Liquids
 Definite volume
 Fluidity – able to flow
 Relative high density
 Relative incompressibility
 Dissolving ability
 Ability to diffuse
 Tendency to evaporate and boil
 Tendency to solidify
Solids
 2 types of solids
 Crystalline solid (crystal)

Arranged in an orderly, repeating pattern
 Amorphous solid (without form)

Arranged randomly – no pattern
Properties of solids
 Definite shape
 Definite volume
 Nonfluidity
 Definite melting point
 High density
 Incompressibility
Crystalline solids
 The total 3-dimensional array of points that describe
the arrangement of particles in a crystal is called a
crystal lattice.
1 repeating piece is a unit cell
Phase Diagram
(Freezing
Points)
Pressure (atm)
Liquid
1
(Boiling Points)
Solid
.
Gas
(Triple Point)
0
100
Temperature (oC)
Mixtures
 3 Types of mixtures
 1. Solution
 Soluble – will dissolve
 Forms a homogeneous mixture
 Very small particles
 2 Parts of a solution
 Solute – stuff that dissolves
 Solvent – stuff that the solute dissolves in
Types of solutions
Solute
Solvent
Example
Gas
Gas
Air
Gas
Liquid
Soda Water
Gas
Solid
-
Liquid
Gas
Humidity
Liquid
Liquid
Juice in water
Liquid
Solid
-
Solid
Gas
Sulfur in air
Solid
Liquid
Kool Aid
Solid
Solid
Alloy (Brass)
 2. Suspensions
 Heterogeneous mixture that settles
 Large particles
 Muddy water, italian salad dressing

(anything that must be shaken)
 3. Colloids
 Intermediate sized particles
 Particles disperse

2 parts of a colloid
 Tyndall Effect

Seeing a beam of light
 (separates colloid from solution)
Examples of Colloids
 Colloid
Phase
 Gel
solid dispersed in liquid
 Liquid emulsion
liquid dispersed in liquid
 Foam
gas dispersed in liquid
 Smoke
solid dispersed in gas
 Fog
liquid dispersed in gas
 Smog
solid & liquid dispersed in gas
3 types of mixtures
 Solutions
 Colloids
 Homogeneous  Homogeneous
 Intermediate
 Very small
sized
particles
 Does not
 Does not
separate
separate
 Tyndall effect
 No light
scattering
 Suspensions
 Heterogeneous
 Large particles
 Separates
 No Tyndall
effect
The solution process
 Increasing the Rate of dissolving
 1. Increase the surface area of solute
 2. Agitating the solution
 3. Heating the solvent
Types of solutions
 Electrolyte
 A solution that has ions in it and can conduct electricity
 Saturated solution
 Contains the maximum amount of solute
 Unsaturated solution
 Contains less than the maximum amount of solute
 Supersaturated solution
 Contains more than the maximum amount of solute

(Rock candy, crystals)
Factors affecting solubility
 1.
Types of solvents and solutes
 Like dissolves like



Refers to polarity
 Water is a polar molecule
 Oil is a nonpolar molecule
If they are the same polarity, the compounds are miscible
(mixable) - salt in water, vinegar in water
If they are not soluble, they are immiscible (not mixable) - oil
in water, salt in oil
 2.
Pressure
 Under pressure a gas will enter and dissolve in a liquid

fizz in a bottle of pop
 If pressure is released, the liquid can’t hold as much gas

 3.
Effervescence
Temperature
 Warmer liquids hold less gas

Burp more from warm pop