Reactions And Reactions Of Redox Reactions

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Without the millions of chemical reactions that occur every day, life would be completely different. An important class of common reactions includes those which involve the simultaneous transfer of electrons between chemicals, commonly referred to as redox reactions or oxidation-reduction reactions. Redox reactions are whole reactions composed of two different half reactions known as oxidation (where electrons are lost) and reduction (where electrons are gained) (Chemguide, 2013). When there is an increase in the oxidation state, the reaction is oxidation; when there is a decrease, it is reduction. Oxidation cannot possibly occur without an affiliated reduction, and vice versa. Redox reactions are notated as such:
Cu(s)  Cu2+ + 2e-
In the half-reaction above, a copper ion (with a plus 2 charge) is formed from the oxidation of solid copper (with no charge). The "e-" in the equation is an electron which is free to reduce other chemical atoms, such as in the half-reaction:
2Ag+(aq) + 2e-  2Ag(s)
Two electrons are added to the two silver ions in this half-reaction, in order to produce a solid silver. These two half-reactions can be combined to form a redox equation as follows:
Cu(s)  Cu2+(aq) + 2e-
2 Ag+(aq) + 2e-  2Ag(s)
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Cu(s) + 2Ag+(aq) + 2e-  Cu2+(aq) + 2Ag(s) + 2e-
Cu(s) + 2Ag+(aq)  Cu2+(aq) + 2Ag(s)
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