Syllabus: Mr. C. Rodriguezap Chemistrymiami Beach Senior High School

Syllabus: Mr. C. RodriguezAP ChemistryMiami Beach Senior High School

Syllabus: Mr. C. RodriguezAP ChemistryMiami Beach Senior High School

Course Description

This AP Chemistry course is designed to be the equivalent of the general chemistry course usually taken during the first year of college. For most students, the course enables them to undertake, as a freshman, second year work in the chemistry sequence at their institution or to register in courses in other fields where general chemistry is a prerequisite. This course is structured around the six big ideas articulated in the AP Chemistry curriculum framework provided by the College Board. [CR2] A special emphasis will be placed on the seven science practices, which capture important aspects of the work that scientists engage in, with learning objectives that combine content with inquiry and reasoning skills. AP Chemistry is open to all students that have completed a year of chemistry who wish to take part in a rigorous and academically challenging course.

Big Idea 1: Structure of matter

Big Idea 2: Properties of matter-characteristics, states, and forces of attraction

Big Idea 3: Chemical reactions

Big Idea 4: Rates of chemical reactions

Big Idea 5: Thermodynamics

Big Idea 6: Equilibrium

Textbooks and Lab Books

The College Board.AP Chemistry Guided Inquiry Experiments: Applying the Science Practices. 2013.

Brown, Theodore L.; LeMay, H. Eugene; Bursten, Bruce and Murphy, Catherine. Chemistry The Central Science 11th edition, New Jersey: Pearson Prentice Hall, 2009 [CR1]

Randall, Jack. Advanced Chemistry with Vernier. Oregon: Vernier Software and Technology, 2004.

Holmquist, Dan; Randall, Jack and Volz, Don.Chemistry with Calculators.Oregon: Vernier Software and Technology, 2006

Required Materials

Graphing calculator, splash proof goggles, and a laboratory notebook

The student will be expected to:

1. Read all the chapters in the book. Tests and quizzes will be based on it plus material covered in the lectures. Tests will be worth 3 grades, quizzes 1 grade.

2. Complete ALL laboratory work. Labs will be worth 2 grades and will be graded using the Lab Rubric.

3. Homework- It is important that you complete and understand all HW assignments. Tests and quizzes will be based on them. Some HW will be collected and will be worth 1 grade.

4. No late assignments will be accepted.

5. Make up assignments will only be given with an excused absence. Any make up tests or quizzes will be after school. This should not be a common occurrence.

6. Five or more unexcused absences during the year could result in a no credit.

Class Expectations:

1. Be on time and ready to learn each class period

2. Participate- Ask questions in class.

3. Respect all your classmates- be willing to help each other.

4. Attend after school tutoring if needed- do not fall behind.

5. Read and UNDERSTAND the material in the book.

6. Always do your best. Take pride in your work.

7. NO CHEATING- NOT TOLERATED-This will not help you in the future and speaks badly of you as a person.

Labs

The labs completed require following or developing processes and procedures, taking observations, and data manipulation. See lab list provided for lab details. Students communicate and collaborate in lab groups; however, each student writes a laboratory report in a lab notebook for every lab they perform. A minimum of 25% of student contact time will be spent doing hands-on laboratory activities. [CR5a]

The Parts of a Laboratory Report [CR7]

A specific format will be given to the student for each lab. Students must follow that format and label all sections very clearly. AP Chemistry lab reports are much longer and more in depth than the ones completed in the first year chemistry course. Therefore, it is important that students don’t procrastinate when doing pre-lab and post-lab work. Late labs will not be accepted. Labs not completed in class must be done during lunch or after school by appointment ONLY.

Pre-Lab Work Pre-lab work is to be completed and turned in on the day the lab is performed.

1. Title The title should be descriptive. For example, “pH Titration Lab” is a descriptive title and “Experiment 5” is not a descriptive title.

2. Date This is the date the student performed the experiment.

3. Purpose A purpose is a statement summarizing the “point” of the lab.

4. Variables

5. Materials

6. Procedure Outline Students need to write an outline of the procedure. They should use bulleted statements or outline format to make it easy to read. If a student is doing a guided inquiry lab, they may be required to write a full procedure that they develop.

7. Pre-Lab Questions:Students will be given some questions to answer before the lab is done. They willneed to either rewrite the question or incorporate the question in the answer. The idea here is that when someone (like a college professor) looks at a student’s lab notebook, they should be able to tell what the question was by merely looking at their lab report. It is important to produce a good record of lab work.

