Untitled - Kelly Walsh High School

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CHAPTER 8 ◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆ Periodic Trends ◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆ You should read this chapter if you need to review or learn about: ➜ Ionization energy and electron affinity ➜ Periodic trends 119 Copyright © 2007 by John Moore and Richard Langley. Click here for terms of use.
120 CHEMISTRY FOR THE UTTERLY CONFUSED Get Started The goal of this chapter is to help you relate the properties of elements to their position on the periodic table. These properties include ionization energies and electron affinities. You may want to review the basic structure of the periodic table in Chapter 2 and electron configurations in Chapter 7. And Don’t forget!— Practice, Practice, Practice. 8-1 Periodic Table Revisited In Chapter 2, we showed you the arrangement of the periodic table. The columns are groups or families. The group members have similar chemical properties and somewhat similar physical properties. The rows are periods. The row members have predictably different properties. In Chapter 7, we showed you the electron configurations of the elements. You learned how similar electron configurations lead to similar chemical properties. There are, however, other periodic properties. These properties relate to the magnitude of the attractive force that the protons in the nucleus have for electrons. These include atomic radii, ionization energies, and electron affinities. The inner electrons (core electrons) somewhat screen the valence electrons from the attraction of the nucleus. The effective nuclear charge is the nuclear charge minus the screening effect of the core electrons. This screening is essentially constant for all of the elements in any period on the periodic table. However, the screening increases towards the bottom of any family. The effective nuclear charge is useful in explaining most of the observed trends. For example, there is a trend of decreasing atomic radii when moving from left to right across any period on the periodic table. The atomic radius is the distance the valence electrons are from the nucleus. In going from top to bottom on the periodic table, each row adds an additional energy level. Thus, the valence electrons are farther from the nucleus and the atoms increase in size. (There are some minor exceptions, especially in the transition metals.) The atomic radius decreases when moving from left to right within a period. The nuclear charge is increasing across the period. The number of core electrons is constant, so the screening is constant. The effective nuclear charge is increasing due to the increase in nuclear charge minus the constant screening. This increase exerts a greater attractive force on the valence electrons. The increased attraction pulls the outer electrons closer to the nucleus, resulting in a smaller atom.
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Chemistry for the Utterly Confused
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We would like to dedicate this book
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Contents ix Chapter 5 Gases 79 Do I
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Contents xi Get Started 146 10-1 Mo
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Contents xiii 15-4 pH 222 15-5 Acid
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Contents xv Chapter 20 Nuclear Chem
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CHAPTER 1 ◆◆◆◆◆◆◆◆
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Chemistry: First Steps 3 compound b
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Chemistry: First Steps 5 exact norm
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Chemistry: First Steps 7 We now nee
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Chemistry: First Steps 9 mathematic
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Chemistry: First Steps 11 we do not
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Chemistry: First Steps 13 19. How m
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CHAPTER 2 ◆◆◆◆◆◆◆◆
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Atoms, Ions, and Molecules 17 Caref
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Atoms, Ions, and Molecules 19 table
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Atoms, Ions, and Molecules 21 If a
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Atoms, Ions, and Molecules 23 Once
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Atoms, Ions, and Molecules 25 and n
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Atoms, Ions, and Molecules 27 1. Th
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Atoms, Ions, and Molecules 29 20. N
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CHAPTER 3 ◆◆◆◆◆◆◆◆
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Mass, Moles, and Equations 33 Caref
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Mass, Moles, and Equations 35 Quick
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Mass, Moles, and Equations 41 Caref
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Mass, Moles, and Equations 43 the b
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Mass, Moles, and Equations 45 7. Th
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Mass, Moles, and Equations 47 17. a
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CHAPTER 4 ◆◆◆◆◆◆◆◆
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Aqueous Solutions 51 4-2 Solubility
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Aqueous Solutions 53 Don’t Forget
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Aqueous Solutions 55 Quick Tip Cert
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Aqueous Solutions 57 Quick Tip Quic
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Aqueous Solutions 63 Quick Tip Mg(N
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Aqueous Solutions 65 All the separa
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Page 92 and 93: Aqueous Solutions 69 There will be
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Page 98 and 99: Aqueous Solutions 75 The calculatio
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Page 104 and 105: Gases 81 Quick Tip Don’t Forget!
Page 106 and 107: Gases 83 Quick Tip Let’s see how
Page 108 and 109: Gases 85 Don’t Forget! Quick Tip
Page 110 and 111: Gases 87 Second, the KMT relates th
Page 112 and 113: Gases 89 The larger the gas particl
Page 114 and 115: Gases 91 Note that the mandatory co
Page 116 and 117: Gases 93 If it was not clear before
Page 118 and 119: Gases 95 ANSWER KEY 1. PTotal PA
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Page 122 and 123: Thermochemistry 99 Quick Tip Don’
Page 124 and 125: Thermochemistry 101 Don’t Forget!
