Research Article  Open Access
Computational Studies on the Molecule 1(2Hydroxyethyl)5Fluorouracil in Gas Phase and Aqueous Solution and Prediction of Its Confinement inside Capped Nanotubes
Abstract
Density functional theory (DFT) calculations were performed on a fluorouracil derivative at the B3LYP/6−31+G(d) level. Furthermore, the ONIOM method was performed to investigate the possibility of its confinement inside capped nanotubes. The results found of the structural parameters of the optimized molecule are in good agreement with experimental data. The analysis of thermodynamic properties leads us to predict that the confinement of the studied molecule inside capped nanotubes SWCNT(12,0), SWCNT(14,0), and SWCNT(16,0) is possible. The large values found suggest a good stability for the studied molecule. The predicted nonlinear optical (NLO) properties of the studied molecule are much greater than those of urea. Thereby, it is a good candidate as secondorder NLO material. The calculated values suggest that the studied molecule is more soluble than the 5FU molecule. The results of quantum molecular descriptors show that the studied molecule is hard electrophile and strongly reactive.
1. Introduction
Experimental and theoretical studies have been previously done on the molecule uracil and its derivatives [1], especially the anticarcinogenic drug 5fluorouracil (5FU) [2] employed for treating solids tumors, especially those of gastrointestinal tract, brain, breast, pancreas, and liver [3]. One of the 5FU derivatives recently characterized by Xray diffraction is the molecule 1(2hydroxyethyl)5fluorouracil [4]. A good understanding of properties of molecules with therapeutic effects is very crucial, as well as their direct delivery to the right target. The study of interactions between nanostructures and therapeutic molecules is very important for the carrying and targeted delivery of drugs and other biomolecules. Various types of hybrid nanostructures modeled by the interaction of therapeutic molecules or chemical substances with nanometric structures such as phagraphene [5], fullerenes [6], and boron nitride nanoparticles [7] have been reported in the literature. These nanostructures can also be very important for applications such as the design of sensor systems [8] and energy storage devices [9]. The carbon nanotube is one of the most popular nanostructures used as nanocarrier on the basis of interactions with chemical compounds.
The confinement of molecules inside carbon nanotubes remains a big challenge. The confinement of therapeutic molecules inside nanotubes is very interesting due to the fact that the nanotube protects the biologically active molecule from degradation, and the hybrid nanostructure formed by the nanotube and the confined molecule can overcome the resistance of mechanical, physicochemical, and enzymatic barriers. Nanotubes can even cross biological barriers [10], thus offering the possibility of using them in gene therapy. Zare et al. [11] have reported a research work on the comparison of drug delivery systems. They have shown that carbon nanotubes deliver the 5FU molecule better than the psulfonatocalixarene. Carbon nanotubes have a great potential to carry molecules. Many studies on medical and biomedical applications [12, 13] of carbon nanotubes have been reported in the literature. Robinson et al. [14] have developed a generalized numerical method for generating the atomic coordinates of nanotube caps.
Many computational methods [15] have been developed to investigate the properties of molecules. Density functional theory (DFT) is greatly used in molecular computational study. This computational method reproduces very well the experimental properties of molecules such as geometrical structures, vibrational properties, and nonlinear and electronic properties [16, 17]. Recently, it has been reported that the van der Waals interactions play a major role in the encapsulation of molecules inside carbon nanotubes [18]. The van der Waals interactions can be taken into consideration in the modeling of hybrid nanostructures using the quantum mechanics (QM)/molecular mechanics (MM) calculations, especially the ONIOM method. The ONIOM method [19] has proved to be a powerful tool in combining quantum mechanics and molecular mechanics calculations. Chung et al. [20] have reported a review on the ONIOM method and its applications. In their review, many theoretical investigations using ONIOM methods on the encapsulation of molecules inside carbon nanotubes and other nanostructures have been reported. In particular, Garcia et al. [21] have studied the confinement of carotene inside carbon nanotubes using an ONIOM method. Ahmadi et al. [22] have studied the adsorption of ammonia molecules inside aluminum nitride nanotubes using an ONIOM method. To experimentally encapsulate a drug into a capped carbon nanotube, the first step is to synthesize the carbon nanotube [23]. As the synthesized nanotubes are usually closed by domes, at least one end must be opened before incorporation of the drug. The opening of the nanotube can be done by chemical oxidation [24] or thermal oxidation [25]. Yudasaka et al. [26] have developed two different methods, called nanoextraction and nanocondensation, to incorporate guest molecules into singlewalled carbon nanotubes in liquid phases. Ren et al. [27] have applied the nanoextraction method to incorporate the antitumor agent hexamethylmelamine into carbon nanotubes. Recently, Wu et al. [28] have also used the nanoextraction method to incorporate the antitumor agent oxaliplatin into multiwalled carbon nanotubes. Satishkumar et al. [24] have reported experimental methods for closing carbon nanotubes. They have experimentally shown that uncapped nanotubes can be closed by the reaction at high temperature with benzene vapour in a reducing atmosphere of hydrogen and argon.
To the best of our knowledge, this is the first theoretical study on the molecule 1(2hydroxyethyl)5fluorouracil published. The aim of this work is to investigate the properties of the molecule 1(2hydroxyethyl)5fluorouracil in gas phase and aqueous solution. Furthermore, the changes occurring in the molecular geometrical structure and the thermodynamic stability when it is confined inside the hollow space of capped nanotubes SWCNT(12,0), SWCNT(14,0), and SWCNT(16,0) by considering mainly the van der Waals interaction have been investigated. This study is performed to predict the encapsulation of this molecule into carbon nanotubes; the longterm objective is to perform a targeted delivery of this molecule in cancer cells following the model proposed by Hilder et al. [29]. In this study, the molecular structure analysis of the studied molecule has been performed in gas phase and aqueous solution by a DFT method and inside the nanotube cavity by an ONIOM(DFT:MM) method. The thermodynamic properties of the studied molecule and the thermodynamic stability study of the optimized hybrid nanostructures have been investigated at different temperatures. The vibrational analysis, the nonlinear and electronic properties, the Gibbs free energy of solvation, and the quantum molecular descriptors of the studied molecule have been investigated in gas phase and aqueous solution.
