2. Chapter 10 – States of Matter 10.1 The Kinetic Molecular Theory of Matter

3. The Kinetic Molecular Theory KMT – based on the idea that particles of matter are always in motion. Used to explain properties of s, l, and g’s in terms of the energy of particles and the forces between them.

4. The KMT and Gases Provides a model of an ideal gas Ideal gas – a hypothetical gas that fits all assumptions of the KMT.

5. The 5 Assumptions 1.Gases consist of large # of tiny particles that are far apart. 2.Collisions b/t particles and their container walls are elastic. 3.Particles r in continuous, rapid, random motion. 4.No attractive forces b/t them. 5.Temp of gas depends on kinetic E of par

6. Kinetic Energy KE = ½ mv 2 m = mass of particle, v = velocity All particles of the same gas have the same mass, so as temp changes, so does v. At the same temp, gases w/ higher masses move slower

7. Properties of gases and the KMT Expansion – no def. vol or shape –# 3 and 4 Fluidity – particles glide past others –# 4 Low Density – Far apart –# 1

8. Properties of gases and the KMT Compressibility – far apart –# 1 Diffusion and Effusion – # 3 –Diffusion – spontaneous mixing of particles of 2 subs. caused by random motion. –Effusion – gas particles pass thru tiny opening

9. Real vs. Ideal Real gas – does not behave completely according to KMT Polar gas molecules are more likely to deviate from ideal behavior. Try the section review on page 332 numbers 2-7.