ROSE TREE MEDIA SCHOOL DISTRICT
Course Curriculum
GRADE/SUBJECT: Chemistry, Level I/Advanced Placement
ESSENTIAL QUESTIONS, CONCEPTS, AND THEMES
A. Math Review
B. Measurement of matter
C. Atoms, Molecules, and Ions
D. Stoichiometry, calculations with Chemical Equations
E. Aqueous Reactions and Solution Stoichiometry
F. Introduction to Thermochemistry
G. Electronic and Quanatum Structure of Atoms
H. Periodic Properties of the Atoms
I. Basic Concepts and Shapes in Chemical Bonding
J. Gas Laws, History and Application
K. Phase Changes, Intermolecular Forces
L. Properties of Solutions
M. Chemical Kinetics
N. Chemical Equilibrium
O. Acid-Base and Aqueous Equilibria
P. Selected Environmental Chemistry
Q. Chemical Thermodynamics
R. Electrochemistry
PENNSYLVANIA STANDARDS
A. 3.1.12.A, B
B. 3.2.12.A, B, C, D; 3.4.12.A, C; 3.7.12.A, B, C,
C. 3.2.12.A-D; 3.4.12.A, C; 3.6.12.B; 3.7.12.A, B
D. 3.1.12 C, D; 3.2.12.A-D; 3.3.12A; 3.4.12.A; 3.7.12.A, B
E. 3.2.12.C; 3.4.12.A; 3.7.12.B
F. 3.1.12.A-B; 3.2.12.A-D; 3.4.12.A-C; 3.7.12.B; 3.8.12.A, C
G. 3.1.12.A, B; 3.2.12.A-D; 3.4.12.A, B; 3.7.12.A, B
H. 3.1.12.A; 3.2.12.A, B, C, D; 3.4.12.A; 3.7.12.A, B
I. 3.1.12.A, B, C, B; 3.2.12.A-D; 3.3.12.A; 3.4.12A; 3.7.12.A, B; 3.8.12.A
J. 3.1.12.A, B, D; 3.2.12.A-D; 3.4.12.A-D; 3.7.12.A; 3.8.12.A
K. 3.1.12.A, B, D; 3.2.12.A-D; 3.4.12.A-D; 3.5.12.A-D; 3.7.12.A, B
L. 3.2.12.A, D; 3.7.12.A, B
M. 3.1.12.B; 3.2.12.C, D; 3.4.12.A, D; 3.7.12.A, B, C;
N. 3.1.12.A; 3.2.12.A-D; 3.4.12.A, E; 3.5.12.A-D; 3.7.12.A-D; 3.8.10.A-C
O. 3.1.12.A, C; 3.2.12.A-D; 3.4.12.A, B; 3.5.12.A, D; 3.6.12.A; 3.7.12.A-C; 3.8.10.A-C
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P. 3.1.12.A, B; 3.2.12.A-D; 3.4.12.A, B; 3.5.12.A-D; 3.7.12.A-D; 3.8.10.A-C
Q. 3.1.12.A; 3.2.12.A-D; 3.4.12.A, B; 3.5.12.A; 3.7.12.A-C
R. 3.1.12.A, C; 3.2.12.A-D; 3.4.12.A-C; 3.7.12.A-C
BENCHMARKS & SKILL SETS
A. Math Review
Benchmark # 1 Students will review their basic math skills to achieve a proficiency necessary
to do all Chemistry problem-solving and graphing throughout the year.
a.) Use basic Algebra to solve for unknown quantities, convert units, use scientific notation, use
significant figures and quadratic equations.
Benchmark # 2
Students will review graphing data and analyzing slopes and intercepts.
B. Measurement and matter
Benchmark # 1 Describe and evaluate the amount and volume of matter, micro and
macroscopically, identify Physical and Chemical changes.
Benchmark # 2 Interpret laboratory events both analytically and descriptively.
a.) Define distance, volume, and mass. Evaluate uncertainty in measurement and define
significant figures.
b.) Graph these quantities to define density.
c.) Write a lab report presenting purpose through conclusion using significant figures and
dimensional analysis.
