document_title: Periodic table

question_text: what is another name for groups in the periodic table

question_tokens: what is another name for groups in the periodic table

text: Periodic table

text: Overview

text:
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Periodic table

Group
1
2
3

4
5
6
7
8
9
10
11
12
13
14
15
16
17
18

Alkali metals
Alkaline earth metals

Pnictogens
Chalcogens
Halogens
Noble gases

Period
1

Hydrogen1H

Helium2He

2
Lithium3Li
Beryllium4Be

Boron5B
Carbon6C
Nitrogen7N
Oxygen8O
Fluorine9F
Neon10Ne

3
Sodium11Na
Magnesium12Mg

Aluminium13Al
Silicon14Si
Phosphorus15P
Sulfur16S
Chlorine17Cl
Argon18Ar

4
Potassium19K
Calcium20Ca
Scandium21Sc

Titanium22Ti
Vanadium23V
Chromium24Cr
Manganese25Mn
Iron26Fe
Cobalt27Co
Nickel28Ni
Copper29Cu
Zinc30Zn
Gallium31Ga
Germanium32Ge
Arsenic33As
Selenium34Se
Bromine35Br
Krypton36Kr

5
Rubidium37Rb
Strontium38Sr
Yttrium39Y

Zirconium40Zr
Niobium41Nb
Molybdenum42Mo
Technetium43Tc
Ruthenium44Ru
Rhodium45Rh
Palladium46Pd
Silver47Ag
Cadmium48Cd
Indium49In
Tin50Sn
Antimony51Sb
Tellurium52Te
Iodine53I
Xenon54Xe

6
Caesium55Cs
Barium56Ba
Lanthanum57La

Hafnium72Hf
Tantalum73Ta
Tungsten74W
Rhenium75Re
Osmium76Os
Iridium77Ir
Platinum78Pt
Gold79Au
Mercury80Hg
Thallium81Tl
Lead82Pb
Bismuth83Bi
Polonium84Po
Astatine85At
Radon86Rn

7
Francium87Fr
Radium88Ra
Actinium89Ac

Rutherfordium104Rf
Dubnium105Db
Seaborgium106Sg
Bohrium107Bh
Hassium108Hs
Meitnerium109Mt
Darmstadtium110Ds
Roentgenium111Rg
Copernicium112Cn
Nihonium113Nh
Flerovium114Fl
Moscovium115Mc
Livermorium116Lv
Tennessine117Ts
Oganesson118Og

Cerium58Ce
Praseodymium59Pr
Neodymium60Nd
Promethium61Pm
Samarium62Sm
Europium63Eu
Gadolinium64Gd
Terbium65Tb
Dysprosium66Dy
Holmium67Ho
Erbium68Er
Thulium69Tm
Ytterbium70Yb
Lutetium71Lu

Thorium90Th
Protactinium91Pa
Uranium92U
Neptunium93Np
Plutonium94Pu
Americium95Am
Curium96Cm
Berkelium97Bk
Californium98Cf
Einsteinium99Es
Fermium100Fm
Mendelevium101Md
Nobelium102No
Lawrencium103Lr

black=solid
green=liquid
red=gas
gray=unknown
Color of the atomic number shows state of matter (at 0 °C and 1 atm)

Primordial

From decay

Synthetic
Border shows natural occurrence of the element

Background color shows subcategory in the metal–metalloid–nonmetal trend:

Metal
Metalloid
Nonmetal
Unknown
chemical
properties

Alkali metal
Alkaline earth metal
Lanthanide
Actinide
Transition metal
Post-transition metal
Polyatomic nonmetal
Diatomic nonmetal
Noble gas

tag: table

text: Each chemical element has a unique atomic number (Z) representing the number of protons in its nucleus.[n 2] Most elements have differing numbers of neutrons among different atoms, with these variants being referred to as isotopes. For example, carbon has three naturally occurring isotopes: all of its atoms have six protons and most have six neutrons as well, but about one per cent have seven neutrons, and a very small fraction have eight neutrons. Isotopes are never separated in the periodic table; they are always grouped together under a single element. Elements with no stable isotopes have the atomic masses of their most stable isotopes, where such masses are shown, listed in parentheses.[4]

text: In the standard periodic table, the elements are listed in order of increasing atomic number Z (the number of protons in the nucleus of an atom). A new row (period) is started when a new electron shell has its first electron. Columns (groups) are determined by the electron configuration of the atom; elements with the same number of electrons in a particular subshell fall into the same columns (e.g. oxygen and selenium are in the same column because they both have four electrons in the outermost p-subshell). Elements with similar chemical properties generally fall into the same group in the periodic table, although in the f-block, and to some respect in the d-block, the elements in the same period tend to have similar properties, as well. Thus, it is relatively easy to predict the chemical properties of an element if one knows the properties of the elements around it.[5]

text: As of 2016, the periodic table has 118 confirmed elements, from element 1 (hydrogen) to 118 (oganesson). Elements 113, 115, 117 and 118, the most recent discoveries, were officially confirmed by the International Union of Pure and Applied Chemistry (IUPAC) in December 2015. Their proposed names, nihonium (Nh), moscovium (Mc), tennessine (Ts) and oganesson (Og) respectively, were announced by the IUPAC in June 2016 and made official in November 2016.[6][7][8][9]

text: The first 94 elements occur naturally; the remaining 24, americium to oganesson (95–118) occur only when synthesized in laboratories. Of the 94 naturally occurring elements, 83 are primordial and 11 occur only in decay chains of primordial elements.[3] No element heavier than einsteinium (element 99) has ever been observed in macroscopic quantities in its pure form, nor has astatine (element 85); francium (element 87) has been only photographed in the form of light emitted from microscopic quantities (300,000 atoms).[10]

text: Grouping methods

text: Groups

text: A group or family is a vertical column in the periodic table. Groups usually have more significant periodic trends than periods and blocks, explained below. Modern quantum mechanical theories of atomic structure explain group trends by proposing that elements within the same group generally have the same electron configurations in their valence shell.[11] Consequently, elements in the same group tend to have a shared chemistry and exhibit a clear trend in properties with increasing atomic number.[12] However, in some parts of the periodic table, such as the d-block and the f-block, horizontal similarities can be as important as, or more pronounced than, vertical similarities.[13][14][15]

text: Under an international naming convention, the groups are numbered numerically from 1 to 18 from the leftmost column (the alkali metals) to the rightmost column (the noble gases).[16] Previously, they were known by roman numerals. In America, the roman numerals were followed by either an "A" if the group was in the s- or p-block, or a "B" if the group was in the d-block. The roman numerals used correspond to the last digit of today's naming convention (e.g. the group 4 elements were group IVB, and the group 14 elements were group IVA). In Europe, the lettering was similar, except that "A" was used if the group was before group 10, and "B" was used for groups including and after group 10. In addition, groups 8, 9 and 10 used to be treated as one triple-sized group, known collectively in both notations as group VIII. In 1988, the new IUPAC naming system was put into use, and the old group names were deprecated.[17]

text: Some of these groups have been given trivial (unsystematic) names, as seen in the table below, although some are rarely used. Groups 3–10 have no trivial names and are referred to simply by their group numbers or by the name of the first member of their group (such as "the scandium group" for group 3), since they display fewer similarities and/or vertical trends.[16]

text: Elements in the same group tend to show patterns in atomic radius, ionization energy, and electronegativity. From top to bottom in a group, the atomic radii of the elements increase. Since there are more filled energy levels, valence electrons are found farther from the nucleus. From the top, each successive element has a lower ionization energy because it is easier to remove an electron since the atoms are less tightly bound. Similarly, a group has a top-to-bottom decrease in electronegativity due to an increasing distance between valence electrons and the nucleus.[18] There are exceptions to these trends, however: for example, in group 11, electronegativity increases farther down the group.[19]

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Groups in the periodic table

IUPAC group
1
2
3a
a
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18

Mendeleev (I–VIII)
IA
IIA
IIIB

IVB
VB
VIB
VIIB
VIIIB
IB
IIB
IIIB
IVB
VB
VIB
VIIB
b

CAS (US, A-B-A)
IA
IIA
IIIB

IVB
VB
VIB
VIIB
VIIIB
IB
IIB
IIIA
IVA
VA
VIA
VIIA
VIIIA

old IUPAC (Europe, A-B)
IA
IIA
IIIA

IVA
VA
VIA
VIIA
VIIIB
IB
IIB
IIIB
IVB
VB
VIB
VIIB
0

Trivial name
Alkali metals
Alkaline earth metalsr

Coinage metals
Volatile metals
Icosagens
Crystallogens
Pnictogensr
Chalcogensr
Halogensr
Noble gasesr

Name by elementr
Lithium group
Beryllium group
Scandium group

Titanium group
Vanadium group
Chromium group
Manganese group
Iron group
Cobalt group
Nickel group
Copper group
Zinc group
Boron group
Carbon group
Nitrogen group
Oxygen group
Fluorine group
Helium or Neon group

Period 1
h H h

He

Period 2
Li
Be

B
C
N
O
F
Ne

Period 3
Na
Mg

Al
Si
P
S
Cl
Ar

Period 4
K
Ca
Sc

Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Ga
Ge
As
Se
Br
Kr

Period 5
Rb
Sr
Y

Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
In
Sn
Sb
Te
I
Xe

Period 6
Cs
Ba
La
Ce–Lu
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Tl
Pb
Bi
Po
At
Rn

Period 7
Fr
Ra
Ac
Th–Lr
Rf
Db
Sg
Bh
Hs
Mt
Ds
Rg
Cn
Nh
Fl
Mc
Lv
Ts
Og

a Group 3 has scandium (Sc) and yttrium (Y). For the rest of the group, sources differ as either being (1) lutetium (Lu) and lawrencium (Lr), or (2) lanthanum (La) and actinium (Ac), or (3) the whole set of 15+15 lanthanides and actinides. IUPAC has initiated a project to standardize the definition as either (1) Sc, Y, Lu and Lr, or (2) Sc, Y, La and Ac.[20]

b Group 18, the noble gases, were not discovered at the time of Mendeleev's original table. Later (1902), Mendeleev accepted the evidence for their existence, and they could be placed in a new "group 0", consistently and without breaking the periodic table principle.

r Group name as recommended by IUPAC.

h Hydrogen (H), while placed in group 1, is not considered to be part of the alkali metals.

