Oxidation Definition
During the reaction by the oxidizing molecule, atom or ion, the electrons are damaged.
Oxidation occurs when the oxidation status of molecule, atom or ion increases. The opposite process is called deficiency, which occurs when the electrons benefit or the oxidation status of the atom, molecule or ion decreases.
If you are a fan of oxygen-based cleaners, or are grateful for the sterilization powers of hydrogen peroxide, then you have oxidation to thank you. On the other hand, if you ever have to deal with a wild car or have to toss the fruit of brown, then you have oxidizing defects. Oxidation can be a smooth process or it can be started artificially. Sometimes it is helpful, and sometimes it is very destructive.
At its most basic level, oxidation is the loss of electrons. This happens when the atom or compounds lose one or more electrons. Some elements lose electrons more easily than others. These elements are easily called oxidation. Generally, metals including sodium, magnesium and iron are easily oxidized.
Elements that are more reluctant to lose electrons are not easily oxidized; They hold tightly on their electrons. Nonmetals including nitrogen, oxygen, and chlorine are not easily oxidized.
An example of the reaction is to create hydrofluoric acid between hydrogen and fluorine gas:
H2 + F2 → 2 HF
In this reaction, hydrogen is oxidized and fluorine is being reduced. The reaction can be considered better if it is written in the context of two half reactions.
H2 → 2H + 2E-
F2 + 2E- → 2F-
Note that there is no oxygen anywhere in this reaction!
Historical Definition of Oxygen Included Oxidation
An old meaning of oxidation was when oxygen was added to a compound. This was because oxygen gas (O2) was the first known oxidizing agent. Whereas in addition to oxygen in a compound generally meets the increase in electron loss criteria and oxidation status, the definition of oxidation was extended to include other types of chemical reactions. Read More
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