Chapter 16: Solids, Liquids, and Gases

Chapter 16 Overview Kinetic Theory A. States of Matter 1. Solids 2. Liquid a. Melting point b. Heat of Fusion 3. Gas a. Boiling Point b. Heat of Vaporization 4. Plasma B. Thermal Expansion Behavior of Gases A. Pressure - pascal B. Boyle’s Law C. Charles’s Law

Kinetic Theory explanation of how particles in matter behave All matter is composed of small particles. These particles are in constant, random motion. These particles are colliding with each other and the walls of their container.

Phases of Matter Phases The arrangement of particles Motion of molecules Definite shape? Definite volume? Solid Packed tightly and vibrate in place Yes Liquid Able to slide past each other No take the shape of the container Gas Bounce far apart

Phase Changes Phase Changes From what Phase-to-Phase does change occur? Point at which Phase Change occurs Melting Solid to Liquid Melting point Freezing Liquid to Solid Freezing point Vaporization Liquid to Gas Boiling point Condensation Gas to Liquid Condensation point Sublimation Solid to Gas Sublimation point

Phase Change Diagram Heat of vaporization Heat of fusion Gas Liquid Heat of Fusion: energy require to change a solid to a liquid *heat absorbed *no change in temp. Heat of Vaporization: energy require to change a liquid to a gas Gas Heat of vaporization Liquid Heat of fusion Solid

Thermal Expansion Increase in the size of a substance when temperature increases. Exception to the rule: WATER Water expands as it cools. Structure of Water

Gas Laws: Boyle’s, Charles’s, Gay-Lussac’s Phases Special Properties Solid *Crystals: particles are in regular repeating patterns *Amorphous: solids that don’t have highly ordered structure like crystals – “without form” Liquid Viscosity: resistance to flow Liquid crystals: start to flow during melting phase but don’t lose all their geometric order Gas Gas Laws: Boyle’s, Charles’s, Gay-Lussac’s

Gas Laws show relationship between pressure, temperature, and volume Explanation Boyle’s As volume decreases, pressure increases. Charles‘s As temperature increases, volume increases. Gay-Lussac’s As temperature increases, pressure increases.

Which Gas Law is this?

Which Gas Law is this?

Graphing: Phase Changes

Lab: Four States of Matter Corrections to Lab Procedure: 1.            Put 5 ice cubes in a 150 mL beaker.   2.          Observe temperature every minute. 3.          Take 2 readings before putting beaker on hot plate. 4.          Put hot plate on medium until ice has completely melted 5.          Once ice has melted turn hot plate up to high. 6.          After boiling occurs, continue to record temperatures every 1 minute for 2 minutes.

Lab: Pop Can and Gas Laws Procedure: 1. Pour 5 mL of water into the pop can. 2. Put pop can on hot plate. Let it boil for 1 minute. 3. With tongs, put pop can upside down in beaker of COLD water. Observations: (Describe what happened.) Gas Law: (What Gas Law does this apply to?) Conclusion: (Explain why the can behaved as it did according to the Gas Law.)

Lab: Gas Pressure and Volume