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Journal of Molecular Structure (Theochem), 304 (1994) 45-5 1
0166-1280/94/$07.00 0 1994 - Elsevier Science Publishers B.V. All rights reserved 45
Computationa imidazoles
1 study of
Michael Meyer
i midazole and methyl
GBF, Gesellschaft fiir Biotechnologische Forschung, Department of Molecular Structure Research, Mascheroder Weg 1, D-38124 Braunschweig, Germany
(Received 23 July 1993; accepted 10 August 1993)
Abstract
A semiempirical and ab initio study of the structures of imidazole, methyl imidazoles and the corresponding protonated and deprotonated ions is presented. The energies of the different isomers and tautomers are discussed and the protonation and deprotonation energies are given. Dipole moments and the barriers hindering internal rotation of the methyl group were determined. The heats of formation were derived from an isodesmic reaction - _ scheme and semiempirical calculations.
Introduction
Imidazole (CsH4N2 (IA)), is a five-membered
heterocyclic system with basic and acidic proper-
ties. The IA ring of histidine plays an important
role in proton transfer processes at the active site
of certain enzymes. Thus IA may be used as a
simple model to study enzymatic modes of action
with semiempirical and ab initio methods [l]. The
structure of this molecule is available from micro-
wave spectroscopy [2] and computational studies
[3]. Nitrogen nuclear coupling constants, the
dipole [2] and molecular quadrupole moments [4],
the heat of formation [5] and the proton affinity [5,
61 have been determined experimentally. Less is
known about the methyl imidazoles (C4H6N2
(MIA)). The microwave spectra are more difficult
to analyse because the methyl group gives rise to a
torsional fine structure in addition to the nitrogen
nuclear quadrupole hyperfine structure. Further-
more, experimental investigations of 4-MIA and
5-MIA are complicated by the tautomeric equi-
librium of these molecules. So far the proton
affinities have been determined and the structures
have been calculated using a minimal basis set [6].
SSDI 0166-1280(93)03457-I
A study of IA, the MIA and the corresponding
protonated and deprotonated ions is presented
here. The structures were calculated using semiem-
pirical and ab initio methods based on the
Hartree-Fock (HF) theory. The accuracy of the
calculated structure of IA was checked by compar-
ing it with the experimental results. The structures
of the ions and the substituted molecules were
compared with the parent species IA. These calcu-
lations give insight into the methyl torsional angles,
referred to the lowest energy, which are difficult to
estimate from simple chemical arguments. The
influence of different basis sets and of correlation
effects on the energies was investigated in order to
determine the stabilities of the different tautomers
and isomers and to calculate the protonation and
deprotonation energies. The heats of formations of
the MIA were derived from ab initio calculations
and experimental data using isodesmic reaction
schemes and from semiempirical calculations.
Computational details
The ab initio calculations were carried out using
the GAUSSIAN 90 [7] and GAMESS [8] programs. All
46
geometries were optimized at the HF level, employ-
ing the 6-31G* split valence basis [9] with polariz-
ation functions on the heavy atoms. This level of
theory is generally considered to be sufficient to
provide consistent molecular geometries [lo].
Single-point calculations at the HF/6-3 lG*
geometries were carried out using the triple split
6-3 11 G** basis set with additional polarization
functions on hydrogen atoms [l 11. For the calcu-
lation of the deprotonation energies, the 6-3 1 + G*
basis set supplemented with diffuse functions on
the heavy atoms [12] was applied. For an estimate
of correlation effects, Moller~Plesset perturbation
theory of second order (MP2) was used with the
HF/6-31G* structures. For the parent species,
MP3 and MP4(SDTQ) calculations of the energies
were used to estimate the influence due to single,
double, triple and quadruple excitations on the
energies.
All semiempirical calculations were carried out
using the MNDO [14]. AMI [15] and PM3 [16]
methods of MOPAC 5.0 [13].
Results and discussion
Molecular structures
The structure of IA obtained with the HF/6-
31G* method is given in Table I together with
the experimental one derived from microwave
spectroscopy [2]. The computed structure is close
to the results of Mb et al. [3], who obtained a better
reproduction of the bond lengths and larger devi-
ations of the angles with the 6-31G basis. The mean
absolute deviation between the experimental
and calculated heavy atom bond lengths of the
imidazole ring is 0.014A and the error in the
angles is 0.2’. The corresponding errors of the
semiempirical methods MNDO, AMI and PM3
are 0.024, 0.028 and 0.024 A and I. 1, 0.6 and
2.5’, respectively. All semiempirical methods over-
estimate the heavy atom bond lengths, whereas the
ab initio calculations underestimate them. N-H
and CH bonds obtained via ab initio calculations
are a little too short.
