Unit 3_ Atoms and Atomic Theory by hcj

VIEWS: 70 PAGES: 28

									Chemistry Unit Overviews


                         NATURE OF SCIENCE STANDARDS
                                     9-12


   Indicator 1: Understand the nature and origin of scientific knowledge.

                                  Core HS Standards

   9-12.N.1.1. (Evaluation) Evaluate a scientific discovery to determine and
   describe how societal, cultural, and personal beliefs influence scientific
   investigations and interpretations.

   9-12.N.1.2. (Synthesis) Describe the role of observation and evidence in the
   development and modification of hypotheses, theories, and laws.


   Indicator 2: Apply the skills necessary to conduct scientific investigations.

                                  Core HS Standards

   9-12.N.2.1. (Synthesis) Apply science process skills to design and conduct
   student investigations.

   9-12.N.2.2. (Application) Practice safe and effective laboratory techniques.

                               Advanced HS Standards

   9-12.N.2.1A. (Synthesis) Manipulate multiple variables with repeated trials.

   9-12.N.2.2A. (Evaluation) Use statistical analysis of data to evaluate the validity
   of results.

   9-12.N.2.3A. (Analysis) Demonstrate correct precision in measurements and
   calculations.




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Chemistry Unit Overviews


                         PHYSICAL SCIENCE STANDARDS
                                     9-12


   Indicator 1: Describe structures and properties of, and changes in, matter.

                                  Core HS Standards

   9-12.P.1.1. (Analysis) Use the Periodic Table to determine the atomic structure
   of elements, valence number, family relationships, and regions (metals,
   nonmetals, and metalloids).

   9-12.P.1.2. (Comprehension) Describe ways that atoms combine.

   9-12.P.1.3. (Application) Predict whether reactions will speed up or slow down
   as conditions change.

   9-12.P.1.4. (Application) Balance chemical equations by applying the Law of
   Conservation of Matter.

   9-12.P.1.5. (Comprehension) Distinguish among chemical, physical, and nuclear
   changes.

                               Advanced HS Standards

   9-12.P.1.1A. (Analysis) Distinguish between the changing models of the atom
   using the historical experimental evidence.

   9-12.P.1.2A. (Synthesis) Predict electron configuration, ion formation,
   reactivity, compound formation, periodic trends, and types of compounds formed
   based on location on the Periodic Table.

   9-12.P.1.3A. (Synthesis) Identify five basic types of chemical reactions and
   predict the products.

   9-12.P.1.4A. (Synthesis) Describe factors that affect solution interactions.

   9-12.P.1.5A. (Application) Examine energy transfer as matter changes.

   9-12.P.1.6A. (Application) Perform stoichiometric calculations.

   9-12.P.1.7A. (Application) Apply the kinetic molecular theory to solve
   quantitative problems involving pressure, volume, temperature, and number of



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Chemistry Unit Overviews


   moles of gas.

   9-12.P.1.8A. (Synthesis) Use models to make predictions about molecular
   structure, chemical bonds, chemical reactivity, and polarity of molecules.

   9-12.P.1.9A. (Analysis) Describe the characteristics of equilibria.



   Indicator 3: Analyze interactions of energy and matter.

                                 Core HS Standards

   9-12.P.3.1. (Application) Describe the relationships among potential energy,
   kinetic energy, and work as applied to the Law of Conservation of Energy.




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Chemistry Unit Overviews



                      EARTH/SPACE SCIENCE STANDARDS
                                   9-12


   Indicator 1: Analyze the various structures and processes of the Earth system.

                                Core HS Standards

   9-12.E.1.1. (Comprehension) Explain how elements and compounds cycle
   between living and non-living systems.

   9-12.E.1.2. (Application) Describe how atmospheric chemistry may affect global
   climate.

   9-12.E.1.3. (Analysis) Assess how human activity has changed the land, ocean,
   and atmosphere of Earth.

                             Advanced HS Standards

   9-12.E.1.1A (Application) Explain how elements and compounds cycle between
   living and non-living systems.




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Chemistry Unit Overviews



   SCIENCE, TECHNOLOGY, ENVIRONMENT, AND SOCIETY STANDARDS
                             9-12


   Indicator 1: Analyze various implications/effects of scientific advancement
   within the environment and society.

                                  Core HS Standards

   9-12.S.1.1. (Application) Explain ethical roles and responsibilities of scientists
   and scientific research.

   9-12.S.1.2. (Evaluation) Evaluate and describe the impact of scientific
   discoveries on historical events and social, economic, and ethical issues.

                               Advanced HS Standards
       See note below.


   Indicator 2: Analyze the relationships/interactions among science, technology,
   environment, and society.

                                  Core HS Standards

   9-12.S.2.1. (Evaluation) Describe immediate and long-term consequences of
   potential solutions for technological issues.

