An ab initioand AIM investigation into the hydration of 2-thioxanthine
© Yuan et al 2010
Received: 18 December 2009
Accepted: 23 March 2010
Published: 23 March 2010
Hydration is a universal phenomenon in nature. The interactions between biomolecules and water of hydration play a pivotal role in molecular biology. 2-Thioxanthine (2TX), a thio-modified nucleic acid base, is of significant interest as a DNA inhibitor yet its interactions with hydration water have not been investigated either computationally or experimentally. Here in, we reported an ab initio study of the hydration of 2TX, revealing water can form seven hydrated complexes.
Hydrogen-bond (H-bond) interactions in 1:1 complexes of 2TX with water are studied at the MP2/6-311G(d, p) and B3LYP/6-311G(d, p) levels. Seven 2TX...H2O hydrogen bonded complexes have been theoretically identified and reported for the first time. The proton affinities (PAs) of the O, S, and N atoms and deprotonantion enthalpies (DPEs) of different N-H bonds in 2TX are calculated, factors surrounding why the seven complexes have different hydrogen bond energies are discussed. The theoretical infrared and NMR spectra of hydrated 2TX complexes are reported to probe the characteristics of the proposed H-bonds. An improper blue-shifting H-bond with a shortened C-H bond was found in one case. NBO and AIM analysis were carried out to explain the formation of improper blue-shifting H-bonds, and the H-bonding characteristics are discussed.
2TX can interact with water by five different H-bonding regimes, N-H...O, O-H...N, O-H...O, O-H...S and C-H...O, all of which are medium strength hydrogen bonds. The most stable H-bond complex has a closed structure with two hydrogen bonds (N(7)-H...O and O-H...O), whereas the least stable one has an open structure with one H-bond. The interaction energies of the studied complexes are correlated to the PA and DPE involved in H-bond formation. After formation of H-bonds, the calculated IR and NMR spectra of the 2TX-water complexes change greatly, which serves to identify the hydration of 2TX.
Hydration is a universal phenomenon in nature, many biological processes occur in aqueous media. The structure, dynamics and stability of biological macromolecules are influenced by their interactions with hydration water [1–5]. Thus, hydrogen bonds (H-bonds) between biomolecules and water play a vital role in molecular biology. Many efforts have been made to study H-bond interactions between water and nucleic acid bases, both experimentally [6–12] and theoretically [13–31]. Kong et al.  have used resonantly enhanced multiphoton ionization (REMPI) and laser-induced fluorescence (LIF) spectroscopy to study a thymine-water complex. The results indicated that hydration water can stabilize the base. Similar results were obtained for microhydrated uracil . De Vries investigated the hydration of guanine base pairs and found a single water molecule suffices to stabilise the base pair structure . Adamowiz and Maes reported a combined experimental and theoretical study of hydrogen-bond interactions of adenine and hypoxanthine with water [11, 12]. In theoretical approaches [13–19], ab initio and density functional theory (DFT) calculations have been carried out to study H-bonds resulting from 1:1 complexes formed between water and uracil [14–16], cytosine , thymine [18–20], guanine [21–23] and adenine [11, 23]. Kim and Schafer  investigated the microsolvation effects on the stabilities of uracil and its anion. Hobza and co-workers reported serial theoretical works on the tautomers of cytosine , guanine , adenine , uracil and thymine  in the gas phase and a microhydrated environment. Experimental and theoretical investigations on the hydration of nucleic acid bases have been reviewed by Hobza . Schafer and co-workers [29–31] highlighted their theoretical explorations of the molecular mechanisms of DNA damage using quantum mechanical models. They studied electron attachment to DNA subunit anions or base pairs and found the effect of water-hydration in stabilizing the radical anions of the DNA component is crucial .
Sulfur-substituted nucleic acid bases have been found to be clinically useful drugs [35–39], as such, 2-thioxanthine evokes intensive interest [40–48]. An earlier 1H NMR spectroscopic experimental study of 2TX by Twanmoh et al.  revealed that the predominant tautomer of this compound (in DMSO) is a structure in its oxothoine form with the imidazole proton on N(7), which was also corroborated by the subsequent theoretical calculations [42, 43]. Spectrophotometric titration experiment by Kierdaszuk et al. demonstrated the pKa of 2TX is 5.9 . Shugar et al.  reviewed the acid/base properties of 2TX. Tudek and co-workers  studied the inhibition of formamidopyrimidine-DNA glycosylases DNA base analogs and found 2TX to be the most efficient inhibitor of the seventeen tested compounds . Investigations of xanthine oxidase-catalyzed reactions  and deactivation of xanthine permease in the presence of high affinity xanthine analogues  also featured 2TX.
It is noteworthy then that 2TX is of significant interest as a DNA inhibitor [45–48], and that H-bonds between 2TX and water are important. However, to the best of our knowledge, the interactions between the water of hydration and 2TX have not been investigated either computationally or experimentally.
Herein we describe ab initio calculations of the intermolecular interactions in 1:1 complexes of 2-thioxanthine and water, H-bond interactions in the obtained theoretical complexes are investigated and discussed. The infrared and NMR spectra are calculated to facilitate analysis of the H-bonding interactions. Their bonding characteristics are also analysed by Natural Bond Orbital (NBO)  and Atoms In Molecules (AIM) theory .
