1. I. Matter
Matter is anything that has mass and takes up space. (Mass is the measurement you make using a balance.)

2. A. States of Matter A solid has definite volume and definite shape.
A liquid has definite volume but
indefinite shape. It assumes the shape
of its container.
A vapor or gas has neither definite
volume nor definite shape. It assumes
both the volume and shape of its
container.

3. B. Changes of State
1. melting : solid changing to liquid 2. vaporization : liquid changing to vapor 3. condensation : vapor changing to liquid 4. freezing : liquid changing to solid 5. sublimation : solid changing directly to vapor without going through liquid phase 6. deposition : vapor changing directly to solid without going through liquid phase
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4. II. Classification of Matter Matter can be classified into two categories: pure substances and mixtures.

5. Pure Substances
A pure substance has a uniform,
unchanging composition. Every
sample of a pure substance has
exactly the same characteristic
properties and composition.
Pure substances exist as either
elements or compounds.

6. Elements are found on the periodic table
Elements are found on the periodic table. An element cannot be separated into simpler substances by physical or
chemical means.
2. Compounds are combinations of two or more different elements that are chemically bonded.
3. A chemical change is required to combine elements into compounds and to separate compounds back into elements.

7. B. Mixtures
A mixture is a combination of two or more pure substances in which each pure substance retains its individual chemical properties.

8. 1. A physical change is required to combine pure substances into mixtures and to separate mixtures back into pure substances. 2. Homogeneous mixtures or solutions are uniform in appearance. 3. Heterogeneous mixtures are not uniform in appearance. Individual substances remain distinct and are not blended smoothly throughout.

9. In summary

10. PRACTICE: Classify the following list into elements, compounds, homogeneous mixtures and heterogeneous mixtures.
Air
aluminum
baking soda
blood
chicken soup
chlorine
dirt
homogeneous (N2 and O2)
element (Al)
compound (NaHCO3)
Heterogeneous
element (Cl2)

11. III. Properties A property is a characteristic that distinguishes a substance.

12. Some examples of properties include:
Boiling point Color Density Flammability Ability to react with acid Mass Ability to rust Length Ability to react with a base volume Ability to react with water Ability to tarnish Ability to conduct electricity
These properties can be described as either physical or chemical properties.

13. Physical properties describe the substance itself.
A. Physical Properties
Physical properties describe the
substance itself.
They can be observed or measured
without altering the chemical identity
of the substance.

14. Example 1 Write only the physical properties given in the list above.
boiling point
Color
ability to conduct electricity
density
Length
mass
volume
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15. Physical properties are further broken down into either
extensive or intensive properties.
1. Extensive properties depend on the amount of matter present. These properties vary with the amount of substance present and therefore cannot be used to uniquely identify a substance.

16. Example 2 Write only the extensive physical properties given in the list above.
area
length
mass
volume

17. 2. Intensive properties do not depend on the amount of matter present
2. Intensive properties do not depend on the amount of matter present. These properties stay the same regardless of the amount of substance present and therefore are frequently used to uniquely identify a substance.

18. Example 3: Write only the intensive physical properties given in the list above.
boiling point
color
ability to conduct electricity
density

19. B. Chemical Properties
Chemical properties describe the ability of a substance to undergo changes that transform it into different substances.

20. Example 4: Write only the chemical
properties given in the list above.
flammability
ability to react with acid
ability to react with base
ability to react with water
ability to rust
ability to tarnish

21. Example 5: Read the following passage and answer the questions:
Consider the following properties (underlined) for the metal sodium.
Sodium is a (1)soft, (2)silvery-colored metal with a (3)density of 0.97 g/cm3. When a (4)2 gram sample of sodium metal is ignited, it (5)burns with a yellow flame. It (6)reacts vigorously with chlorine gas to form the salt sodium chloride. Sodium (7)melts at 97.7º C and boils at (8)883º C.

22. Which are physical properties?
1, 2, 3, 4, 7, 8
Which are extensive physical properties? 4
Which are intensive physical properties?
1, 2, 3, 7, 8
Which are chemical properties?
5, 6

23. Some examples of changes include: Bending boiling Burning condensing
Corroding cutting
Depositing dissolving
Exploding freezing
Grinding melting
Reacting rotting
Rusting subliming
Tarnishing vaporizing
These changes can be described as either physical or chemical changes.

24. A. Physical Changes
Physical changes do not
change the identity of the substance. Changes of state are all physical changes. Most physical changes are reversible.

25. Example 6: Write only the physical changes given in the list above.
Bending boiling
Condensing cutting
Depositing dissolving
Freezing grinding
Melting subliming
vaporizing
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26. B. Chemical Changes
Chemical changes transform one or more substances into different substances.

27. Example 7: Write only the chemical changes given in the list above.
burning
corroding
exploding
reacting
rotting
rusting
tarnishing

28. 1. Evidence of chemical change
change in energy (light, heat)
a gas is produced
color change
a solid (precipitate) is produced