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 Fixed Fixed
Volume Fixed Fixed Volume of
container
Flows? No Yes Yes
Shape Fixed Shape of container Shape of container
Compressible? No No yes
Expands? No No yes
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