Computational molecular characterization of the flavonoid rutin
© Glossman-Mitnik et al 2010
Received: 18 March 2010
Accepted: 22 June 2010
Published: 22 June 2010
In this work, we make use of a model chemistry within Density Functional Theory (DFT) recently presented, which is called M05-2X, to calculate the molecular structure of the flavonoid Rutin, as well as to predict the infrared (IR) and ultraviolet (UV-Vis) spectra, the dipole moment and polarizability, the free energy of solvation in different solvents as an indication of solubility, the HOMO and LUMO orbitals, and the chemical reactivity parameters that arise from Conceptual DFT. The calculated values are compared with the available experimental data for this molecule as a means of validation of the used model chemistry.
Flavonoids are phenolic substances characterized for a low molecular weight and they are abundant in plant tissues, apple being one of the most important (particularly its skin) [1, 2]. In the human body they show a lot of biological properties as antioxidants, antiallergenic, antibacterial, antifungal, antiviral and anticarcinogenic agents. These characteristics confer to them pharmacological properties useful for the treatment of diseases that go from allergies, bacterial and viral infectious processes, to those of greater risk like the coronary diseases, cancer and HIV [3–5]. The mechanism by which flavonoids carry out their properties, mainly their antioxidant power, is either by inhibiting the formation or activity of reactive oxygen species, or by direct interaction with DNA, enzymes and membrane receptors.
Theoretical investigations of the physical and chemical properties of flavonoids are very important in order to disclose the relationship between the structure, properties and performance, and to help in the design and synthesis of new derivatives with improved properties. We have experimentally found that some natural flavonoids have a strong ability for complexing metal ions, in particular, those related to heavy metals [6–8]. Thus, natural flavonoids could be useful in water treatment, cleaning and purification. The objective of this letter is to report the results of the calculation of the molecular structure and properties of the flavonoid Rutin using a recently developed density functional . The IR and UV-Vis spectra, the dipole moment and polarizability, the free energy of solvation in different solvents as an indication of solubility, the HOMO and LUMO orbitals, and the chemical reactivity parameters that arise from Conceptual DFT [10, 11] are reported. The calculated values are compared with the available experimental data for this molecule as a means of validation of the used model chemistry. The spectra and the calculated values are important in the sense that they are an indication of the chemical stability, the thermochemistry, the color and the region of the solar spectrum where the absorption takes place, the solubility and the chemical reactivity which is useful to predict the possible complexation sites.
Theory and Computational Details
For all the calculations, we have chosen the hybrid meta-GGA M05-2X functional , which consistently provides satisfactory results for several structural and thermodynamic properties. Although there are a new class of functionals, the so called M06 functionals, our own experience indicates that the improvement in the calculated molecular structure and properties of systems of the size that we are considering in this paper is only marginal. The 3-21G(d) basis set was used for the geometry optimizations and evaluations of harmonic frequencies both in the gas phase and in aqueous solution of the flavonoid. It has been found that this basis set has a remarkable ability to predict the molecular structure and properties of large systems when coupled withe B3LYP density functional , and the same has been our own experience when the M05-2X functional is considered. The equilibrium geometry of the studied molecule was determined by means of the gradient technique. The force constants and vibrational frequencies were determined from calculation using the FREQ keyword on the stationary points obtained after the optimization to check if they were true minima. The electronic properties were calculated with the 6-31+G(d) basis set. A suitable description of this basis set is provided in some of the most important Computational Chemistry recent books [13–16]. Solvation energies were computed by the Integral Equation Formalism - Polarizable Continuum Model (IEF-PCM) , including the UAHF model. All the calculations have been performed with the Gaussian 03W series of programs .
The calculation of the ultraviolet (UV-Vis) spectra of the flavonoid and their metallic complexes has been performed by solving the time dependent Kohn-Sham equations according to the method implemented in Gaussian 03W [13, 19–21]. The equations have been solved for 10 excited states.
