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Oxidation Reduction Reactions

Oxidation Reduction Reactions. Redox Reactions Electron-Transfer Reactions. Oxidation Numbers: A set of rules for tracking charges for atoms in covalent compounds. Each atom in a pure element has an oxidation number of zero.

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Oxidation Reduction Reactions

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  1. Oxidation Reduction Reactions Redox Reactions Electron-Transfer Reactions

  2. Oxidation Numbers: A set of rules for tracking charges for atoms in covalent compounds • Each atom in a pure element has an oxidation number of zero. • 2. For monatomic ions, the oxidation number is equal to the charge on the ion. • 3. Fluorine always has an oxidation number of –1 in compounds with all other • elements. • 4. Cl, Br, and I always have oxidation numbers of –1 in compounds, except when • combined with oxygen or fluorine. • 5. The oxidation number of H is +1 and of O is –2 in most compounds. • Exception for H: In compounds with metals, H is –1. • Exception for O: In peroxides, O22- ion gives O an oxidation number of –1. • 6. The algebraic sum of the oxidation numbers for the atoms in a neutral compound • must be zero; in a polyatomic ion, the sum must be equal to the ion charge.

  3. Oxidation States, Energy, the Economy, and Global Warming

  4. Oxidation-Reduction Reactions Oxidation = loss of electrons = increase in ox # Reduction = gain of electrons = decrease in ox # 4 Fe + 3 O2 2 Fe2O3 Oxidizing agent = oxidant = gains electrons Reducing agent = reductant = loses electrons

  5. Recognizing Redox Reactions: Always involves changes in oxidation numbers Metals reacting with Nonmetals: 2 Al + 3 Br2 Al2Br6 Almost anything with Oxygen: 2 Mg + O2  2 MgO S + O2  SO2 Organic Compounds: CH4 + 2 O2  CO2 + H2O Others, more difficult to detect: 5 Fe2+ + MnO4- + 8 H+  5 Fe3+ + Mn2+ + 4 H2O

  6. 4 Al(s) + 3 O2(g)  2 Al2O3(s) • 2. CuO(s) + H2(g)  Cu(s) + H2O()

  7. CaCO3(s) CaO(s) + CO2(g) • 4. MnO4-(aq) + 5 Fe2+(aq) + 8 H+(aq) Mn2+(aq) + 4 H2O() + 5 Fe3+(aq)

  8. 2 H2O2(aq)  2 H2O() + O2(g) • 6. CaCO3(s) + 2 H+(aq)  CO2(g) + H2O() + Ca2+(aq)

  9. Balancing Redox Reactions

  10. Combination and Decomposition Reactions Thermal decomposition of metal carbonates: MCO3(s)  MO(s) + CO2(g) Combination of two elements to form a compound Zn + S  ZnS

  11. Organic Reactions A. Combustion Reactions Reaction with oxygen gas to form CO2 and H2O. C3H8(g) + 5 O2(g)  3 CO2(g) + 4 H2O(l) B. Substitution Reactions Exchange of one atom or molecular fragment.

  12. C. Addition Reactions Addition of two molecules together. D. Elimination Reactions Ejection of a small molecule from a larger one.

  13. E. Isomerization (Rearrangement) Reactions Change of shape of a molecule without gain or loss of any atoms.

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