Kinetic Molecular Theory

1. Kinetic Molecular Theory • A theory that envisions molecules in motion • Best describes properties and behaviors of gases • Can be applied to all states of matter

2. Solid - Molecules are held close to each other by their attractions of charge. They will bend and/or vibrate, but will stay in close proximity. • Liquid - Molecules will flow or glide over one another, but stay toward the bottom of the container. Motion is a bit more random than that of a solid. • Gas - Molecules are in continual straightline motion. The kinetic energy of the molecule is greater than the attractive force between them, thus they are much farther apart and move freely of each other.

3. 6 Basic Principles of KMT 1. Gases consist of tiny (submicroscopic) particles.

4. 2. Gas particles are very far apart; the volume occupied by a gas consists mostly of empty space (typically about 99.9% empty). 3. Gas particles are not attracted to each other.

5. 4. Gas particles move randomly in all directions, traveling in straight lines. * Gas molecules travel at very high speeds, about 6000 km/hr (~2700 mi/hr). 5. The higher the average speed of the particles, the higher the temperature of that substance. • Absolute temperature: T based on average particle speed; measured in Kelvin (K) • Absolute zero (0 K): particles are not moving; there is no T below 0 K. K = °C + 273

6. 6. Gas particles collide with each other and with the walls of the container without losing energy. These are called Elastic collisions. There is no loss of energy. Pressure= the collision of gas particles with a surface; force per unit area

7. Nature of Gases • Expandable – no definite shape or volume; completely fill their container • Compressible – Particles very far apart are able to be crowded close together; volume can be decreased as the pressure increases • Fluid – having insignificant attractive forces, gas particles easily glide past each other. Like a liquid, a gas has the ability to flow.

8. Low density – gas molecules are very far apart which lead to their low density (1/1000 the density of the same substance as a liquid or solid.) • Diffuse - spontaneous mixing of two gases or liquids because particles move randomly • Effuse - process by which gas molecules pass through a small opening from a container at higher pressure to one oflower pressure (a bike tire with a hole)

9. Kinetic Molecular applies to Ideal Gases but real gases do not behave completely according to the KMT. • Very high pressures and very low temperatures, gases will be closer together and attractive forces will apply. (Remember, with the KMT there are no attractive forces.)

10. Liquids and the KMT • Properties of a liquid • Definite volume; takes the shape of its container (fluid) • More ordered than a gas du to attractive forces • Attractive forces are intermolecular • Dipole-dipole • London dispersion forces • Hydrogen bonding

11. Con’t • Particles not bound together in fixed positions but are in constant motion *interesting fact: helium can flow uphill at temperatures close to absolute zero

12. Relatively High Density • Higher density due to closer arrangement of molecules as compared to a gas

13. Relatively Incompressible • Liquids behave more like a solid than a gas regarding compressibility due to the closeness of the molecules • Liquids behave more like a gas in that they are able to transmit pressure equally in all directions.

14. Diffusion • Able to diffuse due to constant random motion of the particles but it is slower than the diffusion of a gas • Increase the temperature…..increase KE ….increase the rate of diffusion

15. Surface tension Force that tends to pull adjacent part’s of a liquid’s surface together thereby decreasing the surface area Results from attractive forces

16. Physical properties Water: • Is clear, colorless, odorless, and tasteless * Colors, tastes and odors are caused by substances dissolved in the water. • Boils at 100°C • Freezes at 0°C • Density = 1.0 g/mL (at 4°C)

17. Vaporization Evaporation: • The fastest molecules break the H bonds and escape from the surface and become a gas; can occur at any T. * What is left behind is cooler than before because a high energy (i.e. hot!) molecule escaped, thus removing heat; ex: sweating Boiling: • Fastest molecules overcome H bonds and change phase beneath the surface. * The gas rises because it is less dense (about 1000 times less dense) than the liquid. http://www.visionlearning.com/library/science/chemistry-1/CHE1.1-matter.htm Gaseous matter - steam simulation

18. 13.2 Boiling Point: overcome attractive forces and escape the liquid • Altitude and Boiling Point

19. Sublimation Why does it bypass the liquid state? • Tends to occur in substances that have very low attractions between molecules. • Ex: dry ice (solid CO2) and iodine (I2) http://cwx.prenhall.com/petrucci/medialib/media_portfolio/13.html http://library.thinkquest.org/2690/exper/exp19.htm

20. Mercury Water Cohesion & Adhesion Cohesion: attractions within a liquid Adhesion: attractions between a liquid and something else • For water, adhesion is stronger than cohesion Meniscus: curve at the surface of a liquid • If cohesion is stronger than adhesion, meniscus is convex (like mercury)

21. Capillary action • Attraction of the surface of a liquid to the surface of a solid • Closely related to surface tension • A liquid will rise quite high in a very narrow tube and will wet the tube

22. http://kingfish.coastal.edu/biology/sgilman/770lecwatersalt.htmhttp://kingfish.coastal.edu/biology/sgilman/770lecwatersalt.htm Freezing: removal of heat • Density of ice (at 0°C) is 0.917 g/mL, so ice floats in water. • Most liquids become more dense as you cool them. However, when water freezes, a large expansion occurs. http://www.anglianwater.co.uk/schools/noscript/f1.htm * Where have you see H2O in repeating hexagonal patterns before? Water “organizing” with H bonds as it freezes. Forms hexagon shapes.

23. B.P. Temp (°C) M.P. C.P. F.P. Six Phase Changes GAS Vaporization Condensation LIQUID Sublimation Deposition SOLID Melting Freezing

24. Solids and the KMT

25. Phase Diagrams • The conditions of pressure and temperature at which two phases exist in equilibrium are indicated on a phase diagram by a line separating the phases. • Triple point is where all 3 phases exist at equilibrium