The infrared (IR) and ultraviolet (UV-Vis) spectra were calculated and visualized using the Swizard program . In all cases the displayed spectra show the calculated frequencies and absorption wavelengths. The vertical ionization potential I and electron affinity A were calculated in two ways: i) as the difference between the total energy of the neutral molecule and the corresponding ions, taken at the geometry of the neutral molecule in order to keep the external potential constant, and ii) considering the approximation given by the Koopmans' theorem [13–16], where the HOMO energy is equal to -I and the LUMO energy is equal to -A.
Results and Discussion
Experimental, computed and scaled frequencies (cm-1) for the rutin molecule calculated at the M05-2X/3-21G(d) level of theory
Electronic transition states of rutin (nm, eV, oscillator strengths (f), and transition assignments as calculated with TD-DFT and the M05-2X/6-31+G(d,p) level of theory
Assignment; H = HOMO, L = LUMO
S H-4 → L+0(+69%)
S H-0 → L+0(+81%)
S H-1 → L+0(+59%) H-0 → L+1(14%)
H-2 → L+1(6%) H-3 → L+6(+5%)
S H-3 → L+0(+31%) H-2 → L+0(+17%)
H-1 → L+1(15%) H-0 → L+9(14%)
H-0 → L+7(+9%)
S H-2 → L+0(+43%) H-3 → L+0(23%)
H-1 → L+0(+7%)
S H-0 → L+1(+37%) H-1 → L+0(+15%)
H-1 → L+1(+9%) H-2 → L+0(8%)
H-3 → L+0(+8%)
S H-0 → L+1(+26%) H-2 → L+1(17%)
H-5 → L+0(+13%) H-1 → L+1(7%)
H-3 → L+6(+5%)
S H-0 → L+5(+42%) H-0 → L+2(9%)
H-0 → L+6(+6%) H-0 → L+7(+5%)
S H-3 → L+0(+20%) H-0 → L+7(14%)
H-0 → L+9(+13%) H-2 → L+0(+9%)
H-1 → L+1(+8%)
S H-0 → L+6(+32%) H-1 → L+6(+12%)
H-2 → L+0(9%) H-3 → L+1(+7%)
H-2 → L+1(7%) H-0 → L+5(7%)
The molecular dipole moment is perhaps the simplest experimental measure of charge distribution in a molecule. The accuracy of the overall distribution of electrons in a molecule is hard to quantify, since it involves all the multipoles. The polarizability a contributes to the understanding of the response of the system when the external field is changed, while the number of electrons N is kept fixed. The polarizability is calculated as the average of the polarizability tensor . From the present calculations, the total energy, the total dipole moment and the isotropic polarizability of the ground state with the 6-31+G(d,p) model chemistry are -2250.341 au, 7.6877 Debye and 177.57 Bohr3 for the rutin molecule. These results for the dipole moment and the isotropic polarizability could be of interest as an indication of the solubility and chemical reactivity of the studied molecule, not only for it synthesis but for the potential application in complexation of metal cations for water cleaning and purification.
The free energy of solvation ΔG(solv) of the molecule have been calculated for rutin by resorting to the M05-2X/6-31+G(d,p) model chemistry coupled with the Integral-Equation-Formalism of the Polarized Continuum Model (IEF-PCM) for different solvents as implemented in Gaussian 03. The solubility of a molecule will depend on several kinetic and thermodynamic factors. However, it can be said that the magnitude and the sign of ΔG(solv) could be a good approximation as an index of solubility. In this way, a negative sign and a large magnitude will be an indication of increased solubility. The results of these calculations for the studied molecule can be summarized as follows: Acetone = -18.36 Kcal/mol, Acetonitrile = -6.05 Kcal/mol, Aniline = 11.36 Kcal/mol, Benzene = 0.10 Kcal/mol, CCl4 = -0.14 Kcal/mol, Chlorobenzene = -5.42 Kcal/mol, Chloroform = -9.03 Kcal/mol, Cyclohexane = -6.32 kcal/mol, Dichloroethane = -13.37 Kcal/mol, Dichloromethane = -15.59 Kcal/mol, Diethylether= -13.74 Kcal/mol, DMSO = -15.05 Kcal/mol, Ethanol = -52.88 Kcal/mol, Heptane = -7.73 Kcal/mol, Methanol = -56.35 Kcal/mol, Nitromethane = -14.48 Kcal/mol, THF = - 10.58 Kcal/mol, Toluene = -2.36 Kcal/mol, and Water = -49.42 Kcal/mol. These values could be an indication that the studied molecule will be mostly soluble in ethanol, methanol, and water, and this can be related to the results obtained for the dipole moment and polarizability.
where χ is the electronegativity.
where ϵ H and ϵ L are the energies of the highest occupied and the lowest unoccupied molecular orbitals, HOMO and LUMO, respectively.
