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Chem 152 Dr. Saidane

Final Practice Test

1. What is the difference between a hypothesis and a scientific theory? A) A hypothesis is a tentative proposal and a theory is a tested proposal. B) A theory is a tentative proposal and a hypothesis is a tested proposal. C) A hypothesis requires an experiment and a theory does not. D) A theory requires an experiment and a hypothesis does not. E) none of the above 2. What is the term for the digits obtained from an instrumental measurement? A) certain digits B) instrumental digits C) nonsignificant digits D) significant digits E) none of the above 3. What is the term for the inexactness of an instrumental measurement? A) accuracy B) error C) precision D) uncertainty E) none of the above 4. Which of the following metric rulers has the least uncertainty? A) Ruler A, ± 1 cm B) Ruler B, ± 0.1 cm C) Ruler C, ± 0.5 cm D) Ruler D, ± 0.05 cm E) Ruler E, ± 5 cm 5. How many significant digits are in the length measurement 100.60 centimeters? A) 1 B) 2 C) 3 D) 4 E) none of the above 6. Round off the following measurement to three significant digits: 19.945 g. A) 19.0 g B) 19.9 g C) 19.950 g D) 19.945 g E) 20.0 g 7. Add 7.77 g to 11.666 g and round off the answer. A) 19.0 g B) 19.4 g C) 19.43 g D) 19.44 g E) 19.436 g 8. A sample of rose gold is: 12.0 grams gold, 5.0 grams silver, and 7.0 grams copper by mass. What is the percent of copper in the sample? A) 12% B) 29% C) 50% D) 58% E) 75% 9. Stainless steel is composed of iron, manganese, chromium, and nickel. If a 2.00 g sample was analyzed and found to contain 2.75% manganese, what is the mass of manganese in the sample? A) 0.0138 g B) 0.0550 g C) 0.182 g D) 0.727 g E) 1.38 g 10. Which of the following is a currently accepted basic unit and symbol in the metric system? A) centimeter (cm) B) kilogram (kg) C) milliliter (mL) D) all of the above E) none of the above 11. A 10.0 cm3 volume of alcohol has a mass of 7.05 g. What is the density of the alcohol in grams per cubic centimeter? A) 0.0705 g/cm3 B) 0.705 g/cm3 C) 10.0 g/cm3 D) 70.5 g/cm3 E) 7.05 g/cm3 12. What is the term for the smallest particle that represents an element? A) atom B) entity C) formula unit D) molecule E) none of the above 13. What is the term for the number that identifies a particular element? A) atomic number B) element number C) mass number D) substance number E) none of the above 14. What is the term for a change that requires altering the composition of a substance? A) atomic change B) chemical change C) molecular change D) physical change E) none of the above 15. What is the term for the symbolic representation of a compound that indicates the number of atoms of each element in the compound? A) atomic number B) atomic notation C) chemical formula D) chemical symbol E) none of the above 16. What is the term for a pure substance that can be broken down into two or more substances by chemical reaction? A) compound B) element C) homogeneous D) matter E) none of the above 17. What is the term for a direct change of state from a gas to a solid? A) condensation B) deposition C) sublimation D) vaporization E) none of the above 18. What is the term for the property of a metal to be drawn into a wire? A) alloy B) ductile C) malleable D) tensile E) none of the above 19. What is the term for matter having an indefinite composition and variable properties? A) compound B) element C) heterogeneous mixture D) homogeneous mixture E) none of the above 20. What is the term for an element that is generally shiny, has a high density and high melting point, and is a good conductor of heat and electricity? A) metal B) nonmetal C) semimetal D) all of the above E) none of the above 21. What is the term for a particle composed of two or more nonmetal atoms? A) atom B) entity C) formula unit D) molecule E) none of the above 22. What is the term for the condition of matter existing as a solid, liquid, or gas? A) atomic state B) chemical state C) molecular state D) physical state E) none of the above 23. Which of the following describes a substance in the gaseous physical state? A) The substance has a variable shape. B) The substance has a variable volume. C) The substance compresses significantly. D) all of the above E) none of the above 24. Air contains nitrogen, oxygen, argon, and other gases. Which of the following describes air? A) compound B) element C) heterogeneous mixture D) homogeneous mixture E) none of the above 25. Refer to a periodic table and predict which of the following is a liquid nonmetal at 25°C and one atmosphere pressure. A) As B) Br C) Cl D) Hg E) Xe 26. Cyanocobalamin, C63H88CoN14O14P, is a water-soluble vitamin. What is the total number of atoms in the chemical formula? A) 6 B) 179 C) 180 D) 181 E) none of the above 27. Which of the following is not an example of a physical property? A) density B) ductility C) conductivity D) flammability E) none of the above 28. Which of the following is an example of a chemical property? A) conductivity B) malleability C) reactivity D) solubility E) none of the above 29. According to the kinetic theory, what happens to the kinetic energy and velocity of gaseous particles when the temperature decreases? A) Kinetic energy increases and velocity decreases. B) Kinetic energy decreases and velocity increases. C) Kinetic energy and velocity increase. D) Kinetic energy and velocity decrease. E) Kinetic energy and velocity remain constant. 