Conceptual Chemistry– Curriculum Pacing Guide – 2012-2013

Content Areas / Unit 1 - Scientific Inquiry / Unit 2 - Atomic Structure and Nuclear Processes
Pacing / Daily - 19 days
A/B - 9 days / Daily - 24 days
A/B - 13 days / First Nine Weeks Exam
SC Standards/ Indicators / C-1.1Apply established rules for significant digits, both in reading a scientific instrument and in calculating a derived quantity from measurement.
C-1.2Use appropriate laboratory apparatuses, technology, and techniques safely and accurately when conducting a scientific investigation.
C-1.3Use scientific instruments to record measurement data in appropriate metric units that reflect the precision and accuracy of each particular instrument.
C-1.4Design a scientific investigation with appropriate methods of control to test a hypothesis (including independent and dependent variables), and evaluate the designs of sample investigations.
C-1.5Organize and interpret the data from a controlled scientific investigation by using mathematics (including formulas, scientific notation, and dimensional analysis), graphs, models, and/or technology.
C-1.6Evaluate the results of a scientific investigation in terms of whether they verify or refute the hypothesis and what the possible sources of error are.
C-1.7Evaluate a technological design or product on the basis of designated criteria.
C-1.8Use appropriate safety procedures when conducting investigations. / C-2.1Illustrate electron configurations by using orbital notation for representative elements.
C-2.2Summarize atomic properties (including electron configuration, ionization energy, electron affinity, atomic size, and ionic size).
C-2.3Summarize the periodic table’s property trends (including electron configuration, ionization energy, electron affinity, atomic size, ionic size, and reactivity).
C-2.4Compare the nuclear reactions of fission and fusion to chemical reactions (including the parts of the atom involved and the relative amounts of energy released).
C-2.5Compare alpha, beta, and gamma radiation in terms of mass, charge, penetrating power, and the release of these particles from the nucleus.
C-2.6Explain 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

Suggested Activities /
  • 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)
Chemistry IF8766 book, Instructional Fair, Inc.
  • 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
Chemistry IF8766 book, Instructional Fair, Inc.
  • 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
/ First Nine Weeks Exam
Suggested Activities /
  • 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

Textbook Correlation / Pearson-Prentice Hall Conceptual Chemistry, 3rd Edition
Index B (A4-A6) / Pearson-Prentice Hall Conceptual Chemistry, 3rd Edition
Chapters 2, 3,4, and 5
Content Areas / Unit 3 - Chemical Compounds / Unit 4 - Chemical Reactions
(Part 1)
Pacing / Daily-24 days
A/B-12 days / Daily-19 days
A/B- 10 days / Second Nine Weeks Exam
SC Standards/ Indicators / C-3.1Predict the type of bonding (ionic or covalent) and the shape of simple compounds by using Lewis dot structures and oxidation numbers.
C-3.2Interpret the names and formulas for ionic and covalent compounds.
C-3.3Explain how the types of intermolecular forces present in a compound affect the physical properties of compounds (including polarity and molecular shape).
C-3.4Explain the unique bonding characteristics of carbon that have resulted in the formation of a large variety of organic structures.
C-3.5Illustrate the structural formulas and names of simple hydrocarbons (including alkanes and their isomers and benzene rings). / C-4.1Analyze and balance equations for simple synthesis, decomposition, single replacement, double replacement, and combustion reactions.
C-4.2Predict the products of acid-base neutralization and combustion reactions.
C-4.4Apply 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.
C-4.5Predict 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

Suggested Activities /
  • Building Hydrocarbons with Models
  • Making Ionic Compounds (text, p. 279)
  • Molecular Models PowerPoint
Chemistry IF8766 book, Instructional Fair, Inc.
  • 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
Chemistry IF8766 book, Instructional Fair, Inc.
  • 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

Suggested Activities /
  • 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
/
  • 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
/ Second Nine Weeks Exam
Textbook Correlation / Pearson-Prentice Hall Conceptual Chemistry, 3rd Edition
Chapters 6 and 12 / Pearson-Prentice Hall Conceptual Chemistry, 3rd Edition
Chapters 7, 9, and 10
Content Areas / Unit 5 - Chemical Reactions
(Part 2) / Unit 6 - Phases of Matter
(Part 1)
Pacing / Daily - 24 days
A/B - 12 days / Daily - 19 days
A/B - 8 days / Third Nine Weeks Exam
SC Standards/ Indicators / C-4.3Analyze the energy changes (endothermic or exothermic) associated with chemical reactions.
C-4.6Explain the role of activation energy and the effects of temperature, particle size, stirring, concentration, and catalysts in reaction rates.
C-6.5Summarize the properties of salts, acids, and bases.
C-6.6Distinguish between strong and weak common acids and bases.
C-6.7Represent common acids and bases by their names and formulas. / C-5.4Illustrate 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 /
  • 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
/
  • Phase Changes
  • Phase Diagrams
  • Temperature/Time Graph
  • Evaporation vs. Boiling

Suggested Activities /
  • 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)
Chemistry IF8766 book, Instructional Fair, Inc.
  • 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
/
  • Graham’s Law (not on disk)
  • Demo of Balloon in a Bell Jar (not on disk)
  • Grahams Law Lab (not on disk)
Chemistry IF8766 book, Instructional Fair, Inc.
  • Graham’s Law of Effusion, p. 25
  • Heat and Its Measurement, p. 15
  • Vapor Pressure and Boiling, p. 16

Textbook Correlation / Pearson-Prentice Hall Conceptual Chemistry, 3rd Edition / Pearson-Prentice Hall Conceptual Chemistry, 3rd Edition
Chapters 7 and 17 / Third Nine Weeks Exam
Content Areas / Unit 7 - Phases of Matter
(Part 2) / Unit 8 - Chemical Solutions
Pacing / Daily - 9 days
A/B - 4 days / Daily - 34 days
A/B - 16 days / End of Course Exam
SC Standards/ Indicators / C-5.2Explain 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.
C-5.3Apply 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-6.1Summarize 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.
C-6.2Compare solubility of various substances in different solvents (including polar and nonpolar solvents and organic and inorganic substances).
C-6.3Illustrate the colligative properties of solutions (including freezing point depression and boiling point elevation and their practical uses).
C-6.4Carry 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

Suggested Activities /
  • Heating of Fusion of Ice
Chemistry IF8766 book, Instructional Fair, Inc.
  • 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
Chemistry IF8766 book, Instructional Fair, Inc.
  • 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

Textbook Correlation / Pearson-Prentice Hall Conceptual Chemistry, 3rd Edition / Pearson-Prentice Hall Conceptual Chemistry, 3rd Edition
Chapters 7, 10, 17, and 8

Anderson School District Five1July 1, 2012