Greene County Schools Course Sequence Guide. Lesson#/Day SPI Topics to be Covered Supplemental Resources 1(Ch.1) N/A Syllabus/Intro to Class

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1 School: Subject: West Greene Chemistry Greene County Schools Course Sequence Guide Lesson#/Day SPI Topics to be Covered Supplemental Resources 1(Ch.1) N/A Syllabus/Intro to Class Classroom Handouts Pretest 2 (Ch. 2) CLE 3221.I Inq.1 & 2 CLE 3221.I.2.1 Identify areas of chemistry Pure and applied chemistry Identify reasons to study chemistry Examples and demos; inquiry questions CLE 3221.I Inq. 1 & 3, T/E.3 ID areas and examples of research ID reasons to study chemistry CLE 3221.I 1,2, & 6 Scientific method; collaboration & communication CLE 3221.I. Math 2 ID steps and practice problem solving CLE 3221.I.Inq 4 3 CLE ; CLE 3221.I Inq. 2 &3 ID intensive and extensive properties Define, describe and list physical properties Differentiate among states of matter Categorize matter as a substance or mixture Distinguish between homogeneous and heterogeneous Describe ways that mixtures can be separated Explain elements and compounds Distinguish between substance and a mixture 4 CLE , Inq. 2 & 3 CLE ; CLE 3221.Math.1 ID elements and compounds Distinguish between substance and mixtures, ID chemical symbols of elements, and names of elements Examples and demos; inquiry questions Examples and demos; inquiry questions

2 Describe what happens during 4 cont. chemical changes; ID evidences of chemical changes; Apply law of conservation of mass in chemical reactions 5 CLE 3221.; CLE Substances and mixtures; physical and chemical changes 6 CLE ; CLE 3221; CLE 3221.I Inq.1 & 2 CLE 3221.I.2.1;CLE 3221.I Inq. 1 & 3, T/E.3 ;CLE 3221.I 1,2, & 6 CLE 3221.I. Math 2 CLE 3221.I.Inq 4 Lab on physical and chemical changes; Examples of elements, compounds, physical and chemical changes; lab equipment info sheet Lab and workbook 7 See above Review for chapter 1 & 2 test Notes and workbook study-guide 8 See above See above Chapter 1 & 2 test 9 (Ch. 3) CLE 3221.Math 1 &2, CLE Inq3, CLE Inq4 Examples on board 10 CLE 3221.Math 1 & 2; CLE 3221 Inq 2 Explore scientific notation, distinguish between accuracy and precision, and error of measurement; Introduce significant digits SI units of measurement; distinguish between weight and mass; covert C & K temp scales Conversion factors; Using dimensional analysis 11 CLE ; CLE 3221 Inq & 3; Conversion factors; Using dimensional analysis Calculate and density and describe how it varies with temp 12 CLE 3221.Math 1 & 2; Density and conversions CLE 3221 Inq 2&3; CLE CLE 3221.Math 1 & 2; Review Ch. 3 for test Information handout of SI units; examples on board Information handout of SI units; examples on board Ex. Problems on board; Galileo thermometer Density lab Notes and workbook study guide CLE 3221 Inq 2&3; CLE See above Ch. 3 test Ch. 3 test 15 (Ch. 4) CLE , CLE 3221.T/E.3, Describe Democritus s ideas about Models; examples

3 15 (cont.) CLE 3221.Inq. 1 & 3 CLE , CLE Inq.1 & 2 16 CLE ; CLE 3221.Inq.1,2,&3 CLE 3221.Math 1 &2, atoms; Explain Dalton s atomic theory; ID instruments used to observe atoms; ID 2 types of subatomic particles; Describe the structure of atoms according to Rutherford Explain the difference between elements and isotopes; calculate neutrons and atomic mass; explain why chemists use the periodic table (cont.) Isotope worksheet; examples; periodic table 17 See above Review for Ch 4 test Notes and workbook study guide 18 See above Chapter 4 test 19 Ch. 5, CLE , CLE , CLE , ; CLE 3221.Inq.1, & 2 ID inadequacies in Rutherford theory; ID Bohr s model; Describe energies and Flame test lab position of electrons; Orbital shapes 20 CLE ; CLE Describe and explain electron configuration 21 CLE , CLE , CLE 3221.Inq.2&3;CLE3221.Math2 22 &23 CLE , CLE , CLE , CLE 3221.Inq.1, CLE 3221.Inq. 2 Describe relationship between wavelength and light; ID source of atomic emission spectra; Distinguish between quantum mechanics and classical mechanics ID the inadequacies in the Rutherford atomic model. ID the new proposal in the Bohr model of the atom. Describe the energies and positions of electrons according to the quantum mechanical model. Describe how the shapes of orbitals related to different sub-levels differ. 24 CLE , CLE Describe the electron configuration for an atom. Explain the actual electron configurations for some elements differ from those predicted by the aufbau principle 25 &26 CLE , CLE , CLE Inq. 2, Describe the relationship between the wavelength and frequency of light. ID Class activity writing electron configuration Class activity view light through prism glasses Models; Wintergreen mint activity Do electron configurations for the first 20 elements using the aufbau Black box activity;

