Test Bank For Chemistry, 6th Edition

Chapter 2: Atoms, Ions, and Molecules: Matter Starts Here MULTIPLE CHOICE 1. Who discovered electrons? a. Robert Boyle b. Robert Millikan c. Joseph John Thomson d. John Dalton e. Albert Einstein ANS: C DIF: Easy REF: 2.2 OBJ: Explain how the experiments of Thomson, Millikan, and Rutherford contributed to our understanding of atomic structure. MSC: Remembering 2. Who was the first scientist to determine the charge of an electron? a. Robert Boyle d. John Dalton b. Robert Millikan e. Albert Einstein c. Joseph John Thomson ANS: B DIF: Easy REF: 2.2 OBJ: Explain how the experiments of Thomson, Millikan, and Rutherford contributed to our understanding of atomic structure. MSC: Remembering 3. In the atoms in the Rutherford–Geiger–Marsden experiment, the alpha particles were repelled by ________ a. electrons. d. nuclei. b. protons. e. gravity. c. neutrons. ANS: D DIF: Easy REF: 2.2 OBJ: Describe the evidence obtained from the Rutherford–Geiger–Marsden experiment with alpha particles and how it rejected the plum-pudding model and led to the nuclear model of atomic structure. MSC: Remembering 4. The Rutherford–Geiger–Marsden gold foil experiments paved the way for the nuclear model of the atom, replacing ________ of the atom. a. the quantum mechanical model d. the plum-pudding model b. Dalton’s theory e. Einstein’s relativistic theory c. Avogadro’s law ANS: D DIF: Easy REF: 2.2 OBJ: Describe the evidence obtained from the Rutherford–Geiger–Marsden experiment with alpha particles and how it rejected the plum-pudding model and led to the nuclear model of atomic structure. MSC: Remembering 5. Which one of the following experiments provided evidence that atoms contained small massive nuclei with positive charges? a. Bunsen and Kirchoff’s flame test b. Fraunhofer lines c. the Rutherford–Geiger–Marsden experiment d. Thomson’s experiments with cathode ray tubes e. Millikan’s oil-drop experiment ANS: C DIF: Easy REF: 2.2 OBJ: Describe the evidence obtained from the Rutherford–Geiger–Marsden experiment with alpha particles and how it rejected the plum-pudding model and led to the nuclear model of atomic structure. MSC: Remembering 6. What is the correct symbol for an electron? a. b. d. e. c. ANS: A DIF: Easy REF: 2.2 OBJ: Identify and describe the particles that comprise an atom and their symbols. MSC: Remembering 7. What is the correct symbol for a proton? a. b. d. e. c. ANS: C DIF: Easy REF: 2.2 OBJ: Identify and describe the particles that comprise an atom and their symbols. MSC: Remembering 8. What is the correct symbol for a neutron? a. b. d. e. c. ANS: A DIF: Easy REF: 2.2 OBJ: Identify and describe the particles that comprise an atom and their symbols. MSC: Remembering 9. Protons and neutrons are examples of ________ a. nuclei. d. isotopes. b. nuclides. e. charged particles. c. nucleons. ANS: C DIF: Easy REF: 2.2 OBJ: Identify and describe the particles that comprise an atom and their symbols. MSC: Remembering 10. The 4He nucleus is an example of ________ a. a nuclide. b. a muon. d. a neutron. e. a nucleon. c. a proton. ANS: A DIF: Easy REF: 2.2 OBJ: Identify and describe the particles that comprise an atom and their symbols. MSC: Remembering 11. Which statement is correct? a. Electrons, protons, and neutrons have about the same mass. b. Electrons have a much smaller mass than that of protons and neutrons. c. Neutrons are much more massive than protons. d. Protons are much more massive than neutrons. e. Electrons have a much larger mass than that of protons and neutrons. ANS: B DIF: Easy REF: 2.2 OBJ: Compare the relative masses of electrons, protons, and neutrons. MSC: Remembering 12. Which statement is not correct? In atomic mass units (amu or u), ________ a. the mass of an electron, proton, or neutron is approximately 1 u. b. the mass of a proton or neutron is approximately 1 u, and the mass of an electron is approximately 0 u. c. the mass of an atom is approximately equal to the number of protons and neutrons in the nucleus of the atom. d. the mass of a carbon-12 atom is exactly 12 u. e. the mass of an oxygen-16 atom is approximately 16 u. ANS: A DIF: Easy REF: 2.2 OBJ: Compare the relative masses of electrons, protons, and neutrons. MSC: Remembering 13. Which statement is not correct? a. Electrons have a negative electrical charge. b. Protons have a positive electrical charge. c. Neutrons do not have an electrical charge. d. In an atom, the interaction between electrons and protons is attractive. e. In an atom, the interaction between electrons and neutrons is repulsive. ANS: E DIF: Easy REF: 2.2 OBJ: Compare the electrical charges of electrons, protons, and neutrons. MSC: Remembering 14. Which statement about isotopes of the same element is not correct? a. They have the same number of protons. b. They have different numbers of neutrons. c. They have essentially the same chemical properties. d. They have the same atomic mass. e. They have the same number of electrons. ANS: D DIF: Easy REF: 2.3 OBJ: Write a definition of the term isotope, and identify the feature that distinguishes one isotope from another. MSC: Remembering 15. Which statement best describes isotopes? a. They have the same atomic mass. b. They have the same total number of protons and neutrons. c. They have the same number of neutrons but a different number of protons. d. They have the same number of protons but a different number of neutrons. e. They have very different chemical reactivity. ANS: D DIF: Easy REF: 2.3 OBJ: Write a definition of the term isotope, and identify the feature that distinguishes one isotope from another. MSC: Remembering 16. 