1. Properties and Change 8.P.1
Matter
Properties and Change 8.P.1

2. Atom Def. Basic unit of a chemical element.
Protons; a subatomic particle that has a positive charge.
Neutrons; a subatomic particle with no charge (neutral).
Electrons; a subatomic particle that has a negative charge.
Valence electron; electrons on the outer valence shell.
It’s important because; they determine which atoms they are most likely to combine with.

3. Atomic Theory
Atomic Number; the number that tells the number of protons in the nucleus of an atom. Write 10 element symbols with their atomic #.
Atomic Mass; the total number of protons and neutrons in the nucleus.
Atomic Mass Number; the average mass of that element and its isotopes.

4. Atomic models 12 11 Mg Na Magnesium Sodium 24.31 22.99
Figure out how many protons, electrons and neutrons are in these atoms

5. Bohr Models
Draw Bohr models of three elements and give the valence number of each. Here is an example of Helium, valence of 2 electrons.

6. Periodic Table of Elements
Dmitri Mendeleev created the PTE
The periodic table is set up from most reactive to less reactive. Grouped by metals, metalloids, nonmetals. Increasing atomic # from left to right.

7. Two elements that have similar chemical properties…
The most reactive group of metals is ____________the second most reactive is _______________
The most reactive group of nonmetals is ____________
The least reactive elements are at the bottom of the group.
The _____________ will not react with other elements.
Periods
As you go from left to right the number of protons and electrons increase, the valence level is the same.

8. Properties of Metals, Non-metals and Metalloids.

9. Chemical and Physical Properties and Changes.

10. Pure substance vs. mixture

12. Chemical Reactions
Reactant; the materials present at the beginning of a reaction.
Photosynthesis
6H2O + 6CO2 + light energy → C6H12O6 + 6O2
Product; substance that results from the reactants.
Respiration
C6H12O6 + 6O2 → chemical energy + 6H2O + 6CO2
Law of Conservation of Matter
Matter can neither be created nor destroyed. It can, however be changed.
 2H2 +O2 → 2H2O
H=4 O=2 → H=4 O=2

13. Evidence of Chemical Reactions
Description
Example 1.
Color change
Mixing Kool-Aid in water
Fire works 2.
Temperature change
Increase or decrease in temp.
Yeast in vinegar
Baking soda/vinegar 3.
Gas formation
Formation of bubbles (CO2) 4.
Percipitate
A solid forms in a liquid.
Silver nitrate in alcohol