Chemistry Human Activity, Chemical Reactivity (International Edition by Paul Treichel - Test Bank

NETA Assessment: Test Bank to accompany Chemistry: Human Activity, Chemical Reactivity, Second International Edition By Peter G. Mahaffy, Robert Bucat, Roy Tasker, John C. Kotz, Paul M. Treichel, Gabriela C. Weaver, John McMurry Test Bank prepared by Brett McCollum, Mount Royal University Text ISBN: 0176660887 NETA copy editor: Kelli Howey For more information contact Nelson, 1120 Birchmount Road, Toronto, Ontario M1K 5G4. Or you can visit our Internet site at . ALL RIGHTS RESERVED. No part of this work covered by the copyright hereon may be reproduced or used in any form or by any means—graphic, electronic, or mechanical, including photocopying, recording, taping, web distribution or information storage and retrieval systems—without the written permission of the publisher COPYRIGHT ©2015 by Nelson Education Ltd. Nelson is a registered trademark used herein under licence. All rights reserved. ii TABLE OF CONTENTS Part 1: Chemistry: A Human Activity CHAPTER 1: Human Activity, Chemical Reactivity .....................................................................1-1 Part 2: An Overview of Materials and Reactions CHAPTER 2: Building Blocks of Materials ....................................................................................2-1 CHAPTER 3: Models of Structure to Explain Properties .............................................................3-1 CHAPTER 4: Carbon Compounds ..................................................................................................4-1 CHAPTER 5: Chemical Reaction, Chemical Equations ................................................................5-1 CHAPTER 6: Chemistry of Water, Chemistry in Water ..............................................................6-1 CHAPTER 7: Chemical Reactions and Energy Flows ...................................................................7-1 Part 3: Relating the Structure and Behaviour of Substances CHAPTER 8: Modelling Atoms and Their Electrons ....................................................................8-1 CHAPTER 9: Molecular Structures, Shapes, and Stereochemistry—Our Evidence ..............................................................................................................................................9-1 CHAPTER 10: Modelling Bonding in Molecules ..........................................................................10-1 CHAPTER 11: States of Matter .....................................................................................................11-1 CHAPTER 12: Solutions and Their Behaviour ............................................................................12-1 Part 4: Competing Influences on Chemical Reactions CHAPTER 13: Dynamic Chemical Equilibrium ..........................................................................13-1 CHAPTER 14: Acid-Base Equilibria in Aqueous Solution ..........................................................14-1 CHAPTER 15: Solubility, Precipitation, and Complexation .......................................................15-1 CHAPTER 16: Electron Transfer Reactions and Electrochemistry ...........................................16-1 CHAPTER 17: Spontaneous Change: How Far? .........................................................................17-1 CHAPTER 18: Spontaneous Change: How Fast? ........................................................................18-1 Part 5: Carbon Compounds: Patterns of Structure and Reactivity CHAPTER 19: Alkenes and Alkynes .............................................................................................19-1 CHAPTER 20: Aromatic Compounds ...........................................................................................20-1 CHAPTER 21: Halogenated Organic Compounds .......................................................................21-1 CHAPTER 22: Alcohols, Phenols, and Ethers ..............................................................................22-1 CHAPTER 23: Carbonyl Compounds: Part I ..............................................................................23-1 CHAPTER 24: Carbonyl Compounds: Part II .............................................................................24-1 CHAPTER 25: Amines and Nitrogen Heterocycles ......................................................................25-1 Part 6: Compounds of the Elements: Patterns of Structure and Reactivity CHAPTER 26: Main Group Elements and Their Compounds ...................................................26-1 CHAPTER 27: Transition Elements and Their Compounds ......................................................27-1 Part 7: Chemistry of Materials, Life, and the Nucleus CHAPTER 28: The Chemistry of Modern Materials ...................................................................28-1 CHAPTER 29: Biomolecules ..........................................................................................................29-1 CHAPTER 30: Nuclear Chemistry ................................................................................................30-1 iii PREFACE In most post-secondary courses, a large percentage of student assessment is based on multiple- choice testing. Many instructors use multiple-choice reluctantly, believing that it is a methodology best used for testing what a student remembers rather than what she or he has learned. Nelson Education Ltd. understands