ISRN Physical Chemistry

Volume 2013 (2013), Article ID 753139, 16 pages

http://dx.doi.org/10.1155/2013/753139

## Stability Analysis and Frontier Orbital Study of Different Glycol and Water Complex

Department of Metallurgical and Materials Engineering, Indian Institute of Technology Kharagpur, Kharagpur, West Bengal 721302, India

Received 20 October 2012; Accepted 7 November 2012

Academic Editors: J. G. Han, T. Kar, and A. M. Koster

Copyright © 2013 Snehanshu Pal and T. K. Kundu. 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.

#### Abstract

A detailed theoretical study of hydrogen-bond formation in different polyethylene glycol + water complex and dipropylene glycol + water have been performed by Hartree Fock (HF) method, second-order Møller-Plesset perturbation theory (MP2), and density functional theory (DFT) using 6-31++G(d,p) basis set. B3LYP DFT-D, WB97XD, M06, and M06-2X functionals have been used to describe highly dispersive hydrogen-bond formation appropriately. Geometrical parameters, interaction energies, deformation energies, deviation of potential energy curves of hydrogen bonded O–H from that of free O–H, frontier orbitals, and charge transfer have been studied to analyze stability and nature of hydrogen bond formation of various glycol and water complexes. It is found that WB97XD is best among all the applied DFT functionals to describe hydrogen bond interaction, and intermolecular hydrogen bonds have higher covalent character and accordingly higher strength when glycol acts as proton donor for glycol + 1 water complex system.

#### 1. Introduction

Polyethylene glycol and its derivatives are applied extensively as drag delivering medium in medical industry [1] and gas hydrate inhibitor in petroleum industry [2, 3]. Experimental study of ethylene glycol molecule and ethylene glycol aqueous solution has been performed using nuclear magnetic resonance (NMR) spectroscopy [4, 5], infrared spectroscopy (IR) [6–9], ultraviolet (UV) spectroscopy [9], Raman Spectroscopy [10], X-ray, and Neutron diffraction techniques [11]. Quantum chemical-based study on different conformers of ethylene glycol has revealed that the gauche form is the most stable conformer in aqueous solution [12, 13]. Hydrogen-bond, an attractive proton donor-acceptor interaction between donor (bonded combination of hydrogen with other electronegative atom) and acceptor (electron-rich region) [14, 15], plays crucial role in determining microscopic and macroscopic behaviour of glycols and water system. Since aqueous solution of glycols are used as gas hydrate inhibitor during drilling practice in petroleum industry, detailed scientific understanding of hydrogen-bond interaction between glycol and water is essential to utilize glycols more efficiently as gas hydrate inhibitor. Quantum chemical calculation is very effective to investigate the hydrogen-bond interaction and its impact on the performance of gas hydrate inhibitors. The effect of microsolvation on ethylene glycol has been studied using density functional theory considering the contribution of many body energies by Chaudhari and Lee [16]. A polymer reference interaction site model theory-based study of polyethylene glycol-water system has been reported by Xu et al. [17]. Theoretical study of hydrogen-bond interaction in ethylene glycol cluster, carried out by Kumar et al., has revealed that the presence of water destroys the intermolecular hydrogen-bonds in ethylene glycol cluster [18]. Quantum chemical analysis of hydrogen-bond interaction in trimethylene glycol-water complex has been performed by Pal and Kundu [19]. Though literature of quantum chemical study of hydrogen-bond formation in different complexes is vast [20–26], quantum chemical study of hydrogen-bond interaction between water and glycols other than ethylene glycol and trimethylene glycol has not been reported so far. Electronic structure-based studies on hydrogen-bond formation between water and glycol having ether functional group (C–O–C) (e.g., diethylene glycol, triethylene glycol and dipropylene glycol) have not been performed till date.

