A Correlation of. To the Alabama Course of Study Science Chemistry
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1 A Correlation of To the Science Chemistry
2 Table of Contents Matter and Its Interactions... 3 Motion and Stability: Forces and Interactions... 6 Energy
3 CHEMISTRY Matter and Its Interactions 1. Obtain and communicate information from historical experiments (e.g., work by Mendeleev and Moseley, Rutherford s gold foil experiment, Thomson s cathode ray experiment, Millikan s oil drop experiment, Bohr s interpretation of bright line spectra) to determine the structure and function of an atom and to analyze the patterns represented in the periodic table. 2. Develop and use models of atomic nuclei to explain why the abundance-weighted average of isotopes of an element yields the published atomic mass. 3. Use the periodic table as a systematic representation to predict properties of elements based on their valence electron arrangement. a. Analyze data such as physical properties to explain periodic trends of the elements, including metal/nonmetal/metalloid behavior, electrical/heat conductivity, electronegativity and electron affinity, ionization energy, and atomic-covalent/ionic radii and how they relate to position in the periodic table. b. Develop and use models (e.g., Lewis dot, 3-D ball-and-stick, space-filling, valence-shell electron-pair repulsion [VSEPR]) to predict the type of bonding and shape of simple compounds. SE/TE: 102, , 109 (Lesson Check: #10, 12, 13, 14, 15), 122 (Assessment: #39, 43, 44, 46), , 133, , , , , 166 (Lesson Check: #2) TE: 133 (Chemistry & You), 147 (Explore) SE/TE: , 119 (Lesson Check: #28, 32), 120 (Lab), 123 (Assessment: #64) SE/TE: 162, , 173 (Lesson Check: #15, 16), 186 (Assessment: #36, 37) SE/TE: 162, , 166 (Lesson Check: #5, 6, 7), 167, 173 (Lesson Check: #14), , 180 (Quick Lab), , 182 (Lesson Check: #18, 20, 22, 24, 25), 184 (Small-Scale Lab), 186 (Assessment: #28-32, 38-45) TE: 163 (Chemistry & You) SE/TE: 195, 201, 205, , (Assessment: #73, 87), , , , 235, 238 (Lesson Check: #20), , 246 (Lesson Check: #24, 26), (Assessment: #49, 51, 52, 53, 60, 72, 73, 74) TE: 242 (Explore), 243 (Explain) 3
4 c. Use the periodic table as a model to derive formulas and names of ionic and covalent compounds. SE/TE: , 267, , 269 (Lesson Check: #6, 7), , , 278 (Lesson Check: #21, 23, 25, 26), , 283 (Lesson Check: #31, 32), , 294 (Lesson Check: #53, 54, 55), 295 (Lab), (Assessment: #66, 72, 80-85) TE: 274 (Explore), 275 (Explore) 4. Plan and conduct an investigation to classify properties of matter as intensive (e.g., density, viscosity, specific heat, melting point, boiling point) or extensive (e.g., mass, volume, heat) and demonstrate how intensive properties can be used to identify a compound. 5. Plan and conduct investigations to demonstrate different types of simple chemical reactions based on valence electron arrangements of the reactants and determine the quantity of products and reactants. a. Use mathematics and computational thinking to represent the ratio of reactants and products in terms of masses, molecules and moles. SE/TE: 34-35, 92 (Small-Scale Lab) TE: 35 (Explore), 77 (Explore), 81 (Explore), 428 (Explore) Lab 4: Mass, Volume and Density; Lab Practical 3-2: Density SE/TE: 324 (Small-Scale Lab), 374 (Small- Scale Lab), 399 (Lab) TE: 313 (Explore), 314 (Explore), 350 (Explore), 360 (Explore), 362 (Explore), 365 (Explore), 366 (Explore), 392 (Explore), 396 (Explore) SE/TE: , , , 315 (Lesson Check: #12, 13, 14, 15), , 323 (Lesson Check: #26, 27), 338 (Assessment: #52, 54, 60-65), , , 389 (Lesson Check: #9, 10), , 398 (Lesson Check: #23, 24), , 404 (Quick Lab), , 408 (Lesson Check: #37, 38), (Assessment: #44, 45, 46, 47, 49, 50, 56, 57) TE: 309 (Sample Practice Problem), 311 (Explain; Sample Practice Problem), 312 (Explain), 315 (Sample Practice Problem; Evaluate), 319 (Sample Practice Problem), 361 (Sample Practice Problem), 363 (Sample Practice Problem), 365 (Sample Practice Problem), 387 (Explore), 391 (Sample Practice Problem), 392 (Explore), 397 (Chemistry & You), 405 (Class Activity) 4
