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- Herausgeber: John Wiley & Sons
- Kategorie: Wissenschaft und neue Technologien
- Sprache: Englisch
Practice your way to a better grade in your Chemistry class
Chemistry: 1001 Practice Problems For Dummies gives you 1,001 opportunities to practice solving problems on all the topics covered in your chemistry class—in the book and online! Get extra practice with tricky subjects, solidify what you’ve already learned, and get in-depth walk-throughs for every problem with this useful book. These practice problems and detailed answer explanations will catalyze the reactions in your brain, no matter what your skill level. Thanks to Dummies, you have a resource to help you put key concepts into practice.
- Work through multiple-choice practice problems on all Chemistry topics covered in class
- Step through detailed solutions to build your understanding
- Access practice questions online to study anywhere, any time
- Improve your grade and up your study game with practice, practice, practice
The material presented in Chemistry: 1001 Practice Problems For Dummies is an excellent resource for students, as well as parents and tutors looking to help supplement classroom instruction.
Chemistry: 1001 Practice Problems For Dummies (9781119883531) was previously published as 1,001 Chemistry Practice Problems For Dummies (9781118549322). While this version features a new Dummies cover and design, the content is the same as the prior release and should not be considered a new or updated product.
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Chemistry: 1001 Practice Problems For Dummies®
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Copyright © 2022 by John Wiley & Sons, Inc., Hoboken, New Jersey
Published simultaneously in Canada
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Library of Congress Control Number: 2022934818
ISBN 978-1-119-88353-1 (pbk); ISBN 978-1-119-88354-8 (ebk); ISBN 978-1-119-88355-5 (ebk)
Chemistry: 1001 Practice Problems For Dummies®
To view this book's Cheat Sheet, simply go to www.dummies.com and search for “Chemistry: 1001 Practice Problems For Dummies Cheat Sheet” in the Search box.
Table of Contents
Cover
Title Page
Copyright
Introduction
What You’ll Find
Beyond the Book
Where to Go for Additional Help
Part 1: The Questions
Chapter 1: Units and Unit Conversions
The Problems You’ll Work On
What to Watch Out For
Understanding Metric Prefixes and Units
Choosing Appropriate Units
Doing Metric Conversions
Converting between Systems of Measurement
Using Dimensional Analysis
Chapter 2: Scientific Notation and Significant Figures
The Problems You’ll Work On
What to Watch Out For
Putting Numbers in Scientific Notation
Taking Numbers out of Scientific Notation
Calculating with Numbers in Scientific Notation
Recognizing Significant Figures
Writing Answers with the Right Number of Sig Figs
Chapter 3: Matter and Energy
The Problems You’ll Work On
What to Watch Out For
Phases of Matter and Phase Changes
Classifying Substances and Mixtures
Properties of Matter
Calculating Density
Working with Energy
Chapter 4: The Atom and Nuclear Chemistry
The Problems You’ll Work On
What to Watch Out For
Isotopes and Subatomic Particles
Electrons and Quantum Mechanics
Average Atomic Mass
Nuclear Reactions and Nuclear Decay
Completing Nuclear Reactions
Half-Lives
Chapter 5: Periodicity and the Periodic Table
The Problems You’ll Work On
What to Watch Out For
Element Symbols and Names
Structure of the Periodic Table
Periodic Trends
Chapter 6: Ionic Bonding
The Problems You’ll Work On
What to Watch Out For
Naming Binary Compounds
Naming Compounds with Polyatomic Ions
Writing Formulas of Binary Compounds
Writing Formulas of Compounds with Polyatomic Ions
Chapter 7: Covalent Bonding
The Problems You’ll Work On
What to Watch Out For
Prefixes in Covalent — Compound Names
Naming Covalent Compounds
Writing Formulas of Covalent Compounds
Chapter 8: Molecular Geometry
The Problems You’ll Work On
What to Watch Out For
Valence Electrons
Predicting Bond Types
Basic Molecular Shapes
Exceptional Molecular Shapes
Polarity of Molecules
Chapter 9: Chemical Reactions
The Problems You’ll Work On
What to Watch Out For
Classifying Reactions from Chemical Equations
Classifying Reactions from Word Equations
Predicting Reactions
Balancing Chemical Reactions
Balancing Reactions from Word Equations
Predicting Products and Balancing Reactions
Redox and Acid-Base Reactions
Chapter 10: Molar Calculations
The Problems You’ll Work On
What to Watch Out For
Calculating Molar Mass
Finding Mass Percent
Empirical Formulas
Molecular Formulas
Mole Calculations
Percent Yield
Limiting Reactants
Chapter 11: Thermochemistry
The Problems You’ll Work On
What to Watch Out For
Converting Temperatures
Phase Changes and Energy
Specific Heat and Calorimetry
Heats of Formation
Enthalpy Changes with Hess’s Law
Chapter 12: Gases
The Problems You’ll Work On
What to Watch Out For
Converting Pressure Units
Boyle’s Law
Charles’s Law
Gay-Lussac’s Law
The Combined Gas Law
Avogadro’s Law
The Ideal Gas Law
Dalton’s Law of Partial Pressures
Graham’s Law
Gas Stoichiometry
Chapter 13: Solutions (The Chemistry Kind)
The Problems You’ll Work On
What to Watch Out For
Solutions, Solvents, and Solutes
Concentration Calculations
Dilution
Molality
Colligative Properties
Chapter 14: Acids and Bases
The Problems You’ll Work On
What to Watch Out For
Identifying Acids and Bases
Conjugate Acids and Bases
Finding pH and pOH of Strong Acids and Bases
Finding pH and pOH of Weak Acids and Bases
Stoichiometry of Titrations
Buffer Solutions
Titrations and pH Changes
Chapter 15: Graphing Basics
The Problems You’ll Work On
What to Watch Out For
Graphing
Part 2: The Answers
Chapter 16: Answers and Explanations
Appendix: The Periodic Table of Elements
Index
About the Authors
Advertisement Page
Connect with Dummies
End User License Agreement
Guide
Cover
Title Page
Copyright
Table of Contents
Begin Reading
Appendix: The Periodic Table of Elements
Index
About the Authors
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Introduction
Whether you’re taking your first chemistry course, you’re taking your last chemistry course, or you just need a little practice before taking a test that contains chemistry questions (like a nursing, pre-med, or teacher certification test), doing problems is a fine way to prepare.