text: Periods

text: A period is a horizontal row in the periodic table. Although groups generally have more significant periodic trends, there are regions where horizontal trends are more significant than vertical group trends, such as the f-block, where the lanthanides and actinides form two substantial horizontal series of elements.[21]

text: Elements in the same period show trends in atomic radius, ionization energy, electron affinity, and electronegativity. Moving left to right across a period, atomic radius usually decreases. This occurs because each successive element has an added proton and electron, which causes the electron to be drawn closer to the nucleus.[22] This decrease in atomic radius also causes the ionization energy to increase when moving from left to right across a period. The more tightly bound an element is, the more energy is required to remove an electron. Electronegativity increases in the same manner as ionization energy because of the pull exerted on the electrons by the nucleus.[18] Electron affinity also shows a slight trend across a period. Metals (left side of a period) generally have a lower electron affinity than nonmetals (right side of a period), with the exception of the noble gases.[23]

text: Blocks

text: Specific regions of the periodic table can be referred to as blocks in recognition of the sequence in which the electron shells of the elements are filled. Each block is named according to the subshell in which the "last" electron notionally resides.[24][n 3] The s-block comprises the first two groups (alkali metals and alkaline earth metals) as well as hydrogen and helium. The p-block comprises the last six groups, which are groups 13 to 18 in IUPAC group numbering (3A to 8A in American group numbering) and contains, among other elements, all of the metalloids. The d-block comprises groups 3 to 12 (or 3B to 2B in American group numbering) and contains all of the transition metals. The f-block, often offset below the rest of the periodic table, has no group numbers and comprises lanthanides and actinides.[25]

text: Metals, metalloids and nonmetals

text: According to their shared physical and chemical properties, the elements can be classified into the major categories of metals, metalloids and nonmetals. Metals are generally shiny, highly conducting solids that form alloys with one another and salt-like ionic compounds with nonmetals (other than the noble gases). The majority of nonmetals are coloured or colourless insulating gases; nonmetals that form compounds with other nonmetals feature covalent bonding. In between metals and nonmetals are metalloids, which have intermediate or mixed properties.[26]

text: Metal and nonmetals can be further classified into subcategories that show a gradation from metallic to non-metallic properties, when going left to right in the rows. The metals are subdivided into the highly reactive alkali metals, through the less reactive alkaline earth metals, lanthanides and actinides, via the archetypal transition metals, and ending in the physically and chemically weak post-transition metals. The nonmetals are simply subdivided into the polyatomic nonmetals, which, being nearest to the metalloids, show some incipient metallic character; the diatomic nonmetals, which are essentially nonmetallic; and the monatomic noble gases, which are nonmetallic and almost completely inert. Specialized groupings such as the refractory metals and the noble metals, which are subsets (in this example) of the transition metals, are also known[27] and occasionally denoted.[28]

text: Placing the elements into categories and subcategories based on shared properties is imperfect. There is a spectrum of properties within each category and it is not hard to find overlaps at the boundaries, as is the case with most classification schemes.[29] Beryllium, for example, is classified as an alkaline earth metal although its amphoteric chemistry and tendency to mostly form covalent compounds are both attributes of a chemically weak or post-transition metal. Radon is classified as a nonmetal and a noble gas yet has some cationic chemistry that is more characteristic of a metal. Other classification schemes are possible such as the division of the elements into mineralogical occurrence categories, or crystalline structures. Categorizing the elements in this fashion dates back to at least 1869 when Hinrichs[30] wrote that simple boundary lines could be drawn on the periodic table to show elements having like properties, such as the metals and the nonmetals, or the gaseous elements.

text: Periodic trends and patterns

text: Electron configuration

text: The electron configuration or organisation of electrons orbiting neutral atoms shows a recurring pattern or periodicity. The electrons occupy a series of electron shells (numbered shell 1, shell 2, and so on). Each shell consists of one or more subshells (named s, p, d, f and g). As atomic number increases, electrons progressively fill these shells and subshells more or less according to the Madelung rule or energy ordering rule, as shown in the diagram. The electron configuration for neon, for example, is 1s2 2s2 2p6. With an atomic number of ten, neon has two electrons in the first shell, and eight electrons in the second shell—two in the s subshell and six in the p subshell. In periodic table terms, the first time an electron occupies a new shell corresponds to the start of each new period, these positions being occupied by hydrogen and the alkali metals.[31][32]

text: Since the properties of an element are mostly determined by its electron configuration, the properties of the elements likewise show recurring patterns or periodic behaviour, some examples of which are shown in the diagrams below for atomic radii, ionization energy and electron affinity. It is this periodicity of properties, manifestations of which were noticed well before the underlying theory was developed, that led to the establishment of the periodic law (the properties of the elements recur at varying intervals) and the formulation of the first periodic tables.[31][32]

text: Atomic radii

text: Atomic radii vary in a predictable and explainable manner across the periodic table. For instance, the radii generally decrease along each period of the table, from the alkali metals to the noble gases; and increase down each group. The radius increases sharply between the noble gas at the end of each period and the alkali metal at the beginning of the next period. These trends of the atomic radii (and of various other chemical and physical properties of the elements) can be explained by the electron shell theory of the atom; they provided important evidence for the development and confirmation of quantum theory.[33]

text: The electrons in the 4f-subshell, which is progressively filled from cerium (element 58) to ytterbium (element 70), are not particularly effective at shielding the increasing nuclear charge from the sub-shells further out. The elements immediately following the lanthanides have atomic radii that are smaller than would be expected and that are almost identical to the atomic radii of the elements immediately above them.[34] Hence hafnium has virtually the same atomic radius (and chemistry) as zirconium, and tantalum has an atomic radius similar to niobium, and so forth. This is known as the lanthanide contraction. The effect of the lanthanide contraction is noticeable up to platinum (element 78), after which it is masked by a relativistic effect known as the inert pair effect.[35] The d-block contraction, which is a similar effect between the d-block and p-block, is less pronounced than the lanthanide contraction but arises from a similar cause.[34]

text: Ionization energy

text: The first ionization energy is the energy it takes to remove one electron from an atom, the second ionization energy is the energy it takes to remove a second electron from the atom, and so on. For a given atom, successive ionization energies increase with the degree of ionization. For magnesium as an example, the first ionization energy is 738 kJ/mol and the second is 1450 kJ/mol. Electrons in the closer orbitals experience greater forces of electrostatic attraction; thus, their removal requires increasingly more energy. Ionization energy becomes greater up and to the right of the periodic table.[35]

text: Large jumps in the successive molar ionization energies occur when removing an electron from a noble gas (complete electron shell) configuration. For magnesium again, the first two molar ionization energies of magnesium given above correspond to removing the two 3s electrons, and the third ionization energy is a much larger 7730 kJ/mol, for the removal of a 2p electron from the very stable neon-like configuration of Mg2+. Similar jumps occur in the ionization energies of other third-row atoms.[35]

text: Electronegativity

text: Electronegativity is the tendency of an atom to attract electrons.[36] An atom's electronegativity is affected by both its atomic number and the distance between the valence electrons and the nucleus. The higher its electronegativity, the more an element attracts electrons. It was first proposed by Linus Pauling in 1932.[37] In general, electronegativity increases on passing from left to right along a period, and decreases on descending a group. Hence, fluorine is the most electronegative of the elements,[n 5] while caesium is the least, at least of those elements for which substantial data is available.[19]

text: There are some exceptions to this general rule. Gallium and germanium have higher electronegativities than aluminium and silicon respectively because of the d-block contraction. Elements of the fourth period immediately after the first row of the transition metals have unusually small atomic radii because the 3d-electrons are not effective at shielding the increased nuclear charge, and smaller atomic size correlates with higher electronegativity.[19] The anomalously high electronegativity of lead, particularly when compared to thallium and bismuth, appears to be an artifact of data selection (and data availability)—methods of calculation other than the Pauling method show the normal periodic trends for these elements.[38]

text: Electron affinity

text: The electron affinity of an atom is the amount of energy released when an electron is added to a neutral atom to form a negative ion. Although electron affinity varies greatly, some patterns emerge. Generally, nonmetals have more positive electron affinity values than metals. Chlorine most strongly attracts an extra electron. The electron affinities of the noble gases have not been measured conclusively, so they may or may not have slightly negative values.[41]

text: Electron affinity generally increases across a period. This is caused by the filling of the valence shell of the atom; a group 17 atom releases more energy than a group 1 atom on gaining an electron because it obtains a filled valence shell and is therefore more stable.[41]

text: A trend of decreasing electron affinity going down groups would be expected. The additional electron will be entering an orbital farther away from the nucleus. As such this electron would be less attracted to the nucleus and would release less energy when added. However, in going down a group, around one-third of elements are anomalous, with heavier elements having higher electron affinities than their next lighter congenors. Largely, this is due to the poor shielding by d and f electrons. A uniform decrease in electron affinity only applies to group 1 atoms.[42]

text: Metallic character

text: The lower the values of ionization energy, electronegativity and electron affinity, the more metallic character the element has. Conversely, nonmetallic character increases with higher values of these properties.[43] Given the periodic trends of these three properties, metallic character tends to decrease going across a period (or row) and, with some irregularities (mostly) due to poor screening of the nucleus by d and f electrons, and relativistic effects,[44] tends to increase going down a group (or column or family). Thus, the most metallic elements (such as caesium and francium) are found at the bottom left of traditional periodic tables and the most nonmetallic elements (oxygen, fluorine, chlorine) at the top right. The combination of horizontal and vertical trends in metallic character explains the stair-shaped dividing line between metals and nonmetals found on some periodic tables, and the practice of sometimes categorizing several elements adjacent to that line, or elements adjacent to those elements, as metalloids.[45][46]

text: Linking or bridging groups

text:
Hydrogen

Helium

Lithium
Beryllium

Boron
Carbon
Nitrogen
Oxygen
Fluorine
Neon

Sodium
Magnesium

Aluminium
Silicon
Phosphorus
Sulfur
Chlorine
Argon

Potassium
Calcium
Scandium

Titanium
Vanadium
Chromium
Manganese
Iron
Cobalt
Nickel
Copper
Zinc
Gallium
Germanium
Arsenic
Selenium
Bromine
Krypton

Rubidium
Strontium
Yttrium

Zirconium
Niobium
Molybdenum
Technetium
Ruthenium
Rhodium
Palladium
Silver
Cadmium
Indium
Tin
Antimony
Tellurium
Iodine
Xenon

