ORIGINAL RESEARCH Properties, aromaticity, and substituents effects in poly nitro- and amino-substituted benzenes Irina V. Omelchenko • Oleg V. Shishkin • Leonid Gorb • Frances C. Hill • Jerzy Leszczynski Received: 11 December 2011 / Accepted: 4 February 2012 / Published online: 24 February 2012 Ó Springer Science+Business Media, LLC 2012 Abstract Geometrical parameters, aromaticity, and con- formational flexibility of the set of polysubstituted ben- zenes with different number and position of nitro and amino groups were calculated at the MP2/cc-pvdz level of theory. The key factor for structural and energetic changes has been identified. This is related to the presence of nitro and amino groups in vicinal positions that forms strong intramolecular resonance-assisted hydrogen bonds with a binding energy of 7–14 kcal/mol. Increasing number of such bonds facilitates a cooperative effect, inducing nota- ble changes in molecular geometry (particularly increasing bond alternation within H 2 N–C–C–NO 2 fragment and planarization of amino group), drastic increasing of con- formational flexibility and decreasing of aromaticity. In spite of well-known p-electron effects of nitro and amino substituents, influence of their push–pull interaction through aromatic moiety is negligible compared to the effect of the hydrogen bonding. That results in great dif- ference of the ortho-isomers as compared to meta- and para-isomers. Keywords Aromaticity Á Push–pull effect Á Intramolecular hydrogen bond Á Quantum chemical calculations Introduction Aromaticity is one of the most general and important concepts in organic chemistry [1]. This phenomenon also provides the background to understanding the influence of substituents on reactivity and stability of the very wide range of organic species containing aromatic and hetero- aromatic moieties. The numerous examples of such influ- ence are available in the literature elsewhere [2–4]. Among them, famous Hammett’s constants describing electronic strength of substituents were derived for aromatic mole- cules. Using this approach, it is very easy to understand that mechanism of such influence also including changes in aromaticity of benzene ring. Influenced by the Hammett equation, there have been numerous attempts to describe substituent effect on aro- matic moiety quantitatively [5]. The common way is the usage of some characteristic physicochemical properties (such as amino group basicity, catalytic activity, change of infrared, or NMR properties of substance) as an aromaticity measure [6]. Such characteristics are usually called aro- maticity indexes. Recently, aromaticity indexes were used to estimate substituent effect [7, 8]. Analysis of mono- substituted benzenes revealed that influence of a single Electronic supplementary material The online version of this article (doi:10.1007/s11224-012-9971-8) contains supplementary material, which is available to authorized users. I. V. Omelchenko (&) Á O. V. Shishkin STC’Institute for Single Crystals, National Academy of Sciences of Ukraine, 60 Lenina Ave, Kharkiv 61001, Ukraine e-mail: [email protected]O. V. Shishkin V.N. Karazin Kharkiv National University, 4 Svobody sq, Kharkiv 61077, Ukraine L. Gorb Badger Technical Services, LLC, Vicksburg, MS, USA F. C. Hill Á J. Leszczynski US Army ERDC, 3532 Manor Dr, Vicksburg, MS 39180, USA J. Leszczynski Interdisciplinary Center for Nanotoxicity, Department of Chemistry and Biochemistry, Jackson State University, P.O. Box 17910, 1325 Lynch Street, Jackson, MS 39217, USA 123 Struct Chem (2012) 23:1585–1597 DOI 10.1007/s11224-012-9971-8
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ORIGINAL RESEARCH
Properties, aromaticity, and substituents effects in polynitro- and amino-substituted benzenes
Irina V. Omelchenko • Oleg V. Shishkin •
Leonid Gorb • Frances C. Hill • Jerzy Leszczynski
Received: 11 December 2011 / Accepted: 4 February 2012 / Published online: 24 February 2012
� Springer Science+Business Media, LLC 2012
Abstract Geometrical parameters, aromaticity, and con-
formational flexibility of the set of polysubstituted ben-
zenes with different number and position of nitro and
amino groups were calculated at the MP2/cc-pvdz level of
theory. The key factor for structural and energetic changes
has been identified. This is related to the presence of nitro
and amino groups in vicinal positions that forms strong
intramolecular resonance-assisted hydrogen bonds with a
binding energy of 7–14 kcal/mol. Increasing number of
such bonds facilitates a cooperative effect, inducing nota-
ble changes in molecular geometry (particularly increasing
bond alternation within H2N–C–C–NO2 fragment and
planarization of amino group), drastic increasing of con-
formational flexibility and decreasing of aromaticity. In
spite of well-known p-electron effects of nitro and amino
substituents, influence of their push–pull interaction
through aromatic moiety is negligible compared to the
effect of the hydrogen bonding. That results in great dif-
ference of the ortho-isomers as compared to meta- and
para-isomers.
