Northwestern University graduate student Jonathan Barnes had a hunch for creating an exotic new chemical compound, and his idea that the force of love is stronger than hate proved correct. He and his colleagues are the first to permanently interlock two identical tetracationic rings that normally are repelled by each other. Many experts had said it couldn't be done.
On the surface, the rings hate each other because each carries four positive charges (making them tetracationic). But Barnes discovered by introducing radicals (unpaired electrons) onto the scene, the researchers could create a love-hate relationship in which love triumphs.
Unpaired electrons want to pair up and be stable, and it turns out the attraction of one ring's single electrons to the other ring's single electrons is stronger than the repelling forces.
The process links the rings not by a chemical bond but by a mechanical bond, which, once in place, cannot easily be torn asunder.
The study detailing this new class of stable organic radicals is published Science.
"It's not that people have tried and failed to put these two rings together—they just didn't think it was possible," says Sir Fraser Stoddart, a senior author of the paper. "Now this molecule has been made. I cannot overemphasize Jonathan's achievement—it is really outside the box. Now we are excited to see where this new chemistry leads us."
Sir Fraser is the Board of Trustees Professor of Chemistry in the Weinberg College of Arts and Sciences at Northwestern. In the late 1980s, he was one of the early pioneers to introduce an additional type of bond, the mechanical bond, into chemical compounds.
The new Northwestern compound has attractive electronic characteristics and can be made quickly and inexpensively. Down the road, it may be possible to expand this first linked pair into a longer chain-like polymer where this methodology could be useful in new technologies for batteries, semiconductors, and electronic memory devices.
Driven by curiosity, Barnes only began to look at the radical chemistry of the ring cyclobis (paraquat-p-phenylene) two years ago, nearly 25 years after the ring was first made.
"I wondered what would happen if we took it all the way to the max," says Barnes, the paper's first author and a member of Stoddart's group. "Can we take two of these rings, each with four positive charges, and make them live together?"
The rings repel each other like the positive poles of two magnets. Barnes saw an opportunity where he thought he could tweak the chemistry by using radicals to overcome the hate between the two rings.
"We made these rings communicate and love each other under certain conditions, and once they were mechanically interlocked, the bond could not be broken," Barnes says.
Barnes' first strategy—adding electrons to temporarily reduce the charge and bring the two rings together—worked the first time he tried it. He, Stoddart, and their colleagues started with a full ring and a half ring that they then closed up around the first ring (using some simple chemistry), creating the mechanical bond.
When the compound is oxidized and electrons lost, the strong positive forces come roaring back—"It's hate on all the time," Barnes says—but then it is too late for the rings to be parted. "That's the beauty of this system," he adds.
Most organic radicals possess short lifetimes, but this unusual radical compound is stable in air and water. The compound tucks the electrons away inside the structure so they can't react with anything in the environment. The tight mechanical bond endures despite the unfavorable electrostatic interactions.
The two interlocked rings house an immense amount of charge in a mere cubic nanometer of space. The compound, a homocatenane, can adopt one of six oxidation states and can accept up to eight electrons in total.
"Anything that accepts this many electrons has possibilities for batteries," Barnes says.
"Applications beckon," Stoddart agrees. "Now we need to spend more time with materials scientists and people who make devices to see how this amazing compound can be used."
Source: Northwestern University