Welcome to AP/DE Chemistry, AP/DE CHEMISTRY Summer Assignment AP/DE Chemistry is a challenging yet extremely rewarding college level course. AP/DE Chemistry involves problem solving to integrate your laboratory, math and logical reasoning skills. My goal is to prepare you for the AP exam & for college chemistry. Whether you plan to be a science or engineering major this class will help you tremendously. You are among the best students at THS and I know that you are up to the challenge of AP/DE Chemistry. I promise that you will have support when you need it and the help you need to achieve beyond where you ever thought you could! THIS SUMMER ASSIGNMENT IS Graded!!!. In order to start the school year prepared, please complete this summer assignment. It will be counted as your first assignment grade and most importantly, it will help you prepare for the first test. We will conduct a general review of first-year chemistry material during the first day of school and we will have an assessment on the first week of class on items that are in this summer review packet. I hope that you have an enjoyable, exciting and educational summer. Looking forward to seeing you all in August! Go Shine, Angelin Daniel angelin.daniel@lcps.org 1
Show ALL work and units. Use significant figures. Neatly organize your work. Atoms and Molecules 1. Determine the missing values for each atom listed. 55 Mn 1+ 25 Number of protons Number of electrons Number of neutrons Atomic number Atomic mass 75 As 3 33 Number of protons Number of electrons Number of neutrons Atomic number Atomic mass 2. Write the valence electron configuration for a. P 2- b. Al3+ 3. For each compound: draw the structure, state the geometry and state the polarity. a. PF3 b. BeCl2 4. Write and name the compound formed by the combination of these ions a. Mg 2+ + Br 1- b. Al 3+ + CO 2-3 c. NH 1+ 4 + SO 2-3 d. Ti 3+ + PO 3-3 Conversions 5. A mole of hydrogen atoms contains 6.02 x 10 23 atoms and occupies 22.4 L. How many hydrogen atoms are contained in 25.00 ml of this gas? 6. A sample of seawater contains 0.075 g of sodium chloride per ml of solution. How many moles of sodium chloride are there per liter of this solution? 7. Convert 7.098 mol of CO 2 to grams of CO 2. 8. Convert 4.12 x10 21 molecules of SiO 2 to grams of SiO 2 2
9.How many grams of calcium carbonate, CaCO 3, contain 48 grams of oxygen atoms? 10.When a 1.25-gram sample of limestone, that contains CaCO 3 and inert impurities was dissolved in acid, 0.22 grams of CO 2 was generated. What was the percent of CaCO 3 by mass in the limestone? Significant Figures 11.Express the answer to each of the following calculations with the correct number of significant figures. a. 80 cm + 13.0 cm b. (0.0130 mm)(2.4 mm) c. 2.3 x 1.45 + 10.6 Reaction Prediction 12. For each set of reactants: state the type of reaction, write the formulas of the reactants and predict the products a. Solid sodium carbonate is heated. b. Aqueous solutions of potassium sulfate and zinc phosphate are mixed. c. Liquid bromine and sodium iodide are mixed. d. Solid calcium oxide is added to water. Determining Oxidation Numbers 13.Determine the oxidation number of the underlined atom. [Note the overall charge of the molecule is equal to the sum of the oxidation numbers of each individual atom] 2- a. Cr 2O 7 Cr = b. Fe 2O 3 Fe = c. P 4O 6 P = 3
. Equation Writing and Balancing 14.Balance each equation. Write the formulas where required. a. Zn + H 2 SO 4 ZnSO 4 + H 2 b. H 2 O H 2 + O 2 c. HNO 3 + LiOH _H 2 O + LiNO 3 d. mercury (II) oxide mercury + oxygen e. f. nitrogen + hydrogen ammonia copper + iron (III) nitrate copper (II) nitrate + iron Molecular and Empirical Formulas 15.A certain compound was analyzed and found to have the following composition: 54.6g carbon, 9.0g hydrogen and 71.1g oxygen. The molar mass of this compound is 90.0. What are the empirical and molecular formulas of this compound? 16.A gaseous compound is found to have the following composition: 30.5% nitrogen, and the rest oxygen. The molar mass of this gas is 91.8. What are the empirical and molecular formulas of the compound? Acid Base Problems 17.If a solution has a hydrogen ion concentration of 1.0 x 10-7 M, what is the ph of the solution? 18.What is the poh of a solution that has a hydrogen ion concentration, [H + ], of 2.4 x 10-5? 4