Keywords Aromaticity � Push–pull effect �Intramolecular hydrogen bond � Quantum chemical
calculations
Introduction
Aromaticity is one of the most general and important
concepts in organic chemistry [1]. This phenomenon also
provides the background to understanding the influence of
substituents on reactivity and stability of the very wide
range of organic species containing aromatic and hetero-
aromatic moieties. The numerous examples of such influ-
ence are available in the literature elsewhere [2–4]. Among
them, famous Hammett’s constants describing electronic
strength of substituents were derived for aromatic mole-
cules. Using this approach, it is very easy to understand
that mechanism of such influence also including changes in
aromaticity of benzene ring.
Influenced by the Hammett equation, there have been
numerous attempts to describe substituent effect on aro-
matic moiety quantitatively [5]. The common way is the
usage of some characteristic physicochemical properties
(such as amino group basicity, catalytic activity, change of
infrared, or NMR properties of substance) as an aromaticity
measure [6]. Such characteristics are usually called aro-
maticity indexes. Recently, aromaticity indexes were used
to estimate substituent effect [7, 8]. Analysis of mono-
substituted benzenes revealed that influence of a single
Electronic supplementary material The online version of thisarticle (doi:10.1007/s11224-012-9971-8) contains supplementarymaterial, which is available to authorized users.
I. V. Omelchenko (&) � O. V. Shishkin
STC’Institute for Single Crystals, National Academy of Sciences
mechanism and its energetic barrier, biological activity,
photoelectronic properties, etc., are widely discussed in
such studies. However, there are much less studies focused
on aromaticity and cooperative substituent effects of amino
and nitro groups [11–13].
In this article, we study the dependence of structural
parameters of molecular system, aromaticity of benzene
ring, and its rigidity on the nature, amount, and the position
of substituents. The aminonitrobenzene derivatives having
different number and position of amino and nitro groups
are selected as the model systems to investigate coopera-
tive influence of substituents.
R4
R3
R2
R1
R6
R5
1
2
34
5
6
Methods of calculation
The structures of all examined molecules (Table 1) have
been optimized using the Møller–Plesset second-order
perturbation theory [31] with correlation-consistent double-
zeta basis set [32] (MP2/cc-pVDZ method). Normal
vibrational modes were founded by calculations of Hes-
sian, at the same level of theory. No negative eigenvalues
of Hessian were found for the studied species.
Aromaticity of molecules under study was described by
aromaticity indices [33]. All indices have restrictions in use
[34]; therefore, it is preferred to use several different
indices [35–38]. In this study, structural Bird (Ia) [39] and
HOMA [40] indices, and magnetic index NICS(1)zz [41]
were used. As for commonly used energetic indices, there
is no unambiguous scheme of calculation of aromatic sta-
bilization energies (ASE) for polysubstituted molecules
[34] using the most reliable homodesmotic reaction
scheme.
