1. Chapter 8 Section 1 Describing Chemical Reactions p. 261-275 1 Gases Chapter 10/11 Modern Chemistry Sections 10.1, 11.1-11.3 The Kinetic Molecular Theory of Matter Gases and Pressure The Gas Laws Gas Volumes and the Ideal Gas Law

2. Chapter 10 Section 1 Kinetic Molecular Theory p. 329-332 2 The Kinetic Molecular Theory of Matter Section 10.1

3. Chapter 10 Section 1 Kinetic Molecular Theory p. 329-332 3 KMT Animation Insert Holt Visualizing Matter Disc 2

4. Chapter 10 Section 1 Kinetic Molecular Theory p. 329-332 4 Based on the idea that particles of matter are always in motion. Explains the properties of gases, liquids and solids in terms of energy of particles and the forces that act between them. Provides a model of an ideal gas Ideal gas: A hypothetical gas that perfectly fits all the assumptions of the kinetic molecular theory. Kinetic Molecular Theory of Gases

5. Chapter 10 Section 1 Kinetic Molecular Theory p. 329-332 5 KMT Animation

6. Chapter 10 Section 1 Kinetic Molecular Theory p. 329-332 6 1.Gases consist of large numbers of tiny particles that are far apart in relation to their size. TINY PIECES – LARGE SPACES IN BETWEEN 2.Collisions between gas particles and between particles and container walls are elastic collisions ELASTIC COLLISIONS - NO ENERGY LOSS Kinetic Molecular Theory

7. Chapter 10 Section 1 Kinetic Molecular Theory p. 329-332 7 3.Gas particles are in continuous, rapid random motion. The particles have kinetic energy. PARTICLES ARE IN MOTION 4.There are no forces of attraction between gas particles. NO FORCES OF ATTRACTION Kinetic Molecular Theory

8. Chapter 10 Section 1 Kinetic Molecular Theory p. 329-332 8 p. 330 Gas Particle Motion Gas particles gravel in a straight-line motion until they collide with each other or the walls of their container.

9. Chapter 10 Section 1 Kinetic Molecular Theory p. 329-332 9 5.The temperature of a gas depends on the average kinetic energy of the particles. AVERAGE KINETIC ENERGY…TEMP m = mass v = velocity All the particles in a sample of gas have the same mass so K.E. depends only on velocity Kinetic Molecular Theory K.E. = mv2v2 1 2

10. Chapter 10 Section 1 Kinetic Molecular Theory p. 329-332 10 Temperature and K.E. Insert Holt Visualizing Matter Disc 2

11. Chapter 10 Section 1 Kinetic Molecular Theory p. 329-332 11 The KMT applies only to IDEAL gases. Gases behave ideally most of the time. What is your ideal?

12. Chapter 10 Section 1 Kinetic Molecular Theory p. 329-332 12 Gases behave ideally at common temperatures and pressures. At high pressures and low temperatures gases behave non-ideally. Polar gases deviate from ideal behavior more than nonpolar gases Ideal vs. Real Gases

13. Chapter 10 Section 1 Kinetic Molecular Theory p. 329-332 13 Gases completely fill their container. –Particles move rapidly in all directions. (3) –There are no attractions between particles. (4)Expansion Gas particles glide past each other to flow. –There are no attractions between particles. (4) Fluidity

14. Chapter 10 Section 1 Kinetic Molecular Theory p. 329-332 14 The density of a gas is 1/1000 th of a liquid or solid. –Particles are far apart. (1) Low Density Molecules of a gas can be pushed together and the volume decreased. –Particles are far apart. (1) Compressibility

15. Chapter 10 Section 1 Kinetic Molecular Theory p. 329-332 15 Gas Properties Animaiton

16. Chapter 10 Section 1 Kinetic Molecular Theory p. 329-332 16 The spontaneous mixing of the particles of two substances –Particles move rapidly. (3) –Particles are far apart. (4) –caused by their random motion.Diffusion p. 331

17. Chapter 10 Section 1 Kinetic Molecular Theory p. 329-332 17 Diffusion vs. Effution

18. Chapter 10 Section 1 Kinetic Molecular Theory p. 329-332 18 A process by which gas particles pass through a tiny opening. The rate of effusion is directly proportional to the velocity of the particles…so… low mass particles diffuse faster.Effusion

19. Chapter 10 Section 1 Kinetic Molecular Theory p. 329-332 19 Particle Mass & Effusion

20. Chapter 10 Section 1 Kinetic Molecular Theory p. 329-332 20 Ch 10 Sec 1 Homework Page 332 # 1-7