19.If 200. ml of 0.80 M MgCl 2 (aq) is added to 600. ml of distilled water, what is the concentration of Cl - (aq) in the resulting solution? Gas Law Problems 20. Calculate the density of carbon monoxide gas at STP. 21. What mass of oxygen is contained in a 3.50 L tank where the temperature is 50.0 C and the pressure is maintained at 4.5 atm? 22. What pressure will be exerted by each of the gases in the following mixture if the total pressure of the mixture amounts to 768.8 torr? 0.500 g H 2, 0.245 g O 2 and 0.335g N 2 23. A gaseous mixture containing 7.0 moles of hydrogen, 2.5 moles of oxygen, and 0.50 mole of helium at a total pressure of 0.60 atmospheres. What is the partial pressure of the hydrogen? 24. The density of an unknown gas is 2.00 grams per liter at 3.00 atmospheres pressure and 127 C. What is the molecular weight of this gas? (R = 0.0821 liter-atm / mole-k) Energy 21. Calculate the amount of heat needed to heat 40.0 g of water from 25.0 C to 60.0 C, specific heat of 4.184 J/g C. 22. How much heat is needed to evaporate 125 g of Sb if the heat of vaporization is 380 cal/g? 23. A reaction begins with the reactants at 120.0 J of energy. When the reaction is over the products have 95.0 J of energy. What is the heat of reaction? Is this reaction exothermic or endothermic? 5
Stoichiometry 24. When sodium carbonate reacts with hydrochloric acid, the carbonic acid that is formed immediately breaks down into carbon dioxide and water. What mass of sodium carbonate would have been originally present if 5.0 L of carbon dioxide was produced? [hint - molar volume of a gas is 22.4 L/mol] Na 2CO 3 + HCl NaCl + CO 2 + H 2O 25. What mass of Cu is produced when 0.0500 mol of Cu 2S is reduced completely with excess H 2? CS 2 (l) + 3 O 2 (g) CO 2 (g) + 2 SO 2 (g) 26. What number of moles of O 2 is needed to produce 71 grams of P 4O 10 from P? (Molecular weight P 4O 10 = 284) Memorize 27. Element Names and Symbols of Common Elements & Phases 28. Al aluminum 29. Sb antimony 30. Ar argon 31. As arsenic 32. Ba barium 33. Be beryllium 34. B boron 35. Br bromine 36. Cd cadmium 37. Ca calcium 38. C carbon 39. Cs cesium 40. Cl chlorine 41. Cr chromium 42. Co cobalt 43. Cu copper 44. F fluorine 45. Fr francium 46. Ge germanium 47. Au gold 48. He helium 49. H hydrogen 50. I iodine 51. Fe iron 52. Kr krypton 53. Pb lead 54. Li lithium 6 55. Mg magnesium 56. Mn manganese 57. Hg mercury 58. Ne neon 59. Ni nickel 60. N nitrogen 61. O oxygen 62. Pd palladium 63. P phosphorous 64. Pt platinum 65. Pu plutonium 66. K potassium 67. Ra radium 68. Rn radon 69. Rb rubidium 70. Se selenium 71. Si silicon 72. Ag silver 73. Na sodium 74. Sr strontium 75. S sulfur 76. Te tellurium 77. Th thorium 78. Sn tin 79. W tungsten 80. U uranium 81. Xe xenon
82. - All metals are solid except for mercury which is a liquid. 83. - All metalloids are solids. 84. - Nonmetals: carbon, phosphorus, sulfur, & selenium are solids; bromine is a liquid; and the rest are gases. 85. - Elements with Subscripts: Br2, I2, N2, Cl2, H2, O2, F2, P4, S8 Polyatomic Ions H2PO4 - C2H3O2 - HSO3 - HSO4 - HCO3 - NO2 - NO3 - CN - SCN - OH - MnO4 - ClO - ClO2 - ClO3 - ClO4 - BrO - BrO2 - BrO3 - dihydrogen phosphate acetate hydrogen sulfite (bisulfite) hydrogen sulfate (bisulfate) hydrogen carbonate (bicarbonate) nitrite nitrate cyanide thiocyanate hydroxide permanganate hypochlorite chlorite chlorate perchlorate hypobromite bromite bromate BrO4 - IO - IO2 - IO3 - IO4 - HPO4 2- C2O4 2- SO3 2- SO4 2- CO3 2- CrO4 2- Cr2O7 2- SiO3 2- O2 2- PO3 3- PO4 3- BO3 3- NH4 + per bromate hypoiodite iodite iodate periodate hydrogen phosphate oxalate sulfite sulfate carbonate chromate dichromate silicate peroxide phosphite phosphate borate ammonium 7
Metals with Multiple Oxidation States Element Symbol Oxidation # Old System New System Iron Fe +2 Ferrous Iron (II) +3 Ferric Iron (III) Copper Cu +1 Cuprous Copper (I) +2 Cupric Copper (II) Mercury Hg2 +2 Mercurous Mercury (I) Hg +2 Mercuric Mercury (II) Lead Pb +2 Plumbous Lead (II) +4 Plumbic Lead (IV) Tin Sn +2 Stannous Tin (II) +4 Stannic Tin 8
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