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Dear Chemistry Student, I am excited that you have chosen to challenge yourself by taking on the rigors of AP Chemistry here at Cathedral Catholic High School. In order to prepare you for the expected performance outcomes of the course, every one will be expected to complete a Summer Independent Study Program. Since students entering AP Chemistry will have had a full year of Chemistry, the summer assignment is intended to help students maintain old skills and prepare them for the exam that will be given during the first week of school. In the past, I have found that students who have failed to master the concepts in the summer assignment struggle during the semester to manage the workload and maintain a satisfactory grade. A completed summer assignment is the key to success in this class. Additionally, there are 85 polyatomic ions that will not be provided during the year and will be tested on directly during the first week of school and indirectly throughout the remainder of the school year. Some review videos have been posted onto my You Tube page. Although they are not comprehensive, they do cover some of the more challenging aspects of the Chemistry 1 curriculum. Another resource for material you may need help reviewing will be your textbook. Please be sure to purchase it at the beginning of the summer! I look forward to having you in my class next year! - Mrs. Martin Summer Assignment Due: First Day of Class! Summer Assignment Exam: First Week of School! Summer Assignment Review Videos: https://www.youtube.com/playlist?list=PLwi78F-QlPg-NqpzQhOvKZSHjR4FFcYgy AP Chemistry Summer Study Assignment 2016 Make sure to complete these ON YOUR OWN PAPER, in order! Don’t wait until the last minute!!! The purpose of the summer assignment is three-fold. First, it should serve as a basic review of Chemistry 1 material, just in case you’ve forgotten some of the information since you took the class. Two, it will prepare you for the first week of Chemistry class, as we will “hit the ground running” with a test over the summer assignment (including all 85 polyatomic ions) and quickly move on to AP Chemistry topics. Lastly, it gives you a week by week breakdown for your summer work. Students who have slacked off on the summer assignment in the past have performed poorly in the class itself. Don’t let this be you! This summer assignment is due on the first day of class. Good luck! Week 1: Get Organized! -Purchase your textbook now! You will need it to study and look up concepts that you may not remember from Chemistry 1. Getting familiar with your book will help you be better prepared for the rigors of the school year. You can order from Amazon or any other book site. Chemistry-6th Edition – Zumdahl ISBN-13: 978-0618221561 -Begin memorizing the 85 Polyatomic Ions list. You will need to know both name and ion formulas. These are the easiest exam points you will earn all year so be sure to make it happen! =) - Check out Mrs. Martin’s video page on You Tube. There are some review videos that may help you with various parts of last year’s chemistry content. Additionally, this is where you will be getting your lecture notes during the school year. Getting familiar now is always a good thing! https://www.youtube.com/playlist?list=PLwi78F-QlPg-NqpzQhOvKZSHjR4FFcYgy Week 2: Nomenclature/Lewis Dot Structures/Shapes/Ionic/Covalent Identification 1. Write the formulas for the following compounds: a. mercury(I) chloride h. phosphorus tetrachloride o. potassium chlorate b. zinc hydroxide i. barium