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BY-NC-ND 4.0 license Open Access Published by De Gruyter Open Access February 21, 2018

Spectroscopic (FT-IR, FT-Raman, UV, 1H and 13C NMR) insights, electronic profiling and DFT computations on ({(E)-[3-(1H-imidazol-1-yl)-1-phenylpropylidene] amino}oxy)(4-nitrophenyl)methanone, an imidazole-bearing anti-Candida agent

Lamya H. Al-Wahaibi, Munusamy Govindarajan, Ali A. El-Emam and Mohamed I. Attia
From the journal Open Chemistry


The anti-Candida agent, ({(E)-[3-(1H-imidazol-1-yl)-1-phenylpropylidene]amnio}oxy(4-nitropheny) methanone (IPAONM), was subjected to comprehensive spectroscopic (FT-IR, FT-Raman, UV–Vis 1H and 13C NMR) characterization as well as Hartree Fock and density functional theory computation studies. The selected optimized geometric bond lengths and bond angles of the IPAONM molecule were compared with the experimental values. The calculated wavenumbers have been scaled and compared with the experimental spectra. Mulliken charges and natural bond orbital analysis of the title molecule were calculated and interpreted. The energy and oscillator strengths of the IPAONM molecule were calculated by time-dependent density functional theory (TD-DFT). In addition, frontier molecular orbitals and molecular electrostatic potential diagram of the title compound were computed and analyzed. A study on the electronic properties, such as HOMO, HOMO-1, LUMO and LUMO+1 energies was carried out using TD-DFT approach. The 1H and 13C NMR chemical shift values of the title compound were calculated by the gauge independent atomic orbital method and compared with the experimental results.

Graphical Abstract

1 Introduction

Invasive fungal infections are an ever-growing health problem worldwide causing high rates of morbidity and mortality particularly in chronically ill individuals or those taking anticancer or immunosuppressant drugs [1]. Candida albicans (C. albicans) has been identified as a leading invasive fungal pathogen and accounts for up to 70% of global fungal incidents with 30-55% mortality rate [2]. The current repertoire of antifungal drugs to treat C. albicans is limited and suffers from significant adverse effects and resistance [3,4]. Consequently, it is highly desirable to search for new alternative anti-C. albicans agents endowed with high potency and improved safety.

Azole antifungal agents are widely used to treat invasive fungal infections caused by C. albicans and they rapidly became the most clinically prescribed antifungals worldwide [5]. They target sterol 14α-demethylase enzyme leading to fungal cell death due to inhibition of the biosynthesis of ergosterol, a vital component of the fungal cell membrane, and accumulation of the methylated sterol side products [6,7].

The title compound, namely ({(E)-[3-(1H-imidazol-1-yl)-1-phenylpropylidene] amnio}oxy(4-nitropheny) methanone (IPAONM) is an imidazole-bearing anti-C. albicans agent with minimum inhibitory concentration (MIC) value of 0.7 μmol/mL being about fourfold more potent than the reference antifungal drug, fluconazole [8]. The displayed anti-C. albicans activity of the IPAONM molecule represents a strong motive for exploring a comprehensive spectroscopic characterization and density functional theory (DFT) computations on this interesting compound. Thus, its Mulliken charges, natural bond orbital (NBO) analysis and molecular electrostatic potential (MEP) were investigated. NBO analysis determines the possible intermolecular delocalization or hyper-conjugation for the IPAONM molecule. Moreover, its frontier molecular orbitals (FMO), HOMO and LUMO energies were also computed. The HOMO and LUMO molecular orbitals investigations give insight into the possible way in which the IPAONM molecule can interact with its target receptors. The results of the current study could provide a useful platform to develop new chemical entities characterized by potent and safe anti-C. albicans profile.

2 Experimental Section

2.1 General

The FT-IR spectrum of the IPAONM molecule has been recorded with a Perkin-Elmer 180 Spectrometer in the range of 4000–400 cm−1 with spectral resolution ± 2 cm-1. Its FT-Raman spectrum was also recorded in the same instrument with FRA 106 Raman module equipped with Nd: YAG laser source operating in the region 100-4000 cm−1 at 1.064 μm line widths with 200 mW powers. The spectra were recorded with scanning speed of 30 cm-1. min-1 with spectral width of 2 cm-1. The frequencies of all sharp bands were accurate to ± 1 cm-1. NMR spectra of the IPAONM were recorded on a Bruker NMR spectrometer (Bruker Biospin, Billerica, MA, USA). 1H spectrum was run at 500 MHz and 13C spectrum was run at 125 MHz in deuterated dimethyl sulfoxide (DMSO-d6). The UV–Vis spectrum of the title molecule was registered in the range of 200–400 nm in acetonitrile using Shimadzu UV-2101 PC, UV–Vis recording spectrometer. All solvents and reagents were purchased from Sigma-Aldrich Chemie GmbH (Taufkirchen, Germany) and were pure enough to be used without further purification.

