Synthesis of a rare metal complex of nitrous oxide opens new vistas for the degradation of a potent greenhouse gas

A comprehensive analysis of the global N₂O budget has shown that its emissions have been increasing for the past four decades, with agricultural activities responsible for the growth. Even though N₂O is present in the atmosphere at a concentration 1000 times less than CO₂, it is approximately 300 times more potent as a greenhouse gas.

In nature, N₂O is converted by enzymes into N₂ and H₂O. The process can be mimicked in a laboratory setting using catalytic metal complexes. Surprisingly, well-defined complexes of N₂O with transition metals are exceedingly rare, even though CO₂ has rich and well-documented coordination chemistry. The vastly dissimilar behaviour of these two related small molecules has been attributed to the poor ligand characteristics of N₂O in comparison to CO₂, but the origins and details of this justification are difficult to track.

"The more information we tried to find on the topic, the closer we headed to circular reasoning," says Dr. Heikki M. Tuononen from the University of Jyväskylä, Finland. "In many cases, some property of N₂O was highlighted, but they are almost all characteristic to CO₂ as well," he continues.

"This puzzle was one of the reasons why, during Dr. Tuononen's visit to Calgary as a Killam Scholar, our research teams decided to join forces and synthesize analogous metal complexes of N₂O and CO₂, and study the metal-ligand interaction in detail," tells Dr. Roland Roesler from the University of Calgary, Canada.

A rare metal complex of N₂O stable even at room temperature

The results of the two-year investigation showed that, contrary to the general view, the metal binding ability of N₂O is equally good or even better than that of CO₂.

"It appears that the oxidizing character of N₂O is mostly, if not entirely, responsible for the scarcity of metal complexes employing this ligand," says Dr. Tuononen.

"Once we had the right metal partner for N₂O, their binding was strong enough that a rare side-on bound complex could be isolated and characterized even at room temperature," continues Dr. Chris Gendy, a former Ph.D. student at University of Calgary who was partially responsible of the synthetic work.

In addition to showing that N₂O has better intrinsic ability to bind to metals than heretofore recognized, the work of the two research teams allows the rational design of N₂O complexes that are even more stable than the ones characterized thus far. This could, in turn, open new avenues for using N₂O in synthetic chemistry.

"N₂O is in many ways a great oxidant. It is thermodynamically strong, relatively cheap, and gives N2 as the only side product," explains Dr. Tuononen.

"It would certainly be great to see more widespread use of N₂O as an oxidant in metal-catalysed reactions. At the same time, we should not forget the role it plays in the atmosphere," adds Dr. Roesler.

"Nature has found elegant enzymatic pathways to convert N₂O into products that are harmless to the atmosphere. We should aim for the same with our humanmade emissions using novel catalysts," the research teams conclude.