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Volume 15, Issue 1

Issues

Volume 13 (2015)

Comprehensive spectroscopic (FT-IR, FT-Raman, 1H and 13C NMR) identification and computational studies on 1-acetyl-1H-indole-2,3-dione

Maha S. Almutairi
  • Department of Pharmaceutical Chemistry, College of Pharmacy, King Saud University, Riyadh 11451, Saudi Arabia
  • Other articles by this author:
  • De Gruyter OnlineGoogle Scholar
/ S. Muthu / Johanan C. Prasana / B. Chandralekha / Alwah R. Al-Ghamdi
  • Department of Pharmaceutical Chemistry, College of Pharmacy, King Saud University, Riyadh 11451, Saudi Arabia
  • Other articles by this author:
  • De Gruyter OnlineGoogle Scholar
/ Mohamed I. Attia
  • Corresponding author
  • Department of Pharmaceutical Chemistry, College of Pharmacy, King Saud University, Riyadh 11451, Saudi Arabia
  • Medicinal and Pharmaceutical Chemistry Department, Pharmaceutical and Drug Industries Research Division, National Researsh Centre (ID: 60014618), El Bohooth Street, Dokki, Giza 12622, Egypt
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  • Other articles by this author:
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Published Online: 2017-11-04 | DOI: https://doi.org/10.1515/chem-2017-0026

Abstract

Fourier transform infrared (FT-IR) and FT-Raman spectra of 1-acetyl-1H-indole-2,3-dione (N-acetylisatin) were recorded in the solid phase and analyzed. The molecular geometry, vibrational frequencies, infrared intensities, Raman activities and atomic charges were calculated using density functional theory (DFT/B3LYP) calculations with a standard 6-311++G(d,p) basis set. The fundamental vibrational modes of N-acetylisatin were analyzed and fully assigned with the aid of the recorded FT-IR and FT-Raman spectra. The simulated FT-IR and FT-Raman spectra showed good agreement with the experimental spectra. The stability of the molecule, arising from hyper-conjugative interactions and charge delocalization, was analyzed using natural bond orbital (NBO) analysis. The dipole moment (µ), polarization (α) and hyperpolarization (β) values of N-acetylisatin were also computed. The potential energy distribution (PED) was computed for the assignment of unambiguous vibrational fundamental modes. The HOMO and LUMO energy gap illustrated the chemical activity of N-acetylisatin. The energy and oscillator strength were calculated by DFT. Gauge–including atomic orbital NMR (1H and 13C) chemical shift calculations were performed and compared with the experimental values. Thermodynamic properties (heat capacity, entropy and enthalpy) of the compound at different temperatures were also calculated.

This article offers supplementary material which is provided at the end of the article.

Keywords: N-Acetylisatin; FT-IR; FT-Raman; DFT; NBO; HOMO-LUMO

1 Introduction

Isatin (1H-indole-2,3-dione) is an endogenous compound that has been known for about 150 years. It is an attractive substrate in both organic and medicinal chemistry as it constitutes the core structure of many bioactive molecules endowed with diverse biological activities for anticancer [1, 2] antibacterial [3, 4] antifungal [5] anti-HIV [6, 7] and anticonvulsant [8] applications.

The ease of synthetic accessibility of N-acetylisatins and their synthetic utility as precursors to prepare bioactive molecules bearing a glyoxylamide scaffold, gave them a respectable attention in different areas of chemistry including medicinal chemistry [9, 10, 11]. Ring opening of N-acetylisatin (Figure 1), via attack of its C2-carbonyl group with various amines, gives the corresponding glyoxylamide derivatives which have widespread applications in organic chemistry in addition to their incorporation in numerous biologically active molecules [12, 13, 14, 15].

Chemical structure of 1-acetyl-1H-indole-2,3-dione (N-acetylisatin).
Figure 1

Chemical structure of 1-acetyl-1H-indole-2,3-dione (N-acetylisatin).

