Content Areas Unit 1 - Introduction to Chemistry Unit 2 - Measurement: Significant Digits, Scientific Notation Daily - 10 days A/B - 5 days Daily - 15 days A/B - 7 days C-1.2 C-1.4 C-1.6 C-1.7 C-1.8 Use appropriate laboratory apparatuses, technology, and techniques safely and accurately when conducting a scientific investigation. Design a scientific investigation with appropriate methods of control to test a hypothesis (including independent and dependent variables), and evaluate the designs of sample investigations. Evaluate the results of a scientific investigation in terms of whether they verify or refute the hypothesis and what the possible sources of error are. Evaluate a technological design or product on the basis of designated criteria. Use appropriate safety procedures when conducting investigations. C-1.1 C-1.3 C-1.5 Apply established rules for significant digits, both in reading a scientific instrument and in calculating a derived quantity from measurement. Use scientific instruments to record measurement data in appropriate metric units that reflect the precision and accuracy of each particular instrument. Organize and interpret the data from a controlled scientific investigation by using mathematics (including formulas, scientific notation, and dimensional analysis), graphs, models, and/or technology. Content Focus Lab Techniques Lab Safety Scientific Method Evaluate Scientific Investigations Technological Design Review of Properties and Classifications of Matter Significant Digits Scientific Notation Dimensional Analysis Precision/Accuracy Density Calculations Corn Starch Lab (text, p. 6) Bubble Lab (salt) (text, p. 23) Mystery Powder (text, p. 38) Paper Chromatography (text, p. 45) Chapters 1 and 2 Percent Composition M&M Lab (Graphing) Measurement Lab Sig Figures Lab (text, p. 72) Candy Bar Density Density Lab Unit Conversions Lab (text, p. 87) Chapter 3 Anderson School District Five 1 July 1, 2012
First Nine Weeks Exam Content Areas Unit 3 - Atomic Structure and Electron Configuration Unit 4 - Chemical Periodicity Daily - 15 days A/B - 7 days Daily - 5 days A/B - 3 days SC Standards/ Content Focus C-2.1 Illustrate electron configurations by using orbital notation for representative elements. Tested 1 st Nine Weeks Structure of the Atom Determining Valence Electrons Using Mass Number and Atomic Weight Tested 2 nd Nine Weeks Quantum Numbers Electron Configuration Exceptions to Normal Filling Order Explain Bright Line Spectrum Wintergreen Mints Lab (not on disk) Flame Tests (text, p. 142) Electron Configurations of Selected Elements C-2.2 Summarize atomic properties (including electron configuration, ionization energy, electron affinity, atomic size, and ionic size). C-2.3 Summarize the periodic table s property trends (including electron configuration, ionization energy, electron affinity, atomic size, ionic size, and reactivity). Electron Configurations Ionization Energy Electron Affinity Atomic Radius Ionic Radius Reactivity Electronegativity Metals/Nonmetals/Metalloids Structure of Periodic Table Getting to Know the Periodic Table (Periodic Table Coloring) Group 2: The Alkaline Earth Metals Chapter 4 and 6 Chapter 6 Anderson School District Five 2 July 1, 2012
Second Nine Weeks Exam Content Areas Unit 5 - Names and Formulas Ionic/Covalent Unit 6 - Carbon Chemistry Daily - 30 days A/B - 15 days Daily - 5 days A/B - 3 days C-3.1 C-3.2 C-3.3 C-5.1 Predict the type of bonding (ionic or covalent) and the shape of simple compounds by using Lewis dot structures and oxidation numbers. Interpret the names and formulas for ionic and covalent compounds. Explain how the types of intermolecular forces present in a compound affect the physical properties of compounds (including polarity and molecular shape). Explain the effects of the intermolecular forces on the different phases of matter. C-3.2 C-3.4 C-3.5 Interpret the names and formulas for ionic and covalent compounds. Explain the unique bonding characteristics of carbon that have resulted in the formation of a large variety of organic structures. Illustrate the structural formulas and names of simple hydrocarbons (including alkanes and their isomers and benzene rings). Content Focus Ionic and Covalent Bonding Hydrogen Bonding Covalent Bonds Shapes of Molecules Lewis Dot Structures Ionic Bonds Oxidation Numbers Polyatomic Ions Naming and Writing Formulas Polar, Nonpolar Degree of Ionic Character Bonding in Carbon Sp 3 Hybridization Single, Double, Triple Bonds Ring Structures Covalent Network IUPAC Naming Naming Alkanes Isomers Benzene Structural/Molecular Formulas Making Ionic Compounds (text, p. 279) Molecular Models PowerPoint Building Hydrocarbons with Models Chapters 7, 8, and 9 Chapters 22 and 23 Anderson School District Five 3 July 1, 2012