   9-12.S.2.2. (Analysis) Analyze factors that could limit technological design.

   9-12.S.2.3. (Synthesis) Analyze and describe the benefits, limitations, cost, and
   consequences involved in using, conserving, or recycling resources.




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Chemistry Unit Overviews



Introduction to Chemistry      Mrs. Tucker

Objectives: By the end of the unit students will be able to….
        List the location of the safety equipment in the science room.
        Identify correct procedures for handling chemicals and equipment.
        Identify the name and use of various lab equipment.
        Analyze a graph (dependent variable, independent variable, meaning, plot
           points, defend appropriate regression model, interpolate, extrapolate, r value,
           r^2 value).
        Distinguish between precise and accurate data.
        Gather accurate data.
        List the steps of the scientific method and explain what each entails.
        Gather observations, construct hypotheses, and modify hypotheses based upon
           observations and tests.
        Describe procedure, observations and results of lab.
        Demonstrate proper techniques for weighing, measuring, transferring, and
           filtering.
        Determine the density of various liquids.
        Convert between metric measurements and English measurements.

SD State Standards
   Indicator 2: Apply the skills necessary to conduct scientific investigations.
   9-12.N.2.1. (Synthesis) Apply science process skills to design and condu ct student
   investigations.
   9-12.N.2.2. (Application) Practice safe and effective laboratory techniques.
   9-12.N.2.3A. (Analysis) Demonstrate correct precision in measurements and
   calculations.




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Chemistry Unit Overviews



Day 1       Hand out syllabus, book, safety rules, internet permission, and expectations.
            Hand out equipment packets. HW: look at equipment and answer the
            questions. Meet your textbook. Read packet #1.
Day 2       Go over lab equipment and purpose, collect expectations and permission
            slips. Do acid in eye demonstration. Equipment packet #2. Dichotomous
            key example. (for lab equipment tomorrow)
Day 3       measurement stations (weighing, equipment, liquids, and separations).Go
            over answers to questions in packets#2. Assign packet #3. Equipment
            dichotomous keys.
Day 4       measurement stations (weighing, equipment, liquids, and separations).Safety
            Quiz. Answers to packet #3.
Day 5       Density of drinks lab. Have students bring their own sample of drink to find
            the density of and they can drink the rest.
Day 6       Quiz over measuring and equipment. Density of drinks lab results to post
            graph on large paper or my computer.
Day 7       Popcorn lab intro-book from library and eat popcorn. Assignment.
Day 8       Popcorn lab
Day 9       Test over measurement, equipment, density of drinks lab and popcorn lab.

?You can pick: density lab or popcorn lab write up after the unit is over. Follow rubric.
Due in 3 days.




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Chemistry Unit Overviews




Unit 2: Atoms and Atomic Theory

Standards:
9-12.N.2.1. Students are able to apply science process skills to design and conduct
student investigations.
9-12.N.2.2. Students are able to practice safe and effective laboratory techniques.


9-12.N.2.3A. Students are able to demonstrate correct precision in measurements
and calculations.

9-12.P.1.1. Students are able to use the Periodic Table to determine the atomic
structure of elements, valence number, family relationships, and regions (metals,
nonmetals, and metalloids).
9-12.P.1.1A. Students are able to distinguish between the changing models of the
atom using the historical experimental evidence.



Day 1     Go over test . Discuss three laws: Law of conservation of mass, law of
          definite proportions, and law of multiple proportions. Page 68. Venn diagram.
Day 2     Discuss models of the atom and how they have changed over the years and
          atomic vocabulary on page 77-83..
Day 3     Finish atomic vocabulary. Introduce the concept of a mole. Group problems
          conversions (spread this out)
Day 4     Partner problems and individual conversion problems. Chapter review due in
          2 days.
Day 5     Chemistry quiz on conversions and atomic vocabulary.
Day 6     Bean Bag isotope Lab. Atomic parts/# worksheet. Lab due tomorrow. Read
          pages 97-103 in your book and outline the pages.
Day 7     Properties of Light ppt. Students can print off ppt if they would like.
Day 8     Introduce quantum numbers and practice
Day 9     Practice with quantum numbers and electron configuration.
Day 10    Flame test pre lab. Students need to identify goal, procedure, hypothesis
          before we begin lab tomorrow. Model how to do a flame test. Reminders of
          safety with Bunsen Burners.
Day 11    Flame tests
Day 12    Review for test. Bingo electron configuration. And ppt reviews.
Day 13    Test




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Chemistry Unit Overviews



Chemistry    Unit 3
Chapter 5 Periodicity

SD State Content Standard:
Physical Science
Indicator 1: Describe structures and properties of, and changes in, matter
         9-12.P.1.1. Students are able to use the Periodic Table to determine the atomic
         structure of elements, valence number, family relationships, and regions (metals,
         nonmetals, and metalloids).
         9-12.P.1.2A. Students are able to predict electron configuration, ion formation,
         reactivity, compound formation, periodic trends, and types of compounds formed
         based on location on the Periodic Table.
         9-12.P.1.6A. Students are able to perform stoichiometric calculations.
Nature of Science
Indicator 2: Apply the skills necessary to conduct scientific investigations.
         9-12.N.2.1. Students are able to apply science process skills to design and
         conduct student investigations.
         9-12.N.2.2. Students are able to practice safe and effective laboratory
         techniques.

