CHM‐100 CHEMISTRY MAN & ENVIRONMENT Comprehensive – Sample Final Exam Multiple Choice: Identify the choice that best completes the statement or answers the question. 1. Which is the correct SI unit for mass? a. gram b. pound c. ounce d. kilogram e. ton 2. Which of these acids is responsible for the sourness in many fruits? a. muriatic b. citric c. sulfuric d. acetic e. benzoic 3. Which of the following is true for a hydrocarbon? a. It consists of carbon and hydrogen atoms.
b. It can form a ring structure. c. It is a good fuel for combustion reactions.
d. It can contain double or triple bonds.
e. All of the above. 4. Which of these is the most likely identity of element A in the Lewis dot structure? ____ ____ ____ ____ a. Ca b. Li c. Al d. Cs e. P 5. Calculate the mass in grams of a 1.07 moles of acetylene, C2H2. a. 0.0243 grams b. 0.044 grams c. 14.98 grams d. 25.68 grams e. 27.82 grams 6. How many lone pairs of electrons are around the central atom in CH4? a. 0 b. 1 c. 2 d. 3 e. 4 7. Which of these acids is found in stomach acid? a. malic b. hydrochloric c. phosphoric ____ ____ ____ d. acetic e. lactic What is the charge on an ion that contains 16 protons and 18 electrons? a. 0 b. +2 c. ‐2 d. It depends on the number of neutrons.
e. None of these. Which of these is not a subfamily of the hydrocarbon family? a. alkenes b. alkynes c. alkanes d. All of these are correct. e. A and B are not correct. A 5% acetic acid solution contains ____ grams of acetic acid per ____ grams of solution. a. 5, 10 b. 95, 100 c. 100, 500 d. 5, 500 e. 50, 1000 Which of these is the correct name for N 2O3? a. nitrogen trioxide b. trinitrogen dioxide c. dinitrogen trioxide d. nitrogen dioxygenide e. dinitrogenide dioxygenide What is the concentration in molarity of a solution made by dissolving 20 grams of KOH in 150 mL of H2O? a. 0.133 M b. 0.421 M c. 2.37 M d. 4.35 M e. 7.5 M A statement which summarizes the data obtained from a series of observations is known as a(n) ____. a. observation b. law c. theory d. conclusion e. experiment Which of these is the correct Lewis dot structure for chlorine? a. ____ 8. ____ 9. ____ 10. ____ 11. ____ 12. ____ 13. ____ 14. b. c. d. e. ____ 15. Which of these is the correct chemical symbol for potassium? a. K b. Po c. P d. Pd e. Pt 16. Attractions between molecules which hold liquids together are known as ____. a. density b. adhesive forces c. cohesive forces d. pressure e. attractive forces 17. Determine the correct number of protons and electrons in P3‐ ? a. 3 protons, 6 electrons b. 15 protons, 18 electrons c. 15 protons, 12 electrons d. 31 protons, 28 electrons e. 31 protons, 34 electrons 18. Which of these is the correct condensed structural formula for pentane? a. CH3CH2CH3 b. CH3CH2CH2CH3 c. CH3CH2=CH2CH3 d. CH3CH2HC=CHCH3 e. CH3CH2CH2CH2CH3 19. Which of these substances is a base? a. NaHCO3 b. HCl c. HNO3 d. H3PO4 e. CH3COOH 20. Which of these gases combine with water to form acid rain? I. SO2 II. NO2 III. H2 IV. N2 V. Cl2 a. I only b. II only c. I and II d. I and IV e. I, III and V 21. Which of these represents the SI prefix for centi (c)? a. 10‐6 b. 10‐3 c. 10‐1 d. 10‐2 e. 106 ____ ____ ____ ____ ____ ____ ____ 22. Convert 4.5 inches to meters. (2.54 cm = 1 inch) a. 0.1143 m b. 1.77 m c. 11.43 m d. 0.0177 m e. 1143 m 23. The long jump record is 8.90 m. What is the length in inches? (1 m = 39.37 inches) a. 9.73 inches b. 293 inches c. 350 inches d. 4204 inches e. 5000 inches 24. Identify the third‐row element X which forms the compound ____ ____ a. S b. Cl c. P d. Si e. Al 25. Which of these substances are heterogeneous mixtures? I. steam II. milk of magnesia III. crude oil IV. rubbing alcohol a. II and III b. I and IV c. II, III and IV d. I, III and IV e. I, II, and III 26. Which of these is the correct name for the structural formula? ____ ____ a. b. c. d. ethane butane propane hexane e. methane 27. A 4.5 L sample of