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Prentice Hall Chemistry - Indiana Edition © 2012
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Indiana’s Revised Academic Standards for Chemistry I / 3064 (High School)
Chemistry - Indiana Edition © 2012 Correlated to: Indiana’s Revised Academic Standards for Chemistry I / 3064 (High School)
INDIANA ACADEMIC STANDARDS
SE Lessons (chapter & lesson numbers)
SE, TE, TR, TECH (page numbers)
Chemistry I Students should understand that scientific knowledge is gained from observation of natural phenomena and experimentation, by designing and conducting investigations guided by theory, and by evaluating and communicating the results of those investigations according to accepted procedures. Thus, scientific knowledge is scientists' best explanations for the data from many investigations. Further, ideas about objects in the microscopic world that we cannot directly sense are often understood in terms of concepts developed to understand objects in the macroscopic world that we can see and touch. In the science classroom student work should align with this process of science and should be guided by the following principles. These should be woven throughout the daily work that students are doing when learning the content presented in the standard indicators. SE: Representative Pages: 120, 142, 200, * Develop explanations based on SE: 1.3, 2.2, 3.1, 4.2, 5.3, 6.3, 7.1, 7.2, 208, 238, 328, 355, 583, 699, 744, 849 (All reproducible data and observations gathered 8.2, 9.2, 10.3, 11.1, 12.3, 13.4, 14.3, 15.1, Quick Labs and Small-Scale Labs) during laboratory investigations. 16.1, 17.3, 18.1, 19.2, 20.1, 21.3, 22.3, TR: Lab Manual: Representative Pages: 25, 23.3, 24.5, 25.4 45, 67, 101, 155, 167, 203, 255, 271, 305 * Recognize that their explanations must be based both on their data and other known information from investigations of others.
SE: 3.1, 4.2, Ch 16
SE: 72, 109, 545 (Can Also Be Developed From all Quick Labs and Small-Scale Labs) TR: Lab Manual: 126, 216, 265 (Can Also Be Developed From Any Lab Activity)
* Clearly communicate their ideas and results of investigations verbally and in written form using tables, graphs, diagrams, and photographs.
SE: Ch 4, 6.3, Ch 7, Ch 9, 10.3, Ch 13, Ch 15, Ch 18, Ch 19
SE: Representative Pages: 120, 180, 200, 295, 328, 435, 508, 635, 641(108), 681 TR: Lab Manual: Representative Pages: 7071, 81-83, 94-96, 106-107, 129-132, 142145, 150-153, 158-161, 206-209, 220-223
* Regularly evaluate the work of their peers and in turn have their work evaluated by their peers.
SE: 3.1, 4.2
SE: 72, 109 TR: Lab Manual: 126, 216
* Apply standard techniques in laboratory investigations to measure physical quantities in appropriate units and convert known quantities to other units as necessary.
SE: 3.1, Ch 5, Ch 6, Ch 10, 10.3, 12.1, 12.2, 12.3
SE: 72, 149, 184, 324, 328, 545, 571, 583 TR: Lab Manual: 56, 81, 83, 88, 124-125, 150-151, 182, 215, 221
SE = Student Edition
TE = Teacher’s Edition
TR = Teaching Resources 1
TECH = Technology
Chemistry - Indiana Edition © 2012 Correlated to: Indiana’s Revised Academic Standards for Chemistry I / 3064 (High School)
INDIANA ACADEMIC STANDARDS
SE Lessons (chapter & lesson numbers)
SE, TE, TR, TECH (page numbers)
* Use analogies and models (mathematical and physical) to simplify and represent systems that are difficult to understand or directly experience due to their size, time scale, or complexity, and recognize the limitations of analogies and models.
SE: Ch 6, Ch 7, Ch 10, 13.3, 22.3, Ch 22, 24.5
SE: 184 (Small-Scale Lab), 200(Small-Scale Lab), 316 (Chemistry & You), 324 (SmallScale Lab), 431-434, 778 (Quick Lab), 787(Small-Scale Lab), 856 (Quick Lab) TR: Lab Manual: Representative Pages: 60, 130-131, 143, 153, 159-160, 207, 236, 294, 302, 308
* Focus on the development of explanatory models based on their observations during laboratory investigations.
