Unit 1: Chemical Fundamentals
AP Chemistry Syllabi/Prospectus
2015-2016
Mr. Niedenzu
AP/IB Exam Policy:
As you are aware, CMS pays the exam fee for students to take AP and IB exams
- Students must take the AP exam or take a teacher made exam at the end of the year that will count as 20% of their final grade
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: Are no longer part of the AP exam specifically but a good knowledge thereof is essential to answer some questions.
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. Assignments will be listed as either formal (70% of the quarter grade) or informal (30% of the quarter grade) I will follow CMS guidelines on grade distribution which this year is on a ten point scale where 100-90 is an A, 89-80 is a B, 79-70 is a C, 69-60 is a D, below 60 is an F. 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. Before school is an option this year since I have first block planning all year.
Unit 1: Chemical Fundamentals Approximate 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:
1. Nomenclature
a. Inorganic nomenclature
b. Organic nomenclature
i. give examples of alkanes, alkenes, alkynes, aromatics and aliphatics
ii. review structural formulas and functional groups
iii. review IUPAC nomenclature system
c. Transition Metals and Coordination chemistry - Complex nomenclature
C. Content:
1. English and metric systems
2. SI units and prefixes
3. Precision and accuracy
4. Fahrenheit, Celsius, and Kelvin temperature scales
5. Conversion factors
6. Density calculations
7. Classification of matter into subgroups
8. Properties of matter
9. Separation of mixtures
10. Significant figures – on AP test allowed +/- one figure (put 3 and you will be ok most of the time)
D. 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;
E. Labs: synthesis and analysis of aspirin lab – also Lab Safety Rules and procedures
Unit 2: Atomic Structure and the Periodic Table Approximate number of days: 10
A. General aim:
To gain an understanding of the development of atomic structure.
B. Content:
1. Basic assumptions of Dalton’s atomic theory
2. J.J Thompson’s determination of charge-to-mass ratio
3. Millikan’s oil drop experiment
4. Rutherford’s nuclear atom
C. General aim: To study nuclear particles, half life and radioactive decay.
D. Content:
1. Characteristics of radiation
a. alpha particles
b. beta particles
c. positron production
d. electron capture
e. gamma radiation
2. Nuclear stability
a. zone of stability
b. magic numbers
3. Rate of decay
a. half-life
b. first-order process
4. Transformations
a. accelerators
b. synthesis of some transuranium elements
5. Detection
a. Geiger counter
b. scintillation counter
c. radiocarbon dating
6. Binding energy-mass defect
7. Nuclear fission
a. chain reaction
b. critical mass
8. Nuclear fusion
9. Nuclear reactors
E. Assignments: Homework set p337 # 40 thru 50 even, other practice problems and quizzes, test
Unit 3: Chemical Stoichiometry Approximate 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:
1. Mole concept
2. Percent composition
3. Determination of the empirical and molecular formula for a compound
4. Write and balance equations for:
a. combustion reactions
b. synthesis reactions
c. decomposition reactions
d. single replacement reactions
e. double replacement reactions
f. begin practicing reaction predictions (note new format on AP test for this year!!) – 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
5. Mass-mass calculations
6. Calculations involving a limiting reagent
7. 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:
1. Electromagnetic radiation: wavelength, frequency, velocity
2. Planck’s constant: energy and frequency
3. Dual nature of light
4. Bohr model
5. Heisenberg’s uncertainty principle
6. Electron probability distribution
7. Quantum numbers and electron orbitals
8. Paramagnetic vs. diamagnetic
9. Shapes of probability charge clouds for s, p, d, f orbitals
10. Pauli’s exclusion principle
11. Wave mechanical model
12. Aufbau principle
13. Hund’s rule
14. Electron configurations and dot diagrams for atoms
15. IUPAC periodic table
16. Effective nuclear charge and shielding
17. Periodic trends in ionization energy, electron affinity, atomic and ionic radius
18. Properties of elements by their periodic table group
19. Lanthanide contraction
20. Colors- solutions/flame tests/precipitates/elements, especially transition metal salts
C. 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 Bonding Approximate 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:
1. Types of chemical bonds
a. why an ionic bond forms
b. why a covalent bond forms
c. electronegativity
d. polar bonds, dipole moment
2. Ionic bonds
a. electron configurations
b. formulas
c. lattice energy
3. Covalent bonds
a. localized electron-pair model
i. bond energy
ii. Lewis structures
iii. octet rule and exceptions
iv. molecular geometry, VSEPR, sigma and pi bonds
v. formal charge
b. shortcomings of valence bond theory: resonance
c. molecular orbital model
i. bond order
ii. 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: Gases Approximate 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:
1. Measuring pressure: units, manometers and barometers
2. Gas laws: Boyle, Charles, Guy Lussac, Avogadro, Ideal, Dalton, Graham
3. Gas stoichiometry
a. STP
b. molar volume
c. mass-volume calculations
4. Kinetic-molecular theory
a. explain properties of gases
b. define temperature
5. Real gases
a. deviation from ideal behavior
b. van der Waals correction
C. 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
D. 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:
1. Intermolecular forces
a. dipole-dipole forces
b. hydrogen bonding
c. London dispersion forces
2. Properties of the liquid state
a. surface tension
b. capillary action
c. viscosity
d. vapor pressure
3. Types of solids
a. amorphous
b. crystalline cubic forms, close-packed forms
4. Determination of crystal structure
5. Bonding in metals
a. electron-sea model
b. band model
6. Network atomic solids
a. properties of carbon and silicon
b. semiconductors
7. Comparison of types of solids and properties
8. Changes of state
a. specific heat
b. freezing point
c. boiling point
d. heat of fusion
e. heat of vaporization
9. Heating curve
10. Phase diagrams
a. water
b. carbon dioxide
C. Assignments: homework sets page p. 500 – 505, # 36 – 90 even over several days; test; magnet demo; old AP essay questions; sodium polyacrylate demo (“waterlok”)
D. Lab: Spec 20 lab and chromatography labs using column chromatography (use Beer’s law)
Unit 8: Thermochemistry/Thermodynamics Approximate 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:
1. Concept of energy
a. potential energy, kinetic energy
b. first law of thermodynamics
c. heat
d. work
e. state functions