Day 1          Go over chapter ¾ tests. Content Reading 5-1: Mendeleev and the
               Periodic Table. HW: Mole Day Project
Day 2          Work on Mole Day Project (National Mole Day 6.022 x 1023 October
               23rd
Day 3          5-1 Review worksheets. List of elements to memorize. Elements EC
               crossword. Due on test day.
Day 4          JigSaw activity: periodic table characteristics. HW: Correctly identify
               mystery elements based upon characteristics.
Day 5          It’s In the Cards Lab go over mystery elements.
Day 6          Its’ In the Cards Lab. Discuss results of the lab. Discuss atomic radius,
               electronegativity, ionization energy, electron affinity, ionic radii, valence
               electrons. Read and fill out vocabulary cards and definitions book, me ,
               group picture?
Day 7          Video: Periodic Table. Vocabulary practice activity
Day 8          Periodic Trends Activity: math work first, then cut straws.
Day 9          Quiz over material covered thus far. Periodic Trends Activity, finish
               cutting straws and write conclusions.
Day 10         Periodic Trends Activity assess each group’s work.
Day 11         Quiz over vocabulary, conversions. Work on chapter review, STP
               assignment in class.
Day 12         Review for test
Day 13         Test. EC elements crossword due today.


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Chemistry Unit Overviews



Unit 4
Chapter 6 Chemical Bonding

Goals:
Describe why atoms bond together.
Define chemical bond, ionic bond, and covalent bond.
Define electronegativity.
Calculate the difference in two atoms’ electronegativities in order to estimate their degree
of ionic or covalent bonding.
Correctly represent a partial charge with the appropriate symbol.
Describe the difference between nonpolar covalent bond and polar covalent bond.
Define molecule and molecular formula.
Explain the relationships among potential energy, distance between approaching atoms,
bond length, and bond energy.
State the octet rule.
Be able to write Lewis dot structures of atoms with single bonds, double bonds, and triple
bonds.
Explain how resonance is used to represent some compounds.
Compare and contrast a chemical formula for a molecular compound with one for an
ionic compound.
Discuss the arrangements of ions in crystals.
Define lattice energy and explain its significance.
List and compare the distinctive properties of ionic and molecular compounds.
Write the Lewis dot structure for a polyatomic ion given the identify of the atoms
combined and other appropriate information.
Compare and contrast ionic compound characteristics and covalent compound
characteristics.
Given a compound predict whether the compound is held together by a covalent bond or
ionic bond.
Describe the type of bond within a polyatomic ion.
Describe the electron sea model of metallic bonding and explain why metals are good
electrical conductors.
Explain why metal surfaces are shiny.
Explain why metals are malleable and ductile, but ionic crystalline compounds are not.
Explain VSEPR theory.
Predict the shapes of molecules of polyatomic ions using VSEPR theory.
Explain how the shapes of molecules are accounted for by hybridization theory.
Describe dipole-dipole forces, hydrogen bonding, induced dipoles, and London
dispersion forces and their effects on properties such as boiling and melting points.
Explain what determines molecular polarity.
Perform mole-gram-atoms calculations.




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Chemistry Unit Overviews




Standards:

Indicator 1: Describe structures and properties of, and changes in, matter.
              9-12.P. 1.2. Students are able to describe ways that atoms combine.
              9-12.P. 1.2A Students are able to predict electron configuration, ion
              formation, reactivity, compound formation, periodic trends, and types of
              compounds formed based on the location on the Periodic Table.
              9-12.P.1.6A. Students are able to perform stoichiometric calculations.
              9-12.P.1.8A. Students are able to use models to make predictions about
                              molecular structure, chemical bonds, chemical reactivity,
                              and polarity of molecules.

Indicator 2: Apply the skills necessary to conduct scientific investigations.
              9-12.N.2.1. Students are able to apply science process skills to design and
                               conduct student investigations.
              9-12.N.2.2. Students are able to practice safe and effective laboratory
                               techniques.



