End of First Nine Weeks Content Areas Unit 1 - Scientific Inquiry Unit 2 - Atomic Structure and Nuclear Processes Daily - 19 days A/B - 9 days Daily - 24 days A/B - 13 days SC Standards/ C-1.1 C-1.2 C-1.3 C-1.4 C-1.5 C-1.6 C-1.7 C-1.8 Apply established rules for significant digits, both in reading a scientific instrument and in calculating a derived quantity from measurement. Use appropriate laboratory apparatuses, technology, and techniques safely and accurately when conducting a scientific investigation. Use scientific instruments to record measurement data in appropriate metric units that reflect the precision and accuracy of each particular instrument. 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. 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. 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-2.1 C-2.2 C-2.3 C-2.4 C-2.5 C-2.6 Illustrate electron configurations by using orbital notation for representative elements. Summarize atomic properties (including electron configuration, ionization energy, electron affinity, atomic size, and ionic size). Summarize the periodic table s property trends (including electron configuration, ionization energy, electron affinity, atomic size, ionic size, and reactivity). 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 Science of Matter Laboratory Safety Significant Digits Safety Guidelines Scientific Investigation Electron Configuration Atomic Properties Periodic Table s Properties and Trends Nuclear Reactions of Fusion and Fission Alpha, Beta, and Gamma Radiation Half-Life Anderson School District Five 1 July 1, 2013
End of First Nine Weeks Content Areas Unit 1 - Scientific Inquiry Unit 2 - Atomic Structure and Nuclear Processes Metric Madness Lab Corn Starch Lab (text, p. 6) Bubble Lab (salt) (text p. 23) Mystery Powder (text, p. 38) Paper Chromatography (text, p. 45) Percent Composition M&M Lab (Graphing) Measurement Lab Significant Figures Lab (text, p. 72) Candy Bar Density Density Lab Unit Conversions Lab (text, p. 87) Laboratory Dos and Don ts, p. 1 Laboratory Equipment, p. 2 The Triple and Four Beam Balances, p. 3 Measuring Liquid Volume, p. 4 Reading Thermometers, p.5 Dimensional Analysis (Factor Label Method), p. 6 Half-Life Lab, (text, p. 122) Wintergreen Mints Lab (not on disk) Flame Tests, (text, p. 142) Getting to Know the Periodic Table (Periodic Table Coloring) Group 2: The Alkaline Earth Metals Element Symbols, p. 26 Atomic Structure, p. 27 Isotopes and Average Atomic Mass, p.28 Electron Configuration (Level One), p. 29 Electron Configuration (Level Two), p. 30 Valence Electrons, p. 31 Lewis Dot Diagrams, p. 32 Atomic Structure Crossword, p. 33 Nuclear Decay, p. 34 Half-Life of Radioactive Isotopes, p. 35 Periodic Table Worksheet, p. 36 Periodic Table Puzzle, p. 37 Metrics and Measurements, p. 7 Scientific Notation, p. 8 Calculations Using Significant Figures, p. 10 Percentage Error, p. 11 Temperature and Its Measurement, p. 12 Freezing and Boiling Point Graph, p. 13 Phase Diagram, p. 14 Index B (A4-A6) Chapters 2, 3,4, and 5 Anderson School District Five 2 July 1, 2013
Midterm Exam Content Areas Unit 3 - Chemical Compounds Unit 4 - Chemical Reactions (Part 1) SC Standards/ C-3.1 C-3.2 C-3.3 C-3.4 C-3.5 Daily-24 days A/B-12 days 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 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). C-4.1 C-4.2 C-4.4 C-4.5 Daily-19 days A/B- 10 days Analyze and balance equations for simple synthesis, decomposition, single replacement, double replacement, and combustion reactions. Predict the products of acid-base neutralization and combustion reactions. 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. Predict the percent yield, the mass of excess, and the limiting reagent in chemical reactions. Content Focus Ionic and Covalent Bonding Names and Formulas of Ionic and Covalent Compounds Intermolecular Forces in Compounds Bonding Characteristics of Carbon Hydrocarbons Mole Relationships Percent Composition Molar Mass Types of Reactions Symbols for Equations Predicting Products Write and Balance Equations Stoichiometric Calculations Limiting Reactants Building Hydrocarbons with Models Making Ionic Compounds (text, p. 279) Molecular Models PowerPoint Ionic Bonding, p. 38 Covalent Bonding, p. 39 Types of Chemical Bonds, p. 40 Shapes of Molecules, p. 41 Polarity of Molecules, p.42 Observing Chemical Reactions Types of Chemical Reactions Lab Moles and Mass, p. 50 The Mole and Volume, p. 51 The Mole and Avogadro s Number, p. 52 Mixed Mole Problems, p. 53 Percentage Composition, p. 54 Determining Emperical Formulas, p. 55 Anderson School District Five 3 July 1, 2013