Caesium
Barium
Lanthanum
Cerium
Praseodymium
Neodymium
Promethium
Samarium
Europium
Gadolinium
Terbium
Dysprosium
Holmium
Erbium
Thulium
Ytterbium
Lutetium
Hafnium
Tantalum
Tungsten
Rhenium
Osmium
Iridium
Platinum
Gold
Mercury (element)
Thallium
Lead
Bismuth
Polonium
Astatine
Radon

Francium
Radium
Actinium
Thorium
Protactinium
Uranium
Neptunium
Plutonium
Americium
Curium
Berkelium
Californium
Einsteinium
Fermium
Mendelevium
Nobelium
Lawrencium
Rutherfordium
Dubnium
Seaborgium
Bohrium
Hassium
Meitnerium
Darmstadtium
Roentgenium
Copernicium
Nihonium
Flerovium
Moscovium
Livermorium
Tennessine
Oganesson

32-column periodic table showing, from left to right, the location of group 3; lutetium and lawrencium; groups 11–12; and the noble gases

text: From left to right across the four blocks of the long- or 32-column form of the periodic table are a series of linking or bridging groups of elements, located approximately between each block.[47] These groups, like the metalloids, show properties in between, or that are a mixture of, groups to either side. Chemically, the group 3 elements, scandium, yttrium, lanthanum and actinium behave largely like the alkaline earth metals[48] or, more generally, s block metals[49][50] but have some of the physical properties of d block transition metals.[51] Lutetium and lawrencium, at the end of the end of the f block, may constitute another linking or bridging group. Lutetium behaves chemically as a lanthanide but shows a mix of lanthanide and transition metal physical properties.[52][53] Lawrencium, as an analogue of lutetium, would presumable display like characteristics.[n 6] The coinage metals in group 11 (copper, silver, and gold) are chemically capable of acting as either transition metals or main group metals.[56] The volatile group 12 metals, zinc, cadmium and mercury are sometimes regarded as linking the d block to the p block. Notionally they are d block elements but they have few transition metal properties and are more like their p block neighbors in group 13.[57][58] The relatively inert noble gases, in group 18, bridge the most reactive groups of elements in the periodic table—the halogens in group 17 and the alkali metals in group 1.[47]

text: History

text: First systemization attempts

text: In 1789, Antoine Lavoisier published a list of 33 chemical elements, grouping them into gases, metals, nonmetals, and earths.[59] Chemists spent the following century searching for a more precise classification scheme. In 1829, Johann Wolfgang Döbereiner observed that many of the elements could be grouped into triads based on their chemical properties. Lithium, sodium, and potassium, for example, were grouped together in a triad as soft, reactive metals. Döbereiner also observed that, when arranged by atomic weight, the second member of each triad was roughly the average of the first and the third;[60] this became known as the Law of Triads.[61] German chemist Leopold Gmelin worked with this system, and by 1843 he had identified ten triads, three groups of four, and one group of five. Jean-Baptiste Dumas published work in 1857 describing relationships between various groups of metals. Although various chemists were able to identify relationships between small groups of elements, they had yet to build one scheme that encompassed them all.[60]

text: In 1857, German chemist August Kekulé observed that carbon often has four other atoms bonded to it. Methane, for example, has one carbon atom and four hydrogen atoms.[62] This concept eventually became known as valency; different elements bond with different numbers of atoms.[63]

text: In 1862, Alexandre-Emile Béguyer de Chancourtois, a French geologist, published an early form of periodic table, which he called the telluric helix or screw. He was the first person to notice the periodicity of the elements. With the elements arranged in a spiral on a cylinder by order of increasing atomic weight, de Chancourtois showed that elements with similar properties seemed to occur at regular intervals. His chart included some ions and compounds in addition to elements. His paper also used geological rather than chemical terms and did not include a diagram; as a result, it received little attention until the work of Dmitri Mendeleev.[64]

text: In 1864, Julius Lothar Meyer, a German chemist, published a table with 44 elements arranged by valency. The table showed that elements with similar properties often shared the same valency.[65] Concurrently, William Odling (an English chemist) published an arrangement of 57 elements, ordered on the basis of their atomic weights. With some irregularities and gaps, he noticed what appeared to be a periodicity of atomic weights among the elements and that this accorded with "their usually received groupings".[66] Odling alluded to the idea of a periodic law but did not pursue it.[67] He subsequently proposed (in 1870) a valence-based classification of the elements.[68]

text: English chemist John Newlands produced a series of papers from 1863 to 1866 noting that when the elements were listed in order of increasing atomic weight, similar physical and chemical properties recurred at intervals of eight; he likened such periodicity to the octaves of music.[69][70] This so termed Law of Octaves, however, was ridiculed by Newlands' contemporaries, and the Chemical Society refused to publish his work.[71] Newlands was nonetheless able to draft a table of the elements and used it to predict the existence of missing elements, such as germanium.[72] The Chemical Society only acknowledged the significance of his discoveries five years after they credited Mendeleev.[73]

text: In 1867, Gustavus Hinrichs, a Danish born academic chemist based in America, published a spiral periodic system based on atomic spectra and weights, and chemical similarities. His work was regarded as idiosyncratic, ostentatious and labyrinthine and this may have militated against its recognition and acceptance.[74][75]

text: Mendeleev's table

text: Russian chemistry professor Dmitri Mendeleev and German chemist Julius Lothar Meyer independently published their periodic tables in 1869 and 1870, respectively.[76] Mendeleev's table was his first published version; that of Meyer was an expanded version of his (Meyer's) table of 1864.[77] They both constructed their tables by listing the elements in rows or columns in order of atomic weight and starting a new row or column when the characteristics of the elements began to repeat.[78]

text: The recognition and acceptance afforded to Mendeleev's table came from two decisions he made. The first was to leave gaps in the table when it seemed that the corresponding element had not yet been discovered.[79] Mendeleev was not the first chemist to do so, but he was the first to be recognized as using the trends in his periodic table to predict the properties of those missing elements, such as gallium and germanium.[80] The second decision was to occasionally ignore the order suggested by the atomic weights and switch adjacent elements, such as tellurium and iodine, to better classify them into chemical families. Later in 1913, Henry Moseley determined experimental values of the nuclear charge or atomic number of each element, and showed that Mendeleev's ordering actually corresponds to the order of increasing atomic number.[81]

text: The significance of atomic numbers to the organization of the periodic table was not appreciated until the existence and properties of protons and neutrons became understood. Mendeleev's periodic tables used atomic weight instead of atomic number to organize the elements, information determinable to fair precision in his time. Atomic weight worked well enough in most cases to (as noted) give a presentation that was able to predict the properties of missing elements more accurately than any other method then known. Substitution of atomic numbers, once understood, gave a definitive, integer-based sequence for the elements, and Moseley predicted (in 1913) that the only elements still missing between aluminium (Z=13) and gold (Z=79) were Z = 43, 61, 72 and 75, all of which were later discovered. The sequence of atomic numbers is still used today even as new synthetic elements are being produced and studied.[82]

text: Second version and further development

text: In 1871, Mendeleev published his periodic table in a new form, with groups of similar elements arranged in columns rather than in rows, and those columns numbered I to VIII corresponding with the element's oxidation state. He also gave detailed predictions for the properties of elements he had earlier noted were missing, but should exist.[83] These gaps were subsequently filled as chemists discovered additional naturally occurring elements.[84] It is often stated that the last naturally occurring element to be discovered was francium (referred to by Mendeleev as eka-caesium) in 1939.[85] However, plutonium, produced synthetically in 1940, was identified in trace quantities as a naturally occurring element in 1971.[86]

text: The popular[87] periodic table layout, also known as the common or standard form (as shown at various other points in this article), is attributable to Horace Groves Deming. In 1923, Deming, an American chemist, published short (Mendeleev style) and medium (18-column) form periodic tables.[88][n 7] Merck and Company prepared a handout form of Deming's 18-column medium table, in 1928, which was widely circulated in American schools. By the 1930s Deming's table was appearing in handbooks and encyclopaedias of chemistry. It was also distributed for many years by the Sargent-Welch Scientific Company.[89][90][91]

text: With the development of modern quantum mechanical theories of electron configurations within atoms, it became apparent that each period (row) in the table corresponded to the filling of a quantum shell of electrons. Larger atoms have more electron sub-shells, so later tables have required progressively longer periods.[92]

text: In 1945, Glenn Seaborg, an American scientist, made the suggestion that the actinide elements, like the lanthanides, were filling an f sub-level. Before this time the actinides were thought to be forming a fourth d-block row. Seaborg's colleagues advised him not to publish such a radical suggestion as it would most likely ruin his career. As Seaborg considered he did not then have a career to bring into disrepute, he published anyway. Seaborg's suggestion was found to be correct and he subsequently went on to win the 1951 Nobel Prize in chemistry for his work in synthesizing actinide elements.[93][94][n 8]

text: Although minute quantities of some transuranic elements occur naturally,[3] they were all first discovered in laboratories. Their production has expanded the periodic table significantly, the first of these being neptunium, synthesized in 1939.[95] Because many of the transuranic elements are highly unstable and decay quickly, they are challenging to detect and characterize when produced. There have been controversies concerning the acceptance of competing discovery claims for some elements, requiring independent review to determine which party has priority, and hence naming rights.[96] In 2010, a joint Russia–US collaboration at Dubna, Moscow Oblast, Russia, claimed to have synthesized six atoms of tennessine (element 117), making it the most recently claimed discovery. It, along with nihonium (element 113), moscovium (element 115), and oganesson (element 118), are the four most recently named elements, whose names all became official on 28 November 2016.[97]

text: Different periodic tables

text: The long- or 32-column table

text: The modern periodic table is sometimes expanded into its long or 32-column form by reinstating the footnoted f-block elements into their natural position between the s- and d-blocks. Unlike the 18-column form this arrangement results in "no interruptions in the sequence of increasing atomic numbers".[98] The relationship of the f-block to the other blocks of the periodic table also becomes easier to see.[99] Jensen advocates a form of table with 32 columns on the grounds that the lanthanides and actinides are otherwise relegated in the minds of students as dull, unimportant elements that can be quarantined and ignored.[100] Despite these advantages the 32-column form is generally avoided by editors on account of its undue rectangular ratio (compared to a book page ratio),[101] and the familiarity of chemists with the modern form (as introduced by Seaborg).[102]

text: Tables with different structures

text: Within 100 years of the appearance of Mendeleev's table in 1869 it has been estimated that around 700 different periodic table versions were published.[103] As well as numerous rectangular variations, other periodic table formats have been shaped, for example,[n 9] like a circle, cube, cylinder, building, spiral, lemniscate,[104] octagonal prism, pyramid, sphere, or triangle. Such alternatives are often developed to highlight or emphasize chemical or physical properties of the elements that are not as apparent in traditional periodic tables.[103]

