1. Matter Unit Periodic Table Notes

2. The Periodic Table Dmitri Mendeleev (1834 - 1907)

3. P ZnAs Sb PtBi Midd. -1700 CrMn Li K NOF Na BBe H AlSiCl CaTiVCoNiSeBr SrYZrNbMoRhPdCdTeI BaTaWOsIr Mg CeTbEr ThU 1735-1843 Discovering the Periodic Table C S FeCu AgSn AuHgPb Ancient Times He ScGaGe RbRuIn CsTl PrNdSmGdDyHoTmYb La 1843-1886 Ne Ar Kr Xe PoRn Ra EuLu Pa Ac 1894-1918 Tc HfReAt Fr Pm NpPuAmCmBkCfEsFmMdNoLr 1923-1961 Rf Db SgBhHsMt 1965- Journal of Chemical Education, Sept. 1989

4. Elements are arranged: Vertically into Groups Horizontally Into Periods

5. Why?

6. If you looked at one atom of every element in a group you would see…

7. Each atom of a group has the same number of electrons in its outermost shell. An example…  Valence electrons are the electrons in the outermost energy level.  The number of “valence” electrons in an atom affects the way an atom bonds.  The way an atom bonds determines many properties of the element.  This is why elements within a group usually have similar properties.

8. The group 2 atoms all have 2 electrons in their outer shells Be (Beryllium) Atom Mg (Magnesium) Atom

9. If you looked at an atom from each element in a period you would see…

10. Each atom of the period has the same number of electron shells or energy levels. An example…

11. The period 4 atoms each have 4 electron containing shells K (Potassium) Atom Fe (Iron) Atom Kr (Krypton) Atom 4 th Shell

12. Each group has distinct properties The periodic Table is divided into several groups based on the properties of different atoms.

13. Alkali Metals Soft, silvery colored metals Very reactive!!! http://www.lyon. edu/webdata/U sers/DMcDowel l/GenChem/alka lishow.html

14. Group 1A: Alkali Metals Cutting sodium metal Reaction of potassium + H 2 O http://www.youtube.com/watch?v=m55kgyApYrY&safety_mode=true&persist_safety_mode=1&safe= active

15. Alkali Metals reacting with water: Li (Lithium) – least reactiveLi (Lithium) Na (Sodium) K (Potassium) Rb (Rubidium) Cs (Cesium) – more reactiveCs (Cesium)– What would you expect from Francium?!?!

16. Magnesium Magnesium oxide Group 2A: Alkaline Earth Metals

17. Alkaline Earth Metals Silvery-White Metals Fairly reactive Many are found in rocks in the earth’s crust

18. Transition Metals Malleable (easily bent/hammered into wires or sheets) Most are good conductors of electricity

19. How many things can you think of that have Transition Metals in them?

21. Metalloids  Lie on either side of the “staircase” They share properties with both metals and non- metals Si (Silicon) and Ge (Germanium) are very important “semi- conductors”

22. Metals and Nonmetals Li 3 He 2 C6C6 N7N7 O8O8 F9F9 Ne 10 Na 11 B5B5 Be 4 H1H1 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 K 19 Ca 20 Sc 21 Ti 22 V 23 Cr 24 Mn 25 Fe 26 Co 27 Ni 28 Cu 29 Zn 30 Ga 31 Ge 32 As 33 Se 34 Br 35 Kr 36 Rb 37 Sr 38 Y 39 Zr 40 Nb 41 Mo 42 Tc 43 Ru 44 Rh 45 Pd 46 Ag 47 Cd 48 In 49 Sn 50 Sb 51 Te 52 I 53 Xe 54 Cs 55 Ba 56 Hf 72 Ta 73 W 74 Re 75 Os 76 Ir 77 Pt 78 Au 79 Hg 80 Tl 81 Pb 82 Bi 83 Po 84 At 85 Rn 86 Fr 87 Ra 88 Rf 104 Db 105 Sg 106 Bh 107 Hs 108 Mt 109 Mg 12 Ce 58 Pr 59 Nd 60 Pm 61 Sm 62 Eu 63 Gd 64 Tb 65 Dy 66 Ho 67 Er 68 Tm 69 Yb 70 Lu 71 Th 90 Pa 91 U 92 Np 93 Pu 94 Am 95 Cm 96 Bk 97 Cf 98 Es 99 Fm 100 Md 101 No 102 Lr 103 La 57 Ac 89 1 2 3 4 5 6 7   METALS Nonmetals Metalloids

23. What are semiconductors used in?

24. Nonmetals Brittle Do not conduct electricity

25. Nonmetals Most are poisonous Fairly reactive – react with alkali metals (eg) Na + and Cl - Halogens

26. Chlorine Gas was used as a chemical weapon during World War I. It was used by the Germans in World War II.

27. Chlorine Gas The Germans were the first to use Chlorine gas at Ypres in 1915 Chlorine gas is a lung irritant The symptoms of gas poisoning are bright red lips, and a blue face People affected die a slow death by suffocation Decades later men who thought they had survived the war died from lung diseases such as Emphysema

28. CHLORINE

29. Nonmetals Unreactive Gases at room temperature Noble Gases

30. Jellyfish lamps made with noble gases artist- Eric EhlenbergerEric Ehlenberger

31. Colors Noble Gases produce in lamp tubes: Ne (Neon): orange-red Ar (Argon): pale lavender He (Helium): pale peach Kr (Krypton): pale silver Xe (Xenon): pale, deep blue

32. Lanthanide Series Actinide Series The lanthanide series can be found naturally on Earth. Only one element in the series is radioactive. Also called rare-earth metals or inner-transition elements. You might find some of these elements in superconductors, glass production, or lasers The actinide series is much different. They are all radioactive Some are not found in nature. Some of the elements with higher atomic numbers have only been made in labs.

33. ELEMENTS THAT EXIST AS DIATOMIC MOLECULES Remember: The “GENS” These elements exist as PAIRS when ALONE. Hydrogen (H 2 ) Nitrogen (N 2 ) Oxygen (O 2 ) Halogens (F 2, Cl 2, Br 2, I 2 ) (P 4 and S 8 )

34. Diatomic Elements H2H2 N2N2 O2O2 F2F2 Cl 2 Br 2 I2I2 Tl At S Li Na K Fr Be Mg Ca Ra Sc Ac He Ne Ar Kr Rn Ti V Cr Mn Fe Co Ni Cu ZnGa Ge As Se Rb Sr Y Xe Zr Nb Mo Tc Ru Rh Pd Ag CdIn Sn Sb Te Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Pb Bi Po Al Si P B C Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er TmYb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm MdNo Lr S Tl