hydroxide p. zinc nitrite c. ferric fluoride j. potassium permanganate q. lithium sulfite d. silver nitrate k. sulfuric acid r. strontium bromide e. calcium bromate l. lead(II) iodide s. aluminum oxide f. acetic acid m. hydrogen chloride t. lithium phosphate g. magnesium bisulfate n. sodium chlorite u. sodium bicarbonate 2. Write the name of the following compounds: a. MgCl2 e. HClO b. CuSO4 f. Mg(OH)2 c. KMnO4 g. H2O2 d. Na2CO3 h. LiBr 3. Name the following compounds a. CO2 f. AlCl3 b. O2 g. CrI3 c. KCl h. N2O5 d. Sn(NO3)4 i. NaOH e. Na2S j. CaCO3 i. j. k. l. MnF4 HgO Al2O3 Fe2O3 k. phosphorus trichloride l. lithium oxide m. ammonium phosphate n. strontium nitrate o. beryllium chloride m. AgNO3 n. H2SO4 o. BaS p. nitrogen oxide q. hydrogen peroxide r. ferric sulfate s. diarsenic trichloride t. sodium bromide 4. a. b. c. d. e. Name the following compounds. NaCl f. KBr H2SO4 g. S8 CaF2 h. O2 H2 O i. SO4 N2 O4 j. Os k. l. m. n. o. C5O3 H2 O2 NaH2SO4 SrBr2 CO p. q. r. s. t. CO3 I2 MgCl2 SF5 FeCl3 u. KOH v. HF w. HNO3 5. Name the following compounds: a. H2SO4 b. SCNc. N2 d. Hg2I2 e. ZnS f. AlPO3 g. KNO3 h. HF i. CoCO3 j. NaCl k. Mg(OH)2 l. H3BO3 m. Bi(OH)5 n. AgHCO3 o. NH3 p. AlBr3 q. HCl r. H2S s. C4H4 t. LiMnO4 6. Write the name or formula for the following: a. NaBr b. Ca(C2H3O2)2 c. P2O5 d. Ti(SO4)2 e. FePO4 f. K3N g. SO2 h. CuOH i. Zn(NO2)2 j. V2S3 k. silicon dioxide l. nickel (III) sulfide m. manganese (II) phosphate n. silver acetate o. diboron tetrabromide p. magnesium sulfate heptahydrate q. potassium carbonate r. ammonium oxide s. tin (IV) selenide t. carbon tetrachloride Week 3: Balancing/Writing/Product ID/Rxn Type Chemical Equations/Lewis Dot Structures 7. Predict products and/or write/balance equations for the following, and state what kind of reaction would occur: a. calcium carbonate (aq) + magnesium bromate (aq) b. HNO3 is added to KOH c. hydrogen is mixed with sodium fluoride d. AlBr3 is strongly heated (decomposes!) e. ammonium perchlorate (aq) + Li2O (aq) f. C6H12 is burned in oxygen g. balance: CH4 + O2 → CO2 + H2O h. balance: K + H2O → KOH + H2 i. the reaction of ammonia with iodine to form nitrogen triiodide (NI3) and hydrogen gas j. the combustion of propane (C3H8) k. the reaction of nitric acid with potassium hydroxide l. the reaction of copper (II) oxide with hydrogen to form copper metal and water m. the reaction of AlBr3 with Mg(OH)2 n. the decomposition of calcium carbonate. o. lithium hydroxide is added to aluminum sulfate. p. pentene, C5H10, is burnt in air. q. sodium is mixed with chlorine. r. sodium is added to water. 8. Draw the best Lewis Dot Structures for each of the following molecules. Be sure to include molecular shape, bond angles and formal charges for each and resonance where necessary. a. NH3 b. SO42- c. CCl4 d. NO3-1 e. SF6 f. XeF4 g. H2S h. CO2 i. O2 j. BF3 k. CClF3 l. XeF2 m. CO32- n. NH4+1 o. PF5 Week 4: The Mole/Stoich/LR/ER/%yield/%comp/EF/MF 9. Answer the questions below using the equation provided. Na + Cl2 → NaCl a. How many moles of chlorine gas (Cl2) would react with 5 moles of sodium (Na) according to the chemical equation above? (Balance equation!) b. Using the equation above, determine the amount of product that can be produced from 24.7 g Na. c. How many molecules of product would be produced from 24.7g Na? 10. Chlorine is used by textile manufacturers to bleach cloth. Excess chlorine is destroyed by its reaction with sodium thiosulfate, Na2S2O3: Na2S2O3(aq) + 4Cl2(g) + 5H2O(aq) → 2NaHSO4(aq) + 8HCl(aq) a. How many moles of Na2S2O3 are needed to react with 0.12mol of Cl2? b. How many moles of HCl can form from 0.12mol of Cl2? c. How many moles of H2O are required for the reaction of 0.12mol of Cl2? d. How many moles of H2O react if 0.24mol HCl is formed? 