Research Article - (2016) Volume 7, Issue 1

FT-IR and FT-Raman Spectral Investigation and DFT Computations of Pharmaceutical Important Molecule: Ethyl 2-(4-Benzoyl-2,5- Dimethylphenoxy) Acetate

Amalanathan M1*, Suresh DM2, Hubert Joe I3, Bena Jothy V4, Sebastian S5 and Ayyapan S6
1Annai Velankanni College, Department of Physics, Tholayavattam, Tamil Nadu, India
2Department of Physics, Government Arts College, Ushagamandalam, Tamil Nadu, India
3Centre for Molecular and Biophysics Research, Department of Physics, Mar Ivanios College, Thiruvananthapuram, Kerala, India
4Department of Physics, Women’s Christian College, Nagercoil, Tamil Nadu, India
5P.G and Research Department of Physics, St.Joseph’s College of Arts and Science (Autonomous), Cuddalore, India
6Government College of Technology, Coimbatore 641 013, India
*Corresponding Author: Amalanathan M, Annai Velankanni College, Department of Physics, Tholayavattam, Tamil Nadu, India, Tel: +91-9940347178 Email:


The vibrational contribution studies of Pharmaceutical activity of Ethyl 2-(4-benzoyl-2,5-dimethylphenoxy)acetate (EBDA) have been performed using FTIR, FT-Raman analysis. More support on the experimental findings were added from the quantum chemical studies performed with DFT (B3LYP) method using 6-311++G (d, p) basis sets. The observed FT-IR and FT-Raman spectra have been compared with the calculated theoretical data. The calculated vibrational data have also been found in good agreement with the experimental results. Natural bond orbital analysis revealed important details of the electronic structure and dominant intramolecular interactions in Ethyl 2-(4-benzoyl-2,5-dimethylphenoxy)acetate. The HOMO and LUMO analysis reveals the possibility of charge transfer within the molecule and the possibility of Pharmaceutical activity of EBDA molecule. In addition, molecular electrostatic potential (MEP), charge analysis also were investigated using theoretical calculations.

Keywords: Vibrational spectra; DFT; NBO; PED; HOMO-LUMO; Pharmaceutical important


Phenoxyacetic acid, a well-known aryloxyacetic acid, which is useful in the treatment of insulin resistance, and hyperglycaemia, has been investigated by various researchers [1-3]. Phenoxyacetic acid and substituted phenoxyacetic acids have potential biological properties and so these acids are widely used in herbicides [4] and pesticides [5] formulations. Antimicro-bioactivity [6], anticancer, antitumor, analgesic, anti-inflammatory, plant growth regulation and inhibition of tillage are also some of its reported properties. Hydroxy benzophenones can be attained from natural products [7,8] and also by synthetic methods [9-11]. The enormous importance of these substances is essentially due to the diverse biological and chemical properties they acquire. Benzophenone analogues with nitro substituent exhibit significant in vivo antitumor activity and they have been reported to show activity such as immune modulators [12]. The title compound Ethyl 2-(4-benzoyl-2, 5-dimethylphenoxy) acetate (EBDA), has been synthesized via Fries rearrangement of hydroxy benzophenone [13].

In recent years, there has been an increasing interest in the application of DFT calculations to pharmaceutical drugs as calculations provide additional interpretation of the vibrational spectroscopic data collected [14-17]. During the past decade, DFT [18] has been accepted by the ab initio quantum chemistry community as a popular approach for the computation of molecular structure, vibrational frequencies and energies of chemical reactions. Calculation of vibrational frequencies using DFT provides a promising cost effective approach for calculating vibrational spectra of large molecules. In recent theoretical studies, the harmonic vibrational frequencies for a larger number of small and well studied organic molecules have been computed with HF, MP2 and DFT methods [19-21].

Vibrational spectroscopy is highly sensitive to the structural changes and is useful for the study of the pharmacological properties [22,23]. Accordingly, in order to understand the relationship between molecular structure and biological activity, the knowledge of the electronic structure and complete vibrational spectra are particularly important. Information about the geometry and structure of the molecule and its electrostatic potential surfaces, together with a complete analysis of the vibrational spectra using Raman and infrared techniques, based on frequency, intensity and potential energy distribution over the internal coordinates helps in understanding the structural and spectral characteristics, by allowing us to obtain a quantitative as well as qualitative understanding of energy distribution. ab initio HF and DFT calculations have been independently performed as they form the basis of the assignment of the vibrational spectrum.