8. Data Tables Students will need to create any data tables or charts necessary for data collection in the lab.

During the Lab

1. Data Students need to record all their data directly in their lab notebook. They are NOT to be recording data on their separate lab sheet. They need to label all data clearly and always include proper units of measurement. Students should underline, use capital letters, or use any device they choose to help organize this section well. They should space things out neatly and clearly.

Post-Lab Work

2. Calculations and Graphs Students should show how calculations are carried out. Graphs need to be titled, axes need to be labeled, and units need to be shown on the axis. To receive credit for any graphs, they must be at least ½ page in size.

3. Conclusions This will vary from lab to lab. Students will usually be given direction as to what to write, but it is expected that all conclusions will be well thought out and well written.

4. Post Lab Error Analysis Questions Follow the same procedure as for Pre-Lab Questions

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AP Chemistry Course Outline [CR2]

(BI) refers to Big Ideas. Big Idea 1- Structure of matter, Big Idea 2- Properties of matter, characteristics, states and forces of attraction, Big Idea 3- Chemical Reactions, Big Idea 4- Rates of chemical reactions, Big Idea 5- Thermodynamics, Big Idea 6- Equilibrium

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AP Chemistry Chapters Outline and Timeline:

Chapters 1-3Chemistry Fundamentals

Class Periods (90 minutes):9 periods

Homework sets assigned:Read the chapters and Chapter 1 (1 set), Chapter 2 (2 sets), and Chapter 3 (2sets)

Number of Exams1 exam with 2 quizzes

Topics Covered: Curriculum Framework Articulation:

1. Scientific MethodBI 1.D.1:a

2. Classification of Matter

a. pure substances vs mixtures1.A.1:b

b. law of definite proportions1.A.1:c

c. law of multiple proportions 1.A.1:d

d. chemical and physical changes 3.C.1:b, 3.C.1:c, 5.D:2

3. Nomenclature and formula of binary

Compounds1.E.2:b

4. Polyatomic ions and other compounds 1.E.2:b

5. Determination of atomic masses 1.A.1:a

6. Mole concept1.A.3:b, 1.A.3:c, 1.A.3:d, 1.E.2:b

7. Percent composition 1.A.2:a

8. Empirical and molecular formula1.A.2:b

9. Writing chemical equations and drawn

Representations1.E.1:a, 1.E.1:c, 3.C.1:a

10. Balancing chemical equations1.A.3:a, 1.E.2:c, 1.E.2:d, 3.A.1:a

11. Applying mole concept to chemical

equations (Stoich)1.A.3:a, 1.E.1:b

12. Determine limiting reagent, theoretical and

% yield3.A.2:a

Chapter 4Aqueous Reactions and Solution Stoichiometry

Class Periods (90 minutes):6 periods

Homework sets assigned:Read the Chapter and 2 HW sets

Number of Exams:1 exam and 2 quizzes

Topics Covered:Curriculum Framework Articulation:

1. Electrolytes and properties of water2.A.3:h

2. Molarity and preparation of solutions 1.D.3:c, 2.A.3:i, 2.A.3:j

3. Precipitation reactions and solubility rules6.C.3:d

4. Acid Base reactions and formation of a salt

by titration1.E.2:f, 3.A.2:c

5. Balancing redox 3.B.3:a, 3.B.3:b, 3.B.3:c, 3.B.3:d

6. Simple redox titrations 1.E.2:f

7. Gravimetric calculations1.E.2:e

8. Redox and single replacement reactions3.A.1, 3.B.3:e, 3.C.1:d

9. Double replacement reactions 3.A.1, 3.C.1:d

10. Combustion reactions3.A.1, 3.B.3:e

11. Addition reactions3.A.1, 3.B.1:a

12. Decomposition reactions 3.A.1, 3.B.1:a, 3.C.1:d

Student Activity: Students will observe a series of chemical reactions using video demonstrations from websites. For each they will: Classify the type of reaction, 2. Write a balanced net ionic equation, 3. Write a brief description for each reaction. LO 3.1, 3.2 [CR3c]

Chapter 10Gases

Class Periods (90 minutes):5 periods

Homework sets assigned:Read the Chapter and 2 HW sets

Number of Exams:1 exam and 1 quiz

Topics Covered: Curriculum Framework Articulation:

