SC72W CP Chemistry Using Modeling Instruction 2010-11
Instructor: Ray Hayes (rhayes@mpsaz.org)
Best time to call Mon. – Fri. 6:15 – 7:50 a.m.
Office Hours: Mon. – Fri. 1:10 – 2:01 p.m. (5th hr. prep)
Description:
This course focuses on key concepts in high school chemistry from a model-centered perspective.
Prerequisites:
Students should have strong math skills an interest in science and have demonstrated the ability to master difficult
concepts.
Course Objectives:
The emphasis is on learning concepts in chemistry from the perspective of systematically developed particle
models for matter. Instructional strategies include a coherent approach to the role of energy in phase change and
chemical change.
Grading:
This course is considered an accelerated (Honors) course and involves weighted grades toward the
overall g.p.a..
Grades are based on attendance, exams, homework and class participation.
Notebooks: An organized Chemistry notebook consisting of problems solved, labs done, worksheets on classroom
activities and assigned readings; is expected to be maintained throughout the year (as a study guide for the
semester & District finals). Work from notebooks are collected & graded for each unit.
Course Content (Major topics in bold; suggested topics below each major topic.)
A. Particulate structure of matter
Macroscopic vs microscopic descriptions. compounds, elements and mixtures.
Explanation of (observed) macroscopic properties using microscopic models.
Systematic explanation of details with models of increasing complexity.
Macroscopic evidence for microscopic structure (ionic vs molecular substances).
B. Energy and Kinetic Molecular Theory
Visualizable models (macroscopic analogs) for solids, liquids and gases.
Energy storage modes and transfer mechanisms.
Role of energy in phase change.
Distinction between heat and temperature.
C. Stoichiometry
The mole concept – relating how much to how many.
Using equations to represent chemical change.
Non-algorithmic approaches to chemical calculations.
D. Energy and chemical change (Thermodynamics)
Attractions vs chemical bonds.
Chemical potential energy and ∆H.
Activation energy and rates of chemical reactions.
Modeling Chemistry
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Syllabus
E. Molecular models
Diagrammatic representations of molecular structure.
3D models of molecular shapes.
Macroscopic behavior based on molecular structure.
F. History of the Models of the Atom
Examination of the scientists responsible for each of the Atomic Models. Ranging from Dalton to the present day.
Explanation of (observed) macroscopic properties using each model.
Macroscopic evidence for microscopic structure (ionic vs molecular substances).
G. Electrons
Visualizable models (macroscopic analogs) for the presence and behavior of electrons.
Evaluate the factors that influence the deflection of a charged particle.
Differentiate between atoms and ions.
Identify the characteristics of subatomic particles.
Distinguish between atomic number and atomic mass.
Determine the number of protons, neutrons and electrons in an isotope from its name or symbol.
Describe properties of waves and energy.
Explain the relationship between energy and the frequency of light.
Compare & contrast the different regions of the electromagnetic spectrum.
Explain how the bright-line spectrum of hydrogen demonstrates the quantized nature of energy.
Predict the position(s) of electrons in an atom, using the concepts of quantum numbers & orbitals.
H. Periodicity
Classification schemes used to arrange elements in Mendeleev’s periodic table & in modern periodic tables.
Distinguish between periods & groups on the periodic table.
Relate the electron configuration of an element to its position in the periodic table & its chemical properties.
Determine the valence electrons of representative elements, using the periodic table.
Predict the stable ions formed by a representative element, using the periodic table.
Understand the periodic nature of atomic radius & ionization energy.
Compare the size of an atom to the size of its ion & reason the difference.
Predict the properties of an element, using the periodic table.
I. Chemical bonding
Describe the nature of chemical bonding.
Compare & contrast the difference between ionic & covalent bonding.
Predict types of bonding; ionic, polar or polar covalent.
Determine the partial charge distribution of a polar covalent bond.
Apply the octet rule to write electron dot structures of simple molecules & polyatomic ions.
Identify limitations to the octet rule.
Predict molecular shapes.
Determine molecular polarity.
J. Reaction rates & Equilibrium
Explain rate & data necessary to determine rate.
Calculate the rate of reaction.
Determining rates from experiments
Identify factors that can affect the rate of reaction & recognize how a change in each factor can affect the rate.
Compare the rate of a reaction with & without a catalyst.
Demonstrate how potential energy of a substance is involved in a chemical reaction as the reaction progresses,
using a graph.
Modeling Chemistry
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Syllabus
Define a reaction mechanism & explain how the rate-determining step of the mechanism affects the overall rate
of reaction.
Explain & apply the macroscopic and microscopic definitions of equilibrium.
Identify chemical reactions that come to equilibrium and describe the process of reaching equilibrium.
Write the equilibrium constant expression for any reaction at equilibrium.
Calculate the equilibrium constant for any reaction at equilibrium.
Determine equilibrium concentrations, using the Keq
Explain LeChatelier’s principle & predict changes in equilibrium using this principle.
K. Acids & Bases
Distinguish between an acid and a base, using observable properties.
Define acids & bases by applying the Bronsted-Lowery definition.
Identify conjugate acid-base pairs.
Describe titration & calculate the concentration of an acid or base, using the results of a titration.
Apply the concept of pH to the description of acid and base solutions.
Interpret the pH scale using the ion-product constant of water, Kw
Compare acid strength using the acid dissociation constant, Ka
Study the affects of a buffer in preventing changes in pH.
L. Nuclear Chemistry
Understand the difference between ionizing & nonionizing radiation.
Identify the different types of radioactive decay & use equations to represent changes.
Determine mass loss in nuclear decay & using Einstein’s equation, calculate the energy released.
Predict fraction of radioactive nuclei remaining after time, when given the half-life. (T1/2)
Comparative study of nuclear fission and nuclear fusion.
Overview of America’s development of its Atomic Program.
Modeling Chemistry
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Syllabus