The present work deals with the optimization of molecular structure and analysing the vibrational spectra using FT-Raman and FT-IR techniques for the title compound and comparing them with the theoretical Raman and IR spectra computed by DFT method. Calculated Potential energy distribution enables to make a detailed assignment of the vibrational spectra. Natural bond orbital analysis has been performed to identify the possible intra- and inter- molecular interactions present in the compound. HOMO-LUMO energy gap calculated confirms the occurrence of charge transfer interaction. Electrostatic potential analysis has also been made to identify the mapping surface of the molecule.

Materials and Methods


Molecular structure, vibrational frequencies and energies of optimized geometries have been computed employing DFT [24] with Gaussian ‘09 program package [25] using Becke’s three parameter hybrid exchange functional with Lee-Yang-Parr correlation functional (B3LYP) [26-28] as a cost effective approach. The basis set 6-311++G (d, p) augmented by ‘d’ polarization functions on heavy atoms and ‘p’ polarization functions on hydrogen atoms have been used [29,30]. Absolute Raman intensities and infrared absorption intensities have been calculated with harmonic approximation at the same level of theory as used for optimized geometries from the derivatives of polarizability and dipole moment associated with each normal mode. Owing to the complexity of the molecule, Potential Energy Distribution has been carried out to obtain complete information of the molecular motions involved in the normal modes. The experimentally observed spectral data of the compound are found to be in good agreement with the spectral data obtained by quantum chemical calculations.

The vibrational modes have been assigned on the basis of PED analysis using VEDA program [31]. Vibrational wave numbers calculated have been scaled [32] with the scale factor in order to figure out how the calculated data are in agreement with those of the experimental ones. Calculated vibrational frequencies have been scaled down by using the scaling factor [32] to offset the systematic error caused by neglecting anharmonicity and electron density. Raman activities (Si) calculated have been converted to relative Raman intensities (Ii) using the following relationship derived from the basic theory of Raman scattering [33,34] .


where υo is the exciting frequency ( in cm-1 units), υi is the vibrational wave number of the ith normal mode, h, c and k are universal constants, and S is the suitably chosen common scaling factor for all the peak intensities.


The infrared spectrum of the sample was recorded between 4000 and 400 cm-1 on a Mattson 1000 FT-IR spectrometer which was calibrated using polystyrene bands. The sample was prepared as a KBr disc. FT-Raman spectrum of the sample was recorded between the region 3500 and 50 cm-1 on a Bruker FRA 106/S FT-Raman instrument using 1064 nm excitation from an Nd: YAG laser. The detector used was a liquid nitrogen cooled Ge detector.

Results and Discussion

Optimized geometry

Initial geometry generated from standard geometrical parameters was optimized and equilibrium geometry has been determined by the energy minimization. The ground state optimized structure of the molecule is presented in Figure 1. The optimized structure of EBDA and experimental structure of EBDA [13] were compared. The agreement between the optimized and experimental crystal structure is quite good showing that the geometry optimization almost exactly reproduces the experimental conformation (Figure 1) (Table 1).


Figure 1: Optimized molecular structure of EBDA.

