1. Electron and Orbital ConfigurationsCa Cl Na Cu

2. Periodicy The periodic table was proposed by Mendeleev in the 1860’s
It correctly predicted the properties of new elements, making it a useful and powerful tool
The vertical columns in the periodic table are called groups
The horizontal rows in the periodic table are called periods

3. Important groups Group 1A – Alkali Metals
Group 2A – Alkaline Earth Metals
Group 7A – Halogens
Group 8A – Noble Gases / Inert Gases

4. Elements can be divided into 3 categories
Classes of Elements
Elements can be divided into 3 categories
Metals
Non-metals
Metalloids

5. Properties of Metals Good conductors of heat and electricity
Solid at room temp. (exception: Hg)
Most are malleable and ductile (can be made into wire)
Groups 3-12 are called transition metals
Have varied levels of reactivity

6. Properties of Non-Metals
Poor conductors of heat and electricity
All gases are non-metals
Non-metals that are solid tend to be VERY brittle
Varied levels of reactivity, however F is the most reactive non-metal, while Noble Gases tend to not react

7. Properties of Metalloids
A metalloids ability to conduct electric current varies with temperature
Metalloids’ properties tend to fall in between those of metals and non-metals
Metalloids are B, Si, Ge, As, Sb, Te, Po, and At.

8. Alkali Metals Have 1 valence electron Most are exceptionally reactive
Most alkali metals can not be stored with air, because they tend to react with water vapor
Include Li, Na, K, Rb, Cs, and Fr

9. Alkaline Earth Metals
Have 2 valence electrons
All react with water except Be
Mg and Ca are important in biological processes
Mg is often used to make metals lighter without sacrificing strength