Ms. Keever's Science Classes
There is a $30 lab fee for all science lab classes. Fees can be paid by cash or check (payable to Butler High School). Fees must be paid for supplies to be purchased so students to participate in lab.
CHEMISTRY SYLLABUS
Activities and Labs are subject to change.
| DATE | DAY | SECTION | TOPIC | ACTIVITIES/LABS | OUTCOMES | |
| Unit 1: Getting Started (4 days) | ||||||
| 6-Jan | W | 1 | 1-3 | Guidelines/Classroom Rules Chemistry & Math Pre-Test Introduction to Periodic Table |
Forms to be signed. TEST.
Issue books. List of ions for homework. Unit 1 Vocabulary |
1.2 Contrast properties of metals, nonmetals, and metalloids. Given symbol, identify element. Given element, identify symbol. Identify the metals and nonmetals on the periodic table. Describe the arrangement of the periodic table. |
| 7-Jan | R | 2 | 7-1, 22-2, 22-3 | Naming and Writing Chemical Formulas, Part 1 LTF Lesson 13 (180 min / 2) |
LTF - Chemical Nomenclature |
2.0 Describe the structure of carbon chains, branched chains, and rings. 3.1 Utilize electron configurations, Lewis dot structures, and orbital notations to write chemical formulas. 6.3 Identify the nomenclature of ionic compounds, binary compounds, and acids. Learn to apply the rules of chemical nomenclature. |
| 11-Jan | M | 3 | 7-1, 22-2, 22-3 | Naming and Writing Chemical Formulas, Part 2 LTF Lesson 13 (180 min / 2) |
LTF - Chemical Nomenclature (continued) Formula Writing & Naming worksheet. |
2.0 Describe the structure of carbon chains, branched chains, and rings. 3.1 Utilize electron configurations, Lewis dot structures, and orbital notations to write chemical formulas. 6.3 Identify the nomenclature of ionic compounds, binary compounds, and acids. Master the skill of writing and naming chemical formulas. |
| 12-Jan | T | 4 | Lab Safety & Lab Equipment Unit 1 TEST |
Lab Tour & Equipment Worksheet TEST Unit 2 Vocabulary |
Complete a unit assessment. Define vocabulary for next unit. AHSGE #1 Select appropriate laboratory glassware, balances, time measuring equipment, and optical instruments to conduct an experiment. |
|
| Unit 2: Math & Measurement (9 days) | ||||||
| 13-Jan | W | 5 | 2-2 | Units of Measurement: SI/Metric Density Conversion Factors |
Name and use SI units. Perform density calculations Transform a statement of equality into a conversion factor. |
|
| 14-Jan | R | 6 | 2-3 | Numbers in Science: Measurements, Sig Figs, Dimensional Analysis LTF Foundation Lesson II (180 min / 2) |
LTF - Numbers in Science | Use correct measurement techniques, correct use of sig figs, and dimensional analysis. |
| 15-Jan | F | 7 | 2-3 | Numbers in Science: Measurements, Sig Figs, Dimensional Analysis LTF Foundation Lesson II (180 min / 2) |
LTF - Numbers in Science (continued) | Use correct measurement techniques, correct use of sig figs, and dimensional analysis. |
| 19-Jan | T | 8 | 2-3 | Accuracy & Precision Percent Error Dimensional Analysis LTF Lesson 2 (45 min) |
LTF - Dimensional Analysis | Distinguish between accuracy and precision. Calculate percent error. Become more proficient in solving mathematical science problems. |
| Monday Jan 18 - MLK Holiday - No School | ||||||
| 20-Jan | W | 9 | 2-3 | Dimensional Analysis QUIZ Scientific Notation Manipulating Variables and Constants LTF Foundation Lesson III (45 min) |
QUIZ Scientific Notation worksheet LTF - Literal Equations |
Complete an assessment. Convert measurements into scientific notation and perform calculations in scientific notation. Solve literal equations for a particular variable. |
| 21-Jan | R | 10 | 2-3 | Graphing; Inverse & Direct Relationships LTF Foundation Lesson IV (45 min) |
LTF - Graphing Skills | Become familiar with basic line graphing skills to be used throughout their
science course of study. Differentiate between direct and inverse relationships. |
| 22-Jan | F | 11 | 2-1 | Graphing Quiz Scientific Method LTF Foundation Lesson I ( 90 min / 2) |