To the best of our knowledge, the molecular structure of N-acetylisatin has not previously been investigated via computational approaches. Thus, the current study reports the spectroscopic analysis (FT-IR, FT-Raman and NMR) of N-acetylisatin with the aid of density functional theory (DFT) calculations in order to understand its structural geometry, inter- and intra-molecular interactions and hydrogen bonding. Moreover, the frontier molecular orbitals (HOMO-LUMO) were computed to predict structural changes and reactive sites. Hyperconjugative interactions and charge delocalization in N-acetylisatin were studied using natural bond orbital (NBO) analysis and the potential energy distribution (PED) was computed for the assignment of the unambiguous vibrational fundamental modes of N-acetylisatin. Thermodynamic properties (heat capacity, entropy and enthalpy) were also calculated at different temperatures.

2 Experimental Section

2.1 General

N-Acetylisatin was synthesized according to the literature procedure [16]. The FT-Raman spectrum of N-acetylisatin was recorded in the region of 4000 to 500 cm-1 in pure mode with a Nd:YAG laser of 100 mW with 2 cm-1 resolution on a Bruker RFS 27 at SAIF, IIT, Chennai, India. The FT-IR spectrum was also recorded in the region of 4000 to 500 cm-1 in evacuation mode using the KBr pellet technique with 1 cm-1 resolution on a Perkin Elmer FT-IR spectrophotometer. NMR (1H and 13C) spectra (Figures S1 and S2) were measured in DMSO-d6 on a Bruker NMR spectrometer (Ettlingen, Germany) operating at 500 MHz for 1H and 125.76 MHz for 13C at the Research Centre of the College of Pharmacy of King Saud University, Riyadh, Saudi Arabia. Chemical shifts are expressed in δ-values (ppm), relative to TMS as the internal standard.

2.2 Synthesis

Isatin (10 mmol) was suspended in acetic anhydride (10 mL) and the reaction mixture was heated under reflux for four hours. The cooled reaction mixture was filtered and the collected solid was dried under reduced pressure to give N-acetylisatin as yellow solid m.p. 79-81 °C in 85% yield. 1H-NMR (CDCl3): δ (ppm) 2.73 (s, 3H, CH3), 7.35 (t, J = 7.5 Hz, 1H, Ar-H), 7.71 (dd, 1H, J = 1.0, 8.5 Hz, Ar-H), 7.77 (d, J = 7.0 Hz, 1H, Ar-H), 8.40 (d, J = 8.5 Hz, 1H, Ar-H); 13C-NMR (CDCl3): δ (ppm) 26.5 (C14), 118.2 (C4), 119.2 (C8), 125.3 (C6), 126.2, (C5), 138.9 (C7), 148.6 (C9), 157.9 (C2), 169.7 (C12), 180.2 (C3).

2.3 Quantum Chemical Calculations

All quantum chemical density functional calculations, using the Becke three parameter (B3LYP) hybrid DFT level implemented with the standard 6-311++G(d,p) basis set, were carried out using Gaussian 03W [17] to optimize the molecular geometry. The optimized molecular geometry, corresponding to the minimum potential energy surface, was obtained by solving the self-consisting field equation iteratively. For the optimized structure of N-acetylisatin, no negative frequency modes were obtained, proving that a true potential energy minimum had been found. We utilized gradient corrected DFT with a three-parameter hybrid function (B3) for the exchange part of the calculations. Whereas, the Lee-Yang-Parr (LYP) correlation function [18] was accepted as an effective approach for the computation of the molecular structure, vibrational frequencies and energies of the optimized structures. By combining the results of the Gauss view program [19] with symmetry considerations, vibrational frequency assignments were made with a high degree of accuracy.

The calculated normal mode vibrational frequencies provided thermodynamic properties by the means of statistical mechanics. To improve the agreement between the predicted and observed frequencies, the computed harmonic frequencies were usually scaled for comparative purposes. The descriptions of the predicted frequencies during the scaling process followed the PED matrix. The vibrational frequency assignment was carried out by combining the results of the Gauss view program, symmetry considerations and the VEDA 4 program [20]. The NBO calculations were performed using the NBO 3.1 program as implemented in the Gaussian 03 package at the DFT/B3LYP level, in order to understand the intra-molecular delocalization or hyperconjugation. The NMR (1H and 13C) data was obtained from the DFT method using the 6-311++G(d,p) basis set. Characterization of the excited states and electronic transitions was performed using DFT on the corresponding optimized ground state geometries.

