Test Bank for Chemistry: An Atoms-Focused Approach, 2nd Edition

Test Bank Chemistry: An Atoms-­Focused Approach second edition Test Bank Chemistry: An Atoms-­Focused Approach second edition Thomas R. Gilbert, Rein V. Kirss, Natalie Foster Daniel Autrey fayetteville state University Scott Reid marquette University Bn W • W • Norton & Company • New York • London W. W. Norton & Company has been in­de­pen­dent since its founding in 1923, when William Warder Norton and Mary D. Herter Norton first published lectures delivered at the People’s Institute, the adult education division of New York City’s Cooper ­Union. The Nortons soon expanded their program beyond the Institute, publishing books by celebrated academics from America and abroad. By mid-­century, the two major pillars of Norton’s publishing program—trade books and college texts—­were firmly established. In the 1950s, the Norton family transferred control of the company to its employees, and today—with a staff of four hundred and a comparable number of trade, college, and professional titles published each year—W. W. Norton & Company stands as the largest and oldest publishing ­house owned wholly by its employees. Copyright © 2017 by W. W. Norton & Company, Inc. All rights reserved. Media Editor: Chris Rapp Associate Media Editors: Julia Sammaritano and Michael Jaoui Production Manager: Eric Pier-­Hocking Media Editorial Assistant: Doris Chiu Composition by Westchester Publishing Ser­vices W. W. Norton & Company, Inc., 500 Fifth Avenue, New York, NY 10110 wwnorton.com W. W. Norton & Company Ltd., Castle ­House, 75/76 Wells Street, London W1T 3QT 1 2 3 4 5 6 7 8 9 0 Contents Preface vii Chapter 1 | Matter and Energy—An Atomic Perspective 1 Chapter 2 | Atoms, Ions, and Molecules—The Building Blocks of Matter 42 Chapter 3 | Atomic Structure—Explaining the Properties of Elements 76 Chapter 4 | Chemical Bonding—Understanding Climate Change 120 Chapter 5 | Bonding Theories—Explaining Molecular Geometry 168 Chapter 6 | Intermolecular Forces—Attractions between Particles 216 Chapter 7 | Stoichiometry—Mass Relationships and Chemical Reactions 255 Chapter 8 | Aqueous Solutions—Chemistry of the Hydrosphere 297 Chapter 9 | Thermochemistry—Energy Changes in Chemical Reactions 350 Chapter 10 | Properties of Gases—The Air We Breathe 414 Chapter 11 | Properties of Solutions—Their Concentrations and Colligative Properties 469 Chapter 12 | Thermodynamics—Why Chemical Reactions Happen 510 Chapter 13 | Chemical Kinetics—Clearing the Air 554 Chapter 14 | Chemical Equilibrium—Equal but Opposite Reaction Rates 637 Chapter 15 | Acid-­Base Equilibria—­Proton Transfer in Biological Systems 682 Chapter 16 | Additional Aqueous Equilibria—­Chemistry and the Oceans 717 Chapter 17 | Electrochemistry—The Quest for Clean Energy 754 Chapter 18 | The Solid State—A Particulate View 812 Chapter 19 | Organic Chemistry—Fuels, Pharmaceuticals, and Modern Materials 856 Chapter 20 | Biochemistry—­The Compounds of Life 913 Chapter 21 | Nuclear Chemistry—­The Risks and Benefits 970 Chapter 22 | The Main Group Ele­ments—­Life and the Periodic ­Table 1012 Chapter 23 | Transition Metals—­Biological and Medical Applications 1040 v Preface How Does It Work? The Test Bank author listed the learning objectives from each chapter believed to be the most important for students to learn. The author then developed questions designed to test students’ knowledge of a par­tic­u­lar learning objective. By asking students questions that vary in both type and level of difficulty, instructors can gather different types of evidence, which will allow them to more effectively assess how well students understand specific concepts. Six Question Types: 1. Remembering questions—test declarative knowledge, including textbook definitions and relationships between two or more pieces of information. Can students recall or remember the information in the same form it was learned? 2. Understanding questions—pose problems in a context different from the one in which the material was learned, requiring students to draw from their declarative and/or procedural understanding of important concepts. Can students explain ideas or concepts? 3. Applying questions—ask students to draw from their prior experience and use critical-­thinking skills to take part in qualitative reasoning about the real world. Can students use learned information in another task or situation? 4. Analyzing questions—test students’ ability to break down information and see how different elements relate to each other and to the ­whole. Can students distinguish among the different parts? 5. Evaluating questions—ask students to assess information as a ­whole and frame their own argument. Can students justify a stand or decision? 6. Creating questions—pose questions or objectives that prompt students to put elements they have learned together into a coherent ­whole to generate new ideas. Can students create a new product or point of view based on data? Three Difficulty Levels: 1. Easy questions—require a basic understanding of the concepts, definitions, and examples. 2. Moderate questions—direct students to use critical-­ thinking skills, to demonstrate an understanding of core concepts in­de­pen­dent of specific textbook examples, and to connect concepts across chapters. 