Organization of the Periodic Table



Aim: 

To Discuss and Illustrate the History and Organization of the Periodic Table
Students should be able to explain the contributions of J. A. R. Newlands, Dmitri Mendeleev, Lothar Meyer and H. G. J. Moseley. Students should be able to apply the following trends, atomic radius, ionization energy, electronegativity, succesive ionization energy and ion size versus atomic radius.
Questions: 
What are the law of octaves and periodic law?   Why was Mendeleev credited with the first periodic table of elements and what are the specific details about his periodic table (what it was based upon, the gaps that he discovered, what was left out, and what was inaccurate about it)?  How does the  modern periodic law differ from Mendeleev’s arrangement of the periodic table? Why is the periodic table is such a valuable tool?  Why groups have similar properties? What are the periodic trends?
Student Activity:
 Students will create charts:
Write equations demonstrating ionization energy
Write electron configurations
Draw electron orbital diagrams
Define and determine number of valence electrons
Define and identify valence electrons and state their importance in terms of the periodic table(show this using a chart of the representative elements)
Identify elements by their group/family and period
Use the various schemes for labeling the groups of the periodic table (use EOC table as a guide)
Identify what elements are metals, nonmetals, and metalloids( illustrate using the zig zag line)
Recognize and list characteristics of metals, nonmetals, and metalloids(organize into a table format)
Define and identify examples of the following categories: s-block elements, p-block elements, d-block elements, f-block elements(label on chart which groups belong to which blocks)Be sure to label each of the following: 
alkali metals, Halogens, transition metals, inner transition metals, alkaline metals,  Noble gases. 

Summary Study the Periodic Table Study Guide document