Aminolysis of Aryl Chlorothionoformates
as the expulsion rate from T( decreases, the intermedi-
ate, T(, becomes more stable (stability of T( with anilines
is reported to be greater than that with secondary
alicyclic amines)11 and the possibility of a stepwise
mechanism increases, i.e., the aminolysis with anilines
is more likely to proceed by the stepwise mechanism than
with the secondary alicyclic amines under the same
reaction conditions.10 For example, the aminolyses of
O-ethyl S-(2,4-dinitrophenyl)- (9a: EtO-C(dO)‚SC6H3‚
2,4-(NO2)2) and O-ethyl S-(2,4,6-trinitrophenyl)carbon-
ates (9b: EtO-C(dO)‚SC6H2‚2,4,6-(NO2)3) have been
studied in water at 25 °C with amines of the increasing
order of expulsion rate from T(, pyridines12 < anilines11
of T( (to formation of T() to concerted with increasing
nucleofugality of the amines from T( is generally fol-
lowed, and an inversion of the sequence has rarely been
observed.
The stepwise mechanism predicted for 6 and 7 with
anilines in water is, however, in contrast to the concerted
mechanism found for the aminolysis of 6 with anilines
in acetonitrile.5 The solvent change from water to a less
polar solvent, MeCN, thus causes a mechanistic change
for 6 from stepwise in water to concerted in MeCN. The
change of solvent from water to acetonitrile destabilizes
the zwitterionic intermediate resulting in an increase in
the rate of expulsion of amines from T(. The lower
stability of T( leading to the higher expulsion rate of a
given amine from T( in a less polar solvent compared to
a more polar one is due to the zwitterionic nature of T(.
Mechanistic changes from stepwise to concerted incurred
by a solvent change from water to acetonitrile are often
observed. An example is the aminolysis of O-ethyl aryl
dithiocarbonate (EtO-C(dS)‚SAr), which proceeds by a
stepwise mechanism with pyridines8 and secondary ali-
cyclic amines21 in water but concertedly with anilines14
and benzylamines22 in acetonitrile. As noted above,
anilines should also react by the stepwise mechanism in
water since the expulsion rate of aniline is less than that
of the secondary alicyclic amines. Similarly, the aminoly-
sis of O-ethyl 2,4,6-trinitrophenyl dithiocarbonate is
stepwise with a biphasic plot in water, but is concerted
(âX ) 0.53) in a less polar solvent (44 wt % EtOH-H2O).23
This was attributed to the enhanced expulsion rate of
the amine from T( in the less polar solvent while the
nucleofugality of the leaving group remains practically
unaffected by the solvent nature resulting in the more
destabilized T( kinetically in the less polar solvent.23
It is therefore highly likely that the aminolysis of 7
with anilines in acetonitrile also proceeds by a concerted
mechanism.
We propose a concerted mechanism for the aminolysis
of aryl chlorothionoformate, 7, in acetonitrile on the
following grounds: (i) The rate sequence for the phenoxy
series, k2 (6 with CdO) > k2 (7 with CdS) in acetonitrile,
is a reverse of that for the alkoxy series, k2 (1 with CdO)
< k2 (3 with CdS) in water, reflecting a mechanistic
change from a rate-limiting formation of T( for the alkoxy
series in water to a concerted mechanism for the phenoxy
series in acetonitrile. A change of CdO to CdS leads to
a decrease in push provided to expel the leaving group,
Cl-, in the tetrahedral TS (8b), and this will result in a
decrease in the rate of the concerted process for 7 relative
to 6.4,8 Of course, the same rate decrease may be expected
from the intermediate, T( (8a), in a rate-limiting break-
down of T(. However, the stepwise mechanism with rate-
limiting breakdown of T( has never been found, either
for 6 or for 7 in water or in acetonitrile with any type of
amines. The stepwise mechanism with rate-limiting
formation of T( has been reported for 7 with pyridines
in water.4b Pyridines are known to have a stronger ability
to stabilize the intermediate, T(, than anilines,11 and
< secondary alicyclic amines13 < quinuclidines10a
<
(benzylamines).14 A gradual shift of mechanism was
observed from stepwise to concerted as the expulsion rate
of amine from T( increased: For the aminolyses with
pyridines both 9a and 9b were found to react by a
stepwise mechanism,11 whereas those with secondary
alicyclic amines13 and quinuclidines10a proceed by a
concerted mechanism. Quite interestingly, the aminolysis
with anilines12 is stepwise with 9a but is concerted with
9b, which should form a less stable intermediate than
9a due to the stronger nucleofugality of the trini-
trothiophenolate in 9b than the dinitrothiophenolate
leaving group in 9a. The aminolysis with benzylamines14
is also concerted (in acetonitrile). Similarly, the aminoly-
sis of aryl dithioacetates, 10, in acetonitrile is stepwise
with pyridines15 (with a change of the rate-limiting step
from breakdown, âX ) 0.9, to formation, âX ) 0.4, of T()
and anilines16 (with rate-limiting breakdown of T(, âX )
0.84), but is concerted with benzylamines16 (âX ) 0.55).
