silenes form via alpha elimination
TRANSCRIPT
RESEARCH
Silenes form via alpha elimination Dow Corning chemists detect silenes spectroscopically during thermolysis of methoxy-substituted polysilanes
Two chemists at Dow Corning have found a way to generate silenes that has enabled them to considerably expand the study of these short-lived intermediates. Dr. William H. Atwell and Dr. Donald R. Weyenberg of the Midland, Mich., company find that these divalent organosilicon compounds—for example, dimethylsilylene, (CH : i)2Si:—can be made by thermally decomposing methoxy-substituted polysilanes.
Dr. Weyenberg told conferees at last week's International Symposium on Organometallic Chemistry (sponsored by the International Union of Pure and Applied Chemistry), in Munich, West Germany, that the reaction involves an alpha elimination to form the silenes. Evidence for this mechanism comes from the structure of reac
tion products, reaction kinetics, and mass spectral studies. In their spectral studies, Dr. Atwell, Dr. Weyenberg, and Dr. Roland S. Gohlke (also at Dow Corning) have actually detected formation of the dimethylsilylene intermediate during thermolysis of 1,2-dimethoxytetramethyldisilane in the inlet chamber of a mass spectrograph.
Dr. Atwell and Dr. Weyenberg find that the silenes react with a variety of acetylenes to give a disilacyclohex-adiene ring system. The reaction route appears to be a rather specific dimerization of silacyclopropene intermediates. In another reaction with substituted butadiene, the silene intermediate gives a silacyclopentene ring system. The product is the same whether the silene is generated from a
disilane or from a 7-silanorbornadiene. Interest in the divalent silicon inter
mediates has grown steadily in the last five years after research in the Soviet Union suggested their transient existence as products from the reaction of diorganodichlorosilanes with metals or from the thermal decomposition of polysilanes. Since then, a number of specific studies using these two general approaches have been made, notably by Dr. M. E. Vol'pin and Dr. O. M. Nefedov in the U.S.S.R. and Dr. Philip S. Skell at Pennsylvania State University. The Dow Corning research has centered on methoxy-substituted polysilanes, which enable multiple syntheses useful in explaining the role played by these novel divalent species.
Last year, Dr. Atwell and Dr. Weyenberg found that thermolysis of 1,2-dimethoxytetramethyldisilane proceeds readily at 225° to 250° C. to give di-methyldimethoxysilane and o:,w-dime-thoxypermethyl polysilanes having three, four, and five dimethylsilyl groups. Their data strongly suggest a mechanism for the reaction involving insertion of the silene in unreacted disilane molecules after alpha elimination of the starting compound.
Thermolysis in the presence of a trapping agent such as diphenylacetyl-ene allows interception of the intermediate before it inserts in the disilane. The resulting product is 1,1,-4,4-tetramethyl - 2,3,5,6-tetraphenyl-1,4-disilacy clohexadiene.
Since their first example of silene preparation from 1,2-dimethoxytetra-methyldisilane, the Midland chemists have studied enough related polysilane reactions to suggest that generation of silenes by thermolysis of methoxy-substituted polysilanes is a general reaction. The reaction is not limited to disilanes. The tetramethyl tetra-phenyl (TMTP) disila ring compound also forms (in 35% yield) when 1,3-di-methoxyhexamethyltrisilane is heated at 250° to 275° C. with diphenylacety-lene. Moreover, methoxy groups are not essential, Dr. Weyenberg says, since disilanes bearing other groups such as (CH3)3SiO or CI also yield divalent intermediates.
Further examples of this reaction include thermolysis of tetramethoxydi-methyldisilane. In the presence of di-
Heat decomposes a variety of silicon compounds
CH* CH* i * l 3
C H i - O - S i — S i - O - C H a 0 I l °
CH* CH*
CjH5 C f tHj
H5C6C=CC*H5
Dimethylsilylene C H 3 C H 3
/ri - j Thermolysis of polysilanes, methoxy-substituted
polysilanes, and 7-silanorbornadienes yields di-X M i l valent organosilicon intermediates (silenes).
* c ; " ' These silenes, such as dimethylsilylene, react *CHi I wrth acety ,enes or butadienes to produce di-
silacyciohexadienes or silacyclopentenes through J presumed intermediate silacyclopropenes or
silacyclopropanes
\ ! J > H i CH
H 5 C i ^ j 5 ' i
CH3 C H j
1,1,4,4-Tetramethyl-2,3,5,6-tetra phenyl-1,4-disilacyclohendieiie
30 C&EN SEPT. 4, 1967
RING SYSTEMS. Dr. William H. Atwell (left) and Dr. Donald R. Weyenberg of Dow Corning find that silènes, divalent organosilicon compounds, react with a variety of acetylenes to give disilacyclo-hexadiene ring systems
phenylacetylene, this reaction produces 30 to 35% of the 1,4-dimethoxy-substituted analog of the TMTP disila ring compound. The intermediate in this case is methylmethoxysilylene (CH3SiOCH3) . The product is about a three-to-one mixture of as-yet-unassigned cis and trans isomers.