Bond length Value(Å) Angle Value(/°) Dihedral angles Value(/°)
C1-C2 1.407 C1-C2-C3 117.0 C1-C2-C3-C4 1.37
C2-C3 1.387 C2-C3-C4 123.2 C2-C3-C4-C5 -0.42
C3-C4 1.407 C3-C4-C5 119.1 C3-C4-C5-C6 -1.14
C4-C5 1.409 C4-C5-C6 118.1 C6-C1-C2-C7 179.33
C5-C6 1.399 C1-C2-C7 120.6 C3-C2-C7-H8 -0.66
C2-C7 1.506 C2-C7-H8 110.6 C3-C2-C7-H9 120.02
C7-H8 1.091 C2-C7-H9 111.2 C3-C2-C7-H10 -121.56
C7-H9 1.094 C2-C7H10 111.3 C1-C2-C3-H11 179.73
C7-H10 1.094 C2-C3-H11 118.0 C2-C3-C4-C12 175.6
C3-H11 1.084 C3-C4-C12 119.5 C3-C4-C12-O13 -142.36
C4-C12 1.494 C4-C12-O13 121.2 C3-C4-C5-C14 179.41
C12-O13 1.223 C4-C5-C14 123.4 C4-C5-C14-H15 42.79
C5-C14 1.511 C5-C14-H15 112.1 C2-C5-C14-H16 -75.76
C14-H15 1.091 C5-C14-H16 110.9 C4- C5-C14-H17 163.87
C14-H16 1.092 C5-C14-H17 110.3 C4-C5-C6-H18 -178.64
C14-H17 1.092 C5-C6-H18 118.1 C3-C4-C12-C19 37.37
C6-H18 1.082 C4-C12-C19 119.6 C4-C12-C19-C20 32.08
C12-C19 1.505 C12-C19-C20 122.6 C12-C19-C20-C21 176.14
C19-C20 1.401 C19-C20-C21 120.4 C19-C20-C21-C22 0.9
C20-C21 1.394 C20-C21-C22 120.1 C20-C21-C22-C23 -0.89
C21-C22 1.394 C21-C22-C23 119.9 C4-C12-C19-C24 -151.92
C22-C23 1.396 C12-C19-C24 118.2 C12-C19-C20-H25 -2.63
C19-C24 1.402 C19-C20-H25 119.9 C19-C20-C21-H26 -179.03
C20-H25 1.083 C20-C21-H26 119.8 C20- C21-C22-H27 179.4
C21-H26 1.084 C21-C22-H27 120.0 C21-C22-C23-H28 -179.81
C22-H27 1.084 C22-C23-H28 120.0 C22-C23-C24-H29 -178.49
C23-H28 1.084 C23-C24-H29 120.9 C3-C2-C1-O30 179.15
C24-H29 1.083 C2-C1-O30 115.1 C2-C1-C30-C31 179.02
C1-O30 1.366 C1-C30-C31 119.1 C1-C30-C31-H32 60.08
C30-C31 1.408 C30-C31-H32 111.7 C1-C30-C31-H33 -60.77
C31-H32 1.097 C30-C31-H33 111.7 C1-C30-C31-C34 179.4
C31-H33 1.096 C30-C31-C34 108.7 C30-C31-C34-O35 -3.75
C31-C34 1.522 C31-C34-O35 126.4 C30-C31-C34-O36 176.59
C34-O35 1.2 C31-C34-O36 108.6 C31-C34-C36-C37 179.3
C34-O36 1.347 C34-C36-C37 116.6 C34-C36-C37-H38 -60.27
C36-C37 1.453 C36-C37-H38 108.4 C34-C36-C37-H39 56.65
C37-H38 1.092 C36-C37-H39 108.4 C34-C36-C37-C40 178.22
C37-H39 1.092 C36-C37-C40 107.6 C36-C37-C40-H41 179.88
C37-C40 1.514 C37-C40-H41 109.5 C36-C37-C40-H42 -60.6
C40-H41 1.093 C37-C40-H42 111.1 C36-C37-C40-H43 60.32
C40-H42 1.092 C37-C40-H43 111.1    
C40-H43 1.092        

Table 1: Optimized parameters of EBDA on B3LYP/6-31++G(d,p) level.

The relative energies of the molecule have been calculated employing ab initio functions and DFT functional (B3LYP). The optimized structural parameters (bond lengths, bond angles, dihedral angle) have been compared with those obtained experimentally for the EBDA as shown in Table 1. The table reveals that, all the theoretical values agree well with the experimental values. Calculated C-H bond length is around 1.08 Å, while the experimental value from the neutron diffraction method is 0.93 Å.The difference in C-H bond is due to experimental values taken from X-ray diffraction method that is solid phase, but the theoretical method is the gas phase. From the above figure it is seen that the EBDA molecule consists of mono substituted phenyl ring (Ph1), Tetra substituted phenyl ring (Ph2), three methyl groups and two methylene groups. Table shows that the bond length of C12-O13 and C34-O35 varies from 1.20 Å-1.22 Å whereas the bond length of C1-O30 and C34-O36 varies from 1.34 Å-1.36 Å, which substantiate the single bond and double bond nature of carbonyl group. The C-C bond length of C5-C14 and C20-C7 is around 1.50 Å while the normal C-C bond length is 1.40 Å. The increase in bond length from the normal value is due to electron transfer from a ring (Ph2) to the methyl group. EBDBA molecular structure is shown as a non planer surface due to the twisting between Ph1 to Ph2 and this twisting takes place due to the steric repulsion between the ring hydrogen H25 and H11. From the table, it is seen that all the experimental bond angles are in good agreement with the theoretical values.

