1. Section 2.1 Matter Objectives
Identify the characteristics of matter and substances
Differentiate among the three states of matter
Define physical property and list several common physical properties of substances

2. Properties of Matter Matter
anything that has _____________________________________
Mass
The amount of ______________________________________.
Note ______________________________________________.
Substance
_______________________________contain only one kind of matter.

3. Physical Properties
Physical Property – a quality or condition of a substance that
Examples of physical properties are

4. Properties of Solids, Liquids, Gases
Has a definite ________________________
Does not depend on the shape of its container
Almost incompressible
Liquid
Particles are in close contact but not rigidly packed
Can flow and _______________________________
__________________________________________

5. Properties of Solids, Liquids, Gases
_________________________
“Gas” is limited to those substances who are in a gaseous state at room temperature.
“Vapor” describes the gaseous state of a substance that is a liquid or a solid at room temperature.

6. Physical Changes
A change which alters a given material without changing its composition is called a
Examples are
Melting a metal, melting ice, boiling water

7. Section 2.2 - Mixtures Objectives
Categorize a sample of matter as a substance or a mixture
Distinguish between homogeneous and heterogeneous samples of matter

8. Classifying Mixtures
A mixture is a physical blend of two or more substances.
Salad with lettuce, tomatoes, carrots
Blood – with water, cells, chemicals
Each of these mixtures can vary in composition
____________________________________ – if you were to sample the mixture in two different places the composition wouldn’t be the same (salad)
____________________________________– if you were to sample the mixtures in two different places, the composition would be the same (salt water)

9. Phases in Mixtures
System
Examples
Carbon dioxide and oxygen in nitrogen (air)
Water vapor in air (moist air)
Carbon dioxide in water (soda water)
Acetic acid in water (vinegar)
Sodium chloride in water (salt water or brine)
Copper in silver (sterling silver, an alloy)
Phase – any part of a system with uniform composition and properties is a phase.
Homogeneous mixtures are one phase.

10. Separating Mixtures __________________________________________________
Magnet to separate iron filings from sulfur.
Distillation can be used to separate pure water from impurities.

11. Section 2.3 – Elements and Compounds
Objectives
Explain the difference between an element and a compound.
Identify the chemical symbols of common elements, and name common elements given their symbols

12. Elements vs. Compounds
_______________________ are the simplest forms of matter that can exist under normal laboratory conditions.
Elements cannot be separated into simpler substances by
Examples:
_______________________ are made when two or more elements combine chemically, like H2O or CO2 .
Compounds can be separated into simpler substances by

13. Chemical Symbols Some chemical symbols are easy to remember
Others are not so easy, and come from Latin or other sources

14. Section 2.4 – Chemical Reactions
Objectives
Differentiate between physical and chemical changes in matter
Apply the law of conservation of mass

15. Changing reactants to products
_________________________________- one or more substances react and change into a new substance
Example:
The starting substances are called
The ending substances are called
Words that convey that a chemical change has occurred include:

16. Chemical Properties
Chemical properties tell you something about the ability of a substance to undergo a chemical reaction to form new substances
____________________ is a chemical property of iron
____________________ is a chemical property of waste organic material
____________________ is a chemical property of wood

17. Chemical reactions How can you tell if a reaction has taken place?
Energy is always ____________________________ ____________________________during a reaction
Change in _________________________________
silver chromate forms when yellow sodium chromate is added to clear silver nitrate
Production of _________________________________
zinc + hydrochloric acid releases H2 gas
Most chemical changes are not easily reversed, like many physical changes are.

18. Conservation of Mass – Key concept
_______________________________________________– mass is neither created or destroyed in a chemical reaction.
When you burn wood at a beach bonfire, the reaction produces
It may seem that the amount of matter has been reduced when you look at the ash pile.
However, if you carefully measure the mass of the reactants and the mass of the products, you would find they are the same.

19. Conservation of Mass