A detail theoretical analysis is reported here to comprehend the electronic nature of the hydrogen-bond formation in various polyethylene glycol-water and dipropylene glycol-water systems, and its property using Hartree Fock, Møller-Plesset is truncated at second-order (MP2), density function theory (DFT), and density functional theory with dispersion function (DFT-D). The detail study of geometrical parameters of optimized structures, interaction energies, deformation energies, relaxation energies, many body energy contributions, charge transfer, potential energy plots, and frontier orbitals reported in this paper should provide electronic structure-based insights on hydrogen-bond formation in glycol-water complex and scientific understanding on application of different glycols as a gas hydrate inhibitors.

#### 2. Computational Detail

Geometry optimization and interaction energy calculation have been carried out using Hartree Fock (HF) [27] method, second-order Møller-Plesset perturbation theory (MP2) [28], density functional theory (DFT) [29, 30], and density functional theory with dispersion function (DFT-D) [31]. The calculations for DFT and DFT-D level of theory have been performed using different functionals, namely, B3LYP [32, 33], WB97XD [34], M06 [35], and M062X [35]. As polarity [36] of molecule has great influence on intermolecular hydrogen bonding, hydrogen-bond-forming orbitals require larger space occupation [37]. Thus diffuse and polarization functions augmented split valence 6-31++G(d,p) basis set that is used for better description of molecular orbitals for geometry optimization. Since hydrogen bonding is a kind of donor-acceptor interaction, additional dispersion function with density functional theory, that is, DFT-D-based calculation, has also been performed. Natural energy decomposition analysis (NEDA) has been performed using WB97XD/6-31++G(d,p) method.

Interaction energy () for hydrogen-bonded complex is calculated as the difference between the energy of hydrogen-bonded complex and the summation of the energies of each component monomer [38] as where and are optimized energy of hydrogen-bonded complex and each individual component monomer, respectively. Interaction energies have corrected for the basis set superposition error (BSSE) by virtue of counterpoise method [39]. A hydrogen-bonded complex is more stable if interaction energy is more negative compared to other hydrogen-bonded configurations. In order to measure the change in conformation of glycol molecules due to presence of water, deformation energy () [40] for a glycol molecule in any cluster/complex is calculated, as the difference of total electronic energies of glycol in its complex and free state is as follows: Hydrogen-bond cooperativity is studied by calculating relaxation energy (), two-body energy (), and three-body energy () using the following [41, 42]: Here, , , and are the energies of the monomer, dimer, and trimer in complex or cluster, and are the energies of glycols, water in free state and is number of component molecule in complex (, one glycol and two water molecules), and is number of water molecule () in complex. Gaussian 09 software package has been used to perform all the calculations reported here [43].

#### 3. Results and Discussion

The optimized structures of ethylene glycol (EG), diethylene glycol (DEG), triethylene glycol (TEG), and dipropylene glycol (DPG) molecule, their dimer, their complex with one and two water molecules have been obtained by HF, MP2, and DFT methods using 6-31++G(d,p) basis set and B3LYP DFT-D, WB97XD, M06, and M06-2X functionals, and the corresponding structures obtained by using WB97XD functional DFT method are shown in Figures 1, 2, 3, and 4, respectively. For present study, two cases like glycol acts as proton donor (referred by GD) and water act as proton donor (referred by WD) are considered for different glycols, and one water complex and their optimized structures are presented in Figure 3. The calculated geometrical parameters using 6-31++G(d,p) basis set and different levels of theory are summarized in Tables 1, 2, 3, and 4. The calculated hydrogen-bond distances obtained using MP2, WB97XD, B3LYP DFT-D, and parameterized functional (M06, M06-2X) based methods are less than hydrogen-bond distances obtained from HF method for all the systems studied here. The calculated hydrogen-bond distance for EG dimer using MP2 and DFT methods corresponds well with experimental value, that is, 1.80 Å [11]. The calculated hydrogen-bonded O–H bond distance and free O–H bond distance for EG dimer using MP2 and DFT methods is equal to 0.97 Å and 0.96 Å, respectively, and is in good agreement with experimental value, that is, 0.96 Å [11]. It is also observed that hydrogen-bond angle values for intermolecular hydrogen bonds in all the glycol + water and their dimer are greater than except for EG + 1 water (WD) complex according to all the calculation methods used. Thus intramolecular hydrogen bonds of these complex are almost linear and strong. Dipole moments of different glycols + water systems along with dimer have been given in Tables 1–4. As hydrogen-bond formation helps in superposition of moment and delocalization of *π* electrons in hydrogen-bonded molecular cluster, the dipole moment is increased by stronger intermolecular hydrogen-bond formation [44]. The dipole moment values are higher and consequently forming stronger intermolecular hydrogen-bond when glycols are acting as proton donor compared to when water is acting as proton donor in different glycols + 1 water complex as evident in Tables 1–4.