Second-order Møller-Plesset perturbation theory (MP2) and density functional theory (DFT)  were applied to optimise the structures of the parent monomer and possible hydrated complexes and to predict the harmonic vibrational frequencies. Becke's three-parameter nonlocal exchange function and the Lee, Yang and Parr nonlocal correlation functional (B3LYP) [53, 54] were employed in the DFT calculations. A moderate basis set, 6-311G(d, p), was used for optimization and frequency calculations, followed by single-point calculations with a larger 6-311++G(2df,2p) basis set to obtain more accurate energetics. The interaction energies have been calculated and the basis set superposition error (BSSE) was eliminated by the standard counterpoise (CP) correction method of Boys and Bernardi.
The proton affinities (PAs) and deprotonantion enthalpies (DPEs) relate to acidity and basicity of the sites involved in H-bond formation of hydrated nucleic acid bases . We computed the PA and DPE to discuss why the studied complexes have different interaction energies. The PA and DPE can be defined as the negative enthalpy change of the gas-phase protonation reaction B + H+ → BH+ and enthalpy change of the gas-phase deprotonation reaction AH → A- + H+, respectively, where the A and B represent the acid and base, respectively. The temperature-dependent enthalpy corrections were calculated at 298K and 1 atmosphere pressure.
The NMR chemical shifts for 2TX and its monohydrated complexes were calculated with the "gauge-including atomic orbital" (GIAO) method [56, 57] at the MP2/6-311G(d, p) level. The chemical shift is a measure of difference in shielding (1H) with respect to the standard reference compound e.g. tetramethylsilane, Si(CH3)4.
NBO analysis  was carried out to further understand the interactions. The bonding characteristics of the different hydrogen bonded complexes were analyzed using the AIM theory of Bader . Additionally the theory based on a topological analysis of the electron charge density and its Laplacian has proved invaluable for investigating the properties of H-bonding systems [58, 59]. The MP2-optimized structures were used for the AIM analysis with the MP2 wave functions as input.
Results and Discussion
Structures and Interaction Energies of the 2TX...H2O complexes
Hydrogen bonds are commonly of the format X-H...Y, where the H atom is bound to proton donor X, and proton acceptor Y (which has a lone pair of electrons), X and Y are both electronegative atoms. The four hydrogen atoms of 2TX are composed of three N-H moieties and one C-H, which are potential proton donors for the potential acceptor, oxygen, in water. Additionally there are nitrogen, oxygen and sulfur atoms, which could serve as proton acceptors to water's H-donor potential. Thus, water could approach several different sites of 2TX to form various H-bonded complexes.
Interaction energies including BSSE corrections (ΔE) of the seven 2TX...H2O complexes, BSSE, bond lengths of X--H (RX--H), hydrogen bond distances (rY...H), selected change of X--H bond lengths (ΔrX-H), stretching vibrational frequency of monomer upon complex formation (ΔνX-H), and the corresponding calculated change of infrared intensities (ΔIX-H) at the MP2/6-311G (d, p) level.
R X-H b
r Y ... H b
As shown in Figure 2 and Table 1, the MP2 calculated bond lengths, angles, and interaction energies are very close to the B3LYP estimations. Unless specifically stated, those computed values discussed in the following sections are obtained from the MP2 method.
From Figure 2 it can be seen that only complex VII has an "open structure", whereas the other six hydrated 2TX complexes are "closed" with two nonlinear H-bonds . Five different types of H-bond, denoted N-H...O, O-H...N, O-H...O, O-H...S and C-H...O can be found in these complexes, listed in Table 1. Analysis of the complexes' hydrogen bond distances revealed that the C-H...O distance in complex IV (2.510 Å) is considerably longer than those of the other four types of H-bond, which indicates this H-bond is the weakest one. The N-H...O distances in complexes I, II, III, VI and V are in the region of 1.79-1.92 Å while the O-H...N H-bonds in III and IV are longer, 2.08-2.12 Å. The O-H...O distance in structures I, II, III and IV are in the range of 1.91 to 2.01 Å. The sulfur atom in 2TX can also function as a proton acceptor and interact with water, but the O-H...S distance is relatively long at approximately 2.45 Å.
Compared with the isolated 2TX parent monomer, the core structure of 2TX in the identified complexes is little changed although some of the bonds involved in the formation of H-bonds are modified. All the N-H bonds interacting with H2O are elongated by about 0.0138-0.020 Å, the O-H bond of water in the complexes is also longer than that of in an isolated H2O molecule. These elongations of the proton donor X-H bond display the characteristic classical red-shifting H-bonds, it is noteworthy that the C-H bond in complex IV is shortened by about 0.001 Å, which indicates that the C-H...O may be an improper blue-shifting H-bond.
As shown in Table 1, the interaction energies (ΔE) with BSSE corrections are all negative, which indicates that the hydrogen bonds do indeed stabilise the complexes. The MP2 method shows ΔE to be very close to that obtained from B3LYP, but the B3LYP BSSE is a little smaller than that obtained by MP2. At the MP2 level of theory, the calculated ΔE of the seven H-bond complexes is about 3-13 kcal mol-1. Generally, based on the interaction energy, the H-bonds can be classified into strong (15-45 kcal mol-1), medium (4-15 kcal mol-1), and weak (1-4 kcal mol-1) . The present results show that medium H-bonds are formed in the most hydrated 2TX complexes. Complex VII, however, has a weak H-bond with a ΔE of -3.3 kcal mol-1, and is the least stable structure of the seven 2TX...H2O complexes. It is well known that long range dispersion interactions play a dominant role in weak intermolecular interactions . Whilst MP2 theory considers dispersion energy the B3LYP method does not account for such long-range correlations . The weak H-bond of the complex VII, the B3LYP ΔE is -2.6 kcal mol-1, which is very close to the MP2 result (-3.3 kcal mol-1). This result indicates that dispersion forces make little contribution to the interaction between water and 2TX, as such our results indicate that the B3LYP method is also able to provide reliable results. This may be useful when larger systems prohibitive to the MP2 estimation are studied. As such B3LYP calculations could be used for the study of H-bonds in such a system.