that a good quality multiple-choice test bank can provide the means to measure higher-level thinking skills as well as recall. Recognizing the importance of multiple-choice testing in today’s classroom, we have created NETA—the Nelson Education Teaching Advantage program—to ensure the value of our high quality test banks. The NETA program was created in partnership with David DiBattista, a 3M National Teaching Fellow, professor of psychology at Brock University, and researcher in the area of multiple- choice testing. NETA ensures that subject-matter experts who author test banks have had training in two areas: avoiding common errors in test construction, and developing multiple- choice test questions that “get beyond remembering” to assess higher-level thinking. All NETA test banks include David DiBattista’s guide for instructors, “Multiple Choice Tests: Getting Beyond Remembering.” This guide has been designed to assist you in using Nelson test banks to achieve your desired outcomes in your course. The Test Bank for Chemistry, Second International Edition has been revised for Canadian students by Brett McCollum, Mount Royal University. The multiple-choice questions were written and edited to conform to NETA guidelines, which emphasize the development of higher- order thinking and the effective construction of questions. NETA principles of question construction help eliminate ambiguity, arguable answers, guesswork, and unconscious cues to test-savvy students, resulting in a test that accurately reflects student understanding. The Test Bank offers about 1764 questions, including 1357 multiple choice, 151 true/false, 58 completion questions, 120 short answer, 32 problems, 32 essay style questions, and 14 matching items. In addition to providing a variety of questions related to each chapter objective, this test bank also employs a series of tags that can help design effective, balanced tests by the measure of course outcomes. All of the tags are included with the question in the test bank. These tags include: iv  ANS: The correct answer. (Suggested answers are provided for the short answer questions.)  PTS: The number of points an instructor can assign for each question. The default is 1 point.  BLM: The category from Bloom’s taxonomy for learning (Remember or Higher Order). This category is included to assist instructors in assessing student’s higher-order cognitive skills.  REF: The related page number in the text.  DIF: An assigned difficulty rating of 1, 2, 3. The Computerized Test Bank The NETA Test Bank is available in a new, cloud-based platform. Nelson Testing Powered by Cognero® is a secure online testing system that allows you to author, edit, and manage test bank content from any place you have Internet access. No special installations or downloads are needed, and the desktop-inspired interface, with its drop-down menus and familiar, intuitive tools, allows you to create and manage tests with ease. You can create multiple test versions in an instant, and import or export content into other systems. Tests can be delivered from your learning management system, your classroom, or wherever you want. Cognero and Full-Circle Assessment are registered trademarks of Madeira Station LLC. v Chapter 1—Human Activity, Chemical Reactivity TRUE/FALSE 1. Knowledge of chemistry applies to your everyday life. ANS: T PTS: 1 REF: p. 1 2. Electromagnetic radiation can be used as a type of chemotherapy. ANS: F PTS: 1 REF: p. 3 3. Oxygen (O2) can exist only in one energy state. ANS: F PTS: 1 REF: p. 3 BLM: Remember BLM: Remember BLM: Remember 4. The toxicity of substances can be used to good advantage in chemotherapy. ANS: T PTS: 1 REF: p. 3 BLM: Remember 5. Singlet oxygen can be used to destroy cancer cells. ANS: T PTS: 1 REF: p. 4 BLM: Remember 6. Electromagnetic radiation of the right energy can cause chemical reactions. ANS: T PTS: 1 REF: p. 4 BLM: Remember 7. Porphyrin rings are found in hemoglobin and in chlorophyll. ANS: T PTS: 1 REF: p. 4 BLM: Remember 8. In nature, the nitrogen atoms in porphyrins are usually bound to sulfur. ANS: F PTS: 1 REF: p. 4 BLM: Remember 9. A gas chromatogram is used to determine the molecular weight of compounds. ANS: F PTS: 1 REF: p. 9 BLM: Remember 10. Karrikinolide is the only compound found in nature that causes seeds to germinate. ANS: F PTS: 1 REF: p. 11 BLM: Higher Order 11. KAR1 has been shown to promote germination of a range of plants beyond kangaroo paw. ANS: T PTS: 1 REF: p. 12 BLM: Remember 12. The most common colour of the Northern or Southern Lights is violet. ANS: F PTS: 1 REF: p. 12 BLM: Remember Copyright © 2015 Nelson Education Limited 1-1 Chapter 1 13. All compounds found in wood smoke are beneficial. ANS: F PTS: 1 REF: p. 13 14. A cup of coffee contains toxic natural substances. ANS: T PTS: 1 REF: p. 13 Mahaffy International 2e TB BLM: Remember BLM: Remember 15. The World Health Organization estimates that less than 70% of the world’s population uses medicines made from plants and herbs. ANS: F PTS: 1 REF: p. 13 BLM: Remember 16. Most modern drugs are modified from chemicals originally found in plants and herbs. ANS: T PTS: 1 REF: p. 13 BLM: Remember MULTIPLE CHOICE 1. Which of the following techniques could be used to separate compounds in a mixture? a. spectroscopy b. chromatography c. chemotherapy d. photodynamic therapy ANS: B PTS: 1 REF: p. 2 2. Which of the following can be determined by spectroscopy? a. the structure of