It was already demonstrated [8, 42–44] that aromaticity
of cyclic conjugated system is closely related with its
conformational flexibility. Energy of ring out-of-plane
deformation and other characteristics of ring flexibility
correlate well with aromaticity degree. Therefore, they also
may be used as aromaticity indices.
1586 Struct Chem (2012) 23:1585–1597
123
All aromaticity indices (Ia, NICS(1)zz, HOMA) were
calculated using MP2/cc-pVDZ level of theory. Gordy
bond order calculation scheme [45] with empirical con-
stants was applied to calculation of Ia index according to
the standard equation [33]. Nucleus-independent chemical
shifts were calculated in the point located by 1 A above the
center of the ring (NICS(1)zz) as it was recommended [46]
for obtaining more accurate data.
Conformational flexibility of rings was studied on the
same level of theory by scan of each of symmetry-inde-
pendent endocyclic torsion angles in the range ±30� with
5� steps. All remaining geometrical parameters were opti-
mized at every step of scan. For each molecule, the angle
with the smallest energy of deformation E(def) (difference
in energy between equilibrium and twisted on 30� geom-
etries) was chosen.
All calculations have been performed using the
Gaussian03 [47] and GAMESS US [48] program packages.
Electron density properties were studied using Bader’s
‘‘Atoms in Molecules’’ theory (AIM) with AIM2000 pro-
gram [49] Energy of intramolecular hydrogen bonds was
estimated following the Espinosa equation [50] based on
value of local potential energy in bond critical point for
interaction.
Results and discussion
Molecular structure
Homosubstituted molecules
Analysis of the structural parameters of homosubstituted
molecules reveals good agreement of the current data with
the previous results [8, 11, 15]. Presence of nitro substit-
uents leads to small elongation of the C–C bond lengths
through the whole ring (1.398–1.406 vs 1.394 A in ben-
zene) and to increasing of ipso bond angle (120.3–123.2).
Only the angle at the ‘‘central’’ NO2 group in the 1,2,3-
trinitrobenzene (123N) slightly decreases (118.0). As for
aminobenzenes, the geometric changes are more pro-
nounced but local elongation of bonds is limited to the
Ci–Co bonds (1.407–1.417 A). Ipso bond angles slightly
decrease (117.8�–119.8�). Thus, the homosubstitution
affects molecular structure of the benzene ring according to
the r-electronic effect model. Experimental data for the gas
phase reveal the same trend (see Tables 2, 3 and references
below), except the nitrobenzene case with notable alter-
nation of the bond length (1.375 A Ci–Co bonds, 1.403 A
Co–Cm, and 1.396 A Cm–Cp).
In the nitrobenzene, as well as in 1,3- and 1,4-dinitro-
benzenes, the nitro group tends to be coplanar with aromatic
ring through conjugation of their p-systems. 1,2-dinitro-
benzene and polynitrobenzenes with adjacent nitro groups
undergo notable steric repulsion that can be roughly esti-
mated by examination of torsion angle between planes of
base ring and substituent (Table 2). The maximum rotation
angle corresponds to ‘‘central’’ nitro group in 1,2,3-trini-
trobenzene that undergo the maximum repulsion. Rotation
of these nitro groups causes no evident structural effect on
the aromatic moiety (see Table S1 in Supplementary mate-
rial). However, one can note decreasing of the C–NO2 bond
length for adjacent nitro groups. In addition, big values of
rotation angles result in reducing the p-conjugation with
aromatic system. At the time, there is very weak but quite
clear trend for elongation of the C–N bond for substituents
located in meta-position, with respect to para-position.