1. Measurement of gases

2. General gas laws - Boyle, Charles, Combined,

and Ideal2.A.2:a, 2.A.2:c

3. Dalton’s Law of partial pressure 2.A.2:b

4. Molar volume of gases and Stoichiometry3.A.2:b

5. Graham’s Law

6. Kinetic Molecular Theory2.A.2:d, 5.A.1

7. Real Gases and deviation from ideal gas law 2.A.2:e, 2.A.2:f, 2.A.2:g, 2.B.2:c,2.B.2:d

8. Graham’s Law demonstrationLO 2.6; SP 1, 6

Chapters 6 and 7Atomic Structure

Class Periods (90 minutes):5 periods

Homework sets assigned:Read chapters and Chapter 6 (1 set), Chapter 7 (1 set)

Number of Exams1 exam and 1 quiz

Topics Covered:Curriculum Framework Articulation:

1. Electron configuration and the Aufbau

Principle1.B.2:a

2. Valence electrons and Lewis dot structures 1.B.2:c

3. Periodic trends 1.B.1:b, 1.B.1:c, 1.B.2:b, 1.B.2:d,1.C.1:c, 1.D.1:b, 2.C.1:a, 2.C.1:b

4. Table arrangement based on

electronic properties1.C.1:a, 1.C.1:b, 1.C.1:d

5. Properties of light and study of waves 1.C.2:e, 1.D.3:a, 5.E.4:b

6. Atomic spectra of hydrogen and energy levels1.B.1:d, 1.B.1:e, 1.D.3:b

7. Quantum mechanical model1.C.2:d

8. Quantum theory and electron orbitals 1.C.2:c

9. Orbital shape and energies 1.C.2:b

10. Spectroscopy 1.D.2:a, 1.D.2:b, 1.D.2:c, 1.D.3:b

Student Activity: Students enter data and construct graphs using Microsoft Excel to predict, demonstrate, and identify periodic trends. Class presentations of results and justify exceptions to the trends. LO 1.9 [CR3a]

Chapters 8 and 9Chemical Bonding

Class Periods (90 minutes):5 periods

Homework sets assigned:Read chapters and Chapter 8 (1 set), Chapter 9 (1 set)

Number of Exams1 exam and 1 quiz

Topics Covered:Curriculum Framework Articulation:

1. Lewis Dot structures 2.C.4:a

2. Resonance structures and formal charge 2.C.4:c, 2.C.4:d, 2.C.4:e

3. Bond polarity and dipole moments2.C.1:c, 2.C.1:e, 2.C.1:f

4. VSEPR models and molecular shape 2.C.4:b, 2.C.4:e, 2.C.4:f

5. Polarity of molecules2.C.1:e

6. Lattice energies1.B.1:a, 1.C.2:a, 2.C.1:d (1-2),2.C.2:a, 2.C.2:b, 2.D.1:b

7. Hybridization 2.C.4:g

8. Molecular orbitals and diagrams 2.C.4:h, 2.C.4:i

Chapters 11, 13Liquids, Solids and Solutions

Class Periods (90 minutes):5 periods

Homework sets assigned:Read chapters and Chapter 11 (1 set), Chapter 13 (1 set)

Number of Exams1 exam and 1 quiz

Topics Covered: Curriculum Framework Articulation:

1. Structure and bonding

a. metals, network, and molecular 2.A.1:a, 2.A.1:d, 2.C.3, 2.D.1:a,2.D.2:a, 2.D.1:b, 2.D.3, 2.D.4

b. ionic, hydrogen, London, van der Waals 2.A.1:b, 2.B.1:a, 2.B.1:b, 2.B.1:c,

2.B.2:a, 2.B.2:b, 2.B.2:c, 2.B.2:d,2.B.3:a, 5.D:1

2. Vapor pressure and changes in state

3. Heating and cooling curves 2.A.1:e, 5.B.3:c, 5.B.3:d

4. Composition of solutions 2.A.1:c, 2.A.3:b, 2.A.3:c, 2.B.

5. Colloids and suspensions 2.A.3:a, 2.A.3:b, 2.A.3:g

6. Separation techniques2.A.3:e, 2.A.3:f

7. Effect on biological systems2.B.3:e, 2.D.3, 5.E.4:c

Teacher Lab Demo: Evaporation of liquidsLO 2.11, 2.18, 5.9, 5.12;

