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Oxidation-Reduction Reactions

This guide explores oxidation-reduction reactions, focusing on predicting products of single replacement reactions. It highlights the activity series of metals and nonmetals, demonstrating how a more reactive element replaces a less reactive one within a compound. Key concepts include using standard reduction potentials for prediction, the roles of acids, and the reactions of metals with acids. Through practice problems and illustrative examples, students will learn to identify reaction types, determine possible products, and apply these principles effectively in AP Chemistry.

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Oxidation-Reduction Reactions

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  1. Oxidation-Reduction Reactions Predicting Products of Reactions AP Chemistry Ms. Paskowski

  2. Single Replacement Reactions More reactive element will replace a less reactive element Metals – use the activity series or the Standard reduction tables Nonmetals – use the activity table (easier)

  3. Activity Series

  4. Single Replacement Reactions of Metals • The more reactive metal will replace the less reactive metal within a compound • Example • Zn (s) + CuSO4 Cu (s) + ZnSO4 • The more reactive zinc replaces copper.

  5. Single Replacement Reactions Standard reduction potentials • All reactions listed are reduction reactions. • The reactions most likely to occur have the largest positive value. • The more positive, the more likely to be reduced

  6. Predicting Products of Single Replacement Reactions • M + AB or N + CD • where M = metal and N = Nonmetal • Use Activity table to determine whether • M is more active than A or less likely to be reduced, if so a reaction will occur. • N is more active than D or more likely to be reduced, if so a reaction will occur

  7. Practice Problems • Chemistry: Matter and Its Changes • Page 224 #5.50 and 5.51

  8. Elements with Water • Very active metals will combine with water to form bases • Hydroxides • Often produce hydrogen gas • Very Reactive Nonmetals will react with water to form acids • Conditions will dictate which acid is formed.

  9. Oxidizing Power of Acids • Nonoxidizing acids– i.e. HCl, HBr • Hydrogen will be replaced by a more active metal. H will be reduced and the metal will be oxidized. Anion does not participate • Oxidizing Acids always contain oxygen. • Anion is sometimes a stronger oxidizer than H+ • i.e. HNO3, H2SO4 (under certain conditions)

  10. Reactions of Metals with Acids • Acids will react with active metals • Using the Standard Reduction Potential table • If the reduction value is negative , the metal will replace the H in the acid and Hydrogen gas will be produced. • If the reduction value is positive, no reaction will occur.

  11. Predicting Products of the Metal/Acid Reactions • For anoxy acids, the products are a salt and hydrogen gas • M + HA  MA + H2 • For oxoacids, the products are a salt, water, and a gas • M + HAxOy  H2O + M+ + AzOq • Practice Problems • Page 224 # 46-49

  12. Molecular Oxygen • Oxidizer! • Combustion is the adding of oxygen to carbon and hydrogen (and sulfur and nitrogen). • Reaction with metals form oxides • Reaction with nonmetals produce nonmetallic oxides

  13. Oxides and Water • Soluble Metallic oxides • MxOy produce bases (hydroxides) when dissolved in water • Example • NaOH + H2O  Na+ + OH- • Nonmetallic oxides • Produce acids when dissolved in water • Example • N2O5 + H2O  H+ + NO3 –

  14. Oxides and Acids or Bases • Metallic oxides plus acid • Produce a salt and water • Metallic oxides are weak bases and will react with the acid to produce salt and water • Nonmetallic oxides plus bases • Nonmetallic oxides are acidic • Produce a salt and water • Nonmetallic oxides are weak acids and will react with the base to produce salt and water

  15. Metallic Oxides and Nonmetallic Oxides • Metallic oxides and nonmetallic oxides will combine to form a salt • Example • MgO + CO2  MgCO3 • CaO + SO3  CaSO4

  16. Synthesis Reactions • Metals plus nonmetals • Adding Hydrogen makes hydrides • Adding halogens makes halides • Adding nitrogen makes nitrides • Adding sulfur makes sulfides • Adding oxygen makes oxides • Adding LOTS of oxygen makes peroxides • Adding water makes hydroxides or oxides and hydrogen gas

  17. Decomposition • Problems given will usually produce a oxygen or water • Examples • CaCO3  CaO + CO2 • H2O2  H2O + O2 • KClO3  KCl + O2 • Al(OH)3  Al2O3 + H2O

  18. Helpful Hints • Write all the species down in their physical state, i.e. liquid, solid, gas, or ions in solution • Determine the type of reaction that could occur • Double replacement – acid/base or precipitate • Oxidation-Reduction – single replacement, combustion, decomposition (only one reactant), synthesis • If nothing else fits, use a simple redox reaction where the charges on the ions change.

  19. Let’s Practice

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