As for aminobenzenes, C–NH2 bond length and pyramidality
of NH2 group increases in the ortho- and para-diaminobenzenes
in comparison with aniline and meta-diaminobenzene, and
in the ortho,para-triaminobenzene (124A) in comparison
Table 1 Molecules under consideration
Molecule R1 R2 R3 R4 R5 R6
Benzene H H H H H H
1N NO2 H H H H H
12N NO2 NO2 H H H H
13N NO2 H NO2 H H H
14N NO2 H H NO2 H H
123N NO2 NO2 NO2 H H H
135N NO2 H NO2 H NO2 H
1A NH2 H H H H H
1N2A NO2 NH2 H H H H
1N3A NO2 H NH2 H H H
1N4A NO2 H H NH2 H H
13N2A NO2 NH2 NO2 H H H
13N4A NO2 H NO2 NH2 H H
13N5A NO2 H NO2 H NH2 H
135N2A NO2 NH2 NO2 H NO2 H
12A NH2 NH2 H H H H
13A NH2 H NH2 H H H
14A NH2 H H NH2 H H
1N24A NO2 NH2 H NH2 H H
1N35A NO2 H NH2 H NH2 H
13N24A NO2 NH2 NO2 NH2 H H
13N25A NO2 NH2 NO2 H NH2 H
123N46A NO2 NO2 NO2 NH2 H NH2
135N24A NO2 NH2 NO2 NH2 NO2 H
124A NH2 NH2 H NH2 H H
135A NH2 H NH2 H NH2 H
1N246A NO2 NH2 H NH2 H NH2
13N246A NO2 NH2 NO2 NH2 H NH2
135N246A NO2 NH2 NO2 NH2 NO2 NH2
Struct Chem (2012) 23:1585–1597 1587
123
with meta,meta-isomer (135A) (Table 3). Adding extra
amino groups results in elongation of C–NH2 bond lengths in
all isomers as compared to aniline. Presence of amino groups
increases vicinal endocyclic C–C bond length up to
1.410–1.419 A (1.394 A for benzene) regardless of the rel-
ative substituents position. This effect is larger than analo-
gous increase predicted for any nitrobenzene derivatives
(1.398–1.406 A, Table S1 in Supplementary material).
Therefore, one may conclude that structure of the ben-
zene moiety is quite resistant to the perturbations caused by
the presence of several nitro groups and, in some less
extent, one or two amino groups (see Table S1 in Sup-
plementary material).
Isomeric nitroanilines
Molecules with both p-donor and p-acceptor substituents
are considered to reveal strong push–pull effect [10] that is
transmitted through aromatic system. It should change
molecular structure of ortho- and para-isomers according
to the quinoid canonical resonance structures with partial
charge transfer through p-system. Scheme 1 represents a
set of canonical structures for para-nitroaminobenzene.
Therefore, ortho- and para-nitroanilines 1N2A and 1N4A
are expected to reveal alternation in the benzene ring,
shortening of the C–NH2 and the C–NO2 bond lengths,
and flattening of the amino group, in contrast to meta-
nitroaniline 1N3A which does not share a push–pull effect
[10].
However, the results of calculation do not reveal sig-
nificant deformation of bond lengths within benzene ring in
para-isomer 1N4A as compared to meta-isomer 1N3A.
Slight changes in bond lengths may be explained by
superposition of the effects of nitro and amino groups
mentioned above (see Tables S1, S2 in Supplementary
material). There are only some shortening of the C–NH2
bond and flattening of amino group as compared to aniline.
These effects reflect conjugation interactions between
substituents (Table 4).
