High School Chemistry Workbook

This document is the table of contents for a chemistry workbook created by CK-12 Foundation, a non-profit group. CK-12's goal is to make textbooks cost less for students in kindergarten through 12th grade, both in the United States and around the world. They do this by using an "open-content" model, which means the material is free for anyone to use and can be edited or improved by many people working together online. CK-12 calls this collaborative approach the "FlexBook" system. Their hope is to create excellent educational materials that can serve as a main textbook while also adjusting to fit each student's own learning needs.

The workbook itself covers many major topics in chemistry, organized into numbered chapters and lessons. Below is a summary of what students will find in each section:

Chapter 1 introduces the science of chemistry, covering the scientific method (the step-by-step process scientists use to test ideas), the history of chemistry, and basic concepts like matter (anything that has mass and takes up space) and energy.

Chapter 2 focuses on chemistry as a physical science, teaching students how to take measurements, use math, and apply algebra when solving chemistry problems.

Chapter 3 covers laboratory skills, including how to make observations, take measurements, and use and interpret data.

Chapter 4 explains atomic theory — the scientific explanation of how atoms are built — including its early history and important vocabulary used to describe atoms.

Chapter 5 discusses the Bohr model of the atom, a scientific model that explains how electrons behave, along with lessons on light waves, the dual nature of light (light acting like both a wave and a particle), and atomic spectra (the specific patterns of light given off by different elements).

Chapter 6 dives deeper into the quantum mechanics model of the atom, a more advanced and accurate description of atomic structure. It includes lessons on the wave-particle duality of matter, Schrödinger's wave functions (mathematical descriptions of where electrons are likely to be), Heisenberg's contributions to atomic theory, quantum numbers (values that describe an electron's energy and position), and the shapes of atomic orbitals (regions where electrons are most likely found).

Chapter 7 explains electron configurations, which describe how electrons are arranged in an atom. Topics include the electron spin quantum number, the Pauli Exclusion Principle (a rule stating that no two electrons in an atom can have the exact same set of quantum numbers), the Aufbau Principle (a rule for how electrons fill orbitals), and how to write electron configurations.

Chapter 8 connects electron configurations to the periodic table, showing how the arrangement of elements relates to their electron patterns.

Chapter 9 explores relationships between elements, including element families (groups with similar properties), electron configurations, Lewis electron dot diagrams (simple drawings that show an atom's outer electrons), transition elements, and the lanthanide and actinide series (two special rows of elements usually shown at the bottom of the periodic table).

Chapter 10 examines patterns, or trends, across the periodic table, such as atomic size, ionization energy (the energy needed to remove an electron from an atom), and electron affinity (how strongly an atom attracts an extra electron).

Chapter 11 covers ions (atoms that have gained or lost electrons, giving them an electric charge) and the compounds they form, including ionic bonding and the properties of ionic compounds.

Chapter 12 teaches students how to write and name ionic formulas, including predicting the formulas of ionic compounds and using proper chemical naming rules.

Chapter 13 introduces covalent bonding, a type of bond where atoms share electrons, along with which atoms typically form these bonds and how to name covalent compounds.

Chapter 14 discusses molecular architecture — the shapes and structures of molecules. Topics include different types of bonds, covalent molecules formed by certain element families, resonance (when a molecule's structure can be drawn in more than one valid way), electronic and molecular geometry (the shapes molecules take), and molecular polarity (how unevenly electrons are shared within a molecule).

Chapter 15 focuses on the mathematics of compounds, including how to calculate formula and molecular mass, understand the mole (a unit chemists use to count extremely large numbers of particles), calculate percent composition (the percentage of each element in a compound), and determine empirical and molecular formulas (different ways of expressing a compound's makeup).

Chapter 16 covers chemical reactions, including how to write chemical equations, balance them, and identify different types of reactions.

Chapter 17 applies mathematics to chemical equations, teaching students about the mole concept, mass-to-mass calculations, limiting reactants (the substance that runs out first in a reaction, stopping it), percent yield (how much product is actually made compared to the expected amount), and energy calculations.

Chapter 18 introduces the kinetic molecular theory, which explains the behavior of matter in its three states — solid, liquid, and gas. This includes lessons on gases, gas pressure, gas laws, the universal gas law, molar volume, and how gases are involved in chemical calculations.

Chapter 19 explores the liquid state, covering the properties of liquids, forces of attraction between molecules, vapor pressure, boiling point, and heat of vaporization (the energy needed to turn a liquid into a gas).

Chapter 20 examines the solid state, showing how the arrangement of molecules affects a solid's characteristics, along with lessons on melting, types of attractive forces in solids, and phase diagrams (charts that show how matter changes between solid, liquid, and gas depending on temperature and pressure).

Chapter 21 discusses the solution process — how substances dissolve into one another — including why solutions form, key vocabulary, how to measure concentration, solubility graphs, factors that affect solubility, colligative properties (properties of a solution that depend on how many particles are dissolved in it), colloids (mixtures where tiny particles are spread through another substance), and how to separate mixtures.

Chapter 22 covers ions in solution, including how covalent compounds behave in solution and how ions react with each other.

Chapter 23 introduces chemical kinetics, the study of how fast reactions happen. This includes reaction rates, collision theory (the idea that particles must collide to react), potential energy diagrams, factors that affect reaction speed, and reaction mechanisms (the step-by-step process of how a reaction occurs).

Chapter 24 explains chemical equilibrium, a state where a reaction happens forward and backward at the same rate. Topics include the equilibrium constant, how stress or changes affect a reaction at equilibrium, and slightly soluble salts.

Chapter 25 focuses on acids and bases, covering Arrhenius acids and bases (substances that release specific ions in water), strong versus weak acids, salts, pH (a scale that measures how acidic or basic a substance is), weak acid and base equilibria, Brønsted-Lowry acids and bases (a broader definition based on transferring particles called protons), and Lewis acids and bases (an even broader definition based on sharing electron pairs).

Chapter 26 covers water, pH, and titration (a lab method used to find the concentration of a solution), including how water naturally splits into ions and how indicators are used to show changes in acidity.