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Wavenumber (cm-1)
Fig 5.5 Comparison of observed and calculated FT-Raman spectra of p-
chloronitrobenzene
(a) calculated with B3 LYP/6-31G**
(b) observed with KBr disc
(a)
(b)
Ram
an
In
tensity (
Arb
itr.
Units)
CHAPTER-VI
HYDROGEN BONDING AND MOLECULER VIBRATIONS
OF 2-BROMO-4-CHLORO PHENOL AND
2, 4-DICHLORO PHENOL
Abstract
The vibrational spectra of 2-bromo-4-chloro phenol (BCP) and 2,
4-dichloro phenol (DCP) have been computed using B3LYP methodology and
6-31 G* basis set. The solid phase FTIR and FT-Raman were recorded in the
region 4000-4000 cm-1 and 4000-50 cm-1 respectively. The effects of
hydrogen bonding were studied between the OH and halogen (Br-, Cl-)
atoms. On the basis of SQm methodology, a normal coordinate analysis was
performed to assign the various fundamental frequencies according to the
potential energy distribution (PED). Simulation of infrared and Raman spectra
utilizing the results of these calculations led to a good overall agreement with
observed spectral patterns.
CHAPTER-VI
HYDROGEN BONDING AND MOLECULER VIBRATIONS OF
2-BROMO-4-CHLORO PHENOL AND 2, 4-DICHLORO PHENOL
6.1 INTRODUCTION
Phenols and their derivatives are biologically and industrially useful
compounds. The properties of phenol and its derivatives are determined by
their hydrogen and π-bonding systems [181]. Their principle use is in the
manufacture of phenol formaldehyde polymers [182]. It also used in the
manufacture of many products including insulation materials, adhesives,
paint, rubber, ink, dyes, illuminating gases, perfumes, soap and toys and
cosmetics including sunscreens, hair dyes and skin lightening preparations
[183, 184]. Phenol is used in embalming and research laboratories. It is a
product of the decomposition of organic materials, liquid manure and the
atmospheric degradation of benzene. It is found in some commercial
disinfectants, antiseptics, lotions and ointments. Phenol is active against a
wide range of microorganisms and there are some medical and
pharmaceutical applications including topical anesthetic and eardrops,
sclerosing agent. It is also used in the treatment of ingrown nails in the “nail
matrix phenolization method”. Another medical application of phenol is its use
as a neurolytic agent, applied in order to relieve spasms and chlonic pain.
The inclusion of a substituent group in phenols leads to the variation of
charge distribution in molecules and consequently this greatly affects the
structural, electronic, and vibrational parameters. The bromo and chloro
groups are generally referred to as electron with drawing substituents in
aromatic systems. In BCP and DCP, the hydroxyl group is a powerful
activating group.
The modern vibrational spectrometry has proven to be an exceptionally
powerful technique for solving many chemistry problems. It has been
extensively employed both in the study of chemical kinetics and chemical
analysis. The problem of signal assignment however, as well as
understanding the relationship between the observed spectral features and
molecular structure, and reactivity can be difficult. Even identification of
fundamental vibrational wavenumbers often generates controversy.
Harmonic force fields derived from quantum mechanics are widely
used for the calculation of wavenumbers and the modes of normal vibrations.
Indeed, applying current quantum mechanical methods have opened up the
way for calculating the wavenumbers and intensities of spectral bands with a
minimum degree of arbitrariness (although the degree depends on the level of
the quantum-mechanical treatment) and finding rational explanation for a
number of chemical and physical properties of substances[24, 68, 69, 185].