2. Computational Methodology
Density functional theory (DFT) was performed for the calculations of properties of the studied molecule in gas phase and aqueous solution, while the ONIOM(DFT:MM) method was performed to study the hybrid nanostructures. The hybrid nanostructures were obtained by the confinement of the studied molecule inside the nanotube cavities. We used capped nanotubes SWCNT(12,0), SWCNT(14,0), and SWCNT(16,0) of 336, 428, and 488 carbon atoms, respectively. The diameters of these nanotubes are 9.402 Å, 10.968 Å, and 12.536 Å. These nanotubes were chosen to point up the diameter range of carbon nanotubes that allow the studied molecule to be confined without any significant molecular geometry alteration. The uncapped nanotubes SWCNT(12,0), SWCNT(14,0), and SWCNT(16,0) have a finite length of 17.39 Å, and they have 204, 238, and 272 carbon atoms, respectively. Each cap of these nanotubes was formed with pentagonal defects. The 2D projections of the capped nanotubes are shown in Figure 1(a). The full geometry optimizations were performed on the studied molecule and the hybrid nanostructures using Gaussian 09 W program [30]. The results of simulations were visualized by GaussView 5 program [31]. We used the functional B3LYP with the 6−31+G(d) basis set to implement DFT calculations. The polarizable continuum model with a conductor solvent model (CPCM) was applied to account for solvation effects. In our calculations, water (dielectric constant () of 78.4) was used as solvating medium. The Gibbs free energy of solvation was calculated by taking the difference between the total electronic energy in water after polarized continuum model (PCM) corrections using the SMD continuum model [32] and the total electronic energy in gas phase.
(a)
(b)
(c)
The inclusion of van der Waals (vdW) interactions [18] for an accurate description of the molecular structure of nanostructures designed by encapsulation of molecule inside the hollow space of nanotube is indispensable. The combination of DFT with the united force field (UFF) has been widely used [33, 34]. The noncovalent interactions were applied during the optimization of the hybrid nanostructures with the ONIOM method by combining the B3LYP/6−31+G(d) level with the united force field (UFF). The stability constant and thermodynamic quantities such as enthalpy, Gibbs free energy, and entropy were computed to analyze the stability of the optimized hybrid nanostructures. The use of localized basis sets reduces the amount of computational work required. However, calculations using finite basis sets are susceptible to basis set superposition errors (BSSEs). The changes of energies in all complexes nanostructures were corrected by calculating the basis set superposition error using the counterpoise method [35]. In this method, the BSSE is calculated using the mixed basis sets, and the error is then subtracted a posteriori from the uncorrected energy. The mixed basis sets are realized by introducing “ghost orbitals” (basis set functions which have no electrons or protons).
Unscaled vibrational properties of the studied molecule were computed in gas phase and aqueous solution. The nonlinear and electronic properties were calculated using the optimized molecular structure. A dipole moment can be induced through the electric polarizability under the influence of an external electric field E. For an intense electric field the total dipole moment can be written as a Taylor series expansion induced by the field:where is the permanent dipole moment and and are the components of the polarizability and firstorder hyperpolarizability, respectively. The total dipole moment (), the mean polarizability (), and the static firstorder hyperpolarizability () are calculated from the Gaussian output by using the equations found in the literature [36]. The total density of states (DOS) of the studied molecule was plotted with the data of molecular orbitals obtained using GaussSum 2.2 program [37]. The difference between the energies of the LUMO and HOMO orbitals corresponds to the energy gap. Furthermore, the HOMO energy and LUMO energy were used to calculate the quantum molecular descriptors. The ionization potential (IP) and the electron affinity (EA) were derived from the frontier molecular orbital energies using the following relations, respectively, and . The hardness (), softness (), electronegativity (), chemical potential (), and electrophilicity index () were calculated using the equations reported in the literature [38].
The molecular electrostatic potential (MEP) is related to the electronic density. It is a very useful descriptor in understanding sites for electrophilic attack, nucleophilic reactions, and intermolecular interactions with other molecular compounds. The molecular electrostatic potential created at any given point in the vicinity of a molecule by its electrons and nuclei is found by where is the charge of nucleus A located at , is the electronic density function for the molecule, and is the dummy integration variable [39].
3. Results and Discussion
3.1. Optimized Structure
The optimized geometrical parameters of the studied molecule in gas phase, aqueous solution, and the hollow space of the capped nanotubes SWCNT(12,0), SWCNT(14,0), and SWCNT(16,0) are gathered in Table 1. The molecular structure of the studied molecule and the optimized hybrid nanostructures are shown in Figures 1(b) and 1(c), respectively. The computed bond lengths of the studied molecule in gas phase and aqueous solution and inside the capped nanotubes change slightly in comparison to experimental values of the crystal structure [4]. The changes of structural parameters of the studied molecule in aqueous solution in comparison to those in gas phase are induced by the dipolar interaction between it and the solvating medium. Inside the nanotube cavity, the van der Waals interactions applied between the confined molecule and the nanotube contribute mainly to the changes of structural parameters of the studied molecule in comparison to those in gas phase.

