Beginner Chemistry Course

Lesson 1 • The Scientific Method in Chemistry

Outlines hypothesis formation, controlled experimentation, and data interpretation. Students apply this framework to structure all lab work in the course.

Lesson 2 • What Chemistry Studies

Defines chemistry's scope and its role in science and daily life. Establishes context for all subsequent topics by linking chemistry to observable phenomena.

Lesson 3 • Classifying Matter

Distinguishes pure substances from mixtures and elements from compounds. Provides the vocabulary needed to describe and categorize all chemical systems.

Lesson 4 • Measurement and SI Units

Introduces the International System of Units and precision in measurement. Accurate unit use underpins every quantitative calculation in the course.

Lesson 1 • Organization of the Periodic Table

Explains periods, groups, and element families and their arrangement logic. Table structure reflects electron configuration and predicts element behavior.

Lesson 2 • Subatomic Particles and Atomic Number

Identifies protons, neutrons, and electrons and their roles in atomic identity. Atomic number and mass number define every element uniquely.

Lesson 3 • Historical Models of the Atom

Traces atomic theory from Dalton through Bohr to the quantum model. Understanding model evolution shows how evidence shapes scientific knowledge.

Lesson 4 • Periodic Trends

Quantifies how atomic radius, ionization energy, and electronegativity vary across the table. These trends enable prediction of bonding type and reactivity.

Lesson 1 • Writing Chemical Formulas

Teaches criss-cross and charge-balance methods for writing correct formulas. Formula accuracy is foundational for stoichiometry and equation balancing.

Lesson 2 • Naming Ionic Compounds

Covers naming binary ionic compounds and those with polyatomic ions. Correct nomenclature is essential for communicating chemical identity in lab and industry.

Lesson 3 • Naming and Writing Acid Formulas

Introduces binary acid and oxyacid naming rules and formula derivation. Acid nomenclature connects directly to solution chemistry and reaction prediction.

Lesson 1 • Intermolecular Forces

Distinguishes London dispersion, dipole-dipole, and hydrogen bonding forces. IMF strength explains boiling points, solubility, and surface tension.

Lesson 2 • Lewis Structures and Resonance

Teaches step-by-step Lewis structure drawing including formal charge and resonance. Accurate Lewis structures are prerequisite for geometry and polarity prediction.

Lesson 3 • Molecular Geometry: VSEPR Theory

Applies VSEPR theory to predict three-dimensional shapes from electron pair repulsion. Geometry determines polarity and physical properties of molecules.

Lesson 4 • Covalent Bonding

Explains electron sharing between nonmetals and distinguishes single, double, and triple bonds. Bond order and length directly affect molecular stability and reactivity.

Lesson 1 • Types of Chemical Reactions

Classifies reactions as synthesis, decomposition, single replacement, double replacement, or combustion. Classification enables systematic product prediction.

Lesson 2 • Writing and Balancing Equations

Introduces reactant-product notation and systematic balancing by inspection. Balanced equations are the foundation for all stoichiometric and thermodynamic calculations.

Lesson 3 • Net Ionic Equations

Teaches dissociation of strong electrolytes and cancellation of spectator ions. Net ionic equations reveal the actual chemical change in aqueous reactions.

Lesson 1 • The Mole Concept

Defines the mole, Avogadro's number, and molar mass as conversion tools. The mole bridges atomic-scale counts and laboratory-scale masses.

Lesson 2 • Solution Stoichiometry and Molarity

Defines molarity and applies it to dilution and titration calculations. Solution stoichiometry is essential for quantitative analytical chemistry.

Lesson 3 • Mole Ratios and Stoichiometry

Uses balanced equation coefficients as mole ratios for mass-to-mass calculations. Mole ratios are the core tool for predicting reaction quantities.

Lesson 1 • Phase Changes and Phase Diagrams

Identifies all six phase transitions and interprets phase diagrams. Phase diagrams map stable states across temperature and pressure conditions.

Lesson 2 • Kinetic Molecular Theory

Describes particle motion assumptions underlying all three states of matter. KMT explains macroscopic properties like pressure and temperature at the molecular level.

Lesson 3 • Ideal Gas Law and Dalton's Law

Unifies gas variables in PV = nRT and applies Dalton's law to gas mixtures. These laws enable molar mass determination and partial pressure calculations.

Lesson 4 • Properties of Solids and Liquids

Contrasts crystalline and amorphous solids and explains liquid surface phenomena. IMF strength determines melting point, viscosity, and surface tension.

Lesson 1 • Solubility Equilibrium and Ksp

Introduces the solubility product constant and predicts precipitation from ion concentrations. Ksp calculations are essential for water treatment and analytical chemistry.

Lesson 2 • Le Chatelier's Principle

Predicts equilibrium shifts in response to concentration, temperature, and pressure changes. Applying Le Chatelier's principle optimizes yield in industrial chemical processes.

Lesson 3 • Energy, Heat, and Enthalpy

Distinguishes heat, work, and enthalpy and classifies reactions as exothermic or endothermic. Enthalpy change is the primary energy quantity measured in calorimetry.

Lesson 4 • Introduction to Chemical Equilibrium

Defines dynamic equilibrium and the equilibrium constant expression. Equilibrium concepts govern reaction completeness in industrial and biological systems.