Summary:Per- and polyfluoroalkyl substances (PFASs) contain bonds between carbon and fluorine atoms considered the strongest in organic chemistry. New research shows that using excess electrons shatters the carbon-fluorine bond of these chemicals in water, leaving by-products that might even accelerate the process.
Synthetic chemicals known as per- and polyfluoroalkyl substances (PFASs) contain bonds between carbon and fluorine atoms considered the strongest in organic chemistry. Unfortunately, the widespread use of these nonbiodegradable products since the 1940s has contaminated many water supplies across America.
Engineers at UC Riverside have now shown in modeling experiments that using excess electrons shatters the carbon-fluorine bond of PFASs in water, leaving by-products that might even accelerate the process. The paper is published in Physical Chemistry Chemical Physics.
Impervious to heat, chemicals, and physical force, the carbon-fluorine bond makes PFASs ubiquitous in food packaging, stain and water repellent fabrics, polishes and waxes, firefighting foams, cleaning products, carpets and thousands of other common household and industrial products. The Environmental Protection Agency estimates that most of the population has been exposed to PFASs that accumulate in the body over time because these “forever chemicals” do not biodegrade.
Sharma Yamijala, a postdoctoral researcher in the Marlan and Rosemary Bourns College of Engineering and first author of the paper, ran simulations on both perfluorooctanoic acid and perfluorooctanesulfonic acid molecules, the most common PFA contaminants in the environment, surrounded by water molecules. He found that they instantly lost their fluorine atom in the presence of excess electrons.
The PFA molecules broke down into an intermediate chemical species whose composition could further accelerate the decomposition of other PFA molecules. The reaction also formed a hydrogen fluoride molecule. Whether or not these shortchain molecules are carcinogens at typical concentrations in water has not yet been determined.
“In a real water treatment scenario, the excess electrons could come from metal-containing compounds placed in the water under ultraviolet radiation. The electrons from these compounds will interact with the PFA molecules and break them,” Yamijala said.
The simulations describe in precise detail a process that scientists have known is possible.
“People knew you could do this but didn’t know why,” said Bryan Wong, an associate professor of chemical and environmental engineering and the paper’s senior author. “Our simulations define the bigger picture that we can refine to find ways to break down PFAs faster or more efficiently in the future.”
The research was supported by grants from the U.S. Department of Energy, Office of Science, Early Career Research Program Award No. DE-SC0016269 and the National Science Foundation Grant No. CHE-1808242.