The maximum difference between the theoretical and experimental bond lengths is found at C8−C9 bond. The bond lengths N1−C10, N1−C7, N2−C10, N2−C9, and C8−C9 in the gas phase and aqueous solution and inside nanotubes are close to the experimental values of the studied molecule and slightly lower than the corresponding experimental bonds of the 5fluorouracil (5FU) molecule [2]. The bonds O4−C10 and O5−C9 are very close to the experimental values of the studied molecule and slightly greater than the corresponding experimental bonds of the 5FU molecule [2].
As illustrated in Table 1, most computed angles are slightly different from experimental ones. In comparison to experimental bond angles, the maximum shifts occur at C10−N1−C11 bond angle in gas phase and at N1−C11−C12 bond angle in aqueous solution and inside nanotubes. The most discrepancy between the studied fluorouracil derivative and the 5FU molecule occurs at the N2−C9−C8 bond angle. Thus, the replacement of the hydrogen atom in the 5FU molecule at the position N1 by the 1(2hydroxyethyl) fragment induces changes of molecular geometrical parameters of the pyrimidine ring. The dihedral angles N1−C11−C12−06 of the confined molecule are 94.223°, 52.307°, and 51.057, and the dihedral angles C11−C12−06−H14 are −54.497°, 41.838°, and 35.051° inside SWCNT(12,0), SWCNT(14,0), and SWCNT(16,0), respectively. Clearly, the structure of the studied molecule can be affected by the confinement into the capped nanotube SWCNT(12,0) because the dihedral angles N1−C11−C12−06 and C11−C12−06−H14 of the isolated molecule are 50.822° and 37.769°, respectively. When the studied molecule is confined inside the nanotube SWCNT(14,0) or SWCNT(16,0), its structural parameters are not evidently affected by the nanotube. The geometries of the confined molecule inside SWCNT(14,0) and SWCNT(16,0) are very similar to those of the isolated molecule. The confined molecule approximately locates in the middle axis of SWCNT(12,0) and SWCNT(14,0), but it is in the side of SWCNT(16,0). We can conclude that any nanotube whose diameter is greater than 10.968 Å will have no significant influence on the geometry of the studied molecule. However, nanotubes whose diameter is less than 9.402 Å can significantly change or destroy the molecular structure of the confined molecule. The results found for structural parameters of the studied molecule are in good agreement with Xray crystallographic data [4].
3.2. Thermodynamic Properties of the Studied Molecule and Thermodynamic Stability Study of the Optimized Hybrid Nanostructures
The vibrational analysis and statistical thermodynamics were applied to compute the standard thermodynamic properties of the studied molecule. The computed thermodynamic properties, namely, enthalpy (), Gibbs free energy (), and entropy (), are gathered in Supplementary Material S1. Figure 2 shows the changes of , , and with the temperature. As illustrated in Figure 2, the values of and increase while the values decrease with the increasing of the temperature from 50 to 950 K. These changes occur because the intensities of the molecular vibrations increase with the increasing temperature. The quadratic correlation equations of the studied molecule are given below.These equations have strong correlations with the computed thermodynamic properties. Thereby, the values of the standard thermodynamic properties , , and of the studied molecule can be predicted at any temperature with these correlation equations and will be helpful for further studies.
(a)
(b)
(c)
The twolayered ONIOM method has been used to study the confinement of the studied molecule inside capped nanotubes SWCNT(12,0), SWCNT(14,0), and SWCNT(16,0). In this work, the ONIOM method is implemented by treating the full system at the low level of theory (a molecular mechanics method) and the interesting part of the system at high level of theory (a quantum mechanics method). The enthalpy change, , and the change of Gibbs free energy, , for the confinement reaction between the studied molecule and the nanotubes were estimated on the basis of the confinement energy found in the literature [34, 40, 41]. The entropy change was derived from and . The enthalpy change , the entropy change , the change of Gibbs free energy and the stability constant for the confinement reaction leading to the optimized hybrid nanostructures are reported in Supplementary Material S2. As illustrated in Figure 3(a), the values are negative and increase at any temperature from 100 to 900 K. Hence, the formation of optimized hybrid nanostructures is an exothermic process. The thermodynamic quantity provides information about the order or disorder of optimized hybrid nanostructures. The values are negative at any temperature from 100 to 900 K. Thus, the formation of optimized hybrid nanostructures is done in an ordered way. However, as illustrated in Figure 3(b), a reduction of the degree of organization of hybrid nanostructures is done with the increasing temperature because the values increase. As shown in Figure 3(c) the values increase in the range of 100900 K. In addition, the values under 900 K are negative (see Supplementary Material S2), which implies that the confinement of the studied molecule inside the hollow space of capped nanotubes SWCNT(12,0), SWCNT(14,0), and SWCNT(16,0) is possible. Thus, the formation process of optimized hybrid nanostructures is spontaneous and thermodynamically favorable for temperatures under 900 K. As shown in Figure 3(d), the stability constant values decrease with the increasing temperature. This implies that the interaction between the confined molecule and each capped nanotube decreases with the increasing temperature. At low temperatures, the interaction between the confined molecule and the nanotube is relatively weak.
(a)
(b)
(c)
(d)
According to the thermodynamic properties and the stability constant computed, the confinement of the studied molecule inside capped nanotubes SWCNT(12,0), SWCNT(14,0), and SWCNT(16,0) is possible and the formation of optimized hybrid nanostructures is thermodynamically favorable.
3.3. Vibrational Analysis of the Studied Molecule in Gas Phase and Aqueous Solution
Vibrational results are useful to better characterize the studied molecule. The quantities of interest in vibrational spectra are frequencies and intensities. The PCM model has been extended to vibrational studies [42]. In aqueous solution, the reaction field of water perturbs the molecular potential energy surface (PES) and induces changes of vibrational frequencies. The vibrational frequencies, IR intensities, Raman activities, and assignments of strong vibrational modes of the studied molecule in gas phase and aqueous solution are reported in Table 2. Most modes are not pure but contain significant contributions of other modes. The IR intensity and Raman activity spectra are shown in Figure 4.
