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					                          BLUE RIDGE HIGH SCHOOL
                            2010-2011 SCHOOL YEAR
                      SYLLABUS FOR CHEMISTY HONORS
                                UNIT CREDIT = 1
                       INSTRUCTOR: MR. JOEL T. PERKIN

Course Description:
Chemistry Honors is a college preparatory course designed to challenge and give students
the skills needed to prepare for work in a science related field, medicine or engineering.
Chemistry Honors is not a memorization course. Students must build on previous
knowledge obtained throughout the semester. The skills and concepts taught in the class
includes but not limited to: laboratory safety and proper use of handling chemicals,
atomic structure, chemical bonding, chemical nomenclature, writing formulas, balancing
equations, mass-mole conversions, stoichiometric calculations, gas laws, etc.

Textbook: Modern Chemistry: Holt, Rinehart, Winston

Course Outline:
                        Course Pre-Assessment: 17 August 2010

Unit 1 Introduction to Chemistry and Matter
            Chapter 1     Matter and Change
            Chapter 2     Measurements and Calculations
                          Assessment 1: 26 August 2010

Unit 2 Organization of Matter
           Chapter 3      Atoms: The Building Blocks of Matter
           Chapter 4      Arrangement of Electrons in Atoms
           Chapter 5      The Periodic Law
           Chapter 6      Chemical Bonding
                         Assessment 2: 15 September 2010

Unit 3 Language of Chemistry
           Chapter 7     Chemical Formulas and Chemical compounds
           Chapter 8     Chemical Equations and Reactions
           Chapter 9     Stoichiometry
                          Assessment 3: 1 October 2010

Unit 4 Phases of Matter
           Chapter 10       States of Matter
           Chapter 11       Gases
                             Assessment 4: 18 October 2010

Unit 5 Solutions
           Chapter 12        Solutions


                                      Page 1 of 20
             Chapter 13    Ions in Aqueous Solutions and Colligative Properties
             Chapter 14    Acids and Bases
             Chapter 15    Acid-Base Titration and pH
                           Assessment 5: 5 November 2010

Unit 6 Kinetics
           Chapter 16      Reaction Energy
           Chapter 17      Reaction Kinetics
           Chapter 18      Chemical Equilibrium
                           Assessment 6: 22 November 2010

Unit 7 Electron Chemistry
            Chapter 19    Oxidation-Reduction Reactions
            Chapter 20    Electrochemistry
                          Assessment 7: 6 December 2010

Unit 8 Advanced Topics in Chemistry
           Chapter 21     Nuclear Chemistry
           Chapter 22     Organic Chemistry
           Chapter 23     Biological Chemistry
                          Assessment 8: 5 January 2011

                                  Final Exam: TBA




                                    Page 2 of 20
Unit 1 | Scientific Inquiry
South Carolina Standard C-1
The student will demonstrate an understanding of how scientific inquiry and
technological design, including mathematical analysis, can be used appropriately to pose
questions, seek answers, and develop solutions.

C-1.1                                            C-1.5
Apply established rules for significant          Organize and interpret the data from a
digits, both in reading a scientific             controlled scientific investigation by
instrument and in calculating a derived          using mathematics (including formulas,
quantity from measurement.                       scientific notation, and dimensional
                                                 analysis), graphs, models, and/or
C-1.2                                            technology.
Use appropriate laboratory apparatuses,
technology, and techniques safely and            C-1.6
accurately when conducting a scientific          Evaluate the results of a scientific
investigation.                                   investigation in terms of whether they
                                                 verify or refute the hypothesis and what
C-1.3                                            the possible sources of error are.
Use scientific instruments to record
measurement data in appropriate metric           C-1.7
units that reflect the precision and             Evaluate a technological design or
accuracy of each particular instrument.          product on the basis of designated
                                                 criteria.
C-1.4
Design a scientific investigation with           C-1.8
appropriate methods of control to test a         Use appropriate safety procedures when
hypothesis (including independent and            conducting investigations.
dependent variables), and evaluate the
designs of sample investigations.

Unit 2 | Atomic Structure and Nuclear Processes
South Carolina Standard C-2
Students will demonstrate an understanding of atomic structure and nuclear processes.

