SciELO - Scientific Electronic Library Online

 
vol.59 número4DEVELOPMENT AND VALIDATION OF A REVERSED-PHASE HPLC METHOD FOR THE SIMULTANEOUS ESTIMATION OF DICYCLOMINE HYDROCHLORIDE AND FAMOTIDINE IN BULK AND TABLETSSYNTHESIS OF TRI-ARM STAR SHAPED 1, 3, 5-TRIAZINES CATALYZED BY 1,5,7-TRIAZABICYCLO[4.4.0] DEC-5-ENE (TBD) índice de autoresíndice de assuntospesquisa de artigos
Home Pagelista alfabética de periódicos  

Serviços Personalizados

Journal

Artigo

Indicadores

Links relacionados

  • Em processo de indexaçãoCitado por Google
  • Não possue artigos similaresSimilares em SciELO
  • Em processo de indexaçãoSimilares em Google

Compartilhar


Journal of the Chilean Chemical Society

versão On-line ISSN 0717-9707

J. Chil. Chem. Soc. vol.59 no.4 Concepción dez. 2014

http://dx.doi.org/10.4067/S0717-97072014000400008 

 

A DENSITY FUNCTIONAL THEORY STUDY ON STRUCTURE AND PROPERTIES OF BENZENE AND BORAZINE-BASED CHROMOPHORES

 

REZA GHIASI*, SARA AKBARI

Department of Chemistry, East Tehran Branch, Qiam Dasht, Tehran, Islamic Azad University, IRAN
* e-mail: rezaghiasi1353@yahoo.com


ABSTRACT

Density functional theory (DFT) calculations were employed to investigate the structural characteristics, electronic properties, and nonlinear optical properties of borazine-based chromophores at B3LYP/ 6-311G(d,p) level. We studied the effects of various donor and acceptor substituents (H, F, Cl, Br, Me, NH2, OH, COOH, CHO, CN, NO2) on the stability, dipole moment, polarizability, frontier orbitals, structure, the most intense electronic transition, and hyperpolarizabilities. These calculations indicate B-isomer is more stable than N-isomer. On the other hand, the most stable isomer confirms the minimum polarizability and maximum hardness principles in the most molecules. Also, we obtained good linear relations between some of the studied properties. The predicted first hyperpolarizability also shows that the substituted molecules might have a reasonably good nonlinear optical (NLO) behavior.

Keywords: Borazine-Based Chromophores, Subsituent effect, Frontier orbitals analysis, Nonlinear optics.


 

INTRODUCTION

There is growing attention in materials with high non-linear optical (NLO) properties due to their potential application in technologies such as lasers, telecommunications, photovoltaic cells, organic light emitting diodes, and semiconductor layers in field-effect transistors [1] information processing and holography. Organic π-conjugated oligomers and polymers represent an excellent alternative to traditional inorganic NLO crystals because they can be easily synthesized and chemically modified. Extremely fast switching times, resistance to high intensity radiation, possibility of thin-layer fabrication, and low electric permittivity (related to low-frequency dependence in nonresonant regime) are important properties in favor of organic NLO materials. A variety of inorganic, organic, and organometallic molecular systems have been studied for NLO activity [2-10].

We report here on a systematic computational investigation of the NLO properties of borazine-based chromophores. The main purpose here is to assess the use of borazine moieties for the design of molecular NLO chromophores and to obtain insight into the structure-function relationships of these systems.

Computational Methods

All calculations were carried out with the Gaussian 03 suite of program [11]. All molecules were described by the standard 6-31G(d,p) basis set [12-15]. Geometry optimization was performed using Beckes hybrid three-parameter exchange functional and the nonlocal correlation functional of Lee, Yang, and Parr (B3LYP) [16]. A vibrational analysis was performed at each stationary point which corresponds to an energy minimum.

Geometries were optimized at this level of theory without any symmetry constraints followed by the calculations of the first order hyperpolarizabilities. The total static first hyperpolarizability β was obtained from the relation:

upon calculating the individual static components

Due to the Kleinman symmetry [17]:

one finally obtains the equation that has been employed:

The electronic spectra for the studied compounds were calculated by TD-DFT [18] using the same hybrid functionals and basis sets as used for the calculation of the hyperpolarizabilities. The 10 lowest excitation energies were computed.

