1. If there only about 100 types of elements in the world, why are there so many different kinds of matter?
matter of
Types

2. Can it be physically separated?
Matter Flowchart
MATTER
yes no
Can it be physically separated?
MIXTURE
PURE SUBSTANCE
Is the composition uniform? no
yes
Can it be chemically decomposed? no
yes
Homogeneous Mixture
(solution)
Heterogeneous Mixture
Compound
Element
Colloids
Suspensions

3. Solutions
I. The Nature of Solutions Make a list of as many different solutions as you can think of.

4. A. Definitions Solution - homogeneous mixture
Solute - substance being dissolved
Solvent - present in greater amount

5. A. Definitions
Solute - KMnO4
Solvent - H2O

6. B. Solvation First... Then... Solvation – the process of dissolving
solute particles are surrounded by solvent particles
First...
solute particles are separated and pulled into solution
Then...

7. B. Solvation Non- Electrolyte Weak Electrolyte Strong Electrolyte+
sugar - +
acetic acid - +
salt
Non-
Electrolyte
Weak
Electrolyte
Strong
Electrolyte
solute exists as
molecules only
solute exists as
ions and
molecules
solute exists as
ions only
DISSOCIATION
IONIZATION
View animation online.

8. NaCl(s)  Na+(aq) + Cl–(aq)
B. Solvation
Dissociation
separation of an ionic solid into aqueous ions
NaCl(s)  Na+(aq) + Cl–(aq)

9. HNO3(aq) + H2O(l)  H3O+(aq) + NO3–(aq)
B. Solvation
Ionization
breaking apart of some polar molecules into aqueous ions
HNO3(aq) + H2O(l)  H3O+(aq) + NO3–(aq)

10. B. Solvation
“Like Dissolves Like”
NONPOLAR
POLAR

11. B. Solvation Soap/Detergent polar “head” with long nonpolar “tail”
dissolves nonpolar grease in polar water

12. C. Solubility UNSATURATED SOLUTION more solute dissolves
no more solute dissolves
SUPERSATURATED SOLUTION
becomes unstable, crystals form
concentration

13. C. Solubility Solubility
maximum grams of solute that will dissolve in 100 g of solvent at a given temperature
varies with temp
based on a saturated solution

14. C. Solubility Solubility Curve
shows the dependence of solubility on temperature

15. C. Solubility Solids are more soluble at... high temperatures.
Gases are more soluble at...
low temperatures &
high pressures (Henry’s Law).
EX: nitrogen narcosis, the “bends,” soda

16. Quiz
1. In a solution the substance that is being dissolved is called the___ a) Solvent b) Emulsifier c) Solute d) Filtrate
2. An emulsion is always between___ a) Two solids b) A solid and liquid c) Two gases d) Two liquids
3. What is one property of a suspension that is different from that of a solution or a colloid? a) If left to rest, the particles of a suspension will settle out. b) The particles of a suspension reflect light. c) A suspension is always clear d) Suspensions are colorless

17. Quiz
4. A What is the size of particles in a solution? a) More than 10,000 Angstroms b) Between 10,000 and 100,000 Angstroms c) Between 10 and 10,000 Angstroms d) Molecule size
5. A solution that cannot hold any more solute at room temperature is ___ a) A weak solution b) A concentrated solution c) A saturated solution d) A supersaturated solution

18. Quiz
6. An example of a colloid which is an emulsion is ___ a) Whipped cream b) Mayonnaise c) Fog d) Gelatin
7. An example of a solution is ___ a) Sugar and water b) Sand and water c) Milk d) Whipped Cream
8. Oil floats on water. The most accurate reason for this is a) oil is less dense than water b) oil is immiscible (does not dissolve) in water c) oil is both less dense and immiscible with water d) water is heavier than oil

19. Quiz
9. The best method to separate the solute from the solvent in a solution would be ___ a) Distillation b) Filtration c) Sedimentation d) all of the above will work
10. What makes water such a good solvent? a) Water is a good solvent because it is a
negatively charged ion. b) Water is such a good solvent because it repels most molecules b) Water is such a good solvent because it is such a small molecule d) Water is a good solvent due to its polarity and small molecular size