1. Complete Ionic Equations

2. Reactants: Zn + I 2 Product: Zn I 2

3. Murphy's Laws of Science and Technology Any instrument when dropped will roll into the least accessible corner.

4. Complete Ionic Equations: At the conclusion of our time together, you should be able to: 1.Define molecular, complete and net ionic equations 2.Write molecular, complete and net ionic equations 3. Identify a neutralization reaction 4. Realize that this is one of the 5 basic types of chemical reactions

5. Double Replacement Reactions Double Replacement Reactions occur when a metal replaces a metal in a compound and a nonmetal replaces a nonmetal in a compound Double Replacement Reactions occur when a metal replaces a metal in a compound and a nonmetal replaces a nonmetal in a compound Compound + compound  compound+ compound Compound + compound  compound+ compound AB + CD  AD + CB AB + CD  AD + CB

6. Double Replacement Reactions Think about it like “foil”ing in algebra, first and last ions go together + inside ions go together Think about it like “foil”ing in algebra, first and last ions go together + inside ions go together Example: Example: AgNO 3(aq) + NaCl (s)  AgCl (s) + NaNO 3(aq) AgNO 3(aq) + NaCl (s)  AgCl (s) + NaNO 3(aq) Another example: Another example: K 2 SO 4(aq) + Ba(NO 3 ) 2(aq)  KNO 3(aq) + BaSO 4(s) 2

7. 3 Driving Forces for Double Replacement Reactions Water Forms Gas Forms Solid Forms If one of the above is not a product, there will be no reaction.

8. Practice Predict the products. Balance the equation Predict the products. Balance the equation 1. HCl (aq) + AgNO 3 (aq)  2. CaCl 2 (aq) + Na 3 PO 4 (aq)  3. Pb(NO 3 ) 2(aq) + BaCl 2 (aq)  4. FeCl 3 (aq) + NaOH (aq)  5. H 2 SO 4 (aq) + NaOH (aq)  6. KOH (aq) + CuSO 4 (aq)  7. Ba(NO 3 ) 2(aq) + K 2 CrO 4 (aq)  8. Demo Time!! AgCl + HNO 3 NaCl + Ca 3 (PO 4 ) 2 Ba(NO 3 ) 2 + PbCl 2 NaCl + Fe(OH) 3 Na 2 SO 4 + H 2 O Cu(OH) 2 + K 2 SO 4 BaCrO 4 + KNO 3

9. Complete Ionic Equations Once you write the molecular equation (synthesis, decomposition, etc.), you should check for reactants and products that are soluble or insoluble. Once you write the molecular equation (synthesis, decomposition, etc.), you should check for reactants and products that are soluble or insoluble. We usually assume the reaction is in water We usually assume the reaction is in water We can use a solubility table to tell us what compounds dissolve in water. We can use a solubility table to tell us what compounds dissolve in water. If the compound is soluble (does dissolve in water), then split the compound into its component ions If the compound is soluble (does dissolve in water), then split the compound into its component ions If the compound is insoluble (does NOT dissolve in water), then it remains as a compound If the compound is insoluble (does NOT dissolve in water), then it remains as a compound

10. Solubility Table

11. Solubilities Not on the Table! Gases will only slightly dissolve in water Gases will only slightly dissolve in water Strong acids and bases dissolve in water Strong acids and bases dissolve in water Hydrochloric, Hydrobromic, Hydroiodic, Hydrochloric, Hydrobromic, Hydroiodic, (All Binaries) (All Binaries) Nitric, Sulfuric, Perchloric Acids Nitric, Sulfuric, Perchloric Acids (Ternary Acids with 2 more O than H) (Ternary Acids with 2 more O than H) Group I hydroxides Group I hydroxides Water slightly dissolves in water! (H+ and OH-) Water slightly dissolves in water! (H+ and OH-)

12. Complete Ionic Equations Molecular Equation: K 2 CrO 4(aq) + Ba(NO 3 ) 2(aq)  BaCrO 4(s) + 2 KNO 3(aq) Soluble Soluble Insoluble Soluble Soluble Soluble Insoluble Soluble Complete Ionic Equation: 2 K + + CrO 4 -2 + Ba +2 + 2 NO 3 -  BaCrO 4 (s) + 2 K + + 2 NO 3 -

13. Net Ionic Equations These are the same as complete ionic equations, but you should cancel out ions that appear on BOTH sides of the equation These are the same as complete ionic equations, but you should cancel out ions that appear on BOTH sides of the equation Complete Ionic Equation: 2 K + + CrO 4 -2 + Ba +2 + 2 NO 3 -  2 K + + CrO 4 -2 + Ba +2 + 2 NO 3 -  BaCrO 4 (s) + 2 K + + 2 NO 3 - Net Ionic Equation: CrO 4 -2 + Ba +2  BaCrO 4 (s) Spectator Ion

14. Neutralization Reaction Acid + Base  Salt + Water Molecular Equation: HCl + NaOH  NaCl + H 2 O SolubleSoluble Soluble Insoluble SolubleSoluble Soluble Insoluble Complete Ionic Equation: H + + Cl - + Na + + OH -  H + + Cl - + Na + + OH -  H 2 O ( l ) + Na + + Cl - H 2 O ( l ) + Na + + Cl -

15. Net Ionic Equation for Neutralization Reactions These are the same as complete ionic equations, but you should cancel out ions that appear on BOTH sides of the equation These are the same as complete ionic equations, but you should cancel out ions that appear on BOTH sides of the equation Complete Ionic Equation: H + + Cl - + Na + + OH -  H + + Cl - + Na + + OH -  H 2 O ( l ) + Na + + Cl - H 2 O ( l ) + Na + + Cl - Net Ionic Equation: H + + OH -  H 2 O ( l )

16. Complete Ionic Equations: Let’s see if you can: 1.Define molecular, complete and net ionic equations 2.Write molecular, complete and net ionic equations 3. Identify a neutralization reaction 4. Realize that this is one of the 5 basic types of chemical reactions

17. Familiar Saying One pyrus malus per diem restrains the arrival of the Hippocratic apostle. An apple a day keeps the doctor away!!

18. Practice Quiz Net Ionic Equations Write the molecular, complete ionic, and net ionic equations for this reaction: Silver nitrate reacts with calcium chloride Write the molecular, complete ionic, and net ionic equations for this reaction: Silver nitrate reacts with calcium chlorideMolecular: 2AgNO 3 + CaCl 2  2AgCl + Ca(NO 3 ) 2 Complete Ionic: 2Ag + + 2NO 3 - + Ca 2+ + 2Cl -  2AgCl + Ca 2+ + 2NO 3 - Net Ionic: 2Ag + + 2Cl -  2AgCl

19. I don’t feel so stupid now…