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A redox reaction occurs when there is a chemical change that involves the transfer of electrons. A non redox reaction occurs when there is not a transfer of electrons.
For redox reactions, which are reduction-oxidation reactions, a change in the oxidation number occurs. Elements that are reduced gain electrons, and elements that are oxidized lose electrons. Rusting is a good example of a redox reaction.
For non redox reactions, a change in the oxidation number does not occur. There are several classifications for non redox reactions, including combination, decomposition, single displacement, and double displacement. The reactants and all products must be compounds (not single elements) and must not have a change in oxidation number.
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A redox reaction involves either oxidation or reduction reactions. In these reactions, elements either gain or lose electrons.
It is easy to spot them because the oxidation number of some elements would change.
A non redox on the other hand is the typical decomposition, single displacement, and double displacement reaction. A non redox reaction, there is no difference in the oxidation charge.
For this we'll have to look into the many aspects of reduction and oxidation
- Addition of hydrogen
- Removal of oxygen
- Gain of electron
- Addition of Oxygen
- Removal of hydrogen
- Loss of electron
Now, if a molecules undergo both reduction and oxidation according to the definitions given, then 110% its redox.
Non redox when either or none of the above mentioned terms take place
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