2.2 Synthesis

Preparation of ({(E)-[3-(1H-imidazol-1-yl)-1-phenylpropylidene] aminooxy)(4-nitro phenyl)methanone (5)

The title compound 5 was prepared according to the previously reported method [8]. The NMR spectral data of compound 5 are in agreement with the previously reported ones [8].

2.3 Quantum Chemical Calculations

The entire quantum chemical calculations have been performed using Hartree Fock (HF) and density functional theory (DFT, B3LYP) methods with 6-311G(d,p) basis set using the Gaussian 09 W program [9]. The optimized structural parameters have been evaluated for the calculations of vibrational frequencies at different level of theories. At the optimized geometry for the IPAONM molecule no imaginary wavenumbers were obtained, so there is a true minimum on the potential energy surface. As a result, the calculated frequencies, reduced masses, force constants, infrared intensities, Raman activities and depolarization ratios were obtained. In order to improve the computed values to be in agreement with the observed experimental values, it was necessary to scale down the calculated harmonic frequencies. Hence, the wavenumbers calculated at HF level were scaled by 0.9067 and the range of wavenumbers above 1700 cm-1 were scaled by 0.958 and below 1700 cm-1 by 0.983 for the B3LYP method [10,11]. The assignments of the calculated modes have been made on the basis of the corresponding PEDs. The vibrational frequencies were calculated using VEDA program [12]. GaussView program [13] was used in order to get visual animation and also for the verification of the normal modes assignments. The electronic absorption spectra for the optimized molecule were calculated with the time dependent density functional theory (TD-DFT) at B3LYP/6-311G(d,p) level.

Ethical approval: The conducted research is not related to either human or animals use.

3 Results and Discussion

3.1 Synthesis

The title compound 5 was prepared by adopting the previously reported literature procedure [8] as illustrated in Scheme S1. The spectral data of the title compound 5 are consistent with the previously reported ones [8].

3.2 Molecular Geometry

Molecules bearing oxygen or nitrogen substituents on their ring systems have the mono substituent co-planar with the ring. The selected optimized DFT geometries of the IPAONM molecule are calculated by HF and B3LYP methods with 6-311G(d,p) as a basic set with atom numbering as shown in Figure 1. The calculations are converged to optimized geometries, which correspond to the true energy minima, as revealed by the lack of imaginary frequencies in the vibrational mode calculations.

Figure 1 The optimized possible geometric structure with atoms numbering of the IPAONM molecule.

Figure 1

The optimized possible geometric structure with atoms numbering of the IPAONM molecule.

3.3 Geometric Structure

A conformation analysis was carried out on the IPAONM molecule in order to determine its most stable conformation. The crystal structure of the title compound is indicated in the Figure 2. The potential energy obtained by the rotation of the two dihedral angles C5-C7-C8-C9 and O16-C17-C18-O19 group from 0° to 360° in PM6 method is depicted in Figure 3. The most stable conformers are at 90° for SC1 and at 320° for SC2 with energy value = 0.0761424 a.u. The optimized geometry of the title molecule afforded one conformer at this stage. The selected optimized parameters were collected and compared with the experimental X-ray data [8] as illustrated in Table 1. The most stable conformer possesses the global minima on its potential energy surface as its calculated vibrational spectrum contains no imaginary wavenumbers.

Figure 2 The crystal structure of the IPAONM molecule.

Figure 2

The crystal structure of the IPAONM molecule.

Figure 3 The potential energy scan picture the IPAONM molecule.

Figure 3

The potential energy scan picture the IPAONM molecule.

Table 1

Selected optimized geometrical parameters and XRD values of bond lengths (Å) and bond angles (°) of the IPAONM molecule.

ParametersHF/6-311G(d,p)B3LYP/6-311G(d,p)XRD values
Bond lengths (Å)
Bond angles (°)
C14-N13-C12105.14105.66104.9 0

These optimized parameters are in agreement with the crystallographic values (Table 1). The aromatic N-O bond distances of IPAONM were found to have lower values in case of HF calculations with respect to B3LYP computations. The oxygen–carbon bonds are not of the same length. The elongation of O16-C17 could be attributed to its presence in the main chain. The N-C bond distances are present between 1.469 to 1.265 Å. The N42-C22 is the longest bond among the N-C bonds and its length is 1.469 Å. In the imidazole ring, the bonds N10-C9, N13-C12, N13-C14, N10-C11 and N10-C14 are 1.453, 1.355, 1.371, 1.309 and 1.414 Å in length, respectively.

The HF and B3LYP calculations also gave dihedral angles values that are consistent with the selected experimental values (Table 1). The highest value was 127.82° in case of C9-N10-C11, while the bond angle C14-N10-C11 possesses the smallest selected bond angle being about 104.9°. Moreover, the bond angles, O19-C17-O16 and O25-N42-O43 have the values of 125.13° and 123.17°, respectively.