The 1,001 practice questions in this book cover topics that you might encounter in a high school chemistry course, an introductory college chemistry course, the first semester of a general chemistry course for science majors, or a general science test for entry into a pre-professional program. The types of questions found here are similar to the ones you may see on homework assignments, quizzes, practice tests, or actual tests.
You can start at Question 1 or Question 121 or skip around. You may find that your instructor (or textbook) covers topics in a different order from this book. That’s okay; just go to the table of contents, find the topic you need, and start there.
Completing 1,001 chemistry practice questions is no small undertaking, but the time you spend practicing valuable science, math, and chemistry skills can improve your scores and help you “know what you know.”
What You’ll Find
The 1,001 chemistry practice questions in this book are divided among 15 chapters, each one representing a few major subject areas in chemistry. Within each chapter, questions are grouped by topic and arranged from easy to hard, allowing you to answer beginner questions as well as multi-step and more difficult questions. Some questions are accompanied by an image or diagram that you need in order to answer the question correctly.
After you answer the questions for one chapter or subcategory — or even after you answer just one question — you can flip to the last chapter of the book and check your answers. There, you find thorough answer explanations for each problem, often covering processes, formulas, and definitions. In many cases, studying an answer explanation can help you better understand a difficult subject, so spend as much time as you need reviewing the explanations.
Beyond the Book
In addition to what you’re reading right now, this book comes with a free, access-anywhere Cheat Sheet that includes tips and other goodies you may want to have at your fingertips. To get this Cheat Sheet, simply go to www.dummies.com and type Chemistry: 1001 Dummies Cheat Sheet into the Search box.
The online practice that comes free with this book offers you the same 1,001 questions and answers that are available here, but presented in a multiple-choice format. The beauty of the online problems is that you can customize your online practice to focus on the topic areas that give you trouble. If you’re short on time and want to maximize your study, you can specify the quantity of problems you want to practice, pick your topics, and go. You can practice a few hundred problems in one sitting or just a couple dozen, and you can focus on a few types of problems or a mix of several types. Regardless of the combination you create, the online program keeps track of the questions you get right and wrong so you can monitor your progress and spend time studying exactly what you need to.
To gain access to the online practice, you simply have to register. Just follow these steps:
Register your book or ebook at Dummies.com to get your PIN. Go to
www.dummies.com/go/getaccess
.
Select your product from the drop-down list on that page.
Follow the prompts to validate your product, and then check your email for a confirmation message that includes your PIN and instructions for logging in.
If you don’t receive this email within two hours, please check your spam folder before contacting us through our Technical Support website at http://support.wiley.com or by phone at 877-762-2974.
Now you’re ready to go! You can come back to the practice material as often as you want — simply log in with the username and password you created during your initial login. No need to enter the access code a second time.
Your registration is good for one year from the day you activate your PIN.
Where to Go for Additional Help
It’s easy to get overwhelmed when trying to study a subject as multifaceted as chemistry. But don’t despair. This book is designed to break everything into less complex categories so you can concentrate on one topic at a time. Practicing in smaller areas within each topic helps you identify your strong points and your weak points.
After you use this book and identify the areas you feel need extra effort, you can start studying on your own and then come back here to answer the questions again to measure your improvement. For example, if your knowledge of molarity is a little hazy (or nonexistent), try reviewing the molar calculations in Chapter 10. Check your answers and jot down notes or questions you may have. Then research, say, how solution concentration is expressed using molarity or which biology applications might use molarity. You can look for resources at your local library or online, or you can ask a friend, coworker, or professor to coach you if they seem to spend a lot of time in the lab. You can also check out the For Dummies series for books about many of the topics covered in chemistry. Head to www.dummies.com to see the many books and articles that can help you in your studies.
Chemistry: 1001 Practice Problems For Dummies gives you just that — 1,001 practice questions and answers in order for you to practice your chemistry skills. If you need more in-depth study and direction for your chemistry courses, you may want to try out the following For Dummies products.
Chemistry Essentials For Dummies:
This book is a quick-reference resource that outlines key topics found in a first-year high school chemistry course or a first-semester college chemistry course.
Chemistry For Dummies:
This book provides content parallel to the 1,001 chemistry practice problems found in this book.
Chemistry II For Dummies:
This book provides content similar to what you may encounter in a second-year high school chemistry course or a second-semester college chemistry course.
AP Chemistry For Dummies:
This book prepares the Advanced Placement chemistry student to take the College Board’s AP Chemistry exam. It also includes tools for organizing and planning your study time.
Chemistry Workbook For Dummies:
This book includes basic instruction, chemistry problems with step-by-step solutions, shortcuts, and more practice problems.
Several For Dummies chemistry titles are also available for download to your electronic devices.
