AP Chemistry Syllabus
Instructor Information:
Teacher:
Mrs. Amber Null
Room:
Belle Vernon Area High School, Room 106
Contact:
Phone:
Email:
Website:
http://www.bellevernonarea.net/
Required Text:
Tro; Chemistry: A Molecular Approach AP® Edition 3e 2014 with
MasteringChemistry (eText on iPad)
Additional Resources:
http://www.studyisland.com
iTunes U course (see teacher for enrollment code)
Mastering Chemistry program (see teacher for code)
724-808-2500; ext. 2106
amber.null@bellevernonarea.net
Course Description:
This AP Chemistry course is designed to be the equivalent of the general chemistry course usually taken
during the first year of college. For most students, the course enables them to undertake, as a freshman,
second year work in the chemistry sequence at their institution or to register in courses in other fields
where general chemistry is a prerequisite. This course is structured around the six big ideas articulated
in the AP Chemistry curriculum framework provided by the College Board. [CR2] A special emphasis will
be placed on the seven science practices, which capture important aspects of the work that scientists
engage in, with learning objectives that combine content with inquiry and reasoning skills. During the
year students will use demonstrations and other simulations that work with course content in ways that
cannot easily be duplicated in the lab [CR3]. AP Chemistry is open to all students that have completed a
year of chemistry who wish to take part in a rigorous and academically challenging course. This course
can be taken either after or along with a full year Organic Chemistry course for additional work with the
concepts, reactions, and processes from organic chemistry. To keep the students in the cumulative
mindset needed to prepare for the AP exam, as well as exams in a university setting, there will be a
weekly quiz in non-test weeks on the last student day of the week and each unit exam administered will
have questions from previous units included. Students will also take part in discussions that will relate
topics covered to real world applications of the concepts [CR4].
Course Objectives (see AP Chemistry Curriculum
Framework from College Board)
http://media.collegeboard.com/digitalServices/pdf/ap/IN120085263_ChemistryCED_Effectiv
e_Fall_2013_lkd.pdf
By the end of this course, students should be prepared to take the AP chemistry exam offered by the
College Board.
Course Outline:
1.0 Lab Safety, lab equipment, reading a grad cylinder correctly
1.2 Scientific Method
1.3 Classification of matter (heterogeneous, homogeneous, element, compound, substance vs. mixture)
1.4 Chemical vs. physical Changes
1.5 Energy
1.6 SI Units, Density, Unit conversions, metric system
1.7 Significant Figures
1.8 Unit conversions, dimensional analysis
2.1-2.4 Atomic Theory
2.5 Structure of the Atom
2.6 P, N, E, Isotopes, Ions
2.7 Families on the Periodic Table
2.8 Average atomic mass
2.9 Molar Mass and Mole Conversions
*Mass Spectrometry
3.2 Ionic vs. Covalent Bonding
3.3 Chemical formulas and molecular models
3.4 Atomic-level View of Elements and Compounds
3.5 Ionic Nomenclature, Writing Formulas
3.6 Covalent Nomenclature, Acid Nomenclature
3.7 Summary of Nomenclature
3.8 Molar Mass and Mole Conversions
3.9 % by mass
3.10 Empirical and Molecular Formulas
3.11 Balancing Equations
3.12 Organic Compounds
4.2 Stoichiometry
4.3 Limiting reactant, theoretical yield, percent yield
4.4 Solution Concentration (Molarity, Dilution), solution stoichiometry
4.5 Electrolytes vs. non-electrolytes (solubility)
4.6 Precipitation reactions
4.7 Molecular, Ionic, Net ionic equations
4.8 Acid-Base/Gas-evolution reactions
4.9 Redox Reactions
5.1-5.2 Pressure
5.3 Gas Laws
5.4 Ideal Gas Law
5.5 Molar Volume, Density, Molar Mass
5.6 Partial Pressure