Among the seven hydrated complexes, the structure II is the most stable. At the MP2/aug-cc-pVDZ//MP2/6-311G(d, p) and B3LYP/6-311++G(d, p)//B3LYP/6-311G(d, p) level, its interaction energies are -12.1 and -12.7 kcal mol-1, respectively. The values are larger than those of other hydrated nuclear bases such as uracil (-9.6 kcal mol-1 at the MP2/aug-cc-pVDZ level) , cytosine (-8.6 kcal mol-1 at the B3LYP/6-311++G(d, p) level)  and thymine (-7.9 kcal mol-1 at the B3LYP/6-311++G(d, p) level). The results indicate that the H-bond in the hydrated 2TX complex is a little stronger than those in the other hydrated nuclear base complexes.
Structure II has the shortest N-H...O distance of 1.796 Å. The N-H...O hydrogen distance of the complex VI is 1.800 Å, but the O-H...S hydrogen bond in this system is weaker than the O-H...O hydrogen bond of complex II. Thus, the ΔE of the former is 4.5 kcal mol-1 smaller than that of the latter. Complex IV has two H-bonds but it is the second least stable structure among the hydrated complexes studied. Its ΔE is just 1.5 kcal mol-1 larger than that of complex VII (the least stable). The hydrogen bond angle ∠C-H...O is 109.5° for complex IV, which is much smaller than those of other complexes. The bent structure of IV results in a weak H-bond with a small interaction energy.
MP2/6-311++G(2d,2p)//MP2/6-311G(d, p) proton affinity (PA) of O, S, and N atoms, deprotonation enthalpy (DPE) of N--H and C--H bonds in the 2TX, and 1.5DPE--PA of seven 2TX...H2O complexes. All the values are in kcal mol-1.
atoms and bonds
O(11) (N(1) side)
O(11) (N(7) side)
S(10) (N(1) side)
S(10) (N(3) side)
Zeegers-Huyskens and co-workers have reported theoretical studies on acidity and basicity of guanine, adenine, urail, thymine, and cytosine[14, 16–19, 23]. Their results suggest that hydrogen bond energies of these hydrated nucleobases are correlated to the PA and DPE of the sites involved in interaction with water. They obtained a good quantitative relationship between the ΔE and the values of 1.5DPE-PA [16, 17, 23], the smaller 1.5DPE-PA, the larger ΔE.
Complexes I and II have close PAs but the latter's DPE is l6.1 kcal mol-1 lower than that of the former. The much stronger acidity of N(7)-H compensates the lower basicity of O11 (N(7) site) in structure II. As a result, complex II has lower values of 1.5DPE-PA than I. In addition, the hydrogen bond angle ∠O-H...O in complexes is small compared to ordinary O-H...O H-bond angles, about 141.8°. The weaker acidity of N(1)-H and small hydrogen bond angle in complex I result in it being 5.1 kcal mol-1 less stable than complexes II. Compared with structure I, complexes III and VI have lower DPEs of N(3)-H and higher PAs of the S atom. The stronger acidity and basicity of the sites involved the H-bond formation result in the two complexes are more stable than the complex I. The acidity of C(8)-H bond is the weakest, thus complex VII has the highest 1.5DPE-PA and is the least stable among the seven complexes. The relative stability order of the studied complexes can be explained by the acidity and basicity of the sites satisfactorily forming H-bonds, which agrees with previous conclusion on the cyclic hydrated nucleobases by Zeegers-Huyskens and coworkers [14, 16–19, 23].
In summary, the present studies on the hydration of 2TX show that the water can interact with the nucleobase in different sites to form various H-bonds. The intrinsic acidity and basicity of the sites forming H-bonds leads to the different interaction energies. When H2O approaches the N(7)-H site, a closed complex II with two H-bonds is the most stable. In the C-H site, complex VII with only one H-bond is the least stable one.
Infrared and NMR spectroscopy
Comparing the IR spectra of the parent 2TX and hydrated 2TX, it can be seen that the latter is quite different, especially in the area from 3000 to 4000 cm-1. As show in the Figure 3, three weak peaks corresponding to N-H vibrational stretches and one very weak C-H stretch are observed, 3616 (N(1)-H), 3651 (N(3)-H), 3671 (N(7)-H), and 3296 cm-1 (C-H). After forming H-bonds, a much stronger red-shifting band will appear in the area between 3000 and 4000 cm-1 for the hydrated 2TX complexes. In Table 1, the changes of X-H bond lengths (ΔrX-H) and corresponding stretching vibrational frequencies upon complex formation (ΔνX-H) are listed. The results indicate that most complexes have an elongated X-H bond with a red-shift stretching frequency of 78-366 cm-1. The relative infrared intensities also increase (100-600 km/mol). That these shifts can be observed in the theoretical IR spectra of the complexes, confirms the existence of the formation of H-bonds.
