1. Classification of Matter Properties of Matter
Unit 1 – Matter
Classification of Matter
Properties of Matter

2. Science: Man made pursuit to understand natural phenomena
Chemistry: The study of matter

3. Can it be physically separated?
A. 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

4. Pure Substances 1. Element composed of identical atoms
EX: copper wire, aluminum foil

5. Pure Substances 2. Compound
composed of 2 or more elements in a fixed ratio
properties differ from those of individual elements
EX: table salt (NaCl)

6. (suspensions & colloids)
Mixtures
Variable combination of 2 or more pure substances.
Heterogeneous
uneven distribution
(suspensions & colloids)
Homogeneous
even distribution
( solutions)

7. Mixtures 1. Solution homogeneous very small particles
no Tyndall effect
Tyndall Effect
particles don’t settle
EX: rubbing alcohol

8. Mixtures Not all solutions are liquid
Alloys – solids dissolved in solids
EX: 10 K gold = gold + copper brass = copper + zinc
Air – oxygen + other gases dissolved in nitrogen

9. Solutions Solute- substance that gets dissolved
Solvent- substance that does the dissolving
Saturated- holding max. amount of solute per volume at a given temp.
Supersaturated- holding more than the max. solute per volume after changing the conditions of the solvent (temp. or pressure)
Unsaturated- can hold more solute in a given amount of solvent

10. Mixtures 2. Colloid heterogeneous medium-sized particles
Tyndall effect
particles don’t settle
EX: milk

11. The Tyndall Effect
Colloids scatter light, making a beam visible. Solutions do not scatter light.
Which glass contains a colloid?
colloid
solution

12. Mixtures 3. Suspension heterogeneous large particles – can see
Tyndall effect
particles settle
(needs to be shaken)
EX: fresh-squeezed lemonade

13. Mixtures Examples: jello muddy water Fog saltwater
Italian salad dressing
colloid
suspension
solution

14. Mixtures vs. Compounds Components may be in any proportion
Individual components retain their own identities
Components may be separated physically
When mixture is formed there is little to no evidence of a reaction
Components are in fixed proportions
Individual components lose their identities, new set of properties result
Components may be separated only chemically
When compound is formed there is evidence of a reaction

15. Physical Separation Techniques
Difference in Densities (density column – some objects float in others)
Filtration (separate solids from liquids)
Magnetism
Chromatography
Distillation (separation by boiling points)
Evaporation (separate solids and liquids)

16. Separation of a Mixture
The constituents of the mixture retain their identity and may be separated by physical means.

17. Separation of a Mixture
The components of dyes such as ink may be separated by paper chromatography.

18. Separation of a Mixture
Distillation

19. Types of Properties Physical
Properties that describe the substance itself, rather than describing how it can change
Example: boiling point, color, size
Chemical
Properties that describe the substances ability to undergo changes that transform it into other substances
Example: charcoal has the ability to burn in air

20. Types of Physical Properties
depend on the amount of matter that is present.
Extensive properties
Volume
Mass
Energy Content (think Calories!)
do not depend on the amount of matter present.
Intensive properties
Melting point
Boiling point
Density

21. Changes in Matter Physical Change
Change in form or state of matter without altering chemical composition
Examples: slicing a banana, boiling water, dissolving sugar; *** phase changes are physical!
Chemical Change
Changing substance into new substance by reorganizing atoms…chemical bonds are made or broken
Examples: burning, rusting, copper turns green

22. 5 Indicators of a chemical change
Color Change
Light emitted (glow sticks, candle burning)
Temperature change (happens on its own – you don’t supply heat)
Precipitate forms (solid from 2 liquids)
Gas production (you see bubbles)

23. Three Phases

24. Solids Definite shape/definite volume
Molecules are tightly packed, but can still move slightly
Most Dense state of matter (because particles are the closest)

25. Liquids
Definite volume/no definite shape (takes the shape of its container)
Fluid – because it “flows”
Particles are not as close as solids, but are more dense than gases

26. Gases No definite shape or volume
Least dense of the 3 states of matter because the particles are far apart

27. Which state of matter are they?

28. Phase Differences
Solid – definite volume and shape; particles packed in fixed positions.
Liquid – definite volume but indefinite shape; particles close together but not in fixed positions
Gas – neither definite volume nor definite shape; particles are at great distances from one another

29. Phase Changes Freezing (liquid to solid) Melting (solid to liquid)
Vaporization (liquid to gas)
Condensation (gas to liquid)
Sublimation (solid to gas)
Deposition (gas to solid)
**** Phase changes are PHYSICAL changes!!!!