Nguồn ngoài
CHEM 202: General Chemistry II OER
CHEM 202: General Chemistry II is a continuation of General Chemistry I (CHEM 201) that covers more advanced topics in chemistry. The course includes lectures, problem-solving activities, and laboratory investigations. Key topics include chemical kinetics, equilibrium, thermodynamics, electrochemistry, transition metals, and nuclear chemistry.
- Tác giả
- Patricia Foley
- Nhà xuất bản
- College of the Canyons
- Nguồn
- LibreTexts
- Ngôn ngữ
- EN
- Danh mục
- Khoa học cơ bản
Mục lục· 91 mục
- 01: Introduction to Organic Chemistry
- 1.01: General Characteristics of Organic Molecules
- 1.02: Drawing Chemical Structures
- 1.03: Alkanes
- 1.04: Unsaturated Hydrocarbons
- 1.05: Organic Compounds with Functional Groups
- 1.06: Structural Isomerism in Organic Molecules
- 1.07: Stereoisomerism in Organic Molecules
- 1.08: Optical Isomerism in Organic Molecules
- 1.09: Organic Reactions
- 1.10: Organic Chemistry (Exercises)
- 02: Coordination Chemistry of Transition Metals
- 2.01: Properties of Transition Metals
- 2.02: Coordination Chemistry of Transition Metals
- 2.03: Nomenclature for Coordination Compounds
- 2.04: Geometries of Coordination Complexes
- 2.05: Isomerism
- 2.06: Optical and Magnetic Properties of Coordination Compounds
- 2.07: Transition Metals and Coordination Chemistry (Exercises)
- 03: Chemical Kinetics
- 3.01: Chemical Reaction Rates
- 3.02: Factors Affecting Reaction Rates
- 3.03: Rate Laws
- 3.04: Integrated Rate Laws
- 3.05: Collision Theory
- 3.06: Reaction Mechanisms
- 3.07: Catalysis
- 3.E: Kinetics (Exercises)
- 04: Chemical Equilibrium
- 4.01: Chemical Equilibria
- 4.02: Equilibrium Constants
- 4.03: Gas Phase Equilibria and Heterogeneous Systems
- 4.04: Shifting Equilibria - Le Chateliers Principle
- 4.05: Calculating Equilibrium Constants and Equilibrium Concentrations
- 4.06: Calculating Equilibrium Concentrations with the x-is-small Approximation
- 4.07: Equilibrium Constant Manipulations
- 4.E: Fundamental Equilibrium Concepts (Exercises)
- 05: Acid-Base Equilibria
- 5.01: Brnsted-Lowry Acids and Bases
- 5.02: pH and pOH
- 5.03: Relative Strengths of Acids
- 5.04: pH Calculations for Weak Acids
- 5.05: Relative Strengths of Bases
- 5.06: Relating Structure to Acidity and Basicity
- 5.07: Hydrolysis of Salt Solutions
- 5.E: Acid-Base Equilibria (Exercises)
- 06: Acid-Base Equilibria in Mixtures
- 6.01: Mixtures of Acids
- 6.02: Polyprotic Acids
- 6.03: Buffers
- 6.04: Henderson-Hasselbalch Approximation
- 6.05: Acid-Base Titrations
- 6.06: pH Calculations for AcidBase Titrations
- 6.E: Acid-Base Equilibria (Exercises)
- 07: Solubility and Complex-Ion Equilibria
- 7.01: Solubility Product Constant Ksp
- 7.02: Relationship Between Solubility and Ksp
- 7.03: Common-Ion Effect in Solubility Equilibria
- 7.04: Criteria for Precipitation and its Completeness
- 7.05: Fractional Precipitation
- 7.06: Solubility and pH
- 7.07: Equilibria Involving Complex Ions
- 7.08: Qualitative Cation Analysis
- 7.09: Equilibria of Other Reaction Classes (Exercises)
- 08: Thermodynamics
- 8.01: Spontaneity- The Meaning of Spontaneous Change
- 8.02: The Concept of Entropy
- 8.03: Evaluating Entropy and Entropy Changes
- 8.04: Criteria for Spontaneous Change- The Second Law of Thermodynamics
- 8.05: Standard Gibbs Energy Change G
- 8.06: Gibbs Energy Change and Equilibrium
- 8.07: G and K as Functions of Temperature
- 8.08: Coupled Reactions
- 8.E: Chemical Thermodynamics (Exercises)
- 09: Electrochemistry
- 9.01: Balancing Oxidation-Reduction Reactions
- 9.02: Galvanic Cells
- 9.03: Standard Reduction Potentials
- 9.04: The Nernst Equation
- 9.05: Batteries and Fuel Cells
- 9.06: Corrosion
- 9.07: Electrolysis
- 9.E: Electrochemistry (Exercises)
- 10: Nuclear Chemistry
- 10.01: Nuclear Equations
- 10.02: Radioactive Decay
- 10.03: Nuclear Structure and Stability
- 10.04: Transmutation and Nuclear Energy
- 10.05: Uses of Radioisotopes
- 10.06: Biological Effects of Radiation
- 10.E: Nuclear Chemistry (Exercises)