Science Topic/Unit: Chemistry/Chemistry A – Acids and ... Science/H… · Chapter Vocabulary . ... Percent water in a Hydrate ... Determine the empirical and molecular formula of

Science Topic/Unit: Chemistry/Chemistry A – Acids and Bases Grade Level: 10-12 Curricular Goals/ Learning Outcomes: (1) Students will be able to define Arrhenius’ theory of acids and bases in terms of the presence of hydronium and hydroxide ions, and Bronsted’s theory of acids and bases in terms of proton donor and accepter, and relate their concentrations to the pH scale. (2) Students will be able to assign oxidation numbers in a reaction. (3) Students will be able to describe oxidation and reduction reactions and give some everyday examples. (4) Identify items that you encounter everyday and use Arrhenius theory and/or Bronsted-Lowry theory to classify them as acids or bases. (5) Use the pH scale to differentiate between acids and bases. (6) Balance Oxidation-Reduction equations using half-reactions. Essential Questions: Define Arrhenius and Bronstead-Lowry acids and Bases. Calculate the concentration of an acid or base through titration. Suggested Number of Sessions: 10 Blocks Content Suggested Instructional

Activities/Technology Resources Suggested Assessments

CH 8.1 Define the Arrhenius theory of acids and bases in terms of the presence of hydronium and hydroxide ions in water and the Bronsted-Lowry theory of acids and bases in terms of proton donors and acceptors. CH 8.2 Relate hydrogen ion concentrations to the pH scale and to acidic, basic, and neutral solutions. Compare and contrast the strengths of various common acids and bases (e.g., vinegar, baking soda, soap, citrus juice). CH 8.3 Explain how a buffer works. CH 8.4 Describe oxidation and reduction reactions and give some everyday examples, such as fuel burning and corrosion. Assign oxidation numbers in a reaction.

CH 8.1 Lecture with notes. Worksheets on Arhenius and Bronstead Lowry Acids and Bases. Chapter Vocabulary CH 8.2 Demonstration: pH and Invisible Ink. Demonstration: Titration of an Acid with a base. Lab. Acids, Bases and pH. Journal Article. Conceptual and Procedural Knowledge of Acid-Base Behavior of Substances, Carles furio-Mas, Journal of Chemical Education, 2007. CH 8.3 Activity: Explain how Antacids work. CH 8.4 Worksheet on Oxidation and Reduction Numbers. Balancing Oxidation-Reduction equations by using half-reactions. Lab: Observing an Oxidation-Reduction Reaction.

Chemistry: Matter and Change. Glencoe-McGraw, 2002. Wilbraham, A.C.; Staley, D.D. Matta, M.S.; Waterman, E.L. Chemistry, Prentice Hall, 2005. Laboratory Manual: Matter and Change Laboratory Manual, Glencoe-McGraw, 2002. Prentice Hall Lab Manual United Streaming Movie: Acids and Bases. Discovery Education. United Streaming Movie: Predicting Oxidation-Reduction Reactions.

Grading of worksheets Laboratory reports Test on Acids and Bases Summarize Journal Article Grading of Journal Article. Grading of Movie notes.

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Science Topic/Unit: Chemistry/Chemistry A – Acids and Bases Grade Level: 10-12 Curricular Goals/ Learning Outcomes: (1) Students will be able to define Arrhenius’ theory of acids and bases in terms of the presence of hydronium and hydroxide ions, and Bronsted’s theory of acids and bases in terms of proton donor and accepter, and relate their concentrations to the pH scale. (2) Students will be able to assign oxidation numbers in a reaction. (3) Students will be able to describe oxidation and reduction reactions and give some everyday examples. (4) Identify items that you encounter everyday and use Arrhenius theory and/or Bronsted-Lowry theory to classify them as acids or bases. (5) Use the pH scale to differentiate between acids and bases. (6) Balance Oxidation-Reduction equations using half-reactions. Essential Questions: Define Arrhenius and Bronstead-Lowry acids and Bases. Calculate the concentration of an acid or base through titration. Suggested Number of Sessions: 10 Blocks

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Science Topic/Unit: Chemistry/Chemistry A - Chemical Reactions and Stoichiometry Grade Level: 10-12 Curricular Goals/ Learning Outcomes: Students will be able to balance chemical equations by applying the law of conservation of mass. Explain how the law of conservation of mass is used to calculate the amount of products formed and reactants used in a chemical reaction. Essential Questions: Use the periodic table to determine gram atomic and gram molecular masses. Balance chemical equations. Calculate the percent composition by mass of elements in a compound. Determine the empirical and molecular formula of compouinds. Determine limiting reactant in a chemical reaction and use it to calculate percent yield of a reaction. Suggested Number of Sessions: 14 Blocks

Content Suggested Instructional Activities/Technology

Resources Suggested Assessments

CH 5.1 Balance chemical equations by applying the laws of conservation of mass and constant composition (definite proportions). CH 5.2 Classify chemical reactions as synthesis (combination), decomposition, single displacement (replacement), double displacement, and combustion. CH 5.3 Use the mole concept to determine number of particles and molar mass for elements and compounds. CH 5.4 Determine percent compositions, empirical formulas, and molecular formulas.

CH 5.1 Lecture with notes. Worksheets on Balancing chemical equations. Chapter Vocabulary Lab: Law of Conservation of Mass Activity with COW. Students will balance chemical equations. http://funbasedlearning.com/chemistry/chembalancer/ques3.htm CH 5.2 Demonstration: Four main types of Chemical. Lab: Different types of Chemical Reactions. CH 5.3 Activity: Mole Relationships in a Chemical Reaction. Activity. Concept mapping on Moles, Atomic Mass, Molecular Mass, Molar Volume, Avogadro’s Number. CH 5.4 Worksheet on Percent Compositions, Empirical Formulas and Molecular Formulas. Lab: Percent water in a Hydrate.

Chemistry: Matter and Change. Glencoe-McGraw, 2002. Wilbraham, A.C.; Staley, D.D. Matta, M.S.; Waterman, E.L. Chemistry, Prentice Hall, 2005. Laboratory Manual: Matter and Change Laboratory Manual, Glencoe-McGraw, 2002. Prentice Hall Lab Manual Study Guide Study Guide for Content Mastery. Glencoe-McGraw, 2002. Prentice Hall Chemistry United Streaming Movie: Different types of Chemical Reactions. Discovery Education.

