SAT II (Chemistry)

• Matter and Energy : Matter; Substances ;Chemical and Physical Properties; Energy;  Types of Energy ; Endothermic and Exothermic Reactions

• Phases of Matter : Gases :Kinetic Molecular Theory ; Pressure ; Boyle’s Law; Charles’Law ;Temperature ; Standard Temperature and Pressure;  Average Kinetic Energy of Gases ;Combined Gas Law ; Dalton’s Law of Partial Pressures; Avogadro’s Law ; Graham’s Law of Diffusion/ Effusion and Density of Gases ; Ideal Gas Law—Relating Pressure, Volume, Temperature, and Moles; Liquids ; Boiling Point ; Solids ; Sublimation and Deposition ; Phase Changes

• Atomic Structure : A Brief History of the Atom ; Subatomic Particles ; Isotopes; The Bohr Model of the Atom; Wave-Mechanical Model ; Valence Electrons and Dot Diagrams ; Effective Nuclear Charge—Zeff ; Quantum Numbers; Hybridization ; Ions and the Octet Rule ; Exceptions to the Octet Rule ; Isoelectronic Series 

• The Periodic Table and Periodic Trends : History of the Periodic Table Arrangement of the Periodic Table ; Metals, Nonmetals, and Semimetals ; The Families ; Electronegativity ; Ionization Energy ; Atomic Radius ; Ionic Radius ; The s, p, d, and f Blocks 

• Bonding : Intramolecular Bond versus Intermolecular Bonds ; Ionic Bonding ; Covalent Bonding ; Sigma and Pi Bonds ; Network, Coordinate Covalent, and Metallic Bonds ; Dipole Forces and Polarities of Molecules ; Resonance Structures ; VSEPR Theory ; Hydrogen Bonding ; Van der Waals (London Dispersion) Forces ; Molecule-Ion Attraction ; Naming Compounds ; Determining Chemical Formulas ; Stock Method 

• Stoichiometry and Solution Chemistry : Chemical Formulas: Balancing Chemical Equations ; Mole Ratios; Moles, Mass, Volumes, and Molecules ; Limiting and Excess Reagents ; Percent Composition ; Empirical Formulas from Percent Composition ; Concentration and Dilutions ; Colligative Properties ; Solubility of Compounds ; Net Ionic Equations ; Percent Yield

• Energy and Chemical Reactions : Potential Energy Diagrams Revisited ; Heat and Changes in Phase ; Thermometry ; Hess’s Law ; Bond Dissociation Energy ; Entropy, Gibbs Free Energy, and Spontaneous Reactions

• Reaction Rates and Chemical Equilibrium : Reaction Rates ; Reverse Reactions and Potential Energy Diagrams; Equilibrium ; Le Châtelier’s Principle ; Equilibrium Constants and Mass Action Equations; Solubility Product Constants ; Common Ion Effect; Reactions That Go to Completion 

• Acids and Bases : Naming Acids and Bases; Operational Definitions of Acids and Bases; Conceptual Definition of Acids and Bases; Arrhenius Acids and Bases; Brønsted-Lowry Acids and Bases and Conjugate Pairs; Lewis Acids and Bases; Titration and Neutralization ; Hydrolysis ; Ka and the Strength of Acids;  pH and the pH Scale; Buffers

• Redox and Electrochemistry : Redox Defined : Oxidation Numbers; Writing Half Reactions; Strength of Oxidizing and Reducing Agents ; Balancing Half Reactions; The Voltaic Cell ; E° Values and Spontaneous Reactions The Electrolytic Cell 

• Organic Chemistry : Carbon; Hydrocarbons; Naming Organic Compounds; Naming Hydrocarbons and Their Isomers; Cyclic Hydrocarbons ; Aromatics ; Alcohols and Ethers; Carbonyl-Containing Compounds; Compounds Containing Nitrogen; Organic Reactions with Halogens

• Nuclear Chemistry : Radioactive Isotopes ; Radioactive Emanations ; Separating Nuclear Emanations; Nuclear Fusion and Fission ; Half-Life (t1/2); Dangers and Benefits of Using Radioisotopes

• Laboratory Skills : Laboratory Safety; The Meniscus; Collecting Gases Dehydration of a Salt; Methods for Separation; Titration; The Metric System; Dimensional Analysis ; Percent Error Accuracy versus Precision ; Significant Figures


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