AP Chemistry Syllabi/Prospectus
2010-2011
Mr. Niedenzu
New information from CMS: -very important-!
AP/IB Exam Policy:
As you are aware, effective with the 2010-2011 school year, CMS is no longer paying for students to take AP and IB exams as a result of the 2010-2011 budget adopted by the CMS Board of Education.
-The requirement that students in AP and IB courses must take the corresponding exam has been removed from CMS policy and regulations.
-There will be no penalty (i.e. reducing the student’s final letter grade) for students who choose not to take AP/IB exams.
-All students in these courses will be required to take a teacher-made comprehensive exam, which will count as 25% of their final course grade.
Payment Information and Options:
An individual will need to be designatedat each high school to be in charge of collecting and monitoring fees for AP and IB exams. Instructional Accountability Facilitators at each school may assist with this. The financial secretary at each school will have a separate account for AP exam fees and a separate account for IB exam fees if applicable.
All fees for AP and IB tests may be paid through the online credit card payment system, check, or money order. No cashwill be accepted. There will be a small convenience fee for paying online. The online payment system may be accessed through the CMS website on the Advanced Studies, Advanced Placement or IB pages. Checks and money orders will be received and receipted at the schools.
All Advanced Placement examination fees must be paid no later than Tuesday, September 28, 2010. The amount owed will vary from student to student based on the number of exams being taken. The AP exam fee is $86 per exam. Fees must be paid at the student’s high school or online. Students will be notified by their school of the exact amount that needs to be paid. Schools will order AP tests as usual for those students who have paid. Any test ordered but not paid for or waived will be paid by school funds. These exam orders are handled by the school test coordinator as in the past.
Fee Waivers: AP
Students who are economically disadvantaged and cannot afford AP exams can complete a form (the Application for Needs-Based Assistance) certifying a certain income level that will entitle them to a fee waiver [funded by the College Board and a grant at NCDPI]. This form is attached. Schools should forward AP fee waivers to the Office of Accountability.
Students who do not submit an Application for Needs-Based Assistance, and who do not meet the deadline for exam fee payment will NOT receive a test. Schools are responsiblefor tracking fees and informing students.
Students who do not submit an Application for Needs-Based Assistance, and who do not meet the deadline for exam fee payment will NOT receive a test. Schools are responsiblefor tracking fees and informing students. IB students who do not meet the deadline for exam fee payment will be given a communication upon missing the deadline outlining the impact on program participation. Schools are responsible for tracking fees and informing students.
Sponsorship Opportunities:
For families and students interested in sponsorship, a tip sheet and sponsorship form may be found online on the CMS Advanced Placement and IB homepages.
For questions or concerns please contact Kathleen Koch in the Advanced Studies Office– , 980-343-2701.
Overview: The AP Chemistry course meets daily for one 90 minute period. Labs are conducted during the week on alternating days. This course is designed to provide a solid, first-year college chemistry experience, both conceptually and in the laboratory. The labs serve to supplement the learning in the lecture section of the course. Problem-solving skills, both on paper and in the lab, are emphasized. There are weekly labs and during the last quarter three full practice AP tests are taken and graded according to AP grading scale.
Laboratory: Students are required to submit a complete report for each lab experiment, including a hypothesis, procedure, observations/data, calculations, sources of error, and a conclusion. All reports are kept in a lab notebook. The students are also called upon to make a presentation to the class about their hypotheses, calculations, and conclusions – in this way students can collaborate on the objectives and design of an experiment, and assist each other in reaching conclusions, and gain insights into variance and sources of error. Lab descriptions are listed at end of syllabus after the resources.
Reaction sets: Nationwide scores on the reaction sets on the AP exam are generally lower than one might or should expect. Our scores are always higher than the national average by a large margin because we practice these every week. We use all of the old AP reactions along with other sources including all the study guides – students receive a set each Monday and are required to turn them in on Friday. This year I have also included the balancing component which will be added on the exam this year along with a separate question on each – i.e. on a redox reaction can they identify which is the reducing agent or on an electrolysis reaction which gas is formed and on which electrode.