For complexes I, II, III, V, and VI, the N-H and O-H stretching frequency changes with a large red-shift upon H-bond formation, whereas in IV and VII the O-H and C-H stretching frequencies are a little altered. These results indicate that the N-H...O, O-H...O and O-H...S interactions are classical red-shifting H-bonds. However, the calculated IR spectrum of complex IV is distinctly different from those of the other complexes with two H-bonds. The complex has a slightly shortened C-H bond with a corresponding frequency of 3306 cm-1. Thus in contrast to the C-H stretching frequency of 3296 cm-1 in 2TX, the C-H stretching frequency of complex IV has a blue-shift of 10 cm-1. This result indicates that the C-H...O H-bond in complex IV is not a classical red-shifting H-bond but an improper blue-shifting H-bond [67–69]. Complex VII also has a C-H...O bond, the relative C-H bond is elongated and the corresponding stretching frequency has a red-shift of 31 cm-1, i.e. a classical red-shifting H-bond.
2TX has four hydrogen atoms, N(1)H, N(3)H, N(7)H, and C(8)H (see scheme 1). Their calculated 1H NMR chemical shifts (δ) are 7.76, 8.75, 7.93 and 8.75 ppm, respectively. Twanmoh reported the experimental NMR spectrum of 2TX in DMSO solution. The oxygen atom of DMSO can interact with the hydrogen atoms of 2TX. Thus, the corresponding proton chemical shifts of 2TX increase. Kupka and Hannongbua reported the experimental NMR spectra of uracil and nevirapine in DMSO, respectively. Their results show that the hydrogen bonds between the acidic protons and polar solvent molecules leads to the augmentation of the corresponding proton chemical shifts. As shown in Table 2, after the formation of H-bonds in complexes, the computed 1H NMR chemical shifts of H-bonded protons increases, whereas the non-H-bonding protons change very little. The proton of N(7)H, complex II, has a chemical shift of 13.2 ppm, whilst in the parent structure it is 8.75 ppm. The calculated chemical shift of 13.2 ppm for N(7)H is very close to the experimental values of 13.3 ppm in DMSO solution . The theoretical results show that the increase in δ of the H-bonded N-H proton in the complex is about 3-5 ppm, whilst for the H-bonded C-H proton, the changes are about 0.5-1.5 ppm. In complexes IV and VII, the C-H...O bond are improper blue-shifting and classical red-shifting H-bonds respectively, both of these types of H-bond give an increased 1H NMR chemical shift, with the largest increases being due to the classical red-shifting H-bond.
These results indicate that after formation of H-bonds, IR and NMR spectra change greatly, which further facilitates the identification of hydration of 2TX.
NBO and AIM analysis
For better understanding of the bonding characteristics in the hydrated 2TX complexes, NBO and AIM analysis were carried out at the MP2/6-311G(d, p) level.
The calculated NBO charges show that forming an H-bond will result in hydrogen possessing a greater positive charge, whereas X and Y have a more negative charge. But for the complex IV, the C atom of the C-H...O hydrogen bond has more positive charge. Electron density transfer (EDT) from water to 2TX for the most complexes is positive but the charge is transferred from 2TX to water in the complex IV. Thus, the improper blue-shifting C-H...O H-bond has different bonding characteristics from the other classical H-bonds.
GIAO MP2/6-311G(d, p) calculated 1H chemical shielding (δ/ppm) for isolated and monohydrated 2TX
Second-order perturbation stabilization energies ΔE(2) (kcal mol-1) of the H-bonded complexes
AIM theory has been successfully applied to characterizing hydrogen bonds of a series of H-bonded complexes [58, 59]. Popelier proposed a set of criteria for the existence of H-bonding based on AIM analysis. These criteria for hydrogen bonding are: (1) Correct topological pattern (i.e., the existence of a bond critical point (BCP) and a bond path); (2) proper value of electron density; (3) the Laplacian of electron density at the BCP; (4) mutual infiltration of H and Y atoms; (5) loss of hydrogen atom net charge; (6) energetic destabilization of hydrogen; (7) decrease of dipolar polarization; (8) decrease of hydrogen atomic volume. Here, these eight criteria are used to examine the studied H-bonded complexes.
Table 4 lists the topological properties of the BCP of the H-bonded complexes. The electron density (ρ) at the BCP varies from 0.0156 to 0.0335 au, which falls within the proposed range of 0.002-0.035 au for H-bonds. It has been shown the ρ at the BCP correlates with the interaction energy and H-bond length . As shown in Table 4, the ρ of the N-H...O bond is larger than that of the O-H...O bond, which is consistent with the N-H...O interaction having a shorter H-bond distance.
The third necessary criterion focuses on the Laplacian of the charge density (∇2ρ) at the BCP. It has been observed that for closed-shell interactions including ionic bonds, hydrogen bonds and van der Waals interactions, the ∇2ρ is positive . It can be seen that all the ∇2ρ at the BCP of the present studied H-bonds are positive ~0.0446-0.1009 au, which lies within the proposed range of 0.024 to 0.139 au [58, 59].
Electron density topological properties at the BCP of the X--H...Y H-bonds in the 2TX...H2O complexes.
Atomic basin integrated propertiesaof the hydrogen atoms in H-bond interactions and the relative difference between H-bonded complexes and parent molecule.