3 Results and Discussion

3.1 Molecular Geometry

The first aim of the computational work was to determine the optimized geometry of N-acetylisatin. The optimized molecular structure of N-acetylisatin, with numbering of the atoms, is shown in Figure 2. The optimized structural parameters such as bond lengths and angles were determined by the B3LYP method with 6-311++G(d,p) as the basis set. The geometry was considered on the basis of C1 point group symmetry.

Molecular structure of N-acetylisatin along with numbering of atoms.
Figure 2

Molecular structure of N-acetylisatin along with numbering of atoms.

All calculated geometrical parameters obtained using DFT are in good agreement with the experimental structural parameters [21]. Table 1 summarises the calculated and experimental geometrical parameters of N-acetylisatin. The optimized parameters are slightly different from the experimental ones which might be attributed to the fact that the experimental results are for the solid phase, while our theoretical calculations are for the isolated molecule in the gas phase. The heterocyclic ring is essentially planar, making a dihedral angle of 7.96° with the acetyl moiety. The C(2)-C(3) bond length of 1.583 Å is significantly longer than the expected value for a carbon (sp2)-(sp2) single bond (1.48 Å).

Table 1

Optimized geometrical parameters bond length, bond angle of the title molecule BYLYP/6-311++G(d,p) in comparison with experimental data.

3.2 Vibrational Spectral Analysis

Vibrational spectra are mainly determined by the modes of free molecules observed at higher wavenumbers and the lattice (translational and vibrational) modes in the low wavenumber region. Vibrational spectral assignment was performed for the recorded FT-IR and FT-Raman spectra based on the theoretically predicted wavenumbers by DFT and the results are presented in Table 2. N-Acetylisatin contains 21 atoms and therefore has 57 fundamental modes of vibration. All the vibrations were active in both the IR and Raman spectra. The vibrational band assignments were done on the basis of normal coordinate analysis [22] and the PED. None of the predicted vibrational spectra have imaginary frequencies. Discrepancies were corrected by implementing scaling calculations on the wavenumbers with factors of 0.983 and 0.958 for values below and above 1700 cm-1 above 1700 cm-1, respectively. The selected scaling factors were incorporated according to the SQM procedure using a set of 17 transferable scale factors. The PED was calculated by the VEDA 4 program [20]. The obtained experimental spectra and theoretical FT-IR and FT-Raman spectra of the title molecule are shown in Figures 3 and 4, respectively.

Experimental and calculated FT-IR of N-acetylisatin.
Figure 3

Experimental and calculated FT-IR of N-acetylisatin.

Experimental and calculated FT-Raman spectra of N-acetylisatin.
Figure 4

Experimental and calculated FT-Raman spectra of N-acetylisatin.

Table 2

Vibrational assignment of fundamental modes of N-acetylisatin along with calculated FT-IR, FT-Raman intensities and normal mode descriptions (characterized by PED) based on quantum mechanical force field calculations using the B3LYP6-311++G(d,p) method.

C-H Vibrations

The FT-IR spectra of the heteroatomic structures show the presence of C-H stretching vibrations in the region of 3100-3000 cm-1 [23], which is the characteristic region for the recognition of C-H stretching vibrations. In this region, bands are not considerably affected by the nature of the substituents. In the FT-IR spectrum of N-acetylisatin, bands were observed at 3130, 3072, 2972, 2994 and 2939 cm-1.

The FT-Raman modes are located in the range of 3215-3010 cm-1 with the B3LYP/6-311++G(d,p) method with a PED contribution of above 96%. As expected these modes are stretching modes, as is evident from the PED column in Table 2. FT-Raman bands were identified experimentally at 3130, 3082, 3054, 3021, 2995 and 2940 cm-1 due to C-H stretching vibrations.

