Oct
31
Atomic Force Microscope Design Helps Make Solar Fuels
October 31, 2019 | 1 Comment
University of Oregon researchers used an atomic-force microscope fitted with an electrode tip 1,000 times smaller than a human hair to identify in real time how nanoscale catalysts collect charges that are excited by light in semiconductors. It’s a discovery that could help efforts to design devices that can store solar power for later use.
In their paper published in the journal Nature Materials, they discovered that as the size of the catalytic particles shrinks below 100 nanometers the collection of excited positive charges (holes) becomes much more efficient than the collection of excited negative charges (electrons). This phenomenon prevents the excited positive and negative charges from recombining and thus increases the system efficiency.
Tiny electrode tip moves over the interface of nickel nanoparticles on a silicon wafer. Image Credit: Shannon Boettcher, University of Oregon . Click image for the largest view.
The findings open the door to improving systems that use light to make chemicals and fuels, for example by splitting water to make hydrogen gas or by combining carbon dioxide and water to make carbon-based fuels or chemicals, said Shannon W. Boettcher, a professor in the UO’s Department of Chemistry and Biochemistry and member of the university’s Materials Science Institute.
Boettcher expands, “We found a design principle that points to making catalytic particles really small because of the physics at the interface, which allows one to increase efficiency. Our technique allowed us to watch the flow of excited charges with nanometer-scale resolution, which is relevant for devices that use catalytic and semiconductor components to make hydrogen that we can store for use when the sun is not shining.”
In the research, Boettcher’s team used a model system consisting of a well-defined single-crystal silicon wafer coated with metallic nickel nanoparticles of different sizes. The silicon absorbs sunlight and creates excited positive and negative charges. The nickel nanoparticles then selectively collect the positive charges and speed up the reaction of those positive charges with electrons in water molecules, pulling them apart.
Previously, Boettcher said, researchers could only measure the average current moving across such a surface and the average voltage generated by the light hitting the semiconductor. To look closer, his team collaborated with Bruker Nano Surfaces, the manufacturer of the UO’s atomic force microscope that images the topography of surfaces by tapping a sharp tip over it – much like a blind person tapping their cane – to develop the techniques needed to measure voltage at the nanoscale.
As the electrode tip touched each of the nickel nanoparticles, the researchers were able to record the buildup of holes by measuring a voltage – similar to how one tests the voltage output from a battery.
Surprisingly, the voltage measured as the device was operating depended strongly on the size of the nickel nanoparticle. Small particles were able to better select for the collection of excited positive charges over negative charges, reducing the rate of charge recombination and generating higher voltages that better split apart water molecules.
A key, Boettcher said, is that oxidation at the nickel nanoparticle surface leads to a barrier, much like overlapping ridges in a mountain valley, that prevents the negatively charged electrons from flowing to the catalyst and annihilating the positively charged holes. This effect has been termed “pinch-off” and was hypothesized to occur in solid-state devices for decades but never before directly observed in fuel-forming photoelectrochemical systems.
The study’s lead author Forrest Laskowski, who was a National Science Foundation graduate research fellow in Boettcher’s lab, said, “This new technique is a general means to investigate the state of nanoscale features in electrochemical environments. While our results are useful for understanding photoelectrochemical energy storage, the technique could more broadly be applied to study electrochemical processes in actively-operating systems such as fuels cells, batteries, or even biological membranes.”
This work is quite interesting as the word platinum is absent. The potential for hydrogen depends in a major way to getting around the huge cost platinum catalysts load into the hydrogen economy. Platinum used at scale would skyrocket the price of the element.
That makes the innovative use of new tools crucial for more progress. The innovation and drive this team has shown is welcomed with thanks as hydrogen seems to have stalled a bit and needs more progress – if only to light a fire under the effort to find a way to store the universe’s smallest atom.
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The Problem with new microscopic catalysts is that the cost to manufacture seems to show an inverse correlation to the size of the particles. Too expensive to escape the laboratory!