 
a: limited to the description of strong vibrational modes of the studied molecule and the reported vibrational modes are those of the studied molecule in gas phase although many descriptions are identical in the two media (in gas and water). b: , , and , stretching (simple, symmetric, and asymmetric); : in plane bending (simple, scissoring); : out of plane bending (twisting, overtone, wagging, deformation); : rocking. 
The solvation of the studied molecule produces greater shifts between the computed values in gas phase and aqueous solution of IR intensities and Raman activities. The maximum IR intensities are 717.354 and 1468.833 Km/mol and are observed in gas phase and aqueous solution at 1762.630 and 1707.784 cm^{−1}, respectively. Similarly, the maximum Raman activities are 202.427 and 368.806 A^{4}/AMU and are observed in gas phase and aqueous solution at 3000.562 and 3031.451 cm^{−1}, respectively. Identical vibrational modes contribute to the maximum IR intensities and Raman activities in gas phase and aqueous solution but with different intensities. The stretching vibrational mode of the bond C10=O and the bending vibrational mode of angles formed with the N2−H bond in the plane of the pyrimidine ring constitute two contributions to maximum IR intensities of the studied molecule in gas phase and aqueous solution. The symmetric stretching vibrational modes of the −CH2 group at position C12 contribute to maximum Raman activities of the studied molecule in gas phase and aqueous solution. The first three maximum unscaled vibrational frequencies are found at 3693.369, 3586.430, and 3238.231 cm^{−1} in gas phase and 3705.977, 3577.938, and 3251.219 cm^{−1} in aqueous solution and correspond to the O−H stretching vibration, N2−H stretching vibration, and C7−H stretching vibration, respectively. The scaling factor 0.95 is appropriated to compute vibrational frequencies at B3LYP/6−31+G level [43]. The maximum vibrational frequencies found with the scaling factor 0.95 are 3508.701, 3407.109, and 3076.319 cm^{−1} in gas phase and 3520.678, 3399.041, and 3088.658 cm^{−1} in aqueous solution, respectively. The maximum vibrational modes of the studied molecule have been observed experimentally at 3520, 3410, and 2994 cm^{−1} [4]. The O−H stretching vibration usually occurs in the region 3300−3600 cm^{−1} [44]. The vibrational stretching modes N2−H and C7−H have been experimentally observed in the molecule 5FU at 2992 and 2815 cm^{−1} [4] and theoretically observed without scaling factor with the 3P86/6−31G(d,p) level at 3640 and 3258 cm^{−1} [2], respectively. In the uracil molecule, the N2−H and C7−H vibrational modes have been experimentally observed at 3160 and 3090 cm^{−1} [1] and theoretically observed without scaling factor with the B3LYP/6−311++G(d,p) basis at 3597 and 3244 cm^{−1} [1], respectively. Thereby, with the scaling factor 0.95, the computed vibrational frequencies at B3LYP/6−31+G(d) are in good agreement with the experimental IR frequencies values [4].
3.4. Nonlinear and Electronic Properties, Gibbs Free Energy of Solvation, and Quantum Molecular Descriptors of the Studied Molecule
The nonlinear optical (NLO) properties of organic molecules are extensively investigated with density functionals [45]. The values of the computed NLO properties are gathered in Table 3. The following relations have been used to convert the mean polarizability () and the static firstorder hyperpolarizability () in electrostatic units (esu): 1 a.u. of esu and 1 a.u. of esu. In aqueous solution, the values of , , and increase. When the studied molecule is solvated, the reaction field of water modifies the nonlinear responses. The calculated dipole moment is 5.117 D in gas phase. The computed value of the urea molecule is with the B3LYP/6−31+G(d) method. Gester et al. [46] have reported a value of 3.93 D in gas phase and 5.91 D in aqueous solution for the 5FU molecule. The polarizability tensor () is dominated by the diagonal components and the highest value is obtained for the component . In this direction, the found value is in gas phase and in aqueous solution. The value of the studied molecule is greater than that of urea ( at B3LYP/6−31+G(d) level). Basis sets have effects on the hyperpolarizability. Fernando et al. [47] have shown that the inclusion of diffuse functions into basis sets is crucial to obtain accurate results of the hyperpolarizability. Therefore, diffuse basis sets give acceptable values of the hyperpolarizability. The urea molecule is a wellknown NLO material and is widely used to predict good NLO material on the basis of the static firstorder hyperpolarizability. The value of urea computed at the B3LYP/6−31+G(d) level is . This value is slightly lower than the value reported in the literature at B3LYP/6−31++G(d,p) level () [48]. The value of the studied molecule is , which is theoretically 2.82 times greater than that of urea at B3LYP/6−31+G(d) level. These results show that the studied molecule is a good candidate as secondorder NLO material.

The analysis of electronic properties of organic molecules is usually related to frontier orbitals [17]. The HOMO and LUMO orbitals and the density of states (DOS) plot of the studied molecule are shown in Figures 5 and 6. The LUMO orbital is mainly localized on the pyrimidine ring, while the HOMO orbital is localized on the whole molecule. The HOMO and LUMO values are −7.122 eV and −1.955 eV in gas phase and −6.947 eV and −1.782 eV in aqueous solution. The solvation modifies slightly the band structure of the studied molecule. The results of the energy gap () gathered in Table 3 show that the solvation decreases slightly the value when the studied molecule is moved from the gas phase to aqueous solution. The large values found refer to high excitation energies for many excited states and suggest a good stability for the studied therapeutic molecule.
