Basic Chemistry 2014 Timberlake

Transcription

1 A Correlation of 2014 Timberlake

2 A Correlation of, INTRODUCTION This document demonstrates how, Timberlake 2014 meets the, grades Correlation page references are to the Student Edition. Maintaining the clear and approachable writing style characteristic of author Karen Timberlake, adds to its suite of problem-solving tools and techniques necessary for educational and workforce success. Engaging new features such as Key Math Skills and Core Chemistry Skills, and Math Review Modules allow students of various levels and learning styles to practice and master quantitative skills. Popular features, including Combining Ideas sections and end-ofchapter questions, have also been strengthened and expanded. Modern real-world applications help students connect chemical principles to events in their world, while stories involving careers illustrate the importance of chemistry in future careers. This new edition also expands the resources available in MasteringChemistry, the most widely used and effective online homework, tutorial, and assessment system for the sciences. The Pearson Advantage Unique Guide to Problem-Solving strategy provides a visual, step-by-step plan that helps to solve a wide variety of problems. New! Key Math Skill feature indicates when a math skill relevant to chemistry is introduced. New! Core Chemistry Skill shows students when important chemistry skills (that will be used throughout the course) are introduced. New! Chapter Readiness indicates what Key Math Skills and Core Chemistry Skills previously introduced will be needed in a specific chapter. Concept Checks throughout each chapter allow students to check their understanding of new chemical terms and ideas. Learning Goals at the beginning of each chapter section clearly identify the key concept of the section, providing a road map for studying. Analyze the Problem features included in most of the Sample Problems strengthen critical-thinking skills by showing students how to break down a word problem in components required to solve it. SE=Student Edition 2

3 A Correlation of, ALABAMA COURSE OF STUDY SCIENCE CHEMISTRY CORE HIGH SCHOOL Students will: 1. Differentiate among pure substances, mixtures, elements, and compounds. Distinguishing between intensive and extensive properties of matter Contrasting properties of metals, nonmetals, and metalloids Distinguishing between homogeneous and heterogeneous forms of matter 2. Describe the structure of carbon chains, branched chains, and rings. 3. Use the periodic table to identify periodic trends, including atomic radii, ionization energy, electronegativity, and energy levels. Utilizing electron configurations, Lewis dot structures, and orbital notations to write chemical formulas Calculating the number of protons, neutrons, and electrons in an isotope Utilizing benchmark discoveries to describe the historical development of atomic structure, including photoelectric effect, absorption, and emission spectra of elements Example: Thompson's cathode ray, Rutherford's gold foil, Millikan's oil drop, and Bohr's bright line spectra experiments SE: 70-72, 72-73, 74 (# ), 98 (#3.51), 99 (# ), 105, 169, 193 Opportunity to address this standard can be found on the following pages: SE: 54, 75, 76, 76 (Table 3.2), 77 (Table 3.5), SE: , 112 (Table 4.3), 114 (# ) SE: 72-73, 74 (# ), 99 (# ) Opportunity to address this standard can be found on the following pages: SE: , 197, , 264, 266, 597, 605 SE: , , 114 (# ), , , , , , 158, 160 (# , ), 161 (# ), 165 (# ), , 343 (# ) Opportunity to address this standard can be found on the following pages: SE: 145, , , SE: , 125 (# ), 130 (# , 4.77), 131 (#4.80) SE: , SE=Student Edition 3

4 A Correlation of, 4. Describe solubility in terms of energy changes associated with the solution process. Using solubility curves to interpret saturation levels Explaining the conductivity of electrolytic solutions Describing acids and bases in terms of strength, concentration, ph, and neutralization reactions Describing factors that affect the rate of solution Solving problems involving molarity, including solution preparation and dilution 5. Use the kinetic theory to explain states of matter, phase changes, solubility, and chemical reactions. Example: water at 25 degrees Celsius remains in the liquid state because of the strong attraction between water molecules while kinetic energy allows the sliding of molecules past one another 6. Solve stoichiometric problems involving relationships among the number of particles, moles, and masses of reactants and products in a chemical reaction. Predicting ionic and covalent bond types and products given known reactants Assigning oxidation numbers for individual atoms of monatomic and polyatomic ions SE: 297 (Chemistry Link), 393, 396 SE: SE: 396, SE: , 486 (# ), , 491 (#14.33, ), , 498 (# ), , 515 (# ) SE: SE: , 411 (# ), , 417 (# ), 433 (# ), 434 (# , ) SE: 70, 76 (Figure 3.4), 251, 326, 329, SE: , 212, 212 (# ), 213 (# ), , 215 (# ), , 219 (# ), 233 (# , 7.61), , 284 (# ), , 287 (# ), , 291 (# ), 292 (# ), 302 (# ), 303 (# ) SE: , 181, 182 (# ), 187 (# , ), 191, 193 ( ), 194, 204 (# ), 247, 252, 253 (# ) SE: , , 553 (# ) SE=Student Edition 4

5 A Correlation of, Identifying the nomenclature of ionic compounds, binary compounds, and acids Classifying chemical reactions as composition, decomposition, single replacement, or double replacement Determining the empirical or molecular formula for a compound using percent composition data 7. Explain the behavior of ideal gases in terms of pressure, volume, temperature, and number of particles using Charles's law, Boyle's law, Gay-Lussac's law, the combined gas law, and the ideal gas law. 8. Distinguish among endothermic and exothermic physical and chemical changes. Examples: - endothermic physical phase change from ice to water, - endothermic chemical reaction between citric acid solution and baking soda, - exothermic physical phase change from water vapor to water, - exothermic chemical formation of water from combustion of hydrogen and oxygen Calculating temperature change by using specific heat Using Le Châtelier s principle to explain changes in physical and chemical equilibrium 9. Distinguish between chemical and nuclear reactions. SE: , 181 (# ), 182 (# ), 183, , 186 (# , ), , , 193 (# , ), 203 (# ), , 478 (# ), 515 (# ) SE: , 253 (# ), 276 (# ) SE: , 226 (# ), , 229 (# ), 233 (# ), 234 (# ) SE: , 361 (# ), 362 (# ), , 365 (# ), , 368 (# ), , 371 (# ), , 374 (# ), , 378 (# ), , 379 (# ), 388 (# ), 389 (# ) SE: 76 (Figure 3.4), 251, 295, 297 (Chemistry Link), 297 (# ) SE: 85-89, 91 (# ) SE: , 460 (# ) SE: , , 588 (# ) SE=Student Edition 5

6 A Correlation of, Identifying atomic and subatomic particles, including mesons, quarks, tachyons, and baryons Calculating the half-life of selective radioactive isotopes Identifying types of radiation and their properties SE: , 561, 563 (# ) SE: , 578, 578 (# ), 589 (#16-68) SE: , 573, 577, 581 Contrasting fission and fusion SE: , 584 (# ), 589 (#16.69, ) Describing carbon-14 decay as a dating method SE: 577 (Chemistry Link) SE=Student Edition 6