2. Experimental Section
In addition, it could be clearly observed molecular orbital
energy level changed by introducing different substituents.
Compared with the compound 4a, introduction of benzene,
naphthalene and thiophene groups to the para-position of
phenyl(4b,4c and 4d) could effectively extend the conjugate
chain. It could increase HOMO level and decrease LUMO level.
The π-π* transition energy would reduce and cause the band
bathochromic shift in the absorption and emission spectrum [28].
Simultaneously, introducing strong electronegative groups into
the compounds could reduce the HOMO and LUMO levels of the
compounds, but the effect of LUMO was more obvious, thus a
red-shift of the absorption band was caused [29]. In contrast, the
introduction of electron-donating group into the compounds
could significantly elevate the HOMO and alter the LUMO
moderately. There was considerable electronic coupling between
the electron-donating group and the diimidazolepyridine core,
thus decreasing the HOMO-LUMO energy gaps and causing red-
shift of 4f.[30] The HOMO-LUMO energy gaps of these
compounds were ranged from 2.89 to 3.23 eV. The wide energy
gap of 4f was higher than 4e and 4g, and this could be explained
that the strong electron-donating substituents reduced the
oxidation resistance of the molecule. So combining with the
electron acceptor core and electron donor substituent (-OCH3)
could allow the electronic directional movement and be helpful
to electronic transfer and transport. [31]
2.1 Materials and Measurements
All starting materials were purchased from TCI; the reagents
were obtained from J&K Chemical Company and used without
further purification. Synthetic process of materials was monitored
by thin layer chromatography (TLC), and the materials were
purified by column chromatography carried out on silica gel (200
~ 300 mesh). 1H NMR and 13C NMR spectra were recorded on a
Bruker DRX 400 MHz and 100 MHz spectrometer in CDCl3 or
DMSO. Chemical shifts were reported in ppm with
tetramethylsilane (TMS) as internal standard, and coupling
constants (J) were reported in Hertz (Hz). High resolution mass
spectra were recorded on Agilent 1100 (VL) mass spectrometer.
Thermogravimetric (TGA) measurements were performed on
Shimadzu DTG-60 A thermal analyzers at a heating rate of
10 °C/min under nitrogen atmosphere. UV-visible spectra and
photo-luminescence (PL) spectra were measured by Shimadzu
UV-2501PC UV-visible spectrophotometer and Shimadzu RF-
5301PC fluorescence spectrophotometer, respectively. Cyclic
voltammetric(CV) measurements were carried out on the Chi
1200A system in a conventional three-electrode cell with a glass
carbon working electrode, a platinum-wire counter electrode and
a
Ag/AgCl reference electrode referenced in anhydrous
dichloromethane solution of C16H36ClNO4 (0.10 M) at a
sweeping rate of 100 mV/s at room temperature. Density
functional theory (DFT) calculations were applied to characterize
the frontier molecular orbital energy levels of the compounds at
the B3LYP/6-31G(d) level by using the Gaussian 03 program.
Melting points were measured on a digital melting point
apparatus without correction. Infrared spectroscopy (IR) was
measured by SP-100 Fourier transform infrared spectroscopy.
2.2 Synthesis of materials
Main synthetic routes of diimidazolepyridine derivatives were
shown in Scheme 1. To begin our study, 4-bromobenzaldehyde
was selected as the starting material. The 4-arylbenzaldehydes
(2b-2g) were obtained by Suzuki coupling reaction.
Intermediates (3a-3g) were synthesized by refluxing cyclization
of compounds 2a-2g with 2, 3, 5, 6-tetraaminopyridine
trihydrochloride under acidic condition in methanol solution.
Finally, the target products (4a-4g) were obtained by alkylation
reaction with 1-bromobutane under basic condition.
Fig.1. Spatial distributions of frontier orbitals of the target
compounds at the B3LYP/6-31G(d) level
3.2 Thermal analysis
The thermal stabilities of the target compounds were
determined by thermogravimetric analysis (TGA) in N2
atmosphere and data were shown in Fig. 2 and Table 1.
Decomposition temperatures (Td, corresponding to 5% weight
loss) were measured to be 416, 443, 490, 458, 463, 484 and
467 °C for 4a-g, respectively. The thermodynamic data
demonstrated that the Td values of 4b-g were higher than 4a, it
was mainly related to the introduction of different aryl
substituents. The Td value of compound 4c was higher than 4b
and 4d. Thence, the Td values increased with the increase of their
rigid structure and conjugation degree[32]. In addition, compared
with 4b, the Td values of 4e, 4g and 4f were increased by 20, 24
and 41 °C, respectively. The reason is that introducing
substituents into the target compounds leaded to an increase in
molecular weights. This would increase the energy required for
molecular cleavage to result in an increase of Td values.
Moreover, the melting points(Tm) of these compounds were 181,
229, 261, 252, 244, 236 and 213 °C, respectively. The Tms of 4b-
4g were higher than 4a, this is due to the introduction of different
aryl substituents which made the molecular weight increase, then
resulted in an increase in the intramolecular π-π interactions.
Therefore, these compounds showed good thermal stability.
3. Results and Discussion
3.1. Theoretical calculations
For better understanding the structure-property relationship of
the diimidazolepyridine derivatives, the molecular configuration
and the frontier molecular orbital energy levels were determined
using DFT at the B3LYP/6-31G(d) level in the Gaussian 03
software. The results of HOMO and LUMO distribution of these
seven compounds were shown in Fig.1. Their computed frontier
orbital energies were shown in Table 1.
As shown in the Fig.1, the optimized structures of these
derivatives revealed that the diimidazolepyridine derivatives had
axial aryl substitutes. Such structural features could influence the
electrochemical and physicochemical properties. The HOMO and
LUMO of the compounds were all populated on the central
diimidazolepyridine. But it was found that the LUMO levels
were also located over the conjugate parts and electron
withdrawing groups. The HOMO levels were also located over
the electron-donating group. Obviously, by changing the
substitutes, a large difference of electronic density was found.
3