C. Atoms, Molecules and Ions
Benchmark # 1 Appreciate the history of ancient atomic theory.
Benchmark # 2 Understand the work of Dalton, Maxwell, Thompson, Rutherford, Millikan,
and Curie.
a.) Calculate number and type of electrons, protons and neutrons in an atom from atomic
number, charge, mass number .
b.) Predict empirical formulae from ionic charges.
D. Stoichiometry, Calculations with Chemical Equations.
Benchmark # 1 Use models to demonstrate chemical reactions.
Benchmark # 2 Define the mole using atomic and molecular weights and the number of
particles.
Benchmark # 3 Use moles to predict masses in chemical reactions; stoichiometry.
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Benchmark # 4 Determine empirical and molecular formulae using percent composition and
combustion products.
Benchmark # 5 Define limiting reactants and theoretical yields.
a.) Use dimensional analysis to convert units.
b.) Interpret lab work to demonstrate stoichiometry, limiting reactants, and theoretical yields.
c.) Use scientific notation for calculations in atomic masses.
E. Aqueous Reactions and Solution Stoichiometry.
Benchmark # 1 Students will differentiate between ionic and molecular compounds in water.
Benchmark # 2 Students will generate and use solubility guidelines.
Benchmark # 3 Students will define basic acid-base and oxidation-reduction reactions.
a.) From precipitation labs determine solubility tables.
b.) Determine molarity and use molarity to predict the mass of precipitates.
c.) Use electrical conduction to determine which substances dissolve into ions or molecules.
F. Introduction to Thermo- chemistry
Benchmark # 1 Students will understand different forms of energy.
Benchmark # 2 Students will relate energy, work, and heat to each other.
Benchmark # 3 Students will understand calorimetry.
Benchmark # 4 Students will relate temperature changes and stoichiometry to enthalpy
changes.
Benchmark # 5 Students will use lab work to demonstrate fuel to mass ratio.
a.) Use formulae to calculate potential energy- kinetic energy to heat problems.
b.) Use lab work to determine the specific heat of a solid.
c.) From lab work and knowledge of stoichiometry demonstrate Hess’s Law.
G. Electronic and Quantum Structure of Atoms
Benchmark # 1 Appreciate the work of Bohr, Einstein, Planck, Schrodinger, Heisenberg, De
Broglie, Hund, and Pauli.
Benchmark # 2 Understand the nature of light as both waves and photons.
Benchmark # 3 Relate basic Spectroscopy to Energy Levels in atoms.
Benchmark # 4 Arrange electrons into the standard representation of Orbitals with the
appropriate Quantum Numbers.
Benchmark # 5 Show how Electron Configuration and the Periodic Table are related.
a.) Calculate wavelength, speed, and/or frequency of wave forms.
b.) Calculate Energy Levels from the frequency or wavelength of photons.
c.) Determine the ground state electron configuration for atoms to Z=38. (Strontium)
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d.) Be able to run around a soccer field in a pattern approximating a two dimensionsl path of an
electron in any orbital up to 3d.
H. Periodic Properties of the Atoms
Benchmark # 1 Predict the different Atomic Radii, Ionic Radii, Ionization Energies, and
Electronegativities as atomic numbers increase.
Benchmark # 2 Explain the trends in the above parameters of different atoms.
Benchmark # 3 Correlate the above trends with bonding behaviour of diferent groups.
Skills:
a.) Pattern recognition.
b.) Using the two criteria of Energy Level and Effective Nuclear Charge compare and contrast
the tendencies of atoms to gain or lose elcetrons and their relative tendencies to share
electrons.
I. Basic Concepts and Shapes in Chemical Bonding
Benchmark # 1 Illustrating the Octet Rule using Lewis Dot Structures.
Benchmark # 2 Using Electron Configurations to determine Ionic Bonding.
