two non metal which are good oxidising agent
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Common Oxidizing Agents and Reducing Agents
In looking at oxidation-reduction reactions, we can focus on the role played by a particular reactant in a chemical reaction. What is the role of the permanganate ion in the following reaction, for example?
2 MnO4-(aq) + 5 H2C2O4(aq) + 6 H+(aq) " width="54" height="12">10 CO2(g) + 2 Mn2+(aq) + 8 H2O(l)
Oxalic acid is oxidized to carbon dioxide in this reaction and the permanganate ion is reduced to the Mn2+ ion.
Oxidation:H2C2O4CO2+3+4Reduction:MnO4-Mn2++7+2
The permanganate ion removes electrons from oxalic acid molecules and thereby oxidizes the oxalic acid. Thus, the MnO4- ion acts as an oxidizing agent in this reaction. Oxalic acid, on the other hand, is a reducing agent in this reaction. By giving up electrons, it reduces the MnO4- ion to Mn2+.
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
In looking at oxidation-reduction reactions, we can focus on the role played by a particular reactant in a chemical reaction. What is the role of the permanganate ion in the following reaction, for example?
2 MnO4-(aq) + 5 H2C2O4(aq) + 6 H+(aq) " width="54" height="12">10 CO2(g) + 2 Mn2+(aq) + 8 H2O(l)
Oxalic acid is oxidized to carbon dioxide in this reaction and the permanganate ion is reduced to the Mn2+ ion.
Oxidation:H2C2O4CO2+3+4Reduction:MnO4-Mn2++7+2
The permanganate ion removes electrons from oxalic acid molecules and thereby oxidizes the oxalic acid. Thus, the MnO4- ion acts as an oxidizing agent in this reaction. Oxalic acid, on the other hand, is a reducing agent in this reaction. By giving up electrons, it reduces the MnO4- ion to Mn2+.
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
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