However, for a proper understanding of IR and Raman spectra, a
reliable assignment of all vibrational bands is essential. Recently,
computational methods based on density functional theory are becoming
widely used. These methods predict relatively accurate molecular structure
and vibrational spectra with moderate computational effort. In particular, for
polyatomic molecules the DFT methods lead to the prediction of more
accurate molecular structure and vibrational wavenumbers than the
conventional ab initio restricted Hartree-Fock (RHF) and Moller-plesset
second order perturbation theory (MP2) calculation to understand the
structures and the fundamental vibrational wavenumbers of the title
compounds. DFT calculations are carried out to present a full description of
the vibrational spectra of these two important molecules, especially the
assignment of the vibrational modes, using B3LYP/6-31G*, to obtain the
geometrics, vibrational wavenumbers, IR intensities and Raman activities.
6.2 METHODS
6.2.1 Experimental Details
The commercial crystalline samples (99% purity) of BCP and DCP were
obtained from Lancaster chemical company, UK and used as such for the
spectral measurements. The Fourier trasform infrared spectrum of the title
compounds were recorded in the region 400–4000 cm-1 using Perkin-Elmer
spectrum RXI spectrophotometer equipped with He-Ne laser source, KBr
beam splitter and LiTaO3 detector. The samples were prepared by pressing
BCP and DCP with KBr into pellet form.
The FT-Raman spectra of BCP and DCP were recorded on a BRUKER
IFS–66V model interferometer equipped with an FRA-106 FT-Raman
accessory in the 4000-50 cm-1 Stokes region using the 1064 nm line of a
Nd:YAG laser for excitation operating at 200mW power. The reported wave
numbers are believed to be accurate within ± 1 cm-1.
6.2.2 Computational Details
In order to perform geometrical optimization and energy calculation of
the title compounds the GAUSSIAN 03 W software package [83] was used.
The calculations were carried out using the B3LYP functional [81, 82]
combined with standard 6-31 G* basis set. In order to express the normal
modes in a molecular fixed coordinate system, a set of local symmetry
coordinates for the title compounds were defined as recommended by Pulay
et al [186, 132]. The transformation of force field from Cartesian to internal
coordinates, the scaling, the subsequent normal coordinate analysis (NCA)
and the prediction of Raman intensities were done by employing the
procedure described in Chapter IV – section 4.3.
For the plot of spectra, digital versions of the observed and simulated
spectra of the title compounds were used. For visual comparison, these
spectra were plotted on a common frequency scale using ORIGIN software.
6.3 RESULTS AND DISCUSSION
6.3.1 Geometrical parameters
Geometrical optimization was first performed to establish reliable structures
using B3LYP/6-31G* basis set from the optimized structure were real and
positive and then the local minimum was defined to be a sTable conformer.
For BCP and DCP, the computationally predicted conformers are shown in
Figs 6.1(a)-6.1(b) and 6.2(a)-6.2(b), respectively. The total energies obtained
for these conformers are listed in Table 6.1. It is clear from the Table 6.1 that
the conformer in Fig 6.1(b) of BCP and Fig 6.2(b) of DCP produced the global
minimum energy and it forms the most sTable conformer as shown in Figs
6.1(c) and 6.2(c).
The calculated optimized geometrical parameters obtained in the study
for the title compounds presented in Table 6.2. The energy obtained in this
study is different which is clearly understandable. Since the environments of
the molecule are different. This clearly shows that the optimized structure
obtained for BCP and DCP are due to intramolecular hydrogen bonding. The
substitution of benzene with OH group and electronegativities (Br-, Cl-) in
ortho and para positions leads to intramoleculer hydrogen bonding.
In comparison BCP and DCP, both of the compounds having highly
electronegative atoms at the 2nd and 4th position, the electronic effect is
operating. Due to –I effect, the bond length is increased between C-Br and
C-Cl atoms. The bond length between carbon and chlorine atoms is shorter
than carbon and bromine atom due to chlorine highly electronegative than
bromine and hence the force constants are increased.
In para substitution both inductive and measomeric effects become
important and the domination of one over the other will decide the
wavenumber of absorption in the title compounds. In ortho substituted
compounds, the lone pair of electrons on two atoms influences each other
through space interactions and changes the vibrational frequencies of both
the groups. This effect is called field effect.
