Metallocorroles are transition metal
complexes showing great promise
as oxygen reduction reaction catalysts. The performance of metallocorrole
catalysts is highly sensitive to the nature of the transition metal
employed, although currently this dependence remains elusive. In the
current work, we present a first principles density functional theory
(DFT) investigation of the oxygen reduction reaction mechanism in
acidic media using several first-row transition metal corroles. We
show that the identity of the metal center, M, determines the relative
formation free energies of the reaction intermediates, and thus the
potential-determining step in the four-electron reduction process
directly to water. For MMn, Fe, and Co, the hydroperoxyl intermediate
is a thermodynamic maximum along the reaction path, whereas for Ni
and Cu, the formation of the hydroperoxyl intermediate is a thermodynamic
trap, with the following oxo intermediate being highly unstable. The
formation of the oxo intermediate was carefully investigated using
several flavors of DFT. The calculations suggest that in the oxo intermediate,
the spin density on the oxygen atom increases from MMn to
MCu, indicating a purely metal oxygen double bond for MMn,
a single metal oxygen bond with an unpaired electron on the oxygen
atom for MNi and Cu, whereas for MFe and Co, the spin
density on the oxygen atom has intermediate values. When plotting
the experimentally observed onset potentials as a function of the
computed O2 adsorption free energies, a volcano-like plot
is observed, indicating that for the best catalyst, [Co(tpfcBr8)],
a negative binding free energy is observed. A good correlation between
the computed limiting and the experimental onset potentials indicates
that the computationally proposed reaction intermediates are viable
states along the reaction coordinate. The current work is expected
to be of importance for the future design of efficient metallocorrole-based
catalysts.