A computational study on the substituent effects and product stereoselectivity of the intermolecular...
Transcript of A computational study on the substituent effects and product stereoselectivity of the intermolecular...
A computational study on the substituent effects and product stereoselectivity
of the intermolecular formal aza-[3C3] cycloaddition reaction between
vinylogous amides and a,b-unsaturated imine cations
Yan Wang, De-Cai Fang *, Ruo-Zhuang Liu **
College of chemistry, Beijing Normal University, 19th Xin Wai St., Beijing 100875, China
Received 23 March 2006; received in revised form 31 May 2006; accepted 1 June 2006
Available online 10 June 2006
Abstract
The substituent effects and product stereoselectivity of the title reaction has been studied using density functional theory (DFT) calculations at
the B3LYP/6-31G(d,p) level of theory. It was found that the substituents do not perturb the mechanism of intermolecular formal aza-[3C3]
cycloaddition. Our calculations also show that methyl or benzyl groups on the N atom of vinylogous amide favor the addition step, but alkyl
substituents on the either N atom or terminal C atom of a,b-unsaturated imine cation have opposite effects. Alkyl substituents on the N atom of
a,b-unsaturated imine cation may lower the activation barriers for elimination of amide. The steric interaction between two substituents leads to
the formation of major product both thermodynamically and kinetically.
q 2006 Elsevier B.V. All rights reserved.
Keywords: [3C3] Cycloaddition; Vinylogous amide; a, b-Unsaturated imine cation; DFT calculations; Substituent effects; Stereoselectivity
1. Introduction
The reactions of vinylogous amides with a,b-unsaturated
iminium salts leading to 1,2-dihydropyridines [1–8] (Scheme 1)
have attracted intensive attention of experimental chemists in
recent years as these reactions may be used to synthesize various
piperidinyl heterocycles, representing useful fundamental
synthetic building blocks. This type of reaction may be charac-
terized as a formal aza-[3C3] cycloaddition reaction [9–13] due
to the fact that each portion provides three atoms to form a new
six-membered heterocycle in either intermolecular [1–4] or
intramolecular [5–7] fashion. Experimental chemists have
also assumed that intermolecular reactions involve a sequence
that consists of C-1,2-addition to an iminium salt followed by
b-elimination giving an 1-azatriene and a 6p-electron electro-
cyclic ring-closure of 1-azatriene as shown in Scheme 1,
proceeding with high stereoselectivity (Scheme 2). In previous
work, a simple model of the above intermolecular reaction has
been studied theoretically [14] (Scheme 3). However, the
substituent effect and stereoselectivity are still unreported.
0166-1280/$ - see front matter q 2006 Elsevier B.V. All rights reserved.
doi:10.1016/j.theochem.2006.06.004
* Corresponding authors. Tel./fax: C86 10 58805422.
E-mail addresses: [email protected] (D.-C. Fang), [email protected]
(R.-Z. Liu).
In this article, 12 differing substituted modes, as shown in
Scheme 4, are reported to elucidate the substituent effect and
stereoselectivity.
2. Computational methods
All calculations were carried out with Gaussian 03 suite of
programs [15]. The structures of reactants, complexes, tran-
sition states, intermediates and products were optimized at
density functional theory (DFT) B3LYP level using the
6-31G(d,p) basis set. The stationary points were characterized
by frequency calculations in order to verify that minima and
transition structures (TS) have zero and one imaginary
frequency, respectively. Zero-point energy (ZPE) corrections
were included without scaling. The solvent effects were
considered by performing B3LYP/6-31G(d,p) single-point
calculations on the gas-phase optimized geometries using the
self-consistent reaction field (SCRF) method based on the
polarizable continuum model (PCM) [16–25], in which
toluene was used as solvent to mimic experimental conditions
(3Z2.379).
3. Results and discussions
As shown in Scheme 3, there are three generalized steps for
the reactions investigated herein. The first step is the addition
Journal of Molecular Structure: THEOCHEM 770 (2006) 169–178
www.elsevier.com/locate/theochem
Scheme 1.
