1. Matter and Change

2. Matter Defined as anything that has a mass and takes up space.
The mass of an object is the amount of matter that an object contains.
Does a golf ball or tennis ball contain more matter?
A golf ball has more mass, therefore, it contains more matter.

4. Density the ratio of the mass of an object to its volume
Density = Mass
Volume
Lead has a density of 11.3 g/mL. What is the the volume of a sample of lead that has a mass of 32.0 g?

5. Density Density = Mass Volume 11.3 g/mL = 32.0 g x mL 11.3 x = 32

6. Mixtures
A mixture is a physical blend of two or more substances. (Heterogeneous and Homogeneous Matter)
Heterogeneous mixture: not uniform in composition
Any physically separate part of the material is called a phase.
A phase is any region with a uniform set of properties.
Heterogeneous material is composed of more than one phase.
The boundaries of each phase are called interfaces.

7. Homogeneous Matter
Materials which consist of only one phase are called homogeneous materials.
Examples: salt water, glass,etc.
A homogeneous mixture is called a SOLUTION.
Solute (the dissolved material)
Solvent (the dissolving material)
In salt water, the salt is the solute and the water is the solvent.

8. Substance: Matter that has a uniform and definite composition.
Elements: Simplest form of matter. They can not be separated by physical or chemical means.
Compounds:Two or more elements combine chemically with one another; they can be separated only by chemical means.

9. Physical Properties
All elements have different physical and chemical properties
Physical Property: a quality of a substance that can be measured without changing the substance’s composition.
Color, solubility, odor, hardness, density, melting point, and boiling point, and length are all physical properties. (p. 29 in your text)

10. Physical Properties
Physical Properties can be divided into two groups:
Extensive properties: depends on the amount of matter present.
Mass, length, and volume
Intensive properties: do not depend on the amount of matter present.
Density,color,crystalline shape, melting point, boiling point, etc.

11. Separation Techniques
Separate based on physical properties:
Iron is magnetic, salt will dissolve in water. Etc
Distillation:
salt water could be boiled, the water vapor would then be cool and allowed to condense into another flask, leaving the salt behind.
Crystallization:
Most substances have a limited amount of solute that can be dissolved in the solvent. When there is too much of the solute, the solute will begin to crystallize.
For example: salt water

12. Four States of Matter

13. Phase Changes
Heating a material can cause a phase change, however, it still has the same composition.
The four states of matter are: solid, liquid, gas, and plasma.
The energy of the atoms gets greater as a substance moves from solid to liquid to gas, to plasma.

15. Definitions Solids: Have a definite shape and a definite volume.
Liquids: DO NOT have a definite shape, but they do have a definite volume.
Gases: Do NOT have a definite shape or definite volume. They can be compressed.
Plasma is the highest energy phase and is quite rare on earth. It is primarily found in stars.

16. Physical Change
Physical Changes do not change the chemical character of a substance.
Pounding, pulling, heating, cutting, bending, freezing, melting, etc.
One slice of bread is made out of the same composition as one loaf of bread
Ice and water are still composed of H2O

17. Chemical Properties
Chemical Property: the substance forms into a new substance during a chemical reaction.
chemical properties are only observed when a substance undergoes a chemical change.
Rusting (oxidation) is a chemical property of iron that is observed when iron is exposed to oxygen.

18. Chemical Change
Whenever a substance undergoes a change so that one or more new substances with different properties are formed.
Examples: Burning, digesting, fermenting, rusting, heat forms, change of color, etc.
Reactants  products
Law of conservation of mass

19. Symbols and Formulas
All matter in the universe is composed of elements.
Each element is represented by a one or two letter chemical symbol.
The first letter is always capitalized. The second is always lowercased.
Some chemical symbols are derived from Latin or Greek names for the element. (Table 2.4)
Sodium’s Latin name is natrium and thus the symbol is Na.

20. International Union of Pure and Applied Chemistry
The IUPAC has devised a systematic naming process for elements that have not been officially named yet.
The name is determined from the atomic number. Each digit is represented by a prefix. All the prefixes are put together and the ending of -ium is attached to the end.

21. IUPAC Element Naming Rules
The final “n” of “enn” is omitted when it occurs before “nil”.
The final “I” of “bi” and “tri” is omitted when it occurs before “ium”.
The symbol of the element is composed of the first letter of each prefix.
0 = nil 4 = quad 7 = sept
1 = un 5 = pent 8 = oct
2 = bi 6 = hex 9 = enn
3 = tri

22. Examples 901 116 203 (Enn)(nil)(un)-ium: Ennilunium (Enu)
(un)(un)(hex)-ium: Ununhexium (Uuh)
203
(Bi)(nil)(tri)-ium: Biniltrium (Bnt)

23. Elements
An element symbol represents one atom of that particular element.
If a hydrogen atom was bonded to another hydrogen atom, it would be called a molecule and would be written as H2
A molecule is when 2 or more (same) atoms are joined together.
A compound is when 2 or more different elements are joined together.

24. Sites
www2.mcas.k12.in.us