AP Chemistry Summer Work

Read through the syllabus so that you know what is expected of you over the course of this upcoming year.

DO NOT BE OVERWHELMED. THE COURSE LOAD IS MANAGABLE!

Read the photocopied chapter of our text and answer the circled questions. Remember to use dimensional analysis, show all of your work (with UNITS), and keep track of significant figures. This homework is due on or before August 17th, so I can correct it by the first day of school. Please put it in my mailbox, as I will be picking it up in the afternoon on the 17h.

Also you will need to buy a marbled notebook to use as your lab notebook. Leave the first page blank for a table of contents.

Finally, STUDY YOUR IONS and COMPOUNDS. I attached a list of ions and compounds I expect you to know by the first day of school. You should already know most of these, but the last few on the list may be new to you. Be ready for a test sometime early in the first week of school.

If you have any questions feel free to contact me via email. My address is: nicholas_guerin@wrsd.net. Have a great summer and I am looking forward to the fall.

-Guerin

AP® Chemistry

Wachusett Regional High School Nicholas A. Guerin

Course Description AP® Chemistry is designed to be the equivalent of a first year college general chemistry course and

follows the College Board’s AP® Chemistry syllabus. As such, the course is suitable for the best and brightest

at the regional that have excelled in their first year chemistry course. Students wishing to take AP® Chemistry

must exhibit high levels of commitment, motivation, and academic maturity. This course presents a rigorous

treatment of the following concepts: the nature of matter, gas laws, thermodynamics, stoichiometry, bonding,

chemical kinetics, chemical equilibria, and more. Successful completion of this course requires strong math

skills, and students will also develop the ability to tie multiple concepts into one complex calculation. These

problem-solving strategies obtained during this course will prepare college-bound students for careers in the

sciences, medicine, engineering, and other technical areas.

This course will nurture the student's ability to incorporate mathematical skills in the solution of

chemistry problems, both through the use of textbook problems and laboratory activities. Since the AP® exam

no longer allows the use of calculators during specific sections, significant emphasis will be placed on

developing the student's ability to solve problems through dimensional analysis and estimation. Students will

be required to do extensive writing, and to keep a thorough and accurate laboratory notebook.

To cover all of the material in the appropriate depth, AP® Chemistry will meet as a class and a half in

the 14-day rotating schedule. This means the class meets for a total of 11 hours every 14 school days, instead

of the usual 7 hours of class time for a regular class. Labs will be accommodated during the double periods or

the period + 90-minute long-block combination, which occur at least once every school week.

AP® Chemistry requires extensive laboratory work to reinforce and demonstrate key course concepts

and ready the student for college chemistry. Each student is required to keep a detailed lab notebook. This

notebook will be used to record every procedure, observation, and calculation. Each lab will also require a

written lab report, where the student will explain and outline each facet of the experiment conducted.

The students’ grade will be calculated by taking a percentage of points you have compared to how

many you could have. It is imperative that each student behaves properly, respect each other, respect the

instructor, and respect the room in which the class is taught. Inappropriate behavior will not be tolerated in

any form, especially in the laboratory. Lab safety is of the utmost importance. Any misconduct during a

laboratory will result in a zero for that lab assignment.

Required Materials All students are expected to bring a writing implement, scientific calculator (graphing calculators

are prohibited), and a three ring binder to each class. A three ring binder to accommodate class notes,

homework, handouts, quizzes, tests, and other class work is required. Students also need a composition

notebook to outline each laboratory procedure. Students will not be supplied any of these items if they are

forgotten. Promptness is also desired. After a student’s first late arrival I will deduct one point from your

point totals, which can have a dramatic impact on your grade.

Text

Chemistry by Zumdahl and Zumdahl, 7th ed., Houghton Mifflin Company, 2007.

Lab Resources

Laboratory Experiments for Advanced Placement Chemistry by Vonderbrink, Flinn Scientific, Inc., 1995.

Laboratory Investigations: AP® Chemistry by David Hostage and Martin Fosset, People’s Education, 2006.

Additional lab assignments that have been recommended and obtained from the following AP workshops will

also be used.

AP® Institute at St. Johnsbury, St. Johnsbury, VT.

Taft AP® Institute at the Taft School, Waterbury, CT.

Laboratory assignments will be taken from these sources and will be given to students as handouts.