The validity of the Koopmans' theorem within the DFT approximation is controversial. However, it has been shown  that although the KS orbitals may differ in shape and energy from the HF orbitals, the combination of them produces Conceptual DFT reactivity descriptors that correlate quite well with the reactivity descriptors obtained through Hartree-Fock calculations. Thus, it is worth to calculate the electronegativity, global hardness and global electrophilicity for the rutin molecule using both approximations in order to verify the quality of the procedures.
The results for the vertical I and A of the rutin molecule obtained through energy differences between the ionized and the neutral state, calculated at the geometry of the neutral molecule are I = 7.284 eV and A = 0.067 eV. The HOMO and LUMO energies are -6.836 eV and -0.522 eV, respectively. It can be seen that there is a good qualitative agreement between both results for I, but not for A. The calculated values of the electronegativity, global hardness and global electrophilicity using the I and A are χ = 3.676 eV, = 3.608 eV, and ω = 1.873 eV. Using the HOMO and LUMO energies, within the Koopmans' theorem, the corresponding values are χ = 3.679 eV, η = 3.158 eV, and ω = 2.143 eV. Again, there is a good qualitative agreement for the reactivity parameters calculated through both procedures. It can be concluded that for the particular case of the rutin molecule, the M05-2X/6-31+G(d,p) model chemistry is able to predict the Conceptual DFT reactivity indices calculated through HOMO and LUMO energies as well as from the I and A obtained through energy differences with qualitative similar good accuracy.
The condensed Fukui functions can also be employed to determine the reactivity of each atom in the molecule. The corresponding condensed functions are given by (for nucleophilic attack), (for electrophilic attack), and (for radical attack), where qk is the gross charge of atom k in the molecule.
The results from the calculation of the condensed Fukui functions for nucleophilic, electrophilic and radical attack have been obtained by resorting to the AOMix molecular analysis program . The sites for electrophilic attack will be those atoms bearing a negative charge and where the Fukui function is a maximum. These values confirm that the sites for the electrophilic attack are the C12 and C22 atoms. The site for potential nucleophilic attack would depend on the values of on the atoms with a positive charge density. The results indicate that the site for nucleophilic attack will be the C11 and C13 atoms. Finally, the site for radical attack, governed by the values of will be the C12 atom. The glycoside rings are not very reactive in this context.
In this work, the M05-2X/3-21G(d) and M05-2X/6-31+G(d,p) model chemistries have been applied to the study of a molecule which is potentially useful for water cleaning and purification. The molecular structure for the rutin molecule has been determined by using the M05-2X/3-21G(d) model chemistry. A comparison has been made with the results from the experimental X-ray crystallography for the flavonoid quercetin. The agreement is generally good. Two internal H-bonds have been described that could be an explanation for the increased solubility of rutin in water, ethanol and methanol.
The shape of the frontier orbitals of this molecule were displayed as well as some electronic parameters like the total energy, the dipole moment and the polarizability and the infrared (IR) and ultraviolet (UV-Vis) spectra for the rutin molecule have been predicted according to the M05-2X/6-31+G(d,p) model chemistry, and an assignment of the principal peaks has been achieved.
The free energy of solvation ΔG(solv) of the rutin molecule has been calculated by resorting to the M05-2X/6-31+G(d,p) model chemistry coupled with the Integral-Equation-Formalism of the Polarized Continuum Model (IEF-PCM) for different solvents and the results gave an indication of water, ethanol and methanol as the solvents in which this molecule could be potentially soluble.
The ionization potential I and the electron affinity A have been calculated through energy differences between the ionic and the neutral states, all at the geometry of the neutral molecule, and they have been compared well with the results obtained from the HOMO and LUMO energies obtained through the Koopmans' theorem procedure. The results indicate a qualitative good agreement, which can be consider an indication of the goodness of the proposed model chemistry.