3. Difficult questions—ask students to synthesize textbook concepts with their own experience, making analytical inferences about biological topics and more. Each question mea­sures and explicitly links to a specific competency and is written with clear, concise, and grammatically correct language that suits the difficulty level of the specific competency being assessed. To ensure the validity of the questions, no extraneous, ambiguous, or confusing material is included, and no slang expressions are used. In developing the questions, every effort has been made to eliminate bias (e.g., race, gender, cultural, ethnic, regional, handicap, age) to require specific knowledge of material studied, not of general knowledge or experience. This ensures accessibility and validity. Key to the Question Meta-­Data Each question in the Test Bank is tagged with five pieces of information designed to help instructors create the most ideal mix of questions for a quiz or exam. These tags are: vii viii | Preface ANS: This is the correct answer for each question. Or, in the case of some short-­answer questions, a possible correct answer to the given question. DIF: This is the difficulty assigned to the problem. Problems have been classified as Easy, Medium, or Difficult. REF: This is the section in the textbook from which a question is drawn. OBJ: This is the learning objective that the question is designed to test. MSC: This is the knowledge type (see above) the question is designed to test. Chapter 1: ­Matter and Energy—­An Atomic Perspective Learning Objectives Describe what is meant by the term scientific theory and distinguish it from natu­ral philosophy. Describe how temperature affects the properties of ­ atter. m Distinguish between ele­ments and compounds. Describe the pro­cesses of sublimation, melting, vaporization, condensation, freezing, and deposition. Describe the scientific method and define a law, a theory, and a hypothesis. Define energy, work, and heat. Describe the law of definite proportions. Distinguish between potential and kinetic energy. Describe the law of constant composition. State the law of conservation of energy. Describe the law of multiple proportions. Recognize and interpret the dif­fer­ent ways of representing molecules (diatomic, molecular formula, structural formula, condensed structural formula, ball-­and-­stick, space-­filling). Write chemical formulas from the ratios of the ele­ments in a compound. Describe and apply the COAST method. Describe ionic compounds and identify an empirical formula. Distinguish between pure substances and mixtures. Describe SI and US mea­sure­ments. Define ­matter and mass. Distinguish between exact and uncertain values. Describe and give examples of extensive and intensive properties. Distinguish between precision and accuracy. Describe and give examples of chemical and physical properties. Apply the rules for significant figures (weak-­link princi­ple). Use density in calculations. Use the unit-­factor method to convert mea­sure­ments. Distinguish between molecules and ions. Distinguish between and convert Fahrenheit, Celsius, and Kelvin temperatures. Distinguish between physical and chemical changes. Describe the function of a control sample. Distinguish between homogeneous and heterogeneous mixtures. Describe the methods that can be used to separate the components of a mixture: distillation, filtration, and chromatography. For a data set, calculate the mean, standard deviation, and confidence interval. Use Grubb’s test to determine if a data point is an outlier. Distinguish between the states of ­matter: solid, liquid, and gas. 1 • Chapter 1 Chapter 1: Matter and Energy—An Atomic Perspective MULTIPLE CHOICE 1. Which step is NOT a part of the scientific method? a. Form a testable hypothesis. b. Make observations. c. Conduct reproducible experiments. d. Identify different factors that affect results. e. Stop experimentation once the desired results are achieved. ANS: E DIF: Easy REF: 1.1 OBJ: Describe the scientific method and define a law, a theory, and a hypothesis. MSC: Remembering 2. For a hypothesis to be considered a valid scientific theory, it must ________ a. summarize experimental data without trying to predict future results. b. be impossible to prove wrong by experiment. c. explain widely observed phenomena based on extensive testing. d. never be modified or expanded. e. be voted on by the scientific community and accepted by all. ANS: C DIF: Easy REF: 1.1 OBJ: Describe the scientific method and define a law, a theory, and a hypothesis. MSC: Understanding 3. According to the law of definite proportions, ________ a. atoms forming a given compound react in variable proportions depending on conditions. b. different samples of the same compound contain the same proportions of the same elements. c. all compounds containing the same types of atoms have identical properties. d. all compounds containing the same types of atoms have relative masses that are whole-number multiples. e. only one type of molecule can be produced when two elements combine. ANS: B DIF: Easy REF: 1.1 OBJ: Describe the law of definite proportions. MSC: Understanding 4. The law of definite proportions states that ________ a. compounds such as NO and NO2 have identical chemical properties. b. compounds such as NO and NO2 must have masses that are whole-number multiples of each other. c. nitrogen and oxygen can combine to form a variety of compounds, such as NO or NO2. d. the elements forming a given compound always react in the same proportions. e. only one compound can be produced when two elements combine. ANS: D DIF: Easy REF: 1.1 OBJ: Describe the law of definite proportions. 