Interaction energies for glycols (including dimers) and water systems with and without BSSE correction have been summarized in Tables 5–8. The complex formed by hydrogen bonding with more negative interaction energy should have better stability compared to the hydrogen-bonded complex having less negative interaction energy. Accordingly the stability order for EG and water complex, as observed from Table 5 is water dimer < EG + 1 water complex (GD) < EG + 1 water complex (WD) < EG dimer < EG + 2 water complex from MP2 and WB97XD functional-based calculation. On the other hand the stability order found by B3LYP, B3LYP DFT-D, M06, and M06-2X functional-based calculation is water dimer < EG + 1 water complex (GD) < EG dimer < EG + 1 water complex (WD) < EG + 2 water complex and the stability order obtained by HF theory based calculation as: EG dimer < EG + 1 water complex (WD) < water dimer < EG + 1 water complex (GD) < EG + 2 water complex. The stability order for DEG and water complex as evident from Table 6 is DEG + 1 water complex (GD) < DEG + 1 water complex (WD) < DEG dimer < DEG + 2 water complex as per MP2 method and WB97XD, B3LYP DFT-D, M06, M06-2X, and B3LYP functional-based calculation, differing with the stability order obtained using HF theory, that is, DEG dimer < DEG + 1 water complex (WD) < DEG + 1 water complex (GD) < DEG + 2 water complex. Similarly from Table 7, the observed stability order is TEG + 1 water complex (GD) < TEG + 1 water complex (WD) < TEG + 2 water complex as per MP2 method and WB97XD, B3LYP DFT-D, M06, M06-2X, and B3LYP functional-based calculation, contrasting the stability order determined using HF theory, that is, TEG + 1 water complex (WD) < TEG + 1 water complex (GD) < TEG + 2 water complex. It is also found from Table 8 that the stability order in ascending sense is: DPG + 1 water complex (GD) < DPG + 1 water complex (WD) < DPG + 2 water complex as per MP2 method and WB97XD, B3LYP DFT-D, M06, M06-2X, and B3LYP functional-based calculation, contrasting the stability order determined using HF theory, that is, DPG + 1 water complex (WD) < DPG + 1 water complex (GD) < TEG + 2 water complex. The interaction energies are overestimated by HF theory-based calculation as found in Tables 5–8, because HF theory does not include or consider electron correlation factor. HF theory is found to be inappropriate for describing hydrogen-bond interaction, as results obtained using HF method differ significantly from the results of MP2 method, one of the most reliable ways to describe hydrogen bonding [45, 46]. It can be inferred based on the comparison of different DFT methods with MP2 method with respect to the values of interaction energies and stability trends of hydrogen-bonded complexes that WB97XD is the best among all the applied DFT functionals to describe hydrogen-bond interaction. Stronger hydrogen-bond is formed in glycols + water complex compared to the hydrogen-bond formed in water dimer system according to all the quantum chemical calculation methods applied as evident in Tables 5–8. Relaxation energies and deformation energies for various glycols and water system are summarized in Tables 9, 10, 11, and 12. The positive values of both deformation energy and relaxation energy depict that the molecules or ligands in their complex form become destabilized compared to their free state form. Many body energies for glycols + 2 water complex calculated at WB97XD/6-31++G(d,p) level of theory have been summarized in Table 13. Two-body energy is found to be negative and consequently attractive in nature, whereas three-body energy is found to be positive and consequently repulsive in nature for all the glycols + 2 water system studied. It is found that two-body energy contribution is maximum (compared to relaxation and three-body energy) toward interaction energy, and consequently two-body energy is most significant for the stability of such hydrogen-bonded complexes.