1 H, 2H, and 3H are examples of ________ because they have different numbers of ________. a. isotopes; protons d. allotropes; neutrons b. isotopes; neutrons e. allotropes; protons c. isotopes; electrons ANS: B DIF: Easy REF: 2.3 OBJ: Write a definition of the term isotope, and identify the feature that distinguishes one isotope from another. MSC: Remembering 17. Which of the following atoms contains the least number of neutrons? a. d. b. e. c. ANS: B DIF: Easy REF: 2.3 OBJ: Convert between an atomic symbol and the number of protons, neutrons, nucleons, and electrons comprising an ion. MSC: Applying 18. Which particle-level diagram is the best representation of a a. c. b. d. ion? ANS: D DIF: Easy REF: 2.3 OBJ: Describe how particles are distributed in an atom given its atomic symbol. MSC: Understanding 19. Which particle-level diagram is the best representation for a atom? a. c. b. d. ANS: B DIF: Easy REF: 2.3 OBJ: Describe how particles are distributed in an atom given its atomic symbol. MSC: Understanding 20. A Mn2+ ion has ________ protons, ________ neutrons, and ________electrons. a. 23; 30; 25 d. 25; 30; 25 b. 25; 30; 23 e. 30; 25; 30 c. 30; 25; 23 ANS: B DIF: Easy REF: 2.3 OBJ: Convert between an atomic symbol and the number of protons, neutrons, nucleons, and electrons comprising an ion. MSC: Applying 21. A Cl atom has ________ protons, ________ neutrons, and ________ electrons. a. 17; 18; 19 d. 17; 18; 17 b. 17; 20; 17 e. 18; 17; 18 c. 17; 17; 20 ANS: D DIF: Easy REF: 2.3 OBJ: Convert between an atomic symbol and the number of protons, neutrons, nucleons, and electrons comprising an ion. MSC: Applying 22. A O ion has ________ protons, ________ neutrons, and ________ electrons. a. 8; 8; 6 d. 8; 8; 8 b. 8; 10; 10 e. 8; 16; 8 c. 8; 8; 10 ANS: C DIF: Easy REF: 2.3 OBJ: Convert between an atomic symbol and the number of protons, neutrons, nucleons, and electrons comprising an ion. MSC: Applying 23. What is the symbol of the ion having 12 protons and 10 electrons? a. Mg2+ d. Na2+ 3+ b. Al e. Mg c. Mg2− ANS: A DIF: Easy REF: 2.3 OBJ: Convert between an atomic symbol and the number of protons, neutrons, nucleons, and electrons comprising an ion. MSC: Applying 24. What is the symbol of the ion having 17 protons and 18 electrons? a. S2− d. Cl+ b. Cl e. K+ c. Cl− ANS: C DIF: Easy REF: 2.3 OBJ: Convert between an atomic symbol and the number of protons, neutrons, nucleons, and electrons comprising an ion. MSC: Applying 25. A hypothetical element has two stable isotopes: one isotope has a mass of 106.9051 amu with an abundance of 48.183%, the other isotope has a mass of 108.9048 amu with an abundance of 51.825%. What is the average atomic mass of this element? a. 107.980 amu d. 107.950 amu b. 107.970 amu e. 107.940 amu c. 107.960 amu ANS: D DIF: Easy REF: 2.4 OBJ: Use natural abundance data for isotopes to calculate an average atomic mass. MSC: Applying 26. An unknown element is found to contain isotopes with the following masses and natural abundances: 38.9637 amu (93.08%), 39.9640 amu (0.012%), and 40.9618 amu (6.91%). Using these data, identify the element. a. S d. K b. Cl e. Ca c. Ar ANS: D DIF: Difficult REF: 2.4 OBJ: Use natural abundance data for isotopes to calculate an average atomic mass. MSC: Applying 27. Enriched weapons-grade uranium consists of 80% uranium-235 (235.044 amu) and 20% uranium-238 (238.051 amu). What is the average atomic mass of weapons-grade uranium, assuming the percentages are exact? a. 235.044 amu d. 235.645 amu b. 236.547 amu e. 235.754 amu c. 238.051 amu ANS: D DIF: Medium REF: 2.4 OBJ: Use natural abundance data for isotopes to calculate an average atomic mass. MSC: Applying 28. The Curiosity rover now on Mars analyzed rocks and found magnesium to have the following isotopic composition. What is the average atomic mass of magnesium in these rocks? Mass (u) 23.9872 24.9886 25.9846 a. 24.31 u b. 24.29 u c. 24.33 u % Abundance 79.70 10.13 10.17 d. 24.99 u e. 33.33 u ANS: B DIF: Easy REF: 2.4 OBJ: Use natural abundance data for isotopes to calculate an average atomic mass. MSC: Applying 29. There are three major isotopes of silicon: silicon-28, silicon-29, and silicon-30. Given the average atomic mass of silicon is 28.10 amu, estimate the percent abundance of the most abundant isotope of silicon. a. 8% d. 80% b. 20% e. 92% c. 66% ANS: E DIF: Medium REF: 2.4 OBJ: Identify the isotope that is likely to be the most abundant, given the masses of the isotopes and the average atomic mass. MSC: Understanding 30. For each of the elements below, there are only two naturally occurring isotopes. Using information in your periodic table, identify the pair in which the heavier isotope is the more abundant one. a. 63Cu and 65Cu d. 79Br and 81Br b. 85Rb and 87Rb e. 14N and 15N 10 11 c. B and B ANS: C DIF: Medium REF: 2.4 OBJ: Identify the isotope that is likely to be the most abundant, given the masses of the isotopes and the average atomic mass. MSC: Understanding 31. For each of the elements below, there are only two naturally occurring isotopes. Using information in your periodic table, identify the pair in which the lighter isotope is the more abundant one. a. 6Li and 7Li d. 191Ir and 193Ir 79 81 b. Br and Br e. 50V and 51V 10 11 c. B and B ANS: B DIF: Medium REF: 2.4 OBJ: Identify the isotope that is likely to be the most abundant, given the masses of the isotopes and the average atomic mass. MSC: Understanding 32. Zinc has five naturally occurring isotopes with an average mass of 65.39 amu. Three isotopes, in roughly equal amounts, account for 95% of zinc. Which isotope is most abundant? a. 64Zn, 63.9291 amu d. 68Zn, 67.9249 amu b. 66Zn, 65.9260 amu e. 70Zn, 69.9253 amu 67 c. Zn, 66.9271 amu ANS: A DIF: Difficult REF: 2.4 OBJ: Identify the isotope that is likely to be the most abundant, given the masses of the isotopes and the average atomic mass. MSC: Understanding 33. The average atomic mass of zinc is 65.39 amu. Given the data in the following table, what is the natural abundance of 66Zn? Isotope 64 Zn 66 Zn 67 Zn 68 Zn 70 Zn Mass (amu) 63.9291 65.9260 66.9271 67.9249 69.9253 Natural Abundance (%) 48.89 ? 