QUIZ LTF - Come Fly With Us LAB LTF - Scientific Method Practice 1 |
Complete an assessment. Identify & apply the steps of the scientific method. |
| 25-Jan | M | 12 | 2-1 | Scientific Method LTF Foundation Lesson I ( 90 min / 2) |
LTF - Penny Test LAB LTF - Scientific Method Practice 2 |
Learn about controls and variables in an experiment. Learn what constitutes valid experimental procedure. |
| 26-Jan | T | 13 | Unit 2 Review & TEST Lab Safety Video & Test |
TEST Unit 3 Vocabulary |
Complete a unit review and assessment. Define vocabulary for next unit. Describe lab safety procedures and complete an assessment with 80% or higher. |
|
| Unit 3: Matter & Energy (5 days) | ||||||
| 27-Jan | W | 14 | 1-2 | Properties & Changes in Matter Classifying Matter |
1.0 Differentiate among pure substances, mixtures, elements, and compounds. 1.1 Distinguish between intensive and extensive properties of matter. 1.3 Distinguish between homogeneous and heterogeneous forms of matter. 5.0 Use the kinetic theory to explain states of matter, phase changes, solubility, and chemical reactions. Distinguish between the physical and chemical properties of matter. Classify changes of matter as physical or chemical. Distinguish between an element, compound, pure substance, and mixture. |
|
| 28-Jan | R | 15 | 1-2 | Chromatography LTF Lesson 3 (90 min) |
LTF- Separating Metal Ions in Solution LAB | 1.0 Differentiate among pure substances, mixtures, elements, and compounds. 1.3 Distinguish between homogeneous and heterogeneous forms of matter. Use paper chromatography to physically separate and determine the metal ions in an unknown solution. |
| 29-Jan | F | 16 | 16-1 | Energy/Specific Heat/Exothermic & Endothermic | Specific Heat Calculations worksheet Endothermic & Exothermic Lab |
1.0 Differentiate among pure substances, mixtures, elements, and compounds. 1.1 Distinguish between intensive and extensive properties of matter. 5.0 Use the kinetic theory to explain states of matter, phase changes, solubility, and chemical reactions. Distinguish between endothermic and exothermic processes. Perform specific heat calculations. |
| 1-Feb | M | 17 | 16-1 | Specific Heat Lab | Specific Heat LAB | 8.0 Distinguish among endothermic and exothermic physical changes. 8.1 Calculate temperature change by using specific heat. |
| 2-Feb | T | 18 | Unit 3 Review & TEST | TEST Unit 4 Vocabulary |
8.0 Distinguish among endothermic and exothermic physical changes. 8.1 Calculate temperature change by using specific heat. Complete a chapter review and assessment. Define vocabulary for next unit. |
|
| Unit 4: Atomic Structure (6 days) | ||||||
| 3-Feb | W | 19 | 3-2, 3-3 | Structure of the Atom Atomic & Mass Numbers, Isotopes LTF Lesson 8 (20 min) |
LTF - Isotopic Pennies LAB | 3.2 Calculate the number of protons, neutrons, and electrons in an isotope. 3.3 Utilize benchmark discoveries to describe the historical development of atomic structure. List the properties of protons, neutrons, and electrons. Describe the arrangement of protons, neutrons, and electrons in an atom. Determine the percent abundance of sample pennies and then practice calculations involving abundance, isotopes, and atomic mass. |
| 4-Feb | R | 20 | 3-3 | Average Atomic Mass, Moles, Molar Mass | 6.0 Solve stoichiometric problems involving relationships among the number
of particles, moles, and masses of reactants and products in a chemical
reaction. Calculate average atomic mass. Determine molar mass for an element and a compound. |
|
| 5-Feb | F | 21 | 3-1, 3-2, 4-1, 4-2, 7-3 |
Mole <---> Gram Conversions Atomic Theory & Experiments |
6.0 Solve stoichiometric problems involving relationships among the number
of particles, moles, and masses of reactants and products in a chemical
reaction. Convert between moles and grams using molar mass. Summarize Dalton's, Thompson's, Rutherford's, and Bohr's contributions to atomic theory. |
|
| 8-Feb | M | 22 | 4-1 & 4-2 | Atomic Theory & Experiments Quantum Mechanical Model LTF Lesson 4 (10 min) |
