Transcript Solids, Liquids and Gases
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