SE: Ch 6, 10.1
SE: 184(Small-Scale Lab), 316 TR: Lab Manual: Representative Pages: 60, 130-131, 143, 153, 159-160, 207, 222, 230, 302, 308; Small-Scale Chemistry Lab Manual: 63-68, 213-218
* Explain that the body of scientific knowledge is organized into major theories, which are derived from and supported by the results of many experiments, and allow us to make testable predictions. * Recognize that new scientific discoveries often lead to a re-evaluation of previously accepted scientific knowledge and of commonly held ideas. * Describe how scientific discoveries lead to the development of new technologies, and conversely how technological advances can lead to scientific discoveries through new experimental methods and equipment. * Explain how scientific knowledge can be used to guide decisions on environmental and social issues.
SE: 1.1, 1.3
SE: 3, 4-5, 17 TR: Guided Reading and Study Workbook: 1, 6-7
SE: 1.3, 5.1
SE: 17, 133 TR: Guided Reading and Study Workbook: 7-8
SE: 1.2
SE: 8-11
SE: 1.2, Ch 2, Ch 13, Ch 14
SE: Can Be Developed From: 8-11, 52, 440, 476 TR: Guided Reading and Study Workbook: 3-5
SE = Student Edition
TE = Teacher’s Edition
TR = Teaching Resources 2
TECH = Technology
Chemistry - Indiana Edition © 2012 Correlated to: Indiana’s Revised Academic Standards for Chemistry I / 3064 (High School)
INDIANA ACADEMIC STANDARDS
SE Lessons (chapter & lesson numbers)
SE, TE, TR, TECH (page numbers)
Standard 1: Properties and States of Matter Core Standard - Describe the nature of physical and chemical properties and changes of matter. Core Standard - Compare and contrast states of matter at the molecular level. C.1.1 Based on physical properties, SE: 2.1, 2.2, 2.3 SE: 39-44, 51-52 differentiate between pure substances and mixtures. SE: 2.1 SE: Can Be Developed From: 34 C.1.2 Observe and describe chemical and TR: Can Be Developed From: Small Scale physical properties of different types of Chemistry Lab Manual: 17-21; Guided matter and designate them as either Reading and Study Workbook: 11 extensive or intensive. C.1.3 Recognize observable indicators of chemical changes.
SE: 2.4
SE: 33 TR: Small-Scale Chemistry Lab Manual: 2330; Guided Reading and Study Workbook: 17-18
C.1.4 Describe physical and chemical changes at the molecular level.
SE: 2.1, 2.4, 11.1, 11.2
SE: 37, 48-51, 346-354, 356-367 TR: Guided Reading and Study Workbook: 13-14, 17-18, 115-116
C.1.5 Describe the characteristics of solids, liquids, and gases and state changes at the molecular level.
SE: 2.1, 13.1, 13.2, 13.2, 13.3, 13.4
SE: 34-37, 420-424, 425-430, 431-434, 436-439 TR: Guided Reading and Study Workbook: 137-143
C.1.6 Explain and apply the law of conservation of mass as it applies to chemical processes.
SE: 2.4, 12.1, 12.2
SE: 50, 355, 405 TR: Guided Reading and Study Workbook: 114, 128
C.1.7 Define density and distinguish among materials based on densities. Perform calculations involving density.
SE: 3.2, Chapter 3, 10.2
SE: 80-82, 92 (Small-Scale Lab) , 322 TR: Guided Reading and Study Workbook: 29, 30, 31
SE = Student Edition
TE = Teacher’s Edition
TR = Teaching Resources 3
TECH = Technology
Chemistry - Indiana Edition © 2012 Correlated to: Indiana’s Revised Academic Standards for Chemistry I / 3064 (High School)
INDIANA ACADEMIC STANDARDS
SE Lessons (chapter & lesson numbers)
SE, TE, TR, TECH (page numbers)
Standard 2: Atomic Structure and the Periodic Table Core Standard - Describe how the properties and arrangement of the subatomic particles contributes to the structure of the atom. Core Standard - Describe how the structure of the periodic table reflects the numbers of electrons and protons and the configuration of the electrons in an atom. SE: 4.1, 4.2, 4.3, 5.1, 5.2, 5.3 SE: 102-103, 107-109, 128-132, 133 C.2.1 Describe how models of atomic TR: Guided Reading and Study Workbook: structure changed over time based on 43 available experimental evidence and understand the current model of atomic structure. SE: 4.2 SE: 105-109 C.2.2 Describe how the subatomic particles TR: Guided Reading and Study Workbook: (protons, neutrons, and electrons) 34-36, 43 contribute to the structure of an atom and recognize that the particles within the nucleus are held together against the electrical repulsion of the protons. SE: 4.2, 4.3 SE: 114-115 C.2.3 Determine the number of protons, TR: Guided Reading and Study Workbook: neutrons, and electrons in isotopes and in 35, 37 those isotopes that comprise a specific element. Relate these numbers to atomic number and mass number. C.2.4 Calculate the average atomic mass of SE: 4.3 SE: 116-119, 120 an element from isotopic abundance data. TR: Guided Reading and Study Workbook: 40 C.2.5 Write the electron configuration of an element and relate this to its position on the periodic table.
