PRE AP CHEMISTRY
INSTRUCTOR
Mrs. Cheryl A. Graves
email: cgraves@casciahall.org
Online Textbook www.hrw.com
WEB PAGE http://teacherweb.com/ok/casciahall/cgrraves/
TEXT
Modern Chemistry (Holt, Rinehart and Winston 2006)
INTRODUCTION
The Chemistry course is designed to cover the basic facts of
chemistry presented in a framework of laboratory experiments,
textual material, and review and evaluation techniques.
OBJECTIVES
Our first objective is to show students the importance of
chemistry in their major areas of study as well as in their daily
lives. In addition, we want students to see not only that
chemistry
provides the basis for much of what goes on in our world, but
also
that it is a vital, continually developing science. Students will
be prepared to enroll in AP
Chemistry at the completion of the course.
STRUCTURE
CURRICULUM OUTLINE FOR PRE-AP CHEMISTRY
I. FALL SEMESTER
A. First Six Weeks
1. Unit 1 – Introduction, Dimensional Analysis, Sig Figs,
Rounding, Metrics
a. scientific notation
b. learning to use a scientific calculator
c. metric prefixes
d. metric to metric conversions
e. metric to American and vice versa conversions
f. double-label conversions
g. cubic conversions
h. percent error, accuracy and precision
i. problem solving with dimensional analysis
j. significant digits and scientific rounding
2. Unit 2 – Lab Equipment, Safety, Properties of Matter
a. identification and function of laboratory equipment
b. safety rules, correct laboratory techniques and first
aid
c. MSDS sheets, NFPA hazard codes
d. physical and chemical properties of matter, intensive
and extensive
e. physical and chemical changes in matter
f. difference in weight and mass
g. theory, hypothesis, law
3. Unit 3 – Isotopes, Ions, Atoms
a. density and specific gravity
b. atomic structure of atoms and ions
c. isotopes, atomic number, mass number
d. average atomic mass
e. history of the evolution of the concept of the atom
4. Unit 4 – Light and Electron Configuration
a. electromagnetic spectrum
b. wavelength, frequency, energy of photons
c. writing electron configuration with the Diagonal Rule
d. writing electron configuration directly from the
Periodic Chart
e. abbreviated electron configuration
f. quantum numbers, Pauli’s Exclusion Principle, Hund’s
Rule
g. numbers of paired and unpaired electrons in atoms,
ions
h. irregular electron configuration
B. 2nd Nine Weeks
1. Unit 5– Periodic Chart and Trends
a. atomic size
b. ionization energy
c. electron affinity
d. electronegativity
e. ion size,
f. activity of metals and non-metals
g. multiple ionization energies
2. Unit 6 – Writing Correct Formulas for Compounds and Naming
Them
a. ion formation and oxidation numbers
`b. ions and oxidation numbers to memorize
c. ions with variable oxidation number
d. common acids
e. writing and naming binary compounds
f. writing and naming polyatomic compounds
g. writing and naming molecular compounds
h. writing and naming hydrocarbons
3 Unit 7 – Compound Stoichiometry
a. formula mass
b. moles
c. percent composition
d. empirical and molecular formulas
e. hydrates
f. Avogadro’s number problems
4. Unit 8 – Writing and Balancing Equations and Predicting
Products
a. Law of Conservation of Matter applied to atoms
b. writing and balancing equations with products and
reactants given
c. writing and balancing equations by predicting products
d. using the activity series of metals and non-metals to
predict products
5. Unit 9 – Reaction Stoichiometry
a. mass-mass, mass-mole, and mass-molecule problems
b. mass-volume and volume-volume problems at STP
c. limiting and excess reactants
d. percent yield and purity
II. SPRING SEMESTER
A. 3rd Nine Weeks
1. Unit 10 – Pressure, Temperature, Kinetic Energy and Gas Laws
a. kinetic energy
b. pressure conversions
c. temperature conversions
d. Boyle’s, Charles’, Gay-Lussac, combined gas laws
e. manometers
f. Dalton’s Law of Partial Pressure and gases collected