sea water contains 32.7 mg of strontium. Determine the concentration of strontium in mg/L. a. 0.138 mg/L b. 7.27 mg/L c. 28.2 mg/L d. 32.7 mg/L e. 37.2 mg/L 28. Carbon and oxygen react to form carbon dioxide. What mass of carbon dioxide is produced when 12.0 g of carbon react with 32.0 g of oxygen? a. 44 g b. 38 g c. 28 g d. 20 g e. 2.67 g 29. Which of these has the greatest [H3O+]? a. pH = 2 b. pH = 5 c. pH = 7 d. pH = 11 e. pH = 13 30. The number of protons in a neutral atom is equal to the ____ of the atom. a. mass b. atomic weight c. atomic number d. mass number e. valence electron number 31. How many kilograms of calcium are there in 173 pounds of calcium? (1 pound = 454 grams) a. 1.1 kg b. 78.54 kg c. 1.1 102 kg d. 3.8 104 kg e. 7.85 104 kg 32. Which of these is the correct name for the structural formula? ____ ____ ____ ____ ____ ____ a. ethane b. butane c. heptane d. hexane e. methane 33. Which of these substances would have the strongest cohesive forces in combination with the greatest molecular mobility? ____ a. H2O(l) b. CH4(g) c. KCl(s) d. O2(g) e. Au(s) 34. Which of these alkanes would be gases at room temperature? I. C2H6 II. C3H8 III. C5H10 IV. C6H14 V. CH4 a. I and II b. I, II and III c. III and IV d. I, II and V e. I and V 35. Which of these is the most likely identity of element A in the Lewis dot structure? ____ ____ a. Ca b. K c. Al d. C e. P How many lone pairs of electrons are around the central atom in PCl3? a. 0 b. 1 c. 2 d. 3 e. 20 How many moles of calcium atoms are 2.5 moles of calcium carbonate, CaCO3? a. 1 mole b. 1.25 moles c. 2.5 moles d. 5.0 moles e. 100 moles Which of these statements about alkanes is not correct? a. Alkanes are nonpolar. b. Alkanes are nonflammable. c. Carbon must always form four bonds.
d. Alkanes have a general formula CnH2n +2.
e. Interior carbons will always be bound to two other carbons.
Which of these is an ionic compound? a. AlCl3 b. H2O c. SiO2 d. IBr e. S8 ____ 36. ____ 37. ____ 38. ____ 39. ____ 40. Arrange CH4, Cl2, and CO2 in order of increasing strength of dispersion forces. (least to the greatest) a. CH4< CO2< Cl2 b. Cl2< CO2 <CH4 c. CH4< Cl2< CO2 d. Cl2<CH4< CO2 e. CO2 < Cl2<CH4 41. Which of these alkanes would be liquids at room temperature? I. C2H6 II. C3H8 III. C5H10 IV. C6H14 V. CH4 a. I and II b. I, II and III c. III and IV d. I, II and V e. I and V 42. How many protons, neutrons and electrons are in an 25Mg+2 ion? a. 12 protons, 12 electrons, 13 neutrons
b. 12 protons, 10 electrons, 12 neutrons
c. 13 protons, 10 electrons, 12 neutrons
d. 12 protons, 10 electrons, 13 neutrons
e. 12 protons, 14 electrons, 13 neutrons
43. Which of these is not an alkane? a. C2H6 b. C3H8 c. C5H10 d. C6H14 e. CH4 44. Determine the mass in grams of a gold sample which occupies a volume of 16.39 mL? Gold has a density of 19.3 g/mL. a. 0.118 g b. 0.316 g c. 0.849 g d. 1.18 g e. 316 g 45. What is the molecular weight of PCl3? a. 66.5 amu b. 106.5 amu c. 137.5 amu d. 180 amu e. 360 amu 46. Mendeleev organized the elements of the periodic table: a. by increasing atomic number and similar properties.
b. by increasing atomic weight and similar properties.
c. by increasing number of electrons.
d. by increasing number of isotopes.
e. alphabetically. ____ ____ ____ ____ ____ ____ ____ 47. Which of these is a nonmetal? a. Mg b. Br c. Cu d. Ge e. Li 48. Which substance has the highest boiling point? a. Ne b. Kr c. He d. Xe e. Ar 49. If 15.0 mL of a metal has a mass of 103.0 g, what is the density of the metal? a. 6.87 g/mL b. 1550 g/mL c. 0.146 g/mL d. 1.46 g/mL e. none of these 50. Which of these statements about atoms is incorrect? a. Atoms are the smallest visible amount of an element.
b. Atoms are composed of protons, neutrons, and electrons.
c. Atoms are the building blocks of all matter.
d. Atoms are the smallest identifiable unit of an element.
e. There are 90 different naturally occurring atoms.