The potential energy curves for a free O–H bond of single DEG, TEG, and DPG molecule are represented in Figures 5(a), 5(c), and 5(e), respectively. The potential energy curves for hydrogen-bonded O–H of DEG + 1 water complex (GD), TEG + 1 water complex (GD), and DPG + 1 water complex (GD) are also shown in Figures 5(b), 5(d), and 5(f), respectively. The broadening in potential energy curve of hydrogen-bonded O–H reveals that a strong intermolecular hydrogen-bond is formed in DEG + 1 water complex (GD), TEG + 1 water complex (GD), and DPG + 1 water complex (GD) complexes [47]. The broadening width of potential energy curve due to hydrogen bonding is highest for DEG + 1 water complex (GD), and consequently the hydrogen-bond between DEG and water is the strongest compared to other complexes (Figure 5). Appearance of prominent asymmetrical double minimum and high energy barrier in potential energy curve of hydrogen-bonded O–H for trimethylene glycol (TMG) + 1 water complex (TMG as proton donor) has been reported earlier [19]. These attributes (asymmetrical double minimum and high energy barrier) in the potential energy curves for hydrogen-bonded O–H of DEG + 1 water complex (GD), TEG + 1 water complex (GD), and DPG + 1 water complex (GD) are not present. This depicts that glycols having ether group (DEG, TEG, and DPG) have stronger hydrogen-bond interaction with water molecule compared to glycols without ether group (TMG).

Highest occupied molecular orbital (HOMO) and lowest unoccupied molecular orbital (LUMO) of different glycol molecules and glycols + 1 water systems (both GD and WD complex), simulated by WB97XD/6-31++G(d,p) method, have been shown in Figure 6. The LUMO energies of different glycol + 1 water complexes are less compared to that of respective single glycol and water molecule. The LUMO of glycol + 1 water complex (GD) originates essentially from the LUMO of water with negligible contribution of antibonding orbital of respective glycol, but the HOMO of the same complex arises largely from the HOMO of respective glycol. On the other hand, for glycol + 1 water complex (WD), LUMO evolves mainly from the LUMO of the respective glycol, and HOMO is from the intermixing of lone pairs of both the respective glycol and water molecules. It is seen from frontier orbital analysis that the intermolecular hydrogen-bond of glycol + 1 water complex (GD) has more covalent characters compared to the intermolecular hydrogen-bond of glycol + 1 water complex (WD).

The charge transfer (CT) energies calculated using natural energy decomposition analysis (NEDA) for different glycol + 1 water complex and glycol dimer are summarized in Table 14. Charge transfer (CT) is a part of the interaction energy of molecular cluster, representing electron delocalization interaction between occupied molecular orbital of one molecule and unoccupied molecular orbital of another molecule, and it helps to elucidate intermolecular interaction like hydrogen bonding or electron donor-acceptor interaction [48–50]. The charge transfer value of EG dimer is found to be much lower than the charge transfer values of both type of EG + 1 water complexes. Similarly, the charge transfer value for DEG dimer is also much lower than the charge transfer values of both type DEG + 1 water complexes. But the charge transfer values for DPG dimer and TEG dimer are higher (less negative) than the charge transfer values of DPG + 1 water complex (WD) and TEG + 1 water complex (WD), respectively, as evident in Table 14. According to the charge transfer values, DPG and TEG molecules form stronger intermolecular hydrogen-bond with water molecule when water acts as a proton donor, compared to the hydrogen-bond of their dimer complex where EG and DEG molecules form weaker intermolecular hydrogen-bond with water molecule compared to the hydrogen-bond of their dimer complex. It is advisable to use both of EG and DEG solution for inhibiting water cluster formation at low concentration, such that possibilities of their dimer formation would become very less.

