It is recommended that every student obtain the following items for use during the school year in AP Chemistry:

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1 Welcome to AP Chemistry! I am very excited that you have decided to take AP Chemistry next year. I promise that you will have fun learning Chemistry, and that you will also be challenged academically. AP Chemistry is a rigorous course that is designed to be just like a General Chemistry course that is offered to science majors at a college or university. Here is your summer assignment: 1. Memorize the names and symbols for elements 138, 42, 4756, 74, 7888, and 92. I know that you learned them during your first year Chemistry course, but I want to make sure that you will still remember them. Please make a set of flash cards with the element symbol on one side and the name of the element on the other side. This set of flash cards will be turned in on the first day of school. 2. Memorize the common ions. They can be found on the common ion chart. During your first year Chemistry course, you got to use the common ion chart on all of your tests and now during AP Chemistry you will have to memorize them because you will not be allowed to use the common ion chart on your exams (or the AP Exam). Please make a set of flash cards with the formula for the common ion on one side and the name of the common ion on the other side. This set of flash cards will be turned in on the first day of school. AP Chemistry is a difficult course. It is not all about memorization; however, having these items memorized (along with many others) is essential for success in learning the concepts covered in the course. Make flashcards, have your friends and family quiz you, take the flash cards with you on vacation, or do whatever it takes to get this information firmly planted in your head. Do not wait until the night before school begins. 3. Finally, the last part of your assignment will be to complete a review sheet. This sheet will cover some of the major concepts from your first year Chemistry course that are the foundation for AP Chemistry. You must show all of your work on the problems that require calculations. Most of these topics are covered in Chapters 13 of your AP Chemistry textbook, Chemistry 7 th Edition by Zumdahl & Zumdahl. There will be a test on this material on the first day of class. This test will show how much information you have retained from your first year Chemistry class and will also be used as a guide for your performance in AP Chemistry. Please take this summer assignment seriously. I do not believe in busy work. It is recommended that every student obtain the following items for use during the school year in AP Chemistry: a databook: quadruled composition book two notebooks: 3subject, college ruled, spiral notebooks graphing calculator: TI83 or TI84 is recommended Please feel free to me at any time during the summer while you are working on your summer work assignment at dawn_toth@redlands.k12.ca.us with any questions or concerns you might have even if they are little ones!! I look forward to meeting you all next year! Enjoy the summer! Mrs. Toth

2 AP Chemistry Summer Work Review Sheet Everything I should know or need to know from Chemistry 1. How many significant figures are in the following? a) g f) km b) L g) o C c) cm h) m d) L i) 5 x 10 5 mm e) 7.4 x 10 3 m j) ml 2. Complete the following calculations. Make sure your answer has the correct number of significant figures. a) cm cm f) 6.13x10 7 cm x 1.1x10 2 cm b) g 2.1 g g) 2500 g g g c) 45.0 cm x 3 cm h) (6.8173x10 6 cm 3 ) ⅓ d) g x 4.2x10 3 cm i) (2.61 cm) 3 e) 6.2 cm x 18.0 cm x 3.1 cm / 4210 g 3. Complete the following unit conversions using dimensional analysis: a) 291 km mm j) A car uses gasoline at a rate of 22 b) 3120 J cal miles per gallon. What is its rate c) o C K in kilometers per liter? (1 gal = d) 14 K o C L) & (1 mi = 5280 ft) e) 1.5 m cm k) The length of a wave of green f) 2.61 m 2 cm 2 light is 580 nanometers (1 nm = g) m 3 cm m). How many waves of h) g/cm 3 cg/m 3 green light could fit through a slit i) convert your age to milliseconds that is 2.0 centimeters wide? 4. Complete the following density calculations: a) A metal bar has a mass of 348 g and a volume of 54 cm 3. What is the density of the metal bar? b) Aluminum has a density of g/cm 3. What volume of aluminum has a mass of 60. g? c) A large block of an unidentified substance measures 7.2 feet by 9.2 feet by 2.5 feet. Its mass is 5230 kg. What is the density of the block in terms of g/cm 3? (1 inch = 2.54 cm) 5. Complete the following chart by using the information given to determine the number of protons, neutrons, and electrons in a species: Symbol Charge Atomic # Mass # Protons Neutrons Electrons In neutral 17 18