6.3.2 Force constants
The output of the quantum-mechanical calculations contains the force
constant matrix in Cartesian coordinates and in Hartree/Bohr2 units. These
force constants were transformed to the force fields in the internal local-
symmetry coordinates. The local-symmetry coordinates, defined in terms of
the internal valence coordinates following the IUPAC recommendations
[187, 133] are given in Tables 6.3 and 6.4 for BCP and DCP, respectively.
The force fields determined were used to calculate the vibrational potential
energy distribution (PED) among the normal coordinates.
The bonding properties of BCP and DCP are influenced by the
rearrangements of electrons during substitutions and addition reactions. The
values of the stretching force constants between carbon atoms in BCP are
shorter than DCP due to bromine atom having high reduced mass so it
reduced the force constants. In the halogen compounds, the C-H stretching
shifts to higher wave number due to the –I effect of the halogen atom. Due to
the –I (inductive) effect of halogen, C-H part of the molecule becomes rich in
s-component and hence force constant increases. Since chlorine is more
electronegative, the bonded electrons between the carbon atoms are slightly
shifted towards the halogen atoms of the title compounds. The values of the
stretching force constants between carbon and chlorine atoms of BCP are
found to be lesser than the values of stretching force constant between
carbon and chlorine atoms of DCP due to chemical environmental changes.
The most important diagonal force constants (stretching only) of BCP and
DCP are listed in Tables 6.5
6.3.3 Molecular vibrations
The molecule BCP and DCP belongs to cS point group symmetry, 33
normal modes of vibrations of BCP and DCP are distributed among the
symmetry species as, Γvib = 23A′+10A″. The A′ and A″ represents the in-plane
and out-of-plane vibrations, respectively. All vibrations are active both in
infrared absorption and Raman scattering.
Detailed description of vibrational modes can be given by means of
normal coordinate analysis. For this purpose, the full set of (45 for BCP and
DCP) standard internal coordinates (containing 12 redundancies for both the
title compounds) and a non-redundant set of local symmetry coordinates were
constructed by suiTable linear combinations of internal coordinates following
the recommendations of Forgarasi and Pulay [132] et.al. The theoretically
calculated DFT force fields were transformed to this later set of vibrational
coordinates and used in all subsequent calculations.
The IR and Raman intensities and normal mode descriptions
(characterized by PED) for the title compounds (BCP and DCP) are reported
in Tables 6.6 and 6.7, respectively. For visual comparison the observed and
simulated FTIR and FT-Raman spectra of the title compounds are presented
in Figs 6.3 - 6.6, which help to understand observed spectral features.
6.3.4 SQM analysis and assignments
The unscaled frequencies obtained by B3LYP method are larger than
the experimental values of both BCP and DCP. The RMS errors between the
unscaled and experimental frequencies are 39.8 cm-1 and 35.1 cm-1
respectively for BCP and DCP. In order to reproduce the calculated
frequencies close to the observed frequencies, a selective scaling procedure
was employed. The calculated frequencies were scaled using a set of
transferable scale factors recommended by Rauhut and Pulay [136]. The
SQM treatment improved the agreement between the experimental and the
scaled frequencies considerately, leading to an RMS deviation of 9.3 cm -1 for
BCP and 10.4 cm-1 for DCP.
6.3.5 OH group vibrations
The free hydroxyl group stretching vibrations occur in the region
3690-3600 cm-1. Hydrogen bonding alters the frequencies of the stretching
and bending vibrations. The OH stretching bands move to lower frequencies
usually with increased intensity and band broadening in the hydrogen bonded
species. In the present study, the stretching vibration of hydroxyl group of
BCP was observed at 3616 cm-1 and 3439 cm-1 for DCP. This shift in
frequencies towards lower wavenumber reflects the strength of hydrogen
bond. The OH stretching vibrations are overlapped together with the weak
C-H stretching bands [151, 188, 189, 190]. The strong bands observed at
1105 cm-1 and 1409 cm-1 were assigned to the OH in-plane vibration of BCP
and DCP, respectively [191, 192].