M. Me,wr:J. Mol. Smut. (Theochcmj 304 (1994) 45-51
Table 1
Experimental and ab initio structures of imidazole and its
protonated and deprotonated ions
C~H~INI” GH,Nl C~HSNZ + C,H,NY
Bond length (k)
NlLC2 1.364 1.349 1.313 1.327
C2-N3 1.314 1.289
N3-C-4 1.382 1.372 1.382 1.357
C4GC5 1.364 1.350 1.340 1.372
C5-Nl 1.377 1.372
N1 HI 0.998 0.993 I .ooo
Bond anglr ideg)
N 1 -C2-N3 112.0 112.2 108.0 117.0
C2-N3-C4 104.9 105.3 109.5 102.3
N3-C4-C5 110.7 110.5 106.5 109.2
C4-C5 Nl 105.5 105.2
CS-Nl C2 106.9 106.8
’ Experimental value [2].
The Cl,. symmetric structures of the protonated
cation and the deprotonated anion derived from IA
are also compiled in Table 1. The protonation of
the N3 nitrogen atom of IA causes an increase in
the endocyclic angles X2N3C4 and /C5N 1 C2 and
a decrease in iNlC2N3. A removal of the hydro-
gen at Nl of IA leads to the opposite structural
changes in the anion. The bonds Nl-C2 and C2-
N3 of both ions are shorter than they are in the
neutral molecule. The heavy atom geometries of
the MIA are given in Table 2. The effects of methyl
substitution on the ring geometry are very small.
Substitution at carbon atoms leads to a slight elon-
gation of the imidazole ring along the bond to the
methyl carbon atom and a corresponding narrow-
ing of the ring. The endocyclic angle between the
carbon atoms, where the substitution takes place,
and the adjacent atoms is decreased. Both bond
lengths to the neighbouring atoms of the ring
are increased. Similar substitution effects have
been derived from the experimental structures of
benzene and toluene [ 171.
The complete structures of all MIA are shown in
Fig. 1 to indicate the torsional angles of the methyl
groups referring to the lowest energies. On the basis
of a previous calculation without polarization
M. Meyer/J. Mol. Struct. (Theochem) 304 (1994) 45-51
Table 2 Energies Structures of l-, 2-, 4- and 5-methylimidazoP
41
l-MIA 2-MIA 4-MIA 5-MIA
Bond length (A) Nl-C2 1.349 C2pN3 1.291 N3-C4 1.369 C4&C5 1.352 C5pNl 1.372
NlLC, 1.444 c2P& c4-c, c5w&
Bond angle (deg) NlPJ2pN3 112.9 C2pN3-C4 105.0 N3%C4-C5 110.3 C4&C5-Nl 105.8 C5-Nl X2 106.0
C,-NlWZ5 126.9 C,+ZZpNl c,-c4-c5 c,-c5wZ4
1.353 1.356 1.352 1.292 1.289 1.286 1.374 1.376 1.374 1.347 1.352 1.352 1.375 1.375 1.376
1.495 1.496
1.494
111.3 112.2 112.1 105.8 105.7 105.2 110.5 109.7 111.0 105.1 105.7 104.5 107.3 106.6 107.2
122.9 129.0
132.5
a HF/6-31G*.
functions [6], it was concluded that methyl
groups in the Q position to the basic nitrogen atom
N3 have a minimum-energy conformation that
contains one hydrogen atom in the ring plane
near to the nitrogen. However, the calculations
with the enlarged basis show (in agreement with
MNDO, AM1 and PM3) that this is only valid
for 2-MIA, and not for 4-MIA. As shown in
Fig. 1, the in-plane hydrogen atom of the methyl
group of 4-MIA is directed towards C5 and not to
N3.
The total energies of all ionic and neutral
molecules are listed in Table 3. The ions derived
from 4-MIA and 5-MIA are identical. The proton-
ation and deprotonation energies, defined as the
energy difference between the protonated and the
deprotonated species, are listed in Table 4. At
the HF level, the calculations with the 6-31G* and
6-31 lG* basis sets lead to similar results for
energy differences. The protonation energies of
IA are lower than those previously calculated
without polarization functions [3,6]. MP2 correc-
tions reduce the protonation and deprotonation
energies further to 234.0 kcalmol-‘. From the
data of IA it may be seen that both energy differ-
ences oscillate with the order of the perturbation
treatment. The HF method provides an upper limit
and the MP2 method provides a lower limit for MP
calculations of higher order. Hence, only the
former methods are applied to MIA. When calcu-
lating deprotonation energies, diffuse functions
on the heavy atoms must be taken into account.
Additional diffuse functions on hydrogen do not
influence the energies significantly.
