Marin: CHEM 114 - Introductory Chemistry (Daubenmire)
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Chapter 1
Chapter 1: The Chemical World 1.1: The Scope of Chemistry 1.2: Chemicals Compose Ordinary Things 1.3: Hypothesis, Theories, and Laws 1.4: The Scientific Method: How Chemists Think 1.5: A Beginning Chemist: How to Succeed
• Chapter 2
Chapter 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.E: Measurement and Problem Solving (Exercises)
• Chapter 3
Chapter 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
• Chapter 4
Chapter 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
• Chapter 5
Chapter 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
• Chapter 6
Chapter 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
• Chapter 7
Chapter 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
• Chapter 8
Chapter 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
Chapter 9
Chapter 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
• Chapter 10
Chapter 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
• Chapter 11
Chapter 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
• Chapter 12
Chapter 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
• Chapter 13
Chapter 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
• Chapter 14
Chapter 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