Reza Omidyan*,
Masoud Omidyan and
Atefeh Mohammadzadeh
Department of Chemistry, University of Isfahan, 81746-73441, Isfahan, Iran. E-mail: r.omidyan@sci.ui.ac.ir; reza.omidyan@u-psud.fr; Fax: +98 311 6689732
First published on 29th March 2016
The second-order approximate coupled-cluster (RI-CC2) method was employed to investigate photoinduced hydrogen-bond weakening or strengthening in neutral and protonated indole–, 5-hydroxyindole–water clusters. In addition to the protonation effect on the electronic structure of 5-hydroxyindole, the intermolecular H-bond weakening or strengthening of selected systems in the S1 excited state has been investigated. According to our calculated results, it has been predicted that the electronic excitation effect on the hydrogen-bond strength in protonated clusters is essentially more pronounced than neutral analogues. Also, a charge transfer character of the excited state over the chromophore moiety can be suggested for interpreting the excited state dynamics of H-bonds in protonated complexes. Moreover, it has been predicted that protonation is accompanied by a strong red-shift effect (∼1.10 eV) on the S1–S0 transition energy of 5-hydroxyindole.
So far, the hydrogen bonding has been studied in the ground state by many different experimental and theoretical methods.2,4,7–10 However, little is known about electronic excited-state characters of hydrogen bonding. Fortunately, based on the new advances in computational methods during last two decades, it is now possible to investigate the physical properties of hydrogen-bond complexes in their excited electronic states accurately.11–15 According to pioneer studies of Zhao et al.,4,6,16–19 it has been established that photoexcitation may induce essential alterations on hydrogen bond characters.20–23 In this regard, Zhao and co-workers have demonstrated that intermolecular hydrogen bonds can be significantly strengthened or weakened in electronically excited states.23–25 In addition, the intermolecular hydrogen bonding interactions in electronically excited state was investigated by Liu et al.26 It has been clarified that intermolecular hydrogen bonds of CO⋯H–O and N–H⋯O–H are significantly strengthened upon photoexcitation to electronically excited states. Additionally, Chudoba et al.20 studied the excited-state infrared (IR) spectra of coumarin 102 dye in hydrogen-donating solvents.20 They proposed that intermolecular hydrogen bond CO⋯H–C forming between C102 and chloroform solvent can be broken following electronic excitation. However, in contrast to the vast numbers of reports dealing with H-bond characters in neutral clusters, rare reports has been dedicated to this subject in ionic states.27,28
Protonated aromatic molecules29 are short lives species which are important in the wide range of science from astrochemistry,30 environment,31 jet engine gas exhaust and hydrocarbon plasmas.32 They are also intermediates in electrophilic aromatic substitution reactions (EAS),29 one of the most commonly reaction mechanisms in organic chemistry. The effects of protonation on aromatic biomolecular systems is an interesting issue for models rationalizing the UV photostability of biological macromolecules, such as proteins and DNA.30,33
In the present study, our results on protonation and excited state hydrogen-bond characters of indole34–42/5-hydroxyindole37,43,44 with one water molecule will be presented. In addition to excited state dynamics of hydrogen bonding in neutral clusters, we have investigated the corresponding parameters of protonated systems. Thus, the geometry and electronic structures, electronic transition energies and oscillator strength of neutral/protonated clusters of indole, 5-hydroxyindole and water, will be accurately addressed. Then, the weakening and strengthening of H-bond following photoexcitation will be explored and discussed.
The abbreviations of “H-bond, In, InH+, 5-HIn, 5-HIn–H+ and W” have been used instead of hydrogen bond, indole, protonated indole, 5-hydroxyindole, protonated 5-hydroxyindole and water, respectively.
Therefore, the N–H and C–H of pyrrole ring, in addition to C–H of benzene and O–H⋯π interaction have been studied. It has been found that H-bond formation between the N–H side of indole and water molecule produces the most stable structure for indole–water complex (Fig. 1(a1)). As shown in Fig. 1, the structure is stabilized by a strong N–H⋯OH hydrogen bond.
