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AP Chemistry Summer Assignment 2017-2018 Greetings! Welcome to AP Chemistry! Dear student and parents/guardians of student, You are receiving this letter because you have signed up for Advanced Placement Chemistry for the 2017-2018 school year. In order to be successful in this course it is highly recommended that you have had successful completion of a first-year high school chemistry course and also had successful completion of a second-year algebra course. Why Take AP Chemistry? There are several reasons why a student might want to take AP Chemistry, including (but not limited to) the following. 1. AP Chemistry will challenge you to the limits of your academic ability. In the past you may have found classes “too easy”, and therefore not stimulated you do your very best. This will not be the case in AP Chemistry. 2. AP Chemistry should allow you to earn college credit while still enrolled in high school. This will save time and money. Some students who passed the AP Chemistry exam elect to take first year college chemistry anyway, where they find the material easy review and achieve top grades while other students around them are frustrated and struggling in a class which is too large and/or the instructor is unavailable for help! 3. Being a “straight A” student no longer carries the weight it once did when applying for college. Many 4.0 grade average students are finding themselves denied entry at the college of their choice. Taking AP Chemistry is a way to distinguish yourself in high school. 4. AP Chemistry is an intense course where students really get to know each other. It is to a student’s advantage for the teacher to know them well when they need a letter of recommendation. The AP Chemistry class is a yearlong college level chemistry course, at the end of which you will take an exam to see your proficiency in college level Chemistry. The AP Chemistry test is in early May 2018 for all students world-wide. We start school later then many students (up to a month in some cases!), so we are behind from day 1. Because of this, I require a summer assignment that assures students are proficient in areas that will help them to be successful throughout the year. Much of this will be review of 1st year Chemistry, but there will be some “add ons” (for example, naming acid rules). Because of this, you will need to use your chemistry notebook and access to online chemistry resources. If you do not have online access at home, see me. Summer topics: 1. Math skills: significant figures, metric system, conversions, basic algebra skills 2. Atomic structure: counting subatomic particles, isotopes 3. Nomenclature: naming molecules and compounds (including acids), naming polyatomic ions 4. Balancing equations and identifying types of reactions 5. Solubility rules 6. Stoichiometry: g mol calculations, predicting the mass of product formed, limiting reactants Your assignment: 1. Complete all practice questions/tasks 2. Self grade your work in a second color (checking the ones correct and marking/second attempt to those incorrect) Online resources: (If you do not have online access over the summer, please see/email me) 1. My website (this will be a work in progress through the summer- see it for updates!): https://sites.google.com/a/k12.shorelineschools.org/ap-chemistry/ 2. Textbook (for quick help on definitions and topics): https://open.umn.edu/opentextbooks/BookDetail.aspx?bookId=69. 3. Bozeman Science videos (I will make you watch them later anyways!): http://www.bozemanscience.com/ap-chemistry/ 4. Khan Academy videos (excellent resource): https://www.khanacademy.org/science/chemistry 5. Crash course videos: https://www.youtube.com/playlist?list=PL8dPuuaLjXtPHzzYuWy6fYEaX9mQQ8oGr 6. Sciencegeek website for AP chem students (has lots of good info and resources linked): http://www.sciencegeek.net/APchemistry/index.shtml 7. AP chemistry college board website: https://apstudent.collegeboard.org/apcourse/ap-chemistry The summer assignment will be due on the first day of school next fall. During the first week of school, we will have a proficiency test over what you have done over the summer so that we can use our time as best as possible