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Chemistry Chemical Reactions Single and Double Replacement Reactions

Chemistry Chemical Reactions Single and Double Replacement Reactions. PERIODIC TABLES REQUIRED CALCULATORS OPTIONAL. Oxidation and Reduction. Single replacement reactions are driven by oxidation and reduction . Oxidation is the loss of electrons Reduction is the gain of electrons

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Chemistry Chemical Reactions Single and Double Replacement Reactions

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  1. ChemistryChemical ReactionsSingle and Double Replacement Reactions PERIODIC TABLES REQUIRED CALCULATORS OPTIONAL

  2. Oxidation and Reduction • Single replacement reactions are driven by oxidation and reduction. • Oxidation is the loss of electrons • Reduction is the gain of electrons • LEO goes GER • OIL RIG

  3. Oxidation-Reduction • Example: • AgNO3 + Cu  Cu(NO3)2 + Ag • What is oxidized? What is reduced? • Single replacement reactions are also known as redox reactions as a result.

  4. Activity Series • How do we know whether a single replacement reaction will happen? • The activity series tells you how active a metal is, or how able it is to displace another metal in a single replacement reaction.

  5. Activity Series • Compare the two metals or involved in the reaction. • The metal or that is higher on the activity series will be paired with the ion.

  6. Practice • Zn + HCl 

  7. Practice • Au + HCl 

  8. Double Replacement (Metathesis) • Double replacement reactions occur when two ionic solutions combine, switch ions, and one ionic compound is no longer soluble and comes out as a precipitate. • The water molecules can no longer hold the precipitate in solution, similar to how when liquid water becomes too large for air, it comes out as rain.

  9. Double Replacement (Metathesis) Reactions When one mixes ions that form compounds that are insoluble (as could be predicted by the solubility guidelines), a precipitate is formed.

  10. Double Replacement Reactions • In double replacement, the ions in the reactant compounds exchange, or transpose, ions • AgNO3(aq) + KCl(aq)  AgCl(s) + KNO3(aq)

  11. Solubility Rules (Ion Exchange) • This table should be referenced when deciding whether or not a double replacement reaction occurs. • Whenever a liquid, solid, or gas is formed from two aqueous solutions, the reaction occurs. • If you are left with two aqueous solutions, there is no reaction.

  12. Solubility Rules • Example: • AgNO3(aq) + NaCl(aq)

  13. Solubility Rules (Ion Exchange) • Example: • AgNO3(aq) + NaCl(aq) • Potential products: • AgCl (insoluble) • NaNO3 (soluble)

  14. Solubility Rules (Ion Exchange) • Example: • LiNO3(aq) + NaCl(aq) ?

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