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Oxidation And Reduction

Oxidation And Reduction. Oxidation. Process in which atoms or ions attain a more + oxidation state Ex. Na → Na + + e Cl - → Cl + e Ca + → Ca 2+ + e. Reduction. Atoms or ions of elements attain a more negative oxidation state Ex. Cl + e → Cl -

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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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