C-2.1                                            C-2.3
Illustrate electron configurations by            Summarize the periodic table’s property
using orbital notation for representative        trends (including electron configuration,
elements.                                        ionization energy, electron affinity,
                                                 atomic size, ionic size, and reactivity).
C-2.2
Summarize atomic properties (including
electron configuration, ionization
energy, electron affinity, atomic size,
and ionic size).


                                        Page 3 of 20
C-2.4                                            C-2.7
Compare the nuclear reactions of fission         Apply the predictable rate of nuclear
and fusion to chemical reactions                 decay (half-life) to determine the age of
(including the parts of the atom involved        materials.
and the relative amounts of energy
released).                                       C-2.8
                                                 Analyze a decay series chart to
C-2.5                                            determine the products of successive
Compare alpha, beta, and gamma                   nuclear reactions and write nuclear
radiation in terms of mass, charge,              equations for disintegration of specified
penetrating power, and the release of            nuclides.
these particles from the nucleus.
                                                 C-2.9
C-2.6                                            Use the equation E = mc2 to determine
Explain the concept of half-life, its use        the amount of energy released during
in determining the age of materials, and         nuclear reactions.
its significance to nuclear waste
disposal.

Unit 3 | Chemical Bonding and Structures
South Carolina Standard C-3
The student will demonstrate an understanding of the structures and classifications of
chemical compounds.

C-3.1                                            C-3.5
Predict the type of bonding (ionic or            Illustrate the structural formulas and
covalent) and the shape of simple                names of simple hydrocarbons
compounds by using Lewis dot                     (including alkanes and their isomers and
structures and oxidation numbers.                benzene rings).

C-3.2                                            C-3.6
Interpret the names and formulas for             Identify the basic structure of common
ionic and covalent compounds                     polymers (including proteins, nucleic
                                                 acids, plastics, and starches).
C-3.3
Explain how the types of intermolecular          C-3.7
forces present in a compound affect the          Classify organic compounds in terms of
physical properties of compounds                 their functional group.
(including polarity and molecular
shape).                                          C-3.8
                                                 Explain the effect of electronegativity
C-3.4                                            and ionization energy on the type of
Explain the unique bonding                       bonding in a molecule.
characteristics of carbon that have
resulted in the formation of a large
variety of organic structures.


                                        Page 4 of 20
C-3.9                                             C-3.10
Classify polymerization reactions as              Classify organic reactions as addition,
addition or condensation.                         elimination, or condensation.


Unit 4 | Chemical Reactions and Stoichiometry
South Carolina State Standard C-4
The student will demonstrate an understanding of the types, the causes, and the effects of
chemical reactions.

C-4.1                                             C-4.6
Analyze and balance equations for                 Explain the role of activation energy and
simple synthesis, decomposition, single           the effects of temperature, particle size,
replacement, double replacement, and              stirring, concentration, and catalysts in
combustion reactions.                             reaction rates.

C-4.2                                             C-4.7
Predict the products of acid-base                 Summarize the oxidation and reduction
neutralization and combustion reactions.          processes (including oxidizing and
                                                  reducing agents).
C-4.3
Analyze the energy changes                        C-4.8
(endothermic or exothermic) associated            Illustrate the uses of electrochemistry
with chemical reactions.                          (including electrolytic cells, voltaic cells,
                                                  and the production of metals from ore by
C-4.4                                             electrolysis).
Apply the concept of moles to determine
the number of particles of a substance in         C-4.9
a chemical reaction, the percent                  Summarize the concept of chemical
composition of a representative                   equilibrium and Le Châtelier’s principle.
compound, the mass proportions, and the
mole-mass relationships.                          C-4.10
                                                  Explain the role of collision frequency,
C-4.5                                             the energy of collisions, and the
Predict the percent yield, the mass of            orientation of molecules in reaction
excess, and the limiting reagent in               rates.
chemical reactions.

Unit 5 | Phases of Matter
South Carolina Standard C-5
The student will demonstrate an understanding of the structure and behavior of the
different phases of matter.