during the school year. Since this is a college level course taught in high school, it is very demanding, both in time and effort required. Students who are heavily involved in after school activities and/or jobs will have to learn to budget their time very carefully. We move at an incredibly fast pace as there is much to cover before the AP Exam. Parents/Guardians: This is a class that truly depends on the learning. Not only do students have to do the work but they need to understand and be able to process what is being done. Since AP Chemistry class is the same world-wide it is easy to find answers to almost every problem we assign online via search engines. This gives the student the right answer, but does not show them how to do the problem. Please encourage your student to try things on their own and get help when they need it. Remember, it is not about the grade, it is about the learning. Recommended Text Cracking the AP Chemistry Exam by Princeton Review 2017 edition (can be purchased via Amazon)- has lots of practice problems that we will work from. I have a personal copy that students can reference, but it cannot leave my classroom. Thank you! I will be online via email periodically (Ha!) throughout the summer if you have questions. I look forward to exploring deeper about chemistry with you next year! ~Gloria Horne [email protected] Summer Homework Assignment: YOUR JOB: Work through the concepts and practice problems provided. You will use the answer key at the end to check your work in a second color! If you get a problem wrong, try it again until you get it right! I want to see your work the first day of school. It is important that you do this work. Some time during the first week of school, you will have a proficiency test on the concepts in this assignment, so I want you to be prepared when you arrive. Part I: MATH review! Practice conversion calculations, scientific notation and significant figures! (essential skills in Ch 1 and 3 of online textbook) 1. How many SF in each number? a. 1234 f. 90210 b. 0.023 g. 1090.0010 c. 890 h. 0.00120 d. 91010 i. 780 e. 9010.0 j. 1000. 2. Convert the following to scientific notation: a. 1,200,000 ______________ b. 345,450,000 _____________ 3. Round the following to 2 sig figs: a. 0.436 ________ b. 27.2 _________ c. 0.000354 _______________ d. 0.000000045801 _________ c. 9.000 _________ d. 10000.0 _______ Calculations: Perform the following calculations and give the answer with the correct number of sig figs: 4) 628 * 342 = ___________________ 5) (5.63 x 102) * (7.4 x 103) = ____________________ 6) 2734/28.0 = ______________________ 7) 14.98 + 27.340 + 84.7539 = __________________ 8) 44.5 – 33.57 = ___________________ 9) 8119 x 0.000023 = _____________________ Metric conversions- convert these quantities to the requested units- don’t forget sig figs! 10) 4.32 x 10-2 mL to L 11) 0.0655 kg to g 12) 4.62 x 103 cm to km Dimensional analysis: Use the conversion factors and common metric conversions to perform the following calculations. Don’t forget sig figs! 1 lb = 0.454 kg 1 m = 1.09 yd 1 hr = 60 min 1 mile = 1760 yd 1 km = 0.621 mi 1 min = 60 sec. 13) A dog is 28.7 pounds. What is his weight in kg? What is his weight in grams? 14) A marathon is 26.2 miles. What is this distance in yards? What is the distance in meters? (Hint: use your answer in yards to convert to meters!) 15) Racing cars travel at a speed of 225 miles/hour. What is this speed in km/minute? (Hint: you will need two sets of conversions- one for time and one for distrance!) Part II: Atomic structure Fill in the chart with the chemical name, symbol and number of subatomic particles. The first one has been done for you. Chemical name Chlorine Chemical symbol 35 131 # of protons # of neutrons # of electrons Mass number 17 16 18 17 16 35 32 Cl 17 Xe 131 54 13 2 14 N 20 14 40 4 7 7 Phosphorus 31 30 P 15 16) Isotopes: Explain why atoms have different isotopes. In other words, how is it that carbon can exist in three different forms (carbon-12, carbon-13 and carbon-14)? 