a quantum-mechanical study on the complexation of β-cyclodextrin with quercetin
TRANSCRIPT
A quantum-mechanical study on the complexation
of b-cyclodextrin with quercetin
Chunli Yan a, Xiaohui Li a, Zhilong Xiu a,*, Ce Hao b
a Department of Bioscience and Biotechnology, School of Environmental and Biological Science and Technology,
Dalian University of Technology, Dalian 116024, Liaoning, People’s Republic of Chinab Department of Chemistry, School of Chemical Science and Engineering, Dalian University of Technology,
Dalian 116024, Liaoning, People’s Republic of China
Received 26 September 2005; received in revised form 15 February 2006; accepted 19 February 2006
Available online 5 April 2006
Abstract
The inclusion process involving b-cyclodextrin (b-CD) and quercetin has been investigated by using the PM3 quantum-mechanical semi-
empirical method. In the b-CD quercetin inclusion complex, a large portion of the flavonoid skeleton is included in the b-CD cavity and the bond
connected ring B with ring C is inclined to the molecular axis of b-CD. The orientation in which the B ring of the guest molecule located near the
secondary hydroxyls of the b-CD cavity is preferred in energy. One intermolecular hydrogen bond is formed. The molecular modeling results are
in agreement with the NMR observations and molecular dynamics (MD) simulations. The statistical thermodynamic calculations at 1 atm and
298.15 K by PM3 demonstrate that 1:1 quercetin/b-CD complex is favored by a negative enthalpy change.
q 2006 Elsevier B.V. All rights reserved.
Keywords: Cyclodextrin; Quercetin; PM3; Semi-empirical method; Inclusion complexation
1. Introduction
Naturally occurring cyclodextrins (CDs) are a-1,4-linkedcyclic oligomers of D-glucopyranose which possess the
remarkable property of forming inclusion complexes with a
variety of small molecules appropriate size through the
influences of noncovalent interactions. The resultant inclusion
complexes can induce modification of the physicochemical
properties of the ‘guest’ molecules, particularly in terms of
water solubility and solution stability [1–3]. Therefore, it is
important to clarify the structures of the inclusion complexes
from a viewpoint of enzyme-substrates within the hydrophobic
cavities of CDs [4]. The most common CDs are a-, b- andg-CDs which consist of 6–8 glucopyranose units, respectively.
Nevertheless, b-CD (Fig. 1(a)) is by far the most widely used
compound owing to the optimal size of its internal cavity (8 A),
the most accessibility, and the lowest price for the encapsula-
tion of molecules [5].
Quercetin (3, 3 0, 4 0, 5, 7-penthydroxy flavone, Fig. 1(b)) is
an important constituent of the flavonoid family and is found
0166-1280/$ - see front matter q 2006 Elsevier B.V. All rights reserved.
doi:10.1016/j.theochem.2006.02.008
* Corresponding author. Tel./fax: C86 411 84706369.
E-mail address: [email protected] (Z. Xiu).
in many fruits and vegetables, as well as olive oil, red wine,
and tea [6–8]. It has been demonstrated to possess many
biological effects that are considered beneficial to health,
including antioxidation by scavenging free radicals, antic-
ancer, antiviral prevention of atherosclerosis, and chronic
inflammation activities [9,10]. In spite of this wide spectrum
of pharmacological properties, its use in pharmaceutical field
is limited by its low aqueous solubility [11]. In recent years,
CD complexation has been successfully used to improve
solubility, chemical stability and bioavailability of such
polyphenolic flavonoids [12–15] and other active ingredient
of Chinese herbal medicine, such as alkaloids [16],
terpennoids [17] and so on. The major driving forces for
the complex formation have been proposed to include the
release of entropy-rich water molecules from the cavity, van
der Waals interactions, hydrophobic interactions, hydrogen
bonding and release of ring strain in the CD molecule.
However, the relative contributions and even the nature of
the different forces are not well-known [18]. Due to the
limitations of the experimental methods, molecular modeling
is frequently used to rationalize experimental findings
concerning molecular and chiral recognition by CDs.
