Chapter EightOutlineGoalsGoals Contd.8.1 States of Matter and Their ChangesSlide 6Slide 7Slide 88.2 Gases and the Kinetic-Molecular TheorySlide 10Slide 118.3 PressureSlide 138.4 Boyle’s Law: The Relation Between Volume and PressureSlide 15Slide 168.5 Charles’ Law: The Relation Between Volume and TemperatureSlide 18Slide 198.6 Gay-Lussac’s Law: The Relation Between Pressure and TemperatureSlide 218.7 The Combined Gas Law8.8 Avogadro’s law: The Relation Between Volume and Molar AmountSlide 248.9 The Ideal Gas LawSlide 268.10 Partial Pressure and Dalton’s law8.11 Intermolecular ForcesSlide 29Slide 30Slide 31Slide 328.12 LiquidsSlide 34Slide 35Slide 368.13 Water: A Unique LiquidSlide 388.14 SolidsSlide 408.15 Changes of StateSlide 42Chapter SummaryChapter Summary Contd.Slide 45Slide 46Key WordsKey Words Contd.Slide 49Chapter EightGases, Liquids, and SolidsFundamentals of General, Organic and Biological Chemistry 6th EditionJames E. MayhughCopyright © 2010 Pearson Education, Inc.Copyright © 2010 Pearson Education, Inc.Chapter Eight2Outline►8.1 States of Matter and Their Changes►8.2 Gases and the Kinetic–Molecular Theory►8.3 Pressure►8.4 Boyle’s Law: The Relation between Volume and Pressure►8.5 Charles’s Law: The Relation between Volume and Temperature►8.6 Gay-Lussac’s Law: The Relation between Pressure and Temperature►8.7 The Combined Gas Law►8.8 Avogadro’s Law: The Relation between Volume and Molar Amount►8.9 The Ideal Gas Law►8.10 Partial Pressure and Dalton’s Law►8.11 Intermolecular Forces►8.12 Liquids►8.13 Water: A Unique Liquid►8.14 Solids►8.15 Changes of StateCopyright © 2010 Pearson Education, Inc.Chapter Eight3Goals►1. How do scientists explain the behavior of gases? Be able to state the assumptions of the kinetic–molecular theory of gases and use these assumptions to explain the behavior of gases.►2. How do gases respond to changes in temperature, pressure, and volume? Be able to use Boyle’s law, Charles’s law, Gay-Lussac’s law, and Avogadro’s law to explain the effect on gases of a change in pressure, volume, or temperature.►3. What is the ideal gas law? Be able to use the ideal gas law to find the pressure, volume, temperature, or molar amount of a gas sample.►4. What is partial pressure? Be able to define partial pressure and use Dalton’s law of partial pressures.Copyright © 2010 Pearson Education, Inc.Chapter Eight4Goals Contd.►5. What are the major intermolecular forces, and how do they affect the states of matter? Be able to explain dipole–dipole forces, London dispersion forces, and hydrogen bonding, and recognize which of these forces affect a given molecule.►6. What are the various kinds of solids, and how do they differ? Be able to recognize the different kinds of solids and describe their characteristics.►7. What factors affect a change of state? Be able to apply the concepts of heat change, equilibrium, and vapor pressure to changes of state.Copyright © 2010 Pearson Education, Inc.Chapter Eight58.1 States of Matter and Their Changes►Matter exists in any of three phases, or states—solid, liquid, and gas, depending on the attractive forces between particles, temperature and pressure.►In a gas, the attractive forces between particles are very weak compared to their kinetic energy, so the particles move about freely, are far apart, and have almost no influence on one another. ►In a liquid, the attractive forces between particles are stronger, pulling the particles close together but still allowing them considerable freedom to move about.Copyright © 2010 Pearson Education, Inc.Chapter Eight6In a solid, the attractive forces are much stronger than the kinetic energy of the particles, so the atoms, molecules, or ions are held in a specific arrangement and can only wiggle around in place.Copyright © 2010 Pearson Education, Inc.Chapter Eight7►Phase change or change of state: The transformation of a substance from one state to another. ►Melting point (mp): The temperature at which solid and liquid are in equilibrium.►Boiling point (bp): The temperature at which liquid and gas are in equilibrium. ►Sublimation: A process in which a solid changes directly to a gas.►Melting, boiling, and sublimation all have H>0, and S>0. This means they are nonspontaneous below and spontaneous above a certain temperature.Copyright © 2010 Pearson Education, Inc.Chapter Eight8Copyright © 2010 Pearson Education, Inc.Chapter Eight98.2 Gases and the Kinetic-Molecular Theory►The behavior of gases can be explained by a group of assumptions known as the kinetic–molecular theory of gases. The following assumptions account for the observable properties of gases:►A gas consists of many particles, either atoms or molecules, moving about at random with no attractive forces between them. Because of this random motion, different gases mix together quickly.Copyright © 2010 Pearson Education, Inc.Chapter Eight10►The amount of space occupied by the gas particles themselves is much smaller than the amount of space between particles. Most of the volume taken up by gases is empty space, accounting for the ease of compression and low densities of gases.►The average kinetic energy of gas particles is proportional to the Kelvin temperature. Thus, gas particles have more kinetic energy and move faster as the temperature increases. (In fact, gas particles move much faster than you might suspect. The average speed of a helium atom at room temperature and atmospheric pressure is approximately 1.36 km/s, or 3000 mi/hr, nearly that of a rifle bullet.)Copyright © 2010 Pearson Education, Inc.Chapter Eight11►Collisions of gas particles, either with other particles or with the wall of their container, are elastic; that is, the total kinetic energy of the particles is constant. The pressure of a gas against the walls of its container is the result of collisions of the gas particles with the walls. The number and force of collisions determines the pressure.►A gas that obeys all the assumptions of the kinetic–molecular theory is called an ideal gas. All gases behave somewhat differently than predicted by the kinetic–molecular theory at very high pressures or very low temperatures. Most real gases display nearly ideal behavior under normal conditions.Copyright © 2010 Pearson Education, Inc.Chapter Eight128.3 Pressure►Pressure (P) is defined as a force (F) per unit area (A) pushing against a