From the preceding discussion, the eight AIM criteria of hydrogen bonds are all echoed in the studied H-bonding interactions in the hydrated 2TX complexes. Electron density topological analysis does not show any obvious difference between the classical red-shifting and improper blue-shifting H-bonds. The classical red-shifting and improper blue-shifting H-bonds have consistent changes including the loss of charge, energetic destabilization, decrease of dipolar polarization, and decreased volume of the hydrogen atom in H-bonds.
MP2 and B3LYP calculations have been carried out to study the interactions between of 2-thioxanthine and water 1:1 complexes. Seven theoretical monohydrated complexes have been identified and reported for the first time. Harmonic vibrational frequency analysis confirms that these complexes are minima on the potential energy surface. The MP2 calculated bond lengths, angles and interactions energy are very close to the B3LYP results, which indicates the B3LYP method could also be a suitable tool for the study of similar H-bonded systems. Among the seven hydrated complexes, the closed complex II with N(7)-H...O and O-H...O hydrogen bonds is the most stable. The hydrogen bond energies of the complexes are correlated to the PA and DPE of the sites involved in interaction with water. The theoretical IR spectra show that most complexes have classical H-bonds with a stretching frequency red-shifted by 78-366 cm-1 accompanied by an increase in the relative infrared intensities of 100-600 km mol-1. An improper blue-shifting H-bond with a shortened C-H bond was found in complex IV. The theoretical GIAO NMR estimations show that the H-bonded proton of the complex has an increased chemical shift. There is a good linear correlation between the ΔE and δ of the H-bonded proton. NBO analysis shows that the absence of orbital interactions and repulsive electrostatic interactions results in the formation of a blue-shifting H-bond in complex IV. The eight AIM criteria of hydrogen bonds suggested by Popelier are all met in the studied H-bonding systems. However, electron density topological analysis does not show an obvious difference between the classical red-shifting and improper blue-shifting H-bonds.
XW is grateful for the support of National Science Foundation of China under Grant No 20503018. JSF and WC thank the Leverhulme Trust (F/00 351/P and F/00 094/BC). XW and JSF are grateful to the Royal Society UK and National Science Foundation China for facilitating UK China workshop events which led to completion of this work (Bath UK, CASE08 and East China University of Science and Technology CASE09).
- Fitter J, Lechner RE, Dencher NA: Interactions of hydration water and biological membranes studied by neutron scattering. J Phys Chem B. 1999, 103: 8036-8050. 10.1021/jp9912410.View ArticleGoogle Scholar
- Kim NJ, Kim YS, Jeong G, Ahn TK, Kim SK: Hydration of DNA base cations in the gas phase. Int J Mass Spectrom. 2002, 219: 11-21. 10.1016/S1387-3806(02)00547-X.View ArticleGoogle Scholar
- Pohil W, Gauger DR, Donrnberger U, Birch-hirschfeld E, Selle C: Hydration of biological molecules: lipids versus nucleic acids. Biospectroscopy. 2002, 67: 499-503.Google Scholar
- Bagchi B: Water dynamics in the hydration layer around proteins and micelles. Chem Rev. 2005, 105: 3197-6219. 10.1021/cr020661+.View ArticleGoogle Scholar
- Sokolov AP, Roh JH, Mamontov E, Garćia Sakai V: Role of hydration water in dynamics of biological macromolecules. Chem Phys. 2008, 345: 212-218. 10.1016/j.chemphys.2007.07.013.View ArticleGoogle Scholar
- He YG, Wu CY, Kong W: Photophysics of methyl-substituted uracils and thymines and their water complexes in the gas phase. J Phys Chem A. 2004, 108: 943-949. 10.1021/jp036553o.View ArticleGoogle Scholar
- Hendricks JH, Lyapustina SA, de Clercq HL, Bowen KH: The dipole bound-to-covalent anion transformation in uracil. J Chem Phys. 1998, 108: 8-11. 10.1063/1.475360.View ArticleGoogle Scholar
- Abo-Riziq A, Crews B, Grace L, de Vries MS: Microhydration of guanine base pairs. J Am Chem Soc. 2005, 127: 2374-2375. 10.1021/ja043000y.View ArticleGoogle Scholar
- Schiedt J, Weinkauf R, Neumark DM, Schlag EW: Anion spectroscopy of uracil, thymine and the amino-oxo and amino-hydroxy tautomers of cytosine and their water clusters. Chem Phys. 1998, 239: 511-524. 10.1016/S0301-0104(98)00361-9.View ArticleGoogle Scholar
- Chin W, Mons M, Piuzzi F, Tardivel B, Dimicoli I, Gord L, Leszczynski J: Gas phase rotamers of the nucleobase 9-methylguanine enol and its monohydrate: optical spectroscopy and quantum mechanical calculations. J Phys Chem A. 2004, 108: 8237-8243. 10.1021/jp048492f.View ArticleGoogle Scholar