The OH torsional vibration is very anharmonic and hence it is difficult to
reproduce this frequency with a harmonic approach. For BCP the frequency of
this vibration was observed at 389 cm-1 and for DCP 404 cm-1 [151].
6.3.6 C-H Vibrations
In Infrared spectrum, most of the aromatic compounds have strong
peaks in the region of 3100-3000 cm-1 due to C-H stretching vibrations. In
BCP these nodes are observed at 3088, 3071 and 3068 cm-1and in DCP
these modes are identified at 3092, 3081 and 3071 cm-1.
The C-H in-plane bending vibrations are usually weak and observed in
1000-1300cm-1 region [193,194]. The C-H out-of-plane bending modes are
observed in the region 1000 – 800 cm-1 [151, 195]. In the present work, the
bands observed at 1492, 1277 in FTIR and 1139 cm-1 in FT-Raman for BCP
and 1180, 1137, 1094 cm-1 in FTIR for DCP are assigned to C-H in-plane
bending vibrations. The C-H out-of-plane bending modes for BCP and DCP a
assigned within characteristic region [196] and are depicted in Tables 6.6 and
6.7.
6.3.7 Halogen vibrations
The vibrations belonging to the bond between the ring and the
halogen atoms are worth to discuss here, since mixing of vibrations are
possible due to the lowering of the molecular symmetry and the presence of
heavy atoms on the periphery of molecule. [174, 197]
(a) C-Cl vibrations
Most aromatic chloro compound has strong absorptions at 760-395
cm-1, which is due to a combination of vibrational modes and dihalogen-
substituted benzenes exhibit in the former band [174,151]. In the present
work, the C-Cl stretching vibrations are identified at 648 cm-1 in FTIR spectra
for BCP and 729 cm-1 and 452 cm-1 in FTIR and FT-Raman spectrum for
DCP. The C-Cl in-plane bending and out-of-plane bending modes for BCP
and DCP were also assigned within the characteristic region and were
presented in Tables 6.6 and 6.7.
(b) C-Br vibrations
The C-Br stretching vibration of the title compound has been
observed at 266 cm-1. The in-plane and out-of-plane bending vibrational
assignments of C-Br are shown in Table 6.6. These assignments are in good
agreement with the literature [151].
6.3.8 Ring vibrations
The ring stretching vibrations are very important in the spectrum of
benzene and its derivatives are highly characteristic of the aromatic ring itself.
The ring carbon-carbon stretching vibrations occur in the region 1430-1625
cm-1. For aromatic six membered rings there are two to three bands in this
region due to skeletal vibrations [151]. In the present work, the observed and
calculated wavenumbers are in excellent agreement with the literature. The
FTIR bands identified at 1590, 1403, 1323, 1100 and 844 cm-1 and FT-Raman
band at 1594 cm-1 in BCP are attributed to C=C stretching vibrations
[194,195]. The FTIR bands at 1595,1486,1371,1251 and 822 cm-1 and
FT-Raman band at 1596 cm-1 are assigned to C=C stretching vibrations in
DCP [194, 177]
The ring deformation vibrations are ascribed to the FTIR band at 1042
cm-1 and FT-Raman bands at 705 and 350 cm-1 in BCP and the FTIR band at
1054 and 653 cm-1 and FT-Raman band at 349 cm-1 in DCP [194, 198, 153,
199]. The out-of-plane deformations are established at 548 and 425 cm-1 in
FTIR spectra and 339 cm-1 in FT-Raman for BCP and 694 and 440 cm-1 in
FTIR spectra and 120 cm-1 in FT-Raman spectra for DCP [200, 194, 195]. The
calculated C-C out-of-plane and in-plane bending modes have been found to
be consistent with the recorded spectral values.
