What makes something a strong oxidizing agent

The permanganate ion removes electrons from oxalic acid molecules and thereby oxidizes the oxalic acid. Thus, the MnO 4 - ion acts as an oxidizing agent in this reaction. Oxalic acid, on the other hand, is a reducing agent in this reaction. Atoms, ions, and molecules that have an unusually large affinity for electrons tend to be good oxidizing agents.

Elemental fluorine, for example, is the strongest common oxidizing agent. F 2 is such a good oxidizing agent that metals, quartz, asbestos, and even water burst into flame in its presence. Note that while a specific atom typically has an odization state changes, the agents are the actual species, not the atoms. Oxidizing and reducing agents are important in industrial applications.

They are used in processes such as purifying water, bleaching fabrics, and storing energy such as in batteries and gasoline. Oxidizing and reducing agents are especially crucial in biological processes such as metabolism and photosynthesis.

All combustion reactions are also examples of redox reactions. A combustion reaction occurs when a substance reacts with oxygen to create heat. One example is the combustion of octane, the principle component of gasoline:. By looking at each element's oxidation state on the reactant side of a chemical equation compared with the same element's oxidation state on the product side, one can determine if the element is reduced or oxidized, and can therefore identify the oxidizing and reducing agents of a chemical reaction.

Oxidizing and Reducing Agents An oxidizing agent , or oxidant , gains electrons and is reduced in a chemical reaction. An oxidizing agent oxidizes other substances and gains electrons; therefore, its oxidation state decreases. Applications Oxidizing and reducing agents are important in industrial applications. How do you determine which oxidizing agent is stronger? Chemistry Electrochemistry Oxidation and Reduction Reactions. David Drayer. Dec 26, Explanation: Oxidation is the removal of electrons from an atom or polyatomic ion.

Ernest Z. You compare their standard reduction potentials. Not all oxidizers and reducers are created equal. Examples of strong oxidizers include hydrogen peroxide, permanganate, and osmium tetroxide. Reducing agents are typically electropositive elements such as hydrogen, lithium, sodium, iron, and aluminum, which lose electrons in redox reactions. Hydrides compounds that contain hydrogen in the formal -1 oxidation state , such as sodium hydride, sodium borohydride and lithium aluminum hydride, are often used as reducing agents in organic and organometallic reactions.

This fact might be surprising because cesium, not lithium, is the least electronegative element. The apparent anomaly can be explained by the fact that electrode potentials are measured in aqueous solution, where intermolecular interactions are important, whereas ionization potentials and electron affinities are measured in the gas phase.

Lithium metal is therefore the strongest reductant most easily oxidized of the alkali metals in aqueous solution. The standard reduction potentials can be interpreted as a ranking of substances according to their oxidizing and reducing power.