3.4 Mulliken Atomic Charges

Mulliken atomic charge calculations have a substantial role in the quantum chemical calculations of molecular systems because they affect a lot of their properties. The calculated Mulliken charge values of the title compound IPAONM are listed in Table S1 and its charge distribution is shown in Figure 4. The Mulliken charges of the IPAONM molecule presumably occur due to polarization on the molecule. The charges of the NO2 moiety are -0.258427 e_ on one oxygen atom, -0.259955 e- on the other oxygen atom and 0.173708 e- on the nitrogen atom using B3LYP/6-311G(d,p) method which are less than the values obtained by HF/6-311G(d,p) method. All nitrogen atoms are negatively charged except for N42. The Mulliken charges on nitrogen atoms N10 and N13 are more negative than that on N15. All aromatic carbon atoms are negatively charged using B3LP/6-311G(d,p) method except C22 due to its bonding with the nitro group . C7 and C17 are the highest positively charged carbon atoms by B3LYP method due to their bonding to nitrogen and oxygen atoms, respectively. All hydrogen atoms are positively charged using both HF and B3LP methods (Figure 4).

Figure 4 The Mulliken charge distribution for the IPAONM molecule.

Figure 4

The Mulliken charge distribution for the IPAONM molecule.

3.5 Frontier Molecular Orbitals (FMOs)

HOMO is the highest occupied molecular orbital and LUMO is the lowest-lying unoccupied molecular orbital and together they are named frontier molecular orbitals (FMOs). The FMOs play a crucial role in many optical and electric properties as well as in quantum chemistry and UV–Vis spectra of molecules [14]. The HOMO makes up the ability to donate electrons, while LUMO as an electron acceptor. The energy gap between HOMO and LUMO decides the kinetic stability, chemical reactivity, optical polarizability and chemical hardness–softness of a molecule [15].

The energies of the four important molecular orbitals, the highest and the second highest occupied MO’s (HOMO and HOMO–1) as well as the lowest and the second lowest unoccupied MO’s (LUMO and LUMO+1), of the IPAONM molecule were calculated using B3LYP method at 6-311G(d,p) level. The 3D plots of the HOMO-1, HOMO, LUMO and LUMO+1 orbitals computed at the B3LYP/6-311G(d,p) level for the IPAONM molecule are illustrated in Figure 5. The positive phase is red and the negative one is green. It is clear from Figure 5 that while the HOMO is localized on the imidazole moiety of the IPAONM molecule, the LUMO is localized on the nitrophenyl ring. However, the HOMO-1 is localized on the other phenyl ring, LUMO+1 is localized on both phenyl ring and the nitro group of the title molecule. Both the HOMOs and the LUMOs are mostly π-antibonding type orbitals.

Figure 5 The molecular orbitals and energies for the HOMO-1, HOMO, and LUMO and LUMO+1 of the IPAONM molecule.

Figure 5

The molecular orbitals and energies for the HOMO-1, HOMO, and LUMO and LUMO+1 of the IPAONM molecule.

The calculated energy values of the title molecule are HOMO = −6.5688 and LUMO = −3.1197 eV. The value of energy separation between the HOMO and LUMO is -3.4491 eV (Table 2). The HOMO–LUMO energy gap of the title molecule explains the charge transfer interaction inside the molecule, which influences its bioactivity. Increasing the value of the energy gap indicates more stability of the molecule.

Table 2

Calculated molecular orbital energy values of the title molecule.

TD-DFT/B3LYP/6-311G(d,p)Gas PhaseChloroform Phase
Etotal (Hartree)-1253.72-1253.42
EHOMO (eV)-6.56868-6.27965
ELUMO (eV)-3.11963-2.86721
ΔEHOMO-LUMO gap (eV)-3.44905-3.41245
EHOMO-1 (eV)-7.14673-6.7403
ELUMO+1 (eV)-2.09123-1.68318
ΔEHOMO-1-LUMO+1 gap (eV)-5.0555-5.05713
Electronegativity X (eV)4.84414.5734
Chemical hardness η (eV)1.72451.7062
Electrophilicity index ψ (eV)6.80366.1293
Dipole moment (Debye)7.30898.4214

3.6 Electrostatic Potential, Total Electron Density and Molecular Electrostatic Potential

The electrostatic potential (ESP), total electron density (TED) and molecular electrostatic potential (MEP) of the title molecule are illustrated in Figure 6. The yellowish blob in the ESP Figure reflects the negative portion of the title molecule. However, the MEP diagram represents the constant electron density surface of the IPAONM molecule. The MEP diagram is a useful tool to analyze the reactivity of the molecules toward electrophiles and nucleophiles. In the majority of the MEPs, the maximum positive and negative regions in the molecule are indicated by red and green colors which are the preferred sites to be attacked by electrophiles and nucleophiles, respectively. The importance of the MEPs resides in the fact that they display at the same time the molecular size, shape as well as positive, negative and neutral electrostatic potential regions of the molecule in terms of color grading. They are also a very useful tool correlating molecular structure with the physiochemical properties of the molecule [16,17,18].

Figure 6 Electrostatic potential (ESP), electron density (ED) and the molecular electrostatic potential map (MEP) for the IPAONM molecule.

Figure 6

Electrostatic potential (ESP), electron density (ED) and the molecular electrostatic potential map (MEP) for the IPAONM molecule.