- Schoone K, Smets J, Houben L, Van Bael MK, Adamowicz L, Maes G: Matrix-isolation FT-IR studies and theoretical calculations of hydrogen-bonded complexes of molecules modeling adenine tautomers. 1. H-Bonding of benzimidazoles with H2O in Ar Matrices. J Phys Chem A. 1998, 102: 4863-4877. 10.1021/jp980373a.View ArticleGoogle Scholar
- Ramaekers R, Dkhissi A, Adamowicz L, Maes G: Matrix-tsolation FT-IR study and theoretical calculations of the hydrogen-bond interaction of hypoxanthine with H2O. J Phys Chem A. 2002, 106: 4502-4512. 10.1021/jp013610+.View ArticleGoogle Scholar
- Kabeláč M, Hobza P: Hydration and stability of nucleic acid bases and base pairs. Phys Chem Chem Phys. 2007, 9: 903-917. 10.1039/b614420a.View ArticleGoogle Scholar
- Tho Nguyen M, Chandra A, Zeegers-Huyskens T: Protonation and deprotonation energies of uracil: Implications for the uracil-water complex. J Chem Soc Faraday Trans. 1998, 94: 1277-1280. 10.1039/a708804c.View ArticleGoogle Scholar
- Van Mourik T, Price SL, Clary DC: Ab initio calculations on uracil-Water. J Phys Chem A. 1999, 103: 1611-1618. 10.1021/jp983337k.View ArticleGoogle Scholar
- Kryachko ES, Nguyen MT, Zeegers-Huyskens T: Theoretical study of uracil tautomers. 2. interaction with Water. J Phys Chem A. 2001, 105: 1934-1943. 10.1021/jp0019411.View ArticleGoogle Scholar
- Chandra AK, Michalska D, Wysokiñsky R, Zeegers-Huyskens T: Theoretical study of the acidity and basicity of the cytosine tautomers and their 1:1 complexes with water. J Phys Chem A. 2004, 108: 9593-9600. 10.1021/jp040206c.View ArticleGoogle Scholar
- Chandra AK, Nguyen MT, Zeegers-Huyskens T: Theoretical study of the interaction between thymine and water. Protonation and deprotonation enthalpies and comparison with uracil. J Phys Chem A. 1998, 102: 6010-6016. 10.1021/jp981259v.View ArticleGoogle Scholar
- Zhang RB, Zeegers-Huyskens T, Ceulemans A, Nguyen MT: Interaction of triplet uracil and thymine with water. Chem Phy. 2005, 316: 35-44. 10.1016/j.chemphys.2005.04.028.View ArticleGoogle Scholar
- Frigato T, Svozil D, Jungwirth P: Valence- and dipole-bound anions of the thymine-water complex: ab initio characterization of the potential energy surfaces. J Phys Chem A. 2006, 110: 2916-2923. 10.1021/jp054090b.View ArticleGoogle Scholar
- Chandra AK, Nguyen MT, Uchimaru T, Zeegers-Huyskens T: DFT study of the interaction between guanine and water. J Mol Struct. 2000, 555: 61-66. 10.1016/S0022-2860(00)00587-1.View ArticleGoogle Scholar
- Shishkin OV, Sukhanov OS, Gorb L, Leszczynski J: The interaction of the most stable guanine tautomers with water. The structure and properties of monohydrates. Phys Chem Chem Phys. 2002, 4: 5359-5364. 10.1039/b205351a.View ArticleGoogle Scholar
- Chandra AK, Nguyen MT, Uchimarua T, Zeegers-Huyskens T: Protonation and deprotonation enthalpies of guanine and adenine and implications for the structure and energy of their complexes with water: comparison with uracil, thymine, and cytosine. J Phys Chem A. 1999, 103: 8853-8860. 10.1021/jp991660x.View ArticleGoogle Scholar
- Kim S, Schaefer HF: Effects of microsolvation on uracil and its radical anion: uracil. (H2O)n n = 1-5. J Chem Phys. 2006, 125: 144305-10.1063/1.2356464.View ArticleGoogle Scholar
- Trygubenko SA, Bogdan TV, Rueda M, Orozco M, Luque F, Šponer J, Slavíček P, Hobza P: Correlated ab initio study of nucleic acid bases and their tautomers in the gas phase, in a microhydrated environment and in aqueous solution. Phys Chem Chem Phys. 2002, 4: 4192-4203. 10.1039/b202156k.View ArticleGoogle Scholar
- Hanus M, Ryjáček F, Kabeláč M, Kubaø T, Bogdan TV, Trygubenko SA, Hobza P: Correlated ab initio study of nucleic acid bases and their tautomers in the gas phase, in a microhydrated environment and in aqueous solution. guanine: surprising stabilization of rare tautomers in aqueous solution. J Am Chem Soc. 2003, 125: 7678-7688. 10.1021/ja034245y.View ArticleGoogle Scholar
- Hanus M, Kubaø T, Rejnek J, Ryjáček F, Hobza P: Correlated ab initio dtudy of nucleic acid bases and their tautomers in the gas phase, in a microhydrated environment, and in aqueous solution. Part 3. adenine. J Phys Chem B. 2004, 108: 2087-2097. 10.1021/jp036090m.View ArticleGoogle Scholar
- Rejnek J, Hanus M, Kubaø T, Ryjáček F, Hobza P: Correlated ab initio study of nucleic acid bases and their tautomers in the gas phase, in a microhydrated environment and in aqueous solution. Part 4. Uracil and thyminewz. Phys Chem Chem Phys. 2005, 7: 2006-2017. 10.1039/b501499a.View ArticleGoogle Scholar