30. Ethyl alcohol always contains 52% carbon, 13% hydrogen, and 35% oxygen by mass. What law is illustrated by this statement? A) law of conservation of mass B) law of constant composition C) law of constant percentages D) law of multiple proportions E) none of the above 31. Which of the following compounds has physical and chemical properties similar to the element sodium? A) NaCl B) NaClO3 C) Na2CO3 D) all of the above E) none of the above 32. What is the term for the weighted average mass of all the naturally occurring isotopes of an element? A) atomic notation B) atomic number C) atomic mass D) mass number E) none of the above 33. What is the term for the value which indicates the number of protons for an atom of a given element? A) atomic notation B) atomic number C) atomic mass D) mass number E) none of the above 34. What is the term for the atomic model that describes electrons circling the nucleus in an orbit of specific energy? A) Bohr atom B) Rutherford atom C) Thomson atom D) quantum mechanical atom E) none of the above 35. What is the subatomic particle having a negligible mass and a negative charge? A) electron B) neutron C) proton D) quark E) none of the above 36. What is the term for the shorthand description of the arrangement of electrons by sublevels according to increasing energy? A) atomic notation B) atomic number C) continuous spectrum D) electron configuration E) none of the above 37. What is the term for the collection of narrow bands of light that results from excited atoms of a given element releasing energy? A) continuous spectrum B) electromagnetic spectrum C) emission line spectrum D) radiant energy spectrum E) none of the above 38. What is the term for an orbit that electrons occupy at a fixed distance from the nucleus; designated 1, 2, 3, 4 ...? A) energy level B) orbital C) shell D) subshell E) none of the above 39. What is the term for an electron energy level resulting from the splitting of a main energy level; designated s, p, d, f ...? A) energy sublevel B) orbital C) shell D) subshell E) none of the above 40. What is the term for two atoms of the same element that differ by the number of neutrons in the nucleus? A) atomic mass units B) isotopes C) nucleons D) photons E) none of the above 41. What is the term for the value which indicates the total number of protons and neutrons in an atom of a given element? A) atomic notation B) atomic number C) atomic mass D) mass number E) none of the above 42. What is the subatomic particle having a mass of ~1 amu and a neutral charge? A) electron B) neutron C) proton D) quark E) none of the above 43. What is the term for the spatial region about the nucleus of an atom where there is a high probability of finding an electron with a given energy? A) electron shell B) electron subshell C) orbital D) quantum level E) none of the above 44. What is the term for the atomic model that describes the energy of an electron in terms of its probable location about the nucleus? A) Bohr atom B) nuclear atom C) planetary atom D) quantum mechanical atom E) none of the above 45. What is the term for the statement that it is impossible to precisely measure both the location and energy of a particle at the same time? A) exclusion principle B) quantum principle C) spectrum rule D) uncertainty principle E) none of the above 46. How many neutrons are in the nucleus of an atom of silver-107? A) 47 B) 60 C) 107 D) 154 E) none of the above 47. Given that the only naturally occurring isotope of aluminum is 27AI, what is its isotopic mass? A) 13.00 amu B) 13.98 amu C) 14.00 amu D) 26.98 amu E) 39.98 amu 48. Element X has two natural isotopes: X-6 (6.015 amu) and X-7 (7.016 amu). Calculate the atomic mass of element X given the abundance of X-7 is 92.5%. A) 6.09 amu B) 6.50 amu C) 6.52 amu D) 6.94 amu E) 12.5 amu 49. Boron occurs naturally as 10B and 11B. Which isotope is most abundant? A) boron-5 B) boron-6 C) boron-10 D) boron-11 E) none of the above 50. Which of the following energy-level changes for an electron is most energetic? A) 3 → 1 B) 4 → 1 C) 5 → 1 D) 6 → 1 E) All changes have the same energy. 51. How many energy sublevels are in the 3rd energy level? A) 1 B) 2 C) 3 D) 4 E) none of the above 52. What is the maximum number of electrons in a p energy sublevel? A) 2 B) 6 C) 10 D) 14 E) none of the above 53. Which electron sublevel follows the 4d sublevel according to increasing energy? A) 4s B) 4p C) 5s D) 5p E) 5d 54. What is the electron configuration for an atom of nickel? A) 1s2 2s2 2p6 3s2 3p6 3d8 B) 1s2 2s2 2p6 3s2 3p6 4s2 3d8 C) 1s2 2s2 2p6 3s2 3p6 4s2 4p8 D) 1s2 2s2 2p6 3s2 3p6 4s2 4d8 E) none of the above 55. What term best describes the shape of a p orbital? A) sphere B) dumbbell C) clover D) ellipse E) wave 56. Which of the following orbitals has a spherical shape? A) 4s B) 4px C) 4dxy D) all of the above E) none of the above 57. Which of the following orbitals is the largest in size? A) 1s B) 2s C) 3s D) 4s E) All s orbitals are the same size. 58. Which of the following orbitals is the lowest energy? A) 1s B) 2s C) 3s D) 4s E) All s orbitals are the same energy. 