RESULTS AND DISCUSSION

1. Energetic aspects

Figure 1 shows benzene and borazine-Based chromophores investigated in this paper. Table 1 presents the computed energies, relative energies, for all molecules. The relative energies show that B-isomer is more stable than N-isomer in all species. We believe the added stability of the B- isomer systems is due to the degree of polarization of the B-C bond is greater than the N-F bond. For example, in B-isomer (X=H) the charges on B1 and C2' are +0.920e and -0.480e respectively. In N-isomer, the charges on N1 and C2' are -0.888e and +0.064 (Table 1). There is a good linear relation between the relative energies values and along with their Hammett constants (σP) [19]. (Figure2).

 

Figure 1. Resonance forms of Borazine-based chromophores with various
X-groups. For acceptors, the zwitterionic form has the opposite charge
separation.

 

Table1. Absolute energy (Hartree), relative energy (kcal/mol), Hammet constant (σp),
dipole moment (μ, Debye) and NBO Charges of C2', N1, and B1 atoms of borazine-based
chromophores with various X-groups.

 

Figure 2. Relative energy (=EN-isomer-EB-isomer) versus Hammett
constants (σp)

 

2. Dipole moment

The dipole moment values have been gathered in Table 1. These values present N-isomer has a larger dipole moment rather than B-isomer. A good correlation between μ and Hammett constants (σp) has been shown. See Figure 3. As a consequence, dipole moment values also increases with an increase in the accepting strength of the X-group.

 

Figure 3. Dipole moment (μ) versus σp Hammett constants (σp).

 

3. Polarizability

Polarizabilities describe the response of a system in an applied electric field [20]. They determine not only the strength of molecular interactions (such as the long range intermolecular induction, dispersion forces, etc.) as well as the cross sections of different scattering and collision processes, but also the nonlinear optical properties of the system [21].

The isotropic polarizability <α> is calculated as the mean value as given in the following equation:

And the polarizability anisotropy invariant is:

The calculated isotropic and anisotropic polarizability values indicate these values decrease in the stable complexes, as expected from the principles of minimum energy and minimum polarizability in most cases (expect, X=NH2, OH; Table 2) [22]. On the other hand, there is a good correlation between isotropic and anisotropic polarizability values with relative energy values (Figure 4).

 

Table 2. Isotropic polarizability <α> and anisotropy polarizability
α) of borazine-based chromophores with various X-groups.

N-isomer


B-isomer

 

Figure 4. α(iso)N-isomer-α(iso)B-isomer and α(aniso)N-isomer-α
(aniso)B-isomer values versus relative energy.

 

4. Frontier orbital analysis

A particularly interesting property for these molecules is the energy gap (Eg) between the highest occupied molecular orbital (HOMO) and the lowest unoccupied molecular orbital (LUMO). The energy gap is considered as a reflection of the molecule's chemical activity. The frontier orbital energies values have been gathered in Table 3. These values display HOMO and LUMO energy values decrease in substituted molecules, except X=Me, NH2, OH. Also, these values decrease in more stable isomer. Figure 5 presents linear correlation between frontier orbital energies and hammet constant values. A good correlation found suggests that the electron withdrawing/donating groups influences the E(HOMO), and this correlation may be used as a tool to predict E(HOMO) for other substituents for which σp is known. The same correlation is observed for E(LUMO) energies.

 

Table 3. Frontier orbital energies (Hartree), HOMO-LUMO gap energy (eV),
hardness (eV), and chemical potential (eV) for Borazine-Based Chromophores
with Various X-Groups.

N-isomer



B-isomer

 

Figure 5. Frontier orbital values versus relative energy.

 

Table 3 exhibits the HOMO-LUMO gaps of all structures. These values indicate substitution causes decreasing of energy gaps. On the other hand, the calculated the HOMO-LUMO gaps values indicate these values increase in the stable isomer, as expected from the principles of minimum energy and maximum hardness in most cases (expect, X=NH2, OH; Table 3). There is a good correlation between relative hardness values with constant values (Figure 6).

 

Figure 6. (a)Hardness (except for Me, NH2, OH) and (b)
chemicalpotential values versus hammet constant.

 

To evaluate the chemical potential (μ) of these complexes, these values can be calculated from the HOMO and LUMO orbital energies using the following approximate expression [23-29]:

The chemical potential characterizes the tendency of electrons to escape from the equilibrium system. As expected, more stable isomer has less chemical potential.

To evaluate the electrophilicity of these complexes, we have calculated the electrophilicity index,to, using the expression:

The values of electrophilicity index in Table 3 indicate more stable isomer has the largest electrophility.

5. Structural analysis

The optimized geometries of borazine-based chromophores studied in work with atom labeling are depicted in Figure 1. All studied molecules are essentially nonplanar. Table 4 shows the B3LYP/6-311G(d,p) selected structural data for the optimized structures with various X-groups.