#### 4. Conclusion

A thorough analysis of hydrogen-bond formation in polyethylene glycol + water complex () and dipropylene glycol + water complex () has been performed based on interaction energies, relaxation energies, deformation energies, potential energy curve for hydrogen-bonded O–H, frontier orbitals, structural parameters of optimized geometry, and charge transfer. Different polyethylene glycol + 2 water complexes are found to be most stable compared to polyethylene glycol + 1 water complexes, polyethylene dimer and water dimer as per calculated interaction energies. DPG + 2 water complex is also found to be most stable compared to DPG + 1 water complexes, DPG dimer and water dimer as per calculated interaction energies. The broadening of potential energy curve of hydrogen-bonded O–H reveal that the intermolecular hydrogen-bond formed between different glycol and water is strong. Intermolecular hydrogen bonds for different glycol + 1 water complex (glycol as proton donor) has higher covalent character and accordingly higher strength compared to that of glycol + 1 water complex (water as proton donor) according to frontier orbital analysis. WB97XD functional-based DFT is found to provide similar stability trends of hydrogen-bonded complexes as that of MP2 method. Theoretical analysis of hydrogen-bond formation in different glycols and water complexes applying natural bond orbital analysis, bond order, and frequency calculation-based study would be of great help, and the same would be our future endeavour. The elucidation of electronic structure property correlation-based study of different glycol in aqueous solution carried out in this paper can significantly help in designing inhibitors for water cluster/clathrate system like methane hydrate.

#### Acknowledgments

This work is financially supported by Ministry of Earth Science, India (Project no. MoES/16/48/09—RDEAS (MRDM5)). The authors also acknowledge accelrys Inc. for providing free Discovery Studio 3.1 visualization tool.

