Chapter 16 – SOLIDS, LIQUIDS & GASES

Section 1 – KINETIC THEORY

States of Matter GAS SOLID                                                                          LIQUID

The Kinetic Theory Explains how particles behave All matter is made of small particles These particles are in constant, random motion Particles collide with each other & with the walls of containers                              

Total energy of a material’s particles                                 Thermal Energy Causes particles to vibrate in place

Average Kinetic Energy = temperature of a substance                  How fast the particles are moving The the temp, the slower the motion

Solid State of Matter Particles closely packed together in specific geometric arrangement                                                                

Liquid State of Matter Liquids flow and take the shape of their container Solids begin to liquefy at the melting point as particles gain energy to overcome arrangement                                                                 Heat of FUSION

Gaseous State of Matter Gases spread evenly throughout their container (diffusion) When a liquid has enough energy to escape the attractive forces of other particles                                                                                                      

Gaseous State of Matter Heat of Vaporization Energy changing a liquid to a gas At the boiling point – Pressure of the liquid’s vapor = the presure of the atmosphere                                                                                                                                  

Heating Curve of a Liquid Melting Point & Freezing Point                                                                 Melting Point & Freezing Point Boiling Point

Plasma State of Matter High temperature gas Balanced positively and negatively charged particles Most abundant state                                                                

Happens in most solids, liquids & gases Thermal Expansion Increase in the size due to an increase in temperature If temp then size Happens in most solids, liquids & gases Water is an exception – it expands as it becomes a solid!

Exceptions – these do not act as expected - Liquid Crystals Amorphous Solids

AMORPHOUS SOLIDS Lack tight ordered structure No definite temperature for change from solid to liquid. Glass, ceramic & plastics

LIQUID CRYSTALS Don’t completely lose ordered arrangement upon melting Used in LCD’s Watches, clocks, notebook computers & TV’s

Properties of Fluids Chapter 16 - 2

Buoyant Force Buoyancy = the ability of a fluid to exert an upward force on an object immersed in it. Buoyant Force – the supporting force on an immersed object If force = weight, object will… If force is less than weight, object will… FLOAT SINK

The older one b/c he displaces more water. Archimedes’ Principle The buoyant force on an object is equal to the weight of the water displaced by the object Which has a higher buoyant force, a baby in a bath tub or a 40 year old person? The older one b/c he displaces more water.

D = m / v Density… Objects will float if their density is less that the density of the fluid it is placed in Why do ships float???

Pascal’s Principle Pressure applied to a fluid is transmitted throughout the fluid. What are some everyday examples of this? Toothpaste tubes, balloon animals

Bernoulli’s Principle As velocity of a fluid increases, the pressure exerted by the fluid decreases. The faster air flows over the wings. What do we know about the pressure above the wing? It’s lower!

Viscosity = resistance to flow Different structures cause different tendencies to flow Particles “pull” other particles with them increasing the flow As temperature increases, viscosity decreases allowing for easier flow Ex: Honey has a higher viscosity than water, b/c it does not flow as easily.

Sec. 16.3 Behavior of Gases

Pressure : SI Unit = Pascals (Pa) Pressure = Force/Area Collisions of particles in air result in atmospheric pressure – Highs and Lows in weather Particles colliding with walls of a container create GAS pressure

Why does this balloon stay inflated? The particles in air striking the balloon’s walls forces them outward.

British scientist, Robert Boyle 1. Boyle’s Law – relates pressure and volume British scientist, Robert Boyle At a constant temp, volume of gas decreases as pressure increases. (inverse relationship) P1V1 = P2V2 Why does a weather balloon expand as it rises in the atmosphere?

French scientist, Jacques Charles 2. Charle’s Law – relates volume and temp French scientist, Jacques Charles At a constant pressure, volume increases as temp increases. (direct relationship) V1T2 = V2T1 Explain this using Kinetic Theory of Matter.

3. Gay-Lussac’s Law – relates pressure and temp At a constant volume, as temp increases, pressure increases. (what kind of relationship is this?) T1P2 = T2P1 Explain what will happen to a canister that says “keep away from heat” if placed in a heated area?