Among the vast array of catalysts, why has platinum long been regarded as the benchmark for performance? The answer lies in its unique physicochemical properties. As a member of the platinum group metals, platinum exhibits outstanding corrosion resistance, thermal stability, and electrical conductivity. More importantly, it can efficiently activate multiple types of chemical bonds under mild conditions, enabling reactions that would otherwise be slow or nearly impossible—while maintaining high selectivity, which minimizes unwanted side reactions and ensures product purity.
Take hydrogenation reactions as an example: many organic syntheses require saturating unsaturated bonds (e.g., double or triple bonds) with hydrogen. Platinum catalysts can achieve this transformation at ambient temperature and pressure, avoiding the high energy consumption and safety risks associated with extreme conditions. In environmental applications, platinum is a core component of three-way catalytic converters, effectively treating toxic gases in vehicle emissions. In the emerging green hydrogen economy, while alternative materials are often explored for the oxygen evolution reaction (OER) during water electrolysis, the hydrogen evolution reaction (HER) at the cathode still heavily relies on platinum-based catalysts for high efficiency and long-term stability.
It should be noted that platinum catalysts are not a universal solution. Their high cost and limited global reserves drive scientists to seek alternatives, such as palladium, ruthenium-based systems, or non-precious metal catalysts. Yet, in applications demanding extreme stability and high activity, platinum remains unmatched. Through precise microstructural engineering—such as single-atom catalysts or core-shell architectures—researchers are striving to “do more with less platinum.” This relentless pursuit of ultimate efficiency embodies the true fascination of modern catalytic science.
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