Solids, Liquids and Gases

Chapter 16

Section 1 – Kinetic Theory

1.

States of matter you saw at lunch?

Kinetic Theory

– explanation of how particles in matter behave All matter is composed of small particles (atoms, molecules, ions)

Kinetic Theory

2.

3.

Particles in constant, random motion Particles are colliding Energy that particles lose from collisions is negligible

Average Kinetic Energy

Temperature is measure of

average kinetic energy

.

Warmer – particles have MORE energy  Move

faster

Cooler – particles have LESS energy  Move

slower

Solid State – H 2 O

Particles in fixed position

Liquid State

Particles in solid gain energy and move faster  break out of fixed position

Melting point:

temperature where solid begins to liquefy

Heat of fusion:

amount of energy needed to change a solid to liquid

Liquids Flow

Particles have energy to break

SOME

attraction and flow

Gas State

Particles have energy to escape

ALL

attraction

Vaporization

Liquid particles gain enough energy to escape to gas phase

Evaporation:

vaporization at the surface of liquid, spontaneously

Boiling point:

applying heat, temperature at which pressure of vapor is equal to external pressure, liquid to gas

Heat of vaporization:

amount of energy needed for liquid to be a gas

Gases fill their Container Diffusion:

spreading of particles throughout until they are mixed

Heating Curve of a Liquid

Heating Curve of a Liquid a

and

c

– increasing in energy

b

and

d

– energy used to break attraction between particles

Plasma Def:

consists of positive and negative particles Very HIGH temperature Particles moving so fast  e stripped off are Lightning, sun, neon lights

Thermal Expansion

Thermal Expansion

Spaces are expansion joints Prevent cracks Absorbs heat – expands Cools – shrinks

Expansion of Matter Thermal Expansion:

increase in the size of a substance when the temperature is increased Warmer = less attraction b/ particles = move freer Cooler = more attraction = closer together

Expansion of Matter

Expansion of Matter

Strange Water

Ice is

less

dense than liquid water (+) and (-) ends arrange themselves next to each other Create empty spaces

Strange Water

Solid or Liquid?

Amorphous Solids:

“without” form, change to liquid over

range

of temperatures Ex: glass, plastic Liquid turned to solid too quickly

Solid or Liquid Liquid crystals:

change to liquid but don’t lose their ordered form Ex: liquid crystal display (LCD)  calculators, etc.

Properties of Fluids

Section 2

How do ships float?

Buoyancy:

ability of fluid to exert

upward force

on object.

If force equal to weight = float

Archimedes’ Principle Def:

buoyant force on an object is equal to the

weight of the fluid displaced

by the object

Density

Same size blocks - wood and steel Displace same amount of water BUT, wood block floats and steel block sinks Different densities – object has less density than density of fluid to float

Archimedes’ Principle

Pascal’s Principle Pressure

: force exerted per unit area Pressure applied to fluid is exerted throughout the fluid Used in hydraulic lifts – use your weight to lift something much heavier

Bernoulli’s Principle Def:

as velocity of fluid

increases

pressure of fluid

decreases



Fluid Flow Viscosity:

the resistance of a fluid to flow Syrup – high viscosity Water – low viscosity

Behavior of Gases

Section 3

Pressure

Result of gas particle collisions with the container More collisions = More pressure Pressure unit =

Pascal (Pa)

How do we get

high

pressure?

Boyle’s Law

Relationship between pressure and volume  volume, size of container, what will pressure do?

 Pressure  Inversely related: as one goes  other goes  , or vice versa the

Charles’s Law

Relationship between volume and temperature “Keep away from heat” on pressurized can  temperature what will volume do?

  volume Directly related: as one goes  goes  , or vice versa the other

Kelvin Scale

All (+) numbers 0K =

absolute zero

– all particle motion stops 0K = -273 o C K = o C + 273