1 Day for Review but the objective is embedded and Ongoing throughout the Semester. What is chemistry? How do scientists solve problems?

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1 Goal 1: The learner will develop abilities necessary to do and understand scientific inquiry. Objective Essential Questions/Extended Content Suggested Activities # Days Design, conduct, and analyze investigations to answer questions related to chemistry. Identify questions and suggest hypotheses. Identify variables Use a control when appropriate. Select and use appropriate measurement tools Collect and organize date in table, charts, and graphs. Analyze and interpret data. Explain observations. Make inferences and predictions. Explain the relationship between evidence and explanation. Identify how scientists share findings Evaluate reports of scientific investigations from an informed scientifically-literate viewpoint including considerations of: Appropriate samples. Adequacy of experimental controls. Replication of findings. What is chemistry? How do scientists solve problems? How are investigations organized and conducted? Students should be given numerous opportunities to design and conduct experiments within the context of the entire course. Integrate follow-up questions for lab activities and experiment summaries which focus on experiment design and appropriate conclusions. 1 Day for Review but the objective is embedded and Ongoing throughout the Semester 2 days for content specific introduction but objective is embedded and Ongoing

2 Alternative interpretation of the data throughout the Semester 1.03 Evaluate experimental designs with regard to safety and use safe procedures in laboratory investigations: Identify and avoid potential safety hazards given a scenario. Differentiate between safe and unsafe procedures. Use information from MSDS(Material Safety Data Sheets) to assess chemical hazards. What information is necessary for the safe use of chemicals? (H) How much water is needed to raise the ph of a strong acid by one ph unit? (H) What is the impact of ph on various organisms and life? (H) Does ph have an affect on man-made materials? (H) How are organisms used as "bioindicators"? Data sets and experimental outcomes should be presented to students for analysis within the context of the entire course. Each lab activity should include safety hazards and MSDS data as appropriate Embedded and Ongoing throughout the Semester

3 Goal 2: The learner will build an understanding of the structure and properties of matter Objective Essential Questions/Extended Content Suggested Activities # Days Analyze the historical development of the current atomic theory. Early contributions: Democritus and Dalton. The discovery of the electron: Thomson and Millikan The discovery of the nucleus, proton, and neutron: Rutherford and Chadwick. The Bohr model The quantum mechanical model. What is the composition of the atom and what experiments led to this information? How did Rutherford predict the composition of the nucleus? Are the relationships between wavelength, frequency and energy direct or indirect, and what are the explanations for such relationships? How would one explain the diagram of the Bohr model of the hydrogen atom in terms of allowed, discrete energy levels in the emission spectrum? Animations from R Calculations of energies and wavelengths in Bohr Examine the nature of atomic structure. Subatomic particles: protons, neutrons, and electrons. Mass number. Atomic number Isotopes. How can the electron cloud of the atom be described in terms of the probability model? What are the characteristics of the proton, neutron and electron in terms of location, relative charge, and relative mass? What are the symbols for mass number and atomic number? How do you write an isotope using isotopic symbols do these symbols translate into protons, neutrons, and electrons? The Atom Activity What is an Atom? curriculum support activity (pg in instructional material section). O: Calculating average atomic mass of atoms from relative abundance (%) and actual isotopic mass. Mass defect and E=mc² 3

4 2.03 Apply the language and symbols of chemistry. Name compounds using the IUPAC conventions. Write formulas of simple compounds from their names Identify substances using their physical properties. Melting points. Boiling points. Density. Solubility. How could average atomic mass be explained and illustrated? How would you determine the state of matter of a substance and indicate that state in writing? How are binary, ternary, and compounds with polyatomic ions named? What are the names and formulas of common laboratory acids? What are the correct applications for BP, MP, and density from reference table and how can this information be used to find the identity of unknown substances? How can density be calculated? O: ic/-ous method for copper, iron, manganese, mercury, tin, etc. ite/-ate, hypo-/per- with names of polyatomic ions. Names and formulas for other acids Organic nomenclature Density lab: curriculum support activity (starts on pg. 38 in the instructional materials section). Density activity Unknown liquid lab Analyze the basis assumptions of kinetic molecular theory and its applications: Ideal Gas Equation. Combined Gas Law. Dalton s Law of Partial Pressures. How can solubility rules (and solubility vs. temperature) be used to identify substances and make simple calculations about the solutions? What are the characteristics of ideal gases? How do you apply general gas solubility characteristics? What are the following formulas and concepts with regard to kinetic molecular theory: STP, Ideal Gas Equation, Combined gas law, Avogadro's law, Dalton's Law, and Vapor pressure of water as a Boyle s Law Lab uses CBL/LabPro technology: Dalton s Law Demonstration and Mg-HCI-Drying a Gas O: Graham s Law Calculate MW from effusion of gases. Calculation of KE of gas molecules. Calculate the distribution 5