1 2 • Chapter 1 MSC: Understanding 5. Which one of the following is a hypothesis? a. Energy is required to vaporize a liquid. b. The composition of a pure substance is fixed and definite. c. Hydrogen gas and oxygen gas can react to form water. d. A Car’s battery must be dead because the car won’t start. e. Matter is composed of atoms. ANS: D DIF: Moderate REF: 1.1 OBJ: Describe the scientific method and define a law, a theory, and a hypothesis. MSC: Applying 6. Which of the following illustrates the law of multiple proportions? a. The mass ratio of O to N in NO2 is twice that in NO. b. NO2 always contains one nitrogen atom and two oxygen atoms. c. The mass of NO2 is a small whole-number multiple of the mass of NO. d. NO and NO2 have similar chemical and physical properties. e. NO2 and N2O4 are the same compound. ANS: A DIF: Moderate REF: 1.1 OBJ: Describe the law of multiple proportions. MSC: Understanding 7. Which of the following does NOT illustrate the law of multiple proportions? a. The N-to-O mass ratio in NO is 0.875, whereas that in N2O is 1.75. b. C2H2 has a 12:1 C-to-H mass ratio, while C2H6 has a 4:1 C-to-H mass ratio. c. The ratio of O:C by mass in CO2 is twice that of CO. d. If a sample of H2O contains 16 g of oxygen, a sample of H2O2 with the same number of molecules would contain 32 g of oxygen. e. H2S and H2O contain the same mass of hydrogen. ANS: E DIF: Difficult REF: 1.1 OBJ: Describe the law of multiple proportions. MSC: Applying 8. Which of the following statements is NOT true? a. The relative numbers of each type of atom in a given compound do not vary. b. A compound always contains the same mass percentages of its constituent elements. c. A large sample and a small sample of a given compound contain the same number of each type of atom. d. A large sample and a small sample of a given compound contain the same types of atoms combined in the same proportions. e. A large sample and a small sample of a compound share the same chemical formula. ANS: C DIF: Difficult REF: 1.1 OBJ: Describe the law of constant composition. 2 3 • Chapter 1 MSC: Analyzing 9. Which of the following statements is NOT true? a. Given that the chemical formula of methanol is CH4O, the number of carbon atoms in a sample of methanol will be the same as the number of oxygen atoms. b. If a compound is 75% carbon and 25% hydrogen by mass, 12 g of the compound contains 9 g C and 3 g H. c. If a compound contains 76 g of chlorine and 12 g of carbon, it will always have a 6.33:1 mass ratio of Cl to C. d. A compound containing 17.1 g of phosphorus and 58.9 g of chlorine has the same identity as a compound containing 35.7 g P and 204.3 g Cl. e. A compound containing 106.6 g of copper and 13.4 g of oxygen has the same identity as a compound containing 159.9 g Cu and 20.1 g O. ANS: D DIF: Difficult REF: 1.1 OBJ: Describe the law of constant composition. MSC: Evaluating 10. A pure substance ________ a. must be composed of atoms of the same type. b. cannot be separated into simpler substances by physical means. c. must be a compound. d. has different chemical properties depending on its source. e. can have a composition that varies from sample to sample. ANS: B DIF: Easy REF: 1.3 OBJ: Distinguish between pure substances and mixtures. 11. Which of the following is NOT a pure substance? a. sparkling water d. b. gold metal e. c. oxygen gas water vapor dry ice (solid CO2) ANS: A DIF: Easy REF: 1.3 OBJ: Distinguish between pure substances and mixtures. 12. Which of the following is a pure substance? a. seawater b. blood c. brass (an alloy of copper and zinc) d. e. MSC: Remembering MSC: Understanding table sugar(sucrose, C12H22O11) beer ANS: D DIF: Easy REF: 1.3 OBJ: Distinguish between pure substances and mixtures. MSC: Understanding 13. A molecule ________ a. must contain at least two types of atoms. b. can be an element or a compound. c. cannot form a solid. d. cannot be broken into its constituent atoms by any means. e. can contain only one type of atom. ANS: B DIF: Easy REF: 1.3 OBJ: Distinguish between elements and compounds. 3 4 • Chapter 1 MSC: Remembering 14. A sample of a compound ________ a. breaks into its constituent atoms during phase changes. b. is a homogeneous mixture. c. contains atoms that can be physically separated from each other. d. contains at least two types of atoms in a constant, fixed ratio. e. has a variable composition depending on its temperature. ANS: D DIF: Easy REF: 1.3 OBJ: Distinguish between elements and compounds. 15. Which of the following is an element? a. C6H12O6 b. HNO3 c. NaCl d. e. CH4 O3 ANS: E DIF: Easy REF: 1.3 OBJ: Distinguish between elements and compounds. 16. Which of the following is NOT an element? a. Cs b. Au c. CS2 d. e. MSC: Remembering MSC: Understanding Ar Co ANS: C DIF: Easy REF: 1.3 OBJ: Distinguish between elements and compounds. MSC: Understanding 17. An element ________ a. can be separated into its components by physical methods. b. has different chemical properties depending on its state. c. cannot be separated into simpler substances by chemical methods. d. can also be a compound. e. exists only as atoms, not as molecules. ANS: C DIF: Easy REF: 1.3 OBJ: Distinguish between elements and compounds. MSC: Understanding 18. Table sugar (sucrose, C12H22O11) dissolves in water. This process ________ a. is a chemical change. b. is a physical change. c. produces a heterogeneous mixture. d. is a chemical property of sucrose. e. converts sucrose to carbon dioxide and water. ANS: B DIF: Easy REF: 1.3 OBJ: Distinguish between physical and chemical changes. 