Also, when additional water molecule connects to indole, by formation a hydrogen bond between pyrrole's C–H and H2O, the b1 complex is produced. This cluster has been found to be 24 kJ mol−1 less stable than a1 (at the RI-MP2/aug-cc-pVDZ level of theory). Also, adding a water molecule between pyrrole and benzene rings, obtains another complex (c1, see Fig. 1), with 6.8 kJ mol−1 less stability than a1 complex. The CH⋯OH hydrogen bond between water and benzene ring obtains another structure which is less stable than other CH⋯OH and NH⋯OH hydrogen bond clusters. Finally, we have considered a OH⋯π interaction between water and indole chromophore. The optimized structure is depicted in Fig. 1(d1), involving the H(water)⋯π hydrogen bond. That is also more stable than CH⋯OH hydrogen bounded systems; nevertheless, it is 12.5 kJ mol−1 less stable than a1, (the most stable structure). Thus, from inspection of relative stabilities in Fig. 1, the decreasing pattern of H-bond interactions in indole–water clusters can be presented as: NH⋯OH > H(water)⋯π > CH⋯OH.
The protonation effect on electronic structure and spectroscopic properties of indole has been extensively investigated by Alata et al.60 Based on their report, the pyrrole ring provides the most attractive site of protonation. The relevant protonated isomer has been reported to be ∼37 kJ mol−1 more stable than others. Thus, we have selected this isomer60 and investigated its mono-hydration from different sites. As the same as neutral indole, we have considered three type complexes, with N–H, C–H and also OH⋯π interaction. However, no local minimum has been found involving the OH⋯π interaction. As shown in Fig. 1(a2–d2), the NH⋯OH hydrogen bounded is the most stable complex, being ∼37.0 kJ mol−1 more stable than other clusters. Comparing the stability of different clusters of protonated indole–water, it is seen that the NH⋯OH hydrogen bond cluster of protonated indole–water is substantially more stable (∼41.5 kJ mol−1) than all of CH⋯OH clusters. This stabilization is arising from increasing the polarity of N–H bond, due to presence of additional positive charge density on pyrrole ring.
In addition, one may compare the H-bond strength between neutral and protonated indole, by considering the hydrogen bond binding energies (EHb), of the ground state for the most stable isomer of neutral and protonated indole–water complexes (Fig. 1(a1 and a2)).
The ground state EHb has been calculated by comparing the ground state optimized energy of complex and individual monomers:61
EHb(S0) = [EGs]complex − ([EGs]Ch + [EGs]H2O) | (1) |
As shown in Fig. 1, the absolute value of ground state binding energies of protonated indole–water clusters have been determined to be 29 kJ mol−1 larger than those of neutral homologues, indicating to stronger interactions between protonated chromophores and water molecule.
Regarding the transition energies and electronic structures, for the most stable isomers of monohydrated systems (a1 and a2 in Fig. 1), the first and second singlet transition energies have been calculated, using the RI-CC2 method and the cc-pVDZ/aug-cc-pVDZ basis functions.
The results have been tabulated in Table 1. According to the RI-CC2 results, it has been found that the S1–S0 transition in neutral system is corresponding to the HOMO–LUMO single electron transition (80%) and it is arising from HOMO−1–LUMO in protonated system (70%). We have depicted few selected MOs of the most stable isomers of our clustered systems in Fig. 2. As shown, both HOMO and HOMO−1 for neutral and protonated indole–water clusters are of the π character and the LUMO orbital of both systems are of the π* nature. Thus the S1–S0 transition can be assigned as 1ππ* nature in both systems. Additionally, from inspection of Fig. 2, it can be seen that both of the HOMO−1 and LUMO locate over the neutral or protonated chromophores, and no contribution of water molecule is presented on the S1–S0 transition. Thus the S1–S0 transition of neutral/protonated clusters of indole–water can be identified as local transitions.