4.11 18.56 0.62 a. 27.83% b. 0.2783% c. 50.00% d. 2.783% e. 28.73% ANS: A DIF: Easy REF: 2.4 OBJ: Determine the abundance of an isotope given the average atomic mass, isotope masses, and abundances of the other isotopes. MSC: Applying 34. The mass of thallium (Tl) on the periodic table is given as 204.3833 without any units. There are 47 isotopes of thallium, but only two are stable and abundant, thallium-203, with a mass of 202.9723 amu, and thallium-205, with a mass of 204.9744 amu. What is the percentage of each of these isotopes in naturally occurring thallium? a. 29.5% 203Tl and 70.5% 205Tl d. 74.5% 203Tl and 25.5% 205Tl 203 205 b. 70.5% Tl and 29.5% Tl e. 32.5% 203Tl and 67.5% 205Tl 203 205 c. 25.5% Tl and 74.5% Tl ANS: A DIF: Medium REF: 2.4 OBJ: Determine the abundance of an isotope given the average atomic mass, isotope masses, and abundances of the other isotopes. MSC: Applying 35. Which statement regarding the organization of the periodic table is not correct? a. Mendeleev arranged known elements with similar chemical properties in columns. b. Mendeleev’s predictions of the chemical properties of unknown elements facilitated their discovery. c. Mendeleev arranged the elements in order of increasing atomic mass. d. The modern periodic table arranges elements in order of increasing atomic number. e. The elements go from gases to liquids to solids in order down the columns in Mendeleev’s periodic table. ANS: E DIF: Easy REF: 2.5 OBJ: Describe how Mendeleev’s early periodic table differs from the modern periodic table. MSC: Remembering 36. What is the symbol for silicon? a. S b. Sn c. Sr d. Se e. Si ANS: E DIF: Easy REF: 2.5 OBJ: Convert between the name and symbol of an element. 37. What is the symbol for magnesium? a. M b. Mg c. Mn d. Mo e. Ma ANS: B DIF: Easy REF: 2.5 OBJ: Convert between the name and symbol of an element. 38. He is the symbol for ________ a. hydrogen. b. hafnium. c. mercury. MSC: Remembering MSC: Remembering d. helium. e. holmium. ANS: D DIF: Easy REF: 2.5 OBJ: Convert between the name and symbol of an element. MSC: Remembering 39. Ca is the symbol for ________ a. cesium. b. cobalt. c. cadmium. d. calcium. e. cerium. ANS: D DIF: Easy REF: 2.5 OBJ: Convert between the name and symbol of an element. MSC: Remembering 40. The sixth period of the periodic table contains ________ elements. a. 18 d. 16 b. 32 e. 8 c. 24 ANS: B DIF: Medium REF: 2.5 OBJ: Write definitions of the terms period and group as used with the periodic table. MSC: Applying 41. Which of the following is an alkaline earth metal? a. K d. Cu b. Mg e. Na c. Al ANS: B DIF: Easy REF: 2.5 OBJ: Associate elements with the group to which they belong. 42. Elements 21–30 are known as ________ a. alkaline earths. b. chalcogens. c. halides. d. transition metals. e. rare earths. ANS: D DIF: Easy REF: 2.5 OBJ: Associate elements with the group to which they belong. 43. Cesium is an example of ________ a. an alkali metal. b. a transition metal. c. an alkaline earth metal. MSC: Remembering MSC: Remembering d. a halogen. e. a chalcogen. ANS: A DIF: Easy REF: 2.5 OBJ: Associate elements with the group to which they belong. MSC: Remembering 44. Elements in group 16 (VIA) are called ________ a. alkali metals. b. pnictogens. c. alkaline earth metals. d. halogens. e. chalcogens. ANS: E DIF: Easy REF: 2.5 OBJ: Associate elements with the group to which they belong. MSC: Remembering 45. Which letter below represents the halogen group? A B C D E a. A b. B c. C d. D e. E ANS: D DIF: Easy REF: 2.5 OBJ: Associate elements with the group to which they belong. MSC: Remembering 46. Which letter below represents the chalcogen group? A B a. A b. B c. C CD E d. D e. E ANS: C DIF: Easy REF: 2.5 OBJ: Associate elements with the group to which they belong. 47. Identify the letter of the group that contains the most metalloids. MSC: Remembering a. A b. B c. C d. D e. E ANS: B DIF: Easy REF: 2.5 OBJ: Associate elements with the group to which they belong. MSC: Remembering 48. Identify the letter of the group that contains the most nonmetals. a. A b. B c. C d. D e. E ANS: E DIF: Easy REF: 2.5 OBJ: Associate elements with the group to which they belong. MSC: Remembering 49. Elements in group 17 (VIIA) are called ________ a. alkali metals. d. halogens. b. pnictogens. e. chalcogens. c. alkaline earth metals. ANS: D DIF: Easy REF: 2.5 OBJ: Associate elements with the group to which they belong. 50. Which statement below is not correct? a. Oxygen is a chalcogen. b. Calcium is an alkaline earth metal. c. Silicon is a nonmetal. MSC: Remembering d. Sodium is an alkali metal. e. Bromine is a halogen. ANS: C DIF: Easy REF: 2.5 OBJ: Associate elements with the group to which they belong. MSC: Remembering 51. The elements below are used in fireworks. Which one is not classified correctly according to its position in the periodic table? a. Sodium is an alkali metal. d. Phosphorus is a nonmetal. b. Strontium is an alkaline earth metal. e. Sulfur is a metalloid. c. Iron is a transition metal. ANS: E DIF: Easy REF: 2.5 OBJ: Associate elements with the group to which they belong. 