59. What is the term for the elements with atomic numbers 90 to 103? A) actinide series B) lanthanide series C) rare-earth elements D) transuranium elements E) none of the above 60. What is the name of the family of elements in Group IA/1? A) alkali metals B) alkaline earth metals C) halogens D) noble gases E) none of the above 61. What is the term for that portion of the atom that includes protons, neutrons, and inner electrons that are not available for bonding? A) center B) core C) nucleus D) valence E) none of the above 62. What is the term for a method of writing the electron configuration whereby all the inner electrons are represented by a noble gas symbol in brackets followed by the valence electrons? A) atomic notation B) core notation C) electron notation D) noble gas notation E) none of the above 63. What is the term for a representation of an atom and its valence electrons that shows the chemical symbol surrounded by a dot for each valence electron? A) atom dot notation B) core notation C) electron dot formula D) valence formula E) none of the above 64. What is the term for the minimum amount of energy to remove an electron from a neutral atom in the gaseous state? A) atomic energy B) electron energy C) ionization energy D) nuclear energy E) none of the above 65. What is the term for the electrons that occupy the outermost s and p sublevels of an atom? A) core electrons B) kernel electrons C) sublevel electrons D) valence electrons E) none of the above 66. Which of the following is a representative element? A) B B) Be C) Br D) all of the above E) none of the above 67. Which of the following is a transition element? A) Cu B) Ag C) Au D) all of the above E) none of the above 68. Which fourth period transition element has the highest atomic number? A) Ca B) Cd C) Kr D) Zn E) none of the above 69. Which of the following elements are fifth period semimetals? A) As and Sb B) Ge and As C) Sb and Te D) Po and At E) none of the above 70. Which of the following is an alkali metal? A) Al B) Cs C) Cu D) Mg E) none of the above 71. Which of the following is the highest atomic number actinide? A) Ce B) Lr C) Lu D) Th E) none of the above 72. Which of the following has the most metallic character? A) Na B) K C) Ca D) Fe E) Al 73. Which of the following has the largest atomic radius? A) Na B) K C) Ca D) Fe E) Al 74. Which of the following has chemical properties most similar to zinc? A) Al B) Ga C) Cd D) Ag E) Cu 75. Given the chemical formulas MgO, Al2O3, and SiO2, predict the formula for germanium oxide, Ge?O?. A) GeO B) Ge2O C) GeO2 D) Ge2O3 E) Ge3O2 76. Which energy sublevel is being filled by the elements K through Ca? A) 3d B) 4s C) 4p D) 4d E) 4f 77. What is the core notation for the electron configuration of an iodine atom? A) [Kr] B) [Kr] 5s2 4p5 C) [Kr] 5s2 4d10 5p5 D) [Kr] 5s2 4d10 5d6 E) [Xe] 78. Which element has the following electron configuration: [Ar] 4s2 3d5? A) Br B) Cl C) Kr D) Mn E) Tc 79. Predict the number of valence electrons for a Group VIA/16 element. A) 2 B) 4 C) 6 D) 8 E) 16 80. Which of the following groups of elements has the highest ionization energy? A) Group IA/1 B) Group IIA/2 C) Group IIB/12 D) Group VIIA/17 E) Group VIIIA/18 81. Which of the following elements has the lowest ionization energy? A) H B) He C) Li D) Be E) B 82. What is the predicted ionic charge for an Al ion? A) 1+ B) 1- C) 3+ D) 3- E) none of the above 83. What is the predicted ionic charge for a P ion? A) 3+ B) 3- C) 5+ D) 5- E) none of the above 84. What is the electron configuration for a magnesium ion, Mg2+? A) 1s2 2s2 2p6 B) 1s2 2s2 2p6 3s1 C) 1s2 2s2 2p6 3s2 D) 1s2 2s2 2p6 3s2 3p1 E) none of the above 85. What is the electron configuration for a nitride ion, N3-? A) 1s2 2s2 2p3 B) 1s2 2s2 2p4 C) 1s2 2s2 2p5 D) 1s2 2s2 2p6 E) none of the above 86. What is the term for a compound containing hydrogen and a nonmetal dissolved in water? A) binary acid B) binary base C) ternary acid D) ternary base E) none of the above 87. What is the term for a compound containing one metal and one nonmetal? A) binary acid B) binary ionic C) binary molecular D) ternary ionic E) ternary molecular 88. What is the term for a compound containing two nonmetals? A) binary acid B) binary ionic C) binary molecular D) ternary ionic E) ternary molecular 89. What is the general term for any positively charged ion? A) anion B) cation C) monoatomic ion D) polyatomic ion E) none of the above 90. What is the term for a group of atoms bound together and having an overall positive or negative charge? A) anion B) cation C) monoatomic ion D) polyatomic ion E) none of the above 91. What is the term for a compound containing hydrogen, a nonmetal, and oxygen dissolved in water? A) binary acid B) binary molecular C) ternary ionic D) ternary molecular E) ternary oxyacid 92. The compound Au2Se3 is classified as which of the following? A) binary ionic B) ternary ionic C) binary molecular D) binary acid E) ternary oxyacid 93. The compound CaCO3 is classified as which of the following? A) binary ionic B) ternary ionic C) binary molecular D) binary acid E) ternary oxyacid 94. The NH4+ ion is classified as which of the following? A) monoatomic cation B) monoatomic anion C) polyatomic cation D) polyatomic anion E) none of the above - 2- - 2- 95. What is the chemical formula for the oxide ion? A) O B) O C) O2 D) O2 E) none of the above 96. What is the predicted ionic charge of an element in Group VIA/16? A) 2+ B) 6+ C) 2- D) 6- E) none of the above 97. What is the chemical formula for the binary compound composed of Al3+ and O2- ions? A) AlO B) Al2O3 C) Al3O2 D) Al6O6 E) none of the above 98. What is the ionic charge for the cobalt ion in Co3N2? A) zero B) 1+ C) 2+ D) 3+ E) none of the above 99. What is the chemical formula for strontium iodide? A) SrI B) SrI2 C) SrI3 D) Sr3I2 E) Sr2I3 100. What is the chemical formula for mercury(I) nitride? A) HgN3 B) Hg2N3 C) Hg3N2 D) (Hg2)2N3 E) (Hg2)3N2 101. What is the systematic name for CdI2? A) cadmium iodide B) cadmium diiodide C) cadmium(I) iodide D) cadmium(II) iodide E) cadmium(IV) iodide 102. What is the Stock system name for Cu3N? A) copper nitride B) cuprous nitride C) cupric nitride D) copper(I) nitride E) copper(II) nitride 