Please refer to the table below. In the Reading column, the ChemWiki and outside links are taken after the Table of Contents of the Zumdahl textbook whose topic organization the course generally follows. (NOTE: Any commmonly used General Chemistry book, print, or free Open Educational Resource (OER), would suit this purpose.) The Reading column also includes short, printable Peer Led Team Learning (PLTL) "Executive Summaries" (.pdf) of important topics & concepts within the Chapter. Class Presentations contain links to Powerpoint (.pptx), Web-based Powerpoint (.htm), and printable Powerpoint (.pdf) files that capture the in-class activities, which reflect the course's pedagogy. All three types of Presentation files (.pptx, .htm, .pdf) provide the same information. The Presentations should be used as the principal resource-guide to the topics and provide a sense of their relative importance. They include embedded i-clicker questions (without answers). Correctly answering as many i-clicker questions as possible before class is most important. This portion of graded work constitutes 10% of the overall course grade. I-clicker questions and Homework Questions are both very important resources for exam and quiz preparation, which will in a large part be fashioned from them. In the Questions column, interactive examples and other practice tools are also provided. The Animations column includes links to those used for in-class presentations plus other related on-line resources for your use. Vocabulary focuses on minimal, essential terms. It is not a comprehensive list. [NOTE: Chem 120 Collaborative Worksheets, which are required and assigned throughout the course, are only available in the printed Chem 120 Lab Manual specifically for Dr. R's sections. It is available at the DVC Bookstore.]
Chapter: 1) Chemical Foundations; 2) Atoms, Compounds, and Ions; 3) Stoichiometry; 4) Types of Chemical Reactions and Solution Stoichiometry; 5) Gases; 6) Thermochemistry; 7) Atomic Structure and Periodicity; 8) Bonding: General Concepts; 10) Liquids and Solids; 11) Properties of Solutions; 13) Chemical Equilibrium; 14) Acid and Base Equilibria
Unit I: Chapters 1-4 (Exam 1); Unit II: Chapters 5-8 (Exam 2); Chapters 10, 11, 13, 14 (Exam 3)
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1.1: Chemical Foundations 1.2: The Scientific Method 1.3: Units of Measurement 1.4: Uncertainty in Measurement 1.5: Significant Figures and Calculations 1.6: Systematically Solving Problems
1.7: Dimensional Analysis: Unit Conversions 1.8: Temperature 1.9: Density 1.10: Classification of Matter |
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Powers of Ten (Movie) Powers of Ten (Images) |
Homework Density Problem (interactive) Elements, Compounds and Mixtures Quiz
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uncertainty |
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2.1: The Early History of Chemistry Timeline of Chemistry 2.2: The Fundamentals of Chemistry 2.3: Dalton's Atomic Theory 2.4: Early Atomic Experiments 2.5: Modern Atomic Theory 2.6: Molecules and Ions 2.7: The Periodic Table 2.8: Chemical Nomenclature |
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Lawrence Berkeley National Lab: Electron Microscope |
Homework Homework |
nucleus (chemical) proton neutron electron ionic covalent isotope atomic mass atomic number bonds (chemical) cation anion group (periodic table) period metal non-metal metalloids |
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3.1: Counting with Mass 3.2: Average Atomic Masses 3.3: Avogadro's Number 3.4: Molar Mass 3.5: Problem Solving 3.6: Percent Composition 3.7: Empirical and Molecular Formulas 3.8: Writing Chemical Equations 3.9: Balancing Chemical Equations 3.10: Determining the Amount of Reactant and Product 3.11: Limiting and Excess Reagents |
Part I: _____________ Molecular Formula Calculations: % Water in a Hydrate Experimental (Calculations): Periodic Table
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Nitrogen triiodide Decomposition Silver formation - Single Displacement Zn + S → CH4 + O2→ Stoichiometry NO + Cl2 → Limiting Reagent Zn + HCl → Limiting Reactants (Interactive) Mass Percent Problem (Interactive) Mass to atoms or molecules Problem (Interactive) |
Homework Homework Limiting Reactant (Interactive) Limiting Reagent Prroblem (Interactive) |
stoichiometry molar mass empirical formula molecular formula mole ratio limiting reactant (limiting reagent) theoretical yield percent yield |
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4.1: Water as a Solvent 4.2: Strong and Weak Electrolytes 4.3: Molarity and Dilution 4.4: Chemical Reactions 4.5: Precipitation Reactions 4.6: Types of Equations that Represent Reactions in Solution 4.7: Stoichiometry for Reactions in Solution 4.8: Acid-Base Reactions 4.9: Redox Reactions 4.10: Balancing Redox Reactions |
Part 1: _____________ Balancing Redox Reactions .htm Selective Precipitaton & Separation of metal ions .htm, .pdf, .pptx Solubility of Ionic Compounds
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Strong- Weak- Non- Electrolytes Solution Stoichiometry |
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solute |
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5.1: Gas Pressure 5.2: The Empirical Gas Laws 5.3: Ideal Gases 5.4: Stoichiometry and Gases 5.5: Mixtures of Gases
5.6: The Kinetic Molecular Theory 5.7: Molecular Effusion and Diffusion 5.8: Non-ideal Gases 5.9: Properties of Some Non-ideal Gases 5.10: Chemistry in Earth's Atmosphere |
Gases I .htm Gases III .htm _____________ Boyle's Law - Sphagnum Moss .htm Mass of Magnesium (%Mg) Experiment + Molar Mass (Calculations) .htm, .pdf, .pptx |
