The periodic table

1	2	3	4	5	6	7	8	9	10	11	12	13	14	15	16	17	18
1 H 1.008																	2 He 4.003
3 Li 6.941	4 Be 9.012											5 B 10.811	6 C 12.011	7 N 14.007	8 O 15.999	9 F 18.998	10 Ne 20.180
11 Na 22.990	12 Mg 24.305											13 Al 26.982	14 Si 28.086	15 P 30.974	16 S 32.065	17 Cl 35.453	18 Ar 39.948
19 K 39.098	20 Ca 40.078	21 Sc 44.956	22 Ti 47.867	23 V 50.942	24 Cr 51.996	25 Mn 54.938	26 Fe 55.845	27 Co 58.933	28 Ni 58.693	29 Cu 63.546	30 Zn 65.38	31 Ga 69.723	32 Ge 72.63	33 As 74.922	34 Se 78.96	35 Br 79.904	36 Kr 83.798
37 Rb 85.468	38 Sr 87.62	39 Y 88.91	40 Zr 91.22	41 Nb 92.91	42 Mo 95.96	43 Tc 98.91	44 Ru 101.07	45 Rh 102.91	46 Pd 106.42	47 Ag 107.87	48 Cd 112.41	49 In 114.82	50 Sn 118.71	51 Sb 121.76	52 Te 127.6	53 I 126.90	54 Xe 131.29
55 Cs 132.91	56 Ba 137.33	57* La 138.91	72 Hf 178.49	73 Ta 180.95	74 W 183.84	75 Re 186.21	76 Os 190.23	77 Ir 192.22	78 Pt 195.08	79 Au 196.97	80 Hg 200.59	81 Tl 204.38	82 Pb 207.2	83 Bi 208.98	84 Po [209]	85 At [210]	86 Rn [222]
87 Fr 223.0	88 Ra 226.0	89* Ac 227.0	104 Rf 267.0	105 Db 268.0	106 Sg 269.0	107 Bh 270.0	108 Hs 270	109 Mt [276]	110 Ds [281]	111 Rg [280]	112 Cn [285]	113 Nh [284]	114 Fl [289]	115 Mc [288]	116 Lv [292]	117 Ts [292]	118 Og [294]

Lanthanides

58
Ce
140.12

59
Pr
140.91

60
Nd
144.24

61
Pm
[145]

62
Sm
150.36

63
Eu
151.96

64
Gd
157.25

65
Tb
158.93

66
Dy
162.5

67
Ho
164.93

68
Er
167.26

69
Tm
168.93

70
Yb
173.05

71
Lu
174.97

Actinides (radioactive elements)

90
Th
232.04

91
Pa
231.04

92
U
238.03

93
Np
[237]

94
Pu
[244]

95
Am
[243]

96
Cm
[247]

97
Bk
[247]

98
Cf
[251]

99
Es
[252]

100
Fm
[257]

101
Md
[258]

102
No
[259]

103
Lr
[262]

Metals						Metalloids	Non-Metals			Unknown
Alkaline Metals/Alkali Metals	Alkaline-Earth Metals	Transition Metals	Lanthanoids	Actinoids	Poor Metals		Nonmetals	Halogens	Noble Gases

Cells with text in red are gaseous at room temperature.
Cells with text in green are liquid at room temperature.
Cells with text in black are solid at room temperature.
Cells with a dashed red outline are not found naturally on earth.
Elements 43, 61, and 84 and greater are only known as radioactive.

Blocks

s-block

s-block consistes of group 1 and group 2 elements. their oxidation state is as per their group number. They are alkali and alkali earth metals. Helium is another s-block element but appear in last group(G18).

p-block

p-block consists of group 13-18 and among these are halogens and nobles gases.

d-block

d-block consists of transition metals from group 3-12. They are all metals and they work as bridge between s to p-block hence their name i.e. transition metals.

f-block

f-block consists of Lanthanides and Actinides far below the below the periodic table.

Subject classification: this is a chemistry resource.

How to use this periodic table

The periodic table lists all the known elements. As of 2016, following the IUPAC's (International Union of Pure and Applied Chemists) naming of nihonium, Moscovium, Tennessine(non-existence, extremely unstable), and Oganesson (elements 113, 115, 117, and 118 respectively), there are 118 elements currently known and officially named. Many of them are naturally occurring, but some were made in a laboratory and are not present in nature.

The periodic table arranges the elements according to their atomic number and fits them into a logical pattern (made by Henri Moseley in 1910), while when Russian scientist Dimitri Mendeleev (1870) created the periodic table, he arranged it by atomic mass.

There are 18 columns that divide the elements into groups with closely related chemical properties. Rows, or periods, help list elements in order of mass and atomic number. Properties of elements change in systematic ways throughout the periodic table.

Groups and Periods

The periodic table is arranged into groups (columns) and periods (rows).