52. Silicon is best described as a ________ MSC: Remembering a. metalloid. b. metal. c. transition metal. d. noble gas. e. nonmetal. ANS: A DIF: Easy REF: 2.5 OBJ: Identify elements as metals, metalloids, and nonmetals, and describe the general differences among these three categories. MSC: Remembering 53. Potassium is best described as a ________ a. metalloid. b. metal. c. transition metal. d. noble gas. e. nonmetal. ANS: B DIF: Easy REF: 2.5 OBJ: Identify elements as metals, metalloids, and nonmetals, and describe the general differences among these three categories. MSC: Remembering 54. Oxygen is best described as a ________ a. metalloid. b. metal. c. transition metal. d. noble gas. e. nonmetal. ANS: E DIF: Easy REF: 2.5 OBJ: Identify elements as metals, metalloids, and nonmetals, and describe the general differences among these three categories. MSC: Remembering 55. Iron is best described as a(n) ________ a. metalloid. b. transition metal. c. chalcogen. d. alkaline earth metal. e. nonmetal. ANS: B DIF: Easy REF: 2.5 OBJ: Identify the transition metal elements. MSC: Remembering 56. Identify the statement regarding H2, He, and NH3 that is correct. a. H2 and He are chemical elements. d. All are chemical elements. b. Only He is a chemical element. e. All are chemical compounds. c. Only H2 is a chemical compound. ANS: A DIF: Easy REF: 2.6 OBJ: Distinguish between a chemical element and a chemical compound. MSC: Understanding 57. Which one of the following statements is not consistent with Dalton’s atomic view of matter? a. Atoms of one element can be converted into atoms of another element. b. Each element is composed of atoms that are identical in size, mass, and chemical properties. c. Compounds are formed from different atoms in simple whole number ratios. d. Atoms of different elements can combine in several different proportions to make different compounds. e. Matter is discrete, as proposed by Democritus. ANS: A DIF: Easy REF: 2.6 OBJ: State Dalton’s law of multiple proportions, explain its significance, and use it to determine combining ratios of elements in forming compounds. MSC: Understanding 58. Dalton’s law of multiple proportions deals with ________ a. the proportions of reacting chemicals that maximize the reaction rate. b. the total number of different compounds that can be made from two elements. c. the volumes of two elements that can combine to form two or more compounds. d. the relative masses of two elements that can combine to form two or more compounds. e. reactions that involve multiple steps. ANS: D DIF: Medium REF: 2.6 OBJ: State Dalton’s law of multiple proportions, explain its significance, and use it to determine combining ratios of elements in forming compounds. MSC: Understanding 59. Nitrogen and oxygen combine to form several different nitrogen oxides. In one case, 8.4 g of nitrogen reacted completely with 4.8 g of oxygen. In another case, 4.2 g of nitrogen reacted with 9.6 g of oxygen. Which pair of nitrogen oxides is consistent with these data? a. NO and N2O d. NO and N2O4 b. NO and NO2 e. N2O and N2O4 c. N2O and N2O5 ANS: E DIF: Difficult REF: 2.6 OBJ: State Dalton’s law of multiple proportions, explain its significance, and use it to determine combining ratios of elements in forming compounds. MSC: Applying 60. When 10.0 g of sulfur is combined with 10.0 g of oxygen, 20.0 g of sulfur dioxide is formed. What mass of oxygen would be required to convert 10.0 g of sulfur into sulfur trioxide? a. 5.0 g d. 30 g b. 10 g e. 20 g c. 15 g ANS: C DIF: Difficult REF: 2.6 OBJ: State Dalton’s law of multiple proportions, explain its significance, and use it to determine combining ratios of elements in forming compounds. MSC: Applying 61. How many atoms of each element are there in the compound Na3(PO4)3? a. sodium 3, phosphorus 3, oxygen 12 b. sodium 9, phosphorus 3, oxygen 12 c. sodium 3, phosphorus 1, oxygen 4 d. sodium 3, potassium 1, oxygen 4 e. sodium 9, potassium 3, oxygen 12 ANS: A DIF: Easy REF: 2.6 OBJ: Interpret a molecular formula (a.k.a. chemical formula) or drawing in terms of the number of atoms of each element in a molecule of the compound. MSC: Applying 62. Which one of the following is an anion? a. Na+ b. CO2 c. Cl− d. Na e. O3 ANS: C DIF: Easy REF: 2.6 OBJ: Distinguish between anions and cations. 63. Which one of the following is a cation? a. NO3− b. SO2 c. Ca2+ d. Na e. O2 MSC: Remembering ANS: C DIF: Easy REF: 2.6 OBJ: Distinguish between anions and cations. MSC: Remembering 64. What is the empirical formula for dioxane, C4H8O2? a. CHO d. CH2O b. C4H8O2 e. CHO2 c. C2H4O ANS: C DIF: Easy REF: 2.6 OBJ: Distinguish among molecular formulas, empirical formulas, and formula units. MSC: Applying 65. Locate each element in the periodic table and identify which statement is not correct. The common ion of ________ has ________ electrons and a charge of ________. a. Na; 10; +1 d. O; 10; −2 b. K; 18; +1 e. F; 10; −2 c. Mg; 10; +2 ANS: E DIF: Easy REF: 2.6 OBJ: Relate the number of electrons and charge for an atom or atomic ion to the atom’s position in the periodic table. MSC: Applying 66. Locate each element in the periodic table and identify which statement is not correct. The common ion of ________ has ________ electrons and a charge of ________. a. Cs; 55; +1 d. S; 18; −2 b. Ca; 18; +2 e. Cl; 18; −1 c. Ba; 54; +2 ANS: A DIF: Easy REF: 2.6 OBJ: Relate the number of electrons and charge for an atom or atomic ion to the atom’s position in the periodic table. MSC: Applying 67. Based on the element’s position in the periodic table, which statement below is not correct? a. The charge on an ion of sodium is 1+. b. The charge on an ion of magnesium is 2+. c. The charge on an ion of oxygen is 2−. d. The charge on an ion of chlorine is 1−. e. Ca2+ has more electrons than Ar. ANS: E DIF: Easy REF: 2.6 OBJ: Relate the number of electrons and charge for an atom or atomic ion to the atom’s position in the periodic table. MSC: Applying 68. Which element labeled A−E in the periodic table below