Part 1
The Questions
IN THIS PART …
One thousand one chemistry problems — that’s a lot of chemistry practice. Hundreds of our former students have persevered through what we’re sure they felt was even more than that. Here are the general types of questions you’ll be dealing with:
The basics of chemistry (
Chapters 1
–
5
)
Chemical bonding (
Chapters 6
–
8
)
Chemical reactions (
Chapters 9
–
11
)
Gases, acids, bases, and liquids (
Chapters 12
–
14
)
Graphing (
Chapter 15
)
Chapter 1
Units and Unit Conversions
Many aspects of chemistry are quantitative, and you use units to measure these quantities. In many cases, you have to convert from one unit to another. Most people in the United States initially learn the English system of units, but most chemists use the Système international d’unités (the SI system), derived from the older metric system. Unit conversions relate these two systems. Dimensional analysis provides a systematic means to not only perform these conversions but also to work many of the other problems in this book. Dimensional analysis lets the units solve the problem for you.
The Problems You’ll Work On
In this chapter, you work with units and unit conversions in the following ways:
Choosing appropriate units
Interpreting metric prefixes
Converting metric and English units
Solving problems with dimensional analysis
What to Watch Out For
Don’t let common mistakes trip you up; remember the following when working on units and unit conversions:
Always include your units when setting up equations and answering questions.
Set up your problem so that units cancel to leave the desired units.
Make sure your answer looks reasonable and the final units match what they describe. For example, s
–1
represents 1/seconds, which is frequency, not time.
When rounding your answer for significant figures, remember that many, but not all, conversions are exact numbers and therefore don’t affect the number of significant figures in the answer.
Understanding Metric Prefixes and Units
1–10 Answer the questions on metric prefixes and metric units used in the laboratory.
1. What is a common metric unit of mass used in the laboratory?
2. What is a common metric unit of length used for measuring small objects in the laboratory?
3. What is a common metric unit of volume used in the laboratory?
4. What is a common metric unit of pressure used in the laboratory?
5. What is a common metric unit of energy?
6. What is the metric prefix that represents 1,000?
7. What is the metric prefix that represents ?
8. What is the metric prefix that represents ?
9. What is the metric prefix that represents 10–9?
10. What is the metric prefix that represents 106?
Choosing Appropriate Units
11–20 Choose appropriate metric or English units for measuring everyday objects.
11. Which metric unit is most appropriate for expressing the mass of an adult human?
12. Which metric unit is most appropriate for recording the volume of a child’s wooden block?
13. Which metric unit would a scientist use to measure the temperature on a warm autumn day?
14. Which metric unit is most often used for small doses of solid medications?
15. Which SI base unit is named after a person?
16. Which English unit is most similar in volume to a liter?
17. Which English unit is most similar in length to a meter?
18. How many fluid ounces are in a cup?
19. An Olympic swimmer competes in the 100-meter freestyle. What is the comparable English unit?
20. If a wooden board’s width is 6 in., what is an appropriate metric unit to express this width?
Doing Metric Conversions
21–32 Complete the conversion between metric units.
21. How many milligrams are in 1 dg?
22. How many deciliters are in 1 L?
23. How many kilometers are in 1 m?
24. How many centimeters are in 1 m?
25. How many grams are in 1 hg?
26. How many milliliters are in 2.5 daL?
27. How many centigrams are in 49 kg?
28. How many gigawatts are in 370,000 W?
29. How many micrograms are in 0.126 Mg?
30. How many kilometers are in 80 pm?
31. How many cubic meters are in 2 L?
32. How many milliliters are in 0.64 m3?
Converting between Systems of Measurement
33–59Convert between metric and English units.
33. How many miles are in 35 km?
34. How many inches are in 0.20 cm?
35. How many yards are in 202 m?
36. How many pounds are in 58 kg?
37. How many quarts are in 7.54 L?
38. How many centimeters are in 0.087 in.?
39. How many kilometers are in 463 mi.?
40. How many grams are in 91 lb.?
41. How many liters are in 525 gal.?
42. How many atmospheres are in 44 psi?
43. How many cups are in 2.00 L?
44. How many pounds are in 164 hg?
45. How many gallons are in 587 mL?
46. How many centimeters are in 6.02 mi.?
47. How many decigrams are in 225 lb.?
48. How many milliliters are in 6.8 qt.?
49. How many centimeters are in 15.3 ft.?
50. How many liters are in 99 pt.?
51. How many kilograms are in 1.00 short ton?
52. How many centimeters are in 6.04 yd.?
53. How many cups are in 15 cc?
54. How many millimeters are in 1,760 yd.?
55. How many pints are in 250 hL?
56. How many grams are in 0.35 slugs?
57. How many kilometers are in 9,999 in.?
58. How many ounces are in 0.734 kg?
59. How many microliters are in 55 oz.?
Using Dimensional Analysis
60–75 Solve the word problem using a setup similar to those used in unit conversions.
60. How many dozen eggs are in 17,981 eggs?
61. How many years are in 6,250 days?
62. How many weeks are in 2.5 centuries?
63. If the average penny has a mass of 3.16 g, what is the dollar value of 1.00 short ton of pennies?
64. If an athlete runs the 100-yard dash in 10.0 s, how long will it take for the athlete to run 400 m?
65. You’re planning a party and need enough soda for 60 guests. How many liters will you need, assuming each guest drinks 10 fl. oz. of soda?
66. You plan to serve sub sandwiches at a party. How many 6.0-foot subs will you need to feed the 60 guests if each person eats a 25.4-cm length of sandwich?
