Periodic table

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The periodic table of the chemical elements is a tabular display of the known chemical elements. The elements are arranged by electron structure so that many chemical properties vary regularly across the table. Each element is listed by its atomic number and chemical symbol.

The standard table provides the necessary basics. There are also other methods for displaying the chemical elements for more details or different perspectives.

Table of contents

1 Groups

1.1 Group numbers

2 Standard periodic table
3 Other methods for displaying the chemical elements
4 Explanation of the structure of the periodic table
5 History
6 Further resources
7 See also
8 External links

Groups

A group is a vertical column in the periodic table of the elements. There are 18 groups in the standard periodic table. Elements in a group have similar configurations of their valence shell electrons, which gives them similar properties.

Group numbers

There are three systems of group numbers; one using Arabic numerals and the other two using Roman numerals. The Roman numeral names are the original traditional names of the groups; the Arabic numeral names are a newer naming scheme recommended by International Union of Pure and Applied Chemistry (IUPAC). The IUPAC scheme was developed to replace both older Roman numeral systems as they confusingly used the same names to mean different things.

Standard periodic table

Group &rarr

Period &darr

1
H

2
He

3
Li

4
Be

5
B

6
C

7
N

8
O

9
F

15
P

16
S

19
K

23
V

39
Y

53
I

74
W

* Lanthanides

** Actinides

92
U

Chemical Series of the Periodic Table
Alkali metals	Alkaline earths	Lanthanide	Actinides	Transition metals
Poor metals	Metalloids	Nonmetals	Halogens	Noble gases

Color coding for atomic numbers:

Elements numbered in blue are liquids at standard temperature and pressure (STP);
those in green are gases at STP;
those in black are solid at STP;
those in red are synthetic (all are solid at STP).
those in gray have not yet been discovered (they also have muted fill colors indicating the likely chemical series they would fall under).

Other methods for displaying the chemical elements

The standard table (same as above) provides the basics.
Alternate Table
Anti table
The big table provides the basics plus full element names.
The huge table provides the basics plus full element names and atomic masses.
Wide Table
Extended Table
Table in Chinese
Electron Configurations
Metals and Non Metals
Periodic table filled by blocks
List of elements by name
List of elements by symbol
List of elements by atomic number
List of elements by boiling point
List of elements by melting point
List of elements by density
List of elements by atomic mass

And here is the periodic table for magnetic resonance.

Explanation of the structure of the periodic table

The number of electron shells an atom has determines what period it belongs to. Each shell is divided into different subshells, which as atomic number increases are filled in roughly this order:

1s

2s           2p

3s           3p

4s        3d 4p

5s        4d 5p

6s     4f 5d 6p

7s     5f 6d 7p

8s  5g 6f 7d 8p

...

Hence the structure of the table. Since the outermost electrons determine chemical properties, those tend to be similar within groups. Elements adjacent to one another within a group have similar physical properties, despite their significant differences in mass. Elements adjacent to one another within a period have similar mass but different properties.

For example, very near to nitrogen (N) in the second period of the chart are carbon (C) and oxygen (O). Despite their similarities in mass (they differ by only a few atomic mass units), they have extremely different properties, as can be seen by looking at their allotropes: diatomic oxygen is a gas that supports burning, diatomic nitrogen is a gas that does not support burning, and carbon is a solid which can be burnt (yes, diamonds can be burnt!).

In contrast, very near to chlorine (Cl) in the next-to-last group in the chart (the halogens) are fluorine (F) and bromine (Br). Despite their dramatic differences in mass within the group, their allotropes have very similar properties: They are all highly corrosive (meaning they combine readily with metals to form metal halide salts); chlorine and fluorine are gases, while bromine is a very low-boiling liquid; chlorine and bromine at least are highly colored.

History

Main article: History of the periodic table

The original table was created without a knowledge of the inner structure of atoms: if one orders the elements by atomic mass, and then plots certain other properties against atomic mass, one sees an undulation or periodicity to these properties as a function of atomic mass. The first to recognize these regularities was the German chemist Johann Wolfgang Döbereiner who, in 1829, noticed a number of triads of similar elements:

Some triads
Element Atomic mass Density
chlorine 35.5 0.00156 g/cm³
bromine 79.9 0.00312 g/cm³
iodine 126.9 0.00495 g/cm³

calcium 40.1 1.55 g/cm³
strontium 87.6 2.6 g/cm³
barium 137 3.5 g/cm³

Some triads
Element	Atomic mass	Density
chlorine	35.5	0.00156 g/cm³
bromine	79.9	0.00312 g/cm³
iodine	126.9	0.00495 g/cm³

calcium	40.1	1.55 g/cm³
strontium	87.6	2.6 g/cm³
barium	137	3.5 g/cm³

This was followed by the English chemist John Alexander Reina Newlands, who in 1865 noticed that the elements of similar type recurred at intervals of eight, which he likened to the octaves of music, though his law of octaves was ridiculed by his contemporaries. Finally, in 1869, the German Lothar Meyer and the Russian chemist Dmitry Ivanovich Mendeleev almost simultaneously developed the first periodic table, arranging the elements by mass. However, Mendeleev plotted a few elements out of strict mass sequence in order to make a better match to the properties of their neighbours in the table, corrected mistakes in the values of several atomic masses, and predicted the existence and properties of a few new elements in the empty cells of his table. Mendeleev was later vindicated by the discovery of the electronic structure of the elements in the late 19th and early 20th century.

Further resources

Mazurs, E.G., "Graphical Representations of the Periodic System During One Hundred Years". University of Alabama Press, Alabama. 1974.
Bouma, J., "An Application-Oriented Periodic Table of the Elements". J. Chem. Ed., 66 741 (1989).

External links

"Presentation forms of the periodic table". Western Oregon University.
"A Brief History of the Development of Periodic Table". Western Oregon University.
"Visual Periodic Table". ChemSoc.org.
Barbalace, Kenneth L., "Biochemical Periodic Tables". KLBProductions.com.
"Periodic table (professional edition)". WebElements.
Counterman, Craig, "Periodic Table of the Elements : Atomic Number". MIT Course 3.091.
Holler, F. James, and John P. Selegue, "Periodic Table of Comic Books". Department of Chemistry, University of Kentucky. 1996-2002.
Heilman, Chris, "The Pictorial Periodic Table". (Includes alternate styles: Stowe, Benfey, Zmaczynski, Giguere, Tarantola, Filling, Mendeleev)
"Periodic table". Los Alamos National Laboratory's Chemistry Division.
"Periodic Table of the Fermi Surfaces of Elemental Solids". The Fermi Surface Database
"Interactive NMR Frequency Map". Texas A&M.
"Periodic Table Elements". Israel Science and Technology Directory. 1999-2004. (sorted by physical characteristics)
Barthelmy, David, "Periodic table" Mineralogy Database. (mineral emphasis)
Gray, Theodore, "Wooden Periodic Table Table" (with samples)
"Periodic table applet". Dartmouth College. (Java)
Jacobs, Bob, "Periodic Tables (in case you were thinking that the Internet needed one more)". The Chemistry Coach.
"Periodic Table.Com".