Grading of worksheets Laboratory reports Quiz on Balancing Chemical Equations Grading Computer Activity on Balancing Chemical Equations Test on Chemical Reactions and Stoichiometry Grading of Concept mapping on Moles.

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http://funbasedlearning.com/chemistry/chembalancer/ques3.htm

http://funbasedlearning.com/chemistry/chembalancer/ques3.htm

Science Topic/Unit: Chemistry/Chemistry A - Chemical Reactions and Stoichiometry Grade Level: 10-12 Curricular Goals/ Learning Outcomes: Students will be able to balance chemical equations by applying the law of conservation of mass. Explain how the law of conservation of mass is used to calculate the amount of products formed and reactants used in a chemical reaction. Essential Questions: Use the periodic table to determine gram atomic and gram molecular masses. Balance chemical equations. Calculate the percent composition by mass of elements in a compound. Determine the empirical and molecular formula of compouinds. Determine limiting reactant in a chemical reaction and use it to calculate percent yield of a reaction. Suggested Number of Sessions: 14 Blocks CH 5.5 Calculate the mass-to-mass stoichiometry for a chemical reaction. CH 5.6 Calculate percent yield in a chemical reaction.

CH 5.5 Worksheets on Stoichiometry and Mole Ratios. CH 5.6 Lab: Percent yield of a Chemical Reaction.

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Science Topic/Unit: Chemistry/Chemistry A - Chemical Reactions and Stoichiometry Grade Level: 10-12 Curricular Goals/ Learning Outcomes: Students will be able to balance chemical equations by applying the law of conservation of mass. Explain how the law of conservation of mass is used to calculate the amount of products formed and reactants used in a chemical reaction. Essential Questions: Use the periodic table to determine gram atomic and gram molecular masses. Balance chemical equations. Calculate the percent composition by mass of elements in a compound. Determine the empirical and molecular formula of compouinds. Determine limiting reactant in a chemical reaction and use it to calculate percent yield of a reaction. Suggested Number of Sessions: 14 Blocks

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Science Topic/Unit: Chemistry/Chemistry A – Chemical Bonding Grade Level: 10-12 Curricular Goals/ Learning Outcomes: Students will be able to explain how atoms combine to form compounds through ionic and covalent bonding. Explain how atoms bond with each other by transferring or sharing valence electrons to form compounds. Explain how the valence-shell electron-pair repulsion theory (VSEPR) is used to predict the molecular geometry (linear, trigonal, planar, and tetrahedral) of simple molecules. Essential Questions: Compare and Contrast ionic and covalent bonding. Draw Lewis dot structures for ionic and covalent molecules. Use the VSEPR to draw the shapes of covalent molecules. Use electronegativity difference to determine the polarity of covalent molecules. Suggested Number of Sessions: 12 Blocks



CH 4.1 Explain how atoms combine to form compounds through both ionic and covalent bonding. Predict chemical formulas based on the number of valence electrons. CH 4.2 Draw Lewis dot structures for simple molecules and ionic compounds. CH 4.3 Use electronegativity to explain the difference between polar and nonpolar covalent bonds. CH 4.4 Use valence-shell electron-pair repulsion theory (VSEPR) to predict molecular geometry (linear, trigonal, planar, and tetrahedral) of simple molecules. CH 4.5 Identify how hydrogen bonding in water affects a variety of physical, chemical, and biological phenomena (e.g., Surface tension,

CH 4.1 Lecture with notes. Worksheets on Naming Ionic and Covalent Compounds. Chapter Vocabulary CH 4.2 Flinn Activity: Lewis Electron Dot Models kit. CH 4.3 Worksheet: Electronegativity difference and bonding types. Journal article on bonding and electronegativity difference. CH 4.4 Use models (VSEPR) to understand molecular structure. Illustrate Electron pair repulsions with balloons. CH 4.5 Lab on hydrogen bonding and adhesive, cohesive properties.

Chemistry: Matter and Change. Glencoe-McGraw, 2002. Wilbraham, A.C.; Staley, D.D. Matta, M.S.; Waterman, E.L. Chemistry, Prentice Hall, 2005. Laboratory Manual: Matter and Change Laboratory Manual, Glencoe-McGraw, 2002. Prentice Hall Lab Manual Study Guide Study Guide for Content Mastery. Glencoe-McGraw, 2002. Prentice Hall Chemistry United Streaming Movie on VSEPR models and Molecular Structures. Discovery Education.

Grading of worksheets on Ionic and Covalent Compounds. Laboratory Report. Test on Chemical Bonding. Grading of Lewis Electron Dot Models of Compounds Grading of VSEPR models of Molecular Structures

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capillary action, density, boiling point). CH 4.6 Name and write the chemical formulas for simple ionic and molecular compounds, including those that contain the polyatomic ions: ammonium, carbonate, hydroxide, nitrate, phosphate and sulfate.

CH 4.6 Lab: writing formulas, oxidation numbers and chemical names. Worksheets on Writing Formula of Ionic and Covalent Compounds. Ionic Compounds Activity: Students will cut and paste ions to make ionic compounds and name them. Journal Article. Science Daily, Chemists Set New World Record For Shortest Chemical Bond Between Metals. http://www.sciencedaily.com/releases/2007/11/ 071121094742.htm Concept mapping on Chemical Bonding, Ionic and Covalent Bonds, Lewis Structures, VSPER models

Quiz on naming and writing chemical formulas Grading Ionic Compounds Activity Grading of Journal Article on Chemical Bond Grading of Concept Mapping

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Science Topic/Unit: Chemistry/Chemistry A – Solutions, Rates of Reaction, and Equilibrium Grade Level: 10-12 Curricular Goals/ Learning Outcomes: (1) Students will be able to describe the process by which solutes dissolve in solvents. (2) Students will be able to identify and explain the factors that affect the rate of dissolving, that is, temperature, concentration, surface area and mixing. (3) Students will be able to describe four colligative properties of solutions. (4) Collect and predict evidence demonstrating that the rate of a reaction can be increased by increasing temperature, concentration or surface area of a reaction. (5) Use LeChatelier’s principle to predict the shift in equilibrium when a system is subjected to a stress (changes in temperature, concentration, pressure or volume). Essential Questions: Calculate the freezing point and boiling temperature of sodium chloride solution and relate to the concentration of the solution. How does Le Chatelier’s Principle predict changes in equilibrium? What is the equilibrium constant expression of a given solution at equilibrium. Suggested Number of Sessions: 12 Blocks



