Chemistry: 1001 Practice Problems For Dummies (+ Free Online Practice) (eBook)

Heather Hattori, Richard H. Langley (Autoren)

eBook Download: EPUB

2022
John Wiley & Sons (Verlag)
9781119883555 (ISBN)

Infos

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.

Heather Hattori has taught both high school and college level chemistry during her 30+ years in education.

Richard H. Langley, PhD, is on the faculty of Stephen F. Austin State University in Nacogdoches,Texas, where he teaches chemistry.

Inhalt

Introduction 1

Part 1: The Questions 5

Chapter 1: Units and Unit Conversions 7

Chapter 2: Scientific Notation and Significant Figures 13

Chapter 3: Matter and Energy 19

Chapter 4: The Atom and Nuclear Chemistry 25

Chapter 5: Periodicity and the Periodic Table 33

Chapter 6: Ionic Bonding 39

Chapter 7: Covalent Bonding 47

Chapter 8: Molecular Geometry 53

Chapter 9: Chemical Reactions 61

Chapter 10: Molar Calculations 71

Chapter 11: Thermochemistry 83

Chapter 12: Gases 97

Chapter 13: Solutions (The Chemistry Kind) 107

Chapter 14: Acids and Bases 115

Chapter 15: Graphing Basics 125

Part 2: The Answers 131

Chapter 16: Answers and Explanations 133

Appendix: the Periodic Table of Elements 425

Index 427

Textauszug

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...

Produkt-Details

• Erscheint lt. Verlag: 10.5.2022
• Sprache: englisch
• Themenwelt: Sachbuch/Ratgeber ► Natur / Technik ► Naturwissenschaft
• Themenwelt: Schulbuch / Wörterbuch
• Themenwelt: Naturwissenschaften ► Chemie ► Organische Chemie
• Themenwelt: Sozialwissenschaften ► Pädagogik
• Schlagworte: answer explanations • ap chemistry • Basic chemistry • Chemie • Chemistry • Chemistry 1 • chemistry class • chemistry fd • chemistry for dummies • Chemistry practice • chemistry problems • CHEMISTRY REVIEW • chemistry study guide • chemistry supplement • Dummies guide to chemistry • Einführung in die Chemie • General K-12 School • High school chemistry • K-12 School • mcat • Naturwissenschaften • online chemistry practice • Preparatory / Introductory Chemistry • Science/Chemistry/K-12
• ISBN-13: 9781119883555 / 9781119883555