Unit Plan
Day 1        Go over tests from last chapter. Content Reading lesson as pre-homework
             for the chapter. Advance Organizer discussing types of bonding and using
             electronegativities to calculate ionic or covalent bonding pattern. Section 6-
             1. HW: section 6-1 review questions or 6-1 review worksheet.
Day 2        Correct 6-1 questions. Puzzle pieces activity worksheet. Describe
             differences between covalent and ionic bonds (prior knowledge and
             discovery). HW: naming whether compounds are held together by ionic or
             covalent bonds.
Day 3        Section 6-2. Definitions of vocabulary. Why do covalent bonds form?
             What are characteristics of covalent bonds? The octet rule. Electron Dot
             notation. Lewis dot structures. HW: electron dot and lewis dot structures.
Day 4        Section 6-2: Single bonds, double bonds, triple bonds, resonance structures,
             covalent network bonding. Section 6-2 review worksheet.
Day 5        Quiz: vocab. Lab: ionic vs. covalent bonds.
Day 6        Lab ionic vs. covalent bonds. Solids lab
Day 7        Section 6-3. Vocabulary. Formation of Ionic Compounds. Characteristics of
             ionic bonding, polyatomic ions. HW: section 6-3 review worksheet
Day 8        Writing compounds practice. Identifying bonds practice.
Day 9        Quiz. Metallic Bonding: Section6-4 Vocab
Day 10       Section 6-5 VSEPR theory. Explain the VSEPR theory. Predict the
             molecular geometry of compounds. VSEPR theory and unpaired electrons.
Day 11       Section 6-5 VSEPR theory. Hybridization. Intermolecular forces.


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Chemistry Unit Overviews


           Molecular polarity and dipole dipole forces. Review
Day 12     Demonstrations. Hydrogen bonding, London dispersion forces. Review 6-5
           worksheet.
Day 13     Station Review: vocabulary, covalent bonds, ionic bonds, metallic bonds,
           molecular geometry, conversions, trends in the periodic table.
Day 14     Station Review: vocabulary, covalent bonds, ionic bonds, metallic bonds,
           molecular geometry, conversions, trends in the periodic table.
Day 15     Chapter review
Day 16     Test




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Chemistry Unit Overviews




Introduction to Naming chemical compounds
Standards
   Indicator 2: Apply the skills necessary to conduct scientific investigations.

                                   Core HS Standards
   9-12.N.2.1. (Synthesis) Apply science process skills to design and conduct student
   investigations.
   9-12.N.2.2. (Application) Practice safe and effective laboratory techniques.
   9-12.N.2.3A. (Analysis) Demonstrate correct precision in measurements and
   calculations.

   Indicator 1: Describe structures and properties of, and changes in, matter.

                                 Core HS Standards

   9-12.P.1.1. (Analysis) Use the Periodic Table to determine the atomic structure
   of elements, valence number, family relationships, and regions (metals,
   nonmetals, and metalloids).

   9-12.P.1.2. (Comprehension) Describe ways that atoms combine.

   9-12.P.1.2A. (Synthesis) Predict electron configuration, ion formation,
   reactivity, compound formation, periodic trends, and types of compounds formed
   based on location on the Periodic Table.

   9-12.P.1.6A. (Application) Perform stoichiometric calculations.


Goals
1. Identify whether a chemical compound contains ionic or covalent bonds.
2. Name ionic compounds, including those with polyatomic ions.
3. Name covalent compounds the old style and the new stock system style.
4. Determine the formula mass of a compound.
5. Determine the molar mass of a compound.
6. Determine the amount in grams of a compound, number of atoms or number of moles.
7. Determine the percent composition of an element in a compound.
8. Determine the empirical formula of a compound.
9. Determine the molecular formula of a covalent compound.
10. Determine oxidation numbers using a set of given rules.




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Chemistry Unit Overviews




Day 1     Go over tests. Discuss Rules for naming ionic compounds and polyatomic
          ions. Do sample problems in the book. Hw naming ionic compounds
Day 2     Finish naming covalent compounds and acids. Do sample problems in the
          book. HW naming covalent compounds
Day 3     Mixed naming review worksheets.
Day 4     Mixed naming practice
Day 5     Determining oxidation numbers given a set of rules. And molecular stock
          system of naming
Day 6     Quiz: naming Revisit the mole concept.
Day 7     Introduce Formula Mass. Problems together then individual. Formula mass,
Day 8     Practice problems. Formula mass, All problem sets will be done in class with
          extras assigned for extra credit opportunity .
Day 9     Practice problems empirical formulas
Day 10    Practice problems empirical formulas
Day 11    Correct and begin next set examples.
Day 12    Practice problems % composition.
Day 13    Practice problems % composition.
Day 14    Correct and begin next set examples.
Day 15    quiz
Day 16    MgO Lab empirical formula.
Day 17    Hydrate lab

Day 18    Mixed Review (naming and problems)
Day 19    Mixed Review (naming and problems)
Day 20    Test

Lab write up for either MgO lab or hydrate lab?