Dr. Atwell and Dr. Weyenberg have tried extending the methoxy substitution a step further by studying thermolysis of hexamethoxydisilane. However, no tetramethoxy ring compound resulted from hexamethoxydisilane thermolysis in the presence of diphen-ylacetylene. Instead, they obtained only tetrakis(trimethoxysilyl)silane resulting from reaction of the supposed (CH 3 0) 2 Si with the starting disilane. This shows that diphenylacetylene does not compete effectively with hexamethoxydisilane for this particular intermediate. The two chemists note that the apparent change in reactivity of the dimethoxysilylene intermediate in this reaction parallels the behavior of dialkoxycarbenes.
Mechanism. Dr. Atwell and 'Dr. Weyenberg suggest that the divalent species is formed by an alpha-elimination route from the original polysilane material. This is consistent with the formation of the disila ring compound during thermolysis of variously substituted disilanes in the presence of diphenylacetylene.
New evidence of silène formation now comes from mass spectral studies showing the silènes as directly observed, short-lived intermediates. This elimination mechanism is also indicated in the kinetics of thermolysis. Distribution of thermolysis products remains constant upon dilution with
either dioxane or diphenyl ether. In addition, the rate of disilane consumption is not accelerated by the presence of trapping agents such as acetylenes.
Although the mechanism for the reaction of silènes with acetylenes is not completely worked out, Dr. Atwell and Dr. Weyenberg have shown that the disilacyclohexadienes seem to be formed from the silènes by a rather specific dimerization of silacyclopro-pene intermediates. Thus, they propose the novel small-ring intermediate structure originally considered by the U.S.S.R. scientists as the structure of the TMTP disila ring compound.
This selectivity in forming products is shown by the absence of products which might be expected from simple reaction paths such as pi-dimerization (linkage of two silacyclopropene rings to form a six-membered compound such as the TMTP disila ring compound). For example, research at Midland on thermolysis of 1,2-dime-thoxytetramethyldisilane in the presence of a mixture of diphenylacetylene and dimethylacetylene shows no resulting 3,5-diphenyl-substituted di-silacyclohexadiene compound. This effectively eliminates pi-dimerization as a possible mechanism.
Dr. Atwell and Dr. Weyenberg also rule out formation of disilacyclohexadienes by dimerization of an initial diradical in which the silène is bound to one carbon of the acetylenic compound. This does not seem likely because the low-concentration diradical should reasonably react with excess acetylene to give a substituted silacy-clopentadi^ne. In fact, no such Rve-membered ring has been detected despite repeated efforts.
The two chemists have also turned to other unsaturated trapping agents besides acetylenes. Heating 1,2-di-methoxytetramethyldisilane with 2,3-dimethylbutadiene gives the five-mem-bered ring product 1,1,3,4-tetramethyl-l-silacyclopent-3-ene (14%) . The same product also results (40%) when a 7-silanorbornadiene is used as the source of the dimethylsilylene. The lower yield in the first instance is a consequence of the competing insertion reaction of the ( CH3 ) 2Si intermediate with the disilane starting material.
Dr. Atwell and Dr. Weyenberg foresee future work on thermolysis of other substituted polysilanes. Current work indicates that thermolysis in the vapor phase proceeds along very similar lines. Vapor phase reactions are especially interesting because of the possibility they offer for detecting the so-far elusive silacyclopropene intermediates. These intermediates may be in a more isolated state in the vapor phase and could perhaps be detected prior to dimerization.
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B12 coenzyme bonds measured precisely
Bond distances within the molecule of vitamin B12 coenzyme (5'-deoxyaden-osylcobalamin) have been measured precisely in work at Vanderbilt University's department of physics. Dr. P. Galen Lenhert, continuing x-ray diffraction studies of the coenzyme begun seven years ago at Oxford University, described his results at the 7th International Congress of Biochemistry, in Tokyo.
The 2.24-A. cobalt-benzimidazole bond in the coenzyme is about 0.2 A. longer than that in vitamin B12 (cyano-cobalamin). The distances between the coenzyme's cobalt atom and the four nitrogen atoms in the corrin nucleus surrounding it are apparently slightly longer than are those for vitamin B12. The cobalt-carbon bond, connecting the adenine nucleoside to the cobinamide portion of the molecule, is surrounded by two methyl and two methylene groups, all of which project 2 A. above the cobalt atom. Along with the adenosine itself, these groups protect the organometallic bond from the approach of reagents. Judging from the distances separating the corrin nucleus from some atoms in the adenosine portion, Dr. Lenhert points out, free rotation of adenosine about the cobalt-carbon bond in solution doesn't seem likely.
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RESEARCH IN BRIEF
The antibiotic Myxin decomposes violently on combustion, according to Dr. A. I. Rachlin of Hoffmann-La Roche research laboratories, Nutley, N.J. Dr. Rachlin cautions that "utmost care" should be used if large quantities of Myxin are heat dried. Pure Myxin, heated at 20° C. per minute, is strongly exothermic at 149° C.
32 C&EN SEPT. 4, 1967