Chapter 11 Study Guide
FALCON SCIENCE
LESSON 1
1. Pure Substance-a single kind of matter with a specific
make up or composition.
2. Mixture- is 2 or more substances that are together
physically but not chemically.
3. Substances = 1 of the same kind
 Mixture
= more than 1 kind together
4. Elements-a substance cannot be broken down into
any other substances by chemical or physical means
5. Compounds-a substance made of 2 or more elements
chemically combined.
6. 2 types are Homogeneous, Heterogeneous
7. Example of Heterogeneous=
8. Example of Homogeneous=
9. Mixtures are easy to separate, because they are NOT
chemically combined.
10 1. Distillation, 2. Filtration, 3. Evaporation, 4. Magnet
Lesson 2
1. Mixtures are classified by Solution, Colloid, or
Suspension.
2. Solution – mixture containing a solvent & at least 1
solute.
3. Solvent- is the part of the solution usually present in
the largest amount. (water, liquid, etc.)
4. Solute – the substance dissolved by the solvent.
5. Universal solvent is water….
6. Air (O2 and other gases), teeth filling (silver in
mercury)
7. Examples of Colloids
8. Example of Suspension
 "In chemistry, a suspension is a heterogenous fluid
containing solid particles that are sufficiently large for
sedimentation. "
Mud or muddy water, is where soil, clay, or silt
particles are suspended in water.
Flour suspended water
Paint
Chalk powder suspended in water.
Dust particles suspended in air.
juice w/ pulp
italian dressing
sea salt in the air from crashing ocean waves
clouds, fog
9. A solution forms when particles of the solute
separate from each other and become surrounded by
particles of the solvent (the greater amount).
10. Salt has an Ionic bond (not holding hands) it’s more
an attraction, so they can be separated and be attracted
to other ions in the water.
Sugar has a Covalent bond remains unbroken even if
there is a polar attraction.
11. Solutes raise the boiling point above the solvent’s
normal point – Solutes lower the freezing point of a
solution below that of the solvent.
Lesson 3
1. Dilute solution – a mixture with only a little solute
dissolved.
2. Concentrated solution –a mixture that has a lot of
solute dissolved in the solvent.
3. Solubility-the measure of how much solute can
dissolve in a solvent at a given temperature.
4. Factors Affecting Solubility- 1. pressure, 2.solvents
used, 3. Temperature
5. Saturated solution – when you’ve added so much
solute that no more dissolves
6. How Pressure Affects Solubility
Pressure has a negative affect on solubility. The
higher the air pressure, the lower the solubility. This is
because pressure causes the molecules of the liquid to
be forced closer together which decreases the solubility
of gases in the liquid.
7. How Other Solvents Affect Solubility
Solubility of a solute in a solvent purely
depends on the nature of both solute and solvent.
A polar solute dissolved in polar solvent.
Solubility of a non-polar solute in a solvent is large.
A polar solute has low solubility or insoluble in a nonpolar solvent.
8. How Temperature Affects Solubility
Solubility generally increases with increase
temperature, however gases are more soluble in cold
solvent than in hot.