Mrs. Sutherland s Chemistry/Honor s Chemistry Syllabus Below is the syllabus for both the honors chemistry and chemistry classes offered for the 2016-2017 school year at JCHS. This is an estimate of the content that will be taught along with the approximate time span these topics will take. More frequent than not, students take more time than I have allotted to complete these units. The timeline will be flexible and move at a pace that encourages all students achievement towards mastering the objectives provided. If students finish the required content before the end of the semester, the remainder of the class time available will contain enrichment activities to build lab skills and prepare for their upcoming science classes. If you have questions, please do not hesitate to contact me at 423-727-2620 from 1:45-3:15 first semester or 8:15-9:40 second semester. I am also available via email at csutherland2@jocoed.net. Standards: Unit 1: Scientist Skills SPI 3221 Inq.1 Select a description or scenario that reevaluates and/or extends a scientific finding. SPI 3221 Inq.2 Analyze the components of a properly designed scientific investigation. SPI 3221 Inq.3 Determine appropriate tools to gather precise and accurate data. SPI 3221 Inq.4 Evaluate the accuracy and precision of data. SPI 3221 Inq.5 Defend a conclusion based on scientific evidence. SPI 3221 Inq.6 Determine why a conclusion is free of bias. SPI 3221 Inq.7 Compare conclusions that offer different, but acceptable explanations for the same set of experimental data. Objectives: (ALL objectives are meant to be passed at 80%) 1. TSW analyze situations to see if they are safe for the laboratory. 2. Given a scenario and possible procedures, TSW select the safest procedure to follow in labs. 3. TSW measure mass using an electronic balance scale and triple beam balance. 4. TSW measure the volume of a solid and liquid using a ruler and/or graduated cylinder. 5. TSW measure the density of any given substance using the proper formula. 6. Given a task, TSW label the proper lab tool to complete the task. 7. Given volume, mass, or density, TSW list the units of measurements used to collect that type of data. 8. Shown a lab tool, TSW label the tool with the correct name. 9. TSW list the 5 steps of the scientific method. 10. TSW analyze an experiment to identify errors. 11. TSW conduct an experiment using the proper components of the scientific method. 12. TSW present an experiment that you conduct to the class. 13. TSW write a lab report based on the experiment conducted. 14. TSW compare and contrast the terms precise and accurate. 15. Given a set of data and the methods to collect it, TSW evaluate it to see if it is accurate or precise. 16. Given experimental situations, TSW identify any biases in the experiment. 17. TSW compare and contrast the difference in scientific laws, theories, hypothesis, and observations. 18. Given a set of data, TSW identify the correct type of graph to use. 19. Given a set of data, TSW create a graph to represent it. 20. Determine ways to build onto current scientific scenarios for further research.
21. Given a conclusion, reason why the hypothesis is supported or rejected using data findings. 22. Given a scientific scenario, decide if it is free from bias. Day 1 Student Info Cards/Introductions Starting Off With A Bang I have, who has? Affirmation Bingo Counting the F s 1) Lab safety contract and syllabus signed by your guardian- 1 st quiz grade and 1 st homework grade 2) All about me board 2 nd Quiz grade Day 2 All About Me Board Go Over Syllabus Day 3 Day 4 Common Ground Go Over Lab Safety Pass the beans, please! Seeing the forest for the trees Can you stand it? Making a Machine How full is your bucket? Following Directions Off to the Races! Lab Tools Pre- Assessment Lab Tools Description/Notes Let s Ski! Plenty of Hot Air Pass the Hoop! Don t step there! Lab Safety Test 1) Study for lab safety test 1) Lab safety test- 1 st Test Grade (Must make an 80 or above to participate in labs) 2) Lab Tools and Measurements Magic Square Worksheet- 2 nd Homework Grade 3) Study for lab tools quiz