 

Table 4. Optimized Bond lengths (Å) of Borazine-Based Chromophores with Various X-Groups.

N-isomer



B-isomer

 

These values indicate bonds C1C2, C3C4, and C5C6 are longer, while bonds B1N2 and B3N3 are shorter. These changes in the bond lengths indicate a larger contribution of the zwitterionic (nonaromatic) resonance structure to the ground state of these derivatives.

6. Electronic spectra

We found the most intense electronic transition (λmax) of molecules. The wavelength, oscillator strength and the composition of the transitions obtained by TD-DFT calculations are given in Table 5. The most intense electronic transition for all molecules is attributed to HOMO®LUMO transition. The λmax is a function of substituent, the stronger the donor character of substituent, the more electron push into the molecule, the less λmax. These calculations illustrate the decreasing of λmax in B-isomer, which is compatible with larger HOMO-LUMO gap in this isomer. There is a good correlation between HOMO-LUMO gap and λmax (Figure 7).

 

Table 5. Maximum Absorption wavelength (λmax), Oscillator strength (f), and its
character for borazine-based chromophores with various X-groups.

 

Figure 7. HOMO-LUMO gap versus λmax.

 

7. Hyperpolarizability

The first static hyperpolarizability (βtot) values for the all molecules are shown in Table 6. The results show that the magnitude of the first hyperpolarizability tensor of all molecules is rather moderate, and NO2 and NH2 substations have the most value in N- and B-isomers, respectively. Also, these values indicate the first hyperpolarizability values of N-isomer are more than B-isomer with withdrawing substitutions. On the other hand, these values of N-isomer are less than B-isomer with donor substitutions.

 

Table 6. β components and βtot values (10-30 esu) for Borazine-Based Chromophores with
Various X-Groups.

N-isomer

B-isomer

 

This chromophore exhibits larger non-linearity and its λmax is red-shifted in B-isomers (except β in X=Me, CN) and N-isomers when compared with unsubstituted molecule. Therefore, it is clear that the hyperpolarizability is a strong function of the absorption maximum. Since even a small absorption at the operating wavelength of optic devices can be detrimental, it is important to make NLO chromophores as transparent as possible without compromising the molecule's non-linearity.

A good correlation has been shown between βtot and λmax in N-isomer for all substituents (Figure 8). But, there is similar correlation in B-isomer for donor substituents and withdrawing substituents.

 

Figure 8. The first static hyperpolarizability (βtot) versus λmax.

 

CONCLUSION

The study of electronic, structural and spectroscopic properties as well as the static first hyperpolarizabilities of the borazine-based chromophores indicated stability of B-isomer species is more than N-isomer. The decreasing of isotropic and anisotropic polarizability values and increasing of HOMO-LUMO gaps values in the stable complexes is compatible with the principles of minimum energy and minimum polarizability in most cases (expect, X=NH2, OH). Calculations showed that the most intense electronic transition is due to HOMO→LUMO transition in all molecules. Theoretical studies indicated acceptor substitutions causes to increasing the first hyperpolarizability values in N-isomer rather than B-isomer, whist, these values of N-isomer are less than B-isomer with donor substitutions.

 

REFERENCES

1. C.D. Dimitrakopolous, P. Malenfant, Adv. Mater. 14, 29, (2002).         [ Links ]

2. D.R. Kanis, M.A. Ratner, T.J. Marks, Chem. Rev 94, 195, (1994).         [ Links ]

3. P.J. Mendes, T.J.L. Silva, A.J.P. Carvalho, J.P.P. Ramalho, Journal of Molecular Structure: THEOCHEM 946, 33.         [ Links ]

4. D. Avci, A. Basoglu, Y. Atalay, Struct Chem 21, 213, (2010).         [ Links ]

5. M. Medved, S. Budzák, I. Cernusák, Journal of Molecular Structure: THEOCHEM 961, 66, (2010).         [ Links ]

6. W. Bartkowiak, K. Strasburger, Journal of Molecular Structure: THEOCHEM 960, 93, (2010).         [ Links ]

7. L.A.D. Souza, A.M.D.S. Jr., G.M.A. Junqueira, A.C.M. Carvalho, H.F.D. Santos, Journal of Molecular Structure: THEOCHEM 959, 92, (2010).         [ Links ]

