Academic Chemistry Fall 2016 Semester Practice Test (Clarke, Eller, Hessel, and White)
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1 Name: Academic Chemistry Fall 2016 Semester Practice Test (Clarke, Eller, Hessel, and White) Period: Test Format: 100 multiple choice questions at 1 point each I. MEASUREMENT AND CALCULATION 1. List the metric system prefixes, abbreviations, and meanings for kilo- through milli-. Give the appropriate metric unit for making the following 5 measurements: 2. Mass of a German Shepherd 5. Volume of a bathtub 3. Length of your arm 6. Distance from Houston to Austin 4. Volume of a liquid medicine dispenser 7. Convert ml to liters. 8. Convert the mass of a cat from 4500 g to kg. 9. How many dm in 14.5 mm? 10. What is the formula for density? 11. What is the density of an object with a mass of 5.72 g and a volume of 8.6 ml? 12. What is the volume of a necklace if the density is 21.9 g/ml and the mass is 0.99 g? 13. If a metal peg has a density of 18.2 g/ml and it is cut in half and then in half again, what is the density of the smallest remaining piece of the peg? 14. How can you experimentally determine the density of an irregularly shaped object, like a rock? 15. Define accuracy and precision as related to scientific measurement. Accuracy: Precision: 16. The true volume of a liquid is 45.5 ml. The volume is experimentally measured three times, with the following results: 35.5 ml, 35.6 ml, and 35.5 ml. Are these results accurate, precise, both, or neither? Determine how many significant figures are in the following examples: x
2 For the following 4 questions, calculate and round the answer to the correct number of sig figs: g + 13 g g + 9 g =? ml ml ml ml =? g / 4 ml =? cm x 3.5 cm x 8.5 cm =? 26. Convert to scientific notation: a b Convert to regular (standard) notation: a x 10-3 b x 10 2 c d c x 10-6 d. 7.2 x 105 Use the following conversion factors to solve the next 6 calculations BY DIMENSIONAL ANALYSIS: 1 mile = 5280 feet 1 gallon = 4 quarts 1 hour = 60 min 1 kg = lbs 1 mile = km 1 quart = 2 pints 1 min = 60 s 1 lb = 16 oz 1 inch = 2.54 cm 1 pint = 2 cups 1 cup = 16 T 1 T = 3 t 28. How many quarts are in 10. gallons? 29. How many teaspoons (t) are in 8 cups? 30. How many kilometers are in inches? 31. How many ounces are in 50 kilograms? 32. How many miles are in 10. kilometers? 33. How many seconds are in 1.56 days? II. MATTER AND CHANGE 34. Contrast the 3 states of matter in terms of shape and volume (definite or indefinite?) 35. Contrast the 3 states of matter in terms of how closely packed the particles are. 36. What are the two major types of mixtures? Define each (tell how you recognize them). Give 2 examples of each. 2
3 37. What are the two types of pure substances? Define each and give 2 examples of each. 38. How can a mixture of salt and water be separated? Can a compound be separated? How? Can an element be separated? 39. Consider the following equation: CH4 + 2 O2 CO2 + 2 H2O If the mass of the reactants is 80 g, and the mass of the CO2 is 44 g, what is the mass of the water? What law does this illustrate? 40. What is the difference between a chemical property and a physical property? 41. What are the five signs of a chemical reaction? 42. What is an intensive property? An extensive property? 43. How can exothermic and endothermic reactions be identified? Determine whether each of the following is a physical (P) or chemical (C) change: 44. iron rusting 47. a leaf changing color in the fall 45. wood burning 48. meat rotting 46. punching holes in a piece of paper 49. water freezing Determine whether each of the following is an intensive or extensive property: 50. Mass 52. Temperature 51. Density 53. Color Determine which type of thermal energy transfer is occurring in each of the following (convection, conduction, radiation): 54. A flask on a hot plate becomes warm after the hot plate is turned on. 55. Hot steam from the shower warms the air in the bathroom. 56. Sunlight travels through space to the earth. *Know the different forms of energy (kinetic, potential, chemical, thermal, electrical, radiant, & nuclear) and how they can be transferred from one to the other. III. ATOMIC STRUCTURE/ NUCLEAR CHEMISTRY 57. What is the definition of an atom? 58. How does Dalton's atomic theory help to explain the Law of Conservation of Mass? 59. Explain Rutherford s gold foil experiment. What did Rutherford discover about the structure of the atom? 3
4 60. Where are each of subatomic particles located in the atom? What is the charge on each particle? 61. Why is an atom electrically neutral? 62. How do isotopes of an element differ? 63. Define: atomic number: mass number: atomic mass: 64. Calculate the number of protons, neutrons and electrons in the following isotopes: a. Oxygen-18 c. Tellurium-128 b. Cadmium-112 d. Neon An element is defined by the number of it has, also known as the. 66. Find the average atomic mass for oxygen, which has 3 isotopes: oxygen-16 (mass amu and 99.8%), oxygen-17 (mass amu and 0.04%), and oxygen-18 (mass amu and 0.2%). 67. Where are the following located on the periodic table? a. metals b. metalloids c. nonmetals 68. Classify the following elements as metal (M), nonmetal (NM), or metalloid (MD): carbon hydrogen tin germanium iron potassium silicon boron 69. What are cations? anions? Which one is formed from metals? From nonmetals? 70. Give the charge for the following ions: sodium ion chloride ion nitrate ion phosphate ion ammonium ion oxide ion sulfate ion 71. Write the complete reaction for the following radioactive decay processes: 96 6 Alpha: 42 Mo 3 Li Md Beta: U Pa Ac 72. Define half-life: **Know the characteristics of alpha, beta, and gamma radiation. ***Know the definitions and characteristics of fission and fusion, and examples of each. 4