Day 5 Lost at Sea Talk Behind Their Backs Group Grope Silent Tower Solo 1) Lab Tools Quiz- 3 rd Quiz Grade Lab Tools Quiz Day 6 Practice EOC ***Syllabus, Lab Safety Contract, All About Me Board, and Supplies are due today for a quiz pass*** Day 7 Volume, Mass, and Density Notes Density Lab 1) Volume, Mass, or Density Worksheet- 3 rd Homework Grade 2) Density Lab Sheet- 4 th Quiz Grade 3) ***Turn in Bell Ringers since day 1***- 1 st Participation Grade Day 8 Scientific Method Notes 1) Diane s Experiment Worksheet-4 th Homework Grade 2) Identify the Controls and Variables- 5 th Homework Worksheet Day 9 Start Experiments 1) Experiment participation (Peer Assessed) 2 nd participation grade 2) Experiment lab report and presentation- 5 th Quiz Grade Day 10 Day 11 Work on Experiments Finish Experiments Start Experiment Presentations Check Worksheets 1) ***ALL WORK IS DUE TODAY*** 2) Work on Objectives Day 12 Kahoot! Review Unit Test: Scientist skills Start Math Units/ Notes 1) Unit Test: Science skills- 2 nd Test Grade Unit 2: Math Skills Standards: CLE 3224.Math.1 Understand the mathematical principles associated with the science of chemistry. CLE 3224.Math.2 Utilize appropriate mathematical equations and processes to solve chemistry problems. 3224.Math.1 Use a variety of appropriate notations (e.g., exponential, functional, square root). 3224.Math.2 Select and apply appropriate methods for computing with real numbers and evaluate the reasonableness of the results. 3224.Math.7 Apply and interpret algebraic properties in symbolic
3224.Math.8 Apply and communicate measurement units, concepts and relationships in algebraic problem-solving situations. 3224.Math.9 Select appropriate units, scales, and measurement tools for problem situations involving proportional reasoning and dimensional analysis. 3224.Math.13 Convert among the quantities of a substance: mass, number of moles, number of particles, molar volume at STP. Objectives: (All objectives are meant to be passed at 80%) 23. Convert standard notation numbers to scientific notation. 24. Convert scientific notation numbers to standard notation. 25. Add numbers in scientific notation. 26. Subtract numbers in scientific notation. 27. Multiply numbers in scientific notation. 28. Divide numbers in scientific notation. 29. Compare and contrast accurate and precise. 30. Describe which type of numerical value would require the use of significant figures. 31. Given a value, list the number of significant figures in it. 32. Given a problem to solve, list the correct number of significant figures in it. 33. Given a scenario, calculate the percent of error. 34. Using dimensional analysis, convert units in one step problems. 35. Using dimensional analysis, convert units in two step problems. 37. Given a chemical formula, calculate the molar mass of a substance. 38. Using dimensional analysis, convert moles to grams or grams to moles. Day 13 Scientist Skills Unit Test Corrections 1) Standard and Scientific Notation Worksheet 2) Operations with Scientific Notation 3) Significant Figures Practice Worksheet 4) Calculating Using Significant Figures Math Unit Notes Day 14 Finish Math Notes 1) Percent of Error Worksheet 2) Conversions and Dimensional Analysis Worksheet 3) Molar Mass Worksheet 4) Gram/Mole Conversions Worksheet Day 15 Math Quiz 1) Math Quiz Day 16 Day 17 Work on Math Worksheets Rotating Lab Stations (Review for the test) Work on Objectives Get help on what you got wrong on the quiz Kahoot! Math Unit Test 1) Lab Sheet (per group) Group with the most correct answers will receive 5 pts. extra credit on their test. 1) Objectives (optional) Math Unit Test Unit 3: Matter Properties and Changes
