1. Matter

2. Outline Properties of Matter Changes in Matter
States of matter
Physical properties
Chemical properties
Changes in Matter
Physical changes
Chemical changes
Law of Conservation of Mass
Mixtures, Elements and Compounds
Heterogeneous, Homogeneous mixtures
Separating Mixtures
Elements and Compounds

3. What is matter? Everything in the universe is made of matter.
Matter is made of tiny particles called atoms.

4. States of Matter
All matter exists as one of the three physical forms, which are called the states of matter.
Solid
Liquid
Gas
Definite Shape
Definite Volume
Particles held tightly together

5. Physical Properties
A physical property is a characteristic of matter that can be observed directly or measured without changing the substance’s composition.
Examples of Physical Properties are:
Boiling point Ductility
Melting point Elasticity
Density Brittleness
Color
Odor
Malleability

6. Chemical Properties
Characteristic of matter that can only be observed when one substance changes into a different substance
Examples of Chemical Properties:
Flammability
Reactivity with acids
Ability to rust

7. Identifying Changes
Physical Changes
Physical state
Chemical Changes

8. Types of Change Type of Change Products of Change Physical Change
No new substance, but physical state is changed.
Example:_____________________
Chemical Change
New substances are formed.
Also called a chemical reaction.

9. Chemical Reactions Color Change Temperature change Change in odor
A chemical reaction is a process in which atoms of one or more substances rearrange to form one or more new substances.
When a new substance(s) is formed, there are indications.
Color Change
Change in odor
Formation of Bubbles
Formation of Precipitate
Temperature change
Light

10. Conservation of Mass
The Law of Conservation of Mass states that mass is neither created nor destroyed during a chemical reaction. Mass is always conserved in a chemical reaction.

11. Chemical Reactions and Chemical Equations
Chemical reactions are written in the form of a chemical equation.
The starting substances are called the reactants.
The substances produced, or formed, are called the products.
Reactant + Reactant  Product + Product
Eg.

12. Elements and Compounds
An element is a pure substance that cannot be separated into simpler substances by any means.
Each element has a name and a chemical symbol.
Elements are organized in the periodic table.
A compound is made up of two or more different elements that are combined chemically.

13. Mixtures
A mixture is a combination of two or more pure substances. Each substance in a mixture keeps its chemical properties.
A pure substance is a substance that is the same throughout.
Example:

14. Compounds: Law of Definite Proportions
A compound is always composed of the same elements in the same proportion by mass.
Mass of a compound = sum of the masses of the elements that make up the compound

15. Compounds: Law of Multiple Proportions
When different compounds are formed by a combination of the same elements,
If two elements form more than one compound between them, then the ratios of the masses of the second element (which combine with a fixed mass of the first element) will be ratios of small whole numbers
Example:

16. Elements, Mixtures and Compounds

29. Mixtures
Types of Mixtures:
Homogeneous: “the same” A mixture that has constant composition throughout.
Example:
Heterogeneous: “different” A mixture that does not blend smoothly and has a non-uniform composition

32. Separating Mixtures
Because substances in a mixture are physically combined, the processes used to separate a mixture are physical (no need for chemical reactions)
Filtration
Distillation
Crystallization
Sublimation
Chromatography

33. 1. Filtration

34. 2. Distillation

36. 3. Crystallization
Formation of pure solid particles of a substance from a solution containing the dissolved substance.

37. 4. Sublimation or Evaporation
Sublimation: Solid changes to vapor without melting
Eg.
Evaporation: Liquid changes to gas

39. 5. Chromatography