Chapter 16 –

SOLIDS, LIQUIDS &

GASES

Section 1 –

KINETIC THEORY

States of Matter

GAS                                                                         

                             

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

•Causes particles to vibrate in place

                               

•How fast the particles are moving

•The the temp, the slower the motion

= temperature of a substance

                

Solid State of MatterParticles closely packed together in specific geometric arrangement

                                                               

Heat of FUSION

Liquid State of MatterLiquids flow and take the shape of their container

Solids begin to liquefy at the melting point as particles gain energy to overcome arrangement

                                                               

Gaseous State of MatterGases spread evenly throughout their container (diffusion)

When a liquid has enough energy to escape the attractive forces of other particles

                                                                                                     

Gaseous State of MatterHeat 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

Boiling Point

Plasma State of MatterHigh temperature gasBalanced positively and negatively charged particles –Most abundant state

                                                               

Thermal ExpansionIncrease in the size due to an

increase in temperature

If temp then size

Happens in most solids, liquids &

gasesWater is an exception – it expands

as it becomes a solid!

Exceptions – these do not act as expected -

Amorphous Solids

Liquid Crystal

s

AMORPHOUS SOLIDSLack tight ordered structure–No definite temperature for change from solid to liquid.

–Glass, ceramic & plastics

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

Properties of FluidsChapter 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 objectIf force = weight, object will…

FLOAT

If force is less than weight, object will…

SINK

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.

Density…D = m /

v

Objects will float if their density is less that the density of the fluid it is

placed inWhy 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.

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?

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?