International Journal of Computational and Theoretical Chemistry
Volume 3, Issue 6, November 2015, Pages: 50-57

Computational Investigation on Substituent and Solvent Effects on the Electronic, Geometric and Spectroscopic Properties of Azobenzene and Some Substituted Derivatives

Isaiah Ajibade Adejoro, Oluwatoba Emmanuel Oyeneyin*, Babatunde Temitope Ogunyemi

Department of Chemistry, University of Ibadan, Oyo State, Nigeria

Email address:

(I. A. Adejoro)
(O. E. Oyeneyin)
(B. T. Ogunyemi)

To cite this article:

Isaiah Ajibade Adejoro, Oluwatoba Emmanuel Oyeneyin. Computational Investigation on Substituent and Solvent Effects on the Electronic, Geometric and Spectroscopic Properties of Azobenzene and Some Substituted Derivatives. International Journal of Computational and Theoretical Chemistry. Vol. 3, No. 6, 2015, pp. 50-57. doi: 10.11648/j.ijctc.20150306.12


Abstract: Computational investigation on the ground state properties of trans-azobenzene and four kinds of hydroxy-ended azobenzene-type chromophores containing different substituent groups as electron donor and acceptor in different solvent media was carried out. The effects ofsubstituents -I2, -OH- and -CH3, -NH2, and –Cl2 on the electronic properties like the EHOMO, ELUMO, band gap, dipole moments, global hardness, electrophilicity indices were studied using the Ab initio restricted DFT self-consistent field method with the Becke Three Lee Yang Parr (B3LYP)/6-31G* method in vacuum, water, diethylether, ethanol and acetone. The results showed that these properties were altered upon substitution with different groups. The azobenzene gave a slight difference in its band gap in different solvent changing from (3.95 eV) in vacuum to the lowest (3.87 eV) in acetone but changes drastically as we introduce different substituents. It was also found that the dipole moment (μ), polarizability (α), absorption wavelength (λab) gave slight change in different solvents but rapidly increased as the band gap reduces, invoking their reactivities. They are also red-shifted as different substituents are added. Of all the studied molecules, compound H gave the lowest band gap of 0.46 eV, the highest dipole moment (875.02 D), the highest polarizability (64.97C.m2V-1) and it is the most red-shifted (401.13 nm). Molecule H therefore, has the lowest band gap, highest polarizability and dipole moment. It also has the highest molecular size and the highest planarity. This means that the molecule is the most reactive, most polarizable, highest electro-optic response and it is the softest.

Keywords: Molecular Structure, Azobenzene, Solvent Effects, Band Gap, Ab initio Restricted Hf-Dft Self-Consistent Field Calculations, Dipole Moment


1. Introduction

The importance of azo-dyes organic compounds, among all other colourants cannot be over emphasized owing to their various applications [1]. Azobenzene is the simplest example of the various theoretically and pratically important class of organic dyes [2]. They are used in traditional textile applications such as in the dyeing of textile fibres, plastics, leathers, paper and biomedical studies[3,4], they are capable of producing different high intensity colors such as yellows, oranges and reds more readily because of their π-delocalization [5,6]. Methyl orange and disperse orange are examples of such azo compounds. Azobenzene exists mainly as the trans-isomer, this is because the cis-isomer is less stable than the trans-isomer. The trans-isomer can be converted to the cis-isomer upon photolysis [7]. Azobenzene molecules can be incorporated into polymer matrices as stabilizers. Recently, electronic industries have employed the use of dyes as colorimetric sensors and NLO devices [8,9].

Unsubstituted trans-azobenzene has a low intensity n-π* (occurs near 450 nm and is symmetry forbidden and less intense) absorption in the visible region and a higher intensity π-π* (occurs near 320 nm and is symmetry allowed) absorption in the near ultraviolet region while those that are ortho- and para- substituted with electron donating groups like the amino azobenzenes closely space the n-π* and π-π* bands in the violet or near-visible UV due to an increase in the π orbital energy and a decrease in the energy of the π* orbital. Chromophores having a donor-acceptor π-charge transfer structure exhibit high molecular hyperpolirizability (β) [10]. Substitution of the 4 and 4’ positions of the two azo rings with electron withdrawing and electron donating groups causes a push-pull configuration in a strongly asymmetric electron distribution, leading to a pronounced increment in the value of β.

The compound of interest is trans-azobenzene whose properties were investigated in vacuum and other solvents. Different kinds of hydroxy-ended azobenzene chromophores containing different electron withdrawing and electron donating substituents [10] were also considered.