4 25 & 26 cont. CLE 3221.Inq. 3. CLE 3221 math.2 the source of atomic emission spectra. Explain how the frequencies of emitted light are related to changes in electron energies. Distinguish between quantum mechanics and classical mechanics. 27 See above Review for assessment of chapter 5 Workbook and quiz 28 See above Assessment of Chapter 5 Ch. 5 test 29 Ch. 6, CLE , Explain how elements are organized in Teacher Demo on organizing CLE 3221.Inq.1 the periodic table. Compare early and modern periodic table. ID 3 broad classes of elements. 30 CLE ,, CLE Describe the information on the periodic table. Classify elements based on electron configuration. Distinguish representative elements and transition elements. I Have Who has Game 31 CLE , CLE , CLE 3221.Inq.2 Describe the trends among the elements for atomic size. Explain how ions form. Describe periodic trends for 1 st ionization energy, ionic size, and electronegativity Label periodic table with trends 32 See Above Review for Chapter 6 Test Workbook and quiz 33 See Above Chapter 6 Assessment Chapter 6 Test 34 Ch. 7. CLE , CLE , CLE 3221.Inq.2 Determine the number of valence electrons in an atom of a representative element. Explain how the octet rule applies to atoms of metallic and nonmetallic elements. Describe how cations form. Explain how anions form. 35 CLE , Ionic bonds and ionic compounds. Explain the electrical charge of an ionic compound. Describe three properties of ionic compounds 36 CLE Model the valence electrons of model Write symbols and names of ions. Draw dot diagrams; quiz on polyatomic ions Quiz on polyatomic ions

5 36 cont. Cont. atoms. Describe the arrangement of atoms in a metal. Explain the importance of alloys. 37 See Above Review for Chapter 7 Test Workbook and worksheets 38 See Above Chapter 7 assessment Chapter 7 Test 39 CLE Distinguish between the melting point Teacher Demo: Molecular models and boiling points of molecular compounds and ionic compounds. 40, 41, & 42 Ch. 8 CLE , Describe how electrons are shard to form covalent bonds and identity exceptions to the octet rule. Demonstrate how electron dot structures represent shared electrons. Describe how atoms form double or triple covalent bonds. Describe how Drawing dot diagrams for polyatomic ions 43 CLE & 45 CLE , CLE , CLE , CLE 3221.Inq.3, oxygen atoms are bonded in ozone. Describe the relationship between atomic and molecular orbitals. Describe how VSPER theory helps predict the shapes or molecules. Identify ways in which orbital hybridization is useful in describing molecules. Describe how electronegativity values determine the distribution of charge in a polar molecule. Describe what happens to polar molecules when they are placed between oppositely charged metal plates. Evaluate the strength of intermolecular attractions compared with the strength of ionic and covalent bonds. Identify the reason why network solids have high melting points. Molecular geometry 46 See Above Review for Ch. 8 assessment 47 See Above Ch. 8 Test Paper chromatography lab.

6 48 Mid Term Exam 49 Ch. 9 CLE , CLE ID the charges of monatomic ions by using the periodic table and name the ion. Define polyatomic ion and write the names and formulas of the most common polyatomic ions. ID the endings for the names of most polyatomic ions. 50 CLE , Apply the rules for naming and writing formulas for binary ionic compounds. Apply the rules for naming and writing formulas for compounds with polyatomic ions. 51 CLE Interpret the prefixes in the names of molecular compounds in terms of their chemical formulas. 52 CLE Apply 3 rules for naming acids. Apply the rules in reverse to write the formulas of acids. Apply the rules for 53 CLE naming bases. Define the laws of definite proportions and multiple proportions. Apply the rules for naming chemical compounds by using a flowchart. Apply the rules for writing the formulas of chemical compounds using a flowchart. Label periodic table with charges Worksheets with naming compounds Oxidation numbers and formulas activity; Worksheets with covalent bonding. Races with naming compounds. Workbook pages 54 See Above Review for Ch. 9 Assessment Chapter 9 Test 55 Ch. 10 CLE , CLE Math.1, CLE Math.2 Describe methods of measuring the amount of something. Define Avogadro s number as it relates to a mole of a substance. Distinguish between the atomic mass of an element and its molar mass. Describe how the mass of a mole of a Demo: Moles and mass Demo: how many is 6.02 x Sample problems and worksheetconverting moles, grams and representative units

