1.  (m) c (ms -1 ) E =  [C] c [D] d [A] a [D] b 1.Numbers – Significant Figures, Rounding Rules, Accuracy, Precision, Statistical Treatment of the Data 2.Units – 5 of the 7 1.Time – seconds 2.Length – Meters Density? 3.Mass – grams Molecular Weight (Mass) 4.Amount – Moles Mole Ratio, Molarity, molality 5.Temperature – Kelvins 3.Vocabulary – Approximately 100 new terms or words and applying new or more rigid definitions to words you may already own. 4.Principles (Theories and Laws) – Stoichiometry, Quantum Theory, Bonding, Chemical Periodicity, Solutions, Thermodynamics, Intermolecular Forces, Gas Laws, Collogative Properties, Kinetics, Equilibrium, Electrochemistry c p = q/m  Trate = k[A] m [B] n ∆E = q + w c p = q/m  Trate = k[A] m [B] n ∆E = q + w  G =  H – T  SE o cell = E cathode = E anode PV = nRT%yield = actual/theoretical * 100%K =  T = Kmi

2. MonovalentDivalentTrivalent HydroniumH3O+H3O+ MagnesiumMg 2+ AluminiumAl 3+ (or hydrogen)H+H+ CalciumCa 2+ Antimony IIISb 3+ LithiumLi + StrontiumSr 2+ Bismuth IIIBi 3+ SodiumNa + BerylliumBe 2+ PotassiumK+K+ Manganese IIMn 2+ RubidiumRb + BariumBa 2+ CesiumCs + ZincZn 2+ FranciumFr + CadmiumCd 2+ SilverAg + Nickel IINi 2+ AmmoniumNH 4 + Palladium IIPd 2+ ThaliumTl + Platinum IIPt 2+ Copper ICu + Copper IICu 2+ Mercury IIHg 2+ Mercury IHg 2 2+ Iron IIFe 2+ Iron IIIFe 3+ Cobalt IICo 2+ Cobalt IIICo 3+ Chromium IICr 2+ Chromium IIICr 3+ Lead IIPb 2+ Tin IISn 2+ Table of Common Ions Common Positive Ions (Cations)

3. MonovalentDivalentTrivalent HydrideH-H- OxideO 2- NitrideN 3- FluorideFl - PeroxideO 2 2- ChlorideCl - SulfideS 2- BromideBr - SelenideSe 2- IodideI-I- OxalateC 2 O 4 2- HydroxideOH - ChromateCrO 4 2- PermanganteMnO 4 - DichromateCr 2 O 7 2- CyanideCN - TungstateWO 4 2- ThiocynateSCN - MolybdateMoO 4 2- AcetateC2H3O2-C2H3O2- tetrathionateS 4 O 6 2- NitrateNO 3 - ThiosulfateS 2 O 3 2- BisulfiteHSO 3 - SulfiteSO 3 2- BisulfateHSO 4 - SulfateSO 4 2- BicarbonateHCO 3 - CarbonateCO 3 2- Dihydrogen phosphateH 2 PO 4 - Hydrogen phosphateHPO 4 2- PhosphatePO 4 3- NitriteNO 2 - AmideNH 2 - HypochloriteClO - ChloriteClO 2 - ChlorateClO 3 - PerchlorateClO 4 - Table of Common Ions Common Negative Ions (Anions)

5. Intramolecular forces Intermolecular forces Hydrogen Bonding Henry’s Law Vapor Pressure Heat of Vaporization Phase Diagram Critical Pressure Critical Temperature Le Chatelier’s Principle Solid Liquid Gas Triple Point Critical Point Super Critical Fluid Colloid, sol, gel Emulsion Suspension Micelle Polarization Polarizability Solution Melting Freezing Deposition Sublimation Evaporation Condensation Normal Boiling/Freezing Point

6. Molality is a concentration unit based on the number of moles of solute per kilogram of solvent. Mole fraction Colligative properties are properties of solutions that depend solely on the number of particles dissolved in the solution. –Colligative properties do not depend on the kinds of particles dissolved. Colligative properties are a physical property of solutions. There are four common types of colligative properties: 1. Vapor pressure lowering 2. Freezing point depression 3. Boiling point elevation 4. Osmotic pressure  Vapor pressure lowering is the key to all four of the colligative properties.

7. Addition of a nonvolatile solute to a solution lowers the vapor pressure of the solution. –The effect is simply due to fewer solvent molecules at the solution’s surface. –The solute molecules occupy some of the spaces that would normally be occupied by solvent. Raoult’s Law models this effect in ideal solutions. Boiling Point Elevation Fractional Distillation Freezing Point Depression Osmotic Pressure