will have an ionic charge of +2? a. A b. B c. C d. D e. E ANS: D DIF: Easy REF: 2.6 OBJ: Relate the number of electrons and charge for an atom or atomic ion to the atom’s position in the periodic table. MSC: Understanding 69. Which element labeled A–E in the periodic table below will have an ionic charge of +3? a. A b. B c. C d. D e. E ANS: B DIF: Easy REF: 2.6 OBJ: Relate the number of electrons and charge for an atom or atomic ion to the atom’s position in the periodic table. MSC: Understanding 70. Which element labeled A–E in the periodic table below will have an ionic charge of −2? a. A b. B c. C d. D e. E ANS: A DIF: Easy REF: 2.6 OBJ: Relate the number of electrons and charge for an atom or atomic ion to the atom’s position in the periodic table. MSC: Understanding 71. Which element labeled A–E in the periodic table below will have an ionic charge of −1? a. A b. B c. C d. D e. E ANS: E DIF: Easy REF: 2.6 OBJ: Relate the number of electrons and charge for an atom or atomic ion to the atom’s position in the periodic table. MSC: Understanding 72. Based on its position in the periodic table, which atom would you predict to form an ionic compound with two bromine atoms? a. sodium d. calcium b. aluminum e. carbon c. lithium ANS: D DIF: Easy REF: 2.6 OBJ: Identify combining ratios of atoms based on their positions in the periodic table. MSC: Applying 73. Based on its position in the periodic table, which atom would you predict to form a compound with one chlorine atom? a. boron d. calcium b. aluminum e. carbon c. lithium ANS: C DIF: Easy REF: 2.6 OBJ: Identify combining ratios of atoms based on their positions in the periodic table. MSC: Applying 74. Based on its position in the periodic table, which atom would you predict to form a compound with three lithium atoms? a. boron d. sulfur b. carbon e. fluorine c. nitrogen ANS: C DIF: Easy REF: 2.6 OBJ: Identify combining ratios of atoms based on their positions in the periodic table. MSC: Applying 75. What is the correct formula for the compound formed between sodium and iodine based on their positions in the periodic table? a. Na2I d. Na2I2 b. NaI2 e. Na3I c. NaI ANS: C DIF: Easy REF: 2.6 OBJ: Identify combining ratios of atoms based on their positions in the periodic table. MSC: Applying 76. What is the correct formula for the compound formed between potassium and phosphorus based on their positions in the periodic table? a. K2P d. K2P2 b. KP2 e. K3P c. KP ANS: E DIF: Easy REF: 2.6 OBJ: Identify combining ratios of atoms based on their positions in the periodic table. MSC: Applying 77. Which one of the following is an ionic compound? a. SO2 d. TiO2 b. ClO2 e. CO2 c. H2O ANS: D DIF: Easy REF: 2.6 OBJ: Characterize and classify a compound as molecular or ionic. MSC: Understanding 78. Which one of the following is a molecular compound? Molecular compounds also are known as covalent compounds. a. Na2O d. CCl4 b. CaO e. Fe2O3 c. FeO ANS: D DIF: Easy REF: 2.6 OBJ: Characterize and classify a compound as molecular or ionic. MSC: Understanding 79. Which of the following is most likely to exhibit covalent bonding? a. NaF d. CO2 b. CaCl2 e. NaCl c. Cs2O ANS: D DIF: Easy REF: 2.6 OBJ: Characterize and classify a compound as molecular or ionic. MSC: Understanding 80. Identify the binary compound that has ionic bonding. a. H2O d. CH4 b. NO e. CF4 c. LiF ANS: C DIF: Easy REF: 2.6 OBJ: Characterize and classify a compound as molecular or ionic. MSC: Understanding 81. Which of the following molecular compounds has an incorrect formula or is not named correctly? a. CCl4, carbon tetrachloride d. NO2, nitrogen dioxide b. P2N5, phosphorus pentanitride e. SO, sulfur monoxide c. SF6, sulfur hexafluoride ANS: B DIF: Easy REF: 2.7 OBJ: Convert between the name and formula of a binary molecular compound. MSC: Applying 82. Name the following oxides of nitrogen in this sequence: NO, N2O, NO2, N2O4. a. nitrogen monoxide, dinitrogen monoxide, nitrogen dioxide, dinitrogen tetroxide b. nitrox, dinitrox, nitridiox, dinitritetrox c. mononitrogen monoxide, dinitrogen monoxide, mononitrogen dioxide, dinitrogen tetraoxide d. nitrogen oxide, nitrogen(II) oxide, nitrogen oxide(II), nitrogen(II) oxide(IV) e. nitrous oxide, nitric oxide, nitrogen dioxide, nitrogen tetraoxide ANS: A DIF: Easy REF: 2.7 OBJ: Convert between the name and formula of a binary molecular compound. MSC: Applying 83. Which one of these formula–name combinations is not correct? a. diphosphorus tetroxide: P2O4 b. tetraphosphorus nonoxide: P4O9 c. diphosphorus pentoxide: P2O5 d. tetraphosphorus heptoxide: P4O6 e. phosphorus monoxide: PO ANS: D DIF: Medium REF: 2.7 OBJ: Convert between the name and formula of a binary molecular compound. MSC: Applying 84. Active metals often form a protective oxide surface film that prevents further reaction of the metal with oxygen in the air. Which one of the following formulas for the metal oxide is not correct? a. Al2O3 is aluminum oxide. d. MgO2 is magnesium oxide. b. Fe2O3 is iron(III) oxide. e. FeO is iron(II) oxide. c. Na2O is sodium oxide. ANS: D DIF: Easy REF: 2.7 OBJ: Convert between the name and formula of a binary ionic compound. MSC: Applying 85. What is the formula for calcium nitride? a. CaN b. Ca2N3 c. Ca2N d. Ca3N2 e. CaN2 ANS: D DIF: Easy REF: 2.7 OBJ: Convert between the name and formula of a binary ionic compound. MSC: Applying 86. Zinc oxide is found in ointments for the skin. What formula best describes this compound, which has Zn as a doubly charged cation? a. ZnO d. Zn2O2 b. Zn2O e. Zn2O3 c. ZnO2 ANS: A DIF: Medium REF: 2.7 OBJ: Convert between the name and formula of a binary ionic compound. MSC: Applying 87. Titanium forms different ionic oxides. One, TiO2, is a white oxide used in