LTF - Matter Waves | 3.3 Utilize benchmark discoveries to describe the historical development of
atomic structure. Summarize Einstein's, de Broglie's, Heisenberg's, and Schrödinger's contributions to atomic theory. Use the traditional Einsteinian equations to derive the de Broglie equation for matter waves. |
| 9-Feb | T | 23 | 4-2 & 4-3, 7-2 | Quantum Numbers, Electron Configurations, & Electrons, Oxidation Numbers LTF Lesson 5 (90 min) |
LTF - Electron Configurations, Orbital Notation, and Quantum Numbers | 3.3 Utilize benchmark discoveries to describe the historical development of
atomic structure. 6.2 Assign oxidation numbers for individual atoms of monoatomic and polyatomic ions. 6.3 Identify the nomenclature of ionic compounds, binary compounds, and acids. Write correct electron configurations, orbital notations, and quantum numbers for the valence electrons in certain elements. Justify oxidation states based on electron configurations and enhance understanding of chemical formula writing. |
| 10-Feb | W | 24 | Unit 4 Review & TEST | TEST Unit 5 Vocabulary |
Complete a chapter review and assessment. Define vocabulary for next unit. |
|
| Unit 5: Periodic Properties (3 days) | ||||||
| 11-Feb | R | 25 | 5-1, 5-2 | Periodic Table - definitions of properties | 3.0 Use the periodic table to identify periodic trends, including atomic
radii, ionization energy, electronegativity, and energy levels. 3.3 Utilize benchmark discoveries to describe the historical development of atomic structure. Describe the history of the Periodic Table. Describe the modern Periodic Table. Locate the four blocks of the Periodic Table. Describe several periodic properties. |
|
| Friday Feb. 12 - Teacher Inservice/LTF Training - No School for Students | ||||||
| Monday Feb. 15 - President's Day - No School | ||||||
| 16-Feb | T | 26 | 5-2 | Periodic Trends LTF Lesson 7 (45 min) |
LTF - Why Do They Call It a Periodic Table? | 3.0 Use the periodic table to identify periodic trends, including atomic
radii, ionization energy, electronegativity, and energy levels. 3.3 Utilize benchmark discoveries to describe the historical development of atomic structure. Graph various periodic properties to examine the trends of the elements as they are arranged on the periodic table. |
| 17-Feb | W | 27 | Alabama Direct Assessment of Writing, Grade 10 | Puzzles & Review for students not testing. | ||
| 18-Feb | R | 28 | Unit 5 Review & TEST | TEST Unit 6 Vocabulary |
Complete a chapter review and assessment. Define vocabulary for next unit. |
|
| Unit 6: Composition Stoichiometry, Chemical Reactions, & Reaction Stoichiometry (9 days) | ||||||
| 19-Feb | F | 29 | 7-3 | Using Chemical Formulas: Percent Composition Mole <---> Gram Conversions |
6.0 Solve stoichiometric problems involving relationships among the number
of particles, moles, and masses of reactants and products in a chemical
reaction. 6.5 Determine the empirical or molecular for a compound using percent composition data. Calculate the percent composition of a given compound. Convert between moles and grams for a given compound (review). |
|
| 22-Feb | M | 30 | 7-4 | Determining Chemical Formulas: Empirical Formulas LTF Lesson 17 (45 min) |
LTF - Simple vs. True | 6.5 Determine the empirical or molecular for a compound using percent
composition data. Calculate empirical and molecular formulas using logical problem-solving steps. |
| 23-Feb | T | 31 | 8-1 | Describing Chemical Reactions | List observations that indicate a chemical change has taken place. Write a word equation and a formula equation for a given chemical reaction. |
|
| 24-Feb | W | 32 | 8-1 | Balancing Chemical Reactions | 6.0 Solve stoichiometric problems involving relationships among the number
of particles, moles, and masses of reactants and products in a chemical