C-5.1                                             C-5.2
Explain the effects of the intermolecular         Explain the behaviors of gas; the
forces on the different phases of matter.         relationship among pressure, volume,


                                         Page 5 of 20
and temperature; and the significance of        C-5.5
the Kelvin (absolute temperature) scale,        Analyze the energy changes involved in
using the kinetic-molecular theory as a         calorimetry by using the law of
model.                                          conservation of energy as it applies to
                                                temperature, heat, and phase changes
C-5.3                                           (including the use of the formulas
Apply the gas laws to problems                  q = mcT [temperature change] and
concerning changes in pressure, volume,         q = mLv and q = mLf [phase change] to
or temperature (including Charles’s law,        solve calorimetry problems).
Boyle’s law, and the combined gas law).
                                                C-5.6
C-5.4                                           Use density to determine the mass,
Illustrate and interpret heating and            volume, or number of particles of a gas
cooling curves (including how boiling           in a chemical reaction.
and melting points can be identified and
how boiling points vary with changes in         C-5.7
pressure).                                      Apply the ideal gas law (pV = nRT) to
                                                solve problems.

                                                C-5.8
                                                Analyze a product for purity by
                                                following the appropriate assay
                                                procedures.

                                                C-5.9
                                                Analyze a chemical process to account
                                                for the weight of all reagents and
                                                solvents by following the appropriate
                                                material balance procedures.


Unit 6 | Properties of Solutions
South Carolina State Standard C-6
The student will demonstrate an understanding of the nature and properties of various
types of chemical solutions.

C-6.1                                           C-6.2
Summarize the process by which solutes          Compare solubility of various substances
dissolve in solvents, the dynamic               in different solvents (including polar and
equilibrium that occurs in saturated            nonpolar solvents and organic and
solutions, and the effects of varying           inorganic substances).
pressure and temperature on solubility.




                                      Page 6 of 20
C-6.3                                               C-6.10
Illustrate the colligative properties of            Interpret solubility curves to determine
solutions (including freezing point                 saturation at different temperatures.
depression and boiling point elevation
and their practical uses).                          C-6.11
                                                    Use a variety of procedures for
C-6.4                                               separating mixtures (including
Carry out calculations to find the                  distillation, crystallization filtration,
concentration of solutions in terms of              paper chromatography, and centrifuge).
molarity and percent weight (mass).
                                                    C-6.12
C-6.5                                               Use solubility rules to write net ionic
Summarize the properties of salts, acids,           equations for precipitation reactions in
and bases.                                          aqueous solution.

C-6.6                                               C-6.13
Distinguish between strong and weak                 Use the calculated molality of a solution
common acids and bases                              to calculate the freezing point depression
                                                    and the boiling point elevation of a
C-6.7                                               solution.
Represent common acids and bases by
their names and formulas.                           C-6.14
                                                    Represent neutralization reactions and
C-6.8                                               reactions between common acids and
Use the hydronium or hydroxide ion                  metals by using chemical equations.
concentration to determine the pH and
pOH of aqueous solutions.                           C-6.15
                                                    Analyze the composition of a chemical
C-6.9                                               sample by using gas chromatography
Explain how the use of a titration can
determine the concentration of acid and
base solutions




                                           Page 7 of 20
Classroom Expectations:
    Prompt:
         o Students are expected to arrive to class on time each day.
    Productive:
         o Students are expected to follow directions the first time given.
         o Students are expected to complete assignments by the given due date.
    Prepared:
         o Students are required to handle themselves in a professional manner at all
             times.
         o Students are expected come to class prepared to work each day.
         o Students are expected to bring necessary materials to class every day.
    Polite:
         o Students are expected respect the privacy of others and respect all
             members of the class.
    Problem-Solver:
         o Students are expected follow all school, class, and lab rules.
         o Students are expected to anticipate and head off problems.


Classroom Management Policy:
1st Offense      Student-Teacher Conference
 nd
2 Offense        Parent Contact
3rd Offense      After-School Detention
 th
4 Offense        Written Reprimand

Severe Disruptions     Parent Contact and Written Reprimand
Tardies                Follow Guidelines /Student Handbook
ID Violations          Follow Guidelines/Student Handbook

A teacher log of infractions will be kept on file.

