1. Matter – Properties & Changes
Mr. Stripling
Pre – AP Chemistry
Room 402

2. States of Matter
The physical forms of matter, either solid, liquid, or gas, are called the states of matter.
Solids are a form of matter that have their own definite shape and volume.
Liquids are a form of matter that have a definite volume but take the shape of the container.

3. States of Matter True or False A liquid conforms to it container.
A solid has definite shape but changeable volume.

4. States of Matter
Gases have no definite shape or volume. They expand to fill their container.
Vapor refers to the gaseous state of a substance that is a solid or liquid at room temperature.

5. Physical Properties of Matter
A physical property is a characteristic that can be observed or measured without changing the sample’s composition.

6. Physical Properties of Matter
Extensive properties are dependent on the amount of substance present.
Intensive properties are dependent on the what the substance is, not how much there is.
Name examples of both

7. Physical Properties of Matter
Extensive properties, such as mass, length, volume, and shape are dependent on the amount of substance present.
Intensive properties, such as smell, taste, melting point, boiling point, luster, density, and temperature, are dependent on the what the substance is, not how much there is.

8. Chemical Properties of Matter
The ability of a substance to combine with or change into one or more other substances is called a chemical property. Examples include:
Iron forming rust
Copper turning green in the air

9. Observing Properties of Matter
A substance can change form—an important concept in chemistry.
Both physical and chemical properties can change with specific environmental conditions, such as temperature and pressure.

10. Section 1 Review
Classify each of the following as a physical (A) or a chemical (B) property:
1. Iron and oxygen form rust
2. Iron is more dense than aluminum
3. Magnesium burns brightly when ignited
4. Oil and water do not mix
5. Mercury melts at -39oC

11. Physical Changes
A change that alters the substance without changing its composition
Phase change – transition of matter from one state to another
Water cycle

12. Physical Changes crushing a can melting an ice cube boiling water
mixing sand and water
breaking a glass
dissolving sugar and water
shredding paper
chopping wood
mixing red and green marbles
sublimating dry ice

13. Chemical Changes
Involves one or more substances changing into new substances
Terms that generally refer to chemical reactions include: decompose, explode, rust, oxidize, corrode, tarnish, ferment, burn, rot

14. Chemical Changes Change of odor.
Change of color (for example, silver to reddish-brown when iron rusts).
Change in temperature or energy, such as the production (exothermic) or loss (endothermic) of heat.
Change of composition - paper turning to ash when burned.
Light and/or heat given off.
Formation of gases, often appearing as bubbles in liquids.
Formation of a precipitate (insoluble particles).
The decomposition of organic matter (for example, rotting food).
The change is difficult or impossible to reverse.

15. Conservation of Mass
Mass is neither created nor destroyed during a chemical reaction – it is conserved.
Mass of reactants = mass of products

16. Conservation of Mass

17. Section 2 Review
On page do problems 5-8, 10 (a-c), and 13(a & b)
On page 94 do problems 50-55
Show work where appropriate or receive no credit