text: A popular[105] alternative structure is that of Theodor Benfey (1960). The elements are arranged in a continuous spiral, with hydrogen at the centre and the transition metals, lanthanides, and actinides occupying peninsulas.[106]

text: Most periodic tables are two-dimensional;[3] however, three-dimensional tables are known to as far back as at least 1862 (pre-dating Mendeleev's two-dimensional table of 1869). More recent examples include Courtines' Periodic Classification (1925),[107] Wringley's Lamina System (1949),[108] Giguère's Periodic helix (1965)[109] and Dufour's Periodic Tree (1996).[110] Going one further, Stowe's Physicist's Periodic Table (1989)[111] has been described as being four-dimensional (having three spatial dimensions and one colour dimension).[112]

text: The various forms of periodic tables can be thought of as lying on a chemistry–physics continuum.[113] Towards the chemistry end of the continuum can be found, as an example, Rayner-Canham's "unruly"[114] Inorganic Chemist's Periodic Table (2002),[115] which emphasizes trends and patterns, and unusual chemical relationships and properties. Near the physics end of the continuum is Janet's Left-Step Periodic Table (1928). This has a structure that shows a closer connection to the order of electron-shell filling and, by association, quantum mechanics.[116] A somewhat similar approach has been taken by Alper,[117] albeit criticized by Eric Scerri as disregarding the need to display chemical and physical periodicity.[118] Somewhere in the middle of the continuum is the ubiquitous common or standard form of periodic table. This is regarded as better expressing empirical trends in physical state, electrical and thermal conductivity, and oxidation numbers, and other properties easily inferred from traditional techniques of the chemical laboratory.[119] Its popularity is thought to be a result of this layout having a good balance of features in terms of ease of construction and size, and its depiction of atomic order and periodic trends.[67][120]

text:
[hide]

v
t
e

Left-step periodic table (by Charles Janet)

f1
f2
f3
f4
f5
f6
f7
f8
f9
f10
f11
f12
f13
f14
d1
d2
d3
d4
d5
d6
d7
d8
d9
d10
p1
p2
p3
p4
p5
p6
s1
s2

1s

H
He

2s

Li
Be

2p 3s

B
C
N
O
F
Ne
Na
Mg

3p 4s

Al
Si
P
S
Cl
Ar
K
Ca

3d 4p 5s

Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Ga
Ge
As
Se
Br
Kr
Rb
Sr

4d 5p 6s

Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
In
Sn
Sb
Te
 I
Xe
Cs
Ba

4f 5d 6p 7s
La
Ce
Pr
Nd
Pm
Sm
Eu
Gd
Tb
Dy
Ho
Er
Tm
Yb
Lu
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Tl
Pb
Bi
Po
At
Rn
Fr
Ra

5f 6d 7p 8s
Ac
Th
Pa
U
Np
Pu
Am
Cm
Bk
Cf
Es
Fm
Md
No
Lr
Rf
Db
Sg
Bh
Hs
Mt
Ds
Rg
Cn
Nh
Fl
Mc
Lv
Ts
Og
119
120

f-block
d-block
p-block
s-block

This form of periodic table is more congruent with the order in which electron shells are ideally filled according to the Madelung rule, as shown in the accompanying sequence in the left margin (read from top to bottom, left to right). In reality, the filling of electron shells is characterized by a number of irregularities.

text: Open questions and controversies

text: Placement of hydrogen and helium

text: Simply following electron configurations, hydrogen (electronic configuration 1s1) and helium (1s2) should be placed in groups 1 and 2, above lithium ([He]2s1) and beryllium ([He]2s2).[24] However, such placing is rarely used outside of the context of electron configurations: When the noble gases (then called "inert gases") were first discovered around 1900, they were known as "group 0", reflecting no chemical reactivity of these elements known at that point, and helium was placed on the top that group, as it did share the extreme chemical inertness seen throughout the group. As the group changed its formal number, many authors continued to assign helium directly above neon, in group 18; one of the examples of such placing is the current IUPAC table.[121]

text: Hydrogen's chemical properties are not very close to those of the alkali metals, which occupy group 1, and on that basis hydrogen is sometimes placed elsewhere: one of the most common alternatives is in group 17;[118] one of the factors behind it is the strictly univalent predominantly non-metallic chemistry of hydrogen, and that of fluorine (the element placed on the top of group 17) is strictly univalent and non-metallic. Sometimes, to show how hydrogen has properties both corresponding to those of the alkali metals and the halogens, it may be shown in two columns simultaneously.[122] Another suggestion is above carbon in group 14: placed that way, it fits well into the trends of increasing ionization potential values and electron affinity values, and is not too far from the electronegativity trend, even though hydrogen cannot show the tetravalence characteristic of the heavier group 14 elements.[123] Finally, hydrogen is sometimes placed separately from any group; this is based on how general properties of hydrogen differ from that of any group. The other period 1 element, helium, is sometimes placed separately from any group as well.[124] The property that distinguishes helium from the rest of the noble gases (even though the extraordinary inertness of helium is extremely close to that of neon and argon[125]) is that in its closed electron shell, helium has only two electrons in the outermost electron orbital, while the rest of the noble gases have eight.

text: Group 3 and its elements in periods 6 and 7

text: Although scandium and yttrium are always the first two elements in group 3, the identity of the next two elements is not completely settled. They are commonly lanthanum and actinium, and less often lutetium and lawrencium. The two variants originate from historical difficulties in placing the lanthanides in the periodic table, and arguments as to where the f block elements start and end.[126][n 10][n 11] It has been claimed that such arguments are proof that, "it is a mistake to break the [periodic] system into sharply delimited blocks".[128] A third variant shows the two positions below yttrium as being occupied by the lanthanides and the actinides.

text: Chemical and physical arguments have been made in support of lutetium and lawrencium[129][130] but the majority of authors seem unconvinced.[131] Most working chemists are not aware there is any controversy.[132] In December 2015 an IUPAC project was established to make a recommendation on the matter.[133]

text: Lanthanum and actinium

text: La and Ac below Y

text: Lanthanum and actinium are commonly depicted as the remaining group 3 members.[134][n 12] It has been suggested that this layout originated in the 1940s, with the appearance of periodic tables relying on the electron configurations of the elements and the notion of the differentiating electron. The configurations of caesium, barium and lanthanum are [Xe]6s1, [Xe]6s2 and [Xe]5d16s2. Lanthanum thus has a 5d differentiating electron and this establishes "it in group 3 as the first member of the d-block for period 6".[135] A consistent set of electron configurations is then seen in group 3: scandium [Ar]3d14s2, yttrium [Kr]4d15s2 and lanthanum [Xe]5d16s2. Still in period 6, ytterbium was assigned an electron configuration of [Xe]4f135d16s2 and lutetium [Xe]4f145d16s2, "resulting in a 4f differentiating electron for lutetium and firmly establishing it as the last member of the f-block for period 6".[135] Later spectroscopic work found that the electron configuration of ytterbium was in fact [Xe]4f146s2. This meant that ytterbium and lutetium—the latter with [Xe]4f145d16s2—both had 14 f-electrons, "resulting in a d- rather than an f- differentiating electron" for lutetium and making it an "equally valid candidate" with [Xe]5d16s2 lanthanum, for the group 3 periodic table position below yttrium.[135] Lanthanum, however, has the advantage of incumbency since the 5d1 electron appears for the first time in its structure whereas it appears for the third time in lutetium, having also made a brief second appearance in gadolinium.[136]

text: In terms of chemical behaviour,[137] and trends going down group 3 for properties such as melting point, electronegativity and ionic radius,[138][139] scandium, yttrium, lanthanum and actinium are similar to their group 1–2 counterparts. In this variant, the number of f electrons in the most common (trivalent) ions of the f-block elements consistently matches their position in the f-block.[140] For example, the f-electron counts for the trivalent ions of the first three f-block elements are Ce 1, Pr 2 and Nd 3.[141]

text: Lutetium and lawrencium

text: Lu and Lr below Y

text: In other tables, lutetium and lawrencium are the remaining group 3 members.[n 13] Early techniques for chemically separating scandium, yttrium and lutetium relied on the fact that these elements occurred together in the so-called "yttrium group" whereas La and Ac occurred together in the "cerium group".[135] Accordingly, lutetium rather than lanthanum was assigned to group 3 by some chemists in the 1920s and 30s.[n 14] Several physicists in the 1950s and 60s favoured lutetium, in light of a comparison of several of its physical properties with those of lanthanum.[135] This arrangement, in which lanthanum is the first member of the f-block, is disputed by some authors since lanthanum lacks any f-electrons. However, it has been argued that this is not valid concern given other periodic table anomalies—thorium, for example, has no f-electrons yet is part of the f-block.[142] As for lawrencium, its gas phase atomic electron configuration was confirmed in 2015 as [Rn]5f147s27p1. Such a configuration represents another periodic table anomaly, regardless of whether lawrencium is located in the f-block or the d-block, as the only potentially applicable p-block position has been reserved for nihonium with its predicted configuration of [Rn]5f146d107s27p1.[143][n 15]

text: Chemically, scandium, yttrium and lutetium (and presumably lawrencium) behave like trivalent versions of the group 1–2 metals.[145] On the other hand, trends going down the group for properties such as melting point, electronegativity and ionic radius, are similar to those found among their group 4–8 counterparts.[135] In this variant, the number of f electrons in the gaseous forms of the f-block atoms usually matches their position in the f-block. For example, the f-electron counts for the first five f-block elements are La 0, Ce 1, Pr 3, Nd 4 and Pm 5.[135]

text: Lanthanides and actinides

text: Markers below Y

text: A few authors position all thirty lanthanides and actinides in the two positions below yttrium (usually via footnote markers). This variant emphasizes similarities in the chemistry of the 15 lanthanide elements (La–Lu), possibly at the expense of ambiguity as to which elements occupy the two group 3 positions below yttrium, and a 15-column wide f block (there can only be 14 elements in any row of the f block).[n 16]

text: Groups included in the transition metals

text: The definition of a transition metal, as given by IUPAC, is an element whose atom has an incomplete d sub-shell, or which can give rise to cations with an incomplete d sub-shell.[146] By this definition all of the elements in groups 3–11 are transition metals. The IUPAC definition therefore excludes group 12, comprising zinc, cadmium and mercury, from the transition metals category.