4 5 • Chapter 1 MSC: Understanding 19. Which of the following is a homogeneous mixture? a. an egg b. smoke c. beach sand d. dry ice (solid CO2) e. a salt solution (NaCl dissolved in water) ANS: E DIF: Easy REF: 1.3 OBJ: Distinguish between homogeneous and heterogeneous mixtures. MSC: Understanding 20. Which of the following is a heterogeneous mixture? a. concrete d. mercury metal b. sweet tea e. an intravenous (IV) solution c. black coffee ANS: A DIF: Easy REF: 1.3 OBJ: Distinguish between homogeneous and heterogeneous mixtures. MSC: Understanding 21. Distillation may be used to separate components in a mixture based on ________ a. solubilities. d. densities. b. masses. e. colors. c. volatilities. ANS: C DIF: Easy REF: 1.3 OBJ: Describe the methods that can be used to separate the components of a mixture: distillation, filtration, and chromatography. MSC: Remembering 22. Which of the following is a chemical property of formaldehyde (CH2O)? a. It is flammable. d. It dissolves in water. b. It has a density of 1.09 g/mL. e. It is a gas at room temperature. c. It is colorless. ANS: A DIF: Easy REF: 1.3 OBJ: Describe and give examples of chemical and physical properties. MSC: Remembering 23. Which of the following is a chemical property of copper metal? a. It conducts heat. b. It reacts with nitric acid to produce copper(II) nitrate. c. It melts at 1085°C d. It conducts electricity. e. It has an orange color. ANS: B DIF: Easy REF: 1.3 OBJ: Describe and give examples of chemical and physical properties. MSC: Remembering 5 6 • Chapter 1 24. Which of the following represents a physical property of water? a. It boils at 100°C. b. An electrical current decomposes water into hydrogen gas and oxygen gas. c. It reacts with iron metal and oxygen to form rust. d. It reacts with carbon monoxide to form carbon dioxide and hydrogen gas. e. It is used in photosynthesis. ANS: A DIF: Easy REF: 1.3 OBJ: Describe and give examples of chemical and physical properties. MSC: Remembering 25. Which of the following represents a chemical property of iron? d. Its melting point is 1538°C. a. Its density is 7.84 g/cm3. b. It is magnetic. e. It conducts electricity. c. It reacts with oxygen in moist air. ANS: C DIF: Easy REF: 1.3 OBJ: Describe and give examples of chemical and physical properties. MSC: Remembering 26. Which of the following is a chemical property of acetone (C 3H6O)? a. It readily evaporates at room temperature. b. It has a pungent, irritating odor. c. It can be ignited in oxygen. d. It boils at 56°C. e. It is miscible with water. ANS: C DIF: Easy REF: 1.3 OBJ: Describe and give examples of chemical and physical properties. MSC: Remembering 27. Which of the following is a chemical property of platinum? a. It conducts heat and electricity. b. It can react with chlorine gas to form platinum(IV) chloride. c. The difference between its melting and boiling points is 2057°C. d. It is a gray-white metal. e. Sound travels through it at a speed of 2680 m/s. ANS: B DIF: Easy REF: 1.3 OBJ: Describe and give examples of chemical and physical properties. MSC: Remembering 28. Extensive properties are ________ a. dependent on the amount of substance present. b. identical for all substances. c. independent of a substance’s phase. d. the physical properties of a substance. e. dependent on the reactivity of the substance. ANS: A DIF: Easy REF: 1.3 OBJ: Describe and give examples of extensive and intensive properties. MSC: Remembering 6 7 • Chapter 1 29. Which one of the following represents a physical change? a. Milk turns sour. d. An egg begins to smell very bad. b. Rust forms on iron nails. e. Sugar melts and forms a syrupy liquid. c. Sugar ferments to form ethanol. ANS: E DIF: Easy REF: 1.3 OBJ: Distinguish between physical and chemical changes. MSC: Understanding 30. Which one of the following represents a chemical change? a. Mercury(II) oxide is heated up and forms mercury metal and oxygen gas. b. Rubbing alcohol evaporates. c. Iodine vapor deposits on a surface. d. Iron metal is separated from sand using a magnet. e. Rock salt is pulverized. ANS: A DIF: Easy REF: 1.3 OBJ: Distinguish between physical and chemical changes. MSC: Understanding 31. Which one of the following is NOT an intensive physical property of a pure liquid? a. boiling point d. density b. conductivity e. color c. mass ANS: C DIF: Moderate REF: 1.3 OBJ: Describe and give examples of extensive and intensive properties. MSC: Remembering 32. Which statement is true regarding ammonia, NH3? a. It can also be correctly represented as N 2H6. b. It cannot be decomposed into simpler substances by any means. c. Its decomposition produces three volumes of hydrogen for every one volume of nitrogen. d. It can be separated into nitrogen and hydrogen atoms using distillation. e. It is not a stable molecule and does not exist at room temperature. ANS: C DIF: Moderate REF: 1.3 OBJ: Distinguish between elements and compounds. MSC: Understanding 33. When copper metal is dropped into nitric acid, a blue solution containing copper(II) ions is produced along with brown nitrogen monoxide gas. Which of the following is an example of a chemical property? a. copper’s red-orange appearance b. nitrogen monoxide’s irritating odor c. the blue color of aqueous copper(II) ions d. the viscosity of nitric acid at room temperature e. nitric acid’s ability to react with copper metal ANS: E DIF: Moderate REF: 1.3 OBJ: Describe and give examples of chemical and physical properties. MSC: Analyzing 7 8 • Chapter 1 34. If you had equal masses of each of the following substances, which would occupy the greatest volume? a. ice (d = 0.917 g/mL) d. cocoa butter (d = 0.910 g/mL) b. water (d = 0.997 g/mL) e. aluminum (d = 2.70 g/mL) c. beeswax (d = 0.960 g/mL) ANS: D MSC: Analyzing DIF: Moderate REF: 1.3 OBJ: Use density in calculations. 35. The densities of glycerol and of mercury are 1.26 g/mL and 13.5 g/mL, respectively. What volume of glycerol has the same mass as 25.0 mL of mercury? a. 268 mL d. 1.47 mL b. 426 mL e. 338 mL c. 2.33 mL ANS: A MSC: Applying DIF: Moderate REF: 1.3 OBJ: Use density in calculations. 