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Unit 7: Predicting Products

Unit 7: Predicting Products. Chapter 11.1 Pages 330-339. Predicting Products. Synthesis A + B  AB Practice Sodium metal reacts with chlorine gas Na (s) + Cl 2(g)  Solid Magnesium reacts with fluorine gas Mg (s) + F 2(g) 

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Unit 7: Predicting Products

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  1. Unit 7:Predicting Products Chapter 11.1 Pages 330-339

  2. Predicting Products • Synthesis • A + B  AB • Practice • Sodium metal reacts with chlorine gas Na(s) + Cl2(g)  • Solid Magnesium reacts with fluorine gas Mg(s) + F2(g)  • Aluminum metal reacts with fluorine gas Al(s) + F2(g) 

  3. Predicting Products • Decomposition • AB  A + B • Practice • Solid Lead (IV) oxide decomposes PbO2(s)  • Aluminum nitride decomposes AlN(s) 

  4. Predicting Products • Single Replacement • AB + C  AC + B • Must use activity series to determine if a reaction will take place (page 333) • Practice • Sodium chloride solid reacts with fluorine gas NaCl(s) + F2(g)  • Aluminum metal reacts with aqueous copper (II) nitrate Al(s)+ Cu(NO3)2(aq)

  5. Predicting Products • Double Replacement • AB + CD  AD + CB • Practice • Calcium chloride reacts with sodium phosphate CaCl2(aq) + Na3PO4(aq)  • Lead (II) nitrate reacts with barium chloride Pb(NO3)2(aq) + BaCl2(aq) 

  6. Predicting Products • Acid/Base (a special type of double replacement reaction) • HA + B(OH)  H2O + BA • Practice • Hydrochloric acid reacts with sodium hydroxide HCl(aq) + NaOH(aq)  • Sulfuric acid reacts with copper (II) hydroxide H2SO4(aq) + Cu(OH)2(aq) 

  7. Predicting Products • Combustion • Always produces carbon dioxide and water • Practice • Pentane reacts with oxygen C5H12 + O2 • Decane reacts with oxygen C10H22 + O2 

  8. Net Ionic Equations • A complete ionic equation shows dissolved ionic compounds as dissociated free ions. • Example: • Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq)  AgCl (s) + Na+ (aq) + NO3- (aq)

  9. Net Ionic Equations • Spectator ions – those ions not directly involved in the chemical reaction. • Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq)  AgCl (s) + Na+ (aq) + NO3- (aq) • Net ionic equation – equation for reaction in solution that shows only those particles that are directly involved the chemical change. • Ag+ (aq) + Cl- (aq)  AgCl (s)

  10. Net Ionic Equations • You can predict which compounds are the spectator ions by using the following solubility rules:

  11. Net Ionic Equations • Pb(NO3) 2 (aq) + H2SO4 (aq)  PbSO4 (s) + HNO3 (aq) • Pb2+ + (NO3) -+ H2+ + SO4  PbSO4 + H+ + NO3- • H+ + NO3- spectator ions because nitrate salts are soluble and will not form precipitates. • PbSO4 is not a spectator ion because the sulfate is combined with lead, one of the noted exceptions. • Net ionic reaction Pb2+ + SO4  PbSO4

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