Class rules
Students need to have access to the internet to access my website and other resources we will use during the year.
Cell phone use is not allowed during the school day – if I see it or hear it, it will be confiscated and turned in to the front office.
No food is allowed in class. Only clear, colorless water bottles containing water will be permitted.
Cheating will not be tolerated.
Late work will have a letter grade deduction for each day late (unless there is some extenuating circumstance).
Behavior issues will be dealt with “in house” – the administration has many other things to deal with and I will handle these issues as they arise. Also, be forewarned, I DO call parents at home and at work, and I will call you at home if you have been absent or are absent to check on things.
Required materials:
materials for taking notes
scientific or graphing calculator
graph paper
colored pencils
Absences: I will follow the CMS guidelines on absences, please recheck your handbook on this.
If you are absent and want to stay current – email me immediately at school
I will respond immediately!!!
Lab safety:
All students will undergo a review of lab safety rules and have to sign (along with the parents) that they have read the safety rules, watched the safety video, know where all the safety equipment in the room is located and the proper way to use it.
Homework:
I do not assign a lot of homework at once – the problems I do assign are carefully selected – some of the assignments are already on my web page, some will have answers with the questions.
Assignments/quizzes:
BEWARE: I will give short quizzes in class almost every day!!! I do give retakes on these if needed.
Missed assignments:
CMS allows you 5 days to schedule a time/due date to turn in missed assignments – remember it is your duty to take care of this!
Grades:
I operate on the point system and generally most classes will have over 1000 points accumulated for each quarter. I will follow CMS guidelines on grade distribution. Point distribution is as follows:
Quizzes: anywhere from 5 – 20 points
Homework: from 10 – 20 points
Lab reports: from 20 – 50 points
Tests: from 30 – 70 points
We will go over lab report format in class – be aware that this area is usually where many student’s grades suffer because they do not turn in reports on time! In general you will have a week to turn in reports after the lab is done.
Tutoring:
The chemistry department will have weekly scheduled tutoring availability – the schedule will be given to you during the first week of school. In the fall I have limited availability for tutoring due to coaching responsibilities. In the winter and spring I will be available after school each day for help.
Unit 1: Chemical FundamentalsApproximate number of days: 5
A.General aim:
To describe the properties of matter, scientific matter, and chemical calculations. Students should become familiar with the various pieces of lab equipment, working with sig figs, metric system, naming compounds, the mole concept
B. Content:
- Nomenclature
- Inorganic nomenclature
- Organic nomenclature
- give examples of alkanes, alkenes, alkynes, aromatics and aliphatics
- review structural formulas and functional groups
- review IUPAC nomenclature system
- Transition Metals and Coordination chemistry - Complex nomenclature
C.Content:
- English and metric systems
- SI units and prefixes
- Precision and accuracy
- Fahrenheit, Celsius, and Kelvin temperature scales
- Conversion factors
- Density calculations
- Classification of matter into subgroups
- Properties of matter
- Separation of mixtures
- Significant figures – on AP test allowed +/- one figure (put 3 and you will be ok most of the time)
- Assignments: Organic HW sets 1 p1091 #24 thru 40 even,and 2 p1093 #52-60 even, complex nomenclature practice sheet, organic test, complex nomenclature qz, old reaction prediction sets involving organic compounds;
- Labs: synthesis and analysis of aspirin lab – also Lab Safety Rules and procedures
Unit 2: Atomic Structure and the Periodic TableApproximate number of days: 10
A.General aim:
To gain an understanding of the development of atomic structure.