The decrease in endocyclic angles C23-C22-C21 and C20-C19-C24 from the normal value shows the electron with drawing nature of ring. The endocyclic angle of Ph2, C4-C5-C6 (118.13°) is decreased and the exocyclic angle, C4-C5-C14 (123.384°) is increased from the normal value which confirms the heavy substitution of the ring. Similarly the endocyclic angle C3-C2-C1 (116.99°) and exocyclic angle C3-C2-C7 (122.42°) shows that the methyl substitution of the ring Ph2 is at the para position.

NBO Analysis

NBO analysis has been proved to be an effective tool for chemical interpretation of hyper conjugative interaction and electron density transfer (EDT) from filled lone electron pairs of the n(Y) of the ‘‘Lewis base’’ Y into the unfilled anti bond σ*(X-H) of the ‘‘Lewis acid’’ X-H in X-H…..Y hydrogen bonding systems [35]. Also, in order to obtain structure of molecule, the main natural orbital interactions have been analyzed with the NBO 5.0 program [36]. Lowering of the orbital energy due to the interaction between the doubly occupied orbital and the unoccupied ones is a very convenient guide to interpret the molecular structure. In energy terms, hyper conjugation is an important effect [37,38] in which an occupied Lewis-type natural bond orbital is stabilized by overlapping with a non Lewis-type orbital. This electron delocalization can be described as a charge transfer from a Lewis valence orbital (donor), with a decrease of its occupancy, to a non-Lewis orbital (acceptor). Several other types of valuable data, such as directionality, hybridization and partial charges, were analyzed in the output of NBO analysis.

Table 2 gives the second-order perturbation energy values, Eij(2) corresponding to the interactions and the overlap integral of each orbital pair. From the analysis, it is seen that the intermolecular C-H….O Hydrogen bonding is formed due to the overlap between the LPO13 and σ* (C14-H17) which result in ICT causing stabilization of the Hydrogen bond system. The NBO analysis of EBDA clearly shows the evidence of the formation H-bonded interaction between oxygen lone pairs and σ* (C14-H17) antibonding orbital having stabilization energy 99.84 KJ/mol (Table 2).

Donar (i) Acceptor (j) E(2)a (KJ/mol) E(j)-E(i)b a.u. F(ij)c a.u
π(C1-C6) π*(C2-C3) 23.38 0.22 0.065
π(C1-C6) π*(C4-C5) 22.95 0.30 0.075
σ(C1-O30) σ*(C7-H9) 1657.20 0.03 0.192
σ(C1-O30) σ*(C12-C19) 1422.18 0.03 0.192
σ(C3-C4) π*(C19-C20) 3731.85 o.59 1.451
π(C4-C5) π*(C2-C3) 29.89 0.20 0.070
π(C4-C5) π*(C12-O13) 33.40 0.10 0.055
π(C19-C20) σ*(C5-C14) 269.28 0.57 0.385
π(C19-C20) σ*(C7-H10) 84.75 0.82 0.259
π(C19-C20) π*(C12-O13) 213.41 0.46 0.293
π(C19-C20)) σ*(C14-H15) 231.89 0.65 0.382
π(C19-C20)) σ*(C14-H17) 1148.22 0.24 0.512
π(C19-C20)) σ*(C31-H32) 108.98 0.72 0.275
π(C19-C20)) σ*(C31-H33) 103.63 0.74 0.271
π(C19-C20)) σ*(C31-C34) 518.18 0.37 0.422
LP(2)O35 σ*(C31-C34) 296.83 0.05 0.111
LP(2)O35 σ*(C34-O36) 30.98 0.65 0.129
LP(1)O13 σ*(C14-H16) 99.84 0.23 0.136
LP(2)O36 π*(C34-O35) 43.91 0.36 0.112

Table 2: Second order perturbation theory analysis of Fock matrix in NBO basis for EBDA.

The larger the E(2) values, the more intensive is the interaction between the electron donors and the electron acceptors. Among the most energetic donor acceptor NBO interactions, those involving p-type lone pair of oxygen atom, σ(C40-H43) with σ* (C14-H17) antibonding have energy contributions 4661.89KJ-mol-1 which shows the intermolecular dislocations in EBDA. The intermolecular hyper conjugative interactions are formed by the orbital overlap between π(C-C) and π*(C-C) bond orbital’s, which results in intermolecular charge transfer (ICT) and causes stabilization of system. Table shows the most important interactions between Lewis and non- Lewis orbital with oxygen lone pairs and the second order perturbation energy values E (2) corresponding to this interaction. From the Table 2. it is seen that a very strong interaction between the p-type orbital containing the lone electron pair of O35 and neighbour σ*(C31-C34) anti bonding orbital exists.