Student Reminders:
    Cell phones should not be visible or audible or ever used between 8:45 and 3:45.
    Proper shoes must be worn in the chemistry lab. No open toed shoes will be
      tolerated during lab activities.
    IDs are to be worn at all times in class, except during laboratory exercises when
      they may be dangerous.
    You must have your agenda and ticket to use the restroom for an emergency. No
      exceptions.
    White slips must be presented when you are absent from class.




                                        Page 8 of 20
Instructional Materials:
   1. Textbook: Modern Chemistry- Holt, Rinehart, Winston
   2. Three (3) folders with clasps
   3. Notebook for daily notes
   4. Composition book for lab activities
   5. A scientific calculator (capable of scientific notation)
   6. Pencils, blue or black ink pens only.

Grading of Course:
Your grade in Chemistry Honors will be a combination of all assessments given during
the duration of the semester. Assessments include tests (50%), quizzes (20%), lab work
(10%), worksheets, homework(10%) and projects (10%). Final exam counts 20% of your
overall grade in course.

Grading Procedures:
All major assessments will be returned within two days. You must keep all tests, quizzes,
and worksheets in one of your three folders. Progress reports will be issued according to
guidelines in your handbook. Report cards will be issued at the end of the nine weeks.

Student Records:
All grades are kept on PowerSchool. Grades are available online. Parents wanting
updates more often must place this information in writing. I will provide parents with
progress grades every two weeks.

Assessment Dates:
All major tests will be given once each unit. Concept quizzes will be given once each
chapter. Labs will be assessed by lab reports, lab quizzes, or review of conclusion
questions. Computer simulations will be done when possible. All major projects will be
announced one month in advance of the due date. Post test will be administered one week
before final exam.

Missing Work/Make-Up Policy:
Students who are absent will be allowed to make up missing assignments if the absence is
excused. Work should be made up upon student return to school. Make-up for test will
be on Tuesdays and Thursdays only from 4:00-5:00 PM.

Students References for Assessments:
    Students will be allowed to use the periodic table for all tests.
    Students will apply significant figures in problem solving.
    Students must memorize polyatomic ions for use in writing formulas.
    Students will be allowed to use a calculator during all class assessments.

Laboratory Reports:
Laboratory write-ups are due on a specific date, generally 2-5 days after completion of
the laboratory investigation. Late reports will be assessed a 15% per day penalty except
in the case of an excused absence or illness. Not all labs will require reports.


                                      Page 9 of 20
Extra Help Days:
Extra help is available any day after school except for meeting days by appointment.
Morning appointments must be made on an individual basis with the teacher.

Teacher Contact Information:
Joel Perkin
Blue Ridge High School

Email: jtperkin@greenville.k12.sc.us
Phone: 355-1864
Room #: F111

All parent contacts will be addressed within 48 hours.

Grading Scale:
A            93-100
B            85-92
C            77-84
D            70-76
F            69-0

Assignments/Tests/Quizzes:
    Daily assignments can be expected and must be submitted by the due date.
    Students are responsible for missed work on the days of absences. Make-up
      assignments due to an excused absent will be accepted no later than 3 days after
      the student returns to class.
    During testing (quiz/test) students are expected not to talk, leave their seat, and
      have unauthorized study materials. Any violation of these rules will result in a
      grade of zero and a phone call home.
    Missing a scheduled make-up lab, quiz or test without notification will result in a
      zero credit.




                                       Page 10 of 20
Attendance:
Students are responsible for being in school each day. You may not have more than five
unexcused absences before credit is denied in this course. Attendance affects your
performance in class.

TEACHING SCHEDULE FALL SEMESTER 2010

1ST BLOCK     8:45 - 10:15          Chemistry 1 Honors
2ND BLOCK     10:20 - 11:55         Planning
3RD BLOCK     12:00 – 2:10          Chemistry CP
4TH BLOCK     2:15 - 3:45           Chemistry 2 Honors

TEACHING SCHEDULE SPRING SEMESTER 2011

1ST BLOCK     8:45 - 10:15          Chemistry CP Advanced
2ND BLOCK     10:20 - 11:55         Chemistry CP Advanced
3RD BLOCK     12:00 – 2:10          Chemistry 1 Honors
4TH BLOCK     2:15 - 3:45           Planning




                                    Page 11 of 20
                 Appendix A: Lab Notebook for Honors Chemistry

Purpose:
   1. The lab notebook provides a permanent record of your work in lab and can be
      used as a reference in college courses. Some colleges require students to submit
      their lab notebooks before giving them credit for the lab component of the course.
      It is also handy to review your lab notebook for the lab question on the AP exam.
   2. If you are working professionally in a lab it would provide legal evidence of the
      conception of an idea and the date of that conception. It can be used in disputes
      about patents, royalties, and legal issues.

