1. Chapter 2 Matter and Change
Charles Page High School
Dr. Stephen L. Cotton

2. Section 2.1 Matter OBJECTIVES:
Identify the characteristics of matter and substances.

3. Section 2.1 Matter OBJECTIVES:
Differentiate among the three states of matter.

4. Section 2.1 Matter OBJECTIVES:
Define physical property, and list several common physical properties of substances.

5. What is Matter? Matter is anything that takes up space and has mass.
Mass- amount of material or “stuff” in an object
Weight is due to gravity, and changes from location to location; mass is always constant.

6. Types of Matter
Substance- a particular kind of matter - pure; is uniform (all the same) and has a definite composition (examples are elements & compounds)
water; gold; lemonade?
Mixture- more than one kind of matter; has a variable composition

7. Properties Words that describe matter (adjectives)
Physical Properties- a property that can be observed and measured without changing the composition.
Examples- color, hardness, m.p., b.p.
Chemical Properties- a property that can only be observed by changing the composition of the material.

8. States of matter
Solid- matter that can not flow (definite shape) and has definite volume.
Liquid- definite volume but takes the shape of its container (flows).
Gas- a substance without definite volume or shape and can flow.
Vapor- a substance that is currently a gas, but normally is a liquid or solid at room temperature. (water vapor?)

9. States of Matter Definite Volume? Definite Shape? Temp. increase
Com-pressible?
Small Expans.
Solid
YES
YES NO
Small Expans.
Liquid NO NO
YES
Large Expans.
Gas NO NO
YES

10. Condense
Freeze
Melt
Evaporate
Solid
Liquid
Gas

11. Physical Changes
A change that changes appearances, without changing the composition.
Ex. Boil, melt, cut, bend, split, crack
Boiled water is still water.
Chemical changes - a change where a new form of matter is formed.
Ex. Rust, burn, decompose, ferment

12. Section 2.2 Mixtures OBJECTIVES:
Categorize a sample of matter as a substance or a mixture.

13. Section 2.2 Mixtures OBJECTIVES:
Distinguish between homogeneous and heterogeneous samples of matter.

14. Mixtures
Physical blend of at least two substances; variable composition
Heterogeneous- mixture is not uniform in composition
Chocolate chip cookie, gravel, soil.
Homogeneous- same composition throughout; called “solutions”
Kool-aid, air, salt water
Every part keeps it’s own properties.

15. Solutions Homogeneous mixture Mixed molecule by molecule
Can occur between any state of matter
Table 2.3, page 33
gas in gas; liquid in gas; gas in liquid; solid in liquid; solid in solid (alloys), etc.

16. Solutions
Like all mixtures, they keep the properties of the components.
Some can be separated easily by physical means: rocks and marbles, iron filings and sulfur
Other methods: distillation- takes advantage of different boiling points

17. Section 2.3 Elements and Compounds
OBJECTIVES:
Explain the differences between an element and a compound.

18. Section 2.3 Elements and Compounds
OBJECTIVES:
Identify the chemical symbols of common elements, and name common elements given their symbols.

19. Substances Elements- simplest kind of matter
cannot be broken down any simpler
all one kind of atom.
Compounds are substances that can be broken down only by chemical methods
When broken down, the pieces have completely different properties than the original compound.
Made of two or more atoms, chemically combined (not physical blend!)

20. Compound or Mixture Compound Mixture Made of one kind of material
Made of more than
one kind of material
Made by a
chemical change
physical change
Definite
composition
Variable

21. Which is it?
Compound
Mixture
Element

22. Chemical Symbols & Formulas
Currently, there are 115 elements
Each has a 1 or two letter symbol
First letter always capitalized; the second never; chemical “shorthand”
Don’t need to memorize all of them; know Table A.3 inside back cover
Some from Latin or other languages; note Table 2.4, page 40

23. Section 2.4 Chemical Reactions
OBJECTIVES:
Differentiate between physical and chemical changes in matter.

24. Section 2.4 Chemical Reactions
OBJECTIVES:
Apply the Law of Conservation of Mass.

25. Chemical Reactions
When one or more substances are changed into new substances.
Reactants- stuff you start with
Products- What you make
ability to undergo chemical reaction is called a chemical property
products have NEW PROPERTIES
Arrow from reactants to products

26. Indications of a chemical reaction:
Energy absorbed or released (temperature changes hotter or colder)
Color change
Gas production (bubbling, fizzing, or odor change)
formation of a precipitate- a solid that separates from solution (won’t dissolve)
Irreversibility- not easily reversed

27. Law of Conservation of Mass
Mass can not be created or destroyed in ordinary (not nuclear) chemical reactions or physical change
All the mass can be accounted for.
Burning of wood results in products that appear to have less mass as ash; where is the rest?