5 IV. NOMENCLATURE 73. How can ionic compounds be recognized? What type of bond do they have? 74. Which type of ion comes first in an ionic compound formula? 75. How can molecular compounds be recognized? What type of bond do they have? 76. The elements of which group/family do not typically form bonds? Why not? Classify each of the following as ionic (I), molecular (M), acid (A), or base (B): 77. Na2S 80. KOH 78. H2CO3 81. (NH4)3PO4 79. P4O10 Ionic Compounds: write the name. 82. Na2O 83. Cu3PO4 84. Sn(CO3)2 Molecular Compounds: write the name. 85. As2S3 86. XeF4 Acids: write the name. 87. HBr 88. HC2H3O2 Ionic Compounds: write the formula. 89. aluminum chlorate 90. iron (III) nitrate Molecular Compounds: write the formula. 91. phosphorus pentachloride 92. dichlorine heptoxide Acids: write the formula. 93. hydrofluoric acid 94. nitric acid V. CHEMICAL QUANTITIES (MOLES, EMP/MOLEC FORMULAS, % COMP) 95. Find the molar mass for K2SO Find the molar mass for Ca3(PO4) Find the molar mass for NH4NO Convert 65.4 mol Na3PO4 to molecules. 99. Convert 1.23 moles KCl to grams Convert 5.97 grams BF3 to molecules. 5
6 101. Convert 9.5 L CO2 gas (at STP) to grams Calculate the percent composition of phosphorus in AlPO Determine the mass of aluminum in a 150. g sample of AlPO Determine the empirical formula for a compound containing 40.0% C, 6.7% H, and 53.3% O The empirical formula for vitamin C is C3H4O3. Experimental data indicates that the molar mass of vitamin C is g/mol. What is the molecular formula of vitamin C? VI. ELECTRONS IN ATOMS Given information: c = λ f c = speed of light = 3.00 x 10 8 m/s E = h f h = Planck s constant = x J. s 106. What is the frequency of radiation with a wavelength of 3.82 x 10-7 m? 107. Gamma rays have frequencies around 1.0 x Hz. What wavelength does this correspond to? 108. It takes 6.63 x J of energy to eject an electron from a certain atom. What frequency of light is this? 109. List the number of orbitals contained in the following sublevels: a. s b. p c. d d. f 110. How many electrons can occupy the following sublevels? a. s b. p c. d d. f 111. Write electron configurations and orbital (arrow) diagrams for these elements: a. B c. Ne b. N d. K 112. Identify the element with electron configuration 1s 2 2s 2 2p 6 3s 2 3p Define valence electrons: Explain how you would find the valence electrons for an element and give an example. 6
7 114. Draw electron dot diagrams for: a. Ca b. O c. Ar d. P 115. Write the electron configuration for both a sodium atom and a sodium ion (charge?) Write the electron configuration for both an oxygen atom and an oxide ion (charge?) Draw a diagram using dots and arrows to show the compound that forms when sodium and oxygen react. VII. THE PERIODIC TABLE 118. Who is credited with developing the first periodic table? 119. Mendeleev s periodic table was arranged in order of increasing atomic Discuss the power of Mendeleev s periodic table; what was he able to predict? 121. Mosely made an adjustment to Mendeleev s table by realizing that the elements are arrange in order of increasing atomic Why is Mendeleev's table called periodic? 123. What can be said about the properties of elements in the same group or column in the periodic table? 124. Where are the following families found on the periodic table? (list their group #): a. alkali metals b. alkaline earth metals c. halogens d. noble gases 125. Where are the transition metals on the periodic table? In what block are they found? 126. Where are the lanthanides and actinides on the periodic table? In what block are they found? 127. Define atomic radius: 128. How does atomic radius change? a. going down a group: b. across a period left to right: 7
8 129. Define ionization energy: 130. How does ionization energy change? a. going down a group: b. across a period left to right: 131. Define electronegativity: 132. How does electronegativity change? a. going down a group: b. across a period left to right: c. Considering this information, what is the most electronegative element on the periodic table? (Do not consider noble gases, because they generally do not participate in bonding) 133. On what side of the Periodic Table do elements have more: a. metallic character? b. nonmetallic character? 134. What type of element tends to: a. gain electrons to become stable? b. lose electrons to become stable? 8
1 mile = 5280 feet 1 gallon = 4 quarts 1 hour = 60 min 1 kg = lbs. 1 mile = km 1 quart = 2 pints 1 min = 60 s 1 lb = 16 oz
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