Molecular modeling methods of CD complexes are powerful
tools for deriving information on the geometry and the
interaction energy of the inclusion compounds.
Journal of Molecular Structure: THEOCHEM 764 (2006) 95–100
www.elsevier.com/locate/theochem
Fig. 1. Molecular structures of b-cyclodextrin (a), quercetin (b) and PM3-optimized quercetin (c).
C. Yan et al. / Journal of Molecular Structure: THEOCHEM 764 (2006) 95–10096
Intensive theoretical works have been performed over the
past few years on CDs. Owing to their conformational
flexibility and large size, most computations on CD-effective
constituents of Chinese medicine are carried out with
molecular mechanics (MM) [19] or molecular dynamics
(MD) methods [20,21]. These methods are unable to fully
account for the inherent quantum-mechanical effects, as the
molecular mechanics and dynamics methods are based on the
classical physics of balls and springs. Nevertheless, in recent
years, with increased availability of computer resources, the
number of studies reporting the use of quantum mechanics
(QM) for investigating the 3D structure and properties of such
complexes has increased dramatically. QM method can
provide information about the electronic structure of the
system and hence, better understanding of the inclusion
structure. There have been a series of QM studies on the
complexation of CDs with small organic compounds, and these
methods have been successfully applied to these CD systems.
Again, most guests considered were simple, disubstituted
benzenes [18,22]. But very few calculations were performed
for CD complexation with herbal constituents based on QM
methods [16], and the optimum positions of complexation were
determined by only trying several starting points rather than by
a global search.
The inclusion of quercetin with native and modified b-CDshas been studied by other authors and an inclusion complex
with a stoichiometry of 1:1, in solid-state and in aqueous
solution, was attained by different preparation techniques: free-
drying, co-evaporation and kneading method [13,20,23].
Furthermore, a spatial configuration of the b-CD with quercetin
was proposed on the basis of NMR and molecular dynamics
simulations [20]. However, to our best knowledge, quantum
mechanics studies on the inclusion complexation of b-CD with
quercetin, a rather flexible molecule, have been scarcely
reported by far. Furthermore, the studies of noncovalent
interactions involving aromatic substrates are pivotal to both
chemical and biological recognition, as reviewed and evaluated
by Meyer et al. [24].
As applied by Liu and Guo [22], Parametric Model 3 (PM3)
[25] has been chosen to study host–guest complexes between
b-CD and quercetin. Due to the molecular size, PM3 is a
powerful technique which can be currently applied and
performs better than Austin model 1 (AM1) in biochemical
systems due to its improved description of the interactions
between nonbonded atoms, e.g. hydrogen bond and steric
effects [26]. It has high computational efficiency and its
precision is comparable to that of ab initio with medium-sized
basis sets. Conformational flexibility of the quercetin molecule
includes the orientation of the linkage between ring B and C.
Previous NMR studies and MD simulation on the inclusion of
quercetin by b-CD yield ambiguous results for the configur-
ation of quercetin in the complexes and the driving forces
contributing to complexes formation have not been known
clearly yet [20]. The aim of the present work is to re-investigate
their difference in energy, conformations of quercetin in the
complex and the effect of hydroxyl attached to quercetin on the
complexation process with b-CD using the PM3 method.
2. Computational methodology
All theoretical calculations were performed using GAUSSIAN
03 software package [27]. For all the systems, a full geometry
optimization was done at the PM3 level, and a harmonic
frequency analysis was followed to characterize the located
stationary points as true minima (all eigenvalues of the Hessian
matrix are positive).
C. Yan et al. / Journal of Molecular Structure: THEOCHEM 764 (2006) 95–100 97
The initial structures of b-CD and quercetin were
constructed with the help of CS Chem3D Ultra (Version 6.0,
CambridgeSoft.com) from the crystal structure [28,29] and
were fully optimized with PM3. Calculations were carried out
in the gas phase, and solvation effects were not considered.