B.Content:
- Basic assumptions of Dalton’s atomic theory
- J.J Thompson’s determination of charge-to-mass ratio
- Millikan’s oil drop experiment
- Rutherford’s nuclear atom
C. General aim: To study nuclear particles, half life and radioactive decay.
D.Content:
- Characteristics of radiation
- alpha particles
- beta particles
- positron production
- electron capture
- gamma radiation
- Nuclear stability
- zone of stability
- magic numbers
- Rate of decay
- half-life
- first-order process
- Transformations
- accelerators
- synthesis of some transuranium elements
- Detection
- Geiger counter
- scintillation counter
- radiocarbon dating
- Binding energy-mass defect
- Nuclear fission
- chain reaction
- critical mass
- Nuclear fusion
- Nuclear reactors
E.Assignments: Homework set p337 # 40 thru 50 even, other practice problems and quizzes, test
Unit 3:Chemical StoichiometryApproximate number of days: 10
A.General aim:
To calculate quantities of materials reacted or produced in chemical reactions. Students will also apply the periodic law to chemical reactivity in predicting products along with discussing the activity series of the elements, distinguish between metals and nonmetals, use the properties of metals and nonmetals to predict reaction products including using the activity series to predict single replacement reactions. Also use the periodic table to predict common oxidation states.
B. Content:
- Mole concept
- Percent composition
- Determination of the empirical and molecular formula for a compound
- Write and balance equations for:
- combustion reactions
- synthesis reactions
- decomposition reactions
- single replacement reactions
- double replacement reactions
- begin practicing reaction predictions (note new format on AP test for thisyear!!) – 3 given, have to do all three, balance and answer other questions on them – used to pick 5 of 8 with no balancing or other questions
- Mass-mass calculations
- Calculations involving a limiting reagent
- Calculation of percent yield
C.Assignments: homework sets 1 page 124 # 34 – 58 even, set 2 page 125 # 60 – 96 even (a,b only), test, first sets of reaction prediction
D. Labs: % of Sulfate lab (gravimetric analysis), formula of hydrate lab (copper sulfate), molar ratio lab (single replacement with copper sulfate solution and solid iron)
Unit 4:Electronic structure and Periodicity(see also stoichiometry general aim)Approximate number of days: 6
A.General aim:
To describe the electronic arrangement within an element and to account for the periodicity of elements. Students should be able to name the major subatomic particles in an atom, types of radioactive emissions, discuss the Bohr model and the other models, work problems involving quantum numbers and energies of electron transitions, the various Rules and Principles, shapes of orbitals, basics of the periodic law, work problems involving nuclear binding energy and half-life, balance nuclear equations
B.Content:
- Electromagnetic radiation: wavelength, frequency, velocity
- Planck’s constant: energy and frequency
- Dual nature of light
- Bohr model
- Heisenberg’s uncertainty principle
- Electron probability distribution
- Quantum numbers and electron orbitals
- Paramagnetic vs. diamagnetic
- Shapes of probability charge clouds for s, p, d, f orbitals
- Pauli’s exclusion principle
- Wave mechanical model
- Aufbau principle
- Hund’s rule
- Electron configurations and dot diagrams for atoms
- IUPAC periodic table
- Effective nuclear charge and shielding
- Periodic trends in ionization energy, electron affinity, atomic and ionic radius
- Properties of elements by their periodic table group
- Lanthanide contraction
20. Colors- solutions/flame tests/precipitates/elements, especially transition metal salts
- Assignments: flame test demo, homework set 1 page 338 # 52,60,62 64,66, 68-80 even, set 2 page 340 #86-96 even; test
Unit 5:Chemical BondingApproximate number of days: 15
A. General aim:
To characterize chemical compounds according to the type of bonding and the structure of molecules. Students should be able to draw Lewis structures, use electronegativity to predict bond types, distinguish between polar and nonpolar, ude bonding principles to determine oxidation states, draw resonance structures, assign formal charge, compare VB theory to MO theory, use VSEPR, draw MO diagrams
B. Content:
- Types of chemical bonds