5.7 Gas Stoichiometry and Molar Volume
5.8 KMT
5.9 Diffusion/Effusion
5.10 Real Gases, IMF’s
6.1-6.2 Nature of Energy/Definitions
6.3 1st Law of Thermodynamics
6.4 Heat and Work
6.5 Measuring Energy
6.6 Enthalpy
6.7 Measuring delta H
6.8 Relationships involving delta H
6.9 Enthalpies of Reaction from enthalpies of formation
7.1-7.2 The Nature of Light
7.3 Atomic Spectroscopy and the Bohr Model
7.4 Wave Nature of Matter
7.5 Quantum mechanics and the atom
7.6 Shapes of Atomic Orbitals
*Beer’s Law
8.1-8.2 Development of the Periodic Table
8.3 Electron Configurations
8.4 Electron Configurations, Valence Electrons
8.5 Quantum-Mechanical Model
8.6 Periodic Trends
8.7 Ions-Trends
8.8 Electron Affinities
8.9 Examples of Periodic Behavior
*PES, Coulomb’s Law
9.1-9.2 Types of Chemical Bonds
9.3 Valence Electrons as dots
9.4 Ionic Bonding-Lewis symbols and Lattice energies
9.5 Covalent bonding-Lewis Structures
9.6 Electronegativity and Bond Polarity
9.7 Lewis Structures of Molecular Compounds and Polyatomic Atoms
9.8 Resonance and Formal Charge
9.9 Exceptions to the octet rule
9.10 Bond Energies and Bond Length
9.11 Bonding in Metals-Electron Sea Model
23.4-Alloys
10.2-VSEPR-Shapes
10.3 VSEPR-Lone Pairs
10.4 VSEPR-Molecular Geometries
10.5-Molecular Shape and Polarity
10.6-Valence bond theory-orbital overlap
10.7-Hybridization
10.8-Molecular orbital theory
11.2-Solids, liquids, gases
11.3-IMF’s
11.4-Surface tension, viscosity, capillary action
11.5-Vaporization and vapor pressure
11.6- Sublimation and fusion
11.7-Heating Curve for Water
11.8-Phase Diagrams
11.9-Water
11.10-X-ray crystallography
11.11-Crystalline solids-unit cells
11.12-Types of Crystalline Solids
11.13-Band Theory (Semiconductors)
*Chromatography (in relation to IMF’s)
12.1-12.2-Types of Solutions and Solubility
12.3-Energetics of Solution Formation
12.4-Solution Equilibrium and Factors affecting solubility
12.5-Expression Solution concentration
12.8-Colloids
12.6-7-Colligative Properties
*Beer’s Law
13.2-Rate of a chemical reaction
13.3-Rate Law
13.4-Integrated Rate Law
13.5-Effect of Temperature on Reaction Rate
13.6-Reaction Mechanisms
13.7-Catalysis
14.1-14.2-Dynamic Equilibrium
14.3-Equilibrium Constant
14.4-Expressing the equilibrium constant in terms of pressure
14.5-Heterogeneous equilibria: reactions involving solids and liquids
14.6-Calculating Equilibrium constant from measured equilibrium concentrations
14.7-Reaction Quotient
14.8-Finding Equilibrium Concentrations
14.9-Le Chatelier’s Principle
15.1-15.2-Nature of Acids and Bases
15.3-Definitions of Acids and Bases
15.4-Acid Strength and Ka
15.5-Autoionization of water and pH
15.6-Finding [H3O+] for strong and weak acid solutions
15.7-Base Solutions
15.8-Acid-base properties of Ions and Salts
15.9-Polyprotic Acids
15.10-Acid Strength and Molecular Structure
15.11-Lewis Acids and Bases
15.12-Acid Rain
16.2-Buffers (Henderson-Hasselbach)
16.3-Buffer Capacity
16.4-Titrations and pH Curves
16.5-Solubility Equilibria (Ksp)
16.6-Precipitation (selective precipitation)
16.7-Qualitative Chemical Analysis
17.2-Spontaneous (Favorable) vs. Non-spontaneous
17.3- Entropy and 2nd law of thermodynamics
17.4-Heat Transfer and Changes in the Entropy of the Surroundings
17.5-Gibbs Free Energy
17.6-Entropy Changes, Calculating delta S
*Maxwell-Boltzman distribution
17.7-Free Energy, Calculating delta G
17.8-Free Energy Changes in non-standard states
17.9-Free Energy and Equilibrium
Chapter 20
 Organic chemistry-nomenclature
 Organic chemistry-functional groups
 Polymers
 Biomolecules/Polymers with IMF’s
18.2-Balancing Redox Equations
18.3-Voltaic Cells
18.4-Standard Electrode Potentials
18.5-Cell Potential, Free Energy, and the Equilibrium Constant
18.6-Cell Potential and Concentration
18.7-Batteries
18.8-Electrolysis
18.9-Corrosion
AP chemistry exam review!!!