However, the obtained results are qualitatively useful. As
shown in Fig. 1(c), a conformation for quercetin was obtained
with a minimum energy, where the dihedral angle 6 0-1 0-2-3
(Fig. 1(b)) is equal to 64.58. Experimental evidence suggests
that the B ring of the substrate is preferentially inserted in the
cavity of b-CD [20]. So we constructed substrate/b-CDcomplexes by manually introducing the reactive guest in a
vertical position into the b-CD cavity through the secondary or
primary rim of the latter and perpendicular to the rim diameter.
The coordinate system used to define the process of
complexation is shown in Fig. 2. The method used by Liu
and Guo [22] was referred. The glycosidic oxygens of b-CDwere placed onto the XY plane and their center was defined as
the center of the coordination system. The 1 0-2 bond of
quercetin (Fig. 1(b)) was coincident with the Z-axis, and the
relative position between the host and the guest was measured
by the Z-coordinate of the labeled carbon atom of the guest
(Fig. 2). For the complexation process, the host b-CD was kept
in this position while the guest approached along the Z-axis
toward the wide or narrow edge of the b-CD torus. Fig. 2
depicts the two possible approaches, which will be denoted by
head down and head up approaches, respectively.
The guest was initially located at a Z-coordinate of 8 A and
was moved through the host cavity along the Z-axis to K3 A
at with a stepwise 1 A. For each step, the geometry of
OHO
HO
(a)
(b)
O H
O H OHO
O
Y
X
Z*
OHO
HO
OH
OHOHO
O
Y
X
Z*
Fig. 2. Coordinate systems used to define the process of complexation for: (a)
head up and (b) head down.
the complex was fully optimized by PM3 without imposing any
symmetrical restrictions. In order to find an even more stable
structure of the complex, each guest molecule was calculated
for all of the structures obtained by scanning q, circling around
Z-axis, at 208 intervals from 0 to 3608 and scanning
Z-coordinate at 1 A intervals from K2 to C2 A. Here, q is
the angles circling around the Z-axis of the system and the 1 0-2
bond of quercetin (Fig. 1(b)) is coincident with the Z-axis. The
angle, qZ0, between XZ and the B ring plane of quercetin is
defined as the reference point (Fig. 2). Stabilization energy
(DE) upon complexation between quercetin and the b-CD was
calculated for the minimum energy structure according to
Eq. (1) as a previous work [30]
DEZEcomplxKðEsubst CEbKCDÞ (1)
where Ecomplx, Esubst and Eb-CD represent HF energies (heats
of formation) of the complex, the free substrate and the free
b-CD, respectively. The magnitude of the energy change
would be a sign of the driving force towards complexation. The
more negative the stabilization energy is, the more thermo-
dynamically favorable is the inclusion complex.
3. Results and discussions
The potential energy surfaces of DE versus q and Z for all
the optimized structures obtained by scanning the q angle, from
0 to 3608 at 208 intervals, and the coordinate Z, fromK2 to 2 A
at 1 A intervals, were used to find the most favorable approach
of the quercetin to the b-CD. Two DE minima were found at
qZ40 and 608 for head up and head down, respectively. All
calculations reported thereinafter use the approach of quercetin
into b-CD where the Z coordinate ranged from 8 to K3 A at a
fixed q of 408 (head up) and 608 (head down).
The optimum position and angle for quercetin into b-CD at
head up and head down can be, respectively, determined
according to stability energy as shown in Figs. 3 and 4. Other
possible locations and angle of quercetin were examined using
PM3 method, but were shown to be energetically less favorable
and so they were not listed. As shown in Figs. 3 and 4, the
complexation process is energetically favorable. The stable
structure is reached at approximately ZZK1 A for both head
up at qZ408 and head down at qZ608, respectively.