reaction. Balance a formula equation by inspection/atom inventory/trial-and-error. AHSGE #3 Identify reactants and products associated with photosynthesis and cellular respiration, and the purposes of these two processes. |
|
| 25-Feb | R | 33 | 8-2 | Types of Chemical Reactions | 3.1 Utilize electron configurations, Lewis dot structures, and orbital
notations to write chemical formulas. 6.4 Classify chemical reactions as composition, decomposition, single replacement, or double replacement. Give general equations for the five main types of chemical reactions. Classify a chemical reaction as one of the five main types. Predict the products of simple reactions given the reactants. |
|
| 26-Feb | F | 34 | 8-3 | Activity Series of the Elements | 6.4 Classify chemical reactions as composition, decomposition, single
replacement, or double replacement. Use an activity series to predict whether a given reaction will occur and what the products will be. |
|
| 1-Mar | M | 35 | AHSGE | Puzzles & Review for students not in testing during shortened 2nd period. | ||
| 2-Mar | T | 36 | AHSGE | |||
| 3-Mar | W | 37 | AHSGE | |||
| 4-Mar | R | 38 | AHSGE | |||
| 5-Mar | F | 39 | AHSGE | |||
| 8-Mar | M | 10 | 9-1 | Balancing Quiz Introduction to Stoichiometry LTF Lesson 16 (45 min) |
QUIZ LTF - Stoichiometry |
6.0 Solve stoichiometric problems involving relationships among the number
of particles, moles, and masses of reactants and products in a chemical
reaction. Complete an assessment. Describe the importance of a mole ratio in stoichiometry. Students will be introduced to an alternative and student-friendly method of stoichiometry which will enhance their readiness for solving equilibrium problems. |
| 9-Mar | T | 41 | 9-2 | Ideal Stoichiometric Calculations | 6.0 Solve stoichiometric problems involving relationships among the number
of particles, moles, and masses of reactants and products in a chemical
reaction. Perform moles-moles, moles-gram, and gram-gram stoichiometric calculations. |
|
| 10-Mar | W | 42 | 9-3 | Limiting Reactants & Percent Yield LTF Lesson 18 (45 min) |
LTF - Limiting Reactant LAB | 6.0 Solve stoichiometric problems involving relationships among the number
of particles, moles, and masses of reactants and products in a chemical
reaction. Determine which of the two reactants is limiting. Distinguish between theoretical and actual yield. Calculate percent yield. React aluminum with copper(II) chloride to determine the limiting reactant and present results in a formal lab report. |
| 11-Mar | R | 43 | Exam Review | Complete practice assessments. | ||
| 12-Mar | F | 44 | Midterm EXAM (Units 1-6) | MIDTERM EXAM Unit 7 Vocabulary (Spring Break Assignment) |
Complete a term assessment. Define vocabulary for next unit. |
|
| Mon. Mar. 15 through Fri. Mar. 19 - Spring Break - No School | ||||||
| Unit 7: Bonding & Molecular Geometry (6 days) | ||||||
| 22-Mar | M | 46 | 6-1, 6-2, 6-3, 6-4, 6-5 |
Chemical Bonding LTF Lesson 10 (90 min) |
LTF - Chemical bonding | 1.0 Differentiate among pure substances, mixtures, elements, and compounds. 3.1 Utilize electron configurations, Lewis dot structures, and orbital notations to write chemical formulas. 6.1 Predict ionic and covalent bond types and products given known reactants. 6.2 Assign oxidation numbers for individual atoms of monoatomic and polyatomic ions. Identify characteristics for the three most common types of chemical bonds: ionic, covalent, and metallic. From drawn structures, shapes and hybridizations will be determined and properties will be discussed. |
| 23-Mar | T | 47 | 6-2 | Covalent Bonding, Octet Rule Lewis Dot Structures, Resonance |
3.1 Utilize electron configurations, Lewis dot structures, and orbital
notations to write chemical formulas. 6.1 Predict ionic and covalent bond types and products given known reactants. 6.2 Assign oxidation numbers for individual atoms of monoatomic and polyatomic ions. Use electronetativity difference to determine bond type. Construct Lewis structures using the octet rule. Describe resonance and the structures used to represent some molecules. |