6.4 CONCLUSION
Complete vibrational analysis of BCP and DCP are performed on the
basis of DFT calculations at the B3LYP/6-31G* levels of theory. The
influences of hydroxyl group and in the vibrational wavenumbers of the title
compounds are discussed. The substituents of chlorine and bromine atoms in
the ortho position of phenol give rise to strong intramolecular hydrogen
bonding. The role of strong intramolecular hydrogen bonding on the molecular
geometry of the most sTable conformer and on the vibrational frequencies is
confirmed by the quantitative agreement between the calculated and the
observed band intensities and also polarization properties and it is believed to
be unambiguous.
Table6.1
Total energies (in Hartrees) based on B3LYP/6-31G* basis set for BCP
and DCP.
Conformers
Energy calculation
BCP DCP
a -3338.1613 -1226.6517
b -3338.1675 -1226.6560
Table 6.2
Optimized geometrical parameters of BCP and DCP obtained by
B3LYP6-31G* density functional calculations.
The atom indicated in tne parenthesis belongs to DCP; For numbering of atoms refer figs. 6.1 (c) and 6.2(c).
Bond length
Value(A°) Bond angles
Value(°)
BCP DCP BCP DCP
C1−C2 1.402 1.403 C1−C2−C3 121.895 121.730
C2−C3 1.391 1.392 C2−C3−C4 118.645 118.719
C3−C4 1.392 1.392 C3−C4−C5 120.816 120.845
C4−C5 1.395 1.395 C4−C5−C6 119.671 119621
C5−C6 1.390 1.390 C6−C1−O7 118.207 118.226
C1−O7 1.354 1.355 C1−C2−Br8(Cl8) 118.309 118.553
C2−Br8(Cl8) 1.916 1.762 C2−C3−H9 120.904 120.259
C3−H9 1.083 1.083 C3−C4−Cl10 119.872 119.284
C4−Cl10 1.757 1.757 C4−C5−H11 120.024 120.066
C5−H11 1.064 1.084 C5−C6−H12 120.937 120.937
C6−H12 1.085 1.085 C1−O7−H13 108.578 108.993
O7−H13 0.974 0.973
Table 6.3
Definition of internal coordinates of BCP and DCP.
The atom indicated in tne parenthesis belongs to DCP. For numbering of atoms refer figs. 6.1 (c) and 6.2(c).
No.(i) Symbol Type Definition
Stretching
1−6 ri C−C C1−C 2, C2−C3, C3−C4, C4−C5, C5−C6, C6−C1.
7−9 Ri C−H C3−H9, C5−H11, C6−H12.
10 Pi C−Br(Cl) C2−Br8(Cl8).
11 qi C−O C1−O7.
12 pi C−Cl C4−Cl10
13 Qi O−H O7−H13
Bending
14−19 δi bC−H C2−C3−H9, C4−C3−H9, C4−C5−H11, C6−C5−H11, C5−C6−H12, C1−C6−H12.
20−21 βi bC−Br(Cl) C1−C2−Br8(Cl), C3−C2−Br8(Cl8).
22−23 αi bC−O C6−C1−O7,C2−C1−O7.
24−25 γi bC−Cl C3−C4−Cl10,C5−C4−Cl10
26 ρi bO−H C1−O7−H13.
27−32 βi Ring C1−C2−C3, C2−C3−C4, C3−C4−C5, C4−C5−C6, C5−C6−C1, C6−C1−C2.
Out-of-plane bending
33−35 ωi gC−H H9−C3−C2−C4, H11−C5−C4−C6, H12−C6−C5−C1.
36 ωi gC−Br(Cl) C1−C3−C2−Br8(Cl8)..
37 ωi gC−Cl C3−C5−C4−Cl10.
38 ωi gC−O C2−C6−C1−O7
Torsion 39 i tO−H (C6)C2−C1−O7−H13.
40−45 i Tring C1−C2−C3−C4, C2−C3−C4−C5, C3−C4−C5−C6, C4−C5−C6−C1, C5−C6−C1−C2, C6−C1−C2−C3.