Course Overview (Note: that labs may be done out of sequence and dates may change based on progress)

Chapter 1: Chemical Foundation Summer Work (Due August 17th)

Topics Covered: Scientific Method, Units of Measurement, Significant Figures, Dimensional Analysis,

Temperature, Density, Classification of Matter

Lab Experiment: % T Gatorade Lab

Chapter 2: Atoms, Molecules, and Ions Aug 28th-Sept. 7th (1.5 Weeks)

Topics Covered: Fundamental Chemical Laws, Dalton’s Atomic Theory, Atomic Structure and Classic

Experiments, Modern Atomic Theory, Molecules, Ions, Periodic Table, Naming Simple Compounds

Lab Experiment: % Cu in Brass Lab

Chapter 3: Stoichiometry Sept. 10th-14th (1 Week)

Topics Covered: Atomic Masses, Mole Concept, Percent Composition, Formula Determination, Balancing

Chemical Equations, Stoichiometric Calculations, Limiting Reactant

Lab Experiments: The Size of a Molecule (Calculating Avogadro’s Number)

Gravimetric Analysis of Epsom Salt

Job’s Method of Continuous Variation

Chapter 4: Types of Reactions and Solution Stoichiometry Sept. 17th-Oct. 4th (3 Weeks)

Topics Covered: Water, Nature of Aqueous Solutions, Electrolytes, Composition of Solutions, Types of

Reactions, Precipitation Reactions, Ionic Equations, Precipitation Stoichiometry, Acid-Base Reactions,

Balancing Redox Reactions

Lab Experiments: Qualitative Analysis (Identification Through Precipitation Reactions)

Acid-Base Titration (Volumetric Analysis)

Redox Titration

(Course Overview con’t)

Chapter 6: Thermochemistry Oct. 5th-23rd (2.5 Weeks)

(Note: Chapter 5: Gases has been skipped to cover at a later date. This is done to get to the harder material

(Equilibrium, Rate Laws) faster and to spend more time with them.)

Topics Covered: Nature of Energy, Enthalpy and Calorimetry, Hess’s Law, Enthalpies of Formation, Present

and New Sources of Energy

Lab Experiments: Calorimetry of Endothermic and Exothermic Reactions

Thermochemistry and Hess’s Law

Chapter 7: Atomic Structure and Periodicity Oct. 24th-Nov. 5th (2 Weeks)

Topics Covered: Electromagnetic Radiation, Bohr Model, Bright Line Spectra, Quantum Model of the Atom,

History of the Periodic Table, Periodic Trends in Atomic Properties, Group Properties

Lab Experiments: Atomic Spectroscopy and Bohr’s Model

Flame Tests Revisited

Chapters 8 & 9: Bonding: General Concepts Nov. 7th- Nov. 16th (1.5 Weeks)

Covalent Bonding: Orbitals

Topics Covered: Types of Bonds, Electronegativity, Bond Polarity, Ionic Compounds, Bond Character,

Covalent Bonds, Bond Energies and Reactions, Lewis Structures, Octet Rule and Exceptions, Resonance,

VSEPR, Hybridization, σ- and π-bonds

Chapters 10 & 11: Liquids and Solids Nov. 19th– Dec. 6th (2.5 Weeks)

Properties of Solutions

Topics Covered: Intermolecular Forces, The Liquid State, Types of Solids, Metallic Bonding, Molecular

Solids, Ionic Solids, Vapor Pressure and Changes of State, Phase Diagrams, Solution Composition, Energies

of Solution Formation, Solubility, Vapor Pressure, Colligative Properties, Boiling Point Elevation, Freezing

Point Depression, Osmotic Pressure, Colloids

Lab Experiment: Molar Mass by Freezing Point Depression

Chapter 12: Chemical Kinetics Dec. 7th - Dec. 20th (2 Weeks)

Topics Covered: Reaction Rates, Rate Laws, Determining the Form of a Rate Law, Integrated Rate Law,

Reaction Mechanisms, Collision Theory, Catalysis

Lab Experiments: Rate Law Determination of the Crystal Violet Reaction

Differential and Integrated Rate Laws

Chapter 13: Chemical Equilibrium Dec 21th-Jan. 10th (2 Weeks)

Topics Covered: Equilibrium Condition, Equilibrium Constant, Pressure and Equilibrium, Heterogeneous

Systems, Applications of K, Equilibrium Calculations, Le Châtlier’s Principle

Lab Experiment: Determination of Equilibrium Constant for the Formation of FeSCN2+

(Course Overview con’t)

Chapter 14: Acids and Bases Jan. 11th-Jan. 25th (2 Weeks)

Topics Covered: Nature of Acids and Bases, Acid Strength, pH Scale, pH Calculations for Strong and Weak

Acids, Bases, Polyprotic Acids, Acid-Base Properties of Salts and Oxides, Lewis Acids and Bases

Lab Experiments: Finding Mass Percent of Acetic Acid in Vinegar

Determination of Acid Ionization Constant of a Weak Acid

Chapter 15: Application of Aqueous Equilibria Jan 28th-Feb 15th (3 Weeks)

Topics Covered: Acid Base Equilibria, Common Ion Effect, Buffered Solution, Titrations, pH Curves,

Indicators, Solubility Equilibria, Solubility Product Constant, Precipitation Reactions, Complex Ion Equilibria