paints. What is the proper name for TiO2? a. titanium oxide d. titanium oxide(II) b. titanium(IV) oxide e. titanium dioxide c. titanium(II) oxide ANS: B DIF: Easy REF: 2.7 OBJ: Convert between the name and formula of transition metal compounds. MSC: Applying 88. Manganese(IV) oxide is a brown insoluble solid often found as a product of reactions of potassium permanganate. What is the formula of manganese(IV) oxide? a. Mn4O d. MnO2 b. MnO4 e. Mn2O2 c. MnO ANS: D DIF: Easy REF: 2.7 OBJ: Convert between the name and formula of transition metal compounds. MSC: Applying 89. What is the correct name for FeCl3? a. iron(III) chloride b. iron trichloride c. ferrum trichloride d. ferric trichloride e. iron chloride ANS: A DIF: Medium REF: 2.7 OBJ: Convert between the name and formula of transition metal compounds. MSC: Applying 90. Which one of the following ionic compounds has an incorrect formula or is not named correctly? a. CoO, cobalt oxide d. Cu2S, copper(I) sulfide b. Co2O3, cobalt(III) oxide e. MgS, magnesium sulfide c. CoO2, cobalt(IV) oxide ANS: A DIF: Medium REF: 2.7 OBJ: Convert between the name and formula of transition metal compounds. MSC: Applying 91. Which anion is not labeled correctly? a. NO2− nitrite b. SO42− sulfate c. Br− bromide d. SO32− sulfite e. All are labeled correctly. ANS: E DIF: Easy REF: 2.7 OBJ: Convert between the name and the chemical formula of compounds with a polyatomic ion. MSC: Remembering 92. Which polyatomic ion is not labeled correctly? a. NH4+ ammonium d. NO3− nitrate − b. ClO4 perchlorate e. All are labeled correctly. − c. CN cyanate ANS: C DIF: Medium REF: 2.7 OBJ: Convert between the name and the chemical formula of compounds with a polyatomic ion. MSC: Remembering 93. Based on its position in the periodic table, which single atom would you predict to form a compound with two nitrate polyatomic ions? a. boron d. calcium b. aluminum e. carbon c. lithium ANS: D DIF: Easy REF: 2.7 OBJ: Convert between the name and the chemical formula of compounds with a polyatomic ion. MSC: Applying 94. Based on its position in the periodic table, which single atom would you predict to form a compound with two ammonium ions? a. boron d. sulfur b. carbon e. fluorine c. nitrogen ANS: D DIF: Easy REF: 2.7 OBJ: Convert between the name and the chemical formula of compounds with a polyatomic ion. MSC: Applying 95. Sodium nitrite, which is used in meat processing, has been implicated as a possible health hazard because it can react with amines present in meat to form trace quantities of carcinogenic nitrosamines. What is the formula of sodium nitrite? a. Na2NO3 d. Na2NO4 b. NaNO2 e. Na2NO2 c. NaNO3 ANS: B DIF: Easy REF: 2.7 OBJ: Convert between the name and the chemical formula of compounds with a polyatomic ion. MSC: Applying 96. The formula for a terbium phosphate compound is Tb3(PO4)4. What would be the formula for a terbium sulfate compound given that the charge of terbium is the same in both compounds? a. Tb2(SO3)3 d. Tb3(SO4)4 b. Tb(SO4)2 e. Tb(SO4)3 c. Tb(SO3)2 ANS: B DIF: Medium REF: 2.7 OBJ: Convert between the name and the chemical formula of compounds with a polyatomic ion. MSC: Applying 97. The formula for a lutetium carbonate compound is Lu2(CO3)3. What would be the formula for a lutetium nitrate compound given that the charge of lutetium is the same in both compounds? a. LuNO3 d. Lu2NO3 b. Lu(NO3)2 e. Lu2(NO3)3 c. Lu(NO3)3 ANS: C DIF: Medium REF: 2.7 OBJ: Convert between the name and the chemical formula of compounds with a polyatomic ion. MSC: Applying 98. Copper(II) sulfate is a common fungicide. What is the correct formula for copper(II) sulfate? a. CoSO4 d. CuSO3 b. CuSO4 e. Cu2SO4 c. Cu(SO3)2 ANS: B DIF: Medium REF: 2.7 OBJ: Convert between the name and the chemical formula of compounds with a polyatomic ion. MSC: Applying 99. Radium often is found in uranium ores and can be separated from solutions by precipitation as radium sulfate. What is the formula for radium sulfate? a. RnSO4 d. Ra2SO4 b. RaSO4 e. Ra(SO4)2 c. Rn2SO3 ANS: B DIF: Medium REF: 2.7 OBJ: Convert between the name and the chemical formula of compounds with a polyatomic ion. MSC: Applying 100. What is the correct name for Ni(NO2)2? a. nickel dinitrate b. nickelous nitrite c. nickel(II) dinitrate d. nickel(II) nitrite e. nickel(II) nitrate ANS: D DIF: Difficult REF: 2.7 OBJ: Convert between the name and the chemical formula of compounds with a polyatomic ion. MSC: Applying 101. Buffer solutions that maintain certain levels of pH or acidity are widely used in biochemical experiments. One common buffer system uses sodium dihydrogenphosphate and sodium monohydrogenphosphate. What are the formulas of these two compounds? a. Na(HPO4) and Na(HPO4)2 b. NaH2PO4 and Na2HPO4 c. Na2H2PO4 and NaHPO4 d. NaPO4 and NaHPO4 e. Na2(HPO4)2 and Na2(HPO4) ANS: B DIF: Medium REF: 2.7 OBJ: Convert between name and formula of compounds containing a polyatomic ion. MSC: Applying 102. The following salts are used in fireworks. Which one has an incorrect formula or is not named correctly? a. Li2CO3, lithium carbonate d. CuO, copper(II) oxide b. CaSO4, calcium sulfate e. NH4Cl, ammonium chloride c. BaNO3, barium nitrate ANS: C DIF: Easy REF: 2.7 OBJ: Convert between name and formula of compounds containing a polyatomic ion. MSC: Applying 103. Sulfur combines with oxygen and hydrogen to form two acids. Sulfuric acid has the formula ________, and sulfurous acid has the formula ________. a. H2SO4; H2SO3 d. HSO3; HSO4 b. H2SO3; H2SO4 e. H2SO3; H2SO2 c. HSO4; HSO3 ANS: A DIF: Easy REF: 2.7 OBJ: Convert between the name and the chemical formula of an acid. MSC: Applying 104. Aqua regia is a mixture of hydrochloric acid and nitric acid that is capable of dissolving