Azobenzenes and its derivatives are aromatic in that they obey the aromaticity rule because they are cyclic, planar, and sp2hybridized. Addition of substituents to a molecular structure leads to great variations in the properties like stability, optical electronic properties such as the band gap, electron affinity, ionization potential and other properties of the molecules [11] and particularly alters the electric dipole moment (μ) of the molecule [23]. These changes however, might also occur if the molecules is effected by the environment, for instance, a solvent medium can shift the absorption spectrum which can greatly alter the electronic properties of the molecules [12,13]. It was observed that the ground state molecular geometries, dipole moments and polarizabilities of some aniline derivatives were associated with a decrease in the band gap upon substitution or with the presence of a solvent [14,48]. The theoretical investigation on the ground state properties of isomeric benzofused thieno [3, 2-b]furans was carried using the semi-empirical AM1 and Density functional theory with bias with the B3LYP using the 6-31G* basis set and it was observed that substituents like Br2, I2 and OH- alter the properties, stabilities and reactivities of the isomers [15].

Owing to the π-delocalization of these molecules, there is a redistribution of electronic charge across the entire length of conjugation under the influence of an external electric field, which should increase vastly for the functionalized molecules (having electron donating and electron withdrawing groups at the 4 and 4’ positions. The intra-molecular charge transfer (ICT) is an important process which focuses on systems in which the donor and acceptor groups are directly connected through a single or π-bond. These azobenzenes can be incorporated into self-assembled monolayers and superlattices [16], sol-gel silica glasses [17], various biomaterials [18], nonlinear optical devices [10]. Azobenzenes have been attached to some molecules in order to control their properties; this is due to the photochromic and photoswitchable natures of the azobenzenes. It has been reported to attach to cyclodextrins [19, 20], organometallic ferrocene polymers [21], dendrimers [22] among others.

As earlier mentioned, experimental dipole moments have been used to describe and measure the electron distribution. Meaning that adding substituents to the azobenzene chromophores can greatly alter the dipole moments as well as the polarizabilities therefore, invoking both IR and Raman activity simultaneously [24]. Another way to predict the both the intra-molecular and inter-molecular charge transfer is through the natural bond orbitals (NBOs) of molecules, with the intra-molecular interaction due to the overlapping of the bonding and the anti-bonding orbitals [25].

A lot of experimental and theoretical work have been used to study the nonlinear optical properties of inorganic and organic molecules with the later having a lot of advantages in that they are easier to synthesize, posses higher electrical conductivity, presence of delocalized electrons and possession of better mechanical properties. So, quantum chemical studies on molecules such as azobenzene and its derivatives will be carried out to understand their various properties and investigate the influence different solvent media and substituents play on these properties. It will enable researchers who are interested in synthesizing similar molecules of the same properties have a prior knowledge about them prior synthesis. It also allows for chemical tunability to obtain toward desired applicability. This work therefore, will provide theoretical explanations on the variations of the molecular dipole moments, polarizability, EHOMO and ELUMO (the frontier orbital energies), and UV absorptions of the various azobenzene chromophores. The ab initio Hartree-Fock/Density Functional Theory calculations with bias with the Becke Three Lee Yang Parr (B3LYP) functional and a basis set 6-31G* has proved to be the most used and reliable method in predicting the ground state electronic properties and molecular structure of organic systems [13,14,15,24,26,28]. The thermodynamic properties and the hyperpolarizabilities were predicted using the semi-empirical Austin Model 1 model.

2. Computational Details

The computational method used to study the electronic properties of the polymers is the ab initio restricted HF-DFT self consistent field (B3LYP) level of theory [29,30,31,49] (DFT/B3LYP) for which the energy of a system is described as a function of the electronic density. Spartan14 [35] program package was used to run calculations on intel®Core (TM) i5-3317U CPU @1.70GHz 1.70Hz computer with the Becke Three Lee-Yang- Parr (B3LYP) exchange- correlation method [31]). It has been shown that this functional gives an adequate description of carbon-based materials. In order to obtain an accurate description of the physical system, the standard polarized 6-31G* basis set [36-38] was used to investigate the electronic properties of the modeled compounds. Structural optimization was done without any constraints. It has been shown that B3LYP/6-31G* gives decent ground state structures of conjugated polymers [32]. For this work, semi-empirical Austin Model 1 (AM1) [33] as well as DFT/B3LYP/6-31G* calculations were carried out on them.

