An accurate spectrophotometric method of determining relative equilibrium acidities of carbon acids in DMSO has been developed. The pK scale in DMSO has been anchored by comparisons of values obtained by the spectrophotometric method with those obtained potentiometrically in the 8 to 11 pK range. As a result, the pK of fluorene, formerly arbitrarily taken as 20.5, has been raised to an absolute value of 22.6. The pA"s of other carbon acids previously reported, including nitromethane, acetophenone, acetone, phenylacetylene, dimethyl sulfone, acetonitrile, and the corresponding indicator pX's must also be raised. The pK's have been found to be correlated with heats of deprotonation in DMSO by potassium dimsyl, and evidence is presented to show that pK measurements in DMSO are free from ion association effects. Data are presented which indicate a pK of 35.1 for DMSO. In the methane carbon acids, CHyEWG, the order of acidities is NO2 » CH3CO > CN, CH3SO2. The differences amount to 12.2 and 6.8 kcal/mol, respectively, which are believed to be of a comparable magnitude to gas-phase substituent effects. Carbon acids wherein the charge on the anion resides mainly on oxygen, such as ketones and nitroalkanes, are found to be weaker acids in DMSO than in water by 5.5 to 9.6 pK units. On the other hand, carbon acids wherein the charge on the anion is delocalized over a large hydrocarbon matrix, such as in the anion derived from 9-cyanofluorene, are stronger acids in DMSO than in water. Factors that may contribute to this reversal are discussed. The scale of pX's for 9-substituted fluorenes in DMSO is shown to be expanded when compared to the earlier pK scale determined by the Hmethod. A rationale is presented. The apparent relative acidities of fluorenes and phenylacetylene differ by 6 and 11 pK units, respectively, for cyclohexylamine (CHA) vs. DMSO solvents and benzene vs. DMSO solvents. Similarly, in benzene, acetophenone is a stronger acid than fluorene by ca. 6 pK units, whereas in DMSO acetophenone is a weaker acid by 3.2 pK units. These differences result from ion association effects that occur in solvents of low dielectric constant (benzene, ether, CHA, etc.) causing relative acidities to be dependent on the reference base, as well as the solvent. This is not true in strongly dissociating solvents of high dielectric constant, such as DMSO. A list of 13 indicators covering the pAT range 8.3 to 30.6 in DMSO is presented. Equilibrium acidities of weak (i.e., pX ^15) carbon acids have been measured by a variety of methods3 in a variety of solvents including ether,4a benzene,4b diglyme,5 cyclohexylamine (CHA),6 mixtures of dimethyl sulfoxide (DMSO) with ethanol, methanol, or water,7•8•9 and pure DMSO.10 We have chosen DMSO for our studies because it allows accurate measurements to be made spectrophotometrically for many different types of carbon acids over a wide range of pK (ca. 30 pK units) with apparently little or no interference from ion association effects.1 Furthermore,

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Results of the replacement of one or two hydrogen atoms in CH3EWG carbon acids (EWG = CHZSO, CN, PhS02, CH&O, F:jCS02, and the like) by phenyl on equilibrium acidities in Mens0 are reported. The progressive decrease in phenyl acidifying effects with a progressive increase in acidity of the CHzEWG parent acids is interpreted as a resonance saturation effect. The acidifying effects of phenyl on PhCHZEWG, 9,10-dihydroanthracene, and xanthene are found to be severely attenuated by steric inhibition of resonance. Similar effects were observed on substitution of a second Ph group into PhCHzEWG to give PhZCHEWG. The ratios of resonance to polar contributions to the acidifying effect of P h were estimated by (a) removing the resonance contribution through steric inhibition of resonance and (b) by using the MeZN+ group as a model for polar effects. The first method indicated a ratio of 4:l. the second a ratio of 4.61 to 6.6:l depending on the nature of EWG. The resonance to polar ratio for phenyl was found to be larger than that for PhCO (or CH&O), which, in turn, is much larger than that for NOe, CN, or PhSOz.

Electron-withdrawing groups (EWG), such as nitro, carbonyl, and sulfonyl, have been shown by equilibrium acidity measurements in dimethyl sulfoxide (DMSO) solution to have acidifying effects of over 30 powers of ten on a-C-H bonds in methane carbon acids, CH3EWG.1'2 The present paper extends the study to the SO2CF3 group,3 and to cyclopropane carbon acids, c-PrEWG (Table I).4There is abundant evidence that carbanions a to nitro and carbonyl groups derive much of their stability by rehybridizing from sp3 to sp2, thus allowing delocalization of charge to the more electronegative oxygen atoms, but it has

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tures of the conjugated diene units (Si.3 E 1.44 eV). The observed positions of the first two bands in the spectrum of 2 are therefore in excellent agreement with the predictions of the simple SR method.The zero-order SR method also predicts the position of Consecutive 3,5 Shifts in Pyridine 1-Oxide Rearrangements. One-Step Furopyridine SynthesisSir:When the 3-and 5-positions are blocked in a pyridine 1oxide, reaction with benzyne gives, under conditions of kinetic control, products resulting from 1,3-and/or 1,5-sigmatropic shifts in the original 1,2-dihydropyridine 1,3-cycloadduct.' With 3,5-dihalogenated pyridine 1 -oxides (1) elimination of hydrogen halide from the 1,5-sigmatropic shift product leads to benzofuro[ 3,2-b]pyridines in good yield.' Furopyridines are of interest since perhydro derivatives occur in the alkaloids febrifugine and jervine2 and furo [2,3-b]quinolines are present in dictamnine and related alkaloid^.^ Little work has been carried out on the synthesis Communications to the Editor