Vibrational analysis

The vibrational spectral analysis was performed on the basis of the characteristic vibrations of the amino group, hydroxyl group, carbonyl group and methyl group. The computed wave numbers, their IR intensities and Raman activity corresponding to different modes are listed in Table 3 along with detailed assignments. The observed and simulated FT-IR and FT-Raman spectra and selected vibrational normal modes are shown in Figures 2 and 3.


Figure 2: Experimental and (b) simulated FT-IR spectra of EBDA in the range 4000-400 cm-1.


Figure 3: (a) Experimental and (b) simulated FT-Raman spectra of EBDA in the range 3500-50 cm-1.

CalFreq. Exp IR Exp. Raman TED (%)
3091 - 3106 w υC-H ar in ring 1 (88)
3087 3086 w 3083 w υC-H ar in ring 1 (88)
3086 - - υC-H ar in ring 2 (45)
3078 - - υC-H ar in rin(88)g 1(83)
3073 - 3072 w υC-H ar in ring 2 (96)
3068 3060 w - υC-H ar in ring 1 (82)
3058 3045 w 3052 w υC-H ar in ring 1 (87)
3015 - 3023 w C37-H2 Asym Stretching (96)
3006 - 3005 w Me1 Asym. Stretching (90)
3006 - - Me1 Asym. Stretching (96)
3002 - - Me3 Asym. Stretching (95)
2997 - - C31-H2 Sym. Stretching (97)
2989 - 2986 w Me2 Asym. Stretching (95)
2979 2960 w 2968 w Me3 Asym. Stretching (99)
2955 - 2952 w C31-H2 Sym. Stretching (98)
2946 - - C31-H2 Asym Stretching C31H2 Sym. Stretching (97)
2939 - - Me2 Sym. Stretching C31H2 Sym. Stretching (98)
2938 -   Me3 Sym. Stretching C31H2 Sym. Stretching (99)
2931 2930 w 2930 w Me1 Sym. Stretching (84)
2909 - 2895 w C31-H2 Sym Stretching (98)
1764 1750 s - C34-O35 Stretching (90)
1647 1640 m - C12-O13 Stretching (85)
1589 1600 m - υC-C ar in ring 2 (45)
1582 1580 m - υC-C ar in ring 1 (67)
1563 1558 m 1555 w υC-C ar in ring 1 (47)
1541 - - υC-C ar in ring 2 (57)
1483 1500 m 1501 w υC-C ar in ring 2 (49)
1469 - - C37-H2 Sissoring (86)
1467 - - υC-C ar in ring 2 (71)
1449 - - Me1, Me2 Asym.Bending (67)
1448 - - Me3 Asym.Bending (63)
1439 1440 m - C31-H2 Sissoring (72)
1438 - - Me3 Asym. Bending (61)
1435 - - C31-H2 Sissoring (66)
1428 - - Me1, Me2 Asym. Bending (77)
1428 - - Me1, Me2 Asym. Bending (64)
1426 - - δC-H ar in ring 1 (20)
1385 - - C37-H2 Wagging (28)
1377 1380 m - Me1 Sym. Bending (60)
1373 - - Me2 Sym. Bending (75)
1369 - - C31-H2 Wagging (33)
1359 - - Me1 Sym. Bending (23)
1348 - - δC-H ar in ring 2 (65)
1306 1310 s - δC-H ar in ring 2 (75)
1303 - - υC-C ar in ring 1 (26)
1288 1280 s - δC-H ar in ring 2 (63)
1265 - - C37-H2 Twisting (49)
1256 1258 s - δC-H ar in ring 2 (76)
1243 - - δC-H in ring 1 (69)
1236 - - C31-H2 Twisting (42)
1218 1200 vs - δC-H ar in ring 2 (88)
1171 - - C31-H2 Rocking (38)
1170 - - δC-H ar in ring 1 (51)
1162 - - δC-H ar in ring 1 (46)
1149 1157 vs 1152 m δC-H ar in ring 2 (41)
1143 - - δC-H ar in ring 2 (79)
1137 1120 vvs 1132 m C37-H2 Twisting (76)
1098 - 1100 m C37-H2 Rocking (70)
1092 - - δC-H ar in ring 1 (40)
1067 1070 s - δC-H ar in ring 1 (71)
1041 - -
C5-C14 Stretch (28)
1028 - - Me1 Bending (77)
1019 - - Me2 Bending (61)
1013 1014 s   δC-H ar in ring 1 (42)
1011 - - Me2 Bending (41)
1001 - - Me3 Bending (65)
1000   991 vvs C37-H2 Rocking (66)
983 - - Radial skel. in ring 1 (36)
982 - - Me2 Bending (44)
975 977 m - δC-H ar in ring 1 (79)
962 - - δC-H ar in ring 1 (86)
923 - - δC-H ar in ring 2(52)
922 - - δC-H ar in ring 1 δC-H ar in ring 1 (66)
901 - - δC-H ar in ring 2 δC-H ar in ring 1 (50)
888 899 m 881 w δC-H in ring 2 δC-H ar in ring 1 (36)
852 m 854 m - Me1 out of plane δC-H ar in ring 1 (76)
834 m 834 m - Me2 out of plane δC-H ar in ring 1 (94)
828 w - - δC-H ar in ring 2 (82)
807 w - 805 w δC-H in ring 1 (17)
791 w - - δC-H ar in ring 2 (27)
787 w 764 w 769 Me3 out of plane Bending (88)
741 w 751 w 755 w Radial skel. in ring 2 (29)
726 w - - δC-H ar in ring 2 (37)
699 w - - Radial skel. in ring 2 (34)
695 w - - δC-H ar in ring 2 (38)
685 w 686 vvw 684 w OP skel. in ring 1 (54)
667 w - 647 w Radial skel. in ring 1 (42)
630 637 w 632 w OP skel. in ring 2 (25)
611 615 s 619 w 6b Radial skel. in ring 1
590 - - OP skel. in ring 2 (29)
586 - - OP skel. in ring 2 (25)
563 - 575 w OP skel. in ring 2 (23)
508 516 w 543 w OP ring 1 (26)
457 470 vw 466 w C2-C7 stretching (40)
450 445 vw 450 w OP ring 1 (21)
436 - - OP ring 2 (53)
409 416 vw - OP ring 1 (58)
401 - - OP ring 1 (78)
384 - - OP ring 2 (30)
367 - 377 w OP ring 1 (29)
340 - 347 w C-C Bending (29)
318 - - Me1 Torsion (39)
267 - - Me2 Torsion (61)
255 - - Me3 Torsion (59)
252 - 248 w Me2 Torsion (18)
247 - - OP ring 1 (43)
209 - - OP ring 1 (46)
186 - 186 w OP ring 1 (48)
171 - - OP ring 2 (28)
150 - 158 w C-O Bending (61)
147 - - C-O Bending (66)
143 - - C-O out of plane Bending (72)
132   134 w OP ring 2 (47)
120   119 w OP ring 2 (59)
103     OP ring 1(71)
90   83 w OP ring 2 (21)
64     C-O out of plane Bending (51)
59     C-O out of plane Bending (36)
53     OP ring 2 (51)
44     OP ring 2 (55)
32     OP ring 2 (50)
22     C-O out of plane Bending (76)
15     OP ring 2 (73)

