Coyle/Tang-JohnsonChemistry Study Guide

Chapter 13Study Guide–States of Matter

TEST: Thursday 4/7/11

13.1The Nature of Gases

Define the following terms:

-kinetic energy (KE = 1/2 mv2)

-kinetic theory

-gas pressure

-vacuum

-atmospheric pressure

-barometer/manometer

-pascal (Pa)

-standard atmosphere (atm)

1. What is STP in…

a) atm?b) mmHg (torr)?c) kPa?d) lbs/in2?

2. 0◦C = ____ K

3. What is the formula for pressure?

4. What are the 4 fundamental assumptions about gases in the kinetic molecular theory for ideal gases?

13.2The Nature of Liquids

Define the following terms:

-vaporization

-evaporation

-vapor pressure

-boiling point

-normal boiling point

1. Why do liquids have a definite volume?
2. Where does evaporation occur?

3. As evaporation occurs, which particles tend to escape the liquid first?

4. Circle the correct word: As evaporation takes place, the liquid’s temperature (increases/decreases), therefore, evaporation is a (heating/cooling) process and is (exothermic/endothermic).

5. What happens to the rate of evaporation as liquid is heated?

6. In a closed container or system at constant vapor pressure, how does the rate of evaporation of liquid compare to the rate of condensation of vapor?

7. What is boiling?

8. True or False? When the external pressure is greater than the vapor pressure of the bubbles in the liquid, boiling does not happen.

9. Why does water boil at a lower temperature at high altitudes?

13.3The Nature of Solids

Define the following terms:

-melting point

-crystal

-unit cell

-allotropes

-amorphous solid

-glass

1. True or False? The melting point is a different temperature than the freezing point.
2. Why do ionic solids have high melting points?

3. What’s the difference between a crystal lattice and a unit cell?

4. What are the three types of unit cells that can make up a cubic crystal system? Sketch a diagram of each.

5. Give three examples of amorphous solids:

13.4Changes of States

Define the following terms:

-sublimation

-phase diagram

-triple point

1. At what temperature does sublimation occur?

2. What do the lines separating the phases in a phase diagram represent?

The common phase or state changes are listed in the table below:

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Condensed state / Process / Less condensed state / Heat effect / Name for heat effect
Solid / melting → / Liquid / endothermic / Heat of fusion
Liquid / boiling → / Gas / endothermic / Heat of vaporization
Solid / sublimation→ / Gas / endothermic / Heat of sublimation
Gas / condensation→ / Liquid / exothermic / Heat of condensation
Gas / deposition→ / Solid / exothermic / Heat ofdeposition
Liquid / crystallization→ / Solid / exothermic / Heat of crystallization

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Note that the changes are endothermic when the system goes from a condensed state to a less condensed state. This results from the fact that energy is needed to "pry' apart a condensed state. The particles are attracted to one another in the condensed state by intermolecular forces. The stronger the forces the bigger the energy change. The reverse process has the opposite sign.

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