Groups

Elements in the same group, or family, have similar chemical properties. Elements from the same group are found in vertical columns. Elements in the same group act similarly because they have the same valence electron configuration.

Periods

Each elements in the same period have the same number of electron shells. For example, the first period consists of Hydrogen and Helium, which both have one electron shell. While the second period have elements that have two electron shells (the first electron shell contains two electrons, and the second shell can hold up to eight). As you read across the period, the elements in the period increase with electrons on their electron shell (they do not increase in electron shell if you go left to right on a period in the periodic table, only the electrons on the electron shell increase).

So, Lithium has one electron on the outer shell while Beryllium has two electrons on its outer shell (while the 1st shell is full). By the time you get to Neon, the electron shells are completely full!

Non-metals

Non-metals are found on the top-right corner of the p-block elements. These elements tend to gain electrons when forming a bond with metals or share electrons between two non-metals to form a covalent bond.

Alkaline Metals

Alkaline metals are known as the most reactive metals. This can be especially observed by their reaction with water, for example. Their reactivity is attributed to the low ionization energy of the outermost electron in the atom (one valence electron). Their most common oxidative state is +1. They tend to lose 1 electron to complete their outer shells. Reactivity increases down the group, which explains why Francium is the most reactive metal. Francium reacts easily due to its low ionization energy. In the electron configuration of Francium the valence electron is at very far distance so that's why electron need very less energy to emit that electron (due to less attraction force) . And this is also a reason for its lowest ionisation energy.

Alkaline-Earth Metals

Alkali-Earth Metals have the second lowest ionization energy. Their most common oxidation state is +2. According to Moseley's Period table, These elements are found in 2nd Group.

Transition Metals

The atoms of the transition metals have more complicated electron arrangements than other atoms. These metals have varying valence electrons, can have more than 1 oxidation state, and are always positive. The d orbitals of these elements are being filled. This group contains many well-known metals, such as iron (Fe), nickel (Ni), copper (cu), Chromium (Cr), mercury (Hg), and Gold (Au).

The Inner transition metals - the separated rows at the bottom of the periodic table, "f block", are mostly synthetic:

Lanthanides and Actinides

The Lanthanides metals - Shiny (luster), metallic elements with atomic numbers #57-71 that fill 4f orbitals.
The Actinides metals - Metallic elements with atomic numbers #89-103 that fill 5f orbitals; all are very radioactive, such as Uranium. Their radioactivity is due to the fact that any nucleus with greater than 82 protons cannot be stable(and hence they are useful for nuclear fission). Others elements in other periods are also radioactive such as polonium from per-6.

Poor Metals

The poor metals consist of aluminum, gallium, indium, thallium, tin, lead, and bismuth.

Metalloids

Metalloids roughly form a staircase line in the periodic table. This line divides metals and nonmetals. The elements around this partition have intermediate metal- and non-metal-like properties. Many of them can be used as semiconductors(due to their high control over electricity and ability to form any shape).

Halogens

All halogens are missing just one electron to fill their valence electron shell. For this reason, in most chemical reactions, halogens tend to gain one electron.

Halogens always exist as diatomic molecules (live in pairs). Going down the group, the color of elements increase; due to decreasing effective nuclear charge, atomic radius increase, and electronegativity decreases.

Hydrogen also shows property like Halogens but exceptionally According to electron configuration it's placed in 1st group of the period table.

Halogens are not always in -1 oxidation state (but can be -1 oxidation state in order to be isoelectronic with their respective noble gases); when reacting with other more electronegative atoms, they give positive oxidation states. Examples are Cl₂O₇, and BrO^-.

Noble Gases

This group consists of the elements helium, neon, argon, krypton, and xenon. The noble gases have a full valence electron shell. For this reason, noble gases do not normally react (but they rarely do) with other elements (unreactive/stable), hence their former title inert gases. In fact, until 1962, they were thought completely nonreactive. (But fluorides and oxides are known for Xenon(z=54), and a lesser extent for Krypton(z=36).)

Noble gas elements form monatomic molecules, and do not form ionic compounds or solution. They can be ionized in an electrified gas plasma, though. Hence, Noble gases are highly unreactive.

All members of this group are colorless gases (nonmetals), except Bromine which exist as liquid in room temperature. If you look at any periodic table, the density of these gases increases as you go downwards. This is because the mass of the atoms gets larger due to increasing nuclear charge and addition of new shells.

Undiscovered

There are some undiscovered elements on the periodic table. However, due to the understanding of periodic table positions, their descriptions can be estimated. Approximately 172 or more are estimated to fill pertable.

Fun Facts

Iridium and Osmium have the greatest density
Francium is the least electronegative element and Fluorine is the most electronegative element
Elements after Uranium are called Transuranium.
Halogens are the most electronegative elements from other set of Groups.

External Links

Periodic videos