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General Chemistry 1


This highly interactive course covers the complete first semester of General Chemistry. It includes extensive and engaging practice for students including: problems with detailed feedback, adaptive exercises, simulations, interactive examples, virtual lab activities and more all integrated together in a seamless flow.


This course is intended for Majors and is adapted from OpenStax Chemistry with many additions and modifications including: activities with PHeT simulations; problem sets that revolve around real-world scenarios; interactive examples; simulations, instructor-led videos demonstrating problem solving methods; animations; and more.  The course is highly interactive and engaging, designed in a logical flow that transitions smoothly between small amounts of expository text, worked examples, activities, interactives, simulations, and other media.

Adhering to OLI philosophy, this course provides immediate and detailed feedback for its many formative assessment activities, appropriate scaffolding, and clearly aligned learning objectives. General Chemistry 1 covers all content typically covered in the first semester of a college course.

What students will learn

Coming soon.

Learning objectives by module

Unit 1: Foundations of Chemistry

Module 2: Properties of Matter

  • Classify matter as element, compound, or mixtures.
  • Describe the four states of matter.
  • Recognize physical and chemical changes and properties.


Module 3: Measurements

  • Convert among the temperature scales of Fahrenheit, Celsius, and Kelvin.
  • Convert units using dimensional analysis.
  • Determine the accuracy and precision of sets of data.
  • Record measurements and calculations using the correct number of significant figures.
  • Use the International System of Units for measurements.


Module 4: Atomic Theory

  • Describe the contributions of John Dalton to modern atomic theory.
  • Describe the evolution of the atomic theory.


Module 5: Elements and Compounds

  • Apply the concepts of isotopes and their percent abundance to make calculations associated with atomic mass.
  • Describe how chemical bonds form.
  • Describe the arrangement of the periodic table of elements.
  • Distinguish between molecular and ionic compounds.
  • Interpret chemical symbols for isotopes and ions.
  • Name chemical compounds.
  • Write chemical formulas for compounds.


Unit 2: Reactions and Stoichiometry

Module 7: The Mole

  • Calculate the percent composition of a compound.
  • Convert amounts of substances among moles, particles, and mass.
  • Determine formulas for empirical and molecular formulas.


Module 8: Aqueous Solutions

  • Apply concepts of mass percentage, volume percentage, parts per million, and parts per billion.
  • Calculate concentrations of solutions that involve molarity.
  • Describe aqueous solutions.


Module 9: Chemical Equations

  • Describe acid-base reactions.
  • Describe oxidation-reduction reactions.
  • Describe precipitation reactions.
  • Represent chemical reactions with chemical equations.


Module 10: Reaction Stoichiometry

  • Apply stoichiometric relationships to calculate amounts of substances involved in chemical reactions.
  • Calculate the percent yield of a chemical reaction.
  • Identify limiting reactants in chemical reactions.


Unit 3: Gases

Module 12: Gas Laws

  • Calculate pressure, temperature, volume, or amount of gas by applying the appropriate gas law.
  • Make calculations involving gas pressure as it relates to the measurement of gas pressure.


Module 13: Stoichiometry of Gases

  • Apply combined concepts of stoichiometry and the ideal gas law to calculate the amounts of substances in a chemical reaction.
  • Apply Dalton’s law of partial pressures.
  • Apply stoichiometric relationships to calculate amounts of substances involved in chemical reactions.


Module 14: The Kinetic-Molecular Theory

  • Describe the relationship between molecular velocities, kinetic energy, and molar mass of gases.
  • Describe the relationship between the kinetic molecular theory and the gas laws.
  • Explain the differences between ideal gases and real gases.


Unit 4: Thermochemistry

Module 16: Introduction to Energy

  • Calculate internal energy for processes and explain its classification as a state function.
  • Describe the nature of energy changes that accompany chemical and physical changes.


Module 17: Calorimetry

  • Calculate heat transferred in chemical and physical processes.
  • Distinguish the related properties of heat, thermal energy, and temperature.


Module 18: Enthalpy

  • Calculate enthalpy changes for various chemical reactions.

Unit 5: Electronic Structure and Periodic Properties


Module 20: Electromagnetic Energy and the Bohr Model of the Atom

  • Describe the Bohr model of the hydrogen atom.
  • Describe the particle nature of light.
  • Describe the wave nature of light.


Module 21: Quantum Theory

  • Describe the general idea of the quantum mechanical model of the atom.
  • List and describe traits of the four quantum numbers that form the basis for completely specifying the state of an electron in an atom.
  • Write electron configurations for elements and identify valence electrons from them.


Module 22: Periodic Properties

  • Describe and distinguish between ionization energy and electron affinity.
  • Describe and explain the observed periodic trends of atomic and ionic size.


Unit 6: Chemical Bonding and Molecular Geometry

Module 24: Ionic and Covalent Bonding

  • Assess the polarity of covalent bonds.
  • Describe covalent bond formation.
  • Describe ionic bond formation.


Module 25: Lewis Structures

  • Draw Lewis structures depicting the bonding in molecules.
  • Explain the concept of resonance and draw Lewis structures representing resonance forms for a given molecule.
  • Use average covalent bond energies to estimate enthalpies of reactions.
  • Use formal charges to identify the most reasonable Lewis structure for a given molecule.