Standards: SPI 3221.2.1 Distinguish among elements, compounds, and mixtures. SPI 3221.2.2 Identify properties of a solution: solute and solvent in a solid, liquid or gaseous solution; procedure to make or determine the concentration of a solution in units of ppm, ppb, morality, percent composition, factors that affect the rate of solution. SPI 3221.2.3 Classify a solution as saturated, unsaturated, or supersaturated based on its composition and temperature and a solubility graph. SPI 3221.2.4 Identify properties of matter (e.g. physical: density, boiling point, melting point, or chemical: ability to rust or tarnish, be sour) or changes in matter (e.g., physical: phase change, shape, color, or chemical: formation of a gas or precipitate.) SPI 3221.2.6 Investigate similarities and differences among solids, liquids and gases in terms of energy and particle spacing. Predict how changes in volume, temperature, and pressure affect the behavior of a gas. Objectives: (All objectives are meant to be passed at 80%) 39. Define chemistry. 40. Define a substance. 41. Draw a picture of the particle arrangement for a solid, liquid, and gas. 42. List the 4 states of matter. 43. Given characteristics of a substance, label it as solid, liquid, or gas. 44. Describe what happens to the state of a substance as heat or energy is applied. 45. Compare and contrast gas and vapor. 46. Compare and contrast physical and chemical properties. 47. Given a list of descriptions, classify them as chemical or physical. 48. Given an item, list its extensive and intensive properties. 49. Given a change, identify it as a chemical or physical change. 50. List some ways to know if a chemical change is happening. 51. Explain the Law of Conservation of Mass 52. List the type of solution system used in a mixture. 53. Compare and contrast heterogeneous and homogeneous mixtures. 54. List the 5 ways to separate mixtures. 55. Given a substance, classify it as element, compound, or mixture. 56. Define compound. 57. Describe how to separate compounds. 58. Define the law of definite proportions. 59. Define the law of multiple proportions. 60. Calculate problems using the laws of definite and multiple proportions. 61. Define Entropy 62. Define Enthalpy 63. Given a scenario determine if entropy or enthalpy is increasing. 64. Interpret Phase Diagrams 65. Interpret Solubility Graphs Day 18 Math Unit Test Corrections Matter Notes 3) Test Corrections 4) Physical and Chemical Changes Worksheet 5) Elements, Compounds, and Mixtures Worksheet 6) Matter Flow Chart
Day 19 Day 20 Finish Matter Notes Chromatography Lab Penny Demo 5) Percent By Mass 1) Chem Lab Report Chem Lab Day 21 Identification of Unknowns Lab 2) Identification of Unknowns Lab Report Day 22 Finish Identification of Unknowns Lab Day 23 Pg. 98-99 in book Jeopardy 1) Pg. 98-99 in book Post-Assessment Matter Day 24 Unit Test 1) Objectives (Optional) 2) Unit Test Unit 4: Atomic Structure Standards: CLE 3221.1.1 Compare and contrast historical models of the atom. CLE 3221.1.3 Describe an atom in terms of its composition and electron characteristics. 93221.1.1 Identify the contributions of major atomic theorists: Bohr, Chadwick, Dalton, Planck, Rutherford, and Thomson. 93221.1.6 Apply the periodic table to determine the number of protons and electrons in a neutral atom. 93221.1.7 Determine the number of protons and neutrons for a particular isotope of an element. Objectives: (All objectives are meant to be passed at 80%) 66. Explain the theories of Early Greek Philosophers concerning matter. 67. Describe the flaw with early matter theories. 68. Given a theory of matter, determine who formed it. 69. List the name of Dalton s Book. 70. List the type of microscope used to look at atoms. 71. Describe J.J. Thompson s Experiment. 72. List the importance of Millikan s experiment. 73. List the name of the experiment that Rutherford is most noted for. 74. Explain the significance of Rutherford s experiment. 75. List where protons and neutrons are housed at. 76. Identify the current atomic model on which current knowledge is based on. 77. Explain the plum pudding model of the atom. 78. Identify the scientist responsible for the plum pudding model. 79. List the charge of the proton, electron, and neutron. 80. Identify what makes up the most mass of the atom. 81. List the approximate mass of protons, neutrons, and electrons. 82. List the name of the scientist responsible for the discovery of the neutron. 83. List the proton, neutron, and electron in ascending order from smallest mass to largest mass. 84. Given an element from the periodic table, determine the protons, neutrons, atomic number atomic mass, and mass number using a periodic table.
