Honors Chemistry
2012 - 2013 Academic Year
Instructor: Jim Dahlman, Brent Rehfuss
Mr. Rehfuss Room 107
Brent.rehfuss@totinograce.org Ext: 703
wikispace: http://tg107.wikispaces.com
Course Description
Chemistry is defined as the science that deals with the materials of the universe and the changes
that these materials undergo. The field of chemistry is based observation and experimentation, leading
to a greater understanding of the nature of matter.
Chemistry is all around us. The food, clothing, building materials, medicines and sources of
energy are products of the application of chemical knowledge. Chemistry can also help us understand
the causes and possible solutions to the great problems facing our society like global warming, the
energy crisis and pollution.
This course will examine the basic chemical principles governing the materials in nature and
how these principles affect how materials interact with one another.
Course Goals and Objectives
1. Students learn the facts, formulas and principles that compose the standard high school
chemistry curriculum.
2. Students understand the basic chemical concepts that underlie the facts, formulas and principles.
3. Students develop critical-thinking and problem-solving skills not only to be used in chemistry,
but also used in every-day life to address problems that will occur as adults.
4. Students develop the knowledge base, laboratory skills and classroom habits necessary for
success at college in science and related fields.
5. Students will have a greater appreciation for the history, nature and role of science in today’s
global society.
Student Responsibilities/Keys to Success
1.
2.
3.
4.
Work Hard
Ask Questions
Come Prepared
Be Respectful
Course Requirements
Materials:
Textbook: Zumdahl, Decoste. Introductory Chemistry, Houghton Mifflin, 6th Ed, 2008. (Covered)
Notebook/Three-ring binder
Pencils/Pens
Scientific Calculator
Attendance:
You are expected to be in class every day. If you know you are going to be absent, it is your
responsibility to talk with your teacher and find out what you will miss. For any excused absence, you
have two days to make up missing work. No extra time will be given to complete work missed by an
unexcused absence.
Homework:
The answers to the homework are not nearly as important as how you came up with those
answers. You are required to show all of your work on anything you turn in. The maximum score on
any late assignment is ½ credit. Any assignment turned in after the test which the covers the
assignment’s material will receive no credit.
Quizzes and Exams:
Quizzes will be given about once a Unit, some will be announced, some will be unannounced.
Tests will be given at the end of every Unit. There will be a final exam at the end of each semester.
Labs and Projects:
The laboratory is an essential component of this class, since chemistry is an experimental
science. Labs will be 50 points each. Labs will be written up in a lab notebook (see separate handout
on lab notebooks). There will be about 1 lab per unit. If you hand in a lab late, you will lose 25% per
day late. That means if an experiment is four or more days late, it’s a zero!
Academic Dishonesty:
Academic dishonesty will not be tolerated in any form. Cheating will result in a zero score on
the assignment, a call home and any other appropriate penalties according to the student handbook and
the school administration. Working together is highly encouraged, but copying papers and turning in
identical homework are considered cheating, not working together. Anything you turn in must be a
product of your own thought.
Grading:
Weighting:
50%
25%
10%
15%
Exams/Quizzes
Labs/Projects
Homework
Final Exam
Grade Breakdown:
A >93.0%
C >73.0%
A- >90.0%
C- >70.0%
B+ >87.0%
D+ >67.0%
B >83.0%
D >63.0%
B- >80.0%
D- >60.0%
C+ >77.0%
F <59.9%
**Other policies and procedures will be introduced as the class progresses.
UNIT 1: Introduction to Chemistry (Ch. 1-3)
Timeline: 14 Days
Learner Objectives:
After completion of this unit, the student will be able to:
1.
2.
3.
4.
5.
Describe how chemists study chemistry.
Describe the scientific method and its use in problem-solving.
Use the SI system, significant figures and scientific notation.
Express and convert quantities using the SI system and dimensional analysis.
Distinguish between precision and accuracy as well as relate physical measurements to
significant figures.
6. Define and classify matter as solid, liquid or gas as well as describe and give examples of each.
7. Describe and classify physical properties.
8. Describe and classify chemical properties.
9. Describe and classify physical changes.
10. Describe and classify chemical changes.
11. Describe and apply proper laboratory safety procedures.
12. Define an element, compound, mixture, and solution.
13. Name the common elements and recognize their symbols.
14. Differentiate between an element, compound, and mixture on the atomic level.
15. Describe physical separation techniques of mixtures.
Labs: Analysis of a Mixture
Chemical or Physical?
Assessments:
Measurement Quiz
Element Quiz
Unit 1 Test
UNIT 2: Atomic and Nuclear Structure (Ch.4.3-4.7, 4.10, Ch. 19)
Timeline: 17 Days
Learner Objectives:
After completion of this unit, the student will be able to:
1.