5 function of temperature? of speeds as a function of temperature. Relate real gases and the van der Waals equation. Differentiate between ideal gases and real gases (conceptually, no calculations). Be able to explain the Density/MW variations of the Ideal gas equation calculations Assess bonding metals and ionic compounds as related to chemical and physical properties How is the concept of sharing electrons to form a covalent compound applied? How is the location of an atom on the Periodic Table an indicator of bond type? Bonding Type Triangle O: Coulomb s Law (F=kq 1 q 2 /r²) Crystal shapes 5 How are ions formed and which arrangements are most stable? Lattice energies What are cations and anions and how are their charges predicted? How is an ionic bond's intermolecular attraction explained as an electrostatic attraction? How are MP, BP, hardness and conductivity explained with regard to ionic forces? How are MP, BP, malleability, ductility, luster, and conductivity explained with regard to metallic bonding?

6 2.07 Assess covalent bonding in molecular compounds as related to molecular geometry and chemical and physical properties. Molecular Macromolecular Hydrogen bonding and other intermolecular forces (dipole/dipole interaction, dispersion, etc.) VSEPR theory 2.08 Assess the dynamics of physical equilibria. Interpret phase diagrams. Factors that affect phase changes. How do covalent bonds in compounds determine the characteristics of that compound? How is the concept of sharing electrons in a covalent compound explained? What is the difference is a single, double, or triple bond in a diatomic molecule? How would you explain covalent bonding with regard to the following concepts: Carbon bonds Lewis dot diagrams Valence Shell Electron pair Repulsion Theory Electron pairs Linear framework Trigonal planar Tetrahedral framework Bond angles Bond polarity Macromolecules and intermolecular structures H-bonds London dispersion forces Relative strengths (Van der Waals)? What is physical equilibrium? How could phase diagrams be explained for water and carbon dioxide? How can phase changes be related to heating Molecular and intermolecular Bonds Lab Bond-Type Triangle Activity O: Molecular geometries (VSEPR) expanded octet Valence bond theory: hybrid orbitals sigma and pi bond Molecular orbital Theory. Formal charge calculations Additonal macromolecules Dipole moment - conceptual Heat of Fusion Ice Cream Lab O: Calculations with Raoult s Law 3 2

7 and cooling curves? How are phase changes related to temperature and pressure?

8 Goal 3: The learner will build an understanding of regularities in chemistry. Objective Essential Questions/Extended Content Suggested Activities # Days Analyze periodic trends in chemical properties and use the periodic table to predict properties of elements Group (families) Periods. Representative elements (main group) and transition elements Electron configuration and energy levels. Ionization energy Atomic and ionic radii Electronegativity What are Groups (families) on the periodic table and how are elements in groups similar? What are periods on the periodic table? How are electron configuration and energy levels related to groups and periods? What are periodic trends relative to ionization energy, atomic radii, and electronegativity? Periodic Table Mystery Building and using a 3-D Periodic Table Photoelectron Spectroscopy activity O: Electron affinity Examine the shapes of different orbitals Apply the mole concept. Avogadro s number and conversion factors to chemical calculations: Particles to moles. Mass to moles Volume of gas to moles. Molarity of solutions. Empirical and molecular formula. Percent composition How are moles converted to particles and particles to moles? How are moles converted to mass and mass to moles? How is volume converted to moles and moles to volume at STP? How is molarity calculated? How are dilution problems calculated? Observations Copper Chloride and Aluminum Lab O: Molality Write formulas for and name hydrates. 7 How can an empirical formula be calculated

9 for mass or percent using experimental data? 3.03 Calculate quantitative relationships in chemical reactions (stoichiometry): Moles of each species in a reaction Mass of each species in a reaction Volumes of gaseous species in a reaction. How can percent composition be determined from the mass of a given compound? What is the relationship between coefficients in a balanced equation and mole ratios? How can mole ratios from the balanced equation be used to calculate the quantity of one substance in a reaction given the quantity of another substance in the reaction? Investigation involving quantitative mole relationships. Construction of Air Bags Observation: Copper Chloride and Aluminum O. Limiting reactant problems Percent Yield 8