11. Determine the empirical formula of a compound with the following composition by mass: 48.0 % C, 8.0 % H, 28.0 % N and 16.0 % O. If this compound has a molar mass of 200 g/mol , what is its molecular formula? 12. Determine the empirical formula of a compound with 20.8 % hydrogen, 36.3 % oxygen, and 42.9 % carbon 13. Determine the molecular formula of CHO, given the molecular mass of 174.9 amu. 14. Calculate the number of molecules in 325 grams of lithium oxide. 15. If 4.50 g of Li reacts with 4.5 g of O2, what mass of lithium oxide is produced? 16. If 27.3g of C8H18 are combusted, what mass of water will be produced? 17. The actual yield of a solution is 3.0 x 103, the theoretical yield is 3.5 x 103, what is the percent yield? 18. A compound is found to contain 71.9% potassium and 28.1% sulfur. Find the empirical formula. 19. How many grams of NO can be produced from 65 grams of NH3? 4NH3 + 5O2 →4NO + 6H2O 20. HCl + NaOH → NaCl + H2O a. Given that there is 2 moles of HCl and 2.5 moles of NaOH reacting, find the limiting reactant (hint: write a balanced equation). 21. 2HNO3(aq) + 3H2S(g) -> 2NO(g) + 4H2O(l) +3S(s) In the reaction above, 4.62g HNO3(aq) and 1.84g H2S(g) are mixed. How many grams of NO(g) is formed? 22. A compound containing carbon, hydrogen, and oxygen is 52.11% carbon, 13.14% hydrogen, and 34.75% oxygen. What is the empirical formula of this compound? 23. Calculate the indicated quantity for each of the given chemical reactions: a. Theoretical yield= 1.0g, percent yield= 90.0%, actual yield= ? b. Theoretical yield= 3.45g, percent yield= 48.0%, actual yield= ? 24. Give the empirical formula for a compound made up of, 24% C, 48%O, and 28% N. 25. Determine the percentage of sodium in sodium sulfate. 26. Draw the periodic trend of electron affinity. 27. Calculate the percent composition of the elements in HNO3. 28. Given the equation, 2Fe+ 3Cu(OH)2 → 2Fe(OH)3 + 3Cu, a. If 1 mole of iron reacts completely, how many grams of Cu is formed? If 28.4 grams of Fe(OH)3 is produced, how many grams of Fe reacted? 29. Aluminum hydroxide reacts completely with acetic acid (HC2H3O2) a. Write the reaction. b. If 100 grams of aluminum hydroxide reacts with 100 mL of 3 M acetic acid, what is the limiting reactant? 30. Ba2+ + 2Cl+ à BaCl2 According to the reaction above, how many grams of chlorine are required to completely react to form 208.2g of barium chloride. Week 5: Gas Laws 31. What is the equation for the combined gas law 32. What is the equation for Boyle’s Law? 33. What is the equation for Charle’s Law? 34. What is the equation for Gay-Lussac’s Law? 35. What is the equation for the Combined gas law? 36. What is the equation for the Ideal gas law? 37. When 5.0 moles of O2 are confined to a 24 liter container at 87°C, the pressure is 6.0 atm. If the oxygen is allowed to isothermally expand to 36 liters, what is the new pressure? 