The C-H in-plane and out-of-plane bending vibrations are normally present as a number of strong sharp bands in the regions of 1300-1000 and 1000-750 cm-1, respectively [24]. In the present work, the in-plane bending vibrations are observed at 1376, 1334, 1306, 1210, 1163, 1112, 1094, 1039 and 1012 cm-1 in the FT-IR spectrum and at 1379, 1334, 1307, 1263, 1215, 1172, 1152, 1100, 1042 and 1017 cm-1 in the FT-Raman spectrum. The theoretically computed frequencies for C-H vibrations by the B3LYP/6-311++G(d,p) method showed good agreement with the recorded spectra of the title molecule.

C=O and C-O Vibrations

The carbonyl bands are one of the most characteristic bands in IR spectra. Both the carbon and oxygen atoms of the carbonyl group move during bond vibration and they have nearly equal amplitudes. The carbonyl group is highly polar and therefore gives rise to an intense IR absorption band. The carbonyl frequencies can be altered by inter-molecular hydrogen bonding. The carbonyl band is reasonably easy to recognize due to its high intensity. However, it might overlap with other bands that are caused by aromatic vibrations meaning that their undisputed assignment is often difficult. A great deal of structural information can be derived from the exact position of the carbonyl group vibrations, which occur in the region of 1800-1700 cm-1 [25]. Also, Ibrahim et al. documented that the C=O stretching vibration occurs at 1768-1614 cm-1 and they have assigned a strong FT-IR band at 1703 cm-1 to be for a carboxyl C=O stretching vibration [26].

The C=O vibration bands in the FT-IR spectrum were observed at 1782 cm-1 for the ketone carbonyl (C3-O11), at 1751 cm-1 for the lactam carbonyl (C2-O10) and at 1711 cm-1 for the amide carbonyl (C12-O13) and they occurred at 1781, 1759 and 1704 cm-1 in its FT-Raman spectrum, respectively, with an 85% PED contribution. The calculated C=O vibration bands using B3LYP are in agreement with the experimentally determined bands in the FT-IR and FT-Raman spectra of the title compound and they are in accordance with the reported values [25, 26]

C-C Vibrations

The bands between 1650 and 1400 cm-1 in aromatic and heteroatomic compounds are assigned to carbon vibrations [27]. The actual positions are determined not by the nature of the substituents, but rather by the form of the substitution around the aromatic ring. The C-C stretching vibrations of N-acetylisatin were observed at 1592 and 1460 cm-1 in the FT-IR spectrum. In the FT-Raman spectrum, the vibrations were observed at 1610, 1592 and 1476 cm-1. Torsion CCCC, NCCC, ONCC and OCCC vibrations are presented in Table 2. The theoretically scaled vibrations also showed good agreement with the experimentally recorded data.

C-N Vibrations

The identification of C=N and C-N vibrations is a very difficult task, since the mixing of several modes is possible in this region [28]. The C-N stretching vibrations were observed at 1267 and 909 cm-1 in the FT-IR spectrum. In the FT-Raman spectrum, the vibrations were observed at 1263 and 930 cm-1. The theoretically scaled wave vibrations showed good agreement with the experimental data.

3.3 Natural bond orbital (NBO) analysis

NBO analysis provides the most accurate possible ‘natural Lewis structure’ picture of φ, because all orbital details are mathematically chosen to include the highest possible percentage of electron density. A useful aspect of the NBO method is that it gives information about interactions in both filled and virtual orbital spaces, which can enhance the analysis of intra- and inter-molecular interactions. The second Fock matrix was carried out to evaluate donor-acceptor interactions in the NBO analysis [29]. The interaction results in a loss of occupancy from the localized NBO of the idealized Lewis structure into an empty non-Lewis orbital. For each donor (i) and acceptor (j), the stabilization energy, E2, associated with the delocalization, ij, is estimated as: E2=ΔEij=qiF(i,j)2(ϵjϵi)(1)

where qi is the donor orbital frequency, εi and εj are diagonal elements and F(i, j) is the off diagonal NBO Fock matrix element.