The M05-2X density functional in combination with several basis sets appears to be a useful tool for the study of the molecular structure and electronic properties of flavonoids and the possible nanostructures derived from them, and further applications to several molecular systems of this kind are being pursued in our laboratory.
This work has been partially supported by Consejo Nacional de Ciencia y Tecnología (CONACYT, Mexico) and by Fondo Mixto del Estado de Baja California (FOMIX-BC) through Project 69363. SAPG gratefully acknowledges a fellowship from CONACYT. NFH, APH and DGM are researchers of CONACYT and CIMAV.
- Pietta PG: Flavonoids as antioxidants. J Nat Prod. 2000, 63: 1025-1042. 10.1021/np9904509.View ArticleGoogle Scholar
- Wolfe K, Wu X, Liu RH: Antioxidant activity of apple peels. J Agric Food Chem. 2003, 51: 609-614. 10.1021/jf020782a.View ArticleGoogle Scholar
- Scalbert A, Williamson G: Dietary intake and bioavailability of polyphenols. J Nutr. 2000, 130: 2073S-2085S.Google Scholar
- Erkoc S, Erkoc F, Keskin N: Theoretical investigation of quercetin and its radical isomers. J Mol Struct - THEOCHEM. 2003, 631: 141-146. 10.1016/S0166-1280(03)00237-9.View ArticleGoogle Scholar
- Russo N, Toscano M, Uccella N: Semiempirical molecular modeling into quercetin reactive site: Structural, conformational, and electronic features. J Agric Food Chem. 2000, 48: 3232-3237. 10.1021/jf990469h.View ArticleGoogle Scholar
- Payán-Gómez SA, Flores-Holguín N, Pérez-Hernández A, Pinón-Miramontes M, Glossman-Mitnik D: Computational molecular characterization of the flavonoid morin and its Pt(II), Pd(II) and Zn(II) complexes. J Mol Mod
- Lekka CE, Ren J, Meng S, Kaxiras E: Structural, electronic and optical properties of representative Cu-flavonoid complexes. J Phys Chem B. 2009, 113: 6478-6483. 10.1021/jp807948z.View ArticleGoogle Scholar
- Malesev D, Kuntic V: Investigation of metal-flavonoid chelates and the determination of flavonoids via metal-flavonoid complexing reactions. J Serb Chem Soc. 2007, 72: 921-939. 10.2298/JSC0710921M.View ArticleGoogle Scholar
- Zhao Y, Truhlar DG: Density functionals with broad applicability in chemistry. Acc Chem Res. 2008, 41: 157-167. 10.1021/ar700111a.View ArticleGoogle Scholar
- Parr RG, Yang W: Density Functional Theory of Atoms and Molecules. 1989, New York: Oxford University PressGoogle Scholar
- Geerlings P, DeProft F, Langenaeker W: Conceptual density functional theory. Chem Rev. 2003, 103: 1793-1873. 10.1021/cr990029p.View ArticleGoogle Scholar
- Zandler ME, D'Souza F: The remarkable ability of B3LYP/3-21G(*) calculations to describe geometry, spectral and electrochemical properties of molecular and supramolecular porphyrin-fullerene conjugates. Comptes Rendus Chimie. 2006, 9: 960-981. 10.1016/j.crci.2005.12.008.View ArticleGoogle Scholar
- Lewars E: Computational Chemistry - Introduction to the Theory and Applications of Molecular and Quantum Mechanics. 2003, Norwell, MA: Kluwer Academic PublishersGoogle Scholar
- Young D: Computational Chemistry: A Practical Guide for Applying Techniques to Real-World Problems. 2001, New York: John Wiley & SonsView ArticleGoogle Scholar
- Jensen F: Introduction to Computational Chemistry. 2007, Chichester: John Wiley & SonsGoogle Scholar