103. Predict the chemical formula for cadmium sulfide. A) CdS B) Cd2S C) CdS3 D) Cd2S3 E) Cd3S2 104. What is the chemical formula for barium phosphate? A) Ba3P2 B) BaPO3 C) BaPO4 D) Ba3(PO4)2 E) Ba2(PO4)3 105. What is the systematic name for Li2Cr2O7? A) lithium chromate B) lithium dichromate C) dilithium chromate D) dilithium dichromate E) lithium chromium heptaoxide 106. What is the chemical formula for dinitrogen tetraoxide? A) N2O B) N2O3 C) N2O4 D) N2O5 E) N2O9 107. What is the chemical formula for hydroselenic acid? A) HSe(aq) B) H2Se(aq) C) HSeO2(aq) D) H2SeO3(aq) E) H2SeO4(aq) 108. What is the chemical formula for sulfurous acid? A) H2S(aq) B) HSO3(aq) C) HSO4(aq) D) H2SO3(aq) E) H2SO4(aq) 109. What is the chemical formula for chloric acid? A) HCl(aq) B) HClO(aq) C) HClO2(aq) D) HClO3(aq) E) HClO4(aq) 110. What is the systematic name for aqueous H3PO3? A) hydrogen phosphate B) hydrophosphoric acid C) hydrophosphorous acid D) phosphorous acid E) phosphoric acid 111. Which of the following compounds is named using an -ide suffix? A) LiClO B) LiClO2 C) LiClO3 D) ClO2 E) none of the above 112. Which of the following compounds is named using an -ate suffix? A) LiClO B) LiClO2 C) LiClO3 D) ClO2 E) none of the above 113. What is the term for the relative order of metals arranged by their ability to undergo reaction? A) activity series B) elemental series C) reactivity series D) productivity series E) none of the above 114. What is the term for a compound that releases hydroxide ions when dissolved in water? A) acid B) base C) aqueous acid D) aqueous base E) none of the above 115. What is the term for a substance that speeds up a reaction without being permanently changed? A) accelerator B) catalyst C) inhibitor D) reactant E) none of the above 116. What is the term for a shorthand representation using formulas and symbols to describe a chemical change? A) chemical equation B) chemical formula C) chemical reaction D) chemical symbol E) none of the above 117. What is the term for a digit in front of a chemical formula that helps to balance a chemical equation? A) coefficient B) exponent C) subscript D) superscript E) none of the above 118. What is the term for a type of reaction in which two substances react to produce a single compound? A) combination B) decomposition C) double replacement D) neutralization E) single replacement 119. What is the term for a type of reaction in which two cations in different compounds exchange anions? A) combination B) decomposition C) double replacement D) neutralization E) single replacement 120. What is the term for a type of reaction in which an acid and a base react to produce a salt and water? A) combination B) decomposition C) double replacement D) neutralization E) single replacement 121. What term refers to an insoluble solid substance that is produced from a chemical reaction in aqueous solution? A) condensate B) precipitate C) salt D) suspension E) none of the above 122. Which of the following is evidence for a chemical reaction? A) change in physical state B) change in color C) change in mass D) all of the above E) none of the above 123. Which of the statements below best describes the following reaction?  Ni(NO3)2(s) Ni(NO2)2(s) + O2(g) A) Nickel(II) nitrate decomposes with heat. B) Nickel(II) nitrate decomposes to nickel(II) nitrite and oxygen. C) Nickel(II) nitrate decomposes to nickel(II) nitrite and oxygen gas. D) Nickel(II) nitrate is heated to give nickel(II) nitrite and oxygen. E) Solid nickel(II) nitrate is heated to give solid nickel(II) nitrite and oxygen gas. 124. Which of the following formulas represents an element in its natural state? A) B2 B) C2 C) N2 D) P2 E) none of the above 125. Which of the following is a general guideline for balancing an equation? A) Write correct formulas for reactants and products. B) Begin balancing with the most complex formula. C) Balance polyatomic ions as a single unit. D) Check each reactant and product to verify the coefficients. E) all of the above 126. What is the coefficient of oxygen gas after balancing the following equation? ___P(s) + ___O2(g) → ___P2O5(s) A) 1 B) 2 C) 4 D) 5 E) none of the above 127. What is the coefficient of carbon dioxide after balancing the following equation?__  KHCO3(s) __K2CO3(s) + __H2O(g) + __CO2(g) A) 1 B) 2 C) 3 D) 4 E) none of the above 128. What is the coefficient of water after balancing the following equation?__ H3PO4(aq) + __Ba(OH)2(aq) → __Ba3(PO4)2(s) + __H2O(l) A) 1 B) 2 C) 3 D) 6 E) none of the above 129. What is the predicted product from the following combination reaction?  Li(s) + O2(g) A) LiO B) Li2O C) LiO2 D) Li2O3 E) Li3O2 130. Which of the following metals reacts with aqueous FeSO4?Partial Activity Series: Fe > Co > (H) > Cu > Ag A) Co B) Cu C) Ag D) all of the above E) none of the above 131. What are the products from the following single-replacement reaction? Cd(s) + AgNO3(aq) → A) Ag and Cd(NO3)2 B) Ag and Cd(NO2)2 C) Ag2O and Cd(NO3)2 D) Ag2O and Cd(NO2)2 E) no reaction 132. Which of the following solid compounds is soluble in water? A) CaCO3 B) PbSO4 C) AlPO4 D) all of the above E) none of the above 133. Which of the following solid compounds is insoluble in water? A) Li2CO3 B) AgC2H3O2 C) Cu(NO3)2 D) all of the above E) none of the above 134. What are the products from the following double-replacement reaction? AgNO3(aq) + Li3PO4(aq) → A) Ag3P and LiNO3 B) Ag3PO3 and LiNO2 C) Ag3PO3 and LiNO3 D) Ag3PO4 and LiNO2 E) Ag3PO4 and LiNO3 135. What are the predicted products from the following neutralization reaction? HC2H3O2(aq) + Ca(OH)2(aq) → A) CaCO3 and H2O B) Ca(HCO3)2 and H2 C) Ca(HCO3)2 and H2O D) Ca(C2H3O2)2 and H2 E) Ca(C2H3O2)2 and H2O 136. What are the products from the complete neutralization of carbonic acid with aqueous potassium hydroxide? A) K2CO3(aq) and H2O(l) B) KHCO3(aq) and H2O(l) C) KHCO4(aq) and H2O(l) D) KC2H3O2(aq) and H2O(l) E) K2C2H3O2(aq) and H2O(l) 137. Propane, C3H8, is flammable and used in rural areas where natural gas is not available. What is the coefficient of oxygen in the balanced equation for the combustion of propane?  __C3H8(g) + __O2(g) __CO2(g) + __H2O(g) A) 1 B) 5 C) 7 D) 10 E) none of the above 138. What is the term for the value corresponding to the number of atoms in 12.01 g of carbon? A) Avogadro's number B) atomic number C) mass number D) mole number E) none of the above 139. What general term refers to the mass of 1 mol of any substance? A) gram-atomic mass B) gram- molecular mass C) gram-formula mass D) molar mass E) none of the above 140. What is the term for the volume occupied by 1 mol of any gas at STP? A) Avogadro's volume B) molar volume C) standard volume D) STP volume E) none of the above 141. What is the term for the amount of substance that contains 6.02 × 1023 particles? A) Avogadro's number B) formula mass C) molar mass D) mole E) none of the above 142. What is the term for the mass percent of each element in a compound? A) compound composition B) elemental composition C) mass composition D) percent composition E) none of the above 143. What is the term for a temperature of 0°C and a pressure of 1 atm? A) atmospheric temperature and pressure B) experimental temperature and pressure C) ideal gas temperature and pressure D) standard temperature and pressure E) none of the above 144. What is the number of magnesium atoms that equal a mass of 24.31 amu? A) 1 B) 12 C) 24 D) 6.02 × 1023 E) none of the above 145. Given that P-31 is the only natural isotope of phosphorus, what is the mass of one P atom and Avogadro's number of P atoms, respectively? A) 30.97 amu and 30.97 g B) 30.97 g and 30.97 amu C) 31 amu and 31 g D) 31 g and 31 amu E) none of the above 146. How many moles of argon gas contain 7.52 × 1022 Ar atoms? A) 0.0125 mol B) 0.0801 mol C) 0.125 mol D) 0.801 mol E) 1.25 mol 147. What is the molar mass of aspirin, C9H8O4? A) 29.02 g/mol B) 116.08 g/mol C) 180.17 g/mol D) 244.17 g/mol E) 252.25 g/mol 148. What is the mass of 3.30 × 1023 atoms of silver, Ag? A) 0.549 g B) 25.8 g C) 59.1 g D) 85.7 g E) 197 g 149. How many bromine molecules, Br2, have a mass equal to 31.8 g? A) 1.20 × 1023 molecules B) 1.51 × 1024 molecules C) 1.91 × 1025 molecules D) 2.40 × 1023 molecules E) 3.03 × 1024 molecules 150. What is the volume of 1.20 × 1022 molecules of nitric oxide gas, NO, at STP? A) 0.0199 L B) 0.447 L C) 2.24 L D) 5.02 L E) 1120 L 151. How many carbon dioxide molecules are in 500.0 mL of CO2 gas at STP? A) 1.34 × 1022 molecules B) 2.23 × 1021 molecules C) 2.23 × 1025 molecules D) 2.70 × 1022 molecules E) 2.70 × 1025 molecules 152. What is the mass of 5.00 liters of oxygen gas, O2, at STP? A) 0.286 g B) 3.50 g C) 6.40 g D) 7.14 g E) 112 g 153. What is the volume occupied by 11.0 g of propane gas, C3H8, at STP? A) 0.250 L B) 4.00 L C) 5.59 L D) 21.6 L E) 89.6 L 154. What is the density of ozone gas, O3, at STP? A) 0.467 g/L B) 0.714 g/L C) 1.40 g/L D) 2.14 g/L E) 22.4 g/L 155. If 1.00 L of an unknown gas at STP has a mass of 3.40 g, what is its molar mass? A) 3.40 g/mol B) 6.59 g/mol C) 22.4 g/mol D) 76.2 g/mol E) 340 g/mol 156. The first inert gas compound to be synthesized was XePtF6. What is the percentage of fluorine in the compound? A) 4.31% B) 5.50% C) 25.9% D) 29.8% E) 44.3% 157. If 1.823 g of cobalt metal react with 0.495 g of oxygen gas, what is the empirical formula of the cobalt oxide product? A) CoO B) CoO2 C) CoO3 D) Co2O3 E) Co3O2 158. Acetylene is used in oxyacetylene gas welding. Calculate the empirical formula for acetylene given its percent composition: 92.25% C and 7.75% H. A) CH B) CH2 C) CH8 D) C8H8 E) C12H 159. What is the molecular formula of lysine if the empirical formula is C3H7NO, and the approximate molar mass is 146 g/mol? A) CHNO B) C3H7NO C) C3H7NO2 D) C6H14NO2 E) C6H14N2O2 160. Find the molecular formula for lindane given its percent composition: 24.78% C, 2.08% H, and 73.14% Cl. The approximate molar mass is 290 g/mol. A) CHCl B) C3H3Cl3 C) CHCl6 D) C6H6Cl6 E) C12HCl35 161. What is the volume of 1.51 × 1024 atoms of an unknown gas at STP? A) 0.112 L B) 2.51 L C) 8.93 L D) 56.2 L E) not enough information is given 162. What principle states that equal volumes of gases, at the same temperature and pressure, contain equal numbers of molecules? A) Avogadro's theory B) law of combining volumes C) law of conservation of mass D) law of constant composition E) none of the above 163. What principle states the total mass of products from a chemical reaction must equal the sum of the masses of reactants? A) Avogadro's theory B) law of combining volumes C) law of conservation of mass D) law of constant composition E) none of the above 164. What is the term for the substance in a chemical reaction that controls the maximum amount of product? A) limiting reactant B) limiting product C) maximum reactant D) maximum product E) none of the above 165. What term expresses the ratio of moles of reactants and products according to the coefficients in the balanced chemical equation? A) mole ratio B) reactant ratio C) product ratio D) yield ratio E) none of the above 166. What term expresses the amount of the actual yield compared to the theoretical yield? A) experimental yield B) percent yield C) ratio yield D) stoichiometric yield E) none of the above 167. How many moles of carbon monoxide react with 1 mol of oxygen gas according to the balanced  chemical equation? 