The electrostatic potential at the surface of the IPAONM molecule is represented by different colors in the order red < orange < yellow < green < blue in the range between -0.0568 a.u. (deepest red) to 0.0568 (deepest blue). The blue color indicates the strongest attraction, while the red color indicates the strongest repulsion. The negative potential was manifested over the electronegative oxygen atoms of the nitro group in the MEP diagram of the title molecule with values of -0.04086 and -0.04019 a.u.

3.7 Natural Bond Orbital (NBO) Analysis

The larger the stabilization energy value of the molecule, the more significant is the interaction between the donors and acceptors, i.e. the more giving tendency there is from donors to acceptors, the greater the extent of conjugation of the entire system. The intramolecular interactions of the title molecule are formed by the orbital overlap between σ(C-N), σ*(C-N), σ(N-C), σ*(N-C), σ(C-O), σ*(C-O), σ(O-N), σ*(O-N), σ(N-O), σ*(N-O) and π(C-C), π*(C-C) bond orbitals. These fundamental interactions were observed as a gain in the electron density (ED) in the C-C antibonding orbitals that weaken the respective bonds. These intramolecular charge transfers (σ → σ*, π → π*) can induce large nonlinearity of the IPAONM molecule.

Natural bond orbital (NBO) analysis has been carried out on the IPAONM molecule at the B3LYP/6-311G(d,p) level in order to elucidate its possible intramolecular, rehybridization and delocalization of the electron density within the molecule. The intramolecular hyperconjugation interactions of the σ and π electrons of C-N, N-C, C-O, O-N and N-O to the anti C-C, C-H, C-N and N-O bonds in the title molecule lead to stabilization of the respective moieties within the molecule as evident from Table S2. The strong hyperconjugative interactions of the σ electron of σ (N10–C11) are distributed to σ*(C9-N10), N10-C14, C11-C12, C12-N13, C12-H36, N13-C14 and C14-H37 of the imidazole ring with energy values of 1.86, 2.47, 1.47, 0.73, 3.19, 0.63 and 2.89 kcal/mol, respectively. On the other hand, the σ (C17-O19) and π (C17-O19) bonds are distributed to π*(C18-C20) with energy values of 1.08 and 4.36 kcal/mol, respectively. In addition, in the LP N10 and LP N13 are distributed to the LP*(1) (C11-C12) bond with energy values of 30.68 and 5.46 kcal/mol, respectively.

3.8 Electronic Absorption Spectra

Based on a fully optimized ground-state structure of the of the IPAONM molecule, B3LYP/6-311G(d,p) calculations have been carried out to determine its low-lying excited states. The experimental (in acetonitrile) and theoretical UV absorption wavelengths (in acetonitrile, aniline, chloroform, DMSO, ethanol, methanol and toluene) of the title compound are shown in Figure S1 and Table 3. Calculations involving the vertical excitation energies, oscillator strengths (f) and wavelengths (λ) have been performed and the results were compared with experimental values [19]. The major contributions of the transitions of the IPAONM molecule were designated with the aid of SWizard program [20]. The predicted wavelengths using B3LYP/6-311G(d,p) calculations in acetonitrile are 411.65, 358.21, 318.02, 315.99 and 299.80 nm, whereas the experimental wavelengths in acetonitrile are 235.10 and 282.80 nm. In view of the calculated absorption spectra of the title compound, the maximum absorption wavelengths correspond to the electronic transitions from the highest occupied molecular orbital HOMO to the lowest unoccupied molecular orbital LUMO with 100% contribution and the transitions from HOMO-9 to LUMO with 85% except with chloroform and toluene.

Table 3

The calculated absorption wavelengths (λ), excitation energies (E) and oscillator strengths (f) of the IPAONM molecule using B3LYP/311G(d,p) level.

Solventλ (nm)E (ev)f (a.u.)Major contribution
Acetonitrile411.653.010.0007HOMO->LUMO (100%)
358.213.460.1343H-1->LUMO (99%)
318.023.890.0001H-9->LUMO (86%)
315.993.920.0029H-2->LUMO (99%)
299.804.130.0023H-3->LUMO (86%),
Aniline409.143.030.0008HOMO->LUMO (100%)
355.993.480.1473H-1->LUMO (99%)
319.943.870.0000H-9->LUMO (85%)
313.553.950.0037H-2->LUMO (99%)
299.594.140.0040HOMO->L+1 (87%)
Chloroform408.053.030.0007HOMO->LUMO (100%)
354.223.500.1419H-1->LUMO (99%)
320.893.860.0000H-9->LUMO (84%)
312.133.970.0036H-2->LUMO (99%)
299.974.130.0035HOMO->L+1 (96%)
DMSO411.853.010.0007HOMO->LUMO (100%)
358.533.450.1382H-1->LUMO (99%)
317.933.890.0001H-9->LUMO (86%)
316.133.920.0030H-2->LUMO (99%)
299.864.130.0023H-3->LUMO (88%)
Ethanol411.343.010.0007HOMO->LUMO (100%)
357.983.460.1353H-1->LUMO (99%)
318.243.890.0001H-9->LUMO (86%)
315.733.920.003H-2->LUMO (99%)
299.714.130.0025H-3->LUMO (83%)
Methanol411.593.010.0007HOMO->LUMO (100%)
358.123.460.1334H-1->LUMO (99%)
318.063.890.0001H-9->LUMO (86%)
315.933.920.0029H-2->LUMO (99%)
299.784.130.0023H-3->LUMO (86%)
Toluene405.663.050.0007HOMO->LUMO (100%)
349.723.540.1486H-1->LUMO (99%)
323.523.830.0000H-9->LUMO (78%)
307.914.020.0041H-2->LUMO (98%)
301.724.100.0033HOMO->L+1 (99%)