text: Some chemists treat the categories "d-block elements" and "transition metals" interchangeably, thereby including groups 3–12 among the transition metals. In this instance the group 12 elements are treated as a special case of transition metal in which the d electrons are not ordinarily involved in chemical bonding. The 2007 report of mercury(IV) fluoride (HgF4), a compound in which mercury would use its d electrons for bonding, has prompted some commentators to suggest that mercury can be regarded as a transition metal.[147] Other commentators, such as Jensen,[148] have argued that the formation of a compound like HgF4 can occur only under highly abnormal conditions; indeed, its existence is currently disputed. As such, mercury could not be regarded as a transition metal by any reasonable interpretation of the ordinary meaning of the term.[148]

text: Still other chemists further exclude the group 3 elements from the definition of a transition metal. They do so on the basis that the group 3 elements do not form any ions having a partially occupied d shell and do not therefore exhibit any properties characteristic of transition metal chemistry.[149] In this case, only groups 4–11 are regarded as transition metals. However, though the group 3 elements show few of the characteristic chemical properties of the transition metals, they do show some of their characteristic physical properties (on account of the presence in each atom of a single d electron).[51]

text: Elements with unknown chemical properties

text: Although all elements up to oganesson have been discovered, of the elements above hassium (element 108), only copernicium (element 112), nihonium (element 113), and flerovium (element 114) have known chemical properties, and only for the copernicium is there enough evidence for a conclusive categorisation at present. The other elements may behave differently from what would be predicted by extrapolation, due to relativistic effects; for example, flerovium has been predicted to possibly exhibit some noble-gas-like properties, even though it is currently placed in the carbon group.[150] More recent experiments have suggested, however, that flerovium behaves chemically like lead, as expected from its periodic table position.[151]

text: Further periodic table extensions

text:
Hydrogen

Helium

Lithium
Beryllium

Boron
Carbon
Nitrogen
Oxygen
Fluorine
Neon

Sodium
Magnesium

Aluminium
Silicon
Phosphorus
Sulfur
Chlorine
Argon

Potassium
Calcium
Scandium

Titanium
Vanadium
Chromium
Manganese
Iron
Cobalt
Nickel
Copper
Zinc
Gallium
Germanium
Arsenic
Selenium
Bromine
Krypton

Rubidium
Strontium
Yttrium

Zirconium
Niobium
Molybdenum
Technetium
Ruthenium
Rhodium
Palladium
Silver
Cadmium
Indium
Tin
Antimony
Tellurium
Iodine
Xenon

Caesium
Barium
Lanthanum

Cerium
Praseodymium
Neodymium
Promethium
Samarium
Europium
Gadolinium
Terbium
Dysprosium
Holmium
Erbium
Thulium
Ytterbium
Lutetium
Hafnium
Tantalum
Tungsten
Rhenium
Osmium
Iridium
Platinum
Gold
Mercury (element)
Thallium
Lead
Bismuth
Polonium
Astatine
Radon

Francium
Radium
Actinium

Thorium
Protactinium
Uranium
Neptunium
Plutonium
Americium
Curium
Berkelium
Californium
Einsteinium
Fermium
Mendelevium
Nobelium
Lawrencium
Rutherfordium
Dubnium
Seaborgium
Bohrium
Hassium
Meitnerium
Darmstadtium
Roentgenium
Copernicium
Nihonium
Flerovium
Moscovium
Livermorium
Tennessine
Oganesson

Ununennium
Unbinilium
Unbiunium

Unquadquadium
Unquadpentium
Unquadhexium
Unquadseptium
Unquadoctium
Unquadennium
Unpentnilium
Unpentunium
Unpentbium
Unpenttrium
Unpentquadium
Unpentpentium
Unpenthexium
Unpentseptium
Unpentoctium
Unpentennium
Unhexnilium
Unhexunium
Unhexbium
Unhextrium
Unhexquadium
Unhexpentium
Unhexhexium
Unhexseptium
Unhexoctium
Unhexennium
Unseptnilium
Unseptunium
Unseptbium

Unbibium
Unbitrium
Unbiquadium
Unbipentium
Unbihexium
Unbiseptium
Unbioctium
Unbiennium
Untrinilium
Untriunium
Untribium
Untritrium
Untriquadium
Untripentium
Untrihexium
Untriseptium
Untrioctium
Untriennium
Unquadnilium
Unquadunium
Unquadbium
Unquadtrium

Periodic table with eight rows, extended to element 172[152]

text: It is unclear whether new elements will continue the pattern of the current periodic table as period 8, or require further adaptations or adjustments. Seaborg expected the eighth period to follow the previously established pattern exactly, so that it would include a two-element s-block for elements 119 and 120, a new g-block for the next 18 elements, and 30 additional elements continuing the current f-, d-, and p-blocks, culminating in element 168, the next noble gas.[153] More recently, physicists such as Pekka Pyykkö have theorized that these additional elements do not follow the Madelung rule, which predicts how electron shells are filled and thus affects the appearance of the present periodic table. There are currently several competing theoretical models for the placement of the elements of atomic number less than or equal to 172.[154]

text: Element with the highest possible atomic number

text: The number of possible elements is not known. A very early suggestion made by Elliot Adams in 1911, and based on the arrangement of elements in each horizontal periodic table row, was that elements of atomic weight greater than 256± (which would equate to between elements 99 and 100 in modern-day terms) did not exist.[155] A higher—more recent—estimate is that the periodic table may end soon after the island of stability,[156] which is expected to centre around element 126, as the extension of the periodic and nuclides tables is restricted by proton and neutron drip lines.[157] Other predictions of an end to the periodic table include at element 128 by John Emsley,[3] at element 137 by Richard Feynman,[158] and at element 155 by Albert Khazan.[3][n 17]

text: The Bohr model exhibits difficulty for atoms with atomic number greater than 137, as any element with an atomic number greater than 137 would require 1s electrons to be travelling faster than c, the speed of light.[159] Hence the non-relativistic Bohr model is inaccurate when applied to such an element.

text: The relativistic Dirac equation has problems for elements with more than 137 protons. For such elements, the wave function of the Dirac ground state is oscillatory rather than bound, and there is no gap between the positive and negative energy spectra, as in the Klein paradox.[160] More accurate calculations taking into account the effects of the finite size of the nucleus indicate that the binding energy first exceeds the limit for elements with more than 173 protons. For heavier elements, if the innermost orbital (1s) is not filled, the electric field of the nucleus will pull an electron out of the vacuum, resulting in the spontaneous emission of a positron;[161] however, this does not happen if the innermost orbital is filled, so that element 173 is not necessarily the end of the periodic table.[158]

text: Optimal form

text: The many different forms of periodic table have prompted the question of whether there is an optimal or definitive form of periodic table. The answer to this question is thought to depend on whether the chemical periodicity seen to occur among the elements has an underlying truth, effectively hard-wired into the universe, or if any such periodicity is instead the product of subjective human interpretation, contingent upon the circumstances, beliefs and predilections of human observers. An objective basis for chemical periodicity would settle the questions about the location of hydrogen and helium, and the composition of group 3. Such an underlying truth, if it exists, is thought to have not yet been discovered. In its absence, the many different forms of periodic table can be regarded as variations on the theme of chemical periodicity, each of which explores and emphasizes different aspects, properties, perspectives and relationships of and among the elements.[n 18]


document_title: Devon Ke Dev...Mahadev

question_text: who played the role of nandi in mahadev

question_tokens: who played the role of nandi in mahadev

root

text: Devon Ke Dev...Mahadev

text: Cast[edit]

text:
Actor
Character

Mohit Raina
Shiva / Mahadev / Mahakala / Nataraja / Nilakantha

Jalandhara

Jatta

Virabhadra

Kal Bhairav

Ardhanarishvara

Chandrashekar

Dattatreya

Lohitang(elder)

Yaksha

Kiraat/ Vyadh

Aadi Yogi

Aghora/Martand (Khandoba)

Nat Bhairav

Acharya Mahatapa

Vrishabh

Loknath

Bhoothnath

Pashupatinath

Shambhu

Vaidhyanath

Har-Narayan/Harihara

Bhola

Sonarika Bhadoria / Pooja Bose /
Suhasi Goradia Dhami

Parvati/Adi Parashakti / Adi Shakti / Durga

Matsya Kanya

Ashta-Matrikas

Navadurga

Kali / Mahakali

Dasha-Mahavidyas

Ardhanarishvara

Kaalratri

Bhramari Devi

Bheelni

Gayatri Devi

Goddess Bhairavi

Mahalasa

Mouni Roy
Sati

Adi Parashakti / Adi Shakti / Durga

Saurabh Raj Jain
Lord Vishnu / Narayana

Lord Krishna

Dattatreya

Guru Pratyaya

Har-Narayan/Harihara

Nara-Narayana

Vikramjeet Virk
Banasur

Falaq Naaz / Ragini Dubey
Goddess Lakshmi

Haripriya

Rukmini

Radha Krishna Dutt
Lord Brahma

Dattatreya

Via Roy Choudhury / Salina Prakash
Saraswati

Rushiraj Pawar
Senapati Kartikeya/ Murugan

Tanya Sharma
Devasena

Ahsaas Channa
Ashokasundari

Ashnoor Kaur
Young Ashokasundari

Lavanya Bhardwaj
Nahusha

Shailesh Dattar
Narad Muni

Sadhil Kapoor
Ganesha / Vinayak (younger)

Alpesh Dhakan / Ehsaan Bhatia
Ganesha / Vinayak

Aarya Vora
Siddhi

Amrita Singh
Buddhi

Kumar Hedge
Nandi

Priyanka Thakare
Suyasha [ Nandi's wife]

