1. Periodic Table Organization

2. Main Block Elements (RepresentaTive Elements)
Valance electrons are s and p orbitals
The A group or 1-2 and 13-18

3. (Outer) transition metals
Group B
Valence electrons are in the d orbital
Common metals fall into this group

4. Inner Transition Metals
Group B
Valence electrons are f orbitals
Rare earth metals, less common

5. Alkali Metals Group 1A (Hydrogen not included)
Metallic, the softest of metals, lowest density of metals, low melting points, very reactive
s orbital , 1 valence electron

6. Alkaline earth Metals Group 2A
Reactive, but not as much as Alkali metals, low density, soft
S orbital, 2 valence electrons

7. Transition metals (in the middle)
Common metals
Generally hard, high melting and boiling points, high density
Reactivity varies
d orbital valence electrons

8. Inner transition:lanthanides and actinides
Lanthanides have similar properties to the alkaline earth metals, used in small quantities in some industry
Actinides are similar to alkaline earth metals, but are very dense with high melting points. Many are man made and radioactive.
f orbital valance electrons

9. Noble Gases
Group 18 or 8A; Very stable, with a full outer shell of valence electrons (8), following the octet rule.

10. Halogens
Group 7A or 17
7 valence electrons in the p orbital, 1 short of full shell
Very reactive and very useful

11. Pnictogens and chalcogens and others
Pnictogens, group 15 (5A), chalcogens, group 16(6A), and group 13-14(3A and 4A) are made of metals, non-metals and metalloids.
They have a variety of properties
The number in front of the A indicate number of valence electrons

12. Hydrogen Under 1A, but it is its own group.
Gains and loses electrons, but not as reactive a alkali metals or halogens
Very useful and abundant element.

13. Metals On the wall they are blue Most elements
Silver-ish, except copper and gold
Solid at room temperature, except mercury which is a liquid
Lustrous or shiny
Malleable, ductile
Conduct heat and electricity
High melting point, dense and react with acids

14. Non-metals Near the Noble Gases
On the wall, they are orange, yellow and Hydrogen
Dull in appearance
Brittle
Poor conductors of heat and electricity
Not too reactive with acids
Low melting points
Solids, liquids or gases at room temperature

15. Metalloids or semi-metals
On the wall, they are green
Zigzag on the Periodic Table
Properties of both metals and non-metals
May or may not conduct electricity, conduct best when mixed with other elements.

16. Solids, Liquids, and Gases (room Temp.)
Solids: Most elements
Liquids: Mercury and Bromine(Br2)
Gases: Nobles, H2, N2,O2, F2, Cl2
last diatomic solid I2; The 7 Diatomics have to bond with themselves to exist in nature, so the 2 subscript

17. Valence electrons
Outermost electrons in an orbital of an element
These are responsible for reactions and bonding; They are shared or transferred (given/taken)

18. Electron configuration
How electrons orbit the nucleus of an atom, with s,p,d and f indicating general shape of orbital
These will be represented in various distances or levels from the nucleus
The outermost electrons are called valence electrons

19. Octet Rule
The outer shells of elements will react or bond until they have a full valence shell like the noble gases
This is usually 8 valence electrons obtained from sharing or transferring of electrons in bonding