Volume-Temperature (liquid nitrogen) Volume vs. Temperature (graph) Kinetic Energy (gases) Kinetic Energy - Temperature (gases) Distribution of Molecular Speeds (Interactive) Pressure-Volume-Temperature (collapsing coke can) Moles - Volume (gases) Effusion (gases) Sphagnum Moss Videos: Ideal Gas Law (Interactive) Gas Density (Interactive) |
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ideal gas |
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6.1: Energy 6.2: Enthalpy and Calorimetry 6.3: Hess's Law 6.4: Standard Enthalpies of Formation and Reaction 6.5: Current Sources of Energy 6.6: Potential Sources of Energy |
Thermochemistry .htm Thermochemistry .pdf Thermochemistry .pptx |
Thermite Reaction Activation Energy Specific Heat Capacity (Interactive) Calorimetry: Heat of Reaction (Interactive) Heat Transfer (Interactive) Hess's Law |
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energy heat work state function enthalpy (H) exothermic (exergonic) endothermic (endergonic) heat capacity calorimetry Hess's Law standard state greenhouse effect |
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7.1: Electromagnetic Radiation 7.2: Matter 7.3: Hydrogen Emission Spectrum 7.4: Bohr's Model of the Hydrogen Atom 7.5: Quantum Theory 7.6: Quantum Numbers 7.7: Shapes and Energies of Hydrogen Orbitals 7.8: The Pauli Exclusion Principle 7.9: Polyelectronic Atoms 7.10: Development of the Periodic Table 7.11: The Aufbau Principle 7.12: Periodic Trends 7.13: The Alkali Metals in Group 1 |
Quantum Chemistry .htm Periodicity .htm Periodic Table |
Electron Spin 1 Electron Configurations 1 Paramagnetism 1 Atomic Orbital Energies (Interactive) Periodic Trends: Electronegativity
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electromagnetic radiation
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8.1: Classification of Chemical Bonds 8.2: Electronegativity 8.3: Polarity 8.4: Electron Configurations of Ions 8.5: Lattice Energy 8.6: Percent Ionic Character of a Bond 8.7: Bonding in Covalent Molecules 8.8: Bond Energies and Enthalpies 8.9: The Localized Electron Model 8.10: Drawing Lewis Structures 8.11: Octet Rule Exceptions 8.12: Resonance Structures 8.13: VSEPR Theory |
Periodicity .htm Lewis Structures - VSEPR .htm Periodic Table |
Periodic Trends: Electronegativity Relative Sizes of Atoms & Ions (Interactive) Lewis Dot Structures Lewis Structures - Resonance (SO2) Drawing Lewis Structures 1 Drawing Lewis Structures 2 Resonance Structures Determining Molecular Shapes 1 Determining Molecular Shapes 2 Determining Molecular Polarity |
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Lewis Structure |
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10.1: Intermolecular Forces 10.2: Liquids 10.3: Types of Solids 10.4: Metallic Solids 10.5: Covalent-Network Solids 10.6: Molecular Solids 10.7: Ionic Solids 10.8: Vapor Pressure and Phase Changes 10.9: Phase Diagrams |
Intermolecular Forces / States of Matter Part 2: Intermolecular Forces 2.htm |
Vapor Pressure 1 Vapor Pressure 2 Changes of State Claussius - Clapyron Osmosis |
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intermolecular forces |
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11.1: Molality, Mass Percent, and Mole Fraction 11.2: Thermodynamics of Solubility 11.3: Effects of Structure, Temperature, and Pressure on Solubility 11.4: The Vapor Pressures of Solutions 11.5: Boiling-Point Elevation and Freezing-Point Depression 11.6: Osmotic Pressure 11.7: Colligative Properties of Electrolyte Solutions 11.8: Colloids |
Intermolecular Forces / States of Matter Part 2: Intermolecular Forces 2.htm |
Vapor Pressure 1 Vapor Pressure 2 Changes of State Claussius - Clapyron Osmosis |
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molality mass percent parts per million (ppm) parts per billion (ppb) heat of solution colligative properties osmosis Henry's Law Raoult's Law colloid |
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13.1: Introduction to Equilibrium 13.2: The Equilibrium Constant and Expression 13.3: Pressure Equilibrium Expressions 13.4: Heterogeneous Equilibria 13.5: Utilizing the Equilibrium Constant 13.6: Solving Equilibrium Expressions
13.7: Effect of Concentration, Temperature, and Pressure Changes on Equilibrium |
Chemical Equilibria .htm Chemical Equilibria .pdf Chemical Equilibria .pptx |
Le Chatelier's Principle NO2⇄ N2O4
The Equilibrium State The Equilibrium Constant Equilibrium Expressions .1 (Interactive) Equilibrium Expressions .2 (Interactive) Using an ICE Table |
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homogeneous equilibrium heterogeneous equilibrium Equilibrium expression Equilibrium constant reaction quotient Le Chatelier's Principle |
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Suggested Homework (Chem121) |
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14.1: Models for Acids and Bases 14.2: Effect of Molecular Structure on Acid Strength 14.3: pH and pOH 14.4: Strong Acids 14.5: Weak Acids 14.6: Bases 14.7: Diprotic and Polyprotic Acids 14.8: Acidic and Basic Salt Solutions 14.9: Relationship Between Structure and Acid-Base Properties 14.10: Acidic and Basic Oxides 14.11: Lewis Acids and Bases 14.12: Solving Acid-Base Problems |
Acids & Bases .htm Acids & Bases .pdf Acids & Bases .pptx |
Conjugate Acids-Bases Acid reacting with a Base Properties of Water Acid Ionization [H+][OH-] pH Estimation (Interactive) Ka x Kb = Kw Acid-Base Reactions Acid-Base Titrations (Interactive) pH of Salt Solutions |
Homework: Homework |
acid-base definitions conjugates strong-weak amphoteric dissociation constant autoionization percent dissociation salts acid-base character pH pOH pKw pKa pKb |
