments||Exp *|
|AIC||341||0.67||H→L (0.70)||340||375||0.55||H→L (0.70)||375|
|1||334||0.45||H-1→L (0.69)||346||0.64||H-1→L (0.69)|
|2||357||0.80||H-1→L (0.69)||366||0.80||H-1→L (0.68)|
|3||368||0.53||H-1→L (0.62)||388||0.80||H-1→L (0.66)|
|4||689||0.07||H→L (0.71)||457||0.21||H-1→L (0.54)|
|5||379||0.93||H-1→L (0.69)||383||0.93||H-1→L (0.69)|
H→L + 1 (0.13)
*Experimental results were taken from .
|Table 5. Fluorescence (λfl) wavelengths (in nm), the oscillator strength f, and assignments (coefficient) for AIC and 1–5 and their anions in CH3CN at the TD-BLYP/6-31+G(d,p) level, along with available experimental data.|
|400||465||0.02||H←L + 1 (0.75)||432|
|3||416||0.37||H←L + 1 (0.28)|
|527||0.07||H←L + 1 (0.69)|
|4||579||0.02||H←L + 1 (0.45)|
|514||0.25||H←L + 1 (0.29)|
|438||0.85||H←L + 1 (0.36)|
*Experimental results were taken from .
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