Unit 1: Chemical Fundamentals - rdorrmets

CHEMISTRY II - ADVANCED PLACEMENT
2011-2012 SYLLABUS COURSE OVERVIEW: AP Chemistry meets every day during the school year for a
90 minute block. Students receive a packet of work to complete over the
summer that is due the first day of school. This reinforces the
fundamentals learned in Chemistry I. AP Chemistry is a rigorous class that
includes laboratory work at least once a week. This class is designed to
give high school students the same experience they would receive in a first
year college chemistry course. A major emphasis of this course is problem
solving, which must be practiced in both lab and daily in class work. Two
full length AP practice exams will be given during the 4th quarter and
graded according to the AP scale in preparation for the exam in May. LABORATORY: Lab experience is essential to a thorough understanding of a
concept in any science class. For each experiment, students are required
to submit a formal report which includes a hypothesis, procedure,
observations and data, calculations, sources of error, and a conclusion.
For several experiments students may be called on to present any aspect of
their report and lab experience to the rest of the class. This allows
students to critique each other and collaborate on concepts and make
connections between concepts with others. REACTION PREDICTION SETS: Reaction prediction is a concept that is
stressed in this course. Reaction prediction is practiced daily in this
class with warm ups after the second unit and weekly problem sets which
students turn in at the end of the week. I use problems from old AP Exams
as well as those found in several college textbooks. In response to the
change in format of Section II on the exam this year, students must also
answer two questions about each reaction (ex- precipitate color). 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, reaction prediction sets involving organic compounds for
warm ups
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, periodic trends project 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 - 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: formula of hydrate lab (copper sulfate), molar ratio lab
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 and identify hybridization.
B. Content:
1. Types of chemical bonds
a. why an ionic b