Table 2 Values of the C–N bond lengths (A) and the C–C–N–O
torsion angles (�) in nitrobenzenes
Molecule C–NO2 C–C–N–O
1N 1.483 0.0
Exp.a 1.492(1) 0.0(1)
12N 1.472 42.5
13N 1.487 0.0
14N 1.482 0.0
123N 1.477 (C1) 35.8
1.473 (C2) 62.4
135N 1.489 0.0
Identical values for symmetrically equivalent groups are omitteda Gas-phase electron diffraction and microwave spectroscopy
experiment, rs distances [51]
Table 3 Values of the C–N bond lengths (A), pyramidality of amino
group estimated as sum of bond angles centered at the nitrogen atom
(P
(NH2), �), and angle between planes of amino group and benzene
ring (u(NH2), �) in amino benzenes
C–NH2
P(NH2) u(NH)
1A 1.410 332.2 44.4
Exp.a 1.406(3) 44(4)
Exp.b 1.402(2) 37(2)
12A 1.416 328.7 54.6
13A 1.413 331.2 50.0
14A 1.417 329.5 51.3
Exp.c 1.422(2) 43(4)
124A 1.423 (C1) 326.8 57.0
1.415 (C2) 329 53.7
1.418 (C3) 329.2 51.8
135A 1.414 (C1, C5) 330.5 50.6
1.414 (C3) 330.9 50.3
Identical values for symmetrically equivalent groups are omitteda Gas-phase electron diffraction experiment, rg distances [52]b Gas-phase microwave and electronic spectroscopy experiment [53]c Gas-phase electron diffraction experiment, rg distances [54]
NH H
N+
OO
NH H
N+
OO
NH H
N+
OO ON
+O
NH H
ON
+O
NH H
ON
+O
NH H
ON
+O
NH H
+ +
+
+ +
-
- - +
+
Scheme 1 Canonical resonance structures for para-nitroaminobenzene (1N4A)
1588 Struct Chem (2012) 23:1585–1597
123
In ortho-isomer, the C–NH2 bond length is notably
shorter, and amino group is more flattened than in meta-
and para-isomers (Table 4). Nitro group in 1N2A is not
coplanar to benzene ring (Table 4) and the C–NO2 bond is
slightly shorter than in 1N3A and 1N4A. That is accom-
panied by alternation of endocyclic bond lengths (short-
ening of C(3)–C(4) and C(5)–C(6) bonds) and by
decreasing of the CC(NH2)C angle. Although such struc-
tural changes are typical for conjugative interaction as
well, no similar changes are observed in the para-nitro-
aniline structure. Thus, para- and meta-nitroanilines pos-
sess very close geometrical parameters that differ from
ortho-nitroaniline. This set of data does not match the
values expected due to push–pull effect but may be caused
by direct local interaction between vicinal substituents.
These results do not match experimental results obtained
from X-ray diffraction study of the crystalline state [56–59]
in which noticeable structural changes that correspond to
the push–pull effect are clearly observed in both ortho-
[56] and para- [57, 58] nitroanilines as compared to meta-
nitroaniline [59]. However, effect of the polar medium and
strong intermolecular hydrogen bonding that are observed
in crystals of all isomeric nitroanilines can affect properties
related to the p-electron system dramatically [60, 61].
These effects are a subject of particular study and therefore
crystal structure data as well as data obtained in polar
solvents cannot be a reference for molecules examined in
vacuum. Available gas-phase data exist only for para-
nitroaniline. Experimental C–NH2 and C–NO2 bond
lengths are some smaller than calculated (Table 4) but
precision of their determination is rather low, and only
averaged endocyclic bond length was given (rg(C–C) =
1.402(4) A). Thus, push–pull effect cannot be revealed
from these data.
Analysis of the electron density distribution using
Bader’s AIM theory demonstrated existence of the
N–H���O hydrogen bond between substituents bonding
(H���O 1.957 A, N–H���O 125.6�). Taking into account that
proton donating and withdrawing sites of this bond are
connected by benzene ring as resonant spout it is possible
to consider it [62–66] as resonance-assisted hydrogen bond
(RAHB) (Scheme 2). Considerable contribution of the
resonance structure C in the total structure of the 1N2A
molecule should cause shortening of the C–N bonds, flat-
tening of amino group mentioned above, and elongation of
the C1–C2 endocyclic bond which is 1.420 A. Taking into
account pyramidal configuration of amino group rotation of
the nitro group creates more favorable conditions for for-
mation of the N–H���O hydrogen bond. The N–O bond of the
nitro group of 1N2A that participates in RAHB is slightly
longer (1.240 A) than the other N–O bond (1.231 A). In all
other nitroanilines and homosubstituted molecules under
study, length of the N–O bonds of nitro groups are the same.