Table 3: Calculated and observed vibrational frequencies for EBDA and their tentative assignment.

Phenyl ring vibrations: The hetero aromatic structure shows the presence of C-H stretching vibration in the region of 3100-3000 cm-1 which is the characteristic region for the ready identification of C-H stretching vibration [39]. In this region, the bands are not affected appreciably by the nature of the substituent. The C-H stretching modes usually appear with strong Raman intensity and are highly polarized. Owing to this high polarization, Raman bands have not been observed in the experimental spectra. The observed weak band in IR at 3086 cm-1 and in Raman at 3106 and 3083 cm-1 are assigned to the C-H stretching mode of ring 1. The same mode observed in IR at 3060 and 3045 cm-1 and in Raman at 3072 and 3052 cm-1 is assigned for ring 2 (Figures 2 and 3) (Table 3).

PED corresponding to this vibration is a pure mode as it is evident from the contribution of ~ 100%. The C-H stretching anharmonic wave number lies between 3100 and 3000 cm-1. The C-H in-plane bending frequencies appear in the range of 1000-1300 cm-1 and are very useful for characterization purposes [39]. The observed series of strong bands in IR at 1310, 1280, 1258, 1200, 1157 cm-1 is assigned to the C-H inplane bending vibration of phenyl ring 2. The observed strong bands at 1070, 1014 cm-1 in IR are assigned to the C-H in plane bending vibration of phenyl ring 1. The same mode of vibration of ring 2 is observed in Raman at 1152 cm-1 as a medium band. PED confirms that these vibrations are of mixed mode as is evident from the table.