Third Nine Weeks Exam Content Areas Unit 7 - Moles/Chemical Quantities Unit 8 - Chemical Reactions Daily - 15 days A/B - 10 days (Begin teaching in 2 nd nine weeks; not tested until 3 rd nine weeks) C-4.4 Apply the concept of moles to determine the number of particles of a substance in a chemical reaction, the percent composition of a representative compound, the mass proportions, and the mole-mass relationships. Content Focus Mole Relationships Percent Composition Molar Mass Molar Volume for Gases Daily - 15 days A/B - 10 days C-4.1 Analyze and balance equations for simple synthesis, decomposition, single replacement, double replacement, and combustion reactions. C-4.2 Predict the products of acid-base neutralization and combustion reactions. (No Neutralization) Types of Reactions Symbols for equations Predicting Products Write and Balance Equations Activity Series Solubility Rules Mole Bean Lab Composition of Hydrates Lab Everyday Moles Mole Tray Demo (not on disk) Observing Chemical Reactions Types of Chemical Reactions Lab Chapter 10 Chapter 11 Anderson School District Five 4 July 1, 2012
Content Areas Unit 9 - Stoichiometry Unit 10 - Matter Daily - 20 days A/B - 10 days (Begin teaching in 3 rd nine weeks; not tested until end of year) C-4.5 Predict the percent yield, the mass of excess, and the limiting reagent in chemical reactions. C-5.4 Daily - 3 days A/B - 2 days Illustrate and interpret heating and cooling curves (including how boiling and melting points can be identified and how boiling points vary with changes in pressure). Content Focus Stoichiometric Calculations Mass-Mass Limiting Reactants Percent Yield Phase Changes Phase Diagrams Temperature/Time Graph Evaporation vs. Boiling Reaction Lab 2 (not on disk) How Much Carbon Dioxide is Given Off in Alka-Seltzer Lab Heat of Fusion of Ice (text, p. 522) Chapter 12 Chapter 13 Anderson School District Five 5 July 1, 2012
Content Areas Unit 11 - Gases and Gas Laws Unit 12 - Nuclear Daily - 7 days A/B - 4 days Daily - 3 days A/B - 2 days C-5.2 C-5.3 Explain the behaviors of gas; the relationship among pressure, volume, and temperature; and the significance of the Kelvin (absolute temperature) scale, using the kineticmolecular theory as a model. Apply the gas laws to problems concerning changes in pressure, volume, or temperature (including Charles s law, Boyle s law, and the combined gas law). C-2.4 C-2.5 C-2.6 Compare the nuclear reactions of fission and fusion to chemical reactions (including the parts of the atom involved and the relative amounts of energy released). Compare alpha, beta, and gamma radiation in terms of mass, charge, penetrating power, and the release of these particles from the nucleus. Explain the concept of half-life, its use in determining the age of materials, and its significance to nuclear waste disposal. Content Focus Kinetic and Molecular Theory Temperature and Average Kinetic Energy Charles and Boyle s Laws Balloon in a Bell Jar (not on disk) Grahams Law Lab (not on disk) Half-Life Alpha, Beta, and Gamma Waves Writing Nuclear Reactions Fission/Fusion Chemical Reactions Half-Life, (text, p. 809) Chapter 14 Chapter 25 Anderson School District Five 6 July 1, 2012
Content Areas Unit 13 - Solutions Unit 14 - Reaction Rates Daily - 7 days A/B - 4 days Daily - 5 days A/B - 3 days C-6.1 C-6.2 C-6.3 C-6.4 Summarize the process by which solutes dissolve in solvents, the dynamic equilibrium that occurs in saturated solutions, and the effects of varying pressure and temperature on solubility. Compare solubility of various substances in different solvents (including polar and nonpolar solvents and organic and inorganic substances). Illustrate the colligative properties of solutions (including freezing point depression and boiling point elevation and their practical uses). Carry out calculations to find the concentration of solutions in terms of molarity and percent weight (mass). C-4.3 C-4.6 Analyze the energy changes (endothermic or exothermic) associated with chemical reactions. Explain the role of activation energy and the effects of temperature, particle size, stirring, concentration, and catalysts in reaction rates. Content Focus Solubility of Various Substances Colligative Properties Molarity and Percent Weight Solutions, Suspensions, and Colloids LeChatelier s Principle Saturated, Unsaturated, and Supersaturated Solutions Like Dissolves Like Endothermic/Exothermic Reactions Enthalpy Entropy Activation Energy Diagram Solubility Lab Polar and Non-polar Alka-Seltzer Demo (not on disk) Mentos and Diet Coke Demo (not on disk) Chapter 16 Chapter 18 (section 18.4) Chapter 1 Anderson School District Five 7 July 1, 2012
End of Course Exam Content Areas C-4.2 C-6.5 C-6.6 C-6.7 Unit 15 - Acids and Bases Daily - 6 days A/B - 3 days Predict the products of acid-base neutralization and combustion reactions. (Only neutralization) Summarize the properties of salts, acids, and bases. Distinguish between strong and weak common acids and bases. Represent common acids and bases by their names and formulas. Content Focus Properties of Acids, Bases, and Salts Differentiate Strong/Weak vs. Concentrated/Dilute Recognize Ionization Reactions Define/Contrast Acids and Bases Conjugate Acid/Base Pairs Recognize Common Acid and Base Formulas Acids and Bases Activity Red Cabbage Scale Chapter 19 Anderson School District Five 8 July 1, 2012