38. A 502.8g sample of X2(g) has a volume 9.0 L at 10 atm and 102°C. What is element X? 39. If a baloon with a volume of 12.2 L is at 22.5 oC what will be its new volume when placed in a freezer at 0 oC? 40. If I have 5.6 liters of gas in a piston at a pressure of 1.5 atm and compress the gas until its volume is 4.8 L, what will the new pressure inside the piston be? 41. A toy balloon has an internal pressure of 1.05 atm and a volume of 5.0 L. If the temperature where the balloon is released is 20°C, what will happen to the volume when the balloon rises to an altitude where the pressure is 0.65 atm and the temperature is –15°C? 42. Calculate the pressure of 2 moles of a gas at 20°C with a volume of 200mL. 43. If there is a solid, rigid container holding 3 moles of N2 gas at 760 torr and 25oC, and then the container is heated to 50oC, what is the new pressure of the gas in atm? 44. If there is a 5.00L container holding O2 gas at standard temperature and pressure, how many grams of O2 are in the container? Week 6: Solutions 45. What is the equation for molarity? 46. What is the equation for molality? 47. What is the equaiton for dilutions? 48. The molarity of a solution is 0.75M. How many moles of the solute is needed in 500mL of solvent? 49. What is the molarity of a solution containing 0.32 moles of NaCl in 3.4 liters? 50. How many moles of KBr are in 25.0 mL of a 1.23 M KBr solution? 51. Determine molarity of 11.4 g of ammonia in 200. mL of water. 52. What is the concentration of a solution made by diluting 40 mL of 9 M H2SO4 to a total volume of 600 mL? 53. What volume of a 5.0M solution is needed to make 20.0L of .50M of the same solution? 54. How many moles of NaOH are there in 500 mL of a 2.0 M solution? 55. If 80.2g of calcium are added to 10000mL of water, what is the molarity of the resulting solution? 56. If 167.385mL of water are added to 86.3L of ammonium nitrate solution, what is the resulting volume in liters? (sig figs) 57. How many milliliters of a 2.0 M H2SO4 is needed to make 45.0 mL of a 0.10 M H2SO4 solution? 58. 16.7 grams of substance X is dissolved in 100 mL water and gives a molarity of 2.5 M. What is the molecular mass of substance X? Week 7: Acids and Bases 51. According to Bronsted-Lowry, what are acids? 52. According to Bronsted-Lowry, what are bases? 53. What does amphoteric mean? 54. What is the value of Kw? 55. The [H3O+] is 0.0543 M. What is the pOH? 56. What is [H3O+] in a solution with a pH of 3? 57. The pH of a solution is 7.8. What is the pOH and [H3O+]? 58. Calculate the pH of each solution: a. [H+] = 1.4 x 10-3 M b. [H+] = 2.5 x 10-10 M c. [H+] = 6.1 M d. [OH-] = 3.5 x 10-2 M e. [OH-] = 8 x 10-11 M f. [OH-] = 5.0 M Week 8: Chemical Changes, Sig Figs, Density, Periodic Trends. 59. 60. 61. 62. What type of bond is NaCl? List the seven diatomic elements. What is the difference between polar and non-polar bonds? Which of the following is a chemical change? a. Metal melting into a molten liquid b. Metal rusting c. Water expanding as it freezes d. Ink spreading on paper e. Cutting paper in half 63. Which of the following is true? a. chemical changes change the properties of the substance b. physical changes change the properties of the substance c. chemical changes always change colors d. physical changes involve color changes e. chemical changes is filtering two substances 64. Chemical or physical: ice melting. 65. Metals _____________ electrons. (Gain or lose) 66. Nonmetals ___________ electrons. (Gain or lose) 67. A brick of salt measuring 10.0 cm x 10.0 cm x 2.0 cm weighs 433 grams. What is its density? 68. How many sig figs are in the following number 5700? 69. Is O2 a compound or an element? 70. Is melting ice a physical or a chemical change? 71. Give the definition of a mixture. 72. Is magnesium or chlorine more electronegative? List the seven diatomic elements. How many sig figs are in the number 33,516? Convert 0.25 nanometers to cm. Write the long electron configuration for chlorine. What volume of silver metal will weigh exactly 2500.0 grams? The density of silver is 10.5 g/cm3. 