3 6. Write the atomic symbol for each of the following isotopes described below (put the atomic # on the bottom left and the mass # in the top left): a) p = 106, n = 157, e = 106 b) p = 56, n = 61, e = 54 c) p = 16, n = 16, e = Name the following compounds: a) HCl e) BaBr 2 b) H 2 SO 4 f) Hg 2 CO 3 c) NaNO 3 g) PbCl 4 d) H 2 S h) CBr 4 i) Mn(OH) 2 j) KrF 4 k) MgO l) PtSO 4 m) Hg 2 Cl 2 n) BaCr 2 O 7 o) XeF 6 p) UF 6 8. Write formulas for the following compounds: a) ammonium sulfate b) acetic acid c) copper(i) bromide d) silicon tetrafluoride e) trinitrogen octaoxide f) sulfuric acid g) manganese(iv) oxide h) disulfur trioxide i) lithium cyanide j) chromium(iii) phosphate 9. Write reactions from the situations given: a) When sodium metal is placed in water, it makes hydrogen gas and a solution of sodium hydroxide. b) The combustion of ethyl alcohol, C 2 H 5 OH, in oxygen gas is catalyzed by platinum. It results in the typical combustion products of carbon dioxide and water both in the gaseous state. c) Solution of barium nitrate and sodium hydroxide produce a precipitate of barium hydroxide while the sodium nitrate remains in solution. d) When calcium carbonate is heated strongly, it breaks down into calcium oxide lime and carbon dioxide gas. e) Copper as a wire can replace silver in silver nitrate solution. The solution would then end up being copper (II) nitrate. 10. Balance the following reactions: a) Mg + Ca(NO 3 ) 2 Ca + Mg(NO 3 ) 2 b) Pb(C 2 H 3 O 2 ) 4 + NaOH Pb(OH) 4 + NaC 2 H 3 O 2 c) C 7 H 16 OH + O 2 H 2 O + CO 2 d) Al + O 2 Al 2 O 3 e) NaCl + H 2 O NaOH + H 2 + Cl 2 f) NCl 3 + H 2 O NH 3 + HOCl g) CH 3 NH 2 + O 2 CO 2 + H 2 O + N Calculate the molar mass for the following: a) C 2 H 5 OH b) Ba(NO 3 ) 2 c) Pt d) TiO 2

4 12. Complete the following mole house conversions: a) 76.5 g SO 3 = moles b) 1.62 mol CaCO 3 = grams c) 2.67x10 22 atoms Mg = mol d) 83.5 L CO 2 = mol e) 1.5 g CH 4 = molecules f) 100. L CH 4 = molecules g) 2.83x10 24 atoms gold = grams 13. Calculate the amount of product or reactant made or used up from an amount given: a) In reaction 10c, 35.6 grams of heptanol is combusted. How many grams of water should be produced from complete combustion? b) In the process written in 10e, how many grams of salt are necessary to produce g of chlorine gas? c) How much pure silver can be made from a 1.4 gram wire of copper from the reaction in 9e? Use the concepts of limiting reactants to calculate the theoretical yields in problem 14 & grams of each of the reactants in problem 10a are allowed to react fully. a) Which reactant is the limiting reactant? b) What will be the theoretical yield of calcium metal? 15. A strip of zinc metal weighing 2.00 grams is placed into an aqueous solution containing 2.50 grams of silver nitrate. a) Which reactant is the limiting reactant? b) How many grams of silver are produced? c) How many grams of zinc nitrate will form?

5 COMMON ION CHART Positive Ions (Cations) Aluminum Al 3+ Ammonium + NH 4 Barium Ba 2+ Cadmium Cd 2+ Calcium Ca 2+ Chromium (II), chromous Cr 2+ Chromium (III), chromic Cr 3+ Cobalt (II), cobaltous Co 2+ Copper (I), cuprous Cu + Copper (II), cupric Cu 2+ Gold (III) Au 3+ Hydrogen, hydronium H +, H Iron (II), ferrous Fe 2+ Iron (III), ferric Fe 3+ Lead (II) Pb 2+ Lead (IV) Pb 4+ Lithium Li + Magnesium Mg 2+ Manganese (II), manganous Mn 2+ Mercury (I), mercurous 2+ Hg 2 Mercury (II), mercuric Hg 2+ Nickel (II) Ni 2+ Nickel (III) Ni 3+ Potassium K + Silver Ag + Strontium Sr 2+ Sodium Na + Tin (II), stannous Sn 2+ Tin (IV), stannic Sn 4+ Zinc Zn 2+ Negative Ions (Anions) Acetate CH 3 COO ; C 2 H 3 O 2 Bromide Br Bromate BrO 3 Carbonate 2 CO 3 Hydrogen carbonate, bicarbonate HCO 3 Chlorate ClO 3 Chloride Cl Chlorite ClO 2 Chromate 2 CrO 4 Dichromate 2 Cr 2 O 7 Cyanide CN Fluoride F Hydride H Hydroxide OH Hypochlorite ClO Iodide I Iodate IO 3 Nitrate NO 3 Nitride N 3 Nitrite NO 2 Oxalate 2 C 2 O 4 Hydrogen oxalate, binoxalate HC 2 O 4 Oxide O 2 Perchlorate ClO 4 Permanganate MnO 4 Phosphate 3 PO 4 2 Monohydrogen phosphate HPO 4 Dihydrogen phosphate H 2 PO 4 Phosphite 3 PO 3 Silicate 2 SiO 3 Sulfate 2 SO 4 Hydrogen sulfate, bisulfate HSO 4 Sulfite 2 SO 3 Hydrogen sulfite, bisulfite HSO 3 Thiosulfate 2 S 2 O 3 Sulfide S 2 Hydrogen sulfide, Bisulfide HS Tartrate 2 C 4 H 4 O 6 Thiocyanate SCN