85. Describe how to calculate the atomic number of an element. 86. Describe how to calculate the number of protons and electrons found in an atom. 87. Given the atomic number, name, symbol, mass, or number of protons or electrons, identify the missing values in a table. 88. Define isotope. 89. Calculate the mass number of an isotope. 90. Write isotopes in correct notations. 91. Given an isotope, determine the number of protons, neutrons, electrons, and mass number. 92. Given abundance and mass, calculate atomic mass. 93. Given a list of masses for a set of isotopes, predict which has the highest abundance. 94. Explain why radioactive elements emit radiation. 95. Describe what is gained in alpha radiation. 96. Describe what is gained in beta radiation. 97. Explain what charge gamma radiation has. 98. Predict the new atoms formed by the three types of radiation. 99. Write nuclear equations to represent the new products of radiation. Day 25 Matter Unit Test Corrections Atomic Structure Notes Subatomic Particles Worksheet 1) Subatomic Particles Worksheet 7) Isotopes Worksheet Day 26 Day 27 Day 28 Isotopes Worksheet Finish Atomic Structure Notes Personal Radiation Calculator Nuclear Weapons Discussion Nuclear Chemistry Worksheet Half-Life Lab Snackmium Lab Jeopardy Green Pages at the end of the chapter for Atomic Structure in the book 1) Nuclear Chemistry Worksheet 2) Personal Radiation Calculator 3) Nuclear Weapons Paper- Describe some form(s) of a chemical weapon. List how it is used, what its effects are, how it affects the target, what type of isotope is used, what type of radiation the weapon uses, and whether or not you support the use of it. (The length has no set parameters, but be thorough with the information you provide.) 1) Half-Life Worksheet 2) Half-Life Lab 3) Snackmium Lab 1) Green Pages Atomic Structure Post Assessment Day 29 Unit Test: Atomic Structure 1) Objectives (Optional) 2) Unit Test Unit 5: Electrons in an Atom
Standards: CLE 3221.1.1 Compare and contrast historical models of the atom. CLE 3221.1.3 Describe an atom in terms of its composition and electron characteristics. 93221.1.2 Compare the Bohr model and the quantum mechanical electron-cloud models of the atom. 93221.1.3 Draw Bohr models of the first 18 elements. 93221.1.4 Interpret a Bohr model of an electron moving between its ground and excited states in terms of the absorption or emission of energy. 93221.1.12 Represent an atom s electron arrangement in terms of orbital notation, electron configuration notation, and electron- dot notation. 93221.1.13 Compare s and p orbitals in terms of their shape, and order the s, p, d and f orbitals in terms of energy and number of possible electrons. SPI 3221.1.1 Compare and contrast the major models of the atom (i.e., Bohr, and the quantum mechanical model). SPI 3221.1.2 Interpret the periodic table to describe an element s atomic makeup. SPI 3221.1.4 Determine the Lewis electron dot structure or number of valence electrons for an atom of any main-group element from its atomic number or position in the periodic table. SPI 3221.1.5 Represent an electron s location in the quantum mechanical model of an atom in terms of the shape of electron clouds (s and p orbitals in particular), relative energies of orbitals, and the number of electrons possible in the s, p, d and f orbitals. Objectives: (All objectives are meant to be passed at 80%) 100. Describe Planck s contribution to the atomic theory. 101. List the subatomic particle in an atom that is responsible for its chemical behavior. 102. Define a quantum. 103. Define a photon. 104. Define quantum mechanics. 105. Compare and contrast the Bohr and Quantum Mechanics Atomic Models. 106. Calculate the number of electrons found in each orbital according to the Bohr model. 107. Given an element, draw a Bohr model of the atom s composition. 108. Define principle energy levels/ principle quantum levels. 109. Given a scenario, list whether it will require more or less energy to move principle energy levels. 110. List the number of orbitals found in each principle energy level. 111. List the name of the scientist that developed the quantum mechanics model. 112. Describe the way that the quantum mechanics atomic model decides where electrons will be. 113. Draw the shape of the S and P models of the quantum mechanics atomic model. 114. Describe the Aufbau principle. 115. Explain Pauli s Exclusion principle. 116. Explain Hund s Rule. 117. Calculate the longhand electron configuration of an element. 118. Calculate the short hand electron configuration of an element. 119. Explain how to figure electron configurations. 120. Identify how many boxes are present for each energy level using electron orientations. 121. Given an element, write the shorthand electron configuration of that element. 122. Explain what a Lewis Electron Dot Structure is. 123. Write an electron dot structure for an element using electron configurations. 124. Given a periodic table, determine the number of valence electrons an element has. 125. Given a periodic table, write an electron dot structure of an element using the element s group.
