Hydrogen bonds and redox processes are highly connected in nature: redox enzymes use specific noncovalent interactions to control the redox behavior of organic cofactors such as quinones, flavins, nicotinamides, and pterins.[1] Among these cofactors, quinone and hydroquinone species play a central role in energy transduction, by shuttling electrons between the various components of electron-transport chains.[2] The role of hydrogen bonding in modifying the reduction potential and the reactivity of quinones has been extensively studied by using hydrogen-bond-donating solvents [3] and biomimetic receptors.[4] The impact of hydrogen bonding on the oxidation of hydroquinones to give hydrogen-bonded neutral semiquinones has received somewhat less attention, despite this reaction having been reported to be crucial for the cytochrome bc 1 complex, [5] a component of respiratory electron-transfer chains, and despite it being the basis of the antioxidant action of hydroquinones in apolar solvents.[6] The presence of a neutral semiquinone intermediate has also been proposed to be formed in the high affinity site (Q H ) of cytochrome bo 3 from Escherichia coli.[7] To better understand the mechanism of the enzymatically catalyzed oxidation of ubiquinol, and to inspire the synthesis of new antioxidants, the relationship between the hydrogen-atom-donating ability of hydroquinones and the hydrogen-bonding behavior of the reduced (hydroquinone) and partially oxidized (semiquinone) species should be rationalized quantitatively.We report herein that the increase observed in the reactivity of a model hydroquinone toward free radicals upon addition of small amounts of hydrogen-bond-acceptor (HBA) solvents can be explained quantitatively in terms of the different strengths of the hydrogen bonds formed in the parent phenol and in the phenoxyl radical.The reaction of 2,5-di-tert-amylhydroquinone (1) with the 2,2-diphenyl-1-picrylidrazyl radical (DPPHC) was studied by following the pseudo-first-order decay of the absorbance of DPPHC in the presence of 1 in a nitrogen-saturated CCl 4 solution containing small amounts of each of two HBA solvents, that is, acetonitrile (CH 3 CN) and dimethylsulfoxide (DMSO).[8] The experimental k DPPH values (Figure 1) show an initial increase at low concentrations of the cosolvent, then reach a maximum (1.1 10 4 m À1 s À1 at DMSO = 0.02 m and 4 10 3 m À1 s À1 at CH 3 CN = 0.2 m), and decrease on further addition of the cosolvent. This behavior, which can be interpreted on the basis of Scheme 1 and Equation (1), [9] which is derivedunder the assumption that a phenolic OH group bound to a solvent molecule is not reactive toward free radicals, [10] implies that the free OH group of the partially solvated species 1S reacts with DPPHC much faster than those of the uncomplexed hydroquinone 1 (that is, k 2 > k 1 ). The values obtained by this procedure are reported in Table 1; in the case of CH 3 CN, the equilibrium constants for the sequential complexation of the two hydroxy groups of 1 (K 1 and K 2 ) were also...