Procedures:
   1. All entries must be orderly, legible, and in permanent black or blue ink.
   2. Errors should be crossed out with a single line. You will not be penalized for any
      material neatly crossed out. Do not try to obliterate the mistake. DO NOT USE
      WHITE OUT. Using white out or obliterating entries will result in a loss of
      points.
   3. Number all pages in the lab book, consecutively, in the top right corner. Pages
      should NEVER be torn out.
   4. Reserve the first 2 pages for the Table of Contents. The last couple of pages will
      be an Appendix.
   5. Each entry must be dated, i.e., each day you work in your lab notebook should be
      dated. Begin each lab’s work on a separate page. USE YOUR NOTEBOOK
      DURING LAB. Do not wait and write your entries in later.
   6. If you do not have your lab notebook on a lab day, you will not be permitted to
      take part in the lab that day and must make up the lab on your time within the next
      two days.

Content for Each Lab:
  1. Title
  2. Prelab: Take notes during the prelab discussion.
  3. Overview: Summarize the purpose for doing the lab and give a very brief
      explanation of what you are doing.
  4. Personal Account: Describe what you did clearly enough that someone else could
      repeat the experiment. This should be written in narrative form and should be a
      conceptual account of what you did with enough details.
          a. Discussion of equipment: What does the equipment do? How does it
              work? Any difficulties you had using the equipment? Diagrams and
              sketches of the setup are often helpful.
          b. Use of proper chemical and lab terminology: Describe what data you are
              collecting and why you are collecting it.
          c. Qualitative observations: Document changes of color, exo- or
              endothermic, precipitates, etc. Describe the chemistry of these
              observations.




                                     Page 12 of 20
   5. Data Tables and Figures: Organize your observations and your data in NEAT
      tables. Be sure to label all units and record the correct number of sig figs. Graphs
      should be set up properly. Axes should be labeled, rates calculated, etc.
   6. Calculations: Show at least one sample for all calculations. Write formulas, show
      substitutions with units, and record the answer with correct digits and units.
   7. Discussion: You will usually be asked to answer the questions from the lab sheet.
   8. Evaluation: Compare your results to what is expected (standards), analyze errors
      that could have cause “your” error, and suggest ways you could improve on this
      experimental procedure.
   9. Conclusion: Summarize what you did in the lab (similar to overview) and report
      results.

Evaluation Options: Each lab will be assessed using one of these three methods:
   1. Lab Notebook Evaluation
   2. Lab Report
   3. Open-Lab-Book Quiz




                                     Page 13 of 20
                   Appendix B: How to Write a Formal Lab Report

The purpose of a lab report is to present in a clear, concise, and organized manner the
work you did in the laboratory and the results you obtained.

The lab report should include the following sections:
    Introduction
    Methods and Materials
    Results
    Discussion with conclusion

In writing a lab report, always indicate clearly the title of the experiment and then clearly
identify and separate each of the above mentioned sections. Data tables, diagrams, and
graphs should either be done on a computer or neatly taped into the lab report. Although
content is the most important feature of a lab report, neatness is a close second. The
neatness of the overall report is important and neatness in the organization is essential. A
lab report is not intended to be a piece of literature; however, it should be written in good
English. It should be written in the third person and it is preferable that it be written in
the past tense. Your formal lab reports must be typed and double-spaced. The text of a
formal lab should be continuous so do not leave blank paper at the bottom of a page to
start the next section on a new sheet of paper.

The Introduction should state as clearly as possible the nature of the experiment and
why you are doing the experiment. Second, the introduction should give a brief overview
of the method used. Try to assimilate the instructions in the lab manual and express them
in your own words. Frequently you will be asked to include background information you
have read in other articles or books; it is important that the authors of information be
cited when you include their ideas.

