Reactivity of 4Fe+(CO)n=0-2 + O2: oxidation of CO by O2 at an isolated metal atom

The kinetics of Fe-4(+)(CO)(n= 0-2) + O-2 are measured under thermal conditions from 300-600 K using a selected-ion flow tube apparatus. Both the bare metal and n = 2 cations are inert to reaction over this temperature range, but Fe-4(+)(CO) reacts rapidly (k = 3.2 +/- 0.8 +/- 10 +/- 10 cm(3) s(-1) at 300 K, 52% of the collisional rate coefficient) to form FeO+ + CO2. This is an example of the oxidation of CO by O-2 occurring entirely on a single non-noble metal atom. The reaction of the bare metal reaction is known to be endothermic, such that this result is expected; however, the n = 2 reaction has highly exothermic product channels available, such that the lack of reaction is surprising in light of the n = 1 reactivity. Stationary points along all three reaction coordinates are calculated using the TPSSh hybrid functional. These surfaces show that the n = 1 reaction is an example of two-state reactivity; the reaction proceeds initially on the sextet surface over a submerged barrier to a structure with an O-O bond distance longer than that in O-2, but must cross to the quartet surface in order to proceed over a second submerged barrier to rearrange to form CO2. The n = 2 reaction does not proceed because, on all spin surfaces, the transition state corresponding to O-O separation is at higher energy than the separated reactants. The difference between the n = 1 and n = 2 reactions is not a result of steric effects, but rather because the O-2 is more strongly bound to Fe in the entrance well of the n = 1 case, and that energy is available to overcome the rate-limiting barrier to O-O cleavage. Experimental verification of some of these details are provided by guided ion beam tandem mass spectrometry results. The kinetic energy dependence of the n = 1 reaction shows evidence for a curve crossing and yields relevant thermochemistry for competing reaction channels.