SE: 6.2
SE: 170-172, 173 TR: Guided Reading and Study Workbook: 54
C.2.6 Use the periodic table and electron configurations to determine an element's number of valence electrons, and chemical and physical properties.
SE: 6.1, 6.2, 6.3, Ch 6, 7.1, Ch 7
SE: 164-166, 167-173, 180, 184, 194-195, 200 TR: Guided Reading and Study Workbook: 52-55
SE = Student Edition
TE = Teacher’s Edition
TR = Teaching Resources 4
TECH = Technology
Chemistry - Indiana Edition © 2012 Correlated to: Indiana’s Revised Academic Standards for Chemistry I / 3064 (High School)
INDIANA ACADEMIC STANDARDS
SE Lessons (chapter & lesson numbers)
SE, TE, TR, TECH (page numbers)
SE: 25.1, 25.2, 25.3, 25.4 SE: 876, 888-891 C.2.7 Compare and contrast nuclear TR: Guided Reading and Study Workbook: reactions with chemical reactions. For 272 nuclear reactions, describe how the fusion and fission processes transform elements present before the reaction into elements present after the reaction. SE: 25.2, Ch 25 SE: 882- 886, 887 (Small-Scale Lab) C.2.8 Understand that the radioactive decay TR: Small-Scale Chemistry Lab Manual: process is random for any given atom, but 287-291; Guided Reading and Study that this property leads to a predictable and Workbook: 270, 274 measurable exponential decay of a sample of radioactive material. Calculate the initial amount, the fraction remaining, or the halflife of a radioactive isotope, given two of the three variables. Standard 3: Bonding and Molecular Structure Core Standard - Describe how the configuration of electrons within an atom determines its interactions with other atoms. Core Standard - Describe the attractive forces between molecules and how their effect on chemical and physical properties. C.3.1 Describe, compare, and contrast the SE: 7.2, 8.1, 8.2, 8.3, 8.4 SE: 223, 224-225, 226-238 characteristics of the interactions between TR: Guided Reading and Study Workbook: atoms in ionic and covalent compounds. 61-62, 69-70 C.3.2 Compare and contrast how ionic and covalent compounds form. C.3.3 Compare and contrast ionic, covalent network, metallic and polar and non-polar molecular crystals with respect to constituent particles, strength of bonds, melting and boiling points and conductivity; provide examples of each type. C.3.4 Draw structural formulas for and name simple molecules.
SE = Student Edition
SE: 7.2, 8.1, 8.2, 8.3, 8.4
SE: 223, 224-225, 226-238
SE: 7.1, 7.2, 7.3, 8.1, 8.2, 8.3, 8.4, 13.2, 13.3, 15.1
SE: Can Be Developed From: 194, 200, 202, 204, 205, 206, 208, 210-211, 217, 432
SE: 8.3, 9.3, 9.4, 9.5, 22.1, 22.2, 22.3, 22.4
SE: 226-237, 766-771, 772-773, 774, 778, 784, 787, 789, 803, 821 TR: Lab Manual: 295-296; Guided Reading and Study Workbook: 238, 250
TE = Teacher’s Edition
TR = Teaching Resources 5
TECH = Technology
Chemistry - Indiana Edition © 2012 Correlated to: Indiana’s Revised Academic Standards for Chemistry I / 3064 (High School)
INDIANA ACADEMIC STANDARDS C.3.5 Write chemical formulas for ionic compounds given their names and vice versa.