2.1. Dipole Moments (μ) [12, 23, 26]

The knowledge of the intermolecular forces helps us to get a clear picture of the interaction between atoms in same or different kind of molecules. Dipole moment, μ, is the measure of net polarity, which is the product of the charge, Q, at the end of the molecular dipole and the distance, r, between the charges. That is it tells us about the charge separation in a molecule.

(1)

Electric dipole moment is a measure of the electrical polarity of a system of charges, be it an electron or a molecule. It is used to study the intermolecular interactions involving non-bonded type dipole-dipole interactions because the higher the dipole moment, the stronger will be the intermolecular interactions [34]. It has been found to increase with a decrease in the HOMO-LUMO energy gap of molecular systems [14].

2.2. Polarizability (α)

This is a property of matter that measures the ability of a molecule to be polarized. That is, it measures the response of a molecule to external fields. Electric polarizability measures the tendency of a charge distribution to be distorted from its normal shape by an external field [39]. The electronic probability, α, is defined as the ratio of the induced dipole moment, , of an atom to the electric field, ε, that produces the dipole moment [40]. ε is the strength of the electric field and therefore vary proportionally with the induced dipole moment ;

(2)

where α is the polarizability of the molecule measured in C.m2V-1. It increases as the volume occupied by electrons increases, this is because the control the nuclear charge has on charge distribution becomes lesser as the number of electrons is increased [14].

(3)

According to equation (2.3), it is also found out that it increases with a decreased band gap between the EHOMO and ELUMO.

2.3. Frontier Orbitals (EHOMO and ELUMO)

Highest Occupied Molecular Orbital energy (EHOMO) and Lowest Unoccupied Molecular Orbital energy (ELUMO), also called the frontier orbitals, determine the interaction of the molecules with other species. The HOMO is the orbital that could act as an electron donor, since it is the outermost (highest energy) orbital containing electrons while the LUMO is the orbital that could act as the electron acceptor, since it is the innermost (lowest energy) orbital that has room to accept electrons. According to the frontier molecular orbital theory, the formation of a transition state is due to an interaction between the frontier orbitals (HOMO and LUMO) of reactants. According to Koopman’s theorem associated within the framework of Hartree Fock’s self consistent field molecular orbital theory, the ionization energy and electron affinity can be expressed through HOMO and LUMO energies. The energy of the HOMO is directly related to the ionization potential [41];

(4)

and the energy of the LUMO was generalized to also be directly related to the electron affinity;

(5)

The HOMO–LUMO gap is an important stability index. A large HOMO–LUMO gap implies low stability for the molecule in chemical reactions as the stabilization energy is inversely proportional to the energy gap. The concept of ‘‘activation hardness" has been also defined on the basis of the HOMO–LUMO energy gap. The qualitative definition of hardness is closely related to the polarizability, since a decrease of the energy gap usually leads to easier polarization of the molecule [42, 43]. Generally, HOMO energy level and LUMO energy levels depend on the electron-donating strength of donor and the electron-withdrawing strength of acceptor, respectively [44].

(6)

(7)

where ELUMO and EHOMO are the energies associated with the lowest unoccupied molecular orbital and the highest occupied molecular orbital respectively.

3. Results and Discussion

3.1. Results

The results of the DFT/B3LYP/6-31G* calculations for the ground state geometric properties (dihedral angles) for all the studied compounds are summarized in tables 1. The molecular energies, dipole moments, polarizabilities, frontier orbitals and other electronic properties of the studied compounds in different solvents (vacuum, diethylether, acetone, ethanol and water) and with different substituents (B, C, D, E, F and G) are summarized in tables 2 and 3. The UV absorption wavelengths are recorded and summarized in table 4.

3.2. Discussion

3.2.1. Geometry Properties

The bond distances and dihedral angles were calculated using DFT/B3LYP/6-31G*, there are no observable changes as the molecules were optimized in different solvents but there were observable changes in both the bond distances and dihedral angles as different substituents were introduced. Since there is no observable difference in the dihedral angles for molecule A in different solvents, that is, the molecule A is inclined to their aromatic ring planes at almost the same angles, this shows that the –N=N- group of the studied molecules is planar with the aromatic ring and were only distorted as different substituent groups are introduced. That is why in table 4, the molecules B, C, D, E, F, G and H inclined to their aromatic planes, especially for N3-N2-C4-C5 and N3-N2-C4-C3angles. There is a drastic alteration in the displacement (torsional angles between the substituted azobenzene with the torsional angles of molecule G and H 8.65° and -5.95° respectively. That is their planarity has greatly increased. It is of note that this is in accordance with the free electron molecular orbital approximation [45], which states that the band gap of molecules decrease with increased molecular size and planarity.

