Marin: CHEM 114 - Introductory Chemistry (Daubenmire)
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- 1: The Chemical World
- 2: Measurement and Problem Solving
- 2.1: Taking Measurements
- 2.2: Scientific Notation: Writing Large and Small Numbers
- 2.3: Significant Figures: Writing Numbers to Reflect Precision
- 2.4: Significant Figures in Calculations
- 2.5: The Basic Units of Measurement
- 2.6: Problem Solving and Unit Conversions
- 2.7: Solving Multistep Conversion Problems
- 2.8: Units Raised to a Power
- 2.9: Density
- 2.10: Numerical Problem-Solving Strategies and the Solution Map
- 2.1: Taking Measurements
- 2.E: Measurement and Problem Solving (Exercises)
- 3: Matter and Energy
- 3.1: In Your Room
- 3.2: What is Matter?
- 3.3: Classifying Matter According to Its State: Solid, Liquid, and Gas
- 3.4: Classifying Matter According to Its Composition
- 3.5: Differences in Matter: Physical and Chemical Properties
- 3.6: Changes in Matter: Physical and Chemical Changes
- 3.7: Conservation of Mass: There is No New Matter
- 3.8: Energy
- 3.9: Energy and Chemical and Physical Change
- 3.10: Temperature: Random Motion of Molecules and Atoms
- 3.11: Temperature Changes: Heat Capacity
- 3.12: Energy and Heat Capacity Calculations
- 3.E: Exercises
- 4: Atoms and Elements
- 4.1: Experiencing Atoms at Tiburon
- 4.2: Indivisible: The Atomic Theory
- 4.3: The Nuclear Atom
- 4.4: The Properties of Protons, Neutrons, and Electrons
- 4.5: Elements: Defined by Their Numbers of Protons
- 4.6: Looking for Patterns: The Periodic Law and the Periodic Table
- 4.7: Ions: Losing and Gaining Electrons
- 4.8: Isotopes: When the Number of Neutrons Varies
- 4.9: Atomic Mass: The Average Mass of an Element’s Atoms
- 5: Molecules and Compounds
- 5.1: Sugar and Salt
- 5.2: Compounds Display Constant Composition
- 5.3: Chemical Formulas: How to Represent Compounds
- 5.4: A Molecular View of Elements and Compounds
- 5.5: Writing Formulas for Ionic Compounds
- 5.6: Nomenclature: Naming Compounds
- 5.7: Naming Ionic Compounds
- 5.8: Naming Molecular Compounds
- 5.9: Naming Acids
- 5.10: Nomenclature Summary
- 5.11: Formula Mass: The Mass of a Molecule or Formula Unit
- 6: Chemical Composition
- 6.1: How Much Sodium?
- 6.2: Counting Nails by the Pound
- 6.3: Counting Atoms by the Gram
- 6.4: Counting Molecules by the Gram
- 6.5: Chemical Formulas as Conversion Factors
- 6.6: Mass Percent Composition of Compounds
- 6.7: Mass Percent Composition from a Chemical Formula
- 6.8: Calculating Empirical Formulas for Compounds
- 6.9: Calculating Molecular Formulas for Compounds
- 7: Chemical Reactions
- 7.1: Grade School Volcanoes, Automobiles, and Laundry Detergents
- 7.2: Evidence of a Chemical Reaction
- 7.3: The Chemical Equation
- 7.4: How to Write Balanced Chemical Equations
- 7.5: Aqueous Solutions and Solubility: Compounds Dissolved in Water
- 7.6: Precipitation Reactions: Reactions in Aqueous Solution That Form a Solid
- 7.7: Writing Chemical Equations for Reactions in Solution: Molecular, Complete Ionic, and Net Ionic Equations
- 7.8: Acid–Base and Gas Evolution Reactions
- 7.9: Oxidation–Reduction Reactions
- 7.10: Classifying Chemical Reactions
- 7.11: The Activity Series
- 8: Quantities in Chemical Reactions
- 8.1: Climate Change: Too Much Carbon Dioxide
- 8.2: Stoichiometry
- 8.3: Making Molecules: Mole-to-Mole Conversions
- 8.4: Making Molecules: Mass-to-Mass Conversions
- 8.5: Limiting Reactant, Theoretical Yield, and Percent Yield
- 8.6: Limiting Reactant, Theoretical Yield, and Percent Yield from Initial Masses of Reactants
- 8.7: Enthalpy: A Measure of the Heat Evolved or Absorbed in a Reaction
- 9: Electrons in Atoms and the Periodic Table