Benchmark # 3 Correlate Relative Ion sizes with different Crystal Shapes.
Benchmark # 4 Determine Polarity of Covalent Bonds using Electronegativity.
Benchmark # 5 Identifying Resonance Structures as an example of misusing a model when
another explanation is superior. (delocalized orbitals)
Benchmark # 6 Understand how the strength of covalent bonds relates to enthalpies of
reactions.
Benchmark # 7 Comparing Valence Shell Electron Pair Repulsion (VSEPR) theory with
hybrid orbital and delocalized orbital theories to predict molecular shapes.
Benchmark # 8 The effect of Non-Bonding Electron Pairs on Molecular Shapes.
Benchmark # 9 Drawing (for a multiple intelligence assessment) multiple bonds and
Molecular Orbitals.
Benchmark # 10 Be able to approximate all the bond angles in a sucrose (or similar) molecule.
a.) More pattern recognition in both two and three dimensions.
b.) To determine molecular polarity two criteria must again be applied, students must first
determine whether a sufficient difference in electronegativity exists to cause a dipole (or
dipoles) and then whether or not the shape of the molecule would create opposing dipoles
that would add to counteract each other.
c.) Draw many molecules indicating bond angles (shapes) and polarities.
J.
Gas Laws, History and Application.
Benchmark # 1 Appreciate the work of Avogadro, Boyle, Charles, Kelvin, Gay Lusac,
Graham, and van der Waals.
Benchmark # 2 Define Temperature, Pressure in basic units.
Benchmark # 3 Be abe to derive the ideal gas law from experimental information.
Benchmark # 4 Use Avogadro’s Law in stoichiometry.
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Benchmark # 5
Benchmark # 6
Law)
Benchmark # 7
Calculate densities of gases and partial pressures.
Use Kinetic Molecular Theory to compare molecular velocities (Graham’s
Deviating from ideal behavior, van der Waals.
a.) Be able to work with multi-variable equations, the ideal gas law, Graham’s Law and van der
Waals’ Law.
b.) Interpret graphs and set up experiments to isolate variables.
K. Intermolecular Forces, Phase Changes
Benchmark 1
Compare molecular motions in gases, liquids and solids.
Benchmark 2
Understand London dispersion forces, hydrogen bonding, ion dipole forces.
Benchmark 3
Compare intermolecular forces to predict boiling point.
Benchmark 4
Energy changes when phases change, as in how hurricanes get their energy,
and why we sweat.
Benchmark 5
Reading phase diagrams, understand Triple Point of Critical Point.
Benchmark 6
Use ionic sizes to calculate unit cell dimension and density.
Benchmark 7
Bonding in allotropic carbon forms and others.
a.) Be able to work with 3 dimensional structures in unit cells.
b.) The chapter Modern Materials in Chemistry, the Central Science, (Brown, LeMay)
is covered by student reports, posters, powerpoint presentations and skits.
L. Properties of Solutions
Benchmark 1
Describe the three steps (and energies) described in the process of dissolving
including the role of entropy.
Benchmark 2
Use of bond types in predicting solubility.
Benchmark 3
Predict pressure and temperature changes in solubility.
Benchmark 4
Use different measurement of solubility to calculate Colligative properties.
(M, m, X, %) for Osmotic P; Freezing, Boiling changes; Raoult’s Law.
a.) Deal with lots of conversions of units.
M. Chemical Kinetics
Benchmark 1
Collision Theory – number of collisions; energy of collisions; orientation of
collisions.
Benchmark 2
Calculate rate laws in terms of concentration changes with respect to time.
Benchmark 3
Describe how concentration, surface area and catalyst affect reaction rates.
Benchmark 4
Calculate first and second order reaction rate constants.
Benchmark 5
Review Arrhenius equation to find Activation Energy.
Benchmark 6
Demonstrate Activation Energy in distribution of Kinetic Energy Graphs.
Benchmark 7
Use elementary steps to determine rate laws.