NBO analysis provides an efficient method for studying intra- and inter-molecular binding and interactions between bonds and also provides a convenient basis for investigating charge transfer and conjugative interactions in molecular systems. Electron donor orbitals, acceptor orbitals and interacting stabilization energy, resulting from the second order micro-disturbance theory, were reported. The more intensive interaction between the electron donors and acceptors, i.e. more donating tendency from the electron donors to the electron acceptors, lead to a greater extent of conjugation in the whole system. Delocalization of the electron density between occupied Lewis-type (bond or lone pair) NBO orbitals and formally unoccupied (anti-bonding or Rydberg) non Lewis NBO orbitals corresponds to a stabilising donor-acceptor interaction. NBO analysis has been performed on the N-acetylisatin at the B3LYP/6-311++G(d,p) level in order to elucidate the intra-molecular re-hybridization and electron density delocalization within the molecule. The intra-molecular hyperconjugative interactions were formed by orbital overlap between σ and π(N-C, C-C, C-O and C-H) as well as between σ* and π*(N-C, C-C, C-O and C-H) bond orbitals, which results in an intra-molecular charge transfer, which stabilizes the system. These interactions were observed as an increase in electron density (ED) in the (N-C, C-C, C-O and C-H) anti-bonding orbitals, which weakened the respective bonds. The strong intra-molecular hyperconjugative interaction of the σ and π electrons of N-C, C-C, C-O and C-H to the N-C, C-C, C-O and C-H bonds of the ring led to the stabilization of some parts of the ring, as shown in Table S1. For example, the intra-molecular hyperconjugative interaction of N1-C2 distributes to σ*(N1-C9, N1-C12, C3-O11, C4-C9, C8-C9 and C12-C13) leading to a stabilization of 4.68 KJ/mol. This enhanced conjugation in the π bonding orbital (C7-C8) distributes to π*(C4-C9 and C5-C6) which leads to strong delocalization of 27.43 and 17.65 KJ/mol, respectively. The same kind of interactions have been calculated in the C3-O11, C4-C9, C5-C6 and C12-C13 bonds, as shown in Table S1. The stabilization energies associated with the hyperconjugative interactions, LP(1) O10-(C2-O10) and LP(l)-(N1-C2), are found to be 1.36 and 2.59 KJ/mol, respectively, as shown in Table S1, which act to extend the inter-molecular hydrogen bonding. The most important interaction energies, related to the resonance in the molecule, result from electron donation from the bonding donors, σ(C14-H19) and σ(C12-C14), to the bonding acceptor, σ*(C14-H21), with stabilization energies of 10.88 and 4.14 KJ/mol calculated, respectively.

3.4 Non Linear Optical (NLO) Effects

Non linear optical (NLO) effects arise from the interaction of electromagnetic fields in various media, which produces) new fields with altered phase, frequency, amplitude or other propagation characteristics [30]. The first order hyperpolarizability (β0) and related properties (β, α0 and Δα)of N-acetylisatin are calculated using the B3LYP/6-311++G(d, p) method based on the finite field approach. In the presence of an applied electric field, the energy of a system is a function of the electric field. First order hyperpolarizability is a third rank tensor that can be described using 3x3x3 matrices. The 27 components of the 3D matrix can be reduced to 10 components according to Kleinman symmetry [30]. These can be given in the lower tetrahedral format, as it is obvious that the lower parts of the 3x3x3 matrices are tetrahedral. The components of β are defined as the coefficients of a Taylor series expansion of the energy in an external electric field. When the external electric field is weak and homogeneous, the expansion becomes: E=E0μαFα1/2ααβFαFβ1/6βαβγFαFβFγ+(2)