Pienko et al. [49] have reported in the literature that the solubility is a crucial parameter for bioavailability prediction of therapeutic molecule. The Gibbs free energy of solvation () is a physicochemical parameter related to the solubility, which can be derived from quantum mechanical calculations. From thermodynamic consideration, negative values of mean that the process of solvation is spontaneous. The more negative the value, the higher the degree of solubility. The computed value of the studied molecule is −18.524 Kcal/mol. Therefore, the dissolution in water of the studied molecule is spontaneous. The computed value of the 5FU molecule is −15.950 Kcal/mol with the CPCM/B3LYP/6−31+G(d) method. This shows that the studied molecule is more soluble than the 5FU molecule. The increase in the degree of solubility in water of the studied molecule in comparison to 5FU molecule is probably induced by the presence of the 1(2hydroxyethyl) fragment. Recently, Zafar et al. [50] have estimated the range of Gibbs free energy of solvation in drug design; they have reported that the value of quality drug candidates should be less than −12 Kcal/mol. the value of the studied molecule is much less than −12 Kcal/mol. Therefore, the studied molecule is a promising quality drug candidate.
Table 4 shows the calculated quantum molecular descriptors of the studied molecule in gas phase and aqueous solution. When the studied molecule is moved from the gas phase to aqueous solution, the values of EA, IP, , , , and decrease.

The computed values of the electron affinity (EA) and the ionization potential (IP) of the 5FU molecule are 1.955 and 7.276 eV with the B3LYP/6−31+G(d) method, respectively. The IP value of the studied molecule decreases in comparison to that of the 5FU molecule. However, the EA value does not change because the LUMO orbital, which is directly related to the electron affinity, is localized on the pyrimidine ring. Furthermore, the values of and of the 5FU molecule are 4.615 and −4.615 eV, respectively. These results show that the reactivity of the studied molecule is improved because its IP value decreases, while its value increases in comparison to those of the 5FU molecule. The harness of a molecule refers to its resistance toward deformation in presence of an electric field. Usually, a soft molecule has a small energy gap, while a hard molecule has a large energy gap. The studied molecule is hard because its harness is greater than its softness. This result is in agreement with the large energy gap found. The computed values of and of the 5FU molecule are 2.660 eV and 0.375 eV^{−1} with the B3LYP/6−31+G(d) method, respectively. The comparison of the harness and softness of the studied molecule with those of the 5FU molecule indicates that the studied molecule is more soft and less hard than the 5FU molecule. Schwöbel et al. [51] have reported a review of experimental and theoretical methods of measurement and estimation of electrophilic reactivity. It appears that the electrophilicity index is a good descriptor to measure the electrophilic reactivity of chemical compounds. Parthasarathi et al. [52] have reported in the literature a study on the biological activity prediction with the electrophilicity index. Their results show that the biological activity of chemical compounds may be effectively described with the electrophilicity index. Furthermore, Roy et al. [53] have reported research work on the toxicity prediction with the electrophilicity. They showed that the electrophilicity is a promising descriptor for toxicological prediction considering the case of aliphatic compounds. The value of the studied molecule varies very slightly in comparison to 5FU molecule ( with the B3LYP/6−31+G(d) method). This molecule is hard electrophile.
The sites for nucleophilic and electrophilic reactions have been determined with the molecular electrostatic potential (MEP). Figure 7 shows the total electron density surface mapped with electrostatic potential of the studied molecule. Potential increases in the order red < orange < yellow < green < blue. Atoms localized in the red regions are negative potential sites and participate in electrophilic reactions, while atoms localized in the blue regions are positive potential sites and participate in nucleophilic reactions. The V(r) values near the atoms O5, O6, O4, and F of the studied molecule are −0.052, −0.041, −0.033, and −0.022 au, respectively. These sites are the most negative potential sites and are involved in electrophilic reactions. The most positive potential sites are localized near the C7−H and N2−H bonds. The V(r) values near the C7−H and N2−H bonds are 0.055 and 0.052 au, respectively. These sites are involved in nucleophilic reactions. These results provide information of sites where the studied molecule can have intermolecular interactions with other compounds (as a nanotube during the confinement process and water during the solvation process) and covalent bonding with toxic proteins in the inhibition process of their activities.
4. Conclusions
Density functional theory calculations have been performed on the molecule 1(2hydroxyethyl)5fluorouracil in gas phase and aqueous solution, and the ONIOM method has been performed to investigate the possibility of its confinement inside capped carbon nanotubes SWCNT(12,0), SWCNT(14,0), and SWCNT(16,0). The results found for structural parameters of the studied molecule are in good agreement with the Xray crystallographic data. The solvation and the confinement inside nanotubes of the studied molecule change slightly its molecular geometrical parameters. Correlation equations have been obtained to predict the standard thermodynamics properties , , and of the studied molecule at any temperatures. The analysis of the thermodynamic properties , , and and the stability constant leads to the prediction that the confinement of the studied molecule inside these nanotubes is possible and the formation of optimized hybrid nanostructures is thermodynamically favorable. Vibrational analysis has been performed to better characterize the optimized molecule in gas phase and aqueous solution. The solvation of the studied molecule produces greater shifts between the computed values in gas phase and aqueous solution of IR intensities and Raman activities. The predicted nonlinear properties of the studied molecule are much greater than those of urea. The studied molecule is a good candidate as secondorder NLO material. The large values found suggest a good stability for the studied molecule. The calculated values suggest that the studied molecule is more soluble than the 5FU molecule. Frontier molecular orbital (FMO) energies have been employed to study the quantum molecular descriptors according to Koopmans theorem. The solvation decreases the values of EA, IP, , , , and . The results of EA and IP show that the studied molecule has the same tendency to accept electrons as the 5FU molecule from a donor and its reactivity is higher than that of the 5FU molecule. The value of this fluorouracil derivative confirms that its reactivity is improved in comparison to that of the 5FU molecule. The studied molecule is more soft and less hard than the 5FU molecule. The value of the studied molecule changes very slightly in comparison to that of the 5FU molecule. We hope that these results will be helpful for other researches on new organic materials, drugs, and hybrid nanostructures.
