Organization of The Periodic Table

1. Organization of The Periodic Table Mrs. Russotto

2. ALKALI 1 H 1.008 METALS 3 Li 6.941 • Group 1A Characteristics • The most reactive metals, with the exception of hydrogen – need to be stored under oil to prevent reactions with oxygen. • They are soft enough to be cut by a knife. • They lose their one valence (outermost) electron to nonmetals. • React violently with water. • React with halogens to form salts. 11 Na 22.99 19 K 39.10 37 Rb 85.47 55 Cs 132.9 Electron configuration ends in s1 87 Fr (223)

3. 4 Be 9012 • Group 2A Characteristics • Harder, denser, stronger & have higher melting points than Alkali Metals • These elements are also very reactive (not as reactive as Group 1), losing their two valence electrons to nonmetals. 12 Mg 24.31 20 Ca 40.08 38 Sr 87.62 Electron configuration ends in s2 Alkaline 56 Ba 137.3 Earth Metals 88 Ra 226

4. Halogens 9 F 18.998 17 Cl 35.453 35 Br 79.909 53 I 126.90 85 At (210) • Group 7A (or 17) Characteristics: • These elements all form diatomic molecules. Ex: F2, Cl2 • With the exception of Astatine, they all react with metals to form salts. (The most reactive nonmetals on the table) Ex: NaCl, MgBr2 • They want to gain one electron to the outermost level to become stable. Electron configuration ends in p5

5. 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: • These elements exist under normal conditions as gases – noble gases that have little chemical reactivity. (inert) • They rarely form compounds since they do not need to gain or lose any electrons. • All other elements want to gain or loseelectrons to have an electron configuration of a noble gas. Noble Gases Electron configuration ends in p6

6. 21 Sc 44.96 22 Ti 47.88 23 V 50.94 24 Cr 52.00 25 Mn 54.94 26 Fe 55.85 27 Co 58.93 28 Ni 58.69 29 Cu 63.55 30 Zn 65.38 39 Y 88.91 40 Zr 91.22 41 Nb 92.91 42 Mo 95.94 43 Tc (98) 44 Ru 101.1 45 Rh 102.9 46 Pd 106.4 47 Ag 107.9 48 Cd 112.4 57 La 138.9 72 Hf 178.9 73 Ta 180.9 74 W 183.9 75 Re 186.2 76 Os 190.2 77 Ir 192.2 78 Pt 195.1 79 Au 197.0 80 Hg 200.6 89 Ac (227) 104 Rf 105 Db 106 Sg 107 Bh 108 Hs 109 Mt 110 Ds 111 Uuu TRANSITION METALS • d-block Characteristics: • They lose their 2 valence electrons in reactions (a few exceptions). • Not as reactive but are harder, denser, and have higher melting points than the Alkali & Alkaline Earth Metal families. • All are solid at room temperature with the exception of mercury.

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

8. 90 Th 232.0 91 Pa (231 92 U 238. 93 Np (237) 94 Pu (234) 95 Am (243) 96 Cm (247) 97 Bk (247) 98 Cf (252) 99 Es (254) 100 Fm (257) 101 Md (257) 102 No (255) Actinide Series • Characteristics: • Members of the Rare Earth Metals • They have an unstable arrangement of protons and neutrons in the nucleus. • All have radioactive forms. Electron configuration ends in 5f ?

9. The Periodic Table Nonmetals Noble Gases Metalloids Alkali Halogens Alkaline Earth Metals Transition Lanthanide Actinide