molecules b. the natural abundance of isotopes c. the biological activity of ions d. the toxicity of compounds ANS: A PTS: 1 REF: p. 2 3. The earth’s crust is made primarily of which element? a. silicon b. nitrogen c. sulfur d. oxygen ANS: D PTS: 1 REF: p. 2 4. Which of the following can spectroscopy tell us about a molecule? a. its name b. its history c. its location d. its structure ANS: D PTS: 1 REF: p. 2 BLM: Remember BLM: Remember BLM: Remember BLM: Higher Order Copyright © 2015 Nelson Education Limited 1-2 Chapter 1 Mahaffy International 2e TB 5. Which of the following is used in spectroscopy to elucidate the structure of molecules? a. triplet oxygen b. photosensitizers c. energy d. neutrons ANS: C PTS: 1 REF: p. 2 BLM: Higher Order 6. Which of the following oxygen containing chemical species is toxic to human cells? a. dihydrogen monoxide (water) b. heme c. triplet oxygen d. singlet oxygen ANS: D PTS: 1 REF: p. 3–4 BLM: Remember 7. There are three components required for the use of photodynamic therapy in the treatment of skin cancer. Which of the following is NOT one of those components? a. a photosensitizer b. red light c. lipoproteins d. triplet oxygen ANS: C PTS: 1 REF: p. 4 BLM: Remember 8. Which of the following techniques uses electromagnetic radiation to kill cancer cells? a. spectroscopy b. chromatography c. chemotherapy d. photodynamic therapy ANS: D PTS: 1 REF: p. 4 9. The porphyrin ring in heme is bound to which metal? a. iron b. magnesium c. cobalt d. copper ANS: A PTS: 1 REF: p. 4 BLM: Remember BLM: Remember Copyright © 2015 Nelson Education Limited 1-3 Chapter 1 Mahaffy International 2e TB 10. The structure of the porphyrin ring matches which of the following chemical representations? a. structure a b. structure b c. structure c d. structure d ANS: C PTS: 1 REF: p. 4 BLM: Remember 11. What porphyrin-containing substance that absorbs light and transfers energy is found in plants? a. hemoglobin b. Visudyne c. Gavinone d. chlorophyll ANS: D PTS: 1 REF: p. 4 BLM: Remember 12. There are two different energy states for oxygen. Which of the following is the energy state for singlet oxygen? a. ground state b. normal state c. excited state d. absorbed state ANS: C PTS: 1 REF: p. 4 BLM: Remember Copyright © 2015 Nelson Education Limited 1-4 Chapter 1 Mahaffy International 2e TB 13. What do photosensitizers do? a. They energize porphyrin. b. They transfer energy to triplet oxygen and convert it to singlet oxygen. c. They make cancer cells sensitive to light. d. They convert singlet oxygen into triplet oxygen. ANS: B PTS: 1 REF: p. 4 BLM: Remember 14. People with a medical disorder known as porphyria are required to avoid bright sunlight and wear long-sleeve shirts, hats, and gloves. Considering the name of the disorder, which of the following chemical substances would you expect to be involved in porphyria? a. chlorophyll b. hemoglobin c. testosterone d. pyran ANS: B PTS: 1 REF: p. 4 BLM: Higher Order 15. Which of the following medical conditions is currently being treated by photodynamic therapy? a. cataracts b. macular degeneration c. astigmatism d. arthritis ANS: B PTS: 1 REF: p. 5 16. Approximately how long does singlet oxygen exist? a. 10–6 seconds b. 10–3 seconds c. 100 seconds d. 101 seconds ANS: A PTS: 1 REF: p. 5 BLM: Remember BLM: Remember 17. Why is the location of a tumour important in determining whether photodynamic therapy (PDT) may be an effective method of treatment? a. PDT works only on certain types of tumours. b. Photosensitizers will only go to certain locations in the body. c. The red light from the laser cannot penetrate very far below the skin. d. Triplet oxygen is found only in certain parts of the body. ANS: C PTS: 1 REF: p. 5 BLM: Higher Order 18. What feature describes two molecules that are isomers? a. They have the same number of protons but different number of neutrons. b. They have the same molecular weight but different types of atoms. c. They have the same chemical reactivity in solution but different in the human body. d. They have the same formula but different arrangement of atoms. ANS: D PTS: 1 REF: p. 6 BLM: Remember Copyright © 2015 Nelson Education Limited 1-5 Chapter 1 Mahaffy International 2e TB 19. Research groups are trying to use the light-absorbing ability of porphyrins to do many new things. Which one of the following research projects involves the use of porphyrins? a. treatment of age-related macular degeneration b. generation of heat resistant crops c. conversion of nitrogen gas to ammonia d. transmutation of bismuth into gold ANS: C PTS: 1 REF: p. 6 BLM: Remember 20. Why would a compound that causes seed germination be useful to the agricultural industry? a. Plants could be grown at reclaimed mine sites. b. Endangered native species of plants could be regenerated. c. Weeds could be made to germinate before a crop is sown. d. Seeds could be kept dormant until planting is convenient for the farmer. ANS: C PTS: 1 REF: p. 7 21. What is NOT a possible source of natural products? a. flowers b. insects c. minerals d. animals ANS: C PTS: 1 REF: p. 7 BLM: Higher Order BLM: Higher Order 22. Seeds can remain dormant until suitable for the growth of a plant. Which of the following environmental conditions is necessary for seed germination? a. good soil b. sufficient moisture c. low levels of weeds d. low temperatures ANS: B PTS: 1 REF: p. 7 23. What is a bioactive compound? a. a compound that is found in biological systems