Data Availability
The data used to support the findings of this study are included within the article.
Conflicts of Interest
The authors declare that there are no conflicts of interest as concerns this article.
Acknowledgments
We are thankful to the Council of Scientific and Industrial Research (CSIR), India, forfinancial support through Emeritus Professor scheme (grant no. 21(0582)/03/EMRII) to Late Prof. A.N. Singh of the Physics Department, Bahamas Hindu University, India, which enabled him to purchase the Gaussian Software. We are most grateful to Late Emeritus Prof. A.N. Singh for donating this software to one of us, Dr. Geh Wilson Ejuh, and to the Materials Science Laboratory of the University of Yaoundé I for enabling us to use their computing facilities.
Supplementary Materials
The standard enthalpy, Gibbs free energy, and entropy of the studied fluorouracil derivative at temperatures in the range of 50950 K are listed in Supplementary Material 1. The enthalpy change, the change of Gibbs free energy, the entropy change, and stability constant for the confinement reaction of the optimized hybrid nanostructures at temperatures in the range of 100−900 K are listed in Supplementary Material 2 associated with this manuscript. (Supplementary Materials)
References
 J. Singh, “FTIR and Raman spectra, ab initio and density functional computations of the vibrational spectra, molecular geometries and atomic charges of uracil and 5methyluracil (thymine),” Spectrochimica Acta Part A: Molecular and Biomolecular Spectroscopy, vol. 137, pp. 625–640, 2015. View at: Publisher Site  Google Scholar
 V. K. Rastogi, V. Jain, R. A. Yadav, C. Singh, and M. A. Palafox, “Fourier transform Raman spectrum and ab initio and density functional computations of the vibrational spectrum, molecular geometry, atomic charges and some molecular properties of the anticarcinogenic drug 5‐fluorouracil,” Journal of Raman Spectroscopy, vol. 31, no. 7, pp. 595–603. View at: Publisher Site  Google Scholar
 J. L. Arias, “Novel strategies to improve the anticancer action of 5fluorouracil by using drug delivery systems,” Molecules, vol. 13, no. 10, pp. 2340–2369, 2008. View at: Publisher Site  Google Scholar
 X. Xu, G. Yao, Y. Li et al., “5Fluorouracil derivatives from the sponge Phakellia fusca,” Journal of Natural Products, vol. 66, no. 2, pp. 285–288, 2003. View at: Publisher Site  Google Scholar
 R. Bagheri, M. Babazadeh, E. Vessally, M. Es'haghi, and A. Bekhradnia, “Sidoped phagraphene as a drug carrier for adrucil anticancer drug: DFT studies,” Inorganic Chemistry Communications, vol. 90, pp. 8–14, 2018. View at: Publisher Site  Google Scholar
 S. A. Siadati, K. Kula, and E. Babanezhad, “The possibility of a twostep oxidation of the surface of C20 fullerene by a single molecule of nitric (V) acid, initiate by a rare [2+3] cycloaddition,” Chemical Review and Letters, vol. 2, pp. 2–6, 2019. View at: Google Scholar
 R. Rostamoghli, M. Vakili, A. Banaei, E. Pourbashir, and K. Jalalierad, “Applying the B12N12 nanoparticle as the CO, CO2, H2O and NH3 sensor,” Chemical Review and Letters, vol. 1, pp. 31–36, 2018. View at: Google Scholar
 E. Babanezhad and A. Beheshti, “The possibility of selective sensing of the straightchain alcohols (including methanol to npentanol) by using the C20 fullerene and C18NB nano cage,” Chemical Review and Letters, vol. 1, pp. 82–88, 2018. View at: Google Scholar
 S. A. Siadati and S. Rezazadeh, “Switching behavior of an actuator containing germanium, silicondecorated and normal C20 fullerene,” Chemical Review and Letters, vol. 1, pp. 77–81, 2018. View at: Google Scholar
 J. M. Rabanel, V. Aoun, I. Elkin, M. Mokhtar, and P. Hildgen, “Drugloaded nanocarriers: passive targeting and crossing of biological barriers,” Current Medicinal Chemistry, vol. 19, no. 19, pp. 3070–3102, 2012. View at: Publisher Site  Google Scholar
 K. Zare and N. Shadmani, “Comparison of drug delivery systems: nanotube and p sulphonatocalix[4]arene, by density functional theory,” Journal of Nanostructure in Chemistry, vol. 3, pp. 72–77, 2013. View at: Publisher Site  Google Scholar
 A. R. Harutyunyan, B. K. Pradhan, G. U. Sumanasekera, E. Y. Korobko, and A. A. Kuznetsov, “Carbon nanotubes for medical applications,” European Cells and Materials, vol. 3, pp. 84–87, 2002. View at: Google Scholar
 S. Costa, E. BorowiakPalen, A. Bachmatiuk, M. H. Rümmeli, T. Gemming, and R. J. Kaleńczuk, “Filling of carbon nanotubes for bio‐applications,” Physica Status Solidi (b) – Basic Solid State Physics, vol. 244, no. 11, pp. 4315–4318, 2007. View at: Publisher Site  Google Scholar
 M. Robinson, I. SuarezMartinez, and N. A. Marks, “Generalized method for constructing the atomic coordinates of nanotube caps,” Physical Review B: Condensed Matter and Materials Physics, vol. 87, no. 15, pp. 1–8, 2013. View at: Publisher Site  Google Scholar