Y. Wang et al. / Journal of Molecular Structure: THEOCHEM 770 (2006) 169–178170
reaction between two reactants 1 and 2 with formation of a
cationic intermediate INT1. The second step is the removal of
HC and subsequent 1,4-elimination of HNR12 (NH3 in parent
reaction) from INT1 to form a molecular intermediate INT3
promoted by the nucleophilic attack of AcOK in the reaction
medium. The final step is the subsequent isomerization of
INT3 and electrocyclic ring-closure yielding the final
product. The differing substituent groups in varied positions
do not change the above mechanism, however stereoselectivity
for the final products is evident, rationalized in the following
discussion.
3.1. Substituent effect on the addition step
In this section, because trans-isomer of 2 is more stable
than cis-one (4.9–8.8 kcal/mol), only trans-isomer of 2 was
considered. The addition step proceeds via a transition state
Scheme
(TS1) connecting INT1 directly with complex (COM1)
between 1 and 2. Three substitution sites investigated
herein are as follows: N atom of 1, N atom of 2 and terminal
C atom of 2. The inclusion of larger substituents leads to
more complicated structures of COM1, as shown in Fig. 1,
along with the values of intermolecular distance for H/O.
Three types of structures for COM1 have been located in the
12 cases considered, in which two conformers are stabilized
in the form of intermolecular ionic [26] C–H/O hydrogen
bonding [27–30], denoted as COM1-X and COM1-Y,
respectively. Another type of complexes is produced in the
form of intermolecular ionic N–H/O hydrogen bonding
denoted as COM1-Z. Due to the fact that N–H/O type
hydrogen bonding is usually stronger than C–H/O, N–H/O hydrogen bonded complexes, for reactions h and l, can be
optimized. Extensive exploratory searches on the complexes
for reactions b, d and f located only one C–H/O hydrogen
bonded complex, as indicated in Fig. 1. The energy
difference for two different C–H/O hydrogen bonded
complexes is very small, usually less than 0.3 kcal/mol, so
it is not important to differentiate them. By comparing the
bond length of H/O in Fig. 1 with energy changes in
Table 1, it is clear that the longer H/O is, the weaker the
intermolecular stabilization of the complex is. The molecular
graphs of TS1 and INT1, obtained with the AIM2000
program [31,32], are depicted in Fig. 2, from which it can
be found that inclusion of methyl or benzyl groups at the N
atom of 1 may shorten the intermolecular distance for H/O
of COM1, but also increases the length of the C–C bond
forming in TS1. Opposite effects are observed for alkyl
groups at the N or terminal C atom of 2.
The computed relative energies of stationary points for the
addition step are listed in Table 1, from which one may observe
2.
Scheme 3.
Y. Wang et al. / Journal of Molecular Structure: THEOCHEM 770 (2006) 169–178 171
that the substituted groups affect the relative energies of TS1
and INT1 more significantly than that of COM1. The methyl
or benzyl groups of R2 can lower the relative energies of
COM1, TS1 and INT1, while opposite effects are seen for
Scheme
alkyl groups of R1 or R3. In addition, methyl or benzyl groups
of R2 can give an early and more stable transition state along
the reaction path, while alkyl groups of R1 or R3 have inverse
effects. When all three substituent positions are other than
4.
Fig. 1. Three conformations of COM1, including the intermolecular distances (A) for H/O optimized at the B3LYP/6-31G(d,p) level of theory and eight structures
of INT3.
Y. Wang et al. / Journal of Molecular Structure: THEOCHEM 770 (2006) 169–178172
hydrogen atoms, the overall result is an elevation of relative
energies for COM1, TS1 and INT1.
For reactions a and f, the relative energies of SCRF-
B3LYP/6-31G(d,p) single-point calculations are very close
to those of the optimized geometries in solution phase at
same level (see Table 1). Thus, the solvent effects were
characterized by SCRF-B3LYP/6-31G(d,p) single-point
calculations on the gas-phase optimized geometries,
employing the relatively simple polarizable continuum
model (PCM) [16–25]. The relative energies in toluene
together with relative free energies of stationary points for
reactions a and f only either in gas phase or in solution
phase are also summarized in Table 1 from which one may
observe that the solvent makes ionic reactant 2 more stable
and leads to the relative energies of COM1, TS1 and
INT1 in toluene being higher than corresponding results in
gas phase, which is similar to the parent reaction (without
any substituted groups). The changes of the relative
energies of COM1, TS1 and INT1 are 8–14, 5–13 and
6–15 kcal/mol, respectively. In consequence, the inclusion
of solvent is not in favor of addition step, both thermo-
dynamically and kinetically. From Table 1, it can also be
found that the influences of the substituted groups and the
solvent toluene on relative free energies are similar to
those on relative energies although the magnitude of
relative free energies is different somewhat from that of
relative energies, i.e. the trend of change of relative
energies is the same as that of relative free energies.