36. Based on values for the volume per gram of the given materials, which of the following would NOT float in water (density = 0.997 g/cm3)? a. b. c. Substance g/cm3 Balsa wood 0.120 Cork Charcoal (from oak) 0.240 0.571 Human fat 0.943 Ethylene glycol 1.11 balsa wood cork charcoal ANS: E MSC: Applying d. e. DIF: Moderate human fat ethylene glycol REF: 1.3 OBJ: Use density in calculations. 37. Calcite has a chemical formula of CaCO3, and 1.0 g occupies approximately 0.369 cm3. Pyrite (FeS2) is 1.8 times denser than calcite. What is the density of FeS 2? a. 2.7 g/cm3 d. 2.2 g/cm3 b. 0.66 g/cm3 e. 1.5 g/cm3 c. 4.9 g/cm3 ANS: C MSC: Applying DIF: Moderate REF: 1.3 8 9 • Chapter 1 OBJ: Use density in calculations. 38. Which of the following can be separated by filtration? a. rust particles in water d. salt dissolved in water b. air dispersed in whipped cream e. nitrogen from air c. alcohol dissolved in water ANS: A DIF: Moderate REF: 1.3 OBJ: Describe the methods that can be used to separate the components of a mixture: distillation, filtration, and chromatography. MSC: Understanding 39. Which process would be a practical and effective way to separate beta-carotene, an orange pigment, from hexane liquid? a. filtration d. scanning tunneling microscopy b. chromatography e. sublimation c. combustion ANS: B DIF: Moderate REF: 1.3 OBJ: Describe the methods that can be used to separate the components of a mixture: distillation, filtration, and chromatography. MSC: Applying 40. Acetone and water mix to form a homogeneous solution. Acetone has a boiling point of 56°C. Which of the following would be a suitable method for separating acetone from water? a. filtration d. scanning tunneling microscopy b. combustion e. sublimation c. distillation ANS: C DIF: Moderate REF: 1.3 OBJ: Describe the methods that can be used to separate the components of a mixture: distillation, filtration, and chromatography. MSC: Applying 41. Which of the following is an intensive property of chlorine? a. It has mass. b. It boils at −34°C. c. Chlorine gas expands to fill a balloon. d. The reaction of chlorine with hydrogen releases a given amount of energy. e. Chlorine gas in a container exerts a given pressure at a given temperature. ANS: B DIF: Moderate REF: 1.3 OBJ: Describe and give examples of extensive and intensive properties. MSC: Analyzing 42. Which represents an extensive property of hydrogen? a. Hydrogen gas is odorless and colorless. b. A hydrogen gas molecule is composed of two hydrogen atoms. c. Hydrogen gas is flammable. d. Hydrogen releases a given amount of energy when it reacts with oxygen. e. Hydrogen gas under normal conditions is nonmetallic. ANS: D DIF: Moderate REF: 1.3 OBJ: Describe and give examples of extensive and intensive properties. MSC: Analyzing 9 10 • Chapter 1 43. The densities of cork, lead, and water are 0.240 g/cm 3, 11.34 g/cm3, and 0.997 g/cm3 at 25°C, respectively. If 20.0 g of lead are placed inside an 85.0 cm3 piece of cork, what is the overall density, and will it float on water? d. 4.25 g/cm3; No, it will not float. a. 0.466 g/cm3; Yes, it will float. 3 e. 2.15 g/cm3; No, it will not float. b. 0.235 g/cm ; Yes, it will float. 3 c. 0.211 g/cm ; Yes, it will float. ANS: A MSC: Applying DIF: Difficult REF: 1.3 OBJ: Use density in calculations. 44. Soft solder is a blended alloy of tin (7.31 g/cm 3) and lead (11.34 g/cm3) that is used in plumbing and electronics. It is 63.5% tin by mass. What is the density of the alloy? d. 8.79 g/cm3 a. 9.87 g/cm3 3 b. 8.27 g/cm e. 9.33 g/cm3 3 c. 7.83 g/cm ANS: D MSC: Evaluating DIF: Difficult REF: 1.3 OBJ: Use density in calculations. 45. Gold (19.3 g/cm3) and copper (8.96 g/cm3) can be blended to form an alloy called rose gold. Suppose a rose-gold bar has a mass of 117 g and a volume of 7.00 cm3. Calculate the mass percentage of gold in the bar. a. 46.4% d. 75.0% b. 53.6% e. 86.6% c. 38.7% ANS: D MSC: Evaluating DIF: Difficult REF: 1.3 OBJ: Use density in calculations. 46. Which statement correctly describes the properties of gaseous helium (He)? a. The gas is not highly compressible even though the atoms do not occupy the entire volume of the container. b. The gas is highly compressible because there is a lot of empty space between the atoms. c. The atoms are moving rapidly about the container, giving the gas its definite shape. d. The gas has a definite volume and shape because the atoms are not moving about the container. e. A gas takes the shape of the container, but its total volume cannot change. ANS: B DIF: Easy REF: 1.4 OBJ: Distinguish between the states of matter: solid, liquid, and gas. MSC: Remembering 10 11 • Chapter 1 47. Solid carbon dioxide (CO2) can undergo sublimation to form gaseous CO2. Which of the following statements is true? a. In the solid phase, CO2 molecules easily slip past each other, and there are areas of randomly ordered molecules. b. In the gas phase, CO2 molecules are strongly attracted to each other. c. The motion of the CO2 molecules in the solid phase is much more restricted than in the gas phase. d. CO2 molecules in the solid phase are easily compressed to smaller volumes. e. The CO2 molecules decompose to form carbon and oxygen when they enter the gas phase. ANS: C DIF: Easy REF: 1.4 OBJ: Distinguish between the states of matter: solid, liquid, and gas. MSC: Understanding 48. Which statement describing the properties of the different phases of a sample of matter is true? a. The particles in both the gas and liquid phases are highly ordered and in close proximity to one another. b. The particles in the liquid phase are highly compressible because they can slip past one another. c. The particles in both the solid and liquid phases are free to assume any shape, and their