10 Goal 4: The learner will build an understanding of energy changes in chemistry. Objective Essential Questions/Extended Content Suggested Activities # Days Analyze the Bohr model in terms of electron energies in the hydrogen atom. The spectrum of electromagnetic energy. Emission and absorption of electromagnetic energy as electrons change energy levels. What are quanta? How are atoms moved to an excited state and what happens when the atom returns to its ground state? What is a photon and when it is emitted? How are color, frequency, and wavelength of light emitted used to explain the energy of a photon? What is the historical significance of the Bohr model and what are the limitations of the model? Who is Neils Bohr and how was the Bohr model produced? A: Spectrum Lab O: Calculation of wavelengths and energies in Bohr atom Analyze the law of conservation of energy, energy transformation, and various forms of energy involved in chemical and physical processes. Differentiate between heat and temperature. Analyze heating and cooling How can the wave/particle duality of electrons be explained? What are the implications of the law of conservation of mass and energy? How can heating and cooling curves, phase diagrams, and Energy vs. reaction diagrams be interpreted? What are enthalpy, entropy, specific heat Heat of Solution Lab O: Hess s Law calculations (multi-step) Heats of formation Stoichiometric calculations with heat. 2

11 curves. Calorimetry, heat of fusion and heat of vaporization calculations. Endothermic and exothermic processes including interpretation of potential energy Diagrams (energy vs reaction pathway), enthalpy and activation energy Analyze the relationship between entropy and disorder in the universe capacity, temperature, joule, endothermic reactions, exothermic reactions, and catalysts? What is the difference is heat and temperature and how what units are used in the calculations? What is entropy and how would entropy be used to explain phases of matter? What is the tendency for systems with regard to entropy? Phase Change Demonstration O: Understand Gibbs free energy and how it is used to predict spontaneity. Calculations with Delta G = Delta H- Temp. changes Analyze nuclear energy. Radioactivity: characteristics of alpha, beta, and gamma radiation Decay equations for alpha and beta emission. Half-life Fission and fusion What is the difference between alpha, beta, and gamma radiations and what are the damaging affects of each? How can nuclear decay be explained using the terms random event, decay equation, and half-life? What is the difference is fission and fusion? A: "Penny's Lab or M&M Lab O: Calculation with halflife O: Transmutation 2 What are some used of nuclear energy?

12 Goal 5: The learner will develop an understanding of chemical reactions. Objective Essential Questions/Extended Content Suggested Activities # Days Evaluate various types of chemical reactions Analyze reactions by types: single replacement, double replacement (including acid-based neutralization), decomposition, synthesis, and combustion of simple hydrocarbons. Predict products How can single replacement, double replacement, decomposition, synthesis, and combustion reactions be identified? How can reference table rules be used to predict the products of all types of reactants? Reaction Type Demonstration Solubility Rule Activity Evaluate the law of conservation of matter to the balancing of chemical equations. Write and balance formulas and equations Write net ionic equations How are balanced chemical equations written? What are net ionic reactions and how are they written? How are reference tables used to predict and write formulas for equations? 5.03 Identify and predict the indicators Based on the following criteria: precipitate of chemical change: information, product testing, color change, and temperature change, how can a chemical Formu lation of a precipitate change be detected? Evolution of a gas. Color change Absorption or release of heat O: Balancing REDOX reactions by halfreaction method or electron transfer method. Solubility Rule Activity write equations for reactions observed O: Calculate heat of reaction - delta H A: Decomposition NaHCO Test for reaction products of 3 4

13 5.04 Assess the physical and chemical properties of acids and bases General properties of acids and bases. Concentration and dilution of acids and bases. Ionization and the degree of dissociation (strengths) of acids and bases Indicators Acid-base titration ph and poh How are acids and bases distinguished from one another using formulas and chemical properties? What is the difference between Arrhenius acids and bases and Bronsted-Lowry acids and bases? How are concentrations (molarity) of acids and bases determined? What is the difference in concentration and strength? O: Acid-base equilibria: Ka, Kb, Kw Lewis theory Weak acids and weak bases in titrations. Buffer system Henderson-Hasselbalch equation A: An acid-based Titration Lab 6 What is ph and poh and how are they calculated using titration? 5.05 Analyze oxidation/reduction reactions with regard to the transfer of electrons. Assign oxidation numbers to element in REDOX reactions Identify the elements oxidized and reduced Write simple half reactions Assess the practical applications of oxidation and reduction reactions What is an indicator and how is it used to determine ph? How is the oxidation number of an element in a REDOX reaction determined? How are oxidized and reduced elements determined? How are half reaction written to indicate the gain or loss of electrons? What are some practical applications of oxidation/reduction reactions? O: Oxidizing agents, reducing agents Balancing REDOX reactions by half reaction method or electron transfer method. Determine anode and cathode Cell potential calculations 5 A: Electrochemistry Law

14 5.06 Analyze the factors that affect the rates of chemical reactions. The nature of the reactants Temperature Concentration Surface Area Catalyst What is the collision theory? What is the qualitative explanation of a reaction rate? What factors affect reaction rates? How do catalysts work? O: Rate from concentration vs time graph Order of reaction and graphs used to determine order: Rate law, rate constant, overall order. Determine mechanisms from rate law Rate determining step 4 A: Reaction Rates Lab Mr. Potato Inquires

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