|
| 24-Mar | W | 48 | 6-3, 6-4 | Ionic Bonding Metallic Bonding |
1.0 Differentiate among pure substances, mixtures, elements, and compounds. 3.1 Utilize electron configurations, Lewis dot structures, and orbital notations to write chemical formulas. 6.1 Predict ionic and covalent bond types and products given known reactants. Describe ionic and metallic bonding. Compare bond energy and lattice energy. Compare the properties of covalent, ionic, and metallic bonds and compounds. |
|
| 25-Mar | R | 49 | 6-5 | Molecular Geometry: VSEPR Theory LTF Lesson 12 (45 min) |
LTF - Molecular Geometry | 3.1 Utilize electron configurations, Lewis dot structures, and orbital
notations to write chemical formulas. Explain VSEPR theory. Draw Lewis (electron) dot diagrams and then build models. Use models to visualize the shape of the molecule and determine the hybridization. |
| 26-Mar | F | 50 | 6-5 | Polarity, Intermolecular Forces LTF Lesson 11 (45 min) Hybrid Orbitals, Sigma & Pi Bonds |
LTF - Don't Flip Your Lid | Explain what determines molecular polarity. Describe the intermolecular forces. Use knowledge of intermolecular forces (IMF) to explain relative differences in melting points. |
| 29-Mar | M | 51 | Unit 7 Review & TEST | TEST Unit 8 Vocabulary |
Complete a chapter review and assessment. Define vocabulary for next unit. |
|
| Unit 8: Gas Laws (7 days) | ||||||
| 30-Mar | T | 52 | 10-1, 11-1 | The KMT of Matter Pressure |
5.0 Use the kinetic theory to explain states of matter, phase changes,
solubility, and chemical reactions. 7.0 Explain the behavior of ideal gases in terms of pressure, volume, temperature, and number of particles using Charles's, Boyle's, Gay-Lussac's, combined, and ideal gas laws. Describe the five assumptions of the kinetic molecular theory and the behavior of solids, liquids, and gases. Convert between different units of pressure. |
|
| 31-Mar | W | 53 | 11-2 | Boyle's & Charles's Laws LTF Lesson 19 (45 min) |
LTF - Charles' Law LAB | 7.0 Explain the behavior of ideal gases in terms of pressure, volume,
temperature, and number of particles using Charles's, Boyle's, Gay-Lussac's,
combined, and ideal gas laws. State Boyle's and Charles's laws and perform gas law calculations. Investigate the relationship between the volume of a gas and the temperature. Extrapolate the data to determine a value for absolute zero. |
| 1-Apr | R | 54 | 11-2 | Gay-Lussac's & Combined Gas Laws | 7.0 Explain the behavior of ideal gases in terms of pressure, volume,
temperature, and number of particles using Charles's, Boyle's, Gay-Lussac's,
combined, and ideal gas laws. State Gay-Lussac's and the Combined Gas Law and perform gas law calculations. |
|
| 2-Apr | F | 55 | 11-1 | Dalton's Law of Partial Pressures Graham's Law: Diffusion & Effusion |
5.0 Use the kinetic theory to explain states of matter, phase changes,
solubility, and chemical reactions. 7.0 Explain the behavior of ideal gases in terms of pressure, volume, temperature, and number of particles using Charles's, Boyle's, Gay-Lussac's, combined, and ideal gas laws. State Dalton's and Graham's laws and perform gas law calculations. |
|
| 5-Apr | M | 56 | 11-4 | Gas Stoichiometry LTF Lesson 20 (45 min) |
LTF - Airbags LAB | 6.0 Solve stoichiometric problems involving relationships among the number
of particles, moles, and masses of reactants and products in a chemical
reaction. 7.0 Explain the behavior of ideal gases in terms of pressure, volume, temperature, and number of particles using Charles's, Boyle's, Gay-Lussac's, combined, and ideal gas laws. Describe the law of combining volumes and use it to perform gas stoichiometry calculations. Design an airbag with baking soda, hydrochloric acid, and a resealable plastic bag. Perform calculations to determine optimum quantities to just fill the bag with gas. |
| 6-Apr | T | 57 | 11-3 | Ideal Gas Law Gas Density & Molecular Mass |
