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CHEMISTRY FINAL EXAM 1. The following molecule, H2, is: A. Organic B. Inorganic C. A gas D. Both B and C 2. Matter is anything that has: A. force and weight B. Kinetic energy and Potential energy C. Volume and Mass D. Electrons and a nucleus 3. The law of conservation and energy states that energy cannot be: A. Created or changed B. Created or destroyed C. Changed or destroyed D. None of the above 4. The 5 states of matter are solid, liquid, gas, : A. Silly Putty and Jell-O B. Plasma star and neutron C. Plasma and neutron star D. Ice and heat 5. Express the following calculation in the proper number of significant figures for this calculation, 3.034 + 5.1 : A. 8.134 B. 8.13 C. 8 D. 8.1 6. Choose the correct number of significant figures for this calculation, 3.034 X 5.1: A. 15.4 B. 15.47 C. 15 D. 15.5 7. Determine the kinetic energy of Mr. Carlson’s golf ball with a mass of .55 kg as it rolls down the fairway with a velocity of 9.3 m/s: A. 23.8 J B. 24. J C. 2.6 J D. 2.56 J 8. Calculate the mass of a substance with a volume of 30. mL and a density of 5.00 g/mL : A. 150 g B. 6.0 g C. 1.5 X 102 D. 1.5 X 103 9. The chemical names for these elements, respectively, Li, C, and F are: A. Lithium, Calcium, Fluorine B. Lithium, Carbon, Fluorine C. Lead, Carbon, Fluorine D. Carbon, Lithium, Fluorine 10. These elements are in Group 2: A. Barium and Hydrogen B. Lithium and Barium C. Beryllium and Magnesium D. Sodium and Magnesium 11. These elements are Alkali metals: A. Hydrogen and Lithium B. Beryllium and Magnesium C. Lithium and Beryllium D. Potassium and Rubidium 12. The chemical symbol for Sodium is: A. S B. So C. Na D. N 13. Which one of these theories was a flaw in Dalton’s model of the atom: A. Atoms of different elements have different physical and chemical properties B. Atoms of different elements combine in simple, whole number ratios to form chemical compounds C. All matter is made of indivisible and indestructible atoms D. None of these were flaws. 14. The flaw that existed in Thomson’s plum pudding model of the atom was that: A. Atoms cannot be subdivided or combined B. A ball of positive charge with electrons in it. C. A ball of negative charge with protons in it D. Too much pudding, not enough plums. 15. The element Oxygen has how many protons, electrons, and neutrons, respectively: A. 8,16,8 B. 8,8,8 C. 16,16,8 D. 8,8,16 16. The atomic mass of Boron, using 3 significant figures, is: A. 11 B. 11.0 C. 10.8 D. 10.9 17. The electron configuration for Magnesium is: A . 1s22s22p6 B. 1s22s23s22p6 C. 1s22s22p63s2 D. 1s22s42p6 18. The orbital diagram for Lithium is: A. B. C. D. 2s 2s 1s 1s 1s 2s 1s 3s 19. The three quantum numbers for Sodium are : A. n=2, l=s, ms= +/- ½ B. n=3, l=s, ms= +/- ½ C. n=3, l=p, ms= +/- ½ D. n=1, l=s, ms= +/- ½ 20. Determine the number of neutrons for 157 N: A. 7 B. 8 C. 9 D. 15 21. The alkaline-earth metals are found in Group: A. 1 B. 2 C. 13 D. 14 22. The main-block elements are Group 1 and 2 and Groups: A. 13-18 B. 14-18 C. 13-17 D. 3-18 23. Which group is stable and unreactive? : A. Halogens