Student activity: Students are given structures of different compounds and must explain why they differ in physical states at various temperatures; then predict the type(s) of bonding present based on the atom’s position on the periodic table. LO 2.1, 2.13, 2.17, 2.19 [CR3b]

Chapter 14Kinetics

Class Periods (90 minutes):5 periods

Homework sets assigned:Read the chapters and Chapter 14 (2 sets)

Number of Exams1 exam and 1 quiz

Topics Covered: Curriculum Framework Articulation:

1. Rates of reactions 4.A.1:a

2. Factors that affect rates of reactions/

collision theory4.A.1:b, 4.A.1:c, 4.D.1, 4.D.2

3. Reaction Pathways 4.B.3:a, 4.B.3:b

4. Rate equation determination4.A.2:a

a. rate constants 4.A.3

b. mechanisms4.B.1, 4.C.1, 4.C.2, 4.C.3

c. method of initial rates4.A.2:c

d. integrated rate laws4.A.2:b, 4.A.3:d

5. Activation energy and Boltzmann

Distribution4.B.2, 4.B.3:c

Student Activity: Students present orally in class the solution to a problem given a set of data of the change of concentration versus time to the class, indicating the order of the reaction and the rate constant with appropriate units. LO 4.2 [CR3d]

Chapter 15Chemical Equilibrium

Class Periods (90 minutes):5 periods

Homework sets assigned:Read the chapters and Chapter 15 (2 sets),

Number of Exams1 exam and 1 quiz

Topics Covered: Curriculum Framework Articulation:

1. Characteristics and conditions of chemical

Equilibrium6.A.1, 6.A.3:a, 6.A.3:f

2. Equilibrium expression derived from rates 6.A.3:b

3. Factors that affect equilibrium 6.A.3:c

4. Le Chatelier’s principle 6.A.3:b, 6.B.1, 6.B.2, 6.C.3:e,6.C.3:f

5. The equilibrium constant 6.A.3:d, 6.A.3.e, 6.A.4

6. Solving equilibrium problems 6.A.2

Chapter 16Acids and Bases

Class Periods (90 minutes):5 periods

Homework sets assigned:Read the chapters and Chapter 16 (2 sets),

Number of Exams1 exam and 1 quiz

Topics Covered: Curriculum Framework Articulation:

1. Definition and nature of acids and bases 3.B.2, 6.C.1:c, 6.C.1:d, 6.C.1:e,6.C.1:f

2. Kw and the pH scale6.C.1:a, 6.C.1:b, 6.C.1:g

3. pH of strong and weak acids and bases 6.C.1:h

4. Polyprotic acids 6.C.1:n

5. pH of salts

6. Structure of Acids and Bases

Chapter 17Additional Aspects of Aqueous Equilibria

Class Periods (90 minutes):5 periods

Homework sets assigned:Read the chapters and Chapter 17 (2 sets),

Number of Exams1 exam and 1 quiz

Topics Covered: Curriculum Framework Articulation:

1. Characteristics and capacity of buffers 6.C.2

2. Titrations and pH curves 6.C.1:i, 6.C.1:j, 6.C.1:k, 6.C.1:l,6.C.1:m

3. Choosing Acid Base Indicators

4. pH and solubility

5. Ksp Calculations and Solubility Product 6.C.3:a, 6.C.3:b

Student Activity: Students determine the pH of different buffer solutions and describe the mechanism that would occur within the buffer system upon the addition of an acid or a base. LO 6.20 [CR3f]

Student Activity: Students conduct an investigation into the major components of acid rain and write the reactions that occur between the pollutant and the compounds naturally present. LO 3.2 {CR3c] and [CR4]

Chapters 5, 8.8 and 19Thermodynamics

Class Periods (90 minutes):10 periods

Homework sets assigned:Read the chapters and HW (6 sets)

Number of Exams1 exam and 3 quiz

Topics Covered: Curriculum Framework Articulation:

