|
|
The High School Chem Solutions package comes with a lesson for each of
the following topics.
1. Atomic Theory and Periodicity
1.1 The Histroy of Atomic Theory
1.2 Isotopes and Average Atomic Mass
1.3 Waves
1.4 Quantum Theory
1.5 Atomic Emission Spectrum
1.6 DeBroglie Wave Equation
1.7 Quantum Numbers
1.8 Electron Configuration and Orbital Diagrams
1.9 Periodicity
2. Nomenclature
2.1 Naming Ionic Compounds and Ionic Formulas
2.2 Naming Covalent Compounds and Molecular Formulas
2.3 Naming Acids
3. Quantitative Chemistry
3.1 Molecular Weight and Mass Percent
3.2 The Mole
3.3 Mole to Mole Problems
3.4 Mass to Mass Problems
3.5 Limiting Reactant Problems
3.6 Empirical and Molecular Formulas
4. Chemical Bonding
4.1 Ionic and Covalent Bonding
4.2 Lewis Structures
4.3 Exceptions to the Octet Rule
4.4 Formal Charge
4.5 Resonance Structures
4.6 VSEPR I
4.7 VSEPR II
4.8 Valence Bond Theory and Hybrid Orbital Theory
4.9 Polar and Non-Polar Molecule
5. Intermolecular Forces
5.1 Types of Intermolecular Forces
6. Solutions
6.1 Types of Solutions
6.2 Expressing Concentration
6.3 Solubility and Precipitation Reactions
6.4 Factors Affecting Solubility, Solubility Curves and Supersaturated Solutions
6.5 Factors Affecting the Solubility of Gases
6.6 Colligative Properties
7. Redox Reactions
7.1 Redox Reactions and Oxidation Numbers
7.2 Balancing Redox Reactions in Acidic and Basic Solutions
7.3 The Activity Series and Types of Redox Reactions
8. Thermodynamics
8.1 Endothermic / Exothermic Reactions and Enthalpy
8.2 Average Bond Enthalpy
8.3 Calorimetry
8.4 Hess' Law
8.5 Enthalpy of Formation
8.6 Enthalpy of Vaporization and Enthalpy of Fusion
8.7 Entropy
8.8 Free Energy
9. Equilibrium
9.1 Dynamic Equilibrium and the Equilibrium Expression
9.2 The Pressure Constant and Equilibrium Position
9.3 Calculating Equilibrium Concentrations and Partial Pressures
9.4 The Reaction Quotient
9.5 Le Chatelier's Principle
9.6 Manipulating Equilibrium Constants
9.7 The Solubility Product Constant and Predicting Precipitates
9.8 Free Energy and Equilibrium
10. Gases
10.1 Pressure, Kinetic Molecular Theory, Boyle's Law, Charles Law, and Combined Gas Law
10.2 Avogadro's Principle and STP
10.3 Ideal Gas Law
10.4 Dalton's Law of Partial Pressure and Collecting Gas over Water
10.5 Mole Fractions and Partial Pressures
10.6 Average Kinetic Energy and Speed of a Gas
10.7 Effusion and Diffusion
10.8 Real vs. Ideal Gases
11. Solids
11.1 Unit Cells, Molecular Solids, Covalent Network Solids, and Metallic Solids
12. Phase Diagrams
12.1 Phase Diagrams
13. Electrochemistry
13.1 Voltaic Cells and Standard Cell Potentials
13.2 Spontaneous Redox Reactions and Free Energy
13.3 Nernst Equation and Concentration Cells
13.4 Electrolytic Cells
14. Acids and Bases
14.1 Defining Acids and Bases
14.2 Strengths of Acids and Bases
14.3 Acid and Base Dissociation Constants
14.4 The pH of Strong Acids and Bases
14.5 Calculating the pH of Weak Acids
14.6 Calculation the pH of Weak Bases
14.7 Reactions of Acids and Bases
14.8 Soluble Salts and pH
14.9 The Common Ion Effect
14.10 Buffered Solutions
14.11 Solubility and pH
14.12 Complex Ion Formation
14.13 Acid Base Titrations
15. Kinetics
15.1 Reaction Rates, Order of Reactions, and Rate Laws
15.2 Integrated Rate Laws
15.3 Factors Affecting Reaction Rates and Activation Energy
15.4 Reactions Mechanisms and Catalysis
16. Nuclear Chemistry
16.1 Modes of Nuclear Decay
16.2 Configurations for Nuclear Stability
16.3 Half Life
16.4 Nuclear Fission and Fusion
17. Organic Chemistry
17.1 Naming Alkanes and Structural Isomerism
17.2 Naming Alkenes, Alkynes, and Aromatic Compounds
17.3 Naming Functional Groups
17.4 Reactions of Hydrocarbons
