1. MATTER
What it is all about

2. Chemistry – Matter Unit
What is matter?
What is the organization of matter?
What is the nature of matter?

3. MATTER Mixtures Pure Substances Heterogeneous Homogeneous
Can the matter be separated by physical means?
Mixtures
Pure Substances
Constant composition
Separation by chemical means
Heterogeneous
Homogeneous
Compounds
Elements

4. The particle theory of matter.
Matter is anything that occupies space and has mass.
The particle theory of matter.
The particle theory states that…
all matter is made from particles
different particles have different properties
particles are constantly in motion

5. States of Matter
A solid has a definite shape and volume.
A liquid has a definite volume but no definite shape.
A gas has neither a definite volume or shape.
Gas
Liquid
Solid

6. SOLIDS
the attraction between particles is strong so the matter holds its shape. The particles are still moving, but they are not able to slide past each other
LIQUIDS
the attractive forces are not as strong. The particles are able to move past each other and slide around
GAS
the attraction between particles is so weak that they fly in every direction filling the container that they are held

7. Phases Changes of Matter
sublimation
vaporization
sublimation
condensation
Phase changes
solidification (freezing)
melting

8. Ex. oxidation, flammability, corrosiveness, pH, reactivity
Properties of Matter
Physical Properties:
a quality of a substance that can be observed or measured without changing the substance’s chemical composition
Examples: color, texture, boiling point, density, mass etc…
Chemical properties
Properties that do change the chemical nature of matter
Properties the matter exhibits when chemical change occurs
Ex. oxidation, flammability, corrosiveness, pH, reactivity

9. Physical Properties Subcategories
Extensive Properties depend upon the amount of matter that is present.
Ex. Length, mass, volume, heat …etc
Intensive Properties do not depend on the amount of matter present. These properties are the same for a given substance regardless of how much of the substance is present.
Ex. Color, density, melting point, ductility, temp… etc

10. Examples of physical properties
Boiling point
Specific gravity (at constant temperature)
Surface tension
Viscosity (at constant pressure and temp.)
Freezing point
Solubility in water (hot/cold)
Density
Melting point
Mass
Volume
Specific heat capacity
Heat
Temperature

11. Density the mass of a substance per a specific amount of volume
Density = mass
volume
The mass and volume are directly proportional. If one increases the other increases
mass
volume

12. Physical and chemical change
Physical change
the altering of the physical form but not composition of matter
ex. Pounding, pulling, changes of state
Knowledge of physical change leads to…
the understanding of separation of mixtures
ex. Distillation, crystallization, chromatography, filtration

13. Chemical change Chemical change
change in which the matter is converted into matter with different composition and properties

14. Indicators of chemical change
heat and/or light energy
Energy changes within the system
Production of gas
- release of gas from the system

15. 3. Formation of a precipitate
- when two (or more) solutions are put together an insoluble solid is produced
4. Color change
- the system changes color
- not always an indicator of chemical change (can be physical

16. MATTER Mixtures Pure Substances Heterogeneous Homogeneous
Can the matter be separated by physical means?
Mixtures
Pure Substances
Constant composition
Separation by chemical means
Heterogeneous
Homogeneous
Compounds
Elements

17. MIXTURES
mixture:
- combination of two or more kinds of matter each of which retains its own composition and properties
- physical blend of two or more substances

18. More of Mixtures: heterogeneous mixture: Phase
- a mixture containing substances that are not evenly distributed
- different from point to point
ex. granite ---> quartz, feldspar, and mica
Phase
mixtures that are obviously heterogeneous and have separate, distinct parts
Ex. Oil forming layers in water is another
Interface – the region where two or more phases meet

19. M o M homogeneous mixture
- a mixture containing substances that are uniformly distributed with the particles blended completely
- composition and properties are uniform throughout
- also called solutions (mixed on a scale of individual particles) ex. I molar copper II sulfate
To the eye, the mixture appears to be pure substance.

20. Solutions (Homogeneous Mixtures)
Can you tell the difference?
To play the movies and simulations included, view the presentation in Slide Show Mode.

21. Parts of a Solution
SOLUTE – the part of a solution that is being dissolved (usually the lesser amount)
SOLVENT – the part of a solution that dissolves the solute (usually the greater amount)
Solute + Solvent = Solution
Solute
Solvent
Example
solid
Brass: Copper and Zinc
liquid
Seawater: NaCL in water
gas
Moth balls: naphthalene
Ethyl alcohol and water (miscible)
SODA: CO2 gas in water
AIR: O2 gas, N2 gas

22. Definitions Solutions can be classified as saturated or unsaturated.
A saturated solution contains the maximum quantity of solute that dissolves at that temperature.
An unsaturated solution contains less than the maximum amount of solute that can dissolve at a particular temperature

23. Definitions
SUPERSATURATED SOLUTIONS contain more solute than is possible to be dissolved in a given amount of solvent
Supersaturated solutions are unstable.
-- the supersaturation is only temporary
-- need to warm the solvent so that it will dissolve more
-- then need to cool the solution slowly

25. Somewhere In Between
Some mixtures are in-between heterogeneous mixtures and homogeneous solutions.
suspension
has clumps that stay floating
filtering a suspension will usually separate the particles.
colloid
has very small clumps that almost make a solution
the clumps are so small that they pass through most filters
milk is an example of a colloid.
emulsion
the clumps of particles are held with an emulsifying agent.
mayonnaise as an example

26. Define the following words
solubility.
Miscible
Immiscible

27. Separation of Mixtures types of…
Filtration
Separation of mixture on the basis of differences in the size of the particles
Mostly used to separate solids from liquids (but filtration is used to separate all phases of matter from one another)
Ex. Air filters separate gas (air) from solid (dirt particles)

28. Distillation
Based on the tendency of a substance to vaporize (turn to a gas)
Based on boiling point differences
The substance in the mixture with the lowest boiling point will vaporize first from the mixture
Ex. Crude oil 

29. Chromatography Based on the differences in solubility
Two types  Gas and Paper
Mixture separates as it travels (most soluble separates first)
Solute – substance that gets dissolved
Solvent – substance that does the dissolving
Ex. Separating ink in a marker

30. Crystallization
Separation of the mixture is based on solubility differences
Temperature changes within the mixtures change solubility of parts of the mixture
Solubility – the amount of a solute that is able to dissolve in a given amount of solvent
Ex. Rock candy

31. SOLUTION CHEMISTRY Concentration:
amount of solute in a given amount of solvent (can be determined quantitatively)
Dilute:
a solution with a small amount of solute per solvent amount (relative term)
Concentrated:
a solution with a large amount of solute per solvent amount (relative term)
BOTH DILUTE AND CONCENTRATED ARE QUALITATIVE

32. Concentration of Solute
The amount of solute in a solution is given by its concentration.
Molarity ( M ) =
moles solute
liters of solution
The concentration of a solution is said to be its molarity.
Ex. 1 M CuSO4
“1 molar copper II sulfate