The oxidation of SiC and Si provide a unique opportunity for studying oxidation mechanisms because the product is the same, SiO 2 . Silicon oxidation follows a linear-parabolic law, with molecular oxygen identified as the oxidant. SiC oxidation obeys the same linearparabolic law but has different rates and activation energies and exhibits much stronger facedependence. Using results from first-principles calculations, we show that atomic and molecular oxygen are the oxidant for Si-and C-face SiC respectively. Comparing SiC with Si, we elucidate how the interface controls the competition between atomic and molecular mechanisms.Oxidation is a ubiquitous process that occurs in most solids including metals, insulators, and semiconductors. The atomic-scale processes that underlie oxidation are of fundamental interest as they control the quality of both the resulting oxide and its interface with the substrate.Furthermore, elucidation of these processes would also benefit applications as thermal oxidation is widely used to fabricate oxide films, such as gate dielectrics and insulating layers, in electronic devices, [1,2] in nanostructures, [3] and in applications of ceramics materials [4]. The best-known example is Si oxidation, which produces a high-quality oxide/semiconductor interface and is one of the most important techniques that enable semiconductor technology. Meanwhile, for materials used at high temperatures, stability against thermal oxidation is a major concern [5].Silicon and SiC provide a unique opportunity for investigating thermal oxidation because they have the same native oxide, SiO 2 . Si oxidation has been extensively studied and the kinetics has been well described by a model proposed by Deal and Grove,[6] where the oxidation time t and the oxide thickness x are related by: t = x 2 /B + x/(B/A).The parabolic rate B is related to the oxidant diffusivity D by: