WAYNESBORO AREA SCHOOL DISTRICT CURRICULUM - CHEMISTRY

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1 WAYNESBORO AREA SCHOOL DISTRICT CURRICULUM - CHEMISTRY UNIT: Introduction KEY LEARNING(S): UNIT : How is Chemistry important in your life? Reading R11.A.2.1, R11.A.2.2.2, R11.A Math M11.A.1.1.3, M11.A1.2.3, M11.A.2.2.1, M11.A Science S11.A.2.2.1, S11.A.3.1.1, S11.A.3.2.1, S11.C Eligible Content & Skills How is Chemistry important in your life? Why do we study Chemistry? What are areas of research in Chemistry? What steps do scientists use to solve problems? NO. OF : 6 days Matter Chemistry Technology Macroscopic Microscopic Scientific Method Observation Hypothesis Experiment Manipulated Variable Responding Variable Theory Scientific Law Quantitative Qualitative Traditional Application Conservation Production Pollutant Communication Collaboration Analyze Evaluate Calculate Organic Chemistry Inorganic Chemistry Biochemistry Analytical Chemistry Physical Chemistry Pure Chemistry Applied Chemistry

2 UNIT: Matter and Change (chapter 1) KEY LEARNING(S): matter, mixtures, changes, law of conservation of matter UNIT : How does matter undergo physical and chemical changes? CHEM.A.1.1 Identify and describe how observable and measurable properties can be used to classify and describe matter and energy. CHEM.A.1.2 Compare the properties of mixtures. Reading R11.A.2.1, R11.A.2.2.2, R11.A Math M11.A.1.1.3, M11.A.1.2.3, M11.A.2.2.1, M11.A Science S11.A.2.2.1, S11.A.3.1.1, S11.A.3.2.1, S11.C Eligible Content & Skills CHEM.A Classify physical or chemical changes within a system in terms of matter and/or energy. CHEM.A Classify observations as qualitative and/or quantitative. CHEM.A Differentiate between homogeneous and heterogeneous mixtures (e.g., how such mixtures can be separated). SAS EQ: what are the difference between pure substances and mixtures? How are changes in matter accompanied by changes in energy? Local EQ: How are physical properties and physical changes of matter related? How can the different types of mixtures be separated? How do elements, compounds, and mixtures differ? How can you identify that a chemical change has occurred? NO. OF : 12 days Matter Mixture Pure Substance Molecule Compound Element Atom Subscript Reactants Solution Alloy Heterogeneous Homogeneous Volume Mass Filtration Physical properties Physical change Chemical properties Chemical change Reaction Vapor Chemical symbol Reversible Irreversible Classify Formula Chemical symbol Law of Conservation of Mass Distillation Extensive Properties Intensive Properties Precipitate

3 UNIT: Matter and Change NO. OF : 12 KEY LEARNING(S): matter, mixtures, changes, law of conservation of matter UNIT : How does matter undergo physical and chemical changes? CONCEPT FORMATIVE ASSESSMENTS SUMMATIVE ASSESSMENTS SUGGESTED INSTRUCTIONAL ACTIVITIES Exit Pass Google Form Padlet Chemistry in a Bag Lab Matter Map Chapter 1 Assessment Chemistry in a Bag Lab Matter Concept Map

4 UNIT: Scientific Measurement KEY LEARNING(S): conversions, metrics, significant figures, density, SI measurement UNIT : How is measurement applied to science? CHEM.A.1.1 Identify and describe how observable and measurable properties can be used to classify and describe matter and energy. Reading R11.A.2.1, R11.A.2.2.2, R11.A Math M11.A.1.1.2, M11.A.2.2.1, M11.A Science S11.A.2.2.1, S11.A.3.1.2, S11.A.3.2.1, S11.C Eligible Content & Skills CHEM.A Utilize significant figures to communicate the uncertainty in a quantitative observation. SAS EQ: What are the differences between pure substances and mixtures? Local EQ: How are accuracy and precision different? How does measurement error affect a calculation? How do significant figure rules affect calculations? What are basic units of the SI system? What are the prefixes and their values? How is dimensional analysis used to make unit conversions? How is density determined? How can graphs, equations, and models be used to analyze systems? NO. OF : 16 days Measurement Scientific notation Accuracy Precision Accepted Value Experimental Value Percent error SI system Weight Celsius Conversion Factor Dimensional Analysis Density Error International System of units Length Volume Mass Scale Temperature Energy Converting Significant Figures Kelvin Absolute Zero

5 UNIT: Scientific Measurement NO. OF : 16 KEY LEARNING(S): conversions, metrics, significant figures, density, SI measurement UNIT : How is measurement applied to science? CONCEPT FORMATIVE ASSESSMENTS SUMMATIVE ASSESSMENTS SUGGESTED INSTRUCTIONAL ACTIVITIES Exit Slips Google Forms Padlet Conversions Graphics Worksheet (with conversion factor pictures) Sugar Content of Beverages Lab Report Chapter 2 Assessment(s) Sugar Content of Beverages (Density) lab Conversion Quest Sig. Fig/Scientific Notation Quiz Test concentrating on dimensional analysis

6 UNIT: Atomic Structure KEY LEARNING(S): atomic structure: parts, number, and location, atomic models, average atomic mass UNIT : How has the model of the atom changed over time? CHEM.A.1.1 Identify and describe how observable and measurable properties can be used to classify and describe matter and energy. CHEM.A.2.1 Explain how atomic theory serves as the basis for the study of matter. Reading R11.A.2.1, R11.A.2.2.2, R11.A Math M11.A.1.1.3, M11.A.2.2.1, M11.A Science S11.A.2.2.1, S11.A.3.1.1, S11.A.3.2.1, S11.C.1.1.1, S11.C Eligible Content & Skills CHEM.A Relate the physical properties of matter to its atomic or molecular structure. CHEM.A Describe the evolution of atomic theory leading to the current model of the atom based on the works of Dalton, Thomson, Rutherford, and Bohr. CHEM.A Differentiate between the mass number of an isotope and the average atomic mass of an element. SAS EQ: In what ways has the theory of the atom changed over time due to technological improvements? What are the difference between pure substances and mixtures? How are changes in matter accompanied by changes in energy? LOCAL EQ: What were the contributions of Democritus and Dalton to the atomic theory? What were the contributions of Thompson and Rutherford to the atomic theory? How are the three types of subatomic particles different from one another? How is the identity of an atom affected by each subatomic particle? How is atomic mass different from mass number? NO. OF : 12 days Atom Electrons Protons Neutrons Nucleus Atomic Number Mass Number Isotopes Period Group Model Indivisible Indestructible Theory Particles Average Weighted Dalton s Atomic Theory Cathode Ray Atomic Mass Unit Average Atomic Mass Periodic Table

7 UNIT: Atomic Structure NO. OF : 12 KEY LEARNING(S): atomic structure: parts, number, and location, atomic models, average atomic mass UNIT : How has the model of the atom changed over time? CONCEPT FORMATIVE ASSESSMENTS SUMMATIVE ASSESSMENTS SUGGESTED INSTRUCTIONAL ACTIVITIES Exit Slips Google Forms Padlet Atom/Ion/Isotope Model Atomic Structure Illustration visually display location of protons, neutrons, and electrons in a diagram Chapter 3 Assessment Element Builder Gizmo (simulation lab) Atomic Timeline Atomic Mass of Candium Lab Atom/Ion/Isotope Model

8 UNIT: Electrons KEY LEARNING(S): Quantum numbers, electron configuration, orbital diagram, light properties UNIT : How are electrons arranged in an atom? CHEM.A.2.1 Explain how atomic theory serves as the basis for the study of matter. CHEM.A.2.2 Describe the behavior of electrons in atoms. Reading R11.A.2.1, R11.A.2.2.2, R11.A Math M11.A.1.1.2, M11.A.2.2.1, M11.A Science S11.A.1.1.4, S11.A.1.1.5, S11.A.3.2.3, S11.C.1.1.2, S11.C Eligible Content & Skills CHEM.A Describe the evolution of atomic theory leading to the current model of the atom based on the works of Dalton, Thomson, Rutherford, and Bohr. CHEM.A Predict the ground state electronic configuration and/or orbital diagram for a given atom or ion. CHEM.A Predict characteristics of an atom or an ion based on its location on the periodic table(e.g., number of valence electrons, potential types of bonds, reactivity). CHEM.A Explain the relationship between the electron configuration and the atomic structure of a given atom or ion (e.g., energy levels and/or orbitals with electrons, distribution of electrons in orbitals, shapes of orbitals). CHEM.A Relate the existence of quantized energy levels to atomic emission spectra. SAS EQ: How are changes in matter accompanied by changes in energy? How does the distribution of electrons in atoms affect the formation of a compound? In what ways has the theory of the atom changed over time due to technological improvements? LOCAL SAS: How did the Bohr Model and Quantum Mechanical Model change the atomic theory? How does the periodic table reflect quantum numbers? How do the Aufbau principle, Pauli exclusion principle, and Hund s rule determine an element s electron configuration? Why do we see light? NO. OF : 12 days Amplitude Electromagnetic Radiation Frequency Hertz Photons Quantum Spectrum Wavelength Orbital Shell Sublelvel Stable Inversely proportional Ground state (or level) Excited State (or level) Atomic Emission Spectrum (spectra) Aufbau Principle Electron Configuration Energy Levels Hund s Rule Pauli Exclusion Principle Quantum Mechanical Model

9 UNIT: Electrons NO. OF : 12 KEY LEARNING(S): Quantum numbers, electron configuration, orbital diagram, light properties UNIT : How are electrons arranged in an atom? CONCEPT FORMATIVE ASSESSMENTS SUMMATIVE ASSESSMENTS SUGGESTED INSTRUCTIONAL ACTIVITIES Exit Slips Google Forms Padlet Electron Configuration of atom and its common ion Poster Chapter 4 Assessment Spectrum Activity Flame Test lab Electron Configuration Gizmo (lab Simulation) Atomic Timeline

10 UNIT: Periodic Table of the Elements KEY LEARNING(S): predicting properties of the periodic table, periodic law UNIT : How is the periodic table organized? CHEM.A.2.3 Explain how periodic trends in the properties of atoms allow for the prediction of physical and chemical properties. Reading R11.A.2.1, R11.A.2.2.2, R11.A Math M11.A.1.1.3, M11.A.2.2.1, M11.A Science S11.A.2.2.1, S11.A.3.2.3, S11.A.3.3.1, S11.C Eligible Content & Skills CHEM.A Explain how the periodicity of chemical properties led to the arrangement of elements on the periodic table. CHEM.A Compare and/or predict the properties (e.g., electron affinity, ionization energy, chemical reactivity, electronegativity, atomic radius) of selected elements by using their locations on the periodic table and known trends. SAS EQ: How does the distribution of electrons in atoms affect the formation of a compound? LOCAL EQ: How has the Periodic Table been modified since its development? Where are the different groups on the periodic table located? How can the periodic table be used to predict physical and chemical properties of elements? How are trends in atomic size, ionic size, ionization energy, and electronegativity reflected on the periodic table? NO. OF : 12 days Ion Metalloids Metals Nonmetals Semimetals Trend Organizing Groups Families Alkali metal Alkaline Earth Metal Anion Cation Atomic Radius Electronegativity Halogen Inner Transition metal Ionization Energy Noble Gases Periodic Law Representative Elements Transition Metal Periodicity Nuclear Charge Shielding effect

11 UNIT: Periodic Table of the Elements NO. OF : 12 KEY LEARNING(S): predicting properties of the periodic table, periodic law UNIT : How is the periodic table organized? CONCEPT FORMATIVE ASSESSMENTS SUMMATIVE ASSESSMENTS SUGGESTED INSTRUCTIONAL ACTIVITIES Exit Slips Google Forms Padlet Predicting the Density Based on Group Properties Lab Ch. 5 Assessment Graphing of trends activity 3D Trends Model Predicting the Density Lab

12 UNIT: Bonding KEY LEARNING(S): Draw Lewis Structures, build 3-D VSPER theory models, predict polarity UNIT : How are compounds formed? Why do molecules have different shapes? CHEM.B.1.3 Explain how atoms form chemical bonds. CHEM.B.1.4 Explain how models can be used to represent bonding. CHEM.A.1.2 Compare the properties of mixtures. R11.A.2.1, R11.A.2.2.2, R11.A Math M11.A.1.1.3, M11.A.2.2.1, M11.A Science S11.A.1.1.5, S11.A.3.2.3, S11.C Eligible Content & Skills CHEM.B Explain how atoms combine to form compounds through ionic and covalent bonding. CHEM.B Classify a bond as being polar covalent, non polar covalent, or ionic. CHEM.B Use illustrations to predict the polarity of a molecule. CHEM.B Recognize and describe different types of models that can be used to illustrate the bonds that hold atoms together in a compound (e.g., computer models, ball and stick models, graphical models, solid sphere models, structural formulas, skeletal formulas, Lewis dot structures). CHEM.B Utilize Lewis dot structures to predict the structure and bonding in simple compounds. CHEM.A Describe how chemical bonding can affect whether a substance dissolves in a given liquid. SAS EQ: What factors determine the types of chemical bonds that form between particles? How does the distribution of electrons in atoms affect the formation of a compound? LOCAL EQ: How is the octet rule applied to all elements? How do the different types of ions form? How do you draw Lewis dot structures for elements and compounds? How are ionic compounds formed? How are metallic compounds formed? How are alloy different from the elements they are made from? How do the properties of ionic compounds differ from molecular compounds? How are molecular compounds formed? How is VSEPR theory used to determine molecular shape? How does molecular shape affect polarity? NO. OF : 12 days Chemical Formula Ionic Bond Ionic Compound Metallic Bond Octet Rule Covalent Bond Hydrogen Bonds Molecular Compound Molecular Formula Molecule Van der Waal Forces Salt Brittle Ductile Malleable Dissolved Conduct Alloy Diatomic Single bond Double bond Triple bond Electron Dot Structure Formula Unit Halide Ion Valence Electron Diatomic Molecule Dipole Polar Covalent Bond Nonpolar Covalent Bond Polar molecule Polyatomic ion Unshared pairs VSEPR Theory Shared pair Structural formula

13 UNIT: Bonding NO. OF : 12 KEY LEARNING(S): Draw Lewis Structures, build 3-D VSPER theory models, predict polarity UNIT : How are compounds formed? Why do molecules have different shapes? CONCEPT FORMATIVE ASSESSMENTS SUMMATIVE ASSESSMENTS SUGGESTED INSTRUCTIONAL ACTIVITIES Exit Slips Google Forms Padlet Chapter 6 Assessment VSPER Theory Model Building activity (with pretzels, marshmallows, and m&m s) Polarity Comic Book polar bears & penguins Visible Representation of the 3 Types of Bonds (Venn Diagram, etc.)

14 UNIT: Nomenclature KEY LEARNING(S): naming binary and molecular compounds using the stock naming system UNIT : How are the names of compounds determined? CHEM.A.1.1 Identify and describe how observable and measurable properties can be used to classify and describe matter and energy. CHEM.B.1.2 Apply the mole concept to the composition of matter. Reading R11.A.2.1, R11.A.2.2.2, R11.A Math M11.A.1.1.3, M11.A.2.2.1, M11.A Science S11.A.3.1.1, S11.C.1.1.4, S11.C Eligible Content & Skills CHEM.A Apply a systematic set of rules (IUPAC) for naming compounds and writing chemical formulas (e.g., binary covalent, binary ionic, ionic compounds containing polyatomic ions). CHEM.B Apply the law of definite proportions to the classification of elements and compounds as pure substances. SAS EQ: What are the difference between pure substances and mixtures? LOCAL EQ: How are the different types of ions named? How do you translate between an ionic compound s name and formula? When do ionic compounds need roman numerals in their name? How do you translate between a molecular compound s name and formula? What are the prefixes used in naming molecular compounds? How are acids and bases named differently? How do the laws of definite and multiple proportions describe chemical compounds? NO. OF : 10 days Acid Base Monatomic ion Binary Polyatomic ion Formulas Subscripts Balance Charges Oxidation state Molecular compound Prefix Roman numeral Suffix Law of Definite Proportions Law of Multiple Proportions Nomenclature

15 UNIT: Nomenclature NO. OF : 10 KEY LEARNING(S): naming binary and molecular compounds using the stock naming system UNIT : How are the names of compounds determined? CONCEPT FORMATIVE ASSESSMENTS SUMMATIVE ASSESSMENTS SUGGESTED INSTRUCTIONAL ACTIVITIES Exit Slips Google Forms Padlet Chapter 7 Assessment Compounds Scavenger Hunt ex. Household items to give formula and name (that we have learned about in class)

16 UNIT: Moles KEY LEARNING(S): converting moles, empirical and molecular formulas, percent composition UNIT : How is matter measured? CHEM.B.1.1 Explain how the mole is a fundamental unit of chemistry. CHEM.B.1.2 Apply the mole concept to the composition of matter. Reading R11.A.2.1, R11.A.2.2.2, R11.A Math M11.A.1.1.3, M11.A.2.2.1, M11.A Science S11.A.2.2.1, S11.A.3.1.3, S11.C Eligible Content & Skills CHEM.B Apply the mole concept to representative particles (e.g., counting, determining mass of atoms, ions, molecules, and/or formula units). CHEM.B Determine the empirical and molecular formulas of compounds. CHEM.B Relate the percent composition and mass of each element present in a compound. SAS EQ: How do stoichiometric ratios relate reactants to products in a chemical reaction? LOCAL EQ: Why are moles so important? How is the molar mass determined for elements and compounds? How can a mole be converted into mass, volume, and representative particles? How is percent composition calculated? How is empirical formula determined from percent composition? How is a molecular formula determined from an empirical formula? NO. OF : 14 days Molecules Atoms Ions Convert (ing) Mass Atomic mass Relationship Avogadro s Hypothesis Avogadro s Number Empirical Formula Molar Mass Molar Volume Mole Molecular formula Percent Composition Representative Particle Standard Temperature & Pressure Formula Units Avogadro s number

17 UNIT: Moles NO. OF : 14 KEY LEARNING(S): converting moles, empirical and molecular formulas, percent composition UNIT : How is matter measured? CONCEPT FORMATIVE ASSESSMENTS SUMMATIVE ASSESSMENTS SUGGESTED INSTRUCTIONAL ACTIVITIES Exit Slips Google Forms Padlet Mole Worksheet #2 Mole Project Chapter 9 Assessment Mole Lab: measuring varying units with accuracy Mole Project compare everyday materials to a mole Mole Worksheet #2 (new name TBD) Mole Roadmap picture representation, etc.

18 UNIT: Equations KEY LEARNING(S): writing and balancing equations, identifying the type, predicting the products of SR and DR reactions UNIT : Why is it important to balance and classify chemical reactions? CHEM.B.2.1 Predict what happens during a chemical reaction. Reading R11.A.2.1, R11.A.2.2.2, R11.A Math M11.A.1.1.3, M11.A.2.2.1, M11.A.2.2 Science S11.A.1.3.2, S11.A.2.1.3, S11.A.3.1.2, S11.C Eligible Content & Skills CHEM.B Classify reactions as synthesis, decomposition, single replacement, double replacement, or combustion. CHEM.B Predict products of simple chemical reactions (e.g., synthesis, decomposition, single replacement, double replacement, combustion). CHEM.B Balance chemical equations by applying the Law of Conservation of Matter. SAS EQ: What factors identify the types of chemical reactions? How do stoichiometric ratios relate reactants to products in a chemical reactions? LOCAL EQ: What are the steps in writing a balanced chemical equation? How do the 5 classifications of chemical reactions differ from each other? How are the products of a chemical reaction predicted? NO. OF : 8 days Chemical Equation Coefficients Subscripts Yield Reactants Products Reaction Skeleton equation Catalyst Classify Compound Substance Element Heat Energy Hydrocarbon Balanced Equations Combustion RXN Synthesis RXN Combustion RXN Decomposition RXN Double Replacement RXN Single Replacement RXN Activity series

19 UNIT: Equations NO. OF : 8 KEY LEARNING(S): writing and balancing equations, identifying the type, predicting the products of SR and DR reactions UNIT : Why is it important to balance and classify chemical reactions? CONCEPT FORMATIVE ASSESSMENTS SUMMATIVE ASSESSMENTS SUGGESTED INSTRUCTIONAL ACTIVITIES Exit Slips Google Forms Padlets Chapter 8 Assessment Balancing Blocks Predicting Products Lab students will predict single/double replacement products (some may not react)

20 UNIT: Stoichiometry KEY LEARNING(S): using stoichiometry to solve for reactants & products, limiting reactant, percent yield UNIT : Why is stoichiometry essential to chemistry? CHEM.B.2.1 Predict what happens during a chemical reaction. Reading R11.A.2.1, R11.A.2.2.2, R11.A Math M11.A.1.1.3, M11.A.2.2.1, M11.A Science S11.A.2.2.1, S11.A.3.1.2, S11.C Eligible Content & Skills CHEM.B Describe the roles of limiting and excess reactants in chemical reactions. CHEM.B Use stoichiometric relationships to calculate the amounts of reactants and products involved in a chemical reaction. SAS EQ: How do stoichiometric ratios relate reactants to products in a chemical reaction? LOCAL EQ: How does the mole ratio relate the reactants and products of a chemical equation? How are mole ratios used to predict the amounts of reactants and/or products What is the limiting reactant and how is it determined? NO. OF : 16 days Quantitative Calculate Conservation Mass Mole Volume Predicting Conversion factor Formed Ratio Efficiency Actual Yield Excess Reagent Limiting Reagent Mole Ratio Percent Yield Stoichiometry Theoretical Yield

21 UNIT: Stoichiometry NO. OF : 16 KEY LEARNING(S): using stoichiometry to solve for reactants & products, limiting reactant, percent yield UNIT : Why is stoichiometry essential to chemistry? CONCEPT FORMATIVE ASSESSMENTS SUMMATIVE ASSESSMENTS SUGGESTED INSTRUCTIONAL ACTIVITIES Exit Slips Google Forms Padlet Chapter 9 Assessment(s) Baking Soda Decomposition Lab with accuracy component Recipe to Grocery List Activity apply stoichiometric principles to it

22 (NOT DIRECTLY INCLUDED IN KEYSTONE CONTENT DOCUMENT ) UNIT: States of Matter KEY LEARNING(S): UNIT : How does the kinetic theory apply to solids, liquids, and gases? Eligible Content & Skills Why do gases behave the way they do? How do gases behave differently than liquids? How do gases behave differently than solids? How does a phase diagram represent the changes in states of matter? NO. OF : 2 days Gas Pressure Pressure Atmospheric Pressure Barometer Pascal Model Collisions Elastic Constant Random Motion Insignificant Particles Kinetic energy Kelvin temperature Evaporation Condensation Melting Freezing Boiling Sublimation Deposition Crystal Solid Liquid Gas Kinetic Theory Standard Atmosphere Vapor Pressure Allotropes Amorphous Phase diagram Triple point Critical point

23 UNIT: States of Matter NO. OF : 8 KEY LEARNING(S): UNIT : How does the kinetic theory apply to solids, liquids, and gases? CONCEPT FORMATIVE ASSESSMENTS SUMMATIVE ASSESSMENTS SUGGESTED INSTRUCTIONAL ACTIVITIES

24 UNIT: Gas Laws KEY LEARNING(S): UNIT : What are the relationships between volume, temperature, pressure, and moles of a gas? CHEM.B.2.2 Explain how the kinetic molecular theory relates to the behavior of gases. Reading R11.A.2.1, R11.A.2.2.2, R11.A Math M11.A.1.1.3, M11.A.2.2.1, M11.A Science S11.A.1.1.4, S11.A.2.1.3, S11.A.3.1.2, S11.C Eligible Content & Skills CHEM.B Utilize mathematical relationships to predict changes in the number of particles, the temperature, the pressure, and the volume in a gaseous system (i.e., Boyle s law, Charles s law, Dalton s law of partial pressures, the combined gas law, and the ideal gas law). CHEM.B Predict the amounts of reactants and products involved in a chemical reaction using molar volume of a gas at STP. SAS EQ: In what ways has the theory of the atom changed over time due to technological improvements? LOCAL EQ: How is gas pressure affected? How did Boyle, Charles, and Gay-Lussac describe the relationships among, the temperature, pressure, and volume of a gas? What is the difference between a real and an ideal gas? How can the Ideal Gas Law be applied to stoichiometry? How can partial pressure be used to calculate total pressure? NO. OF : 16 days Evaporation Boiling Point Compressible Inverse Direct Indirect Constant Sum Total Boyle s Law Charles Law Gay-Lussac Law Combined Law Dalton s Law of Partial Pressure Ideal Gas Constant Ideal Gas Law Partial pressure

25 UNIT: Gas Laws NO. OF : 16 KEY LEARNING(S): solve problems using the appropriate gas law equation UNIT : What are the relationships between volume, temperature, pressure, and moles of a gas? CONCEPT FORMATIVE ASSESSMENTS SUMMATIVE ASSESSMENTS SUGGESTED INSTRUCTIONAL ACTIVITIES Exit Slips Google Forms Padlet Chapter 11 Assessment(s) Pressure Temperature Lab Pressure Volume Lab Molar Mass of Butane Lab

26 UNIT: Solubility KEY LEARNING(S): UNIT : How are solutions formed? NO. OF : 10 days CHEM.A.1.2 Compare the properties of mixtures. Reading R11.A.2.1, R11.A.2.2.2, R11.A Math M11.A.1.1.3, M11.A.2.2.1, M11.A Science S11.A.1.1.4, S11.A.2.1.3, S11.A.3.1.2, S11.C Eligible Content & Skills CHEM.A Compare properties of solutions containing ionic or molecular solutes (e.g., dissolving, dissociating). CHEM.A Describe how factors (e.g., temperature, concentration, surface area) can affect solubility. SAS EQ: LOCA EQ: How is solubility affected? How do you read a solubility curve? How are the concentrations of a solution described? Saturated Solution Solubility Unsaturated Solution Supersaturated Solution Concentration Dilute Solution Concentrated Solution Dissolve Agitate Surface area Particle size Units Miscible Immiscible Molarity Percent Mass Percent Volume

27 UNIT: Solubility NO. OF : 10 KEY LEARNING(S): converting among solution units: molarity, % mass, % volume, predicting solubility UNIT : How are solutions formed? CONCEPT FORMATIVE ASSESSMENTS SUMMATIVE ASSESSMENTS SUGGESTED INSTRUCTIONAL ACTIVITIES Exit Slips Google Forms Padlet Chapter 12 Assessments Making a Solubility Curve Activity Solubility Lab Beer s Law Lab copper composition Unsaturated/Saturated/Supersaturated Solutions Lab hand warmers (sodium acetate)

28 (OPTIONAL NOT REQUIRED BY KEYSTONE CONTENT DOCUMENT ) UNIT: Acids and Bases KEY LEARNING(S): UNIT : Why are acid and base reactions important for life? Reading R11.A.2.1, R11.A.2.2.2, R11.A Math M11.A.1.1.3, M11.A.2.2.1, M11.A Science S11.A.1.1.4, S11.A.2.1.3, S11.A.3.1.2, S11.C Eligible Content & Skills How do the properties of acids and bases differ? How can ph be measured? How are strong acids and bases differentiated from weak acids and bases? Why is an acid/base reaction called a neutralization reaction? NO. OF : Strong acid Strong base Weak acid Weak base Neutralization Salt Binary acid Oxyacid Arhenius acid Arhenius base BronstedLlowry Acid Bronsted-Lowry Base Bronssted-Lowry Acid-Base Reaction Monoprotic Acid Polyprotic Acid Diprotic Acid Triprotic Acid Lewis Acid Lewis Base Lewis Acid-Base Reaction Conjugate Acid Conjugate Base Amphoteric

29 UNIT: Acids and Bases NO. OF : KEY LEARNING(S): UNIT : Why are acid and base reactions important for life? CONCEPT FORMATIVE ASSESSMENTS SUMMATIVE ASSESSMENTS SUGGESTED INSTRUCTIONAL ACTIVITIES Exit Slips Google Forms Padlet Chapter 14 Assessment Test ph of Household Items Cabbage Juice ph Indicator

30 COURSE NAME: General Chemistry (OPTIONAL NOT REQUIRED BY KEYSTONE CONTENT DOCUMENT ) UNIT: Nuclear Chemistry KEY LEARNING(S): UNIT : How is nuclear chemistry used in everyday life? Reading R11.A.2.1, R11.A.2.2.2, R11.A Math M11.A.1.1.3, M11.A.2.2.1, M11.A Science S11.A.1.1.4, S11.A.2.1.3, S11.A.3.1.2, S11.C Eligible Content & Skills Why are certain elements radioactive? How are the 3 types of radiation different from each other? How is nuclear energy generated? What are the pros and cons of nuclear fission and fusion? How is radiation detected and used in your life? NO. OF : Nuclear Reaction Radioactive Decay Nuclear Radiation Film Badge Geiger-Muller Counter Radioactive Dating Nuclear Waste Nuclear Fission Chain Reaction Nuclear Reactor Nuclear Power Plant Nuclear Fusion Nucleon Nuclide Mass Defect Nuclear Binding Energy Nculear Shell Model Magic Number Transmutation Radioactive Nuclide Alpha Particle Beta Particle Positron Electron Capture Gamma Ray Half-life Decay Series Parent Nuclide Daughter Nuclide Artificial Transmutation Transuranium Element Roetgen Rem Scintillation Counter Radioactive Tracer Critical Mass Shielding Control Rod Moderator

31 UNIT: Nuclear Chemistry NO. OF : KEY LEARNING(S): UNIT : How is nuclear chemistry used in everyday life? CONCEPT FORMATIVE ASSESSMENTS SUMMATIVE ASSESSMENTS SUGGESTED INSTRUCTIONAL ACTIVITIES Exit Slips Google Forms Padlet Chapter 21 Assessment Student Research & Presentation Areas of Nuclear Chemistry Gizmo Half-life & Radioactive Decay