7 compound is calculated. 56 CLE CLE , CLE Math 1, CLE Math 2, Describe how to convert the mass of a substance to the number of moles of a substance, and mole to mass. 57 CLE CLE , CLE Describe how to convert the mass of a 3221.Math 1, substance the number of moles of a substance and moles to mass. ID the volume of a quantity of gas at STP. 58 & 60 CLE CLE Describe how to calculate the percent CLE 3221.Math.1, by mass of an element in a compound. CLE 3221.Math.2, Interpret an empirical formula. Distinguish between empirical and molecular formulas. 61 See Above Review for Ch. 10 Test Workbook pages, quizzes 62 See Above Ch. 10 Assessment Ch. 10 Test 63 & 64 Ch. 11 CLE , CLE 3221.Math.1, CLE 221.Math.2, Describe how to write a word equation. Describe how to write a skeleton equation. Describe the steps for writing a balanced chemical equation. 65 CLE Describe the five general types of reactions. Predict the products of the five general types of reactions. 66 & 67 CLE , Describe the information found in a net ionic equation. Predict the formation a precipitate in a double replacement reaction. Practice problems and worksheets. Demo: Molar volume Practice problems and worksheets. Quiz on molar conversions. Practice problems and worksheets. Empirical Formula Lab. Quiz on molar conversions. Demo: why balance chemical equations Balancing chemical equations practice and worksheet. Demo types of reactions. ID types of reactions on balancing equations worksheet. Writing and Balancing net ionic equations worksheet and Types of Reactions Lab 68 See Above Review for Ch. 11 Test Workbook, Ch. 11 Quiz 69 See Above Ch. 11 Assessment Ch. 11 Test 70 Ch. 12 CLE , CLE 3221.Math.1, CLE 3221.Math 2, 71 & Math.1, CLE 3221.Math 2, CLE Explain how balanced equations apply to both chemistry and everyday life. Interpret balanced chemical equations in terms of mole, representative particles, mass and gas volume at STP. Construct mole ratios from balanced chemical equations and apply these Stoichiometry worksheet and practice problems. Stoichiometry worksheet and practice problems. Chapter Review questions

8 Cont. Cont Math.1, CLE 3221.Math 2, CLE ratios in stoichiometric calculations. Calculate stoichiometric quantities from balanced chemical equations using units of moles, mass, representative particles, and volumes of gases at STP. Identify the limiting reagent in a reaction. Calculate theoretical yield, actual yield given appropriate and problems. Stoichiometry worksheet and practice problems. Chapter Review questions and problems. information. 74 See Above See Above Stoichiometric Lab 75 See Above Ch. 12 Review Workbook 76 See Above Ch. 12 Assessment Ch. 12 Test 77 Ch. 13 CLE 3221.Math.1, CLE 3221.Math 2, CLE CLE CLE CLE CLE CLE 80 CLE , CLE Describe the assumptions of the kinetic theories it applies to gases. Interpret gas pressure in terms of kinetic theory. Define the relationship between Kelvin temperature and average kinetic energy. ID the factors that determine physical properties of a liquid. Define evaporation in terms of kinetic energy. Describe the equilibrium between a liquid and it vapor. ID the conditions at which boiling occurs. Evaluate how the way particles are organized explains the properties of solids. ID the factors that determine the shape of a crystal. Explain how allotropes of an element are different. ID the conditions necessary for sublimation. Describe how equilibrium conditions are represented in a phase diagram. Demo: air pressure Sample and practice problems Class activity water versus alcohol. Demo: crystalline solid model Allotropic forms of carbon Demo: sublimation CO 2 Lab-Changes of physical states 81 See Above Review for Chapter 13 Assessment Workbook pages, quiz

9 82 83 See Above CLE CLE CLE , CLE 3221.Math.1, CLE 3221.Math.2 85 CLE , CLE 3221.Math.1, CLE 3221.Math.2 86 CLE , CLE 3221.Math.1, CLE 3221.Math.2 CLE Inq.2 Ch. 13 Assessment Explain why gases are easier to compress than solids or liquids are. Describe the three factors that affect gas pressure. Describe the relationships among the temperature, pressure, and volume of a gas. Use the combined gas law to solve problems. Compute the value of an unknown using the ideal gas law. Compare and contrast real and ideal gas. Relate the total pressure of a mixture of gases to the partial pressures of the component gases. Explain how the molar mass of a gas affects the rate at Ch. 13 Test Demo: Pressure and particle size Demo: pressure and volume Lab: Boyle s Law Lab: Charles s Law Quick Lab: carbon dioxide from antacid tablets. Lab: Diffusion of Gases which the gas diffuses and effuses. 87 See Above Review for Ch. 14 Assessment Workbook 88 See Above Ch. 14 Assessment Ch. 14 Test 89 All CLE covered this semester Review for semester test Notes, formulas, past tests 90 All CLE covered this semester Semester Test Semester Test