#### References

- S. S. Banerjee, N. Aher, R. Patil, and J. Khandare, “Poly (ethylene glycol)-prodrugconjugates: concept, design, and applications,”
*Journal of Drug Delivery*, vol. 2012, Article ID 103973, 17 pages, 2012. View at Google Scholar - W. S. Halliday, D. K. Clapper, M. R. Smalling, and R. G. Bland, “Blends of Glycol derivatives as gas hydrate inhibitors in water base drilling, drill-in, and completion fluids,”
*US Patent*US006165945A, 2000. View at Google Scholar - G. Jiang, T. Liu, F. Ning et al., “Polyethylene glycol drilling fluid for drilling in marine gas hydrates-bearing sediments: an experimental study,”
*Energies*, vol. 4, no. 1, pp. 140–150, 2011. View at Publisher · View at Google Scholar · View at Scopus - K. J. Liu and J. L. Parsons, “Solvent effects on the preferred conformation of poly(ethylene glycols),”
*Macromolecules*, vol. 2, no. 5, pp. 529–533, 1969. View at Google Scholar · View at Scopus - S. Lüsse and K. Arnold, “The interaction of poly(ethylene glycol) with water studied by 1H and 2H NMR relaxation time measurements,”
*Macromolecules*, vol. 29, no. 12, pp. 4251–4257, 1996. View at Google Scholar · View at Scopus - M. W. A. Skoda, R. M. J. Jacobs, J. Willis, and F. Schreiber, “Hydration of oligo(ethylene glycol) self-assembled monolayers studied using polarization modulation infrared spectroscopy,”
*Langmuir*, vol. 23, no. 3, pp. 970–974, 2007. View at Publisher · View at Google Scholar · View at Scopus - P. Buckley and P. A. Giguere, “Infrared studies on rotational isomerism. I. ethylene glycol,”
*Canadian Journal of Chemistry*, vol. 45, 1967. View at Google Scholar - E. L. Hommel, J. K. Merle, G. Ma, C. M. Hadad, and H. C. Allen, “Spectroscopic and computational studies of aqueous ethylene glycol solution surfaces,”
*Journal of Physical Chemistry B*, vol. 109, no. 2, pp. 811–818, 2005. View at Publisher · View at Google Scholar · View at Scopus - Z. JianBin, Z. PengYan, M. Kai, H. Fang, C. GuaHua, and W. XiongHui, “Hydrogen bonding interactions between ethylene glycol and water: density, excess molar volume, and Spectral Study,”
*Science in China B*, vol. 51, no. 5, pp. 420–426, 2008. View at Google Scholar - C. Murli, N. Lu, Z. Dong, and Y. Song, “Hydrogen bonds and conformations in ethylene glycol under pressure,”
*The Journal of Physical Chemistry B*, vol. 116, no. 41, Article ID 306220, pp. 12574–12580, 2012. View at Google Scholar - I. Bakó, T. Grósz, G. Pálinkás, and M. C. Bellissent-Funel, “Ethylene glycol dimers in the liquid phase: a study by x-ray and neutron diffraction,”
*Journal of Chemical Physics*, vol. 118, no. 7, pp. 3215–3221, 2003. View at Publisher · View at Google Scholar · View at Scopus - M. A. Murcko and R. A. DiPaola, “Ab initio molecular orbital conformational analysis of prototypical organic systems. 1. Ethylene glycol and 1,2-dimethoxyethane,”
*Journal of the American Chemical Society*, vol. 114, no. 25, pp. 10010–10018, 1992. View at Google Scholar · View at Scopus - C. J. Cramer and D. G. Truhlar, “Quantum chemical conformational analysis of 1,2-Ethanediol: correlation and solvation effects on the tendency to form internal hydrogen bonds in the gas phase and in aqueous solution,”
*Journal of the American Chemical Society*, vol. 116, no. 9, pp. 3892–3900, 1994. View at Google Scholar · View at Scopus - G. R. Desiraju, “A bond by any other name,”
*Angewandte Chemie*, vol. 50, no. 1, pp. 52–59, 2011. View at Publisher · View at Google Scholar · View at Scopus - S. J. Graowski,
*Hydrogen Bonding—NewInsights*, Springer, Amsterdam, The Netherlands, 2006. - A. Chaudhari and S. L. Lee, “A computational study of microsolvation effect on ethylene glycol by density functional method,”
*Journal of Chemical Physics*, vol. 120, no. 16, pp. 7464–7469, 2004. View at Publisher · View at Google Scholar · View at Scopus - Q. Xu, J. Mi, and C. Zhong, “Structure of poly(ethylene glycol)—water mixture studied by polymer reference interaction site model theory,”