3.9 Topological Analysis

The structure of the IPAONM molecule was also analysed by Bader’s charge electron density topological analysis [21,22]. In the topological atoms in molecules (AIM) theory, the chemical bonds and molecular reactivity are interpreted in terms of the total molecular electronic density ρ(r) and its corresponding Laplacian ∇2ρ(r). The ρ(r) and ∇2ρ(r) values at the bond critical points (BCP1 and BCP2) allow the characterization of the chemical bonds between atoms of the molecule. Different studies have pointed out that formation of hydrogen bonds was associated with the appearance of BCP1 and BCP2 between hydrogen atoms and the acceptor atoms, which are linked by the concomitant bond path [23,24,25]. The positive Laplacian value of the electron density ∇2ρ(r) indicates that the interaction is dominated by the contraction of charge away from the interatomic surface toward each nuclei. Figure 7 illustrated the AIM molecular graphic of the title molecule showing its different bonds and ring critical points obtained by B3LYP/6-311G(d,p) method. The Laplacian values of the IPAONM molecule at the BCP1 and BCP2 of H37-H38 and H30-H32 bonds are 0.0069 and 0.0473 a.u., respectively, while their Lagrangian kinetic energy density G(r) and energy density H(r) values are 0.0013, 0.0096 and 0.0004, 0.0022 a.u., respectively.

Figure 7 The topological diagram of the IPAONM molecule.

Figure 7

The topological diagram of the IPAONM molecule.

3.10 Vibrational Analysis

All vibrations are active in both Raman and infrared absorptions. The detailed vibrational assignments of the experimental wavenumbers are based on normal mode analyses and a comparison with theoretically scaled wavenumbers with PED by B3LYP method. Since the scaled wavenumbers following B3LYP/6-311G(d,p) method were found to be close to the experimental data than the results obtained using HF method, so only the PEDs from this set of data are discussed in detail. The observed and simulated FT-IR and laser Raman spectra of the IPAONM molecule are shown in Figures 8 and 9, respectively. The observed and scaled theoretical frequencies using HF and DFT (B3LYP) with 6-311G(d,p) basis set, infrared intensities and Raman activities of B3LYP/6-311G(d,p) are listed in Table 4.

Figure 8 Experimental FT-IR and FT-Raman and spectra of the IPAONM molecule.

Figure 8

Experimental FT-IR and FT-Raman and spectra of the IPAONM molecule.

Figure 9 Simulated FT-IR and FT-Raman and spectra of the IPAONM molecule.

Figure 9

Simulated FT-IR and FT-Raman and spectra of the IPAONM molecule.

Table 4

Detailed assignments of vibrational bands of the IPAONM molecule along with potential total energy distribution.

No.ExperimentalTheoretical HF/6-311G(d,p)B3LYP/6-311G(D,P)Vibrational Assessment

  1. I: IR intensity; S: Raman scattering activity; γ: stretching; β: in-plane bending; φ: out-of-plane bending

3.10.1 C-H Vibrations

Aromatic derivatives gave rise to C-H stretching, C-H inplane and C-H out-of-plane bending vibrations. Aromatic compounds commonly exhibit multiple weak bands in the region of 3100–3000 cm−1 due to aromatic C-H stretching vibrations and they are not appreciably affected by the nature of the substituents [26,27]. The aromatic vibrations of the title compound were observed at 3123, 3052 and 3003 cm-1 in its FT-IR spectrum and at 3069 and 3034 cm-1 in its FT-Raman spectrum. The remaining C-H vibrations occurred at 2925 cm-1 in the FT-IR spectrum and at 2979 and 2958 cm-1 in the FT-Raman spectrum.

The bands due to C-H in-plane bending vibrations are expected to be in the region of 1000–1300 cm−1 [28]. The bands observed at 1182 and 973 cm−1 in the FT-IR spectrum and at 1000 cm−1 in the FT-Raman spectrum were assigned to be the C-H in-plane bending vibrations of the IPAONM molecule. The theoretically scaled C-H vibrations by B3LYP/6-311G(d,p) level of theory showed good agreement with the experimentally recorded data. The C-H out-of-plane bending vibrations usually appear within the region of 900-675 cm−1 [28]. The out-of-plane C-H vibrations of the title compound arose at 621 and 513 cm-1 in its FT-IR spectrum and at 441 and 406 cm-1 in its FT-Raman spectrum. The other C-H out-of-plane bending vibrations are within the characteristic region.