- why an ionic bond forms
- why a covalent bond forms
- electronegativity
- polar bonds, dipole moment
- Ionic bonds
- electron configurations
- formulas
- lattice energy
- Covalent bonds
- localized electron-pair model
- bond energy
- Lewis structures
- octet rule and exceptions
- molecular geometry, VSEPR, sigma and pi bonds
- formal charge
- shortcomings of valence bond theory: resonance
- molecular orbital model
- bond order
- delocalization of orbitals
4. Isomerism
a. Geometric isomers
b. Stereoisomers
C.Assignments:Molecular model labs, synthesis and analysis of alum lab, homework sets # 22-90 even (due various days, a and b only on those that have more two questions) p. 403-406, quizzes, test
D.Labs: .Molecular model labs, synthesis and analysis of alum lab
Unit 6:GasesApproximate number of days: 8
A. General aim:
To investigate the laws and models that describe the properties and behavior of gases. Students should know the kinetic-molecular theory, intermolecular forces, units used in gas law problems, interpret phase diagrams and solubility curves along with working out gas law problems
B.Content:
- Measuring pressure: units, manometers and barometers
- Gas laws: Boyle, Charles, Guy Lussac, Avogadro, Ideal, Dalton, Graham
- Gas stoichiometry
- STP
- molar volume
- mass-volume calculations
- Kinetic-molecular theory
- explain properties of gases
- define temperature
- Real gases
- deviation from ideal behavior
- van der Waals correction
- Assignments: homework sets 1,2,3 (set 1 p. 233 32-46 even, set 2 48-60 even, set 3 64-80 even) gas test; old AP essay questions
- Labs: Molar volume of gas lab, Dumas method lab (molar mass of gas), R constant lab using decomposition of potassium chlorate
Unit 7:Liquids and Solids Approximate number of days: 7
A. General aim:
To describe the intermolecular forces responsible for properties of liquids and solids and the process of changing from one state to another.
B.Content:
- Intermolecular forces
- dipole-dipole forces
- hydrogen bonding
- London dispersion forces
- Properties of the liquid state
- surface tension
- capillary action
- viscosity
- vapor pressure
- Types of solids
- amorphous
- crystalline cubic forms, close-packed forms
- Determination of crystal structure
- Bonding in metals
- electron-sea model
- band model
- Network atomic solids
- properties of carbon and silicon
- semiconductors
- Comparison of types of solids and properties
- Changes of state
- specific heat
- freezing point
- boiling point
- heat of fusion
- heat of vaporization
- Heating curve
- Phase diagrams
- water
- carbon dioxide
- Assignments: homework sets page p. 500 – 505, # 36 – 90 even over several days; test; magnet demo; old AP essay questions; sodium polyacrylate demo (“waterlok”)
- Lab: Spec 20 lab and chromatography labs using column chromatography(use Beer’s law)
Unit 8:Thermochemistry/ThermodynamicsApproximate number of days: 10
A.General aim:
To relate the fundamental aspects of the energy changes that accompany chemical reactions. Students should be able to solve problems involving Hess’s law, heat problems, calorimetry problems and interconvert with electro and equilibrium problems
B.Content:
- Concept of energy
- potential energy, kinetic energy
- first law of thermodynamics
- heat
- work
- state functions
- system and surroundings
- endothermic and exothermic reactions
- internal energy of a system
- Calorimetry
- use of a calorimeter
- heat capacity
- energy released as heat
- Enthalpy change for a chemical reaction
- Hess’s law
- standard enthalpies of formation
- heat of reaction, e.g., heat of combustion
C.General aim:
To predict whether or not a process is spontaneous, based on properties of the reactants and products.
D.Content:
- Second law of thermodynamics
- Spontaneity of process determined by entropy calculations
- ∆Gsurroundings = -∆Hsystem / T
- Calculation of ∆G for a process from standard free energies of formation
- ∆G = ∆H - T∆S
- Predicting spontaneity from ∆G
- Calculation of ∆G at conditions other than standard temperature
- Predicting spontaneity from sign notation of enthalpy and entropy
- Calculation of Keq from ∆G
E.Assignments: Specific heat lab, heat of neutralization lab, old AP essays, homework set 1 p. 819 #20-50 even, set 2 p. 282 #34-62 even, quizzes, test
F. Lab: Specific heat lab, heat of neutralization lab
Unit 9:SolutionsApproximate number of days: 8