2.
3.
4.
5.
6.
Discuss early developments in atomic theory.
Explain the Law of Constant Composition
Write chemical formulas for compounds.
Differentiate among the major subatomic particles.
Discuss the development of modern atomic theory.
Determine the atomic mass and number of given isotopes of elements.
7. Use and interpret the symbols for isotopes to give the number of protons, neutrons, and
electrons for a given atom.
8. Explain alpha, beta, and gamma decay using nuclear equations.
9. Explain the concept of half-life.
10. Discuss some of the applications of radioactivity/nuclear energy and the consequences of its
use.
11. Explain the mass defect and how it applies to nuclear reactions.
12. Define ion.
13. Describe ion formation
14. Write nuclear bombardment calculations.
15. Calculate the age of a material based on its half-life
16. Describe the carbon dating process
17. Explain the principles behind nuclear fission
18. Explain the concept of nuclear fusion
19. Explain how a nuclear reactor works
Labs: Thickness of Aluminum Foil Lab
Penny Lab
Cloud Chambers
Half-Life
Assessments: Quizzes and Unit Test
UNIT 3: Modern Atomic Theory and the Periodic Table (Ch. 4.8-4.11,Ch. 11)
Timeline: 20 Days
Learner Objectives:
After completion of this unit, the student will be able to:
1. Describe the wave-mechanical view of the hydrogen atom.
2. Describe the Heisenberg Uncertainty Principle relating the position and velocity of an electron
in an atom.
3. Describe the differences in shapes of atomic orbitals.
4. Use the Pauli Exclusion Principle to determine the electron configuration of an atom.
5. Describe earlier attempts to classify elements.
6. Use the periodic table to predict the electron configurations of elements.
7. Explain the basis for the arrangement of the modern periodic table.
8. Identify metals, nonmetals, metalloids, alkali metals, alkali earth metals, halogens, and noble
gases on the periodic table.
9. Predict chemical stability of atoms using the octet rule.
10. Define atomic radius, ionization energy, electronegativity, ionic radius and electron affinity.
11. Use the periodic table to determine trends in elemental properties.
12. Describe the Bohr model of the atom.
13. Relate energy to the electromagnetic spectrum.
14. Describe how an atom emits light.
15. Describe how the modern periodic table developed.
Labs:
Introduction to Electronic Structure
Periodic Trends Lab
Assessments: Quizzes and Unit Test
UNIT 4: Nomenclature and Chemical Bonding (Ch. 5, Ch. 12)
Timeline: 15 Days
Learner Objectives:
After completion of this unit, the student will be able to:
1. Write simple chemical formulas.
2. Name simple chemical compounds.
3. Recite common polyatomic ions.
4. Name acids.
5. Identify the type of bonding between two elements or ions.
6. Use the periodic table and ionization energy to determine the charge of ions.
7. Differentiate between the properties of ionic, covalent, and metallic bonds.
8. Distinguish between polar and nonpolar covalent bonds.
9. Define electronegativity
10. Use electronegativity, dipole moments, and Van der Waals forces to compare bond polarities.
11. Draw Lewis structures of atoms and molecules.
12. Define resonance structures
13. Predict molecular geometry using VSEPR theory.
Labs:
Lewis Structures and Molecular Shapes
Assessments: Quizzes and Unit Test
UNIT 5: The Mole, Stoichiometry, and Chemical Equations (Ch. 6-9)
Timeline: 21 Days
Learner Objectives:
After completion of this unit, the student will be able to:
1.
2.
3.
4.
5.
Use the Avagadro Constant to define the mole and calculate molecular and molar mass.
Use the molar mass to calculate the percent composition.
Determine the formulas for hydrates.
Use coefficients to balance chemical equations.
Write chemical equations to represent reactions.
6. Differentiate between the different types of chemical reactions.
7. Determine the mass of a reactant or product based on the mass of another reactant or product in
a given chemical reaction.
8. Calculate the percent yield using actual and theoretical yields.
9. Solve any stoichiometric problem.
10. Identify the limiting reagent and solve stoichiometric problems based on it.
Labs: Class Action Lab
Formula of a Hydrate
Calorimetry and Limiting Reactant
S’more Chemistry
Assessments: Quizzes and Unit Test
UNIT 6: Gases and the Gas Laws
Timeline: 17 Days
Learner Objectives:
After completion of this unit, the student will be able to:
1. Define pressure
2. Convert between the different units of pressure.
3. Use Boyle’s, Charles’, Gay-Lussac’s, Avogadro’s and Dalton’s Laws to explain gas behavior
4. Perform calculations using the gas laws.
5. Explain the concept of an ideal gas as well as use the ideal gas law.
6. Explain the basic assumptions of the kinetic molecular theory.
7. Define molar volume
8. Use molar volume in stoichiemetric calculations.
9. Relate temperature and pressure to molecular motion
10. Describe the conditions of STP in various pressure units.
11. Describe the characteristics of substances in each of the three common states of matter in terms
of kinetic theory.