The most stable structure can be obtained by comparing the
characteristic energies of the complexes between head up and
head down orientation at the optimum position and angle. As
listed in Table 1, the negative DE changes upon complexation
clearly demonstrate that b-CD can form stable complex with
quercetin. The changes in the binding energy are of similar
magnitude to those reported in most MM studies on CD
systems [31], which is reasonable for nonbonded supramole-
cular complexation. The (ELUMOKEHOMO) gap is an important
stability index [32], and chemicals with larger (ELUMOKEHOMO) values tend to have higher stability. Therefore, with
the increase of the (ELUMOKEHOMO) gap, the complexes
formed are more stable, which agrees with the calculated
results of the stability energies. It can also be seen that the head
–4 –2 0 2 4 6 8
Z (Å)
–60
–50
–40
–30
–20
–10
0
10
Stab
ility
Ene
rgy
(kJ/
mol
)
–60
–50
–40
–30
–20
–10
0
10(a)
(b)
–4 –2 0 2 4 6 8
Z (Å)
Stab
ility
Ene
rgy
(kJ/
mol
)
Fig. 3. Stability energies of the inclusion complexation of quercetin into b-CD
at different positions (Z) and orientations: (a) head up; (b) head down. The
position of the guest was determined by the Z-coordinate of the carbon atom in
the phenyl group from the center of the glycosidic oxygens.
–60
–50
–40
–30
–20
–10
0(a)
(b)
0 50 100 150 200
q250 300 350 400
Stab
ility
ene
rgy
(kJ/
mol
)
–60
–50
–40
–30
–20
–10
0
0 50 100 150 200 250 300 350 400
q
Stab
ility
ene
rgy
(kJ/
mol
)
Fig. 4. Stability energies of the inclusion complexation of quercetin into b-CD at
different scanning q (ZZK1 A) and orientations: head up (a) and head down (b).
Table 1
Interaction energies and thermodynamic properties for the inclusion
complexation of b-CD with quercetin
Species Quercetin b-CD Head up Head
down
Ea(kJ molK1) K946.39 K6096.50 K7096.57 7090.59
DEa(kJ molK1) K53.68 K47.70
Hf(kJ molK1) K270.36 K2792.00 K3111.18 K3108.82
DH8b(kJ molK1) K48.82 K46.46
Gf(kJ molK1) K447.12 K3298.87 K3718.60 K3720.54
DG8b(kJ molK1) 27.39 25.45
DS8c(J molK1 KK1) K255.61 K241.19
EHOMOd(ev) K8.98 K10.83 K9.06 K9.04
ELUMOe(ev) K0.89 1.47 K0.79 K1.00
EHOMOKELUMO gap (ev) K8.89 K12.30 K8.27 K8.04
a E is the HF energy, DE is the stabilization energy upon complex, DEZEcomplxK(EsubstCEb-CD).b DA8ZAcomplxK(AsubstCAb-CD); AZH, G.c DS8Z(DH8KDG8)/T.d Energy of the highest occupied molecular orbital.e Energy of the lowest unoccupied molecular orbital.
C. Yan et al. / Journal of Molecular Structure: THEOCHEM 764 (2006) 95–10098
up orientation was significantly more favorable than the head
down orientation by an energy difference of K5.98 kJ molK1.
The driving forces for the stable structures can also be
analyzed by using the PM3 method. Fig. 5 presents the
proposed favorable structures for the 1:1 inclusion complex of
both the head down and head up orientations at each energy
minimum. At the head up orientation, the aromatic B-ring of
quercetin entered fully into cavity of b-CD so that the
7-hydroxy group (OH) of quercetin was close to 6-OH of b-CD. The O/O PM3 calculated distance (of cyclodextrin) was
2.73 A. It is suggested that an intermolecular hydrogen bond
which contributes a stabilization energy of 16–25 kJ molK1
[33] to the complex is formed between quercetin and b-CD.The head down orientation does not seem to be stabilized by
such an interaction. Even though we work in the theoretical
treatment in a vacuum, it is known from the literature that
secondary OH groups form intramolecular hydrogen bonds and
the rate of exchange of protons for head down orientation is
much lower (stronger bonding) than that of head up orientation.