7.0 Explain the behavior of ideal gases in terms of pressure, volume,
temperature, and number of particles using Charles's, Boyle's, Gay-Lussac's,
combined, and ideal gas laws. State the Ideal gas law and perform gas law calculations. Calculate a gas's density and molar mass using the Ideal gas law. |
|
| 7-Apr | W | 58 | Unit 8 Review & TEST | TEST Unit 9 Vocabulary Take-home work for next unit. |
Complete a chapter review and assessment. Define vocabulary for next unit. |
|
| Unit 9: Liquids & Solids (2 days) | ||||||
| 8-Apr | R | 59 | 10-4 | Changes of State: Phase Diagrams LTF Lesson 21 (25 min) |
LTF - Heating Curves and Phase Diagrams (activity 2) | 5.0 Use the kinetic theory to explain states of matter, phase changes,
solubility, and chemical reactions. 8.0 Distinguish among endothermic and exothermic physical and chemical changes. 8.2 Use Le Chatlier's principle to explain changes in physical and chemical equilibrium. Develop and enrich understanding of phase changes by investigating phase diagrams. Use the diagrams to solve problems and apply the information to enrich understanding of the underlying physical phenomena. |
| 9-Apr | F | 60 | 10-2 & 10-3 | Liquids & Solids (go over packet) Unit 9 TEST |
TEST Unit 10 Vocabulary |
5.0 Use the kinetic theory to explain states of matter, phase changes,
solubility, and chemical reactions. Describe the properties of liquids and solids and the phase changes they undergo. Describe the four types of crystals. Complete a chapter review and assessment. Define vocabulary for next unit. |
| Unit 10: Solutions (7 days) | ||||||
| 12-Apr | M | 61 | 12-1 & 12-2 | Types of Mixtures The Solution Process |
1.0 Differentiate among pure substances, mixtures, elements, and compounds. 1.3 Distinguish between homogeneous and heterogeneous forms of matter. 4.0 Describe solubility in terms of energy changes associated with the solution process. 4.2 Explain the conductivity of electrolytic solutions. 4.4 Describe factors that affect the rate of solution. 5.0 Use the kinetic theory to explain states of matter, phase changes, solubility, and chemical reactions. 8.0 Distinguish among endothermic and exothermic physical and chemical changes. Describe the properties of solutions, colloids, and suspensions; electrolytes and nonelectrolytes. Describe three factors that affect the rate of dissolution. Describe the meaning of "like dissolves like" and solution equilibrium. Compare the effects of temperature and pressure on solubility. |
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| 13-Apr | T | 62 | 12-3 | Concentration of Solutions | 4.5 Solve problems involving molarity, including solution preparation and
dilution. Perform molarity and molality calculations. |
|
| 14-Apr | W | 63 | 13-1 | Compounds in Aqueous Solutions Precipitation Reactions |
4.2 Explain the conductivity of electrolytic solutions. 6.4 Classify chemical reactions as composition, decomposition, single replacement, or double replacement. 8.0 Distinguish among endothermic and exothermic physical and chemical changes. Write dissociation equations and compare dissociation and ionization. Predict whether a precipitate will form when solutions of soluble ionic compounds are combined and write net ionic equations for those precipitates. |
|
| 15-Apr | R | 64 | 13-1 | Solubility Rules & Net Ionic Equations LTF Lesson 14 (45 min) |
LTF - Net Ionic Equations | 4.2 Explain the conductivity of electrolytic solutions. 6.4 Classify chemical reactions as composition, decomposition, single replacement, or double replacement. 8.0 Distinguish among endothermic and exothermic physical and chemical changes. Write net ionic equations from balanced molecular equations. |
| 16-Apr | F | 65 | 13-1 | Ionization & Electrolytes LTF Lesson 22 (45 min) |
LTF - Conductivity of Ionic Solutions LAB (If CBLs can be obtained) |
