Untitled - Kelly Walsh High School

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CHAPTER 11 ◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆ Intermolecular Forces, Solids and Liquids ◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆ You should read this chapter if you need to review or learn about: ➜ Types of intermolecular forces ➜ Properties of liquids ➜ Surface tension ➜ Viscosity ➜ ➜ ➜ Capillary action Structures of solids Phase changes and diagrams 157 Copyright © 2007 by John Moore and Richard Langley. Click here for terms of use.
158 CHEMISTRY FOR THE UTTERLY CONFUSED Get Started Quick Tip The goal of this chapter is to help you learn about intermolecular forces. Intermolecular forces are interactions between atoms, molecules, and/or ions. We can use these forces to explain both macroscopic and microscopic properties of matter. The state of matter in which a substance exists depends upon two factors. One of these factors is the kinetic energy of the particles. The other factor is the intermolecular forces between the particles. The average kinetic energy of the molecules relates directly to the temperature. Kinetic energy tends to move particles away from each other. As the temperature increases, the average kinetic energy increases. When the kinetic energy increases, the particles move faster. In a solid, the intermolecular forces are sufficiently great to minimize particle movement. When the temperature increases, the kinetic energy increases and eventually will overcome the intermolecular forces. The substance might in fact melt. While a substance is melting, the temperature remains constant even though we are adding energy. The temperature at which the solid converts into the liquid state is the melting point (mp). Melting is an example of a change in state. Changes of state, called phase changes, depend on the temperature. In some cases, the pressure can also influence these changes. The melting point of a substance and its freezing point (fp) are identical. In this chapter, we will concentrate on the solid and liquid states. It may be useful to review the section in Chapter 10 that deals with the polarity of molecules. And again, Practice, Practice, Practice. 11-1 Types of Intermolecular Forces Intermolecular forces are attractive or repulsive forces between atoms, molecules, and/or ions. The attractive forces compete with the randomizing factor of kinetic energy. The structure that a particular substance exhibits depends on the
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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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Aqueous Solutions 69 There will be
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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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CHAPTER 6 ◆◆◆◆◆◆◆◆
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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
Page 130 and 131: CHAPTER 7 ◆◆◆◆◆◆◆◆
Page 132 and 133: Quantum Theory and Electrons 109 Al
Page 134 and 135: Quantum Theory and Electrons 111 Th
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
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Page 144 and 145: Periodic Trends 121 8-2 Ionization
Page 146 and 147: Periodic Trends 123 The general tre
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
Page 168 and 169: CHAPTER 10 ◆◆◆◆◆◆◆◆
Page 170 and 171: Molecular Geometry and Hybridizatio
Page 182 and 183: Intermolecular Forces, Solids and L
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Page 196 and 197: Solutions 173 ways of expressing th
Page 198 and 199: Solutions 175 Don’t Forget! Don
Page 200 and 201: Solutions 177 12-3 Colligative Prop
Page 202 and 203: Solutions 179 Just as the freezing
Page 204 and 205: Solutions 181 Don’t Forget! Using
Page 206 and 207: Solutions 183 Quick Tip A molar mas
Page 208 and 209: Solutions 185 3. All methods of num
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Page 212 and 213: Kinetics 189 4. Physical state of r
Page 214 and 215: Kinetics 191 Don’t Forget! consta
Page 216 and 217: Kinetics 193 Don’t Forget! the co
Page 218 and 219: Kinetics 195 Quick Tip Careful! Rem
Page 220 and 221: Kinetics 197 The decomposition of h
Page 222 and 223: Kinetics 199 reaction is first orde
Page 224 and 225: Kinetics 201 energy of a reaction.
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Page 228 and 229: 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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Untitled - Kelly Walsh High School

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