67. A textbook measures 230 mm long, 274 mm wide, and 60.0 mm thick. What is the volume in cubic centimeters?
68. A textbook measures 230 mm long, 274 mm wide, and 60.0 mm thick. What is the surface area of the front cover in square meters?
69. A hallway measures 10.0 ft. by 5.0 ft. How many square tiles, measuring 10.0 in. on each side, are necessary to cover the floor?
70. If a car is going 20 mph through a school zone, how many centimeters per minute is it traveling?
71. A solid sphere made of pure gold has a volume of 2.0 L. What is the mass of the sphere, in pounds, if 1.00 cm3 of gold has a mass of 19.3 g?
72. How many minutes does it take a horse to run 12 furlongs at 35.3 mph?
73. If a pitcher throws a 96-mph fastball, how many seconds will it take to travel the 60.5 ft. from the pitcher’s mound to home plate?
74. Pure gold can be made into extremely thin sheets called gold leaf. Suppose that 25 kg of gold is made into gold leaf having a surface area of 1,810 m2. How thick is the gold leaf in millimeters? The density of gold is 19.3 g/cm3.
75. Radio waves travel at 300,000,000 m/s. If you asked a question of someone who was on the moon, 239,000 mi. from the Earth, what is the minimum time that you would have to wait for a reply?
Chapter 2
Scientific Notation and Significant Figures
Scientific notation allows you to write very large and very small numbers, which are common in chemistry, in a simplified manner. Many chemical experiments involve very precise measurements. The significant figures are an indication of the precision of these measurements. In calculations involving more than one measurement, you need to maintain the precision inherent in the significant figures.
The Problems You’ll Work On
In this chapter, you work with scientific notation and significant figures in the following ways:
Expressing numbers in standard and scientific notation
Doing calculations with numbers in scientific notation
Determining significant figures
Combining math operations with significant figures
What to Watch Out For
Remember the following when working on scientific notation and significant figures:
All nonzero digits and zeros between nonzero digits are significant. Zeros to the left in the number (leading zeros) are never significant. Zeros to the right are significant only if they aren’t just indicating the power of ten.
Don’t confuse the addition/subtraction rule with the multiplication/division rule. Be extra careful when solving mixed-operation problems.
Most calculators convert to and from scientific notation, but double-check the answer. Calculators are complete idiots concerning the rules for significant figures.
Putting Numbers in Scientific Notation
76–80 Express the given number in scientific notation.
76. 876
77. 4,000,001
78. 0.000510
79. 900 × 104
80. 10
Taking Numbers out of Scientific Notation
81–85 Convert the given number to nonscientific notation (regular decimal form).
81. 2.00 × 102
82. 9 × 10–2
83. 4.7952 × 103
84. 1.64 × 10–5
85. 0.83 × 10–1
Calculating with Numbers in Scientific Notation
86–105 Complete the calculations and record your answer in scientific notation. (If you use a calculator, choose a mode that doesn’t put the numbers in scientific notation for you.)
86.
87.
88.
89.
90.
91.
92.
93.
94.
95.
96.
97.
98.
99.
100.
101.
102.
Chapter 3
Matter and Energy
Chemists deal with matter. Matter occurs in many forms with certain observable properties. One easily observable property of matter is density, which is the mass of a sample of matter divided by its volume. It’s possible to alter matter either physically or chemically. All alterations involve energy.
The Problems You’ll Work On
In this chapter, you work with matter and energy in the following ways:
Describing phases of matter
Classifying matter as substances and mixtures
Understanding properties of matter
Determining density
Calculating energy and temperature
What to Watch Out For
Remember the following when working on matter and energy:
Know the properties of solids, liquids, and gases on microscopic and macroscopic levels.
Remember that a density must have a mass unit divided by a volume unit.
Phases of Matter and Phase Changes
136–143 Check your understanding of phases of matter and phase changes.
136. Which phase of matter doesn’t have a definite shape or a definite volume under normal conditions?
137. Which phase of matter has a definite shape and a definite volume?
138. Which phase of matter has a definite volume but takes the shape of the container that it’s in?
139. When matter changes from a liquid to a solid, which phase change is it going through?
140. When matter changes from a gas to a liquid, which phase change is it going through?
141. When matter changes from a liquid to a gas, which phase change is it going through?
142. When matter changes from a solid to a gas without becoming a liquid in between, which phase change is it going through?
143. When matter changes from a gas to a solid without becoming a liquid in between, which phase change is it going through?
Classifying Substances and Mixtures
144–152 Classify each type of matter as a pure substance or mixture. Then classify each pure substance as an element or compound and each mixture as homogeneous or heterogeneous.
144. Gold
145. Table sugar
146. Fresh air
147. Oxygen
148. Vegetable soup
149. Fruit salad
150. Calcium
151. Concrete
152. Smog
Properties of Matter
153–165 Check your understanding of the properties of matter.
153. Which type of property of matter doesn’t depend on the amount of the substance that’s present?
154. Which type of change involves a change in the form of a substance?
155. Which type of change involves a change in the identity of a substance?
156. Which type of property of matter depends on exactly how much of the substance is present?
157. Density is a(n) _______________ (chemical/extensive physical/intensive physical) property.
158. Length is a(n) _______________ (chemical/extensive physical/intensive physical) property.
159. Color is a(n) _______________ (chemical/extensive physical/intensive physical) property.
160. Flammability is a(n) ___________ (chemical/extensive physical/intensive physical) property.
161. Mass is a(n) _______________ (chemical/extensive physical/intensive physical) property.
162. Odor is a(n) _______________ (chemical/extensive physical/intensive physical) property.
163. Ductility is a(n) _______________ (chemical/extensive physical/intensive physical) property.
164. Electrical conductivity is a(n) _______________ (chemical/extensive physical/intensive physical) property.
165. Solubility is a(n) _______________ (chemical/extensive physical/intensive physical) property.
Calculating Density
166–174 Perform the density calculations. Be sure to round your answers to the correct number of significant figures. (See Chapter2 for significant figure problems.)
