1. Homework & Formative Assessment Review

2. Questions??

3. Check for Understanding
Physical Property
Chemical Property
Blue Color
Density
Flammability
Solubility
Reacts with acid to form H2
Supports combustion
Volume
Melts at 32C
Reacts with water to form a gas
Baking soda and vinegar form CO2
Diamond scratches wood surface
Water boils at 100 C
HCl is used to neutralize NaOH by producing water
The rock has a shiny, luster appearance

4. Check for Understanding
A physical property is observed with the senses and can be determined without destroying the object.
A chemical property indicates how a substance reacts with something else. The original substance is fundamentally changed when observing a chemical property.

5. Test 1 – 30 minutes Matter Classification of Matter
Physical/Chemical Changes-Properties
Chemical Reactions
COMPLETE INDIVIDUALLY, NO NOTES!!
Submit on front table when completed.
Review reading Chapter 10 pages ( )
Begin working on Part 4 of Unit Packet!!

6. Learning Objective(s)
I can explain the differences between gases, liquids, and solids using the kinetic molecular theory (KMT)
I can analyze phase diagrams and explain phase changes.

7. States of Matter
What happens when a cube of ice is melted?

8. Nanoscopic
Molecules are very close together and densely packed
Molecules are closer together but still very separated
Molecules are very far apart
Shape
Will form its own shape and be rigid or fixed
Will take the shape of the container
Volume
Has a constant volume independent of the size of the container
Takes the volume of the container
Particle motion
Local vibration in a fixed position, no long-range motion
Random motion throughout the container

9. Kinetic Molecular Theory
These assumptions are true for an ideal gas (hypothetical gas that perfectly fits all assumptions of the kinetic molecular theory)
Real gases behave like ideal gases at low pressure and high temperatures.

10. Kinetic Molecular Theory
Gases consist of large numbers of tiny particles that are far apart relative to their size.
Collisions between gas particles and between particles and container walls are elastic collisions (no net loss of total kinetic energy)
Gas particles are in continuous, rapid, random motion
There are no forces of attraction between gas particles (bounce off)
The temperature of a gas depends on the average kinetic energy of the particles of the gas.
KE = 1/2mv2
Temperature is a measure of KE

11. Kinetic Molecular Theory - GASES
Expansion
No definite shape or volume
Fill container and take its shape
Fluidity
Glide past one another easily
Ability to flow and act like liquids (both are “fluids”)
Low Density
Compressibility
Far apart push closer together
Volume decreases
Diffusion and Effusion
Spread out and Mix together
Diffusion
Spontaneous mixing of particles of two substances caused by random motion
Effusion
A process by which gas particles pass through a tiny opening
Real Gas
A gas that does not behave completely according to the assumptions of the kinetic molecular theory
High pressure and low temperature

12. Kinetic Molecular Theory - GASES
Describe conditions under which a real gas is not likely to behave ideally.
Which of the following gases would you expect to deviate significantly from ideal behavior: Ne, F2, Cl2, CO2, HBr, or NH3?
What happens to gas particles when a gas is compressed and cooled?

13. Kinetic Molecular Theory - Liquids
Definite volume and takes shape of its container
Particles are in constant motion
Closer together in liquids than gases
Caused by intermolecular forces
Dipole-dipole forces
London dispersion forces
Hydrogen bonding
More ordered than gases
Particles not bonded together in fixed positions
Move about constantly
Fluids
Relatively high density
Due to close arrangement of particles
Relative incompressibility
Compress very little because particles are more closely packed together

14. Kinetic Molecular Theory - Liquids
Ability to diffuse
Mix with other liquids
Slower in liquids than gases
High temperature = higher rate of diffusion
Surface Tension
A force that tends to pull adjacent parts of a liquid’s surface together, thereby decreasing surface area to the smallest possible size.
Capillary Action
Attraction of the surface of a liquid to the surface of a solid.
Evaporation and Boiling
Vaporization
Liquid or solid changes to a gas
Evaporation
Particles escape from the surface of a nonboiling liquid and enter a gas state.
Formation of Solids
Freezing
Physical change of a liquid to a solid by removal of energy as heat or solidification

15. Kinetic Molecular Theory - Liquids
Describe a liquid (apply KMT).
High Density
Diffuse (compare to gases)
Evaporate
Capillary Action … why does it occur?
Difference between vaporization and evaporation, provide an example of both.