Lab Experiments: Titration Curve Lab

Determination of the Equilibrium Constant of an Indicator

Determination of the Solubility Product Constant of Calcium Hydroxide

Chapter 18: The Nucleus: A Chemists View February Break

Topics Covered: Nuclear Stability and Radioactive Decay, Nuclear Transformations, Detection and Uses of

Radioactivity, Stability of the Nucleus, Nuclear Fission and Fusion, Effects of Radiation

Chapter 16: Spontaneity, Entropy, and Free Energy Feb 25th-Mar. 6th (1.5 Weeks)

Topics Covered: Spontaneity of Processes, Entropy, Second Law of Thermodynamics, Free Energy, Entropy

Changes, Free Energy in Chemical Reactions, ∆G and Pressure, ∆G and Equilibrium, ∆G and Work

Chapter 17: Electrochemistry Mar. 8th-Mar. 20th (1.5 Weeks)

Topics Covered: Galvanic Cells, Standard Reduction Potentials, Cell Potential, Electrical Work, and Free

Energy, Dependence of Cell Potential on Concentration, Batteries, Corrosion, Electrolysis

Lab Experiment: Electrochemical Cells

Chapter 22: Organic Chemistry Mar. 21st –Mar. 27th (1 Week)

Topics Covered: Alkanes, Alkenes, Alkynes, Nomenclature of Organic Compounds, Reactions of Organic

Compounds, Functional Groups

Lab Experiments: Modeling Lab

Electrolytic Synthesis of Iodoform

Chapter 5: Gases March 28th- Apr. 9th (1.5 - 2 Weeks)

Topics Covered: Pressure, Boyle’s Law, Charles’ Law, Avogadro’s Principle, Ideal Gas Law, Gas

Stoichiometry, Dalton’s Law, Kinetic Molecular Theory, Effusion and Diffusion, Real Gases

Lab Experiments: Molar Mass of a Volatile Liquid

Molar Volume of Gas

(Course Overview con’t)

AP® Exam Review and Preparation Apr. 10th - Early May (2 Weeks)

During this time we will review material, discuss the examination, test taking strategies, and how multiple

concepts that we have discussed will be bridged together. This will be accomplished by review lab reports,

past exam questions from the multiple-choice sections and open-response, and practice tests will be

administered. Emphasis will be placed on ionic equations, equilibrium problems, predicting redox reactions,

and solubility rules.

AP Chemistry Exam May 6th

TBD

After the Exam

Decompression, Airbag Lab, Unknowns Lab, Acid ID Lab, Analysis of Antacid Lab

Senior Exams Last Week in May

Congraduations

1

Name_____________________

Ions and Formulas For AP Chemistry

1. Chromic

2. Flouride

3. Sodium

4. Mercury (II)

5. Calcium

6. Chloride

7. Ammonia

8. Iodide

9. Sulfide

10. Hydrogen Sulfate

11. Bisulfate

12. Chlorate

13. Copper (II)

14. Hydrogen

15. Peroxide

16. Hydroxide

17. Hydrogen Carbonate

18. Bicarbonate

19. Ferrous

20. Oxygen

21. Tin (IV)

22. Perchlorate

23. Beryllium

24. Zinc

25. Copper (I)

26. Iron (II)

27. Plumbous

28. Stannic

29. Sodium Chloride

30. Nickel (I)

31. Nickel (II)

32. Chromous

33. Phosphate

34. Mercuric

35. Sodium Hydroxide

36. Neon

37. Water

38. Chromium (III)

39. Barium

40. Nitric Acid

41. Chlorite

42. Carbon Monoxide

43. Magnesium

44. Chromate

45. Dichromate

46. Aluminum

47. Iron (III)

48. Hydrogen ion

49. Methane

50. Cuprous

51. Ammonium

52. Stannous

53. Nitrite

54. Hydronium

55. Nitrogen

56. Bromine

57. Nickelous

58. Mercurous

59. Plumbic

60. Acetate

61. Bromide

62. Diarsenic pentoxide

63. Oxide

64. Helium

65. Glucose

66. Cupric

67. Nitrate

68. Silver

69. Sulfite

70. Carbon Dioxide

71. Ferric

72. Carbonate

73. Potassium

74. Carbon tetrachloride

75. Mercury (I)

76. Hypochlorite

77. Lead (IV)

78. Sulfate

79. Permanganate

80. Nickelic

81. Lead (II)

82. Proton

83. Sucrose

84. Chromium (II)

85. Sulfuric Acid

86. Hydorchloric Acid

87. Flourine

88. Chlorine

89. Iodine

90. Lithium

91. Bromate

92. Cobalt (II)

93. Nitride

94. Manganese (II)

95. Tin (II)

96. Cyanate

97. Thiocyanate

98. Thiosulfate

99. Oxalate

100. Cyanide