b. a compound that is produced by a living organism c. a compound that is used to test for biological activity d. a compound that has an effect on living tissue ANS: D PTS: 1 REF: p. 7–10 BLM: Remember BLM: Higher Order 24. What reproducible source of smoke did Flematti use for his experiments? a. smoke from a forest fire b. smoke from a bush fire c. smoke from filter paper d. smoke from leaf lettuce ANS: C PTS: 1 REF: p. 8 BLM: Remember Copyright © 2015 Nelson Education Limited 1-6 Chapter 1 Mahaffy International 2e TB 25. What is a bioassay? a. a measure of optical activity b. a test for biological activity c. an extraction technique d. a type of spectroscopy ANS: B PTS: 1 REF: p. 8 BLM: Remember 26. Which of the following would NOT be appropriate to use in a bioassay? a. mice b. insects c. fish d. fossils ANS: D PTS: 1 REF: p. 8 BLM: Higher Order 27. Which of the following is NOT a structural determination method? a. mass spectroscopy b. nuclear magnetic resonance c. x-ray crystallography d. bioassay ANS: D PTS: 1 REF: p. 8 28. Why did Flematti and his co-workers burn filter paper? a. to obtain a reproducible source of smoke water b. because it is illegal to start forest or bush fires c. to calculate the amount of smoke produced per gram d. because they did not have a reliable source of wood ANS: A PTS: 1 REF: p. 8 BLM: Remember BLM: Higher Order 29. When trying to determine the structure of a compound, how does knowledge of the molecular weight help? a. It reveals which isotopes are present in the molecule. b. It tells you about the solubility of the molecule. c. It is needed to determine the molecular formula. d. It is equal to the number of carbons and hydrogens in the molecule. ANS: C PTS: 1 REF: p. 9 BLM: Higher Order 30. Extraction techniques are based on differences in physical or chemical properties. Which physical property was used in the extraction of Gavinone? a. solubility b. colour c. odour d. viscosity ANS: A PTS: 1 REF: p. 9 BLM: Remember Copyright © 2015 Nelson Education Limited 1-7 Chapter 1 Mahaffy International 2e TB 31. Many organic compounds are detected in the gas chromatogram of smoke. Which of the following processes should be used to isolate one compound? a. separate the mixture into smaller groups by extraction b. run the gas chromatogram with smaller amounts of smoke c. use a mass spectrometer to determine the molar mass of the mixture d. separate the mixture into smaller groups using a bioassay ANS: A PTS: 1 REF: p. 9 BLM: Higher Order 32. What is a major difference between Gavinone and the model compound shown below? a. the location of the CH3 b. the number of atoms c. the size of the rings d. the way the rings are connected ANS: A PTS: 1 REF: p. 10 33. Why was the name “Gavinone” problematic? a. It did not give enough information about the structure. b. It is not appropriate to name compounds after people. c. It wasn’t considered to be sufficiently formal. d. It implied a functional group not present in the structure. ANS: D PTS: 1 REF: p. 10 BLM: Higher Order BLM: Remember 34. The systematic name for “Gavinone” is based on rules from what organization? a. IUPAC: International Union of Pure and Applied Chemistry b. USFDA: United States Food and Drug Administration c. CSC: Canadian Society for Chemistry d. RACI: Royal Australian Chemical Institute ANS: A PTS: 1 REF: p. 10 BLM: Remember 35. The seed germination trigger compound karrikinolide was originally named after which scientist? a. Gavin Flematti b. Emilio Ghisalberti c. David Dolphin d. Guilio Natta ANS: A PTS: 1 REF: p. 11 BLM: Remember Copyright © 2015 Nelson Education Limited 1-8 Chapter 1 Mahaffy International 2e TB 36. Which of the following is the name for the class of compounds that trigger germination? a. gavinones b. karrikinolides c. KAR1 d. porphyrins ANS: B PTS: 1 REF: p. 11 BLM: Remember 37. What do the Northern Lights or Southern Lights and “neon” lights have in common? a. being caused by magnetic flux b. atoms in the ground state c. atoms in the excited state d. their colour ANS: C PTS: 1 REF: p. 12 BLM: Higher Order 38. Why is it sometimes preferable in research to use a pure synthetic substance rather than the natural product? a. It is easier to obtain the pure substance. b. Research wastes natural products that we should be conserving. c. Natural products are not better than synthetic substances. d. Natural products can contain toxic components. ANS: D PTS: 1 REF: p. 13 39. What is the definition of an organic compound? a. a compound containing no pesticides or herbicides b. a compound containing carbon c. a compound not made synthetically d. a compound that occurs only in nature ANS: B PTS: 1 REF: p. 13 BLM: Higher Order BLM: Higher Order 40. What approach to learning was illustrated in the stories of Gavinone and photodynamic therapy? a. the discovery method b. the investigative method c. the scientific method d. the Suzuki method ANS: C PTS: 1 REF: p. 13 BLM: Higher Order Copyright © 2015 Nelson Education Limited 1-9 Chapter 2—Building Blocks of Materials TRUE/FALSE 1. In a liquid, the particles are vibrating with sufficient energy that they do not have fixed positions, but not enough energy that they can fill any container. ANS: T PTS: 1 REF: p. 21 BLM: Remember 2. One mole of dinitrogen tetroxide molecules, N2O4, contains the same number of atoms as one mole of phosphorus pentachloride, PCl5. ANS: T PTS: 1 REF: p. 26 BLM: Higher Order 3. All atoms of oxygen