Page 126 and 127: Thermochemistry 103 C2H2(g) (5/2) O
Page 128 and 129: Thermochemistry 105 Quick Tip Some
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Page 132 and 133: Quantum Theory and Electrons 109 Al
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Page 136 and 137: Quantum Theory and Electrons 113 Do
Page 138 and 139: Quantum Theory and Electrons 115 Do
Page 140 and 141: Quantum Theory and Electrons 117 AN
Page 144 and 145: Periodic Trends 121 8-2 Ionization
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Page 148 and 149: Periodic Trends 125 in its ground s
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Page 152 and 153: Chemical Bonding 129 Quick Tip In S
Page 154 and 155: Chemical Bonding 131 9-3 Ionic Bond
Page 156 and 157: Chemical Bonding 133 Quick Tip Neve
Page 158 and 159: Chemical Bonding 135 Don’t Forget
Page 160 and 161: Chemical Bonding 137 9-6 Bond Energ
Page 162 and 163: Chemical Bonding 139 Quick Tip invo
Page 164 and 165: Chemical Bonding 141 Quick Tip Elem
Page 166 and 167: Chemical Bonding 143 11. a 12. b 13
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Page 170 and 171: Molecular Geometry and Hybridizatio
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Page 182 and 183: Intermolecular Forces, Solids and L
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Intermolecular Forces, Solids and L
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CHAPTER 12 ◆◆◆◆◆◆◆◆
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Solutions 173 ways of expressing th
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Solutions 175 Don’t Forget! Don
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Solutions 177 12-3 Colligative Prop
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Solutions 179 Just as the freezing
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Solutions 181 Don’t Forget! Using
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Solutions 183 Quick Tip A molar mas
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Solutions 185 3. All methods of num
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CHAPTER 13 ◆◆◆◆◆◆◆◆
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Kinetics 189 4. Physical state of r
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Kinetics 191 Don’t Forget! consta
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Kinetics 193 Don’t Forget! the co
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Kinetics 195 Quick Tip Careful! Rem
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Kinetics 197 The decomposition of h
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Kinetics 199 reaction is first orde
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Kinetics 201 energy of a reaction.
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CHAPTER 14 ◆◆◆◆◆◆◆◆
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Chemical Equilibria 205 Quick Tip D
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Chemical Equilibria 207 14-3 Le Ch
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Chemical Equilibria 209 Given the f
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Chemical Equilibria 211 Careful! Do
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Chemical Equilibria 213 Quick Tip F
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Chemical Equilibria 215 Quick Tip I
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Chemical Equilibria 217 10. Write K
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CHAPTER 15 ◆◆◆◆◆◆◆◆
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Acids and Bases 221 Don’t Forget!
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Acids and Bases 223 The pH of pure
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Acids and Bases 225 Quick Tip Quick
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Acids and Bases 227 15-7 Lewis Acid
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Acids and Bases 229 We do not have
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Acids and Bases 231 Quick Tip We ne
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Acids and Bases 233 2. Alkali metal
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CHAPTER 16 ◆◆◆◆◆◆◆◆
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Buffers and Other Equilibria 237 we
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Buffers and Other Equilibria 239 Do
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Buffers and Other Equilibria 241 16
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Buffers and Other Equilibria 243 Qu
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Buffers and Other Equilibria 245 Qu
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Buffers and Other Equilibria 247 pK
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Buffers and Other Equilibria 249 Th
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CHAPTER 17 ◆◆◆◆◆◆◆◆
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Entropy and Free Energy 253 17-2 En
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Entropy and Free Energy 255 17-5 Ut
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Entropy and Free Energy 257 Quick T
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Entropy and Free Energy 259 Be Care
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Entropy and Free Energy 261 Before
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Entropy and Free Energy 263 ANSWER
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CHAPTER 18 ◆◆◆◆◆◆◆◆
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Electrochemistry 267 Quick Tip Some
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Electrochemistry 269 Don’t Forget
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Electrochemistry 271 We can use thi
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Electrochemistry 273 do is reverse
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Electrochemistry 275 Don’t Forget
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Electrochemistry 277 Be Careful! Th
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Electrochemistry 279 ANSWER KEY 1.
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CHAPTER 19 ◆◆◆◆◆◆◆◆
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Chemistry of the Elements 283 19-2
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Chemistry of the Elements 285 Be Ca
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Chemistry of the Elements 287 Don
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Chemistry of the Elements 289 6. Wh
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CHAPTER 20 ◆◆◆◆◆◆◆◆
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Nuclear Chemistry 293 The sum of th
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Nuclear Chemistry 295 Don’t Forge
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Nuclear Chemistry 297 that is not a
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Nuclear Chemistry 299 Don’t Forge
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Nuclear Chemistry 301 t 1/2 (ln 2)
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Nuclear Chemistry 303 1. A typical
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CHAPTER 21 ◆◆◆◆◆◆◆◆
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Organic, Biochemistry, and Polymers
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Index 327 chemical formulas, 19-21
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Index 329 Gibbs free energy (G), 25
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Index 331 octet rule, 128, 135, 140
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Index 333 viscosity, 161 voltaic ce
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