Electronic state | Vertical transition energy/eV | Adiabatic transition energy/eV | ||||
---|---|---|---|---|---|---|
aug-cc-pVDZ | Oscillator strength | cc-pVDZ | aug-cc-pVDZ | cc-pVDZ | ||
a The experimental S1(0–0) band of indole has been adopted from ref. 62.b The experimental S1(0–0) band of protonated indole has been adopted from ref. 60.c The experimental S1(0–0) band of indole–water cluster has been adopted from ref. 63. | ||||||
Indole (In) | S1(ππ*) | 4.83 | 0.0022 | 4.89 | 4.66 | 4.71 (4.50) |
4.37a | ||||||
S2(ππ*) | 5.29 | 0.0053 | 5.20 | |||
Protonated indole (In–H+) | S1(ππ*) | 3.97 | 0.0419 | 4.08 | 3.43 | 3.68 (3.46) |
3.45b | ||||||
S2(ππ*) | 4.12 | 0.157 | 4.24 | |||
In–W | S1(ππ*) | 4.70 | 0.0328 | 4.86 | 4.37 | 4.67 (4.60) |
4.31c | ||||||
S2(ππ*) | 5.51 | 0.0930 | 5.08 | — | — | |
[In–W]H+ | S1(ππ*) | 4.18 | 0.0351 | 4.28 | 3.56 | 3.68 (3.52) |
S2(ππ*) | 4.31 | 0.1713 | 4.43 | — | — |
Fig. 2 The HOMO, HOMO−1 and LUMO, of neutral and protonated cluster systems, having the most important contributions on the S1–S0 electronic transitions. |
The electronic spectrum of indole and indole–water cluster has been reported by several groups.34,35,37,41,42,44 Recently, Alata et al.,60 reported the electronic spectrum of protonated indole in the jet-cold molecular beam. In order to evaluate our method and basis sets, we have recalculated the S1–S0 adiabatic transition energies of neutral and protonated individual indole, in addition to indole–water cluster. The gas-phase experimental S1(0–0) band of indole, indole–water complex and protonated indole have been reported to be 4.37 eV (35232 cm−1),62,64 4.31 eV (34782 cm−1)63 and 3.45 eV (27826 cm−1)60 respectively. The calculated results are comparable with corresponding experimental results. The best agreement is related to protonated indole, which has been determined to be 3.45 eV at the RI-CC2/aug-cc-pVDZ level and 3.46 eV at the RI-CC2/cc-pVDZ; (corrected by the difference between the zero point vibrational energy of the ground and S1 excited state, ΔZPE = −0.22 eV). Nevertheless, the adiabatic S1–S0 electronic transition energy of indole and indole–water cluster are comparable with experimental values by small errors (ΔE < 0.30 eV). As clarified by Aquino et al.,48,65 this error is mostly related to over-estimation occurred by CC2 method.
EHb(S1) = [EGs + Eex]complex − ([EGs + Eex]Ch + [EGs]H2O) | (2) |
Electronic state | In–H2O | [In–W]H+ | |
---|---|---|---|
a The experimental values for the S0 and S1 vibrational frequencies of N–H bond stretching have been adopted from ref. 12. | |||
l(O⋯H)/Å | S0 | 1.946 | 1.693 |
l(N–H)/Å | 1.019 | 1.047 | |
l(O⋯H)/Å | S1 | 1.511 | 1.951 |
l(N–H)/Å | 1.093 | 1.026 | |
vN–H/cm−1 | S0 | 3545 | 3067 |
3436a | |||
S1 | 3446 | 3425 | |
3387a | |||
EHb (kJ mol−1) | E(S0) | −28.0 | −73.0 |
BSSE | (3.9) | (5.3) | |
E(S0, c) | −24.1 | −67.7 | |
E(S1) | −56.0 | −60.4 | |
BSSE | (9.7) | (6.8) | |
E(S1, c) | −46.3 | −53.6 |
As shown in Table 2, the H-bond binding-energy of neutral and protonated indole–water clusters has been determined to be 24.1 kJ mol−1 and 67.7 kJ mol−1 respectively. The corresponding values of binding energies for the S1 excited-state have been determined to be 46.3 and 53.6 kJ mol−1 respectively, (the BSSE corrections have been considered). Thus, it can be concluded that photoexcitation of neutral and protonated indole–water clusters are accompanied by 22.2 kJ mol−1 increasing and 14.2 kJ mol−1 decreasing in the H-bond binding energies respectively.