3.10.2 Ring Vibrations

Most of the aromatic ring modes are due to C-C bands. The ring stretching vibrations are expected within the region 1620-1390 cm−1 [29]. Most of the aromatic ring modes are altered by the substitution on the ring. The C-C stretching vibrations in aromatic compounds usually form strong bands. The title compound manifested bands of different intensities at 1517, 1495, 1480, 1452, 1405, 1392, 1369 and 1304 cm-1 in its FT-IR spectrum and at 1627, 1500, 1369 and 1355 cm-1 in its FT-Raman spectrum and they have been assigned to be for the C-C stretching vibrations. The calculated values by B3LYP/6-311G(d,p) method are consistent with the experimental values. The theoretical ring in-plane bending and out-of-plane bending modes are also in a good agreement with experimental data.

Only five infrared bands at 1104, 1078, 1025, 778 and 758 cm−1 and one Raman band at 1169 cm−1 were assigned to the C–C-C in-plane bending vibrations of the IPAONM molecule. In addition, one band was assigned to the C-C-C out-of-plane bending vibration of the title molecule at 696 cm−1 in its FT-IR spectrum.

3.10.3 C-N and C-O Vibrations

C–N vibrations are usually mixed with several other bands and thus it is more difficult for them to be identified in a specific region. The observed bands at 1569 and 1469 cm−1 in the FT-IR spectrum of 2-formylpyridine were assigned to be due to C–N stretching [30], while they were noticed at 1580 and 1260 cm−1 in ethyl pyridine [31]. In the present work, the observed bands at 1615, 1608, 1575 and 1339 cm−1 in the FT-IR spectrum and at 1597 and 1500 cm−1 in the FT-IR spectrum have been assigned to C–N stretching vibrations, whereas the title compound manifested CCN in-plane bending at 1031 and 929 cm−1 in its FT-Raman spectrum and only one band at 929 cm−1 in its FT-IR spectrum. The CCN out-of-plane bending modes were observed at 657 cm−1 in the FT-IR spectrum of the IPAONM molecule and at 645 and 617 cnr1 in its FT-Raman spectrum. The C-O stretching vibrations are well correlated with the experimental values at 1636 cm−1 in the FT-IR spectrum and at 1285 in the FT-Raman spectrum. The calculated C-N and C-O vibration frequencies by B3LYP/6-311G(d,p) method coincide with the experimental values.

3.10.4 N-O vibrations

The N-O stretching vibration of the title compound was observed at 1751 cm-1 in its FT-IR spectrum and its N-O inplane bending vibration appeared at 1240 cm-1, while its N-O out-of-plane bending vibration was identified at 645 cm-1 in its FT-Raman spectrum. All the theoretical values of N-O vibrations of the IPAONM molecule are in agreement with the recorded experimental data.

3.11 NMR Analysis

The calculated 1H and 13C NMR chemical shift values of the IPAONM molecule are presented in Table 5 and have been compared with the experimental data. 1H and 13C NMR chemical shifts are reported in ppm relative to TMS. Full geometry optimization of the IPAONM molecule was carried out at the gradient corrected density functional level of theory using the hybrid B3LYP method based on Becke’s three parameters functional of DFT. Thereafter, gauge-including atomic orbital (GIAO) 1H and 13C chemical shift calculations of the title compound was performed by the same method using 6-311G(d,p) basis set and integral equation formalism-polarizable continuum model (IEF-PCM)/DMSO variant.

Table 5

Theoretical and experimental 13C and 1H NMR chemical shift values (ppm) with respect to TMS in DMSO solution of the IPAONM molecule.

AtomsTheoretical HF/6-311G(d,p)ExperimentalAtomsTheoretical HF/6-311G(d,p)Experimental

  1. Atoms were numbered as illustrated in Figure 1.

Aromatic carbons gave calculated signals in the overlapped areas of the 13C spectrum of the title molecule with chemical shift values in the range of 134.4 to 158.1 ppm. Their corresponding experimental chemical shift values occurred in the range of 128.5-150.4 ppm. Moreover, the highest 13C chemical shift values were observed for C17 and C7 to be 165.1 and 161.4 ppm due to their connection to oxygen and nitrogen atoms, respectively, while the imidazole carbons C11, C12 and C14 were noticed at 119.4, 127.3 and 137.2 ppm, respectively, in which C14 is the most downfield carbon atom due to its bonding with two nitrogen atoms. One the other hand, the ethylene carbons, C8 and C9, manifested the lowest chemical shift values at 30.1 and 43.0 ppm, respectively, in the 13C NMR spectrum of the IPAONM molecule.

