Chemistry Chemical Reactions Single and Double Replacement Reactions PERIODIC TABLES REQUIRED CALCULATORS OPTIONAL

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Chemistry Chemical Reactions Single and Double Replacement Reactions PERIODIC TABLES REQUIRED CALCULATORS OPTIONAL Slide 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 Slide 3 Oxidation-Reduction Example: AgNO 3 + Cu Cu(NO 3 ) 2 + Ag What is oxidized? What is reduced? Single replacement reactions are also known as redox reactions as a result. Slide 4 Activity Series How do we know whether a single replacement reaction will happen? 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. The activity series tells you how active a metal is, or how able it is to displace another metal in a single replacement reaction. Slide 5 Activity Series Compare the two metals or involved in the reaction. 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. The metal or that is higher on the activity series will be paired with the ion. Slide 6 Practice Zn + HCl Zn + HCl Slide 7 Practice Au + HCl Au + HCl Slide 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. Slide 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. Slide 10 Double Replacement Reactions In double replacement, the ions in the reactant compounds exchange, or transpose, ions AgNO 3(aq) + KCl (aq) AgCl (s) + KNO 3(aq) Slide 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. Slide 12 Solubility Rules Example: AgNO 3(aq) + NaCl (aq) Slide 13 Solubility Rules (Ion Exchange) Example: AgNO 3(aq) + NaCl (aq) Potential products: AgCl (insoluble) NaNO 3 (soluble) Slide 14 Solubility Rules (Ion Exchange) Example: LiNO 3(aq) + NaCl (aq) ?