 F. Jensen, Introduction to Computational Chemistry, John Wiley & Sons, 2017.
 F. Sen, M. Dincer, A. Cukurovali, and I. Yilmaz, “N[4(3methyl3mesitylcyclobutyl)thiazol2yl]succinamic acid: Xray structure, spectroscopic characterization and quantum chemical computational studies,” Journal of Molecular Structure, vol. 1046, pp. 1–8, 2013. View at: Publisher Site  Google Scholar
 G. W. Ejuh, N. Samuel, T. N. Fridolin, and N. J. Marie, “Computational determination of the electronic and nonlinear optical properties of the molecules 2(4aminophenyl) quinoline, 4(4 aminophenyl) quinoline, anthracene, anthraquinone and phenanthrene,” Materials Letters, vol. 178, pp. 221–226, 2016. View at: Publisher Site  Google Scholar
 Y. J. Dappe, “Encapsulation of organic molecules in carbon nanotubes: role of the van der waals interactions,” Journal of Physics D: Applied Physics, vol. 47, no. 8, pp. 1–16, 2014. View at: Publisher Site  Google Scholar
 T. Vreven, K. S. Byun, I. Komáromi et al., “Combining quantum mechanics methods with molecular mechanics methods in ONIOM,” Journal of Chemical Theory and Computation, vol. 2, no. 3, pp. 815–826, 2006. View at: Publisher Site  Google Scholar
 L. W. Chung, W. M. Sameera, R. Ramozzi et al., “The ONIOM method and its applications,” Chemical Reviews, vol. 115, no. 12, pp. 5678–5796, 2015. View at: Publisher Site  Google Scholar
 G. García, I. Ciofini, M. FernándezGómez, and C. Adamo, “Confinement effects on UV–visible absorption spectra: βcarotene inside carbon nanotube as a test case,” The Journal of Physical Chemistry Letters, vol. 4, no. 8, pp. 1239–1243, 2013. View at: Publisher Site  Google Scholar
 A. Ahmadi, M. Kamfiroozi, J. Beheshtian, and N. L. Hadipour, “The effect of surface curvature of aluminum nitride nanotubes on the adsorption of NH3,” Structural Chemistry, vol. 22, no. 6, pp. 1261–1265, 2011. View at: Publisher Site  Google Scholar
 J. Prasek, J. Drbohlavova, J. Chomoucka et al., “Methods for carbon nanotubes synthesis—review,” Journal of Materials Chemistry, vol. 21, no. 40, pp. 15872–15884, 2011. View at: Publisher Site  Google Scholar
 B. C. Satishkumar, A. Govindaraj, J. Mofokeng, G. N. Subbanna, and C. N. Rao, “Novel experiments with carbon nanotubes: opening, filling, closing and functionalizing nanotubes,” Journal of Physics B: Atomic, Molecular and Optical Physics, vol. 29, no. 21, pp. 4925–4934, 1996. View at: Publisher Site  Google Scholar
 P. M. Ajayan, T. W. Ebbesen, T. Ichihashi, S. Iijima, K. Tanigaki, and H. Hiura, “Opening carbon nanotubes with oxygen and implications for filling,” Nature, vol. 362, no. 6420, pp. 522–525, 1993. View at: Publisher Site  Google Scholar
 M. Yudasaka, K. Ajima, K. Suenaga, T. Ichihashi, A. Hashimoto, and S. Iijima, “Nanoextraction and nanocondensation for C_{60} incorporation into singlewall carbon nanotubes in liquid phases,” Chemical Physics Letters, vol. 380, no. 12, pp. 42–46, 2003. View at: Publisher Site  Google Scholar
 Y. Ren and G. Pastorin, “Incorporation of hexamethylmelamine inside capped carbon nanotubes,” Advanced Materials, vol. 20, no. 11, pp. 2031–2036, 2008. View at: Publisher Site  Google Scholar
 L. Wu, C. Man, H. Wang et al., “PEGylated multiwalled carbon nanotubes for encapsulation and sustained release of oxaliplatin,” Pharmaceutical Research, vol. 30, no. 2, pp. 412–423, 2013. View at: Publisher Site  Google Scholar
 T. A. Hilder and J. M. Hill, “Encapsulation of the anticancer drug cisplatin into nanotubes,” in Proceedings of the International Conference on Nanoscience and Nanotechnology, ICONN '08, pp. 109–112, Australia, 2008. View at: Google Scholar
 M. J. Frisch, G. W. Trucks, H. B. Schlegel et al., Gaussian 09, Revision A.02, Gaussian, Inc., Wallingford, CT, USA, 2009.