- Cramer CJ: Essentials of Computational Chemistry - Theories and Models. 2002, Chichester: John Wiley & SonsGoogle Scholar
- Tomasi J, Mennucci B, Cancès E: The IEF version of the PCM solvation method: An overview of a new method addressed to study molecular solutes at the QM ab initio level. J Mol Struct - THEOCHEM. 1999, 464: 211-226. 10.1016/S0166-1280(98)00553-3.View ArticleGoogle Scholar
- Frisch MJ, Trucks GW, Schlegel HB, Scuseria GE, Robb MA, Cheeseman JR, Montgomery JA, Vreven T, Kudin KN, Burant JC, Millam JM, Iyengar SS, Tomasi J, Barone V, Mennucci B, Cossi M, Scalmani G, Rega N, Petersson GA, Nakatsuji H, Hada M, Ehara M, Toyota K, Fukuda R, Hasegawa J, Ishida M, Nakajima T, Honda Y, Kitao O, Nakai H, Klene M, Li X, Knox JE, Hratchian HP, Cross JB, Bakken V, Adamo C, Jaramillo J, Gomperts R, Stratmann RE, Yazyev O, Austin AJ, Cammi R, Pomelli C, Ochterski JW, Ayala PY, Morokuma K, Voth GA, Salvador P, Dannenberg JJ, Zakrzewski VG, Dapprich S, Daniels AD, Strain MC, Farkas O, Malick DK, Rabuck AD, Raghavachari K, Foresman JB, Ortiz JV, Cui Q, Baboul AG, Clifford S, Cioslowski J, Stefanov BB, Liu G, Liashenko A, Piskorz P, Komaromi I, Martin RL, Fox DJ, Keith T, Al-Laham MA, Peng CY, Nanayakkara A, Challacombe M, Gill PMW, Johnson B, Chen W, Wong MW, Gonzalez C, Pople JA: Gaussian 03, Revision E.01. 2004, Gaussian, Inc., Wallingford, CTGoogle Scholar
- Stratmann RE, Scuseria GE, Frisch MJ: An efficient implementation of time-dependent density-functional theory for the calculation of excitation energies of large molecules. J Chem Phys. 1998, 109: 8218-8224. 10.1063/1.477483.View ArticleGoogle Scholar
- Bauernschmitt R, Ahlrichs R: Treatment of electronic excitations within the adiabatic approximation of time-dependent density functional theory. Chem Phys Lett. 1996, 256: 454-464. 10.1016/0009-2614(96)00440-X.View ArticleGoogle Scholar
- Casida ME, Jamorski C, Casida KC, Salahub DR: Molecular excitation energies to high-lying bound states from time-dependent density-functional response theory: Characterization and correction of the time-dependent local density approximation ionization threshold. J Chem Phys. 1998, 108: 4439-4449. 10.1063/1.475855.View ArticleGoogle Scholar
- Gorelsky SI: Swizard program. [http://www.sg-chem.net/]
- ChemCraft 1.6. [http://www.chemcraftprog.com]
- Gorelsky SI: AOMix program. [http://www.sg-chem.net/]
- Mendoza-Wilson AM, Glossman-Mitnik D: CHIH-DFT deternmination of the molecular structure, infrared and ultraviolet spectra of the flavonoid quercetin. J Mol Struct - THEOCHEM. 2004, 681: 71-76. 10.1016/j.theochem.2004.04.054.View ArticleGoogle Scholar
- Mendoza-Wilson AM, Glossman-Mitnik D: CHIH-DFT study of the electronic properties and chemical reactiviy of quercetin. J Mol Struct - THEOCHEM. 2005, 716: 67-72. 10.1016/j.theochem.2004.10.083.View ArticleGoogle Scholar
- Fossen T, Andersen OM: Spectroscopic techniques applied to flavonoids. Flavonoids - Chemistry, Biochemistry and Applications. Edited by: Andersen OM, Markham KR, Boca Ratón. 2006, FL: Taylor and Francis, LLC, 1: 37-142. 1Google Scholar
- Zevallos J, Toro-Labbé A: A theoretical analysis of the Kohn-Sham and Hartree-Fock orbitals and their use in the determination of electronic properties. J Chil Chem Soc. 2003, 48: 39-47. 10.4067/S0717-97072003000400007.View ArticleGoogle Scholar