Electrophilic Cleavage of Cyclopropylmethystannanes
in predominant formation of the Z rather than E ring
fission product 4b (E/Z ) 0.37). The regiochemistry of
acidolysis of 3g in CDCl3 (entry 12) favored attack at the
less substituted ring carbon (4c/5c ) 9.0) to a slightly
greater extent than was observed for sulfination.
The halogenolysis of carbon-tin bonds has been ex-
tensively investigated as an archetypal electrophilic
substitution. Iodinolysis of organostannanes can proceed
via an electrophilic or radical-chain mechanism with the
latter becoming competitive for slow reactions in nonpolar
solvents on irradiation with visible light. The iodinolyses
of cyclopropylmethylstannanes 3 were performed in the
dark and in solvents for which electrophilic substitution
has been reported to be the exclusive reaction pathway.
The regiochemistry of cleavage was as observed for
acidolysis, i.e., ring fission to yield iodides 4 and 5 (E )
I) in CDCl3 (entries 14, 20, and 22) and with substitution
at the less substituted carbon (4c/5c ) 9.0), but exclusive
methyl cleavage in coordinating solvents (entries 15-17,
21, and 23) to provide cyclopropylmethyldimethyltin
iodides 6 and iodomethane. Iodinolysis of triphenylstan-
nane 3e in either CDCl3 or CD3OD (entries 18 and 19)
proceeded exclusively with phenyl cleavage to yield 6c
and iodobenzene. While the regiochemistry of iodinolysis
was similar to that of acidolysis, the stereochemistry of
reaction of 3f in CDCl3 (entry 20) resembled that of
sulfination, providing a 3.5:1 ratio of the isomeric iodides
4b in favor of the E isomer. Again, this ratio was constant
throughout the reaction, suggesting a kinetically deter-
mined product ratio. Treatment of predominantly Z-4b
(Z/E ) 9.0, prepared by treatment of 1b with MgI2) with
excess iodine in chloroform under the same conditions
did not result in any observable isomerization over 4
days.
FIGURE 1. Pseudo-first-order rate constants as a function
of stannane concentration for the iodinolysis of 3d in dichlo-
romethane (25 °C).
TABLE 2. Relative Second-Order Rate Constants for
the Iodinolysis of Various Organostannanes at 25.0 °C
a
entry
stannane
krel
ref
1
2
3
4
5
6
Me4Sn
i-Pr4Sn
3d
allylSnPh3
(allyl)4Sn
allylSnMe3
1
9b
9b
b
9a
9a
b
0.38
79
3.5 × 107 c
ca. 5 × 109 c
>1010
a In dichloromethane, unless otherwise stated. b This work. c In
acetone.
relative to a number of other tetraorganostannanes is
presented in Table 2.
We next turned our attention to the potentially more
useful cleavage reactions involving aldehydes (Scheme
2). The corresponding reactions of allylic stannanes
generally require heat, high pressure, or Lewis acid
A second-order rate constant was measured for the
iodinolysis of 3d at 25.0 ( 0.3 °C in dichloromethane by
monitoring the disappearance of iodine at 502 nm.
Reactions were relatively rapid and required the use of
a stop-flow apparatus. The concentration of iodine after
mixing was 1.395 × 10-3 M while the concentration of
stannane was between 9.274 × 10-3 and 2.899 × 10-2
M
(5) (a) Lucke, A. J.; Young, D. J. Tetrahedron Lett. 1991, 32, 807.
(b) Lucke, A. J.; Young, D. J. Tetrahedron Lett. 1994, 35, 1609.
(6) Hrubiec, R. T.; Smith, M. B. J. Org. Chem. 1984, 49, 431.
(7) Corey, E. J.; Kim, C. U.; Takeda, M. Tetrahedron Lett. 1972,
4339.
(8) Wickham, G.; Young, D.; Kitching, W. J. Org. Chem. 1982, 47,
4884.
