INTRODUCTION: In our everyday lives the matter that we encounter can be classified in one of three states, solid, liquid or gas. There is a fourth and even fifth state of matter but these are not part of our everyday existence. The fourth state is plasma and the fifth state is speculated as the state of matter in a neutron star or black hole. Chemists have developed the kinetic theory of matter with which they describe the behavior of the particular state in terms of the behavior of particles of matter. For example, gaseous particles are far apart from each other and colliding with no attraction between the particles, whereas the particles in a liquid or solid state are in contact with each other and sticking together to various degrees. Gases, in particular, have been the subject of separate study for more than 300 years. Gases have received this attention because their behavior can be idealized. This means that scientists can make some assumptions about gases and the particles that make them up. Because of the reasonable nature of these assumptions, scientists have been able to model gas behavior with a simple mathematical relationship. In this unit we will learn about the kinetic theory of matter and apply its explanations to the three common states. We will also examine the simple relationship between the volume, pressure, amount and temperature of a gas, called the Ideal Gas Law.
OBJECTIVES: As you study this unit, you should be able to do the following:
1.
Describe the kinetic-molecular theory, and explain how it accounts for
observed physical behavior in solids, liquids and gases. (13-1 and 14-1)
2.
Explain what gas pressure means and describe how it is measured by
reading a barometer or manometer. (13-2)
3.
State the gas laws, give their mathematical relationships and describe
the relationships in terms of the kinetic molecular theory.
(Boyle’s Law, Charles’ Law, Gay-Lussac’s Law, Avogadro’s Law, and
Dalton’s Law) (13-3)
4.
Discuss the significance of the ideal gas equation, pointing out the
assumptions behind the equation. Compare
ideal and real gases.
5.
Describe the different types of intermolecular forces. (14-1)
Define viscosity and surface tension, and explain their relationship to
intermolecular forces. (14-2)
6.
Compare the structure and bonding in the four categories of solids to the
properties they exhibit. (14-3)
7.
Describe vaporization, condensation, boiling, freezing and melting.
(14-4)
8.
Identify the features of a phase diagram of a pure substance. (14-4)
LEARNING ACTIVITIES:
To learn about objectives 1-4: (Ch. 13 questions due 2nd class meeting of week of March 7, 2005.)
1. READ Chapter 13, pp. 417-449.
2. WRITE answers to end of the chapter question #s 1-8, 15, 16, 19, 30, 32, 35-40, 42, 44, 47 found on pp. 452-455.
3. COMPLETE worksheet, “Ten Elementary Gas Law Problems.”
4. READ and PERFORM “Getting the Volume Right” Lab exercise.
To learn about objective 5-8: (Ch. 14 questions due – )
1. READ Section 13-1; pp. 417-423, and Chapter 14; pp. 456-489. See objectives for specific section.
2. WRITE answers to end of the chapter question #s 1-4, 7, 8, 10-14, 18, 19, 23, 25, 28-32 found on pp. 492-493.
3. READ and PERFORM “Observing and Measuring the Triple Point of Dry Ice” lab sheet.
4. EXPLORE interactive phase diagram at: http://titanium.fullerton.edu/shock/PHASED.htm
5. WRITE essay according to the CPR assignment on “Interpreting Single Substance Phase Diagrams.” (Maximum 300 words) found at CPR site: http://cpr.molsci.ucla.edu/cpr/cpr/login.asp
To make sure you understand the objectives for this unit:
ASK me, the teacher, any lingering QUESTIONS
TAKE the Unit’s Self-Test
Quiz on Ch. 13 (Ch.
13 HW also due): 2nd Class meeting week of March 7, 2005.
.
“Getting The Volume Right” write-up due:
“Observing and Measuring the Triple Point of Dry Ice”
write-up due:
CPR Essay due: Thursday March 17, 2005 by 11:30 pm on the CPR site.
CPR Final Assignment completion date: Wed. March 23, 2005 by 11:30 pm.