5 b. Use mathematics and computational thinking to support the claim that atoms, and therefore mass, are conserved during a chemical reaction. 6. Use mathematics and computational thinking to express the concentrations of solutions quantitatively using molarity. SE/TE: , 354 (Quick Lab), 355 (Chemistry & You), 367 (Lesson Check: #23), 377 (Assessment: #37-42), , 389 (Lesson Check: #8, 9, 10) TE: 388 (Explain) SE/TE: , , 531 (Lesson Check: #19, 22, 23, 24), 545 (Small-Scale Lab), 548 (Assessment: #57, 58, 59, 60), 551 (Assessment: #100) TE: 527 (Explore), 528 (Explore), 530 (Explore) a. Develop and use models to explain how solutes are dissolved in solvents. b. Analyze and interpret data to explain effects of temperature on the solubility of solid, liquid, and gaseous solutes in a solvent and the effects of pressure on the solubility of gaseous solutes. c. Design and conduct experiments to test the conductivity of common ionic and covalent substances in a solution. SE/TE: , 501 (Lesson Check: #17), 510 (Assessment: #37, 38), , 523 (Figure 16.6), 548 (Assessment: #54, 55), (Assessment: #96, 99) SE/TE: 519, 521 TE: 521 (Explain; Extend), 522 (Explore) SE/TE: , 501 (Lesson Check: #11), 508 (Small-Scale Lab), (Assessment: #44, 45, 46, 80) TE: 497 (Explore) Lab 29: Electrolytes and Nonelectrolytes; Lab Practical 15-1: Electrolytes and Nonelectrolytes 7. Use the concept of ph as a model to predict the relative properties of strong, weak, concentrated, and dilute acids and bases (e.g., Arrhenius and Brønsted-Lowry acids and bases). SE/TE: , 651 (Table 19.4), 652 (Lesson Check: #3, 4, 6), , , 662 (Quick Lab), 663 (Chemistry & You) TE: 649 (Check for Understanding), 657 (Sample Practice Problem), 658 (Sample Practice Problem; Explore), 659 (Explore; Sample Practice Problem), 660 (Explore), 662 (Explore) 5
6 8. Plan and carry out investigations to explain the behavior of ideal gases in terms of pressure, volume, temperature, and number of particles. SE/TE: 467 (Quick Lab) TE: 452 (Explore), 460 (Explore), 465 (Explain) Lab 23: Pressure-Volume Relationships for Gases; Lab 24: Temperature-Volume Relationships for Gases; Lab Practical 14-1: Boyle s Law; Lab Practical 14-2: Charles Law a. Use mathematics to describe the relationships among pressure, temperature, and volume of an enclosed gas when only the amount of gas is constant. b. Determine molar quantities using the ideal gas law. SE/TE: , , 463 (Lesson Check: #22), , (Assessment: #54-58, 60, 61, 65-69, 83, 96) TE: 457 (Sample Practice Problem), 458 (Extend), 459 (Sample Practice Problem), 460 (Explore), 461 (Sample Practice Problem), 462 (Sample Practice Problem) SE/TE: , 467 (Quick Lab), 468 (Lesson Check: #30) TE: 466 (Sample Practice Problem) 9. Refine the design of a given chemical system to illustrate how LeChâtelier s principle affects a dynamic chemical equilibrium when subjected to an outside stress (e.g., heating and cooling a saturated sugar-water solution).* SE/TE: TE: 612 (Explore), 613 (Explain), 614 (Sample Practice Problem), 615 (Explore) Lab38: Disturbing Equilibrium; Small Scale Lab Manual Lab 29: LeChâtelier s Principle and Chemical Equilibrium Motion and Stability: Forces and Interactions 10. Analyze and interpret data (e.g., SE/TE: , , 439 (Lesson melting point, boiling point, solubility, Check: #26, 28, 29), phase-change diagrams) to compare the (Assessment: #48, 59, 61), 521 (Figure strength of intermolecular forces and how 16.5) these forces affect physical properties and changes. TE: 252 (Explore) 6
7 Energy 11. Plan and conduct experiments that demonstrate how changes in a system (e.g., phase changes, pressure of a gas) validate the kinetic molecular theory. SE/TE: 420, 424 (Lesson Check: #3, 4), , 436, 437 (Quick Lab), TE: 421 (Explore), 422 (Explore), 423 (Explore), 427 (Explore), 429 (Explore) Lab 22: Changes of Physical State; Lab Practical 13-1: Changes of Physical State a. Develop a model to explain the relationship between the average kinetic energy of the particles in a substance and the temperature of the substance (e.g., no kinetic energy equaling absolute zero [0K or oC]). 12. Construct an explanation that describes how the release or absorption of energy from a system depends upon changes in the components of the system. a. Develop a model to illustrate how the changes in total bond energy determine whether a chemical reaction is endothermic or exothermic. b. Plan and conduct an investigation that demonstrates the transfer of thermal energy in a closed system (e.g., using heat capacities of two components of differing temperatures). SE/TE: , 424 (Lesson Check: #5), , 430 (Lesson Check: #10, 11, 13, 15, 16) TE: 423 (Explore) SE/TE: , 561 (Lesson Check: #8), TE: 557 (Explore) SE/TE: , 568 (Lesson Check: #18-21), TE: 570 (Explore), 572 (Explore), 574 (Explore) SE/TE: 559, , 571 (Quick Lab), 583 (Small-Scale Lab) TE: 559 (Explore), 563 (Explore) Lab 35: Heats of Reactions 7
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