15 Part III: Reviewing Nomenclature (Ch 2 of online textbook) Polyatomic Ions: Please memorize and be able to name compounds using all of the following ions! Making flash cards could help! 1. Table of Polyatomic Ions for AP Chemistry Symbol Name Symbol Name BO33– B4O72 C2H3O2 C2O42 ClO ClO2 ClO3 ClO4 CN CO32 CrO42 Cr2O72 Fe(CN)63 Fe(CN)64 HCO3 HC2O4 HPO42 H2PO4 HSO3 HSO4 H3O+ Hg22+ borate tetraborate acetate oxalate hypochlorite chlorite chlorate perchlorate cyanide carbonate chromate dichromate ferricyanide ferrocyanide hydrogen carbonate hydrogen oxalate hydrogen phosphate dihydrogen phosphate hydrogen sulfite hydrogen sulfate hydronium mercury (I) MnO4 MoO42 N3 NH2 NH4+ NO2 NO3 OH PO33 PO43 P2O74 SO32 SO42 S2O32 S2O42 S2O62 S2O72 S2O82 SeO42 SiO32 VO3 permanganate molybdate azide amide ammonium nitrite nitrate hydroxide phosphite phosphate diphosphate sulfite sulfate thiosulfate dithionite dithionate disulfate peroxydisulfate selenate silicate vanadate 17) Name these binary compounds of two nonmetals. IF7__________________ N2O5_______________ XeF2 _________________ N2O4_______________ As4O10_______________ SF6________________ PCl3________________ S2Cl2_______________ 18) Name these binary compounds with a fixed charge (main group) metal. AlCl3 _______________ MgO_______________ BaI2_________________ KI_______________ SrBr2 _______________ Na2S _______________ CaF2 _____________ Al2O3_______________ 19) Name these binary compounds of cations with variable charge (transition metals). CuCl2 _____________ Fe2O3______________ SnO_________________ PbCl4______________ Cu2S_______________ HgS_________________ AuI3_______________ CoP________________ 20) Name these compounds with polyatomic ions. Fe(NO3)3_____________ NaOH_____________ Cu2SO4_______________ Ca(ClO3)2_____________ KNO2_____________ NaHCO3______________ NH4NO2______________ Cu2Cr2O7 ___________ 21) Name these binary acids – look up acid naming rules! HCl ________________ HOCl ________________ HI ________________ 22) Name these acids with polyatomic ions. HClO4________________ H2SO4_______________ HC2H3O2____________ H3PO4________________ HNO2_______________ H2CrO4_____________ 23) mixed bag: Name these compounds appropriately. CO________________ NH4CN ___________ HIO3_______________ NI3_______________ AlP _______________ OF2_____________ LiMnO4____________ HClO _____________ NaH2PO4_____________ SO2_______________ CuCr2O7____________ K2O______________ FeF3______________ KC2H3O2__________ MnS______________ 24) Write the formulas. Tin (IV) phosphide__________ copper (II) cyanide_____________ Magnesium hydroxide____________ sodium peroxide_____________ Sulfurous acid____________ lithium silicate __________ Potassium nitride ____________ chromium (III) carbonate____________ Gallium arsenide______________ cobalt (II) chromate____________ Zinc fluoride________________ dichromic acid________________ Part IV: Solubility rules 25) Review the solubility rules found in your notes from last year, or in Chapter 4: precipitation reactions of the online text book, Identify each of the following compounds as soluble or insoluble in water. Na2CO3___________ CoCO3_______________ Pb(NO3)2___________ K2S______________ BaSO4________________ (NH4)2S ___________ AgI______________ Ni(NO3)2______________ KI________________ FeS______________ PbCl2_________________ CuSO4_____________ Li2O_____________ Mn(C2H3O2)2___________ Cr(OH)3______________________________ AgClO3 __________ SnS2 _______________ FeF2______________ 26) Predict whether each of these double replacement reactions will give a precipitate or not based on the solubility of the products. If yes, identify the precipitate. (Hint: it may help to look up the definitions of a double replacement reaction and of a precipitate). a) silver nitrate and potassium chloride _________ b) strontium bromide and potassium sulfate ________ c) cobalt (III) bromide and potassium sulfide __________ d) ammonium hydroxide and copper (II) acetate __________ e) lithium nitrate and chromium (III) fluoride ___________ Part IV: Balancing Equations 27) Balance the following equations with the lowest whole number coefficients. a) S8 + O2 SO3 b) C10H16 + Cl2 C + HCl e) KClO3 KCl + O2 f) H3AsO4 As2O5 + H2O c) Fe + O2 Fe2O3 g) V2O5 + HCl VOCl3 + H2O d) C7H6O2 + O2 CO2 + H2O h) Hg(OH)2 + H3PO4 Hg3(PO4)2 + H2O Part V: Stoichiometry and Limiting Reactants (Khan Academy is best for this) 28) Given the equation below, what mass of water would be needed to react with 10.0g of sodium oxide? Na2O + H2O 2NaOH 29) What mass of sodium chloride is formed if 45.0g of oxygen gas is also formed? 