CH 7.1 Describe the process by which solutes dissolve in solvents. CH 7.2 Calculate concentration in terms of molarity. Use molarity to perform solution dilution and solution stoichiometry. CH 7.3 Identify and explain the factors that affect the rate of dissolving (e.g., temperature, concentration, surface area, pressure, mixing). CH 7.4 Compare and contrast qualitatively the properties of solutions and pure solvents (colligative properties such as boiling point and freezing point). CH 7.5 Identify the factors that affect the rate of a chemical

CH 7.1 Lecture with notes Worksheets on solutions-Solutes, Solvent and Saturated and Unsaturated Solutions Chapter Vocabulary Demonstration: Various solutes and their Dissolving Times CH 7.2 Demonstration: Preparation of a solution and determination of its concentration. CH 7.3 Lab: Factors affecting the formation of a Solution. CH 7.4 Worksheet on Colligative Properties of Solutions Lab: Freezing Point Depression of Sodium Chloride Solution

CH 7.5 Worksheet on Factors that Affect Rate of Solution-Stirring,

Chemistry: Matter and Change. Glencoe-McGraw, 2002. Wilbraham, A.C.; Staley, D.D. Matta, M.S.; Waterman, E.L. Chemistry, Prentice Hall, 2005. Laboratory Manual: 1. Matter and Change Laboratory Manual, Glencoe-McGraw, 2002. 2. Prentice Hall Lab Manual United Streaming Movie: Different types of Chemical Reactions. Discovery Education.

Grading of worksheets Laboratory reports. Test on Solutions and LeChateliers Principle.

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Science Topic/Unit: Chemistry/Chemistry A – Solutions, Rates of Reaction, and Equilibrium Grade Level: 10-12 Curricular Goals/ Learning Outcomes: (1) Students will be able to describe the process by which solutes dissolve in solvents. (2) Students will be able to identify and explain the factors that affect the rate of dissolving, that is, temperature, concentration, surface area and mixing. (3) Students will be able to describe four colligative properties of solutions. (4) Collect and predict evidence demonstrating that the rate of a reaction can be increased by increasing temperature, concentration or surface area of a reaction. (5) Use LeChatelier’s principle to predict the shift in equilibrium when a system is subjected to a stress (changes in temperature, concentration, pressure or volume). Essential Questions: Calculate the freezing point and boiling temperature of sodium chloride solution and relate to the concentration of the solution. How does Le Chatelier’s Principle predict changes in equilibrium? What is the equilibrium constant expression of a given solution at equilibrium. Suggested Number of Sessions: 12 Blocks reaction (temperature, mixing, concentration, particle size, surface area, catalyst). CH 7.6 Predict the shift in equilibrium when a system is subjected to a stress (LeChatelier’s principle) and identify the factors that can cause a shift in equilibrium (concentration, pressure, volume, temperature).

Surface Area and Temperature. Activity: Explain the rates of Chemical Reactions in terms of temperature, mixing, concentration, particle size, surface area, catalyst). CH 7.6 Lab: LeChatelier’s principle and Shifts in chemical reactions.

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Science Topic/Unit: Chemistry/Chemistry A – Solutions, Rates of Reaction, and Equilibrium Grade Level: 10-12 Curricular Goals/ Learning Outcomes: (1) Students will be able to describe the process by which solutes dissolve in solvents. (2) Students will be able to identify and explain the factors that affect the rate of dissolving, that is, temperature, concentration, surface area and mixing. (3) Students will be able to describe four colligative properties of solutions. (4) Collect and predict evidence demonstrating that the rate of a reaction can be increased by increasing temperature, concentration or surface area of a reaction. (5) Use LeChatelier’s principle to predict the shift in equilibrium when a system is subjected to a stress (changes in temperature, concentration, pressure or volume). Essential Questions: Calculate the freezing point and boiling temperature of sodium chloride solution and relate to the concentration of the solution. How does Le Chatelier’s Principle predict changes in equilibrium? What is the equilibrium constant expression of a given solution at equilibrium. Suggested Number of Sessions: 12 Blocks

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Science Topic/Unit: Chemistry/Chemistry A – States of Matter Grade Level: 10-12 Curricular Goals/ Learning Outcomes: Students will understand that the amount of energy involved in changes of state of molecular liquids and solids is determined by the type of attractive forces between the molecules. Use the kinetic molecular theory to model the behavior of gases. Describe energy changes in relationships to phase changes. Investigate and describe the idea that the total quantity of energy in a closed system remains constant in any chemical of physical change. Use Hess’s Law to calculate the enthalpy changes of chemical reactions. Essential Questions: Describe a gas at the atomic model. Use Boyles law, Charles law and Combined gas Law to calculate the volume and temperature of a given gas. Apply stoichiometric principles to calculate the amount of gas produced in a chemical reaction. Suggested Number of Sessions: 10 Blocks Content Suggested Instructional

Activities/Technology Resources Suggested Assessments

CH 6.1 Using the kinetic molecular theory, explain the behavior of gases and the relationship between pressure and volume (Boyle’s law), volume and temperature (Charles’s law), pressure and temperature (gay-Lussac’s law), and the number of particles in a gas sample (Avogadro’s hypothesis). Use the combined gas law to determine changes in pressure, volume, and temperature. CH 6.2 Perform calculations using the ideal gas law. Understand the molar volume at 273 K and 1 atmosphere (STP). CH 6.3 Using the kinetic molecular theory, describe and contrast the properties of gases, liquids, and solids. Explain, at the molecular level, the behavior of matter as it undergoes phase transitions. CH 6.4 Describe the law of conservation of energy. Explain the difference between an endothermic process and an exothermic process.

CH 6.1 Lecture with notes Worksheets Chapter Vocabulary Computer project with COW on the Gas Laws with student presentations Compare and Contrast: Charles Law, Boyles Law, Gay-Lussacs Law, Avogadro’s Hypothesis. CH 6.2 Lab: Using the Ideal Gas Law to Calculate the Molar Mass of a volatile Gas. CH 6.3 Worksheets on Kinetic Molecular Theory and Gas Laws Demonstration: Phase changes of water CH 6.4 Lab: Design a Simple Calorimeter. Analyze Energy changes and Calculate the heat produced by a Chemical Reaction.

Chemistry: Matter and Change. Glencoe-McGraw, 2002. Wilbraham, A.C.; Staley, D.D. Matta, M.S.; Waterman, E.L. Chemistry, Prentice Hall, 2005. Laboratory Manual: Matter and Change Laboratory Manual, Glencoe-McGraw, 2002. Prentice Hall Lab Manual Study Guide Study Guide for Content Mastery. Glencoe-McGraw, 2002. Prentice Hall Chemistry United Streaming Movie: Gas Laws and phase transitions. Discovery Education.

Grading of worksheets Laboratory reports Quiz on Gas Laws Grading student presentations on Gas Laws Grading of Gas Laws Activity: Compare and Contrast

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Science Topic/Unit: Chemistry/Chemistry A – States of Matter Grade Level: 10-12 Curricular Goals/ Learning Outcomes: Students will understand that the amount of energy involved in changes of state of molecular liquids and solids is determined by the type of attractive forces between the molecules. Use the kinetic molecular theory to model the behavior of gases. Describe energy changes in relationships to phase changes. Investigate and describe the idea that the total quantity of energy in a closed system remains constant in any chemical of physical change. Use Hess’s Law to calculate the enthalpy changes of chemical reactions. Essential Questions: Describe a gas at the atomic model. Use Boyles law, Charles law and Combined gas Law to calculate the volume and temperature of a given gas. Apply stoichiometric principles to calculate the amount of gas produced in a chemical reaction. Suggested Number of Sessions: 10 Blocks CH 6.5 Recognize that there is a natural tendency for systems to move in a direction of disorder or randomness (entropy).

CH 6.5 Demonstration: Enthalpy, Entropy and Free energy-concepts and Relationships.

United Streaming Movie: Hess’s Law and Enthalpy. Discovery Education.

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Science Topic/Unit: Chemistry/Chemistry A – States of Matter Grade Level: 10-12 Curricular Goals/ Learning Outcomes: Students will understand that the amount of energy involved in changes of state of molecular liquids and solids is determined by the type of attractive forces between the molecules. Use the kinetic molecular theory to model the behavior of gases. Describe energy changes in relationships to phase changes. Investigate and describe the idea that the total quantity of energy in a closed system remains constant in any chemical of physical change. Use Hess’s Law to calculate the enthalpy changes of chemical reactions. Essential Questions: Describe a gas at the atomic model. Use Boyles law, Charles law and Combined gas Law to calculate the volume and temperature of a given gas. Apply stoichiometric principles to calculate the amount of gas produced in a chemical reaction. Suggested Number of Sessions: 10 Blocks

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Science Topic/Unit: Chemistry/Chemistry A – Atomic Structure Grade Level: 10-12 Curricular Goals/ Learning Outcomes: Students will be able to identify the major components of the nuclear atom (protons, neutrons, and electrons) and explain how they interact. Compare nuclear fission and nuclear fusion and mass defect. Describe and explain the atomic model of each scientist. Essential Questions: Draw diagrams of Dalton, Thomson, Rutherford, Bohr, and modern atom models. How does the nucleus of an atom disintegrate to form particles and what are the mass number and atomic number of each particle formed. Write electron configuration and draw orbital energy diagrams for the first twenty elements. Suggested Number of Sessions: 14 Blocks



CH 2.1 Recognize discoveries from Dalton (atomic theory), Thomson (the electron), Rutherford (the nucleus) and Bohr (planetary model of the atom), and understand how each discovery leads to modern theory. CH 2.2 Describe Rutherford’s “gold foil” experiment that led to the discovery of the nuclear atom. Identify the major components (proton, neutrons, and electrons) of the nuclear atom and explain how they interact. CH 2.3 Interpret and apply the laws of conservation of mass, constant composition (definite proportions), and multiple proportions.

CH 2.1 Lecture with notes Computer Project with COW. Timeline of the development of the Atom from Dalton to the modern model of the Atom. Study Guide Worksheets Chapter Vocabulary Journal Article. How Atoms Work. http://science.howstuffworks.com/ atom.htm CH 2.2 Chapter Worksheets Demonstration: How small is an atom? Balloon with vanilla flavoring). CH 2.3 Chapter Worksheets Lab: Law of Conservation of Mass. Matter is neither created or destroyed in a chemical reaction.

Chemistry: Matter and Change. Glencoe-McGraw, 2002. 2. Wilbraham, A.C.; Staley, D.D. Matta, M.S.; Waterman, E. L. Chemistry, Prentice Hall, 2005. Laboratory Manual: Matter and Change Laboratory Manual, Glencoe-McGraw, 2002. Prentice Hall Lab Manual United Streaming movie on Atoms

Grading of worksheets Laboratory Report Quiz on Atoms Grading Journal Article Grading of Computer Project on the timeline development of the atom. Grading of electron configuration and orbital diagrams Vocabulary Test on Atoms and Electron Configuration

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http://science.howstuffworks.com/


CH 2.4 Write the electronic configuration for the first twenty elements of the periodic table. CH 2.5 Identify the three types of radioactive decay (alpha, beta, and gamma) and compare their properties (composition, mass, charge, and penetrating power). CH 2.6 Describe the process of radioactive decay by using nuclear equations, and explain the concept of half-life for an isotope (for example, C-14 is a powerful tool in determining the age of objects). CH 2.7 Compare and contrast nuclear fission and nuclear fusion.

CH 2.4 Electron configuration and orbital diagrams for first twenty elements. Lab: Introduction to the Spectrophotometer. Lab: Flame test for metals Lab on Visible sunscreen (Ultraviolet sunscreen protection activity) CH 2.5 Balance nuclear equation worksheets CH 2.6 Worksheets Lab: Half-Life Simulation by Radioactive Decay Decomonstration: Chain Reaction with Dominos. CH 2.7 Worksheets Computer project with “COW” on uses of radioactivity. Mind Jogger Quiz on Atoms

Powerpoint presentation on introduction to lab on sunscreens United Streaming Video on Radioactive decay. Discovery Education. Mind Jogger Video Quiz on Atoms. Chemistry, Matter and Change. Glencoe. Quiz on Chapter 4

Grading of Computer Project

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Science Topic/Unit: Chemistry/Chemistry A - Periodicity Grade Level: 10-12 Curricular Goals/ Learning Outcomes: Students will be able to use the periodic table to explain and identify periodic patterns of physical and chemical properties that occur within groups and periods of elements. Essential Questions: Determine the number of valence electrons for an element using the periodic table. Describe the periodic nature of atomic radius and ionization energy. Suggested Number of Sessions: 14 Blocks



CH 3.1 Explain the relationship of an element’s position on the periodic table to its atomic number. Identify families (groups) and periods on the periodic table. CH 3.2 Use the periodic table to identify the three classes of elements: metals, nonmetals, and metalloids.

CH 3.1 Lecture with notes Worksheets Chapter Vocabulary CH 3.2 Chapter Worksheets Lab: Metal, Nonmetal or Metalloid? Activity of labeling and coloring a blank periodic table to identify the various groups of elements and their names. Also to identify the s, p, d and f blocks and to identify the position of metals, nonmetals and metalloids. Journal Article: Fluorine. United Streaming. Discovery Education. 2005.

Chemistry: Matter and Change. Glencoe-McGraw, 2002. Wilbraham, A.C.; Staley, D.D. Matta, M.S.; Waterman, E. L. Chemistry, Prentice Hall, 2005. Laboratory Manual: Matter and Change Laboratory Manual, Glencoe-McGraw, 2002. Prentice Hall Lab Manual Study Guide Study Guide for Content Mastery. Glencoe-McGraw, 2002. Prentice Hall Chemistry United Streaming Video on “The Periodic Table.” Discovery education.

Grading of worksheets Laboratory Report Quiz Test on Periodic Table Grading of Computer Project Grading of Periodic Table Activity Grading of Journal Article

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CH 3.3 Relate the position of an element on the periodic table to its electron configuration and compare its reactivity to the reactivity of other elements in the table. CH 3.4 Identify trends on the periodic table (ionization energy, electro negativity, and relative sizes of atoms and ions).

CH 3.3 Worksheets Computer Project with COW on Elements. Students will Choose an Element on the Periodic Table and Research on it and Present to the Class. CH 3.4 Project on Trends in the Periodic Table with Graphing-Ionization Energy, Electron Affinity, Ionic Radii with Atomic Number of the Elements.

Grading of Project on Elements and Student Presentations. Grading of Project on Graphing Periodic Trends.

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Science Topic/Unit: Chemistry/Chemistry A – Properties of Matter Grade Level: 10-12 Curricular Goals/ Learning Outcomes: Students will be able to identify and explain physical and chemical properties used to classify and describe matter. Students will be able to explain the difference between mixtures and pure substances. Students will be able to describe the three states of matter (solid, liquid, gas) in terms of energy, particle motion and phase transitions. Essential Questions: How is energy related to different phases of matter? What chemicals are present around us? What physical and chemical changes occur around us? Suggested Number of Sessions: 7 Blocks



CH 1.1 Identify and explain physical properties (e.g., density, melting point, boiling point, conductivity, malleability) and chemical properties (e.g., ability to form new substances). Distinguish between physical and chemical changes. CH 1.2 Explain the difference between pure substances (elements and compounds) and mixtures. Differentiate between heterogeneous and homogeneous mixtures. CH 1.3 Describe the three normal states of matter (solid, liquid, gas) in terms of energy, particle motion, and phase transitions.

CH 1.1 Lecture with notes Lab: Physical and Chemical Methods Demonstration: Wine to Milk. Density Lab Lab: Reaction between CaCl2 and NaSO3. Demonstration of chemical changes. Study Guide Worksheets Chapter Vocabulary CH 1.2 Demonstration:

a. Electrolysis of water b. Separation between Sulfur and Iron

Lab Separation of a mixture Study Guide Worksheets CH 1.3 Study Guide Worksheets on States of Matter Demonstration: Phase transitions

from solid to liquid, and liquid to gas

Lab: Melting and Boiling of a solid with graphing

Compare and Contrast. Solid, Liquid and Gas

Chemistry: Matter and Change. Glencoe-McGraw, 2002. Wilbraham, A. C.; Staley, D. D. Matta, M. S.; Waterman, E. L. Chemistry. Prentice Hall, 2005. Laboratory Manual: Matter and Change Laboratory Manual, Glencoe-McGraw, 2002. Prentice Hall Lab Manual. 2004. Flinn Scientific kit-Wine to milk. United Streaming movie: Phases of Matter. Discovery Education.

Grading Lab Reports Grading of Worksheets Chapter Test Grading of Work on Solids, Liquids and Gases.

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SOUTHWICK-TOLLAND REGIONAL SCHOOL DISTRICT

Course Title: Chemistry

Chemistry A

Grade: 10-12

CONTENT: THE NATURE OF CHEMISTRY

Chemistry-Description, Branches Measurement-Accuracy and Precision Matter and Energy-Forms and Classifications Energy Transfer-Heat and Work Law of Conservation of Mass Energy Scientific Method Use of SI units for Measurement Calculations Relating to Specific Heat Use significant digits, scientific notation, and the factor-label method in chemical calculations.

FRAMEWORKS/CURRICULUM STANDARDS: MEASURING

1.1 Identify and explain some of the physical properties that are used to classify matter, e.g. density, melting point, and boiling point.

PROPERTIES OF MATTER 1.2 Explain the difference between mixtures and pure substances.* 1.3 Describe the four states of matter (solid, liquid, gas, plasma) in terms of

energy, particles motion, and phase transitions. 1.4 Distinguish between chemical and physical changes

INSTRUCTIONAL METHODOLOGIES: Lectures Readings Videos Directed Questioning Demonstrations

Wine to Milk Making Synthetic Fiber: Nylon Inertia

Skills Worksheets: Significant Digits, Scientific Notation, Factor-Label Method Study Guide Review Sheets

Lab Activities: Observing and Questioning Scientific Method Law of Conservation and Mass-Energy Density Chemical and Physical Changes in Matter Specific Heat of a Metal

INSTRUCTIONAL RESOURCES: CHEMISTRY Text Chemistry- A Modern Course. Merrill, 1990. Lab Manual Chemistry- A Modern Course. Merrill, 1990. Misc. Kit: “Making Nylon Rope”

Videos CHEMISTRY A Text Chemistry: Matter and Change. Glencoe-McGraw-Hill, 2005. Lab Manual Chemistry: Matter and Change Laboratory Manual. Glencoe-

McGraw-Hill, 2005. Instructor’s Guides

Chemistry: Matter and Change Laboratory Manual. Glencoe-McGraw-Hill, 2005. [Teacher Edition]

Chemistry: Matter and Change Block Scheduling Lesson Plans, Chemistry Matter and Change. Glencoe-McGraw-Hill, 2005.

4/9/14 1



Chemistry A

Grade: 10-12

Small-Scale Laboratory Manual, Teacher Edition, Chemistry; Matter and Change. Glencoe-McGraw-Hill, 2005.

Chemlab and Minilab Worksheets Chemistry: Matter and Change. Glencoe –McGraw-Hill, 2005.

Laboratory Management and Safety in the Science Classroom. Glencoe-McGraw-Hill, 2005.

Math Skills Transparency Masters Chemistry: Matter and Change. Glencoe-McGraw-Hill, 2005.

Study Guide for Content Mastery Teacher Edition Chemistry: Matter and Change. Glencoe-McGraw-Hill, 2005.

Solutions Manual Chemistry: Matter and Change. Glencoe-McGraw-Hill, 2005.

Solving Problems: A Chemistry Handbook for Chemistry: Matter and Change. Glencoe-McGraw-Hill, 2005.

Supplemental Problems for Chemistry: Matter and Change. Glencoe-McGraw-Hill, 2005.

Block Scheduling Lesson Plans for Chemistry: Matter and Change. Glencoe-McGraw-Hill, 2005.

Reviewing Chemistry: The Princeton Review for Chemistry: Matter and Change. Glencoe-McGraw-Hill, 2005.

Chapter Assessment for Chemistry: Matter and Change. Glencoe-McGraw-Hill, 2005.

Transparency Masters for Merrill Chemistry. Glencoe-McGraw-Hill, 1993.

ACADEMIC SUPPORT: Individual Modification according to the Students’ IEP, 504 plan

Graphic Organizers/Visual Aids

Accommodations for Gifted and Talented Students Hands on Materials Preferred Seating Outlining Test Modifications Partner/ Peer teams Student Notebook and Lab. Journal TECHNOLOGY RESOURCES:

Computers Video Tapes Television Video Discs VCR and DVD CD ROM Programs Overhead Projector/Projecturals

METHODS OF ASSESSMENT: Tests/Quizzes Lab Reports Notebook Requirements Worksheets Classroom Participation Interest and Attentiveness Final Examination

4/9/14 2



Chemistry A

Grade: 10-12

CONTENT: NUCLEAR CHEMISTRY

Natural and Artificial Nuclear Reactions Instruments Used to Prepare, Study, Control and Use Radioactive Materials and Nuclear Processes Half-Life

Calculations of Half-Lives of Radioactive Substances Nuclear Equations Nuclear Power-Pros and Cons

FRAMEWORKS/CURRICULUM STANDARDS: NUCLEAR CHEMISTRY

2.8 Describe alpha, beta, and gamma particles; discuss the properties of alpha, beta, and gamma radiation; and write balanced nuclear reactions.

2.9 Compare nuclear fission and nuclear fusion and mass defect. * 2.10 Describe the process of radioactive decay as the spontaneous breakdown of

certain unstable elements (radioactive) into new elements (radioactive or not) through the spontaneous emission by the nucleus of alpha or beta particles. Explain the difference between stable and unstable isotopes.

2.11 Explain the concept of half-life of a radioactive element, e.g. explain why the half-life of C14 has made carbon dating a powerful tool in determining the age of very old objects.


Cloud Chamber Chain Reaction with Dominos Use of Spectrophotometer

Skills Worksheets: Worksheets to reinforce vocabulary Balancing Nuclear Equations Worksheet

Lab Activities: Half-Life Simulation by Radioactive Decay Rate of Radioactive Decay Using a Geiger Counter

INSTRUCTIONAL RESOURCES: CHEMISTRY Text Chemistry- A Modern Course. Merrill, 1990. Lab Manual Chemistry- A Modern Course. Merrill, 1990. CHEMISTRY A Text Chemistry: Matter and Change. Glencoe-McGraw-Hill, 2005. Lab Manual Chemistry: Matter and Change Laboratory Manual. Glencoe-




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Chemistry A

Grade: 10-12


















4/9/14 4



Chemistry A

Grade: 10-12

CONTENT: THE STRUCTURE OF MATTER

Development of Modern Atomic Theory Laws of Multiple Proportions and Definite Proportions Major Subatomic Particles

Electron Configuration Periodic Table Group of Elements

FRAMEWORKS/CURRICULUM STANDARDS: ATOMIC STRUCTURE

2.1 Trace the development of atomic theory and the structure of the atom from the ancient Greeks to the present (Dalton, Thompson, Rutherford, Bohr, and modern theory).

2.2 Interpret Dalton’s atomic theory in terms of the Laws of Conservation of Mass, Constant Composition, and Multiple Proportions.

2.3 Identify the major components of the nuclear atom (protons, neutrons, and electrons) and explain how they interact. *

2.4 Understand that matter has properties of both particles and waves. 2.5 Using Bohr’s model of the atom interprets changes (emission/absorption) in

electron energies in the hydrogen atom corresponding to emission transitions between quantum levels.

2.6 Describe the electromagnetic spectrum in terms of wavelength and energy; identify regions of the electromagnetic spectrum.

2.7 Write the electron configurations for elements in the first three rows of the periodic table.

PERIODICITY 3.1 Explain the relationship of an element’s position on the periodic table to its

atomic number and mass* 3.2 Use the periodic table to identify metals, nonmetals, metalloids, families

(groups), periods, valence electrons, and reactivity with other elements in the table.

3.3 Relate the position of an element on the periodic table to its electron configuration.

3.4 Identify trends on the periodic table (ionization energy, electronegativity, electron affinity, and relative size of atoms and ions).


How small is an atom? (Balloon with vanilla flavoring) Use of Spectrophotometer

Skills Worksheets: Worksheets for Chapters 7,5,12,9,10, and 11

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Chemistry A

Grade: 10-12

Lab Activities:

Identifying elements through flame tests Continuous-Emission Spectra differences Electron Configuration Periodic Table Periodicity and Chemical Reactivity #19, The Activity Groups 1,2, and 17

INSTRUCTIONAL RESOURCES: CHEMISTRY Text Chemistry- A Modern Course. Merrill, 1990. Lab Manual Chemistry- A Modern Course. Merrill, 1990. Video The Atom CHEMISTRY A Text Chemistry: Matter and Change. Glencoe-McGraw-Hill, 2005. Lab Manual Chemistry: Matter and Change Laboratory Manual. Glencoe-
















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Chemistry A

Grade: 10-12






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Chemistry A

Grade: 10-12

CONTENT: INTERACTIONS OF MATTER

Chemical Formulas Naming Compounds – What is the MOLE? Oxidation Number for Monatomic and Polyatomic Icons Molecular and Empirical Formulas

Structure of Organc and Inorganic Nolecules Chemical Equations – Writing and Balancing Types of Chemical Reactions

FRAMEWORKS/CURRICULUM STANDARDS: CHEMICAL BONDING

4.1 Explain how atoms combine to form compounds through both ionic and covalent bonding. *

4.2 Draw Lewis dot structures for simple molecules. 4.3 Relate electronegativity and ionization energy to the type of bonding an

element is likely to undergo. 4.5 Identify the types of intermolecular forces present based on molecular

geometry and polarity. 4.6 Predict chemical formulas based on the number of valence electrons. 4.7 Name and write the chemical formulas for simple ionic and molecular

compounds, including those that contain common polyatomic ions. 5.4 Determine molar mass, percent compositions, empirical formulas, and

molecular formulas. 5.5 Calculate mass-mass, mass-volume, volume-volume, and limiting reactant

problems for chemical reactions. 5.6 Calculate percent yield in a chemical reaction.

INSTRUCTIONAL METHODOLOGIES: Lectures Readings Videos Directed Questioning

Names and Symbols of Elements Combining Elements to Form Compounds Writing Chemical Formulas Ions-Relationship to Oxidation Number Relate Coefficients to Formula Units

Demonstrations Use Models (VSEPR) to Understand Molecular Structure Electron Pair Repulsions with Balloon Model Sigma & Pi Bonds (Two Different Colored Trans. Sheets)

Skills Worksheets: Lab Activities:

Experiment #6- Writing Formulas and Oxidation Numbers Foam Ball and Toothpicks- Model multiple molecular bonds Demo. 6:3 p. 966, Four Main Types of Chemical Reactions Experiment #7- Chemical Changes and Equations Lab #10- Quantitative Study of a Reaction Experiment #11- Mole Relationship in a Chemical Reaction

4/9/14 8



Chemistry A

Grade: 10-12



















Accommodations for Gifted and Talented Students

Hands on Materials

Preferred Seating Outlining Test Modifications Partner/ Peer teams

Student Notebook and Lab. Journal

4/9/14 9



Chemistry A

Grade: 10-12

TECHNOLOGY RESOURCES:



4/9/14 10



Chemistry A

Grade: 10-12

CONTENT: STOICHIOMETRY

Molecular Mass and Formula Mass Calculations- Hydrates Avogadro Number, The Molecular Molar Mass, Molarity of Solutions Percentage Composition- Enthalpy- Entropy- Free Energy- Energy in Chemical Systems

FRAMEWORKS/CURRICULUM STANDARDS: CHEMICAL REACTIONS AND STOICHIOMETRY

5.1 Balance chemical equations by applying the law of conservation of mass. * 5.2 Recognize synthesis, decomposition, and single displacement, double

displacement, and neutralization reactions. 5.3 Understand the mole concept in terms of number of particles, mass, and

gaseous volume. 5.4 Determine molar mass, percent compositions, empirical formulas, and

molecular formulas. 5.1 Calculate mass-mass, mass-volume, volume-volume, and limiting reactant

problems for chemical reactions. 5.6 Calculate percent yield in a chemical reaction.

10.1 Interpret the law of conservation of energy. 10.2 Explain the relationship between energy transfer and disorder in the universe. 10.3 Analyze the energy changes involved in physical and chemical processes using

calorimetry. 10.4 Apply Hess’s law to determine the heat of reaction.

INSTRUCTIONAL METHODOLOGIES: Lectures Readings Videos Directed Questioning

Calculations for Molecular and Formula Mass Use of Avogadro Constant to Define the mole. Calculate Molarity of Solutions, Percentage Composition and Empirical Formulas Using Molar Masses Formula for Hydrates

Demonstrations Enthalpy, Entropy and Free Energy- Concepts and Relationships Hess’s Law- Use of a map and airline flights

Skills Worksheets: Lab Activities:

Exp. #7- Quantitative Determination of an Empirical Formula Exp. #8- Make Hydrated Crystals Exp. #31- Demonstrate Enthalpy and Exp. #30- Demonstrate Entropy Design a Simple Colorimeter- Analyze energy changes and calculate the heat produced by a chain


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Chemistry A

Grade: 10-12



















Hands on Materials


Student Notebook and Lab. Journal TECHNOLOGY RESOURCES:


4/9/14 12



Chemistry A

Grade: 10-12

METHODS OF ASSESSMENT:

Tests/Quizzes Lab Reports Notebook Requirements Worksheets Classroom Participation Interest and Attentiveness Final Examination

4/9/14 13



Chemistry A

Grade: 10-12

CONTENT: KINETIC THEORY

Relationship to Behavior of Gases Boyle’s Charles’, Dalton’s, and Graham’s Laws

FRAMEWORKS/CURRICULUM STANDARDS: KINETIC THEORY

6.1 Using the kinetic molecular theory, explain the relationship between pressure and volume (Boyle’s law), volume and temperature (Charles’ law), and the number of particles in a gas sample (Avogadro’s hypothesis).

6.2 Explain the relationship between temperature and average kinetic energy. 6.3 Perform calculations using the ideal gas law. 6.4 Describe the conditions under which a real gas deviates from ideal behavior.