51. Covalent bonds are formed when electrons are ____. a. transferred b. split c. shared d. destroyed e. heated 52. Which of these is the best definition of matter? a. The pull of gravity on an object.
b. Anything that has weight and volume.
c. Anything that has mass and occupies space.
d. Anything that is directly proportional to weight.
e. The measure of the amount of space an object occupies.
53. Which of these numbers has the most significant figures? a. 0.5071 b. 0.201 c. 6.02 1023 d. 51 e. 103 54. Which substance has the lowest boiling point? a. Br2 b. F2 c. I2 d. Cl2 e. D and C 55. Which is the correct SI unit for length? a. meter b. feet c. mile ____ ____ ____ ____ ____ ____ ____ ____ d. kilometer e. centimeter 56. Which of these is the Bronsted‐Lowry base in this chemical equation? ____ a. HSO4‐ b. H2O c. S d. OH‐ e. NH3 A ____ is an explanation of a scientific observation. a. law b. theory c. conclusion d. prediction e. epiphany A substance composed of two or more different elements in fixed proportions is known as a(n) ____. a. atom b. element c. molecule d. ion e. compound Which of these is not a covalent compound? a. SiO2 b. CH4 c. N2O d. CaO e. ICl3 What is the coefficient in front of sodium nitride when the equation is balanced? __ Na3N __ Na(s) + __ N2(g) a. 0 b. 1 c. 2 d. 3 e. 4 Which of these is the correct name for the structure below? ____ 57. ____ 58. ____ 59. ____ 60. ____ 61. a. b. c. d. e. butenol isobutanol 2‐methyl‐1‐propanol isopropanol both C and D are correct ____ 62. How many total valence electrons are there in the Lewis structure of NO3‐1? a. 32 b. 30 c. 20 d. 22 e. none of these 63. Which of these is not a method for measuring the concentration of a solution? a. percent by mass b. percent by volume c. pressure per volume d. parts per million e. molarity 64. Drinking water contains 175 ppm of dissolved CaCO3 per liter. How many grams of CaCO3 are in 2.0 L of water? a. 0.0035 g b. 0.0175 g c. 0.035 g d. 0.175 g e. 0.350 g 65. Which of these substances is a compound? a. air b. salt water c. gasoline d. salt e. lemonade 66. Which of these substances would you expect to have the lowest boiling point? a. diamond b. graphite(pencil lead) c. water d. gasoline e. lead 67. Which of these statements best explains the designation "organic"? a. Any naturally occurring substance.
b. Any substance which contains carbon.
c. Any substance which contains ionic bonds.
d. Any substance which is formed by synthetic means.
e. A substance which must be formed as a result of vitalism.
68. Which of these is the best definition of a Bronsted‐Lowry acid? a. Any substance that donates H+ ions in solution.
b. Any substance that produces OH‐ ions in solution.
c. Any substance that accepts a lone pair of electrons.
d. Any substance that neutralizes a base in solution.
e. Any substance that accepts H+ ion in solution.