Day 30 Atomic Structure Unit Test Corrections Begin Electron Notes Day 31 Day 32 Flame Test Demo Electrons Notes Electron Configuration Orbital Diagrams Finish Electron Notes Lewis Dot-Structure 8) Draw Bohr Models of the first 18 elements 9) Electron Configuration Worksheet 10) Orbital Diagrams and Longhand Configurations Worksheet 6) Chemical Bonds-Ionic Bonds Worksheet 7) Pg. 170-171 #2-19. Day 33 Pg. 170-171 #2-19 Jeopardy 1) Objectives 2) Study for your test Work on Objectives Day 34 Unit Test: Electrons in an Atom 1) Unit Test Unit 6: The Periodic Table Standards: CLE 3221.1.2 Analyze the organization of the modern periodic table. CLE 3221.1.3 Describe an atom in terms of its composition and electron characteristics. 93221.1.5 Use the periodic table to identify an element as a metal, nonmetal, or metalloid. 93221.1.8 Explain the formation of anions and cations, and predict the charge of an ion formed by the main-group elements. 93221.1.9 Sequence selected atoms from the main-group elements based on their atomic or ionic radii. 93221.1.10 Sequence selected atoms from the main-group elements based on first ionization energy, electron affinity, or electronegativity. SPI 3221.1.2 Interpret the periodic table to describe an element s atomic makeup. SPI 3221.1.3 Describe the trends found in the periodic table with respect to atomic size, ionization energy, or electronegativity. Objectives: (All objectives are meant to be passed at 80%) 126. List the number of elements found in the periodic table. 127. List the number of naturally occurring elements. 128. List the name of the scientist responsible for the Law of Octaves. 129. Summarize the Law of Octaves. 130. Write the name of the two people responsible for the first periodic table. 131. List the name of the scientist that created the modern day periodic table. 132. Compare and contrast the first periodic table with the modern day periodic table. 133. Define Periodic Law.
134. List the groups that combine to make the representative elements. 135. List the groups that combine to make the transition elements. 136. Given an element, list its group number, period number, and type of element. 137. Given an element, list it as a metal, non-metal, or metalloid. 138. Given a metal, list it as an alkali metal, alkaline earth metal, transition metal, or inner transition metal. 139. Define atomic radius. 140. Describe trends in atomic radius throughout the periodic table. 141. Define ion. 142. Describe ionic trends throughout the periodic table. 143. Define Ionization energy. 144. Describe the trend in ionization energy found throughout the periodic table. 145. Explain the Octet Rule. 146. Given an element, determine the likelyhood of it gaining/losing electrons based on the octet rule. 147. Define electronegativity. 148. Describe the trend in electronegativity throughout the periodic table. 149. Make comparisons in two elements using all current knowledge about periodic trends. 150. Based on experimental data, determine if an element is a metal, metalloid, or non-metal. 151. Create a periodic table with items you choose to represent periodic trends. Day 35 Electrons in an Atom Unit Test Corrections 1) Periodic Table Project 2) Study for Element Quiz 1-30 Day 36 Periodic Table Notes Finish Notes The Periodic Table Worksheet 1) Elements and Bonding Worksheet 2) The Periodic Table Worksheet Elements and Bonding Worksheet Day 37 Element Quiz Lab: Metal, Non- Metal, or Metalloid Day 38 Pg. 202 1) Element Quiz 1-30 2) Lab Sheet: Metal, Non-Metal, or Metalloid 1) Pg. 202 Day 39 Element Bingo Jeopardy Unit Test: The Periodic Table 1) Objectives 2) Unit Test: The Periodic Table Unit 7: Ionic/Covalent Compounds Standards: CLE 3221.1.2 Analyze the organization of the modern periodic table. CLE 3221.1.3 Describe an atom in terms of its composition and electron characteristics. CLE 3221.3.1 Investigate chemical bonding.