nearest neighbors change over time. d. The solid phase is rigid, even though its constituent particles may vibrate a little depending on their temperature. e. Localized areas of order can form in the gas phase because the particles experience significant attractions to one another. ANS: D DIF: Easy REF: 1.4 OBJ: Distinguish between the states of matter: solid, liquid, and gas. MSC: Remembering 49. Equal amounts of water undergo the following changes. Which of the following would involve the largest change in energy? a. Ice is melted to form liquid water at 0°C. b. Ice at −25°C is heated to 0°C. c. Water is heated from 25°C to 50°C. d. Steam at 100°C is cooled and condensed to form liquid water at 85°C. e. Water at 0°C is heated and vaporized to form steam at 120°C. ANS: E DIF: Moderate REF: 1.4 OBJ: Describe how temperature affects the properties of matter. MSC: Analyzing 50. Equal amounts of a pure substance undergo the following changes. Which process would you predict releases the greatest amount of energy? a. deposition (gas → solid) d. condensation (gas → liquid) b. vaporization (liquid → gas) e. melting (solid → liquid) c. freezing (liquid → solid) ANS: A DIF: Moderate REF: 1.4 OBJ: Describe the processes of sublimation, melting, vaporization, condensation, freezing, and deposition. MSC: Analyzing 11 12 • Chapter 1 51. Which of the following is an example of potential energy? a. water running down a hill b. chemical bonds in table sugar (sucrose) c. electrons flowing through a wire d. a crowd moving a barricade e. molecules moving randomly in a liquid ANS: B DIF: Easy REF: 1.5 OBJ: Distinguish between potential and kinetic energy. MSC: Understanding 52. Equal amounts of water are present under the following conditions. In which case do the water molecules have the highest kinetic energy? a. as ice at −10°C d. in the gas phase at 150°C e. in the solid phase at 0°C b. as steam at 100°C c. in the liquid phase at 80°C ANS: D DIF: Easy REF: 1.5 OBJ: Distinguish between potential and kinetic energy. MSC: Understanding 53. If the speed of an object triples, its kinetic energy ________ a. increases by a factor of 3. d. decreases by a factor of 9. b. increases by a factor of 9. e. is unaffected. c. decreases by a factor of 3. ANS: B DIF: Easy REF: 1.5 OBJ: Distinguish between potential and kinetic energy. MSC: Applying 54. Which of the following statements about energy, work, and heat is NOT true? a. Adding heat to a sample of matter increases the average kinetic energy of its constituent particles. b. Thermal energy is the portion of the energy of an object that increases as temperature increases. c. When an object does work, part of the energy it expends is destroyed as it converts to heat. d. The energy available from some chemical reactions can be used to do work and/or produce heat. e. Heat involves the transfer of energy from a hotter object to a cooler one. ANS: C DIF: Moderate OBJ: Define energy, work, and heat. REF: 1.5 MSC: Analyzing 55. Consider electrons traveling through a copper (Cu) wire at a speed of 0.024 cm/s. What is true about the energy of their motion? a. It is primarily kinetic. b. It is primarily potential. c. It would be unaffected if the speed of the electrons increased. d. It is strongly affected by gravity. e. It cannot be used to do work. ANS: A DIF: Moderate REF: 1.5 OBJ: Distinguish between potential and kinetic energy. 12 13 • Chapter 1 MSC: Applying 56. Work is defined as the exertion of force through a distance. Which of the following is NOT an example of work? a. Molecules in the air push against the blades of a windmill. b. Blood is pumped through the circulatory system. c. Electrons flow against the resistance present in a copper wire. d. Thermal energy (heat) is transferred from a hot stove to the surrounding air. e. A student lifts a book off of the floor. ANS: D DIF: Moderate REF: 1.5 OBJ: Distinguish between potential and kinetic energy. MSC: Analyzing 57. Which has the highest kinetic energy, assuming all follow the equation KE = ½ mu2, where m is the mass and u is the velocity? a. a one-ton (910 kg) truck traveling at 65 miles per hour (29 m/s) b. an electron with a mass of 9.11 × 10−27 kg traveling at 2.97 × 108 m/s (99% of the speed of light) c. an oxygen molecule with a mass of 5.31 × 10−26 kg traveling at 394 m/s (roughly its speed at room temperature) d. Usain Bolt, who has a mass of approximately 94 kg, running at 10 m/s (22.4 miles per hour) e. an oil tanker with a mass of 3 × 107 kg traveling at 9 m/s (20 miles per hour) ANS: E DIF: Moderate REF: 1.5 OBJ: Distinguish between potential and kinetic energy. MSC: Analyzing 58. At what velocity would a proton be traveling if it had the same kinetic energy as an electron traveling at 10.0% of the speed of light? KE = ½ mu2, where m is the mass and u is the velocity; proton mass = 1.673 × 10−27 kg; electron mass = 9.109 × 10−31 kg; speed of light = 2.998 × 108 m/s. a. 4.89 × 1011 m/s d. 7.00 × 105 m/s 11 b. 2.45 × 10 m/s e. 3.50 × 105 m/s 5 c. 4.95 × 10 m/s ANS: D DIF: Difficult REF: 1.5 OBJ: Distinguish between potential and kinetic energy. MSC: Evaluating 59. The electrostatic potential energy (Eel) between a pair of charged particles is proportional to their charges, Q1 and Q2, and inversely proportional to the distance between the centers of the ions, d. Oppositely charged particles attract each other, while like particles repel. Which statement is true? Q1 × Q2 E el∝ d a. As the distance between particles with like charges increases, the potential energy decreases. b. If d is doubled and Q1 is doubled, the potential energy doubles. c. As the distance between particles with opposite charges increases, the potential energy decreases. d. If the magnitude of the charges increases, the potential energy decreases. e. If both Q1 and Q2 have a value of −1, the potential energy is negative. ANS: A DIF: Difficult REF: 1.5 OBJ: Distinguish between potential and kinetic energy. 