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Introduction to Redox

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Introduction to Redox

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    1. Introduction to Redox Mrs. Kay Chemistry 12 Chapter 18 Pages:713-720

    2. Redox Reactions combustion of gas in a car rusting of metals bleaching hair reactions in batteries Cut apples turning brown What do you think Redox stands for?

    3. Redox = oxidation and reduction reactions Oxidation: loss of electrons Reduction: gain of electrons Hint: Leo the lion says Ger

    4. redox reactions are a family of reactions that are concerned with the transfer of electrons between species Like acid-base reactions, redox reactions are a matched set -- you don't have an oxidation reaction without a reduction reaction happening at the same time

    5. Single Displacement redox reaction Cu(s) + 2AgNO3(aq) ---> Cu(NO3)2(aq) + 2Ag(s) The silver nitrate solution is transparent, when the copper wire is placed in it, the reaction begins slowly. The wire is coated with silver, while the copper is broken down into ions

    6. Ex: Mg(s) + O2(g) ? MgO(s) Mg loses 2 electrons to become Mg+2 O2 gains 2 electrons to become O-2 The total reaction = redox reaction The half reactions = oxidation and reduction reactions

    7. half reactions for the overall redox reaction Mg ? Mg+2 + 2e- (Magnesium loses electrons, so it is oxidized) O2 + 4e- ? 2O2- (Oxygen gains electrons, so it is reduced)

    8. Were Not Finished yet! When combining half reactions, you must make sure that the electrons gained = the electrons lost. This ensures balancing of the redox reaction. (so we multiplied the first half reaction by 2, so that the 4e- balanced out) 2Mg ? 2Mg+2 + 4e- O2 + 4e- ? 2O2- Total redox reaction is: 2Mg + O2 ? 2MgO

    9. Lets see that again The unbalanced reaction is as follows: Look at each half reaction separately: aluminum metal being oxidized to form an aluminum ion with a +3 charge and oxygen being reduced to form two (2) oxygen ions, each with a charge of -2.

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