2. Organization of The Periodic Table Mrs. Russotto

3. Mendeleev’s Periodic Table Dmitri Mendeleev Mendeleev put the elements in order of relationships of reactivity & increasing mass, discovering the elements could be placed in columns of similar properties. His table had holes in it that allowed for other elements to be discovered at a later time. The Modern Periodic Table Henry Moseley reorganized the Periodic Table in order of increasing atomic number. This removed the problems in Mendeleev’s table.

4. Parts of the Periodic Table Metals Nonmetals Metalloids

5. Properties of Metals Good conductors of heat and electricity Malleable Examples: Lead, Calcium, Aluminum Ductile Have high tensile strength Have luster

6. 50 Sn 118.69 82 Pb 207.19 83 Bi 208.98 13 Al 26.981 31 Ga 69.72 49 In 114.82 81 Tl 204.37 84 Po (210) Metals

7. Properties of Nonmetals Carbon, the graphite in “lead pencils” is a great example of a nonmetallic element. Nonmetals are poor conductors of heat and electricity. Nonmetals tend to be brittle Many nonmetals are gases at room temperature Examples: Argon, Oxygen, Iodine, Phosphorus

8. 7 N 14.006 15 P 30.973 6 C 12.011 Nonmetals 8 O 15.999 16 S 32.064 34 Se 78.96

9. Properties of Metalloids Metalloids straddle the border between metals and nonmetals on the periodic table. They have properties of both metals and nonmetals. Metalloids are more brittle than metals, less brittle than most nonmetals. Metalloids are semiconductors of electricity. Some metalloids possess metallic luster Examples: Silicon and Germanium

10. 5 B 10.811 32 Ge 72.61 14 Si 28.085 51 Sb 121.76 33 As 74.92 52 Te 127.60 Metalloids

11. 1 H 1.008 3 Li 6.941 11 Na 22.99 19 K 39.10 37 Rb 85.47 55 Cs 132.9 87 Fr (223) ALKALI METALS Group 1A Characteristics 1.The most reactive metals, with the exception of hydrogen – need to be stored under oil to prevent reactions with oxygen. 2.They are soft enough to be cut by a knife. 3.They lose their one valence (outermost) electron to nonmetals. 4.React violently with water. 5.React with halogens to form salts. Electron configuration ends in s 1

12. 4 Be 9012 12 Mg 24.31 20 Ca 40.08 38 Sr 87.62 56 Ba 137.3 88 Ra 226 Alkaline Earth Metals Group 2A Characteristics 1.Harder, denser, stronger & have higher melting points than Alkali Metals 2.These elements are also very reactive (not as reactive as Group 1), losing their two valence electrons to nonmetals. Electron configuration ends in s 2

13. 9 F 18.998 17 Cl 35.453 35 Br 79.909 53 I 126.90 85 At (210) Group 7A (or 17) Characteristics: 1.These elements all form diatomic molecules. Ex: F 2, Cl 2 2.With the exception of Astatine, they all react with metals to form salts. (The most reactive nonmetals on the table) Ex: NaCl, MgBr 2 3.They want to gain one electron to the outermost level to become stable. Electron configuration ends in p 5

14. 2 He 4.0026 10 Ne 20.179 18 Ar 39.498 36 Kr 83.80 54 Xe 131.30 86 Rn (222) Group 8A (or 18) Characteristics: 1.These elements exist under normal conditions as gases – noble gases that have little chemical reactivity. (inert) 2.They rarely form compounds since they do not need to gain or lose any electrons. 3.All other elements want to gain or lose electrons to have an electron configuration of a noble gas. Electron configuration ends in p 6

15. 39 Y 88.91 57 La 138.9 89 Ac (227) 21 Sc 44.96 73 Ta 180.9 105 Db 41 Nb 92.91 23 V 50.94 72 Hf 178.9 104 Rf 40 Zr 91.22 22 Ti 47.88 42 Mo 95.94 74 W 183.9 24 Cr 52.00 106 Sg 48 Cd 112.4 30 Zn 65.38 80 Hg 200.6 47 Ag 107.9 29 Cu 63.55 79 Au 197.0 111 Uuu 46 Pd 106.4 28 Ni 58.69 78 Pt 195.1 110 Ds 45 Rh 102.9 27 Co 58.93 77 Ir 192.2 109 Mt 44 Ru 101.1 26 Fe 55.85 76 Os 190.2 108 Hs 43 Tc (98) 25 Mn 54.94 75 Re 186.2 107 Bh d-block Characteristics: 1.They lose their 2 valence electrons in reactions (a few exceptions). 2.Not as reactive but are harder, denser, and have higher melting points than the Alkali & Alkaline Earth Metal families. 3.All are solid at room temperature with the exception of mercury.

16. 64 Gd 157.2 65 Tb 158.9 66 Dy 162.5 67 Ho 164.93 68 Er 167.2 69 Tm 168.9 58 Ce 140.1 59 Pr 140. 60 Nd 144. 61 Pm (147) 62 Sm 150.35 63 Eu 151.9 70 Yb 173.04 Characteristics: 1.Members of the Rare Earth Metals 2.Shiny, reactive metals—some having practical uses. Electron configuration ends in 4f ?

17. 96 Cm (247) 97 Bk (247) 98 Cf (252) 99 Es (254) 100 Fm (257) 101 Md (257) 90 Th 232.0 91 Pa (231 92 U 238. 93 Np (237) 94 Pu (234) 95 Am (243) 102 No (255) Characteristics: 1.Members of the Rare Earth Metals 2.They have an unstable arrangement of protons and neutrons in the nucleus. 3.All have radioactive forms. Electron configuration ends in 5f ?

18. Alkali Alkaline Earth Transition Metals Metalloids Nonmetals HalogensNoble Gases Lanthanide Actinide