In the Methods and Materials you should briefly explain how the experiment was done.
This should be written as a narrative, not as a step-by-step detailed “cookbook”
procedure. Pick out what was essential to the method. This section must be written in
the past tense. Do not list the materials you used. A correctly-written M&M would say,
“the test tubes were filled,” not, “we/he/I filled the test tubes.”

The Results sections should contain the data collected in the lab organized in table form,
a sample of any calculations (including formulas and substitutions), and graphs that
demonstrate relationships between data and variables. Each table and figure must be
numbered and have a title. You should include a narrative paragraph in the results
section that briefly describes each table and figure (do not interpret data or graphs in the
results section). Graphs are either to be done on graph paper or generated by computer.
Tables and figures must be numbered separately of each other.

The Discussion is the most important part of the report because this is where you will:
    Analyze the data: explain how you reached your conclusions
    Compare your results with expected results


                                       Page 14 of 20
         Analyze your experimental error
         Summarize the conclusions (the last paragraph should always summarize what
          you “did” and what you “got”)


Grading Policy for Formal Lab Report

Format ............................................................20 points
Introduction ....................................................10 points
Method & Materials .......................................10 points
Results: Tables ...............................................5 points
Results: Graphs ..............................................10 points
Results: Narrative...........................................5 points
Discussion: Analysis of Data .........................5 points
Discussion: Comparison with Expected ........5 points
Discussion: Error Analysis ............................5 points
Discussion: Conclusion..................................5 points
Participation in Lab ........................................20 points


You can expect to do one formal lab report each nine weeks.




                                                     Page 15 of 20
           August 16                            17                        18                       19                            20
Intro                    Pre-Test                    1.1 Chemistry is a        1.3 Elements              2.1 Scientific Method
                                                     Physical Science          Lab: Mixture Separation   2.2 Units of
                                                     1.2 Matter and Its                                  Measurement
                                                     Properties
            August 23                           24                        25                       26                         27
2.3 Using Scientific  Lab: Percentage of             Review                    Unit 1 Assessment       3.1 The Atom: From
Measurements          Water in Popcorn                                                                 Philosophical Idea to
Lab: Percentage of                                                                                     Scientific Theory
Water in Popcorn                                                                                       3.2 The Structure of the
                                                                                                       Atom
            August 30                      31                  September 1                           2                         3
3.3 Counting Atoms    Lab: Conservation of           4.2 The Quantum Model 4.3 Electron                5.1 History of the
                      Mass                           of the Atom             Configurations            Periodic Table
                      4.1 The Development of         4.3 Electron            Lab: Flame Tests          5.2 Electron
                      a New Atomic Model             Configurations                                    Configuration and the
                                                                                                       Periodic Table
        September 6                             7                         8                          9                        10
Labor Day           5.3 Electron                     Lab: The Mendeleev      6.2 Covalent Bonding      6.3 Ionic Bonding and
                    Configuration and                Lab of 1869             and Molecular             Ionic Compounds
                    Periodic Properties              6.1 Introduction to     Compounds                 6.4 Metallic Bonding
                                                     Chemical Bonding
         September 13                           14                       15                        16                         17
6.5 Molecular Geometry   Review                      Unit 2 Assessment       7.1 Chemical Names        7.2 Oxidation Numbers
Lab: Types of Bonding                                                        and Formulas              7.3 Using Chemical
in Solids                                                                                              Formulas
         September 20                           21                       22                        23                         24
7.3 Using Chemical       Lab: Determining the        8.1 Describing Chemical 8.2 Ideal Stoichiometric 8.3 Limiting Reactants
Formulas                 Empirical Formula of        Reactions               Calculations              and Percentage Yield
7.4 Determining          Magnesium Oxide                                                               Lab: Blueprint Paper
Chemical Formulas
         September 27                          28                      29                          30                 October 1
9.1 Introduction to      9.2 Ideal Stoichiometric 9.3 Limiting Reactants  Review                         Unit 3 Assessment
Stoichiometry            Calculations             and Percentage Yield
                                                  Lab: Stoichiometry and
                                                  Gravimetric Analysis