78. Draw the periodic trend of ionization energy. 79. What is density equal to? 80. What is the density of 57.8g of NaCl in 147.4mL of water? 83. The density of chlorine is 35.9 g/mL. If you have 20 mL, what is the weight of the sample? 84. Write the electron configuration of nitrogen. 85. Write the noble gas electron configuration of chlorine. 73. 74. 75. 76. 77. 86. Classify each as a solution, colloid or suspension (heterogeneous mixture), element, or compound: a. salt water b. milk c. sodium d. carbon monoxide e. muddy water f. sweet tea 87. How many electrons are in the valence shell of a. the halogens d. boron b. oxygen e. neon c. the alkali metals f. the alkaline earth metals g. carbon h. nitrogen 88. Write the electron configuration for the element copper. 89. What is the weight of the ethyl alcohol that exactly fills a 200.0 mL container? The density of ethyl alcohol is 0.789 g/mL. 90. How many sig figs are in the number 7.080 x 10-7? 91. Answer with the correct number of sig figs: (37.14 cm)(0.1458 cm) 92. Answer with the correct number of sig figs: 4.57 mL + 89.14 mL 93. Find the density of a sample that weighs 6.39g with the volume of 15mL. 94. If the density of a sample is 15.24 g/mL and the volume is 25mL. Find the mass in grams. 95. Give the longhand electron configuration for Os. 96. The following electron configuration is for what element? 1s22s22p63s23p64s23d104p65s24d4 97. Which one have the highest ionization: N O F Cl 98. How many sig figs are in each of these numbers: a. 1.543 c. 10250 e. 0.02750 b. 0.003 d. 1.57x1012 f. 27.861 99. What is the full electron and noble gas electron configuration of Sn? a. Out of the elements Rb, Fe, F, and Se, which one has the highest: a. atomic radius b. electronegativity c. electron affinity d. ionization energy 100. Write the electron configuration for the following: a. Ca+2 b. Cl-1 c. Co+1 101. Write the noble gas configuration for: a. O-2 b. U 102. How many sig figs do each of the following numbers have? a. 101.000 b. 1012300 c. 0.000032 103. Which has the smallest atomic radius? Ca+2, Na+1, O-2, or Ne 104. Which is most electronegative? C, N, O, F? c. W d. 1.09800 e. 0.900 -2- GO ON TO THE NEXT PAGE. All My Ions A List of 85 Ions to MEMORIZE Cations Aluminum Ammonium Antimony Al3+ NH4+ (III) Sb3+ (V) Sb5+ Arsenic (III) As3+ (V) As5+ Barium Ba2+ Bismuth (III) Bi3+ (V) Bi5+ Calcium Ca2+ Cadmium Cd2+ Chromium (II) or chromous Cr2+ (III) or chromic Cr3+ Cobalt (II) or cobaltous (III) or cobaltic Co2+ Co3+ Copper (I) or cuprous (II) or cupric Cu+ Cu2+ Hydrogen H+ Hydronium H3O+ Iron (II) or ferrous Fe2+ (III) or ferric Fe3+ week 1 Lead (II) or plumbous (IV) or plumbic Lithium Magnesium Manganese Li+ Mg2+ (II) Mn2+ (IV) Mn4+ Mercury (I) or mercurous (II) or mercuric Hg2+ Nickel Potassium Silver Sodium Strontium (II) Ni2+ (III) Ni3+ K+ Ag+ Na+ Sr2+ Tin (II) or stannous Sn2+ (IV) or stannic Sn4+ Zinc Pb2+ Pb4+ Zn2+ Hg22+ Anions Acetate C2H3O2Arsenate AsO43Bicarbonate HCO3Binoxalate HC2O4Bisulfate HSO4Bisulfide HSBisulfite HSO3Borate BO33Bromate BrO3Bromide BrBromite BrO2Carbonate CO32Chlorate ClO3Chloride ClChlorite ClO2Chromate CrO42Cyanide CNDichromate Cr2O72Dihydrogen phosphate H2PO4Ferrocyanide Fe(CN)64Ferricyanide Fe(CN)63Fluoride FHydroxide OHHypobromite BrOHypochlorite ClOHypoiodite IOIodate IO3Iodide IIodite IO2Nitride N3Nitrate NO3Nitrite NO2Oxalate C2O42Oxide O2Perbromate BrO4Perchlorate ClO4Permanganate MnO42Peroxide O2 Phosphate PO43Phosphide P3Phosphite PO33Sulfate SO42Sulfide S2Sulfite SO32Tartrate C4H4O62Thiocyanate SCNThiosulfate S2O32- week 2 week 3 week 4