AP Chemistry Summer Assignment s1

AP Chemistry Summer Assignment May 2012

Future AP Chemistry Student,

Welcome to AP Chemistry! I am eagerly anticipating a great year of Chemistry. In order to ensure the best start for everyone next fall, I have prepared a Summer Assignment that reviews basic chemistry concepts. Most of the material covered in the summer packet will be familiar to you, but is designed to strengthen your foundation in chemistry and ensure that all students are on a relatively even plane. It will be important for everyone to come prepared to class on the first day. While we will review, extensive remediation is not an option as we work towards the goal of being prepared for the AP Exam in early May. The Summer Assignment is DUE THE FIRST DAY OF SCHOOL! There will be a quiz covering the basic concepts included in the summer packet during the first week of school.

I hope you are gearing up for an exciting, challenging and rewarding academic course. The grades you earn on tests in AP Chemistry will probably be lower than those you’ve earned in Honors Chem. That is the nature of a difficult AP course, and this is one of the “tough” AP courses. But, I know you will learn a lot in AP Chemistry, and it will be an excellent way for you to prepare for college. It will build your knowledge base, enhance your work habits and your organizational skills, and you will grow as an independent learner. You are all certainly fine students, and with motivation and hard work, you should find AP Chemistry a successful and rewarding experience.

Finally, I recommend that you find a “study buddy” and spread out the summer assignment. Please do not try to complete it all in one day. Chemistry takes time to process and grasp at a level necessary for success in AP Chemistry. Remember, AP Chemistry is equivalent to a first- year chemistry college course, and should be considered as such. College Board recommends that students taking AP Chemistry put in a minimum of 5 hours of study per week outside the classroom. Taking a college level course in high school is difficult, requires dedication, and is a great investment in your education, so prepare yourself and arrive ready to learn.

Have a great summer and enjoy the chemistry.

Mrs. Heitmann Perry High School Chemistry

Textbook and Materials for first day of class:  (Zumdahl & Zumdahl) Chemistry, 7th Edition. Houghton Mifflin Company. ISBN 978-0-618-71370-7 (to be checked out from me in Rm F203 BEFORE summer break)  Completed Summer Assignment  Scientific Calculator  3-Ring Binder  Graph Paper Composition Book – (Bound Lab Book)

1 PART ONE Make flashcards and memorize the names, symbols and charges of the common ions listed below.

Names, Formulas, and Charges of Some Common Polyatomic Ions + 2- - NH4 Ammonium SO4 Sulfate FO Hypofluorite - - - C2H3O2 Acetate HSO4 Hydrogen sulfate ClO Hypochlorite 2- 2- - CO3 Carbonate SO3 Sulfite ClO2 Chlorite - - - HCO3 Hydrogen carbonate HSO3 Hydrogen sulfite ClO3 Chlorate 2- 2- - C2O4 Oxalate S2O3 Thiosulfate ClO4 Perchlorate CN- Cyanide HS- Hydrogen sulfide BrO- Hypobromite - - - OCN Cyanate OH Hydroxide BrO3 Bromate - 2- - SCN Thiocyanate O2 Peroxide BrO4 Perbromate - 2- - NO2 Nitrite CrO4 Chromate IO Hypoiodite - 2- - NO3 Nitrate Cr2O7 Dichromate IO3 Iodate 3- - - PO4 Phosphate MnO4 Permanganate IO4 Periodate 2- 2- HPO4 Hydrogen phosphate MnO4 Manganate - H2PO4 Dihydrogen phosphate

Names, Formulas, and Charges of Some Common Ions Al3+ Aluminum Au3+ Gold (III) or auric Fe3+ Iron (III) or ferric H- Hydride Sn2+ Tin (II) or stannous Co2+ Cobalt (II) or cobaltous Mn2+ Manganese (II) Sn4+ Tin (IV) or stannic Co3+ Cobalt (III) or cobaltic Ni2+ Nickel (II) Pb2+ Lead (II) or plumbous Cu+ Copper (I) or cuprous Zn2+ Zinc Pb4+ Lead (IV) or plumbic Cu2+ Copper (II) or cupric 2+ 2+ 2+ Cd Cadmium Cr Chromium (II) or chromous Hg2 Mercury (I) or mercurous Ag+ Silver Cr3+ Chromium (III) or chromic Hg2+ Mercury (II) or mercuric Au+ Gold (I) or aurous Fe2+ Iron (II) or ferrous

PART TWO More Memorization.

1. Know solubility rules for common ions. (See pg. 144, Table 4.1)

2. Know rules for assigning oxidation numbers. (See pg. 156, Table 4.2)

2 PART THREE Start learning the following special case examples of reaction types.

Synthesis:

Metal oxide + water à metal hydroxide MgO + H2O à Mg(OH)2

Nonmetal oxide + water à acid (polyatomic) CO2 + H2O à H2CO3

Decomposition:

Metal carbonate à metal oxide + carbon dioxide Cs2CO3 à Cs2O + CO2

Metal hydroxide à metal oxide + water 2 LiOH à Li2O + H2O

Metal chlorate à metal chloride + oxygen gas 2 LiClO3 à 2 LiCl + 3 O2

Acid/Base Reactions

acid + base  salt + water H2SO4 + NaOH  Na2SO4 + H2O

metal + acid  salt + hydrogen gas 3Mg + 2H3PO4  Mg3(PO4)2 + 3H2

metal oxide + acid  salt + water CaO + HCl  CaCl2 + H2O

carbonate + acid  salt + carbon dioxide + water BaCO3 + H2SO4  BaSO4 + CO2 + H2O (The carbonate ion breaks apart. The other negative ion becomes part of the salt)

nonmetal oxide + hydroxide  salt + water CO2 + Ba(OH)2  BaCO3 + H2O

metal oxide + nonmetal oxide  salt Na2O + SO3  Na2SO4 PART FOUR Read/review textbook chapters 1 through 4.

PART FIVE Complete the following End of Chapter (EOC) problems on a separate sheet of loose-leaf paper. When applicable, show your work, label, and pay attention to significant digits.

Chapter 1: EOC Problems (pgs. 33-35) 27, 31, 49, 59, 67, 69, 71, 73, 79.

Chapter 2: EOC Problems (pgs. 70-73) 9, 19, 49, 51, 65, 67, 77.

Chapter 3: EOC Problems (pgs. 117-121) 27, 33, 61, 73, 83, 95.

Chapter 4: EOC Problems (pgs. 170-174) 9, 27, 35, 37, 43, 69, 71. 3