Table 6.4
Definitions of local symmetry coordinate of BCP and DCP.
a These symbols are used for description of the normal modes by PED in Tables 6.6 and 6.7.
b The internal coordinates used here are defined in Table 6.3.
No.(i) Symbol a Definition b
5 CC r1,r2,r3,r4,r5,r6
7−9 CH R7,R8,R9
10 CBr (CCl) P10 11 OH Q11
12 CCl p12
13 CO q13 14−16 bCH (δ14− δ15)/√2,( δ16− δ17)/√2,(δ18− δ19)/√2.
17 bCBr (bCCl) (β20−β21)/√2
18 bCO (α22 –α23)/√2
19 bCCl (γ24− γ25)/√2
20 bCOH ρ26
21 bRtrigd (β27− β28+ β29− β30+ β31− β32)/√6
22 bRsymd (−β27− β28+2 β29− β30+ β31−2 β32)/√12
23 bRasymd (β27− β28+ β29− β30)/√12
24−26 ωCH ω33, ω34, ω35
27 ωCBr (ωCCl) ω36
28 ωCO ω37 29 ωCCl ω38
30 OH 39
31 Rtrig ( 409− 41+ 42− 43+ 444− 45)/√6
32 Rsym (− 40+ 42+ 43− 44)
33 Rasym (− 40+2 41− 42− 43+2 44− 45)/√2
Table 6.5
Diagonal stretching force constants of BCP and DCP
a The atoms indicated in the parenthesis belongs to DCP; for numbering of atoms refer
Figs.6.1 (c) and 6.2(c)
b Stretching force constants are given in mdyn
0
A−1
.
Descriptiona
Force constantsb
BCP DCP
C1−C2 6.638 6.876
C2−C3 6.642 6.934
C3−C4 6.667 6.978
C4−C5 6.569 6.869
C5−C6 6.807 7.112
C6−C1 6.491 6.806
C1−O7 6.514 6.827
C2−Br8 (Cl8) 1.758 4.040
C3−H9 5.224 5.235
C4−Cl10 3.512 4.171
C5−H11 5.177 5.199
C6−H12 5.158 5.179
O7−H13 7.319 6.620
Table 6.6
Calculated frequencies (cm-¹) of BCP by B3LYP/6-31 G* method and vibrational assignment based on potential energy
distribution (PED).
Sl. No
Symmetry species
Observed frequencies (cm-1)
Calculated frequencies
B3LYP/6-31G* force field (cm-1)
IR Intensity
Raman activity
Characterization of normal modes with PED (%)
FTIR Raman unscaled scaled
Q1 A′ 3616 − 3663 3616 81.577 58.289 OH(100)
Q2 A′ 3088 − 3249 3087 0.561 56.296 CH(99)
Q3 A′ − 3071 3233 3077 1.723 146.678 CH(99)
Q4 A′ 3068 − 3218 3063 1.756 71.756 CH(99)
Q5 A′ − 1594 1649 1598 5.625 18.864 CC(65), bCH(16)
Q6 A′ 1590 − 1630 1592 15.568 11.742 CC(68), bCH(11)
Q7 A′ 1492 − 1523 1496 219.678 2.173 bCH(47), CC(36), CO(11)
Q8 A′ 1403 − 1454 1402 0.976 3.284 CC(53), bCH(24)
Q9 A′ 1323 − 1389 1329 3.767 2.914 CC(42), bCH(33), bOH(16)
Q10 A′ − 1292 1331 1296 80.798 6.603 CO(57), CC(24), bCH(10)
Q11 A′ 1277 − 1289 1265 20.293 2.427 bCH(42), CC(38), CO(13)
Q12 A′ 1175 − 1234 1174 156.597 1.684 bOH(39), bCH(29), CC(25)
Q13 A′ − 1139 1162 1134 48.337 5.670 bCH(37), CC(33), bOH(18)
Q14 A′ 1100 − 1115 1092 3.681 8.578 CC(42), CCl(22), bCH(14), Rtrigd(14)
Q15 A′ 1042 − 1049 1045 14.788 2.329 Rtrigd(52), CC(26), bCH(12)
Q16 A″ 863 − 957 896 0.206 0.897 ωCH(83),tRtrig(12)
Q17 A″ − 847 897 831 11.536 1.171 CH(79)
Abbreviations; R, ring; b, bending; d, deformation; sym, symmetric; asy, asymmetric; ω, ωagging; t, torsion; trig, trigonal; , stretching. Only contributions larger than 10% are given.
