Group (periodic table)

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Group periodic table
Groups in periodic table | Image: Learnool

In chemistry, a group (also referred to as a family) is a column of elements in the periodic table. Each group contains elements that share the same number of valence electrons and exhibit similar chemical and physical properties. The periodic table is divided into 18 numbered groups, each having a unique set of elements. Groups can also be identified by the topmost element in the group, or by a specific name.

The 18 groups in the periodic table are numbered from 1 to 18 according to the modern numbering system recommended by the International Union of Pure and Applied Chemistry (IUPAC) since 1988. However, there are different systems of group numbering which can cause confusion as the same number may be assigned to different groups depending on the system being used. Nevertheless, the modern numbering system is generally accepted by the chemistry community.

Groups 1 to 2 are known as the s-block, groups 3 to 12 are known as the d-block, groups 13 to 18 are known as the p-block, and the 14 f-block columns are located between groups 2 and 3, but are not numbered. Each block contains elements that have the same number of valence electrons in their outermost shells. The properties of elements within a group vary with their atomic number, and the properties of elements in the same group are more similar to each other than to those in other groups.

In addition to being identified by number, each group may also have a specific name. For example, group 1 is commonly known as the alkali metals, while group 17 is known as the halogens. These names are used to describe the common properties and behavior of elements in that particular group. It is important to note that not all groups have a specific name, and some elements may belong to multiple groups depending on the criteria used for classification.

On periodic table

group 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18
period
1 1
H
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Hydrogen
2
He
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Helium
2 3
Li
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Lithium
4
Be
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Beryllium
5
B
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Boron
6
C
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Carbon
7
N
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Nitrogen
8
O
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Oxygen
9
F
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Fluorine
10
Ne
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Neon
3 11
Na
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Sodium
12
Mg
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Magnesium
13
Al
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Aluminium
14
Si
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Silicon
15
P
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Phosphorus
16
S
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Sulfur
17
Cl
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Chlorine
18
Ar
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Argon
4 19
K
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Potassium
20
Ca
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Calcium
21
Sc
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Scandium
22
Ti
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Titanium
23
V
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Vanadium
24
Cr
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Chromium
25
Mn
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Manganese
26
Fe
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Iron
27
Co
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Cobalt
28
Ni
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Nickel
29
Cu
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Copper
30
Zn
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Zinc
31
Ga
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Gallium
32
Ge
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Germanium
33
As
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Arsenic
34
Se
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Selenium
35
Br
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Bromine
36
Kr
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Krypton
5 37
Rb
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Rubidium
38
Sr
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Strontium
39
Y
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Yttrium
40
Zr
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Zirconium
41
Nb
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Niobium
42
Mo
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Molybdenum
43
Tc
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Technetium
44
Ru
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Ruthenium
45
Rh
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Rhodium
46
Pd
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Palladium
47
Ag
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Silver
48
Cd
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Cadmium
49
In
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Indium
50
Sn
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Tin
51
Sb
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Antimony
52
Te
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Tellurium
53
I
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Iodine
54
Xe
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Xenon
6 55
Cs
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Caesium
56
Ba
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Barium
72
Hf
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Hafnium
73
Ta
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Tantalum
74
W
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Tungsten
75
Re
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Rhenium
76
Os
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Osmium
77
Ir
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Iridium
78
Pt
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Platinum
79
Au
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Gold
80
Hg
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Mercury
81
Tl
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Thallium
82
Pb
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Lead
83
Bi
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Bismuth
84
Po
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Polonium
85
At
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Astatine
86
Rn
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Radon
7 87
Fr
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Francium
88
Ra
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Radium
104
Rf
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Rutherfordium
105
Db
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Dubnium
106
Sg
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Seaborgium
107
Bh
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Bohrium
108
Hs
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Hassium
109
Mt
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Meitnerium
110
Ds
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Darmstadtium
111
Rg
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Roentgenium
112
Cn
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Copernicium
113
Nh
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Nihonium
114
Fl
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Flerovium
115
Mc
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Moscovium
116
Lv
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Livermorium
117
Ts
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Tennessine
118
Og
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Oganesson
57
La
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Lanthanum
58
Ce
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Cerium
59
Pr
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Praseodymium
60
Nd
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Neodymium
61
Pm
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Promethium
62
Sm
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Samarium
63
Eu
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Europium
64
Gd
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Gadolinium
65
Tb
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Terbium
66
Dy
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Dysprosium
67
Ho
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Holmium
68
Er
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Erbium
69
Tm
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Thulium
70
Yb
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Ytterbium
71
Lu
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Lutetium
89
Ac
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Actinium
90
Th
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Thorium
91
Pa
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Protactinium
92
U
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Uranium
93
Np
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Neptunium
94
Pu
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Plutonium
95
Am
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Americium
96
Cm
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Curium
97
Bk
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Berkelium
98
Cf
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Californium
99
Es
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Einsteinium
100
Fm
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Fermium
101
Md
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Mendelevium
102
No
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Nobelium
103
Lr
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Lawrencium
group
– alkali metal – post-transition metal
– alkaline earth metal – metalloid
– lanthanide – reactive nonmetal
– actinide – noble gas
– transition metal – unknown properties

The periodic table consists of 18 numbered groups, organized from left to right. The main groups include metals (which consist of alkali metals, alkaline earth metals, lanthanides, actinides, transition metals, and post-transition metals), metalloids, and nonmetals (which include reactive nonmetals and noble gases).

