Index 329 Gibbs free energy (G), 253–254 glycoside linkages, 319 Graham’s law, 87 ground state, 109, 112 groups, periodic table, 19 half-cell potentials, 270 half-lives (t 1/2), 193, 198–202, 296–298, 302 half-reactions, 56, 266, 269–272, 275–277 heat, 98, 208 heat capacity, 99–101, 162 heat of vaporization, 162 Henderson-Hasselbalch equation, 236 Hess’s law, 102–103 heterogeneous catalysts, 197 homogeneous catalysts, 196 Hund’s rule, 112 hybridization, 149–155 hydrocarbons, 306–311, 322 hydrogen, 160, 166, 270, 282 ideal gas equation, 82–84, 89, 92–93 ideal gases, 86, 88 ideal solutions, 177–178 IE (ionization energy), 121–122, 124 indicators, 71, 237–238 inner transition elements, 19 integrated rate laws, 192–193, 200 intensive properties, 98 intermolecular forces, 157–169 liquids, 161–162 overview, 157–158 phase diagrams, 163–165 solids, 162–163 types of, 158–161 ion-dipole intermolecular forces, 159 ion-electron method, 267 ionic bonds, 129, 130–132, 165–166 ionic compounds, 20, 51, 131–132 ionic equations, 59 ionic solids, 163 ion-induced dipole intermolecular forces, 160 ionization, 51, 63 ionization energy (IE), 121–122, 124 ion product, 240 ions: chemical formulas, 19–21 common-ion effect, 236 complex, 241, 287–288 ionic radii, 122 ions (Cont.): net ionic equations, 58–70 nomenclature, 21–26 overview, 121 isoelectronic, 128 isomers, 308 isotopes, 17, 295 joules (J), 98 K a (acid dissociation constant), 223–225 K b (base dissociation constant), 225–226 K c and K p (equilibrium constants), 205–206 K f (formation constant), 241 kinetic molecular theory (KMT), 86–88 kinetics, 187–202 Arrhenius equation and activation energy, 194–196 catalysis, 196–197 integrated rate laws, 192–193 overview, 187–188 rate laws, 189–192, 198–200 reaction mechanisms, 197–198 reaction rates, 188–189 KMT (kinetic molecular theory), 86–88 K sp (solubility product constant), 238–240 K w (water dissociation constant), 221–222 l (angular momentum quantum number), 110 lattice energy, 131–132 laws: gas, 80–83, 89–93 Hess’s, 102–103 integrated rate, 192–193, 200 Law of Conservation of Mass, 32 rate, 189–193, 198–202 reaction rate, 189–192 thermodynamics, 252 Le Châtelier’s principle, 207–209, 216, 249 Lewis Acid-Base theory, 227, 232 Lewis electron-dot symbols, 128–130, 137–141 Lewis structural formulas, 129–130, 133 ligands, 287–288 light, 108–109, 115–116, 316–317 limiting reactants, 36–38 liquids, 3, 161–164, 167 London (dispersion) intermolecular forces, 160–161, 165–167
330 INDEX M (molarity), 50, 73, 174, 175 macroscopic level, 3 magnetic quantum number, 111 main-group elements, 19 mass, 31–47 atomic, 16–17, 34 Avogadro’s number and molar mass, 34–35 balancing chemical equations, 32–34 finding moles, 40–44 limiting reactants and percent yield, 36–38 mass/energy conversions, 298–299 overview, 31–32 percent composition and empirical formulas, 38–39 stoichiometry, 35–36 mass (weight) percentage, 173 mass/energy conversions, 298–299 mass/volume percentage, 173–174 matter, 3–4, 108–109, 115–116 measurement, units of, 4–6 melting point (mp), 158 meniscus, 162 metallic bonds, 163, 165 metallic solids, 163 metalloids, 18 metals, 18, 283–284, 288 Metric (SI) system, 4–6 microscopic level, 3 MO (molecular orbital) theory, 151–154 molar heat capacity (C), 99–101 molarity (M), 50, 73, 174, 175 molecular compounds, 21–22, 51 molecular equations, 59 molecular formulas, 19, 39, 129 molecular geometry, 145–155 molecular orbital theory, 151–153 overview, 145–149 valence bond theory, 149–151 valence-shell electron pair repulsion theory, 146–149 molecular orbital (MO) theory, 151–154 molecular solids, 163 molecules: chemical formulas, 19–21 and covalent bonds, 132 intermolecular forces, 157–169 liquids, 161–162 phase changes, 163–165 solids, 162–163 types, 158–161 molecules (Cont.): nomenclature, 21–26 moles, 31–47 Avogadro’s number and molar mass, 34–35 balancing chemical equations, 32–34 finding, 40–44 limiting reactants and percent yield, 36–38 mole fraction, 175 overview, 31–32 percent composition and empirical formulas, 38–39 stoichiometry, 35–36 monatomic ions, 121 monosaccharides, 314 mp (melting point), 158 n (amount) gas law constants, 80–83 natural decay modes, 302 Nernst equation, 272–273 net ionic equations, 58–70 network covalent solids, 163 neutralization reactions, 53–55 neutral pH, 223 neutron-poor isotopes, 295 neutrons, 16–17 nomenclature: alkane, 306–311 atoms, 21–26 nonelectrolytes, 51 nonideal gases, 88–89 nonmetals: general properties of, 284–285 ionization energies, 285 nomenclature, 24 overview, 18 oxidation numbers, 285 periodic trends of, 285–286 nonpolar covalent bond, 133 nonspontaneous half-reactions, 276 nonstoichiometric compounds, 282 nuclear chemistry, 291–304 fission and fusion, 299–300 half-lives, 296–298 mass and energy conversions, 298–299 nuclear decay, 300–302 nuclear reactions, 292–295 nuclear stability, 295 overview, 291–292 nucleic acids, 315–316, 322 nucleotides, 315
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Chemistry for the Utterly Confused
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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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Chemistry for the Utterly Confused
