Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
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1 Chapter 11 THE NATURE OF GASES States of Matter Describe the motion of gas particles according to the kinetic theory Interpret gas pressure in terms of kinetic theory Key Terms: 1. kinetic energy 2. gas pressure 3. atmospheric pressure 4. vacuum 5.barometers 6. standard atmosphere (atm) 7. kinetic theory 8. pascal (Pa) Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank can be completed with a term, short phrase, or number. The kinetic theory describes the 1 of particles in matter, and the forces of attraction between them. The theory assumes that the volume occupied by a gas is mostly 2, that the particles of gas are 3, move 4 of each other, and are in constant 5 motion. Furthermore, the 6 between particles are elastic so that the total 7 remains constant. The pressure of a gas results from the counties' collisions of the gas particles with an object. Barometers are used to measure 8 pressure. Standard conditions are defined as a temperature of 9 and a pressure of 10. Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 11. Atmospheric pressure is 760 mm Hg. 12. The SI unit of pressure is the pascal. 13. Atmospheric pressure increases as you climb a mountain because the air layer that surrounds the earth thins out. 14. When particles of a substance are heated, some of the energy is absorbed by the particle and stored in the form of potential energy. 15. The Kelvin temperature of a substance describes the total kinetic energy of the particles in the substance. 16. At any given temperature, the particles of all substances have the same average kinetic energy. H. Cannon, C. Clapper and T. Guillot Klein High School
2 Part C Matching Match each description in Column B to the correct term in Column A. Column A Column B 17. vacuum 18. kinetic energy States of Matter a. an instrument used to measure atmospheric pressure b. a space where no particles of matter exist 19. gas pressure 20. atmospheric pressure 21. barometer c. the energy an object has because of its motion d. the force resulting from the simultaneous collisions of billions of gas particles on an object e. the pressure that results from the collisions of air molecules with objects Part D Questions and Problems 22. A gas is at a pressure of 4.30 atm. What is this pressure in kilopascals? In mmhg? 23. Describe the motion of particles of a gas according to kinetic theory. 24. What simple evidence demonstrates that gas particles are in motion? 11-2
3 THE NATURE OF LIQUID Describe the nature of a liquid in terms of the attractive forces between the particles * Differentiate between evaporation and boiling of a liquid, using kinetic theory Key Terms vaporization boiling point normal boiling point evaporation vapor pressure Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank can be completed with a term, short phrase, or number. Liquids and solids are known as 1 states of matter. Liquids are much 2 than gases. The conversion of a liquid to a gas or vapor is called 3. When a liquid becomes a gas below the boiling point of the 4, the process is called evaporation. Liquid evaporates faster when heated; however, evaporation itself is a 5 process. When a partially filled container of liquid is sealed, some of the particles in the liquid _6_. These particles collide with the walls of the container, producing a force called 7. The vapor pressure of a liquid can be determined by a device called a(n) 8. A liquid boils when its 9 equals the external pressure. The normal boiling point of a liquid is the temperature at which the vapor pressure is equal to 10. Part B True - False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 11. The particles of a liquid do not have enough kinetic energy to overcome the attractive forces between them to escape. 12. When a liquid occupies a closed container, there are more particles entering the vapor than condensing. 13. The change of a substance directly from a solid to a gas or vapor is called condensation 14. The rates of evaporation and condensation are equal at equilibrium. 15. Adding heat to a liquid will increase the temperature of the liquid. 16. During evaporation, the temperature of a liquid decreases. 11-3
4 Part C Matching Match each description in Column B to the correct term in Column A. Column A Column B. 17. vapor pressure. 18. condensation. 19. normal boiling point.20. liquid.21. intermolecular forces a. the pressure above a liquid in a sealed container b. the attractive forces between molecules c. the boiling point of a liquid at a pressure of kpa d. a relatively incompressible form of matter with a fixed volume but not fixed shape. e. the change of a gas or vapor to the liquid state Part D Questions and Problems 22. Describe what happens on a particle level when a liquid is at its boiling point. 23. Liquid A has a vapor pressure of 7.37 kpa at 40 C. Liquid B has a vapor pressure of kpa at 40 C. Which liquid would evaporate faster at 40 C? Explain your answer. 11-4
5 THE NATURE OF SOLID Describe how the degree of organization of particles distinguishes solids from gases and liquids Distinguish between a crystal lattice and a unit cell Explain how allotropes of an element differ Key Terms melting point allotropes amorphous solids glasses crystal unit cell Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank can be completed with a term, short phrase, or number. Solids tend to be dense and 1_. They do not flow or take the shape of their containers, like liquids do, because the particles in solids vibrate around 2 points. When a solid is sufficiently heated and its particles vibrate so strongly that they are no longer held in fixed positions, the solid 3. The 4 is the temperature at which a solid turns to liquid. The melting and 5 of a substance are at the same temperature. In general, ionic solids tend to have relatively 6 melting points while molecular solids tend to have relatively low melting points. Most solids are 7 in nature. The particles are arranged in a pattern known as a crystal 8. The smallest subunit of a crystal lattice is the 9. Some solids have a disordered array of particles and are 10_. 11-5
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