166. In grams per cubic centimeter, what is the density of a substance with a mass of 57.5 g and a volume of 5.0 cm3?
167. A 25.0-mL sample of a liquid has a mass of 22.1 g. What is the liquid’s density in grams per milliliter?
168. The mass of 2.00 m3 of a gas is 3,960 g. What is the density of this gas in kilograms per cubic meter?
169. What is the mass, in grams, of 0.200 L of a saltwater solution with a density of 1.2 g/mL?
170. Aluminum is a metal that has a density of 2.7 g/cm3. How many grams are in a solid cube of aluminum that measures 3.00 cm per side?
171. If a block has a length of 5.0 cm, a width of 3.0 cm, a height of 2.0 cm, and a mass of 120 g, what is the block’s density?
172. What is the mass, in kilograms, of 1.5 L of solid gold? Solid gold has a density of 19.3 g/cm3.
173. If a sample of gasoline has a mass of 77.0 g and a density of 0.71 g/mL, what is the volume of the gasoline in milliliters?
174. What is the length of one side of a metallic cube that has a density of 10.5 g/cm3 and a mass of 672 g?
Working with Energy
175–190 Assess your understanding of energy and related calculations.
175. Which unit represents the amount of energy necessary to raise the temperature of 1 g of water by 1°C?
176. Which SI unit is used to express the heat content of a mole of a chemical?
177. Which unit is used to express the energy found in food?
178. A bucket on a ladder has __________ (kinetic/potential) energy, which is the energy of __________ (motion/position).
179. A rolling ball has __________ (kinetic/potential) energy, which is the energy of __________ (motion/position).
180. Fuels contain __________ (moving/stored) energy, which is __________ (kinetic/potential) energy.
181. How many kilocalories are in 25,970 J?
182. How many joules are in 3.1 × 108 kilocalories?
183. Average kinetic energy can be measured in what units?
184. If water is heated to 80.0°C, how many kelvins is that?
185. The melting point of sodium chloride is 1,074 K. What temperature is this in degrees Celsius?
186. Liquid oxygen boils at –183°C. How many degrees Fahrenheit is this?
187. Normal human body temperature is considered to be around 98.6°F. How many degrees Celsius is this?
188. Adding dry ice to acetone brings the temperature down to –78°C. What is this temperature in degrees Fahrenheit?
189. One summer day, the temperature was recorded as 113°F. How many kelvins is this?
190. Room temperature is about 300 K. How many degrees Fahrenheit is this?
Chapter 4
The Atom and Nuclear Chemistry
An atom consists of a nucleus surrounded by one or more electrons. Although the number of protons identifies the element, the electrons are the key to the chemistry. The arrangement of electrons in an atom influences the atom’s ability to gain, lose, or share electrons and therefore form compounds. Quantum numbers describe the arrangement of the electrons. Unstable atoms undergo nuclear decay to transform to stable atoms. Atoms may be broken apart by fission or joined by fusion.
The Problems You’ll Work On
In this chapter, you work with atoms and nuclear chemistry in the following ways:
Counting subatomic particles
Interpreting isotope notation
Writing electron configurations
Calculating average atomic mass and percent abundance
Understanding nuclear decay and balancing nuclear equations
Note: For access to the periodic table, see the Appendix.
What to Watch Out For
Remember the following when working on atoms and nuclear chemistry:
Note that unlike the atomic mass, the mass number is usually not found on the periodic table.
Remember the maximum number of electrons possible in each subshell, and follow Hund’s rule and the Aufbau principle when filling orbitals. Know the rules for assigning the four quantum numbers.
Know the common nuclear decay modes.
Remember that balancing nuclear equations depends on both the mass numbers and the atomic numbers.
Know how to calculate the half-life and how to use it.
Isotopes and Subatomic Particles
191–219 Answer the question on isotopes and subatomic particles.
191. How many protons are in an atom of sodium?
192. How many electrons are in an atom of bromine?
193. How many electrons are in an atom of nickel?
194. How many protons are in an atom of radon?
195. How many neutrons are in an atom of isotope potassium-40?
196. How is the atomic number related to the number of protons in an atom?
197. How is the mass number of an atom related to the number of neutrons?
198. How many protons, electrons, and neutrons are in an atom of isotope copper-63?
199. An atom has a mass number of 14 and 6 electrons. How many protons and neutrons does it have?
200. An atom has 40 electrons and 51 neutrons. What is its mass number, and how many protons does it have?
201. What does the top number in isotope notation represent?
202. What does the bottom number in isotope notation represent?
203. How many protons and neutrons are in ?
204. How many protons and neutrons are in ?
205. What is the isotope notation for an atom of carbon-12?
206. What is the isotope notation for an atom of chlorine-37?
207. What is the name of ?
208. How does an ion differ from an atom of the same element with regard to the numbers of subatomic particles?
209. When two atoms or ions have the same number of electrons, they’re said to be __________.
210. When an ion has a positive charge, how do the numbers of subatomic particles differ?
211. When an ion has a negative charge, how do the numbers of subatomic particles differ?
212. How many protons and electrons does have?
213. How many protons and electrons does have?
214. How many protons and electrons does have?
215. How many protons and electrons does have?
216. What is the isotope notation for an ion of silver-109 with a charge of positive 1?
217. What is the isotope notation for an ion of sulfur-34 with a charge of negative 2?
218. How many protons, neutrons, and electrons are in ?
219. How many protons, neutrons, and electrons are in ?
Electrons and Quantum Mechanics
220–234 Answer the questions on electrons and quantum mechanics.