where E0 is the energy of the unperturbed molecules, Fα is the field at the origin and µα, ααβ and βαβγ are the: components of the dipole moment, polarizability and first order hyperpolarizabilities, respectively. The total static dipole moment (µ), mean polarizability (α0) anisotropy of the polarizability (Δα) and mean first order hyperpolaraizability (β), using the x, y and z components, are defined as follows: μ=(μx2+μy2+μz2)1/2(3) Δα=21/2[(αχχαγγ)2+(αγγαzz)2+(αzzαxx)2+6αχχ2]1/2(4) μtot=μ0+αiEj+βijkEjEk+.....(5) αtot=αxx+αyy+αZZ3(6) βtot=βx2+βy2+βz2(7) βtot=(βxxx+βxyy+βxzz)2+(βyyy+βyzz+βxxy)2+(βzzz+βxxz+βyyz)2(8)

Since the values of the polarizabilities (α) and hyperpolarizabilities (β) from the Gaussian 03W output are reported in atomic units (a.u.), the calculated values have been converted into electrostatic units (esu). The dipole moment, first order hyperpolarizability and mean polarizability values are summarised in Table 3.

Table 3

NLO properties of N-acetylisatin.

3.5 Analysis of the Molecular Electrostatic Potential (MEP)

The mapping of the electrostatic potential onto the isoelectron density surface simultaneously displays the electrostatic potential (electron + nuclei) distribution, molecular shape, size and dipole moments of the molecule and it provides a visual method for understanding the relative polarity [31]. The total electron density and MEP surfaces of the molecule under investigation are constructed using the B3LYP/6-311++G(d,p) method (Figure 5). The charges, derived from an electrostatic potential computation, gave useful information about chemical reactivity. The electrostatic potential was computed by creating an electrostatic potential grid. These atomic point charges gave a better indication of the likely sites of attack.

Molecular electrostatic potential map of N-acetylisatin calculated at B3LYP/6 311++G(d,p) level.
Figure 5

Molecular electrostatic potential map of N-acetylisatin calculated at B3LYP/6 311++G(d,p) level.

The color scheme for the MEP surface is red for electron rich and partial negative charge regions, blue for electron deficient and partial positive charge regions, light blue for slightly electron deficient regions, yellow for slightly electron rich regions and green for neutral regions. The regions around the carbonyl groups (red) have the most negative potentials. The predominance of light green regions in the MEP surfaces corresponds to a potential balance between the two extremes, red and dark blue.

3.6 HOMO–LUMO Analysis

Both the highest occupied molecular orbitals (HOMO) and lowest unoccupied molecular orbitals (LUMO) play a role in the chemical stability of compounds [32]. The HOMO represents the ability to donate an electron, while the LUMO represents the ability to obtain an electron. The HOMO and LUMO energy values for N-acetylisatin, calculated by the B3LYP/6-311++G(d,p) method, are given in Table 4.

Table 4

HOMO-LUMO energies of N-acetylisatin.

Molecular orbitals can provide insight into the nature of reactivity and some of the structural and physical properties of molecules. The electronic transition absorption corresponds to the transition from the ground state to the first excited state, and is mainly described by a one electron excitation from the HOMO to the LUMO [33]. The energy gap between the HOMO and LUMO has been used to prove bioactivity from intra-molecular charge transfer. The frontier molecular orbitals are mainly composed of p atomic orbitals, so electronic transitions from the HOMO to LUMO are mainly derived from the electronic transition of π−π*. The energy gap demonstrates the kinetic stability of the molecules. A molecule with a small frontier orbital gap is more polarizable, which implies high chemical activity and low kinetic stability. The HOMO–LUMO energies and the orbital energy gaps for N-acetylisatin were calculated using the B3LYP/6-311++G(d,p) method and the pictorial representation of its frontier molecular orbitals is shown in Figure 6. The red and blue solid regions represent the molecular orbitals with completely opposite phases.

Frontier molecular orbitals of N-acetylisatin.
Figure 6

Frontier molecular orbitals of N-acetylisatin.