Q18 A′ 844 − 859 830 3.947 23.742 CC(38), CO(23), Rsymd(17), Rtrigd(11)
Q19 A″ 807 − 837 779 29.067 2.602 CH(75), tRasym(11)
Q20 A′ − 705 714 703 22.353 5.312 Rasym(70), CC(13), CBr(10)
Q21 A″ − 662 704 661 1.242 0.540 ωCO(66), tRtrig(10)
Q22 A′ 648 − 657 656 55.103 0.926 CCl(42), Rsymd(25)
Q23 A″ 548 − 561 559 4.476 0.560 tRasym(38), CCl(36)
Q24 A′ 497 − 500 496 21.251 1.198 bCO(61),bCBr(11)
Q25 A″ 425 − 454 422 0.000 0.105 tRsym(51), ωCBr(21)
Q26 A″ − 389 438 390 104.650 2.092 tOH(99))
Q27 A′ − 360 381 359 0.620 7.410 Rsymd59), CCl(27)
Q28 A″ − 339 341 333 0.293 0.804 tRtrig(43),ωCBr(17), ωCCl(16), ωCH(14)
Q29 A′ − 264 334 283 2.567 2.759 CBr(30), bCCl(30), bCBr(27)
Q30 A′ − 249 250 235 2.566 2.926 bCBr(46), CBr(32), bCO(10)
Q31 A′ − 167 164 143 0.168 3.114 bCCl(62),bCBr(22)
Q32 A″ − 140 160 141 0.034 0.794 ωCCl(45), tRasym(19) ,ωCBr(15),ωCH(14)
Q33 A″ − 125 126 122 0.046 3.256 ωCBr(50),tRsym(21), tRasym(20)
Table 6.7
Calculated frequencies (cm-¹) of DCP by B3LYP/6-31 G* method and vibrational assignment based on potential energy
distribution (PED).
Sl. No
Symmetry species
Observed frequencies (cm-1)
Calculated frequencies B3LYP/6-31G*
force field (cm-1)
IR Intensity
Raman activity
Characterization of normal modes with PED (%)
FTIR Raman unscaled scaled
Q1 A′ 3439 − 3700 3439 77.605 64.956 OH(100) Q2 A′ 3092 − 3240 3091 0.358 67.847 CH(99) Q3 A′ 3081 − 3232 3084 1.547 132.734 CH(99) Q4 A′ 3071 3071 3218 3069 1.883 69.569 CH(99) Q5 A′ 1596 1652 1602 3.998 20.075 CC(72), bCH(12) Q6 A′ 1595 − 1632 1595 29.096 9.904 CC(75) Q7 A′ 1480 − 1526 1486 243.508 3.367 CC(44), bCH(30), CO(18) Q8 A′ 1409 − 1454 1408 61.737 2.211 bOH(42), CC(36), bCH(12) Q9 A′ 1371 − 1380 1364 44.814 2.897 CC(69), bOH(15), bCH(13) Q10 A′ 1326 − 1331 1310 18.136 6.736 CO(43), CC(27), bCH(20) Q11 A′ 1251 − 1284 1256 101.055 2.152 CC(47), bOH(18), bCH(15)), CO(14) Q12 A′ 1180 − 1226 1190 67.098 1.985 bCH(56), CC(21), bOH(10)) Q13 A′ 1137 − 1165 1130 4.693 8.932 bCH(45), CC(26), CCl(19) Q14 A′ 1094 − 113 1092 12.283 3.179 bCH(46), CC(28), CCl(12) Q15 A′ 1054 − 1064 1044 20.283 1.199 Rtrigd(33), CC(23), bCH(19), CCl(18) Q16 A″ 955 − 950 948 0.206 0.754 ωCH(88) Q17 A″ 867 − 874 865 15.849 1.386 ωCH(86) Q18 A′ 822 − 864 844 17.312 16.080 CC(27), Rtrigd(23), CCl(18),Rsymd(14),
CO(13)
Abbreviations; R, ring; b, bending; d, deformation; sym, symmetric; asy, asymmetric; ω, ωagging; t, torsion; trig, trigonal; , stretching. Only contributions
larger than 10% are given.
