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

2. C 3 H 8 (g)+ O 2 (g)  A. Combustion n Reactants:  Often hydrocarbons O2O2 n Products:  All contain oxygen  hydrocarbons form CO 2 + H 2 O

3. Fe(s)+ CuSO 4 (aq)  D. Single Replacement n Products:  metal  metal (+)  nonmetal  nonmetal (-) Br 2 ( l )+ NaCl(aq) 

4. Pb(NO 3 ) 2 (aq)+ KI(aq)  E. Double Replacement n Products:  switch negative ions NaNO 3 (aq)+ NiCl 2 (aq) 

5. Neutralization Reaction n Neutralization Reactions always result in the formation of a salt and water n HBr + LiOH  n H 2 SO 4 + Al(OH) 3 

6. Practice n Na + CaCl 2  n HCl + Ba(OH) 2  n MgSO 4 + PbCl 2  n C 3 H 8 + O 2 

7. Net Ionic Equations n Complete ionic equation = equation that shows all dissolved ionic compounds as dissociated free ions n 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 n Spectator Ion = an ion that appears on both sides of an equation and is not directly involved in the reaction

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

9. Net Ionic Equations AgNO 3 (aq) + KCl(aq)  AgCl(s) + KNO 3 (aq) Ag + (aq) + NO 3 – (aq) + K + (aq) + Cl – (aq)  AgCl(s) + K + (aq) + NO 3 – (aq) CIE: Molecular (or Full) Equation: NIE: Ag + (aq) + Cl – (aq)  AgCl(s) SI: K + (aq) and NO 3 – (aq)

10. Example K 3 PO 4 (aq) + Al(NO 3 ) 3 (aq)  AlPO 4(s) + 3KNO 3(aq)

11. Practice n BeI 2(aq) + Cu 2 SO 4(aq)  2CuI (s) + BeSO 4(aq) n Ni(NO 3 ) 3(aq) + 3KBr (aq)  NiBr 3(s) + 3KNO 3(aq) 3Ca(OH) 2(aq) + 2FeCl 3(aq)  2Fe(OH) 3(s) + 3CaCl 2(aq)

12. Solubility Rules n All chlorides, bromides, and iodides are soluble except those containing Ag +, Pb 2+, or Hg 2 2+. n All compounds containing NO 3 -, ClO 4 -, ClO 3 -, and C 2 H 3 O 2 - anions are soluble.

13. n All sulfates (SO 4 -2 ) are soluble except those containing Hg 2 2+, Pb 2+, Sr 2+, Ca 2+, or Ba 2+. n All compounds containing alkali metal cations (Na+, K+, H+) and the ammonium ion (NH4+) are soluble

14. n All compounds containing OH -, PO 4 3-, S 2-, CO 3 2-, O 2-,CrO 4 -2 and SO 3 2- ions are insoluble, n OH - or S 2- soluble with group 1, Ba 2+, NH 4 + n CO 3 2-, O 2-, SO 3 2- soluble with group 1 and NH 4 + n CrO 4 2- soluble with group 1, Ca 2+, Sr 2+, and NH 4 +

15. n A double replacement reaction will "fail" if n One or more of the reactants are insoluble.  Example: PbS + AgNO3 --> n If both products are soluble.  Example: NaCl + HC2H3O2 --> NaC 2 H 3 O 2 + HCl No reaction. No ppt. Rule 2 and Rule 4

16. Practice n KBr n PbCO 3 n Li 2 SO 3 n Zn(OH) 2 n NaC 2 H 3 O 2 n AgI n CdS n ZnCO 3 Soluble Insoluble