1. The Periodic Table

2. Alkali Metals
They are very reactive. Why? They all have one electrons in their outer shell. That's one electron away from being happy (full shells)
*Shiny
*Their light weight and physical properties separate them from other metals.
*They are malleable (bendable)
*Alkali metals are not the type of metals you would use for coins or houses.

3. Alkaline Earth Metals
*When these compounds are mixed in solutions, they are likely to form solutions with a pH greater than 7. Those higher pH levels means that they are defined as "basic" or "alkaline" solutions.
While not as reactive as the alkali metals, this family knows how to make bonds very easily. Each of them has two electrons in their outer shell.

4. Transition Metals Summary of Common Properties *Very hard
*High melting points
*High boiling points
*High electrical conductivity
*Malleable

5. Metalloids or Semimetals
Summary of Common Properties
Electronegativities between those of metals and nonmetals
Ionization energies between those of metals and nonmetals
Possess some characteristics of metals/some of nonmetals
Reactivity depends on properties of other elements in reaction
Often make good semiconductors

6. Halogen Group Summary of Common Properties *Very high electronegative
*Seven valence electrons (one short of a stable octet)
*Highly reactive, especially with alkali metals and alkaline earths

7. Noble Gases Summary of Common Properties *Fairly nonreactive
That seven-electron trait applies to all of the halogens. 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. They are very reactive.
Summary of Common Properties
*Fairly nonreactive
*Complete valence shell
*High ionization energies
*Very low electronegativities
*Low boiling points (all gases at room temperature)