- Zhang JD, Chen ZF, Schaefer HF: Electron attachment to the hydrogenated watson-crick guanine cytosine base pair (GC+H): conventional and proton-transferred structures. J Phys Chem A. 2008, 112: 6217-6226. 10.1021/jp711958p.View ArticleGoogle Scholar
- Lyngdoh RHD, Schaefer HF: Elementary lesions in DNA subunits: electron, hydrogen atom, proton, and hydride transfers. Acc Chem Res. 2009, 42: 563-572. 10.1021/ar800077q.View ArticleGoogle Scholar
- Gu JD, Xie YM, Henry F, Schaefer : Electron attachment to oligonucleotide dimers in water: microsolvation-assisted base-stacking forms. Chem Phys Letts. 2009, 473: 213-219. 10.1016/j.cplett.2009.03.032.View ArticleGoogle Scholar
- Spiller GA: Caffeine. Boca Raton. 1998, Florida, CRC PressGoogle Scholar
- Miyamoto K, Yamamoto Y, Kurita M, Sakai R, Konno K, Sanae F, Ohshima T, Takagi K, Hasegawa T, Iwasaki N, Kakiuchi M, Kato H: Bronchodilator activity of xanthine derivatives substituted with functional groups at the 1- or 7-Position. J Med Chem. 1993, 36: 1380-1389. 10.1021/jm00062a010.View ArticleGoogle Scholar
- Yasui K, Komiyama A: New clinical applications of xanthine derivatives: modulatory actions on leukocyte survival and function. Int J Hematol. 2001, 73: 87-92. 10.1007/BF02981908.View ArticleGoogle Scholar
- Wang Z, Rana TM: RNA conformation in the Tat-TAR complex eetermined by site-specific photo-cross-linking. Biochem. 1996, 32: 6491-6499.View ArticleGoogle Scholar
- Darensbourg DJ, Frost BJ, Derecskei-Kovacs A, Reibenspies JH: Coordination chemistry, structure, and reactivity of thiouracil derivatives of tungsten(0) hexacarbonyl: a theoretical and experimental investigation into the chelation/dechelation of thiouracil via CO loss and addition. Inorg Chem. 1999, 38: 4715-4723. 10.1021/ic990758n.View ArticleGoogle Scholar
- Dafali A, Hammouti B, Mokhlisse R, Kertit S: Substituted uracils as corrosion inhibitors for copper in 3% NaCl solution. Corrosion Science. 2003, 45: 1619-1630. 10.1016/S0010-938X(02)00255-X.View ArticleGoogle Scholar
- Nielsen OH, Vainer B, Rask-Madsen J: The treatment of inflammatory bowel disease with 6-mercaptopurine or azathioprine. Aliment Pharmacol Ther. 2001, 15: 1699-1708. 10.1046/j.1365-2036.2001.01102.x.View ArticleGoogle Scholar
- Neunert CE, Buchanan GR: 6-Mercaptopurine: teaching an old drug new tricks. Pediatr Blood Cancer. 2009, 52: 5-6. 10.1002/pbc.21785.View ArticleGoogle Scholar
- Mautner HG, Bergson G: Some remarks on position-conditioned differences of the ultraviolet spectra and chemical reactivities of disubstituted pyrimidines and purines. Acta Chem Scand. 1963, 17: 1694-1704. 10.3891/acta.chem.scand.17-1694.View ArticleGoogle Scholar
- Twanmoh LM, Wood HB, Driscoll JS: NMR spectral characteristics of N-H protons in purine derivatives. J Heterocycl Chem. 1973, 10: 187-190. 10.1002/jhet.5570100210.View ArticleGoogle Scholar
- Civcir PU: Tautomerism of 2-thioxanthine in the gas and aqueous phases using AM1 and PM3 methods. J Mol Struct (Theochem). 2001, 546: 163-173. 10.1016/S0166-1280(01)00442-0.View ArticleGoogle Scholar
- Li BZ: Density functional theory calculation on 2-thioxanthine tautomers. Acta Phys Chim Sin. 2004, 20: 1455-1458.Google Scholar
- Stoychev G, Kierdaszuk B, Shugar D: Xanthosine and xanthineSubstrate properties with purine nucleoside phosphorylases, and relevance to other enzyme systems. Eur J Biochem. 2002, 269: 4048-4057. 10.1046/j.1432-1033.2002.03097.x.View ArticleGoogle Scholar
- Kulikowska E, Kierdaszuk B, Shugar D: Xanthine, xanthosine and its nucleotides: solution structuresof neutral and ionic forms, and relevance to substrate properties in various enzyme systems and metabolic pathways. Acta Biochim Polon. 2004, 51: 493-531.Google Scholar
- Speina E, Cieśla JM, Grąziewicz MA, Laval J, Kazimierczuk Z, Tudek B: Inhibition of DNA repair glycosylases by base analogs and tryptophan pyrolysate, Trp-P-1. Acta Biochim Polon. 2005, 52: 167-178.Google Scholar
- Tamta H, Kalra S, Thilagavathi R, Chakraborti AK, Mukhopadhyay AK: Nature and position of functional group on thiopurine substrates influence activity of xanthine oxidase -- Enzymatic reaction pathways of 6-mercaptopurine and 2-mercaptopurine are different. Biochemistry (Moscow). 2007, 72: 170-177. 10.1134/S000629790702006X.View ArticleGoogle Scholar
- Papakostas K, Georgopoulou E, Frillingos S: Cysteine-scanning analysis of putative helix XII in the YgfO xanthine permease. J Biol Chem. 2008, 283: 13666-13678. 10.1074/jbc.M800261200.View ArticleGoogle Scholar
- Reed AE, Curtiss LA, Weinhold F: Intermolecular interactions from a natural bond orbital, Donor-Acceptor Viewpoint. Chem Rev. 1988, 88: 899-926. 10.1021/cr00088a005.View ArticleGoogle Scholar