Hemant Choudhary
Prajapati Vishwaroop

Jiten Lalwani / Vikram Aditya
Lord Indra

Shivangi Sharma
Indrani

Manish Bishla
Surya

Vicky Batra
Chandra

Deepika Upadhyay / Sangeeta Khanayat
Goddess Ganga

Godavari

Banai

Anjali Abrol
Meenakshi

Mohit Sharma
Vasuki

Piyush Sahdev
Rama

Rubina Dilaik
Sita

Kunal Verma
Lakshman

Garima Jain
Urmila

Vishal Kotian
Hanuman

Vineett Kumar
Bharat

Harshad Arora
Shatrughna

Ulka Gupta
Devi Kanya Kumari

Arbaaz Ali Khan
Balarama

Reem Sheikh
(Younger) Manasa

Vishesh Bansal
Tripati

Kratika Sengar
Manasa

Manoj Kolhatkar
Sage Dadhichi

Rajeev Bharadwaj
Sage Kashyap

Romanch Mehta
Sage Atri

Jayant Rawal
Maharishi Halahal

Jeetendra Trehan
Sage Markandeya

Shailesh Dattar
Sage Narada

Darshan Kumar
Sage Shukracharya

Raman Khatri
Sage Atharvan

Atul Singh
Sage Pulaha

Sushil Parashar
Sage Pitamber

Mohit Dagri
(younger) Lohitang

Raj Premi
Demon Tarakasur

Rahul Dev
Demon Arunasur

Chetan Hansraj
Nighas

Deepak Jethi
Mahishasura

Manav Gohil
Andhaka

Tej Sapru
Shankhachudha

Ankur Nayyar
Krauncha Giri

Ibrar Yakub
Tuhund

Tushar Jha
(younger)Jalandhara

Arun Bali
Vajranaka (Tarakasur's father)

Akhilendra Mishra
King Mahabali

Sanjay Swaraj
Bhasmasur

Manish Wadhwa / Tarun Khanna
Ravan

Sudesh Berry
Malla-Manika

Abhaas Mehta
Adi

Rakshanda Khan
Madanike

Anupam Bhattacharya
Ripunjay / Devodas

Ojaswi Oberoi / Parakh Madan[1]
Mohini

Ritu Chauhan
Devi Rati

Pankaj Dheer
King Himavan

Mugdha Shah / Shilpa Tulaskar
Queen Mainavati

Khyati Khandke Keswani
Kritika

Surendra Pal
Prajapati Daksha

Shalini Kapoor Sagar
Queen Prasuti

Rishina Kandhari / Riyanka Chanda
Princess Khyati

Priyanka Panchal
Princess Aditi

Charu Asopa / Kanishka Soni
Princess Revati

Surbhi Shukla
Princess Rohini

Manini Mishra
Princess Vijaya

Annapurna Vitthal Bhairi
Shanta

Suhasini Mulay
Parvati's grandmother

Deepraj Rana
Parshuram

Amrapali Gupta
Matsyakanya

Prabhat Bhattacharya
King Aayu

Neha Kaul
Indumathi

Rishi Khuranna
Nahusha

Jaya Bhattacharya
Diti

Anand Goradia
Pushpadanta

Dolly Sohi
Mahalasa's mother

Shilpa Shinde
Mahananda

Vivek Mishra
Yella koti

Pankaj Berry
Raja Durdum

Mitika Sharma
Queen Sunaina

Mohit Chauhan
King Janaka

Mihir Mishra
King Dashratha

Gauri Singh
Queen Kaushalya

Anushka Singh
Queen Sumitra

Manasi Vyas
Queen Kaikeyi

Tapeshwari Sharma
Usha / Behula

Aarti Singh
Baani

Bhavna Khatri
Chitralekha

Daya Shankar Pandey
Lakulish

Tushar Dalvi
Chandradhar

Malhar Pandya
Aniruddha/Lakhsmichandra

Parul Chaudhary
Sanaka

Deepali Pansare
Tulsi

Rajendra Chawla
Acharya Gyanmurti

Gungun Uprari
Maharani

Neha Marda
Vrinda

Chestha Mehta
Prithvi

text: Production and distribution[edit]

text: Ritoo Jenjani has done the prosthetic makeup for the presentation of Kali.[2]

tag: p

text: The show has been dubbed in Bengali, Tamil, Malayalam, Oriya, Telugu, Assamese, Marathi, and Indonesian with titles Devadidev Mahadev, Shivam, Kailasanathan, Mahadev, Hara Hara Mahadeva, Mahadev, Devanche Dev Mahadev, and Mahadewa respectively. In Indonesia, the drama was broadcast on antv. It was remade in Kannada as HaraHara Mahadeva The official DVD version of the series Season 1 up to Shiv Parvati wedding is available.

text: In Telugu, due to reception it being re-telecast at third time in star maagold and star maa respectively.

text: Reception[edit]

text: The episode of 9 September 2012, featuring Kali killing the demon Raktabija rated the shows highest TRP with an 8.2 TVR.[3]


document_title: Appalachian Spring

question_text: simple gifts from aaron copland's appalachian spring is in

question_tokens: simple gifts from aaron copland 's appalachian spring is in

text: Appalachian Spring

text: Composition process[edit]

text:
Opening: Appalachian Spring, original version for 13 instruments

Sample of the opening movement in Copland's ballet

Problems playing this file? See media help.

text: In 1942, Martha Graham and Elizabeth Sprague Coolidge commissioned Copland to write a ballet with "an American theme". Copland did the bulk of the work in 1943/44, and the work was premiered at the Library of Congress on Oct. 30, 1944, with Graham dancing the lead role. In 1945, Copland was commissioned by conductor Artur Rodzinski to rearrange the ballet as an orchestral suite, preserving most of the music. Copland cut about 10 minutes from the original 13-instrument score to make the suite. From the preface in the original Boosey & Hawkes publication of the suite:

text: The original scoring called for a chamber ensemble of thirteen instruments. The present arrangement for symphony orchestra was made by the composer in the Spring of 1945. It is a condensed version of the ballet, retaining all essential features but omitting those sections in which the interest is primarily choreographic.[3]

text: The Orchestral Suite from 1945 was first recorded by Serge Koussevitzky with the Boston Symphony Orchestra.[4] In 1954, Eugene Ormandy asked Copland to expand the orchestration for the full score of the ballet. In 1972, Boosey & Hawkes published a version of the suite fusing the structure of it with the scoring of the original ballet: double string quartet, bass, flute, clarinet, bassoon, and piano. Thus there are four versions of Appalachian Spring, dating from 1944 (13-player complete), 1945 (orchestral suite), 1954 (orchestral complete) and 1972 (13-player suite).

text: The 1944 version was recorded in 1991 by Hugh Wolff with the Saint Paul Chamber Orchestra for Teldec.[5] The 1954 version was recorded by Michael Tilson Thomas and the San Francisco Symphony Orchestra for RCA Victor in May 1999.

text: The original ballet and the orchestral suite were well received. The latter was credited as more important in popularizing the composer.

text: Copland's inspiration arrived in the form of an Edward Deming Andrews book, The Gift to be Simple - Songs, Dances and Rituals of the American Shakers, J.J. Augustin; Republished by Dover. Copland stated that the book's title composition jumped into him immediately upon receipt (see Winterthur archives). Originally, Copland did not have a title for the work, referring to it simply as "Ballet for Martha"—a title as simple and direct as the Shaker tune 'Tis the Gift to be Simple quoted in the music.[6] Shortly before the premiere, Graham suggested Appalachian Spring, a phrase from a Hart Crane poem, "The Dance" from a collection of poems in his book "The Bridge."

text:
O Appalachian Spring! I gained the ledge;
Steep, inaccessible smile that eastward bends
And northward reaches in that violet wedge
Of Adirondacks!

text: Because he composed the music without the benefit of knowing what the title was going to be, Copland was often amused when people told him he captured the beauty of the Appalachians in his music, a fact he alluded to in an interview with NPR's Fred Calland.[7] Little known is that the word "spring" denotes a source of water in the Crane poem; however the poem is a journey to meet springtime.

text: Ballet storyline[edit]

text: The story tells of a spring celebration of the American pioneers of the 19th century, after building a new Pennsylvania farmhouse. Among the central characters are a bride, a groom, a pioneer woman, a preacher and his congregation. The L.A. Times provides a concise summary of the storyline in its transitions between the choreographed sequences stating:

text: Created in 1944, the ballet tells a simple story. A young farm couple ruminate on their lives before getting married and setting up house in the wilderness. An itinerant preacher delivers a sermon. An older pioneer woman oversees the events with sympathy and wisdom. The newlyweds muse on their future as night falls. In the course of the dance, Graham reveals the inner lives of the four principal characters -- Wife, Husbandman, Pioneer Woman and Preacher. She shows that the couple will face a future that will not be all sweetness and light, but she also draws out the private and shared emotional resources they will be able to bring to the challenges. Such is the power of Graham's images, however, that this very particular story broadens out to become a parable about Americans conquering a new land.[8]

text: Form of the piece[edit]

text: The orchestral suite is divided into eight sections. Copland describes each scene thus:

text:
Very slowly. Introduction of the characters, one by one, in a suffused light.
Fast/Allegro. Sudden burst of unison strings in A major arpeggios starts the action. A sentiment both elated and religious gives the keynote to this scene.
Moderate/Moderato. Duo for the Bride and her Intended – scene of tenderness and passion.
Quite fast. The Revivalist and his flock. Folksy feeling – suggestions of square dances and country fiddlers.
Still faster/Subito Allegro. Solo dance of the Bride – presentiment of motherhood. Extremes of joy and fear and wonder.
Very slowly (as at first). Transition scene to music reminiscent of the introduction.
Calm and flowing/Doppio Movimento. Scenes of daily activity for the Bride and her Farmer husband. There are five variations on a Shaker theme. The theme, sung by a solo clarinet, was taken from a collection of Shaker melodies compiled by Edward D. Andrews, and published under the title "The Gift to Be Simple." The melody borrowed and used almost literally is called "Simple Gifts."
Moderate. Coda/Moderato - Coda. The Bride takes her place among her neighbors. At the end the couple are left "quiet and strong in their new house." Muted strings intone a hushed prayerlike chorale passage. The close is reminiscent of the opening music.

tag: ol

text: Themes[edit]

text: Variations[edit]

text: The original ballet version is divided into 14 movements. The movements that do not appear in the orchestral suite occur mostly between the 7th and last movement as variations on the Shaker melody Simple Gifts (1848). The second variation provides a lyrical treatment in the low register while the third contrasts starkly in a fast staccato. The last two variations of this section use only a part of the folk tune, first an extraction treated as a pastoral variation and then as a majestic closing. In the ballet, but not the suite, there is an intermediary section that moves away from the folk tune preceding the final two variations.

text: Shaker melody[edit]

text:
Shaker music

Music

* Issachar Bates, Ode to Contentment

Joseph Brackett, Simple Gifts
Wyeth and Hammond, The Humble Heart

Works inspired by Simple Gifts

* Air and Simple Gifts

Joel Cohen, Simple Gifts
Aaron Copland, Appalachian Spring
Roger Lee Hall, Four New England Shaker Spirituals
Lord of the Dance
Old American Songs
Weezer, The Greatest Man That Ever Lived