over water
2 Unit 11 , Ideal Gas Law and Gas Stoichiometry at Non-STP
a. solving for every variable in the ideal gas law
b. mass-volume and volume-volume problems at non-STP
conditions
c. mass-volume with limiting reactants at non-STP
d. Graham’s law of diffusion
3. Unit 12 – Bonding, Molecular Geometries, Bond Angles, Hybrids
a. Lewis dot structures for atoms and ions
b. Lewis structures for ionic compounds
c. Lewis structures for molecular compounds and
polyatomic ions
d. resonance
f. exceptions to the octet rule
g. geometric shape and bond angles of molecules and
polyatomic ions
h. hybridization of the central atom
i. polar and non-polar bonds and particles
4. Unit 13 – Intermolecular Forces, Solutions, Colligative
Properties
a. Intermolecular forces and boiling point, vapor
pressure
b. solubility rules for ionic compounds in water
c. interpreting solubility curves
d. calculating concentrations of molarity, molality and
mole fraction
e. calculation freezing points and boiling points of
solutions
f. using freezing point depressions and boiling point
elevation to find MW
B. 4th Nine Weeks
1. Unit 14 – Acids, Bases and Salts
a. conjugate acids and bases
b. naming binary and oxyacids
c. pH, hydrogen and hydroxide ion concentrations
d. calculating pH of strong monoprotic acids
e. calculating pH of weak monoprotic acids
f. calculating pH of strong mono and di-hydroxic bases
g. calculating pH of pH of weak bases
h. calculating pH of acidic and basic salts
i. percent ionization
j. hydrolysis of salts
k. calculating the equilbrium constant of weak acids and
bases
2 Unit 15 – Thermodynamics
a. interpretation of values in a thermodynamics table
b. enthalpy changes in chemical reactions
c. entropy changes in chemical reactions
d. Gibb’s free energy and spontaneity
e. equilibrium temperature
f. calculating missing heat of formation values
g. thermochemical equations and mass-heat problems
h. interpretation of energy profile graphs
3. Unit 16 – REDOX
a. assigning oxidation numbers to each element in
polyatomic ions
b. identifying what is oxidized/reduced
c. identifying the oxidizing/reducing agents in a
reaction
d. balancing molecular redox equations in acidic solution
e. completing and balancing partial redox equations in
acidic solution
ACTIVITIES
Chapter exams will be given for each chapter and at least one
laboratory exercise per chapter completed. Homework will be
given
most evenings. Assignments will be on the "web" page by 5:00 pm.
In case of
computer problems call one of your classmates for the assignment.
GRADING
Grades will be calculated on a total point system.
Examinations
will comprise 60% of the grade with laboratory reports,homework
and quizzes
making up the remaining40%. All Lab reports must be computer
generated and submitted on time. Tests will be given on
Tuesdays.
In case of absence on the Monday before a test or on the actual
test
day, you will be expected to take your exam on Wednesday morning
at
7:20 and complete the test during the activity period or after
school. In
case of an absence of more than one day, arrangements can be made
for makeup
as the situation warrants. Students that "qualify" for extra teme
will begin
their test in Mrs. Clancy's office at 7:20 am and will complete
the exam
during their normal classroom time. ("qualify" = Counselor
Referral)
Grading Scale:
90-100 A
80-89 B
70-79 C
60-69 D
0-59 F
DAILY REQUIREMENTS
1. Students must bring their OWN TI-30 or above scientific
calculator to
class each day. TI-84 are recomended. Calculators are to be
clearly
labeled. An engraver will be furnished.
2. Students must furnish their own goggles labled Z-87 for
laboratory
experiments. Again, goggles mut be dlearly labeled.
3. Students must bring their OWN book, calculator, notebook and
pencil EVERY
day.
4. All assignments will be given on the teacher web page. It is
the
student's responsibility to check the web each evening.