16. Kinetic Molecular Theory - Solids
Definite shape and volume
Particles are more closely packed than liquid or gas
Intermolecular forces are more effective
Relatively fixed positions
Vibrational movement around fixed points
More order
Crystalline solids
Consist of crystals
Crystals are substances in which particles are arranged in an orderly, geometric, repeating patter
Amorphous Solids
Particles are arranged randomly
Glass, plastics
Definite Melting Point
High Density and Incompressibility
Low rate of diffusion

17. Kinetic Molecular Theory - Solids
Describe the solid state.
Volume
Shape
Density
Diffusion
Amorphous solid vs. crystalline solid?

18. Water … H2O Diagram of water Hydrogen bonds between water molecules
Why does ice float
Less dense due to empty space between particles
Therefore it only forms on the surface of lakes and insulates the liquid beneath it (prevent total freezing which would kill living things in the lake)

19. Questions?

20. Formative Assessment

21. Average 22/25 (88%) Questions? Next assessment…Tomorrow!
Test #1 Analysis
Average 22/25 (88%)
Questions?
Next assessment…Tomorrow!

22. Phase Change Check-Up List the 6 phase changes.
Describe the particle motion between them
Use words like: energy, motion, close together, far apart…

23. Phase Diagrams Identify the following parts of the phase diagram… W PB C W P R

24. Changes of State Phase: Condensation: Equilibrium:
Any part of a system that has uniform composition and properties.
See Table 2 page 342
Condensation:
The process by which a gas changes to a liquid.
Equilibrium:
A dynamic condition in which two opposing changes occur at equal rates in a closed system. (i.e. water vapor in bottle)

25. Heat Removed
The three diagrams above, if viewed from left to right, show the processes of
a. melting and then boiling.
b. sublimation and then deposition.
c. condensation and then freezing.
d. a new substance being formed.

26. Changes of State Diagram of Table 2 pg 342

27. Phase Diagram
A graph of pressure versus temperature that shows the conditions under which the phases of substance exist.
The curves represent states of equilibrium between phases.
Triple point
Indicates the temperature and pressure conditions at which the solid, liquid, and vapor of the substance can coexist at equilibrium. (where all curves meet)
Critical point
Indicates the critical temperature and critical pressure of a substance.
Critical temperature
The temperature above which the substance cannot exist in the liquid state. (water C)
Critical pressure
The lowest pressure at which the substance can exist as a liquid at the critical temperature. (water atm)

28. Equilibrium Vapor Pressure of Liquid
The pressure exerted by a vapor in equilibrium with its corresponding liquid at a given temperature.
Proportional to the concentration of vapor molecules.
Volatile liquids
Liquids that evaporate readily.
Weak forces of attraction between their particles.

30. Analyzing Phase Diagrams
Describe all the changes a sample of solid carbon dioxide would undergo when heated from -85 °C to its critical temperature at a pressure of 1.00 atm.
Describe all the changes a sample of solid carbon dioxide would undergo when heated from -85 °C to its critical temperature at a pressure of 73 atm.

31. Analyzing Phase Diagrams
Describe all the changes a sample of carbon dioxide vapor would undergo when cooled from 31.1 °C to -85 °C at a pressure of 8.00 atm.

32. Analyzing Phase Diagrams
At approximately what pressure will carbon dioxide be a vapor at 0 °C ?

33. Analyzing Phase Diagrams
Determine the critical temperature and pressure for carbon dioxide.

34. Phase Change Check-Up List the 6 phase changes.
Describe the particle motion between them
Use words like: energy, motion, close together, far apart…

35. Phase Diagrams Identify the following parts of the phase diagram… W PB C W P R

36. Exam 2 TOMORROW!!