1. The Periodic Table
Proposed by Mendeleev

2. Dmitri Ivanovich Mendeleev 1834-1907
Born in Siberia, the last of at least 14 children, Dmitri Mendeleev revolutionized our understanding of the properties of atoms and created a table that probably adorns every chemistry classroom in the world.

3. Arrangements
Periods – Rows – determines the number of energy levels in an atom
Lanthanide Series (57-71) – rare earth elements
Actinide Series (89-109) – radioactive elements

4. Lanthanide Series – Rare Earth Elements
                 
                                                     
Not as rare as once thought
The lanthanides have many scientific and industrial uses. Their compounds are used as catalysts in the production of petroleum and synthetic products. Lanthanides are used in lamps, lasers, magnets, phosphors, motion picture projectors, and X-ray intensifying screens.

5. Cerium
Lanthanum

6. Actinide Series - Radioactive
                                                     
They are all radioactive and some are not found in nature. Some of the elements with higher atomic numbers have only been made in labs.

8. Arrangements (cont.)
Groups or Families – arranged according to the number of electrons in the outer energy level
IA or 1 – alkali metals
IIA or 2 – alkali earth metals
VIIB or 17 – halogens
VIII or 18 – noble gases – inert gases

9. Alkali Metals Very reactive One electron in the outer shell Shiny
                                                     .
Very reactive
One electron in the outer shell
Shiny
Light weight

10. Sodium

11. Alkaline Earth Metals Two electrons in the outer shell
                                                      So we just
                                                     .
Two electrons in the outer shell
Fairly reactive (not as reactive as Alkali metals

12. Magnesium - Mg
Magnesium tarnishes slightly in air, and finely divided magnesium readily ignites upon heating in air and burns with a dazzling white flame. Normally magnesium is coated with a layer of oxide, MgO, that protects magnesium from air and water.

13. The Halogens
                                                   
They have seven electrons in their outer shell. They are all just one electron shy of having full shells. Because they are so close to being “happy”, they have the trait of combining with many different elements. You will often find them bonding with metals and elements from Group One of the periodic table.

14. Halogens
The Halogens are a generally nasty bunch. Think toxic choking fumes. But in compounds with the similarly strong-willed alkali earths, they can be delicious.
Fluorine F

15. Inert Gases - Noble Gases
                                                  
All of the inert gases have full outer shells with eight electrons. Oh wait! That's not totally correct. At the top of the inert gases is little helium (He) with a shell that is full with two electrons. The fact that their outer shells are full means they are quite happy not reacting with other elements.