220. What is the name of the premise that one electron fills each orbital in a subshell until all orbitals contain one electron and then electrons are added to fill in the second available spot in the subshell?
221. What rule or principle describes the order in which electrons fill orbitals?
222. What is the maximum number of electrons that can be in the f orbitals?
223. What is the maximum number of electrons that can be in the p orbitals?
224. What is the electron configuration of carbon?
225. What is the electron configuration of magnesium?
226. What is the electron configuration of argon?
227. What is the electron configuration of bromine?
228. What is the electron configuration of zirconium?
229. What is the expected electron configuration of plutonium?
230. Which quantum number describes the spin of the electron?
231. Which quantum number describes the average distance between the nucleus and the orbital?
232. Which quantum number describes how the various orbitals are oriented in space?
233. Which quantum number describes the shape of the orbital?
234. What are the possible values for the spin quantum number?
Average Atomic Mass
235–242 Answer the questions on average atomic mass.
235. The decimal numbers in the blocks of the periodic table represent the __________.
236. What is the average atomic mass of lithium that is 7.59% lithium-6 (mass of 6.0151 amu) and 92.41% lithium-7 (mass of 7.0160 amu)?
237. What is the average atomic mass of chlorine that is 75.78% chlorine-35 (mass of 34.96885 amu) and 24.22% chlorine-37 (mass of 36.9659 amu)?
238. What is the average atomic mass of magnesium, given the information in the following table?
Isotope
Percent Abundance
Atomic Mass (amu)
78.99
23.985
10.00
24.986
11.01
25.983
239. What is the average atomic mass of potassium, given the information in the following table?
Isotope
Percent Abundance
Atomic Mass (amu)
93.258
38.9637
0.01170
39.9640
6.7302
40.9618
240. What is the average atomic mass of iron, given the information in the following table?
Isotope
Percent Abundance
Atomic Mass (amu)
5.845
53.9396
91.754
55.9349
2.119
56.9354
0.282
57.9333
241. What is the average atomic mass of krypton, given the information in the following table?
Isotope
Percent Abundance
Atomic Mass (amu)
0.350
77.9204
2.28
79.9164
11.58
81.9135
11.49
82.9141
57.00
83.9115
17.30
85.9106
242. If the average atomic mass of boron is 10.81 amu, what is the percent abundance of boron-11 (mass of 11.009306 amu) if the only other isotope is boron-10 (mass of 10.012937 amu)?
Nuclear Reactions and Nuclear Decay
243–252 Answer the question on aspects of nuclear reactions and nuclear decay.
243. What is the primary nuclear process that occurs in the sun?
244. In which nuclear process does a nucleus split into two or more smaller elements and possibly some extra neutrons?
245. What is it called when a helium nucleus is ejected from the nucleus of an atom during a nuclear reaction?
246. When a ray is a byproduct of a nuclear reaction, what nuclear process has occurred?
247. What is the isotope (nuclear) notation for a particle that is produced from beta decay?
248. A particle is a product of which nuclear reaction?
249. is an example of what type of nuclear reaction?
250. is an example of what type of nuclear reaction?
251. is an example of what type of nuclear reaction?
252. is an example of what type of nuclear reaction?
Completing Nuclear Reactions
253–260 Determine the missing part of the equation.
253.
254.
255.
256.
257.
258.
259.
260.
Half-Lives
261–270 Answer the question on half-lives.
261. After five half-lives, how many grams of a 400 g radioactive sample remain undecayed?
262. After three half-lives, how many grams of a 50.0 g radioactive sample have decayed?
263. If 5.15 g of a radioactive sample remains undecayed after six half-lives, how many grams were in the original sample?
264. A radioactive sample starts with 1.500 × 1020 undecayed atoms. When measured again at a later date, the sample has 9.375 × 1018 undecayed atoms. How many half-lives have passed?
265. What fraction of a sample remains undecayed after 39 hours if the half-life of the sample is 13 hours?
266. Iodine-131 has a half-life of 8.02 days. If the original sample contained 25.0 g of iodine-131, how many grams have decayed after 56.14 days?
267. Strontium-90 has a half-life of 28.9 years. How many grams were in the original sample if 11 g remain undecayed after 115.6 years?
268. In 5 minutes, a radioactive sample decays from 2.56 × 1010 atoms to 8.00 × 108 atoms. How long is the isotope’s half-life?
Chapter 5
Periodicity and the Periodic Table
The periodic table is much more than a simple listing of the symbols of the elements with additional information about each element. The position of an element on the periodic table indicates many of the element’s properties. In addition, the position gives information on how the properties of an element relate to those of its neighbors. However, watch out for exceptions to the general trends.
The Problems You’ll Work On
In this chapter, you work with periodicity and the periodic table in the following ways:
Recognizing element symbols
Understanding the structure of the periodic table
Identifying periodic trends
Note: For reference, you can find the periodic table in the Appendix.
What to Watch Out For
Don’t let common mistakes trip you up; remember the following when working on periodicity and the periodic table:
The position of an element on the periodic table gives important information.
Don’t confuse periods (rows) with groups (columns).
