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Oxidation And Reduction

This guide provides an overview of oxidation and reduction processes, including how they are defined, important concepts like oxidation numbers, and their significance in redox reactions. Learn about the mnemonic "OIL RIG" which helps remember that oxidation involves loss and reduction involves gain. Key features include oxidation states of elements, examples of common redox reactions such as combustion and synthesis, and practice exercises to determine oxidation states in various compounds.

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Oxidation And Reduction

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  1. Oxidation And Reduction

  2. Oxidation • Process in which atoms or ions attain a more + oxidation state • Ex. Na → Na+ + e Cl-→ Cl + e Ca+ → Ca2+ + e

  3. Reduction • Atoms or ions of elements attain a more negative oxidation state • Ex. Cl + e → Cl- • Mnemonic: “OIL RIG” Oxidation involves loss, reduction involves gain

  4. Oxidation Number • Uncombined elements have oxidation # of 0 • Monoatomic ions have oxidation # equal to their ion charge • F is always –1 in a compound • O is almost always –2 in a compound • H is +1 in all compounds except those with metals (then its –1) • More electronegative element is assigned a number equal to its ion charge • Algebraic sum of oxidation numbers in a compound is always zero

  5. Practice • Determine the oxidation numbers for each element in the compounds below NaCl H2SO4 NO3- CO2 SF6 AgNO3

  6. Redox Reactions • Redox reactions are among the most common of all chemical processes • Combustion, synthesis, decomposition, and single replacements are all redox reactions

  7. Definition • Reaction in which a change in oxidation number occurs • Oxidation – becomes more positive • Reduced – becomes more negative • Oxidation and reduction always come in pairs • Electrons are transferred from the substance being oxidized to the substance being reduced

  8. Example • In the reactions below, identify what is oxidized and what is reduced 2PH3 + 4O2 P2O5 + 3H2O 2H2O + Al + MnO4-  Al(OH)4- + MnO2

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