The aminolysis of 10 with secondary alicyclic amines17
was found to proceed by rate-limiting formation of T( in
water. Another interesting case is the aminolysis of aryl
dithiobenzoates (YC6H4C(dS)‚SC6H4Z) in acetonitrile.18-20
The intermediates, T(, are so stable that the reactions
are stepwise all the way from pyridines through anilines
to benzylamines in the increasing order of nucleofugality
of amines from T(. However, there is a subtle shift of
the rate-limiting step from biphasic plots with a change
of the rate-determining step from breakdown (âX ) 0.8)
to formation (âX ) 0.2) of T( with pyridines,18 to the
simple rate limiting breakdown of T( with anilines (âX
) 0.8),19 and to the rate-limiting formation of T( with
benzylamines (âX ) 0.24).20 Thus, the shift of aminolysis
mechanism from stepwise with rate-limiting breakdown
(11) Castro, E. A.; Leandro, L.; Millan, P.; Santos, J. G. J. Org.
Chem. 1999, 64, 1953.
(12) Castro, E. A.; Pizarro, M. I.; Santos, J. G. J. Org. Chem. 1996,
61, 5982.
(13) (a) Castro, E. A.; Ibanez, F.; Salas, M.; Santos, J. G. J. Org.
Chem. 1991, 56 4819. (b) Castro, E. A.; Salas, M.; Santos, J. G. J. Org.
Chem. 1994, 59, 30.
(14) (a) Oh, H. K.; Lee, Y. H.; Lee, I. Int. J. Chem. Kinet. 2000, 32,
131. (b) Oh, H. K.; Lee, J.-Y.; Park, Y. S.; Lee, I. Int. J. Chem. Kinet.
1998, 30, 419.
(15) Oh, H. K.; Ku, M. H.; Lee, H. W.; Lee, I. J. Org. Chem. 2002,
67, 3874.
(16) Oh, H. K.; Woo, S. Y.; Shin, C. H.; Park, Y. S.; Lee, I. J. Org.
Chem. 1997, 62, 5780.
(17) Castro, E. A.; Ibanez, F.; Santos, J. G.; Ureta, C. J. Chem. Soc.,
Perkin Trans. 2 1991, 1919.
(18) Oh, H. K.; Lee, J. M.; Lee, H. W.; Lee, I. Int. J. Chem. Kinet.
2004, 36, 434.
(21) Castro, E. A.; Ibanez, F.; Salas, M.; Santos, J. G.; Sepulveda,
P. J. Org. Chem. 1993, 58, 459.
(19) Oh, H. K.; Shin, C. H.; Lee, I. J. Chem. Soc., Perkin Trans. 2
1995, 1169.
(22) Oh, H. K.; Oh, J. Y.; Sung, D. D.; Lee, I. Collet. Czech. Chem.
Commun. In press.
(20) Oh, H. K.; Shin, C. H.; Lee, I. Bull. Korean Chem. Soc. 1995,
16, 657.
(23) Castro, E. A.; Cubillos, M.; Munoz, G.; Santos, J. G. Int. J.
Chem. Kinet. 1994, 26, 571.
J. Org. Chem, Vol. 69, No. 24, 2004 8221