Learn the basic periodic trends. Note that hydrogen is an exception to nearly all trends and that the top member of each group on the periodic table shows a slight variation to most trends.
Element Symbols and Names
271–290 Check your knowledge of the symbols and names of elements on the periodic table.
271. What is the symbol for the element carbon?
272. What is the symbol for the element chlorine?
273. What is the symbol for the element aluminum?
274. What is the symbol for the element cadmium?
275. What is the symbol for the element copper?
276. What is the symbol for the element arsenic?
277. What is the symbol for the element sodium?
278. What is the symbol for the element potassium?
279. What is the symbol for the element iron?
280. What is the symbol for the element silver?
281. What is the name of the element that has the symbol N?
282. What is the name of the element that has the symbol S?
283. What is the name of the element that has the symbol Br?
284. What is the name of the element that has the symbol P?
285. What is the name of the element that has the symbol Mn?
286. What is the name of the element that has the symbol At?
287. What is the name of the element that has the symbol Ra?
288. What is the name of the element that has the symbol Hg?
289. What is the name of the element that has the symbol Sn?
290. What is the name of the element that has the symbol Pa?
Structure of the Periodic Table
291–310 Answer the questions on the structure of the periodic table.
291. A period goes in which direction on the periodic table?
292. Where are the metalloids located in the periodic table?
293. Where on the periodic table are the alkaline earth metals located?
294. Where on the periodic table are the transition metals located?
295. Where on the periodic table are the noble gases located?
296. Where on the periodic table are the inner transition metals located?
297. Where on the periodic table are the alkali metals located?
298. Which chemist is most often recognized for basing the arrangement of the periodic table on atomic mass and other physical properties of the elements?
299. Which scientist placed the elements in order of increasing atomic number on the periodic table?
300. Where on the periodic table are most of the elements that exist as gases at room temperature?
301. To which family does the element potassium belong?
302. To which family does the element silver belong?
303. To which family does the element selenium belong?
304. To which family does the element tin belong?
305. To which family does the element iodine belong?
306. To which family does the element calcium belong?
307. To which family does the element aluminum belong?
308. To which family does the heaviest naturally occurring element belong?
309. Which family of elements contains the only metal that’s liquid at room temperature?
310. Which family of elements contains the only nonmetal that’s liquid at room temperature?
Periodic Trends
311–330 Examine your knowledge of periodic trends.
311. Members of which family have three valence electrons?
312. Members of which family have five valence electrons?
313. Members of which family have two valence electrons?
314. The atomic masses of the elements generally __________ (increase/decrease/remain the same) going from left to right in a period and __________ (increase/decrease/remain the same) going down a family.
315. The atomic radii of the elements __________ (increase/decrease/remain the same) going from left to right in a period and __________ (increase/decrease/remain the same) going down a family.
316. What term describes the amount of energy needed to remove an electron from a gaseous atom?
317. What term describes the energy change that results from adding an electron to a gaseous atom or ion?
318. The ionic radius of an anion is __________ (larger than/smaller than/the same size as) the atomic radius of the neutral atom because the ion has __________ (more/fewer/an equal number of) electrons compared to the atom.
319. The atomic radii of the elements __________ (increase/decrease/remain the same) going from left to right in a period because the effective nuclear charge __________ (increases/decreases).
320. Rank the following elements from smallest to largest atomic radius: Ba, Be, Ca.
321. Rank the following elements from smallest to largest atomic radius: Cl, P, S.
322. Rank the following elements from lowest to highest ionization energy: B, C, Li.
323. Rank the following elements from lowest to highest ionization energy: Br, Cl, I.
324. Rank the following elements from lowest to highest electron affinity: F, O, N.
325. Rank the following elements from lowest to highest electron affinity: S, Se, Te.
326. Rank the following elements from most to least metallic character: Cl, Si, Sn.
327. Rank the following elements from smallest to largest atomic radius: K, Mg, Na.
328. Rank the following ions from largest to smallest ionic radius: F–, O2–, S2–.
329. Rank the following elements from highest to lowest ionization energy: Cs, F, Li.
330. Rank the following elements from lowest to highest ionization energy: Ba, Bi, N.
Chapter 6
Ionic Bonding
Ionic compounds usually contain a metal (from the left side of the periodic table) and a nonmetal (from the right side of the periodic table, other than the noble gases). Some ionic compounds contain polyatomic ions, such as the sulfate ion SO42–. Ternary compounds technically contain three elements; however, more may be present. The names of ionic compounds consist of two or more words. The last word in the name of a binary compound has an -ide suffix. The last word in the name of a ternary compound usually has an -ite or an -ate suffix. Pure acids are generally not ionic, but they produce ions in solution.
The Problems You’ll Work On
In this chapter, you work with ionic bonding in the following ways:
Naming binary compounds
Naming ternary compounds
Writing formulas for ionic compounds
Note: See the Appendix if you need to check the periodic table.
What to Watch Out For
Remember the following when working on ionic bonding problems:
The names of inorganic compounds normally consist of two words.
All simple binary compounds have an
-ide
suffix on the second word in the name.
The
-ide
suffix is not common in compounds containing three or more elements. Most compounds containing three or more elements have either an
-ite
or
-ate
suffix.
Don’t use multiplying prefixes, such as
di-
and
tri-,
for ionic compounds.
If you use the “crisscross” rule, don’t forget to reduce.
Acids follow their own rules for naming.
Naming Binary Compounds
331–347 Name the binary ionic compound given the formula.