May 4-AP chemistry exam
Possible Lab Experiments:
The laboratory component of this course may include the following
experiments (but is not limited to) [CR5b and CR6]:
Traditional Labs: [Science Practices in brackets]
1.
2.
3.
4.
5.
6.
7.
8.
9.
Safety in the lab (proper use of equipment)
Accuracy and precision in measurements [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3]
Water of crystallization and formula of a hydrate [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3]
Evidence of a chemical change and energy changes in chemical reactions [4.3, 4.4, 5.1, 5.2,
5.3]
Percent oxygen in potassium chlorate [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3]
Flame tests and spectroscopy [1.2, 4.3, 5.1, 5.2, 5.3]
Molecular modeling to show molecular geometries [1.1, 1.3]
Analysis of a sodium bicarbonate-sodium chloride mixture [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3]
Finding the ratio of reactants in a chemical reaction (Stoichiometry of a reaction) [1.4, 2.1,
2.2, 2.3, 4.3, 5.1, 5.2, 5.3]
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
Reacting ionic species in aqueous solution [4.3, 5.1, 5.2, 5.3]
Molecular mass of a volatile liquid [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3]
Graham’s law [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3]
Titration experiment [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3]
Standardization of a base and then an acid [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3]
Analysis of a commercial bleach [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3]
Determination of an equilibrium constant [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3]
Ksp of an ionic compound [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3]
Determination of the dissociation constants of weak acids [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3]
Kinetics of a reaction [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3]
Redox titration with potassium permanganate [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3]
Electrochemical cells [1.2, 1.3, 1.4, 4.3, 5.1, 5.2, 5.3]
Thermochemistry and Hess’s law [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3]
Guided-inquiry labs: [3.1, 3.2, 3.3, 4.1, 4.2, 4.4, 6, 7.2]
1. How Can Color Be Used to Determine the Mass Percent of Copper in Brass?
2. How Much Acid Is in Fruit Juices and Soft Drinks?
3. How Can We Determine the Actual Percentage of H2O2 in a Drugstore Bottle of Hydrogen
Peroxide?
4. The Hand Warmer Design Challenge: Where Does the Heat Come From?
5. Can We Make the Colors of the Rainbow? An Application of Le Châtelier’s Principle
6. To What Extent Do Common Household Products Have Buffering Activity?
7. Photoelectric spectroscopy
AP 1-to-1 Initiative
As an AP student, you have been issued an iPad mini for class use, which is a privilege and a
responsibility.
Bring your device fully charged daily. Loss of class points and possible disciplinary referral will result
from failure to bring your device to class or inappropriate use of it (games , social media, etc).
Remember, your iPad is your responsibility; however, it is the property of the BVA School District, and its
content may be viewed by administration at any time.
Also, be advised that you are financially responsible for loss or damage to the device.
Academic Honesty:
Any work submitted by the student shall be his/her own. Work taken from others shall be
deemed as unacceptable. Any doubts will initiate the completion of an alternative assignment
or a zero on the required effort, depending on the severity of the infraction.
Class Policies and Expectations:
Classroom and Laboratory Expectations
1. Be on time and prepared for class (iPad, notebook, homework, pen, pencil, calculator,
etc.)
2. No food or drink.
3. No horseplay.
4. Respect others, their property, and this classroom.
Academic Expectations
All students are expected to participate in classroom activities and labs and to complete homework
assignments. Success in chemistry requires practice. Each assignment is designed to help you
succeed in this class. Therefore, you will be held accountable for completing every assignment.
Homework may be graded on accuracy, completeness, or both. Homework is due at the beginning
of class.
Class begins when the bell rings, and the expectation is that all students are in their seats and ready
to work. There will be a warm-up each day, which students are to begin as they enter the room.
If I see or hear your cell phone or iPod, I will take it off of you and give it to administration.
Assignments are due at the beginning of class. Points will be deducted from your score if the
assignment is turned in late.
Late Work
With an excused absence, students have the same number of days to make-up work as the number
of days they were absent. For example, if you are absent two days (Monday and Tuesday), you
have two days (Wednesday and Thursday) to make up work. Homework or other work that is one
day late will be worth half credit. Work will not be accepted more than one day late unless you
have spoken to the teacher ahead of time.
Chemistry is a cumulative subject which means that each topic builds on top of the previous topic.
Therefore, it is crucial that you attend EVERY class period ON TIME. Tests and quizzes will be
given approximately once a week. It is very difficult to catch up on classwork or make up labs
from several absences. Missing work will result in a zero on that assignment. It is your
responsibility to see the teacher after class or after school to make up any missed work.
