External
Bellingham Technical College CHEM 121
- Author
- Spencer Berger
- Publisher
- Bellingham Technical College
- Source
- LibreTexts
- Language
- EN
- Category
- Basic Sciences
Contents· 81 sections
- 01: Module 1 - Matter and Measurement
- 1.01: Chemistry- The Study of Matter
- 1.02: Classifying Matter According to Its StateSolid Liquid and Gas
- 1.03: Classifying Matter According to Its Composition
- 1.04: Differences in Matter- Physical and Chemical Properties
- 1.05: Changes in Matter - Physical and Chemical Changes
- 1.06: Conservation of Mass - There is No New Matter
- 1.07: Element Symbols and Chemical Formulas
- 1.08: Looking for Patterns - The Periodic Table
- 1.09: Energy
- 1.10: Scientific Notation - Writing Large and Small Numbers
- 1.11: Significant Figures - Writing Numbers to Reflect Precision
- 1.12: Significant Figures in Calculations
- 1.13: The Basic Units of Measurement
- 1.14: Problem Solving and Unit Conversions
- 1.15: Solving Multi-step Conversion Problems
- 1.16: Units Raised to a Power
- 1.17: Density
- 02: Module 2 - Atoms and Bonding
- 2.01: Indivisible - The Atomic Theory
- 2.02: The Nuclear Atom
- 2.03: The Properties of Protons Neutrons and Electrons
- 2.04: Elements- Defined by Their Number of Protons
- 2.05: Ions - Losing and Gaining Electrons
- 2.06: Isotopes - When the Number of Neutrons Varies
- 2.07: Atomic Mass - The Average Mass of an Elements Atoms
- 2.08: The Bohr Model - Atoms with Orbits
- 2.09: Quantum-Mechanical Orbitals and Electron Configurations
- 2.10: Electron Configurations and the Periodic Table
- 2.11: Representing Valence Electrons with Dots
- 2.12: Lewis Structures of Ionic Compounds- Electrons Transferred
- 2.13: Covalent Lewis Structures- Electrons Shared
- 2.14: Writing Lewis Structures for Covalent Compounds
- 2.15: Predicting the Shapes of Molecules
- 2.16: Electronegativity and Polarity - Polar Bonds and Polar Molecules
- 2.17: Writing Formulas for Ionic Compounds
- 2.18: Naming Ionic Compounds
- 2.19: Naming Molecular Compounds
- 03: Module 3 - Stoichiometry
- 3.01: Avogadro's Number and the Mole
- 3.02: Mole Ratios Within Compounds
- 3.03: Molar Mass of Molecules
- 3.04: Mass Percent Composition of Compounds
- 3.05: Mass Percent Composition from a Chemical Formula
- 3.06: The Chemical Equation
- 3.07: Balancing Chemical Equations
- 3.08: Mole-to-Mole Stoichiometry
- 3.09: Gram-to-Gram Stoichiometry
- 3.10: Limiting Reactant
- 3.11: Theoretical Yield and Percent Yield
- 3.12: Enthalpy Change is a Measure of the Heat Evolved or Absorbed
- 04: Module 4 - Gases and Liquids
- 4.01: Pressure - The Result of Constant Molecular Collisions
- 4.02: Boyles Law - Pressure and Volume
- 4.03: Charless Law- Volume and Temperature
- 4.04: Gay-Lussac's Law- Temperature and Pressure
- 4.05: Avogadros Law- Volume and Moles
- 4.06: The Ideal Gas Law- Pressure Volume Temperature and Moles
- 4.07: Dalton's Law of Partial Pressure
- 4.08: Intermolecular Forces
- 4.09: Properties of Liquids
- 4.10: Phase Transitions
- 4.11: Phase Diagrams
- 4.12: Water - A Remarkable Molecule
- 05: Module 5 - Solution Chemistry
- 5.01: Solutions - Homogeneous Mixtures
- 5.02: Specifying Solution Concentration- Mass Percent
- 5.03: Specifying Solution Concentration- Molarity
- 5.04: Solution Dilution
- 5.05: Solution Stoichiometry
- 5.06: Electrolytes
- 5.07: Molecular Definitions of Acids and Bases
- 5.08: Acids- Properties and Examples
- 5.09: Bases- Properties and Examples
- 5.10: Strong and Weak Acids and Bases
- 5.11: Conjugate Acids and Bases
- 5.12: Reactions of Acids and Bases
- 5.13: AcidBase Titration
- 5.14: Water - Acid and Base in One
- 5.15: The pH and pOH Scales - Ways to Express Acidity and Basicity
- 5.16: Buffers- Solutions that Resist pH Change