2 CO(g) + O2(g) 2 CO2(g) A) 1 mol B) 2 mol C) 3 mol D) 4 mol E) none of the above 168. In an experiment, 5.585 g of iron metal reacts with 3.207 g of yellow sulfur. Using the  conservation of mass law, predict the mass of product. Fe(s) + S(s) FeS(s) A) 2.198 g B) 2.378 g C) 4.396 g D) 8.792 g E) 17.584 g 169. How many moles of oxygen gas react to yield 0.100 mol water?  __C5H12(g) + __O2(g) __CO2(g) + __H2O(g) A) 0.100 mol B) 0.500 mol C) 0.600 mol D) 0.800 mol E) none of the above 170. What is the mass of silver bromide (187.77 g/mol) precipitated from 2.96 g of iron(III) bromide (295.55 g/mol)? __FeBr3(s) + __AgNO3(aq) → __AgBr(s) + __Fe(NO3)3(aq) A) 0.940 g B) 0.627 g C) 1.88 g D) 5.64 g E) 3.76 g 171. What is the mass of aluminum metal that reacts to give 1.00 g of iron?  __FeO(l) + __Al(l) __Fe(l) + __Al2O3(l) A) 0.322 g B) 0.483 g C) 0.725 g D) 0.966 g E) 1.449 g 172. What is the volume of oxygen gas at STP from the decomposition of 1.70 g of sodium nitrate  (85.00 g/mol)? __NaNO3(s) __NaNO2(s) + __O2(g) A) 0.224 L B) 0.448 L C) 0.896 L D) 3.23 L E) 12.9 L 173. What volume of oxygen gas reacts with 20.0 mL of hydrogen chloride?  __HCl(g) + __O2(g) __Cl2(g) + __H2O(g) A) 5.00 mL B) 10.0 mL C) 20.0 mL D) 40.0 mL E) none of the above 174. How many moles of copper(I) sulfide are produced from the reaction of 1.00 mol of copper and  1.00 mol of sulfur? 2 Cu(s) + S(s) Cu2S(s) A) 0.500 mol B) 1.00 mol C) 1.50 mol D) 2.00 mol E) none of the above 175. What mass of cobalt(III) sulfide (214.07 g/mol) is produced from 0.750 g of cobalt and 0.350 g of  sulfur? 2 Co(s) + 3 S(s) Co2S3(s) A) 0.779 g B) 1.36 g C) 2.34 g D) 2.72 g E) 5.45 g 176. What is the volume of NO gas produced from 30.0 L of nitrogen gas and 20.0 L of oxygen gas?  (Assume constant conditions.) N2(g) + O2(g) 2 NO(g) A) 20.0 L B) 30.0 L C) 40.0 L D) 60.0 L E) none of the above 177. Starting with 1.550 g of potassium chlorate, a student releases 0.617 g of oxygen gas. If the calculated mass of oxygen gas is 0.607 g, what is the percent yield? A) 39.2% B) 39.8% C) 98.4% D) 102% E) 255% 178. The decomposition of 1.500 g of sodium nitrate produced 195 mL of oxygen gas. If the calculated volume of oxygen gas is 198 mL, what is the percent yield? A) 65.7% B) 68.0% C) 98.5% D) 102% E) 152% 179. What is the theoretical temperature at which the kinetic energy of a gas is zero? A) absolute zero B) -100°C C) -273°F D) -273 K E) none of the above 180. What is the term for the pressure exerted by the gas molecules in air? A) atmospheric pressure B) gas pressure C) partial pressure D) vapor pressure E) none of the above 181. Which of the following states that the pressure exerted by a mixture of gases is equal to the sum of the individual gas pressures? A) Boyle's law B) Charles' law C) Dalton's law D) Gay-Lussac's law E) none of the above 182. What is the term for gas molecules colliding with no change in total energy? A) elastic collision B) isokinetic collision C) isothermal collision D) molecular collision E) none of the above 183. What is the term that refers to the frequency and energy of gas molecules colliding with the walls of the container? A) atmospheric pressure B) gas pressure C) partial pressure D) vapor pressure E) none of the above 184. Which of the following is described by the equation: PV = nRT? A) Boyle's law B) Charles' law C) Gay-Lussac's law D) ideal gas law E) none of the above 185. What is the term for the pressure exerted by gaseous vapor above a liquid in a sealed container when the rates of evaporation and condensation are equal? A) atmospheric pressure B) gas pressure C) partial pressure D) vapor pressure E) none of the above 186. If a gas pressure gauge reads 15 mm Hg, what is the pressure in atmospheres? A) 0.020 atm B) 0.20 atm C) 15 atm D) 1100 atm E) 11,000 atm 187. Which of the following changes increases the pressure of a gas? A) decreasing the volume B) increasing temperature C) increasing the number of molecules D) all of the above E) none of the above 188. A sample of neon gas at 1.20 atm compresses from 0.250 L to 0.125 L. If the temperature remains constant, what is the final pressure? A) 0.600 atm B) 1.00 atm C) 1.20 atm D) 2.40 atm E) none of the above 189. If a volume of air at 375 K increases from 100.0 mL to 150.0 mL, what is the final Kelvin temperature? Assume pressure remains constant. A) 153 K B) 250 K C) 375 K D) 344 K E) 563 K 190. If a 50.0 mL sample of xenon gas is at 0.921 atm and 27°C, what is the volume of the gas at STP? A) 41.9 mL B) 49.4 mL C) 50.6 mL D) 54.9 mL E) 59.7 mL 191. If the temperature decreases, what happens to the vapor pressure? A) increases B) decreases C) remains constant D) unpredictable E) none of the above 192. If carbon dioxide gas is collected over water at 25°C and 775 torr, what is the partial pressure of the CO2? The vapor pressure of water is 23.8 torr at 25°C. A) 23.8 torr B) 750 torr C) 751 torr D) 775 torr E) 799 torr 193. An atmospheric sample is composed of nitrogen, oxygen, argon, and traces of other gases. If the partial pressure of nitrogen is 587 torr, oxygen is 158 torr, and argon is 7 torr, what is the observed barometric pressure? A) 8 torr B) 100 torr C) 422 torr D) 752 torr E) 1512 torr 194. Which of the following is true according to the kinetic theory of gases? A) Molecules lose energy after colliding. B) Molecules remain in fixed positions. C) Molecules are attracted to one another. D) all of the above E) none of the above 195. At the same temperature, which of the following gases contains molecules with the fastest average velocity? A) carbon monoxide, CO B) carbon dioxide, CO2 C) nitrogen monoxide, NO D) nitrogen dioxide, NO2 E) The average velocity is the same. 196. If 0.795 mol of ammonia gas occupies 24.5 L at 0.853 atm, what is the Celsius temperature? (R = 0.0821 L•atm/mol•K) A) -71°C B) 5°C C) 47°C D) 278°C E) 320°C 197. If a nitrogen gas sample occupies a volume of 2.55 L at 22.0°C and 0.860 atm, what is the mass of the N2 gas? (R = 0.0821 L•atm/mol•K) A) 0.394 g B) 1.27 g C) 2.54 g D) 5.13 g E) 34.0 g 198. A 0.079-g sample of an unknown metal is dropped into hydrochloric acid and reacts to produce 66.00 mL of dry hydrogen gas at 22°C and 732 mm Hg. What is the unknown metal (X)? 