Midterm Exam Content Areas Unit 3 - Chemical Compounds Chemical Bonding Crossword, p. 43 Writing Formulas (Criss-Cross Method), p. 44 Naming Ionic Compounds, p. 45 Naming Molecular Compounds, p. 46 Naming Hydrocarbons,p. 96 Structure of Hydrocarbons, p. 97 Functional Groups, p. 98 Naming Other Organic Compounds, p. 99 Structures of Other Organic Compounds, p. 100 Organic Chemistry Crossword, p. 101 Unit 4 - Chemical Reactions (Part 1) Stoichiometry: Mole-Mole Problems, p. 62 Stoichiometry: Volume-Volume Problems, p. 63 Stoichiometry: Mass-Mass Problems, p. 54 Stoichiometry: Mixed Problems, p. 65 Stoichiometry: Limiting Reagent, p. 66 Writing Formulas from Names, p. 48 Balancing Chemical Equations, p. 58 Word Equations, p. 59 Classification of Chemical Reactions, p. 60 Predicting Products of Chemical Reactions, p. 61 Chapters 6 and 12 Chapters 7, 9, and 10 Anderson School District Five 4 July 1, 2013
End of Third Nine Weeks Content Areas Unit 5 - Chemical Reactions (Part 2) Unit 6 - Phases of Matter (Part 1) Daily - 24 days A/B - 12 days SC Standards/ C-4.3 Analyze the energy changes (endothermic or exothermic) associated with chemical reactions. C-4.6 Explain the role of activation energy and the effects of temperature, particle size, stirring, concentration, and catalysts in reaction rates. C-6.5 Summarize the properties of salts, acids, and bases. C-6.6 Distinguish between strong and weak common acids and bases. C-6.7 Represent common acids and bases by their names and formulas. Content Focus Endothermic/Exothermic Reactions Enthalpy Entropy Properties of Acids, Bases, and Salts Recognize Ionization Reactions Define Contrast Acids and Bases Recognize Common Acid and Base Formulas Acid-Base Titration Lab Mole Bean Lab Composition of Hydrates Lab Everyday Moles Mole Tray Demo (not on disk) Reaction Lab 2 (not on disk) How Much Carbon Dioxide is Given Off in Alka-Seltzer Lab Alka Seltzer Demo (not on disk) Mentos and Diet Coke Demo (not on disk) C-5.4 Daily - 19 days A/B - 8 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). Phase Changes Phase Diagrams Temperature/Time Graph Evaporation vs. Boiling Graham s Law (not on disk) Demo of Balloon in a Bell Jar (not on disk) Grahams Law Lab (not on disk) Graham s Law of Effusion, p. 25 Heat and Its Measurement, p. 15 Vapor Pressure and Boiling, p. 16 Naming Acids, p. 47 Acid-Base Titration, p. 88 Acids and Bases Crossword, p. 90 ph and poh, pp. 86-87 Bronsted-Lowry Acids and Bases, p. 84 Chapters 7 and 17 Anderson School District Five 5 July 1, 2013
End of Course Exam Content Areas Unit 7 - Phases of Matter (Part 2) Unit 8 - Chemical Solutions Daily - 9 days A/B - 4 days Daily - 34 days A/B - 16 days SC Standards/ 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 kinetic-molecular 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-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). Content Focus Kinetic and Molecular Theory Temperature and Average Kinetic Energy Charles and Boyle s Laws Solubility Solutes/Solvents Polar and Non-polar Solvents Colligative Properties of Solutions Heating of Fusion of Ice Boyle s Law, p. 20 Charles Law, p. 21 Combined Gas Law, p. 22 Dalton s Law of Partial Pressures, p. 23 Ideal Gas Law, p. 24 Solubility Lab Polar and Nonpolar Solubility Curves, p. 67 Molarity (M), p. 68 Molarity by Dillution, p. 69 Molality (m), p. 70 Normality (N), p. 71 Electrolytes, p. 72 Effect of a Solute on Freezing and Boiling Points, p. 73 Solubility (Polar vs. Nonpolar), p. 74 Solutions Crosswordp. 75 Chapters 7, 10, 17, and 8 Anderson School District Five 6 July 1, 2013