have the same mass. ANS: F PTS: 1 REF: p. 29 BLM: Higher Order 4. Atoms with the same number of neutrons but a different number of protons are called isotopes of the same element. ANS: F PTS: 1 REF: p. 29 BLM: Remember 5. In the mass spectrometer, the high-energy electron beam gives particles of the vaporized sample a negative charge. ANS: F PTS: 1 REF: p. 33–34 BLM: Remember MULTIPLE CHOICE 1. According to the kinetic-molecular model of matter, how are the particles in a gas arranged? a. They are far apart from each other but confined to specific positions. b. They are packed closely together but not confined to specific positions. c. They vibrate back and forth in relation to a fixed position. d. They are far apart from each other and move about randomly. ANS: D PTS: 1 REF: p. 21 BLM: Remember 2. Which of the following phenomena cannot be accounted for using the kinetic-molecular model of matter? a. An ice cube will melt when it is heated to room temperature. b. Vinegar and olive oil separate into two layers in a bottle of salad dressing. c. The scent from a bunch of flowers diffuses in a room with no air currents. d. The colour from a drop of blue food dye spreads in a glass of water. ANS: B PTS: 1 REF: p. 21 BLM: Higher Order Copyright © 2015 Nelson Education Limited 2-1 Chapter 2 Mahaffy International 2e TB 3. Which of the following is a most likely to be a homogeneous mixture? a. butter b. ethanol c. gasoline d. tomato soup ANS: C PTS: 1 REF: p. 22 BLM: Higher Order 4. Which of the following is most likely to be a heterogeneous mixture? a. blood b. windshield washer fluid c. sodium chloride dissolved in water d. air trapped inside an inflated balloon ANS: A PTS: 1 REF: p. 22 BLM: Higher Order 5. Suppose a lighted splint is used to ignite a test tube of hydrogen gas. Which statement about this situation would be at the molecular level of operation? a. A loud popping sound is heard by an observer when ignition occurs. b. After the reaction, condensation appears on the inside surface of the test tube. c. The provided energy breaks some covalent bonds, initiating a series of chemical reactions. d. A chemical reaction occurs that releases heat energy to the surroundings. ANS: C PTS: 1 REF: p. 23 BLM: Higher Order 6. Suppose a lighted splint is used to ignite a test tube of hydrogen gas. Which statement about this situation would be at the symbolic level of operation? a. ANS: A PTS: 1 REF: p. 23 BLM: Higher Order 7. Which of the following elements exists as separate, individual atoms? a. bromine b. neon c. phosphorus d. zinc ANS: B PTS: 1 REF: p. 24 BLM: Remember 8. Which of the following formulas represents an elemental substance? a. C60 The chemical equation for the reaction is 2H2(g) + O2(g) 2H2O(l). b. After the reaction, condensation appears on the inside surface of the test tube. c. The reaction of hydrogen and oxygen releases heat to the surroundings. d. In the reaction, 1.0 g of hydrogen combines with 8.0 g of oxygen. b. NO c. HI d. CS2 ANS: A PTS: 1 REF: p. 24 BLM: Higher Order Copyright © 2015 Nelson Education Limited 2-2 Chapter 2 Mahaffy International 2e TB 9. What is the symbol for chromium? a. Ch b. Co c. Cr d. Cu ANS: C PTS: 1 10. What is the symbol for silver? a. Ag b. Au c. Se d. Sr ANS: A PTS: 1 REF: p. 24–25 REF: p. 24–25 BLM: Remember BLM: Remember BLM: Remember BLM: Remember 11. What is the name of the element with the symbol Ar? a. americium b. argentum c. argon d. arsenic ANS: C PTS: 1 REF: p. 24–25 12. What is the name of the element with the symbol W? a. darmstadtium b. hafnium c. tungsten d. wolfium ANS: C PTS: 1 REF: p. 24–25 13. How is a mixture of iron and sulfur different from a compound of these elements? a. A mixture has a fixed composition of iron and sulfur, but a compound does not. b. A mixture is more difficult to separate into iron and sulfur than a compound. c. A mixture is a homogeneous substance, but a compound is heterogeneous. d. A mixture shows the properties of iron and sulfur, but a compound does not. ANS: D PTS: 1 REF: p. 25 BLM: Remember 14. Which of the following formulas represents a chemical compound? a. Cl2 b. CO c. Co d. O3 ANS: B PTS: 1 REF: p. 26 BLM: Higher Order Copyright © 2015 Nelson Education Limited 2-3 Chapter 2 Mahaffy International 2e TB 15. Which of the following is a chemical property? a. the flammability of phosphorus b. the electrical conductivity of aluminum c. the malleability of gold d. the viscosity of antifreeze ANS: A PTS: 1 REF: p. 27 BLM: Higher Order 16. Which of the following is an example of a chemical change? a. Sodium chloride melts at 801 oC. b. The density of water decreases when it changes from a liquid to a solid. c. Silver cutlery tarnishes after a few weeks. d. Steam condenses on a cold surface. ANS: C PTS: 1 REF: p. 27 BLM: Higher Order 17. When ethanol undergoes complete combustion, the reaction equation is C2H5OH(l) + 3 O2(g) 2 CO2(g) + 3 H2O(g). What information does this equation provide? a. The chemical reaction releases heat energy. b. This reaction takes place in the gas phase. c. The number of molecules in the reaction vessel changes. d. The redistribution of atoms represents a spontaneous reaction. ANS: C PTS: 1 REF: p. 27 BLM: Higher Order 18. Iron metal is produced from iron oxide by reacting iron oxide with carbon monoxide. Which of the following equations represents this reaction? a. b. c. d. ANS: A Fe2O3(s) + Fe2O3(s) + 3 Fe2O3(s) 2 Fe2O3(s) 3 CO(g) 3 C(s) CO(g) 4 