1. Matter and Change

2. B. Physical Properties
1. can be observed without changing the chemical composition
2. Examples
Color
Melting point
Density
Hardness
Malleability

3. C. Chemical Properties
1. determined by how a chemical reacts (or doesn’t) with another chemical
2. Examples –
Rusts
Reacts with HCl
Reacts with water

4. Physical or Chemical Property?
7) Water boils at 100°C.
8) Zinc reacts with hydrochloric acid.
9) Sodium chloride dissolves in water.
10) Aluminum is shiny silver in color.
11) Copper is ductile.
12) Calcium reacts with water.
13) The density of aluminum is 2.7 g / mL.

5. D. States of Matter Solids a) definite mass? b) definite volume?
c) definite shape?
d) compressible?
e) able to flow?

6. D. States of Matter Liquids a) definite mass? b) definite volume?
c) definite shape?
d) can be compressed?
e) flows?

7. D. States of Matter Gases a) definite mass? b) definite volume?
c) definite shape?
d) can be compressed?
e) flows?

8. D. States of Matter 1) summary chart
Property
Solid
Liquid
Gas
Mass
Fixed
Volume
Volume of container
Flows? No
Yes
Shape
Shape of container
Compressible?
yes
Expands?

9. D. States of Matter 2) Vapors
a) = substances in the gaseous state which are usually in the liquid or solid state at room temperature
b) ex. – gasoline fumes, moth ball odors, steam, “fog” from dry ice

10. E. Classification of Matter
1. Substances
= definite or fixed composition
can write a chemical formula for it
pure

11. E. Classification of Matter
1. Substances
a) Elements
Listed on periodic table
Mg, Ne, Cl, C, etc.

12. E. Classification of Matter
1. Substances
b) Compounds
Contain two or more elements in fixed ratio
Ex. – NaCl, CO, H2O

13. E. Classification of Matter
2. Mixtures
= composition is NOT fixed or definite; it varies
Cannot write a formula for it

14. E. Classification of Matter
2. Mixtures
a) homogeneous mixtures
*uniform (same throughout)
*one phase
*also called solutions
(but can be s, l or g)
*ex. – saline solution, tap water, brass, hot tea, air

15. E. Classification of Matter
2. Mixtures
b) heterogeneous mixtures
*not uniform
*two or more phases
*ex. – soil, fresh-squeezed orange juice, sand and water

16. F. How to separate parts of a mixture?
1. Magnetism

17. F. How to separate parts of a mixture?
2. Filtration

18. F. How to separate parts of a mixture?
3. Density

19. F. How to separate parts of a mixture?
4. Distillation
(different boiling points)

20. F. How to separate parts of a mixture?
5. Chromatography
(ex. – paper + ink)

21. G. Changes 1. Physical Changes
a) chemical composition of material does NOT change
b) may be reversible
c) examples
Tearing paper
Boiling water
Crushing salt
Crumpling foil

22. G. Changes 2. Chemical changes a) change in chemical composition
b) examples
Iron rusting
Zinc + hydrochloric acid
Digestion of food
Burning wood
Lithium + water

23. H. Clues for a chemical change (reaction)
1. formation of bubbles (gas)
Ex. – metal + acid

24. H. Clues for a chemical change (reaction)
2. formation of precipitate (insoluble powder)

25. H. Clues for a chemical change (reaction)
3. release or absorption of energy (heat or light)
Ex. – burning of wood

26. H. Clues for a chemical change (reaction)
4. change in color
Ex. – meat changes color when cooked
Ex. – changing in color of leaves in fall

27. H. Clues for a chemical change (reaction)
5. change in pH (acidity level)

28. I. Sometimes the “clues” indicate a physical change!
1. color change could be dilution (ex. – add water to Kool-Aid)
2. bubbles could be boiling liquid
3. heat absorbed during a change in state (ex. - melting ice)

29. J. Law of conservation of mass
1. Mass cannot be created or destroyed in a chemical reaction or physical change