3.2.2. Electronic Properties

The importance of band gap engineering cannot be downplayed in modern technologies as it has been referred to in various articles and it is also an interesting topic. The band gap is the energy difference between the highest occupied molecular orbital (HOMO) and the lowest unoccupied molecular orbital (LUMO). It measures the electron density hardness and determines the molecular admittance in that molecules with high hardness (high ΔE) are termed hard molecules and those with low hardness (low ΔE) are termed soft molecules [46]. Results show that there is a slight difference in the band gaps of the molecules in different solvents, the highest difference coming from acetone (table 2). But as different substituents are added to the azobenze molecule there is a gradual reduction in the band gap, molecule H has the lowest band gap of 0.46 eV, and this is due to the replacement chlorine with iodine in molecule G. This is in line with Shikarawa’s work [47], where he doped polyacetylene with iodine to increase its conductivity. This is because the gap between the HOMO and LUMO is greatly reduced and allowseasy flow of electrons from the HOMO (electron donor) to the LUMO (electron acceptor). It is observed that the band gap of these molecules reduced as the dipole moment, polarizability, molecular size and planarity increase. The molecule with the lowest band gap (G) happens to be the one with the highest polarizability and dipole moment. It also has the highest molecular size and the highest planarity. This means that the molecule is the most reactive, most polarizable, highest electro-optic response and it is the softest.

The UV absorptions (λabs) in table 4 show that compound G is mostly red-shifted with the most intense absorption band at 401.13 nm. All studied molecules have are absorbed above 200 nm, that is the energy transitions present are n-π* and π-π* and therefore, any electron promotion will be from the HOMO, usually the singlet ground state (S0), to the LUMO (S1). The most known stable and bright chromophores absorb and emit in the wavelength range of 300 and 700 nm. As absorption is increased, it is always observed that the energy difference S1 and S0. This is also exhibited by all studied molecules, though the trend is not too noticeable in different solvent media but with different substituents, the absorption increased with decreased band gap.

Table 1. Results of DFT/B3LYP/6-31G* calculations on some selected dihedral angles of compound A in vacuum, acetone, ethanol, water and diethylether and for B, C, D, E, F, G and H. All dihedral angles were measured in (°).

Compounds/solvent N3-N2-C4-C5 Molecule N3-N2-C4-C5
A/vacuum 0.01 C 0.15
A/diethylether 0.01 D 1.40
A/ethanol 0.00 E 0.35
A/water 0.00 F 0.26
A/acetone 0.00 G 171.35
B -0.25 H -174.05

A= trans-azobenzene; B= 4-Hydroxy-azobenzene, C= 4-Amino-azobenzene, D= 4-Nitro-4'-hydroxy-azobenzene, E= 3,5-Dimethyl-4-(4'-nitrophenylazo)-phenol, F= 2,5-Dimethyl-4-(4'-nitrophenylazo)-phenol, G= 2,5-Dimethyl-4-(2'-chloro-4'-nitrophenylazo)-phenol, H= 2,5-Dimethyl-4-(2'iodo-4'-nitrophenylazo)-phenol

Table 2. Results of B3LYP/6-31G* calculations on the electronic properties of compound A in vacuum, acetone, ethanol, water and diethylether.

Compounds/solvent Energy(a.u) ELUMO(eV) EHOMO(eV) I(eV) A(eV) ΔE(eV) η(eV) µ(D) α()
A/vacuum -572.76 -2.17 -6.12 6.12 2.17 3.95 1.98 0.00 56.88
A/diethylether -572.78 -2.34 -6.25 6.25 2.34 3.91 1.96 0.00 56.89
A/ethanol -572.78 -2.44 -6.33 6.33 2.44 3.89 1.95 0.00 56.89
A/water -572.77 -2.46 -6.34 6.34 2.46 3.88 1.94 0.00 56.90
A/acetone -572.78 -2.41 -6.28 6.28 2.41 3.87 1.94 0.00 56.90

A= trans-azobenzene.

Table 3. Results of B3LYP/6-31G* calculations on the electronic properties of compound B, C, D, E, F, G and H.