The C-H out of plane bending vibrations is strongly coupled vibrations and occurs in the region of 1000-750 cm-1 [40,41]. The aromatic C-H out-of-plane bending vibrations of EBDA are assigned to the bands observed at 898 and 803 cm-1 in the FT-IR spectrum which is well correlated with the B3LYP method as shown in table with a PED contribution of ~ 70-90%. Also the bands in the FT-IR spectrum, at 899, 764 cm-1 and in FT-Raman spectrum at 881 and 805 cm-1 are assigned to C-H stretching vibrations. Benzene ring possesses six stretching vibrations, of which four occur near the highest wave number 1600, 1580, 1490 and 1440 cm-1. In the absence of ring conjugation, the band near 1580 cm-1 is usually weaker than that near 1600 cm-1. The fifth ring stretching vibration is active near 1335 ± 35 cm-1, the region which overlaps strongly with that of the C-H in-plane deformation and the intensity is in general, low, medium or high [41].

The sixth ring stretching vibration or ring breathing mode appears as a weak band near 1000 cm-1 in mono, 1,3-di and 1,3,5-trisubstituted benzenes. For substituted benzene, however, this vibration is substituent sensitive and is difficult to distinguish from the ring inplane deformation. In EBDA the C-C stretching vibrations are observed in the FT-IR and FT-Raman spectra at 1550, 1558, 1500 cm-1 as a medium band and at 1555, 1501 cm-1 as a weak band, which correlate well with the predicted theoretical data. The PED corresponding to all C-C vibrations lies between 40% and 50% as shown in Table 3 with a combination of C-H in-plane bending in this region. The in-plane deformation vibration is at higher wave numbers than the out-ofplane vibrations [41] gave the frequency data for these vibrations for different benzene derivatives as a result of normal coordinate analysis. The theoretically computed C-C-C in-plane and out-of-plane bending vibration by the B3LYP/6-31G (d, p) method shows good agreement with the recorded spectral data.

Carbonyl group vibrations: The carbonyl group stretching vibrations give rise to the characteristic bands in IR and Raman. The intensity of these bands can increase because of the formation of hydrogen bonds. The carbonyl group vibration is observed in the region 1760-1730 cm-1 [42,43]. The strong band at 1750 cm-1 is assigned to carbonyl C34-O35 stretching mode. The C12-O13 stretching mode is observed in IR at 1640 cm-1 as a medium band and the C12-O13 stretching vibrations are lower from the normal value. The red shifting of carbonyl stretching mode is attributed to the fact that the carbonyl group chelate with the other nucleophilic group, thereby forming both intra- and inter-molecular hydrogen bonding in the crystal. The C12-O13 stretching is lowered due to the formation of C-H...O hydrogen bonding in the molecule.

Methyl group vibration: Methyl group vibrations are generally referred to as electron donating substituent in the aromatic ring system, the asymmetric and symmetric C-H stretching mode of CH3 are expected to occur around 2980cm-1 and 2870 cm-1 [44]. The medium band observed in IR at 3005 cm-1 is assigned to the symmetric stretching of Me1. The same vibration is observed in IR and in Raman at 2986 cm-1 as a weak band and is assigned for Me2. The Me3 asymmetric stretching vibration is observed in IR at 2960 cm-1 and in Raman at 2968 cm-1 as a weak band. The shifting of the methyl (Me1 and Me2) asymmetric stretching wave number is due to the influence of the electronic effect resulting from the hyper conjugation and induction of methyl group in the aromatic ring [45]. Hyper conjugation causes the interaction of the orbital of the methyl group with the π orbital of an aromatic ring system [46]. The Methyl Symmetric bending of Me1 is observed at 1380 cm-1 in IR as a medium band. This characteristic wave number is in close agreement with those reported for the similar compounds [46]. The band observed at 854 cm-1 in IR is CH3 out of plane bending of Me1. The observed band in IR at 764 cm-1 and in Raman at 769 cm-1 is assigned to the CH3 out of plane bending modes of Me3.

Methylene group vibration: The methylene group vibrations are assigned on the basis of the spectral similarity to the related amino acid compounds. In amino acids, the CH2 asymmetric and symmetric vibrations are expected to occur in the regions 3100-3000 and 3000- 2900 cm-1 respectively [47-49]. The observed weak band in Raman at 3023 cm-1 is assigned to asymmetric stretching of C37-H2. The C31-H2 symmetric stretching is observed as a weak band in Raman at 2985 cm-1. Electronic effects including back-donation, mainly caused by the presence of nitrogen atom adjacent to methylene groups, which can shift the position and alter the intensity of C-H stretching and bending modes. The scissoring mode of the CH2 group gives rise to characteristic band near 1420-1412 cm-1. The scissoring mode of the C31-H2 group is observed in IR at 1440 cm-1 as a medium band. The rocking and wagging vibrations appear in the region of 1309-1288 cm-1 and 910-905 cm-1 respectively. The observed CH2 deformations are given in Table 3.