 R. Dennington, T. Keith, and J. Millam, GaussView, Version 5, Semichem Inc., Shawnee Mission, Kan, USA, 2009.
 A. V. Marenich, C. J. Cramer, and D. G. Truhlar, “Universal solvation model based on solute electron density and on a continuum model of the solvent defined by the bulk dielectric constant and atomic surface tensions,” The Journal of Physical Chemistry B, vol. 113, no. 18, pp. 6378–6396, 2009. View at: Publisher Site  Google Scholar
 L. X. Wang, C. H. YI, H. T Zou, J. Xu, and W. L. Xu, “cistrans isomerization of azobenzene confined inside an armchair (8, 8) singlewalled carbon nanotube,” Acta PhysicoChimica Sinica, vol. 26, pp. 149–154, 2010. View at: Google Scholar
 L. Wang, C. Yi, H. Zou, J. Xu, and W. Xu, “On the isomerization and dissociation of nitramide encapsulated inside an armchair (5,5) singlewalled carbon nanotube,” Materials Chemistry and Physics, vol. 127, no. 12, pp. 232–238, 2011. View at: Publisher Site  Google Scholar
 S. F. Boys and F. Bernardi, “The calculation of small molecular interactions by the differences of separate total energies. Some procedures with reduced errors,” Molecular Physics, vol. 19, no. 4, pp. 553–566, 1970. View at: Publisher Site  Google Scholar
 R. A. Yossa Kamsi, G. W. Ejuh, F. Tchoffo, P. Mkounga, and J. B. Ndjaka, “Electronic structure, spectroscopic (IR, Raman, UVVis, NMR), optoelectronic, and NLO properties investigations of rubescin E(C31H36O7) molecule in gas phase and chloroform solution using Ab initio and DFT methods,” Advances in Condensed Matter Physics, vol. 2019, Article ID 4246810, 22 pages, 2019. View at: Publisher Site  Google Scholar
 N. M. O'boyle, A. L. Tenderholt, and K. M. Langner, “cclib: a library for packageindependent computational chemistry algorithms,” Journal of Computational Chemistry, vol. 29, no. 5, pp. 839–845, 2008. View at: Publisher Site  Google Scholar
 Y. Tadjouteu Assatse, G. Ejuh, F. Tchoffo, and J. Ndjaka, “DFT studies of nanomaterials designed by the functionalization of modified carboxylated carbon nanotubes with biguanide derivatives for nanomedical, nonlinear and electronic applications,” Chinese Journal of Physics, vol. 58, pp. 253–262, 2019. View at: Publisher Site  Google Scholar
 P. Politzer and J. S. Murray, “The fundamental nature and role of the electrostatic potential in atoms and molecules,” Theoretical Chemistry Accounts, vol. 108, pp. 134–142, 2002. View at: Google Scholar
 B. Trzaskowski and L. Adamowicz, “Chloromethane and dichloromethane decompositions inside nanotubes as models of reactions in confined space,” Theoretical Chemistry Accounts, vol. 124, no. 12, pp. 95–103, 2009. View at: Publisher Site  Google Scholar
 L. Wang, C. Yi, H. Zou, J. Xu, and W. Xu, “Rearrangement and thermal decomposition of nitromethane confined inside an armchair (5,5) singlewalled carbon nanotube,” Chemical Physics, vol. 367, no. 23, pp. 120–126, 2010. View at: Publisher Site  Google Scholar
 B. Mennucci and R. Cammi, Continuum Solvation Models in Chemical Physics: From Theory to Applications, John Wiley & Sons, 2007.
 M. s. Boobalan, D. Tamilvendan, M. Amaladasan, S. Ramalingam, G. Venkatesa Prabhu, and M. Bououdina, “Vibrational spectra and electronic structure of 3((1Hpyrrol1yl) methyl) naphthalen2ol–A computational insight on antioxidant active Mannich base,” Journal of Molecular Structure, vol. 1081, pp. 159–174, 2015. View at: Publisher Site  Google Scholar
 M. Szafran, A. Komasa, and Z. DegaSzafran, “Spectroscopic and theoretical studies of bis(dimethylphenyl betaine) hydrochloride monohydrate,” Vibrational Spectroscopy, vol. 79, pp. 16–23, 2015. View at: Publisher Site  Google Scholar
 B. Champagne, E. A. Perpète, D. Jacquemin et al., “Assessment of conventional density functional schemes for computing the dipole moment and (hyper) polarizabilities of push− pull πconjugated systems,” The Journal of Physical Chemistry A, vol. 104, no. 20, pp. 4755–4763, 2000. View at: Publisher Site  Google Scholar
 R. M. Gester, C. Bistafa, H. C. Georg, K. Coutinho, and S. Canuto, “Theoretically describing the 17O magnetic shielding constant of biomolecular systems: uracil and 5fluorouracil in water environment,” Theoretical Chemistry Accounts, vol. 133, no. 1424, pp. 1–8, 2014. View at: Publisher Site  Google Scholar
 F. D. Vila, D. A. Strubbe, Y. Takimoto et al., “Basis set effects on the hyperpolarizability of CHCl3: Gaussiantype orbitals, numerical basis sets and realspace grids,” The Journal of Chemical Physics, vol. 133, no. 3, pp. 1–23, 2010. View at: Google Scholar
 H. Tanak, ““Molecular structure, spectroscopic (FTIR and UVVis) and DFT quantumchemical studies on 2[(2, 4dimethylphenyl) iminomethyl]6methylphenol,” Molecular Physics, vol. 112, no. 11, pp. 1553–1565, 2014. View at: Publisher Site  Google Scholar
 T. Pieńko, M. Grudzień, P. P. Taciak, and A. P. Mazurek, “Cytisine basicity, solvation, log P, and log D theoretical determination as tool for bioavailability prediction,” Journal of Molecular Graphics and Modelling, vol. 63, pp. 15–21, 2016. View at: Publisher Site  Google Scholar
 A. Zafar and J. Reynisson, “Hydration free energy as a molecular descriptor in drug design: a feasibility study,” Molecular Informatics, vol. 35, no. 5, pp. 207–214, 2016. View at: Publisher Site  Google Scholar
 J. A. Schwöbel, Y. K. Koleva, S. J. Enoch et al., “Measurement and estimation of electrophilic reactivity for predictive toxicology,” Chemical Reviews, vol. 111, no. 4, pp. 2562–2596, 2011. View at: Publisher Site  Google Scholar
 R. Parthasarathi, V. Subramanian, D. R. Roy, and P. K. Chattaraj, “Electrophilicity index as a possible descriptor of biological activity,” Bioorganic & Medicinal Chemistry, vol. 12, no. 21, pp. 5533–5543, 2004. View at: Publisher Site  Google Scholar
 D. R. Roy, R. Parthasarathi, B. Maiti, V. Subramanian, and P. K. Chattaraj, “Electrophilicity as a possible descriptor for toxicity prediction,” Bioorganic & Medicinal Chemistry, vol. 13, no. 10, pp. 3405–3412, 2005. View at: Publisher Site  Google Scholar
Copyright
Copyright © 2019 Y. Tadjouteu Assatse et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.