12. Explain the concept of absolute zero.
13. Explain Graham’s Law in relation to molecular speed.
14. Define Avogadro’s Law
15. Use Dalton’s Law of Partial Pressures to calculate pressures of gas mixtures
Labs: Properties of Gases
Determining Absolute Zero
Put of the Fire!
Molecules in Motion
Assessments: Quizzes and Unit Test
UNIT 7: Liquids and Solutions (Ch. 14.1-14.4, 15.1-15.6)
Timeline: 17 Days
Learner Objectives:
After completion of this unit, the student will be able to:
1. Explain the unique properties of water in terms of its molecular structure.
2. Describe the difference between inter and intramolecular forces.
3. Explain the different types of intermolecular forces including hydrogen bonding, dipole, and
dispersion forces.
4. Define vapor pressure.
5. Describe the evaporation process.
6. Explain why evaporation is a cooling process
7. Describe and explain the processes of solvation, dissociation, and dissolving.
8. Differentiate among and solve problems involving molarity.
9. Explain qualitatively the effect of solute particles on the boiling and freezing points of a solvent.
10. Define solute, solution and solvent.
11. Determine the relationship between energy and changes of state as well as perform related
calculations.
12. Define solubility.
13. Interpret solubility curves to determine solubility.
14. Calculate the % mass of a solution.
15. Perform dilution calculations
16. Determine whether a compound will be soluble in water based on solubility rules or
intermolecular forces.
17. Calculate the molarity and molality of a solution
18. Define colligative properties and calculate changes in melting and boiling point
Labs:
Colors in Motion
Beer’s Law
Assessments: Quizzes and Unit Test
UNIT 8: Reaction Rates and Equilibrium (Ch.17)
Timeline: 15 Days
Learner Objectives:
After completion of this unit, the student will be able to:
1. Name the factors that influence a reaction rate and explain how they effect the rate of a reaction.
2. Explain collision theory as it relates to chemical bond formation.
3. Define chemical equilibrium.
4. Determine the equilibrium constant explression for a reaction at equilibrium.
5. Use Le Chatelier’s Principle to explain the effects of concentration, pressure, and temperature
on an equilibrium system.
6. Calculate equilibrium constants and concentrations of reactants and products of a reaction.
7. Calcuate the solubility product of a salt given its solubility.
8. Relate relative amounts of products and reactants for a reaction.
9. Describe how a catalyst increases the rate of a reaction.
Labs: Restoring Balance Lab
Determining an Equilibrium Constant
Assessments: Quizzes and Unit Test
UNIT 9: Acids and Bases (Ch.16)
Timeline: 18 Days
Learner Objectives:
After completion of this unit, the student will be able to:
1. Distinguish between the definitions of acids and bases as outlined by the theories of Arrehius,
Bronstead-Lowry, and Lewis.
2. Name acids and bases.
3. Define and give examples of strong and weak acids and bases.
4. Describe what a conjugate acid or base is.
5. Discuss the auto-ionization of water and solve problems using the ion product constant for
water.
6. Define pH and calculate the pH of a given solution.
7. Explain the concept of neutralization and composition of a salt.
8. Describe the processes of hydrolysis and buffering.
9. Explain the process of titrating and perform titrations to determine concentrations of unknown
acids and bases.
10. State how indicators work and the common acid/base indicators.
Labs: Determination of % acetic acid in household vinegar
pH Lab
Buffers Lab
Properties of Acids and Bases
Assessments: Quizzes and Unit Test
UNIT 10: Organic and Biochemistry (Ch. 20, 21)
Timeline: 18 Days
Learner Objectives:
After completion of this unit, the student will be able to:
1.
2.
3.
4.
Define organic and biochemistry.
State the differences between saturated and unsaturated hydrocarbons.
Differentiate between alkanes, alkenes, and alkynes.
Name and recognize the common functional groups of organic chemistry, including benzene
rings, alcohols, aldehydes, ketones, and carboxylic acids.
5. Define proteins, enzymes, carbohydrates, nucleic acids, and lipids.
6. State the composition of a protein, including its amino acids, secondary and tertiary structure.
7. Recognize the structure of common amino acids.
8. State the fundamental properties and structure of carbohydrates, nucleic acids, and lipids.
9. State how nucleic acids synthesize proteins.
10. Differentiate among the four classes of lipids and their functions.
11. Determine whether a molecule is a protein, carbohydrate, nucleic acid or lipid based on its
structure.
Labs: Examples of Polymers
Testing for Biomolecules
Assessments: Quizzes and Unit Test