The hydrogen bond here is defined as an O–H/O interaction
in which the O/O distance is less than or equal to 3.2 A and
the angle at H is greater than 908 [34]. Possible hydrogen
bonding is shown in Fig. 5(a and b) as a dotted line. On
the other hand, in the head up structure, the quercetin B-ring
projects onto the 2-OH/3-OH face of b-CD, and the A-ring
projects from the 6-OH face. The four phenolic hydroxyl
groups of the A and B rings of quercetin are left out of the
hydrophobic cavity of b-CD because of their hydrophilic
(a) (b)
(c) (d)
Fig. 5. Structures of the b-CD-quercetin complex with minimum energies obtained by PM3 calculations at different orientations: (a) head up perpendicular to the
cavity axis; (b) head up along the cavity axis from the primary side; (c) head down perpendicular to the cavity axis; (d) head down along the cavity axis from the
secondary side.
C. Yan et al. / Journal of Molecular Structure: THEOCHEM 764 (2006) 95–100 99
characters. There is a good agreement between the experimen-
tal NMR and MD simulations about the overall orientation of
the quercetin ligand in the b-CD cavity: the B-ring, C-ring, and
part of the A-ring of quercetin display favorable interaction
with the hydrophobic cavity of the b-CD [20]. By MD
calculation (MM2 empirical force field), Ding et al. [19] also
confirmed that the phenyl group of rutin (quercetin-3-
rhamnosylglucoside) penetrates into the cavity from the
primary edge of b-CD for the rutin-b-CD complex.
The conformation of quercetin was significantly altered
during complexation (seen in Fig. 5). The dihedral angle (6 0-1 0-
2-3) was changed to 84.8 and 66.48 for the head up and head
down orientation, respectively. It is suggested that, in b-CD-quercetin complexes, the B ring of quercetin can rotate around
the molecular axis of b-CD because of inclusion interaction.
And so the bond connected C1 0 with C2 is inclined to the
molecular axis of b-CD, which results in one hydrogen bond
formation between 7-OH of quercetin and 6-OH of b-CD. Asimilar experiment was conducted by using NMR for
complexation of (C)-catechin into b-CD [35]. The results
revealed that upon inclusion complex formation with (C)-
catechin, the axis of the C1 0–C4 0 of the B ring of (C)-catechin
inclined to the molecular axis of b-CD in the cavity. This
indicates that the guest conformation is easily affected during
CD complexation. Therefore, the assumption in many MM
studies that inclusion complexation did not affect the structure
of the guest molecule should be taken cautiously [31].
To investigate the thermodynamics of the binding process,
the statistical thermodynamic calculation were carried out at
1 atm and 298.15 K in vacuo by PM3. The thermodynamic
quantities, the enthalpy change, the thermal Gibbs free energy
(DG) and entropy contribution (DS) are given in Table 1. FromTable 1, we can be seen that the complexation reactions of
quercetin with b-CD are exothermic judged from the negative
enthalpy changes. And the negative enthalpy changes suggest
that both the inclusion processes are enthalpically favorable in
nature. On the other hand, the enthalpy changes for the head up
orientation is more negative than the head down orientation,
which is surely attributed to the more tightly van der Waals
interactions. The enthalpy changes are of similar magnitude
to the experimental data DHZK26.70 kJ molK1, showing that
the structure and the reaction energy considered are well
described by the PM3 semi-empirical method. However, one
very important aspect of the inclusion process relative to the
entropy contribution should be pointed out. According to the
experimental study [20], the DS for the quercetin-b-CDinclusion process was found to be K32.20 J molK1 KK1. The
PM3 calculated DS was K255.61 J molK1 KK1, which is
C. Yan et al. / Journal of Molecular Structure: THEOCHEM 764 (2006) 95–100100
completely different from the expected value. As a conse-
quence, the standard DG is K17.20 (experimental) and
C27.39 kJ molK1 (PM3 for head up orientation). This
discrepancy can be attributed, in part, to the neglect of the
hydrophobic effect that involves a gain in entropy due to the
assimilation of the solvation water molecules by the medium
after the inclusion takes place [36]. That step of the inclusion
process should be more important in the complexation of
cyclodextrin with the hydrophobic substrate. Therefore, the
Gibbs free energy obtained from static methods (as applied
here) has no absolute meaning and should be considered only
in a relative way.