Works inspired by Shakers

* William Coulter, Shaker trilogy

Roger Lee Hall, Four New England Shaker Spirituals
David Johansen, Shaker
R.E.M., Fireplace (Document)
Eric W. Sawyer, The Humble Heart
Kevin Siegfried, Angel of Light

v
t
e

text: Known as the "Shaker Melody", "Shaker Song", and the "Shaker Hymn", the music Copland based his ending variations on was actually called Simple Gifts. This same Shaker tune was used by Sydney Carter in a widely recognized hymn entitled "Lord of the Dance". Copland published independent arrangements of this section for band (1958) and orchestra (1967) titled Variations on a Shaker Melody.

text: In popular culture[edit]

text: For many years part of the seventh movement of the orchestral suite was used as the opening music to CBS Reports.[9]

text: Notes[edit]

text:
Jump up ^ Dickinson, Peter (2002). Copland Connotations. Rochester: Boydell Press. p. 30. ISBN 978-0-85115-902-7.
Jump up ^ Pulitzer winners for Music category
Jump up ^ http://archives.nyphil.org/index.php/artifact/fcdf250d-65fc-4c11-95ac-a16530000dbc
Jump up ^ http://www.americanmusicpreservation.com/Coplandtribute.htm
Jump up ^ http://www.allmusic.com/album/copland-appalachian-spring-mw0001814338
Jump up ^ Matthew Naughtin, Ballet Music, 2014, p. 147
Jump up ^ Milestones of the Millennium: Appalachian Spring
Jump up ^ CHRIS PASLES. "Appalacian Spirng: Martha's Ballet". L.A. Times. January 03, 1991. [1].
Jump up ^ David Shedden. "Today in Media History: Remembering the “CBS Reports” documentary 'Harvest of Shame'". The Poynter Institute, October 27, 2014


document_title: Flannan Isles Lighthouse

question_text: when did the events at flannan isle occur

text: Flannan Isles Lighthouse

text: History[edit]

text: The 23-metre (75 ft) lighthouse was designed by David Alan Stevenson for the Northern Lighthouse Board (NLB). Construction, between 1895 and 1899, was undertaken by George Lawson of Rutherglen at a cost of £6,914 inclusive of the building of the landing places, stairs, railway tracks etc. All of the materials used had to be hauled up the 45-metre (148 ft) cliffs directly from supply boats, no trivial task in the ever-churning Atlantic. A further £3,526 was spent on the shore station at Breasclete on the Isle of Lewis.[3] It was first lit on 7 December 1899.

text: The purpose of the railway tracks was to facilitate the transport of provisions for the keepers and fuel for the light (paraffin, at that date; the light consumed twenty barrels a year) up the steep gradients from the landing places by means of a cable-hauled railway. This was powered by a small steam engine in a shed adjoining the lighthouse. A track descended from the lighthouse in a westerly direction and then curved round to the south. In the approximate centre of the island it forked by means of a set of hand-operated points humorously dubbed "Clapham Junction"; one branch continued in its curvature to head eastwards to the east landing place, on the south-east corner of the island, thus forming a half-circle, while the other, slightly shorter, branch curved back to the west to serve the west landing, situated in a small inlet on the island's south coast. The final approaches to the landing stages were extremely steep. The cable was guided round the curves by pulleys set between the rails, and a line of posts set outside the inner rail prevented it from going too far astray should it jump off the pulleys. The cargo was carried in a small four-wheeled bogie.[4]

text: In 1925, the lighthouse was one of the first Scottish lights to receive communications from the shore by wireless telegraphy.[5] In the 1960s, the island's transport system was modernised. The railway was removed, leaving behind the concrete bed on which it had been laid to serve as a roadway for a "Gnat" – a three-wheeled, rubber-tyred cross-country vehicle powered by a 400cc four-stroke engine, built by Aimers McLean of Galashiels. This had a somewhat shorter working life than the railway, becoming redundant in its turn when the helipad was constructed.[6]

text: On 28 September 1971, the lighthouse was automated. A reinforced concrete helipad was constructed at the same time to enable maintenance visits in heavy weather. The light is produced by burning acetylene gas and has a range of 17 nautical miles; 20 miles (32 km). It is now monitored from the Butt of Lewis[7] and the shore station has been converted into flats.[8]

text: Mystery of 1900[edit]

text: Other than for its relative isolation, the lighthouse would be relatively unremarkable, were it not for the events which took place just over a year after it was commissioned.

text: Discovery[edit]

text: The first hint of anything untoward on the Flannan Isles came on 15 December 1900. The steamer Archtor on passage from Philadelphia to Leith passed the islands in poor weather and noted that the light was not operational. The ship suffered the misfortune to run aground on Carpie Rock in the Firth of Forth [9] some time after passing the lighthouse and after the struggle to save the ship, the fact of the lighthouse light being unlit was not reported on arrival at Oban for some time, the ship's master, Captain Holman, being distracted by the damage to his ship, and the procedures for dealing with her on arrival in port. The island lighthouse was manned by a three-man team (Thomas Marshall, James Ducat, and Donald MacArthur), with a rotating fourth man spending time on shore. The relief vessel, the lighthouse tender Hesperus, was unable to set out on a routine visit from Lewis planned for 20 December due to adverse weather and did not arrive until noon on Boxing Day (26 December).[7] On arrival, the crew and relief keeper found that the flagstaff was bare of its flag, none of the usual provision boxes had been left on the landing stage for re-stocking, and more ominously, none of the lighthouse keepers were there to welcome them ashore. Jim Harvie, captain of Hesperus, gave a strident blast on his whistle and set off a distress flare, but no reply was forthcoming.

text: A boat was launched and Joseph Moore, the relief keeper, was put ashore alone. He found the entrance gate to the compound and main door both closed, the beds unmade, and the clock stopped. Returning to the landing stage with this grim news, he then went back up to the lighthouse with Hesperus's second-mate and a seaman. A further search revealed that the lamps were cleaned and refilled. A set of oilskins was found, suggesting that one of the keepers had left the lighthouse without them, which was surprising considering the severity of the weather on the date of the last entry in the lighthouse log. The only sign of anything amiss in the lighthouse was an overturned chair by the kitchen table. Of the keepers there was no sign, neither inside the lighthouse nor anywhere on the island.[7][10]

text: Moore and three volunteer seamen were left to attend the light and Hesperus returned to the shore station at Breasclete. Captain Harvie sent a telegram to the Northern Lighthouse Board dated 26 December 1900, stating:

text: A dreadful accident has happened at the Flannans. The three keepers, Ducat, Marshall and the Occasional have disappeared from the Island... The clocks were stopped and other signs indicated that the accident must have happened about a week ago. Poor fellows they must have been blown over the cliffs or drowned trying to secure a crane.[7][10]

text: The men remaining on the island scoured every corner for clues as to the fate of the keepers. At the east landing everything was intact, but the west landing provided considerable evidence of damage caused by recent storms. A box at 33 metres (108 ft) above sea level had been broken and its contents strewn about; iron railings were bent over, the iron railway by the path was wrenched out of its concrete, and a rock weighing more than a ton had been displaced above that. On top of the cliff at more than 60 metres (200 ft) above sea level, turf had been ripped away as far as 10 metres (33 ft) from the cliff edge. The missing keepers had kept their log until 9 a.m. on 15 December, however, and their entries made it clear that the damage had occurred before the disappearance of the writers.[7][11]

text: Speculations and misconceptions[edit]

text: No bodies were ever found and the loneliness of the rocky islets may have lent itself to feverish imaginings. Theories abounded and resulted in "fascinated national speculation".[12] Some were simply elaborations on the truth. For example, the events were commemorated in Wilfrid Wilson Gibson's 1912 ballad Flannan Isle.[13] The poem refers erroneously to an uneaten meal laid out on the table, indicating that the keepers had been suddenly disturbed.

text:
Yet, as we crowded through the door,
We only saw a table spread
For dinner, meat, and cheese and bread;
But, all untouch'd; and no-one there,
As though, when they sat down to eat,
Ere they could even taste,
Alarm had come, and they in haste
Had risen and left the bread and meat,
For at the table head a chair
Lay tumbled on the floor.[14]

text: However, Nicholson (1995) makes it clear that this does not square with Moore's recorded observations of the scene, which state that: "The kitchen utensils were all very clean, which is a sign that it must be after dinner some time they left."[7][15]

text: Other less plausible rumours ensued—that one keeper had murdered the other two and then thrown himself into the sea in a fit of remorse (which is likely not the case, simply because the keepers only had to work together for short amounts of time, and none of the men reported any psychotic behaviour); that a sea serpent (or giant seabird) had carried the men away; that they had been abducted by foreign spies; or that they had met their fate through the malevolent presence of a boat filled with ghosts—and the baleful influence of the "Phantom of the Seven Hunters" was widely suspected locally.[7]

text: Northern Lighthouse Board investigation[edit]

text: On 29 December 1900, Robert Muirhead, a Northern Lighthouse Board (NLB) superintendent, arrived to conduct the official investigation into the incident.

