The periodic reactivity trend and the connection of kinetics to the thermodynamic activity of oxygen are established for the oxidation of methanol on metal clusters. Firstorder rate coefficients are a single-valued function of the O 2 -to-CH 3 OH ratio, because this ratio, together with the rate constants for O 2 and CH 3 OH activation, determine the oxygen chemical potential, thus the relative abundance of active sites and bulk chemical state of the clusters. CH 3 OH activation rate constants on oxygen-covered Ag, Pt, and Pd and on RuO 2 clusters vary with the metal-oxygen binding strength in a classical volcano-type relation, because the oxygenbinding strength directly influences the reactivities of oxygen as H abstractors during the kinetically relevant CH 3 OH activation step. The differences in oxygen thermodynamic activity lead to five orders of magnitude variation in rates (Pt > Pd > RuO 2 > Ag, 373 K), because of its strong effects on the activation enthalpy and more prominently activation entropy in CH 3 OH activation. Figure 4. a) Volcano plots of activation barriers (E A ), b) rate constants (k M,[O*-O*] , 373 K), and c) activation free energies (DG°), which include activation enthalpies (DH°) and entropies (plotted as ÀTDS°), for CH 3 OH oxidative dehydrogenation on O*-covered Ag, Pt, and Pd clusters and RuO 2 clusters measured from this work plotted against the O* binding energy [9] calculated from DFT on closed packed metal surfaces. (O 2 -to-CH 3 OH ratios of 20-60 for Ag, 10-60 for Pt, 40-60 for Pd, and 20-60 for Ru).