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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 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 37 Quick
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Mass, Moles, and Equations 39 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 59 Don’t Forget
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Aqueous Solutions 61 Don’t Forget
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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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Aqueous Solutions 67 Don’t Forget
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Aqueous Solutions 69 There will be
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Aqueous Solutions 71 Don’t Forget
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Aqueous Solutions 73 Don’t Forget
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Aqueous Solutions 75 The calculatio
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Aqueous Solutions 77 25. The titrat
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CHAPTER 5 ◆◆◆◆◆◆◆◆
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Gases 81 Quick Tip Don’t Forget!
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Gases 83 Quick Tip Let’s see how
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Gases 85 Don’t Forget! Quick Tip
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Gases 87 Second, the KMT relates th
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Gases 89 The larger the gas particl
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Gases 91 Note that the mandatory co
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Gases 93 If it was not clear before
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Gases 95 ANSWER KEY 1. PTotal PA
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Thermochemistry 99 Quick Tip Don’
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Thermochemistry 101 Don’t Forget!
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Thermochemistry 103 C2H2(g) (5/2) O
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Thermochemistry 105 Quick Tip Some
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Quantum Theory and Electrons 109 Al
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Quantum Theory and Electrons 111 Th
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Quantum Theory and Electrons 113 Do
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Quantum Theory and Electrons 115 Do
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Quantum Theory and Electrons 117 AN
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Periodic Trends 121 8-2 Ionization
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Periodic Trends 123 The general tre
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Periodic Trends 125 in its ground s
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Chemical Bonding 129 Quick Tip In S
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Chemical Bonding 131 9-3 Ionic Bond
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Chemical Bonding 133 Quick Tip Neve
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Chemical Bonding 135 Don’t Forget
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Chemical Bonding 137 9-6 Bond Energ
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Chemical Bonding 139 Quick Tip invo
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Chemical Bonding 141 Quick Tip Elem
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Chemical Bonding 143 11. a 12. b 13
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Molecular Geometry and Hybridizatio
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Molecular Geometry and Hybridizatio
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Molecular Geometry and Hybridizatio
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Molecular Geometry and Hybridizatio
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Molecular Geometry and Hybridizatio
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Intermolecular Forces, Solids and L
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Intermolecular Forces, Solids and L
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Intermolecular Forces, Solids and L
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Intermolecular Forces, Solids and L
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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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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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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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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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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 247 pK
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Buffers and Other Equilibria 249 Th
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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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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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