93221.1.8 Explain the formation of anions and cations, and predict the charge of an ion formed by the main-group elements. 93221.3.1 Determine the type of chemical bond that occurs in a chemical compound. 93221.3.2 Differentiate between ionic and covalent bond models. 93221.3.3 Identify the chemical formulas of common chemical compounds. 93221.3.4 Employ a table of polyvalent cations and polyatomic ions to name and describe the chemical formula of ionic compounds. SPI 3221.3.1 Analyze ionic and covalent compounds in terms of their formation (electron transfer versus sharing), names, chemical formulas (e.g., molecular: H2O, CO2, NH3; empirical: NaCl, CaBr2, Al(NO3)3), percent composition, and molar masses. Objectives: (All objectives are meant to be passed at 80%) 152. Define a chemical bond. 153. Define cation. 154. Define anion. 156. Given an ion, determine if it is an anion or a cation. 157. Given an element, list the monatomic ion that it will form. 158. Given the ions forming a compound, write the name of compound. 159. Define Ionic Compound. 160. Determine the charge a transition metal ion needed to complete the compound. 160. Given one element in an ionic compound, compute the amount and charge of the other element. 162. Describe the physical features of an ionic bond that make it so strong. 163. List 5 physical properties of ionic compounds. 164. Define Electrolyte. 165. Define Monoatomic ion. 166. Define Polyatomic ions. 167. Define oxidation number. 168. Given an element, list its oxidation number. 169. Define Oxyanion. 170. Given oxyanions, determine the name of the polyatomic ion. 171. Given a polyatomic ion, list its formula. 172. Given a formula for a polyatomic ion, list the name of the ion. 173. List the five rules for naming ions. 174. Given the name of an ion, list the formula for the ion. Day 40 Periodic Table Unit Test Corrections Element Quiz 1-30 3) Element Quiz 1-30 Day 41 Ionic Compound Notes Finish Ionic Compound Notes Naming Ionic Compounds Worksheet Lots of Ionic Naming Practice Problems 1) Naming Ionic Compounds Worksheet 2) Lots of Ionic Naming Practice Problems Worksheet 3) Write the formula/formula unit worksheet 4) Polyatomic Ion Worksheet
Day 42 Day 43 Naming Acids Ion Poker Sweet Sixteen Ion Tournament ChemLab: Pg. 230 Demo Polyatomic Ions Quiz Pg. 236-237 (2-20) 1) Naming Acids Worksheet 2) Sweet Sixteen Ion Tournament 1) Polyatomic Ions Quiz 2) Pg. 236 & 237 (2-20) Day 44 Compounds Naming Race Unit Test: Ionic Compounds Covalent Bonds Notes 1) Objectives 2) Unit Test: Ionic Compounds Unit 8: Chemical Reactions and the Mole Standards: CLE 3221.3.3 Explore the mathematics of chemical formulas and equations. 93221.2.3 Express the concentration of a solution in units of ppm, ppb, molarity, molality, and percent composition. 93221.3.3 Identify the chemical formulas of common chemical compounds. 93221.3.4 Employ a table of polyvalent cations and polyatomic ions to name and describe the chemical formula of ionic compounds. 93221.3.5 Convert percent composition information into the empirical or molecular formula of a compound. 93221.3.6 Apply information about the molar mass, number of moles, and molar volume to the number of particles of the substance. 93221.3.7 Balance an equation for a chemical reaction. 