13 14 • Chapter 1 MSC: Evaluating 60. The chemical formula of dimethyl ether can be represented in different ways. When its formula is written as C2H6O, ________ a. the arrangement of the atoms in the molecule is evident. b. only the number and type of atoms of each element are given. c. its structural formula can be deduced. d. it shows that no other molecules can have that formula. e. it lists only one of many possible elemental compositions for dimethyl ether. ANS: B DIF: Easy REF: 1.6 OBJ: Recognize and interpret the different ways of representing molecules (diatomic, molecular formula, structural formula, condensed structural formula, ball-and-stick, space-filling). MSC: Remembering 61. What type of chemical formula is shown for diethyl ether? a. b. c. molecular structural condensed structural d. e. ball-and-stick space-filling ANS: B DIF: Easy REF: 1.6 OBJ: Recognize and interpret the different ways of representing molecules (diatomic, molecular formula, structural formula, condensed structural formula, ball-and-stick, space-filling). MSC: Remembering 62. The space-filling model of a molecule ________ a. clearly shows bond angles. b. gives little idea of how atoms are arranged. c. is best suited for very large molecules. d. gives an indication of three-dimensional shape. e. spreads atoms out so they are easy to view. ANS: D DIF: Easy REF: 1.6 OBJ: Recognize and interpret the different ways of representing molecules (diatomic, molecular formula, structural formula, condensed structural formula, ball-and-stick, space-filling). MSC: Remembering 14 15 • Chapter 1 63. Ethanol and dimethyl ether molecules both contain two carbon atoms, six hydrogen atoms, and one oxygen atom. Which statement is true? a. Their molecular formulas are different. b. They show the same physical properties but different chemical properties. c. The arrangement of the atoms in each type of molecule is different. d. Their melting points and boiling points are the same. e. There is no physical method that can distinguish between the two. ANS: C DIF: Moderate REF: 1.6 OBJ: Recognize and interpret the different ways of representing molecules (diatomic, molecular formula, structural formula, condensed structural formula, ball-and-stick, space-filling). MSC: Analyzing 64. Which of the following is the SI base unit for mass? a. g d. lb b. kg e. m c. mg ANS: B DIF: Easy REF: 1.7 OBJ: Describe SI and US measurements. 65. Which of the following is not an SI base unit? d. a. °C b. s e. c. kg MSC: Remembering mol m ANS: A DIF: Easy REF: 1.7 OBJ: Describe SI and US measurements. MSC: Remembering 66. Which of the following does not show a correct relationship between units? d. 1 GB = 1 × 109 B a. 1 × 103 g = 1 kg −3 b. 1 × 10 s = 1 ms e. 1 × 10−6 µL = 1 L −9 c. 1 nm = 1 × 10 m ANS: E DIF: Easy REF: 1.7 OBJ: Describe SI and US measurements. MSC: Understanding 67. Which of the following does NOT show an exact relationship? a. 100 cm = 1 m d. 1 km = 0.6214 mi e. 1 dozen = 12 objects b. 1 m3 = 1000 L c. 1 in = 2.54 cm ANS: D DIF: Easy REF: 1.7 OBJ: Distinguish between exact and uncertain values. MSC: Remembering 68. Green light in the visible portion of the electromagnetic radiation spectrum has wavelengths around 550 nm. Express this wavelength in meters using exponential notation. d. 5.5 × 107 m a. 5.5 × 10−9 m b. 5.5 × 10−7 m e. 5.5 × 109 m c. 5.5 m ANS: B DIF: Easy REF: 1.7 OBJ: Describe SI and US measurements. 15 16 • Chapter 1 MSC: Understanding 69. The diameter of the sun is approximately 1,390,000 km. In correct scientific notation, this is ________ a. 1.39 × 10−6 km. d. 139 × 104 km. −9 b. 1.39 × 10 m. e. 1.39 × 103 m. 6 c. 1.39 × 10 km. ANS: C DIF: Easy REF: 1.7 OBJ: Describe SI and US measurements. MSC: Understanding 70. The atomic radius of a uranium atom is approximately 175 pm. In correct scientific notation, this is ________ d. 175 × 10−12 m. a. 1.75 × 10−10 m. −11 b. 1.75 × 10 m. e. 1.75 × 1010 m. −12 c. 1.75 × 10 m. ANS: A DIF: Easy REF: 1.7 OBJ: Describe SI and US measurements. MSC: Understanding 71. The following measurements of the mass of an aspirin tablet were made by different students in a lab. Which set is the most precise? a. 1.513 g, 1.503 g, 1.523 g d. 1.513 g, 1.517 g, 1.512 g b. 1.513 g, 1.511 g, 1.450 g e. 1.513 g, 1.505 g, 1.553 g c. 1.513 g, 1.459 g, 1.533 g ANS: D DIF: Easy REF: 1.7 OBJ: Distinguish between precision and accuracy. MSC: Understanding 72. A student conducts repeated trials to determine the density of a sample of seawater and obtains the following results: 1.321 g/mL, 1.323 g/mL, 1.319 g/mL, and 1.321 g/mL. Known values are reported to be in the 1.02 to 1.09 g/mL range. The experimental results are ________ a. less precise than the known values. d. precise and accurate. b. more accurate than the known values. e. inaccurate but precise. c. imprecise but accurate. ANS: E DIF: Easy REF: 1.7 OBJ: Distinguish between precision and accuracy. MSC: Understanding 73. If the following arithmetic operations were carried out, how many significant figures should the answer contain? 