2NaClO3 2NaCl + 3O2 30) What mass of water will be produced when 100.0g of ammonia is reacted with excess oxygen? 4NH3 + 5O2 4NO + 6 H2O 31) If the reaction in #30 is done with 25.0g of each reactant, which would be the limiting reactant (also called limiting reagent)? How many moles of each product would form? 32) Na2S + 2AgNO3 Ag2S + 2NaNO3 a) If the above reaction is carried out with 35.0g of sodium sulfide and 50.0g of silver nitrate, which is the limiting reactant? b) What mass of silver sulfide would precipitate? c) challenge- try it!! What mass of the excess reactant remains? 33) What volume of hydrogen gas (measured at STP) would result from reacting 75.0g of sodium hydroxide with 50.0g of aluminum? 6NaOH + 2Al 2Na3AlO3 + 3H2 END OF ASSIGNMENT Answers: 1. a. b. 2. a. b. 3. a. b. 4 2 c. 2 d. 4 e. 5 f. 4 g. 8 h. 3 1.2 x 106 3.4545 x 108 c. 3.54 x 10-4 d. 4.5801 x 10-8 0.44 27 c. 9.0 d. 1.0 x 104 4. 215000 5. 4200000 6. 97.6 7. 127.07 8. 10.9 9. 0.19 10. 4.32 x 10-5 L or 0.0000432 L chart: Chemical name Chlorine sulfur xenon i. 2 j. 4 11. 65.5 g 12. 0.04620 km 13. 13.0 kg, 13000g 14. 46100 yd, 42300 m 15. 6.04 km/min Chemical symbol # of protons # of neutrons # of electrons Mass number 17 18 17 35 S 16 16 16 32 Xe 54 77 54 131 Ca 20 20 20 40 35 17 Cl 32 16 131 54 Calcium 40 20 aluminum 27 13 Al 13 14 13 27 helium 4 2 He 2 2 2 4 7 7 7 14 Nitrogen 14 7 Phosphorus 31 15 P 15 15 16 31 Phosphorus 30 15 P 15 15 15 30 N 16. They have different numbers of neutrons (and a different mass), but they all have the same number of protons (same element) 17. IF7 Iodine heptafluoride N2O5 dinitrogen pentoxide XeF2 xenon difluoride N2O4 dinitrogen tetraoxide As4O10 tetraarsenic decoxide SF6 sulfur hexafluoride PCl3 phosphorus trichloride S2Cl2 disulfur dichloride 18. AlCl3 aluminum chloride MgO magnesium oxide BaI2 barium iodide KI potassium iodide SrBr2 strontium bromide Na2S sodium sulfide CaF2 calcium fluoride Al2O3 aluminum oxide 19. CuCl2 copper II chloride Fe2O3 iron III oxide SnO tin II oxide PbCl4 lead IV chloride Cu2S copper I sulfide HgS mercury II sulfide AuI3 gold III iodide CoP cobalt III phosphide 20. Fe(NO3)3 Iron III nitrate NaOH sodium hydroxide Cu2SO4 copper I sulfate Ca(ClO3)2 calcium chlorate KNO2 potassium nitrite NaHCO3 sodium hydrogen carbonate NH4NO2 ammonium nitrite Cu2Cr2O7 copper I dichromate 21. HCl hydrochloric acid HOCl hypochlorous acid HI hydroiodic acid 22. HClO4 perchloric acid H2SO4 sulfuric acid HC2H3O2 acetic acid H3PO4 phosphoric acid HNO2 nitrous acid H2CrO4 chromic acid 23. COcarbon monoxide NH4CN ammonium cyanide HIO3 iodic acid NI3 nitrogen triiodide AlP aluminum phosphide OF2oxygen difluoride LiMnO4lithium permanganate HClO hypochlorus acid NaH2PO4 sodium dihydrogen phosphate SO2 sulfur dioxide CuCr2O7copper II dichromate K2Opotassium oxide FeF3 Iron III fluoride KC2H3O2 potassium acetate MnS manganese II sulfide 24. Tin (IV) phosphide Sn3P4 copper (II) cyanide Cu(CN)2 Magnesium hydroxide Mg(OH)2 sodium peroxide Na2O2 Sulfurous acid H2SO3 lithium silicate Li2SiO3 Potassium nitride K3N chromium (III) carbonate Cr2(CO3)3 Gallium arsenide GaAs cobalt (II) chromate CoCrO4 Zinc fluoride ZnF2 dichromic acid H2Cr2O7 25. Na2CO3 soluble K2S soluble CoCO3 insoluble BaSO4 insoluble Pb(NO3)2 soluble (NH4)2S soluble AgI insoluble Ni(NO3)2 soluble KI soluble FeS insoluble PbCl2 insoluble Li2O soluble Mn(C2H3O2)2 soluble Cr(OH)3 insoluble AgClO3 insoluble CuSO4 soluble SnS2 insoluble FeF2 insoluble 26. silver nitrate and potassium chloride solid = AgCl strontium bromide and potassium sulfate SrSO4 cobalt (III) bromide and potassium sulfide Co2S3 ammonium hydroxide and copper (II) acetate Cu(OH)2 lithium nitrate and chromium (III) fluoride none 27. a. S8 + 12 O2 8 SO3 e. 2KClO3 2KCl +3 O2 b. C10H16 + 8Cl2 10 C + 16HCl f. 2H3AsO4 As2O5 + 3H2O c. 4Fe + 3O2 2Fe2O3 g. V2O5 + 6HCl 2VOCl3 + 3H2O d. 2C7H6O2 + 15O2 14CO2 + 6H2O h. 3Hg(OH)2 + 2H3PO4 Hg3(PO4)2 + 6H2O 28. 2.90 g 29. 54.6 g 30. 158.8 g 31. oxygen is LR, 0.625 mol NO, 0.938 mol H2O 32. a. silver nitrate 33. 21.0 L H2 (L.R. NaOH) b. 36.5 g c. 23.5 g