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IV. Predicting Products

Ch. 11 – Chemical Reactions. IV. Predicting Products. A. Combustion. Reactants: Often hydrocarbons O 2 Products : All contain oxygen hydrocarbons form CO 2 + H 2 O. C 3 H 8 (g)+ O 2 (g) . D. Single Replacement. Products : metal  metal (+) nonmetal  nonmetal (-).

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IV. Predicting Products

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  1. Ch. 11 – Chemical Reactions IV. Predicting Products

  2. A. Combustion • Reactants: • Often hydrocarbons • O2 • Products: • All contain oxygen • hydrocarbons form CO2 + H2O C3H8(g)+ O2(g) 

  3. D. Single Replacement • Products: • metal  metal (+) • nonmetal  nonmetal (-) Fe(s)+ CuSO4(aq)  Br2(l)+ NaCl(aq) 

  4. E. Double Replacement • Products: • switch negative ions Pb(NO3)2(aq)+ KI(aq)  NaNO3(aq)+ NiCl2 (aq) 

  5. Neutralization Reaction • Neutralization Reactions always result in the formation of a salt and water • HBr + LiOH  • H2SO4 + Al(OH)3

  6. Practice • Na + CaCl2 • HCl + Ba(OH)2  • MgSO4 + PbCl2 • C3H8 + O2

  7. Net Ionic Equations • Complete ionic equation = equation that shows alldissolved ionic compounds as dissociated free ions • Net ionic equation = Equation for a reaction in solution that shows only those substances who do not remain as ions on both sides of the equation • Spectator Ion = an ion that appears on both sides of an equation and is not directly involved in the reaction

  8. Net Ionic Equations • Substances that are solid, liquid, or gas should not be broken down into ions • The formulas of these substances remains unchanged

  9. Net Ionic Equations Molecular (or Full) Equation: AgNO3(aq) + KCl(aq) AgCl(s) + KNO3(aq) CIE: Ag+(aq) + NO3–(aq) + K+(aq) + Cl–(aq)AgCl(s) + K+(aq) + NO3–(aq) Ag+(aq) + Cl–(aq)AgCl(s) NIE: K+(aq) and NO3–(aq) SI:

  10. Example K3PO4(aq) + Al(NO3)3(aq)  AlPO4(s) + 3KNO3(aq)

  11. Practice • BeI2(aq) + Cu2SO4(aq) 2CuI(s) + BeSO4(aq) • Ni(NO3)3(aq) + 3KBr(aq)  NiBr3(s) + 3KNO3(aq) 3Ca(OH)2(aq) + 2FeCl3(aq) 2Fe(OH)3(s) + 3CaCl2(aq)

  12. Solubility Rules • All chlorides, bromides, and iodides are soluble except those containing Ag+, Pb2+, or Hg22+. • All compounds containing NO3-, ClO4-, ClO3-, and C2H3O2- anions are soluble.

  13. All sulfates (SO4-2) are soluble except those containing Hg22+, Pb2+, Sr2+, Ca2+, or Ba2+. • All compounds containing alkali metal cations (Na+, K+, H+) and the ammonium ion (NH4+) are soluble

  14. All compounds containing OH-,  PO43-, S2-, CO32-, O2-,CrO4-2 and SO32-ions are  insoluble, • OH- or S2- soluble with group 1, Ba2+, NH4+ • CO32-, O2-, SO32- soluble with group 1 and NH4+ • CrO42- soluble with group 1, Ca2+, Sr2+, and NH4+

  15. A double replacement reaction will "fail" if • One or more of the reactants are insoluble. • Example: PbS + AgNO3 --> • If both products are soluble. • Example: NaCl + HC2H3O2 --> NaC2H3O2 + HCl No reaction. No ppt. Rule 2 and Rule 4

  16. Practice Soluble • KBr • PbCO3 • Li2SO3 • Zn(OH)2 • NaC2H3O2 • AgI • CdS • ZnCO3 Insoluble Soluble Insoluble Soluble Insoluble Insoluble Insoluble

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