69. Which of these particles has a negative charge? a. proton b. neutron c. electron d. nucleus e. an atom 70. Determine the volume occupied by a 1.5 g sample of ethyl alcohol. The density of ethyl alcohol is 0.7893 g/mL. a. 1.9 mL ____ ____ ____ ____ ____ ____ ____ ____ b. 1.3 mL c. 0.53 mL d. 0.526 mL e. 1.331 mL What is the molecular geometry of NH 3? a. tetrahedral b. bent c. pyramidal d. trigonal planar e. linear Ionic bonds are formed when electrons are ____. a. transferred b. split c. shared d. destroyed e. heated The simplest form of substance is known as a(n) ____. a. element b. ion c. mixture d. nucleus e. homogeneous What is the coefficient in front of oxygen (O2) when the equation is balanced? __ C3H8 + __ O2 __ CO2 + __ H2O a. 2 b. 3 c. 4 d. 5 e. 10 Which of these is/are properties of acids? I. sour II. turn litmus blue III. dissolve some metals IV. slippery a. I only b. III only c. I and II d. I and III e. II, III and IV Which of these elements is a metal? a. Mg b. Br c. Ar d. Ge e. B What is the correct name of K2O? a. dipotassium monoxide b. dipotassium oxide ____ 71. ____ 72. ____ 73. ____ 74. ____ 75. ____ 76. ____ 77. c. potassium monoxide d. potassium oxygen e. potassium oxide Which of these elements has the highest electronegativity? a. Ca b. N c. Se d. P e. O Which of these is the correct name for CH 3CH2HC=CHCH3? a. pentene b. pentyne c. hexene d. hexyne e. butadiene The point at which a liquid is converted to a gas is known as the ____. a. boiling point b. melting point c. sublimation point d. deposition point e. freezing point Which of these is the correct name for Ca(OH)2? a. calcium carbonate b. calcium oxide c. calcium dihydride d. calcium oxygen hydride e. calcium hydroxide Which of these acids is also called muriatic acid? a. H2SO4 b. HCl c. HNO3 d. NaOH e. CH3COOH Which of the following is not true for 3 moles of CaCO3? a. It contains 3 moles of O. b. It contains 3 moles of Ca. c. It contains 3 moles of C. d. It contains 9 moles of O. e. None of the above. Which is the correct SI unit for time? a. meter b. hour c. second d. minute e. gram Which of these describes the process by which a liquid molecule at the surface of a liquid escapes to the gas phase? a. melting b. sublimation c. evaporation d. deposition e. condensation ____ 78. ____ 79. ____ 80. ____ 81. ____ 82. ____ 83. ____ 84. ____ 85. ____ 86. The stronger the cohesive forces in a substance a. the higher the boiling point and the melting point.
b. the lower the boiling point and higher the melting point.
c. the lower the boiling point and the melting point.
d. the higher the boiling point the lower the melting point.
e. Boiling and melting point are independent of forces.
87. Which of these substances is an ionic compound? I. NCl3 II. MgF2 III. AlBr3 IV. CH4 a. I and II b. II and III c. II and IV d. II, III and IV e. II only 88. Which of these statements is correct? a. The amount of carbon on earth is essentially constant.
b. The amount of carbon on earth fluctuates with the seasons.
c. The amount of carbon on earth is increasing due to plant and animal growth. d. The amount of carbon on earth is decreasing due to consumption of carbon based fuels. e. Both B and C are correct. 89. Which of these are pure substances? I. steam II. crude oil III. salt water IV. gun powder V. oxygen VI. mercury a. I, II and III b. I and III c. I, II, III and V d. I, III and V e. I, V, and VI 90. Which of these is the correct chemical symbol for carbon? a. C b. Ca c. Cl d. Cb e. Co 91. When properly balanced, what are the correct coefficients for the reaction. H2 + O2 H20 ? a. 1,1,1 b. 1,1/2,1 c. 1,2,1 d. 2,1,2 ____ ____ ____ ____ ____ e. 10,5,10 92. An element has two naturally occurring isotopes. One has an abundance of 37.4% and an isotopic mass of 184.953 amu. The other has an abundance of 62.6% and a mass of 186.956 amu. What is the atomic weight of the element? a. 185.702 amu b. 185.954 amu c. 186.207 amu d. 186.956 amu e. 190.234 amu 93. How many bonding pairs of electrons are around the central atom in CO2? a. 0 b. 1 c. 2 d. 3 e. 4 94. Based on Rutherford's model of the atom, how many electrons would be found in an atom with 7 protons? a. 1 b. 2 c. 4 d. 7 e. 14 95. Which of these statements best explains the Law of Conservation of Mass? a. All atoms of a given element have the same weight.
b. Atoms of different elements combine in fixed whole number ratios.
c. The weight of an object is neither created nor destroyed in a chemical reaction. d. All samples of a given compound have the same proportion of constituent elements.
e. The sum of the masses of the reactants equals the sum of the masses of the products in a normal chemical reaction. 96. An irregular shaped piece of metal with a mass of 220 g was placed in a graduated cylinder that contained 35.00 mL of water. This raised the water level to 52.50 mL. What is the density of the metal? a. 0.285 g/mL b. 4.19 g/mL c. 17.5 g/mL d. 12.6 g/mL e. 38.5 g/mL 97. Which of these acids is a component in vinegar? a. H2SO4 b. HCl c. HNO3 d. NaOH e. CH3COOH 98. A chocolate chip cookie is an example of what type of matter? a. element b. compound c. homogeneous mixture d. heterogeneous mixture e. a cookie is not matter 99. What does the V in VSEPR theory stand for? a. very b. variable c. valence ____ ____ ____ ____ ____ ____ ____ ____ d. vanadium e. volume ____ 100. Which of these is the correct formula for aluminum oxide? a. Al2O2 b. Al2O3 c. AlO d. Al3O2 e. AlO2