1. The Periodic Table

2. How would you organize all of the students within the school?

3. The Mayan Periodic Table

4. The Telluric Helix or Screw-Shaped (1862)

5. Newlands' Octaves (1864) – arranged by atomic weights

6. Mendeleev's Periodic Table (1871)

7. Ingo Hackh's Periodic Table (1914)

8. Modern Periodic Table (almost)

9. Modern Periodic Table (extended) This is actually the preferred way to organize the periodic table. It isn’t used because it takes up too much room!

10. Modern Periodic Table (compressed)

11. Andreas von Antropoff (1926)

12. Edgar Longman's (1951)

13. A Spiral Periodic Table by Thoedor Benfey (1960)

14. The Dufour Periodic Tree (1992) & A Physicist's Periodic Table (1988)

15. Alexander Periodic Table (1994) This “arrang[es] the elements contiguously and continuously according to the atomic number without disturbing the accepted group and property interrelationships previously found in the periodic chart.” http://periodictable.com/pages/AAE_Descript1.html

16. A Triangular Periodic Table by Emil Zmaczynski (1935) & A Helical Periodic Table (1995)

17. The Bayley-Thomsen-Bohr Periodic Table (1997)

18. Philip Stewart's 'Chemical Galaxy II' (2005)

19. Eric Scerri's Periodic Table (2006) Eric Scerri, The Periodic Table: Its Story and Its Significance, Oxford University Press, 2006The Periodic Table: Its Story and Its Significance

20. Spiral Periodic Table (2006)

21. ADOMAH Periodic Table by Valery Tsimmerman (2007)

22. Ca 20 40.078

23. Periodic Table Lingo Groups –Also called families –The elements in vertical columns –Elements in a group have similar properties –Labeled 1A-8A or 1B-8B

24. Periods –Horizontal rows of elements –Numbered 1 - 7

26. The Block at the Bottom The two rows at the bottom are actually removed from the middle of the periodic table to make the table more condensed.

27. Classification of Elements 1. Metals  Most elements are metals  Have luster (shininess)  Conduct heat and electricity  Most are solid at room temperature  Are malleable and ductile

28. 2. Nonmetals  Opposite of metals  No luster  Poor conductors of heat and electricity  Not malleable or ductile  Solid, Liquid or gases  Physical properties vary greatly

29. 3. Metalloids  Can have the properties of metals or nonmetals or a combination of both

30. Most General Breakdown:

31. Special Group Names  Group 1A – Alkali Metals  Group 2A – Alkaline Earth Metals  Group 7A – Halogens  Group 8A – Noble Gases

33. Family Characteristics  Alkali Metals- they are VERY reactive –Because of this, they usually exist as compounds with other elements –Two familiar Alkali metals: Na in salt and Li in batteries  Alkali Metals React! Alkali Metals React! Alkali Metals React!

34. Family Characteristics  Alkaline Earth Metals- also highly reactive –Calcium and Magnesium as minerals are important for your health

35. Family Characteristics  Transition Metals- 38 elements –Have “metals” characteristics –Have valence electrons in 2 shells –Iron, Nickel and Cobalt are magnetic  Other Metals- 7 elements –Not the same as transition metals –Valence e’s only in 1 shell –Solid, high density, opaque

36. Family Characteristics  Halogens- 5 elements –Highly reactive –Compounds containing these are called salts –They exist at room temperature in all 3 states of matter  Iodine and Astatine=solid  Bromine=liquid  Fluorine and Chlorine=gas

37. Family Characteristics  Noble Gases- 6 elements –Considered “inert” until 1960s because their full outer shells prevent them from readily forming compounds –They are stable  Inner Transition Metals (Rare Earth Elements) -30 elements –Most are man-made

39. s, p, d, and f Blocks The PT can be used to double check electron configurations. The last letter and superscript should be the same as the letter and superscript for the column it is in.

42. Valence electrons  These are the electrons on the outermost ring. They are available for bonding.  They can be found by counting the columns on the Periodic Table.  EX: P in group 5A = 5 valence electrons

43. Lewis Dot Structures  Simple way to show the valence electrons. –There are four spots to place electrons in these dot structures- top, bottom, left and right. –Remember the most valence electrons an element or ion can have is 8. –Don’t pair up the electrons until they have to. X

44. Example  Beryllium- –2 valence electrons –2 dots (don’t pair them) (don’t pair them)  Selenium- –6 valence electrons –6 dots Be Se

45. Common Ion  In order to be stable, all elements want an electron configuration of a NOBLE GAS.  They will gain or lose electrons to complete their outside shell.  The periodic table will help you to be able to predict this.

46.  Draw the Lewis Dot Structure for –Cl –Ca –Li –N +2

49. Organizing the PT Activity  Groups of 4  1 textbook per group, 1 piece of printer paper per group  Each person needs their own piece of notebook paper  Turn to page 193, do the mini lab  Answer questions 4 and 5  Due tomorrow