1. History of Periodic Table

2. Evaluation/ Assessment
Objective
Today I will be able to:
Analyze how elements are arranged on the periodic table based on properties
Explain the history of the periodic table.
Apply the trends of ionization energy, electronegativity and atomic radius, electron affinity and ionic radius to problem solving.
Evaluation/ Assessment
Informal assessment – Listening to group interactions and discussions as they activity and complete practice
Formal Assessment – Analyzing student responses to the exit ticket and practice
Common Core Connection
Build Strong Content Knowledge
Value Evidence
Reason abstractly and quantitatively
Look for and make use of structure

3. Lesson Sequence Evaluate: Warm-Up
Engage/Explore: Periodic Table Activity
Explain: History of Periodic Table Notes
Elaborate: Periodic Trends Intro
Evaluate: Exit Ticket

4. Warm-Up
Which of the following ions are not likely to form? Explain your answer based off of the trends we have discussed this unit.
Al3+ Al2+ Al5-

5. Objective Today I will be able to:
Analyze how elements are arranged on the periodic table based on properties
Explain the history of the periodic table.
Apply the trends of ionization energy, electronegativity and atomic radius, electron affinity and ionic radius to problem solving.

6. Homework
STEM Fair Due Friday, November 19

7. Agenda Warm-Up Periodic Table Activity History of Periodic Table Notes
Periodic Trends Intro
Exit Ticket

8. Periodic Table Activity
Recreating the periodic table

9. Periodic Table Activity Directions
Work with your row to complete the activity
Arrange the known elements on the cards into the order of the periodic table
Place the unknown’s in their spot based on the properties of the elements
Hint: you are only working with elements in the s and p block

10. Discussion
What process did you use to arrange your unknowns on the periodic table?
Did some properties help determine the unknowns more than others?
Were there any exceptions?

11. Answers
Unknown
Element 1 Mg 2 F 3 Rb 4 Kr 5 S 6 Ge 7 Sb

12. History of the Periodic Table

13. Johann Dobereiner (1829)
Law of Triads - in triads of elements the middle element has properties that are an average of the other two members when ordered by the atomic weight
Example - halogen triad composed of chlorine, bromine, and iodine

14. John Newlands (1864)
Law of Octaves - states that any given element will exhibit analogous behavior to the eighth element following it in the periodic table

15. Dmitri Mendeleev (1871) Developed the first Periodic Table
He arranged his table so that elements in the same column (groups) have similar properties; increasing atomic mass

16. Dmitri Mendeleev (1871)
Broke the trend of arranging elements solely by their atomic mass
Wanted to keep elements with similar properties in the same columns
Left gaps in his early tables; predicted elements that had not been discovered would fill in those gaps
- Ekasilicon  Germanium
- Germanium was discovered in 1886

17. Dmitri Mendeleev (1871)

18. Henry Moseley (1913)
Periodic Law - when elements are arranged in order of increasing atomic number, their physical and chemical properties show a periodic (repeating) pattern
The periodic law is the basis for arranging elements in the periodic table

19. Glenn Seaborg
He reconfigured the periodic table by placing the actinide series below the lanthanide series
Awarded a Nobel Prize in 1951
Element 106, Seaborgium (Sg), is named in his honor

20. Introduction to the Periodic Trends

21. Atomic Radius
Distance from the center of an atom to the outermost edge of the electron cloud

22. Electronegativity
The ability to attract electrons in a chemical bond

23. Ionization Energy Energy needed to remove an electron from an atom
High ionization energy means atoms hold their electrons very tightly

24. Exit Ticket – Make a prediction
Which elements do you think would have a higher ionization energy?
Na or Ne
Mg or Ba