According to pioneer works of Nibbering,66 Zhao and Han,67 it has been established that hydrogen-bonding dynamics can be investigated by monitoring the vibrational absorption spectra of H-bonded groups at the ground and excited states. In Fig. 3, we have given the stretching vibrational frequency of N–H bond in different electronic states of neutral and protonated indole–water clusters. As shown the ground state N–H vibrational frequency of neutral and protonated indole–water clusters have been determined to be 3550 and 3067 cm−1 respectively (see blue curves of Fig. 3 and also see Table 2), while the corresponding values of S1 excited states have been determined to 3446 cm−1 and 3425 cm−1 (red spectra in Fig. 3). Thus, the N–H vibrational frequency in neutral indole–water cluster moves to the red by 105 cm−1, and the corresponding frequency of protonated system moves to the blue by 342 cm−1. The red and blue shifts on frequencies of N–H bond-stretching in neutral and protonated clusters following photoexcitation are in accord with increasing and decreasing of N–H bond-length respectively in neutral and protonated systems.
It is noteworthy that experimental vibrational frequencies, corresponding to the ground and S1 excited states of N–H stretching mode of indole–water cluster, have been reported respectively to be 3436 and 3387 cm−1 by Zwier's group.12 As seen, our theoretical values of 3545 and 3446 cm−1 (respectively for the ground and excited states), can be compared with corresponding experimental values of Zwier et al.12 by applying the scaling factors of 0.97 and 0.98 on the respective S0 and S1 simulated spectra.
One may expect several protonated isomers for 5-HIn, corresponding to its different carbon sites. We have determined the optimized structures and consequently the relative stability of these isomers at the RI-MP2/cc-pVDZ level of calculation (see Fig. 4 and its inset for numbering). As shown, protonation of C2 carbon site, leads to the most stable isomer. Also, the C4 carbon atom is the second attractive-position for protonation, producing another protonated isomer with 15.4 kJ mol−1 (0.15 eV) less stability than C2 isomer. With exception of C4 isomer, other protonated isomers of 5-HIn, have been predicted to contain higher internal-energy of 43 kJ mol−1, in respect to C2, the most stable protonated isomer. Moreover, protonation of C3, C8 and oxygen atoms, obtain other high-energy isomers (ΔE > 100 kJ mol−1). Because of the low possibility for populating these isomers in a gas phase study, we ignored to present further details of these isomers. Therefore, in the next sections, we will only consider the most stable structure of protonated 5-HIn (i.e. C2 isomer) for further calculations.
OH(5-HIn)⋯OH(W) > NH(5-HIn)⋯OH(W) > OH(water)⋯π(5-HIn) > CH(5-HIn)⋯OH(W). |
For mono-hydration of protonated 5-HIn, four different isomers, based on the O–H, N–H, C–H and H⋯π interactions have been considered. The results have been presented in Fig. 5(a2–d2). Comparison the total binding energies in neutral and protonated clusters (a1, a2 and b1, b2), the H-bond interaction in protonated species has been found to be substantially stronger than neutral homologues. Also, in contrast to neutral clusters, for protonated 5-HIn–W, the most stable configuration arises from the NH⋯OH H-bond formation. The large charge-density on pyrrole ring strongly affects the NH⋯OH hydrogen bond interaction.
