Electrochemistry has become an important topic for nanomaterials because of applications in energy storage and conversion. 1 In particular, ACS Nano has witnessed explosive growth in articles on electrocatalysis using new nanomaterials as well as novel strategies for improving the performance of known nanomaterials. Progress in controlled syntheses and characterization of nanomaterials has benefitted the field of electrocatalysis through better understanding of fundamental mechanisms and development of practical catalysts. 2 This experimental effort has been complemented by improvements in numerical models that are able to predict free energies of successive steps involved in electrocatalytic reactions. Thus, substantial progress has been made toward understanding fundamental processes involved in important electrochemical reactions such as hydrogen evolution (HER), oxygen evolution (OER), oxygen reduction (ORR), and CO2 reduction (CO2RR). A side effect of so many papers, however, is that it has become difficult to compare the catalytic properties of different nanomaterials fairly for a given reaction. Therefore, to maintain progress in the field, the adoption of a standard methodology for analyzing catalytic performance of nanomaterials is needed. Similar standards have been suggested and implemented, for example, in the fields of solar cells and energy storage. 3− 5 Similarly, other ACS journals have also recommended guidelines and best practices for reporting catalysis results, and we recommend readers consult them for benchmarking their catalysts. 6, 7 In this Editorial, we propose best practices for presenting electrocatalytic results in ACS Nano. These guidelines, we hope, will provide deeper understanding of the intrinsic performance of new electrocatalytic nanomaterials and will enable researchers to compare their results objectively with other reports.

Electrochemical reactions are based on conversion of chemicals assisted by exchange of electrons via electron transfer. 8 These reactions typically occur at a standard redox potential, E, which corresponds to the equilibrium potential. To trigger the reaction in one direction, a potential is applied to the electrode onto which the catalysts are deposited. The Sabatier principle states that the free energy for absorption of reactants and reaction intermediates should ideally be