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Chemistry Unit Overviews



Unit: Chemical Reactions

Standards:
   Indicator 2: Apply the skills necessary to conduct scientific investigations.

                                  Core HS Standards

    9-12.N.2.1. (Synthesis) Apply science process skills to design and conduct
    student investigations.

    9-12.N.2.2. (Application) Practice safe and effective laboratory techniques.

    9-12.N.2.3A. (Analysis) Demonstrate correct precision in measurements and
    calculations.


   Indicator 1: Describe structures and properties of, and changes in, matter.

                                  Core HS Standards

    9-12.P.1.1. (Analysis) Use the Periodic Table to determine the atomic structure
    of elements, valence number, family relationships, and regions (metals,
    nonmetals, and metalloids).

    9-12.P.1.2. (Comprehension) Describe ways that atoms combine.

    9-12.P.1.3. (Application) Predict whether reactions will speed up or slow down
    as conditions change.

    9-12.P.1.4. (Application) Balance chemical equations by applying the Law of
    Conservation of Matter.

    9-12.P.1.5. (Comprehension) Distinguish among chemical, physical, and nuclear
    changes.

    9-12.P.1.2A. (Synthesis) Predict electron configuration, ion formation,
    reactivity, compound formation, periodic trends, and types of compounds formed
    based on location on the Periodic Table.

    9-12.P.1.3A. (Synthesis) Identify five basic types of chemical reactions and
    predict the products.




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Chemistry Unit Overviews



Goals:
1. Distinguish between evidence that suggests a chemical reaction may have occurred
    and conclusive proof of a chemical reaction.
2. Use a word equation to describe a chemical reaction.
3. Explain why some reactions are endothermic and others are exothermic.
4. Relate conservation of mass to the rearrangement of atoms in a chemical equation.
5. Explain why reactants must be brought into contact for a reaction to occur.
6. Translate word equations into formula equations and chemical equations.
7. Relate conservation of mass to a balanced equation.
8. Distinguish between coefficients in a chemical equation and subscripts in a chemical
    formula.
9. Properly balance formula equations.
10. Use information from a chemical equation to describe the energy change involved in
    a reaction.
11. List states of matter for reactants and products.
12. Interpret a chemical equation in terms of the relative number of molecules involved
    and the moles of reactants and products.
13. Categorize reactions as belonging to one (or more) of five basic types of chemical
    reactions.
14. Write chemical equations representing each type of chemical reaction.
15. Use an activity series to predict whether a given reactions will occur and what its
    products will be.
16. Given the reactants in the chemical equations predict the products based upon the
    classification of the chemical reaction.
Day 1         Go over tests from last unit. Begin PPT How to balance equations, evidence
              of chemical changes, HW: practice balancing equations
Day 2         Go over practice problems. Word equations and balancing reactions.
Day 3         Practice word equations and balancing equations.
Day 4         Quiz: balancing equations and writing word equations.PPt: How to classify
              equations as combustion, single replacement, double replacement, synthesis,
              or decomposition. Practice HW: classifying equations. Correct balancing
              equations and writing word equations.
Day 5         Bag of reactions lab, Hollow Penny set up
Day 6         Finish bag of reactions lab. Prelab for chemical reactions lab. Hollow penny
              observations.
Day 7         8 Chemical reactions lab
Day 8         8 chemical reactions lab
Day 9         Finish chemical reactions lab. Finish hollow penny and activity series in
              book.
Day 11        Review
Day 12        Test EC cartoon for each type of reaction due.




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Chemistry Unit Overviews


                                         Chemistry
Chapter 9: Stoichiometry

Chapter 9 Goals
Distinguish between composition stoichiometry and reaction stoichiometry.

Solve stoichiometric problems.

Use mole ratios and molar masses to create conversion factors for solving stoichiometry
problems.

Distinguish between a limiting reactant and an excess reactant.

Identify the limiting reactant in a problem, and calculate the theoretical yield.

Use percent yield to calculate actual yield.

Relate volume calculations in stoichiometry to the inflation of automobile safety air bags.

Use the concept of limiting reactants to explain why changing fuel-air ratios affects
engine performance.

Use percent yield to compare the efficiency of pollution-control mechanisms in cars.

Standards Covered:
   Indicator 2: Apply the skills necessary to conduct scientific investigations.

                                    Core HS Standards

    9-12.N.2.1. (Synthesis) Apply science process skills to design and conduct
    student investigations.

    9-12.N.2.2. (Application) Practice safe and effective laboratory techniques.

                                 Advanced HS Standards

    9-12.N.2.3A. (Analysis) Demonstrate correct precision in measurements and
    calculations.


