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AP Chemistry Summer 2009-2010 Assignment Posted June 2009 Thinking about next year already? Yes, we are! Because this is a test-driven course, and because this test is administered in early May, you need to come already warmed up and ready to go on day one in August! This summer assignment serves as a review of a select few basic skills as well as a list of some items that you need to have ready at your fingertips. (Note: former students have indicated this served as a tremendous help!) Download this assignment so that you may click on the hyperlinks provided. Follow the website links and instructions below. You will get immediate feedback on some of your answers as you progress. Setups, labels, sig figs, canceling all count! Have this ready for submission on your first day back to school. Your first test will be the second day of school and will cover the information included in this assignment. If you need a refresher you should consult last year’s notes and/or check the website links. If a problem arises this summer with one of the websites, I have included many different websites as alternative references. Please send me a confirmation email ASAP to [email protected] indicating that (1) you have received this assignment, and (2) you can access these websites. If you have any questions, please email me before August 12. Enjoy your summer! I look forward to seeing you all again this fall! Mrs. Zebris Rocky River High School/AP Chemistry Instructor Name_______________________________________ 1. Indicate the number of protons, neutrons, and electrons for each symbol. 1) 40 20 Ca 5) Carbon-14 12 6 C 2) 127 3) 6) Uranium-235 7) Uranium-238 53 I 4) 36 17 Cl 8) Xenon-131 2. Memorize these polyatomic ions. Make flashcards if necessary! Go to http://wps.prenhall.com/wps/media/objects/4974/5093961/emedia/ch03/PolyatomicIons.html and practice. Ammonium NH4+ Acetate C2H3O2Nitrate NO3Nitrite NO2Hydroxide OH Hypochlorite ClO Chlorite ClO2- Carbonate Peroxide Sulfate Sulfite Thiosulfate Chromate Dichromate CO3 2O2 2SO4 2SO3 2S2O3 2CrO4 2Cr2O7 2- Chlorate ClO3 Perchlorate ClO4 Permanganate MnO4Bicarbonate HCO3 Cyanate CNThiocyanate SCN 2+ Cobalt Co Co3+ Phosphate PO4 3Arsenate AsO4 3Borate BO3 3iron Fe2+ Fe3+ copper Cu+ Cu2+ tin Sn2+ Sn4+ lead Pb2+ Pb4+ 3. Inorganic Nomenclature Review (Ionic and Covalent compounds) Write the formulas/names for the following ionic compounds. Then go to http://wps.prenhall.com/wps/media/objects/4974/5093961/emedia/ch03/IonicCompounds.html to check your answers 1|Page Barium hydroxide _____________ NH4OH __________________________ Calcium sulfide _____________ NaOH __________________________ Silver chloride _____________ AgNO3 __________________________ Iron (II) nitrate _____________ FeS __________________________ Lead (II) sulfate _____________ LiClO3 __________________________ Aluminum hydroxide _____________ FeCl3 __________________________ Ammonium phosphate _____________ Na2S __________________________ Sodium perchlorate _____________ Na2SO4 __________________________ Calcium carbonate _____________ Pb(NO3)2 __________________________ Sodium carbonate _____________ LiOH __________________________ Go to http://wps.prenhall.com/wps/media/objects/4974/5093961/emedia/ch03/AAEDKKE0.html and write the name and formulas for 10 items. 1.__________________________________________ 6. .__________________________________________ 2. .__________________________________________ 7. .__________________________________________ 3. .__________________________________________ 8. .__________________________________________ 4. _________________________________________ 9..__________________________________________ 5.__________________________________________ 10. _________________________________________ 4. Mole/Mass/Particles Conversions Show your factor-labeling work formally for the following. Round all molar masses from the periodic table to the hundredths place. Be sure to watch your units and sig figs! 2.4 mol H2O = ____ particles of H2O 5.9 x 1020 atoms of O2 = ____ mol 9.98 x 10-3 mol carbon monoxide = ____ grams 0.25 mol silver acetate = _______ particles 2.35 mol disulfur trinitride = ______ grams 3.80 Kg of copper (II) phosphate =______ particles 2|Page 1.378 x 10-3 grams Ar gas = ______ Liters 5.989 x 1030 molecules sulfuric acid = ________ grams 2.1 x 103 liters oxygen = ____ particles 50.0 g sodium hydrogen carbonate = ____ mol 5. Percent Composition Show your work formally for the formulas below. Go to http://wps.prenhall.com/wps/media/objects/4974/5093961/emedia/ch03/MWweightPercent/j2bl/MWweightPercent.html to review and to check your answers. Other sites for more review include http://www.shodor.org/UNChem/basic/stoic/ . NH3 CH4 Pb(NO3)2 6. Empirical & Molecular Formulas For review go to http://wps.prenhall.com/wps/media/objects/4974/5093961/emedia/ch03/EmpFormulaDetermin.html . Also check out the hint cards. Then show your work to calculate the formulas. A. A 100. gram sample of compound of sodium contains 36.5 grams of sodium, 25.4 grams of sulfur, and 38.1 grams of oxygen. What is the empirical formula for the compound? B. Fat makes up a major portion of all soaps. A fat used in many soaps is 76.5% carbon, 12.2% hydrogen, and 11.3% oxygen. What is its empirical formula? What is the molecular formula of a fat with a molecular mass of 705 g/mol? C. A sample of a substance is determined to be composed of 0.89 g of potassium, 1.18 g of chromium, and 1.27 g of oxygen. Calculate the empirical formula. 3|Page D. Strychnine, a deadly poison, has a molecular mass of 334 g/mol and a percentage composition of 75.42% carbon, 6.63% hydrogen, 8.38% nitrogen, and the balance oxygen. What is the molecular formula of strychnine? (Hint: DO NOT round up the number found for carbon in the empirical formula.) E. A 10. gram sample of a compound contains 7.22 grams of magnesium and 2.78 grams of nitrogen. What is its empirical formula? F. An organic compound with a molecular mass of 140 g/mol is 68.54% carbon, 8.63% hydrogen, and 22.83% oxygen. What is the molecular formula of the compound? G. To find the experimental empirical formula of a compound, a student heats a coil of magnesium ribbon (0.25 g) in a crucible. Oxygen combines with the magnesium when heated to form magnesium oxide. Data recorded: Mass of empty crucible and cover - 20.74g Mass of magnesium ribbon - 0.25g Mass of crucible, cover, and final product - 21.17g What is the empirical formula for magnesium oxide that was the final product? Show EVERY mathematical step fully. H. What is a hydrate?______________________________________________ Name the following hydrates: CuSO4 * 5H2O ________________ MgSO4 * 7H2O________________ Na2CO3*10H2O_______________ I. Cerium iodide (CeI3) occurs as a hydrate with the composition 76.3% CeI3 and 23.7% H2O. Calculate the formula of this hydrate. 4|Page II. Cobalt (II) nitrate, Co(NO3)2, is used in ceramic glazes. The compound exists as a hydrate that is 37.1% water and 62.9% cobalt (II) nitrate. What is the formula for this hydrate? 9. Stoichiometry: For a review of the topics below, you can refer to your honors chemistry notes or check the index on the prior sites in this assignment. Show your work on your own paper for each problem below. Circle your final answer. Then write your final answer on the line provided on this sheet with sig figs and units. Staple your work to the back of this packet. 1. Stoichiometry refers to _____________________________________. _____________2. Given the following reaction: GeH4 + 3GeF4 4 GeF3H this reaction, how many moles of GeF4 are needed? In order to product 8.00 mol of GeF3H with _____________3. Given the following reaction: AgNO3 + AlCl3Al(NO3)3 + AgCl be produced by 2.75 mol aluminum chloride? How many moles of silver chloride can 4. Write the balanced reaction for the complete combustion of propane (C3H8) _____________________________________ ______________The reaction of 2.5 mol of O 2 will produce how many mol of H2 0? 5. Under appropriate conditions, nitrogen and hydrogen combine to yield ammonia. ___Mg + ___N2 ___Mg3N2 _____________a. A 7.1 g sample of N2 requires ____ g of Mg for a complete reaction? _____________b. 100.0 g of N2 gas will theoretically yield how many grams of Mg3N2? _____________c. If the actual yield from an experiment is only 300.0 g, what is the percent yield of this reaction? _____________d. If 25.0 g of Mg are react with 14.0 g N2, which is the limiting reactant and how many grams of Mg3N2 will form? 6. Balance first: __LiOH + __KCl __ LiCl + __KOH _____________a. If you begin this with 20.00 grams of lithium hydroxide, what is your theoretical yield of LiCl? _____________b. If you actually produced 6.00 grams of lithium chloride, what is your percent yield? 7. Balance first: __C3H8 + __O2 __CO2 + __ H2O _____________a. If 5 grams of C3H8 is used what is the theoretical yield of water? _____________b. If you produced a percent yield of 75%, how many grams of water did you make? 8. Aluminum reacts with chlorine as described: ___Al s + ___Cl2 g___AlCl3 s _____________a. If you begin with 4.599 x 10-3 g Al and 2.332 x 10-2 g of chlorine gas, which is the limiting reactant? _____________b. How many grams of aluminum chloride can be produced from this reaction? _____________c. Calculate the mass of excess reactant that remains after the reaction is complete. _____________d. If you needed to make 100.0 g of AlCl3, how many liters of Cl2 do you need? 5|Page