*Journal of Chemical Physics*, vol. 133, no. 17, Article ID 174104, 2010. View at Publisher · View at Google Scholar · View at Scopus - R. M. Kumar, P. Baskar, K. Balamurugan, S. Das, and V. Subramanian, “On the perturbation of the H-bonding interaction in ethylene glycol clusters upon hydration,”
*Journal of Physical Chemistry A*, vol. 116, pp. 4239–4247, 2012. View at Google Scholar - S. Pal and T. K. Kundu, “Theoretical study of hydrogen bond formation in trimethylene glycol-water complex,”
*ISRN Physical Chemistry*, vol. 2012, Article ID 570394, pp. 1–12, 2012. View at Publisher · View at Google Scholar - A. Mandal, M. Prakash, R. M. Kumar, R. Parthasarathi, and V. Subramanian, “Ab Initio and DFT studies on methanol-water clusters,”
*Journal of Physical Chemistry A*, vol. 114, no. 6, pp. 2250–2258, 2010. View at Publisher · View at Google Scholar · View at Scopus - O. V. Shishkin, I. S. Konovalova, L. Gorb, and J. Leszczynski, “Novel type of mixed O-H
*⋯*N/O-H*⋯**π*hydrogen bonds: monohydrate of pyridine,”*Structural Chemistry*, vol. 20, no. 1, pp. 37–41, 2009. View at Publisher · View at Google Scholar · View at Scopus - P. K. Sahu and S. L. Lee, “Hydrogen-bond interaction in 1:1 complexes of tetrahydrofuran with water, hydrogen fluoride, and ammonia: a theoretical study,”
*Journal of Chemical Physics*, vol. 123, no. 4, Article ID 044308, 2005. View at Publisher · View at Google Scholar · View at Scopus - P. K. Sahu, A. Chaudhari, and S. L. Lee, “Theoretical investigation for the hydrogen bond interaction in THF—water complex,”
*Chemical Physics Letters*, vol. 386, no. 4–6, pp. 351–355, 2004. View at Publisher · View at Google Scholar · View at Scopus - X. M. Zhou, Z. Y. Zhou, H. Fu, Y. Shi, and H. Zhang, “Density functional complete study of hydrogen bonding between the dichlorine monoxide and the hydroxyl radical (Cl2O
*·*HO),”*Journal of Molecular Structure*, vol. 714, no. 1, pp. 7–12, 2005. View at Publisher · View at Google Scholar · View at Scopus - D. Peeters, “Hydrogen bonds in small water clusters: a theoretical point of view,”
*Journal of Molecular Liquids*, vol. 67, pp. 49–61, 1995. View at Google Scholar · View at Scopus - S. J. Grabowski, “What is the covalency of hydrogen bonding?”
*Chemical Reviews*, vol. 111, no. 4, pp. 2597–2625, 2011. View at Publisher · View at Google Scholar · View at Scopus - C. C. J. Roothaan, “New developments in molecular orbital theory,”
*Reviews of Modern Physics*, vol. 23, no. 2, pp. 69–89, 1951. View at Publisher · View at Google Scholar · View at Scopus - M. Head-Gordon, J. A. Pople, and M. J. Frisch, “MP2 energy evaluation by direct methods,”
*Chemical Physics Letters*, vol. 153, no. 6, pp. 503–506, 1988. View at Google Scholar · View at Scopus - P. Hohenberg and W. Kohn, “Inhomogeneous electron gas,”
*Physical Review*, vol. 136, no. 3, pp. B864–B871, 1964. View at Publisher · View at Google Scholar · View at Scopus - W. Kohn and L. J. Sham, “Self-consistent equations including exchange and correlation effects,”
*Physical Review*, vol. 140, no. 4, pp. A1133–A1138, 1965. View at Publisher · View at Google Scholar · View at Scopus - S. Grimme, “Accurate description of van der Waals complexes by density functional theory including empirical corrections,”
*Journal of Computational Chemistry*, vol. 25, no. 12, pp. 1463–1473, 2004. View at Publisher · View at Google Scholar · View at Scopus - A. D. Becke, “Density-functional exchange-energy approximation with correct asymptotic behavior,”
*Physical Review A*, vol. 38, no. 6, pp. 3098–3100, 1988. View at Publisher · View at Google Scholar · View at Scopus - C. Lee, W. Yang, and R. G. Parr, “Development of the Colle-Salvetti correlation-energy formula into a functional of the electron density,”
*Physical Review B*, vol. 37, no. 2, pp. 785–789, 1988. View at Publisher · View at Google Scholar · View at Scopus - J. D. Chai and M. Head-Gordon, “Long-range corrected hybrid density functionals with damped atom-atom dispersion corrections,”
