Overview

This course in General Chemistry aims to provide learners with a foundational understanding of chemistry concepts. By the end of the course, students will be able to identify different types of matter, balance chemical equations, understand atomic theory, comprehend the periodic table, and grasp concepts related to chemical bonding, thermodynamics, kinetics, equilibria, acids and bases, electrochemistry, and nuclear reactions. The course teaches skills such as calculating formulas, writing chemical equations, and measuring pressure. The teaching method includes lectures, demonstrations, and problem-solving exercises. This course is intended for high school and college students taking introductory chemistry courses or anyone interested in gaining a basic understanding of chemistry.

Syllabus

Introduction to Chemistry.
Types of Matter: Elements, Compounds, and Mixtures.
Measurement and Significant Figures.
Scientific Notation and Dimensional Analysis.
History of Atomic Theory.
Nuclide Symbols: Atomic Number, Mass Number, Ions, and Isotopes.
Balancing Chemical Equations.
The Mole: Avogadro's Number and Stoichiometry.
Limiting Reagents and Percent Yield.
Elemental Analysis: Empirical and Molecular Formulas.
Kinetic Molecular Theory and the Ideal Gas Laws.
Wave-Particle Duality and the Photoelectric Effect.
Bohr Model of the Hydrogen Atom.
Quantum Mechanics of the Electron.
Quantum Numbers, Atomic Orbitals, and Electron Configurations.
The Periodic Table: Atomic Radius, Ionization Energy, and Electronegativity.
The Chemical Bond: Covalent vs. Ionic and Polar vs. Nonpolar.
Naming Ionic Compounds.
Lewis Dot Structures.
VSEPR Theory and Molecular Geometry.
Intermolecular Forces and Boiling Points.
Thermochemistry: Heat and Enthalpy.
Hess's Law and Heats of Formation.
Heat Capacity, Specific Heat, and Calorimetry.
Phase Changes, Heats of Fusion and Vaporization, and Phase Diagrams.
Solution Chemistry and Net Ionic Equations.
Molarity and Dilution.
Solubility and the Born-Haber Cycle.
Molality and Colligative Properties.
The Laws of Thermodynamics, Entropy, and Gibbs Free Energy.
Kinetics: Initial Rates and Integrated Rate Laws.
Energy Diagrams, Catalysts, and Reaction Mechanisms.
Chemical Equilibria and Reaction Quotients.
Le Chatelier's Principle.
Valence Bond Theory, Hybrid Orbitals, and Molecular Orbital Theory.
Acids and Bases, pH and pOH.
Acid-Base Equilibria and Buffer Solutions.
Acid-Base Titration.
Oxidation-Reduction Reactions.
Electrochemistry.
Nuclear Reactions, Radioactivity, Fission and Fusion.
Accuracy and Precision for Data Collection.
Converting Between Temperature Scales (Celsius, Fahrenheit, and Kelvin).
Visualizing Molecular Geometry With 3D Software.
Calculating Percent Error.
Nomenclature of Oxyacids.
Nomenclature of Hydrated Salts.
Writing Chemical Equations in Words.
The Law of Conservation of Matter.
Expressing Concentration by Mass Percent.
Calculating the Formulas of Hydrated Salts.
What Are Electrolytes?.
Calculating Ion Concentrations in Solution.
Neutralization Reactions.
Dalton's Law and Partial Pressures.
What Are Standard Conditions?.
Molar Gas Volume: Stoichiometry With Gases.
Kinetic Molecular Theory and its Postulates.
Temperature and Gas Solubility.
Balancing Redox Reactions in Acidic and Basic Conditions.
Pseudo Noble Gas Electron Configurations.
Complex Ion Formation.
Lattice Structures in Ionic Solids.
Covalent Bond Energy and Length.
Limitations of VSEPR Theory.
Examples of s-p Mixing in Molecular Orbital Theory.
Measuring Pressure With Barometers and Manometers.
Non-Ideal Gases and the Van der Waals Equation.
Viscosity, Cohesive and Adhesive Forces, Surface Tension, and Capillary Action.
Types of Colloids and Their Properties.
Solubility Product Constant (Ksp).
Predicting Precipitation With Ksp Values.
Selective Precipitation.
The Common Ion Effect.
Coordination Compounds: Geometry and Nomenclature.
Crystal Field Theory.
Radiometric Dating: Carbon-14 and Uranium-238.
Conductivity and Semiconductors.
Spectrophotometry and Beer's Law.
The Chemistry of Air Purification.