(9) (a) Roberts, R. M. G. J. Organomet. Chem. 1970, 24, 675. (b)
Fukuzumi, S.; Kochi, J. K. J. Phys. Chem. 1980, 84, 2254. (c) Kashin,
A. N.; Beletskaya, I. P.; Malkhasyan, A. T.; Sollov’yanov, A. A.; Reutov,
O. A. J. Org. Chem. (U.S.S.R.) 1974, 10, 2257. (d) Fukuzumi, S.; Kochi,
J. K. J. Org. Chem. 1980, 45, 2654. (e) Buchman, O.; Grosjean, M.;
Nasielski, J.; Wilmet-Devos, B. Helv. Chim. Acta 1964, 47, 1688. (f)
Buchman, O.; Grosjean, M.; Nasielski, J. Helv. Chim. Acta 1964, 47,
1679. (g) Fukuzumi, S.; Kochi, J. K. J. Am. Chem. Soc. 1980, 102, 2141.
(h) Petrosyan, V. S. J. Organomet. Chem. 1983, 250, 157. (i) Hoffmann,
R. W. Angew Chem., Int. Ed. Engl. 1982, 21, 555.
(10) McCormick, J. P.; Barton, D. L. J. Org. Chem. 1980, 45, 2566.
(11) Young, D.; Kitching W. Aust. J. Chem. 1985, 38, 1767.
(12) Negishi, E.; Swanson, D. R.; Rousset, C. J. J. Org. Chem. 1990,
55, 5406.
(13) Mangravite, J. A.; Verdone, J. A.; Kuivila, H. G. J. Organomet.
Chem. 1976, 104, 303.
(14) Patz, M.; Mayr, H. Tetrahedron Lett. 1993, 34, 3393.
(15) (a) Grignon-Dubios, M.; Dunogues, J.; Calais, R. Tetrahedron
Lett. 1981, 22, 2883. (b) Ryu, I.; Hirai, A.; Suzuki, H.; Sonoda, N.;
Murai, S. J. Org. Chem. 1990, 55, 1409. (c) Ryu, I.; Suzuki, H.; Murai,
S.; Sonoda, N. Organometallics 1987, 6, 212.
(i.e., 6.6 to 20.8 equiv). At least five pseudo-first-order
rate constants were measured at each of five concentra-
tions over this range. The rate equation for the disap-
pearance of iodine is satisfactorily described by -d[I2]/
dt ) k[CPMSn(Me)3][I2] and the plot of observed rate
constant versus stannane concentration was linear within
experimental error (Figure 1) and yielded the second-
order rate constant, k ) 4.6 ( 0.8 × 10-1 M-1 s-1
.
An attempt was made to measure the rate constant
for the corresponding iodinolysis of allyltrimethylstan-
nane. The reaction was too rapid, however, being com-
plete in less than 0.01 s at millimolar concentrations of
stannane and iodine (1:1) in dichloromethane. Thus, the
second-order rate constant is > ca. 108 M-1 s-1 (ap-
proaching diffusion control), which is consistent with the
value of ca. 3 × 107 M-1 s-1 determined for the corre-
sponding reaction of tetraallyltin with iodine in acetone.9a
A comparison of rate constants for the iodinolysis of 3d
(3) For reviews see: (a) Denmark, E. E.; Fu, J. Chem. Rev. 2003,
103, 2763. (b) Marshall, J. A. Chem. Rev. 1996, 96, 31. (c) Yamamoto,
Y.; Asao, N. Chem. Rev. 1993, 93, 2207.
(4) Brown, R. S.; Eaton, D. F.; Hosomi, A.; Traylor, T. G.; Wright,
J. M. J. Organomet. Chem. 1974, 66, 249.
(16) Castaing, M.; Pereyre, M.; Ratier, M.; Blum, P. M.; Davies, A.
G. J. Chem. Soc., Perkin Trans. 2 1979, 3, 287.
(17) Kitching, W.; Olszowy, H. A.; Harvey, K. J. Org. Chem. 1982,
47, 1893.
J. Org. Chem, Vol. 70, No. 9, 2005 3581