Table 1
The B3LYP/6-31G(d,p) computed relative energies with ZPE correction and relative free energies (DE and DG298 K, kcal/mol) of stationary points for addition step
COM1-X COM1-Y COM1-Z TS1 INT1
DE DG DE DG DE DE DG DE DG
a K26.5 K26.3 K16.8 K4.8 7.9 K14.2 K1.7
(K14.8)a (K14.8) (4.1) (K5.4)
[K13.6]b [K4.1] [5.1] [17.5] [K3.0] [9.5]
b K23.5 7.7 K1.2
(K14.5) (12.3) (3.7)
c K27.8 K27.5 K8.5 K19.7
(K15.2) (K15.1) (2.1) (K8.2)
d K24.6 3.1 K6.1
(K14.9) (10.2) (0.8)
e K28.5 K28.4 K11.1 K21.6
(K15.2) (K15.2) (1.6) (K8.7)
f K22.9 K13.6 6.1 19.1 K1.5 12.1
(K13.6) (12.6) (5.6)
[K12.2] [K1.8] [13.5] [26.7] [7.1] [20.6]
g K25.1 K24.8 0.3 K8.1
(K14.7) (K14.3) (9.3) (0.1)
h K30.3 4.2 K4.3
(K18.6) (10.0) (1.3)
i K23.1 K23.2 9.8 1.1
(K15.3) (K15.4) (15.0) (6.0)
j K21.7 K21.8 11.9 3.2
(K14.5) (K14.7) (16.4) (7.4)
k K21.9 K21.8 10.4 4.1
(K14.0) (K14.2) (15.6) (8.9)
l K28.9 6.3 K1.7
(K18.0) (11.5) (3.0)
a The data in parentheses are for solution phase single-point calculations.b The data in square bracket are optimized results in solution phase.
Y. Wang et al. / Journal of Molecular Structure: THEOCHEM 770 (2006) 169–178 173
In addition, the rate constants of addition reactions a, j and k
in toluene solution were calculated approximately according to
the transition state theory (TST) with POLYRATE program
[33]. The calculated results are shown in Table 2, from which
one can see that the rate constants for reactions j and k at room
temperature of 298.15 K, are quite small, but when the
temperature is raised to 423.15 K (experimental temperature),
the reactions can proceed in moderate rate.
3.2. Substituent effect on the elimination of HC and HNR12
From the previous work, one may observe that the elimin-
ation of NH3 has two pathways, which has no substantial
difference, so here only one situation is considered for
simplicity. The nucleophilic attack of the O atom in AcOK
on H atom of C1 in INT1 forms complex COM2, corre-
sponding to a molecular complex between AcOH and INT2.
The combination of one anion (AcOK) with cationic inter-
mediate INT1 is barrier-less. There exists a novel
intramolecular N–H/N hydrogen bond in INT2, which is
relevant to HNR12 elimination. The removal of HNR1
2 from
INT2 is finalized via TS2 by way of an 1,4-elimination to form
an intermolecular hydrogen bonded complex COM3 between
HNR12 and INT3 on the reaction profile. The geometries of
INT2 and TS2 are given in Fig. 2 together with the values of
the bond lengths directly involved in the reaction mechanism.
The computed relative energies of stationary points for HC
and HNR12 elimination are listed in Table 3, from which one
can see that the energies of the optimized stationary points are
below those of AcOKCINT1. The energy barriers for
the subsequent removing of HNR12 range from 18.1 to
24.8 kcal/mol, in which that of reaction f is the smallest.
Such barriers are easily overcome due to the larger exothermic
effect for the formation of COM2. For example, more than 130
(in gas phase) or 70 kcal/mol (in toluene solution) of energy is
released (see Table 3).
The energy of AcOK in solution is lowered by much more
than those of other stationary points, thus the relative energies
of neutral molecules are raised noticeably in toluene solvent.
However, solvent effect does not have a noticeable influence on
the energy barrier of HNR12 elimination, as neutral molecules
are stabilized to approximately uniform extent by less polar
solvent.