However, the f-block elements between groups 2 and 3 (lanthanides and actinides) do not have any group number. These elements are commonly referred to as the inner transition metals and are placed below the main table to conserve space.

In addition, the elements with atomic numbers 109 to 118 are referred to as unknown chemical properties, because they are highly unstable and can only be produced artificially in a lab.

Group names

IUPAC name
Old IUPAC name (Europe)
CAS name (U.S.)
Group (or family) name
IUPAC trivial name
Other names
Group 1 â… A â… A lithium group hydrogen and alkali metals
Group 2 â…¡A â…¡A beryllium group alkaline earth metals
Group 3 â…¢A â…¢B scandium group
Group 4 â…£A â…£B titanium group
Group 5 â…¤A â…¤B vanadium group
Group 6 â…¥A â…¥B chromium group
Group 7 â…¦A â…¦B manganese group
Group 8 â…§ â…§B iron group
Group 9 â…§ â…§B cobalt group
Group 10 â…§ â…§B nickel group
Group 11 â… B â… B copper group coinage metals
Group 12 â…¡B â…¡B zinc group volatile metals
Group 13 â…¢B â…¢A boron group triels (from the Greek word “tri”, three, â…¢) icosagens
Group 14 â…£B â…£A carbon group tetrals (from the Greek word “tetra”, four, â…£) crystallogens
adamantogens
merylides
Group 15 â…¤B â…¤A nitrogen group pnictogens
pentels (from the Greek word “penta”, five, â…¤)
Group 16 â…¥B â…¥A oxygen group chalcogens
Group 17 â…¦B â…¦A fluorine group halogens
Group 18 0 â…§A helium group or neon group noble gases aerogens

Properties and trends

The properties of elements in the periodic table are fundamental to the study of chemistry. Each group in the periodic table shares similar chemical and physical properties, making it a useful tool for predicting the behavior of elements. For example, the alkali metals in group 1, including lithium, sodium, and potassium, all have one valence electron, which makes them highly reactive and good conductors of heat and electricity.

The physical and chemical properties of elements in each group are unique and often have practical applications. For example, the alkaline earth metals in group 2, including magnesium and calcium, are important components in the manufacturing of construction materials and batteries. The noble gases in group 18, including helium and neon, are used in lighting and as insulators due to their low reactivity.

Trends in the periodic table, such as atomic radius and electronegativity, are important for understanding the behavior of elements in each group. For example, as you move from left to right across a period, the atomic radius decreases due to increasing nuclear charge. Similarly, as you move from the bottom to the top of a group, the electronegativity increases, which affects the reactivity of the elements.

The trends in the periodic table can be further explained with the help of examples. For instance, the halogens in group 17, including chlorine and iodine, become less reactive as you move from top to bottom. This is because the atomic radius increases, making it harder for them to attract electrons and form bonds. Another example is the transition metals in group 3 to group 12, including iron and copper, which become less reactive as you move from left to right. This is because the electronegativity of the elements increases, making it harder for them to lose electrons and form bonds.

Naming and numbering

The naming and numbering of groups in the periodic table has been a subject of discussion and has undergone evolution over time. There are three different systems of group numbering that have been used in the past. However, the modern numbering system has been recommended by the International Union of Pure and Applied Chemistry (IUPAC) since 1988, and it is widely used today. In this system, groups are numbered from 1 to 18, with the f-block elements (lanthanides and actinides) not assigned any number.

Before the modern system, there were two different systems of naming and numbering of groups. The first system was developed by the Chemical Abstract Service (CAS) and was more popular in the United States. This system assigned group numbers from â… A to â…§A for the main-group elements and from â… B to â…§B for the transition elements. The second system was developed by IUPAC and was more popular in Europe. This system used Roman numerals with the letters A and B to distinguish between the left (A) and right (B) side of the periodic table.

The modern system of group numbering is now widely accepted by the chemistry community, although there is still some debate over the placement of elements 1 and 2 (hydrogen and helium) and the inner transition metals. Despite this, the modern system has several advantages, including being more systematic and easier to use than the previous systems.

In addition to the numbered groups, some groups in the periodic table are also identified by their topmost element or a specific name. For example, group 16 is commonly referred to as the “oxygen group” or “chalcogens,” while group 18 is called the “noble gases.” Another example is the “iron group,” which usually refers to group 8 but can also include iron, cobalt, and nickel or some other set of elements with similar chemical properties.

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Learnool.com was founded by Deep Rana, who is a mechanical engineer by profession and a blogger by passion. He has a good conceptual knowledge on different educational topics and he provides the same on this website. He loves to learn something new everyday and believes that the best utilization of free time is developing a new skill.

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