Course Syllabus - 2 -
XAVIER ALMAGUER
CHEMISTRY II AP
2017-2018
INSTRUCTIONAL OBJECTIVES: The AP Chemistry course is designed to be the
equivalent of the general inorganic chemistry course usually taken during
the first year of college. For some students, this course enables them to
undertake, as freshmen, second-year work in the chemistry sequence or to
register in other courses where the general chemistry course is a
prerequisite. The AP Chemistry course should be rigorous enough to
contribute to the development of the students’ abilities to think clearly
and to express their ideas logically and with clarity. The course covers
chemistry topics more in depth and with greater emphasis on chemical
calculations, mathematical formulation, and the theoretical aspects
involved in chemistry. (College Board, 2016).
The AP Chemistry course is designed and conducted to give the student a
deeper understanding in chemistry. Students are expected to take the
AP Chemistry exam given in May of each year. Passing this exam may allow
the student to enter the college chemistry sequence at a knowledge level
above that of the normal student. Students are expected to work at levels
higher (college level) than those found in a regular class, including
conducting advanced chemistry laboratories. Additionally, intense studying
outside of the regular class will be required for the student to be
successful. Even though students will be working on college level
material, it is advantageous to complete certain courses in high school
because teacher’s are able to tutor and encourage in a manner not usually
found in college.
Students entering the AP Chemistry course need to have a strong
mathematical background and to have successfully completed first year
chemistry. Completion of first year physics is also required. Concurrent
enrollment in AP Physics B and the AP Lab courses are required.
STUDENT OUTCOMES AND STANDARDS: Times listed for each section are approximations. At the end of the section, The student will be able to:
INSTRUCTIONAL STRATEGIES AND ACTIVITIES: The objectives will be addressed
through a combination of the following strategies:
1. Interactive class discussion and lecture with extensive question and
answer format.
2. Guided practice using sample problems that is extended to independent
practice in problem solving.
3. Laboratories using the scientific method, problem solving and
scientific measurements.
4. Data collection and analyses utilizing CBL and computer technology.
5. Use of video technology and computer simulation to enhance
instructional activities.
GRADING POLICY
Assignments may be entered into more than one category.
Tests 30%
Projects 20%
Participation/Progress Monitoring 10%
Class work/ Homework 40% _____
100%
FALL SEMESTER
Chapter 1: Foundations & Introduction 1.50 Hours
TOPICS COVERED / BIG IDEA / EU / EK / LOStudents Will:
1. Classify a substances properties as chemical or physical.
2. Compare the properties of compounds, mixtures & elements.
3. Perform calculations with numbers written in exponential notation using significant digits and SI units using dimensional analysis.
4. Solve problems using the mass, volume, and density relationship.
5. Distinguish between accuracy and precision.
6. Complete Quest Assignment: Scientific Measurements. / 1
3 / 1.A
1.B
1.E
3.C / 1.A.1a-d
1.B.1a-e
1.E.1.a
1.E.2.b
3.C.1.a-d / 1.1
1.17
3.10
Chapter 2 and 3: Atoms, Molecules and Moles 2.25 Hours
TOPICS COVERED / BIG IDEA / EU / EK / LOStudents Will:
1. Compare and contrast electrons, protons and neutrons in terms of location, charge, relative charge and relative mass.
2. Distinguish among atoms, molecules, ions and isotopes.
3. Determine the atomic mass of an element based on relative isotope abundance data.
4. Apply the following terms to locations on the periodic table: groups, periods, representative elements, transition elements, inner-transition elements, metals, nonmetals, metalloids, alkali metals, alkaline-earth metals, halogens, noble gases.
5. Describe the general properties of families in the representative elements and of the transition elements in general.
6. Apply concepts of the mole, gram-atomic mass (molar mass), molar volume at STP and Avogadro's number in problem-solving for elements and compounds.