3.3. Substituent effect on isomerization and cyclization
Following the two steps above, the remaining INT3 has
only eight different forms (Fig. 1), of which the former five will
yield two identical products and hence only the latter three
INT3j, INT3k and INT3l are discussed here (see Scheme 5). It
must be indicated that the methyl group in cyclohexane chair
conformation is in either equatiorial or axial form, but only
Fig. 2. Molecular graphs of some optimized stationary points in the gas phase (obtained with the AIM2000 program). The bond lengths directly involved in the
reaction are given in angstrom and the nuclear repulsion energies are given in atomic unit.
Table 2
The rate constants k (cm3 molK1 sK1) of addition reaction a, j and k in toluene
solution
298.15 K 423.15 K
a 3.49!104 6.91!105
j 6.68!10K6 6.34!10K2
k 2.64!10K6 1.84!10K2
Y. Wang et al. / Journal of Molecular Structure: THEOCHEM 770 (2006) 169–178174
equatiorial form will be discussed in this section as it is more
stable for a bulky group to be in the equatiorial position. It was
also found that toluene as solvent has only negligible influence
on the geometries and relative energies of isomerization and
final cyclization, due to only neutral species being involved in
these steps. Therefore, only gas phase results are reported for
reactions j, k and l herein.
Table 3
The B3LYP/6-31G(d,p) computed relative energies (DE, kcal/mol) with ZPE correction of stationary points for HC and HNR12 elimination step
INT1CAcOK COM2 INT2CAcOH TS2CAcOH COM3CAcOH INT3CHNR12CAcOH
a 0.0 K139.1 K132.9 K108.1 K121.3 K119.3
(0.0)a (K76.7) (K73.1) (K47.0) (K57.8) (K55.8)
[0.0]b [K74.4] [K72.0] [K47.8] [K59.8] [K58.9]
b 0.0 K136.6 K132.6 K111.0 K120.3 K117.5
(0.0) (K77.1) (K75.6) (K52.9) (K60.6) (K58.6)
c 0.0 K132.9 K126.5 K102.8 K117.3 K114.5
(0.0) (K73.6) (K70.0) (K44.5) (K56.6) (K53.5)
d 0.0 K131.7 K127.8 K107.3 K116.9 K114.2
(0.0) (K74.1) (K72.5) (K50.4) (K58.5) (K56.3)
e 0.0 K131.6 K124.9 K102.2 K116.3 K113.9
(0.0) (K72.7) (K68.9) (K44.3) (K56.4) (K53.4)
f 0.0 K130.0 K126.1 K108.0 K117.2 K114.4
(0.0) (K72.9) (K71.5) (K51.9) (K60.0) (K57.8)
[0.0] [K70.5] [K70.2] [K52.0] [K61.1] [K59.6]
g 0.0 K129.2 K125.4 K105.7 K115.7 K112.6
(0.0) (K72.7) (K71.2) (K49.9) (K58.8) (K55.9)
h 0.0 K136.4 K130.1 K105.8 K122.1 K118.5
(0.0) (K75.4) (K71.7) (K46.3) (K60.3) (K56.7)
i 0.0 K129.2 K125.4 K105.1 K116.8 K113.4
(0.0) (K72.6) (K71.1) (K49.7) (K59.9) (K56.9)
j 0.0 K128.5 K124.7 K104.3 K117.1 K112.7
(0.0) (K72.3) (K70.8) (K49.2) (K60.7) (K56.9)
k 0.0 K128.8 K125.6 K101.9 K114.3 K110.5
(0.0) (K72.9) (K72.4) (K47.9) (K58.5) (K55.2)
l 0.0 K135.5 K129.1 K105.0 K121.3 K117.7
(0.0) (K75.1) (K71.5) (K46.1) (K60.1) (K56.6)
a The data in parentheses are for solution phase single-point calculations.b The data in square bracket are optimized results in solution phase.