2 X(s) + 6 HCl(aq) → 2 XCl3(aq) + 3 H2(g) A) Al B) Co C) Ga D) Fe E) Sc 199. What type of bond is characterized by sharing two pairs of electrons? A) single bond B) double bond C) triple bond D) electrovalent bond E) none of the above 200. What is the term for the smallest representative unit in a compound held together by ionic bonds? A) formula unit B) molecule C) monoatomic ion D) polyatomic ion E) none of the above 201. What is the term for a chemical bond characterized by the attraction between a cation and anion? A) coordinate covalent bond B) ionic bond C) nonpolar bond D) polar bond E) none of the above 202. What is the term for the valence electrons in a molecule that are not shared? A) bonding electrons B) core electrons C) kernel electrons D) nonbonding electrons E) none of the above 203. What is the term for a bond in which a pair of electrons is shared equally? A) coordinate covalent bond B) electrovalent bond C) nonpolar bond D) polar bond E) none of the above 204. What is the term for the statement that an atom tends to bond in such a way so as to acquire eight valence electrons? A) atomic rule B) bonding rule C) electron rule D) octet rule E) none of the above 205. What is the term for a group of atoms held together by covalent bonds and having an overall positive or negative charge? A) formula unit B) molecule C) monoatomic ion D) polyatomic ion E) none of the above 206. What type of bond is characterized by sharing three pairs of electrons? A) single bond B) double bond C) triple bond D) electrovalent bond E) none of the above 207. What is the term for the electrons in the highest s and p sublevels in an atom that undergo reaction and form chemical bonds? A) s electrons B) p electrons C) bonding electrons D) valence electrons E) none of the above 208. Predict which of the following has an ionic bond (refer to Periodic Table). A) HI B) IBr C) LiH D) all of the above E) none of the above 209. Which of the following is not held together by ionic bonds? A) CoO B) Cu2O C) H2O D) SnO2 E) ZnO 210. How many valence electrons are in a nitrogen atom and a nitride ion? A) 3 and 8, respectively B) 5 and 8, respectively C) 8 and 5, respectively D) 7 and 10, respectively E) none of the above 211. Which of the following statements is true regarding an ionic bond between a metal and nonmetal in a formula unit? A) An ionic bond is the attraction between a metal and nonmetal ion. B) Metal atoms lose electrons, and nonmetal atoms gain electrons. C) The ionic radius of a metal ion is less than its atomic radius. D) Breaking an ionic bond between two ions requires energy. E) all of the above 212. What is the core notation for the electron configuration of a cobalt(II) ion, Co2+? A) [Ar] 4s2 3d5 B) [Ar] 4s2 3d7 C) [Ar] 4s2 3d9 D) [Ar] 3d7 E) none of the above 213. What is the term for a compound which reacts with water to produce an acidic solution? A) anhydrous B) hydrate C) metal oxide D) nonmetal oxide E) none of the above 214. What is the term for water molecules bound to a formula unit in a hydrate? A) anhydrous water B) deliquescent water C) efflorescent water D) water of hydration E) none of the above 215. Which of the following is an observed property of liquids? A) Liquids have a fixed shape and variable volume. B) Liquids that are soluble mix homogeneously. C) Liquids compress and expand significantly. D) Liquids are less dense than gases. E) none of the above  216. Complete the following chemical reaction and indicate the products. C2H4(g) + O2(g) A) C + H2O B) CO + H2 C) CO + H2O D) CO2 + H2 E) CO2 + H2O 217. What are the products from a neutralization reaction? A) metal oxide and water B) nonmetal oxide and hydrogen C) salt and water D) salt and hydrogen E) none of the above 218. Complete the following chemical reaction and indicate the products. HCl(aq) + NH4OH(aq) → A) NH4Cl and O2 B) NH4Cl and H2O C) NH4Cl and H2O2 D) NH3, Cl2, and H2O E) NH3, HCl, and H2O 219. What is the term that refers to liquids that do not dissolve in one another and separate into two layers? A) immiscible B) insoluble C) miscible D) soluble E) none of the above 220. What is the term for the general principle that solubility is greatest when the polarity of the solute is similar to that of the solvent? A) like dissolves like rule B) polarity rule C) solute rule D) solvent rule E) none of the above 221. What is the term for a solution that contains the maximum amount of solute that can dissolve at a given temperature? A) concentrated B) saturated C) supersaturated D) unsaturated E) none of the above 222. What is the term for a solution that contains more solute than is ordinarily soluble at a given temperature? A) concentrated B) saturated C) supersaturated D) unsaturated E) none of the above 223. Which of the following illustrates