17.5 Reactions of Functional Groups
1. Atomic Theory and Periodicity
1.1 The Histroy of Atomic Theory
1.2 Isotopes and Average Atomic Mass
1.3 Waves
1.4 Quantum Theory
1.5 Atomic Emission Spectrum
1.6 DeBroglie Wave Equation
1.7 Quantum Numbers
1.8 Electron Configuration and Orbital Diagrams
1.9 Periodicity
2. Nomenclature
2.1 Naming Ionic Compounds and Ionic Formulas
2.2 Naming Covalent Compounds and Molecular Formulas
2.3 Naming Acids
3. Quantitative Chemistry
3.1 Molecular Weight and Mass Percent
3.2 The Mole
3.3 Mole to Mole Problems
3.4 Mass to Mass Problems
3.5 Limiting Reactant Problems
3.6 Empirical and Molecular Formulas
4. Chemical Bonding
4.1 Ionic and Covalent Bonding
4.2 Lewis Structures
4.3 Exceptions to the Octet Rule
4.4 Formal Charge
4.5 Resonance Structures
4.6 VSEPR I
4.7 VSEPR II
4.8 Valence Bond Theory and Hybrid Orbital Theory
4.9 Polar and Non-Polar Molecule
5. Intermolecular Forces
5.1 Types of Intermolecular Forces
6. Solutions
6.1 Types of Solutions
6.2 Expressing Concentration
6.3 Solubility and Precipitation Reactions
6.4 Factors Affecting Solubility, Solubility Curves and Supersaturated Solutions
6.5 Factors Affecting the Solubility of Gases
6.6 Colligative Properties
7. Redox Reactions
7.1 Redox Reactions and Oxidation Numbers
7.2 Balancing Redox Reactions in Acidic and Basic Solutions
7.3 The Activity Series and Types of Redox Reactions
8. Thermodynamics
8.1 Endothermic / Exothermic Reactions and Enthalpy
8.2 Average Bond Enthalpy
8.3 Calorimetry
8.4 Hess' Law
8.5 Enthalpy of Formation
8.6 Enthalpy of Vaporization and Enthalpy of Fusion
8.7 Entropy
8.8 Free Energy
9. Equilibrium
9.1 Dynamic Equilibrium and the Equilibrium Expression
9.2 The Pressure Constant and Equilibrium Position
9.3 Calculating Equilibrium Concentrations and Partial Pressures
9.4 The Reaction Quotient
9.5 Le Chatelier's Principle
9.6 Manipulating Equilibrium Constants
9.7 The Solubility Product Constant and Predicting Precipitates
9.8 Free Energy and Equilibrium
10. Gases
10.1 Pressure, Kinetic Molecular Theory, Boyle's Law, Charles Law, and Combined Gas Law
10.2 Avogadro's Principle and STP
10.3 Ideal Gas Law
10.4 Dalton's Law of Partial Pressure and Collecting Gas over Water
10.5 Mole Fractions and Partial Pressures
10.6 Average Kinetic Energy and Speed of a Gas
10.7 Effusion and Diffusion
10.8 Real vs. Ideal Gases
11. Solids
11.1 Unit Cells, Molecular Solids, Covalent Network Solids, and Metallic Solids
12. Phase Diagrams
12.1 Phase Diagrams
13. Electrochemistry
13.1 Voltaic Cells and Standard Cell Potentials
13.2 Spontaneous Redox Reactions and Free Energy
13.3 Nernst Equation and Concentration Cells
13.4 Electrolytic Cells
14. Acids and Bases
14.1 Defining Acids and Bases
14.2 Strengths of Acids and Bases
14.3 Acid and Base Dissociation Constants
14.4 The pH of Strong Acids and Bases
14.5 Calculating the pH of Weak Acids
14.6 Calculation the pH of Weak Bases
14.7 Reactions of Acids and Bases
14.8 Soluble Salts and pH
14.9 The Common Ion Effect
14.10 Buffered Solutions
14.11 Solubility and pH
14.12 Complex Ion Formation
14.13 Acid Base Titrations
15. Kinetics
15.1 Reaction Rates, Order of Reactions, and Rate Laws
15.2 Integrated Rate Laws
15.3 Factors Affecting Reaction Rates and Activation Energy
15.4 Reactions Mechanisms and Catalysis
16. Nuclear Chemistry
16.1 Modes of Nuclear Decay
16.2 Configurations for Nuclear Stability
16.3 Half Life
16.4 Nuclear Fission and Fusion
17. Organic Chemistry
17.1 Naming Alkanes and Structural Isomerism
17.2 Naming Alkenes, Alkynes, and Aromatic Compounds
17.3 Naming Functional Groups
17.4 Reactions of Hydrocarbons
17.5 Reactions of Functional Groups