Chapter 16
Solids, Liquids, and Gases
Matter
Anything that has mass and takes
up space
4 States of matter
 Solid
 Liquid
 Gas
 Plasma
Each is designated by the energy, movement,
and behavior of the particles
Kinetic Theory
 An explanation of how particles in matter behave
1. All matter is composed of small particles (atoms,
molecules, and ions)
2. These particles are in constant, random motion
3. These particles are colliding with each other and the
sides of their container
Solid State
 Energy
 Very little energy
 Movement
 Vibrate against each other, but don’t move around much
 Particle Spacing
 Very little space between particles, packed closely together
 Volume/Shape
 Definite volume and definite shape
 Particles have a specific type of geometric arrangement that
they form in when cooled
 Determined by chemical and physical properties of solids
Liquid State
 Energy
 More Energy than solids
 Movement
 Flow around each other
 Particle Spacing
 Particles have space between them
 Volume/Shape
 Definite volume but NO definite shape
Gas State
 Energy
 Tons of Energy!
 Movement
 Flow around past each other
 Particle Spacing
 Particles are far apart
 Volume/Shape
 No definite volume and no definite shape
Plasma State
 Plasma – An electrically charged gas
 Created at very high temperatures (like
on the sun) (collisions between particles
result in the electrons being stripped
from the atom)
 Most common state of matter in the
universe (not Earth)
 Found on stars
 Found in lightning bolts, neon, fluorescent
light tubes
Diffusion
 Diffusion – the spreading of particles throughout a given
volume until they are uniformly distributed
 Occurs in solids and liquids, but most rapidly in gases
 Ex. Spray air freshener, dye in water
Changes in State
 ENERGY of the particles influences the state of
matter
 Temperature is something we can easily measure
instead of Energy
 Increased Energy
 Molecules move faster and spread out
 Temperature increases
 Decreased Energy
 Molecules move slower and are closer together
 Temperature decreases
Phase changes
 Due to changing in the
movement (Energy) of the
particles
 Solid to Liquid and Back
 Freezing Point
 Point at which liquid
becomes solid
 Melting Point
 Point at which solids
become liquid
Phase Changes
 Liquid to Gas and Back
 Boiling Point – Point at which liquid becomes gas
 AKA: vaporization
2 types of vaporization
 Evaporation – occurs at the liquid’s surface and even at a temp.
below the liquids boiling point
 Boiling – occurs through a liquid at a specific temperature
 Condensation – gas changes to liquid
 Ex: Mirror fogging up
Phase Changes
 Heat of fusion – The amount of energy required to
change a substance from the solid phase to the liquid
phase at its melting point
 Heat of vaporization – the amount of energy required
for the liquid at its boiling point to become a gas
Thermal Expansion
 An increase in the size of a substance when the
temperature is increased
 Kinetic Theory – particles move faster and separate as the
temperature rises -> causes expansion of the entire object
Water
 Exception to thermal expansion
 Have highly charged areas that affect the behavior
 b/c the molecules orient themselves according to charge,
empty spaces occur, so water expands when going from a
liquid to a solid