4.2 Explain the conductivity of electrolytic solutions. 6.4 Classify chemical reactions as composition, decomposition, single replacement, or double replacement. 8.0 Distinguish among endothermic and exothermic physical and chemical changes. Investigate the electrical conductivity of several ionic solutions and relate this to the number of ions formed during dissociation. |
| 19-Apr | M | 66 | 13-2 | Colligative Properties of Solutions LTF Lesson 23 (45 min) |
LTF - Colligative Properties LAB | 4.2 Explain the conductivity of electrolytic solutions. 6.4 Classify chemical reactions as composition, decomposition, single replacement, or double replacement. 8.0 Distinguish among endothermic and exothermic physical and chemical changes. Describe the four colligative properties. Explore the nature of colligative properties and calculate changes in boiling point and freezing point of various solutions. Determine the molecular mass of an unknown solute using freezing point data. AHSGE #2 Describe cell processes necessary for achieving homeostasis, including active and passive transport, osmosis, diffusion, exocytosis, and endocytosis. |
| 20-Apr | T | 67 | Unit 10 Review & TEST | TEST Unit 11 Vocabulary |
Complete a chapter review and assessment. Define vocabulary for next unit. |
|
| Unit 11: Kinetics & Equilibrium (6 days) | ||||||
| 21-Apr | W | 68 | 17-1 | The Reaction Process & Reaction Mechanisms | 5.0 Use the kinetic theory to explain states of matter, phase changes,
solubility, and chemical reactions. Explain the concept of reaction mechanism. Use the collision theory to interpret chemical reactions. Relate activation energy to enthalpy of reaction. |
|
| 22-Apr | R | 69 | 17-2 | Reaction Rate & Rate Laws | Describe two conditions necessary for reactions to occur. Discuss the factors that influence reaction rate. Relate the order of a reaction to the rate law for the reaction. Explain and write rate laws for chemical reactions. |
|
| 23-Apr | F | 70 | 18-1 | LTF Lesson 26 (45 min) The Equilibrium Concept |
LTF - The Iodine Clock Reaction LAB | Time a classic iodine clock reaction and subsequently graph data to
determine the order of a reactant involved in the reaction. Describe equilibrium and explain the nature of the equilibrium constant. Write equilibrium expressions and carry out calculations involving them. |
| 26-Apr | M | 71 | 18-1 | Using RICE Tables LTF Lesson 27 (90 min) |
LTF - General Chemical Equilibrium | Solve gas-phase and concentration equilibrium problems using the RICE table
approach. Equate Kc to Kp. |
| 27-Apr | T | 72 | 18-2 | Le Chatelier's Principle LTF Lesson 28 (45 min) |
LTF - Disturbing Equilibrium LAB | 8.2 Use Le Chatlier's principle to explain changes in physical and chemical
equilibrium. State Le Chatlier's principle. Observe the effect of a change to conditions on a system at equilibrium and then explain the effects observed by application of Le Chatlier's Principle. |
| 28-Apr | W | 73 | Unit 11 Review & TEST | TEST Unit 12 Vocabulary |
Complete a chapter review and assessment. Define vocabulary for next unit. |
|
| Unit 12: Acid/Base Equilibrium (6 days) | ||||||
| 29-Apr | R | 74 | 14-1 & 14-2 | Properties of Acids & Bases Acid/Base Definitions |
4.3 Describe acids and bases in terms of strength, concentration, pH, and
neutralization reactions. 6.3 Identify the nomenclature of ionic compounds, binary compounds, and acids. List physical and chemical properties of acids and bases and the uses of common examples. Describe the three acid/base definitions. Explain conjugate acids and bases. |
|
| 30-Apr | F | 75 | 14-3, 15-1 | Acid/Base Reactions pH |
4.3 Describe acids and bases in terms of strength, concentration, pH, and
neutralization reactions. 6.4 Classify chemical reactions as composition, decomposition, single replacement, or double replacement. Write neutralization reactions. Describe pH and perform pH and pOH calculations. Calculate [|H+] and {OH-] from pH and pOH. |
|
| 3-May | M | 76 | 15-2 | Titrations | 4.3 Describe acids and bases in terms of strength, concentration, pH, and
