1. Classifying Matter
Properties of Matter

2. Matter is anything that takes up space and has mass.
The Nature of Matter
Matter is anything that takes up space and has mass.
The word matter comes from the Latin word materia, meaning “material” or “stuff”
First we need to ask . . .
What is matter?
Examples of Matter:
You can observe matter easily with your senses rocks, trees, bicycles, air Basically everything and anything!
The only thing that wouldn’t be matter would be energy (sunlight, heat, electricity). - no mass or volume so they can’t be matter!

3. Elements, Molecules, and Compounds
Elements and compounds make up all the different kinds of matter in the universe.
Elements are the simplest form of matter
Cannot be broken down into simpler substances.
Each element is made of atoms of the same type.
Each has a unique set of physical and chemical properties.
117 known elements in the universe.
Approximately 92 are found naturally on Earth.
Six elements make up 99% of all living matter!
Sulfur
Potassium
Oxygen
Examples of Elements:
gold
silver
oxygen
hydrogen
Nitrogen
Carbon
Hydrogen
aluminum
nitrogen
tin
calcium

4. Soft metal explodes in H20 Poisonous greenish gas
Compounds, Molecules, and Elements
Compounds are two or more elements combined chemically together.
Properties are different from the properties of the elements that make them up.
Example:
Most matter in the universe is in the form of compounds! H
(hydrogen)
Explosive gas Na
(Sodium)
Soft metal explodes in H20 + Cl
(chlorine)
Poisonous greenish gas O2
(oxygen)
Explosive gas = =
Salt
Water +

5. Molecules, Elements, and Compounds
When two or more atoms combine, they form a molecule.
Most molecules are made of two or more atoms
A molecule is the smallest particle of a substance with the same properties of the substance.
NOTE: Compounds are different than molecules because I said so. Worry about it more later (like 8th grade).

6. Mixtures, Solutions, and Suspensions
A mixture is a combination of two or more substances NOT combined chemically.
May be a mixture of both elements and compounds
Substances keep their unique properties and can be separated by physical means.

7. Mixtures, Solutions, and Suspensions
There are two types of mixtures . . .
Heterogeneous – the parts of the mixture are noticeably different from one another.
Homogeneous – the parts (substances) are evenly distributed. It is difficult to tell one substance from another.

8. Solutions, and Suspensions and Colloids
A solution is a mixture that looks like a single substance and has the same properties throughout.
Solute ~ The substance that dissolves in a solution.
Solvent ~ The substance into which the solute dissolves.

9. Solution
Stirring & Higher Temperatures will allow solute to dissolve faster in the solvent

10. Saturated Solution
Solubility has been reached when the solution is saturated. In a saturated solution no more of the solute will dissolve in the solvent under normal conditions.

11. Which is Solute? Solvent?
Sugar is dissolved in iced tea
Oxygen is dissolved in water
Water has salt added to it
Jello is added to hot water

12. Physical Properties
Physical property is a property that can be observed without changing the identity of the substance.
Examples:
viscosity
conductivity
malleability
hardness
magnetism
melting point
boiling point
density
color

13. Examples of Physical Properties
Viscosity of a substance is its resistance to flow.
Examples: water = low viscosity
honey = high viscosity
Conductivity is a material’s ability to allow heat to flow.
Examples: metal = high conductivity wood = poor conductivity

14. Examples of Physical Properties
Malleability of a substance is its ability to be hammered into a thin sheet
Melting and Boiling points are the temperatures at which a solid becomes a liquid and a liquid becomes a gas.
Density of a substance is the ratio of its mass compared to its volume.

15. Chemical Properties
Chemical property is any ability to produce a change in the composition of matter.
Examples of chemical properties . . .
flammability
reactivity
Material’s ability to burn in the presence of oxygen.
How readily a substance combines chemically with other substances.