MAKEUP TESTS: You have one week to make up a missed test, quiz, or lab. It is your
responsibility to schedule a time before or after school. This is done by scheduling an appointment
with the teacher. If you need to make up a lab or a test, you must arrange a time during study hall
or before school to meet with the teacher. If you are absent the day before a test you must still
take the test on test day. If you have an excused absence, you will have an equal number of days
to make up the work for full credit. Make up tests will be different than the test given on the
assigned date.
Plagiarism/Cheating:
Plagiarism or cheating will not be tolerated. Plagiarism or cheating in any form will result in a
zero on the assignment with notification of the parents and administration. Each and every
student is responsible for his/her own work.
Supplies
All students are expected to keep a notebook. The notebook is designed to help you stay
organized and as a studying tool. Please use it to your advantage.
You should bring the following supplies to class every day:
 Three ring binder or folder to keep papers organized
 Pen or pencil (preferably both)
 iPad
 Scientific Calculator
Course Grading Criteria:
All quizzes, tests, and projects will be graded according to the Belle Vernon Area School District
grading policy. Total points will be accumulated for all evaluated efforts in this class rather than
having letter grades per each effort. The grading scale is as follows:
A
B
C
D
F
-
90-100
80-89
70-79
60-69
0-59
Emphasis will be on formal assessments. Therefore grades will be weighted in this course.
Formal Assessments will account for 90% of a student’s grade (quizzes, tests, projects,
performance-based rubrics, essays, graded homework, etc.)
Informal Assessments will account for 10% of a student’s grade (homework for completion,
class participation, exit tickets, etc.)
Assignments per Quarter:
Homework/Classwork: 10 points each (approximately 20) =
Quizzes: 10 points each (approximately 7 quizzes) =
Tests: 150-200 points each (approximately 3-4 tests) =
Labs: 10 points each (approximately 8 per quarter) =
approx.. 200 pts
approx.. 70 pts
approx.. 600 pts
approx.. 80 pts
TOTAL POINTS = 950 Points (approximate)
*Assignments or assessments may vary due to pace of class and individualized
instruction.
Study Island:
Students will be expected to take advantage of the Study Island Preparation Software aligned to
the Keystone Exam Standards, AP Course Competencies, and SAT/ACT Preparation. The
students that invest their time utilizing this program have overwhelming performed better than
those that do not. If you are unable to have access to a computer or internet for this
requirement, there are ample opportunities during the school day to utilize laptops or the
computers in the Library.
Academic Standards:
Students will be reacquainted with the Pennsylvania Academic Standards that have been
adopted by the Department of Education, along with the Common Core Standards that are in
the process of being implemented nationwide. Students will be made aware of the importance
of the standards and the efforts to meet them.
Edline:
If
Grades will be updated every week on Edline. If you lost or cannot remember log in
information, please contact our Child Accounting Department at 724-808-2500 ext. 1108.
Schoolwires (Website):
My website will be updated every Friday. Course Topics, Assignments, and Quizzes and Tests
are also posted weekly. In this course, I will also use the iTunes U course to assign homework.
Contact Information
Email:
School phone: (724)808-2500 ext.
Chemistry can be a difficult subject for some students. My goal is to help each student succeed,
but the responsibility is shared. Each student is expected to participate, work on assignments and
ask questions. If you feel your student is struggling, please contact the teacher immediately.
I look forward to a new and exciting year of chemistry!
Course Policy-AP Chemistry 2014-2015
Please sign to indicate that you have read and understand the expectations for the class this year
as stated in the course syllabus and return it to the teacher.
Student’s Name
_____________________________________________________
Student’s Signature ____________________________________________________
Student’s Email Address:________________________________________________
Parent/Guardian’s Name _________________________________________________
Parent/Guardian’s Signature_______________________________________________
Date__________________________________________________________________
Parent/Guardian’s Email:_________________________________________________
Parent/Guardian’s Home phone number:___________________________________
Parent/Guardian’s Work phone number:___________________________________
Parent/Guardian’s Cell phone number:_____________________________________
Would you (the parent/guardian) like to receive email updates about the class?_______
Which phone number would you prefer the teacher to call to contact you?___________
What is the best time to contact you? _______________________________________
Comments or any other information you would like to share? _____________________
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Does your child have access to a computer or the internet at home to complete homework
assignments?
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