Chapter 13 Objectives: 1) Define the gaseous state in terms of particle volume, shape, motion, and energy. 2) Define kinetic energy. 3) Explain temperature in terms of kinetic energy. 4) Define pressure in regard to particle size, density, and motion. 5) Explain how pressure is measured. Be able to calculate pressure as measured using both open and closed ended manometers. Perform conversions between mm of Hg and Kpa. 6) Explain Dalton’s Law of Partial Pressures. Be able to perform Dalton’s Law calculations. 7) Define the liquid state in regard to shape, volume, and particle motion.

8) For the liquid state, define viscosity, surface tension, and capillary action; providing examples of each. 9) Define the solid state in regard to shape, volume, and particle motion. 10) Define crystalline solid and unit cell. 11) Describe the three types of unit cells. 12) Know the seven main shapes of crystals. 13) Define amorphous solids and provide examples.

14) Be able to label the parts of a Change of State Diagram 14) Be able to label the parts of a Change of State Diagram. Be able to gather information from the change of state diagram for a given substance. 15) Differentiate between evaporation and boiling point. 16) Be able to label the parts of a Phase Diagram. Be able to obtain information from a phase diagram for a given substance.

Ch. 13 States of Matter I) Gases A) The Kinetic-Molecular Theory 1) ____: A form of matter that flows to conform to the shape of its container, fills the container, and is easily compressed. 2) ____________________________: A theory that explains the properties of gases in terms of _______, ______, and ________ of its particles.

a) _______________: The particle size is very _______ relative to the empty space between them, therefore there is _______ attractive or repulsive forces between the particles. b) _________________: Particles move in ________ straight line paths until they collide with another particle (________ collisions: collide and bounce apart with little to no loss of energy). c) _________________: _________ Energy, __________ (m = mass and v= velocity or speed). _____________: A measure of the average kinetic energy of the particles in a substance.

*Through elastic collisions with the substances surrounding particles, the thermometer’s particles transfer energy in (temperature goes ______) or out (temperature goes ______).

B) Gas Pressure *_________: Force per unit area.

1) Measuring Air Pressure: *Air pressure pushes the mercury up the tube where it can be measured. *___________: An instrument used to measure air pressure. a) Average air pressure:

2) Measuring Gas Pressure: a) __________: An instrument used to measure gas pressure. b) Types of Manometers: b1) Open Ended:

b2) Closed Ended:

c) Units of Pressure: “Convert 680 mm of Hg to kPa?” d) __________ Law of Partial Pressures: The total gas pressure of a mixture is equal to the ____ of all the individual pressures.

Example problem 13-2 on page 391:

II) Liquids and Solids A) _________: A form of matter that flows, has definite volume, and takes the shape of its container. 1) Liquids and gases are ________ (they can flow through other fluids).

2) __________: A measure of a fluids resistance to flow 2) __________: A measure of a fluids resistance to flow. The stronger the attractive forces in the substance, the _________ the viscosity. *What happens to viscosity as temperature increases?

3) _________________: The energy required to increase the surface area of a liquid by a given amount (a measure of the inward pull of particles due to attractive forces). soap

4) __________________: The “creeping up” of a liquid onto the sides of its container (cohesive and adhesive forces).

B) ________: A form of matter that has its own definite shape and volume. 1) _____________ Solids: A solid whose particles are arranged in an orderly, geometric, 3-Dimensional structure. a) __________: The smallest arrangement of particles that takes a particular shape. a1) The three types of Unit Cells:

Simple: Body-Centered: Face-Centered:

a2) The Main Crystalline Shapes (page 401; Figure 13-19):

2) ___________ Solids: “Without shape,” a solid that lacks any crystalline structure. Examples:

III) Phase Changes *It’s all about losing or gaining energy (K.E.)! A) Change of State Diagram:

A) B) C) D) ________: Process in which the forces holding a solid together are broken and the substance becomes a liquid. E) __________: Opposite of melting. F) __oi____ : The temperature at which a liquid’s vapor pressure is equal to atmospheric pressure.

*Vapor: The gaseous state of a substance that is normally a liquid or solid at room temperature. *_____________: The process in which vaporization occurs only at the surface of a liquid. G) _______________: Opposite of boiling.

H) _____________: An energy requiring process in which a solid changes directly to a gas without passing through the liquid state. I) _____________: Opposite of sublimation.

B) Phase Diagrams

1) Phase Diagram: A graph of Pressure v 1) Phase Diagram: A graph of Pressure v. Temperature showing all three states of matter. a) ______________: The exact pressure and temperature at which all three states of matter exist simultaneously. *See page 409, Figure 13-28.