- 9.1: Blimps, Balloons, and Models of the Atom
- 9.2: Light: Electromagnetic Radiation
- 9.3: The Electromagnetic Spectrum
- 9.4: The Bohr Model: Atoms with Orbits
- 9.5: The Quantum-Mechanical Model: Atoms with Orbitals
- 9.6: Quantum-Mechanical Orbitals and Electron Configurations
- 9.7: Electron Configurations and the Periodic Table
- 9.8: The Explanatory Power of the Quantum-Mechanical Model
- 9.9: Periodic Trends: Atomic Size, Ionization Energy, and Metallic Character
- 10: Chemical Bonding
- 10.1: Bonding Models and AIDS Drugs
- 10.2: Representing Valence Electrons with Dots
- 10.3: Lewis Structures of Ionic Compounds: Electrons Transferred
- 10.4: Covalent Lewis Structures: Electrons Shared
- 10.5: Writing Lewis Structures for Covalent Compounds
- 10.6: Resonance: Equivalent Lewis Structures for the Same Molecule
- 10.7: Predicting the Shapes of Molecules
- 10.8: Electronegativity and Polarity - Why Oil and Water Don’t Mix
- 11: Gases
- 11.1: Extra-Long Straws
- 11.2: Kinetic Molecular Theory: A Model for Gases
- 11.3: Pressure: The Result of Constant Molecular Collisions
- 11.4: Boyle’s Law: Pressure and Volume
- 11.5: Charles’s Law: Volume and Temperature
- 11.6: Gay-Lussac's Law: Temperature and Pressure
- 11.7: The Combined Gas Law: Pressure, Volume, and Temperature
- 11.8: Avogadro’s Law: Volume and Moles
- 11.9: The Ideal Gas Law: Pressure, Volume, Temperature, and Moles
- 11.10: Mixtures of Gases: Why Deep-Sea Divers Breathe a Mixture of Helium and Oxygen
- 11.11: Gases in Chemical Reactions
- 12: Liquids, Solids, and Intermolecular Forces
- 12.1: Interactions between Molecules
- 12.2: Properties of Liquids and Solids
- 12.3: Intermolecular Forces in Action: Surface Tension and Viscosity
- 12.4: Evaporation and Condensation
- 12.5: Melting, Freezing, and Sublimation
- 12.6: Types of Intermolecular Forces: Dispersion, Dipole–Dipole, Hydrogen Bonding, and Ion-Dipole
- 12.7: Types of Crystalline Solids: Molecular, Ionic, and Atomic
- 12.8: Water: A Remarkable Molecule
- 13: Solutions
- 13.1: Prelude - Tragedy in Cameroon
- 13.2: Solutions: Homogeneous Mixtures
- 13.3: Solutions of Solids Dissolved in Water: How to Make Rock Candy
- 13.4: Solutions of Gases in Water: How Soda Pop Gets Its Fizz
- 13.5: Solution Concentration: Mass Percent
- 13.6: Solution Concentration: Molarity
- 13.7: Solution Dilution
- 13.8: Solution Stoichiometry
- 13.9: Freezing Point Depression and Boiling Point Elevation: Making Water Freeze Colder and Boil Hotter
- 13.10: Osmosis: Why Drinking Salt Water Causes Dehydration
- 14: Acids and Bases
- 14.1: Sour Patch Kids and International Spy Movies
- 14.2: Acids: Properties and Examples
- 14.3: Bases: Properties and Examples
- 14.4: Molecular Definitions of Acids and Bases
- 14.5: Reactions of Acids and Bases
- 14.6: Acid–Base Titration: A Way to Quantify the Amount of Acid or Base in a Solution
- 14.7: Strong and Weak Acids and Bases
- 14.8: Water: Acid and Base in One
- 14.9: The pH and pOH Scales: Ways to Express Acidity and Basicity
- 14.10: Buffers: Solutions That Resist pH Change
This is a lecture and laboratory course that covers the fundamental concepts of chemistry. This course assumes no previous knowledge of chemistry, presenting both chemical problem solving and laboratory skills.
1: The Chemical World
2: Measurement and Problem Solving
3: Matter and Energy
4: Atoms and Elements
5: Molecules and Compounds
6: Chemical Composition
7: Chemical Reactions
8: Quantities in Chemical Reactions
9: Electrons in Atoms and the Periodic Table
10: Chemical Bonding
11: Gases
12: Liquids, Solids, and Intermolecular Forces
13: Solutions
14: Acids and Bases