B. Alkali metals C. Noble gases D. Metalloids 24. Which group has a single electron in the highest energy level?: A. Alkali metals B. Alkaline-earth metals C. Halogens D. Noble gases 25. Which element reacts more readily with chlorine: A. Sodium B. Fluorine C. Magnesium D. Calcium 26. The group that has the most negative electron affinity is the: A. Halogens B. Noble gases C. Alkali metals D. Pink Floyd 27. The most electronegative group is the : A. Noble gases B. Halogens C. Alkali metals D. Hydrogen 28. This element has the highest ionization energy: A. Lithium B. Sodium C. Potassium D. Cesium 29. What is the mass in grams of 5.20 X 1010 mol of uranium. The molar mass of uranium is 238 g: A. 2.10 X 108 g B. 1.238 X 1013 g C. 2.184 X 108 g D. 1.24 X 1013 g 30. Calculate the number of atoms in 10.0g of sulfur: A. 5.31 X 10-22 atoms B. 5.91 X 10-22 atoms C. 1.88 X 1023 atoms D. 1.88 X 1023 grams 31. Calculate the number of atoms in 54.0g of Magnesium: A. 1.34 X 1024 atoms B. 5.91 X 1023 atoms C. 2.10 X 10-21 atoms D. 1.45 X 1023 atoms 32. The formula for aluminum fluoride is : A. AlF2 B. AlF C. AlF3 D. Al2F3 33. The formula for ammonium hydroxide is: A. NH3O B. NH3 H2O C. NH4OH D. NH4HO 34. The formula for copper (II) phosphate is: A. Cu2(PO4)2 B. Cu2P3 C. Cu3(PO4)2 D. Cu3P2 35. The name for this compound is, (NH4)2SO4 : A. Ammonia sulfate B. Ammonium sulfite C. Ammonia sulfate D. Ammonium sulfate 36. The molar mass of zinc (II) carbonate is: A. 159 g/mol B. 175 g/mol C. 109 g/mol D. 125 g/mol 37. The molar mass of ZnS is 97.5 g/mol. The molar mass of SO2 is 64.1 g/mol. The percentage of sulfur in SO2 is : A. 25 % B. 50 % C. 75 % D. 33 % 38. Aluminum chlorohydrate is an ingredient used in some antiperspirants. In its anhydrous form, it has 30.93 % Al, 45.86 % O, 20.32 % Cl, and 2.89 % H. What is the empirical formula for aluminum chlorohydrate: A. Al3H6ClO2 B. AlHClO3 C. Al2H5ClO5 D. Al5H3Cl2O2 39. The C-H bond in polyethylene is: A. Ionic B. Polar covalent C. Nonpolar covalent D. Dipole force 40. The oxidation number for oxygen is Fe2O3 is: A. +2 B. –3 C. +3 D. –2 41. The name for the following compound NO, is: A. Nitrogen monoxide B. Nitrogen dioxide C. Nitrogen oxide D. Nitrous oxide 42. The shape of a compound that has a central carbon atom with double bonds to two sulfur atoms is: A. Tetrahedral B. Trigonal planar C. Linear D. Bent 43. What is the molecular formula of paradichlorobenzene, an ingredient in moth balls that has a molar mass of 147.00 g/mol and an empirical formula of C3ClH2?: A. C3ClH2 B. C9Cl3H6 C. C6Cl2H4 D. C1.5Cl.5H1 44. Put the following word equation into a balanced formula equation: nitrogen dioxide + water nitric acid + nitrogen monoxide A. NO2 + H2O 2HNO3 + NO B. 2NO2 + H2O HNO3 + 3NO C. 3NO2 + H2O 3NO3 + NO D. 3NO2 + H2O 2HNO3 + NO 45. Balance the following equation: CaH2 (s) + H2 (l) Ca(OH)2 (aq) + H2 (g) A. 1:2:1:1 B. 1:1:2:1 C. 1:2:1:2 D. 2:1:2:1 46. Al2O3 + 3H2SO4 Al2(SO4)3 + 3H2O. How many moles of Al2(SO4)3 would would be produced if 6 mol of H2SO4 reacted with an excess of Al2O3? A. 3 B. 1 C. 6 D. 2 47. The balanced chemical equation for the synthesis of the pollutant nitrogen dioxide from nitrogen monoxide and oxygen gas is: A. 6NO2 6NO + 3O2 B. 2NO2 + O2 2NO C. 3NO NO2 + O2 D. 2NO + O2 2NO2 48. Mass-Mass If 0.500g of sulfur dioxide from pollutants reacts with excess water and oxygen found in the air, how many grams of sulfuric acid are produced? 