   Indicator 1: Describe structures and properties of, and changes in, matter.

                                    Core HS Standards

    9-12.P.1.1. (Analysis) Use the Periodic Table to determine the atomic structure
    of elements, valence number, family relationships, and regions (metals,



                                                                                         17
Chemistry Unit Overviews


    nonmetals, and metalloids).

    9-12.P.1.4. (Application) Balance chemical equations by applying the Law of
    Conservation of Matter.

    9-12.P.1.5. (Comprehension) Distinguish among chemical, physical, and nuclear
    changes.

                                  Advanced HS Standards

    9-12.P.1.2A. (Synthesis) Predict electron configuration, ion formation,
    reactivity, compound formation, periodic trends, and types of compounds formed
    based on location on the Periodic Table.

    9-12.P.1.3A. (Synthesis) Identify five basic types of chemical reactions and
    predict the products.

    9-12.P.1.5A. (Application) Examine energy transfer as matter changes.

    9-12.P.1.6A. (Application) Perform stoichiometric calculations.

    9-12.P.1.8A. (Synthesis) Use models to make predictions about molecular
    structure, chemical bonds, chemical reactivity, and polarity of molecules.


Outline:
Day 1       Go over last chapter’s tests. Revisit the mole concept and make the “road
            map”
Day 2       Begin mole ratios ppt.
Day 3       Mole ratios ppt and stoichiometry problems together.
Day 4       Chemical Reaction: molar ratios Lab
Day 5       stoichiometry problems together. Assignment on their own.
Day 6       stoichiometry Assignment on their own.
Day 7       stoichiometry Assignment on their own.
Day 8       Limiting Reactants problems: splits, and pizzas. Limiting problems
            together.
Day 9       Limiting Reactant Stoichiometry problems in class
Day 10      Limiting Reactant Stoichiometry problems in class
Day11       Stoichiometric balloons lab
Day 12      Correcting day and sample problems
Day 13      % yield, actual yield, theoretical yield problems together
Day 14      % yield, actual yield, theoretical yield problems
Day 15      Percent yield Lab Day 1
Day 16      Finish percent yield lab day 2% yield, actual yield, theoretical yield problems


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Chemistry Unit Overviews


           in class
Day 17     % yield, actual yield, theoretical yield problems in class
Day 18     Correct % problems and begin review problems
Day 19     Mixed review problems
Day 20     Mixed review problems
Day 21     Correct Mixed review problems
Day 22     test
Day 23     Banana Splits day




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Chemistry Unit Overviews




Unit 10: State of Matter

Standards:
   Indicator 1: Describe structures and properties of, and changes in, matter.

                                   Core HS Standards

    9-12.P.1.4. (Application) Balance chemical equations by applying the Law of
    Conservation of Matter.

    9-12.P.1.5. (Comprehension) Distinguish among chemical, physical, and nuclear
    changes.

                                Advanced HS Standards

    9-12.P.1.5A. (Application) Examine energy transfer as matter changes.

    9-12.P.1.8A. (Synthesis) Use models to make predictions about molecular
    structure, chemical bonds, chemical reactivity, and polarity of molecules.


Goals:
Use the kinetic molecular theory to explain the properties of solids, liquids, and gases.
Differentiate between a real gas and an ideal gas.
Be able to identify a real gas or ideal gas based upon a description.
Be able to define the following words relating to gases: expansion, density, fluidity,
compressibility, diffusion, and effusion.
Place gases in order from the lowest rate of effusion to the greatest or vice versa.
Be able to list characteristics of gases in terms of molecule closeness and speed.
Define a fluid and give two examples.
Define the following words as they relate to liquids: density, incompressibility,
diffusion, surface tension, capillary action, vaporization, boiling, evaporation, and
freezing.
Differentiate between an amorphous solid and a crystalline solid.
Define the following words as they relate to solids: melting, melting point, supercooled
liquids, density, and incompressibility.
Be able to match examples of ionic crystals, covalent network crystals, metallic crystals,
and covalent molecular crystals.
Be able to list a phase change as a physical change.
Be able to describe the changes that occur during melting, freezing, sublimation,
deposition, vaporization (boiling, evaporating), and condensation.
Define equilibrium, equilibrium vapor pressure, volatile liquids.
Describe the intermolecular forces of volatile liquids and nonvolatile liquids.


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Chemistry Unit Overviews


Describe the meanings of molar enthalpy of vaporization and molar enthalpy of fusion.
Distinguish between the two. What are the two a measure of?
Define the critical point and the triple point.
Define the critical temperature and the critical pressure.
Be able to find the critical point and triple points on a phase diagram.
Be able to interpret what changes would occur if the temperature and pressure on a phase
diagram change.
Name two units that are used to measure temperature.
Name two units that are used to measure pressure.
Define pressure as a force per unit area.
List characteristics of water.
Be able to calculate energy absorbed or released during phase changes.
Be able to calculate masses or moles during phase changes.

