Chapter 6 Outline - Chemistry 101 Vandan Desai Chapter 6:...

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Chemistry 101 Vandan Desai P a g e | 1 Chapter 6: Oxidation-Reduction Reactions (Lecture Outline) --------------------------------------------------------------------------------------------------------------------------- I. Oxidation-reduction reactions involve electron transfer A. Reactions that involve transfer of electrons called oxidation-reduction/redox reactions i. Oxidation is the loss of electrons by a reactant ii. Reduction is the gain of electrons by a reactant B. Oxidation and reduction always occur together C. The total number of electrons lost by one substance is the same as the total number of electrons gained by the other D. For a redox reaction to occur, something must accept electrons that are lost by another i. The substance that accepts the electrons is called the oxidizing agent ii. The substance that lost the electrons is called the reducing agent E. Note that the oxidizing agent is reduced and the reducing agent is oxidized F. For example: 2 Na + Cl 2 → 2 NaCl i. Na is the reducing agent b/c it lost electrons and was oxidized ii. Cl 2 is the oxidizing agent b/c it gained electrons and was reduced G. Oxidation numbers are use to follow redox changes i. Oxidation number does not equal a charge on an atom ii. When writing oxidation number , the sign is written before the number (+1) and after the number when writing the electrical charge (1+) iii. Redox rxn is a chemical reaction in which changes in oxidation numbers occur H. Assignment of oxidation numbers: i. Oxidation number of any free element is zero . ii. Oxidation number of any simple, monoatomic ion is equal to charge on ion . iii. Sum of all oxidation number of the atoms in a molecule or polyatomic ion must equal the charge on the particle. iv. In its compounds, fluorine has an oxidation number of –1 . v.
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Chapter 6 Outline - Chemistry 101 Vandan Desai Chapter 6:...

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