Q19 A″ 816 − 831 825 29.518 2.948 ωCH(82)
Q20 A′ 729 728 739 61.458 9.620 CCl(38), CC(21), Rasymd(20)
Q21 A″ 694 − 694 694 1.426 0.263 tRtrig(64),ωCO(17), ωCCl(11)
Q22 A′ 653 − 658 646 12.626 4.616 Rasymd(39), CCl(27), Rsymd(11)
Q23 A″ 490 − 560 530 1.208 0.627 ωCO(28), ωCCl(22), tRsym(21), tRasym(19)
Q24 A′ 452 − 515 434 3.727 7.461 CCl(31), bCCl(23), bCO(17), Rasymd(14)
Q25 A″ 440 − 447 431 0.008 0.032 tRsym(41), tRasym(26), ωCCl(21)
Q26 A″ − 404 411 403 121.645 2.298 tOH(96)
Q27 A′ − 389 398 392 3.224 3.339 bCCl(57), Rasymd(14), CCl(12)
Q28 A′ − 349 379 336 0.097 5.794 Rsynd(76), CCl(11)
Q29 A″ − 341 340 312 0.047 0.818 ωCCl(49), tRasym(19), ωCO(16)
Q30 A′ − 203 282 209 5.221 0.421 bCO(67), bCCL(23)
Q31 A′ − 195 198 196 2.182 2.296 bCCl(79), bCO(10)
Q32 A″ − 139 174 154 0.071 2.396 ωCCl(75), tRsym(17)
Q33 A″ − − 125 120 0.056 0.525 tRasym(33), ωCCl(30), tRsym(18), ωCH(11)
(c)
Fig.6.1 (a) and (b) Two conformers of 2-bromo-4-chloro phenol
(c) STable conformers of 2-bromo-4-chloro phenol along with
numbering of atoms
(c)
Fig.6.2 (a) and (b) Two conformers of 2, 4-dichloro phenol
(c) STable conformers of 2, 4-dichloro phenol along with numbering of
atoms
Wavenumber (cm-1)
Fig 6.3 Comparison of observed and calculated FTIR spectra of
2- bromo- 4– chloro phenol
(a) calculated with B3 LYP/6-31G*
(b) observed with KBr disc
(a)
(b)
Absorb
ance (
Arb
itr.
Units)
Wavenumber (cm-1)
Fig 6.4 Comparison of observed and calculated FT-Raman spectra of
2- bromo-4- chlorophenol
(a) calculated with B3 LYP/6-31G*
(b) observed with KBr disc
(a)
(b)
Ram
an
In
tensity (A
rbitr.
Un
its)
Wavenumber (cm-1)
Fig 6.5 Comparison of observed and calculated FTIR spectra of
2,4 - dichlorophenol
(a) calculated with B3 LYP/6-31G*
(b) observed with KBr disc
(a)
(b)
Absorb
ance (
Arb
itr.
Units)
Wavenumber (cm-1)
Fig 6.6 Comparison of observed and calculated FT-Raman spectra of
2, 4- dichlorophenol
(a) calculated with B3 LYP/6-31G*
(b) observed with KBr disc
(a)
(b)
Ram
an I
nte
nsi
ty (
Arb
itr.
Un
its)