gold. What are the formulas of these acids? a. HClO, HNO4 d. HCl, HNO3 b. HClO4, HNO3 e. HCl, HNO c. HCl, HNO2 ANS: D DIF: Medium REF: 2.7 OBJ: Convert between the name and the chemical formula of an acid. MSC: Applying 105. Which one of the oxoacid formulas and names is not correctly matched? a. H2SO3 sulfurous acid d. HNO3 nitric acid b. HCl hydrochloric acid e. All are correct. c. H2SO4 sulfuric acid ANS: E DIF: Medium REF: 2.7 OBJ: Convert between the name and the chemical formula of an acid. MSC: Remembering 106. Which one of the following acids has an incorrect formula or is not named correctly? a. HI, hydroiodic acid d. H2SO3, sulfuric acid b. H2CO3, carbonic acid e. H3PO4, phosphoric acid c. HNO3, nitric acid ANS: D DIF: Medium REF: 2.7 OBJ: Convert between the name and the chemical formula of an acid. MSC: Remembering 107. Which one of the following acids has an incorrect formula or is not named correctly? a. HCl, hydrochloric acid d. H2CO3, carbonic acid b. HF, hydrofluoric acid e. H2SO4, sulfuric acid c. HNO2, nitric acid ANS: C DIF: Medium REF: 2.7 OBJ: Convert between the name and the chemical formula of an acid. MSC: Remembering 108. Which one of the following acids is not named correctly? a. H2SO3, sulfurous acid d. HBr, hydrobromic acid b. H2S, hydrosulfuric acid e. HNO3, nitric acid c. H3PO3, phosphoric acid ANS: C DIF: Medium REF: 2.7 OBJ: Convert between the name and the chemical formula of an acid. MSC: Remembering 109. Hypochlorous acid has the formula ________ a. HClO4. d. HClO. b. HClO3. e. H2ClO2. c. HClO2. ANS: D DIF: Easy REF: 2.7 OBJ: Convert between the name and the chemical formula of an acid. MSC: Remembering 110. According to the Big Bang theory, which statement about the origin of the elements is not correct? a. Initially, energy was transformed into electrons and other elementary particles. b. As the universe cooled, neutrons and protons were formed. c. Collisions of neutrons and protons produced deuterons, which then led to the formation of alpha particles. d. The nuclides of the elements were formed by nuclear reactions in the interior of stars. e. These nuclear reactions all require the addition of energy to form the elements. ANS: E DIF: Medium REF: 2.9 OBJ: Describe the sequence of events that is part of the Big Bang theory. MSC: Remembering 111. A supernova event is the explosion caused by the collapse of a dying star that has run out of its nuclear fuel. These stars and events are responsible for ________ a. the production of elements heavier than iron-56. b. nuclear fission of heavy elements. c. the distribution of heavy elements throughout the universe. d. both a and c. e. both b and c. ANS: D DIF: Medium REF: 2.9 OBJ: Describe the sequence of events that is part of the Big Bang theory. MSC: Remembering 112. Quarks ________ a. were initially formed along with electrons microseconds after the Big Bang. b. combined as the universe cooled to form protons and neutrons. c. are the primary particle involved in nucleosynthesis. d. both a and b. e. both b and c. ANS: D DIF: Medium REF: 2.9 OBJ: Describe the sequence of events that is part of the Big Bang theory. MSC: Remembering 113. The emission of a  particle is associated with the ________ a. conversion of a neutron to a proton. b. conversion of a proton to a neutron. c. increase in mass number. d. decrease in mass number. e. formation of an isotope. ANS: A DIF: Medium REF: 2.9 OBJ: Identify reactants and products in nucleosynthesis. MSC: Remembering 114. Heavy elements in the universe are formed by ________ a. fission reactions of hydrogen nuclei. b. quark formation. c. supernova explosions. d. star collapse into black holes. e. fusion reactions of iron nuclei. ANS: E DIF: Medium REF: 2.9 OBJ: Identify reactants and products in nucleosynthesis. MSC: Remembering 115. What is the correct symbol for an alpha particle? a. d. b. e. c. ANS: D DIF: Medium REF: 2.9 OBJ: Identify reactants and products in nucleosynthesis. MSC: Remembering 116. Which stellar nuclear reaction is not correctly written? a. d. b. e. c. ANS: C DIF: Easy REF: 2.9 OBJ: Write nuclear reaction equations that describe nucleosynthesis. MSC: Applying SHORT ANSWER 1. In one sentence, describe the picture of the atom that emerged from the Rutherford–Geiger–Marsden experiment with alpha particles. ANS: The atom was pictured as consisting of a tiny, positively charged nucleus surrounded by a diffuse cloud of negatively charged electrons. DIF: Easy REF: 2.2 OBJ: Describe the evidence obtained from the Rutherford–Geiger–Marsden experiment with alpha particles and how it rejected the plum-pudding model and led to the nuclear model of atomic structure. MSC: Remembering 2. What distinguishes one isotope from another? ANS: Isotopes have the same number of protons but different numbers of neutrons. DIF: Easy REF: 2.3 OBJ: Write a definition of the term isotope, and identify the feature that distinguishes one isotope from another. MSC: Applying 3. Provide the number of protons, neutrons, and electrons in a silicon-29 isotope. ANS: 14 protons, 15 neutrons, and 14 electrons DIF: Easy REF: 2.3 OBJ: Convert between an atomic symbol and the number of protons, neutrons, nucleons, and electrons comprising an ion. MSC: Applying 4. Write the complete atomic symbol with both a superscript and a subscript for a sodium ion that contains 11 protons, 10 electrons, and 12 neutrons. ANS: DIF: Easy REF: 2.3 OBJ: Convert between an atomic symbol and the number of protons, neutrons, nucleons, and electrons comprising an ion. MSC: Applying 5. Nuclear reactors used for power generation require uranium enriched in uranium-235. What is the average atomic mass of enriched uranium consisting of exactly 