ADVERTISEMENT
2 /3 FREE ARTICLES LEFT THIS MONTH Remaining
Chemistry matters. Join us to get the news you need.

If you have an ACS member number, please enter it here so we can link this account to your membership. (optional)

ACS values your privacy. By submitting your information, you are gaining access to C&EN and subscribing to our weekly newsletter. We use the information you provide to make your reading experience better, and we will never sell your data to third party members.

ENJOY UNLIMITED ACCES TO C&EN

Separations

Model could improve promising C-H activation

Theory reveals hidden energy costs and points to new chemistry

by Sam Lemonick
November 14, 2018 | APPEARED IN VOLUME 96, ISSUE 46

20181114lnp1-oxidation.jpg
Credit: C&EN
Theoretical modeling of C-H functionalization by proton-coupled electron transfer revealed a surprising energy penalty getting the oxygen and hydrogen lined up.

Carbon and hydrogen make stable bonds that are ubiquitous in organic molecules. That’s why chemists spend so much energy looking for ways to break them and replace hydrogens with more useful moieties. One group recently found a new way to make a carbon atom release a hydrogen and accept new substituents. But they didn’t understand why the intramolecular reshuffling worked as well as it did with relatively weak oxidants (Sci. Adv. 2018, DOI: 10.1126/sciadv.aat5776). Now their colleagues have made an accurate theoretical model that can explain the reaction’s dynamics (J. Am. Chem. Soc. 2018, DOI: 10.1021/jacs.8b10461). It points to ways to improve this method and hints at possible electrochemistry applications.

In July, James M. Mayer’s group at Yale University described a method for C-H functionalization under mild conditions by proton-coupled electron transfer (PCET) reaction.

Hammes-Schiffer’s theory explains that the reaction happens by simultaneous tunneling of the proton and electron between energy states. “All the transitions are downhill,” Hammes-Schiffer says, meaning they release energy. She thinks this is why the strength of the oxidant has relatively little effect on how quickly the reaction proceeds. Robert Knowles, a synthetic organic chemist at Princeton University, calls it a “beautiful theoretical study,” which he says “will serve as a road map for much future work in this area.” Hammes-Schiffer and Mayer think the unexpected ease of oxidizing the C-H bond could point researchers to possible new chemistry for for more efficient fuel cells that operate at lower voltages than current ones.

Mayer says he also discovered from the analysis that the hydrogen and oxygen atoms in his molecule are not as close together as he thought, meaning there’s an energy penalty incurred to twist the players into position. “If they can avoid that large conformational change,” the reaction may proceed faster, Hammes-Schiffer says. The two hope to collaborate to improve the molecule and the reaction with a combination of theoretical and experimental work. “I think there’s more to come,” says Mayer.

X

Article:

This article has been sent to the following recipient:

Leave A Comment

*Required to comment