A cool photographic Periodic Table:
http://periodictable.com/
A fun
Quiz
Periodic Table of Elements The periodic table is the most important reference a chemist has because it puts all the known elements into a meaningful pattern. Elements are arranged left to right and top to bottom in order of increasing atomic number. This order generally goes with increasing atomic mass.
Click on an element for more information (clicks take you to the Los Alamos National Laboratory site):
| Period |
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1
IA
1A |
| 18
VIIIA
8A |
| 1 | 1
H
1.008 | 2
IIA
2A |
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| 13
IIIA
3A | 14
IVA
4A | 15
VA
5A | 16
VIA
6A | 17
VIIA
7A | 2
He
4.003 |
| 2 | 3
Li
6.941 | 4
Be
9.012 |
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| 5
B
10.81 | 6
C
12.01 | 7
N
14.01 | 8
O
16.00 | 9
F
19.00 | 10
Ne
20.18 |
| 3 | 11
Na
22.99 | 12
Mg
24.31 | 3
IIIB
3B | 4
IVB
4B | 5
VB
5B | 6
VIB
6B | 7
VIIB
7B | 8 | 9 | 10 | 11
IB
1B | 12
IIB
2B | 13
Al
26.98 | 14
Si
28.09 | 15
P
30.97 | 16
S
32.07 | 17
Cl
35.45 | 18
Ar
39.95 |
–––- VIII –––-
–––- 8 –––- |
| 4 | 19
K
39.10 | 20
Ca
40.08 | 21
Sc
44.96 | 22
Ti
47.88 | 23
V
50.94 | | | 26
Fe
55.85 | 27
Co
58.47 | 28
Ni
58.69 | | 30
Zn
65.39 | 31
Ga
69.72 | 32
Ge
72.59 | 33
As
74.92 | 34
Se
78.96 | 35
Br
79.90 | 36
Kr
83.80 |
| 5 | 37
Rb
85.47 | 38
Sr
87.62 | 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 | 49
In
114.8 | 50
Sn
118.7 | 51
Sb
121.8 | 52
Te
127.6 | 53
I
126.9 | 54
Xe
131.3 |
| 6 | 55
Cs
132.9 | 56
Ba
137.3 | 57
La*
138.9 | 72
Hf
178.5 | 73
Ta
180.9 | 74
W
183.9 | 75
Re
186.2 | 76
Os
190.2 | 77
Ir
190.2 | 78
Pt
195.1 | 79
Au
197.0 | 80
Hg
200.5 | 81
Tl
204.4 | 82
Pb
207.2 | 83
Bi
209.0 | 84
Po
(210) | 85
At
(210) | 86
Rn
(222) |
| 7 | 87
Fr
(223) | 88
Ra
(226) | 89
Ac~
(227) | 104
Rf
(257) | 105
Db
(260) | 106
Sg
(263) | 107
Bh
(262) | 108
Hs
(265) | 109
Mt
(266) | 110
Uun
() | 111
Uuu
() | 112
Uub
() |
| 114
Uuq
() |
| 116
- - -
() |
| 118
- - -
() |
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| Lanthanide Series | 58
Ce
140.1 | 59
Pr
140.9 | 60
Nd
144.2 | 61
Pm
(147) | 62
Sm
150.4 | 63
Eu
152.0 | 64
Gd
157.3 | 65
Tb
158.9 | 66
Dy
162.5 | 67
Ho
164.9 | 68
Er
167.3 | 69
Tm 168.9 | 70
Yb
173.0 | 71
Lu
175.0 |
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| Actinide Series | 90
Th
232.0 | 91
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) |
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The different rows of elements are called periods. The period number of an element signifies the highest energy level an electron in that element occupies (in the unexcited state). The number of elements in a period increases as one moves down the periodic table because as the energy level of the atom increases, the number of energy sub-levels per energy level increases. |
In 1869, the Russian chemist Mendeleev noted that the repeating patterns of behavior could be arranged in a sequence of elements. This led to the first "Periodic Table" of the elements.
Scientists and students who are familiar with the periodic table use the position in the table to extract information about individual elements.
Chemistry in a Nutshell
For a list of the element names and symbols in alphabetical order. |
Another way to explain it:
The periodic table arranges the chemical elements into a pattern so that you can predict the properties of elements based on where they are located on the table. Elements are arranged from left to right and from top to bottom in order of increasing atomic number or number of protons in the element.
Rows of elements are called periods. The period number of an element signifies the highest unexcited energy level for an electron in that element. The number of elements in a period increases as you move down the periodic table because there are more sublevels per level as the energy level of the atom increases.
Columns of elements help define element groups. Elements within a group share several common properties.
http://chemistry.about.com/library/blperiodictablekids.htm
A more complex way to explain it:
The periodic table is a chart of the elements arranged according to
the
periodic law discovered by Dmitri I.
Mendeleev and revised by Henry G. J.
Moseley. In the periodic table the elements are arranged in columns and rows according to increasing
atomic number (see the table entitled
Periodic Table). The vertical columns, or groups, are numbered from I to VIII, with a final column numbered 0. Each group is divided into two categories, or families: one called the a series (the representative, or main group, elements); the other the b series (the transition, or subgroup, elements).
All the elements in a group have the same number of
valence electrons and hence similar chemical properties.
The horizontal rows of the table are called periods. The elements of a period are characterized by the fact that they have the same number of electron shells; the number of electrons in these shells, which equals the element's atomic number, increases from left to right within each period.
In each period the lighter metals appear on the left, the heavier metals in the center, and the nonmetals on the right. Elements on the borderline between metals and nonmetals are called metalloids.Group Ia (with one valence electron) and group IIa (with two valence electrons) are called the
alkali metals and the
alkaline-earth metals, respectively.
Two series of elements branch off from group IIIb, which contains the
transition elements, or transition metals; elements 57 to 71 are called the
lanthanide series, or rare earths, and elements 89 to 103 are called the
actinide series, or radioactive rare earths; a third group, the superactinide group (elements 122—153), is predicted to fall outside the main body of the table, but none of these has yet been synthesized or isolated.
The nonmetals in group VIIa (with seven valence electrons) are called the
halogens.
The elements grouped in the final column have no valence electrons and are called the
inert gases, or noble gases, because they react chemically only with extreme difficulty.
In a relatively simple type of periodic table, each position gives the name and chemical symbol for the element assigned to that position; its atomic number; its
atomic weight (the weighted average of the masses of its stable isotopes, based on a scale in which carbon-12 has a mass of 12); and its electron configuration, i.e., the distribution of its electrons by shells.
The only exceptions are the positions of elements 103 through 116; complete information on these elements has not been compiled.
Larger and more complicated periodic tables may also include the following information for each element: atomic diameter or radius; common valence numbers or oxidation states; melting point; boiling point; density; specific heat; Young's modulus; the quantum states of its valence electrons; type of crystal form; stable and radioactive isotopes; and type of magnetism exhibited by the element (paramagnetism or diamagnetism).
See P. W. Atkins, The Periodic Kingdom: A Journey into the Land of Chemical Elements (1997).