SE Lessons (chapter & lesson numbers) SE: 9.1, 9.2, 9.5
SE, TE, TR, TECH (page numbers) SE: 264-269, 271-279, 292-294, 295, 296, 297 TR: Guided Reading and Study Workbook: 81-82, 83-84, 88-89
Standard 4: Reactions and Stoichiometry Core Standard - Use balanced chemical equations and the mole concept to determine the quantities of reactants and products. C.4.1 Predict products of simple reactions SE: Ch 7, 11.1, 11.2, 11.3 SE: 203, 345, 356-365, 366-367 such as synthesis, decomposition, single TR: Small-Scale Chemistry Lab Manual: 108 replacement and double replacement. SE: 11.1, 12.1, 23.1 SE: 349-354, 371-373, 415 C.4.2 Balance chemical equations using the TR: Lab Manual: 121-126; Small-Scale law of conservation of mass and use them to Chemistry Lab Manual: 108-109 describe chemical reactions. C.4.3 Use the mole concept to determine the number of moles and number of atoms or molecules in samples of elements and compounds, given mass of the sample.
SE: 10.1, 10.2, 10.3, 12.1, 12.2, 12.3
SE: 305, 309, 311, 319, 391, 404 TR: Lab Manual: 121-126; Small-Scale Chemistry Lab Manual: 91-94, 324, 399; Guided Reading and Study Workbook:93-94, 99-105
C.4.4 Using a balanced chemical equation, calculate the quantities of reactants needed and products made in a chemical reaction that goes to completion. C.4.5 Describe, classify and give examples of various kids of reactions-synthesis (combination), decomposition, single displacement, double displacement and combustion. C.4.6 Determine oxidation states and identify the substances apparently gaining and losing electrons in redox reactions. C.4.7 Perform calculations to determine percent composition by mass of a compound or mixture when given the formula.
SE: 12.1
SE: 384-389 TR: Lab Manual: 127-132; Small-Scale Chemistry Lab Manual: 399
SE: 11.2, 11.3, 23.1, 23.2, 23.3
SE: 345, 356-365, 366-367, 368 TR: Small-Scale Chemistry Lab Manual: 109
SE: 20.1, 20.2, 20.3
SE: 691, 692-696, 700, 716 TR: Lab Manual: 275-278
SE: 10.3
SE: 325-329 TR: Guided Reading and Study Workbook: 106-109
SE = Student Edition
TE = Teacher’s Edition
TR = Teaching Resources 6
TECH = Technology
Chemistry - Indiana Edition © 2012 Correlated to: Indiana’s Revised Academic Standards for Chemistry I / 3064 (High School)
INDIANA ACADEMIC STANDARDS
SE Lessons (chapter & lesson numbers)
SE, TE, TR, TECH (page numbers)
Standard 5: Behavior of Gases Core Standard - Using the kinetic molecular theory, describe and explain the behavior of ideal gases. Core Standard - Examine the relationship between number of moles, volume, pressure, and temperature for ideal gases, using the ideal gas equation of state PV = nRT. C.5.1 Use kinetic molecular theory to explain SE: 14.1, 14.2, 14.3 SE: 464-467 changes in gas volumes, pressure, moles, TR: Lab Manual: 147-153, 155-161; Guided and temperature. Reading and Study Workbook: 147-155 SE: 14.3, Ch 14 SE: 466, 479 C.5.2 Using the ideal gas equation of state, PV = nRT, calculate the change in one variable when another variable is changed and the others are held constant. SE: 14.3, 18.3 SE: 467, 614 C.5.3 Given the equation for a chemical TR: Guided Reading and Study Workbook: reaction involving one or more gases as 156 reactants and/or products calculate the volumes of gas assuming the reaction goes to completion and the ideal gas law holds. Standard 6: Thermochemistry Core Standard - Recognize that chemical reactions result in either the release or absorption of energy. Core Standard - Apply the law of conservation of energy. SE: 2.1, 13.4, 15.3 SE: 36-37, 436, 506 C.6.1 Explain that atoms and molecules that TR: Lab Manual: 229, 239; Guided Reading make up matter are in constant motion and and Study Workbook: 138, 139 that this motion increases as thermal energy increases. SE: 17.1 SE: 556-561 C.6.2 Distinguish between the concepts of temperature and heat flow in macroscopic and microscopic terms. SE:17.1, 17.3 SE: 561, 570 C.6.3 Solve problems involving heat flow TR: Guided Reading and Study and temperature changes, using known Workbook:191-192 values of specific heat and/or phase change constants (latent heat values). C.6.4 Classify chemical reactions and phase SE: 17.2, 17.3 SE: 555, 558, 576 changes as exothermic or endothermic. TR: Guided Reading and Study Workbook: 184
SE = Student Edition
TE = Teacher’s Edition
TR = Teaching Resources 7
TECH = Technology
Chemistry - Indiana Edition © 2012 Correlated to: Indiana’s Revised Academic Standards for Chemistry I / 3064 (High School)
INDIANA ACADEMIC STANDARDS
SE Lessons (chapter & lesson numbers)
SE, TE, TR, TECH (page numbers)
Standard 7: Solutions Core Standard - Describe the composition and characteristics of solutions. Core Standard - Identify the factors that qualitatively affect solubility, reaction rates and dynamic equilibrium. C.7.1 Describe the composition and SE: 15.3, 16.1, 16.2, 16.3, 16.4 SE: 504-507, 518-524 properties of types of solutions. TR: Guided Reading and Study Workbook: 168-169, 172 C.7.2 Explain how temperature, pressure and polarity of the solvent affect the solubility of a solute.
