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This list pulls data from {{Element-symbol-to-oxidation-state-data}} for each element then formats the result with {{Element-symbol-to-oxidation-state-row}} See also: oxidation states in {{infobox element}}
The international pictogram for oxidizing chemicals. Dangerous goods label for oxidizing agents. An oxidizing agent (also known as an oxidant, oxidizer, electron recipient, or electron acceptor) is a substance in a redox chemical reaction that gains or "accepts"/"receives" an electron from a reducing agent (called the reductant, reducer, or electron donor).
S. Selenium hexasulfide; Selenium trioxide; Silver bromate; Silver chlorate; Silver chromate; Silver dichromate; Silver iodate; Silver nitrate; Silver perchlorate
"Oxidation-reduction potentials, absorbance bands and molar absorbance of compounds used in biochemical studies" (PDF). Fasman GD, Editor. 1: 122– 130. Alberty, Robert A. (1998). "Calculation of standard transformed formation properties of biochemical reactants and standard apparent reduction potentials of half reactions".
The oxidizing tendency of peroxides is related to the electronegativity of the substituents. Electrophilic peroxides are stronger oxygen-atom transfer agents. The oxygen-atom donor tendency correlates with the acidity of the O−H bond. Thus, the order of oxidizing power is CF 3 CO 3 H > CH 3 CO 3 H > H 2 O 2.
Organic redox reactions: the Birch reduction. Organic reductions or organic oxidations or organic redox reactions are redox reactions that take place with organic compounds.In organic chemistry oxidations and reductions are different from ordinary redox reactions, because many reactions carry the name but do not actually involve electron transfer. [1]
An oxidizing acid is a Brønsted acid that is a strong oxidizing agent. Most Brønsted acids can act as oxidizing agents, because the acidic proton can be reduced to hydrogen gas. Some acids contain other structures that act as stronger oxidizing agents than hydrogen ions. Generally, they contain oxygen in their anionic structure.
In the context of electron transfer, these groups enhance the oxidizing power tendency of the attached species. For example, Tetracyanoethylene serves as an oxidant due to its attachment to four cyano substituents, which are electron-withdrawing groups. [5] Oxidants with EWGs are stronger than the parent compound.