2H2O + O2 + 2SO2 2H2SO4 A. .382 grams B. 1.53 grams C. .765 grams D. .510 grams 49. The two compounds being compared in #48 are: A. O2 and H2SO4 B. SO2 and H2SO4 C. H2O and H2SO4 D. O2 and SO2 50. The last step in determining how many grams of sulfuric acid are produced is: A. 2mol H2SO4 B. 2mol SO2 C. 98.09g H2SO4 D. 82.09 g H2SO4 2mol SO2 2mol H2SO4 1mol H2SO4 1mol H2SO4 51. Mole-Mass 2KClO3 2KCl + 3O2 If I have 4.0 moles of KClO3, how many grams of O2 do I have?: A. 1.62 X 102 g B. 1.9 X 102 g C. 4.7 X 103 g D. 5.7 X 105 g 52. For #51, I have 4.0 moles of KClO3, how many moles of O2 do I have?: A. 4.0 B. 3.0 C. 8.0 D. 6.0 53. Density 4NH3 + 5O2 4NO + 6H2O ; Ammonia gas= 25.0 mol ; Density of NO = 1.340 g/L ; How many moles of NO will be produced if I have an excess of O2?: A. 6 mol B. 6.25 mol C. 25.0 mol D. 100. mol 54. How many grams of NO will be produced if I have an excess of O2?: A. 750.g B. 180. g C. 25.0 mol D. 100. mol 55. How many liters of NO will be produced?: A. 134. L B. 140. L C. 2.24 X 103 L C. 600. L 56. Limiting Reactant O H O OH + H3C-OH + H2O O Butanoic acid Methanol Methyl butanoate Water What is the chemical formula for butanoic acid?: A. C3H5O2 B. C3H7O2 C. C4H6O2 D. C4H8O2 57. If 50.0 g of butanoic acid react with 40.0g of methanol, then which compound is limiting reactant? : A. Methyl butanoate B. Methanol C. Butanoic acid D. Water 58. Refer to #57. How many grams of Methyl butanoate can be produced?: A. 81.3 g B. 57.9 g C. 103. g D. 21.4 g 59. Percent Yield MgCl2 Mg + Cl2 ; If I have 50.0g of MgCl2, and I produce 30.0g of Cl2, what is my percent yield? A. 52% B. 33% C. 60% D. 80% 60. 2C + 2H2O CH4 + CO2 ; If this reaction has a percent yield of 85.0%, how much methane can be obtained from 1250g of carbon?: A. 620.g B. 546.g C. 233.g D. 710.g EXTRA CREDIT (Put work and answer on the answer sheet) +5 E.C. points 61. Plaster of Paris, CaSO4 ½ H2O, has many uses, including castings and dental cement. It can be obtained by heating gypsum CaSO4 2H2O. How many liters of water vapor evolve when 5.00L of gypsum are heated at 110C to produce plaster of Paris? At 110C the density of CaSO4 2H2O is 2.32 g/mL, and the density of water Vapor is 0.581 g/L. CaSO4 2H2O CaSO4 ½ H2O + 3H2O 1.______ 2.______ 3.______ 4.______ 5.______ 6.______ 7.______ 8.______ 9.______ 10._____ 11._____ 12._____ 13._____ 14._____ 15._____ 16._____ 17._____ 18._____ 19._____ 20._____ 21._____ 22._____ 23._____ 24._____ 25._____ 26._____ 27._____ 28._____ 29._____ 30._____ 31._____ 32._____ 33._____ 34._____ 35._____ 36._____ 37._____ 38._____ 39._____ 40._____ 41._____ 42._____ 43._____ 44._____ 45._____ 46._____ 47._______ 48._______ 49._______ 50._______ 51._______ 52._______ 53._______ 54._______ 55._______ 56._______ 57._______ 58._______ 59._______ 60._______ 61. Show Work