Plans:
Day 1       Go over last chapter’s tests.
Day 2       How Cool is that Lab: testing evaporation rates of different liquids and
            comparing their intermolecular forces. HW: read 10-1 and fill in follow
            along
Day 3       10-1 ppt and go over follow along
Day 4       Surface tension demonstration. Read 10-2 and fill in follow along for
            liquids.
Day 5       Liquids Lab
Day 6       Phase change ppt and phase change worksheet.
Day 7       10-3 solids ppt, and solids review
Day 8       Changes of State and Phase Diagrams ppt
Day 9       Phase diagrams
Day 10      Water properties
Day 11      Phase Change Lab
Day 12      Water Lab
Day 13      Molar enthalpy of vaporization and molar enthalpy of fusion problems.
Day 14      Molar enthalpy of vaporization and molar enthalpy of fusion problems. Quiz
            over changes in phase and vocabulary
Day 15      Review activities
Day 16      test




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Chemistry Unit Overviews




Gas Laws:
Be able to use the equations:

P=F/A           PV =k           V=kT             PV=nRT        √MB/√MA=rate A/Rate B
                                                      2      2
Pt= P1 + P2…    P1 V1=P2 V2     V1/T1 = V2/T2    1/2Mv =1/2Mv

List the units of pressure, force, area and convert between various units of pressure.
Describe how a barometer works and how it can be used as an altimeter.
Defend applications of Boyle’s Law.
Defend applications of Charles’s Law.
Convert between units of temperature. ( ○C, ○F, K)
Use the chart of R values to figure out which R value is needed based upon the units in
the equation.
Describe the process of diffusion and effusion.
State the relationship between the average molecular velocities of two gases and their
molar masses.
Discuss why helium is placed in scuba tanks.
Explain what the “bends” refers to.
Interpret graphs of various temperatures, pressures and volumes of gases.
Be able to determine R in a gas lab.
List the greenhouse gases and how they contribute to global warming.

   Indicator 2: Apply the skills necessary to conduct scientific investigations.

                                   Core HS Standards

    9-12.N.2.1. (Synthesis) Apply science process skills to design and conduct
    student investigations.

    9-12.N.2.2. (Application) Practice safe and effective laboratory techniques.

                                Advanced HS Standards

    9-12.N.2.1A. (Synthesis) Manipulate multiple variables with repeated trials.

    9-12.N.2.2A. (Evaluation) Use statistical analysis of data to evaluate the validity
    of results.

    9-12.N.2.3A. (Analysis) Demonstrate correct precision in measurements and
    calculations.
        Indicator 1: Describe structures and properties of, and changes in,




                                                                                          22
Chemistry Unit Overviews


         matter.



   9-12.P.1.7A. (Application) Apply the kinetic molecular theory to solve
   quantitative problems involving pressure, volume, temperature, and number of
   moles of gas.

   Indicator 1: Analyze the various structures and processes of the Earth system.

   9-12.E.1.2. (Application) Describe how atmospheric chemistry may affect global
   climate.



Day 1       Go over tests. Discussion Questions 1, 2 on page 368 for Scuba diving.
            Units for pressure, measuring pressure, converting between units, partial
            pressures. Assign 10-1 review. Mustard Gas Reading (not a gas at all)
Day 2       Go over 10-1 review. Gas Laws ppt.
Day 3       Boyle’s law lab HW: boyle’s law problems.
Day 4       Finish boyle’s law lab
Day 5       Gay Lussac’s Law
Day 6       Ideal Gas Law Lab
Day 7       Finish ideal gas law lab and problems.
Day 8       Ideal gas law problem work day
Day 9       Rates of effusion problems
Day 10      Review
Day 11      Test HW: greenhouse gases and global warming.




                                                                                        23
Chemistry Unit Overviews




Unit 12 Solutions
   Indicator 2: Apply the skills necessary to conduct scientific investigations.

                                  Core HS Standards

   9-12.N.2.1. (Synthesis) Apply science process skills to design and conduct
   student investigations.

   9-12.N.2.2. (Application) Practice safe and effective laboratory techniques.

                               Advanced HS Standards

   9-12.N.2.1A. (Synthesis) Manipulate multiple variables with repeated trials.

   9-12.N.2.2A. (Evaluation) Use statistical analysis of data to evaluate the validity
   of results.

   9-12.N.2.3A. (Analysis) Demonstrate correct precision in measurements and
   calculations.

   Indicator 1: Describe structures and properties of, and changes in, matter.