Fe(s) PTS: 1 2 Fe(s) + 3 CO2(g) 2 Fe(s) + 3 CO(g) + 2 Fe3O4(s) + CO2(g) 3 O2(g) REF: p. 27 19. Which of the following is NOT a physical property? a. the viscosity of motor oil at minus 20 oC b. the flash point of alcohol c. the melting point of gold d. the electrical conductivity of copper wire ANS: B PTS: 1 REF: p. 28 BLM: Higher Order BLM: Higher Order 20. How many protons, neutrons, and electrons are in an yttrium-89 atom? a. 39 protons, 50 neutrons, 39 electrons b. 39 protons, 89 neutrons, 39 electrons c. 50 protons, 39 neutrons, 50 electrons d. 39 protons, 11 neutrons, 39 electrons ANS: A PTS: 1 REF: p. 29 BLM: Higher Order Copyright © 2015 Nelson Education Limited 2-4 + Chapter 2 21. Which two of the following atoms are isotopes? ,,, Mahaffy International 2e TB a. b. c. d. ANS: D and and and and PTS: 1 REF: p. 29 BLM: Higher Order 22. What is the atomic symbol for an element with 38 protons and 50 neutrons? a. b. c. d. ANS: B PTS: 1 REF: p. 29–30 BLM: Higher Order 23. Which two of the atoms below have the same number of neutrons? ,,, a. b. c. d. and and and and ANS: A PTS: 1 REF: p. 29–30 REF: p. 32 BLM: Higher Order BLM: Remember BLM: Remember 24. How is an atomic mass unit (u) defined? a. the mass of one hydrogen-1 atom b. 1/12 the mass of one carbon-12 atom c. 1/16 the mass of one oxygen-16 atom d. the mass of one proton ANS: B PTS: 1 25. What is the role of the magnets in a mass spectrometer? a. to ionize the vaporized sample b. to accelerate the ionized particles of the sample c. to deflect the ionized particles of the sample d. to focus the ionized particles into a narrow beam ANS: C PTS: 1 REF: p. 33 Copyright © 2015 Nelson Education Limited 2-5 Chapter 2 Mahaffy International 2e TB 26. What properties are used to separate particles in a mass spectrometer? a. mass and size b. mass and charge c. mass and reactivity d. mass and density ANS: B PTS: 1 REF: p. 33 BLM: Remember 27. Suppose an element consists of two isotopes. The abundance of one isotope is 60.1%, and its atomic mass is 68.9 u. The atomic mass of the second isotope is 70.9 u. What is the average atomic mass of the element? a. 69.5 u b. 69.7 u c. 69.9 u d. 70.1 u ANS: B PTS: 1 REF: p. 33–34 BLM: Higher Order 28. Cesium has only one stable isotope. What is the atomic mass of this isotope? a. 131. b. 132. c. 133. d. 134. ANS: B PTS: 1 REF: p. 33–34 BLM: Higher Order 29. Antimony consists of two stable isotopes. The lighter isotope, Sb-121, has atomic mass 120.904 u. The heavier isotope, Sb-123 has atomic mass 122.904 u. What is the percent natural abundance of the lighter stable isotope of antimony? a. 39.0% b. 42.8% c. 57.2% d. 61.0% ANS: C PTS: 1 REF: p. 34 30. Consider the following data. 1 mol Al 2 mol O2 3 mol C 4 mol H2 Which sample has the greatest number of atoms? a. Al b. O2 c. C d. H2 ANS: D PTS: 1 REF: p. 35 BLM: Higher Order Copyright © 2015 Nelson Education Limited 2-6 BLM: Higher Order Chapter 2 Mahaffy International 2e TB 31. Consider the following data. 1 mol Al 2 mol O2 3 mol C 4 mol H2 Which sample has the greatest mass? a. Al b. O2 c. C d. H2 ANS: B PTS: 1 REF: p. 35 BLM: Higher Order 32. Lithium metal has a density of 0.535 g/mL. How many moles of lithium atoms are present in a cube of the metal with sides of 2.00 cm? a. 0.154 mol b. 0.539 mol c. 0.617 mol d. 2.15 mol ANS: C PTS: 1 REF: p. 36–37 BLM: Higher Order 33. What is the mass of tin that contains the same number of atoms as there are in 100.0 g of lead? a. 57.29 g b. 60.97 g c. 164.0 g d. 174.6 g ANS: A PTS: 1 REF: p. 36–37 34. What is the mass of 2.41x1022 atoms of the element boron? a. 0.432 g b. 4.32 g c. 27.0 g d. 270 g ANS: A PTS: 1 REF: p. 36–37 BLM: Higher Order BLM: Higher Order 35. What type of elements are found in the upper-right corner of the periodic table? a. main group metals b. transition metals c. metalloids d. non-metals ANS: D PTS: 1 REF: p. 38 BLM: Remember 36. Which group in the periodic table contains metallic, non-metallic, and metalloid elements? a. 11 b. 13 c. 15 d. 17 ANS: C PTS: 1 REF: p. 38 Copyright © 2015 Nelson Education Limited BLM: Remember 2-7 Chapter 2 Mahaffy International 2e TB 37. Which of the following did Mendeleev NOT do when he constructed his version of the periodic table? a. leave gaps for undiscovered elements b. place elements with similar properties in the same horizontal row c. order the elements on the basis of increasing atomic mass d. correctly predict the properties of some undiscovered elements ANS: B PTS: 1 REF: p. 39 BLM: Remember 38. In which of the following groups are the three elements likely to have similar chemical and physical properties? a. boron, silicon, and germanium b. sodium, magnesium, and aluminum c. magnesium, calcium, and strontium d. carbon, nitrogen, and oxygen ANS: C PTS: 1 REF: p. 39 BLM: Higher Order COMPLETION 1. Homogeneous mixtures can also be referred to as ____________________. ANS: solutions PTS: 1 REF: p. 22 BLM: Remember 2. Since the composition of a mixture can vary, it is impossible to assign a mixture a chemical ____________________. ANS: formula PTS: 1 REF: p. 26 BLM: Remember 3. For an atom of an element, the symbol Z represents the number of ____________________. ANS: protons PTS: 1 REF: p. 29 BLM: Remember 4. The atomic weight of an element is the average relative atomic mass of a representative sample of its atoms, taking into account the ____________________. ANS: relative abundances of its isotopes PTS: 1 REF: p. 29 BLM: Remember Copyright © 2015 Nelson Education Limited 2-8 Chapter 2 Mahaffy International 2e TB SHORT ANSWER 1. How can isotope ratio mass spectrometry tell whether testosterone in an athlete’s body is exogenous or endogenous? ANS: The ratio of the carbon-12 and carbon-13 isotopes in the testosterone is different for the two sources of the hormone. Measuring the ratio of the two isotopes will therefore determine whether the testosterone was naturally produced by the athlete or added illegally to the body. PTS: 1 REF: p. 19 BLM: Remember 2. State TWO similarities of liquids and solids. ANS: 1. The particles are closely packed. 