Therefore, some deformation of geometry of 1N2A may be
explained by the formation of intramolecular RAHB rather
than push–pull p-electronic effects.
Polyheterosubstituted molecules
Geometrical parameters of polynitroaminobenzenes vary in
a much more wide range than parameters of species dis-
cussed above. The specific structural feature of highly
substituted molecules with adjacent nitro and amino sub-
stituents is reflected by a minor non-planarity of benzene
rings in equilibrium geometry (endocyclic torsion angles
vary up to 6�, see Table 5). In the previous theoretical
studies of 2,4,6-triamino-1,3,5-trinitrobenzene (135N246A,
TATB), it was found that degree of non-planarity of mol-
ecule strongly depends on the level of theory and quality
of basis applied to chemical modeling [15, 29, 67–69].
High-quality calculations reveal non-planarity of TATB
Table 4 Values of the C–N bond lengths (A), pyramidality of amino
group estimated as sum of bond angles centered at the nitrogen atom
(P
(NH2), �) and the C–C–N–O torsion angles (�) in nitroanilines,
nitrobenzene, and aniline
Molecule C–NH2
P(NH2) C–NO2 C–C–N–O
1N – – 1.483 0.0
1A 1.410 332.2 – –
1N2A 1.387 341.3 1.473 16.1
1N3A 1.400 335.8 1.475 0.9
1N4A 1.400 336.2 1.481 0.3
Exp.a 1.36(3) (360) 1.47(1) (0)
a Gas-phase electron diffraction experiment, rg distances [55]. Values
in parenthesis were fixed during experiment analysis so they are non-
informative
N+
NH
OOH N
+
N+
O OH
H
N+
N
H
H
OO
A B C
Scheme 2 Resonance
structures proposed for
hydrogen bonding of ortho-
nitroaniline
Struct Chem (2012) 23:1585–1597 1589
123
molecule in equilibrium geometry that arises from an
extremely low energy of out-of-plane deformation of
molecule [12]. Experimental values of torsion angles [70]
measured by XRD method cannot be hold as reference due
to the strong influence of polar medium and intramolecular
interactions in crystal.
As may be seen from Table 5, non-planarity of benzene
ring is observed mainly for molecules with at least two
nitro groups and two vicinal locations of nitro and amino
groups. This allows to assume that non-planarity is caused
by interaction between these substituents.
Analysis of bond lengths within benzene ring in poly-
substituted molecules indicates only one type of deformation
namely elongation of bonds. No alternation of bonds is
observed. The most significant elongation is found for mol-
ecules with vicinal arrangement of nitro and amino groups
(Table 6). In these cases, length of the C–C bond between
substituents is within 1.421–1.446 A. These values are dis-
tinct from the value of bond length in benzene (1.394 A).
This effect is promoted by increase of number of vicinal nitro
and amino groups and it becomes maximal in symmetric
trinitrotriaminobenzene 135N246A (Table 6).
Geometrical parameters of substituents reveal the same
tendency as in the case of nitroanilines. Vicinal location of
nitro and amino groups results in shortening of the C–NH2
bonds, flattening of the NH2 group, and nitro group rotation
with respect to the ring plane (Table 7). In the series of
isomeric dinitroanilines, diaminonitrobenzenes, and diam-
inodinitrobenzenes, amino groups adjacent to the two nitro
groups (13N2A and amino group at the C2 atom of
13N24A) reveals the shortest C–NH2 bond (1.360–1.364 A)
and the most planar amino group (pyramidality degree
described as sum of bond angles centered at the nitrogen
atom is within 350.5�–352.6�). Amino groups in the 13N4A,
123N46A, at the C2 atom of the 1N24A and at the C4 atom of
13N24A (ortho-positions, with one nitro group adjacent to