The substitution of hydrogen with methyl groups
cause a small increase in the deprotonation protona-
tion energies of approximately 1 kcalmoll’ The
protonation energies rise by 4 kcal mol-’ . Hence IA
and 4-MIA seem to be interchangeable in model
studies of the protonation of histidine.
The calculated energies of the MIA are also given
in Table 3. The total energy of 4-MIA is only
0.16 kcal mol-’ smaller than the energy of the tauto-
merit species 5-MIA. Single-point calculations
Fig. 1, The structures of l-, 2-, 4- and 5-methylimidazole.
Tab
le
3
Tot
al
ener
gies
’ (H
, kc
al
mol
-‘)
IA
I-M
IA
2.M
IA
4.M
IA
S-M
IA
CxH
,Nl
CIH
~N:
C,H
,N;
CdH
,Nz
C,H
,N:
CdH
,N,
CdH
,N:
ChH
,N;
CIH
,N~
CdH
,N:
C,H
,N,
Czt
HaN
z
HF/
6-3l
G*
-224
.814
43
-225
.196
35
-224
.224
70
-263
.846
36
-264
.235
52
-263
.857
92
-264
.248
53
-263
26
562
-263
.855
59
-264
.243
09
-263
26
500
-263
.855
34
HF/
6-31
+
G*
-224
.822
82
-224
24
834
-263
86
561
-263
.288
36
-263
.863
98
-263
.286
99
-263
.863
40
HF’
b-31
f +G
* -2
24.8
2293
-
224
2484
0
HF
,6-3
1 I’
S**
-224
.869
86
-225
25
309
-224
28
080
-263
.908
49
-264
.299
45
-263
.922
23
~- 26
4.31
449
-263
.330
75
-263
.919
85
~264
.308
93
-263
.329
47
-263
.919
25
MP2
!6-3
lG*
-225
.538
40
-225
.91
I38
-224
.959
98
-264
.707
29
-265
.087
19
-264
.717
61
-265
.098
12
-264
.137
32
-264
.716
09
-265
.094
87
-264
.136
99
-264
.715
68
MP3
:6-3
I G
* -2
25.5
3 I I
1
-225
.909
17
-224
.946
65
MP4
/6-3
lG*
-225
.570
28
--22
5.94
551
-224
.988
41
a A
t th
e H
F/6-
3lG
* ge
omet
ry
M. Meyer/J. Mol. Struct. (Theochem) 304 (1994) 45-51 49
Table 4
Protonation and deprotonation energies
IA
Protonation energy (kcalmol-‘)
HF/6-31G* 239.1
HF/6-311G** 240.5
MP2/6-31G* 234.0
MP3/6-31G* 237.2
MP4/6-3 1 G* 235.5
Deprotonation energy (kcalmol-‘)
HF/6-31G* 370.1
HF/6-31 + G* 360.5 HF/6-31 + + G* 360.5
HF/6-311G** 369.6
MP2/6-31G* 363.0 MP3/6-31G* 367.2
MP4/6-31G* 365.1
l-MIA 2-MIA 4-MIA 5-MIA
244.2 245.1 243.2 243.3
245.3 246.1 244.2 244.5
238.4 238.8 231.1 231.9
311.1 310.6 310.4
362.2 362.1 361.1
311.2 370.5 310.1
364.1 363.4 363.1
confirm this order of the energies and yield
slightly larger energy differences of 0.38 kcal mol-’
(HF/6-31 lG**) and 0.27 kcalmoll’ (MP2/6-31G*).
The potential V(a) of a methyl top rigidly
rotating relative to a frame may be expressed as a
Fourier series of the torsional angle cy:
l’(o) = V,/2( 1 - cos 3~) + V6/2( 1 - cos 6cr) + .
(1)
The barrier height of the three-fold potential is
given by Vs. The term I’,, which modifies the
shape of the potential, is generally much smaller
than I’,. It is possible to estimate V’s by calculating
the energies using the structures indicated in Fig. 1
and then calculating the energies with the methyl
groups rotated by 180”. Barrier heights of 0.57,
0.53, 1.08 and 1.45 kcalmol-’ have been deter-
mined this way for l-, 2-, 4- and 5-MIA, respec-
tively. Similar barrier heights have been observed
experimentally for 2-, 4- and 5-methyl oxazole. The
barrier heights of these molecules are 0.7200 (35),
1.2237 (35) and 1.3663 (37) kcal mol-‘, respectively
]181. Except for 2-MIA, the conformations of the
methyl groups referring to the energy minima are
generally the same for the ions and neutral mole-
cules. As the methyl top with a three-fold symmetry
is rotating with respect to the frame of two-fold
symmetry for the ions derived from 2-MIA, indis-
tinguishable conformations are obtained at
intervals of 2rr/6. The potential function has
six-fold symmetry; V3 in Eq. (1) cancels and the
barriers are expected to be very low.