3.7 Local Reactivity Descriptors

The most relevant local descriptor of reactivity is the Fukui function, which is the derivative of the electronic chemical potential with respect to the external potential due to compensation of nuclear charges in the system. These reactivity indices are directly concerned with the selectivity of the molecule towards specific chemical events. The Fukui function of the system defines the more reactive regions in a molecule. Using Mulliken atomic charges of the neutral, cation and anion states of N-acetylisatin, Fukui functions (fk+;fk;fk0), local softness (sk+;sk;sk0) and local electrophilicity indices (ωk+;ωk;ωk0) are calculated [34, 35]. Fukui functions are calculated using the following equations: fk+=[q(N+1)q(N)]for nucleophilic attack(9) fk-=[q(N)q(N1)]for electrophilic attack(10) fk0=1/2[q(N+1)q(N1)]for radical attack(11)

Local soft ness and electrophilicity indices are calculated using the following equations: Sk+=Sfk+,Sk-=Sfk-,Sk0=Sfk0(12) ωk+=ωfk+,ωk-=ωfk-,ωk0=ωfk0(13)

where +, - and 0 show nucleophilic, electrophilic and radical attack, respectively.

Fukui functions, local softness and local electrophilicity indices for selected atomic sites in the title molecule are listed in Table 5. The maximum values of all three local electrophilic reactivity descriptors (fk+ ; Sk+ ; mk+) at atom H24 indicate that this site is prone to nucleophilic attack. In the same way, the maximum values of the nucleophilic reactivity descriptors (fk+ ; Sk+ ; mk+) at C6 indicate that this site is more prone to electrophilic attack [36].

Table 5

Mulliken population analysis, Fukui functions, local softness in eV, electrophilicity indices in eV for atoms of N-acetylisatin.

3.8 Mulliken Population Analysis

Mulliken atomic charge calculation has an important role in the application of quantum chemical calculations to molecular systems because atomic charges affect the dipole moment, molecular polarizability, electronic structure and a number of other properties of molecular systems [31]. The charge distribution over the atoms suggest the formation of donor and acceptor pairs involving charge transfer in the molecule. The Mulliken population analysis of N-acetylisatin is calculated using B3LYP with the 6-311++G(d,p) basis set and is presented in Table 5. It is noteworthy that the C4 atom of the title compound exhibited more positive charge, whereas the C3, C5, C6, C7, C8, C10, C11, C13 and C14 atoms exhibited negative charges. The N1, C2, C4, C9, O12 and H15-H21 atoms exhibited only positive charges. The charge on H18 has the maximum magnitude of 0.29381 among the hydrogen atoms and C8 has the least magnitude in the molecule. However, H15-H21 atoms possess positive charge distributions due to the large negative charges on the carbon atoms. The charge distribution of N-acetylisatin is shown in Figure 7.

Mulliken population analysis of N-acetylisatin.
Figure 7

Mulliken population analysis of N-acetylisatin.

3.9 Thermodynamic Properties

The total energy of a molecule is the sum of the translational, rotational, vibrational and electronic energies, i.e. E = Et + Er + Ev + Ee. A statistical thermochemical analysis of N-acetylisatin was carried out with the assumption of room temperature and one atmospheric pressure. On the basis of vibrational analysis and statistical thermodynamics, the standard thermodynamic functions, heat capacity (C0p,m), entropy (S0m), and enthalpy (H0m) were obtained and are listed in Table 6. C0p,m, S0p,m and H0m all increased with increasing temperature from 100 to 1000 K. This might be attributed to the enhancement of the molecular vibration as a result of increasing temperature [37]. The corresponding fitting factors (R2) for these thermodynamic properties are 0.9996, 0.99996 and 0.99934, respectively. The correlation between these thermodynamic properties and temperature is shown in Figure 8 and the equations are given below: C0p,m=14.96578+0.67679T2.94375×104T2;(R2=0.9996)(14) S0m=233.81496+0.75417T1.86536×104T2;(R2=0.99996)(15) H0p,m=8.29573+0.09023T+1.76561×104T2;(R2=0.99934)(16)

Correlation graphs of thermodynamic properties at different temperature of N-acetylisatin.
Figure 8

Correlation graphs of thermodynamic properties at different temperature of N-acetylisatin.

