Mole Course

Lesson 1 • What Is a Mole?

Defines the mole as a standard SI unit for amount of substance. Establishes the conceptual bridge between atomic-scale particles and measurable macroscopic quantities.

Lesson 2 • Avogadro's Number Explained

Introduces 6.022 × 10²³ as the number of entities per mole. Connects this constant to atomic mass and the periodic table.

Lesson 3 • Mole vs. Mass vs. Number

Distinguishes moles, mass in grams, and particle count as three interconvertible quantities. Prepares students for conversion calculations in later sections.

Lesson 1 • Atomic Mass and the Periodic Table

Explains how atomic mass values on the periodic table represent weighted averages of isotopes. Links atomic mass units to grams per mole for practical use.

Lesson 2 • Precision and Significant Figures

Applies significant figure rules to molar mass calculations to ensure reportable accuracy. Connects precision standards to real laboratory and industrial contexts.

Lesson 3 • Molar Mass of Compounds

Teaches summation of atomic masses weighted by subscripts to find compound molar mass. Reinforces formula reading and arithmetic precision.

Lesson 1 • Moles to Mass Conversions

Uses molar mass as a conversion factor to convert moles into grams. Builds the core calculation skill applied throughout all subsequent chapters.

Lesson 2 • Moles to Particles Conversions

Applies Avogadro's number to convert moles into atoms, molecules, or formula units. Extends conversion skills to the particle level.

Lesson 3 • Conversion Practice and Fluency

Provides varied practice sets to consolidate all conversion types. Identifies and corrects persistent errors before advancing to stoichiometry.

Lesson 4 • Multi-Step Conversion Problems

Chains mass-to-moles and moles-to-particles conversions in a single calculation. Develops problem-solving fluency for complex real-world scenarios.

Lesson 1 • Deriving Empirical Formulas

Converts percent composition data to mole ratios and reduces to the simplest whole-number formula. Builds the analytical skill of interpreting elemental analysis results.

Lesson 2 • Molecular Formulas from Empirical Formulas

Uses molar mass data to scale the empirical formula to the true molecular formula. Connects empirical formula work to real compound identification.

Lesson 3 • Percent Composition by Mass

Defines percent composition as the mass fraction of each element in a compound. Uses molar mass to calculate theoretical percent composition from a formula.

Lesson 1 • Mole-to-Mole Stoichiometry

Calculates moles of product or reactant from given moles of another substance. Isolates the mole ratio step before introducing mass conversions.

Lesson 2 • Balancing Chemical Equations

Reviews conservation of mass and the rules for balancing equations by inspection. Provides the balanced equations required for all stoichiometric calculations.

Lesson 3 • Mass-to-Mass Stoichiometry

Chains molar mass conversions with mole ratios to convert grams of one substance to grams of another. Integrates all prior skills into the standard stoichiometry workflow.

Lesson 4 • Mole Ratios from Balanced Equations

Extracts mole ratios from stoichiometric coefficients and uses them as conversion factors. Establishes the central tool of all stoichiometry calculations.

Lesson 1 • Excess Reagent Calculations

Determines the mass of excess reagent remaining after a reaction reaches completion. Completes the full quantitative picture of a limiting reagent problem.

Lesson 2 • Concept of the Limiting Reagent

Explains why the reagent present in the smallest stoichiometric amount controls product yield. Uses analogies and visual models to build intuitive understanding.

Lesson 3 • Theoretical Yield Calculations

Calculates the maximum possible product mass using the limiting reagent. Establishes the benchmark against which actual experimental yield is measured.

Lesson 4 • Percent Yield and Reaction Efficiency

Computes percent yield from actual and theoretical yield and interprets its meaning. Connects yield analysis to quality control and process optimization.

Lesson 1 • Concentration and Molarity

Defines molarity as moles of solute per liter of solution and distinguishes it from other concentration units. Establishes the vocabulary and formula used throughout solution chemistry.

Lesson 2 • Titration and Stoichiometric Equivalence

Introduces titration as a technique for determining unknown concentration using stoichiometric equivalence. Applies all solution and stoichiometry skills to a standard analytical method.

Lesson 3 • Dilution Calculations

Applies the dilution equation (C₁V₁ = C₂V₂) to calculate concentrations after dilution. Builds skill in preparing working solutions from stock solutions.

Lesson 4 • Preparing Solutions of Known Molarity

Describes the laboratory procedure for dissolving a solute to reach a target molarity. Connects calculation to practical volumetric glassware technique.

Lesson 1 • Moles and Ideal Gas Law

Applies the ideal gas law (PV = nRT) to relate moles of gas to pressure, volume, and temperature. Extends mole calculations into the gas phase.

Lesson 2 • Electrochemistry and Faraday's Law

Uses moles of electrons transferred to calculate mass deposited or dissolved in electrolytic processes. Applies mole concepts to electrochemical stoichiometry.

Lesson 3 • Multi-Concept Integration Problems

Presents complex problems requiring simultaneous use of stoichiometry, solution chemistry, and gas laws. Builds the integrative reasoning needed for advanced coursework and professional work.

Lesson 4 • Moles in Thermochemical Equations

Connects mole quantities to enthalpy changes expressed per mole in thermochemical equations. Enables energy calculations scaled to any reaction amount.