0.750 × 11 / 9.250 a. 1 b. 2 c. 3 d. e. 4 5 ANS: B DIF: Easy REF: 1.7 OBJ: Apply the rules for significant figures (weak-link principle). MSC: Remembering 16 17 • Chapter 1 74. What value should be reported as the volume of a strip of aluminum foil measuring 15.37 cm × 42.5 cm × 0.0010 cm? a. 0.65322 cm3 d. 0.65 cm3 3 b. 0.6532 cm e. 0.7 cm3 3 c. 0.653 cm ANS: D DIF: Easy REF: 1.7 OBJ: Apply the rules for significant figures (weak-link principle). MSC: Remembering 75. A metal object weighing 43.905 g has a volume of 6.0 cm3. What is the density of the metal? d. 7.3 g/cm3 a. 7.3175 g/cm3 3 b. 7.318 g/cm e. 7 g/cm3 3 c. 7.32 g/cm ANS: D DIF: Easy REF: 1.7 OBJ: Apply the rules for significant figures (weak-link principle). MSC: Understanding 76. Based on the following figure, which of the measurements listed is the best estimate of the length of the object? a. b. c. 1.8 cm 1.81 cm 1.810 cm d. e. 1.90 cm 1.9 cm ANS: D DIF: Easy REF: 1.7 OBJ: Apply significant figures to precision of measurement. MSC: Understanding 77. Which of the following common laboratory devices will deliver 25 mL of a solution with the greatest precision? a. a 100 mL beaker without volume divisions b. a 50 mL beaker with volume divisions every 10 mL c. a 50 mL graduated cylinder with volume divisions every 2 mL d. a 25 mL beaker without volume divisions e. a 25 mL pipet with a to-deliver error of 0.01 mL ANS: E DIF: Easy REF: 1.7 OBJ: Apply significant figures to precision of measurement. 17 18 • Chapter 1 MSC: Understanding 78. White fuming nitric acid should contain no more than 2% water by mass. The water content in four samples was measured. What is the average value, and which measured value is closest to the average? a. b. c. Sample % water, by mass 1 1.983 2 1.927 3 1.946 4 1.956 1.953, sample 4 1.95, sample 4 1.9530, sample 4 d. e. 1.9530, sample 3 1.953, sample 3 ANS: A DIF: Easy REF: 1.7 OBJ: Apply significant figures to precision of measurement. MSC: Understanding 79. The average volume of a red blood cell is approximately 90 fL. Express the average value in liters using correct exponential notation and number of significiant figures. d. 9 × 10−14 L a. 90 × 10−15 L −15 b. 9 × 10 L e. 9.0 × 10−14 L –15 c. 9.0 × 10 L ANS: D DIF: Moderate REF: 1.7 OBJ: Describe SI and US measurements. MSC: Understanding 80. If the following arithmetic operations are carried out, how many significant figures should be reported in the answer? 32 + 0.56 + 0.210 + 3.3 a. 1 b. 2 c. 3 d. e. 4 5 ANS: B DIF: Moderate REF: 1.7 OBJ: Apply the rules for significant figures (weak-link principle). MSC: Applying 81. What value should be reported for the total mass of three samples of iron weighing 117.0 g, 19.43 g, and 6.1043 g? a. 143 g d. 142.5 g b. 142.53 g e. 142.5343 g c. 142.534 g ANS: D DIF: Moderate REF: 1.7 OBJ: Apply the rules for significant figures (weak-link principle). MSC: Applying 18 19 • Chapter 1 82. If the following arithmetic operations are carried out, how many significant figures should be reported in the answer? (0.600)(1.5366 − 0.708) 4.510 + 2.105 − 1.83 0.752 a. 1 d. 4 b. 2 e. 5 c. 3 ANS: B DIF: Moderate REF: 1.7 OBJ: Apply the rules for significant figures (weak-link principle). MSC: Applying 83. A rectangular sheet of aluminum foil has a length of 8.0 cm, a width of 4.0 cm, and a mass of 864 mg. Determine the thickness of the foil, given that the density of aluminum is 2.70 g/cm3. a. 1.0 mm d. 10. µm b. 0.10 mm e. 1.0 × 102 cm c. 0.010 mm ANS: B DIF: Moderate REF: 1.7 OBJ: Apply the rules for significant figures (weak-link principle). MSC: Applying 84. A graduated cylinder is filled with water to the 25.0 mL mark. After 27.5 g of titanium dioxide (TiO 2) is added, the volume is 31.5 mL. Calculate the density of TiO2. a. 0.873 g/cm3 d. 4.23 g/cm3 3 b. 0.87 g/cm e. 2.05 g/cm3 c. 4.2 g/cm3 ANS: C DIF: Moderate REF: 1.7 OBJ: Apply the rules for significant figures (weak-link principle). MSC: Applying 85. Which of the following represents the largest mass? a. 250 ng d. 0.25 kg b. 25 µg e. 25 mg c. 2.5 g ANS: D DIF: Moderate REF: 1.7 OBJ: Describe SI and US measurements. MSC: Analyzing 86. Which of the following represents the smallest mass? d. 4.0 × 102 µg a. 4.0 × 100 mg 2 b. 4.0 × 10 ng e. 4.0 × 10−6 kg −4 c. 4.0 × 10 g ANS: B DIF: Moderate REF: 1.7 OBJ: Describe SI and US measurements. 19 20 • Chapter 1 MSC: Analyzing 87. The distance between the two hydrogen atoms in a water molecule is about 1.355 × 10−10 m. This is equal to ________ a. 1.355 × 10−8 mm. d. 13.55 nm. b. 1.355 × 106 cm. e. 135.5 pm. c. 1.355 × 10−6 µm. ANS: E DIF: Moderate REF: 1.7 OBJ: Describe SI and US measurements. MSC: Analyzing 88. The calculated diameter of a carbon atom is about 0.000000000340 m. In correct scientific notation, this is equal to ________ d. 3.40 × 100 nm. a. 3.40 × 10−12 km. −12 b. 3.40 × 10 cm. e. 3.40 × 102 pm. −8 c. 3.40 × 10 mm. ANS: E DIF: Moderate REF: 1.7 OBJ: Describe SI and US measurements. MSC: Analyzing 89. The average diameter of a red blood cell is about 7 × 10−6 m. Choose the best way to represent this distance using SI units and prefixes. a. 7 µm d. 7000 nm b. 0.007 mm e. 7000000 pm c. 0.000007 m ANS: A DIF: Moderate REF: 1.7 OBJ: Describe SI and US measurements. 20 21 • Chapter 1 MSC: Analyzing 90. An irregularly shaped metal object with a mass of 25.43 g was placed in a graduated cylinder with water. The before and after volumes are shown below. What is the density of the metal? a. b. c. 2.826 g/cm3 2.8 g/cm3 0.35 g/cm3 d. e. 0.3539 g/cm3 2.5 g/cm3 ANS: B DIF: Moderate REF: 1.7 OBJ: Apply the rules for significant figures (weak-link principle). MSC: Applying 91. An 84.6419 g antique coin is thought to be gold. When the coin is placed in a graduated cylinder containing 15.53 mL of water, the water level rises to 24.64 mL. Calculate the density of the coin. a. 9.29 g/mL d. 9.2911 g/mL b. 5.450 g/mL e. 3.435 g/mL c. 0.73833 g/mL ANS: A DIF: Moderate REF: 1.7 OBJ: Apply the rules for significant figures (weak-link principle). MSC: Applying 21 22 • Chapter 1