Nature of the radical intermediates in a substituted cyclopropylcarbiny-allylcarbinyl system

<p>We have sought to determine the nature of the free-radical precursors to ring-opened hydrocarbon <u>5</u> and ring-closed hydrocarbon <u>6</u>. Reasonable alternative formulations involve the postulation of hydrogen abstraction (a) by a pair of rapidly equilibrating classical radicals (the ring-opened allylcarbinyl-type radical <u>3</u> and the ring-closed cyclopropylcarbinyl-type <u>4</u>), or (b) by a nonclassical radical such as homoallylic radical <u>7</u>.</p> <p>[Figure not reproduced.]</p> <p>Entry to the radical system is gained via degassed thermal decomposition of peresters having the ring-opened and the ring-closed structures. The ratio of <u>6</u>:<u>5</u> is essentially independent of the hydrogen donor concentration for decomposition of the former at 125° in the presence of triethyltin hydrdride. A deuterium labeling study showed that the α and β methylene groups in <u>3</u> (or the equivalent) are rapidly interchanged under these conditions.</p> <p>Existence of two (or more) product-forming intermediates is indicated (a) by dependence of the ratio <u>6</u>:<u>5</u> on the tin hydride concentration for decomposition of the ring-closed perester at 10 and 35°, and (b) by formation of cage products having largely or wholly the structure (ring-opened or ring-closed) of the starting perester.</p> <p>Relative rates of hydrogen abstraction by <u>3</u> could be inferred by comparison of ratios of rate constants for hydrogen abstraction and <u>ortho</u>-ring cyclization:</p> <p>[Figure not reproduced.]</p> <p>At 100° values of k_a/k_r are 0.14 for hydrogen abstraction from 1,4-cyclohexadiene and 7 for abstraction from triethyltin hydride. The ratio <u>6</u>:<u>5</u> at the same temperature is ~0.0035 for hydrogen abstraction from 1,4-cyclohexadiene, ~0.078 for abstraction from the tin hydride, and ≥ 5 for abstraction from cyclohexadienyl radicals. These data indicate that abstraction of hydrogen from triethyltin hydride is more rapid than from 1,4-cyclohexadiene by a factor of ~1000 for <u>4</u>, but only ~50 for <u>3</u>.</p> <p>Measurements of product ratios at several temperatures allowed the construction of an approximate energy-level scheme. A major inference is that isomerization of <u>3</u> to <u>4</u> is exothermic by 8 ± 3 kcal/mole, in good agreement with expectations based on bond dissociation energies. Absolute rate-constant estimates are also given.</p> <p>The results are nicely compatible with a classical-radical mechanism, but attempted interpretation in terms of a nonclassical radical precursor of product ratios formed even from equilibrated radical intermediates leads, it is argued, to serious difficulties. </p> <p>The roles played by hydrogen abstraction from 1,4,-cyclohexadiene and from the derived cyclohexadienyl radicals were probed by fitting observed ratios of <u>6</u>:<u>5</u> and <u>5</u>:<u>10</u> in the sense of least-squares to expressions derived for a complex mechanistic scheme. Some 30 to 40 measurements on each product ratio, obtained under a variety of experimental conditions, could be fit with an average deviation of ~6%. Significant systematic deviations were found, but these could largely be redressed by assuming (a) that the rate constant for reaction of <u>4</u> with cyclohexadienyl radical is inversely proportional to the viscosity of the medium (i.e., is diffusion-controlled), and (b) that k_a/k_r for hydrogen abstraction from 1,4-cyclohexadiene depends slightly on the composition of the medium. An average deviation of 4.4% was thereby attained.</p> <p>Degassed thermal decomposition of the ring-opened perester in the presence of the triethyltin hydride occurs primarily by attack on perester of triethyltin radicals, presumably at the –O-O- bond, even at 0.01 M tin hydride at 100 and 125°. Tin ester and tin ether are apparently formed in closely similar amounts under these conditions, but the tin ester predominates at room temperature in the companion air-induced decomposition, indicating that attack on perester to give the tin ether requires an activation energy approximately 5 kcal/mole in excess of that for the formation of tin ester. </p>