3.0% uranium-235 (235.04 amu) and 97.0% uranium-238 (238.05 amu)? ANS: 237.96 amu DIF: Medium REF: 2.4 OBJ: Use natural abundance data for isotopes to calculate an average atomic mass. MSC: Applying 6. Boron, which has an average atomic mass of 10.81 amu, has two stable isotopes: boron-10 (19.78%) and boron-11 (80.22%). Boron-10 has an atomic mass of 10.0129 amu; what is the atomic mass of boron-11? ANS: 11.01 amu DIF: Medium REF: 2.4 OBJ: Determine the mass of an isotope from the average atomic mass and natural abundances of other isotopes. MSC: Applying 7. Give an example of an alkali metal. ANS: Sodium; answers will vary. DIF: Easy REF: 2.5 OBJ: Associate elements with the group to which they belong. MSC: Remembering 8. Give an example of an alkaline earth metal. ANS: Calcium; answers will vary. DIF: Easy REF: 2.5 OBJ: Associate elements with the group to which they belong. MSC: Remembering 9. Give an example of a halogen. ANS: Bromine; answers will vary. DIF: Easy REF: 2.5 OBJ: Associate elements with the group to which they belong. MSC: Remembering 10. Give an example of a nonmetal. ANS: Sulfur; answers will vary. DIF: Easy REF: 2.5 OBJ: Identify elements as metals, metalloids, and nonmetals, and describe the general differences among these three categories. MSC: Remembering 11. Give an example of a metalloid (a.k.a semimetal). ANS: Silicon; answers will vary. DIF: Easy REF: 2.5 OBJ: Identify elements as metals, metalloids, and nonmetals, and describe the general differences among these three categories. MSC: Remembering 12. Give an example of a transition metal. ANS: Iron; answers will vary. DIF: Easy REF: 2.5 OBJ: Identify the transition metal elements. MSC: Remembering 13. Identify the letter that corresponds to each of the following groups of the periodic table: a) chalcogens b) noble gases c) alkaline earth metals d) halogens ANS: a) C b) E c) B d) D DIF: Easy REF: 2.5 OBJ: Associate elements with the group to which they belong. MSC: Remembering 14. Label the highlighted regions of the periodic table. ANS: a) alkali metals, b) transition metals, c) main group elements/p block, and d) lanthanide and actinides DIF: Easy REF: 2.5 OBJ: Associate elements with the group to which they belong. MSC: Remembering 15. Nitrogen and oxygen combine to form several different nitrogen oxides. Chemical analysis found that the N:O mass ratio in NO is 0.875. Two other nitrogen oxides were produced by reacting 8.4 g of nitrogen completely with 4.8 g of oxygen in one case and in another case by reacting 4.2 g of nitrogen with 9.6 g of oxygen. What are the empirical formulas of these two nitrogen oxides? ANS: N2O and NO2 DIF: Difficult REF: 2.6 OBJ: State Dalton’s law of multiple proportions, explain its significance, and use it to determine combining ratios of elements in forming compounds. MSC: Applying 16. A cation has a ________ charge, and an anion has a ________ charge. ANS: positive ; negative DIF: Easy REF: 2.6 MSC: Remembering OBJ: Distinguish between anions and cations. 17. Give an example of a molecular compound (a.k.a. a covalent compound). ANS: Carbon dioxide, CO2; answers will vary. DIF: Easy REF: 2.6 OBJ: Characterize and classify a compound as molecular or ionic. MSC: Applying 18. Give an example of an ionic compound. ANS: Sodium chloride, NaCl; answers will vary. DIF: Easy REF: 2.6 OBJ: Characterize and classify a compound as molecular or ionic. MSC: Applying 19. Identify each of the following compounds as molecular or ionic: a) NO3 b) CaCl2 c) Cu(NO3)2 d) CH3OH. ANS: a) molecular b) ionic c) ionic d) molecular DIF: Easy REF: 2.6 OBJ: Characterize and classify a compound as molecular or ionic. MSC: Applying 20. What is the chemical formula for hexasulfur monoxide? ANS: S6O DIF: Easy REF: 2.7 OBJ: Convert between the name and formula of a binary molecular compound. MSC: Applying 21. What is the chemical formula for dinitrogen tetroxide? ANS: N2O4 DIF: Easy REF: 2.7 OBJ: Convert between the name and formula of a binary molecular compound. MSC: Applying 22. What is the correct name for SO3? ANS: Sulfur trioxide DIF: Easy REF: 2.7 OBJ: Convert between the name and formula of a binary molecular compound. MSC: Applying 23. What is the correct name for PCl5? ANS: Phosphorus pentachloride DIF: Easy REF: 2.7 OBJ: Convert between the name and formula of a binary molecular compound. MSC: Applying 24. What is the chemical formula for manganese(IV) oxide? ANS: MnO2 DIF: Medium REF: 2.7 OBJ: Convert between the name and formula of transition metal compounds. MSC: Applying 25. What is the chemical formula for potassium sulfite? ANS: K2SO3 DIF: Easy REF: 2.7 OBJ: Convert between the name and formula of compounds with a polyatomic ion. MSC: Applying 26. What is the chemical formula for calcium nitrite? ANS: Ca(NO2)2 DIF: Easy REF: 2.7 OBJ: Convert between the name and formula of compounds with a polyatomic ion. MSC: Applying 27. What is the correct name for CuCl2? ANS: Copper(II) chloride DIF: Medium REF: 2.7 OBJ: Convert between the name and formula of transition metal compounds. MSC: Applying 28. What is the correct name for PbS2? ANS: Lead(IV) sulfide DIF: Medium REF: 2.7 OBJ: Convert between the name and formula of ionic compounds. MSC: Applying 29. What is the correct name for the acid HNO2? ANS: Nitrous acid DIF: Medium REF: 2.7 OBJ: Convert between the name and the chemical formula of an acid. MSC: Applying 30. What is the chemical formula for hypochlorous acid? ANS: HClO DIF: Medium REF: 2.7 OBJ: Convert between the name and the chemical formula of an acid. MSC: Applying 31. What is the chemical formula for hydroselenic acid? ANS: H2Se DIF: Medium REF: 2.7 OBJ: Convert between the name and the chemical formula of an acid. MSC: Applying