Compounds Energy(a.u) ELUMO(eV) EHOMO(eV) I(eV) A(eV) ΔE(eV) η(eV) µ(D) α()
B -647.98 -2.02 -5.77 5.77 2.02 3.75 1.88 1.51 57.50
C -628.19 -1.82 -5.37 5.37 1.82 3.55 1.78 3.12 57.81
D -852.48 -2.90 -6.28 6.28 2.90 3.38 1.69 7.20 59.33
E -931.11 -2.82 -6.15 6.15 2.82 3.33 1.67 7.30 62.22
F -931.12 -2.84 -6.08 6.08 2.84 3.24 1.62 7.73 62.31
G -1390.71 -3.01 -6.16 6.16 3.01 3.15 1.58 8.02 63.44
H -941.89 6.17 5.71 -5.71 -6.17 0.46 0.23 875.02 64.97

B= 4-Hydroxy-azobenzene, C= 4-Amino-azobenzene, D= 4-Nitro-4'-hydroxy-azobenzene, E= 3,5-Dimethyl-4-(4'-nitrophenylazo)-phenol, F= 2,5-Dimethyl-4-(4'-nitrophenylazo)-phenol, G= 2,5-Dimethyl-4-(2'-chloro-4'-nitrophenylazo)-phenol, H= 2,5-Dimethyl-4-(2'iodo-4'-nitrophenylazo)-phenol

Table 4. Results of the absorption wavelength (λabs) obtained by DFT/B3LYP/6-31G* for compounds a in different solvents.

Compounds/solvent Wavelength/nm (intensity) Wavelength/nm (intensity) Compounds Wavelength/nm (intensity) Wavelength/nm (intensity)
A/vacuum 297.75 (0.12) 309.75 (1.03) C 266.27 (0.09) 339.73 (1.25)
A/diethylether 305.22 (0.26) 314.78 (0.94) D 307.53 (0.04) 367.34 (1.09)
A/ethanol 307.24 (0.33) 316.27 (0.88) E 336.69 (0.02) 371.35 (1.11)
A/water 307.62 (0.35) 315.56 (0.86) F 339.41 (0.08) 382.29 (1.03)
A/acetone 307.77 (0.35) 316.80 (0.87) G 333.38 (0.03) 392.56 (1.01)
B 260.36 (0.03) 325.51 (1.16) H 368.19 (0.22) 401.13 (0.81)

A= azobenzene; B= 4-Hydroxy-azobenzene, C= 4-Amino-azobenzene, D= 4-Nitro-4'-hydroxy-azobenzene, E= 3,5-Dimethyl-4-(4'-nitrophenylazo)-phenol, F= 2,5-Dimethyl-4-(4'-nitrophenylazo)-phenol, G= 2,5-Dimethyl-4-(2'-chloro-4'-nitrophenylazo)-phenol, H= 2,5-Dimethyl-4-(2'iodo-4'-nitrophenylazo)-phenol.

Fig. 1. Optimized structure of compound A.

Fig. 2. Optimized structure of compound B.

Fig. 3. Optimized structure of compound C.

Fig. 4. Optimized structure of compound D.

Fig. 5. Optimized structure of compound E.

Fig. 6. Optimized structure of compound F.

Fig. 7. Optimized structure of compound G.

Fig. 8. Optimized structure for compound H.

Fig. 9. UV spectrum of compound A in vacuum.

Fig. 10. UV spectrum of compound A in acetone.

Fig. 11. UV spectrum of compound A in diethylether.

Fig. 12. UV spectrum of compound A in ethanol.

Fig. 13. UV spectrum of compound A in water.

Fig. 14. UV spectrum for compound B.

Fig. 15. UV spectrum for compound C.

Fig. 16. UV spectrum of compound D.

Fig. 17. UV spectrum for compound E.

Fig. 18. UV spectrum of compond F.

Fig. 19. UV spectrum of compound G.

Fig. 20. UV spectrum for compound H.

4. Conclusion

Theoretical calculations have been carried out on azobenzene chromophores. Their electronic properties and geometric properties have been keenly studied in different solvent media and with the introduction of different substituting groups. It is of note that among all these molecules, H (2,5-Dimethyl-4-(2'iodo-4'-nitrophenylazo)-phenol) is the most planar, with the highest molecular size, lowest band gap (0.46 eV), highest dipole moment (875.02D) and polarizability (64.97 C.m2V-1), it also has the highest absorption (401.13 nm). That is, it has the best nonlinearity, when compared to others. The changes that occurred as different solvents and substituents were added are what we investigated here and it was observed that obvious changes occurred as different substituents were added but with different solvents, only little changes were observed. Because compound H has the lowest band gap and consequently, the softest, highest dipole moment, highest polarizability and it was red-shifted the most from the undoped azobenzene, it is suggested that it can be used for electronic applicabilities.

Acknowledgement

We wish to express our profound gratitude to the Senate, University of Ibadan, Oyo State for making available research grant and for also creating an enabling and conducive environment for this research work.


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