'The secondary deuterium isotope effects have been measured for the reaction between sodium thiosulphate and a-deuterated methyl, ethyl, and n-propyl bromide, and also for 3-and ydeutcrated n-propyl bromide, in aqueous ethanol solvent. The a-deuterium isotopic rate ratios ( k a / k~) are all greater than unity. These unexpected results are discussed with respect to the suggested use of the a-deuterium isotope effect as a test of mechanism in nucleophilic substitutions.There are many examples in the literature of changes in the rates of nucleophilic substitutions when some of the hydrogen atoms of the reactant, which are not directly involved in the reaction, are replaced by deuterium (1-5). However, nearly all of these examples pertain to Sxl-type solvolytic reactions. Of the binlolecular reactions studied, Inany are solvolyses in water which show regular changes of isotope effect with changes of alkyl group and the site deuterated (6-9) ; I ery few isotope effects have been measured in non-solvolytic SN2 reactions (10, 11). I t is not known whether the regularities found in the solvolytic reactions are general for all biniolecular suhstitutioris; hence, the present investigation is part of a program of systematic study of secondary deuterium isotope effects in non-solvolytic bimolecular substitutions.Since the known isotope effects in this type of substitutio~l are small (11), it is necessary t o choose reactions for study which allow the precise determination of their rate constants. The attack of thiosulphate ion on alkyl bromides, in 30y0 v / v ethanol-water solvent, to yield S-alkyl thiosulphates, known as Bunte salts (12), is one such group of reactions, and may be represented by the equationThe unreacted sodium thiosulphate call be estinlated quite accurately by titration with standard iodine solution.H a~n m e t t and co-workers (13, 14) made a careful investigation of this reaction in their study of the changes which occur in the enthalpy and entropy of activation with structure of the alkyl group. They used an acetate buffer to avoid decomposition of thiosulphate ion in an acidic medium which could result from solvolysis of the alkyl bromide to give hydrobromic acid and an alcohol (or ether). The rate of acetate ion attack on the alkyl bromide was found t o be ~legligibly slow under the conditions of reaction. For the straightchain alkyl bro~uides, the rate of solvolysis was too slow to necessitate correction of the observed rate constants of the thiosulphate reaction.Subsequently, Bevan and Monk showed that Hainmett's rate constants for the reaction of sodium thiosulphate with n-propyl bromide in 50% v / v ethanol-water solvent, calculated using stoichiometric rnolarities of thiosulphate, are not the true rate constants