text: The explanation offered by Muirhead is more prosaic than the fanciful rumours suggested. He examined the clothing left behind in the lighthouse and concluded that James Ducat and Thomas Marshall had gone down to the western landing stage, and that Donald MacArthur (the 'Occasional') had left the lighthouse during heavy rain in his shirt sleeves. He noted that whoever left the light last and unattended was in breach of NLB rules.[7] He also noted that some of the damage to the west landing was "difficult to believe unless actually seen".[13]

text: From evidence which I was able to procure I was satisfied that the men had been on duty up till dinner time on Saturday the 15th of December, that they had gone down to secure a box in which the mooring ropes, landing ropes etc. were kept, and which was secured in a crevice in the rock about 110 ft (34 m) above sea level, and that an extra large sea had rushed up the face of the rock, had gone above them, and coming down with immense force, had swept them completely away.[16]

text: Whether this explanation brought any comfort to the families of the lost keepers is unknown. The deaths of Thomas Marshall, James Ducat (who left a widow and four children), and Donald MacArthur (who left a widow and two children) cast a shadow over the lighthouse service for many years.[13]

text: Later theories and interpretations[edit]

text: Christopher Nicholson offers an alternative idea for the demise of the keepers.[7] The coastline of Eilean Mòr is deeply indented with narrow gullies called geos. The west landing, which is situated in such a geo, terminates in a cave. In high seas or storms, water would rush into the cave and then explode out again with considerable force. Nicholson speculates that McArthur may have seen a series of large waves approaching the island, and knowing the likely danger to his colleagues, ran down to warn them, only to suffer the same fate as well.[17] This theory has the advantages of explaining the over-turned chair, and the set of oilskins remaining indoors,[7] although perhaps, not the closed door and gate.[18]

text: Haswell-Smith (2004) attributes the origins of the theory to Walter Aldebert, a keeper on the Flannans from 1953 to 1957. Aldebert believed one man may have been washed into the sea, that his companion rushed back to the light for help but that both would-be rescuers also were washed away by a second freak wave.[18]

text: McCloskey (2014) states that a fight broke out near the cliff edge, by the West Landing, between the three Keepers started by the allegedly volatile Macarthur and the three fell to their deaths.[19]

text: The event remains a popular issue of contention among those who are interested in paranormal activity. Inevitably perhaps, modern imaginations speculate about abduction by aliens.[12] A fictional use of this idea is the basis for the Doctor Who serial Horror of Fang Rock.[20] The mystery also was the inspiration for the composer Peter Maxwell Davies's modern chamber opera The Lighthouse (1979).[21] The British rock group Genesis wrote and recorded "The Mystery of Flannan Isle Lighthouse" in 1968 while working on their first album, but it was not released until 1998 in Genesis Archive 1967-75.[22] Angela J. Elliott wrote a novel which was published in 2005 about the disappearance of the lighthouse keepers, entitled Some Strange Scent of Death after a line from Gibson's poem.[23] The "haunted" islands and the lighthouse also feature heavily as a hideout for a villain in British author Manda Benson's novel Pilgrennon's Beacon.[24] In 2008, the New Zealand band Beltane wrote a song about the lighthouse and its mysterious disappearances on the album ...Through Darker Seasons.[25]

text: All the main theories are examined in the (Discovery) Science Channel The Unexplained Files Season 2 Episode 5


document_title: List of shortest players in National Basketball Association history

question_text: who is the shortest player in the nba 2018

text: This is a complete listing of the shortest players in National Basketball Association history at a listed height of 5 feet 9 inches (175 cm) or shorter. Only 25 players in NBA history have been at a listed height of 5' 9" or shorter.[1] Two are currently active. The shortest NBA player to be inducted into the Naismith Memorial Basketball Hall of Fame is Calvin Murphy at 5' 9". With one exception, Dino Martin (a forward), all of the players listed here have played or play the position of point guard.

text:
^
Active NBA player

*
Inducted into the Naismith Memorial Basketball Hall of Fame

GP
Games played
Pts
Points
PPG
Points per game

FG%
Field goal percentage
FT%
Free throw percentage
Ast
Assists

APG
Assists per game
Stl
Steals
SPG
Steals per game

text:
Height
Weight
Player
Nationality
Teams
GP
Pts
PPG
FG%
FT%
Ast
APG
Stl
SPG
Notes

5 ft 3 in (1.60 m)
136 lb (62 kg)
Muggsy Bogues[2]
 USA
Washington Bullets (1987–1988)
Charlotte Hornets (1988–1997)
Golden State Warriors (1997–1999)
Toronto Raptors (1999–2001)
889
6,858
7.7
.458
.827
6,726
7.6
1,369
1.54
Played alongside the original one of the two tallest players in NBA history, Manute Bol, during the 1987–88 season for the Washington Bullets; their difference in height was 28 inches (71 cm).

5 ft 5 in (1.65 m)
135 lb (61 kg)
Earl Boykins[3]
 USA
New Jersey Nets (1999)
Cleveland Cavaliers (1999, 2000)
Orlando Magic (1999)
Los Angeles Clippers (2001–2002)
Golden State Warriors (2002–03)
Denver Nuggets (2003–2007)
Milwaukee Bucks (2007, 2011)
Charlotte Bobcats (2008)
Washington Wizards (2009–10)
Houston Rockets (2012)
652
5,791
8.9
.417
.876
2,092
3.2
390
0.60

5 ft 6 in (1.68 m)
165 lb (75 kg)
Mel Hirsch[4]
 USA
Boston Celtics (1946–1947)
13
19
1.5
.200
.500
10
0.8
—
—
During his time, was the NBA's shortest player.

5 ft 7 in (1.70 m)
140 lb (64 kg)
Greg Grant[5]
 USA
Phoenix Suns (1989–1990)
New York Knicks (1990–1991)
Charlotte Hornets (1991–1992)
Philadelphia 76ers (1991–1992, 1992–1993, 1995–1996)
Washington Bullets (1995–1996)
Denver Nuggets (1994–1995, 1995–1996)
274
767
2.8
.383
.710
751
2.7
161
0.59

5 ft 7 in (1.70 m)
160 lb (73 kg)
Keith Jennings[6]
 USA
Golden State Warriors (1992–1995)
164
1,090
6.6
.436
.852
614
3.7
164
1.00

5 ft 7 in (1.70 m)
150 lb (68 kg)
Herm Klotz[7]
 USA
Baltimore Bullets (1947–1948)
11
15
1.4
.226
.333
7
0.6
—
—
Shortest player to ever win an NBA championship. Later served as longtime head coach of the Washington Generals.

5 ft 7 in (1.70 m)
150 lb (68 kg)
Wataru Misaka[8]
 USA
New York Knicks (1947–1948)
3
7
2.3
.333
0
0.0
—
—
—
First Non-Caucasian player and first Asian player in the NBA.

5 ft 7 in (1.70 m)
150 lb (68 kg)
Monte Towe[9]
 USA
Denver Nuggets (1976–1977)
51
130
2.5
.406
.720
87
1.7
16
0.31
The shortest player in the original ABA.

5 ft 7 in (1.70 m)
133 lb (60 kg)
Spud Webb[10]
 USA
Atlanta Hawks (1985–1991, 1995–1996)
Sacramento Kings (1991–1995)
Minnesota Timberwolves (1996)
Orlando Magic (1998)
814
8,072
9.9
.452
.848
4,342
5.3
922
1.13
Won the NBA Slam Dunk Contest in 1986; shortest player to participate in the Slam Dunk Contest.

5 ft 8 in (1.73 m)
165 lb (75 kg)
Charlie Criss[11]
 USA
Atlanta Hawks (1977–1981, 1983–1984, 1984–1985)
San Diego Clippers (1981–1982)
Milwaukee Bucks (1982–1984)
418
3,534
8.5
.432
.831
1,335
3.2
366
0.88

5 ft 8 in (1.73 m)
160 lb (73 kg)
Dino Martin[12]
 USA
Providence Steamrollers (1946–1948)
92
834
9.1
.294
.638
73
0.8
—
—
The only player on this list who did not play the guard position.

5 ft 8 in (1.73 m)
170 lb (77 kg)
Willie Somerset[13]
 USA
Baltimore Bullets (1965–1966)
8
45
5.6
.419
.818
9
1.1
—
—

5 ft 9 in (1.75 m)
160 lb (73 kg)
Howie Carl[14]
 USA
Chicago Packers (1961–1962)
31
170
5.5
.333
.706
57
1.8
—
—

5 ft 9 in (1.75 m)
158 lb (72 kg)
Charlie Hoefer[15]

Toronto Huskies (1946–1947)
Boston Celtics (1947–1948)
65
361
5.6
.250
.646
36
0.6
—
—

5 ft 9 in (1.75 m)
150 lb (68 kg)
Lionel Malamed[16]
 USA
Indianapolis Jets (1948)
Rochester Royals (1948–1949)
44
258
5.9
.334
.831
61
1.4
—
—

5 ft 9 in (1.75 m)
170 lb (77 kg)
Ed Melvin[17]
 USA
Pittsburgh Ironmen (1946–1947)
57
281
4.9
.263
.654
37
0.6
—
—

5 ft 9 in (1.75 m)
165 lb (75 kg)
Calvin Murphy*[18]
 USA
San Diego/Houston Rockets (1970–1983)
1,002
17,949
17.9
.482
.892
4,402
4.4
1,165[19]
1.53[19]
Shortest NBA player to be inducted to the Hall of Fame, as well as appear in at least one All-Star Game.++

5 ft 9 in (1.75 m)
145 lb (66 kg)
Angelo Musi[20]
 USA
Philadelphia Warriors (1946–1949)
161
1,359
8.4
.290
.771
117
0.7
—
—

5 ft 9 in (1.75 m)
160 lb (73 kg)
Ralph O'Brien
 USA
Indianapolis Olympians (1951–1952)
Baltimore Bullets
119
848
7.1
.360
.830
180
1.5
—
—

5 ft 9 in (1.75 m)
180 lb (82 kg)
Nate Robinson[21]
 USA
New York Knicks (2005–2010)
Boston Celtics (2009–2011)
Oklahoma City Thunder (2011)
Golden State Warriors (2011–12)
Chicago Bulls (2012–2013)
Denver Nuggets (2013–2015)
Los Angeles Clippers (2015)
New Orleans Pelicans (2015)
574
6,569
11.4
.427
.800
1,725
3.0
522
0.91
The only three-time winner of the NBA Slam Dunk Contest, winning in 2006, 2009 and 2010.

5 ft 9 in (1.75 m)
155 lb (70 kg)
Gene Rock[22]
 USA
Chicago Stags (1947–1948)
11
10
0.9
.222
.500
0
0.0
—
—

5 ft 9 in (1.75 m)
165 lb (75 kg)
Yuta Tabuse[23]
 JPN
Phoenix Suns (2004–2005)
4
7
1.8
.167
1.000
3
0.8
0
0.00
The first (and so far, only) Japanese born player to ever play in the NBA.

5 ft 9 in (1.75 m)
185 lb (84 kg)
Isaiah Thomas^[24]
 USA
Sacramento Kings (2011–2014)
Phoenix Suns (2014–2015)
Boston Celtics (2015–2017)
Cleveland Cavaliers (2017–2018)
Los Angeles Lakers (2018–present)
389
6,877
22.2
.438
.871
1,973
6.2
383
0.99
Shortest player to be included in an All-NBA Team. Shortest player to play in an NBA All-Star game joined by Calvin Murphy. Shortest player to play in multiple All-Star games. Shortest player to record a triple-double in a game.

5 ft 9 in (1.75 m)
176 lb (80 kg)
Kay Felder^[25]
 USA
Cleveland Cavaliers (2016–2017)
Chicago Bulls (2017)
Detroit Pistons (2018–present)
56
221
3.9
.366
.754
78
1.4
21
0.4

text: ++Note: The shortest player in the Naismith Memorial Basketball Hall of fame is pre-NBA player Barney Sedran, at 5 feet 4 inches.[26]