“…As a strong one-electron transfer (acceptor or donor) oxidant (eqs and ), Mn(III) is considered to play an important role in bio-geochemical process and water treatment. − In nature, Mn(III) can arise from direct dissolution of hausmannite or from interaction between pyrolusite or manganite with divalent manganese . It can also be produced by the oxidation of Mn(II) using photooxidation, bacteria, enzyme, humic acid, and chemical agents (dissolved oxygen, Cr 2 O 7 2– , and so on) ,− or the reduction of permanganate or manganese dioxide (MnO 2 ) using oxalate, Mn 2+ , and other reductants. − Nevertheless, free Mn(III) is unstable and it can rapidly disproportionate to Mn 2+ and MnO 2 (eq ) because of its tetragonally distorted electron configuration . Most studies on the reaction of organic contaminants with Mn(III) were focused on long-lived Mn(III) species, including Mn(III/IV) oxide, Mn(III)-rich MnO 2 , and soluble Mn(III) complexes with organic or inorganic ligands (such as citrate, oxalate, pyrophosphate (PP; eq ), ethylenediaminotetraacetate (EDTA), humic substances, and siderophores, etc.…”