Table 6

Thermodynamic properties for N-acetylisatin obtained by B3LYP/6-311++G(d,p) method.

These equations could be used for further studies of N-acetylisatin. For instance, when we investigate the interaction between N-acetylisatin and another compound, the thermodynamic properties could be obtained from these equations and then used to calculate the change in the Gibbs free energy of the reaction, which will help us to judge the spontaneity of the reaction.

They can also be used to compute other thermodynamic functions and estimate the directions of chemical reactions according to the second law of thermodynamics. All thermodynamic calculations were performed for the gas phase. Scale factors have been recommended [38] for accurate prediction of the zero-point vibration energies, heat capacities, entropies and enthalpies.

3.10 NMR Spectral Analysis

Isotropic chemical shifts are frequently used as an aid for the identification of reactive organic species. It is recognized that accurate prediction of molecular geometry is essential for reliable calculations of magnetic properties. Therefore, full geometry optimization of N-acetylisatin was performed using the B3LYP/6-311++G(d,p) method. Then, Gauge-including atomic orbital 1H and 13C chemical shift calculations of N-acetylisatin were carried out using the same method. Such density functional methodologies offer an effective calculation method due to their low computational cost. The experimental and calculated NMR chemical shift values for N-acetylisatin are summarised in Table 7. The 1H chemical shifts for N-acetylisatin were obtained by the complete analysis of its 1H-NMR spectrum and interpreted critically in an attempt to understand the possible different effects acting on the shielding constants of the protons. The 1H NMR spectrum was assigned according to the coupling pattern and constants. Additionally, the chemical shift value for C3 in N-acetylisatin was observed at higher value (180.16 ppm) than all other carbon atoms (26.45-169.71 ppm).

Table 7

Experimental and computed NMR (13C and 1H) chemical shifts of t N-acetylisatin using B3LYP/6-311++G(d,p).

4 Conclusions

In this investigation, the optimized molecular structure, thermodynamic, electronic, vibrational and spectroscopic properties of 1-acetyl-1H-indole-2,3-dione (N-acetylisatin) were calculated by DFT using the B3LYP/6-311++G(d,p) method. The optimized geometric parameters (bond lengths and angles) were theoretically determined by DFT and compared with the experimental values. Vibrational FT-IR and FT-Raman spectra were recorded. On the basis of agreement between the calculated and experimental results, the assignment of all fundamental vibrational modes of N-acetylisatin was carried out based on the results of the PED output obtained from normal coordinate analysis. NBO analysis indicated the intra-molecular charge transfer between the bonding and anti-bonding orbitals. In addition, the electric dipole moment, polarizabilities and the hyperpolarizabilities were calculated by the B3LYP/6-311++G(d,p) method. The MEP and HOMO-LUMO energy separation indicated the kinetic stability of N-acetylisatin. The HOMO-LUMO energy gap reflected the chemical activity of N-acetylisatin. Orbital energy interactions between selected functional groups were analyzed by the density of states. Fukui functions, local softness and electrophilicity indices for selected atomic sites in the title compound were calculated. Calculated and experimental NMR chemical shift values were also compared. In summary, the experimental data, along with the simulations, have allowed for the integrated characterization of N-acetylisatin.

Supplementary information

Figures S1 and S2 as well as Table S1 are provided as supporting information.

Acknowledgement

The authors would like to extend their sincere appreciation to the Deanship of Scientific Research at King Saud University for its funding of this research through the Research Group Project no. RGP-196.

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Footnotes

    About the article

    Received: 2017-08-10

    Accepted: 2017-09-20

    Published Online: 2017-11-04


    Citation Information: Open Chemistry, Volume 15, Issue 1, Pages 225–237, ISSN (Online) 2391-5420, DOI: https://doi.org/10.1515/chem-2017-0026.

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    © 2017 Maha S. Alumutairi et al. This work is licensed under the Creative Commons Attribution-NonCommercial-NoDerivatives 4.0 License. BY-NC-ND 4.0

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