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Types of Reactions

Types of Reactions. Chapter 7. Synthesis(Combination) Reaction. Na (l) + Cl 2 (g) --> NaCl(s) Balance the reaction. You know you have a synthesis reaction when… 2 Reactants, 1 Product Reactants are elements or simpler compound Product is a compound. Decomposition Reaction.

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Types of Reactions

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  1. Types of Reactions Chapter 7

  2. Synthesis(Combination) Reaction • Na (l) + Cl2(g) --> NaCl(s) • Balance the reaction. • You know you have a synthesis reaction when… • 2 Reactants, 1 Product • Reactants are elements or simpler compound • Product is a compound

  3. Decomposition Reaction • Cu(NO3)2 (aq) --> NO2 (g) + O2 (g)+ CuO (s) • Balance the reaction • You know you have a decomposition reaction when… • 1 Reactant, 2+ products

  4. Single Replacement • Al (s) + Fe2O3 (s) --> Al2O3 (s) + Fe(l) • Balance the equation • You know you have a single replacement reaction when… • Element + compound element + compound

  5. Combustion • CH4(g) + 2O2(g)  CO2 (g) +2H2O(g) • You know you have a combustion reaction when… • Oxygen is a reactant and carbon dioxide + water are the products.

  6. Double Replacement • NaOH (aq) + AgNO3 (aq) --> AgOH (s) + NaNO3(aq) • You know you have a double replacement reaction when… • Compound + Compound Compound + Compound

  7. Back to ions… • What is an ionic compound? • What happens when an ionic compound dissolves in water? • The compound dissociates, or separates into the individual ions.

  8. So… • When mixing two dissolved ionic compounds, you are really mixing the ions together. • A chemical reaction can occur! • A precipitation reaction: reaction in which a solid forms and separates from the solution.

  9. How do precipitation reactions work? • Example: Let’s mix potassium chromate solution and barium nitrate solution together • What is the chemical equation (reactants only) for this reaction? • K2CrO4 (aq) + Ba(NO3)2 (aq) • But these are ionic compounds, so it’s really the ions dissolved in water • 2K+ (aq) + CrO42- (aq) + Ba2+ (aq) + 2NO3- (aq)

  10. The reaction

  11. But what are the products? • Experimental evidence tells us that one product is a solid. A solid must be electrically neutral, a cation with an anion • What are the options? • K2CrO4 ; Ba(NO3)2 • KNO3 ; BaCrO4 • But which one is the solid?

  12. Use solubility rules!

  13. What does it all mean? • Nitrate and potassium salts are soluble, so potassium nitrate cannot be a precipitate. • Therefore, barium chromate is the solid.

  14. How do you write all of this • Molecular (undissociated) equation • K2CrO4 (aq) + Ba(NO3)2 (aq)  KNO3(aq) + BaCrO4 (s) • Complete ionic equation (any ionic “aq” broken up into ions. • 2K+(aq) + CrO42-(aq) + Ba2+(aq) + 2NO3- (aq) 2K+(aq) + 2NO3- (aq)+BaCrO4 (s) • Net ionic equation(eliminate spectator ions) • CrO42-(aq) + Ba2+(aq) BaCrO4 (s)

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