the like dissolves like rule for a solid solute in a liquid solvent? A) An ionic compound is soluble in a nonpolar solvent. B) A polar compound is soluble in a nonpolar solvent. C) A nonpolar compound is soluble in a polar solvent. D) A nonpolar compound is soluble in a nonpolar solvent. E) none of the above 224. What is the mass of solute dissolved in 10.0 g of a 5.00% sugar solution? A) 0.180 g B) 0.500 g C) 0.900 g D) 9.50 g E) 10.0 g 225. What is the molarity of a glucose solution that contains 10.0 g of C6H12O6 (180.18 g/mol) dissolved in 100.0 mL of solution? A) 0.00555 M B) 0.0555 M C) 0.555 M D) 1.80 M E) 18.0 M 226. What is the mass of nickel(II) nitrate (182.71 g/mol) dissolved in 25.0 mL of 0.100 M Ni(NO3)2 solution? A) 0.250 g B) 0.457 g C) 4.00 g D) 45.7 g E) 457 g 227. What is the volume of 3.00 M sulfuric acid that contains 9.809 g of H2SO4 solute (98.09 g/mol)? A) 0.300 mL B) 30.0 mL C) 33.3 mL D) 333 mL E) 3330 mL 228. What is the molarity of a nitric acid solution prepared by diluting 250.0 mL of 6.00 M HNO3 to a total volume of 2.50 L? A) 0.0600 M B) 0.250 M C) 0.600 M D) 2.50 M E) 6.00 M 229. What volume of 0.100 M nitric acid reacts completely with 0.500 g of sodium carbonate, Na2CO3 (105.99 g/mol)? Na2CO3(s) + 2 HNO3(aq) → 2 NaNO3(aq) + H2O(l) + CO2(g) A) 10.6 mL B) 23.6 mL C) 47.2 mL D) 94.3 mL E) 1.00 L 230. What is the molarity of aqueous silver nitrate if 50.0 mL of AgNO3 reacts with 25.0 mL of 0.100 M K2CrO4? 2 AgNO3(aq) + K2CrO4(aq) → Ag2CrO4(s) + 2 KNO3(aq) A) 0.0250 M B) 0.0500 M C) 0.100 M D) 0.200 M E) 0.400 M 231. If 45.5 mL of 0.150 M sodium sulfate solution reacts completely with aqueous barium nitrate, what is the mass of BaSO4 (233.40 g/mol) precipitate? Ba(NO3)2(aq) + Na2SO4(aq) → BaSO4(s) + 2 NaNO3(aq) A) 0.0292 g B) 0.769 g C) 1.59 g D) 6.83 g E) 34.1 g 232. What is the term for a substance that acts as a proton donor in one reaction and as a proton acceptor in another? A) amphiprotic B) buffer C) salt D) zwitterion E) none of the above 233. What is the term for a substance that releases hydroxide ions in water? A) Arrhenius acid B) Arrhenius base C) Brønsted-Lowry acid D) Brønsted-Lowry base E) none of the above 234. What is the term for a substance that donates a proton in an acid-base reaction? A) Arrhenius acid B) Arrhenius base C) Brønsted-Lowry acid D) Brønsted-Lowry base E) none of the above 235. What is the term for a chemical equation that portrays an ionic reaction after spectator ions have been canceled? A) dissociation equation B) ionization equation C) net ionic equation D) total ionic equation E) none of the above 236. What is the term for a solution that is a good conductor of electricity? A) aqueous electrolyte B) nonelectrolyte C) strong electrolyte D) weak electrolyte E) none of the above 237. What is the term for the laboratory procedure of delivering a measured volume of solution through a buret? A) conditioning B) standardizing C) transferring D) titration E) none of the above 238. Which of the following is a general property of an acidic solution? A) tastes sour B) feels slippery C) turns litmus blue D) pH greater than 7 E) none of the above 239. If stomach digestive juice has a pH of 1, the solution is which of the following? A) strongly acidic B) weakly acidic C) neutral D) weakly basic E) strongly basic 240. Which of the following is a weak Arrhenius acid? A) HCl(aq) B) HNO3(aq) C) HC2H3O2(aq) D) all of the above E) none of the above 241. What acid and base are neutralized to give potassium nitrate salt? A) HCl(aq) and KOH(aq) B) HNO3(aq) and KOH(aq) C) HNO3(aq) and KNO3(aq) D) HOH(aq) and KNO3(aq) E) none of the above 242. In the following reaction, which reactant is a Brønsted-Lowry acid?H2CO3(aq) + Na2HPO4(aq) → NaHCO3(aq) + NaH2PO4(aq) A) H2CO3 B) Na2HPO4 C) NaH2PO4 D) NaHCO3 E) none of the above 243. In the following reaction, which reactant is a Brønsted-Lowry acid?NaHCO3(aq) + NaH2PO4(aq) → Na2HPO4(aq) + H2CO3(aq) A) NaHCO3 B) NaH2PO4 C) Na2HPO4 D) H2CO3 E) none of the above 244. If 25.0 mL of 0.100 M HCl is titrated with 0.150 M Ba(OH)2, what volume of barium hydroxide is required to neutralize the acid?2 HCl(aq) + Ba(OH)2(aq) → BaCl2(aq) + 2 H2O(l) A) 8.33 mL B) 16.7 mL C) 18.8 mL D) 33.3 mL E) 37.5 mL 245. An ammonia solution is 6.00 M and the density is 0.950 g/mL. What is the mass/mass percent concentration of NH3 (17.04 g/mol)? A) 0.0971% B) 0.108% C) 9.71% D) 10.2% E) 10.8% 246. What is the molarity of a sulfuric acid solution if 30.00 mL of H2SO4 is required to neutralize 0.840 g of sodium hydrogen carbonate (84.01 g/mol)?H2SO4(aq) + 2 NaHCO3(aq) → Na2SO4(aq) + 2 H2O(l) + 2 CO2(g) A) 0.167 M B) 0.300 M C) 0.333 M D) 0.500 M E) 0.667 M 247. Lactic acid is found in sour milk and can be abbreviated HLac. If 47.50 mL of 0.275 M NaOH neutralizes 1.180 g of HLac, what is the molar mass of the acid? HLac(aq) + NaOH(aq) → NaLac(aq) + H2O(l) A) 45.1 g/mol B) 90.1 g/mol C) 111 g/mol D) 181 g/mol E) 204 g/mol 248. If a solution is a poor conductor of electricity, which of the following is true? A) The solution is highly ionized. B) The solution is slightly ionized. C) The solution is highly reactive. D) The solution is slightly reactive. E) none of the above 249. Which of the following in aqueous solution is a weak electrolyte? A) H2CO3(aq) B) LiOH(aq) C) NH4Cl(aq) D) all of the above E) none of the above 250. What percentage of the concepts in this course do you think you mastered? A) About 20% B) Between 20 and 40 % C) Between 40 and 60% D) Between 60 and 80% E) Between 80 and 100%

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