4. Conclusions
The stable structures and the inclusion process for
quercetin-b-CD inclusion complexes were studied by use of
quantum mechanics PM3 method. One intermolecular hydro-
gen bond is formed, a driving force responsible for its stability.
Its calculations on the complexation of b-CD with quercetin
support the simulations by molecular dynamics (MD) and the
experimental observation by NMR. The orientation in which
the B ring of the guest molecule located near the secondary
hydroxyls of the b-CD is preferred according to the
characteristic energies. The statistical thermodynamic calcu-
lations suggest that both of the complex processes are
enthalpically favorable in nature.
Acknowledgements
We are grateful to the supports from National Natural
Science Foundation of China (20176005) and a project of ‘973’
plans (2003CB716000). We also appreciate Prof. C. Hao from
Dalian University of Technology, who generously offered the
GAUSSIAN 03W software package for the whole computational
tasks.
References
[1] S.K. Dordunoo, M. Burt, Int. J. Pharm. 133 (1996) 191.
[2] S.M.O. Lyng, M. Passos, D. Fontana, Process Biochem. 40 (2005) 865.
[3] S. Tommasini, D. Raneri, R. Ficarra, M.L. Calabro, R. Stancanelli,
P. Ficarra, J. Pharm. Biomed. Anal. 35 (2004) 379.
[4] R. Breslow, D. Dong, Chem. Rev. 98 (1998) 1997.
[5] E.M.M. Del Valle, Process Biochem. 39 (2004) 1033.
[6] M.G.L. Hertog, P.C.H. Hollman, B. Katan, J. Agric. Food Chem. 40
(1992) 2379.
[7] A. Crozier, M.E.J. Lean, M.S. McDonald, C. Black, J. Agric. Food Chem.
45 (1997) 590.
[8] M.S. McDonald, M. Hughes, J. Burns, M.E.J. Lean, D. Matthews,
A. Crozier, J. Agric. Food Chem. 46 (1998) 368.
[9] A.S. Meyer, M. Heinonen, N. Frankel, Food Chem. 61 (1998) 71.
[10] E. Corvazier, J. Maclouf, Biochem. Biophys. Acta 835 (1985) 315.
[11] R. Gugler, M. Leschik, J. Dengler, Eur. J. Clin. Pharmacol. 9 (1975) 229.
[12] M.L. Calabro, S. Tommasini, P. Donato, R. Stancanelli, D. Raneri,
S. Catania, C. Costa, V. Villari, P. Ficarra, R. Ficarra, J. Pharm. Biomed.
Anal. 36 (2005) 1019.
[13] T. Pralhad, K. Rajendrakumar, J. Pharm. Biomed. Anal. 34 (2004) 333.
[14] M.L. Calabro, S. Tommasini, P. Donato, D. Raneri, R. Stancanelli,
P. Ficarra, R. Ficarra, C. Costa, S. Catania, C. Rustichelli, G. Gamberini,
J. Pharm. Biomed. Anal. 36 (2005) 1019.
[15] S. Tommasini, M.L. Calabro, P. Donato, D. Raneri, G. Guglielmo,
P. Ficarra, R. Ficarra, J. Pharm. Biomed. Anal. 35 (2004) 389.
[16] X.H. Wen, Z.Y. Liu, T.Q. Zhu, M.Q. Zhu, K.Z. Jiang, Q. Huang, Bioorg.
Chem. 32 (2004) 223.
[17] J.F. Li, Y.X. Wei, L.H. Ding, C. Dong, Spectrochim. Acta Part A 59
(2003) 2759.
[18] M.J. Huang, J.D. Watts, N. Bodor, Int. J. Quantum Chem. 64 (1997) 711.
[19] H.Y. Ding, J.B. Chao, G.M. Zhang, S.M. Shuang, J.H. Pan, Spectrochim.
Acta Part A 59 (2003) 3421.