Benchmark 8
Understand the role to catalysts.
a.) Plotting tangents to determine reaction rates.
b.) Adding the elementary steps to determine the chemical reaction.
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N. Chemical Equilibrium
Benchmark 1
Use experiments to establish the fundamental idea of chemical equilibrium:
reverse reactions in a closed system.
Benchmark 2
Use the competing rate constants to determine the equilibrium constant in
both concentration and pressure.
Benchmark 3
Calculate equilibrium constants from concentrated and vice versa.
Benchmark 4
Use LeChatelier’s Principle to predict changes in a system.
a.) Use stoichiometry to predict changes in concentration as a reaction progresses.
O. Acid-Base and Aqueous Equilibria
Benchmark 1
Review definition of acids and bases.
Benchmark 2
The autoionization of water to define pH.
Benchmark 3
The use of indicators in titrations.
Benchmark 4
Use of Ka and Kb for weak acids and bases to determine pH and vice versa.
Benchmark 5
Relating Ka to Kb through Kw.
Benchmark 6
How ions break down water.
Benchmark 7
Compare oxy acids, amino acids, and Lewis acids.
Benchmark 8
Common ion effect is studied for butter and solubility products.
Benchmark 9
Relating butter capacity to pH. Henderson-Haselbach equation.
Benchmark 10 Study neutratization curves in titrations.
Benchmark 11 Solubility and pH (H+or OH- as common ions)
Benchmark 12 Qualitative analysis. Use of flow charts.
a.) Extensive use of quadratic equations.
b.) Ph calculations require logarithms.
P. Selected Environmental Chemistry
Benchmark 1
Study of atmosphere and ozone reactions with CFL’s.
Benchmark 2
Show how acid rain is formed and how it affects materials and chlorophyl.
Benchmark 3
Understand the greenhouse effect.
Benchmark 4
The process of desalinization.
Q. Chemical Thermodynamics
Benchmark 1
Review spontaneous, reversible and irreversible processes.
Benchmark 2
The second Law of Thermodynamics and Entropy.
Benchmark 3
Appreciate why order requires so much energy to be maintained.
Benchmark 4
Apply the third law of thermodynamics to find entropy changes in a reaction.
Benchmark 5
Use Gibbs free energy to determine spontaneity.
Benchmark 6
Using free energy to solve for temperatures at equilibrium and the equilibrium
constant.
Benchmark 7
Clausius-Clapeyron equation.
R. Electrochemistry and Oxidation
Benchmark 1
Balancing oxidation-reduction reactions by numbers
Benchmark 2
Balancing by half reactions
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Benchmark 3
Benchmark 4
Benchmark 5
Benchmark 6
Benchmark 7
Benchmark 8
Benchmark 9
Benchmark 10
Benchmark 11
Oxidation and Reduction Potentials.
The molecular view of the electrode processes.
Using standard reduction potentials to calculate voltaic potentials.
Oxidizing and reducing agents.
Spontaneity of Redox reaction; free energy and voltage.
The Nernst equation – concentration and cell potential equilibrium.
Common batteries. Lead-acid, alkaline, nickel-cadmium
Fuel cells: theory and practice
Corrosion: the use of anodic zinc and magnesium
PRODUCTS, PERFORMANCES, ASSESSMENTS
ALIGNED MATERIALS/RESOURCES/TECHNOLOGY
INSTRUCTIONAL STRATEGIES
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ADAPTATIONS/INCLUSION TECHNIQUES
All units A - L can be adapted to any individual IEP.
. Students with physical handicaps have full access to academic classroom exercises, as well as
laboratory exercise. We have handicapped accessible desks. We also rotate student lab groups,
which will also change their contribution to the group during each lab exercise.
. Students with mental handicaps can have individual IEP's developed so that they can compete
to the best of their ability with all comparably capable students.
ENRICHMENT STRATEGIES
REMEDIATION STRATEGIES
INTERDISCIPLINARY CONNECTIONS/MULTICULTURAL STRANDS
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