The calculated chemical shift values for the aromatic hydrogens of the title compound lie in the range of 7.7-8.7 ppm and their respective observed values occurred in the range of 7.5-8.4 ppm. The aromatic protons H38, H39, H40 and H41 are the most downfield protons due to their connection to the nitro-substituted aromatic ring, whereas the ethylene protons H31, H32, H33 and H34 appear in the range of 3.6-4.3 ppm being the most upfield protons in the 1H NMR spectrum of the IPAONM molecule. There is a good agreement between the experimental and theoretical chemical shift values of the title compound.

4 Conclusion

A comprehensive spectroscopic profiling and vibrational analysis of the anti-Candida agent IPAONM have been performed using HF and DFT computation methods with 6-311G(d,p) basis set. The optimized geometry of the title molecule afforded only one conformer. The Mulliken charge distribution study revealed that all nitrogen atoms have negative charge except N42 and N15 is less negative than N10 and N13. The HOMO–LUMO energy gap explained the possible charge transfer inside the IPAONM molecule, which influences its biological activity. The Laplacian of charge density at the BCP1 and BCP2 of H37-H38 and H30-H32 bond critical points are 0.0069 and 0.0473 a.u., respectively. The theoretically scaled C-H vibrations by B3LYP/6-311G (d,p) method showed good agreement with the experimentally recorded data. It is believed that the results of the current exploration could support the development of new potent anti-Candida agents to be appropriate for clinical harnessing.

  1. Supplementary information: Tables S1 and S2 as well as Scheme S1 and Figure S1 are provided as supporting information.

  2. Conflict of interest: Authors state no conflict of interest.


This work was funded by the Deanship of Scientific Research at Princess Nourah bint Abdulrahman University through the Research Group Program (Grant No. RGP-1438-0010).


[1] Ngo H.X., Garneau-Tsodikova S., Green K.D., A complex game of hide and seek: the search for new antifungals, Med. Chem. Comm., 2016, 7, 1285-1306.10.1039/C6MD00222FSearch in Google Scholar

[2] Vandeputte P., Ferrari S., Coste A.T., Antifungal resistance and new strategies to control fungal infections, Int. J. Microbiol., 2012, 2012, 1-24, Article ID 713687.10.1155/2012/713687Search in Google Scholar

[3] Denning D.W., Kibbler C.C., Barnes R.A., British society for medical mycology proposed standards of care for patients with invasive fungal infections, The Lancet Infect. Dis., 2003, 3, 230-240.10.1016/S1473-3099(03)00580-2Search in Google Scholar

[4] Kathiravan M.K., Salake A.B., Chothe A.S., Dudhe P.B., Watode R.P., Mukta M. S., Gadhwe S., The biology and chemistry of antifungal agents: a review. Bioorg. Med. Chem., 2012, 20, 5678-5698.10.1016/j.bmc.2012.04.045Search in Google Scholar PubMed

[5] Holbrook S.Y., Garzan A., Dennis E.K., Shrestha S.K., Garneau-Tsodikova S., Repurposing antipsychotic drugs into antifungal agents: Synergistic combinations of azoles and bromperidol derivatives in the treatment of various fungal infections. Eur. J. Med. Chem., 2017, 139, 12-21.10.1016/j.ejmech.2017.07.030Search in Google Scholar PubMed

[6] Ghannoum M.A., Rice L.B., Antifungal agents: mode of action, mechanisms of resistance, and correlation of these mechanisms with bacterial resistance. Clin. Microbiol. Rev., 1999, 12, 501-517.10.1128/CMR.12.4.501Search in Google Scholar PubMed PubMed Central

[7] Sheehan D.J., Hitchcock C.A., Sibley C.M., Current and emerging azole antifungal agents. Clin. Microbiol. Rev., 1999, 12, 40-79.10.1128/CMR.12.1.40Search in Google Scholar PubMed PubMed Central

[8] Attia M.I., Ghabbour H.A., Zakaria A.S., Fun H.-K., In vitro anti-Candida activity and single crystal X-ray structure of ({(1E)-[3-(1H-imidazol-1-yl)-1-phenylpropylidene]amino}oxy) (4-nitrophenyl)methanone. Bangladesh J. Pharmacol., 2014, 9, 43-48.10.3329/bjp.v9i1.16990Search in Google Scholar

[9] Frisch M., Trucks G., Schlegel H.B., Scuseria G., Robb M., Cheeseman J., Montgomery Jr J., Vreven T., Kudin K., Burant J., Gaussian 03, revision C. 02; Gaussian, Inc. Wallingford, CT, 2004.Search in Google Scholar

[10] Arslan H., Algül Ö., Synthesis and Ab Initio/DFT Studies on 2-(4-methoxyphenyl)benzo[d]thiazole, Int. J. Mol. Sci., 2007, 8, 760-776.10.3390/i8080760Search in Google Scholar

[11] Sundaraganesan N., Ilakiamani S., Saleem H., Wojciechowski P.M., Michalska D., FT-Raman and FT-IR spectra, vibrational assignments and density functional studies of 5-bromo-2-nitropyridine, Spectrochim. Acta A Mol. Biomol. Spectrosc., 2005, 61, 2995-3001.10.1016/j.saa.2004.11.016Search in Google Scholar PubMed