[20] Y. Zheng, I.S. Haworth, Z. Zuo, M.S.S. Chow, A.H.L. Chow, J. Pharm.
Sci. 94 (2005) 1079.
[21] Z. Krız, J. Koca, A. Imberty, A. Charlot, R. Auzely-Velty, Org. Biomol.
Chem. 1 (2003) 2590.
[22] L. Liu, X. Guo, J. Incl. Phenom. Macrocycl. Chem. 50 (2004) 95.
[23] M.L. Calabro, S. Tommasini, P. Donato, D. Raneri, R. Stancanelli,
P. Ficarra, R. Ficarra, C. Costa, S. Catania, C. Rustichelli, G. Gamberini,
J. Pharm. Biomed. Anal. 35 (2004) 365.
[24] E.A. Meyer, R.K. Castellano, F. Diederich, Angew. Chem. Int. Ed. 42
(2003) 1210.
[25] J.J.P. Stewart, J. Comput. Chem. 10 (1989) 209.
[26] L. Liu, X. Guo, J. Incl. Phenom. Macrocycl. Chem. 50 (2004) 95.
[27] J. Frisch, G.W. Trucks, H.B. Schlegel, G.E. Scuseria, M.A. Robb, J.R.
Cheeseman, J.A. Montgomery, Jr., T. Vreven, K.N. Kudin, J.C. Burant,
J.M. Millam, S.S. Iyengar, J. Tomasi, V. Barone, B. Mennucci, M. Cossi,
G. Scalmani, N. Rega, G.A. Petersson, H. Nakatsuji, M. Hada, M. Ehara,
K. Toyota, R. Fukuda, J. Hasegawa, M. Ishida, T. Nakajima, Y. Honda, O.
Kitao, H. Nakai, M. Klene, X. Li, J.E. Knox, H.P. Hratchian, J.B. Cross,
C. Adamo, J. Jaramillo, R. Gomperts, R.E. Stratmann, O. Yazyev, A.J.
Austin, R. Cammi, C. Pomelli, J.W. Ochterski, P.Y. Ayala, K. Morokuma,
G.A. Voth, P. Salvador, J.J. Dannenberg, V.G. Zakrzewski, S. Dapprich,
A.D. Daniels, M.C. Strain, O. Farkas, D.K. Malick, A.D. Rabuck, K.
Raghavachari, J.B. Foresman, J.V. Ortiz, Q. Cui, A.G. Baboul, S.
Clifford, J. Cioslowski, B.B. Stefanov, G. Liu, A. Liashenko, P. Piskorz, I.
Komaromi, R.L. Martin, D.J. Fox, T. Keith, M.A. Al-Laham, C.Y. Peng,
A. Nanayakkara, M. Challacombe, P.M.W. Gill, B. Johnson, W. Chen,
M.W. Wong, C. Gonzalez, J.A. Pople, GAUSSIAN 03, Revision B.05,
Gaussian, Inc., Pittsburgh, PA, 2003.
[28] T. Steiner, G. Koellner, J. Am. Chem. Soc. 116 (1994) 5122.
[29] G.Z. Jin, Y. Yamagata, K.I. Tomita, Acta Crystallogr. 46 (C) (1990) 310.
[30] G. Piel, G. Dive, B. Evrard, Eur. J. Pharm. Sci. 13 (2001) 271.
[31] E. Alvira, J.A. Mayoral, J.I. Garcia, Chem. Phys. Lett. 271 (1997) 178.
[32] M. Karelson, V.S. Lobanov, R. Katritzky, Chem. Rev. 96 (1996) 1027.
[33] G.A. Jeffrey, W. Saenger, Hydrogen Bonding in Biological Structures,
Springer, Berlin, 1991.
[34] E.B. Starikov, W. Saenger, T. Steiner, Carbohydr. Res. 307 (1998) 343.
[35] T. Ishizu, K. Kintsu, H. Yamamoto, J. Phys. Chem. B 103 (1999) 8992.
[36] W. Saenger, Angew. Chem. Int. Ed. Engl. 19 (1980) 344.