7. Complete Quest Assignment: Atoms and Moles. / 1
3 / 1.A
1.B
1.E
3.C / 1.A.1a-d
1.B.1a-e
1.E.1.a
1.E.2.b
3.C.1 / 1.1
1.17
3.10
Chapter 2 and 3: Formulas and Nomenclature 5.25 Hours
TOPICS COVERED / BIG IDEA / EU / EK / LOStudents Will:
1. Discuss the differences between ionic and molecular (covalent) compounds.
2. Identify and use elements and ions.
3. Write formulas and/or names for ionic compounds, molecular (covalent) compounds, acids and oxyacids, and selected organic compounds including simple alkanes, alkenes, alkynes, alcohols and carboxylic acids containing chains of 1-10 carbons.
4. Calculate the molar mass of a substance; use the molar mass and Avogadro's number to convert among mass, moles and number of particles.
5. Determine the percent composition (by mass) of a compound from its formula and/or from lab data and determine the empirical and molecular formulas.
6. Complete Quest Assignment: Nomenclature. / 1
2
5 / 1.A
2.A
2.B
5.D / 1.A.1.c,d
1.A.2.a-c
1.A.3.a-d
1.E.2.a
2.A.3,e,f
2.B.1.a-c
5.D.3.b / 1.1
1.2
1.3
1.4
1.17
1.18
2.10
2.11
5.11
Chapter 22: Organic 3.00 Hours
TOPICS COVERED / BIG IDEA / EU / EK / LOStudents Will:
1. Write condensed and expanded structural formulas and name alkanes, alkenes and alkynes.
2. Draw isomers (including cis-trans).
3. Describe the structure and bonding of benzene.
4. Recognize the basic functional groups (alcohols, carboxylic acids, esters, ketones, aldehydes, ethers, and amines, amino acids), name and draw structures for compounds containing these groups, and describe general characteristics of these groups.
5. Describe the structures, functions and formation of proteins, and their role in DNA and RNA.
6. Be familiar with the structures and characteristics of carbohydrates and lipids.
7. Complete Quest Assignment: Organic Chemistry. / 1
2
5 / 1.A
2.A
2.B
5.D / 1.A.1.c,d
1.A.2.a-c
1.A.3.a-d
1.E.2.a
2.A.3,e,f
2.B.1.a-c
5.D.3.b / 1.1
1.2
1.3
1.4
1.17
1.18
2.10
2.11
5.11
Chapter 3: Chemical Equations and Stoichiometry 6.00 Hours
TOPICS COVERED / BIG IDEA / EU / EK / LOStudents Will:
1. Write and balance chemical equations for these types of reactions:
(a) Redox, composition, decomposition, single and double displacement.
(b) Combustion of hydrocarbons.
(c) Precipitation reactions.
(d) Common acid-base reactions.
(e) Reaction of acidic and basic anhydrides.
2. Calculate the masses of reactants and products using chemical equations
(stoichiometric calculations) including the use of limiting reagents.
3. Calculate theoretical and percentage yields of reactions.
4. Perform percentage and empirical formula calculations using reaction data.
5. Identify and write net ionic equations for reactions.
6. Complete Quest Assignment Chemical Reactions. / 1
2
3
5
6 / 1.A
1.D
1.E
2.A
3.A
3.B
3.C
6.C / 1.A.1.a-d
1.A.2.a-c
1.A.3.a-d
1.D.2.a-c
1.E.1.a-c
1.E.2.a,c-f
2.A.3.a, h-j
3.A.1.a-d
3.A.2.a
3.A.2.c
3.B.1.a
3.B.3.a-d
3.C.1.d
6.C.3.d / 1.1
1.2
1.3
1.4
1.14
1.17
1.18
1.19
2.8
2.9
2.14
3.1
3.2
3.3
3.4
3.5
3.6
3.8
3.9
3.10
Chapter 4 and 11: Solutions and Reactions in Aqueous Solutions 13.50 Hours
TOPICS COVERED / BIG IDEA / EU / EK / LOStudents Will:
1. Describe the nature of aqueous solutions including the action of water as a solvent and characterize strong and weak electrolytes.
2. Write equations for dissolution of electrolytes and nonelectrolytes and write net ionic equations for reactions in aqueous solutions.
3. Use the concepts of molecular structure, pressure and temperature to explain solubility of a solute in a given solvent.