[12] Jamróz M.H., Vibrational energy distribution analysis (VEDA): scopes and limitations. Spectrochim. Acta A Mol. Biomol. Spectrosc., 2013, 114, 220-230.10.1016/j.saa.2013.05.096Search in Google Scholar

[13] Dennington R., Keith T., Millam J., Eppinnett K., Hovell W., Gilliland R.G., Version 3.09, Semichem. Inc., Shawnee Mission, KS, 2003.Search in Google Scholar

[14] Fleming I., Frontier orbitals and organic chemical reactions, Wiley, 1977.Search in Google Scholar

[15] Kosar B., Albayrak C., Spectroscopic investigations and quantum chemical computational study of (E)-4-methoxy-2-[(p-tolylimino)methyl]phenol, Spectrochim. Acta A Mol. Biomol. Spectrosc., 2011, 78, 160-167.10.1016/j.saa.2010.09.016Search in Google Scholar

[16] Luque F., Orozco M., Bhadane P., Gadre S., SCRF calculation of the effect of water on the topology of the molecular electrostatic potential. J. Phys. Chem., 1993, 97, 9380-9384.10.1021/j100139a021Search in Google Scholar

[17] Murray J.S., Sen K., Molecular electrostatic potentials: concepts and applications, Elsevier, 1996, Vol. 3.Search in Google Scholar

[18] Alkorta I., Perez J.J., Molecular polarization potential maps of the nucleic acid bases, Int. J. Quantum Chem., 1996, 57, 123-135.10.1002/(SICI)1097-461X(1996)57:1<123::AID-QUA14>3.0.CO;2-9Search in Google Scholar

[19] Silverstein R.M., Webster F.X., Kiemle D.J., Bryce D.L., Spectrometric identification of organic compounds, John Wiley & Sons, USA, 2014.Search in Google Scholar

[20] Gorelsky S., SWizard Program Revision 4.5, University of Ottawa, Ottawa, Canada, 2010.Search in Google Scholar

[21] Bader R.F.W., Atoms in molecules, A quantum theory, Clarendon: Oxford, UK, 1990.Search in Google Scholar

[22] Biegler-Konig F., Schonbohm J., Bayles D., Software news and updates-AIM2000-A program to analyze and visualize atoms in molecules. John Wiley & Sons Inc. 605 Third Ave, New York, NY, USA, 2001, 22, 545-559.Search in Google Scholar

[23] Carroll M.T., Bader R.F., An analysis of the hydrogen bond in BASE-HF complexes using the theory of atoms in molecules, Mol. Phys., 1988, 65, 695-722.10.1080/00268978800101351Search in Google Scholar

[24] Koch U., Popelier P., Characterization of CHO hydrogen bonds on the basis of the charge density, J. Phys. Chem., 1995, 99, 9747-9754.10.1021/j100024a016Search in Google Scholar

[25] Carroll M.T., Chang C., Bader R.F., Prediction of the structures of hydrogen-bonded complexes using the Laplacian of the charge density, Mol. Phys., 1988, 63, 387-405.10.1080/00268978800100281Search in Google Scholar

[26] Socrates G., Infrared and Raman characteristic group frequencies: tables and charts, John Wiley & Sons, USA, 2004.Search in Google Scholar

[27] Colthup N., Introduction to infrared and Raman spectroscopy, Elsevier, 2012.Search in Google Scholar

[28] Jamróz M.H., Dobrowolski J.C., Brzozowski R., Vibrational modes of 2, 6-, 2, 7-, and 2, 3-diisopropylnaphthalene. A DFT study, J. Mol. Struct., 2006, 787, 172-183.10.1016/j.molstruc.2005.10.044Search in Google Scholar

[29] Madhavan V., Varghese H.T., Mathew S., Vinsova J., Panicker C.Y., FT-IR, FT-Raman and DFT calculations of 4-chloro-2-(3,4-dichlorophenylcarbamoyl) phenyl acetate, Spectrochim. Acta A Mol. Biomol. Spectrosc., 2009, 72, 547-553.10.1016/j.saa.2008.10.061Search in Google Scholar

[30] Umar Y., Density functional theory calculations of the internal rotations and vibrational spectra of 2-, 3-and 4-formyl pyridine., Spectrochim. Acta A Mol. Biomol. Spectrosc., 2009, 71, 1907-1913.10.1016/j.saa.2008.07.009Search in Google Scholar

[31] Shakila G., Periandy S., Ramalingam S., Molecular structure and vibrational analysis of 3-Ethylpyridine using ab initio HF and density functional theory (B3LYP) calculations, Spectrochim. Acta A Mol. Biomol. Spectrosc., 2011, 78, 732-739.10.1016/j.saa.2010.12.005Search in Google Scholar PubMed

Received: 2017-10-25
Accepted: 2017-12-02
Published Online: 2018-02-21

© 2018 Lamya H. Al-Wahaibi et al., published by De Gruyter

This work is licensed under the Creative Commons Attribution-NonCommercial-NoDerivatives 4.0 License.

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