Electronic state | Vertical transition energy/eV | Adiabatic transition energy/eV | ||||
---|---|---|---|---|---|---|
aug-cc-pVDZ | Oscillator strength | cc-pVDZ | aug-cc-PVDZ | cc-pVDZ | ||
a The experimental band origin of 5-HIn has been adopted from ref. 73. | ||||||
5-HIn | S1(ππ*) | 4.33 | 0.0580 | 4.50 | 4.13 | 4.29 (4.11) |
4.05a | ||||||
S2(ππ*) | 4.64 | 0.0002 | 5.18 | — | — | |
5-HIn–H+ | S1(ππ*) | 3.43 | 0.0240 | 3.49 | 3.05 | 3.12 (2.96) |
S2(ππ*) | 4.11 | 0.0053 | 4.28 | — | — | |
5-HIn(OH)–W | S1(ππ*) | 4.28 | 0.0786 | 4.45 | 4.06 | 4.24 (4.04) |
S2(ππ*) | 4.42 | 0.1182 | 5.24 | — | — | |
5-HIn(NH)–W | S1(ππ*) | 4.31 | 0.0570 | 4.46 | 4.10 | 4.26 (4.07) |
S2(ππ*) | 4.49 | 0.0005 | 5.08 | — | — | |
[5-HIn(NH)–W]H+ | S1(ππ*) | 3.63 | 0.2487 | 3.71 | 3.11 | 3.21 (3.01) |
S2(ππ*) | 4.33 | 0.0048 | 4.43 | — | — | |
[5-HIn(OH)–W]H+ | S1(ππ*) | 3.19 | 0.2776 | 3.23 | 2.71 | 2.88 (3.92) |
S2(ππ*) | 4.11 | 0.0056 | 4.19 | — | — |
The former result (4.13 eV) is comparable with experiment while the later is far. However, when the difference between the zero point vibrational energy of the ground and S1 excited state (ΔZPE = −0.19 eV at the RI-CC2/cc-pVDZ level of theory), is taken to account, the corresponding transition energy (4.10 eV) will be in well agreement with experiment.
In addition, the adiabatic S1–S0 transition of protonated 5-HIn has been determined to be 3.05 and 2.96 eV (corrected by ΔZPE = −0.16 eV), at the RI-CC2/aug-cc-pVDZ and cc-pVDZ level respectively. Thus, the S1–S0 transition of protonated 5-HIn is predicted to be strongly red shifted in comparison with its neutral homologue; (by around 1.00 eV).
In order to investigate the H-bond characters, we have considered two isomers for monohydrating of neutral and protonated 5-HIn, based on the connection of water to N–H or O–H groups, obtaining the 5-HIn(NH)–W/[5-HIn(NH)–W]H+ and 5-HIn(OH)–W/[5-HIn(OH)–W]H+ clusters. The results have been presented in Table 3. As shown, mono-hydration dose not significantly affect the S1–S0 transition energies.
Concerning the nature of electronic transitions, the RI-CC2 calculated results, predicted that S1–S0 and S2–S0 for bare 5-HIn, [5-HIn]H+ and their monohydrated systems arise from HOMO–LUMO and HOMO−1–LUMO transitions respectively. The contribution of HOMO and LUMO for the first electronic transition is more than 90% while the second electronic transition is mostly arising from HOMO−1–LUMO single electron transition (75%). In Fig. 2, the selected frontier MOs of the bare and hydrated systems are presented. As shown, both HOMO, HOMO−1 have π character and LUMO is a π* orbital. Thus the S1 and S2 states can be assigned as 1ππ* nature. In addition, in ESI† file further details on electronic transitions and configurations of our studied systems have been presented.
