1. Groups of Elements 1A 8A H He 2A 3A 4A 5A 6A 7A Li Be B C N O F Ne Na
Alkali metals 5A
Nitrogen group H 1 2A
Alkali earth metals 6A
Oxygen group He 2 1 1 2A
Transition metals 7A
Halogens 3A 4A 5A 6A 7A 3A
Boron group 8A
Noble gases Li 3 Be 4 B 5 C 6 N 7 O 8 F 9 Ne 10 2 2 4A
Carbon group
Hydrogen
Inner transition metals Na 11 Mg 12 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 3 3 8B 3B 4B 5B 6B 7B 1B 2B 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 4 4 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 5 5 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 6 6 * * Fr 87 Ra 88 Rf
104 Db
105 Sg
106 Bh
107 Hs
108 Mt
109 7 7 W W La 57 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 * Ac 89 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 W

2. Groups of Elements 1 18 He Ne Ar Kr Xe Rn 2 13 14 15 16 17 Li Na K Rb10 Ar 18 Kr 36 Xe 54 Rn 86 2 13 14 15 16 17 Li 3 Na 11 K 19 Rb 37 Cs 55 Fr 87 Be 4 Ca 20 Sr 38 Ba 56 Ra 88 Mg 12 N 7 P 15 As 33 Sb 51 Bi 83 O 8 S 16 Se 34 Te 52 Po 84 F 9 Cl 17 Br 35 I 53 At 85
The Noble Gases
At the start of the 1890s, no one had any idea that there was a separate group of gases in the periodic table, the noble gases. Noble gases are familiar to us from their use in neon signs and helium balloons. By 1900 this whole new group had been identified and isolated. While trying to determine an accurate atomic mass for nitrogen, British physicist Lord Raleigh ( ) discovered that nitrogen prepared from ammonia was noticeably lighter than nitrogen that came from the atmosphere. He and William Ramsay ( ) both studied “atmospheric” nitrogen. By removing the nitrogen from it, they produced a tiny quantity of another gas. Since it did not react with anything they called it argon, from the Greek word for lazy. The discovery of helium followed a year later in Ramsay and his assistant Morris Travers ( ) then started to search for additional elements in this new group. They attempted this by fractional distillation of large quantities of liquid air and argon. In 1898, their efforts were rewarded; they had prepared krypton, neon, and xenon.
Eyewitness Science “Chemistry” , Dr. Ann Newmark, DK Publishing, Inc., 1993, pg 32 1
Alkali metals 16
Oxygen family 2
Alkaline earth metals 17
Halogens 15
Nitrogen family 18
Noble gases
Dorin, Demmin, Gabel, Chemistry The Study of Matter , 3rd Edition, 1990, page 367

3. Chemistry of the Groups1A 8A H 1 He 2 1 1 2A 3A 4A 5A 6A 7A Li 3 Be 4
Transition Metals B 5 C 6 N 7 O 8 F 9 Ne 10 2 2 Na 11 Mg 12 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 3 3 8B 3B 4B 5B 6B 7B 1B 2B 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 4 4 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 5 5 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 6 6 * *
Elements in each column of the d block have vertical similarities in chemical behavior and also display strong horizontal similarities.
Horizontal trends compete with vertical trends.
Transition metals have multiple oxidation states that are separated by only one electron.
Group-6 elements chromium, molybdenum, and tungsten illustrate the competition that occurs between these horizontal and vertical trends — transition metals in Group 6 have different tendencies to achieve their maximum oxidation state.
Groups 3 (scandium, lanthanum, actinium), 11 (copper, silver, gold) and 12 (zinc, cadmium, mercury) are the only transition metal groups in which the oxidation state predicted by the valence-electron configuration dominates the chemistry of the group.
Transition metals contain partially filled sets of d orbitals and the lanthanides and actinides are those groups in which f orbitals are being filled.
These groups exhibit strong horizontal similarities in behavior.
Many of the transition metals form M2+ ions.
Chemistry of lanthanides and actinides is dominated by M3+ ions. Fr 87 Ra 88 Rf
104 Db
105 Sg
106 Bh
107 Hs
108 Mt
109 7 7 W W La 57 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
Lanthanides * Ac 89 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
Actinides W