331. What is the name of NaCl?
332. What is the name of CaO?
333. What is the name of AlBr3?
334. What is the name of K2S?
335. What is the name of Al2O3?
336. What is the name of Li3N?
337. What is the name of MgI2?
338. What is the name of SrSe?
339. What is the name of BaF2?
340. What is the name of NaH?
341. What is the name of Zn3P2?
342. What is the name of CuBr2?
343. What is the name of AuCl3?
344. What is the name of CoS?
345. What is the name of MnF3?
346. What is the name of Hg2I2?
347. What is the name of SnO2?
Naming Compounds with Polyatomic Ions
348–364 Name the compounds containing polyatomic ions.
348. What is the name of NaClO?
349. What is the name of KOH?
350. What is the name of SrSO3?
351. What is the name of CaCO3?
352. What is the name of AlPO4?
353. What is the name of NaClO3?
354. What is the name of GaPO3?
355. What is the name of NH4Cl?
356. What is the name of ZnSO4?
357. What is the name of (NH4)2C2O4?
358. What is the name of KMnO4?
359. What is the name of Be(NO2)2?
360. What is the name of Cu(CN)2?
361. What is the name of AgBrO?
362. What is the name of (NH4)3PO4?
363. What is the name of Ni2(SO4)3?
364. What is the name of Pb(C2H3O2)2?
Writing Formulas of Binary Compounds
365–390 Give the chemical formula for the binary ionic compound.
365. What is the chemical formula for cesium chloride?
366. What is the chemical formula for indium(III) fluoride?
367. What is the chemical formula for magnesium oxide?
368. What is the chemical formula for barium bromide?
369. What is the chemical formula for potassium iodide?
370. What is the chemical formula for aluminum chloride?
371. What is the chemical formula for chromium(III) fluoride?
372. What is the chemical formula for iron(II) sulfide?
373. What is the chemical formula for copper(I) nitride?
374. What is the chemical formula for lead(II) oxide?
375. What is the chemical formula for nickel(I) selenide?
376. What is the chemical formula for silver oxide?
377. What is the chemical formula for strontium bromide?
378. What is the chemical formula for magnesium nitride?
379. What is the chemical formula for lithium hydride?
380. What is the chemical formula for zinc chloride?
381. What is the chemical formula for chromium(II) sulfide?
382. What is the chemical formula for manganese(II) selenide?
383. What is the chemical formula for tin(IV) fluoride?
384. What is the chemical formula for copper(I) iodide?
385. What is the chemical formula for nickel(III) phosphide?
386. What is the chemical formula for aluminum selenide?
387. What is the chemical formula for tin(IV) oxide?
388. What is the chemical formula for calcium phosphide?
389. What is the chemical formula for iron(III) oxide?
390. What is the chemical formula for manganese(IV) sulfide?
Writing Formulas of Compounds with Polyatomic Ions
391–420 Give the formula for the compound containing a polyatomic ion.
391. What is the chemical formula for rubidium hypochlorite?
392. What is the chemical formula for beryllium carbonate?
393. What is the chemical formula for aluminum phosphite?
394. What is the chemical formula for sodium hydrogen carbonate?
395. What is the chemical formula for sodium hydroxide?
396. What is the chemical formula for potassium hydrogen sulfate?
397. What is the chemical formula for lithium perchlorate?
398. What is the chemical formula for barium oxalate?
399. What is the chemical formula for chromium(III) arsenate?
400. What is the chemical formula for silver nitrate?
401. What is the chemical formula for lead(II) sulfite?
402. What is the chemical formula for thallium(I) bromite?
403. What is the chemical formula for gold(III) phosphate?
404. What is the chemical formula for iron(II) sulfate?
405. What is the chemical formula for calcium thiosulfate?
406. What is the chemical formula for sodium peroxide?
407. What is the chemical formula for ammonium nitrite?
408. What is the chemical formula for beryllium chlorite?
409. What is the chemical formula for sodium cyanide?
410. What is the chemical formula for magnesium permanganate?
411. What is the chemical formula for ammonium dichromate?
412. What is the chemical formula for cobalt(III) periodate?
413. What is the chemical formula for lead(IV) oxalate?
414. What is the chemical formula for calcium hydrogen phosphate?
415. What is the chemical formula for iron(III) acetate?
416. What is the chemical formula for potassium thiocyanate?
417. What is the chemical formula for copper(II) hydrogen sulfite?
418. What is the chemical formula for mercury(II) peroxide?
419. What is the chemical formula for gold(I) cyanate?
420. What is the chemical formula for aluminum dihydrogen phosphate?
Chapter 7
Covalent Bonding
In intro-level chemistry courses, most covalent compounds contain only nonmetals (elements to the right on the periodic table plus hydrogen). As with ionic compounds, the last word in the name of a covalent compound has an -ide suffix. Unlike ionic compounds, multiplying prefixes are typically present. For example, the compound S2Cl2 is disulfur dichloride, which uses the multiplying prefix di- twice. Organic compounds are another major group of covalent compounds, but they’re beyond the scope of this text.
The Problems You’ll Work On
In this chapter, you work with covalent bonding in the following ways:
Naming compounds containing covalent bonds
Writing formulas for covalent compounds
Note: You can go to the Appendix if you need to check the periodic table.
What to Watch Out For
Don’t let common mistakes trip you up; remember the following when working on covalent bonding:
The names of inorganic compounds normally consist of two words.
All simple binary compounds have an
-ide
suffix on the second word in the name.
The
-ite
and
-ate
suffixes normally don’t occur in covalent compounds.
The names of covalent compounds use multiplying prefixes, such as
di-, tri-, tetra-,
and
penta-.
The prefix
mono-
