For the elements in column 1,2 and 13-18 the atoms in the same column have the same amount of outermost electrons, called valence electrons.
Atoms in column 1 (H, Li and Na for example) have 1 valence electron.
Column 2 have 2 valence electrons, 13 have 3, 14 have 4 and so on.
An atom can have at a maximum 8 valence electrons (this becomes a bit more complicated after the third row). And the "goal" of an atom is to have its outermost electron filled (either by emptying the outermost shell making the filled, second outermost shell the outermost or by filling the outermost shell).
This affects which charge ion of the columns produce
Column 1 produce 1+, column 2 2+, column 13 3+, column 15 3-, column 16 2- and column 17 1-.
The column of the atom also affect the amount of bonds an atom can participate in but this is not as simple.
One reason the periodic table of the elements is so useful is that it is a means of arranging elements according to their similar properties. This is what is meant by periodicity or periodic table trends.
There are multiple ways of grouping the elements, but they are commonly divided into metals, semimetals (metalloids), and nonmetals. You'll find more specific groups, like transition metals, rare earths, alkali metals, alkaline earth, halogens, and noble gasses.
Groups in the Periodic Table of Elements
Click on an element to read about the chemical and physical properties of the group to which that element belongs.
Alkali Metals
- Less dense than other metals
- One loosely bound valence electron
- Highly reactive, with reactivity increasing moving down the group
- The largest atomic radius of elements in their period
- Low ionization energy
- Low electronegativity
Alkaline Earth Metals
- Two electrons in the valence shell
- Readily form divalent cations
- Low electron affinity
- Low electronegativity
Transition Metals
The lanthanides (rare earth) and actinides are also transition metals. The basic metals are similar to transition metals but tend to be softer and to hint at nonmetallic properties. In their pure state, all of these elements tend to have a shiny, metallic appearance. While there are radioisotopes of other elements, all of the actinides are radioactive.
- Very hard, usually shiny, ductile, and malleable
- High melting and boiling points
- High thermal and electrical conductivity
- Form cations (positive oxidation states)
- Tend to exhibit more than one oxidation state
- Low ionization energy
Metalloids or Semimetals
- Electronegativity and ionization energy intermediate between that of metals and nonmetals
- May possess a metallic luster
- Variable density, hardness, conductivity, and other properties
- Often make good semiconductors
- Reactivity depends on the nature of other elements in the reaction
Nonmetals
The halogens and noble gases are nonmetals, although they have their own groups, too.
- High ionization energy
- High electronegativity
- Poor electrical and thermal conductors
- Form brittle solids
- Little if any metallic luster
- Readily gain electrons
Halogens
The halogens exhibit different physical properties from each other but do share chemical properties.
- Extremely high electronegativity
- Very reactive
- Seven valence electrons, so elements from this group typically exhibit a -1 oxidation state
Noble Gases
The noble gasses have complete valence electron shells, so they act differently. Unlike other groups, noble gasses are unreactive and have very low electronegativity or electron affinity.
Periodic Table of Element Groups
Click on the element symbol in the table for further information.
1
IA
1A18
VIIIA
8A1
H
1.0082
IIA
2A13
IIIA
3A14
IVA
4A15
VA
5A16
VIA
6A17
VIIA
7A2
He
4.0033
Li
6.9414
Be
9.0125
B
10.816
C
12.017
N
14.018
O
16.009
F
19.0010
Ne
20.1811
Na
22.9912
Mg
24.313
IIIB
3B4
IVB
4B5
VB
5B6
VIB
6B7
VIIB
7B8
←
←9
VIII
810
→
→11
IB
1B12
IIB
2B13
Al
26.9814
Si
28.0915
P
30.9716
S
32.0717
Cl
35.4518
Ar
39.9519
K
39.1020
Ca
40.0821
Sc
44.9622
Ti
47.8823
V
50.9424
Cr
52.0025
Mn
54.9426
Fe
55.8527
Co
58.4728
Ni
58.6929
Cu
63.5530
Zn
65.3931
Ga
69.7232
Ge
72.5933
As
74.9234
Se
78.9635
Br
79.9036
Kr
83.8037
Rb
85.4738
Sr
87.6239
Y
88.9140
Zr
91.2241
Nb
92.9142
Mo
95.9443
Tc
(98)44
Ru
101.145
Rh
102.946
Pd
106.447
Ag
107.948
Cd
112.449
In
114.850
Sn
118.751
Sb
121.852
Te
127.653
I
126.954
Xe
131.355
Cs
132.956
Ba
137.3*72
Hf
178.573
Ta
180.974
W
183.975
Re
186.276
Os
190.277
Ir
190.278
Pt
195.179
Au
197.080
Hg
200.581
Tl
204.482
Pb
207.283
Bi
209.084
Po
(210)85
At
(210)86
Rn
(222)87
Fr
(223)88
Ra
(226)**104
Rf
(257)105
Db
(260)106
Sg
(263)107
Bh
(265)108
(265)109
Mt
(266)110
Ds
(271)111
Rg
(272)112
Cn
(277)113
Uut
--114
Fl
(296)115
Uup
--116
Lv
(298)117
Uus
--118
Uuo
--
*
Lanthanide
Series57
La
138.958
Ce
140.159
Pr
140.960
Nd
144.261
Pm
(147)62
150.463
Eu
152.064
Gd
157.365
Tb
158.966
Dy
162.567
Ho
164.968
Er
167.369
Tm
168.970
Yb
173.071
Lu
175.0**
Actinide
Series89
Ac
(227)90
Th
232.091
Pa
(231)92
U
(238)93
Np
(237)94
Pu
(242)95
Am
(243)96
Cm
(247)97
Bk
(247)98
Cf
(249)99
Es
(254)100
Fm
(253)101
Md
(256)102
No
(254)103
Lr
(257)
- Alkali Metal
- Alkaline Earth
- Transition Metal
- Basic Metal
- Semi Metal
- Nonmetal
- Halogen
- Noble Gas
- Lanthanide
- Actinide
Cite this Article
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Helmenstine, Anne Marie, Ph.D. "Periodic Table of Element Groups." ThoughtCo. //www.thoughtco.com/periodic-table-of-element-groups-4006869 (accessed January 2, 2023).