Chemistry Honors Schedule
              October 4                           5                        6                          7                         8
10.1 Kinetic Theory of    10.3 Solids                 Lab: “Wet” Dry Ice        Lab: “Wet” Dry Ice      11.2 The Gas Laws
Matter                    10.4 Changes of State                                 11.1 Gases and Pressure
10.2 Liquids
            October 11                        12                           13                         14                       15
11.3 Gas Volumes and      Lab: Mass and Density  Review                         No School                  No School
the Ideal Gas Law         of Air at Different
Lab: Mass and Density     Pressures
of Air at Different
Pressures
            October 18                         19                       20                      21                      22
Unit 4 Assessment         12.1 Types of Mixtures  12.3 Concentration of    Lab: Separation of Pen  Lab: Separation of Pen
                          12.2 The Solution       Solutions                Inks by Paper           Inks by Paper
                          Process                                          Chromatography          Chromatography
                                                                                                   Mole Day!

            October 25                          26                     27                          28                           29
13.1 Compounds in         Lab: Testing Water for   14.2 Acid-Base Theories Lab: Is It an Acid or a         15.1 Aqueous Solutions
Aqueous Solutions         Ions                     14.3 Acid-Base          Base?                           and the Concept of pH
13.2 Colligative          14.1 Properties of Acids Reactions                                               15.2 Determining pH
Properties of Solutions   and Bases                                                                        and Titrations

           November 1                         2                       3                               4                         5
15.2 Determining pH     Election Day            Lab: How Much                   Review                     Unit 5 Assessment
and Titrations                                  Calcium Carbonate Is in
Lab: How Much                                   an Eggshell?
Calcium Carbonate Is in
an Eggshell?
           November 8                         9                      10                               11                        12
16.1 Thermochemistry    16.2 Driving Force of   Lab: Calorimetry and            17.1 The Reaction          Lab: Rate of a Chemical
                        Reactions               Hess’s Law                      Process                    Reaction
                        Lab: Calorimetry and                                    17.2 Reaction Rates
                        Hess’s Law




Chemistry Honors Schedule
         November 15                          16                         17                      18                    19
Lab: Rate of a Chemical 18.2 Shifting               18.4 Solubility         Lab: Measuring Ka for   Review
Reaction                Equilibrium                 Equilibrium             Acetic Acid
18.1 The Nature of      18.3 Equilibria of Acids,   Lab: Measuring Ka for
Chemical Equilibrium    Bases, and Salts            Acetic Acid
         November 22                          23                         24                      25                    26
Unit 6 Assessment       19.1 Oxidation and          Thanksgiving Break      Thanksgiving Break      Thanksgiving Break
                        Reduction
                        19.2 Balancing Redox
                        Equations
         November 29                          30               December 1                        2                     3
19.3 Oxidizing and      Lab: Reduction of Mn in     20.2 Voltaic Cells      Lab: Voltaic Cells       Review
Reducing Agents         MnO4-                       20.3 Electrolytic Cells
Lab: Reduction of Mn in 20.1 Introduction to
MnO4-                   Electrochemistry
          December 6                           7                             8                 9                      10
Unit 7 Assessment       21.1 The Nucleus                                 Lab: Simulation of
                                                    21.3 Nuclear Radiation                       22.2 Hydrocarbons
                        21.2 Radioactive Decay      21.4 Nuclear Fission Nuclear Decay Using     22.3 Functional Groups
                                                    and Nuclear Fusion   Pennies and Paper
                                                                         22.1 Organic Chemistry
        December 13                           14                      15                     16                       17
22.4 Organic Reactions Lab: Synthesis of         23.1 Carbohydrates and 23.3 Metabolism          Lab: Tie-Dye
Lab: Synthesis of      Aspirin                   Lipids                  23.4 Nucleic Acids
Aspirin                                          23.2 Amino Acids and
                                                 Proteins
            January 3                          4                       5                       6                       7
Lab: Casein Glue      Lab: Casein Glue           Review                  Unit 8 Assessment       Catch-up Day
           January 10                         11                      12                     13                       14
Exams                 Exams                      Exams                   Exams




Chemistry Honors Schedule
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