                                  Core HS Standards

   9-12.P.1.3. (Application) Predict whether reactions will speed up or slow down
   as conditions change.

   9-12.P.1.4A. (Synthesis) Describe factors that affect solution interactions.

   9-12.P.1.6A. (Application) Perform stoichiometric calculations.


      Distinguish between solutions and suspensions.
      Given various types of solutions, determine the solute and solvent.
      Interpret solubility graphs and tables.
      Distinguish among unsaturated, saturated, and supersaturated solutions.
      Relate various ways of expressing concentration data.
      Recognize that units of concentration represent a ratio.
      Use units of molarity in stoichiometric calculations.
      Describe the process for making solutions of different molarities.
      Relate solvent type and solubility to the dry-cleaning process.


                                                                                         24
Chemistry Unit Overviews


        Relate solubility principles of gases to applications in carbonation and diving.



Day 1         Go over tests, types of mixtures 12-1, solubility graphs, molarity of solutions
Day 2         solubility graphs
Day 3         Molarity of solutions, strong or weak solutions, % acid in vinegar
Day 4         Finish % acid in vinegar
Day 5         Using eggs shells to determine % acid in vinegar
Day 6         Using eggs shells to determine % acid in vinegar. Molarity problems
Day 7         Molarity problems
Day 8         Molarity of carbon dioxide and sugar in pop lab. Have students bring their
              own 7-up/Sprite, or Ginger ale and they can drink their own when they are
              done.
Day 9         Beers Law Lab.
Day 10        Molarity test




                                                                                            25
Chemistry Unit Overviews




Unit 13 Acids and Bases
   Indicator 2: Apply the skills necessary to conduct scientific investigations.

                                  Core HS Standards

   9-12.N.2.1. (Synthesis) Apply science process skills to design and conduct
   student investigations.

   9-12.N.2.2. (Application) Practice safe and effective laboratory techniques.

                               Advanced HS Standards

   9-12.N.2.1A. (Synthesis) Manipulate multiple variables with repeated trials.

   9-12.N.2.2A. (Evaluation) Use statistical analysis of data to evaluate the validity
   of results.

   9-12.N.2.3A. (Analysis) Demonstrate correct precision in measurements and
   calculations.

   Indicator 1: Describe structures and properties of, and changes in, matter.

                                  Core HS Standards

   9-12.P.1.1. (Analysis) Use the Periodic Table to determine the atomic structure
   of elements, valence number, family relationships, and regions (metals,
   nonmetals, and metalloids).

   9-12.P.1.2. (Comprehension) Describe ways that atoms combine.

   9-12.P.1.4. (Application) Balance chemical equations by applying the Law of
   Conservation of Matter.

   Indicator 1: Describe structures and properties of, and changes in, matter.

                                  Core HS Standards

   9-12.P.1.1. (Analysis) Use the Periodic Table to determine the atomic structure
   of elements, valence number, family relationships, and regions (metals,
   nonmetals, and metalloids).



                                                                                         26
Chemistry Unit Overviews


   9-12.P.1.2. (Comprehension) Describe ways that atoms combine.

   9-12.P.1.3. (Application) Predict whether reactions will speed up or slow down
   as conditions change.

   9-12.P.1.4. (Application) Balance chemical equations by applying the Law of
   Conservation of Matter.

   9-12.P.1.2A. (Synthesis) Predict electron configuration, ion formation,
   reactivity, compound formation, periodic trends, and types of compounds formed
   based on location on the Periodic Table.

   9-12.P.1.3A. (Synthesis) Identify five basic types of chemical reactions and
   predict the products.

   9-12.P.1.4A. (Synthesis) Describe factors that affect solution interactions.

   9-12.P.1.6A. (Application) Perform stoichiometric calculations.

   9-12.P.1.9A. (Analysis) Describe the characteristics of equilibria.

      Describe the characteristic properties of aqueous acids and bases
      Explain the difference between a strong acid and a weak acid and between a
       strong base and a weak base.
      Relate the reactions of anhydrides to acid rain.
      Explain and use the pH scale to calculate the concentration of H 3O + and OH-
       given thepH of a solution.
      Write the equation for a neutralization reaction.
      Describe how an acid-base titration is performed.
      Determine the molarity of an acid or base solution using titration data.

Standards
Day 1       Acid and Bases of household items. Inquiry lab.
Day 2       Indicators Lab
Day 3       Introduce pH scale and calculations.
Day 4       Calculations of [H30+], [OH-], pH, pOH worksheets
Day 5       Correct work. Introduce titrations.
Day 6       Titration lab.
Day 7       Salts Lab and neutralization reaction.
Day 8       Acid base
Day 10      pH Test
Day 11      Equilibrium Lab
Day 12      Ksp lab
Day 13      Vitamin C lab


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Chemistry Unit Overviews




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