6.5 Interpret Dalton’s empirical Law of Partial Pressures and use it to calculate partial pressures and total pressures.

6.6 Use the combined gas law to determine changes in pressure, volume, or temperature

INSTRUCTIONAL METHODOLOGIES: Lectures Readings Videos Directed Questioning Demonstrations Skills Worksheets: Lab Activities:

Making a Working Model of Boyle’s and Charles’ Law Temperature Versus Kinetic Energy










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Chemistry A

Grade: 10-12











Hands on Materials


Student Notebook and Lab. Journal TECHNOLOGY RESOURCES:



4/9/14 15



Chemistry A

Grade: 10-12

CONTENT: SOLUTIONS ACIDS AND BASES FRAMEWORKS/CURRICULUM STANDARDS: SOLUTIONS

7.1 Describe the process by which solutes dissolve in solvents. * 7.2 Identify and explain the factors that affect the rate of dissolving, i.e.,

temperature, concentration, and mixing. * 7.3 Describe the dynamic equilibrium that occurs in saturated solutions. 7.4 Calculate concentration in terms of molarity, and percent by mass. 7.5 Use a solubility curve to determine saturation values at different temperatures. 7.6 Calculate the freezing point depression and boiling point elevation of a

solution. 7.7 Write net ionic equations for precipitation reactions in aqueous solutions.

ACIDS AND BASES 8.1 Define Arrhenius’ theory of acids and bases in terms of the presence of

hydronium and hydroxide ions, and Bronsted’s theory of acids and bases in terms of proton donor and acceptor, and relate their concentrations to the pH scale. *

8.2 Compare and contrast the nature, behavior, concentration and strength of acids and bases.

a. Acid-base neutralization b. Degree of dissociation or ionization c. Electrical conductivity

8.3 Identify a buffer and explain how it works. 8.4 Explain how indicators are used in titrations and how they are selected. 8.5 Describe an acid-base titration. Identify when the equivalence point is reached

and its significance. 8.6 Calculate the pH or pOH of aqueous solutions using the hydronium or

hydroxide ion concentration INSTRUCTIONAL METHODOLOGIES:

Lectures Readings Videos Directed Questioning Demonstrations Skills Worksheets:

Comparison of Arrhenius’ Theory and Bronsted’s Theory of Acids and Bases Lab Activities:

Various Solutes and Their Dissolving Times Acid/ Base Neutralization Buffers and How They Work Titration pH Identification

INSTRUCTIONAL RESOURCES: CHEMISTRY Text Chemistry- A Modern Course. Merrill, 1990. Lab Manual Chemistry- A Modern Course. Merrill, 1990.

4/9/14 16



Chemistry A

Grade: 10-12

CHEMISTRY A Text Chemistry: Matter and Change. Glencoe-McGraw-Hill, 2005. Lab Manual Chemistry: Matter and Change Laboratory Manual. Glencoe-




















4/9/14 17



Chemistry A

Grade: 10-12

METHODS OF ASSESSMENT:

Tests/Quizzes Lab Reports Notebook Requirements Worksheets Classroom Participation Interest and Attentiveness Final Examination

4/9/14 18



Chemistry A

Grade: 10-12

CONTENT: REACTION RATE

Causes of Reversible Reactions Factors the Affect the Rate of Reaction

Chemical Equilibrium Le Chatelier’s Principle Activation Energy

Activation Energy’s Role in a Chemical Reaction FRAMEWORKS/CURRICULUM STANDARDS: EQUILIBRIUM AND KINETICS

9.1 Write the equilibrium expression and calculate the equilibrium constant for a reaction.

9.2 Predict the shift in equilibrium when the system is subjected to a stress (LeChatelier’s principle).

9.3 Identify the factors that affect the rate of a chemical reaction (temperature, concentration) and the factors that can cause a shift in equilibrium (concentration, pressure, volume, temperature).

9.4 Explain rates of reaction in terms of collision frequency, energy of collisions, and orientation of colliding molecules.

9.5 Define the role of activation energy in a chemical reaction. INSTRUCTIONAL METHODOLOGIES:

Lectures Readings Videos Directed Questioning Demonstrations Skills Worksheets: Lab Activities:









Study Guide for Content Mastery Teacher Edition Chemistry: Matter 4/9/14 19



Chemistry A

Grade: 10-12

and Change. Glencoe-McGraw-Hill, 2005. Solutions Manual Chemistry: Matter and Change. Glencoe-McGraw-

Hill, 2005. Solving Problems: A Chemistry Handbook for Chemistry: Matter and

Change. Glencoe-McGraw-Hill, 2005. Supplemental Problems for Chemistry: Matter and Change. Glencoe-

McGraw-Hill, 2005. Block Scheduling Lesson Plans for Chemistry: Matter and Change.

Glencoe-McGraw-Hill, 2005. Reviewing Chemistry: The Princeton Review for Chemistry: Matter

and Change. Glencoe-McGraw-Hill, 2005. Chapter Assessment for Chemistry: Matter and Change. Glencoe-

McGraw-Hill, 2005. Transparency Masters for Merrill Chemistry. Glencoe-McGraw-Hill,

1993. ACADEMIC SUPPORT: Individual Modification according to the Students’ IEP, 504 plan





4/9/14 20



Chemistry A

Grade: 10-12

CONTENT: OXIDATION-REDUCTION

Reactions Assign Oxidation Numbers Balance Redox Equations

ELECTROCHEMISTRY Voltaic and Electrolytic Cells Voltage of Cells

FRAMEWORKS/CURRICULUM STANDARDS: OXIDATION-REDUCTION ELECTROCHEMISTRY

11.1 Describe the chemical processes known as oxidation and reduction. 11.2 Assign oxidation numbers. 11.3 Balance oxidation-reduction equations by using half-reactions. 11.4 Identify the components, and describe the processes that occur in an

electrochemical cell. 11.5 Explain how a typical battery, such as a lead storage battery or a dry cell,

works. 11.6 Compare and contrast voltaic and electrolytic cells and their uses. 11.7 Calculate the net voltage of a cell given a table of standard reduction potentials

INSTRUCTIONAL METHODOLOGIES: Lectures Readings Videos Directed Questioning Demonstrations Skills Worksheets: Lab Activities:










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Chemistry A

Grade: 10-12













4/9/14 22

Documents

Science Topic/Unit: Chemistry/Chemistry A – Acids and ... Science/H… · Chapter Vocabulary . ... Percent water in a Hydrate ... Determine the empirical and molecular formula of