SE: 16.1
SE: 521-523, 524 TR: Lab Manual: 189-193; Guided Reading and Study Workbook: 167, 168-169
C.7.3 Describe the concentration of solutes in solution in terms of molarity. Perform calculations using molarity, mass, and volume. C.7.4 Prepare a specific volume of a solution of a given molarity when provided with a known solute.
SE: 16.2, 16.4
SE: 525-526, 533 TR: Guided Reading and Study Workbook: 176-177
SE: 15.3, 16.1
SE: 507, 518-524 TR: Guided Reading and Study Workbook: 168-169, 172
C.7.5 Explain how the rate of a reaction is qualitatively affected by changes in concentration, temperature, surface area, and the use of a catalyst. C.7.6 Write equilibrium expressions for reversible reactions.
SE: 16.1
SE: 521-523, 524 TR: Lab Manual: 189-193; Guided Reading and Study Workbook: 167, 168-169
SE: 18.3
SE: Can Be Developed From: 609-614 TR: Guided Reading and Study Workbook: 176-177
Standard 8: Acids and Bases Core Standard - Use acid-base definitions to identify acids and bases given their formulas and reactions. Core Standard - Explain the meaning of the value indicated by the pH scale in terms of the hydrogen ion concentration for any aqueous solution. SE:19.1 SE:646-652 C.8.1 Use Arrhenius and Brønsted-Lowry TR: Small-Scale Chemistry Lab Manual: definitions to classify substances as acids or 227-234 bases.
SE = Student Edition
TE = Teacher’s Edition
TR = Teaching Resources 8
TECH = Technology
Chemistry - Indiana Edition © 2012 Correlated to: Indiana’s Revised Academic Standards for Chemistry I / 3064 (High School)
INDIANA ACADEMIC STANDARDS
SE Lessons (chapter & lesson numbers)
SE, TE, TR, TECH (page numbers)
C.8.2 Describe the characteristic properties of acids and bases.
SE:19.1
SE: 652 TR: Small-Scale Chemistry Lab Manual: 232; Guided Reading and Study Workbook: 209-212
C.8.3 Compare and contrast the dissociation and strength of acids and bases in solution.
SE:19.3
SE: 664-670, 671 TR: Guided Reading and Study Workbook: 214-215
SE:19.2 SE:657, 658, 659 C.8.4 Given the hydronium (H3O+) ion concentration in a solution, calculate the pH, and vice versa. Explain the meaning of these values. C.8.5 From acid-base titration data, SE: 19.4 SE: 675 calculate the concentration of an unknown TR: Lab Manual: 259-266 solution. Standard 9: Organic Chemistry and Biochemistry Core Standard - Describe the unique nature of carbon atoms demonstrated by their ability to bond to one another and other elements, forming countless carbon-based substances and macromolecules. SE: 22.1, 22.2, 22.3, 22.4, 22.5 SE: 762-771, 772-773, 775-778, 779-781, C.9.1 Use structural formulas to illustrate 782-783, 789 carbon atoms’ ability to bond covalently to TR: Guided Reading and Study Workbook: one another to form many different 237-246, 247-254 substances. C.9.2 Illustrate the variety of molecular types formed by the covalent bonding of carbon atoms and describe the typical properties of these molecular types.
SE = Student Edition
SE: 22.1, 22.2, 22.3, 22.4, 23.1
TE = Teacher’s Edition
SE: 798-802, 804-811, 812-820, 822-827, 828 TR: Guided Reading and Study Workbook: 237-246, 247-254
TR = Teaching Resources 9
TECH = Technology