1. Law of conservation of energy, work, and

internal energy5.B.1, 5.E.2:a

2. Endothermic and exothermic reactions 3.C.2, 5.B.3:e, 5.B.3:f

3. Potential energy diagrams 3.C.2, 5.C.2:c, 5.C.2:d, 5.C.2:e

4. Calorimetry, heat capacity, and specific heat 5.A.2, 5.B.2, 5.B.3:a, 5.B.3:b, 5.B.4

5. Hess’s law 5.B.3:a

6. Heat of formation/combustion 5.C.2:g

7. Bond energies 2.C.1:d, 5.C.1, 5.C.2:a, 5.C.2:b

8. Laws of thermodynamics

9. Spontaneous process and entropy 5.E.1

10. Spontaneity, enthalpy, and free energy 5.E.2:c, 5.E.3,

11. Free energy 5.E.2:d, 5.E.2:e, 5.E.2:f, 6.C.3:c,6.D.1:a

12. Free energy and equilibrium 5.E.2, 6.D.1:b, 6.D.1:c, 6.D.1:d

13. Rate and Spontaneity 5.E.2:e, 5.E.5

Student Activity: Given a set of conditions, the students determine if the situation is thermodynamically favored or not favored by looking at entropy, enthalpy, and Gibb’s Free Energy. LO 5.13 [CR3e}

Chapter 20Electrochemistry

Class Periods (90 minutes):6 periods

Homework sets assigned:Read the chapter and HW (3 sets),

Number of Exams1 exam and 2 quiz

Topics Covered: Curriculum Framework Articulation:

1. Balancing redox equations 3.B.3:a, 3.B.3:b, 3.B.3:c, 3.B.3:d

2. Electrochemical cells and voltage 3.C.3:a, 3.C.3:b, 3.C.3:c, 5.E.4:a

3. The Nernst equation 3.C.3:d

4. Spontaneous and non-spontaneous

Equations3.C.3:e

5. Chemical applications3.C.3:f

Laboratories: [CR5a]

Inquiry Skills Labs [CR6]

1. Spectrophotometry: How Can Color Be Used

to Determine the Mass Percent of Copper in Brass?LO 1.5, 1.6, 1.7, 1.8, 1.14, 1.15; SP 1, 6

2. Gravimetric Analysis: What Makes Hard Water Hard?LO 1.19, 2.10, 3.2, 3.3; SP 4,5,6,7

3. Titration:

How Much Acid Is in Fruit Juice and Soft Drinks?LO 1.20, 3.3; SP 2, 4, 5, 6

4. Bonding in Solids: What’s in That Bottle?LO 2.22, 2.24, 2.28, 2.32; SP 1, 4, 6, 7

5. Kinetics: Rate of Reaction: How Long Will

That Marble Statue Last?LO 4.1, 4.2; SP 4, 5, 6

6. Buffer Design: The Preparation and Testing of an

Effective Buffer: How Do Components Influence a

Buffer’s pH and Capacity?LO 1.4, 6.18; SP 2,4,6,7

Labs completed in traditional format: [CR5b]

7. Math and Measurements in ScienceLO 1.3, SP2, 5

8. Spectroscopy: What Is the Relationship between the

Concentration of a Solution and the Amount of

Transmitted Light through the Solution?LO 1.5, 1.6, 1.7, 1.8, 1.14, 1.15; SP 1, 6

9. Chromatography: Sticky Question: How Do You

Separate Molecules That Are Attracted to

One Another?LO 2.10, 2.13; SP 1,4,5,6

10. Redox Titration: How Can We Determine the Actual

Percentage of H2O2 in a Drugstore Bottle of

Hydrogen Peroxide?LO 1.20, 3.3, 3.9; SP 2,4,5,6

11. Kinetics: Rate Laws: What Is the Rate Law of the

Fading of Crystal Violet .Using Beer’s Law?LO 4.1, 4.2; SP 4, 5, 6

12. Acid-Base Titration: How Do the Structure and the

Initial Concentrationof an Acid and a Base Influence

the pH of the Resultant Solution during aTitration?LO 1.18, 1.20, 6.11,6.12; SP 1, 5, 6

13. Buffering Activity: To What Extent Do Common

Household Products HaveBuffering Activity?LO 1.20, 6.20; SP 4, 5, 6

14.The Determination of the X moles of water ratio in

aHydrate.LO 3.5; SP 1,2,5,6

15.Determining the Enthalpy of a Chemical Reaction.LO 1.20, 6.20; SP 4, 5

16.Electrochemical CellsLO 3.12, 3.13 SP 2,5,6

17.Determining the Ksp of Calcium HydroxideLO6.21, 6.22, 6.23; SP 1,6

18.Freezing Point Depression LO 2.8; SP 1,6

19.Evaporation and Intermolecular ForcesLO 2.11, 2.13; SP 6, 7

20.Molecular Model Lab-LO 2.21; SP 1,3

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