*Physical Chemistry Chemical Physics*, vol. 10, no. 44, pp. 6615–6620, 2008. View at Publisher · View at Google Scholar · View at Scopus - Y. Zhao and D. G. Truhlar, “The M06 suite of density functionals for main group thermochemistry, thermochemical kinetics, noncovalent interactions, excited states, and transition elements: two new functionals and systematic testing of four M06-class functionals and 12 other functionals,”
*Theoretical Chemistry Accounts*, vol. 120, no. 1–3, pp. 215–241, 2008. View at Publisher · View at Google Scholar · View at Scopus - P. C. Hariharan and J. A. Pople, “The influence of polarization functions on molecular orbital hydrogenation energies,”
*Theoretica Chimica Acta*, vol. 28, no. 3, pp. 213–222, 1973. View at Publisher · View at Google Scholar · View at Scopus - J. Chandrasekhar, J. G. Andrade, and P. Von Ragué Schleyer, “Efficient and accurate calculation of anion proton affinities,”
*Journal of the American Chemical Society*, vol. 103, no. 18, pp. 5609–5612, 1981. View at Google Scholar · View at Scopus - M. S. Gordon and J. H. Jensen, “Understanding the hydrogen bond using quantum chemistry,”
*Accounts of Chemical Research*, vol. 29, no. 11, pp. 536–543, 1996. View at Google Scholar · View at Scopus - S. F. Boys, “Calculation of small molecular interactions by the differences of separate total energies. Some procedures with reduced errors,”
*Molecular Physics*, vol. 19, no. 4, 1970. View at Google Scholar - C. H. S. Wong, F. M. Siu, N. L. Ma, and C. W. Tsang, “A theoretical study of potassium cation-glycine (K+-Gly) interactions,”
*Journal of Molecular Structure*, vol. 588, pp. 9–16, 2002. View at Publisher · View at Google Scholar · View at Scopus - D. W. Boo, “Ab initio calculations of protonated ethylenediamine-(water)3 complex: roles of intramolecular hydrogen bonding and hydrogen bond cooperativity,”
*Bulletin of the Korean Chemical Society*, vol. 22, no. 7, pp. 693–698, 2001. View at Google Scholar · View at Scopus - S. S. Xantheas, “Ab initio studies of cyclic water clusters (H
_{2}O)_{n}, $n=1-6$. II. Analysis of many-body interactions,”*The Journal of Chemical Physics*, vol. 100, no. 10, pp. 7523–7534, 1994. View at Google Scholar · View at Scopus - M. J. Frisch, G. W. Trucks, H. B. Schlegel et al., Gaussian, Wallingford CT, Gaussian 09, Revision B. 01.
- A. E. Lutskii and N. I. Gorokhova, “Intramolecular hydrogen bonds and molecular dipole moments,”
*Theoretical and Experimental Chemistry*, vol. 4, no. 6, pp. 532–534, 1968. View at Publisher · View at Google Scholar · View at Scopus - P. Hobza and R. Zahradník, “Intermolecular interactions between medium-sized systems. Nonempirical and empirical calculations of interaction energies: successes and failures,”
*Chemical Reviews*, vol. 88, no. 6, pp. 871–897, 1988. View at Google Scholar · View at Scopus - K. E. Riley, M. Pitončák, P. Jurecčka, and P. Hobza, “Stabilization and structure calculations for noncovalent interactions in extended molecular systems based on wave function and density functional theories,”
*Chemical Reviews*, vol. 110, no. 9, pp. 5023–5063, 2010. View at Publisher · View at Google Scholar · View at Scopus - G. A. Jeffrey,
*An Introduction to Hydrogen Bonding*, Oxford University Press, New York, NY, USA, 1997. - H. Umeyama and K. Morokuma, “Origin of alkyl substituent effect in the proton affinity of amines, alcohols, and ethers,”
*Journal of the American Chemical Society*, vol. 98, no. 15, pp. 4400–4404, 1976. View at Google Scholar · View at Scopus - H. Umeyama and K. Morokuma, “The origin of hydrogen bonding. An energy decomposition study,”
*Journal of the American Chemical Society*, vol. 99, no. 5, pp. 1316–1332, 1977. View at Google Scholar · View at Scopus - A. van der Vaart and K. M. Merz Jr., “Charge transfer in small hydrogen bonded clusters,”
*Journal of Chemical Physics*, vol. 116, no. 17, pp. 7380–7388, 2002. View at Publisher · View at Google Scholar · View at Scopus