CHEM 115 1st Edition Lecture 11Outline of Last LectureI. Water as a SolventOutline of Current LectureI. Molecular EquationII. Total Ionic EquationIII. Net Ionic EquationIV. Precipitate ReactionV. Solubility RulesCurrent Lecture Molecular Equation: shows all reactants and products as if they were intact, undissociated compounds- Gives least information about species in solutionTotal Ionic Equation: shows soluble ionic substances dissociated into ions- Gives most accurate information about species in solution- Spectator ions: are not involved in actual chemical change - Balances chargesNet Ionic Equation: simplified equation without spectator ions- Include (s), (l), and (g) NOT (aq)2AgNO3(aq) + Na2CrO4(aq) Ag2CrO4(s) + 2NaNO3(aq)Molecular2Ag+ + 2NO3- + 2Na+ + CrO4-2 Ag2CrO4(s) + 2Na+ + 2NO3-Total Ionic2Ag+ + CrO4-2 Ag2CrO4(s) NetPrecipitate Reaction: 2 soluble ionic compounds react to give an insoluble products called a precipitateThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.Solubility Rules1. All common group 1A ions and NH4+ are soluble2. NO3-, CH3COO-, C2H3H2-, and most ClO4- are soluble3. Cl-, Br-, I- are soluble EXCEPT with Ag+, Pb+2, Cu+, Hg+24. Sulfides insoluble EXCEPT with 1A, 2A, and NH4+5. F- are soluble EXCEPT with Pb+2 and 2A6. SO2-2 are soluble EXCEPT with Ca+2, Sr+2, Ba+2, Ag+, Pb+7. CO3-2, PO4-3 are insoluble EXCEPT with 1A and NH4+8. Metal hydroxides insoluble EXCEPT with 1A, 2A (beginning with
View Full Document
Unlocking...