Module 26: Molecular Structure and Polarity

  • Assess the polarity of a molecule based on its bonding and structure.
  • Predict the structures of small molecules using valence shell electron pair repulsion (VSEPR) theory.


Module 27: Advanced Theories of Covalent Bonding

  • Apply the concept of Covalent Bond Theory to describe covalent bonds in molecules.
  • Apply the concept of hybridization to describe covalent bonds.


Unit 7: Solids and Liquids

Module 29: Intermolecular Forces

  • Describe the roles of intermolecular attractive forces in viscosity, surface tension, and capillary rise.
  • Describe the types of intermolecular forces possible between atoms or molecules in condensed phases.
  • Identify the types of intermolecular forces experienced by specific molecules based on their structures.


Module 30: Phase Changes

  • Describe the processes represented by typical heating and cooling curves, and compute heat flows and enthalpy changes accompanying these processes.
  • Explain the relation between phase transition temperatures and intermolecular attractive forces.
  • Use phase diagrams to identify stable phases at given temperatures and pressures, and to describe phase transitions resulting from changes in these properties.


Module 31: The Solid State of Matter

  • Define and describe the bonding and properties of ionic, molecular, metallic, and covalent network crystalline solids.


Unit 8: Solutions

Module 33: Solubility

  • Describe the basic properties of solutions and how they form.
  • Describe the solubility of gases, liquids, and solids in liquids.
  • Explain solute-solvent interactions of ionic and covalent electrolytes.


Module 34: Colligative Properties

  • Express concentrations of solution components using mole fraction and molality.
  • Perform calculations using the mathematical equations that describe various colligative effects.

Course assessments, activities, and outline

UNIT 1: Foundations of Chemistry

Module 1: Course Introduction

Module 2: Properties of Matter

QUIZ: Properties of Matter

Module 3: Measurements

QUIZ: Measurements

Module 4: Atomic Theory

QUIZ: Atomic Theory

Module 5: Elements and Compounds

QUIZ: Elements and Compounds

UNIT 2: Reactions and Stoichiometry

Module 6: Introduction

Module 7: The Mole

QUIZ: The Mole

Module 8: Aqueous Solutions

QUIZ: Aqueous Solutions

Module 9: Chemical Equations

QUIZ: Chemical Equations

Module 10: Reaction Stoichiometry

QUIZ: Reaction Stoichiometry

Module 11: Reactions and Stoichiometry: Unit Practice

UNIT 3: Gases

Module 12: Introduction

Module 13: Gas Laws

QUIZ: Gas Laws

Module 14: Stoichiometry of Gases

QUIZ: Stoichiometry of Gases

Module 15: The Kinetic-Molecular Theory

QUIZ: The Kinetic Molecular Theory

UNIT 4: Thermochemistry

Module 16: Introduction

Module 17: Introduction to Energy

QUIZ: Introduction to Energy

Module 18: Calorimetry

QUIZ: Calorimetry

Module 19: Enthalpy

QUIZ: Enthalpy

UNIT 5: Electronic Structure and Periodic Properties

Module 20: Introduction

Module 21: Electromagnetic Energy and the Bohr Model of the Atom

QUIZ: Electromagnetic Energy and the Bohr Model of the Atom

Module 22: Quantum Theory

QUIZ: Quantum Theory

Module 23: Periodic Properties

QUIZ: Periodic Properties

Module 24: Electronic Structure and Periodic Properties: Unit Practice

UNIT 6: Chemical Bonding and Molecular Geometry

Module 25: Introduction

Module 26: Ionic and Covalent Bonding

QUIZ: Ionic and Covalent Bonding

Module 27: Lewis Structures

QUIZ: Lewis Structures

Module 28: Molecular Structure and Polarity

QUIZ: Molecular Structure and Polarity

Module 29: Advanced Theories of Covalent Bonding

QUIZ: Advanced Theories of Covalent Bonding

UNIT 7: Solids and Liquids

Module 30: Introduction

Module 31: Intermolecular Forces

QUIZ: Intermolecular Forces

Module 32: Phase Changes

QUIZ: Phase Changes and Diagrams

Module 33: The Solid State of Matter

QUIZ: The Solid State of Matter

UNIT 8: Solutions

Module 34: Introduction

Module 35: Solubility

QUIZ: Solubility

Module 36: Colligative Properties

QUIZ: Colligative Properties

UNIT 9: Appendix

Module 37: Appendix

Other course details

Adapted from OpenStax Chemistry by Sandra Raysor with contributions from David Yaron and Mark Blaser.

System requirements

OLI system requirements, regardless of course:

  • internet access
  • an operating system that supports the latest browser update
  • the latest browser update (Chrome recommended; Firefox, Safari supported; Edge and Internet Explorer are supported but not recommended)
  • pop-ups enabled
  • cookies enabled

Some courses include exercises with exceptions to these requirements, such as technology that cannot be used on mobile devices.

This course’s system requirements:

  • A full desktop operating system, such as Windows or Mac OS X.
  • Flash
  • Java

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$25 per student

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