4. Apply Le Chatelier's Principle to the factors affecting solubility.
5. Explain the effects of colligative properties on the properties of solutions.
6. Determine the f.p. or b.p. of a nonelectrolytic solution or calculate the molar mass of a nonvolatile solute from f.p. or b.p. data.
7. Describe the applications of osmosis and osmotic pressure; relate osmotic pressure mathematically to solution concentration.
8. Compare the colligative properties of electrolytes to those of nonelectrolytes.
9. Characterize and give examples of colloidal dispersions.
10. Identify common strong and weak acids and bases; write their dissociation equations.
11. Determine the solubility of ionic compounds from general solubility rules.
12. Describe the preparation of and calculate the molarity of a specified solution.
13. Calculate mass of solute, volume of solution or concentration of solution
using molarity as the concentration term.
14. Convert among concentration terms for solutions: molarity, molality, mass percent, mole fraction.
15. Interpret and apply qualitative concentration terms: saturated, supersaturated, unsaturated, miscible, immiscible.
16. Perform dilution calculations.
17. Perform stoichiometric calculations for solutions using molarity.
18. For metathesis reactions:
(a) Predict the products of these reactions, identifying the reactants & products by phases.
(b) Perform stoichiometric calculations for these reactions.
(c) Perform calculations involved in acid-base volumetric analysis.
(d) Perform calculations of chemical analysis of precipitation reactions.
19. Describe the process and uses of titration
20. Assign oxidation numbers to various the elements in various species and identify the oxidized and reduced substances.
21. Balance redox reactions in acidic and basic solutions.
22. Perform calculations associated with redox titrations.
23. Complete Quest Assignment: Solution Basics.
24. Complete Quest Assignment: Redox Reactions.
25. Complete Quest Assignment: Solution Properties. / 1
2
3
6 / 1.E
2.A2.D
3.A
3.B
6.C / 1.E.1.a-c
1.E.2.a-f
2.A.1.c,e
2.A.3.a-j
2.B.2.b
2.B.3.a,b
2.D.1.a.1-5
3.A.1.a-d
3.B.2.b
3.B.3.a-e
6.C.1.a-d
6.C.3.d / 1.16
1.17
1.18
1.20
2.1
2.2
2.3
2.7
2.8
2.9
2.10
2.13
2.15
2.16
2.24
3.2
3.7
3.8
3.9
6.11
6.12
6.13
6.15
Chapter 18: Electrochemistry 6.00 Hours
TOPICS COVERED / BIG IDEA / EU / EK / LOStudents Will:
1. Assign oxidation numbers to each element in a compound or ion and identify oxidizing and reducing agents.
2. Write and balance net ionic equations for redox reactions.
3. Solve titration problems for redox reactions, using molarity.
4. Distinguish between galvanic and electrolytic cells.
5. For voltaic, electrolytic or galvanic cells:
(a) Diagram and label parts of the cell, including electron flow.
(b) Write half-reactions for processes at the electrodes.
(c) Write the balanced equation and the line notation for the cell.
(d) Determine the anode and cathode from reaction data.
6. Use standard reduction potentials to compare strengths of oxidizing and reducing agents, to calculate cell potential; and to predict spontaneity of a redox reaction.
7. Use the Nernst Equation to calculate EMF at non-standard conditions.
8. Relate cell potential to free energy and equilibrium values.
9. Apply Faraday's Law to electrolytic cells in calculating amount of products formed, time or current required or energy used.
10. Explain the electrochemical nature of lead storage batteries, corrosion.
12. Relate voltaic cells and Nernst to free energy and equilibrium.
13. Complete Quest Assignment: Electrochemistry. / 3
5
6 / 3.A
3.B
3.C
5.E
6.A / 3.A.1.a
3.B.3.a,c,d
3.C.3.a-f
5.E.4.a
6.A.1.b / 3.2
3.8
3.12
3.13
5.15
6.1
Chapter 6: Thermochemistry 6.00 Hours
TOPICS COVERED / BIG IDEA / EU / EK / LOStudents Will:
1. Describe the energy flow between a system and its surroundings.
2. Explain the significance of the first law of thermodynamics.
3. Distinguish among heat, temperature, work, kinetic and potential energies.
4. Use calorimetric data to determine the energy changes that occur.
5. Describe and discuss energy and the relationships between phases.
6. Use Hess's law to calculate the enthalpy change.
7. Write and solve equations to define enthalpies of formation.
8. Complete Quest Assignment: Thermochemistry. / 3
5 / 3.C
5.A
5.B
5.C
5.E / 3.C.2.a-d
5.A.2.a-f
5.B.1.a-c
5.B.2.a,b
5.B.3.a,b,e,f
5.B.4.a-c
5.C.2.c,f,g
5.E.2.a / 3.11
5.3
5.4
5.5
5.6
5.7
5.13
OBJECTIVES: Chapter 17: Thermodynamics 7.50 Hours
TOPICS COVERED / BIG IDEA / EU / EK / LOStudents Will:
1. Discuss First Law of Thermodynamics.
2. Define entropy in terms of positional probability.
3. Predict and relate the signs of DH and DS to "favored" direction of a reaction.
4. Describe and evaluate the Second and Third Laws of Thermodynamics.
5. Apply the relationship between DS, DH to the surroundings.
6. Calculate DS for reactions or phase changes.
7. Use the Gibbs-Helmholtz equation to calculate the free energy for a
reaction and relate DG, DH, and DS to reaction spontaneity.
8. Relate thermodynamic values of enthalpy, entropy, and free energy to equilibrium and electrochemistry both qualitatively and quantitatively.
9. Complete Quest Assignment: Thermodynamics. / 2
5
6 / 2.B
5.A
5.C
6.D / 2.B.3.b
5.A.2.a,b,c,e
5.C.2.d,e
5.E.1.a,b,c
5.E.2.b-f
5.E.3.a-c
5.E.4.a-c
5.E.5.a,b
6.D.1.a-d / 2.15
5.3
5.12
5.13
5.14
5.15
5.16
5.17
5.18
6.25
Chapter 7: Quantum Mechanics, Atomic Structure and Periodicity 10.50 Hours
TOPICS COVERED / BIG IDEA / EU / EK / LOStudents Will:
1. Describe and discuss atomic models and their formation.
2. Describe, relate and quantify the electromagnetic spectrum sections of the spectrum, relative frequencies, wavelengths and energies of the sections.
3. Use photoelectron spectrophotometry data to explain and evaluate electron location.
4. Describe Planck's concept of quantitized energy.
5. Calculate the energy of a photon using the relationship
A = hv.
6. State the significance of the de Broglie relationship, and use this
relationship in calculations.
7. Relate Bohr's model of the atom to the quantum theory.
8. Calculate the energy difference resulting from the change in electron levels of an electron; calculate the ionization energy for an electron.
9. Describe the contributions of Heisenberg and Schrodinger to the wave mechanical model concept of the atom.
10. State the meaning and possible values of the quantum numbers assigning them to a given sublevel or orbital.
11. Describe a given sublevel, orbital or electron in quantum number terms and use Hund's Rule to assign an electron configuration for a given element or ion.
12. Construct the orbital diagram of an element.
13. Identify paramagnetism and diamagnetism through electronic structure.
14. Describe how effective nuclear charge varies with position on the
periodic table.
15. Use Coulomb’s Law to explain periodic patterns and electron locations.
16. Using the electron configurations and the concept of effective nuclear charge, interpret the trends within the periodic table for the following
properties: atomic and ionic radii, ionization energy, electron affinity.
17. Complete Quest Assignment: Quantum Theory.
18. Complete Quest Assignment: Periodic Trends. / 1
4
5 / 1.B
1.C
1.D
4.A
5.E / 1.B.1.a-d
1.B.2.a-d
1.C.1.a-d
1.C.2
1.D.1.a,b
1.D.3.a,b
4.A.1.b
5.E.4.b.1 / 1.5
1.6
1.7
1.8
1.9
1.10
1.11
1.12
1.13
1.15
4.a.1
5.e.4
Chapter 19: Nuclear Chemistry 2.25 Hours