Chemistry Packet # 12

Name ______Hr. ______

  1. Phase diagram
  2. Viscosity
  3. Pressure
  4. Diffusion
  5. Kinetic Molecular Theory
  6. Amorphous Solid
  7. Melting Point
  8. Barometer
  9. Sublimation
  10. Boiling Point
  11. Surface Tension
  12. Freezing Point
  13. Temperature
  14. Elastic Collisions
    Kinetic molecular theory

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  1. Convert the following to Kelvin:
  1. 320Cb. 00 Cc. -26 0C
  1. The kinetic molecular theory describes the behavior of gases in terms of particles in ______.
  1. The kinetic molecular theory makes the following assumptions:
  2. In a sample of a gas, the volume of the gas particles themselves is very ______compared to the volume of the sample.
  1. Because gas particles are far apart, there are no significant attractive or repulsive ______between the particles.
  2. Gas particles are in constant and ______motion.
  1. The collision between gas particles are ______; that is, no ______energy is lost.
  1. The kinetic energy of a particle is represented by the equation ______
  1. ______is a measure of the average kinetic energy of the particle.
  1. Gases are ______dense than solids because there is a lot of space between the particles of a gas.
  2. The ______motion of a gas particles causes a gas expand until it fills its container.
  1. The density of a gas ______as it is compressed.
  1. The diffusion of a gas is caused by the ______motion of the particles of the gas.
  1. Lighter gas particles diffuse ______rapidly that do heavier gas particles.

Forces of Attraction

Notes:

  1. Ionic, metallic, and covalent bonds are examples of what type of force?
  2. Dispersion forces, dipole-dipole, and hydrogen bonds are examples of what type of force.
  3. Describe dispersion forces.
  4. Describe dipole – dipole forces.
  5. Describe a hydrogen bond.

Lab section:

  1. How many drops of water fit onto a penny before it over flows?
  2. With a beaker of water, could you float a paper clip?

9-17 Terms: Cohesion, Adhesion, Surface Tension, Physical Change, Chemical change

Which term or terms above best describe the situation (you may use multiple terms)?

  1. An ice cube melts into liquid water ______
  2. The morning dew makes the grass wet ______
  3. A belly flop hurts______
  4. Hydrogen gas burns in oxygen gas to make water______
  5. Water boils______
  6. A meniscus forms in a graduated cylinder______
  7. A big water drop forms a round shape______
  8. Water condenses into drops on the bathroom mirror______
  9. You get out of the shower and you are still wet______
  10. Honey has high viscosity therefore flows very slowly.______

Date ______Name ______

Lab graphing water phase changes

Purpose: To graph the phase changes form melting ice to boiling water and to compare

heat intake to temperature during phase changes.

Procedure: 1) Fill a beaker full of ice.

2) Put beaker of ice on a ring stand under Bunsen burner.

3) Record the temperature of the beaker with the thermometer that is 2 cm

fromtop of the beaker every 30 seconds until it has been boiling for

three or four minutes.

***Mark the time the ice is all gone and when itstarts to boil.

4) Make a graph of temperature vs. time.

Data:

TimeTemperatureTimeTemperature

010

30 sec10:30 1 11

1:3011:30

212

2:3012:30

3 13

3:3013:30

4 14

4:3014:30

515

5:3015:30

616

6:3016:30

717

7:3017:30

818

8:3018:30

919

9:3019:30

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GRAPH:

CONCLUSIONS:

Use above graph to answer the following questions.

1.Identify the point on the graph where each of the following occurs.

melting begins freezing begins boiling begins condensation begins

2.(T or F) As the substance goes from D to C, it gives off heat.

3.Why does the temperature remain constant from A to B? (Speak in terms of motion and bonds.)

4. Why does steam at 100 C (pt D) produce a more serious burn than liquid water at 100 C (pt C)?

Phase changes

Notes:

Complete the table by writing the initial and final phases for each phase change and making a check(√ ) in the correct energy column.

Phase / Phase / Energy / Energy
Phase change / initial / final / required / released
1. Condensation
2. Deposition
3. Freezing
4. Melting
5. Sublimation
6. Vaporization

7. Temperature at which a liquid is converted into a solid. ______

8. Temperature at which the forces holding a solid together at broken.______

9. Temperature at which the vapor pressure of a liquid equals the atmospheric pressure.______

From the graph above answer the following:

1. What will be the boiling point of C2H5OH when the vapor pressure is 600 mm Hg?

2.What is the normal boiling point for (C2H5)2O ?

3.What is the pressure when water boils at 70 C?

4.Which liquid on the chart has molecules that exert the strongest cohesive forces on each other?

5.Which of the liquids would be the easiest to evaporate?

6.(T or F) Increasing the temperature usually causes the vapor pressure to increase.

On the graph: label each numbered point as ∆KE (change in kinetic energy) or ∆PE (change in potential energy).

  1. What are the variables on the phase diagram? ______
  2. What phase of water is represented by each of the following regions?
  3. Region I ______
  4. Region II ______
  5. Region III ______
  6. What does point 2 represent? ______
  7. What do the following lines represent?
  8. A______
  9. B______
  10. C______
  11. What do the following points represent?
  12. 1______c. 3______
  13. 2______d. 4______

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