2. Solids and liquids both have fixed volumes. PTS: 1 REF: p. 21 BLM: Remember 3. In devising a model of the atom, a student used a one-cent coin of diameter 2 cm to represent the diameter of the nucleus. Estimate the radius of the atom in this model. ANS: The radius of the atom is about 105 times as large as the radius of the nucleus. This makes the diameter of the atom 2000 m, and its radius 1000 m or 1 km. PTS: 1 REF: p. 28 BLM: Higher Order 4. Give the atomic notation for an element with 53 protons and 78 neutrons. ANS: PTS: 1 REF: p. 29 BLM: Higher Order 5. The element boron consists of two isotopes, boron-10 (10.0129 u) and boron-11 (11.0093 u). If a sample of boron from another planet in our galaxy were found to have an atomic mass of 10.724, what would be the percentage abundances of the two isotopes? ANS: Boron-10—28.63% Boron-11—71.37% PTS: 1 REF: p. 33 BLM: Higher Order Copyright © 2015 Nelson Education Limited 2-9 Chapter 2 Mahaffy International 2e TB PROBLEM 1. What mass of fluorine gas, F2, will contain the same number of molecules as there are in 92.91 g of phosphorus, P4? ANS: 28.50 g PTS: 1 REF: p. 37 BLM: Higher Order 2. What is the mass of 1.8066x1022 molecules of sulfur, S8? ANS: 76.968 g PTS: 1 REF: p. 37 BLM: Higher Order Copyright © 2015 Nelson Education Limited 2-10 Chapter 3—Models of Structure to Explain Properties TRUE/FALSE 1. Typical $20 bills in Canada are found to contain less than one nanogram of cocaine; $20 bills associated with criminal cases are found to contain 50 to 1000 nanograms of cocaine. ANS: T PTS: 1 REF: p. 50 BLM: Remember 2. Chlorine forms ions that have the same number of electrons as neon. ANS: F PTS: 1 REF: p. 58 BLM: Higher Order 3. Intermolecular forces of attraction hold atoms together in molecules. ANS: F PTS: 1 REF: p. 64 BLM: Higher Order 4. Intramolecular covalent bonds remain intact when a molecular substance is melted. ANS: T PTS: 1 REF: p. 64 BLM: Higher Order 5. The electrons around each atom within a molecule are best imagined as a disperse “cloud” of negatively charged matter around the nucleus. ANS: T PTS: 1 REF: p. 66 BLM: Higher Order 6. The number of shared electrons between two atoms has no effect on the strength of the bond. ANS: F PTS: 1 REF: p. 67 BLM: Higher Order 7. The energy of infrared radiation required to cause a carbon-carbon single bond to vibrate is higher than a carbon-carbon double bond. ANS: F PTS: 1 REF: p. 67 BLM: Higher Order Copyright © 2015 Nelson Education Limited 3-1 Chapter 3 Mahaffy International 2e TB MULTIPLE CHOICE 1. When a Canadian $20 banknote is examined for forensic evidence, what is the approximate mass of cocaine detected by the mass spectrometer? a. 0.13–0.49 milligrams b. 0.13–0.49 micrograms c. 0.13–0.49 nanograms d. 0.13–0.49 picograms ANS: C PTS: 1 REF: p. 50 2. What type of substance melts at –114 oC and boils at 78 oC? a. ionic b. metallic c. covalent network d. molecular ANS: D PTS: 1 REF: p. 50 BLM: Higher Order BLM: Higher Order 3. What type of substance melts at 801 oC, dissolves easily in water, and conducts electricity when in solution? a. ionic b. metallic c. covalent network d. molecular ANS: A PTS: 1 REF: p. 52 BLM: Higher Order 4. What type of substance is a black powder that decomposes at 2730 oC, does not conduct electricity, and is extremely hard? a. ionic b. metallic c. covalent network d. molecular ANS: C PTS: 1 REF: p. 53 BLM: Higher Order 5. Which of the following is the only covalent network solid that conducts electricity? a. silicon carbide b. diamond c. germanium dioxide d. graphite ANS: D PTS: 1 REF: p. 53 BLM: Higher Order Copyright © 2015 Nelson Education Limited 3-2 Chapter 3 Mahaffy International 2e TB 6. What type of bond connects the atoms in the crystal lattice of diamond? a. ionic b. covalent c. hydrogen d. metallic ANS: B PTS: 1 REF: p. 53 7. Why does a covalent network solid NOT conduct electricity? a. The atoms are uncharged. b. The atoms cannot move. c. There are no electrons. d. Too much energy is required. ANS: A PTS: 1 REF: p. 53 BLM: Higher Order BLM: Higher Order 8. The distortion of an ionic solid causes displacement of layers and results in repulsions between particles. This fact is responsible for which of the following properties? a. high melting point b. electrical conductivity c. hardness d. brittleness ANS: D PTS: 1 REF: p. 55 BLM: Higher Order 9. What would be the charge of the most easily formed ion of a Group 13 element? a. –3 b. –1 c. +1 d. +3 ANS: D PTS: 1 REF: p. 56 BLM: Higher Order 10. What would be the charge of the most easily formed ion of a Group 2 metal? a. –2 b. –1 c. +1 d. +2 ANS: D PTS: 1 REF: p. 56 BLM: Higher Order 11. How many electrons are there in the common anion of sulfur? a. 14 b. 16 c. 18 d. 20 ANS: C PTS: 1 REF: p. 57 BLM: Higher Order Copyright © 2015 Nelson Education Limited 3-3 