- Bader RWF: Atoms in molecules. a quantum theory. 1990, Oxford University Press: Oxford, UKGoogle Scholar
- Møller C, Plesset MS: Note on an approximation treatment for many-electron systems. Phys Rev. 1934, 46: 618-622. 10.1103/PhysRev.46.618.View ArticleGoogle Scholar
- Parr RG, Yang WT: Density-functional theory of atoms and molecules. 1989, Oxford University Press: New YorkGoogle Scholar
- Lee C, Yang WT, Parr RG: Development of the colle-salvetti correlation-energy formula into a functional of the electron density. Phys Rev B. 1988, 37: 785-789. 10.1103/PhysRevB.37.785.View ArticleGoogle Scholar
- Becke AD: Density-functional thermochemistry. III. The role of exact exchange. J Chem Phys. 1993, 98: 5648-5652. 10.1063/1.464913.View ArticleGoogle Scholar
- Boys SF, Bernardi F: The calculation of small molecular interactions by the differences of separate total energies. Some procedures with reduced errors. Molecular Physics. 1970, 19: 553-566. 10.1080/00268977000101561.View ArticleGoogle Scholar
- Ditchfield R: Self-consistent perturbation theory of diamagnetism I. A gauge-invariant LCAO method for N.M.R. chemical shifts. Molecular Physics. 1974, 27: 789-807. 10.1080/00268977400100711.View ArticleGoogle Scholar
- Wolinski K, Hilton JF, Pulay P: Efficient implementation of the gauge-independent atomic orbital method for NMR chemical shift calculations. J Am Chem Soc. 1990, 112: 8251-8260. 10.1021/ja00179a005.View ArticleGoogle Scholar
- Koch U, Popelier PLA: Characterization of C-H-O hydrogen bonds on the basis of the charge density. J Phys Chem. 1995, 99: 9747-9754. 10.1021/j100024a016.View ArticleGoogle Scholar
- Popelier PLA: Characterization of a dihydrogen bond on the basis of the electron density. J Phys Chem A. 1998, 102: 1873-1878. 10.1021/jp9805048.View ArticleGoogle Scholar
- Biegler-König F, Schönbohm J, Bayles D: AIM2000--A Program to Analyze and Visualize Atoms in Molecules. J Comput Chem. 2001, 22: 545-559. 10.1002/1096-987X(20010415)22:5<545::AID-JCC1027>3.0.CO;2-Y.View ArticleGoogle Scholar
- Biegler-König F, Schönbohm J, Bayles D, Bader RFW: AIM version 2.0. 2000, McMaster University, CanadaGoogle 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, et al: Gaussian 03 Revision D.01. 2004, Gaussian, Inc., Wallingford CTGoogle Scholar
- Jeffrey GA: An introduction to hydrogen bonding. 1989, Oxford University Press New YorkGoogle Scholar
- Rappé AK, Bernstein ER: Ab initio calculation of nonbonded interactions: Are ee there yet?. J Phys Chem A. 2000, 104: 6117-6128. 10.1021/jp0008997.View ArticleGoogle Scholar
- Del Bene JE, Perera SA, Bartlett RJ: Vibrational spectroscopic and NMR properties of hydrogen-bonded complexes: Do they tell us the same thing?. J Am Chem Soc. 2000, 122: 4794-4797. 10.1021/ja994458g.View ArticleGoogle Scholar
- Becker ED: In encyclopaedia of nuclear magnetic resonance. Edited by: Grant DM, Harris RK. 1996, John Wiley and Sons: New York, 2409-2415. and references thereinGoogle Scholar
- Hobza P, Havlas Z: Blue-shifting hydrogen bonds. Chem Rev. 2000, 100: 4253-4264. 10.1021/cr990050q.View ArticleGoogle Scholar
- Li XS, Liu L, Schlegel HB: On the physical origin of blue-shifted hydrogen bonds. J Am Chem Soc. 2002, 124: 9639-9647. 10.1021/ja020213j.View ArticleGoogle Scholar
- Hermansson K: Blue-shifting hydrogen bonds. J Phys Chem A. 2002, 106: 4695-4702. 10.1021/jp0143948.View ArticleGoogle Scholar
- Blicharska B, Kupka T: Theoretical DFT and experimental NMR studies on uracil and 5-fluorouracil. J Mol Struct. 2002, 613: 153-166. 10.1016/S0022-2860(02)00171-0.View ArticleGoogle Scholar
- Vailikhit V, Treesuwan W, Hannongbua S: A combined MD-ONIOM2 approach for 1H NMR chemical shift calculations including a polar solvent. J Mol Struct (Theochem). 2007, 806: 99-104. 10.1016/j.theochem.2006.11.013.View ArticleGoogle Scholar
- Del Bene JE, Perera SA, Bartlett RJ: Hydrogen bond Types, binding energies, and 1H NMR chemical shifts. J Phys Chem A. 1999, 103: 8121-8124. 10.1021/jp9920444.View ArticleGoogle Scholar
- Wang X, Zhou G, Tian AM, Wong NB: Ab initio investigation on blue shift and red shift of C-H stretching vibrational frequency in NH3...CHnX4-n (n = 1, 3, X = F, Cl, Br, I) complexes. J Mol Struct (Theochem). 2005, 718: 1-7. 10.1016/j.theochem.2004.10.039.View ArticleGoogle Scholar
This article is published under license to BioMed Central Ltd. This is an Open Access article distributed under the terms of the Creative Commons Attribution License (http://creativecommons.org/licenses/by/2.0), which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.