8. A. Karton, M.A. Iron, M.E.v.d. Boom, J.M.L. Martin, J. Phys. Chem. A 109, 5454, (2005).         [ Links ]

9. P.C. Ray, Chemical Physics Letters 354, (2004).         [ Links ]

10. A. Hameed, A. Rybarczyk-Pirek, J. Zakrzewski, Journal of Organometallic Chemistry 656, 102, (2002).         [ Links ]

11. M.J. Frisch, G.W. Trucks, H.B. Schlegel, G.E. Scuseria, M.A. Robb, J.R. Cheeseman, J.A. Montgomery, Jr., T. Vreven, K.N. Kudin, J.C. Burant, J.M. Millam, S.S. Iyengar, J. Tomasi, V. Barone, B. Mennucci, M. Cossi, G. Scalmani, N. Rega, G.A. Petersson, H. Nakatsuji, M. Hada, M. Ehara, K. Toyota, R. Fukuda, J. Hasegawa, M. Ishida, T. Nakajima, Y. Honda, O. Kitao, H. Nakai, M. Klene, X. Li, J.E. Knox, H.P. Hratchian, J.B. Cross, C. Adamo, J. Jaramillo, R. Gomperts, R.E. Stratmann, O. Yazyev, A.J. Austin, R. Cammi, C. Pomelli, J.W. Ochterski, P.Y. Ayala, K. Morokuma, G.A. Voth, P. Salvador, J.J. Dannenberg, V.G. Zakrzewski, S. Dapprich, A.D. Daniels, M.C. Strain, O. Farkas, D.K. Malick, A.D. Rabuck, K. Raghavachari, J.B. Foresman, J.V. Ortiz, Q. Cui, A.G. Baboul, S. Clifford, J. Cioslowski, B.B. Stefanov, G. Liu, A. Liashenko, P. Piskorz, I. Komaromi, R.L. Martin, D.J. Fox, T. Keith, M.A. Al-Laham, C.Y. Peng, A. Nanayakkara, M. Challacombe, P.M.W. Gill, B. Johnson, W. Chen, M.W. Wong, C. Gonzalez, J.A. Pople, Gaussian 03, Gaussian, Inc., Pittsburgh PA, 2003.         [ Links ]

12. M.J.S. Dewar, C.H. Reynolds, J. Comp. Chem. 2, 140, (1986).         [ Links ]

13. K. Raghavachari, J.A. Pople, E.S. Replogle, M. Head-Gordon, J. Phys. Chem. A 94, 5579, (1990).         [ Links ]

14. A.D. McLean, G.S. Chandler, J. Chem. Phys. 72, 5639, (1980).         [ Links ]

15. R. Krishnan, J.S. Binkley, R. Seeger, J.A. Pople, J. Chem. Phys. 72, 650, (1980).         [ Links ]

16. A.D. Becke, J. Chem. Phys 98, 5648, (1993).         [ Links ]

17. D.A. Keleiman, Phy. Rev. 126, 1977, (1962).         [ Links ]

18. E. Runge, E.K.U. Gross, Phys. Rev. Lett. 52, 997, (1984).         [ Links ]

19. C. Hansch, A. Leo, R.W. Taft, Chem. Rev. 97, 165, (1991).         [ Links ]

20. C.R. Zhang, H.S. Chen, G.H. Wang, Chem. Res. Chinese 20, 640, (2004).         [ Links ]

21. H. Cheng, J. Feng, A. Ren, J. Liu, Acta Chim. Sin. 60, 830, (2002).         [ Links ]

22. D.R. Roy, P.K.r. Chattaraj, J. Phys. Chem. A 112, 1612, (2008).         [ Links ]

23. P. Geerlings, F.D. Proft, W. Langenaeker, Chem. Rev. 103, 1793, (2003).         [ Links ]

24. H. Chermette, J. Comput. Chem. 20, 129, (1999).         [ Links ]

25. C.-G. Zhan, J.A. Nichols, D.A.J. Dixon, J. Phys. Chem. A 107, 4184, (2006).         [ Links ]

26. R.G. Parr, Z. Zhou, Acc. Chem. Res. 26, 256, (1993).         [ Links ]

27. L.G. Arnaut, S.J. Formosinho, Chem. Eur. J. 14, 6578, (2008).         [ Links ]

28. R.G. Pearson, J. Chem. Educ. 64, 561, (1987).         [ Links ]

29. R.G. Parr, P.K. Chattaraj, J. Am. Chem. Soc. 113, 1854, (1991).         [ Links ]

 

Creative Commons License Todo o conteúdo deste periódico, exceto onde está identificado, está licenciado sob uma Licença Creative Commons