93221.3.8 Classify a chemical reaction as composition, decomposition, single replacement, double replacement, and combustion. SPI 3221.2.2 Identify properties of a solution: solute and solvent in a solid, liquid or gaseous solution; procedure to make or determine the concentration of a solution in units of ppm, ppb, molarity, percent composition, factors that affect the rate of solution. SPI 3221.2.5 Compare and contrast heat and temperature changes (endothermic / exothermic) in chemical (e.g., combustion) or physical (e.g., phase transformations) processes. SPI 3221.3.1 Analyze ionic and covalent compounds in terms of their formation (electron transfer versus sharing), names, chemical formulas (e.g., molecular: H2O, CO2, NH3; empirical: NaCl, CaBr2, Al(NO3)3), percent composition, and molar masses. SPI 3221.3.2 Determine the reactants, products, and types of different chemical reactions: composition, decomposition, double replacement, single replacement, combustion. SPI 3221.3.3 Predict the products of a chemical reaction (e.g., composition and decomposition of binary compounds). SPI 3221.3.4 Balance a chemical equation to determine molar ratios. SPI 3221.3.5 Convert among the following quantities of a substance: mass, number of moles, number of particles, molar volume at STP. Objectives: (All objectives are meant to be passed at 80%)
175. Explain what an arrow in a chemical formula represents. 176. Balance chemical equations. 177. Given a chemical reaction, identify it as composition/synthesis, decomposition, combustion, single, or double replacement. 178. List the product of a combustion reaction. 179. Explain how to tell if a reaction is a single or double replacement. 180. Define Mole. 181. Define molar mass. 182. Given a chemical formula, calculate the molar mass of the chemical. 183. Calculate the mass of a chemical compound given the number of moles that are present. 184. Calculate the number of moles in a chemical compound given the mass of the element. 185. List Avogadro s Number. 186. Explain what Avogadro s number represents. 187. Convert moles to representative particles. 188. Convert representative particles to moles. 189. Convert the mass of a compound to the number of representative particles in a compound. 190. Convert the number of representative particles in a compound to the mass in grams of the compound or an element in the compound. 191. Determine the molar ratio of a given equation. 192. Solve stoichiometric problems. 193. Given a compound, determine the percent composition of the elements within it. 194. List the formula for calculating molarity. 195. Calculate the molarity of substances. 196. Determine the number of moles, volume, or mass of a substance given the molarity. Day 45 Chemical Equation Notes 11) Balancing Chemical Equations Worksheet 12) Types of Chemical Reactions Worksheet Day 46 Finish Chemical Equation Notes Finish Worksheets 1) Mole, Molecules, and Grams Worksheet 2) Moles, Molar Mass, and Avogadro s Number 3) Using Molarity Worksheet Day 47 Balancing Equations Race 1) Stoichiometry Worksheet 2) Percent Composition Worksheet Start Stoichiometry Day 48 Chemical Reactions and the Mole Take Home Quiz 1) Objectives 2) Unit Quiz Unit 9: Gas Laws Start Gas Laws Unit 10: Review Day 49 Any Questions?
Day 50 Day 51 Review past EOC questions Finish Past EOC question review Examine chemistry questions from other states Day 52 Take a Post-Test EOC 1) Post-test projection level Day 53 Day 54 Day 55 Evaluate weak areas in subgroups of objectives. Go over EOC to find out why mistakes were made. Break into small groups that are also weak in the area you are to find out how to gain points Look at reference sheet Look at study guide Test Taking Strategies Day 56 EOC 1) EOC A complete list of standards can be located at: https://www.tn.gov/assets/entities/education/attachments/std_sci_3221.pdf