neutralization reactions. 4.5 Solve problems involving molarity, including solution preparation and dilution. 6.0 Solve stoichiometric problems involving relationships among the number of particles, moles, and masses of reactants and products in a chemical reaction. Explain how to carry out an acid/base titration. Calculate the molarity of a solution from titration data. |
|
| 4-May | T | 77 | 18-3 | Equilibria of Acids, Bases, & Salts | 8.2 Use LeChatlier's principle to explain changes in physical and chemical
equilibrium. Explain the concept of acid ionization constants and write acid ionization expressions. Explain buffering. |
|
| 5-May | W | 78 | 18-3 | LTF Lesson 29 (90 min) | LTF - Acid-Base Equilibrium | Solve acid-base equilibrium problems using the RICE table problem-solving method. |
| 6-May | R | 79 | Unit 12 Review & TEST | TEST | Complete a chapter review and assessment. Define vocabulary for next unit. |
|
| Unit 13: Thermodynamics (3 days) | ||||||
| 7-May | F | 80 | 16-1 | Enthalpy | 8.0 Distinguish among endothermic and exothermic physical and chemical
changes. 8.1 Calculate temperature change by using specific heat. Review specific heat. Explain enthalpy and changes in enthalpy. Solve problems involving enthalpy. |
|
| 10-May | M | 81 | 16-2 | Entropy, Gibbs Free Energy | 5.0 Use the kinetic theory to explain states of matter, phase changes,
solubility, and chemical reactions. 8.0 Distinguish among endothermic and exothermic physical and chemical changes. 8.2 Use Le Chatlier's principle to explain changes in physical and chemical equilibrium. Explain the relation between enthalpy, entropy, and Gibbs free energy, and the tendency for a reaction to occur. |
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| 11-May | T | 82 | Unit 13 TEST | TEST | Complete a chapter review and assessment. Define vocabulary for next unit. |
|
| Unit 14: Nuclear Chemistry (4 days) | ||||||
| 12-May | W | 83 | 21-1 & 21-2 | The Nucleus & Radioactive Decay | 9.0 Distinguish between chemical and nuclear reactions. 9.1 Identify atomic and subatomic particles, including mesons, quarks, tachyons, and baryons. 9.2 Calculate the half-life of selective radioactive isotopes. Describe nuclear binding energy and its relation to a stable nucleus. Describe different types of radioactivity. Balance nuclear equations. Perform half-life calculations. |
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| 13-May | R | 84 | LTF Lesson 9 (45 min) | LTF - Red Hot Half-Life LAB | 9.2 Calculate the half-life of selective radioactive isotopes. 9.3 Identify types of radiation and their properties. Model a system of nuclear decay using red hots. Analyze the data using a graphing calculator. Perform half-life calculations. |
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| 14-May | F | 85 | 21-3 & 21-4 | Nuclear Radiation, Fission, & Fusion | 9.3 Identify types of radiation and their properties. 9.4 Contrast fission and fusion. 9.5 Describe carbon-14 decay as a dating method. Compare the penetrating power and shielding requirements of alpha, beta, and gamma radiation. Describe the devices used in radiation detection. Describe applications of radioactive nuclides. Distinguish between nuclear fission and fusion, and describe their uses. |
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| 17-May | M | 86 | Unit 14 Review & Test | TEST | Complete a chapter review and assessment. Begin final exam review. |
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| 18-May | T | 87 | Exam Review | Complete practice assessments. | ||
| 19-May | W | 88 | Exam Review | Complete practice assessments. | ||
| 20-May | R | 89 | Exam Review | Complete practice assessments. | ||
| 21-May | F | 90 | Exam Review | Complete practice assessments. | ||
| 24-May | M | 91 | 1ST & 2ND PERIOD FINAL EXAMS | EXAM | Complete a semester assessment. | |
| 25-May | T | 92 | 3RD & 4TH PERIOD FINAL EXAMS | |||
| 26-May | W | 93 | EXAM MAKE UP DAY | |||