Chapter 3 Mahaffy International 2e TB 12. Which of the following is the correct number of protons and electrons for the iron(III) ion? a. 26 protons, 26 electrons b. 26 protons, 23 electrons c. 23 protons, 26 electrons d. 23 protons, 23 electrons ANS: B PTS: 1 REF: p. 57 BLM: Higher Order 13. Which of the following is the correct number of protons and electrons for the potassium ion? a. 18 protons, 18 electrons b. 18 protons, 19 electrons c. 19 protons, 18 electrons d. 19 protons, 19 electrons ANS: C PTS: 1 REF: p. 57 BLM: Higher Order 14. Which noble gas has the same number of electrons as a strontium ion? a. neon b. argon c. krypton d. xenon ANS: C PTS: 1 15. Which of the following is ionic? a. FeCl3 b. NCl3 c. ClF3 d. OF2 ANS: A PTS: 1 16. What is the correct name for Sn2+? a. tin two plus b. tin(II) cation c. stannide d. tin cation ANS: B PTS: 1 REF: p. 58 REF: p. 59 REF: p. 59 BLM: Higher Order BLM: Higher Order BLM: Higher Order 17. Which of the following terms describe the bonding between atoms of a polyatomic ion? a. covalent bonds b. hydrogen bonds c. ionic bonds d. disulfide bonds ANS: A PTS: 1 REF: p. 59 BLM: Higher Order Copyright © 2015 Nelson Education Limited 3-4 Chapter 3 Mahaffy International 2e TB 18. Which of the following is the correct formula for the ionic compound composed of calcium cations and nitrite anions? a. Ca3N2 b. Ca(NO2)2 c. Ca(NO3)2 d. Ca(NO)2 ANS: B PTS: 1 REF: p. 59 BLM: Higher Order 19. Which of the following is the correct formula for the ionic compound composed of potassium and permanganate ions? a. KMnO4 b. K2MnO4 c. KMn2O7 d. K2Mn2O7 ANS: A PTS: 1 REF: p. 59 BLM: Higher Order 20. Which of the following formulae has an overall charge (or net charge) of zero? a. Ca3N2 b. NaCl2 c. SrF3 d. KS ANS: A PTS: 1 REF: p. 59 BLM: Higher Order 21. Which of the following samples has the largest number of ions? a. 1.0 mole of FeS2 b. 1.0 mole of SiC c. 1.0 mole of CaSO4 d. 1.0 mole of Ca(NO3)2 ANS: D PTS: 1 REF: p. 59 BLM: Higher Order 22. Which of the following is the correct molar mass for magnesium dihydrogenphosphate in grams per mole? a. 121.29 b. 120.28 c. 218.28 d. 216.26 ANS: C PTS: 1 REF: p. 60–61 BLM: Higher Order 23. Which of the following is the correct molar mass for sodium perchlorate in grams per mole? a. 74.44 b. 90.44 c. 106.44 d. 122.44 ANS: D PTS: 1 REF: p. 60–61 Copyright © 2015 Nelson Education Limited BLM: Higher Order 3-5 Chapter 3 Mahaffy International 2e TB 24. What kind of substance is a shiny solid that melts at 727 oC and conducts electricity in both the solid and liquid state? a. ionic b. metallic c. covalent network d. molecular ANS: B PTS: 1 REF: p. 62 BLM: Higher Order 25. Which of the following is the best description of metallic bonding? a. Electrons are shared between two atoms. b. Electrons move freely through the lattice. c. Electrons are transferred from one atom to another. d. Electrons move freely throughout the molecule. ANS: B PTS: 1 REF: p. 62 BLM: Higher Order 26. Metallic bonding is retained even if distortion of the metal causes regions of ions to be displaced with respect to each other. This fact is responsible for which of the following properties? a. thermal conduction b. density c. malleability d. lustre ANS: C PTS: 1 REF: p. 62 27. What is the principle force that forms a covalent bond? a. the repulsion between the electrons b. the attraction of each nucleus for the shared electrons c. the repulsion between the nuclei d. the attraction of each nucleus for its electrons ANS: B PTS: 1 REF: p. 66 BLM: Higher Order BLM: Higher Order 28. Which is the correct definition of an isotopologue? a. molecules that are identical except for the three dimensional arrangement of their atoms b. molecules that contain the least abundant isotope of each atom c. molecules that are identical except that their atoms have different isotopic compositions d. molecules that always contain a carbon-12 isotope ANS: C PTS: 1 REF: p. 68 BLM: Higher Order Copyright © 2015 Nelson Education Limited 3-6 Chapter 3 Mahaffy International 2e TB 29. The mass of a molecular ion as measured in a high-resolution mass spectrometer is 30.01057. The exact masses of the most abundant ions are as follows: carbon 12C 12.00000 oxygen 16O 15.99491 hydrogen 1H 1.00783 nitrogen 14N 14.00307 Using the above data, which of the following is the formula of the most abundant isotopolgue? a. N2H2 b. CH2NH2 c. CH2O d. NO ANS: C PTS: 1 REF: p. 68 BLM: Higher Order 30. Use the average atomic mass on a periodic table and determine the molar mass of aniline (molecular formula C6H5NH2) to two decimal places. Which of the following measurements is correct? a. 93.13 g mol–1 b. 93.16 g mol–1 c. 94.13 g mol–1 d. 94.16 g mol–1 ANS: A PTS: 1 REF: p. 69 BLM: Higher Order 31. A drop of acetone, C3H6O, has a volume of about 0.05 mL. If acetone has a density of 0.79 g 3 cm , how many molecules of acetone are in a drop of acetone? a. 4x1023 b. 6x1020 c. 4x1020 d. 7x101 ANS: C PTS: 1 REF: p. 69 BLM: Higher Order 32. Which of the following indicates the presence of chlorine in a mass spectrum? a. two peaks, two m/z units apart, with peak heights in a 1:1 ratio of low mass versus higher mass b. two peaks, one m/z unit apart, with peak heights in a 10:1 ratio of low mass versus higher mass c. one peak at m/z = 63 and a peak at m/z = 65 d. two peaks, two m/z units apart, with peak heights in a 3:1 ratio of low mass versus higher mass ANS: D PTS: 1 REF: p. 70 BLM: Higher Order