HOMO-LUMO energy gap

Spatial distribution of molecular orbital’s, especially those of highest occupied molecular orbital and lowest available unoccupied molecular orbital, are excellent indicators of electron transport in molecular systems. Conjugated molecules are generally characterized by a small HOMO-LUMO separation, which is the result of a significant degree of intra molecular change transfer (ICT) from the end-capping electron donor groups to the efficient electron acceptor groups through conjugated path. In EBDA, the HOMO-LUMO energy gap is 4.4913 eV and the lowering of this gap is essentially a consequence of the large stabilization of the LUMO due to the strong electron-accepting ability of the electron-acceptor group. The HOMO and LUMO orbital’s are shown in Figure 4. In EBDA the atomic π-orbital’s point towards each other and have better overlap, an increase in π-character points the fact that sigma bonds are stronger as evidenced by NBO analysis. A highly delocalized LUMO indicates that the electrons can more readily move around the molecule from HOMO-LUMO and hence an improved ICT [50] (Figure 4).


Figure 4: HOMO and LUMO plot of EBDA.

In EBDA the LUMO strongly localizes on the phenyl ring indicating the presence of favourable atomic centres within EBDA for possible nucleophile attacks revealing its bioactivity and pharmaceutical activity. The Lowering of HOMO-LUMO energy gap confirms the possibility of ICT and HOMO-LUMO delocalization showing its possibility of nucleophile attacks which serves as an evidence for the pharmaceutical activity of the EBDA molecule. The HOMO-LUMO plot shows that both the HOMO and LUMO orbital’s predominantly localize on the phenyl ring. The HOMO, LUMO and HOMO-LUMO energy gap of EBDA in the DFT level at 6-311++G (d, p) basis set has been calculated.

Molecular electrostatic potential

Molecular electrostatic potential is used primarily for predicting sites and relative reactivity’s towards electrophilic attack, in studies of biological recognition and hydrogen bonding interactions [51]. To predict the reactive sites for electrophilic and nucleophilic attack for EBDA, the MEP at the B3LYP/6- 311++G (d, p) method was calculated as shown in Figure 5. The different values of the electrostatic potential at the surface are represented by different colours. Electrostatic potential increases in the order redFigure 5).


Figure 5: The MESP mapped surface of the EBDA molecule.

As seen from Figure 5, in EBDA, the region having negative potential are over carbonyl group, the region having the positive potential are over the Phenyl ring and methyl group, the predominance of the light green region the MEPs surface corresponding to a potential halfway between the two extremes red and dark blue colour. The positive (blue) regions of MEP are related to electrophilic reactivity and the negative (red) regions to nucleophilic reactivity as shown in Figure 5. It can be seen from the MEP map of the present molecule that the negative regions are mainly localized on the O13 and O36 atoms. A maximum positive region is localized on the carbonyl carbon atom indicating a possible site for nucleophilic attack. MEP map shows that the negative potential sites are on electronegative atoms as well as the positive potential sites are around the carbonyl atom.


The detailed interpretation of the vibrational spectra has been carried out for the pharmaceutically important molecule Ethyl 2-(4-benzoyl-2, 5-imethylphenoxy) acetate. Molecular geometry, HOMO and LUMO energy and vibrational wave numbers of EBDA in the ground state have been calculated by using density functional theory. FT-IR and FT-Raman spectra of the EBDA have been recorded and analyzed. Observed and calculated wave numbers are found to be in good agreement. The lowering of carbonyl stretching wave number is due to the p-electron being localized. Lowering of the HOMO-LUMO energy gap value has substantial influence on the intra molecular charge transfer and pharmaceutical nature of the molecule.


Citation: Amalanathan M, Suresh DM, Joe IH, Jothy VB, Sebastian S, et al. (2016) FT-IR and FT-Raman Spectral Investigation and DFT Computations of Pharmaceutical Important Molecule: Ethyl 2-(4-Benzoyl-2,5-Dimethylphenoxy) Acetate. Pharm Anal Acta 7:457.

Copyright: © 2016 Amalanathan M, et al. This is an open-access article distributed under the terms of the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original author and source are credited.