Heats of formation
Ab initio calculations of the energies were com-
bined with experimental heats of formation (AHr)
of imidazole (35 kcal mall’), ethane (-20 kcal
mall’), methane (- 18 kcal mall’), methylamine
(-5 kcal mall’) and ammonia (- 11.02 kcal mol-‘)
[5] in order to determine the heats of formation of
the MIA from the following isodesmic reaction
schemes:
C3H4NZ + CH3CH3 + C4H6N2 + CH4
for 2-, 4- and 5-MIA
C3H4N2 + NH2CH3 --) C4H6N2 + NH,
for l-MIA
Differences in the zero-point energies between reac-
tants and products are neglected in this approach.
The energies of IA and its derivatives are listed in
Table 3, and the energies of the other molecules
used for the isodesmic reaction are compiled in
Table 5. The heats of formation shown in Table 6
50
Table 5 Total energies (H, kcalmol-‘)
M. Meyer:J. Mol. Strut. (Theochem) 304 (1994) 45-51
HF/6-3 lG* -19.22816 -40.19517 -95.20983 -56.18436 HF/6-31 lG** -79.25170 -40.20901 -95.24251 -56.21039 MP2/6-3 1 G* -79.50376 -40.33695 -95.51380 -56.35690
increase from 2-MIA to 4- and 5-MIA, for which
the calculated AH, values are almost identical. The
AH, of l-MIA is the highest of the substituted
molecules. An increase in the basis quality from
6-31G* to 6-31 lG** hardly affects AH,-. The
MP2 results for all molecules have lower values
than the HF data. The semiempirical methods
MNDO and PM3 yield heats of formation up to
4 kcal mall’ below the experimental value for IA.
Similarly, these methods give lower heats of for-
mation than the ab initio calculations for the
MIA. AM1 overestimates the heat of formation
of IA significantly. The calculated data for the
substituted molecules also seem too high. This
overestimation of AH, by AM1 is apparent in
case of oxazole too [19].
Dipole moment
The results of the ab initio calculations of the
dipole moments are summarized in Table 7.
These data show only a small change with respect
to an increase in the basis at the HF level. The MP2
values obtained using the z-vector method [20] are
close to the dipole moments obtained with the HF
Table 6 Heats of formation (kcal mol-‘)
IA” l-MIA 2-MIA 4-MIA j-MIA
HF/6-31G* ~ 37.0 26.8 28.1 28.4 HF/6-31 lG** - 36.9 26.9 28.4 28.8 MP2/6-3 1 G* - 33.5 25.2 26.2 26.4 MNDO 33.3 32.5 21.6 21.7 21.6 AMI 50.8 55.1 42.8 43.0 42.3 PM3 31.3 29.8 21.3 21.8 21.2
a Experimental value 35 kcalmol-’ [5].
method. For IA the calculated dipole moments are
in good agreement with the experimental value
(3.67 (5)D) obtained from Stark-effect measure-
ments [2]. Semiempirical calculations lead to
results of similar quality (MNDO 3.48 D; AM1
3.60D; PM3 3.86D). The substitution of methyl
groups at Nl and C5 increases the dipole
moment, whereas substitution at C2 and C4
decreases the dipole moment. The sequence of
the magnitude of dipole moments of IA, 2-MIA,
4-MIA and 5-MIA is the same as for the corre-
sponding methyl oxazoles [17].
Conclusion
Accurate structures of IA and its methyl deriva-
tives were determined. The heats of formation of
the methyl substituted species were obtained by
using isodesmic reaction schemes. The semiempiri-
cal MNDO and PM3 methods give good results for
IA. AM 1 predicts much higher heats of formation
for the type of molecules studied than any other
method. The predicted methyl group torsional
barriers may be used to assist in the assignment
of the microwave spectra of the MIA. The
sequence of the magnitudes of the dipole moments
and the torsional barriers resembles those of the
methyl oxazoles.
Table 7 Dipole moments (D)
IAa I-MIA 2-MIA 4-MIA 5-MIA
HF/6-31G* 3.86 4.17 3.72 3.60 4.03 HF/6-31 lG** 3.85 4.19 3.73 3.55 4.06 MP2/6-31G* 3.84 4.13 3.68 3.52 4.01
a Experimental value 3.67 (5) D [2].
M. Meyer/J. Mol. Struct. (Theochem) 304 (1994) 45-51
Acknowledgements
The calculations were carried out at the com-
puter centres of the GBF and Kiel University. 1
thank H. Hartwig at the Chemical Physics Depart-
ment of Kiel University for supporting this study.
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