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Predicting Chemical Reaction Products: A Comprehensive Guide

This chapter focuses on predicting the products of various chemical reactions, including synthesis, decomposition, single replacement, double replacement, acid-base reactions, and combustion. Detailed practice problems are provided, including helpful examples such as the reactions between sodium metal and chlorine gas, magnesium with fluorine, and the decomposition of lead(IV) oxide. The section also covers net ionic equations, identifying spectator ions, and the importance of solubility rules. This guide is essential for understanding chemical reactivity and product formation.

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Predicting Chemical Reaction Products: A Comprehensive Guide

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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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