As mentioned before, there is another possibility for adding water molecule to the N–H bond of neutral and protonated 5-HIn, constructing the NH(5-HIn)⋯OH(W) H-bond. The results of NH⋯OH H-bond parameters have been presented in Table 5. As shown, the NH⋯OH bond lengths in the ground state of neutral and protonated 5-HIn(NH)–W have been determined to be 1.953 and 1.699 Å respectively. The substantially shorter H-bond of protonated system indicates to stronger hydrogen bond in protonated cases. Also, the corresponding value of NH⋯OH bond lengths for the S1 excited state have been determined to be 1.918 and 1.931 Å in neutral and protonated systems respectively. Thus, photoexcitation of neutral 5-HIn(NH)–W is accompanied by only 1.7% shortening of NH⋯OH bond length, and 15% lengthening of NH⋯OH bond in protonated system.
In addition, from inspection of hydrogen-bond binding energies of NH⋯OH for ground and excited states of neutral and protonated systems, it is seen that NH⋯OH bond in neutral stays roughly unchanged following photoexcitation; (based on the small alteration of EHb from −24.1 to −24.5 kJ mol−1 respectively from ground to the S1 excited state).
Also, for protonated system, photoexcitation is accompanied by slightly strengthening of NH⋯OH hydrogen bond; (increasing the absolute value of EHb by 7.8 kJ mol−1 after excitation).
The increasing in the absolute value of binding energy after excitation for protonated systems is in accord with NH⋯OH H-bond shortening, and indicating to strengthening of NH⋯OH bond after excitation.
Additionally, we have determined the ground and S1 state IR spectra of 5-HIn–W clusters in neutral and protonated cases. A selected part for IR spectra has been presented in Fig. 6. Considering the vibrational frequencies of normal modes and IR spectra of Fig. 6, it is seen that in neutral and protonated systems, involving OH⋯OH H-bond, the O–H bond stretching of chromophore, shows red-shift in the S1 excited state, by decreasing with 230 and 526 cm−1 respectively in neutral and protonated systems. This decreasing pattern of O–H vibrational frequency is accompanied by increasing of the O–H bond lengths of chromophore and also decreasing of OH⋯OH bond lengths, following photoexcitation of both clustered systems, indicating to H-bond strengthening.
In contrast to OH⋯OH H-bond of neutral and protonated 5-HIn–W clusters, for the NH⋯OH (see Fig. 6c and d), the S1 excitation leads to the significant blue shift of N–H bond stretching (+295 cm−1), in protonated cluster, while that red shifted by 107 cm−1 in neutral homologue. These alterations in IR spectra are in agreement with shortening of N–H and lengthening of NH⋯OH hydrogen bonds in protonated system. Thus, the IR spectra of NH(5-HIn)⋯OH(W) clusters, confirm the H-bond weakening for protonated and slightly strengthening for neutral system following photoexcitation.
(1) According to our RI-MP2 results, it has been predicted that C2 carbon site of pyrrole ring obtains the most stable protonated isomer of 5-hydroxyindole (see Fig. 4).
(2) A large red shift effect (∼1.0 eV) on the S1–S0 transition energy of 5-HIn has been predicted as the most important consequence of protonation.
(3) The most attractive site for monohydration of neutral 5-HIn has been predicted to be the O–H group, while that is the N–H moiety in protonated analogue, which obtains the most stable water cluster.
(4) Concerning the weakening or strengthening of intermolecular H-bonds, it has been found that the S1–S0 excitation effect on the H-bond strength in protonated systems is more pronounced than that of neutral clusters.
(5) Although, there is no explicit interpretation for hydrogen-bond dynamics of neutral systems, a simple explanation based on the CT character of excited state has been proposed for interpretation of weakening or strengthening of H-bonds in protonated clusters. This CT character of excited state, occurring from benzene to the pyrrole ring, increases the positive charge on the phenolic part and decreases that of pyrrole ring following photoexcitation of cluster system from ground to excited state. Thus, the S1–S0 transition in protonated indole–water cluster is along with weakening of NH⋯OH and strengthening of OH⋯OH hydrogen bonds respectively.
Footnote |
† Electronic supplementary information (ESI) available. See DOI: 10.1039/c6ra06716f |
This journal is © The Royal Society of Chemistry 2016 |