1. How the periodic table is put together

2. What is the Periodic Table?
It is an organizational system for elements.

3. Who created it?
The quest for a systematic arrangement of the elements started with the discovery of individual elements.
  By 1860 about 60 elements were known and a method was needed for organization. 
In 1869, Russian chemist Dimitri Mendeleev proposed arranging elements by atomic number and properties.
The table contained gaps but Mendeleev predicted the discovery of new elements.

4. Patterns of repeating properties
So how is it arranged?
The genius of the periodic table is that elements are placed in specific places because of the way they look and act.
Patterns of repeating properties

5. What do all the numbers mean ?
From

6. You've got Your Periods...
When you look at a periodic table, each of the rows is considered to be a different period (as in the PERIODic table.)

7. Periods = Rows
In the periodic table, elements have something in common if they are in the same row.
All of the elements in a period have the same number of atomic orbitals. (orbitals are specific areas around an atom that contain electrons)
Every element in the top row (the first period) has one orbital for its electrons. All of the elements in the second row (the second period) have two orbitals for their electrons, and so on…

8. And you got your groups…
The columns are made up of similar behaving (reacting) elements called groups.

9. Groups = Columns
The elements in a group have the same number of electrons in their outer orbital.
Every element in the first column (group one) has one electron in its outer shell.
Every element on the second column (group two) has two electrons in the outer shell.
As you keep counting the columns, you'll know how many electrons are in the outer shell.
These #s of electrons help determine charge
The exception to this is the transition elements, which make up the middle part of the table

10. Other than periods and groups, the table is divided into families.

11. NATURAL STATES

12. METALS, NONMETALS, & METALLOIDS

13. METALS, NONMETALS, & METALLOIDS
Lustrous, malleable, ductile
Conductors (of heat and electricity)
Nonmetals:
Dull, brittle (if solid), nonconductors
More variety in properties than metals
Metalloids:
Mix of metallic or nonmetallic properties
Semi-conductors

14. ALKALI METALS very reactive metals that do not occur freely in nature
malleable, ductile (soft), good conductors of heat and electricity.
Very reactive to water
+1 charge

15. From www.science-class.net
ALKLINE EARTH METALS
very reactive
+2 charge
Also not found free in nature
From

16. TRANSITION METALS Harder metals (still ductile and malleable)
Less reactive
Various charges, many ions

17. RARE EARTH ELEMENTS Inner Transition elements Many are man-made
Lanthanides
Actinides

18. OTHER METALS
are ductile and malleable
are solid, have a high density,

19. METALLOIDS have properties of both metals and non-metals
Some are semi-conductors - they can carry an electrical charge under special conditions.
This property makes metalloids useful in electronics

20. HALOGENS Corrosive, colored gas, liquid, & solid
Very reactive - not found uncombined
-1 charge
"halogen" means "salt-former" and compounds containing halogens are called "salts"

21. NOBLE GASES All gasses in natural form Do not form compounds easily
Happy/Inert Elements (Full outer shells)

22. Other NON-METALS Not able to conduct electricity or heat very well
Very brittle (if solid) and dull - do not reflect light
Various properties & charges
Solid or gas, some diatomic
Important organic elements

23. CHARGES FIXED & VARIABLE

24. Trends!
(more on this in later units…)