Y. Wang et al. / Journal of Molecular Structure: THEOCHEM 770 (2006) 169–178 175
After INT3j, the isomerization may take place in two
different directions, generating two different gauche inter-
mediates shown in Fig. 2, from which one may see that
the nuclear repulsion energy of INT4j 0 is about 14 a.u.
less than that of INT4j. The dihedral angle C4–C3–C2–
C1 in INT4j and INT4j 0 are K61.6 and 48.08, respect-
ively, which results from the differing steric repulsions of
substituents at the C1 and N7 atoms, while the corre-
sponding values for model reaction are only K29.0 and
30.08. The relative energies of INT4j and INT4j 0 are
increased by 3.6 and 2.6 kcal/mol, respectively, when
compared to the parent reaction. The difference of
nuclear repulsion energy between two TSs of the cycliza-
tion process is also about 14 a.u., leading to TS4j 0 being
approximately 4 kcal/mol lower than TS4j.
The potential energy surfaces obtained are shown in Fig. 3,
together with the relative free energies of stationary points for
reaction a either in gas phase or in solution phase, from which
one can realized that the relative free energies are very close to
relative energies for reaction a, i.e. the entropy factor is not
crucial for this process. From Fig. 3, it can also be seen that the
forming gauche intermediates are much less stable than the
trans intermediate INT3j. With the transition state theory
(TST), the reaction rate constants of isomerization from
INT3j to INT4j or INT4j 0, at an experimental temperature
of 423 K, are 1.896!107 and 2.758!107 sK1, respectively,
and those for the cyclization processes are 1.072!105 and
5.964!106 sK1, i.e. these two processes are comparable.
However, the processes of conversion from INT4j or INT4j 0
to INT3j are much faster, and the rate constants are 1.621!1012 and 7.011!1011 sK1, i.e. the concentrations of INT4j and
INT4j 0 in the reaction system are very small. Therefore, such
two-step reaction processes might be simplified to be one-step
in order to calculate the overall reaction rate constant from
INT3j to final products. The ratio of rate constants for
generating 3j and 3j 0 is 187.1, a little larger than the experi-
mental one. Such difference may be due to the DFT
approximation errors. If the energy of TS4j were lowered by
2 kcal/mol, the calculated ratio would be within experimental
one.
As for the reaction k, the difference for the relative
energies of two transition states TS4k and TS4k 0 are
comparable to their counterparts in reaction j (see Fig. 3)
and the energy difference for the final products is also
approximately 5 kcal/mol. The calculated overall rate
constants for the formation of two different products are
14.07 and 922.1 sK1, respectively, with our calculations
representing the experimental observed stereoselectivity. In
order to further characterize the intrinsic bases of high
stereoselectivity, a reaction (denoted as reaction l) with H
atom to replace methyl on N atom in reaction j has been
designed. From Fig. 3, it is clear that the final products
Scheme 5.
Y. Wang et al. / Journal of Molecular Structure: THEOCHEM 770 (2006) 169–178176
become more stable, almost equivalent to those of the
model reaction, indicating that the interaction between R2
and R3 groups not only makes final products unstable
relative to INT3 but also makes the energy difference
between two products increase.
4. Conclusions
According to the above discussions, the following con-
clusions may be drawn:
1. The substituted groups on three sites do not change the
overall reaction mechanisms.
2. The addition step is favored by substituting 1 with methyl
or benzyl groups while opposite effects are observed by
substituting 2 with alkyl groups at N and/or terminal C
atoms. Alkyl substituent groups on the N atom of the a,b-
unsaturated imine cation can lower energy barrier for the
elimination of HNR12 by approximately 3 kcal/mol or
perhaps more, while substituents at other positions
change the barrier only slightly, usually less than
1 kcal/mol.
3. The substituted groups on 1 and 2 can make the
isomerization and cyclization steps slightly less favorable
thermodynamically, and they can also lead to larger
energy difference between the two final products. The
formation of the major product is favored not only
thermodynamically but also kinetically.
4. Our calculated rate constants accounts for the experimen-
tally observed ratio of final products.
Fig. 3. Potential energy profile of the isomerization and cyclization step for reactions a, j, k and l. The data in parentheses are relative free energies DG298 K in gas
phase and the data in square bracket are relative free energies in solution phase.
Y. Wang et al. / Journal of Molecular Structure: THEOCHEM 770 (2006) 169–178 177
Acknowledgements
Authors L.R.Z. and F.D.C. express thanks to the Major State
Basic Research Development Programs (Grant no.
2004CB719900) for support and author F.D.C. thanks the
National Natural Science Foundation of China (no.
20372011) and the Program for New Century Excellent
Talents in University (NCET) for support.
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